What does collision theory state about chemical reactions?

Collision theory explains how chemical reactions take place based on the interactions of particles. According to this theory, for a reaction to occur, reactant particles must collide with enough energy to overcome the activation energy barrier. When particles collide with sufficient energy, they can rearrange their bonds and transform into products. This highlights the importance of both the frequency of collisions and the energy involved in those collisions.

The correct answer emphasizes that successful collisions—the ones that lead to a reaction—must have adequate energy. This is a fundamental concept in understanding reaction kinetics and helps in predicting how changes in conditions, such as temperature or concentration, can affect the rate of a chemical reaction.

Other options propose conditions under which reactions can occur but do not encapsulate the core principle of collision theory as effectively as the idea of energy-rich collisions. High pressure and the presence of catalysts can indeed influence reactions, but they are not prerequisites for the occurrence of all chemical reactions.