Chlorine perchlorate is a chemical compound with the formula Cl2O4. This chlorine oxide is an asymmetric oxide, with one chlorine atom in +1 oxidation state and the other +7, with proper formula ClOClO3. It is produced by the photodimerization of chlorine dioxide (ClO2) at room temperature by 436 nm ultraviolet light:[1] [2] [3]
2ClO2 → ClOClO3
Chlorine perchlorate can also be made by the following reaction at −45 °C.
CsClO4 + ClOSO2F → Cs(SO3)F + ClOClO3
Chlorine perchlorate is a pale greenish liquid. It is less stable than ClO2 (chlorine dioxide) and decomposes at room temperature to give O2 (oxygen), Cl2 (chlorine) and Cl2O6 (dichlorine hexoxide):
2ClOClO3 → O2 + Cl2 + Cl2O6
Chlorine perchlorate reacts with metal chlorides to form chlorine and the corresponding anhydrous perchlorate:
CrO2Cl2 + 2ClOClO3 → 2Cl2 + CrO2(ClO4)2
TiCl4 + 4ClOClO3 → 4Cl2 + Ti(ClO4)4
2AgCl + 2 ClOClO3 → 2AgClO4 + Cl2
| Reactant | Conditions | Products | |
|---|---|---|---|
| — | Heat | dichlorine hexoxide (80%), chlorine dioxide, chlorine, oxygen | |
| — | dichlorine heptoxide, chlorine, oxygen | ||
| −45 °C | Cs[I(OClO<sub>3</sub>)<sub>4</sub>] | ||
| — | MClO4(M = Cs or NO2) | ||
| −45 °C | bromine perchlorate (BrOClO3) | ||
| iodine(0.33 mol) | −50 °C | I(OClO3)3 |