A highly selective fluorescent chemosensor for Pb2+

Article abstract of DOI:10.1021/ja051075b

A new fluorescent sensor based on rhodamine B for Pb²⁺ was synthesized. The new fluorescent sensor showed an extreme selectivity for Pb²⁺ over other metal ions examined in acetonitrile. Upon the addition of Pb²⁺, an overall emission change of 100-fold was observed, and the selectivity was calculated to be 200 times that of Zn ²⁺. The signal transduction occurs via of reversible CHEF (chelation-enhanced fluorescence) with this inherent quenching metal ion.

Full text of DOI:10.1021/ja051075b

Published on Web 06/25/2005
A Highly Selective Fluorescent Chemosensor for Pb2+
Ji Young Kwon,† Yun Jung Jang,† Yoon Ju Lee,† Kwan Mook Kim,†,‡
Mi Sook Seo,†,‡ Wonwoo Nam,*,†,‡ and Juyoung Yoon*,†
Contribution from the Department of Chemistry and DiVision of Nano Sciences, Ewha Womans
UniVersity, 11-1 Daehyon-Dong, Sodaemun-Ku, Seoul 120-750, Korea, and CreatiVe Research
InitiatiVe Program for Biomimetic Systems, Ewha Womans UniVersity,
11-1 Daehyon-Dong, Sodaemun-Ku, Seoul 120-750, Korea
Received March 2, 2005; E-mail: jyoon@ewha.ac.kr; wwnam@ewha.ac.kr
Abstract: A new fluorescent sensor based on rhodamine B for Pb2+ was synthesized. The new fluorescent
sensor showed an extreme selectivity for Pb2+ over other metal ions examined in acetonitrile. Upon the
addition of Pb2+, an overall emission change of 100-fold was observed, and the selectivity was calculated
to be 200 times that of Zn2+. The signal transduction occurs via of reversible CHEF (chelation-enhanced
fluorescence) with this inherent quenching metal ion.
on the dansyl-tetrapeptide framework.6 On the other hand,
Introduction
Czarnik and co-workers reported a N-methyl-9-anthrylthio-
The selective binding of chemical species upon molecular
recognition can lead to large perturbations in the host environ-
ment, particularly when the guest is ionic. Since fluoroiono-
phores can provide chemical information on the ion concen-
trations, they are important subjects in metal ion analysis.1
Among the metal ions, Pb2+ is one of the important targets
because of the adverse health effects of lead exposure, particu-
larly in children.2 Even though considerable efforts have been
devoted to developing fluorescent chemosensors for various
metal ions over the last few decades,1 there have been relatively
few reports on Pb2+-selective fluorescent chemosensors. Lu et
al. utilized catalytic DNAs as a unique class of biosensors for
Pb2+.3 Ma and co-workers reported a fluorescent probe based
on the Pb2+-catalyzed hydrolysis of phosphodiester.4 Even
hydroxamic acid as a new fluorescent chemosensor for Pb2+ 7
.
In addition, some of fluorophore-appended macrocycles have
been reported.8
Rhodamine dyes have been used extensively for conjugation
with biomolecules, owing to their excellent fluorescence proper-
ties. A few rhodamine B derivatives have also been used as
fluorescent chemosensors for metal ions.9,10 Czarnik et al.
reported that rhodamine B hydrazide could be used as a
fluorescent chemodosimeter for Cu2+ 9
.
We report a new fluorescent sensor 1 based on rhodamine B
for Pb2+. The structure of compound 1 was confirmed by X-ray
crystallography in addition to NMR and mass data. The new
fluorescent sensor 1 displayed an extreme selectivity for Pb2+
in acetonitrile compared with other metal ions examined. The
signal transduction occurs via of reversible CHEF (chelation-
enhanced fluorescence) with this inherent quenching metal ion.
