Explaining Reaction Rates Flashcards
What does the collision theory state?
That chemical reactions occur if reactant atoms, molecules or ions collide
First criteria for collision theory to be successful
Correct orientation
Second criteria for collision theory to be successful
Sufficient kinetic energy to break the bonds in the reactants
What does the rate of reaction depend on?
The frequency and proportion of successful collisions that convert reactants to products
An increase in successful collisions correlates too…
An increase in reaction rate
Correct Orientation
- Reactants need to face the right way so that a new chemical bond can be formed
- Can have more then one “correct” orientation
What happens if reactants don’t have the correct orientation?
The reactant bond will break but the desired chemical bond will not form
Activation Energy
Minimum amount of energy a reactant must have for a collision to be effective
An increase in activation energy correlates too…
- Decrease in the # of collisions
- Decrease in reaction rate
Transition State
Highest energy point of the graph where the activated complex is formed
Activated Complex
Unstable arrangement of atoms at the peak of the potential energy hill
Effective collions at activated complex…
Break into the products
Ineffective collisions at activated complex…
Break into the reactants
