Inorganic chemistry Lithium perchlorate is used as a source of
oxygen in some
chemical oxygen generators. It decomposes at about , yielding
lithium chloride and
oxygen: Lithium perchlorate is used as an
oxidizer in some experimental (as of 1975)
solid rocket propellants, and rarely to produce red
colored flame in pyrotechnic compositions.
Organic chemistry 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. 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.
Batteries Lithium perchlorate is also used as an
electrolyte salt in
lithium-ion batteries. Lithium perchlorate is chosen over alternative salts such as
lithium hexafluorophosphate or
lithium tetrafluoroborate when its superior
electrical impedance,
conductivity,
hygroscopicity, and anodic stability properties are of importance to the specific application. However, these beneficial properties are often overshadowed by the electrolyte's strong
oxidizing properties, making the electrolyte reactive toward its
solvent at high temperatures and/or high
current loads. Due to these hazards the battery is often considered unfit for industrial applications.
Biochemistry Concentrated solutions of lithium perchlorate () are used as a
chaotropic agent to denature
proteins. ==Production==