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.
Over 60% of the mass of the lithium perchlorate is released as oxygen.[2] 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.[6]
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 acidicLi+ binds to Lewis basic sites on the dienophile, thereby accelerating the reaction.[8]
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.[9]
Solid lithium perchlorate is found to be a mild and efficient Lewis acid for promoting cyanosilylation of carbonyl compounds under neutral conditions.[10]
Lithium perchlorate is also used as an electrolyte salt in lithium-ion batteries. Lithium perchlorate is chosen over alternative salts such as lithium hexafluorophosphateorlithium tetrafluoroborate when its superior electrical impedance, conductivity, hygroscopicity, and anodic stability properties are of importance to the specific application.[11] 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.[11]
^Wickleder, Mathias S. (2003). "Crystal Structure of LiClO4". Zeitschrift für Anorganische und Allgemeine Chemie. 629 (9): 1466–1468. doi:10.1002/zaac.200300114.
^Markowitz, M. M.; Boryta, D. A.; Stewart, Harvey Jr. (1964). "Lithium Perchlorate Oxygen Candle. Pyrochemical Source of Pure Oxygen". Industrial & Engineering Chemistry Product Research and Development. 3 (4): 321–330. doi:10.1021/i360012a016.
^Herbert Ellern (1968). Military and Civilian Pyrotechnics. Chemical Publishing Company. p. 237. ISBN978-0-8206-0364-3. OL37082807M.
^Basil T. Fedoroff; Oliver E. Sheffield (January 1975). "Lithium Perchlorate". Encyclopedia of explosives and related items. Vol. 7. Picatinny Arsenal. p. L45. LCCN61-61759.
^Charette, A. B. "Lithium Perchlorate" in Encyclopedia of Reagents for Organic Synthesis (Ed: L. Paquette) 2004, J. Wiley & Sons, New York. doi:10.1002/047084289X.
^N. Azizi, M.R. Saidi (2003). "An improved synthesis of cyanohydrins in the presence of solid LiClO4 under solvent-free conditions". Journal of Organometallic Chemistry. 688 (1–2): 283–285. doi:10.1016/j.jorganchem.2003.09.014.
^ abHelmut Vogt, Jan Balej, John E. Bennett, Peter Wintzer, Saeed Akbar Sheikh, Patrizio Gallone "Chlorine Oxides and Chlorine Oxygen Acids" in Ullmann's Encyclopedia of Industrial Chemistry 2002, Wiley-VCH. doi:10.1002/14356007.a06_483
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