Chemical elements
    Physical Properties
    Chemical Properties
      Hypovanadous Oxide
      Vanadous Oxide
      Hypovanadic Oxide
      Vanadic Oxide
      Hypovanadous Fluoride
      Vanadous Fluoride
      Vanadium Tetrafluoride
      Vanadium Pentafluoride
      Vanadyl Difluoride
      Vanadium Oxytrifluoride
      Vanadium Dioxyfluoride
      Hypovanadous Chloride
      Vanadous Chloride
      Hypovanadic Chloride
      Divanadyl Chloride
      Vanadium Oxymonochloride
      Vanadyl Dichloride
      Vanadium Oxytrichloride
      Vanadium Oxydichloride
      Vanadous Bromide
      Hypovanadic Bromide
      Vanadium Oxymonobromide
      Vanadyl Dibromide
      Vanadium Oxytribromide
      Hydrated Vanadium Tri-iodide
      Vanadium Suboxide
      Hypovanadous Oxide
      Vanadous Oxide
      Hypovanadic Oxide
      Intermediate Vanadium Oxides
      Vanadium Pentoxide
      Sodium Stannovanadates
      Double Vanadates
      Heteropoly-Acids with Vanadium
      Pervanadic Acid
      Vanadium Monosulphide
      Vanadium Trisulphide
      Vanadium Pentasulphide
      Vanadium Oxysulphides
      Hypovanadous Sulphate
      Vanadous Sulphate
      Vanadyl Sulphites
      Vanadyl Sulphates
      Vanadic Sulphates
      Vanadyl Dithionate
      Ammonium Orthothiovanadate
      Ammonium Pyroxyhexathiovanadate
      Sodium Orthoxytrithiovanadate
      Sodium Orthoxymonothiovanadate
      Vanadium Selenides
      Vanadyl Selenite
      Vanadyl Selenates
      Vanadium Subnitride
      Vanadium Mononitride
      Vanadium Dinitride
      Alkali Vanadyl Nitrites
      Vanadium Nitrates
      Vanadyl Hypophosphite
      Vanadyl Phosphates
      Vanadous Pyrophosphate
      Vanadyl Arsenates
      Vanadium Carbide
      Vanadyl Cyanide
      Potassium Vanadocyanide
      Potassium Vanadicyanide
      Vanadium Ferrocyanides
      Ammonium Vanadyl Thiocyanate
      Vanadium Subsilicide
      Vanadium Disilicide
      Vanadium Boride
    Detection, Estimation
    PDB 1b8j-2i4e
    PDB 2jhr-6rsa

Hypovanadous Chloride, VCl2

Solutions of vanadium dichloride can be prepared by electrolytic reduction of higher chlorides, or by the addition of amalgamated zinc to a hydrochloric acid solution of vanadium pentoxide. The solution undergoes very rapid oxidation, hence the isolation of vanadium dichloride cannot be effected by a wet method. It is deposited in apple-green hexagonal flakes when the vapour of vanadium tetrachloride mixed with dry hydrogen is passed through a glass tube heated to dull redness.Vanadium trichloride undergoes decomposition to the dichloride and tetrachloride when heated to 900° C. in a stream of nitrogen or carbon dioxide. The tetrachloride produced at the same time distils away at the temperature of the reaction. More recently, vanadium dichloride has been obtained by the action of hydrogen chloride on commercial ferrovanadium. Its density at 18° C. is 3.23. It is a hygroscopic solid which deliquesces with oxidation to a brown liquid. In the presence of mineral acid a violet solution is formed, which, like all other solutions of divalent vanadium salts, acts as an extremely powerful reducing agent; it is, in fact, one of the strongest reducing agents known. It slowly evolves hydrogen from its aqueous or acid solutions, with formation of the trichloride; a vigorous evolution of hydrogen takes place from the acid solution in the presence of platinum foil. It bleaches litmus and indigo, precipitates the metals from solutions of salts of copper, tin, silver, gold and platinum, and has been successfully employed in the isolation of certain organic radicals, as, for example, the triphenylmethyl radical from triphenyl carbinol. At a bright red heat it reduces carbon dioxide to the monoxide:

3VCl2 + 2CO2 = 2VOCl + VCl4 + 2CO;

and with even stronger heating the reaction proceeds further,

4VCl2 + 3CO2 = V2O3 + 2VCl4 + 3CO,

pure vanadium sesquioxide being produced.

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