|Jmol-3D images||Image 1|
|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|
|Solubility in water||soluble|
|Main hazards||Reacts with oxygen rapidly|
|Other anions||vanadium(II) fluoride,
|Other cations||titanium(II) chloride, chromium(II) chloride|
|Related compounds||vanadium(III) chloride|
| (what is: / ?)
Except where noted otherwise, data are given for materials in their standard state (at 25 °C (77 °F), 100 kPa)
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:
- 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).
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.