| |||
| Names | |||
|---|---|---|---|
| Preferred IUPAC name
Chlorine monoxide | |||
| Systematic IUPAC name
Chlorooxidanyl | |||
| Other names
Chlorine(II) oxide | |||
| Identifiers | |||
3D model (JSmol) |
|||
| Abbreviations | ClO• | ||
| ChEBI | |||
| ChemSpider | |||
| MeSH | Chlorosyl | ||
PubChem CID |
|||
| UNII | |||
CompTox Dashboard (EPA) |
|||
| |||
| |||
| Properties | |||
| ClO | |||
| Molar mass | 51.45 g·mol−1 | ||
| Thermochemistry | |||
Std enthalpy of formation (ΔfH⦵298) |
101.8 kJ⋅mol−1[1] | ||
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
| |||
Chlorine monoxide is a chemical radical with the chemical formula ClO•. It plays an important role in the process of ozone depletion. In the stratosphere, chlorine atoms react with ozone molecules to form chlorine monoxide and oxygen.
- Cl• + O3 → ClO• + O2
This reaction causes the depletion of the ozone layer.[1] The resulting ClO• radicals can further react:
- ClO• + O• → Cl• + O2
regenerating the chlorine radical. In this way, the overall reaction for the decomposition of ozone is catalyzed by chlorine, as ultimately chlorine remains unchanged. The overall reaction is:
- O• + O3 → 2 O2
Chlorofluorocarbons (CFCs) are able to pass into the stratosphere due to their non-reactive nature, where they undergo photo-dissociation to form Cl radicals. These then readily form chlorine monoxide, and this cycle can continue until two radicals react to form dichlorine monoxide, terminating the radical reaction.
References
- Holleman, Arnold Frederik; Wiberg, Egon (2001), Wiberg, Nils (ed.), Inorganic Chemistry, translated by Eagleson, Mary; Brewer, William, San Diego/Berlin: Academic Press/De Gruyter, p. 462, ISBN 0-12-352651-5