What is Ozone? How do we produce them.?
157011
Ozone: A molecule made up of three atoms of oxygen. Occurs naturally in the stratosphere and provides a protective layer shielding the Earth from harmful ultraviolet radiation. In the troposphere, it is a chemical oxidant, a greenhouse gas, and a major component of photochemical smog.\n\nOzone precursors: Chemical compounds, such as carbon monoxide, methane, nonmethane hydrocarbons, and nitrogen oxides, which in the presence of solar radiation react with other chemical compounds to form ozone.
788575
Ozone is trigonal planar.  The lone pairs on the terminal oxygens give the trigonal structure, and the molecule is planar (2 dimensional) mainly due to the double bonds in the most stable resonance structure of ozone.\n\nH2Se should be a bent molecule.  The lone pairs take up maximum available space forcing the tiny hydrogen atoms closer together than they's like to be at an angle of about 91 deg from the Se atom.
120036
I agree with the previous answer, while ozone is a powerful cleaning agent, it has also been proven to be harmful. I am a certified Indoor Air Quality professional and I recently wrote an article about things to consider in a home air purifier: \nhttp://www.breathepureair.com/airqualityblog/residential-air-purifiers/\n\nYou may also want to check the Maerican Lung Association, which also has a section titled "Problems with Ozone"\nhttp://www.lungusa.org/site/pp.asp?c=dvLUK9O0E&b=39289\n\nThe EPA also has some great information on their Indoor Air Quality Fact Sheet: Ozone Generators that are Sold as Air Cleaners: An Assessment of Effectiveness and Health Consequences:\nhttp://www.epa.gov/iaq/pubs/ozonegen.html\n\nThe Canadian Center for Occupational Health and Safety also has a published report about the negative health effects of ozone:\nhttp://www.ccohs.ca/oshanswers/chemicals/chem_profiles/ozone/health_ozo.html
1138971
Environmental groups have recently voiced concern that exhaust from the space shuttle and other rockets could harm the protective ozone layer. But measurements taken by satellites after shuttle launches do not show any sign of stratospheric ozone destruction, atmospheric scientists report.\n\nSolid-propellant motors used to loft some rockets pose a potential threat to the ozone layer because their exhaust contains chlorine, which in some forms can destroy ozone. Indeed, a scientific flight through a rocket's exahust plume in the 1970s detected a 40 percent decrease in ozone levels in the plume, reports Steven Aftergood of the Washington, D.C.-based American Federation of Scientists in the Sept. 20 JOURNAL Of GEOPHYSICAL RESEARCH. Aftergood suggests that launches may produce local ozone "holes" that persist for several hours.\n\nIn the same journal, Richard McPeters of NASA's Goddard Space Flight Center in Greenbelt, Md., and his colleagues respond to Aftergood's comments by examining satellite measurements of ozone in the shuttle launch area. They find no detectable ozone decrease after several launches.
348996
NO! Ozone is toxic!\n\nFresh air and supplemental oxygen will help.
308119
You have a misconception as to what an ozone layer is.  Ozone is a gas and is found throughout the atmosphere, even at ground level.  The ozone layer is the range in the atmosphere where ozone levels are the highest.  Oxygen O2 is present in the ozone layer as well (as are all other atmospheric gasses).  You should also note that in the ozone layer there isn't actually a whole lot of ozone, just more than there is anywhere else.  I think it's around 5 parts per million; meaning there is 1 molecule of ozone for every 200,000 other molecules.  There isn't a blanket of ozone, it's just an area where ozone is 5-10ppm instead of 1ppm or less.  \n\nWhy does most of it stay where it is?  Ozone is a somewhat unstable molecule and the same mechanism that typically forms ozone also breaks it down.  Simply, O2 gets hit by some photons of the right energy (some kind of UV light) and is split into O and O, one (or both) of those O's bonds to another O2 molecule to form O3, ozone.  Sooner or later, that O3 gets hit by the right energy of UV light and one of the O's break off to form O2 and a spare O which will find another O2 to bond with and repeat the cycle.  A small percent of the ozone does drop into the statosphere (where we live).