1H NMR, 13C NMR, IR, and the electrospary ionization (ESI)
mass data were used to explain the binding mode of 1 with
metal ions.
though the above results were excellent examples of Pb2+
-
selective fluorescent sensors, the probes were hydrolyzed by
Pb2+ in both cases, and these are irreversible processes. For a
real-time fluorescent sensor, Chen et al. used a ketoamino-
coumarine derivative bearing a azacrown binding site as a new
ratiometric fluorescent sensor for Pb2+.5 Godwin et al. also
reported a new ratiometric fluorescent sensor for Pb2+ based
Experimental Section
General Methods. Unless otherwise noted, materials were obtained
from commercial suppliers and were used without further purification.
† Department of Chemistry and Division of Nano Sciences.
‡ Creative Research Initiative Program for Biomimetic Systems.
(1) (a) Fluorescent Chemosensors for Ion and Molecular Recognition; Czarnik,
A. W., Ed.; American Chemical Society: Washington, DC, 1993. (b)
Czarnik, A. W. Acc. Chem. Res. 1994, 27, 302. (c) Fabbrizzi, L.; Poggi,
A. Chem. Soc. ReV. 1994, 197. (d) de Silva, A. P.; Gunaratne, H. Q. N.;
Gunnlaugsson, T. A.; Huxley, T. M.; McCoy, C. P.; Rademacher, J. T.;
Rice, T. E. Chem. ReV. 1997, 97, 1515. (e) Chemosensors of Ion and
Molecular Recognition; Desvergne, J.-P., Czarnik, A. W., Eds.; Kluwer
Academic Publishers: Dordrecht, The Netherlands, 1997. (f) Amendola,
V.; Fabbrizzi, L.; Lincchelli, M.; Mangano, C.; Pallavicini, P.; Parodi, L.;
Poggi, A. Coord. Chem. Chem. ReV. 1999, 190-192, 649.
(6) Deo, S.; Godwin, H. A. J. Am. Chem. Soc. 2000, 122, 174.
(7) Chae, M.-Y.; Yoon, J.; Czarnik, A. W. J. Mol. Recognit. 1996, 9, 297.
(8) (a) Xia, W.-S.; Schmehl, R. H.; Li, C.-J.; Mague, J. T.; Iuo, C.-P.; Guldi,
D. M. J. Phy. Chem. B 2002, 106, 833. (b) Padilla-Tosta, M. E.; Lloris, J.
M.; Martinez-Ma´n˜ez, R.; Marcos, M. D.; Miranda, M. A.; Pardo, T.;
Sanceno´n, F.; Soto, J. Eur. J. Inorg. Chem. 2001, 1475. (c) Addleman, R.
S.; Bennett, J.; Tweedy, S. H.; Elshani, S.; Wai, C. M. Talanta 1998, 46,
573. (d) Shen, Y.; Sullivan, B. P. J. Chem. Educ. 1997, 74, 685. (e) Beeby,
A.; Parker, D.; Williams, J. A. G. J. Chem. Soc., Perkin Trans. 2 1996,
1565.
(9) (a) Dujols, V.; Ford, F.; Czarnik, A. W. J. Am. Chem. Soc. 1997, 119,
7386.
(10) (a) Hojo, M.; Ueda, T.; Yamasaki, M.; Inoue, A.; Tokita, S.; Yanagita, M.
Bull. Chem. Soc. Jpn. 2002, 75, 1569. (b) Thorn, D. L.; Fultz, W. C. J.
Phys. Chem. 1989, 96, 1234. (c) Arbeloa, L.; Rohatgi-Mukherjee, K. K.
Chem. Phys. Lett. 1986, 128, 474. (d) Oshima, G.-I.; Nagasawa, K. Chem.
Pharm. Bull. 1970, 18, 687.
(2) Needleman, H. L. Human Lead Exposure; CRC Press: Boca Raton, FL,
1992.
(3) (a) Liu, J.; Lu, Y. J. Am. Chem. Soc. 2003, 125, 6642. (b) Li, J.; Lu, Y. J.
Am. Chem. Soc. 2000, 122, 10466.
(4) Sun, M.; Shangguan, D.; Ma, H.; Nie, L.; Li, X.; Xiong, S.; Liu, G.;
Thiemann, W. Biopolymers 2003, 72, 413.
(5) Chen, C.-T.; Huang, W.-P. J. Am. Chem. Soc. 2002, 124, 6246.
