Zinc ion has been known as the second most abundant transition metal ion in human body. While most zinc ions are tightly bound in proteins, a small amount of free Zn2+ ions is presented in various human tissues      . Some neurologic diseases are found to associate with free Zn2+. For instance, the abnormal accumulation of Zn2+ is found in patients with Alzheimer’s disease  . Moreover, Zn2+ plays an important role in the regulation of apoptosis (programmed cell death)  . Aluminum is the third most abundant element in earth’s crust, and it is the most abundant metal on earth. High concentration of aluminum in soils may lead to environmental issues such as acid soils   . In human body, aluminum is known to associate with the development of Alzheimer’s disease and Parkinson’s disease    . Therefore, the development of Zn2+ and Al3+ sensors for environmental and biological monitoring is critical. Compare to traditional detection methods such as atomic absorption spectroscopy, electrochemical sensor, and inductively coupled plasma atomic emission spectrometry, fluorescent sensors have become a popular tool for the detection of metal ions due to their simple operating processes    .
Schiff base moieties have been extensively applied as ionophores in fluorescent sensors due to their ability to form coordination complexes with metal ions    . Some fluorescent sensors based on Schiff base moieties have been synthesized to detect Zn2+    or Al3+    . However, only a few sensors demonstrated fluorescence responses toward multiple metal ions. Besides, some of these sensors exhibited responses toward multiple metal ions simultaneously   . Therefore, it is highly desirable to synthesize fluorescent sensors with specific responses toward multiple metal ions.
In this work, a novel fluorescent sensor PySb was synthesized and characterized. Fluorescent pyrene moiety was selected as fluorophore to enhance sensitivity. 2-amino-2-(hydroxymethyl)propane-1,3-diol was chosen as part of binding moiety. By forming imine via reaction with 2-hydroxybenzaldehyde, the three alcoholic -OH along with phenolic -OH should be able to interact with multiple metal ions   . Accordingly, specific responses toward Zn2+ and Al3+ can be expected.
2.1. Materials and Measurements
All the reagents and solvents were purchased from commercial sources and were used without further purification. 4-(2-hydroxyethyl)-1-piperazineethanesulfonic acid) (HEPES) was dissolved in water (2.5 × 10−4 M) which was used as buffer solution. Nitrate salts of Na+, K+, Ca2+, Cu2+, Ni2+, Co2+, Zn2+, Pb2+, Fe3+, Cr3+ and Al3+ were dissolved in the HEPES(aq) buffer to prepare their stock solutions (10−2 M). PySb was dissolved in ethanol, DMF, or DMSO; the concentration was 2 × 10−5 M. 1H NMR spectra with the chemical shifts reported in ppm were recorded on a Bruker AMX-600 MHz spectrometer, using tetramethylsilane (TMS) as an internal standard. Elemental analysis (EA) of carbon, hydrogen, and nitrogen were measured on a Heraus CHN-Rapid elemental analyzer. The UV-Vis absorption spectra were recorded on a Jasco V-550 spectrophotometer using a quartz cuvette (path length = 1 cm). Photoluminescence (PL) spectra were recorded on a fluorescence spectrophotometer (Hitachi F-4500) in mixtures of water with appropriate organic solvents.
2.2. Synthesis of PySb (Scheme 1)
To a sodium carbonate solution (0.6 M, 2.8 ml) in 50-mL glass reactor was added with 5-bromo-2-hydroxybenzaldehyde (1: 0.264 g, 1.32 mmol), 2,7-bis(4,4,5, 5-tetramethyl-1,3,2-dioxaborolan-2-yl)pyrene (2:0.2 g, 0.44 mmol), and tri-tert-
Scheme 1. Synthesis of fluorescent sensor PySb.
