iodyl fluoride
{{Chembox
| Name = Iodyl fluoride
| ImageFile1 = IO2F.svg
| ImageSize1 = 200px
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| ImageSize2 = 200px
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| IUPACName = {{ubl|Fluoro(dioxo)-λ5-iodane|Iodine(V) fluoride dioxide}}
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|Section1={{Chembox Identifiers
| CASNo = 28633-62-7
| CASNo_Ref = {{cascite|correct|CAS}}
| ChemSpiderID = 57449638
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| DTXSID =
| EINECS =
| Gmelin =
| PubChem = 44546993
| SMILES = O=I(F)=O
| StdInChI=1S/FIO2/c1-2(3)4
| StdInChIKey = FRYHXHDHQQGJSF-UHFFFAOYSA-N
}}
|Section2={{Chembox Properties
| Formula = {{chem2|IO2F}}
| F=1 | O=2 |I=1
| Appearance = colorless crystals
| Density = 4.982 g/cm3
| MeltingPtC = 200
| BoilingPtC =
| Solubility = Reacts with water}}
|Section3={{Chembox Hazards
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|Section6={{Chembox Related
| OtherCompounds = {{ubl|Chloryl fluoride|Bromyl fluoride|Iodosyl pentafluoride|Iodosyl trifluoride|Periodyl fluoride|Iodyl trifluoride}}
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Iodyl fluoride is an inorganic compound of iodine, fluorine, and oxygen with the chemical formula {{chem2|IO2F|auto=1}}. It is in the form of colorless crystals. Iodyl fluoride features iodine in the oxidation state of +5. The compound was initially synthesized in 1951.{{cite journal |last1=Aynsley |first1=E. E. |last2=Nichols |first2=R. |last3=Robinson |first3=P. L. |title=126. Reactions of iodine pentafluoride with inorganic substances. Iodine oxytrifluoride and iodyl fluoride |journal=Journal of the Chemical Society |date=1 January 1953 |pages=623–626 |doi=10.1039/JR9530000623 |url=https://pubs.rsc.org/en/content/articlelanding/1953/JR/jr9530000623 |access-date=24 May 2023 |language=en |issn=0368-1769}}
Synthesis
Iodyl fluoride can be decomposed by iodosyl trifluoride heated to {{cvt|110|C|F}} in nitrogen. Since this reaction is reversible, the reaction requires constant removal of iodine pentafluoride.
:{{chem2|2 IOF3 ⇌ IO2F + IF5}}
It can also be obtained by dissolving iodine pentoxide, {{chem2|I2O5}}, in anhydrous hydrogen fluoride.{{cite book |last1=Wiberg |first1=Egon |last2=Wiberg |first2=Nils |title=Inorganic Chemistry |date=2001 |publisher=Academic Press |isbn=978-0-12-352651-9 |page=468 |url=https://books.google.com/books?id=Mtth5g59dEIC&dq=Iodosyl+trifluoride&pg=PA468 |access-date=24 May 2023 |language=en}}
:{{chem2|I2O5 + HF -> IO2F + HIO3}}
Physical properties
Iodyl fluoride forms colorless crystals of orthorhombic system.{{cite journal |last1=Minkwitz |first1=Rolf |last2=Berkei |first2=Michael |last3=Ludwig |first3=Ralf |title=Crystal Structure of IO2F |journal=Inorganic Chemistry |date=1 December 2001 |volume=40 |issue=25 |pages=6493–6495 |doi=10.1021/ic0105462 |pmid=11720506 |url=https://pubs.acs.org/doi/10.1021/ic0105462 |access-date=24 May 2023 |language=en |issn=0020-1669}} Reacts with water.{{cite book |last1=Haynes |first1=William M. |title=CRC Handbook of Chemistry and Physics |date=4 June 2014 |publisher=CRC Press |isbn=978-1-4822-0868-9 |page=4-67 |url=https://books.google.com/books?id=bNDMBQAAQBAJ&dq=Iodosyl+trifluoride&pg=SA4-PA67 |access-date=24 May 2023 |language=en}}
Chemical properties
Iodyl fluoride is stable in dry air, but slowly hydrolyzes to iodic and hydrofluoric acids in moisture.
:{{chem2|IO2F + H2O -> HIO3 + HF}}
The compound reacts with strong fluorinating agents such as bromine trifluoride and selenium tetrafluoride to form iodine pentafluoride. Iodyl fluoride can be reduced to elemental iodine by pure hydrogen peroxide.{{cite journal |last1=Schmeisser |first1=M. |last2=Brändle |first2=K. |title=Oxides and Oxyfluorides of the Halogens |journal=Advances in Inorganic Chemistry and Radiochemistry |date=1 January 1963 |volume=5 |pages=41–89 |url=https://www.sciencedirect.com/science/article/abs/pii/S0065279208601521 |access-date=24 May 2023 |publisher=Academic Press |doi=10.1016/S0065-2792(08)60152-1 |isbn=9780120236053 |language=en}}{{cite book |title=Advances in Inorganic Chemistry and Radiochemistry |date=1 January 1963 |publisher=Academic Press |isbn=978-0-08-057854-5 |url=https://books.google.com/books?id=pRXIwIV-hB8C&dq=%22Iodyl+fluoride%22&pg=PA83 |access-date=24 May 2023 |language=en}}
References
{{Reflist}}
{{Iodine compounds}}
{{Oxygen compounds}}
{{Fluorine compounds}}