Phosphorus halide

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In chemistry, there are three series of binary phosphorus halides, containing phosphorus in the oxidation states +5, +3 and +2. All compounds have been described, in varying degrees of detail, although serious doubts have been cast on the existence of PI5. [1] Mixed chalcogen halides also exist.

Contents

Oxidation state +5

Chemical formula CAS number Melting point Boiling point P–Xax bond length P–Xeq bond lengthXeq–P–Xeq bond angle Xax–P–Xeq bond angle
PF5 [7647-19-0]-93.7°C-84.5°C153 pm158 pm120°90°
PCl5 [10026-13-8]160°C167°C214 pm202 pm120°90°
PBr5 [7789-69-7]~106°C d     
PBr7 [14337-11-2]      
PI5  See Tornieporth-Getting & Klapötke 1990

In the gas phase the phosphorus pentahalides have a trigonal bipyramidal molecular geometry as explained by VSEPR theory. Phosphorus pentafluoride is a relatively inert gas, notable as a mild Lewis acid and a fluoride ion acceptor. It is a fluxional molecule in which the axial (ax) and equatorial (eq) fluorine atoms interchange positions by the Berry pseudorotation mechanism. Phosphorus pentachloride, pentabromide and heptabromide are ionic in the solid and liquid states; PCl5 is formulated as PCl+4PCl−6, but in contrast, PBr5 is formulated as PBr+4Br−, and PBr7 is formulated as PBr+4Br−3 with the tribromide ion. They are widely used as chlorinating and brominating agents in organic chemistry.

Oxidation state +3

Chemical formula CAS number Melting point Boiling point P–X bond lengthX–P–X bond angle Dipole moment
PF3 [7783-55-3]-151.5°C-101.8°C156 pm96.3°1.03 D
PCl3 [7719-12-2]-93.6°C76.1°C204 pm100°0.56 D
Br3 [7789-60-8]-41.5°C173.2°C222 pm101° 
PI3 [13455-01-1]61.2°C227°C243 pm102° 
P(CN)3 (pseudo-halide)203°C179 pm

The phosphorus(III) halides are the best known of the three series. They are usually prepared by direct reaction of the elements, or by transhalogenation. Phosphorus trifluoride is used as a ligand in coordination chemistry, where it resembles carbon monoxide. Phosphorus trichloride is a major industrial chemical and widely used starting material for phosphorus chemistry. Phosphorus tribromide is used in organic chemistry to convert alcohols to alkyl bromides and carboxylic acids to acyl bromides (e.g. in the Hell-Volhard-Zelinsky reaction). Phosphorus triiodide also finds use in organic chemistry, as a mild oxygen acceptor. The trihalides are fairly readily oxidized by chalcogens to give the corresponding oxyhalides or equivalents.

Oxidation state +2

Chemical formula CAS number Melting point Boiling point P–X bond lengthP–P bond lengthX–P–X bond angleX–P–P bond angle
P2F4 [13824-74-3]-86.5°C-6.2°C159 pm228 pm99.1°98.4°
P2Cl4 [13467-91-1]-28°C~180°C d    
P2Br4 [24856-99-3]poorly characterized
P2I4 [13455-00-0]125.5°Cd248 pm221 pm102.3°94.0°

Phosphorus(II) halides may be prepared by passing an electric discharge through a mixture of the trihalide vapour and hydrogen gas.[ citation needed ] The relatively stable diphosphorus tetraiodide is known to have a trans, bent configuration similar to hydrazine and finds some uses in organic syntheses, the others are of purely academic interest at the present time. Diphosphorus tetrabromide is particularly poorly described. They are subhalides of phosphorus.

Oxyhalides, thiohalides and selenohalides

Chemical formula CAS number EINECS number Melting point Boiling point Density Refractive index Dipole moment
POF3 [13478-20-1] ?−39.1°C−39.7°C0,003596 g/cm3 ? ?
POCl3 [10025-87-3]233-046-71.2°C105.1°C1.675 g/cm31.4612.54 D
POBr3 [7785-59-5]232-177-756°C192°C2.82 g/cm3 ? ?
P2O3Cl4 [13498-14-1] ?66–68 °C (0.01 Torr)1.74 g/cm3 ? ?
PSF3 [2404-52-6] ?−148.8°C−52.2°C1.56 g/cm3(l)1.353 ?
PSCl3 [3982-91-0]223-622-6-35°C125°C1.668 g/cm31.555 ?
PSBr3 [3931-89-3] ?37.8°C212°C decomp ? ? ?
PSI3 [63972-04-3] ?48°Cdecomp ? ? ?

The oxyhalides may be prepared from the corresponding trihalides by reaction with organic peroxides or ozone: they are sometimes referred to as phosphoryl halides. The thiohalides, also known as thiophosphoryl halides may be prepared from the trihalides by reaction with elemental sulfur in an inert solvent. The corresponding selenohalides are also known. The oxyhalides and thiohalides are significantly more electrophilic than the corresponding phosphorus(III) species, and present a significant toxic hazard. Selenophosphoryl fluoride is unstable at room temperature, decomposing to PF3 and Se. [2]

References

  1. ↑ I. Tornieporth-Getting & T. Klapötke, J. Chem. Soc., Chem. Commun.1990, 132. doi:10.1039/C39900000132
  2. ↑ Hagen, Arnulf P.; Elphingstone, Eugene A. (February 1973). "High pressure interaction of phosphorus trifluoride with oxygen, sulfur, selenium, and tellurium". Inorganic Chemistry. 12 (2): 478–480. doi:10.1021/ic50120a050.
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