Ozone

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Ozone
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General
Systematic name Trioxygen
Molecular formula O3
Molar mass 47.998 g·mol−1
Appearance bluish colored gas
CAS number [10028-15-6]
Properties
Density and phase 2.144 g·L−1 (0 °C), gas
Solubility in water 0.105 g·100mL−1 (0 °C)
Melting point 80.7 K, −192.5 °C
Boiling point 161.3 K, −111.9 °C
Thermodynamic data
Standard enthalpy of
formation
ΔfH°solid
+142.3 kJ·mol−1
Standard molar entropy
S°solid
237.7 J·K−1.mol−1
Hazards
EU classification not listed
NFPA 704
Supplementary data page
Structure and
properties
n, εr, etc.
Thermodynamic
data
Phase behaviour
Solid, liquid, gas
Spectral data UV, IR, NMR, MS
Regulatory data Flash point,
RTECS number, etc.
Except where noted otherwise, data are given for
materials in their standard state (at 25 °C, 100 kPa)
Infobox disclaimer and references

Ozone (O3) is a triatomic molecule, consisting of three oxygen atoms. It is an allotrope of oxygen that is much less stable than the diatomic species O2. Ground-level ozone is an air pollutant with harmful effects on the respiratory systems of animals. Ozone in the upper atmosphere filters potentially damaging ultraviolet light from reaching the Earth's surface. It is present in low concentrations throughout the Earth's atmosphere. It has many industrial and consumer applications. Ozone therapy is a controversial alternative medicine practice; mainstream scientific medicine has found ozone to be harmful to humans,[1] and equipment intended to be used for ozone therapy is banned in the United States.[2]

Ozone, the first allotrope of a chemical element to be described by science, was discovered by Christian Friedrich Schönbein in 1840, who named it after the Greek word for smell (ozein), from the peculiar odor in lightning storms.[3] The odor from a lightning strike is from ions produced during the rapid chemical changes, not the ozone itself.[4]

Physical properties

Undiluted ozone is a pale blue gas at standard temperature and pressure; it forms a dark blue liquid below −112 °C and a violet-black solid below −193 °C.[5] At concentrations found in the atmosphere it is colorless.[6] The concentration above which it can be smelled (odor threshold) is between 0.0076 and 0.036 ppm.[7]

Structure

The structure of ozone, according to experimental evidence from microwave spectroscopy, is bent, with C2v symmetry (similar to the water molecule), O – O distance of 127.2 pm and O – O – O angle of 116.78°.[8] The central atom forms an sp² hybridization with one lone pair. Ozone is a polar molecule with a dipole moment of 0.5337 D.[9] The bonding is single bond on one side and double bond on the other side, and these bonds are blended to become known as resonance structures. The bond order is 1.5 for each side.

Chemistry

Ozone is a powerful oxidizing agent. It is also unstable at high concentrations, decaying to ordinary diatomic oxygen (in about half an hour in atmospheric conditions[10]):

2 O3 → 3 O2.

This reaction proceeds more rapidly with increasing temperature and decreasing pressure. Ozone will oxidize metals (except gold, platinum, and iridium) to oxides of the metals in their highest oxidation state:

2 Cu2+(aq) + 2 H3O+(aq) + O3(g) → 2 Cu3+(aq) + 3 H2O(l) + O2(g)

Ozone also increases the oxidation number of oxides:

NO + O3NO2 + O2

The above reaction is accompanied by chemiluminescence. The NO2 can be further oxidized:

NO2 + O3 → NO3 + O2

The NO3 formed can react with NO2 to form N2O5:

NO2 + NO3 → N2O5

Ozone reacts with carbon to form carbon dioxide, even at room temperature:

C + 2 O3 → CO2 + 2 O2

Ozone does not react with ammonium salts but it reacts with ammonia to form ammonium nitrate:

2 NH3 + 4 O3 → NH4NO3 + 4 O2 + H2O

Ozone reacts with sulfides to make sulfates:

PbS + 4 O3PbSO4 + 4 O2

Sulfuric acid can be produced from ozone, either starting from elemental sulfur or from sulfur dioxide:

S + H2O + O3 → H2SO4
3 SO2 + 3 H2O + O3 → 3 H2SO4

All three atoms of ozone may also react, as in the reaction with tin(II) chloride and hydrochloric acid:

