46
M. Flores-Jarillo et al. / Dyes and Pigments 133 (2016) 41e50
to observe both transitions separated in the same UV spectrum
there are a few cases, for example with 5- or 6-hydroxyindole [21],
in which this has been possible. Among different indole derivatives,
2-phenyl indoles are fluorescent molecules with quantum yields
larger than 0.8 [12]. On the other hand, phenyeleneethynylenes
(PEs) are fluorophores which display medium-high quantum yields
in solution [13,14] and usually have only one emitting state due to a
be considered for some selected molecules in future work. Whereas
no general feature can describe the emission behavior of the whole
series, there are some interesting observations: i) 1a, 1b show
excitonic like spectra and no significant solvatochromism as the
differences in the emission maxima and quantum yields are within
the experimental error of the determination, ii) the spectra of 1c,
1e, 1f, 1g, 1h and 1i, which are excitonic in toluene, become broader
in dichloromethane and even more in DMSO. For example, the
HHBW of 1f increases from 49 nm in toluene to 79 nm in CH2Cl2
and to 89 nm in DMSO, accordingly, the Stokes shift also increases,
iv) for all these molecules, the quantum yield decreases with the
polarity of the solvent.
p-p* electronic transition. This localized excited state makes the
maximum emission wavelength independent of the solvent. As
found in the theoretical calculations, Fig. 1, the indole and the
phenyleneethynylene are practically coplanar in the ground state
with an extended electronic delocalization.
When absorption of compounds 1a-i was studied in toluene,
dichloromethane and DMSO the absorption coefficient was high
and no significant changes in the wavelength maxima were
observed. For these compounds the main peak in the UV spectra
The Stokes shift values (Dn) in toluene are in the range of mol-
ecules that undergo geometry change after excitation [26,27], but
in general lower to those usually reported for ICT states [31].
Intramolecular charge transfer can eventually occur in DMSO, and
in particular for 1h and 1i, which is in agreement with their
observed large HHBW and Stokes shift and can explain their lower
fluorescence quantum yields found in this solvent.
(labs) is located between 330 nm and 406 nm, depending on the
overall conjugation of the molecule that in turn is modulated by the
substituents on the aryl groups. (Tables 2e4). There is a good
agreement between the experimental and simulated spectra and
between the absorption maxima collected in Table 1 (theoretical)
and 2 (experimental), theoretical values are slightly larger than
experimental ones as usually found when TDDFT simulation is
carried out. [ 26,27] On the other hand, pronounced changes in the
emission spectra of these compounds due to change in solvent
polarity were observed (Tables 2e4). For example, while compound
1c showed nearly identical UV absorption spectra in all solvents
A particular case is compound 1d, for which the fluorescence
spectrum strongly red shifts and decreases in intensity with
increasing excitation wavelength (Fig. 4). Contrary to what was
observed for the rest of the compounds, the excitation spectrum of
1d does not show the electronic transition that gives rise to the
absorption band at 403 nm. This result could be explained on the
basis that a non-emissive state is reached after excitation, perhaps
related to the nitrophenyl chromophore which by coincidence ap-
pears at the same wavelength (400e405 nm). There is overlap
between the absorption and emission spectra and then we cannot
discard that the fluorescence bands are derived from internal
charge transfer. This interpretation could explain why the emission
band shifts and the large Stokes shift; the shift of the emission band
in a very polar solvent (DMSO) and the low quantum yield found. As
pointed out previously, indoles present two excited states S1 and
(labs 363 nm in toluene, 367 nm in dichloromethane and 360 nm in
DMSO, see entry 3 in Tables 2e4), its emission spectra showed a
bathochromic shift with the polarity of the solvent (lem 416,
431 nm in toluene, 426 nm in dichloromethane and 460 nm in
DMSO). This solvatofluorochromism is in line with reported ob-
servations in indole derivatives [21e24,28]. It is worth mentioning
that solvent dependent spectral shifts of dyes are ordinarily studied
by applying the Lippert-Mataga equation [29,30]. This equation
describes the Stokes shifts as a function of the change in the dipole
moment of the dye upon excitation. Plots of the Stokes shift vs. the
polarizability function of several solvents are drawn, and the slope
of the fitted lines can give the difference between the ground and
excited state dipole moment Dmeg. When the ground state dipole
moment is known or calculated (as in our case), the excited state
dipole moment can be derived. In this paper, we used DCM, DMSO
and toluene as they are good solvents for the entire family, allowing
a quantitative and overall picture of the photophysical properties of
the molecules. Several solvents of different polarity, normally 10 to
20, are needed to build those plots. However, some of them such as
alkanes and alcohols do not dissolve any of the molecules studied in
this work, others such as THF and acetonitrile dissolve, at least
partially, some molecules but not all of them. Based on these lim-
itations, the determination of the excited state dipole moment
could not be realized at this time by Lippert-Mataga plots but will
0
ꢀ
S1 , which according to the recent model by Catalan [24] the lower
0
energy excited state S1 is highly dipolar giving a structureless
emission that shifts depending of the polarity of the medium.
However, the theoretical study of the molecules in this work
already mentioned, suggested that conjugation involves both the
indole and phenyleethynylene moieties, i.e. the indole group is not
acting as an isolated chromophore and in consequence we do not
relate entirely the behavior of these molecules to the S10 properties
of the pure indole chromophore.
Besides 1d, all of the other molecules had very high fluorescence
quantum yields (
times between 1 and 2 ns? Notably, the measured quantum yield
) for 1a, 1 b and 1c (in toluene) 1a, 1e (in dichloromethane) and
4) with monoexpontential time decay and life-
(4
1b (in DMSO) gave a value larger than 1, which for definition must
be ꢂ 1. It is important to specify that the fluorescence quantum
yield was determined by the indirect dilution method of Williams
[15] using quinine sulfate as standard and full precautions were
Table 2
Optical properties of compounds 1a-i in toluene.
Compound
Egopt [eV]
labs [nm]
ε [104 Mꢁ1cmꢁ1
]
lem [nm]
HHBWem [nm]
Dn [cmꢁ1
]
F
[%]a
t
[ns]
krad [sꢁ1
]
1a
1b
1c
1d
1e
1f
1g
1h
1i
3.31
3.29
3.04
2.69
3.27
2.94
2.89
2.98
2.99
330
333
363
397
333
382
385
360
357
3.4
3.5
4.6
3.9
4.3
4.7
2.5
3.6
2.0
382, 399
385, 403
416, 431
495
384, 402
419, 440
427, 450
422
56
56
55
75
56
49
53
63
45
4125
4056
3510
4987
3989
2312
2555
4081
4030
108.0
124.5
123.0
15.7
101.9
91.2
76.3
60.0
43.7
1.21
1.14
1.34
1.51
1.14
1.10
1.12
1.51
1.18
8.92$108
1.09$109
0.92$109
0.10$109
0.89$109
0.83$109
0.68$109
0.39$109
0.37$109
417, 435
a
The quantum yield has an accuracy of 10% of the value shown.