Editing Lithium chloride

{{short description|Chemical compound}}
{{Chembox
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| verifiedrevid = 410218986
| ImageFile1 = Lithium chloride.jpg
| ImageName1 = Sample of lithium chloride in a watch glass
| ImageFile = Lithium-chloride-3D-ionic.png
| ImageSize = 150px
| ImageFile2 = File:NaCl polyhedra.svg
| ImageCaption2 = <span style="color:#C0C0C0; background-color:#C0C0C0;">__</span> [[Lithium|Li]]<sup>+</sup>&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;<span style="color:#00FF00;background-color:#00FF00;">__</span> [[Chloride|Cl]]<sup>−</sup>
| ImageName = Unit cell model of lithium chloride
| PIN = Lithium chloride
| SystematicName = Lithium(1+) chloride
|Section1={{Chembox Identifiers
| InChI1 = 1/ClH.Li/h1H;/q;+1/p-1
| InChIKey1 = KWGKDLIKAYFUFQ-REWHXWOFAB
| CASNo = 7447-41-8
| CASNo_Ref = {{cascite|correct|CAS}}
| ChEMBL_Ref = {{ebicite|changed|EBI}}
| ChEMBL = 69710
| PubChem = 433294
| ChemSpiderID = 22449
| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}}
| UNII = G4962QA067
| UNII_Ref = {{fdacite|correct|FDA}}
| EINECS = 231-212-3
| UNNumber = 2056
| MeSHName = Lithium+chloride
| ChEBI_Ref = {{ebicite|correct|EBI}}
| ChEBI = 48607
| RTECS = OJ5950000
| StdInChI_Ref = {{stdinchicite|changed|chemspider}}
| StdInChI = 1S/ClH.Li/h1H;/q;+1/p-1
| StdInChIKey_Ref = {{stdinchicite|changed|chemspider}}
| StdInChIKey = KWGKDLIKAYFUFQ-UHFFFAOYSA-M
| SMILES = [Li+].[Cl-]
| InChI = 1S/ClH.Li/h1H;/q;+1/p-1
| InChIKey = KWGKDLIKAYFUFQ-UHFFFAOYSA-M}}
|Section2={{Chembox Properties
| Formula = LiCl
| Li=1|Cl=1
| Appearance = white solid <br> [[hygroscopic]], sharp
| Density = 2.068 g/cm<sup>3</sup> 
| Solubility = 68.29 g/100 mL (0&nbsp;°C)<br> 74.48 g/100 mL (10&nbsp;°C)<br> 84.25 g/100 mL (25&nbsp;°C)<br> 88.7 g/100 mL (40&nbsp;°C)<br> 123.44 g/100 mL (100&nbsp;°C)<ref name=chemister />
| SolubleOther = soluble in [[hydrazine]], [[n-Methylformamide|methylformamide]], [[n-Butanol|butanol]], [[selenium(IV) oxychloride]], [[1-propanol]]<ref name=chemister />
| Solvent1 = methanol
| Solubility1 = 45.2 g/100 g (0&nbsp;°C)<br> 43.8 g/100 g (20&nbsp;°C)<br> 42.36 g/100 g (25&nbsp;°C)<ref name=sioc>{{cite book|last1 = Seidell|first1 = Atherton|last2 = Linke|first2 = William F.|year = 1952|title = Solubilities of Inorganic and Organic Compounds|publisher = Van Nostrand|url =https://books.google.com/books?id=k2e5AAAAIAAJ|access-date = 2014-06-02}}</ref><br> 44.6 g/100 g (60&nbsp;°C)<ref name=chemister>[http://chemister.ru/Database/properties-en.php?dbid=1&id=614 lithium chloride<!-- Bot generated title -->]</ref>
