days 1- 2 Flashcards
kinetics
how fast things change. area of chemistry concerned with reaction rates and sequence of steps in which a reaction occurs
reaction rate
the increase in concentration of a product per unit of time or the decrease in concentration of a reactant per unit of time
rate law
an equation that shows the dependance of the reaction rate on the concentration of each reactant
halflife
the time required for the reactant concentration to reach 1/2 of its original value
arrhenius equation
equation that finds reaction rates including tempurature
typically, as tempurature increases…
the molecular speed is faster and more collisions occur, causing faster reaction rate(s)
transition state
the configuration of atoms at the maximum in the potential energy profile (top of the action potential bell curve)
collision theory
as the average kinetic energy increases, the average molecular speed increases, and thus the collision rate increases
reaction mechanism
a sequence of reaction steps that describes the pathway from reactants to products
elementary reaction
a single step in a reaction mechanism (describes individual molecular events)
overall reaction
describes the reaction stoichiometry and is a sum of all elementary reactions (all elementary reactions MUST sum to the overall reaction)
reactive intermediate
is not a product OR reactant but helps get to final products, formed in one step and consumed in a subsiquent one
molecularity
a classification of an elementary reaction based on the number of molecules (or atoms) on the reactant side of the chemical equation
unimolecular, bimolecular, termolecular
rate determining step
the slow step in a reaction mechanism that acts as a bottleneck and limits the rate at which reactants can be converted into products
catalyst
a substance that increases the rate of a reaction. it is not itself consumed in the reaction, used in one step and regenerated in a later step