9
10.1021/ja051075b CCC: $30.25 © 2005 American Chemical Society
J. AM. CHEM. SOC. 2005, 127, 10107-10111
10107

A R T I C L E S
Kwon et al.
Scheme 1. Synthesis of 1
Flash chromatography was carried out on silica gel 60 (230-400 mesh
ASTM; Merck). Thin-layer chromatography (TLC) was carried out
using Merck 60 F254 plates with a thickness of 0.25 mm. Preparative
TLC was performed using Merck 60 F254 plates with a thickness of 1
mm.
Melting points were measured using a Buchi 530 melting point
1
apparatus, and are uncorrected. H NMR and 13C NMR spectra were
recorded using Bruker 250 or Varian 500. Chemical shifts were
expressed in ppm and coupling constants (J) in Hz. Mass spectra were
obtained using a JMS-HX 110A/110A Tandem Mass Spectrometer
(JEOL). UV absorption spectra were obtained on UVIKON 933 Double
Beam UV/vis Spectrometer. Fluorescence emission spectra were
obtained using RF-5301/PC Spectrofluorophotometer (Shimadzu).
Electrospray ionization mass (ESI-MS) spectra were performed on a
Thermo Finnigan (San Jose, CA) LCQ Advantage MAX quadrupole
ion trap instrument with samples of metal complexes.
1 (RBDPA-1). A solution of rhodamine B base (1.0 g, 2.3 mmol)
in 1,2 dichloromethane (12 mL) was stirred, and phosphorus oxychlo-
ride (0.6 mL) was added dropwise over 5 min. The solution was
refluxed for 4 h. The reaction mixture was cooled and evaporated in
vacuo to give rhodamine B acid chloride, which was not purified but
treating rhodamine B with POCl3,4a which was followed without
purification by (2-aminoethyl)bis(2-pyridylmethyl)amine. After
column chromatography using CHCl3:MeOH (9:1, v/v), 1 was
obtained in a 42% yield (Scheme 1).
1
confirmed with the reported H NMR.9
A single crystal of 1 was grown from a CHCl3/CH3CN
solution and was characterized using X-ray crystallography
(Figure 1). The crystal structure clearly represents the unique
spirolactam-ring formation. Even though the crystal and mo-
lecular structures of several fluoran-based color formers by
single-crystal X-ray diffraction analysis have been reported,12
as far as we are aware, the X-ray structure of the rhodamine B
derivative bearing the lactam moiety has not been reported.
The crude acid chloride was dissolved in acetonitrile (125 mL) and
added dropwise over 5 h to a solution of (2-aminoethyl)bis(2-
pyridylmethyl)amine11 (1.1 g, 4.6 mmol) in acetonitrile (50 mL) at room
temperature. The reaction mixture was then refluxed for 1 h. After the
solvent was evaporated under reduced pressure, the crude product was
purified by column chromatography (CHCl3:MeOH ) 9:1, v/v) to give
1
the 643 mg of 1 (yield; 42%): mp 56-59 °C.; H NMR (CDCl3) δ
8.44 (d, 2H, J ) 4.8 Hz), 7.87 (t, 1H, J ) 2.9 Hz), 7.57 (t, 1H, J ) 7.7
Hz), 7.41 (m, 4H), 7.06 (m, 3H), 6.35 (m, 4H), 6.20 (dd, 2H, J ) 8.8
and 2.6 Hz), 3.69 (s, 4H), 3.34 (m, 10H), 2.38 (t, 2H, J ) 7.9 Hz),
1.16 (t, 2H, J ) 7.0 Hz);13C NMR (CDCl3) δ 168.4, 159.3, 153.9,
153.6, 149.8, 137.5, 132.7, 131.6, 129.2, 128.4, 126.3, 124.2, 123.4,
123.1, 122.3, 108.6, 108.4, 105.8, 98.3, 65.3, 60.1, 52.6, 44.8, 38.6,
14.5; HRMS (FAB) m/z ) 667.3755 (M + H)+, calcd for C42H47N6O2
) 667.3761.
