Exploring the Chelating Potential of an Easily Synthesized Schiff Base for Copper Sensing

Abstract

The present study deals with the investigation of Cu²⁺, Ni²⁺ and Pd²⁺ chelating potential of the Schiff base, (E)-N-(2-((2-hydroxybenzylidene)amino)benzyl)-4-methylbenzenesulfonamide (H₂SB). Crystal structures of Ni(HSB)₂, Pd(HSB)₂ and Cu(HSB)₂ have been elucidated from single crystal X-ray diffraction data. NMR spectroscopy showed the presence of two conformers of Pd(HSB)₂ in solution, both with an E configuration of the ligand. The determination of binding constants by fluorescence quenching showed that affinity of H₂SB to Cu²⁺ in solution is higher than for Ni²⁺ and Pd²⁺. Since there is a high demand for selective, sensitive, rapid and simple methods to detect copper in aqueous samples (both as Cu²⁺ ions and as CuO NPs), we have explored H₂SB as an optical chemosensor. H₂SB interacts with increasing concentrations of Cu²⁺ ions, giving rise to a linear increase in the absorbance of a band centered at about 392 nm. H₂SB displays a high selectivity toward Cu²⁺, even in the presence of the most common metal ions in water (Ca²⁺, Mg²⁺, Na⁺, K⁺, Al³⁺ and Fe³⁺), and some heavy transition metal ions such as the soft acids Pd²⁺ and Cd²⁺. H₂SB also interacts with increasing concentrations of CuO NPs, which gives rise to a linear decrease in its fluorescence intensity (λ_em = 500 nm, λ_ex = 390 nm). Quenching has occurred as a result of the formation of a non-fluorescent ground-state surface complex H₂SB–CuO NPs. The limits of detection and quantification of CuO NPs were 9.8 mg/L and 32.6 mg/L, respectively. The presence of TiO₂, Ag and Au NPs does not interfere with the determination of CuO NPs.

1. Introduction

A number of methods for selective and highly sensitive detection of Cu²⁺ ions have been developed including, among others, inductively-coupled plasma mass spectrometry [1], electrochemical methods [2] and fluorescence spectroscopy [3,4,5,6]. However, these techniques frequently involve time-consuming sample pre-treatment methods and a need for sophisticated instrumentation and highly trained operators, precluding their routine application. This has stimulated the development of a variety of chemosensors based on absorption changes for the rapid and easy detection of Cu²⁺ ions [7,8,9,10,11,12]. Most of these reported colorimetric chemosensors have one or more of the following drawbacks: poor detection limit, long response time, tedious synthetic procedures, use of organic solvent or interference from other transition metal ions. Thus, a need exists for the exploration of new, simple and easy-to-make chemosensors based on absorption changes for detection of Cu²⁺ in aqueous solution.

Human and environmental health risks of CuO NPs are demanding affordable and reliable techniques for their detection [13,14,15]. This would increase safety related to the handling and release into the environment of NPs. Due to their selectivity, sensitivity and simplicity, chemical sensors such as fluorescent probes are very promising methods to be used not only for detection, but for quantification as well. Three fluorescent sensors have been developed for detection of Ag NPs [16,17,18], but investigation of optical sensors to detect and quantify CuO NPs remains virtually unexplored. Recently, we have reported a fluorescent probe for detecting Cu²⁺ ions in aqueous samples, as well as some preliminary studies for detecting CuO NPs [19].

