Chlorate

The chlorate ion ClO₃⁻.

A chlorate (compound) is a compound that contains this group, with chlorine in oxidation state +5.

If a Roman numeral in brackets follow the word chlorate, this refers to the oxo-anion containing chlorine in the respective oxidation state, namely:
Name Oxidation state Formula
Chlorate(I) +1 ClO^-
Chlorate(III) +3 ClO₂^-
Chlorate>Chlorate(V) +5 ClO₃^-
Chlorate(VII) +7 ClO₄^-

Name	Oxidation state	Formula
Chlorate(I)	+1	ClO^-
Chlorate(III)	+3	ClO₂^-
Chlorate>Chlorate(V)	+5	ClO₃^-
Chlorate(VII)	+7	ClO₄^-

Examples

ClO₃ has a trigonal planar structure, with 120 degree bond angle.

potassium chlorate, KClO₃

sodium chlorate, NaClO₃

magnesium chlorate, Mg(ClO₃)₂

See for a bigger list.

Preparation

Metal chlorates can be prepared by adding Chlorine to hot metal hydroxides, for example, KClO₃:

3Cl₂ + 6KOH → 5KCl + KClO₃ + 3H₂O

Industrial scale synthesis for sodium chlorate starts from sodium chloride. If the electrolysis is not done with the method described at chlorine, but a mixing of the devoloping chlorine and the sodium hydroxide is allowed, the reaction mentioned above takes place. The heating to 50-70°C is done by the electrical power applied for electrolysis.

Discussion

Chlorates are the salts of chloric acid.

Chlorates are powerful oxidizers and should be kept away from organics or easily reducible materials. Chlorates were once widely used in pyrotechnics, though their use has fallen due to their instability. Most pyrotechnic applications which used chlorates in the past now use perchlorates instead.

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