Defect-enriched CuO/CeO2 nanostructure: in-depth structural characterization and photocatalytic performance†

Ajit Kumar Dhankaa, Balaram Panib and Nityananda Agasti*a aDepartment of Chemistry, University of Delhi, North Campus, Delhi 110007, India. E-mail: nnagasti@chemistry.du.ac.in bDepartment of Chemistry, Bhaskaracharya College of Applied Sciences, University of Delhi, Dwarka, New Delhi, 110075, India

First published on 15th April 2025

1 Introduction

Pesticides are a group of chemical substances that include insecticides, rodenticides, molluscicides, fungicides, herbicides, and nematicides. They are used to control pests, such as insects, fungi, weeds, rodents, spiders, ticks, mites, birds, slugs, snails, and nematodes, which can significantly harm crop production.1,2 The annual loss of food due to pests is estimated to be 45%.3 Keeping the demand for food in mind, crop productivity enhancement requires the application of pesticides. Approximately 3 million tons of pesticides are applied each year to agricultural fields globally, which is a value 15 to 20 times higher than those for the last three decades.4 Alternatively, the widespread use of pesticides in agriculture raises critical concerns owing to their persistence and potential toxicity to the ecosystem and human health.5-7 Pesticide residues detected in vegetables, fruits, agricultural lands, and even in drinking water cause various diseases.8 Pesticide contamination poses a higher risk of developing cancers in organs, including the kidneys, lungs, and stomach.9,10

Commonly applied pesticides in agriculture include isoproturon, glyphosate, acephate, propoxur, metaldehyde, diazinon, chlorpyrifos, dichlorodiphenyltrichloroethane (DDT), and malathion. Among these, “N,N-dimethyl-N′-[4-(1-methylethyl)phenyl]urea” or “3-(4-isopropylphenyl)-1,1-dimethylurea”, which is commercially known as isoproturon (IPU) (C12H18N2O), belongs to the phenylurea family,11 and it is widely used to prevent the growth of unwanted plants or broad-leaved weeds in cotton, wheat, cereal, and sugarcane fields and citrus, and asparagus fruit farms.12 Although the herbicide IPU helps in farming, its toxicity causes adverse effects on the ecosystem.13 The Lethal Dose 50 (LD50) toxicity (the dose that results in death of 50% of a test group of animals, usually mice) of isoproturon for rats is 1826 mg kg−1 when ingested orally, and more than 2000 mg kg−1 when it encounters the skin.14,15 IPU also affects the photosystem II (PSII) in plants by inhibiting electron transport and consequently promoting oxidative stress.16 Due to its poor biodegradation, low volatility, low tendency to sorb to soil and high solubility in water (65 mg L−1 at 22 °C), it persists in water.17,18 In water, the half-life cycle of IPU is 1210, 1560 and 540 days at pH 5, 7 and 9, respectively.19 Reupert et al. have detected the concentration of IPU to be in the range of 0.1 to 0.125 μg L−1 in surface water and 0.05 to 0.1 μg L−1 in groundwater in Germany. Sometimes, the level of IPU in drinking water has been investigated to be more than 0.1 μg L−1.20,21 Another study reports that approximately one-third of the surface water is contaminated with IPU in the concentration range of 0.01 to 0.06 μg L−1 in Wielkopolska Province in Poland.21 IPU residues have been found worldwide in different environments at concentrations that often exceed the allowed limit of 0.1 μg L−1.22,23 Isoproturon has been included in the list of the 33 most potential water contaminants.24 It has been reported that IPU can harm the human immune system and disrupt the thyroid gland or thyroid hormones.25,26 It is a deadly carcinogen for human health. Therefore, it is imperative to develop a suitable approach for the degradation of IPU in water.

