6.2.2-6.2.3

6.2.2 Define the term activation energy (Ea)

Activation energy is the minimum energy required for a reaction to take place 

6.2.3 Describe the collision theory

Three factors affect the rate of reaction:

1. Collision Frequency- The more likely the chance of particles colliding with each other the faster the rate of reaction 
2. Number of particles with greater kinetic energy than activation energy (E>Ea)- For a reaction to take place, the particles must have enough energy to overcome the activation energy of the reaction. Successful reactions take place when the kinetic energy is greater than than the activation energy. This is so that the particles do not repel each other.
3. Collision geometry or orientation- The collision must occur in the correct geometrical alignment, this means that reactive parts of the molecule have to be arranged specifically in a collision to enable a reaction with another particle. (see picture below)