AP Chemistry Unit 5 Test

Front

What is an elementary reaction?

Back

An elementary reaction is a single step reaction that describes a direct interaction between reactants, resulting in products without any intermediates.

Front

Define reaction rate.

Back

The reaction rate is the speed at which reactants are converted into products in a chemical reaction, typically expressed as the change in concentration of a reactant or product per unit time.

Front

What is an intermediate in a chemical reaction?

Back

An intermediate is a species that is formed in one step of a reaction mechanism and consumed in a subsequent step.

Front

How does the orientation of reactants affect reaction rates?

Back

The orientation of reactants affects reaction rates because only certain orientations lead to successful collisions that result in a reaction.

Front

What is the rate law for a reaction?

Back

The rate law is an equation that relates the rate of a reaction to the concentration of the reactants, typically in the form rate = k[A]^m[B]^n, where k is the rate constant and m and n are the orders of the reaction.

Front

What is the significance of the slow step in a reaction mechanism?

Back

The slow step in a reaction mechanism determines the overall rate of the reaction, as it is the step that limits how quickly the reaction can proceed.

Front

Explain the concept of collision theory.

Back

Collision theory states that for a reaction to occur, reactant particles must collide with sufficient energy and proper orientation.

Front

What is the difference between a fast and slow reaction step?

Back

A fast reaction step occurs quickly and does not significantly affect the overall rate, while a slow reaction step takes longer and determines the overall rate of the reaction.

Front

How do you determine the overall rate of a reaction mechanism?

Back

The overall rate of a reaction mechanism is determined by identifying the slowest step in the mechanism.

Front

What is the role of catalysts in chemical reactions?

Back

Catalysts speed up chemical reactions by lowering the activation energy, allowing more collisions to result in a reaction without being consumed in the process.