Chemical elements
  Titanium
    Isotopes
    Energy
    Preparation
    Physical Properties
    Chemical Properties
      Titanium Trifluoride
      Titanium Tetrafluoride
      Hydrofluotitanic acid
      Potassium Titanifluoride
      Sodium Titanifluoride
      Titanium Dichloride
      Titanium Trichloride
      Titanium Tetrachloride
      Titanic Chloride
      Titanium Oxychlorides
      Hydrochlorotitanic Acid
      Addition Compounds of Titanium Tetrachloride
      Titanium Tribromide Hexahydrate
      Titanium Tetrabromide
      Titanic Bromide
      Hydrobromotitanic Acid
      Titanium Chlorobromides
      Titanium Di-iodide
      Titanium Tri-iodide
      Titanium Tetra-iodide
      Titanic Iodide
      Titanium Monoxide
      
Titanium Sesquioxide
      Titanium Dioxide
      Titanic Oxide
      Titanic Hydroxides
      Metatitanic Acid
      Titanates
      Titanium Monosulphide
      Titanium Sesquisulphide
      Titanium Disulphide
      Titanium Sulphates
      Titanous Sulphate
      Titanium Sesquisulphate
      Complex Sulphates of Tervalent Titanium
      Normal Titanic Sulphate
      Potassium Titanisulphate
      Potassium and Ammonium Titanylsulphates
      Titanous Nitride
      Titanic Nitride
      Titanamide
      Titanium Nitrogen Halides
      Titaninitric Acid
      Titanium Phosphide
      Titaniphosphoric Acid
      Titanium Carbide
      Titanium Cyanonitride
      Titanium Thiocyanates
      Titanium Sesquioxalate
      Titanitartrates and Allied Salts
      Titanium Silicide
      Pertitanates

Titanium Dichloride, TiCl2






Titanium Dichloride, TiCl2, was first prepared by Friedel and Guerin, who heated the trichloride to a red heat in a current of hydrogen, thus decomposing it into the tetrachloride, which distilled, and the dichloride, which remained behind; von der Pfordten, however, reduced the cold tetrachloride with sodium amalgam or hydrogen sulphide, and distilled off the unchanged tetrachloride in a current of carbon dioxide. Stahler and Bachran have obtained the dichloride nearly pure by heating the trichloride at 660°-700° C. in an atmosphere of hydrogen:

2TiCl3TiCl2 + TiCl4.

The dichloride remains after the volatilisation of the tetrachloride as a deep black powder which begins to sublime at 300° C. in a vacuum.

The properties of the dichloride have been variously described. According to Friedel and Guerin it is a brown powder which decomposes water and alcohol, evolving hydrogen and forming a yellow solution; while, according to von der Pfordten, it dissolves unchanged in these solvents, forming yellow solutions which gradually oxidise in the air. It is insoluble in non-hydroxylic solvents - a fact which suggests its saline character; it burns in the air, evolving titanium tetrachloride vapour and forming titanic oxide; it combines with bromine to form a chlorobromide. A satisfactory test for bivalent titanium is the formation of a violet colour, due to TiCl3, when it is mixed with a hydrochloric acid solution of titanium tetrachloride.


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