Chlorine perchlorate
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Names | |||
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IUPAC name
Chloro perchlorate[1]
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Systematic IUPAC name
Chloro perchlorate[1] | |||
Other names
Chlorine(I,VII) oxide
Dichlorine tetroxide | |||
Identifiers | |||
3D model (
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ChemSpider | |||
PubChem CID
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CompTox Dashboard (EPA)
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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 | |||
Occupational safety and health (OHS/OSH): | |||
Main hazards
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oxidizer | ||
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Chlorine perchlorate is a
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
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
Reactant | Conditions | Products |
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— | 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 = NO2)[note 2]
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bromine | −45 °C | bromine perchlorate (BrOClO3)[note 2] |
iodine(0.33 mol) | −50 °C | I(OClO3)3[note 3] |
Notes
- ^ Cs[I(OClO3)4] is a pale yellow salt which is stable at room temperature. It has a square IO4 unit.
- ^ 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).
- ^ 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
- ^ a b "Chloro Perchlorate - PubChem Public Chemical Database". The PubChem Project. USA: National Center for Biotechnology Information.
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- ^ PMID 20345093.
- doi:10.1070/RC1988v057n11ABEH003410. Translated from Uspekhi Khimiivolume 57 (1988), pp. 1815-1839.
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