Why all $P - F$ bonds in $PF_5$ are not equivalent ?
Updated On: Jul 7, 2022
$PF_5$ has $sp^3d$ hybridisation, out of five $P - F$ bonds three are equatorial which have different lengths
$PF_5$ has $sp^3$ hybridisation, out of five $P - F$ bonds two are equatorial which have different lengths
Out of five $P - F$ bonds two are axial and three equatorial. All five bonds have different bond lengths
$PF_5$ is made up of two types of bonds namely covalent and coordinate, hence are not equivalent
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The Correct Option isA
Solution and Explanation
Structure of $PF _{5}$$PF _{5}$ has three axial bonds and two equitorial bonds and has $sp ^{3} d$ hybridisation $PCl _{5}$ has trigonal bipyramidal structure .
Due to this two $Cl$ atoms lie along axial line and other three $Cl$ atoms lie along the equatorial plane.
Hence $Cl$ atoms which lie along axis have different bond length than that of $Cl$ atoms lying on equatorial plane.
P block elements are those in which the last electron enters any of the three p-orbitals of their respective shells. Since a p-subshell has three degenerate p-orbitals each of which can accommodate two electrons, therefore in all there are six groups of p-block elements.
P block elements are shiny and usually a good conductor of electricity and heat as they have a tendency to lose an electron. You will find some amazing properties of elements in a P-block element like gallium. It’s a metal that can melt in the palm of your hand. Silicon is also one of the most important metalloids of the p-block group as it is an important component of glass.
