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Chapter 7 Electrochemistry
§7.13 Corrosion and protection of metals
1) Corrosion:
Destruction of materials due to the chemical, electrochemical and physical attack of the media.
Railway bridge in Boston
White marble of Jinshui Bridge, Beijing
Stone Sculpture before the Capitol, Washington D.C.
1. General introduction
One-fifth of the iron and steel produced annually in the world is used to replace rusted metal.
Since corroded metal often loses its structural integrity and attractiveness, corrosion of metal probably results in disaster and has great impact on national economics and safety.
Brass sculpture before the Capitol, Washington D.C. Brooklyn Bridge,
New York
Warship of Pacific Fleet, Russia
2) Why does metal undergo corrosion?
Only few elements exist in free element state in natural circumstance. Corrosion of metal, i.e. conversion of element to stable compound, is thermodynamically favored.
Naturally occurring copper single crystals, Museum of Natural Sci., Washington, D.C. USA
Naturally occurring copper sheet
Naturally occurring gold
2. Classification of corrosion
1) Based on materials:
Corrosion of metals; Corrosion of non-metals (wood, plastic, concrete, stone, etc.)
2) Based on Media:
natural corrosion; industrial corrosion (with surface solution containing acid, base, H2S, etc.)
3) Based on mechanism:
chemical corrosion (2Fe + O2 = 2FeO);
electrochemical corrosion; biochemical corrosion
4) Based on uniformity:
general corrosion; local corrosion
5) Other kinds:tension corrosion; contact corrosion;
friction corrosion; external current corrosion;
Concussion corrosion
3. local corrosion
Local corrosion is initiated du
e to the ununiformity of metal a
nd / or solution.
1) The ununiformity of metal:
2) The ununiformity of metal surface
3) The ununiformity of solution
(1) multiphase texture;
(2) crystal boundary;
(3) crystal facet;
(4) impurities;
(5) enrichment;
(6) tension and deformity
1) The ununiformity of metal:
Corrosion of crystal boundary
intergranular corrosion
Trans-crystal corrosion
transgranular corrosion
(1) multiphase texture (2) crystal boundary;
Crystal plane (111) (100) (110) (120)
Relative corrosion rate 1 0.9 0.55 0.32
(3) crystal facet;
(4) impurities; (5) enrichment;
Fe
Fe = Fe2+ + 2e
Fe2+
Fe2+
Fe2+OH
Cl
Cl
ClCl
Fe2+
Impurity
O2
O2 + 2H2O + 4e 4OH
Mechanism of Pitting corrosionpH can
attain 3.5 ~ 4
Tension corrosion
Anodic region
Cathodic region
Reactions:
Anodic reaction: Fe Fe2++2e¯
Cathodic reaction: 2H2O + 2e¯ H2+2OH ¯
Nails in a solution with phenolphthalein and K3[Fe(CN)6]
(6) tension and deformity
Where is anodic region and cathodic region?
These two beakers contain 1.0 mol·dm-3 Cu(NO3)2 solutions, a
copper electrode, and a salt bridge. If the two copper
electrodes were connected together, would a current flow
between them?
3) The ununiformity of solution
(1) Concentration difference of metal ions;
(2) Concentration difference of media ions;
(3) Accumulation of H+ in pit or cracks;
(4) Concentration difference of dissolved oxygen
2) The ununiformity of metal surface
(1) Smoothness of the surface;
(2) Micropore in protective layer;
(3) Corrosion products
Different aeration corrosion
Waterline corrosion
Crack corrosion
(4) Concentration difference of
dissolved oxygen
O2
O2
O2
O2O2
Where does corrosion take place and
where does rust form?
4 Theoretical consideration of electrochemical corrosion
Zn + 2 HCl ZnCl2 + H2
Why does Zn of 99.5 % purity dissolve in dilute HCl in 1 min,
while that of 99.999% purity does not dissolve even after 8 h?
anode reaction:
Zn Zn2+ + 2e
Cathode reaction:
2H+ + 2e H2 Conjugation reaction
2H+ + 2e H2
H2 2H+ + 2e
Zn Zn2+ + 2e
Zn2+ + 2e Zn
re Zn2+/Zn
re H+/H2
lg jcorr
/ V
lg j
corr
Conjugation reaction
Corrosion current
Corrosion / stable /
mixed potential
re Zn2+/Zn
re H+/H2
2H+ + 2e H2
H2 2H+ + 2e
Zn Zn2+ + 2e
Zn2+ + 2e Zn
lg jcorr
/ V
lg j
corr
Positive shift of the metal or increase of the hydrogen evo-lution overpotential can both hinder the corrosion of the metal.
Copper wire Why does copper wire accelerate corrosion of iron nail?
metal a
Fe 0.7
Cu 0.87
value of a in Tafel equation
5. Corrosion protection
1) Application of coatings: (1) metal coating:
electroplating, chemical plating
Zn (anodic protective layer)
Sn (cathodic protective layer)
(2) non-metal coating:
paint (polymer coating); anticorrosion oil; porcelain enamel; plastic; glass (packaging of IC); inherent oxide layer, etc.
Coating forms a barrier layer to inhibit corrosive species from reaching metal surface.
coating
Corrosive species
metal
Both thick inorganic coating and organic coating were applied to protect the cable and steel structure of Brooklyn Bridge, New York, USA.
When Al contacting with the air, a thin inherent layer of aluminum oxide forms on its surface. Being stable in the air, water and even some dilute acidic solution, this thin oxide layer inhibits further corrosion of the metal. With potential of naked aluminum of – 0.6 V, the oxide-coated aluminum becomes more stable even than the common metals, such as iron, zinc, etc.
2) Alloying
Stainless steel:
containing chromium and nickel, both of which form inherent oxide film that change steel’s reduction potential.
To be stainless steel, the chromium content needs to be at
least 10.5%.
The corrosion rate of stainless steel at general corrosion
may be as low as 1 cm for 106 years.
3) Electrochemical protection
Let the potential of iron kept at the stable zone of iron.
Cathodic protection:
with sacrificial anode
with auxiliary anode
Anodic protection:
set the metal at stale zone of Fe3O4. passivation potential
Fe2+
Fe2O3
Fe
pH
/ V
2 4 6 8 10 12 140
Fe3O4
Fe3+
FeO22
Cathodic protection: with sacrificial anode
magnesium / aluminum / zinc alloys
Cathodic protection: with auxiliary anode:
Pipeline
4) Inhibitor
(1) Inorganic inhibitor:
Anodic inhibitor
cathodic inhibitor
C / mol·dm-3
Cor
rosi
on r
ate
mm
/ h
NO2
CrO42 SiO3
2 HPO42
CO32
10-5 10-4 10-3 10-2
0.5
1.5
2.5
react with corrosion product or ions in solution to form inorganic deposition coating.
silicate, phosphate, chromate, nitrite, etc.
Self-assembled monolayer of alkanethiols
(2) Organic inhibitor:
small molecules, usually containing N, S, O, P atoms, can readily adsorb onto metal surface.
metal
1) Cu does not react with dilute sulfuric acid, but why do
es the solution gradually turn blue upon exposure of the
system to the air?
2) Why can Au dissolve in NaCN solution when the air w
as purged.
3) Annihilation can reduce corrosion rate of metal, why?
Discussion: