Chemistry:Iodine pentafluoride

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Iodine pentafluoride
Stereo structural formula of iodine pentafluoride
Space-filling model of iodine pentafluoride
Names
Preferred IUPAC name
Iodine(V) fluoride
Systematic IUPAC name
Pentafluoro-λ5-iodane
Other names
Iodic fluoride
Identifiers
3D model (JSmol)
ChemSpider
EC Number
  • 232-019-7
UNII
Properties
IF5
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)
Reacts
−58.1·10−6 cm3/mol
Viscosity 2.111 mPa·s
Structure
Monoclinic
point group C2/c
Square pyramidal
square pyramidal[1]
Hazards
Main hazards Toxic, oxidiser, corrosive, reacts with water to release HF
Safety data sheet External MSDS
GHS pictograms GHS03: Oxidizing GHS05: Corrosive GHS06: Toxic GHS09: Environmental hazard
GHS Signal word Danger
H271, H301+311+331Script error: No such module "Preview warning".Category:GHS errors, H314, H371, H410[2]
P202, P232, P304, P310[2]
NFPA 704 (fire 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 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]

Preparation

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

Reactions

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]

References

  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. 2.0 2.1 http://www.chemadvisor.com/Matheson/database/msds/mat11440000800003.PDF
  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. http://gallica.bnf.fr/ark:/12148/bpt6k34894x/f222.tableDesMatieres. 
  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)]" (in German). Zeitschrift für Anorganische und Allgemeine Chemie 201 (1): 245–258. doi:10.1002/zaac.19312010122. 
  6. Ruff, O.; Keim, R. (1930). "Das Jod-7-fluorid [The iodine-7-fluoride]" (in German). Zeitschrift für anorganische und allgemeine Chemie 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

External links