1. Basic Concepts of Electrochemical Cells
Electrifying!
Anode
Cathode

2. CHEMICAL CHANGE ---> ELECTRIC CURRENT
With time, Cu plates out onto Zn metal strip, and Zn strip “disappears.”
Zn is oxidized and is the reducing agent Zn(s) ---> Zn2+(aq) + 2e-
Cu2+ is reduced and is the oxidizing agent Cu2+(aq) + 2e- ---> Cu(s)

3. CHEMICAL CHANGE ---> ELECTRIC CURRENT
Electrons are transferred from Zn to Cu2+, but there is no useful electric current.
Oxidation: Zn(s) ---> Zn2+(aq) + 2e-
Reduction: Cu2+(aq) + 2e- ---> Cu(s)
Cu2+(aq) + Zn(s) ---> Zn2+(aq) + Cu(s)

4. CHEMICAL CHANGE ---> ELECTRIC CURRENT
To obtain a useful current, we separate the oxidizing and reducing agents so that electron transfer occurs thru an external wire.
This is accomplished in a GALVANIC or VOLTAIC cell.
A group of such cells is called a battery.

5. Zn --> Zn2+ + 2e-
Cu2+ + 2e- --> Cu
Oxidation
Anode
Negative
Reduction
Cathode
Positive
<--Anions
Cations-->
•Electrons travel thru external wire.
Salt bridge allows anions and cations to move between electrode compartments.

6. The Cu|Cu2+ and Ag|Ag+ Cell
Electrons move from anode to cathode in the wire.
Anions & cations move thru the salt bridge.

7. Anode, site of oxidation,
negative
Cathode, site of reduction, positive

8. CELL POTENTIAL, E
1.10 V
1.0 M
Zn and Zn2+,
anode
Cu and Cu2+,
cathode
Electrons are “driven” from anode to cathode by an electromotive force or emf.
For Zn/Cu cell, this is indicated by a voltage of 1.10 V at 25 ˚C and when [Zn2+] and [Cu2+] = 1.0 M.

9. CELL POTENTIAL, E
For Zn/Cu cell, potential is V at 25 ˚C and when [Zn2+] and [Cu2+] = 1.0 M.
This is the STANDARD CELL POTENTIAL, Eo
—a quantitative measure of the tendency of reactants to proceed to products when all are in their standard states at 25 ˚C.
This means pure solids or in solution at a concentration of 1M!!!!

10. Calculating Cell Voltage
Balanced half-reactions can be added together to get overall, balanced equation.
Zn(s) ---> Zn2+(aq) + 2e-
Cu2+(aq) + 2e- ---> Cu(s)
Cu2+(aq) + Zn(s) ---> Zn2+(aq) + Cu(s)
If we know Eo for each half-reaction, we could get Eo for net reaction.
Lets revisit my haiku!

11. Oxidation Haiku!
Lost an electron
But now feeling positive
Oxidized is cool!
What is that? You want a reduction Haiku?

12. Reduction Haiku!!! Gained some electrons Gave me a negative mood!
Now I can say Ger!
Thank you… Enjoy the buffet… Don’t eat the chemicals or furniture kids!

13. 2 H+(aq, 1 M) + 2e- <----> H2(g, 1 atm)
CELL POTENTIALS, Eo
Can’t measure 1/2 reaction Eo directly. Therefore, measure it relative to a STANDARD HYDROGEN CELL, SHE.
2 H+(aq, 1 M) e- <----> H2(g, 1 atm)
Eo = 0.0 V

14. Supplier of electrons Acceptor of electrons
Zn/Zn2+ half-cell hooked to a SHE.
Eo for the cell = V
Negative electrode
Positive electrode
Supplier of electrons
Acceptor of electrons
Zn --> Zn2+ + 2e-
Oxidation
Anode
2 H+ + 2e- --> H2
Reduction
Cathode

15. Reduction of H+ by Zn
Figure 20.10

16. Overall reaction is reduction of H+ by Zn metal.
Zn(s) + 2 H+ (aq) --> Zn2+ + H2(g) Eo = V
Therefore, Eo for Zn ---> Zn2+ (aq) + 2e- is V
Zn is a (better) (poorer) reducing agent than H2.