Among various methods,27-34 photocatalytic degradation, owing to low cost, stability and high efficiency, has received much attention for the decomposition of residual pesticides in wastewater.35,36 Additionally, the use of light irradiation for the catalytic decomposition of pollutants offers a sustainable solution to combat water contamination.37 Besides light, the role of the catalyst material is also important for the efficient degradation of contaminants in water. As photocatalysts, metal oxides are effective due to their tunable band gap, which is sensitive to light for producing electron-hole pairs responsible for the chemical conversion of molecules. Among various metal oxides38-40 CeO2 has been found to be more effective owing to its excellent redox catalytic property facilitated by the reversible interconversion of Ce4+ and Ce3+.41 Additionally, CeO2, with a band gap of approximately 3.3 eV, can absorb light in the near UV region, and to a lesser extent, in the visible region, making it a promising photocatalyst, especially at the nanoscale.42 The band gap of CeO2 nanoparticles can be modified to regulate its catalytic properties. The flexible interconversion of oxidation states between Ce4+ and Ce3+ generates defects in CeO2, thus modifying its catalytic properties. The most favorable defect is oxygen vacancies, Ce4+-OV-Ce3+ (OV - oxygen vacancy), generated in the CeO2 lattice structure. Thus, the catalytic property of CeO2 can be regulated by modulating its oxygen vacancies. The addition of metal or metal oxide nanoparticles into CeO2 is an effective strategy to enhance oxygen vacancies due to strong synergistic metal-CeO2 interactions. This interaction enhances interfacial redox reactions and promotes the formation of oxygen vacancies.43 Though there are reports on the increase in CeO2 defects caused by the addition of metals and metal oxide nanoparticles,44-46 there is scope to study defect-induced photocatalytic activity of ceria-based materials. Moreover, studies on the photocatalytic degradation of isoproturon by ceria-based materials and in-depth mechanistic studies along with degradation patterns are limited.

Therefore, considering the effectiveness of the defect-mediated catalytic property of CeO2 and the need for efficient photocatalytic degradation of pesticides in water, the present study reports the preparation of CuO/CeO2 and evaluation of its photocatalytic performance for the degradation of isoproturon. This study provides a detailed insight into the structural characterization of defects in CeO2, including the estimation of oxygen vacancies based on Raman and XPS studies. Herein, we introduce CuO into CeO2 for generating oxygen vacancies (CeO2−x) and found that CuO/CeO2 showed markedly enhanced photocatalytic activity. Structural characterization confirms the generation of oxygen vacancies and interfacial charge transfer between CuO and CeO2. The photocatalytic efficiency of CuO/CeO2 nanocomposites was evaluated by the degradation of isoproturon (IPU) in an aqueous medium under UV light exposure, representing a model system for pesticide removal from wastewater. The degradation process was monitored using UV-vis absorption spectroscopy. Compared to pristine CeO2, the CuO/CeO2 exhibited superior photocatalytic performance at room temperature. To determine the active species responsible for the degradation, trapping experiments were performed. A detailed investigation into the reaction mechanism was conducted, leading to the proposal of a possible degradation pathway for IPU. The results suggest that the interaction between CuO and CeO2 generates oxygen vacancies, which facilitate the dissociation of water molecules into ˙OH radicals and promote the reduction of O2 to ˙O2− species. These reactive species, ˙OH and ˙O2−, significantly enhance the photocatalytic degradation of IPU in water.

2 Experimental section

2.1 Materials

All chemicals utilized were of analytical grade and used directly without further purification. A reported method47 was followed to prepare the CuO/CeO2 nanocomposite. Cerium nitrate hexahydrate (99%) (Ce(NO3)3·6H2O), sodium hydroxide (98%) (NaOH) and isoproturon (C12H18N2O) were purchased from CDH India; copper nitrate (Cu(NO3)2) was purchased from Merck; ethanol (C2H5OH), methanol (CH3OH), ethylenediaminetetraacetic acid (EDTA), p-benzoquinone (pBQ) and tert-butyl alcohol (t-BuOH) were purchased from Sigma-Aldrich India.

