Chapter 11, Problem 11.1QP

(a)

Interpretation Introduction

Interpretation:

An example for Dipole-Dipole interaction, has to be given.

Concept Introduction:

Intermolecular forces are the forces existing between molecules, atoms, ions or dipoles.

Depending upon the type of species involved, the intermolecular forces can be classified as follows:

• Dipole-Dipole interactions.
• Ion-Dipole interactions.
• Dipole-induced dipole interactions.
• Ion-induced dipole interactions.
• Dispersion forces.
• Van der waals forces.
• Dipole-Dipole interaction is the interaction between two polar molecules which have net dipole moments.
• Ion-Dipole interaction is the interaction between an ionic species (such as cation or anion) and a polar molecule.
• Dipole-induced dipole is the interaction between an atom (non- polar species) and a polar molecule. In this interaction, a polar molecule induces its dipole moment to a non-polar species which lacks dipole moment.
• Ion-induced dipole interaction is the interaction between an atom (non- polar species) and an ionic species. In this interaction, an ionic species such as cation or anion, induces dipole in a non-polar species which lacks dipole moment.
• Dispersion force is the interaction between non-polar molecules.
• Van der waals forces are intermolecular forces which are of two types: Stronger and weaker. Dipole-Dipole interaction is the strong Van der waals force and dispersion force is the weak Van der waals force.

Explanation of Solution

An example for Dipole-Dipole interaction is between $\text{LiF}$ molecules.

The intermolecular force existing between $\text{LiF}$ molecules, is Dipole-Dipole interaction.

$\text{LiF}$ is an ionic species.

The ions present in $\text{LiF}$ are:

${\text{Li}}^{+}$-Cation

${\text{F}}^{\text{-}}$-Anion

These two ionic species constitute a dipole in the molecule.  So, the interaction existing between $\text{LiF}$ molecules is the Dipole-Dipole interaction.

(b)

Interpretation Introduction

Interpretation:

An example for Dipole-induced dipole, has to be given.

Concept Introduction:

Intermolecular forces are the forces existing between molecules, atoms, ions or dipoles.

Depending upon the type of species involved, the intermolecular forces can be classified as follows:

• Dipole-Dipole interactions.
• Ion-Dipole interactions.
• Dipole-induced dipole interactions.
• Ion-induced dipole interactions.
• Dispersion forces.
• Van der waals forces.
• Dipole-Dipole interaction is the interaction between two polar molecules which have net dipole moments.
• Ion-Dipole interaction is the interaction between an ionic species (such as cation or anion) and a polar molecule.
• Dipole-induced dipole is the interaction between an atom (non- polar species) and a polar molecule. In this interaction, a polar molecule induces its dipole moment to a non-polar species which lacks dipole moment.
• Ion-induced dipole interaction is the interaction between an atom (non- polar species) and an ionic species. In this interaction, an ionic species such as cation or anion, induces dipole in a non-polar species which lacks dipole moment.
• Dispersion force is the interaction between non-polar molecules.
• Van der waals forces are intermolecular forces which are of two types: Stronger and weaker. Dipole-Dipole interaction is the strong Van der waals force and dispersion force is the weak Van der waals force.

Explanation of Solution

An example for Dipole-induced dipole interaction is between a helium atom (non-polar species) and a polar molecule which is in proximity to it.

The intermolecular force existing between a polar molecule and a helium atom is Dipole-induced dipole interaction.

A polar molecule has permanent dipole moment which can cause distortion to the spherical electronic distribution of helium atom. The extend of distortion depends on the strength of the polarizability of the polar molecular species. The distortion caused in the helium atom is the dipole moment which has been induced or created by the interaction with a polar molecule. So such an interaction is known as dipole-induced-dipole moment.

(c)

Interpretation Introduction

Interpretation:

An example for Ion-Dipole interaction, has to be given.

Concept Introduction:

Intermolecular forces are the forces existing between molecules, atoms, ions or dipoles.

Depending upon the type of species involved, the intermolecular forces can be classified as follows:

• Dipole-Dipole interactions.
• Ion-Dipole interactions.
• Dipole-induced dipole interactions.
• Ion-induced dipole interactions.
• Dispersion forces.
• Van der waals forces.
• Dipole-Dipole interaction is the interaction between two polar molecules which have net dipole moments.
• Ion-Dipole interaction is the interaction between an ionic species (such as cation or anion) and a polar molecule.
• Dipole-induced dipole is the interaction between an atom (non- polar species) and a polar molecule. In this interaction, a polar molecule induces its dipole moment to a non-polar species which lacks dipole moment.
• Ion-induced dipole interaction is the interaction between an atom (non- polar species) and an ionic species. In this interaction, an ionic species such as cation or anion, induces dipole in a non-polar species which lacks dipole moment.
• Dispersion force is the interaction between non-polar molecules.
• Van der waals forces are intermolecular forces which are of two types: Stronger and weaker. Dipole-Dipole interaction is the strong Van der waals force and dispersion force is the weak Van der waals force.

