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AP Chemistry
Unit 5: Kinetics
5.4 Collision Model
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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.
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