Lithium perchlorate

Applications

Inorganic chemistry

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:{{cite journal|title=Lithium Perchlorate Oxygen Candle. Pyrochemical Source of Pure Oxygen|first1=M. M.|last1=Markowitz|first2=D. A.|last2=Boryta|first3=Harvey Jr.|last3=Stewart|journal=Industrial & Engineering Chemistry Product Research and Development|year=1964|volume=3|issue=4|pages=321–330 : Over 60% of the mass of the lithium perchlorate is released as oxygen. It has both the highest oxygen to weight and oxygen to volume ratio of all practical perchlorate salts, and higher oxygen to volume ratio than liquid 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.

Solid lithium perchlorate is found to be a mild and efficient Lewis acid for promoting cyanosilylation of carbonyl compounds under neutral conditions.{{cite journal

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

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.

Safety

Perchlorates often give explosive mixtures with organic compounds, finely divided metals, sulfur, and other reducing agents.

References

References

1. "Lithium perchlorate".
2. (October 1963). "AMCP 706-187 Military Pyrotechnics - Properties of Materials". [[US Army Materiel Command]].
3. (2003). "Crystal Structure of LiClO4". Zeitschrift für Anorganische und Allgemeine Chemie.
4. {{Sigma-Aldrich
5. Herbert Ellern. (1968). "Military and Civilian Pyrotechnics". Chemical Publishing Company.
6. (January 1975). "Encyclopedia of explosives and related items". Picatinny Arsenal.
7. (15 April 2001). "Lithium Perchlorate". J. Wiley & Sons.
8. Xu, Kang. (2004). "Nonaqueous liquid electrolytes for lithium-based rechargeable batteries". Chemical Reviews.
9. "Chlorine Oxides and Chlorine Oxygen Acids".