Consider the following hypothetical molecular collisions and predict which of the following will form potential products, given the values for the energy of activation, Ea, and enthalpy of the reaction, ΔH, in combination with the molecular orientation.

Collision theory provides a qualitative explanation of chemical reactions and the rates at which they occur. A basic principle of collision theory is that, in order to react, molecules must collide. This fundamental rule guides any analysis of an ordinary reaction mechanism.

At the time of reaction, the particles of the reactant collide with each other and make a bond by using energy.

The collision occurs with adequate energy to permit mutual penetration of the reacting species. The two physical factors are the following in these collision depends

For example, look at the combination reaction of carbon dioxide.

After a collision between carbon monoxide and oxygen, the reaction is

According to the collision theory, the energy is sufficient to make the new compound after the collision of reactants.

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The collision theory is defined as the rate of a reaction is proportional to the rate of reactant collisions.

Explanation:

The reacting species should collide with orientation that allows contract between the atoms that will become bonds together in the product.

The collision occurs with adequate energy  to permit mutual penetration of the reacting species. The two physical factors based on the orientation and energy of collision, the following reaction with carbon monoxide with oxygen is considered.

 2CO(g) + O2(g) → 2CO2 (g)

After collision between the carbon monoxide and oxygen the reaction is

 CO(g) + O2(g) → CO2 (g) + O(g)

Based on the theories of chemical reaction the molecules collide with sufficient amount of energy an activated complex is formed.

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