Electrochemistry: From soft interfaces to bioanalytics · Molecular dynamic representation!...
Transcript of Electrochemistry: From soft interfaces to bioanalytics · Molecular dynamic representation!...
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Electrochemistry: From soft interfaces to
bioanalyticsHubert H. Girault
ENS Lyon Septembre-Octobre 2010
Saturday, September 18, 2010
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Molecular Electrocatalysis for Oxygen Reduction by CobaltPorphyrins Adsorbed at Liquid/Liquid Interfaces
Bin Su,†,9 Imren Hatay,†,! Antonın Trojanek,‡ Zdenek Samec,‡ Tony Khoury,§
Claude P. Gros,§ Jean-Michel Barbe,§ Antoine Daina,¶ Pierre-Alain Carrupt,¶ andHubert H. Girault*,†
Laboratoire d’Electrochimie Physique et Analytique, Ecole Polytechnique Federale deLausanne, Station 6, CH-1015 Lausanne, Switzerland, J. HeyroVsky Institute of Physical
Chemistry of ASCR, V.V.i, DolejskoVa 3, 182 23 Prague 8, Czech Republic, Institut deChimie Moleculaire de l’UniVersite de Bourgogne, ICMUB (UMR 5260),
BP 47870, 21078 Dijon Cedex, France, Department of Chemistry, Selcuk UniVersity,42031 Konya, Turkey, Section des Sciences Pharmaceutiques, Quai Ernest-Ansermet 30,
CH-1211 GeneVe 4, Switzerland
Received October 5, 2009; E-mail: [email protected]
Abstract: Molecular electrocatalysis for oxygen reduction at a polarized water/1,2-dichloroethane (DCE)interface was studied, involving aqueous protons, ferrocene (Fc) in DCE and amphiphilic cobalt porphyrincatalysts adsorbed at the interface. The catalyst, (2,8,13,17-tetraethyl-3,7,12,18-tetramethyl-5-p-amino-phenylporphyrin) cobalt(II) (CoAP), functions like conventional cobalt porphyrins, activating O2 viacoordination by the formation of a superoxide structure. Furthermore, due to the hydrophilic nature of theaminophenyl group, CoAP has a strong affinity for the water/DCE interface as evidenced by lipophilicitymapping calculations and surface tension measurements, facilitating the protonation of the CoAP-O2
complex and its reduction by ferrocene. The reaction is electrocatalytic as its rate depends on the appliedGalvani potential difference between the two phases.
Introduction
Molecular oxygen (O2) reduction reaction (ORR) is animportant topic in biological and energy-related chemistry.1,2
However, it is a spin-forbidden process, which is kineticallyslow at ambient temperature unless a catalyst is present. Naturehas made the choice in aerobic organisms by evolving membrane-bound enzymes that contain a porphyrin substructure ascatalysts.1,3-6 Inspired by their role in nature, a number ofmetalloporphyrins have been chemically synthesized.7-9 Their
catalytic activity has been investigated either electrochemicallyusing the modified electrode methodology9-25 or chemicallyusing molecular electron donors, such as ferrocene (Fc) and its
† Ecole Polytechnique Federale de Lausanne.‡ J. Heyrovsky Institute of Physical Chemistry of ASCR.§ Institut de Chimie Moleculaire de l’Universite de Bourgogne.! Selcuk University.¶ Section des Sciences Pharmaceutiques.9 Present Address: Institute of Microanalytical Systems, Department of
Chemistry, Zhejiang University, Hangzhou 310058, China.(1) Boulatov, R. In N4-Macrocyclic Metal Complexes; Zagal, J. H.,
Bedioui, F., Dodelet, J.-P., Eds.; Springer: New York, 2006; pp 1-36.
(2) Shukla, A. K.; Raman, R. K. Ann. ReV. Mater. Res. 2003, 33, 155–168.
(3) Babcock, G. T. Proc. Natl. Acad. Sci. U.S.A. 1999, 96, 12971–12973.(4) Babcock, G. T.; Wikstrom, M. K. F. Nature 1992, 356, 301–309.(5) Sono, M.; Roach, M. P.; Coulter, E. D.; Dawson, J. H. Chem. ReV.
1996, 96, 2841–2887.(6) Wikstrom, M. K. F. Nature 1977, 266, 271–273.(7) Collman, J. P.; Boulatov, R.; Sunderland, C. J.; Fu, L. Chem. ReV.
2004, 104, 561–588.(8) Kim, E.; Chufan Eduardo, E.; Kamaraj, K.; Karlin Kenneth, D. Chem.
ReV. 2004, 104, 1077–1133.(9) Zagal, J. H.; Paez, M. A.; Silva, J. F. In N4-Macrocyclic Metal
Complexes; Zagal, J. H., Bedioui, F., Dodelet, J.-P., Eds.; Springer:New York, 2006; pp 41-75.
(10) Anson, F. C.; Shi, C.; Steiger, B. Acc. Chem. Res. 1997, 30, 437–444.
(11) Chang, C. J.; Deng, Y.; Nocera, D. G.; Shi, C.; Anson, F. C.; Chang,C. K. Chem. Commun. 2000, 1355–1356.
(12) Chang, C. J.; Loh, Z. H.; Shi, C.; Anson, F. C.; Nocera, D. G. J. Am.Chem. Soc. 2004, 126, 10013–10020.
(13) Collman, J. P. Acc. Chem. Res. 1977, 10, 265–272.(14) Collman, J. P.; Boulatov, R.; Sunderland, C. J. In The Porphyrin
Handbook; Kadish, K. M., Smith, K. M., Guilard, R., Eds.; AcademicPress: San Diego 2003; Vol. 11, pp 1-49.
