1 Introduction

Schiff base (SB) group is a valuable subunit (R1R2C=NR3) present in a wide spectrum of compounds. These compounds are accessible from condensation of amines with aldehydes or ketones under conventional or microwave heating. Since the first reported procedure by Schiff [1] in 1864, tremendous efforts have been paid to synthesize a diversity of molecules with this functional feature. The structural variation of SB-containing compounds allowed their utilization in many applications including nonlinear optical materials, optic data storage, anticancer agents, anticorrosive materials, and coordination chemistry [2,3,4,5]. The chelation properties of SB ligands towards coordination to transition metals can be empowered by introducing electron-donating atom such as oxygen, nitrogen, sulfur, and phosphorus to SB scaffold, delivering very stable complexes.

The presence of salicyl moiety attached to SB derivatives could demonstrate exceptional photo- and thermochromism properties in different physical state. These attributes are typically generated from proton transfer from the o-hydroxyaryl moiety to the attached azomethine (imine) functional group [6,7,8]. Depending on the electronic conditions of substituents, the o-hydroxyaryl SB–containing compounds could exist in the keto form, enol form, keto/enol mixtures, or rarely in a zwitterionic form [9,10,11,12,13].

Numerous copper (II) complexes bearing SB functional groups have been synthesized, characterized, and served efficiently in several organic transformations, particularly in oxidation reactions [14,15,16]. Selective oxidation of alcohols to aldehydes and ketones over transition metal catalysts has been intensively pursued under a number of heterogeneous and homogeneous conditions, since carbonyl derivatives are considered significant intermediates employed in the production of dyes, flavors, fragrances, and medicines [17,18,19,20]. Many sustainable catalytic transformations have been accomplished in the presence of molecular oxygen and hydrogen peroxide as oxidants. However, peroxide is broadly used for possessing greater oxidation potential than oxygen [17,21,22].

Thus, there is a need to synthesize novel multi-dentate SB ligands and their metal complexes for more potent biological and catalytical applications. In this work, we report the synthesis and full characterization of (E)-4-nitro-2-(((2-(piperazin-1-yl)ethyl)imino)methyl)-phenol as a SB-functionalized compound from condensation of 2-hydroxy-5-nitrobenzaldehyde and 2-(1-piperazinyl)ethylamine. Since the synthesized SB symbolizes an appropriate tetradentate ligand via three N and one O atoms, we have performed the coordination experiment with three copper(II) salts through subsequent deprotonation/coordination process in the absence of base. The solvatochromic, halochromtic, thermochromic, florescence, and thermal behaviors were investigated. Moreover, selective catalytic oxidation of benzyl alcohol to benzyl aldehyde was evaluated using the desired complexes in the presence of hydrogen peroxide as a green oxidant.

2 Experimental

2.1 Materials and measurements

Fine chemicals were of reagent grade and solvents were of analytical grade; all were harnessed directly without any purification process. Copper(II) bromide, 2-hydroxy-5-nitrobenzaldehyde, and 2-(1-piperazinyl)ethylamine were received from Sigma-Aldrich. Copper(II) nitrate trihydrate and copper(II) chloride were procured from Acros Organics. FT-IR transmission spectra were recorded in solid state through Bruker ALPHA FT-IR spectrometer in the range of 400–4000 cm−1. NMR spectra were recorded on JOEL 600 MHz spectrometer with internal reference to the residual solvent signal, CHCl3: δ = 7.24 ppm for 1H-NMR and δ = 77.00 ppm for 13C-NMR. The UV-Vis measurements were accomplished in neat water using Agilent 8453 single-beam spectrophotometer. Relative fluorescence was measured using Shimadzu Spectrofluorophotometer RF-6000. Mass spectra were collected employing Shimadzu GC-MS QP2010. The CHN analysis was performed using Thermo Scientific™ FLASH™ 2000 Organic Elemental Analyzer. The magnetic behavior was demonstrated using Magnetic Susceptibility Balance MK1 from Sherwood Scientific Ltd. TGA and DSC analyses were performed using PerkinElmer TGA 4000 and PerkinElmer DSC 4000, respectively. Quanta 200 Environmental Scanning Electron Microscope with EDAX-EDSSEM was used to record images and chemical composition.

