Daniel Nocera -- Artificial Photosynthesis ![](0logo.gif) **[rexresearch.com](../index.htm)** --- **Daniel NOCERA** **Artificial Photosynthesis** --- **[MIT Researchers Inch Toward Photosynthesis in a Beaker](#mit1)** **[Anne Trafton : Major Discovery from MIT Primed to Unleash Solar Revolution](#mit2)** **[Jonathan Fahey : Solar Energy, All Night Long](#forbes)** **[Daniel Nocera, *et al*.: US Patent # 6,863,781 : Process for Photocatalysis...](#6863781)** **[Google Search Results](#google)** --- [**http://web.mit.edu/newsoffice/2001/nocera.html**](http://web.mit.edu/newsoffice/2001/nocera.html) **MIT Researchers Inch Toward Photosynthesis in a Beaker** ( August 30, 2001 ) CAMBRIDGE, Mass. -- In a step toward creating energy from sunlight as plants do, MIT researchers have invented a compound that produces hydrogen gas with the help of a catalyst and a zap of light. The researchers, Professor Daniel G. Nocera of chemistry and former MIT graduate student Alan F. Heyduk, reported their discovery in the August 31 issue of Science. Creating a molecule to replace a leaf -- essentially, photosynthesis in a beaker -- could provide a cheap, clean future energy source, Professor Nocera said. "We have been seeking a future alternative fuel source by studying the principles that govern the conversion of photon energy into chemical potential," he said. "Our strategy is to use the energy of sunlight to drive reactants uphill to energy-rich products, thus harnessing the sun's energy to create a renewable energy source in the future." **Splitting chemical bonds** Nocera and Heyduk created a compound based on the metal rhodium. When the rhodium photocatalyst is dissolved in solution, the researchers add to it a hydrogen-containing acid (also called a hydrohalic acid -- one example is hydrochloric acid), and shine light on it. "In the leaf, sugar and oxygen are energy-rich products. In our beaker, the sought-after fuels are hydrogen and a halogen, produced catalytically from the photochemical splitting of hydrohalic acid," Nocera said. The structure of the rhodium compound allows it to break the hydrohalic acid's chemical bonds. Hydrogen gas, with a byproduct of bromides and chlorides, is produced. The by-products are chemically trapped and recycled into the reaction. While not as complete and efficient as photosynthesis, this system comes close to the ideal use of a molecular catalyst as part of a homogeneous reaction for which scientists have been searching for more than three decades. **Plant power** The African violet on your windowsill converts sunlight into a high-energy fuel over and over again in a process so complicated that scientists have yet to come close to duplicating it. Attempts to mimic it so far have not produced an energy conversion process efficient enough to compete with fossil fuels. However, future generations will require alternatives to limited petroleum-based fuels. If scientists can make hydrogen, it could combine with the oxygen in the air to make water. This is the process that fuel cells use to generate energy. Within fuel cells, which are now being produced by various manufacturers for vehicles and buildings, it would take a photocatalyst and solar energy to start the reaction all over again from water. In the work reported in Science, the MIT researchers' goal was to trap the photon energy in a structurally well-defined molecule and control the subsequent reactions to convert light into hydrogen. Previously, the closest scientists have come to achieving this goal is to use photocatalysts that are solids, which need massive surface areas. In a chemical reaction, the trick is to design a system where the energy needed to break a chemical bond is compensated by the absorption of a photon. The payoff: an alternative, clean fuel source produced with the help of sunlight. "Heyduk and Nocera have taken fundamental ideas of photochemistry and harnessed them to achieve a long sought-after but elusive goal: molecular-based photocatalytic production of a useable fuel," writes James K. McCusker, a chemistry professor at Michigan State University, in a perspective for Science. "The importance of this work is not the specificity of the catalyst's performance, but rather that a new door has been opened." Putting sunlight to work Sunlight is the perfect energy source -- readily available and free. According to the National Renewable Energy Laboratory of Golden, Colo., the sun bathes us every day with more energy than humans could use in 30 years. Nocera says that their new process is not perfect, but it is a beginning that may re-ignite solar energy research that has been largely dormant since the 1970s. "As it stands, we have performed half of the photosynthetic reaction by generating hydrogen. If we can now get the other half of the process to work (getting the halogen), we would have a framework for future energy production," Nocera said. This work is supported by the National Science Foundation. --- **Daniel Nocera** ![](nocera1.jpg) ... ![](nocera3.jpg) ![](animtn.gif) --- [**http://web.mit.edu/newsoffice/2008/oxygen-0731.html**](http://web.mit.edu/newsoffice/2008/oxygen-0731.html) **Major Discovery from MIT Primed to Unleash Solar Revolution ---** **Scientists mimic essence of plants' energy storage system** **Anne Trafton**, News Office ( July 31, 2008 ) In a revolutionary leap that could transform solar power from a marginal, boutique alternative into a mainstream energy source, MIT researchers have overcome a major barrier to large-scale solar power: storing energy for use when the sun doesn't shine. Until now, solar power has been a daytime-only energy source, because storing extra solar energy for later use is prohibitively expensive and grossly inefficient. With today's announcement, MIT researchers have hit upon a simple, inexpensive, highly efficient process for storing solar energy. Requiring nothing but abundant, non-toxic natural materials, this discovery could unlock the most potent, carbon-free energy source of all: the sun. "This is the nirvana of what we've been talking about for years," said MIT's Daniel Nocera, the Henry Dreyfus Professor of Energy at MIT and senior author of a paper describing the work in the July 31 issue of Science. "Solar power has always been a limited, far-off solution. Now we can seriously think about solar power as unlimited and soon." Inspired by the photosynthesis performed by plants, Nocera and Matthew Kanan, a postdoctoral fellow in Nocera's lab, have developed an unprecedented process that will allow the sun's energy to be used to split water into hydrogen and oxygen gases. Later, the oxygen and hydrogen may be recombined inside a fuel cell, creating carbon-free electricity to power your house or your electric car, day or night. The key component in Nocera and Kanan's new process is a new catalyst that produces oxygen gas from water; another catalyst produces valuable hydrogen gas. The new catalyst consists of cobalt metal, phosphate and an electrode, placed in water. When electricity -- whether from a photovoltaic cell, a wind turbine or any other source -- runs through the electrode, the cobalt and phosphate form a thin film on the electrode, and oxygen gas is produced. Combined with another catalyst, such as platinum, that can produce hydrogen gas from water, the system can duplicate the water splitting reaction that occurs during photosynthesis. The new catalyst works at room temperature, in neutral pH water, and it's easy to set up, Nocera said. "That's why I know this is going to work. It's so easy to implement," he said. 'Giant leap' for clean energy Sunlight has the greatest potential of any power source to solve the world's energy problems, said Nocera. In one hour, enough sunlight strikes the Earth to provide the entire planet's energy needs for one year. James Barber, a leader in the study of photosynthesis who was not involved in this research, called the discovery by Nocera and Kanan a "giant leap" toward generating clean, carbon-free energy on a massive scale. "This is a major discovery with enormous implications for the future prosperity of humankind," said Barber, the Ernst Chain Professor of Biochemistry at Imperial College London. "The importance of their discovery cannot be overstated since it opens up the door for developing new technologies for energy production thus reducing our dependence for fossil fuels and addressing the global climate change problem." 'Just the beginning' Currently available electrolyzers, which split water with electricity and are often used industrially, are not suited for artificial photosynthesis because they are very expensive and require a highly basic (non-benign) environment that has little to do with the conditions under which photosynthesis operates. More engineering work needs to be done to integrate the new scientific discovery into existing photovoltaic systems, but Nocera said he is confident that such systems will become a reality. "This is just the beginning," said Nocera, principal investigator for the Solar Revolution Project funded by the Chesonis Family Foundation and co-Director of the Eni-MIT Solar Frontiers Center. "The scientific community is really going to run with this." Nocera hopes that within 10 years, homeowners will be able to power their homes in daylight through photovoltaic cells, while using excess solar energy to produce hydrogen and oxygen to power their own household fuel cell. Electricity-by-wire from a central source could be a thing of the past. The project is part of the MIT Energy Initiative, a program designed to help transform the global energy system to meet the needs of the future and to help build a bridge to that future by improving today's energy systems. MITEI Director Ernest Moniz, Cecil and Ida Green Professor of Physics and Engineering Systems, noted that "this discovery in the Nocera lab demonstrates that moving up the transformation of our energy supply system to one based on renewables will depend heavily on frontier basic science." The success of the Nocera lab shows the impact of a mixture of funding sources - governments, philanthropy, and industry. This project was funded by the National Science Foundation and by the Chesonis Family Foundation, which gave MIT $10 million this spring to launch the Solar Revolution Project, with a goal to make the large scale deployment of solar energy within 10 years. --- [**http://www.forbes.com/energy/2008/07/30/nocera-solar-power-biz-energy-cz\_jf\_0731solar.html**](http://www.forbes.com/energy/2008/07/30/nocera-solar-power-biz-energy-cz_jf_0731solar.html) 07.31.08, 2:30 PM ET **Solar Energy, All Night Long** **Jonathan Fahey** MIT professor Daniel G. Nocera has long been jealous of plants. He desperately wanted to do what they do -- split water into hydrogen and oxygen and use the products to do work. That, he figures, is the only way we humans can solve our energy problems; enough energy pours down from the sun in one hour to power the planet's energy needs for a year. In January, only a month after reevaluating his methodology in the face of a frustratingly slow process, he finally found a way. "For six months now I've been looking at the leaves and saying 'I own you guys!'" Nocera's discovery -- a cheap and easy way to store energy that he thinks will be used to change solar power into a mainstream energy source -- will be published in the journal Science on Friday. "This is the nirvana of what we've been talking about for years," said Nocera, the Henry Dreyfus Professor of Energy at MIT. "Solar power has always been a limited, far-off solution. Now we can seriously think about solar power as unlimited--and soon." Plants catch light and turn it into an electric current, then use that energy to excite catalysts that split water into hydrogen and oxygen during what is called photosynthesis' light cycle. The energy is then used during the dark cycle to allow the plant to build sugars used for growth and energy storage. Nocera and Matthew Kanan, a postdoctoral fellow in Nocera's lab, focused on the water-splitting part of photosynthesis. They found cheap and simple catalysts that did a remarkably good job. They dissolved cobalt and phosphate in water and then zapped it with electricity through an electrode. The cobalt and phosphate form a thin-film catalyst around the electrode that then use electrons from the electrode to split the oxygen from water. The oxygen bubbles to the surface, leaving a proton behind. A few inches away, another catalyst, platinum, helps that bare proton become hydrogen. (This second reaction is a well-known one, and not part of Nocera and Kanan's study.) The hydrogen and oxygen, separated and on-hand, can be used to power a fuel cell whenever energy is needed. "Once you put a photovoltaic on it," he says, "you've got an inorganic leaf." James Barber, a biochemistry professor at Imperial College London who studies artificial photosynthesis but was not involved in this research, called the discovery by Nocera and Kanan a "giant leap" toward generating clean, carbon-free energy on a massive scale. "This is a major discovery with enormous implications for the future prosperity of humankind," he said. "The importance of their discovery cannot be overstated." Nocera's discovery arose from frustration. Disappointed with the pace of his lab's progress, Nocera and his team decided in December to question some of the basic assumptions they had made in setting up earlier experiments. Chemists, it turns out, are always worrying about the stability of their catalysts and end up doing backflips to try to synthesize materials that won't corrode. Photosynthesis, though, is so violently reactive that the catalysts involved break down every 30 minutes. The leaf has to constantly rebuild them. Maybe, thought Nocera, instead of fighting corrosion, he should work with it. "It's a bias a lot of scientists have. We want something to be structurally stable. But all it has to be is functionally stable." This thinking led Nocera to try his cobalt-phosphate mixture. He knew it wouldn't hold together, but he thought it might still work. Sure enough, Nocera's catalyst breaks down whenever the electricity is cut, but it assembles itself again when electricity is reapplied. Nocera's discovery is still a science experiment. It needs plenty of engineering before it can be a useful device. The cobalt and phosphate at the center of Nocera's work is cheap and plentiful, but the hydrogen reaction uses platinum, which is rare and expensive. The electrode needs to be improved so the oxygen-making process can speed up. And the system needs to be integrated into some kind of electricity-producing device, ideally powered by solar or wind on one end and a fuel cell on the other. But splitting the oxygen away from the water was the hard part, and Nocera has done it. "Now we can start thinking about a totally distributed solar [photovoltaic] system," he said. "We couldn't have a solar economy unless it could produce energy 24/7. Now we can." His hope is that because unlike traditional electrolysis devices, which are expensive and require toxic alkaline solutions, his system is so cheap, simple and benign that scientists and engineers around the world will be able to improve it quickly. For his part, Nocera says he will work to understand and improve both sides of his new discovery. His lab will try to learn every detail about just how his catalyst is making the oxygen. And he is going to work with his engineering colleagues at MIT to try to integrate his storage device into systems that he hopes one day will power homes and cars all day and all night. --- > [**http://v3.espacenet.com/textdoc?DB=EPODOC&IDX=US2003201161&F=0**](http://v3.espacenet.com/textdoc?DB=EPODOC&IDX=US2003201161&F=0) > > **US Patent # 6,863,781** > > **Process for Photocatalysis and > Two-Electron Mixed-Valence Complexes** > **( March 8, 2005 )** > > **Abstract ---** Embodiments for the invention include a > process for the production of hydrogen comprising a protic > solution, a photocatalyst capable of a two-electron reduction > of hydrogen ions; and a coproduct trap. The embodiment > includes exposing the reaction medium to radiation capable of > photoexciting the photocatalyst to produce hydrogen. The > protic solution may comprise at least one of hydrohalic acid, > a silane, and water, and the hydrohalic acid may be > hydrochloric acid, hydrogen bromide, hydrogen fluoride or > hydrogen iodide. The present application also describes novel > transition metal compounds. Embodiments of the compounds > include a compound comprising two transition metal atoms, > wherein the transition metal atoms are in a two-electron mixed > valence state and at least one transition metal is not > rhodium; and at least one ligand capable of stabilizing the > transition metal atom in a two-electron mixed valence state. > > Current U.S. Class: 204/157.52 ; 204/157.15 > Current International Class: B01J 31/18 (20060101); B01J > 31/16 (20060101); B01J 35/00 (20060101); C07F 9/00 (20060101); > C07F 9/24 (20060101); C01B 3/04 (20060101); C01B 3/00 > (20060101); C07F 15/00 (20060101); B01J 31/26 (20060101); B01J > 31/30 (20060101); C07C 001/00 (); C01B 003/00 () > *References Cited* [Referenced By] -- U.S. Patent > Documents : 5223634 June 1993 Gratzel et al. > > *Other References* > > MacQueen et al., "Competitive Hydrogen Production and > Emission Through the Photochemistry of Mixed-Metal Bimetallic > Complexes", Inorganic Chemistry (no month, 1990), vol. 29, No. > 12, pp. 2313-2320.\* . > Heyduk, A.F., Nocera D.G.: "Hydrogen produced from hydrohalic > acid solutions by a two-electron mixed valence photocatalyst" > Science, American Association for the Advancement of Science, > US., vol. 293, Aug. 31, 2001, pp. 1639-1641, XP002217879. . > Heyduk, A.F., Nocera D.G.: "Hydrido, halo, hydrido-halo > complexes of two-electron mixed valence diiridium cores" > Journal of the American Chemical Society American Chemical > Society, Washington, D.C., US, vol. 122, 2000, pp. 9415-9426 > Xp002217880, no month. . > Heyduk, A.F., Nocera D.G.: "A novel two-electron mixed-valence > Ir(II)-Ir(O) complex" Chemical Communications, Royal Society > of Chemistry, GB, 1999, pp. 1519-1520, XP002217881, no month.. > > **Description** > > **TECHNICAL FIELD** > > Embodiments of the present invention relate to photocatalytic > chemical processes. Embodiments of the present invention > relate to the production of hydrogen from a hydrohalic acid > solution using a homogenous photocatalyst. Embodiments of the > present invention also include novel two-electron > mixed-valence complexes. > > **DESCRIPTION** > > Photocatalytic production of chemical products offers an > inexpensive method of driving a chemical reaction toward the > production of molecules comprising more energy than the raw > materials. Photocatalysts having excitation energies that fall > within the spectrum of solar radiation at the surface of earth > are of particular interest. The potential of solar chemistry > in the generation of energy-rich molecules from inexpensive > energy-poor raw materials has been extensively researched. > Embodiments of the present invention comprise transition metal > complexes capable of mediating multielectron transformations. > These multielectron transformations allow activation of small > molecules. Embodiments of the present invention comprise > catalysts with a multinuclear core transition metal complex in > a two electron mixed valence state. The two-electron > mixed-valence state may mediate chemical processes, such as > atom transfer, bond activation, and substrate > functionalization, for example. > > The multicore transition metal complexes may be stabilized by > the chemical composition of the ligands coordinated with the > multinuclear transition metal core. For example, the > electronic and steric properties of bridging > bis(phosphine)amine ligands favor disproportionation of > valence-symmetric binuclear cores. Such properties in the > bis(difluorophosphine)methyl amine ("dfpma") ligand stabilizes > Rh.sup.0 --Rh.sup.II cores. The disproportionation of > embodiments of the present invention include new ligands to > stabilize two-electron mixed-valence complexes were developed > by manipulation of the stereo-electronic effects engendered by > phosphine and nitrogen functionalization. > > An embodiment of the present invention is a process having a > reaction medium comprising a protic solution, a photocatalyst > capable of a two-electron reduction of hydrogen ions, and a > coproduct trap. The reaction medium may be exposed to > radiation capable of photoexciting the photocatalyst to > produce hydrogen. The reaction medium may comprise any protic > solution, such as a hydrohalic acid of hydrochloric acid, > hydrogen bromide, hydrogen fluoride, and hydrogen iodide. A > coproduct is any compound or atom produced other than the > desired product, for example, the desired product may be > hydrogen. A coproduct trap is any material, such as an atom or > chemical compound, which may attach, react or bind with the > coproduct to prevent the coproduct from interfering with the > desired reaction. For example, the coproduct trap may be a > compound capable of bonding with a halogen atom, such as, for > example, tetrahydrofuran, dihydroanthracene, a silane, > isopropanal and 2,3 dimethylbutadiene. > > The photocatalyst of the present invention may be any > photocatalyst capable of a two electron reduction of hydrogen > ions and comprises a multinuclear transition metal core. An > embodiment of the photocatalyst of the present invention is a > multinuclear transition metal core which is capable of a two > electron reduction of hydrogen atoms. The photocatalyst may > also comprise a ligand that is capable of stabilizing a > two-electron mixed-valence state of the binuclear transition > metal core. > > A further embodiment of the present invention includes a > reaction medium comprising a protic solution; a photocatalyst > comprising a binuclear transition metal complex and a ligand > capable of supporting the photocatalyst in a two-electron > mixed-valence state; and a coproduct trap. The photocatalyst > may then be photoexcited to produce hydrogen from the reaction > medium. The ligand may be, for example, a diphosphazane ligand > or a ligand having a strongly .PI.-acidic phosphine group. > > Another embodiment of the present invention comprises a > process involving exciting at least two photocatalysts to an > active state wherein the photocatalysts comprise two rhodium > atoms; contacting the photocatalysts with hydrogen ions and > halogen ions of a hydrohalic acid solution, thereby producing > hydrogen and a photocatalyst in a mixed valence state > comprising halogen atoms; and irradiating the photocatalyst in > a mixed valence state to eliminate at least a portion of the > halogen atoms. The embodiment may include a hydrogen ion and a > halogen ion binding to the photocatalysts prior to reacting to > produce hydrogen and an unidentified photocatalytic > intermediate. It is theorized that the photocataltic > intermediate reacts with additional hydrogen ions and halogen > ions to form a photocatalyst comprising four halogen atoms and > additional hydrogen. The process may then be continued by > further radiation of the photocatalyst to eliminate the > halogen atoms and absorbing the halogen atoms in a > halogen-atom trap. Preferably, the photocatalyst is excited by > irradiation with sunlight. > > An additional embodiment of the present invention includes a > compound comprising two iridium atoms, wherein the iridium > atoms are in a two-electron mixed-valence state, and at least > one ligand. The iridium compound may be stabilized by at least > one ligand, such as, for example, a diphosphazane ligand. > > **BRIEF DESCRIPTION OF THE DRAWINGS** > > The features and advantages of embodiments of the present > invention may be better understood by reference to the > accompanying figures, in which: > > **FIG. 1(a)** is a thermal ellipsoid plot (50% > probability) for Rh.sub.2.sup.0,II (dfpma).sub.3 Cl.sub.2 > (PEt.sub.3) (1-PEt.sub.3) and FIG. 1(b) is a thermal ellipsoid > plot (50% probability) for Rh.sub.2.sup.0,II (dfpma).sub.3 > Br.sub.2 (PPh.sub.3) (2-PPh.sub.3), and wherein the hydrogen > atoms and solvent molecules have been omitted for clarity; > > **FIG. 2(a)-(d)** are the following NMR spectra of > dirhodium dfpma complexes: FIG. 2(a) is the .sup.19 F NMR of > Rh.sub.2.sup.II,II (dfpma).sub.3 Cl.sub.4 (4) in CDCl.sub.3 ; > FIG. 2(b) is the .sup.19 F{.sup.31 P} NMR spectra of > Rh.sub.2.sup.II,II (dfpma).sub.3 Cl.sub.4 (4) in CDCl.sub.3 ; > FIG. 2(c) is the .sup.19 F NMR of Rh.sub.2.sup.0,II > (dfpma).sub.3 Cl.sub.2 (PPh.sub.3) ("1-PPh.sub.3") in > CDCL.sub.3 ; and FIG 2(d) .sup.19 F {.sup.31 P} NMR spectra of > Rh.sub.2.sup.0,II (dfpma).sub.3 Cl.sub.2 (PPh.sub.3) > (1-PPh.sub.3) in CDCl.sub.3 (wherein the signals at -74 and > -68 ppm in spectra 2(b) and 2(d) are artifacts due to the > .sup.31 P decoupling pulse, and the insets in FIG. 2(a) and > FIG. 2(c) show the Neumann Projection structures of 4 and > 1-PPh.sub.3, respectively); > > **FIG. 3** is a thermal ellipsoid plot (50% probability) > for Rh.sub.2 (dmpma).sub.2 Cl.sub.2 (.mu.-CO).sub.2 (6) > wherein the hydrogen atoms have been omitted for clarity; > > **FIG. 4** is the thermal ellipsoid plot (50% > probability) for Rh.sub.2 (dppma).sub.2 Cl.sub.2 > (.mu.-CO).sub.2 (9) wherein the hydrogen atoms and a CH.sub.2 > Cl.sub.2 solvent molecule have been omitted and only the ipso > carbons of the phenyl ring are shown for clarity; > > **FIG. 5(a)** is the thermal ellipsoid plot (50% > probability) for Rh.sub.2 (dppma).sub.3 (CO).sub.2 (12) and **FIG. > 5(b)** is the thermal ellipsoid plot (50% probability) for > Rh.sub.2 (dppma).sub.2 Cl.sub.4 (CO).sub.2 (13) wherein the > hydrogen atoms and solvent molecules have been omitted and > only the ipso carbons of the phenyl ring are shown for > clarity; > > **FIG. 6** is a thermal ellipsoid plot (50% probability) > for Rh.sub.2.sup.0,II (tfepma).sub.3 Cl.sub.2 (CO) (16) > wherein for clarity, only the methylene carbons of the > CH.sub.2 CF.sub.3 groups are shown; > > **FIG. 7(a)** is a thermal ellipsoid plot (50% > probability) for syn-Rh.sub.2.sup.II,II (tfepma).sub.3 > Cl.sub.4 (19) and FIG. 17(b) is a thermal ellipsoid plot (50% > probability) for anti-Rh.sub.2.sup.II,II (tfepma).sub.3 > Cl.sub.4 (20), wherein the hydrogen atoms and solvent > molecules have been omitted for clarity; > > **FIG. 8** includes the solution absorption and > solid-state emission spectra of syn-Rh.sub.2.sup.II,II > (tfepma).sub.3 Cl.sub.4 (19) and anti-Rh.sub.2.sup.II,II > (tfepma).sub.3 Cl.sub.4 (20); > > **FIG. 9** is a thermal ellipsoid plot for > Rh.sub.2.sup.0,II (tfepma).sub.3 Cl.sub.2 (21) from > preliminary X-ray data wherein for clarity, only the methylene > carbons of the CH.sub.2 CF.sub.3 groups are shown; > > **FIG. 10** is the thermal ellipsoid plot (50% > probability) for Rh.sub.2.sup.0,II (dfpx).sub.3 Br.sub.2 > (PPh.sub.3) (22) wherein the solvent molecules and hydrogen > atoms have been omitted for clarity; > > **FIG. 11** is a thermal ellipsoid plot (50% probability) > for [ClRh(tfepx)].sub.2 (.mu.-tfepx) (23) wherein for clarity, > only the methylene carbons of the CH.sub.2 CF.sub.3 groups are > shown; > > **FIG. 12** is a thermal ellipsoid plot (50% probability) > of Ir.sub.2.sup.I,III (dfpma).sub.2 Cl.sub.4 (cod) (1) wherein > hydrogen atoms have been omitted for clarity; > > **FIG. 13** depicts the molecular structure of > Ir.sub.2.sup.I,III (dppma).sub.3 Cl.sub.2 (2), taken from > preliminary X-ray crystal structure data wherein for clarity, > hydrogen atoms have been omitted and only the ipso carbons of > the phenyl rings are shown; > > **FIG. 14** is a thermal ellipsoid plot (50% probability) > of Ir.sub.2.sup.0,II (tfepma).sub.3 Cl.sub.2 (3) wherein for > clarity, hydrogen atoms have been omitted and only the > methylene carbons of the trifluoroethyl groups are shown; > > **FIG. 15** includes .sup.31 P and partial .sup.1 H NMR > spectra of Ir.sub.2.sup.0,II (tfepma).sub.2 Cl.sub.2 (3) in > d.sup.8 -THF at wherein FIG. 15(a) is at 20.degree. C. and > FIG. 15(b) is at -80.degree. C.; > > **FIG. 16(a)** is a thermal ellipsoid plot (50% > probability) of Ir.sub.2.sup.0,II (tfepma).sub.3 Cl.sub.2 > (MeCN) (4) and FIG. 16(b) is the thermal ellipsoid plot (50% > probability) of Ir.sub.2.sup.0,II (tfepma).sub.3 Cl.sub.2 > (CN.sup.t Bu) (5-CN.sup.t Bu) wherein for clarity, hydrogen > atoms have been omitted and only the methylene carbons of the > trifluoroethyl groups are shown; > > **FIG. 17** is a thermal ellipsoid plot (50% probability) > of the Ir.sub.2.sup.0,II (tfepma).sub.3 (MeCN).sub.3.sup.2+ > (6) cation wherein for clarity, hydrogen atoms and two > PF.sub.6.sup.- anions have been omitted and only the methylene > carbons of the trifluoroethyl groups are shown; > > **FIG. 18(a)** is a thermal ellipsoid plot (50% > probability) of Ir.sub.2.sup.I,III (tfepma).sub.3 Cl.sub.4 > (7), and **FIG. 18(b)** is a thermal ellipsoid plot (50% > probability) of Ir.sub.2.sup.II,II (tfepma).sub.2 Cl.sub.4 > (MeCN).sub.2 (8), wherein for clarity, hydrogen atoms have > been omitted and only the methylene carbons of the > trifluoroethyl groups are shown; > > **FIG. 19** is a thermal ellipsoid plot (50% probability) > of Ir.sub.2.sup.I,III (tfepma).sub.2 HCl.sub.3 (10) wherein > for clarity, hydrogen atoms have been omitted and only the > methylene carbons of the trifluoroethyl groups are shown; > > **FIG. 20** shows .sup.1 H NMR spectra of (a) the > equatorial isomer of Ir.sub.2.sup.I,III (tfepma).sub.3 > HCl.sub.3 (10), (b) the axial isomer of Ir.sub.2.sup.I,III > (tfepma).sub.3 HCl.sub.3 (9), (c Ir.sub.2.sup.I,III > (tfepma).sub.3 HCl.sub.2 (MeCN)][PF.sub.6 ].sub.2 (11), and > (d) Ir.sub.2.sup.I,III (tfepma).sub.3 H.sub.2 Cl.sub.2 (12), > wherein the spectra were acquired at room temperature in > CD.sub.3 CN; > > **FIG. 21** is a thermal ellipsoid plot (50% probability) > of Ir.sub.2.sup.I,III (tfepma).sub.2 H.sub.2 Cl.sub.2 (12) > wherein for clarity, hydrogen atoms have been omitted and only > the methylene carbons of the trifluoroethyl groups are shown; > > **FIG. 22** is a pictorial representation of the HOMO and > LUMO of Ir.sub.2 (PH.sub.3).sub.6 Cl.sub.2 as calculated by > the extended Huckel program YAeHMOP; > > **FIG. 23** is a qualitative potential energy diagram for > MeCN exchange from [Ir.sub.2.sup.I,III (tfepma).sub.3 > HCl.sub.2 (MeCN)].sup.2+ (11), illustrating the origin of the > inverse isotope effect; > > **FIG. 24** depicts molecular structures of the homologous > series of binuclear rhodium complexes wherein FIG. 24(a) > depicts Rh.sub.2.sup.0,0 (dfpma).sub.3 (PF.sub.3).sub.2, FIG. > 24(b) depicts Rh.sub.2.sup.0,II (dfpma).sub.3 Cl.sub.2 > (PF.sub.3), and FIG. 24(c) depicts Rh.sub.2.sup.II,II > (dfpma).sub.3 Cl.sub.4 ; > > **FIG. 25(a)** is an electronic absorption spectrum of > Rh.sub.2.sup.0,0 (dfpma).sub.3 (.eta..sup.1 -dfpma).sub.2, > FIG. 25(b) is electronic absorption spectra of > Rh.sub.2.sup.0,II (dfpma).sub.3 Cl.sub.2 (.eta..sup.1 -dfpma) > and Rh.sub.2.sup.0,II (dfpma).sub.3 Br.sub.2 (.eta..sup.1 > -dfpma), and FIG. 25(c) is electronic absorption spectra of > Rh.sub.2.sup.II,II (dfpma).sub.3 Cl.sub.4 and > Rh.sub.2.sup.II,II (dfpma).sub.3 Br.sub.4 in THF at room > temperature; > > **FIG. 26** is a plot of the energy maximum of the > d.sigma..fwdarw.d.sigma.\* transition of Rh.sub.2.sup.0,0 > (dfpma).sub.3 (L).sub.2 (L=PEt.sub.3, P(OMe).sub.3, P(O.sup.i > Pr).sub.3, PPh.sub.3, and PF.sub.3) vs. Tolman electronic > parameter; > > **FIG. 27** is a graph depicting spectral changes in the > electronic absorption spectrum during the photolysis > (.lambda..sub.exc >335 nm) of Rh.sub.2.sup.II,II > (dfpma).sub.3 Br.sub.4 in THF and in the presence of 250 > equiv. of dfpma at 0.degree. C. wherein the spectra were > recorded over the span of 2 hours; > > **FIG. 28** is the .sup.19 F NMR (C.sub.6 D.sub.6) > spectrum of the photoproduct obtained from the irradiation > (.lambda..sub.exc.gtoreq.335 nm) of Rh.sub.2.sup.II,II > (dfpma).sub.3 Br.sub.4 in the presence of excess dfpma in THF > at 0.degree. C.; > > **FIG. 29(a)** is a graph depicting the spectral changes > in the electronic absorption spectrum during the photolysis > (.lambda..sub.exc.gtoreq.436 nm) of Rh.sub.2.sup.II,II > (dfpma).sub.3 Br.sub.4 in THF and in the presence of 250 > equiv. of dfpma at 0.degree. C. wherein the spectra were > recorded over the span of 15 min. and the photolysis was > terminated when the 358-nm absorption was maximized, and FIG. > 29(b) is a graph depicting spectral changes associated with > continued irradiation of the solution resulting from the > photolysis depicted in FIG. 29(a) with higher energy light > (.lambda..sub.exc.gtoreq.335 nm) wherein spectra were recorded > over the span of 3 hours; > > **FIG. 30** is a graph depicting the spectral changes > associated with the monochromatic irradiation > (.lambda..sub.exc =335 nm) of Rh.sub.2.sup.II,II (dfpma).sub.3 > Br.sub.4 in THF at 0.degree. C.; > > **FIG. 31** is a graph of the .sup.1 H NMR (CDCl.sub.3) > spectrum of the photoproduct obtained from the irradiation > (.lambda..sub.exc >335 nm) of Rh.sub.2.sup.II,II > (dfpma).sub.3 Br.sub.4 in the presence of 4.3 equiv. of > 2,6-lutidine and 2.5 equiv. of PPh.sub.3 in THF at 0.degree. > C., showing the methyl resonances of the Rh.sub.2.sup.0,II and > Rh.sub.2.sup.0,0 photoproducts and the high frequency > resonance for protonated 2,6-lutidine; > > **FIG. 32(a)** depicts the HOMO and LUMO for > Rh.sub.2.sup.0,0 (dfpma).sub.3 (PF.sub.3).sub.2, **FIG. > 32(b)** depicts the HOMO and LUMO for Rh.sub.2.sup.0,II > (dfpma).sub.3 Br.sub.2 (PF.sub.3), and **FIG. 32(c)** > depicts the HOMO and LUMO for Rh.sub.2.sup.II,II (dfpma).sub.3 > Br.sub.4 as determined at the extended Huckel level using > YAeHMOP; > > **FIG. 33** is a graph of the UV-Vis spectral changes > associated with the irradiation > (300.ltoreq..lambda..sub.exc.ltoreq.400 nm) of > Rh.sub.2.sup.0,0 (dfpma).sub.3 (CN.sup.t Bu).sub.2 in CH.sub.2 > Cl.sub.2 containing 0.1 M HBr wherein the spectra were > acquired at t.sub.irr =0, 10, 20, 30, 50, 70, 90, 120 and 180 > min.; > > **FIG. 34(a)** is a graph of UV-Vis absorption changes > associated with the photolysis (.lambda..sub.exc.gtoreq.335 > nm) of Rh.sub.2.sup.0,0 (dfpma).sub.3 (CO)(PPh.sub.3) in > CH.sub.2 Cl.sub.2 solution containing 0.1 M HCl, and FIG. > 34(b) is a graph of UV-Vis absorption changes associated with > the photolysis (.lambda..sub.exc.gtoreq.335 nm) of > Rh.sub.2.sup.0,0 (dfpma).sub.3 (CO)(PPh.sub.3) in CH.sub.2 > Cl.sub.2 solution containing 0.1 M HBr, wherein the spectra of > FIG. 34(a) were acquired at t.sub.irr =0, 2, 5, 7, 10, 15, 20 > and 25 min. and the spectra of FIG. 34(b) were acquired at > t.sub.irr =0, 2, 5, 7, 10, 12, 15, 20, 25 and 30 min.; > > **FIG. 35(a)** is a graph of the changes in electronic > absorption spectrum during monochromatic UV photolysis > (.lambda..sub.exc =335 nm) of Rh2(dfpma).sub.3 (CO)(PPh.sub.3) > in 0.1 M HCl/THF solution at 20.degree. C. wherein the spectra > were collected at t.sub.irr =0, 10, 20, 30, 40, 50, 60 and 90 > min., and FIG. 35(b) is a graph of changes in the electronic > absorption of the continued photolysis of the sample in FIG. > 35(a) using white light (.lambda..sub.exc.gtoreq.335 nm) > wherein spectra of FIG. 35(b) were acquired at t.sub.irr =5, > 10, 15 and 20 min. after the last spectrum of FIG. 35(a); > > **FIG. 36** is a graph of UV-Vis absorption changes > associated with photolysis (.lambda..sub.exc.gtoreq.365 nm) of > Rh.sub.2.sup.0,II (dfpma).sub.3 Br.sub.2 (CN.sup.t Bu) in > CH.sub.2 Cl.sub.2 containing 0.1 M HBr wherein the spectra > were acquired at t.sub.irr =0, 5, 10, 20, 30, 40, 50 and 60 > min.; > > **FIG. 37(a)** is a plot of total hydrogen collected as a > function of time for UV-Vis white light irradiation > (.lambda..sub.exc.gtoreq.335 nm) of Rh.sub.2.sup.0,II > (dfpma).sub.3 Cl.sub.2 (PPh.sub.3) in 0.1 M HCl/THF solution > at 20.degree. C., and FIG. 37(b) is a graph of UV-Vis > absorption spectra of the sample of FIG. 37(a) indicating the > decay of the Rh.sub.2.sup.0,II (dfpma).sub.3 Cl.sub.2 > (PPh.sub.3) catalyst during irradiation; > > **FIG. 38** is a plot of predicted H.sub.2, D.sub.2, and > HD production based on irradiation of Rh.sub.2.sup.0,II > (dfpma).sub.3 Cl.sub.2 (PPh.sub.3) in d.sup.8 -THF initially > containing 10 equiv. of HCl; > > **FIG. 39(a)** is a graph of changes in electronic > absorption spectrum during the monochromatic UV photolysis > (.lambda..sub.exc =335 nm) of Rh.sub.2.sup.0,II (dfpma).sub.3 > Cl.sub.2 (PPh.sub.3) in 0.1 M HCl/THF solution at 20.degree. > C. wherein the spectra were acquired at t.sub.irr =0, 10, 20, > 30 and 40 min., and FIG. 39(b) is a graph of spectral changes > for the solution in FIG. 39(a) kept in the dark for five > minutes and wherein the spectra were recorded 5 and 10 minutes > after the last spectrum of FIG. 39(a); > > **FIG. 40** is a graph of absorption spectra recorded > during photolysis (300 nm.ltoreq..lambda..sub.exc <400 nm) > of Rh.sub.2.sup.II,II (dfpma).sub.3 Br.sub.4 at 20.degree. C. > in THF solution containing 0.1 M HCl wherein the spectra were > acquired at t.sub.irr =0, 1, 2, 3, 4 and 5 min.; > > **FIG. 41(a)** is a .sup.19 F NMR spectrum for the > photoreaction of Rh.sub.2.sup.II,II (dfpma).sub.3 Cl.sub.4 > with HCl in d.sup.8 -THF, FIG. 41(b) is .sup.19 F NMR spectrum > for the photoreaction of Rh.sub.2.sup.II,II (dfpma).sub.3 > CO.sub.4 with HCl in d.sup.8 -THF after the addition of 0.2 M > HCl, FIG. 41(c) is a .sup.19 F NMR spectrum for the > photoreaction of Rh.sub.2.sup.II,II (dfpma).sub.3 Cl.sub.4 > with HCl in d.sup.8 -THF after addition of 0.2 M HCl and > irradiation (300 nm.ltoreq..lambda..ltoreq.400 nm) for 3 hr., > FIG. 41(d) is a .sup.19 F NMR spectrum for the photoreaction > of Rh.sub.2.sup.II,II (dfpma).sub.3 Cl.sub.4 with HCl in > d.sup.8 -THF after addition of 0.2 M HCl and irradiation (300 > nm.ltoreq..lambda..ltoreq.400 nm) for 18 hr., and FIG. 41(e) > is a .sup.19 F NMR spectrum of independently prepared > Rh.sub.2.sup.0,II (dfpma).sub.3 Cl.sub.2 in d.sup.8 -THF; and > > **FIG. 42** is a .sup.19 F NMR spectrum of > Rh.sub.2.sup.II,II (dfpma).sub.3 Cl.sub.2 Br.sub.2 in d.sup.8 > -THF from the reaction of Rh.sub.2.sup.0,II (dfpma).sub.3 > Cl.sub.2 with bromine. > > **CHARACTERIZATION OF LIGAND EFFECTS ON BINUCLEAR CORES** > > Research in inorganic chemistry includes preparation of new > molecules to mediate multi-electron transformations. Such > transformations assist in the activation of small molecules > and allow more controlled reactivity of small molecules. > Excited-state valence disproportionation of symmetric > quadruply-bonded dimers may be observed by transient > spectroscopic techniques. The present inventors developed > complexes in which two-electron mixed valency could be > incorporated into ground state configurations of the > transition metal complexes. > > Preparation of two-electron mixed-valence compounds is > accomplished through the internal disproportionation of > valence symmetric metal complexes. The inventors envisioned > three different approaches to internal disproportionation, > depicted in Scheme 1, were envisioned to effect this reaction > and determine ligands which are capable of stabilizing a two > electron mixed valence state of a multinuclear transition > metal core, and more specifically a binuclear transition metal > core. In Case I of Scheme 1, an asymmetric ligand is > constructed from disparate electron withdrawing and electron > donating fragments. In such a case, the electron-withdrawing > group may stabilize low-valent metal centers whereas the > electron-donating group may stabilize high-valent metal > centers such as an oxypiridinate ligand. Synthetically, > disporoportionation by the method of Case I is challenging for > at least two reasons. General strategies for the preparation > of simple asymmetric bridging ligands utilize a complex > multi-step procedure. Secondly, it is difficult to control the > linkage isomerism of ligands that possess inherent asymmetry > such as oxypyridinate ligands. Typically, two asymmetric > ligands add to a binuclear metal core in a head-to-tail > fashion, ##STR1## > > yielding a net symmetric electronic environment. > > Preparation of two-electron mixed-valence complexes may also > be accomplished by induced asymmetry of the bridging ligand > framework. See Cases II and III in Scheme 1. A bridging ligand > between the metal centers may be used to create an induced > asymmetric environment suitable for late transition metals. > For example, a three atom bridging ligand, with .pi.