Chlorine perchlorate
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| Names | |||
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| IUPAC name
Chlorine perchlorate
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| Systematic IUPAC name
Chloro perchlorate[1] | |||
| Other names
Chlorine (I,VII) oxide
Dichlorine tetroxide | |||
| Identifiers | |||
3D model (JSmol)
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| ChemSpider | |||
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). | |||
| 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[edit]
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[edit]
- ^ "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.
Compounds containing perchlorate group
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| HClO4 | He | ||||||||||||||||||
| LiClO4 | Be(ClO4)2 | B(ClO 4)− 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 | |||||