butylphosphonium tetrafluoroborate (0.032 g, 0.11 mmol). Tris(dibenzylideneacetone)dipalladium(0) (Pd2(dba)3: 57 mg, 0.06 mmol) was dissolved in THF (18 ml) and added into the reactor by a syringe. The mixture was degassed by the freeze-pump-thaw cycle for three times. Next, the mixture was stirred at 65˚C for two days; then it was poured into water and extracted with dichloromethane. The combined organic layer was concentrated under reduced pressure, poured into n-hexane to obtain precipitate as crude product. The crude product was purified by flash column chromatography (eluent: dichloromethane) to afford 5,5’-(pyrene-2,7-diyl)bis(2-hydroxybenzaldehyde) (3) (yield: 0.11 g, 56.4%). 1H NMR (600 MHz, DMSO-d6, TMS, 25˚C): δ 10.80 - 11.03 (s, 2H, -CHO), 10.47 - 10.36 (s, 2H, -OH), 8.62 - 8.57 (s, 4H, Ar-H), 8.31 - 8.26 (s, 6H,Ar-H), 8.23 - 8.13 (d, 2H, Ar-H), 7.28 - 7.20 (d, 2H, Ar-H).
A mixture of 3 (0.15 g, 0.39 mmol), 2-amino-2-(hydroxymethyl)propane- 1,3-diol (4:0.41 g, 3.9 mmol) and methanol (150 ml) was stirred at 65˚C for two days. Methanol was evaporated by a rotavapor. The crude product was washed by water and acetone several times to obtain PySb (yield: 0.20 g, 90.8%). 1H NMR (600 MHz, DMSO-d6, TMS, 25˚C): δ 14.79 - 14.64 (s, 2H, phenolic OH), 8.80 - 8.71 (s, 2H, CNH), 8.63 - 8.55 (s, 4H, Ar-H), 8.28 - 8.19 (s, 4H, Ar-H), 8.17 - 8.09 (s, 2H, Ar-H), 8.03 - 7.95 (d, 2H, Ar-H), 7.01 - 6.93 (d, 2H, Ar-H), 4.90 - 4.78 (s, 6H, OH), 3.71 - 3.63 (d, 12H, CH2). Anal. Calcd. for C38H36N2O8 (%): C, 70.36; H, 5.59; N, 4.32. Found: C, 69.47; H, 5.56; N, 4.20.
3. Results and Discussion
3.1. Synthesis of Fluorescent Sensor PySb
The new fluorescent sensor PySb was synthesized in two steps as shown in Scheme 1. First, the bis(2-hydroxybenzaldehyde) derivative (3) of pyrene was synthesized from 5-bromo-2-hydroxybenzaldehyde (1) and diboronate derivative of pyrene (2) via the Suzuki coupling reaction (Figure S1, Supplementary Material). It was further condensed with 2-amino-2-(hydroxymethyl)propane- 1,3-diol (4) via imine formation to obtain the fluorescent sensor PySb. The PySb was characterized by 1H NMR spectrum, mass spectra, and elemental analysis. The 1H NMR spectrum of PySb is demonstrated in Figure 1, in which the respective protons can be readily assigned due to its chemically symmetric structure. The chemical shifts at 3.71 - 3.63 ppm (i) are assigned to the protons of methylene protons next to alcoholic -OH, whereas those at 4.90 - 4.78 ppm (h) are assigned to the protons of alcoholic -OH. The chemical shifts at 7.01 - 6.93 ppm (g), 8.03 - 7.95 ppm (f), and 8.17 - 8.09 ppm (e) have been assigned to the protons on benzene rings. The chemical shifts at 8.28 - 8.19 ppm (d) and 8.63 - 8.55 ppm (c) are assigned to the protons on pyrene core. Finally, the chemical shifts at 8.80 - 8.71 ppm (b) are arisen from the protons on C=N bond. The chemical shifts at 14.79 - 14.64 ppm (a) are assigned to phenolic protons. The mass spectrum of PySb was measured by positive ion mode (M + H) (Figure S2). The average neutral mass of PySb is 648.70 (Figure S3). Setting m/z value of 649.25 to 100.00%, the corresponding m/z value of 650.25, 651.26, 652.26, and 653.26 were 42.57%, 10.48%, 1.89%, and 0.26%, respectively.