2.2 Preparation of CuO/CeO2

The CuO/CeO2 nanocomposites were synthesized using cerium nitrate (Ce(NO3)3·6H2O) and copper nitrate (Cu(NO3)2) via a solvothermal method, as shown in Scheme 1.48 In a typical preparation route for CuO/CeO2 nanocomposites with a 1:10 wt. ratio, 0.1 g of Cu(NO3)2 and 1.0 g of Ce(NO3)3·6H2O were dissolved in 50 mL of methanol solution. 0.25 g of sodium hydroxide (NaOH) was added to the solution while stirring vigorously for 30 minutes. The resulting mixture was transferred to a Teflon-lined stainless-steel autoclave and heated at 180 °C for a duration of 18 hours in an oven. The autoclave was allowed to cool gradually to room temperature. The solid precipitate formed was collected and subsequently washed with ethanol through centrifugation at 3000 rpm for 10 minutes, and the washing was repeated 3-4 times. Finally, the precipitate was dried at 80 °C for 4 hours and calcined at 250 °C for 2 hours to obtain the CuO/CeO2 nanocomposites. For comparison, CeO2 nanoparticles were prepared using the same method, except for the addition of Cu(NO3)2. CuO nanoparticles were synthesized using a method similar to that of CeO2 nanoparticles, with the only modification being the precursor. All the remaining steps of the synthesis followed the same procedure as used for CeO2 nanoparticles.

2.3 Sample characterizations

The structural and morphological features of the synthesized nanocomposites were analyzed using multiple characterization techniques. The powder X-ray diffraction (PXRD) for CuO/CeO2, CeO2 and CuO was performed. The X-ray diffraction (XRD) patterns were recorded using a Rigaku Miniflex X-ray diffractometer equipped with a Cu Kα anode (λ = 0.1542 nm) operated at 40 kV and 15 mA. Data were collected in the 2θ range from 20° to 80°, with a step size of 0.02° per step and a scan rate of 3° per minute. The obtained diffraction patterns were matched with the reference pattern of the JCPDS database. The FTIR spectra of the samples were recorded using a Nicolet™ iS50 Fourier-transform infrared (FTIR) spectrometer in the wavelength range of 500-4000 cm−1 with KBr pellets at a resolution of 4 cm−1 and in the attenuated total reflection (ATR) mode. To understand the optical behavior of the materials, the UV-visible spectra of the powder sample dispersed in water were obtained by a Shimadzu UV-1800 spectrophotometer (Shimadzu, Japan). The sample was first placed on the sample holder, and its absorbance was measured in the wavelength range of 200 to 800 nm with deuterium and tungsten-halogen lamps as light sources. The UV-vis diffuse reflectance spectroscopic (DRS) measurements were carried out using an Agilent Cary 5000 in the wavelength range from 200 nm to 800 nm at a resolution of 1 nm, and the samples were used in the powder form. The Raman spectroscopic analysis was performed using an Invia Reflex Renishaw microscope with a 532 nm, 50 mW diode laser in the wave number range from 100 cm−1 to 900 cm1, and the samples analyzed were in powder form. A field emission scanning electron microscope (FESEM) with Oxford-EDX system IE 250 X Max 80 (FEI Quanta 200 F SEM) was used to study the morphology of CuO/CeO2 and CeO2. The elemental composition of the samples was analyzed using energy-dispersive X-ray spectroscopy (EDX). Moreover, to gain a thorough insight into the packing pattern of CuO/CeO2 nanocomposites, high-resolution transmission electron microscopy (HRTEM) images were collected using a transmission electron microscope TECNAI G20 HR-TEM 200 kV. Thermogravimetric analysis (TGA) was also performed on HITACHI STA7300 up to 600 °C in a nitrogen atmosphere with a controlled gas flow of 150 bar. The samples were analyzed in the alumina crucible at a heating rate of 10 °C min−1 to determine their thermal stability. The surface area and pore size of the synthesized materials were evaluated using an Autosorb-iQ XR analyzer (Quantachrome Instruments) through N2 adsorption/desorption isotherms. Before the analysis, the samples underwent degassing under vacuum (∼1 × 10−5 bar) at 150 °C for 10 hours. The adsorption/desorption isotherm measurements were then conducted in a liquid nitrogen bath at 77 K. X-ray photoelectron spectroscopy (XPS), using a Kratos Axis Supra Plus XPS equipped with a monochromatic Al Kα X-ray source (1486.6 eV), was employed to study the surface elemental oxidation state and composition of samples. The high-resolution mass spectrometric (HRMS) technique G6530AA (LC-HRMS-Q-TOF) with the ESI and APCI source was used to identify the possible degradation intermediates and pathways. The photoluminescence (PL) study was performed at room temperature on Horiba Yvon PTI QuantaMaster (8450-11) spectrophotometer using an excitation source of 375 nm nano-LED. The charge carrier lifetimes are ascertained using time-resolved photoluminescence (TRPL) measurements (in micro and milliseconds) employing a 980 nm laser and xenon lamp as the source in modulated mode.

