Discriminative ‘Turn-on’ Detection of Al3+ and Ga3+ Ions as Well as Aspartic Acid by Two Fluorescent Chemosensors

In this work, two Schiff-base-based chemosensors L1 and L2 containing electron-rich quinoline and anthracene rings were designed. L1 is AIEE active in a MeOH-H2O solvent system while formed aggregates as confirmed by the DLS measurements and fluorescence lifetime studies. The chemosensor L1 was used for the sensitive, selective, and reversible ‘turn-on’ detection of Al3+ and Ga3+ ions as well as Aspartic Acid (Asp). Chemosensor L2, an isomer of L1, was able to selectively detect Ga3+ ion even in the presence of Al3+ ions and thus was able to discriminate between the two ions. The binding mode of chemosensors with analytes was substantiated through a combination of 1H NMR spectra, mass spectra, and DFT studies. The ‘turn-on’ nature of fluorescence sensing by the two chemosensors enabled the development of colorimetric detection, filter-paper-based test strips, and polystyrene film-based detection techniques.


Introduction
Earth's crust consists of various metals, out of which aluminum is the third most abundant [1,2]. Aluminum metal and its compounds enter into the environment through various anthropogenic activities such as building materials, transportation, electronics, industrial effluents, wastewater treatment plants, utensils, and food additives [3][4][5][6]. As a result, aluminum gets absorbed and accumulated in the human body due to its excessive exposure [6][7][8]. Although aluminum is a nonessential metal in the human body, once inside, it competes with other important metals with similar properties (e.g., Mg 2+ , Ca 2+ , and Fe 3+ ions) to bind to various proteins [9][10][11][12]. The high concentration of aluminum in humans can cause severe neurodegenerative diseases such as Alzheimer's, amyotrophic lateral sclerosis, and Parkinson's diseases along with various other diseases including microcytic hypochromic anemia, dialysis encephalopathy, and Al-related bone disease [1,[13][14][15]. As per the World Health Organization (WHO), the permissible limit of aluminum ions in drinking water is 7.4 µM while the daily average intake should not exceed 3-10 mg [15][16][17]. Therefore, efforts have been made to develop efficient sensors that can detect aluminum ion (Al 3+ ) selectively and sensitively [10]. Similarly, gallium ions (Ga 3+ ), belonging to the identical IIIA group as Al 3+ , have also been recognized as a potential risk to human health [4,[18][19][20].
Amino acids, as building blocks, are essential for living organisms for various vital functions [21][22][23]. Amongst all nonessential amino acids, Aspartic Acid (Asp) plays several critical roles in various biological and physiological processes [24][25][26]. Asp is specifically required for its role in the tricarboxylic acid (TCA) cycle [27,28]. Asp also serves as the main precursor for the synthesis of two amino acids, i.e., Glutamic acid and Glycine [24,29]. Asp acts as a major excitatory neurotransmitter in the mammalian central nervous system [24,30]. Studies have shown the use of K + Asp as a cure for heart and liver diseases and diabetes, but a higher amount of Asp can also cause Lou Gehrig's disease, and it is also connected 149. 19 13

Physical Measurements
FTIR spectra (Zn-Se ATR) were recorded using a PerkinElmer, USA Spectrum-Two spectrometer. NMR spectra were obtained from a JEOL, Japan 400 MHz spectrometer. High-resolution mass spectra were obtained with an Agilent G6530AA, USA (Q-TOF LC-HRMS) mass spectrometer. Fluorescence spectral studies were performed with a Cary Eclipse fluorescence spectrometer or Edinburgh Instrument, UK FLS 900 luminescence spectrometer. Time-resolved fluorescence spectra were recorded using a picosecond Fluorimeter from Horiba Jobin Yvon (FluoroHub), USA. DLS measurements were recorded on a Malvern zetasizer ZS90 instrument, UK.

Crystallography
X-ray diffraction intensity data of L1 (CCDC No. 2232788) were collected at 298 K on a Bruker SMART APEX-II CCD diffractometer equipped with graphite-monochromatic Mo Kα radiation (λ = 0.71073 Å) [43]. The structure was solved using direct methods using the SIR97 program [44] and was refined on F 2 using all data by full-matrix least squares procedures with SHELXL 2018/3 [45]. The hydrogen atoms were placed at the calculated positions and were included in the last cycles of the refinement. All the calculations were conducted using the WinGX (ver. 2018.3) software package [46]. The crystallographic data collection and structure solution parameters are summarized in Table S1 in the Supplementary Materials.

DFT Studies
The geometrical optimization of chemosensors L1 and L2 and their complexes L1-Al 3+ , L1-Ga 3+ , and L2-Ga 3+ was achieved under C1 symmetry by employing the density functional theory (DFT) method [47]. Becke's three parameter exchange correlation functional by Lee, Yang, and Parr (B3LYP) was utilized as a hybrid functional for the calculations using Gaussian09W suits [48]. Two different basis sets were used for the geometrical optimization: viz., LANL2DZ for the Al 3+ and Ga 3+ ions and 6-311 + G (d, p) for the rest of the atoms [49,50]. The solvent effect was taken into account with a conductor-like polarizable continuum model (CPCM) using ethanol as a solvent [51]. The optimized geometries were subjected to frequency calculations to confirm if the global minima was achieved. The frontier molecular orbitals (FMOs) and molecular electrostatic potential surfaces were visualized using the optimized structures. All geometrical modifications were made using GaussView 5.0 package [52]. The FMOs were plotted using the Avogadro software [53].

Determination of Binding Constant (K b )
The binding constant (K b ) was computed using the Benesi-Hildebrand Equation (1) where I, I 0 , and I max are the emission intensities of the chemosensors (L1 or L2) in the presence of analytes (Al 3+ , Ga 3+ , or Asp), in the absence of analytes, and the maximum fluorescence intensity in the presence of the analytes, respectively [54]. K b was obtained by using the ratio of the intercept and slope from 1/(I − I 0 ) vs. 1/[A] plot where [A] refers to the concentration of analytes, i.e., Al 3+ , Ga 3+ , or Asp.

Determination of Detection Limit
The detection limit was calculated from the fluorescence spectral titration according to Equation (2), where k is the slope of a plot of the emission intensity of the chemosensors (L1 or L2) versus the concentration of analytes (Al 3+ , Ga 3+ or Asp) while σ is the standard deviation of ten blank replicate fluorescence measurements of chemosensors (L1 or L2) [55,56].

Determination of Quantum Yield
The relative fluorescence quantum yields (Φ F ) of L1, L1 at f w = 70% L1-Al, L1-Ga, L1-Asp, L2, and L2-Ga were calculated using Equation (3) [57][58][59]: where Φ F is the fluorescence quantum yield of the samples. Here in the equation, the subscripts u and st refer to the unknown and standard samples, respectively. Φ st refers to the fluorescence quantum yield of the Quinine sulfate (Φ st = 0.54) used as the standard sample here. A u and A st are the absorbance of the unknown and standard samples, respectively. S u and S st refer to the integrated emission band areas of the unknown and standard samples, respectively. nD st and nD u represent the solvent refractive index of the standard and the unknown sample, respectively.

