English

• Aggregation-induced emission (AIE), as an extraordinary photophysical phenomenon, has been recognized as a frontier research topic over the last two decades [1–3]. Soon after the concept of AIE was stated, the AIE-active Re(Ⅰ) complexes were reported by Manimaran et al., named as aggregation induced phosphorescent emission (AIPE) [4]. In 2008, Zhu et al. reported a class of AIPE-active dicationic terpyridyl-platinum(Ⅱ) complexes [5]. To date, AIPE-active cationic Pt(Ⅱ) complexes have focused on two-ligand molecular frameworks consisting of one tridentate ligand and one monodentate ligand, while the C^N bidentate ligands modified cationic Pt(Ⅱ) complexes are still infrequent and need further exploration (Table S1 in Supporting information) [6–10].

  As a unique C^N bidentate ligand, 2-(2,4-difluorophenyl)-pyridine (dfppy) can serve as an excellent cyclometalating ligand for tuning the performances of the corresponding cyclometalated Pt(Ⅱ) complexes [11–14]. Compared to 2-phenylpyridine (ppy), the complexes constructed by dfppy demonstrated impressive photophysical properties [15–18]. Besides, the intermolecular hydrogen bonds induced by fluorine atoms can significantly enhance the molecular aggregation to influence their properties [19]. In 2021, Shahsavari and colleagues reported several dfppy-based Pt(Ⅱ) complexes, exhibiting higher quantum yields compared to their ppy analogues [13]. Recently, Hamidizadeh et al. showed that the emission intensity of the Pt(Ⅱ) complexes significantly enhanced after replacing ppy with dfppy [14].

  Picric acid (PA) is commonly used to manufacture high explosives, posing a serious threat to human life [20]. Hence, it is necessary to develop a sensitive and selective detection method for PA. To date, a number of fluorescent and phosphorescent materials have been synthesized to serve as sensors for PA [21–27]. Among them, Pt(Ⅱ) complexes are predominantly concentrated on the metallacycles and metallacages from the self-assembly of organoplatinum compounds (Table S2 in Supporting information) [28,29].

  Our group has a long-term interest in the relationship between the molecular structures of the cyclometalated Pt(Ⅱ) and Ir(Ⅲ) complexes and their properties [30–37]. Recently, we designed and synthesized several AIPE-active cationic Ir(Ⅲ) complexes, which demonstrated efficient detection of PA in aqueous media [36,37]. However, the development of cyclometalated Pt(Ⅱ) complexes is far behind in comparison [38]. Specifically, AIPE-active cationic cyclometalated Pt(Ⅱ) complexes for detecting PA in aqueous media have not been reported. In this study, a novel cationic cyclometalated Pt(Ⅱ) complex 2 using dfppy as the cyclometalating ligand and 1,10-phenanthroline as the auxiliary ligand has been prepared. The properties of 2 have been systematically investigated compared with a non-fluorinated complex 1. In addition, the detection of PA using the Pt(Ⅱ) complex as a probe in aqueous media was studied. The structures of 1 and 2 are depicted in Fig. 1a.

  Figure 1

  

  Figure 1.  (a) The structures of 1 and 2. (b) Normalized emission spectra (solution: solid trace, solid: dash trace) of 1 (black) and 2 (red) at room temperature (50 µmol/L in CH₃CN). (c) Emission spectra of 2 and (d) emission intensity curves of 1 and 2 at 50 µmol/L in CH₃CN/H₂O with different water fractions. (e) Time-dependent emission spectra of 2 (CH₃CN/H₂O, v/v = 1:9, 50 µmol/L). (f) TEM image of aggregates of 2 (CH₃CN/H₂O, v/v = 1:9, 50 µmol/L). The excitation wavelength was 400 nm.

