AP Chemistry Flashcards: Collision Model
Written by AP Content Team, Verified for 2026 AP Exams, Last updated: May 2026
Review key ideas with interactive flashcards. This set includes 10 cards to help you master important concepts.
What is the role of activation energy in the Collision Model?
Activation energy is the minimum energy that colliding reactant particles must possess for a collision to be successful and initiate a chemical reaction.
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What is the role of activation energy in the Collision Model?
Activation energy is the minimum energy that colliding reactant particles must possess for a collision to be successful and initiate a chemical reaction.
How does an increase in temperature affect the fraction of successful collisions, as explained by the Maxwell-Boltzmann distribution?
Increasing temperature shifts the Maxwell-Boltzmann curve, increasing the fraction of particles with energy greater than or equal to the activation energy, which in turn increases the frequency of successful collisions.
What fundamental process must occur for reactants to form products in an elementary reaction, according to the Collision Model?
Reactants must successfully collide to initiate the bond-breaking and bond-making events that lead to the formation of products.
What three factors, based on the Collision Model, collectively determine the rate of an elementary reaction?
The rate is determined by the collision frequency, the fraction of collisions with sufficient energy, and the fraction of collisions with the proper orientation.
Define a "successful collision" in the context of the Collision Model.
A successful collision is one between reactant particles that has both sufficient energy (activation energy) and the correct orientation to initiate bond-breaking and bond-making events, resulting in products.
What is the relationship between the rate of an elementary reaction and the frequency of collisions?
The rate of an elementary reaction is directly related to the frequency of *successful* collisions, not just the total frequency of all collisions.
If a reaction has a very high collision frequency but a very low reaction rate, what two factors could be the primary cause?
The low rate could be caused by a very high activation energy (few collisions are energetic enough) or a very specific orientation requirement (few collisions have the correct geometry).
According to the Collision Model, what two conditions must be met for a collision to result in a chemical reaction?
For a collision to be successful, the colliding particles must have sufficient energy (equal to or greater than the activation energy) and the proper orientation.
What does a Maxwell-Boltzmann distribution curve illustrate in relation to reaction kinetics?
The curve shows the distribution of kinetic energies for a sample of particles at a specific temperature, allowing one to visualize the fraction of particles that have sufficient energy to react.
Why do only a small fraction of collisions in most reactions lead to the formation of products?
Only a small fraction of collisions are successful because most lack either the required activation energy or the precise orientation needed for bonds to break and form.