Leighton relationship

In atmospheric chemistry, the Leighton relationship is an equation that determines the concentration of tropospheric ozone in areas polluted by the presence of nitrogen oxides. Ozone in the troposphere is primarily produced through the photolysis of nitrogen dioxide by photons with wavelengths (λ) less than 420 nanometers[1], which are able to reach the lowest levels of the atmosphere, through the following mechanism:[2]

NO2 + hν (λ < 420 nm) → NO + O (3P)

 

 

 

 

(J1)

O (3P) + O2 + M → O3 + M

 

 

 

 

(k2)

NO + O3 → NO2 + O2

 

 

 

 

(k3)

This series of reactions creates a null cycle, in which there is no net production or loss of any species involved. Since O (3P) is very reactive and O2 is abundant, O (3P) can be assumed to be in steady state, and thus an equation linking the concentrations of the species involved can be derived:

The Leighton relationship above shows how production of ozone is directly related to the solar intensity, and hence to the zenith angle, due to the reliance on photolysis of NO2. The yield of ozone will therefore be greatest during the day, especially at noon and during the summer season. This relationship also demonstrates how high concentrations of both ozone and nitric oxide are unfeasible.[3] However, NO can react with peroxyl radicals to produce NO2 without loss of ozone:

RO2 + NO → NO2 + RO

thus providing another pathway to allow for the buildup of ozone by breaking the above null cycle.

This relationship is named after Philip Leighton, author of the groundbreaking 1961 book Photochemistry of Air Pollution, as recognition of his contributions in the understanding of tropospheric chemistry. Computer models of atmospheric chemistry utilize the Leighton relationship to minimize complexity by deducing the concentration of one of ozone, nitrogen dioxide, and nitric oxide when the concentrations of the other two are known.[1]

References
  1. Barbara J. Finlayson-Pitts; James N. Pitts (2000). Chemistry of the Upper and Lower Atmosphere: Theory, Experiments, and Applications. Academic Press. p. 266. ISBN 9780122570605.
  2. John Roger Barker (1995). Progress And Problems In Atmospheric Chemistry. World Scientific. p. 22. ISBN 9789810221133.
  3. James Pfafflin; Edward Ziegler (2006). Encyclopedia of Environmental Science And Engineering. 1. CRC Press. p. 122. ISBN 9780849398438.
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