Caesium sulfide
 | |
| Names | |
|---|---|
| IUPAC name Cesium sulfide | |
| Identifiers | |
CAS Number |
|
3D model (JSmol) |
|
| ChemSpider |
|
PubChem CID |
|
CompTox Dashboard (EPA) |
|
InChI
| |
| |
| Properties | |
Chemical formula | Cs2S |
| Molar mass | 297.876 g/mol |
| Appearance | White crystal |
| Density | 4.19 g·cm−3[1] |
| Melting point | 480 °C[2] |
Solubility in water | Hydrolyzes to form caesium bisulfide[3] |
| Solubility in ethanol and glycerol | Soluble |
| Structure | |
Crystal structure | cubic, anti-fluorite |
| Hazards | |
| Occupational safety and health (OHS/OSH): | |
Main hazards | toxic |
| GHS labelling: | |
  | |
| 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). Infobox references | |
Chemical compound
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
- ^ 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
- ^ 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).
- ^ 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).
- ^ 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.
- ^ Biltz, Wilhelm; Wilke-Dörfurt, Ernst (1905). "Über Sulfide des Rubidiums und Cäsiums". Zeitschrift für Anorganische Chemie. 48: 297–318. doi:10.1002/zaac.19060480122.
- ^ R. Abegg, F. Auerbach: 'Handbuch der anorganischen Chemie'. Verlag S. Hirzel, Bd. 2, 1908. S. 430.Volltext
- v
- t
- e