2.2 Synthesis

2.2.1 Synthesis of SB ligand

A solution of 334 mg (2.2 mmol) of 2-hydroxy-5-nitrobenzaldehyde dissolved in a minimum amount of THF (~ 10 mL) was added to THF solution (5 mL) of 270 μL (2.1 mmol) of 2-(1-piperazinyl)ethylamine at room temperature. The mixture was subjected to vigorous stirring until the color turned to light brown. After 2 h, a yellow precipitate was formed, filtered, and washed well with 20 mL of n-hexane and 40 mL of distilled water and then dried. The final product ((E)-4-nitro-2-(((2-(piperazin-1-yl)ethyl)imino)methyl)phenol) was obtained in 84% yield, having a mp = 81 °C. Anal. Calcd. for C13H18N4O3: C, 56.10; H, 6.52; N, 20.13. Found: C, 56.06; H, 6.41; N, 20.05. [M+] m/z = 278.2 (278.14, theoretical). FT-IR: 3240 (νC-OH), 3110 (νC-H-Ph), 2910 (νC-H), 1680 (νC=N) cm−1. UV/Vis. Abs. in MeOH, λmax = 231, 315, and 398 nm. 1H-NMR (600 MHz, CDCl3): δ = at 1.23 (s, 1H, N-H), 2.50 (br, 4H, 2 × CH2-pip), 2.72 (t, J = 6.8 Hz, 2H, CH2N), 2.88 (t, J = 4.7 Hz, 4H, 2 × CH2-pipN), 3.67 (t, J = 6.8 Hz, 2H, C=NCH2), 6.84 (d, J = 8.5 Hz, 1H, Ph), 7.19 (dd, J = 9.0, 2.4 Hz, 1H, Ph), 7.41 (s, 1H, Ph), 7.42 (s, 1H, HC=N), 16.33 (br, 1H, OH) ppm. 13C-NMR (600 MHz, CDCl3): δ = 45.14 (2C, 2 × (CH2)2NH), 47.04 (CH2Npip), 54.81(2C, 2 × (CH2)2N), 58.86 (=NCH2), 119.76 (CAr), 120.61 (CAr), 121.31 (CAr), 127.47 (CAr), 132.52 (CAr), 163.27 (CAr), 171.12 (C=N) ppm.

2.2.2 Synthesis of Cu(II) complexes

A solution 3.60 mmol of copper(II) salt dissolved in 10-mL THF was added to a solution of 3.60 mmol (1.00 g) of NNNO-tetradentate ligand in 10 mL of hot THF. The color of the reaction mixture was turned to green directly within a minute before it started to precipitate. Stirring at room temperature was continued for 10 min to ensure completeness of the reaction. The desired complex was then filtrated and washed with diethyl ether and n-hexane and then dried under vacuum.

Complex 1

A mass of 0.48 g of CuCl2 afforded green water-soluble powder of complex 1 with 80% yield, mp = 198 °C. Anal. Calcd. for C13H19ClCuN4O4: C, 39.60; H, 4.86; N, 14.21%. Found: C, 39.35; H, 4.74; N, 14.09%. FT-IR: 3455 (νH2O), 3375 (νH-N), 3122 (νC-H of ph), 2895 (νC-H), 1620 (νN=C), 1520, 1442, 1378 (νNO2), 1180 (νN-C), 610, 540, and 450 (νCu-N) [23]. UV-Vis in water: λmax nm (εmax in M−1 cm−1): 255 (5 × 104), 375 (2.5 × 104), 670 (160).

Complex 2

A mass of 0.80 g of CuBr2 gave green water-soluble powder of complex 2 with 84% yield, mp = 183 °C. Anal. Calcd. for C13H19BrCuN4O4: C, 35.59; H, 4.36; N, 12.77%. Found: C, 35.44; H, 4.28; N, 12.59%. FT-IR: 3440 (νH2O), 3355 (νH-N), 3116 (νC-H-Ph), 2874 (νC-H), 1610 (νN=C), 1530, 1452, 1376 (νNO2), 1170 (νN-C), 612, 542, and 453 (νCu-N). UV-Vis in water: λmax nm (εmax in M−1 cm−1): 240 (3.0 × 104), 350 (2.2 × 104), 650 (120).

