Lihat sumber Litium sulfida

{{Chembox
| Watchedfields = changed
| Name = Litium sulfida
| verifiedrevid = 446984298
| IUPACName = Litium hidrosulfida
| ImageFile = Sodium-oxide-unit-cell-3D-balls-B.png
| ImageSize = 250px
| PIN = Litium sulfida
|Section1={{Chembox Identifiers
| SMILES1 = [Li+].[Li+].[S-2]
| InChI = 1S/2Li.S/q2*+1;-2
| InChIKey1 = GLNWILHOFOBOFD-UHFFFAOYSA-N
| CASNo = 12136-58-2
| CASNo_Ref = {{cascite|correct|CAS}}
| PubChem = 10290727
| ChemSpiderID = 8466196
| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}}
| EINECS = 235-228-1
| RTECS = OJ6439500
| SMILES = [Li+].[Li+].[S-2]
| StdInChI_Ref = {{stdinchicite|correct|chemspider}}
| StdInChI = 1S/2Li.S/q2*+1;-2
| StdInChIKey_Ref = {{stdinchicite|correct|chemspider}}
| StdInChIKey = GLNWILHOFOBOFD-UHFFFAOYSA-N}}
|Section2={{Chembox Properties
| Formula = Li<sub>2</sub>S
| MolarMass = 45,95 g/mol
| Appearance = padatan putih
| Density = 1,66 g/cm<sup>3</sup>
| MeltingPt = 938&nbsp;°C
| BoilingPt = 1372&nbsp;°C
| Solubility = sangat mudah larut
| SolubleOther = sangat mudah larut dalam [[etanol]]
  }}
|Section3={{Chembox Structure
| CrystalStruct = [[Antifluorit]] (kubik), [[Simbol Pearson|''cF12'']]
| SpaceGroup = Fm<u style="text-decoration:overline">3</u>m, No. 225 
| Coordination = Tetrahedral (Li<sup>+</sup>); kubik (S<sup>2−</sup>)
| LattConst_a = 
| LattConst_alpha = 
  }}
|Section4={{Chembox Thermochemistry
| DeltaHf = -9,401 kJ/g atau -447 kJ/mol
| DeltaHc = 
| Entropy = 63 J/mol K
| HeatCapacity = 
  }}
|Section7={{Chembox Hazards
| ExternalSDS = [http://www.espi-metals.com/msds%27s/Lithium%20Sulfide.htm External MSDS]
| EUClass = 
| RPhrases = 
| SPhrases = 
| MainHazards = 
| NFPA-H = 3
| NFPA-F = 1
| NFPA-R = 1
| NFPA-S = 
| FlashPt = 
| AutoignitionPt = 
| LD50 = 240 mg/kg (oral, tikus)<ref>http://chem.sis.nlm.nih.gov/chemidplus/rn/12136-58-2</ref>
  }}
|Section8={{Chembox Related
| OtherAnions = [[Litium oksida]]
| OtherCations = [[Natrium sulfida]]<br/>[[Kalium sulfida]]
| OtherFunctn = 
| OtherFunctn_label = 
| OtherCompounds = [[Litium hidrosulfida]]
  }}
}}
'''Litium sulfida''' adalah [[senyawa anorganik]] dengan [[rumus kimia]] Li{{sub|2}}S. Senyawa ini mengkristal dengan motif antifluorit, yang dijelaskan sebagai garam (Li<sup>+</sup>)<sub>2</sub>S<sup>2−</sup>. Senyawa ini berbentuk padatan kuning-putih serbuk [[higroskopi]]s. Di udara, senyawa ini mudah terhidrolisis dan melepaskan [[hidrogen sulfida]] (bau telur busuk).<ref>Greenwood, N. N.; & Earnshaw, A. (1997). Chemistry of the Elements (2nd Edn.), Oxford:Butterworth-Heinemann. {{ISBN|0-7506-3365-4}}.</ref>

== Pembuatan ==
Litium sulfida dibuat dengan cara memberi perlakuan litium dengan belerang.<ref>{{cite web | title= Webelements – Lithium Sulfide | url=http://www.webelements.com/webelements/compounds/text/Li/Li2S1-12136582.html | accessdate = 2005-09-16}}</ref> Reaksi ini mudah dilakukan dalam [[amonia anhidrat]].<ref>{{Cite journal | doi = 10.1002/9780470132463.ch40 | author = Rankin, D. W. H. | isbn = 978-0-470-13246-3 | title = Digermanyl Sulfide | journal = [[Inorganic Syntheses|Inorg. Synth.]] | year = 1974 | volume = 15 | pages = 182–84}}</ref>
:<chem>2Li + S -> Li2S</chem>
{{Ill|Aduk|en|adduct}} [[trietilborana]] litium sulfida yang larut dalam THF dapat dibuat menggunakan [[superhidrida]].<ref>Gladysz, J. A.; Wong, V. K. and Jick, B. G., "Reduction of S-S Bonds with LiBHEt3", Tetrahedron, 1979, 35, 2329.</ref>

== Reaksi dan aplikasi ==
Litium sulfida telah dipertimbangkan untuk digunakan dalam [[baterai litium belerang]].<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>

== Referensi ==
{{Reflist}}

== Pranala luar ==
* [http://loradchemical.com/sulf/lithium-sulfide.html Lithium Sulfide]

{{Senyawa litium}}
{{Sulfida}}

{{Authority control}}


{{Senyawa-stub}}