Introduction to Electrochemistry
Electrochemistry is the branch of chemistry that studies the
relationship between electricity and chemical
reactions. It involves the study of redox (oxidation-reduction)
reactions where electrons are transferred between
species.
Key Concepts:
1. Oxidation and Reduction:
- Oxidation: Loss of electrons.
- Reduction: Gain of electrons.
- These processes occur simultaneously in a redox reaction.
2. Electrochemical Cells: Devices that convert chemical energy into
electrical energy or vice versa.
- Galvanic (Voltaic) Cells: Generate electrical energy from
spontaneous redox reactions (e.g., batteries).
- Electrolytic Cells: Use electrical energy to drive non-spontaneous
chemical reactions (e.g., electrolysis).
3. Electrode Types:
- Anode: The electrode where oxidation occurs.
- Cathode: The electrode where reduction occurs.
4. Cell Potential (Electromotive Force, EMF): A measure of the driving
Electrochemistry is the branch of chemistry that studies the
relationship between electricity and chemical
reactions. It involves the study of redox (oxidation-reduction)
reactions where electrons are transferred between
species.
Key Concepts:
1. Oxidation and Reduction:
- Oxidation: Loss of electrons.
- Reduction: Gain of electrons.
- These processes occur simultaneously in a redox reaction.
2. Electrochemical Cells: Devices that convert chemical energy into
electrical energy or vice versa.
- Galvanic (Voltaic) Cells: Generate electrical energy from
spontaneous redox reactions (e.g., batteries).
- Electrolytic Cells: Use electrical energy to drive non-spontaneous
chemical reactions (e.g., electrolysis).
3. Electrode Types:
- Anode: The electrode where oxidation occurs.
- Cathode: The electrode where reduction occurs.
4. Cell Potential (Electromotive Force, EMF): A measure of the driving