We have chosen for our investigation the Schiff base (E)-N-(2-((2-hydroxybenzylidene)amino)benzyl)-4-methylbenzenesulfonamide, which will be abbreviated as H₂SB (Figure 1). This ligand can be easily synthesized by reaction of the previously prepared N-(2-aminobenzyl)-4-methylbenzenesulfonamide [20] with 2-hydroxybenzaldehyde, as we have previously reported [21]. We have found that H₂SB can simultaneously bind two divalent ions through µ₂-N_sulfonamide bridges, allowing complexes of the type M₂(SB)₂ to be obtained (where the dianionic SB^2- is acting as a tridentate ligand, and M is Pd²⁺ or Cu²⁺ [21]. Now, the ligand can also behave as a monoanionic bidentate O,N-donor chelator, which also seems adequate to interact with the CuO surface due to its structural similarity with salicylate-type ligands. As the metal ion of a mineral surface acts as a Lewis acid and exchanges its coordinated hydroxyl groups with other ligands (ligand exchange), studying formation reactions of solution complexes will aid understanding of the interaction of anionic ligands with metal oxide surfaces. Keeping in mind that H₂SB is a Lewis base with N and O donor atoms, this ligand may be suitable for binding to either hard, borderline or even soft acids, depending on circumstances. Hence, we have also studied its coordination behavior toward another borderline acid such as Ni²⁺, and a softer acid as Pd²⁺. Therefore, we have investigated the formation of the solution complexes Cu(HSB)₂, Ni(HSB)₂ and Pd(HSB)₂ using a combination of UV-Vis, FT-IR, NMR and fluorescence spectrometry as well as elemental analysis and X-ray diffraction. Then, we have investigated changes in the UV-Vis absorbance and fluorescence spectra of H₂SB upon titration with Cu²⁺ and CuO NPs, respectively, also in comparison with other common metal species in water.

2. Experimental 2.1. Materials and Methods

The reagents and starting materials were commercially available, and used without further purification. The synthesis of H₂SB (Figure 1) has been previously reported [20,21]. Infrared spectra were recorded as KBr pellets on a Jasco FT/IR-410 spectrophotometer in the range 4000–600 cm⁻¹. Elemental analyses were performed on a Carlo Erba EA 1108 analyzer. The UV-Vis spectra were performed on a Uvikon 810 spectrophotometer (Kontron Instruments) using a methanol-water solution (in 80:20 v/v) as solvent. ¹H NMR spectra (400 MHz) were measured in dmso-d₆. NMR assignments were carried out by a combination of COSY and NOESY experiments. In order to simplify, the NMR numbering scheme is equivalent to that shown for the molecular structures of Ni(HSB)₂, Pd(HSB)₂ and Cu(HSB)₂.

2.2. Crystal Structure Analysis Data

Diffraction data for Ni(HSB)₂, Pd(HSB)₂ Cu(HSB)₂ were collected at 100(2) K, using graphite-monochromatized Mo-Kα radiation (λ = 0.71073 Å). Some significant refinement data and crystal parameters are summarized in Table S1. Data were corrected for polarization and Lorentz effects, while multi-scan absorption corrections were performed with SADABS [22]. The structures were solved by standard direct methods [23], and then refined by full matrix least squares on F² [24]. All non-hydrogen atoms were anisotropically treated. Hydrogen atoms were included in the structure factor calculation, by using a riding model, with thermal parameters depending on the parent atom in geometrically idealized positions.

2.3. Synthesis of Pd(HSB)₂ A methanol solution (40 mL) of H₂SB (0.15 g, 0.39 mmol) and Pd(OAc)₂·4H₂O (0.05 g, 0.18 mmol) was stirred for 4 h at room temperature. The resulting orange precipitate was filtered off, washed with methanol and then dried under vacuum. Yield = 0.15 g (86%). Prismatic orange crystals of Pd(HSB)₂ suitable for single-crystal X-ray studies were obtained by recrystallization in acetone. 2.4. Synthesis of Ni(HSB)₂ A methanol solution (40 mL) of H₂SB (0.10 g, 0.26 mmol) and Ni(OAc)₂·4H₂O (0.04 g, 0.13 mmol) was stirred for 4 h at room temperature. The resulting green precipitate was filtered off, washed with cooled methanol and then dried under vacuum. Yield = 0.07 g (70%). Rhombic green crystals of Ni(HSB)₂ suitable for single-crystal X-ray studies were obtained by recrystallization in methanol. 2.5. Synthesis of Cu(HSB)₂ A methanol solution (40 mL) of H₂SB (0.10 g, 0.26 mmol) and Cu(OAc)₂·H₂O (0.03 g, 0.13 mmol) was stirred for 4 h at room temperature. The resulting green precipitate was filtered off, washed with cooled methanol and then dried under vacuum. Yield = 0.08 g (75%). Rhombic green crystals of Cu(HSB)₂ obtained by recrystallization in methanol were suitable for single-crystal X-ray studies. 3. Results and Discussion

In contrast with the previously reported dianionic tridentate O,N,N-donor behavior of the ligand [21], now we have achieved that this ligand can also behave as a monoanionic bidentate O,N-donor chelating agent. This is due to the use of softer reaction conditions, i.e., room temperature instead of reflux temperature, and with a 1:2 metal–ligand ratio, instead of the formerly used 1:1 ratio.