Complex 3

A mass of 0.87 g of Cu(NO3)2 3H2O yielded dark-green water-soluble powder of complex 3 with 65% yield, mp = 235 °C. Anal. Calcd. for C13H19CuN5O7: C, 37.10; H, 4.55; N, 16.64. Found C, 37.38; H, 4.68; N, 16.36%, FT-IR: 3450 (νH2O), 3355 (νH-N), 3118 (νC-H of ph), 2884 (νC-H), 1630 (νN=C), 1525, 1443, 1367 (νNO2), 1168 (νN-C), 615, 542, 458 (νCu-N). UV-Vis in water: λmax nm (εmax in M−1 cm−1): 265 (1.0 × 104), 370 (7.2 × 103), 615 (80).

2.3 Catalytic oxidation of alcohol

The oxidation of benzyl alcohol was achieved by using hydrogen peroxide in the presence of copper(II) complex as a catalyst. Typically, a mixture of 2.5 mmol of benzyl alcohol, 5 mmol of 30% hydrogen peroxide, 1 mol% of copper catalyst, and 10 mL of solvent (see Table 1) was heated at 50 °C for 24 h in two-necked round-bottomed flask connected to reflux column. The reaction was monitored by FT-IR focusing on the C=O vibration at ~ 1700 cm−1. When the reaction was finished, the whole mixture was transferred to 100 mL separatory funnel containing 20 mL of CH2Cl2 and water. The organic layer was evaporated and the produced benzaldehyde was confirmed by IR and NMR.

Table 1 Catalytic oxidation of benzyl alcohol
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3 Results and discussion

3.1 Synthesis and characterization

In the condenzation reaction of 2-(1-piperazinyl)ethylamine with 2-hydroxy-5-nitrobenzaldehyde, SB-functionalized ligand, (E)-4-nitro-2-(((2-(piperazin-1-yl)ethyl)imino)methyl)phenol, was afforded in a very good yield within 2 h at ambient conditions. The presence of different functional groups on the skeleton of the ligand makes it an appropriate tetradentate ligand via three N and one O atoms. Hence, in an equimolar ratio with three copper(II) salts (CuCl2, CuBr2, and Cu(NO3)2 3H2O), separately, the ligand was coordinated in an NNNO-fashion to the metal center in a consecutive deprotonation/coordination process in the absence of base (Scheme1). The ligand and the complexes have reflected good solubility in common polar solvents such as MeOH, DMF, DMSO, and water.

The 1H-NMR spectrum of the ligand in CDCl3 revealed the corresponding peaks for the expected structure (Fig. 1a). The N-H of piperazinyl moiety was found as a broad peak at 1.23 ppm, while the two methylenes of piperazinyl ring were detected at 2.50 (br, 2 × CH2NH) and 2.88 (t, 2 × CH2N) ppm. The two aliphatic methylenes were observed as triplet signal at 2.72 (CH2N) and 3.67 (C=NCH2) ppm. The three aromatic protons were seen as expected at 6.84 (d), 7.19 (dd), and 7.41(s) ppm. The singlet peak at 7.42 ppm was assigned to the proton of imine group. Remarkably, the phenolic proton was extremely deshielded to appear as a broad peak at 16.33 ppm. The 13C-NMR spectrum, on the other hand, displayed all aliphatic, aromatic, and iminic carbon peaks at the expected range of chemical shifts, as illustrated in Fig. 1b.

