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We have learnt that ionic compounds conduct electricity when molten or aqueous.

( Introduction ). ( Molten electrolyte ). ( Aqueous electrolyte ). ( Summary ). We have learnt that ionic compounds conduct electricity when molten or aqueous.

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We have learnt that ionic compounds conduct electricity when molten or aqueous.

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  1. ( Introduction ) ( Molten electrolyte ) ( Aqueous electrolyte ) ( Summary ) We have learnt that ionic compounds conduct electricity when molten or aqueous. When an electric current passes through such compounds, the compounds are decomposed in a chemical reaction. This is known as electrolysis. The ionic compound is called anelectrolyte. In this lesson, we will learn about the electrolysis of ( Exit ) • Molten ionic compounds ( Worksheet ) • Aqueous ionic compounds 4

  2. ( Introduction ) ( Molten electrolyte ) ( Aqueous electrolyte ) ( Summary ) Let us look at the electrolysis of molten lead (II) bromide. The experimental setup is shown below. Carbon electrodes Porcelain crucible ( Exit ) Molten lead(II) bromide Clay triangle Heat ( Worksheet ) 4

  3. The electrode attached to the negative terminal of the cell. • Cations are attracted to it. • The electrode attached to the positive terminal of the cell. • Anions are attracted to it. ( Introduction ) ( Molten electrolyte ) ( Aqueous electrolyte ) ( Summary ) ELECTRODES Anode Cathode ( Exit ) Electrodes are usually made of carbon or platinum, as they are unreactive or inert. They do not react with the compounds in electrolysis. ( Worksheet ) 4

  4. e- Pb Pb2+ + e- Pb2++ 2e- Pb ( Introduction ) ( Molten electrolyte ) ( Aqueous electrolyte ) ( Summary ) At the cathode The lead ions take electrons from the cathode to become lead atoms(reduction). ( Exit ) Lead forms molten globules at the bottom of the crucible. We say the lead ions have been discharged. ( Worksheet ) 4

  5. Br - + e- e- Br - Br Br 2Br - Br2+ 2e- ( Introduction ) ( Molten electrolyte ) ( Aqueous electrolyte ) ( Summary ) At the anode The bromide ions donate electrons to the anode to become bromide molecules(oxidation). ( Exit ) The bromine is seen as a reddish-brown gas around the anode during the electrolysis. ( Worksheet ) 4

  6. PbBr2 Pb + Br2 cathode Pb2+ Br - Pb2+ Br - Molten lead (II) bromide ( Introduction ) ( Molten electrolyte ) ( Aqueous electrolyte ) ( Summary ) The overall chemical reaction is anode Lead ions are attracted to the cathode Bromide ions are attracted to the anode ( Exit ) ( Worksheet ) 4

  7. cathode anode Pb2+ Br - Pb2+ Br - ( Introduction ) ( Molten electrolyte ) ( Aqueous electrolyte ) ( Summary ) Lead ions move near to cathode Bromide ions move near to anode ( Exit ) Molten lead (II) bromide ( Worksheet ) 4

  8. cathode anode Bromide ions donate electrons Pb2+ Br - Pb2+ Br - ( Introduction ) ( Molten electrolyte ) ( Aqueous electrolyte ) ( Summary ) e- e- ( Exit ) Molten lead (II) bromide ( Worksheet ) 4

  9. cathode anode Bromide ions donate electrons Pb2+ Br - Pb2+ Br - ( Introduction ) ( Molten electrolyte ) ( Aqueous electrolyte ) ( Summary ) e- e- Electrons flow from anode to battery e- e- ( Exit ) Molten lead (II) bromide ( Worksheet ) 4

  10. cathode anode Bromide ions donate electrons Pb2+ Br - Pb2+ Br - ( Introduction ) ( Molten electrolyte ) ( Aqueous electrolyte ) ( Summary ) Battery pumps electrons e- e- e- e- e- ( Exit ) Molten lead (II) bromide ( Worksheet ) 4

  11. cathode anode Bromide ions donate electrons Pb2+ Br - Pb2+ Br - ( Introduction ) ( Molten electrolyte ) ( Aqueous electrolyte ) ( Summary ) e- e- e- e- Electrons flow from battery to cathode e- e- ( Exit ) Molten lead (II) bromide ( Worksheet ) 4

  12. cathode anode Bromide ions donate electrons Pb2+ Br - Pb2+ Br - ( Introduction ) ( Molten electrolyte ) ( Aqueous electrolyte ) ( Summary ) e- e- e- e- e- Electrons flow from battery to cathode e- e- e- Lead ions accept electrons e- e- ( Exit ) e- Molten lead (II) bromide ( Worksheet ) 4

