Vanadium(II) chloride
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Names | |
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IUPAC name
Vanadium(II) chloride
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Other names
Vanadous chloride
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Identifiers | |
3D model (JSmol)
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ChemSpider | |
ECHA InfoCard | 100.031.057 |
PubChem CID
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RTECS number |
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CompTox Dashboard (EPA)
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Properties | |
VCl2 | |
Molar mass | 121.847 g/mol |
Appearance | pale green solid |
Density | 3.230 g/cm3 |
Melting point | 1,027 °C (1,881 °F; 1,300 K) |
Boiling point | 1,506 °C (2,743 °F; 1,779 K) |
soluble | |
Structure | |
CdI2 | |
octahedral | |
Hazards | |
Occupational safety and health (OHS/OSH): | |
Main hazards
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Reacts with oxygen rapidly |
Related compounds | |
Other anions
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vanadium(II) fluoride, vanadium dibromide |
Other cations
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titanium dichloride, chromium(II) chloride |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Vanadium(II) chloride is the inorganic compound with the formula VCl2. This purple solid is the most reduced vanadium chloride. Like other metal dihalides, it is a polymer. Vanadium(II) chloride dissolves in water to give purple solutions.
It is prepared by thermal decomposition of VCl3, which leaves a residue of VCl2:[1]
- 2 VCl3 → VCl2 + VCl4
VBr2 and VI2 are structurally and chemically similar to the dichloride. All have the d3 configuration, with a quartet ground state, akin to Cr(III).[2]
Vanadium dichloride is a powerful reducing species, being able to reduce sulfoxides to sulfides, organic azides to amines, as well as reductively coupling some alkyl halides. VCl2 dissolves in water to give the hexaaquo ion [V(H2O)6]2+. Evaporation of such solutions produces crystals of [V(H2O)6]Cl2.
References
- ^ Young, R. C.; Smith, M. E. "Vanadium(II) Chloride" Inorganic Syntheses, 1953 volume IV, page 126-127.doi:10.1002/9780470132357.ch42
- ^ Holleman, A. F.; Wiberg, E. "Inorganic Chemistry" Academic Press: San Diego, 2001. ISBN 0-12-352651-5.