Chlorine monoxide: Difference between revisions
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| PIN = Chlorine monoxide |
| PIN = Chlorine monoxide |
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| SystematicName = Chlorooxidanyl |
| SystematicName = Chlorooxidanyl |
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| OtherNames = Chlorine(II) oxide |
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| Section1 = {{Chembox Identifiers |
| Section1 = {{Chembox Identifiers |
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| Abbreviations = ClO(.) |
| Abbreviations = ClO(.) |
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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: |
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: |
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:O + {{chem|O|3}} → + 2{{chem|O|2}} |
:O· + {{chem|O|3}} → + 2{{chem|O|2}} |
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This has been a significant impact of the use of [[CFC]]'s in 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. |
This has been a significant impact of the use of [[CFC]]'s in 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. |
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Revision as of 02:53, 27 May 2012
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| Names | |||
|---|---|---|---|
| Preferred IUPAC name
Chlorine monoxide | |||
| Systematic IUPAC name
Chlorooxidanyl | |||
| Other names
Chlorine(II) oxide
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| 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 CFC's in 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.
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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