The bond dissociation energy of H 2 + is to be estimated and the explanation is to be stated. Concept introduction: The electrons present in the bonding orbitals of molecular orbital have lower energy than the parent atomic orbital. Each electron in bonding orbitals contributes towards the stability of bond. The required energy to break a chemical bond in a molecule is known as the bond dissociation energy.

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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 1, Problem 1.18P

Interpretation Introduction

Interpretation:

The bond dissociation energy of $H2+$ is to be estimated and the explanation is to be stated.

Concept introduction:

The electrons present in the bonding orbitals of molecular orbital have lower energy than the parent atomic orbital. Each electron in bonding orbitals contributes towards the stability of bond.

The required energy to break a chemical bond in a molecule is known as the bond dissociation energy.

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Answer 2

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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 1, Problem 1.18P

Interpretation Introduction

Interpretation:

The bond dissociation energy of $H2+$ is to be estimated and the explanation is to be stated.

Concept introduction:

The electrons present in the bonding orbitals of molecular orbital have lower energy than the parent atomic orbital. Each electron in bonding orbitals contributes towards the stability of bond.

The required energy to break a chemical bond in a molecule is known as the bond dissociation energy.

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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 1, Problem 1.18P

Interpretation Introduction

Interpretation:

The bond dissociation energy of $H2+$ is to be estimated and the explanation is to be stated.

Concept introduction:

The electrons present in the bonding orbitals of molecular orbital have lower energy than the parent atomic orbital. Each electron in bonding orbitals contributes towards the stability of bond.

The required energy to break a chemical bond in a molecule is known as the bond dissociation energy.

Expert Solution & Answer

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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 1, Problem 1.18P

Interpretation Introduction