3.2. Photophysical Properties in Ethanol Buffer Solutions
The absorption spectra of PySb with various metal ions in ethanol buffer solutions
Figure 1. 1H NMR spectrum of PySb in DMSO-d6.
are depicted in Figure 2. The absorption band at 306 nm is attributed to the π-π* transitions of pyrene core  . Upon addition of Na+, K+, Ca2+, the absorption of PySb remains nearly unchanged, indicating that PySb does not interact with these ions. On the other hand, the absorption intensities increased with little red or blue shifts (1 - 10 nm) when Cu2+, Ni2+, Co2+, Zn2+, Pb2+, Fe3+, Cr3+, or Al3+ were added. This suggests that PySb might have interaction with these ions.
PySb itself exhibits very weak fluorescence in ethanol buffer solution (Figure 3). The fluorescence quenching can be explained by the photo-induced electron-transfer (PET) mechanism   as illustrated in Figure 4. The fluorescent relaxation of photo-excited electron from pyrene core is forbidden, because the HOMO has been fully filled by obtaining an electron from high-lying HOMO of the terminal 2-iminophenol groups. Upon addition of various metal ions, only Zn2+ ion caused a significant enhancement of fluorescence intensity (51 times compared to free PySb, λem = 470 nm). The enhanced sky-blue fluorescence can be clearly observed by naked eyes (Figure 5). The result shows that PySb can be applied as an efficient Zn2+ sensor in ethanol solution.
The binding stoichiometry between PySb and Zn2+ was determined by the Job plot. By plotting the fluorescence intensities versus the molar fraction of Zn2+, two regression lines are obtained and they intersect at about 0.66 (Figure 6), indicating 1:2 stoichiometric ratio between PySb and Zn2+. In other words, each terminal Schiff base moiety in PySb chelates with one Zn2+.
Figure 2. UV-Vis spectra of PySb (10−5 M) with various metal ions (2 × 10−4 M) in HEPES buffer solution (Ethanol/H2O = 9/1, v/v).
Figure 3. Fluorescence spectra of PySb (10−5 M) with various metal ions (2 × 10−4 M) in HEPES buffer solutions (Ethanol/H2O = 9/1, v/v), λex = 309 nm.
Figure 4. PET mechanism of PySb.
Figure 5. Photographs of PySb (10−5 M) with various metal ions (2 × 10−4 M) in HEPES buffer solutions (Ethanol/H2O = 9/1, v/v) under UV-light.
Figure 6. Job plot of PySb and Zn2+ in HEPES buffer solutions (Ethanol/H2O = 9/1, v/v). The total concentration of PySb and Zn2+ was 10−5 M (λex = 309 nm, λem = 470 nm).
To further investigate the sensitivity of this fluorescence enhancement, PL spectra of PySb were measured with increasing amount of Zn2+ (from 0.1 to 20 equivalents). As depicted in Figure 7, the fluorescence intensity increases gradually with increasing Zn2+ concentration and reaches the asymptotic value at approximately 12 equivalents of Zn2+ ion. The binding constant (Ka) of PySb was evaluated from titration data as 2 × 109 M−1 using the Benesi-Hildebrand plot. Moreover, the limit of detection (LOD) was 2.39 × 10−8 M using the equation LOD = 3σ/m, where σ and m represent the standard deviation (0.558) of blank solutions and the slope (7 × 107) of fluorescence intensity versus Zn2+ concentration plot respectively (Figure S5).
For real-time application, it is important to evaluate the interference from other metal ions. As shown in Figure 8, only Na+, K+, and Ca2+ show no interference against Zn2+ sensing. This is coincident with the above-mentioned spectral observation of PySb, i.e., no obvious spectral change in the presence of these three ions. However, the fluorescence intensities of PySb were partially diminished by Ni2+, Co2+, and Pb2+. Moreover, the fluorescence intensities were dramatically debilitated in the presence of Fe3+, Cr3+, or Al3+, indicating that these ions bind strongly with PySb to quench the fluorescence. Finally, Cu2+ was the only metal ion that completely quenched the fluorescence. This quenching phenomenon is commonly seen in many fluorescent sensors owning to the
Figure 7. Fluorescence spectra of PySb (10−5 M) with increasing amount of Zn2+ in HEPES buffer solutions (Ethanol/H2O = 9/1, v/v), (λex = 309 nm, λem = 470 nm).
