Chapter 10.3, Problem 10.9AFP

(a)

Interpretation Introduction

Interpretation:

The bond polarity and molecular polarity in dichloromethane $\left({\text{CH}}_2{\text{Cl}}_2\right)$ are to be determined.

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 nonpolar molecules have zero net dipole moment.

(b)

Interpretation Introduction

Interpretation:

The bond polarity and molecular polarity in iodine oxide pentafluoride $\left({\text{IOF}}_5\right)$ are to be determined.

Concept introduction:

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 nonpolar molecules have zero net dipole moment.

(c)

Interpretation Introduction

Interpretation:

The bond polarity and molecular polarity in iodine pentafluoride $\left({\text{IF}}_5\right)$ are to be determined.

Concept introduction:

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 nonpolar molecules have zero net dipole moment.