3.1. Crystal Structures of Pd(HSB)₂, Ni(HSB)₂ and Cu(HSB)₂

Single crystal X-ray diffraction techniques have shown that the asymmetric unit only contains half a complex, with the metal ion (i.e., Pd²⁺, Ni²⁺ or Cu²⁺) sited on an inversion center, so that the other half is generated by symmetry. The coordination environment of the metal ion can be qualified as a slightly distorted square, formed by the O,N-chelating binding domains of both ligand units, with bite angles of ca. 90.5°, while the whole chromophore is absolutely planar, including the central metal ion. The loss of conjugation of the phenyl ring corresponding to the diamine residue (C8–C13), in relation to the salicylaldimine aromatic system (C14–C20) should be mentioned, since their respective planes form a wide angle of ca. 75.7°. The main angles and bond distances are collected in Tables S2–S4.

The molecular structure of Cu(HSB)₂, which is represented in Figure 2 (top), shows a trans disposition of the N and O donor atoms related to both salicylaldehyde residues. This appears to be favored by both intramolecular N–H···O interactions between sulfonamide and phenoxo groups (about 2.9 Å), as well as by the significant steric hindrance that the diamine residue and the uncoordinated tosyl groups can exert. Tosyl groups show an anti-conformation, as they are positioned at opposite sides of the plane formed by the CuN₂O₂ chromophore. With this spatial arrangement their tosyl rings (C1–C6) are stacked with those of their corresponding salicylaldimine residues (C15–C20), with a distance between their respective centroids of ca. 4.15 Å. Neighboring neutral complex molecules are not interacting via classic H bonds, but the packing scheme is mostly based on C–H···O interactions between aromatic H atoms and one of O atoms of the tosyl groups, as well as on π–π stacking interactions between the phenyl rings of the diamine residues.

The great coincidence between the molecular structures of Cu(HSB)₂, Pd(HSB)₂ and Ni(HSB)₂ seems to indicate that the spatial arrangement observed for the complex in the solid state must be highly favored (Figure 2, bottom). The molecular structures of Pd(HSB)₂ and Ni(HSB)₂ are shown in supplementary material (Figures S1 and S2), while their geometric parameters are also collected in the supplementary information (Tables S2 and S3).

3.2. Spectroscopic Characterisation of Pd(HSB)₂, Ni(HSB)₂ and Cu(HSB)₂ Elemental analysis data and spectroscopic data, obtained from FT-IR, UV-Vis and ¹H NMR spectrometry, were as follows. Pd(HSB)₂: ¹H NMR (500 MHz, dmso-d₆, δ in ppm): 7.89 (s, 2H, H14), 7.88 (s, 2H, H14′), 7.79 (t, 2H, HN′), 7.69 (t, 2H, HN), 7.51 (d, 4H, H2 + H6), 7.43 (d, 4H, H2′ + H6′), 7.39 (d, 2H, H9), 7.34 (t, 2H, H11), 7.30 (d, 2H, H16), 7.15 (t, 2H, H18), 7.05 (d, 4H, H3 + H5), 6.92 (d, 4H, H3′ + H5′), 6.52 (t, 2H, H17 and H17′), 5.82(d, 2H, H19 and H19′), 4.23 (d, 1H, H7_eq), 3.95 (d, 1H, H7_ax), 4.21 (d, 2H, H7′_eq), 3.86 (d, 2H, H7′_ax), 2.18 (s, 6H, H40 and H40′). UV-Vis (λ in nm): 210, 226, 270, 336. IR (KBr, ν in cm⁻¹): ν(NH) 3272, ν(C=N_imine) 1609, ν_as(SO₂) 1320, ν_s(SO₂) 1158. Elemental analysis (found): C 58.3; H 4.3; N 6.3; S 7.2%; calc. for C₄₂H₃₈N₄O₆PdS₂: C 58.3; H 4.4; N 6.5; S 7.4%. Ni(HSB)₂: UV-Vis (λ in nm): 204, 230, 268, 392. IR (KBr, ν in cm⁻¹): ν(NH) 3270, ν(C=N_imine) 1608, ν_as(SO₂) 1318, ν_s(SO₂) 1160. Elemental analysis (found): C 61.8; H 4.7; N 6.8; S 7.8%; calc. for C₄₂H₃₈N₄NiO₆S₂: C, 61.7; H, 4.7; N, 6.9; S 7.8%. Cu(HSB)₂: UV-Vis (λ in nm): 206, 230, 288, 392. IR (KBr, ν in cm⁻¹): ν(NH) 3271, ν(C=N_imine) 1585, ν_as(SO₂) 1327, ν_s(SO₂) 1156. Elemental analysis (found): C 61.3; H 4.7; N 6.7; S 7.7%; calc. for C₄₂H₃₈CuN₄O₆S₂: C 61.3; H 4.7; N 6.8; S 7.8%.

