A Novel Thiophene-Based Fluorescent Chemosensor for the Detection of Zn2+ and CN-: Imaging Applications in Live Cells and Zebrafish.

A novel fluorescent turn-on chemosensor DHADC ((E)-3-((4-(diethylamino)-2-hydroxybenzylidene)amino)-2,3-dihydrothiophene-2-carboxamide) has been developed and used to detect Zn2+ and CN-. Compound DHADC displayed a notable fluorescence increase with Zn2+. The limit of detection (2.55 ± 0.05 μM) for zinc ion was far below the standard (76 μM) of the WHO (World Health Organization). In particular, compound DHADC could be applied to determine Zn2+ in real samples, and to image Zn2+ in both HeLa cells and zebrafish. Additionally, DHADC could detect CN- through a fluorescence enhancement with little inhibition with the existence of other types of anions. The detection processes of compound DHADC for Zn2+ and CN- were demonstrated with various analytical methods like Job plots, 1H NMR titrations, and ESI-Mass analyses.

1. Introduction

The design of chemosensors with high selectivity and sensitivity has received great interest because they can recognize environmentally and biologically crucial metal ions and anions [1,2]. Among these ions, zinc ion is not only one of the essential metal ions in the human body, but is also the second richest transition metal ion [3,4]. It has large roles at catalytic sites of myriad Zn2+-containing metalloenzymes and in DNA-binding proteins [5,6]. Meanwhile, an uncontrolled zinc concentration in the body creates a wide variety of troubles like epilepsy, Parkinson disease, and ischemic stroke [7]. Hence, it is of great significance to design chemosensors for the selective sensing of Zn2+ in biological systems [8,9,10,11].

Recently, anions have attracted notable interest, owing to their various roles in clinical, environmental, and biological applications [12,13,14]. In particular, cyanide has been extensively used in numerous territories like synthetic fiber, gold mining, resin industries, and metallurgy [15,16,17,18]. Thus, the voluminous usage of cyanide is ineludible, and numerous industries yield about 140 k tons/year of cyanide [19,20,21]. However, cyanide acts as a strong poison. Its toxicity induces the susceptibility of binding to iron ion in metalloprotein cytochrome oxidase, blocking the electron transfer chain in mitochondria [22,23,24]. Moreover, high levels of cyanide can cause convulsions, vomiting, loss of consciousness, and ultimately death [25,26]. Thus, it is essential to develop an effective sensing tool to recognize the cyanide level in living organisms and environments [27,28].

Among various analytical methods, a fluorescent method has attracted much attention due to its high selectivity, simplicity, and bioimaging ability [29,30,31,32]. Until now, a few fluorescence chemosensors for detecting both Zn2+ and CN− were developed, but they are still rare. In addition, zinc fluorescent chemosensors for bioimaging in living cells and zebrafish are very rare (Table S1) [33,34,35,36,37,38,39]. Therefore, the development of fluorescent chemosensors with high selectivity and bioimaging ability in both living cells and zebrafish is needed.

Thiophene derivatives have been extensively utilized as a fluorescence signaling promoter to anions, organic acids, and metal ions [40,41]. Moreover, 4-diethylaminosalicylaldehyde moiety is an outstanding fluorophore that has a water-soluble electron-donor property [42,43]. Thus, we combined the two functional groups to design a novel and practical fluorescent sensor, which is expected to sense a particular analyte through a unique fluorescent property with bioimaging ability in both living cells and zebrafish.

Here, we demonstrate a novel and stable fluorescent chemosensor DHADC, comprised of 3-aminothiophene-2-carboxamide as a fluorescence-signaling group and 4-diethylaminosalicylaldehyde as an electron-donating group (Scheme 1). Chemosensor DHADC detected both Zn2+ and CN− by fluorescent turn-on. To interpret their detecting systems, diverse analytical investigations like ESI-mass analyses, 1H NMR titrations, and Job plots were carried out.

Scheme 1

Synthesis procedure of DHADC.

