1 4 electrochemistry(30) 101013
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Introduction
One phase contains electrons. Other phase contains ions.
e-
- - - - - - - - - - - - > +
Fundamental act in electrochemistry
Passage of Current Caused by Chemical Changes
Broad Field: sensors, electro-analysis, electro-synthesis,
electrodeposition, corrosion, and
dye-sensitized solar cell (DSC), fuel cell, and battery.
Electrochemistry is the Study of Phenomena atthe Electrode/ElectrolyteInterfaces.
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Introduction
Electrode reactions such as (1), (2), and (3)can only happen at the interface.
_______ 2
Cu2+
+ 2e
Cu (2) _______ _____
FeCp2 FeCp2+ + e (3)
ReactantProduct
composition in the nearby solution,
different from that further away.
There is a tendency for the system to transport
reactants from remote points and the depleted
zone widens as the reaction proceeds (Fig.1(b)). ______
Faulkner, Journal of Chem., Education, 1983
Just as the reactants is depleted near the interface,
the product accumulates nearby as shown in Fig.
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Potential is an Expression of Electron Energy.
The energy required to add or subtract an electron
an ar po en a : ox a on re uc on poss e.
potential.
Any electrode process is characterized by its ownreducedstandard potential E0.
On the positive side ofE0, the oxidized form of the
,
stable on the potential more negative than E0.
In the zone ~100 mV wide centered on E0, statistical
Fe/Pt = 0.27 oxidized
equilibrium of electrons on the electrode and species
in the solution permits mixtures of oxidized and
reduced forms with appreciable amounts (transition.
Faulkner ournal o Chem. Education 1983
Po ten t i a l i s an exp r ess ion o f elect r on energy .
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Work Function (not real)
s cro , o a e ys cs
__
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Double Layer Work Function
Ashcroft
Solid State Physics
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Work Function
th. , ,
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Electron Transfer at the Interface
LUMOMagnitude of the potential controls the direction
and rate of charge transfer.
HOMO
As a potential is moved negative, the species will
be reduced first with the least negative E0.a speciesA in solution
LUMO
. . ar , ec roc em ca e o s, e on
HOMO
_______________________________________
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Standard Electrode Potential
NHE (= SHE)
Normal Hydrogen Electrode- Neglect any orientational dependence
- 298 K
- Acid solution with
A. J. Bard, Electrochemical Methods, 2ndedition
an activity of H+ = 1 mol/liter (pH 0)
eV
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2 e =
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Band Structure Determined by Cyclic Voltammetry for CdSe Nanocrystals
Valence band
maximum
_
Conduction bandminimum
________ ________________
______________
Thomas Nanns Group, Journal of Chemical Physics (2003)
Freiburg Materials Research Center (Germany)
Electrochemistry Yejun (The contents of page 10 are the same as those of page 27.) http://bp.snu.ac.kr 10
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Current is an Expression of Rate.
Suppose ferrocene is being oxidized.
Usually we focus attention on a singleelectrode called the working electrode
FeCp2 FeCp2+ + e (3)
Each molecule that is oxidized ives u electrons to
________
the working electrode.
The electron will pass through the external circuit,
Fe/Pt = 0.27
an ac nto t e so ut on at a secon e ectro e
called the counter electrode.
Electrons at either electrode can flow into or out of____________
the electrode by way of external circuit which can be
oxidizing or reducing current_________
.e ow o e ectrons s rect y proport ona to t e rateof reaction there. So, t h e cu r r en t i s an exp ression o f ra t e .
Faulkner, Journal of Chem., Education, 1983
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Reference Electrode
Potentials actually mean the voltage differences
between a working electrode and a reference electrode.
an ar y r ogen ec r o e =
The reference electrode is arranged
so that it does not pass current,and is in equilibrium.
The reference electrode is constructed so that it
Fe/Pt = 0.27
conta ns ot forms of re ox coup e
(e.g., H+/H2, Hg/Hg2SO4, or Ag/AgCl)at fixed composition.
Electron energies in the metallic part of the electrode
are fixed at a value near the E0.1. Platinized platinum electrode.
2. H dro en as.
(image from Wikipedia)
3. Acid solution with an activity of H+ = 1 mol/liter.
4. Hydroseal for prevention of oxygen interference.
5. Reservoir via which the second half-element of
e ga van c ce s ou e a ac e .
