Lithium sulfide

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Lithium sulfide
Sodium-oxide-unit-cell-3D-balls-B.png
Names
IUPAC name
Lithium hydrosulfide
Preferred IUPAC name
Lithium sulfide
Identifiers
12136-58-2 YesY
ChemSpider 8466196 YesY
EC Number 235-228-1
Jmol 3D model Interactive image
Interactive image
PubChem 10290727
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
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[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]