(15) Collman, J. P.; Chang, L. L.; Tyvoll, D. A. Inorg. Chem. 1995, 34,1311–1324.
(16) Collman, J. P.; Denisevich, P.; Konai, Y.; Marrocco, M.; Koval, C.;Anson, F. C. J. Am. Chem. Soc. 1980, 102, 6027–6036.
(17) Collman, J. P.; Fu, L.; Herrmann, P. C.; Zhang, X. Science 1997, 275,949–951.
(18) Collman, J. P.; Hutchison, J. E.; Lopez, M. A.; Tabard, A.; Guilard,R.; Seok, W. K.; Ibers, J. A.; L’Her, M. J. Am. Chem. Soc. 1992,114, 9869–9877.
(19) Collman, J. P.; Marrocco, M.; Denisevich, P.; Koval, C.; Anson, F. C.J. Electroanal. Chem. Interfacial Electrochem. 1979, 101, 117–22.
(20) Deng, Y.; Chang, C. J.; Nocera, D. G. J. Am. Chem. Soc. 2000, 122,410–411.
(21) Durand, R. R., Jr.; Anson, F. C. J. Electroanal. Chem. InterfacialElectrochem. 1982, 134, 273–89.
(22) Shi, C.; Anson, F. C. Inorg. Chem. 1990, 29, 4298–4305.(23) Shi, C.; Steiger, B.; Yuasa, M.; Anson, F. C. Inorg. Chem. 1997, 36,
4294–4295.(24) Collman, J. P.; Wagenknecht, P. S.; Hutchison, J. E. Angew. Chem.,
Int. Ed. 1994, 33, 1620–1639.(25) Le Mest, Y.; Inisan, C.; Laouenan, A.; L’Her, M.; Talarmin, J.; El
Khalifa, M.; Saillard, J. Y. J. Am. Chem. Soc. 1997, 119, 6095–6106.
Published on Web 02/04/2010
10.1021/ja908488s " 2010 American Chemical Society J. AM. CHEM. SOC. 2010, 132, 2655–2662 9 2655
Molecularcatalyst
Electron donors
Protons
O2
H2 O2
ΔφN
N
N
N
NH2
Co
AmphiphilicCoAP porphyrin
J. AM. CHEM. SOC. 2010, 132, 2655–2662Saturday, September 18, 2010
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Electrochemistry is great!
The only problem is the electrode...Jean-Michel SavéantAustin 4- 2- 2010
Three periods :
- Mercury electrode - Polarography- Single crystal- Molecular grafting - Diazonium chemistry
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Membrane Electrochemistry
Membrane function :Separate reactants and productsProvide an electrochemical driving force
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Bio-inspired electrochemistry
ITIES functions :Separate reactants and productsProvide an electrochemical driving force
water
organic
ITIES Highly reproducible
Defect free
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Electrochemistry
Study of chemical reactions for which the standard Gibbs energy depends not only on the temperature,
but also on a potential difference.
We can also drive electrochemical reactions without electrodes
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Liquid-liquid interfaces
• Interfacial structure
• Polarised liquid-liquid interfaces
• Electrocapillary phenomena
• Charge transfer reactions
• Photocurrent
• Nanoparticle adsorption - Plasmonics
• Artificial photosynthesis
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Interfacial structure
• Classical systems : water-nitrobenzene, 1,2-dichloroethane, heptanone, octanol and 2-nitrophenyloctylether (NPOE)
• Dynamic molecular interface with thermal fluctuations
• Relatively sharp at the molecular level but with corrugations caused by thermal fluctuations and capillary waves
• Water molecules tend to arrange themselves so as to maximize the number of hydrogen bonds and to minimize their potential energy
• Hydrogen bond lifetime τw-DCE = 15 ps, τw-NB = 10 ps, τw-
CCl4 = 7 ps, longer than the bulk value of about 5 ps.
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Molecular dynamic representation
!Distribution of all CCD– anions and of Cs+ ions within 10 Å from the interface. The surface of the interface is color coded as a function of its z-position
G. Chevrot, R. Schurhammer, and G. Wipff, in J Phys Chem B, Vol. 110, 2006, p. 9488
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Surface roughness
Effect of the probe sphere radius on the identification of the interfacial molecules. The upper part of the figure shows the same water configuration with three different probe spheres of the radii Rps = 0.5 Å (left), Rps = 2.0 Å (middle), and Rps =10.0 Å (right). The molecules that are not identified as interfacial ones with a given probe sphere are plotted in lighter colors.
L. B. Partay, G. Hantal, P. Jedlovszky, A. Vincze, and G. Horvai, in J Comput Chem, Vol. 29, 2008, p. 945.
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Bivariate representation
Orientational maps of the surface water molecules located at the surface layer (first column), in regions C and B of the surface layer (second and third column), and in region A of the surface layer (fourth column) of the aqueous phase of the system simulated. Lighter shades of grey indicate higher probabilities; the spacing of the contour lines is 10–4. The water orientations corresponding to the observed peaks are also illustrated. X is the surface normal vector pointing to the vapour phase.
L. B. Partay, G. Horvai, and P. Jedlovszky, in Phys Chem Chem Phys, Vol. 10, 2008, p. 4754.
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Surface water structure
Illustration of the relation of the preferred water orientations and local curvature of the interface. The insets demonstrate the similarities between the water orientations found to be preferred at positions of locally concave curvature (i.e., at the ‘‘wells’’) of the interface that is flat on the macroscopic scale, and at the surface of small apolar solutes.
