Barium sulfide

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Not to be confused with Barium sulfate.
Barium sulfide
Identifiers
3D model (JSmol)
ChEBI
ChemSpider
ECHA InfoCard 100.040.180 Edit this at Wikidata
EC Number
  • 244-214-4
13627
UNII
  • InChI=1S/Ba.S/q+2;-2 checkY
    Key: CJDPJFRMHVXWPT-UHFFFAOYSA-N checkY
  • InChI=1/Ba.S/q+2;-2
    Key: CJDPJFRMHVXWPT-UHFFFAOYAO
  • [Ba+2].[S-2]
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
2.155
Structure
Halite (cubic), cF8
Fm3m, No. 225
Octahedral (Ba2+); octahedral (S2−)
Hazards
GHS labelling:
GHS07: Exclamation markGHS09: Environmental hazard
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)
NFPA 704 four-colored diamondHealth 2: Intense or continued but not chronic exposure could cause temporary incapacitation or possible residual injury. E.g. chloroformFlammability 3: Liquids and solids that can be ignited under almost all ambient temperature conditions. Flash point between 23 and 38 °C (73 and 100 °F). E.g. gasolineInstability 2: Undergoes violent chemical change at elevated temperatures and pressures, reacts violently with water, or may form explosive mixtures with water. E.g. white phosphorusSpecial hazards (white): no code
2
3
2
Lethal dose or concentration (LD, LC):
226 mg/kg humans
Related compounds
Other anions
 Barium oxide
Other cations
 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).
checkY verify (what is checkY☒N ?)

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 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

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

BaS is quite poisonous, as are related sulfides, such as CaS, which evolve toxic hydrogen sulfide upon contact with water.

References

  1. ^ Lide, David R., ed. (2006). CRC Handbook of Chemistry and Physics (87th ed.). Boca Raton, FL: CRC Press. ISBN 0-8493-0487-3.
  2. ^ 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
  3. ^ Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 978-0-08-037941-8.
  4. ^ Holleman, A. F.; Wiberg, E. "Inorganic Chemistry" Academic Press: San Diego, 2001. ISBN 0-12-352651-5.
  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. Proceedings of SPIE. Vol. 1523. pp. 608–612. Bibcode:1992SPIE.1523..608V. doi:10.1117/12.634082.
  6. ^ 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
  7. ^ 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.
  8. ^ 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.
  9. ^ 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.
  10. ^ Hardev Singh Virk (2014). "History of Luminescence from Ancient to Modern Times". ResearchGate. Retrieved 6 March 2021.
  11. ^ "Lapis Boloniensis". www.zeno.org. Archived from the original on 2012-10-23. Retrieved 2011-01-03.
  12. ^ Lemery, Nicolas (1714). Trait℗e universel des drogues simples.
  13. ^ Ozanam, Jacques; Montucla, Jean Etienne; Hutton, Charles (1814). Recreations in mathematics and natural philosophy .
  14. ^ P. Ehrlich (1963). "Alkaline Earth Metals". In G. Brauer (ed.). Handbook of Preparative Inorganic Chemistry, 2nd Ed. Vol. 2pages=937. NY, NY: Academic Press.
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