Chlorine monoxide: Difference between revisions
Remove setting ImageSize, use default (100px L, R; 200px single), removed: | ImageSizeL1 = 100px (2) using AWB |
removed Category:Oxides using HotCat |
||
| Line 59: | Line 59: | ||
{{DEFAULTSORT:Chlorine Monoxide}} |
{{DEFAULTSORT:Chlorine Monoxide}} |
||
[[Category: |
[[Category:Chlorine oxides]] |
||
[[Category:Oxides]] |
|||
[[Category:Free radicals]] |
[[Category:Free radicals]] |
||
{{Inorganic-compound-stub}} |
{{Inorganic-compound-stub}} |
||
Revision as of 10:40, 12 August 2014
| |||
| 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
|
|||
CompTox Dashboard (EPA)
|
|||
| |||
| |||
| Properties | |||
| ClO | |||
| Molar mass | 51.45 g·mol−1 | ||
| Thermochemistry | |||
Std enthalpy of
formation (ΔfH⦵298) |
101.8 kJ/mol[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 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· + O
3 → ClO· + O
2
This reaction causes the depletion of the ozone layer.[1] This reaction can go on and the ClO· radicals can go on to react as such:
- ClO· + O· → Cl· + O
2
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· + O
3 → + 2O
2
This has been a significant impact of the use of CFCs on the upper stratosphere. The nonreactive nature of CFC's allows them to pass into the stratosphere, 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 dioxide, terminating the radical reaction. Because the concentration of CFCs in atmosphere is very low, the probability of a terminating reaction is exceedingly low, meaning each radical can decompose many thousands of molecules of ozone.
References
- ^ a b Egon Wiberg; Nils Wiberg; Arnold Frederick Holleman (2001). Inorganic chemistry. Academic Press. p. 462. ISBN 0-12-352651-5.
 | This inorganic compound–related article is a stub. You can help Wikipedia by expanding it. |