SF6 does not have symmetrical geometry, while PF5 does. This is because SF6 has a trigonal bipyramidal molecular geometry, with six bonding pairs and no lone pairs, leading to an overall asymmetrical shape. In contrast, PF5 has a trigonal bipyramidal molecular geometry with five bonding pairs and one lone pair, resulting in a symmetrical shape due to the lone pair occupying one of the equatorial positions.
it shows tetrahedral geometry for the electron pairs geometry and trigonal pyramid the molecular geometry.
No, PF5 is not a dipole-dipole molecule. It has a trigonal bipyramidal geometry with fluorine atoms arranged symmetrically around the central phosphorus atom, resulting in a nonpolar molecule.
3 bonding pairs between P and 3x F atoms.1 free pair at central P atom.3 free pairs on each of the F atoms.Cf in 'Related links' below this answer page
sp3d2 hybridization. Example: sulfur hexafluoride (SF6)
Iit is phosphorus penta fluoride a molecule with Trigonal bipyramidal geometry.
The electron geometry (and also, the molecular geometry) of PF5 is Trigonal Bipyramidal.
Trigonal Bipyramidal
trigonal planar
The neutral SF6 molecule has no dipole moment. The gas phase SF6- ion is not that well understood- on the basis that the shape is distorted octahedral a small dipole would be expected.
it shows tetrahedral geometry for the electron pairs geometry and trigonal pyramid the molecular geometry.
No, PF5 is not a dipole-dipole molecule. It has a trigonal bipyramidal geometry with fluorine atoms arranged symmetrically around the central phosphorus atom, resulting in a nonpolar molecule.
It is symmetrical
The different types of symmetry in geometry are symmetrical and asymmetrical.
3 bonding pairs between P and 3x F atoms.1 free pair at central P atom.3 free pairs on each of the F atoms.Cf in 'Related links' below this answer page
sp3d2 hybridization. Example: sulfur hexafluoride (SF6)
Nonpolar Why: Fluorine is more electronegative than sulfur, so the bond dipoles point toward fluorine. The six S-F bonds are arranged octahedrally around the central sulfur. F F \ / F-S-F / \ F F Because the octahedral geometry is symmetrical, the bond dipoles cancel, and the molecule is nonpolar, meaning that µ = 0. Source: Straight from Chemistry: The Central Science. 11e. Brown/LeMay/Bursten/Murphy
Iit is phosphorus penta fluoride a molecule with Trigonal bipyramidal geometry.