Phosphorus trifluoride

Phosphorus trifluoride

Names
IUPAC names Phosphorus trifluoride Phosphorus(III) fluoride Trifluorophosphane Trifluoridophosphorus
Other names Trifluorophosphine Phosphorous fluoride
Identifiers
CAS Number	7783-55-3 Y
3D model (Jmol)	Interactive image
ChEBI	CHEBI:30205 Y
ChemSpider	56416 Y
ECHA InfoCard	100.029.098
PubChem	62665
RTECS number	TH3850000
InChI InChI=1S/F3P/c1-4(2)3 Y Key: WKFBZNUBXWCCHG-UHFFFAOYSA-N Y InChI=1/F3P/c1-4(2)3 Key: WKFBZNUBXWCCHG-UHFFFAOYAK
SMILES FP(F)F
Properties
Chemical formula	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)
Solubility in water	slow hydrolysis
Structure
Molecular shape	Trigonal pyramidal
Dipole moment	1.03 D
Hazards
Safety data sheet	See: data page
NFPA 704	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
Structure and properties	Refractive index (n), Dielectric constant (εr), etc.
Thermodynamic data	Phase behaviour solid–liquid–gas
Spectral data	UV, IR, NMR, MS
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
Y  (what is YN ?)
Infobox references

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, and indeed its toxicity is due to its binding with the iron in blood hemoglobin in a similar way to carbon monoxide.

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).

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.