Hypochlorite
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2008-06-22T07:12:14Z
Footballplar951
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/* Examples */
[[Image:Hypochlorite-3D-vdW.png|thumb|right|200px|The chlorate(I) ion]]
The '''hypochlorite(I)''' [[ion]] is [[Chlorine|Cl]][[Oxygen|O]]<sup>−</sup>. A chlorite(I) compound is a [[chemical compound]] containing this group, with chlorine in [[oxidation state]] +1.
Chlorites(I) are the [[salt (chemistry)|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(I) 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. Chlorites(I) decompose in sunlight, giving chlorides and oxygen.
Due to their low stability, chlorites(I) are very strong [[oxidizing agent]]s. They react with many organic and inorganic compounds. Reaction with organic compounds is very exothermic and may cause [[Combustion|ignition]], so chlorites(I) should be handled with care. They can oxidize manganese compounds, converting them to [[permanganate]]s.
==Strength of oxidation==
Chlorate(I) is the strongest oxidizer of the generalized [[chlorate]]s. It is also the least stable.
==Stability==
Many chlorate(I) compounds exist only in solution, and are nonexistent in a pure form, as is [[Chloric acid|chloric(I) acid]] itself.
Besides oxidizing almost any [[reducing agent]], chlorate(I) is unstable with respect to [[disproportionation]] (that is, it will oxidize itself); chlorate(I) will often degrade to some mixture of [[chloride]] and chlorate, especially if not kept cool.
[[Category:Hypochlorites]]
[[Category:Oxoanions]]
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[[fr:Hypochlorite]]
[[it:Ipoclorito]]
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[[ru:Гипохлориты]]
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[[zh:次氯酸盐]]