Why benzene fails to react under the given reaction conditions has to be explained. Concept Introduction: Radical reaction: It is reacting to electron octet of valence shell. A radical can break a bond in another molecular and abstract a partner with an electron, giving substitution in the original molecule. A radical can added to an alkene to given a new radical causing an addition reaction. Radical chain reaction: Initiation reaction: Chain propagation: Chain termination: Bond dissociation energy is a measure of bond strength in a chemical bond . It is a change in enthalpy of a hemolysis reaction at absolute zero where a molecule is broken down into two free radicals.

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Answer 1

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Formula Formula Bond dissociation energy (BDE) is the energy required to break a bond, making it an endothermic process. BDE is calculated for a particular bond and therefore consists of fragments such as radicals since it undergoes homolytic bond cleavage. For the homolysis of a X-Y molecule, the energy of bond dissociation is calculated as the difference in the total enthalpy of formation for the reactants and products. X-Y → X + Y BDE = Δ H f X + Δ H f Y – Δ H f X-Y where, ΔHf is the heat of formation.

Chapter 21, Problem 21.44P

(a)

Interpretation Introduction

Interpretation:

Why benzene fails to react under the given reaction conditions has to be explained.

Concept Introduction:

Radical reaction: It is reacting to electron octet of valence shell.

A radical can break a bond in another molecular and abstract a partner with an electron, giving substitution in the original molecule.

A radical can added to an alkene to given a new radical causing an addition reaction.

Radical chain reaction:

Initiation reaction:

Chain propagation:

Chain termination:

Bond dissociation energy is a measure of bond strength in a chemical bond.

It is a change in enthalpy of a hemolysis reaction at absolute zero where a molecule is broken down into two free radicals.

(b)

Interpretation Introduction

Interpretation:

Why the bond dissociation enthalpy of a C-H bond in benzene is significantly greater than that in alkanes, has to be explained.

Concept Introduction:

Hybridization: It is the mixing atomic orbitals into new hybrid orbitals with different energies, shapes, etc., than the component atomic orbitals suitable for the paring of electrons to from chemical bonds in valance bond theory.

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Biphenyl has the following structure.(a) Is biphenyl a (fused) polynuclear aromatic hydrocarbon?(b) How many pi electrons are there in the two aromatic rings of biphenyl? How does this number compare with that for naphthalene?(c) The heat of hydrogenation for biphenyl is about 418 kJ>mol (100 kcal>mol). Calculate theresonance energy of biphenyl.(d) Compare the resonance energy of biphenyl with that of naphthalene and with that of two benzene rings. Explain thedifference in the resonance energies of naphthalene and biphenyl.

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Answer 2

Question

Formula Formula Bond dissociation energy (BDE) is the energy required to break a bond, making it an endothermic process. BDE is calculated for a particular bond and therefore consists of fragments such as radicals since it undergoes homolytic bond cleavage. For the homolysis of a X-Y molecule, the energy of bond dissociation is calculated as the difference in the total enthalpy of formation for the reactants and products. X-Y → X + Y BDE = Δ H f X + Δ H f Y – Δ H f X-Y where, ΔHf is the heat of formation.

Chapter 21, Problem 21.44P

(a)

Interpretation Introduction

Interpretation:

Why benzene fails to react under the given reaction conditions has to be explained.

Concept Introduction:

Radical reaction: It is reacting to electron octet of valence shell.

A radical can break a bond in another molecular and abstract a partner with an electron, giving substitution in the original molecule.

A radical can added to an alkene to given a new radical causing an addition reaction.

Radical chain reaction:

Initiation reaction:

Chain propagation:

Chain termination:

Bond dissociation energy is a measure of bond strength in a chemical bond.

It is a change in enthalpy of a hemolysis reaction at absolute zero where a molecule is broken down into two free radicals.

(b)

Interpretation Introduction

Interpretation:

Why the bond dissociation enthalpy of a C-H bond in benzene is significantly greater than that in alkanes, has to be explained.

Concept Introduction:

Hybridization: It is the mixing atomic orbitals into new hybrid orbitals with different energies, shapes, etc., than the component atomic orbitals suitable for the paring of electrons to from chemical bonds in valance bond theory.

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Answer 3

Question

Formula Formula Bond dissociation energy (BDE) is the energy required to break a bond, making it an endothermic process. BDE is calculated for a particular bond and therefore consists of fragments such as radicals since it undergoes homolytic bond cleavage. For the homolysis of a X-Y molecule, the energy of bond dissociation is calculated as the difference in the total enthalpy of formation for the reactants and products. X-Y → X + Y BDE = Δ H f X + Δ H f Y – Δ H f X-Y where, ΔHf is the heat of formation.

Chapter 21, Problem 21.44P

(a)

Interpretation Introduction

Interpretation:

Why benzene fails to react under the given reaction conditions has to be explained.

Concept Introduction:

Radical reaction: It is reacting to electron octet of valence shell.

A radical can break a bond in another molecular and abstract a partner with an electron, giving substitution in the original molecule.

A radical can added to an alkene to given a new radical causing an addition reaction.

Radical chain reaction:

Initiation reaction:

Chain propagation:

Chain termination:

Bond dissociation energy is a measure of bond strength in a chemical bond.

It is a change in enthalpy of a hemolysis reaction at absolute zero where a molecule is broken down into two free radicals.

(b)

Interpretation Introduction

Interpretation:

Why the bond dissociation enthalpy of a C-H bond in benzene is significantly greater than that in alkanes, has to be explained.

Concept Introduction:

Hybridization: It is the mixing atomic orbitals into new hybrid orbitals with different energies, shapes, etc., than the component atomic orbitals suitable for the paring of electrons to from chemical bonds in valance bond theory.

