S. Khene et al. / Electrochimica Acta 56 (2010) 706–716
715
Fig. 6A shows that for -NiPc(OH)4 the frontier MO (LUMO)
is localized on the ligand and partly on the Ni atom. Also Fig. 6
shows that the LUMO of -NiPc(OH)4 appear as an antibonding
pi orbital (*) and the LUMO of -Ni(O)Pc(OH)4 appear as an
antibonding sigma orbital (*). When -NiPc(OH)4 interacts with
p-chlorophenol (Fig. 6B) the LUMO shows extensive localization
of MO mainly on the Pc ligand with some on the Ni atom. For
-Ni(O)Pc(OH)4 in the presence p-chlorophenol (Fig. 6D), there
is less extensive delocalization on the Pc ring compared to when
-NiPc(OH)4 interacts with p-chlorophenol. This suggests that for
-NiPc(OH)4 the ring is more extensively involved in the oxida-
tion of 4-chlorophenol when compared to -Ni(O)Pc(OH)4. When
adsorbed specie (without cycling or conditioning in 0.1 mol dm−3
NaOH) are employed for the catalytic oxidation of 4-chlorophenol,
the oxidation potentials are observed at different values com-
4-chlorophenol compared to -NiPc(OH)4 in terms of catalytic cur-
rents (Fig. 4).
6. Conclusions
NiPc
derivatives:
poly-␣-Ni(O)Pc(OH)4-OPGE,
poly-␣-
Ni(O)Pc(OH)8-OPGE and poly--Ni(O)Pc(OH)4-OPGE and their
adsorbed counterparts (ads-␣-NiPc(OH)4-OPGE, ads-␣-NiPc(OH)8-
OPGE and ads--NiPc(OH)4-OPGE) were studied for their catalytic
activity towards the oxidation of p-chlorophenol. In terms of
electrocatalytic activity, poly-␣-Ni(O)Pc(OH)4-OPGE and poly-
␣-Ni(O)Pc(OH)8-OPGE, showed evidence for the involvement
of the NiIII/NiII couple in the oxidation of 4-chlorophenol, but
the catalytic currents were less than those of the bare OPGE.
Poly--Ni(O)Pc(OH)4-OPGE showed higher currents than the bare
OPGE showing good electrocatalytic activity compared to for poly-
␣-Ni(O)Pc(OH)4-OPGE and poly-␣-Ni(O)Pc(OH)8-OPGE. We have
shown, using interaction energy values that when p-chlorophenol
interacts better with -NiPc(OH)4 than -Ni(O)Pc(OH)4, hence the
former is a better catalyst in terms of lowering of overpotential.
We have used the condensed Fukui function to determine the
reactive sites where electron transfer would take place between
p-chlorophenol and the nickel phthalocyanine complexes. We
have theoretically rationalised the interaction of p-chlorophenol
with nickel phthalocyanine complexes.
pared to when the electrode has been cycled in 0.1 mol dm−3
,
suggesting that there are different catalytic sites involved. Fol-
reaction.
The oxidation process of p-chlorophenol is viewed as a nucle-
ophilic attack of -NiPc(OH)4 by p-chlorophenol. According to Eqs.
condensed Fukui function (f(r) and fA+k), one needs to determine the
electron density of the molecule and the charges of the atoms in the
molecule. In this work we have used the Mulliken gross population
analysisfor qAk, Eqs. (15)and (18) to determine the condensedFukui
function and the condensed local softness.
Acknowledgements
Tetra substituted phthalocyanine derivatives contain a mix-
ture of four possible structural isomers, with the position of the
erally substituted derivatives and at 1(4), 6(11), 15(18) and 22(25)
for non-peripherally substituted derivatives (see numbering in
Fig. 7). However for the purposes of the present calculations, the
substituents have been fixed to one position on each benzene
metallated. Comparing Fig. 7A and B, we see that the condensed
local softness (less reactive) values for carbons at 5, 12, 19, 26
(red region) lie below the ones at 7, 14, 21, 28 (blue regions),
(red region) have increased (more reactive) to a point where
they have surpassed the values for carbons at 7, 14, 21, 28 (blue
regions).
This work was supported by the Department of Science and
Technology (DST) and National Research Foundation (NRF) of South
Africa through DST/NRF South African Research Chairs initiative for
Professor of Medicinal Chemistry and Nanotechnology and Rhodes
University.
References
[1] T. Nyokong, in: J.H. Zagal, F. Bedioui, J.-P. Dodelet (Eds.), N4-Macrocyclic Metal
Complexes, Springer, United States of America, 2006.
[2] D.R. Trackley, G. Dent, W.E. Smith, Phys. Chem. Chem. Phys. 2 (2001) 1419.
[3] M.S. Ureta-Zanartu, P. Bustos, C. Berrios, M.C. Diez, M.L. Mora, C. Guitierrez,
Electrochim. Acta 47 (2002) 2399.
[4] S. Griveau, F. Bedioui, Electroanalysis 13 (2001) 253.
[5] G. Heimel, L. Romaner, J.-L. Bredas, E. Zojer, Phys. Rev. Lett. 96 (2006) 196806.
