[Cu-Ag 2 ]O–C 3 N 4 nanoframeworks for efficient photodegradation of wastewaters

Materials and preparation method

Urea was used to prepare g-C₃N₄ powder. Cu(NO₃)₂ and AgNO₃ were used to load the Ag₂O and CuO nanoparticles on the surface of the supports. Ethanol, tetramethylammonium hydroxide (TMAOH), isopropanol, HNO₃, and all the other chemicals were purchased from Merck Co. and utilized without further purification. Acid Blue 92 (AB92) azo dye powder (as a typical textile wastewater component) was provided by Chaprang Co., Tabriz, Iran.

A crucible containing urea, well-covered by Al foil, was transferred to an oven, and the temperature was increased to 500°C at a rate of 10°C min⁻¹. After 180 min, the crucible was cooled to room temperature, and the content was finely crushed, washed repeatedly with 0.1 M HNO₃ solution, and kept at 60°C for 24 h. The product (50 mg) was poured into a beaker containing 100 mL of isopropanol, and the vessel was ultrasonicated for 1 hr. The suspension was then centrifuged, and the precipitate was dried at 60°C for 6 h. The product, C₃N₄ nanosheets was denoted as NS throughout.

AgNO₃ solution was slowly added to a solution containing TMAOH and oleic acid, and the mixture was stirred for 1 h. A specific amount of the as-prepared NS powder was poured into the vessel and stirred magnetically for 1 h. The precipitate was filtered off and heated at 60°C for 24 h. The product was denoted as Ag₂O-NS. CuO-NS was prepared by the same method, with copper nitrate used as the metallic source.

Photocatalytic tests

The experiments were conducted in a double-layer reactor made of Pyrex which was kept at room temperature. The visible light source was a 125 W OSRAM lamp which was surrounded by a reflective Al jacket to concentrate the beam on the reaction medium. The suspension comprising specific concentrations of the AB92 solution and catalyst powder was stirred magnetically for 15 min and then the lamp was turned on. The total concentration of AB92 (AB92 was provided by Chaprang Co., Tabriz, Iran, as a gift.) at different time intervals was measured using a UV spectrophotometer set at λ_max of the azo dye (574 nm).

Characterization of the samples

Powder X-ray diffraction analysis

The X-ray diffraction (XRD) patterns of the nanostructures are shown in Figure 1. The dominant diffraction peak at 2θ = 27.7°, which can be observed in all the samples, is assigned to the (002) diffraction planes of g-C₃N₄ and a small diffraction peak at approximately 13° is indexed to the in-plane of tris-triazine units (in-plane of tris-triazine units means in- plane structural packing motif of tristriazine units). ²⁴ As can be seen, the latter peak was surprisingly intensified by decorating the surfaces with CuO nanoparticles. This sharp peak in CuO-NS corresponds to the CuO crystal planes. Moreover, the characteristic peak assigned to the cubic structure of Ag₂O in the XRD pattern of the sample appeared around 2θ = 33° (JCPDS file no. 41-1104). From the patterns, the (002) diffraction peak of g-C₃N₄ is sharper in the NS compared to bulk g-C₃N₄.

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Figure 1.

The XRD patterns of the photocatalysts.

Fourier transform–infrared spectroscopy

The Fourier transform–infrared (FTIR) spectra of the samples are shown in Figure 2. The broadened peak above 3400 cm⁻¹ is due to water molecules adsorbed on the surface. The sharp peak at 808 cm⁻¹ originates from the triazine ring system. ²⁵ The peak at 1636 cm⁻¹ is attributable to C═N stretching vibration modes. Moreover, the other bands appearing at 1240, 1320, and 1403 cm⁻¹ could be related to the aromatic C–N stretching vibrations. ²⁶

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Figure 2.

FTIR spectra of the samples.

