1. Electroanalytical techniques
1.1. Control voltage
1.1.1. Voltammetry
1.1.1.1. Cyclic
1.1.1.2. AC
1.1.1.3. Micro-electrode
1.1.2. Constant potential
1.1.2.1. Coulometry
1.1.2.2. Chronoamperometry (i-t)
1.2. Control current
1.2.1. i=0
1.2.1.1. Potentiometry
1.2.2. i#0
1.2.2.1. Controlled-current coulometry
2. Junction potential
2.1. Type 1
2.2. Type 2
3. Voltammetry
3.1. Charging current
3.2. Faradaic current
3.3. Movement methods
3.3.1. Mass transfer
3.3.2. Diffusion
3.3.3. Convection
3.3.4. Migration of charged molecules
4. Electrochemistry
4.1. Reduction
4.1.1. Cu2+ + 2e- ⇋ Cu
4.2. Oxidation
4.2.1. Zn ⇋ Zn2+ + 2e
4.3. Redox reaction
4.3.1. Galvanic cells
4.3.1.1. Spontaneous: Ecell>0 & dG<0
4.3.2. Electrolytic cells
4.3.2.1. Non-spontaneous; dG>0; Ecell<0
4.3.3. Ecell
4.3.3.1. Ecell=Ecathode−Eanode
4.3.4. Cell notation
4.3.4.1. Co(s)∣Co2+(aq,1M)∥Cu2+(aq,1M)∣Cu(s)
4.3.5. Half cell reactions
4.3.5.1. Zn+2H+→Zn2++H2
5. Electrodes
5.1. Reference electrode
5.1.1. The electrode against which potential of the working electrode is measured/applied
5.1.1.1. Ideal polarizable->well defined i/ behaves like a capacitor
5.1.1.2. Ideal non-polarizable-> different i/no change in pot.
5.1.2. Common Ref. electrodes
5.1.2.1. SCE
5.1.2.2. Ag/AgCl/KCl
5.1.2.3. Hg/HgSO4/K2SO4
5.2. Working electrode
5.2.1. Second kind/Ag/AgCl(s)/ metal electrode responds to other species/anion.
5.2.2. Membrane electrodes-pH, Na, Ca
5.2.2.1. Liquid/polymer/glass membrane
5.2.3. Inert metal electrode
5.2.4. Inactive (C/Pt) vs Active (metal)
5.2.5. First kind/ pure metal electrode/obey Nerst eqtn
5.2.6. Third kind->responds to another competitive reaction i.e. a cation
5.3. Charge type
5.3.1. Anode
5.3.1.1. Oxidation
5.3.2. Cathode
5.3.2.1. Reduction
5.4. Ion Selective electrode
5.5. 2-electrode system
5.5.1. Working/Reference/Counter electrode
5.6. 3-electrode system
5.6.1. Working/Reference electrode