L. B. Partay, G. Horvai, and P. Jedlovszky, in Phys Chem Chem Phys, Vol. 10, 2008, p. 4754.
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Liquid-liquid interfaces
• Interfacial structure
• Polarised liquid-liquid interfaces
• Electrocapillary phenomena
• Charge transfer reactions
• Photocurrent
• Nanoparticle adsorption - Plasmonics
• Artificial photosynthesis
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Inner Potential - Galvani Potential
The potential is constant in a phase that is neutral by definition
Sphère
ψ =Q / 4πε0R
Surface potential
Outer potential
+++++
Positively chargedsphere
Pote
ntia
l
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Electrochemical Potential
%µi = µi + ziFχ + ziFψ = µi + ziFφ
= µio + RT lnai + ziFφ
µi : Chemical contribution All short-range interactions includingelectrostatic interactions
ziFψ : Electrical approach work
ziFχ : Electrical entry work
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Gibbs energy of transfer
ΔGtr,i
w→o = %µio − %µi
w
Also, the difference between solvation and hydration energy
At equilibrium ΔGtr,i
w→o = 0
%µi
o ,o + RT ln aio + ziFφ
o = %µio ,w + RT ln ai
w + ziFφw
I w I o
%µi
o ,o + RT ln aio + ziFφ
o = %µio ,w + RT ln ai
w + ziFφw
Nernst equation Δo
wφ = Δowφtr,i
o +RTziF
lnai
o
aiw
⎛
⎝⎜⎜
⎞
⎠⎟⎟
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Standard transfer potential
lipophilic ion µio ,w
µio ,o
ΔGtr,io ,w→o
ΔGtr,io ,w→o = µi
o ,o − µio ,wStandard Gibbs energy of
transfer
Δowφi
o =ΔGtr,i
o ,w→o
ziFStandard transfer potential
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Salt partition
water solvent
C+ C+
A– A–
At equilibrium, both phases are neutralbut the interface is charged.
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Distribution Potential
�
Δowφ = Δo
wφC+o +
RTF ln
aC+o
aC+w
⎛
⎝ ⎜ ⎜
⎞
⎠ ⎟ ⎟
�
Δowφ = Δo
wφA–o −
RTF ln
aA–o
aA–w
⎛
⎝ ⎜ ⎜
⎞
⎠ ⎟ ⎟
Nernst equation for both the cation and the anion
�
Δowφdis =
ΔowφC+
o / + ΔowφA–
o /
2 =ΔowφC+
o + ΔowφA–
o
2 +RT2F ln
γC+o γ A−
w
γC+w γ A–
o
⎛
⎝ ⎜ ⎜
⎞
⎠ ⎟ ⎟
Distribution potential independent of phase ratio
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Distribution Potential
C+ C+
A– A– Δowφdis =
ΔowφC+
o + ΔowφA–
o
2
�
ΔDCEeau φTBACl = −360mV
Cl–
-0.5 0
�
Δφ /VTBA+
-0.22
�
ΔDCEeau φNaTPB = 445mV
0 0.5
�
Δφ /VNa+
0.560.33
TPB–
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Potential determining Ion
I+ I+
A– X–3 Nernst equations2 electroneutrality conditions
cI+tot
1+ reF(Δo
wφ−ΔowφI+o / )/RT
−cX–tot
1+ re−F(Δo
wφ−Δowφ
X−o / )/RT
−cA–tot
1+ re−F(Δo
wφ−Δowφ
A−o / )/RT
= 0
cI+w = cIA
w cI+o = cIX
o
Δowφ = Δo
wφI+o +
RTFln
aI+o
aI+w
�
�
�����
�
�
������= Δo
wφI+o +
RTFln aIX
o
aIAw
�
�����
�
������
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How to polarise a liquid|liquid interface?
Pioneered by C. Gavach et al., J. Koryta et al., M. Senda et al.
Hydrophilic aqueous electrolytee.g. LiCl
Lipophilic organic electrolytee.g. BATBRef : Junction BATB/BACl
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Potential window
TPB-
TBA+
Li+
SO2-4
0 0.1 0.2 0.3 0.4 0.5-0.1-0.2-0.3-0.4
Δowφ / Volts
PPPh
Ph
Ph
Ph
Ph
Ph
N+
4
BCl
-
Lipophilic cation bis(triphenylphosphoranylidene)ammonium
Lipophilic aniontetrakis(pentafluorophenyl)borate
+
–
–
+
Lithium sulfate in water / Tetrabutylammonium tetraphenylborate in 1,2-DCE
Absolute potential scale
FF
F F
F
B-
FF
F
F F F
FF
F
F F F
F
FF
Lipophilic aniontetrakis(pentafluorophenyl)borate
Lipophilic cation bis(triphenylphosphoranylidene)ammonium
P N P+
BA+ TB−
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Molecular Electrocatalysis for Oxygen Reduction
!
Ag AgCl
DCE Water
Ag2SO4 Ag
Water Ref
0.01 M LiCl1 mM BACl
5 mM BATB0 or 50 μM CoAP
0 mM Fc
0.01 M LiClHCl pH=2
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How to pump protons to the organic phase?
HCl
BATB
H+
TB–
Potentiostatic control
HCl + LiTB HTB
Chemical control
+
–F
F
F F
F
B-
FF
F
F F F
FF
F
F F F
F
FF
TB−
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Distribution concentration10 mM HCl + 5 mM LiTB
5 mM BATB
Δowφtr
o / V
H+ Li+ BA+ TB– Cl–
0.55 0.59 –0.6 0.65 –0.53
At equilibrium Δo
wφeq = 0.541V
5.8 mM H+ 4.3 mM Li+ 0.14 mM TB– 10 mM Cl–
5 mM BA+ 4.2 mM H+ 0.7 mM Li+ 9.86 mM TB–
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(a) Aqueous phase: 5 mM LiTB + 10 mM HCl.DCE phase: 1 mM Fc + 5 mM BATB (flask 1), 1 mM Fc + 20 M CoAP + 5 mM BATB (flask 2) and 20 M CoAP + 5 mM BATB (flask 3). The upper left inset shows the colors of three DCE solutions before contacting with the water solution
!