-acid > groups to coordinate the metal centers and a Lewis-basic > bridgehead atom, may induce an asymmetric environment via > directional lone pair donation from the bridgehead atom to one > .pi.-acid group. In another embodiment, a ligand composed of > hard .pi.-donating coordination groups and a Lewis .pi.-acidic > bridgehead atom may lead to valence disproportionation in > high-valent early transition metal complexes. Embodiments of > the present invention may comprise any ligand capable of > stabilizing a mixed valence state in the binuclear transition > metal core. An embodiment of the present invention of a Case > II ligand may be a ligand of the formula, RN(PY.sub.2).sub.2, > wherein the ligand comprises a phosphazane group, P--N--P. The > Y groups may be independently selected and may be any > combination of groups which give at least one phosphorous atom > of the phosphazane group strong .pi.-acid characteristics, > preferably both phosphorous atoms have strong .pi.-acid > characteristics. The Y groups may not all be identical atoms > or groups and all the Y's need not contribute to the > .pi.-acidity of the coordinating atoms. The Y group may be, > for example, but not limited to, at least one of halogen, > fluorine, chlorine, halogenated alkanes, halogenated alkenes, > aryl substituted with electron withdrawing groups, and > alcohols. The ligands have strong .pi.-acid characteristics, > if at least a portion of the transition metal complexes are > present in the two electron mixed valence state. As the > strength of the .pi.-acidity of the attached ligands of > binuclear transition metal complexes increase, the complexes > will form an equilibrium wherein at least a portion of the > complexes will exist in the two electron mixed valence state. > These complexes will be photocatalytically active in the > present invention. As the pi-acidity of the ligands increases > the equilibrium of the complexes will shift toward a state in > which all of the complexes are in the two electron mixed > valence state. Additionally, the Figures and the Examples use > three ligands to stabilize the mixed valence state of the > photocatalyst, however, it is contemplated that a single > ligand may be prepared comprising the characteristics > necessary to stabilize the mixed valence state. The single > ligand may be, for example, a multidentate ligand which > comprises the electronic and steric properties described > above. Such as, for example, the ligands described herein > connected through the R group. > > The R attached to a nitrogen atom of the phosphazane group > may be any atom or group which allows participation of a lone > pair of electrons to participate in .pi.-bonding with the > phosporus atoms. The R attached to a nitrogen atom may be, for > example, but not limited to, a substituted or unsubstituted > C.sub.1 -C.sub.10 alkyl groups, methyl, ethyl, propyl, butyl, > pentyl, hydrogen and a substituted phenyl, wherein the alkyl > group may be a branched or an unbranched alkyl group. > > A Case II ligand may be prepared by the reaction of PCl.sub.3 > with primary amines which leads to the formation of a > bis(dichlorophosphine)amine fragment as shown in Scheme 2. > This reaction has been observed for a variety of starting > materials, ##STR2## > > including simple alkyl amines and substituted aniline > derivatives. Reaction with Grignard and alkyl lithium reagents > affords alkyl phosphines; rapid reaction with alcohols in the > presence of tertiary amine bases gives the corresponding > phosphite derivatives. Finally, metathesis with antimony > trifluoride provides a high-yield route to the > bis(difluorophosphine)amine derivative, which possess more > .pi.-acidic phosphines of the PNP-type ligands. These > synthetic routes are versatile. Electronic and steric > parameters of the ligand can be finely manipulated by > functionalization at both the nitrogen and phosphorus centers. > > The ligands as described above may be used to stabilize > internal disproportionation on any binuclear transition metal > transition metal complex. The core may comprise different > transition metals. The transition metals comprising the > binuclear core may be independently selected from, for > example, Rh, Ir, Cu, Fe, Ru, Cr, Mo, W, Co, Re, No, Mn, V, Nb, > Ta, Zn, Au, Pd, Pt and Ag. > > The chemistry of dfpma with Group VI metals was determined > shortly after its preparation. Three ligands were observed to > span d.sup.9 --d.sup.9 metal cores, as observed for > Co.sub.2.sup.0,0 (dfpma).sub.3 (CO).sub.2. UV-irradiation of > this complex in alkane solutions containing phosphine ligands > leads to carbonyl loss and coordination of the phosphine in > the axial site. An extensive redox chemistry was explored for > Co.sub.2.sup.0,0 (dfpma).sub.3 (CO).sub.2. For example, > oxidation with Br.sub.2 gave a four electron oxidized species, > Co.sub.2.sup.II,II (dfpma).sub.3 Br.sub.4, whereas > electrochemical reduction gave a two-electron reduced anionic > complex, [Co.sub.2.sup.-I,-I (dfpma).sub.3 (CO).sub.2 ]. > > An embodiment of the present invention may also comprise a > Case III ligand. A nonlimiting example of a Case III ligand is > one of the formula, RN(BY.sub.1), wherein the R is as > described above and the Y.sub.1 may be independently selected > and may be any atom or group which contributes to hard > .pi.-donating characteristic of the coordination groups. > Embodiments of the present invention may comprise any ligand > capable of causing internal disproportionation of the > multinuclear core and capable of stabilizing a mixed valence > state. > > Unless otherwise indicated, all numbers expressing quantities > of ingredients, time, temperatures, and so forth used in the > present specification and claims are to be understood as being > modified in all instances by the term "about." Accordingly, > unless indicated to the contrary, the numerical parameters set > forth in the following specification and claims are > approximations that may vary depending upon the desired > properties sought to be obtained by the present invention. At > the very least, and not as an attempt to limit the application > of the doctrine of equivalents to the scope ##STR3## > > of the claims, each numerical parameter should at least be > construed in light of the number of reported significant > digits and by applying ordinary rounding techniques. > > Notwithstanding that the numerical ranges and parameters > setting forth the broad scope of the invention are > approximations, the numerical values set forth in the specific > examples are reported as precisely as possible. Any numerical > value, however, may inherently contain certain errors > necessarily resulting from the standard deviation found in > their respective testing measurements. > > To extend the two-electron mixed-valence chemistry of these > ligands, the steric and electronic characteristics of the PNP > ligands framework that favor the valence disproportionation of > symmetric binuclear cores was explored. Embodiments described > herein suggest that the induced asymmetry of Case II in Scheme > 1 is effective in promoting the formation of two-electron > mixed-valence complexes. The electronic and the steric > parameters of the bridging PNP ligand may be controlled to > favor valence disproportionation resulting in two-electron > mixed-valence species. > > The reaction of dfpma with the rhodium(I) dimers, such as, > [XRh.sup.I (PF.sub.3).sub.2 ].sub.2 or XRhP.sub.4, for > example, where X=Cl, Br, I, alkyl, triflates, hydrides, and > other monodentate anionic ligands, produces two-electron > mixed-valence complexes Rh.sub.2.sup.0,II (dfpma).sub.3 > X.sub.2 (L), in which L may be, for example, PF.sub.3 or a > monodentate dfpma ligand, depending on reaction stoichiometry, > with yields of ca. 25%. A more reliable and general path into > the rhodium complexes was sought from [XRh.sup.I > (cyclooctadiene)].sub.2 ("[XRh.sup.I (cod)].sub.2 ") starting > materials. Rh.sub.2.sup.0,II (dfpma).sub.3 X.sub.2 (L) was > therefore prepared by the addition of three equivalents of > dfpma and one equivalent of a two electron donor ligand (for > example, P(OR).sub.3, PR.sub.3, and CNR) to benzene solutions > of [XRh.sup.I (cod)].sub.2, as depicted in Scheme 3. Stirring > at room temperature resulted in precipitation of most of the > product over the span of 24 hr. Concentration by solvent > distillation followed by the addition of pentane typically > provided high yields of Rh.sub.2.sup.0,II (dfpma).sub.3 > X.sub.2 (L) (X=Cl ("1-L" in Scheme 3), Br ("2-L" in Scheme 3); > L=P(OR).sub.3, PR.sub.3, CNR). In the case of the carbonyl > adduct, Rh.sub.2.sup.0,II (dfpma).sub.3 Cl.sub.2 (CO) > ("1-CO"), dfpma was reacted with the carbonyl dimer > [ClRh(CO).sub.2 ].sub.2 in CH.sub.2 Cl.sub.2 rather than > benzene. The CH.sub.2 Cl.sub.2 was then removed and the > residue washed with 1:5 benzene/pentane to afford an orange > powder that was dried briefly in vacuo. 1-CO left under vacuum > for extended periods of time (a few hours) changed color from > orange to green-blue. This color change was accompanied by > disappearance of the carbonyl resonance in the IR spectrum, > indicating loss of an axial CO ligand. > > The solid-state structures for several of the two-electron > mixed-valence complexes have been determined from single > crystal X-ray diffraction data. Thermal ellipsoid plots for > two derivatives, Rh.sub.2.sup.0,II (dfpma).sub.3 Cl.sub.2 > (PEt.sub.3) ("1-PEt.sub.3 ") and Rh.sub.2.sup.0,II > (dfpma).sub.3 Br.sub.2 (PPh.sub.3) ("2-PPh.sub.3 "), are shown > in FIGS. 1(a) and (b). Thermal ellipsoid plots are ball and > stick type illustrations of structures of chemical compounds. > The 50% probability thermal motion ellipsoids of the atomic > sites are derived from anisotropic temperature factor > parameters to indicate the thermal motion of the atom 50% of > the time. Tables 1 and 2 list a few metrical parameters of > complexes comprising the dirhodium cores. The dfpma bond > distances of these derivatives indicates stabilization of the > two-electron mixed-valence dirhodium core. For example, > contraction of the N--P bond distance is observed for the > phosphorus atoms coordinated to the high-valent Rh.sup.II (avg > N--P.sup.Rh(II) =1.634(4) .ANG. for 1-PEt.sub.3 and > 1.633(6.ANG. for 2-PPh.sub.3) center, suggesting, but not > meant to limit the present invention, that the nitrogen lone > pair moderates the electronic properties of the .pi.-acid > PF.sub.2 groups. A longer N--P bond distance is observed for > the phosphorus coordinated to the Rh.sup.0 (avg N--P.sup.Rh(0) > =1.659(4) .ANG. for 1-PEt.sub.3 and 1.684(5) .ANG. for > 2-PPh.sub.3), consistent with a mechanism theory that there is > little donation of the nitrogen lone pair to the PF.sub.2 > group coordinated to the low-valent Rh.sup.0 center of the > complex. > > TABLE 1 N--P bond lengths (.ANG.) of the bridging dfpma > ligands of Rh.sub.2.sup.0,II (dfpma).sub.3 Cl.sub.2 > (PEt.sub.3) (1-PEt.sub.3) and Rh.sub.2.sup.0,II (dfpma).sub.3 > Br.sub.2 (PPh.sub.3) (2-PPh.sub.3). N--P Bond Distances in > 1-PE.sub.t3 (.ANG.) P(1)-N(1) 1.663(4) P(2)-N(1) 1.633(4) > P(3)-N(2) 1.670(4) P(4)-N(2) 1.633(4) P(5)-N(3) 1.675(4) > P(6)-N(3) 1.636(5) N--P Bond Distances in 2-PPh.sub.3 (.ANG.) > P(1)-N(1) 1.684(5) P(2)-N(1) 1.630(6) P(3)-N(2) 1.684(5) > P(4)-N(2) 1.634(6) P(5)-N(3) 1.685(6) P(6)-N(3) 1.636(6) > > Other metrical parameters of interest include the bond > distances of the dirhodium core for various Rh.sub.2.sup.0,II > (dfpma).sub.3 X.sub.2 (L) derivatives. Lengthening of the > dirhodium core bond length indicates stability in the > mixed-valence structure. Several factors lead to structural > perturbations along the Rh.sup.0 --Rh.sup.II axis, including, > but not limited to, axial ligand coordination to the Rh.sup.0 > center and halogen coordination to the Rh.sup.II center. The > metrical data in Table 2 for selected Rh.sub.2.sup.0,II > complexes gives insight into the effects of each of these > substitutions. A lengthening of the Rh.sup.0 --Rh.sup.II bond > distance occurs upon phosphine substitution. Exchange of an > axial PF.sub.3 in Rh.sup.0,II (dfpma).sub.3 > (Cl.sub.2)(PF.sub.3)("1-PF.sub.3 ") for PEt.sub.3 to form > Rh.sup.0,II (dfpma).sub.3 (Cl.sub.2) (PEt.sub.3)("1-PEt.sub.3 > ") results in a 0.0405 .ANG. increase in the Rh.sup.0 > --Rh.sup.II separation; similarly, exchange of an axial > .eta..sup.1 -dfpma for PPh.sub.3 in Rh.sub.2.sup.0,II > (dfpma).sub.3 Br.sub.2 (.eta..sup.1 -dfpma) ("2-(.eta..sup.1 > -dfpma)") and 2-PPh.sub.3 results in a 0.0403 .ANG. increase > in the Rh.sup.0 --Rh.sup.II separation. Spectroscopic studies > presented herein indicate that PF.sub.3 and .eta..sup.1 -dfpma > exert similar stereo-electronic influence on the dirhodium > core, permitting a comparison of the ligand effect of > 1-PF.sub.3 with 2-(.eta..sup.1 -dfpma). Substitution of > bromide for chloride in complexes with these .pi.-acidic axial > phosphines results in a lengthening of the Rh.sup.0 > --Rh.sup.II bond by 0.013 .ANG.. The magnitude of the > perturbation exerted by halogen and phosphine substitution on > the Rh.sup.0 --Rh.sup.II bond distance follows directly from > the relative donor abilities of each axial ligand. Whereas > exchange of bromide for chloride at the axial Rh.sup.II > position results in only a small change in .sigma. donor > ability, PEt.sub.3 and PPh.sub.3 are significantly better > .sigma. donors than PF.sub.3 and dfpma, and accordingly weaken > the metal-metal interaction to a greater extent. > > TABLE 2 Rh.sup.0 --Rh.sup.II bond lengths (.ANG.) for > Rh.sub.2.sup.0,II (dfpma).sub.3 X.sub.2 (L) (X = Cl (1-L), X = > Br (2-L)). Bond Distances (.ANG.) 2-(.eta.1- 1-PF3a dfpma)b > 1-PEt3 2-PPh3 Rh(1)-Rh(2) 2.785(1) 2.798(2) 2.8255(5) > 2.8383(9) Rh(1)-P(1) 2.254(2) 2.246(7) 2.2342(13) 2.238(2) > Rh(1)-P(3) 2.209(2) 2.229(7) 2.1906(13) 2.202(2) Rh(1)-P(5) > 2.248(2) 2.243(6) 2.2228(13) 2.259(2) Rh(1)-P(7) 2.168(2) > 2.203(6) 2.3277(13) 2.335(2) Rh(2)-X(1) 2.431(2) 2.579(3) > 2.4530(12) 2.6066(10) Rh(2)-X(2) 2.385(2) 2.524(4) 2.3905(12) > 2.5020(11) Rh(2)-P(2) 2.251(2) 2.241(7) 2.2434(13) 2.254(2) > Rh(2)-P(4) 2.183(2) 2.185(7) 2.1610(13) 2.184(2) Rh(2)-P(6) > 2.258(2) 2.247(7) 2.2420(14) 2.249(2) > > The preparation of two-electron reduced binuclear rhodium > complexes was achieved from [XRh(cod)].sub.2 starting > materials. Treatment of [CIRh(cod)].sub.2 with three > equivalents of dfpma, followed by two equivalents each of > cobaltocene and a two-electron donor ligand resulted in the > formation of binuclear rhodium complexes of the general > formulation Rh.sub.2.sup.0,0 (dfpma).sub.3 (L).sub.2 (3-L > where L may be PR.sub.3, P(OR).sub.3, CNR for example), which > are structurally analogous to Co.sub.2 (dfpma).sub.3 (L).sub.2 > (Scheme 4). The coordination environment is characterized by > trigonal bipyramidal Rh.sup.0 centers. A formal metal-metal > bond is supported by three bridging dfpma ligands; the > PF.sub.2 groups of these bridging ligands define the > equatorial plane of each Rh.sup.0 center. The axial position, > trans to the metal-metal bond is capped by a donor ligand, > electron accepting axial ligands such as, for example, > PF.sub.3, phosphites or isonitriles impart substantial > stability, and aryl and alkyl phosphines continuing complexes > have been prepared as well. The stability of the reduced > species is illustrated by sublimation of Rh.sub.2.sup.0,0 > (dfpma).sub.3 (PF.sub.3).sub.2 ("3-PF.sub.3 ") and > Rh.sub.2.sup.0,0 (dfpma).sub.3 (72 .sup.1 -dfpma).sub.2 > ("3-(.eta..sup.1 -dfpma)") under vacuum at 110.degree. C. > > The two-electron oxidized rhodium dimers may be prepared from > [XRh(cod)].sub.2 by the addition of three equivalents of dfpma > and five equivalents of PhICl.sub.2 or Br.sub.2 (Scheme 5). > The excess oxidant may be required to drive the reaction to > completion, since coordination of the dfpma resulted in the > production of free 1,5-cyclooctadiene, ##STR4## ##STR5## > > which in turn consumed the halogen oxidant. Use of excess > oxidant afforded pure Rh.sub.2.sup.II,II (dfpma).sub.3 X.sub.4 > (X=Cl (4), Br (5)) in yields of greater then 90%. The oxidized > Rh.sub.2.sup.II,II (dfpma).sub.3 X.sub.4 species comprises > octahedral Rh.sup.II centers connected by a metal-metal bond. > Three dfpma ligands maintain a bridging coordination mode, and > halogen ligands occupy axial and equatorial portions on each > metal center. > > In general, the .sup.1 H and .sup.19 F NMR spectra are useful > for characterizing the complexes, however due to excessively > broad peaks in the output, .sup.31 P NMR cannot be used to > probe the dfpma backbone. The dfpma complexes were not > fluxional on the NMR time scale. The reduced complexes, > Rh.sub.2.sup.0,0 (dfpma).sub.3 L.sub.2 (3-L), which display > D.sub.3d symmetry in solution, show the simplest NMR patterns; > .sup.1 H and .sup.19 F NMR data for 3-CO, 3-PPh.sub.3, > 3-CN.sup.t Bu, 3-PF.sub.3 and 3-(72 .sup.1 -dfpma) are > presented in Table 3. In addition to resonances for the axial > L ligands, a singlet, the electronic state in which the total > spin angular momentum is zero, is observed for the methyl > groups of the bridging dfpma ligands in the 2-3 ppm region. > One resonance is observed for the dfpma ligands near -40 ppm > in the .sup.19 F NMR spectrum, and is easily identified by a > strong .vertline..sup.1 J.sub.PF +.sup.3 J.sub.PF.vertline. of > 1110-1120 Hz. > > TABLE 3 .sup.1 H and .sup.19 F NMR data for Rh.sub.2.sup.0,0 > (dfpma).sub.3 L.sub.2 (3-L; L = CO, PPh.sub.3, CN.sup.t Bu, > PF.sub.3 and .eta..sup.1 -dfpma). Spectra were acquired in > C.sub.6 D.sub.6 except as noted. Compound .sup.1 > H(.delta./ppm) .sup.19 F(.delta./ppm).sup.a 3-CO 2.17(s) > -40.31(d, 1116Hz) 3-PPh.sub.3.sup.b 2.68(s, 9H) -43.18(d, > 1113Hz) 7.45(m, 30H) 3-CN.sup.t Bu 0.956(s, 18H) -40.53(d, > 1083Hz) 2.58(s, 9H) 3-PF.sub.3 2.12(s) -7.16(d, 1359Hz, 6F) > -40.74(d, 1109Hz, 12F) 3-(.eta..sup.1 -dfpma) 2.29(s, 9H) > -29.73(d, 1175Hz, 4F) 2.34(d, 7Hz, 6H) -40.94(d, 1116Hz, 12F) > -76.28(d, 1252Hz, 4F) .sup.a Listed coupling constant is > .vertline. .sup.1 J.sub.PF + .sup.3 J.sub.PF .vertline., > .sup.b Spectra acquired in CDCl.sub.3. > > TABLE 4 .sup.19 F NMR (.delta. and .vertline. .sup.1 J.sub.PF > + .sup.3 J.sub.PF .vertline.) data for Rh.sub.2.sup.II,II > (dfpma).sub.3 X.sub.4 (X = Cl (4), Br (5)), the designations > F.sub.a-e refer to the Neumann Projections in FIG. 1.2. > Spectra were acquired in CDCl.sub.3. Assignment 4 > (.delta./ppm) 5 (.delta./ppm) F.sub.a -78.7(1164Hz) 5 > -73.9(1101Hz) F.sub.c -46.6(1128Hz) 2 -44.5(1128Hz) F.sub.d > -47.3(1295Hz) 0 -47.6(1320Hz) F.sub.e -54.9(1160Hz) 6 > -48.9(1150Hz) F.sub.b -60.6(1200Hz) 2 -59.3(1185Hz) > > TABLE 5 .sup.19 F NMR (.delta. and .vertline. .sup.1 J.sub.PF > + .sup.3 J.sub.PF .vertline.) data for Rh.sub.2.sup.0,II > (dfpma).sub.3 X.sub.2 (L) (X = Cl (1-L), Br (2-L)), the > designations F.sub.a-e refer to the Neumann Projections in > FIG. 1.2. Spectra were acquired in CDCl.sub.3. 2-P(O.sup.i > Pr).sub.3 Assignment 1-PPh.sub.3 (.delta./ppm) 2-PPh.sub.3 > (.delta./ppm) (.delta./ppm) F.sub.c -35.7(1047Hz) 0 > -35.7(1067Hz) 4 -39.6(1089Hz) F.sub.e -40.6(1181Hz) 0 > -40.4(1122Hz) 0 -40.9(1155Hz) F.sub.f -41.8(1106Hz) 0 > -41.5(1187Hz) 0 -41.8(1115Hz) F.sub.b -49.5(1166Hz) 3 > -46.8(1174Hz) 0 -46.5(1174Hz) F.sub.d -52.0(1121Hz) 0 > -52.0(1118Hz) 1 -51.3(1117Hz) F.sub.a -79.1(1121Hz) 5 > -74.1(1132Hz) 1 -73.0(1120Hz) > > The .sup.1 H NMR spectra of the Rh.sub.2.sup.II,II > (dfpma).sub.3 X.sub.4 (X=Cl (4), Br (5)) complexes show the > resonances for the methyl groups of the bridging dfpma ligands > as a multiplet at 3.2 ppm. The .sup.19 F NMR spectrum contains > several first- and second-order spin systems, but simplifies > to a five-line pattern upon .sup.31 P decoupling, consistent > with a C.sub.2 symmetric structure for 4 and 5 in solution. > For illustrative purposes the .sup.19 F and .sup.19 F{.sup.31 > P} NMR spectra of 4 are displayed in FIGS. 2(a) and (b), > respectively (Table 4 contains the chemical shift values and > .vertline..sup.1 J.sub.PF +.sup.3 J.sub.PF.vertline. coupling > constants for both 4 and 5). Notably, the fluorine atoms of > the PF.sub.2 groups located trans to the halide ligands > (F.sub.a in the Neumann Projection of FIG. 2(a)) are shifted > to low frequency at -78.7 ppm. Four AB sub-spectra observed > inside and outside of the .vertline..sup.1 J.sub.PF +.sup.3 > J.sub.PF.vertline. doublet is indicative of direct (.sup.1 > J.sub.PF) and indirect (.sup.3 J.sub.PF) phosphorus coupling > constants of opposite sign. Similar XX'AA'X"X'" coupling > patterns in the resonances at -60.6 and -46.6 ppm identify > these resonances as the fluorine atoms F.sub.b and F.sub.c, > respectively, coupled to F.sub.a through the nitrogen > bridgehead. The remaining resonances at -47.3 and -54.9 ppm > are assigned as F.sub.d and F.sub.e, respectively, each > displaying only a doublet with a coupling constant given by > .vertline..sup.1 J.sub.PF +.sup.3 J.sub.PF.vertline.. > > Interpretation of the NMR spectra for the Rh.sub.2.sup.0,II > (dfpma).sub.3 X.sub.2 (L) (X=Cl (1-L), Br (2-L)) complexes > follows along similar lines. The coordination of a PF.sub.2 of > one dfpma ligand trans to a halogen on the octahedral > Rh.sup.II center gives rise to two .sup.1 H NMR methyl > resonances at 2.8 and 2.9 ppm for the bridging dfpma ligands, > integrating in a 1:2 ratio, respectively. Additionally, the > .sup.1 H NMR displays resonances diagnostic of the axial > ligand, L, capping the Rh.sup.0 center. The .sup.19 F and > .sup.19 F{.sup.31 P} NMR spectra of 1-PPh.sub.3 are presented > in FIGS. 2(c) and 2(d) (representative .sup.19 F NMR data for > 1-L can be found in Table 5). Several complex spin systems are > observed in the .sup.19 F NMR absorption spectrum, but > simplify to a six-line pattern for the dfpma ligands upon 31P > decoupling. The structure of 1-PPh.sub.3 is C.sub.s symmetric > in solution, as can be seen in the Neumann Projection inset > into FIG. 2(c); the mirror plane is defined by the two rhodium > centers and the equatorial halogen ligand. By analogy to the > spectra of 4, the low frequency resonance at -79.3 ppm is > indicative of a PF.sub.2 group coordinated trans to the halide > ligand, thus assigned to F.sub.a ; the fluorine atoms of the > Rh.sup.0 -coordinated PF.sub.2 group (F.sub.b) of this dfpma > ligand are resolved at -49.5 ppm. The two Rh.sup.0 > -coordinated PF.sub.2 groups (F.sub.e and F.sub.f) are > observed as .vertline..sup.1 J.sub.PF +.sup.3 > J.sub.PF.vertline. doublets at -40.6 and -41.8 by analogy to > the Rh.sub.2.sup.0,0 complexes, 3-L. The remaining resonances > at -35.7 and -52.0 ppm are assigned to the fluorine atoms of > the remaining Rh.sup.II PF.sub.2 groups, F.sub.c and F.sub.c. > > **Bis(dimethylphosphite)methyl amine** > > The preparation of bis(dimethylphosphite)methyl amine (dmpma) > and bis(diphenylphosphite)methyl amine (dppma) is > straightforward. Treatment of MeN(PCl.sub.2).sub.2 with four > equivalents of methanol or phenol and four equivalents of a > tertiary amine base in ether or pentane gave the ligand and > HCl salt. The dmpma and dppma ligands were purified by > distillation and recrystallization, respectively. > > Addition of dmpma to CH.sub.2 Cl.sub.2 solutions of > [ClRh(CO).sub.2 ].sub.2 resulted in an immediate color change, > affording an intense red solution. Precipitation yielded the > product as an orange powder, which analyzed as Rh.sub.2 > (dmpma).sub.2 Cl.sub.2 (CO).sub.2 (6). This compound has been > characterized by X-ray diffraction and has the structure > depicted in Scheme 6. Infrared spectroscopy showed two CO > frequencies, at 1989 and 1808 cm.sup.-1, for both terminal and > bridging CO ligands. However, .sup.31 P NMR spectroscopy > showed a single resonance at 132.81 ppm with a > .vertline..sup.1 J.sub.PRh +.sup.n J.sub.PRh.vertline. of 142 > Hz. VT NMR studies suggested a fluxional dirhodium core. > Cooling of CD.sub.2 Cl.sub.2 solutions of 6, led to broadening > of the .sup.31 P NMR resonance and a decrease in the observed > phosphorus-rhodium ##STR6## > > coupling constant; however, the exchange process could not be > arrested within the accessible temperature range. The solution > NMR data is nevertheless consistent with the solid-state > structure of 6 reported in the literature, in which a single > CO ligand bridges the binuclear Rh.sup.l core. > > Single crystals of 6 were obtained from CH.sub.2 Cl.sub.2 > /heptane solution. Here the X-ray diffraction study gave an > isomeric structure with two bridging CO groups (FIG. 3). Two > dmpma ligands bridge a valence-symmetric binuclear rhodium > core possessing terminal chloride ligands. A Rh--Rh separation > of 2.7155(10) .ANG. and an intra-ligand P . . . P separation > of 2.913(3) .ANG. indicate the presence of a formal > metal-metal bond. Other parameters of note are an average > Rh--P distance of 2.2867(19) .ANG. and an average P--N > distance of 1.666(6) .ANG.. The Rh(1)'-Rh(1)-Cl(1) angle is > 159.73(12).degree., and the Rh(1)-Cl(1) distance is normal at > 2.418(4) .ANG.. > > **Bis(diphenylphosphite)methyl amine (dppma)** > > Similar RhI2 products were obtained for the reaction of dppma > with [ClRh(CO).sub.2 ].sub.2 in CH.sub.2 Cl.sub.2 solution, as > shown in Scheme 7. Ligand addition resulted in an immediate > color change from pale yellow-orange to very dark purple. > Addition of cold pentane caused precipitation of a purple > powder in moderate yields; elemental analysis suggested the > formulation Rh.sub.2 (dppma).sub.2 Cl.sub.2 (CO).sub.2 (7). > Infrared spectra obtained for KBr pellets of the product > showed only a terminal carbonyl frequency at 2009 cm.sup.-1. > This, taken with the intense purple color of the complex > suggested a structure containing face-to-face square planar > rhodium(I) centers as shown for 7 in Scheme 7. However, > solutions of the complex showed both bridging and terminal > carbonyl resonances, and VT NMR studies suggested an > equilibrium between the face-to-face structure and a structure > with one bridging carbonyl (8), as observed for 6. > > In solution, 7 slowly rearranged to give a new isomer with > two bridging CO ligands and two terminal halides, Rh.sub.2 > (dppma).sub.2 Cl.sub.2 (.mu.-CO).sub.2 (9), characterized by a > single .nu..sub.CO at 1828 cm.sup.1. The .sup.1 H and .sup.31 > P NMR spectra of 9 revealed that this isomer is not fluxional > in solution. The .sup.1 H NMR spectrum displayed a single > methyl resonance for the bridging dppma ligands at 2.86 ppm; > the protons of the phenyl rings are observed in ##STR7## > > the 6.8-7.5 ppm region. A single phosphorus resonance was > observed in the .sup.31 P NMR spectrum of 9 at 122.61 ppm > (.vertline..sup.1 J.sub.PRh +.sup.n J.sub.PRh.vertline.=170 > Hz) > > Single crystals suitable for X-ray diffraction studies were > obtained for 9 and the data confirmed the solution structure > assignments. FIG. 4 shows a structure with two dppma ligands > and two CO ligands spanning a short metal-metal separation of > 2.7076(8) .ANG.. The carbonyl ligands bridge the dirhodium > core in a symmetric fashion with Rh--C(1) and Rh'--C(1) > distances of 1.990(13) and 2.010(13) .ANG., respectively; the > Rh--C(1)-Rh' angle is 85.2(4).degree.. The axial halogen has a > normal Rh--X distance of 2.3379(15) .ANG., and the Cl--Rh--Rh' > angle is nearly linear at 175.64(6). The PNP backbone is > symmetric with N--P distances of 1.661(5) and 1.676(5) .ANG., > and the intra-ligand P . . . P separation is 2.886(3) .ANG.. > > Solutions of 9 decomposed slowly by loss of the carbonyl > ligands. The final product observed was the chelated dimer, > [ClRh(tfepma)].sub.2 (11), which was characterized by a single > resonance in the .sup.31 P NMR spectrum at 91.13 ppm and an > apparent J.sub.RhP coupling constant of 280 Hz. Purging > solutions of 11 with carbon monoxide regenerated rhodium dimer > 7. CO loss from 9 is proposed to proceed through a > two-electron mixed-valence complex based on a literature > report of a monocarbonyl derivative of the related > bis(diphenylphosphite)ethyl amine (dppea) ligand. Single > crystals of Rh.sub.2.sup.0,II (dppea).sub.2 Cl.sub.2 (CO) > reportedly were obtained from CHCl.sub.3 solutions of > Rh.sub.2.sup.I,I (dppea).sub.2 Cl.sub.2 (CO).sub.2 and > provided the coordination environment depicted for 10 in > Scheme 7. However, 10 was not explicitly isolated nor > characterized as an intermediate in the conversion of 9 to 11. > > The dppma ligand supported two-electron oxidation and > reduction of the binuclear rhodium core, yielding > Rh.sub.2.sup.0,0 and Rh.sub.2.sup.II,II products. 9 was > reduced with two equivalents of cobaltocene in the presence of > dppma, affording Rh.sub.2 (dppma).sub.3 (CO).sub.2 (12) as a > yellow microcrystalline solid. Alternatively, 12 was directly > prepared from the reaction of [ClRh(CO).sub.2 ].sub.2 with > three equivalents of dppma and cobaltocene. Single crystals of > 12 were obtained by cooling CH.sub.2 Cl.sub.2 /pentane > solutions to -35.degree. C. The molecular structure is > presented in FIG. 5(a) and pertinent metrical parameters are > listed in Table 6. The metal-metal separation in 12 is long at > 2.8687(8).ANG., however, it is within the range expected for a > single Rh--Rh bond. The equatorial coordination planes are > staggered with respect to one another, adopting a torsion > angle of 35.2.degree.. A C(3)-O(7) bond distance of 1.138(6) > .ANG. is relatively long, reflecting a decrease in bond order > of the carbonyl ligand due to coordination to the > electron-rich Rh.sup.0 center. As expected, the PNP backbone > of the bridging dppma ligands is symmetric with an average > P--N distance of 1.681(4) .ANG.. > > Oxidation of 9 with dichloroiodobenzene afforded the > valence-symmetric Rh.sub.2.sup.II,II dimer Rh.sub.2 > (dppma).sub.2 Cl.sub.4 (CO).sub.2 (13), presented as a thermal > ellipsoid plot in FIG. 5(b). Alternatively, the reaction of > [ClRh(cod)].sub.2 with PhICl.sub.2 and dppma yielded 13 > directly. In 13, only two dppma ligands coordinate to the > bimetallic core, and small donor ligands such as CO or > isonitrile must be incorporated to yield the six-coordinate > octahedral geometry at each rhodium center. The metal-metal > separation is significantly contracted relative to the reduced > complex, 12. A Rh--Rh' distance of 2.705(3) .ANG. in 13 is > complimented by a torsion angle for the equatorial planes of > only 0.9.degree.. The dppma ligands coordinate trans to one > another, with average Rh--P distances of 2.300(6) .ANG.. The > Rh--Cl(2) distance of 2.382(7) .ANG. is in the typical range > for halogens coordinated trans to a Rh--Rh bond. The > equatorial chloride and carbonyl ligands are coordinated in an > anti conformation, with Rh--Cl(1) and Rh--C(1) distances of > 2.365(8) and 1.95(4) .ANG., respectively. A short C(1)-O(1) > bond distance of 1.09(4) reflects little decrease in the CO > bond order. > > TABLE 6 Selected bond lengths (.ANG.) for Rh.sub.2 > (dppma).sub.3 (CO).sub.2 (12) and Rh.sub.2 (dppma).sub.2 > Cl.sub.4 (CO).sub.2 (13). Selected Bond Lengths (.ANG.) > Rh.sub.2 (dppma).sub.3 (CO).sub.2 Rh.sub.2 (dppma).sub.2 > Cl.sub.4 (CO).sub.2 Rh-Rh' 2.8687(8) Rh-Rh' 2.705(3) Rh-P(1) > 2.2911(15) Rh-Cl(1) 2.365(8) Rh-P(2) 2.2615(15) Rh-Cl(2) > 2.382(7) Rh-P(3) 2.2987(15) Rh-P(1) 2.293(6) Rh-C(3) 1.886(6) > Rh-P(2) 2.307(6) C(3)-O(7) 1.138(6) Rh-C(1) 1.95(4) P(1)-N(1) > 1.686(4) C(1)-O(1) 1.09(4) P(2)-N(2) 1.678(3) P(1)-N(1) > 1.680(17) P(3)-N(1)' 1.678(4) P(2)-N(1)' 1.674(17) > > The oxidized and reduced complexes, 12 and 13, of dppma were > prepared with isonitrile ligands replacing the carbonyl > groups. An X-ray structure obtained on single crystals of > Rh.sub.2 (dppma).sub.2 Cl.sub.4 (CN.sup.t Bu).sub.2 confirmed > that it is isostructural with the carbonyl derivative, > including the eclipsed geometry of the rhodium coordination > spheres. > > **Bis(bis(trifluoroethyl)phosphite)methyl amine ("tfepma")** > > Based on the results of the methoxy- and phenoxy-substituted > PNP ligands, a phosphorus substituent was sought with stronger > .pi.-acid properties and a steric parameter larger than > fluorine. Tolman's steric and electronic map for tertiary > phosphine ligands shows that functionalization with > halogenated alkanes and alcohols result in strong .pi.