Chemical elements
  Phosphorus
    Isotopes
    Energy
    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

Alkylphosphines






On account of the instability of the phosphines and phosphonium salts, the hydrogen valency of phosphorus is more clearly displayed in their alkyl substitution products which also, as is usual, possess a more pronounced basigenic character than the hydrogen compounds themselves. The methods of preparation of these compounds, and their properties, closely resemble those of the alkylamines.

The tertiary alkylphosphines were discovered by Thenard in 1845, and the primary and secondary by Hofmann in 1871. All may be prepared by general methods—by the action of phosphonium iodide on alkyl iodides or on alcohols, and by the action of zinc alkyls on phosphorus trichloride. The primary and secondary alkylphosphines are obtained as crystalline double salts with zinc iodide when the alkyl iodides are heated to 150° C. with phosphonium iodide in the presence of zinc oxide. The primary base is first liberated as a gas (PH2CH3) or as a volatile liquid (PH2C2H5) on the addition of water, and is distilled off and condensed. The secondary bases P(CH3)2H and P(C2H5)2H can be set free by the addition of potassium hydroxide to their hydriodides. The tertiary bases are prepared (as hydriodides) by heating phosphonium iodide with alcohols (CH3OH, C2H5OH) at 150° to 180° C., and also by the action of zinc alkyls on phosphorus trichloride.

Alkyliodides of the quaternary phosphonium bases are made by heating (to over 150° C.) the theoretical proportions of the alcohols with phosphonium iodide, thus:—

4CH3OH + PH4I = P(CH3)4I + 4H2O

They are well-crystallised salts, easily soluble in water, and highly dissociated even at dilutions of 32 litres to the mol. The bases, liberated by the action of silver oxide on the iodides, are also highly dissociated, and therefore behave as strong alkalies. Thus, in the case of P(CH3)4OH:—

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The mobility of the ion P(CH3)4+ is 42.3, that of P(C2H5)4+ 32.7, the mobility diminishing with increasing addition of -CH2- to about 23 in the case of P(C5H11)(C6H5)3+ (isoamyltriphenylphosphonium ion). Alkylphosphines differ from the corresponding ammonia derivatives by the great ease with which they are oxidised even by atmospheric oxygen, either with spontaneous inflammation, as in the case of some of the less alkylated members, or with the formation of phosphine oxides, as in the case of trialkylphosphines. Thus oxygen at ordinary temperatures combines with P(C2H5)3, giving P(C2H5)3O, which may be distilled with steam.

Triethylphosphine Oxide may be made in quantity by heating 1 part of phosphorus with 13 parts of ethyl iodide in a sealed tube at 175°-180° C. The product is distilled, first with ethyl alcohol to remove excess ethyl iodide, and then with concentrated potash, which removes the iodine and oxidises the compound. Thus:—

P(C2H5)4I + KOH = P(C2H5)3O + KI + C2H6

Triethylphosphine also combines with sulphur with evolution of heat to give the corresponding triethylphosphine sulphide, P(C2H5)3S, a very stable compound, which can also be made by oxidation, or by hydrolysis, of the curious addition compound P(C2H5)3.CS2, a red crystalline solid which is itself made by direct union of P(C2H5)3 and CS2. The oxidation is effected by silver oxide, according to the equation

P(C2H5)3CS2 +2Ag2O = Ag2S +2Ag + CO2 +P(C2H5)3S

The hydrolysis occurs at 100° C. and yields the oxide as well as the sulphide:—

4P(C2H5)3CS2 +2H2O = 2P(C2H5)3S + P(C2H5)3O + P(C2H5)3CH3OH + 3CS2

The structural formulae of these compounds, whether written with the usual bonds or with valency electrons, are clearly quite analogous to those of the alkyl derivatives of ammonia. Thus the presence of even one methyl group enables the phosphorus to accept a hydrogen ion from hydrogen iodide, giving a crystalline product which is not dissociated under ordinary conditions:—



In the alkylphosphine oxide (and sulphide) the lone pair of electrons on the phosphorus atom completes the octet of the oxygen (or sulphur), as in the case of amine oxides:—



Oxidation of the primary and secondary alkylphosphines gives alkyl acids, and chlorination of these with PCl5 gives the corresponding acid chlorides. These substances are of importance in elucidating the structure of the phosphorous acids, etc. (q.v.), in one tautomeric form of which the phosphorus is not trivalent, but has the same valency as exhibited in phosphoric acid or quaternary phosphonium bases. This form is fixed in the compounds obtained as follows:—

When methylphosphine is passed into concentrated nitric acid it gives a crystalline dibasic acid (methylphosphinic acid), P(CH3)O(OH)2, and the action of PCl5 on this yields P(CH3)OCl2. Oxidation of P(CH3)2H with nitric acid gives the monobasic dimethylphosphinic acid. Corresponding ethyl derivatives are also known.
V1664256 litres per mol
λ214221233 litres per mol


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