The C-H bonds of Trans-3-hexene are to be ranked in the order of decreasing bond dissociation enthalpy. Concept introduction: Bond dissociation enthalpy is the amount of energy required to break a covalent bond. The stronger the bond, the higher the bond dissociation enthalpy. The C-H bond in alkenes is stronger than the C-H bond in alkanes. The sp 2 -hybridized carbon atoms have stronger C-H bonds than C-H bonds in sp 3 -hybridized carbon atoms. Allylic C-H bonds are weaker than non-allylic (alkyl) C-H bonds.

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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 11.3, Problem 7P

Interpretation Introduction

Interpretation:

The C-H bonds of Trans-3-hexene are to be ranked in the order of decreasing bond dissociation enthalpy.

Concept introduction:

Bond dissociation enthalpy is the amount of energy required to break a covalent bond.

The stronger the bond, the higher the bond dissociation enthalpy.

The C-H

bond in alkenes is stronger than the C-H

bond in alkanes. The sp2-hybridized carbon atoms have stronger C-H

bonds than C-H

bonds in sp3-hybridized carbon atoms.

Allylic C-H bonds are weaker than non-allylic (alkyl) C-H bonds.

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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 11.3, Problem 7P

Interpretation Introduction

Interpretation:

The C-H bonds of Trans-3-hexene are to be ranked in the order of decreasing bond dissociation enthalpy.

Concept introduction:

Bond dissociation enthalpy is the amount of energy required to break a covalent bond.

The stronger the bond, the higher the bond dissociation enthalpy.

The C-H

bond in alkenes is stronger than the C-H

bond in alkanes. The sp2-hybridized carbon atoms have stronger C-H

bonds than C-H

bonds in sp3-hybridized carbon atoms.

Allylic C-H bonds are weaker than non-allylic (alkyl) C-H bonds.

Expert Solution & Answer

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Check out a sample textbook solution

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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 11.3, Problem 7P

Interpretation Introduction

Interpretation:

The C-H bonds of Trans-3-hexene are to be ranked in the order of decreasing bond dissociation enthalpy.

Concept introduction:

Bond dissociation enthalpy is the amount of energy required to break a covalent bond.

The stronger the bond, the higher the bond dissociation enthalpy.

The C-H

bond in alkenes is stronger than the C-H

bond in alkanes. The sp2-hybridized carbon atoms have stronger C-H

bonds than C-H

bonds in sp3-hybridized carbon atoms.

Allylic C-H bonds are weaker than non-allylic (alkyl) C-H bonds.

Expert Solution & Answer

Want to see the full answer?

Check out a sample textbook solution

See solution

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 11.3, Problem 7P

Interpretation Introduction