Strontium sulfide

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title: "Strontium sulfide" type: doc version: 1 created: 2026-02-28 author: "Wikipedia contributors" status: active scope: public tags: ["strontium-compounds", "monosulfides", "rock-salt-crystal-structure"] topic_path: "general/strontium-compounds" source: "https://en.wikipedia.org/wiki/Strontium_sulfide" license: "CC BY-SA 4.0" wikipedia_page_id: 0 wikipedia_revision_id: 0

| Verifiedfields = changed | Watchedfields = changed | verifiedrevid = 432800585 | Reference= | ImageFile = NaCl polyhedra.png | IUPACName = | OtherNames = Strontium monosulfide C.I. 77847 |Section1={{Chembox Identifiers | CASNo_Ref = | CASNo = 1314-96-1 | ChemSpiderID = 8394912 | EC_number = 215-249-2 | UNII_Ref = | UNII = 06I13IA27T | PubChem = 14820 | InChI = 1S/S.Sr | StdInChIKey = XXCMBPUMZXRBTN-UHFFFAOYSA-N | SMILES = S=[Sr] |Section2={{Chembox Properties | Formula = SrS | MolarMass = 119.68 g/mol | Appearance = white solid (spoiled samples are colored) | Odor = none (degraded samples smell of hydrogen sulfide) | Density = 3.70 g/cm3 | MeltingPtC = 2002 | BoilingPt = | Solubility = slightly soluble | Solvent = acids | SolubleOther = decomposes | RefractIndex = 2.107 |Section3={{Chembox Structure | CrystalStruct = Halite (cubic), cF8 | SpaceGroup = Fm3m, No. 225 | Coordination = Octahedral (Sr2+); octahedral (S2−) | LattConst_a = |Section7={{Chembox Hazards | ExternalSDS = External MSDS | GHS_ref=https://pubchem.ncbi.nlm.nih.gov/compound/14820#section=Safety-and-Hazards | GHSPictograms = | GHSSignalWord = Danger | HPhrases = | PPhrases = | NFPA-H = | NFPA-F = | NFPA-R = | NFPA-S = |Section8={{Chembox Related | OtherAnions = Strontium oxide Strontium selenide | OtherCations = Magnesium sulfide Calcium sulfide Barium sulfide | OtherFunction = | OtherFunction_label = | OtherCompounds =

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.

Production and reactions

Strontium sulfide is produced by roasting celestine with coke at 1100–1300 °C. The sulfate is reduced, leaving the sulfide: :SrSO4 + 2 C → SrS + 2 CO2 About 300,000 tons are processed in this way annually.

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. :SrS + H2O + CO2 → SrCO3 + H2S :SrS + Na2CO3 → SrCO3 + Na2S Strontium nitrate can also be prepared in this way.

References

References

  1. [http://cameochemicals.noaa.gov/chemical/21036 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. "Celestine".
  4. (21 March 2011). "List of Minerals".
  5. (2006). "Dissolution kinetics of celestite (SrSO4) in HCl solution with BaCl2". Hydrometallurgy.
  6. Both luminous and nonluminous sulfide phases are known, impurities, defects, and dopants being important.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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strontium-compoundsmonosulfidesrock-salt-crystal-structure