Part 1: Oxidation and OH radicals – Harvard University

Loading...

Taking too long?

Reload document

| Open in new tab

Part 1: Oxidation and OH radicals

Oxidation in the Atmosphere

Many chemical compounds are emitted into the atmosphere but removal
processes prevent them accumulating in the air. Species are removed
by dry deposition of gases or particles or can be incorporated into rain
and removed by wet deposition. For gas phase organic chemicals,
removal is easiest if they are first oxidised to a less volatile, water
soluble form.

Oxidation in a chemical sense does not necessarily
mean a reaction with oxygen containing compounds, it
is rather the loss of electrons. However, in the air,
oxidation does generally involve the reaction of a
chemical species with an oxygen containing compound.

The three most important oxidising species in the air
are:

1. Hydroxyl radicals (OH)
clean the air. Image:
Elmar Uherek.

the hydroxyl radical OH
the nitrate radical NO3
the ozone molecule O3

Hydroperoxy radicals (HO2) are also important and the
sum of HO2 and OH is sometimes referred to as HOx.

The most important oxidising species is the hydroxyl
radical (OH). It is extremely reactive and able to
oxidise most of the chemicals found in the
troposphere. The hydroxyl radical is therefore known as
the ‘detergent of the atmosphere’.

Only a few compounds in the
troposphere do not react at all or
react only very slowly with the
hydroxyl radical. These
include the chlorofluorocarbons
(CFC’s), nitrous oxide (N2O) and
carbon dioxide (CO2). The rate of
methane (CH4) oxidation by OH is
also very slow, between 100 and
1000 times slower than other
organic compounds. This is why
methane concentrations in the
atmosphere can reach around 1.7
ppm (1.7 µmol mol-1), a value
significantly higher than
the concentrations of other
organic trace gas concentrations
present which are generally below
1 ppb (1 nmol mol-1)*.

2. Formation of OH: More than 97% of the O atoms
which are formed by photolysis of ozone, react back
again to ozone. Less than 3% start the formation of
the most important radical in the atmosphere, OH. If
two molecules or atoms collide to form a product,
a third species M is needed to take away some excess
energy. M (usually nitrogen N2) does not react itself.

ESPERE Climate Encyclopaedia – www.espere.net – Lower Atmosphere More – page 2
English offline version
supported by the International Max Planck Research School on Atmospheric Chemistry and Physics

How is OH formed?

OH governs atmospheric
chemistry during the day since its
formation depends on radiation
from the Sun. The initial reaction
(shown above) involves the
breakdown (photolysis) of ozone
by solar radiation
with wavelengths less than 310
nm. The oxygen atom (O) formed
then reacts with water to form
OH. This reaction mechanism
is why a small amount of ozone is
essential in the troposphere.
Other sources of OH are:
the photolysis of nitrous acid
(HONO), hydrogen peroxide
(H2O2) or peroxy-methane
(CH3OOH)
the reaction of nitrogen monoxide
(NO) with the hydroperoxy radical
(HO2) or the reaction of alkenes
with ozone.
The scheme on the left shows
how OH chemistry is
fundamentally linked with the
day-time reaction cycles of the
nitrogen oxides.

4. Zonal distribution of OH. A pressure of 250 hPa is
reached at roughly 11 km altitude (the tropopause in
the mid latitudes). Source: presentation by J. Lelieveld
– MPI Mainz, 2003.

3. OH and the nitrogen oxide cycle
Scheme by Elmar Uherek

How much OH is formed?

Since OH is an extremely reactive
radical it reacts as soon as it is
formed. It’s lifetime is less than a
second. This means the
concentration is extremely low, in
the range of 1×105 to 2×107
molecules cm-3. At sea level
pressure this is equivalent to a
mixing ratio of 0.01 – 1 ppt.
Since it’s formation depends
on water vapour, the
concentration of OH tends to
decrease with altitude as the
air becomes cooler and drier.

ESPERE Climate Encyclopaedia – www.espere.net – Lower Atmosphere More – page 3
English offline version
supported by the International Max Planck Research School on Atmospheric Chemistry and Physics

Hydroxyl radical concentrations
not only decrease with altitude
but also decrease with latitude
since both the water vapour
concentrations and sunlight
intensity decrease as you move
towards the poles.

How does OH react?

The figure on the right shows low
levels of OH near the ground
over the tropical rainforest. Why
is this the case? Plants emit
organic gases with isoprene being
the most abundant. This isoprene
reacts with OH, removing it from
the air, and forming water and a
reactive organic radical (R). OH
has a strong tendancy to remove
(abstract) a hydrogen atom from
organic species (RH) whenever
possible. The organic radical
(R) then reacts with oxygen (O2)
to form organic peroxides (RO2).
These compounds are an essential
part of the ozone formation cycle.

On a global scale, OH reacts primarily with carbon monoxide (40%) to form
carbon dioxide. Around 30% of the OH produced is removed from the
atmosphere in reactions with organic compounds and 15% reacts with methane
(CH4). The remaining 15% reacts with ozone (O3), hydroperoxy radicals (HO2)
and hydrogen gas (H2).

5. OH distribution in the tropics. Top: the global
distribution in tropical regions, below: profile over the
Manaus rain forest station (Brazil). Source:
p
resentation J. Lelieveld MPI Mainz, 2003.

The oxidation of carbon monoxide
and methane by OH are very
important as they are the major
ways by which OH is removed
from the atmosphere. Reaction of
OH with alkenes, a special class of
organic compounds, is also very
important as this reaction results
in the formation of peroxides.

6 . Important OH reactions in the troposphere.

ESPERE Climate Encyclopaedia – www.espere.net – Lower Atmosphere More – page 4
English offline version
supported by the International Max Planck Research School on Atmospheric Chemistry and Physics

OH is the most important oxidant
in the atmosphere. However OH
concentrations are close to zero
during the night since sunlight is
needed for its formation. So
during dark periods and during
night-time, ozone and nitrate
radical (NO3) chemistry become
important.

7. Time profile of OH concentrations over several
days. Source: Presentation J. Lelieveld MPI Mainz,
2
* The mixing ratio ppb (1 molecule in 1 billion molecules of air) or ppm (1 molecule in 1 million
molecules of air) is often used in scientific publications as well as in other literature on the
atmosphere and climate. Because of this we use it here in the Climate Encyclopaedia. However, the
correct unit is 1 nmol mol-1 (equivalent to 1 ppb) or 1 µmol m-1 (for 1 ppm) since mole is the
standard unit of concentration.

003.

Part 2: Night and nitrate

Night-time conditions and chemistry

The chemistry of the atmosphere depends not only on the chemical
compounds present in the air but also on the physical conditions. These
physical conditions depend, for example, on the season, whether it’s day
or night, what the temperature is and how humid the air is.

The diurnal cycle

In the last section we saw that
OH concentrations are highest
during the day and approach zero
at night when there is no sunlight
present. Temperature and other
physical properties also show
a diurnal or daily cycle.
Conditions close to the ground in
the planetary boundary layer vary
and do not always follow the
general rule (e.g. of decreasing
temperature with increasing
altitude) because of interactions
with the Earth’s surface. A very
typical example is the night-time
inversion layer which collapses in
the morning.

1. Collapsing temperature inversion on a July
morning (Isar Valley / Germany). By Elmar Uherek
and adapted from: Schirmer – Wetter und Klima – Wie
f
unktioniert das?

ESPERE Climate Encyclopaedia – www.espere.net – Lower Atmosphere More – page 5
English offline version
supported by the International Max Planck Research School on Atmospheric Chemistry and Physics