The compound that exhibits weaker intermolecular forces has to be given. Concept introduction: London Dispersion forces: London dispersion forces are weak interactions due to the temporary changes in electron density in a molecule. All covalent compound exhibits London dispersion forces. These intermolecular forces are the only intermolecular forces present in nonpolar compounds. Hydrogen Bonding: A chemical bond in which a hydrogen atom of one molecule is attracted to an electronegative atom especially a nitrogen, oxygen, or fluorine atom, usually of another molecule. Dipole-dipole interactions: Dipole–dipole interactions are electrostatic interactions between molecules which have permanent dipoles. This interaction is stronger than the London forces but is weaker than ion-ion interaction because only partial charges are involved positive end of a polar molecule will attract the negative end of the other molecule and influence its position

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Answer 1

Question

Chapter 4, Problem 4.59AP

(a)

Interpretation Introduction

Interpretation:

The compound that exhibits weaker intermolecular forces has to be given.

Concept introduction:

London Dispersion forces:

London dispersion forces are weak interactions due to the temporary changes in electron density in a molecule. All covalent compound exhibits London dispersion forces. These intermolecular forces are the only intermolecular forces present in nonpolar compounds.

Hydrogen Bonding:

A chemical bond in which a hydrogen atom of one molecule is attracted to an electronegative atom especially a nitrogen, oxygen, or fluorine atom, usually of another molecule.

Dipole-dipole interactions:

Dipole–dipole interactions are electrostatic interactions between molecules which have permanent dipoles. This interaction is stronger than the London forces but is weaker than ion-ion interaction because only partial charges are involved positive end of a polar molecule will attract the negative end of the other molecule and influence its position

(b)

Interpretation Introduction

Interpretation:

The compound, which has higher boiling point, has to be given.

(c)

Interpretation Introduction

Interpretation:

The compound, which has higher melting point, has to be given.

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Answer the following questions about pentane (C 5H 12), heptane (C 7H 16), and decane (C 10H 22). a. Which compound has the highest boiling point? b. Which compound has the lowest boiling point? c. Which compound has the highest melting point? d. Which compound has the lowest melting point?

Normal boiling point of ethanol (C2H5OH) is 78 °C, and of propanol (C3H7OH) is 97 °C. a. Explain the reason for the difference in boiling points of these two alcohols. b. When the underline methyl group in propanol, CH3CH2CH2OH, is replaced with a hydroxyl group (HOCH2CH2OH), boiling point of the molecule increases to 197 °C. Explain the reason for observed increase in the boiling point.

1. What functional group increases the boiling point of straight chain primary alcohols and carboxylic acids by 18 degrees Celsius? methane methylane ethylene methylene 2. What type of bonds are present between alcohol molecules that allow them to have a higher boiling point than saturated hydrocarbons? A. Van der Waals forces B. hydrogen bond C. london forces D. dipole-dipole bonds 3. It is a compound composed of 2 similar subunits or held together by ionic or covalent bonds. primer chiral monomer dimer

Answer 2

Question

Chapter 4, Problem 4.59AP

(a)

Interpretation Introduction

Interpretation:

The compound that exhibits weaker intermolecular forces has to be given.

Concept introduction:

London Dispersion forces:

London dispersion forces are weak interactions due to the temporary changes in electron density in a molecule. All covalent compound exhibits London dispersion forces. These intermolecular forces are the only intermolecular forces present in nonpolar compounds.

Hydrogen Bonding:

A chemical bond in which a hydrogen atom of one molecule is attracted to an electronegative atom especially a nitrogen, oxygen, or fluorine atom, usually of another molecule.

Dipole-dipole interactions:

Dipole–dipole interactions are electrostatic interactions between molecules which have permanent dipoles. This interaction is stronger than the London forces but is weaker than ion-ion interaction because only partial charges are involved positive end of a polar molecule will attract the negative end of the other molecule and influence its position

(b)

Interpretation Introduction

Interpretation:

The compound, which has higher boiling point, has to be given.

(c)

Interpretation Introduction

Interpretation:

The compound, which has higher melting point, has to be given.

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Answer 3

Question

Chapter 4, Problem 4.59AP

(a)

Interpretation Introduction

Interpretation:

The compound that exhibits weaker intermolecular forces has to be given.

Concept introduction:

London Dispersion forces:

London dispersion forces are weak interactions due to the temporary changes in electron density in a molecule. All covalent compound exhibits London dispersion forces. These intermolecular forces are the only intermolecular forces present in nonpolar compounds.

Hydrogen Bonding:

A chemical bond in which a hydrogen atom of one molecule is attracted to an electronegative atom especially a nitrogen, oxygen, or fluorine atom, usually of another molecule.

Dipole-dipole interactions:

Dipole–dipole interactions are electrostatic interactions between molecules which have permanent dipoles. This interaction is stronger than the London forces but is weaker than ion-ion interaction because only partial charges are involved positive end of a polar molecule will attract the negative end of the other molecule and influence its position

(b)

Interpretation Introduction

Interpretation:

The compound, which has higher boiling point, has to be given.

(c)

Interpretation Introduction

Interpretation:

The compound, which has higher melting point, has to be given.

Expert Solution & Answer

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Answer 4

Question

Chapter 4, Problem 4.59AP

(a)

Interpretation Introduction

Interpretation:

The compound that exhibits weaker intermolecular forces has to be given.

