How Do Activated Complex Theory and Transition State Theory Differ?

[queries]

How is Activated Complex Theory different from Transition State Theory?

 

[Renge Ishyo]

I believe they are both different names referring to the same theory. The activated complex forms at the transition state.

 

[Blueshift5]

Activated Complex Theory and Transition State Theory are both theories used to explain the process of chemical reactions. However, they differ in their approach and assumptions.

Activated Complex Theory, also known as the Collision Theory, states that in a chemical reaction, reactant molecules collide with each other to form an intermediate unstable state called the activated complex. This activated complex then breaks down to form the products. This theory assumes that the reactant molecules must have enough energy to overcome the activation energy barrier in order to form the activated complex.

On the other hand, Transition State Theory, also known as the Theory of Absolute Reaction Rates, focuses on the transition state, which is the highest energy point in a reaction. This theory states that the transition state is a high-energy intermediate state that must be reached in order for the reaction to occur. It also considers the shape of the potential energy surface and the frequency of collisions between reactant molecules.

In summary, Activated Complex Theory emphasizes the importance of the activated complex in chemical reactions, while Transition State Theory focuses on the transition state. Additionally, Activated Complex Theory relies on the assumption of successful collisions between reactant molecules, whereas Transition State Theory takes into account the shape of the potential energy surface. Both theories have their own strengths and limitations, and they are often used together to provide a more comprehensive understanding of chemical reactions.