Collision Theory

To understand the kinetics of chemical reactions, and the factors that affect kinetics, we should first examine what happens during a reaction on the molecular level. According to the collision theory of reactivity, reactions occur when reactant molecules “effectively collide.” For an “effective collision” to occur, the reactant molecules must be oriented in space correctly to facilitate the breaking and forming of bonds and the rearrangement of atoms that result in the formation of product molecules (Figure 1.3 “Collision Visualizations“).

Figure 1.3. Collision Visualizations

This visualization shows an ineffective and effective collision based on molecular orientation.

During a molecular collision, molecules must also possess a minimum amount of kinetic energy for an effective collision to occur. This energy varies for each reaction, and is known as the activation energy (E_a) (Figure 1.4 “Potential Energy and Activation Energy“). The rate of reaction therefore depends on the activation energy; a higher activation energy means that fewer molecules will have sufficient energy to undergo an effective collision.

Figure 1.4. Potential Energy and Activation Energy

This potential energy diagram shows the activation energy of a hypothetical reaction.

مواضيع ذات صلة

The Molecular Interpretation of Entropy

Spontaneous Change

Biological Catalysts

Homogeneous Catalysts

Heterogeneous Catalysts

The Rate-Determining Step

Multistep Mechanisms

Elementary Steps and Rate Laws

Elementary Steps

Half-Life

Graphical Methods for Determining Reaction Order

Zero-Order Reactions