Transition metal dioxygen complex

Dioxygen complexes are coordination compounds that contain O₂ as a ligand.^[1] The study of these compounds is inspired by oxygen-carrying proteins such as myoglobin, hemoglobin, hemerythrin, and hemocyanin.^[2] Several transition metals form complexes with O₂, and many of these complexes form reversibly.^[3] The binding of O₂ is the first step in many important phenomena, such as cellular respiration, corrosion, and industrial chemistry. The first synthetic oxygen complex was demonstrated in 1938 with cobalt(II) complex reversibly bound O₂.^[4]

Mononuclear complexes of O₂

O₂ binds to a single metal center either “end-on” (η¹-) or “side-on” (η²-). The bonding and structures of these compounds are usually evaluated by single-crystal X-ray crystallography, focusing both on the overall geometry as well as the O---O distances, which reveals its bond order.

Complexes of η¹-O₂ ligands

O₂ adducts derived from cobalt(II) and iron(II) porphyrin complexes and related anionic ligands exhibit this bonding mode. Myoglobin and hemoglobin are famous examples, and many synthetic analogues have been described that behave similarly. Binding of O₂ is usually described as proceeding via electron transfer from the metal(II) center to give superoxide (O₂^-) complexes of metal(III) centers.

Complexes of η²-O₂ ligands

η²- bonding is the most common motif seen in coordination chemistry of dioxygen. Such complexes can generated by treating low-valent metal complexes with gaseous oxygen. For example, Vaska's complex reversibly binds O₂ (Ph = C₆H₅):

IrCl(CO)(PPh₃)₂ + O₂ $\overrightarrow{\leftarrow}$ IrCl(CO)(PPh₃)₂O₂

The conversion is described as a 2 e^- redox process: Ir(I) converts to Ir(III) as dioxygen converts to peroxide. Since O₂ has a triplet ground state and Vaska's complex is a singlet, the reaction is slower than when singlet oxygen is used.^[5]

Complexes containing η²-O₂ ligands are fairly common, but most are generated using hydrogen peroxide, not O₂. Chromate ([CrO₄)]^2-) can for example be converted to the tetraperoxide [Cr(O₂)₄]^2-. The reaction of hydrogen peroxide with aqueous titanium(IV) gives a brightly colored peroxy complex that is a useful test for titanium as well as hydrogen peroxide.^[6]

Binuclear complexes of O₂

O₂ can bind to one metal of a bimetallic unit via the same modes discussed above for mononuclear complexes. A well known example in nature is hemerythrin, which features a diiron carboxylate that binds O₂ at one Fe center. Dinuclear complexes can also cooperate in the binding, although the initial attack of O₂ probably occurs at a single metal. These binding modes include μ₂-η²,η²-, μ₂-η¹,η¹-, and μ₂-η¹,η²-. Depending on the degree of electron-transfer from the dimetal unit, these O₂ ligands can again be described as peroxo or superoxo. In nature, such dinuclear dioxygen complexes often feature copper.^[7]

Relationship to other oxygenic ligands and applications

Dioxygen complexes are the precursors to other families of oxygenic ligands. Metal oxo compounds arise from the cleavage of the O-O bond after complexation. Hydroperoxo complexes are generated in the course of the reduction of dioxygen by metals. The reduction of O₂ by metal catalysts is a key half-reaction in fuel cells.

Metal-catalyzed oxidations with O₂ proceed via the intermediacy of dioxygen complexes, although the actual oxidants are often oxo derivatives. The reversible binding of O₂ to metal complexes has been used as a means to purify oxygen from air, but cryogenic distillation of liquid air remains the dominant technology.

References

1. ^ Holleman, A. F.; Wiberg, E. "Inorganic Chemistry" Academic Press: San Diego, 2001. ISBN 0-12-352651-5.
2. ^ S. J. Lippard, J. M. Berg “Principles of Bioinorganic Chemistry” University Science Books: Mill Valley, CA; 1994. ISBN 0-935702-73-3.
3. ^ Berry, R. E. "Reactivity and Structure of Complexes of Small Molecules: Dioxygen", Comprehensive Coordination Chemistry II, 2004, 1, 625-629.
4. ^ Tokuichi Tsumaki (1938). "Nebenvalenzringverbindungen. IV. Über einige innerkomplexe Kobaltsalze der Oxyaldimine". Bulletin of the Chemical Society of Japan 13: 252–260. doi:10.1246/bcsj.13.252. 
5. ^ Selke, M. and Foote, C. S., "Reactions of Organometallic Complexes with Singlet Oxygen. Photooxidation of Vaska's Complex", J. Am. Chem. Soc., 1993, volume 115, pages 1166 - 1167.doi:10.1021/ja00056a061
6. ^ Greenwood, N. N.; & Earnshaw, A. (1997). Chemistry of the Elements (2nd Edn.), Oxford:Butterworth-Heinemann. ISBN 0-7506-3365-4.
7. ^ Lewis, E. A. and Tolman, W. B., "Reactivity of Dioxygen-Copper Systems", Chemical Reviews 2004, 104, 1047-1076. doi:10.1021/cr020633r.