Lithium sulfide

__ Li+     __ S2−
IUPAC name
Lithium hydrosulfide
Preferred IUPAC name
Lithium sulfide
3D model (JSmol)
ECHA InfoCard 100.032.013 Edit this at Wikidata
EC Number
  • 235-228-1
RTECS number
  • OJ6439500
  • InChI=1S/2Li.S/q2*+1;-2 checkY
  • InChI=1S/2Li.S/q2*+1;-2
  • [Li+].[Li+].[S-2]
  • [Li+].[Li+].[S-2]
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
Antifluorite (cubic), cF12
Fm3m, No. 225
Tetrahedral (Li+); cubic (S2−)
63 J/mol K
-9.401 kJ/g or -447 kJ/mol
NFPA 704 (fire diamond)
NFPA 704 four-colored diamondHealth 3: Short exposure could cause serious temporary or residual injury. E.g. chlorine gasFlammability 1: Must be pre-heated before ignition can occur. Flash point over 93 °C (200 °F). E.g. canola oilInstability 1: Normally stable, but can become unstable at elevated temperatures and pressures. E.g. calciumSpecial hazards (white): no code
Lethal dose or concentration (LD, LC):
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).
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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]


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]


  1. ^ [dead link]
  2. ^ Greenwood, N. N.; & Earnshaw, A. (1997). Chemistry of the Elements (2nd Edn.), Oxford:Butterworth-Heinemann. ISBN 0-7506-3365-4.
  3. ^ Rankin, D. W. H. (1974). "Digermanyl Sulfide". Inorg. Synth. 15: 182–84. doi:10.1002/9780470132463.ch40. ISBN 978-0-470-13246-3.
  4. ^ 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.
  5. ^ "Battery claims greater capacity than lithium ion". Electronics Weekly. 12 July 2005. Retrieved 2005-09-16.