FcBATB
FcCoAPBATB
CoAPBATB
FcCoAPBATBNo O2
Molecular Electrocatalysis for Oxygen Reduction
(b) The isolated top aqueous solutions with added excess NaI;
(c) Further addition of starch to the flasks shown in (b)
(d) A 4-hour-two-phase reaction in the glovebox with the same solution composition as the flask 2 in (a).
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Liquid-liquid interfaces
• Interfacial structure
• Polarised liquid-liquid interfaces
• Electrocapillary phenomena
• Charge transfer reactions
• Photocurrent
• Nanoparticle adsorption - Plasmonics
• Artificial photosynthesis
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Interfacial tension
γ γ
dW = γ dAWork to enlarge a surface
Work to reduce a volume dW = − p dV
Superhydrophobic surface
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Electrocapillarity
-1.0 -0.5 0 0.5
KOH
NaClKCNS
NaBr
KI
420
380
340
300
(E - Epzc(NaF) ) / V
Tens
ion
Inte
rfaci
ale
/ m
N.m
-1
+ + + _ _ _
Positive charge in solution No adsorption
Negative charge in solutionAdsorption - Interaction
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Lippmann’s equations
Interfacial charge σM = �
∂γ∂E
�����
�����T , p,µi
Differential capacitance
Cd =∂σM
∂E= �
∂2γ∂E2
�
�����
�
������T , p,µi
Gabriel Lippmann1845-1923
Prix Nobel de PhysiquePhotographie couleurElectrocardiographe
ΓCd2+(Hg) dµCd + ΓMg2+
(H2O) dµMgCl2 + ΓH+(H2O) dµHCl + σM dE = − dγ
Gibbs adsorption equation : Hg-Cd/MgCl2 + HCl
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Gouy-Chapman theory
Spatial ionic distribution in solution next to a charged wall
Louis Georges Gouy1854-1926
David Leonard Chapman1869-1958
0.20
0.15
0.10
0.05
0.00
c /
M
20151050
x / nm
c = 0.01 M
φ(0) = 100 mV
Cation
Anion
Next to a positively charged wall, there is an excess of anions and a depletion of cations. Overall, the ionic strength increase
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Polarised liquid-liquid interfaces
Two back-to-back diffuse layers with some interpenetration
Δowφ
few nanometers
+
+
+
+
–
–
–
–
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X-ray reflectivity
23
free energy profile for ion transfer across the interface when this profile is described by a simple
analytic form or by a potential of mean force from molecular dynamics simulations.
Figure 4: (Left) Cross-sectional view of stainless steel sample cell. W: mylar windows; T: thermistors to measure temperature. The kinematics of surface X-ray reflectivity is also indicated: kin is the incoming X-ray wave vector, kscat is the scattered (reflected) wave vector, ! is the angle of incidence and reflection [68] (Middle) X-ray reflectivity, R(Qz), as a function of wave vector transfer Qz from the interface between 0.01 M TBATPB in nitrobenzene and a TBABr in water at five concentrations (0.01, 0.04, 0.05, 0.057, and 0.08 M, bottom to top) at a room temperature of 24 ± 0.5°C. Solid lines are predictions using the potential of mean force from MD simulations. Dashed lines are predicted by the Gouy-Chapman model. No parameters have been adjusted in these two models. Data for different concentrations are offset by factors of 10 (R = 1 at Qz = 0). Error bars are indicated by horizontal lines through the square data points and are usually much smaller than the size of the squares. The points at Qz = 0 are measured from transmission through the bulk aqueous phase. (Inset) The kinematics of x-ray reflectivity: kin, incoming x-ray wave vector; kscat, scattered wave vector; and !, angles of incidence and reflection. (Right) Ion distributions at the interface between a 0.08 M TBABr solution in water and a 0.01 M TBATPB solution in nitrobenzene. Solid lines, TBA+; short-long dashed line, Br–; short dashed line, TPB–. (A) Gouy-Chapman theory. (B) Calculation from MD simulation of the potential of mean force[70]. Reprinted with permission.
When varying the temperature of the system, the authors showed clearly that the measured
interfacial width differs from the predictions of capillary wave theory with a progressively
smaller deviation as the temperature is raised. It was therefore concluded that both molecular
layering and dipole ordering parallel to the interface must take place. Either layering or a
bending rigidity, that can result from dipole ordering, could explain these measurements [69]. It
can be regretted that capacitance measurements were not carried out directly on the systems
Science, 311 (2006) 216
Dashed lines arepredicted by the Gouy-Chapman model.
Ion distributions at the interface between a 0.08 M TBABr solution in water and a 0.01 M TBATPB solution in nitrobenzene.Solid lines, TBA+; short-long dashed line, Br–; short dashed line, TPB–. (A) Gouy-Chapman theory. (B) Calculation from MD simulation of the potential of mean force
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Lipophilicity map
!
�
Pi =aio
aiw= exp ziF Δo
wφ − Δowφi
o( ) / RT[ ]
Ion distribution
�
Pi =aio
aiw= Pi
o exp ziFΔowφ /RT[ ]
�
lnPio = −
µio ,o − µi
o ,w
RT = −ΔGtr,i
o ,w→o
RT = −ziFRT Δo
wφio
ADME-Tox (Absorption, Distribution, Metabolism, Excretion - Toxicology)
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Interfacial acid-base equilibria
AH
AH
A– + H+
A– + H+
Kao =
aA–o aH+
o
aAHo = Ka
w PA–PH+
PAHo = Ka
w PA–o PH+
o
PAHo
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pH titration of CoAP
! !
