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Lithium sulfide: Difference between revisions

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{{Chembox {{Chembox
| Watchedfields = changed | Watchedfields = changed
| verifiedrevid = 396507410 | verifiedrevid = 446984298
| IUPACName = Lithium hydrosulfide | IUPACName = Lithium hydrosulfide
| ImageFile = Sodium-oxide-unit-cell-3D-balls-B.png | ImageFile = File:Lithium-sulfide-2D.png
| ImageSize = 250 | ImageSize = 150px
| ImageFile1 = Sodium-oxide-unit-cell-3D-balls-B.png
⚫ | PIN = Lithium sulfide
| Image = | ImageSize1 = 200
| ImageFile2 = File:CaF2 polyhedra.png
⚫ | Section1 = {{Chembox Identifiers
| ImageSize2 =
⚫ | SMILES1 = ..
| ImageCaption2 = <span style="color:#99CC00;background-color:#99CC00;">__</span> ]<sup>+</sup>&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;<span style="color:#C0C0C0; background-color:#C0C0C0;">__</span> ]<sup>2−</sup>
⚫ | PIN = Lithium sulfide
⚫ |Section1={{Chembox Identifiers
⚫ | SMILES1 = ..
| InChI = 1S/2Li.S/q2*+1;-2 | InChI = 1S/2Li.S/q2*+1;-2
| InChIKey1 = GLNWILHOFOBOFD-UHFFFAOYSA-N | InChIKey1 = GLNWILHOFOBOFD-UHFFFAOYSA-N
| CASNo = 12136-58-2 | CASNo = 12136-58-2
| CASNo_Ref = {{cascite|correct|CAS}} | CASNo_Ref = {{cascite|correct|CAS}}
| UNII_Ref = {{fdacite|correct|FDA}}
⚫ | PubChem = 10290727
| UNII = SW6C51V9JZ
| PubChem_Ref = {{Pubchemcite}}
⚫ | PubChem = 10290727
| ChemSpiderID = 8466196 | ChemSpiderID = 8466196
| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}} | ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}}
| EINECS = 235-228-1
| RTECS = OJ6439500 | EINECS = 235-228-1
| SMILES = .. | RTECS = OJ6439500
| SMILES = ..
| StdInChI_Ref = {{stdinchicite|correct|chemspider}} | StdInChI_Ref = {{stdinchicite|correct|chemspider}}
| StdInChI = 1S/2Li.S/q2*+1;-2 | StdInChI = 1S/2Li.S/q2*+1;-2
| StdInChIKey_Ref = {{stdinchicite|correct|chemspider}} | StdInChIKey_Ref = {{stdinchicite|correct|chemspider}}
| StdInChIKey = GLNWILHOFOBOFD-UHFFFAOYSA-N}} | StdInChIKey = GLNWILHOFOBOFD-UHFFFAOYSA-N}}
| Section2 = {{Chembox Properties |Section2={{Chembox Properties
| Formula = Li<sub>2</sub>S | Formula = Li<sub>2</sub>S
| MolarMass = 45.95 g/mol | MolarMass = 45.95 g/mol
| Appearance = white solid | Appearance = white solid
| Density = 1.66 g/cm<sup>3</sup> | Density = 1.67 g/cm<sup>3</sup>
| MeltingPt = 938 °C (1211 K) | MeltingPtC = 938
| BoilingPt = 1372 °C (1645 K) | BoilingPtC = 1372
| Solubility = decomposes to LiOH and H<sub>2</sub>S
| SolubleOther = very soluble in ]
}} }}
| Section3 = {{Chembox Structure |Section3={{Chembox Structure
| CrystalStruct = ] (cubic), ] | CrystalStruct = ] (cubic), ]
| SpaceGroup = Fm<u style="text-decoration:overline">3</u>m, No. 225 | SpaceGroup = Fm<u style="text-decoration:overline">3</u>m, No. 225
| Coordination = Tetrahedral (Li<sup>+</sup>); cubic (S<sup>2–</sup>) | Coordination = Tetrahedral (Li<sup>+</sup>); cubic (S<sup>2−</sup>)
| LattConst_a = | LattConst_a =
| LattConst_alpha = | LattConst_alpha =
}} }}
| Section4 = {{Chembox Thermochemistry |Section4={{Chembox Thermochemistry
| DeltaHf = -9.401 kJ/g | DeltaHf = -9.401 kJ/g or -447 kJ/mol
| DeltaHc = | DeltaHc =
| Entropy = | Entropy = 63 J/mol K
| HeatCapacity = | HeatCapacity =
}} }}
| Section7 = {{Chembox Hazards |Section7={{Chembox Hazards
| ExternalMSDS = | ExternalSDS =
| MainHazards =
| EUIndex = Not listed
| EUClass = | NFPA-H = 3
| RPhrases = | NFPA-F = 1
| SPhrases = | NFPA-R = 1
| MainHazards = | NFPA-S =
| NFPA-H = 3 | FlashPt =
| NFPA-F = 1 | AutoignitionPt =
| LD50 = 240 mg/kg (oral, rat)<ref>https://chem.nlm.nih.gov/chemidplus/rn/12136-58-2 {{Dead link|date=March 2022}}</ref>
| NFPA-R = 1
| NFPA-O =
| FlashPt =
| Autoignition =
}} }}
| Section8 = {{Chembox Related |Section8={{Chembox Related
| OtherAnions = ] | OtherAnions = ]<br />]<br />]<br />]
| OtherCations = ]<br/>] | OtherCations = ]<br />]<br />]<br />]
| OtherFunctn = | OtherFunction =
| Function = | OtherFunction_label =
| OtherCpds = ] | OtherCompounds = ]
}} }}
}} }}
'''Lithium sulfide''' is the ] with the ] Li<sub>2</sub>S. It crystallizes in the antifluorite motif, described as the salt (Li<sup>+</sup>)<sub>2</sub>S<sup>2–</sup>. It forms a solid yellow-white ] powder. In air, it easily hydrolyses to release ] (rotten egg odor).<ref>Greenwood, N. N.; & Earnshaw, A. (1997). Chemistry of the Elements (2nd Edn.), Oxford:Butterworth-Heinemann. ISBN 0-7506-3365-4.</ref> '''Lithium sulfide''' is the ] with the ] ]<sub>2</sub>]. It crystallizes in the antifluorite motif, described as the salt (Li<sup>+</sup>)<sub>2</sub>S<sup>2−</sup>. It forms a solid yellow-white ] powder. In air, it easily hydrolyses to release foul smelling ] gas.<ref>Greenwood, N. N.; & Earnshaw, A. (1997). Chemistry of the Elements (2nd Edn.), Oxford:Butterworth-Heinemann. {{ISBN|0-7506-3365-4}}.</ref>


