6.2.2 & 6.2.3

6.2.2

Define the term activation energy Ea

<sub>The minimum value of kinetic energy, for a collision to lead to a reaction, is necessary to overcome repulsion between molecules and often to break some bonds in the reactants before they react. When the energy is supplied, the reactant achieve the transition state from which products can form. The energy required represents an energy barrier for the reaction and is known as activation energy. 


6.2.3
Define collision theory</sub> 
The rate of reaction depending on the frequency of collision which occur between particles processing both values of kinetic energy greater than the activation energy or appropriate collision geometry.