Metal carbonyl hydride

A commercially important rhodium carbonyl hydride.

Metal carbonyl hydrides are complexes of transition metals with carbon monoxide and hydride as ligands. These complexes are useful in organic synthesis as catalysts in homogeneous catalysis, such as hydroformylation.[1]

## Contents

* 1 Preparation
* 2 Properties
* 3 Applications and occurrence
* 4 Analytical characterization
* 5 Further reading
* 6 References
* 7 External links

## Preparation

thumb|left|Decacarbonyldihydridotriosmium is one of many polymetallic carbonyl hydrides. Walter Hieber prepared the first metal carbonyl hydride in 1931 by the so-called Hieber base reaction of metal carbonyls. In this reaction a hydroxide ion reacts with the carbon monoxide ligand of a metal carbonyl such as iron pentacarbonyl in a nucleophilic attack to form a metallacarboxylic acid. This intermedia releases of carbon dioxide in a second step, giving the iron tetracarbonyl hydride anion. The synthesis of cobalt tetracarbonyl hydride (HCo(CO)4) proceeds in the same way.[2]

Fe(CO)5 \+ NaOH → Na[Fe(CO)4CO2H]
Na[Fe(CO)4CO2H] → Na[HFe(CO)4] + CO2

A further synthetic route is the reaction of the metal carbonyl with hydrogen.[3] The protonation of metal carbonyl anions, e.g. [Co(CO)4]−, leads also to the formation of metal carbonyl hydrides.

## Properties

Some Metal Carbonyl Hydrides  Metal Carbonyl hydride  | pKa

|

HCo(CO)4 | 1[4]
HCo(CO)3(P(OPh)3)  | 5.0
HCo(CO)3(PPh3)  | 7.0
HMn(CO)5 | 7.1
H2Fe(CO)4 | 4.4, 14
HRh(CO)(PPh3)3 | unknown

The neutral metal carbonyl hydrides are often volatile and can be quite acidic.[5] The hydrogen atom is directly bounded to the metal. The metal-hydrogen bond length is for cobalt 114 pm, the metal-carbon bond length is for axial ligands 176 and 182 for the equatorial ligands.[6]

## Applications and occurrence

Metal carbonyl hydrides are used as catalysts in the hydroformylation of olefins. The catalyst is usually formed in situ in a reaction of a metal salt precursor with the syngas. The hydroformylation starts with the generation of a coordinatively unsaturated 16-electron metal carbonyl hydride complex like HCo(CO)3 or HRh(CO)(PPh3)2 by dissociation of a ligand. Such complexes bind olefins in a first step via π-complexation, thus beginning the transformation of the alkene to the aldehyde.

Iron carbonyl hydrides occur in nature at the active sites of hydrogenase enzymes.

## Analytical characterization

It has been uncertain for a long time whether metal carbonyl hydrides contain a direct metal-hydrogen bond, although this has been suspected by Hieber for H2Fe(CO)4. The precise structure cannot be identified by X-ray diffraction, particularly the length of a possible metal-hydrogen bond remained uncertain.[7] The exact structure of the metal carbonyl hydrides has been determined by using neutron diffraction and nuclear magnetic resonance spectroscopy.[6][8]

## Further reading

## References

1. ↑ J. F. Hartwig; Organotransition metal chemistry - from bonding to catalysis. University Science Books. 2009. 753, 757-578. ISBN:978-1-891-38953-5.
2. ↑ Hieber, W.; Leutert, F. (1931). "Zur Kenntnis des koordinativ gebundenen Kohlenoxyds: Bildung von Eisencarbonylwasserstoff". Die Naturwissenschaften 19 (17): 360–361. doi:10.1007/BF01522286. Bibcode: 1931NW.....19..360H.
3. ↑ Kaesz, H. D.; Saillant, R. B. (1972). "Hydride complexes of the transition metals". Chemical Reviews 72 (3): 231–281. doi:10.1021/cr60277a003.
4. ↑ Holleman, Arnold F.; Wiberg, Egon; Wiberg, Nils (1995) (in de). Lehrbuch der anorganischen Chemie. Berlin. ISBN 978-3-11-012641-9. OCLC 237142268.
5. ↑ Ralph G. Pearson The Transition-Metal-Hydrogen Bond. Chemical Reviews. volume 85, 1985, S. 41–49, doi:10.1021/cr00065a002.
6. ↑ 6.0 6.1 McNeill, E. A.; Scholer, F. R. (1977). "Molecular Structure of the Gaseous Metal Carbonyl Hydrides of Manganese, Iron, and Cobalt". Journal of the American Chemical Society 99 (19): 6243–6249. doi:10.1021/ja00461a011.
7. ↑ Cotton, F. A. (1967). "Structure and Bonding in Metal Carbonyls and Related Compounds". Helvetica Chimica Acta 50: 117–130. doi:10.1002/hlca.19670500910. }
8. ↑ Bau, Robert; Drabnis, Mary H. (1997). "Structures of transition metal hydrides determined by neutron diffraction". Inorganica Chimica Acta 259 (1–2): 27–50. doi:10.1016/S0020-1693(97)89125-6.

## External links

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