The hybridization of each carbon and oxygen atom in aspirin is to be determined. Concept introduction: Hybridization is the process of intermixing of atomic orbital of slightly different energies to form hybrid orbitals that have similar energy. These orbital have lower energy and more stability than the atomic orbital. Hybridization of the central atom can be determined from the number of electron groups around the central atom in the Lewis structure of the molecule. Single bond, double bond, triple bond and lone pair all are considered as single electron group.

Question

Want to see the full answer?

Answer 1

Question

Chapter 11, Problem 11.56P

(a)

Interpretation Introduction

Interpretation:

The hybridization of each carbon and oxygen atom in aspirin is to be determined.

Concept introduction:

Hybridization is the process of intermixing of atomic orbital of slightly different energies to form hybrid orbitals that have similar energy. These orbital have lower energy and more stability than the atomic orbital.

Hybridization of the central atom can be determined from the number of electron groups around the central atom in the Lewis structure of the molecule. Single bond, double bond, triple bond and lone pair all are considered as single electron group.

(b)

Interpretation Introduction

Interpretation:

The number of localized pi bonds in aspirin is to be determined.

Concept introduction:

The sigma bond is the covalent bond that is formed by the axial overlap of orbitals. The pi bond is formed by the lateral overlap of orbitals. Both types of bonds can be bonding or anti-bonding interaction. Bonding interaction takes place when there is an overlap of orbitals in the same phase and antibonding interaction occurs when the orbital overlap in opposite phase. Sigma bond is stronger than the pi bond.

All single bonds are sigma bonds. One double bond is made up of one sigma bond and one pi bond. One triple bond is made up of one sigma bond and two pi bonds.

(c)

Interpretation Introduction

Interpretation:

The number of carbon atoms that have a trigonal planar shape and a tetrahedral shape is to be determined.

Concept introduction:

Hybridization is the process of intermixing of atomic orbital of slightly different energies to form hybrid orbitals that have similar energy. These orbital have lower energy and more stability than the atomic orbital.

Hybridization of the central atom can be determined from the number of electron groups around the central atom in the Lewis structure of the molecule. Single bond, double bond, triple bond and lone pair all are considered as single electron group.

Expert Solution & Answer

Want to see the full answer?

Check out a sample textbook solution

See solution

Students have asked these similar questions

Show work. don't give Ai generated solution. Don't copy the answer anywhere

6. Consider the following exothermic reaction below. 2Cu2+(aq) +41 (aq)2Cul(s) + 12(aq) a. If Cul is added, there will be a shift left/shift right/no shift (circle one). b. If Cu2+ is added, there will be a shift left/shift right/no shift (circle one). c. If a solution of AgNO3 is added, there will be a shift left/shift right/no shift (circle one). d. If the solvent hexane (C6H14) is added, there will be a shift left/shift right/no shift (circle one). Hint: one of the reaction species is more soluble in hexane than in water. e. If the reaction is cooled, there will be a shift left/shift right/no shift (circle one). f. Which of the changes above will change the equilibrium constant, K?

Show work. don't give Ai

Answer 2

Question

Chapter 11, Problem 11.56P

(a)

Interpretation Introduction

Interpretation:

The hybridization of each carbon and oxygen atom in aspirin is to be determined.

Concept introduction:

Hybridization is the process of intermixing of atomic orbital of slightly different energies to form hybrid orbitals that have similar energy. These orbital have lower energy and more stability than the atomic orbital.

Hybridization of the central atom can be determined from the number of electron groups around the central atom in the Lewis structure of the molecule. Single bond, double bond, triple bond and lone pair all are considered as single electron group.

(b)

Interpretation Introduction

Interpretation:

The number of localized pi bonds in aspirin is to be determined.

Concept introduction:

The sigma bond is the covalent bond that is formed by the axial overlap of orbitals. The pi bond is formed by the lateral overlap of orbitals. Both types of bonds can be bonding or anti-bonding interaction. Bonding interaction takes place when there is an overlap of orbitals in the same phase and antibonding interaction occurs when the orbital overlap in opposite phase. Sigma bond is stronger than the pi bond.

All single bonds are sigma bonds. One double bond is made up of one sigma bond and one pi bond. One triple bond is made up of one sigma bond and two pi bonds.

(c)

Interpretation Introduction

Interpretation:

The number of carbon atoms that have a trigonal planar shape and a tetrahedral shape is to be determined.

Concept introduction:

Hybridization is the process of intermixing of atomic orbital of slightly different energies to form hybrid orbitals that have similar energy. These orbital have lower energy and more stability than the atomic orbital.

Hybridization of the central atom can be determined from the number of electron groups around the central atom in the Lewis structure of the molecule. Single bond, double bond, triple bond and lone pair all are considered as single electron group.

Expert Solution & Answer

Want to see the full answer?

