Collision Theory
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15 Terms
What is collision theory?
Chemical reactions occur when reactant particles collide with sufficient energy.
What is a successful collision?
A collision between reactant particles that results in a chemical reaction.
What is activation energy?
The minimum energy that particles must have to react when they collide.
Why do not all collisions lead to reactions?
Some particles collide with less than the activation energy.
What two factors determine the frequency of successful collisions?
The frequency of collisions and the proportion of collisions with sufficient energy.
What happens when the frequency of successful collisions increases?
The rate of reaction increases.
Why must reactant particles collide?
Particles must interact for chemical bonds to break and new bonds to form.
Why is activation energy important?
It determines the minimum energy needed for a reaction to occur.
What happens when particles collide with insufficient energy?
They do not react.
How does increasing temperature affect successful collisions?
It increases collision frequency and the proportion of particles with energy equal to or greater than the activation energy.
How does increasing concentration affect successful collisions?
It increases the frequency of collisions.
How does increasing surface area affect successful collisions?
It exposes more particles to collisions.
How does a catalyst affect successful collisions?
It provides an alternative pathway with lower activation energy, increasing the proportion of successful collisions.
Does every collision between reactant particles cause a reaction?
No, particles must collide with sufficient energy.
What is the relationship between collision frequency and reaction rate?
A higher frequency of successful collisions per second produces a faster reaction.