Concept introduction:

London Dispersion forces:

London dispersion forces are weak interactions due to the temporary changes in electron density in a molecule. All covalent compound exhibits London dispersion forces. These intermolecular forces are the only intermolecular forces present in nonpolar compounds.

Hydrogen Bonding:

A chemical bond in which a hydrogen atom of one molecule is attracted to an electronegative atom especially a nitrogen, oxygen, or fluorine atom, usually of another molecule.

Dipole-dipole interactions:

Dipole–dipole interactions are electrostatic interactions between molecules which have permanent dipoles. This interaction is stronger than the London forces but is weaker than ion-ion interaction because only partial charges are involved positive end of a polar molecule will attract the negative end of the other molecule and influence its position

(b)

Interpretation Introduction

Interpretation:

The compound, which has higher boiling point, has to be given.

(c)

Interpretation Introduction

Interpretation:

The compound, which has higher melting point, has to be given.

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Answer 5

Chapter 4, Problem 4.59AP

(a)

Interpretation Introduction

Interpretation:

The compound that exhibits weaker intermolecular forces has to be given.

Concept introduction:

London Dispersion forces:

London dispersion forces are weak interactions due to the temporary changes in electron density in a molecule. All covalent compound exhibits London dispersion forces. These intermolecular forces are the only intermolecular forces present in nonpolar compounds.

Hydrogen Bonding:

A chemical bond in which a hydrogen atom of one molecule is attracted to an electronegative atom especially a nitrogen, oxygen, or fluorine atom, usually of another molecule.

Dipole-dipole interactions:

Dipole–dipole interactions are electrostatic interactions between molecules which have permanent dipoles. This interaction is stronger than the London forces but is weaker than ion-ion interaction because only partial charges are involved positive end of a polar molecule will attract the negative end of the other molecule and influence its position

(b)

Interpretation Introduction

Interpretation:

The compound, which has higher boiling point, has to be given.

(c)

Interpretation Introduction

Interpretation:

The compound, which has higher melting point, has to be given.

Answer 6

Chapter 4, Problem 4.59AP

(a)

Interpretation Introduction

Interpretation:

The compound that exhibits weaker intermolecular forces has to be given.

Concept introduction:

London Dispersion forces:

London dispersion forces are weak interactions due to the temporary changes in electron density in a molecule. All covalent compound exhibits London dispersion forces. These intermolecular forces are the only intermolecular forces present in nonpolar compounds.

Hydrogen Bonding:

A chemical bond in which a hydrogen atom of one molecule is attracted to an electronegative atom especially a nitrogen, oxygen, or fluorine atom, usually of another molecule.

Dipole-dipole interactions:

Dipole–dipole interactions are electrostatic interactions between molecules which have permanent dipoles. This interaction is stronger than the London forces but is weaker than ion-ion interaction because only partial charges are involved positive end of a polar molecule will attract the negative end of the other molecule and influence its position

Answer 7

Chapter 4, Problem 4.59AP

(a)

Interpretation Introduction

Interpretation:

The compound that exhibits weaker intermolecular forces has to be given.

Concept introduction:

London Dispersion forces:

London dispersion forces are weak interactions due to the temporary changes in electron density in a molecule. All covalent compound exhibits London dispersion forces. These intermolecular forces are the only intermolecular forces present in nonpolar compounds.

Hydrogen Bonding:

A chemical bond in which a hydrogen atom of one molecule is attracted to an electronegative atom especially a nitrogen, oxygen, or fluorine atom, usually of another molecule.

Dipole-dipole interactions:

Dipole–dipole interactions are electrostatic interactions between molecules which have permanent dipoles. This interaction is stronger than the London forces but is weaker than ion-ion interaction because only partial charges are involved positive end of a polar molecule will attract the negative end of the other molecule and influence its position

Answer 8

(b)

Interpretation Introduction

Interpretation:

The compound, which has higher boiling point, has to be given.

Answer 9

(b)

Interpretation Introduction

Interpretation:

The compound, which has higher boiling point, has to be given.

Answer 10

(c)

Interpretation Introduction

Interpretation:

The compound, which has higher melting point, has to be given.

Answer 11

(c)

Interpretation Introduction

Interpretation:

The compound, which has higher melting point, has to be given.

Answer 12

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Answer 13

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Answer 14

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Answer 15

Ch. 4.1 - Prob. 4.1P Ch. 4.1 - Prob. 4.2P Ch. 4.1 - Prob. 4.3P Ch. 4.1 - Prob. 4.4P Ch. 4.2 - Prob. 4.5P Ch. 4.2 - Prob. 4.6P Ch. 4.3 - Prob. 4.7P Ch. 4.3 - Prob. 4.8P Ch. 4.3 - Prob. 4.9P Ch. 4.3 - Prob. 4.10P

Solution Summary: The author explains that London dispersion forces are weak interactions due to the temporary changes in electron density in a molecule.

Interpretation:

The compound, which has higher boiling point, has to be given.

Interpretation:

The compound, which has higher melting point, has to be given.

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Chapter 4 Solutions

Solution Summary: The author explains that London dispersion forces are weak interactions due to the temporary changes in electron density in a molecule.

Interpretation: The compound, which has higher boiling point, has to be given.

Interpretation: The compound, which has higher melting point, has to be given.

Want to see the full answer?

Chapter 4 Solutions

Interpretation:

The compound, which has higher boiling point, has to be given.

Interpretation:

The compound, which has higher melting point, has to be given.