PCl3 is polar because it has a lone pair on the P.
PCl6- is a nonpolar molecule. This is because the molecule has an octahedral geometry with six identical P-Cl bonds arranged symmetrically around the central phosphorus atom. The electronegativity difference between phosphorus and chlorine is not significant enough to create a dipole moment, resulting in a nonpolar molecule.
Phosphorus in PCl6 uses sp3d2 hybrid orbitals, which involve one 3s orbital, three 3p orbitals, and two 3d orbitals. This hybridization allows phosphorus to form six sigma bonds with the six chlorine atoms in PCl6.
The bond angle for PCl6- (hexachlorophosphate ion) is approximately 90 degrees due to its octahedral geometry, where the central phosphorus atom is surrounded by six chlorine atoms.
In the solid state, PCl5 adopts a crystal lattice structure consisting of PCl4+ and PCl6- ions. The PCl4+ ions consist of a central phosphorus atom surrounded by four chlorine atoms, with a distorted tetrahedral geometry. The PCl6- ions consist of a central phosphorus atom surrounded by six chlorine atoms in a trigonal bipyramidal geometry.
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.
PCl6- is a nonpolar molecule. This is because the molecule has an octahedral geometry with six identical P-Cl bonds arranged symmetrically around the central phosphorus atom. The electronegativity difference between phosphorus and chlorine is not significant enough to create a dipole moment, resulting in a nonpolar molecule.
Phosphorus in PCl6 uses sp3d2 hybrid orbitals, which involve one 3s orbital, three 3p orbitals, and two 3d orbitals. This hybridization allows phosphorus to form six sigma bonds with the six chlorine atoms in PCl6.
The bond angle for PCl6- (hexachlorophosphate ion) is approximately 90 degrees due to its octahedral geometry, where the central phosphorus atom is surrounded by six chlorine atoms.
In the solid state, PCl5 adopts a crystal lattice structure consisting of PCl4+ and PCl6- ions. The PCl4+ ions consist of a central phosphorus atom surrounded by four chlorine atoms, with a distorted tetrahedral geometry. The PCl6- ions consist of a central phosphorus atom surrounded by six chlorine atoms in a trigonal bipyramidal geometry.
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.
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 and chlorine form ionic compounds, such as PCl5, due to the large difference in electronegativity between the two atoms. This leads to the transfer of electrons from phosphorus to chlorine, resulting in the formation of ionic bonds.
No its not polar
Polar contains polar. Non-polar contains nothing.
ClO4 is polar.
Nonpolar