Chapter 10, Problem 10.76QP

(a)

Interpretation Introduction

Interpretation: The hybridization of $\text{N}$ in ${\text{N}}_{\text{2}}{\text{F}}_{\text{2}}$ molecule has to be identified.

Concept Introduction:

Hybridization is the phenomenon of intermixing of the atomic orbitals of different energy that results in the formation of a new set of hybrid orbitals which have equivalent energies. The various types of atomic orbitals are: s, p, and d orbitals. Types of hybridization that involves s, p and d orbitals are $\text{sp,}{\text{sp}}^{\text{2}}\text{,}{\text{sp}}^{\text{3}}\text{,}{\text{sp}}^{\text{3}}\text{d,}{\text{sp}}^{\text{3}}{\text{d}}^{\text{2}}\text{,}{\text{sp}}^{\text{3}}{\text{d}}^{\text{3}}.$

(b)

Interpretation Introduction

Interpretation: Among the given two structures of ${\text{N}}_{\text{2}}{\text{F}}_{\text{2}}$, the one with the dipole moment has to be identified.

Concept Introduction:

The term dipole moment refers to the quantitative measure of polarity of a bond. It is represented as $\text{μ}$. It can be defined as the product of the charge $\text{Q}$ and the distance r between the charges. So, its mathematical representation is $\text{μ}\text{=}\text{Q}\times \text{r}$. Dipole moment will be created by the charge separation in a polar molecule.

For example:

The diatomic molecule $\text{HCl}$ possesses dipole moment due to the charge separation in it as shown here:

The crossed arrow represents the direction of the shift of electrons toward the highly electronegative chlorine atom from the least electronegative hydrogen atom.

Dipole moment with respect to cis and trans-forms:

In the trans -form of a compound, the bond moments will be in the opposite direction with the same magnitude. So cancel each other. Hence there won’t be any dipole moment. Whereas in the case of cis-form, the bond moments will be in the same direction with the same magnitude. So does not cancel each other. Hence there will be resultant dipole moment.