3 SnCl2 + 6 HCl + O3 → 3 SnCl4 + 3 H2O

In the gas phase, ozone reacts with hydrogen sulfide to form sulfur dioxide:

H2S + O3 → SO2 + H2O

In an aqueous solution, however, two competing simultaneous reactions occur, one to produce elemental sulfur, and one to produce sulfuric acid:

H2S + O3 → S + O2 + H2O
3 H2S + 4 O3 → 3 H2SO4

Iodine perchlorate can be made by treating iodine dissolved in cold anhydrous perchloric acid with ozone:

I2 + 6 HClO4 + O3 → 2 I(ClO4)3 + 3 H2O

Solid nitryl perchlorate can be made from NO2, ClO2, and O3 gases:

2 NO2 + 2 ClO2 + 2 O3 → 2 NO2ClO4 + O2

Ozone can be used for combustion reactions and combusting gases in ozone provides higher temperatures than combusting in dioxygen (O2). Following is a reaction for the combustion of carbon subnitride:

3 C4N2 + 4 O3 → 12 CO + 3 N2

Ozone can react at cryogenic temperatures. At 77 K (-196 °C), atomic hydrogen reacts with liquid ozone to form a hydrogen superoxide radical, which dimerizes:[11]

H + O3 → HO2 + O
2 HO2 → H2O4

Ozonides can be formed, which contain the ozonide anion, O3-. These compounds are explosive and must be stored at cryogenic temperatures. Ozonides for all the alkali metals are known. KO3, RbO3, and CsO3 can be prepared from their respective superoxides:

KO2 + O3 → KO3 + O2

Although KO3 can be formed as above, it can also be formed from potassium hydroxide and ozone:[12]

2 KOH + 5 O3 → 2 KO3 + 5 O2 + H2O

NaO3 and LiO3 must be prepared by action of CsO3 in liquid NH3 on an ion exchange resin containing Na+ or Li+ ions:[13]

CsO3 + Na+ → Cs+ + NaO3

Treatment with ozone of calcium dissolved in ammonia leads to ammonium ozonide and not calcium ozonide:[14]

3 Ca + 10 NH3 + 6 O3 → Ca•6NH3 + Ca(OH)2 + Ca(NO3)2 + 2 NH4O3 + 2 O2 + H2

Ozone can be used to remove manganese from the water, forming a precipitate which can be filtered:

2 Mn2+ + 2 O3 + 4 H2O → 2 MnO(OH)2 (s) + 2 O2 + 4 H+

Ozone will also turn cyanides to the one thousand times less toxic cyanates:

CN- + O3 → CNO- + O2

Finally, ozone will also completely decompose urea:[15]

(NH2)2CO + O3 → N2 + CO2 + 2 H2O

Ozone in Earth's atmosphere

File:Atmospheric ozone.svg
The distribution of atmospheric ozone in partial pressure as a function of altitude.
File:Nimbus ozone Brewer-Dobson circulation.jpg
Concentration of ozone as measured by the Nimbus-7 satellite.
File:IM ozavg ept 200006.png
Total ozone concentration in June 2000 as measured by EP-TOMS satellite instrument.

The standard way to express total ozone levels (the volume of ozone in a vertical column) in the atmosphere is by using Dobson units. Concentrations at a point are measured in parts per billion (ppb) or in μg/m³.

Ozone layer

The highest levels of ozone in the atmosphere are in the stratosphere, in a region also known as the ozone layer between about 10 km and 50 km above the surface (or between 6.21 and 31.1 miles). Here it filters out the shorter wavelengths (less than 320 nm) of ultraviolet light (270 to 400 nm) from the Sun that would be harmful to most forms of life in large doses. These same wavelengths are also among those responsible for the production of vitamin D, which is essential for human health. Ozone in the stratosphere is mostly produced from ultraviolet rays reacting with oxygen:

O2 + (radiation < 240 nm) → 2 O
O + O2 → O3

It is destroyed by the reaction with atomic oxygen:

O3 + O → 2 O2

(See Ozone-oxygen cycle for more detail.)

The latter reaction is catalysed by the presence of certain free radicals, of which the most important are hydroxyl (OH), nitric oxide (NO) and atomic chlorine (Cl) and bromine (Br). In recent decades the amount of ozone in the stratosphere has been declining mostly due to emissions of CFCs and similar chlorinated and brominated organic molecules, which have increased the concentration of ozone-depleting catalysts above the natural background. See ozone depletion for more information.

