Chemistry:Phosphorus pentafluoride
| |
| |
| Names | |
|---|---|
| IUPAC name
Phosphorus pentafluoride
| |
| Other names
Phosphorus(V) fluoride
Pentafluoridophosphorus Pentafluorophosphorane | |
| Identifiers | |
3D model (JSmol)
|
|
| ChemSpider | |
| EC Number |
|
PubChem CID
|
|
| RTECS number |
|
| UNII | |
| UN number | 2198 |
| |
| |
| Properties | |
| PF5 | |
| Molar mass | 125.965777813 g·mol−1 |
| Appearance | colourless gas |
| Odor | unpleasant |
| Density | 5.527 kg/m3 |
| Melting point | −93.78 °C (−136.80 °F; 179.37 K) |
| Boiling point | −84.6 °C (−120.3 °F; 188.6 K) |
| hydrolysis | |
| Structure | |
| trigonal bipyramidal | |
| 0 D | |
| Hazards | |
| Flash point | Non-flammable |
| Related compounds | |
Other anions
|
Phosphorus pentachloride Phosphorus pentabromide Phosphorus pentaiodide |
Other cations
|
Arsenic pentafluoride Antimony pentafluoride Bismuth pentafluoride |
Related compounds
|
Phosphorus trifluoride |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). | |
 verify (what is   ?)
| |
| Infobox references | |
Phosphorus pentafluoride, PF5, is a phosphorus halide. It is a colourless, toxic gas that fumes in air.[1][2]
Preparation
Phosphorus pentafluoride was first prepared in 1876 by the fluorination of phosphorus pentachloride using arsenic trifluoride, which remains a favored method:[1]
- 3 PCl5 + 5 AsF3 → 3 PF5 + 5 AsCl3
Phosphorus pentafluoride can be prepared by direct combination of phosphorus and fluorine:
- P4 + 10 F2 → 4 PF5
Structure
Single-crystal X-ray studies indicate that the PF5 has trigonal bipyramidal geometry. Thus it has two distinct types of P−F bonds (axial and equatorial): the length of an axial P−F bond is distinct from the equatorial P−F bond in the solid phase, but not the liquid or gas phases due to Berry pseudo rotation.
Fluorine-19 NMR spectroscopy, even at temperatures as low as −100 °C, fails to distinguish the axial from the equatorial fluorine environments. The apparent equivalency arises from the low barrier for pseudorotation via the Berry mechanism, by which the axial and equatorial fluorine atoms rapidly exchange positions. The apparent equivalency of the F centers in PF5 was first noted by Gutowsky.[3] The explanation was first described by R. Stephen Berry, after whom the Berry mechanism is named. Berry pseudorotation influences the 19F NMR spectrum of PF5 since NMR spectroscopy operates on a millisecond timescale. Electron diffraction and X-ray crystallography do not detect this effect as the solid state structures are, relative to a molecule in solution, static and can not undergo the necessary changes in atomic position.
Lewis acidity
Phosphorus pentafluoride is a Lewis acid. This property is relevant to its ready hydrolysis. A well studied adduct is PF5 with pyridine. With primary and secondary amines, the adducts convert readily to dimeric amido-bridged derivatives with the formula [PF4(NR2)]2. A variety of complexes are known with bidentate ligands.[4]
Hexafluorophosphoric acid (HPF6) is derived from phosphorus pentafluoride and hydrogen fluoride. Its conjugate base, hexafluorophosphate (PF6–), is a useful non-coordinating anion. It is often used in lithium-ion batteries, where besides providing good ionic conductivity for the liquid electrolyte, it also passivates positive aluminium current collector.
References
- ↑ 1.0 1.1 Kwasnik, W. (1963). "Phosphorus(V) fluoride". in Brauer, G.. Handbook of Preparative Inorganic Chemistry. 1 (2nd ed.). New York: Academic Press. p. 190.
- ↑ Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 978-0-08-037941-8.
- ↑ Gutowsky, H. S.; McCall, D. W.; Slichter, C. P. (1953). "Nuclear Magnetic Resonance Multiplets in Liquids". J. Chem. Phys. 21 (2): 279. doi:10.1063/1.1698874.
- ↑ Wong, Chih Y.; Kennepohl, Dietmar K.; Cavell, Ronald G. (1996). "Neutral Six-Coordinate Phosphorus". Chemical Reviews 96 (6): 1917–1952. doi:10.1021/cr9410880. PMID 11848816.
 |  |
