Chemistry:Barium sulfide
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| Identifiers | |
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3D model (JSmol)
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| ChEBI | |
| ChemSpider | |
| EC Number |
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| 13627 | |
PubChem CID
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| UNII | |
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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 pictograms |  
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| GHS Signal word | Warning |
| H315, H319, H335, H400 | |
| P261, P264, P271, P273, P280, P302+352, P304+340, P305+351+338, P312, P321, P332+313, P337+313, P362, P391, P403+233, 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 [77 °F], 100 kPa). | |
 verify (what is   ?)
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| Infobox references | |
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
BaS was prepared by the Italian alchemist 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 Casciarolus's process using coke in place of flour and charcoal. This kind of conversion is called a carbothermic reaction:
- BaSO4 + 2 C → BaS + 2 CO2
and also:
- BaSO4 + 4 C → BaS + 4 CO
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
A modern procedure proceeds from barium carbonate:[14]
- BaCO
3 + H
2S → BaS + H
2O + CO
2
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
BaS is quite poisonous, as are related sulfides, such as CaS, which evolve toxic hydrogen sulfide upon contact with water.
References
- ↑ Lide, David R., ed (2006). CRC Handbook of Chemistry and Physics (87th ed.). Boca Raton, FL: CRC Press. ISBN 0-8493-0487-3.
- ↑ 2.0 2.1 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
- ↑ 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.
- ↑ Vij, D. R.; Singh, N. (1992). "Optical and electrical properties of II-VI wide gap semiconducting barium sulfide". Conf. Phys. Technol. Semicond. Devices Integr. Circuits, 1992. 1523. 608–612. doi:10.1117/12.634082. Bibcode: 1992SPIE.1523..608V.
- ↑ 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
- ↑ Kresse, Robert; Baudis, Ulrich; Jäger, Paul; Riechers, H. Hermann; Wagner, Heinz; Winkler, Jochen; Wolf, Hans Uwe (2007). "Ullmann's Encyclopedia of Industrial Chemistry". Ullmann's Encyclopedia of Industrial Chemistry. Weinheim: Wiley-VCH. doi:10.1002/14356007.a03_325.pub2.
- ↑ 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. doi:10.3390/ma3042834. ISSN 1996-1944. Bibcode: 2010Mate....3.2834S.
- ↑ Hardev Singh Virk (2014). "History of Luminescence from Ancient to Modern Times". ResearchGate. https://www.researchgate.net/publication/259713568.
- ↑ "Lapis Boloniensis". www.zeno.org. http://www.zeno.org/Lemery-1721/A/Lapis+Boloniensis.
- ↑ Lemery, Nicolas (1714). Trait℗e universel des drogues simples. https://books.google.com/books?id=K25AAAAAcAAJ&pg=PA458.
- ↑ Ozanam, Jacques; Montucla, Jean Etienne; Hutton, Charles (1814). Recreations in mathematics and natural philosophy ... https://books.google.com/books?id=jAYAAAAAQAAJ&pg=PA411.
- ↑ P. Ehrlich (1963). "Alkaline Earth Metals". in G. Brauer. Handbook of Preparative Inorganic Chemistry, 2nd Ed.. 2pages=937. NY, NY: Academic Press.
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