Examples of ozone in the following topics:
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- Free radicals in the upper stratosphere act as catalysts for ozone decomposition, thereby depleting the ozone layer.
- Ozone depletion describes two distinct but related phenomena observed since the late 1970s: (1) a steady decline of about 4 percent per decade in the total volume of ozone in Earth's stratosphere (the ozone layer); and (2) a much larger springtime decrease in stratospheric ozone over Earth's polar regions.
- The latter phenomenon is referred to as the ozone hole.
- The largest ozone hole was observed in September, 2006.
- The reaction of these free radicals with ozone disrupts the ozone-oxygen cycle, leading to the destruction of stratospheric ozone and the depletion of the ozone layer.
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- Chlorofluorocarbons have disrupted stratospheric ozone generation, resulting in a thinning of the ozone layer at the poles.
- The chlorine radical can then react with ozone, as shown below:
- The chlorine breaks an oxygen off from ozone, producing diatomic oxygen.
- Having destroyed two ozone molecules, the chlorine radical is produced once more and can destroy more ozone molecules.
- CFCs have caused a gradual decrease in ozone levels throughout the stratosphere.
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- Decreased stratospheric ozone: a depletion in ozone levels caused by the release of refrigerants, which produce free radicals that catalyze the decomposition of ozone.
- Increased ozone concentrations at ground levels: an increase in surface ozone that contributes to smog.
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- In total, ozone makes up only 0.6 parts per million of the atmosphere.
- This makes ozone a potent respiratory hazard and pollutant near ground level.
- However, the so-called ozone layer (a portion of the stratosphere with a higher concentration of ozone, from two to eight ppm) is beneficial.
- It is dangerous to allow this liquid to warm to its boiling point because both concentrated gaseous ozone and liquid ozone can detonate.
- Moreover, it is believed that the powerful oxidizing properties of ozone may be a contributing factor of inflammation.
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- While the three major components have remained relatively constant over time and space, the minor components, which also include methane, sulfur dioxide, ozone, and nitrogen oxides, have varied more widely.
- The next layer, the stratosphere, contains an ozone layer that results from the reaction of ionizing solar radiation with oxygen gas; this ozone layer is responsible for the absorption of UV light.
- In the recent past, we have damaged our ozone layer by putting chlorofluorocarbons (CFCs) into the atmosphere.
- The CFCs have damaged ozone, resulting in a hole in the ozone layer.
- In recent years, CFCs have been banned and the ozone layer hole is shrinking.
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- Ultraviolet light can split nitrogen dioxide into nitric oxide and monatomic oxygen; this monatomic oxygen can then react with oxygen gas to form ozone.
- Products like ozone, aldehydes, and peroxyacetyl nitrates are called secondary pollutants.
- These oxidizing compounds have been linked to a variety of negative health outcomes; ozone, for example, is known to irritate the lungs.
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- The reaction between nitric oxide and ozone, $NO(g) + O_3(g)\rightarrow NO_2(g) + O_2(g)$ , is first order in both nitric oxide and ozone.
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- Gases known as greenhouse gases, including water vapor, carbon dioxide, ozone, and methane, absorb and trap this heat as it tries to escape from the atmosphere.
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- You may have heard of the ozone layer, which protects the Earth from ultraviolet radiation.
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- Reactions of alkynes with oxidizing agents such as potassium permanganate and ozone usually result in cleavage of the triple-bond to give carboxylic acid products.