2. What is Corrosion?
Corrosion is the oxidation of a metal due to an
ELECTROCHEMICAL reaction. The oxidizing agent is
most often O2 (atmospheric corrosion) or H+
(chemical
corrosion) or both.
Why is it a problem?
Financial - $350 Billion Dollar Annual Problem in U.S.
(4.25% of GNP) Department of Defense spends $6 –
8 Billion
3. Recipe for corrosion
Active metal
Water
Oxygen
(atmospheric corrosion)
Acid
(chemical corrosion)
Salt
High temperature
4. Chemical vs. Atmospheric Corrosion
(H+
vs. O2)
Anodic Reaction:
Fe0
(s) Fe2+
(aq) + 2e-
Deterioration of metal
Cathodic Reaction:
2H+
(aq) + 2e-
H2 (g) Chemical
O2 (g) + 2H2O (l) + 4e-
4OH-
(aq) Atmospheric
O2 (g) + 4H+
(aq) + 4e-
2H2O (l) Combination
Which of these will oxidize copper? Silver? Gold?
Overall Reaction:
Fe0
(s) + 2H+
(aq) Fe2+
(aq) + H2 (g) Chemical
2Fe0
(s) + O2 (g) + 2H2O (l) 2Fe2+
(aq) + 4OH-
(aq) Atmospheric
2Fe0
(s) + O2 (g) + 4H+
(aq) 2Fe2+
(aq) + 2H2O (l) Combination
Eo
red (V)
Eo
cell (V)
-0.44
0.00
+0.40
+1.23
+1.67
+0.84
+0.44
Cu(s) Cu2+
(aq) + 2e- +0.34Ag(s) Ag+
(aq) + e-
+0.80Au(s) Au3+
(aq) + 3e- +1.50
5. Why won’t iron corrode in pure (degassed) water?
Anodic Reaction:
Fe0
(s) Fe2+
(aq) + 2e-
Cathodic Reaction:
Eo
(V)
-0.44
-0.83
Fe0
(s) + 2H2O (l) Fe2+
(aq) + H2 (g) + 2OH-
(aq)
Eo
cell (V)
-0.39
What metals will corrode in pure (degassed) water?
Any sufficiently active metal Eo
red < -0.83 V
(alkali metals, alkaline earth metals, aluminum, manganese)
Overall reaction:
2H2O (l) + 2e-
H2 (g) + 2OH-
(aq)
6. Example of Atmospheric Corrosion
Corrosion on wing of Navy aircraft
Why does corrosion of an airplane
occur primarily while the plane is on
the ground?
How might this corrosion be
minimized?
F/A-18C Hornet
7. Example of Chemical Corrosion
Nuclear Reactor Vessel Head Degradation
• February 16, 2002, Davis-Besse Nuclear Power Station in Oak Harbor, Ohio
Boric Acid leak from control rod
drive mechanism led to chemical
corrosion of reactor vessel head
Serious potential for loss of
reactor coolant access
8. Corrosion of a Ship’s Hull
Anodic and Cathodic Regions
O2
O2 + 2H2O + 4e-
4OH-
OH-
Fe2+
Fe2+
+ 2OH-
Fe(OH)2
4Fe(OH)2 + O2 2(Fe2O3·H2O) + 2H2O
Fe Fe2+
+ 2e-
Hull of ship
Cathodic Region
RUST
Anodic Region
Electrons Migrate from
Anodic to Cathodic Region
e-
9. STRESS CORROSION
Nail is embedded in a gel.
Gel contains phenolphthalein
and ferricyanide ion.
Phenolphthalein turns pink in
basic solution.
Ferricyanide reacts with Fe2+
to produce a blue color.
2Fe0
(s) + O2 (g) + 2H2O (l) → 2Fe2+
(aq) + 4OH-
(aq)
anode
cathode
13. Preventing the Corrosion of IronPreventing the Corrosion of Iron
(cathodic protection/sacrificial anode)(cathodic protection/sacrificial anode)
Sacrificial anode
14. Applications of Cathodic Protection
• Galvanized Steel
Zinc coating
• Sacrificial Anodes
Ship Hulls
Subs (free flooding areas)
Los Angeles Class Sub
Arleigh-Burke Destroyer
18. There are some leaks in Sampson Hall. Upon
inspection it turns out that copper (Cu) was attached to
lead (Pb) on the roof. I guess it turns out when they
are mixed with water (H2O) or air (N2, O2, CO2, etc) there
is some kind of reaction that breaks down the
properties of the copper and lead.
Hinweis der Redaktion
OK to have attention grabbers at the beginning.
But they can be distracting if used too much. Poor contrast here. I changed font sizes and size of picture
Contrast. What exactly is shown in the pictures? Too wordy.
The gel has been prepared with a little phenolphthalein indicator and a little potassium ferricyanide mixed in. As corrosion occurs, the hydroxide ion produced in the cathodic region turns the phenolphthalein pink while the ferrous and ferric ions produced in the anodic region react with the ferricyanide to make Prussian blue (the deep blue color appears almost black on the photographs).