Phosphorus halides

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There are three series of binary phosphorus halides, containing phosphorus in the oxidation states +5, +3 and +2. All twelve compounds have been described, in varying degrees of detail, although serious doubts have been cast on the existence of PI5. (1)

Contents

[edit] Oxidation state +5 (PX5)

Chemical formula CAS number Melting point Boiling point P–Xax bond length P–Xeq bond length Xax–P–Xeq bond angle Xax–P–Xax bond angle
PF5 [7647-19-0] -93.7°C -84.5°C 153 pm 158 pm 120° 90°
PCl5 [10026-13-8] 167°C 160°C        
PBr5 [7789-69-7] ~106°C d          
PI5   See Note 1.

Phosphorus pentafluoride is a relatively inert gas, notable as a mild Lewis acid and a fluoride ion acceptor. It is fluxional molecule. Phosphorus pentachloride and phosphorus pentabromide are ionic in the solid and liquid states, and are best described as PX4+PX6–. They are widely used as chlorinating and brominating agents in organic chemistry.

[edit] Oxidation state +3 (PX3)

Chemical formula CAS number Melting point Boiling point P–X bond length X–P–X bond angle Dipole moment
PF3 [7783-55-3] -151.5°C -101.8°C 156 pm 96.3° 1.03 D
PCl3 [7719-12-2] -93.6°C 76.1°C 204 pm 100° 0.56 D
PBr3 [7789-60-8] -41.5°C 173.2°C 222 pm 101°  
PI3 [13455-01-1] 61.2°C 227°C 243 pm 102°  

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-Vollhard-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.

[edit] Oxidation state +2 (P2X4)

Chemical formula CAS number Melting point Boiling point P–X bond length P–P bond length X–P–X bond angle X–P–P bond angle
P2F4 [13824-74-3] -86.5°C -6.2°C 159 pm 228 pm 99.1° 98.4°
P2Cl4 [13467-91-1] -28°C ~180°C d        
P2Br4 [24896-99-3] poorly characterized
P2I4 [13455-00-0] 125.5°C d 248 pm 221 pm 102.3° 94.0°

Phosphorus(II) halides may be prepared by passing an electric discharge through a mixture of the trihalide vapour and hydrogen gas. They are of purely academic interest at the present time. Diphosphorus tetrabromide is particularly poorly described.

[edit] Oxyhalides and thiohalides

Chemical formula CAS number EINECS number Melting point Boiling point Density Refractive index Dipole moment
POF3  ?  ? −39.1°C −39.7°C  ?  ?  ?
POCl3 [10025-87-3] 233-046-7 1.2°C 105.1°C 1.675 g/cm3 1.461 2.54 D
POBr3 [7785-59-5] 232-177-7 56°C 192°C 2.82 g/cm3  ?  ?
POI3  ?  ? 53°C –  ?  ?  ?
PSF3  ?  ? −148.8°C −52.2°C  ?  ?  ?
PSCl3 [3982-91-0] 223-622-6 -35°C 125°C 1.668 g/cm3 1.555  ?
PSBr3  ?  ? 37.8°C 212°C decomp  ?  ?  ?
PSI3  ?  ? 48°C decomp  ?  ?  ?

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 solvant. 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.

[edit] See also

[edit] References


[edit] Notes

  1. I. Tournieporth & T. Klapötke, J. Chem. Soc., Chem. Commun. 1990, 132.
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