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  The normalized emission spectra of 1 and 2 in CH₃CN and in the solid state are shown in Fig. 1b. 1 and 2 exhibit evident fine vibronic splitting characteristics at 462–479 nm in CH₃CN, which are assigned to ligand-centered character (³LC) [32]. Introducing fluorine atoms into the benzene ring results in an obvious blue-shift of 17 nm for 2 compared to 1. This may be due to the fact that fluorine atoms effectively stabilize the highest occupied molecular orbital (HOMO) [13], which can be further supported by theoretical calculations. The complexes exhibit extremely broad, featureless peaks in the solid state, which are considerably different from those in solution. Furthermore, the emission spectra of 1 and 2 in the solid state demonstrate significant red-shift compared to the spectra recorded in CH₃CN, which can be attributed to the emission of the aggregates [39]. In the solid state, the maximum emission wavelengths of 1 and 2 are determined as 631 and 646 nm, and the absolute quantum yields are 38.5% and 34.5%, respectively (Table S3 in Supporting information). The ultraviolet–visible (UV–vis) absorption spectra of 1 and 2 in CH₃CN at room temperature were presented in Fig. S1 (Supporting information) and the detailed photophysical data were listed in Table S3.

  The strong emission of complexes in the solid state suggests they are likely to exhibit AIPE activities [40]. To confirm the hypothesis, the emission spectra of the complexes were conducted with different water fractions in CH₃CN/H₂O. As depicted in Fig. 1c and Fig. S2 (Supporting information), 1 and 2 exhibit very weak emission at the water fractions ranging from 0% to 80%, and the emission intensities reach the maximum at a water fraction of 90%, demonstrating obvious AIPE activities. Further analysis reveals that the emission intensity of 2 at the water fraction of 90% is much higher than that of 1 at the same conditions (Fig. 1d), showing that the introduction of fluorine atoms clearly influences the AIPE activity of the complex. This can be assigned to the abundant intermolecular hydrogen bonds induced by the fluorine atoms, which leads to enhanced intermolecular interaction, thus limiting molecular motion and resulting in higher AIPE activity of complex 2 [19].

  In this study, we found that the emission intensities of the complexes increased over time at the water fraction of 90% in CH₃CN/H₂O. Thus, we explored the time-dependent emission spectra of 1 and 2. Fig. 1e and Fig. S3 (Supporting information) show that emission intensities of 1 and 2 are very weak at first, but enhance gradually over time. The relative emission intensity ratios of I₆₀₈/I₆₂₄ indicate that 2 reaches equilibrium at about 35 min (Fig. S4 in Supporting information). However, the equilibrium time of 1 is obviously shortened, within around 5 min. The results suggest that the presence of fluorine atoms affects the aggregation process of the complex. Furthermore, transmission electron microscopy (TEM) images show that the aggregates of 1 and 2 are nanofibers (Fig. 1f and Fig. S5 in Supporting information).

  The UV–vis absorption spectra of 1 and 2 were recorded in CH₃CN/H₂O with different water fractions (Fig. S6 in Supporting information). As the water fraction increases, the absorption peaks below 400 nm decrease gradually and a new absorption tail appears at 450–550 nm. This tail can be assigned to metal-metal-to-ligand charge transfer [7,41].

  The electrochemical properties of 1 and 2 in N,N-dimethylformamide (DMF) solution were studied by cyclic voltammetry (Fig. S7 in Supporting information). Compared to 1, the oxidation and reduction potentials of 2 are notably increased. The energy gaps between HOMOs and lowest unoccupied molecular orbital (LUMO) levels of 1 and 2 are 2.16 and 2.24 eV, respectively, which is consistent with the observed blue-shift in the emission spectra (Table S4 in Supporting information) [13,14].

  Density function theory (DFT) calculations were used to explore the electronic structures of 1 and 2. The HOMOs of 1 and 2 are primarily derived from cyclometalating ligands and Pt center, while the LUMOs are mainly distributed on auxiliary ligands and Pt center. The calculated energy gaps for 1 and 2 are 3.53 and 3.68 eV, respectively (Fig. S8 in Supporting information). The introduction of fluorine atoms onto the cyclometalating ligand significantly affected the HOMO level of the complex, leading to a substantial increase in the energy gap.

  Inspired by the high AIPE activity of 2, we used this complex as a probe to detect picric acid (PA) in CH₃CN/H₂O (v/v = 1:9). Complex 2 exhibits strong emission in the absence of PA, but its emission is quenched gradually upon increasing PA concentrations (Fig. 2a). When the concentration of PA reaches 400 µmol/L, 96% of the emission is quenched. The Stern-Volmer plot of I₀/I (I₀ and I represent the emission intensities before and after the addition of PA) vs. PA concentrations shows a non-linear relationship in the range of 0–800 µmol/L (Fig. 2b), indicating the presence of both static and dynamic quenching processes [42,43]. The Stern-Volmer plot shows good linearity in the concentrations of PA ranging from 0 to 20 µmol/L (–, inset), which is mainly due to the static quenching [44,45]. The quenching constant is 2.3 × 10⁴ L/mol and the limit of detection (LOD) of 2 is calculated to be 0.26 µmol/L (Figs. S9 and S10 and Table S5 in Supporting information). These results exhibit that complex 2 can be used as a probe for efficient detection of PA in aqueous media.

