Chlorine-Oxygen Compounds

From numerous chlorine oxides, only chlorine dioxide, CIO2, is fairly stable under certain conditions. The chlorine oxygen acids (hypochlorous acid, chlorous acid, chloric acid and perchloric acid) are formed by reaction of the corresponding chlorine oxides with water. 

Dichlorine oxide, CI2O, and chlorine dioxide, CIO2, all oxygen acids and their salts, particularly those of sodium and potassium, are used industrially. Their significance is based predominantly on their oxidizing power. The strongest oxidants are those with the lowest oxidation state of the chlorine atom. For 200 years, the textile and paper industry has been a main consumer of CIO2 and hypochlorite. 

Hypochlorous acid is produced by the reaction of chlorine and water 

Its use as water disinfectant is discribed in chapter 14.1 (Use of elemental chlorine). 

Solid hypochlorites are stable up to 80 °C, their stability depending on the water content, which is 1 % for bleaching powder, 0.3 % for tropical bleach. They decompose by reaction with water or by heating to 180 °C. 

---

Feedstocks come mainly from catalytic cracking. The catalyst system is sensitive to contaminants such as dienes and acetylenes or polar compounds such as water, oxygenates, basic nitrogen, organic sulfur, and chlorinated compounds, which usually require upstream treatment. 

Concentrated sulphuric acid has a strong affinity for water and great heat is evolved on mixing hence the acid must be added to water to dilute it. Because of this affinity, the acid can be used to dry gases with which it does not react, for example oxygen, chlorine, sulphur dioxide, and is used in desiccators. It will remove water of crystallisation from some compounds, for example... 

Chlorine and Bromine Oxidizing Compounds. The organo chlorine compounds shown in Table 6 share chemistry with inorganic compounds, such as chlorine/77< 2-3 (9-j5y and sodium hypochlorite/7 )< /-j5 2-5 7. The fundamental action of chlorine compounds involves hydrolysis to hypochlorous acid (see Cm ORiNE oxygen acids and salts). 

The purity of oxygen from chlorate candles before and after gas filtration is indicated in Table 2. A particulate filter is always used. Filter chemicals are HopcaUte, which oxidizes CO to CO2 molecular sieves (qv), which remove chlorine compounds and basic materials, eg, soda lime, which removes CO2 and chlorine compounds. Other than H2O and N2, impurity levels of <1 ppm can be attained. Moisture can be reduced by using a desiccant (see Desiccants). Gas purity is a function of candle packaging as well as composition. A hotter burning unit, eg, one in which steel wool is the binder, generates more impurities. 

HCIO4, one of the strongest of the mineral acids. The perchlorates are more stable than the other chlorine oxyanions, ie, chlorates, CIO chlorites, CIO or hypochlorites, OCf (3) (see Chlorine oxygen acids and salts). Essentially, all of the commercial perchlorate compounds are prepared either direcdy or indirectly by electrochemical oxidation of chlorine compounds (4—8) (see Alkali and chlorine products Electrochemical processing). 

Nevertheless, an anaerobic system may be the method of choice under certain conditions (/) contamination with compounds that degrade only or better under anaerobic conditions, (2) low yield aquifers that make pump and treat methods or oxygen and nutrient distribution impractical, (J) mixed waste contamination where oxidizable compounds drive reductive dehalogenation of chlorinated compounds, or (4) deep aquifers that make oxygen and nutrient distribution mote difficult and cosdy. 

Chlorites and Chlorine Dioxide" under "Chlorine Compounds, Inorganic" in ECT 1st ed., VoL 3, pp. 696—707, byj. F. White, Mathieson Chemical Corp. "Chlorous Acid, Chlorites, and Chlorine Dioxide" under "Chlorine Oxygen Acids and Salts" in ECT 2nd ed., Vol. 5, pp. 27—50, by H. L. Robson, Olin Mathieson Chemical Corp. "Chlorine Dioxide, Chlorous Acid, and Chlorites," in ECT 3rd ed., VoL 5, pp. 612—632, by M. G. Noack and R. L. Doerr, Olin Corp. 

OXIDIZING AGENT Coiupound that gives up oxygen easily or removes hydrogen from another compound. It may comprise a gas, e.g. oxygen, chlorine, fluorine, or a chemical which releases oxygen, e.g. a nitrate or perchlorate. A compound that attracts electrons. 

The pulp and paper industry is the largest industrial process water user in the U.S.5 In 2000, a typical pulp and paper mill used between 15,140 and 45,420 L (4000 to 12,000 gal) of water per ton of pulp produced. 1 2 3 4 General water pollution concerns for pulp and paper mills are effluent solids, biochemical oxygen demand (BOD), and color. Toxicity concerns historically occurred from the potential presence of chlorinated organic compounds such as dioxins, furans, and others (collectively referred to as adsorbable organic halides, or AOX) in wastewaters after the chlorination/ extraction sequence. With the substitution of chlorine dioxide for chlorine, discharges of the chlorinated compounds have decreased dramatically. 

Treatment of triphenylmethyl chloride with silver gave not the expected hydrocarbon but an oxygen-containing compound later found to be the peroxide. The reaction run in an inert atmosphere did give a hydrocarbon, but one with unusual properties. It reacted rapidly with oxygen, chlorine, and bromine, and was quite different from tetra-phenylmethane or what was expected of hexaphenylethane. Gomberg... 

Dioxin or furan refers to molecules or compounds composed of carbon and oxygen. These compounds when reacted with halogens such as chlorine or bromine acquire toxic properties. Most research on halogenated dioxin and furan has been concerned with chlorinated species. It is generally accepted that dioxin and furan are by-products of combustion processes including domestic and medical waste combustion or incineration processes.7 In combustion processes, hydrocar-... 

Chemical Agent HT Agent T is bis [2-(2-chloroethylthio) ethyl] ether (CAS 63918-89-8) and is a sulfur, oxygen and chlorine compound similar in structure to HD. It is 60 percent HD and 40 percent T plus a variety of sulfur contaminants and impurities, and is a blister agent. 

The price of the oxidation equivalent varies with the reagent [288]. Oxygen in air is the cheapest, followed by chlorine, electricity, hydrogen peroxide and finally ozone. Oxydation with oxygen at low temperature is only feasible biologically. Chlorine often forms very stable, highly toxic chlorinated compounds, which often limits its use. 

The double bond difference between the olefins and the paraffins is the quintessential difference between the petrochemicals and petroleum products— the petrochemicals industry depends much more on the chemical reactivity of the double-bonded molecules. While paraffins can be manipulated in refineries by separation or reshaping, olefins in a petrochemical plant are usually reacted with other organic compounds or another kind of atom or compound such as oxygen, chlorine, water, ammonia, or more of itself. The results are more complicated compounds useful in an increasing number of chemical applications. More on this in later chapters. 

Compressed oxygen, and fresh and recycled ethylene, are heated, mixed, and then passed through a reactor with fixed beds of catalyst— silver oxide deposited on alumina pellets. In recent years the catalyst has been improved by the addition of promoters and inhibitors. (Promoters—in this case compounds of alkali or alkaline rare earth metals—enhance the activity of the catalyst inhibitors—in this case chlorine compounds—chloroethane, or vinyl chloride, reduce its rate of activity decline.)... 

---