The bonding in the nitrate ion is to be explained in terms of delocalized molecular orbitals. Concept introduction: According to the valence bond approach, a bond is formed by the overlapping of singly occupied orbitals present on two atoms. A hybrid orbital is formed by the mixing of two or more atomic orbitals. Atomic or hybrid orbitals overlap along the internuclear axis to form a sigma bond, while a sideways overlap of parallel p orbitals forms a pi bond. Two atomic orbitals combine to form a bonding and an antibonding molecular orbital. Orbitals that lie on the internuclear axis combine to form the sigma σ molecular orbital and orbitals parallel to each other combine to form the π molecular orbitals.

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Answer 1

Question

Chapter 9, Problem 66QP

Interpretation Introduction

Interpretation:

The bonding in the nitrate ion is to be explained in terms of delocalized molecular orbitals.

Concept introduction:

According to the valence bond approach, a bond is formed by the overlapping of singly occupied orbitals present on two atoms.

A hybrid orbital is formed by the mixing of two or more atomic orbitals.

Atomic or hybrid orbitals overlap along the internuclear axis to form a sigma bond, while a sideways overlap of parallel p

orbitals forms a pi bond.

Two atomic orbitals combine to form a bonding and an antibonding molecular orbital.

Orbitals that lie on the internuclear axis combine to form the sigma σ

molecular orbital and orbitals parallel to each other combine to form the π molecular orbitals.

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Answer 2

Question

Chapter 9, Problem 66QP

Interpretation Introduction

Interpretation:

The bonding in the nitrate ion is to be explained in terms of delocalized molecular orbitals.

Concept introduction:

According to the valence bond approach, a bond is formed by the overlapping of singly occupied orbitals present on two atoms.

A hybrid orbital is formed by the mixing of two or more atomic orbitals.

Atomic or hybrid orbitals overlap along the internuclear axis to form a sigma bond, while a sideways overlap of parallel p

orbitals forms a pi bond.

Two atomic orbitals combine to form a bonding and an antibonding molecular orbital.

Orbitals that lie on the internuclear axis combine to form the sigma σ

molecular orbital and orbitals parallel to each other combine to form the π molecular orbitals.

Expert Solution & Answer

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Check out a sample textbook solution

See solution

Answer 3

Question

Chapter 9, Problem 66QP

Interpretation Introduction

Interpretation:

The bonding in the nitrate ion is to be explained in terms of delocalized molecular orbitals.

Concept introduction:

According to the valence bond approach, a bond is formed by the overlapping of singly occupied orbitals present on two atoms.

A hybrid orbital is formed by the mixing of two or more atomic orbitals.

Atomic or hybrid orbitals overlap along the internuclear axis to form a sigma bond, while a sideways overlap of parallel p

orbitals forms a pi bond.

Two atomic orbitals combine to form a bonding and an antibonding molecular orbital.

Orbitals that lie on the internuclear axis combine to form the sigma σ

molecular orbital and orbitals parallel to each other combine to form the π molecular orbitals.

Expert Solution & Answer

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Check out a sample textbook solution

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Answer 4

Question

Chapter 9, Problem 66QP

Interpretation Introduction

Interpretation:

The bonding in the nitrate ion is to be explained in terms of delocalized molecular orbitals.

Concept introduction:

According to the valence bond approach, a bond is formed by the overlapping of singly occupied orbitals present on two atoms.

A hybrid orbital is formed by the mixing of two or more atomic orbitals.

Atomic or hybrid orbitals overlap along the internuclear axis to form a sigma bond, while a sideways overlap of parallel p

orbitals forms a pi bond.

Two atomic orbitals combine to form a bonding and an antibonding molecular orbital.

Orbitals that lie on the internuclear axis combine to form the sigma σ

molecular orbital and orbitals parallel to each other combine to form the π molecular orbitals.

Expert Solution & Answer

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Check out a sample textbook solution

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Answer 5

Chapter 9, Problem 66QP

Interpretation Introduction

Interpretation:

The bonding in the nitrate ion is to be explained in terms of delocalized molecular orbitals.

Concept introduction:

According to the valence bond approach, a bond is formed by the overlapping of singly occupied orbitals present on two atoms.

A hybrid orbital is formed by the mixing of two or more atomic orbitals.

Atomic or hybrid orbitals overlap along the internuclear axis to form a sigma bond, while a sideways overlap of parallel p

orbitals forms a pi bond.

Two atomic orbitals combine to form a bonding and an antibonding molecular orbital.

Orbitals that lie on the internuclear axis combine to form the sigma σ

molecular orbital and orbitals parallel to each other combine to form the π molecular orbitals.

Answer 6

Chapter 9, Problem 66QP

Interpretation Introduction

Interpretation:

The bonding in the nitrate ion is to be explained in terms of delocalized molecular orbitals.

Concept introduction:

According to the valence bond approach, a bond is formed by the overlapping of singly occupied orbitals present on two atoms.

A hybrid orbital is formed by the mixing of two or more atomic orbitals.

Atomic or hybrid orbitals overlap along the internuclear axis to form a sigma bond, while a sideways overlap of parallel p

orbitals forms a pi bond.

Two atomic orbitals combine to form a bonding and an antibonding molecular orbital.

Orbitals that lie on the internuclear axis combine to form the sigma σ

molecular orbital and orbitals parallel to each other combine to form the π molecular orbitals.

Answer 7

Chapter 9, Problem 66QP

Interpretation Introduction

Interpretation:

The bonding in the nitrate ion is to be explained in terms of delocalized molecular orbitals.

Concept introduction:

According to the valence bond approach, a bond is formed by the overlapping of singly occupied orbitals present on two atoms.

A hybrid orbital is formed by the mixing of two or more atomic orbitals.

Atomic or hybrid orbitals overlap along the internuclear axis to form a sigma bond, while a sideways overlap of parallel p

orbitals forms a pi bond.

Two atomic orbitals combine to form a bonding and an antibonding molecular orbital.

Orbitals that lie on the internuclear axis combine to form the sigma σ

molecular orbital and orbitals parallel to each other combine to form the π molecular orbitals.

Answer 8

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Answer 9

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Answer 10

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Answer 11

Ch. 9.1 - Practice Problem ATTEMPT Determine the shapes of...Ch. 9.1 - Prob. 1PPB Ch. 9.1 - Prob. 1PPC Ch. 9.1 - 9.1.1 What are the electron-domain geometry and...Ch. 9.1 - What are the electron-domain geometry and...Ch. 9.1 - Prob. 3CP Ch. 9.1 - Prob. 4CP Ch. 9.1 - Prob. 5CP Ch. 9.2 - Practice Problem ATTEMPT Ethanolamine has a...Ch. 9.2 - Practice Problem BUILD The bond angle in is...

Solution Summary: The author explains the bonding in the nitrate ion in terms of delocalized molecular orbitals.

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