Chlorine perchlorate

Chlorine perchlorate
Names
	IUPAC name Chloro perchlorate
	Systematic IUPAC name Chloro perchlorate
	Other names Chlorine(I,VII) oxide; Dichlorine tetroxide; (Chlorooxy)chlorane trioxide;
Identifiers
CAS Number	27218-16-2 ;
3D model (JSmol)	Interactive image;
ChEBI	CHEBI:52353;
ChemSpider	147540 ;
PubChem CID	168667;
	InChI InChI=1S/Cl2O4/c1-6-2(3,4)5 Key: JRONPIZRZBBOBR-UHFFFAOYSA-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).
	verify (what is ?)
	Infobox references

Chlorine perchlorate is a chemical compound with the formula Cl
2O
4. This chlorine oxide is an asymmetric oxide, with one chlorine atom in +1 oxidation state and the other +7, with proper formula Cl–O–ClO
3. It is produced by the photodimerization of chlorine dioxide (ClO
2) at room temperature by 436 nm ultraviolet light:^[3]^[4]^[5]

2 ClO
2 → ClOClO
3

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

CsClO
4 + ClOSO
2F → CsSO
3F + ClOClO
3

Properties

Chlorine perchlorate is a pale greenish liquid. It is less stable than ClO
2 (chlorine dioxide)^{[citation needed]} and decomposes at room temperature to give O
2 (oxygen), Cl
2 (chlorine) and Cl
2O
6 (dichlorine hexoxide):

2 ClOClO
3 → O
2 + Cl
2 + Cl
2O
6

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

CrO
2Cl
2 + 2 ClOClO
3 → 2 Cl
2 + CrO
2(ClO
4)
2

TiCl
4 + 4 ClOClO
3 → 4 Cl
2 + Ti(ClO
4)
4

2 AgCl + 2 ClOClO
3 → 2 AgClO
4 + Cl
2

Reactions

Reactant	Conditions	Products
—	Heat	dichlorine hexoxide (80%), chlorine dioxide, chlorine, oxygen
—	Ultraviolet light	dichlorine heptoxide, chlorine, oxygen^[5]
caesium iodide	−45 °C	caesium tetraperchloratoiodate(III) Cs+ [I(OClO 3) 4]− ^{[note 1]}
ClOSO 2F or ClF	—	M+ ClO− 4 (M = Cs or [NO 2])^{[note 2]}
bromine	−45 °C	bromine perchlorate (BrOClO 3)^{[note 2]}
iodine(0.33 mol)	−50 °C	iodine(III) perchlorate I(OClO 3) 3^{[note 3]}
CF₃I	-112 °C	CF₃OClO₃, O₂, Cl₂, Cl 2O 7, and I 2O 5.^[8]

Notes

↑ Cs+
[I(OClO
3)
4]−
is a pale yellow salt which is stable at room temperature. It has a square IO
4 unit.
↑ ^2.0 ^2.1 M+
ClO−
4 (M = Cs or [NO
2]) reacts with BrOSO
2F at −20 °C and produces bromine perchlorate (BrOClO
3). Bromine perchlorate then reacts with hydrogen bromide (HBr) at −70 °C and produces elemental bromine (Br
2) and perchloric acid (HClO
4).
↑ The last^[6] attempt to form iodine monoperchlorate (IOClO
3) occurred in 1972,^[7] and even at low temperatures yielded instead the triperchlorate. On warming, the latter then decomposes to iodate.

