Chlorine perchlorate

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Chlorine perchlorate
Dichlorine tetraoxide.svg
Chlorine perchlorate molecule spacefill.png
Names
IUPAC name
Chloro perchlorate[1]
Systematic IUPAC name
Chloro perchlorate[1]
Other names
Chlorine (I,VII) oxide
Dichlorine tetroxide
Identifiers
3D model (JSmol)
ChemSpider
Properties
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)
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

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 photolysis 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

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
— 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(0.33mol) -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. 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. ^ Jump up to: a b "Chloro Perchlorate - PubChem Public Chemical Database". The PubChem Project. USA: National Center for Biotechnology Information.
  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. ^ Jump up to: 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. doi:10.1021/es903065f. ISSN 0013-936X. PMID 20345093.
  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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Compounds containing perchlorate group
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