Check out a sample textbook solution

See solution

Answer 3

Question

Chapter 11, Problem 11.56P

(a)

Interpretation Introduction

Interpretation:

The hybridization of each carbon and oxygen atom in aspirin is to be determined.

Concept introduction:

Hybridization is the process of intermixing of atomic orbital of slightly different energies to form hybrid orbitals that have similar energy. These orbital have lower energy and more stability than the atomic orbital.

Hybridization of the central atom can be determined from the number of electron groups around the central atom in the Lewis structure of the molecule. Single bond, double bond, triple bond and lone pair all are considered as single electron group.

(b)

Interpretation Introduction

Interpretation:

The number of localized pi bonds in aspirin is to be determined.

Concept introduction:

The sigma bond is the covalent bond that is formed by the axial overlap of orbitals. The pi bond is formed by the lateral overlap of orbitals. Both types of bonds can be bonding or anti-bonding interaction. Bonding interaction takes place when there is an overlap of orbitals in the same phase and antibonding interaction occurs when the orbital overlap in opposite phase. Sigma bond is stronger than the pi bond.

All single bonds are sigma bonds. One double bond is made up of one sigma bond and one pi bond. One triple bond is made up of one sigma bond and two pi bonds.

(c)

Interpretation Introduction

Interpretation:

The number of carbon atoms that have a trigonal planar shape and a tetrahedral shape is to be determined.

Concept introduction:

Hybridization is the process of intermixing of atomic orbital of slightly different energies to form hybrid orbitals that have similar energy. These orbital have lower energy and more stability than the atomic orbital.

Hybridization of the central atom can be determined from the number of electron groups around the central atom in the Lewis structure of the molecule. Single bond, double bond, triple bond and lone pair all are considered as single electron group.

Expert Solution & Answer

Want to see the full answer?

Check out a sample textbook solution

See solution

Answer 4

Question

Chapter 11, Problem 11.56P

(a)

Interpretation Introduction

Interpretation:

The hybridization of each carbon and oxygen atom in aspirin is to be determined.

Concept introduction:

Hybridization is the process of intermixing of atomic orbital of slightly different energies to form hybrid orbitals that have similar energy. These orbital have lower energy and more stability than the atomic orbital.

Hybridization of the central atom can be determined from the number of electron groups around the central atom in the Lewis structure of the molecule. Single bond, double bond, triple bond and lone pair all are considered as single electron group.

(b)

Interpretation Introduction

Interpretation:

The number of localized pi bonds in aspirin is to be determined.

Concept introduction:

The sigma bond is the covalent bond that is formed by the axial overlap of orbitals. The pi bond is formed by the lateral overlap of orbitals. Both types of bonds can be bonding or anti-bonding interaction. Bonding interaction takes place when there is an overlap of orbitals in the same phase and antibonding interaction occurs when the orbital overlap in opposite phase. Sigma bond is stronger than the pi bond.

All single bonds are sigma bonds. One double bond is made up of one sigma bond and one pi bond. One triple bond is made up of one sigma bond and two pi bonds.

(c)

Interpretation Introduction

Interpretation:

The number of carbon atoms that have a trigonal planar shape and a tetrahedral shape is to be determined.

Concept introduction:

Hybridization is the process of intermixing of atomic orbital of slightly different energies to form hybrid orbitals that have similar energy. These orbital have lower energy and more stability than the atomic orbital.

Hybridization of the central atom can be determined from the number of electron groups around the central atom in the Lewis structure of the molecule. Single bond, double bond, triple bond and lone pair all are considered as single electron group.

Expert Solution & Answer

Want to see the full answer?

Check out a sample textbook solution

See solution

Answer 5

Chapter 11, Problem 11.56P

(a)

Interpretation Introduction

Interpretation:

The hybridization of each carbon and oxygen atom in aspirin is to be determined.

Concept introduction:

Hybridization is the process of intermixing of atomic orbital of slightly different energies to form hybrid orbitals that have similar energy. These orbital have lower energy and more stability than the atomic orbital.

Hybridization of the central atom can be determined from the number of electron groups around the central atom in the Lewis structure of the molecule. Single bond, double bond, triple bond and lone pair all are considered as single electron group.

(b)

Interpretation Introduction

Interpretation:

The number of localized pi bonds in aspirin is to be determined.

Concept introduction:

The sigma bond is the covalent bond that is formed by the axial overlap of orbitals. The pi bond is formed by the lateral overlap of orbitals. Both types of bonds can be bonding or anti-bonding interaction. Bonding interaction takes place when there is an overlap of orbitals in the same phase and antibonding interaction occurs when the orbital overlap in opposite phase. Sigma bond is stronger than the pi bond.

All single bonds are sigma bonds. One double bond is made up of one sigma bond and one pi bond. One triple bond is made up of one sigma bond and two pi bonds.

