Collision Theory and Activation Theory Flashcards

1
Q

What are the two basic assumptions of the collision theory?

A
  1. For a reaction to occur, the reacting particles must collide with each other
  2. A collision only results in the formation of products if a certain minimum energy is exceeded in the collision. Such a collision is called an effective collision
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2
Q

Define an effective collision

A

Is a collision that results in the formation of products

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3
Q

What happens when an effective collision occurs?

A

Bonds are broken and new bonds are formed

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4
Q

What does the breaking of bonds and formation of new bonds in an effective collision result in?

A

The formation of products

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5
Q

According to the collision theory, what does the rate of reaction depend on?

A

The number of collisions per second that take place between the reacting particles
The fraction of these collisions that are effective

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6
Q

The total number of collisions does not determine the rate of reactions, instead what does?

A

The number of effective collisions

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7
Q

What happens when molecules with low energies collide?

A

They simply bounce apart without any reaction taking place

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8
Q

Only what type of molecules form products when they collide?

A

High enough energy molecules

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9
Q

A certain amount of what is necessary for a chemical reaction to occur when molecules collide?

A

Energy

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10
Q

Define activation energy

A

The minimum energy that colliding particles must have for a reaction to occur

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11
Q

How does collision theory explain why reactions are faster at higher temperatures?

A

As a greater number of collisions reach the activation energy

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12
Q

Define an energy profile diagram

A

A graph which shows the change in energy of a chemical reaction with time as the reaction progresses

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