Iron tetracarbonyl hydride

Iron tetracarbonyl hydride
Names
Preferred IUPAC name
Tetracarbonyldihydroiron
Other names
Iron tetracarbonyl dihydride, tetracarbonyldihydroiron[1]
Identifiers
3D model (JSmol)
ChemSpider
Properties
FeC
4H
2O
4
Molar mass 169.901 g mol−1
Appearance Liquid (at -20 °C)
Melting point −70 °C (−94 °F; 203 K)
Boiling point −20 °C (−4 °F; 253 K) (decomposes)
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Infobox references

Iron tetracarbonyl hydride is the organometallic compound with the formula H2Fe(CO)4. Also known as tetracarbonyldihydridoiron, tetracarbonyldihydroiron, or iron tetracarbonyl dihydride, this compound was the first metal hydride discovered. The complex is only stable at low temperatures and decomposes rapidly at temperatures above –20 °C.

Preparation

Iron tetracarbonyl hydride was originally produced by Hieber and Leutert, who developed a two-step process starting from iron pentacarbonyl:[2][3]

Fe(CO)5 + 2OH− → HFe(CO)−
4 + HCO−
3
HFe(CO)−
4 + H+ → H2Fe(CO)4

Current procedures consist of treatment of iron pentacarbonyl with potassium hydroxide and barium hydroxide to yield an orange solution. From this point in the reaction, ideal conditions consist of a cold dark environment, thus dubbing the method the "polar night synthesis".[4] This dark, cold environment stabilizes the dianion species Fe(CO)2−
4, which is light and temperature sensitive. The orange solution is then treated with sulfuric acid to protonate the anionic intermediate, giving the neutral product.

Structure and properties

In iron tetracarbonyl hydride the Fe(CO)4 group has C2v molecular symmetry with a geometry intermediate between octahedral and tetrahedral. Viewed as an octahedral complex, the hydride ligands are cis. Viewed as a tetrahedral Fe(CO)4 complex, the hydrides occupy adjacent faces of the tetrahedron.[5] Although the structure of tetracarbonyliron with the hydrogen atoms bound as a single H2 ligand has been proposed as an intermediate in some rearrangement reactions,[6] the stable state for the compound has the two atoms as independent ligands.[7]

Reactions

H2Fe(CO)4 undergoes rapid ligand substitutions. Upon warming, the complex liberates H2, giving tetracarbonyliron derivatives.[8]

H2Fe(CO)4 + PPh3 → H2Fe(CO)3PPh3
H2Fe(CO)3PPh3 → trans-Fe(CO)3PPh3 + H2

Another way the complex has been used is for cooperative bimetallic activation of CO2.[9]

Cp2MoCO2 + H2Fe(CO)4 → Cp2MoHCO+ HFe3(CO)−
11 + H2O

[HFe(CO)4]−

H2Fe(CO)4 has pK1 of 6.8 and pK2 of 15.[10] The monoanion [HFe(CO)4]− has more extensive reaction chemistry because it is more stable than the dihydride.[11][12] The monoanion is an intermediate in the homogeneous water-gas shift reaction (WGSR). The slow step in the iron carbonyl-catalyzed WGSR is the proton transfer from water to the iron hydride anion.[13]

HFe(CO)−
4 + H2O → H2Fe(CO)4 + OH−

References

  1. ↑ SciFinder entry for CAS #12002-28-7, accessed 2012-06-14
  2. ↑ Hieber, W.; Leutert, F. (1931). "Zur Kenntnis des koordinative gebundene Kohlenoxyds: Bildung von Eisencarbonylwasserstoff". Naturwissenschaften. 19 (17): 360. doi:10.1007/BF01522286.
  3. ↑ Rittmeyer, P.; Wietelmann, U. (2005), "Hydrides", Ullmann's Encyclopedia of Industrial Chemistry, Weinheim: Wiley-VCH, doi:10.1002/14356007.a13_199
  4. ↑ Vancea, L.; Graham, W.A.G. (1977). "Stereochemically Nonrigid Six-Coordinate Metal Carbonyl Complexes". J. Organomet. Chem. 134 (2): 219. doi:10.1016/S0022-328X(00)81421-7.
  5. ↑ McNeill, E. A.; Scholer, F. R. (1977). "Molecular structure of the gaseous metal carbonyl hydrides of manganese, iron, and cobalt". J. Am. Chem. Soc. 99 (19): 6243. doi:10.1021/ja00461a011.
  6. ↑ Soubra, C.; Oishi, Y.; Albright, T. A.; Fujimoto, H. (2001). "Intramolecular Rearrangements in Six-Coordinate Ruthenium and Iron Dihydrides". Inorg. Chem. 40 (4): 620–627. doi:10.1021/ic0006089.
  7. ↑ Drouin, B. J.; Kukolich, S. G. (1998). "Molecular Structure of Tetracarbonyldihydroiron: Microwave Measurements and Density Functional Theory Calculations". J. Am. Chem. Soc. 120 (27): 6774–6780. doi:10.1021/ja9741584.
  8. ↑ Peason, R. G.; Walker, H. W.; Mauermann, H.; Ford, P.C. (1981). "Hydrogen migration mechanism for ligand substitution reactions in metal carbonyl hydrides". Inorg. Chem. 20 (8): 2741. doi:10.1021/ic50222a078.
  9. ↑ Tsai, J.-C.; Khan, M.A.; Nicholas, K.M. (1991). "Reduction of Coordinated Carbon Dioxide by Transition-Metal Hydrides". Organometallics. 10: 29. doi:10.1021/om00047a016.
  10. ↑ Walker, H.W.; Kresge, C.T.; Ford, P.C.; Pearson, R. G. (1979). "Rates of Deprotonation and pKa Values of Transition Metal Carbonyl Hydrides". J. Am. Chem. Soc. 101 (24): 7428. doi:10.1021/ja00518a061.
  11. ↑ Brunet, J.-J.; Chauvin, R.; Diallo, O.; Kindela, F.; Leglaye, P.; Neibecker, D., "Coordination chemistry of mononuclear iron carbonyl complexes", Coordination Chemistry Reviews 1998, 178-180, 331-352. doi:10.1016/S0010-8545(98)00075-7
  12. ↑ Brunet, J.J. (1990). "Tetracarbonylhydridoferrates, MHFe(CO)4: Versatile tools in Organic Synthesis and Catalysis". Chem. Rev. 90 (6): 1041. doi:10.1021/cr00104a006.
  13. ↑ Crabtree R.H.; Mingos D.M.P. 2007. Comprehensive Organometallic Chemistry III From Fundamentals to Applications. Elsevier Ltd.
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