Dichlorine hexoxide

In today's world, Dichlorine hexoxide occupies a central place in our lives. Whether through its impact on society, fashion, science or culture, Dichlorine hexoxide arouses constant interest and generates a variety of opinions and debates. From its origins to its influence on the present, the presence of Dichlorine hexoxide is undeniable and inevitable. In this article, we will closely explore the importance of Dichlorine hexoxide and its role in different aspects of everyday life, as well as its evolution over time.

Dichlorine hexoxide
Space-filling model of the dichlorine hexoxide molecule
Space-filling model of the component ions of dichlorine hexoxide
Names
IUPAC name
Dichlorine hexoxide
Other names
Chlorine trioxide; Chloryl perchlorate; Chlorine(V,VII) oxide
Identifiers
3D model (JSmol)
ChemSpider
  • InChI=1S/Cl2O6/c3-1(4)8-2(5,6)7
    Key: BMVIIZAOKBSWDS-UHFFFAOYSA-N
  • O=(=O)O(=O)(=O)=O
  • O==O.Cl(=O)(=O)=O
Properties
Cl2O6
Molar mass 166.901 g/mol
Appearance red liquid
Density 1.65 g/cm3
Melting point 3.5 °C (38.3 °F; 276.6 K)
Boiling point 200 °C (392 °F; 473 K)
Reacts
Hazards
Occupational safety and health (OHS/OSH):
Main hazards
 oxidizer
Except where otherwise noted, data are given for materials in their standard state (at 25 °C , 100 kPa).
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Dichlorine hexoxide is the chemical compound with the molecular formula Cl
2O
6, which is correct for its gaseous state. However, in liquid or solid form, this chlorine oxide ionizes into the dark red ionic compound chloryl perchlorate +
−
, which may be thought of as the mixed anhydride of chloric and perchloric acids. This compound is a notable perchlorating agent.[1]

It is produced by reaction between chlorine dioxide and excess ozone:

2 ClO
2 + 2 O
3 → 2 ClO
3 + 2 O
2 → Cl
2O
6 + 2 O
2

Molecular structure

It was originally reported to exist as the monomeric chlorine trioxide ClO3 in gas phase,[2] but was later shown to remain an oxygen-bridged dimer after evaporation and until thermal decomposition into chlorine perchlorate, Cl2O4, and oxygen.[3] The compound ClO3 was then rediscovered.[4]

It is a dark red fuming liquid at room temperature that crystallizes as a red ionic compound, chloryl perchlorate, +
−
. The red color shows the presence of chloryl ions. Thus, chlorine's formal oxidation state in this compound remains a mixture of chlorine (V) and chlorine (VII) both in the gas phase and when condensed; however by breaking one oxygen-chlorine bond some electron density does shifts towards the chlorine (VII).

Properties

Cl2O6 is diamagnetic and is a very strong oxidizing agent. Although stable at room temperature, it explodes violently on contact with organic compounds[5] It is a strong dehydrating agent:

Cl2O6 + H2O → HClO4 + HClO3

Many reactions involving Cl2O6 reflect its ionic structure, +
−
, including the following:[6]

NO2F + Cl2O6 → NO2ClO4 + ClO2F
NO + Cl2O6 → NOClO4 + ClO2
2 V2O5 + 12 Cl2O6 → 4 VO(ClO4)3 + 12 ClO2 + 3 O2
SnCl4 + 6 Cl2O6 → 2 + 4 ClO2 + 2 Cl2

It reacts with gold to produce the chloryl salt +
−
:[7]

2Au + 6Cl2O6 → 2+
−
 + Cl2

Several other transition metal perchlorate complexes are prepared using dichlorine hexoxide.

Nevertheless, it can also react as a source of the ClO3 radical:[citation needed]

2 AsF5 + Cl2O6 → 2 ClO3AsF5
Synthesis:
4ClO2 + 2O3→2Cl2O6+O2(UV)

References

  1. ^ Jean-Louis Pascal; Frédéric Favier (1998). "Inorganic perchlorato complexes". Coordination Chemistry Reviews. 178–180 (1): 865–902. doi:10.1016/S0010-8545(98)00102-7.
  2. ^ C. F. Goodeve, F. A. Todd (1933). "Chlorine Hexoxide and Chlorine Trioxide". Nature. 132 (3335): 514–515. Bibcode:1933Natur.132..514G. doi:10.1038/132514b0. S2CID 4116929.
  3. ^ Lopez, Maria; Juan E. Sicre (1990). "Physicochemical properties of chlorine oxides. 1. Composition, ultraviolet spectrum, and kinetics of the thermolysis of gaseous dichlorine hexoxide". J. Phys. Chem. 94 (9): 3860–3863. doi:10.1021/j100372a094.
  4. ^ Grothe, Hinrich; Willner, Helge (1994). "Chlorine Trioxide: Spectroscopic Properties, Molecular Structure, and Photochemical Behavior". Angew. Chem. Int. Ed. 33 (14): 1482–1484. doi:10.1002/anie.199414821.
  5. ^ Mary Eagleson (1994). Concise encyclopedia chemistry. Walter de Gruyter. p. 215. ISBN 3-11-011451-8.
  6. ^ Harry Julius Emeléus, Alan George Sharpe (1963). Advances in Inorganic Chemistry and Radiochemistry. Academic Press. p. 65. ISBN 0-12-023605-2.
  7. ^ Cunin, Frédérique; Catherine Deudon; Frédéric Favier; Bernard Mula; Jean Louis Pascal (2002). "First anhydrous gold perchlorato complex: ClO
    2    Au(ClO
    4    )
    4    . Synthesis and molecular and crystal structure analysis". Inorganic Chemistry. 41 (16): 4173–4178. doi:10.1021/ic020161z. PMID 12160405.