Barium sulfide

Not to be confused with Barium sulfate.
Barium sulfide
Identifiers
CAS number 21109-95-5 Y
PubChem 6857597
ChemSpider 5256933 Y
EC number 244-214-4
ChEBI CHEBI:32590 Y
Jmol-3D images Image 1
Properties
Molecular formula BaS
Molar mass 169.39 g/mol
Density 4.25 g/cm3 [1]
Melting point

1200 °C
Boiling point

decomposes
Solubility in water 2.88 g/cm3 (0 °C)
7.68 g/cm3 (20 °C)
60.3 g/100 mL (100 °C)
Solubility insoluble in alcohol
Refractive index (nD) 2.155
Structure
Crystal structure Halite (cubic), cF8
Space group Fm3m, No. 225
Coordination
geometry		 Octahedral (Ba2+); octahedral (S2–)
Hazards
EU Index 016-002-00-X
EU classification Harmful (Xn)
Dangerous for the environment (N)
R-phrases R20/22, R31, R50
S-phrases (S2), S28, S61
NFPA 704
3
2
0
Related compounds
Other anions Barium oxide
Other cations Magnesium sulfide
Calcium sulfide
Strontium sulfide
 Y (verify) (what is: Y/N?)
Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa)
Infobox references

Barium sulfide is the inorganic compound with the formula BaS. BaS is an important precursor to other barium compounds including BaCO3 and the pigment lithopone, ZnS/BaSO4.[2] Like other chalcogenides of the alkaline earth metals, BaS is a short wavelength emitters for electronic displays.[3] It is colorless, although like many sulfides, it is commonly obtained in impure colored forms.

Discovery, production, properties

The BaS was prepared by Vincentius (or Vincentinus) Casciarolus (or Casciorolus, 1571-1624) via reduction of BaSO4 (available as the mineral barite).[4] It is currently manufactured by an improved version of Casciarolus's route using coke in place of flour. This kind of conversion is called a carbothermic reaction:

BaSO4 + 2 C → BaS + 2 CO2

The phosphorescence of the substance made the material a curiosity and various alchemists and chemists made experiments with the material which was known as Lapis Boloniensis, Chrysolapis or bologna stone.[5][6][7]

Andreas Sigismund Marggraf showed that calcite and gypsum were not very suitable for the production of the bologna stone, but a special heavy fluorspar, in the end he concluded that calcium sulfate is the material from which the bologna stone is made.[8]

BaS crystallizes with the NaCl structure, featuring octahedral Ba2+ and S2- centres.

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. ^ Holleman, A. F.; Wiberg, E. "Inorganic Chemistry" Academic Press: San Diego, 2001. ISBN 0-12-352651-5.
  3. ^ Vij, D. R.; Singh, N. "Optical and electrical properties of II-VI wide gap semiconducting barium sulfide" Proceedings of SPIE (1992), 1523 (Conf. Phys. Technol. Semicond. Devices Integr. Circuits, 1992), 608-12.
  4. ^ 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
  5. ^ "Lapis Boloniensis". www.zeno.org. http://www.zeno.org/Lemery-1721/A/Lapis+Boloniensis. 
  6. ^ Lemery, Nicolas (1714). Trait℗e universel des drogues simples. http://books.google.de/books?id=K25AAAAAcAAJ&pg=PA458#v=onepage&q&f=false. 
  7. ^ Ozanam, Jacques; Montucla, Jean Etienne; Hutton, Charles (1814). Recreations in mathematics and natural philosophy ... http://books.google.de/books?id=jAYAAAAAQAAJ&pg=PA411. 
  8. ^ Marggraf, Andreas Sigismund (1767). Chymische Schriften. http://books.google.de/books?id=Obc5AAAAcAAJ&pg=PA113.