Low level ozone

Low level ozone (or tropospheric ozone) is regarded as a pollutant by the World Health Organization.[16] It is not emitted directly by car engines or by industrial operations. It is formed by the reaction of sunlight on air containing hydrocarbons and nitrogen oxides that react to form ozone directly at the source of the pollution or many kilometers down wind. For more details of the complex chemical reactions that produce low level ozone see tropospheric ozone.

Ozone reacts directly with some hydrocarbons such as aldehydes and thus begins their removal from the air, but the products are themselves key components of smog. Ozone photolysis by UV light leads to production of the hydroxyl radical and this plays a part in the removal of hydrocarbons from the air, but is also the first step in the creation of components of smog such as peroxyacyl nitrates which can be powerful eye irritants. The atmospheric lifetime of tropospheric ozone is about 22 days and its main removal mechanisms are being deposited to the ground, the above mentioned reaction giving OH, and by reactions with OH and the peroxy radical HO2· (Stevenson et al, 2006).[17]

As well as having an impact on human health (see below) there is also evidence of significant reduction in agricultural yields due to increased ground-level ozone and pollution which interferes with photosynthesis and stunts overall growth of some plant species.[18][19]

Ozone as a greenhouse gas

Although ozone was present at ground level before the industrial revolution, peak concentrations are far higher than the pre-industrial levels and even background concentrations well away from sources of pollution are substantially higher.[20][21] This increase in ozone is of further concern as ozone present in the upper troposphere acts as a greenhouse gas, absorbing some of the infrared energy emitted by the earth. Quantifying the greenhouse gas potency of ozone is difficult as it is not present in uniform concentrations across the globe. However, the most recent scientific review on the climate change (the IPCC Third Assessment Report[22]) suggests that the radiative forcing of tropospheric ozone is about 25% that of carbon dioxide.

Ozone and health

Ozone in air pollution

There is a great deal of evidence to show that high concentrations (ppm) of ozone, created by high concentrations of pollution and daylight UV rays at the earth's surface, can harm lung function and irritate the respiratory system.[16][23] A connection has also been shown to exist between increased ozone caused by thunderstorms and hospital admissions of asthma sufferers.[24] Air quality guidelines such as those from the World Health Organization are based on detailed studies of what levels can cause measurable health effects.

A common British folk myth dating back to the Victorian era holds that the smell of the sea is caused by ozone, and that this smell has "bracing" health benefits.[25] Neither of these is true. The characteristic "smell of the sea" is not caused by ozone, but by the presence of dimethyl sulfide generated by phytoplankton, and dimethyl sulfide, like ozone, is toxic in high concentrations.[26]

The United States Environmental Protection Agency has developed an Air Quality index to help explain air pollution levels to the general public. 8-hour average ozone concentrations of 85 to 104 ppbv are described as "Unhealthy for Sensitive Groups", 105 ppbv to 124 ppbv as "unhealthy" and 125 ppb to 404 ppb as "very unhealthy".[27] The EPA has designated over 300 counties of the United States, clustered around the most heavily populated areas (especially in California and the Northeast), as failing to comply with the National Ambient Air Quality Standards.

Physiology of ozone

Ozone, along with reactive forms of oxygen such as superoxide, singlet oxygen (see 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. Also, when ozone breaks down to dioxygen it gives rise to oxygen free radicals, which are highly reactive and capable of damaging many organic molecules. Ozone has been found to convert cholesterol in the blood stream to plaque (which causes hardening and narrowing of arteries). 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. A team headed by Dr. Paul Wentworth Jr. of the Department of Chemistry at the Scripps Research Institute has shown evidence linking the antibody-catalyzed water-oxidation pathway of the human immune response to the production of ozone. In this system, ozone is produced by antibody-catalyzed production of trioxidane from water and neutrophil-produced singlet oxygen.[28] See also trioxidane for more on this biological ozone-producing reaction.

Ozone has also been proven to form specific, cholesterol-derived metabolites that are thought to facilitate the build-up and pathogenesis of atherosclerotic plaques (a form of heart disease). These metabolites have been confirmed as naturally occurring in human atherosclerotic arteries and are categorized into a class of secosterols termed “Atheronals”, generated by ozonolysis of cholesterol's double bond to form a 5,6 secosterol as well as a secondary condensation product via aldolization.[29]

Production techniques

Ozone used in industry is measured in g/Nm³ or weight percent. The regime of applied concentrations ranges from 1 to 5 weight percent in air and from 6 to 13 weight percent in oxygen.

