2. The ionic compound is called an electrolyte.
( 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 an electrolyte.
In this lesson, we will learn about the electrolysis of
( Exit )
Molten ionic compounds
( Worksheet )
Aqueous ionic compounds 4

3. ( 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
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4. ELECTRODES Anode Cathode
( Introduction )
( Molten electrolyte )
( Aqueous electrolyte )
( Summary )
ELECTRODES
Anode
Cathode
The electrode attached to the positive terminal of the cell.
Anions are attracted to it.
The electrode attached to the negative terminal of the cell.
Cations are attracted to it.
( Exit )
Electrodes are usually made of carbon or platinum, as they are unreactive or inert. They do not react with the compounds in electrolysis.
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5. Pb2+ + 2e- Pb At the cathode
( Introduction )
( Molten electrolyte )
( Aqueous electrolyte )
( Summary )
At the cathode
The lead ions take electrons from the cathode to become lead atoms (reduction).
Pb2+ e- Pb +
Pb e Pb
( Exit )
Lead forms molten globules at the bottom of the crucible. We say the lead ions have been discharged.
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6. ( Introduction )
( Molten electrolyte )
( Aqueous electrolyte )
( Summary )
At the anode
The bromide ions donate electrons to the anode to become bromide molecules (oxidation).
Br - Br e- +
2Br Br e-
( Exit )
The bromine is seen as a reddish-brown gas around the anode during the electrolysis.
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7. Lead ions are attracted to the cathode
( Introduction )
( Molten electrolyte )
( Aqueous electrolyte )
( Summary )
The overall chemical reaction is
PbBr Pb Br2
cathode
Pb2+
Br -
Molten lead (II) bromide
anode
Lead ions are attracted to the cathode
Bromide ions are attracted to the anode
( Exit )
( Worksheet ) 4

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

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

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

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

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

13. e- e- e- e- e- e- e- e- e- e- e- Bromide ions donate electrons Pb2+
( Introduction )
( Molten electrolyte )
( Aqueous electrolyte )
( Summary ) e- e-
Bromide ions donate electrons
anode
cathode
Pb2+
Br - 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

14. Lead atoms are produced Bromine atoms combine to form bromine gas Mg
( Introduction )
( Molten electrolyte )
( Aqueous electrolyte )
( Summary )
cathode
anode Br
Lead atoms are produced
Bromine atoms combine to form bromine gas Mg Pb Br Cl
( Exit ) Mg Br Cl
Molten lead (II) bromide
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15. ( 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
Click on the correct answer
Next question

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

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

19. H+ + e- H H + H H2 At the cathode
( Introduction )
( Molten electrolyte )
( Aqueous electrolyte )
( Summary )
At the cathode
The hydrogen ions take electrons from the electrode to become hydrogen atoms (reduction). H+ H + e-
H e H
When two of the newly formed atoms combine, hydrogen gas is produced.
( Exit ) H +
H H H2
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20. 4OH- O2 + 2H2O + 4e- At the anode
( 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. O + e- H
OH -
4OH O H2O e-
( Exit )
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21. ( 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.
oxygen
carbon electrodes - +
hydrogen
dilute hydrochloric acid
( Exit )
( Worksheet ) 4

22. How do you explain this phenomenon?
( 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.
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( Worksheet )

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

25. 1. When we electrolyse a solution, what takes place at the cathode?
( 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 )
Next question 4
Click on the correct answer

26. ( 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

27. Industrial Applications of Electrolysis

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

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

30. Observe the reactions at the electrodes
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-  Cl e-

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

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

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

35. Production of aluminum by electrolysis (Hall-Héroult Process)
1. Al2O3 is dissolved in cryolite, Na3AlF6.
2. The Al3+ is reduced to Al(l) and the O2- oxidized to O2, which reacts with the carbon anode to produce CO2.
3. Molten aluminum is periodically drawn off and additional Al2O3 is added.
4. The carbon anodes must occasionally be replaced as they are
consumed by the reaction with oxygen.

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

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

38. Production of solid Mg applications
• Magnesium is used in many “light weight” structural
applications
• A major source of magnesium is seawater
• Seawater is made basic causing Mg2+ to precipitate as Mg(OH)2
• The precipitate is separated by filtration and dissolved in hydrochloric acid:
Mg(OH)2(s)+2HCl(aq) MgCl2(aq)+2H2O
• The resulting solution is evaporated to give solid MgCl2, which is melted and electrolyzed:
MgCl2(l) Mg(l)+Cl2(g)

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

41. Electrolysis of brine using a mercury cell.
• At the anode, chloride ions are oxidized to chlorine.
• At the cathode, sodium ions are reduced to sodium atoms, which dissolve in the mercury.
• The mercury is pumped into a separate compartment and exposed to water.
• The dissolved sodium reacts with the water to form H2 and NaOH.

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

43. ( 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 )
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44. ( 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 )
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45. When a molten electrolyte is electrolysed,
( 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

46. When a aqueous electrolyte is electrolysed,
( 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

47. ( 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

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