-acid > characteristics. Tris(2,2,2-trichloroethyl)phosphite has a > cone angle comparable to other primary alcohol derivatives, > yet is a stronger .pi.-acid. Therefore, it was surmised that > the 2,2,2-trifluoroethanol derivative would give a PNP ligand > with enhanced .pi.-acid character while maintaining steric > characteristics similar to those of dmpma. > > The reaction of 2,2,2-trifluoroethanol with > MeN(PCl.sub.2).sub.2 in ether/pentane mixtures at > dry-ice/acetone temperatures proceeded smoothly to afford > MeN[P(OCH.sub.2 CF.sub.3).sub.2 ].sub.2 (tfepma) in moderate > yield after distillation. The viscous liquid was characterized > by .sup.1 H NMR spectroscopy, which showed a > triplet-of-doublets pattern at 2.51 ppm for the methyl protons > of the methylamine bridgehead and a doublet-of-pentets pattern > at 3.55 ppm for the methylene protons of the trifluoroethyl > substituents. The .sup.31 P{.sup.1 H} NMR spectrum showed a > singlet at 148.6 ppm and the .sup.19 F NMR spectrum showed a > multiplet centered at -76.90 ppm. > > **Complexes with Bridging tfepma Ligands** > > The pale orange color of [ClRh(CO).sub.2 ].sub.2 in methylene > chloride immediately changed to dark red upon dropwise > addition of tfepma. Concentration by vacuum distillation > followed by addition of pentane afforded a yellow-orange > powder in moderate yield. Elemental analysis suggested the > formulation Rh.sub.2 (tfepma).sub.2 Cl.sub.2 (CO).sub.2 (14), > and infrared spectra obtained on KBr pellets of this product > showed a carbonyl stretch at 2007 cm.sup.-1. As with the dmpma > and dppma complexes, 14 is fluxional in solution. At room > temperature, time-averaged NMR spectra were obtained: a single > methyl resonance was observed at 2.94 ppm in the .sup.1 H NMR > spectrum and a symmetric .sup.31 P resonance was observed at > 131.16 ppm (.vertline..sup.1 J.sub.PRh +.sup.n > J.sub.PRh.vertline.=149 Hz) in the .sup.31 P NMR spectrum. > Based on the observed .vertline..sup.1 J.sub.PRh +.sup.n > J.sub.PRh.vertline. coupling constant, a structure with two > tfepma ligands spanning a Rh.sup.I.sub.2 core, axial Cl > ligands, and bridging and terminal carbonyl ligands is > assigned for 14 as shown in Scheme 8. > > Modified forcing reaction conditions afforded a doubly > CO-bridged isomer. Refluxing [ClRh(CO).sub.2 ].sub.2 with two > equivalents of tfepma in toluene gave Rh.sub.2 (tfepma).sub.2 > Cl.sub.2 (.mu.-CO).sub.2 (15) in quantitative yield. Infrared > spectroscopy showed only a bridging carbonyl stretch at 1824 > cm.sup.-1. .sup.31 P NMR spectroscopy again revealed a > symmetric complex, with a single resonance at 128.4 ppm > (.vertline..sup.1 J.sub.PRh +.sup.n J.sub.PRh.vertline.=164 > Hz). The IR and NMR data are consistent with rearrangement of > the metal core to give a structure analogous to 9. However, > unlike the dppma compound, 15 is thermally robust and is not > subject to further rearrangements of the metal core in the > absence of other reagents: even at reflux in toluene, CO was > not lost from the complex. ##STR8## > > Treatment of solutions of 14 or 15 with one equivalent of > tfepma gave a dark red solution from which maroon crystals > were deposited upon prolonged standing. The crystals proved > suitable for X-ray diffraction studies and yielded the > molecular structure presented in FIG. 6 for Rh.sub.2.sup.0,II > (tfepma).sub.3 Cl.sub.2 (CO) (16). As observed for the dfpma > chemistry of rhodium, three tfepma ligands span the bimetallic > core of 16. The two-electron mixed-valence complex comprises > octahedral Rh.sup.II and trigonal bipyramidal Rh.sup.0 > centers. The axial site of the Rh.sup.0 is coordinated by a CO > ligand, and two chloride ligands occupy axial and equatorial > sites of the Rh.sup.II. The metal-metal separation is normal > at 2.7662(11) .ANG.. Rh--P bond distances are longer by an > average of 0.037 .ANG. than those observed for the dfpma > complexes due to the greater steric demand of the P(OCH.sub.2 > CF.sub.3).sub.2 groups. Other metrical parameters for 16 are > listed in Table 7, and in general suggest an expanded core > coordination environment for the dirhodium center. > > In solution, the two-electron mixed-valence complex was > unstable with respect to loss of the axial CO ligand. The > principal species observed by NMR spectroscopy was in fact the > halogen-bridged Rh.sup.I.sub.2 dimer with two chelating tfepma > ligands, [ClRh(tfepma)].sub.2 (17). This complex was prepared > independently by the addition of two equivalents of tfepma to > [ClRh(cod)].sub.2. The symmetric dimer was treated with one > equiv of tfepma and one equiv of CN.sup.t Bu to reform the > two-electron mixed-valence complex, Rh.sub.2.sup.0,II > (tfepma).sub.3 Cl.sub.2 (CN.sup.t Bu), with an axial > isonitrile ligand; however, the product was always > contaminated with 17. > > TABLE 7 Bond lengths (.ANG.) and angles (deg) for > Rh.sub.2.sup.0,II (tfepma).sub.3 Cl.sub.2 (CO) (16). Selected > Bond Lengths (.ANG.) Rh(1)-Rh(2) 2.7662(11) Rh(2)-Cl(1) > 2.513(3) Rh(1)-P(1) 2.284(3) Rh(2)-Cl(2) 2.399(3) Rh(1)-P(3) > 2.255(3) Rh(2)-P(2) 2.308(3) Rh(1)-P(5) 2.287(3) Rh(2)-P(4) > 2.214(3) Rh(1)-C(4) 1.895(12) Rh(2)-P(6) 2.281(3) P(1)-N(1) > 1.685(10) P(2)-N(1) 1.670(10) P(3)-N(2) 1.686(9) P(4)-N(2) > 1.667(9) P(5)-N(3) 1.673(10) P(6)-N(3) 1.658(10) Selected Bond > Angles (deg) Rh(2)-Rh(1)-C(4) 176.9(4) Cl(1)-Rh(2)-Cl(2) > 91.51(10) Rh(1)-Rh(2)-Cl(1) 176.54(7) Cl(1)-Rh(2)-P(2) > 82.86(10) Rh(1)-Rh(2)-Cl(2) 87.97(7) Cl(1)-Rh(2)-P(4) > 87.23(10) Cl(2)-Rh(2)-P(2) 87.34(11) Cl(1)-Rh(2)-P(6) > 98.51(10) Cl(2)-Rh(2)-P(4) 175.59(11) P(7)-Rh(1)-P(1) 90.0(3) > Cl(2)-Rh(2)-P(6) 85.20(11) C(4)-Rh(1)-P(3) 94.5(4) > P(1)-Rh(2)-P(3) 110.68(12) C(4)-Rh(1)-P(5) 90.0(3) > P(1)-Rh(2)-P(5) 130.87(12) Rh(1)-C(4)-O(1) 177.8(11) > > The tfepma ligand supports two-electron reduced species, > Rh.sub.2.sup.0,0 (tfepma).sub.3 L.sub.2, (18-L) upon reduction > of [ClRh(CO).sub.2 ].sub.2 with cobaltocene in the presence of > three equiv tfepma and two equiv of L (L=CO, CN.sup.t Bu). > Alternatively, cobaltocene reduced 15 to 18-L in the presence > of L and one equivalent of tfepma. Spectroscopic data is > consistent with a binuclear Rh.sup.0 core bridged by three > tfepma ligands. The .sup.31 P NMR of 18-CN.sup.t Bu showed a > single resonance at 142.08 ppm displaying a 216 Hz coupling > constant. Similarly, the .sup.1 H NMR showed one methyl and > one methylene resonance for the bridging tfepma ligands at > 2.44 and 4.18 ppm, respectively, and a resonance for the > CN.sup.t Bu ligands at 1.05 ppm. > > Oxidation of the dirhodium core proceeded smoothly but > yielded different structural isomers depending on reaction > conditions. The reaction of tfepma and PhICl.sub.2 with > [ClRh(CO).sub.2 ].sub.2 at room temperature in CH.sub.2 > Cl.sub.2 afforded a bright yellow powder with the formula > Rh.sub.2.sup.II,II (tfepma).sub.3 Cl.sub.4 in moderate yields. > X-ray diffraction studies on single crystals of this product > yielded the molecular structure depicted in FIG. 7(a), > identifying the complex as the syn isomer, > syn-Rh.sub.2.sup.II,II (tfepma).sub.3 Cl.sub.4 (19). If the > reaction instead was conducted at reflux in toluene, an orange > product was obtained, the solid-state structure as determined > by X-ray diffraction identified this product as the anti > isomer, anti-Rh.sub.2.sup.II,II (tfepma).sub.3 Cl.sub.4 (20). > The molecular structure for 20 is presented in FIG. 7(b). > Selected bond distances and angles for each complex are > presented in Table 8. Comparison of the two isomers reveals a > significant contraction of the metal core for 19. The > Rh(1)-Rh(2) separation in the syn isomer is 2.6688(8) .ANG., > whereas the metal-metal distance in 20 is 2.7152(10) .ANG.. > Similarly, the metal-phosphorus and metal-halogen distances > are markedly different: the Rh--P distances in 20 are longer > by 0.045 .ANG. and the axial and equatorial Rh--Cl distances > are elongated by 0.062 and 0.061 .ANG., respectively. The syn > isomer also shows a much smaller twist about the Rh--Rh axis, > with an average torsion angle of 26.8.degree. as compared to > that of the anti isomer at 40.4.degree., which is almost > perfectly eclipsed. > > TABLE 8 Bond lengths (.ANG.) for syn-Rh.sub.2.sup.II,II > (tfepma).sub.3 Cl.sub.4 (19) and anti-Rh.sub.2.sup.II,II > (tfepma).sub.3 Cl.sub.4 (20). Selected Bond Lengths (.ANG.) > syn-Rh.sub.2.sup.II,II (tfepma).sub.3 Cl.sub.4 > anti-Rh.sub.2.sup.II,II (tfepma).sub.3 Cl.sub.4 Rh(1)-Rh(2) > 2.6688(8) Rh(1)-Rh(2) 2.7152(10) Rh(1)-Cl(1) 2.401(2) > Rh(1)-Cl(1) 2.456(2) Rh(1)-Cl(2) 2.334(2) Rh(1)-Cl(2) 2.398(2) > Rh(2)-Cl(3) 2.385(2) Rh(2)-Cl(3) 2.455(2) Rh(2)-Cl(4) 2.342(2) > Rh(2)-Cl(4) 2.399(2) Rh(1)-P(1) 2.281(2) Rh(1)-P(1) 2.223(2) > Rh(1)-P(3) 2.152(2) Rh(1)-P(3) 2.271(2) Rh(1)-P(5) 2.248(2) > Rh(1)-P(5) 2.329(2) Rh(2)-P(2) 2.258(2) Rh(2)-P(2) 2.275(2) > Rh(2)-P(4) 2.154(2) Rh(2)-P(4) 2.216(2) Rh(2)-P(6) 2.271(2) > Rh(2)-P(6) 2.319(2) > > The structural differences between the syn and anti isomers > of Rh.sub.2.sup.II,II (tfepma).sub.3 Cl.sub.4 are manifested > in the absorption and emission spectra of each complex, > presented in FIG. 8. The absorption spectra of 19 and 20 are > dominated by three bands in the near-UV and visible regions. > Two high-energy bands, assigned to transitions from the > configurationally mixed Cl(.sigma.)/d.sub.z.sub..sup.2 .sigma. > to the d.sub.z.sub..sup.2 .sigma.\* LUMO, shift little between > the two isomeric forms. However, the lowest energy transition > shows a pronounced dependence on the geometry of the dirhodium > core: the transition, of d.pi.\*.fwdarw.d.sub.z.sub..sup.2 > .sigma.\* parentage, shifts from 352 nm in 19 to 458 nm in 20. > This red shift of over 6500 cm.sup.-1 is accompanied by a > decrease in the extinction coefficient of the band from 11,000 > M.sup.-1 cm.sup.-1 to 4700 M.sup.-1 cm.sup.-1 for the syn and > anti isomers, respectively. Excitation of solid samples of > both 19 and 20 cooled to 77 K results in visible luminescence. > The emission spectrum of 19 is dominated by bright, long-lived > phosphorescence observed at 819 nm (.tau.=350 .mu.s). A > high-energy band is also observed at 578 nm (.tau.<8 ns), > but has only 1/100.sup.th of the intensity of the > phosphorescent peak, suggesting facile deactivation of the > .sup.1 d.sub.z.sub..sup.2 .sigma.\* excited state. Conversely, > both fluorescence and phosphorescence are strong for 20. A > high-energy emission band at 573 nm (.tau.<8 ns) and a > low-energy emission band at 857 nm (.tau.=150 .mu.s) are > observed with an intensity ratio of 1:2 (the relative > intensities of 19 to 20 were not determined). > > The influence of structure on electronic character is further > emphasized by the similarity between the electronic features > of 20 and the dfpma congener, Rh.sub.2.sup.II,II (dfpma).sub.3 > Cl.sub.4 (4). The absorption maxima of the two high-energy > transitions are essentially identical and the low energy > d.pi.\*.fwdarw.d.sub.z.sub..sup.2 .sigma.\* transition of 20 is > red-shifted by only 640 cm.sup.-1 relative to the same > transition in 4. Though negligible differences are observed in > the fluorescence emission maxima, the phosphorescence of 20 is > red shifted by 511 cm.sup.-1. This small low-energy shift is > diagnostic of a weaker metal-metal interaction in 20, and > correlates well with the observed difference in metal-metal > separation for 4 and 20 (.DELTA.Rh(1)-Rh(2)=0.008(1) .ANG.). > > **A Chelating tfepma Ligand** > > The tfepma ligand may be used to stabilize a new two-electron > mixed-valence rhodium platform in the absence of an axial > donor ligand. [ClRh(cod)].sub.2 reacted with three equivalents > of tfepma in CH.sub.2 Cl.sub.2, affording Rh.sub.2.sup.0,II > (tfepma).sub.3 Cl.sub.2 (21). Dark green single crystals of 21 > were obtained by diffusing pentane into a CH.sub.2 Cl.sub.2 > solution of the complex. The structure presented in FIG. 9 was > obtained from X-ray diffraction studies; selected bond > distances and angles are presented in Table 9. The molecular > structure of 21 reveals a departure from the coordination > geometry observed for other diphosphazane complexes of > rhodium. In the absence of a suitable donor ligand for the > Rh.sup.0 center, a tfepma ligand binds in a chelating mode > leaving only two tfepma ligands to bridge the bimetallic core. > A consequence of this chelating ligand is the vacant axial > coordination site at the Rh.sup.II center. Two phosphorus of > the bridging tfepma ligands and one phosphorus of the > chelating tfepma ligand define the equatorial plane of a > distorted trigonal bipyramidal Rh.sup.0 center. The axial > positions are capped by the other phosphorus of the chelate > and the proximate Rh.sup.II center, bound at a metal-metal > separation of 2.7529(19) .di-elect cons.. The Rh.sup.0 center > defines the apex of a square pyramid about the Rh.sup.II > center. Two phosphorus of the bridging tfepma ligands and two > chloride ligands occupy cis positions of the basal plane, with > P(2)-Rh(2)-P(4) and Cl(1)-Rh(2)-Cl(2) angles of > 95.65(18).degree. and 86.52(18).degree., respectively. > > TABLE 9 Bond lengths (.ANG.) and angles (deg) for > Rh.sub.2.sup.0,II (tfepma).sub.3 Cl.sub.2 (21) from > preliminary X-ray data. Selected Bond Lengths (.ANG.) > Rh(1)-Rh(2) 2.7529(19) Rh(2)-Cl(1) 2.359(5) Rh(1)-P(1) > 2.240(5) Rh(2)-Cl(2) 2.361(5) Rh(1)-P(3) 2.295(5) Rh(2)-P(2) > 2.188(5) Rh(1)-P(5) 2.285(5) Rh(2)-P(4) 2.190(5) Rh(1)-P(6) > 2.176(5) P(1)-N(1) 1.689(16) P(2)-N(1) 1.692(17) P(3)-N(2) > 1.668(13) P(4)-N(2) 1.677(14) Selected Bond Angles (deg) > P(5)-Rh(1)-P(1) 137.48(18) Cl(1)-Rh(2)-Cl(2) 86.52(18) > P(5)-Rh(1)-P(3) 114.79(17) Cl(1)-Rh(2)-P(2) 88.15(18) > P(5)-Rh(1)-P(6) 70.07(18) Cl(1)-Rh(2)-P(4) 171.09(18) > P(6)-Rh(1)-Rh(2) 164.31(15) > > **Aniline-Derived Diphosphazanes** > > As a preliminary investigation of the electronic factors > associated with exchanging the methyl group on the nitrogen > bridgehead, 3,5-xylidene was refluxed in PCl.sub.3 to afford > bis(dichlorophosphine)-3,5-xylidene (dcpx). This precursor can > be further functionalized as shown in Scheme 2, yielding the > same variety of phosphorus groups for metal coordination. > Fluorination with SbF.sub.3 provided > bis(difluorophosphine)xylidene (dfpx) in good yields after > recrystallization from pentane and sublimation. Similarly, > 2,2,2-trifluoroethanol reacted with dcpx to yield the > corresponding trifluoroethyl derivative > bis(bis(trifluoroethyl)phosphite)-3,5-xylidene (tfepx) as a > crystalline solid from pentane. > > **Bis(difluorophosphine)-3,5-xylidene (dfpx)** > > Two-electron mixed-valence complexes of dfpx were prepared by > the strategy presented in Scheme 3. A dirhodium core > isostructural to 1 and 2 is presented in FIG. 10 for > Rh.sub.2.sup.0,II (dfpx).sub.3 Br.sub.2 (PPh.sub.3) (22). The > metrical parameters for the metal core of 22 are presented in > Table 10, and are similar to those of the corresponding > dfpma-bridged dirhodium complexes (Table 2); the N--P > distances for the bridging dfpx ligands are 1.611(18) and > 1.679(16) .ANG. for the phosphines coordinated to the > Rh.sup.II and Rh.sup.0 centers, respectively. The aryl rings > on the nitrogen bridgehead align perpendicularly to the > P--N--P plane, with an average dihedral angle of 90.4.degree.. > At 2.819(3) .ANG., the metal-metal separation is slightly > shorter than that of the dfpma derivative; Rh--Br distances of > 2.570(3) and 2.463(5) are contracted as well. Other ligand > distances are undistinguished from the dfpma analog. > > The absorption spectra of the homologous dfpma and dfpx > complexes provided further evidence for the complete > decoupling of the aryl .pi. system of dfpx from the core of > the dirhodium complex. Aside from subtle changes in the peak > intensities, absorption features are identical, displaying the > expected three band pattern: for comparison, .lambda..sub.abs > max =309, 366 and 410 nm for 2-PPh.sub.3 and .lambda..sub.abs > max =314, 370 and 411 nm for 22-PPh.sub.3. > > TABLE 10 Bond lengths (.ANG.) and angles (deg) for > Rh.sub.2.sup.0,II (dfpx).sub.3 Br.sub.2 (PPh.sub.3) (22). > Selected Bond Lengths (.ANG.) Rh(1)-Rh(2) 2.819(3) Rh(2)-Br(1) > 2.570(3) Rh(1)-P(1) 2.227(6) Rh(2)-Br(2) 2.463(5) Rh(1)-P(3) > 2.220(7) Rh(2)-P(2) 2.219(6) Rh(1)-P(5) 2.242(6) Rh(2)-P(4) > 2.184(7) Rh(1)-P(7) 2.330(6) Rh(2)-P(6) 2.262(6) P(1)-N(1) > 1.658(16) P(2)-N(1) 1.641(17) P(3)-N(2) 1.689(17) P(4)-N(2) > 1.571(19) P(5)-N(3) 1.690(15) P(6)-N(3) 1.620(16) Selected > Bond Angles (deg) Rh(2)-Rh(1)-P(7) 179.07(17) > Br(1)-Rh(2)-Br(2) 90.79(13) Rh(1)-Rh(2)-Br(1) 178.13(9) > Br(1)-Rh(2)-P(2) 95.35(17) Rh(1)-Rh(2)-Br(2) 90.68(12) > Br(1)-Rh(2)-P(4) 85.61(18) Br(2)-Rh(2)-P(2) 87.7(2) > Br(1)-Rh(2)-P(6) 91.98(17) Br(2)-Rh(2)-P(4) 176.35(18) > P(7)-Rh(1)-P(1) 93.8(2) Br(2)-Rh(2)-P(6) 84.0(2) > P(7)-Rh(1)-P(3) 92.3(2) P(1)-Rh(2)-P(3) 126.2(2) > P(7)-Rh(1)-P(5) 93.1(2) P(1)-Rh(2)-P(5) 114.2(2) > > **Bis(bis(trifluoroethyl)phosphite)-3,5-xylidene (tfepx)** > > The reaction of tfepx with [ClRh(cod)].sub.2 did not provide > direct access to a two-electron mixed-valence complex. Rather, > a bright yellow microcrystalline product precipitated from the > green solution afforded by 1:3 mixtures of the rhodium > starting material and ligand in CH.sub.2 Cl.sub.2. Elemental > analysis suggested the empirical formulation Rh.sub.2 > (tfepx).sub.3 Cl.sub.2, consistent with the formulation of 21. > However, X-ray diffraction studies revealed a divergent > binuclear RhI structure, [ClRh(tfepx)].sub.2 (.mu.-tfepx) > (23), shown as a thermal ellipsoid plot in FIG. 11. Here, two > four-coordinate RhI fragments are tethered by a bridging tfepx > ligand. A single chloride and a chelating tfepx ligand > complete the distorted square planar coordination environment > about each rhodium center. An average intra-ligand P--Rh--P > angle of 70.38(8).degree. is acute for a square-planar metal > complex, suggesting a significant degree of strain in the > four-membered chelate ring. All tfepx ligands show symmetric > PNP backbones, with an average N--P distance of 1.694(6) > .ANG.. As observed in the structure of 22, the aryl ring of > the bridging tfepx ligand is nearly orthogonal to the > P(2)-N(2)-P(3) plane, adopting a torsion angle of > 81.4.degree.. Conversely, the aryl rings of the chelating > tfepx ligands of 23 are rotated to be coplanar with the > P--N--P triad, displaying torsion angles of 14.30 and 9.10 for > the tfepx ligands of the Rh(1) and Rh(2) centers, > respectively. Rotation of the aryl rings into the P--N--P > plane delocalizes the nitrogen lone pair into the aromatic > system, shortening the N--C bond. In accord with this > suggestion, the average N--C bond length for the chelating > tfepx ligands is 1.446(9) .ANG. versus 1.485(9) .ANG. for the > N--C bond of the bridging tfepx ligand. > > Isolation of discrete two-electron mixed-valence complexes of > rhodium relies on a delicate balance of stereo-electronic > properties within the diphosphazane ligand framework. The > results suggest that in addition to the coordination of three > ligands to the binuclear core, the strong .pi.-acid phosphine > groups and a polarizable lone pair on the nitrogen bridgehead > atom help induce valence-symmetric cores to disproportionate. > > The fluorinated diphosphazane, dfpma, rapidly reacts with > Rh.sup.I starting materials to afford two-electron > mixed-valence complexes in nearly quantitative yields. The > strong .pi.-acid character of the difluorophosphine groups > coupled with the small steric parameter facilitates > coordination of three ligands to the bimetallic core. Crystal > structures of various derivatives of 1 provide evidence for > induced polarization of the PNP backbone as proposed in Scheme > 1. A contracted N--P bond for the phosphines coordinated to > the Rh.sup.II center is indicative of significant N.fwdarw.P > donation, serving to stabilize the .pi.-acid phosphines > coordinated to the oxidized metal center. With the N lone pair > electron density channeled away from the PF.sub.2 groups > bonded to the Rh.sup.0, the strong .pi. accepting properties > of this phosphine are maintained and hence the reduced rhodium > center is stabilized. > > In complexes with only two bridging diphosphazane ligands, > valence disproportion of the binuclear rhodium core is > circumvented. The dmpma and dppma ligands exclusively form 2:1 > complexes with divalent rhodium cores. In these cases, valence > disproportionation is not observed, and only symmetric > Rh.sup.l.sub.2 cores are obtained. Within the framework > outlined in Scheme 1, coordination of two diphosphazane > ligands defeats induced polarization of the ligand backbone. > Scheme 9 shows that coordination of two diphosphazane ligands > to a binuclear complex provides the system a facile > comproportionation pathway to produce symmetric cores. > Polarization of one PNP ligand via donation of the nitrogen > lone pair to one phosphine group is countered by lone pair > donation in the opposite direction for the other bridging > ligand. N--P bond lengths for the Rh.sup.I complexes of dmpma > and dppma support this contention: 6 shows N--P bond distances > of 1.670(6) .ANG. and 1.661(6) .ANG. and 9 shows N--P > distances of 1.661(5) .ANG. and 1.676(5) .ANG.. The literature > report of Rh.sub.2.degree. l(dppea).sub.2 Cl.sub.2 (CO) > indicates that two diphosphazanes may be able to stabilize a > two-electron mixed-valence species transiently, but results > presented here suggest that such a complex rapidly rearranges > in solution to give symmetric species. > > The driving force for valence disproportionation engendered > by coordination of a third PNP ligand is illustrated by the > conversion of 15 to 16 as shown in Scheme 8. In the absence of > a third tfepma ligand, the Rh.sup.I. . . Rh.sup.I core of 15 > is robust, withstanding refluxing toluene without > rearrangement or ligand loss. However, addition ##STR9## > > of one equivalent of tfepma to room temperature solutions of > 15 induces valence disproportionation to the Rh.sub.2.sup.0,II > species, 16. It is suggested that although the symmetrization > mechanism of Scheme 9 is operative in 15, introduction of a > third tfepma ligand "frustrates" the binuclear core, thus > forcing the system to polarize and form the two-electron > mixed-valence complex. > > Interplay of the .pi.-acid phosphine with the nitrogen lone > pair defines the ligands' ability to polarize the binuclear > core. Diphosphazane functionalization at phosphorus and > nitrogen may be used to probe these mediating effects of the > nitrogen atom. The methyl amine bridgehead provides maximum > participation of the nitrogen lone pair in .pi. bonding with > the proximate phosphine groups. Conversely, competition for > the nitrogen lone pair is possible in diphosphazanes with > aniline bridgeheads. Participation of the bridgehead nitrogen > lone pair in the .pi. system of an aryl group might > drastically influence the ability of a diphosphazanes to > stabilize two-electron mixed valence cores. Isolation of 22 in > high yields suggests that the strong .pi.-accepting properties > of the difluorophosphine group override the electron accepting > properties of the dfpx aryl group. Rotation of the aryl group > perpendicular to the P--N--P plane completely decouples the 1 > system from the PNP backbone and indicates complete > utilization of the nitrogen lone pair by the PF.sub.2 groups. > Comparison of the absorption spectrum of 22 to the analogous > dfpma complex 2-PPh.sub.3 lends further support to the > electronic homology between the dfpx and dfpma ligands. The > low energy d.pi.\*.fwdarw.d.sigma.\* transition, which should be > most sensitive to changes in the electronic properties of the > bridging diphosphazane, blue-shifts by only 59 cm.sup.1 upon > substitution of dfpx for dfpma in 22 and 2-PPh.sub.3, > respectively. Conversely, the aryl .pi. system competes > effectively with the weaker .pi.-acid group > bis(trifluoroethyl)phosphite for the nitrogen lone pair of > tfepx. This competition forces the tfepx system to adopt a > valence-symmetric configuration. Whereas the coordination of > three tfepma ligands to a Rh.sub.2 core produces the > two-electron mixed-valence complex 21, tfepx provides a > structure for 23 with two non-interacting Rh.sup.I centers. > Rotation of the aryl ring of the chelating tfepx ligands into > the P--N--P plane indicates a significant degree of > N.fwdarw.aryl lone pair donation. Contracted N--C bond lengths > for the chelating ligands further support this contention. > Apparently, in the tfepx case, interaction of the nitrogen > bridgehead with the aryl .pi. system reduces the > polarizability of the lone pair and thus valence > disproportionation is not observed. > > Manipulation of the steric and electronic properties of the > phosphorus substituents of the PNP ligand set leads to varied > chemical reactivity. The juxtaposition of strong .pi.-acid > phosphines with the nitrogen lone pair in dfpma leads to a > polarization of the PNP backbone to stabilize the two-electron > mixed-valence species. Furthermore, incorporation of > sequentially more .pi.-acidic phosphines revealed a > step-by-step rearrangement of the binuclear Rh.sup.I core > culminating with valence disproportionation and formation of a > two-electron mixed-valence core. Diphosphazane ligands with > small steric requirements, in addition to the requisite > .pi.-acidity, incorporate a third bridging ligand into the > binuclear core. At least three ligands may be required to > stabilize the two-electron mixed-valence complex and overcome > the thermodynamic driving force for valence-symmetric > binuclear cores. > > **Reactivity Studies of the Two-Electron Mixed-Valence > Complex Ir.sub.2.sup.0,II (tfepma).sub.3 Cl.sub.2** > > The chemistry of two-electron mixed valency was generalized > to transition metals other than rhodium. Ongoing interest in > hydrogen photocatalysis, suggested investigation of the > two-electron mixed-valence chemistry of iridium to acquire an > understanding of the hydrido and hydrido-halo chemistry of > this new class of compounds. Ir.sub.2.sup.0,II (tfepma).sub.3 > Cl.sub.2, was used for consideration of the stability of > third-row metal-hydride bonds, to systematically investigate > the reaction chemistry of H.sub.2, HX and X.sub.2 with > M.sub.2.sup.0,II cores. > > Homogeneous metal complexes provide a useful tool for probing > small molecule reactivity with spectroscopic techniques > available for thermodynamic and kinetic studies. Significant > advances have been made in understanding the operation of > industrial catalysts through the reactivity studies of > mononuclear inorganic and organometallic complexes. This > insight has led to the discovery of homogeneous molecular > catalysts that rival their heterogeneous brethren in both > activity and long-term stability. Furthermore, the advantage > of "molecular tuning," provides substrate and product > selectivities unprecedented in heterogeneous catalysis. > > Notwithstanding, an advantage of the heterogeneous catalyst > is the cooperative reactivity afforded by adjacent metal > centers available at the catalyst surface. Many industrial > processes from olefin polymerization to nitrogen fixation and > carbon monoxide functionalization rely on such cooperativity > for efficient operation. Though interest in multi-metallic > homogenous catalysts is longstanding, the chemistry of > transition metal clusters is less advanced than that of > mononuclear compounds. Whereas the same palette of reactions, > such as oxidative-addition, reductive-elimination and atom > transfer, is available to mononuclear and multinuclear metal > complexes, cluster compounds are distinguished by reactivity > patterns arising from cooperative effects. For example, > .beta.-hydrogen elimination is a well-known reaction observed > for late ##STR10## > > transition metal alkyl complexes leading to the formation of > a metal-hydride-olefin complex. Conversely, alkyl cluster > complexes have been observed to react by .alpha.-hydrogen > abstraction pathways; the proximity of the second metal center > can interact in a cooperative fashion to activate the nearest > C--H bond. > > The logical starting point for the development of > multi-metallic catalysts is with the simplest type of cluster > compounds. The chemistry of bimetallic transition metal > complexes largely parallels that of analogous mononuclear > complexes, since their construction is often predicated on the > assembly of mononuclear metal fragments. As an example, in > Scheme 10, the chemistry of square planar d.sup.8 metal > fragments tethered with one or more bridging ligands, typified > by pyrazolate-bridged Rh.sup.I and Ir.sup.I dimers, is > dominated by oxidative addition and reductive elimination. > Addition occurs either across the bimetallic core to yield a > d.sup.9 --d.sup.9 dimer, or is localized at one metal of the > complex to yield a d.sup.8.fwdarw.d.sup.10 complex. Subsequent > functionalization of substrates has been achieved, but > coupling of the two metal centers impedes further reactivity, > which obviates the development of an efficient catalytic > cycle. Binuclear complexes that avoid the alternate making and > breaking of a metal-metal bond show enhanced potential for > catalyst development. For example, the A-frame derived > complexes, [MM'(dppm).sub.2 (CO).sub.3 ] (M=M'=Rh, Ir; M=Ir, > M'=Rh), possess a formal metal-metal bond by virtue of > coordinative unsaturation that is maintained upon substrate > addition. As a result, further substrate addition and > functionalization reactivity is observed after the initial > activation step. > > The diphosphazane ligand framework provides an excellent > opportunity to develop new systems for small molecule > activation and transformation reactions. The coordination > chemistry of dfpma, dppma and tfepma with rhodium elucidates a > ligand framework capable of stabilizing a variety of metal > geometries and oxidation states while preserving a metal-metal > interaction. A foray into the chemistry of these ligands with > iridium, has led to the preparation of a two-electron > mixed-valence complex, Ir.sub.2.sup.0,II (tfepma).sub.3 > Cl.sub.2. The unique electronic and coordinative structure of > this compound provides a novel platform for the detailed study > of small molecule activation reactions en route to catalytic > functionalization schemes. The inventors conducted structure > and reactivity studies of Ir.sub.2.sup.0,II (tfepma).sub.3 > Cl.sub.2 with H.sub.2, HX and X.sub.2 substrates, revealing a > binuclear metal complex that maintains the facile addition > pathways of mononuclear complexes with the caveat of a > neighboring metal center to promote cooperative activation of > small molecule substrates. > > **Iridium Chemistry of dfpma and dppma** > > Building upon studies of bis(phosphine)amine ligands with > rhodium, the chemistry of these ligands with iridium was > developed. The reaction of dfpma (dfpma > =bis(difluorophosphine)methylamine) with monomeric iridium (I) > starting materials such as ClIr(CO)(PPh.sub.3).sub.2 leads to > the formation of monomeric materials, ClIr(L)(dfpma) (L=CO, > PPh.sub.3). Similarly, in the absence of a suitable ligand, > addition of two equivalents of dfpma leads to the formation of > the dfpma-chelated dimer, [ClIr(dfpma)].sub.2. Synthetic > methodologies that typically provided high-yields of > two-electron mixed-valence dirhodium products, invariably gave > intractable oils with iridium, as illustrated by the reaction > of three equivalents of dfpma and one equivalent of L > (L=P(OR).sub.3, PR.sub.3, CNR) with [ClIr(cod)].sub.2, which > affords orange to red oils that elude crystallization. > > A two-electron mixed-valence iridium complex was obtained > when dfpma was added to [ClIr(cod)].sub.2 in the presence of > excess PhICl.sub.2. A yellow microcrystalline powder was > obtained in moderate yield. X-ray diffraction studies on > single crystals yielded the results presented in FIG. 12 and > Table 11. Ir.sub.2.sup.I,III (dfpma).sub.2 Cl.sub.4 (cod) (31) > is structurally divergent from the observed rhodium dfpma > chemistry: two dfpma ligands span a binuclear iridium core > composed of octahedral Ir.sup.I and Ir.sup.III centers rotated > by 47.1.degree.. The metal-metal separation in 31 is long at > 2.8657(6) .ANG., but still within the range observed for other > diiridium complexes with a formal metal-metal bond. A single > 1,5-cyclooctadiene ligand remains coordinated to the Ir.sup.I > center, occupying an axial site and an equatorial site trans > to one chloride ligand. Three chloride ligands coordinate to > the iridium(III) center, adopting a facial geometry, with > surprisingly similar Ir.sup.III --Cl bond distances of > 2.407(3) and 2.417(3) .ANG. for the two equatorial and axial > chloride ligands, respectively. The similarity in Ir.sup.III > --Cl distances further indicates a weakened metal-metal bond; > normally a significant trans influence is observed in the M-X > distances for halogens coordinated opposite to a strong > metal-metal bond. The octahedral Ir.sup.III is completed by > two cis disposed PF.sub.2 groups, bonded at an average Ir--P > distance of 2.170(3) .ANG.. The dfpma ligands display an > induced asymmetry across the binuclear core, with an average > N--P bond distance of 1.639(10) .ANG. to the Ir.sup.III > -coordinated phosphorus and an average N--P bond distance of > 1.660(9) .ANG. to the Ir.sup.I -coordinated phosphorus. The > PF.sub.2 groups coordinated to the Ir.sup.I center adopt a > transoid arrangement (P(1)-Ir(1)-P(3)=155.56(10).degree.), > resulting in significantly longer Ir.sup.I --P distances of > 2.281(3) .ANG.. Metal-olefin distances to the C.dbd.C centroid > of the chelating 1,5-cyclooctadiene ligand are distinguished > for the axial and equatorial coordination sites at 2.222(11) > and 2.182(11) .ANG., respectively. In accord with these > different metal-olefin distances, C(3)-C(4) and C(7)-C(8) > distances of 1.381(16) and 1.356(17) .ANG., respectively, > reflect a slight decrease in C--C bond order for the more > tightly bound equatorial olefin. > > TABLE 11 Bond lengths (.ANG.) for Ir.sub.2.sup.I,III > (dfpma).sub.2 Cl.sub.4 (cod) (31). Selected Bond Lengths > (.ANG.) Ir(1)-Cl(1) 2.385(3) Ir(1)-Ir(2) 2.8657(6) Ir(1)-P(1) > 2.281(3) Ir(2)-Cl(2) 2.417(3) Ir(1)-P(3) 2.281(3) Ir(2)-Cl(3) > 2.407(3) Ir(1)-C(3) 2.294(11) Ir(2)-Cl(4) 2.407(3) Ir(1)-C(4) > 2.283(11) Ir(2)-P(2) 2.169(3) Ir(1)-C(7) 2.314(11) Ir(2)-P(4) > 2.171(3) Ir(1)-C(8) 2.332(10) P(1)-N(1) 1.667(9) P(2)-N(1) > 1.642(10) P(3)-N(2) 1.652(9) P(4)-N(2) 1.636(9) C(3)-C(4) > 1.381(16) C(7)-C(8) 1.356(17) > > To investigate whether a stronger donating, more sterically > demanding ligand might displace the 1,5-cyclooctadiene ligand, > [ClIr(cod)].sub.2 was treated with three equivalents of the > dppma ligand (dppma=MeN[P(OPh).sub.2 ].sub.2) in the absence > of excess oxidant. Insoluble molecular compounds precipitate > from reactions conducted in benzene, yielding a salmon-colored > powder. Analysis suggests the formulation Ir.sub.2 > (dppma).sub.3 Cl.sub.2 (2), indicating complete removal of > 1,5-cyclooctadiene by the three dppma ligands. X-ray quality > crystals of 32 were obtained from methylene chloride solution > cooled to -35.degree. C., and yielded the molecular structure > depicted in FIG. 13. As observed in the structure of 31, two > PNP ligands bridge the binuclear metal core, with a third > chelating dppma ligand replacing the chelating > 1,5-cyclooctadiene ligand of 31. Notably, in the absence of an > external oxidant, the divalent Ir.sub.2 core activates a C--H > bond at an ortho position of the phenyl ring of one of the > bridging dppma ligands. A metal-metal distance of 2.7919(15) > .ANG. is consistent with an Ir.sup.I.fwdarw.Ir.sup.II dative > bond. A vacant coordination site at the Ir.sup.I metal center > (P(3)-Ir(1)-P(5)=160.7(3).degree. and > P(6)-Ir(1)-Ir(2)=167.57(18).degree.) is presumably occupied by > the abstracted hydrogen atom from the orthometallated phenyl > group. .sup.1 H NMR spectroscopy of 32 confirms the presence > of a hydride ligand by the presence of a single low frequency > resonance observed at -17.08 ppm. Coordination to the hydride > to the Ir.sup.I center is established by an apparent > doublet-of-triplet-of-doublets pattern with a .sup.2 J.sub.HP > coupling constant of 218 Hz to the trans phosphorus atoms and > .sup.2 J.sub.HP couplings of 17 and 12 Hz to the cis > phosphorus atoms. > > **Preparation of Ir.sub.2.sup.0,II (tfepma).sub.3 Cl.sub.2** > > In an effort to avoid orthometallation of the bridging PNP > ligands, the reaction chemistry of tfepma with > [ClIr(cod)].sub.2 was investigated. Initial attempts to add > the tfepma ligand to iridium followed the synthetic > methodology used to prepare the dppm-bridged binuclear iridium > complex Ir.sub.2 (dppm).sub.2 Cl.sub.2 (CO).sub.2 : the > dropwise addition of a CH.sub.2 Cl.sub.2 solution of > [ClIr(cod)].sub.2 to a CH.sub.2 Cl.sub.2 solution of tfepma > under an atmosphere of CO resulted in the formation of an > orange solution. After 48 hours, dark green, X-ray quality > crystals precipitated from solution. FIG. 14 presents the > molecular structure of Ir.sub.2.sup.0,II (tfepma).sub.3 > Cl.sub.2 (33) as determined from the X-ray diffraction data, > Table 12 presents selected bond distances and angles of the > bimetallic iridium core. As observed in the structure of 32, > two of the three bidentate ligands bridge the binuclear core > of 33 with the third ligand binding as a chelate. The Ir.sup.0 > center possesses distorted trigonal bipyramidal geometry that > is typical for d.sup.9 metals. Two equatorial sites of the > Ir.sup.0 center are coordinated by phosphites from the > bridging tfepma ligands with the third equatorial site > occupied by one end of a chelating tfepma ligand. The other > end of the chelating ligand caps the axial position of the > Ir.sup.0 center at a short Ir--P distance of 2.201(5) .ANG., > and a metal-metal bond distance of 2.7871(8) .ANG. joins the > two metal centers. The square pyramidal Ir.sup.II center is > characterized by a regular basal plane tilted by 8.degree. > from normal to the Ir(1)-Ir(2) vector. Two cis equatorial > sites are occupied by phosphites from the bridging tfepma > ligands at an average Ir--P distance of 2.192(5) .ANG., while > the other two equatorial sites are occupied by chloride > ligands at an average Ir--Cl distance of 2.372(5) .ANG.. > > TABLE 12 Bond lengths (.ANG.) and angles (deg) for > Ir.sub.2.sup.0,II (tfepma).sub.2 Cl.sub.2 (33). Selected Bond > Lengths (.ANG.) Ir(1)-Ir(2) 2.7876(10) Ir(2)-Cl(1) 2.379(5) > Ir(1)-P(1) 2.235(6) Ir(2)-Cl(2) 2.365(5) Ir(1)-P(3) 2.274(5) > Ir(2)-P(2) 2.198(5) Ir(1)-P(5) 2.268(5) Ir(2)-P(4) 2.186(5) > Ir(1)-P(6) 2.201(5) P(1)-N(1) 1.667(17) P(2)-N(1) 1.693(17) > P(3)-N(2) 1.649(16) P(4)-N(2) 1.686(16) Selected Bond Angles > (deg) P(5)-Ir(1)-P(1) 136.7(2) Cl(1)-Ir(2)-Cl(2) 85.3(2) > P(5)-Ir(1)-P(3) 115.7(2) Cl(1)-Ir(2)-P(2) 88.0(2) > P(5)-Ir(1)-P(6) 69.4(2) Cl(1)-Ir(2)-P(4) 169.50(19) > P(6)-Ir(1)-Ir(2) 164.04(15) > > The synthesis of 33 shown in FIG. 14 can be targeted directly > by reacting [ClIr(cod)].sub.2 with three equivalents of tfepma > in CH.sub.2 Cl.sub.2. Dark green crystalline 33 precipitates > from the dark red solution of tfepma and the iridium starting > material. Alternatively, slightly higher yields are obtained > if the reaction is carried out in refluxing benzene, but the > necessity to recrystallize the product reduces the value of > this preparative method. The reactivity of 33 is outlined in > Scheme 11. > > **Ligand Exchange Reactions of Ir.sub.2 0.sup.,II > (tfepma).sub.3 Cl.sub.2** > > **Solvent Exchange Reactions of 33 (I of Scheme 11)** > > .sup.1 H NMR and .sup.31 P NMR spectroscopy reveal a > fluxional coordination environment for 33 in which the > diiridium complex is under dynamic solvent exchange. At room > temperature, d.sup.8 -THF solutions of 33 show a .sup.31 P NMR > spectrum of four distinct resonances, albeit with significant > line broadening, consistent with a C.sub.s symmetric structure > for 33 in solution (FIG. 15(a)). A low frequency singlet at > 20.91 ppm is assigned to the axial phosphorus coordinated to > the Ir.sup.0 center; the apparent triplet at 65.59 ppm is the > equatorial phosphorus of the chelating tfepma ligand. The > excessively broad singlet at 80.19 ppm is assigned to the > Ir.sup.II -coordinated phosphites leaving the high-frequency > resonance to the Ir.sup.0 -coordinated phosphites of the > bridging tfepma ligands. The .sup.1 H NMR spectrum at > 20.degree. C. is consistent with a symmetric complex as well, > only two methyl resonances at 2.93 and 2.62 ppm are observed > for the tfepma ligands, integrating in a 2:1 ration for the > bridging and chelating ligands, respectively. Upon cooling to > -80.degree. C., the fluxional behavior of 33 is arrested, > giving the NMR spectra of FIG. 15(b). The resonance for the > chelating tfepma ligand is largely unchanged in the .sup.1 H > NMR spectrum, however, the resonance for the bridging tfepma > ligand is split into distinct signals at 3.17 and 2.70 ppm > (.DELTA.