Chemical elements
    Physical Properties
    Chemical Properties
      Barium Hydride
      Barium Subfluoride
      Barium Fluoride
      Acid Barium Fluoride
      Barium Subchloride
      Barium Chloride
      Barium Bromide
      Barium Perbromides
      Barium Iodide
      Barium Periodides
      Barium Mixed Halides
      Barium Mixed Perhalides
      Barium Oxychloride
      Barium Hypochlorite
      Barium Chlorite
      Barium Chlorate
      Barium Perchlorate
      Barium Oxybromide
      Barium Hypobromite
      Barium Bromate
      Barium Perbromate
      Barium Oxyiodide
      Barium Iodate
      Barium Periodate
      Barium Manganites
      Barium Manganate
      Barium Permanganate
      Barium Suboxide
      Barium Oxide
      Barium Hydroxide
      Barium Peroxide
      Barium Peroxyhydrate
      Barium Tetroxide
      Barium Sulphide
      Barium Hydrosulphide
      Barium Polysulphides
      Barium Hydroxyhydrosulphide
      Barium Oxysulphides
      Barium Sulphite
      Barium Thiosulphate
      Barium Dithionate
      Barium Trithionate
      Barium Tetrathionate
      Barium Pentathionate
      Barium Sulphate
      Acid Barium Sulphates
      Barium Pyrosulphate
      Barium Persulphate
      Barium Selenide
      Barium Selenite
      Barium Selenate
      Acid Barium Selenate
      Barium Telluride
      Barium Tellurite
      Barium Tellurate
      Barium Chromite
      Barium Chromate
      Barium Dichromate
      Barium Potassium Trichromate
      Barium Chlorochromate
      Barium Perchromate
      Barium Molybdate
      Barium Permolybdate
      Barium Tungstate
      Barium Uranate
      Barium Diuranate
      Barium Peruranate
      Barium Nitride
      Barium Azide
      Barium Hexammoniate
      Barium Ammonium
      Barium Amide
      Barium Amidosulphonate
      Barium Imide
      Barium Imidosulphonate
      Barium Hyponitrite
      Barium Nitroxysulphite
      Barium Nitrososulphate
      Barium Nitrohydroxylaminate
      Barium Nitrite
      Barium Nitrate
      Barium Phosphide
      Barium Dihydrohypophosphite
      Barium Hydrophosphite
      Barium Hypophosphate
      Barium Orthophosphates
      Barium Pyrophosphate
      Barium Metaphosphate
      Basic Barium Phosphates
      Barium Thiophosphites
      Barium Thiophosphates
      Barium Selenophosphates
      Barium Azophosphates
      Barium Phosphimates
      Barium Arsenide
      Barium Orthoarsenite
      Barium Pyroarsenite
      Barium Orthoarsenates
      Barium Pyroarsenate
      Barium Thioarsenites
      Barium Thioarsenates
      Barium Sodium Selenoxyarsenate
      Barium Metantimonate
      Barium Thioantimonites
      Barium Chloroantimonite
      Barium Orthothioantimonate
      Barium Hypovanadate
      Barium Vanadates
      Barium Metapervanadate
      Barium Niobate
      Barium Tantalate
      Barium Pertantalate
      Barium Carbide
      Barium Carbonyl
      Barium Formate
      Barium Acetate
      Barium Oxalate
      Barium Carbonate
      Barium Thiocarbonate
      Barium Percarbonate
      Barium Cyanide
      Barium Cyanamide
      Barium Cyanate
      Barium Cyanurate
      Barium Thiocyanate
      Barium Selenocyanate
      Barium Silicide
      Barium Silicates
      Barium Fluosilicate
      Barium Stannate
      Barium Orthoplumbate
      Barium Titanate
      Barium Peroxide Pertitanate
      Barium Pertitanate
      Barium Fluoroxytitanate
      Barium Zirconate
      Barium Boride
      Barium Borates
      Barium Fluorborate
      Barium Perborate
      Barium Aluminates
      Barium Ferrite
      Barium Ferrate
      Barium Gobaltite
      Barium Dinickelite
      Barium Platinate
    Detection of Barrium
    PDB 1djh-3iqp
    PDB 3iqr-4e7y

Barium Sulphide, BaS

Barium Sulphide, BaS, may be formed by the action of sulphuretted hydrogen on the hydroxide at 85° C., with subsequent heating in hydrogen at 200° C., on barium carbonate at red heat, or, finally, on the sulphate at 1200° C., in all three cases cooling in hydrogen. It may also be obtained by the action of carbon disulphide on barium carbonate.

BaCO3 + 2CS2 = BaS + 3CO + 3S.

Polysulphides are always formed in this case, but may be reduced to the sulphide by heating in a current of hydrogen.

The method employed for the technical production of barium sulphide is the reduction of barytes by carbon or reducing gases. The sulphide thus formed is the starting-point for the production of all other commercial barium compounds. Laboratory tests indicate that a high temperature for a short time produces a more satisfactory yield than a low temperature with prolonged heating. Good results are obtained with 15-16 per cent, of carbon in muffles at 1000°-1100° C.

Barium sulphide as usually obtained is a greyish white amorphous powder, but after fusion in the electric furnace it forms cubic crystals of density 4.25. The heat of formation is 105.2 Cal.

On exposure to air it turns yellow. It is not reduced by hydrogen at 1200° C., but is readily attacked by halogens and is completely transformed into the sulphate by oxygen at high temperatures. It is attacked by gaseous acids in the cold. Carbon decomposes it at the temperature of the electric arc forming the carbide. Oxidising agents react with incandescence. When it is heated in water vapour, hydrogen and barium sulphate are formed. It is attacked by concentrated nitric acid with incandescence, and reacts with phosphorus trichloride forming barium chloride and phosphorus trisulphide. On heating with an equal quantity of barium chloride it forms an opaque red mass. In general, the crystallised sulphide is less readily attacked than the amorphous.

Barium sulphide is readily soluble in water with hydrolysis, forming the hydroxide and hydrosulphide. The heat of solution is 7.3 Cal. If the aqueous solution be concentrated in vacuo in the presence of free sulphur, a hydrated sulphide, BaS.6H2O, crystallising in hexagonal plates, is obtained. When slowly heated it loses water between 100° and 300° C., and then sulphuretted hydrogen and sulphur.

It is insoluble in alcohol.

A dark red double barium nickel sulphide, BaS.4NiS has been obtained.

Phosphorescent Barium Sulphide

Barium sulphide, under the name of Bolognian phosphorus,11 was the first of the alkaline earth sulphides in which the property of phosphorescence was observed. The conditions affecting the phosphorescence of these sulphides have already been discussed under calcium sulphide.
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