The perchlorate salts of Ag+, Ca2+, Cd2+, Co2+, Cs+, Cu2+
,
Hg2+, K+, Li+, Mg2+, Mn2+, Na+, Ni2+, Pb2+, Rb+, and Zn2+
ions were used to evaluate the metal ion binding properties of
1. Stock solutions (1 mM) of the perchlorate salts of the metal
ions in acetonitrile were prepared. A stock solution of the host
(0.1 mM) in acetonitrile was also prepared. The test solutions
were prepared by placing 4-40 µL of the probe stock solution
into a test tube, adding the appropriate aliquot of each metal
stock, and diluting the solution to 4 mL with acetonitrile. For
all the measurements, excitation wavelength was 510 nm, and
both the excitation and emission slit widths were 5 nm.
Preparation of Fluorometric Metal Ion Titration Solutions. Stock
solutions (1 mM) of the perchlorate salts of Ag+, Ca2+, Cd2+, Co2+
,
Cs+, Cu2+, Hg2+, K+, Li+, Mg2+, Mn2+, Na+, Ni2+, Pb2+, Rb+ and Zn2+
in acetonitrile were prepared. Stock solution of host (0.1 mM) was
also prepared in acetonitrile. Test solutions were prepared by placing
4-40 µL of the probe stock solution into a test tube, adding an
appropriate aliquot of each metal stock, and diluting the solution to 4
mL with acetonitrile.
All titration studies were conducted using a 1 µM concentra-
tion of 1. Using these metal ions (100 equiv), 1 showed a large
CHEF effect only with Pb2+, even though there was a relatively
small CHEQ effect with Cu2+ and Zn2+ (Figure 2). Figure 3
shows the fluorescent emission changes of 1 upon the addition
of Pb2+ ions. As shown in Figures 2 and 3, the addition of Pb2+
and Zn2+ caused a significant red shift (∼30 nm). From the
fluorescent titrations, the association constants for Pb2+ and Zn2+
were calculated to be 195000 and 900 M-1, respectively (errors
<10%).13 The selectivity for Pb2+ over Zn2+ was more than
over 200 times. An overall emission change of 100-fold was
observed for Pb2+. Furthermore, there was no significant change
in the association constant for Pb2+ when excess Zn2+ (0.1 mM)
was present. On the other hand, upon the addition of Cu2+, 1
displayed a CHEF effect without a red shift. As shown in Figure
2, Li+ also caused a similar but smaller fluorescence change to
For all measurements, excitation wavelength was 510 nm. Both
excitation and emission slit widths were 5 nm.
Electrospray Ionization Mass (ESI-MS). The electrospray ioniza-
tion mass (ESI-MS) spectrum of 1 was obtained by direct introduction
of the solution of samples (10 µM) in CH3CN into the source at 25
µL/min using a syringe pump. The spray voltage of the spectrometer
was set at 5 kV, and the capillary temperature, at 150 °C.
X-ray Data. All the X-ray data were collected on a SMART APEX
CCD equipped with a Mo X-ray tube at the ambient temperature.
Crystal data of 1: monoclinic, P21 (No. 4), Z ) 2, a ) 11.896(3) Å,
b ) 11.812(3) Å, and c ) 12.988(3) Å, â ) 90.592(4)°, V ) 1824.8-
(7) Å3, µ ) 0.076 mm-1, dcalc ) 1.214 g/cm3, R1 ) 5.81% and wR2
) 11.62% for 1946 unique reflections and 451 variables. The structure
solution and refinement of the data were handled with the SHELXS-
86 and SHELXL-97 programs.
Cu2+
.
Results and Discussion
(12) (a) Okada, K. J. Mol. Struct. 1996, 380, 235. (b) Ribs, G.; Weis, C. D.
Dyes Pigm. 1991, 15, 107 and 165.
(13) (a) Conners, K. A. Binding Constants; Wiley: New York, 1987. (b)
Association constants were obtained using the computer program ENZFIT-
TER, available from Elsevier-BIOSOFT, 68 Hills Road, Cambridge CB2
1LA, United Kingdom.
(2-Aminoethyl)bis(2-pyridylmethyl)amine was synthesized
according to the published procedure.11 1 was synthesized by
(11) Schatz, M.; Leibold, M.; Foxon, S. P.; Weitzer, M.; Heinemann, F. W.;
Hampel, F.; Walter, O.; Schindler, S. Dalton Trans. 2003, 1480.