=238 Hz), indicating an inequivalence of the bridging > tfepma ligand. Even more dramatic changes are observed in the > .sup.31 P NMR spectrum. In addition to a significant > improvement in line shape for the resonances of the chelating > tfepma ligand, two distinct signals can be resolved in the > 100-110 ppm region for the equatorial phosphites of the > bridging tfepma ligands. The most striking feature is the > separation of two very different Ir.sup.II -phosphite > resonances, at 78.31 and 89.77 ppm (.DELTA.=2321 Hz), > immediately suggesting the coordination of different ligands > across the metal center from the phosphorus atoms. > > Rate constants for the fluxional process equilibrating the > Ir.sup.II -phosphites were determined by monitoring the .sup.1 > H methyl resonances of the bridging tfepma ligands in d.sup.8 > -THF over the temperature range of -70.degree. C. to > +30.degree. C.; analysis of the Eyring plot yields activation > parameters of .DELTA.H.sup.{character pullout} =13.+-.1 kcal > mol.sup.-1 and .DELTA.S.sup.{character pullout} =6.6.+-.2 cal > mole.sup.-1 K.sup.-1. A similar exchange process is observed > in CD.sub.3 CN, and evaluation of the corresponding kinetic > data reveals a strongly solvent dependent process: over a > temperature range of -5.degree. C. to +30.degree. C., > .DELTA.H.sup.{character pullout} and .DELTA.S.sup.{character > pullout} were determined to be 25.+-.4 kcal mol.sup.-1 and > 38.+-.5cal mol.sup.-1 K.sup.-1, respectively. The positive > activation entropies in both solvent systems comply with a > dissociative process. This, taken with the differences in > chemical shift for the Ir.sup.II -phosphites suggests the > equilibrium depicted by reaction (i) of Scheme 11, in which a > THF or MeCN ligand reversibly binds to an equatorial Ir.sup.II > site with concomitant shift of a halide to the position > opposite the metal-metal bond. ##STR11## > > The solvent adduct 34, see FIG. 16 has been isolated and > structurally characterized; FIG. 16(a) shows a thermal > ellipsoid plot for Ir.sub.2.sup.0,II (tfepma).sub.3 Cl.sub.2 > (MeCN) (4-MeCN). As deduced from NMR studies, the coordination > core of the parent complex, 33 in Scheme 11, is mostly > unchanged, with two chelating tfepma ligands and a third > tfepma ligand chelated to the Ir.sup.0 center; a slight > elongation of the metal-metal separation accompanies > coordination of the acetonitrile ligand. Table 13 presents > other pertinent metrical parameters of the Ir.sup.0 > --Ir.sup.II core of 34. > > **Addition of Strong .sigma.-Donors to 33 (ii of Scheme 11)** > > In contrast to the solution behavior of 33, .sigma.-donating > ligands such as isonitriles, phosphines and even halides, > coordinate the Ir.sup.II center at the axial position, trans > to the metal-metal bond yielding species of the formulation > Ir.sub.2.sup.0,II (tfepma).sub.3 Cl.sub.2 (L) (35-L, L=CNR, > PR.sub.3, X.sup.-). As is apparent in the thermal ellipsoid > plot of the CN.sup.t Bu derivative, Ir.sub.2.sup.0,II > (tfepma).sub.3 Cl.sub.2 (CN.sup.t Bu) (35-CN.sup.t Bu) shown > in FIG. 16(b), the Ir.sub.2.sup.0,II mixed-valence core is > preserved upon addition of the donor ligand. Apart from the > differing coordination positions of the MeCN and CN.sup.t Bu > ligands, the X-ray crystal structure of 35-CN.sup.t Bu is > largely undistinguished from that of 34. Metrical parameters > of the bimetallic core are presented for comparison in Table > 13. In agreement with the solid-state results, the integration > ratios for the proton resonances of the axial ligands of 35-L > to those of the tfepma ligands establish that only one donor > ligand is incorporated into the diiridium coordination sphere. > Moreover, room temperature NMR spectra of the addition > products with strong .sigma.-donor ligands reveal static > solution structures that are consistent with the results of > X-ray crystallography. Notably, the Ir.sup.II -coordinated > phosphites of the 35-L species give rise to sharp, apparent > triplets in the .sup.31 P{.sup.1 H} NMR spectrum between 66 > and 73 ppm. The absence of fluxional behavior is also in > evidence from the sharp high frequency doublet resonances at > about 95 ppm for the Ir.sup.0 -coordinated phosphites of the > bridging ligands. The .sup.31 P resonance for the axial > Ir.sup.0 -phosphite is sensitive to the coordination of an > axial ligand at Ir.sup.II, shifting to progressively higher > frequency (.delta.=35.0, 52.5 and 53.3 ppm along the series > L=Br.sup.-, PEt.sub.3, CN.sup.t Bu) with increasing L > .sigma.-donor strength. > > TABLE 13 Selected bond lengths (.ANG.) for Ir.sub.2.sup.0,II > (tfepma).sub.3 Cl.sub.2 (MeCN) (4), Ir.sub.2.sup.0,II > (tfepma).sub.3 Cl.sub.2 (CN.sup.t Bu) (35- CN.sup.t Bu) and > [Ir.sub.2.sup.0,II (tfepma).sub.3 (MeCN).sub.3 ][PF.sub.6 > ].sub.2 (6[PF.sub.6 ].sub.2). Ir.sub.2.sup.0,II (tfepma).sub.3 > Cl.sub.2 (MeCN) Ir.sub.2.sup.0,II (tfepma).sub.3 Cl.sub.2 > (CN.sup.t BU) [Ir.sub.2.sup.0,II (tfepma).sub.3 (MecN).sub.3 > ].sup.2+ Ir(1)-Ir(2) 2.7964(11) Ir(1)-Ir(2) 2.8088(1) > Ir(1)-Ir(2) 2.7805(7) Ir(1)-P(1) 2.216(2) Ir(1)-P(1) 2.215(5) > Ir(1)-P(1) 2.230(3) Ir(1)-P(3) 2.225(2) Ir(1)-P(3) 2.225(6) > Ir(1)-P(3) 2.231(3) Ir(1)-P(5) 2.272(2) Ir(1)-P(5) 2.317(6) > Ir(1)-P(5) 2.280(3) Ir(1)-P(6) 2.227(2) Ir(1)-P(6) 2.233(6) > Ir(1)-P(6) 2.216(4) Ir(2)-P(2) 2.186(2) Ir(2)-P(2) 2.206(6) > Ir(2)-P(2) 2.220(4) Ir(2)-P(4) 2.176(2) Ir(2)-P(4) 2.188(6) > Ir(2)-P(4) 2.194(3) Ir(2)-Cl(1) 2.427(2) Ir(2)-Cl(1) 2.452(5) > Ir(2)-N(5) 2.079(12) Ir(2)-N(4) 2.122(7) Ir(2)-Cl(2) 2.429(6) > Ir(2)-N(6) 2.089(12) Ir(2)-Cl(2) 2.512(2) Ir(2)-C(4) 2.03(2) > Ir(2)-N(4) 2.183(12) > > **Halogen Removal from 33 (iii of Scheme 11)** > > Halogen removal from 33 can be effected with silver or > thallium hexafluorophosphate in acetonitrile solution. A > highly crystalline product analyzing as [Ir.sub.2.sup.0,II > (tfepma).sub.3 (MeCN).sub.3 ][PF.sub.6 ].sub.2 (6[PF.sub.6 > ].sub.2) is recovered in quantitative yield. Solution NMR > spectroscopy suggests preservation of the Ir.sub.2.sup.0,II > core. Excepting the resonance for the PF.sub.6 anions at -143 > ppm, the 31P NMR spectrum of 36 in FIG. 17 shows a four-line > pattern analogous to that observed for the C.sub.s symmetric > complexes 35-L. The axial phosphorus of the chelating tfepma > ligand is observed as a singlet at 28 ppm, whereas the > equatorial phosphorus is observed at 50 ppm as a triplet > displaying a .sup.2 J.sub.PP coupling constant of 273 Hz to > the doublet at 89 ppm for the Ir.sup.0 phosphorus atoms of the > bridging tfepma ligands. Finally, the Ir.sup.II phosphorus > atoms give a single resonance at 57 ppm. Similarly, the .sup.1 > H NMR spectrum of 36 displays two resonances for the tfepma > methyl groups at 2.83 and 2.70 ppm, the 2:1 integration ratio > is consistent with the expected bridging/chelating > coordination mode. Complete exchange of the MeCN ligands > occurs upon dissolution of the solid as evidenced by a singlet > at 1.96 ppm for uncoordinated MeCN. Single crystals > diffraction analysis of the product confirm the preservation > of the Ir.sub.2.sup.0,II core as depicted in FIG. 17. For > comparison purposes, the metric parameters for the core of 36 > are presented in Table 13 alongside those of Ir.sub.2.sup.0,11 > complexes 34 and 35-L. Removal of the halogen ligands results > in a contracted metal-metal separation of 2.7805(7) .ANG., as > well as a shorter axial Ir.sup.0 --P bond. Conversely, whereas > the equatorial Ir.sup.0 --P bond distances are similar in > 34-36, the Ir.sup.II --P distances are elongated by nearly > 0.02 .ANG. in 36. > > **Oxidative Addition Reactions of Ir.sub.2.sup.0,II > (tfepma).sub.3 Cl.sub.2** > > **Chlorine Addition to 3 (iv and v of Scheme 11)** > > Chlorine, in the form of its iodobenzene adduct, facilely > adds to 33 to give the two-electron mixed-valence complex > Ir.sub.2 I,III (tfepma).sub.3 Cl4 (37) as shown in reaction > (iv) of Scheme 11. X-ray crystallographic studies on single > crystals of 37 yielded the molecular structure depicted in > FIG. 18(a). Halogen addition occurs across the metal-metal > bond of 33. The Ir--Ir distance of 2.7765(8) .ANG. (Table 14) > is well within the range for a metal-metal bond. Simple > electron counting arguments are consistent with the > formulation of an Ir.sup.I.fwdarw.Ir.sup.III dative bond where > both metals assume octahedral coordination geometry. The > octahedral metal centers of 37 are rotated with respect to one > another by an average value of 32.degree.. The Ir.sup.III --Cl > bonds are noticeably longer than those for the reduced > Ir.sub.2.sup.0,II complexes, at an average value of 2.446(4) > .ANG.. This result is peculiar in light of the anticipated > contraction of the iridium radius upon oxidation of Ir.sup.II > to Ir.sup.III. The coordination of the bridging tfepma ligands > is unchanged from 33; however, the Ir--P distances associated > with the chelating ligand elongate by .about.0.1 .ANG.. > > NMR spectra of 37 are consistent with the octahedral > coordination geometry of the oxidized metal core. The distinct > environments of a chelating and two bridging ligands are > signified by ligand methyl resonances in the .sup.1 H NMR > spectrum at 2.71 ppm and 2.88 and 2.93 ppm, respectively. The > .sup.31 P{.sup.1 H} NMR spectrum of 37 consists of six > separate resonances, one for each of the unique phosphites > under C.sub.1 symmetry. Referring to the numbering scheme of > FIG. 18(a), P(3) and P(5) are expected to be strongly coupled > owing to their trans arrangement. In this context, signals at > 13.14 and 74.31 ppm are ascribed to P(5) and P(3), > respectively, based on a .sup.2 J.sub.PP coupling constant of > 901 Hz. As in the reduced Ir.sub.2.sup.0,II complexes, a low > frequency resonance at 9.24 ppm is attributed to the P(6) > phosphite trans to the Ir--Ir bond. Based on the .sup.31 P > COSY spectrum of 37, the 66.46-ppm resonance is ascribed to > the Ir.sup.I -bound P(1) phosphite of the bridging ligand, > while the signals at 54.98 and 57.11 ppm are assigned to > Ir.sup.III -bound P(2) and P(4) phosphites of the bridging > ligands, respectively. > > TABLE 14 Selected bond lengths (.ANG.) and angles (deg) for > Ir.sub.2.sup.I,III (tfepma).sub.3 Cl.sub.4 (37),.sup.a > equatorial Ir.sub.2.sup.I,III (tfepma).sub.3 HCl.sub.3 (40) > and Ir.sub.2.sup.I,III (tfepma).sub.3 H.sub.2 Cl.sub.2 (42). > Ir.sub.2.sup.I,III (tfepma).sub.3 Cl.sub.4.sup.b > Ir.sub.2.sup.I,III (tfepma).sub.3 HCl.sub.3.sup.c > Ir.sub.2.sup.I,III (tfepma).sub.3 H.sub.2 Cl.sub.2.sup.d > Selected Bond Lengths (.ANG.) Ir(1)-Ir(2) 2.7765(8) 2.7775(11) > 2.7561(7) Ir(1)-X(1) 2.435(4) -- -- Ir(2)-Cl(2) 2.405(4) > 2.450(2) 2.465(3) Ir(2)-X(3) 2.428(4) 2.418(2) -- Ir(2)-Cl(4) > 2.504(4) 2.487(2) 2.511(3) Ir(1)-P(1) 2.223(4) 2.314(2) > 2.300(3) Ir(1)-P(3) 2.282(4) 2.241(2) 2.259(3) Ir(1)-P(5) > 2.375(4) 2.322(2) 2.271(3) Ir(1)-P(6) 2.350(4) 2.269(2) > 2.278(3) Ir(2)-P(2) 2.198(4) 2.188(2) 2.160(3) Ir(2)-P(4) > 2.191(4) 2.175(2) 2.277(3) Selected Bond Angles (deg) > P(1)-Ir(1)-X(1) 173.3(2) -- -- P(1)-Ir(1)-P(3) 93.4(2) > 100.60(8) 96.70(11) P(1)-Ir(1)-P(5) 99.9(2) 103.61(7) > 93.99(11) P(2)-Ir(2)-P(4) 96.0(2) 94.05(8) 103.61(12) > P(2)-Ir(2)-Cl(2) 170.7(2) 175.14(7) 169.33(12) P(2)-Ir(2)-X(3) > 86.2(2) 89.13(8) -- P(6)-Ir(1)-Ir(2) 165.20(11) 167.41(6) > 158.45(10) Cl(4)-Ir(2)-Ir(1) 178.07(10) 171.62(5) 176.34(8) > Selected Torsion Angles (deg) X(1)-Ir(1)-Ir(2)-Cl(2) 39.4 19.2 > 7.2 P(1)-Ir(1)-Ir(2)-P(2) 24.4 15.2 18.5 P(3)-Ir(1)-Ir(2)-P(4) > 27.0 21.9 11.5 P(5)-Ir(1)-Ir(2)-X(3) 37.9 0.7 1.6 .sup.a The > bond lengths and distances presented for 37 are the average > values for two crystallographically distinct but chemically > equivalent molecules within the unit cell. .sup.b X(1) = X(3) > = Cl. .sup.c X(1) = H, X(3) = Cl. .sup.d X(1) = X(3) = H > > Upon treatment with excess oxidant, 37 loses the chelating > tfepma ligand according to reaction (v) of Scheme 11. The > liberated tfepma is in turn oxidized, preventing its > incorporation back into the coordination sphere of the > binuclear core. A bright yellow solid analyzing as Ir.sub.2 > (tfepma).sub.2 Cl.sub.4 (MeCN).sub.2 (38), and possessing > relatively simple NMR spectra, is obtained. The .sup.1 H NMR > spectrum comprises a single methyl resonance at 2.80 ppm and > four methylene resonances between 4.48 and 5.46 ppm for the > tfepma ligands. The .sup.1 H NMR signal of CH.sub.3 CN is that > of free ligand indicating that the bound solvent molecule is > exchanged immediately upon dissolution of solid samples of the > compound. The .sup.31 P NMR spectrum of 38 exhibits two > resonances at 54.97 and 57.87 ppm with a simple AA'BB' > coupling pattern. These NMR results point towards a symmetric > complex, which is verified by X-ray diffraction studies (FIG. > 18(b)). Two bridging cis-diphosphazane ligands span a > valence-symmetric Ir.sub.2.sup.II,II core supporting > octahedral coordination geometries that are related to each > other by a 30.degree. twist about the Ir--Ir axis. A > metal-metal bond distance of 2.7525(9) .ANG. signifies a > formal bonding interaction that is characteristic of a d.sup.7 > --d.sup.7 complexes. Each metal center is coordinated by one > equatorial and one axial chloride ligand, leaving acetonitrile > to complete the octahedral coordination spheres of the metal > centers. The Ir--P bond distances average 2.206(5) .ANG., and > the Ir--Cl bond distances are 2.432(5) and 2.476(5) .ANG. for > the equatorial and axial halogens, respectively. > > The lability of the acetonitrile ligands suggested that their > displacement by a tfepma ligand would provide access to a > symmetric Ir.sub.2.sup.II,II Cl.sub.4 complex spanned by three > bridging ligands, similar to that observed for the chemistry > of rhodium with dfpma and tfepma. Addition of one equivalent > of tfepma to solutions of 38 in CH.sub.2 Cl.sub.2, however, > leads to nearly quantitative (>90%) conversion to the > Ir.sub.2.sup.I,III complex, 37, as determined with NMR > spectroscopy. > > **Acid Addition to 33 (vi-viii of Scheme 11)** > > Suspensions of 33 in CH.sub.2 Cl.sub.2 readily react with > anhydrous HCl gas. Analysis of the final product provides the > formulation Ir.sub.2 (tfepma).sub.3 HCl.sub.3 (40), indicating > oxidative addition of HCl has occurred. An Ir--H stretch in > the IR spectrum at 2115 cm.sup.-1 is consistent with the > presence of a terminal hydride ligand situated trans to a > phosphorus atom. FIG. 19 displays the results of single > crystal X-ray data analysis of 40 as a thermal ellipsoid plot; > selected bond distances and angles are listed in Table 14. As > observed in the halogen addition reaction, a metal-metal > separation of 2.7775(11) .ANG. is consistent with an > Ir.sup.I.fwdarw.Ir.sup.III formulation containing a dative > bond. Interestingly, the octahedral metal centers are nearly > eclipsed with an average torsion angle of only 14.degree.. A > conspicuously vacant site in the X-ray crystal structure of 40 > confirms the location of the hydride in the equatorial plane > of the Ir.sup.I center (P(3)-Ir(1)-P(5)=153.90(7).degree. and > P(6)-Ir(1)-Ir(2)=167.41(6).degree.). Moreover, subsequent to > the location of all non-hydrogen atoms, the Fourier difference > map showed a single peak in the vacant iridium coordination > site of appropriate intensity for a hydride ligand though the > proximity of the hydride to a heavy nucleus precludes the > determination of an accurate Ir--H distance. Further evidence > for the hydride location comes from the elongated Ir(1)-P(1) > bond distance, resulting from the strong trans influence of > the hydride ligand. The Ir(1)-P(1) bond distance of 2.314(2) > .ANG. is 0.091(3) .ANG. longer than that of observed in the > chloride analog 37. Excluding Ir(1)-P(1), all other > metal-ligand bond distances of 40 are similar to those > observed in 37. > > The results of NMR spectroscopy are consistent with the X-ray > structural studies. A single hydride resonance is observed in > the .sup.1 H NMR spectrum of 40 (FIG. 20(a)) at -10.24 ppm. A > 178 Hz .sup.2 J.sub.PH coupling constant confirms the > coordination of a phosphorus trans to the hydride is > maintained in solution. The three different tfepma ligand > environments are distinguished in the .sup.1 H NMR spectrum by > unique methyl resonances at 2.65, 2.77 and 2.89 ppm. .sup.31 > P-.sup.1 H HMQC experiments were used to assign a .sup.31 P > NMR resonance at 86.4 ppm as the Ir.sup.I phosphite > coordinated trans to the hydride ligand. The high frequency > shift of this resonance follows from the strong trans > influence of the hydride ligand observed in the solid-state > structure. Two resonances at 64.4 and 67.8 ppm in the .sup.31 > P NMR spectrum are assigned to Ir.sup.III phosphites, whereas > the low frequency singlet at 21.6 ppm is assigned to the > axially coordinated phosphite of the chelating ligand. As in > 37, a strong .sup.2 J.sub.PP of 761 Hz observed in resonances > at 26.6 and 82.2 ppm points to their assignment as the trans > disposed Ir.sup.I -phosphites of the chelating and bridging > tfepma ligands, respectively. > > At early reaction times, another isomer of Ir.sub.2 > (tfepma).sub.3 HCl.sub.3 with an axial hydride ligand is > observed (39 in Scheme 11). As indicated by reactions (vi) and > (vii) of Scheme 11, 39 converts to 40 upon stirring in > CH.sub.2 Cl.sub.2. Examination of the Ir--H stretching region > of the IR spectrum gives a single stretch at 2037 cm.sup.1, > and the .sup.1 H NMR spectrum of 39 shown in FIG. 20(b) shows > a single hydride resonance at -13.0 ppm. The absence of a > large .sup.2 J.sub.PH coupling in the low frequency resonance > suggests only cis H,P interactions, requiring protonation to > occur at the axial coordination site of either the Ir.sup.0 or > Ir.sup.II center. The .sup.31 P NMR spectrum of 39 shows > strong .sup.2 J.sub.PP couplings of 795 and 752 Hz in both the > 35.7 and 47.9-ppm resonances of the chelating phosphite, > respectively. Moreover, the resonances for the other Ir.sup.I > phosphites at 80.9 and 88.7 ppm show the same 795 and 752 Hz > coupling constants. Finally, the chemical shifts and coupling > patterns of the Ir.sup.III -coordinated phosphites at 63.8 and > 66.3 ppm suggest an Ir.sup.III center equivalent to that > observed in the final product 40. These NMR data suggest the > reaction sequence shown in Scheme 11. > > In order to elucidate further the initial steps of acid > addition to 33, the protonation reaction was studied with the > acids of non-coordinating anions. Addition of neat triflic > acid to suspensions of 33 in CH.sub.2 Cl.sub.2 yields no > appreciable reaction, even after 24 h, in stark contrast to > the instantaneous addition of HCl to suspensions of 33. > However, if the triflic acid is added as a solution in MeCN, > rapid dissolution of the solid occurs to give a pale yellow, > almost colorless solution from which a pale yellow solid > precipitates. Spectroscopic studies suggest the formulation > Ir.sub.2.sup.I,III (tfepma).sub.3 HCl.sub.2 (MeCN) (41) with a > structure analogous to 39 as shown in reaction viii of Scheme > 11. The presence of a hydride ligand is indicated by an Ir--H > stretching mode at 2042 cm.sup.-1 in the infrared spectrum of > the product as well as a single low frequency hydride > resonance at -12.67 ppm (FIG. 20(c)) in the .sup.1 H NMR > spectrum. The .sup.31 P NMR spectrum of 41 shows other > similarities to 39. Two pairs of strongly coupled phosphite > signals are observed: resonances at 43.0 and 48.4 ppm can be > assigned to the chelating tfepma ligand coordinated to > Ir.sup.I with .sup.2 J.sub.PP coupling constants of 740 and > 720 Hz, respectively, reflected in the resonances for the > other Ir.sup.I phosphites at 75.9 and 85.0 ppm. Two remaining > peaks at 53.6 and 66.9 ppm are in the range for phosphites at > the Ir.sup.III center. In this case the low frequency shift of > the former resonance results from coordination of an > acetonitrile molecule across the Ir.sup.III center as observed > for 33 in solution. > > As observed for 33, the MeCN ligand of 41 undergoes exchange > in CD.sub.3 CN solvent. The disappearance of the coordinated > MeCN signal is complemented by the appearance of a signal for > free MeCN at 1.96 ppm. The exchange process is sufficiently > slow such that the loss in intensity of the .sup.1 H resonance > of the Ir.sup.III -coordinated MeCN may be easily monitored > over the course of a day. A plot of In I vs t is linear > (R.sup.2 =0.9984), yielding a first-order decay rate constant > of k.sub.H =1.25.times.10.sup.-4 s.sup.-1. Interestingly, the > MeCN exchange process is significantly accelerated (k.sub.D > =1.90.times.10.sup.-4 sec.sup.-1, R.sup.2 =0.9985) when 33 is > deuterated by DOTf, yielding an inverse kinetic isotope effect > of 0.66. > > **Reversible H.sub.2 Addition to 33 (ix of Scheme 11)** > > Hydrogen adds to 3 with equal facility to the X.sub.2 and HX. > Suspensions of 3 in CH.sub.2 Cl.sub.2 rapidly afford a pale > yellow solution upon bubbling with hydrogen gas at room > temperature to yield Ir.sub.2 I.sup.,III (tfepma).sub.3 > H.sub.2 Cl.sub.2 (42) as shown in reaction (ix) of Scheme 11. > The reaction can be reversed with N.sub.2 purging. Two > iridium-hydride resonances appear in the low frequency region > of the .sup.1 H NMR spectrum at -11.51 and -8.32 ppm signaling > H.sub.2 addition to the Ir.sub.2.sup.0,II core. FIG. 20(d) > reveals large .sup.2 J.sub.PH coupling constants in both > hydride resonances of 42. A coupling constant of 172 Hz in the > low frequency doublet is commensurate with the 178 Hz coupling > constant observed for the Ir.sup.I hydride in the equatorial > isomer of 40. An even larger .sup.2 J.sub.PH coupling constant > of 270 Hz observed in the -8.32 ppm resonance points toward an > equatorial hydride ligand at the Ir.sup.III center, where the > contracted radius of the oxidized metal center leads to an > even larger coupling constant to a trans phosphorus. The > .sup.31 P NMR spectrum of 42 shows a six-resonance pattern > similar to those observed for complexes 37 and 40, supporting > the Ir.sub.2.sup.I,III (tfepma).sub.3 H.sub.2 Cl.sub.2 > formulation. The chelating ligand resonances appear shifted to > low frequency as a doublet-of-triplets at 17.8 ppm and a > strongly coupled doublet at 45.3 ppm (2J.sub.PP =750 Hz). This > 750-Hz coupling constant is mirrored in a resonance at 95.5 > ppm, easily identifying this resonance as an Irl-phosphite > from a bridging tfepma ligand. .sup.31 P-.sup.1 H HMQC > experiments provided coupling-correlation of the .sup.31 P NMR > resonances at 86.8 ppm and 99.4 ppm to the Ir.sup.III and > Ir.sup.I -coordinated hydrides, respectively. A peak at 71.3 > ppm is assigned to the remaining Ir.sup.III phosphite, located > trans to a chloride ligand. > > Oxidative addition of hydrogen across the diiridium bond to > give a HIr.sup.I.fwdarw.Ir.sup.III Cl.sub.2 H core is > confirmed by the X-ray crystal structure of Ir.sub.2.sup.I,III > (tfepma).sub.3 H.sub.2 Cl .sub.2 shown in FIG. 21; selected > bond distances and angles are presented in Table 14. Though > the Ir.sup.III -coordinated hydride could not reliably be > located (the Ir.sup.I -coordinated hydride was located in the > difference Fourier map), the vacant coordination sites of each > octahedral ligand sphere establishes the location of the > hydride ligands (P(5)-Ir(1)-P(3)=168.72(12), > P(6)-Ir(1)-Ir(2)=158.46(10) and P(2)-Ir(2)-Cl(2)=169.35(12) > Cl(4)-Ir(2)-Ir(1)=176.35(8)). Furthermore, the Ir(1)-P(1) and > Ir(2)-P(4) bond distances of 2.300(3) and 2.277(3) .ANG. are > significantly longer than the same distances in > Ir.sub.2.sup.I,III (tfepma).sub.3 Cl.sub.4, in accord with the > trans influence associated with the terminal hydride ligands. > The average twist angle about the Ir--Ir bond axis is only > 10.degree.; the H(1)-Ir(1)-Ir(2)-H(2) dihedral angle in the > solid state is 88.degree.. The diiridium bond distance is > significantly shorter at 2.7561(7) .ANG. than those observed > in Ir.sub.2.sup.I,III complexes Ir.sub.2.sup.I,III > (tfepma).sub.3 Cl.sub.4 and Ir.sub.2.sup.I,III (tfepma).sub.3 > HCl.sub.3, and in fact is more comparable to the bond distance > observed in the Ir.sub.2.sup.II,II complex, Ir.sub.2.sup.II,II > (tfepma).sub.2 Cl.sub.2 (MeCN).sub.2. Other metrical > parameters of Ir.sub.2.sup.I,III (tfepma).sub.3 H.sub.2 > Cl.sub.2 are largely unchanged from the other > Ir.sub.2.sup.I,III complexes. > > The equilibrium isotope effect may be evaluated for hydrogen > addition to 33 according to reaction (ix) of Scheme 11. > Addition of 1 atm of an equimolar mixture of H.sub.2 and > D.sub.2 to an NMR tube containing 33 in d.sup.8 -THF results > in the rapid color change to yellow associated with hydrogen > addition. Integration of the .sup.1 H NMR spectrum after > .about.30 min yielded a ratio of 42 to 42-d.sub.2 of > 0.90.+-.0.05. The ratio remained constant for several hours, > until significant HID exchange prevented further measurements. > > The .sup.1 H NMR spectrum of 42 in d.sup.8 -THF was observed > to evolve slowly for several days. Heating accelerates this > reaction; d.sup.8 -THF solutions of 42 heated to 80.degree. C. > under an H.sub.2 atmosphere are converted to new products as > evidenced by .sup.1 H and .sup.31 P NMR spectroscopy. An > integration ratio of nine methyl protons of three tfepma > ligands to two hydride ligands suggests that no subsequent > H.sub.2 addition has occurred. Assignment of the reaction > products is preliminary, but .sup.1 H and .sup.31 P NMR > suggest the formation of a 1:1 ratio of two major iridium > hydride products, 43a and 43b depicted in Scheme 12, with the > same empirical formula as 42. Several overlapping resonances > in the tfepma methyl and methylene regions precludes their > utility in making structural assignments. However, the hydride > region shows four distinct signals at -11.23, -12.63, -13.71 > and -14.07 ppm that account for 90% of 42 (additional smaller > peaks are observed at -12.85 and -13.78 ppm). The three high > frequency hydride resonances show .sup.2 J.sub.HP coupling > constants diagnostic of hydride coordination trans to a > phosphorus ligand: .sup.2 J.sub.HP =184, 177 and 181 Hz, > respectively. The low frequency, -14.07-ppm ##STR12## > > resonance is an apparent quartet with only C is .sup.2 > J.sub.HP couplings. The .sup.31 P{.sup.1 H} NMR spectrum > confirms the presence of two principal reaction products by > the appearance of twelve distinct phosphorus resonances (as > discussed above, the Ir.sub.2.sup.I,III complexes 37 and 39-42 > typically show six unique phosphorus environments). > > Assignment of the structure for 43a begins with the > diagnostic pair of resonances observed in the 31P NMR spectrum > for a chelating tfepma ligand at 41.7 and 59.0 ppm, with the > former displaying a 692 Hz coupling constant. This .sup.2 > J.sub.PP coupling is reflected in a high frequency resonance > at 99.9 ppm, confirming a trans phosphite arrangement on an > Ir.sup.I center. The chemical shift of the -11.23-ppm hydride > resonance is consistent with the chemical shift of the > equivalent Ir.sup.I hydride of 32. Selective decoupling > experiments show strong correlation between this and a .sup.31 > P resonance at 85.8 ppm; a .sup.2 J.sub.HP -coupling constant > of 184 Hz is also congruent with the coupling constant for the > same hydride-phosphite pair in 42. .sup.2 J.sub.PP couplings > observed in the 99.9 and 85.8-ppm 31p resonances are reflected > in resonances at 72.5 and 63.6 ppm, respectively, and are > characteristic of phosphorus-phosphorus couplings through the > nitrogen bridgehead of the tfepma ligand. Finally, equatorial > chlorides and an axial hydride (-14.07 ppm) complete the > Ir.sup.III coordination sphere; the axial assignment of the > hydride is based on the observed high frequency shift of the > axial Ir.sup.I phosphite singlet to 59.0 ppm. > > Of the twelve phosphorus resonances the remaining six and two > hydride resonances characterize 13b. Notably, none of the > .sup.31 P resonances display a large .sup.2 J.sub.PP coupling > constants, indicating a lack of trans disposed phosphite > groups, furthermore, both hydride resonances show signature > .sup.2 J.sub.HP couplings distinctive for a hydride > coordinated trans to a phosphorus. Based on this evidence, as > shown in Scheme 2.3, valence disproportionation to yield an > Ir.sub.2.sup.II,II species is tentatively suggested for 43b. > In support of this assignment, the chemical shifts and the > observed phosphorus-hydrogen coupling constants of the hydride > ligands are not consistent with those observed for the > Ir.sup.III -hydride ligand of 42 (.delta.=-8.32 ppm, .sup.2 > J.sub.HP= 270 Hz). Furthermore, no low-frequency .sup.31 P > resonances, characteristic of phosphite coordination to an > Ir.sup.I center, are observed. > > **Organometallic Aspects of Two-Electron Mixed-Valence > Reactivity** > > The reactivity of Ir.sub.2.sup.0,II (tfepma).sub.3 Cl.sub.2 > with dihydrogen provided the impetus for investigating the > organometallic chemistry of the two-electron mixed-valence > platform. Preliminary experiments indicate that alkyl > derivatives of 33 can be prepared, and that the > Ir.sub.2.sup.0,II core is maintained. Treatment of 33 with one > equiv of methide source MeMgBr or MeLi at low temperature in > THF results in a color change from brown to yellow. Upon > warming to room temperature the color returns to brown. > Solvent removal followed by trituration with CH.sub.2 Cl.sub.2 > affords a gray-green powder in moderate yield. The 31P NMR > reveals six different phosphorus environments consistent with > the solution structure shown in reaction (x) of Scheme 11 for > Ir.sub.2.sup.0,II (tfepma).sub.3 (Me)Cl(MeCN) (44). A singlet > is observed at 29.5 ppm for the axial Ir.sup.0 phosphite, with > the typical pseudo-triplet at 44.8 ppm for the equatorial > Ir.sup.0 phosphite of the chelating tfepma ligand. The > equatorial Ir.sup.0 phosphites of the bridging tfepma ligands > appear as two doublets-of-multiplets at 93.8 and 95.5 ppm. One > Ir.sup.II phosphite is observed at 72.5 ppm with the second > shifted to high frequency at 109.3 ppm. The .sup.1 H NMR in > CD.sub.3 CN reveals a doublet-of-doublets resonance at 1.11 > ppm that integrates to three protons. Selective .sup.31 P > decoupling gives a .sup.3 J.sub.HP coupling constant of 8.1 Hz > to the high frequency, 109.3 ppm, phosphite resonance and a > .sup.3 J.sub.HP coupling constant of 2.8 Hz to the 72.5 ppm > phosphite resonance, establishing the equatorial coordination > of a methyl group on the Ir.sup.II center. Coordination of a > solvent molecule is confirmed by the presence of precisely one > equivalent of free THF or MeCN in the .sup.1 H NMR spectrum of > thoroughly dried compound. > > The preparation of two-electron mixed-valence complexes of > iridium would seem to follow directly from studies of the > Rh.sub.2.sup.0,II platform. However, the stronger metal-ligand > bonds of iridium starting materials do not permit > methodologies used in the rhodium chemistry described above to > translate to iridium. In order to isolate binuclear complexes > of the dfpma ligand with iridium, excess oxidant must be > employed to react with 1,5-cyclooctadiene liberated during the > reaction. Nevertheless, the Ir.sup.I center of 31 maintains a > chelated 1,5-cyclooctadiene ligand, presumably because the > poor .sigma.-donor ligand dfpma cannot displace it from the > iridium coordination sphere. Dppma proved to displace > 1,5-cyclooctadiene more efficiently, however, in this case the > metal core inserts into an aryl C--H bond subsequent to the > addition of three dppma ligands. Only the low solubility of > Ir.sub.2.sup.0,II (tfepma).sub.3 Cl.sub.2 (33) in methylene > chloride permits its isolation in moderate yields, free of the > 1,5-cyclooctadiene byproduct that plagues isolation of other > diphosphazane derivatives of iridium. Indeed, attempts to > directly prepare Ir.sub.2.sup.0,II species with an axial > ligand coordinated to the Ir.sup.II center results in the > formation of oils that preclude isolation of the > metal-containing complex. > > The preparation and reactivity of 33 suggests that the > preferred coordination geometry for iridium maintains a > .pi.