Chapter 7.3, Problem 4PPA

(a)

Interpretation Introduction

Interpretation: the intermolecular forces presented in the given molecules ${\text{CH}}_{\text{3}}{\text{CH}}_2{\text{CH}}_2{\text{CH}}_2{\text{CH}}_3\text{(l)}$, ${\text{CH}}_{\text{3}}{\text{CH}}_2\text{OH (l)}$, ${\text{H}}_2\text{CO}\text{(l)}$ and ${\text{O}}_2\text{(l)}$ are to be determined.

Concept introduction:

• Polarity of a bond is due to the difference in electro-negativities of atoms presented in it. The polarities of bonds are represented by using vectors.
• If the result of all bond polarities or vector sum is non-zero in a molecule, then the molecule is called as polar molecule.
• If the result of all bond polarities or vector sum is zero in a molecule, then the molecule is called as nonpolar molecule.
• Intermolecular force is the set of repulsive and attractive forces between molecules that result from the polarity between neighboring molecules. There are four types of intermolecular forces.
• Dipole – Dipole interaction: This force takes place between polar compounds.
• Hydrogen bonding is a type of dipole-dipole interaction of molecules when the hydrogen is bonded to strong electronegative atom (F, O, N, etc) in the molecules.
• Dispersion force is a weak force and this force is present in all compounds force.

(b)

Interpretation Introduction

Interpretation: the intermolecular forces presented in the given molecules ${\text{CH}}_{\text{3}}{\text{CH}}_2{\text{CH}}_2{\text{CH}}_2{\text{CH}}_3\text{(l)}$, ${\text{CH}}_{\text{3}}{\text{CH}}_2\text{OH (l)}$, ${\text{H}}_2\text{CO}\text{(l)}$ and ${\text{O}}_2\text{(l)}$ are to be determined.

Concept introduction:

• Polarity of a bond is due to the difference in electro-negativities of atoms presented in it. The polarities of bonds are represented by using vectors.
• If the result of all bond polarities or vector sum is non-zero in a molecule, then the molecule is called as polar molecule.
• If the result of all bond polarities or vector sum is zero in a molecule, then the molecule is called as nonpolar molecule.
• Intermolecular force is the set of repulsive and attractive forces between molecules that result from the polarity between neighboring molecules. There are four types of intermolecular forces.
• Dipole – Dipole interaction: This force takes place between polar compounds.
• Hydrogen bonding is a type of dipole-dipole interaction of molecules when the hydrogen is bonded to strong electronegative atom (F, O, N, etc) in the molecules.
• Dispersion force is a weak force and this force is present in all compounds force.

(c)

Interpretation Introduction

Interpretation: the intermolecular forces presented in the given molecules ${\text{CH}}_{\text{3}}{\text{CH}}_2{\text{CH}}_2{\text{CH}}_2{\text{CH}}_3\text{(l)}$, ${\text{CH}}_{\text{3}}{\text{CH}}_2\text{OH (l)}$, ${\text{H}}_2\text{CO}\text{(l)}$ and ${\text{O}}_2\text{(l)}$ are to be determined.

Concept introduction:

• Polarity of a bond is due to the difference in electro-negativities of atoms presented in it. The polarities of bonds are represented by using vectors.
• If the result of all bond polarities or vector sum is non-zero in a molecule, then the molecule is called as polar molecule.
• If the result of all bond polarities or vector sum is zero in a molecule, then the molecule is called as nonpolar molecule.
• Intermolecular force is the set of repulsive and attractive forces between molecules that result from the polarity between neighboring molecules. There are four types of intermolecular forces.
• Dipole – Dipole interaction: This force takes place between polar compounds.
• Hydrogen bonding is a type of dipole-dipole interaction of molecules when the hydrogen is bonded to strong electronegative atom (F, O, N, etc) in the molecules.
• Dispersion force is a weak force and this force is present in all compounds force.

To determine: intermolecular forces presented in ${\text{H}}_2\text{CO}\text{(l)}$.

(d)

Interpretation Introduction

Interpretation: the intermolecular forces presented in the given molecules ${\text{CH}}_{\text{3}}{\text{CH}}_2{\text{CH}}_2{\text{CH}}_2{\text{CH}}_3\text{(l)}$, ${\text{CH}}_{\text{3}}{\text{CH}}_2\text{OH (l)}$, ${\text{H}}_2\text{CO}\text{(l)}$ and ${\text{O}}_2\text{(l)}$ are to be determined.

Concept introduction:

• Polarity of a bond is due to the difference in electro-negativities of atoms presented in it. The polarities of bonds are represented by using vectors.
• If the result of all bond polarities or vector sum is non-zero in a molecule, then the molecule is called as polar molecule.
• If the result of all bond polarities or vector sum is zero in a molecule, then the molecule is called as nonpolar molecule.
• Intermolecular force is the set of repulsive and attractive forces between molecules that result from the polarity between neighboring molecules. There are four types of intermolecular forces.
• Dipole – Dipole interaction: This force takes place between polar compounds.
• Hydrogen bonding is a type of dipole-dipole interaction of molecules when the hydrogen is bonded to strong electronegative atom (F, O, N, etc) in the molecules.
• Dispersion force is a weak force and this force is present in all compounds force.