Reaction intermediate
Reaction Intermediate
A reaction intermediate or intermediate is a molecular entity that is formed from the reactants (or preceding intermediates) and reacts further to give the directly observed products of a chemical reaction. Most often it refers to a molecule or ion that is formed during the middle of a reaction that has not yet reached its end.
Pronunciation
- IPA: /rɪˈækʃən ˌɪntərˈmiːdiət/
Etymology
The term "reaction intermediate" is derived from the Latin words "reactio" meaning "a reaction" and "intermedius" meaning "in the middle". It was first used in the field of chemistry to describe the temporary molecular structures that are formed and consumed during the course of a reaction.
Related Terms
- Transition state: A high-energy state of a reaction intermediate, at the maximum energy point along the reaction path.
- Catalyst: A substance that increases the rate of a chemical reaction by reducing the energy of the reaction intermediate.
- Substrate: The molecule upon which an enzyme or other catalyst acts to form a reaction intermediate.
- Product: The final state of a reaction intermediate, after it has undergone all necessary reactions.
- Reactant: The initial state of a reaction intermediate, before it has undergone any reactions.
See Also
References
- IUPAC, Compendium of Chemical Terminology, 2nd ed. (the "Gold Book") (1997). Online corrected version: (2006–) "reaction intermediate".
External links
- Medical encyclopedia article on Reaction intermediate
- Wikipedia's article - Reaction intermediate
This WikiMD dictionary article is a stub. You can help make it a full article.
Languages: - East Asian
中文,
日本,
한국어,
South Asian
हिन्दी,
Urdu,
বাংলা,
తెలుగు,
தமிழ்,
ಕನ್ನಡ,
Southeast Asian
Indonesian,
Vietnamese,
Thai,
မြန်မာဘာသာ,
European
español,
Deutsch,
français,
русский,
português do Brasil,
Italian,
polski