3.2.1. NMR Study of Pd(HSB)₂

The molecular structure of Pd(HSB)₂ in solution has been investigated by 1D (¹H experiment) and 2D (COSY and NOESY experiments) NMR spectroscopy. The diamagnetic nature of Pd(HSB)₂ indicates a square planar environment around the Pd²⁺ ion. The 2D COSY spectrum (Figure S3) allowed us an assignment of the signals with very few shadows, crucial for this study.

The ¹H NMR spectrum shows a shift of about 0.8 ppm to the high field of the signal corresponding to the –CH=N group, which was observed at 8.7 ppm in the free ligand (Figure 3), indicating that the imino group is coordinated to the palladium(II) ion through the lone pair of its nitrogen atom. The absence of the OH signal, as well as the presence of the NH signal, suggests that the ligand is coordinated as a monoanionic species. The clear observation of two sets of signals for both sulfonamide (NH) and methylene protons (H-7) is a clear sign of the presence of two conformational isomers. Each one of these isomers could be stabilized by intramolecular N–H···O and N–H···N interactions, preventing its interconversion by rotations around C–N single bonds.

The 2D NOESY spectrum of Pd(HSB)₂ shows cross peaks due to the coupling of the imine proton (H-14) with aromatic protons H-12 and H-16 (Figure 4), which is indicative of an E configuration in solution. The coupling of the aromatic proton H-9 with methylene protons (H-7) evidences the diastereotopic nature of the latter ones (with signals at about 3.9 ppm and 4.2 ppm).

3.2.2. UV-Vis Absorption Study of Pd(HSB)₂, Ni(HSB)₂ and Cu(HSB)₂

The most remarkable spectral change observed is that complexation of H₂SB with Cu²⁺ and Ni²⁺ (but not with Pd²⁺) gives rise to a new absorption band at about 392 nm, which was assigned to a metal-to-ligand charge transfer (MLTC). In order to explore the ability of H₂SB to perform as a colorimetric chemosensor for detection of Cu²⁺ ions, we have paid special attention to changes on the cited MLTC absorption band.

The UV-Vis spectrum of Cu(HSB)₂ clearly shows that the n→π* transition attributable to the imino group [25] underwent a red (bathochromic) shift from 270 to 285 nm, as a result of coordination (Figure 5). This is due to a remarkable increase in the electron density at the imine nitrogen atom, as a consequence of the Cu²⁺ complexation. By contrast, no change on the wavelength of the n→π* transitions attributable to the imino group were detected in the spectra of Pd(HSB)₂ and Ni(HSB)₂. As this could be related to the strength of the M–N bond (M = Pd²⁺, Ni²⁺ or Cu²⁺), we have measured the binding constants of Pd(HSB)₂, Ni(HSB)₂ and Cu(HSB)₂. Benesi–Hildebrand equation [26] was used for determining the binding constant based on fluorescence spectra (Figure S4). The values of the binding constant (K_b) of H₂SB with Pd²⁺, Ni²⁺ and Cu²⁺ in 2:1 molar ratio, were found to be about 1.92 10³ M⁻¹, 3.54 10³ M⁻¹ and 4.73 10³ M⁻¹, respectively. Thus, the binding affinity of H₂SB to Cu²⁺ in solution is higher than that found for Ni²⁺ and Pd²⁺.

