Heterojunctions have proven to be effective catalysts for removing organic pollutants and heavy metals from wastewater. The following study is also about the formation of 2D heterojunction tellurium-doped zinc oxide composite with sulfur-doped graphitic carbon nitride ([email protected]3N4) by adopting a low-cost, simple, and ecofriendly coprecipitation technique. Thiourea was calcined to prepare S-g-C3N4 using the thermal degradation method. The characterization of synthesized photocatalysts was carried out by using SEM-EDX, FTIR, and XRD. The results obtained showed that the incorporation of tellurium caused an alteration in the wurtzite structure of ZnO. SEM-EDX analysis validated the purity of the synthesized samples due to the absence of any additional peaks. The decrease in the bandgap was also noted by the formation of composites. Using methylene blue as a reference dye, the UV-vis spectrophotometer was utilized to calculate the absorbance for photocatalytic degradation behavior. As a result of tellurium doping into the ZnO lattice, photocatalytic oxidation/reduction was improved, according to the results. 3Te-ZnO NPs showed the best degradation rate among dopant series, while an excellent overall degradation rate was noted by fabricated composite [email protected]3N4. The best doped ZnO and composites were also used as sorbents for the abstraction of heavy metal (Cr(VI)) from water via adsorption. A definite rise in the removal efficiency percentage of chromium ions was observed by using these sorbents. The overall photo degradation rate and adsorption behavior noted were in ZnO<Te-ZnO<Te[email protected]3N4 order. When compared to ZnO, Te-ZnO, SCN, and [email protected], the [email protected] NCs have outstanding antifungal potential. The improved dispersibility and interaction of [email protected] with membrane and intracellular proteins of fungi may be the cause of the greater effect of [email protected]

1. Introduction

Unpredictable climate change and an increase in human population have recently resulted in the crisis of clean water supply for both people and wildlife [1, 2]. Moreover, dye emission from various sectors is another issue that contaminates water and has drawn a lot of attention [3]. The effluents obtained from the printing industry and textile dyeing are complex and contain dissolved and suspended solids, organic compounds, and heavy metals [4]. Since azo dyes do not stick to the cloth during the dyeing process, 15 to 50 percent of them are washed away with the wastewater. This wastewater is employed in irrigation procedures even though it is not beneficial for crop germination or growth [57]. Textile dyes also cause mutations and generate cancer-causing agents [8]. A kind of basic cationic dye that is widely used by many industries is methylene blue (MB). Shock, tissue necrosis, cyanosis, vomiting, and jaundice become more common in affected individuals [8]. Dyes decrease the light penetration in water, thus affecting the photosynthesis process [9]. Therefore, it surely needs to remove these dyes from the wastewater. To treat contaminated effluents, several physical, chemical, and biological techniques have been employed. The photocatalytic degradation of organic pollutants utilizing nanoparticles as the photocatalyst is one of the environmentally friendly methods for treating industrial effluent.

The photocatalysis mechanism involves the conversion of toxic pollutants into nontoxic ones through light irradiation [10]. A wide range of semiconductor photocatalysts (e.g., TiO2 [1115], ZnO [1], CuO [16], NiS [17], SnO2 [18], ZrO2 [19], and WO3 [20]) with various nanostructures have been studied. At ambient temperature, ZnO has a relatively wide bandgap of about 3.37 eV, an excitation energy of about 15 meV, and a significantly high excitation binding energy of around 60 meV. It is a transparent, dielectric, and piezoelectric semiconducting oxide [21]. It is observed from previous studies that the photoactivity of bare ZnO is limited due to the instant recombination of photogenerated e--h+ pairs, photocorrosion, and visible light inactiveness [22]. Metal doping enhances the photocatalytic efficiency of ZnO. By introducing impurities between energy levels in the form of a midgap state, doping aids in the reduction of the bandgap. Dopants can alter the size of the grain and its corresponding surface area, as well as cause structural and microstructural flaws [2325]. The doping of tellurium (Te) in zinc oxide (ZnO) can tailor its (ZnO) luminescence properties through the passivation of oxygen defects [2628]. It has been reported that on doping of ZnO, the bond length between Zn and O will change due to stretching vibrations and shifting to lower and higher energy regions. The bond length value between Zn and O will also decrease at high levels of Te doping and increase at low doping concentrations [29]. Te-ZnO photocatalytic efficiency still falls short of expectations. To increase its catalytic efficiency, it can be coupled with a suitable polymeric molecule. g-C3N4 may be a helpful semiconductor for integrating with other semiconductors, notably ZnO, because of its suitable bandgap (2.7 eV) and absorption in the visible spectrum of light [3033]. The nitrogen incorporated in carbon nitride helps to capture more visible light because of its lower electronegativity and higher potential energy compared to oxygen [1]. It has been thoroughly investigated as a practical, stable, affordable, and safe photocatalyst to address the pollution concerns.