2.4 Photocatalytic degradation of isoproturon under UV light irradiation

To investigate the photocatalytic degradation of isoproturon (IPU), the as-synthesized CuO/CeO2 nanocomposites (10 mg) were dispersed in a 100 mL aqueous solution of IPU (10 μg L−1) and the content was kept under a custom-built solar reactor, illuminated by a 125 W high-pressure mercury lamp (Hg) (Osram, India) emitting UV light (λ < 400 nm), for 2 hours with stirring at room temperature. At every 20 minutes interval, 5 mL aliquots of the suspension were withdrawn and transferred into vials, then centrifuged at 8500 rpm for 10 minutes to precipitate the catalyst particles. Following a typical procedure,49 the supernatant was carefully collected and transferred into a quartz cuvette to measure the UV-vis absorption spectra. The IPU solution, along with the catalyst particles, was reintroduced into the reaction vessel after the absorbance measurement. At specific time intervals, the absorbance was measured to monitor the decomposition rates of isoproturon. To assess its reusability, the catalyst was separated from the reaction mixture via centrifugation after the reaction, washed with deionized water and then dried at 80 °C for three hours. The dried catalyst was then reintroduced into a fresh isoproturon solution, and the photocatalytic procedure was repeated to evaluate its efficiency. Additionally, control experiments were conducted using CuO and CeO2 individually under identical conditions to compare their photocatalytic performances.

To assess the photocatalytic performance of the CuO/CeO2 catalyst, the UV-vis absorption spectra were recorded in the range of 200-325 nm both in the presence and absence of the catalyst under UV light irradiation and in the dark. Blank experiments were performed with an aqueous solution of IPU (i) under the dark condition (without UV light irradiation) (see Fig. S9d-g ESI†) and (ii) in the presence of UV light irradiation (see Fig. S9a-c ESI†). The blank experiment in the absence of UV light irradiation shows negligible degradation of IPU, suggesting the important role of UV light irradiation. Further, the negligible degradation of IPU in the presence of UV light irradiation shows the need for a catalyst. Further, to investigate the role of CuO in the degradation of isoproturon, experiments were conducted with CuO/CeO2, CuO and pristine CeO2 catalysts under UV light irradiation at identical experimental conditions.

2.5 Free radical and hole scavenging experiments

To investigate the mechanism and the principal active species responsible for the photocatalytic degradation of IPU in water under UV light irradiation using CuO/CeO2 as a catalyst, experiments were conducted with the addition of scavengers. The scavengers quench the reaction between the reactive species and the IPU molecule. To understand the role of scavengers, the photocatalytic experiments were performed with and without scavengers under identical reaction conditions. Here, tert-butyl alcohol (t-BuOH) was added to the reaction system as a scavenger for ˙OH, EDTA for photogenerated holes (h+), AgNO3 for photogenerated electrons (e−) and p-benzoquinone (pBQ) for superoxide anion radicals (˙O2−). The effects of various scavengers on the photocatalytic degradation of isoproturon are illustrated in Fig. 5f and S10 ESI.† Based on the result, photocatalytic degradation in the presence of scavengers follows the order EDTA (56%) < AgNO3 (61%) < t-BuOH (87%) < pBQ (91%) < no scavenger (95%). The results showed that the addition of EDTA and AgNO3 significantly inhibited the degradation of isoproturon, suggesting that h+ and e− are the active species playing an important role in the photocatalytic degradation of isoproturon.