Ozone generators currently on the market generate ozone molecules by employing one of the methods below.

Corona discharge method

This is the most popular type of ozone generator for most industrial and personal uses. While variations of the "hot spark" coronal discharge method of ozone production exist, including medical grade and industrial grade ozone generators, these units usually work by means of a corona discharge tube.[30] They are typically very cost-effective, and do not require an oxygen source other than the ambient air. However, they also produce nitrogen oxides as a by-product. Use of an air dryer can reduce or eliminate nitric acid formation by removing water vapor and increase ozone production. Use of an oxygen concentrator can further increase the ozone production and further reduce the risk of nitric acid formation due to removing not only the water vapor, but also the bulk of the nitrogen.

Ultraviolet light

UV ozone generators employ a light source that generates the same narrow-band ultraviolet light that is responsible for the sustenance of the ozone layer in the stratosphere of the Earth [31]. While standard UV ozone generators tend to be less expensive, they usually produce ozone with a concentration of about 2% or lower. Another disadvantage of this method is that it requires the air to be exposed to the UV source for a longer amount of time, and any air that is not exposed to the UV source will not be treated. This makes UV generators impractical for use in situations that deal with rapidly moving air or water streams (in-duct air sterilization, for example).

Cold plasma

In the cold plasma method, pure oxygen gas is exposed to a plasma created by dielectric barrier discharge. The diatomic oxygen is split into single atoms, which then recombine in triplets to form ozone.

Cold plasma machines utilize pure oxygen as the input source, and produce a maximum concentration of about 5% ozone. They produce far greater quantities of ozone in a given space of time compared to ultraviolet production. However, because cold plasma ozone generators are very expensive, and still require occasional maintenance, they are found less frequently than the previous two types.

The discharges manifest as filamentary transfer of electrons (micro discharges) in a gap between two electrodes. In order to evenly distribute the micro discharges, a dielectric insulator must be used to separate the metallic electrodes and to prevent arcing.

Some cold plasma units also have the capability of producing short-lived allotropes of oxygen which include O4, O5, O6, O7, etc. These anions are even more reactive than ordinary O3.

Special considerations

Ozone cannot be stored and transported like other industrial gases (because it quickly decays into diatomic oxygen) and must therefore be produced on site. Available ozone generators vary in the arrangement and design of the high-voltage electrodes. At production capacities higher than 20kg per hour, a gas/water tube heat-exchanger is utilized as ground electrode and assembled with tubular high-voltage electrodes on the gas-side. The regime of typical gas pressures is around 2 bar absolute in oxygen and 3 bar absolute in air. Several megawatts of electrical power may be installed in large facilities, applied as one phase AC current at 600 to 2000 Hz and peak voltages between 3000 and 20000 volts.

The dominating parameter influencing ozone generation efficiency is the gas temperature, which is controlled by the cooling water temperature. The cooler the water, the better the ozone synthesis. At typical industrial conditions, almost 90 percent of the effective power is dissipated as heat and needs to be removed by a sufficient cooling water flow.

Due to the high reactivity of ozone, only few materials may be used like stainless steel (quality 316L), glass, polytetrafluorethylene, or polyvinylidene fluoride. Viton may be used with the restriction of constant mechanical forces and absence of humidity.

Incidental production

Ozone may be formed from O2 by electrical discharges and by action of high energy electromagnetic radiation. Certain electrical equipment generate significant levels of ozone. This is especially true of devices using high voltages, such as ionic air purifiers, laser printers, photocopiers, and arc welders. Electric motors using brushes can generate ozone from repeated sparking inside the unit. Large motors that use brushes, such as those used by elevators or hydraulic pumps, will generate more ozone than smaller motors.

Laboratory production

In the laboratory ozone can be produced by electrolysis using a 9 volt battery, a pencil graphite rod cathode, a platinum wire anode and a 3M sulfuric acid electrolyte.[32] The half cell reactions taking place are

3 H2O → O3 + 6 H+ + 6 e; ΔEo = −1.53 V;
6 H+ + 6 e → 3 H2; ΔEo = 0 V;
2 H2O → O2 + 4 H+ + 4 e; ΔEo = −1.23 V;

so that in the net reaction three equivalents of water are converted into one equivalent of ozone and three equivalents of hydrogen. Oxygen formation is a competing reaction.

