Synthesis of Fe-Modified g-C3N4 Nanorod Bunches for the Efficient Photocatalytic Degradation of Oxytetracycline

Antibiotic residues have been found to have potentially harmful effects on ecological and human health. Carbon nitride-based photocatalysts have widely focused on antibiotic photocatalytic degradation. Herein, we prepared Fe-modified g-C3N4 nanorod bunches (FCNBs) using chemical vapor co-deposition. Specifically, through the process of calcination, a blend of urea and chlorophyllin sodium iron salt underwent an intriguing transformation, resulting in the integration of Fe into the framework of the g-C3N4 nanorod cluster. The resulting photocatalyst exhibited remarkable stability and superior dispersibility. The prepared FCNBs had a unique structure, which was beneficial for increasing light absorption. Furthermore, the Fe species formed a chemical coordination with the g-C3N4 matrix, thereby altering the electronic structure of the matrix. This modification facilitated charge transfer, prolonged the carrier lifetime, and enhanced light absorption, all of which significantly increased the photocatalytic activity. The oxytetracycline degradation efficiency of FCNBs was 82.5%, and they demonstrated outstanding stability in cycle trials. This work introduces a promising photocatalyst for the degradation of antibiotics.


Introduction
Oxytetracycline (OTC), an antibiotic with strong antibacterial action, has been extensively utilized in aquaculture, animal husbandry, and human and animal medicine in recent years [1][2][3][4].Excessive OTC is discharged into wastewater or soil, causing harm to ecosystems and human health [5].The ubiquity of OTC in water severely pollutes the water supply and induces microbial resistance.More and more attention has been paid to adopting effective methods to eliminate OTC in water.Currently, a multitude of methods, including physical adsorption, chemical oxidation, biodegradation, and photocatalytic degradation, have been employed for the elimination of OTC [6][7][8].Among them, the photocatalytic degradation of OTC has attracted wide attention because of its green and sustainable characteristics.In principle, the photocatalytic degradation of oxytetracycline involves the selection of appropriate semiconductors and solar energy as the input to promote a chemical reaction through four main steps, as follows: 1.The catalyst needs to absorb photons whose energy is greater than or equal to the semiconductor band gap to achieve the necessary conditions for photogenerated electron and hole separation.2. Electrons are excited from the valence band (VB) of the semiconductor to the conduction band (CB).3. Optically excited charge carriers migrate to the surface without futile recombination.4. The accumulated photoexcited electrons and holes participate in the redox reaction on the surface to realize the degradation of oxytetracycline [2].The key to photocatalytic degradation technology is the rational design of a photocatalyst to improve the photocatalytic degradation ability.
As an N-type semiconductor, graphitic carbon nitride (g-C 3 N 4 ) has led to great progress in boosting the photocatalytic degradation of oxytetracycline, estrone hormone, and dye and water splitting due to its visible-light response and excellent physicochemical properties [2,[9][10][11][12].However, there is still a need for improvement regarding its flaws, including the short visible-light absorption range, quick photogenerated carrier recombination, and low conductivity [10].Doping, heterostructure construction, dye sensitization, and morphology control have been used to optimize g-C 3 N 4 to enhance its photocatalytic performance [13][14][15][16].Significantly, morphology regulation has been regarded as a simple and effective modification strategy.Jun et al. developed mesoporous g-C 3 N 4 , which enhances its ability to absorb light across a wider spectrum and extends the duration of the photoexcited charge carriers [17].Similarly, Dou et al. prepared g-C 3 N 4 nanosheets, significantly enhancing its photocatalytic degradation ability [18].However, further alterations to its electronic structure are necessary in order to augment the optical, conductive, and other physical characteristics of g-C 3 N 4 .
The electronic structures of g-C 3 N 4 can be successfully improved, and its photocatalytic degradation performance can be enhanced, by adding the highly conductive metal Fe [19].Furthermore, lone pairs of electron, which can combine with Fe to generate Fe-N, are abundant in g-C 3 N 4 [20].Xu et al. utilized a one-step calcination technique for the production of Fe-doped g-C 3 N 4 and this synthesis exhibited notable efficacy in the degradation of TC under visible-light-driven photodegradation reactions [21].To enhance photocatalytic activity by encouraging the separation of electron-hole pairs, Sudrajat et al. incorporated Fe into g-C 3 N 4 [22].Van et al. used a simple and economical heat-stirring technique to create Fe-doped g-C 3 N 4 high-performance photocatalysts [23].However, these methods lead to the formation of Fe-particle-modified g-C 3 N 4 , which reduces the dispersion of Fe.
