Chapter 8, Problem 8.32P

Interpretation Introduction

(a)

Interpretation:

Energy diagram for the given ${\text{S}}_{\text{N}}\text{1}$ reaction, including overall reactants, overall products, the transition state, and the intermediate, is to be drawn.

Concept introduction:

The nucleophilic substitution reaction that takes place in two steps, through the formation of a carbocation intermediate, is called the unimolecular nucleophilic substitution ${\text{(S}}_{\text{N}}\text{1)}$ reaction. The ${\text{S}}_{\text{N}}\text{1}$ reaction is a two-step reaction. For a mechanism that contains n total elementary steps, there must be n total transition states. The energy diagram is a plot of free energy versus reaction coordinates. The intermediate is higher in energy (less stable) than the overall reactants and the overall products. The intermediate occurs at a local minimum in energy along the reaction coordinate, so energy increases when going either forward or backward from the intermediate along the reaction coordinate. The overall reactants are on the left, and the overall products are on the far right.

Interpretation Introduction

(b)

Interpretation:

Energy diagram, for the given ${\text{S}}_{\text{N}}\text{1}$ reaction including overall reactants, overall products, the transition state, and the intermediate, is to be drawn.

Concept introduction:

The nucleophilic substitution reaction that takes place in two steps through the formation of a carbocation intermediate is called unimolecular nucleophilic substitution ${\text{(S}}_{\text{N}}\text{1)}$ reaction. The ${\text{S}}_{\text{N}}\text{1}$ reaction is a three step reaction if the nucleophile is uncharged. For a mechanism that contains n total elementary steps, there must be n total transition states. The energy diagram is a plot of free energy versus reaction coordinates. The intermediate is higher in energy (less stable) than the overall reactants and the overall products. The intermediate occurs at a local minimum in energy along the reaction coordinate, so energy increases when going either forward or backward from the intermediate along the reaction coordinate. The overall reactants are on the left, and the overall products are on the far right.