Chemical elements
    Amorphous Sulphur
    Colloidal Sulphur
    Physical Properties
    Chemical Properties
      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
      Sulphur Trioxide
      Pyrosulphuric Acid
      Sulphuric Acid
      Persulphuric Anhydride
      Persulphuric Acid or Perdisulphuric Acid
      Permonosulphuric Acid
      Amidopermonosulphuric Acid
      Thiosulphuric Acid
      Polythionic Acids
      Dithionic Acid
      Trithionic Acid
      Tetrathionic Acid
      Pentathionic Acid
      Wackenroders Solution
      Hexathionic Acid
      Polythionic Acids
      Sulphur Sesquioxide
      Hydrosulphurous Acid
      Nitrogen Sulphide
      Nitrogen Persulphide
      Nitrogen Pentasulphide
      Nitrogen Chlorosulphide
      Trithiazyl Chloride
      Thiotrithiazyl Chloride
      Dithiotetrathiazyl Chloride
      Nitrogen Bromosulphide
      Thiotrithiazyl Bromide
      Thiotrithiazyl Iodide
      Thiotrithiazyl Nitrate
      Thiotrithiazyl Hydrogen Sulphate
      Thiotrithiazyl Thiocyanate
      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
      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
      Azidodithiocarbonic Acid
      Cyanogen Monosulphide
      Cyanogen Trisulphide
      Sulphur Thiocyanate
      Disulphur Dithiocyanate
      Thiocyanic Acid
      Dithiocyanic Acid
      Trithiocyanuric Acid
      Perthiocyanic Acid

Sulphuryl Chloride, SO2Cl2

As would be expected, it is possible to obtain an Sulphuryl Chloride, SO2Cl2, corresponding with sulphuric acid, SO2(OH)2, but the chloride cannot be prepared by the action of phosphorus pentachloride on sulphuric acid or sulphur trioxide, these reagents yielding pyrosulphuryl chloride.

Formation and Preparation of Sulphuryl Chloride

Chlorine and sulphur dioxide will only unite under some accelerating influence. It was by the interaction of these gases in sunlight that sulphuryl chloride was first obtained by Regnault in 1838.

Bone charcoal or activated wood charcoal is a convenient accelerator, combination occurring instantly. If the vessel in which the reaction is carried out is cooled to 30° C., the sulphuryl chloride is condensed and may be drained away as rapidly as it is formed. The terpene hydrocarbons, especially pinene and limonene, also certain ethers, phenols and esters, are effective catalysts, as also is camphor.

The formation of sulphuryl chloride is favoured by low temperature and its decomposition by high temperature:

SO2 + Cl2SO2Cl2.

Both these reactions are .catalysed by the foregoing catalysts. For the efficient preparation of the chloride, the dry reacting gases are brought together at ordinary temperatures in the presence of a catalyst such as "Norit," a highly activated powdered carbon. The mixture is then cooled to -10° C. to ensure complete combination, filtered from the catalyst and carefully distilled, the heat being applied to the liquid for as short a time as possible.

At 120° C. in a sealed tube boron trichloride and sulphur trioxide react with formation of sulphuryl chloride:

2BCl3 + 4SO3 = 3SO2Cl2 + B2O3.SO3.

A convenient method for the laboratory preparation of sulphuryl chloride consists in boiling chlorosulphonic acid with about one per cent, of mercury or mercuric sulphate under a reflux condenser kept at a temperature of 70° C. in order to return to the flask any unchanged chlorosulphonic acid:

2Cl.SO2.OH = SO2Cl2 + H2SO4.

Any unchanged chlorosulphonic acid in the distillate can be removed by making use of its much more rapid hydrolysis with ice-cold water, the residual liquid being dried and redistilled.

Physical Properties

Sulphuryl chloride is a colourless, fuming liquid, with an extremely pungent odour. D204 = 1.6674; n20D = 1.4437. It boils at 69.1° C. at 760 mm. pressure, and freezes at -46° C. The vapour density is normal at first, but when the chloride is kept, even at 100° C., its vapour commences to dissociate into sulphur dioxide and chlorine. At 200° C. dissociation is almost complete. When dissolved in benzene the substance shows a molecular weight corresponding with SO2Cl2. At ordinary temperatures the specific heat is 0.233, the latent heat of evaporation 52.4 calories per gram, and the heat of formation from the elements approximately 89,540 calories per gram-molecule. The dielectric constant at 20° C. is 8.5. As a solvent, the ebullioscopic constant of sulphuryl chloride has been found to have

the value 45; salts dissolved in the chloride are found to undergo ionic dissociation.

