Iodine pentafluoride
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| Iodine pentafluoride | ||
|---|---|---|
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| General | ||
| Systematic name | iodine(V) fluoride | |
| Other names | iodine pentafluoride | |
| Molecular formula | IF5 | |
| SMILES | ? | |
| Molar mass | 221.89 g mol−1 | |
| Appearance | pale yellow liquid | |
| CAS number | [7783-66-6] | |
| Properties | ||
| Density and phase | 3.250 g cm−3 liquid | |
| Solubility in water | ? g/100 ml (?°C) | |
| Melting point | 9.43°C (282.58 K) | |
| Boiling point | 97.85°C (371.00 K) | |
| Acidity (pKa) | ? | |
| Basicity (pKb) | ? | |
| Viscosity | ? cP at ?°C | |
| Structure | ||
| Molecular shape | tetragonal-pyramidal[1] | |
| Coordination geometry |
tetragonal-pyramidal | |
| Crystal structure | monoclinic point group C2/c |
|
| Dipole moment | ? D | |
| Hazards | ||
| MSDS | External MSDS] | |
| Main hazards | toxic, oxidizer, corrosive | |
| NFPA 704 |
0
3
2
OX
|
|
| Flash point | unflamable | |
| R/S statement | R: R8, R14, R23/24/25R35 S: S7/9, S26, S36/37/39, S45 |
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| RTECS number | ? | |
| Supplementary data page | ||
| Structure and properties |
n, εr, etc. | |
| Thermodynamic data |
Phase behaviour Solid, liquid, gas |
|
| Spectral data | UV, IR, NMR, MS | |
| Related compounds | ||
| Related compounds | Iodine heptafluoride, Chlorine pentafluoride, Bromine pentafluoride |
? |
| Except where noted otherwise, data are given for materials in their standard state (at 25°C, 100 kPa) Infobox disclaimer and references |
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Iodine pentafluoride, IF5, is a fluoride of iodine. It is a colourless or yellow liquid with a density of 3250 kg m−3. It was first synthesized by Henri Moissan in 1891 by burning solid iodine in fluorine gas.[2] This exothermic reaction is still used to produce iodine pentafluoride, although the reaction conditions have been improved.[3][4]
I2 + 5 F2 → 2 IF5
[edit] Chemistry
Iodine pentafluoride is a strong fluoridation agent and is highly oxidative. It reacts vigourus with water forming hydrofluoric acid.
Primary amines react with iodine pentafluoride forming nitriles after hydrolysis with water.[5]
R-CH2-NH2 → R-CN
[edit] References
- ^ R. D. Durbank, G. R. Jones (1974). "Crystal structure of iodine pentafluoride at -80.deg.". Inorganic Chemistry 13 (5): 421-439. DOI:10.1021/ic50135a012.
- ^ M. H. Moissan (1891). "Nouvelles Recherches sur le Fluor". Annales de chimie et de physique 6: 224-282.
- ^ Ruff O., Keim R. (1930). ""Das Jod-7-fluorid" (The iodine-7-fluoride)". Zeitschrift für Anorganische un Allgemeine Chemie 193 (1/2): 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)". Zeitschrift für Anorganische un Allgemeine Chemie 201 (1): 245 - 258. DOI:10.1002/zaac.19312010122.
- ^ T. E. Stevens (1966). "Rearrangement of Amides with Iodine Pentafluoride". Journal of Organic Chemistry 31 (6): 2025 - 2026. DOI:10.1021/jo01344a539.
- R. C. Lord, M. A. Lynch, W. C. Schumb, and E. J. Slowinski (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.
- Max T. Rogers, John L. Speirs, H. Bradford Thompson, and Morton B. Panish (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.
- Max T. Rogers, H. Bradford Thompson, and John L. Speirs (1954). "Dielectric Constants of Liquid Chlorine Trifluoride and Iodine Pentafluoride". Journal of the American Chemical Society 76 (19): 4843 - 4844.
- Harold Simmons Booth, John Turner Pinkston, , Jr. (1947). "The Halogen Fluorides.". Chemical Reviews 41 (3): 421-439. DOI:10.1021/cr60130a001.
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