Gourt Home::Gourt :: 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- |
Examples
ClO3 has a trigonal planar structure, with 120 degree bond angle.
- potassium chlorate, KClO3
- sodium chlorate, NaClO3
- magnesium chlorate, Mg(ClO3)2
See Chlorates 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.
"Chlorate"