Colorimetric Analysis
For colorimetric analysis, standard solutions of assorted metal ions and amino acids (2.5 equiv.) were added to a solution of chemosensor L1 in EtOH. Their photographs were taken under a UV lamp (λ ex = 365 nm) [4,56].

Fabrication of Filter Paper Strips
Strips of Whatman filter paper were dipped in an ethanolic solution of chemosensor L1 followed by drying in the open air to prepare the test strips. Such L1 coated test strips were dipped into an aqueous solution of Al 3+ and Ga 3+ ions as well as Asp (2.5 equiv.). These paper test strips were then investigated under the UV lamp (λ ex = 365 nm) [58,59].

Fabrication of Polystyrene Films
The chemosensor L1 was mixed with styrene (0.5 mL) and α,α'-azoisobutyronitrile (AIBN; 1 mg) in EtOH (0.5 mL). The resultant mixture was heated in a water bath at 80 • C for 30 min. Subsequently, a few drops of the hot clear solution were poured over a glass slide and the resultant glass slide was dried in air to produce the thin films of chemosensor L1-loaded polystyrene. Such polystyrene films were peeled off from the glass slide and were used to detect Al 3+ and Ga 3+ ions as well as Asp by dipping them in their respective aqueous solutions (2.5 equiv.). These polystyrene films were then photographed under the UV lamp (λ ex = 365 nm) [4,57].

Synthesis and Characterization of Chemosensors L1 and L2
An anthracene-based aldehyde, L', was synthesized by reacting o-vanillin with 9-(chloromethyl)anthracene (Scheme 1). L' was characterized by various spectroscopic studies ( Figures S1-S4). The chemosensors L1 and L2 were synthesized by the condensation of L' with 3-aminoquinoline and 5-aminoquinoline, respectively (Scheme 1). The positional isomers L1 and L2 were characterized by various spectroscopic techniques. Both L1 and L2 displayed the characteristic ν C = N stretches at 1626 and 1623 cm −1 , respectively ( Figures S5 and S9). 1 (Figures S8 and S12). To further authenticate the molecular structure, L1 was characterized by the single crystal X-ray diffraction technique (Scheme 1). L1 crystallized in a centrosymmetric space group C2/c. Notably, arene, quinoline, and anthracene rings were making different angles with each other due to the electron cloud repulsion and thus created a cavity to potentially accommodate a suitable analyte.
For colorimetric analysis, standard solutions of assorted metal ions and amino acids (2.5 equiv.) were added to a solution of chemosensor L1 in EtOH. Their photographs were taken under a UV lamp (λex = 365 nm) [4,56].

Fabrication of Filter Paper Strips
Strips of Whatman filter paper were dipped in an ethanolic solution of chemosensor L1 followed by drying in the open air to prepare the test strips. Such L1 coated test strips were dipped into an aqueous solution of Al 3+ and Ga 3+ ions as well as Asp (2.5 equiv.). These paper test strips were then investigated under the UV lamp (λex = 365 nm) [58,59].

Fabrication of Polystyrene Films
The chemosensor L1 was mixed with styrene (0.5 mL) and α,α'-azoisobutyronitrile (AIBN; 1 mg) in EtOH (0.5 mL). The resultant mixture was heated in a water bath at 80 °C for 30 min. Subsequently, a few drops of the hot clear solution were poured over a glass slide and the resultant glass slide was dried in air to produce the thin films of chemosensor L1-loaded polystyrene. Such polystyrene films were peeled off from the glass slide and were used to detect Al 3+ and Ga 3+ ions as well as Asp by dipping them in their respective aqueous solutions (2.5 equiv.). These polystyrene films were then photographed under the UV lamp (λex = 365 nm) [4,57].

Synthesis and Characterization of Chemosensors L1 and L2
An anthracene-based aldehyde, L', was synthesized by reacting o-vanillin with 9-(chloromethyl)anthracene (Scheme 1). L' was characterized by various spectroscopic studies ( Figures S1-S4). The chemosensors L1 and L2 were synthesized by the condensation of L' with 3-aminoquinoline and 5-aminoquinoline, respectively (Scheme 1). The positional isomers L1 and L2 were characterized by various spectroscopic techniques. Both L1 and L2 displayed the characteristic νC = N stretches at 1626 and 1623 cm -1 , respectively ( (Figures S8 and S12). To further authenticate the molecular structure, L1 was characterized by the single crystal X-ray diffraction technique (Scheme 1). L1 crystallized in a centrosymmetric space group C2/c. Notably, arene, quinoline, and anthracene rings were making different angles with each other due to the electron cloud repulsion and thus created a cavity to potentially accommodate a suitable analyte.