First, the Soret band at 423 nm increases at the cost
of the original one at 397 nm, as well as the
appearance of a new band at 356 nm, with increasing
the concentration of TFA. This is assigned to be the
proton of CoAP-O2
Spectra of titrating 25 M CoAP with TFA
When the TFA concentration is higher than 5 mM, both the second Soret band and the band at 356 nm start decreasing due to the protonation of the peripheral amine. As the TFA concentration is above 20 mM, the second Soret band resides at 420 nm, which does not shift but decrease in intensity with the TFA concentration.
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Techniques
• Pendant drop
• Sessile drop
• Quasi electric light scattering
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Pendant drop
!
!
2π xγ sinθ = π x2γ 1
rin+
1rout
⎛
⎝⎜
⎞
⎠⎟ +Vρmg
β =ρmgb
2
γ
At the inflexion plane: γ =
Vρmg2π x sinθ
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Sessile drop
!
!!
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Quasi elastic light scattering
Lamb's equation
�
fo =12π
γ k3
ρw + ρoSaturday, September 18, 2010
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Na4ZnTPPC adsorption
inte
nsity
/ a.
u.
8000600040002000
frequency / Hz
2nd order spot
Pure water/DCE
0.4 mM ZnTPPCaq/DCE
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Potential controlled adsorption of ZnTPPC4–
25x10-6
20
15
10
5
0
Cdl
/ F
cm-2
0.30.20.10.0-0.1-0.2 Δφ / V
DCE/water 0.00 mM0.01 mM0.05 mM0.10 mM
Li2SO4 | BTPPATPFB
Electrocapillary curvesCapacitance dataSaturday, September 18, 2010
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!
Molecular Electrocatalysis for Oxygen Reduction
−dγ T,P = σdΔowφ + ΓH2OdµH2O + Γ
Li+dµLiCl + Γ
H+ + ΓCoAP−O2 H+( )dµHCl
+ ΓCoAP + ΓCoAP-O2+ Γ
CoAP-O2 H+( )dµCoAP + ΓCoAP-O2+ Γ
CoAP-O2 H+( )dµO2
+ ΓDCEdµDCE + ΓBA+ dµBATB
!
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ΓCoAP + Γ Co-O2( )AP + ΓCo-O2H( )AP⎡⎣ ⎤⎦
+ = −1RT
∂γ∂ lncCoAP
⎛⎝⎜
⎞⎠⎟ T ,P,Δowφ ,µi ≠µCoAP
Molecular Electrocatalysis for Oxygen Reduction
! !
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Liquid lenses
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Electrowetting with electrolytes
Courtesy of A. Kucernak, Imperial College, London
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Liquid-liquid interfaces
• Interfacial structure
• Polarised liquid-liquid interfaces
• Electrocapillary phenomena
• Charge transfer reactions
• Photocurrent
• Nanoparticle adsorption - Plasmonics
• Artificial photosynthesis
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Charge Transfer Reactions
IonTransfer
Assisted IonTransfer
ElectronTransfer
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Nernst equation - Ion distribution
Ion distribution is potential dependent
�
izi
�
izi
�
Δowφ = φw −φ o = Δo
wφio +
RTziF
ln aio
aiw⎛
⎝ ⎜ ⎞
⎠ ⎟
ΔGtr,io ,w→o = ziFΔo
wφio
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0.2 0.3 0.4 0.5 0.6
0
2
4
6
8
10
-2
-4
-6
I / A
x 1
0-5
Δ owφ / V
Ion transfer voltammetry
Tetramethylammonium transferwater|1,2-dichloroethane interface
+
Electrochemical methods can measure the Gibbs energy of
transfer
Δowφi
o /
Diffusion
Diffusion
Transfer
+
E / V
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Δowφ
pH
ΔowφBH+
o
pKaw
pKa,effw
logPBBHw+
BHo+
Bo
Distribution diagramof a lipophilic base
Cation transferpH independent
BH+
BH+
pH dependentproton pump
B
H+
BH+
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H2TPP Proton transfer
CVs of blank and in the presence of 0.05mM H2TPP at 50mV/s
20
10
0
-10
j / µ
A c
m-2
0.40.20.0-0.2Δo
wφ / V
pH = 1 Blank 50µM H2TPP
Ag AgCl5 mM BTPPATPFPB
0.05 mM H2TPP0.01 M LiCl
(pH 1)
DCE Water
0.01 M LiCl1 mM BTPPACl AgCl AgCell:
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Scan rate dependence
ip = 0.4463nFcnFvDRT
Randles-Sevcik equation:
slope=1.0624 ± 0.0334
CVs at various scan rates in the presence of 0.05mM H2TPP
The first anodic peak current as a function of square root of scan rate.
DH2 TPP = 6.25 ×10−6 cm2 s-1
20
10
0
-10
j / µ
A c
m-2
0.40.20.0-0.2Δo
wφ / V
pH = 150µM H2TPPScan rate (mV/s): 9,16,25,36,49,64
10
8
6
4
2
0
j p / µA
cm
-2
86420v1/2 / mV1/2s-1/2
Ag AgCl5 mM BTPPATPFPB
0.05 mM H2TPP0.01 M LiCl
(pH 1)
DCE Water
0.01 M LiCl1 mM BTPPACl AgCl AgCell:
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ip = 0.4463nFcnFvDRT
Randles-Sevcik equation:
slope=0.1037 ± 0.00282
v = 25 mV/s
CVs at various H2TPP concentrations at 25mV/s
The first anodic peak current as a function of H2TPP concentration.