[6] R.G. Parr, W. Yang, J. Am. Chem. Soc. 106 (1984) 4049.
[7] R.G. Parr, R.A. Donnelly, M. Levy, W.E. Palke, J. Chem. Phys. 68 (1978) 3801.
[8] R.G. Parr, R.G. Pearson, J. Am. Chem. Soc. 105 (1983) 7512.
[9] M.S. Ureta-Zanartu, A. Alarcon, C. Berrios, G.I. Cardenas-Jiron, J. Zagal, C. Gutier-
rez, J. Electroanal. Chem. 580 (2005) 94.
Fig. 7A and B suggests that when Ni is inserted into the
ring, the carbon atoms at 5, 12, 19, 26 (red region) are acti-
vated differently compared to unmetallated. The 5, 12, 19, 26
(red region) carbons are situated on the side where the OH is
substituted and show greater local softness (hence greater reac-
tivity). The carbons at 7, 14, 21, 28 (blue regions) are situated
bons). This suggests that even though the OH substituents have
no effect on the bond length between the Ni atom and the N
[14], it has some distabilization effect on the 5, 12, 19, 26 car-
bons for -NiPc(OH)4. Fig. 7D shows that for unsubstitured NiPc
all the carbons are activated equally compared to -NiPc(OH)4.
Fig. 7C suggests that, for ␣-NiPc(OH)8, the Ni atom is made softer
or more reactive relative to all other atoms. The Fukui plots of
␣-NiPc(OH)8 suggests that if this complex was to be used for elec-
tro catalytic oxidation of p-chlorophenol, catalysis through the
nickel atom would be favoured over the ring. Fig. 7E shows the
Fukui plots of ␣-NiPc(OH)4, showing that only the carbons are
activated. It is observed experimentally that ␣-NiPc(OH)4 and ␣-
NiPc(OH)8 shows bad catalytic activity towards the oxidation of
[10] M.S. Ureta-Zan˜artu, C. Berríos, J. Pavez, J. Zagal, C. Gutíerrez, J.F. Marco, J. Elec-
troanal. Chem. 553 (2003) 147.
[11] C. Berríos, M.S. Ureta-Zan˜artu, C. Gutíerrez, Electrochim. Acta 53 (2007) 792.
[12] P.W. Ayres, R.G. Parr, J. Am. Chem. Soc. 122 (2000) 2010.
[13] M. Berkowitz, J. Am. Chem. Soc. 109 (1987) 4823.
[14] S. Khene, K. Lobb, T. Nyokong, Inorg. Chim. Acta 362 (2009) 5055.
[15] R.G. Pearson, Acc. Chem. Res. 26 (1993) 250.
[16] B.E. Douglas, D.H. McDaniels, J.J. Alexander, Concept and Models of Inorganic
Chemistry, John Wiley and Sons, Inc., New York, 1994, pp. 193–195.
[17] Y. Li, J.N.S. Evans, J. Am. Chem. Soc. 117 (1995) 7756.
[18] F. Mendez, J.L. Gazquez, J. Am. Chem. Soc. 116 (1994) 9298.
[19] K. Flurchick, L. Bartolotti, J. Mol. Graph. 13 (1995) 10.
[20] M.J. Frisch, G.W. Trucks, H.B. Schlegel, G.E. Scuseria, M.A. Robb, J.R. Cheese-
man, J.A. Montgomery Jr., T. Vreven, K.N. Kudin, J.C. Burant, J.M. Millam, S.S.
Iyengar, J. Tomasi, V. Barone, B. Mennucci, M. Cossi, G. Scalmani, N. Rega, G.A.
Petersson, H. Nakatsuji, M. Hada, M. Ehara, K. Toyota, R. Fukuda, J. Hasegawa,
M. Ishida, T. Nakajima, Y. Honda, O. Kitao, H. Nakai, M. Klene, X. Li, J.E. Knox, H.P.
Hratchian, J.B. Cross, V. Bakken, C. Adamo, J. Jaramillo, R. Gomperts, R.E. Strat-
mann, O. Yazyev, A.J. Austin, R. Cammi, C. Pomelli, J.W. Ochterski, P.Y. Ayala, K.
Morokuma, G.A. Voth, P. Salvador, J.J. Dannenberg, V.G. Zakrzewski, S. Dapprich,
A.D. Daniels, M.C. Strain, O. Farkas, D.K. Malick, A.D. Rabuck, K. Raghavachari,
J.B. Foresman, J.V. Ortiz, Q. Cui, A.G. Baboul, S. Clifford, J. Cioslowski, B.B. Ste-
fanov, G. Liu, A. Liashenko, P. Piskorz, I. Komaromi, R.L. Martin, D.J. Fox, T. Keith,
M.A. Al-Laham, C.Y. Peng, A. Nanayakkara, M. Challacombe, P.M.W. Gill, B. John-
son, W. Chen, M.W. Wong, C. Gonzalez, J.A. Pople, Gaussian 03, Revision E.01,
Gaussian, Inc., Wallingford, CT, 2004.
[21] B.N. Achar, P.K. Jayasree, Synth. Met. 104 (1999) 101.