Collision Model - AP Chemistry

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

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

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

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

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

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

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

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

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

Rate constant. Proportionality constant relating concentration to reaction rate.

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

$E_a$. Energy barrier term in exponential function.

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

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

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

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

Frequency factor. Pre-exponential term representing collision frequency.

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

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

Increases kinetic energy. Higher temperature increases average molecular speeds.

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

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

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

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

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

Direct relationship. Higher temperature exponentially increases rate constant.

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

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

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