Up to now, several reports on the metal doping in ZnO have been demonstrated, which showed an increase in the photocatalytic degradation rate as compared to ZnO [34]. Jamali-Sheini et al. revealed morphological and structural changes due to the Te doping into ZnO. Shanmugam et al. reported the improved photodegradation efficiency of brilliant green (BG) by employing Te-doped ZnO nanosheets. Sher et al. loaded Mo-ZnO on g-C3N4 nanosheets in order to obtain superior photocatalytic efficiency against MB [35]. Ahmad et al. reported that Ag-doped ZnO nanoparticles are efficient photocatalysts to photodegrade methyl orange, rhodamine B, and safranine O in a short time [36]. Equally, the doped metal oxide coupling on g-C3N4 sheets has been stated to demonstrate the improved photocatalytic behavior. Sher et al. and Kuang et al. designed a highly effective g-C3N4/Sn ZnO photocatalyst that showed an improvement in the photocatalytic effectiveness of MB from 35 to 88% [37, 38]. Qamar et al. reported 100% degradation of MB by using g-C3N4/[email protected] under sunlight [39]. Zhang et al. reported 98.97% of MB degradation by using a novel ternary nanocomposite (Ag/g-C3N4/LaFeO3). In order to degrade Rh-B under the influence of visible light, Zhang et al. synthesized g-C3N4/MoS2/grapheme nanocomposite that shows a photodegradation rate nearly 4.8 times superior to that of pristine g-C3N4 [40].

Inspired by the improved photocatalytic performance of metal-doped ZnO and ZnO/S-g-C3N4, we fabricated Te-ZnO and Te-ZnO/S-g-C3N4 via the ecofriendly coprecipitation technique. Thiourea was polycondensed to produce S-g-C3N4. Using a model dye, the photocatalytic characteristics of manufactured catalysts were investigated (MB). The subsequent investigation was divided into two parts. Phase 1 of the investigation looked at the photocatalytic capability of Te-doped zinc oxide NPs (1, 3, 6, 9, 12, and 15 wt%). The greatest dye degradation rate/efficiency was achieved by the 3 percent Te-ZnO NPs (3 Te-ZnO). The 3 percent Te-ZnO NPs were combined with S-g-C3N4 (SCN) concentrations of 20, 40, 60, and 80 weight percent in the second phase to create Te-ZnO/S-g-C3N4 NCs, which further increased the photocatalytic activity. In comparison to other samples, the [email protected] nanocomposite ([email protected]) had the best photocatalytic activity. The synthetic materials might find use in the wastewater treatment industry. Furthermore, nanocomposite uses are not restricted to the purification of wastewater/dye water. They can also be used to fabricate energy storage and conversion devices due to their environmentally pleasant nature [41, 42].

2. Materials and Methods

2.1. Reagents

The zinc chloride (ZnCl2), tellurium (Te), methylene blue, ammonia (NH3), potassium dichromate, polyethylene glycol, and thiourea (CH4N2S) were bought from Merck and employed as such.

