Chapter 7.7, Problem 7.11PP

Interpretation Introduction

(a)

Interpretation:

The types of intermolecular forces present in ${\text{Cl}}_{\text{2}}$ need to be explained.

Concept Introduction:

The forces of attraction between the molecules are the forces that keep them close or bonded together and they are called intermolecular forces.

There are generally 3 types of intermolecular forces-

1. London-dispersion forces- The electrons within a molecule are constantly moving and sometimes this leads to uneven distribution of electrons for a very small interval of time. This unsymmetrical distribution can distort the nearby molecule also leading to the induced dipole−induced dipole interactions between the two molecules. As all the molecules have moving electrons, thus all types of molecules exhibit these forces.
2. Dipole-dipole interactions- When two dipoles (polar molecules) come nearby, then the positive end of one dipole interacts with the negative end of the other dipole or vice-versa. Such interactions are referred to as the dipole-dipole interactions.
3. Hydrogen bonding-It exists when hydrogen bonded to a highly electronegative atom such as O, F or N is attracted by the lone pair on another electronegative atom.

Interpretation Introduction

(b)

Interpretation:

The types of intermolecular forces present in $\text{HCN}$ are to be explained.

Concept Introduction:

The forces of attraction between the molecules are the forces that keep them close or bonded together and they are called intermolecular forces.

There are generally 3 types of intermolecular forces-

1. London-dispersion forces- The electrons within a molecule are constantly moving and sometimes this leads to uneven distribution of electrons for a very small interval time. This unsymmetrical distribution can distort the nearby molecule also leading to the induced dipole −induced dipole interactions between the two molecules. As all the molecules have moving electrons, thus all types of molecules exhibit these forces.
2. Dipole-dipole interactions- When two dipoles (polar molecules) come nearby, then the positive end of one dipole interacts with the negative end of the other dipole or vice-versa. Such interactions are referred to as the dipole-dipole interactions.
3. Hydrogen bonding-It exists when hydrogen bonded to a highly electronegative atom such as O, F or N is attracted by the lone pair on another electronegative atom.

Interpretation Introduction

(c)

Interpretation:

The types of intermolecular forces present in $\text{HF}$ are to be explained.

Concept Introduction:

The forces of attraction between the molecules are the forces that keep them close or bonded together and they are called intermolecular forces.

There are generally 3 types of intermolecular forces-

1. London-dispersion forces- The electrons within a molecule are constantly moving and sometimes this leads to uneven distribution of electrons for a very small interval time. This unsymmetrical distribution can distort the nearby molecule also leading to the induced dipole −induced dipole interactions between the two molecules. As all the molecules have moving electrons, thus all types of molecules exhibit these forces.
2. Dipole-dipole interactions- When two dipoles (polar molecules) come nearby, then the positive end of one dipole interacts with the negative end of the other dipole or vice-versa. Such interactions are referred to as the dipole-dipole interactions.
3. Hydrogen bonding-It exists when hydrogen bonded to a highly electronegative atom such as O, F or N is attracted by the lone pair on another electronegative atom.

Interpretation Introduction

(d)

Interpretation:

The types of intermolecular forces present in ${\text{CH}}_{\text{3}}\text{Cl}$ are to be explained.

Concept Introduction:

The forces of attraction between the molecules are the forces that keep them close or bonded together and they are called intermolecular forces.

There are generally 3 types of intermolecular forces-

1. London-dispersion forces- The electrons within a molecule are constantly moving and sometimes this leads to uneven distribution of electrons for a very small interval time. This unsymmetrical distribution can distort the nearby molecule also leading to the induced dipole −induced dipole interactions between the two molecules. As all the molecules have moving electrons, thus all types of molecules exhibit these forces.
2. Dipole-dipole interactions- When two dipoles (polar molecules) come nearby, then the positive end of one dipole interacts with the negative end of the other dipole or vice-versa. Such interactions are referred to as the dipole-dipole interactions.
3. Hydrogen bonding-It exists when hydrogen bonded to a highly electronegative atom such as O, F or N is attracted by the lone pair on another electronegative atom.

Interpretation Introduction

(e)

Interpretation:

The types of intermolecular forces present in ${\text{H}}_{\text{2}}$ are to be explained.

Concept Introduction:

The forces of attraction between the molecules are the forces that keep them close or bonded together and they are called intermolecular forces.

There are generally 3 types of intermolecular forces-

1. London-dispersion forces- The electrons within a molecule are constantly moving and sometimes this leads to uneven distribution of electrons for a very small interval time. This unsymmetrical distribution can distort the nearby molecule also leading to the induced dipole −induced dipole interactions between the two molecules. As all the molecules have moving electrons, thus all types of molecules exhibit these forces.
2. Dipole-dipole interactions- When two dipoles (polar molecules) come nearby, then the positive end of one dipole interacts with the negative end of the other dipole or vice-versa. Such interactions are referred to as the dipole-dipole interactions.
3. Hydrogen bonding-It exists when hydrogen bonded to a highly electronegative atom such as O, F or N is attracted by the lone pair on another electronegative atom.