The hybrid orbital that will result from the interaction shown is to be derived. Whether the resulting orbital will be different from the ones shown in Figures 3-9a and 3-9b is to be determined. Concept introduction: Orbitals from the same atom can mix to form two or more hybrid orbitals. The number of hybrid orbitals formed is the same as the number of orbitals that mix. When an s and a p orbital mix, they form two hybrid orbitals, oriented at 180 ° . An s orbital has the same phase everywhere. A p orbital, on the other hand, has different phases in the two lobes. Therefore, when an s and a p orbitals mix, they produce hybrid orbitals with unequal lobes. Mixing of the lobe with the same sign as the s orbital leads to constructive interference, increasing the size of the lobe. The other lobe of p orbital has an opposite phase; therefore, its mixing leads to destructive interference on that side. The size of the lobe on this side is smaller than the other lobe. The other hybrid orbital is formed by overlap of the s orbital with the p orbital of reversed phases.

Question

Want to see the full answer?

Answer 1

Question

Chapter 3, Problem 3.5P

Interpretation Introduction

Interpretation:

The hybrid orbital that will result from the interaction shown is to be derived. Whether the resulting orbital will be different from the ones shown in Figures 3-9a and 3-9b is to be determined.

Concept introduction:

Orbitals from the same atom can mix to form two or more hybrid orbitals. The number of hybrid orbitals formed is the same as the number of orbitals that mix. When an s and a p orbital mix, they form two hybrid orbitals, oriented at 180°. An s orbital has the same phase everywhere. A p orbital, on the other hand, has different phases in the two lobes. Therefore, when an s and a p orbitals mix, they produce hybrid orbitals with unequal lobes. Mixing of the lobe with the same sign as the s orbital leads to constructive interference, increasing the size of the lobe. The other lobe of p orbital has an opposite phase; therefore, its mixing leads to destructive interference on that side. The size of the lobe on this side is smaller than the other lobe. The other hybrid orbital is formed by overlap of the s orbital with the p orbital of reversed phases.

Expert Solution & Answer

Want to see the full answer?

Check out a sample textbook solution

See solution

Students have asked these similar questions

4. Provide a clear arrow-pushing mechanism for each of the following reactions. Do not skip proton transfers, do not combine steps, and make sure your arrows are clear enough to be interpreted without ambiguity. a. 2. 1. LDA 3. H3O+ HO

b. H3C CH3 H3O+ ✓ H OH

2. Provide reagents/conditions to accomplish the following syntheses. More than one step is required in some cases. a. CH3

Answer 2

Question

Chapter 3, Problem 3.5P

Interpretation Introduction

Interpretation:

The hybrid orbital that will result from the interaction shown is to be derived. Whether the resulting orbital will be different from the ones shown in Figures 3-9a and 3-9b is to be determined.

Concept introduction:

Orbitals from the same atom can mix to form two or more hybrid orbitals. The number of hybrid orbitals formed is the same as the number of orbitals that mix. When an s and a p orbital mix, they form two hybrid orbitals, oriented at 180°. An s orbital has the same phase everywhere. A p orbital, on the other hand, has different phases in the two lobes. Therefore, when an s and a p orbitals mix, they produce hybrid orbitals with unequal lobes. Mixing of the lobe with the same sign as the s orbital leads to constructive interference, increasing the size of the lobe. The other lobe of p orbital has an opposite phase; therefore, its mixing leads to destructive interference on that side. The size of the lobe on this side is smaller than the other lobe. The other hybrid orbital is formed by overlap of the s orbital with the p orbital of reversed phases.

Expert Solution & Answer

Want to see the full answer?

Check out a sample textbook solution

See solution

Answer 3

Question

Chapter 3, Problem 3.5P

Interpretation Introduction

Interpretation:

The hybrid orbital that will result from the interaction shown is to be derived. Whether the resulting orbital will be different from the ones shown in Figures 3-9a and 3-9b is to be determined.

Concept introduction:

Orbitals from the same atom can mix to form two or more hybrid orbitals. The number of hybrid orbitals formed is the same as the number of orbitals that mix. When an s and a p orbital mix, they form two hybrid orbitals, oriented at 180°. An s orbital has the same phase everywhere. A p orbital, on the other hand, has different phases in the two lobes. Therefore, when an s and a p orbitals mix, they produce hybrid orbitals with unequal lobes. Mixing of the lobe with the same sign as the s orbital leads to constructive interference, increasing the size of the lobe. The other lobe of p orbital has an opposite phase; therefore, its mixing leads to destructive interference on that side. The size of the lobe on this side is smaller than the other lobe. The other hybrid orbital is formed by overlap of the s orbital with the p orbital of reversed phases.

Expert Solution & Answer

Want to see the full answer?