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Adrian W. Botts Group, Current Separations 14:2 (1995)
Bioanalytical Systems West LafayetteReference Electrode
Vycor porous glass
- modest leak rate
- poss e con am na on o so u on
- ionic conducting pathway
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Counter Electrode >> Working Electrode
e e
Power generated
or supplied
e e
Power generated
or supplied
measured measured- - - - - - - - - - - - - - - - - - - - - - - - - - -
A+
B-
ee A+
B-
ee- - - - - - - - - - - - - - - - - - - - - - - - - - - - - - - - - - - - - - - - - - - - - - - - - - - - - - - - - - - - -
RE: Reference electrodeWorking electrode Counter electrodeWorking electrode Counter electrode
RE: Reference electrode
- Surface area:Working electrode
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Counter Electrode ~ Working Electrode
e e
Power generatedor supplied
e e
Power generatedor supplied
measured measured- - - - - - - - - - - - - - - - - - - - - - - - - - - - - - - - - - - - - - - - - - - - - - - - - - - - - - - - - - - - - - - - - - - - - - - - - - - - - - - - - - - - - - - - -
A+
B-
ee A+
B-
ee
Working electrode Counter electrode Working electrode Counter electrodeRE: Reference electrode RE: Reference electrode
- Surface area:Working electrode Counter electrode
- For different potential at working electrode,
different potential at counter electrode
http://bp.snu.ac.kr 15Electrochemistry Yejun
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Electrochemical Cells and Reactions
Fe/Pt = 0.27
A potential difference between two electrodes
. . . ar , ec roc em ca e o s
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Electrochemical Cells and Reactions
The potential that develops in a cell is a measure of the tendency for a reaction to proceedtoward equilibrium.
Standard oxidation/reduction reactions:
All relative to the H2
/H+ reaction, 298 K,
, .
A. J. Bard, Electrochemical Methods, 2ndedition
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Double Layer
A. J. Bard, Electrochemical Methods, 2ndedition
q meta = -q so ut on charge neutrality!
Compact layer = inner and outer Helmholtz planes
Diffuse layer = gradient of charge accumulation
metal = q metal/area (C/cm2)
- e excess c arge on a me a s con ne o e near sur ace reg on.
- However, the balancing charge on the solution side of the interface extends
out into the solution with some thickness (ionic zones in solution).
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.
to specifically adsorbed anions (inner).
2. Solvated ions are distributed in diffuse layer(~100 ), because of thermal agitation in thesolution (diffuse).
.and specifically adsorbed anions in inner layer isequal to the charge from solvated ions in diffuselayer.
metal
+ inner
= - diffuse
Bard, A. J., and Faulkner, L. R.Electrochemical Methods
I n n e r He lm h o l t z La y erD if f u s e La y er ( ~ 1 0 0 )
ey, ew or . , ap.
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Ch a r g e Pr o f i le i n t h e Vi ci n i t y o f I n t e r f ace
I nne r H el m ho l t z Lay er Di f f u se La y er ( ~ 1 0 0 )
-
x +
- Ther e a re e lect r on cloud s sp i l t over
,
i n t he v o l t age p r o f i l e nea r t he m e ta l su r f ace .
a r g e p r o e on e so u on s e s ow snega t i ve cha rg es near t he su r f ace b u t
d i f f us es aw ay w i t h i n inn e r lay er .META
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Vo l t a g e Pr o f i le in t h e Vi ci n i t y o f I n t e r f ace
I nne r H el m ho l t z Lay er D if f us e Lay er ( ~ 100 )
x
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+Schem at i cs o f Doub le Layer i n So lu t ion
- +
Nega t i ve l y
Charged
+ +e a - + Bard, A. J. and Faulkner, L. R.Electrochemical Methods
Wiiey, New York. 1980, Chap. 1.
Hamann, C. H., ElectrochemistryWiley-VCH, 1998, Chap. 3.
(x)
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Double Layer
The CRC Handbook of Solid State ElectrochemistryH. J. M. Bouwmeester, p. 27
Charge distribution
o en a s r u on
Metal Diffuse layer
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Helmholtz Layer and Diffuse Layer
nd. . , ,
_____
_____
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Potential Profile Across the Double-Layer
. . ar , ec roc em ca e o s, e on
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______________ ______________
PL
CV
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Band Structure Determined by Cyclic Voltammetry for CdSe Nanocrystals
Valence band
maximum_
Conduction bandminimum
________ ________________
______________
Thomas Nanns Group, Journal of Chemical Physics (2003)
Freiburg Materials Research Center (Germany)
Electrochemistry Yejun (The contents of page 10 are the same as those of page 27.) http://bp.snu.ac.kr 27
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Experiments and Variables in Electrochemical Cell
1. Mass transfer of reactant/product
to and away from the electrode
n er ace.
2. Electron transfer at the interface.
3. Chemical reactions.
4. Surface processes
(adsorption/desorption)
A. J. Bard, Electrochemical Methods, 2ndedition
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A. J. Bard, Electrochemical Methods, 2ndeditionMass Transport
o es o ass ranspor :
Migration movement of ions by an electric field
Diffusion
by a concentration gradientConvection
by stirring or hydrodynamic transport
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Th S f El t h i t
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The Scope of Electrochemistry
1. Investi ation of chemical henomena associated with
a charge-transfer reaction.
2. To assure electro-neutrality,
two or more half reactions take lace in o osite directions
(oxidation and reduction).
3. If the change of total Gibbs free energy is negative,
.
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