Equilibrium isotope fractionation is the partial separation of isotopes between two or more substances in chemical equilibrium. Equilibrium fractionation is strongest at low temperatures, and forms the basis of the most widely used isotopic paleothermometers : D/H and 18O/16O records from ice cores, and 18O/16O records from calcium carbonate. It is thus important for the construction of geologic temperature records. Isotopic fractionations attributed to equilibrium processes have been observed in many elements, from hydrogen to uranium. In general, the light elements are most susceptible to fractionation, and their isotopes tend to be separated to a greater degree than heavier elements.
Definition
Most equilibrium fractionations are thought to result from the reduction in vibrational energy when a more massive isotope is substituted for a less massive one. This leads to higher concentrations of the massive isotopes in substances where the vibrational energy is most sensitive to isotope substitution, i.e., those with the highest bond force constants. In a reaction involving the exchange of two isotopes, X and X, of element "X" in moleculesAX and BX, each reactantmolecule is identical to a product except for the distribution of isotopes. The amount of isotopic fractionation in an exchange reaction can be expressed as a fractionation factor: indicates that the isotopes are distributed evenly between AX and BX, with no isotopic fractionation. indicates that X is concentrated in substance AX, and indicates X is concentrated in substance BX. is closely related to the equilibrium constant : where is the product of the rotational symmetry numbers of the products, is the product of the rotational symmetry numbers of the reactants, and is the number of atoms exchanged. An example of equilibrium isotope fractionation is the concentration of heavy isotopes of oxygen in liquid water, relative to water vapor, At 20 °C, the equilibrium fractionation factor for this reaction is Equilibrium fractionation is a type of mass-dependent isotope fractionation, while mass-independent fractionation is usually assumed to be a non-equilibrium process. For non-equilibrium reactions, isotopic effects are better described by the GEBIK and GEBIF equations for transient kinetic isotope fractionation, which generalize non-steady isotopic effects in any chemical and biochemical reactions.
Example
When water vapor condenses, the heavier water isotopes become enriched in the liquid phase while the lighter isotopes tend toward the vapor phase.
