Define what is meant by unimolecular and bimolecular steps. Why are termolecular steps infrequently seen in chemical reactions?

Unimolecular steps involve a single molecule undergoing a change or a reaction. These steps can be described by first-order kinetics, as the rate of the reaction depends on the concentration of the single reacting molecule. The general form of a unimolecular step is \(A \rightarrow P\), where A represents the initial molecule and P represents the product(s).

Bimolecular steps involve two molecules interacting or colliding with each other to form a product or undergo a change. These steps can be described by second-order kinetics, as the rate of the reaction depends on the concentration of both reacting molecules. The general form of a bimolecular step is \(A + B \rightarrow P\), where A and B are the initial molecules and P represents the product(s).

Termolecular steps involve the simultaneous collision of three molecules to form a product or undergo a change. These steps are infrequently seen in chemical reactions for several reasons. First, the probability of three molecules colliding at the same time and the proper orientation is very low. Second, termolecular steps usually have very high activation energies, making these reactions difficult to achieve under normal conditions. Finally, termolecular steps often involve complex and unstable intermediates, which may break down or react in alternate pathways before forming the desired product. Due to these factors, termolecular steps are less common compared to unimolecular and bimolecular steps in chemical reactions.