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 Tetrafluoride, TiF4






Impure Titanium Tetrafluoride, TiF4, is formed when magnesium titanifluoride, Mg2TiF6, or the corresponding barium salt, BaTiF6, is decomposed by strong ignition; but it is best prepared by one of the three following methods: (i) the action of fluorine on titanium, (ii) the action of anhydrous hydrogen fluoride on titanium, (iii) the action of anhydrous hydrogen fluoride on titanium tetrachloride at 100°-120° C.; for, owing to the high volatility of hydrogen chloride compared with hydrogen fluoride, the reaction

4HF + TiCl ⇔ 4TiF4 + 4HCl

proceeds in one direction only.

Titanium tetrafluoride is a colourless mass having a density 2.798 at 20.5° C. It boils at 284° C. and at 444° C. has a vapour density of 64.5 (theory = 62.05). It is noteworthy that the boiling-point of the fluoride is above that of the tetrachloride, TiCl4 (136° C.); this probably indicates that the former is polymerised near its boiling-point. This difference between the tetrafluoride and tetrachloride is in marked contrast with that between the silicon halides, SiF4 and SiCl4, and the corresponding halides of other non-metals and metalloids, and relates titanium to the metals rather than the metalloids. The saline nature of the fluoride is further shown by the fact that it is hygroscopic, and forms a clear solution in water, which deposits the hydrate TiF4.2H2O on evaporation. With alcohol the compound TiF4.C2H5OH is formed, and with ammonia the compound TiF4.2NH3; but, singularly, it does not combine directly with hydrogen fluoride, although the salts M2TiF6 are so well known. Roasting with sulphuric acid converts titanium tetrafluoride into titanic oxide.


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