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{{chembox {{chembox
| Watchedfields = changed
| Name = Potassium sulfide
| verifiedrevid = 434168427
| ImageFile = Potassium-sulfide-unit-cell-3D-ionic.png
| Name = Potassium sulfide
<!-- | ImageSize = 200px -->
| ImageName = Potassium sulfide | ImageFile = Potassium-sulfide-unit-cell-3D-ionic.png
| IUPACName = Potassium sulfide | ImageName = Potassium sulfide
| ImageFile1 = Potassium sulfide.JPG
| OtherNames = Dipotassium monosulfide,<br />Dipotassium sulfide,<br />Potassium monosulfide,<br />Potassium sulphide
| IUPACName = Potassium sulfide
| Section1 = {{Chembox Identifiers
| OtherNames = Dipotassium monosulfide,<br />Dipotassium sulfide,<br />Potassium monosulfide,<br />Potassium sulfide
| CASNo = 1312-73-8
|Section1={{Chembox Identifiers
| RTECS = TT6000000
| CASNo_Ref = {{cascite|correct|CAS}}
| CASNo = 1312-73-8
| UNII_Ref = {{fdacite|correct|FDA}}
| UNII = 31R0R7HD0N
| RTECS = TT6000000
| EC_number = 215-197-0
| UNNumber = 1847 1382
| PubChem = 162263
| ChemSpiderID = 142491
| SMILES = ..
| StdInChI = 1S/2K.S/q2*+1;-2
| StdInChIKey = DPLVEEXVKBWGHE-UHFFFAOYSA-N

}}
|Section2={{Chembox Properties
| Formula = K<sub>2</sub>S
| MolarMass = 110.262 g/mol
| Appearance = pure: colourless<br />impure: yellow-brown
| Odor = ]
| Density = 1.74 g/cm<sup>3</sup>
| Solubility = converts to KSH, KOH
| Solvent = other solvents
| SolubleOther = soluble in ], ] <br> insoluble in ]
| MeltingPtC = 840
| BoilingPtC = 912
| BoilingPt_notes = (decomposes)
| MagSus = −60.0·10<sup>−6</sup> cm<sup>3</sup>/mol
}}
|Section3={{Chembox Structure
| CrystalStruct = anti]
}}
|Section4={{Chembox Thermochemistry
|DeltaHf=-406.2&nbsp;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>
|DeltaGf=-392.4&nbsp;kJ·mol<ref name="jct" />
|Entropy=105.00&nbsp;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>
}} }}
| Section2 = {{Chembox Properties |Section7={{Chembox Hazards
| ExternalSDS =
| Formula = K<sub>2</sub>S
| MainHazards = Causes skin burns. Dangerous for the environment
| MolarMass = 110.262 g/mol
| GHSPictograms = {{GHS05}}{{GHS09}}
| Appearance = pure: colourless<br />impure: yellow-brown
| GHSSignalWord = Danger
| Density = 1.8 g/cm<sup>3</sup>
| HPhrases = {{H-phrases|314|400}}
| Solubility = converts to KSH, KOH
| PPhrases = {{P-phrases|260|264|273|280|301+330+331|303+361+353|304+340|305+351+338|310|321|363|391|405|501}}
| Solvent = other solvents
| SolubleOther = soluble in ] and ]
| MeltingPt = 840 °C
| BoilingPt = decomposes
}}<!--
|]
| ? °C
|-


-->
| Section3 = {{Chembox Structure
| CrystalStruct = anti]
}} }}
| Section7 = {{Chembox Hazards |Section8={{Chembox Related
| OtherAnions = ]<br>]<br>]<br>]
| ExternalMSDS =
| OtherCations = ]<br>]<br>]<br>]
| MainHazards = Dangerous for the environment ('''N''')
| OtherCompounds = ]<br>]<br>]<br>]
| RPhrases = {{R17}}, {{R23}}, {{R25}}, {{R31}}, {{R34}}, {{R50}}
| SPhrases = {{S24}}, {{S26}}
}}
| Section8 = {{Chembox Related
| OtherCations = ], ]
| OtherCpds = ], ]
}} }}
}} }}
]

'''Potassium sulfide''' is the ] with the formula K<sub>2</sub>S. The colourless solid is rarely encountered, because it reacts readily and irreversibly with water, a reaction that affords potassium ] (KSH) and potassium hydroxide (KOH). '''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.


==Structure== ==Structure==
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 (Ca<sup>2+</sup>) 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> 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>


==Synthesis and reactions== ==Synthesis and reactions==
It can be produced by ] K<sub>2</sub>SO<sub>4</sub> with carbon (]):
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.
:K<sub>2</sub>SO<sub>4</sub> + 4 C → K<sub>2</sub>S + 4 CO
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>


Sulfide is highly basic, consequently K<sub>2</sub>S completely and irreversibly ] in water according to the following equation:
It can also be produced by heating K<sub>2</sub>SO<sub>4</sub> with coal:
K<sub>2</sub>SO<sub>4</sub> + 2C = K<sub>2</sub>S + 2 CO<sub>2</sub> :K<sub>2</sub>S + H<sub>2</sub>O → KOH + KSH


K<sub>2</sub>SO<sub>4</sub> + 4C = K<sub>2</sub>S + 4 CO

This salt contains the highly basic anion S<sup>2−</sup>, which completely ] in water according to the following equation:
:K<sub>2</sub>S + H<sub>2</sub>O → KOH + KSH
For many purposes, this reaction is inconsequential since the mixture of SH<sup>−</sup> and OH<sup>−</sup> behaves as a source of S<sup>2−</sup>. Other alkali metal sulfides behave similarly.<ref name=Holleman/> For many purposes, this reaction is inconsequential since the mixture of SH<sup>−</sup> and OH<sup>−</sup> behaves as a source of S<sup>2−</sup>. Other alkali metal sulfides behave similarly.<ref name=Holleman/>


==Use in fireworks== ==Use in fireworks==
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> 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>


==See also== ==See also==
*] * ]


==References== ==References==
{{reflist}} {{reflist}}



{{Potassium compounds}} {{Potassium compounds}}
{{Sulfides}}


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