17. Cu/Cu2+ and H2/H+ Cell Eo = +0.34 V Positive Negative
Acceptor of electrons
Supplier of electrons
Cu2+ + 2e- --> Cu
Reduction
Cathode
H2 --> 2 H+ + 2e-
Oxidation
Anode

18. Cu/Cu2+ and H2/H+ Cell
Overall reaction is reduction of Cu2+ by H2 gas.
Cu2+ (aq) + H2(g) ---> Cu(s) H+(aq)
Measured Eo = V
Therefore, Eo for Cu e- ---> Cu is
+0.34 V

19. Zn/Cu Electrochemical Cell+
Anode, negative, source of electrons
Cathode, positive, sink for electrons
Zn(s) ---> Zn2+(aq) + 2e- Eo = V
Cu2+(aq) + 2e- ---> Cu(s) Eo = V
Cu2+(aq) + Zn(s) ---> Zn2+(aq) + Cu(s)
Eo (calc’d) = V

20. Yes It is finally time for a DEMO!!
Do you feel like bridging that salt?

21. TABLE OF STANDARD REDUCTION POTENTIALS
oxidizing
ability of ion E o
(V) Cu 2+
+ 2e Cu
+0.34
2 H +
+ 2e H
0.00 Zn
+ 2e Zn
-0.76
reducing ability
of element 2

22. Potential Ladder for Reduction Half-Reactions
Figure 20.11

23. Table 21.1 Page 970

24. Standard Redox Potentials, EoCu 2+
+ 2e Cu
+0.34 +
2 H
+ 2e H 2
0.00 Zn
+ 2e Zn
-0.76
Any substance on the right will reduce any substance higher than it on the left.
Northwest-southeast rule: product-favored reactions occur between reducing agent at southeast corner (anode) and oxidizing agent at northwest corner (cathode).

25. Standard Redox Potentials, Eo
Any substance on the right will reduce any substance higher than it on the left.
Zn can reduce H+ and Cu2+.
H2 can reduce Cu2+ but not Zn2+
Cu cannot reduce H+ or Zn2+.

26. Using Standard Potentials, Eo Table 20.1
In which direction do the following reactions go?
Cu(s) Ag+(aq) ---> Cu2+(aq) Ag(s)
2 Fe2+(aq) + Sn2+(aq) ---> 2 Fe3+(aq) + Sn(s)
What is Eonet for the overall reaction?

27. Standard Redox Potentials, Eo
E˚net = “distance” from “top” half-reaction (cathode) to “bottom” half-reaction (anode)
E˚net = E˚cathode - E˚anode
Eonet for Cu/Ag+ reaction = V

28. All ingredients are present. Which way does reaction proceed?
Eo for a Voltaic Cell
Cd --> Cd2+ + 2e- or
Cd2+ + 2e- --> Cd
Fe --> Fe2+ + 2e- or
Fe2+ + 2e- --> Fe
All ingredients are present. Which way does reaction proceed?

29. Eo for a Voltaic Cell From the table, you see
• Fe is a better reducing agent than Cd
• Cd2+ is a better oxidizing agent than Fe2+
Overall reaction
Fe + Cd > Cd + Fe2+
Eo = E˚cathode - E˚anode
= (-0.40 V) - (-0.44 V)
= V

30. More About Calculating Cell Voltage
Assume I- ion can reduce water.
2 H2O e- ---> H OH Cathode
2 I > I e Anode
2 I H2O --> I OH H2
Assuming reaction occurs as written,
E˚net = E˚cathode - E˚anode
= ( V) - ( V) = V
Minus E˚ means rxn. occurs in opposite direction

31. If you have reached this far, you need a break!