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For example, the hydrolysis of chlorotert butane can be carried out in two steps:
(CH3) 3ccl → (CH3) 3C + + Cl -
(CH3) 3C + + H2O → (CH3) 3coh + H +
two transition states and one intermediate, positive carbon ion (CH3) 3C +, appear between them. The two reactions pass through two barriers respectively Δ E1 and Δ E2, transition state 1 - (CH3) 3C... Cl and transition state 2 - (CH3) 3C... Oh2 appear at the potential energy peak of each step respectively, while the active intermediate is in the valley between the two peaks. The structure and properties of the active intermediate and the two transition states are similar, but different. Generally, intermediates are very active and have a short life, but they are more stable than transition states, so their structures can be determined by various modern physical and chemical methods. The lower the potential energy of the intermediate between the two transition states, the more stable the intermediate is. Based on the knowledge of the structure and properties of intermediates, the structure and properties of the transition state can be roughly deced to elucidate the reaction mechanism

According to the transition state theory, the relationship between the experimental activation energy EA and the activation enthalpy RHM is: EA= Δ r≠HmӨ- RT

activation energy refers to the energy required for the transition of molecules from normal state to active state prone to chemical reaction. The difference between the potential energy of free state of activation energy EA and activation enthalpy RHM and the potential energy of activated molecules formed by the combination of them is the activation energy required for the reaction

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theoretical viewpoint of transition state theory:

transition state theory holds that reactant molecules do not directly form procts through simple collision, but must pass through a transition state to form a high-energy activated complex, and a certain activation energy is required to reach this transition state, and then converted into procts

when a reacts with B, a and B approach and proce a certain force, while the bond between B and C weakens; The formation of unstable [a ··· B ·· C] is called transition state, or active compound

reactants a + BC and procts AB + C are stable states with low energy, and transition states are unstable states with high energy. When the reactant energy is very high, the transition state is the highest energy point in the reaction process

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