== Preparation == ==Preparation==
Lithium sulfide is prepared by treating lithium with sulfur.<ref>{{cite web | title= Webelements &ndash; Lithium Sulfide | url=http://www.webelements.com/webelements/compounds/text/Li/Li2S1-12136582.html | accessdate = 2005-09-16}}</ref> This reaction is conveniently conducted in ].<ref>{{Cite journal | doi = 10.1002/9780470132463.ch40 | author = Rankin, D. W. H. | isbn = 9780470132463 | title = Digermanyl Sulfide | journal = ] | year = 1974 | volume = 15 | pages = 182–84}}</ref> Lithium sulfide is prepared by treating lithium with sulfur. This reaction is conveniently conducted in ].<ref>{{Cite journal | doi = 10.1002/9780470132463.ch40 | author = Rankin, D. W. H. | isbn = 978-0-470-13246-3 | title = Digermanyl Sulfide | journal = ] | year = 1974 | volume = 15 | pages = 182–84}}</ref>

:2 Li + S → Li<sub>2</sub>S :2 Li + S → Li<sub>2</sub>S
The THF-soluble ] adduct of lithium sulfide can be generated using ].<ref>Gladysz, J. A.; Wong, V. K. and Jick, B. G., "Reduction of S-S Bonds with LiBHEt3", Tetrahedron, 1979, 35, 2329.</ref>

The THF-soluble ] adduct of lithium sulfide can be generated using ].<ref>{{cite journal|author1=Gladysz, J. A. |author2=Wong, V. K. |author3=Jick, B. G. |title=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|journal=Tetrahedron|year=1979|volume=35|pages=2329–2335|doi=10.1016/S0040-4020(01)93746-9}}</ref>


==Reactions and applications== ==Reactions and applications==
Lithium sulfide has been considered for use in ].<ref>{{cite web | title=Battery claims greater capacity than lithium ion | publisher=Electronics Weekly | url=http://www.electronicsweekly.com/Articles/2005/07/12/35830/Batteryclaimsgreatercapacitythanlithiumion.htm | accessdate = 2005-09-16}}</ref> Lithium sulfide has been considered for use in ].<ref>{{cite web | title=Battery claims greater capacity than lithium ion | date=12 July 2005 | publisher=Electronics Weekly | url=http://www.electronicsweekly.com/Articles/2005/07/12/35830/Batteryclaimsgreatercapacitythanlithiumion.htm | access-date = 2005-09-16}}</ref>


==References== ==References==
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{{Lithium compounds}} {{Lithium compounds}}
{{Sulfides}}


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