  Figure 2

  

  Figure 2.  (a) The emission spectra of 2 at 20 µmol/L in CH₃CN/H₂O (v/v = 1:9) with different concentrations of PA. (b) The Stern-Volmer plot of I₀/I vs. the concentration of PA. Insert: the linear part of Stern-Volmer plot in the concentrations of PA ranging from 0 to 20 µmol/L. I₀ represents emission intensity of 2 and I represents emission intensity of 2 containing different amounts of PA. (c, d) Quenching percentages of 2 with different analytes (c) and ionic compounds (d) in CH₃CN/H₂O (v/v = 1:9) before (red) and after (blue) the addition of PA. (e) The photo of the suspensions of 2 upon the addition of various analytes under UV light. The excitation wavelength was 400 nm.

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  Considering the sensitive detection of 2 for PA, selective experiments were further conducted. The analytes (nitrobenzene (NB), 1,3-dinitrobenzene (1,3-DNB), nitromethane (NM), phenol, p-cresol, 4-methoxyphenol (MEHQ) and m-cresol), and the compounds with different ions (NaHCO₃, KBr, KF, MgSO₄, CuSO₄, CaCl₂, AlCl₃, MnCl₂, NiCl₂ and CoCO₃) were selected to investigate the selectivity for detecting PA. As shown in Fig. S11 (Supporting information), compared with the addition of PA, the emission intensities of 2 do not display a noteworthy alteration upon the addition of other analytes and ionic compounds. The phenomena are also confirmed from the corresponding photos under UV light (Fig. 2e and Fig. S12 in Supporting information) [46]. The above results provide evidence for the high selectivity of complex 2 towards PA. This selectivity may be attributed to the fact that PA acts as a typical electron acceptor, while 2 acts as an excellent electron donor, facilitating a photo-induced electron transfer (PET) process [37,47]. Additionally, the strong electrostatic interactions between PA and 2 can also contribute to the high selectivity [24].

  To evaluate the anti-interference ability of a probe, the competitive experiments were studied. The results display that the quenching percentages of 2 caused by PA remain almost constant in the presence of other competitive analytes and ionic compounds (Figs. 2c and d), indicating that 2 exhibits impressive anti-interference ability in the process of PA recognition.

  To explore practical applications, 2 was used to detect PA in various natural water samples, including tap water, river water and rainwater. Fig. 3 displays the emission spectra and quenching percentages of 2 in different water samples, suggesting that 2 works effectively for detecting PA in natural water samples (CH₃CN/H₂O, v/v = 1:9). So far, the majority of reported Pt(Ⅱ) complexes for the detection of PA have been focused on metallacycles and metallacages from the self-assembly of organoplatinum compounds in organic solvents. To the best of our knowledge, this is the first report of the AIPE-active cationic cyclometalated Pt(Ⅱ) complex for efficient detection of PA in aqueous media. The Pt(Ⅱ) complex 2 contains a C^N type cyclometalating ligand of 2-(2,4-difluorophenyl)-pyridine and 1,10-phenanthroline as the auxiliary ligand. This complex demonstrates a limit of detection of 0.26 µmol/L and excellent selectivity towards PA in aqueous media. Moreover, it performs well for the detection of PA in natural water samples, providing a practical method for detecting PA.

  Figure 3

  

  Figure 3.  The emission spectra (a) and quenching percentages (b) of 2 towards PA in different water samples (CH₃CN/H₂O, v/v = 1:9). The excitation wavelength was 400 nm.

