Novel Nd-N/TiO2 Nanoparticles for Photocatalytic and Antioxidant Applications Using Hydrothermal Approach.

In this study, photocatalysis was employed to degrade a wastewater pollutant (AB-29 dye) under visible light irradiation. For this purpose, nitrogen (N)- and neodymium (Nd)-doped TiO2 nanoparticles were prepared using the simple hydrothermal method. X-ray diffraction (XRD) revealed an anatase phase structure of the Nd-N/TiO2 photocatalyst, whereas properties including the surface morphology, chemical states/electronics structure and optical structure were determined using transmission electron microscopy (TEM), X-ray photoelectron spectroscopy (XPS) and UV-visible (UV-vis.) and photoluminescence (PL) spectroscopies. Photocatalytic testing of the prepared nanomaterials was performed to remove acid blue-29 (AB-29) dye under visible-light exposure. The prepared Nd-N/TiO2 nanoparticles demonstrated a superior photocatalytic activity and the decolorization efficiency was about 92% after visible-light illumination for 1 h and 20 min, while N/TiO2, Nd/TiO2 and TiO2 only showed a 67%, 43% and 31% decolorization efficiency, respectively. The enhanced photocatalytic activity of the Nd-N/TiO2 photocatalyst was due to a decrease in the electron/hole's recombination and the increased absorption of TiO2 in the visible range. The reusability results showed that the average photocatalytic activity decrease for all the samples was only about 16% after five consecutive cycles, indicating a good stability of the prepared nanomaterials. Moreover, the radical scavenging activity of the prepared nanomaterials was evaluated using the DPPH method. The novel Nd-N/TiO2 exhibited a higher antioxidant activity compared to all the other samples.

1. Introduction

High rates of industrialization, urbanization and overpopulation result in the production of wastewater on a large scale. Wastewater contains various toxic and harmful substances which are clear threats to human life and the environment [1]. Specially, wastewater contaminants including organic dyes, drugs, pigments, hydrocarbons, etc., are creating permanent damage to ecosystems and the environment [2]. Therefore, wastewater recycling for various objectives requires viable, clean and sustainable technologies for the degradation of toxic water contaminants [3]. For this purpose, the most effective approach is to design an adoptable photocatalyst to decompose the pre-existing environmental pollutants. Heterogeneous photocatalysts such as TiO2, ZnO, Fe2O3, CdS, SnO2, V2O5, g-c3N4, etc., have been found to effectively photodecompose many harmful and toxic organic pollutants of wastewater [4,5,6,7]. Titanium dioxide has been commonly used in heterogeneous photocatalysis owing to its extraordinary characteristics, namely its low cost, strong oxidizing power and stability in aqueous environments [8]. However, intrinsic TiO2 suffers from the lower absorption of visible light, attributable to its broader band gap (~3 eV) and limited photocatalysis activity due to the prompt reunion of charges (electrons and holes) [9,10]. A wide variety of doping techniques have been employed to solve these problems, including doping with transition and noble metals, non-metallic ions and rare earth metals [11,12,13,14,15,16,17]. In particular, the doping of non-metallic ions into TiO2 is very easy and is the most active method to achieve solar light absorption in the visible range and higher photocatalysis. It was previously observed that N doping into TiO2 systems develops N 2p energy states above the valence band edge of TiO2, thus decreasing its band gap and enhancing light utilization in the visible range [18]. Additionally, N doping also reduces the reunion of charges in the N-TiO2 system for the better performance of TiO2 as a photocatalyst. However, N-TiO2 photocatalyst efficiency is still limited because of the low lifetime of the photogenerated charges during photocatalysis. Therefore, doping rare earth metals into TiO2 is also a useful method to advance its photocatalysis efficiency through the reduction in the charge carriers’ recombination [19]. Compared with other rare earth metals, Nd is an efficient element that has gained attention in many studies due to its good properties [20,21]. Nd-doped TiO2 has the ability to reduce band gaps and overcome the reunion of charges for enhanced photocatalytic activity [22,23,24]. To the best of our knowledge, no report can be found in the literature on Nd and N co-doped TiO2 nanomaterials for photocatalytic applications. Therefore, the development of Nd-N/TiO2 photocatalytic systems will be a good strategy to achieve a higher decolorization of organic contaminants under visible-light exposure.

