Cobalt tetracarbonyl hydride

Cobalt tetracarbonyl hydride
Cobalt tetracarbonyl hydride
Other names
cobalt hydrocarbonyl
tetracarbonylhydridocobalt, Tetracarbonylhydrocobalt
Identifiers
CAS number 16842-03-8 YesY=
PubChem 61848
Properties
Molecular formula C4HCoO4
Molar mass 171.98 g/mol
Appearance Light yellow liquid
Melting point

-33 °C, 240 K, -27 °F
Boiling point

47 °C, 320 K, 117 °F
Solubility in water Partially
Solubility soluble in hexane, toluene, ethanol
Acidity (pKa) 8.5
 YesY tetracarbonyl hydride (verify) (what is: YesY/N?)
Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa)
Infobox references

Cobalt tetracarbonyl hydride is the organometallic compound with the formula HCo(CO)4. It is a yellow liquid that forms a colorless vapor and has an intolerable odor.[1] Its main use is as a catalyst in hydroformylation.

Contents

Structure and properties

HCo(CO)4-3D-balls.png

HCo(CO)4 is a trigonal bipyrimidal molecule. The hydride ligand occupies one of the axial positions, thus the symmetry of the molecule is C3v.[2] The Co-CO and Co-H bond distances were determined by gas-phase electron diffraction to be 1.764 and 1.556 Å, respectively.[3]. The oxidation state of cobalt in this compound is -1.

Like some other metal carbonyl hydrides, HCo(CO)4 is acidic, with a pKa of 8.5.[4] HCo(CO)4 melts at -33 °C and above that temperature decomposes to Co2(CO)8 and H2.[1] It undergoes substitution by tertiary phosphines. For example, triphenylphosphine gives HCo(CO)3PPh3 and HCo(CO)2(PPh3)2. These derivatives are more stable than HCo(CO)4 and are used industrially.[5] These derivatives are generally less acidic than HCo(CO)4.[4]

Preparation

Tetracarbonylhydrocobalt was first described by Hieber in the early 1930s.[6] It was the second transition metal hydride to be discovered, after H2Fe(CO)4. It is prepared by reducing Co2(CO)8 with sodium amalgam or a similar reducing agent followed by acidification.[2]

Co2(CO)8 + 2 Na → 2 NaCo(CO)4
NaCo(CO)4 + H+ → HCo(CO)4 + Na+

Since HCo(CO)4 decomposes so readily, it is usually generated in situ by hydrogenation of Co2(CO)8.[5]

Co2(CO)8 + H2 is in equilibrium with 2 HCo(CO)4

The thermodynamic parameters for the equilibrium reaction were determined by infrared spectroscopy to be ΔH = 4.054 kcal mol−1, ΔS = -3.067 cal mol−1 K−1.[5]

Applications

Tetracarbonylhydridocobalt was the first transition metal hydride to be used in industry.[7] In 1940 it was discovered that it catalyzed the conversion of alkenes, CO, and H2 to aldehydes, a process known as hydroformylation (Oxo Reaction). Although it has since been largely superseded by rhodium-based catalysts, the world output of C3-C18 aldehydes produced by tetracarbonylhydrocobalt catalysis is about 100,000 tons/year, roughly 2% of the total.[7]

References

  1. ^ a b Kerr, W. J. (2001). "Sodium Tetracarbonylcobaltate". Encyclopedia of Reagents for Organic Synthesis. doi:10.1002/047084289X.rs105.  edit
  2. ^ a b Donaldson, J. D.; Beyersmann, D. (2005). "Cobalt and Cobalt Compounds". Ullmann's Encyclopedia of Industrial Chemistry. Wiley-VCH. doi:10.1002/14356007.a07_281.pub2.  edit
  3. ^ 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: 6243. doi:10.1021/ja00461a011.  edit
  4. ^ a b Moore, E. J.; Sullivan, J. M.; Norton, J. R. (1986). "Kinetic and thermodynamic acidity of hydrido transition-metal complexes. 3. Thermodynamic acidity of common mononuclear carbonyl hydrides". Journal of the American Chemical Society 108: 2257. doi:10.1021/ja00269a022.  edit
  5. ^ a b c M. Pfeffer, M. Grellier "Cobalt Organometallics" in Comprehensive Organometallic Chemistry III, 2007, Elsevier.doi:10.1016/B0-08-045047-4/00096-0
  6. ^ Hieber, W.; Mühlbauer, F.; Ehmann, E. A. (1932). "Derivate des Kobalt- und Nickelcarbonyls (XVI. Mitteil. über Metallcarbonyle)". Berichte der deutschen chemischen Gesellschaft (A and B Series) 65: 1090. doi:10.1002/cber.19320650709.  edit
  7. ^ a b Rittmeyer, P.; Wietelmann, U. (2000). "Hydrides". Ullmann's Encyclopedia of Industrial Chemistry. Wiley-VCH. doi:10.1002/14356007.a13_199.  edit

Wikimedia Foundation. 2010.

Игры ⚽ Поможем решить контрольную работу

Look at other dictionaries:

  • Cobalt(II) cyanide — IUPAC name Cobalt(II) cyanide Other names cobaltous cyan …   Wikipedia

  • Dictionary of chemical formulas — This is a list of chemical compounds with chemical formulas and CAS numbers, indexed by formula. This complements alternative listings to be found at list of inorganic compounds, list of organic compounds and inorganic compounds by element. Table …   Wikipedia

  • Nuclear weapon design — The first nuclear weapons, though large, cumbersome and inefficient, provided the basic design building blocks of all future weapons. Here the Gadget device is prepared for the first nuclear test: Trinity. Nuclear weapon designs are physical,… …   Wikipedia

  • Metal carbonyl — Iron pentacarbonyl An iron atom with five CO ligands Metal carbonyls are coordination complexes of transition metals with carbon monoxide ligands. These complexes may be homoleptic, that is containing only CO ligands, such as nickel carbonyl… …   Wikipedia

  • Organometallic chemistry — n Butyllithium, an organometallic compound. Four lithium atoms are shown in purple in a tetrahedron, and each lithium atom is bound to a butyl group (carbon is black, hydrogen is white). Organometallic chemistry is the study of chemical compounds …   Wikipedia

  • Nickel — This article is about the chemical element. For other uses, see Nickel (disambiguation). cobalt ← nickel → copper ↑ Ni ↓ Pd …   Wikipedia

  • Dicobalt octacarbonyl — Dicobalt octacarbonyl …   Wikipedia

Share the article and excerpts

Direct link
… Do a right-click on the link above
and select “Copy Link”