Chemistry:Chlorine perchlorate
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| Names | |||
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| IUPAC name
Chloro perchlorate[2]
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| Systematic IUPAC name
Chloro perchlorate[2] | |||
Other names
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| Identifiers | |||
3D model (JSmol)
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PubChem CID
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| 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). | |||
 verify (what is   ?)
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| Infobox references | |||
Tracking categories (test):
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.
Compounds containing perchlorate group
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| 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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