Transition metal dioxygen complex

'''Dioxygen complexes''' are coordination compounds that contain O₂ as a ligand.<ref>{{cite book|first1=Gereon M.|last1=Yee |first2=William B. |last2=Tolman |editor1-first=Peter M. H. |editor1-last=Kroneck |editor2-first=Martha E. |editor2-last=Sosa Torres|title=Sustaining Life on Planet Earth: Metalloenzymes Mastering Dioxygen and Other Chewy Gases|series=Metal Ions in Life Sciences|volume=15|year=2015|publisher=Springer|chapter=Chapter 5: Transition Metal Complexes and the Activation of Dioxygen|pages=131–204|doi=10.1007/978-3-319-12415-5_5|pmid=25707468|isbn=978-3-319-12414-8 }}</ref><ref>{{cite book|last1=Holleman|first1= A. F. |last2=Wiberg |first2=E. |title=Inorganic Chemistry |publisher=Academic Press |location=San Diego, CA|date=2001 |isbn=0-12-352651-5}}</ref> The study of these compounds is inspired by oxygen-carrying proteins such as myoglobin, hemoglobin, hemerythrin, and hemocyanin.<ref>{{cite book|first1=S. J. |last1=Lippard |first2=J. M. |last2=Berg |title=Principles of Bioinorganic Chemistry |publisher=University Science Books|location= Mill Valley, CA|date= 1994| isbn=0-935702-73-3}}</ref> Several transition metals form complexes with O₂, and many of these complexes form reversibly.<ref>{{cite encyclopedia|last=Berry|first= R. E. |encyclopedia= Comprehensive Coordination Chemistry II|date= 2004|volume= 1|pages= 625–629|isbn=978-0-08-043748-4|doi=10.1016/B0-08-043748-6/01161-0|chapter= Reactivity and Structure of Complexes of Small Molecules: Dioxygen}}</ref> 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.<ref>{{cite journal | first= Tokuichi |last=Tsumaki | title = Nebenvalenzringverbindungen. IV. Über einige innerkomplexe Kobaltsalze der Oxyaldimine|trans-title=Secondary valence ring compounds. IV. On some inner-complex cobalt salts of oxyaldimine | journal = Bulletin of the Chemical Society of Japan | year = 1938 | volume = 13 |issue=2 | pages = 252–260 | doi = 10.1246/bcsj.13.252| doi-access = free}}</ref>

==Mononuclear complexes of O₂== O₂ binds to a single metal center either "end-on" (''η''¹-) or "side-on" (''η''²-). 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 the bond order of the O₂ ligand. :220px

===Complexes of ''η''¹-O₂ ligands=== [[image:PicketFenceGenericRevised.png|thumb|right|220px|A picket-fence porphyrin complex of Fe, with axial coordination sites occupied by methylimidazole (green) and dioxygen (R = amide groups).<ref>S. J. Lippard, J. M. Berg "Principles of Bioinorganic Chemistry" University Science Books: Mill Valley, California; 1994. {{ISBN|0-935702-73-3}}.</ref>]] O₂ adducts derived from cobalt(II) and iron(II) complexes of porphyrin (and related anionic macrocyclic 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 by electron transfer from the metal(II) center to give superoxide ({{chem|O|2|−}}) complexes of metal(III) centers. As shown by the mechanisms of cytochrome P450 and alpha-ketoglutarate-dependent hydroxylase, Fe-''η''¹-O₂ bonding is conducive to formation of Fe(IV) oxo centers. O₂ can bind to one metal of a bimetallic unit via the same modes discussed above for mononuclear complexes. A well-known example is the active site of the protein 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.

