Intermediate
| Also Known As | Reactive intermediate, transient intermediate, mechanistic intermediate |
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What is Intermediate?
A species formed during a reaction mechanism that is consumed in a subsequent step and does not appear in the overall balanced equation. Intermediates have finite lifetimes and exist in energy wells between transition states. They can sometimes be isolated or detected spectroscopically.
Properties & Characteristics
Uses & Applications
Safety Information
Always consult the SDS/MSDS before handling any chemical. This information is for educational purposes only.
Key Facts
Frequently Asked Questions
A species formed during a reaction mechanism that is consumed in a subsequent step and does not appear in the overall balanced equation. Intermediates have finite lifetimes and exist in energy wells between transition states. They can sometimes be isolated or detected spectroscopically.
Understanding reaction intermediates is central to: mechanistic organic chemistry (predicting products and stereochemistry), kinetic analysis (steady-state approximation for short-lived intermediates), catalyst design (stabilising or destabilising key intermediates to control reaction rates), and dr…
Many reactive intermediates are highly toxic, mutagenic, or explosive: carbocations alkylate DNA, free radicals cause oxidative stress, nitrene intermediates from azides and organic nitrogen explosives can detonate. Understanding intermediates helps predict unexpected hazardous by-products in chemic…