Chlorine monoxide

This page is about the compound ClO. For the oxoanion with the formula ClO−, see hypochlorite. For the molecule Cl2O, see Dichlorine monoxide.

This article relies largely or entirely on a single source. Please help improve this article by introducing citations to additional sources.
Find sources: "Chlorine monoxide" – news · newspapers · books · scholar · JSTOR (February 2024)

|

Chlorine monoxide  |  |

|

Names
Preferred IUPAC name

Chlorine monoxide

Systematic IUPAC name

Chlorooxidanyl

Other names

Chlorine(II) oxide

Identifiers

CAS Number

* 7791-21-1 Y

3D model (JSmol)

* Interactive image

Abbreviations  | ClO•
ChEBI |

* CHEBI:29314

ChemSpider |

* 145843

MeSH | Chlorosyl

PubChem CID

* 166686

UNII |

* 0EQ5I4TK19 Y

InChI

* InChI=1S/ClO/c1-2

Key: NHYCGSASNAIGLD-UHFFFAOYSA-N

SMILES

* [O]Cl

Properties

Chemical formula

| 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).

Infobox references

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

There has been a significant impact of the use of CFCs on the upper stratosphere, although many countries have agreed to ban the use of CFCs. The nonreactive nature of CFCs 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 monoxide, 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.

Even though the use of CFCs has been banned in many countries, CFCs can stay in the atmosphere for 50 to 500 years. This causes many chlorine radicals to be produced and hence a significant amount of ozone molecules are decomposed before the chlorine radicals are able to react with chlorine monoxide to form dichlorine monoxide.

## References

1. ↑ 1.0 1.1 Egon Wiberg; Nils Wiberg; Arnold Frederick Holleman (2001). Inorganic chemistry. Academic Press. p. 462. ISBN 0-12-352651-5.

* v
* t
* e

Chlorine compounds

* ClF
* ClF3
* ClF5
* ClNO3
* ClO
* ClOF3
* Cl2O2
* ClO2
* ClO2F
* ClO3F
* Cl2O
* Cl2O4
* Cl2O6
* Cl2O7
* HCl
* SiCl4

* v
* t
* e

Oxygen compounds

* AgO
* Al2O3
* AmO2
* Am2O3
* As2O3
* As2O5
* Au2O3
* B2O3
* BaO
* BeO
* Bi2O3
* BiO2
* Bi2O5
* BrO2
* Br2O3
* Br2O5
* CO
* CO2
* C2O3
* CaO
* CaO2
* CdO
* CeO2
* Ce3O4
* Ce2O3
* ClO2
* Cl2O
* Cl2O3
* Cl2O4
* Cl2O6
* Cl2O7
* CoO
* Co2O3
* Co3O4
* CrO3
* Cr2O3
* Cr2O5
* Cr5O12
* CsO2
* Cs2O3
* CuO
* D2O
* Dy2O3
* Er2O3
* Eu2O3
* FeO
* Fe2O3
* Fe3O4
* Ga2O
* Ga2O3
* GeO
* GeO2
* H2O
* H218O
* H2O2
* HfO2
* HgO
* Hg2O
* Ho2O3
* I2O4
* I2O5
* I2O6
* I4O9
* In2O3
* IrO2
* KO2
* K2O2
* La2O3
* Li2O
* Li2O2
* Lu2O3
* MgO
* Mg2O3
* MnO
* MnO2
* Mn2O3
* Mn2O7
* MoO2
* MoO3
* Mo2O3
* NO
* NO2
* N2O
* N2O3
* N2O4
* N2O5
* NaO2
* Na2O
* Na2O2
* NbO
* NbO2
* Nd2O3
* OF2
* O2F2
* O3F2
* O4F2
* O2PtF6

Chemical formulas

0.00

(0 votes)

Original source: https://en.wikipedia.org/wiki/Chlorine monoxide. Read more

|

Retrieved from "https://handwiki.org/wiki/index.php?title=Chemistry:Chlorine_monoxide&oldid=4035828"
*[CID]: Compound ID
*[v]: View this template
*[t]: Discuss this template
*[e]: Edit this template