Collision Theory — GCSE Chemistry Revision
Revise Collision Theory for GCSE Chemistry. Step-by-step explanation, worked examples, common mistakes and exam-style practice aligned to AQA, Edexcel, OCR, WJEC, Eduqas, CCEA, Cambridge International (CIE), SQA, IB, AP.
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Go to Factors Affecting RateWhat is Collision Theory?
Collision theory states that for a chemical reaction to occur, the reactant particles must collide with each other with sufficient energy. The minimum amount of energy required for a successful collision is called the activation energy. Not all collisions result in a reaction; they must have the correct orientation and enough energy.
Board notes: Collision theory is the underlying explanation for why different factors affect reaction rates. It is a key concept for all boards, especially at higher tier. You must be able to use it to explain the effects of temperature, concentration, pressure, and surface area.
Step-by-step explanationWorked example
Increasing the temperature of a reaction mixture gives the particles more kinetic energy. This means they move faster, leading to more frequent collisions. More importantly, a higher proportion of these collisions will have energy greater than the activation energy, so the rate of successful collisions increases, and the reaction speeds up.
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Common mistakes
- 1Stating that increasing a factor (like temperature) just 'increases the number of collisions'. You must specify that it increases the *frequency* of collisions (number of collisions per unit time).
- 2Forgetting to mention the activation energy. For a collision to be successful, the particles must collide with energy *equal to or greater than* the activation energy.
- 3Thinking that any collision with enough energy will lead to a reaction. The particles must also collide in the correct orientation for bonds to be broken and new bonds to be formed.
Collision Theory exam questions
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Step-by-step method
Step-by-step explanation
4 steps · Worked method for Collision Theory
Core concept
Collision theory states that for a chemical reaction to occur, the reactant particles must collide with each other with sufficient energy. The minimum amount of energy required for a successful collis…
Frequently asked questions
What is the activation energy?
The activation energy is the minimum energy that colliding particles need in order to react. It is the energy barrier that must be overcome for a reaction to start.
How does a catalyst work according to collision theory?
A catalyst increases the rate of reaction by providing an alternative pathway with a lower activation energy. This means that more of the colliding particles will have sufficient energy to react, increasing the rate of successful collisions.