9
10108 J. AM. CHEM. SOC. VOL. 127, NO. 28, 2005

+
Selective Fluorescent Chemosensor for Pb2
A R T I C L E S
Figure 1. Side and top view of X-ray crystal structure of 1.
Figure 4. UV absorption changes of 1 (0.1 mM) upon addition of Pb2+ in
acetonitrile.
Figure 2. Fluorescent emission changes of 1 (1 µM) upon addition of Ag+,
Ca2+, Cd2+, Co2+, Cs+, Cu2+, Hg2+, K+, Li+, Mg2+, Mn2+, Na+, Ni2+
Pb2+, Rb+, and Zn2+ (100 equiv) in acetonitrile (excitation at 510 nm).
,
calculated as 52% by using perylene as a reference.14 1 displayed
a similar UV enhancement (∼20-fold) when Zn2+ was added
to acetonitrile. On the other hand, when Cu2+ was added, the 1
did not display a new peak around 550 nm, and only broad
absorption increase was observed around 450 nm (see Support-
ing Information).
1
Figure 5 shows the partial H NMR spectra of 1 upon the
addition of Zn(ClO4)2 (2 equiv). The NMR peaks were assigned
1
on the basis of the H-1H COSY spectrum (see Supporting
Information).
For example, upon the addition of 2 equiv of Zn2+, the Ha
and Hc on the pyridine ring in 1 showed relatively large
downfield shifts (Ha, ∆δ ) 0.44 ppm; Hc, ∆δ ) 0.54 ppm).
The carbonyl carbon peak in the 13C NMR spectra moved
from 167.5 to 171.5 ppm in CD3CN:CDCl3 (9:1, v/v) when 1.2
equiv of Zn(ClO4)2 was added (see Supporting Information).
The cleavage of the lactone ring in the fluoran-based dye was
reported and explained on the basis of the changes in the 13C
NMR spectrum.10a,14 In the case of the fluoran-based dye, the
spiro carbon in the lactone ring moiety appeared at ap-
proximately δ 75-85 ppm and moved to δ ∼160 ppm in the
Figure 3. Fluorescent titrations of 1 (1 µM) upon addition of Pb2+ in
acetonitrile (excitation at 510 nm).
There was also a large enhancement (∼120-fold) in the UV
absorption (λmax ) 553 nm) of 1 upon the addition of Pb2+, as
shown in Figure 4. The fluorescence quantum yield was
(14) Cheng, Y.; Ma, B.; Wudl, F. J. Mater. Chem. 1999, 9, 2183.
9
J. AM. CHEM. SOC. VOL. 127, NO. 28, 2005 10109

A R T I C L E S
Kwon et al.
1
Figure 5. Partial H NMR (250 MHz) of 1 (2 mM) in CD3CN. (a) 1 only; (b) 1 + 2 equiv of zinc(II) perchlorate.
Figure 6. Infrared spectra of 1 (a), 1 with Zn(ClO4)2 (b), 1 with Pb(ClO4)2 (c), and 1 with Cu(ClO4)2 (d).
Figure 7. ESI mass spectra of 1 with Pb(ClO4)2 (a) and 1 with Zn(ClO4)2 (b).
lactone ring-opened structure.10a,15 The spiro carbon in 1
appeared at δ 64.7 ppm in CD3CN:CDCl3 (9:1, v/v). When 1.2
equiv of Zn(ClO4)2 was added, the spiro carbon at δ 64.7 ppm
disappeared and moved to δ 150 ppm. The addition of Pb(ClO4)2
CHCl3 (4:1, v/v). The peak at 1689.53, which corresponds to
the characteristic amide carbonyl absorption, was shifted to
1592.35 (with Zn2+), 1614.72 (with Pb2+), 1614.27 (with Cu2+),
and 1614.72 (with Li+, see Supporting Information). These
results also support that a strong binding participation of the
carbonyl group occurs with metal ions.