2. Experimental

2.1. Reagents and Equipments

Chemicals were purchased from Sigma–Aldrich. A Varian spectrometer was used to obtain 13C (100 MHz) and 1H NMR (400 MHz) spectra. Fluorescence emission and UV-visible absorption spectra were recorded with Perkin Elmer spectrometers. ESI-MS data were obtained by a Thermo quadrupole ion trap. Fluorescence imaging in zebrafish and cells was obtained by a using fluorescence microscope (MDG36, Leica and EVOS FL, Thermo Fisher Scientific). * Caution for the use of cyanide: Skin, respiratory, and eye protection is required.

2.2. Synthesis of Sensor DHADC ((E)-3-((4-(diethylamino)-2-hydroxybenzylidene)amino)-2,3-dihydrothiophene-2-carboxamide)

3-Aminothiophene-2-carboxamide (1.1 mmol, 160 mg) and 4-diethylaminosalicylaldehyde (1 mmol, 200 mg) was dissolved in 12.0 mL of ethanol and blended for 8 h at 20 ℃. The deep orange powder was given by filtration and purified with ether. The yield: 72 % (230 mg); 1H NMR: 11.42 (s, 1H), 8.77 (s, 1H), 8.01 (s, 1H), 7.72 (d, J = 5.2 Hz, 1H), 7.62 (s, 1H), 7.50 (d, J = 8.8 Hz, 1H), 7.38 (d, J = 5.2 Hz, 1H), 6.36 (d, J = 8.8 Hz, 1H), 6.13 (s, 1H), 3.38 (m, 4H), 1.13 (t, J = 5.6 Hz, 6H); and 13C NMR: 163.74, 162.29, 159.94, 159.93, 152.67, 149.72, 132.52, 129.91, 120.31, 109.47, 105.12, 97.26, 44.50, and 12.99. ESI-MS for [DHADC (C16H19N3O2S) + H+]+: calcd, 318.13 (m/z); found, 318.21 (m/z).

2.3. Fluorescence Titrations

1.0 mL of DMSO solvent was used to prepare a stock DHADC solution (1 × 10−2 mmol, 3.2 mg) and 3.0 μL of the stock solution was diluted to 2.997 mL bis-tris buffer (1 × 10−2 M, pH 7.0). 3–45 μL of zinc ion stock solution (0.1 M) dissolved in bis-tris buffer were added to DHADC (3.0 mL, 1 × 10−2 mM). After blending them for 20 sec, fluorescence spectra were obtained. Both DHADC and DHADC-Zn2+ showed no decomposition for 7 h in buffer condition.

For CN−, 1.0 mL of DMSO solvent was used to prepare a stock DHADC solution (1 × 10−2 mmol, 3.2 mg) and its eventual concentration (1 × 10−2 mM) was given by adding 3 μL of stock DHADC solution (1 × 10−2 M) into 2.996 mL MeCN. MeCN (1 mL) was employed to dissolve TEACN (tetraethylammonium cyanide, 33.1 mg (0.2 mmol)). 1.5–18 μL of cyanide (200 mM) were added to the compound DHADC (3.0 mL, 1 × 10−2 mM). After mixing them for 20 sec, fluorescence spectra were obtained. The titrations for Zn2+ and CN− were conducted three times for the average.

2.4. UV-vis Titrations

3 μL of a stock DHADC solution (1 × 10−2 M) was transferred in fluorescent cell containing 2.997 mL bis-tris buffer. 6–42 μL of a zinc ion stock solution (0.1 M) in bis-tris buffer were added to the compound DHADC (3.0 mL, 1 × 10−2 mM). UV-vis spectra were obtained after blending them for 20 s.

For CN−, 3 μL of a stock DHADC solution (1 × 10−2 M) was added into 2.997 mL MeCN. 1.5–15 μL of this CN− (0.2 M) in MeCN were added to the compound DHADC (3.0 mL, 1 × 10–2 mM). UV-vis spectra were obtained after blending them for 20 s.

2.5. Job Plots

350 μL of a stock DHADC solution (1 × 10−2 M) in DMSO was diluted to 49.65 mL bis-tris buffer for producing 0.07 mM. 0.3–2.7 mL of the diluted compound DHADC was added to fluorescent cells, respectively. 35 μL of a Zn2+ ion stock (1 × 10−1 M) solution in bis-tris buffer was diluted to 49.97 mL bis-tris buffer. 2.7–0.3 mL of the diluted zinc ion was added to each DHADC in fluorescent cells. The total volume of each fluorescent cell was 3.0 mL. Fluorescence spectra were obtained after blending them for 20 s.