AIEE Studies
Both L1 and L2 were soluble in various polar and nonpolar solvents such as MeOH, EtOH, THF, CHCl 3 , DCM, DMF, and DMSO but were insoluble in water. Therefore, in order to induce AIEE, the optical properties of L1 and L2 were examined in MeOH (c, 50 µM) after adding different percentages of water (f w = 0 to 95%). In fluorescence spectra, as the percentage of water (f w , %) increased from 0 to 60 in a MeOH solution of L1, the emission intensity increased constantly at 411 nm and attained a maxima at this wavelength ( Figure 1a). This enhancement is attributed to the aggregation of L1 [32,38]. Notably, as the water percentage was further increased to 70%, a significant bathochromic shift to 460 nm (∆λ = 50 nm) was observed. Furthermore, when the water percentage was further increased, the emission intensity decreased but without any shift in wavelength. At f w = 95%, the emission bands were distributed equally at both wavelengths. We believe as the hydrophobic anthracene rings repel water, they minimize their contact with water and thus rupture the aggregates beyond a water percentage of 70% [62,63]. Figure 1b displays changes at various percentages of water varying from 10% to 95% in a MeOH-H 2 O system under UV light. Notably, the emission spectrum of L2 did not display any change with different percentages of water and hence L2 was AIEE inactive ( Figure S15) [32]. In the case of L1, aggregate formation was confirmed by the dynamic light scattering (DLS) studies ( Figure 2). DLS measurements revealed that the average diameter of the aggregates increased from 118 nm at f w = 10% to 610 nm at f w = 70%. However, at f w = 95%, the size of aggregates decreased to 293 nm. These results thus confirm that not only does L1 form aggregates in the presence of water, but maximum aggregation was possible at f w = 70%.    Time-resolved fluorescence spectroscopy was employed to further confirm AIEE and aggregate formation in L1. Since lifetime measurements are independent of the excitation wavelength and concentration, such studies are more conclusive [64]. The fluorescence lifetime (τav) increased from 3.38 ns at fw = 0 % to 5.73 ns at fw = 70%, implying the aggregate formation ( Figure S16 and Table S2). However, τav decreased to 4.47 ns at fw = 95%, further confirming that the maximum aggregation was possible at fw = 70%. To obtain further support, the fluorescence quantum yield (ΦF) was calculated for L1. The quantum yield was very low (ΦF = 0.008) at fw = 0%; however, it increased nearly four-fold at fw = 70% (ΦF = 0.031). As expected, ΦF again decreased to 0.023 at fw = 95%, confirming the formation of maximum aggregates only at fw = 70%.
For L1, both the low quantum yield and lifetime at fw = 0% suggested the operation of Photoinduced Electron Transfer (PET) from imine-N and phenolic-OR (R: -CH2-) to the quinoline and anthracene moieties, respectively (Scheme 2). In addition, the intramolecular rotation of the imine-C bond further quenched the emission intensity via nonradiative decay at fw = 0%. However, as water was added, both imine-N and phenolic-OR groups started forming H-bonds with the water molecule(s), which in turn subdued PET and re- Time-resolved fluorescence spectroscopy was employed to further confirm AIEE and aggregate formation in L1. Since lifetime measurements are independent of the excitation wavelength and concentration, such studies are more conclusive [64]. The fluorescence lifetime (τ av ) increased from 3.38 ns at f w = 0 % to 5.73 ns at f w = 70%, implying the aggregate formation ( Figure S16 and Table S2). However, τ av decreased to 4.47 ns at f w = 95%, further confirming that the maximum aggregation was possible at f w = 70%. To obtain further support, the fluorescence quantum yield (Φ F ) was calculated for L1. The quantum yield was very low (Φ F = 0.008) at f w = 0%; however, it increased nearly four-fold at f w = 70% (Φ F = 0.031). As expected, Φ F again decreased to 0.023 at f w = 95%, confirming the formation of maximum aggregates only at f w = 70%.
For L1, both the low quantum yield and lifetime at f w = 0% suggested the operation of Photoinduced Electron Transfer (PET) from imine-N and phenolic-OR (R: -CH 2 -) to the quinoline and anthracene moieties, respectively (Scheme 2). In addition, the intramolecular rotation of the imine-C bond further quenched the emission intensity via nonradiative decay at f w = 0%. However, as water was added, both imine-N and phenolic-OR groups started forming H-bonds with the water molecule(s), which in turn subdued PET and restricted the intramolecular bond rotation [32,65,66]. Moreover, fluorescence resonance energy transfer (FRET) also occurred from the anthracene ring to the quinoline ring [67]. As a result, aggregation occurred, and the emission intensity increased. stricted the intramolecular bond rotation [32,65,66]. Moreover, fluorescence resonance energy transfer (FRET) also occurred from the anthracene ring to the quinoline ring [67]. As a result, aggregation occurred, and the emission intensity increased.

Detection of Al 3+ and Ga 3+ Ions by UV-Vis Spectral Studies
To understand the detection ability of L1 and L2, absorption spectra of L1 (c, 20 μM) and L2 (c, 20 μM) were examined in the presence of 2.5 equiv. of assorted metal ions (Ag + , Cd 2+ , Mn 2+ , Zn 2+ , Hg 2+ , K + , Na + , Co 2+ , Pd 2+ , Mg 2+ , Pb 2+ , Be 2+ , Ni 2+ , Sn 2+ , Li + , Cr 3+ , Fe 2+ , Fe 3+ , Cu 2+ , Al 3+ , Ga 3+ , In 3+ ) ( Figure 3). The absorption spectra of L1 did not show prominent changes with any of the metal ions except the Al 3+ and Ga 3+ ions. In contrast, the absorption spectra of L2 displayed a significant change only in the presence of Ga 3+ ions. During the absorption spectral titration of L1, the spectral bands at 333, 365, and 385 nm were altered with an isosbestic point at 360 nm, suggesting the formation of a new species ( Figure S17). In the case of L2, the band at 348 nm decreased while two new bands appeared at 270 and 465 nm with an isosbestic point at 283 nm [56]. These spectral titrations supported the formation of a complex between the chemosensors and metal ions.

Detection of Al 3+ and Ga 3+ Ions by UV-Vis Spectral Studies
To understand the detection ability of L1 and L2, absorption spectra of L1 (c, 20 µM) and L2 (c, 20 µM) were examined in the presence of 2.5 equiv. of assorted metal ions (Ag + , Cd 2+ , Mn 2+ , Zn 2+ , Hg 2+ , K + , Na + , Co 2+ , Pd 2+ , Mg 2+ , Pb 2+ , Be 2+ , Ni 2+ , Sn 2+ , Li + , Cr 3+ , Fe 2+ , Fe 3+ , Cu 2+ , Al 3+ , Ga 3+ , In 3+ ) ( Figure 3). The absorption spectra of L1 did not show prominent changes with any of the metal ions except the Al 3+ and Ga 3+ ions. In contrast, the absorption spectra of L2 displayed a significant change only in the presence of Ga 3+ ions. During the absorption spectral titration of L1, the spectral bands at 333, 365, and 385 nm were altered with an isosbestic point at 360 nm, suggesting the formation of a new species ( Figure S17). In the case of L2, the band at 348 nm decreased while two new bands appeared at 270 and 465 nm with an isosbestic point at 283 nm [56]. These spectral titrations supported the formation of a complex between the chemosensors and metal ions.
with any of the metal ions except the Al 3+ and Ga 3+ ions. In contrast, the absorption spectra of L2 displayed a significant change only in the presence of Ga 3+ ions. During the absorption spectral titration of L1, the spectral bands at 333, 365, and 385 nm were altered with an isosbestic point at 360 nm, suggesting the formation of a new species ( Figure S17). In the case of L2, the band at 348 nm decreased while two new bands appeared at 270 and 465 nm with an isosbestic point at 283 nm [56]. These spectral titrations supported the formation of a complex between the chemosensors and metal ions.

