Phosphorus trifluoride

Phosphorus trifluoride
Structure and dimensions of phosphorus trifluoride
Structure and dimensions of phosphorus trifluoride
Space-filling model 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
TL-75
Identifiers
3D model (JSmol)
ChEBI
ChemSpider
ECHA InfoCard 100.029.098 Edit this at Wikidata
RTECS number
  • TH3850000
UNII
  • InChI=1S/F3P/c1-4(2)3 checkY
    Key: WKFBZNUBXWCCHG-UHFFFAOYSA-N checkY
  • InChI=1/F3P/c1-4(2)3
    Key: WKFBZNUBXWCCHG-UHFFFAOYAK
  • FP(F)F
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)
Critical point (T, P) −2.05 °C (28.3 °F; 271.1 K); 42.73 standard atmospheres (4,329.6 kPa; 628.0 psi)
slow hydrolysis
Structure
Trigonal pyramidal
1.03 D
Hazards
NFPA 704 (fire diamond)
NFPA 704 four-colored diamondHealth 3: Short exposure could cause serious temporary or residual injury. E.g. chlorine gasFlammability 0: Will not burn. E.g. waterInstability 1: Normally stable, but can become unstable at elevated temperatures and pressures. E.g. calciumSpecial hazards (white): no code
3
0
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
Phosphorus trifluoride (data page)
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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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.

  1. ^ Chatt, J. (1950). "The Co-Ordinate Link in Chemistry". Nature. 165 (4199): 637–638. Bibcode:1950Natur.165..637C. doi:10.1038/165637a0. PMID 15416738.