===Complexes of ''η''²-O₂ ligands=== ''η''²-bonding is the most common motif seen in coordination chemistry of dioxygen. Such complexes can be generated by treating low-valent metal complexes with oxygen. For example, Vaska's complex reversibly binds O₂ (Ph = C₆H₅): :IrCl(CO)(PPh₃)₂ + O₂ {{eqm}} IrCl(CO)(PPh₃)₂O₂ The conversion is described as a 2&nbsp;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.<ref>{{cite journal|last1=Selke|first1= M. |last2=Foote|first2= C. S.|title=Reactions of Organometallic Complexes with Singlet Oxygen. Photooxidation of Vaska's Complex|journal= J. Am. Chem. Soc.|date= 1993| volume=115 |issue= 3 |pages=1166–1167|doi=10.1021/ja00056a061 |bibcode= 1993JAChS.115.1166S }}</ref> The magnetic properties of some ''η''²-O₂ complexes show that the ligand, in fact, is superoxide, not peroxide.<ref>{{cite journal |doi=10.1021/ja00162a069|title=Crystal structure of a side-on superoxo complex of cobalt and hydrogen abstraction by a reactive terminal oxo ligand|year=1990|last1=Egan|first1=James W.|last2=Haggerty|first2=Brian S.|last3=Rheingold|first3=Arnold L.|last4=Sendlinger|first4=Shawn C.|last5=Theopold|first5=Klaus H.|journal=Journal of the American Chemical Society|volume=112|issue=6|pages=2445–2446 |bibcode=1990JAChS.112.2445E }}</ref>

Most complexes of ''η''²-O₂ are generated using hydrogen peroxide, not from 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.<ref>{{cite book|last1=Greenwood|first1= N. N.|last2= Earnshaw|first2= A. |date=1997 |title=Chemistry of the Elements |edition=2nd |location=Oxford|publisher=Butterworth-Heinemann |isbn=0-7506-3365-4}}</ref>

==Binuclear complexes of O₂== thumb|right|O₂-bound form of hemocyanin, the O₂ carrier for certain molluscs. These binding modes include ''μ''₂-''η''²,''η''²-, ''μ''₂-''η''¹,''η''¹-, and ''μ''₂-''η''¹,''η''²-. Depending on the degree of electron-transfer from the dimetal unit, these O₂ ligands can again be described as peroxo or superoxo. Hemocyanin is an O₂-carrier that utilizes a bridging O2 binding motif. It features a pair of copper centers.<ref name=Tolman>{{cite journal|title=Copper–Oxygen Complexes Revisited: Structures, Spectroscopy, and Reactivity|first1=Courtney E. |last1=Elwell|first2=Nicole L. |last2=Gagnon|first3=Benjamin D. |last3=Neisen|first4=Debanjan |last4=Dhar|first5=Andrew D. |last5=Spaeth|first6=Gereon M. |last6=Yee|first7=William B.|last7=Tolman|journal=Chemical Reviews|year=2017|volume=117|issue=3 |pages=2059–2107 |doi=10.1021/acs.chemrev.6b00636|pmid=28103018 |pmc=5963733}}</ref> :420px [[File:DOESCF10.svg|thumb|right|Structure of [Co(salen)(dmf)]₂O₂.<ref>{{cite journal|journal=J. Chem. Soc. A|author=M. Calligaris |author2=G. Nardin |author3=L. Randaccio |author4=A. Ripamonti |year=1970|page=1069|title=Structural Aspects of the Synthetic Oxygen-Carrier NN′-Ethylenebis(Salicylideneiminato)cobalt(II): Structure of the Addition Compound with Oxygen Containing Dimethylformamide|doi=10.1039/j19700001069}}</ref>]]. Salcomine, the cobalt(II) complex of salen ligand is the first synthetic O₂ carrier.<ref>{{cite journal | author = Tokuichi Tsumaki | title = Nebenvalenzringverbindungen. IV. Über einige innerkomplexe Kobaltsalze der Oxyaldimine | journal = Bulletin of the Chemical Society of Japan | year = 1938 | volume = 13 | issue = 2 | pages = 252–260 | doi = 10.1246/bcsj.13.252| doi-access = free }}</ref> Solvated derivatives of the solid complex bind 0.5 equivalent of O₂: :2 Co(salen) + O₂ → [Co(salen)]₂O₂

Reversible electron transfer reactions are observed in some dinuclear O₂ complexes.<ref>{{cite journal |doi=10.1021/ic50062a022|title=Structure of Decaammine-μ-Peroxo-Dicobalt Disulfate Tetrahydrate|year=1968|last1= Schaefer|first1=William Palzer|journal= Inorganic Chemistry|volume=7|issue=4 |pages=725–731}}</ref> thumb|center|398px|Oxidation of the dicobalt peroxy complex gives the complex of superoxide (O₂⁻). The Co-O-O-Co core flattens in the process and the O-O distance contracts by 10%.

==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== <references /> {{Coordination complexes}}

Category:Coordination complexes Category:Biochemistry Category:Inorganic chemistry