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  2. Reaction intermediate - Wikipedia

    en.wikipedia.org/wiki/Reaction_intermediate

    In chemistry, a reaction intermediate, or intermediate, is a molecular entity arising within the sequence of a stepwise chemical reaction. It is formed as the reaction product of an elementary step, from the reactants and/or preceding intermediates, but is consumed in a later step. It does not appear in the chemical equation for the overall ...

  3. Reactive intermediate - Wikipedia

    en.wikipedia.org/wiki/Reactive_intermediate

    When generated in a chemical reaction, it will quickly convert into a more stable molecule. Only in exceptional cases can these compounds be isolated and stored, e.g. low temperatures, matrix isolation. When their existence is indicated, reactive intermediates can help explain how a chemical reaction takes place. [1] [2] [3] [4]

  4. Reaction mechanism - Wikipedia

    en.wikipedia.org/wiki/Reaction_mechanism

    In chemistry, a reaction mechanism is the step by step sequence of elementary reactions by which overall chemical reaction occurs. [1] A chemical mechanism is a theoretical conjecture that tries to describe in detail what takes place at each stage of an overall chemical reaction. The detailed steps of a reaction are not observable in most cases.

  5. Activated complex - Wikipedia

    en.wikipedia.org/wiki/Activated_complex

    The transition state, represented by the double dagger symbol represents the exact configuration of atoms that has an equal probability of forming either the reactants or products of the given reaction. [5] The activation energy is the minimum amount of energy to initiate a chemical reaction and form the activated complex. [6]

  6. Energy profile (chemistry) - Wikipedia

    en.wikipedia.org/wiki/Energy_profile_(chemistry)

    Figure 6:Reaction Coordinate Diagrams showing reactions with 0, 1 and 2 intermediates: The double-headed arrow shows the first, second and third step in each reaction coordinate diagram. In all three of these reactions the first step is the slow step because the activation energy from the reactants to the transition state is the highest.

  7. Rate-determining step - Wikipedia

    en.wikipedia.org/wiki/Rate-determining_step

    [8] [6] If there is a reaction intermediate whose energy is lower than the initial reactants, then the activation energy needed to pass through any subsequent transition state depends on the Gibbs energy of that state relative to the lower-energy intermediate. The rate-determining step is then the step with the largest Gibbs energy difference ...

  8. Tetrahedral carbonyl addition compound - Wikipedia

    en.wikipedia.org/wiki/Tetrahedral_carbonyl...

    A tetrahedral intermediate is a reaction intermediate in which the bond arrangement around an initially double-bonded carbon atom has been transformed from trigonal to tetrahedral. [1] Tetrahedral intermediates result from nucleophilic addition to a carbonyl group.

  9. Nitrene - Wikipedia

    en.wikipedia.org/wiki/Nitrene

    The generic structure of a nitrene group. In chemistry, a nitrene or imene (R−:Ṅ·) is the nitrogen analogue of a carbene.The nitrogen atom is uncharged and monovalent, [1] so it has only 6 electrons in its valence level—two covalent bonded and four non-bonded electrons.