Collision theory explains how and why chemical reactions occur by describing the conditions under which reactant particles must collide. Effective collisions require proper orientation and sufficient energy to overcome activation energy.
5 Must Know Facts For Your Next Test
For a reaction to occur, particles must collide with the correct orientation and sufficient energy.
The minimum amount of energy required for a reaction to occur is called the activation energy.
Increasing the temperature generally increases the reaction rate because particles have more kinetic energy, leading to more effective collisions.
Catalysts lower the activation energy needed for a reaction, increasing the rate without being consumed in the process.
The collision frequency, which is affected by concentration and temperature, plays a crucial role in determining reaction rates.