3 Result and discussion

3.1 Structure, morphology and elemental analysis

The optical properties were studied to understand the formation of CuO/CeO2 nanocomposites using UV-vis spectroscopy. The band at 303 nm corresponds to CeO2 nanoparticles; however, in the spectra of CuO/CeO2 nanocomposites, the bands at 268 and 299 nm correspond to CuO and CeO2, respectively49,50 (Fig. 1a). The band at 268 nm corresponding to the surface plasmon absorption of CuO suggests the existence of CuO in the CuO/CeO2 nanocomposites.51 The band at 299 nm is due to CeO2, which suffers a blue shift compared to pristine CeO2 nanoparticles52 (Fig. S1 ESI†). This can be attributed to the decrease in the band gap in CuO/CeO253 on account of the fact that incorporating CuO onto CeO2 introduces impurity energy levels between the valence and conduction bands, consequently narrowing the band gap in CuO/CeO2. The reduction in band gap was also verified from the UV-vis diffuse reflectance spectra (DRS) (Fig. S2 ESI†) using the Kubelka-Munk (K-M) function. The plot of the Kubelka-Munk (K-M) function, αhν = A(hν − Eg)n/2 (1)against the energy of the light gives the band gap energy (Eg), where α, A, h, ν, Eg correspond to the absorption coefficient, a constant, Planck's constant, light frequency, and band gap energy, respectively.54 The band gap energy was estimated to be 3.2 eV for CuO/CeO2 and 3.3 eV for CeO2 (Fig. 1b).

The optical properties suggest the incorporation of CuO on the surface of CeO2. Furthermore, the bands in the FTIR spectra of CuO/CeO2 nanocomposites at 698 cm−1 and 745 cm−1, corresponding to Ce-O and Cu-O, respectively, suggest the formation of the composites (Fig. S3 ESI†).55 The formation of the composites is also inferred by assessing the thermal stability of CuO/CeO2. Thermogravimetric analysis (TGA) was performed for both the CuO/CeO2 nanocomposite and pure CeO2 nanoparticles (Fig. S8 ESI†). CuO/CeO2 exhibited higher thermal stability than pristine CeO2, suggesting the formation of the composite material.

To understand the structural characteristics of CuO, CeO2 and CuO/CeO2 nanocomposites, powder X-ray diffraction (XRD) analysis was carried out. In the PXRD patterns of CuO presented in Fig. S4b ESI,† the prominent diffraction peaks observed at 2θ 29.2°, 31.5°, 35.5°, 38.7°, 42.4°, 45.4°, 48.4°, 55.5°, 58.2°, 61.5°, 66.2°, 68.2°,72.3° and 75.3° correspond to the (115), (303), (−111), (111), (200), (200), (−202), (426), (020), (202), (−113), (−310), (311) and (282) crystallographic planes matching with the monoclinic structure of CuO, and two planes at 45.4° and 72.3° correspond to the (200) and (311) planes matching the Cu2O.56 These peaks confirm the formation of the CuO nanoparticle structure, which is consistent with JCPDS card no. 01-1117.57 In the XRD pattern (Fig. 1c), the peaks at 2θ; 28.4°, 32.9°, 47.5°, 56.3°, 59.0°, 69.3°, 76.7°, and 78.8° correspond to the (111), (200), (220), (311), (222), (400), (331), and (420) crystallographic planes, respectively. The XRD pattern of pristine CeO2 nanoparticles matches with the cubic fluorite structure of CeO2 (JCPDS file number 34-0394).49 Besides, the peaks corresponding to CuO appear at 2θ; 36.7°, 42.5°, 61.5° and 73.5° (JCPDS file no. 78-0428),58 suggesting the formation of CuO/CeO2 composites. The diffraction peaks of CuO/CeO2 shift to lower 2θ angles compared to pristine CeO2, with the most prominent shift occurring in the highly intense peak of CuO/CeO2 associated with the (111) diffraction plane at a 2θ of 28.7° (Fig. S4a ESI†). This shift in diffraction peaks suggests the anchoring of CuO on the CeO2 surface. Additionally, there is a decrease in intensity and broadening of the peaks, indicating a reduction in crystallite size. The crystalline size can be estimated using the Scherrer equation,59

D = Kλ/βcosθ (2)where D is the average crystallite size (nm), K is a dimensionless shape factor typically set to 0.98 for spherical crystals, λ = 1.54 Å, θ is the Bragg angle (half of the 2θ angle where the peak occurs), corresponding to the most intense or primary diffraction peak of CeO2, observed at 2θ 28.4° and β is the full-width at half-maximum (FWHM) of the primary diffraction peak. The average crystallite size was determined to be 6.6 nm for CeO2 in CuO/CeO2 nanocomposites and 7.7 nm for pristine CeO2. Moreover, the decrease in the intensity of diffraction peaks can be ascribed to the formation of defects on the surface of ceria. Khan et al. reported that the shift in diffraction peaks towards a lower angle corresponds to an increase in oxygen vacancies in CeO2.60 In the present case, the shifting of diffraction peaks to lower angles suggests an increase in oxygen vacancies in CuO/CeO2.

