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

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

Chemical compound

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]

2ClO2 → ClOClO3

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

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

## Properties

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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 = Cs or NO2)[note 2]
bromine | −45 °C | bromine perchlorate (BrOClO3)[note 2]
iodine(0.33 mol) | −50 °C | I(OClO3)3[note 3]

## Notes

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1. ^ Cs[I(OClO3)4] is a pale yellow salt which is stable at room temperature. It has a square IO4 unit.
2. ^ 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).
3. ^ 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

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1. ^ 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. ^ 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.
5. ^ 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.
6. ^ 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.

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Salts and covalent derivatives of the perchlorate ion

| HClO4 |  |  |  | He

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|
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LiClO4 | Be(ClO4)2 | B(ClO4)−4
B(ClO4)3 | ROClO3 | N(ClO4)3
NH4ClO4
NOClO4
NO2ClO4 | H3OClO4 | FClO4 | Ne
NaClO4 | Mg(ClO4)2 | Al(ClO4)3
Al(ClO4)−4
Al(ClO4)2−5
Al(ClO4)3−6 | Si  | P  | S  | ClO−4
ClOClO3
Cl2O7 | Ar
KClO4 | Ca(ClO4)2 |  | Sc(ClO4)3 | Ti(ClO4)4 | VO(ClO4)3
VO2(ClO4)  | Cr(ClO4)3 | Mn(ClO4)2 | Fe(ClO4)2
Fe(ClO4)3 | Co(ClO4)2
Co(ClO4)3 | Ni(ClO4)2 | Cu(ClO4)2 | Zn(ClO4)2 | Ga(ClO4)3 | Ge  | As  | Se  | BrOClO3 | Kr
RbClO4 | Sr(ClO4)2 |  | Y(ClO4)3 | Zr(ClO4)4 | Nb(ClO4)5 | MoO2(ClO4)2 | Tc  | Ru  | Rh(ClO4)3 | Pd(ClO4)2 | AgClO4 | Cd(ClO4)2 | In(ClO4)3 | Sn(ClO4)4 | Sb(ClO4)3 | TeO(ClO4)2 | I(OClO3)3 | Xe(OClO3)2
CsClO4 | Ba(ClO4)2 | *  | Lu(ClO4)3 | Hf(ClO4)4 | Ta(ClO4)5
TaO(ClO4)3
TaO2ClO4 | WO(ClO4)4 | ReO3ClO4 | Os  | Ir  | Pt  | Au(ClO4)−4 | Hg2(ClO4)2
Hg(ClO4)2 | Tl(ClO4)
Tl(ClO4)3 | Pb(ClO4)2 | Bi(ClO4)3 | Po  | At  | Rn
FrClO4 | Ra  | **  | Lr  | Rf  | Db  | Sg  | Bh  | Hs  | Mt  | Ds  | Rg  | Cn  | Nh  | Fl  | Mc  | Lv  | Ts  | Og

*  | La(ClO4)3 | Ce(ClO4)x | Pr(ClO4)3 | Nd(ClO4)3 | Pm  | Sm(ClO4)3 | Eu(ClO4)3 | Gd(ClO4)3 | Tb(ClO4)3 | Dy(ClO4)3 | Ho(ClO4)3 | Er(ClO4)3 | Tm(ClO4)3 | Yb(ClO4)3
**  | Ac  | Th(ClO4)4 | Pa  | UO2(ClO4)2 | Np  | Pu  | Am  | Cm  | Bk  | Cf  | Es  | Fm  | Md  | No

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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

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Oxygen compounds

* Ag4O4
* Al2O3
* AmO2
* Am2O3
* As2O3
* As2O5
* Au2O3
* B2O3
* BaO
* BeO
* Bi2O3
* BiO2
* Bi2O5
* BrO2
* Br2O3
* Br2O5
* Br

* CO
* CO2
* C3O2
* CaO
* CaO2
* CdO
* CeO2
* Ce3O4
* Ce2O3
* ClO2
* Cl2O
* Cl2O2
* Cl2O3
* Cl2O4
* Cl2O6
* Cl2O7
* CoO
* Co2O3
* Co3O4
* CrO3
* Cr2O3
* Cr2O5
* Cr5O12
* CsO2
* Cs2O3
* CuO
* Dy2O3
* Er2O3
* Eu2O3
* FeO
* Fe2O3
* Fe3O4
* Ga2O
* Ga2O3
* GeO
* GeO2
* H2O
* 2H2O
* 3H2O
* H218O
* H2O2
* HfO2
* HgO
* Hg2O
* Ho2O3
* IO
* 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
* O2F
* OF
* OF2
* O2F2
* O3F2
* O4F2
* O5F2
* O6F2
* O2PtF6
* more...

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