1
caused a broadening of some peaks in the H and 13C NMR
spectra. However, the disappearance of the spiro carbon at δ
64.7 ppm was also confirmed. On the other hand, when 2.0
equiv of LiClO4 was added, the spiro carbon peak was clearly
observed at δ 66.6 ppm, and the carbonyl carbon peak moved
from 167.5 to 170.5 ppm.
Figure 6 shows the partial IR spectra of 1 (50 mM) with 1
equiv of Zn(ClO4)2, Pb(ClO4)2, and Cu(ClO4)2 in CH3CN-
In the ESI mass spectrum of 1, a peak at m/z 973.2 (calculated
value, 973.3) corresponding to [1 + Pb(ClO4)]+ was clearly
observed upon the addition of lead(II) perchlorate (Figure 7).
In addition, a peak at m/z 437.1 (calculated value, 437.2)
corresponding to [1 + Pb]2+ was observed. Upon the addition
of zinc(II) perchlorate, two distinct peaks at m/z 829.2 and 365.3
were observed, which correspond to [1 + Zn(ClO4)]+ and [1
(15) Yanagita, M.; Aoki, I.; Tokita, S. Bull. Chem. Soc. Jpn. 1997, 70, 2757.
9
10110 J. AM. CHEM. SOC. VOL. 127, NO. 28, 2005

+
Selective Fluorescent Chemosensor for Pb2
A R T I C L E S
Scheme 2. Proposed Mechanism for the Fluorescent Changes of 1 upon the Addition of Pb2+
+ Zn]2+, respectively. In a similar way, two distinct peaks at
m/z 828.1 and 364.5 were observed with Cu2+, which correspond
to [1 + Cu(ClO4)]+ and [1 + Cu]2+, respectively (see Support-
ing Information). When cupper nitrate was added, a peak at
m/z 791.2 (calculated value, 791.4) corresponding to [1 + Cu-
(NO3)]+ was observed (see Supporting Information).
Cu2+. Since the compound itself did not exhibit any fluores-
cence, the small CHEF effects with Cu2+ and Li+ can be also
explained by the blocking of the PET (photoinduced electron
transfer) process.
Conclusions
The proposed mechanism for these fluorescent changes is
explained in Scheme 2. Upon the addition of Pb2+ to a colorless
solution of1 in acetonitrile, both a pink color and the fluores-
cence characteristics of rhodamine B appear. Because both
disappear upon the addition of excess cyclen or ethylenediamine,
it is believed that this process is reversible. Also, the 1H NMR
of the extracted product was identical to that of 1. The 13C NMR
data also supports this spiro ring-opening mechanism. On the
other hand, the addition of Cu2+ as well as some other metal
ions caused relatively small CHEF effects without a red shift.
This was also a reversible process since there was no change
on TLC, and the characteristic fluorescent emission was
recovered upon the addition of either cyclen or ethylenediamine.
Furthermore, a chloroform and EDTA aqueous solution was
added to the 1‚Cu2+, and the 1H NMR of the extracted product
was identical to that of 1. As shown in Figure 2, the addition
of Cu2+ and Li+ to 1 caused similar intensity changes. From
the fact that the spiro carbon peak was still observed when 2.0
equiv of LiClO4 was added, it may be possible that the spiro
ring-opening mechanism did not occur upon the addition of
In conclusion, a new fluorescent sensor based on rhodamine
B for Pb2+ was synthesized. The new fluorescent sensor
displayed an extreme selectivity for Pb2+ over the other metal
ions examined in acetonitrile. An overall emission change of
100-fold was observed upon the addition of Pb2+, and the
selectivity for Pb2+ was calculated to be 200 times that of Zn2+
.
Variations in the ligands on the rhodamine B may provide
various fluorescent chemosensors, which are selective for
different metal ions.
Acknowledgment. This work was supported by the Korean
Science and Engineering Foundation (R14-2003-014-01001-0
to J. Y. and Creative Research Initiative Program to W. N.).
Supporting Information Available: NMR spectra, ESI mass
spectra and X-ray crystallographic data (CIF) of 1 and its
complexes. This material is available free of charge via the
Internet at http://pubs.acs.org.
JA051075B
9
J. AM. CHEM. SOC. VOL. 127, NO. 28, 2005 10111