  13. Pb Br Br Br Pb Br Mg Mg Cl Cl ( Introduction ) ( Molten electrolyte ) ( Aqueous electrolyte ) ( Summary ) cathode anode Lead atoms are produced Bromine atoms combine to form bromine gas ( Exit ) Molten lead (II) bromide ( Worksheet ) 4

  14. ( Introduction ) ( Molten electrolyte ) ( Aqueous electrolyte ) ( Summary ) QUIZ 1 1. The electrolysis of molten iron (III) chloride yields iron metal and a gas. What is the colour of this gas produced? A. Reddish-brown. B. Colourless. ( Exit ) C. Yellowish-green. ( Worksheet ) 4 Next question Click on the correct answer

  15. ( Introduction ) ( Molten electrolyte ) ( Aqueous electrolyte ) ( Summary ) QUIZ 1 2. With reference to the previous question, at which electrode is the gas formed? A. Anode. B. Cathode. ( Exit ) ( Worksheet ) 4 Click on the correct answer

  16. test-tubes electrolyte (solution) carbon electrodes ( Introduction ) ( Molten electrolyte ) ( Aqueous electrolyte ) ( Summary ) Solutions can be electrolysed using the apparatus shown below. ( Exit ) - + ( Worksheet ) 4 to battery

  17. test-tubes dilute hydrochloric acid carbon electrodes ( Introduction ) ( Molten electrolyte ) ( Aqueous electrolyte ) ( Summary ) Let us look at the electrolysis of dilute hydrochloric acid. The experimental setup is shown below. ( Exit ) - + ( Worksheet ) 4 to battery

  18. H + e- H+ H++ e- H H H H + H H + HH2 ( Introduction ) ( Molten electrolyte ) ( Aqueous electrolyte ) ( Summary ) At the cathode The hydrogen ions take electrons from the electrode to become hydrogen atoms(reduction). When two of the newly formed atoms combine, hydrogen gas is produced. ( Exit ) ( Worksheet ) 4

  19. H H H H OH- O O OH- O O OH- + + OH- e- e- e- e- 4OH- O2 + 2H2O + 4e- ( Introduction ) ( Molten electrolyte ) ( Aqueous electrolyte ) ( Summary ) At the anode There are two anions in the electrolyte: hydroxide and chloride ions. Since hydroxide ions are easier to discharge, oxygen gas is produced at the anode. ( Exit ) ( Worksheet ) 4

  20. hydrogen oxygen carbon electrodes - + ( Introduction ) ( Molten electrolyte ) ( Aqueous electrolyte ) ( Summary ) The electrolysis of dilute hydrochloric acid is will result in the production of hydrogen gas and oxygen at the cathode and anode respectively. dilute hydrochloric acid ( Exit ) ( Worksheet ) 4

  21. ( Introduction ) ( Molten electrolyte ) ( Aqueous electrolyte ) ( Summary ) What gas do you think will be found at the anode when aqueous copper(II) sulphate is electrolysed? Sulphur dioxide? No, not quite. Oxygen gas is evolved at the anode instead and copper metal is deposited at the cathode. How do you explain this phenomenon? The products can come from the electrolyte or from the water present. The product that is discharged depends on the nature of the ions. ( Exit ) 4 ( Worksheet )

  22. ( Introduction ) ( Molten electrolyte ) ( Aqueous electrolyte ) ( Summary ) Negative ions from the electrolyte are discharged if they are chloride, bromide or iodide ions. For sulphates and nitrates, oxygen from water is discharged. Positive ions from the electrolyte that are below Ni2+(aq) in the electrochemical (or reactivity) series are discharged at the negative cathode. If the positive ions are those of reactive metals above Ni2+(aq) (e.g.. Na+, K+ and Ca2+), hydrogen gas from water is discharged. ( Exit ) ( Worksheet ) 4

  23. Anions Cations SO42- (aq) NO3- (aq) Cl - (aq) Br - (aq) I - (aq) OH - (aq) SO42- (aq) K+ (aq) Na+ (aq) Ca2+ (aq) Mg2+ (aq) Zn2+ (aq) Fe2+ (aq) Pb2+ (aq) H+ (aq) Cu2+ (aq) Ag+ (aq) ( Introduction ) ( Molten electrolyte ) ( Aqueous electrolyte ) ( Summary ) Difficulty of discharge decreases ( Exit ) ( Worksheet ) 4

  24. ( Introduction ) ( Molten electrolyte ) ( Aqueous electrolyte ) ( Summary ) QUIZ 2 1. When we electrolyse a solution, what takes place at the cathode? A. Oxidation. B. Reduction. ( Exit ) ( Worksheet ) 4 Next question Click on the correct answer

  25. ( Introduction ) ( Molten electrolyte ) ( Aqueous electrolyte ) ( Summary ) QUIZ 2 2. During the electrolysis of sulphuric acid, hydrogen gas and another gas are produced. What is the other gas? A. Oxygen. B. Sulphur dioxide. ( Exit ) ( Worksheet ) 4 Click on the correct answer

  26. Industrial Applications of Electrolysis

  27. (a) A silver-plated teapot.(b) Schematic of the electroplating of a spoon.

