Phosphorus trifluoride
| Phosphorus trifluoride | |
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Phosphorus trifluoride |
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Other names
Trifluorophosphine |
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| Identifiers | |
| CAS number | 7783-55-3  |
| PubChem | 62665 |
| ChemSpider | 56416 |
| ChEBI | CHEBI:30205 |
| RTECS number | TH3850000 |
| Jmol-3D images | Image 1 |
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| Properties | |
| Molecular formula | PF3 |
| Molar mass | 87.968971 g/mol |
| Appearance | colorless gas |
| Density | 3.91 g/L, gas |
| Melting point |
-151.5 °C, 122 K, -241 °F |
| Boiling point |
-101.8 °C, 171 K, -151 °F |
| Solubility in water | slow hydrolysis |
| Structure | |
| Molecular shape | Trigonal pyramidal |
| Dipole moment | 1.03 D |
| Hazards | |
| MSDS | External MSDS |
| EU Index | Not listed |
| NFPA 704 |
 0
3
1
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| Flash point | Non-flammable |
| Related compounds | |
| Other anions | Phosphorus trichloride Phosphorus tribromide Phosphorus triiodide |
| Other cations | Nitrogen trifluoride Arsenic trifluoride Antimony trifluoride Bismuth trifluoride |
| Related ligands | Carbon monoxide |
| Related compounds | Phosphorus pentafluoride |
| Supplementary data page | |
| Structure and properties |
n, εr, etc. |
| Thermodynamic data |
Phase behaviour Solid, liquid, gas |
| Spectral data | UV, IR, NMR, MS |
 (verify) (what is:  / ?)Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa) |
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| Infobox references | |
Phosphorus trifluoride (formula PF3), is a colorless and odorless gas. It is highly toxic and it reacts slowly with water. Its main use is as a ligand in metal complexes. As a ligand it parallels carbon monoxide in metal carbonyls,[1] and indeed its toxicity is due to its binding with the iron in blood hemoglobin in a similar way to carbon monoxide.
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[edit] Physical properties
Phophorus trifluoride has a bond angle of 107°. Gaseous PF3 has a standard enthalpy of formation of -945 kJ/mol (-226 kcal/mol). The phosphorus atom has an nuclear magnetic resonance chemical shift of 97 ppm (downfield of H3PO4).
[edit] Properties
Phosphorus trifluoride hydrolyzes especially at high pH, but it is less hydrolytically sensitive than phosphorus trichloride. It does not attack glass except at high temperatures, and anhydrous potassium hydroxide may be used to dry it with little loss. With hot metals, phosphides and fluorides are formed. With Lewis bases such as ammonia addition products (adducts) are formed, and PF3 is oxidized by oxidizing agents such as bromine or potassium permanganate.
As a ligand for transition metals, PF3 is a strong π-acceptor.[2] It forms a variety of metal complexes with metals in low oxidation states. PF3 forms several complexes for which the corresponding CO derivatives (see metal carbonyl) are unstable or nonexistent. Thus, Pd(PF3)4 is known, but Pd(CO)4 is not.[3][4][5] Such complexes are usually prepared directly from the related metal carbonyl compound, with loss of CO. However, Nickel metal reacts directly with PF3 at 100 °C under 35 MPa pressure to form Ni(PF3)4, which is analogous to Ni(CO)4. Cr(PF3)6, the analogue of Cr(CO)6, may be prepared from dibenzenechromium:
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[edit] Preparation
Phosphorus trifluoride is usually prepared from phosphorus trichloride via halogen exchange using various fluorides such as hydrogen fluoride, calcium fluoride, arsenic trifluoride, antimony trifluoride, or zinc fluoride:[6][7][8]
[edit] Biological activity
Phosphorus trifluoride is similar to carbon monoxide in that it is a gas which strongly binds to iron in hemoglobin, preventing the blood from absorbing oxygen.
[edit] Precautions
PF3 is highly toxic, comparable to phosgene.[9]
[edit] References
- ^ J. Chatt (1950). "The Co-Ordinate Link in Chemistry". Nature 165 (4199): 637–8. doi:10.1038/165637a0. PMID 15416738.
- ^ N. N. Greenwood, A. Earnshaw, Chemistry of the Elements, 2nd ed., Butterworth-Heinemann, Oxford, UK, 1997, p 494
- ^ D. Nicholls, Complexes and First-Row Transition Elements, Macmillan Press, London, 1973.
- ^ Kruck, T.“Trifluorphosphin-Komplexe von Übergangsmetallen” Angewandte Chemie 1967, volume 79, p 27-43. DOI: 10.1002/ange.19670790104
- ^ Clark, R. J.; Busch, M. A. “Stereochemical studies of metal carbonylphosphorus trifluoride complexes” Accounts of Chemical Research, 1973, volume 6, pages 246-52.DOI: 10.1021/ar50067a005.
- ^ A. A. Williams, in Inorganic Syntheses, Vol. V, 95-7 (1946).
- ^ Nouveau traité de chimie minérale : Tome X, Masson, Paris, France, 1956.
- ^ Ronald J. Clark, Helen Belefant, Stanley M. Williamson (1990). "Phosphorus Trifluoride". Inorganic Syntheses. Inorganic Syntheses 28: 310–315. doi:10.1002/9780470132593.ch77. ISBN 9780470132593.
- ^ Greenwood, 1997
[edit] Further reading
- Handbook of Chemistry and Physics, 71st edition, CRC Press, Ann Arbor, Michigan, 1990.
- J. March, Advanced Organic Chemistry, 4th ed., p. 723, Wiley, New York, 1992.
- The Merck Index, 7th edition, Merck & Co, Rahway, New Jersey, USA, 1960.
- A. D. F. Toy, The Chemistry of Phosphorus, Pergamon Press, Oxford, UK, 1973.
[edit] External links
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