Chromium carbonyl
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| Chromium carbonyl | |
|---|---|
6.png/150px-Cr(CO)6.png) |
|
| IUPAC name | hexacarbonylchromium(0) |
| Other names | chromium carbonyl |
| Identifiers | |
| CAS number | [13007-92-6] |
| RTECS number | GB5075000 |
| Properties | |
| Molecular formula | C6CrO6 |
| Molar mass | 220.06 g/mol |
| Appearance | colorless crystals |
| Density | 1.77 g/cm3, solid |
| Melting point |
150 °C (decomposition) |
| Boiling point |
sublimes |
| Solubility in water | insoluble |
| Solubility in other solvents | soluble in benzene, THF |
| Structure | |
| Crystal structure | orthrhombic |
| Coordination geometry |
octahedral |
| Dipole moment | 0 D |
| Hazards | |
| Main hazards | CO source |
| R-phrases | R22 |
| S-phrases | S53 S36 S45 |
| Related compounds | |
| Related compounds | V(CO)6, Fe(CO)5-]], CrCl3 |
| Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa) Infobox disclaimer and references |
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Chromium carbonyl, also known as chromium hexacarbonyl, is the chemical compound with the formula Cr(CO)6. At room temperature the solid is stable to air, although it does have a high vapor pressure and sublimes readily. Cr(CO)6 is zerovalent, meaning that Cr has a formal charge of zero, and it is called a homoleptic complex, which means that all the ligands are the same. The complex is octahedral with Cr-C and C-O distances of 1.92 and 1.17 Å, respectively.[1]
Contents |
[edit] Reactions
When heated or photolyzed in tetrahydrofuran (THF) solution, Cr(CO)6 converts to Cr(CO)5(THF) with loss of one CO ligand. Similarly, heating a solution of Cr(CO)6 in an aromatic solvent results in replacement of three CO ligands:
- Cr(CO)6 + C6H5R → Cr(CO)3(C6H5R) + 3 CO
Such reactions proceed particularly well with electron-rich arenes such as anisole, either as the neat reagent or using a mixture of THF and dibutyl ether, the latter to increase the boiling point of the mixture. The products adopt a "piano-stool" structure. These species are typically yellow solids, which dissolve well in common organic solvents. The arene can be liberated from the chromium with iodine or by photolysis in air. In general, substituted derivatives of Cr(CO)6 decompose upon exposure to air.
Alkyl and aryl organolithium reagents RLi add to a carbonyl ligand to give anionic acyl complexes.[2] These species react with alkylating agents such as Me3O+ to form (OC)5Cr=C(OMe)R, an example of a Fischer carbene. If the R group is a vinyl or an aryl group, then the resulting carbene complex can react with an acetylene to form a new benzene ring to which is bonded the chromium tricarbonyl fragment. The two acetylene carbon atoms become part of the new ring, as does a carbon from one of the carbonyl ligands. Also the three carbons from the vinyl carbene become part of the new benzene ring.
[edit] Safety
In common with many of the other homoleptic metal carbonyls (e.g. nickel carbonyl and iron carbonyl), chromium hexacarbonyl is toxic and thought to be carcinogenic. Its vapor pressure is relatively high for a metal complex, 1 mm Hg ( 36 °C).
[edit] References
- ^ Whitaker A.; Jeffery, J. W. “The Crystal Structure of Chromium Hexacarbonyl” Acta Crystallographica 1967, volume 23, pp. 977-984. doi:10.1107/S0365110X67004153.
- ^ Elschenbroich, C. ”Organometallics” (2006) Wiley-VCH: Weinheim. ISBN 978-3-29390-6
