Chlorine perchlorate

Chlorine perchlorate  |

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Names
IUPAC name

Chloro perchlorate[1]

Systematic IUPAC name

Chloro perchlorate[1]

Other names

Chlorine (I,VII) oxide
Dichlorine tetroxide

Identifiers

CAS Number

* 27218-16-2 Y

3D model (JSmol)

* Interactive image

ChemSpider |

* 147540 N

PubChem CID

* 168667

InChI

* InChI=1S/Cl2O4/c1-6-2(3,4)5 N

Key: JRONPIZRZBBOBR-UHFFFAOYSA-N N

SMILES

* ClO[Cl](=O)(=O)=O

Properties

Chemical formula

| Cl2O4
Molar mass | 134.90 g·mol−1
Appearance  | Pale green liquid
Density | 1.81 g·cm−3
Melting point |  −117 °C (−179 °F; 156 K)
Boiling point |  20 °C (68 °F; 293 K) (decomposes)

Solubility in water

| Reacts
Hazards
Main hazards | oxidizer

Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).

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Infobox references

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Chlorine perchlorate is a chemical compound with the formula Cl2O4. This chlorine oxide is an asymmetric oxide, with one chlorine atom in +1 oxidation state and the other +7, with proper formula ClOClO3. It is produced by the photodimerization of chlorine dioxide (ClO2) at room temperature by 436 nm ultraviolet light:[2][3][4]

2 ClO2 → ClOClO3

Chlorine perchlorate can also be made by the following reaction at −45 °C.

CsClO4 \+ ClOSO2F → Cs(SO3)F + ClOClO3

## Contents

* 1 Properties
* 2 Reactions
* 3 Notes
* 4 References

## Properties

Chlorine perchlorate is a pale greenish liquid. It is less stable than ClO2 (chlorine dioxide)[citation needed] and decomposes at room temperature to give O2 (oxygen), Cl2 (chlorine) and Cl2O6 (dichlorine hexoxide):

2 ClOClO3 → O2 \+ Cl2 \+ Cl2O6

Chlorine perchlorate reacts with metal chlorides to form chlorine and the corresponding anhydrous perchlorate:

CrO2Cl2 \+ 2 ClOClO3 → 2 Cl2 \+ CrO2(ClO4)2

TiCl4 \+ 4 ClOClO3 → 4 Cl2 \+ Ti(ClO4)4

2 AgCl + 2 ClOClO3 → 2 AgClO4 \+ Cl2

## Reactions

Reactant | Conditions | Products

|
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— | Heat | dichlorine hexoxide (80%), chlorine dioxide, chlorine, oxygen
— | Ultraviolet light | dichlorine heptoxide, chlorine, oxygen[4]
caesium iodide | −45 °C | Cs[I(OClO3)4][note 1]
ClOSO2F or ClF | — | MClO4(M = Cs or NO2)[note 2]
bromine | −45 °C | bromine perchlorate (BrOClO3)[note 2]
iodine(0.33 mol) | −50 °C | I(OClO3)3[note 3][5]

## Notes

1. ↑ Cs[I(OClO3)4] is a pale yellow salt which is stable at room temperature. It has a square IO4 unit.
2. ↑ 2.0 2.1 MClO4 (M = Cs or NO2) reacts with BrOSO2F at −20 °C and produces bromine perchlorate (BrOClO3). Bromine perchlorate then reacts with hydrogen bromide (HBr) at −70 °C and produces elemental bromine (Br2) and perchloric acid (HClO4).
3. ↑ So far, all attempts to form iodine perchlorate (IOClO3) have failed, because the iodine atom oxidizes to +3 oxidation state immediately.[citation needed]

## References

1. ↑ 1.0 1.1 "Chloro Perchlorate - PubChem Public Chemical Database". The PubChem Project. USA: National Center for Biotechnology Information. https://pubchem.ncbi.nlm.nih.gov/summary/summary.cgi?cid=168667.
2. ↑ A. J. Schell-Sorokin; D. S. Bethune; J. R. Lankard; M. M. T. Loy; P. P. Sorokin (1982). "Chlorine perchlorate a major photolysis product of chlorine dioxide". J. Phys. Chem. 86 (24): 4653–4655. doi:10.1021/j100221a001.
3. ↑ M. I. Lopez; J. E. Sicre (1988). "Ultraviolet spectrum of chlorine perchlorate". J. Phys. Chem. 92 (2): 563–564. doi:10.1021/j100313a062.
4. ↑ 4.0 4.1 Rao, Balaji; Anderson, Todd A.; Redder, Aaron; Jackson, W. Andrew (2010-04-15). "Perchlorate Formation by Ozone Oxidation of Aqueous Chlorine/Oxy-Chlorine Species: Role of ClxOy Radicals". Environmental Science & Technology 44 (8): 2961–2967. doi:10.1021/es903065f. ISSN 0013-936X. PMID 20345093. Bibcode: 2010EnST...44.2961R.
5. ↑ Gomberg, M. (1923-02-01). "The Reaction Between Silver Perchlorate and Iodine. Chlorine Tetra-Oxide". Journal of the American Chemical Society 45 (2): 398–421. doi:10.1021/ja01655a017. ISSN 0002-7863.

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Chlorine compounds

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

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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

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