2.2. Synthesis of Undoped ZnO and Te-Doped ZnO NPs

In a typical ZnO synthesis experiment, 200 ml of distilled water was used to dissolve 3.38 g of ZnCl2 and 4 ml of polyethylene glycol. NH3 (4 ml) was added dropwise and stirred continuously for two hours, causing white precipitates to develop (a milky solution). The precipitates were collected, repeatedly rinsed in a water/ethanol solution, and then dehydrated in an oven for two hours at roughly 80°C. Then, calcination of the precipitates was carried out at 400°C in a muffle furnace for 3 hours. Finally, precipitates were ground and stored. A series of Te-doped ZnO nanoparticles (1, 3, 6, 9, 12, and 15 wt%) were synthesized by the same process except with the addition of various concentrations of tellurium.

2.3. Fabrication of SCN

For the synthesis of S-g-C3N4 nanosheets, 10 g of the thiourea was taken in a covered crucible and placed in a muffle heating system to carry out the calcination. The temperature was gradually increased at a rate of 5°C per minute until it reached 550°C and kept there for about 4 hours [43]. The obtained yellowish product was permitted to cool at room temperature, ground into a fine powder, and then stored safely.

2.4. Synthesis of Nanocomposites ([email protected])

For the preparation of 20, 40, 60, and 80% nanocomposite series, 3% Te-doped ZnO nanoparticles were hybridized with 0.005, 0.13, 0.26, and 0.39 g of S-g-C3N4, respectively. In a typical synthesis of 20% nanocomposites, 0.13 g of Te powder was added into a 0.1 M solution of ZnCl2 under magnetic stirring. To induce precipitation, 4 mL NH3 was added dropwise to the solution, whereas 4 mL polyethylene glycol was added to avoid agglomeration. This solution is marked as solution A. Subsequently, the required S-g-C3N4 was ultrasonically dispersed into 50 ml water to prepare solution B. After that, the two solutions were combined into a single beaker and swirled for around two hours at room temperature. The precipitates were dehydrated in an oven at 80°C for two hours after filtering and washing with water/ethanol. In a muffle furnace, the precipitates were calcined for roughly three hours at 400°C. The finished product was powdered down to a fine consistency.

3. Results and Discussion

3.1. Bandgap Determination: Optical Property

The UV-visible spectroscopy was used to measure the absorbance of the fabricated samples that were further used to draw the “Tauc plot.” The calculated bandgaps for ZnO NPs and g-C3N4 NSs were 3.13 and 2.32 eV, respectively, as shown in Figures 1(a) and 1(b). These bandgaps obtained were similar to the previously reported work [4446]. These bandgap values indirectly confirmed the successful synthesis of the desired ZnO and SCN. The bandgap of 3Te-ZnO NPs was calculated to be 2.59 eV (Figure 1(c)), indicating that doping reduced the bandgap of ZnO. Tellurium (Te) doping on ZnO can tailor its luminous properties by passivation oxygen defects [2729, 47]. The bandgap of [email protected] was calculated as 2.10 eV (Figure 1(d)), indicating that hybridization with SCN further lowered the bandgap of ZnO. In order to make ZnO a more efficient photocatalyst in visible light, the bandgap narrowing showed that ZnO hybridization reduced the bandgap and shifted its light-absorbing ability toward the visible portion of the light spectrum (red shift) [48].

3.2. Validation of Functional Group by FTIR Spectrum

To confirm the functional groups of the manufactured samples, FTIR spectroscopy was performed to characterize them (Figure 2). The FTIR spectra of ZnO showed the fundamental mode of vibration at around 3492 cm-1 due to O-H stretching [49]. For 3% tellurium-doped ZnO, a peak around 3503 cm-1 was observed that indicated stretching vibrations of the -OH group due to the presence of moisture/water. Weak bands for Te-ZnO NDP in the 611-1518 cm-1 range are a sign that Te4+ ions were successfully incorporated into the ZnO NPs. These peaks obtained are almost similar to the absorption band observed for ZnO NPs, with a slightly higher wavenumber cm-1. SCN’s FTIR spectra showed a distinct absorption band at 808 cm-1, which is connected to the triazine group’s stretching vibration. The existence of C-N heterocycles that have undergone vibrational stretching is indicated by the absorption bands that were detected in the 1228-1616 cm–1 range. The water molecule adsorbed and N-H vibration probability associated with uncondensed amine groups are represented by the characteristic band at 3111 cm-1 [43].

