Chlorine is capable to form several various oxides. All of them are applied in the industry in large volumes as are demanded in many fields of the industry.
Chlorine forms a number of oxides which total number is the whole five types with oxygen. Everything them can be described the general formula ClxOy. In them the valency of chlorine changes from 1 to 7. Valency of different oxides of chlorine is various: Cl2O - 1, Cl2O3 - 3, ClO2 - 4, Cl2O6 - 6, Cl2O7 - 7.
Oxide of chlorine (I) is applied to production of hypochlorites which are the strong bleaching and disinfecting agents.
Oxide of chlorine (II) is actively applied to bleaching of flour, cellulose, paper and other things and also to sterilization and disinfection. Oxide of chlorine (VI) and oxide of chlorine (VII) apply to synthesis of organic compounds.
Receiving Cl2O
This oxide on large-capacity productions is received in two ways.1. By the Peluza method. Carry out reaction between gaseous chlorine and oxide of mercury. Depending on conditions other compound of mercury can be formed, however the target product remains. After that gaseous oxide of chlorine is liquefied at a temperature of-60 degrees Celsius. The reaction equations describing the Peluza method: 2HgO + Cl2 = Hg2OCl2 + Cl2OHgO + 2Cl2 = HgCl2 + Cl2O2. Interaction of chlorine with water solution sodium carbonate on reaction: 2Cl2 + 2Na2CO3 + H2O = 2NaHCO3 + Cl2O + 2NaClKarbonat sodium can be replaced with other carbonates of alkaline or alkaline-earth metals.
Receiving ClO2
The only industrial method of receiving dioxide of chlorine is based on interaction of chlorate of sodium and dioxide of sulfur in acidic environment. Reaction becomes result of such interaction: 2NaClO3 + SO2 + H2SO4 = 2NaHSO4 + ClO2
Receiving Cl2O6
In the industry of Cl2O6 receive chlorine dioxide interaction with ozone: 2ClO2 + 2O3 = 2O2 + Cl2O6
Receiving Cl2O7
1. Careful heating of chloric acid with phosphoric anhydride leads to office of oily liquid which is oxide of chlorine (VII). All process is described by reaction: 2HClO4 + P4O10 = H2P4O11 + Cl2O72. The second way of receiving this oxide is connected with electricity. If to carry out electrolysis of solution of chloric acid, then in anode space it is possible to find Cl2O7.3. Heating in a vacuum of perchlorates of transitional metals leads to formation of oxide of chlorine (VII). Most often heat perchlorate of niobium or molybdenum.
Physical properties of oxides
Cl2O: under standard conditions ocherous gas with a chlorine smell, and at a temperature below +2 degrees Celsius golden-red liquid. It is explosive in high concentrations. ClO2: under standard conditions – gas with a characteristic smell of red-yellow color, at a temperature below +10 degrees Celsius – red-brown liquid. Blows up on light, in the presence of reducers and at heating.Cl2O6: unstable gas which begins to decay at a temperature from 0 to +10 degrees Celsius with formation of dioxide of chlorine at 20 degrees Celsius is formed chlorine. In view of formation of dioxide of chlorine – it is explosive. Cl2O7: colourless oily liquid which when heating above 120 degrees Celsius explodes. Can detonate from blow.