For CN−, 0.6 mL of a stock DHADC (1 × 10−2 M) solution in DMSO was diluted to 29.4 mL MeCN/bis-tris buffer (95:5; v/v) to produce 2 × 10−2 M. 0.3–2.7 mL of the diluted compound DHADC was added to fluorescence cells, respectively. 30 μL of a CN− stock solution (0.2 M) in MeCN was diluted to 29.97 mL MeCN/bis-tris buffer solution (95:5). 2.7–0.3 mL of the diluted cyanide was added to each DHADC in fluorescent cells. The total volume of each fluorescent cell was 3.0 mL. UV-visible spectra were obtained after blending them for 20 s.

2.6. Competition Tests

1 × 10−2 mmol of Al(NO3)3 or NaNO3 or Fe(ClO4)2 or In(NO3)3 or KNO3 or Ga(NO3)3 or M(NO3)2 (M = Ni, Pb, Ca, Mg, Cu, Mn, Co, and Cd), or Fe(NO3)3 or Cr(NO3)3 was separately dissolved in 1.0 mL of bis-tris buffer. 42 μL of each metal ion (1 × 10−1 M) was added into 3.0 mL bis-tris buffer to produce 140 equiv. Following the addition of 42.0 μL of a zinc ion stock solution (0.1 M), 3.0 μL of a stock DHADC solution (1 × 10−2 M) was added into the fluorescent cells containing each metal ion. Fluorescence spectra were obtained after blending them for 20 s.

For CN−, 0.2 mmol of NaNO2, tetraethylammonium salts of F−, I− Cl−, and Br−, Na2S and tetrabutylammonium salts of N3−, H2PO4−, OAc−, SCN−, and BzO− was separately dissolved in 1.0 mL of bis-tris buffer. 15 μL (2 × 10−1 M) of each anion was put into 3.0 mL MeCN/bis-tris buffer (95:5) to afford 100 equiv. Following the addition of 15 μL of TEACN solution (200 mM), 2 μL (1 × 10−2 M) of compound DHADC was added into the fluorescent cells containing each anion. Fluorescence spectra were obtained after blending them for 20 s.

2.7. 1H NMR Titrations

DMSO-d6 (2.8 mL) was used to dissolve compound DHADC (6.4 mg and 0.02 mmol) and 700 μL of DHADC was transferred to three NMR tubes, respectively. 0, 0.5, and 1 equiv of Zn2+ dissolved. in 1.2 mL of DMSO-d6 solvent were added to each compound DHADC. 1H NMR spectra were obtained after blending them for 20 s.

For CN−, DMSO-d6 (2.8 mL) was used to dissolve DHADC (6.4 mg, 0.02 mmol) and 700 μL of DHADC was transferred to four NMR tubes, respectively. 0, 0.5, 1, and 2 equiv of TEACN dissolved in 2.4 mL of DMSO-d6 solvent were added to each compound DHADC. 1H NMR spectra were obtained after blending them for 20 s.

2.8. Quantum Yields

The quantum yields of DHADC, DHADC-Zn2+ and DHADC-CN− were determined with fluorescein (ΦF = 0.92) in basic ethanol as a reference fluorophore. By using calibration curves of fluorescein and their absorption spectrum, the concentrations of fluorescein corresponding to each DHADC, DHADC-Zn2+, and DHADC-CN− species were calculated and expressed as fluorescein-DHADC, fluorescein-DHADC-Zn2+, and fluorescein-DHADC-CN−. The quantum yields were calculated with the following equation [44]. ΦF is quantum yield, A is absorbance, F is the area of fluorescence emission curve, n is refractive index of the solvent, S is test sample, and R is a reference sample.

2.9. Quantification of Zn2+ in Real Samples

For fluorescent analysis in real samples, drinking water and tap water were obtained from our laboratory. The fluorescent analysis was carried out by adding 3.0 μL (10−2 M) of compound DHADC and 0.30 mL of a bis-tris buffer (10−2 M) to a 2.697 mL real sample solution having Zn2+. Solutions were thoroughly blended and remained at 20 °C for 5 min. Their fluorescence spectra were obtained.