Chemical Properties of Sulphuryl Chloride

At a dull red heat sulphuryl chloride vapour is completely decomposed into sulphur dioxide and chlorine. At 320° C. the reaction appears to be of the first order, proceeding entirely in the gas phase; at lower temperatures, however, reaction takes place on the wall of the containing vessel.

Water causes sulphuryl chloride to decompose into sulphuric and hydrochloric acids, but with only very little water, or better, with sulphuric acid, chlorosulphonic acid is obtained:

SO2Cl2 + 2H2O = H2SO4 + 2HCl.
SO2Cl2 + H2SO4 = 2Cl.SO2.OH.

At 200° C. sulphuryl chloride converts sulphur into monochloride, this result probably being preceded by dissociation of the sulphuryl chloride into chlorine and sulphur dioxide. In the presence of aluminium chloride this reaction can be effected even at the ordinary temperature, and aluminium chloride is favour the dissociation of sulphuryl chloride:

SO2Cl2 + 2S = S2Cl2 + SO2.

In the presence of aluminium chloride, iodine also reacts easily with sulphuryl chloride:

SO2Cl2 + 2I = SO2 + 2ICl,
2SO2Cl2 + 2ICl = 2SO2 + 2ICl3.

Hydrogen sulphide is attacked according to the equations:

H2S + SO2Cl2 = 2HCl + SO2 + S,
2H2S + SO2Cl2 = 2H2O + S2Cl2 + S;

whilst hydrogen bromide and hydrogen iodide are acted upon vigorously with formation of sulphur dioxide and the free halogen:

SO2Cl2 + 2HBr = SO2 + Br2 + 2HCl.

Phosphorus (red more readily than yellow), arsenic, antimony, mercury, iron, gold and platinum are converted into chlorides, with liberation of sulphur dioxide, e.g.

Hg + SO2Cl2 = HgCl2 + SO2;

with the mercury in excess:

2Hg + SO2Cl2 = 2HgCl + SO2.

In ether solution sulphuryl chloride reacts with zinc, giving zinc chloride and zinc sulphoxylate, ZnSO2.

Phosphorus pentachloride effects a gradual removal of one atom of oxygen from sulphuryl chloride, with formation of thionyl chloride,

PCl5 + SO2Cl2 = POCl3 + SOCl2 + Cl2,

whilst phosphorus trichloride yields the same products, excepting chlorine.

Lead dioxide is converted vigorously into lead chloride and sulphate by the vapour of sulphuryl chloride, oxygen being liberated, whilst mercuric oxide (red at 160° to 180° C., yellow at 150° C.) with excess of sulphuryl chloride gives mercuric chloride and sulphur trioxide:

HgO + SO2Cl2 = HgCl2 + SO3.

With excess of mercuric oxide, mercuric sulphate is also formed.

Selenium is attacked rapidly by sulphuryl chloride:

Se + 2SO2Cl2 = SeCl2 + 2SO2.

The chloride has no action on selenium dioxide even at high temperatures or under great pressure. Sulphuryl chloride reacts with tellurium; with the sulphuryl chloride in excess the reaction is:

Te + 2SO2Cl2 = TeCl2 + 2SO2,

whilst with the tellurium in excess, TeCl2 is obtained. Tellurium dioxide is not acted upon in the cold, but when heated in a sealed tube with the chloride a variety of crystalline products may be formed: 3TeO2.4SO2Cl2, 5TeO2.9SO2Cl2, TeO2.2SO2Cl2, and 2TeO2.5SO2Cl2.

The reaction between sulphuryl chloride and ammonia is complex, various products being obtained under different conditions; the products include iminosulphamide, NH2.SO2.NH.SO2.NH2, which behaves as a monobasic acid, trisulphimide and sulphomelide, both acidic substances of composition (SO2.NH)3, and sulphamide, SO2(NH2)2, which is also acidic.

Like thionyl chloride, sulphuryl chloride is able to replace the hydroxyl groups of organic substances by chlorine.


In view of the possibility of sexavalent sulphur, as demonstrated by the existence of sulphur hexafluoride, there is very little difficulty in accepting the formula for sulphuryl chloride.
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