| Ozone |
|---|
|
| 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, −526.5 °C |
| Boiling point | 161.3 K, −111.9 °C |
| Thermodynamic data |
|---|
Standard enthalpy of
formation Δf''H''°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)
|
'Ozone' ('O
3') is a
triatomic molecule, consisting of three
oxygen atoms. It is an
allotrope of
oxygen that is much less stable than the
diatomic species O
2. 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 C
2v 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 ''sp''² 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 O
3 → 3 O
2.
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 Cu
2+(aq) + 2 H
3O
+(aq) + O
3(g) → 2 Cu
3+(aq) + 3 H
2O
(l) + O
2(g)
Ozone also increases the oxidation number of oxides:
:
NO + O
3 →
NO2 + O
2
The above reaction is accompanied by
chemiluminescence. The NO
2 can be further oxidized:
: NO
2 + O
3 → NO
3 + O
2
The NO
3 formed can react with NO
2 to form
N2O5:
: NO
2 + NO
3 → N
2O
5
Ozone reacts with
carbon to form
carbon dioxide, even at room temperature:
: C + 2 O
3 → CO
2 + 2 O
2
Ozone does not react with ammonium
salts but it reacts with
ammonia to form
ammonium nitrate:
: 2
NH3 + 4 O
3 → NH
4NO
3 + 4 O
2 + H
2O
Ozone reacts with
sulfides to make
sulfates:
:
PbS + 4 O
3 →
PbSO4 + 4 O
2
Sulfuric acid can be produced from ozone, either starting from elemental
sulfur or from
sulfur dioxide:
: S + H
2O + O
3 → H
2SO
4
: 3 SO
2 + 3 H
2O + O
3 → 3 H
2SO
4
All three
atoms of ozone may also react, as in the reaction with
tin(II) chloride and
hydrochloric acid:
: 3 SnCl
2 + 6 HCl + O
3 → 3 SnCl
4 + 3 H
2O
In the
gas phase, ozone reacts with
hydrogen sulfide to form sulfur dioxide:
: H
2S + O
3 → SO
2 + H
2O
In an
aqueous solution, however, two competing simultaneous reactions occur, one to produce elemental sulfur, and one to produce sulfuric acid:
:
H2S + O
3 → S + O
2 + H
2O
: 3 H
2S + 4 O
3 → 3
H2SO4
Iodine perchlorate can be made by treating iodine dissolved in cold
anhydrous perchloric acid with ozone:
: I
2 + 6 HClO
4 + O
3 → 2 I(ClO
4)
3 + 3 H
2O
Solid
nitryl perchlorate can be made from NO
2, ClO
2, and O
3 gases:
: 2 NO
2 + 2 ClO
2 + 2 O
3 → 2 NO
2ClO
4 + O
2
Ozone can be used for
combustion reactions and combusting gases in ozone provides higher temperatures than combusting in
dioxygen (O
2). Following is a reaction for the combustion of
carbon subnitride:
: 3 C
4N
2 + 4 O
3 → 12 CO + 3 N
2
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 + O
3 → HO
2 + O
: 2 HO
2 → H
2O
4
Ozonides can be formed, which contain the
ozonide anion, O
3-. These compounds are explosive and must be stored at cryogenic temperatures. Ozonides for all the
alkali metals are known. KO
3, RbO
3, and CsO
3 can be prepared from their respective superoxides:
: KO
2 + O
3 → KO
3 + O
2
Although KO
3 can be formed as above, it can also be formed from
potassium hydroxide and ozone:
[12]
: 2 KOH + 5 O
3 → 2 KO
3 + 5 O
2 + H
2O
NaO
3 and LiO
3 must be prepared by action of CsO
3 in liquid NH
3 on an
ion exchange resin containing Na
+ or Li
+ ions:
[13]
: CsO
3 + Na
+ → Cs
+ + NaO
3
Treatment with ozone of
calcium dissolved in ammonia leads to ammonium ozonide and not calcium ozonide:
[11]
: 3 Ca + 10 NH
3 + 6 O
3 → Ca•6NH
3 + Ca(OH)
2 + Ca(NO
3)
2 + 2 NH
4O
3 + 2 O
2 + H
2
Ozone can be used to remove
manganese from the
water, forming a
precipitate which can be filtered:
: 2 Mn
2+ + 2 O
3 + 4 H
2O → 2 MnO(OH)
2 (s) + 2 O
2 + 4 H
+
Ozone will also turn
cyanides to the one thousand times less toxic
cyanates:
: CN
- + O
3 → CNO
- + O
2
Finally, ozone will also completely decompose
urea:
[15]
:(NH
2)
2CO + O
3 → N
2 + CO
2 + 2 H
2O
Ozone in Earth's atmosphere
The distribution of atmospheric ozone in partial pressure as a function of altitude.
Concentration of ozone as measured by the
Nimbus-7 satellite.
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
Main articles: 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:
:O
2 + (radiation < 240 nm) → 2 O
:O + O
2 → O
3
It is destroyed by the reaction with
atomic oxygen:
:O
3 + O → 2 O
2
(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
Main articles: Tropospheric ozone,
Photochemical smog
Low level ozone (or tropospheric ozone) is regarded as a pollutant by the
World Health Organization.
[WHO-Europe reports: Health Aspects of Air Pollution (2003) (PDF)] 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 HO
2· (Stevenson et al, 2006).
[16]
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.
[17][18]
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.
[19][20] 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[21]) 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.
A connection has also been shown to exist between increased ozone caused by thunderstorms and hospital admissions of
asthma sufferers.
[23] 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.
[24] 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.
[25]
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".
[26] 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.
[27] 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.
[28]
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. 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
[29].
