| 词条 | Dichlorine hexoxide |
| 释义 |
| Watchedfields = changed | verifiedrevid = 440332808 | ImageFile = Dichlorine hexoxide.svg | ImageSize = 260 | ImageFileL1 = Dichlorine-hexoxide molecule spacefill.png | ImageSizeL1 = 105 | ImageAltL1 = Space-filling model of the dichlorine hexoxide molecule | ImageFileR1 = Dichlorine-hexoxide ions spacefill.png | ImageSizeR1 = 135 | ImageAltR1 = Space-filling model of the component ions of dichlorine hexoxide | IUPACName = Dichlorine hexoxide | OtherNames = Chlorine trioxide; Chloryl perchlorate; Chlorine(V,VII) oxide |Section1={{Chembox Identifiers | CASNo_Ref = {{cascite|correct|??}} | CASNo = 12442-63-6 | PubChem = 129690529 | PubChem_Comment = incorrect diagram | ChemSpiderID = 9564507 | ChemSpiderID_Comment = incorrect charge | SMILES = O=[Cl](=O)O[Cl](=O)(=O)=O | InChI=1S/Cl2O6/c3-1(4)8-2(5,6)7 | InChIKey = BMVIIZAOKBSWDS-UHFFFAOYSA-N |Section2={{Chembox Properties | Formula = Cl2O6 | MolarMass = 166.901 g/mol | Appearance = red liquid | Density = 1.65 g/cm3 | MeltingPtC = 3.5 | BoilingPtC = 200 | Solubility = Reacts |Section3={{Chembox Hazards | MainHazards = oxidizer | FlashPt = | AutoignitionPt = }} Dichlorine hexoxide is the chemical compound with the molecular formula {{chem|Cl|2|O|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 {{chem|[ClO|2|]|+|[ClO|4|]|-}}, which may be thought of as the mixed anhydride of chloric and perchloric acids. It is produced by reaction between chlorine dioxide and excess ozone: 2 {{chem|ClO|2}} + 2 {{chem|O|3}} → 2 {{chem|ClO|3}} + 2 {{chem|O|2}} → {{chem|Cl|2|O|6}} + 2 {{chem|O|2}} Molecular structureIt was originally reported to exist as the monomeric chlorine trioxide ClO3 in gas phase,[1] but was later shown to remain an oxygen-bridged dimer after evaporation and until thermal decomposition into chlorine perchlorate, Cl2O4, and oxygen.[2] The compound ClO3 was then rediscovered.[3] It is a dark red fuming liquid at room temperature that crystallizes as a red ionic compound, chloryl perchlorate, {{chem|[ClO|2|]|+|[ClO|4|]|-}}. 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). PropertiesCl2O6 is diamagnetic and is a very strong oxidizing agent. Although stable at room temperature, it explodes violently on contact with organic compounds[4] and reacts with gold to produce the chloryl salt {{chem|[ClO|2|]|+|[Au(ClO|4|)|4|]|-}}.[5] Many other reactions involving Cl2O6 reflect its ionic structure, {{chem|[ClO|2|]|+|[ClO|4|]|-}}, 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 → [ClO2]2[Sn(ClO4)6] + 4 ClO2 + 2 Cl2 2Au + 6Cl2O6 → 2{{chem|[ClO|2|]|+|[Au(ClO|4|)|4|]|-}} + Cl2 Nevertheless, it can also react as a source of the ClO3 radical: 2 AsF5 + Cl2O6 → 2 ClO3AsF5 References1. ^{{cite journal|journal=Nature|title=Chlorine Hexoxide and Chlorine Trioxide|volume=132|pages=514–515|year=1933|doi=10.1038/132514b0|author=C. F. Goodeve, F. A. Todd|issue=3335}} {{Chlorine compounds}}{{oxygen compounds}}2. ^{{cite journal|first=Maria|last=Lopez|author2=Juan E. Sicre|title=Physicochemical properties of chlorine oxides. 1. Composition, ultraviolet spectrum, and kinetics of the thermolysis of gaseous dichlorine hexoxide|journal=J. Phys. Chem.|year=1990|volume=94|issue=9|pages=3860–3863|doi=10.1021/j100372a094}} 3. ^{{cite journal|first1=Hinrich|last1=Grothe|first2=Helge|last2=Willner|title=Chlorine Trioxide: Spectroscopic Properties, Molecular Structure, and Photochemical Behavior|journal=Angew. Chem. Int. Ed.|year=1994|volume=33|issue=14|pages=1482–1484|doi=10.1002/anie.199414821}} 4. ^{{cite book|title=Concise encyclopedia chemistry|author=Mary Eagleson|url=https://books.google.com/books?id=Owuv-c9L_IMC|isbn=3-11-011451-8|year=1994|publisher=Walter de Gruyter|page=215}} 5. ^{{cite journal|first=Frédérique|last=Cunin|author2=Catherine Deudon |author3=Frédéric Favier |author4=Bernard Mula |author5=Jean Louis Pascal |title=First anhydrous gold perchlorato complex: {{chem|ClO|2|Au(ClO|4|)|4}}. Synthesis and molecular and crystal structure analysis|journal=Inorganic Chemistry|volume=41|issue=16|year=2002|pages=4173–4178|doi=10.1021/ic020161z|pmid=12160405}} 6. ^{{cite book|page=65|url=https://books.google.com/books?id=pRXIwIV-hB8C|title=Advances in Inorganic Chemistry and Radiochemistry|isbn=0-12-023605-2|publisher=Academic Press|year=1963|author= Harry Julius Emeléus, Alan George Sharpe}} 4 : Chlorine oxides|Acidic oxides|Perchlorates|Chloryl compounds |
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