Applications

Industrial applications

Ozone can be used for bleaching substances and for killing microorganisms in air and water sources. Many municipal drinking water systems kill bacteria with ozone instead of the more common chlorine.[33] Ozone has a very high oxidation potential. Ozone does not form organochlorine compounds, nor does it remain in the water after treatment, so some systems introduce a small amount of chlorine to prevent bacterial growth in the pipes, or may use chlorine intermittently, based on results of periodic testing. Where electrical power is abundant, ozone is a cost-effective method of treating water, as it is produced on demand and does not require transportation and storage of hazardous chemicals. Once it has decayed, it leaves no taste or odor in drinking water. Low levels of ozone have been advertised to be of some disinfectant use in residential homes, however, the concentration of ozone required to have a substantial effect on airborne pathogens greatly exceeds safe levels recommended by the U.S. Occupational Safety and Health Administration and Environmental Protection Agency.[citation needed]

Industrially, ozone or ozonated water is used to:

  • Disinfect laundry in hospitals, food factories, care homes etc;[34]
  • Disinfect water before it is bottled;
  • Deodorize air and objects, such as after a fire. This process is extensively used in Fabric Restoration;
  • Kill bacteria on food or on contact surfaces;
  • Ozone swimming pool and spa sanitation
  • Scrub yeast and mold spores from the air in food processing plants;
  • Wash fresh fruits and vegetables to kill yeast, mold and bacteria;
  • Chemically attack contaminants in water (iron, arsenic, hydrogen sulfide, nitrites, and complex organics lumped together as "colour");
  • Provide an aid to flocculation (agglomeration of molecules, which aids in filtration, where the iron and arsenic are removed);
  • Manufacture chemical compounds via chemical synthesis [1]
  • Clean and bleach fabrics (the former use is utilized in Fabric Restoration)(the latter use is patented);
  • Assist in processing plastics to allow adhesion of inks;
  • Age rubber samples to determine the useful life of a batch of rubber;
  • Hospital operating rooms where air needs to be sterile;
  • Eradicate water borne parasites such as Giardia and Cryptosporidium in surface water treatment plants. This process is known as ozonation.

Ozone is a reagent in many organic reactions in the laboratory and in industry. Ozonolysis is the cleavage of an alkene to carbonyl compounds.

Many hospitals in the U.S. and around the world use large ozone generators to decontaminate operating rooms between surgeries. The rooms are cleaned and then sealed airtight before being filled with ozone which effectively kills or neutralizes all remaining bacteria.[citation needed]

Ozone is used as an alternative to chlorine or chlorine dioxide in the bleaching of wood pulp [35] . It is often used in conjunction with oxygen and hydrogen peroxide to completely eliminate the need for chlorine-containing compounds in the manufacture of high-quality, white paper[36]

Ozone can be used to detoxify cyanide wastes (for example from gold and silver mining) by oxidizing cyanide to cyanate and eventually to carbon dioxide.[37]

Consumer applications

Ozone machines, with or without ionisation, are currently used to sanitise (high ozone output) and deodorize non-inhabited rooms, ductwork, vehicles, boats, woodsheds, and buildings.

Some models of air purifiers that also emit low levels of ozone have been sold in the US. These type of air purifiers claim to imitate nature's "filterless" air purifying mechanisms[38] and claim to "sanitise" the air and/or household surfaces. The government successfully sued one company in 1995, ordering them to stop repeating health claims without supporting scientific studies.

Ozonated water is used to launder clothes, sanitise food, drinking water, and surfaces in the home. According to the FDA, it is "amending the food additive regulations to provide for the safe use of ozone in gaseous and aqueous phases as an antimicrobial agent on food, including meat and poultry." Studies at California Polytechnic University, have proven that low levels of ozone dissolved in filtered tapwater can produce more than a four-log (99.99%) reduction in such food-borne microorganisms as salmonella, e. Coli 0157:H7, campylobacter and others.[39] Ironically, while ozone is considered an atmospheric pollutant, pollution and smog by the US government, it can actually decrease the levels of pollutants like pesticides in fruits and vegetables.[40]

Ozone is used in spas or hot tubs with reduced levels of chlorine or bromine for keeping the water free of bacteria. As it does not remain in the water after treatment, it is ineffective at preventing bather cross-contamination, and must be used in conjunction with another sanitizer. Ozone gas is created by an ultraviolet light bulb or corona discharge chip and injected into the plumbing system[citation needed].