Figure 8. Fluorescence intensity of PySb (10−5 M) with various metal ions (2 × 10−5 M) in HEPES buffer solutions (Ethanol/H2O = 9/1, v/v), λex = 309 nm.
paramagnetic nature of Cu2+    .
In preparation of PySb solutions for fluorescence experiments, we observed fluorescence intensity changes of PySb in different solvents. PySb-Zn2+ exhibited stronger fluorescence intensity in ethanol than in DMF. However, ethanol was a poor solvent for PySb while DMF was a good solvent for PySb. Therefore, an experiment was carried out to investigate this interesting phenomenon. The variations of fluorescence spectra of PySb were monitored in mixture solvents of DMF and ethanol. As presented in Figure 9, the fluorescence intensity at ca. 470 nm first remains nearly unchanged from solutions with 100% DMF to DMF/ethanol = 5/5. Then the intensity starts to increase gradually to DMF/ethanol = 1/99. The fluorescence intensity is increased about 1.8 times in 99% ethanol solution, compared to low ethanol content solutions (0 - 50% ethanol). Apparently, the fluorescence emission is enhanced with increasing composition of poor solvent. This phenomenon can be explained by the aggregation-induced emission enhancement (AIEE) caused by restricting intramolecular rotation (RIR). The rotation of the conjugated single bond, which links pyrene core and terminal 2-iminophenol group, consumes part of excitation energy in DMF solution. Such rotation is confined as PySb-Zn2+ starts to form as nanoparticle suspensions in higher ethanol content solutions (>50%). The formation of nanoparticle suspensions can be validated from the level-off tail in UV-Vis spectra (Figure 10) due to Mie effect   . The result reveals that the two terminal benzene rings not only serve as a linker but also facilitate further enhancement in fluorescence intensity. Such molecular design could be applied to enhance sensitivity and detection limit of fluorescent sensors.
It is noteworthy that although ethanol is a poor solvent, ratiometric detection toward Zn2+ as discussed previously still shows good accuracy. The reason can be explained as following: The poor solubility of PySb is mainly attributed to its
Figure 9. Fluorescence spectra of PySb (10−5 M) with Zn2+ (2 × 10−4 M) in different DMF/ethanol ratio solutions (λex = 324 nm, λem = 470 nm).
Figure 10. UV-Vis spectra of PySb (10−5 M) with Zn2+ ion (2 × 10−4 M) in DMSO and ethanol solutions.
Figure 11. (a) Fluorescence spectra of PySb (10−5 M) without Zn2+, (b) with Zn2+ in different pH solutions (Ethanol/H2O = 9/1, v/v), λex = 309 nm.
pyrene core, whereas the binding site in 2-iminophenol group contains four polar -OH groups. Therefore, the binding ability toward Zn2+ is not greatly influenced in ethanol solution, and therefore data with good consistency and accuracy were obtained.
Figure 11 demonstrates pH responses of PySb with and without Zn2+ from pH = 2.0 to pH = 12.0. PySb did not show significant fluorescence enhancement without Zn2+ until pH = 12.0. At pH = 12.0, an emission band at 515 nm appears with a fluorescence enhancement (FE) factor of 17. Clearly, the emission arises from the formation of phenolate anion in basic environment as illustrated in Figure 12. This significant emission enhancement can be explained by intramolecular charge transfer (ICT)    . The stronger electron-donating ability of phenolate anion strengthens its electron delocalization, resulting in an extended conjugation with benzene ring and imino moiety. The red shift of emission band from 470 nm to 515 nm indicates a chromophore change from pyrene moiety to the extended conjugated system.
