Chapter 14, Problem 63A

(a)

Interpretation Introduction

Introduction: Whether $CO$ exhibit dipole-dipole interactions and Hydrogen bonding interactions is to be stated.

Concept introduction: Dipole-dipole interaction is in between two polar molecules. Hydrogen bonding interactions occurs in molecules containing a hydrogen atom linked to a highly electronegative atom.

Answer to Problem 63A

  $CO$ is polar molecule. Hence, forces will be Dipole-dipole attraction.

There is no hydrogen bonding.

Explanation of Solution

  $CO$ is polar molecule which have permanent dipoles. Hence, they exhibit dipole-dipole attraction.

It has no hydrogen bonding because there is no hydrogen in the molecule.

(b)

Interpretation Introduction

Introduction: Whether $N{H}_3$ exhibit dipole-dipole interactions and Hydrogen bonding interactions is to be stated.

Concept introduction: Dipole-dipole interaction is in between two polar molecules. Hydrogen bonding interactions occurs in molecules containing a hydrogen atom linked to a highly electronegative atom.

Answer to Problem 63A

  $N{H}_3$ is polar molecule. Hence, forces will be Dipole-dipole attraction.

There is a hydrogen bonding interactions.

Explanation of Solution

  $N{H}_3$ is polar molecule which have permanent dipoles. Hence, they exhibit dipole-dipole attraction and in $N{H}_3$, nitrogen due to its small size and high electronegativity is directly attached to hydrogen atom and forms H-bond. Therefore, there is hydrogen bonding interactions.

(c)

Interpretation Introduction

Introduction: Whether $C{H}_4$ exhibit dipole-dipole interactions and Hydrogen bonding interactions is to be stated.

Concept introduction: Dipole-dipole interaction is in between two polar molecules. Hydrogen bonding interactions occurs in molecules containing a hydrogen atom linked to a highly electronegative atom.

Answer to Problem 63A

  $C{H}_4$ is non-polar molecule. Hence, forces will not be Dipole-dipole attraction.

There is no hydrogen bonding interactions.

Explanation of Solution

  $C{H}_4$ is non-polar molecule. Hence, it doesn’t exhibit dipole-dipole attraction whereas in it, the carbon due to its small size and less electronegativity doesn’t form H-bond. Therefore, there is no hydrogen bonding interactions.

(d)

Interpretation Introduction

Introduction: Whether $He$ exhibit dipole-dipole interactions and Hydrogen bonding interactions is to be stated.

Concept introduction: Dipole-dipole interaction is in between two polar molecules. Hydrogen bonding interactions occurs in molecules containing a hydrogen atom linked to a highly electronegative atom.

Answer to Problem 63A

  $He$ doesn’t exhibit Dipole-dipole attraction and hydrogen bonding interactions.

Explanation of Solution

  $He$ is non-polar molecule. Hence, it doesn’t exhibit dipole-dipole attraction.

It has no hydrogen bonding because there is no hydrogen in the molecule.

(e)

Interpretation Introduction

Introduction: Whether $HF$ exhibit dipole-dipole interactions and Hydrogen bonding interactions is to be stated.

Concept introduction: Dipole-dipole interaction is in between two polar molecules. Hydrogen bonding interactions occurs in molecules containing a hydrogen atom linked to a highly electronegative atom.

Answer to Problem 63A

  $HF$ is polar molecule. Hence, forces will be Dipole-dipole attraction.

In case of $HF$ , there is a hydrogen bonding interactions.

Explanation of Solution

  $HF$ is polar molecule. Hence, forces will be Dipole-dipole attraction.

In $HF$ , the fluorine due to its small size and high electronegativity is directly attached to hydrogen atom and forms H-bond. Therefore, there is hydrogen bonding interactions in case of hydrogen fluoride.