Detection of Al 3+ and Ga 3+ Ions by Fluorescence Spectral Studies
The emission spectra of both chemosensors L1 (c, 20 µM) and L2 (c, 20 µM) were measured in the presence of 2.5 equiv. of different metal ions: Ag + , Cd 2+ , Mn 2+ , Zn 2+ , Hg 2+ , K + , Na + , Co 2+ , Pd 2+ , Mg 2+ , Pb 2+ , Be 2+ , Ni 2+ , Sn 2+ , Li + , Cr 3+ , Fe 2+ , Fe 3+ , Cu 2+ , Al 3+ , Ga 3+ , and In 3+ (Figure 4). In the case of L1, the emission spectral profile remained unchanged in the presence of nearly all the metal ions except for the Al 3+ and Ga 3+ ions. It is significant to note that L1 showed a 'turn-on' response in the presence of both Al 3+ and Ga 3+ ions with the observation of a new emission band at 465 nm. In contrast, L2 displayed an enhanced emission at 430 nm only in the presence of Ga 3+ ions while no change was noted with the Al 3+ ion as well as other metal ions [6]. Therefore, the chemosensor L2 was able to discriminate between the Al 3+ and Ga 3+ ions. The bar diagram nicely illustrates the change in the emission intensity of L1 and L2 after the addition of different metal ions (Figure 4c). It is important to mention that both chemosensors did not exhibit any spectral change with the In 3+ ion. Al 3+ ion as well as other metal ions [6]. Therefore, the chemosensor L2 was able to discriminate between the Al 3+ and Ga 3+ ions. The bar diagram nicely illustrates the change in the emission intensity of L1 and L2 after the addition of different metal ions (Figure 4c). It is important to mention that both chemosensors did not exhibit any spectral change with the In 3+ ion. To determine the extent of binding, emission spectral titrations were performed (Figure 5a-c). From the concentration variation plots, binding constants (Figures 5d-f) and detection limits (Figures 5g-i) were calculated by using the linear fitting methods. L1 displayed high binding constants of 3.58 × 10 4 and 2.80 × 10 4 M -1 for the Al 3+ and Ga 3+ ions, respectively [54,68]. Further, L1 exhibited remarkable detection limits of 0.19 and 0.22 μM for the Al 3+ and Ga 3+ ions, respectively [69]. On the other hand, L2 displayed a detection limit of 1.31 μM and a binding constant of 2.24 × 10 3 M -1 towards the Ga 3+ ion, which was impressive but a little inferior to that of L1. Importantly, both the detection limit and linear range of the metal ions exhibited by the present chemosensor were better than that of other chemosensors reported in the literature (Table S3). To determine the extent of binding, emission spectral titrations were performed (Figure 5a-c). From the concentration variation plots, binding constants (Figure 5d-f) and detection limits (Figure 5g-i) were calculated by using the linear fitting methods. L1 displayed high binding constants of 3.58 × 10 4 and 2.80 × 10 4 M −1 for the Al 3+ and Ga 3+ ions, respectively [54,68]. Further, L1 exhibited remarkable detection limits of 0.19 and 0.22 µM for the Al 3+ and Ga 3+ ions, respectively [69]. On the other hand, L2 displayed a Sensors 2023, 23, 1798 9 of 20 detection limit of 1.31 µM and a binding constant of 2.24 × 10 3 M −1 towards the Ga 3+ ion, which was impressive but a little inferior to that of L1. Importantly, both the detection limit and linear range of the metal ions exhibited by the present chemosensor were better than that of other chemosensors reported in the literature (Table S3).

Selectivity, Lifetime, and Quantum Yield Measurements
For a chemosensor, selectivity towards a particular analyte is crucial as a chemosensor may have to identify a specific analyte in a competing environment [70,71]. Thus, the selectivity of L1 and L2 towards Al 3+ /Ga 3+ ions in the presence of other competing metal ions was attempted by studying the competitive binding studies (Figures 6 and S18). The emission spectra of L1 and L2 were recorded with Al 3+ /Ga 3+ ions in the presence of the equimolar concentration of other metal ions. Both for L1 and L2, no measurable change in the emission intensity was observed towards the detection of Al 3+ /Ga 3+ ions in the presence of different metal ions including In 3+ ions. Notably, for L2, the emission intensity was unaffected even in the presence of Al 3+ ions. It is, therefore, evident that both L1 and L2 were highly selective for Al 3+ /Ga 3+ ions even in the presence of assorted metal ions.  Determination of binding constants by Benesi-Hildebrand plots for the detection of (d) Al 3+ ion, (e) Ga 3+ ion by L1, and (f) Ga 3+ ion by L2 from the emission spectral profiles. Determination of detection limit of L1 towards the (g) Al 3+ ion, (h) Ga 3+ ion, and (i) L2 towards the Ga 3+ ion. All studies were carried out in EtOH.

Selectivity, Lifetime, and Quantum Yield Measurements
For a chemosensor, selectivity towards a particular analyte is crucial as a chemosensor may have to identify a specific analyte in a competing environment [70,71]. Thus, the selectivity of L1 and L2 towards Al 3+ /Ga 3+ ions in the presence of other competing metal ions was attempted by studying the competitive binding studies (Figures 6 and S18). The emission spectra of L1 and L2 were recorded with Al 3+ /Ga 3+ ions in the presence of the equimolar concentration of other metal ions. Both for L1 and L2, no measurable change in the emission intensity was observed towards the detection of Al 3+ /Ga 3+ ions in the presence of different metal ions including In 3+ ions. Notably, for L2, the emission intensity was unaffected even in the presence of Al 3+ ions. It is, therefore, evident that both L1 and L2 were highly selective for Al 3+ /Ga 3+ ions even in the presence of assorted metal ions. selectivity of L1 and L2 towards Al /Ga ions in the presence of other competing metal ions was attempted by studying the competitive binding studies (Figures 6 and S18). The emission spectra of L1 and L2 were recorded with Al 3+ /Ga 3+ ions in the presence of the equimolar concentration of other metal ions. Both for L1 and L2, no measurable change in the emission intensity was observed towards the detection of Al 3+ /Ga 3+ ions in the presence of different metal ions including In 3+ ions. Notably, for L2, the emission intensity was unaffected even in the presence of Al 3+ ions. It is, therefore, evident that both L1 and L2 were highly selective for Al 3+ /Ga 3+ ions even in the presence of assorted metal ions.  The excitation energy of a chemosensor may change after its interaction with an analyte. Hence, the excited state behavior of L1 and L2 in the absence and presence of Al 3+ /Ga 3+ ions was evaluated through the lifetime measurements [70]. L1 exhibited a biexponential decay with an average lifetime (τ av ) of 3.38 ns. In the presence of Al 3+ and Ga 3+ ions, τ av increased to 14.12 and 13.62 ns, respectively (Figures 7a and S19, and Table S2). A similar four-fold enhancement in τ av of L1 in the presence of Al 3+ and Ga 3+ ions suggested that both these ions offered a similar mode of interaction with L1. However, L2 displayed a triexponential decay with τ av of 0.77 ns, which increased 1.5-fold times to 1.17 ns in the presence of Ga 3+ ions (Figure 7b). The quantum yields of L1 and L2 were also measured in the absence and presence of Al 3+ / Ga 3+ ions by taking Quinine sulfate (Φ F = 0.54) as a reference [55]. The resultant Φ F for L1, L1−Al 3+ , and L1−Ga 3+ were found to be 0.008, 0.065, and 0.062, respectively. Thus, enhancement in the quantum yield was approximately eight-fold both for the Al 3+ and Ga 3+ ions. The calculated Φ F for L2−Ga 3+ (0.010) displayed a 2.5-fold enhancement when compared to L2 (0.003). These results further support the fluorescence lifetime studies. Collectively, all studies suggest that the binding mechanisms of L1 and L2 towards the Al 3+ /Ga 3+ ions were different. The excitation energy of a chemosensor may change after its interaction with an analyte. Hence, the excited state behavior of L1 and L2 in the absence and presence of Al 3+ /Ga 3+ ions was evaluated through the lifetime measurements [70]. L1 exhibited a biexponential decay with an average lifetime (τav) of 3.38 ns. In the presence of Al 3+ and Ga 3+ ions, τav increased to 14.12 and 13.62 ns, respectively (Figures 7a and S19, and Table S2). A similar four-fold enhancement in τav of L1 in the presence of Al 3+ and Ga 3+ ions suggested that both these ions offered a similar mode of interaction with L1. However, L2 displayed a triexponential decay with τav of 0.77 ns, which increased 1.5-fold times to 1.17 ns in the presence of Ga 3+ ions (Figure 7b). The quantum yields of L1 and L2 were also measured in the absence and presence of Al 3+ / Ga 3+ ions by taking Quinine sulfate (ΦF = 0.54) as a reference [55]. The resultant ΦF for L1, L1Al 3+ , and L1Ga 3+ were found to be 0.008, 0.065, and 0.062, respectively. Thus, enhancement in the quantum yield was approximately eightfold both for the Al 3+ and Ga 3+ ions. The calculated ΦF for L2Ga 3+ (0.010) displayed a 2.5fold enhancement when compared to L2 (0.003). These results further support the fluorescence lifetime studies. Collectively, all studies suggest that the binding mechanisms of L1 and L2 towards the Al 3+ /Ga 3+ ions were different.