2.10. Imaging in Live Cells and Zebrafish

In media containing 100 mg/mL streptomycin, the Eagle Medium, 10.0% fetal bovine serum, and 100 U/mL penicillin HeLa cells were kept. The cells grew in a humidified condition at 37.0 °C under 5% CO2. They were then put onto a 12 well plate (SPL Life Sciences, Pocheon, Gyeonggi-do, Republic of Korea) at a density of 1 × 104 cells/0.1 mL, cells were seeded and then incubated at 37.0 °C for 20 h. For fluorescent imaging tests, cells were treated with compound DHADC (dissolved in DMSO, 3 × 10−2 mM) for 10 min, followed by the incubation of Zn(NO3)2 (dissolved in water, 5.0 mM) for 10 min. A EVOS FL fluorescent microscope was employed for imaging [emission 510 (±21) nm; excitation 470 (±11) nm].

The wild types of zebrafish (AB line) were incubated at 29 °C on a 14 h light/12 h dark cycle in E2 media (1 × 10−3 M MgSO4, 1 × 10−3 M CaCl2, 1.5 × 10−4 M KH2PO4, 1.5 × 10−2 M NaCl, 5 × 10−5 M Na2HPO4, 1 × 10−4 M KCl, 0.5 mg/L MB (methylene blue), and 0.7 mM NaHCO3 at pH 7.2). Six-day-old zebrafish were prepared for fluorescence bio-imaging in vivo. Zebrafish were fed with only 5 × 10−3 mM of DHADC in E2 media having 0.05% DMSO at 29 °C for 10 min. After the zebrafish were rinsed with E2 media to get rid of the remaining DHADC, the zebrafish were fed with the solution and had a wide range of concentrations of Zn2+ (20, 50, 100, and 200 μM) for 10 min at 29 °C. They were rinsed with E2 media again and then 0.01% ethyl-3-aminobenzoate methanesulfonate was added for the fixed orientation of zebrafish. A fluorescent microscope (MDG36, Leica) was employed to image all zebrafish (λex = 450–490 nm. λem = 500–550 nm). By using Icy software, the mean fluorescence intensity was determined.

3. Results and Discussion

Probe DHADC was provided by the reaction of 4-diethylaminosalicylaldehyde and 3-aminothiophene-2-carboxamide in ethanol (72% yield, Scheme 1), and affirmed by 13C and 1H NMR and ESI-mass instrument.

3.1. Fluorescence Investigation of DHADC to Metal Cations

The sensing selectivity of DHADC was examined in the presence of various cations (Ni2+, Mn2+, Ga3+, Fe3+, Na+, In2+, Zn2+, Ca2+, Cd2+, Cu2+, Pb2+, Mg2+, Cr3+, Co2+, K+, Al3+, and Fe2+) in bis-tris buffer (Figure 1). By adding each metal ion (140 equiv), Zn2+ only exhibited a striking fluorescence increase (ca. 4500%) (λex = 446 nm, λem = 508 nm). Instead, other cations did not increase the fluorescence. These outcomes illustrated that compound DHADC showed high discrimination towards Zn2+.

Figure 1

Fluorescent changes of DHADC (1 × 10−5 M) with various cations (Al3+, Ga3+, In3+, Cd2+, Cu2+, Fe2+, Fe3+, Mg2+, Cr3+, Hg2+, Ag+, Co2+, Ni2+, Na+, K+, Mn2+, and Pb2+,140 equiv; λex = 446 nm; slit width = 10 nm).

To examine the interaction between DHADC and Zn2+, fluorescent titration of compound DHADC to zinc ion was executed (Figure 2). The emission (508 nm) of compound DHADC steadily increased and indicated a maximum at 140 equiv. (λex = 446 nm). Quantum yields (Φ) of 0.0003 (±0.0001) and 0.0135 (±0.0004) were determined for DHADC and DHADC-Zn2+ (Figure S1; λex = 464 nm). Binding type of DHADC with zinc ion was also analyzed by UV-visible titration (Figure S2). By adding Zn2+ to compound DHADC, the peaks of 320 and 470 nm increased continuously, and that of 430 nm decreased. There were two definite isosbestic points (380 and 447 nm), meaning that the binding of DHADC to Zn2+ formed one product.

