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Vanadium tetrachloride is the chemical compound with the formula VCl4. This bright red liquid is an important starting reagent in the preparation of vanadium compounds. It forms adducts with many donor ligands, for example, VCl4(THF)2. It is also the precursor to vanadocene dichloride.
Additional recommended knowledge
With one more valence electron than diamagnetic TiCl4, VCl4 is a paramagnetic liquid. Few chemical compounds are both liquid (at room temperature) and paramagnetic.
VCl4 is prepared by chlorination of vanadium metal. Notice that VCl5 cannot be prepared under normal conditions: Cl2 lacks the oxidizing power to attack VCl4. In contrast, the heavier analogues NbCl5 and TaCl5 are stable and not particularly oxidizing. Of course, VF5 does exist, reflecting the increased oxidizing power of F2 vs Cl2. Indicative of its oxidizing power, VCl4 releases Cl2 at its boiling point (standard pressure) to afford vanadium(III) chloride.
This reaction highlights the oxidizing ability of VCl4, consistent with it being resistant to further oxidation by Cl2.
VCl4 is a volatile, aggressive oxidant that readily hydrolyzes to release HCl.
|This article is licensed under the GNU Free Documentation License. It uses material from the Wikipedia article "Vanadium_tetrachloride". A list of authors is available in Wikipedia.|