Chemical elements
  Phosphorus
    Isotopes
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    Preparation
    Applications
    Physical Properties
    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 Oxychloride, POCl3






Phosphorus oxytrichloride or phosphoryl chloride, POCl3, was early formed during investigations into the action of the pentachloride on substances containing the hydroxyl group. It was also prepared by the oxidation of the trichloride by air, by oxygen, and by many oxidising agents, e.g. nitrogen trioxide. It is also produced by the action of water in small proportion or acetic acid on PCl3Br2 or by the action of chlorsulphonic acid on red phosphorus.

Two convenient methods of preparation are as follows:—
  1. A current of chlorine is passed through phosphorus trichloride and water is added at the same time, drop by drop. The liquid is kept at its boiling-point, and is distilled at the end of the operation, which is signalised by the appearance of the pentachloride.
  2. 500 grams of PCl3 (free from phosphorus) are placed in a tubulated retort having a capacity of 950 c.c. or more. 160 grams of potassium chlorate are added through the tubulure in lots of about 4 grams. The POCl3 is then distilled:—

    3PCl3 + KClO3 = 3POCl3 + KCl

    The KClO3 should be dry and should previously be covered with some POCl3 before adding to the PCl3. Dried oxalic acid may be used as the oxidising agent, the weight used being half that of the PCl3.


Phosphoryl chloride may be produced on a large scale by passing a mixture of chlorine and carbon monoxide over an intimate mixture of carbon and calcium phosphate (such as charred bone) at 330° to 340° C.:—

Ca3(PO4)2 + 2Cl2 + 2CO = Ca(PO3)2 + 2CO2 + 2CaCl2
Ca(PO3)2 + 4Cl2 + 4CO = 2POCl3 + 4CO2 + CaCl2

By a similar reaction ferric phosphate is decomposed by carbonyl chloride at 300° to 400° C.


Physical Properties

Phosphoryl chloride is a colourless fuming liquid which resembles the trichloride in appearance but boils at a higher temperature, 107° C., and can easily be frozen to a solid which melts slightly above 0° C.

Analysis combined with determinations of vapour density led to the formula POCl3. According to the results of many investigators the density of the liquid at ordinary temperatures is slightly below 1.7. The exact experiments of Thorpe and Tutton gave the following results for the density at 0° C., 1.71165 to 1.71185 (1st series) and 1.71185 to 1.71190 (2nd series), and at the boiling-point, 107.23° C., 1.50967. The specific volumes and thermal expansions between these temperatures are summarised by the formula

vt = v0(1 + 0.0010643092 + 0.05112666t2 + 0.085299t3)

The liquid boils at 107.22° to 107.33° C. at 760 mm. and at 104.5° to 105.5° C. at 783 mm. It freezes at about -10° C. and the melting-point of the solid was +2° C., +1.78° C. The critical temperature is 329° C.

The surface tension, as determined by the capillary tube method, was given as 31.91 dynes/cm. at 18° C. and 28.37 at 46.1° C. Hence the change of molar surface energy with the temperature is normal. This physical constant, together with some others, was determined in order to obtain the parachor [P]. The sample of POCl3 had a boiling- point of 108.7° C. at 769 mm.

Parachor of phosphorus oxychloride

t° C154965
D1.6901.6261.596
σ32.7728.3626.57
[P]217.1217.7218.1


The dielectric constant of the oxychloride is 13.9 at 22° C. The heat of formation is nearly twice that of the trichloride and also greater than that of the pentachloride according to the equation

P (solid) + ½O2 (gas) + 1½Cl2 (gas) = POCl3 (liquid) + 146.0 Cals.,

The heat of formation from the trichloride and oxygen is also considerable, thus

PCl3 (liquid) + ½O2 (gas) = POCl3 (liquid) + 70.66 Cals.

The heat of hydrolysis with water is 74.7 Cals. If much water is used the products are orthophosphoric and hydrochloric acids, but when the compound deliquesces in moist air pyrophosphoryl and metaphosphoryl chlorides (q.v.) are formed as intermediate products. It is also hydrolysed by hydroxylated organic compounds and is much used for preparing chlorinated derivatives, e.g. C2H5Cl and CH3CO,Cl from C2H5OH and CH3COONa respectively. By this means also alkyl chlorophosphates and alkyl phosphates can be prepared, e.g.:—

2C2H5OH + POCl3 = POCl(OC2H5)2 + 2HCl
POCl(OC2H5)2 = C2H5Cl + PO2(OC2H5)

The alcohol must be added drop by drop to the phosphoryl chloride cooled in an ice-salt mixture. Sodium ethoxide yields triethyl phosphate:—

3C2H5ONa +POCl3 = PO(OC2H5)3 + 3NaCl

The oxychloride is also hydrolysed by orthophosphoric acid, which is dehydrated to the meta-acid, and by phosphorous acid, which is dehydrated and oxidised to metaphosphoric acid, thus:—

2H3PO4 + POCl3 = 3HPO3 + 3HCl
2H3PO3 + 3POCl3 = 3HPO3 + 2PCl3 + 3HCl

When the oxychloride is treated with potassium chlorate the chlorine of the former is displaced by oxygen, according to the equation

2POCl3 + KClO3 = P2O5 + 3Cl2 + KCl

A similar displacement can be effected by sulphur trioxide, thus

2POCl3 + 6SO3 = P2O5 + 3S2O5Cl2

Hydrogen sulphide gives a phosphorous oxysulphide, and, when the reaction is carried out at 100° C., an oxychlorosulphide to which the formula P2O2SCl4 was assigned, and which could be distilled under reduced pressure.

Phosphorus oxychloride chlorinates the oxides of several non-metals. The chlorides produced may form addition compounds with excess of the oxychloride: thus SeOCl2 gave SeCl4 and P2O5; TeO2 gave TeCl4.POCl3; B2O3 gave BCl3.POCl3 as well as BPO4. Other addition compounds are as follows SbCl5.POCl3; TiCl4.2POCl3; TiCl4.POCl3; AlCl3.POCl3; SnCl4.POCl3.

Phosphorus oxychloride is a good solvent for various acid chlorides, bromides and iodides such as those of arsenic and antimony, for VOCl3, S2Cl2 and halides of transitional elements such as FeCl3 and PtCl4. For this reason, and on account of its relatively high freezing- point, POCl3 has been much used for the determination of molecular weights by the cryoscopic method.

Combination with dry ammonia in carbon tetrachloride gave a solid product which was said to be the hexammoniate, POCl3.6NH3, while gaseous ammonia gave a white solid from which amides and aminochlorides were isolated.

Metals with widely different electro-affinities ranging from the alkalies to silver and mercury were not found to be affected much in the cold, but when heated they gave oxides, chlorides and phosphides in various cases.

Addition compounds such as CaO.2POCl3 and MgO.3POCl3 were obtained by heating the constituents together.
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