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Phosphorous trihalides

Phosphorous trihalides, PX 3 , are produced from the direct reaction of phosphorous with the appropriate halogen, [link] . The fluoride is readily made from the halide exchange reaction of PCl 3 with fluoride salts, [link] . Mixed trihalides are formed by halide exchange, [link] .

A summary of the physical properties of the phosphorous trihalides is given in [link] . All the compounds have a pyramidal structure in the vapor phase and in solution.

Selected physical properties of the phosphorous trihalides.
Compound Mp (°C) Bp (°C) P-X (Å) X-P-X (°)
PF 3 -151.5 -101.8 1.56 96.3
PCl 3 -93.6 76.1 2.04 100
PBr 3 -41.5 173.2 2.22 101
PI 3 61.2 200 (dec.) 2.43 102

The phosphorous trihalides hydrolyze to phosphoric acid, [link] , and undergo alcoholysis to form the trialkyl phosphite derivative, [link] . Phosphorous trifluoride is only slowly hydrolyzed by water, but reacts readily with alakaline solutions. In contrast, phosphorus triiodide is an unstable red solid that reacts violently with water. Phosphorous trichloride in particular is an excellent synthon for most trialkyl phosphines, [link] .

As with other P(III) compounds such as trialkyl phosphines, phosphorous trihalides can be oxidized to the analogous phosphene oxide, e.g., [link] .

Phosphorous trihalides form Lewis acid-base complexes with main group metals, but the bonding to d n (n ≠ 0) transition metals occurs in the same manner to that of trialkyl phosphine, i.e., with dπ-pπ back donation. In fact one of the first examples of complexation of phosphorous to a low oxidation metal was the formation of PF 3 complexes with Fe-porphyrin.

Phosphorous pentahalides

The reaction of white phosphorous with excess halogen yields the pentahalides, [link] . However, the pentafluoride is best prepared by halide exchange, [link] .

The pentaiodide is unknown, however, selected physical properties are given for the others in [link] .

Selected physical properties of phosphorous pentahalides.
Compound Mp (°C) Bp (°C)
PF 5 -93.78 -84.5
PCl 5 166.8 160 (subl.)
PBr 5 100 106.0

The structures of the phosphorous pentahalides are all trigonal bipyramidal in the gas phase ( [link] ). Phosphorous pentafluoride maintains the trigonal bipyramidal structure in solid state, but the chloride and bromide are ionic solids, [PCl 4 ] + [PCl 6 ] - and [PBr 4 ]Br ( [link] ), respectively. The tetrahedral [PCl 4 ] + ion is also formed with the reaction of PCl 5 with other chloride ion acceptors, [link] and [link] .

The structures of (a) PF 5 and (b) PCl 5 .
The crystal structure of phosphorous pentabromide.

All of the pentahalides undergo thermal decomposition, [link] .

Careful hydrolysis of the pentahalides yields the oxide of the appropriate trihalide, [link] , while excess hydrolysis yields phosphoric acid, [link] .

Questions & Answers

find the 15th term of the geometric sequince whose first is 18 and last term of 387
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salma
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ninjadapaul
20/(×-6^2)
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The answer is neither. The function, 2 = 0 cannot exist. Hence, the function is undefined.
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I start with an easy one. carbon nanotubes woven into a long filament like a string
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In this morden time nanotechnology used in many field . 1-Electronics-manufacturad IC ,RAM,MRAM,solar panel etc 2-Helth and Medical-Nanomedicine,Drug Dilivery for cancer treatment etc 3- Atomobile -MEMS, Coating on car etc. and may other field for details you can check at Google
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At high concentrations (>0.01 M), the relation between absorptivity coefficient and absorbance is no longer linear. This is due to the electrostatic interactions between the quantum dots in close proximity. If the concentration of the solution is high, another effect that is seen is the scattering of light from the large number of quantum dots. This assumption only works at low concentrations of the analyte. Presence of stray light.
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the Beer law works very well for dilute solutions but fails for very high concentrations. why?
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Source:  OpenStax, Chemistry of the main group elements. OpenStax CNX. Aug 20, 2010 Download for free at http://cnx.org/content/col11124/1.25
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