Diagram of a catalytic reaction, showing the energy niveau as a function of the reaction coordinate. For a catalyzed reaction, the activation energy is lower.

In chemistry, a reaction coordinate[1] is an abstract one-dimensional coordinate chosen to represent progress along a reaction pathway. Where possible it is usually a geometric parameter that changes during the conversion of one or more molecular entities, such as bond length or bond angle. For example, in the homolytic dissociation of molecular hydrogen, an apt choice would be the coordinate corresponding to the bond length. Non-geometric parameters such as bond order are also used, but such direct representation of the reaction process can be difficult, especially for more complex reactions.

Molecular dynamics simulations often use collective variables to promote unusual but interesting states. The term collective variable may describe any function of the atom positions. Special collective variables that help to distinguish reactants from products are known as order parameters, terminology that originates in work on phase transitions.[2] Reaction coordinates are special order parameters that describe the entire pathway from reactants through transition states and on to products. Depending on the application, reaction coordinates may be defined by using chemically intuitive variables like bond lengths, or splitting probabilities (also called committors), or using the eigenfunction corresponding to the reactant-to-product transition as a progress coordinate.[3]

A reaction coordinate parameterizes reaction process at the level of the molecular entities involved. It differs from extent of reaction, which measures reaction progress in terms of the composition of the reaction system.

(Free) energy is often plotted against reaction coordinate(s) to demonstrate in schematic form the potential energy profile (an intersection of a potential energy surface) associated with the reaction.

In the formalism of transition-state theory the reaction coordinate for each reaction step is one of a set of curvilinear coordinates obtained from the conventional coordinates for the reactants, and leads smoothly among configurations, from reactants to products via the transition state. It is typically chosen to follow the path defined by potential energy gradient – shallowest ascent/steepest descent – from reactants to products.[1]

Notes and references

  1. ^ a b IUPAC, Compendium of Chemical Terminology, 2nd ed. (the "Gold Book") (1997). Online corrected version: (2006–) "reaction coordinate". doi:10.1351/goldbook.R05168
  2. ^ "Principles of condensed matter physics. P. Chaikin and T. Lubensky, Cambridge University Press, Cambridge, England, 1995".
  3. ^ "Reaction coordinates and mechanistic hypothesis tests, Ann. Rev. Phys. Chem., B. Peters (2016)".


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