Lithium sulfide

Lithium sulfide
Names
IUPAC name
Lithium hydrosulfide
Preferred IUPAC name
Lithium sulfide
Identifiers
3D model (JSmol)
ChemSpider
ECHA InfoCard 100.032.013
EC Number 235-228-1
RTECS number OJ6439500
Properties
Li2S
Molar mass 45.95 g/mol
Appearance white solid
Density 1.66 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
Solubility very soluble in ethanol
Structure
Antifluorite (cubic), cF12
Fm3m, No. 225
Tetrahedral (Li+); cubic (S2−)
Thermochemistry
63 J/mol K
-9.401 kJ/g or -447 kJ/mol
Hazards
Safety data sheet External MSDS
NFPA 704
Flammability code 1: Must be pre-heated before ignition can occur. Flash point over 93 °C (200 °F). E.g., canola oil Health code 3: Short exposure could cause serious temporary or residual injury. E.g., chlorine gas Reactivity code 1: Normally stable, but can become unstable at elevated temperatures and pressures. E.g., calcium Special hazards (white): no codeNFPA 704 four-colored diamond
1
3
1
Lethal dose or concentration (LD, LC):
240 mg/kg (oral, rat)[1]
Related compounds
Other anions
 Lithium oxide
Other cations
 Sodium sulfide
Potassium 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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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.[3] This reaction is conveniently conducted in anhydrous ammonia.[4]

2 Li + S → Li2S

The THF-soluble triethylborane adduct of lithium sulfide can be generated using superhydride.[5]

Reactions and applications

Lithium sulfide has been considered for use in lithium-sulfur batteries.[6]

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. ↑ "Webelements – Lithium Sulfide". Retrieved 2005-09-16.
  4. ↑ Rankin, D. W. H. (1974). "Digermanyl Sulfide". Inorg. Synth. 15: 182–84. ISBN 978-0-470-13246-3. doi:10.1002/9780470132463.ch40.
  5. ↑ Gladysz, J. A.; Wong, V. K. and Jick, B. G., "Reduction of S-S Bonds with LiBHEt3", Tetrahedron, 1979, 35, 2329.
  6. ↑ "Battery claims greater capacity than lithium ion". Electronics Weekly. Retrieved 2005-09-16.
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