Lithium sulfide
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| Names | |
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| IUPAC name
Lithium hydrosulfide |
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| Preferred IUPAC name
Lithium sulfide |
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| Identifiers | |
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3D model (JSmol) |
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| ECHA InfoCard | 100.032.013  |
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PubChem CID |
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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) |
| decomposes to LiOH and H2S | |
| Solubility | very soluble in ethanol |
| Structure | |
| Antifluorite (cubic), cF12 | |
| Fm3m, No. 225 | |
| Tetrahedral (Li+); cubic (S2−) | |
| Thermochemistry | |
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Std molar |
63 J/mol K |
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Std enthalpy of |
-9.401 kJ/g or -447 kJ/mol |
| Hazards | |
| NFPA 704 (fire diamond) | |
| Lethal dose or concentration (LD, LC): | |
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LD50 (median dose) |
240 mg/kg (oral, rat)[1] |
| Safety data sheet (SDS) | External MSDS |
| Related compounds | |
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Other anions |
Lithium oxide Lithium selenide Lithium telluride Lithium polonide |
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Other cations |
Sodium sulfide Potassium sulfide Rubidium sulfide Caesium sulfide |
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Related compounds |
Lithium hydrosulfide |
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Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). |
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.[2]
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]
Lithium sulfide has been considered for use in lithium–sulfur batteries.[5]