the target anions was not observed in the UV-Vis spectrum [see
Fig. S4(A) in the ESIw], while the fluorescence intensity was
quenched or increased upon exposure to anions. The amidic NH
groups linked directly to the HPB unit can be responsible for the
emission intensity change.8 Taking into account these results,
absorption and emission maximum shifts are induced by inter-
action between the hydroxyl group in HPB and the target anion.
Thus the presence of the hydroxyl group in HPB is crucial in
gelation as well as in detecting anionic species.
than that with fluoride anion. Therefore, we believe that gel 1 can
be used as a selective naked-eye sensor system for fluoride anion.
In conclusion, we have demonstrated the self-assembled gel
formation which showed fluorescent properties of the gelator
bearing HPB. As expected, the preferred planar conformation
of the HPB core (caused by intramolecular proton transfer)
played a crucial role in gel formation through its strong p–p
interactions. We observed strong emission from gel 1, but
observed hardly any from the solution, which was induced by
intramolecular proton transfer from the enol to the keto
tautomer. Furthermore, we have described the naked-eye
fluoride sensor which showed the gel-to-sol transition and a
visibly noticeable color change, which were induced by the
interaction between fluoride anion and amidic NH and hydro-
xyl proton in the HPB, respectively.
1
In the H NMR spectra of 1, the hydroxyl proton in HPB
showed peak splitting and the integral decreased by the addition
of fluoride anions, which indicates the possible interaction
between the hydroxyl proton in HPB and the fluoride anion
(see Fig. S5 in the ESIw). The spectral shift and decreased
integral of the proton signals from the urea moieties were due to
the deprotonation of the urea groups by fluoride anions accord-
ing to previous reports.12 In the 1H NMR spectra of 2, all NH
peaks disappeared upon addition of fluoride anion, which
means that almost all NH was deprotonated by fluoride anion.
Furthermore, the major decay time of the wet-gel state was
decreased from 7.2 to 5.8 ns after the addition of 100 equiv. of
fluoride anion [see Fig. S1(D) in the ESIw].
The naked-eye anion detection of 1 toward a number of
selected target anions was examined in a DMF/toluene mixture
as shown in Fig. 4(A). As expected, the color change was
observed only in the presence of the fluoride anion. The presence
of fluoride not only changes the color of the gel, but actively
disrupts a preformed gel, as shown in Fig. 4(B). As discussed
above, the urea moieties are able to bind with fluoride anions,
thus, the intermolecular hydrogen bonding between neighboring
urea moieties was disrupted in the presence of the fluoride
anion.13 Placing fluoride anion on top of the DMF/toluene gel
immediately produces a gel-to-sol transition with a color change
from a translucent colorless gel to a solution with a strong
greenish emission. Completion of the gel-to-sol transition oc-
curred within 30 min. Though the disruption of the gel structure
appeared in the presence of other anions, the dramatic color
change and rapid gel-to-sol transition were observed only in the
case of the fluoride anion. The acetate anion, because a high
concentration was used, exhibited a weakly greenish yellow color
with the gel-to-sol transition; however, the color was even weaker
This work was supported by Korea Science and Engineering
Foundation (KOSEF) grant funded by the Korea Govern-
ment (MOST) (No. R01-2007-000-10740-0).
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Fig. 4 Photographs of 1 (A) in DMF–toluene mixture (9.52 ꢁ 10ꢂ5
M, 1 : 58 (v/v)]; and (B) gel upon addition of 100 equiv. of each anion.
ꢀc
This journal is The Royal Society of Chemistry 2008
2366 | Chem. Commun., 2008, 2364–2366