Stato di transizione

Cinetica chimica
Velocità di reazione
Teoria delle collisioni
Reazione elementare
Molecolarità
Equazione cinetica
Ordine di reazione
Costante di velocità
Equazione di Arrhenius
Equazione di Eyring
Teoria dello stato di transizione
Stato di transizione
Meccanismo di reazione
Energia di attivazione
Approssimazione dello stato stazionario
Effetto isotopico cinetico
Catalisi
Catalizzatore
Catalisi omogenea
Catalisi eterogenea
Catalisi per trasferimento di fase
Catalisi enzimatica
Fotocatalisi
Autocatalisi
Attività catalitica
Sito attivo
Supporto catalitico
Disattivazione dei catalizzatori
Categoria:Cinetica chimica

Si chiama stato di transizione (o complesso attivato) una particolare configurazione lungo la coordinata di reazione, configurazione che corrisponde al punto più alto del grafico dell'energia libera di Gibbs[1] o dell'entalpia[2] in funzione della coordinata di reazione (ad esempio del grado di avanzamento ξ). In altri termini lo stato di transizione corrisponde al momento della reazione in cui i reagenti stanno rompendo i legami per diventare prodotti e, nello stesso tempo, si stanno formando i nuovi legami che permettono la formazione del risultato della reazione.

In base alla teoria dello stato di transizione si può definire come tale un intervallo δ tale da includere il massimo della curva dell'energia libera, lungo l'asse ξ. Tutte le configurazioni di atomi che rientrano in questo intervallo vengono quindi dette stato di transizione.

Lo stato di transizione è in pratica un intermedio di reazione con una vita molto breve (ovvero poco stabile).

Diagramma dell'entalpia lungo la coordinata di reazione. Il complesso attivato si trova in corrispondenza del picco energetico, ovvero ha un contenuto energetico maggiore rispetto ai reagenti e ai prodotti.

Note

  1. ^ (EN) transition state, in IUPAC Gold Book. URL consultato il 19 marzo 2013.
  2. ^ O più in generale di qualsiasi grandezza termodinamica che esprima il contenuto energetico del sistema reattivo.

Voci correlate

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