1. Activity
At your tables, use whatever you have in your backpacks to make model of an electrochemical cell
Be able to explain to another group what each object represents in the “electrochemical cell” and what it does in the “cell”
You have 3 minutes

2. We will go through steps to follow and examples
Electrochemistry: Basic Concepts
Sometimes, you must find a balanced reaction of cells from only reduction half-reactions.
We will go through steps to follow and examples

3. Electrochemistry: Basic Concepts
Equations of Cells
Standard Reduction Potentials: lists which are more likely to reduce (take electrons)
reduced
Cu2+ + 2e- → Cu
Cu2+ | Cu
When comparing standard reduction potentials in a cell, the ½ reaction that is…
more (+) is reduction
more (-) is oxidation

4. So… which is more likely to reduce? Li+|Li or Be2+|Ba
Electrochemistry: Basic Concepts
Equations of Cells
So… which is more likely to reduce?
Li+|Li or Be2+|Ba
Ga3+|Ga or Cr2+|Cr
Cr3+|Cr2+ or Cr2+|Cr
Cl2|2Cl- or Cu+|Cu
Ag+|Ag or Rb+|Rb
Mn2+|Me or Au+|Au

5. To write equations of Cells
1) Identify which reaction is oxidation and which is reduction, 2) write the balanced equation
Ag+(aq) + e- → Ag(s)
Ni2+ + 2e- → Ni(s)
EºAg+|Ag = V
EºNi2+|Ni = V
reduction
oxidation
Ni(s) → Ni2+ + 2e- 2
Ag+(aq) + e- → Ag(s) 2 2
Ni(s) + 2Ag+(aq) → Ni2+ + 2Ag(s)

6. Magnesium in a solution of Mg2+ Lead in a solution of Pb2+
Electrochemistry: Basic Concepts
1) Identify which reaction is oxidation and which is reduction, 2) write the balanced equation
Magnesium in a solution of Mg2+
Lead in a solution of Pb2+
Mg2+(aq) + 2e- → Mg(s)
Pb2+(aq) + 2e- → Pb(s)

7. Mg(s) + Pb2+ → Mg2+(aq) + Pb(s)
Electrochemistry: Basic Concepts
1) Identify which reaction is oxidation and which is reduction, 2) write the balanced equation
Mg2+(aq) + 2e- → Mg(s)
Pb2+(aq) + 2e- → Pb(s)
EºMg2+|Mg = V
EºPb2+|Pb = V ox
red
Mg(s) → Mg2+(aq) + 2e-
Pb2+(aq) + 2e- → Pb(s)
Mg(s) + Pb2+ → Mg2+(aq) + Pb(s)