Chlorine perchlorate
Chemical compound
From Wikipedia, the free encyclopedia
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 Cl−O−ClO3. It is produced by the photodimerization of chlorine dioxide (ClO2) at room temperature by 436 nm ultraviolet light:[3][4][5]
- 2 ClO2 → ClOClO3
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| Names | |||
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| IUPAC name
Chloro perchlorate[1] | |||
| Systematic IUPAC name
Chloro perchlorate[1] | |||
Other names
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| Identifiers | |||
3D model (JSmol) |
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| ChEBI | |||
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PubChem CID |
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CompTox Dashboard (EPA) |
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| Properties | |||
| Cl2O4 | |||
| Molar mass | 134.90 g·mol−1 | ||
| Appearance | Pale green liquid | ||
| Density | 1.81 g·cm−3 | ||
| Melting point | −117 °C (−179 °F; 156 K) | ||
| Boiling point | 20 °C (68 °F; 293 K) (decomposes) | ||
| Reacts | |||
| Hazards | |||
| Occupational safety and health (OHS/OSH): | |||
Main hazards |
oxidizer | ||
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Chlorine perchlorate can also be made by the following reaction at −45 °C.
- CsClO4 + ClOSO2F → CsSO3F + ClOClO3
Properties
Chlorine perchlorate is a pale greenish liquid. It is less stable than ClO2 (chlorine dioxide)[citation needed] and decomposes at room temperature to give O2 (oxygen), Cl2 (chlorine) and Cl2O6 (dichlorine hexoxide):
- 2 ClOClO3 → O2 + Cl2 + Cl2O6
Chlorine perchlorate reacts with metal chlorides to form chlorine and the corresponding anhydrous perchlorate:
- CrO2Cl2 + 2 ClOClO3 → 2 Cl2 + CrO2(ClO4)2
Reactions
| Reactant | Conditions | Products |
|---|---|---|
| — | Heat | dichlorine hexoxide (80%), chlorine dioxide, chlorine, oxygen |
| — | Ultraviolet light | dichlorine heptoxide, chlorine, oxygen[5] |
| caesium iodide | −45 °C | caesium tetraperchloratoiodate(III) Cs+[I(OClO3)4]−[note 1] |
| ClOSO2F or ClF | — | M+ClO−4 (M = Cs or [NO2])[note 2] |
| bromine | −45 °C | bromine perchlorate (BrOClO3)[note 2] |
| iodine(0.33 mol) | −50 °C | iodine(III) perchlorate I(OClO3)3[note 3] |
| CF3I | -112 °C | CF3OClO3, O2, Cl2, Cl2O7, and I2O5.[8] |
Notes
- M+ClO−4 (M = Cs or [NO2]) reacts with BrOSO2F at −20 °C and produces bromine perchlorate (BrOClO3). Bromine perchlorate then reacts with hydrogen bromide (HBr) at −70 °C and produces elemental bromine (Br2) and perchloric acid (HClO4).