Scanning electron microscopy micrographs

To characterize the morphology of the nanostructures, scanning electron microscopy (SEM) analysis was performed, and the images are shown in Figure 3. From the results, the micrographs of NS display a lamellar structure with the thicknesses of the sheets below 50 nm (a-1 and a-2). After the introduction of Ag₂O or CuO nanoparticles, the presence of new species deposited on the surfaces leading to the formation of heterojunction photocatalysts is observable (b and c). The guest nanoparticles are clear in the SEM images of CuO-NS and Ag₂O-NS. Forming this kind of heterojunction can readily increase the half-life of the photogenerated electron–hole pairs by their being transferred between p (CuO or Ag₂O)-n type (C₃N₄) semiconductors which enhances the quantum yield effectively.

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Figure 3.

SEM images of the prepared photocatalysts: (a-1 and a-2) NS, (b) Ag₂O-NS, and (c) CuO-NS.

Diffuse reflectance spectra

To find the effect of the oxide nanoparticles on the band gap of the C₃N₄ photocatalyst, diffuse reflectance spectroscopy (DRS) analysis was performed, and the results are presented in Figure 4. From the recorded spectra, the absorption step is the same for both bulk C₃N₄ and NS, but it shifts to higher wavelengths when the support is decorated with CuO or Ag₂O nanoparticles. The results convinced us that the CuO junction more effectively influenced the band gap compared with the Ag₂O one. According to the DRS results, the energy cut-off for the former case is located at a higher wavelength, which implies its lower band gap.

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Figure 4.

DRS of the samples.

Specific surface area (Brunauer–Emmett–Teller) analysis

As an effective tool for determining the specific surface area and porosity, Brunauer–Emmett–Teller (BET) analysis was conducted. Figure 5 shows a typical hysteresis loop related to the N₂ adsorption–desorption curve for NS, which indicates that the support is expected to be porous. Moreover, the results revealed that deposition of the oxide nanoparticles on the surface decreases the specific surface area smoothly and also influences the morphology. The BET surface areas were 37.9, 38.4, and 31.2 m² g⁻¹ for g-C₃N₄, NS, and Ag₂O-NS, respectively. Furthermore, the total pore volumes were evaluated to be 0.14, 0.16, and 0.17 cm³ g⁻¹ for Ag₂O-NS, NS, and g-C₃N₄, respectively. The pore size distributions of the prepared samples were determined by the Barrett–Joyner–Halenda method which indicated that the maximum distribution for the pores was around 1.6 nm, and there was no significant difference between the results obtained for the products.

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Figure 5.

Nitrogen adsorption–desorption isotherm obtained for the pure NS sample.

Photocatalytic remediation of wastewater

The removal of AB92 from wastewater was studied over the prepared nanostructures under different operational conditions, and the results are shown in Figure 6.

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Figure 6.

Results for AB92 removal: (a) photodegradation over CuO-NS, (b) photodegradation over Ag₂O-NS, (c) photodegradation over NS, (d) photolysis experiment, and (e) dark test over NS.

From the results, the NS powder showed significant photocatalytic activity comparable to Ag₂O-NS sample, which implicates the effect of the sonication process in isopropanol during its preparation. This step increases the availability of the active sites responsible for promoting the photocatalysis. The results of the BET analysis confirmed that there is no significant difference between the specific surface areas of these two samples, which convinced us that the higher activity of the NSs cannot be attributed to this parameter. Furthermore, CuO-NS, as the results of DRS analysis implied its lower band gap, was expected to be more active than Ag₂O-NS. From Figure 6, the removal efficiency became maximum over the former case in a considerably shorter reaction time compared to the other photocatalysts. Ag₂O and CuO are both p-type, while carbon nitride is an n-type semiconductor, and this p-n heterojunction affected the photocatalytic properties of g-C₃N₄ profoundly. Evidently, CuO is a better choice than Ag₂O to achieve the maximum removal efficiency. In fact, the potentials in which the valence and conduction bands of CuO are located and their positions relative to those of g-C₃N₄, provide better possibilities for charge transfer between two junctions.^27,28 This is shown schematically in Figure 7. C₃N₄ is an n-type semiconductor and the most likely species responsible for producing the destroyer radicals (like HO₂^•, O₂^¯•, and OH^•), and promoting the degradation process are the photogenerated electrons in the conduction band. Charge transfer between two bands near to each other (in terms of their potentials) is preferred rather than the other probable route since this transfer proceeds so fast (route 1). However, if the electron should proceed via route 2, then its energy content changes meaningfully, which makes this possibility more difficult.