These spectra’s peaks coincide with previously published research. The precise absorption bands at 3476, 2986, 1381, 1036, 885, and 718 cm-1 were seen in the composite spectra like the peaks in 3Te-ZnO, while the peaks at 808, 1336, and 1544 cm-1 resemble the absorption bands found in SCN spectra. It confirms the successful synthesis of [email protected] nanocomposite. An increase in the transmittance percentage was observed by the incorporation of Te-doped NPs into SCN.

3.3. Structural Confirmation by X-Ray Diffractograms

The phase, purity, and lattice characteristics of the produced nanocatalysts (ZnO, SCN, and [email protected]) were characterized by XRD. The XRD pattern of zinc oxide showed peaks at , 34.94°, 36.77°, 48.04°, 57.08°, 63.33°, 66.89°, 68.41°, 69.52°, 77.03°, and 77.45° which correspond to (100), (002), (101), (102), (110), (103), (200), (112), (201), (004), and (202) crystalline planes of ZnO (Figure 3(a)). All these peaks or characteristics of the Miller indices validate the wurtzite structure of ZnO. The result obtained was the same as the previously reported work [29, 36, 50, 51]. Indicating the successful doping of Te into ZnO and the coupling of SCN with Te-ZnO photocatalysts, the X-ray diffraction patterns of 3Te-ZnO and Te-ZnO/40%SCN exhibit a little shift toward the lower angle (Figure 3(b)). This discovery shows that Te4+ has successfully replaced Zn2+ in the ZnO lattice [29, 52].

Figure 3(c) displays the XRD form for S-g-C3N4 containing the two distinct peaks at 13.02° and 27.3° which correspond to the (100) and (002) facets of the crystals. These two peaks are probably due to the interplanar tri-s-triazine unit and the coupled aromatic arrangement, respectively. In the XRD findings of Te-ZnO/40%SCN, the crystal planes (100) and (002) are due to the peaks at 11.67° and 27.97° confirming the presence of S-g-C3N4 while the peaks appearing (32.25°, 34.8°, 36.7°, 48.0°, 57.0°, 63.3°, 66.8°, 68.4°, 69.4°, 72.9°, and 77.3°) correspond to the crystalline planes of tellurium-doped ZnO. The intensity of all these peaks is slightly lower as compared to peaks present in ZnO and tellurium-doped zinc oxide diffractograms, which indicate successful synthesis of Te-doped zinc oxide composite with SCN (Figure 3(d)).

3.4. SEM-EDX Analysis

The morphological structure and corresponding elemental makeup of ZnO, Te-ZnO NPs, and [email protected] NCs are described using SEM-EDX images in Figures 4(a)4(f). ZnO NPs exhibited porous morphology with particle widths in the range of 100–600 nm, but these NPs had an average particle size of ~291 nm (Figure 4(a)). Zn and O peaks are present in the ZnO EDX spectrum, indicating that the NPs are pure (Figure 4(b)). The particles have a rod-like shape with a preferential horizontal orientation. The Te-ZnO NPs are showing a disordered rod-like structure (Figure 4(c)). In EDX spectrum of Te-ZnO, peaks for the Te, Zn, and O elements are seen (Figure 4(d)). The rod structures of these NPs are more stacked together than ZnO NPs forming the agglomeration. This agglomeration is due to the reduction of the combined total surface energy of all the particles. The average width recorded for these nanorods is 300 nm. The [email protected] NCs’ morphology is seen in Figure 4(e). The elemental peaks for sulfur, carbon, nitrogen, zinc, oxygen, and Te can be seen in the EDX spectrum of [email protected] NCs, which is oriented haphazardly on the surface of the SCN sheets in NCs (Figure 4(f)). No additional peak was present, confirming the purity of the synthesized samples.

