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 |
| ||
PubChem CID
|
|||
CompTox Dashboard (EPA)
|
|||
| |||
| |||
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 | |||
Occupational safety and health (OHS/OSH): | |||
Main hazards
|
Toxic, oxidizing, corrosive. | ||
GHS labelling: | |||
![]() ![]() ![]() ![]() | |||
Danger | |||
H271, H301, H311, H314, H330, H371, H410[3] | |||
P202, P232, P304, P310[3] | |||
NFPA 704 (fire diamond) | |||
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).
|
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
Popular culture
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
- ^ Patnaik, P. (2002). Handbook of Inorganic Chemicals. McGraw-Hill. ISBN 0-07-049439-8.
- ^ 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
- ^ Moissan, M. H. (1891). "Nouvelles Recherches sur le Fluor". Annales de Chimie et de Physique. 6 (24): 224–282.
- ^ 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.
- ^ 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.
- ^ 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.