Chapter 10, Problem 10.57P

(a)

Interpretation Introduction

Interpretation:

The molecule that has greater dipole moment among ${\text{SO}}_3$ and ${\text{SO}}_2$ is to be identified.

Concept introduction:

The dipole moment arises when there is a separation of charges between two ions or atoms involved in the bond. The dipole moment is a vector quantity and its direction towards the most electronegative atom.

The direction of the dipole moment is represented as follows:

The polar and non-polar molecule can be identified on the basis of the net dipole moment. Polar molecules have non zero value of net dipole moment and the non polar molecules have zero net dipole moment.

(b)

Interpretation Introduction

Interpretation:

The molecule that has greater dipole moment among $\text{ICl}$ and $\text{IF}$ is to be identified.

Concept introduction:

Electronegativity is the tendency of an atom to attract the shared electrons in the bond towards itself. The more electronegative atom will more attract the bonding electrons towards itself than the less electronegative atom. Therefore the electrons will spend more time with the more electronegative atom than an electropositive atom. The electronegative atom will acquire the partial negative charge and the electropositive atom will acquire a partial positive charge.

Here, B is the electronegative atom and A is the electropositive atom.

Bond polarity can be estimated by $\Delta \text{EN}$. $\Delta \text{EN}$ is the electronegativity difference between the atoms bonded to each other. The formula to calculate $\Delta \text{EN}$ in AB bond is as follows:

  $\Delta \text{EN}=\left(\text{electronegativity of B}\right)-\left(\text{electronegativity of A}\right)$

Here, B is the electronegative atom and A is the electropositive atom.

The greater electronegativity difference between the atoms induces the greater polarity in the bond thus it generates higher dipole moment.

(c)

Interpretation Introduction

Interpretation:

The molecule that has greater dipole moment among ${\text{SiF}}_4$ and ${\text{SF}}_4$ is to be identified.

Concept introduction:

The dipole moment arises when there is a separation of charges between two ions or atoms involved in the bond. The dipole moment is a vector quantity and its direction towards the most electronegative atom.

The direction of the dipole moment is represented as follows:

The polar and non-polar molecule can be identified on the basis of the net dipole moment. Polar molecules have non zero value of net dipole moment and the non polar molecules have zero net dipole moment.

(d)

Interpretation Introduction

Interpretation:

The molecule that has greater dipole moment among ${\text{H}}_2\text{O}$ and ${\text{H}}_2\text{S}$ is to be identified.

Concept introduction:

Electronegativity is the tendency of an atom to attract the shared electrons in the bond towards itself. The more electronegative atom will more attract the bonding electrons towards itself than the less electronegative atom. Therefore the electrons will spend more time with the more electronegative atom than an electropositive atom. The electronegative atom will acquire the partial negative charge and the electropositive atom will acquire a partial positive charge.

Here, B is the electronegative atom and A is the electropositive atom.

Bond polarity can be estimated by $\Delta \text{EN}$. $\Delta \text{EN}$ is the electro negativity difference between the atoms bonded to each other. The formula to calculate $\Delta \text{EN}$ in AB bond is as follows:

  $\Delta \text{EN}=\left(\text{electronegativity of B}\right)-\left(\text{electronegativity of A}\right)$

Here, B is the electronegative atom and A is the electropositive atom.

The greater electronegativity difference between the atoms induces the greater polarity in the bond thus it generates higher dipole moment.