Figure 2

Fluorescent changes of DHADC (1 × 10−5 M) with different amounts of Zn2+ (from 0 to 150 equiv.). λex = 446 nm; slit width = 10 nm. Inset: Fluorescence intensity at 508 nm vs. the amounts of Zn2+.

The binding process of DHADC and zinc ion was proposed to be a 1:1 interaction with the analysis of Job plot (Figure S3; λex = 446 nm, λem = 508 nm) [45]. The 1:1 interaction of DHADC-Zn2+ was affirmed by the ESI-mass search (Figure S4). The mass data displayed that the peak of 458.00 (m/z) was reminiscent of [DHADC(-H+) + Zn2+ + DMSO]+ (calculated at 458.05). With fluorescent titration, the association constant (K) for DHADC with Zn2+ was given as 1.6 × 103 (±31) M−1 by the equation of Benesi–Hildebrand (Figure S5) [46]. The constant was in the range of those (K = 1–1012) of previously announced probes for Zn2+ [47,48,49]. The binding process of compound DHADC with Zn2+ was further inspected by the titration of 1H NMR (Figure 3). With addition of Zn2+ (1 equiv.), the imine proton of 8.76 ppm was moved to downfield. At the same time, the protons of the thiophene moiety and the benzene ring were also moved to downfield. These results demonstrated that the N atom in the imine component and the O atom in the amide component may bind to Zn2+. No shift of the proton signals was monitored with the addition of more Zn2+ ions, which was indicative of a 1:1 binding of DHADC-Zn2+ species (Scheme 2). On the basis of the previous studies [34,50], the fluorescence turn-on mechanism of DHADC for Zn2+ might have the CHEF effect (chelation-enhanced fluorescence). During complexation of DHADC and Zn2+, the non-radiative transitions such as rotation and vibration were inhibited and the radiative transition was enhanced.

Figure 3

1H NMR titration of DHADC upon addition of Zn2+ (0, 0.5, and 1 equiv.).

Scheme 2

Proposed structure of DHADC-Zn2+.

To test the practicable capability of compound DHADC as a Zn2+ detector, the competitive study was executed in a mixture of Zn2+ (140 equiv.) and various interfering ions (140 equiv.; Al3+, Pb2+, Ga3+, Fe3+, K+, In2+, Ni2+, Cd2+, Mg2+, Fe2+, Cr3+, Na+, Ca2+, Mn2+, Co2+, and Cu2+) (Figure S6; λex = 446 nm, λem = 508 nm). Cu2+ fully interfered, and Fe3+, Cr3+, Fe2+, Co2+, and In3+ quenched 89%, 83%, 67%, 65%, and 22% of the fluorescence obtained with zinc ion alone. Therefore, the paramagnetic metal ions might be avoided for the applicability of the sensor in biological matrices. For practicable applications, the pH response of DHADC-Zn2+ was investigated at a wide variety of pH (2–12) (Figure S7; λex = 446 nm, λem = 508 nm). DHADC-Zn2+ species exhibited a momentous fluorescence enhancement between pH 7 and 10. Therefore, Zn2+ could obviously be sensed by the fluorescent analysis with compound DHADC over the physiologically and environmentally important pH scope of 7.0–8.4 [51].

We established a calibration plot for the quantitative measurement of Zn2+ by compound DHADC (λex = 446 nm, λem = 508 nm). Compound DHADC exhibited a satisfactory linearity between its intensity and the concentration of Zn2+, indicating that compound DHADC could be a possible choice for the quantitative measurement of Zn2+. With the use of 3 σ/slope [52], the detection limit was determined by 2.55 (±0.05) μM (Figure 4), which was much lower than the guideline (76 μM) recommended by the World Health Organization (WHO) [53,54]. To confirm the practicable ability of compound DHADC to Zn2+ in environmental samples, the samples of tap and drinking water were chosen (Table 1; λex = 446 nm, λem = 508 nm). Acceptable recoveries and relative standard deviation (R.S.D.) values were obtained for the samples. Thus, compound DHADC can be operational for the measurement of Zn2+ in practical applications.

