Vanadium(II) chloride

Vanadium(II) chloride
IUPAC name Vanadium(II) chloride
Other names Vanadous chloride
Identifiers
CAS number	10580-52-6
PubChem	66355
ChemSpider	59733 Y
RTECS number	YW1575000
Jmol-3D images	Image 1
SMILES Cl[V]Cl
InChI InChI=1S/2ClH.V/h2*1H;/q;;+2/p-2 Y Key: ITAKKORXEUJTBC-UHFFFAOYSA-L Y InChI=1/2ClH.V/h2*1H;/q;;+2/p-2 Key: ITAKKORXEUJTBC-NUQVWONBAZ
Properties
Molecular formula	VCl2
Molar mass	121.847 g/mol
Appearance	pale green solid
Density	3.230 g/cm3
Melting point	1027 °C, 1300 K, 1881 °F
Boiling point	1506 °C, 1779 K, 2743 °F
Solubility in water	soluble
Structure
Crystal structure	CdI2
Coordination geometry	octahedral
Hazards
R-phrases	20/21/22-34
S-phrases	26-27-36/37/39-45
Main hazards	Reacts with oxygen rapidly
Related compounds
Other anions	vanadium(II) fluoride, vanadium dibromide
Other cations	titanium dichloride, chromium(II) chloride
Related compounds	vanadium trichloride
Y chloride (verify) (what is: Y/N?) Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa)
Infobox references

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.

Preparation, properties, and related compounds

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

1. ^ Young, R. C.; Smith, M. E. "Vanadium(II) Chloride" Inorganic Syntheses, 1953 volume IV, page 126-127.doi:10.1002/9780470132357.ch42
2. ^ Holleman, A. F.; Wiberg, E. "Inorganic Chemistry" Academic Press: San Diego, 2001. ISBN 0-12-352651-5.