AP Chemistry Flashcards: Collision Model

What this deck covers

This deck focuses on Collision Model, giving you a quick way to review the definitions, rules, and examples that matter most for AP Chemistry.

How to use these flashcards

Work through these flashcards in short sessions. Try to answer each prompt before flipping the card, then revisit any cards you miss until the explanation feels automatic.

Flashcard 1: What is the effect of decreasing activation energy on effective collisions?

Answer: Increases effective collisions. More molecules now have sufficient energy to overcome barrier.

Flashcard 2: What is the primary role of a catalyst in a chemical reaction?

Answer: Lowers activation energy. Speeds up reactions by providing alternative reaction pathway.

Flashcard 3: State the effect of decreasing surface area on collision frequency.

Answer: Decreases collision frequency. Less surface area means fewer molecules accessible for collision.

Flashcard 4: What is the role of proper orientation in molecular collisions?

Answer: Ensures effective collisions. Molecules must align correctly for bonds to form.

Flashcard 5: Identify one condition necessary for a collision to be effective.

Answer: Sufficient energy. Energy threshold that molecules must exceed during collision.

Flashcard 6: What does the symbol $R$ stand for in the Arrhenius equation?

Answer: Universal gas constant. Physical constant relating energy and temperature scales.

Flashcard 7: Write the Arrhenius equation.

Answer: $k = A e^{-Ea/RT}$. Mathematical expression showing temperature dependence of rate constant.

Flashcard 8: Define effective collision.

Answer: Collision with sufficient energy and proper orientation. Both energy and orientation requirements must be met.

Flashcard 9: What is the basic principle of the collision model?

Answer: Molecules must collide to react. Fundamental assumption that reactions require molecular contact.

Flashcard 10: What is the impact of a catalyst on the frequency factor $A$?

Answer: No impact on $A$. Catalysts only affect activation energy, not collision frequency.

Flashcard 11: What does the symbol $k$ represent in the Arrhenius equation?

Answer: Rate constant. Proportionality constant relating concentration to reaction rate.

Flashcard 12: Calculate the effect of doubling concentration on reaction rate in a first-order reaction.

Answer: Rate doubles. Rate is directly proportional to concentration in first-order kinetics.

Flashcard 13: Identify the symbol for activation energy in the Arrhenius equation.

Answer: $E_a$. Energy barrier term in exponential function.

Flashcard 14: How does increased temperature affect the rate constant $k$?

Answer: Increases $k$. Exponential increase due to more energetic molecules.

Flashcard 15: Define the term 'frequency factor' in the context of the Arrhenius equation.

Answer: Number of collisions with correct orientation. Represents collision frequency and steric factors in Arrhenius equation.

Flashcard 16: What factor besides temperature can increase the rate constant $k$?

Answer: Catalyst. Only catalysts and temperature significantly affect $k$.

Flashcard 17: How does increasing concentration affect reaction rate?

Answer: Increases reaction rate. More molecules present means higher collision frequency.

Flashcard 18: What does $A$ represent in the Arrhenius equation?

Answer: Frequency factor. Pre-exponential term representing collision frequency.

Flashcard 19: State the effect of a catalyst on the overall reaction rate.

Answer: Increases reaction rate. Lowers activation energy allowing more effective collisions.

Flashcard 20: What is the effect of a higher activation energy on the reaction rate?

Answer: Decreases reaction rate. Fewer molecules have energy to overcome higher barrier.

Flashcard 21: What impact does temperature have on kinetic energy of molecules?

Answer: Increases kinetic energy. Higher temperature increases average molecular speeds.

Flashcard 22: Identify how pressure affects the reaction rate for gaseous reactants.

Answer: Increases reaction rate. Compression brings gas molecules closer increasing collision frequency.

Flashcard 23: What is the relationship between reaction rate and activation energy?

Answer: Inverse relationship. Higher $E_a$ means fewer molecules have sufficient energy to react.

Flashcard 24: Find the effect of increasing the pressure on the reaction rate of gases.

Answer: Increases reaction rate. Higher pressure brings gas molecules closer together.

Flashcard 25: What is the effect of increasing activation energy on the rate constant $k$?

Answer: Decreases $k$. Higher barrier reduces fraction of molecules with sufficient energy.

Flashcard 26: What does the Arrhenius equation describe?

Answer: Relationship between rate constant and temperature. Shows how rate constant depends exponentially on temperature.

Flashcard 27: What is the relationship between reaction rate and temperature?

Answer: Direct relationship. Higher temperature exponentially increases rate constant.

Flashcard 28: Identify how temperature affects the activation energy $E_a$.

Answer: Temperature does not affect $E_a$. Activation energy is an intrinsic property independent of temperature.

Flashcard 29: State the unit of the rate constant $k$ in a zero-order reaction.

Answer: $\text{M} \text{s}^{-1}$. Zero-order rate is independent of concentration.

Flashcard 30: What term describes the minimum energy required for a reaction to occur?

Answer: Activation energy. Energy barrier that must be overcome for bonds to break and form.