Figure 4

Fluorescence intensities (at 508 nm) of DHADC as a function of Zn(II) concentration ([DHADC] = 10 μmol/L and [Zn(II)] = 10–80 μmol/L). Conditions: All samples were conducted in bis-tris buffer solution (10 mM bis-tris, pH 7.0). λex = 446 nm; and slit width = 10 nm.

Table 1

Determination of zinc ion concentration 1.

Sample	Zn(II) Added (µmol/L)	Zn(II) Found (µmol/L)	Recovery (%)	R.S.D. (n = 3) (%)
Drinking Water	0	0	-	-
	20	19.1 ± 0.6	95.5 ± 1.0	3.96 ± 0.5
Tap Water	0	0	-	-
	20	19.7 ± 1.0	98.5 ± 1.4	1.51 ± 1.1

1 Conditions: [DHADC] = 10 µM in 10 mM bis-tris buffer (pH 7.0).

In order to assess the sensing feasibility for biological applications of DHADC, we conducted fluorescent imaging experiments for sensing Zn2+ in living cells (Figure 5). We first incubated the HeLa cells with DHADC (30 μM) for 20 min. Then, the fluorescent emission in cells was not discovered without Zn2+. In contrast, the cells cultured with Zn2+ showed significantly increased fluorescence intensity. To further demonstrate the ability of DHADC in living organisms, the experiment for fluorescence imaging was carried out with zebrafish (Figure 6). When the zebrafish was incubated with DHADC (5 μM, a), there was no fluorescence signal. However, with increasing concentrations (20–200 μM, b–e) of Zn2+, the fluorescence signal gradually increased. By using Icy software, the mean fluorescent emission of the images was analyzed (Figure S8). The limit of detection was analyzed to be 21.44 (±2.6) μM. Thus, compound DHADC may be applied to intracellular sensing of Zn2+ in living organisms.

Figure 5

Fluorescent imaging of HeLa cells incubated with DHADC and Zn(II). Cells were incubated with DHADC and Zn(II) for 20 min. (a,a): DHADC only; (b,b): DHADC with zinc ion. Conditions: [DHADC] = 30 μM; [Zn(II)] = 5 mM; 37 °C; and 5% CO2. λex = 470 ± 11 nm. λem = 510 nm. Scale bar was 50 μm.

Figure 6

Fluorescence images of zebrafish (6-day-old) incubated with DHADC followed by addition of zinc ion. Top line: bright-field image; middle line: fluorescent image; and bottom line: overlay image. (a–a): DHADC only; (b–b): DHADC with 20 μM zinc ion; (c–c): DHADC with 50 μM zinc ion; (d–d): DHADC with 100 μM zinc ion; and (e–e): DHADC with 200 μM zinc ion. [DHADC] = 5 μM. λex = 450–490 nm. λem = 500–550 nm. Scale bar: 1 mm.

3.2. Fluorescence Studies of Compound DHADC to CN−

The fluorescence sensing capability of DHADC to a variety of anions in bis-tris buffer/acetonitrile solution (5:95) was examined (Figure 7; λex = 459 nm, λem = 528 nm). The fluorescent spectra of DHADC with diverse types of anions (I−, S2−, H2PO4−, Cl−, N3−, F−, BzO−, Br−, OAc−, SCN−, and NO2−) showed very weak intensities. In contrast, there was a significant enhancement of fluorescence at 528 nm by adding 100 equiv. of CN−. These outcomes indicated that compound DHADC could have a potential function as a choosy fluorescence receptor for CN−.

Figure 7

Fluorescent changes of DHADC (1 × 10−5 M) with other anions (OAc−, F−, Cl−, Br−, I−, H2PO4−, BzO−, N3−, SCN−, NO2−, and S2−, 100 equiv.; λex = 459 nm; slit width = 10 nm).

To examine the influence of increasing levels of CN− to DHADC solution, the fluorescence titration was carried out (Figure 8; λex = 459 nm, λem = 528 nm). When the CN− (0–120 equiv.) was added into DHADC solution, the fluorescence emission continuously increased at 528 nm and showed a maximum with 100 equiv. Quantum yields (Φ) of 0.0063 (±0.0004) and 0.1118 (±0.0003) were analyzed for DHADC and DHADC-CN− (Figure S1). The binding character of compound DHADC with CN− was inspected by UV-visible titration test (Figure S9). With the addition of cyanide to compound DHADC, the peaks at 315 and 475 nm increased consistently, and 390 nm decreased continuously with two definite isosbestic points (345 and 425 nm).

