Editing Chlorite (section)

==Compounds==
{{See also|Category:Chlorites}}
The free acid, [[chlorous acid]] HClO<sub>2</sub>, is the least stable [[oxoacid]] of chlorine and has only been observed as an [[aqueous solution]] at low concentrations. Since it cannot be concentrated, it is not a commercial product. The [[alkali metal]] and [[alkaline earth metal]] compounds are all colorless or pale yellow, with [[sodium chlorite]] (NaClO<sub>2</sub>) being the only commercially important chlorite. Heavy metal chlorites (Ag<sup>+</sup>, Hg<sup>+</sup>, Tl<sup>+</sup>, Pb<sup>2+</sup>, and also Cu<sup>2+</sup> and {{chem|NH|4|+}}) are unstable and decompose explosively with heat or shock.<ref name=Greenwood>{{cite book|last1=Greenwood|first1=N.N.|last2=Earnshaw|first2=A.|title=Chemistry of the elements|date=2006|publisher=Butterworth-Heinemann|location=Oxford|isbn=0750633654|page=861|edition=2nd}}</ref>

Sodium chlorite is derived indirectly from [[sodium chlorate]], NaClO<sub>3</sub>. First, the explosively unstable gas [[chlorine dioxide]], ClO<sub>2</sub> is produced by reducing sodium chlorate with a suitable reducing agent such as methanol, hydrogen peroxide, hydrochloric acid or sulfur dioxide.