The collision theory explains how and why chemical reactions occur.
Key points:
- Particles must collide: Reactants must physically collide for a reaction to happen.
- Proper orientation: Colliding particles must be oriented correctly to break and form bonds.
- Sufficient energy: Collisions must have enough energy to overcome the activation energy.
Implications:
- Higher concentration → more collisions → faster reaction.
- Higher temperature → faster-moving particles → more collisions with enough energy.
- Catalysts → lower activation energy → more effective collisions.
In short: A reaction occurs when reacting particles collide with the right orientation and enough energy.