key term - Reaction Intermediate

Definition

A reaction intermediate is a short-lived, high-energy, unstable molecule formed during the course of a chemical reaction that does not appear in the overall equation for the reaction as it's consumed in subsequent steps before the final product forms.

Related terms

Transition State:

It's an unstable state that exists at the maximum energy point along the reaction path and represents conditions under which breaking/forming bonds are at equilibrium.

Catalyst:

A substance that increases the rate of a chemical reaction by lowering activation energy but remains unchanged itself after the reaction.

Rate-Determining Step:

The slowest step in any multi-step process or sequence which determines how fast everything else can proceed.