AP Chemistry Practice Quiz: Collision Model
Written by AP Content Team, Verified for 2026 AP Exams, Last updated: May 2026
Test your understanding with short quizzes. This quiz has 10 questions to check your progress.
Question 1 of 10
All Questions (10)
A) Sufficient energy and proper orientation
B) High frequency and low temperature
C) Bond-making and bond-breaking events
D) Particle size and container volume
Correct Answer: A
The provided content explicitly states, 'Successful collisions require both sufficient energy (activation energy) and proper orientation.' The other options describe related concepts but not the two primary requirements for a single collision's success.
A) The rate is directly proportional to the total number of collisions, regardless of their energy or orientation.
B) The rate depends on the frequency of collisions that have both sufficient energy and the correct orientation.
C) The rate is determined solely by the activation energy of the reaction.
D) The rate is determined solely by the orientation of the colliding particles.
Correct Answer: B
The content explains that the reaction rate is related to the frequency, energy, and orientation of collisions. It clarifies that only a small fraction of collisions are successful, meaning the rate is dependent on the frequency of these specific, successful collisions.
A) It shows that at higher temperatures, all particles move with the same increased energy.
B) It illustrates that a higher temperature increases the fraction of particles possessing the necessary activation energy.
C) It proves that temperature only affects the orientation of collisions, not the energy.
D) It demonstrates that the activation energy of the reaction decreases as temperature increases.
Correct Answer: B
The content states the curve shows 'how this fraction [of collisions with sufficient energy to react] changes with temperature.' At a higher temperature, the curve flattens and shifts to the right, meaning a larger proportion of particles has energy equal to or greater than the activation energy, leading to a higher rate.
A) The reactants are not in the same phase of matter.
B) The collisions occur too frequently for bonds to form.
C) The colliding particles lack either sufficient energy or the correct orientation.
D) The products formed are immediately converted back to reactants.
Correct Answer: C
The text directly states, 'In most reactions, only a small fraction of collisions are successful. Successful collisions require both sufficient energy (activation energy) and proper orientation.' Therefore, unsuccessful collisions are those that are missing one or both of these requirements.
A) An increase in the temperature of the system.
B) The release of a photon.
C) The initiation of bond-breaking and bond-making events.
D) A decrease in the total collision frequency.
Correct Answer: C
The content specifies that 'reactants must successfully collide to initiate bond-breaking and bond-making events' in order to produce products. This is the direct chemical consequence of an effective collision.
A) total energy released during a chemical reaction.
B) average kinetic energy of the reactant particles.
C) minimum energy required for a collision to be successful.
D) energy difference between reactants and products.
Correct Answer: C
The text indicates that successful collisions require 'sufficient energy (activation energy).' This defines activation energy as the minimum energy threshold that must be overcome during a collision for a reaction to occur.
A) The activation energy for the reaction is lowered at higher temperatures.
B) The orientation of colliding particles becomes more favorable at higher temperatures.
C) The total number of particles in the container increases.
D) A significantly larger fraction of particle collisions has energy equal to or greater than the activation energy.
Correct Answer: D
The content explains that the Maxwell-Boltzmann distribution shows how the fraction of collisions with sufficient energy changes with temperature. While higher temperature also increases collision frequency, the most significant factor for the rate increase is the exponential growth in the fraction of particles that possess enough energy to overcome the activation energy barrier.
A) The collision frequency was too low.
B) The molecules had an improper orientation relative to each other.
C) The temperature of the system was too high.
D) The bond-making events occurred before the bond-breaking events.
Correct Answer: B
The content states that two conditions must be met for a successful collision: sufficient energy AND proper orientation. If the energy condition is met but the collision is still unsuccessful, the orientation must have been incorrect.
A) All collisions lead to reactions, and the rate is determined by how fast the particles move.
B) The rate of reaction is determined by the frequency of collisions that meet minimum energy and specific orientation requirements to break and form bonds.
C) The Maxwell-Boltzmann distribution ensures that every particle will eventually gain enough energy to react.
D) Reactions occur when particles are close enough, and energy is only required to overcome repulsive forces.
Correct Answer: B
This option correctly synthesizes all the key ideas presented: the rate depends on the frequency of successful collisions, which are defined by having sufficient energy and proper orientation, leading to the initiation of bond-breaking and bond-making.
A) Orientation
B) Collision frequency
C) Activation energy
D) Particle energies
Correct Answer: D
The provided text explicitly states that 'The Maxwell-Boltzmann distribution curve shows the distribution of particle energies'. It is typically a plot of the number of particles versus their kinetic energy.