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 O
4, O
5, O
6, O
7, etc. These anions are even more reactive than ordinary O
3.
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 O
2 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.
[30] The
half cell reactions taking place are
: 3 H
2O → O
3 + 6 H
+ + 6 e
−;
ΔEo = −1.53
V;
: 6 H
+ + 6 e
− → 3 H
2;
ΔEo = 0
V;
: 2 H
2O → O
2 + 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.
[31] Ozone has a very high
oxidation potential. Ozone does not form
organochlorine compounds, but it also does not 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 has 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.
Industrially, ozone or
ozonated water is used to:
★ Disinfect laundry in hospitals, food factories, care homes etc;
[32]
★ 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.
Ozone is used as an alternative to
chlorine or
chlorine dioxide to remove
lignin from
wood pulp[33] . 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[34]
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.
[35]
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
[36] 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.
[37] 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.
[38]
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.
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 reduce "yellowing" of the water. As the Ozone rapidly decomposes, at correctly controlled levels the application has no effect on the fish.
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.
Ozone therapy
Main articles: ozone therapy
Ozone therapy has been used in
alternative medicine as a medical treatment in a number of different countries.
[39] Its use, however, is controversial.
[40]
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.
[Paula Kurtzweil. Ozone Generators Generate Prison Terms for Couple, FDA]
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 is more complex.
See also
★
Ozone depletion, including the phenomenon known as the ozone hole.
★
Ozone layer
★
Tropospheric ozone
★
Tetraoxygen (O
4)
★
Ozoneweb
Notes and references
1. Sax’s Dangerous Properties of Industrial Materials, , R. J., Lewis, Jr, Van Nostrand Rienhold, Co., Inc.,, 1993,
2.
TITLE 21--FOOD AND DRUGS; CHAPTER I--FOOD AND DRUG ADMINISTRATION DEPARTMENT OF HEALTH AND HUMAN SERVICES; SUBCHAPTER H--MEDICAL DEVICES
3. Today in Science History
4. Ozone FAQ
5. Oxygen
6. Ozone: Helpful or Harmful?
7. {{cite web|title=Ozone|work=Haz-MAP (occupational health database}|url=http://hazmap.nlm.nih.gov/cgi-bin/hazmap_generic?tbl=TblAgents&id=68|accessdate =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.
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. Multimodel ensemble simulations of present-day and near-future tropospheric ozone Stevenson et al
17. Rising Ozone Levels Pose Challenge to U.S. Soybean Production, Scientists Say
18. Statewide Potential Crop Yield Losses From Ozone Exposure
19. Tropospheric Ozone in EU - The consolidated report
20. Atmospheric Chemistry and Greenhouse Gases
21. Climate Change 2001
22. Answer to follow-up questions from CAFE (2004) (PDF)
23. Asthma admissions and thunderstorms: a study of pollen, fungal spores, rainfall, and ozone, , W., Anderson, QJM: An International Journal of Medicine,
24. Ashfield District Council: Monitored Air Pollutants, downloaded February 2, 2007
25. University of East Anglia press release, Cloning the smell of the seaside, February 2, 2007
26. Smog - Who does it hurt? What You Need to Know About Ozone and Your Health
27. The Story of O, , Roald, Hoffmann, American Scientist,
28. Evidence for Ozone Formation in Human Atherosclerotic Arteries Paul Wentworth
29. Photochemical Generation of Ozone: Present State-of-the-Art, , J. M., Dohan, Ozone Sci. Eng., 1987
30. Laboratory Experiments on the Electrochemical Remediation of the Environment. Part 7: Microscale Production of Ozone, , Jorge G., Ibanez, Journal of Chemical Education, 2005
31. Handbook of Environmental Chemistry, Vol. 5 part C, p83-141, , J., Hoigné, Springer-Verlag, 1998,
32. Decontamination: Ozone scores on spores
33. Wood Chemistry: Fundamentals and Applications, , Eero, Sjöström, Academic Press, Inc., 1993,
34.
35. Ozone Treatment of Cyanide-Bearing Wastes, EPA Report 600/2-77-104, , L. J., Bollyky, U.S. Environmental Protection Agency, 1977,
36. The Unknown Truth Regarding Ozone!
37. http://www.purityintl.com/Article%20POU.pdf
38. lotus Sanitises Food without Chemicals (2000). Retrieved July 24, 2006.
39. Medical Ozone Therapy Oxygen Therapies
40. Oxygenation Therapy: Unproven Treatments for Cancer and AIDS
41.
TITLE 21--FOOD AND DRUGS; CHAPTER I--FOOD AND DRUG ADMINISTRATION DEPARTMENT OF HEALTH AND HUMAN SERVICES; SUBCHAPTER H--MEDICAL DEVICES
★
★ 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
★
European Environment Agency's near real-time ozone map (ozoneweb)
★
NASA's Ozone Resource Page
★
Paul Crutzen Interview Freeview video of Paul Crutzen Nobel Laureate for his work on decomposition of ozone talking to Harry Kroto Nobel Laureate by the Vega Science Trust.
★
NASA's Earth Observatory article on Ozone
★
International Day for the Preservation of the Ozone Layer
★
International Chemical Safety Card 0068
★
NIOSH Pocket Guide to Chemical Hazards
★
National Institute of Environmental Health Sciences Ozone Alerts
★
Ground-level Ozone Air Pollution
★
NASA Study Links "Smog" to Arctic Warming —
NASA Goddard Institute for Space Studies (GISS) study shows the warming effect of ozone in the Arctic during winter and spring.
★
EPA Assessment of Effectiveness and Health Consequences of Ozone Generators that are Sold as Air Cleaners
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