Iodine pentafluoride
Stereo structural formula of iodine pentafluoride
Stereo structural formula of iodine pentafluoride
Space-filling model of iodine pentafluoride
Space-filling model of iodine pentafluoride
Preferred IUPAC name
Iodine(V) fluoride
Systematic IUPAC name
Other names
Iodic fluoride
3D model (JSmol)
ECHA InfoCard 100.029.108 Edit this at Wikidata
EC Number
  • 232-019-7
  • InChI=1S/F5I/c1-6(2,3,4)5 checkY
  • InChI=1S/F5I/c1-6(2,3,4)5
  • InChI=1/F5I/c1-6(2,3,4)5
  • FI(F)(F)(F)F
Molar mass 221.89 g/mol
Appearance colorless liquid
Density 3.250 g/cm3
Melting point 9.43 °C (48.97 °F; 282.58 K)
Boiling point 97.85 °C (208.13 °F; 371.00 K)
−58.1·10−6 cm3/mol
Viscosity 2.111 mPa·s
point group C2/c
Square pyramidal
square pyramidal[1]
Occupational safety and health (OHS/OSH):
Main hazards
Toxic, oxidiser, corrosive, reacts with water to release HF
GHS labelling:
GHS03: Oxidizing GHS05: Corrosive GHS06: Toxic GHS09: Environmental hazard
H271, H301+H311+H331, H314, H371, H410[2]
P202, P232, P304, P310[2]
NFPA 704 (fire diamond)
Safety data sheet (SDS) External MSDS
Related compounds
Other anions
Iodine pentoxide
Other cations
Bromine pentafluoride
Related compounds
Iodine monofluoride
Iodine trifluoride
Iodine heptafluoride
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Iodine pentafluoride is an interhalogen compound with chemical formula IF5. It is one of the fluorides of iodine. It is a colorless liquid, although impure samples appear yellow. It is used as a fluorination reagent and even a solvent in specialized syntheses.[3]


It was first synthesized by Henri Moissan in 1891 by burning solid iodine in fluorine gas.[4] This exothermic reaction is still used to produce iodine pentafluoride, although the reaction conditions have been improved.[5]

I2 + 5 F2 → 2 IF5


IF5 reacts vigorously with water forming hydrofluoric acid and iodic acid:

IF5 + 3 H2O → HIO3 + 5 HF

Upon treatment with fluorine, it converts to iodine heptafluoride:[6]

IF5 + F2 → IF7

It has been used as a solvent for handling metal fluorides. For example, the reduction of osmium hexafluoride to osmium pentafluoride with iodine is conducted in a solution in iodine pentafluoride:[7]

10 OsF6 + I2 → 10 OsF5 + 2 IF5

Primary amines react with iodine pentafluoride forming nitriles after hydrolysis.[8]


  1. ^ Durbank, R. D.; Jones, G. R. (1974). "Crystal structure of Iodine Pentafluoride at -80°". Inorganic Chemistry. 13 (5): 421–439. doi:10.1021/ic50135a012.
  2. ^ a b[dead link]
  3. ^ Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 978-0-08-037941-8.
  4. ^ Moissan, M. H. (1891). "Nouvelles Recherches sur le Fluor". Annales de Chimie et de Physique. 6 (24): 224–282.
  5. ^ Ruff, O.; Keim, R. (1931). "Fluorierung von Verbindungen des Kohlenstoffs (Benzol und Tetrachlormethan mit Jod-5-fluorid, sowie Tetrachlormethan mit Fluor) [Fluoridation of Carbon Compounds (Benzene and Tetrachlormethane with Iodine-5-Fluoride, and Tetrachloromethane with Fluorine)]". Zeitschrift für Anorganische und Allgemeine Chemie (in German). 201 (1): 245–258. doi:10.1002/zaac.19312010122.
  6. ^ Ruff, O.; Keim, R. (1930). "Das Jod-7-fluorid [The iodine-7-fluoride]". Zeitschrift für anorganische und allgemeine Chemie (in German). 193 (1): 176–186. doi:10.1002/zaac.19301930117.
  7. ^ Holloway, John H.; Mitchell, S. J. (1971). "Preparation and Crystal Structure of Osmium Pentafluoride". Journal of the Chemical Society: 2789–94. doi:10.1039/J19710002789.
  8. ^ Stevens, T. E. (1966). "Rearrangement of Amides with Iodine Pentafluoride". Journal of Organic Chemistry. 31 (6): 2025–2026. doi:10.1021/jo01344a539.

Further reading