(a) Interpretation: The dominant intermolecular force between a pair of helium atoms and a pair H 2 molecule is to be determined. Concept introduction: The dominant intermolecular interaction between non-polar molecules is called induced dipole-induced dipole interaction or London dispersion forces. In a molecule, electrons are constantly moving around, and at some instant in time, there may be more electrons on one side of the molecule than there are on the other. The extra electrons on that one side gives rise to instantaneous dipole which can alter the electron distribution on a second molecule by repelling or attracting nearby electrons. This instantaneous dipole is directly proportional to the number of electrons possessed by the molecule that is on the molar mass.

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Answer 1

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Chapter 2, Problem 2.47P

Interpretation Introduction

(a)

Interpretation:

The dominant intermolecular force between a pair of helium atoms and a pair H2 molecule is to be determined.

Concept introduction:

The dominant intermolecular interaction between non-polar molecules is called induced dipole-induced dipole interaction or London dispersion forces. In a molecule, electrons are constantly moving around, and at some instant in time, there may be more electrons on one side of the molecule than there are on the other. The extra electrons on that one side gives rise to instantaneous dipole which can alter the electron distribution on a second molecule by repelling or attracting nearby electrons. This instantaneous dipole is directly proportional to the number of electrons possessed by the molecule that is on the molar mass.

Interpretation Introduction

(b)

Interpretation:

Why H2 has a higher boiling point than helium is to be explained.

Concept introduction:

The boiling point of a compound depends on the strength of the intermolecular forces that exist between molecules. Boiling point is the energy required to break the bonds to change the state of a given molecule. The molecules with more surface area require more energy to break the bonds than the molecules with less surface area.

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C This question shows how molecular orbital (MO) theory can be used to understand the chemical properties of elemental oxygen O₂ and its anionic derivative superoxide Oz. a) Draw the MO energy diagram for both O2 and O2. Clearly label your diagram with atomic orbital names and molecular orbital symmetry labels and include electrons. Draw the Lewis structure of O2. How does the MO description of O2 differ from the Lewis structure, and how does this difference relate to the high reactivity and magnetic properties of oxygen? ) Use the MO diagram in (a) to explain the difference in bond length and bond energy between superoxide ion (Oz, 135 pm, 360 kJ/mol) and oxygen (O2, 120.8 pm, 494 kJ/mol).

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Answer 2

Question

Chapter 2, Problem 2.47P

Interpretation Introduction

(a)

Interpretation:

The dominant intermolecular force between a pair of helium atoms and a pair H2 molecule is to be determined.

Concept introduction:

The dominant intermolecular interaction between non-polar molecules is called induced dipole-induced dipole interaction or London dispersion forces. In a molecule, electrons are constantly moving around, and at some instant in time, there may be more electrons on one side of the molecule than there are on the other. The extra electrons on that one side gives rise to instantaneous dipole which can alter the electron distribution on a second molecule by repelling or attracting nearby electrons. This instantaneous dipole is directly proportional to the number of electrons possessed by the molecule that is on the molar mass.

Interpretation Introduction

(b)

Interpretation:

Why H2 has a higher boiling point than helium is to be explained.

Concept introduction:

The boiling point of a compound depends on the strength of the intermolecular forces that exist between molecules. Boiling point is the energy required to break the bonds to change the state of a given molecule. The molecules with more surface area require more energy to break the bonds than the molecules with less surface area.

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Answer 3

Question

Chapter 2, Problem 2.47P

Interpretation Introduction

(a)

Interpretation:

The dominant intermolecular force between a pair of helium atoms and a pair H2 molecule is to be determined.

Concept introduction:

The dominant intermolecular interaction between non-polar molecules is called induced dipole-induced dipole interaction or London dispersion forces. In a molecule, electrons are constantly moving around, and at some instant in time, there may be more electrons on one side of the molecule than there are on the other. The extra electrons on that one side gives rise to instantaneous dipole which can alter the electron distribution on a second molecule by repelling or attracting nearby electrons. This instantaneous dipole is directly proportional to the number of electrons possessed by the molecule that is on the molar mass.

Interpretation Introduction

(b)

Interpretation:

Why H2 has a higher boiling point than helium is to be explained.

Concept introduction:

The boiling point of a compound depends on the strength of the intermolecular forces that exist between molecules. Boiling point is the energy required to break the bonds to change the state of a given molecule. The molecules with more surface area require more energy to break the bonds than the molecules with less surface area.

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Answer 4

Question

Chapter 2, Problem 2.47P

Interpretation Introduction

(a)

Interpretation:

The dominant intermolecular force between a pair of helium atoms and a pair H2 molecule is to be determined.

