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{{chembox |
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| verifiedrevid = 393932720 |
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| verifiedrevid = 434168427 |
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| Name = Potassium sulfide |
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| ImageFile = Potassium-sulfide-unit-cell-3D-ionic.png |
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| Name = Potassium sulfide |
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| ImageFile = Potassium-sulfide-unit-cell-3D-ionic.png |
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| ImageName = Potassium sulfide |
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<!-- | ImageSize = 200px --> |
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| ImageName = Potassium sulfide |
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| ImageFile1 = Potassium sulfide.JPG |
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| IUPACName = Potassium sulfide |
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| IUPACName = Potassium sulfide |
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| OtherNames = Dipotassium monosulfide,<br />Dipotassium sulfide,<br />Potassium monosulfide,<br />Potassium sulphide |
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| OtherNames = Dipotassium monosulfide,<br />Dipotassium sulfide,<br />Potassium monosulfide,<br />Potassium sulfide |
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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 = 1312-73-8 |
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| RTECS = TT6000000 |
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| CASNo = 1312-73-8 |
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| UNII_Ref = {{fdacite|correct|FDA}} |
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| UNII = 31R0R7HD0N |
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| RTECS = TT6000000 |
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| EC_number = 215-197-0 |
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| UNNumber = 1847 1382 |
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| PubChem = 162263 |
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| ChemSpiderID = 142491 |
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| SMILES = .. |
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| StdInChI = 1S/2K.S/q2*+1;-2 |
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| StdInChIKey = DPLVEEXVKBWGHE-UHFFFAOYSA-N |
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|Section2={{Chembox Properties |
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| Formula = K<sub>2</sub>S |
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| MolarMass = 110.262 g/mol |
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| Appearance = pure: colourless<br />impure: yellow-brown |
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| Odor = ] |
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| Density = 1.74 g/cm<sup>3</sup> |
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| Solubility = converts to KSH, KOH |
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| Solvent = other solvents |
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| SolubleOther = soluble in ], ] <br> insoluble in ] |
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| MeltingPtC = 840 |
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| BoilingPtC = 912 |
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| BoilingPt_notes = (decomposes) |
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| MagSus = −60.0·10<sup>−6</sup> cm<sup>3</sup>/mol |
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|Section3={{Chembox Structure |
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| CrystalStruct = anti] |
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|Section4={{Chembox Thermochemistry |
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|DeltaHf=-406.2 kJ·mol<sup>−1</sup><ref name="jct">{{cite journal |last1=Johnson |first1=G.K. |last2=Steele |first2=W.V. |title=The standard enthalpy of formation of potassium sulfide (K<sub>2</sub>S) by fluorine bomb calorimetry |journal=The Journal of Chemical Thermodynamics |date=1981 |volume=13 |issue=10 |pages=985-990 |doi=10.1016/0021-9614(81)90075-6 |language=English}}</ref> |
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|DeltaGf=-392.4 kJ·mol<ref name="jct" /> |
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|Entropy=105.00 J·mol<sup>−1</sup>·K<sup>−1</sup><ref>{{cite book |title=CRC Handbook of Chemistry and Physics |date=2014 |publisher=CRC Press |isbn=1482208679 |pages=5-15 |edition=95th}}</ref> |
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| Section2 = {{Chembox Properties |
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|Section7={{Chembox Hazards |
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| ExternalSDS = |
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| Formula = K<sub>2</sub>S |
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| MainHazards = Causes skin burns. Dangerous for the environment |
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| MolarMass = 110.262 g/mol |
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| GHSPictograms = {{GHS05}}{{GHS09}} |
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| Appearance = pure: colourless<br />impure: yellow-brown |
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| GHSSignalWord = Danger |
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| Density = 1.8 g/cm<sup>3</sup> |
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| HPhrases = {{H-phrases|314|400}} |
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| Solubility = converts to KSH, KOH |
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| PPhrases = {{P-phrases|260|264|273|280|301+330+331|303+361+353|304+340|305+351+338|310|321|363|391|405|501}} |
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| Solvent = other solvents |
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| SolubleOther = soluble in ] and ] |
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| MeltingPt = 840 °C |
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| BoilingPt = decomposes |
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| ? °C |