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  The emission quenching mechanism of 2 for PA was explored through DFT calculations. Fig. 4 indicates that the LUMO energy of PA (−3.47 eV) is much lower than that of 2 (−2.58 eV), suggesting that a photo-induced electron transfer (PET) process may occur, leading to the emission quenching [48]. Besides, the energy gaps of 2, PA, and the adduct (2 + PA) are 3.69, 4.34 and 2.71 eV, respectively. Among them, the energy gap of the adduct (2 + PA) is the lowest, showing that the adduct is the most stable. In addition, the ¹H nuclear magnetic resonance (¹H NMR) spectrum of 2 in the presence of PA shows the chemical shifts of proton signals of 2 move towards the high field, supporting the presence of strong electrostatic interactions between PA and 2 (Fig. S13 in Supporting information) [22,49]. These results reveal that the phosphorescent quenching of 2 for the detection of PA is mainly attributed to PET.

  Figure 4

  

  Figure 4.  Calculated energy level diagram of 2, PA and adduct (2 + PA).

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  In summary, two structurally simple cationic Pt(Ⅱ) complexes with AIPE activities have been studied. Complex 2 with a dfppy ligand exhibits much higher AIPE activity than a non-fluorinated complex 1. Complex 2 demonstrates efficient detection on PA with a high quenching constant of 2.3 × 10⁴ L/mol and a low LOD of 0.26 µmol/L in aqueous media. Furthermore, as a sensor for detecting PA, 2 works well in the natural water samples. The detection mechanism is attributed to the photo-induced electron transfer. These findings provide valuable insights in designing efficient AIPE-active Pt(Ⅱ) complexes for the detection of PA in aqueous media.

  Declaration of competing interest

  The authors declare that they have no known competing financial interests or personal relationships that could have appeared to influence the work reported in this paper.

  Acknowledgments

  The authors thank the financial support from the National Natural Science Foundation of China (No. 21978042) and the Fundamental Research Funds for the Central Universities (No. DUT22LAB610).

  Supplementary materials

  Supplementary material associated with this article can be found, in the online version, at doi:10.1016/j.cclet.2023.108819.

  
  
• 1. [1]

     J. Luo, Z. Xie, J.W.Y. Lam, et al., Chem. Commun. 18 (2001) 1740–1741.

  2. [2]

     J. Mei, N.L.C. Leung, R.T.K. Kwok, J.W.Y. Lam, B.Z. Tang, Chem. Rev. 115 (2015) 11718–11940. doi: 10.1021/acs.chemrev.5b00263

  3. [3]

     X. Li, M. Li, M. Yang, et al., Coord. Chem. Rev. 418 (2020) 213358. doi: 10.1016/j.ccr.2020.213358

  4. [4]

     B. Manimaran, P. Thanasekaran, T. Rajendran, et al., Inorg. Chem. 41 (2002) 5323–5325. doi: 10.1021/ic020364n

  5. [5]

     M.X. Zhu, W. Lu, N. Zhu, C.M. Che, Chem. Eur. J. 14 (2008) 9736–9746. doi: 10.1002/chem.200800394

  6. [6]

     J.L.L. Tsai, T. Zou, J. Liu, et al., Chem. Sci. 6 (2015) 3823–3830. doi: 10.1039/C4SC03635B

  7. [7]

     H.K. Cheng, M.C.L. Yeung, V.W.W. Yam, ACS Appl. Mater. Interfaces 9 (2017) 36220–36228. doi: 10.1021/acsami.7b11807

  8. [8]

     J. Wu, Y. Li, C. Tan, et al., Chem. Commun. 54 (2018) 11144–11147. doi: 10.1039/c8cc06839a

  9. [9]

     R. Liang, W. Xiong, X. Bai, L. Du, D.L. Phillips, J. Phys. Chem. C 125 (2021) 11432–11439. doi: 10.1021/acs.jpcc.0c10548

  10. [10]

      X. Yao, W. Zhang, B. Fang, et al., Dyes Pigm. 184 (2021) 108788. doi: 10.1016/j.dyepig.2020.108788

  11. [11]

      C. Li, L. Xu, J. Li, et al., Dyes Pigm. 209 (2023) 110912. doi: 10.1016/j.dyepig.2022.110912

  12. [12]

      C.H. Chen, F.L. Wu, Y.Y. Tsai, C.H. Cheng, Adv. Funct. Mater. 21 (2011) 3150–3158. doi: 10.1002/adfm.201100165

  13. [13]

      H.R. Shahsavari, S. Paziresh, New J. Chem. 45 (2021) 22732–22740. doi: 10.1039/d1nj04242d

