Chlorine monoxide: Difference between revisions
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This has been a significant impact of the use of [[Chlorofluorocarbon|CFC]]s 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 [[Radical (chemistry)|radicals]] react to terminate the radical reaction. |
This has been a significant impact of the use of [[Chlorofluorocarbon|CFC]]s 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 [[Radical (chemistry)|radicals]] react to terminate 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. |
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== References == |
== References == |
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Revision as of 21:57, 24 July 2012
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| Names | |||
|---|---|---|---|
| Preferred IUPAC name
Chlorine monoxide | |||
| Systematic IUPAC name
Chlorooxidanyl | |||
| Other names
Chlorine(II) oxide
| |||
| Identifiers | |||
3D model (JSmol)
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| Abbreviations | ClO(.) | ||
| ChEBI | |||
| ChemSpider | |||
| MeSH | Chlorosyl | ||
PubChem CID
|
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CompTox Dashboard (EPA)
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| 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).
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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 terminate 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.
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