Reversibility Studies
The reversibility of a chemosensor is an essential requirement that endows it for practical applications. The reversibility of L1-Al 3+ and L1-Ga 3+ complexes was checked with various anions; however, the reversibility was only achieved by the addition of fluoride ions (as NaF) (Figure 8) [6]. In fact, the Fion was able to show multiples cycles of reversibility without any potential loss in the chemical and emission behavior of L1. Such a fact suggests that the Fion removed the Al 3+ and Ga 3+ ions from their metal complexes while generating free L1 and were ready for the next round of detection of Al 3+ and Ga 3+ ions.

Reversibility Studies
The reversibility of a chemosensor is an essential requirement that endows it for practical applications. The reversibility of L1-Al 3+ and L1-Ga 3+ complexes was checked with various anions; however, the reversibility was only achieved by the addition of fluoride ions (as NaF) (Figure 8) [6]. In fact, the F − ion was able to show multiples cycles of reversibility without any potential loss in the chemical and emission behavior of L1. Such a fact suggests that the F − ion removed the Al 3+ and Ga 3+ ions from their metal complexes while generating free L1 and were ready for the next round of detection of Al 3+ and Ga 3+ ions.

Reversibility Studies
The reversibility of a chemosensor is an essential requirement that endows it for practical applications. The reversibility of L1-Al 3+ and L1-Ga 3+ complexes was checked with various anions; however, the reversibility was only achieved by the addition of fluoride ions (as NaF) (Figure 8) [6]. In fact, the Fion was able to show multiples cycles of reversibility without any potential loss in the chemical and emission behavior of L1. Such a fact suggests that the Fion removed the Al 3+ and Ga 3+ ions from their metal complexes while generating free L1 and were ready for the next round of detection of Al 3+ and Ga 3+ ions.

Mode of Binding
The absorption and emission spectral studies confirmed the interaction and/or binding of Al 3+ /Ga 3+ ions to L1 and L2. Both chemosensors L1 and L2 offer three types of functional groups: phenolic-OR (R = -CH 2 -or -CH 3 ), imine-N, and quinoline-N. Both Al 3+ and Ga 3+ ions are hard acids and are thus likely to interact and/or bind preferentially with the phenolic-OR followed by imine-N [4,14]. For positional isomers L1 and L2, the position of the quinoline-N is likely to play a crucial role. In the case of L1, the binding of a metal ion through phenolic-OR (R = -CH 2 -), imine-N, and quinoline-N results in the formation of both six-and five-membered chelate rings and supports chelation-enhanced fluorescence. It is important to mention that a metal ion (Al 3+ /Ga 3+ ) is situated significantly above (approx. 2.7-2.8 Å) the plane of L1 to facilitate the simultaneous coordination of phenolic-OR, imine-N, and quinoline groups, as depicted by the DFT studies (vide infra). Due to the formation of such chelate rings, L1 achieves structural rigidity while the intramolecular bond rotation of the imine-N group becomes restricted (Scheme 3). At the same time, excited-state electron transfer from imine-N and phenolic-OR to quinoline rings and anthracenyl moieties also gets inhibited. Collectively, these points suppress the PET [72,73]. Moreover, as PET is subdued, the fluorescence resonance energy transfer (FRET) takes place between the anthracene and quinoline rings [2]. Therefore, as a result of the turning off of the PET process and turning-on of CHEF and FRET, the emission intensity of L1 increases in the presence of Al 3+ /Ga 3+ ions. The absorption and emission spectral studies confirmed the interaction and/or binding of Al 3+ /Ga 3+ ions to L1 and L2. Both chemosensors L1 and L2 offer three types of functional groups: phenolic-OR (R = -CH2-or -CH3), imine-N, and quinoline-N. Both Al 3+ and Ga 3+ ions are hard acids and are thus likely to interact and/or bind preferentially with the phenolic-OR followed by imine-N [4,14]. For positional isomers L1 and L2, the position of the quinoline-N is likely to play a crucial role. In the case of L1, the binding of a metal ion through phenolic-OR (R = -CH2-), imine-N, and quinoline-N results in the formation of both six-and five-membered chelate rings and supports chelation-enhanced fluorescence. It is important to mention that a metal ion (Al 3+ /Ga 3+ ) is situated significantly above (approx. 2.7-2.8 Å) the plane of L1 to facilitate the simultaneous coordination of phenolic-OR, imine-N, and quinoline groups, as depicted by the DFT studies (vide infra). Due to the formation of such chelate rings, L1 achieves structural rigidity while the intramolecular bond rotation of the imine-N group becomes restricted (Scheme 3). At the same time, excited-state electron transfer from imine-N and phenolic-OR to quinoline rings and anthracenyl moieties also gets inhibited. Collectively, these points suppress the PET [72,73]. Moreover, as PET is subdued, the fluorescence resonance energy transfer (FRET) takes place between the anthracene and quinoline rings [2]. Therefore, as a result of the turning off of the PET process and turning-on of CHEF and FRET, the emission intensity of L1 increases in the presence of Al 3+ /Ga 3+ ions. Scheme 3. Sensing mechanism of L1 towards Al 3+ /Ga 3+ ions via fluorescence 'turn-on' strategy.
All studies pointed to a similar mode of binding of both Al 3+ and Ga 3+ ions with L1. To further confirm the binding mode of L1, an 1 H NMR spectral titration with Al 3+ ions was performed (Figures 9 and S20). When sequentially adding one equivalent of Al 3+ ions to a solution of L1, imine-N, phenolic-OR (R = -CH2-), and quinoline-N were shifted downfield, confirming their involvement in binding to the Al 3+ ion. Moreover, the quinoline ring protons also shifted downfield, thus further confirming their role in binding. Importantly, both -CH2-and -CH3 protons were completely resolved, indicating a difference in their chemical environment after the binding of the Al 3+ ion. Further, anthracene ring protons were also perturbed after the potential coordination of an Al 3+ ion. Notably, various aromatic protons were found to split to give multiplets. We propose that imine-N, Scheme 3. Sensing mechanism of L1 towards Al 3+ /Ga 3+ ions via fluorescence 'turn-on' strategy.
All studies pointed to a similar mode of binding of both Al 3+ and Ga 3+ ions with L1. To further confirm the binding mode of L1, an 1 H NMR spectral titration with Al 3+ ions was performed (Figures 9 and S20). When sequentially adding one equivalent of Al 3+ ions to a solution of L1, imine-N, phenolic-OR (R = -CH 2 -), and quinoline-N were shifted downfield, confirming their involvement in binding to the Al 3+ ion. Moreover, the quinoline ring protons also shifted downfield, thus further confirming their role in binding. Importantly, both -CH 2 -and -CH 3 protons were completely resolved, indicating a difference in their chemical environment after the binding of the Al 3+ ion. Further, anthracene ring protons were also perturbed after the potential coordination of an Al 3+ ion. Notably, various aromatic protons were found to split to give multiplets. We propose that imine-N, phenolic-OR, and quinoline-N form a pocket in which a metal ion nicely resides. Such a binding mode affects the chemical environment of nearby arene rings and hence multiplets were observed [4].
OR and imine-N displayed a downfield shift whereas both quinoline and anthracene rings remained unaffected ( Figure S21).
To characterize the actual species formed between L1 and Al 3+ /Ga 3+ ions, ESI + mass spectra were recorded. The mass spectra of L1Al 3+ species displayed a peak at m/z 673.27 which corresponded to [L1 + Al 3+ + 2NO3 -+ OCH3 -+ Na + ] + . On the other hand, L1Ga 3+ species showed a peak at m/z 669.30 corresponding to [L1 + Ga 3+ + 3OCH3 -+ K + ] + ( Figures  S22 and S23). The sources of the NO3 -and OCH3 -ions were from an aluminum precursor, Al(NO3)3, and a CH3OH solvent, respectively. It is important to note that, for both species, the isotopic distribution patterns nicely matched that of the simulated patterns. The mass spectra further asserted a 1:1 metal binding stoichiometry to L1 [58]. The said binding stoichiometry was further confirmed by Job's plot for both Al 3+ and Ga 3+ ions ( Figure S24) [59].  Figure S20 for full-range spectrum.

