ozone

(noun)

a molecule found in the upper regions of the Earth's atmosphere; important for blocking UV light from reaching Earth; chemical symbol O3

Related Terms

  • Chlorofluorocarbons
  • paramagnetic
  • Alkenes
  • oxygen
  • stratosphere
  • diamagnetic

(noun)

An allotrope of oxygen (symbol O3) having three atoms in the molecule instead of the usual two; it is a blue gas, generated from oxygen by electrical discharge; it is poisonous and highly reactive, but it protects life on Earth by absorbing solar ultraviolet radiation in the upper atmosphere.

Related Terms

  • Chlorofluorocarbons
  • paramagnetic
  • Alkenes
  • oxygen
  • stratosphere
  • diamagnetic

(noun)

A triatomic molecule, also called trioxygen, consisting of three oxygen atoms (O3).

Related Terms

  • Chlorofluorocarbons
  • paramagnetic
  • Alkenes
  • oxygen
  • stratosphere
  • diamagnetic

Examples of ozone in the following topics:

  • Ozone Depletion

    • 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.
  • Polar Ozone Holes

    • 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.
  • Air Pollution

    • 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.
  • Ozone

    • 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.
  • Earth's Atmosphere

    • 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.
  • Photochemical Smog

    • 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.
  • The Rate Law

    • 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.
  • The Greenhouse Effect

    • 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.
  • Glow of Space Shuttles

    • You may have heard of the ozone layer, which protects the Earth from ultraviolet radiation.
  • Hydroboration Reactions and Oxidations

    • 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.
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