Ozone is also widely used in treatment of water in aquaria and fish ponds. Its use can minimize bacterial growth control parasites and removes or reduces "yellowing" of the water. As the ozone rapidly decomposes, at correctly controlled levels the application has no effect on the fish[citation needed].

Most countries restrict the amount of ozone that can be generated by popular "ionizing" devices because ozone contributes to the development of smog. Smaller ozone machines may be employed by personal users for home use, and typically produce far less ozone than their larger counterparts. Due to their lower costs, almost all ozone generators designed for personal use employ the corona discharge method. In many countries, the production or operation of ozone generating devices is illegal.[citation needed]

Ozone therapy

Ozone therapy has been used in alternative medicine as a medical treatment in a number of different countries.[41] Its use, however, is controversial.[42]

The United States Food and Drug Administration (FDA) has banned ozone generators or ozone gas from being marketed for treatment of any medical conditions, based on the toxicity of ozone and the lack of scientific evidence for any beneficial effects at non-toxic levels.[2]

One couple, Kenneth R. Thiefault and Mardel Barber, were convicted of and sent to prison in 1999 for violating this ban, which involved marketing ozone generators to cure AIDS, cancer, herpes, hepatitis, gangrene, or "almost any disease", without presenting any evidence to the FDA of effectiveness or safety.[43]

However, it is worth noting that the FDA cannot allow any device to claim to treat any medical condition unless the device and/or treatment have gone through rigorous trials. It is not illegal to sell medical-grade ozone machines in the US, nor is it illegal to own one or use one. What is illegal is to sell them while claiming it treats disease. Many people use ozone therapy in the US, despite its unrecognized status with the FDA and allopathic medicine. It is legal to sell or own a medical-grade ozone machine in the US. It is also legal to self-administer ozone. Whether practitioners can administer or recommend the use of ozone presents a more complex issue.

