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Iodine pentafluoride





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This article is about an interhalogen compound. For the IF5 tornado rating, see International Fujita scale.

Iodine pentafluoride is an interhalogen compound with chemical formula IF5. It is one of the fluoridesofiodine. 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]

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 Edit this at Wikidata
EC Number
  • 232-019-7

PubChem CID
UNII

CompTox Dashboard (EPA)

  • 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

  • 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)

 −58.1·10−6cm3/mol
Viscosity 2.111 mPa·s
Structure

Crystal structure

 Monoclinic
point group C2/c

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 diamondHealth 3: Short exposure could cause serious temporary or residual injury. E.g. chlorine gasFlammability 0: Will not burn. E.g. waterInstability 2: Undergoes violent chemical change at elevated temperatures and pressures, reacts violently with water, or may form explosive mixtures with water. E.g. white phosphorusSpecial hazard W+OX: Reacts with water in an unusual or dangerous manner AND is oxidizer
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

Preparation

edit

It was first synthesized by Henri Moissan in 1891 by burning solid iodineinfluorine 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

edit

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 hexafluoridetoosmium 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

edit
  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.
  • ^ a b http://www.chemadvisor.com/Matheson/database/msds/mat11440000800003.PDF [dead link]
  • ^ Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 978-0-08-037941-8.
  • ^ Moissan, M. H. (1891). "Nouvelles Recherches sur le Fluor". Annales de Chimie et de Physique. 6 (24): 224–282.
  • ^ 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.
  • ^ 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.
  • ^ 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.
  • ^ 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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    Retrieved from "https://en.wikipedia.org/w/index.php?title=Iodine_pentafluoride&oldid=1191133421"
      



    Last edited on 21 December 2023, at 18:29  





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