  28. Schematic of the electroplating of a spoon. AgNO3(aq)

  29. Molten NaCl Observe the reactions at the electrodes - + battery Cl2 (g) escapes Na (l) NaCl (l) Na+ Cl- Na+ Cl- (-) (+) electrode half-cell electrode half-cell Cl- Na+ Na+ + e- Na 2Cl- Cl2 + 2e-

  30. Molten NaCl Electrolytic Cell cathode half-cell (-) REDUCTION Na+ + e- Na anode half-cell (+) OXIDATION 2Cl- Cl2 + 2e- overall cell reaction 2Na+ + 2Cl- 2Na + Cl2 X 2

  31. A schematic diagram of an electrolytic cell for producing aluminum by the Hall-Heroult process.

  32. Fig. 22.19 A schematic diagram of an electrolytic cell for producing aluminum by the Hall-Heroult process.

  33. CO2 bubbles Al2O3 (l) carbon-lined steel vessel acts as cathode e- + graphite anodes From power source Al+3 - Al+3 e- O-2 O-2 O-2 Al (l) Draw off Al (l) Cathode: Al+3 + 3e- Al (l) Anode: 2 O-2 + C (s)  CO2 (g) + 4e-

  34. The Hall Process Cathode: Al+3 + 3e- Al (l) x 4 Anode: 2 O-2 + C (s)  CO2 (g) + 4e- x 3 4 Al+3 + 6 O-2 + 3 C (s)  4 Al (l) + 3 CO2 (g) The graphite anode is consumed in the process.

  35. Production of solid Mg

  36. Anode Chatode impure copper become an anode will reduced during electrolysis. pure copper produced, covering Cathode Fe2+ Zn2+ Cu2+ SO42- H+ pure copper Impure copper CuSO4/ H2SO4 Solution as electrolyte Precipitation of impurities

  37. The Mercury Cell for Production of Chlorine and Sodium Hydroxide

  38. ( Introduction ) ( Molten electrolyte ) ( Aqueous electrolyte ) ( Summary ) • The decomposition of a substance by electricity is called electrolysis. • An electrolyte is an ionic compound, in the molten or aqueous state, that conducts electricity and is decomposed by the current. • The rods through which the direct current enters and leaves the cell are known as electrodes. Electrodes are usually inert. ( Exit ) ( Worksheet ) 4

  39. ( Introduction ) ( Molten electrolyte ) ( Aqueous electrolyte ) ( Summary ) • The anode is the electrode which is connected to the positive terminal of a cell. Anions are attracted to it. Oxidation occurs at the anode. • The cathode is the electrode connected to the negative terminal of the cell. Cations are attracted to the cathode. Reduction occurs at this electrode. ( Exit ) ( Worksheet ) 4

  40. ( Introduction ) ( Molten electrolyte ) ( Aqueous electrolyte ) ( Summary ) • When a molten electrolyte is electrolysed, • a metal (from the positive ions) is discharged at the cathode. • a non-metal (from the negative ions) is discharged at the anode. ( Exit ) ( Worksheet ) 4

  41. ( Introduction ) ( Molten electrolyte ) ( Aqueous electrolyte ) ( Summary ) • When a aqueous electrolyte is electrolysed, • the products come from either the electrolyte or water present. • The product at the cathode is a metal or hydrogen gas. • The product at the anode is a non-metal. ( Exit ) ( Worksheet ) 4

  42. ( Introduction ) ( Molten electrolyte ) ( Aqueous electrolyte ) ( Summary ) • Reactive metals are not discharged at the cathode. Instead, hydrogen from water is evolved. • Sulphate and nitrate ions are not discharged at the anode. Instead, oxygen from water is produced. ( Exit ) ( Worksheet ) 4

  43. ( Introduction ) ( Molten electrolyte ) ( Aqueous electrolyte ) ( Summary ) Credits ( Exit ) return to micro lessons ( Worksheet ) 4

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