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activation energy. activation energy, in chemistry, minimum energy needed to cause a chemical reaction. A chemical reaction between two substances occurs only when an atom, ion, or molecule of one collides with an atom, ion, or molecule of the other.
the activation energy is the difference between the reactants and the highest energy state of the reaction (the transition point) which is represented by b (note this is not the absolute energy of the transition point as d would indicate, but the difference between the highest energy state and the starting energy). And the heat of the reaction is the difference between what you start with and what you end up with which is indicated by c on the graph. One might argue that c and e represent the same energy, but there c represents the direction of the change to a higher potential energy state more accurately.