Phosphorus trifluoride

Phosphorus trifluoride (formula PF3), is a colorless and odorless gas. It is highly toxic and 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.

Phosphorus trifluoride
Structure and dimensions of phosphorus trifluoride
Space-filling model of phosphorus trifluoride
Names
IUPAC names
Phosphorus trifluoride
Phosphorus(III) fluoride
Trifluorophosphane
Trifluoridophosphorus
Perfluorophosphane
Other names
Trifluorophosphine
Phosphorous fluoride
Identifiers
3D model (JSmol)
ChEBI
ChemSpider
ECHA InfoCard 100.029.098
RTECS number
  • TH3850000
UNII
Properties
PF3
Molar mass 87.968971 g/mol
Appearance colorless gas
Density 3.91 g/L, gas
Melting point −151.5 °C (−240.7 °F; 121.6 K)
Boiling point −101.8 °C (−151.2 °F; 171.3 K)
slow hydrolysis
Structure
Trigonal pyramidal
1.03 D
Hazards
Safety data sheet See: data page
NFPA 704 (fire diamond)
Flammability code 0: Will not burn. E.g. waterHealth code 3: Short exposure could cause serious temporary or residual injury. E.g. chlorine gasReactivity code 1: Normally stable, but can become unstable at elevated temperatures and pressures. E.g. calciumSpecial hazards (white): no code
0
3
1
Flash point Non-flammable
Related compounds
Other anions
 Phosphorus trichloride
Phosphorus tribromide
Phosphorus triiodide
Phosphane
Other cations
 Nitrogen trifluoride
Arsenic trifluoride
Antimony trifluoride
Bismuth trifluoride
Related ligands
 Carbon monoxide
Related compounds
 Phosphorus pentafluoride
Supplementary data page
Refractive index (n),
Dielectric constant (εr), etc.
Thermodynamic
data
 Phase behaviour
solid–liquid–gas
UV, IR, NMR, MS
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Infobox references

Physical properties

Phosphorus trifluoride has an F−P−F bond angle of approximately 96.3°. Gaseous PF3 has a standard enthalpy of formation of −945 kJ/mol (−226 kcal/mol). The phosphorus atom has a nuclear magnetic resonance chemical shift of 97 ppm (downfield of H3PO4).

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:

Cr(C6H6)2 + 6 PF3 → Cr(PF3)6 + 2 C6H6
Ball-and-stick model of [Pt(PF3)4]
Space-filling model of [Pt(PF3)4]

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]

2 PCl3 + 3 ZnF2 → 2 PF3 + 3 ZnCl2

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.

Precautions

PF3 is highly toxic, comparable to phosgene.[9]

gollark: People are not idiots, and realized that that could be an issue, so there's work on designing asymmetric encryption schemes (symmetric is mostly safe as far as I know, except for Grover's algorithm) which cannot be broken by quantum computing.
gollark: Which breaks RSA and elliptic curve stuff.
gollark: Quantum computers *cannot* do anything ever a trillion times faster, or something ridiculous like that; they can accelerate some algorithms, for example factoring integers fast and something something discrete logarithm problem.
gollark: There are post-quantum schemes already, they're just annoying and not standardized yet.
gollark: What? No.

References
  1. Chatt, J. (1950). "The Co-Ordinate Link in Chemistry". Nature. 165 (4199): 637–638. doi:10.1038/165637a0. PMID 15416738.
  2. Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. p. 494. ISBN 978-0-08-037941-8.
  3. Nicholls, D. (1973). Complexes and First-Row Transition Elements. London: Macmillan Press.
  4. Kruck, T. (1967). "Trifluorphosphin-Komplexe von Übergangsmetallen". Angewandte Chemie. 79 (1): 27–43. doi:10.1002/ange.19670790104.
  5. Clark, R. J.; Busch, M. A. (1973). "Stereochemical Studies of Metal Carbonyl-Phosphorus Trifluoride Complexes". Accounts of Chemical Research. 6 (7): 246–252. doi:10.1021/ar50067a005.
  6. Williams, A. A.; Parry, R. W.; Dess, H. (1957). "Phosphorus(III) Fluoride". Inorganic Syntheses. 5: 95–97. doi:10.1002/9780470132364.ch26.
  7. Dubrisay, R. (1956). Pascal, P. (ed.). Azote-Phosphore. Nouveau Traité de Chimie Minérale. 10. Paris, France: Masson. ISBN 978-2-225-57123-7.
  8. Clark, R. J.; Belefant, H.; Williamson, S. M. (1990). "Phosphorus Trifluoride". Inorganic Syntheses. 28: 310–315. doi:10.1002/9780470132593.ch77. ISBN 978-0-470-13259-3.
  9. Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 978-0-08-037941-8.

Further reading
  • Toy, A. D. F. (1973). The Chemistry of Phosphorus. Oxford, UK: Pergamon Press.
  • Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 978-0-08-037941-8.
  • Lide, D. R., ed. (1990). Handbook of Chemistry and Physics (71st ed.). Ann Arbor, MI: CRC Press. ISBN 978-0-8493-0471-2.
  • March, J. (1992). Advanced Organic Chemistry (4th ed.). New York: Wiley. p. 723. ISBN 978-0-471-60180-7.
  • Stecher, P. G., ed. (1960). The Merck Index (7th ed.). Rahway, NJ, USA: Merck & Co.
  • Holmes, R. R. (1960). "An Examination of the Basic Nature of the Trihalides of Phosphorus, Arsenic and Antimony". Journal of Inorganic and Nuclear Chemistry. 12 (3–4): 266–275. doi:10.1016/0022-1902(60)80372-7.
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