Collision Theory & Activation Energy (AQA GCSE Chemistry): Flashcards
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Collision Theory explains
Collision Theory explains
How and why chemical reactions happen
Basic requirement for reaction (Collision Theory)
Basic requirement for reaction (Collision Theory)
Particles must collide with each other
Two conditions for successful particle collision
Two conditions for successful particle collision
Enough energy and right direction
Successful collision definition
Successful collision definition
Collision with enough energy to break bonds & form new ones
Rate of reaction depends on
Rate of reaction depends on
Frequency of successful collisions
Effect of more frequent successful collisions
Effect of more frequent successful collisions
Faster reaction rate
Activation Energy definition
Activation Energy definition
Min. energy needed for particles to collide successfully
Activation Energy as a metaphor
Activation Energy as a metaphor
Energy barrier that must be overcome for reaction
Result if particles lack enough energy
Result if particles lack enough energy
They bounce off each other without reacting
Effect of low activation energy on reaction rate
Effect of low activation energy on reaction rate
Reactions happen more quickly
Why low activation energy causes faster reactions
Why low activation energy causes faster reactions
More particles have enough energy to collide successfully
Effect of high activation energy on reaction rate
Effect of high activation energy on reaction rate
Reactions are slower
Why high activation energy causes slower reactions
Why high activation energy causes slower reactions
Fewer particles can overcome the energy barrier