In this study, we prepared a Nd-N/TiO2 photocatalyst using a simple hydrothermal method. The obtained TiO2-based nanomaterials exhibited wider solar light absorption and an enhanced photocatalytic activity in the decomposition of acid blue-29 dye owing to the cooperative effects of the Nd and N atoms in the Nd-N/TiO2 system.

2. Experimental Procedure

2.1. Synthesis of Nd-N/TiO2 Photocatalyst by Hydrothermal Method

The Nd-N/TiO2 photocatalyst was prepared using a single-step hydrothermal process. In the experiment, the reaction was started by adding the tetrabutyl titanate (TBT, 10 mL) to a water, ethanol and acetic acid mixture (25 mL + 25 mL + 10 mL), which was stirred for 20 min at 25 °C. Following previous steps, the required amount of urea and Nd (NO3)3 6H2O were mixed into the initial solution. In the next stage, the solution was transported to a stainless-steel autoclave (100 mL) containing a Teflon beaker and was heat treated at 120 °C for 6 h. After the completion of this process, washing of the obtained material was performed using water. In the final step, it was heated at 100 °C for 9 h in an oven initially and then it was treated at 400 °C for 2 h in a furnace. The molar percentage of Ti to urea was 1:2, and in the Nd/TiO2 and co-doped sample (Nd-N/TiO2), the percentage of the Nd dopant was 2% according to our previous study [23]. The names of the samples were pristine TiO2 (obtained without using Nd and N sources), Nd/TiO2, N/TiO2 and Nd-N/TiO2.

2.2. Characterization of Synthesized Photocatalysts

In this study, the crystallinity and crystalline phase properties of the prepared materials were examined using a Shimadzu XD-5A powder diffractometer. Transmission electron microscopy (TEM, 2100, Jeol, France) determined the morphology of the nanomaterials. XPS (Thermo-VG Scientific, ESCALAB250, monochromatic) was used for the identification of the chemical states and electronic structure of the photocatalysts. UV–visible absorption spectra were observed with the help of a (UV-1800, Shimadzu, Kyoto, Japan) spectrometer. A fluorescence spectrometer (FP-8200, Jasco, Pfungstadt, Germany) was utilized to obtain PL spectra at a 320 nm wavelength (excitation).

2.3. Photocatalytic Efficiency Measurement

To explore the photocatalysis properties of the prepared materials, the degradation of acid blue-29 (AB-29) dye was observed. Its optical absorption maxima occurred at about 630 nm, where the scattering of light was minimum. The experiment was performed in a pyrex glass photoreactor containing water in a circulating case using a halogen lamp (300 W) with a cut-off filter (λ ≥ 420 nm) as the light source. During all the experiments, 100 mg of the photocatalyst material and 10 mg of AB-29 dye was well dispersed in 200 mL of deionized water. Initially, a blank test was accomplished separately for dye degradation without a photocatalyst under light exposure and no appreciable loss of dye was found in the experiment. Moreover, after adding the photocatalyst to the dye solution, the suspension was magnetically stirred for 1 h in the dark to reach adsorption/desorption equilibrium. After the adsorption/desorption equilibrium reaction, the concentration was taken as the initial concentration of the AB-29 dye. Next, under visible light exposure, a photocatalytic experiment was started, and 5 mL of the degraded solution was collected every 30 min to check the degradation of the AB-29 dye using a UV–visible spectrometer (Shimadzu-UV-1800). In addition, every collected 5 mL of solution were centrifuged/filtered and then, after taking UV–visible absorption spectra, they were returned back to the original dye solution immediately.

2.4. Antioxidant Activity Measurement (DPPH Assay)

The antioxidant potential of the prepared samples was monitored via the DPPH (2, 2-diphenyl-1-picrylhidrazyl) method following the protocols of Helmy et al. [21]. Initially, the DPPH (1.97 mg) was dissolved in methanol (50 mL) to prepare a stock solution and it was stored at 4 °C to use it further in the experiment. Next, different sample solutions were made by dissolving TiO2, Nd/TiO2, N/TiO2, Nd-N/TiO2 and/or ascorbic acid in 1 mL of deionized water to obtain a variety of concentrations (20, 40, 60, 80 and 100 µg/mL) of the catalyst and ascorbic acid. After this, 2 mL of the DPPH solution was mixed with 1 mL of the sample solution containing different concentrations as mentioned above. The mixture of deionized water (1 mL) and DPPH (1 mL) played the role of the control. The concentration of the scavenged radicals was then evaluated via measurements of absorption decrease after 25 min at a 517 nm wavelength. Furthermore, in order to measure the scavenging activity of the DPPH radicals, the following equation was used: where control absorbance means absorbance when the antioxidants are not present, while sample absorbance denotes absorbance when the antioxidants are present in the reaction. All the experiments were repeated three times and the mean value was considered for the experimental results plots.

