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Lithium sulfide
	; __ Li+ __ S2−
Names
	IUPAC name Lithium hydrosulfide
	Preferred IUPAC name Lithium sulfide
Identifiers
CAS Number	12136-58-2 ;
3D model (JSmol)	Interactive image; Interactive image;
ChemSpider	8466196 ;
ECHA InfoCard	100.032.013
EC Number	235-228-1;
PubChem CID	10290727;
RTECS number	OJ6439500;
UNII	SW6C51V9JZ ;
CompTox Dashboard (EPA)	DTXSID7065251 ;
	InChI InChI=1S/2Li.S/q2+1;-2 Key: GLNWILHOFOBOFD-UHFFFAOYSA-N ; InChI=1S/2Li.S/q2+1;-2; Key: GLNWILHOFOBOFD-UHFFFAOYSA-N;
	SMILES [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)
Solubility in water	decomposes to LiOH and H2S
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 (S⦵298)	63 J/mol K
Std enthalpy of; formation (ΔfH⦵298)	-9.401 kJ/g or -447 kJ/mol
Hazards
NFPA 704 (fire diamond)	3 1 1
	Lethal dose or concentration (LD, LC):
LD50 (median dose)	240 mg/kg (oral, rat)
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). verify (what is ?) 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 foul smelling hydrogen sulfide gas.^[2]

Preparation

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]

References

^ https://chem.nlm.nih.gov/chemidplus/rn/12136-58-2 ^{[dead link‍]}
^ Greenwood, N. N.; & Earnshaw, A. (1997). Chemistry of the Elements (2nd Edn.), Oxford:Butterworth-Heinemann. ISBN 0-7506-3365-4.
^ Rankin, D. W. H. (1974). "Digermanyl Sulfide". Inorg. Synth. 15: 182–84. doi:10.1002/9780470132463.ch40. ISBN 978-0-470-13246-3.
^ 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.
^ "Battery claims greater capacity than lithium ion". Electronics Weekly. 12 July 2005. Retrieved 2005-09-16.

External links

Lithium Sulfide

[1] ttps://chem.nlm.nih.gov/chemidplus/rn/12136-58-2 ^{[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.

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