Lithium sulfide

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Lithium sulfide
Lithium-sulfide-2D.png
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CaF2 polyhedra.png
__ Li+     __ S2−
Names
IUPAC name
Lithium hydrosulfide
Preferred IUPAC name
Lithium sulfide
Identifiers
  • 12136-58-2 checkY
3D model (JSmol)
ChemSpider
ECHA InfoCard 100.032.013 Edit this at Wikidata
EC Number
  • 235-228-1
RTECS number
  • OJ6439500
UNII
  • InChI=1S/2Li.S/q2*+1;-2 checkY
    Key: GLNWILHOFOBOFD-UHFFFAOYSA-N checkY
  • InChI=1S/2Li.S/q2*+1;-2
  • Key: GLNWILHOFOBOFD-UHFFFAOYSA-N
  • [Li+].[Li+].[S-2]
  • [Li+].[Li+].[S-2]
Properties
Chemical formula
 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
Space group
 Fm3m, No. 225
Tetrahedral (Li+); cubic (S2−)
Thermochemistry
63 J/mol K
Std enthalpy of
formation (ΔfH⦵298)
 -9.401 kJ/g or -447 kJ/mol
Hazards
Safety data sheet (SDS) External MSDS
NFPA 704 (fire diamond)
3
1
1
Lethal dose or concentration (LD, LC):
LD50 (median dose)
 240 mg/kg (oral, rat)[1]
Related compounds
Other anions
 Lithium oxide
Lithium selenide
Lithium telluride
Lithium polonide
Other cations
 Sodium sulfide
Potassium sulfide
Rubidium sulfide
Caesium sulfide
Related compounds
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
checkY  (what is checkY☒N ?)
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).[2]

Preparation[]

Lithium sulfide is prepared by treating lithium with sulfur. This reaction is conveniently conducted in anhydrous ammonia.[3]

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[]

  1. ^ http://chem.sis.nlm.nih.gov/chemidplus/rn/12136-58-2
  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.CS1 maint: uses authors parameter (link)
  5. ^ "Battery claims greater capacity than lithium ion". Electronics Weekly. 12 July 2005. Retrieved 2005-09-16.

External links[]

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