1. Electrolytic Cell Involves non spontaneous redox reactions
Use external power supply to drive the redox reaction (like a battery or plug into wall)
Amount of E needed to drive the reaction depends on the half reactions that make up the cell
Eocell will be negative
Ex. include electroplating and electrolysis of molten salts to the M (s)
2 NaCl (molten) → 2 Na (s) + Cl2 (g)

2. Electrolytic Cell, Parts
Same as galvanic, still have
Electrolytes
Electrodes (cathode and anode)
Salt bridge
Still have AutO and CaR
Anode gets oxidized
Cathode gets reduced

3. How does it work?
Have to put energy into an electrolytic cell to drive the redox rxn (non spont)
Need to connect it to an external power supply (like a battery/galvanic cell)
The - end of battery (anode) hooks to cathode in EC
The + end of battery (cathode) hooks to anode in EC

4. Electrolysis of Water Zap H2O to decompose it to elements
2 H2O → 2 H2 + O2
Who is oxidized? Who is reduced?
Write balanced half reactions.
(note: H2 half reaction is basic, O2 is acidic)

5. Electrolysis of Water Yellow = Acidic 2 H2O → O2 + 4 H+ + 4 e-
Blue = Basic
2 H2O + 2 e- → H2 + 2 OH-

6. Electrolysis of Molten Salts
Process to extract free metal from ores (salts)
Zap molten solution of ore with energy, and get elements
Molten salt is like an aqueous solution, the ions are separated
Ex. Electrolysis of Molten NaCl
Na+ + Cl- → Na + Cl2
Who is oxidized? Reduced?
Write half reactions and NIE.
Draw a pic of cell.
Calc Eocell. Does sign make sense? Interpret in words.
Na/Na+ = V
Cl2/Cl- = 1.36 V

7. Metal in Ore Gets Reduced Nonmetal Gets Oxidized
If you have a mixture of salts like KCl and NaCl, which metal will get reduced first?
Na+ + e- → Na Eo = V
K+ + e- → K Eo = V
Which anion would get oxidized more easily?

8. Quantitative Aspect of Electrolysis
See sheet