DFT Studies
All chemical structures were optimized by the DFT using the suitable basis sets and functional (see Table S4 for the Cartesian coordinates). The molecular electrostatic potential surface (MESP) maps are often employed for the qualitative investigation of the charge distribution in a system. Hence, the optimized structures of chemosensors L1 and L2 were used to study the electropositive and electronegative centers. As shown in Figure 10, the electrostatic potential was scaled between −47.0 and +32.0 kcal/mol for both L1 and L2 with their approximate values marked. Notably, both oxygen and nitrogen centers in L1 and L2 were relatively more electronegative as depicted from the red-colored region around them. The MESP maps therefore suggest that the metal ions can bind with these groups: quoniline-N, imine-N, and phenolic-OR (-CH2-). In L2, the position of quinoline-N was changed, which is now anti to the imine-N group. As a result, the formation of a common binding pocket was not possible. It is therefore proposed that a larger Ga 3+ ion is able to interact with both phenolic-OR (R = -CH 2 -, -CH 3 ) groups and imine-N. As the Al 3+ ion is smaller in size, it could not interact with all three groups, and hence L2 did not show its recognition. The enhanced emission was observed due to the suppression of PET and 'turn-on' of CHEF. As the quinoline ring was not involved in binding to a Ga 3+ ion, FRET was not operative [74,75]. This proposition was further confirmed by the 1 H NMR spectral studies where protons of both phenolic-OR and imine-N displayed a downfield shift whereas both quinoline and anthracene rings remained unaffected ( Figure S21).
To characterize the actual species formed between L1 and Al 3+ /Ga 3+ ions, ESI + mass spectra were recorded. The mass spectra of L1−Al 3+ species displayed a peak at m/z 673.27 which corresponded to [L1 + Al 3+ + 2NO 3 -+ OCH 3 -+ Na + ] + . On the other hand, L1−Ga 3+ species showed a peak at m/z 669.30 corresponding to [L1 + Ga 3+ + 3OCH 3 − + K + ] + (Figures S22 and S23). The sources of the NO 3 − and OCH 3 − ions were from an aluminum precursor, Al(NO 3 ) 3 , and a CH 3 OH solvent, respectively. It is important to note that, for both species, the isotopic distribution patterns nicely matched that of the simulated patterns. The mass spectra further asserted a 1:1 metal binding stoichiometry to L1 [58]. The said binding stoichiometry was further confirmed by Job's plot for both Al 3+ and Ga 3+ ions ( Figure S24) [59].

DFT Studies
All chemical structures were optimized by the DFT using the suitable basis sets and functional (see Table S4 for the Cartesian coordinates). The molecular electrostatic potential surface (MESP) maps are often employed for the qualitative investigation of the charge distribution in a system. Hence, the optimized structures of chemosensors L1 and L2 were used to study the electropositive and electronegative centers. As shown in Figure 10, the electrostatic potential was scaled between −47.0 and +32.0 kcal/mol for both L1 and L2 with their approximate values marked. Notably, both oxygen and nitrogen centers in L1 and L2 were relatively more electronegative as depicted from the red-colored region around them. The MESP maps therefore suggest that the metal ions can bind with these groups: quoniline-N, imine-N, and phenolic-OR (-CH 2 -). The experimental results show that L1 exhibited FRET with both Al 3+ and Ga 3+ ions; however, FRET was not observed for L2 with the Ga 3+ ion. In order to obtain insights about the differences in their binding modes, the structures of chemosensor-metal complexes were optimized (Figure 11). The DFT optimized structures of L1-Al 3+ , L1-Ga 3+ , and L2-Ga 3+ were in line with the experimental results. Notably, in the case of L1, both the Al 3+ and Ga 3+ ions were situated significantly above (approx. 2.7-2.8 Å) the plane of the chemosensor to facilitate the simultaneous coordination of all binding sites. The optimized structure of L2-Ga 3+ confirmed the involvement of the phenolic-OCH3 group (ESP: −21.96 kcal/mol) in binding in addition to the phenolic-OCH2-group. In contrast, quinoline-N was situated farthest at 6.19 Å from the Ga 3+ ion and thus remained uncoordinated. To better understand the electron density shifts, contour plots of the frontier molecular orbitals (FMOs) from HOMO-4 to LUMO+4 were visualized ( Figure S25; see Figure S26 for a magnified view of the HOMO-1 to LUMO+1 orbitals). The electron density was found to be localized on the anthracene ring in HOMO but shifted to the quinoline ring in LUMO. In addition, the HOMO-LUMO band gap energy for L1 (3.42 eV) and L2 (3.64 eV) decreased to 2.42, 2.85, and 3.44 eV corresponding to L1-Al 3+ , L1-Ga 3+ , and L2-Ga 3+ , respectively (see Table S5 for energy values (in eV) for all FMOs). Thus, a decrease in the energy gaps upon metal complexation further supports the chemosensing behavior of these chemosensors.

