Lithium sulfide

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Lithium sulfide
Sodium-oxide-unit-cell-3D-balls-B.png
Identifiers
CAS number 12136-58-2 YesY
PubChem 10290727 YesY
ChemSpider 8466196 YesY
EC number 235-228-1
RTECS number OJ6439500
Jmol-3D images Image 1
Image 2
Properties
Molecular formula 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)
Solubility in water very soluble
Solubility very soluble in ethanol
Structure
Crystal structure Antifluorite (cubic), cF12
Space group Fm3m, No. 225
Coordination
geometry
Tetrahedral (Li+); cubic (S2–)
Thermochemistry
Std molar
entropy
So298
63 J/mol K
Std enthalpy of
formation
ΔfHo298
-9.401 kJ/g or -447 kJ/mol
Hazards
MSDS External MSDS
EU Index Not listed
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
LD50 240 mg/kg (oral, rat)[1]
Related compounds
Other anions Lithium oxide
Other cations Sodium sulfide
Potassium sulfide
Related compounds Lithium hydrosulfide
Except where noted otherwise, 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[edit]

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[edit]

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

References[edit]

  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. doi:10.1002/9780470132463.ch40. ISBN 978-0-470-13246-3. 
  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. 

External links[edit]