Everything about Chlorates totally explained
The
chlorate anion has the formula ClO
3−. In this case, the
chlorine atom is in the +5
oxidation state. "Chlorate" can also refer to
chemical compounds containing this anion; chlorates are the
salts of
chloric acid. As predicted by
VSEPR, chlorate anions have
trigonal pyrimidal structures.
Chlorates are powerful
oxidizers and should be kept away from organics or easily oxidized 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.
Examples of chlorates include:
Preparation
Metal chlorates can be prepared by adding
chlorine to hot metal
hydroxides, for example,
KClO3:
» 3Cl
2 + 6KOH → 5KCl + KClO
3 + 3H
2O
The industrial scale synthesis for
sodium chlorate starts from
sodium chloride. {If the electrolysis isn't done with the method described at
chlorine, but a mixing of the
chlorine evolved 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.
Stock notation
If a Roman numeral in brackets follow the word "chlorate", this refers to the
oxyanion containing chlorine in the respective oxidation state, namely:
| Common name |
Stock name |
Oxidation state |
Formula |
| Hypochlorite |
Chlorate(I) |
+1 |
ClO− |
| Chlorite |
Chlorate(III) |
+3 |
ClO2− |
| Chlorate |
Chlorate(V) |
+5 |
ClO3− |
| Perchlorate |
Chlorate(VII) |
+7 |
ClO4− |
Using this convention, "chlorate" means
any chlorine oxyanion. However, Stock notation for chlorine is quite uncommon, and "chlorate" typically refers only to the +5 oxidation state.
Further Information
Get more info on 'Chlorates'.
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