DH2 TPP = 5.95 ×10−6 cm2 s-1-20
0
20
j / µ
A c
m-2
0.40.20.0-0.2Δo
wφ / V
pH = 120,50,100,200µM
20
10
0j p
/ µA
cm
-2
2001000cH2TPP / µM
Concentration dependence
Ag AgCl5 mM BTPPATPFPB
0.05 mM H2TPP0.01 M LiCl
(pH 1)
DCE Water
0.01 M LiCl1 mM BTPPACl AgCl AgCell:
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pH dependence
CVs in the presence of 0.05mM H2TPP at various pH (25mV/s)
15
10
5
0
-5
-10
j / µ
A c
m-2
0.40.20.0-0.2Δo
wφ / V
50µM H2TPP pH1 pH2 pH3
10
5
0
-5
j / µ
A c
m-2
0.40.20.0-0.2Δo
wφ / V
50µM H2TPP pH5 pH7
Ag AgCl5 mM BTPPATPFPB
0.05 mM H2TPP0.01 M LiCl
(pH = x)
DCE Water
0.01 M LiCl1 mM BTPPACl AgCl AgCell:
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Acidity ConstantsAcidity constants:
Transfer potential dependence on pH.
H4TPPH2+ Ka1⎯ →⎯ H3TPPH
+ + H+
H3TPPHKa2⎯ →⎯ H2TPPH + H+
Ka1=3.83×106
Ka2=1.31×1010
0.6
0.4
0.2
0.0Δ owφ 1o &
Δowφ 2p
c / V
6420pH
Δowφ1
o
Δowφ2
o
Δo
wφ o = Δowφ
H+o −
RTF
ln Kao +
2.303RTF
pH
Δowφ = Δo
wφH+o +
RTF
lna
H+o
aH+w
⎛
⎝⎜⎜
⎞
⎠⎟⎟
Ka1 =aH3TPPH+aH+aH4TPPH2+
Ka2 =aH2TPPaH+aH3TPPH+
Equation de Nernst
Apparent standard transfer potential
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Ion partition diagram
H2TPPo
H4TPP2+ w
H4TPP2+ o
H3TPP
+ o
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Micro-ITIES
!
!Optical microscopic image of a micropipette (Scale bar = 10 μm). Background-subtracted CV of simple TEA+ transfer at a 2.1 μm radius pipette. The open circles represent simulated CVs [110].
!
Video micrographs of a 15.5 m-radius micropipette filled with an aqueous KCl solution and immersed in a DCE solution of DB18C6. (B) No external pressure was applied to the pipette, and the micro-ITIES is flat. The insets show corresponding steady-state voltammograms of facilitated transfer of potassium [239]
Ion transferIngress-egress
Assisted ion transfer
ISS = 3.35π zFDCr
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Nano-ITIES
!
ISS = π zFDcr sinθ
!
Steady-state egress current
4μm
100 nm
1.2 nm
Angew. Chem. Int. Ed. 2009, 48, 8010 –8013
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Redox potential on the SHE scale
ESHE
Working
Electrode
Platinum
Electrode
H2
Acid ª 1M SolutionOx
Red
salt bridge
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Nernst Equation
�
ESHE = EO/Ro[ ]SHE +
RTnF ln
aOaR
⎛ ⎝ ⎜
⎞ ⎠ ⎟
�
EO/Ro[ ]SHE Standard redox potential
with respect to the standard hydrogen electrode
a = γ c
c oActivity : Effective concentration normalised by
the standard concentration of 1 mol·L–1
RT lnγ Activity coefficient : Mesure of the solute-solute interaction energy. γ→1 for diluted solutions
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Nernst Equation
Formal redox potential (Apparent standard)with respect to the standard hydrogen electrode
ESHE = EO/R
o /⎡⎣ ⎤⎦SHE +RTnFln cO
cR
⎛⎝⎜
⎞⎠⎟
EO/R
o /⎡⎣ ⎤⎦SHE
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Ionisation energy
Reduced state
Oxidised state+
electron at rest in vacuum
Gas Phase
Ionisationenergy
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Absolute redox potential
Reduced statein water
Oxidised state in gas phase+
electron at rest in vacuumIonisation
energy
Reduced statein the gas phase
Oxidised state in water+
electron at rest in vacuum
−ΔGhyd(R) ΔGhyd(O)
F EO/R[ ]abs
F EO/R[ ]abs = ΔGhyd(O) − ΔGhyd(R) + EI
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ET at ITIES
O1 + R2 R1 + O2
O1
R2
R1
O2
Water
Organic
Hydrophilic
Lipophilic
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Bulk ET reactionO1 + R2 R1 + O2
The standard Gibbs energy of the reaction
Ce4+ + Fe2+ Ce3+ + Fe3+
Eox/red
o⎡⎣ ⎤⎦SHEFe3+ /Fe
2+
Ce4+ /C
e3+
H+ /H
2
0 0.77 1.44Volt
ΔGro
ΔGr
o = nF EO2 /R2o⎡⎣ ⎤⎦SHE − EO1 /R1
o⎡⎣ ⎤⎦SHE( )
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Non-aqueous redox potential scale
Standard redox potential in the organic phasevs a standard hydrogen electrode
oxo + n/2 H
2 n H
+ + red
o
EO/R
o⎡⎣ ⎤⎦SHE
o= µO
o ,o − µR o ,o − nµ
H+ o ,w + n
2 µH2 o⎡
⎣⎤⎦ / F
Difficult to assemble an aqueous reference electrode for an organic solution. Difficult to determine the liquid junction potential.
