Iodine pentafluoride

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
Names
Preferred IUPAC name
Iodine(V) fluoride
Systematic IUPAC name
Pentafluoro-λ5-iodane
Other names
Iodic fluoride
Identifiers
CAS Number
3D model (JSmol)
ChemSpider
ECHA InfoCard 100.029.108
EC Number
  • 232-019-7
PubChem CID
UNII
CompTox Dashboard (EPA)
InChI
  • InChI=1S/F5I/c1-6(2,3,4)5 checkY
    Key: PJIYEPACCBMRLZ-UHFFFAOYSA-N checkY
  • InChI=1S/F5I/c1-6(2,3,4)5
    Key: PJIYEPACCBMRLZ-UHFFFAOYSA-N
  • InChI=1/F5I/c1-6(2,3,4)5
    Key: PJIYEPACCBMRLZ-UHFFFAOYAU
SMILES
  • FI(F)(F)(F)F
Properties
Chemical formula
 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)
Solubility in water
 Reacts
Magnetic susceptibility (χ)
 −58.1·10−6 cm3/mol
Viscosity 2.111 mPa·s
Structure
Crystal structure
 Monoclinic
Point group
 C4V
Coordination geometry
 Square pyramidal
Molecular shape
 square pyramidal[1]
Hazards
Occupational safety and health (OHS/OSH):
Main hazards
 Toxic, oxidiser, corrosive, reacts with water to release HF
GHS labelling:
Pictograms
 GHS03: Oxidizing GHS05: Corrosive GHS06: Toxic GHS09: Environmental hazard
Signal word
 Danger
Hazard statements
 H271, H301+H311+H331, H314, H371, H410[2]
Precautionary statements
 P202, P232, P304, P310[2]
NFPA 704 (fire diamond)
NFPA 704 four-colored diamond
3
0
2
W
OX
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).
☒N verify (what is checkY☒N ?)
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. ^ a b http://www.chemadvisor.com/Matheson/database/msds/mat11440000800003.PDF
  3. ^ Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. doi:10.1016/C2009-0-30414-6. 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

  • 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. PMID 18895518.
  • Hetherington, G.; Robinson, P.L. (1956). "The Viscosities of Iodine Pentafluoride and Ditellurium Decafluoride". Journal of the Chemical Society (Resumed): 3681. doi:10.1039/jr9560003674. ISSN 0368-1769.
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