To evaluate the formation of defects in CuO/CeO2 nanocomposites, the Raman spectra of pristine CeO2 and CuO/CeO2 nanocomposites were recorded in the range of 280-850 cm−1 (Fig. 1d). In the spectra, a prominent and intense peak at 465 cm−1 corresponds to the F2g symmetric stretching mode of the Ce-O bond, a characteristic of the fluorite crystal structure of CeO2.61 The F2g peak for CuO/CeO2 appears at 464 cm−1, with a downshift compared to the pristine CeO2 (Fig. S5a ESI†). Additionally, a band appearing at 300 cm−1 corresponds to the tenorite phase of copper oxide (CuO), which confirms the presence of Cu in the form of CuO.62 The downshift in the F2g peak for CuO/CeO2 can be ascribed to the formation of oxygen vacancies due to the introduction of CuO63,64 (Fig. S5a ESI†). Besides, there is a band at 615 cm−1, which is also accounted for the defect-induced (D) mode representing oxygen vacancies.65,66 The absence of this band in pristine CeO2 confirms the role of the interfacial interaction between CuO and CeO2, providing information on the oxygen vacancies in CuO/CeO2. Moreover, oxygen vacancies can also be related to the FWHM of the F2g peak. An increase in the FWHM of the F2g peak indicates an increase in the oxygen vacancies in CuO/CeO2,67 which are quantified from the crystallite size of CeO2. The crystallite size of CeO2 is calculated from the F2g peak using the relation

Γ (cm−1) = 5 + 51.8/d (nm) (3)where Γ is the half-width at half maximum (HWHM). The crystallite size, d in nm,68,69 was determined to be 11.51 nm for pristine CeO2 and 12.95 nm for CuO/CeO2, which are consistent with the values obtained from XRD and HRTEM analyses. The d values obtained from Raman spectra were used to calculate the concentration of oxygen vacancies using the following formula: (4) N = 3/4πL3 (5)L represents the correlation length (i.e., the average distance between two lattice defects), r is the radius of the CeO2 units (0.31 nm) and N is the oxygen vacancy concentration in cm−3.70 The concentration of oxygen vacancies was determined to be 8.43 × 1020 cm−3 for CuO/CeO2, which is higher than that of pristine CeO2 (7.45 × 1020 cm−3). Moreover, the ratio of the integrated area of the D peak to the F2g peak (denoted as ID/IF2g) reflects the relative concentration of oxygen vacancies on the surface of CuO/CeO2 and CeO2. Compared to pristine CeO2, the ID/IF2g ratio for the CuO/CeO2 nanocomposite exhibits a significant increase. This increase can be attributed to the strong interactions between the CuO and CeO2. As shown in Fig. S5b (ESI†), the ID/IF2g ratio is higher in CuO/CeO2 (0.123) than in CeO2 (0.006). The presence of CuO in CuO/CeO2 can also be supported by the increase in intensity of the F2g peak due to the strong optical absorption associated with the surface-enhanced Raman scattering effect (SERS).71,72

Photoluminescence (PL) spectroscopy is a sensitive technique used to analyze the defects, oxygen vacancies and effectiveness of trapping charge carriers in semiconductor materials. Therefore, photoluminescence was used to investigate the role of oxygen vacancies in separating photogenerated electron-hole pairs in the CuO/CeO2 nanocomposites. PL spectra (Fig. 2a) show the UV emission band at 394 nm, which is attributed to the electronic transition from the O2p to Ce4f in CeO2.73 The decrease in emission observed for CuO/CeO2 nanocomposites compared to pristine CeO2 suggests that the anchoring of CuO could quench the fluorescence from the CeO2 nanoparticles. The quenching in emission also indicates the effective separation of charge carriers, resulting from the suppression of their recombination. A lower PL intensity is attributed to a low rate of the electron-hole recombination process, consequently increasing the lifetime of photogenerated charge carriers, a favorable factor for the enhancement of photocatalytic performance. Thus, the quenching in PL intensity suggests that the oxygen vacancies on the surface, as well as at the interface of CuO and CeO2, act as sites to trap the charge carriers, leading to suppression in their recombination, which enhances the photocatalytic performance of the CuO/CeO2 nanocomposites.74

