Lithium perchlorate

Lithium perchlorate
IUPAC name Lithium perchlorate
Other names Perchloric acid, lithium salt; Lithium Cloricum
Identifiers
CAS number	7791-03-9 Y
PubChem	23665649
ChemSpider	133514 Y
Jmol-3D images	{{#if:[Li+].[O-]Cl(=O)(=O)=O|Image 1
SMILES [Li+].[O-]Cl(=O)(=O)=O
InChI InChI=1S/ClHO4.Li/c2-1(3,4)5;/h(H,2,3,4,5);/q;+1/p-1 Y Key: MHCFAGZWMAWTNR-UHFFFAOYSA-M Y InChI=1/ClHO4.Li/c2-1(3,4)5;/h(H,2,3,4,5);/q;+1/p-1 Key: MHCFAGZWMAWTNR-REWHXWOFAR
Properties
Molecular formula	LiClO4
Molar mass	106.392 g/mol
Appearance	white crystals
Odor	odorless
Density	2.42 g/cm3, solid
Melting point	236 °C
Boiling point	430 °C (with decomp.)
Solubility in water	60 g/100 mL
Solubility in organic solvents	Soluble
Thermochemistry
Std enthalpy of formation ΔfHo298	-3.581 kJ/g or -380.99 kJ/mol
Hazards
MSDS	MSDS
Main hazards	Oxidizer, irritant
NFPA 704	0 2 0 OX
Related compounds
Other anions	Lithium chloride Lithium hypochlorite Lithium chlorate
Other cations	Sodium perchlorate Potassium perchlorate Rubidium perchlorate
Y (verify) (what is: Y/N?) Except where noted otherwise, data are given for materials in their standard state (at 25 °C (77 °F), 100 kPa)
Infobox references

Lithium perchlorate is the inorganic compound with the formula LiClO₄. This white or colourless 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, the latter being over 60% of its mass. It has both the highest oxygen to weight and oxygen to volume ratio of all perchlorates, except beryllium diperchlorate (which is expensive and highly toxic).

LiClO₄ is highly soluble in organic solvents, even diethyl ether. Such solutions are employed in Diels-Alder reactions, where it is proposed that the Lewis acidic Li⁺ binds to Lewis basic sites on the dienophile, thereby accelerating the reaction.^[1]

Lithium perchlorate is also used as an inert electrolyte in lithium batteries.

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

Lithium perchlorate is also used as a co-catalyst in the coupling of α,β-unsaturated carbonyls with aldehydes, also known as the Baylis-Hillman reaction.^[2]

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.^[3]

Safety

Perchlorates often give explosive mixtures with organic compounds.^[3]

External links

• WebBook page for LiClO4

References