Iodine pentafluoride

Iodine pentafluoride
Names
Preferred IUPAC name
Iodine(V) fluoride
Systematic IUPAC name
Pentafluoro-λ5-iodane
Other names
Iodic fluoride
Identifiers
3D model (JSmol)
ChemSpider
ECHA InfoCard 100.029.108
EC Number 232-019-7
Properties
IF5
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)
Reacts[1]
−58.1·10−6 cm3/mol
Structure
monoclinic
point group C2/c
square pyramidal
square pyramidal[2]
Hazards
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., waterHealth code 3: Short exposure could cause serious temporary or residual injury. E.g., chlorine gasReactivity code 2: Undergoes violent chemical change at elevated temperatures and pressures, reacts violently with water, or may form explosive mixtures with water. E.g., phosphorusSpecial hazard W: Reacts with water in an unusual or dangerous manner. E.g., cesium, sodiumNFPA 704 four-colored diamond
0
3
2
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

Chemistry

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

IF5 + 3H2O → HIO3 + 5HF

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

R−CH2−NH2 → R−CN

Iodine pentafluoride is available as a "Special Gas" for flooding into the atmosphere of the escape shuttle in the terminal sequence of 1979 film Alien.

References

  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 http://www.chemadvisor.com/Matheson/database/msds/mat11440000800003.PDF
  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

  • Lord, R. C.; Lynch, M. A.; Schumb, W. C.; Slowinski, E. J. (1950). "The Vibrational Spectra and Structures of Iodine Pentafluoride and Heptafluoride". Journal of the American Chemical Society. 72 (1): 522–527. doi:10.1021/ja01157a135.
  • Rogers, M. T.; Speirs, J. L.; Thompson, H. B.; Panish, M. B. (1954). "Iodine Pentafluoride, Freezing and Boiling Point, Heat of Vaporization and Vapor Pressure-Temperature Relations". Journal of the American Chemical Society. 76 (19): 4843–4844. doi:10.1021/ja01648a022.
  • Rogers, M. T.; Thompson, H. B.; Speirs, J. L. (1954). "Dielectric Constants of Liquid Chlorine Trifluoride and Iodine Pentafluoride". Journal of the American Chemical Society. 76 (19): 4841–4843. doi:10.1021/ja01648a021.
  • Booth, H. S.; Pinkston, J. T. Jr. (1947). "The Halogen Fluorides". Chemical Reviews. 41 (3): 421–439. doi:10.1021/cr60130a001.
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