Explanation of Solution

An example for Ion-Dipole interaction is between metal ions and water molecules which can be observed in the aqueous solutions of metal ions.

In the aqueous solutions of metal ions, metal ions are ionic species and water molecules are polar molecules. So, water molecules possess permanent dipole moment. Hence, the interaction between metal ions and water molecules is Ion-Dipole interaction.

(d)

Interpretation Introduction

Interpretation:

An example for dispersion forces, has to be given.

Concept Introduction:

Intermolecular forces are the forces existing between molecules, atoms, ions or dipoles.

Depending upon the type of species involved, the intermolecular forces can be classified as follows:

• Dipole-Dipole interactions.
• Ion-Dipole interactions.
• Dipole-induced dipole interactions.
• Ion-induced dipole interactions.
• Dispersion forces.
• Van der waals forces.
• Dipole-Dipole interaction is the interaction between two polar molecules which have net dipole moments.
• Ion-Dipole interaction is the interaction between an ionic species (such as cation or anion) and a polar molecule.
• Dipole-induced dipole is the interaction between an atom (non- polar species) and a polar molecule. In this interaction, a polar molecule induces its dipole moment to a non-polar species which lacks dipole moment.
• Ion-induced dipole interaction is the interaction between an atom (non- polar species) and an ionic species. In this interaction, an ionic species such as cation or anion, induces dipole in a non-polar species which lacks dipole moment.
• Dispersion force is the interaction between non-polar molecules.
• Van der waals forces are intermolecular forces which are of two types: Stronger and weaker. Dipole-Dipole interaction is the strong Van der waals force and dispersion force is the weak Van der waals force.

Explanation of Solution

An example for dispersion force is between ${\text{F}}_2$ molecules.

${\text{F}}_{\text{2}}$ is a homodiatomic molecule, which lacks polarity. Hence, ${\text{F}}_{\text{2}}$ is a non-polar molecule. The electronic distribution in one ${\text{F}}_{\text{2}}$ molecule induces an instantaneous dipole moment in it. This instantaneous dipole moment in each molecule creates a temporary dipole moment among the surrounding molecules. Such an interaction existing between non-polar molecules is the dispersion force.

(e)

Interpretation Introduction

Interpretation:

An example for Van der waals forces, has to be given.

Concept Introduction:

Intermolecular forces are the forces existing between molecules, atoms, ions or dipoles.

Depending upon the type of species involved, the intermolecular forces can be classified as follows:

• Dipole-Dipole interactions.
• Ion-Dipole interactions.
• Dipole-induced dipole interactions.
• Ion-induced dipole interactions.
• Dispersion forces.
• Van der waals forces.
• Dipole-Dipole interaction is the interaction between two polar molecules which have net dipole moments.
• Ion-Dipole interaction is the interaction between an ionic species (such as cation or anion) and a polar molecule.
• Dipole-induced dipole is the interaction between an atom (non- polar species) and a polar molecule. In this interaction, a polar molecule induces its dipole moment to a non-polar species which lacks dipole moment.
• Ion-induced dipole interaction is the interaction between an atom (non- polar species) and an ionic species. In this interaction, an ionic species such as cation or anion, induces dipole in a non-polar species which lacks dipole moment.
• Dispersion force is the interaction between non-polar molecules.
• Van der waals forces are intermolecular forces which are of two types: Stronger and weaker. Dipole-Dipole interaction is the strong Van der waals force and dispersion force is the weak Van der waals force.

Explanation of Solution

Van der waals forces are intermolecular forces which are of two types: Stronger and weaker.

Dipole-Dipole interaction is the strong Van der waals force and dispersion force is the weak Van der waals force.

An example for Dipole-Dipole interaction is between ${\text{SO}}_{\text{2}}$ molecules.

${\text{SO}}_{\text{2}}$ molecule has a net dipole moment. So, it is a polar molecule like water molecule. Hence, the interaction between ${\text{SO}}_{\text{2}}$ molecules is Dipole-Dipole interaction.

An example for dispersion force is between ${\text{Cl}}_2$ molecules.

${\text{Cl}}_{\text{2}}$ is a homodiatomic molecule, which lacks polarity. Hence, ${\text{Cl}}_{\text{2}}$ is a non-polar molecule. The electronic distribution in one ${\text{Cl}}_{\text{2}}$ molecule induces an instantaneous dipole moment in it. This instantaneous dipole moment in each molecule creates a temporary dipole moment among the surrounding molecules. Such an interaction existing between non-polar molecules is the dispersion force.