3.3. Absorption Studies on the H₂SB-Cu²⁺ Interaction

With the aim of studying the enhancement of the absorbance intensity at 392 nm with increasing Cu²⁺ ion concentration, spectral data were recorded after addition of an increasing volume of Cu(OAc)₂·H₂O at concentration 100 μM (0.0 mL, 0.1 mL, 0.2 mL, 0.3 mL, 0.4 mL, 0.5 mL, 0.6 mL, 0.7 mL, 0.8 mL, 0.9 mL and 1.0 mL) to H₂SB at concentration 100 μM (1.0 mL). Results showed that the absorbance of the MLTC band linearly varied with increasing concentrations of Cu²⁺ in the range 0–2.1 mg/L (33.33 µM), tripling its initial value (Figure 6).

The selectivity of H₂SB for Cu²⁺ ions was examined by testing the response of the H₂SB to some other metal ions, including some common ions in water, such as Na⁺, K⁺, Ca²⁺, Mg²⁺, Al³⁺ and Fe³⁺, and some heavy metal ions, such as some borderline acids (Ni²⁺, Co²⁺ and Zn²⁺), as well as some other soft acids (Pd²⁺ and Cd²⁺). By comparison, no increase of the absorbance at 392 nm similar to that displayed in the H₂SB-Cu²⁺ system was observed upon the addition of Na⁺, K⁺, Ca²⁺, Mg²⁺, Al³⁺, Fe³⁺, Pd²⁺ and Cd²⁺ ions), suggesting that H₂SB could potentially be used to detect Cu²⁺ ions in a sample matrix containing both hard and soft metal ions. The addition of other borderline acids such as Ni²⁺, Co²⁺ and Zn²⁺ ions to a solution of H₂SB in 1:1 molar ratio results in an increase of the absorbance at 392 nm (23%, 39% and 85%, respectively. Therefore, these borderline acids could interfere in the determination of Cu²⁺ ions, which led us to abandon the exploration of the ability of H₂SB to function as an absorption chemosensor for detection of Cu²⁺ ions. 3.4. Fluorescence Studies on the Interaction of H₂SB with CuO NPs

Good results in fluorescence studies on the interaction H₂SB-Cu²⁺ [21] encouraged us to extend our investigations to the interaction of H₂SB with CuO NPs. We have speculated that Cu²⁺ ions in the oxide lattice can form inner-sphere surface complexes of HSB⁻ by ligand exchange in a way similar to that occurring in solution. It is known that, since O²⁻ and Cu²⁺ ions at CuO NPs’ surface are incompletely coordinated, they have partial charges. Consequently, CuO NPs immersed in water attract and bind water molecules on their surfaces, and the subsequent dissociation of these surface water molecules leaves hydroxyl groups bound to the surface Cu²⁺ ions, releasing of hydron cations. Similarly, incompletely coordinated O²⁻ can react with water to leave surface hydroxyl groups, releasing hydroxyl anions. Therefore, the surface of nanoparticles quickly becomes covered with hydroxyl groups, and hence, surface hydroxyl groups can act as proton acceptors, leading to more exchangeable ligands. Monodeprotonated HSB⁻ may be absorbed by replacement of a surface OH group (ligand exchange) giving inner-sphere complexes and releasing water (Figure 7). Among the six typical interaction mechanisms between NPs and dissolved organic matter (hydrophobic interaction, electrostatic and van de Waals interactions, ligand exchange, chelation, cation bridging and H-bonding), ligand exchange was reported as the dominant mechanism accounting for sorption of dissolved organic matter on metal oxide NPs [27,28].

To gain a better understanding of the favorable conditions under which binding of H₂SB on CuO NPs surfaces could occur, the effect of pH on the surface charge of CuO NPs has been analyzed (Figure 8). We have found that the pH of zero point of charge (pH_zpc) of CuO NPs is 6.0, and therefore, a pH value in the range 7.0–7.5 could be adequate to form surface complexes H₂SB-CuO NPs. Since it is expected that adsorption of H₂SB on the negatively charged CuO NPs decreases with increasing pH, we have investigated variations in fluorescence intensity of H₂SB with concentration of CuO NPs at near-neutral pH values, so the addition of pH modifiers was not necessary. This presented an additional advantage, and it was that the negatively charged CuO NPs (zeta potential values between −15 mV and −25 mV) should resist aggregation through interparticle electrostatic repulsion.

