Activated complex
Definition
The activated complex, also known as the transition state, is a temporary and unstable arrangement of atoms formed during a chemical reaction. It represents the highest energy point along the reaction pathway.
5 Must Know Facts For Your Next Test
- The activated complex has higher energy than both reactants and products.
- It is formed at the peak of the potential energy barrier in a reaction.
- The formation of an activated complex is essential for a reaction to proceed.
- It is short-lived and cannot be isolated.
- The activated complex can either lead to the formation of products or revert back to reactants.
Review Questions
- What is another name for the activated complex?
- Why can't the activated complex be isolated?
- What role does the activated complex play in determining the rate of a chemical reaction?
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Related terms
Activation Energy: The minimum amount of energy required for reactants to form an activated complex and proceed to form products.
Reaction Rate: The speed at which reactants are converted into products in a chemical reaction.
Potential Energy Diagram: A graphical representation showing the energy changes during a chemical reaction, indicating activation energy and the energies of reactants, products, and the activated complex.