-acid ligand chelated to the low-valent metal center. > Though steric constraints imposed by the tfepma ligand are > initially appealing reasons for this structural departure from > the three bridging ligand motif, the preparation of the > homologous rhodium series based on the tfepma ligand, > Rh.sub.2.sup.0,0 (tfepma).sub.3 (L).sub.2, Rh.sub.2.sup.0,II > (tfepma).sub.3 Cl.sub.2 (L), Rh.sub.2.sup.II,II (tfepma).sub.3 > Cl.sub.4, suggests that three bridging tfepma ligands can be > accommodated by a binuclear core. Furthermore, coordination of > tfepma in a chelating mode to the valence symmetric 38 > suggests a thermodynamic preference for a mixed-valence system > with tfepma chelating the low-valent metal center. > > The reactivity patterns of 33 reveal a complex with > considerable Lewis acid character. In particular, addition of > reducible small molecule substrates Cl.sub.2 and HCl proceeds > with facility. In contrast, MeI, HOTf and MeOTf do not add to > 33 in the absence of suitable donor ligands, suggesting an XY > addition mechanism in which X.sup.- coordination precedes > attack by Y.sup.+. The metal-centered frontier molecular > orbitals for 33, presented in FIG. 22, support this > contention. A HOMO of mixed d.pi.\*/d.delta.\* character is > complemented by a low-energy LUMO of d.sigma.\* parentage. > Coordination of a ligand to the vacant axial site of 33, as in > the reaction of 33 to 34 or 33 to 35, results in the formation > of a stable octahedral iridium center, with the > destabilization of the LUMO providing the required energy > compensation for bond formation. Similarly, oxidative addition > of small molecule substrates to 33 leads to occupation of the > vacant axial site by X.sup.-. Again, destabilization of the > LUMO attends the formation of the ligand-centered bonding > orbital. > > The preference of strong .sigma.-donor ligands for the axial > position of the Ir.sup.II center provides further evidence for > the Lewis acid character of the bimetallic core. Ligands with > .sigma.-donor properties stronger than chloride coordinate to > the Ir.sup.II center opposite the M-M bond whereas the weaker > donor ligands are forced into equatorial positions with > concomitant chloride migration to the axial site. No > spectroscopic evidence for equatorial coordination was > observed among the series CNR, PR.sub.3, Br.sup.-. Conversely, > THF and MeCN were observed to coordinate only in the > equatorial position. These results are in contradistinction to > other studies on binuclear metal complexes that preferentially > coordinate the weakest .sigma.-donor opposite the metal-metal > bond. In the present case, the Lewis acid character of the > d.sigma.\* orbital apparently dominates the trans influence > normally associated with metal-metal bonds. > > The oxidative addition reactivity of 33 is notable in light > of previous studies of two-electron mixed-valence complexes. > The ability of the tfepma ligand to be sufficiently flexible > to support the variant coordination geometries and > correspondent electronic structures of the two-electron > mixed-valence cores is crucial to the reactivity of Scheme 11. > In one-electron mixed-valence compounds, a single electron > change can be accommodated with an inflexible coordination > sphere; however, this is unlikely to be the case for > two-electron mixed-valence species. Significant changes in the > reorganization of the primary coordination environment > typically accompany the addition or removal of more than one > electron from a metal center. As Bosnich postulates in his > studies of 6-4 binucleating complexes, this ligand > reorganization or "mechanical coupling" between metal centers > is manifested in arrested multi-electron redox reactivity of > mixed-valence complexes. In 33, adverse energetics associated > with mechanical coupling are circumvented by the flexible > coordination environment offered by the tfepma ligands. The > three atom diphosphazane backbone can support twist angles > from 0 to 45.degree., thus permitting the preferred trigonal > bipyramidal and octahedral coordination geometries of d.sup.9 > and d.sup.7 metal centers, respectively, to be adopted with > ##STR13## > > facility upon oxidative-addition to the Ir.sub.2.sup.0,II > bimetallic core. > > The addition of H.sub.2 to 33 and its elimination from 42 is > an unusual and intriguing observation. There are relatively > few examples of reversible H.sub.2 addition across metal-metal > bonds, and in no case, has such a reaction been observed to > occur reversibly across a preserved metal-metal single bond. > Variable temperature NMR studies of 33 provide insight into > the H.sub.2 addition mechanism. The addition of weak 2e.sup.- > donors to an equatorial Ir.sup.II site of 33, suggests that > this coordinatively unsaturated metal center is a logical site > for initial H.sub.2 attack as depicted in Scheme 13. The > addition of hydrogen to a single metal center of a binuclear > metal core is consistent with conventional oxidative-addition > mechanisms; furthermore, Poilblanc and Cowie previously have > observed single-site H.sub.2 addition followed by hydride > migration to produce the 1,2-dihydride. Conversely, a > concerted 1,2 addition of H.sub.2 across a metal-metal bond is > forbidden by orbital symmetry considerations, as is the > reverse, reductive elimination. Pre-coordination of dihydrogen > at Ir.sup.II is further supported by the empirical observation > that the rate of H.sub.2 addition to 38 decreases with donor > ability of the solvent, i.e., CH.sub.2 Cl.sub.2 > >THF>MeCN. Presumably, CH.sub.2 Cl.sub.2 cannot compete > with H.sub.2 as a sufficient donor ligand, whereas THF and > MeCN show progressively higher Ir-solvent bond dissociation > energies, slowing the H.sub.2 addition. > > Evaluation of equilibrium isotope effects for the reversible > addition of H.sub.2 to 33 provides mechanistic support for the > addition mechanism of Scheme 13. Recent studies suggest that > inverse EIEs, defined as follows: ##STR14## > > may be characteristic for the concerted addition of H.sub.2 > to a single metal center. For example, an inverse EIE of > 0.70.+-.0.06 was obtained for the coordination of H.sub.2 > versus D.sub.2 in tungsten dihydrogen complexes and an EIE of > 0.63.+-.0.05 was obtained for dihydride/dideuteride formation > from W(PMe.sub.3).sub.4 I.sub.2. A more thorough experimental > and theoretical treatment of equilibrium isotope effects for > the oxidative addition of H.sub.2 to Vaska's complex has been > reported as well (EIE=0.55.+-.0.06). In order to model > accurately both the direction and the magnitude of the > equilibrium isotope effects in the Vaska system, it was > necessary to use a full statistical mechanics treatment of the > isotope equilibrium, as given by: > > where SYM is the symmetry number ratio factored from the > rotational partition function, MMI is EIE component of the > mass moment of inertia, EXC is the vibrational excitation > constant and ZPE is the zero point energy term. The first > three factors describe the entropic element of the > equilibrium. SYM (1.0), MMI (5.66) and EXC (0.84) components > for the Vaska system resulted in a normal contribution to the > isotope effect (i.e., .DELTA.S.degree..sub.H > -.DELTA.S.degree..sub.D >0), leaving the inverse nature of > the EIE to be enthalpic (i.e., .DELTA.H.degree..sub.H > -.DELTA.H.degree..sub.D >0), as reflected by a zero point > energy term of 0.10. The inverse ZPE term turns out to be a > special case for hydrogen addition. Though consideration of > the H--H/D-D bond strength difference (.DELTA.BDE=1.8 kcal > mol.sup.-1) would suggest a strong normal ZPE contribution, > this single isotopically sensitive vibrational mode in the > reactant is dominated by five new isotopically sensitive modes > in the isotope-containing product (i.e., MH.sub.2 /MD.sub.2). > In all other equilibrium isotope studies, the number of > isotopically sensitive modes is essentially the same in > reactant and product, and as such the value of the equilibrium > isotope effect is directly determined by the relative > strengths of the bonds being made and broken. > > A minor inverse equilibrium isotope effect (EIE) of > 0.9.+-.0.05 is observed for the addition of hydrogen versus > deuterium to 33. This is an interesting result in light of the > equilibrium isotope effect reported for the reversible > addition of H.sub.2 to fulvalene dimers of chromium > (EIE=1.45.+-.0.10). In this latter case, ready access to the > diradical as shown in Scheme 14 suggests a symmetric addition > of H.sub.2 across the metal-metal bond, as observed for > rhodium porphyrin dimers. The pre-equilibrium step to form the > diradical is not isotope sensitive, thus the EIE reflects only > the thermodynamic characteristics of the second equilibrium > step, namely the relative ##STR15## > > stability of H-M . . . M-H/D-M . . . M-D versus H.sub.2 > /D.sub.2. Conversely, the proposed two-step hydrogen addition > of 33 as depicted in Scheme 13, is characterized by two > isotope sensitive equilibria: K.sub.1, which is the > equilibrium for binding and forming the putative dihydrogen > complex (eq 3), and K.sub.2, which is the equilibrium for > 1,2-hydride migration (eq 4). Substitution of eq 4 into eq 3 > gives K.sub.1.times.K.sub.2 in terms of measurable species, > i.e., the reactants and the final products (eq 5), which gives > the relation in eq 6 for the EIE experiment ([H.sub.2 > ]=[D.sub.2 ]). > > It has been proposed that EIEs for hydrogen addition to > transition metal complexes are general for a given type of > equilibrium. Thus, referring to eq 4 and 6, the value of > K.sub.1.sup.H /K.sub.1.sup.D can be approximated by Kubas' EIE > of 0.70.+-.0.06 for the formation of W(CO).sub.3 > (PCy.sub.3).sub.2 (.eta..sup.2 -H.sub.2) vs W(CO).sub.3 > (PCy.sub.3).sub.2 (.eta..sup.2 -D.sub.2). Similarly it would > be a reasonable approximation to use Volhardt's EIE of > 1.45.+-.0.10 for the formation of the > 1,2-dihydride/dideuteride of Scheme 14 (K.sub.2.sup.H > /K.sub.2.sup.D). Though crude, this estimation provides a > value for (K.sub.1.sup.H /K.sub.1.sup.D)(K.sub.2.sup.H > /K.sub.2.sup.D) of 1.02, which is in reasonable agreement with > the measured EIE of 0.9.+-.0.05 for hydrogen/deuterium > addition to 33, supporting the intermediacy of a dihydrogen > adduct in the addition mechanism of Scheme 13. > > Isotope effects are also useful in elucidating the solvent > exchange mechanism of 41. Solutions of 41 in CD.sub.3 CN > slowly exchange the coordinated acetonitrile ligand, as > evidenced by decay of the .sup.1 H NMR resonance for the > coordinated ligand with concomitant growth of free MeCN. At > 20.degree. C. an inverse kinetic isotope effect (KIE) of 0.66 > was measured for this process. Such isotope dependencies have > been rationalized by invoking product-like transition states > with higher force constants for isotope-sensitive stretching > and bending modes. As shown qualitatively in FIG. 23, a > "tighter" transition state results in a greater difference in > zero point energy in the transition state relative to the > ground state, thus .DELTA.G.sup.{character pullout}.sub.H is > greater than .DELTA.G.sup.{character pullout}.sub.D. Loss of > the coordinating MeCN ligand followed by rearrangement of the > Ir.sup.III center to square pyramidal in the transition state > is expected to strengthen the remaining interactions along the > metal-metal axis in the transition state. This assumption is > supported by the contracted Ir(1)-Ir(2) and Ir(1)-P(6) bond > distances in 33 relative to those of 37 and 40. Thus, a > one-step solvent exchange process could reasonably give rise > to an inverse KIE via strengthening of the Ir--H bond in the > transition state. However, the magnitude of the KIE is > suspiciously large for a secondary isotope effect. > > Alternatively, the observed inverse KIE could be the result > of an equilibrium step, prior to actual solvent exchange, > which exhibits an inverse isotope effect. Consider the > proposed reaction sequence presented in Scheme 15. Proton > abstraction from 41 by the weakly basic solvent, in this case > CD.sub.3 CN (pK.sub.a.congruent.-10), would (in effect) give > 34 and CD.sub.3 CN . . . H.sup.+. The iridium complex could > then rapidly exchange the coordinated MeCN ligand as > established by studies of the solution NMR spectra of 33. For > this situation, the primary isotope effect (the Ir--H bond is > being broken) arises from the higher force constants > associated with N--H/D.sup.+ species as opposed to M-H/D.sup.+ > species, resulting in a lower activation barrier for deuterium > transfer; that is, ##STR16## > > isotopic labeling of the iridium complex favors proton > transfer to the CD.sub.3 CN solvent. This model is in > agreement with the arrested reactivity of HOTf with 33 in the > absence of MeCN; initial coordination of MeCN to 33 to yield > 34 is apparently prerequisite to the protonation yielding 41, > microscopic reversibility would then require deprotonation of > 41 to occur prior to MeCN exchange. > > **Summary** > > The tfepma ligand presents a novel plafform for binuclear > iridium chemistry, providing a flexible electronic environment > and coordination sphere. A two-electron mixed-valence core is > stabilized by three tfepma ligands in a coordinatively > unsaturated framework providing easy access to multi-electron > reactivity. Oxidative addition of small molecule substrates is > complemented by facile reductive elimination in the case of > hydrogen, suggesting the binuclear framework to be an > excellent model complex for the study of stoichiometric and > catalytic small molecule activation and functionalization. > > TABLE 15 Crystal data and structure refinement parameters for > Ir.sub.2.sup.I,III (dfpma).sub.2 Cl.sub.2 (cod) (1), > Ir.sub.2.sup.I,III (dppma).sub.3 Cl.sub.2 (2) and > Ir.sub.2.sup.0,II (tfepma).sub.3 Cl.sub.2 (3). 1 2 3 Empirical > formula C.sub.10 H.sub.18 Cl.sub.4 F.sub.8 Ir.sub.2 N.sub.2 > P.sub.4 C.sub.76 H.sub.70 Cl.sub.4 Ir.sub.2 N.sub.3 O.sub.12 > P.sub.6 C.sub.275 H.sub.33 Cl.sub.3 F.sub.36 Ir.sub.2 N.sub.3 > O.sub.12 P.sub.6 Formula weight 968.34 1929.37 1958.14 Crystal > system Monoclinic Monoclinic Monoclinic Space group P2.sub.1 > /n P2.sub.1 /n C2/c Unit cell dimensions a = 15.8546(10) .ANG. > a = 14.427(2) .ANG. a = 22.6597(5) .ANG. b = 9.9373(6) .ANG. b > = 24.780(4) .ANG. b = 12.8038(2) .ANG. c = 16.3834(10) .ANG. c > = 26.389(4) .ANG. c = 40.1310(6) .ANG. .alpha. = 90.degree. > .alpha. = 90.degree. .alpha. = 90.degree. .beta. = > 115.4270(10).degree. .beta. = 94.870(3).degree. .beta. = > 92.4210(10).degree. .gamma. = 90.degree. .gamma. = 90.degree. > .gamma. = 90.degree. Volume 2331.2(2) .ANG..sup.3 9400(3) > .ANG..sup.3 11632.8(4) .ANG..sup.3 Z 4 4 4 Density > (calculated) 2.759 Mg/m.sup.3 1.363 Mg/m.sup.3 2.236 > Mg/m.sup.3 Absorption coefficient 12.205 mm.sup.-1 3.095 > mm.sup.-1 5.043 mm.sup.-1 F(000) 1784 3820 7472 Crystal size > (mm) 0.33 .times. 0.21 .times. 0.19 0.40 .times. 0.21 .times. > 0.08 0.30 .times. 0.30 .times. 0.12 .theta. min for data > collection 2.37.degree. 1.13.degree. 1.02.degree. .theta. max > for data collection 23.27.degree. 20.00.degree. 23.24.degree. > Index ranges -10 .ltoreq. h .ltoreq. 17 -13 .ltoreq. h > .ltoreq. 12 -20 .ltoreq. h .ltoreq. 25 -11 .ltoreq. k .ltoreq. > 11 -23 .ltoreq. k .ltoreq. 23 -14 .ltoreq. k .ltoreq. 13 -18 > .ltoreq. l .ltoreq. 15 -25 .ltoreq. l .ltoreq. 21 -44 .ltoreq. > l .ltoreq. 44 Reflections collected 8646 28006 23134 > Independent reflections 3336 [R.sub.int = 0.0542] 8762 > [R.sub.int = 0.1012] 8322 [R.sub.int = 0.0696] Absorption > correction Empirical Empirical psi-scans Max. Transmission > 1.0000 1.000000 0.9876 Min. Transmission 0.3788 0.625348 > 0.4679 Data/restraints/ 3336/0/272 8762/0/474 8312/1/783 > parameters Goodness-of-fit on F2 1.168 1.175 1.054 Final R > indices [l > 2.sigma.(l)] R1 = 0.0444 R1 = 0.1153 R1 = > 0.0593 wR2 = 0.1131 wR2 = 0.2904 wR2 = 0.1253 R indices (all > data) R1 = 0.0469 R1 = 0.1387 R1 = 0.0882 wR2 = 0.1147 wR2 = > 0.3087 wR2 = 0.1476 Extinction coefficient 0.00037(8) > 0.0214(8) 0.000015(11) Largest diff. peak 1.984 e.ANG..sup.-3 > 4.736 e.ANG..sup.-3 2.785 e.ANG..sup.-3 Largest diff. hole > -3.084 e.ANG..sup.-3 -2.038 e.ANG..sup.-3 -1.386 e.ANG..sup.-3 > > TABLE 16 Crystal data and structure refinement parameters for > Ir.sub.2.sup.0,II (tfepma).sub.3 Cl.sub.2 (MeCN) (4), > Ir.sub.2.sup.0,II (tfepma).sub.3 Cl.sub.2 (CN.sup.t Bu) > (5-CN.sup.t Bu) and [Ir.sub.2.sup.0,II (tfepma).sub.3 > (MeCN).sub.3 ][PF.sub.6 ].sub.2 (6 [PF.sub.6 ].sub.2). 4 > 5-CN.sup.t Bu 6 [PF.sub.6 ].sub.2 Empirical formula C.sub.31 > H.sub.39 Cl.sub.2 F.sub.36 Ir.sub.2 N.sub.5 O.sub.12 P.sub.6 > C.sub.32 5 H42Cl.sub.3 F.sub.36 Ir.sub.2 N.sub.4 O.sub.12 > P.sub.6 C.sub.35 H.sub.45 F.sub.48 Ir.sub.2 N.sub.7 O.sub.12 > P.sub.8 Formula weight 1998.79 2041.27 2299.94 Crystal system > Orthorhombic Monoclinic Triclinic Space group P2.sub.1 2.sub.1 > 2.sub.1 P2.sub.1 /n Pī Unit cell dimensions a = > 13.078(6) .ANG. a = 13.0879(2) .ANG. a = 13.1419(3) .ANG. b = > 17.505(9) .ANG. b = 54.4519(9) .ANG. b = 13.3846(4) .ANG. c = > 27.837(14) .ANG. c = 18.4318(3) .ANG. c = 24.1808(6) .ANG. > .alpha. = 90.degree. .alpha. = 90.degree. .alpha. = > 86.3020(10).degree. .beta. = 90.degree. .beta. = > 101.1890(10).degree. .beta. = 84.5500(10).degree. .gamma. = > 90.degree. .gamma. = 90.degree. .gamma. = 62.6840(10).degree. > Volume 6373(5) .ANG..sup.3 12885.9(4) .ANG..sup.3 3760.95(17) > .ANG..sup.3 Z 4 8 2 Density (calculated) 2.083 Mg/m.sup.3 > 2.104 Mg/m.sup.3 2.031 Mg/m.sup.3 Absorption coefficient 4.566 > mm.sup.-1 4.558 mm.sup.-1 3.877 mm.sup.-1 F(000) 3832 7840 > 2212 Crystal size (mm) 0.24 .times. 0.32 .times. 0.32 0.42 > .times. 0.19 .times. 0.14 0.05 .times. 0.50 .times. 0.75 > .theta. min for data 2.43.degree. 1.35.degree. 1.69.degree. > collection .theta. max for data 23.31.degree. 23.27.degree. > 23.27.degree. collection Index ranges -11 .ltoreq. h .ltoreq. > 14 -13 .ltoreq. h .ltoreq. 14 -14 .ltoreq. h .ltoreq. 13 -19 > .ltoreq. k .ltoreq. 18 -51 .ltoreq. k .ltoreq. 60 -12 .ltoreq. > k .ltoreq. 14 -30 .ltoreq. l .ltoreq. 30 -20 .ltoreq. l > .ltoreq. 20 -26 .ltoreq. l .ltoreq. 24 Reflections collected > 25467 52085 15572 Independent 9155 [R.sub.int = 0.0335] 18440 > [R.sub.int = 0.1427] 10588 [R.sub.int = 0.0675] reflections > Absorption correction Empirical psi-scans psi-scans Max. > Transmission 0.427270 1.000 0.3463 Min. Transmission 0.314766 > 0.3175 0.2421 Data/restraints/ 9155/0/848 18405/0/1696 > 10588/0/1017 parameters Goodness-of-fit on F2 1.056 1.171 > 1.152 Final R indices [l > R1 = 0.0290 R1 = 0.0891 R1 = > 0.0743 2.sigma.(l)] wR2 = 0.0699 wR2 = 0.1701 wR2 = 0.1977 R > indices (all data) R1 = 0.0335 R1 = 0.1525 R1 = 0.0790 wR2 = > 0.0721 wR2 = 0.2113 wR2 = 0.2029 Extinction coefficient > 0.00021(5) 0.000000(12) 0.0025(2) Largest diff. peak 0.913 > e.ANG..sup.-3 2.995 e.ANG..sup.-3 4.706 e.ANG..sup.-3 Largest > diff. hole -0.464 e.ANG..sup.-3 -2.759 e.ANG..sup.-3 -2.438 > e.ANG..sup.-3 > > TABLE 17 Crystal data and structure refinement parameters for > Ir.sub.2.sup.I,III (tfepma).sub.3 Cl.sub.4 (7) and > Ir.sub.2.sup.I,III (tfepma).sub.3 Cl.sub.4 (MeCN).sub.2 (8). 7 > 8 Empirical formula C.sub.55 H.sub.68 Cl.sub.10 F.sub.72 > Ir.sub.4 N.sub.6 O.sub.24 P.sub.12 C.sub.225 H.sub.29 Cl.sub.5 > F.sub.24 Ir.sub.2 N.sub.4 O.sub.8 P.sub.4 Formula weight > 4060.09 1625.03 Crystal system Monoclinic Triclinic Space > group P2.sub.1 /c Pī Unit cell a = 23.6253(3) .ANG. > a = 16.5448(11) .ANG. dimensions b = 24.3565(4) .ANG. b = > 16.5925(11) .ANG. c = 24.93500(10) .ANG. c = 19.2595(13) .ANG. > 90.degree. 96.1220(10).degree. 116.5400(10).degree. > 90.0930(10).degree. 90.degree. 104.0800(10).degree. Volume > 12836.3(3) .ANG..sup.3 5096.9(6) .ANG..sup.3 Z 8 4 Density > 4.202 Mg/m.sup.3 2.118 Mg/m.sup.3 (calculated) Absorption > 9.310 mm.sup.-1 5.735 mm.sup.-1 coefficient F(000) 15504 3084 > Crystal size (mm) 0.50 .times. 0.20 .times. 0.08 .theta. min > for data 1.28.degree. 1.27.degree. collection .theta. max for > data 23.25.degree. 23.26.degree. collection Index ranges -26 > .ltoreq. h .ltoreq. 22 -18 .ltoreq. h .ltoreq. 12 -27 .ltoreq. > k .ltoreq. 23 -16 .ltoreq. k .ltoreq. 18 -27 .ltoreq. l > .ltoreq. 27 -21 .ltoreq. l .ltoreq. 20 Reflections 51161 20933 > collected Independent 18247 [R.sub.int = 0.0955] 14281 > [R.sub.int = 0.0419] reflections Absorption Empirical > Empirical correction Max. 0.9884 0.8939 Transmission Min. > 0.5789 0.3785 Transmission Data/restraints/ 18247/0/1646 > 14280/1/1250 parameters Goodness-of-fit 1.144 1.144 on F.sup.2 > Final R indices R1 = 0.0803 R1 = 0.0749 [l > 2.sigma.(l)] > wR2 = 0.1363 wR2 = 0.1598 R indices R1 = 0.1207 R1 = 0.1074 > (all data) wR2 = 0.1504 wR2 = 0.1789 Extinction 0.000188(13) > 0.00054(5) coefficient Largest 1.456 e.ANG..sup.-3 1.484 > e.ANG..sup.-3 diff. peak Largest -1.221 e.ANG..sup.-3 -1.235 > e.ANG..sup.-3 diff. hole > > TABLE 18 Crystal data and structure refinement parameters for > Ir.sub.2.sup.I,III (tfepma).sub.3 HCl.sub.3 (10) and > Ir.sub.2.sup.I,III (tfepma).sub.3 H.sub.2 Cl.sub.2 (12). 10 12 > Empirical formula C.sub.28 H.sub.36 Cl.sub.5 F.sub.36 Ir.sub.2 > N.sub.3 O.sub.12 P.sub.6 C.sub.28 H.sub.37 Cl.sub.4 F.sub.36 > Ir.sub.2 N.sub.3 O.sub.12 P.sub.6 Formula weight 2038.07 > 2003.63 Crystal system Monoclinic Monoclinic Space group > P2.sub.1 /c P2.sub.1 /c Unit cell dimensions a = 12.807(8) > .ANG. a = 10.9265(3) .ANG. b = 17.012(9) .ANG. b = 24.1981(7) > .ANG. c = 28.463(14) .ANG. c = 22.6237(7) .ANG. 90.degree. > 90.degree. 99.200(13).degree. 97.1070(10).degree. 90.degree. > 90.degree. Volume 6121.6(57) .ANG..sup.3 5935.8(3) .ANG..sup.3 > Z 4 4 Density (calculated) 2.211 Mg/m.sup.3 2.242 Mg/m.sup.3 > Absorption 4.881 mm.sup.-1 4.988 mm.sup.-1 coefficient F(000) > 3896 3832 Crystal size (mm) 0.50 .times. 0.32 .times. 0.10 > 0.20 .times. 0.15 .times. 0.06 .theta. min for data > 1.40.degree. 1.24.degree. collection .theta. max for data > 23.29.degree. 23.27.degree. collection Index ranges -14 > .ltoreq. h .ltoreq. 13 -12 .ltoreq. h .ltoreq. 4 -18 .ltoreq. > k .ltoreq. 13 -26 .ltoreq. k .ltoreq. 26 -31 .ltoreq. l > .ltoreq. 24 -25 .ltoreq. l .ltoreq. 24 Reflections 21797 19042 > collected Independent 8704 [R.sub.int = 0.0442] 8475 > [R.sub.int = 0.0717] reflections Absorption Empirical > Empirical correction Max. Transmission 0.9279 0.2661 Min. > Transmission 0.4311 0.1216 Data/restraints/ 8701/0/834 > 8475/3/829 parameters Goodness-of-fit on 1.140 1.263 F.sup.2 > Final R indices R1 = 0.0422 R1 = 0.0549 [l > 2.sigma.(l)] > wR2 = 0.1002 wR2 = 0.1491 R indices (all data) R1 = 0.0487 R1 > = 0.0672 wR2 = 0.1146 wR2 = 0.1550 Extinction 0.00046(5) > 0.00143(10) coefficient Largest diff. peak 1.643 e.ANG..sup.-3 > 2.034 e.ANG..sup.-3 Largest diff. hole -1.667 e.ANG..sup.-3 > -1.569 e.ANG..sup.-3 > > **Reductive Elimination Photochemistry of Rhodium > Diphosphazanes** > > Extending the development of two-electron mixed-valence > complexes, the viability of promoting multi-electron > transformations from the excited state of M.sub.2.sup.0,II > cores was investigated. Excepting H.sub.2 and RH eliminations > that result in the formation of strong H--H and C--H bonds, > scant precedent exists for such multi-electron reactivity > among molecular species. Coupling of individual two-electron > photoreactions with a Rh.sub.2.sup.0,II complex provides the > first example of a four-electron photoreaction among discrete > molecular species. > > Oxidation-reduction reactions of electronically excited > transition metal complexes customarily proceed by one > electron. By itself, single electron transfer is confining > inasmuch as most activation reactions involve multi-electron > processes. Primary one-electron photoredox events must > therefore be coupled to oxidation-reduction processes remote > to the excited state to effect overall multi-electron > reactivity. Such conformity in multi-electron design finds its > origins in the nature of the excited state, which at the most > general level is the same despite the many different types of > transition metal photoreagents. As instructive examples, > consider the three systems schematically represented in Scheme > 16. The photochemistry of mononuclear d.sup.6 metals, for > which tris(bipyridyl)ruthenium(II) is the archetype, > originates from a metal-to-ligand ##STR17## > > charge transfer (MLCT) excited state in which electrons > localized on the metal and ligand are triplet-paired. A relay > catalyst must convey single electron equivalents from the > metal photosensitizer to a homogeneous or heterogeneous site > capable of storing multiple redox equivalents. A biradical > model is also pertinent to the excited state chemistry of > binuclear d.sup.7(9) and d.sup.8(10) metal complexes, but in > different guises. The d.sigma.(or d.pi.\*)d.sigma.\* excited > states of d.sup.7(9) --d.sup.7(9) complexes are short-lived > and dissociative, producing an .M,M. biradical pair. Because > the photogenerated radicals are uncoupled, selective > multi-electron activation of substrates is difficult to > control and therefore free radical reactions are typically > observed Conversely, a stable and long-lived biradical > tethered by a metal-metal bond, .M-M., is produced upon > d.sub.z.sub..sup.2 .sigma.\*.fwdarw.p.sub.z.sigma. (excitation > of d.sup.8(10) . . . d.sup.8(10) complexes The proximity of > the radical metal centers permits coupling of their single > electron reactions to effect selective multi-electron > transformations. > > Whereas the general formalism of biradical excited states > naturally leads to two-electron processes one electron at a > time, approaches to explore photoredox reactions in excess of > two electrons are not at hand. In the absence of a > well-defined framework, it is not surprising to find scant > precedence for three- and four-electron photoreactions. > Photoinduced decomposition of Pt.sup.IV salts to metal > colloids along ill-defined mechanistic pathways is the only > documented photoredox reaction involving more than two > electrons. In no case has a four-electron photoreaction along > a controlled reaction pathway been achieved. > > The challenges confronting the design of multi-electron > photoreactions are formidable. Reorganization of the primary > coordination environment typically accompanies the addition or > removal of more than one electron from a metal center. If > ligand reorganization does not occur, the thermodynamic > barrier associated with the transfer of redox equivalents to > or from the metal center becomes insurmountable at chemically > relevant redox potentials. This is a particularly germane > problem for excited state redox schemes because reactivity is > usually confined to the lowest energy excited state, > constraining the overall internal energy of the system. As an > example, again consider the oxidation-reduction chemistry of > d.sup.6 Ru.sup.II polypyridyl systems. The one-electron > oxidation and reduction potentials of the Ru.sup.II metal, > octahedrally coordinated by a conventional polypyridyl ligand > set, are .about.1.0 to 1.5 V. By virtue of its inflexibility, > the polypyridine coordination sphere imposes thermodynamic > remuneration of an additional 1.5 V and 3.3 V for the > metal-based reduction and oxidation, respectively, of a second > electron equivalent. An excited state energy of only .about.2 > eV therefore confines reaction to single electron transfer. > When the coordination environment of the metal is able to > adopt a geometry to accommodate a two-electron > photoconversion, the electronic structure responsible for > excited state reactivity is invariably lost. A lowest energy, > reactive excited state maintains a fragile existence among the > multitude of energy-dissipating excited states of a metal > complex. Changes in coordination geometry will re-order state > parentages with any one of the neighboring, non-reactive > states ready to assume the lowest energy position. In this > case, an excited state pathway encompassing redox reactivity > beyond two electrons will be circumvented. With these > considerations in mind, further advances in multi-electron > photoredox chemistry must require novel molecular structures > that would preserve the same lowest energy, reactive excited > state across a multi-electron series of complexes. > > As single-electron mixed-valence compounds react in > one-electron steps from their excited states, electronically > excited M.sup.n -M.sup.n+2 complexes may react in two-electron > steps at the bimetallic core. Although the occurrence of > authentic M.sup.n -M.sup.n+2 compounds is unusual > bis(difluorophosphine)methylamine (dfpma) stabilizes a > four-electron series of Rh.sub.2 complexes based upon the > two-electron mixed-valence complex Rh.sub.2.sup.0,II > (dfpma).sub.3 X.sub.2 (L) (L=PR.sub.3, CNR or CO; X=Cl or Br). > Electronic absorption and luminescence spectra of the > Rh.sub.2.sup.0,0, Rh.sub.2.sup.0,II and Rh.sub.2.sup.II,II > dfpma complexes are consistent with each possessing a lowest > energy excited state of d.sigma.\* parentage. The results > presented herein show that the d.sigma.\* excited state permits > interconversion among Rh.sub.2.sup.0,0, Rh.sub.2.sup.0,II and > Rh.sub.2.sup.II,II cores, enabling the rational design of a > system to support four-electron photochemistry among discrete > molecular species. > > **Structure and Electronic Spectroscopy of Rh.sub.2 -dfpma > Complexes** > > The ability of the dfpma ligand to stabilize trigonal > bipyramidal Rh.sup.0 and octahedral Rh.sup.II centers provides > a homologous series of complexes with singly bonded Rh.sup.0 > --Rh.sup.0, Rh.sup.0 --Rh.sup.II and Rh.sup.II --Rh.sup.II > cores. For reference, representative structures of the > Rh.sub.2.sup.0,0 (dfpma).sub.3 (L).sub.2, Rh.sub.2.sup.0,II > (dfpma).sub.3 X.sub.2 (L) and Rh.sub.2.sup.II,II (dfpma).sub.3 > X.sub.4 presented in FIG. 24. > > The electronic absorption and emission spectra clearly > distinguish members of the Rh.sub.2.sup.0,0, Rh.sub.2.sup.0,II > and Rh.sub.2.sup.II,II series. FIG. 25 displays representative > spectra for each compound; Table 19 summarizes both absorption > and emission data for several Rh.sub.2 congeners. The high > optical electronegativity of the terminal fluorophosphine > ligand reduces configurational mixing of the d.sigma. and > L.sigma. orbitals, thus a relatively straightforward > absorption spectrum, typical of d.sup.9 --d.sup.9 compounds, > is observed for Rh.sub.2.sup.0,0 (dfpma).sub.3 (L).sub.2. An > intense 305-nm band, attributable to the allowed > d.sigma..fwdarw.d.sigma.\* transition, is flanked to lower > energy by the less intense d.pi.\*.fwdarw.d.sigma.\* absorption > band for the L=PF.sub.3 derivative. The absorption spectra of > Rh.sub.2.sup.II,II (dfpma).sub.3 X.sub.4 and Rh.sub.2.sup.0,II > (dfpma).sub.3 X.sub.2 (L) complexes exhibit more congested > profiles in the near-UV as a result of configurational mixing > between the metal-d.sub.z.sub..sup.2 and X-p.sub.z .sigma. > orbitals. Significant LMCT character is revealed in the > highest energy absorption band of both Rh.sub.2.sup.II,II > (dfpma).sub.3 X.sub.4 and Rh.sub.2.sup.0,II (dfpma).sub.3 > X.sub.2 (L), red-shifting by 3861 cm.sup.-1 upon substitution > of bromide for chloride. The mid-spectrum band of the > Rh.sub.2.sup.II,II complex also shows a dramatic 4851 > cm.sup.-1 red-shift upon halogen substitution, however, in the > Rh.sub.2.sup.0,II complexes this transition appears to be > equally influenced by the nature of the halogen and the axial > Rh.sup.0 donor ligand. The low energy absorption band > red-shifts to a lesser extent upon halogen substitution > (.about.1254 cm.sup.-1 for Br.sup.- /Cl.sup.-) in both > Rh.sub.2.sup.II,II and Rh.sub.2.sup.0,II, consistent with > greater metal-based character of a d.pi.\*.fwdarw.d.sigma.\* > transition. > > TABLE 19 Absorption and emission spectral data for various > Rh.sub.2.sup.0,0 (dfpma).sub.3 (L).sub.2, Rh.sub.2.sup.0,II > (dfpma).sub.3 X.sub.2 (L) and Rh.sub.2.sup.II,II (dfpma).sub.3 > X.sub.4 complexes. .lambda..sub.max Absorbance (nm) Compound > X(.sigma.)/d.sigma. .fwdarw. d.sigma.\* (1) X(.sigma.)/d.sigma. > .fwdarw. d.sigma.\* (2) d.pi.\* .fwdarw. d.sigma.\* > Rh.sub.2.sup.0,0 (dfpma).sub.3 (PF.sub.3).sub.2.sup.a 305 -- > 440 Rh.sub.2.sup.0,0 (dfpma)3(.eta..sup.1 -dfpma).sub.2.sup.a > 310 -- 411 Rh.sub.2.sup.0,II (dfpma).sub.3 Cl.sub.2 (PF.sub.3) > 270 330 385 Rh.sub.2.sup.0,II (dfpma).sub.3 Br.sub.2 > (.eta..sup.1 -dfpma) 299 358 411 Rh.sub.2.sup.0,II > (dfpma).sub.3 Cl.sub.2 (PPh.sub.3) 275 353 402 > Rh.sub.2.sup.0,II (dfpma).sub.3 Br.sub.2 (PPh.sub.3) 315 371 > 424 Rh.sub.2.sup.II,II (dfpma).sub.3 Cl.sub.4 265 335 445 > Rh.sub.2.sup.II,II (dfpma).sub.3 Br.sub.4 291 400 462 .sup.a > Only one d.sigma. .fwdarw. d.sigma.\* transition is observed > for the Rh.sub.2.sup.0,0 complexes > > Whereas substitution of PF3 by .eta..sup.1 -dfpma barely > perturbs the electronic structure of the dirhodium core, > coordination of the more basic PR.sub.3 ligands to the > Rh.sup.0 center of the Rh.sub.2 dfpma series notably disrupts > the electronic structure of the system. Consistent with the > perturbation of the Rh--Rh bond distances of the > Rh.sub.2.sup.0,II (dfpma).sub.3 X.sub.2 (L) complexes > absorption maxima of complexes with basic phosphines are > red-shifted by >20 nm relative to those with .pi.-accepting > fluorophosphines as the axial ligand. The effect is even more > pronounced in the absorption spectra of the fully reduced > Rh.sub.2.sup.0,0 (dfpma).sub.3 L.sub.2 compounds containing > two axially donor ligands. FIG. 26 plots the absorption > maximum of the d.sigma..fwdarw.d.sigma.\* transition of > Rh.sub.2.sup.0,0 (dfpma).sub.3 L.sub.2 for L=PEt.sub.3, > P(OMe).sub.3, P(O.sup.i Pr).sub.3, PPh.sub.3 and PF.sub.3 vs > the Tolman electronic parameterization of phosphine ligands. > The observed trend of the d.sigma..fwdarw.d.sigma.\* transition > towards lower energy with an increase in the basicity of the > phosphine logically follows from considerations of P.sigma. > orbital mixing into the metal-metal .sigma. framework. > Although linear combinations of P.sigma. orbitals have the > appropriate symmetries to mix with both d.sigma. and > d.sigma.\*, destabilization of the energetically proximate do > orbital will be greater, resulting in the observed red shift. > With the exception of PPh.sub.3, the size of the phosphine is > of little consequence in the overall correlation since the > cone angles of the phosphines are relatively constricted > (<135.degree.). The anomalously small > d.sigma..fwdarw.d.sigma.\* transition energy of PPh.sub.3 is > attributed to structural distortions of the ligand and metal > framework. Steric-induced lengthening of the Rh--Rh bond by > PPh.sub.3 augments the ligand's electronic effect, leading to > a smaller d.sigma./d.sigma.d\* splitting and consequently lower > observed transition energy than that predicted by the Tolman > electronic parameter. > > Excitation into the absorption manifold of crystalline solids > of the Rh.sub.2 dfpma compounds produces a long-lived red > luminescence with spectral features characteristic of a > d.sigma.\* excited state parentage. Luminescence is not > detected from solutions at temperatures equivalent to those at > which the crystalline solids emit. Moreover, the loss of > luminescence from solutions of the Rh.sub.2 dfpma complexes > immediately above solvent glassing transition temperatures > suggested a prevalence for bond cleavage chemistry as a > dominant nonradiative decay pathway of the d.sigma.