Dependence of the fluorescence intensity of H₂SB in an 80:20 ethanol-water mixture at 100 µM concentration with addition of CuO NPs in suspension (100 μM) has been studied. Spectral data were recorded after the addition of CuO NPs (0.00 mL, 0.01 mL, 0.02 mL, 0.03 mL, 0.04 mL, 0.05 mL, 0.06 mL, 0.07 mL, 0.08 mL, 0.09 mL and 0.1 mL) to H₂SB (1.0 mL). The total volume of 3 mL has been achieved by adding the corresponding volume of an 80:20 ethanol-water mixture. No pH modifiers were added to attain a pH of about 7.0. The fluorescence intensity of H₂SB at about 500 nm linearly decreased with increasing concentrations of CuO NPs below 0.26 mg/L of CuO NPs, declining by about 55% at pH 7.0 (Figure 9). The limits of detection (LOD = 3SD/m) and quantification (LOQ = 10SD/m) of CuO NPs were 9.8 μgL⁻¹ and 32.6 μgL⁻¹, respectively. It must be noted that these values are lower than those previously reported by us for a pyrrole-based Schiff base ligand (13.83 μgL⁻¹ and 46.05 μgL⁻¹, respectively) [19].

The quenching mechanism upon titration with CuO NPs was studied with Stern-Volmer plots [29] (I₀/I = 1 + K_SV[quencher]) (Figure S5). According to the slope, the value of the quenching constant (K_SV) for H₂SB-coated CuO NPs is found to be 17.5 10³ M⁻¹ at 20 °C, 9.4 10³ M⁻¹ at 30 °C and 6.7 10³ M⁻¹ at 40 °C. A static quenching mechanism has been deduced from the decrease of quenching efficiency with increasing temperature. Quenching has occurred as a result of the formation of a non-fluorescent ground-state complex through electrostatic attraction, which supports the binding of H₂SB on CuO NPs surfaces.

Studying the effect on the fluorescence intensity of the time elapsed after addition of CuO NPs upon a solution of H₂SB, we have deduced that the ligand can interact with the surface of CuO NPs in about 2 minutes (Figure S6). The selectivity of H₂SB as a fluorescence receptor for CuO NPs was tested in the presence of some other widely used nanomaterials, such as TiO₂, Cu, Ag and Au (Figure S7). As a criterion for interference, a ±10% variation of the average fluorescence intensity was used. These results showed that TiO₂, Ag and Au NPs at the same molar concentration as CuO NPs do not interfere with its determination, although Cu NPs can interfere. This could be due to the rapid surface oxidation of Cu NPs [30], behaving then as CuO NPs.

4. Conclusions Crystal structures of Ni(HSB)₂, Pd(HSB)₂ and Cu(HSB)₂ have been elucidated by using single crystal X-ray diffraction techniques, showing that H₂SB is acting as a monoanionic bidentate O,N-donor chelating ligand. The determination of the corresponding binding constants by fluorescence quenching showed that affinity of H₂SB to Cu²⁺ is higher than for Ni²⁺ and Pd²⁺. The arrangement of the ligand in the three complexes is so similar that they are practically superimposable, indicating a very stable conformation in the solid state. By contrast, a conformational study on Pd(HSB)₂ using 2D NMR spectroscopy showed the presence of two conformers in solution, both with an E configuration of the ligand. H₂SB interacts with increasing concentrations of Cu²⁺ ions in absence of pH modifiers, at room temperature, and in a short time, which gives rise to a linear increase in the absorbance of a band centered at about 392 nm. H₂SB possesses selectivity toward Cu²⁺ in the presence of the most common metal ions in water (Na⁺, K⁺, Ca²⁺, Mg²⁺, Al³⁺ and Fe³⁺) and some heavy transition metal ions, such as the soft acids Pd²⁺ and Cd²⁺. Unfortunately, other borderline acids (such as Ni²⁺, Co²⁺ and Zn²⁺) could interfere in the determination of Cu²⁺ ions. The fluorescence intensity of H₂SB in ethanol:water solutions (80:20 v/v) shows a linear variation with the concentration of CuO NPs in the range 0–0.26 mg/L, decreasing by about 55% (λ_em = 500 nm, λ_ex = 390 nm). LOD and LOQ were 9.8 mg/L and 32.6 mg/L, respectively. TiO₂, Ag and Au NPs can be tolerated without interference at concentrations of 100 µM. In view of the effect of temperature, according to Stern–Volmer plots, quenching has occurred as a result of the formation of a non-fluorescent ground-state surface complex H₂SB-CuO NPs.