3.5. XPS Analysis

XPS measurements were used to look into the constituent elements’ chemical states and composition in the [email protected] NCs. The deconvolution Zn 2p spectrum in Figure 5(a) exhibits two distinct Zn2+ peaks at 1021.82 and 1044.76 eV. It is possible to see two satellite peaks in Zn 2p with binding energies of around 1026.14 and 1049.15 eV [53, 54]. In the XPS spectrum of Te 3d (Figure 5(b)), four characteristic peaks of Te 3d3/2 (583.21 eV), Te 3d5/2 (573.21 eV), and TiOx (587.04 and 576.71 eV) eV were linked with metallic Te and silver ions Te4+, respectively; this fits with the literature perfectly [55]. In the deconvolution O 1s spectra of [email protected] NCs, there are two peaks that correspond to C-O and Zn-O, respectively (Figure 5(c)). At binding energies of 531.47 and 530.48 eV, these peaks were seen. In Figure 4(b), high-resolution N 1s spectra show three distinct peaks. N-(C)3 and sp2-hybridized nitrogen (C-N-C) are responsible for the N 1s peak in the CN network at 398.1 and 399.1 eV, respectively. N-H on the powder surface is often blamed for the peak at 400.69 eV. Two distinct peaks can be seen at 283.21 and 287.61 eV in the high-resolution C 1s spectra (see Figure S1a). The first is made up of graphitic carbon that has been adsorbed onto the surface of CN, and the second is made up of sp2-bonded carbon (N-C-N) in the CN network. [email protected] heterostructure S exhibits two peaks in the S 2p XPS spectra (Figure 1Sb) at 160.10 and 160.98 eV. The XPS measurements confirmed the production of the [email protected] nanostructure and the formation of a heterointerface between Te-ZnO and SCN.

3.6. PL and BET Analyses

As shown in Figure 6(a), the photoinduced charge transfer and separation efficiency of [email protected] NCs were investigated using PL at a 325 nm excitation wavelength. The NCs of [email protected] significantly lowered the surface trap-state PL of the ZnO at 565 nm (Figure 6(a)), exhibiting efficient transport and split of photogenerated e--h+ sets [53]. The [email protected] NCs in this study see a decrease in electron-hole recombination, pointing to a fine heterojunction at the Te-ZnO and SCN interface. ZnO>Te-ZnO>[email protected] is the order of the studied samples’ PL intensity’s downward trend. According to the data, [email protected] NC is enough to give increased charge carrier transport efficacy across the [email protected] interface, leading to a very effective charge transfer technique.

For pure ZnO, Te-ZnO, and [email protected] NCs, Figure 6(b) reveals the N2 adsorption-desorption isotherms. It is not surprising that spherical materials like pure ZnO NPs, Te-ZnO, and [email protected] NCs have specific surface areas of up to 5.73, 17.13, and 51.97 m2/g, correspondingly. The surface area of [email protected] NCs is greater than that of pure ZnO and Te-ZnO because various hybridization materials can aid in the formation of additional surface-active sites. The photocatalytic activities of [email protected] NCs are improved by the ability of mesoporous [email protected] NCs to effectively reduce photoinduced e--h+ pair recombination processes.