3. Results and Discussion

3.1. XRD and TEM Analysis

Figure 1 shows the TiO2, Nd/TiO2, N/TiO2 and Nd-N/TiO2 nanoparticles’ XRD patterns. The bare TiO2 nanoparticles exhibited diffraction peaks at 25.3°, 38.0°, 48°, 54.5°, 62.7°, 69.5° and 75.1°, conforming the values of hkl (101), (004), (200), (105), (204), (220) and (215), respectively. This clearly reveals the anatase crystalline phase of TiO2, agreeing with (JCPDS 21-1272). The Nd/TiO2, N/TiO2 and Nd-N/TiO2 samples also showed the same structure (anatase) except the crystallinity seemed to be reduced, indicating that the dopants retarded the transition of the anatase phase to any other phase (rutile or brookite) [25]. Moreover, the absence of Nd or its oxide phase peaks in the Nd/TiO2 and Nd-N/TiO2 samples might be ascribed to the lower doping contents of Nd or the increased amorphous nature of the doped samples. Moreover, the crystallite size of all the samples was measured using the Scherrer formula [23]. The average crystallite size for the TiO2, Nd/TiO2, N/TiO2 and Nd-N/TiO2 samples were found to be 15.4 nm, 13.3 nm, 12.0 nm and 9.6 nm, respectively. This decrease in crystallite size can be attributed to the cooperative effects of Nd and N doping in the TiO2 nanoparticles.

Figure 1

XRD graphs of different photocatalysts prepared by hydrothermal method.

TEM studies are useful for identifying the size and shape of nanomaterials. Figure 2a,b illustrate TEM images of the TiO2 and Nd-N/TiO2 nanomaterials, respectively. The particles in both materials were nearly spherical and were uniformly separated without any distinguishable agglomeration. The average particle size for both materials was less than 20 nm. Furthermore, in the Nd-N/TiO2 sample, the black Nd was homogeneously dispersed on the TiO2 surface, showing the more defective nature of the Nd-N/TiO2 sample.

Figure 2

TEM images of (a) TiO2 and (b) Nd-N/TiO2 nanoparticles.

3.2. XPS Analysis

The electronic structure and chemical states of Nd-N/TiO2 were studied using XPS. Figure 3 shows the Nd-N/TiO2 sample’s XPS spectra of Ti 2p, O 1s, N 1s and Nd 4d. The stronger peaks, namely, Ti 2p3/2 and Ti 2p1/2, appeared at 458.6 eV and 464.4 eV, respectively (Figure 3a), signifying that titanium metal (Ti) existed as Ti4+ [26,27]. As revealed in Figure 3b, the spectrum of O 1s can be fitted into peaks. The appearance of peak at 530.0 eV shows an oxygen atom’s existence in the TiO2 lattice (Ti-O bond) and the second peak at 531.6 verifies the presence of a surface hydroxyl oxygen [28]. In a highly resolved spectrum of N 1s, as shown in Figure 3d, the first peak at 395.75 eV can be attributed to Ti-N bonds, which confirm that the doping of N into the TiO2 material was substitutional [29]. The other peak at 399.79 verifies the interstitial N doping in the TiO2 nanoparticles (Ti-O-N) [30]. In the Nd 4d spectrum (Figure 3d), the single peak appearing at 121.5 eV shows a positive shift of 3.5 eV from the metallic Nd° (118). This positive shift suggests that the Nd dopant was present in the TiO2 nanoparticles as Nd3+ ions [31,32,33].

Figure 3

XPS core level spectra of (a) Ti 2p, (b) O1s, (c) N 1s, (d) Nd 4d for Nd-N/TiO2 sample.

3.3. UV–Vis Spectroscopy Analysis

Figure 4a shows the absorption spectra of the pristine TiO2, Nd/TiO2, N/TiO2 and Nd-N/TiO2 samples. The band gap energy (E) of all the samples can be calculated using the equation:

Figure 4

(a) Absorption spectra and (b) Tauc plots of TiO2, Nd/TiO2, N/TiO2 and Nd-N/TiO2 nanoparticles.

