Chapter 8, Problem 122A

Interpretation Introduction

(a)

Interpretation:

Whether ${\text{H}}_{\text{3}}{\text{O}}^{+}$ ion is polar or not is to be determined.

Concept introduction:

The asymmetric structure and presence of polar covalent bonds confirms that the molecule is polar in nature. The molecule having some dipole moment is termed as polar molecule and the molecule with no dipole moment or zero dipole moment is identified as nonpolar molecule.

Answer to Problem 122A

The ${\text{H}}_{\text{3}}{\text{O}}^{+}$ ion is identified as polar.

Explanation of Solution

The given ion ${\text{H}}_{\text{3}}{\text{O}}^{+}$ is trigonal pyramidal and therefore asymmetrical. The structure of ${\text{H}}_{\text{3}}{\text{O}}^{+}$ ion is shown below.

In ${\text{H}}_{\text{3}}{\text{O}}^{+}$, the charge distribution at any distance from its center is unequal and different (but not opposite) in direction. Therefore, there is some dipole moment which makes ${\text{H}}_{\text{3}}{\text{O}}^{+}$ a polar compound.

Interpretation Introduction

(b)

Interpretation:

Whether ${\text{PCl}}_5$ molecule is polar or not is to be determined.

Concept introduction:

The asymmetric structure and presence of polar covalent bonds confirms that the molecule is polar in nature. The molecule having some dipole moment is termed as polar molecule and the molecule with no dipole moment or zero dipole moment is identified as nonpolar molecule.

Answer to Problem 122A

The ${\text{PCl}}_5$ molecule is not a polar compound.

Explanation of Solution

The given molecule ${\text{PCl}}_5$ is trigonal bipyramidal and therefore symmetrical. The structure of ${\text{PCl}}_5$ is shown below.

In ${\text{PCl}}_5$, the charge distribution at any distance from its center is equal but opposite in direction. Therefore, the partial charges in ${\text{PCl}}_5$ are balance which makes ${\text{PCl}}_5$ as a nonpolar compound.

Interpretation Introduction

(c)

Interpretation:

Whether ${\text{H}}_{\text{2}}\text{S}$ molecule is polar or not is to be determined.

Concept introduction:

The asymmetric structure and presence of polar covalent bonds confirms that the molecule is polar in nature. The molecule having some dipole moment is termed as polar molecule and the molecule with no dipole moment or zero dipole moment is identified as nonpolar molecule.

Answer to Problem 122A

The ${\text{H}}_{\text{2}}\text{S}$ molecule is identified as polar.

Explanation of Solution

The given molecule ${\text{H}}_{\text{2}}\text{S}$ has bent shape and therefore asymmetrical. The structure of ${\text{H}}_{\text{2}}\text{S}$ molecule is shown below.

In ${\text{H}}_{\text{2}}\text{S}$, the charge distribution at any distance from its center is unequal and different (but not opposite) in direction. Therefore, there is some dipole moment which makes ${\text{H}}_{\text{2}}\text{S}$ as a polar compound.

Interpretation Introduction

(d)

Interpretation:

Whether ${\text{CF}}_{\text{4}}$ molecule is polar or not is to be determined.

Concept introduction:

The asymmetric structure and presence of polar covalent bonds confirms that the molecule is polar in nature. The molecule having some dipole moment is termed as polar molecule and the molecule with no dipole moment or zero dipole moment is identified as nonpolar molecule.

Answer to Problem 122A

The ${\text{CF}}_{\text{4}}$ molecule is not a polar compound.

Explanation of Solution

The given molecule ${\text{CF}}_{\text{4}}$ is tetrahedral and therefore symmetrical. The structure of ${\text{CF}}_{\text{4}}$ is shown below.

In ${\text{CF}}_{\text{4}}$, the charge distribution at any distance from its center is equal but opposite in direction. Therefore, the partial charges in ${\text{CF}}_{\text{4}}$ are balance which makes ${\text{CF}}_{\text{4}}$ as a nonpolar compound.