1. Standard Cell Notation (line notation)
Conventions:
Anode on Left
Single line : represent phase boundaries
Two line : represent liquid junction
Cu2+ V
NO3-
Zn2+ Cu Zn e-
Anode / anode solution // cathode solution / Cathode
Example: Zn / Zn2+ (1.0 M) // Cu2+ (1.0M) / Cu

2. Line Notation solid½Aqueous½½Aqueous½solid
Anode on the left½½Cathode on the right
Single line different phases.
Double line porous disk or salt bridge.
If all the substances on one side are aqueous, a platinum electrode is indicated.

3. For the last reaction Cu(s)½Cu+2(aq)½½Fe+2(aq),Fe+3(aq)½Pt(s)

4. Oxidation
Reduction

7. Copyright McGraw-Hill 2009

8. Practice:
In a galvanic cell, the electrode that acts as a source of electrons to the solution is called the __________; the chemical change that occurs at this electrode is called________.  
a.  cathode, oxidation  
b.  anode, reduction  
c.  anode, oxidation  
d.  cathode, reduction

9. Practice
Under standard conditions, which of the following is the net reaction that occurs in the cell?
Cd|Cd2+ || Cu2+|Cu  
a.  Cu2+ + Cd → Cu + Cd2+  
b.  Cu + Cd → Cu2+ + Cd2+  
c.  Cu2+ + Cd2+ → Cu + Cd  
d.  Cu + Cd 2+ → Cd + Cu2+ 

10. Galvanic Cell
The reaction always runs spontaneously in the direction that produced a positive cell potential.
Four things for a complete description.
Cell Potential
Direction of flow
Designation of anode and cathode
Nature of all the components- electrodes and ions

11. Oxidation Numbers on the Periodic Table

12. Cell Potential Cell Potential / Electromotive Force (EMF):
The “pull” or driving force on electrons
Measured voltage (potential difference)
The total cell potential is the sum of the potential at each electrode.

13. Ecell = V

14. Cell Potential, E0cell E0cell cell potential under standard conditions
elements in standard states (298 K)
solutions: 1 M
gases: 1 atm

15. Practice
Completely describe the galvanic cell based on the following half-reactions under standard conditions.
MnO H+ +5e- ® Mn+2 + 4H2O Eº=1.51 V
Fe+3 +3e- ® Fe(s) Eº=0.036V