Electrochemistry

Electrochemistry: electron transfer, redox reactions, cells, and real-world applications — concise and student-friendly. Introduction to Electrochemistry

Introduction

Electrochemistry studies the relationship between electrical energy and chemical change, focusing on electron transfer events (redox) and how they generate or consume electrical energy.

Fundamental Concepts

• Oxidation: Loss of electrons by a species.
• Reduction: Gain of electrons by a species.
• Redox reactions: Reactions involving electron transfer; one species is oxidized while another is reduced.

Importance of Electrochemistry

Electrochemistry underpins many technologies and industrial processes:

• Batteries & Fuel Cells: Convert chemical energy to electrical energy for devices and vehicles.
• Electroplating: Deposition of a thin metal layer using electrical current.
• Corrosion Prevention: Understanding and mitigating metal degradation.
• Industrial Electrolysis: Extraction and manufacture of important chemicals (e.g., chlorine, NaOH).

Electrochemical Cells

Two main classifications:

• Galvanic (Voltaic) Cells: Produce electrical energy from spontaneous redox reactions (examples: Daniell cell, lead–acid battery).
• Electrolytic Cells: Use electrical energy to drive non-spontaneous reactions (examples: electrolysis, electroplating).

Quiz: Introduction to Electrochemistry

1. What is electrochemistry?
2. Define oxidation and reduction.
3. What type of reaction involves transfer of electrons?
4. Name two common applications of electrochemistry.
5. What is the difference between galvanic and electrolytic cells?

Answers and Explanation

1. Electrochemistry studies the relationship between electrical energy and chemical changes involving electron transfer.
2. Oxidation is loss of electrons; reduction is gain of electrons.
3. Redox (oxidation–reduction) reactions involve electron transfer.
4. Examples: batteries and electroplating.
5. Galvanic cells generate electricity spontaneously; electrolytic cells consume electricity to drive reactions.

Multiple Choice Questions (MCQs)

1. Which term describes loss of electrons?
   a) Reduction   b) Oxidation   c) Ionization   d) Neutralization
2. Which device converts chemical energy into electrical energy?
   a) Battery (galvanic cell)   b) Electrolyzer   c) Distillation column   d) Furnace
3. Electroplating is performed in a:
   a) Galvanic cell   b) Electrolytic cell   c) Fuel cell   d) None

MCQ Answers

1. b) Oxidation
2. a) Battery (galvanic cell)
3. b) Electrolytic cell

FAQ

Q: Why is electrochemistry important?

It powers technologies (batteries, fuel cells), enables industrial processes (electrolysis), and helps prevent corrosion — critical to modern life and industry.Q: Are galvanic and electrolytic cells related?

Yes. Both involve redox reactions; whether a cell is galvanic or electrolytic depends on spontaneity and whether external energy is supplied.

• Electrochemistry — Wikipedia

Galvanic Cells (Daniell Cell), Electrolysis.