References

↑ nih.gov
↑ ^2.0 ^2.1 "Chloro Perchlorate - PubChem Public Chemical Database". The PubChem Project. USA: National Center for Biotechnology Information. https://pubchem.ncbi.nlm.nih.gov/compound/168667.
↑ 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.
↑ ^5.0 ^5.1 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.
↑ Zefirov, N. S.; Zedankin, V. V.; Koz'min, A. S. (1988). "The synthesis and properties of covalent organic perchlorates". Russian Chemical Reviews (Turpion) 57 (11): 1047. doi:10.1070/RC1988v057n11ABEH003410. Translated from Uspekhi Khimii volume 57 (1988), pp. 1815-1839.
↑ Christe, Karl O.; Schack, Carl J. (1972). "Iodine tris(perch1orate) and cesium tetrakis(perchlorato)iodate(III)". Inorganic Chemistry 11 (7): 1684. doi:10.1021/ic50113a047.
↑ Schack, Carl J.; Pilipovich, Don; Christe, Karl O. (1975). "Halogen perchlorates: Reactions with fluorocarbon halides". Inorganic Chemistry 14 (1). doi:10.1021/ic50143a032.

v t e Compounds containing perchlorate group
HClO₄																	He
LiClO₄	Be(ClO₄)₂											B(ClO₄)−4 B(ClO₄)₃	ROClO₃	N(ClO₄)₃ NH₄ClO₄ NOClO₄	O	FClO₄	Ne
NaClO₄	Mg(ClO₄)₂											Al(ClO₄)₃	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)₃	Co(ClO₄)₂, Co(ClO₄)₃	Ni(ClO₄)₂	Cu(ClO₄)₂	Zn(ClO₄)₂	Ga(ClO₄)₃	Ge	As	Se	Br	Kr
RbClO₄	Sr(ClO₄)₂	Y(ClO₄)₃	Zr(ClO₄)₄	Nb(ClO₅)₄	Mo	Tc	Ru	Rh(ClO₄)₃	Pd(ClO₄)₂	AgClO₄	Cd(ClO₄)₂	In(ClO₄)₃	Sn(ClO₄)₄	Sb	TeO(ClO₄)₂	I	Xe
CsClO₄	Ba(ClO₄)₂		Hf(ClO₄)₄	Ta(ClO₅)₅	W	Re	Os	Ir	Pt	Au	Hg₂(ClO₄)₂, Hg(ClO₄)₂	Tl(ClO₄)₃	Pb(ClO₄)₂	Bi(ClO₄)₃	Po	At	Rn
FrClO₄	Ra		Rf	Db	Sg	Bh	Hs	Mt	Ds	Rg	Cn	Nh	Fl	Mc	Lv	Ts	Og
		↓
		La	Ce(ClO₄)_x	Pr	Nd	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	Lu(ClO₄)₃
		Ac	Th(ClO₄)₄	Pa	UO₂(ClO₄)₂	Np	Pu	Am	Cm	Bk	Cf	Es	Fm	Md	No	Lr

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Original source: https://en.wikipedia.org/wiki/Chlorine perchlorate. Read more

[note1-6] Cs+
[I(OClO
3)
4]−
is a pale yellow salt which is stable at room temperature. It has a square IO
4 unit.

[note2-7] 2.0 ^2.1 M+
ClO−
4 (M = Cs or [NO
2]) reacts with BrOSO
2F at −20 °C and produces bromine perchlorate (BrOClO
3). Bromine perchlorate then reacts with hydrogen bromide (HBr) at −70 °C and produces elemental bromine (Br
2) and perchloric acid (HClO
4).

[note3-10] The last^[6] attempt to form iodine monoperchlorate (IOClO
3) occurred in 1972,^[7] and even at low temperatures yielded instead the triperchlorate. On warming, the latter then decomposes to iodate.

[pubchem-1] .gov

[:1-2] 2.0 ^2.1 "Chloro Perchlorate - PubChem Public Chemical Database". The PubChem Project. USA: National Center for Biotechnology Information. https://pubchem.ncbi.nlm.nih.gov/compound/168667.

[3] 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.

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

[:0-5] 5.0 ^5.1 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.

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

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

[11] Schack, Carl J.; Pilipovich, Don; Christe, Karl O. (1975). "Halogen perchlorates: Reactions with fluorocarbon halides". Inorganic Chemistry 14 (1). doi:10.1021/ic50143a032.

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[3]

[4]

[5]

[note 1]

[note 2]

[note 3]

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Chlorine perchlorate

Topic: Chemistry

Contents

Properties

Reactions

Notes

References