What is the difference between the transition state of a reaction and the activated complex of the reaction?

"The activated complex is often confused with the transition state and is used interchangeably in many textbooks. However, it differs from the transition state in that the transition state represents only the highest potential energy configuration of the atoms during the reaction while the activated complex refers to all the configurations that the atoms pass through in the transformation from products to reactants. In terms of free energies, the activated complex represents all the energetic states in between the free energies of the reactants, the transition state, and the products. This can be visualized in terms of a reaction coordinate, where the transition state is the molecular configuration at the peak of the diagram while the activated complex can refer to any point along the continuum." Straight outa Wikipedia. Hope this helps.