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| Section3 = {{Chembox Structure |
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| CrystalStruct = anti] |
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| Section7 = {{Chembox Hazards |
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|Section8={{Chembox Related |
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| OtherAnions = ]<br>]<br>]<br>] |
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| ExternalMSDS = |
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| OtherCations = ]<br>]<br>]<br>] |
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| MainHazards = Dangerous for the environment ('''N''') |
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| OtherCompounds = ]<br>]<br>]<br>] |
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| RPhrases = {{R17}}, {{R23}}, {{R25}}, {{R31}}, {{R34}}, {{R50}} |
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| SPhrases = {{S24}}, {{S26}} |
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| Section8 = {{Chembox Related |
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| OtherCations = ], ] |
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| OtherCpds = ], ] |
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'''Potassium sulfide''' is the ] with the formula K<sub>2</sub>S. The colourless solid is rarely encountered, because it reacts readily with water, a reaction that affords potassium ] (KSH) and potassium hydroxide (KOH). |
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'''Potassium sulfide''' is an ] with the formula ]<sub>2</sub>]. The colourless solid is rarely encountered, because it reacts readily with water, a reaction that affords ] (KSH) and potassium hydroxide (KOH). Most commonly, the term potassium sulfide refers loosely to this mixture, not the anhydrous solid. |
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==Structure== |
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==Structure== |
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It adopts "antifluorite structure," which means that the small K<sup>+</sup> ions occupy the tetrahedral (F<sup>−</sup>) sites in ], and the larger S<sup>2−</sup> centers occupy the eight-coordinate sites. ], ], and Rb<sub>2</sub>S crystallize similarly.<ref name=Holleman>Holleman, A. F.; Wiberg, E. "Inorganic Chemistry" Academic Press: San Diego, 2001. ISBN 0-12-352651-5.</ref> |
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It adopts "antifluorite structure," which means that the small K<sup>+</sup> ions occupy the tetrahedral (F<sup>−</sup>) sites in ], and the larger S<sup>2−</sup> centers occupy the eight-coordinate sites. ], ], and Rb<sub>2</sub>S crystallize similarly.<ref name=Holleman>Holleman, A. F.; Wiberg, E. "Inorganic Chemistry" Academic Press: San Diego, 2001. {{ISBN|0-12-352651-5}}.</ref> |
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==Synthesis and reactions== |
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==Synthesis and reactions== |
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It can be produced by heating K<sub>2</sub>SO<sub>4</sub> with carbon (]): |
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It can be produced by ] K<sub>2</sub>SO<sub>4</sub> with carbon (]): |
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:K<sub>2</sub>SO<sub>4</sub> + 4 C → K<sub>2</sub>S + 4 CO |
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:K<sub>2</sub>SO<sub>4</sub> + 4 C → K<sub>2</sub>S + 4 CO |
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In the laboratory, a number of methods exist.<ref>Handbook of Preparative Inorganic Chemistry, 2nd Ed. Edited by G. Brauer, Academic Press, 1963, NY. Vol. 1. p. 200.</ref> K<sub>2</sub>S arises from the reaction of potassium and sulfur. In the laboratory, this synthesis is usually conducted by combining a solution of potassium in anhydrous ammonia with elemental sulfur. |
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In the laboratory, pure K<sub>2</sub>S may be prepared by the reaction of potassium and sulfur in anhydrous ammonia. <ref>Handbook of Preparative Inorganic Chemistry, 2nd Ed. Edited by G. Brauer, Academic Press, 1963, NY. Vol. 1. p. 360.</ref> |
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Another method of making K<sub>2</sub>S in laboratory involves the reaction of ] and elemental sulfur: |
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: 2 KMnO<sub>4</sub> + S → K<sub>2</sub>S + 2 MnO<sub>2</sub> + 2 O<sub>2</sub> |
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Sulfide is highly basic, consequently K<sub>2</sub>S completely and irreversibly ] in water according to the following equation: |
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Sulfide is highly basic, consequently K<sub>2</sub>S completely and irreversibly ] in water according to the following equation: |
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==Use in fireworks== |
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==Use in fireworks== |
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Potassium sulfides are formed when ] is burned and are important intermediates in many pyrotechnic effects, such as senko hanabi and some glitter formulations.<ref name=Shimizu>Shimizu, Takeo. "Fireworks: the Art, Science, and Technique." Pyrotechnica Publications: Austin, 1981. ISBN 0-929388-05-4.</ref> |
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Potassium sulfides are formed when ] is burned and are important intermediates in many pyrotechnic effects, such as ] and some ] formulations.<ref name=Shimizu>Shimizu, Takeo. "Fireworks: the Art, Science, and Technique." Pyrotechnica Publications: Austin, 1981. {{ISBN|0-929388-05-4}}.</ref> |
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==See also== |
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==See also== |
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==References== |
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==References== |
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{{reflist}} |
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{{Potassium compounds}} |
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{{Potassium compounds}} |
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{{Sulfides}} |
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