429253
If it generates more than 70ppm, then according to the EPA it is unsafe.  Personally, if you can smell the ozone, then it's unsafe.  This means that it's producing at least 30ppm.
234427
The true fucnction of the ozone layer for one. I left you a source below. \n\nAlso the first deep space probes were sent out into the solar system during the 70's. Try to google "Mariner space probe" or "Voyager space probe".
777429
Nitrogen is the most abundent element in our atmosphere.  Bacteria gets N2 from the air.
952260
Many materials can react with ozone to form oxygen as a by-product.  Most all are reducing agents.  A more definitive answer rests on how you are using the term "element".  If you are using it the periodic table sense then your answer would include many of the metals capable of being oxidized.
140016
Ozone Generators works by utilizing high voltages applied to a dielectric plates/surfaces to break up the oxygen molecule into radical oxygen ions (O/1). The ions are highly reactive and bonds with regular oxygen molecule (O/2) producing Ozone (O/3), which is unstable and is reactive as an oxidant, it will readily affect most plastic substances. and quickly combines with CFC (chloro-flouro-carbon) gas. Ozone is produced in nature during a lightning storm. Every lightning strike with its high voltage streams, ionizes atmospheric oxygen and produces ozone. A thin layer of ozone gas covers the earth's atmosphere preventing intense ultraviolet rays from the sun to reach the earth's surface. Ozone is known to have properties to deodorize and disinfect. but caution is expressed that over-exposure to high concentration of ozone gas could be hazardous to ones health. A commercial ozone generator is already adjusted to conform with health and safety laws that makes them available to the public as safe to use.\n~meow
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The Recipe For Ozone Loss\n\nTo summarise then, we have looked at the 'ingredients' or conditions necessary for the destruction of ozone that we see in Antarctica. The same applies more or less to the loss of ozone in the Arctic stratosphere during winter. Although in this case the loss is not nearly so severe.\n\nTo recap then, the requirements for ozone loss are:\n\nThe polar winter leads to the formation of the polar vortex which isolates the air within it.\n\nCold temperatures form inside the vortex; cold enough for the formation of Polar Stratospheric Clouds (PSCs). As the vortex air is isolated, the cold temperatures and the PSCs persist.\n\nOnce the PSCs form, heterogeneous reactions take place and convert the inactive chlorine and bromine reservoirs to more active forms of chlorine and bromine.\n\nNo ozone loss occurs until sunlight returns to the air inside the polar vortex and allows the production of active chlorine and initiates the catalytic ozone destruction cycles. Ozone loss is rapid. The ozone hole currently covers a geographic region a little bigger than Antarctica and extends nearly 10km in altitude in the lower stratosphere.
780167
I doubt it.  Ozone is a highly posionous element!  Ozonated water is used in factories for washing fruit and veg but as far as I know it isnt used for drinking.  Everything you can think of has be blamed for causing cancer at some stage!  Im happy to drink chlorinated water, its better than the consquenses!!!
259202
Here is a link that might help.  It is part of a general page on the Ozone Layer...\n\nhttp://en.wikipedia.org/wiki/Ozone_layer#Ozone_depletion\n\nhttp://en.wikipedia.org/wiki/Ozone_layer
297663
I did an AICHE project on this a year ago.  We set up a model using a tower and extracted CO2 from the atmosphere using NaOH.  CO2 + NaOH yields sodium bicarbonate.  It's very expensive to do, however, because the regeneration process of NaOH required a lot of energy.  Also, we ran into problems with air circulation.  Obviously the percentage of CO2 in the atmosphere is very small in comparison to nitrogen and oxygen, so in order to sequester enough CO2 to make a difference in the atmosphere, you have to be moving air at phenomenal velocities, which requires a lot of energy.  Burning fuel to produce this energy is kind of an oxymoron because you'd be adding to the problem of CO2; therefore, we used solar energy in our model.  We then said we'd store the CO2 in empty oil storages.