Fig. 1
figure 1

1H-NMR (a) and 13C-NMR (b) of the SB-functionalized ligand in CDCl3

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The recorded FT-IR of the synthesized ligand and complex 1 are displayed in Fig. 2. The formation of SB functional group was confirmed via the disappearance of the two weak absorption bands at 3361 and 3275 cm−1 from piperazinyl-ethylamine moiety. However, the evanescence of O―H band in the area of 3100–3500 cm−1 in both starting material and ligand can be attributed to the strong intramolecular hydrogen bonding with C–OH and C=N [24,25]. The typical aliphatic and aromatic C–H stretching vibrations were appeared in the range of 3071 to 2840 cm−1. These C–H bands were displayed as well in the complex; the coordination of the ligand to copper metal center was clearly confirmed via the shifting of C=N stretching band from 1655 to 1624 cm−1. Since the electron pair of nitrogen is involved in coordination bond, the distribution of the electron density to copper metal center and the subsequent polarization led to electron depopulation of the C=N group, resulting a slightly lower shift. Additionally, a broad stretching vibration at 3405 cm−1 strongly indicated the coordination of a water molecule to the complex. Further absorptions were present in the spectrum for other functional groups, such as C=C, C–C, C–N, and C–O.

Fig. 2
figure 2

FT-IR of 2-(1-piperazinyl)ethylamine (a), 2-hydroxy-5-nitrobenzaldehyde (b), ligand (c), complex 1 (d)

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Elemental analyses of SB-functionalized ligand and its complexes 1-3 were in a good agreement with the composition of the expected molecular formula and proposed structures, respectively (Scheme 1). The GC-MS for the ligand and one of the copper complexes, complex 1, reflected an excellent fragment consistent with their expected molecular formulas. Furthermore, the ligand and complex 1 were analyzed via EDX. The tetradentate ligand reflected the presence of C, N, and O atoms, while the complex additionally displayed Cl and three typical signals of Cu atoms, indicating the formation of the complex (Fig. 3a, b). Scanning electron microscopy (SEM) was employed to obtain the morphology of the ligand and its complex. Irregular rod-shaped nanostructure was observed for the ligand, whereas, a block-shaped made of fluffy nano-sheets (larger than 10 μm) is grown by the Cu(II) complex (Fig. 3c, d). Surface properties based on the BET technique with nitrogen physisorption at −196.15 °C (77 K) as a carrier gas were evaluated to be 70 and 45 m2/g for the ligand and complex, respectively.

Scheme 1
scheme 1

Synthesis of SB-functionalized ligand and it complexes

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Fig. 3
figure 3

EDX for ligand (a) and complex 1 (b); SEM images for ligand (c) and complex 1 (d)

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3.2 Electronic absorption and fluorescence spectra

The experimental electronic absorption spectra of the starting materials, synthesized ligand, and complex 1 were acquired from neat methanolic solution in the spectral range of 200–800 nm at ambient conditions. The free amine was characterized with band at λmax = 223 nm resulting from n-σ* electron transition, while two bands in the UV area were displayed by the 2-hydroxy-5-nitrobenzaldehyde derivative at λmax = 240 and 310 nm attributed to n-σ* and π-π* electron transfer, respectively (Fig. 4a, b). Three broad bands with maximum absorption at 231, 315, and 398 were revealed by the ligand, these absorptions could be ascribed to n-σ*, π-π*, and n-π* [26,27]; the last electron transition indicates the formation of the ligand from the condensation reaction (Fig. 4c). Complex 1 has exhibited two strong absorptions at λmax = 252 and 357 nm, the first peak was assigned to n-σ* with distinctive bathochromic shift from the value observed by the ligand. Whereas, the second wide peak could be resonated to ligand-to-metal charge transfer (LMCT) (Fig. 4d) [28]. This spectral pattern indicates the coordination of the tertradentate ligand to copper metal center. Furthermore, at a high level of concentration (as the molar absorptivity is very low), the complex has revealed the d-d absorption band in the visible region, at λmax = 675 nm (Fig. 4e), which is in consistence with similar reported complex systems [5,6,7,8,9,10].

