Lithium bromide: Difference between revisions

| Watchedfields = changed

| verifiedrevid = 450703470

| ImageFile1 = File:NaCl_polyhedra.png

| ImageCaption1 = <span style="color:#C0C0C0; background-color:#C0C0C0;">__</span> [[Lithium|Li]]⁺&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;<span style="color:#00FF00;background-color:#00FF00;">__</span> [[Bromide|Br]]⁻

| ImageFile2 = Lithium-bromide-3D-ionic.png

|Section1={{Chembox Identifiers

| CASNo_Ref = {{cascite|correct|CAS}}

|Section2={{Chembox Properties

| MolarMass = 86.845 g/mol<ref name=r1/>

| Appearance = White [[hygroscopic]] solid<ref name=r1/>

| Density = 3.464 g/cm³<ref name=r1/>

| MeltingPtC = 550

| MeltingPt_ref = <ref name=r1>Haynes, p. 4.70</ref>

| BoilingPtC = 1300

| BoilingPt_ref = <ref name=r1/>

| Solubility = 143 g/100 mL (0 °C) <br> 166.7 g/100 mL (20 °C) <br> 266 g/100 mL (100 °C)<ref>Haynes, p. 5.169</ref>

| SolubleOther = soluble in [[methanol]], [[ethanol]],<ref name=r1/> [[diethyl ether|ether]],<ref name=r1/> [[acetone]] <br> slightly soluble in [[pyridine]]

| RefractIndex = 1.7843 (589 nm)<ref>Haynes, p. 10.249</ref>

| MagSus = −34.3·10⁻⁶ cm³/mol<ref>Haynes, p. 4.128</ref>

| Section3 = {{Chembox Structure

| Structure_ref =<ref>{{cite journal|doi=10.1002/zaac.19723910311|title=Über die Systeme Alkalimetallbromid/Mangan(II)-bromid|year=1972|last1=Seifert|first1=H.-J.|last2=Dau|first2=E.|journal=Zeitschrift für Anorganische und Allgemeine Chemie|volume=391|issue=3|pages=302–312}}</ref>

| CrystalStruct = Cubic, [[Pearson symbol]] cF8, No. 225

| SpaceGroup = Fm{{overline|3}}m

| LattConst_a = 0.5496 nm

}}

|Section4={{Chembox Thermochemistry

| Thermochemistry_ref=<ref>Haynes, p. 5.25</ref>

| DeltaHf = -351.2 kJ/mol

| DeltaHc =

| DeltaGf = -342.0 kJ/mol

| Entropy = 74.3 J/mol K

|Section5={{Chembox Hazards

| GHSPictograms = {{GHS07}}

| GHSSignalWord = Warning

| HPhrases = {{H-phrases|315|317|319}}<ref>[https://www.sigmaaldrich.com/catalog/product/aldrich/229733?lang=en&region=US Lithium bromide]. SIgma Aldrich</ref>

| FlashPt = Not-flammable

| LD50 = 1800 mg/kg (oral, rat)<ref>{{cite web|url=https://chem.nlm.nih.gov/chemidplus/rn/7550-35-8|title=ChemIDplus – 7550-35-8 – AMXOYNBUYSYVKV-UHFFFAOYSA-M – Lithium bromide – Similar structures search, synonyms, formulas, resource links, and other chemical information.|first=Michael|last=Chambers|website=chem.sis.nlm.nih.gov|access-date=3 April 2018}}</ref>

|Section8={{Chembox Related

| OtherAnions = [[Lithium fluoride]]<br/>[[Lithium chloride]]<br/>[[Lithium iodide]]

| OtherCations = [[Sodium bromide]]<br/>[[Potassium bromide]]<br/>[[Rubidium bromide]]<br/>[[Caesium bromide]]

'''Lithium bromide''' ('''LiBr''') is a [[chemical compound]] of [[lithium]] and [[bromine]]. Its extreme [[hygroscopic]] character makes LiBr useful as a [[desiccant]] in certain [[air conditioning]] systems.<ref name=Ullmann>Wietelmann, Ulrich and Bauer, Richard J. (2005) "Lithium and Lithium Compounds" in ''Ullmann's Encyclopedia of Industrial Chemistry'' Wiley-VCH: Weinheim. {{doi|10.1002/14356007.a15_393.pub2}}</ref>

[[File:Sollibr.PNG|thumb|left|Solubility of LiBr in water as a function of temperature]]

[[File:LiBr-Phase.svg|thumb|left|Phase diagram of LiBr]]

LiBr is prepared by treating an aqueous suspension of lithium carbonate with [[hydrobromic acid]] or by reacting [[lithium hydroxide]] with bromine.<ref name=Ullmann/> It forms several crystalline [[water of crystallization|hydrates]], unlike the other alkali metal bromides.<ref>{{Holleman&Wiberg|page=}}</ref>

Lithium hydroxide and hydrobromic acid (aqueous solution of hydrogen bromide) will precipitate lithium bromide in the presence of water.

:LiOH + HBr → LiBr + H₂O

A 50–60% aqueous solution of lithium bromide is used in air-conditioning systems as [[desiccation|desiccant]]. It is also used in absorption chilling along with water (see [[absorption refrigerator]]). Solid LiBr is a useful reagent in [[organic synthesis]]. It is included into oxidation and [[hydroformylation]] catalysts; it is also used for deprotonation and dehydration of organic compounds containing acidic protons, and for the purification of [[steroid]]s and [[prostaglandin]]s.<ref name=Ullmann/>

Lithium bromide was used as a [[sedative]] beginning in the early 1900s, but it fell into disfavor in the 1940s as newer sedatives became available and when some heart patients died after using the salt substitute lithium chloride.<ref>{{cite web|url=http://www.webmd.com/content/Article/87/99356.htm?pagenumber=1|title=Bipolar Disorder: Treatment and Care|website=webmd.com|access-date=3 April 2018}}</ref> Like [[lithium carbonate]] and [[lithium chloride]], it was used as treatment for [[bipolar disorder]].

[[Lithium salts]] are [[psychoactive]] and somewhat corrosive. Heat is quickly generated when lithium bromide is dissolved into water because it has a negative [[enthalpy of solution]].

{{reflist}}

==Cited sources==

*{{cite book | editor= Haynes, William M. | date = 2016| title = [[CRC Handbook of Chemistry and Physics]] | edition = 97th | publisher = [[CRC Press]] | isbn = 9781498754293}}

{{Commons category|Lithium bromide}}

* {{cite web | title= A PDF file from GFS Chemicals, a supplier of lithium bromide | url= http://www.gfschemicals.com/Search/MSDS/5035MSDS.PDF | access-date= 2005-09-15 | archive-url= https://web.archive.org/web/20060316211633/http://www.gfschemicals.com/Search/MSDS/5035MSDS.PDF | archive-date= 2006-03-16 | url-status= dead }}

{{Sedatives}}

{{Mood stabilizers}}

{{GABAAR PAMs}}

{{bromides}}

{{Authority control}}

[[Category:Lithium salts]]

[[Category:Mood stabilizers]]

[[Category:Sedatives]]

[[Category:GABAA receptor positive allosteric modulators]]

[[Category:Rock salt crystal structure]]