Chlorine monoxide

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

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
CompTox Dashboard (EPA)	DTXSID90924342
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
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. 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.