Expert Solution & Answer

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Answer 4

Question

Formula Formula Bond dissociation energy (BDE) is the energy required to break a bond, making it an endothermic process. BDE is calculated for a particular bond and therefore consists of fragments such as radicals since it undergoes homolytic bond cleavage. For the homolysis of a X-Y molecule, the energy of bond dissociation is calculated as the difference in the total enthalpy of formation for the reactants and products. X-Y → X + Y BDE = Δ H f X + Δ H f Y – Δ H f X-Y where, ΔHf is the heat of formation.

Chapter 21, Problem 21.44P

(a)

Interpretation Introduction

Interpretation:

Why benzene fails to react under the given reaction conditions has to be explained.

Concept Introduction:

Radical reaction: It is reacting to electron octet of valence shell.

A radical can break a bond in another molecular and abstract a partner with an electron, giving substitution in the original molecule.

A radical can added to an alkene to given a new radical causing an addition reaction.

Radical chain reaction:

Initiation reaction:

Chain propagation:

Chain termination:

Bond dissociation energy is a measure of bond strength in a chemical bond.

It is a change in enthalpy of a hemolysis reaction at absolute zero where a molecule is broken down into two free radicals.

(b)

Interpretation Introduction

Interpretation:

Why the bond dissociation enthalpy of a C-H bond in benzene is significantly greater than that in alkanes, has to be explained.

Concept Introduction:

Hybridization: It is the mixing atomic orbitals into new hybrid orbitals with different energies, shapes, etc., than the component atomic orbitals suitable for the paring of electrons to from chemical bonds in valance bond theory.

Expert Solution & Answer

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Answer 5

Chapter 21, Problem 21.44P

(a)

Interpretation Introduction

Interpretation:

Why benzene fails to react under the given reaction conditions has to be explained.

Concept Introduction:

Radical reaction: It is reacting to electron octet of valence shell.

A radical can break a bond in another molecular and abstract a partner with an electron, giving substitution in the original molecule.

A radical can added to an alkene to given a new radical causing an addition reaction.

Radical chain reaction:

Initiation reaction:

Chain propagation:

Chain termination:

Bond dissociation energy is a measure of bond strength in a chemical bond.

It is a change in enthalpy of a hemolysis reaction at absolute zero where a molecule is broken down into two free radicals.

(b)

Interpretation Introduction

Interpretation:

Why the bond dissociation enthalpy of a C-H bond in benzene is significantly greater than that in alkanes, has to be explained.

Concept Introduction:

Hybridization: It is the mixing atomic orbitals into new hybrid orbitals with different energies, shapes, etc., than the component atomic orbitals suitable for the paring of electrons to from chemical bonds in valance bond theory.

Answer 6

Chapter 21, Problem 21.44P

(a)

Interpretation Introduction

Interpretation:

Why benzene fails to react under the given reaction conditions has to be explained.

Concept Introduction:

Radical reaction: It is reacting to electron octet of valence shell.

A radical can break a bond in another molecular and abstract a partner with an electron, giving substitution in the original molecule.

A radical can added to an alkene to given a new radical causing an addition reaction.

Radical chain reaction:

Initiation reaction:

Chain propagation:

Chain termination:

Bond dissociation energy is a measure of bond strength in a chemical bond.

It is a change in enthalpy of a hemolysis reaction at absolute zero where a molecule is broken down into two free radicals.

Answer 7

Chapter 21, Problem 21.44P

(a)

Interpretation Introduction

Interpretation:

Why benzene fails to react under the given reaction conditions has to be explained.

Concept Introduction:

Radical reaction: It is reacting to electron octet of valence shell.

A radical can break a bond in another molecular and abstract a partner with an electron, giving substitution in the original molecule.

A radical can added to an alkene to given a new radical causing an addition reaction.

Radical chain reaction:

Initiation reaction:

Chain propagation:

Chain termination:

Bond dissociation energy is a measure of bond strength in a chemical bond.

It is a change in enthalpy of a hemolysis reaction at absolute zero where a molecule is broken down into two free radicals.

Answer 8

(b)

Interpretation Introduction

Interpretation:

Why the bond dissociation enthalpy of a C-H bond in benzene is significantly greater than that in alkanes, has to be explained.

Concept Introduction:

Hybridization: It is the mixing atomic orbitals into new hybrid orbitals with different energies, shapes, etc., than the component atomic orbitals suitable for the paring of electrons to from chemical bonds in valance bond theory.

Answer 9

(b)

Interpretation Introduction

Interpretation:

Why the bond dissociation enthalpy of a C-H bond in benzene is significantly greater than that in alkanes, has to be explained.

Concept Introduction:

Hybridization: It is the mixing atomic orbitals into new hybrid orbitals with different energies, shapes, etc., than the component atomic orbitals suitable for the paring of electrons to from chemical bonds in valance bond theory.

Answer 10

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Answer 12

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Answer 13

Ch. 21.2 - Construct a Frost circle for a planar...Ch. 21.2 - Which compound gives a signal in the 1H-NMR...Ch. 21.2 - Prob. 21.3P Ch. 21.2 - Prob. 21.4P Ch. 21.3 - Prob. 21.5P Ch. 21.4 - Arrange these compounds in order of increasing...Ch. 21.4 - Prob. AQ Ch. 21.4 - Prob. BQ Ch. 21.4 - Prob. CQ Ch. 21.5 - Prob. 21.7P

Solution Summary: The author explains how the bond dissociation enthalpy of a C-H bond in benzene is significantly greater than that in alkanes.

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