Caesium sulfide

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Caesium sulfide
caesium sulfide
IUPAC name
Caesium sulfide
3D model (JSmol)
  • InChI=1S/2Cs.S/q2*+1;-2
  • [S-2].[Cs+].[Cs+]
Molar mass 297.876
Appearance white crystal
Density 4.19 g·cm−3[1]
Melting point 480 °C[2]
hydrolyses to form caesium bisulfide[3]
Solubility in ethanol and glycerol soluble
cubic, anti-fluorite
Occupational safety and health (OHS/OSH):
Main hazards
GHS labelling:
GHS05: CorrosiveGHS09: Environmental hazard
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
Other anions
Caesium oxide
Caesium selenide
Caesium telluride
Caesium polonide
Other cations
Lithium sulfide
Sodium sulfide
Potassium sulfide
Rubidium sulfide
Francium sulfide
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).

Caesium sulfide (also spelled cesium sulfide in American English) is an inorganic salt with a chemical formula Cs2S. It is a strong alkali in aqueous solution. In the air, caesium sulfide emits rotten egg smelling hydrogen sulfide.


Similar to sodium sulfide, anhydrous caesium sulfide can be produced by reacting caesium and sulfur in THF. It needs ammonia or naphthalene to react.[4]

2Cs + S → Cs2S

By dissolving hydrogen sulfide into caesium hydroxide solution, it will produce caesium bisulfide, then it will produce caesium sulfide too.[5][6]

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


  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, at Google 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, at Google Books).
  4. ^ J.-H. So and P. Boudjouk (1992). N. G. Russell (ed.). "Hexamethyldisilathiane". Inorganic Syntheses: 30–32. doi:10.1002/9780470132609.ch11. ISBN 9780470132609.
  5. ^ Wilhelm Blitz, Ernst Wilke-Dörfurt: "Über Sulfide des Rubidiums und Cäsiums" in Zeitschr. f. anorg. Chem. 1906. 48, S. 297–317. Volltext
  6. ^ R. Abegg, F. Auerbach: 'Handbuch der anorganischen Chemie'. Verlag S. Hirzel, Bd. 2, 1908. S. 430.Volltext