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| Names | |||
|---|---|---|---|
| IUPAC name Chloro perchlorate[2] | |||
| Systematic IUPAC name Chloro perchlorate[2] | |||
Other names
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| Identifiers | |||
3D model (JSmol) | |||
| ChEBI | |||
| ChemSpider |
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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 theirstandard state (at 25 °C [77 °F], 100 kPa). | |||
Chlorine perchlorate is achemical compound with the formulaCl2O4. Thischlorine oxide is an asymmetric oxide, with one chlorine atom in +1oxidation state and the other +7, with proper formulaCl−O−ClO3. It is produced by thephotodimerization ofchlorine dioxide (ClO2) at room temperature by 436 nmultraviolet light:[3][4][5]
Chlorine perchlorate can also be made by the following reaction at −45 °C.
Chlorine perchlorate is a pale greenish liquid. It is less stable thanClO2 (chlorine dioxide)[citation needed] and decomposes at room temperature to giveO2 (oxygen),Cl2 (chlorine) andCl2O6 (dichlorine hexoxide):
Chlorine perchlorate reacts with metal chlorides to form chlorine and the corresponding anhydrous perchlorate:
| 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 orClF | — | 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) perchlorateI(OClO3)3[note 3] |
| CF3I | -112 °C | CF3OClO3,O2, Cl2,Cl2O7, andI2O5.[8] |
