Read Chapter 06 Electrolysis of ICSE Class 10 Chemistry
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Chapter 06 Electrolysis PDF Resource
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Chapter 6: Electrolysis
Important Points To Remember
1. The conductors allow the passage of electric current through them in the solid state.
2. The insulators do not allow the passage of electric current through them.
3. In conductors, the current passes by the flow of electrons.
4. The electrolytes allow the passage of electric current through them in molten, fused or aqueous solution.
5. In electrolytes, the current passes by the flow of ions.
6. The non-electrolytes do not allow the passage of electric current through them.
7. When current is passed through electrolyte, it undergoes chemical decomposition, whereas in conductor when the current is passed it gets only heated up and no new product is formed, i.e., a physical change takes place.
| Conductors | Electrolytes |
|---|---|
| (i) They are metals. | (i) They are ionic compounds. |
| (ii) They are solids. | (ii) They exist in fused or molten state and in its aqueous solution. |
| (iii) The passage of electric current is by the flow of electrons. | (iii) The passage of electric current is by the flow of ions. |
| (iv) The passage of electric current through a conductor is a physical change i.e., the conductor gets only heated up, no new product is formed. | (iv) The passage of electric current through an electrolyte is a chemical change. |
8. The two terminals of the cell are called as cathode and anode.
9. Cathode is the negative terminal of the cell. Cations migrate towards cathode. The current leaves the electrolyte through the cathode.
10. Anode is the positive terminal of the cell. Anions migrate towards anode. The current enters the electrolyte through the anode.
11. Electrolysis is a redox reaction. Reduction takes place at cathode and oxidation at anode. The process of reduction and oxidation take place simultaneously. Therefore electrolysis is referred to as redox reaction.
At Cathode: NaCl - Na+ + Cl- Na+ + e- - Na (reduction)
At Anode: Cl- - e- - [Cl] (oxidation) 2[Cl] - Cl2
12. Reduction is the process of gain of electrons and it takes place at cathode. e.g., Na+ + e- - Na
13. Oxidation is the process of loss of electrons and it takes place at anode. e.g., Cl- - e- - [Cl] 2[Cl] - Cl2
Teacher's Note
Electrolysis is used in everyday applications like electroplating jewelry and battery charging, making it essential to understand the movement of ions and electrons in circuits.
Molten Lead Bromide Electrolysis
14. Molten Lead bromide is electrolysed by using inert electrodes. At cathode, lead metal is obtained whereas at anode Bromine vapours are obtained.
PbBr2 - Pb2+ + 2Br-
At Cathode: Pb2+ + 2e- - Pb (reduction)
At Anode: 2Br- - 2e- - 2[Br] (oxidation) 2[Br] - Br2
15. The ionic compounds which in their fused, molten state or in aqueous solution allow the passage of electric current are called as electrolytes.
16. There are eighteen vertical columns in the periodic table. The order for the arrangement of the group is (from left to right) I A, II A, III B, IV B, V B, VI B, VII B, VIII (undivided), I B, II B, III A, IV A, V A, VI A, VII A and zero. But according to the latest recommendations of IUPAC the groups are numbered from 1 to 18.
17. The elements of group 1, 2, 13, 14, 15, 16 and 17 are called as normal elements or representative elements. The elements of these groups are called as normal elements or representative elements. These elements have incomplete outer most shell.
18. The elements of group 3, 4, 5, 6, 7, 8, 9, 11 and 12 are known as transition elements.
19. The elements of group 18 or zero group are called as inert gases or noble gases or rare gases as they have stable configuration following the octet rule.
| Electrolyte | |
|---|---|
| Strong electrolyte / Weak electrolyte / Non-electrolyte |
20. Strong electrolyte: The electrolytes which almost completely dissociate in their aqueous solutions or molten states. The solution mainly consists of ions.
21. Weak electrolyte: The electrolytes which partially or incompletely dissociate in their aqueous solutions. The solution contains both ions and molecules.
22. Non-electrolyte: The solutions which do not ionise are called as non-electrolytes.
Examples Of Strong, Weak And Non-electrolytes
| Strong electrolytes | Weak electrolytes | Non-electrolytes |
|---|---|---|
| (i) Strong acids:HCl, H2SO4, HNO3 | (i) Weak acids: CH3COOH, HF, H2SO3, H3PO4, H2CO3 | (i) Petrol |
| (ii) Strong bases:NaOH, KOH | (ii) Weak bases: H3PO3, NH4OH | (ii) Sugar solution |
| (iii) All salts are strong electrolytes. | (iii) Liquid ammonia (iv) Carbon tetrachloride (v) Non-polar covalent compounds. |
23. Electrolysis: The chemical process in which the ionic compounds in their fused, molten or aqueous solutions allow the passage of electric current, undergo simultaneous chemical decomposition leading to the discharge of ions at electrodes is called as electrolysis.
Teacher's Note
Understanding electrolytes helps explain why salt water conducts electricity while pure water does not, a concept directly related to how our body maintains electrical signals in nerves and muscles.
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Chapter 06 Electrolysis Digital Textbook & Resources for Class 10 Chemistry
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