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Iodine trichloride: Difference between revisions

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Revision as of 00:23, 23 August 2011 edit86.179.6.201 (talk)No edit summary← Previous edit Latest revision as of 01:20, 28 November 2024 edit undoAnomieBOT (talk | contribs)Bots6,590,323 editsm Dating maintenance tags: {{Cn}} 
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{{chembox {{chembox
| Watchedfields = changed
| verifiedrevid = 400117937 | verifiedrevid = 446239317
⚫ | ImageFile = Iodine-trichloride-dimer-3D-vdW.png
| ImageFile = Iodine trichloride.svg
⚫ | ImageSize =
| ImageName = Full structural formula of the dimer
⚫ | ImageFile2 = Iodine trichloride.JPG
⚫ | ImageSize = 140
⚫ | IUPACName = iodine trichloride
⚫ | ImageFile1 = Iodine-trichloride-dimer-3D-vdW.png
⚫ | OtherNames =
| ImageSize1 = 160
⚫ | Section1 = {{Chembox Identifiers
| ImageName1 = Space-filling model of the dimer
⚫ | ImageFile2 = Iodine trichloride cropped.jpg
| ImageSize2 = 180
| ImageName2 = Commercial sample of iodine trichloride
⚫ | IUPACName = Iodine trichloride
⚫ | OtherNames = Diiodine hexachloride
⚫ |Section1={{Chembox Identifiers
| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}} | ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}}
| ChemSpiderID = 63265 | ChemSpiderID = 63265
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| StdInChIKey_Ref = {{stdinchicite|correct|chemspider}} | StdInChIKey_Ref = {{stdinchicite|correct|chemspider}}
| StdInChIKey = PAWIVBWALDNUJP-UHFFFAOYSA-N | StdInChIKey = PAWIVBWALDNUJP-UHFFFAOYSA-N
| CASNo_Ref = {{cascite|correct|??}}
| CASNo = 865-44-1 | CASNo = 865-44-1
| UNII_Ref = {{fdacite|correct|FDA}}
| UNII = 1E5KQ66TRQ
| PubChem = 70076 | PubChem = 70076
| SMILES = ClI(Cl)Cl | SMILES = ClI(Cl)Cl
| SMILES_Comment = ]
| SMILES1 = Cl1(Cl)(1)(Cl)Cl
| SMILES1_Comment = ]
}} }}
| Section2 = {{Chembox Properties |Section2={{Chembox Properties
| Formula = I<sub>2</sub>Cl<sub>6</sub> | Formula = I<sub>2</sub>Cl<sub>6</sub>
| MolarMass = 466.5281 g/mol | MolarMass = 466.5281 g/mol
| Appearance = yellow solid | Appearance = yellow solid
| Density = 3.11 g/cm<sup>3</sup> | Density = 3.11 g/cm<sup>3</sup>
| MeltingPt = 63 °C | MeltingPtC = 63
| BoilingPt = | BoilingPt =
| Solubility = }} | Solubility =
| MagSus = {{val|-90.2e-6|u=cm<sup>3</sup>/mol}}}}
| Section3 = {{Chembox Hazards |Section3={{Chembox Hazards
| MainHazards = | MainHazards =
| FlashPt = | FlashPt =
| Autoignition = }} | AutoignitionPt =
}}
}} }}


'''Iodine trichloride''' is an ] of ] and ]. It is bright yellow and in the solid state is present as a planar dimer I<sub>2</sub>Cl<sub>6</sub>, Cl<sub>2</sub>I(μ-Cl)<sub>2</sub>ICl<sub>2</sub>, with two bridging Cl atoms.<ref>{{cite journal | author = K. H. Boswijk and E. H. Wiebenga | year = 1954 | title = The crystal structure of I<sub>2</sub>Cl<sub>6</sub> (ICl<sub>3</sub>) | journal = Acta Crystallographica | volume = 7 | part = 5 | issue = 5| pages = 417–423 | doi = 10.1107/S0365110X54001260 }}</ref> '''Iodine trichloride''' is an ] compound of ] and ]. It is bright yellow but upon time and exposure to light it turns red due to the presence of elemental iodine. In the solid state is present as a planar ] I<sub>2</sub>Cl<sub>6</sub>, with two bridging Cl atoms.<ref>{{cite journal | author1 = K. H. Boswijk | author2 = E. H. Wiebenga | year = 1954 | title = The crystal structure of I<sub>2</sub>Cl<sub>6</sub> (ICl<sub>3</sub>) | journal = Acta Crystallographica | volume = 7 | issue = 5| pages = 417–423 | doi = 10.1107/S0365110X54001260 | doi-access = free }}</ref>


It can be prepared by reacting iodine with an excess of liquid chlorine at −70&nbsp;°C. In the melt it is conductive, which may indicate dissociation:<ref name = "Greenwood">{{Greenwood&Earnshaw}}</ref> It can be prepared by reacting iodine with an excess of liquid chlorine at −70&nbsp;°C,<ref name=Greenwood/> or heating a mixture of liquid iodine and chlorine gas to 105&nbsp;°C.{{cn|date=July 2024}} In the molten state it is conductive, which may indicate dissociation:<ref name = "Greenwood">{{Greenwood&Earnshaw}}</ref>
⚫ :I<sub>2</sub>Cl<sub>6</sub> {{eqm}} {{chem|ICl|2|+}} + {{chem|ICl|4|−}}

It is an ], capable of causing fire on contact with organic materials.{{cn|date=November 2024}} That oxidizing power also makes it a useful catalyst for organic ]s.<ref>{{cite book|title=Catalysis in Organic Chemistry|first=Paul|last=Sabatier|translator-first=E.&nbsp;Emmet|translator-last=Reid|location=New York, NY|publisher=Van Nostrand|year=1922|p=2|url=https://www.sciencemadness.org/library/books/catalysis_in_organic_chemistry.pdf}}</ref>
⚫ :I<sub>2</sub>Cl<sub>6</sub> {{eqm}} ICl<sub>2</sub><sup>+</sup> + ICl<sub>4</sub><sup>−</sup>

Iodine trichloride can be created by heating a mixture of liquid iodine and chlorine gas to 105&nbsp;°C.

It is an oxidizing agent, capable of causing fire on contact with organic materials.


==References== ==References==
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{{Iodine compounds}} {{Iodine compounds}}
{{Chlorides}}


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{{inorganic-compound-stub}} {{inorganic-compound-stub}}

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