The type of intermolecular forces present in ethanol and dimethyl ether 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

Question

Want to see the full answer?

Answer 1

Question

Chapter 4, Problem 4.36UKC

(a)

Interpretation Introduction

Interpretation:

The type of intermolecular forces present in ethanol and dimethyl ether 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 compounds with higher boiling points has to be given.

Expert Solution & Answer

Want to see the full answer?

Check out a sample textbook solution

See solution

Students have asked these similar questions

Pick the compound with the highest boiling point in each pair.Explain your reasoning.a. CH3OH or CH3SH

Why does ethanol have a higher boiling point than dimethyl ether despite having the same molecular weight? Because alcohols are polar molecules. Neither Because alcohols show hydrogen bonding. Both

An alcohol has a higher boiling point than an alkane with the same length carbon chain. True or false?

Answer 2

Question

Chapter 4, Problem 4.36UKC

(a)

Interpretation Introduction

Interpretation:

The type of intermolecular forces present in ethanol and dimethyl ether 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 compounds with higher boiling points has to be given.

Expert Solution & Answer

Want to see the full answer?

Check out a sample textbook solution

See solution

Answer 3

Question

Chapter 4, Problem 4.36UKC

(a)

Interpretation Introduction

Interpretation:

The type of intermolecular forces present in ethanol and dimethyl ether 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 compounds with higher boiling points has to be given.

Expert Solution & Answer

Want to see the full answer?

Check out a sample textbook solution

See solution

Answer 4

Question

Chapter 4, Problem 4.36UKC

(a)

Interpretation Introduction

Interpretation:

The type of intermolecular forces present in ethanol and dimethyl ether 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 compounds with higher boiling points has to be given.

Expert Solution & Answer

Want to see the full answer?

Check out a sample textbook solution

See solution

Answer 5

Chapter 4, Problem 4.36UKC

(a)

Interpretation Introduction

Interpretation:

The type of intermolecular forces present in ethanol and dimethyl ether 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 compounds with higher boiling points has to be given.

Answer 6

Chapter 4, Problem 4.36UKC

(a)

Interpretation Introduction

Interpretation:

The type of intermolecular forces present in ethanol and dimethyl ether 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 4.36UKC

(a)

Interpretation Introduction

Interpretation:

The type of intermolecular forces present in ethanol and dimethyl ether 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 compounds with higher boiling points has to be given.

Answer 9

(b)

Interpretation Introduction

Interpretation:

The compounds with higher boiling points has to be given.

Answer 10

Expert Solution & Answer

Answer 11

Expert Solution & Answer

Answer 12

Want to see the full answer?

Check out a sample textbook solution

See solution

Answer 13

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 the type of intermolecular forces present in ethanol and dimethyl ether.

Interpretation:

The compounds with higher boiling points has to be given.

Want to see the full answer?

Chapter 4 Solutions

Solution Summary: The author explains the type of intermolecular forces present in ethanol and dimethyl ether.

Interpretation: The compounds with higher boiling points has to be given.

Want to see the full answer?

Chapter 4 Solutions

Interpretation:

The compounds with higher boiling points has to be given.