Nowadays, Barium sulfide is a topic that is becoming more and more relevant in our society. Since its appearance, it has generated great interest and debate among experts and the general population. Over time, Barium sulfide has become a key element in different areas, from politics to popular culture. Its influence has become evident in various manifestations, causing a significant impact on the way we relate, communicate and make decisions. In this article, we will explore in depth the implications of Barium sulfide and its impact on our daily lives.
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 |
Melting point | 2,235 °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)
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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)
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226 mg/kg humans |
Related compounds | |
Other anions
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Barium oxide |
Other cations
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Magnesium sulfide Calcium sulfide Strontium sulfide |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C , 100 kPa).
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Barium sulfide is the inorganic compound with the formula BaS. BaS is the barium compound produced on the largest scale. It is an important precursor to other barium compounds including BaCO3 and the pigment lithopone, ZnS/BaSO4. Like other chalcogenides of the alkaline earth metals, BaS is a short wavelength emitter for electronic displays. It is colorless, although like many sulfides, it is commonly obtained in impure colored forms.
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). 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.
According to Harvey (1957), 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. The phosphorescence of the material obtained by Casciarolo made it a curiosity.
A modern procedure proceeds from barium carbonate:
BaS crystallizes with the NaCl structure, featuring octahedral Ba2+ and S2− centres.
The observed melting point of barium sulfide is highly sensitive to impurities.
BaS is quite poisonous, as are related sulfides, such as CaS, which evolve toxic hydrogen sulfide upon contact with water.