The presence of surface oxygen vacancies in CeO2 and the oxidation states of Ce and Cu were confirmed by the XPS of CuO/CeO2. A comparison of the XPS spectra of pristine CeO2 and that of CuO/CeO2 evaluated the impact of the CuO incorporation on CeO2. The XPS survey spectra (Fig. 2b) confirm the elemental composition of the material, showing the presence of Ce, O, and Cu. The characteristic binding energy peaks were observed in the regions: 877-920 eV, 527-535 eV and 925-960 eV for Ce 3d, O 1s and Cu 2p, respectively.75,76 The high-resolution data were charge corrected to the reference C 1s signal at 284.4 eV. To understand the oxidation states of Ce, the high-resolution scans in the binding energy range of 877-920 eV were deconvoluted and fitted.

The XPS spectra for Ce 3d can be deconvoluted into eight distinct peaks at the following binding energies (eV): 882.3, 885.2, 888.1, 898.3, 900.9, 903.3, 905.7, and 916.6, as shown in Fig. 2c. Among them, the peaks appearing at 882.3 eV and 900.9 eV are due to Ce3+ 3d5/2 and Ce3+ 3d3/2, respectively, whereas the peaks at 898.3 eV and 916.6 eV correspond to Ce4+ 3d3/2 and Ce4+ 3d3/2, respectively.

This confirms that both Ce3+ and Ce4+ coexist in CeO2. The existence of Ce3+ and Ce4+ states reveals the presence of O-vacancies in the CeO2 crystals because of their interconversion from the Ce3+ and Ce4+ states.77,78 Compared to pristine CeO2, the intensity of the Ce4+ peaks is reduced and that of Ce3+ is increased in CuO/CeO2 (Fig. S6 ESI†). This suggests an increase in the amount of Ce3+ due to the addition of CuO into CeO2, and consequently, more oxygen vacancies are generated in CuO/CeO2. The Ce3+ content can be calculated as the ratio of the sum of the integrated areas of all peaks corresponding to Ce3+ to the total area of all the peaks corresponding to Ce 3d in the XPS spectra (Table S1 ESI†).79 In CuO/CeO2, the atom concentration of surface Ce3+ is estimated to be 31.2%, which is higher than that of pristine CeO2 (24.2%). Higher Ce3+ corresponds to an increase in oxygen vacancies in CuO/CeO2. The presence of CuO can also be confirmed from the Cu 2p spectrum shown in Fig. 2d. The two peaks located at the binding energies of 931.5 eV and 951.7 eV could be ascribed to (Cu 2p3/2) and (Cu 2p1/2), respectively. The satellite peak appearing at 938.3 eV is a typical characteristic of Cu2+ species. Further, in the high-resolution XPS spectra of O 1s, distinct peaks were observed at 528.4 eV, 530.1 eV, and 532.7 eV, corresponding to different oxygen species. The peak at 528.4 eV (OL) is associated with lattice oxygen (Ce4+-O2−), while the peak at 530.1 eV (OV) is indicative of oxygen vacancies (Ce3+-O2−). Additionally, the peak at 532.7 eV (OC) corresponds to chemisorbed surface oxygen and hydroxyl groups (-OH).80 The peak at 530.1 eV is attributed to the oxygen vacancies.61

Additionally, oxygen vacancies in CuO/CeO2 and pristine CeO2 can also be assessed by calculating the OV/OL ratio81 derived from the areas under the peaks in the O 1s spectra (Fig. S7 and Table S2 ESI†). The analysis shows that CuO/CeO2 exhibits a higher OV/OL ratio, indicating higher oxygen vacancies compared to pristine CeO2. This is also supported by the greater intensity of the OV peak in CuO/CeO2 (Fig. S7 ESI†) relative to pristine CeO2. The results agree with the previous studies.82

3.2 Morphological and elemental analysis

The morphology of the synthesized CuO/CeO2 nanocomposites was investigated using FESEM. Fig. 3a represents the FESEM images of CuO/CeO2 nanocomposites, revealing spherical morphology. The EDX elemental mapping shown in Fig. 3b demonstrates a uniform distribution of cerium (Ce), copper (Cu), and oxygen (O), confirming the successful synthesis of the CuO/CeO2 nanocomposites. The EDX spectra with atomic and weight percentages of the elements indicate the presence of 84.47% Ce, 4.69% Cu, and 10.84% O, as shown in Fig. 3c.