\* excited > state. These photophysical observations provided the impetus > to undertake investigations of the solution photochemistry of > this series of complexes. > > **Rh.sub.2 -dfpma Reductive Elimination Photochemistry** > > Irradiation of THF solutions of Rh.sub.2.sup.II,II > (dfpma).sub.3 X.sub.4 (X=Cl or Br) in THF solution containing > excess L (L=PF.sub.3, .eta..sup.1 -dfpma) with UV-Vis white > light leads to rapid changes in the absorption spectrum. FIG. > 27 conveys the complexity of Rh.sub.2.sup.II,II (dfpma).sub.3 > Br.sub.4 photochemistry when THF solutions containing > .eta..sup.1 -dfpma are photolyzed at .lambda..sub.exc >335 > nm. Isosbestic points at 311, 373 and 425 nm, maintained early > during photolysis, are lost with continued irradiation, > indicating the occurrence of a secondary reaction at longer > times. Comparison of the terminating absorption profile of the > photolyzed solution to the absorption spectra of FIG. 25(a) > identifies the final photoproduct as Rh.sub.2.sup.0,0 > (dfpma).sub.3 (.eta..sup.1 -dfpma).sub.2. Independent > verification of this assignment was afforded by bulk > photolysis experiments. Irradiation of Rh.sub.2.sup.II,II > (dfpma).sub.3 Br.sub.4 in the presence of .eta..sup.1 -dfpma > in THF followed by solvent removal yielded the final product, > which was extracted into pentane. Recrystallization at low > temperature afforded Rh.sub.2.sup.0,0 (dfpma).sub.3 > (.eta..sup.1 -dfpma).sub.2 as determined by the .sup.19 F NMR > spectrum reproduced in FIG. 28. Three .sup.19 F NMR resonances > are observed in a 1:3:1 ratio. A doublet at -40.96 ppm > displaying a .vertline..sup.1 J.sub.FP +.sup.3 > J.sub.FP.vertline. coupling constant of 1117 Hz identifies the > fluorines of the bridging dfpma ligands. Doublets at -29.72 > (.vertline..sup.1 J.sub.FP +.sup.3 J.sub.FP.vertline.=1252 Hz) > and -76.29 ppm (.vertline..sup.1 J.sub.FP +.sup.3 > J.sub.FP.vertline.=1253 Hz) are assigned to the coordinated > and free PF.sub.2 groups of the .eta..sup.1 -dfpma ligands, > respectively. Similar results are obtained if the photolysis > is carried out in the presence of excess PF.sub.3 : the final > .sup.19 F NMR spectrum of Rh.sub.2.sup.0,0 (dfpma).sub.3 > (PF.sub.3).sub.2 displays doublets at -37.89 (.vertline..sup.1 > J.sub.FP +.sup.3 J.sub.FP.vertline.=1110 Hz) and -4.16 > (.vertline..sup.1 J.sub.FP +.sup.3 J.sub.FP =1359 Hz) ppm for > the bridging dfpma and axial PF.sub.3 ligands, respectively. > > Owing to the well separated spectra of the Rh.sub.2.sup.II,II > (dfpma).sub.3 Br.sub.4 and Rh.sub.2.sup.0,II (dfpma).sub.3 > Br.sub.2 (.eta..sup.1 -dfpma) complexes, wavelength selection > of the excitation light permitted deconstruction of the > overall photo transformation of FIG. 27 into a stepwise > reaction sequence. Though solutions of Rh.sub.2.sup.II,II > (dfpma).sub.3 Br.sub.4 in THF are stable in the absence of > irradiation, FIG. 29(a) displays the changes in the absorption > profile upon photolysis at .lambda..sub.exc.gtoreq.436 nm. > Well-anchored isosbestic points are maintained throughout the > photolysis. Comparison of the terminating absorption spectrum > to those of FIG. 25(b) reveals that Rh.sub.2.sup.0,II > (dfpma).sub.3 Br.sub.2 (.eta..sup.1 -dfpma) is the > photoproduct. On the basis of the measured molar absorption > coefficients, the photoconversion of the Rh.sub.2.sup.II,II > complex to the mixed-valence Rh.sub.2.sup.0,II complex is > quantitative. Although this photoreacted solution is stable > under the low-energy excitation conditions of FIG. 29(a), > further reaction is observed when the excitation wavelength is > moved into the UV spectral region. As shown in FIG. 29(b), the > final absorption spectrum of the solution under 335-nm > irradiation is that of Rh.sub.2.sup.0,0 (dfpma).sub.3 > (.eta..sup.1 -dfpma).sub.2, which is also produced in > quantitative yield. These results demonstrate that the overall > photoreaction proceeds in two steps: Rh.sub.2.sup.II,II > (dfpma).sub.3 Br.sub.4 is photolyzed to Rh.sub.2.sup.0,II > (dfpma).sub.3 Br.sub.2 (.eta..sup.1 -dfpma) for > .lambda..sub.exc.gtoreq.436 nm and subsequently > Rh.sub.2.sup.0,II (dfpma).sub.3 Br.sub.2 (.eta..sup.1 -dfpma) > is photolyzed to Rh.sub.2.sup.0,0 (dfpma).sub.3 (.eta..sup.1 > -dfpma).sub.2 for .lambda..sub.exc.gtoreq.335 nm. > > In the absence of a donor ligand to cap the reduced Rh.sup.0 > center during irradiation of Rh.sub.2.sup.II,II complexes, an > intermediate species is observed at early reaction times (FIG. > 30). Photolysis of Rh.sub.2.sup.II,II (dfpma).sub.3 Br.sub.4 > in THF without any donor ligand causes a rapid color change of > the solution to blue. The color results from the appearance of > a new absorbance in the visible region of the spectrum at 583 > nm. Comparison of the maximum intensity of the 583-nm band > with the absorption bands of the starting Rh.sub.2.sup.II,II > (dfpma).sub.3 Br.sub.4 complex provides a crude estimate of > 4000 M.sup.-1 cm.sup.-1 as the extinction coefficient of this > 583-nm band. If the solutions are maintained in the dark, the > blue color fades within minutes, and the observed absorption > spectrum shows only bands in the near UV region of the > spectrum attributable to the Rh.sub.2.sup.0,II photoproduct. > > **Identification of the Halogen Photoproduct** > > The fate of the halogen in the overall photoreaction sequence > is disclosed by undertaking the appropriate trapping > experiments. Because the weak .alpha. C--H bonds of THF are > susceptible to hydrogen atom abstraction, THF could > participate in the photoreaction as a halogen trap. Two > observations support this contention. No photoreaction is > observed in benzene or CH.sub.2 Cl.sub.2 unless a halogen trap > such as 2,3-dimethyl-1,3-butadiene or 9,10-dihydroanthracene > is present. The inability of these solvents to furnish a > hydrogen atom appears to circumvent net photochemistry as the > halogen photoproduct can simply re-oxidize the reduced metal > center. Conversely, photoreactions in THF proceed with > facility regardless of the concentration of auxiliary trapping > reagent. Addition of 2,3-dimethyl-1,3-butadiene or > 9,10-dihydroanthracene to THF solutions of Rh.sub.2.sup.II,II > (dfpma).sub.3 X.sub.4 or Rh.sub.2.sup.0,II (dfpma).sub.3 > X.sub.2 (.eta..sup.1 -dfpma) has little affect on the overall > conversion efficiency. Considering the high concentration of > neat solvent, auxiliary traps cannot effectively compete for > the halogen photoproduct and thus its presence has little > affect on the outcome of the photochemistry performed in THF. > > If hydrogen atom abstraction from THF does occur, the > ultimate fate of the Br photoproduct should be HX (X=Cl, Br). > The conditions under which the above photolyses reactions were > executed, however, preclude detection of hydrohalic acids. > Because hydrohalic acids readily hydrolyze the N--P bond of > F.sub.2 PNR.sub.2 to form [H.sub.2 NR.sub.2 ].sup.+ X.sup.- > (and PF.sub.2 X), the acid photoproducts would be scavenged by > the excess dfpma present under photolytic conditions, thus > preventing its stoichiometric determination. Accordingly, the > dirhodium photochemistry was investigated in the presence of > PPh.sub.3, as this phosphine effectively coordinates reduced > Rh.sup.0 centers and also offers suitable hydrolytic > stability. > > The photochemistry of Rh.sub.2.sup.II,II (dfpma).sub.3 > Br.sub.4 in the presence of excess PPh.sub.3 proceeds > according to the same two-step reaction sequence that was > described for dfpma with the minor difficulty that > Rh.sub.2.sup.0,II (dfpma).sub.3 Br.sub.2 (PPh.sub.3) can not > be cleanly produced by wavelength selection. As listed in > Table 19, the middle-energy > X(.sigma.)/d.sigma..fwdarw.(d.sigma.\* transition of > Rh.sub.2.sup.0,II (dfpma).sub.3 Br.sub.2 (PPh.sub.3) is > observed at 371 nm. The red-shifted LMCT transition tails > significantly into the visible spectral region such that the > 436-nm excitation wavelength used to photoconvert > Rh.sub.2.sup.II,II (dfpma).sub.3 Br.sub.4 to Rh.sub.2.sup.0,II > (dfpma).sub.3 Br.sub.2 (PPh.sub.3) is also sufficiently > energetic to slowly convert Rh.sub.2.sup.0,II (dfpma).sub.3 > Br.sub.2 (PPh.sub.3), as it is produced, to Rh.sub.2.sup.0,0 > (dfpma).sub.3 (PPh.sub.3).sub.2. Despite experimental > complexity, the PPh.sub.3 system is ideal for quantifying the > HBr produced from the overall photoreaction sequence. > Quantification of HBr was indirectly determined by its > reaction with a nitrogen base. The sterically encumbered > 2,6-lutidine proved most useful, as the methyl groups flanking > the amine prevents competitive coordination of the base to the > metal center. Thus, bulk photolysis > (.lambda..sub.exc.gtoreq.335 nm, THF, 0.degree. C.) of > Rh.sub.2.sup.II,II (dfpma).sub.3 Br.sub.4 (1 equiv, 20 > .mu.mol) was performed in the presence of 2.5 equiv of > PPh.sub.3 and 4.3 equiv of 2,6-lutidine. After solvent removal > the solid residue was taken up in CDCl.sub.3, and the .sup.1 H > NMR spectrum was recorded (FIG. 31). Singlet resonances for > the methyl groups of the bridging dfpma ligands of > Rh.sub.2.sup.0,II at 2.83 and 2.91 ppm and of Rh.sub.2 0,0 at > 2.60 ppm distinguish the Rh.sub.2 dfpma photoproducts. A broad > singlet at 16.8 ppm and sharp singlet at 3.02 ppm are > signatures of the acid proton and methyl groups, respectively, > of lutidinium bromide. Integration of the dfpma methyl proton > signals reveal the production of 0.59 equiv of > Rh.sub.2.sup.0,II (dfpma).sub.3 Br.sub.2 (PPh.sub.3) and 0.41 > equiv of Rh.sub.2.sup.0,0 (dfpma).sub.3 (PPh.sub.3).sub.2 ; > the lutidinium bromide resonance integrates to 3.0 equiv. If > two equiv of HBr are produced for each two-electron > photoconversion of Rh.sub.2.sup.II,II (dfpma).sub.3 Br.sub.4 > and Rh.sub.2.sup.0,II (dfpma).sub.3 Br.sub.2 (PPh.sub.3), then > the production of 1.18 and 1.64 equiv of HBr, respectively, or > total of 2.82 equiv of HBr is required to accompany this > photolysis reaction. The good agreement between the calculated > and experimental yields of lutidinium bromide establishes > Scheme 17 as the overall photoreaction sequence for the > Rh.sub.2 dfpma system. ##STR18## > > **Quantum Yield Determination** > > Determination of the photoreaction stoichiometry permits > measurement of quantum yields (.PHI..sub.p) for the > photoreactions of Scheme 20 at selected excitation wavelengths > as in Table 20. For Rh.sub.2.sup.II,II (dfpma).sub.3 Br.sub.4 > photochemistry, quantum yields are virtually constant from 313 > nm to 405 nm (.PHI..sub.p.sup.313-405 =0.022.+-.0.003) but > then begin to decrease as .lambda..sub.exc is moved into the > visible spectral region (.PHI..sub.p.sup.436-468 > =0.012.+-.0.001). Exchange of bromide for chloride results in > an enhancement in the quantum yield as evidenced by the > .PHI..sub.p.sup.365 of 0.05.+-.0.01 determined for > Rh.sub.2.sup.II,II (dfpma).sub.3 Cl.sub.4. A similar trend is > observed in the attenuated quantum yields measured for > Rh.sub.2.sup.0,II (dfpma).sub.3 X.sub.2 (L) photochemistry. > The onset for the decrease in quantum yield for the > photoreduction of Rh.sub.2.sup.0,II (dfpma).sub.3 Br.sub.2 > (.eta..sup.1 -dfpma) occurs at shorter wavelengths > (.PHI..sub.p.sup.313-365 =0.0035.+-.0.0003, > .PHI..sub.p.sup.405-436 =0.0017.+-.0.0003) than in > corresponding Rh.sub.2.sup.II,II complex, and halogen exchange > results in a slight increase in efficiency upon chloride > substitution. > > TABLE 20 Product quantum yields (%) for photoreduction of > Rh.sub.2.sup.II,II (dfpma).sub.3 X.sub.4 and Rh.sub.2.sup.0,II > (dfpma).sub.3 X.sub.2 (.eta..sup.1 - dfpma) (X = Cl, Br) > complexes according to the stoichiometry of Scheme 17. > .lambda..sub.exc (nm) Starting Rh.sub.2 Complex 313 334 365 > 395 405 436 468 Rh.sub.2.sup.II,II (dfpma).sub.3 Cl.sub.4 -- > -- 5.0 -- -- -- -- Rh.sub.2.sup.II,II (dfpma).sub.3 Br.sub.4 > 2.4 2.5 2.0 1.7 2.2 1.2 1.3 Rh.sub.2.sup.0,II (dfpma).sub.3 > Cl.sub.2 -- -- 0.60 -- -- -- -- (.eta..sup.1 -dfpma) > Rh.sub.2.sup.0,II (dfpma).sub.3 Br.sub.2 0.32 -- 0.38 -- 0.20 > 0.14 -- (.eta..sup.1 -dfpma) > > The efficacy of THF to trap the halogen photoproduct is > effectively illustrated in the quantum yields determined in > the presence and absence of auxiliary coproduct traps. > Irradiation of Rh.sub.2.sup.0,II (dfpma).sub.3 Br.sub.2 > (.eta..sup.1 -dfpma) in THF containing 0.1 M > 2,3-dimethyl-1,3-butadiene and excess dfpma gives a product > quantum yield of 0.0048.+-.0.0005, confirming that the diene > cannot effectively compete with H-atom abstraction from the > THF solvent. Similarly, evaluation of the quantum yields in > the presence and absence of excess donor ligand underscores > the importance of the incoming axial ligand to the overall > stability of the Rh.sup.0 center. If solutions of > Rh.sub.2.sup.0,II (dfpma).sub.3 Br.sub.2 (.eta..sup.1 -dfpma) > in THF are irradiated in the absence of dfpma, the quantum > yield values drop by nearly an order of magnitude > (.PHI..sub.p.sup.365 (no dfpma)=5.8.times.10.sup.-4). > > **Electronic Structure Calculations** > > Molecular orbital calculations emphasize the electronic > structure features that are crucial to promoting the > four-electron photochemistry of the Rh.sub.2 dfpma series. > FIG. 32 shows the HOMOs and LUMOs of Rh.sub.2.sup.II,II > (dfpma).sub.3 Br.sub.4, Rh.sub.2.sup.0,II (dfpma).sub.3 > Br.sub.2 (PF.sub.3), and Rh.sub.2.sup.0,0 (dfpma).sub.3 > (PF.sub.3).sub.2 derived from extended Huckel calculations. > For each complex, the HOMO is approximately two-fold > degenerate and of metal d.pi.\* or d.delta.\* character, while > the LUMO is primarily localized between the metal centers and > of .sigma.\* character. This homology in the HOMOs and the > LUMOs is striking considering the disparate metal coordination > geometries and oxidation states across the Rh.sub.2 dfpma > series. > > The frontier MOs are largely a consequence of the large > one-electron splitting arising from the combination of > spatially directed d.sub.z.sub..sup.2 orbitals of the > individual fragments composing the Rh.sub.2 dfpma complexes. A > qualitative molecular orbital diagram for the > Rh.sub.2.sup.0,0, Rh.sub.2.sup.0,II and Rh.sub.2.sup.II,II > species, adapted from the extended Hucckel calculations, is > shown in Scheme 19. Consider the Rh.sup.0 P.sub.4 (C.sub.3v) > building block of the Rh.sub.2.sup.0,0 (dfpma).sub.3 (L).sub.2 > complex. The fragment has eight electrons residing in > (d.sub.xz, d.sub.yz) and (d.sub.xy, d.sub.x.sub..sup.2 > .sub.-y.sub..sup.2 ) orbitals and the odd electron occupying > the d.sub.z.sub..sup.2 orbital. The d.sub.z.sub..sup.2 > orbitals combine to give rise to the d.sigma.\* LUMO and a > filled d.sigma. level, energetically stabilized relative to > the d.pi./d.pi.\*(d.sub.xz, d.sub.yz) and > d.delta./.delta.\*(d.sub.xy, d.sub.x.sub..sup.2 > .sub.-y.sub..sup.2 ) manifold. Thus the HOMO is either d.pi.\* > or d.delta.\*, with the former prevailing when two Rh.sup.0 > P.sub.4 fragments are combined, and the formal Rh--Rh single > bond results from the pairing of the d.sub.z.sub..sup.2 > electrons within the d.sub.z.sub..sup.2 .sigma. level. Similar > orbital energetics are preserved for the Rh.sub.2.sup.II,II > (dfpma).sub.3 X.sub.4 and Rh.sub.2.sup.0,II (dfpma).sub.3 > X.sub.2 (L).sub.2 complexes. The d.sub.x.sub..sup.2 > .sub.-y.sub..sup.2 level of the Rh.sup.II P.sub.3 X.sub.2 > fragment is empty and displaced to high energy owing to the > destabilizing M-L.sub.eq .sigma.\* interactions. Consequently, > as with the Rh.sup.0 P.sub.4 fragment, the odd electron of the > Rh.sup.II P.sub.3 X.sub.2 fragment resides in the > d.sub.z.sub..sup.2 orbital, with the remaining six electrons > of the d.sup.7 metal center occupying the lower energy > (d.sub.xz, d.sub.yz) and d.sub.xy orbitals. Linear > combinations of the Rh.sup.II P.sub.3 X.sub.2 fragment > orbitals with those of another Rh.sup.II P.sub.3 X.sub.2 > fragment to give Rh.sub.2.sup.II,II (dfpma).sub.3 X.sub.4, or > with those of a Rh.sup.0 P.sub.4 fragment to give > Rh.sub.2.sup.0,II (dfpma).sub.3 X.sub.2 to a d.sigma.\* LUMO. > As was the situation for Rh.sub.2.sup.0,0 (dfpma).sub.3 > (L).sub.2, the d.sigma. level is stabilized significantly with > respect to the energetically proximate d.pi.\* and d.delta.\* > levels, a result of much smaller one-electron splittings > engendered by .pi. and .delta. overlap. The only difference > for the oxidized complexes is that the d.pi.\* orbitals (vs > d.delta.\* orbitals in FIG. 32(a)) emerge as the LUMO. Again, a > single Rh--Rh bond arises from electron pairing within the > d.sub.z.sub..sup.2 .sigma. orbital. ##STR19## > > The preservation of the metal-metal bond and consequently a > lowest energy d.sigma.\* excited state across the Rh.sub.2 > series is the key to the multi-electron photoreactivity. > Scheme 19 displays a simplified orbital diagram for the sigma > manifold along the metal-metal axis of the Rh.sub.2.sup.II,II > complex based on the extended Huckel results of FIG. 32 and > Scheme 18. The oxidized Rh.sub.2.sup.II,II and > Rh.sub.2.sup.0,II compounds are distinguished from their fully > reduced Rh.sub.2.sup.0,0 counterpart by a charge-transfer > component associated with promotion of an electron from the > .sigma.-bonding orbitals (labeled 1a.sub.g and 2a.sub.g in > Scheme 19) to the .sigma.\* LUMO (2a.sub.u). Here, the results > of the extended Huckel calculation and the observed > photochemistry converge. Population of the LUMOs of > Rh.sub.2.sup.II,II and Rh.sub.2.sup.0,II is consistent with > Rh--X bond homolysis and concomitant one-electron reduction of > the Rh.sup.II metal center. Moreover, a stepwise process for > the reductive elimination of bromine is suggested by the nodal > structure of the LUMOs. The localization of antibonding > character along the metal-metal internuclear axis points > towards the initial activation of the Rh--X.sub.ax bond. > ##STR20## > > **Discussion** > > As one-electron mixed-valence bimetallic cores promote single > electron transfer reactions, the results presented here show > that two-electron mixed-valence cores can support two-electron > redox pathways, affording a framework in which to rationally > design multi-electron reactivity. The metal-metal bonded > Rh.sub.2.sup.0,II complex sustains the multi-electron > reactivity of the Rh.sub.2 dfpma system by coupling > two-electron reduced Rh.sub.2.sup.0,0 and two-electron > oxidized Rh.sub.2.sup.II,II species. > > The thermodynamic driving force imparted by Rh--Rh bond > formation (BDE=32.+-.4 kcal mol.sup.-1) precludes the > stabilization of one-electron intermediates that would > short-circuit multi-electron reactivity. Photon absorption > into the X(.sigma.)/d.sigma..fwdarw.d.sigma.\* manifold of > Rh.sub.2.sup.II,II complexes prompts activation of an axial > Rh--X bond leading to one-electron reduction of the bimetallic > core and elimination of the halogen. Two unimolecular pathways > from the one electron intermediate can afford the observed > Rh.sub.2.sup.0,II (dfpma).sub.3 X.sub.2 (L) photoproduct. > Reductive cleavage of the equatorial Rh.sup.I --X bond of the > initial photoproduct would directly yield the reduced metal > center (Scheme 20, top pathway). Coordination of a donor > ligand would then give the Rh.sub.2.sup.0,II (dfpma).sub.3 > X.sub.2 (L) product. Alternatively, the orbital diagram of > Scheme 19 implies that ejection of the remaining axial halogen > might occur rapidly. As shown in the bottom pathway of Scheme > 20, loss of the second axial halogen ligand would produce a > dirhodium core of square planar Rh.sup.I centers, which then > disproportionate to a Rh.sup.0 --Rh.sup.II species to restore > the metal-metal bond. The observation of a blue intermediate > upon irradiation of Rh.sub.2.sup.II,II (dfpma).sub.3 Br.sub.4 > in THF solutions absent a donor ligand supports the > intermediacy of Rh.sup.I centers. In either mechanism, > thermodynamic remuneration afforded by re-establishing the > Rh--Rh bond drives elimination of the second halogen and > stabilizes the binuclear core to oxidative back-reaction. > Similarly, the photochemical reductive elimination chemistry > of Rh.sub.2.sup.0,II (dfpma).sub.3 X.sub.2 (L) appears to > proceed by an initial one-electron halogen elimination. > Formation of the metal-metal bond upon reduction to > Rh.sub.2.sup.0,0 facilitates expulsion of the second halogen > from the bimetallic core. ##STR21## > > Sustaining the metal-metal bond of the Rh.sub.2 dfpma system > also circumvents problems previously associated with the > utilization of two-electron mixed-valency in the design of > multi-electron schemes. Previous to the studies described > here, the presence of a two-electron mixed-valence > intermediate has been observed to render complexes inert to > further oxidation-reduction chemistry. This redox deactivation > has been attributed to the inability of the ligand to > electronically and conformationally support the appropriate > energetics that make the bimetallic core amenable to further > reaction. Along this line, the flexibility of the dfpma ligand > allows for the respective octahedral and trigonal bipyramidal > geometries of di- and zero-valent rhodium to be accommodated > with facility. Stabilization of these disparate coordination > geometries within a single bimetallic core of the > Rh.sub.2.sup.0,II complex maintains the reactivity of the > species by avoiding metal-metal bond cleavage that typically > deactivates binuclear complexes to multi-electron reactivity. > > Coupled two-electron photoreactions assume a prominent > position in energy conversion chemistry, especially when a > metal-halide bond is involved. Consider the splitting of > hydrohalic acids to H.sub.2 and X.sub.2. Whereas the > elimination of H.sub.2 from metal centers is feasible, the > benchmark studies on the energy conversion chemistry of > d.sup.8 . . . d.sup.8 dimers show that the elimination of > X.sub.2 poses a more significant challenge owing to the high > stabilities of the metal-halide bond. For instance, the HX > photochemistry of Rh.sup.I.sub.2 diisocyanide complexes is > stoichiometric because the cycle to regenerate the initial > photoreagent terminates with the formation of the Rh.sup.II > --X bond. The incorporation of a d.sigma.\* excited state > across the Rh.sub.2.sup.II,II (dfpma).sub.3 X.sub.4, > Rh.sub.2.sup.0,II (dfpma).sub.3 X.sub.2 (L), Rh.sub.2.sup.0,0 > (dfpma).sub.3 (L).sub.2 series surmounts the energetic barrier > to halogen atom elimination, and therefore provides a means > for interconversion between the series members in two electron > steps. > > Sequential two-electron reductive-elimination photoreactions > provide for efficient interconversion among the members of the > Rh.sub.2 -dfpma series. Photon absorption promotes activation > of an axial halogen leading to reduction of the metal center > and cleavage of the Rh--X bond. Preservation of the > metal-metal bond across the series maintains the reactivity of > the binuclear core, providing a reasonable platform for the > investigation of multi-electron reactions. > > **HX Photochemistry of Rhodium Diphosphazanes** > > The photochemical activation of M-X bonds in two electron > mixed-valence complexes prompted the development of a scheme > to produce hydrogen photocatalytically from hydrohalic acid. > Initial studies probed whether a Rh0 diphosphazane center > could efficiently reduce protons to dihydrogen. Methods to > couple the stoichiometric proton reduction to the reductive > elimination photochemistry were then be investigated. These > studies led to the construction of two HX splitting cycles > using Rh.sub.2 diphosphazanes as photocatalysts. > > Light driven energy conversion schemes were suggested as an > alternative energy source to expendable fossil fuel reserves > nearly a century ago. The ##STR22## > > target fuel of schemes developed since this proposal has been > hydrogen, generated from protic solutions. The most successful > approaches to date have used a heterogeneous catalyst to > couple the single electron equivalency provided by a > photoexcited transition metal sensitizer (e.g. Ru(II) > polypyridine complexes) to the two-electron equivalency > required for hydrogen production (Scheme 21). Photoexcited > electrons in the conduction bands of semiconducting electrodes > and nanoparticles are especially effective in promoting the > reduction of protons to hydrogen. Utilization of the attendant > hole in the valence band to generate a complementary oxidation > product completes a photocatalytic cycle. Hydrogen production > in the absence of mediators has also been realized, but only > under stoichiometric conditions. Research in the 1950's and > 1960's established that the ultraviolet irradiation of acidic > solutions containing reduced metal ions such as Ce.sup.3+, > Cr.sup.2+ and Fe.sup.2+ produced hydrogen and the one-electron > oxidized metal cation. In these schemes, excitation of a > charge-transfer-to-solvent (CTTS) absorption band effectively > produces a solvated electron that is trapped by a proton to > produce hydrogen atom radicals, which combine to produce > hydrogen. > > Gray and co-workers' seminal work on the photochemistry of > dirhodium(I) isocyanides in hydrohalic acid solutions > established the viability of using a molecular excited state > to promote proton reduction in homogeneous solution (Scheme > 22). Irradiation of the binuclear Rh.sup.I complex, > [Rh.sub.2.sup.I,I (bridge).sub.4 ].sup.2+ (bridge > =1,3-diisocyanopropane) in aqueous concentrated hydrohalic > acid solutions resulted in the stoichiometric production of > one equivalent of H.sub.2 and one equivalent of the > two-electron oxidized complex [Rh.sub.2.sup.II,II > (bridge).sub.4 Cl.sub.2 ].sup.2+. This system was of great > importance because it demonstrated the feasibility of driving > a multi-electron reduction from a discrete molecular excited > state. Whereas Ru-bipyridyl systems exemplified by Scheme 21 > and single-metal CTTS systems were based on single electron > transfer from a molecular excited state, the [Rh.sub.2.sup.I,I > (bridge).sub.4 ].sup.2+ complex could directly provide both > reducing equivalents for H.sub.2 production. The inability to > subsequently activate the Rh.sup.II --X bond of > [Rh.sub.2.sup.II,II (bridge).sub.4 Cl.sub.2 ].sup.2+ obviated > the regeneration of the initial photoreagent, thus ##STR23## > > preventing catalytic turnover. > > The four-electron reductive elimination photochemistry of the > Rh.sub.2 -dfpma class of complexes. Coupling to a viable > proton reduction pathway represents in light-to-chemical > energy scheme for catalytic hydrogen production directly > promoted by ##STR24## > > a molecular photocatalyst (Scheme 23). The M-X > photoactivation from this dirhodium platform allows for the > photocatalytic production of hydrogen from homogeneous > solutions of hydrohalic acid. > > **Hydrogen Production from Rhodium Dihydrides** > > Initial attempts to prepare binuclear rhodium hydride species > involved the treatment of Rh.sub.2.sup.0,II and > Rh.sub.2.sup.II,II halides with hydride transfer reagents. > Upon treatment of Rh.sub.2.sup.II,II (dfpma).sub.3 X.sub.4 > (X.dbd.Cl, Br) with reagents capable of delivering multiple > hydride equivalents such as NaBH.sub.4 or LiAlH.sub.4, > uncontrolled reduction of the rhodium complex was observed, > yielding intractable product mixtures. .sup.19 F NMR > spectroscopy indicated the presence of both Rh.sub.2.sup.0,II > and Rh.sub.2.sup.0,0 products depending on reaction > conditions. > > The preparation of rhodium dihydrides was targeted directly > by the reaction of dfpma with monomeric Rh.sup.I -hydride > starting materials. Rh.sup.I -halides, such as ##STR25## > > Wilkinson's catalyst, react with dfpma to afford two-electron > mixed-valence complexes according to Scheme 24. By analogy, > the reaction of dfpma with HRh(L).sub.n starting materials was > expected to afford species of the general formulation > Rh.sub.2.sup.0,II (dfpma).sub.3 H.sub.2 (L). The addition of > dfpma to HRh(PPh.sub.3).sub.4 in benzene solution resulted in > an immediate color change to red with concomitant gas > evolution. The product, Rh.sub.2.sup.0,0 (dfpma).sub.3 > (PPh.sub.3).sub.2, was isolated as an orange powder from the > reaction mixture in nearly quantitative yield. The product was > identified by .sup.1 H and .sup.19 F NMR spectroscopy. A > single methyl resonance was observed at 2.68 ppm for > methylamine bridgehead of the dfpma ligands and a high > frequency multiplet at 7.39-7.50 ppm was observed for the > axial PPh.sub.3 ligands. Appropriate integration ratios of > 9:30 established the incorporation of two PPh.sub.3 ligands > within the dirhodium framework. A single .sup.19 F NMR doublet > observed at 43.2 ppm and a .vertline..sup.1 J.sub.PF +.sup.3 > J.sub.PF.vertline. coupling constant of 1113 Hz are diagnostic > of the formation of a Rh.sub.2.sup.0,0 ##STR26## > > dimer possessing three bridging dfpma ligands. > > The H.sub.2 gas liberated from the reaction of Scheme 25 was > quantified independently by its collection with a Toepler > pump. Benzene was vacuum distilled from Na/benzophenone to a > flask containing HRh(PPh.sub.3).sub.4. The benzene solution > was frozen and exactly 1.6 equiv of the dfpma ligand was > transferred into the flask. Immediate reaction was observed > upon thawing the benzene solution, as evidenced by a color > change to red and by gas evolution. The solution was frozen > and the H.sub.2 was collected by Toepler pumping. 0.72 equiv > of non-condensable gas was identified to be H.sub.2 by burning > over hot CuO. The Rh.sub.2.sup.0,0 (dfpma).sub.3 > (PPh.sub.3).sub.2 product was collected in 85% yield, > confirming the 1:1 ratio of rhodium dimer:H.sub.2 gas. A > two-electron mixed-valence rhodium dihydride is presumably the > intermediate species from which H.sub.2 is evolved. > > **Stoichiometric Proton Photoreduction** > > The facile elimination of H.sub.2 from a dihydride > intermediate indicated that the binuclear rhodium core is > sufficiently electron-rich to effect the reduction of protons. > This potential reactivity pathway was explored by > investigating the reaction of HX with the Rh.sub.2 plafform. > However, solutions of Rh.sub.2.sup.0,0 (dfpma).sub.3 (L).sub.2 > complexes in CH.sub.2 Cl.sub.2 or THF did not oxidatively add > hydrohalic acids in the absence of light. It is well > established that oxidative addition to electronically > saturated metal complexes must be preceded by dissociation of > a coordinated ligand. Accordingly, the lack of reactivity > observed for Rh.sub.2.sup.0,0 (dfpma).sub.3 (L).sub.2 > complexes with HX is ascribed to the coordinatively saturated, > 36e.sup.-, Rh.sub.2.sup.0,0 core. One strategy for generating > vacant coordination sites is the photoelimination of carbonyl > or isonitrile ligands from a metal core. Thus Rh.sub.2.sup.0,0 > (dfpma).sub.3 (L).sub.2 complexes containing L=CO and CN.sup.t > Bu were prepared. > > Preparation of the symmetric complexes Rh.sub.2.sup.0,0 > (dfpma).sub.3 (CO).sub.2 and Rh.sub.2.sup.0,0 (dfpma).sub.3 > (CN.sup.t Bu).sub.2 followed as previously described. > Treatment of [ClRh(CO).sub.2 ].sub.2 with three equivalents of > dfpma under a CO atmosphere afforded the dicarbonyl complex > after recrystallization from CH.sub.2 Cl.sub.2 /hexanes at > -80.degree. C. Similarly, [ClRh(cod)].sub.2 reacted in the > presence of two equivalents of CN.sup.t Bu to give the > isonitrile derivative after similar workup. The complexes were > readily identified by .sup.19 F NMR spectra, which display > .vertline..sup.1 J.sub.PF +.sup.3 J.sub.PF.vertline. doublets > at -40.3 and -40.5 ppm for the CO and CN.sup.t Bu derivatives, > respectively. Though no net reaction occurs, the rhodium > dimers can be reversibly protonated with strong acids. The > reaction of Rh.sub.2.sup.0,0 (dfpma).sub.3 (CO).sub.2 with HCl > in CH.sub.2 Cl.sub.2 afforded an off-white solid upon > precipitation with pentane. Drying under reduced pressure > resulted in a color change back to yellow, and NMR spectra of > the yellow solid identically match the Rh.sub.2.sup.0,0 > dicarbonyl dimer. Similarly, treatment of Rh.sub.2.sup.0,0 > (dfpma).sub.3 (CN.sup.t Bu).sub.2 with one equivalent of > trifluoromethanesulfonic acid (HOTF, triflic acid) afforded > [HRh.sub.2 (dfpma).sub.3 (CN.sup.t Bu).sub.2 ][OTf] upon > precipitation, as determined by elemental analysis. In > solution, the cation deprotonates to regenerate > Rh.sub.2.sup.0,0 (dfpma).sub.3 (CN.sup.t Bu).sub.2 and the > triflic acid. > > In the absence of light, solutions of Rh.sub.2.sup.0,0 > (dfpma).sub.3 (CN.sup.t Bu).sub.2 with HBr in CH.sub.2 > Cl.sub.2 are stable for hours; however, FIG. 33 presents the > spectral changes observed upon irradiation of a CH.sub.2 > Cl.sub.2 solution containing Rh.sub.2.sup.0,0 (dfpma).sub.3 > (CN.sup.t Bu).sub.2 and 0.1 M HBr. The dicarbonyl compound > gave similar results, as did substitution the reaction with > HCl substituted for HBr. Excitation of the > d.sigma..fwdarw.d.sigma.