3.7. Photocatalytic Ability

Under the influence of sunlight, the photocatalytic ability of constructed samples was assessed. First, as shown in Figure 7(a), the photocatalytic activities of produced nanoparticles (ZnO and Te-ZnO) were investigated employing an aqueous MB solution outdoors. The deterioration contours (Figure S2) and percent degradation plots make this abundantly obvious (Figure 7(b)) that increasing the Te+4 doping up to 3 percent wt. boosted the photocatalytic activity of Te-ZnO NPs, which afterwards reduced up to 15 percent wt. Since Te4+ doping reduces Te-ZnO NPs’ bandgap and makes the e/h+ pair easier to form, Te-ZnO NPs have improved photocatalytic ability than ZnFe2O4. It has been shown that doping pure ZnO with different metal ions may change its optical and structural characteristics and raise the metal-doped ZnO’s photocatalytic efficiency [56]. Therefore, Te (3 wt%) is the ideal doping content for Te-ZnO NPs, and while the content of doped Te4+ ions is raised above this level (3 wt%), Te-ZnO NPs’ photocatalytic activity is reduced (Figures 7(a) and 7(b)). After 120 minutes, 3Te-ZnO NPs and ZnO NPs showed the highest (78%) and lowest (51%) photocatalytic activity, respectively. In comparison to other NPs, the 3Te-ZnO NPs had the best photocatalytic efficiency.

The 3Te-ZnO NPs were then homogenised with various concentrations of S-g-C3N4 (as listed in Table 1) to create [email protected] NCs, and their photocatalytic effectiveness toward MB was assessed. Before exposure to sunlight, the NCs were left in the dark to create a symmetry between dye and photocatalysts [35]. Figures 7(a) and 7(b) show that the photocatalysts only absorbed a little amount of MB. The [email protected] NCs showed the highest dye degradation when compared to the other samples after samples were subjected to sunlight. The photocatalytic performance increased as the SCN nanosheet loading increased from 20 to 40%, as shown by the degradation curves (Figure S3) and percentage removal plots (Figures 8(a) and 8(b)), before declining for NCs containing the SCN more than 40%. Better charge separation and more excellent visible light absorption of the [email protected] are primarily responsible for this enhanced degradation outcome. Thus, according to the current research, the ideal S-g-C3N4 concentration was found to be 40% (wt%), and [email protected] NC was able to degrade ≈96% MB in 90 minutes. It is most likely due to the effective junction of S-g-C3N4 with ZnO. However, increasing the S-g-C3N4 concentration beyond 40% may provide extra e-h pair recombination centers, reducing the photocatalytic efficiency. To better understand this justification, additional research is necessary [5759]. The degradation efficiencies of the synthesized ZnO, SCN, and [email protected] (20, 40, 60, and 80 wt%) SCN NCs after 90 minutes of exposure to sunshine are 62%, 67%, 91%, 96%, 88%, and 82%, respectively. The percent photocatalytic removal of MB by comparable NCs is shown in Figure 7(b).

The kinetics of Te-ZnO/(0, 20, 40, 60, and 80 wt%) SCN NCs were realized using the Langmuir-Hinshelwood model, and the corresponding results are shown graphically in Figure S4 [38]. According to the kinetic investigation, the NCs’ degradation of MB in the presence of sunlight is fit to a first-order function. Table 1 lists the rate constant () values of [email protected] (0, 20, 40, 60, and 80 wt%) SCN NCs.

Thus, the highest and lowest estimated “” values were determined to be, respectively, for [email protected] percent SCN NCs (0.0323 min-1) and ZnO (0.0133 min-1). The MB (96%) was decoloured by the [email protected] percent SCN NCs in 90 minutes, and their “” values were 2.4 and 2.3 times higher than those of ZnO and SCN correspondingly. A further increase in concentration may lead to the production of e-h pair sequence centers, which would progressively lower the photocatalytic efficacy of NCs. The observed optimal concentration of SCN for Te-ZnO/SCN NCs is 40%. Additionally, earlier investigations provide support for the current findings [35, 60]. Additional research is necessary to thoroughly investigate this justification. Comparing [email protected] NC’s photocatalytic efficiency to that of other previously reported research, there is a significant difference (Table 2) [6168]. It is possible that the improvement in the NC’s photocatalytic effectiveness over previously reported composites is attributable to the formation of more excellent heterojunctions between S-g-C3N4 and ZnO. Additionally, the Te ions might make it easier for the NC to transfer and separate the photoinduced e/h+ [25, 39, 69]. To evaluate the practicability of the [email protected] NC, it was further employed in the recycling experiment (Figure S5).

