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The hypochlorite ion is ClO−. A hypochlorite compound is a chemical compound containing this group, with chlorine in oxidation state +1.
Hypochlorites are the salts of hypochlorous acid. Common examples include sodium hypochlorite (chlorine bleach or bleaching agent) and calcium hypochlorite (bleaching powder). Hypochlorites are frequently quite unstable — for example, sodium hypochlorite is not available as a solid, since removal of the water from NaClO solution converts it to a mixture of sodium chloride and sodium chlorate. Heating of NaClO solution also causes this reaction. Hypochlorites decompose in sunlight, giving chlorides and oxygen.
Due to their low stability, hypochlorites are very strong oxidizing agents. They react with many organic and inorganic compounds. Reaction with organic compounds is very exothermic and may cause ignition, so hypochlorites should be handled with care. They can oxidize manganese compounds, converting them to permanganates.
Examples
- Calcium hypochlorite, Ca(ClO)2
- Ethyl hypochlorite, C2H5ClO
- Lithium hypochlorite, LiClO
- Methyl hypochlorite, CH3ClO
- Sodium hypochlorite, NaClO
- tert-Butyl hypochlorite, C4H9ClO
Strength of oxidation
Hypochlorite is the strongest oxidizer of the generalized chlorates. It is also the least stable.
Stability
Many hypochlorite "compounds" exist only in solution, and are nonexistent in a pure form, as is hypochlorous acid itself.
Besides oxidizing almost any reducing agent, hypochlorite is unstable with respect to disproportionation (that is, it will oxidize itself); hypochlorite will often degrade to some mixture of chloride and chlorate, especially if not kept cool.
"Hypochlorite"