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Activation Energy
Minimum energy required for reactants to react.
Exothermic Reaction
Reactants have higher energy than products.
Endothermic Reaction
Reactants have lower energy than products.
Energy Barrier
Energy threshold that reactants must overcome.
Effective Collision
Collision with correct orientation and sufficient energy.
Boltzmann Distribution Curve
Graph showing energy distribution of particles.
Kinetic Energy
Energy of particles due to their motion.
Temperature Increase
Leads to more kinetic energy in particles.
Reaction Rate
Speed at which reactants convert to products.
Proportion of Successful Collisions
Increases with higher temperatures and kinetic energy.
Peak Shift in Curve
Moves right with increased temperature.
Collision Frequency
Rate at which particles collide with each other.
Activation Energy in Endothermic Reactions
Higher than in exothermic reactions.
Activation Energy in Exothermic Reactions
Lower than in endothermic reactions.
Temperature Effect on Reaction
Higher temperature increases reaction rate.
Distribution of Energies
Varies among particles in a substance.
Small Proportion of Molecules
Only few have energy for effective collisions.
Flatter Boltzmann Curve
Indicates more particles with sufficient energy.
Chemical Reaction
Process where reactants transform into products.
Examiner Tip
Key insights for understanding exam content.
Energy Distribution at Temperature
Shows varying energies among particles.
Collision Orientation
Correct alignment needed for effective reactions.
Higher Proportion of Molecules
More molecules exceed activation energy at higher temperatures.
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