Lithium sulfide is the inorganic compound with the formula Li2S. It crystallizes in the antifluorite motif, described as the salt (Li+)2S2−. It forms a solid yellow-white deliquescent powder. In air, it easily hydrolyses to release foul smelling hydrogen sulfide gas.
Preparation
Lithium sulfide is prepared by treating lithium with sulfur. This reaction is conveniently conducted in anhydrous ammonia.2
2 Li + S → Li2SThe THF-soluble triethylborane adduct of lithium sulfide can be generated using superhydride.3
Reactions and applications
Lithium sulfide has been considered for use in lithium–sulfur batteries.4
External links
References
Greenwood, N. N.; & Earnshaw, A. (1997). Chemistry of the Elements (2nd Edn.), Oxford:Butterworth-Heinemann. ISBN 0-7506-3365-4. /wiki/ISBN_(identifier) ↩
Rankin, D. W. H. (1974). "Digermanyl Sulfide". Inorg. Synth. 15: 182–84. doi:10.1002/9780470132463.ch40. ISBN 978-0-470-13246-3. 978-0-470-13246-3 ↩
Gladysz, J. A.; Wong, V. K.; Jick, B. G. (1979). "New Methodology for the Introduction of Sulfur into Organic Molecules. Synthesis of Anhydrous Dilithium Dulfide, Dilithium Disulfide and Lithium Thiolates by Lithium Triethylborohydride Reduction of Elemental Sulfur and Disulfides". Tetrahedron. 35: 2329–2335. doi:10.1016/S0040-4020(01)93746-9. /wiki/Doi_(identifier) ↩
"Battery claims greater capacity than lithium ion". Electronics Weekly. 12 July 2005. Retrieved 2005-09-16. http://www.electronicsweekly.com/Articles/2005/07/12/35830/Batteryclaimsgreatercapacitythanlithiumion.htm ↩