  14. [14]

      P. Hamidizadeh, R.B. Aghakhanpour, S. Chamyani, et al., Organometallics 41 (2022) 1325–1333. doi: 10.1021/acs.organomet.2c00064

  15. [15]

      L. Niu, G. Ren, T. Hou, X. Shen, D. Zhu, Inorg. Chem. Commun. 130 (2021) 108737. doi: 10.1016/j.inoche.2021.108737

  16. [16]

      M. Martínez-Junquera, E. Lalinde, M.T. Moreno, et al., Dalton Trans. 50 (2021) 4539–4554. doi: 10.1039/d1dt00480h

  17. [17]

      M. Martínez-Junquera, R. Lara, E. Lalinde, M.T. Moreno, J. Mater. Chem. C 8 (2020) 7221–7233. doi: 10.1039/d0tc01163k

  18. [18]

      L. Schneider, V. Sivchik, K.Y. Chung, et al., Inorg. Chem. 56 (2017) 4459–4467. doi: 10.1021/acs.inorgchem.7b00006

  19. [19]

      X. Yang, H. Guo, X. Xu, et al., Adv. Sci. 6 (2019) 1801930. doi: 10.1002/advs.201801930

  20. [20]

      X. Liu, Y. Han, Y. Shu, J. Wang, H. Qiu, J. Hazard. Mater. 425 (2022) 127987. doi: 10.1016/j.jhazmat.2021.127987

  21. [21]

      L. Wang, W. Chen, W. Song, et al., Chin. Chem. Lett. 34 (2023) 107291. doi: 10.1016/j.cclet.2022.03.014

  22. [22]

      S.K. Patra, B. Sen, M. Rabha, S. Khatua, New J. Chem. 46 (2022) 169–177. doi: 10.1039/d1nj04798a

  23. [23]

      F. Zhu, H. Fang, W. Liu, et al., Mater. Lett. 306 (2022) 130957. doi: 10.1016/j.matlet.2021.130957

  24. [24]

      S. Jiang, L. Meng, W. Ma, et al., Chin. Chem. Lett. 32 (2021) 1037–1040. doi: 10.1016/j.cclet.2020.09.019

  25. [25]

      J. Liu, Y. Xu, C. Qin, et al., Dalton Trans. 48 (2019) 13305–13314. doi: 10.1039/c9dt02751c

  26. [26]

      R. Zhang, L. Zhu, B. Yue, Chin. Chem. Lett. 34 (2023) 108009. doi: 10.1016/j.cclet.2022.108009

  27. [27]

      N. Yan, J. Song, F. Wang, et al., Chin. Chem. Lett. 30 (2019) 1984–1988. doi: 10.1016/j.cclet.2019.09.039

  28. [28]

      Y. Hou, S. Li, Z. Zhang, L. Chen, M. Zhang, Polym. Chem. 11 (2020) 254–258. doi: 10.1039/c9py00895k

  29. [29]

      Y. Hou, R. Shi, H. Yuan, M. Zhang, Chin. Chem. Lett. 34 (2023) 107688. doi: 10.1016/j.cclet.2022.07.031

  30. [30]

      Y. Yan, Z. Yu, C. Liu, X. Jin, Dyes Pigm. 173 (2020) 107949. doi: 10.1016/j.dyepig.2019.107949

  31. [31]

      Y. Xing, L. Wang, C. Liu, X. Jin, Sens. Actuators B: Chem. 304 (2020) 127378. doi: 10.1016/j.snb.2019.127378

  32. [32]

      Y. Yan, Z. Yu, J. Wang, C. Liu, Tetrahedron Lett. 119 (2023) 154427. doi: 10.1016/j.tetlet.2023.154427

  33. [33]

      Y. Chen, Z. Gao, L. Wang, et al., ACS Appl. Polym. Mater. 4 (2022) 1055–1064. doi: 10.1021/acsapm.1c01495

  34. [34]

      Y. Chen, L. Zhang, L. Wang, L. Guo, C. Liu, Mater. Chem. Front. 21 (2021) 7808–7816. doi: 10.1039/d1qm01012c

  35. [35]

      Y. Chen, Y. Shi, Z. Gao, et al., Angew. Chem. Int. Ed. 62 (2023) e202302581. doi: 10.1002/anie.202302581

  36. [36]

