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Electrochemistry basics
Chemistry
Useful for: OSSC RHT — Regular High School Teacher, OSEPA Upper Primary — Science, OSSC Science, OSSSC Govt TGT Science — CBZ, OSSSC Govt TGT Science — PCM, SSB Lecturer (Degree Colleges), SSB TGT CBZ, SSB TGT PCM
Overview
Electrochemistry links chemical reactions with electricity: galvanic cells produce electricity and electrolysis uses electricity to drive reactions.
Key points
- Oxidation occurs at the anode; reduction at the cathode.
- In the Daniell cell, zinc is the anode and copper the cathode.
- Electrolysis decomposes an electrolyte using electric current.
- Faraday’s laws relate the amount of substance deposited to the charge passed.
- Electroplating coats one metal with another.
- Corrosion of iron is an electrochemical process.
Explanation
- More reactive metals act as anodes.
- Galvanising protects iron with zinc.
- Lithium-ion batteries are rechargeable.
- Electrolysis of brine produces chlorine, hydrogen and sodium hydroxide.
- Conductivity depends on ions in solution.
Step by step
- Identify the concept, method or fact asked.
- Recall the definition, thinker, year or rule.
- Apply it and eliminate extreme or mismatched options.
Examples
- In the Daniell cell, the electrode that dissolves → zinc anode.
- Silver coating on a spoon → electroplating.
- Rusting of iron → electrochemical corrosion.
Traps and advanced points
- Trap: Swapping anode and cathode reactions.
- Trap: Thinking pure water conducts well.
- Trap: Ignoring Faraday’s laws.
Quick revision
- Anode oxidation; cathode reduction.
- Daniell: Zn anode, Cu cathode.
- Faraday’s laws.
Practice MCQs
Oxidation occurs at the —
- electrolyte only
- cathode
- anode
- salt bridge
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Answer: (c) anode. Anode = oxidation.
Reduction occurs at the —
- anode
- cathode
- wire
- voltmeter
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Answer: (b) cathode. Cathode = reduction.
In the Daniell cell, the anode is —
- silver
- carbon
- copper
- zinc
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Answer: (d) zinc. Zinc dissolves.
Electrolysis uses electricity to —
- produce light only
- decompose an electrolyte
- store heat
- melt metals only
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Answer: (b) decompose an electrolyte. Electrical energy drives a reaction.
Coating a spoon with silver using electricity is —
- rusting
- galvanising
- electroplating
- alloying
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Answer: (c) electroplating. Electroplating.
Faraday’s laws relate the mass deposited to the —
- container size
- room temperature
- charge passed
- colour of solution
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Answer: (c) charge passed. Quantity of electricity.
Rusting of iron is —
- a nuclear reaction
- sublimation
- a physical change
- an electrochemical process
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Answer: (d) an electrochemical process. Corrosion is electrochemical.
Galvanising protects iron by coating it with —
- copper
- tin
- silver
- zinc
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Answer: (d) zinc. Zinc is more reactive and protects iron.
Electrolysis of brine produces chlorine, hydrogen and —
- oxygen only
- sodium hydroxide
- sodium carbonate
- calcium oxide
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Answer: (b) sodium hydroxide. Chlor-alkali process.
Pure water is a poor conductor because it has —
- free electrons
- metal atoms
- too many ions
- very few ions
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Answer: (d) very few ions. Conduction needs ions.
More topics in this chapter
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