Insufficient Kinetic Energy:
In order for a reaction to occur between two particles, they must have sufficient kinetic energy to overcome the activation energy barrier. If the particles do not possess enough energy to reach this energy level, the collision will be elastic, meaning the particles will bounce off each other with no chemical reaction taking place.
Improper Geometric Orientation:
Even if there is sufficient kinetic energy, the geometric orientation of the colliding particles must also be favorable for a reaction to occur. For example, in certain chemical reactions, the molecules must collide with the correct orientation for their atomic orbitals to overlap effectively and form new bonds. If the orientation of the particles is not suitable, the collision may not result in a reaction.
In summary, insufficient kinetic energy and improper geometric orientation can both hinder the occurrence of a collision or prevent a reaction from taking place, even if the particles possess enough energy.