Concept introduction:

The dominant intermolecular interaction between non-polar molecules is called induced dipole-induced dipole interaction or London dispersion forces. In a molecule, electrons are constantly moving around, and at some instant in time, there may be more electrons on one side of the molecule than there are on the other. The extra electrons on that one side gives rise to instantaneous dipole which can alter the electron distribution on a second molecule by repelling or attracting nearby electrons. This instantaneous dipole is directly proportional to the number of electrons possessed by the molecule that is on the molar mass.

Interpretation Introduction

(b)

Interpretation:

Why H2 has a higher boiling point than helium is to be explained.

Concept introduction:

The boiling point of a compound depends on the strength of the intermolecular forces that exist between molecules. Boiling point is the energy required to break the bonds to change the state of a given molecule. The molecules with more surface area require more energy to break the bonds than the molecules with less surface area.

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Answer 5

Chapter 2, Problem 2.47P

Interpretation Introduction

(a)

Interpretation:

The dominant intermolecular force between a pair of helium atoms and a pair H2 molecule is to be determined.

Concept introduction:

The dominant intermolecular interaction between non-polar molecules is called induced dipole-induced dipole interaction or London dispersion forces. In a molecule, electrons are constantly moving around, and at some instant in time, there may be more electrons on one side of the molecule than there are on the other. The extra electrons on that one side gives rise to instantaneous dipole which can alter the electron distribution on a second molecule by repelling or attracting nearby electrons. This instantaneous dipole is directly proportional to the number of electrons possessed by the molecule that is on the molar mass.

Interpretation Introduction

(b)

Interpretation:

Why H2 has a higher boiling point than helium is to be explained.

Concept introduction:

The boiling point of a compound depends on the strength of the intermolecular forces that exist between molecules. Boiling point is the energy required to break the bonds to change the state of a given molecule. The molecules with more surface area require more energy to break the bonds than the molecules with less surface area.

Answer 6

Chapter 2, Problem 2.47P

Interpretation Introduction

(a)

Interpretation:

The dominant intermolecular force between a pair of helium atoms and a pair H2 molecule is to be determined.

Concept introduction:

The dominant intermolecular interaction between non-polar molecules is called induced dipole-induced dipole interaction or London dispersion forces. In a molecule, electrons are constantly moving around, and at some instant in time, there may be more electrons on one side of the molecule than there are on the other. The extra electrons on that one side gives rise to instantaneous dipole which can alter the electron distribution on a second molecule by repelling or attracting nearby electrons. This instantaneous dipole is directly proportional to the number of electrons possessed by the molecule that is on the molar mass.

Answer 7

Chapter 2, Problem 2.47P

Interpretation Introduction

(a)

Interpretation:

The dominant intermolecular force between a pair of helium atoms and a pair H2 molecule is to be determined.

Concept introduction:

The dominant intermolecular interaction between non-polar molecules is called induced dipole-induced dipole interaction or London dispersion forces. In a molecule, electrons are constantly moving around, and at some instant in time, there may be more electrons on one side of the molecule than there are on the other. The extra electrons on that one side gives rise to instantaneous dipole which can alter the electron distribution on a second molecule by repelling or attracting nearby electrons. This instantaneous dipole is directly proportional to the number of electrons possessed by the molecule that is on the molar mass.

Answer 8

Interpretation Introduction

(b)

Interpretation:

Why H2 has a higher boiling point than helium is to be explained.

Concept introduction:

The boiling point of a compound depends on the strength of the intermolecular forces that exist between molecules. Boiling point is the energy required to break the bonds to change the state of a given molecule. The molecules with more surface area require more energy to break the bonds than the molecules with less surface area.

Answer 9

Interpretation Introduction

(b)

Interpretation:

Why H2 has a higher boiling point than helium is to be explained.

Concept introduction:

The boiling point of a compound depends on the strength of the intermolecular forces that exist between molecules. Boiling point is the energy required to break the bonds to change the state of a given molecule. The molecules with more surface area require more energy to break the bonds than the molecules with less surface area.

Answer 10

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Answer 11

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Answer 12

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Answer 13

Ch. 2 - Prob. 2.1P Ch. 2 - Prob. 2.2P Ch. 2 - Prob. 2.3P Ch. 2 - Prob. 2.4P Ch. 2 - Prob. 2.5P Ch. 2 - Prob. 2.6P Ch. 2 - Prob. 2.7P Ch. 2 - Prob. 2.8P Ch. 2 - Prob. 2.9P Ch. 2 - Prob. 2.10P

Solution Summary: The author explains that the dominant intermolecular force between helium and hydrogen is called induced dipole interaction or London dispersion forces.

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