Strontium sulfide

Strontium sulfide is the inorganic compound with the formula SrS. It is a white solid. The compound is an intermediate in the conversion of strontium sulfate, the main strontium ore called celestite (or, more correctly, celestine), to other more useful compounds.[2][3][4]

Strontium sulfide[1]
Names
Other names
Strontium monosulfide
C.I. 77847
Identifiers
3D model (JSmol)
ECHA InfoCard 100.013.864
UNII
Properties
SrS
Molar mass 119.68 g/mol
Appearance white solid (spoiled samples are colored)
Odor none (degraded samples smell of hydrogen sulfide)
Density 3.70 g/cm3
Melting point 2,002 °C (3,636 °F; 2,275 K)
slightly soluble
Solubility in acids decomposes
2.107
Structure
Halite (cubic), cF8
Fm3m, No. 225
Octahedral (Sr2+); octahedral (S2−)
Hazards
Safety data sheet External MSDS
Related compounds
Other anions
 Strontium oxide
Other cations
 Magnesium sulfide
Calcium sulfide
Barium sulfide
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
N verify (what is YN ?)
Infobox references

Production and reactions

Strontium sulfide is produced by roasting celestine with coke at 110–1300 °C.[5] The sulfate is reduced, leaving the sulfide:

SrSO4 + 2 C → SrS + 2 CO2

About 300,000 tons are processed in this way annually.[2] Both luminous and nonluminous sulfide phases are known, impurities, defects, and dopants being important.[6]

As expected for a sulfide salt of alkaline earth, the sulfide hydrolyzes readily:

SrS + 2 H2O → Sr(OH)2 + H2S

For this reason, samples of SrS have an odor of rotten eggs.

Similar reactions are used in the production of commercially useful compounds, including the most useful strontium compound, strontium carbonate: a mixture of strontium sulfide with either carbon dioxide gas or sodium carbonate leads to formation of a precipitate of strontium carbonate.[2][5]

SrS + H2O + CO2 → SrCO3 + H2S
SrS + Na2CO3 → SrCO3 + Na2S

Strontium nitrate can also be prepared in this way.

References
  1. Strontium sulfide, cameochemicals.noaa.gov
  2. J. Paul MacMillan, Jai Won Park, Rolf Gerstenberg, Heinz Wagner, Karl Köhler, Peter Wallbrecht “Strontium and Strontium Compounds” in Ullmann's Encyclopedia of Industrial Chemistry 2002, Wiley-VCH, Weinheim. doi:10.1002/14356007.a25_321.
  3. https://www.mindat.org/min-927.html
  4. https://www.ima-mineralogy.org/Minlist.htm
  5. Aydoğan, Salih; Erdemoğlu, Murat; Aras, Ali; Uçar, Gökhan; Özkan, Alper (2006). "Dissolution kinetics of celestite (SrSO4) in HCl solution with BaCl2". Hydrometallurgy. 84 (3–4): 239–246. doi:10.1016/j.hydromet.2006.06.001.
  6. R. Ward, R. K. Osterheld, R. D. Rosenstein "Strontium Sulfide and Selenide Phosphors" Inorganic Syntheses, 1950, vol. III, pp. 11–24. doi:10.1002/9780470132340.ch4


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