Activated complex
Activated Complex
The Activated Complex (pronunciation: ak-ti-vay-ted kom-plex), also known as the transition state, is a term used in Chemical Kinetics to describe a high-energy configuration of atoms that exists momentarily during a Chemical Reaction. The concept of the activated complex is fundamental to the Transition State Theory, which attempts to describe the process of chemical reactions.
Etymology
The term "Activated Complex" is derived from the process it describes. "Activated" refers to the energy that the reactants need to undergo a chemical reaction, while "Complex" refers to the temporary, unstable arrangement of atoms that forms during the reaction.
Definition
In a chemical reaction, the activated complex is the structure at the maximum energy point along the reaction path. It is the most unstable arrangement of atoms that exists momentarily at the peak of the Reaction Coordinate Diagram. The energy required to form the activated complex from the reactants is known as the Activation Energy.
Related Terms
- Transition State Theory: A theory that describes chemical reactions in terms of an activated complex that proceeds to the products through the transition state.
- Reaction Coordinate Diagram: A diagram that shows the energy changes that occur during a chemical reaction.
- Activation Energy: The minimum amount of energy required to initiate a chemical reaction.
- Chemical Kinetics: The study of rates at which reactions occur and the steps by which they proceed.
See Also
External links
- Medical encyclopedia article on Activated complex
- Wikipedia's article - Activated complex
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