1. Working Electrode
1.1. Active Electrode
1.1.1. Metals
1.2. Inactive Electrode
1.2.1. Carbon
1.2.2. Platinum
1.3. As a Cathode
1.3.1. Species reduced
1.4. An a Anode
1.4.1. Species oxidized
2. Reference Electrode
2.1. Ideal
2.1.1. Well-defined Invariant Potential
2.1.2. Zero impedance
2.1.3. No leaking to solution
2.2. Common Types
2.2.1. Saturated Calomel Electrode (SCE)
2.2.2. Silver-Silver Chloride Electrode (Ag/AgCl)
2.2.3. Mercury-Mercurous Sulfate Electrode (Hg/Hg2SO4)
2.3. Finding Potential (Steps)
2.3.1. Half cell reaction
2.3.2. Nernst reaction
2.3.2.1. Ksp for the solution
3. Half Cells
3.1. Redox reactions
3.2. Cell notation
3.3. E cell
3.3.1. Good oxidizing agent
3.3.2. Good reducing agent
3.3.3. Activity Coefficient
3.3.3.1. Nernst Equation
4. Types of Cells
4.1. Galvanic cell
4.1.1. Electrical energy
4.1.2. Spontaneous
4.2. Electrolytic cell
4.2.1. Electrical energy
4.2.2. Non-spontaneous
5. Electrodes
5.1. Ideal Polarizable Electrode
5.1.1. Charge accumulates directly on electrode
5.1.2. Behaves like a capacitor
5.2. Ideal Non-polarizable Electrode
5.2.1. Charge can leak out of electrode
5.3. Real Voltametric Cells
5.3.1. Polarizable working electrode
5.3.2. Non-polarizable reference electrode
5.4. Applied Voltage
5.4.1. One electrode as working, a second as reference
5.4.2. Potential of both electrodes change, not usually symmetrically
5.4.3. Solution is to use an ideal reference electrode where potential does not change