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(Top) 1 Properties 2 Reactions 3 Notes 4 References

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

CompTox Dashboard (EPA)

DTXSID00181686

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

Occupational safety and health (OHS/OSH):

Main hazards

oxidizer

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

N verify (what is ^YN ?)

Infobox references

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 photodimerizationofchlorine dioxide (ClO₂) at room temperature by 436 nmultraviolet light:^[2]^[3]^[4]

2ClO₂ → ClOClO₃

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

CsClO₄ + ClOSO₂F → Cs(SO₃)F + ClOClO₃

Properties[edit]

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):

2ClOClO₃ → O₂ + Cl₂ + Cl₂O₆

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

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

TiCl₄ + 4ClOClO₃ → 4Cl₂ + Ti(ClO₄)₄

2AgCl + 2 ClOClO₃ → 2AgClO₄ + Cl₂

Reactions[edit]

Reactant	Conditions	Products
—	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 = CsorNO₂)^{[note 2]}
bromine	−45 °C	bromine perchlorate (BrOClO₃)^{[note 2]}
iodine(0.33 mol)	−50 °C	I(OClO₃)₃^{[note 3]}

Notes[edit]

^ Cs[I(OClO₃)₄] is a pale yellow salt which is stable at room temperature. It has a square IO₄ unit.

^ ^a ^b 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).

^ The last^[5] attempt to form iodine monoperchlorate (IOClO₃) occurred in 1972,^[6] and even at low temperatures yielded instead the triperchlorate. On warming, the latter then decomposes to iodate.

References[edit]

^ ^a ^b "Chloro Perchlorate - PubChem Public Chemical Database". The PubChem Project. USA: National Center for Biotechnology Information.

^ 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.

^ M. I. Lopez; J. E. Sicre (1988). "Ultraviolet spectrum of chlorine perchlorate". J. Phys. Chem. 92 (2): 563–564. doi:10.1021/j100313a062.

^ ^a ^b 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. Bibcode:2010EnST...44.2961R. doi:10.1021/es903065f. ISSN 0013-936X. PMID 20345093.

^ Zefirov, N. S.; Zedankin, V. V.; Koz'min, A. S. (1988). "The synthesis and properties of covalent organic perchlorates". Russian Chemical Reviews. 57 (11). Turpion: 1047. doi:10.1070/RC1988v057n11ABEH003410. Translated from Uspekhi Khimii volume 57 (1988), pp. 1815-1839.

^ Christe, Karl O.; Schack, Carl J. (1972) [20 September 1971]. "Iodine tris(perch1orate) and cesium tetrakis(perchlorato)iodate(III)". Inorganic Chemistry. 11 (7): 1684. doi:10.1021/ic50113a047.