Transition state
Transition state
The Transition state (pronunciation: tran-zish-uhn steyt) is a term used in Chemistry and Biochemistry to describe a high-energy state of a molecule during a chemical reaction.
Etymology
The term "Transition state" originates from the field of Chemistry. It was first used in the early 20th century to describe the temporary, unstable state of a molecule as it undergoes a chemical reaction.
Definition
In a chemical reaction, the Transition state is the highest energy state along the reaction path. It is a state in which the original bonds have partially broken and new bonds have partially formed. The transition state is often symbolized by a double dagger (‡) in chemical equations.
Related Terms
- Activation energy: The minimum amount of energy required to reach the transition state from the reactant state.
- Reaction rate: The speed at which a chemical reaction proceeds, often influenced by the energy of the transition state.
- Catalyst: A substance that lowers the energy of the transition state, thereby increasing the reaction rate.
- Reaction coordinate: A measure of the progress of a chemical reaction, often plotted against the energy of the system to visualize the transition state.
See Also
External links
- Medical encyclopedia article on Transition state
- Wikipedia's article - Transition state
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