5.4 Collision Model

    Cards (54)

    • For a reaction to occur, the collision must possess sufficient energy to overcome the activation energy.
    • For a collision to be effective, it must have sufficient energy to overcome the activation energy.
    • Collision frequency refers to the number of collisions between reactant particles per unit time.
    • Lower collision frequency results in a slower reaction rate.

      True
    • Higher temperature increases collision frequency.

      True
    • What does the collision model describe?
      Reaction mechanisms
    • What is the minimum energy required for a successful collision called?
      Activation energy
    • What type of relationship exists between activation energy and reaction rate?
      Inverse
    • What happens to the kinetic energy of molecules when temperature increases?
      Increases
    • What is activation energy in the collision model?
      Minimum energy for reaction
    • Why is correct spatial arrangement important for a collision in a chemical reaction?
      Facilitates bond formation
    • What is the effect of higher collision frequency on reaction rate?
      Increases reaction rate
    • What is collision frequency measured in?
      Per unit time
    • What is one key factor that influences collision frequency?
      Concentration
    • Higher pressure increases collision frequency.
    • Sufficient energy is needed to overcome the activation energy.
    • Order the following concepts from general to specific:
      1️⃣ Collision frequency
      2️⃣ Reaction rate
      3️⃣ Activation energy
    • Higher activation energy results in a slower reaction rate.

      True
    • High activation energy results in a slow reaction rate.
    • Higher temperature leads to lower activation energy.
    • Summarize the two necessary conditions for a successful reaction according to the collision model:
      1️⃣ Energy greater than activation energy
      2️⃣ Correct spatial orientation
    • What is collision frequency defined as?
      Collisions per unit time
    • Activation energy is the minimum energy required for a reaction to occur.

      True
    • For the reaction A + B → C + D, the activation energy is the barrier for A and B to combine
      True
    • Reactions with low activation energy require more energy to initiate.
      False
    • Steps for a reaction to occur according to the collision model
      1️⃣ Particles collide with sufficient energy
      2️⃣ Energy exceeds activation energy
      3️⃣ Particles collide with correct orientation
      4️⃣ New bonds form, products emerge
    • What happens to the reaction rate if the activation energy is increased?
      Reaction rate slows down
    • What does the collision model describe in chemistry?
      How reactions occur
    • Correct orientation of reactant molecules is necessary for bond formation in a reaction.

      True
    • If either energy or correct orientation is insufficient, the collision will not result in a successful reaction.

      True
    • Higher concentration of reactants increases collision frequency.
      True
    • Higher collision frequency generally leads to a faster reaction rate.
    • Higher concentration increases collision frequency.
    • Match the phase with its relative collision frequency:
      Gases ↔️ High
      Liquids ↔️ Moderate
      Solids ↔️ Low
    • Correct orientation is necessary for a successful collision.

      True
    • Higher collision frequency generally leads to a faster reaction rate.
    • What is the relationship between activation energy and reaction rate?
      Inverse
    • Reactions requiring a lot of energy to initiate proceed more quickly.
      False
    • The nature of reactants does not influence activation energy.
      False
    • Reactions with weak bonds have lower activation energy.
    See similar decks