Detection of Aspartic Acid
The recognition of amino acids is challenging as they contain both carboxylic acid and amino groups [24,76]. Therefore, designing a chemosensor that can selectively detect The experimental results show that L1 exhibited FRET with both Al 3+ and Ga 3+ ions; however, FRET was not observed for L2 with the Ga 3+ ion. In order to obtain insights about the differences in their binding modes, the structures of chemosensor-metal complexes were optimized ( Figure 11). The DFT optimized structures of L1-Al 3+ , L1-Ga 3+ , and L2-Ga 3+ were in line with the experimental results. Notably, in the case of L1, both the Al 3+ and Ga 3+ ions were situated significantly above (approx. 2.7-2.8 Å) the plane of the chemosensor to facilitate the simultaneous coordination of all binding sites. The optimized structure of L2-Ga 3+ confirmed the involvement of the phenolic-OCH 3 group (ESP: −21.96 kcal/mol) in binding in addition to the phenolic-OCH 2 -group. In contrast, quinoline-N was situated farthest at 6.19 Å from the Ga 3+ ion and thus remained uncoordinated. To better understand the electron density shifts, contour plots of the frontier molecular orbitals (FMOs) from HOMO-4 to LUMO+4 were visualized ( Figure S25; see Figure S26 for a magnified view of the HOMO-1 to LUMO+1 orbitals). The electron density was found to be localized on the anthracene ring in HOMO but shifted to the quinoline ring in LUMO. In addition, the HOMO-LUMO band gap energy for L1 (3.42 eV) and L2 (3.64 eV) decreased to 2.42, 2.85, and 3.44 eV corresponding to L1-Al 3+ , L1-Ga 3+ , and L2-Ga 3+ , respectively (see Table S5 for energy values (in eV) for all FMOs). Thus, a decrease in the energy gaps upon metal complexation further supports the chemosensing behavior of these chemosensors. The experimental results show that L1 exhibited FRET with both Al 3+ and Ga 3+ ions; however, FRET was not observed for L2 with the Ga 3+ ion. In order to obtain insights about the differences in their binding modes, the structures of chemosensor-metal complexes were optimized ( Figure 11). The DFT optimized structures of L1-Al 3+ , L1-Ga 3+ , and L2-Ga 3+ were in line with the experimental results. Notably, in the case of L1, both the Al 3+ and Ga 3+ ions were situated significantly above (approx. 2.7-2.8 Å) the plane of the chemosensor to facilitate the simultaneous coordination of all binding sites. The optimized structure of L2-Ga 3+ confirmed the involvement of the phenolic-OCH3 group (ESP: −21.96 kcal/mol) in binding in addition to the phenolic-OCH2-group. In contrast, quinoline-N was situated farthest at 6.19 Å from the Ga 3+ ion and thus remained uncoordinated. To better understand the electron density shifts, contour plots of the frontier molecular orbitals (FMOs) from HOMO-4 to LUMO+4 were visualized ( Figure S25; see Figure S26 for a magnified view of the HOMO-1 to LUMO+1 orbitals). The electron density was found to be localized on the anthracene ring in HOMO but shifted to the quinoline ring in LUMO. In addition, the HOMO-LUMO band gap energy for L1 (3.42 eV) and L2 (3.64 eV) decreased to 2.42, 2.85, and 3.44 eV corresponding to L1-Al 3+ , L1-Ga 3+ , and L2-Ga 3+ , respectively (see Table S5 for energy values (in eV) for all FMOs). Thus, a decrease in the energy gaps upon metal complexation further supports the chemosensing behavior of these chemosensors.

Detection of Aspartic Acid
The recognition of amino acids is challenging as they contain both carboxylic acid and amino groups [24,76]. Therefore, designing a chemosensor that can selectively detect an amino acid is always difficult [77]. Chemosensors L1 and L2 containing electron-rich groups and various binding sites make them ideal for the detection of amino acids [27,29].

Detection of Aspartic Acid
The recognition of amino acids is challenging as they contain both carboxylic acid and amino groups [24,76]. Therefore, designing a chemosensor that can selectively detect an amino acid is always difficult [77]. Chemosensors L1 and L2 containing electron-rich groups and various binding sites make them ideal for the detection of amino acids [27,29]. Hence, the detection ability of L1 and L2 was checked towards all 20 amino acids: Gly, Ala, Glu, Pro, Cys, Ile, Tyr, Arg, Gln, Lys, Thr, Asp, Asn, His, Leu, Met, Phe, Ser, Trp, and Val. Notably, for L1, the emission intensity increased only in the presence of Asp at 410 nm. In contrast, L2 did not display any change in its emission spectra with any of the amino acids (Figures 12a and S27). It is thus clear that chemosensor L1 is able to selectively detect Asp. Subsequently, an emission spectral titration of L1 was performed after the incremental addition of Asp from 0-200 µM (Figure 12b). From the concentration variation plot, the binding constant and limit of detection were found to be 2.89 × 10 3 M −1 and 0.80 µM, respectively (Figure 12c,d) [78]. Val. Notably, for L1, the emission intensity increased only in the presence of Asp at 410 nm. In contrast, L2 did not display any change in its emission spectra with any of the amino acids (Figures 12a and S27). It is thus clear that chemosensor L1 is able to selectively detect Asp. Subsequently, an emission spectral titration of L1 was performed after the incremental addition of Asp from 0-200 μM (Figure 12b). From the concentration variation plot, the binding constant and limit of detection were found to be 2.89 × 10 3 M -1 and 0.80 μM, respectively (Figures 12c,d) [78]. The selectivity of L1 towards Asp was evaluated by the competitive binding studies in the presence of an equimolar amount of all 20 amino acids [28]. The emission intensity of L1Asp at 410 nm remained unaffected in the presence of other amino acids ( Figure  13). The excited state behavior of L1 was studied in the presence of Asp with the lifetime measurement. With Asp, L1 displayed a biexponential decay with an average lifetime (τav) of 5.09 ns with a nearly 1.5-fold enhancement ( Figure S28 and Table S2). The quantum yield of L1Asp was found to be 0.027 with an approx. three-fold enhancement. Therefore, enhancement both in the lifetime measurement and quantum yield in the presence of Asp supports the interaction of L1 with Asp [57]. The selectivity of L1 towards Asp was evaluated by the competitive binding studies in the presence of an equimolar amount of all 20 amino acids [28]. The emission intensity of L1−Asp at 410 nm remained unaffected in the presence of other amino acids ( Figure 13). The excited state behavior of L1 was studied in the presence of Asp with the lifetime measurement. With Asp, L1 displayed a biexponential decay with an average lifetime (τ av ) of 5.09 ns with a nearly 1.5-fold enhancement ( Figure S28 and Table S2). The quantum yield of L1−Asp was found to be 0.027 with an approx. three-fold enhancement. Therefore, enhancement both in the lifetime measurement and quantum yield in the presence of Asp supports the interaction of L1 with Asp [57].  Figure 13. Selectivity of chemosensor L1 towards Asp in the presence of other amino acid amino acids (yellow cones) and L1 + amino acids + Asp (purple cones). All studies were con in EtOH.
To identify the binding sites, an 1 H NMR spectrum of L1 was recorded in the ence of 1 eq. of Asp. The imine-N and phenolic-OR (R = -CH2-and -CH3) protons disp a downfield shift ( Figure S29). Notably, a small downfield shift in the quinoline rin tons was also noted, suggesting that the quinoline-N was interacting with Asp. Su interaction aligns with both L1 and Asp to maximize their interaction. However, th matic ring protons, i.e., anthracene and arene, remained unaffected. These results su that imine-N, both phenolic-OR groups, and quinoline-N are the potential interactin of L1 towards a molecule of Asp [29]. We propose that due to such interactions, PET was suppressed, resulting in an enhanced emission. Importantly, Asp was not recog by L2 because of the fact that the quinoline-N group was farthest located, which d allow it to interact with Asp to achieve the correct conformation and hence its sensin not observed.

