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 IO2F. 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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