Here, the absorption coefficient is denoted by , while represents the energy of the photon and B is a constant [29]. The values of the band gap of the bare TiO2, Nd/TiO2, N/TiO2 and Nd-N/TiO2 were calculated to be 3.20 eV, 3.19 eV, 2.91 eV and 2.85 eV, respectively, as shown in Figure 4b. This indicates that the N dopant element had more ability to lessen the band gap of TiO2 compared to the Nd dopant. Overall, the doping of Nd and N played an effective role in decreasing the TiO2 band gap (3.2 to 2.85 eV). This good reduction in the band gap of the resulting nanomaterial (Nd-N/TiO2) was due to the fact that the interactive property of the doping element and TiO2 and the creation of new energy states within the TiO2 band gap always results in a band gap decrease [32,33].

3.4. PL Spectroscopy Analysis

PL spectroscopy has been extensively utilized to determine the charge carriers’ trapping efficiency, immigration and transportation to know the destiny of the charges in semiconducting nanomaterials [26]. Figure 5 represents the PL spectra of the TiO2, N/TiO2, Nd-N/TiO2 and Nd-N/TiO2 nanoparticles. As displayed in the results, the pristine TiO2 had a large PL intensity, whereas, after the incorporation of Nd and N, the PL intensity decreased, displaying a suppressed reunion of the electron/hole. Most interestingly, the co-doped Nd-N/TiO2 sample exhibited the lowest PL intensity compared to all the other samples. This is clear evidence that the Nd and N co-doping had a significant influence on separating the charge carriers in TiO2 in order to boost photocatalytic performance for dye degradation.

Figure 5

Photoluminescence spectra of TiO2, Nd/TiO2, N/TiO2 and Nd-N/TiO2 samples.

3.5. Photocatalytic Activty

The effectiveness of the samples in the decolorization of the AB-29 dye was investigated under the exposure of visible light. Figure 6a shows the relative variation in AB-29 concentration (C/C) against time using TiO2-based photocatalytic nanomaterials. The Nd-N/TiO2 photocatalyst demonstrated a 92% degradation of AB-29 dye after 120 min of exposure to solar light, while N/TiO2, Nd/TiO2 and TiO2 only exhibited a 67%, 43% and 31% degradation, respectively. Therefore, it was confirmed that Nd-N/TiO2 had better photocatalysis activity than the single-doped (Nd/TiO2, N/TiO2) or pure TiO2. Moreover, Nida et al. [34] found 82% AB-29 dye degradation in an irradiation time of 90 min when they used CdS/TiO2 nanoparticles. Most of the dyes during photocatalytic degradation followed the Langmuir–Hinshelwood kinetic model [34,35], and the relation is given as:

Figure 6

(a) Concentration variation (C/C) of AB-29 dye degradation, (b) plots of ln (C) against exposure time for decolorization of AB-29, (c) decolorization rate of AB-29 over TiO2, Nd/TiO2, N/TiO2 and Nd-N/TiO2 photocatalysts, (d) recyclability of different photocatalysts for five continuous cycles.

Here, ‘k’ represents the rate constant of the relevant reaction (mM min−1), the adsorption coefficient of the reactants is ‘K’ (mM−1) and C denotes the concentration of the reactants (mM). In the case of a low concentration ‘C’, one can write the above equation in the form of apparent pseudo-first-order kinetics [35].

The degradation curve (Figure 6a) represents exponential decay and follows pseudo-first-order kinetics practically well. The rate constant can be found for the samples via a ln (C/C) plot against illumination time (Figure 6b) using the below equation: where C is the staring dye concentration, C represents the concentration of the AB-29 dye after time ‘t’ and k denotes the apparent rate constant (min−1). Furthermore, the dye degradation rate was determined using the following formula [36]:

Here, ‘k’ denotes the rate constant, C represents the dye concentration, while n represents the reaction’s order. Figure 6c shows the degradation rate, which followed the order TiO2 (1.0 × 10−4) < Nd/TiO2 (1.6 × 10−4) < N/TiO2 (3.5 × 10−4) < Nd-N/TiO2 (5.3 × 10−4). The superior photocatalysis efficiency of the Nd-N/TiO2 photocatalyst was due to broadening the absorption of solar light and the reduced reunion of the electron/hole, as was confirmed in the UV–vis and PL spectroscopies (Figure 5 and Figure 6).

