Chemical elements
  Antimony
    Isotopes
    Energy
    Production
    Application
    Physical Properties
    Chemical Properties
    Compounds
      Antimony Trihydride
      Antimony Trifluoride
      Antimony Pentafluoride
      Antimony Trichloride
      Oxychlorides of Tervalent Antimony
      Antimony Tetrachloride
      Antimony Pentachloride
      Chloroantimonic Acids
      Antimonyl Perchlorate
      Antimony Tribromide
      Antimony Oxybromides
      Antimony Pentabromide
      Antimony Triiodide
      Antimony Oxyiodide or Antimonyl Iodide
      Antimony Thioiodide
      Mixed Antimony Halides
      Antimony Trioxide
      Hydrated Antimony Trioxide
      Antimonites
      Antimony Tetroxide or Antimony Dioxide
      Antimony Pentoxide
      Antimony Trisulphide
      Antimony Pentasulphide
      Thioantimonates
      Normal Antimony Sulphate
      Potassium Stibiothiosulphate
      Antimony Selenate
      Antimony tritelluride
      Antimony Phosphide
      Antimonyl Dihydrogen Phosphite
      Antimony Phosphate
      Antimony Pyrophosphate
      Antimony Thiophosphate
    PDB 1exi-2xqa

Antimony Pentasulphide, Sb2S5






Antimony Pentasulphide, Sb2S5, appears to have been first described by Basil Valentine. Early writers knew it as sulphur auratum, while Glauber (1654) described it in his "Pharmacopoeia spagyrica" as Panacea Antimonialis.

It is doubtful if pure antimony pentasulphide has been prepared, most samples, and certainly all commercial products, containing free sulphur; possibly no higher sulphide exists than antimony tetrasulphide. A fairly pure product may be obtained by passing hydrogen sulphide through a solution containing antimony pentachloride (free from tervalent antimony) and 12 to 15 per cent, free hydrochloric acid. After treatment with carbon disulphide the resulting substance has a composition corresponding to Sb2S5, and does not react with ammoniacal silver nitrate.

Commercial antimony pentasulphide, or "golden antimony sulphide," is as already stated always impure, and is generally supposed to be a mixture of antimony tetrasulphide and free sulphur. The usual method of preparation is by the decomposition of an alkali thioantimonate, such as Schlippe's salt, Na3SbS4, by means of dilute acid:

2Na3SbS4 + 3H2SO4 = (Sb2S4 + S) + 3Na2SO4 + 3H2S
2Na3SbS4 + 6HCl = (Sb2S4 + S) + 6NaCl + 3H2S

Sulphurous acid has also been suggested, and is recommended in preference to the stronger acids since the evolution of hydrogen sulphide by the latter is objectionable. When sulphurous acid is used, the formation of excess of free sulphur (which would contaminate the product) may be prevented by the careful addition of sodium sulphite. In order to avoid the production of brownish products the solution must be kept acid.

Antimony pentasulphide is a reddish-yellow or brown powder with a faint smell and a sweetish taste. When heated it loses sulphur, darkens in colour, and at 170° C. is gradually converted into antimony trisulphide. When heated in air it is oxidised to antimony trioxide, which volatilises. It is reduced to metal by heating in a current of hydrogen, and is decomposed by exposure to moist air, antimony trioxide being formed. It is only partially oxidised by treatment with ammoniacal hydrogen peroxide.

The pentasulphide is partially soluble in ammonium hydroxide, forming a yellowish solution and leaving as residue a mixture of antimony trisulphide and sulphur. It is decomposed by nitric acid, and by hydrochloric acid (density 1.12) forming antimony trichloride, sulphur and hydrogen sulphide; treatment with sulphuryl chloride converts it into antimony pentachloride.

From most commercial samples of antimony pentasulphide sulphur can be removed by treatment with carbon disulphide, or other solvents of sulphur, the proportion removed depending upon the method of preparation of the pentasulphide.

Alkali hydroxides and carbonates react with antimony pentasulphide with formation of a mixture of alkali antimonates and thioantimonates, the former being precipitated. From the solutions obtained on filtering, antimony pentasulphide is reprecipitated by the addition of acids; while from solutions in alkali carbonate the precipitate consists of antimony trisulphide. Barium and strontium hydroxides behave in a somewhat similar manner. Fusion with potassium cyanide causes partial reduction, some potassium thioantimonite being formed.

Commercial antimony pentasulphide is a mixture of variable composition depending upon the method of manufacture. It is employed extensively in the rubber industry, and many methods of assay have been proposed.


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