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Caesium sulfide

From Wikipedia, the free encyclopedia
Caesium sulfide
cesium sulfide
cesium sulfide
Names
IUPAC name
Caesium sulfide
Identifiers
3D model (JSmol)
ChemSpider
  • InChI=1S/2Cs.S/q2*+1;-2
    Key: QTNDMWXOEPGHBT-UHFFFAOYSA-N
  • [S-2].[Cs+].[Cs+]
Properties
Cs2S
Molar mass297.876 g/mol
AppearanceWhite crystal
Density4.19 g·cm−3[1]
Melting point480 °C[2]
Hydrolyzes to formcaesium bisulfide[3]
Solubility inethanol andglycerolSoluble
Structure
cubic,anti-fluorite
Hazards
Occupational safety and health (OHS/OSH):
Main hazards
toxic
GHS labelling:
GHS05: CorrosiveGHS09: Environmental hazard
Danger
H314,H400
P260,P264,P273,P280,P301+P330+P331,P303+P361+P353,P304+P340,P305+P351+P338,P310,P321,P363,P391,P405,P501
Related compounds
Otheranions
Caesium oxide
Caesium selenide
Caesium telluride
Caesium polonide
Othercations
Lithium sulfide
Sodium sulfide
Potassium sulfide
Rubidium sulfide
Francium sulfide
Except where otherwise noted, data are given for materials in theirstandard state (at 25 °C [77 °F], 100 kPa).
Chemical compound

Caesium sulfide is aninorganicsalt with a chemical formula Cs2S. It is a strong alkali in aqueous solution. In the air, caesium sulfide emits rotten egg smellinghydrogen sulfide.

Production

[edit]

Similar tosodium sulfide, anhydrous caesium sulfide can be produced by reactingcaesium andsulfur inTHF. It needsammonia ornaphthalene to react.[4]

2 Cs + S → Cs2S

By dissolvinghydrogen sulfide intocaesium hydroxide solution, it will producecaesium bisulfide, then it will produce caesium sulfide too.[5][6]

CsOH + H2S → CsHS + H2O
CsHS + CsOH → Cs2S + H2O

References

[edit]
  1. ^Sommer, Helmut; Hoppe, Rudolf. The crystal structure of cesium sulfide and a remark about cesium selenide, cesium telluride, rubidium selenide, and rubidium telluride(in German).Zeitschrift für Anorganische und Allgemeine Chemie, 1977. 429: 118-30.ISSN 0044-2313
  2. ^Dale L. Perry, Sidney L. Phillips:Handbook of inorganic compounds. CRC Press, 1995,ISBN 978-0-8493-8671-8, S. 336 ([1], p. 336, atGoogle Books).
  3. ^Jean D'Ans, Ellen Lax:Taschenbuch für Chemiker und Physiker. 3. Elemente, anorganische Verbindungen und Materialien, Minerale, Band 3. 4. Auflage, Springer, 1997,ISBN 978-3-5406-0035-0, S. 692 ([2], p. 692, atGoogle Books).
  4. ^J.-H. So and P. Boudjouk (1992). "Hexamethyldisilathiane". In N. G. Russell (ed.).Inorganic Syntheses. Vol. 29. pp. 30–32.doi:10.1002/9780470132609.ch11.ISBN 978-0-470-13260-9.
  5. ^Biltz, Wilhelm; Wilke-Dörfurt, Ernst (1905)."Über Sulfide des Rubidiums und Cäsiums".Zeitschrift für Anorganische Chemie.48:297–318.doi:10.1002/zaac.19060480122.
  6. ^R. Abegg, F. Auerbach: 'Handbuch der anorganischen Chemie'. Verlag S. Hirzel, Bd. 2, 1908. S. 430.Volltext
Compounds withnoble gases
Compounds withhalogens
Oxides andhydroxides
Compounds withchalcogens
Compounds withpnictogens
Compounds withgroup 14 elements
Compounds withgroup 13 elements
Compounds withtransition metals
Organocaesium compounds
Other compounds
Sulfides(S2−)
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