Chapter 10, Problem 10.16QP

Interpretation Introduction

Interpretation:

• The relationship between the dipole moment and the bond moment has to be discussed.
• The non-polarity of a molecule with bond-moment has to be discussed.

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 $\text{μ}\text{=}\text{Q}\times \text{r}$.  The dipole moment will be created by the charge separation in a polar molecule.

For example:

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

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