Chlorite

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Chlorite

The chlorite ion is the chlorine dioxide anion, with the chemical formula ClO2−. In chlorites, chlorine has an oxidation state of +3. Chlorites are salts that contain this group; the related acid is chlorous acid (HClO2), which is not stable enough to be sold as a chemical product.

The most important chlorite compound is sodium chlorite (NaClO2). It is widely used to bleach textiles, pulp, and paper. Chlorites are strong oxidizers and are often used to generate chlorine dioxide (ClO2) by reacting with hydrochloric acid (HCl).

Some chlorite salts, especially those with heavy metals like silver, mercury, thallium, and lead (as well as copper and ammonium), can be unstable and may explode when heated or shocked.

Structure and properties: The chlorite ion is bent, due to lone pairs on chlorine. The Cl–O bonds are about 156 picometers long, and the O–Cl–O angle is around 111°.

Safety and regulation: In drinking water, California recommended keeping chlorite levels below 50 parts per billion. In the United States, the federal limit allows up to 1,000 ppb. Some studies have suggested chlorite could be carcinogenic at certain levels.

Other chlorine oxyanions exist, with chlorine in different oxidation states: Cl− (chloride), ClO− (hypochlorite), ClO2− (chlorite), ClO3− (chlorate), and ClO4− (perchlorate). These form a family of chlorine oxides.