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Contents

   



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1 Synthesis  




2 Physical properties  




3 Chemical properties  




4 References  













Iodine trifluoride dioxide






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From Wikipedia, the free encyclopedia
  
(Redirected from Iodyl trifluoride)
Iodine trifluoride dioxide
Names
Other names

Iodyl trifluoride

Identifiers

CAS Number

3D model (JSmol)

  • InChI=1S/F3IO2/c1-4(2,3,5)6

    Key: IEYUHHXVKPWNHY-UHFFFAOYSA-N

  • F[I](=O)(=O)(F)F

Properties

Chemical formula

 F3IO2
Molar mass 215.898 g·mol−1
Appearance yellow crystals
Melting point 41 °C (106 °F; 314 K)
Hazards
Occupational safety and health (OHS/OSH):

Main hazards

 ignites on contact with flammable organic substances
Related compounds

Related compounds

 Iodosyl trifluoride
Iodosyl pentafluoride

Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).

Infobox references

Iodine trifluoride dioxide is an inorganic compoundofiodine, fluorine, and oxygen with the chemical formula IO2F3.[1][2][3] The compound was first obtained by Engelbrecht and Petersy in 1969.[4]

Synthesis

[edit]

Iodine trifluoride dioxide may be formed by the reaction of HOIOF4 and oleum.[4]

Physical properties

[edit]

Iodine trifluoride dioxide forms yellow crystals, which melt at 41 °C.[5] Decomposes under direct sunlight or heating.

The molecules in the crystals are dimers. The compound is monomeric above 100 °C.[6]

Chemical properties

[edit]

Iodine trifluoride dioxide decomposes when heated:

2IO2F3 → 2IOF3 + O2

References

[edit]
  1. ^ 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.
  • ^ "iodine trifluoride dioxide". ChemSrc. Retrieved 24 May 2023.
  • ^ Carter, H. A.; Ruddick, J. N.; Sams, J. R.; Aubke, F. (1 January 1975). "Some reactions of iodine(VII) dioxide trifluoride, IO2F3". Inorganic and Nuclear Chemistry Letters. 11 (1): 29–34. doi:10.1016/0020-1650(75)80142-5. ISSN 0020-1650. Retrieved 24 May 2023.
  • ^ a b Advances in Inorganic Chemistry. Academic Press. 1 November 1983. p. 180. ISBN 978-0-08-057876-7. Retrieved 24 May 2023.
  • ^ Downs, A. J.; Adams, C. J. (4 May 2017). The Chemistry of Chlorine, Bromine, Iodine and Astatine: Pergamon Texts in Inorganic Chemistry, Volume 7. Elsevier. p. 1395. ISBN 978-1-4831-5832-7. Retrieved 24 May 2023.
  • ^ Wiberg, Egon; Wiberg, Nils (2001). Inorganic Chemistry. Academic Press. p. 468. ISBN 978-0-12-352651-9. Retrieved 24 May 2023.

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