Herein, urea and a combination of chlorophyll sodium iron salt were utilized as precursors to create the uniformly distributed, Fe-modified, g-C 3 N 4 nanorod bunches (FCNBs), which were then used to break down OTC under irradiation with visible light.The outcomes demonstrated the great stability and superior photocatalytic degradation performance of FCNBs, indicating their potential utility in the removal of organic pollutants such as OTC.

Preparation of FCNBs and g-C 3 N 4
Firstly, the filter paper made from cellulose was cut to a specific size and placed inside a nitrogen muffle furnace.Cellulose-based carbon paper was produced by gradually heating it at a rate of 3 • C/min in a nitrogen environment until it reached 700 • C, where it was held for 1 h.Afterwards, a mixture of 50 g urea and 0.5 g chlorophyll sodium iron salt was dissolved in a combination of 100 mL ethanol and deionized water at a temperature of 95 • C, resulting in the formation of a dark green solution.This solution was then heated under agitation for 2 h to obtain an evenly distributed solid mixture.The cellulose-based carbon paper was positioned on top of an alumina crucible, with its bottom covered by 10 g of the prepared mixture.Subsequently, the crucible underwent heating in a nitrogen atmosphere at a rate of 3 • C/min until reaching up to 550 • C for 2 h.As a result, the iron-modified g-C 3 N 4 material adhered to the surface of the carbon paper, which is referred to as FCNBs.The FCNB on the carbon paper surface was collected into the sample tube by brushing.g-C 3 N 4 was obtained by heating 20 g urea up to 550 • C at an identical heating rate under nitrogen atmosphere for 2 h.

Characterizations
The samples underwent analyses via the utilization of a Hitachi S-4800 scanning electron microscope (SEM) and a Japan Electronics Co., Ltd.(Amagasaki, Japan) JEM-2100 transmission electron microscope (TEM) to characterize their surface morphology and internal structure.Furthermore, functional groups of the composites were assessed through testing, analyzed using a Perkin-Elmer Spectrum One Fourier transform infrared spectrometer (FT-IR) that was equipped to operate within a range of 500-4000 cm −1 .Measurements for X-ray diffraction (XRD) patterns were taken using a Bruker D8 Advance X-ray diffractometer, scanning within a 2θ range of 5-80 • at a rate of 5 • /min.The chemical state of Fe in the FCNBs, as well as the surface element composition and corresponding content distribution, were determined by VG ESCALAB 250Xi (Thermo Fisher Scientific, Waltham, MA, USA) X-ray photoelectron spectroscopy (XPS).To measure the composite material's light absorption range, a Perkin-Elmer Lambda 950 UV-Vis spectrophotometer was utilized for analyses within a measuring range of 200-800 nm.Fluorescence intensity was measured using an FLS 920 fluorescence spectrophotometer (PL) to assess changes in the recombination efficiency of electron-hole pairs before and after modification, with an excitation wavelength set at 360 nm and measurement range from 300 to 700 nm.The Fe content in the samples was quantified using an Agilent 720 inductively coupled plasma optical emission spectrometer (ICP-OES).

Photoelectrochemical Measurements
Utilizing the CHI 760E electrochemical workstation, photoelectrochemical measurements were conducted.The working electrode was fabricated through the attachment of a sample to indium tin oxide glass.A platinum electrode served as the opposing pole, while the reference electrode, Ag/AgCl, was utilized.The utilized electrolyte was a 0.5 M Na 2 SO 4 solution, with a 300 W xenon lamp serving as the illumination source.Analyses of the transient photocurrent response and electrochemical impedance spectroscopy were subsequently performed.

