Iodine pentafluoride

Iodine pentafluoride
Preferred IUPAC name
Iodine(V) fluoride
Systematic IUPAC name
Other names
Iodic fluoride
7783-66-6 N
3D model (Jmol) Interactive image
ChemSpider 455940 YesY
ECHA InfoCard 100.029.108
EC Number 232-019-7
PubChem 522683
Molar mass 221.89 g/mol
Appearance colorless or pale yellow 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)
point group C2/c
square pyramidal
square pyramidal[2]
Main hazards Toxic, oxidizing, corrosive.
Safety data sheet External MSDS
GHS pictograms
GHS signal word Danger
H271, H330, H311, H301, H314, H371, H410[3]
P202, P232, P304, P310[3]
NFPA 704
Flammability code 0: Will not burn. E.g., water Health code 3: Short exposure could cause serious temporary or residual injury. E.g., chlorine gas Reactivity code 2: Undergoes violent chemical change at elevated temperatures and pressures, reacts violently with water, or may form explosive mixtures with water. E.g., phosphorus Special hazard W: Reacts with water in an unusual or dangerous manner. E.g., cesium, sodiumNFPA 704 four-colored diamond
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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Infobox references

Iodine pentafluoride is an interhalogen compound with chemical formula IF5. It is a fluoride of iodine. It is a colorless or yellow liquid with a density of 3.250 g cm−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][6]

I2 + 5 F2 → 2 IF5


Iodine pentafluoride is a strong fluorination agent and is highly oxidative. It reacts vigorously with water forming hydrofluoric acid and with more fluorine forming iodine heptafluoride.

Primary amines react with iodine pentafluoride forming nitriles after hydrolysis with water.[7]

R-CH2-NH2 → R-CN


  1. Patnaik, P. (2002). Handbook of Inorganic Chemicals. McGraw-Hill. ISBN 0-07-049439-8.
  2. Durbank, R. D.; Jones, G. R. (1974). "Crystal structure of Iodine Pentafluoride at -80° ". Inorganic Chemistry. 13 (5): 421–439. doi:10.1021/ic50135a012.
  3. 1 2
  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. (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.
  6. 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.
  7. Stevens, T. E. (1966). "Rearrangement of Amides with Iodine Pentafluoride". Journal of Organic Chemistry. 31 (6): 2025–2026. doi:10.1021/jo01344a539.

Further reading

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