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Chlorine dioxide is a chemical compound with the formula ClO 2 that exists as yellowish-green gas above 11 °C, a reddish-brown liquid between 11 °C and −59 °C, and as bright orange crystals below −59 °C. It is usually handled as an aqueous solution.
The chlorite ion adopts a bent molecular geometry, due to the effects of the lone pairs on the chlorine atom, with an O–Cl–O bond angle of 111° and Cl–O bond lengths of 156 pm. [1] Chlorite is the strongest oxidiser of the chlorine oxyanions on the basis of standard half cell potentials.
Neutral/basic reaction E° (V) ... (The element can also assume oxidation state of +4 is seen in the neutral compound chlorine dioxide ClO 2). Chlorine oxidation state
Chlorine dioxide, ClO 2. [23] This is an unstable gas, which is usually prepared in situ or stored as dilute aqueous solutions. Despite these limitations it finds large-scale applications for the bleaching of wood pulp, fats and oils, cellulose, flour, textiles, beeswax, skin, and in a number of other industries. It has also been used for ...
Chlorous acid is an inorganic compound with the formula HClO 2.It is a weak acid.Chlorine has oxidation state +3 in this acid. The pure substance is unstable, disproportionating to hypochlorous acid (Cl oxidation state +1) and chloric acid (Cl oxidation state +5):
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Chloride can be oxidized but not reduced. The first oxidation, as employed in the chlor-alkali process, is conversion to chlorine gas. Chlorine can be further oxidized to other oxides and oxyanions including hypochlorite (ClO −, the active ingredient in chlorine bleach), chlorine dioxide (ClO 2), chlorate (ClO − 3), and perchlorate (ClO − 4).
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