The Performance Measure of Catalysts
To assess how well the prepared samples degrade OTC under visible light, we dispersed 30 mg of the catalyst into 100 mL of a 10 mg/L OTC aqueous solution.To simulate visible light (λ > 420 nm), we used a 300 W xenon lamp (PLS-SXE300UV, Beijing Perfectlight Technology Co., Ltd., Beijing, China).Before irradiation, we stirred the mixture in darkness for 30 min to achieve an adsorption-desorption equilibrium.Throughout the irradiation process, we collected samples from the reaction solution at specific time intervals and then filtered them to remove the catalyst.We determined the OTC concentration by measuring its absorbance at 354 nm using a TU-1901 spectrophotometer.Additionally, we collected, washed, and dried samples for cycling experiments to evaluate the catalyst's stability.

Characterization of Catalysts
FCNBs were prepared through chemical vapor co-deposition (Scheme 1).SEM and TEM were used to examine the shape and structure of FCNBs.As depicted in Figure 1 and Figure S1, FCNBs exhibit a radial bundle structure, which can be further confirmed by TEM. Figure 2 illustrates the rod-like structural unit of FCNBs, which has a diameter of around 350 nm.Through the corresponding EDS (Figure 2c-e), it can be judged that its constituent elements contain C, N, and Fe.The g-C 3 N 4 boasts a high concentration of N atoms, encompassing six lone pairs of electrons.This unique molecular structure proves to be highly conducive to the bonding of iron, thereby introducing Fe into g-C 3 N 4 .The iron content of FCNBs was measured using ICP-OES and found to be 0.6 wt.% (Table S1), and it presented a uniform distribution across the entire surface of the g-C 3 N 4 .
Materials 2024, 17, x FOR PEER REVIEW 5 of 13 Scheme 1. Flow chart for the synthesis of FCNBs.
Using XRD and FTIR spectroscopy, the materials' structural and chemical characteristics were examined.Figure 3a displays the FTIR spectra of FCNBs and g-C3N4.The vibration peaks corresponding to the triazine unit vibration, stretching vibration of CN, and stretching vibration of N-H in free amino groups were located at 810 cm −1 , 1200-1700 cm −1 , and 3000-3400 cm −1 , respectively [24].g-C3N4 and FCNBs showed similar characteristic peaks, indicating that trace amounts of Fe did not significantly alter the basic structure of g-C3N4.The XRD patterns depicted in Figure 3b reveal the spectra of g-C3N4 and FCNB.Both catalysts show two distinct peaks at around 13.20° and 27.50°, associated with the stacking structure of the conjugated aromatic system and the in-plane structure of the triss-triazine unit, respectively [25].Compared with g-C3N4, the diffraction peaks of FCNBs are generally weaker, which can be attributed to the interaction between the Fe and CN layers.In addition, no distinct diffraction peaks corresponding to elemental iron or iron oxide were observed, suggesting that the iron content may be very low or present in a coordinated form.350 nm.Through the corresponding EDS (Figure 2c-e), it can be judged that its constituent elements contain C, N, and Fe.The g-C3N4 boasts a high concentration of N atoms, encompassing six lone pairs of electrons.This unique molecular structure proves to be highly conducive to the bonding of iron, thereby introducing Fe into g-C3N4.The iron content of FCNBs was measured using ICP-OES and found to be 0.6 wt.% (Table S1), and it presented a uniform distribution across the entire surface of the g-C3N4.Using XRD and FTIR spectroscopy, the materials' structural and chemical characteristics were examined.Figure 3a displays the FTIR spectra of FCNBs and g-C 3 N 4 .The vibration peaks corresponding to the triazine unit vibration, stretching vibration of CN, and stretching vibration of N-H in free amino groups were located at 810 cm −1 , 1200-1700 cm −1 , and 3000-3400 cm −1 , respectively [24].g-C 3 N 4 and FCNBs showed similar characteristic peaks, indicating that trace amounts of Fe did not significantly alter the basic structure of g-C 3 N 4 .The XRD patterns depicted in Figure 3b reveal the spectra of g-C 3 N 4 and FCNB.Both catalysts show two distinct peaks at around 13.20 • and 27.50 • , associated with the stacking structure of the conjugated aromatic system and the in-plane structure of the tris-s-triazine unit, respectively [25].Compared with g-C 3 N 4 , the diffraction peaks of FCNBs are generally weaker, which can be attributed to the interaction