Potassium sulfide: Difference between revisions

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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 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 kJ·mol<ref name="jct" />
			\|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>
	}}		}}
	\| ~~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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Latest revision as of 00:27, 25 September 2023

Potassium sulfide
Names


IUPAC name Potassium sulfide
Other names Dipotassium monosulfide, Dipotassium sulfide, Potassium monosulfide, Potassium sulfide
Identifiers
CAS Number	1312-73-8
3D model (JSmol)	Interactive image
ChemSpider	142491
ECHA InfoCard	100.013.816
EC Number	215-197-0
PubChem CID	162263
RTECS number	TT6000000
UNII	31R0R7HD0N
UN number	1847 1382
CompTox Dashboard (EPA)	DTXSID70909738
InChI InChI=1S/2K.S/q2*+1;-2Key: DPLVEEXVKBWGHE-UHFFFAOYSA-N
SMILES ..
Properties
Chemical formula	K₂S
Molar mass	110.262 g/mol
Appearance	pure: colourless impure: yellow-brown
Odor	H₂S
Density	1.74 g/cm
Melting point	840 °C (1,540 °F; 1,110 K)
Boiling point	912 °C (1,674 °F; 1,185 K) (decomposes)
Solubility in water	converts to KSH, KOH
Solubility in other solvents	soluble in ethanol, glycerol insoluble in ether
Magnetic susceptibility (χ)	−60.0·10 cm/mol
Structure
Crystal structure	antiFluorite
Thermochemistry
Std molar entropy (S₂₉₈)	105.00 J·mol·K
Std enthalpy of formation (Δ_fH₂₉₈)	-406.2 kJ·mol
Gibbs free energy (Δ_fG)	-392.4 kJ·mol
Hazards
Occupational safety and health (OHS/OSH):
Main hazards	Causes skin burns. Dangerous for the environment
GHS labelling:
Pictograms
Signal word	Danger
Hazard statements	H314, H400
Precautionary statements	P260, P264, P273, P280, P301+P330+P331, P303+P361+P353, P304+P340, P305+P351+P338, P310, P321, P363, P391, P405, P501
Related compounds
Other anions	Potassium oxide Potassium selenide Potassium telluride Potassium polonide
Other cations	Lithium sulfide Sodium sulfide Rubidium sulfide Caesium sulfide
Related compounds	Potassium hydrosulfide Potassium sulfite Potassium sulfate Iron(II) sulfide
Except where otherwise noted, data are given for materials in their standard state (at 25 °C , 100 kPa). Y verify (what is ?) Infobox references

Chemical compound

Potassium sulfide is an inorganic compound with the formula K₂S. The colourless solid is rarely encountered, because it reacts readily with water, a reaction that affords potassium hydrosulfide (KSH) and potassium hydroxide (KOH). Most commonly, the term potassium sulfide refers loosely to this mixture, not the anhydrous solid.

Structure

It adopts "antifluorite structure," which means that the small K ions occupy the tetrahedral (F) sites in fluorite, and the larger S centers occupy the eight-coordinate sites. Li₂S, Na₂S, and Rb₂S crystallize similarly.

Synthesis and reactions

It can be produced by heating K₂SO₄ with carbon (coke):

K₂SO₄ + 4 C → K₂S + 4 CO

In the laboratory, pure K₂S may be prepared by the reaction of potassium and sulfur in anhydrous ammonia.

Sulfide is highly basic, consequently K₂S completely and irreversibly hydrolyzes in water according to the following equation:

K₂S + H₂O → KOH + KSH

For many purposes, this reaction is inconsequential since the mixture of SH and OH behaves as a source of S. Other alkali metal sulfides behave similarly.

Use in fireworks

Potassium sulfides are formed when black powder is burned and are important intermediates in many pyrotechnic effects, such as senko hanabi and some glitter formulations.

References

CRC Handbook of Chemistry and Physics (95th ed.). CRC Press. 2014. pp. 5–15. ISBN 1482208679.
^ Johnson, G.K.; Steele, W.V. (1981). "The standard enthalpy of formation of potassium sulfide (K₂S) by fluorine bomb calorimetry". The Journal of Chemical Thermodynamics. 13 (10): 985–990. doi:10.1016/0021-9614(81)90075-6.
^ Holleman, A. F.; Wiberg, E. "Inorganic Chemistry" Academic Press: San Diego, 2001. ISBN 0-12-352651-5.
Handbook of Preparative Inorganic Chemistry, 2nd Ed. Edited by G. Brauer, Academic Press, 1963, NY. Vol. 1. p. 360.
Shimizu, Takeo. "Fireworks: the Art, Science, and Technique." Pyrotechnica Publications: Austin, 1981. ISBN 0-929388-05-4.

v t e Potassium compounds
H, (pseudo)halogens	KF KHF₂ KH KCl KClO KClO₃ KClO₄ KBr KBrO₃ KI KIO₃ KIO₄ KAt KCN KCNO KOCN KSCN
chalcogens	K₂O KOH K₂O₂ KO₂ KO₃ K₂S KHS K₂SO₃ KHSO₃ K₂SO₄ KHSO₄ KHSO₅ K₂S₂O₃ K₂S₂O₅ K₂S₂O₇ K₂S₂O₈ K₂Se K₂SeO₃ K₂SeO₄ K₂Te K₂TeO₃ K₂TeO₄ K₂Po
pnictogens	K₃N KNH₂ KN₃ KNO₂ KNO₃ K₃P KH₂PO₃ K₃PO₄ K₂HPO₄ KH₂PO₄ KPF₆ KAsO₂ K₃AsO₄ K₂HAsO₄ KH₂AsO₄
B, C group	B₄K₂O₇ K₂CO₃ KHCO₃ K₂SiO₃ K₂SiF₆ K₂Al₂O₄ K₂Al₂B₂O₇
transition metals	K₂PtCl₄ K₂Pt(CN)₄ K₂TiF₆ K₂PtCl₆ K₂ReCl₆ K ₂ReF ₆ KAsF₆ K₂ReBr₆ K ₂ReI ₆ K₂ZrF₆ K₄Fe(CN)₆ K₃Fe(CN)₆ K₃Fe(C₂O₄)₃ K₂FeO₄ K₂MnO₄ KMnO₄ K₃CrO₄ K₂CrO₄ K₃CrO₈ KCrO₃Cl K₂Cr₂O₇ K₂Cr₃O₁₀ K₂Cr₄O₁₃ K₄Mo₂Cl₈
organic	KHCO₂ KCH₃CO₂ KCF₃CO₂ K₂C₂O₄ KHC₂O₄ KC₁₂H₂₃O₂ KC₁₈H₃₅O₂ C₃H₂K₂O₄ C₄H₆KO₄ C₅H₇KO₄