| Solvent2 = ethanol
| Solubility2 = 14.42 g/100 g (0&nbsp;°C)<br> 24.28 g/100 g (20&nbsp;°C)<br> 25.1 g/100 g (30&nbsp;°C)<br> 23.46 g/100 g (60&nbsp;°C)<ref name=sioc />
| Solvent3 = formic acid
| Solubility3 = 26.6 g/100 g (18&nbsp;°C)<br> 27.5 g/100 g (25&nbsp;°C)<ref name=chemister />
| Solvent4 = acetone
| Solubility4 = 1.2 g/100 g (20&nbsp;°C)<br> 0.83 g/100 g (25&nbsp;°C)<br> 0.61 g/100 g (50&nbsp;°C)<ref name=chemister />
| Solvent5 = liquid ammonia
| Solubility5 = 0.54 g/100 g (−34&nbsp;°C)<ref name=chemister /><br> 3.02 g/100 g (25&nbsp;°C)
| MeltingPtC = 605–614
| BoilingPtC = 1382
| RefractIndex = 1.662 (24&nbsp;°C)
| VaporPressure = 1 torr (785&nbsp;°C)<br> 10 torr (934&nbsp;°C)<br> 100 torr (1130&nbsp;°C)<ref name=chemister />
| Viscosity = 0.87 cP (807&nbsp;°C)<ref name=chemister />
| MagSus = −24.3·10<sup>−6</sup> cm<sup>3</sup>/mol
  }}
|Section3={{Chembox Structure
| MolShape = Linear (gas)
| Coordination = Octahedral 
| Dipole = 7.13 D (gas)
  }}
|Section4={{Chembox Thermochemistry
| DeltaHf = −408.27 kJ/mol<ref name=chemister />
| DeltaGf = −384 kJ/mol<ref name=chemister />
| DeltaHc = 
| Entropy = 59.31 J/mol·K<ref name=chemister />
| HeatCapacity = 48.03 J/mol·K<ref name=chemister />
  }}
| Section6 = {{Chembox Pharmacology
| Pharmacology_ref = 
| ATCCode_prefix = V04
| ATCCode_suffix = CX11
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|Section7={{Chembox Hazards
| ExternalSDS = [http://www.ilo.org/public/english/protection/safework/cis/products/icsc/dtasht/_icsc07/icsc0711.htm ICSC 0711]
| GHSPictograms = {{GHS07}}<ref name="sigma">{{Sigma-Aldrich|id=203637|name=Lithium chloride|accessdate=2014-05-09}}</ref>
| GHSSignalWord = Warning
| HPhrases = {{H-phrases|302|315|319|335}}<ref name="sigma" />
| PPhrases = {{P-phrases|261|305+351+338}}<ref name="sigma" />
| NFPA-H = 2
| NFPA-R = 0
| NFPA-F = 0
| FlashPt = Non-flammable
| LD50 = 526 mg/kg (oral, rat)<ref>[https://chem.nlm.nih.gov/chemidplus/rn/7447-41-8 ChemIDplus - 7447-41-8 - KWGKDLIKAYFUFQ-UHFFFAOYSA-M - Lithium chloride - Similar structures search, synonyms, formulas, resource links, and other chemical information<!-- Bot generated title -->]</ref>
  }}
|Section8={{Chembox Related
| OtherAnions = [[Lithium fluoride]]<br/>[[Lithium bromide]]<br/>[[Lithium iodide]]<br/>[[Lithium astatide]]
| OtherCations = [[Sodium chloride]]<br/>[[Potassium chloride]]<br/>[[Rubidium chloride]]<br/>[[Caesium chloride]]<br/>[[Francium chloride]]
  }}
}}

