Chemistry:Caesium sulfide
From HandWiki
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| Names | |
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| IUPAC name
Caesium sulfide
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| Identifiers | |
3D model (JSmol)
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| ChemSpider | |
PubChem CID
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| 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 | |
| Main hazards | toxic |
| GHS pictograms |  
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| GHS Signal word | Danger |
| H314, H400 | |
| P260, P264, P273, P280, P301+330+331, P303+361+353, P304+340, P305+351+338, P310, P321, P363, P391, P405, P501 | |
| Related compounds | |
Other anions
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Caesium oxide Caesium selenide Caesium telluride Caesium polonide |
Other cations
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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 | |
Caesium sulfide 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.
Production
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]
- 2 Cs + S → Cs
2S
By dissolving hydrogen sulfide into caesium hydroxide solution, it will produce caesium bisulfide, then it will produce caesium sulfide too.[5][6]。
- CsOH + H
2S → CsHS + H
2O - CsHS + CsOH → Cs
2S + H
2O
References
- ↑ Sommer, Helmut; Hoppe, Rudolf. The crystal structure of cesium sulfide and a remark about cesium selenide, cesium telluride, rubidium selenide, and rubidium telluride Script error: The function "in_lang" does not exist.. 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). "Hexamethyldisilathiane". in N. G. Russell. Inorganic Syntheses. 29. pp. 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. http://www.archive.org/stream/zeitschriftfura45unkngoog#page/n310/mode/1up.
- ↑ R. Abegg, F. Auerbach: 'Handbuch der anorganischen Chemie'. Verlag S. Hirzel, Bd. 2, 1908. S. 430.Volltext
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