In Figure 11(b), the fluorescence is still quenched in the presence of Zn2+ in low pH ranging from 2.0 to 3.0, and it reaches maximum at ca. pH 10.0. This implies that the formation of PySb-Zn2+ complex is more favorable at moderate high pH and it is inhibited by the protonation of N atom at low pH. As pH reached 12.0, the solution exhibits the same green emission (peak at 515 nm) as the one without Zn2+ (Figure 11(a)). The result reveals a competition effect between inhibited PET emission and ICT emission    . The above results validate that PySb can serve as a Zn2+ sensor in a wide pH range. Besides, H+ and OH− do not generate confusing signals against Zn2+ sensing, which is rare for Schiff base PET sensors  .
3.3. Photophysical Properties in Buffered DMSO Solution
Next, we investigated the photophysical properties of PySb in DMSO solution. The absorption spectra [Figure 13(a)] shows similar result to those in ethanol buffer solutions, both metal ions have interactions with PySb. Interestingly, PySb exhibits different fluorescence responses in DMSO solutions [Figure 13(b)]. The fluorescence with addition of Zn2+ became indistinct, while addition of Al3+
Figure 12. (a) Formation of phenolate anion at high pH; (b) Competition between PET and ICT mechanisms.
Figure 13. (a) UV-Vis spectra of PySb (10−5 M) with Zn2+ and Al3+ metal ions (2 × 10−4 M); (b) Fluorescence spectra of PySb (10−5 M) with various metal ions (2 × 10−4 M) in HEPES buffer solution (DMSO/H2O = 9/1, v/v).
Figure 14. Fluorescence spectra of PySb (10−5 M) with increasing amount of Al3+ in HEPES buffer solutions (DMSO/H2O = 9/1, v/v), (λex = 309 nm, λem = 458 nm).
generated strong fluorescence enhancement. Cr3+ also induced weak fluorescence enhancement but with a deeper blue color. Therefore, it appears that PySb can serve as Al3+ sensor in DMSO solution.
The sensitivity of PySb toward Al3+ in DMSO solution was investigated by titration experiment as depicted in Figure 14. Surprisingly, PySb did not exhibit fluorescence enhancement until two equivalents of Al3+ were added. This result reveals that when PySb is dissolved in DMSO solution, strong fluorescence is generated only when both binding sites are chelated with Al3+. It is reasonable to suppose that the quenching ability of imine moieties varies with solvents. In DMSO, both imine moieties can quench the fluorescence completely through the PET mechanism, thus the fluorescence is recovered only when both binding sites are chelated with Al3+. On the contrary, in ethanol the quenching ability of imine moieties is less than 100%, so the fluorescence can be recovered when one of the binding sites is chelated with Zn2+. Since PySb did not show fluorescence response until two equivalent of Al3+ were added, the investigation of Job plot, binding constant and detection limit could not be conducted.
Figure 15 demonstrates competition effects from other metal ions against Al3+ sensing. Aside from Cu2+ which completely quenched the fluorescence as in ethanol solutions, only Fe3+ partially decreased fluorescence intensity. The result agrees with the observation in ethanol solutions that PySb exhibits higher binding tendency toward Al3+. Thus PySb can serve as a highly selective Al3+ sensor in DMSO solution.
3.4. 1H NMR Spectra of PySb-Zn2+ and PySb-Al3+ Complexes
The formation of PySb-Zn2+ complex was further investigated by 1H NMR spectra in deuterated N,N-dimethylformamide (DMF-d7, Figure 16). The one at the bottom represents 1H NMR spectrum of free PySb in DMF-d7, three solvent peaks of DMF, one solvent peak of H2O and all proton signals, except for the proton f which merged into DMF solvent peak near 8.0 ppm, of PySb have been assigned. Upon addition of Zn2+ the signal of phenolic proton (a) significantly shifted from 14.66 ppm to 11.25 ppm, whereas the signal of alcoholic protons (h) at about 4.93 ppm split into three broad peaks ranging from 5 - 7 ppm. However, no shift was observed for the peak of imine protons (b) at 8.92 ppm, but the peak became much broader. The above phenomena indicate that the three alcoholic -OH, phenolic -OH and -H on C=N bond have interactions with Zn2+. Moreover, a new signal appeared at 10.43 ppm, suggesting that the formation of
Figure 15. Fluorescence spectra of PySb (10−5 M) with various metal ions (2 × 10−5 M) in HEPES buffer solutions (DMSO/H2O = 9/1, v/v), λex = 309 nm.
