Chapter 8, Problem 109A

Interpretation Introduction

Interpretation:

The theory of the hybridization and the number of hybrid orbital in ${\text{PCl}}_{\text{5}}$ is to be stated.

Concept introduction:

The combination of two things that have both the characteristic is termed as a hybrid. The process of mixing of atomic orbitals of different energy to form identical hybrid orbitals of equal energy is termed as hybridization.

Answer to Problem 109A

The theory of hybridization explains the shape of the molecule. The hybridization of ${\text{PCl}}_{\text{5}}$ is $s{p}^{3}d$. Therefore, the number of hybrid orbital in ${\text{PCl}}_{\text{5}}$ is five.

Explanation of Solution

In the molecule, the atomic orbitals of atoms undergo hybridization to form identical hybrid orbitals which explains the shape of the molecule.

The given compound is ${\text{PCl}}_{\text{5}}$. The atomic number of phosphorous is 15 with electronic configuration $1s^{2}2s^{2}2p^{6}3s^{2}3p^3$. The hybridization in ${\text{PCl}}_{\text{5}}$ is shown below.

The atomic number of chlorine is 17 with electronic configuration $\left[\text{Ne}\right]3s^{2}3p^5$. Here, $3p$ orbital of chlorine (Cl) overlaps with five $s{p}^{3}d$ hybrid orbitals to form five $\text{P}-\text{Cl}$ sigma bonds.

The geometry of ${\text{PCl}}_{\text{5}}$ is shown below.

Conclusion

The number of hybrid orbital in ${\text{PCl}}_{\text{5}}$ is five.