Course Content
Module 1: Foundations of Redox Reactions
Oxidation and Reduction: Understanding redox in terms of oxygen transfer, hydrogen transfer, and electron transfer. Oxidation Numbers: Rules for assigning oxidation states and identifying oxidizing/reducing agents. Balancing Redox Equations: Half-reaction method and oxidation number method.
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Part 1: Defining Oxidation and Reduction
Part 2: Oxidation Numbers
Part 3: Balancing Redox Equations
Practice Questions on Redox Reactions
00:20:00
TEst For Oxidizing And Reducing Agents
Module 2: Electrolysis (The Electrolytic Cell)
Components of Electrolysis: Electrolytes (strong vs. weak), electrodes (inert vs. active), and the electrolytic tank. Preferential Discharge of Ions: Factors affecting the discharge of ions (position in electrochemical series, concentration, and nature of electrodes). Practical Examples: Electrolysis of acidified water, brine, and copper(II) sulfate solution.
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1. Components of an Electrolytic Cell
2. Preferential Discharge of Ions
3. Practical Examples of Electrolysis
Module 3: Quantitative Electrochemistry (Faraday’s Laws)
Module 3: Quantitative Electrochemistry (Faraday’s Laws)Faraday’s First Law: Relationship between mass ($m$), current ($I$), and time ($t$). Formula: $m = zIt$.Faraday’s Second Law: Chemical equivalents and the Faraday constant ($96,500 text{ C mol}^{-1}$).Calculations: Determining mass deposited, volume of gases at STP, and the charge on ions.
Module 4: Electrochemical Cells (Galvanic/Voltaic)
Cell Construction: Half-cells, salt bridges, and external circuits. Standard Electrode Potential (E ∘ ): The Standard Hydrogen Electrode (SHE) and the Electrochemical Series. Cell Notation: Writing and interpreting cell diagrams (e.g., Zn (s)∣Zn(aq)2+ ∣∣Cu (aq)2+ ∣Cu (s)). Electromotive Force (e.m.f.): Calculating E cell ∘ ​ =E cathode ∘ ​ −E anode
Module 5: Industrial Applications & Corrosion
Electroplating and Purification: How electrolysis is used to coat metals and refine copper. Primary and Secondary Cells: Lead-acid accumulators, dry cells (Leclanché), and fuel cells. Corrosion of Metals: The chemistry of rusting and methods of prevention (cathodic protection, galvanizing).
Module 6: Exam Prep (WAEC/NECO/UTME Focus)
Electrochemistry

Part 1: Defining Oxidation and Reduction

The definition of redox has evolved to become more comprehensive. We’ll look at three ways to define it, with the electron transfer definition being the most powerful for electrolysis.

Definition Oxidation Reduction Mnemonic
1. Oxygen Transfer Gain of oxygen Loss of oxygen Oxidation Is Gain (of oxygen)
2. Hydrogen Transfer Loss of hydrogen Gain of hydrogen Reduction Is Gain (of hydrogen)
3. Electron Transfer Loss of electrons Gain of electrons OIL RIG: Oxidation Is Loss, Reduction Is Gain (of electrons)

Why the Electron Transfer Definition is Key for Electrolysis:

In electrolysis, an external power source (like a battery) forces electrons to move.

  • The positive electrode (anode) is connected to the positive terminal of the power source. It attracts anions (negative ions) and pulls electrons away from them. This is where oxidation (loss of electrons) occurs.

  • The negative electrode (cathode) is connected to the negative terminal. It attracts cations (positive ions) and pushes electrons onto them. This is where reduction (gain of electrons) occurs.

 

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