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Figure 7.

Charge transfer process between the Ag₂O, C₃N₄, and CuO junctions during illumination.

We also found the optimum values for the experimental parameters, including catalyst dosage, AB92 concentration, and pH. As shown in Figure 8(a), increasing the NS powder dosage from 5 to 20 mg enhances the photodegradation efficiency considerably while there is no significant gain in changing from 20 to 50 mg.

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Figure 8.

Effect of (a) catalyst dosage, (b) dye concentration, and (c) pH on the photodegradation efficiency of AB92 over NS.

The availability of active sites is strongly affected by increasing the dosage of catalyst particles in the medium in the range of 5–20 mg, as clearly represented in the results obtained. However, we observed that the reaction medium became opaque on adding the catalyst powder in the range of 20–50 mg, thereby reducing the penetration of the light photons to the photocatalyst surface, which controls the photoreaction rate and efficiency. From Figure 8(b), the optimum value for AB92 concentration was evaluated to be 10 ppm. At higher concentrations, the AB92 molecules induce an inner-filter effect. The acidity of the medium was also optimized by following the reaction efficiency at pH values of 4, 6, 8, and 10 (Figure 8(c)). According to the results, the maximum rate and efficiency were achieved at pH 8. Under mild basic conditions, the hydroxyl anions react with photogenerated positive holes and produce OH^•, which are the most abundant destroyer radicals in an aquatic environment. Meanwhile, higher concentrations of OH¯, inasmuch as AB92 is a negative azo dye (including sulfonate groups in its chemical structure), interfere with the adsorption of the azo dye molecules on the catalyst surface and reduce their removal efficiency. To reach a clearer understanding of the structural effects, we treated AB92 solely in basic (pH of 8 and 11) and acidic (pH of 2 and 4) solutions. From Figure 9, AB92 showed significant red and blue shifts under basic and acidic conditions, respectively. In addition to having red shift behavior, we observed a new characteristic peak between 350 and 400 nm, which implies the development of a chemical reaction in the basic medium, while under acidic conditions we just had a decrease in the absorption at λ_max.

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Figure 9.

The UV spectra of AB92 solutions at different acidities of the medium (blue: neutral, red: pH = 11, gray: pH = 2, green: pH = 4, light gray: pH = 8).

The most likely event in an acidic medium seems to be protonating the sulfonate groups, which is without effect on the azo chromophore. On the other hand, a high concentration of OH¯ could deprotonate two distinct positions of the structure: OH in the naphthalene ring and NH of the aniline group; the former case is preferred due to the higher electronegativity of oxygen. Thus, O¯ can attach to the N═N group and produce a new species, as schematically represented in Figure 10.

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Figure 10.

Effect of strong basic conditions on the structure of AB92.

This kind of interaction can weaken the strength of the azo bond and makes it much more vulnerable to attack. Accordingly, the efficiency of photocatalytic removal reached its highest point at pH 8. ²⁹ Finally, the degradation of a real wastewater provided by Chaprang Co. was studied over the best photocatalyst and under optimized conditions. This sample contained different organic waste compounds from textile activities rather than AB92 and could be an appropriate choice for evaluating the promising photocatalytic capacity of the prepared nanostructures. The results for this experiment are shown in Figure 11, which indicates an effective decrease at all wavelengths after 2 h of irradiation time.

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Figure 11.

Photocatalytic treatment of the real waste sample under the optimized operational conditions.