Check out a sample textbook solution

See solution

Answer 4

Question

Chapter 3, Problem 3.5P

Interpretation Introduction

Interpretation:

The hybrid orbital that will result from the interaction shown is to be derived. Whether the resulting orbital will be different from the ones shown in Figures 3-9a and 3-9b is to be determined.

Concept introduction:

Orbitals from the same atom can mix to form two or more hybrid orbitals. The number of hybrid orbitals formed is the same as the number of orbitals that mix. When an s and a p orbital mix, they form two hybrid orbitals, oriented at 180°. An s orbital has the same phase everywhere. A p orbital, on the other hand, has different phases in the two lobes. Therefore, when an s and a p orbitals mix, they produce hybrid orbitals with unequal lobes. Mixing of the lobe with the same sign as the s orbital leads to constructive interference, increasing the size of the lobe. The other lobe of p orbital has an opposite phase; therefore, its mixing leads to destructive interference on that side. The size of the lobe on this side is smaller than the other lobe. The other hybrid orbital is formed by overlap of the s orbital with the p orbital of reversed phases.

Expert Solution & Answer

Want to see the full answer?

Check out a sample textbook solution

See solution

Answer 5

Chapter 3, Problem 3.5P

Interpretation Introduction

Interpretation:

The hybrid orbital that will result from the interaction shown is to be derived. Whether the resulting orbital will be different from the ones shown in Figures 3-9a and 3-9b is to be determined.

Concept introduction:

Orbitals from the same atom can mix to form two or more hybrid orbitals. The number of hybrid orbitals formed is the same as the number of orbitals that mix. When an s and a p orbital mix, they form two hybrid orbitals, oriented at 180°. An s orbital has the same phase everywhere. A p orbital, on the other hand, has different phases in the two lobes. Therefore, when an s and a p orbitals mix, they produce hybrid orbitals with unequal lobes. Mixing of the lobe with the same sign as the s orbital leads to constructive interference, increasing the size of the lobe. The other lobe of p orbital has an opposite phase; therefore, its mixing leads to destructive interference on that side. The size of the lobe on this side is smaller than the other lobe. The other hybrid orbital is formed by overlap of the s orbital with the p orbital of reversed phases.

Answer 6

Chapter 3, Problem 3.5P

Interpretation Introduction

Interpretation:

The hybrid orbital that will result from the interaction shown is to be derived. Whether the resulting orbital will be different from the ones shown in Figures 3-9a and 3-9b is to be determined.

Concept introduction:

Orbitals from the same atom can mix to form two or more hybrid orbitals. The number of hybrid orbitals formed is the same as the number of orbitals that mix. When an s and a p orbital mix, they form two hybrid orbitals, oriented at 180°. An s orbital has the same phase everywhere. A p orbital, on the other hand, has different phases in the two lobes. Therefore, when an s and a p orbitals mix, they produce hybrid orbitals with unequal lobes. Mixing of the lobe with the same sign as the s orbital leads to constructive interference, increasing the size of the lobe. The other lobe of p orbital has an opposite phase; therefore, its mixing leads to destructive interference on that side. The size of the lobe on this side is smaller than the other lobe. The other hybrid orbital is formed by overlap of the s orbital with the p orbital of reversed phases.

Answer 7

Chapter 3, Problem 3.5P

Interpretation Introduction

Interpretation:

The hybrid orbital that will result from the interaction shown is to be derived. Whether the resulting orbital will be different from the ones shown in Figures 3-9a and 3-9b is to be determined.

Concept introduction:

Orbitals from the same atom can mix to form two or more hybrid orbitals. The number of hybrid orbitals formed is the same as the number of orbitals that mix. When an s and a p orbital mix, they form two hybrid orbitals, oriented at 180°. An s orbital has the same phase everywhere. A p orbital, on the other hand, has different phases in the two lobes. Therefore, when an s and a p orbitals mix, they produce hybrid orbitals with unequal lobes. Mixing of the lobe with the same sign as the s orbital leads to constructive interference, increasing the size of the lobe. The other lobe of p orbital has an opposite phase; therefore, its mixing leads to destructive interference on that side. The size of the lobe on this side is smaller than the other lobe. The other hybrid orbital is formed by overlap of the s orbital with the p orbital of reversed phases.

Answer 8

Expert Solution & Answer

Answer 9

Expert Solution & Answer

Answer 10

Want to see the full answer?

Check out a sample textbook solution

See solution

Answer 11

Ch. 3 - Prob. 3.1P Ch. 3 - Prob. 3.2P Ch. 3 - Prob. 3.3P Ch. 3 - Prob. 3.4P Ch. 3 - Prob. 3.5P Ch. 3 - Prob. 3.6P Ch. 3 - Prob. 3.7P Ch. 3 - Prob. 3.8P Ch. 3 - Prob. 3.9P Ch. 3 - Prob. 3.10P

Solution Summary: The author explains that an s and a p orbital can mix to form two or more hybrid orbitals.

Concept explainers

Want to see the full answer?

Chapter 3 Solutions