between the Fe and CN layers.In addition, no distinct diffraction peaks corresponding to elemental iron or iron oxide were observed, suggesting that the iron content may be very low or present in a coordinated form.Using XRD and FTIR spectroscopy, the materials' structural and chemical characteristics were examined.Figure 3a displays the FTIR spectra of FCNBs and g-C3N4.The vibration peaks corresponding to the triazine unit vibration, stretching vibration of CN, and stretching vibration of N-H in free amino groups were located at 810 cm −1 , 1200-1700 cm −1 , and 3000-3400 cm −1 , respectively [24].g-C3N4 and FCNBs showed similar characteristic peaks, indicating that trace amounts of Fe did not significantly alter the basic structure of g-C3N4.The XRD patterns depicted in Figure 3b reveal the spectra of g-C3N4 and FCNB.Both catalysts show two distinct peaks at around 13.20° and 27.50°, associated with the stacking structure of the conjugated aromatic system and the in-plane structure of the triss-triazine unit, respectively [25].Compared with g-C3N4, the diffraction peaks of FCNBs are generally weaker, which can be attributed to the interaction between the Fe and CN layers.In addition, no distinct diffraction peaks corresponding to elemental iron or iron oxide were observed, suggesting that the iron content may be very low or present in a coordinated form.The XPS analysis of FCNBs revealed a diverse surface elemental composition, as depicted in Figure 4a.Elements including C, N, O, and Fe were identified.The presence of O may be attributed to the adsorption of O 2 or H 2 O on the composite surface [26].Despite the low doping content of iron, distinct peaks corresponding to the iron species were not evident.The Fe 2p high-resolution spectrum (Figure 4b) exhibited peaks at 725.44 and 710.63 eV, indicative of the 2p 1/2 and 2p 3/2 states of Fe 2+ , respectively.Similarly, peaks at 730.01 and 717.05 eV corresponded to the 2p 1/2 and 2p 3/2 states of Fe 3+ [23].This observation confirms the coexistence of Fe 2+ and Fe 3+ in FCNBs.Figure 4c shows the high-resolution C 1s spectrum, which showed three peaks at 284.67, 286.11, and 288.05 eV.The peak at 284.67 eV represents amorphous carbon, while the peak at 286.11 eV indicates the presence of C-O bonds.The peak at 288.05 eV was associated with sp 2 -hybridised carbon in the N-C=N structure of the triazine ring [27].In addition, Figure 4d shows the high-resolution N 1s spectrum with three distinct peaks.The peaks at 398.5, 399.9, and 400.92 eV correspond to sp 2 -bonded N atoms (C-N=C), tertiary nitrogen atoms in N-(C) 3 groups, and N-H groups, respectively [28].The tabulated form of elemental analysis from XPS is shown in Table S2 to confirm the element ratio of FCNB.We also conducted nitrogen adsorption and desorption tests on FCNB and g-C 3 N 4 .As shown in Table S3, the specific surface area of FCNB is slightly smaller than that of g-C 3 N 4 , which can be attributed to the introduction of Fe nanoparticles, leading to the destruction of the layered structure of g-C 3 N 4 [26].
Materials 2024, 17, x FOR PEER REVIEW 6 of 13 The XPS analysis of FCNBs revealed a diverse surface elemental composition, as depicted in Figure 4a.Elements including C, N, O, and Fe were identified.The presence of O may be attributed to the adsorption of O2 or H2O on the composite surface [26].Despite the low doping content of iron, distinct peaks corresponding to the iron species were not evident.The Fe 2p high-resolution spectrum (Figure 4b) exhibited peaks at 725.44 and 710.63 eV, indicative of the 2p1/2 and 2p3/2 states of Fe 2+ , respectively.Similarly, peaks at 730.01 and 717.05 eV corresponded to the 2p1/2 and 2p3/2 states of Fe 3+ [23].This observation confirms the coexistence of Fe 2+ and Fe 3+ in FCNBs.Figure 4c shows the high-resolution C 1s spectrum, which showed three peaks at 284.67, 286.11, and 288.05 eV.The peak at 284.67 eV represents amorphous carbon, while the peak at 286.11 eV indicates the presence of C-O bonds.The peak at 288.05 eV was associated with sp 2 -hybridised carbon in the N-C=N structure of the triazine ring [27].In addition, Figure 4d shows the high-resolution N 1s spectrum with three distinct peaks.The peaks at 398.5, 399.9, and 400.92 eV correspond to sp 2 -bonded N atoms (C-N=C), tertiary nitrogen atoms in N-(C)3 groups, and N-H groups, respectively [28].The tabulated form of elemental analysis from XPS is shown in