Chlorine reactive compounds

Liquid chlorine dioxide, ClOj, boils at 284 K to give an orange-yellow gas. A very reactive compound, it decomposes readily and violently into its constituents. It is a powerful oxidising agent which has recently found favour as a commercial oxidising agent and as a bleach for wood pulp and flour. In addition, it is used in water sterilisation where, unlike chlorine, it does not produce an unpleasant taste. It is produced when potassium chlorate(V) is treated with concentrated sulphuric acid, the reaction being essentially a disproportionation of chloric(V) acid ... 

Derbyshire and Waters202 carried out the first kinetic study, and showed that the chlorination of sodium toluene-m-sulphonate by hypochlorous acid at 21.5 °C was catalysed more strongly by sulphuric acid than by perchloric acid and that the rate was increased by addition of chloride ion. A more extensive examination by de la Mare et al.203 of the rate of chlorination of the more reactive compounds, anisole, phenol, and />-dimethoxybenzene by hypochlorous acid catalysed by perchloric acid, and with added silver perchlorate to suppress the formation of Cl2 and C120 (which would occur in the presence of Cl" and CIO-, respectively),... 

Martin (16) has also suggested such a relationship in the chlorinated polycyclic compounds such as chlordan. Accordingly the author has measured the reactivities of the... 

Chlorine dioxide is a yellow to reddish-yellow gas that can decompose rapidly in air. Because it is a hazardous gas, chlorine dioxide is always made at the place where it is used. Chlorine dioxide is used as a bleach at pulp mills, which make paper and paper products, and in public water treatment facilities, to make water safe to drink. In 2001, chlorine dioxide was used to decontaminate a number of public buildings following the release of anthrax spores in the United States. Chlorine dioxide is soluble in water and will rapidly react with other compounds. When it reacts in water, chlorine dioxide will form chlorite ion, which is also a very reactive compound. 

Chlorine dioxide is a very reactive compound and will not exist in the environment for long periods of time. In air, sunlight will quickly break apart chlorine dioxide into chlorine gas and oxygen. In water, chlorine dioxide will react quickly to form chlorite ions. In water treatment systems, chlorine dioxide will not form certain harmful compounds (e.g., trihalomethanes) when it reacts with dissolved organic compounds. Chlorine dioxide does form other disinfection byproducts, such as chlorite and chlorate ions. 

Like chlorine dioxide, chlorite is a very reactive compound. Since chlorite is an ion, it vrill not exist in air. In water, chlorite ions will be mobile and may move into groundwater. However, reaction with soils and sediments may reduce the concentration of chlorite ions capable of reaching groundwater. For additional information about what happens to chlorine dioxide and chlorite when they enter the environment, see Chapter 6. 

Chlorine dioxide is a very reactive compound and may exist in the environment for only short periods of time (see Section 6.3.2). Chlorine dioxide is readily soluble as a dissolved gas. However, chlorine dioxide can be easily driven out of aqueous solutions with a strong stream of air. The partition coefficient between water and C102(g) is about 21.5 at 35 °C and 70.0 at 0 °C (Aieta and Berg 1986 Kaczur and Cawlfield 1993 Stevens 1982). Transport and partition of chlorine dioxide in soils and sediments will not be significant. Chlorine dioxide is expected to be reduced to chlorite ions in aqueous systems (see Section 6.3.2.2). 

The nucleophilic substitution of 1,2,3-triazole is also activated by A-oxidation. In 3-substituted 1,2,3-triazole 1-oxides, a halogen substituent at C(4) is more reactive than one at C(5) <87ACS(B)724>. Therefore, the C(4) chlorine of compound (221) (Equation (19)) is displaced by methoxide under much milder conditions than the corresponding C(5) chlorine of (222) (Scheme 39), and the only C(5) bromine is displaced in the case of 4,5-dibromotriazole 1-oxide <88BSB573>. 

Bromine pentafluoride is a highly reactive compound combining explosively or with ignition with most elements and their compounds. Spontaneous explosion or flaming can occur when mixed with water, organic compounds, metal powder, metal hahdes, metal oxides, metal sulfides and chlorine (upon warming) (Patnaik, P. 1999. A Comprehensive Guide to the Hazardous Properties of Chemical Substances, 2nd ed. New York John Wdey). 

A computer literature search revealed no direct analytical method specific for sodium dichloroisocyanurate dihydrate (NaDCC) or trichloroisocyanuric acid (TCCA). Each compound dissolved in water released chlorine in the positive oxidation state and formed complex equilibria reactions dependent on the pH of the solutions. NaDCC and TCCA are very strong oxidants and very reactive compounds, therefore, incompatible for chromatographic analysis. The only method that is used for analysis of compounds containing... 

ELUmo measures the ability of a molecule to accept electrons. Compounds with low Elumo tend to accept electrons easily. Thus, the coefficient of ELUMO is negative. Theoretically a compound with more negative AHf or lower AHf is more stable (Fried et al., 1977) therefore, it is reasonable that the coefficient of AHf in Equation (13.50) is positive, as shown in Table 13.13. Thus, the higher the AHf value is, the more unstable or reactive the chlorinated compounds will be. As a result, the log k values are greater. LFER analysis on dechlorination by Fe° of chlorinated aliphatic compounds, ELUMO, and AHf have been confirmed to be more significant molecular descriptors than other... 

The trichlorotriazine molecule was the first reactive compound that was found to be able to form a reactive bridge between dye and substrate. One chlorine atom reacts with the amino group of the dye, and the other two chlorine atoms can then react bifunctionally with the substrate (or water) to form covalent bonds. An example is C.I. Reactive Yellow4, 13190 [1222-45-8] (20). 

There is a general consensus (vide supra) on the environmental importance of catalytic reactions on the surface of many minerals. However, there is limited information in the literature about specific examples [9]. Systematic studies would allow the understanding of the dependence of the catalytic activity on mineral structure, mineral chemistry and surface reactivity. At the same time, this knowledge would be useful in designing remediation techniques based on minerals instead of synthetic catalysts. For example, sphalerite and ilmenite have been shown to be capable of degrading chlorinated carbon compounds via a photo catalytic mechanism [63]. 

These oxidation processes also dominate in the chemistry of air pollution, where the occurrence of harmful levels of O3 and acidic aerosols depends on the relative and absolute levels of urban emissions of NO, CO, RH, and SO2. In the marine and polar troposphere, reactive compounds of chlorine, bromine, and iodine provide a small but significant additional pathway for oxidation besides OH, as discussed by von Glasow and Cmtzen (see Chapter 4.02). 

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