Barium sulfide
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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)
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2.155 |
Structure | |
Halite (cubic), cF8 | |
Fm3m, No. 225 | |
Octahedral (Ba2+); octahedral (S2−) | |
Hazards | |
GHS labelling: | |
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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 Barium selenide Barium telluride Barium polonide |
Other cations
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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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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.
Discovery
[edit]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:
- BaSO4 + 2C → BaS + 2CO2
and also:
- BaSO4 + 4C → BaS + 4CO
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]
Preparation
[edit]A modern procedure proceeds from barium carbonate:[14]
- BaCO3 + H2S → BaS + H2O + CO2
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]
Safety
[edit]BaS is quite poisonous, as are related sulfides, such as CaS, which evolve toxic hydrogen sulfide upon contact with water.
References
[edit]- ^ Lide, David R., ed. (2006). CRC Handbook of Chemistry and Physics (87th ed.). Boca Raton, FL: CRC Press. ISBN 0-8493-0487-3.
- ^ a b Stinn, C., Nose, K., Okabe, T. et al. Metall and Materi Trans B (2017) 48: 2922. https://doi.org/10.1007/s11663-017-1107-5 Archived 2024-01-01 at the Wayback Machine
- ^ Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 978-0-08-037941-8.
- ^ Holleman, A. F.; Wiberg, E. "Inorganic Chemistry" Academic Press: San Diego, 2001. ISBN 0-12-352651-5.
- ^ Proceedings of SPIE. Vol. 1523. pp. 608–612. Bibcode:1992SPIE.1523..608V. doi:10.1117/12.634082.
- ^ F. Licetus, Litheosphorus, sive de lapide Bononiensi lucem in se conceptam ab ambiente claro mox in tenebris mire conservante, Utini, ex typ. N. Schiratti, 1640. See http://www.chem.leeds.ac.uk/delights/texts/Demonstration_21.htm Archived 2011-08-13 at the Wayback Machine
- ^ Kresse, Robert; Baudis, Ulrich; Jäger, Paul; Riechers, H. Hermann; Wagner, Heinz; Winkler, Jochen; Wolf, Hans Uwe (2007). "Barium and Barium Compounds". Ullmann's Encyclopedia of Industrial Chemistry. Weinheim: Wiley-VCH. doi:10.1002/14356007.a03_325.pub2. ISBN 978-3527306732.
- ^ Harvey E. Newton (1957). A History of Luminescence: From the Earliest Times until 1900. Memoirs of the American Physical Society, Philadelphia, J. H. FURST Company, Baltimore, Maryland (USA), Vol. 44, Chapter 1, pp. 11-43.
- ^ Smet, Philippe F.; Moreels, Iwan; Hens, Zeger; Poelman, Dirk (2010). "Luminescence in Sulfides: A Rich History and a Bright Future". Materials. 3 (4): 2834–2883. Bibcode:2010Mate....3.2834S. doi:10.3390/ma3042834. hdl:1854/LU-1243707. ISSN 1996-1944.
- ^ Hardev Singh Virk (2014). "History of Luminescence from Ancient to Modern Times". ResearchGate. Retrieved 6 March 2021.
- ^ "Lapis Boloniensis". www.zeno.org. Archived from the original on 2012-10-23. Retrieved 2011-01-03.
- ^ Lemery, Nicolas (1714). Trait℗e universel des drogues simples.
- ^ Ozanam, Jacques; Montucla, Jean Etienne; Hutton, Charles (1814). Recreations in mathematics and natural philosophy .
- ^ P. Ehrlich (1963). "Alkaline Earth Metals". In G. Brauer (ed.). Handbook of Preparative Inorganic Chemistry, 2nd Ed. Vol. 2pages=937. NY, NY: Academic Press.