3.8. Scavenging Activity

Organic contaminants in water are decomposed primarily by superoxide radicals (O2), hydroxyl radicals (OH), and photogenerated holes (h+) [65]. To test [email protected] NC’s ability to produce active species, scavengers were added to dye solutions containing the photocatalyst. Benzoquinone (BQ) traps superoxide radicals (·O2), ethylenediaminetetraacetic acid- (EDTA-) 2Na catches hydroxyl ions (h+), and isopropanol (IPA) scavenges OH. The efficiency of MB breakdown was reduced by 89% with the addition of benzoquinone. Only 63% and 38%, respectively, of the breakdown rates of MB were reduced by IPA and EDTA-2Na. Figure 9 details how trapping compounds affect dye degradation reactions. Thus, in the photocatalytic dye degradation process, OH and O2 are more reactive than holes (h+).

3.9. Adsorption Activity

The effect of time on chromium adsorption was assessed using various sorbents (ZnO, 3Te-ZnO, SCN, and [email protected]). The synthesized dopant and composite significantly boosted the adsorption capacity. The adsorption capacity showed a consistent uptrend when ZnO defects were covered by the formation of composite ([email protected]), as shown in Figure 10(a). A clear increase in the removal efficiency percentage of chromium ions was being observed by using sorbents (Figure 10(b)). The trend noted was [email protected]>3Te-ZnO>ZnO, which was comparable to that of photocatalysts.

It is well known that too little time must pass between the sorbent and the adsorbate in order for the sorbent to reach its maximum adsorption capacity. A prolonged contact period will be ineffective. Using sorbents and a particular concentration of chromium salt solution, the adsorption time range of 30–1440 min was examined in order to calculate adsorption capacities. Cr(VI) adsorption started off moving along very quickly. Due to the surface pore channels, surface functional groups, and adequate amounts of the sorbent, numerous binding sites can be provided during the initial sorption stage, allowing heavy metal ions to connect to the material’s surface with ease. However, as time goes on, these sites diminish and the electrostatic repulsion between the ions increases, making it more challenging for the adsorption reaction to reach adsorption equilibrium [66]. The synthesized sorbents attained the adsorption equilibrium within 120 to 150 minutes of adsorption (Figure 10(a)).

3.9.1. Adsorption Kinetics

Table 3 includes the experimental equilibrium adsorption capacity for chromium metal ions at a starting concentration of 50 mg L-1, the pseudo-first-order rate constants and , expected equilibrium adsorption capacity , and theoretical equilibrium adsorption capacity . The actual values of were clearly different from the theoretical values of calculated from the pseudo-first-order kinetic model. The theoretical values determined for the pseudo-second-order kinetic model are quite similar but not identical. Additionally, the pseudo-second-order model has a higher correlation value () than the pseudo-first-order model, suggesting that it is more widely used (Figure 11(a)). The initial chromium ion adsorption rate () was calculated using the pseudo-second-order rate equation, and it was found to be 2.51 mg g-1 for ZnO, 6.50 mg g-1 for Te-ZnO, 3.28 mg g-1 for SCN, and 8.82 mg g-1 for [email protected] This indicates that the composite was utilized as the sorbent to produce the higher chromium adsorption rate. This revealed that the total kinetics of the chromium ion adsorption reaction is a pseudo-second-order process (Figure 11(b)), and the use of composite as a sorbent led to the highest values of the correlation coefficients (), equilibrium adsorption capacity , and initial adsorption rate () [66, 67].