Figure 6d demonstrates the photocatalytic decomposition of the AB-29 dye over the TiO2, Nd/TiO2, N/TiO2 and Nd-N/TiO2 nanoparticles over five consecutive cycles. The decrease in the decolorization efficiencies of TiO2, Nd/TiO2, N/TiO2 and Nd-N/TiO2 after five cycles was 17%, 18%, 15% and 15%, respectively. This verifies the good stability of the prepared photocatalyst (Nd-N/TO2) along with its superior photocatalytic activity. Moreover, the excellent photocatalytic activity of Nd-N/TO2 can be understood as indicated in the mechanistic diagram (Figure 7). It is known that rare earth elements were unable to replace Ti4+ in the crystal matrix because of their incompatible ionic radii; therefore, rare earth metal ions could exist in the form of rare earth metal oxides and they could be dispersed on the surface of TiO2 [37]. Additionally, rare earth metal ions could act as a trapping site, which would efficiently reduce the recombination of the photogenerated charge carriers and then a higher photocatalytic performance could be achieved [28]. Therefore, based on these facts, Nd-N/TiO2 (2.85 eV) absorbed visible light photons and, as a result, a higher number of electrons were transported from the valence band to the conduction band of Nd-N/TiO2 via Nd3+ capturing the sites below the conduction band of the material and participating in the reduction process to produce superoxide radicals (•O2−). At the same time, the holes left behind in the valence band reacted with water to generate hydroxyl radicals (OH•). These photogenerated radicals (superoxide and hydroxyl) finally participated in the decomposition of the AB-29 dye when exposed to solar light. Furthermore, as presented in Figure 7, the Nd dopant had the capability to capture electrons from the conduction band of Nd-N/TiO2, reducing the reunion of the charges. Thus, in this way, the Nd dopant contributed to enhancing the photocatalytic efficiency of the prepared photocatalyst.

Figure 7

Schematic illustration of photocatalysis mechanism of Nd-N/TiO2.

3.6. Antioxidant Activity

The scavenging action of all the samples was assessed via a DPPH test. It is well known that DPPH can be easily converted to a DPPH-H compound (stable) when it accepts H2 radicals from the tested nanomaterials [24]. During this process, its color changes from violet (dark) to a dim yellow. Therefore, DPPH reduction gives an estimation of the radical trapping of the tested material. Figure 8 shows the scavenging activity (%) of TiO2, N/TiO2, Nd-N/TiO2 and Nd-N/TiO2 for the DPPH assay. The scavenging performance increases with an increasing concentration of the antioxidant. The activity was boosted in the following order: ascorbic acid (35–93%) > Nd-N/TiO2 (26–82%) > Nd/TiO2 (22–73%) > N/TiO2 (20–61%) > TiO2 (14–57%), with an increasing concentration from 20 to 100 µg/mL. These results show that Nd-N/TiO2 is a superior antioxidant over all other samples. In addition, the results found in this study are good compared with other workers, including plum peals mediated-TiO2 nanoparticles, which exhibited a 78% scavenging activity for DPPH at the same concentration (100 µg/mL) [38]. In another report, Hosney et al. [2] observed a 41.89% DPPH scavenging activity at 50 µg/mL when using a Ag/ZnO@Biochar nanocomposite. Rajeswari et al. [39] found a 55% antioxidant activity at 200 µg/mL for DPPH scavenging using a Pd-RGO-ZnO nanocomposite.

Figure 8

Antioxidant activity of different samples against DPPH assay at different concentrations of nanoparticles in DPPH solution.

4. Conclusions

Nd-N/TiO2 nanoparticles were synthesized via a simple hydrothermal route. The structural, morphological and optical properties were improved due to Nd and N doping. The incorporation of Nd and N played a greater role in decreasing the band gap of TiO2 from 3.20 eV to 2.85 eV, making them able to absorb visible light effectively. In addition, the recombination of the photogenerated charge carriers was greatly reduced due to the co-doping of Nd and N into the Nd-N/TiO2 system. Compared with all the other samples, Nd-N/TiO2 exhibited a higher photocatalytic efficiency (92%) in the removal of AB-29 dye when irradiated with visible light. Moreover, this novel photocatalyst also indicated a good antioxidant efficiency of 82% at the maximum concentration of nanoparticles in the DPPH solution (100 µg/mL).