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Ferrocene scale
Ferrocene
Decamethylferrocene
EDCMFc+ /DCMFc
o⎡⎣ ⎤⎦Fc+ /Fc
o= − 0.6 V
Fe
Fe
15
10
5
I / n
A
1.00.80.60.40.20.0-0.2E/ V
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Ferrocene on SHE scale
EFc+ /Fc
o⎡⎣ ⎤⎦SHE
o= µ
Fc+ o ,o − µ
Fc o ,o( ) − µ
H+ o ,w – 1
2 µH2 o( )⎡
⎣⎢⎤⎦⎥ / F
Standard redox potential in the organic phase
Standard redox potential in the aqueous phase
EFc+ /Fc
o⎡⎣ ⎤⎦SHE
w= µ
Fc+ o ,w − µ
Fc o ,w( ) − µ
H+ o ,w – 1
2 µH2 o( )⎡
⎣⎢⎤⎦⎥ / F
Scale matching
EFc+ /Fc
o⎡⎣ ⎤⎦SHEo
= EFc+ /Fco⎡⎣ ⎤⎦SHE
w+ΔG
tr,Fc+o ,w→o − ΔG
tr,Fco ,w→o
F
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Water / 1,2-dichloroethane
EDCMFc+ /DCMFc
o⎡⎣ ⎤⎦SHE
o= EDCMFc+ /DCMFc
o⎡⎣ ⎤⎦Fc+ /Fc
o+ EFc+ /Fc
o⎡⎣ ⎤⎦SHE
o= 0.04 V
Decamethylferrocene
ΔG
tr,Fc+o ,water→DCE = 0.5 ± 0.5 kJ·mol–1
ΔGtr,Fco ,water→DCE = − 24.5 ± 0.5 kJ·mol–1
Scale matching
EFc+ /Fc
o /⎡⎣ ⎤⎦SHEwater
= 0.380V EFc+ /Fc
o⎡⎣ ⎤⎦SHEDCE
= 0.64 ± 0.05V
EFc+ /Fc
o⎡⎣ ⎤⎦SHEDCE
= EFc+ /Fco⎡⎣ ⎤⎦SHE
water+ΔG
tr,Fc+o ,water→DCE − ΔG
tr,Fco ,water→DCE
F
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Biphasic ET reaction
ΔGr
o = nF EO2 /R2o⎡⎣ ⎤⎦SHE
o− EO1 /R1
o⎡⎣ ⎤⎦SHEw⎡
⎣⎢⎤⎦⎥
Ferrocene scale 0 Volt
Fc+/FcDMFc+/DMFc
–0.6 Eox/red
o⎡⎣ ⎤⎦FcDCE
0.64SHE potential scale 0.04 Eox/red
o⎡⎣ ⎤⎦SHEDCE
SHE potential scale Eox/red
o⎡⎣ ⎤⎦SHEFe3+ /Fe
2+
H+ /H
2
0 0.77Volt
Fe(C
N)63– /Fe
(CN)6
4–
0.36
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Nernst equationO1 R1
O2R2
Aqueous phase
Organic phase %µR1w + %µO2
o = %µO1w + %µR2
o
At equilibrium
Nernst equation ΔowφET = Δo
wφETo +
RTnFln
aR1w aO2
o
aO1w aR2
o
⎛
⎝⎜⎜
⎞
⎠⎟⎟
Standard Galvani potential differencefor Heterogeneous Electron Transfer (HET)
Δo
wφETo = µR1
o ,w + µO2o ,o − µO1
o ,w − µR2 o ,o⎡
⎣⎤⎦ / nF
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Potential control of the reaction
ΔowφET > Δo
wφETo
Nernst equation ΔowφET = Δo
wφETo +
RTnFln
aR1w aO2
o
aO1w aR2
o
⎛
⎝⎜⎜
⎞
⎠⎟⎟
O1 + R2 R1 + O2
ΔowφET < Δo
wφETo O1 + R2 R1 + O2
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Ferrocene oxidation by Ferricyanide
0 Volt
Fc+/FcDMFc+/DMFc
–0.6
0.640.04
Fe3+ /Fe
2+
H+ /H
2
0 0.77Volt
Fe(C
N)63– /Fe
(CN)6
4–
0.36
FeIII
Fc
FeII
Fc+
-80
-60-40
-200
2040
0.40.20.0-0.2
106 i
/ A
TPA+
ET
Δowφ / V
Ag AgCl10 mM BATB
0.4 mM Fc
1.5 M Li2SO4
0.1 M Fe(CN)63–
0.01 M Fe(CN)64–
0.01 M LiCl1 mM BACl Ag2SO4 AgCell:
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Unique potential scale
O2 + e– → O2•– E o⎡
⎣⎤⎦SHE
w= –0.330 V E o⎡
⎣⎤⎦SHE
o≈ −0.81 V
O2 + 2H+ + 2e– → H2O2 E o⎡⎣
⎤⎦SHE
w= 0.695 V E o⎡
⎣⎤⎦SHE
o= 1.12V
O2 + 4H+ + 4e– → 2H2O E o⎡⎣
⎤⎦SHE
w= 1.229 V E o⎡
⎣⎤⎦SHE
o= 1.73V
H2O2 + 2H+ + 2e– → 2H2O E o⎡⎣
⎤⎦SHE
w= 1.763 V E o⎡
⎣⎤⎦SHE
o= 2.31V
E o⎡⎣
⎤⎦SHE
w
E o⎡⎣
⎤⎦SHE
o
O2+ e
– →O 2•–
O2+ 2H
+ + 2e– →
H 2O 2
O2+ 4H
+ + 4e– →
2H2O
H2O 2+ 2H
+ + 2e– →
2H2O
H+ +e
– →1
2H 2
Fc+
+e– →
Fc0 1 2
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Proton coupled electron transfer
Water
1,2-dichloroethane
Private communication:Prof. I. Benjamin
O2 or CO2
Protons
Donors
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CoAP + O2 + Fc
! !
