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An elementary reaction is a chemical reaction in which one or more of the chemical species react directly to form products in a single reaction step and with a single transition state.[1] An apparent ("operational") reaction may be in fact stepwise reactions, i.e. a complicated sequence of chemical reactions, with reaction intermediates of variable lifetimes.

In a unimolecular elementary reaction, a molecule A dissociates or isomerises to form the products(s)

$\mbox{A} \rightarrow \mbox{products.}$

At constant temperature, the rate of such a reaction is proportional to the concentration of the species A

$\frac{d[\mbox{A}]}{dt}=-k[\mbox{A}].$

In a bimolecular elementary reaction, two atoms, molecules, ions or radicals, A and B, react together to form the product(s)

$\mbox{A + B} \rightarrow \mbox{products.}$

The rate of such a reaction, at constant temperature, is proportional to the product of the concentrations of the species A and B

$\frac{d[\mbox{A}]}{dt}=\frac{d[\mbox{B}]}{dt}=-k[\mbox{A}][\mbox{B}].$

The rate expression for an elementary bimolecular reaction is sometimes referred to as the Law of Mass Action as it was first proposed by Guldberg and Waage in 1864. An example of this type of reaction is a cycloaddition reaction. This rate expression can be derived from first principles by using collision theory for ideal gases. For the case of dilute fluids equivalent results have been obtained from simple probabilistic arguments.[2]

According to collision theory the probability of three chemical species reacting simultaneously with each other in a termolecular elementary reactions is negligible. Hence such termolecular reactions are commonly referred as non-elementary reactions and can be broken down into a more fundamental set of bimolecular reactions,[3][4] in agreement with the law of mass action. However it is not always possible to derive overall reaction schemes but solutions based on rate equations are possible in terms of steady-state or Michaelis-Menten approximations.

## reaction mechanismEdit

In chemistry, a reaction mechanism is the step by step sequence of elementary reactions by which overall chemical change occurs.[5]

A chemical mechanism describes in detail exactly what takes place at each stage of an overall chemical reaction (transformation). It also describes each reactive intermediate, activated complex, and transition state, and which bonds are broken (and in what order), and which bonds are formed (and in what order). A complete mechanism must also account for all reactants used, the function of a catalyst, stereochemistry, all products formed and the amount of each. It must also describe the relative rates of the reaction steps and the rate equation for the overall reaction. Reaction intermediates are chemical species, often unstable and short-lived, which are not reactants or products of the overall chemical reaction, but are temporary products and reactants in the mechanism's reaction steps. Reaction intermediates are often free radicals or ions. Transition states can be unstable intermediate molecular states even in the elementary reactions. Transition states are commonly molecular entities involving an unstable number of bonds and/or unstable geometry. They correspond to maxima on the reaction coordinate, and to saddle points on the potential energy surface for the reaction.

The electron or arrow pushing method is often used in illustrating a reaction mechanism; for example, see the illustration of the mechanism for benzoin condensation in the following examples section.

A reaction mechanism must also account for the order in which molecules react. Often what appears to be a single-step conversion is in fact a multistep reaction.

### Chemical kineticsEdit

Information about the mechanism of a reaction is often provided by the use of chemical kinetics to determine the rate equation and the reaction order in each reactant.[6]

Consider the following reaction for example:

CO + NO2 → CO2 + NO

In this case, experiments have determined that this reaction takes place according to the rate law $r = k[NO_2]^2$. This form suggests that the rate-determining step is a reaction between two molecules of NO2. A possible mechanism for the overall reaction that explains the rate law is:

2 NO2 → NO3 + NO (slow)
NO3 + CO → NO2 + CO2 (fast)

Each step is called an elementary step, and each has its own rate law and molecularity. The elementary steps should add up to the original reaction. (Meaning, if we were to cancel out all the molecules that appear on both sides of the reaction, we would be left with the original reaction.)

When determining the overall rate law for a reaction, the slowest step is the step that determines the reaction rate. Because the first step (in the above reaction) is the slowest step, it is the rate-determining step. Because it involves the collision of two NO2 molecules, it is a bimolecular reaction with a rate law of $r = k[NO_2]^2$.

Other reactions may have mechanisms of several consecutive steps. In organic chemistry, one of the first reaction mechanisms proposed was that for the benzoin condensation, put forward in 1903 by A. J. Lapworth.

There are also more complex mechanisms such as chain reactions, in which the propagation steps of the chain form a closed cycle.

### Other experimental methods to determine mechanismEdit

Many experiments that suggest the possible sequence of steps in a reaction mechanism have been designed, including:

### Theoretical modelingEdit

A correct reaction mechanism is an important part of accurate predictive modeling. For many combustion and plasma systems, detailed mechanisms are not available or require development.

Even when information is available, identifying and assembling the relevant data from a variety of sources, reconciling discrepant values and extrapolating to different conditions can be a difficult process without expert help. Rate constants or thermochemical data are often not available in the literature, so computational chemistry techniques or group additivity methods must be used to obtain the required parameters.

Computational chemistry methods can also be used to calculate potential energy surfaces for reactions and determine probable mechanisms.[19]

### MolecularityEdit

Main article: molecularity

Molecularity in chemistry is the number of colliding molecular entities that are involved in a single reaction step.

• A reaction step involving one molecular entity is called unimolecular.
• A reaction step involving two molecular entities is called bimolecular.
• A reaction step involving three molecular entities is called termolecular.

In general, reaction steps involving more than three molecular entities do not occur.

## ReferencesEdit

1. Template:GoldBookRef
2. Gillespie, D.T., A diffusional bimolecular propensity function, The Journal of Chemical Physics 131, 164109 (2009)
3. Cook, GB and Gray, P. and Knapp, DG and Scott, SK, Bimolecular routes to cubic autocatalysis, The Journal of Physical Chemistry 93, 2749--2755 (1989)
4. Aris, R. and Gray, P. and Scott, SK, Modelling cubic autocatalysis by successive bimolecular steps, Chemical Engineering Science 43', 207--211 (1988)
5. Template:JerryMarch
6. Espenson, James H. Chemical Kinetics and Reaction Mechanisms (2nd ed., McGraw-Hill, 2002) chap.6, Deduction of Reaction Mechanisms ISBN 0-07-288362-6
7. Espenson p.156-160
8. Morrison R.T. and Boyd R.N. Organic Chemistry (4th ed., Allyn and Bacon 1983) p.216-9 and p.228-231, ISBN 0-205-05838-8
9. Atkins P and de Paula J, Physical Chemistry (8th ed., W.H. Freeman 2006) p.816-8 ISBN 0-7167-8759-8
10. Moore J.W. and Pearson R.G. Kinetics and Mechanism (3rd ed., John Wiley 1981) p.276-8 ISBN 0-471-03558-0
11. Laidler K.J. and Meiser J.H., Physical Chemistry (Benjamin/Cummings 1982) p.389-392 ISBN 0-8053-5682-7
12. Atkins and de Paula p.884-5
13. Laidler and Meiser p.388-9
14. Atkins and de Paula p.892-3
15. Atkins and de Paula p.886
16. Laidler and Meiser p.396-7
17. Investigation of chemical reactions in solution using API-MS Leonardo Silva Santos, Larissa Knaack, Jurgen O. Metzger Int. J. Mass Spectrom.; 2005; 246 pp 84 - 104; (Review) Template:Doi
18. Espenson p.112
19. Atkins and de Paula p.887-891