Chemical elements
  Sulphur
    Isotopes
    Energy
    Extraction
    Refining
    Applications
    Allotropy
    Crystalline
    Amorphous Sulphur
    Colloidal Sulphur
    Physical Properties
    Chemical Properties
    Detection
    Estimation
    Compounds
      Hydrogen Sulphide
      Metal Polysulphides
      Hydrogen Polysulphides
      Hydrogen Pentasulphide
      Hydrogen Trisulphide
      Hydrogen Disulphide
      Sulphur Monofluoride
      Sulphur Tetrafluoride
      Sulphur Hexafluoride
      Sulphur Monochloride
      Sulphur Dichloride
      Sulphur Tetrachloride
      Sulphur Monobromide
      Thionyl Fluoride
      Sulphuryl Fluoride
      Fluorosulphonic Acid
      Thionyl Chloride
      Sulphuryl Chloride
      Sulphur Oxytetrachloride
      Pyrosulphuryl Chloride
      Chlorosulphonic Acid
      Thionyl Bromide
      Sodium Sulphoxylate
      Sulphur Dioxide
      Sulphurous Acid
      Sulphites
      Sulphur Trioxide
      Pyrosulphuric Acid
      Pyrosulphates
      Sulphuric Acid
      Persulphuric Anhydride
      Persulphuric Acid or Perdisulphuric Acid
      Perdisulphates
      Permonosulphuric Acid
      Amidopermonosulphuric Acid
      Thiosulphuric Acid
      Thiosulphates
      Polythionic Acids
      Dithionic Acid
      Trithionic Acid
      Trithionates
      Tetrathionic Acid
      Tetrathionates
      Pentathionic Acid
      Pentathionates
      Wackenroders Solution
      Hexathionic Acid
      Polythionic Acids
      Sulphur Sesquioxide
      Hydrosulphurous Acid
      Hydrosulphites
      Nitrogen Sulphide
      Nitrogen Persulphide
      Nitrogen Pentasulphide
      Sulphammonium
      Hexasulphamide
      Nitrogen Chlorosulphide
      Trithiazyl Chloride
      Thiotrithiazyl Chloride
      Dithiotetrathiazyl Chloride
      Nitrogen Bromosulphide
      Thiotrithiazyl Bromide
      Thiotrithiazyl Iodide
      Thiotrithiazyl Nitrate
      Thiotrithiazyl Hydrogen Sulphate
      Thiotrithiazyl Thiocyanate
      Thionylamide
      Sulphamide
      Imidodisulphamide
      Sulphimide
      Sulphonic Acids
      Amidosulphonic Acid
      Imidosulphonic Acid
      Nitrilosulphonic Acid
      Hydroxylamine-monosulphonic Acid
      Nitrososulphonic Acid
      Hydroxylamine-disulphonic Acid
      Hydroxylamine-isodisulphonic Acid
      Hydroxylamine-trisulphonic Acid
      Dihydroxylamidosulphonic Acid
      Sulphazinic Acid
      Sulphazotinic Acid
      Dehydrosulphazotinic Acid
      Nitrosulphonic Acid
      Nitrosulphonyl Chloride
      Nitrosulphonic Anhydride
      Nitrosulphuric Acid
      Nitrosodisulphonic Acid
      Sulphonitronic Acid
      Sulphates of Hydroxylamine
      Hydroxylamine Dithionate
      Hydrazine Dithionate
      Hydrazine Amidosulphonate
      Carbon Subsulphide
      Carbon Monosulphide
      Carbon Disulphide
      Thioformaldehyde
      Thiocarbonic Acid
      Ammonium thiocarbonate
      Thiolcarbonic Acid
      Xanthic Acid
      Perthiocarbonic Acid
      Sodium perthiocarbonate
      Carbonyl Sulphide
      Thiocarbonyl Chloride
      Thiocarbonyl Tetrachloride or
      Carbon Hexachlorosulphide
      Trichloromethyl Disulphide
      Thiocarbonyl Sulphochloride
      Carbon Bromosulphide
      Amino-derivatives of Thiocarbonic Acid
      Dithiocarbamic Acid
      Thiocarbamide
      Azidodithiocarbonic Acid
      Thiocyanogen
      Cyanogen Monosulphide
      Cyanogen Trisulphide
      Sulphur Thiocyanate
      Disulphur Dithiocyanate
      Thiocyanic Acid
      Thiocyanates
      Dithiocyanic Acid
      Trithiocyanuric Acid
      Perthiocyanic Acid
      Perthiocyanogen
      Sulphates

Sulphamide, SO2(NH2)2






Sulphamide, SO2(NH2)2, the amide of sulphuric acid, may be obtained by the action of dry ammonia upon a cooled solution of sulphuryl chloride in either ethylene chloride or chloroform solution:

4NH3 + SO2Cl2 = SO2(NH2)2 + 2NH4Cl.

It is better prepared by saturating a solution of sulphuryl chloride in 15 to 20 times its volume of chloroform with ammonia and shaking the product with water until the precipitate has dissolved. The aqueous solution, after boiling with lead oxide or silver oxide to remove chlorine and filtering, yields a viscid, hygroscopic liquid on evaporation.

Another method of preparation for pure sulphamide is to dissolve the product of the reaction between sulphuryl chloride and liquid ammonia in a small quantity of water and acidify the solution in order to cause hydrolysis. After two or three days, when hydrolysis is complete, the mixture is evaporated to dryness in vacuo and the residue extracted with ethyl acetate. The sulphamide is dissolved out and on evaporating off the ethyl acetate, pure sulphamide is obtained.

Sulphamide forms large, colourless, tabular crystals, which melt between 91-5° and 93° C. It is tasteless, only sparingly soluble in water or dilute alcohol, and neutral in reaction. On heating to 100° C. it begins to lose ammonia, with formation of imidodisulphamide, NH2. SO2.NH.SO2.NH2, and at 250° C. it decomposes completely, with loss of sulphur dioxide. With ammoniacal silver nitrate a precipitate is produced, which on heating to a temperature of 170° to 180° C. (preferably with a little ammonium chloride) until evolution of ammonia ceases, deposits the silver salt of sulphimide, SO2NAg. On heating, this compound yields metallic silver mixed with a little silver sulphate. Sulphamide dissolves readily in cold concentrated nitric acid without nitration. On the addition of concentrated sulphuric acid, nitrosulphamide, NH2.SO2.NH.NO2, is precipitated. This, on reduction with zinc dust and dilute sulphuric acid, yields first, hydrazine sulphon- amide, NH2.SO2.NH.NH2, and ultimately, amidosulphonic acid and hydrazine sulphonic acid or their zinc salts.

Sulphamide absorbs

1.4 molecular proportions of dry ammonia at+ 20° C.
3.0 molecular proportions of dry ammonia at0 ° C.
5.4 molecular proportions of dry ammonia at-20° C.


In the pure state, sulphamide is a non-electrolyte, indicating the weakness of its acidic tendencies. With the alkalis it forms salts, but not more than two atoms of hydrogen are displaceable by the metal.

From a consideration of the electrical conductivities of its solutions it has been suggested that sulphamide may also exist in an aci form, thus:

,

just as in the case of carbamide.


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