Chemistry
Chemistry
Problem
Which statement best defines a reaction intermediate in a multistep mechanism? a) A short-lived, high-energy arrangement of atoms that exists at the peak of the potential-energy diagram and cannot be isolated. b) A species that is produced in one elementary step and consumed in a later step, never appearing in the overall balanced equation. c) A species that speeds up a reaction by lowering the activation energy and is regenerated unchanged at the end. d) A species that is produced in one step and remains in the reaction mixture, appearing in the overall balanced equation.Intuitive explanation
A reaction intermediate is a species that is produced in one step and consumed in a later step—it appears in the mechanism but never in the overall balanced equation. The key insight is that intermediates are temporary: they build up and break down as the reaction proceeds, so they don't show up in the final products. Recognizing intermediates helps you understand what's actually happening between reactants and products, and it's crucial for writing rate laws from mechanisms.
Intuitive explanation
A reaction intermediate is a species that is produced in one step and consumed in a later step—it appears in the mechanism but never in the overall balanced equation. The key insight is that intermediates are temporary: they build up and break down as the reaction proceeds, so they don't show up in the final products. Recognizing intermediates helps you understand what's actually happening between reactants and products, and it's crucial for writing rate laws from mechanisms.