\* transition of the Rh.sub.2.sup.0,0 > complex with 300.ltoreq..lambda..ltoreq.400 nm light resulted > in loss of the axial isonitrile ligand from the metal > coordination sphere followed by acid reaction. The absorption > spectrum of the final rhodium-containing product corresponds > to Rh.sub.2.sup.II,II (dfpma).sub.3 Br.sub.4 production. > Attendant H.sub.2 evolution was confirmed by Toepler pump > experiments, which revealed ca. two equivalents of > non-condensable gas that combusted over hot cupric oxide, > establishing the overall stoichiometry of the reaction to be, > ##STR27## > > The photo-inertness of phosphine ligands allows the > four-electron proton reduction of Equation 11 to be > deconstructed into distinct two-electron reactions. A > monocarbonyl dirhodium complex is directly available from the > in situ reduction of Rh.sub.2,II (dfpma).sub.3 Cl.sub.2 (CO) > with cobaltocene in the presence of triphenylphosphine. The > complex, Rh.sub.2.sup.0,0 (dfpma).sub.3 (CO)(PPh.sub.3), is > characterized by two .vertline..sup.1 J.sub.PF +.sup.3 > J.sub.PF.vertline. doublets in the .sup.19 F NMR spectrum at > -41.8 and -43.6 ppm. FIG. 34(a) displays the changes in the > absorption profile when Rh.sub.2.sup.0,0 (dfpma).sub.3 > (CO)(PPh.sub.3) is photolyzed with .lambda..sub.exc.gtoreq.335 > nm light in CH.sub.2 Cl.sub.2 solution containing 0.1 M HCl. > As shown in FIG. 34(b), similar reactivity was observed with > HBr. Examination of the terminating absorption spectrum > revealed that Rh.sub.2.sup.0,II (dfpma).sub.3 Cl.sub.2 > (PPh.sub.3) is the photoproduct. On the basis of the measured > molar absorption coefficients, the photoconversion of the > Rh.sub.2.sup.0,0 complex to the mixed-valence > Rh.sub.2.sup.0,II complex was quantitative. Furthermore, > collection of non-condensable gas with a Toepler pump was > consistent with the formation of one equivalent of H.sub.2 > during the photolysis. > > Wavelength selection of the excitation light suggests that > the two-electron reduction of H.sub.2 proceeds by a stepwise > reaction sequence. Irradiation of Rh.sub.2.sup.0,II > (dfpma).sub.3 Cl.sub.2 (PPh.sub.3) in a 0.1 M HCl/THF solution > with .lambda..sub.exc =335 nm light caused the changes in the > UV-Vis absorption spectrum shown in FIG. 35(a). Disappearance > of the Rh.sub.2.sup.0,0 (dfpma).sub.3 (PPh.sub.3)(CO) > absorption features were accompanied by the growth of an > absorption band centered at 580 nm. After 90 min of > irradiation, no further changes were observed in the 580-nm > absorption band; scaled up reaction conditions provided > 0.35(7) equiv of H.sub.2 per mole of Rh.sub.2 complex. The > 580-nm absorption profile did not change with continued > irradiation nor did its intensity change when solutions were > stored in the dark. Though the 580-nm intermediate has not > been isolated and characterized, its spectral features are > characteristic of linear tetranuclear rhodium clusters > possessing mixed-valence character. As observed by Gray and > co-workers in their studies of [Rh.sub.2.sup.I,I > (bridge).sub.4 ].sup.2+, a tetranuclear rhodium species can > result from the bimolecular reaction of two hydrido-halo > dirhodium cores to produce 0.5 equiv of H.sub.2 and the > tetranuclear species. Upon changing the excitation wavelength > to include visible wavelength frequencies, the absorbance > decreased with the concomitant appearance of the two-electron > mixed-valence dihalide, Rh.sub.2.sup.0,II (dfpma).sub.3 > Cl.sub.2 (PPh.sub.3) (FIG. 35(b)). Consistent with the overall > stoichiometry of eq 11, Toepler pumping of scaled-up > photoreactions gave an additional 0.38(7) equiv of H.sub.2. > > Equation 11 suggests that a second two-electron proton > reduction must be possible for the Rh.sub.2.sup.0,II complex. > Irradiation of Rh.sub.2.sup.II (dfpma).sub.3 Br.sub.2 > (CN.sup.t Bu) in CH.sub.2 Cl.sub.2 solutions containing 0.1 M > HBr gave rise to the absorption changes of FIG. 36. Similar > results were obtained for irradiation of Rh.sub.2.sup.0,II > (dfpma).sub.3 Cl.sub.2 (CN.sup.t Bu) with HCl. Again, > quantitative two-electron reaction was observed, yielding > Rh.sub.2.sup.II,II (dfpma).sub.3 Br.sub.4 and one equivalent > of hydrogen gas. Thus, each metal center appears to react > independently in two-electron steps according to the sequence, > ##STR28## > > **Low-Valent H.sub.2 Photocatalysis** > > Because a Rh.sub.2 0,0 species can be regenerated by > photolysis of Rh.sub.2.sup.0,II (dfpma).sub.3 X.sub.2 > (PPh.sub.3) in the presence of halogen atom traps, eq 12 can > be turned over and H.sub.2 can be generated > photocatalytically. A 50-mL THF solution containing > Rh.sub.2.sup.0,II (dfpma).sub.3 Cl.sub.2 (PPh.sub.3) (0.95 > .mu.mol) and 0.1 M HCl was irradiated with > .quadrature..sub.exc.gtoreq.335 nm after which the photolysis > was halted and H.sub.2 was collected by Toepler pumping. This > procedure was repeated at 3-hour intervals to generate the > plot in FIG. 37(a), which displays total H.sub.2 production > vs. time. A pseudo-initial rate of 27 turnovers per hour was > observed during the first 3-hour interval followed by a > decreased rate of H.sub.2 production with continued > photolysis. An attendant decrease in the absorbance of the > Rh.sub.2.sup.0,II (dfpma).sub.3 Cl.sub.2 (PPh.sub.3) catalyst > is shown in FIG. 37(b), indicating decomposition of the > two-electron mixed-valence dimer. > > Photolyses carried out with high catalyst concentrations for > long irradiation times resulted in polymerization of the THF > solvent. To determine if H.sub.2 formation originated from the > HX or from the decomposition of THF solvent, an isotope > crossover experiment was conducted. A photolysis carried out > using ten equivalents of HCl in d.sup.8 -THF was monitored by > .sup.1 H NMR spectroscopy. Only H.sub.2 was observed during > the first few hours of irradiation (ca. 1-2 turnovers). > Subsequently, HD was observed in the .sup.1 H NMR spectrum, > resulting from deuterium atom abstraction by photo-eliminated > halogen (Scheme 26, presumably D.sub.2 was also formed, but > not observed by .sup.1 H NMR spectroscopy). After five > turnovers of the dirhodium catalyst, the ratio of H.sub.2 :HD > was determined to be 1.4(2). The production of H.sub.2, > D.sub.2 and HD may be modeled as a binomial distribution with > the caveat that once HCl reacts to form H.sub.2 or HD, it is > permentantly removed from the catalytic cycle. Deuterium atom > abstraction from THF gives DCl, thus the total acid > concentration remains constant. Scheme 26 presents projected > H.sub.2, D.sub.2 and HD quantities, based on the reaction > chemistry of Scheme 26. After five turnovers, the projected > H.sub.2 :HD ratio is 1.2, in good agreement with the ratio > measured by NMR spectroscopy. ##STR29## > > Attempts to determine the quantum yield for H.sub.2 > production were complicated by the appearance of the 580-nm > intermediate during monochromatic UV irradiation. FIG. 39(a) > shows the UV-Vis absorption changes associated with the > irradiation (.lambda..sub.exc =335 nm) of Rh.sub.2.sup.0,II > (dfpma).sub.3 Cl.sub.2 (PPh.sub.3) in THF solution containing > 0.1 M HCl. Monitoring the disappearance of the band at 350 nm > provided a crude estimate of 0.005(2) for the photochemical > quantum yield. As seen in FIG. 39(a), the changes in the UV > region of the absorption spectrum were complete after 10 min > of irradiation, yet continued growth of the 580-nm band was > observed. This continued growth resulted from a slower dark > reaction, evident in FIG. 39(b), which shows a slow increase > in intensity for the 580-nm band in the absence of > irradiation. Though inconclusive, such an observation is in > accord with the dimerization of Rh.sup.0 - - - Rh.sup.I > species to form a tetranuclear cluster, as low local > concentrations of the one-electron mixed-valence species > should result in slow rates of formation. Analogous to the > 580-nm intermediate observed for the monochromatic irradiation > of Rh.sub.2.sup.0,0 (dfpma).sub.3 (PPh.sub.3)(CO), excitation > of this intermediate solution within the envelope of the > 580-nm absorption band led to regeneration of the > Rh.sub.2.sup.0,II (dfpma).sub.3 Cl.sub.2 (PPh.sub.3) complex. > > The above results are consistent with the catalytic cycle > shown in Scheme 27. Per Toepler pump experiments, two > equivalents of HX react with two unsaturated LRh.sup.0 > --Rh.sup.0 species to produce one equivalent of H.sub.2 and > the blue intermediate, which is tentatively ascribed to a > tetranuclear rhodium complex. This intermediate species is > photochemically stable in the absence of visible-light > irradiation; however, absorption of a 580 nm photon prompts > cleavage of the suspected tetramer followed by subsequent > reaction to give two molecules of the LRh.sup.0 --Rh.sup.II > X.sub.2 mixed-valence complex with the generation of an > additional equivalent of H.sub.2. The near-UV irradiation of > the two-electron mixed-valence photoproduct in the presence of > halogen atom trap regenerates LRh.sup.0 --Rh.sup.0, which is > available to react with HX to turn the cycle over. > > **High-Valent H.sub.2 Photocatalysis** > > The rate of hydrogen production appears to track both the > wavelength ##STR30## > > dependence (300 nm.ltoreq..lambda..ltoreq.400 nm) as well as > the quantum efficiency (.PHI..about.0.002-0.006) for reductive > elimination from the two-electron mixed-valence species. > Photochemical reductive elimination from Rh.sub.2.sup.II,II > (dfpma).sub.3 X.sub.4 occursat a higher quantum yield > (.PHI..about.0.01-0.05) and with lower energy light (300 > nm.ltoreq..lambda..ltoreq.480 nm) than from Rh.sub.2.sup.0,II > (dfpma).sub.3 X.sub.2 (L). Therefore, one strategy to improve > both quantum efficiency for H.sub.2 production and > photoreaction wavelength would be to catalytically turnover > the proton reduction of eq 13. > > Unlike the photochemistry of the Rh.sub.2.sup.0,II > (dfpma).sub.3 X.sub.2 (L) species, which only show slow > catalyst decomposition during HX photolysis, irradiation of > Rh.sub.2.sup.II,II (dfpma).sub.3 X.sub.4 complexes in the > presence of hydrohalic acids leads to rapid UV-Vis absorption > changes. The spectral changes associated with the > photochemical reaction of Rh.sub.2.sup.II,II (dfpma).sub.3 > Br.sub.4 with 0.1 M HCl in THF are displayed in FIG. 40. An > identical final spectrum was obtained when using > Rh.sub.2.sup.II,II (dfpma).sub.3 Cl.sub.4. Isosbestic points > at 303, 383 and 542 nm are maintained throughout the > transformation. Bands centered at 294 nm (.epsilon.=17,700 > M.sup.-1 cm.sup.-1) and 379 nm (.epsilon.=11,700 M.sup.-1 > cm.sup.-1) are suggestive of > X(.sigma.)/d.sigma..fwdarw.d.sigma.\* transitions derived from > a metal-metal bonded species. A shoulder observed near 450 nm > attributed to a d.pi.\*.fwdarw.d.sigma.\* type transition and a > weak band centered at 583 nm (.epsilon.=525 M.sup.-1 > cm.sup.-1) also grow in with photolysis. Continued irradiation > of the new species led to hydrogen production, as determined > by Toepler pump collection. Moderate turnover numbers varying > between 20 and 50 were obtained for experiments employing > Rh.sub.2.sup.II,II (dfpma).sub.3 Cl.sub.4 and > Rh.sub.2.sup.II,II (dfpma).sub.3 Br.sub.4, respectively (all > used HCl as the acid). > > To help elucidate the molecular structure of the new > dirhodium species, photolyses were carried out on a scale > suitable for NMR analysis. FIG. 41 presents the .sup.19 F NMR > spectra obtained for the irradiation of a 0.7 mL d.sup.8 -THF > solution of Rh.sub.2.sup.II,II (dfpma).sub.3 Cl.sub.4 > containing 0.2 M HCl. The spectrum of FIG. 41(a) is the > .sup.19 F NMR spectrum of Rh.sub.2.sup.II,II (dfpma).sub.3 > Cl.sub.4, showing the five-resonance .vertline..sup.1 J.sub.PF > +.sup.3 J.sub.PF.vertline. doublet pattern characteristic of > the Rh.sub.2.sup.II,II core. Condensation of anhydrous HCl > into the NMR tube resulted in no reaction as evidenced by the > .sup.19 F NMR spectrum presented in FIG. 41(b). The sample was > then irradiated using a 360-nm band-pass filter (300 > nm.ltoreq..lambda..sub.exc.ltoreq.400 nm) at 20.degree. C. > Within minutes the orange-red solution had turned intense > purple. When the sample was removed from the irradiation > source, the purple color rapidly faded to a dark red. After 3 > hours of irradiation, the sample was removed from the light > source and .sup.1 H and .sup.19 F NMR spectra were recorded. > The .sup.1 H NMR spectrum showed a new dfpma methyl resonance > at 3.05 ppm and a small peak at 4.53 ppm, attributed to > H.sub.2 gas. The .sup.19 F NMR, presented in FIG. 41(c), > indicated the formation of a new dirhodium species. The > conversion to the new complex was completed with continued > irradiation (18 hr) as shown in the .sup.19 F NMR spectrum of > FIG. 41(d). The .sup.1 H NMR spectrum showed evidence for > H.sub.2 evolution over the entire 18-hour irradiation period. > Furthermore, a 1:1:1 triplet at 4.50 ppm (.sup.1 J.sub.HD =43 > Hz) indicated the production of HD. As discussed herein, > halogen trapping by d.sup.8 -THF generates DCl, which in turn > enters the photocatalytic cycle to produce HD and D.sub.2. > > The most notable feature of the spectra in FIG. 41(c)-(d) is > the low frequency doublet -15.4 ppm, which is diagnostic of a > PF.sub.2 group coordinated axially to a Rh.sup.0 center. > Rearrangement of a single bridging dfpma ligand to a chelating > coordination mode would account for this low frequency > PF.sub.2 resonance. One possible assignment for this new > rearranged species is shown in Scheme 28. In the absence of a > suitable donor ligand, a structure analogous to that observed > for Ir.sub.2.sup.0,II cores can be obtained by photochemical > reductive elimination from the Rh.sub.2.sup.II,II platform. > ##STR31## > > The new complex, Rh.sub.2.sup.0,II (dfpma).sub.3 Cl.sub.2, > was independently prepared by treating [ClRh(CO).sub.2 ].sub.2 > with three equivalents of dfpma in CH.sub.2 Cl.sub.2. Gas > evolution was accompanied by the formation of a deep red > solution. The solvent was then removed to leave a sticky red > solid that was treated with a 1:2 solution of benzene and > pentane. Rh.sub.2.sup.0,II (dfpma).sub.3 Cl.sub.2 (CO) was > isolated as an orange-red powder. Unlike the other > Rh.sub.2.sup.0,II (dfpma).sub.3 X.sub.2 (L) derivatives > described herein, Rh.sub.2.sup.0,II (dfpma).sub.3 Cl.sub.2 > (CO) is not stable in the solid state. Orange-red samples > turned green if left under active vacuum overnight, with > concomitant loss CO as indicated by the loss of the > .nu..sub.CO stretch at 2057 cm.sup.-1. The green solid affords > deep red solutions in THF, and as shown in FIG. 41(e), the > .sup.19 F NMR spectrum in d.sup.8 -THF solution identically > matches the Rh.sub.2 photoproduct. Presumably, CO loss gives > the intermediate species depicted in Scheme 29, which > rearranges to the final structure in solution. The most > notable features in the .sup.19 F NMR spectrum of > Rh.sub.2.sup.0,II (dfpma).sub.3 Cl.sub.2 product are the high > frequency doublet for the axial PF.sub.2 of the chelating > ligand, observed at -15.4 ppm, and the low frequency > .vertline..sup.1 J.sub.PF +.sup.3 J.sub.PF.vertline. doublet > for the PF.sub.2 groups located trans to the chloride ligands, > observed at -80.8 ppm. A critical difference in the .sup.19 F > NMR spectra of FIG. 41 is the conditions under which the data > were collected. In the spectra of FIG. 41(b)-(d), the d.sup.8 > -THF solution was 0.2 M in HCl; in the spectrum of FIG. 41(e), > no acid was present. Indeed, treatment of d.sup.8 -THF > solutions of Rh.sub.2.sup.0,II (dfpma).sub.3 Cl.sub.2 with up > to 10 equiv of anhydrous HCl gas resulted in no observable > change in either the .sup.1 H or .sup.19 F NMR spectra > (excepting observation of the solvated proton in the .sup.1 H > NMR spectrum). ##STR32## > > In contrast to the low reactivity of Rh.sub.2.sup.0,II > (dfpma).sub.3 Cl.sub.2 with proton sources, pure .sigma.-donor > ligands add to the vacant axial site of the rhodium dimer as > in Scheme 30. The .sup.1 H NMR of the PMe.sub.3 derivative > shows a doublet for the alkyl phosphine ligand at 1.78 ppm > (.sup.2 J.sub.PH =11 Hz) and two distinct methyl resonances at > 2.93 and 3.10 ppm for the chelating and bridging dfpma > ligands, respectively. The .sup.19 F NMR spectrum of the > PMe.sub.3 complex displays a low frequency pattern largely > unchanged from the parent Rh.sub.2.sup.0,II (dfpma).sub.3 > Cl.sub.2 complex, but the high frequency axial PF.sub.2 groups > shifts slightly downfield to -13.1 ppm. Similarly, the .sup.1 > H NMR of the [Rh.sub.2.sup.0,II (dfpma).sub.3 Cl.sub.3 ].sup.- > anion shows resonances at 2.79 and 2.86 ppm for the dfpma > ligands. The signature resonance for the axial PF.sub.2 group > of the [Rh.sub.2.sup.0,II (dfpma).sub.3 Cl.sub.3 ].sup.- anion > is shifted up to +7.4 ppm in the .sup.19 F NMR spectrum. > ##STR33## > > Oxidative addition of halogens to Rh.sub.2.sup.0,II > (dfpma).sub.3 Cl.sub.2 proceeded smoothly, yielding > valence-symmetric Rh.sub.2.sup.II,II (dfpma).sub.3 Cl.sub.2 > X.sub.2 products (Scheme 30). This is a structural departure > from the reactivity displayed by Ir.sub.2.sup.0,II > (tfepma).sub.3 Cl.sub.2, which affords Ir.sub.2.sup.I,III > (tfepma).sub.3 Cl.sub.4 upon oxidation with chlorine. > Moreover, the addition of bromine to Rh.sub.2.sup.0,II > (dfpma).sub.3 Cl.sub.2 proceeded at one metal center, to give > a Br.sub.2 Rh.sup.II --Rh.sup.II Cl.sub.2 oxidation product as > indicated by the .sup.19 F NMR spectrum of Scheme 30. The most > notable indicator of coordination geometry is the > low-frequency resonances at -76.1 and -77.6 ppm, assigned to > PF.sub.2 groups of the dfpma ligands located trans to halide > ligands. The observation of two distinct resonances in this > region unambiguously establishes the absence of a mirror plane > in the Rh.sub.2.sup.II,II product, which would be expected for > a ClBrRh.sup.II --Rh.sup.II BrCl complex. > > Based on the observed reactivity of Rh.sub.2.sup.0,II > (dfpma).sub.3 Cl.sub.2, the cycle shown in Scheme 31 is > proposed for photochemical hydrogen production using the > high-valent catalyst. Irradiation with UV-visible light > promotes halogen elimination from the binuclear Rh.sup.II > complex to afford Rh.sub.2.sup.0,II (dfpma).sub.3 Cl.sub.2 > after rearrangement of a bridging dfpma ligand. As observed in > the chemistry of Ir.sub.2.sup.0,II (tfepma).sub.3 Cl.sub.2, > coordination of a halide to form the 36e.sup.- anion > facilitates protonation of the binuclear species before a > hydrogen-evolving step to regenerate the Rh2.sup.II,II > tetrahalide complex. ##STR34## > > Rh.sub.2 -dfpma complexes have provided a novel platform for > the photocatalytic production of hydrogen from hydrohalic > acids. Irradiation of Rh.sub.2.sup.0,II (dfpma)3X2(L) > complexes in acidic THF solution resulted in hydrogen > production via turnover of a Rh.sub.2.sup.0,II > /Rh.sub.2.sup.0,0 valence couple. Similarly, a high-valent > two-electron couple between Rh.sub.2.sup.II,II and > Rh.sub.2.sup.0,II provides photocatalytic proton reduction. > The unifying feature in these two systems is the preservation > of a metal-metal bond across the four-electron > Rh.sub.2.sup.0,0 /Rh.sub.2.sup.0,II /Rh.sub.2.sup.II,II > series. The formation of a metal-metal bond can provide a > strong driving force for reductive elimination from binuclear > rhodium cores. In this manner, halogen elimination from the > Rh.sub.2 -dfpma core is facilitated and the catalytic cycles > of Schemes 27 and 31 can be successfully turned over. > > This result is where the Rh.sub.2 -dfpma chemistry diverges > from the system of Gray and co-workers shown in Scheme 22. > Here formation of a metal-metal bond provides a strong driving > force for oxidation of a binuclear core, facilitating the > multi-electron proton reduction. However, regeneration of the > Rh.sup.I hydrogen-generating species requires cleavage of the > metal-metal bond in the [Rh.sub.2.sup.II,II (bridge).sub.4 > X.sub.2 ].sup.2+ photoproduct, adding a 32.+-.4 kcal > mol.sup.-1 energy disbursement to the energy required for M-X > bond cleavage. By maintaining the metal-metal bond throughout > the catalytic cycle the Rh.sub.2 -dfpma system circumvents > this operational energy cost. > > Halogen reduction by a sacrificial trap drives the catalytic > turnover of both the high-valent and the low-valent rhodium > systems. Thus, catalytic H.sub.2 production is only realized > in the presence of an external reductant, which in the > Rh.sub.2 -dfpma systems reduces halogen atoms to halides. The > thermodynamic driving force imparted by halogen trapping in > the current scheme obviates the design of an energy storing > cycle, as an authentic light-to-energy strategy requires > isolation of the attendant oxidizing equivalents. As shown in > Scheme 32, for cycles based on HX cleavage, the next step must > be to design a system capable of delivering both H.sub.2 and > X.sub.2 products. ##STR35## > > The processes described in the Examples utilize transition > metal catalyst complexes as homogenous catalysts. However, the > catalysts may be modified to be immobilized on solid surfaces > or as solid surfaces to provide a heterogeneous catalytic > process. Such solid surfaces may include, but are not limited > to, ion exchange resins, silicon containing particles, solid > surfaces, for example. > > **EXAMPLES** > > **General Synthetic Considerations** > > Synthetic manipulations were conducted in the dry, anaerobic > environment provided by a Schlenk-line or by a nitrogen-filled > glove box. Solvents for synthesis were reagent grade or better > and were dried by following standard procedures. Elemental > analyses were performed at H. Kolbe Mikroanalytisches > Laboratorium. > > The starting materials [ClRh(CO).sub.2 ].sub.2 and > [ClRh(cod)].sub.2 (Strem) were used as received. The ligands, > MeN(PF.sub.2).sub.2, (dfpma), MeN[P(OMe).sub.2 ].sub.2 (dmpma) > and MeN[P(OPh).sub.2 ].sub.2 (dppma) were prepared by > published procedures, MeN[P(OCH.sub.2 CF.sub.3).sub.2 ].sub.2 > (tfepma) and ArN(PX2).sub.2 (dfpx) were prepared by adaptation > of these procedures. > > Chlorine was delivered by means of the iodobenzene adduct, > PhICl.sub.2. The starting materials triethylamine > (Alfa-Aesar), 2,2,2-trifluoroethanol (Aldrich), > triphenylphosphine (Alfa-Aesar), trifluoromethanesulfonic acid > (Alfa-Aesar), d1-trifluoromethanesulfonic acid (Aldrich) and > gaseous reactants, bromine, H.sub.2 (BOC Gases, UHP Grade 5), > HCl, D.sub.2 and DCl (Aldrich), were used as received. The > ligand precursor MeN(PCl.sub.2).sub.2 was prepared by > following published procedures. The acid HCl was generated by > dropping concentrated sulfuric acid (95-98%, Alfa-Aesar) onto > anhydrous NaCl (Aldrich). The gas was collected under vacuum > and freeze-pump-thaw degassed once before being introduced to > the reaction vessel. Anhydrous HBr was used from a lecture > bottle (AGA) and freeze-pump-thaw degassed at least twice > before being introduced to the reaction vessel. > > Spectroscopic and photochemistry experiments employed > spectroscopic grade tetrahydrofuran (Burdick & Jackson) > and benzene (Aldrich), which were stored over Nak-benzophenone > under vaccum or in a glove box. Bis(diflurophosphine)methyl > amine was prepared by literature procedures, phosphorous > triflouride (Elf Atochen) and 2,6-Lutidrine (Aldrich, > redistilled) were used as received. Triphenylphosphine (Strem) > and 9,10-dihydroanthracene (Aldrich) were recrystallized at > least once and 2,3-dimethylbutadiene (Aldrich) was distilled > from NaBH.sub.4 and stored under high vaccum. > > **Physical Methods** > > All NMR spectra were collected at the MIT Department of > Chemistry Instrumentation Facility on a Varian Inova-Unity > 500, Varian Unity 300 Spectrometer, or Varian Mercury 300 > Spectrometer at 25.degree. C. The NMR solvents, C.sub.6 > D.sub.6, d8-THF, CD.sub.3 CN and CDCl.sub.3 (Cambridge Isotope > Laboratories) were dried using appropriate agents and degassed > by at least three freeze-pump-thaw cycles or used as received > in glass ampoules. 1H NMR spectra were referenced to TMS using > the residual proteo impurities of the given solvent. 1H NMR > (300 MHz), 19F and 19F{31P} NMR spectra were referenced to an > internal CFCl.sub.3 or TMS standard. All chemical shifts are > reported using the standard .delta. notation in > parts-per-million; positive chemical shifts are to a higher > frequency from the given reference. > > IR spectra were recorded on a Nicolet Impact 410 spectrometer > either as KBr pellets or as CH.sub.2 Cl.sub.2 solutions > between NaCl plates. Absorption spectra were recorded on an > OLIS-modified CARY-17 Spectrophotometer in quartz cells > isolated from air by Teflon valves. Steady-state and > time-resolved emission spectra were recorded on isomorphous > powders contained in quartz tubes, cooled in quartz finger > dewars. > > Emission lifetimes were measured on a nanosecond laser > instrument utilizing a Coherent Infinity XPO laser as the > source. The 3rd-harmonic of a diode pumped Nd:YAG laser passed > through a tunable Type I XPO cavity housing a BBO crystal. The > 710 nm output, was then doubled to 355 nm (.ltoreq.7 ns FWHM > and average power of 1 mJ). Solid samples sealed in a quartz > tube were excited orthogonal to detection. Scattered > excitation light was omitted from the optical detection train > by a 366-nm long pass filter. Emitted light from the sample > passed through f/4 collimating and f/4 focusing lenses onto > the entrance slit of an Instruments SA Triax 320 > monochromator. The signal wavelengths were dispersed by a > grating possessing a blaze wavelength of 500 nm and a 300 > grooves/cm density. Signal was detected with a Hamamatsu R928 > PMT. The output from the PMT was fed into a LeCroy 1 GHz > 9384CM digital oscilloscope, which was triggered from the > Q-switch sync output of the laser. Monochromator operation, > data storage and data manipulation were managed by National > Instruments driver software (Labview) incorporated into > programs written at MIT. Communication between a Dell Optiplex > GX-1 computer and the instrumentation was achieved through a > IEEE-488 (GPIB) interface. Lifetime decays were obtained at > 820 nm and signal averaged at 20 Hz for 1000 pulses. > > Hydrogen gas was collected on a vacuum line equipped with > Toepler pump and CuO burn tube. Solutions were frozen in > liquid nitrogen and the non-condensable gases were passed > through three U-traps maintained at liquid nitrogen > temperatures. Solutions were typically thawed and re-frozen > twice during gas collection to ensure complete removal of > dissolved hydrogen. Gas collection was typically continued for > an hour after visible signs of gas transfer ceased (i.e., no > gas bubbled up past the check valve). The efficiency of the > Toepler pump was determined by collecting gas from a flask > containing a known volume and pressure of hydrogen, and > repeatedly gave collection quantities that were 70-75% of the > known quantity; nevertheless, all H2 quantities reported here > are the measured values and are not adjusted for this > systematic error. Confirmation that the non-condensable gas > was hydrogen came from re-circulating the gas over CuO heated > to 320.degree. C. for an hour followed by collection of > residual non-condensable gas. In all cases, only insignificant > gas quantities remained after combustion. > > **Crystallographic Procedures** > > X-ray diffraction data were collected on a Siemens 3-circle > platform diffractometer equipped with a CCD detector. > Measurements were carried out at -90.degree. C. using Mo > K.alpha. (.lambda.=0.71073 .ANG.) radiation, which was > wavelength selected with a single crystal graphite > monochromator. Four sets of data were collected using .omega. > scans and a -0.3.degree. scan width. All calculations were > performed on a Silicon Graphics Indigo 2 workstation. The data > frames were integrated to hkl/intensity and final unit cells > were calculated by using the SAINT program v.4.050 from > Siemens. The structures were solved and refined with the > SHELXTL v5.03 suite of programs developed by G. M. Sheldrick > and Siemens Industrial Automation, Inc, 1995. > > **General Details of X-Ray Data Collection and Reduction** > > X-ray diffraction data were collected on a Siemens 3-circle > platform diffractometer equipped with a CCD detector. > Measurements were carried out at -90.degree. C. using Mo > K.alpha. (.lambda.=0.71073 .ANG.) radiation, which was > wavelength selected with a single crystal graphite > monochromator. Four sets of data were collected using .omega. > scans and a -0.3.degree. scan width. All calculations were > performed on Windows NT workstations equipped with Intel x86 > processors. The data frames were integrated to hkl/intensity > and final unit cells were calculated by using the SAINT+ > program v.6.01 from Bruker AXS, 1999. The structures were > solved by the Patterson heavy atom method in conjunction with > standard difference Fourier techniques. Fluorine atoms of the > --CF3 groups were placed in ideal positions and refined as a > rigid group before being allowed to refine freely in the final > refinement cycles. Hydrogen atoms were placed in calculated > positions using a standard riding model and they were refined > isotropically. All data manipulations were conducted within > the SHELXTL v5. 1 suite of programs developed by G. M. > Sheldrick and Bruker AXS, 1998. > > **Extended Huckel Calculations** > > Electronic structure calculations were performed on a Silicon > Graphics Indy workstation using the YAeHMOP software, v2.0.69 > Valence orbitals for all atoms were used in the basis set. The > molecular structure of complex 3 was approximated as the > idealized molecule, Ir2(PH3).sub.6 Cl2. Iridium-ligand bond > lengths and angles for the complex were taken from the crystal > structure of 3. Graphic representations of the metal-based > HOMO and LUMO for each molecule were generated from the > Viewkel output of the YAeMOP calculation and subsequently > modified with the ray-tracing program Rayshade. > > The extended Huckel calculations of the Rh.sub.2 0,0 and > Rh.sub.2.sup.II,II complexes were performed by using the > atomic positions taken from the crystal structures of Rh.sub.2 > 0,0(dfpma).sub.3 (PF.sub.3).sub.2 and Rh.sub.2.sup.II,II > (dfpma).sub.3 Br4, respectively. For the mixed-valence > Rh.sub.2.sup.0,II compound, an idealized molecule, > Rh.sub.2.sup.0,II (dfpma).sub.3 Br.sub.2 (PF.sub.3), was > constructed with the atomic positions obtained from the > crystal structure of Rh.sub.2.sup.0,II (dfpma).sub.3 Br.sub.2 > (.eta.1-dfpma). The axially coordinated dfpma ligand was > replaced by PF.sub.3 (P--F bond lengths of 1.57 .ANG. and > Rh--P--F angles of 120.degree.); bond angles and lengths were > obtained from the average values of the terminal PF.sub.3 > ligands in the crystal structure of Rh.sub.2 0,0(dfpma).sub.3 > (PF.sub.3).sub.2. An idealized conformation was adopted such > that the PF.sub.3 fluorines were staggered with respect to the > three phosphorous atoms of the Rh0 equatorial plane. > > **General Photochemical Procedures** > > Small-scale photolysis experiments were carried out in high > vacuum cells composed of a 1-cm clear-fused-quartz cuvette and > 20-ml solvent reservoir isolated from each other and the > atmosphere by Teflon valves. Spectroscopic grade solvent was > dried and added to the cell by vacuum transfer. Hydrogen > halide gases were freeze-pump-thawed once before transfer into > the cell. Large-scale photolysis experiments were performed in > 100-ml custom high-vacuum quartz reaction tubes with a path > length of .about.2.5 cm. Samples were irradiated with light > from a 1000-W high pressure Oriel Hg--Xe lamp. The two-inch > collimated light beam passed through a distilled water filter > to remove infrared wavelengths and long wave pass filters to > remove high-energy light prior to focusing and collimating to > a diameter of 0.5". The high-energy cut-off filters were > replaced with 10-nm bandpass mercury line interference filters > (Oriel) for quantum yield experiments. The light flux used for > quantum yield determination at a given wavelength was measured > using the standard ferrioxalate actinometer just before and > just after sample irradiation. The progress of the > photoreaction was monitored with absorption spectra recorded > on a Spectral Instruments CCD Array Spectrophotometer. > > **HX Control Reactions** > > The thermal reactivity of Rh.sub.2.sup.II,II (dfpma)3X4, > Rh.sub.2.sup.0,II (dfpma).sub.3 X 2(L) and Rh.sub.2 > 0,0(dfpma).sub.3 (L).sub.2 with HX in THF was evaluated under > the conditions employed for photochemical experiments. Thus, a > cuvette of a photolysis cell was charged with either a small > amount of the rhodium complex. THF was distilled into the > solvent reservoir of the cell under vacuum and subjected to > three freeze-pump-thaw cycles. Anhydrous HX was then frozen > into the reservoir after a single freeze-pump-thaw cycle. The > HX/THF solution was thawed and then mixed with the rhodium > complex under photographic darkroom lights. An initial > absorption spectrum was recorded. The cell was wrapped in foil > and maintained at 20.degree. C. overnight. After twelve hours, > another UV-Vis spectrum of the sample showed only negligible > changes in the absorption profile. > > Similarly, thermal hydrogen evolution by the rhodium > complexes was investigated by conducting experiments on a > larger scale. 50-mL THF solutions of each rhodium complex (ca. > 0.1 mM) containing 0.1 M HCl were wrapped in foil and > maintained at 20.degree. C. for 12 h. Toepler pump collection > of all non-condensables afforded an insignificant quantity of > non-condensable gas (.ltoreq.3.times.10-6 mol), which did not > burn over CuO. > > Hydrogen evolution in the absence of a rhodium catalyst was > not observed either. A 50-mL THF solution containing 0.1 M HCl > was irradiated (.lambda.exc.gtoreq.338 nm) for 12 h at > 20.degree. C. Subsequent Toepler pump collection of > non-condensable gases afforded <2.times.10-6 mol gas that > did not combust over CuO. > > **Example 1** > > Preparation of tfepma > > Dropwise addition of CF.sub.3 CH.sub.2 OH (36.8 g, 368 mmol, > 4.25 equiv) to a -80.degree. C. solution of triethylamine > (36.4 g, 360 mmol, 4.16 equiv) and MeN(PCl.sub.2).sub.2 (20.15 > g, 86.56 mmol, 1 equiv) in 500 mL of diethyl ether results in > a rapid and exothermic reaction, with concomitant formation of > the white [Et.sub.3 NH]Cl salt. After warming to room > temperature, the mixture was stirred for 24 h. Filtration > followed by rotary evaporation to remove ether afforded impure > product as a clear, viscous liquid. Distillation under reduced > pressure (75-85.degree. C., 0.5 torr) was accompanied by some > decomposition of the ligand, necessitating a second filtration > to give 23.6 g (58% yield) of pure ligand. 1H NMR (300 MHz, > C.sub.6 D.sub.6) .delta./ppm: 2.506 (td, 3.898 Hz, 0.600 Hz, > 3H), 3.55 (dp, 17.12 Hz, 4.4 Hz, 8H). 31P{1H} NMR (121.4 MHz, > C.sub.6 D.sub.6) .delta./ppm: 148.614 (s). 19F NMR (282MHz, > C.sub.6 D.sub.6) .delta./ppm: -76.90 (m). > > **Example 2** > > Preparation of Bis(dichlorophosphine)-3,5-xylidene (dcpx) > > Freshly distilled 3,5-dimethyl aniline (3,5-xylidene, > .about.97 g, 0.8 mol) was transferred under N.sub.2 with a > cannula to a flask containing rapidly stirred PCl.sub.3 (450 > g, 3.28 mol) at -10.degree. C. White solid began precipitating > immediately with aniline addition. When addition was complete, > the mixture was heated to reflux until all solid had dissolved > (48 hr). The solution was then cooled to room temperature and > stored at -35.degree. C. overnight. A mass of white crystals > was precipitated from solution. The solid was collected by > filtration and recrystallized from hot hexanes to afford 159 g > (62% yield) of product. A second crop of product was obtained > from the reaction solution by reducing the PCl.sub.3 volume to > one fourth and cooling overnight. Recrystallization gave an > additional 40 g (16% yield) of product. 31P{1H} NMR (282.5 > MHz, C.sub.6 D.sub.6) .delta./ppm: 157.04 (s). > > **Example 3** > > Preparation of Bis(difluorophosphine)-3,5-xylidene (dfpx) > > Solid SbF.sub.3 (76.1 g, 0.426 mol) and dcpx (50.4 g, 0.156 > mol) were loaded into a 500-mL flask equipped with stir bar, > reflux condenser and nitrogen inlet. Pentane (250 mL) was > added and the vessel was purged for 5 minutes with N.sub.2. > The mixture was then heated to reflux for 3 hr. Upon cooling > back down to room temperature, the pentane solution was > decanted and the solid antimony residue washed with a 100-mL > aliquot of pentane. The washings were added to the original > reaction solution and the solvent was removed on a rotary > evaporator to afford 35 g (87% yield) of crude product. White > crystalline material is readily obtained by sublimation at > 40-50.degree. C. (0.1 torr). 1H NMR (300 MHz, C.sub.6 D.sub.6) > .delta./ppm: 1.94 (s, 6H), 6.60 (s, 1H), 6.68 (s, 2H). 31P NMR > (121.4 Hz, C.sub.6 D.sub.6) .delta./ppm: 133.22 > (.vertline.1JPF+2JPF.vertline.=1514 Hz). .sup.19 F NMR (282.4 > Hz, C.sub.6 D.sub.6) .delta./ppm: -68.46 > (.vertline.1JPF+2JPF.vertline.=1514 Hz). > > **Example 4** > > Preparation of Bis(bis(trifluoroethyl)phosphite)-3,5-xylidene > (tfepx) > > Pyridine (20 g, 253 mmol) and dcpx (19.8 g, 61.3 mmol) were > added under N.sub.2 to 500 mL of ether in a 1 L flask. The > solution was cooled in a dry ice/acetone bath. > 2,2,2-Trifluoroethanol (25 g, 247 mmol) was added slowly with > a syringe to the rapidly stirred solution, resulting in an > exothermic reaction and formation of a white solid. After the > addition, the mixture was warmed slowly and stirred at room > temperature overnight. The white solid was removed by > filtration, and the ether stripped from the mother liquor by a > rotary evaporator, leaving a yellow solid. Recrystallization > from pentane at -80.degree. C. afforded the product as a white > solid (17.41 g, 49% yield). Concentration of the pentane > mother liquor to 50 mL followed by cooling to -80.degree. C. > provided a second crop of product (10.23 g, 29% yield). 1H NMR > (300 MHz, C.sub.6 D.sub.6) .delta./ppm: 2.09 (s, 6H), 3.62 > (dm, 33 Hz, 8H), 6.64 (s, 1H), 6.86 (s, 2H). 31P NMR (121.4 > Hz, C.sub.6 D.sub.6) .delta./ppm: 141.11 (s). 19F NMR (282.4 > Hz, C.sub.6 D.sub.6) .delta./ppm: -74.86 (m). > > **Example 5** > > Preparation of Rh.sub.2.sup.0,II (dfpma)3X 2L (1-L, 2-L) and > Rh.sub.2.sup.0,II (dfpx).sub.3 X2L (22) > > In a typical experiment, [XRh(cod)].sub.2 is dissolved in 10 > mL of benzene giving a pale orange solution. Successive > additions of three equivalents of dfpma or dfpx and one > equivalent of L (L=CNR, P(OR).sub.3, PR.sub.3) results in > rapid color changes finally giving a dark red solution. > Stirring overnight precipitates an orange to red powder > depending on L. Precipitation is completed by the addition of > an equal volume of pentane. The product is collected by > filtration and washed three times with 1:1 benzene/pentane and > dried in vacuo. Typical yields are 80-90% based on > [ClRh(cod)].sub.2. NMR spectroscopy is useful for > fingerprinting the compound: 1H NMR shows two peaks in the > 2.6-3.2 ppm region integrating in a 2:1 ratio for the methyl > groups of the bridging dfpma ligands plus any signature > resonances for the axial L ligand; .sup.19 F NMR shows a > complex spectrum that simplifies to a six line pattern upon > 31P decoupling. See Results and Discussion. > > **Example 5** > > Preparation of Rh.sub.2 0,0(dfpma).sub.3 L.sub.2 (3-L) > > In a typical reaction, [ClRh(cod)].sub.2 is stirred with > three equivalents of dfpma, two equivalents of cobaltocene and > two equivalents of L (L=CNR, P(OR).sub.3, PR.sub.3) in diethyl > ether or THF. [CoCp.sub.2 ]Cl precipitates as a yellow powder > and is removed by filtration. The solvent is stripped and the > residue taken up in a minimal amount of CH.sub.2 Cl.sub.2, > filtered and diluted with pentane. Cooling to -80.degree. C. > affords the product as yellow to orange micro crystals in > 40-80% yield depending on L. 1H and 19F NMR spectroscopy are > useful for product characterization: a single methyl resonance > is observed in the 1H NMR spectrum in the 2.3-2.7 ppm region > for the bridging dfpma ligands in addition to any signature > resonances for L; the 19F NMR shows a simple doublet near -40 > ppm displaying a 1JFP=1100-1300 Hz. > > **Example 6** > > Preparation of Rh.sub.2.sup.II,II (dfpma)3X4 (4 and 5) > > In a typical experiment, [XRh(cod)].sub.2 is treated with > three equiv of dfpma or dfpx in CH.sub.2 Cl.sub.2. Excess > oxidant is added in excess of 5 equiv (as either PhICl.sub.2 > or Br.sub.2), resulting in an exothermic reaction. The > reaction mixture is stirred for a few hours and the solvent > volume reduced to 3 mL. Pentane addition precipitates the > product as a yellow powder for X=Cl or orange-red powder for > X=Br in 90-95% yield after washing with pentane and drying in > vacuo. NMR spectroscopy can be used to fingerprint the > complexes: 1H NMR shows a multiplet at ca. 3.2 ppm for the > bridging dfpma ligands; the 19F NMR spectrum is complex, but > simplifies upon 31P decoupling to a five line pattern. See > Results and Discussion section. > > **Example 7** > > Preparation of Rh.sub.2 (dmpma).sub.2 Cl.sub.2 (.mu.