R.2.2 how fast?

hmm....

rate of reaction

the speed at which a chemical reaction takes place (ex. change in concentration of a reactant/product per unit time)

steric effect

3d shape, orientation, and size of colliding molecules affect how particles approach and react to one another (affects reaction rate)

activation energy

minimum amount of energy a reactant must have for a collision to be effective

maxwell-boltzmann distribution

describes distribution of KE among particles in an ideal gas at a given temperature. shows how molecular speeds vary and provides insight into how temperature affects reaction rates

enzymes

biological catalysts that speed up chemical reactions in living organisms

substrate

a substance acted upon by an enzyme at its active site

active site

the region on the surface of an enzyme molecule that binds the substrate molecule

reaction mechanism

a series of elementary steps by which a chemical reaction occurs

elementary steps

a reaction with no intermediates; a reaction that takes place in a single step with a single transition state (most commonly unimolecular or bimolecular)

intermediate

a species which is not a reactant or a product but which is formed in one stpe of a reaction and used up in the next

rate determining step (RDS)

the slowest elementary step in a chemical reaction that involves a number of elementary steps

order

shows how the concentration of a chemical, typically a reactant, affects the rate of reaction

transition state

point at which new bonds are being formed and old bonds are being broken

pseudo-first-order reaction

a second order reaction that is made to behave like a first order reaction

collision theory

for a reaction to occur particles must collide in the correct orientation with E > Ea