See also

Notes and references

  1. Lewis, Jr, R. J. (1993). Sax’s Dangerous Properties of Industrial Materials. New York: Van Nostrand Rienhold, Co., Inc.,. ISBN 9780442016753.
  2. 2.0 2.1 "TITLE 21--FOOD AND DRUGS; CHAPTER I--FOOD AND DRUG ADMINISTRATION DEPARTMENT OF HEALTH AND HUMAN SERVICES; SUBCHAPTER H--MEDICAL DEVICES". U.S. Food & Drug Administration (FDA) website. August 30, 2006.
  3. "Today in Science History". Retrieved 2006-05-10.
  4. "Ozone FAQ". Global Change Master Directory. Retrieved 2006-05-10.
  5. "Oxygen". WebElements. Retrieved 2006-09-23.
  6. Ozone: Helpful or Harmful?. Aerias AQS IAQ Resource Center. Retrieved on 2006-09-23.
  7. "Ozone". Haz-MAP (occupational health database}. Retrieved 2006-09-23.
  8. Takehiko Tanaka; Yonezo Morino. Coriolis interaction and anharmonic potential function of ozone from the microwave spectra in the excited vibrational states Journal of Molecular Spectroscopy 1970, 33, 538–551.
  9. Kenneth M. Mack; J. S. Muenter. Stark and Zeeman properties of ozone from molecular beam spectroscopy. Journal of Chemical Physics 1977, 66, 5278–5283. doi:10.1063/1.433909
  10. http://gcmd.gsfc.nasa.gov/Resources/FAQs/ozone.html
  11. Horvath M., Bilitzky L., & Huttner J., 1985. "Ozone." pg 44–49
  12. Housecroft & Sharpe, 2005. "Inorganic Chemistry." pg 439
  13. Housecroft & Sharpe, 2005. "Inorganic Chemistry." pg 265
  14. Horvath M., Bilitzky L., & Huttner J., 1985. "Ozone." pg 44–49
  15. Horvath M., Bilitzky L., & Huttner J., 1985. "Ozone." pg 259, 269–270
  16. 16.0 16.1 WHO-Europe reports: Health Aspects of Air Pollution (2003) (PDF)
  17. Stevenson; et al. (2006). "Multimodel ensemble simulations of present-day and near-future tropospheric ozone". American Geophysical Union. Retrieved 2006-09-16.
  18. "Rising Ozone Levels Pose Challenge to U.S. Soybean Production, Scientists Say". NASA Earth Observatory. 2003-07-31. Retrieved 2006-05-10. Check date values in: |date= (help)
  19. Mutters, Randall (1999). "Statewide Potential Crop Yield Losses From Ozone Exposure". California Air Resources Board. Retrieved 2006-05-10. Unknown parameter |month= ignored (help)
  20. "Tropospheric Ozone in EU - The consolidated report". European Environmental Agency. 1998. Retrieved 2006-05-10.
  21. "Atmospheric Chemistry and Greenhouse Gases". Intergovernmental Panel on Climate Change. Retrieved 2006-05-10.
  22. "Climate Change 2001". Intergovernmental Panel on Climate Change. 2001. Retrieved 2006-09-12.
  23. Answer to follow-up questions from CAFE (2004) (PDF)
  24. Anderson, W. (August 2001). "Asthma admissions and thunderstorms: a study of pollen, fungal spores, rainfall, and ozone". QJM: An International Journal of Medicine. Oxford Journals. 94 (8): 429–433. Retrieved 2006-09-23. Unknown parameter |coauthors= ignored (help)
  25. Ashfield District Council: Monitored Air Pollutants, downloaded February 2, 2007
  26. University of East Anglia press release, Cloning the smell of the seaside, February 2, 2007
  27. "Smog - Who does it hurt? What You Need to Know About Ozone and Your Health". AIRNow.gov. Retrieved 2007-07-10.
  28. Hoffmann, Roald (January 2004). "The Story of O". American Scientist. 92 (1): 23. doi:10.1511/2004.1.23. Retrieved 2006-10-11.
  29. Paul Wentworth (2003). "Evidence for Ozone Formation in Human Atherosclerotic Arteries". Retrieved 2006-08-03. Unknown parameter |month= ignored (help)
  30. Organic Syntheses, Coll. Vol. 3, p.673 (1955); Vol. 26, p.63 (1946). (Article)
  31. Dohan, J. M. (1987). "Photochemical Generation of Ozone: Present State-of-the-Art". Ozone Sci. Eng. 9: 315–334. Unknown parameter |coauthors= ignored (help); |access-date= requires |url= (help)
  32. Ibanez, Jorge G. (2005). "Laboratory Experiments on the Electrochemical Remediation of the Environment. Part 7: Microscale Production of Ozone". Journal of Chemical Education. 82 (10): 1546. Retrieved 2006-05-10. Unknown parameter |month= ignored (help); Unknown parameter |coauthors= ignored (help)
  33. Hoigné, J. (1998). Handbook of Environmental Chemistry, Vol. 5 part C, p83-141. Berlin: Springer-Verlag.
  34. "Decontamination: Ozone scores on spores". Hospital Development. Wilmington Media Ltd. 2007-04-01. Retrieved 2007-05-30.
  35. Sjöström, Eero (1993). Wood Chemistry: Fundamentals and Applications. San Diego, CA: Academic Press, Inc. ISBN 0-12-64748 Check |isbn= value: length (help).
  36. Su, Yu-Chang; Chen, Horng-Tsai (2001), "Enzone Bleaching Sequence and Color Reversion of Ozone-Bleached Pulps", Taiwan Journal of Forest Science, 16 (2): 93–102
  37. Bollyky, L. J. (1977). Ozone Treatment of Cyanide-Bearing Wastes, EPA Report 600/2-77-104. Research Triangle Park, N.C.: U.S. Environmental Protection Agency.
  38. "The Unknown Truth Regarding Ozone!". Retrieved 16-09-2006. Check date values in: |accessdate= (help)
  39. http://www.purityintl.com/Article%20POU.pdf
  40. lotus Sanitises Food without Chemicals (2000). Retrieved July 24, 2006.
  41. "Medical Ozone Therapy Oxygen Therapies". Applied Ozone Systems. Retrieved 2006-11-03.
  42. "Oxygenation Therapy: Unproven Treatments for Cancer and AIDS". Quackwatch. Retrieved 2006-11-03.
  43. Paula Kurtzweil. Ozone Generators Generate Prison Terms for Couple, FDA
  • Series in Plasma Physics: Non-Equilibrium Air Plasmas at Atmospheric Pressure. Edited by K.H. Becker, U. Kogelschatz, K.H. Schoenbach, R.J. Barker; Bristol and Philadelphia: Institute of Physics Publishing Ltd; ISBN 0-7503-0962-8; 2005

External links

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