Chemical elements
  Phosphorus
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    Chemical Properties
      Alkali Phosphides
      Alkaline Earth Phosphides
      Copper Silver and Gold Phosphides
      Zinc Group Phosphides
      Aluminium Phosphide
      Titanium Group Phosphides
      Tin Phosphides
      Lead Phosphides
      Arsenic Phosphides
      Antimony Phosphides
      Bismuth Phosphides
      Chromium Phosphides
      Molybdenum and Tungsten Phosphides
      Manganese Phosphides
      Iron Phosphides
      Cobalt Phosphides
      Phosphonium Chloride
      Phosphonium Bromide
      Phosphonium Iodide
      Hydrogen Phosphides
      Alkylphosphines
      Phosphorus Trifluoride
      Phosphorus Pentafluoride
      Phosphorus Trifluorodichloride
      Phosphorus Trifluorodibromide
      Fluophosphoric Acid
      Phosphorus Dichloride
      Phosphorus Trichloride
      Phosphorus Pentachloride
      Phosphorus Chlorobromides
      Phosphorus Chloroiodides
      Phosphorus Tribromide
      Phosphorus Pentabromide
      Phosphorus Diiodide
      Phosphorus Triiodide
      Phosphorus Oxytrifluoride
      Phosphorus Oxychloride
      Pyrophosphoryl Chloride
      Metaphosphoryl Chloride
      Phosphoryl Monochloride
      Phosphoryl Dichlorobromide
      Phosphoryl Chlorodibromide
      Phosphoryl Tribromide
      Metaphosphoryl Bromide
      Phosphoryl Oxyiodides
      Phosphorus Thiotrifluoride
      Phosphorus Thiotrichloride
      Phosphorus Thiotribromide
      Mixed Phosphorus Thiotrihalides
      Phosphorus Suboxides
      Phosphorus Trioxide
      Phosphorus Dioxide
      Phosphorus Pentoxide
      Hypophosphorous Acid
      Phosphorous Acid
      Meta- and Pyro-phosphorous Acids
      Hypophosphoric Acid
      Tetraphosphorus Trisulphide
      Diphosphorus Trisulphide
      Tetraphosphorus Heptasulphide
      Phosphorus Pentasulphide
      Phosphorus Oxysulphides
      Phosphorus Thiophosphites
      Phosphorus Thiophosphates
      Phosphorus Selenophosphates
      Phosphorus Sulphoselenides
      Diamidophosphorous Acid
      Phosphorus Triamide
      Monamidophosphoric Acid
      Diamidophosphoric Acid
      Triamidophosphoric Acid
      Dimetaphosphimic Acid ≡P=
      Trimetaphosphimic Acid
      Tetrametaphosphimic Acid
      Penta- and Hexametaphosphimic Acid
      Monamidodiphosphoric Acid
      Diamidodiphosphoric Acid
      Triamidodiphosphoric Acid
      Nitrilotrimetaphosphoric acid
      Monothioamidophosphoric Acids
      Thiophosphoryl Nitride
      Di- Tri-imido- and -amido-thiophosphates
      Imidotrithiophosphoric Acid =
      Phosphorus Chloronitrides
      Triphosphonitrilic Chloride
      Tetraphosphonitrilic Chloride
      Pentaphosphonitrilic Chloride
      Hexaphosphonitrilic Chloride
      Heptaphosphonitrilic Chloride
      Triphosphonitrilic Bromide
      Phosphorus Halonitrides
      Phosphorus Nitride
      Phosphine
      Pyrophosphoric Acid
      Phosphoric acids
    Slow Oxidation
    Phosphatic Fertilisers

Phosphorus Pentasulphide, P2S5






The methods which have been already described in connection with the other sulphides have been successfully used in the preparation of Phosphorus Pentasulphide or Diphosphorus Pentasulphide or Phosphorus Tetritadecasulphide, P2S5 or P4S10, from the theoretical proportions of the elements:—
  1. By fusion. This method is used in the preparation of the commercial product, which is not pure. A slight excess of sulphur should be used and the heating should take place in an atmosphere of CO2. The compound may be purified by heating in a vacuous sealed tube for several hours at 700° C., and then by crystallisation from carbon disulphide.
  2. By heating phosphorus (20 grams) and sulphur (60 grams) in a sealed tube with iodine (0.5 gram) and carbon disulphide (150 c.c.) at 211° C., followed by recrystallisation.
  3. By the action of H2S on POCl3.
  4. By passing the vapour of PSCl3 through a red-hot tube.


Details of the preparation have been given by Stock. Pure, dry, red phosphorus (100 grams) is intimately mixed with sulphur (260 grams). Portions of 30 to 40 grams are heated until they combine, in the manner described under P4S3. The product is ground up and heated in an evacuated and sealed glass tube to about 700° C. The contents are powdered and extracted with CS2. They are recrystallised twice from the same solvent and dried at 100° C. in a current of hydrogen. The yield should be about 60 per cent, of the theoretical.


Properties

The compound has been prepared in two forms:—

  1. Pale yellow crystals obtained by repeated recrystallisation from carbon disulphide, in which they are only sparingly soluble (1 in 195). Density 2.03.
  2. A nearly white substance obtained by rapid condensation of the vapour, followed by extraction with carbon disulphide. This form was more soluble in this solvent (1 in 30), had a higher density (2.08) and a lower indefinite melting-point (247° to 276° C.).


The melting-point of the commercial sulphide was 255° C. and that of the recrystallised product 275° to 276° C. The melting-point was raised to 284° to 291° C. by repeated recrystallisation from carbon disulphide. Boiling occurs with partial decomposition at 513° to 515° C. Other values which have been found are 520° C., 523.6° C. The sulphide distils in a water-pump vacuum at 332° to 340° C., probably with considerable dissociation.

The vapour density at temperatures slightly above the boiling- point corresponded to simple molecules P2S5. Later investigators, however, found that it was slightly below the theoretical, being 208 at 300° C., and decreased at higher temperatures, down to 133 at 1000° C. The molecular weight in boiling carbon disulphide was 482 to 491, corresponding approximately to double molecules (P4S10 requires 444).

The compound does not glow in air, but is highly inflammable, giving a mixture of the oxides. It was attacked only slowly by cold water, but rapidly by hot water, giving phosphoric acid and hydrogen sulphide. It did not form addition compounds with bromine or iodine. It was converted into PSCl3 by phosphorus pentachloride and by several other acid chlorides:—

P2S5 + 3PCl5 = 5PSCl3
P2S5 + 5POCl3 = 5PSCl3 + P2O5
2P2S5 + 6SOCl2 = 4PSCl3 + 3SO2 + 9S
P2S5 + SbCl3 = PSCl3 + SbPS4

Ammonia, in the gaseous or liquid form, was readily absorbed by the pentasulphide giving a phosphorus hexammonio-pentasulphide, P2S5.6NH3, as well as lower ammoniates. This compound may be ammonium diimidopentathiopyrophosphate, S{P(SNH4)2(NH)}2.

The pentasulphide dissolved slowly in cold alkalies, quickly in hot, and gave salts of thiophosphoric acid. Sodium sulphide also gave a thiophosphate.
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