(c)

Interpretation Introduction

Interpretation:

The number of carbon atoms that have a trigonal planar shape and a tetrahedral shape is to be determined.

Concept introduction:

Hybridization is the process of intermixing of atomic orbital of slightly different energies to form hybrid orbitals that have similar energy. These orbital have lower energy and more stability than the atomic orbital.

Hybridization of the central atom can be determined from the number of electron groups around the central atom in the Lewis structure of the molecule. Single bond, double bond, triple bond and lone pair all are considered as single electron group.

Answer 6

Chapter 11, Problem 11.56P

(a)

Interpretation Introduction

Interpretation:

The hybridization of each carbon and oxygen atom in aspirin is to be determined.

Concept introduction:

Hybridization is the process of intermixing of atomic orbital of slightly different energies to form hybrid orbitals that have similar energy. These orbital have lower energy and more stability than the atomic orbital.

Hybridization of the central atom can be determined from the number of electron groups around the central atom in the Lewis structure of the molecule. Single bond, double bond, triple bond and lone pair all are considered as single electron group.

Answer 7

Chapter 11, Problem 11.56P

(a)

Interpretation Introduction

Interpretation:

The hybridization of each carbon and oxygen atom in aspirin is to be determined.

Concept introduction:

Hybridization is the process of intermixing of atomic orbital of slightly different energies to form hybrid orbitals that have similar energy. These orbital have lower energy and more stability than the atomic orbital.

Hybridization of the central atom can be determined from the number of electron groups around the central atom in the Lewis structure of the molecule. Single bond, double bond, triple bond and lone pair all are considered as single electron group.

Answer 8

(b)

Interpretation Introduction

Interpretation:

The number of localized pi bonds in aspirin is to be determined.

Concept introduction:

The sigma bond is the covalent bond that is formed by the axial overlap of orbitals. The pi bond is formed by the lateral overlap of orbitals. Both types of bonds can be bonding or anti-bonding interaction. Bonding interaction takes place when there is an overlap of orbitals in the same phase and antibonding interaction occurs when the orbital overlap in opposite phase. Sigma bond is stronger than the pi bond.

All single bonds are sigma bonds. One double bond is made up of one sigma bond and one pi bond. One triple bond is made up of one sigma bond and two pi bonds.

Answer 9

(b)

Interpretation Introduction

Interpretation:

The number of localized pi bonds in aspirin is to be determined.

Concept introduction:

The sigma bond is the covalent bond that is formed by the axial overlap of orbitals. The pi bond is formed by the lateral overlap of orbitals. Both types of bonds can be bonding or anti-bonding interaction. Bonding interaction takes place when there is an overlap of orbitals in the same phase and antibonding interaction occurs when the orbital overlap in opposite phase. Sigma bond is stronger than the pi bond.

All single bonds are sigma bonds. One double bond is made up of one sigma bond and one pi bond. One triple bond is made up of one sigma bond and two pi bonds.

Answer 10

(c)

Interpretation Introduction

Interpretation:

The number of carbon atoms that have a trigonal planar shape and a tetrahedral shape is to be determined.

Concept introduction:

Hybridization is the process of intermixing of atomic orbital of slightly different energies to form hybrid orbitals that have similar energy. These orbital have lower energy and more stability than the atomic orbital.

Hybridization of the central atom can be determined from the number of electron groups around the central atom in the Lewis structure of the molecule. Single bond, double bond, triple bond and lone pair all are considered as single electron group.

Answer 11

(c)

Interpretation Introduction

Interpretation:

The number of carbon atoms that have a trigonal planar shape and a tetrahedral shape is to be determined.

Concept introduction:

Hybridization is the process of intermixing of atomic orbital of slightly different energies to form hybrid orbitals that have similar energy. These orbital have lower energy and more stability than the atomic orbital.

Hybridization of the central atom can be determined from the number of electron groups around the central atom in the Lewis structure of the molecule. Single bond, double bond, triple bond and lone pair all are considered as single electron group.

Answer 12

Expert Solution & Answer

Answer 13

Expert Solution & Answer

Answer 14

Want to see the full answer?

Check out a sample textbook solution

See solution

Answer 15

Ch. 11.1 - What is the hybridization of the central atom in...Ch. 11.1 - Prob. 11.1BFP Ch. 11.2 - Prob. 11.2AFP Ch. 11.2 - Prob. 11.2BFP Ch. 11.3 - Prob. 11.3AFP Ch. 11.3 - Prob. 11.3BFP Ch. 11.3 - Prob. 11.4AFP Ch. 11.3 - Prob. 11.4BFP Ch. 11 - Prob. 11.1P Ch. 11 - What is the orbital hybridization of a central...

Concept explainers

Videos

Want to see the full answer?

Chapter 11 Solutions