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Iit is phosphorus penta fluoride a molecule with Trigonal bipyramidal geometry.
it shows tetrahedral geometry for the electron pairs geometry and trigonal pyramid the molecular geometry.
sp3d2 hybridization. Example: sulfur hexafluoride (SF6)
SF6 is non-polar. Reason: Fluorine is more electronegative than sulfur, so the bond dipoles point toward fluorine. However, all 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 each other, and the molecule is nonpolar, meaning that µ = 0. Source: Another Qs from the same topic (SF6 from wikiANSWERS) which quotes the source as: "Straight from Chemistry: The Central Science. 11e. Brown/LeMay/Bursten/Murphy"
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
The electron geometry (and also, the molecular geometry) of PF5 is Trigonal Bipyramidal.
Trigonal Bipyramidal
trigonal planar
The geometry is different and also reactivity. 2F more than on PF3 trigonal bipyramidal PF5 trigonal pyramidal PF3
Iit is phosphorus penta fluoride a molecule with Trigonal bipyramidal geometry.
It is symmetrical
it shows tetrahedral geometry for the electron pairs geometry and trigonal pyramid the molecular geometry.
The different types of symmetry in geometry are symmetrical and asymmetrical.
sp3d2 hybridization. Example: sulfur hexafluoride (SF6)
PF5 :SP3d
Because of its perfect symmetrical shapes as for example the golden rectangle.
SF6 is non-polar. Reason: Fluorine is more electronegative than sulfur, so the bond dipoles point toward fluorine. However, all 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 each other, and the molecule is nonpolar, meaning that µ = 0. Source: Another Qs from the same topic (SF6 from wikiANSWERS) which quotes the source as: "Straight from Chemistry: The Central Science. 11e. Brown/LeMay/Bursten/Murphy"