'''Lithium chloride''' is a [[chemical compound]] with the [[chemical formula|formula]] [[Lithium|Li]][[Chlorine|Cl]]. The [[salt (chemistry)|salt]] is a typical [[ionic compound]] (with certain covalent characteristics), although the small size of the Li<sup>+</sup> ion gives rise to properties not seen for other alkali metal chlorides, such as extraordinary solubility in polar [[solvent]]s (83.05&nbsp;g/100&nbsp;mL of water at 20&nbsp;°C) and its [[hygroscopic]] properties.<ref name=Ullmann/>

==Chemical properties==
[[File:FlammenfärbungLi.png|thumb|75px|left|Color produced when lithium chloride is heated]]
The salt forms crystalline [[water of crystallization|hydrates]], unlike the other alkali metal chlorides.<ref>Holleman, A. F.; Wiberg, E. ''Inorganic Chemistry'' Academic Press: San Diego, 2001. {{ISBN|0-12-352651-5}}.</ref>  Mono-, tri-, and pentahydrates are known.<ref>{{cite journal |author1=Hönnerscheid Andreas |author2=Nuss Jürgen |author3=Mühle Claus |author4=Jansen Martin | year = 2003 | title = Die Kristallstrukturen der Monohydrate von Lithiumchlorid und Lithiumbromid | journal = Zeitschrift für anorganische und allgemeine Chemie | volume = 629 | issue = 2| pages = 312–316 | doi = 10.1002/zaac.200390049 }}</ref>  The anhydrous salt can be regenerated by heating the hydrates. LiCl also absorbs up to four equivalents of [[ammonia]]/mol. As with any other ionic chloride, solutions of lithium chloride can serve as a source of [[chloride]] ion, e.g., forming a precipitate upon treatment with [[silver nitrate]]:
: LiCl + AgNO<sub>3</sub>  →  AgCl + LiNO<sub>3</sub>

==Preparation==
Lithium chloride is produced by treatment of [[lithium carbonate]] with [[hydrochloric acid]].<ref name=Ullmann>{{Ullmann |doi=10.1002/14356007.a15_393|title=Lithium and Lithium Compounds|first1=Ulrich |last1=Wietelmann|first2=Richard J.|last2=Bauer|year=2005}}</ref> Anhydrous LiCl is prepared from the hydrate by heating in a stream of [[hydrogen chloride]].

==Uses==
===Commercial applications===
Lithium chloride is mainly used for the production of [[lithium]] metal by [[electrolysis]] of a LiCl/[[potassium chloride|KCl]] melt at {{convert|450|C|F}}.  LiCl is also used as a brazing [[Flux (metallurgy)|flux]] for [[aluminium]] in [[automobile]] parts. It is used as a [[desiccant]] for drying air streams.<ref name=Ullmann/>  In more specialized applications, lithium chloride finds some use in [[organic synthesis]], e.g., as an additive in the [[Stille reaction]]. Also, in biochemical applications, it can be used to precipitate [[RNA]] from cellular extracts.<ref>{{cite journal
| doi= 10.1089/dna.1983.2.329
| author1= Cathala, G. | author2=Savouret, J. | author3=Mendez, B. | author4=West, B. L. | author5=Karin, M. | author6=Martial, J. A. | author7=Baxter, J. D.
| title = A Method for Isolation of Intact, Translationally Active Ribonucleic Acid
| journal = DNA
| year = 1983
| volume = 2
| issue = 4
| pages = 329–335
| pmid = 6198133 }}</ref>

Lithium chloride is also used as a [[Pyrotechnic colorant|flame colorant]] to produce dark red flames.

===Niche uses===
Lithium chloride is used as a relative humidity standard in the calibration of [[hygrometer]]s.  At {{convert|25|C|F}} a saturated solution (45.8%) of the salt will yield an equilibrium relative humidity of 11.30%. Additionally, lithium chloride can be used as a hygrometer. This deliquescent salt forms a self-solution when exposed to air.  The equilibrium LiCl concentration in the resulting solution is directly related to the relative humidity of the air. The percent relative humidity at {{convert|25|C|F}} can be estimated, with minimal error in the range {{convert|10-30|C}}, from the following first-order equation: RH=107.93-2.11C, where C is solution LiCl concentration, percent by mass.

Molten LiCl is used for the preparation of [[carbon nanotube]]s,<ref>{{cite journal | doi=10.1016/j.carbon.2014.05.089 | volume=77 | title=Towards large scale preparation of carbon nanostructures in molten LiCl | journal=Carbon | pages=835–845| year=2014 | last1=Kamali | first1=Ali Reza | last2=Fray | first2=Derek J. | doi-access=free }}</ref> [[graphene]]<ref>{{cite journal | journal = Nanoscale| year= 2015|volume = 7| issue= 26|pages= 11310–11320 | doi = 10.1039/c5nr01132a| pmid= 26053881| title=Large-scale preparation of graphene by high temperature insertion of hydrogen into graphite|url= https://www.repository.cam.ac.uk/bitstream/1810/248812/1/Kamali%20%26%20Fray%202015%20Nanoscale.pdf| last1= Kamali| first1= Ali Reza| last2= Fray| first2= Derek J.| doi-access= free}}</ref> and [[lithium niobate]].<ref>{{cite journal | doi = 10.1016/j.ceramint.2013.07.085 | volume=40 | title=Preparation of lithium niobate particles via reactive molten salt synthesis method | journal=Ceramics International | pages=1835–1841| year=2014 | last1=Kamali | first1=Ali Reza | last2=Fray | first2=Derek J. }}</ref>

