Electroplating handout

Electroplating (electrodeposition)
2). Reaction surface
Electroplating is to produce a dense,
uniform, and adherent coating for
decorative and protective purposes, or
enhancing specific properties of the
surface. The surface can be conductors,
such as metal, or nonconductors, such
as plastics. The coating is upon a surface
by the act of electric current.
The rate of reaction would vary due to the size of surface area.
For those which have a broader surface would be coated more
quickly, since the surface area continuously supplied with negative
electron, therefore ions in the solution would be attracted and
reduced in a faster rate.
For those which have a smaller surface area would take a longer
time to be reduces, as ions have to compete more vigorously for a
spot of the surface in order to accept the electrons from the target
Redox reaction
Reaction surface area
3). Faraday’s Laws
Faraday’s Law
1). Redox reaction
Cathode (reduction)
Anode (oxidation)
Ag+(aq)+ e- → Ag(s)
Ag(s) → Ag+(aq)+ e-
The oxidized Ag from anode would migrate to the cathode and
reduce, the purpose of putting Ag in the anode rather than other
kind of metal is the ensure there are continuous supply of Ag+ ion in
the solution so to coat a layer of silver onto our target (fork).
The amount of substance produced or consumed in an electrolysis
reaction is directly proportional to the quantity of electricity that
flows through the circuit.
The mass of the coating metal formed is proportional to the
quantity of the electricity used.
Works Cited
"Chemistry: Faraday's Laws - CliffsNotes." Get Homework Help with
CliffsNotes Study Guides - CliffsNotes. Web. 5 May 2011.
"Electroplating Helen." Electroplating Helen. Ed. Helen H. Lou.
Department of Chemical Engineering, Lamar University,
Beaumont, Texas, U.S.A. Web. 2 May 2011.
Mustoe, Frank J. McGraw-Hill Ryerson Chemistry 12. Toronto:
McGraw-Hill Ryerson, 2002. Print.
"YouTube - Electroplating." YouTube - Broadcast Yourself. Dizzo95,
21 July 2008. Web. 2 May 2011.