Chemistry:Barium sulfide

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Short description: Chemical compound
Not to be confused with Barium sulfate.
Barium sulfide
Identifiers
3D model (JSmol)
ChEBI
ChemSpider
EC Number
  • 244-214-4
13627
UNII
UN number UN3134
Properties[2]
BaS
Molar mass 169.39 g·mol−1
Appearance White solid
Odor Rotten-egg like[1]
Density 4.3 g/cm3 (20 °C (68 °F))
Melting point 2,235 °C (4,055 °F; 2,508 K)[3]
Boiling point decomposes
  • 8.94 g/100 mL (25 °C (77 °F))
  • Reacts (100 °C (212 °F))
10.86
Structure[4]
Halite (cubic), cF8
Fm3m, No. 225
m3m
a = 6.45 Å, b = 6.45 Å, c = 6.45 Å
α = 90°, β = 90°, γ = 90°
268.50 Å3
4
  • Octahedral (Ba2+)
  • Octahedral (S2−)
Thermochemistry[2]
49.4 J.mol-1.K-1
78.2 J.mol-1.K-1
−460.0 kJ⋅mol−1
−456.0 kJ⋅mol−1
Enthalpy of fusion (ΔfH⦵fus)
 63 kJ⋅mol−1
Hazards
GHS pictograms GHS06: ToxicGHS07: HarmfulGHS09: Environmental hazard
GHS Signal word Danger
H290, H301, H314, H332, H400
P234, P260, P264, P270, P271, P273, P280, P301+310+330Script error: No such module "Preview warning".Category:GHS errors, P301+330+331, P303+361+353, P304+340+310, P305+351+338+310, P363, P390, P391, P405, P501
NFPA 704 (fire diamond)
0.5 mg/m3 (as Ba)[5] (TWA)
Lethal dose or concentration (LD, LC):
271 mg/kg (rat, oral)
NIOSH (US health exposure limits):[1]
PEL (Permissible)
 0.5 mg/m3
REL (Recommended)
 0.5 mg/m3
IDLH (Immediate danger)
 50 mg/m3
Related compounds
Other anions
Other cations
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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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.[6] It is an important precursor to other barium compounds including barium carbonate and the pigment lithopone, ZnS/BaSO
4.[7] Like other chalcogenides of the alkaline earth metals, BaS is a short wavelength emitter for electronic displays.[8] 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 barium sulfate (BaSO
4, available as the mineral barite).[9] 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:

BaSO
4 + 2 C → BaS + 2 CO
2

and also:

BaSO
4 + 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 (BaCO
3), a source material for many commercial barium compounds.[10]

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.[11] After grinding and heating the mineral with charcoal under reducing conditions, he obtained a persistent luminescent material that soon came to be known as Lapis Boloniensis, or Bolognian stone.[12][13] The phosphorescence of the material obtained by Casciarolo made it a curiosity.[14][15][16]

Preparation

A modern procedure proceeds from barium carbonate and hydrogen sulfide (H
2S) at 100 °C (212 °F):[17]

BaCO
3 + H
2S ΔHTemplate:Arrow BaS + H
2O + CO
2

It may also be prepared by direct calcination of the elements in a ratio of 1:1.05 (Barium:Sulfur) in an inert atmosphere:[18]

Ba + S ΔHTemplate:Arrow BaS

Various other barium sulfides are produced when an excess of sulfur is used depending on the ratio.[18]

Properties

The observed melting point of barium sulfide is highly sensitive to impurities.[3]

Safety

BaS is poisonous by ingestion or inhalation, as are other water soluble or acid-reactive barium compounds. It evolves toxic hydrogen sulfide gas on contact with acids or high temperature water.

