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Photochlorination is a chlorination reaction that is initiated by light. Usually a C-H bond is converted to a C-Cl bond. Photochlorination is carried out on an industrial scale. The process is exothermic and proceeds as a chain reaction initiated by the homolytic cleavage of molecular chlorine into chlorine radicals by ultraviolet radiation ...
Chlorine: Cl 2 greenish yellow Bromine: Br 2 red/brown Iodine: I 2 dark purple Chlorine dioxide: ClO 2 intense yellow Dichlorine monoxide: Cl 2 O brown/yellow Nitrogen dioxide: NO 2 dark brown Trifluoronitrosomethane: CF 3 NO deep blue Diazomethane: CH 2 N 2 yellow
Hypochlorite salts formed by the reaction between chlorine and alkali and alkaline earth metal hydroxides. The reaction is performed at close to room temperature to suppress the formation of chlorates. This process is widely used for the industrial production of sodium hypochlorite (NaClO) and calcium hypochlorite (Ca(ClO) 2).
The haloform reaction, using chlorine and sodium hydroxide, is also able to generate alkyl halides from methyl ketones, and related compounds. Chloroform was formerly produced thus. [citation needed] Chlorine adds to the multiple bonds on alkenes and alkynes as well, giving di- or tetra-chloro compounds. [citation needed]
[26] [27] Wool scouring is the next process after the woollen fleece of a sheep is cut off. [28] Raw wool is also known as ''Greasy wool.'' "Grease" or "yolk'' is a combined form of dried sweat, oil and fatty matter. [29] Lanolin is the major component (5-25%) of raw wool which is a waxy substance secreted by the sebaceous glands of wool ...
The industrial-scale synthesis for sodium chlorate starts from an aqueous sodium chloride solution (brine) rather than chlorine gas. If the electrolysis equipment allows for the mixing of the chlorine and the sodium hydroxide , then the disproportionation reaction described above occurs.
Acetyl hypochlorite is reported to be produced by the reaction of acetic anhydride and dichlorine monoxide at very low temperatures: [2]. Cl 2 O + (CH3CO) 2 O → 2CH 3 COOCl. The liquid can be distilled at reduced pressure, however it cannot be heated, as it violently decomposes at 100 °C to acetic anhydride, oxygen, and chlorine gas, and reacts with water and alcohols.
The chlorite ion adopts a bent molecular geometry, due to the effects of the lone pairs on the chlorine atom, with an O–Cl–O bond angle of 111° and Cl–O bond lengths of 156 pm. [1] Chlorite is the strongest oxidiser of the chlorine oxyanions on the basis of standard half cell potentials.