Hypochlorite 862860 220928039 2008-06-22T07:12:14Z Footballplar951 6151544 /* 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]] {{chem-stub}} [[de:Hypochlorit]] [[fr:Hypochlorite]] [[it:Ipoclorito]] [[pt:Hipoclorito]] [[ru:Гипохлориты]] [[uk:Гіпохлорити]] [[zh:次氯酸盐]]