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Topic Notes · Easy summaries with diagrams
Chapter 7 — chapter 7
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Topic 1 of 6
📘Easy summary
According to collision theory, reacting particles must collide; a reaction occurs only when the colliding particles have energy equal to or greater than the activation energy (Ea) and are properly oriented. Such collisions are effective collisions. Activation energy is the minimum energy needed for a collision to result in reaction; it is the energy barrier between reactants and products. Ea differs from ΔH: ΔH is the difference in energy between products and reactants, Ea is the height of the barrier above the reactants. Lower Ea → more effective collisions → larger rate constant.
⭐Key points
- Effective collision: E ≥ Ea + correct orientation.
- Ea is a barrier; ΔH is a difference.
- Lower Ea → faster reaction.
🔬Diagram
🌿Real-life example
H₂ and O₂ do not react at room temperature until a spark supplies Ea.
💡Exam tip
- Mention both energy and orientation.
✅Quick check
1. Lower Ea gives:
2. Effective collisions need:
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