Question

According to valence bond theory, which kind of orbitals overlap to form the p−cl bonds in pcl5?

Answer 1

According to the valence bond theory, the orbitals that overlap to form the P-Cl bonds in PCl5 are d, s, and p. The hybridization is dsp³. There are five overlaps that occur but the two bonds are longer than the rest which are the axial bonds.

Answer 2

Answer:

$sp^{3} d$ orbital.

Explanation:

Valence bond theory is the chemical bonding theory which explains the chemical bond between two atoms. Both of the two atoms shares each of the unpaired electron to form a hybrid orbital and together to form a bond.

According to the valence bond theory, P-Cl bond forms by the overlap of a phosphorus $sp^{3} d$ orbital with chlorine 3p orbital to form five sigma bond (P-Cl). The five $sp^{3} d$ orbital are single occupied. $PCl_{5}$ has a trigonal bipyramidal structure, and the bond angle is 90 and 120 degree. The original atomic orbital are no longer exist.