4. Mechanism for Catalytic Degradation

According to the schematic sketch, the formation of e-/h+ pairs in the synthesized samples is responsible for the photocatalytic destruction of MB by the manufactured NCs (Figure 12 and Figure S6). ZnO and SCN are both stimulated by sunlight when it strikes [email protected], and their corresponding bands (conduction bands (CB) or valence bands (VB)) form e/h+ couples as a result [68]. Since the conduction band of SCN has a lower potential than the conduction band of ZnO, the photoinduced electrons can readily move from the conduction band of SCN to the conduction band of SCN due to the edge potentials of CB/VB. Additionally, the potential exists for the holes produced in the VB of SCN to move toward ZnO [74]. Te atoms are present in the heterostructure, which lowers the value of Eg while also facilitating the transfer of electrons from SCN to ZnO. Thus, as shown by the EIS data, Te doping has the ability to lower the charge recombination rate by increasing the spacing of photogenerated e-/h+ couples (Figure S7). Reactive oxygen species (O2 and OH) are created when the e-/h+ pairs contact with the water molecules and oxygen on the photocatalyst surface (ROS) [75]. The MB is then degraded by an oxidative process, using up the produced radicals.

5. Antifungal Activity

Further testing was done on the antifungal effectiveness of ZnO, Te-ZnO NPs, SCN, and [email protected] NCs using the agar well diffusion technique and amphotericin B as a reference. The results are presented in broad strokes in Table 4. The highest zone inhibition values of [email protected] for Alternata sp. and Bacillus sp. are 47.4 mm and 41.5 mm, correspondingly, based on the antifungal activity data (Table 4). They quickly penetrate the fungal cell membrane, bind to functional protein groups and phosphorus- and sulfur-containing materials, such as DNA, and ultimately cause fungal cell death owing to the [email protected] NCs with well-defined heterojunction. [email protected] NCs and a clearly defined heterojunction worked together synergistically to boost the antifungal effect on Alternata sp. and Bacillus sp.

6. Conclusion

Conclusively, the purpose of the current work was to synthesize ZnO NPs, Te-ZnO NPs, and [email protected] NCs using a simple coprecipitation method. FTIR, SEM, EDX, and XRD patterns confirm the chemical purity and elemental compositions of synthesized samples. The photocatalytic performance of the produced samples was evaluated against MB (aqueous solution), and it was discovered that 3Te-ZnO NPs and [email protected] NCs had extraordinarily high catalytic efficiencies. The [email protected] was shown to degrade MB using holes, electrons, and ROS in the radical scavenging experiment. The nanocomposites demonstrated exceptional stability with a steady high degree of MB degradation for 6 consecutive catalytic cycles. Based on EIS measurements, it is possible that the creation of the synergistic interaction and fine interfaces between the Te and ZnO will considerably increase the movement and transportation of photoinduced e-/h+ pairs in [email protected] The adsorption capacity of the synthesized samples was examined via Cr ion adsorption experiments. The results and kinetic models indicate that the adsorption of chromium ions was increased by Te doping into ZnO and composite formation ([email protected]). As a result, the [email protected] heterojunction is a suitable candidate and may be used in the photocatalytic elimination of heavy metal (Cr) and mineralization of organic contaminants (MB) to purify water.

Data Availability

On reasonable request, the corresponding author will provide the datasets collected and/or evaluated during the present study.

Conflicts of Interest

No conflict of interest is disclosed by the authors.


The authors thankfully acknowledge the funding provided by the Scientific Research Deanship, King Khalid University, Abha, Kingdom of Saudi Arabia, under the grant number RGP.1/267/43. The researchers would like to acknowledge the Deanship of Scientific Research, Taif University, for funding this work. This research was funded by the Princess Nourah Bint Abdulrahman University Researchers Supporting Project number (PNURSP2023R156), Princess Nourah Bint Abdulrahman University, Riyadh, Saudi Arabia.

Supplementary Materials

In the supplementary, we described (i) material characterizations; (ii) photocatalytic degradation of MB experiments; (iii) adsorption study of heavy metal ions; (iv) the MB degradation contour of ZnO and Te-ZnO NPs; (v) photodegradation of MB by ZnO, SCN, and [email protected] NCs under sunlight irradiation for 90 minutes (degradation contours); (vi) kinetic characteristics of ZnO, SCN, and [email protected] NCs against MB; (vii) 7 consecutive MB photodegradation experiments and the cyclic stability of [email protected]3N4 NCs; (viii) valence-band XPS spectra; and (ix) EIS Nyquist plots. (Supplementary Materials)