Ag AgCl
DCE Water
Ag2SO4 Ag
Water Ref
0.01 M LiCl1 mM BACl
5 mM BATB25 μM CoAP
5 mM Fc
0.01 M LiClHCl pH=2
No CoAP
No O2
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Influence of pH
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CoAP Shake flask
!(a) Photographs of two-phase reactions.Aqueous phase: 5 mM LiTB + 10 mM HCl.DCE phase: 1 mM Fc + 5 mM BATB (flask 1), 1 mM Fc + 20 M CoAP + 5 mM BATB (flask 2) and 20 M CoAP + 5 mM BATB (flask 3). The upper left inset shows the colors of three DCE solutions before contacting with the water solution(b) The isolated top aqueous solutions with added excess NaI; (c) Further addition of starch to the flasks shown in (b)(d) A 4-hour-two-phase reaction in the glovebox with the same solution composition as the flask 2 in (a).
FcBATB
FcCoAPBATB
CoAPBATB
FcCoAPBATBNo O2
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DCE
Water
CoAP cycle - Ferrocene
Fc+ ET2 Fc
CoII
H+CoIII
OH+
O
H2O2
CoIII
H+
O2
CoIII
O•
OTautomery
Fc+
ET1
Fc
CoIII
OHO
Tautomery
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Cobalt porphine
N
N N
N
Co
!
•Catalyst for oxygen reduction
reported by F. Anson
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Voltammetry
10
5
0
-5
j /
µA
cm
-2
0.40.20.0-0.2
!o
w" / V
Blank
CoP
Fc
CoP+Fc
a
Cl -
H +
/Li +
Fc +
PCET
!
Ag AgCl
DCE Water
AgCl Ag
Water Ref
0.01 M LiCl1 mM BACl
5 mM BATB50 μM CoP
5 mM Fc
0.01 M LiClHCl pH=2
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Oxygen concentration dependence
Ag AgCl
DCE Water
AgCl Ag
Water Ref
0.01 M LiCl1 mM BACl
5 mM BATB50 μM CoP
5 mM Fc
0.01 M LiClHCl pH=2
20
10
0
j /
µA
cm
-2
0.40.20.0-0.2
!o
w" / V
b Air-Saturated N2 -Atmosphere
O2-Saturated
!
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pH dependence
Ag AgCl
DCE Water
AgCl Ag
Water Ref
0.01 M LiCl1 mM BACl
5 mM BATB50 μM CoP
5 mM Fc
0.01 M LiClHCl pH=1, 2, 3
10
5
0
-5
j / µ
A c
m-2
0.40.20.0-0.2
!o
w" / V
Fc+
Fc+
PCET
!
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CoP concentration dependence
Ag AgCl
DCE Water
AgCl Ag
Water Ref
0.01 M LiCl1 mM BACl
5 mM BATBx μM CoP5 mM Fc
0.01 M LiClHCl pH=2
10
5
0
-5
j /
µA
cm
-2
0.40.20.0-0.2
!o
w" / V
a 0
10
25
50
75 µM
Fc+
Fc+
PCET
!
4
2
0
j 0.3
5V
/ µ
A c
m-2
806040200
ccoP
/ µM
b
!
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Fc concentration dependence
Ag AgCl
DCE Water
AgCl Ag
Water Ref
0.01 M LiCl1 mM BACl
5 mM BATB50 μM CoP
x mM Fc
0.01 M LiClHCl pH=2
10
0
j /
µA
cm
-2
0.40.20.0-0.2
!o
w" / V
a
0.2
0.5
1.0
5.0 mM
Fc+
PCET
!
8
6
4
2
0
j 0.3
2V
/ µ
A c
m-2
20151050
cFc
/ mM
b
!
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H2O2 production
!
2.0
1.5
1.0
0.5
0.0
Ab
s
700600500400
! / nm
a
CoP385
(Co-O2)P
402
Fc, 439
Fc+, 620
!
1
23
1.5
1.0
0.5
0.0
Abs
500400300
! / nm
I3
-
b286
352
!
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Donor dependence
Ag AgCl
DCE Water
AgCl Ag
Water Ref
0.01 M LiCl1 mM BACl
5 mM BATB50 μM CoP
5 mM FcA, Fc, DFc
0.01 M LiClHCl pH=2
10
0
-10
j /
µA
cm
-2
0.40.20.0-0.2
!o
w" / V
PCETDFc+/Fc
+
DFc+/Fc
+
a
!
-2.0
-1.5
-1.0
log
(j,
A m
–2)
0.40.30.20.1
!o
w" / V
b
!
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Mechanism
!
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Free base porphyrin
•No adsorption at ITIES!
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H2FAP catalysis - O2 reduction
0.8
0.6
0.4
0.2
0.0
A
150010005000
time / s
H2FAP + HTB + Fc
H2FAP + TFA + Fc
Fc only
!Absorbance at λ = 620 nm to monitor ferrocenium concentration.Initial conditions:0 or 50 μM H2FAP, 2.12mM HTB as shown, 0.1 M TFA as shown and 4.94 mM ferrocene.
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Conclusion
•Voltammetry at ITIES is useful tool to study charge transfer reactions
•Surface tension measurements provide a direct access to the molecular composition of the interface
•“Electrochemistry in a bottle”
•Molecular electrocatalysis offers new routes for interfacial reactivity
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Questions :
• Ion transfer : Transport or reaction?
• Electron transfer : Potential dependent kinetics ?
• Please explain : Phase transfer Catalysis
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Liquid-liquid interfaces
• Interfacial structure
• Polarised liquid-liquid interfaces
• Electrocapillary phenomena
• Charge transfer reactions
• Photocurrent
• Nanoparticle adsorption - Plasmonics
• Artificial photosynthesis
Saturday, September 18, 2010