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Chemical compound From Wikipedia, the free encyclopedia
Barium sulfide is the inorganic compound with the formula BaS. BaS is the barium compound produced on the largest scale.[3] It is an important precursor to other barium compounds including BaCO3 and the pigment lithopone, ZnS/BaSO4.[4] Like other chalcogenides of the alkaline earth metals, BaS is a short wavelength emitter for electronic displays.[5] It is colorless, although like many sulfides, it is commonly obtained in impure colored forms.
Identifiers | |
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3D model (JSmol) |
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ChEBI | |
ChemSpider | |
ECHA InfoCard | 100.040.180 |
EC Number |
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13627 | |
PubChem CID |
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UNII | |
CompTox Dashboard (EPA) |
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Properties | |
BaS | |
Molar mass | 169.39 g/mol |
Appearance | white solid |
Density | 4.25 g/cm3 [1] |
Melting point | 2,235[2] °C (4,055 °F; 2,508 K) |
Boiling point | decomposes |
2.88 g/100 mL (0 °C) 7.68 g/100 mL (20 °C) 60.3 g/100 mL (100 °C) (reacts) | |
Solubility | insoluble in alcohol |
Refractive index (nD) |
2.155 |
Structure | |
Halite (cubic), cF8 | |
Fm3m, No. 225 | |
Octahedral (Ba2+); octahedral (S2−) | |
Hazards | |
GHS labelling: | |
Warning | |
H315, H319, H335, H400 | |
P261, P264, P271, P273, P280, P302+P352, P304+P340, P305+P351+P338, P312, P321, P332+P313, P337+P313, P362, P391, P403+P233, P405, P501 | |
NFPA 704 (fire diamond) | |
Lethal dose or concentration (LD, LC): | |
LD50 (median dose) |
226 mg/kg humans |
Related compounds | |
Other anions |
Barium oxide Barium selenide Barium telluride Barium polonide |
Other cations |
Beryllium sulfide Magnesium sulfide Calcium sulfide Strontium sulfide Radium sulfide |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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BaS was prepared by the Italian alchemist Vincenzo Cascariolo (also known as Vincentius or Vincentinus Casciarolus or Casciorolus, 1571–1624) via the thermo-chemical reduction of BaSO4 (available as the mineral barite).[6] It is currently manufactured by an improved version of Cascariolo's process using coke in place of flour and charcoal. This kind of conversion is called a carbothermic reaction:
and also:
The basic method remains in use today. BaS dissolves in water. These aqueous solutions, when treated with sodium carbonate or carbon dioxide, give a white solid of barium carbonate, a source material for many commercial barium compounds.[7]
According to Harvey (1957),[8] in 1603, Vincenzo Cascariolo used barite, found at the bottom of Mount Paterno near Bologna, in one of his non-fruitful attempts to produce gold. After grinding and heating the mineral with charcoal under reducing conditions, he obtained a persistent luminescent material rapidly called Lapis Boloniensis, or Bolognian stone.[9][10] The phosphorescence of the material obtained by Casciarolo made it a curiosity.[11][12][13]
A modern procedure proceeds from barium carbonate:[14]
BaS crystallizes with the NaCl structure, featuring octahedral Ba2+ and S2− centres.
The observed melting point of barium sulfide is highly sensitive to impurities.[2]
BaS is quite poisonous, as are related sulfides, such as CaS, which evolve toxic hydrogen sulfide upon contact with water.
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