PCl3 is polar because it has a lone pair on the P.
no, it is symetrical
It is a polar molecule because it is asymmetrical and has a negative pole and a positive pole.
its 90
The bonds between phoshorus and chlorine are covalent and polar. Solid PCl5 and PBr5 are ionic, containing polyatomic phosphorus ions PCl4+ PCl6- PBr4+ Br-
sp3d2
ionic, [PCl4]+ [PCl6]-
It is a polar molecule because it is asymmetrical and has a negative pole and a positive pole.
its 90
The bonds between phoshorus and chlorine are covalent and polar. Solid PCl5 and PBr5 are ionic, containing polyatomic phosphorus ions PCl4+ PCl6- PBr4+ Br-
sp3d2
ionic, [PCl4]+ [PCl6]-
electron-pair geometry is octahedral with no LPs and the molecule geometry is octahedral
I believe that it is ionic because PCl5 loses a Cl- ion, and you have two charged parts: PCl4+ and Cl-. wikipedia says PCl4+ PCl6- this is correct- the reason that the molecular form is not favored is probably explained by the substantial "gain" in lattice energy moving to an ionic form from a molecular form with weak intermolecular bonds. Also packing of the PCl5 molecules would be less efficient compared to that of the ionic solid with a mix of 4 and 6 coordinate species.
PCl5 is covalent in the vapour phase with a trigonal biyramidal shape. It is ionic in the solid consisting of PCl4+ PCl6- In solution it can be covalent or ionic depending on the solvent.
In the solid PCl5 is ionic PCl4+ PCl6- In the gas and liquid phases molecular PCl5 is present which does not have a permanent dipole moment. The intermolecular force is a london dispersion force.
Phosphorus pentachloride in the solid state exists as [PCl4+][PCl6-] so has an ionic lattice enthalpy and stronger intermolecular interaction than PCl3
No its not polar
The structures for the phosphorus chlorides are invariably consistent with VESPER theory. The structure of PCl5 depends on its environment. Gaseous and molten PCl5 is a neutral molecule with trigonal bipyramidal . The hypeRVALENT nature of this species can be explained with three-center four-electron bonding model. This trigonal bipyramidal structure persists in non-polar solvents, such as CS2 and CCl4.In the solid state PCl5 is ionic, formulated PCl4+ PCl6−.