Перхлорат лития: свойства, применение и безопасность

Chemical compound
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| Verifiedfields = changed
| Watchedfields = changed
| verifiedrevid = 451153890
| Name = Lithium perchlorate
| ImageFile = Lithium perchlorate. png
| ImageSize = 150px
| ImageFile1 = Lithiumperchlorat. png
| ImageSize1 = 240px
| ImageCaption1 = Li+      Cl7+      O2− Unit cell of lithium perchlorate. | ImageAlt1 = The orthorhombic unit cell of lithium perchlorate under standard conditions. | ImageName = Lithium perchlorate
| IUPACName = Lithium perchlorate
| OtherNames = Perchloric acid, lithium salt; Lithium Cloricum
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| Section4 = Chembox Thermochemistry
| DeltaHf = −380.99 kJ/mol
| DeltaGf = −254 kJ/mol
| GHSSignalWord = Danger
| HPhrases =
LiClO4 → LiCl + 2 O2
Over 60% of the mass of the lithium perchlorate is released as oxygen. Lithium perchlorate is used as an oxidizer in solid rocket propellants, and to produce red colored flame in pyrotechnic compositions.

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. 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.

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.

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