What is the Difference Between Elementary and Complex Reaction?

The main difference between elementary and complex reactions lies in the number of steps involved in the process. Here are the key differences between the two types of reactions:

• Elementary Reactions:
• Occur in a single step, with reactants being converted into products in a single collision.
• Involve a single sub-step.
• Overall order values are small.
• Total and pseudo order values lie between 0, 1, 2.
• Products are formed directly in the reaction.
• Complex Reactions:
• Occur in multiple steps.
• Involve a series of steps and different transition states with varying molecularity.
• Overall order values are large.
• Many side reactions are present.
• Products are not formed directly in steps involving the reactants, and intermediates are formed before giving the final product.

In summary, elementary reactions involve a single step and directly form products, while complex reactions consist of multiple steps, involve intermediates, and have larger overall order values.

Comparative Table: Elementary vs Complex Reaction

The main difference between elementary and complex reactions lies in the number of steps involved in the process. Here is a table comparing the two types of reactions:

An elementary reaction is a chemical reaction that includes a single sub-step, where one chemical species undergoes a direct change to give the final product in one step. On the other hand, a complex reaction consists of more than one elementary reaction and intermediate products. Complex reactions can be explained by a set of elementary reactions, which comprise a reaction mechanism that predicts the elementary steps involved in the complex reaction.