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Phosphorus trifluoride

Phosphorus trifluoride
Structure and dimensions of phosphorus trifluoride
Space-filling model of phosphorus trifluoride
Names
IUPAC names
Phosphorus trifluoride
Phosphorus(III) fluoride
Trifluorophosphane
Trifluoridophosphorus
Other names
Trifluorophosphine
Phosphorous fluoride
Identifiers
7783-55-3 YesY
3D model (Jmol) Interactive image
ChEBI CHEBI:30205 YesY
ChemSpider 56416 YesY
ECHA InfoCard 100.029.098
PubChem 62665
RTECS number TH3850000
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
Flammability code 0: Will not burn. E.g., water Health code 3: Short exposure could cause serious temporary or residual injury. E.g., chlorine gas Reactivity code 1: Normally stable, but can become unstable at elevated temperatures and pressures. E.g., calcium Special hazards (white): no codeNFPA 704 four-colored diamond
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 constantr), 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).
YesY  (what is YesYN ?)
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.


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