Chlorine monoxide: Difference between revisions

Chlorine monoxide
Names
	Preferred IUPAC name Chlorine monoxide
	Systematic IUPAC name Chlorooxidanyl
	Other names Chlorine(II) oxide
Identifiers
CAS Number	7791-21-1 ;
3D model (JSmol)	Interactive image;
Abbreviations	ClO•
ChEBI	CHEBI:29314;
ChemSpider	145843;
MeSH	Chlorosyl
PubChem CID	166686;
UNII	0EQ5I4TK19 ;
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

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Latest revision as of 09:17, 13 September 2024

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

^ ^a ^b Egon Wiberg; Nils Wiberg; Arnold Frederick Holleman (2001). Inorganic chemistry. Academic Press. p. 462. ISBN 0-12-352651-5.

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

[1]

@@ Line 1: / Line 1: @@
-{{about|the compound ClO|the oxoanion with the formula {{chem|ClO|-}}|hypochlorite|the molecule Cl<sub>2</sub>O|Dichlorine monoxide}}
+{{about|the compound ClO|the oxoanion with the formula ClO<sup>−</sup>|hypochlorite|the molecule Cl<sub>2</sub>O|Dichlorine monoxide}}
+{{single source|date=February 2024}}
 {{Chembox
 | Watchedfields = changed
 | ImageFileL1 = Chlorosyl.svg
-| ImageFileR1 = Chlorine-monoxide-3D-vdW.png
+| ImageFileR1 = Chlorine-monoxide-3D-SF.png
 | PIN = Chlorine monoxide
 | SystematicName = Chlorooxidanyl
 | OtherNames = Chlorine(II) oxide
 |Section1={{Chembox Identifiers
-| Abbreviations = ClO(.)
+| Abbreviations = ClO<sup>•</sup>
+| CASNo_Ref = {{cascite|correct|CAS}}
-| CASNo = 12301-79-0
+| CASNo = 7791-21-1
+| UNII_Ref = {{fdacite|correct|FDA}}
+| UNII = 0EQ5I4TK19
 | PubChem = 166686
 | ChemSpiderID = 145843
-| ChemSpiderID_Ref = {{Chemspidercite}}
 | ChEBI = 29314
 | MeSHName = Chlorosyl
@@ Line 20: / Line 23: @@
 |Section2={{Chembox Properties
 | Cl=1 | O=1
 | Appearance =
 | Density =
 | MeltingPt =
 | BoilingPt =
 | Solubility = }}
 |Section3={{Chembox Hazards
 | MainHazards =
 | FlashPt =
 | AutoignitionPt = }}
 |Section4={{Chembox Thermochemistry
 | DeltaHf = 101.8 kJ/mol<ref name="holleman_wiberg"/>
 | DeltaHc =
 | Entropy =
 | HeatCapacity =
   }}
 }}
-'''Chlorine monoxide''' is a chemical [[Radical (chemistry)|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]].
+'''Chlorine monoxide''' is a chemical [[Radical (chemistry)|radical]] with the chemical formula ClO<sup>•</sup>. 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· + {{chem|O|3}} → ClO· + {{chem|O|2}}
+:Cl<sup>•</sup> + O<sub>3</sub> → ClO<sup>•</sup> + O<sub>2</sub>
-This reaction causes the depletion of the ozone layer.<ref name="holleman_wiberg">{{cite book | title = Inorganic chemistry | author1 = Egon Wiberg | author2 = Nils Wiberg | author3 = Arnold Frederick Holleman | publisher = Academic Press | year = 2001 | isbn = 0-12-352651-5 | page = 462}}</ref> This reaction can go on and the ClO· radicals can go on to react as such:
+This reaction causes the depletion of the [[ozone layer]].<ref name="holleman_wiberg">{{cite book | title = Inorganic chemistry | author1 = Egon Wiberg | author2 = Nils Wiberg | author3 = Arnold Frederick Holleman | publisher = Academic Press | year = 2001 | isbn = 0-12-352651-5 | page = 462}}</ref> The resulting ClO<sup>•</sup> radicals can further react:
-:ClO· + O· → Cl· + {{chem|O|2}}
+: ClO<sup>•</sup> + O<sup>•</sup> → Cl<sup>•</sup> + O<sub>2</sub>
 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<sup>•</sup> + O<sub>3</sub> → 2 O<sub>2</sub><!-- The reaction was :O· + O
-:O· + {{chem|O|3}} → + 2{{chem|O|2}}
+→ + 2O
+. Why the "+" on the products side ? was something missing? -->
-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 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.
+There has been a significant impact of the use of [[Chlorofluorocarbon|CFC]]s 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 [[Radical (chemistry)|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 ==
 {{reflist}}
 {{Chlorine compounds}}
+{{oxygen compounds}}
 {{DEFAULTSORT:Chlorine Monoxide}}
 [[Category:Chlorine oxides]]
 [[Category:Free radicals]]
+[[Category:Diatomic molecules]]
-{{Inorganic-compound-stub}}

v t e Chlorine compounds
Chlorides and acids	HCl HClO HClO₂ HClO₃ HClO₄ HSO₃Cl BaClF BCl₃ CCl₄ SiCl₄ TiCl₄ C₃H₅Cl
Chlorine fluorides	ClF ClF₃ ClF₅
Chlorine oxides	ClO ClO₂ Cl₂O Cl₂O₂ Cl₂O₃ Cl₂O₄ Cl₂O₅ Cl₂O₆ Cl₂O₇ ClO₄
Chlorine oxyfluorides	ClOF ClOF₃ ClO₂F ClOF₅ (predicted) ClO₂F₃ ClO₃F
Chlorine(I) derivatives	ClNO₃ ClSO₃F ClN₃ Cl₃N