|Molar mass||121.847 g/mol|
|Appearance||pale green solid|
|Melting point||1,027 °C (1,881 °F; 1,300 K)|
|Boiling point||1,506 °C (2,743 °F; 1,779 K)|
|Main hazards||Reacts with oxygen rapidly|
|titanium(II) chloride, chromium(II) chloride|
Except where noted otherwise, data is given for materials in their standard state (at 25 °C (77 °F), 100 kPa)
|what is: / ?)(|
Vanadium(II) chloride is the inorganic compound with the formula VCl2, and is the most reduced vanadium chloride. Vanadium(II) chloride is an apple-green solid that dissolves in water to give purple solutions.
Solid VCl2 is prepared by thermal decomposition of VCl3, which leaves a residue of VCl2:
- 2 VCl3 → VCl2 + VCl4
Solid VCl2 adopts the cadmium iodide structure, featuring octahedral coordination geometry. 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).
Vanadium dichloride is a powerful reducing species, being able to convert sulfoxides to sulfides, organic azides to amines, as well as reductively coupling some alkyl halides.
- Young, R. C.; Smith, M. E. "Vanadium(II) Chloride" Inorganic Syntheses, 1953, volume IV, page 126-127.doi:10.1002/9780470132357.ch42
- Martin Pomerantz, Gerald L. Combs, N. L. Dassanayake, "Vanadium Dichloride Solution" Inorganic Syntheses, 1982, vol. XXI, pp. 185–187. doi:10.1002/9780470132524.ch42
- Holleman, A. F.; Wiberg, E. "Inorganic Chemistry" Academic Press: San Diego, 2001. ISBN 0-12-352651-5.