3Cl 2FeCl 2Al + 3Cl 2AlCl Cu + Cl CuCl H + Cl 2HCl ; H = 44kCal ∆ XII XII - - - - 2B + 3Cl 2BCl 2S + Cl S Cl P disulphur dichloride + 6Cl 4PCl 2As + 3Cl 2AsCl 2Sb + 3Cl 2SbCl Affinity for hydrogen : When burnt with turpentine it forms carbon and hydrochloric acid. C H + 8Cl 10C + 16HCl It forms dioxygen when reacting with water in presence of sunlight. When chlorine in water is exposed to sunlight it loses its colour and smell as the chlorine is converted into hydrochloric acid. 2Cl + 2H O O + 4HCl Chlorine reacts with ammonia to give ammonium chloride and other products as shown below: With excess ammonia, 2NH + 3Cl N + 6HCl 6HCl + NH NH Cl overall r eaction 8NH + 3Cl N NH Cl NH + 3Cl NCl + 3HCl 3HCl + 3NH 3NH Cl overall re action 4NH + 3Cl NCl 3NH Cl Chlorine oxidises hydrogen sulphide to sulphur and liberates bromine and iodine from iodides and bromides.
However, it doesn't oxidise fluorides H S + Cl 2HCl + S Cl + 2KBr 2KCl + Br Cl + 2KI 2KCl + I Reaction with alkali: Chlorine reacts with cold dilute alkali to give chloride and hypochlorite while with hot concentrated alkali chlorides and chlorates are formed. Cl + H O HCl + HOCl HCl + NaOH NaCl + H O HOCl + NaOH sodium NaOCl + H O overall reaction Cl + 2NaOH NaOCl hypo chlorite + NaCl + H O With excess chlorine, XII XII - - - - Cl + H O HCl + HOCl HCl + NaOH NaCl + H O ) × HOCl + NaOH NaOCl + H O 3NaOCl NaClO + 2NaCl overall reaction 3Cl + 6NaOH NaClO sodium chlorat e + 5NaCl + 3H O Oxidising and bleaching action: Chlorine is a strong oxidising and bleaching agent because of the nascent oxygen. H O + Cl