Collision Theory and Activation Energy (Leaving Cert Chemistry): Flashcards
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Collision theory
Collision theory
Theory explaining reaction rates based on particle collisions
3 requirements for reaction to occur
3 requirements for reaction to occur
Particles collide, sufficient energy, correct orientation
Effective collision
Effective collision
Collision with enough energy & orientation forming products
Correct orientation requirement
Correct orientation requirement
Particles must collide in correct orientation for reaction to occur
Maxwell-Boltzmann distribution shows
Maxwell-Boltzmann distribution shows
Spread of kinetic energies among gas molecules
Activation energy ()
Activation energy ()
Minimum energy colliding particles need for reaction
Large activation energy effect
Large activation energy effect
Few molecules have sufficient energy; slow reaction rate
Small activation energy effect
Small activation energy effect
More molecules have enough energy; faster reaction rate
Activated complex
Activated complex
Highest energy point where bonds break & form (transition state)
Exothermic reaction energy change
Exothermic reaction energy change
Products lower energy than reactants; heat released
Endothermic reaction energy change
Endothermic reaction energy change
Products higher energy than reactants; heat absorbed
Temperature increase main effect
Temperature increase main effect
More particles have energy above activation energy threshold
Concentration increase effect
Concentration increase effect
More particles, closer together; more frequent collisions
Smaller particle size effect
Smaller particle size effect
Greater surface area; more frequent effective collisions
Catalyst function
Catalyst function
Provides alternative pathway with lower activation energy