Fig. 4
figure 4

UV-Vis spectra of 2-(1-piperazinyl)ethylamine (a), 2-hydroxy-5-nitrobenzaldehyde (b), ligand (c), complex 1 (d), and complex 1 at concentrated level (e)

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The emission spectra for the ligand at 360 nm at different concentrations (0–2.9 × 10−4 M) are presented in Fig. 5a. As obvious from the spectra, the emission intensity of the ligand at about 475 nm increased until a concentration of 5.8 × 10−5 M then decreased afterwards. The ligand’s emission intensity vs. its concentration is plotted in Fig. 5b; the ligand’s optimum intensity occurred at a concentration of 5.8 × 10−5 M. The decrease in intensity at high concentrations (e.g., >5.8 × 10−5 M) can be explained by reabsorption of emitted photons by ground-state molecules. The emission spectra for the complex 1 (0–2.0 × 10−4 M) are low and can be neglected compared to the ligand emission at the same concentrations (5.8 × 10−5 M) as seen Fig. 4c, which reflects the maximum emission of the free ligand at 5.8 × 10−5 M. Meanwhile, a turn-off of the complex’s emission intensity occurred at the same concentration. Due to the tetradentate NNNO of the ligand, emission turn-off was recorded upon its coordination to the copper center to form complex 1. Similar observations were reported for the quenching of the fluorescence of certain ligands after complexing with Cu(II) [29,30,31,32]. The reason behind this turn-off phenomenon is unclear but this may be due to the predominance of photo-induced electron transfer (PET) over chelation-enhanced fluorescence (CHEF) [29,30]. Also, this could be due to the alternation of the structure of the ligand upon complexation [33].

Fig. 5
figure 5

Emission spectra of the ligand in DMSO at room temp. (C1 = 0, C2 = 2.9×10−6, C3 = 5.8 × 10−5, C4 = 1.45 × 10−4, C5 = 2.32 × 10−4, C6 = 2.9 × 10−4 M) at different concentrations (a), ligand optimum emission concentrations (b), and free ligand (turn on) and it’s complex 1 (turn off)

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3.3 Job’s method, gravimetric analysis, conductivities, and magnetic susceptibility

Since the prepared complexes did not crystallize in a suitable quality for XRD-crystal measurement, Job’s method was employed to get more information about the stoichiometry of the desired complexes. Therefore, titration of the desired NNNOH ligand with varying concentrations of Cu(II) in water is presented in Fig. 6a. The Job’s plot for NNNO-Cu(II) system (complex 1) is illustrated in Fig. 6b, which reflected the formation of the complex at a 1:1 ratio. Such coordination enabled us to propose a mono-halide octahedral Cu(II) geometry via coordinated tetradentate (NNNO−) SB, as demonstrated in Scheme 1. Thus, to examine the mono-halide structural formula of the complexes, halide quantity in complexes 1 and 2 were gravimetrically evaluated using excess amount of AgNO3(aq) then referenced to CuCl2 3H2O and CuBr2 6H2O respectively. The gravimetric analysis results showed that complexes 1 and 2 have half amounts of halide compared to their corresponding starting complexes. Moreover, the resulting product from gravimetric analysis of both complexes 1 and 2 (Scheme 2) was confirmed by IR and UV-Vis to be complex 3.

Fig. 6
figure 6

UV-Vis absorption spectrum for the titration of SB ligand with Cu(II) at 675 nm (a); Job’s plot for SB-Cu(II) system (b); gravimetric analysis of complex 2 (c); and electrolytic conductivity (I) and magnetic susceptibility (II) of complex 1 (d)

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Scheme 2
scheme 2

Gravimetric analysis of complexes 1 and 2

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The electrolytic conductivity values at 22 °C in 5 mL (4 ×10−5 M) in distilled water were found to be 352, 484, and 285 μS/cm for complexes 1, 2, and 3, respectively. However, the initial copper(II) salt (CuCl2, CuBr2, and Cu(NO3)2) were found to measure 705, 985, and 589 μS/cm under identical concentrations and conditions. Since the conductivity of the prepared complexes measured about half values of starting salts, the desired complexes are expected to be mono-halides or mono-nitrate complexes in its nature form. Remarkably, upon increasing the temperature up to 100 °C for the aqueous solution of complex 1, the ionization behavior of the halide was observed to increase, as seen in Fig. 6d.

