La teoría de las colisiones presume que para generarse un proceso químico es necesario que las sustancias reaccionantes se encuentren en forma libre y choquen en forma “efectiva”, para permitir la interacción química necesaria para la transformación. Es decir, la velocidad de una reacción es directamente proporcional al número de choques por segundo entre las partículas de los reaccionantes y a la efectividad de ese número de choques.
No todo es lo que parece
Es lógico pensar que en la medida que el número de colisiones aumenta, el proceso químico se lleva a cabo con una rapidez mayor; no obstante, la experiencia ha demostrado que no es el único factor, ya que la frecuencia de choques en cualquier material es bastante elevada.
Por ejemplo, en 2 mol de reactivos gaseosos, A y B en condiciones normales, el orden es de 1030, un número tan elevado, que en el caso de que todos diesen lugar a la reacción química, el proceso sería prácticamente instantáneo; de aquí se deduce que solo algunas de las colisiones logran la transformación química.
¿Cómo se explica todo eso?
Las nubes electrónicas asociadas a dos partículas que se acercan tienden a una repulsión por encontrarse con la misma carga; por lo tanto, un choque débil hace que las partículas se alejen bruscamente, sin producirse la interacción química.
En el caso de que las dos partículas, o por lo menos una de ellas, posean mucha energía antes de la colisión permite vencer la fuerza repulsiva y se penetran mutuamente, con una reorganización electrónica, que produce una especie química nueva.
Esta cantidad de energía adicional que hace falta para que un choque sea efectivo es lo que se conoce como energía de activación.
En un próximo post te explicaremos en qué consiste la energía de activación y su repercusión en los procesos químicos.
También te puede interesar: Velocidad de una reacción química
FUENTE
Rodríguez, María del Pilar. (2006). Química 1. (Segunda edición., pág. 95). Fundación Editorial Salesiana.
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