Figure 16. 1H NMR of free PySb (bottom), PySb + Zn2+ (middle), and PySb + Zn2+ + D2O (upper).
PySb-Zn2+ complex might involve an additional hydroxide ion (OH−). The disappearance of signals of alcoholic (h) and alcoholic protons (a) after addition of D2O confirms the presence of these exchangeable protons.
1H NMR spectra of PySb-Al3+ complex in DMSO (Figure 17) shows similar results, but the changes in proton signals are much smaller than in DMF. In fact, it took a long time for PySb to reach saturated fluorescence intensity with Al3+ (about 3 hr). Therefore, the small signal changes are probably due to slow formation of PySb-Al3+ complex.
An efficient fluorescent sensor PySb comprising of pyrene moiety as the fluorophore, benzene ring as the spacer, and 2-(hydroxymethyl)propane-1,3-diol as the ionophore was successfully synthesized and characterized. The PySb itself exhibited weak fluorescence due to PET mechanism; however, the fluorescence
Figure 17. 1H NMR spectra of free PySb (bottom), PySb + Al3+ (middle), and PySb + Al3+ + D2O (upper).
was turned on by Zn2+ in ethanol solution (λem = 470 nm) and by Al3+ in DMSO solution (λem = 458 nm). The complexes of PySb-Zn2+ and PySb-Al3+ were further confirmed by 1H NMR spectra. The stoichiometric ratio between PySb and Zn2+ was 1:2, as obtained from the Job plot. Based on the titration experiment, limit of detection (LOD) and binding constant toward Zn2+ were 2.39 × 10−8 M and 2 × 109 M−1, respectively. The PySb-Zn2+ complex in DMF solution showed aggregation-induced emission enhancement with increasing content of ethanol. It can be utilized as a fluorescent sensor in a wide range of pH (3 - 11). Green emission of PySb (λem = 515 nm) was observed when pH was higher than 12 due to ICT mechanism. Current results indicate that PySb is a promising fluorescent “turn on” sensor for Zn2+ and Al3+ in ethanol and DMSO, respectively.
Authors are thankful to Ministry of Science and Technology, Taiwan for financial support through grant MOST 105-2221-E-006-250. This research was partially funded by the Headquarters of University Advancement at National Cheng Kung University, under the sponsorship of the Ministry of Education, Taiwan.
Figure S1. 1H NMR spectrum of 3.
Figure S2. Mass spectra of PySb.
Figure S3. Isotope pattern of PySb.
The binding constant can be calculated according to Benesi-Hildebrand equation by measuring the fluorescence intensity change upon addition of various concentrations of Zn2+. The equation is depicted as following    :
Assuming 1:2 stoichiometry for association between PySb and Zn2+
F: Observed fluorescence
F0: Fluorescence of free PySb
Fmax: Saturated fluorescence of PySb and [Zn2+] complex
Ka: Binding constant of PySb and [Zn2+]
As illustrated in Figure S4, by plotting against , a linear equation can be obtained: Y = A + BX. Ka was calculated from A/B.
Limit of Detection (LOD)
Detection limit was calculated based on titration experiment, using the equation as following   :
σ = standard deviation of the blank solution, calculated from 10 blank solutions.
Figure S4. Benesi-Hildebrand plot of PySb, assuming 1:2 stoichiometry for association between PySb and Zn2+ in HEPES buffer solutions (Ethanol/H2O = 9/1, v/v).
Figure S5. Detection limit of PySb (10−5 M) toward Zn2+ in HEPES buffer solutions (Ethanol/H2O = 9/1, v/v).
m = slope of fluorescence intensity versus Zn2+ concentration.
The detection limit of PySb toward Zn2+ was M, which is much higher than the World Health Organization guideline for maximum acceptable concentration in drinking water: 76 μM   .
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