| IUPAC name
| Other names
Chlorine trioxide; Chloryl perchlorate; Chlorine(V,VII) oxide
|Molar mass||166.901 g/mol|
|Melting point||3.5 °C (38.3 °F; 276.6 K)|
|Boiling point||200 °C (392 °F; 473 K)|
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
|(what is ?)|
Dichlorine hexoxide is the chemical compound with the molecular formula Cl
6, which is correct for its gaseous state. However, in liquid or solid form, this chlorine oxide ionizes into the dark red ionic compound chloryl perchlorate [ClO
, which may be thought of as the mixed anhydride of chloric and perchloric acids.
- 2 ClO
2 + 2 O
3 → 2 ClO
3 + 2 O
2 → Cl
6 + 2 O
It was originally reported to exist as the monomeric chlorine trioxide ClO3 in gas phase, but was later shown to remain an oxygen-bridged dimer after evaporation and until thermal decomposition into chlorine perchlorate, Cl2O4, and oxygen. The compound ClO3 was then rediscovered.
It is a dark red fuming liquid at room temperature that crystallizes as a red ionic compound, chloryl perchlorate, [ClO
. The red color shows the presence of chloryl ions. Thus, chlorine's formal oxidation state in this compound remains a mixture of chlorine (V) and chlorine (VII) both in the gas phase and when condensed; however by breaking one oxygen-chlorine bond some electron density does shifts towards the chlorine (VII).
Cl2O6 is diamagnetic and is a very strong oxidizing agent. Although stable at room temperature, it explodes violently on contact with organic compounds and reacts with gold to produce the chloryl salt [ClO
. Many other reactions involving Cl2O6 reflect its ionic structure, [ClO
, including the following:
- NO2F + Cl2O6 → NO2ClO4 + ClO2F
- NO + Cl2O6 → NOClO4 + ClO2
- 2 V2O5 + 12 Cl2O6 → 4 VO(ClO4)3 + 12 ClO2 + 3 O2
- SnCl4 + 6 Cl2O6 → [ClO2]2[Sn(ClO4)6] + 4 ClO2 + 2 Cl2
- 2Au + 6Cl2O6 → 2[ClO
Nevertheless, it can also react as a source of the ClO3 radical:
- 2 AsF5 + Cl2O6 → 2 ClO3AsF5
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