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{{chembox |
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| verifiedrevid = 382666003 |
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| verifiedrevid = 432800585 |
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| Reference=<ref>, cameochemicals.noaa.gov</ref> |
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| Reference=<ref>, cameochemicals.noaa.gov</ref> |
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| ImageFile = NaCl polyhedra.png |
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| ImageFile = NaCl polyhedra.png |
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| IUPACName = |
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| IUPACName = |
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| OtherNames = Strontium monosulfide<br/>C.I. 77847 |
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| OtherNames = Strontium monosulfide<br/>C.I. 77847 |
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| Section1 = {{Chembox Identifiers |
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|Section1={{Chembox Identifiers |
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| CASNo_Ref = {{cascite|correct|CAS}} |
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| CASNo = 1314-96-1 |
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| CASNo = 1314-96-1 |
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| CASNo_Ref = {{cascite}} |
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| UNII_Ref = {{fdacite|correct|FDA}} |
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| PubChem = |
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| UNII = 06I13IA27T |
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| PubChem = 14820 |
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| InChI = 1S/S.Sr |
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| SMILES = S= |
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| Section2 = {{Chembox Properties |
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|Section2={{Chembox Properties |
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| Formula = SrS |
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| Formula = SrS |
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| MolarMass = 119.68 g/mol |
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| MolarMass = 119.68 g/mol |
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| Appearance = Grey powder |
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| Appearance = white solid (spoiled samples are colored) |
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| Odor = none (degraded samples smell of hydrogen sulfide) |
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| Density = 3.7 g/cm<sup>3</sup> |
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| Density = 3.70 g/cm<sup>3</sup> |
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| MeltingPt = > 2000°C<ref>, answers.com</ref> |
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| BoilingPt = |
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| MeltingPtC = 2002 |
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| Solubility = slightly soluble |
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| BoilingPt = |
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| Solubility = slightly soluble |
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| Solvent = ] |
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| Solvent = ]s |
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| SolubleOther = decomposes |
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| SolubleOther = decomposes |
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| RefractIndex = 2.107 |
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| Section3 = {{Chembox Structure |
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|Section3={{Chembox Structure |
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| CrystalStruct = ] (cubic), ] |
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| CrystalStruct = ] (cubic), ] |
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| SpaceGroup = Fm<u style="text-decoration:overline">3</u>m, No. 225 |
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| SpaceGroup = Fm<u style="text-decoration:overline">3</u>m, No. 225 |
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| Coordination = Octahedral (Sr<sup>2+</sup>); octahedral (S<sup>2–</sup>) |
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| Coordination = Octahedral (Sr<sup>2+</sup>); octahedral (S<sup>2−</sup>) |
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| LattConst_a = |
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| LattConst_a = |
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}}| Section7 = {{Chembox Hazards |
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| ExternalMSDS = |
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| EUIndex = Not listed |
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| Section8 = {{Chembox Related |
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|Section7={{Chembox Hazards |
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| ExternalSDS = |
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| OtherAnions = ] |
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| HPhrases = |
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| OtherCations = ]<br/>]<br/>] |
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| OtherAnions = ] |
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| OtherCations = ]<br/>]<br/>] |
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'''Strontium sulfide''' is the ] with the formula ]]. It is a white solid. The compound is an intermediate in the conversion of strontium sulfate, the main strontium ] called ] (or, more correctly, celestine), to other more useful compounds.<ref name=Ullmann>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}}.</ref><ref name=Celestine>{{Cite web|url=https://www.mindat.org/min-927.html|title = Celestine}}</ref><ref name=IMA>{{Cite web|url=https://www.ima-mineralogy.org/Minlist.htm|title=List of Minerals|date=21 March 2011}}</ref> |
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'''] ]''' is used as an additive in ] because it creates a bright red flame when burnt. It is also used in ] and luminous ]s, being a ]. |
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==Production and reactions== |
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Strontium sulfide is produced by ] celestine with ] at 1100–1300 °C.<ref name=hydrometallurgy>{{cite journal |journal= Hydrometallurgy |volume= 84 |issue= 3–4 |year= 2006 |pages= 239–246 |title= Dissolution kinetics of celestite (SrSO<sub>4</sub>) in HCl solution with BaCl<sub>2</sub> |first1= Salih |last1= Aydoğan |first2= Murat |last2= Erdemoğlu |first3= Ali |last3= Aras |first4= Gökhan |last4= Uçar |first5= Alper |last5= Özkan |doi= 10.1016/j.hydromet.2006.06.001 |bibcode= 2006HydMe..84..239A }}</ref> The sulfate is ], leaving the sulfide: |
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:SrSO<sub>4</sub> + 2 C → SrS + 2 CO<sub>2</sub> |
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About 300,000 tons are processed in this way annually.<ref name=Ullmann/> Both luminous and nonluminous sulfide phases are known, impurities, defects, and dopants being important.<ref>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}}</ref> |
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As expected for a sulfide salt of alkaline earth, the sulfide hydrolyzes readily: |
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:SrS + 2 H<sub>2</sub>O → Sr(OH)<sub>2</sub> + H<sub>2</sub>S |
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For this reason, samples of SrS have an odor of rotten eggs. |
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Similar reactions are used in the production of commercially useful compounds, including the most useful strontium compound, ]: a mixture of strontium sulfide with either ] gas or ] leads to formation of a ] of strontium carbonate.<ref name=Ullmann/><ref name=hydrometallurgy/> |
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:SrS + H<sub>2</sub>O + CO<sub>2</sub> → SrCO<sub>3</sub> + H<sub>2</sub>S |
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:SrS + Na<sub>2</sub>CO<sub>3</sub> → SrCO<sub>3</sub> + Na<sub>2</sub>S |
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] can also be prepared in this way. |
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== References == |
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== References == |
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==External links== |
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==External links== |
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{{Strontium compounds}} |
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{{Strontium compounds}} |
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{{Sulfides}} |
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{{Authority control}} |
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