Caesium sulfide

Caesium sulfide
cesium sulfide
Names
IUPAC name
Cesium sulfide
Identifiers
3D model (JSmol)
ChemSpider
  • InChI=1S/2Cs.S/q2*+1;-2
    Key: QTNDMWXOEPGHBT-UHFFFAOYSA-N
  • [S-2].[Cs+].[Cs+]
Properties
Cs2S
Molar mass 297.876 g/mol
Appearance White crystal
Density 4.19 g·cm−3[1]
Melting point 480 °C[2]
Hydrolyzes to form caesium bisulfide[3]
Solubility in ethanol and glycerol Soluble
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
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).

Cesium sulfide is an inorganic salt with a chemical formula Cs2S. It is a strong alkali in aqueous solution. In the air, cesium sulfide emits rotten egg smelling hydrogen sulfide.

Production

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

2 Cs + S → Cs2S

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

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

References

  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. 29: 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