Study Sheet for Chapter 13
Table J
Before:
Na 2-8-1
Cl 2-8-7

(oxidation)
(reduction)

e- 
After:
Na2+
2-8
Cl- 2-8-8
“LEO the lion says, ‘GER’ “
Metals
Li
Li wants to
oxidize the
most – best
reducing
agent
Metal A
Metal A –
oxidizes
Metal B+ –
reduces
Metal B
Nonmetals
F2 – Wants
to reduce
the most
Lose Electrons Oxidation
Gain Electrons Reduction
Au
Au+3 – best
oxidizing
agent
Voltaic Cell (Electrochemical cell)
Zn  Zn2+ + 2eOxidation – Anode
Negative electrode
Electrolytic Cell (Plating)
Ag+ + e-  Ag
( at spoon)
Reduction – Cathode
Negative electrode
What is oxidation?
What is reduction?
If you lose an electron what is the resulting charge on the
ion?
How are redox reactions identified?
How do you find the oxidation number for elements in a
compound?
Which metal oxidizes?
Which type of cell creates electricity?
Where does oxidation take place?
Where does reduction take place?
What does the salt bridge do?
Which direction do electrons flow?
In an electrochemical cell, what happens to the mass of
the anode?
In an electrochemical cell, what happens to the mass of
the cathode?
Which type of cell requires electricity?
How do you balance an equation using redox?
Lose electrons oxidation (LEO).
Gain electron reduction (GER).
+1
Oxidation numbers on an element will change from the
left to the right side of the equation.
They can be taken off the periodic table. If there is
more than one oxidation number you chose the
oxidation state that causes the charge on the
compound to add to zero.
The one higher on table J.
Electrochemical (or Voltaic) cell.
Anode (vowels).
Cathode (consonants).
Allows ions to move.
From the more active metal through the wire to the less
active metal.
It gets smaller because atoms are being converted to
ions.
It gets greater because ions are being converted to
atoms.
Electrolytic cell.
Write half reactions and then balance the electrons to
find the coefficients.
Oxidation
__________________________________________________________________
Corrode/Corrosion
__________________________________________________________________
Reduction
__________________________________________________________________
Redox or Oxidation-reduction reactions__________________________________________________________
Oxidation number
__________________________________________________________________
Half-reaction
__________________________________________________________________
Species
__________________________________________________________________
Electrochemical cell
__________________________________________________________________
Voltaic cell
__________________________________________________________________
Electrode
__________________________________________________________________
Salt bridge
__________________________________________________________________
Anode
__________________________________________________________________
Cathode
__________________________________________________________________
Spontaneous
__________________________________________________________________
Electrolytic cell
__________________________________________________________________
Electrolysis
__________________________________________________________________
Conservation of charge
__________________________________________________________________
Oxidizing agent
__________________________________________________________________
Reducing agent
__________________________________________________________________