Chapter 3.9, Problem 34P

(a)

Interpretation Introduction

Interpretation:

The water (${\text{H}}_{\text{2}}\text{O}$) molecule has higher boiling point when compare to other molecules of given in the statement why, this comparison must be explain in each statements.

Concept introduction:

Boiling points: The every chemical compounds is the particular temperature at which its liquid from becomes a gas or (vaporizes). For a compound to vaporize, the forces that hold the individual molecules close to each other in the liquid must be overcome.

Than the boiling point of a each compound depends on the strength of the attractive forces between the individual molecules. If the molecules are held together by strong force then a great deal of energy will be need to pull the molecules away from each other and the compound will have a high boiling point.

On the other hand, if the molecules are held together by weak forces only a small of energy be need to pull the molecules away from each other and the compound will have a low boiling point.

Dipole interaction: The boiling points of all organic molecules like (ether, alkyl halide, amines, alcohols) also increase molecular weight because in the London dispersion forces. The boling points of these compounds, however are also affected the polar ($\text{C-Z}$) bonds here ($\text{Z= N, O, F, Cl}$). Generally alcohols have higher boiling point when compare to other organic molecules, because addition of London dispersion forces and the dipole-dipole interaction of the polar C-O bond, alcohol can from hydrogen bonds.

(b)

Interpretation Introduction

Interpretation:

The water (H₂O) molecule has higher boiling point when compare to other molecules of given in the statement why, this comparison must be explain in each statements.

Concept introduction:

Boiling points: The every chemical compounds is the particular temperature at which its liquid from becomes a gas or (vaporizes). For a compound to vaporize, the forces that hold the individual molecules close to each other in the liquid must be overcome.

Than the boiling point of a each compound depends on the strength of the attractive forces between the individual molecules. If the molecules are held together by strong force then a great deal of energy will be need to pull the molecules away from each other and the compound will have a high boiling point.

On the other hand, if the molecules are held together by weak forces only a small of energy be need to pull the molecules away from each other and the compound will have a low boiling point.

Dipole interaction: The boiling points of all organic molecules like (ether, alkyl halide, amines, alcohols) also increase molecular weight because in the London dispersion forces. The boling points of these compounds, however are also affected the polar (C-Z) bonds here (Z $\text{Z= N, O, F, Cl}$ cause addition of London dispersion forces and the dipole-dipole interaction of the polar C-O bond, alcohol can from hydrogen bonds.

(c)

Interpretation Introduction

Interpretation:

The water (H₂O) molecule has higher boiling point when compare to other molecules of given in the statement why, this comparison must be explain in each statements.

Concept introduction:

Boiling points: The every chemical compounds is the particular temperature at which its liquid from becomes a gas or (vaporizes). For a compound to vaporize, the forces that hold the individual molecules close to each other in the liquid must be overcome.

Than the boiling point of a each compound depends on the strength of the attractive forces between the individual molecules. If the molecules are held together by strong force then a great deal of energy will be need to pull the molecules away from each other and the compound will have a high boiling point.

On the other hand, if the molecules are held together by weak forces only a small of energy be need to pull the molecules away from each other and the compound will have a low boiling point.

Dipole interaction: The boiling points of all organic molecules like (ether, alkyl halide, amines, alcohols) also increase molecular weight because in the London dispersion forces. The boling points of these compounds, however are also affected the polar (C-Z) bonds here (Z= N, O, F, Cl). Generally alcohols have higher boiling point when compare to other organic molecules, because addition of London dispersion forces and the dipole-dipole interaction of the polar C-O bond, alcohol can from hydrogen bonds.

d)

Interpretation Introduction

Interpretation:

The H-F molecule has higher boiling point when compare to other molecules of given in the statement why, this comparison must be explain in each statements.

Concept introduction:

Boiling points: The every chemical compounds is the particular temperature at which its liquid from becomes a gas or (vaporizes). For a compound to vaporize, the forces that hold the individual molecules close to each other in the liquid must be overcome.

Than the boiling point of a each compound depends on the strength of the attractive forces between the individual molecules. If the molecules are held together by strong force then a great deal of energy will be need to pull the molecules away from each other and the compound will have a high boiling point.

On the other hand, if the molecules are held together by weak forces only a small of energy be need to pull the molecules away from each other and the compound will have a low boiling point.

Dipole interaction: The boiling points of all organic molecules like (ether, alkyl halide, amines, alcohols) also increase molecular weight because in the London dispersion forces. The boling points of these compounds, however are also affected the polar (C-Z) bonds here (Z= N, O, F, Cl). Generally alcohols have higher boiling point when compare to other organic molecules, because addition of London dispersion forces and the dipole-dipole interaction of the polar C-O bond, alcohol can from hydrogen bonds.