Chapter 4.3, Problem 4.10P

(a)

Interpretation Introduction

Interpretation:

The type of intermolecular forces present in ${\text{Cl}}_{\text{2}}$ has to be given.

Concept introduction:

London Dispersion forces:

London dispersion forces are weak interactions due to the temporary changes in electron density in a molecule.  All covalent compound exhibits London dispersion forces.  These intermolecular forces are the only intermolecular forces present in nonpolar compounds.

Hydrogen Bonding:

A chemical bond in which a hydrogen atom of one molecule is attracted to an electronegative atom especially a nitrogen, oxygen, or fluorine atom, usually of another molecule.

Dipole-dipole interactions:

Dipole–dipole interactions are electrostatic interactions between molecules which have permanent dipoles. This interaction is stronger than the London forces but is weaker than ion-ion interaction because only partial charges are involved positive end of a polar molecule will attract the negative end of the other molecule and influence its position

(b)

Interpretation Introduction

Interpretation:

The type of intermolecular forces present in $\text{HCN}$ has to be given.

Concept Introduction:

Refer to part (a).

(c)

Interpretation Introduction

Interpretation:

The type of intermolecular forces present in $\text{HF}$ has to be given.

Concept Introduction:

Refer to part (a).

(d)

Interpretation Introduction

Interpretation:

The type of intermolecular forces present in ${\text{CH}}_{\text{3}}\text{Cl}$ has to be given.

Concept Introduction:

Refer to part (a).

(e)

Interpretation Introduction

Interpretation:

The type of intermolecular forces present in ${\text{H}}_{\text{2}}$ has to be given.

Concept Introduction:

Refer to part (a).