ClO4

ClO4 commonly denotes the perchlorate ion, ClO4−, a tetrahedral oxoanion in which chlorine is in the +7 oxidation state. Four oxygen atoms surround a central chlorine atom, giving a -1 overall charge. Perchlorate salts are typically water-soluble and widely used as oxidizers in various industrial applications.

Perchlorates are produced industrially as salts such as ammonium perchlorate (NH4ClO4), sodium perchlorate (NaClO4), and potassium perchlorate (KClO4). Ammonium perchlorate is a major oxidizer in solid rocket propellants and pyrotechnics; perchlorates are also used in electroplating, etching, and analytical chemistry. Perchloric acid (HClO4) is a strong mineral acid used in synthesis and cleaning and as a laboratory reagent.

As strong oxidizers, perchlorates are highly reactive and can form explosive mixtures with organic materials, particularly when dry. They are generally stable under normal conditions but decompose upon heating or shock, releasing oxygen. They react readily with reducing agents and certain metals; therefore, safe storage requires avoiding contact with organics, heat, and incompatible materials.

Environmental and health considerations show that perchlorate is persistent in the environment and can contaminate water near production sites or improper disposal. In humans, perchlorate can interfere with thyroid iodine uptake, potentially affecting thyroid function, with regulatory guidance varying by jurisdiction. Removal from water is often achieved by ion-exchange resins or reverse osmosis; detection is commonly performed by ion chromatography or related analytical techniques.

Regulatory and safety considerations vary by country, reflecting the material’s oxidizing properties and potential health and environmental impacts.