The magnetic susceptibility of 4 ×10−5 mol of desired complexes dissolved in 5-mL distilled water was evaluated. At 22 °C, the direct magnetic susceptibility was found to be 120 for complex 1, 110 for complex 2, and 100 for complex 3. The magnetic behavior has demonstrated very minor changes with increasing temperature from 22 to 100 °C as seen (for complex 1) in Fig. 6d.

3.4 Chromotropism study

The d–d transition of metal ions, metal-to-ligand charge transfers (MLCT) and ligand-to-metal charge transfers (LMCT), are in principle the causes of various good-looking colors in transition metal complexes. However, under chemical or physical conditions, namely chromotropism, the color of some complexes is reversibly altered according to the conditions, which includes electro-redox (electrochromism), ion (ionochromism), light (photochromism), pH (halochromism), pressure (piezochromism), solvent (solvatochromism), and temperature (thermochromism) reactions [34,35].

The Cu(II) complexes with d9 electron configuration are expected to possess explicit Jahn-Teller effect, making them attractive targets for solvatochromic investigation. The selected complex 1 was found to have low solubility in organic solvents. For that reason, the number of solvents introduced to the solvatochromism study was limited to water, methanol, DMSO, and DMF. Different colors have been reflected by dissolving the complex in these solvents, visible to the naked eye. In water, the LMCT showed maxima at 355 nm, shifted to 362 nm in methanol, 373 nm in DMF, and 375 nm in DMSO (Fig. 7a). Similarly, the d-d transition absorptions displayed λmax at 658 nm in water, which shifted to 680 nm in methanol, 685 nm in DMF, and 705 nm in DMSO (Fig. 7b). This phenomenon implies that both bands, LMCT and d-d transition, have the same solvatochromic behavior [36,37,38]. The solvation relation was examined between the observed maxima of both bands and Gutmann’s solvent acceptor numbers (AN) [39], revealing no clear relation (decreased followed by increased). However, a positive linear relation with Gutmann’s solvent donor numbers was displayed with correlation factors (R2) of 0.942 (LMCT) and 0.924 (d-d transition) as shown in Fig. 7c, d. This behavior indicates that the copper(II) complex is acting as a strong Lewis acid.

Fig. 7
figure 7

Solvatochromism of complex 2: Abs vs λmax at LMCT (a) and at d-d (b), λmax vs solvents AN/DN at LMCT (c) and at d-d (d)

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The halochromic effect of complex 1 was demonstrated as an off-on process. The green-colored solution in DMF was turned to colorless (off) upon the addition of acid-like HCl. Subsequently, the initial color was restored reversibly (on) by addition of basic solution such as NaOH. It was noticed that when the concentration of the added acid increased, the λmax at 670 nm started to gradually decrease in terms of intensity without visible shifting of the d–d band, as shown in Fig. 8a. Hence, the de-colorization of the green solution could be rationalized to the protonation of the coordinated ligand that in turn is responsible for the de-structuring process. The spectrophotometric titration of the complex 1 with HCl at λmax = 670 nm showed that the de-colorization is mainly completed after consumption of four equivalent protons (Fig. 8b). Such value is consisted with the tetradentate NNNO protonation nature of the ligand to finish up with hydrated CuCl2 species and expected protonated ligand, ligand (Fig. 8b).

Fig. 8
figure 8

[H+]-dependent visible spectra of the complex 1 in water at RT (a) and Abs vs [H+] relation at constant λmax (b)

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Furthermore, the thermochromic behavior for complex 3 was studied at a temperature range between 20 to 90 °C with the focus on the d–d transition band. A gradual change in color from green to brown has been recorded upon raising up the temperature of the solution of the complex. This could be attributed to the fact that the coordinated halide/nitrate could be dissociated from the metal center and replaced by water-solvent, as seen in Fig. 9a. Therefore, the environmental coordination around the Cu(II) is changed reflecting a nonlinear bathochromic shift from 615 nm at 20 °C to 675 nm at 90 °C (Fig. 9b). The thermochromism here is a reversible process since the initial green color returns back after cooling, indicating recovery of the complex [35].

