Chapter 14, Problem 7A

(a)

Interpretation Introduction

Interpretation :

What types of intermolecular forces are present in the liquid state of neon molecule must be explained.

Concept Introduction :

Neon is a noble gas element it is represented as $\text{Ne}$ with the atomic number $10$ .

Answer to Problem 7A

London dispersion forces of attraction are present in the Neon noble gas.

Explanation of Solution

Neon is a noble gas. The forces are very weak.

In neon, there are very weak forces of attraction present, that is, London dispersion forces.

(b)

Interpretation Introduction

Interpretation:

What types of intermolecular forces are present in the liquid state of carbon monoxide molecule must be explained.

Concept Introduction :

Carbon monoxide is a polar molecule.

Answer to Problem 7A

London dispersion forces of attraction are present in the carbon monoxide.

Explanation of Solution

Carbon monoxide $\text{CO}$ , it has two $\text{C}-\text{O}$ bonds.

The $\text{C}-\text{O}$ bond is a polar bond, which means the oxygen is slightly positively charged and the carbon slightly negatively charged. In $\text{C}-\text{O}$ , the atoms have intermolecular bonds between carbon and oxygen due to attraction between positive and negative charges.

The intermolecular forces in $\text{CO}$ are dipole-dipole.

(c)

Interpretation Introduction

Interpretation:

What types of intermolecular forces are present in the liquid state of the methanol molecule must be explained.

Concept Introduction:

The electronegativity of O is more than C and H.

Answer to Problem 7A

London dispersion forces and Hydrogen bonding is present in the methanol.

Explanation of Solution

Methanol is represented as ${\text{H}}_{\text{3}}\text{C-O-H}$

The weakest intermolecular forces are London dispersion forces. London dispersion forces are attractions between the temporary dipoles formed due to a change in electron distribution. All atoms and molecules containing electrons experiences intermolecular forces. Therefore, molecules of methanol are held through London dispersion forces.

Hydrogen bonds are a special form of dipole-dipole interactions.

When a hydrogen atom is bonded to a small, electronegative atom, then the electronegative atom pulls electron density away from the hydrogen atom. This puts a partial positive charge on the hydrogen atom and a partial negative charge on the electronegative atom. The hydrogen atom on one molecule will be attracted to the electronegative atom on another molecule.

The $-\text{OH}$ group on methanol can undergo hydrogen bonding. Because the $\text{O}-\text{H}$ bond is polar, the oxygen atom will have high electron density (negative charge) and the hydrogen atom will have low electron density (positive charge). Therefore, the hydrogen atom on one molecule of methanol will experience electrostatic attraction to the oxygen atom on another molecule of methanol that is. hydrogen bond.

(d)

Interpretation Introduction

Interpretation:

What types of intermolecular forces are present in the liquid state of the chlorine molecule must be explained.

Concept Introduction:

Chlorine is a nonpolar homodiatomic molecule.

Answer to Problem 7A

London dispersion forces of attraction are present in the chlorine molecule.

Explanation of Solution

The weakest intermolecular forces are London dispersion forces. London dispersion forces are attractions between the temporary dipoles formed due to a change in electron distribution. All atoms and molecules containing electrons experience intermolecular forces. Therefore, molecules of chlorine are held through London dispersion forces.