1.5.2 Collision Theory

• According to collision theory, chemical reactions occur when reactant particles collide with sufficient energy
• Higher activation energy requires more energy
• According to collision theory, reactions occur when particles collide with sufficient energy and the correct orientation
• The Maxwell-Boltzmann distribution shows that particles in a gas all have the same speed.

  False
• At lower temperatures, more particles move at slower speeds
• A higher frequency of collisions always leads to a faster reaction rate.

  False
• Match the collision factor with its effect:

  Orientation ↔️ Correct alignment needed

  Energy ↔️ Overcomes activation energy

  Frequency ↔️ Higher frequency leads to faster reaction
• What is the second requirement for an effective collision according to collision theory?

  Correct orientation
• Collisions in the correct orientation are more likely to result in a successful reaction.


  True
• How does higher temperature affect collision frequency?

  Increases collision frequency
• Match the collision factor with its effect on reaction success:

  Energy ↔️ Overcomes activation energy

  Orientation ↔️ Ensures correct bond formation
• Catalysts increase the rate of reaction by lowering the activation energy barrier.


  True
• The key factors affecting the rate of a chemical reaction are collision frequency, energy, and orientation.


  True
• Match the factor with its effect on collision frequency:

  Concentration ↔️ Higher concentration increases collision frequency

  Temperature ↔️ Higher temperature increases collision frequency
• Match the factor with its effect on collision success:

  Energy ↔️ Overcomes activation energy barrier

  Orientation ↔️ Ensures correct alignment for bonding
• What does the Maxwell-Boltzmann distribution describe?

  Particle speeds in a gas
• Collision theory explains that reactions occur when particles collide with sufficient energy and correct orientation.
• Higher collision frequency increases the rate of reaction according to collision theory.
• Effective collisions require sufficient energy to overcome the activation energy barrier.


  True
• Why is activation energy a key factor in effective collisions?

  Energy threshold for reaction
• Higher concentration of reactant particles increases collision frequency.


  True
• Higher kinetic energy of particles increases the likelihood of successful collisions.
• Higher temperatures relate to collision theory by increasing the frequency of collisions.
• Catalysts speed up reactions by lowering the activation energy required.
• Only effective collisions lead to the formation of products in a chemical reaction.

  True
• The frequency of collisions is influenced by concentration and temperature
• At higher temperatures, more particles move at faster speeds.
• Higher temperatures result in more particles moving at faster speeds according to the Maxwell-Boltzmann distribution.


  True
• Why is collision energy important in collision theory?

  Overcomes activation energy
• Higher activation energy requires more energy in the collision to react.
• Only effective collisions lead to the formation of products in a chemical reaction.
• Arrange the steps to explain how temperature affects collision frequency:

  1️⃣ Higher temperature

  2️⃣ Particles move faster

  3️⃣ More frequent and forceful collisions

  4️⃣ Faster reaction rate
• What happens to the Maxwell-Boltzmann distribution as temperature increases?

  Shifts to the right
• How do catalysts affect the frequency of effective collisions?

  Increase frequency