Figure 1. Schematic representation of the easy synthesis of (E)-N-(2-((2-hydroxybenzylidene)amino)benzyl)-4-methylbenzenesulfonamide (H2SB) with the metal binding site indicated by arrows.

Figure 2. Top: Ellipsoid view of the molecular structure of Cu(HSB)2 with intramolecular N-H···O interactions (only labels for the asymmetric unit, jointly with the donor atoms N2 and O3 generated by symmetry have been included). Bottom: Overlay of the molecular structures of Ni(HSB)2 (in standard colors), Pd(HSB)2 (in red color) and Cu(HSB)2 (in green color).

Figure 3. View of the 1H NMR spectra of Pd(HSB)2 (top) and H2BS (bottom).

Figure 4. View of the NOESY spectrum of Pd(HSB)2 (in dmso-d6), with schematic representation of the metal complex (inset).

Figure 5. Absorption spectra of H2SB, Pd(HSB)2, Ni(HSB)2 and Cu(HSB)2 using a methanol-water solution as solvent (in 80:20 v/v).

Figure 6. UV-Vis titration spectra of H2SB (100 µM) in methanol-water mixture (80:20 v/v) at room temperature and neutral pH, upon sequential addition of Cu2+ (0-1 equiv).

Figure 7. Schematic description of ligand exchange, which is the proposed sorption mechanism of H2SB (acting as bidentate chelating ligand) on the surfaces of CuO NPs (Cu2+ ions are in grey and O2- are in red).

Figure 8. Variation of the Z potential of CuO NPs with pH. The values of Z potential were given as mean ± SD of triplicate samples. The best fit trend line in red.

Figure 9. Variation of the fluorescence intensity of H2SB with concentration of CuO NPs. A fluorescent photographic image under UV lamp (365 nm) obtained for the blue-emitting H2SB has been included.

Supplementary Materials

Supplementary crystallographic data for this paper have been deposited at Cambridge Crystallographic Data Center (CCDC 1563225, 1563226 and 1906115) and can be obtained free of charge via www.ccdc.cam.ac.uk/conts/retrieving.html. The following information is available online at https://www.mdpi.com/2073-4352/10/3/235/s1, Tables S1-S4: Diffraction data for Ni(HSB)2, Pd(HSB)2 and Cu(HSB)2, Figures S1 and S2: Molecular structures of Pd(HSB)2 and Ni(HSB)2, Figure S3: 2 D COSY spectrum of Pd(HSB)2, Figure S4: Benesi-Hildebrand plot from fluorescence titration data of H2SB (100 µM) with Pd2+, Ni2+ and Cu2+, Figure S5: Fluorescence spectrum of H2SB and plot of the intensities of the fluorescence spectra vs the concentration of CuO NPs at 293, 303 and 313K, Figure S6: Plot of the intensity fluorescence vs time elapsed after the addition of CuO NPs to H2SB and Figure S7: Fluorescence responses of H2SB toward a suspension of CuO NPs in the presence of TiO2, Cu, Ag and Au NPs.

Author Contributions

Conceptualization, J.S.-M.; methodology, M.Z.-J. and M.A.-S.; software, A.G.-D., J.S.-M., and M.Z.-J.; validation, J.S.-M. and A.G.-D.; formal analysis, M.F.; investigation, M.Z.-J.; resources, J.S.-M. and P.B.-B.; data curation, M.F.; writing-original draft preparation, J.S.-M; writing-review and editing, J.S.-M. and A.G.-D.; visualization, M.F.; supervision, J.S.-M., P.B.-B. and M.A.-S.; project administration, P.B.-B.; funding acquisition, P.B.-B. All authors have read and agreed to the published version of the manuscript.

Funding

This research was funded by the Ministerio de Ciencia, Innovación y Universidades of Spain and Unión Europea (Fondo europeo de desarrollo regional) Ref. RTI2018-099222-B-I00; Dirección Xeral de I+D-Xunta de Galicia, Grupos de Referencia Competitiva (Ref. ED431C2018/19) and Strategic Grouping in Materials AEMAT (ED431 E2018/0).

Conflicts of Interest

The authors declare no conflict of interest.

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