With reductive workup e. With oxidative workup e. Ozone, along with reactive forms of oxygen such as superoxide, singlet oxygen, hydrogen peroxide, and hypochlorite ions, is naturally produced by white blood cells and other biological systems such as the roots of marigolds as a means of destroying foreign bodies. Ozone reacts directly with organic double bonds. When ozone breaks down to dioxygen, it produces oxygen free radicals, which are highly reactive and capable of damaging many organic molecules.
Moreover, it is believed that the powerful oxidizing properties of ozone may be a contributing factor of inflammation. The cause-and-effect relationship of how the ozone is created in the body and what it does is still under consideration and still subject to various interpretations, since other body chemical processes can trigger some of the same reactions.
Boundless vets and curates high-quality, openly licensed content from around the Internet. This particular resource used the following sources:. Skip to main content. Nonmetallic Elements. Search for:. CFCs are stable. This may be great in an appliance like a refrigerator, but this is disastrous for CFCs that find their way up into the atmosphere. CFCs do not react easily with other chemicals in the lower atmosphere troposphere.
But as CFCs rise, they move into the stratosphere. They release chlorine, and these free chlorine atoms rip oxygen atoms off of ozone, leaving ordinary oxygen gas. This oxygen atom will break apart the chlorine monoxide, releasing the chlorine atom back into the stratosphere to degrade more ozone.
The chlorine atoms keep cycling through the process of breaking up ozone, and it has upset the balance of the ozone system. This reaction happens over and over again, allowing one chlorine atom to destroy many ozone molecules. When a free chlorine atom reacts with other gases that contain hydrogen, the chlorine will be bound to the hydrogen to form HCl hydrochloric acid.
This can be carried into the troposphere and washed away by rain or snow. If humans then quit putting CFCs into the atmosphere, the ozone layer could eventually in theory repair itself. Termite mounds and rice paddies are also significant producers of methane. Ozone formation with the hydrocarbon methane provides a useful example of the general pattern that most such reactions follow.
The methane example is somewhat simpler and easier to follow than the others, described in steps. Most ozone formations in the troposphere involve non-methane hydrocarbons. The chemistry of ozone formation from non-methane hydrocarbons follows the general pattern described above but is much more complex. NO x and VOCs together include about different chemical compounds, and hundreds of chemical reactions can take place. Some of the participating chemicals may be intercepted part of the way through the process by reactions with other chemicals in the atmosphere, and may form intermediate compounds that act as temporary reservoirs for varying amounts of time.
Swirling cloud masses over the Tasman Sea between Australia and New Zealand illustrate the fluidity of our dynamic atmosphere. Winds and weather conditions such as air temperature and humidity influence ozone chemistry.
An additional challenge arising for anyone tracking tropospheric ozone-forming reactions is that they entail interactions between different phases of matter gas, liquid, and particles known as aerosols , and can occur on various kinds of aerosol surfaces in the atmosphere. Changing environmental conditions such as air temperature and humidity also affect ozone chemistry. Furthermore, many of the chemicals involved have very short lifetimes before they react with other chemicals to form new compounds.
Scientists face myriad challenges in their pursuit of understanding tropospheric ozone chemistry. References Finlayson-Pitts, Barbara J. Chemistry of the Upper and Lower Atmosphere. Academic Press P. Fishman, Jack. New York and London: Plenum Press. Fishman, Jack, et al. Madronich, Sacha. Tropospheric photochemistry and its response to UV changes. Amsterdam: Springer-Verlag Pp.
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