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Corrosion of dental materials
1. Corrosion of Dental materials
By
By
Mohamed Mahmoud Abdul-Monem
Assistant lecturer
Dental Biomaterials Department
Alexandria University
Egypt
Mohamed_mahmoud.biomaterials@yahoo.com
2. Corrosion
• Is an electrochemical process
and is dependant on the
ability of metals to conduct
electrical current.
• It causes metal deterioration
and subsequent mechanical
failure.
• It causes pulpal pain(galvanic
shock).
• Toxic and allergic responses
to metal ions.
• Metallic taste
• It may be desirable as in
dental amalgam ?? As
corrosion products seal the
marginal gap.(limitied
corrosion)
Tarnish
• Surface discoloration on a
metal or slight loss or
alteration of the surface
finish or luster.
• Occurs due to formation of
deposits ,oxides, sulfides
and chlorides on the
restoration surface.
• It is an early indication and
precursor of corrosion.
3.
4. Fundamental basis of corrosion
Chemical corrosion
• (Dry corrosion) It occurs in
absence of water or any fluid
electrolyte
• Direct combination of a metallic
and nonmetallic element to yield
a chemical compound through
oxidation reactions.
• E.g (1) Oxidation of Ag-Cu
eutectic alloy particles of dental
amalgam. Oxidation limits their
reactivity with mercury.
• (2) Sulfurization of silver in
amalgam (Ag2S)
Electrochemical corrosion
• Galvanic corrosion/wet corrosion
: requires the presence of water
or any fluid electrolyte and an
electric current .
5. Electrochemical corrosion
• When a metal is in contact with a fluid
electrolyte ,ions dissolve to form a saturated
solution and produce free electrons.
• The loss of electrons by a metal is Oxidation.
• The ease with which a metal gives up
electrons and oxidizes is the Oxidation
potential
6. Electrochemical cell
• Anode : surface where positive ions are formed
(surface undergoing oxidation and corroding).
• Cathode : surface where ions are deposited
(Reduction)
• Electrolyte : supplies ions needed at the cathode
and carries away corrosion products at the
anode.
• External circuit (conduction path) of electric
current.
7.
8. Forms of electrochemical corrosion
• Dissimilar metals.
• Heterogeneous surface composition.
• Stress corrosion
• Concentration cell corrosion.
9. Dissimilar metals
• When combinations of dissimilar metals are in
direct physical contact or between
restorations of similar alloys with different
surface composition.
• Example : Dental amalgam restoration
opposing a gold inlay.
• This results in sharp pain (galvanic shock).
• Saliva acts as an electrolyte and hard and soft
tissues as the external circuit.
13. Stress corrosion
• Stress increases internal energy of an alloy either
through elastic displacements or dislocations.
• It occurs due to fatigue or cyclic loading.
• Small surface irregularities (notches and pits) act
as sites of stress concentration.
• Deformed part of alloy (anode) and undeformed
part (cathode).
• Example: (1) excessive burnishing of margins in
metallic crowns .
• (2) Excessive carving (deep and sharp pits)
14. Concentration cell corrosion
• It occurs whenever there are variations in the
composition of electrolytes.
• Example(1): Accumulation of food debris in
interproximal areas .The debris produce an
electrolyte in this area that is different from
the electrolyte produced by saliva at the
occlusal surface.
15. • Example (2) : Differences in oxygen
concentration between parts of the same
restoration. The greatest attack happens at
the areas containing less oxygen (Anode).
• Pits, scratches and cracks in a restoration are
important example of this phenomenon.