Chapter 8, Problem 129A

Interpretation Introduction

Interpretation:

The Lewis structure of chlorine trifluoride $\left({\text{ClF}}_{\text{3}}\right)$ is to be drawn. The hybridization of chlorine trifluoride $\left({\text{ClF}}_{\text{3}}\right)$ is to be identified.

Concept introduction:

The strategy for drawing Lewis structure is mention below.

• Calculate the number of valence electrons present in the molecule.
• Calculate the electron pairs by dividing number of valence electrons by 2.
• Determine the bond pairs.
• Determine the lone pairs.
• Check whether the central atom satisfies octet rule.

Answer to Problem 129A

The Lewis structure of chlorine trifluoride $\left({\text{ClF}}_{\text{3}}\right)$ is drawn below.

The hybridization of chlorine trifluoride $\left({\text{ClF}}_{\text{3}}\right)$ is $s{p}^{3}d$.

Explanation of Solution

The number of valence electron in chlorine trifluoride is the sum of valence electron in chlorine and fluorine atoms. The valence electron in chlorine and fluorine is seven. Therefore, the valence electron in chlorine trifluoride is calculated as shown below.

$\begin{array}{c}\text{No}\text{.}\text{of}\text{valence}\text{electron}=\text{Cl}+\text{3F}\\ =7{\text{e}}^{-}+3\times 7{\text{e}}^{-}\\ =28{\text{e}}^{-}\end{array}$

The number of electron pair is calculated as shown below.

$\begin{array}{c}\text{electron}\text{pair}=\frac{28{\text{e}}^{-}}{2}\\ =14{\text{e}}^{-}\text{pairs}\end{array}$

Among fourteen electron pairs, three electron pairs are involved in bonding and eleven electron pairs remain as lone pairs. The Lewis structure of chlorine trifluoride is drawn below.

Here, chlorine atom is surrounded by five electron groups (Three F atoms and two lone pairs). Therefore, the hybridization of chlorine atom in chlorine trifluoride $\left({\text{ClF}}_{\text{3}}\right)$ is $s{p}^{3}d$.

Conclusion

The Lewis structure of chlorine trifluoride $\left({\text{ClF}}_{\text{3}}\right)$ is drawn in explanation part. The hybridization of chlorine trifluoride $\left({\text{ClF}}_{\text{3}}\right)$ is $s{p}^{3}d$.