The relation between reactants and products at different stages of a chemical reaction can be explained by considering three steps: reactant conversion, intermediate formation, and product formation.
Reactant Conversion: In this step, the reactants undergo a chemical transformation and are converted into intermediate species. This conversion is typically initiated by breaking or rearranging chemical bonds in the reactants. The reactants are consumed during this stage, and the extent of their conversion depends on factors such as reaction conditions and reactant concentrations.
Intermediate Formation: After reactant conversion, intermediate species are formed. These intermediates are often unstable and have higher energy than both the reactants and the final products. They exist momentarily and undergo further transformations in subsequent steps. Intermediates are transient species and are not typically observed as isolated compounds.
Product Formation: In the final step, the intermediates undergo further chemical transformations to yield the desired products. This involves the formation of new chemical bonds and the rearrangement of atoms to generate stable product molecules. The products have lower energy than the intermediates and are considered the final outcome of the reaction.
Overall, the reaction progresses through a series of steps where reactants are converted into intermediates, which further transform to yield the final products. These steps occur sequentially, with each step being influenced by factors such as reaction kinetics, activation energy barriers, and the stability of intermediate species. The complete reaction mechanism involves all these individual steps and provides a detailed understanding of how reactants are converted into products.