Dichlorine peroxide

Much has been learned in recent years about the 00 dimer , O2O2, produced in reaction 17. It is actually dichlorine peroxide, OOOCl its geometry is now well established from submillimeter wave spectroscopy (15). Photolysis of OOOO around 310 nm the atmospherically important wavelengths -- yields chlorine atoms and ClOO radicals (16), as given in reaction 18, rather than two OO radicals, even though QO-OQ is the weakest bond (it has a strength of about 17 Kcal/mol (17)). Thermal decomposition of QOOQ (the reverse of reaction 17) occurs very fast at room temperature, but more slowly at polar stratospheric temperatures. Hence, photolysis is the predominant destruction path for CIOOQ in the polar stratosphere and two Q atoms are produced for each ultraviolet photon absorbed. 

In this manner, it is estimated that one chlorine atom could be the catalyst for the destruction of as many as 100,000 ozone molecules before it is tied up in some inert form or moves out of the stratosphere. The preceding sequence is only one set of ozone-eating reactions. Others involve the formation of dichlorine peroxide, CI2O2, which is subsequently photochemically broken apart to two CIO molecules. 

Ammonia can also react violently with a large selection of chemicals including ethylene oxide, halogens, heavy metals, and oxidants such as chromium trioxide, dichlorine oxide, dinitrogen tetroxide, hydrogen peroxide, nitric acid, liquid oxygen, and potassium chlorate. 

Arsenic is violently oxidised by strong oxidants. This applies to potassium superoxide (incandescence of the element), dichlorine oxide (the released heat causes the chlorinated derivative to detonate), chromium (III) oxide Oncande-scence), potassium or silver nitrates (ignition), potassium permanganate or sodium peroxide (detonations). 

Sulfoxidation is usually carried out at an atmospheric pressure and the ratio of gaseous reactants S02 02 = 2 l [1-5]. The temperature of sulfoxidation depends upon the source of initiation. When the reaction is initiated by the UV light or 7-radiation [5,8-11], ozone [12-14], and dichlorine [5], it occurs at room temperature. Sulfoxidation initiated by peroxides or azo-compounds [13,15] occurs at elevated temperatures (320-360 K). 

Adipic acid, 2441 1,4-Benzoquinone, 2214 f 1,3-Butadiene, 1480 Cinnamaldehyde, 3134 Copper iron(II) sulfide, 4269 Dibromomethylborane, 0426 f Di-fe/7-butyl peroxide, 3074 Dichlorine oxide, Hydrocarbons, 4095... 

Dichlorine oxide Carbon, or Oxidisable materials Fluorine Non-metals Hydrogen peroxide Carbon Iodine heptafluoride Carbon Iodine(V) oxide Non-metals Nitrogen oxide Non-metals Nitrogen trifluoride Charcoal Oxygen difluoride Non-metals Oxygen (Liquid) Charcoal Ozone Charcoal, Potassium iodide... 

Oxidants. Hydrogen sulfide ignites on contact with silver bromate,8 bromine pentafluoride,9 mercury(I) bromate,10 lead hypochlorite,11 copper chromate,12 fluorine,13 fuming nitric acid,14 solid sodium peroxide,15 and dry or moist lead oxide.5 16 Dichlorine oxide17 or chlorine trifluoride18 explodes on contact with hydrogen sulfide. Heated chromium trioxide incandesces in a stream of hydrogen sulfide. 

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