Lithium perchlorate

Chembox new
Name = Lithium perchlorate
ImageFile = Lithium perchlorate.png ImageSize = 150px
ImageName = Lithium perchlorate
IUPACName = Lithium perchlorate
OtherNames = Perchloric acid, lithium salt
Section1 = Chembox Identifiers
CASNo = 7791-03-9
Section2 = Chembox Properties
Formula = LiClO₄
MolarMass = 106.39 g/mol
Appearance = white crystals
Density = 2.43 g/cm³, solid
Solubility = 60 g/100 mL
MeltingPt = 236 °C
BoilingPt = 430 °C (with decomp.)
Section3 = Chembox Structure
Coordination =
CrystalStruct =
Section7 = Chembox Hazards
ExternalMSDS = [http://www.jtbaker.com/msds/englishhtml/l7000.htm External MSDS]
MainHazards = Oxdizer
Irritatant
Section8 = Chembox Related
OtherCations = Caesium perchlorate; potassium perchlorate

Lithium perchlorate is the chemical compound with the formula LiClO₄. This white crystalline salt is noteworthy for its high solubility in many solvents. It exists both in anhydrous form and as a trihydrate.

Uses

Lithium perchlorate is used as a source of oxygen in some chemical oxygen generators. It decomposes at about 400 °C, yielding lithium chloride and oxygen. It has both the highest oxygen to weight and oxygen to volume ratio of all perchlorates, which makes it especially advantageous in aerospace applications.

LiClO₄ is highly soluble in organic solvents, even diethyl ether. Such solutions are employed in the Diels-Alder reactions, where it is proposed that the Lewis acidic Li⁺ binds to substituents on the diene, thereby accelerating the reaction. [Charette, A. B. "Lithium Perchlorate" in Encyclopedia of Reagents for Organic Synthesis (Ed: L. Paquette) 2004, J. Wiley & Sons, New York. DOI: 10.1002/047084289.]

Lithium perchlorate is also extensively used as an electrolyte in lithium batteries, as it does not undergo oxidization on the anode.

Concentrated solutions of lithium perchlorate (4.5 mol/l) are used as a chaotropic agent to denature proteins.

Production

Lithium perchlorate can be manufactured by reaction of sodium perchlorate with lithium chloride. It can be also prepared by electrolysis of lithium chlorate at 200 mA/cm² at temperatures above 20 °C.Fact|date=February 2007

afety

Perchlorates often give explosive mixtures with organic compounds.

References