A chemical reaction that involves only one single phase, meaning all reactants and products coexist uniformly in the same gas or liquid phase without phase boundaries.
Heterogeneous Reaction
A chemical reaction that includes more than one phase, where the chemical transformation typically takes place directly at the interface between the distinct phases.
Irreversible Reaction
A reaction that occurs strictly in one direction and continues forward until all the available reactants are completely consumed, unlike reversible equilibria systems.
Reversible Reaction
A reaction that can proceed in either the forward or reverse direction, depending on the relative concentrations of reactants and products compared to equilibrium concentrations.
Molecularity
The exact number of atoms, ions, or molecules that collide simultaneously in a given reaction step to form products or intermediates.
Unimolecular Reaction
A reaction step containing a single atom or molecule undergoing decomposition or rearrangement, such as the radioactive decay of uranium.
Bimolecular Reaction
A reaction step containing two atoms or molecules colliding simultaneously, which represents one of the most common collision types in chemical kinetics.
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Termolecular Reaction
A reaction step containing three atoms or molecules colliding simultaneously, which has an extremely low statistical probability of occurring directly in nature.
Reaction Rate Constant (k)
A proportionality factor in rate laws that is a direct function of temperature and determines the intrinsic speed of a chemical reaction.
Reaction Order
The sum of the powers to which the reactant concentrations are raised in a kinetic rate law, determining how concentration changes affect the reaction rate.