Figure 8

Fluorescent changes of DHADC (1 × 10−5 M) with different amounts of cyanide (from 0 to 120 equiv.). λex = 459 nm; slit width = 10 nm. Inset: Fluorescence intensity at 528 nm vs. the amounts of cyanide.

To investigate the binding mode of DHADC and CN−, Job plot analysis was performed (Figure S10; λex = 459 nm, λem = 528 nm) [45]. This result showed a 1:1 complexation, which was affirmed by ESI-MS analysis (Figure S11). Addition of CN− (1 equiv.) into compound DHADC exhibited the production of the [DHADC - H+]− [m/z: 316.21; calculated at 316.11]. With the results of the fluorescent titration, the K value for DHADC with CN− was given as 1.6 × 103 (±50) M−1 (Figure S12). The detection limit (3σ/slope) was determined by 44.6 (±1.5) μM (Figure 9) [52].

Figure 9

Determination of the detection limit of DHADC (10 μM) for CN− based on the change of intensity at 528 nm. λex = 459 nm; slit width = 10 nm.

To elucidate the detection process of compound DHADC with CN−, we carried out the titration experiments of 1H NMR (Figure S13). The proton of the hydroxyl component did not show up because of the possible inter or intra-molecular hydrogen bonds [55]. With the addition of CN (2 equiv.) to compound DHADC, all protons of the thiophene group and the benzene ring shifted to upfield. In contrast, one of the amide protons (H3) was shifted to downfield, suggesting that the H3 proton might hydrogen bond to CN− or HCN species (Scheme 3). These outcomes implied that the negative charge generated from the deprotonation of compound DHADC by cyanide was delocalized through the DHADC [56]. No movement of the proton signals was detected with addition of more amounts of CN− (>2 equiv.). On the basis of the previous studies and our experimental data [34,57,58], we can propose that the deprotonation of DHADC could cause the suppression of ICT (intramolecular charge transfer), which induces fluorescence turn-on of DHADC-H+ species. With the analysis results of ESI-mass, 1H NMR study and Job plot, the possible recognizing process of compound DHADC with CN− was depicted in Scheme 3.

Scheme 3

Proposed sensing mechanism of DHADC for CN−.

To inspect the inhibition of different types of anions, the competitive tests were achieved and are shown in Figure 10 (λex = 459 nm, λem = 528 nm). Compound DHADC was mixed with CN− (100 equiv.) and a wide variety of anions (S2−, F−, BzO−, Cl−, SCN−, Br−, NO2−, OAc−, N3−, H2PO4−, and I−; 100 equiv.). Some inhibition was observed with F−, but its fluorescence was still discernible. These observations illustrated that compound DHADC may be an excellent selective fluorescence detector for CN−.

Figure 10

Competitive test of DHADC (1 × 10−5 M) to cyanide (100 equiv.) with other anions (100 equiv.). λex = 459 nm; slit width = 10 nm.

4. Conclusions

We demonstrated a unique fluorescent turn-on probe DHADC having a thiophene moiety. Compound DHADC could selectively sense Zn2+ and CN− through fluorescence enhancement. Binding ratios of compound DHADC with Zn2+ and CN− were proposed to be 1:1, with the analysis of ESI-mass data and Job plots. Detection limits for zinc ion and CN− were 2.55 (±0.05) μM and 44.6 (±1.5) μM, respectively. The value for zinc ion was far below the standard (76 μM) of the WHO. Importantly, compound DHADC could be used to analyze zinc ion in water samples and to image zinc ion in both zebrafish and live cells. Additionally, compound DHADC could detect CN− with little interference of competitive anions. Moreover, the detection processes of DHADC with Zn2+ and CN− were proposed through 1H NMR titrations and ESI-Mass analyses. Therefore, the results observed in this study illustrate that DHADC can be a detector to selectively detect Zn2+ and CN− by the fluorescent turn-on method in aqueous and living organisms.