E. W.-G. Diau, C.-Y. Yeh et al.
Table 1. Electronic absorption and emission data for porphyrins 1–12.[a]
Porphyrin
Absorption
Emission
lmax [nm]
lmax [nm] (e [103 mꢀ1 cmꢀ1])
1
2
3
4
5
6
7
8
445 (282), 579 (9.5), 636 (24.8)
445 (231), 582 (8.2), 632 (19.4)
451 (117), 680 (30.6)
653[b]
651[b]
707[c]
454 (283), 668 (51.0)
687[c]
448 (194), 601 (8.3), 654 (29.7)
430 (616), 565 (20.7), 605 (14.7)
455 (106), 571 (7.1), 636 (8.4)
451 (129), 564 (11.7), 613 (11.1)
434 (326), 567 (12.9), 607 (7.7)
433 (409), 566 (16.3), 609 (10.7)
442 (348), 574 (21.0), 618 (13.0)
444 (375), 575 (25.1), 618 (16.3)
687[c]
617, 660[b]
659[d]
666[d]
631[b]
630[b]
635[b]
635[b]
9
10
11
12
[a] Absorption and emission data were measured for (CH2Cl2/pyridine=
100:1) solutions at 298 K. The excitation wavelengths were [b] 550 nm,
[c] 650 nm, and [d] 600 nm.
Figure 2. Cyclic voltammograms of a) 1, b) 4, and c) 6 in THF containing
0.1m TBAPF6.
The electron-withdrawing property of the carboxyl an-
choring group through a PE linker in 1 has no significant in-
fluence on its oxidation potential. The first oxidation is shift-
ed only slightly by 40 mV to the positive relative to porphy-
rin 6; we attribute this property to the strong electronic in-
teraction between the carboxyl group and the porphyrin
macrocycle through the PE linker, which allows positive
charge to delocalize over the PE unit upon oxidation. The
effect of the electron-withdrawing ability of the carboxyl PE
linker on the oxidation potential is thus partially compensat-
ed by the charge delocalization. In contrast, the significant
shift of the first reduction of 1 versus 6 by 170 mV to the
positive indicates that both electron withdrawal and elec-
tronic delocalization influence the reduction potential in the
same direction. A similar trend of the reduction potentials
of 4 was also observed. As shown in Table 2, the half-wave
potentials for the first abstraction of an electron from the
porphyrin ring, except for 3 and 5, are in a small range
+0.96 to +1.05 V, whereas those for the first reduction span
a large range of ꢀ1.06 to ꢀ1.41 V. The electrochemical
HOMO–LUMO energy gap decreases as the p conjugation
is extended, consistent with red shifts of both Soret and
Q bands in the electronic absorption spectra. The potential
for the first oxidation of porphyrins corresponds to the
HOMO level. The LUMO energy level is predictable from
the HOMO and the absorption threshold. In our new por-
phyrins, the LUMO levels are more negative than the con-
duction-band edge (ꢀ0.5 V vs. normal hydrogen electrode)
and the HOMO levels are more positive than the oxidation
systematically with increasing p conjugation.[29] A similar
trend was observed in the fluorescence spectra.
We investigated the electrochemical properties of these
porphyrins with cyclic voltammetry. Because the solubility
of some of these porphyrins in CH2Cl2 was poor, we dis-
solved them in THF. In general, two oxidations and two re-
ductions are expected for a zinc porphyrin under our elec-
trochemical conditions. For some porphyrins, the oxidation
waves were irreversible under ambient conditions; the elec-
trochemical reactions of these porphyrins were therefore in-
vestigated at low temperatures. The measured oxidation and
reduction potentials of these porphyrins are listed in
Table 2. Figure 2 shows examples of cyclic voltammograms
Table 2. Electrochemical data for porphyrins 1–12.[a]
Porphyrin
Oxidation E1/2 [V]
Reduction E1/2 [V]
1
2
3
4
5
6
7
8
+1.00
ꢀ1.19
+1.05[b]
ꢀ1.24
+0.86, +1.02
ꢀ1.08
+0.98
ꢀ1.06
+0.87[a] (+0.79, +1.05, +1.73)[c]
ꢀ1.11[a] (ꢀ1.02)[c]
ꢀ1.36
+0.96
+1.03
+0.98
+1.04[b]
+0.95
+1.00
+0.99
ꢀ1.21[b]
ꢀ1.36[b]
ꢀ1.41
9
10
11
12
ꢀ1.35
ꢀ1.36[b]
ꢀ1.40[b]
[a] Electrochemical measurements were performed at ꢀ208C in THF
containing TBAPF6 (0.1m) as supporting electrolyte. Potentials [V] are
reported versus Ag/AgCl and reference to the ferrocene/ferrocenium
(Fc/Fc+) couple (THF, ꢀ208C, +0.57 V). [b] Irreversible process Epa or
Epc. [c] Electrochemical measurements were performed at ꢀ208C in
CH2Cl2 containing TBAPF6 (0.1m) as supporting electrolyte.
ꢀ
potential for Iꢀ/I3 , which meets the requirement for effec-
tive electron injection and dye regeneration in a DSSC
system.[1–3]
The cyclic voltammogram of 3 shows that the first and
second 1ꢀeꢀ oxidations, E
1/2ACHTUNGTERNNUG(ox1)=+0.86 and E1/2ACHTUTGNREN(NUGN ox2)=+
1.02 V, overlap, which one can resolve by using differential
pulse voltammetry (Figure 3). The first reduction of the por-
phyrin ring was observed at ꢀ1.08 V. The oxidation centers
are identified by comparison with those of the correspond-
ing triarylamine and porphyrin components, with reduction
at E1/2 =+0.91 and +0.99 V, respectively. The first oxidation
for porphyrins 1, 4, and 6 in THF containing tetrabutylam-
monium hexafluorophosphate (TBAPF6; 0.1m) at ꢀ208C.
For porphyrin 1, the first oxidation at E1/2ACTHUNRTGNEUNG(ox1)=+1.00 V
and the first reduction at E
N
1406
ꢀ 2009 Wiley-VCH Verlag GmbH & Co. KGaA, Weinheim
Chem. Eur. J. 2009, 15, 1403 – 1412