Collision Theory (HSC SSCE Chemistry): Flashcards
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What collision theory explains
What collision theory explains
How and why reactions occur at different rates
Activation energy () definition
Activation energy () definition
Energy barrier reactants must overcome to form products
Three requirements for chemical reaction
Three requirements for chemical reaction
Collision, sufficient energy, correct orientation
If any requirement not met
If any requirement not met
Collision unsuccessful, no reaction occurs
Result of insufficient energy collision
Result of insufficient energy collision
Particles bounce apart, remain as unreacted reactants
Effect of concentration on collisions
Effect of concentration on collisions
Increases collisions per unit volume per unit time
Temperature & average kinetic energy link
Temperature & average kinetic energy link
Average KE directly proportional to absolute temperature (K)
Maxwell-Boltzmann distribution shows
Maxwell-Boltzmann distribution shows
Spread of kinetic energies among gas molecules
Why higher temp increases reaction rate
Why higher temp increases reaction rate
Larger fraction of molecules has energy exceeding
Why molecular orientation matters
Why molecular orientation matters
Determines if bonds can break and new bonds form