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).[2]
Names | |
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IUPAC name Lithium hydrosulfide | |
Preferred IUPAC name Lithium sulfide | |
Identifiers | |
3D model (JSmol) | |
ChemSpider | |
ECHA InfoCard | 100.032.013 |
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UNII | |
CompTox Dashboard (EPA) | |
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Properties | |
Li2S | |
Molar mass | 45.95 g/mol |
Appearance | white solid |
Density | 1.67 g/cm3 |
Melting point | 938 °C (1,720 °F; 1,211 K) |
Boiling point | 1,372 °C (2,502 °F; 1,645 K) |
very soluble, hydrolyses to LiOH and H2S | |
Solubility | very soluble in ethanol |
Structure | |
Antifluorite (cubic), cF12 | |
Fm3m, No. 225 | |
Tetrahedral (Li+); cubic (S2−) | |
Thermochemistry | |
Std molar entropy (S⦵298) | 63 J/mol K |
Std enthalpy of formation (ΔfH⦵298) | -9.401 kJ/g or -447 kJ/mol |
Hazards | |
NFPA 704 (fire diamond) | |
Lethal dose or concentration (LD, LC): | |
LD50 (median dose) | 240 mg/kg (oral, rat)[1] |
Safety data sheet (SDS) | External MSDS |
Related compounds | |
Other anions | Lithium oxide Lithium selenide Lithium telluride Lithium polonide |
Other cations | Sodium sulfide Potassium sulfide Rubidium sulfide Caesium sulfide |
Related compounds | Lithium hydrosulfide |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). |
Preparation
Lithium sulfide is prepared by treating lithium with sulfur. 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]
Reactions and applications
Lithium sulfide has been considered for use in lithium–sulfur batteries.[5]
References
External links
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