-CO)(CO) > (6) > > An 8-mL THF solution of [ClRh(CO).sub.2 ].sub.2 (203 mg, > 0.522 mmol) was treated dropwise with dmpma (238 mg, 1.11 > mmol) dissolved in 2 mL of THF. The solution turned red with > gas evolution as ligand was added. The solution was stirred at > room temperature for 15 minutes, then a 10 mL aliquot of > hexanes was added. Cooling the solution to -35.degree. C. > overnight caused 338 mg (85% yield) of orange powder to be > deposited. Anal. Calcd for C1.sub.2 H.sub.3 0Cl.sub.2 N.sub.2 > O10P4Rh.sub.2 : C, 18.89; H, 3.96; N, 3.67. Found C, 19.01; H, > 3.67; N, 3.50. 1H NMR (300 MHz, C.sub.6 D.sub.6) .delta./ppm: > 2.51 (p, 3.6 Hz, 3H), 3.817 (dp, 60.0 Hz, 3.6 Hz, 12H). 31P > NMR (121.4 Hz, C.sub.6 D.sub.6) .delta./ppm: 132.81 > (.vertline.1JPRh+nJPRh.vertline.=142 Hz). IR (CHCl.sub.3) > .nu.CO/cm-1: 1989 (vs), 1808 (s). > > **Example 8** > > Preparation of Rh.sub.2 (dppma).sub.2 Cl.sub.2 (CO).sub.2 (7) > > An 8-mL THF solution of [ClRh(CO).sub.2 ].sub.2 (212 mg, > 0.545 mmol) and a 2-mL THF solution of dppma (508 mg, 1.10 > mmol) were frozen in a liquid N.sub.2 cold well. The solutions > were removed from cold well and the solution of the ligand was > added dropwise to the rapidly stirred solution of the rhodium > carbonyl dimer immediately after thawing. The solution turned > purple with gas evolution as ligand was added. After addition, > the purple solution was added to 150 mL of cold pentane, > prompting a fine purple powder to precipitate. The solid was > washed with cold pentane and dried in vacuo to yield 412 mg > (60% yield) of product. Anal. Calcd for C.sub.52 H.sub.46 > Cl.sub.2 N.sub.2 O.sub.10 P.sub.4 Rh.sub.2 : C, 49.59; H, > 3.68; N, 2.22. Found: C, 49.23; H, 3.72; N, 2.56. IR (KBr) > .nu.CO/cm-1: 2009 (vs). Recrystallization of this compound > results in isomerization to Rh.sub.2 (dppma).sub.2 Cl.sub.2 > (.mu.-CO).sub.2 in quantitative yield. 1H NMR (300 MHz, > C.sub.6 D.sub.6) .delta./ppm: 2.860 (t, 3.6 Hz, 3H), 6.8-7.5 > (m, 20H), 31P NMR (121.4 Hz, C.sub.6 D.sub.6) .delta./ppm: > 122.61 (.vertline.1JPRh+nJPRh.vertline.=170 Hz IR (KBr) > .nu.CO/cm-1: 1828 (vs). > > **Example 9** > > Preparation of [ClRh(dppma)].sub.2 (11) > > Rh.sub.2 (dppma).sub.2 Cl.sub.2 (CO).sub.2 (137 mg, 0.109 > mmol) was dissolved in 12 mL of benzene in a Schlenk tube. The > purple solution was heated to reflux under N.sub.2 prompting a > color change to orange. The solution was cooled to room > temperature and 10 mL of pentane was added to precipitate 92 > mg (70% yield) of yellow product. Anal. Calcd for C.sub.50 > H.sub.46 Cl.sub.2 N.sub.2 O.sub.8 P.sub.4 Rh.sub.2 : C, 49.90; > H, 3.85; N, 2.33. Found: C, 50.01; H, 3.84; N, 2.16. 1H NMR > (300 MHz, C.sub.6 D.sub.6) .delta./ppm: 2.394 (t, 12.0 Hz, > 3H), 6.82 (t, 7.5 Hz, 4 H), 6.96 (tt, 7.5 Hz, 2.1 Hz, 8), 7.43 > (d, 8.1 Hz, 8H). 31P NMR (121.4 Hz, C.sub.6 > D.sub.6).delta./ppm 91.13 (d, 280 Hz). > > **Example 10** > > Preparation of Rh.sub.2 (tfepma).sub.2 Cl.sub.2 (CO).sub.2 > (14) > > A scintillation vial containing [ClRh(CO).sub.2 ].sub.2 (99 > mg, 0.255 mmol) in 5 mL of CH.sub.2 Cl.sub.2 was treated with > tfepma (255 mg, 0.523 mmol) resulting in gas evolution and the > solution to turn dark red. The solution was stirred at room > temperature for 5 minutes after gas evolution ceased. The > volume was reduced to 1 mL by vacuum distillation and 10 mL of > pentane was added to cause an orange powder to precipitate. > The solid was collected by filtration and washed with > 4.times.2 mL of pentane. The yield of the bright orange-yellow > product was 206 mg (62% yield). Anal. Calcd for C.sub.20 > H.sub.22 Cl.sub.2 F.sub.24 N.sub.2 O.sub.10 P.sub.4 Rh.sub.2 : > C, 18.38; H, 1.70; N, 2.14. Found: C, 18.42; H, 1.65; N, 2.25. > 1H NMR (500 MHz, CDCl.sub.3) .delta./ppm: 2.94 (t, 3.5 Hz, > 3H), 4.45-4.77 (m, 8H). 31P NMR (202.5 Hz, CDCl3) .delta./ppm: > 131.16 (.vertline.1JPRh+nJPRh.vertline.=149 Hz). IR > (CHCl.sub.3) .nu.CO/cm-1: 2007 (vs), 1820 (m). > > **Example 11** > > Preparation of Rh.sub.2 (tfepma).sub.2 Cl.sub.2 > (.mu.-CO).sub.2 (15) > > A Schlenk tube was charged with [ClRh(CO).sub.2 ].sub.2 (92 > mg, 0.235 mmol) and tfepma (238 mg, 0.489 mmol) in 15 mL of > toluene. The orange solution was heated to reflux under > N.sub.2 overnight. Cooling to room temperature followed by the > addition of 30 mL of pentane caused 290 mg (95% yield) of a > salmon colored powder to precipitate. > > Anal. Calcd for C.sub.20 H.sub.22 Cl.sub.2 F.sub.24 N.sub.2 > O.sub.10 P.sub.4 Rh.sub.2 : C, 18.38; H, 1.70; N, 2.14Found: > C, 18.35; H, 1.43; N, 2.26. 1H NMR (500 MHz, C.sub.6 D.sub.6) > .delta./ppm: 2.52 (p, 4.0 Hz, 3H), 4.22 (dm, 83 Hz, 4H), 4.523 > (m, 4H). 31P NMR (121.4 Hz, C.sub.6 D.sub.6) .delta./ppm: > 128.40 (.vertline.1JPRh+nJPRh.vertline.=164 Hz). IR > (CHCl.sub.3) .nu.CO/cm-1: 1824 (vs). > > **Example 12** > > Preparation of Rh.sub.2 (tfepma).sub.3 Cl.sub.2 (CO) (16) > > An 8-mL THF solution of [ClRh(CO).sub.2 ].sub.2 (203 mg, > 0.522 mmol) was treated by the dropwise addition of with dmpma > (238 mg, 1.11 mmol) dissolved in 2 mL of THF. The solution > turned red with gas evolution as ligand was added. The > solution was stirred at room temperature for 15 minutes, then > a 10 mL aliquot of hexanes was added. The mixture was cooled > to -35.degree. C. overnight, depositing 338 mg (85% yield) of > orange powder. 1H and 31P NMR spectra indicate immediate > formation of [ClRh(tfepma)].sub.2 upon dissolution in > CDCl.sub.3. Anal. Calcd for C.sub.28 H.sub.33 Cl.sub.2 > F.sub.36 N.sub.3 O.sub.13 P.sub.6 Rh.sub.2 : C, 19.04; H, > 1.88; N, 2.38. Found: C, 19.14; H, 1.94; N, 2.09. IR (KBr) > .nu.CO cm-1: 2020 (vs). > > **Example 13** > > Preparation of [ClRh(tfepma)].sub.2 (17) > > Tfepma (200 mg, 0.410 mmol) was added to > BrRh(PPh.sub.3).sub.3 (151 mg, 0.156 mmol) in CH.sub.2 > Cl.sub.2 giving a bright yellow solution. The solution was > stirred for 6 hr then concentrated to 2 mL by vacuum > distillation. Pentane (6 mL) was added and the solution was > cooled to -35.degree. C.; yellow crystals (60 mg, 50% yield) > were deposited overnight. Anal. Calcd for C.sub.18 H.sub.22 > Cl.sub.2 F.sub.24 N.sub.2 O.sub.8 P.sub.4 Rh.sub.2 : C, 17.28; > H, 1.77; N, 2.24. Found: C 18.76; H, 1.92; N, 2.36. 1H NMR > (300 MHz, C.sub.6 D.sub.6) .delta./ppm: 1.99 (p, 5.7 Hz, 3H), > 4.34 (m, 4H), 4.64 (m, 4H). 31P NMR (202.5 Hz, C.sub.6 > D.sub.6) .delta./ppm: 109.9 (d, 179.6 Hz). > > **Example 14** > > Preparation of Rh.sub.2 (tfepma).sub.3 (CNtBU).sub.2 (18) > > A mixture of [ClRh(CO).sub.2 ].sub.2 (82.5 mg, 0.212 mmol), > tfepma (326 mg, 0.669 mmol), cobaltocene (88 mg, 0.466 mmol) > and tert-butylisonitrile (42 mg, 0.506 mmol) in Et.sub.2 O was > stirred at room temperature for 3 hr. Solid [CoCp.sub.2 ]Cl > was removed by filtration leaving an orange solution. The > solvent was stripped and the residue taken up in pentane. > Cooling to -35.degree. C. overnight afforded 349 mg (90% > yield) of an orange powder. 1H NMR (500 MHz, CDCl.sub.3) > .delta./ppm: 1.41 (s, 18H), 2.70 (s, 9H), 4.12 (dp, 51 Hz, 8 > Hz, 24H). 31P NMR (121.4 Hz, C.sub.6 H.sub.6) .delta./ppm: > 142.1 (.vertline.1JPRh+nJPRh.vertline.=216 Hz). > > **Example 15** > > Preparation of syn-Rh.sub.2 (tfepma).sub.3 Cl.sub.4 (19) > > A 10-mL CH.sub.2 Cl.sub.2 solution of [ClRh(CO).sub.2 ].sub.2 > (104 mg, 0.270 mmol) was treated successively with tfepma (393 > mg, 0.810 mmol) dissolved in 2 mL of CH.sub.2 Cl.sub.2 and > solid dichloroiodobenzene (182 mg, 0.660 mmol). The orange > solution was stirred at room temperature for 15 min, and then > concentrated to a few milliliters. Pentane addition prompted > precipitation of 260 mg (53% yield) of product as a yellow > powder. > > Anal. Calcd for C.sub.27 H.sub.33 Cl.sub.4 F.sub.36 N.sub.3 > O.sub.12 P.sub.6 Rh.sub.2 : C, 17.93; H, 1.84; N, 2.32Found: > C, 18.12; H, 1.95; N, 2.34. 1H NMR (500 MHz, CDCl.sub.3) > .delta./ppm: 2.89 (7, 7.7 Hz, 6H), 2.99 (t, 22 Hz, 3H), > 4.32-4.55 (m, 8H), 4.63 (m, 2H), 4.78 (m, 4H), 5.07 (m, 2H), > 5.15 (m, 4H), 5.41 (m, 2H), 5.58 (m, 2H). 31P NMR (202.5 Hz, > CDCl.sub.3) .delta./ppm: 105.62 (m), 109.79 (m). > > **Example 16** > > Preparation of anti-Rh.sub.2 (tfepma).sub.3 Cl4 (20) > > A Schlenk tube was charged with [ClRh(cod)].sub.2 (514 mg, > 1.04 mmol), tfepma (1.58 g, 3.24 mmol) and dichloroiodobenzene > (420 mg, 1.5 mmol) in 35 mL of toluene. The solution was > refluxed under N.sub.2 for 60 min to give a red solution. > Cooling to 0.degree. C. followed by pentane addition caused > 1.27 g (68% yield) of orange product to precipitate. The solid > was washed with pentane and dried. Anal. Calcd for C.sub.27 > H.sub.33 Cl.sub.4 F.sub.36 N.sub.3 O.sub.12 P.sub.6 Rh.sub.2 : > C, 17.93; H, 1.84; N, 2.32. Found: C, 18.09; H, 2.02; N, 2.14. > 1H NMR (500 MHz, CDCl.sub.3) .delta./ppm: 2.88 (m, 9H), 4.26 > (m, 2H), 4.30-4.52 (m, 8H) 4.61 (m, 4H), 4.80 (m, 2H), > 5.12-5.30 (m, 8H). 31P NMR (202.5 Hz, CDCl.sub.3) .delta./ppm: > 100.2 (m), 105.4 (m), 109.9.(m), 112.4 (m), 114.8 (m). > > **Example 17** > > Preparation of Rh.sub.2.sup.0,II (tfepma).sub.3 Cl.sub.2 (21) > > In the glove box, [ClRh(cod)].sub.2 (0.518 g, 1.05 mmol) and > tfepma (1.58 g, 3.24 mmol) were combined with 25 mL of > CH.sub.2 Cl.sub.2 in a 50 mL flask. The solution color > progressed from orange to green and finally red. The red > solution was set aside for two days, during which time a green > microcrystalline solid was deposited (680 mg, 37% yield). This > solid was collected and the mother liquor concentrated to 10 > mL. After several days a second crop of product was collected > (150 mg, 8% yield). > > **Example 18** > > Preparation of [ClRh(tfepx)].sub.2 (.mu.-tfepx) (33) > > Three equivalents of tfepx (740 mg, 1.28 mmol) was added to a > 10-mL CH.sub.2 Cl.sub.2 solution of [ClRh(cod)].sub.2 (203 mg, > 0.412 mmol). The solution color immediately changed from > yellow-orange to olive green. A bright yellow solid began to > precipitate after an hour, concentration of the solvent volume > to a few milliliters afforded 230 mg (48% yield) of product, > which was washed with pentane and dried. The 1H NMR spectrum > of analytically pure samples of 43 suggests the presence of > multiple species in solution, yet the 31P NMR shows only two > phosphorus resonances. 1H NMR (500 MHz, CD.sub.3 CN) > .delta./ppm: 2.21 (s), 2.23 (s), 2.29 (s), 4.69 (m), 4.79 (m), > 4.97 (m), 6.74 (s), 6.85 (s), 6.89 (s), 6.95 (s), 7.05 (s), > 7.23 (s), 7.86 (s). 31P NMR (121.5 Hz, CD.sub.3 CN) > .delta./ppm : 108.8 (d, 2JRhP=181 Hz), 111.1 (d, 2JRhP=252 > Hz). > > **Example 19** > > Preparation of Ir.sub.2 I,II(dfpma).sub.2 Cl4(cod) (31) > > A 20-mL scintillation vial containing 202 mg of > [ClIr(cod)].sub.2 (0.301 mmol) in 10 mL of CH.sub.2 Cl.sub.2 > was successively treated with 155 mg of dfpma (0.928 mmol) and > 455 mg of PhICl.sub.2 (1.66 mmol). The solution was stirred at > ambient, glove-box temperature for a few hours and then the > volume was reduced to .about.3 mL. Addition of a 10 mL aliquot > of pentane precipitated a sticky yellow-orange solid, which > was collected and repeatedly washed with pentane to afford 154 > mg of a yellow-orange powder (53% yield). 1H NMR (300 MHz, > C.sub.6 D.sub.6) .delta./ppm: 2.506 (td, 3.898 Hz, 0.600 Hz, > 3H), 3.55 (dp, 17.12 Hz, 4.4 Hz, 8H). 31P{1H} NMR (121.4 MHz, > C.sub.6 D.sub.6) .delta./ppm: 148.614 (s). 19F NMR (282 MHz, > C.sub.6 D.sub.6) .delta./ppm: -76.90 (m). > > **Example 20** > > Preparation of Ir.sub.2 I,III(dppma).sub.2 {MeN[P(OPh).sub.2 > ][P(OPh)(OC.sub.6 H4)]}HCl.sub.2 (32) > > In a glove box, 137 mg of [ClIr(cod)].sub.2 (0.204 mmol) and > 282 mg of dppma (0.608 mmol) were combined in 20 mL of benzene > in a three-neck round-bottomed flask. The flask was fitted > with a reflux condenser and nitrogen inlet, removed from the > box and heated to reflux for 12 h under a N.sub.2 atmosphere > provided by a Schlenk line. The solvent volume was reduced to > 5 mL by vacuum distillation and 15 mL of pentane was added to > precipitate a fluffy yellow solid, which was collected and > washed with 3.times.15 mL of pentane to yield 299 mg of > product (80% yield). Anal. Calcd For C.sub.75 H.sub.69 > Cl.sub.2 Ir.sub.2 N.sub.3 O.sub.12 P.sub.6 : C, 48.81; H, > 3.77; N, 2.28. Found: C, 48.61; H, 3.73; N, 2.42. 1H NMR (300 > MHz, CD.sub.3 CN) .delta./ppm: -17.08 (dtd, 213 Hz, 16.5 Hz, > 12.3 Hz, 1H), 2.1-3.2 (m, 9H), 6.0-7.9 (m, 59H). > > **Example 21** > > Preparation of Ir.sub.2.sup.0,II (tfepma).sub.3 Cl.sub.2 (33) > > In a nitrogen atmosphere, 734 mg (0.493 mmol) of dfpma was > added to a solution of 331 mg (0.493 mmol) of > [ClIr(cod)].sub.2 dissolved in 15 mL of CH.sub.2 Cl.sub.2. The > mixture was stirred at room temperature for 24 h during which > a dark precipitate formed. A green powder precipitated from > solution over several days. The solid was collected by > filtration, washed with 5 mL of benzene and three 5-mL > aliquots of pentane and then dried in vacuo to yield 590 mg > (62%) of the analytically pure product. Anal. Calcd for > C.sub.27 H.sub.33 Cl.sub.2 F.sub.36 Ir.sub.2 N.sub.3 O.sub.12 > P.sub.6 : C, 16.92; H, 1.74; N, 2.19; P, 9.70. Found. 17.06; > H, 1.65; N, 2.29; P, 9.63. 1H NMR (CD.sub.3 CN, 300 MHz) > .delta./ppm: 2.576 (t, 10.5 Hz, 3H), 2.763 (s, 6H), 4.0-5.5 > (m, 24H). 31P NMR (CD.sub.3 CN, 121 MHz) .delta./ppm: 32.710 > (s), 47.665 (dd, 299 Hz, 292 Hz), 64.702 (m), 70.509 (m), > 94.002 (m). > > Dark green crystals of 33 are obtained by dissolving > microcrystalline samples of the compound in a minimal amount > of MeCN, diluting the resulting solution with CH.sub.2 > Cl.sub.2, filtering and layering the filtrate with an alkane > solvent. Occasionally, a small crop of large yellow crystals > (34) would co-precipitate from solution. The 31P NMR spectra > of the green-brown crystals of 33 and the yellow crystals of 4 > dissolved in CD.sub.3 CN are identical; however, the 1H NMR > spectrum of 34 shows an additional peak at 1.963 ppm, > attributed to approximately one equivalent of uncoordinated > proteo MeCN. > > **Example 22** > > Reaction of 3 with Donor Ligands (35-L) > > For illustrative purposes, the preparation of > Ir.sub.2.sup.0,II (tfepma).sub.3 Cl.sub.2 (PEt.sub.3) > (35-PEt.sub.3) is described; the preparation of other L > derivatives follow similar methodology. In an N.sub.2 > atmosphere, PEt.sub.3 (19 mg, 0.160 mmol) was added to 33 (102 > mg, 0.053 mmol) suspended in 10 mL of CH.sub.2 Cl.sub.2 at > room temperature. The solution immediately turned yellow and > all solids dissolved. The solution was concentrated and 10 mL > of pentane was added. Cooling to -35.degree. C. overnight > caused a yellow microcrystalline solid to precipitate from > solution. Yield, 87 mg (81%). Anal. Calcd for C.sub.33 > H.sub.48 Cl.sub.2 F.sub.36 Ir.sub.2 N.sub.3 O.sub.12 P.sub.7 : > C, 19.22; H, 2.12; N, 2.80. Found: C, 19.58; H, 2.55; N, 2.12. > 1H NMR (CD.sub.3 CN, 300 MHz) .delta./ppm: 1.230 (dt, 13.2 Hz, > 7.6 Hz, 9H), 2.114 (dq, 7.4 Hz, 7.5 Hz, 6H), 2.559 (dd, 11.7 > Hz, 8.7 Hz, 3H), 2.648 (m, 6H), 4.040 (m, 2H), 4.29-4.87 (m, > 18H), 5.010 (m, 4 H). 31P NMR (CD.sub.3 CN, 121 MHz) > .delta./ppm: -18.189 (dd, 205 Hz, 18.8 Hz), 44.238 (t, 288 > Hz), 53.340 (d, 208 Hz), 65.967 (t, 71.4 Hz), 97.496 (dm, 291 > Hz). > > NMR data for Ir.sub.2.sup.0,II (tfepma).sub.3 Cl.sub.2 > (CNtBu) (5-CNtBu). 1H NMR (CD.sub.3 CN, 300 MHz) > .quadrature./ppm: 1.510 (s, 9H), 2.494 (dd, 12.3 Hz, 9.0 Hz, > 3H), 2.730 (dt, 9.0 Hz, 3.6 Hz, 6H), 4.15-4.95 (m, 24H). 31P > NMR (CD.sub.3 CN, 121 MHz) .quadrature./ppm: 46.056 (t, 290 > Hz), 52.509 (s), 72.530 (t, 75.4 Hz), 93.960 (dm, 290 Hz). > > NMR data for [Bu4N][Ir.sub.2.sup.0,II (tfepma).sub.3 Cl.sub.2 > (Br)] (5-Br--). 1H NMR (CD.sub.3 CN, 202.5 MHz) .delta./ppm: > 0.961 (t, 7.39 Hz, 12H), 1.352 (dq, 15.0 Hz, 7.38 Hz, 8H), > 1.604 (m, 8H), 3.109 (m, 9H), 4.2-6.0 (m, 24H). 31P{1H} NMR > (CD.sub.3 CN) .delta./ppm: 35.015 (s, 1P) 41.074 (t, 303 Hz, > 1P), 70.748 (t, 70.6 Hz, 2P), 98.240 (dm, 308 Hz, 2P). > > **Example 23** > > Halide Removal from 33 > > Thallium hexafluorophosphate (40 mg, 0.11 mmol) was added to > 33 (100 mg, 0.052 mmol) dissolved in 4 mL of MeCN. A rapid > color change was accompanied by the formation of a white > precipitate. The mixture was stirred at ambient temperature > for 3 h, then concentrated to 1 mL and filtered. The remaining > MeCN was removed and the residue washed with 10 mL of a 1:5 > mixture of CH.sub.2 Cl.sub.2 and pentane. Drying gave 102 mg > (87% yield) of 6 as a yellow powder that slowly turns reddish > under prolonged drying. 1H NMR (CD.sub.3 CN, 300 MHz) > .delta./ppm: 2.70 (t, 12 Hz, 3H), 2.83 (s, 6H), 4.1-4.7 (m, > 24H). 31P NMR (CD.sub.3 CN, 121.5 MHz) .delta./ppm: -143 > (sept, 730 Hz), 28 (s, 1P), 50 (t, 273 Hz, 1P), 57 (t, 60 Hz, > 2P), 89 (dm, 300 Hz, 2P) > > **Example 24** > > Preparation of Ir.sub.2 I,III (tfepma).sub.3 Cl4 (37) > > PhICl.sub.2 (20 mg, 0.073 mmol, 1.3 equiv) in 2 mL of > CH.sub.2 Cl.sub.2 was added to an 8-mL CH.sub.2 Cl.sub.2 > suspension of 33 (105 mg, 0.055 mmol, 1 equiv). As 33 reacts, > the suspension is brought into solution, which turns bright > yellow and a yellow solid subsequently forms; to ensure > complete reaction, stirring was continued at room temperature > for 2 h after the onset of precipitation. Addition of pentane > followed by filtration gave 54 mg (37% yield) of a bright > yellow powder. Single crystals of 37 were grown from saturated > solutions of the complex in CH.sub.2 Cl.sub.2, layered with > heptane. Anal. Calcd for C.sub.27 H.sub.33 Cl.sub.4 F.sub.36 > Ir.sub.2 N.sub.3 O.sub.12 P.sub.6 : C, 16.32; H, 1.67; N, > 2.11; P, 9.35. Found: C, 16.37: H, 1.78; N, 2.09; P, 9.40. 1H > NMR (CD.sub.3 CN) .delta./ppm: 2.71 (t, 8.40 Hz, 3H), 2.87 (t, > 9.38 Hz, 3H), 2.93 (t, 7.78 Hz, 3H), 4.3-4.6 (m, 6H), 4.7-5.1 > (m, 12H), 5.40 (ddqd 179.6 Hz, 12.14 Hz, 8.80 Hz, 2.93 Hz, > 2H), 5.91 (ddq, 151.1 Hz, 12.20 Hz, 8.81 Hz, 2H). 31P{1H} NMR > (CD.sub.3 CN) .delta./ppm: 9.24 (dt, 80.50 Hz, 25.86 Hz, 1P), > 13.14 (ddd, 900.7 Hz, 79.93 Hz, 31.16 Hz, 1P), 54.98 (dt, > 136.2 Hz, 29.08 Hz, 1P), 57.11 (dt, 125.6 Hz, 28.48 Hz, 1P), > 66.46 (dt, 124.5 Hz, 30.50 Hz, 1P), 74.31 (ddd, 900.8 Hz, > 136.6 Hz, 30.89 Hz, 1P). > > **Example 25** > > Preparation of Ir.sub.2.sup.II,II (tfepma).sub.2 Cl.sub.4 > (MeCN).sub.2 (38 > > A solution of 33 (150 mg, 0.078 mmol, 1 equiv) and > PhICl.sub.2 (150 mg, 0.50 mmol, 6 equiv of Cl.sub.2) in 10 mL > CH.sub.3 CN was heated to reflux for 48 h. The solvent was > removed under reduced pressure and the residue was taken up in > 5 mL of CH.sub.2 Cl.sub.2. The solution was filtered and then > concentrated to 2 mL by vacuum distillation. Addition of a > 10-mL aliquot of pentane caused 100 mg (81% yield) of 38 to > precipitate as a yellow powder, which was collected and dried > in vacuo. Layering saturated CH.sub.2 Cl.sub.2 solutions of > the complex with heptane gave single crystals of 8. Anal. > Calcd for C.sub.22 H.sub.28 Cl.sub.4 F.sub.24 Ir.sub.2 N.sub.4 > O.sub.8 P.sub.4 : C, 16.70; H, 1.78; N, 3.54. Found: C, 16.58: > H, 1.88; N, 3.52. 1H NMR (CD.sub.3 CN) .delta./ppm: 2.80 (t, > 8.13 Hz, 6H), 4.48 (q, 2.93 Hz, 4H), 4.6-4.8 (m, 4H), > 4.95-5.15 (m, 6H), 5.46 (dqd, 12.31 Hz, 8.93 Hz, 3.62 Hz, 2H). > 31P{1H} NMR .delta./ppm: 54.97 (dd, 121.4 Hz, 42.41 Hz, 2P), > 57.87 (dd, 121.4 Hz, 41.64 Hz, 2P). > > **Example 26** > > Reaction of 33 with HCl > > A suspension of 33 (120 mg, 0.063 mmol) in 10 mL of CH.sub.2 > Cl.sub.2 was purged with HCl gas. Within 5 min, all solid had > dissolved to give a yellow solution. Immediate solvent removal > gave 131 mg (97% yield) of 39 with an empirical formula > Ir.sub.2 (tfepma).sub.3 HCl.sub.3. Anal. Calcd. for C.sub.27 > H.sub.34 Cl.sub.3 F.sub.36 Ir.sub.2 N.sub.3 O.sub.12 P.sub.6 : > C, 16.60; H, 1.75; N, 2.15; P, 9.52. Found: C,16.57: H, 1.84; > N, 2.08; P, 9.68. 1H NMR (CD.sub.3 CN) .delta./ppm: -12.985 > (m, 1H), 2.757 (t, 11.2 Hz, 3H), 2.916 (s, 6H), 4.0-5.9 (m, > 24H). 31P{1H} NMR (CD.sub.3 CN) .delta./ppm: 35.712 (ddd, 795 > Hz, 44 Hz, 18.9 Hz, 1P), 47.878 (dd, 752 Hz, 49 Hz, 1P), > 63.794 (dd, 147 Hz, 34 Hz, 1P), 66.339 (dd, 146 Hz, 35 Hz, > 1P), 80.880 (ddd 795 Hz, 146 Hz, 54 Hz, 29 Hz, 1P), 88.657 > (dddd, 751 Hz, 147 Hz, 44 Hz, 29 Hz, 1P). IR (KBr) > .nu.Ir--H/cm-1: 203 > > When solvent was not immediately removed, and the solution > was stirred for 24 h at room temperature, a very pale yellow > solid precipitated from solution. NMR analysis of this solid > in CD.sub.3 CN revealed the formation of an isomer of Ir.sub.2 > (tfepma).sub.3 HCl.sub.3, 40, in 68% isolated yield. The > preparation of 10 on a larger scale proceeds smoothly by > treating a suspension of 33 (1.153 g, 0.6016 mmol) in 150 mL > of CH.sub.2 Cl.sub.2 with HCl gas for 10 min. The flask > headspace was purged with N.sub.2 and the solution was stirred > for 24 h. The volume of the mixture was reduced to ca. 40 mL > by distillation under reduced pressure. Addition of 60 mL of > pentane facilitated the precipitation of 640 mg (54%) of > analytically pure 40, which was washed with pentane and dried > in vacuo. Single crystals of this complex are readily obtained > by layering a CH.sub.2 Cl.sub.2 solution of 40 with heptane. > Anal. Calcd. for C.sub.27 H.sub.34 Cl.sub.3 F.sub.36 1r.sub.2 > N.sub.3 O.sub.12 P.sub.6 : C, 16.60; H, 1.75; N, 2.15; P, > 9.52. Found: C, 16.47: H, 1.74; N, 2.15; P, 9.58. 1H NMR > (CD.sub.3 CN) .delta./ppm: -10.261 (ddt, 178 Hz, 18.2 Hz, 12.2 > Hz, 1H), 2.65 (t, 10.84 Hz, 3H), 2.77 (t, 7.49 Hz, 3H), 2.89 > (t, 7.74 Hz, 3H), 4.1-5.1 (m, 21H), 5.3-5.5 (m, 1H), 5.7-6.1 > (m, 2H). 31P{1H} NMR (CD.sub.3 CN) .delta./ppm: 21.64 (tp, > 34.17 Hz, 21.68 Hz, 1P), 26.61 (dtd, 761.5 Hz, 33.05 Hz, 10.27 > Hz, 1P), 64.38 (dddd, 130.6 Hz, 35.66 Hz, 21.52 Hz, 10.06 Hz, > 1P), 67.79 (ddd, 162.2 Hz, 36.45 Hz, 19.99 Hz, 1P), 82.15 > (dddd, 760.1 Hz, 130.8 Hz, 22.02 Hz, 13.08 Hz, 1P), 86.40 (dm, > 162.6 Hz, 1P). IR (KBr) .nu.Ir--H/cm-1: 2115. > > **Example 27** > > Reaction of 33 with Triflic Acid > > An NMR tube was charged with 33 (74 mg, 0.039 mmol, 1 equiv) > in 0.7 mL of CD.sub.3 CN. The solution was treated with 34 > .mu.L of HOTf (OTf =OSO.sub.2 CF.sub.3) (0.39 mmol of HOTf, 10 > equiv), delivered via auto pipette. Upon mixing, the solution > turned pale yellow. [HIr.sub.2 (tfepma).sub.3 Cl.sub.2 > (MeCN)]OTf (41) was obtained quantitatively. Alternatively, > treatment of a suspension of 33 (192 mg, 0.100 mmol, 1 equiv) > in 9 mL of CH.sub.2 Cl.sub.2 with HOTf (20 mg, 0.13 mmol, 1.3 > equiv) in 1 mL of MeCN caused all solid to dissolve, giving a > very pale yellow solution. Precipitation of an eggshell solid > was aided by the addition of 10 mL of pentane, affording 163 > mg (77%) of 41. 1H NMR (CD.sub.3 CN) .delta./ppm: -12.669 (m, > 1H), 1.964 (s, see text), 2.586 (d, 1 Hz, see text), 2.728 (t, > 11.5 Hz, 3H), 2.865 (dd, 8.84 Hz, 7.53 Hz, 3H), 3.092 (t, 7.86 > Hz, 3H), 4.1-5.3 (m, 24H) 31P{1H} NMR (CD.sub.3 CN) > .delta./ppm: 43.007 (dd, 744 Hz, 35.3 Hz, 1P), 48.383 (ddt, > 716 Hz, 45.6 Hz, 17.9 Hz, 1P), 53.628 (dd, 147 Hz, 38.0 Hz, > 1P), 66.898 (dd, 150 Hz, 39.3 Hz, 1P), 75.931 (ddt, 739 Hz, > 148 Hz, 39.7 Hz, 1P), 84.947 (ddt, 722 Hz, 146 Hz, 34.9 Hz > 1P). IR (Fluorolube) .nu.Ir--H/cm-1: 2042. > > **Example 28** > > Addition of H.sub.2 to 33 > > Dihydrogen was bubbled slowly into a 10-mL CH.sub.2 Cl.sub.2 > suspension of 33 (76 mg, 0.040 mmol). The solid dissolved > immediately to give a yellow solution, which returned to brown > with concomitant formation of solid upon purging with N.sub.2. > Treating with H.sub.2 regenerated the yellow solution. The > solution could be cycled reversibly between yellow and brown > with treatment of H.sub.2 and N.sub.2, respectively. The > reaction proceeds with equal facility in CD.sub.3 CN. > Integration of the 1H NMR spectra obtained on solutions before > and after H.sub.2 addition indicates a quantitative reaction. > A pale yellow solid is isolated when CH.sub.2 Cl.sub.2 > solutions were concentrated under a stream of H.sub.2 to a few > mL, followed by pentane addition and cooling to -80.degree. C. > Meaningful yields and elemental analyses of the compound could > not be determined because the complex loses H.sub.2 in an > atmosphere devoid of dihydrogen. The reaction is so prevalent > that it occurs even in the solid state thus requiring us to > grow X-ray quality single crystals of the complex from a > CH.sub.2 Cl.sub.2 solution of 12 layered with octane under a > dihydrogen atmosphere. 1H NMR (CD.sub.3 CN) .delta./ppm: > -11.626 (dq, 188 Hz, 16.0 Hz, 1H), -8.174 (d, 278 Hz, 1H), > 2.81 (t, 6.72 Hz, 3H), 2.82 (t, 7.37 Hz, 6H), 4.2-5.7 (m, > 24H). 31P{1H} NMR (CD.sub.3 CN) .delta./ppm: 17.85 (s, 1P), > 45.26 (d, 746 Hz, 1P), 71.34 (d, 159 Hz, 1P), 86.84 (d, 155 > Hz, 1P), 95.50 (dd, 752 Hz, 218 Hz, 1P), 99.40 (d, 222 Hz, > 1P). IR (KBr) .nu.Ir--H/cm-1: 2053, 2071. > > **Example 29** > > Thermolysis of 42 > > An NMR tube equipped with a Teflon valve was charged with 20 > mg of 33 (0.01 mmol). d8-THF was distilled in under vacuum and > the tube was pressurized with H.sub.2 to 1 atm at 20.degree. > C. After acquiring an initial 1H NMR spectrum, the solution > was heated overnight to 80.degree. C. After cooling to room > temperature, 1H NMR revealed the formation of equal quantities > of 43a and 43b, accounting for 90% of the starting iridium > complex. 1H NMR (d8-THF, 500 MHz) .delta./ppm: -14.07 (q, 12 > Hz, 1H), -13.71 (dm, 181 Hz, 1H), -12.63 (dt, 177 Hz, 18 Hz, > 1H)-11.23 (dq, 184 Hz, 16 Hz, 1H), 2.7-3.1 (m, 9H), 3.82 (dq, > 28 Hz, 5 Hz, 2H), 4.2-5.9 (m, 24H). 31P{I H} NMR (d8-THF, > 202.5 MHz .delta./ppm: 41.73 (d, 692 Hz), 59.00 (s), 63.65 > (dd, 118 Hz, 30 Hz), 67.04 (ddd, 167 Hz, 38 Hz, 14 Hz), 70.28 > (dt, 162 Hz, 32 Hz), 72.54 (dt, 132 Hz, 35 Hz), 82.44 (dt, 117 > Hz, 30 Hz), 84.15 (dq, 142 Hz, 35 Hz), 85.77 (dm, 117 Hz), > 90.34 (d, 165 Hz), 94.60 (d, 130 Hz), 99.90 (dd, 698 Hz, 130 > Hz). > > **Example 30** > > Preparation of Ir.sub.2.sup.0,II (tfepma).sub.3 (Me)Cl(MeCN) > (44) > > An 8-mL THF solution of 33 (117 mg, 0.061 mmol) and a 2-mL > THF solution containing 21 .mu.L of 3.0 M MeMgBr (0.063 mmol) > were frozen in the liquid nitrogen cold well of a glove box. > The solutions were removed from the cold well and mixed > immediately upon thawing prompting a color change from dark > brown to yellow. As the yellow solution warmed to room > temperature the color darkened to brown. After 1 h, the > solvent was stripped and the residue triturated three times > and washed once with CH.sub.2 Cl.sub.2 before drying to yield > the product as a green powder. 1H NMR (CD.sub.3 CN) > .delta./ppm: 1.11 (dd, 8 Hz, 3 Hz, 3H), 2.61 (t, 6 Hz, 3H), > 2.70 (m, 3H), 2.80 (m, 3 H), 4.1-5.4 (m, 24H). 31P NMR > (CD.sub.3 CN) .delta./ppm: 29.5 (s, 1P), 44.8 (t, 303 Hz, 1P), > 72.5 ( 134 Hz, 1P), 93.8 (dm, 298 Hz, 1P), 95.5 (dm, 310 Hz, > 1P), 109.3 (dm, 152 Hz, 1P). > > **Example 31** > > Rh.sub.2.sup.0,II (dfpma).sub.3 Cl.sub.2 (PPh.sub.3) > photochemistry in d8-THF > > An NMR tube with a resealable Teflon valve was charged with > 15 mg of Rh.sub.2.sup.0,II (dfpma).sub.3 Cl.sub.2 (PPh.sub.3) > (0.014 mmol) in the glove box. The NMR tube was brought out of > the glove box and connected to the vacuum line. d8-THF (ca. > 0.7 mL) was distilled into the NMR tube. HCl was generated > from the reaction of H.sub.2 SO4 with NaCl and collected in a > 25 mL flask, then freeze-pump-thaw degassed once. The pressure > was adjusted to 129 mm of Hg (0.18 mmol HCl), and the HCl was > transferred into the NMR tube. The solution was thawed and an > initial 1H NMR spectrum recorded. Irradiation was carried out > at 20.degree. C. with .lambda..gtoreq.338 nm excitation light, > after three hours, irradiation was halted and another NMR > spectrum was recorded. A singlet at 4.53 ppm signaled the > formation of H.sub.2. Irradiation was continued for a total of > 18 h after which a final 1H NMR spectrum was recorded. An > increased intensity for the H.sub.2 resonance was accompanied > by a 1:1:1 triplet at 4.50 ppm (1JHD 43 Hz) for HD gas. All > non-condensable gas was collected by Toepler pumping. Hydrogen > formation (0.096 mmol) was confirmed by complete combustion > over hot CuO. > > **Example 32** > > Reaction of dfpma with HRh(PPh.sub.3)4 > > A 100-mL flask was charged with 190 mg (0.165 mmol) of > HRh(PPh.sub.3).sub.4 in the glove box and fitted with a Teflon > valve. The vessel was removed from the glove box, attached to > a vacuum line and evacuated. Benzene (20 mL), stored under > vacuum over Na/benzophenone-ketyl, was then condensed into the > reaction flask. Due to its high volatility, dfpma was added to > the flask by standard gas transfer techniques. A flask with a > nominal volume of 36 mL was filled with dfpma to a pressure of > 134 mm of Hg (0.27 mmol dfpma). The ligand was > freeze-pump-thaw degassed once prior to its condensation into > the reaction flask containing the frozen benzene solution. > Thawing of the solution prompted immediate reaction as > evidenced by a slight color change and gas evolution. After > stirring overnight, a bright orange solid precipitated from > solution. The solvent was frozen and 0.059 mmol of hydrogen > was collected via Toepler pumping (72% yield based on rhodium > starting material). The reaction solution was then thawed and > brought into the glove box. After reducing the solvent volume > to .about.10 mL, a 10 mL-aliquot of pentane was added. The > orange solid was collected by filtration and washed with > 3.times.5 mL of pentane to yield 86 mg (85%) of dirhodium > product. The 1H and 19F NMR data for the product match the > data presented for Rh.sub.2 0,0(dfpma).sub.3 (PPh.sub.3).sub.2 > (3-PPh.sub.3) in Table 1.3. > > **Example 33** > > Preparation of Rh.sub.2.sup.0,II (dfpma).sub.3 Cl.sub.2 (CO) > and Rh.sub.2.sup.0,II (dfpma).sub.3 Cl.sub.2 > > A 20-mL scintillation vial was charged with 255 mg (0.656 > mmol) of [ClRh(CO).sub.2 ].sub.2 and 10 mL of CH.sub.2 > Cl.sub.2. Dfpma was then added dropwise (336 mg, 2.01 mmol) > under rapid stirring, prompting gas evolution and a concurrent > color change from orange to dark blue and finally deep red. > The solvent was removed to afford a sticky red solid that was > treated with 5 mL of benzene and 10 mL of pentane to give 400 > mg of orange powder analyzing as Rh.sub.2.sup.0,II > (dfpma).sub.3 Cl.sub.2 (CO) (76%). This product was > characterized by a strong carbonyl stretch in the IR at 2057 > cm-1. A portion of this material was exposed to high vacuum > (10-5 torr) for several days resulting in a color change to > green. The infrared spectrum of a KBr pellet showed no > absorption corresponding to a carbonyl ligand. For > Rh.sub.2.sup.0,II (dfpma).sub.3 Cl.sub.2 : 1H NMR (d8-THF) > .delta./ppm: 3.05 (m). 19F NMR (d8-THF) .delta./ppm: -15.4 (d, > 1186 Hz), -38.2 (d 1180, Hz), -42.4 (d, 1271 Hz), -49.5 (d, > 1101 Hz), -53.8 (d, 1073 Hz), -80.8 (d, 1158 Hz). > > **Example 34** > > Preparation of Rh.sub.2 0,0(dfpma).sub.3 (CO)(PPh.sub.3) > > In the glove box, Rh.sub.2.sup.0,II (dfpma)3Cl.sub.2 (CO) > (185 mg, 0.230 mmol) was dissolved in 8 mL of THF and treated > successively with cobaltocene (91 mg, 0.48 mmol) and > triphenylphosphine (63 mg, 0.24 mmol). The solution turned red > with concomitant precipitation of yellow [CoCp.sub.2 ]Cl. The > mixture was filtered and the solvent removed. The residue was > re-dissolved in CH.sub.2 Cl.sub.2 and filtered through a plug > of Florisil. The volume was reduced to 5 mL and pentane was > added. Cooling to -80.degree. C. overnight afforded 189 mg of > the product as a yellow-orange microcrystalline solid (83% > yield). 1H NMR (CDCl.sub.3) .delta./ppm: 2.74 (s, 9H), 7.36 > (m, 15H). 19F NMR (CDCl.sub.3) .delta./ppm: -41.75 (d, 1125 > Hz, 6F), -43.56 (d, 1115 Hz, 6F). > > **Example 35** > > Addition of [PPN]Cl to Rh.sub.2.sup.0,II (dfpma).sub.3 > Cl.sub.2 > > Dissolution of Rh.sub.2.sup.0,II (dfpma).sub.3 Cl.sub.2 (295 > mg, 0.379 mmol) in 10 mL of THF afforded a deep red solution. > Solid bis(triphenylphosphine)iminium chloride ([PPN]Cl) was > then sifted into the solution prompting a color change to > orange. The solution volume was reduced to 3 mL and ether was > added to precipitate the product as an orange microcrystalline > solid in 70% yield (360 mg). 1H NMR (d8-THF) .delta./ppm: 2.79 > (t, 3 Hz, 3H), 2.86 (s, 6H), 7.48-7.70 (m, 30H). .sup.19 F NMR > (d8-THF) .delta./ppm: 7.36 (d, 1260 Hz, 2F), -43.93 (d, 1084 > Hz, 2F), -46.75 (d, 1109 Hz, 2F), -52.64 (d, 1160 Hz, 2F), > -54.69 (d, 1109 Hz, 2F), -80.90 (d, 1135 Hz, 2F). > > **Example 36** > > Oxidation of Rh.sub.2.sup.0,II (dfpma).sub.3 Cl.sub.2 with > Br.sub.2 > > A dark red THF solution of Rh.sub.2.sup.0,II (dfpma).sub.3 > Cl.sub.2 (97 mg, 0.125 mmol) was reacted with 12 .mu.L (37 mg, > 0.23 mmol) of bromine delivered with an auto pipette. The > solution immediately turned transparent red. The solvent was > removed by vacuum distillation and the resulting residue was > taken up in a minimal volume of CH.sub.2 Cl.sub.2. Pentane > addition caused the precipitation of 80 mg of the product as a > bright orange-red powder (68% yield). 1H NMR (d8-THF) > .delta./ppm: 3.38 (m). 19F NMR (d8-THF) .delta./ppm: -47.5 (d, > 930 Hz), -49.9 (d, 1186 Hz), -50.6 (d, 1214 Hz), -51.3 (d, > 1017 Hz), -62.6 (d, 1101 Hz), -63.9 (d, 1186 Hz), -76.4 (d, > 1214 Hz), -77.8 (d, 1130 Hz). > > **Example 37** > > Rh.sub.2.sup.II,II (dfpma).sub.3 Br4 and Rh.sub.2.sup.0,II > (dfpma).sub.3 Br.sub.2 (.eta.1-dfpma) Dark Reactions > > The thermal reactivity of Rh.sub.2.sup.II,II (dfpma).sub.3 > Br4 and Rh.sub.2.sup.0,II (dfpma).sub.3 Br.sub.2 > (.eta.1-dfpma) in THF was evaluated under the conditions > employed for photochemical experiments. Thus, a cuvette of a > photolysis cell was charged with either a small amount of the > Rh.sub.2.sup.II,II or Rh.sub.2.sup.0,II complex. THF was > distilled into the solvent reservoir of the cell under vacuum > and subjected to three freeze-pump-thaw cycles. The solvent > was then mixed with the rhodium complex under photographic > darkroom lights and an initial absorption spectrum was > recorded. The cell was wrapped in foil and maintained at > 0.degree. C. overnight. After twelve hours, another UV-Vis > spectrum of the sample showed only negligible changes in the > absorption profile. > > **Example 38** > > Identification of the Rh.sub.2 0,0 Product from > Rh.sub.2.sup.II,II (dfpma).sub.3 Br4 Photochemistry > > A 200-mL quartz photolysis tube was charged with 45 mg > (44,mol) of Rh.sub.2.sup.II,II (dfpma).sub.3 Br4 in 20 mL of > THF under nitrogen. The solution was degassed by three > freeze-pump-thaw cycles and 0.178 mmol of dfpma was added to > the cell by vacuum distillation. The solution was irradiated > at 0.degree. C. with 395-nm longpass filtered light for 46 h. > After solvent removal, the residue was extracted with pentane > and removing solvent in vacuo to afford the orange > photoproduct. 19F NMR (C.sub.6 D.sub.6), .delta./ppm: -29.72 > (d, 1252 Hz, 4F), -40.96 (d, 1117 Hz, 12F), -76.29 (d, 1252 > Hz, 4F). > > **Example 39** > > Identification of the Bromine Product from Rh.sub.2 -dfpma > Photochemistry > > In the environment of a nitrogen-filled glove box, 21 mg (20 > .mu.mol) of Rh.sub.2.sup.II,II (dfpma).sub.3 Br4 was dissolved > in 150 mL of THF contained within a quartz photolysis tube. > The solution was cooled to -78.degree. C. and 13 mg (50 > .mu.mol) of triphenylphosphine was added, followed by the > addition of 10 .mu.l (9.2 mg, 86 .mu.mol) of 2,6-lutidine. The > sealed tube was removed from the glove box and the solution > was irradiated at .lambda..gtoreq.335 nm for 17 h at 0.degree. > C. Solvent was distilled from the photolyzed solution and the > entire residue was dissolved in CDCl.sub.3. 1H NMR > (CDCl.sub.3), .delta./ppm: 2.60 (bs, 0.96H), 2.70 (bs, 0.27H), > 2.83 (bs, 0.59H), 2.91 (bs, 1.18H), 3.23 (s, 0.09H), 16.77 > (bs, 3.00H). ---