Lithium chloride has been shown to have strong [[acaricide|acaricidal]] properties, being effective against ''[[Varroa destructor]]'' in populations of [[honey bee]]s.<ref>{{Cite journal|last1=Ziegelmann|first1=Bettina|last2=Abele|first2=Elisabeth|date=January 12, 2018|title=Lithium chloride effectively kills the honey bee parasite ''Varroa destructor'' by a systemic mode of action|journal=[[Scientific Reports]]|volume=8|issue=1|doi=10.1038/s41598-017-19137-5|pmid=29330449|pmc=5766531|page=683 |bibcode=2018NatSR...8..683Z}}</ref>

Lithium chloride is used as an aversive agent in lab animals to study [[conditioned place preference|conditioned place preference and aversion]].

==Precautions==
Lithium salts affect the [[central nervous system]] in a variety of ways. While the [[lithium citrate|citrate]], [[lithium carbonate|carbonate]], and [[lithium orotate|orotate]] salts are currently used to treat [[bipolar disorder]], other [[lithium salts]] including the chloride were used in the past. For a short time in the 1940s lithium chloride was manufactured as a [[salt substitute]] for people with hypertension, but this was prohibited after the toxic effects of the compound ([[tremor|tremors]], [[fatigue]], [[nausea]]) were recognized.<ref name="talbott">{{cite journal
| author= Talbott J. H.
| title = Use of lithium salts as a substitute for sodium chloride
| journal = Arch Intern Med
| year = 1950
| volume = 85
| issue = 1
| pages = 1–10
| pmid = 15398859
| doi=10.1001/archinte.1950.00230070023001}}</ref><ref>{{cite journal
| author1= L. J. Stone | author2=M. luton | author3=J. Gilroy
| title = Lithium Chloride as a Substitute for Sodium Chloride in the Diet
| journal = Journal of the American Medical Association
| year = 1949
| volume = 139
| issue = 11
| pages = 688–692
| doi =10.1001/jama.1949.02900280004002
| pmid= 18128981 }}</ref><ref>{{cite news | magazine = [[Time (magazine)|Time]] | title = Case of trie Substitute Salt | date = 28 February 1949 | url = http://www.time.com/time/magazine/article/0,9171,799873,00.html| archive-url = https://web.archive.org/web/20070302040542/http://www.time.com/time/magazine/article/0,9171,799873,00.html| url-status = dead| archive-date = March 2, 2007}}</ref> It was, however, noted by J. H. Talbott that many symptoms attributed to lithium chloride toxicity may have also been attributable to [[salt deficiency|sodium chloride deficiency]], to the diuretics often administered to patients who were given lithium chloride, or to the patients' underlying conditions.<ref name="talbott" />

==See also==
*[[Lithium chloride (data page)]]
*[[Solubility table]]

==References==
{{reflist}}
* ''Handbook of Chemistry and Physics'', 71st edition, CRC Press, Ann Arbor, Michigan, 1990.
* N. N. Greenwood, A. Earnshaw, ''Chemistry of the Elements'', 2nd ed., Butterworth-Heinemann, Oxford, UK, 1997.
* R. Vatassery, titration analysis of LiCl, sat'd in Ethanol by AgNO<sub>3</sub> to precipitate AgCl(s). EP of this titration gives %Cl by mass.
* H. Nechamkin, ''The Chemistry of the Elements'', McGraw-Hill, New York, 1968.

==External links==

* [https://cdnsciencepub.com/doi/pdf/10.1139/v52-020 Radiochemical measurements of activity coefficients, from Betts & MacKenzie, Can. J. Chem.] 
{{Commons category|Lithium chloride}}

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[[Category:Chlorides]]
[[Category:Alkali metal chlorides]]
[[Category:Lithium salts]]
[[Category:Metal halides]]
[[Category:Mood stabilizers]]
[[Category:Desiccants]]
[[Category:Rock salt crystal structure]]