University of Benin CHM212 intermediate

CHM212: Oxidation and reduction reaction

Free study notes for CHM212 (CHM 212) — Oxidation and reduction reaction at University of Benin, one topic at a time, each with worked examples and a practice quiz.

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Course Syllabus

  1. Fundamentals of Oxidation and Reduction
  2. Oxidation Numbers and Redox Systems
  3. Electrochemistry: Galvanic Cells
  4. Electrochemistry: Nernst Equation and Applications
  5. Electrochemistry: Electrolytic Cells and Corrosion

Study Notes

Fundamentals of Oxidation and Reduction

Oxidation and reduction are everywhere in chemistry, from how your body processes food to how batteries produce electricity. You'll often hear them referred to jointly as redox reactions.

The most fundamental way to think about oxidation and reduction is in terms of electron transfer.

  • Oxidation: This is the loss of electrons. When an atom or ion loses electrons, its charge becomes more positive.
  • Reduction: This is the gain of electrons. When an atom or ion gains electrons, its charge becomes more negative.
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Oxidation Numbers and Redox Systems

Redox reactions (short for reduction-oxidation) are fundamental chemical processes involving the transfer of electrons. Understanding them hinges on correctly assigning oxidation numbers (also called oxidation states).

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Electrochemistry: Galvanic Cells

The key components of a galvanic cell are:
* Anode: The electrode where oxidation occurs. It's negatively charged because it's the source of electrons.
* Cathode: The electrode where reduction occurs. It's positively charged because it accepts electrons.
* Electrolyte: An ion-conducting solution in each half-cell where the electrodes are immersed.
* External Circuit (Wire): Connects the anode and cathode, allowing electrons to flow from the anode to the cathode.
* Salt Bridge: A U-shaped tube containing an inert electrolyte (like KNO₃ or NaCl). It connects the two half-cells, allowing ions to migrate to maintain electrical neutrality and complete the circuit. Without it, charge would build up, and the reaction would stop.

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Electrochemistry: Nernst Equation and Applications

You already know that standard cell potentials (E°) are measured under specific conditions: 1 M concentration for solutions, 1 atm pressure for gases, and 25 °C. But what happens when these conditions aren't met? That's where the Nernst Equation comes in.

It allows you to calculate the non-standard cell potential (E) using the standard cell potential (E°) and accounting for changes in concentration (or partial pressures for gases) and temperature.

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CHM212: common questions

What does CHM212 cover?

This CHM212 study guide covers 5 topics: Fundamentals of Oxidation and Reduction, Oxidation Numbers and Redox Systems, Electrochemistry: Galvanic Cells, Electrochemistry: Nernst Equation and Applications, Electrochemistry: Electrolytic Cells and Corrosion.

Are these CHM212 notes free?

Yes. Every CHM212 note on this page is free to read without an account. A free account adds practice quizzes, flashcards and a revision plan.

How do I revise for my CHM212 exam?

Read the CHM212 note for each topic, then take its practice quiz: the questions you get wrong come back as flashcards until you know them. Save the course to get a revision plan built around your exam date.