The relative ease of radical halogenation at H a is to be explained, and between H b and H c which one can more readily undergo radical halogenation is to be determined. Concept introduction: A type of halogenation in which alkanes and aromatic compounds , which are alkyl-substituted, react chemically in presence of light is known as free radical halogenation. It involves chain initiation, propagation, and termination steps in its whole mechanism. The free radical halogenation reaction is used in industries to synthesize dichloromethane and chloroform.

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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 10, Problem 27P

Interpretation Introduction

Interpretation:

The relative ease of radical halogenation at Ha is to be explained, and between Hb and Hc which one can more readily undergo radical halogenation is to be determined.

Concept introduction:

A type of halogenation in which alkanes and aromatic compounds, which are alkyl-substituted, react chemically in presence of light is known as free radical halogenation. It involves chain initiation, propagation, and termination steps in its whole mechanism. The free radical halogenation reaction is used in industries to synthesize dichloromethane and chloroform.

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Compounds P and Q can undergo a Diels-Alder reaction to form two regioisomeric products R and S as shown in Figure 5. OMe P H C8H1202 R C8H1202 S Figure 5 Draw the chemical structures of regioisomeric compounds R and S. (ii) Using possible resonance contributors of P and Q predict which of the two regioisomers will be favoured in the reaction. (iii) Using curly arrows, draw the mechanism for the reaction of P and Q to form the dominant regioisomer you have predicted in your answer to part (ii) above.

Practical aspects of radical halogenation Radical halogenation of ethane is a major industrial sands of tons of chloro- and bromoethane are produced annually. proces, thou- However, radical fluorination and iodination are not practical. Using thermodynamic analysis (similar to one we did in class), explain why radical iodination and fluorination are not practical. Use values in Table 1 for your calculations. Table 1: Bond dissociation energies for various bond types (in kJ/mol) Bond BDE Bond BDE CH3CH2-F CH3CH2-Cl F-F 159 456 Cl-Cl 243 351 СH3CH2- Br CH3CH2-I Br – Br 193 301 I-I 151 238 CH3 -H CH3CH2-H Н-F 569 439 Н-СІ 431 423 (CH3)2CH-H (CH3)3C-H CH2=CH2 Н-Br 366 414 Н-І 299 404 636 CH2 =CH2 (7) 272

1.For substance A: a)Draw a picture of substance A showing the orbitals involved in the sigma and pi bonds, including its lone pairs. b) Discuss the stability of substance A in the presence of water and the expected reaction. c) Predict the reactivity of substance A towards nucleophiles and justify your answer. d) Discuss the stability of substance A in the presence of water and the expected reaction. e) What type of intermolecular forces would you expect between molecules of substance A? Explain.

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 10, Problem 27P

Interpretation Introduction

Interpretation:

The relative ease of radical halogenation at Ha is to be explained, and between Hb and Hc which one can more readily undergo radical halogenation is to be determined.

Concept introduction:

A type of halogenation in which alkanes and aromatic compounds, which are alkyl-substituted, react chemically in presence of light is known as free radical halogenation. It involves chain initiation, propagation, and termination steps in its whole mechanism. The free radical halogenation reaction is used in industries to synthesize dichloromethane and chloroform.

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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 10, Problem 27P

Interpretation Introduction

Interpretation:

The relative ease of radical halogenation at Ha is to be explained, and between Hb and Hc which one can more readily undergo radical halogenation is to be determined.

Concept introduction:

A type of halogenation in which alkanes and aromatic compounds, which are alkyl-substituted, react chemically in presence of light is known as free radical halogenation. It involves chain initiation, propagation, and termination steps in its whole mechanism. The free radical halogenation reaction is used in industries to synthesize dichloromethane and chloroform.

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 10, Problem 27P

Interpretation Introduction