Iodyl fluoride

Last updated
Iodyl fluoride
IO2F.svg
Names
IUPAC name
  • Fluoro(dioxo)-λ5-iodane
  • Iodine(V) fluoride dioxide
Identifiers
3D model (JSmol)
ChemSpider
PubChem CID
  • InChI=1S/FIO2/c1-2(3)4
    Key: FRYHXHDHQQGJSF-UHFFFAOYSA-N
  • O=I(F)=O
Properties
IO2F
Molar mass 177.901 g·mol−1
Appearancecolorless crystals
Density 4.982 g/cm3
Melting point 200 °C (392 °F; 473 K)
Reacts with water
Related compounds
Related compounds
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).

Iodyl fluoride is an inorganic compound of iodine, fluorine, and oxygen with the chemical formula I O 2 F . 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. [1]

Contents

Synthesis

Iodyl fluoride can be decomposed by iodosyl trifluoride heated to 110 °C (230 °F) in nitrogen. Since this reaction is reversible, the reaction requires constant removal of iodine pentafluoride. [1]

2 IOF3 ⇌ IO2F + IF5

It can also be obtained by dissolving iodine pentoxide, I2O5, in anhydrous hydrogen fluoride. [2]

I2O5 + HF → IO2F + HIO3

Physical properties

Iodyl fluoride forms colorless crystals of orthorhombic system. [3] Reacts with water. [4]

Chemical properties

Iodyl fluoride is stable in dry air, but slowly hydrolyzes to iodic and hydrofluoric acids in moisture. [1]

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. [5] [6]

3 IO2F + 4 BrF3 → 3 IF5 + 2 Br2 + 3 O2
IO2F + 2 SeF4 → IF5 + 2 SeOF2

References

  1. 1 2 3 Aynsley, E. E.; Nichols, R.; Robinson, P. L. (1 January 1953). "126. Reactions of iodine pentafluoride with inorganic substances. Iodine oxytrifluoride and iodyl fluoride" . Journal of the Chemical Society : 623–626. doi:10.1039/JR9530000623. ISSN   0368-1769 . Retrieved 24 May 2023.
  2. ↑ Wiberg, Egon; Wiberg, Nils (2001). Inorganic Chemistry. Academic Press. p. 468. ISBN   978-0-12-352651-9 . Retrieved 24 May 2023.
  3. ↑ Minkwitz, Rolf; Berkei, Michael; Ludwig, Ralf (1 December 2001). "Crystal Structure of IO2F" . Inorganic Chemistry . 40 (25): 6493–6495. doi:10.1021/ic0105462. ISSN   0020-1669. PMID   11720506 . Retrieved 24 May 2023.
  4. ↑ Haynes, William M. (4 June 2014). CRC Handbook of Chemistry and Physics. CRC Press. p. 4-67. ISBN   978-1-4822-0868-9 . Retrieved 24 May 2023.
  5. ↑ Schmeisser, M.; Brändle, K. (1 January 1963). "Oxides and Oxyfluorides of the Halogens" . Advances in Inorganic Chemistry and Radiochemistry. 5. Academic Press: 41–89. doi:10.1016/S0065-2792(08)60152-1. ISBN   9780120236053 . Retrieved 24 May 2023.{{cite journal}}: ISBN / Date incompatibility (help)
  6. ↑ Advances in Inorganic Chemistry and Radiochemistry. Academic Press. 1 January 1963. ISBN   978-0-08-057854-5 . Retrieved 24 May 2023.{{cite book}}: ISBN / Date incompatibility (help)
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