Potassium sulfide: Difference between revisions

| verifiedrevid = 393932720

| Name = Potassium sulfide

| ImageFile = Potassium-sulfide-unit-cell-3D-ionic.png

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| ImageName = Potassium sulfide

| IUPACName = Potassium sulfide

| OtherNames = Dipotassium monosulfide,<br />Dipotassium sulfide,<br />Potassium monosulfide,<br />Potassium sulphide

| Section1 = {{Chembox Identifiers

| CASNo = 1312-73-8

| RTECS = TT6000000

| Section2 = {{Chembox Properties

| Formula = K₂S

| MolarMass = 110.262 g/mol

| Appearance = pure: colourless<br />impure: yellow-brown

| Density = 1.8 g/cm³

| Solubility = converts to KSH, KOH

| Solvent = other solvents

| SolubleOther = soluble in [[ethanol]] and [[glycerol]]

| MeltingPt = 840 °C

| BoilingPt = decomposes

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|[[Boiling point]]

| ? °C

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| Section3 = {{Chembox Structure

| CrystalStruct = anti[[Fluorite]]

| Section7 = {{Chembox Hazards

| ExternalMSDS =

| MainHazards = Dangerous for the environment ('''N''')

| RPhrases = {{R17}}, {{R23}}, {{R25}}, {{R31}}, {{R34}}, {{R50}}

| SPhrases = {{S24}}, {{S26}}

}}

| Section8 = {{Chembox Related

| OtherCations = [[Sodium sulfide]], [[Iron(II) sulfide]]

| OtherCpds = [[Potassium sulfite]], [[Potassium sulfate]]

'''Potassium sulfide''' is the [[inorganic compound]] with the formula K₂S. The colourless solid is rarely encountered, because it reacts readily with water, a reaction that affords potassium [[bisulfide]] (KSH) and potassium hydroxide (KOH).

It adopts "antifluorite structure," which means that the small K⁺ ions occupy the tetrahedral (F⁻) sites in [[fluorite]], and the larger S²⁻ centers occupy the eight-coordinate sites. [[lithium sulfide|Li₂S]], [[sodium sulfide|Na₂S]], and Rb₂S crystallize similarly.<ref name=Holleman>Holleman, A. F.; Wiberg, E. "Inorganic Chemistry" Academic Press: San Diego, 2001. ISBN 0-12-352651-5.</ref>

It can be produced by heating K₂SO₄ with carbon ([[coke (fuel)|coke]]):

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> K₂S 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.

Another method of making K₂S in laboratory involves the reaction of [[potassium permanganate]] and elemental sulfur:

: 2 KMnO₄ + S → K₂S + 2 MnO₂ + 2 O₂

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.<ref name=Shimizu>Shimizu, Takeo. "Fireworks: the Art, Science, and Technique." Pyrotechnica Publications: Austin, 1981. ISBN 0-929388-05-4.</ref>

*[[Liver of sulfur]]

[[ar:كبريتيد البوتاسيوم]]

[[ca:Sulfur de potassi]]

[[de:Kaliumsulfid]]

[[fr:Sulfure de potassium]]

[[it:Solfuro di potassio]]

[[lv:Kālija sulfīds]]

[[hu:Kálium-szulfid]]

[[nl:Kaliumsulfide]]

[[ja:硫化カリウム]]

[[pl:Siarczek potasu]]

[[pt:Sulfeto de potássio]]

[[ru:Сульфид калия]]

[[simple:Potassium sulfide]]

[[sv:Kaliumsulfid]]

[[zh:硫化钾]]