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

Write structural formulas for the major products by doing addition reactions 1. You must add H2 as Pt is catalyst it does not take part in reactions only speed up the process H₂ CH2=CH-CH3 Pt 2. Add HCI break it into H and Cl CH3 HCI 3. Add Br2 only CC14 is catalyst CH3-CH=CH2 B12 CCl4 4. Add water to this and draw major product, H2SO4 is catalyst you have add water H20 in both the reaction below H₂SO4 CH3-CH=CH2 CH3 H2SO4/H₂O CH3-C=CH2 reflux ?

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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Write structural formulas for the major products by doing addition reactions 1. You must add H2 as Pt is catalyst it does not take part in reactions only speed up the process H₂ CH2=CH-CH3 Pt 2. Add HCI break it into H and Cl CH3 HCI 3. Add Br2 only CC14 is catalyst CH3-CH=CH2 B12 CCl4 4. Add water to this and draw major product, H2SO4 is catalyst you have add water H20 in both the reaction below H₂SO4 CH3-CH=CH2 CH3 H2SO4/H₂O CH3-C=CH2 reflux ?

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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