      P. He, Y. Chen, X. Li, Y. Yan, C. Liu, Chemosensors 11 (2023) 177. doi: 10.3390/chemosensors11030177

  37. [37]

      P. He, Y. Chen, X. Li, Y. Yan, C. Liu, Dalton Trans. 52 (2023) 128–135. doi: 10.1039/d2dt03537e

  38. [38]

      P. Maity, A. Bhatt, B. Agrawal, A. Jana, Langmuir 33 (2017) 4291–4300. doi: 10.1021/acs.langmuir.7b00869

  39. [39]

      Z. Gong, K. Tang, Y. Zhong, Inorg. Chem. 60 (2021) 6607–6615. doi: 10.1021/acs.inorgchem.1c00403

  40. [40]

      L. Wang, Z. Gao, C. Liu, X. Jin, Mater. Chem. Front. 3 (2019) 1593–1600. doi: 10.1039/c9qm00227h

  41. [41]

      B. Li, Z. Liang, H. Yan, Y. Li. Mol. Syst. Des. Eng. 5 (2020) 1578–1605. doi: 10.1039/d0me00113a

  42. [42]

      Z. Li, Z. Yao, R. Feng, et al., Chin. Chem. Lett. 32 (2021) 3095–3098. doi: 10.3390/w13213095

  43. [43]

      P. Ju, E. Zhang, L. Jiang, et al., RSC Adv. 8 (2018) 21671–21678. doi: 10.1039/c8ra02602e

  44. [44]

      Z. Luo, B. Liu, S. Si, et al., Dyes Pigm. 143 (2017) 463–469. doi: 10.1016/j.dyepig.2017.05.002

  45. [45]

      N. Wang, J. Yang, L. Chen, et al., New J. Chem. 41 (2017) 2786–2792. doi: 10.1039/C6NJ03989H

  46. [46]

      L. Zhang, Y. Sun, Y. Jiang, et al., Chin. Chem. Lett. 31 (2020) 2428–2432. doi: 10.1016/j.cclet.2020.04.003

  47. [47]

      T. Feng, X. Li, J. Wu, C. He, C. Duan, Chin. Chem. Lett. 31 (2020) 95–98. doi: 10.1016/j.cclet.2019.04.059

  48. [48]

      F. Zu, F. Yan, Z. Bai, et al., Microchim. Acta 184 (2017) 1899–1914. doi: 10.1007/s00604-017-2318-9

  49. [49]

      H. Ma, C. He, X. Li, et al., Sens. Actuators B: Chem. 230 (2016) 746–752. doi: 10.1016/j.snb.2016.02.112

• 

  Figure 1  (a) The structures of 1 and 2. (b) Normalized emission spectra (solution: solid trace, solid: dash trace) of 1 (black) and 2 (red) at room temperature (50 µmol/L in CH₃CN). (c) Emission spectra of 2 and (d) emission intensity curves of 1 and 2 at 50 µmol/L in CH₃CN/H₂O with different water fractions. (e) Time-dependent emission spectra of 2 (CH₃CN/H₂O, v/v = 1:9, 50 µmol/L). (f) TEM image of aggregates of 2 (CH₃CN/H₂O, v/v = 1:9, 50 µmol/L). The excitation wavelength was 400 nm.

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  Figure 2  (a) The emission spectra of 2 at 20 µmol/L in CH₃CN/H₂O (v/v = 1:9) with different concentrations of PA. (b) The Stern-Volmer plot of I₀/I vs. the concentration of PA. Insert: the linear part of Stern-Volmer plot in the concentrations of PA ranging from 0 to 20 µmol/L. I₀ represents emission intensity of 2 and I represents emission intensity of 2 containing different amounts of PA. (c, d) Quenching percentages of 2 with different analytes (c) and ionic compounds (d) in CH₃CN/H₂O (v/v = 1:9) before (red) and after (blue) the addition of PA. (e) The photo of the suspensions of 2 upon the addition of various analytes under UV light. The excitation wavelength was 400 nm.

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  Figure 3  The emission spectra (a) and quenching percentages (b) of 2 towards PA in different water samples (CH₃CN/H₂O, v/v = 1:9). The excitation wavelength was 400 nm.

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  Figure 4  Calculated energy level diagram of 2, PA and adduct (2 + PA).

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