Chlorine perchlorate
| |||
| Names | |||
|---|---|---|---|
| IUPAC name
Chlorine perchlorate | |||
| Systematic IUPAC name
Chloro perchlorate[1] | |||
| Other names
Chlorine (I,VII) oxide Dichlorine tetroxide | |||
| Identifiers | |||
27218-16-2  | |||
| 3D model (Jmol) | Interactive image | ||
| ChemSpider | 147540  | ||
| PubChem | 168667 | ||
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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 ?) | |||
| Infobox references | |||
Chlorine perchlorate is the chemical compound with the formula Cl2O4. This chlorine oxide is an asymmetric oxide, with one chlorine atom in oxidation state +1 and the other +7, with proper formula ClOClO3. It is produced by the photolysis of chlorine dioxide at room temperature with 436 nm ultraviolet light:[2][3]
- 2 ClO2 → ClOClO3
Chlorine perchlorate can also be made the following reactions at −45 °C.
- CsClO4 + ClOSO2F → Cs(SO3)F + ClOClO3
Chlorine perchlorate is a pale greenish liquid which decomposes at room temperature.
Properties
It is less stable than ClO2 and decomposes to O2, Cl2 and Cl2O6 at room temperature.
Chlorine perchlorate reacts with metal chlorides forming anhydrous perchlorates:
- CrO2Cl2 + 2 ClOClO3 → 2 Cl2 + CrO2(ClO4)2
- TiCl4 + 4 ClOClO3 → 4 Cl2 + Ti(ClO4)4
References
- ↑ "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.
| Salts and the ester of the perchlorate ion | |||||||||||||||||||
|---|---|---|---|---|---|---|---|---|---|---|---|---|---|---|---|---|---|---|---|
| HClO4 | He | ||||||||||||||||||
| LiClO4 | Be(ClO4)2 | B(ClO4)4− | ROClO3 | N(ClO4)3 NH4ClO4 |
O | FClO4 | Ne | ||||||||||||
| NaClO4 | Mg(ClO4)2 | Al(ClO4)3 | Si | P | S | ClO4− ClOClO3 Cl2O7 |
Ar | ||||||||||||
| KClO4 | Ca(ClO4)2 | Sc(ClO4)3 | Ti(ClO4)4 | VO(ClO4)3 | 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 | Zr | Nb | Mo | Tc | Ru | Rh | Pd(ClO4)2 | AgClO4 | Cd(ClO4)2 | In | Sn | Sb | Te | I | Xe | ||
| CsClO4 | Ba(ClO4)2 | Hf | Ta | W | Re | Os | Ir | Pt | Au | Hg2(ClO4)2, Hg(ClO4)2 |
Tl(ClO4)3 | Pb(ClO4)2 | Bi(ClO4)3 | Po | At | Rn | |||
| Fr | Ra | Rf | Db | Sg | Bh | Hs | Mt | Ds | Rg | Cn | Nh | Fl | Mc | Lv | Ts | Og | |||
| ↓ | |||||||||||||||||||
| La | Ce(ClO4)x | Pr | Nd | Pm | Sm | Eu | Gd | Tb | Dy | Ho | Er | Tm | Yb | Lu | |||||
| Ac | Th | Pa | UO2(ClO4)2 | Np | Pu | Am | Cm | Bk | Cf | Es | Fm | Md | No | Lr | |||||
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