695248
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. It is present in low concentrations throughout the Earth's atmosphere. It has many industrial and consumer applications as well as being used in ozone therapy.\n\nOzone, 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 odour in lightning storms.[1] The odour from a lightning strike is from electrons freed during the rapid chemical changes, not the ozone itself.[2]\n\nPhysical properties\nUndiluted 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 [3]. At concentrations found in the atmosphere it is colorless [4]. The concentration above which it can be smelt (odor threshold) is between 0.0076 and 0.036 ppm[5].\n\n\n[edit] Chemistry\nOzone is a powerful oxidizing agent. It is also unstable at high concentrations, decaying to ordinary diatomic oxygen:\n\n2 O3 → 3 O2. \nThis 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:\n\n2 Cu2+ + 2 H+ + O3 → 2 Cu3+ + H2O + O2 \nOzone converts oxides to peroxides:\n\nSO2 + O3 → SO3 + O2 \nIt also increases the oxidation number of oxides:\n\nNO + O3 → NO2 + O2 \nThe above reaction is accompanied by chemiluminescence. The NO2 can be further oxidized:\n\nNO2 + O3 → NO3 + O2 \nThe NO3 formed can react with NO2 to form N2O5:\n\nNO2 + NO3 → N2O5 \nOzone reacts with carbon to form carbon dioxide, even at room temperature:\n\nC + 2 O3 → CO2 + 2 O2 \nOzone does not react with ammonium salts but it reacts with ammonia to form ammonium nitrate:\n\n2 NH3 + 4 O3 → NH4NO3 + 4 O2 + H2O \nOzone reacts with sulfides to make sulfates:\n\nPbS + 4 O3 → PbSO4 + 4 O2 \nSulfuric acid can be produced from ozone, either starting from elemental sulfur or from sulfur dioxide:\n\nS + H2O + O3 → H2SO4 \n3 SO2 + 3 H2O + O3 → 3 H2SO4 \nAll three atoms of ozone may also react, as in the reaction with tin(II) chloride and hydrochloric acid:\n\n3 SnCl2 + 6 HCl + O3 → 3 SnCl4 + 3 H2O \nIn the gas phase, ozone reacts with hydrogen sulfide to form sulfur dioxide:\n\nH2S + O3 → SO2 + H2O \nIn an aqueous solution, however, two competing simultaneous reactions occur, one to produce elemental sulfur, and one to produce sulfuric acid:\n\nH2S + O3 → S + O2 + H2O \n3 H2S + 4 O3 → 3 H2SO4 \nIodine perchlorate can be made by treating iodine dissolved in cold anhydrous perchloric acid with ozone:\n\nI2 + 6 HClO4 + O3 → 2 I(ClO4)3 + 3 H2O \nSolid nitryl perchlorate can be made from NO2, ClO2, and O3 gases:\n\n2 NO2 + 2 ClO2 2 O3 → 2 NO2ClO4 + O2 \nOzone 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:\n\n3 C4N2 + 4 O3 → 12 CO + 3 N2 \nOzone can react at cryogenic temperatures. At 77 K (-196 °C), atomic hydrogen reacts with liquid ozone to form a hydrogen superoxide radical, which dimerizes[6]:\n\nH + O3 → HO2 + O \n2 HO2 → H2O4 \nOzonides 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:\n\nKO2 + O3 → KO3 + O2 \nAlthough KO3 can be formed as above, it can also be formed from potassium hydroxide and ozone:[7]\n\n2 KOH + 5 O3 → 2 KO3 + 5 O2 + H2O \nNaO3 and LiO3 must be prepared by action of CsO3 in liquid NH3 on an ion exchange resin containing Na+ or Li+ ions:[8]\n\nCsO3 + Na+ → Cs+ + NaO3 \nTreatment wit
1065551
The ozone layer is thining through incresed pollutio by planes brought about by a peak in flyers, green house emissions, increased industrial pollution, forest degradation. all these allow more UV light penetration into earth and will continue to increase unless we stop polluting the environement.:(