Acute barium poisoning through ingestion or inhalation of large amounts causes a rapid onset of gastrointestinal symptoms and hypoalkemia. Chronic exposure may cause adverse renal effects. It is believed that the mechanism of toxicity may be due to the action of barium as a competive potassium channel antagonist, which shifts extracellular potassium to intracellular resultsing in a diminished ability of nerve cells to respond to stimulation.[19]

References

  1. ↑ 1.0 1.1 1.2 "SDS - Barium sulfide" (pdf). ThermoFisher Scientific. 24 December 2025. https://www.fishersci.com/store/msds?partNumber=AA1284818&productDescription=BARIUM+SULFIDE+50G&vendorId=VN00024248&countryCode=US&language=en. 
  2. ↑ 2.0 2.1 Template:RubberBible97th
  3. ↑ 3.0 3.1 Stinn, Caspar; Nose, Katsuhiro; Okabe, Toru; Allanore, Antoine (December 2017). "Experimentally Determined Phase Diagram for the Barium Sulfide-Copper(I) Sulfide System Above 873 K (600 °C)". Metallurgical and Materials Transactions B 48 (6): 2922–2929. doi:10.1007/s11663-017-1107-5. 
  4. ↑ "Materials Data on BaS". Lawrence Berkeley National Laboratory (LBNL), Berkeley, CA: LBNL Materials Project. 13 July 2020. doi:10.17188/1190987. https://next-gen.materialsproject.org/materials/mp-1500. 
  5. ↑ 5.0 5.1 Sigma-Aldrich Co., Barium sulfide.
  6. ↑ Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. p. 678. ISBN 978-0-08-037941-8. 
  7. ↑ Holleman, Arnold Frederik; Wiberg, Egon (2001), Wiberg, Nils, ed., Inorganic Chemistry, San Diego/Berlin: Academic Press/De Gruyter, ISBN 0-12-352651-5 
  8. ↑ 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. 
  9. ↑ 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
  10. ↑ 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. 
  11. ↑ Harvey, E. Newton (1957). "1 - Far Eastern and Classical Antiquity". A History of Luminescence from the Earliest Times Until 1900. Memoirs of the American Philosophical Society. 44. Philadelphia, PA: The American Philosophical Society. pp. 11-43. OCLC 390708. https://archive.org/details/historyoflumines00harv/page/10/mode/2up. 
  12. ↑ 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. 
  13. ↑ Hardev Singh Virk (2014). "History of Luminescence from Ancient to Modern Times". ResearchGate. https://www.researchgate.net/publication/259713568. 
  14. ↑ "Lapis Boloniensis". www.zeno.org. http://www.zeno.org/Lemery-1721/A/Lapis+Boloniensis. 
  15. ↑ Lemery, Nicolas (1714). Trait℗e universel des drogues simples. https://books.google.com/books?id=K25AAAAAcAAJ&pg=PA458. 
  16. ↑ Ozanam, Jacques; Montucla, Jean Etienne; Hutton, Charles (1814). Recreations in mathematics and natural philosophy ... https://books.google.com/books?id=jAYAAAAAQAAJ&pg=PA411. 
  17. ↑ Ehrlich, P. (1963). "17. Alkaline Earth Metals". Handbook of Preparative Inorganic Chemistry. 1 (2 ed.). New York, NY: Academic Press. p. 968-9. OCLC 843200092. https://archive.org/details/Handbook_of_Preparative_Inorganic_Chemistry_1_2_Brauer/page/n962/mode/1up. 
  18. ↑ 18.0 18.1 Ropp, R.C. (6 March 2013). "Group 16 (O, S, Se, Te) Alkaline Earth Compounds". Encyclopedia of the Alkaline Earth Compounds. Aalborg, Denmark: Elsevier A/S. pp. 105–197. doi:10.1016/B978-0-444-59550-8.00003-X. ISBN 9780444595508. https://www.sciencedirect.com/topics/chemistry/barium-sulfides. 
  19. ↑ "Barium | Medical Management Guidelines | Toxic Substance Portal | ATSDR". Agency for Toxic Substances and Disease Registry. https://wwwn.cdc.gov/tsp/MMG/MMGDetails.aspx?mmgid=321&toxid=57. 



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