To ascertain the microstructure of CuO/CeO2 nanocomposites, high-resolution transmission electron microscopy (HRTEM) was conducted (Fig. 3d). The HRTEM image confirms the presence of CuO and CeO2 in the CuO/CeO2 nanocomposites. The lattice fringes of 0.231 nm and 0.310 nm, corresponding to the (111) planes of CuO and CeO2, respectively (Fig. 3e), clearly identify the presence of CuO and CeO2. The distinct circles made up of bright spots in the selected area electron diffraction (SAED) pattern (Fig. 3f) of CuO/CeO2 indicate the polycrystallinity of CuO/CeO2 nanocomposites. The interplanar spacings (d values) from a large to a small ring in the SAED pattern for CuO/CeO2 nanocomposites are 0.326, 0.280, 0.195, 0.167, 0.126, and 0.114 nm, which correspond to the crystal planes (111), (200), (111), (311), (220), and (420), respectively. These values closely match with the X-ray diffraction (XRD) pattern of the CuO/CeO2 nanocomposites. The HRTEM images show the CuO nanoparticles of size 4-7 nm deposited on the surface of CeO2 nanoparticles, with a size of 6-9 nm, which agrees with the crystallite size calculated from XRD. The HRTEM image (Fig. 3e) of the CuO/CeO2 nanocomposites reveals that CuO nanoparticles are in close contact with CeO2. The interaction between CuO and CeO2 increases the oxygen vacancies owing to interfacial charge transfer, which plays an important role in improving the photocatalytic performance of CuO/CeO2.

To assess the surface area of the CuO/CeO2 nanocomposite, N2 adsorption-desorption isotherm measurement was conducted (Fig. 4). The Brunauer-Emmett-Teller (BET) specific surface area of CuO/CeO2 was found to be 59.85 m2 g−1, which is higher than that of pristine CeO2 (36.01 m2 g−1). The total pore volume and the average pore diameter of CuO/CeO2 were 0.210 cm3 g−1 and 5.40 nm, respectively, whereas those of pristine CeO2 were 0.153 cm3 g−1 and 7.56 nm, respectively. The change in surface properties accounts for the dispersion of CuO on CeO2. The increased surface area of CuO/CeO2 nanocomposites is favorable for more dispersion and high photocatalytic degradation of IPU.83

3.3 Catalytic degradation of isoproturon

Isoproturon (IPU) is primarily effective against gramineous (grass-like) weeds. It is typically applied to the soil and can be absorbed by plants, mainly through their roots. Once absorbed, it inhibits weed growth by interfering with the photosynthesis process in plants. Isoproturon exhibits absorption bands at 203 nm and 240 nm, with a lower absorbance shoulder at 275 nm, in the UV-visible spectra84,85 (Fig. 5a). Therefore, the degradation of isoproturon can be monitored through its UV-vis absorption spectra.

A 100 mL aqueous solution of IPU (at a concentration of 10 mg L−1) was treated with 10 mg of the catalyst and exposed to UV light. The progress of the degradation was monitored by the changes in the UV-visible absorption intensities of bands at the wavelengths of 240 and 275 nm with time. With CuO/CeO2, there was a significant decrease in the intensity and complete disappearance of the bands at 240 and 275 nm within an interval of 120 minutes of UV light irradiation, indicating the complete degradation of isoproturon (Fig. 5b). However, with CeO2 and CuO, the band does not disappear completely even after 120 minutes (Fig. S9b and c ESI†). According to the C/C0 plot, the degradation efficiency of CuO/CeO2 was approximately 95% (Fig. 5c). The degradation efficiency was calculated using the formula;

Degradation (%) = (C0 − Ct)/C0 × 100% (6)Here, C0 is the initial concentration, and Ct is the concentration of isoproturon at time t.86

To quantitatively assess the