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electrolysis

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Electrolysis 1. Electrolysis : The process due to which a chemical compound in fused state or in aqueous state conducts direct electric current, resulting in the discharge of ions of an electrolyte so as to form neutral atoms at their respective electrodes is called electrolysis. 2. Electrolyte : A chemical compound in fused state or in aqueous state which conducts direct electric current and at the same time decomposes to form neutral atoms at the electrodes is called an electrolyte. 3. Electrodes : The metal rods or plates through which current enters or leaves an electrolyte are called electrodes. 4. Cathode : The electrode connected to the negative terminal of a battery is called cathode. 5. Anode : The electrode connected to the positive terminal of a battery is called anode. 6. Cations : The positively charged ions which discharge at cathode are called cations. 7. Anions : The negatively charged ions which discharge at anode are called anions. 8. Electrolytic Cell : A glass vessel (or any other insulating material), containing two electrodes and an electrolyte is collectively called electrolytic cell. 9. Ionisation : The process of formation of positively charged and negatively charged ions from the molecules of polar covalent compounds is called ionisation. 10. Electrolytic Dissociation : The process in which separation of ions of an electrovalent compound takes place on heating or in aqueous solution is called electrolytic dissociation. 1 Key Points 11. Electropositive Series : Depending upon the ease with which metals lose electrons from their valence shell to form ions, they are arranged in a vertical column called electropositive series. 12. Electro-refining : The electrolytic process by which impurities are removed from an impure metal is called electro-refining. 13. Electroplating : The process of depositing a thin layer of a superior metal on the clean surface of a base metal, by the process of electrolysis is called electroplating. 14. Electrometallurgy : The extraction of metals from their fused ores by the process of electrolysis is called electrometallurgy. Chemical Equations at a Glance 1. Electrolysis of lead bromide using graphite electrodes ZZ X Pb 2+ + 2Br (i) Dissociation of lead bromide (i) PbBr2 YZZ (ii) Pb 2+ + 2e Pb. (ii) Reaction at cathode Br (iii) Br e Br + Br Br2 2. Electrolysis of acidulated water using platinum electrodes 2 ZZ X 2H + + SO 4 (i) H 2SO 4 YZZ (i) Ionisation of sulphuric acid ZZ X H + + OH (ii) H 2 O YZZ (ii) Ionisation of water (iii) Reaction at anode (iii) Reaction at cathode (iii) H + + e H H + H H 2 (g) (iv) Reaction at anode (iv) OH e OH 4OH 2H 2 O + O 2 (g) 2 Key Points 3. Electrolysis of acidified aqueous copper sulphate using copper electrodes ZZ X Cu 2+ + SO 2 (i) Dissociation of copper (i) CuSO 4 YZZ 4 sulphate ZZ X 2H + + SO 2 (ii) H 2SO 4 YZZ (ii) Ionisation of sulphuric acid 4 ZZ X H + + OH (iii) Ionisation of water (iii) H 2 O YZZ (iv) Cu 2 + 2e Cu (iv) Reaction at cathode (v) Reaction at anode (v) Cu 2e Cu 2+ 4. Electrolysis of acidified aqueous copper sulphate using platinum anode and copper cathode. ZZ X Cu 2+ + SO 2 (i) Dissociation of copper sulphate (i) CuSO 4 YZZ 4 + 2 ZZ X 2H + SO 4 (ii) H 2SO 4 YZZ (ii) Ionisation of sulphuric acid ZZ X H + + OH (iii) H 2 O YZZ (iv) Cu 2+ + 2e Cu (iii) Ionisation of water (iv) Reaction at cathode (v) OH 2e Cu 4OH 2H 2 O + O 2 (g) (v) Reaction at anode 5. Silver plating using silver anode (i) Dissociation of sodium ZZ X Na + + Ag + + 2CN argento cyanide (i) NaAg(CN) 2 YZZ ZZ X H + + CN (ii) Ionisation of HCN (ii) HCN YZZ (iv) Reaction at cathode ZZ X H + + OH (iii) H 2 O YZZ (iv) Ag + + e Ag (v) Reaction at anode (v) Ag e Ag + (iii) Ionisation of water 3 Key Points 6. Nickel plating using nickel anode 2 ZZ X Ni 2+ + SO 4 (i) Dissociation of nickel sulphate (i) NiSO 4 YZZ 2 ZZ X 2H + + SO 4 (ii) Ionisation of sulphuric acid (ii) H 2SO 4 YZZ ZZ X H + + OH (iii) H 2 O YZZ (iii) Ionisation of water (iv) Ni + + 2e Ni (iv) Reaction at cathode (v) Ni 2e Ni 2+ (v) Reaction at anode 7. Electro-refining of copper using pure copper as cathode and impure copper as anode ZZ X Cu 2+ + SO 2 (i) Dissociation of copper sulphate (i) CuSO 4 YZZ 4 ZZ X 2H + + SO 2 (ii) Ionisation of sulphuric acid (ii) H 2SO 4 YZZ 4 ZZ X H + + OH (iii) H 2 O YZZ (iii) Ionisation of water (iv) Cu 2+ + 2e Cu (iv) Reaction at cathode (v) Cu 2e Cu 2+ (v) Reaction at anode 8. Electrometallergy of sodium, using steel cathode and graphite anode ZZ X Na + + CI (i) Dissociation of fused (i) NaCI YZZ sodium chloride (ii) Na + + e Na (ii) Reaction at cathode (iii) CI + CI CI 2 (iii) Reaction at anode 9. Electrometallergy of potassium, using steel cathode and graphite anode ZZ X K + + CI (i) Dissociation of fused potassium (i) KCI YZZ chloride (ii) Reaction at cathode (ii) K + + e K (iii) CI e CI CI + CI CI 2 (iii) Reaction at anode 4 Key Points 10. Electrometallergy of calcium, using steel cathode and graphite anode ZZ X Ca 2+ + 2CI (i) Dissociation of fused (i) CaCI 2 YZZ calcium chloride (ii) Ca 2 + 2e (ii) Reaction at cathode Ca (iii) CI e CI CI + CI CI 2 11. Electrometallergy of aluminium using gas carbon anode and graphite cathode ZZ X 2Al3+ + 3O 2 (i) Dissociation of fused (i) Al2 O3 YZZ alumina ZZ X 3Na + + Al3+ + 6F (ii) Na 3 AlF6 YZZ (ii) Dissociation of fused cryolite (iii) Reaction at cathode (iii) Al3+ + 3e 3Na + + Al3+ + 6F (iii) Reaction at anode (iv) Reaction at anode (iv) O 2 2e [O] C + 2[O] CO 2 5 Key Points

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