Fig. 9
figure 9

Complex 3 aqua thermochromism: Abs vs wavelength at different temperatures, and λmax vs temperature relations (b)

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3.5 Thermogravimetric analysis

The material purity and thermal stability of the free SB ligand and complex 1 were investigated via thermal gravimetric analysis (TGA) and differential thermal analysis (DTA) in the range of 20 to 900 °C and heating rate of 10 °C per minute in an open-atmosphere (Fig. 10). The SB ligand reflected an acceptable stability up to 200 °C, then started to completely decay in a single step with Toff ~ 450 °C and TDTA = 270 °C. However, complex 1 showed a completely different decomposition pattern with three successive pyrolysis steps. The first stage of decomposition was recorded between 138 and 155 °C for the loss of the coordinated water molecule from Cu(L)Cl H2O structure with TDTA = 148 °C. This loss is equivalent to 4.5% mass (theoretically 4.7%) to produce Cu(L)Cl complex. The second step started from 280 to 500 °C involving approximately 71% mass loss (theoretically 70.5%) for the dissociation of the ligand from the former copper complex residue in a very broad complex step, finished with four TDTA = 295, 340, 430, 470 °C. Finally, the residual CuCl decomposed to give Cl and Cu, the later reacted with oxygen to produce Cu=O as final remaining, having TDTA = 650 °C with 18.8% yield (theoretically 19.1%).

Fig. 10
figure 10

TGA (a) and DTG (b) of the free SB and complex 1

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3.6 Selective catalytic oxidation

The capability of the three complexes towards selective catalytic oxidation of benzyl alcohol to benzaldehyde has been evaluated using hydrogen peroxide as a green oxidant. The conversion rate, product selectivity, and benzaldehyde yield of the model reaction are demonstrated in Table 1. Typically, a mixture of 2.5 mmol of benzyl alcohol and 5 mmol of 30% hydrogen peroxide in the presence of 1 mol% of copper catalyst in 10 mL of solvent was heated at 50 °C for 24 h in a 20-mL vial.

At a temperature of 50 °C, all copper complexes displayed excellent selectivity, but with variable conversion rate to yield the desired aldehyde without the formation of the unwanted benzoic acid (entries 1–3). When the temperature was raised to 70 °C or the time was extended to 48 h (entries 4 and 5), the conversion of benzyl alcohol was accomplished to deliver the product in a moderate yield along with benzoic acid, thermodynamically favored product. Other polar organic solvents, such as THF, MeCN, and DMSO, have demonstrated high percentage of conversion of the starting material (entries 6–8). Moreover, the reaction did not proceed in the absence of copper catalyst (entry 9) and only traces of the product were detected when no hydrogen peroxide was used (entry 10). Overall, complex 1 was demonstrated as the most active precatalyst at the abovementioned optimized conditions (as seen in Fig. 11a); the temperature was found to be a key factor to control the selectivity of the catalyst. It was noticed that no oxidation reaction was achieved in the presence of trace amounts of HCl or NaOH, even after about 50% of conversion of benzyl alcohol; the addition of acid or base as additive will cease the catalytic reaction. Eventually, to investigate the progress of the reaction, small amounts of samples were taken at appropriate time intervals for direct IR analysis. The concentration of carbonyl functional group of benzaldehyde product was observed to increase by time, as seen in Fig. 11b.

Fig. 11
figure 11

Conversion % vs time for the three copper complexes (a) and IR-monitored formation of benzaldehyde (b)

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4 Conclusion

New NNNOH tetradentate SB–functionalized ligand and its copper(II) complexes were characterized by several spectral analysis. These complexes showed an interesting similar solvatochromic behavior at LMCT and d-d bands, acid-base turn-off-on halochromic effect, and bathochromic thermochromisim behavior. The florescence behavior of the free ligand at λmax = 475 nm started to turn off by complexation to the copper(II) center as in complex 1. The synthesized complexes reflected high degree of catalytic activity in selective oxidation of benzyl alcohol to benzaldehyde using H2O2 as a green oxidant under mild reaction conditions. Based on the chromotropism and oxidation results, the new Cu(II) complexes could be utilized as an efficient catalyst in oxidation reactions and material for applications as optical sensors and Lewis acid-base color indicators [34,40].