6.1.7 Collision Theory & Activation Energy

Collision Theory:

Successful Collisions:

• Not all collisions result in a reaction. A successful collision is one where particles collide with enough energy to break their bonds and form new ones, leading to the creation of products.
• The rate of reaction depends on how often these successful collisions occur. The more frequent the successful collisions, the faster the reaction.

Activation Energy:

Impact on Reaction Rate:

• Reactions with low activation energy happen more quickly because more particles have enough energy to collide successfully.
• Reactions with high activation energy are slower because fewer particles can overcome the energy barrier during collisions.