| A | B |
|---|
| collision theory | for reaction to happen reacting molecules must collide with one another with sufficient energy to break bonds and with proper orientation |
| reactions are...at higher T bc... | faster, a larger fraction of reactant molecules have enough energy to convert to product molecules and there are more collisions |
| activation energy | minimum amount of energy to react. or energy required to form the activated complex |
| transition state | highest E, bonds 1/2 broken. there is an activated complex that has sufficent energy to become a product |
| catalysts | neither consumed or produced by a reaction (dont appear in balanced equation). change the mechanism of the reaction. lower activation energy of a reaction allowing it to reach equilibrium much faster. homogenous or heterogenuos |
| mechanism | the sequence of elementary steps that make up the overall reaction |
| elementary step | a process occurring for a small number of moleculs |
| unimolecular | occurs to one isolates molecule with enough energy |
| bimolecular | two molecules collide with enough energy |
| termolecular | stimultaneous collision of three molecules with enough energy is of very low probability unless concentrations are very high |
| for an elementary reaction and only an elementary reaction the rate is... | the rate constant multiplied by the concentration of all reactants raised to the power of their balanced coefficients |
