• Collision Model: the energy (for breaking bonds of reactants) comes from the kinetic energies possessed by the reacting molecules before the collision

           ○ Key idea: the rate of a reaction depends on the number of successful collisions and these collisions provide the energy for molecules to react and form products

  • In order for a reaction to occur and products to be made

          ○ Reactant molecules must collide

          ○ Must collide with enough energy

          ○ Must make contact at correct molecular orientation that allow the bonds to rearrange in the required manner

                 ■ Collision orientation is important for molecules, but not for atoms

  • Only a small fraction of collisions produce a reaction bcuz…

          ○ The collision energy must equal or exceed the activation energy

           ○ Reactants must collide at a correct molecular orientation

                ■ Is why the observed rate of reaction is less than the number of collisions that have the minimum energy