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

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

Flashcard 2: How does surface area affect the rate of reaction?

Answer: Increases the rate of reaction. More exposed reactant particles available for collisions.

Flashcard 3: How does surface area affect the rate of reaction?

Answer: Increases the rate of reaction. More exposed reactant particles available for collisions.

Flashcard 4: What impact does temperature have on kinetic energy of molecules?

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

Flashcard 5: Choose the correct unit for the rate constant $k$ in a first-order reaction.

Answer: $\text{s}^{-1}$. First-order rate depends linearly on one concentration.

Flashcard 6: Find the unit for the rate constant $k$ in a second-order reaction.

Answer: $\text{M}^{-1}\text{s}^{-1}$. Second-order reactions have rate proportional to concentration squared.

Flashcard 7: What is the role of proper orientation in molecular collisions?

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

Flashcard 8: What does the symbol $R$ stand for in the Arrhenius equation?

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

Flashcard 9: Identify the symbol for activation energy in the Arrhenius equation.

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

Flashcard 10: What does the symbol $R$ stand for in the Arrhenius equation?

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

Flashcard 11: How does increased temperature affect the rate constant $k$?

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

Flashcard 12: Write the Arrhenius equation.

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

Flashcard 13: 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 14: What is the basic principle of the collision model?

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

Flashcard 15: What is the relationship between reaction rate and temperature?

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

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

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

Flashcard 17: 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 18: Identify the symbol for activation energy in the Arrhenius equation.

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

Flashcard 19: State the effect of temperature on collision frequency.

Answer: Increases collision frequency. Higher temperature means faster molecular motion and more collisions per unit time.

Flashcard 20: Choose the factor that does not affect the frequency factor $A$ in the Arrhenius equation.

Answer: Catalyst. Among temperature, concentration, and pressure, catalysts don't affect $A$.

Flashcard 21: State the effect of decreasing surface area on collision frequency.

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

Flashcard 22: 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 23: State the impact of a catalyst on the equilibrium position.

Answer: No impact on equilibrium position. Catalysts only affect reaction rates, not thermodynamic equilibrium.

Flashcard 24: What is the effect of a non-effective collision on reaction rate?

Answer: No effect on reaction rate. Unsuccessful collisions do not produce products or affect rate.

Flashcard 25: 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 26: 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 27: Choose the correct unit for the rate constant $k$ in a first-order reaction.

Answer: $\text{s}^{-1}$. First-order rate depends linearly on one concentration.

Flashcard 28: 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 29: 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 30: Identify one condition necessary for a collision to be effective.

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

Flashcard 31: What does the Arrhenius equation describe?

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

Flashcard 32: Identify the effect of catalysts on activation energy.

Answer: Catalysts lower activation energy. Provides alternative pathway with lower energy barrier.

Flashcard 33: How does increasing concentration affect reaction rate?

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

Flashcard 34: Identify how pressure affects the reaction rate for gaseous reactants.

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

Flashcard 35: 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 36: 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 37: What does the symbol $k$ represent in the Arrhenius equation?

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

Flashcard 38: 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 39: Identify how pressure affects the reaction rate for gaseous reactants.

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

Flashcard 40: 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 41: 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 42: Choose the factor that does not affect the frequency factor $A$ in the Arrhenius equation.

Answer: Catalyst. Among temperature, concentration, and pressure, catalysts don't affect $A$.

Flashcard 43: State the effect of decreasing surface area on collision frequency.

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

Flashcard 44: 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 45: What does the Arrhenius equation describe?

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

Flashcard 46: Identify the effect of catalysts on activation energy.

Answer: Catalysts lower activation energy. Provides alternative pathway with lower energy barrier.

Flashcard 47: 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 48: 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 49: Define effective collision.

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

Flashcard 50: 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 51: What does $A$ represent in the Arrhenius equation?

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

Flashcard 52: 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 53: State the effect of a catalyst on the overall reaction rate.

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

Flashcard 54: What is the basic principle of the collision model?

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

Flashcard 55: 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.

Flashcard 56: What impact does temperature have on kinetic energy of molecules?

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

Flashcard 57: State the effect of temperature on collision frequency.

Answer: Increases collision frequency. Higher temperature means faster molecular motion and more collisions per unit time.

Flashcard 58: 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 59: 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 60: 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.

Flashcard 61: What does the symbol $k$ represent in the Arrhenius equation?

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

Flashcard 62: 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 63: Find the unit for the rate constant $k$ in a second-order reaction.

Answer: $\text{M}^{-1}\text{s}^{-1}$. Second-order reactions have rate proportional to concentration squared.

Flashcard 64: What is the effect of a non-effective collision on reaction rate?

Answer: No effect on reaction rate. Unsuccessful collisions do not produce products or affect rate.

Flashcard 65: What factor besides temperature can increase the rate constant $k$?

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

Flashcard 66: Write the Arrhenius equation.

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

Flashcard 67: Identify one condition necessary for a collision to be effective.

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

Flashcard 68: Define effective collision.

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

Flashcard 69: What is the relationship between reaction rate and temperature?

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

Flashcard 70: What is the role of proper orientation in molecular collisions?

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

Flashcard 71: State the effect of a catalyst on the overall reaction rate.

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

Flashcard 72: 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 73: State the impact of a catalyst on the equilibrium position.

Answer: No impact on equilibrium position. Catalysts only affect reaction rates, not thermodynamic equilibrium.

Flashcard 74: What does $A$ represent in the Arrhenius equation?

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

Flashcard 75: How does increasing concentration affect reaction rate?

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

Flashcard 76: Find the effect of increasing the pressure on the reaction rate of gases.

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