Strontium sulfide

Strontium sulfide^[1]
Names
	Other names Strontium monosulfide; C.I. 77847
Identifiers
CAS Number	1314-96-1 ;
3D model (JSmol)	Interactive image;
ECHA InfoCard	100.013.864
PubChem CID	14820;
UNII	06I13IA27T ;
CompTox Dashboard (EPA)	DTXSID70927179 ;
	InChI InChI=1S/S.Sr;
	SMILES S=[Sr];
Properties
Chemical formula	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)
Solubility in water	slightly soluble
Solubility in acids	decomposes
Refractive index (nD)	2.107
Structure
Crystal structure	Halite (cubic), cF8
Space group	Fm3m, No. 225
Coordination geometry	Octahedral (Sr2+); octahedral (S2−)
Hazards
Safety data sheet (SDS)	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). verify (what is ?) Infobox references

Strontium sulfide is the inorganic compound with the formula Sr S. 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]

Production and reactions

Strontium sulfide is produced by roasting celestine with coke at 1100–1300 °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

^ Strontium sulfide, cameochemicals.noaa.gov
^ ^a ^b ^c 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.
^ "Celestine".
^ "List of Minerals". 21 March 2011.
^ ^a ^b 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. Bibcode:2006HydMe..84..239A. doi:10.1016/j.hydromet.2006.06.001.
^ 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

External links

Strontium Sulfide Info American Elements

[1] Strontium sulfide, cameochemicals.noaa.gov

[Ullmann-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.

[Celestine-3] "Celestine".

[IMA-4] "List of Minerals". 21 March 2011.

[hydrometallurgy-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. Bibcode:2006HydMe..84..239A. 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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