chloraten

Chloraten is not a standard English term in chemistry. It may be encountered as a misspelling or as a non-English form referring to chlorates, the salts and esters of chloric acid (HClO3). In widely used English nomenclature, the correct term is chlorate, and the corresponding anion is ClO3−.

Chlorates and chlorate salts are strong oxidizers. The chlorate ion has chlorine in the +5 oxidation state. Common chlorate salts include sodium chlorate (NaClO3) and potassium chlorate (KClO3). They are typically soluble in water and are stable under ordinary conditions, though heating or shock can promote decomposition and release oxygen or chlorine dioxide, sometimes with hazardous consequences. Chlorates are reactive with reducing agents and with certain fuels, and they can pose fire and explosion risks if misused or improperly stored.

Production and applications vary. Industrially, chlorates are produced mainly by the electrolytic oxidation of sodium chloride brines to form sodium chlorate, which can be converted into other chlorate salts. Chlorates have historically been used in bleaching and papermaking, as well as in disinfection and chemical synthesis. They have also served as oxidizers in pyrotechnics and, in the past, in some types of matches. Due to safety concerns, their use is regulated in many countries.

Safety and regulation. Because chlorates are potent oxidizers, they must be stored away from organic materials and reductants, kept in appropriate containers, and handled with proper protective equipment. They can be toxic if ingested or inhaled in significant amounts, and improper handling can lead to dangerous reactions.

See also: chlorate, chloric acid, sodium chlorate, potassium chlorate.