Lithium sulfide
| Lithium sulfide | |
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Lithium hydrosulfide |
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Lithium sulfide |
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| Identifiers | |
| CAS number | 12136-58-2  |
| PubChem | 10290727 |
| ChemSpider | 8466196 |
| EC number | 235-228-1 |
| RTECS number | OJ6439500 |
| Jmol-3D images | Image 1 Image 2 |
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| Properties | |
| Molecular formula | Li2S |
| Molar mass | 45.95 g/mol |
| Appearance | white solid |
| Density | 1.66 g/cm3 |
| Melting point |
938 °C (1211 K) |
| Boiling point |
1372 °C (1645 K) |
| Structure | |
| Crystal structure | Antifluorite (cubic), cF12 |
| Space group | Fm3m, No. 225 |
| Coordination geometry |
Tetrahedral (Li+); cubic (S2–) |
| Thermochemistry | |
| Std enthalpy of formation ΔfH |
-9.401 kJ/g |
| Hazards | |
| MSDS | External MSDS |
| EU Index | Not listed |
| NFPA 704 |
 1
3
1
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| Related compounds | |
| Other anions | Lithium oxide |
| Other cations | Sodium sulfide Potassium sulfide |
| Related compounds | Lithium hydrosulfide |
 (verify) (what is:  / ?)Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa) |
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| Infobox references | |
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 hydrogen sulfide (rotten egg odor).[1]
Contents |
[edit] Preparation
Lithium sulfide is prepared by treating lithium with sulfur.[2] This reaction is conveniently conducted in anhydrous ammonia.[3]
- 2 Li + S → Li2S
The THF-soluble triethylborane adduct of lithium sulfide can be generated using superhydride.[4]
[edit] Reactions and applications
Lithium sulfide has been considered for use in lithium-sulfur batteries.[5]
[edit] References
- ^ Greenwood, N. N.; & Earnshaw, A. (1997). Chemistry of the Elements (2nd Edn.), Oxford:Butterworth-Heinemann. ISBN 0-7506-3365-4.
- ^ "Webelements – Lithium Sulfide". http://www.webelements.com/webelements/compounds/text/Li/Li2S1-12136582.html. Retrieved 2005-09-16.
- ^ Rankin, D. W. H. (1974). "Digermanyl Sulfide". Inorg. Synth. 15: 182–84. doi:10.1002/9780470132463.ch40. ISBN 9780470132463.
- ^ Gladysz, J. A.; Wong, V. K. and Jick, B. G., "Reduction of S-S Bonds with LiBHEt3", Tetrahedron, 1979, 35, 2329.
- ^ "Battery claims greater capacity than lithium ion". Electronics Weekly. http://www.electronicsweekly.com/Articles/2005/07/12/35830/Batteryclaimsgreatercapacitythanlithiumion.htm. Retrieved 2005-09-16.
[edit] External links
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