The water ( H 2 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 ( 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.

Question

Deducing the reactants of a Diels-Alder reaction vn the molecule on the right-hand side of this organic reaction be made in good yield from no more than two reactants, in one step, by moderately heating the reactants? ? Δ O If your answer is yes, then draw the reactant or reactants in the drawing area below. You can draw the reactants in any arrangement you like. • If your answer is no, check the box under the drawing area instead. Click and drag to start drawing a structure. Product can't be made in one step. Explanation Check

Answer 1

Question

Chapter 3.9, Problem 32P

(a)

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.

(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 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.

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Deducing the reactants of a Diels-Alder reaction vn the molecule on the right-hand side of this organic reaction be made in good yield from no more than two reactants, in one step, by moderately heating the reactants? ? Δ O If your answer is yes, then draw the reactant or reactants in the drawing area below. You can draw the reactants in any arrangement you like. • If your answer is no, check the box under the drawing area instead. Click and drag to start drawing a structure. Product can't be made in one step. Explanation Check

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> Can the molecule on the right-hand side of this organic reaction be made in good yield from no more than two reactants, in one step, by moderately heating the reactants? ? Δ • If your answer is yes, then draw the reactant or reactants in the drawing area below. You can draw the reactants in any arrangement you like. If your answer is no, check the box under the drawing area instead. Explanation Check Click and drag to start drawing a structure. Х © 2025 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Acces

Answer 2

Question

Chapter 3.9, Problem 32P

(a)

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.

(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 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.

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Answer 3

Question

Chapter 3.9, Problem 32P

(a)

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.

(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 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.

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Answer 4

Question

Chapter 3.9, Problem 32P

(a)

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.

(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 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.

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Answer 5

Chapter 3.9, Problem 32P

(a)

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.

(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 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.

Answer 6

Chapter 3.9, Problem 32P

(a)

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.

Answer 7

Chapter 3.9, Problem 32P

(a)

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.

Answer 8

(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 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.

Answer 9

(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 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.

Answer 10

(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.

Answer 11

(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.

Answer 12

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.

Answer 13

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.

Answer 14

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Ch. 3.1 - Name each of the following:Ch. 3.1 - Draw the structure of a compound with molecular...Ch. 3.1 - Draw the structures and name the four...Ch. 3.1 - Prob. 6P Ch. 3.1 - Draw the structure for each of the following: a....Ch. 3.1 - Name the following compounds: a. CH3OCH2CH3 b....Ch. 3.2 - Prob. 11P Ch. 3.2 - Prob. 12P Ch. 3.3 - Prob. 13P Ch. 3.3 - Prob. 14P

Solution Summary: The author explains that the boiling point of a chemical compound depends on the strength of the attractive forces between the individual molecules.

Chapter 3 Solutions