Low-Cost Detection Methods
The 'turn-on' detection of Al 3+ and Ga 3+ ions by both chemosensors prompted attempt different low-cost detection methods. As the best sensing results were obs for L1, low-cost detection methods were explored using the chemosensor L1 (Figu The colorimetric detection was attempted by introducing different metals (c, 2.5 mM amino acids (c, 2.5 mM) to an EtOH solution of L1. Notably, L1 displayed detectab hanced emission under UV light (λex = 365 nm) with both Al 3+ and Ga 3+ ions and Asp compared to other metals and amino acids [79]. Next, polystyrene films were pre containing the chemosensor L1 [4]. Such peelable polystyrene films displayed enh emission under UV light for the detection of both Al 3+ and Ga 3+ ions as well as Asp their aqueous solutions. Similarly, filter paper test strips containing L1 were able to both Al 3+ and Ga 3+ ions (c, 2.5 mM) and Asp (c, 2.5 mM) from the aqueous soluti different metal ions and amino acids [56]. Importantly, such filter paper test strips, with different concentrations of Al 3+ ions (0, 5, 20, and 50 μM), were able to detect co trations as low as 5 μM by showing color change from blue to cyan under the UV ( Figure S30). Hence, low-cost detection methods can be utilized to detect both A Ga 3+ ions as well as Asp for practical on-site detections. To identify the binding sites, an 1 H NMR spectrum of L1 was recorded in the presence of 1 eq. of Asp. The imine-N and phenolic-OR (R = -CH 2 -and -CH 3 ) protons displayed a downfield shift ( Figure S29). Notably, a small downfield shift in the quinoline ring protons was also noted, suggesting that the quinoline-N was interacting with Asp. Such an interaction aligns with both L1 and Asp to maximize their interaction. However, the aromatic ring protons, i.e., anthracene and arene, remained unaffected. These results suggest that imine-N, both phenolic-OR groups, and quinoline-N are the potential interacting sites of L1 towards a molecule of Asp [29]. We propose that due to such interactions, PET in L1 was suppressed, resulting in an enhanced emission. Importantly, Asp was not recognized by L2 because of the fact that the quinoline-N group was farthest located, which did not allow it to interact with Asp to achieve the correct conformation and hence its sensing was not observed.

Low-Cost Detection Methods
The 'turn-on' detection of Al 3+ and Ga 3+ ions by both chemosensors prompted us to attempt different low-cost detection methods. As the best sensing results were observed for L1, low-cost detection methods were explored using the chemosensor L1 ( Figure 14). The colorimetric detection was attempted by introducing different metals (c, 2.5 mM) and amino acids (c, 2.5 mM) to an EtOH solution of L1. Notably, L1 displayed detectable enhanced emission under UV light (λ ex = 365 nm) with both Al 3+ and Ga 3+ ions and Asp when compared to other metals and amino acids [79]. Next, polystyrene films were prepared containing the chemosensor L1 [4]. Such peelable polystyrene films displayed enhanced emission under UV light for the detection of both Al 3+ and Ga 3+ ions as well as Asp from their aqueous solutions. Similarly, filter paper test strips containing L1 were able to detect both Al 3+ and Ga 3+ ions (c, 2.5 mM) and Asp (c, 2.5 mM) from the aqueous solutions of different metal ions and amino acids [56]. Importantly, such filter paper test strips, tested with different concentrations of Al 3+ ions (0, 5, 20, and 50 µM), were able to detect concentrations as low as 5 µM by showing color change from blue to cyan under the UV lamp ( Figure S30). Hence, low-cost detection methods can be utilized to detect both Al 3+ and Ga 3+ ions as well as Asp for practical on-site detections.

Conclusions
This work illustrates two Schiff-base-based chemosensors, L1 and L2, decorated with electron-rich quinoline and anthracene rings. Chemosensor L1 displayed AIEE in a MeOH-H2O solvent system due to the suppression of PET. DLS measurements and fluorescence lifetime studies confirmed the aggregation of L1 in the presence of water. Chemosensor L1 was utilized for the sensitive, selective, and reversible detection of Al 3+ and Ga 3+ ions in the presence of other metal ions. L1 displayed 'turn-on' emission in the presence of both Al 3+ and Ga 3+ ions with high binding constants and low detection limits. Chemosensor L2, a structural isomer of L1, was able to discriminate between the Al 3+ and Ga 3+ ions and was exclusively selective for the Ga 3+ ion with an impressive detection limit and a high binding constant. The discriminative sensing ability of L2 was due to the presence of different binding sites which was substantiated by the 1 H NMR spectra, mass spectra, and DFT studies. The chemosensor L1 was further utilized for the selective and sensitive detection of Asp amongst all 20 amino acids. Chemosensor L1 exhibited a 'turn-on' fluorescence response in the presence of Asp with a remarkable detection limit and binding constant. The 'turn-on' nature of the fluorescence sensing by these chemosensors allowed for the fabrication of colorimetric detection, filter-paper-based test strips, and polystyrene-film-based detection strategies.

Conclusions
This work illustrates two Schiff-base-based chemosensors, L1 and L2, decorated with electron-rich quinoline and anthracene rings. Chemosensor L1 displayed AIEE in a MeOH-H 2 O solvent system due to the suppression of PET. DLS measurements and fluorescence lifetime studies confirmed the aggregation of L1 in the presence of water. Chemosensor L1 was utilized for the sensitive, selective, and reversible detection of Al 3+ and Ga 3+ ions in the presence of other metal ions. L1 displayed 'turn-on' emission in the presence of both Al 3+ and Ga 3+ ions with high binding constants and low detection limits. Chemosensor L2, a structural isomer of L1, was able to discriminate between the Al 3+ and Ga 3+ ions and was exclusively selective for the Ga 3+ ion with an impressive detection limit and a high binding constant. The discriminative sensing ability of L2 was due to the presence of different binding sites which was substantiated by the 1 H NMR spectra, mass spectra, and DFT studies. The chemosensor L1 was further utilized for the selective and sensitive detection of Asp amongst all 20 amino acids. Chemosensor L1 exhibited a 'turn-on' fluorescence response in the presence of Asp with a remarkable detection limit and binding constant. The 'turn-on' nature of the fluorescence sensing by these chemosensors allowed for the fabrication of colorimetric detection, filter-paper-based test strips, and polystyrene-filmbased detection strategies.