vanadium(II) fluoride
{{Chembox
| ImageFile= Rutile structure.png
| OtherNames = Vanadium(II) fluoride
|Section1={{Chembox Identifiers
| CASNo = 13842-80-3
| PubChem=101602874
| StdInChI=1S/2FH.V/h2*1H;/q;;+2/p-2
| StdInChIKey=XHZLWOBYMWIKHM-UHFFFAOYSA-L
| SMILES=[F-].[F-].[V+2]
}}
|Section2={{Chembox Properties
|V=1|F=2
| Appearance= blue crystals
| Density=
| MeltingPt=
| BoilingPt=
| Solubility= soluble in water, forms [V(H2O)6]2+{{Holleman&Wiberg|edition=102 |page=1550 }}
}}
}}
Vanadium(II) fluoride is a fluoride of vanadium, with the chemical formula of VF2. It forms blue crystals.
Preparation
Vanadium(II) fluoride can be produced by the reduction of vanadium trifluoride by hydrogen in a hydrogen fluoride atmosphere at 1150 °C:Lothar Kolditz: Anorganische Chemie Teil 2. VEB Deutscher Verlag der Wissenschaften, Berlin, 1980, S. 641.
:{{chem2|2 VF3 + H2 -> 2 VF2 + 2 HF}}
Properties
= Physical properties =
Vanadium(II) fluoride crystallizes in the tetragonal crystal system with space group P42/mnm (No. 136). Its lattice constants are a = 480.4 pm and c = 323.7 pm.J. W. Stout, W. O. J. Boo: Crystalline vanadium (II) fluoride, VF2. Preparation, structure, heat capacity from 5 to 300 K and magnetic ordering. In: The Journal of Chemical Physics. 71, 1, 1979, S. 1–8, {{doi|10.1063/1.438115}}.
= Reactions =
Vanadium(II) fluoride is a strong reducing agent that can reduce nitrogen to hydrazine in the presence of magnesium hydroxide.
It dissolves in water to form [V(H2O)6]2+ ions.
:{{Chem2|V^{2+} + 6 H2O -> [V(H2O)6]^{2+} }}