Table S2 to confirm the element ratio of FCNB.We also conducted nitrogen adsorption and desorption tests on FCNB and g-C3N4.As shown in Table S3, the specific surface area of FCNB is slightly smaller than that of g-C3N4, which can be attributed to the introduction of Fe nanoparticles, leading to the destruction of the layered structure of g-C3N4 [26].Figure 5a depicts the UV-Vis absorption spectra of g-C3N4 and FCNBs.Although g-C3N4 absorbs light across the ultraviolet and visible-light ranges, its absorption in the visible region is relatively weak.In contrast, FCNBs exhibited significantly improved absorption properties in the visible-light range due to the incorporation of Fe.Furthermore, there is a noticeable shift towards longer wavelengths in the absorption edge of FCNBs compared to that of g-C3N4, indicating that the addition of Fe can greatly enhance the capacity to absorb visible light.The improvement in the efficiency of solar energy utilization and Figure 5a depicts the UV-Vis absorption spectra of g-C 3 N 4 and FCNBs.Although g-C 3 N 4 absorbs light across the ultraviolet and visible-light ranges, its absorption in the visible region is relatively weak.In contrast, FCNBs exhibited significantly improved absorption properties in the visible-light range due to the incorporation of Fe.Furthermore, there is a noticeable shift towards longer wavelengths in the absorption edge of FCNBs compared to that of g-C 3 N 4 , indicating that the addition of Fe can greatly enhance the capacity to absorb visible light.The improvement in the efficiency of solar energy utilization and boosting of the visible-light catalytic activity of the catalyst are the benefits of this enhancement.The evaluation of the photocatalytic performance of the photocatalysts was primarily determined by their efficiency in separating photogenerated electron-hole pairs.Therefore, we carried out photoluminescence (PL) testing.Figure 5b shows that g-C 3 N 4 has a significant fluorescence peak at 450 nm, indicating a high rate of electron-hole pair recombinations after irradiation.In contrast, the fluorescence intensity of FCNBs notably decreased, suggesting that the incorporation of Fe can effectively suppress carrier recombination and enhance photocatalytic activity.
boosting of the visible-light catalytic activity of the catalyst are the benefits of this enhancement.The evaluation of the photocatalytic performance of the photocatalysts was primarily determined by their efficiency in separating photogenerated electron-hole pairs.Therefore, we carried out photoluminescence (PL) testing.Figure 5b shows that g-C3N4 has a significant fluorescence peak at 450 nm, indicating a high rate of electron-hole pair recombinations after irradiation.In contrast, the fluorescence intensity of FCNBs notably decreased, suggesting that the incorporation of Fe can effectively suppress carrier recombination and enhance photocatalytic activity.We carried out an in-depth study of the light-induced electron transfer process and enhanced photocatalytic activity using electrochemical impedance spectroscopy (EIS) and photocurrent testing.The objective of this study is to explore the charge transfer resistance and efficiency in photogenerated electron-hole pairs' separation.A comparison of the Nyquist plots of g-C3N4 and FCNBs in Figure 6a reveals that the arc radius of FCNBs is significantly smaller, the charge transfer resistance is reduced, and the electron transfer rate is accelerated.In addition, Figure 6b illustrates that the photocurrent intensity of FCNBs surpasses that of g-C3N4, indicating a substantial enhancement in the separation of the photogenerated electron-hole pairs.We carried out an in-depth study of the light-induced electron transfer process and enhanced photocatalytic activity using electrochemical impedance spectroscopy (EIS) and photocurrent testing.The objective of this study is to explore the charge transfer resistance and efficiency in photogenerated electron-hole pairs' separation.A comparison of the Nyquist plots of g-C 3 N 4 and FCNBs in Figure 6a reveals that the arc radius of FCNBs is significantly smaller, the charge transfer resistance is reduced, and the electron transfer rate is accelerated.In addition, Figure 6b illustrates that the photocurrent intensity of FCNBs surpasses that of g-C 3 N 4 , indicating a substantial enhancement in the separation of the photogenerated electron-hole pairs.
hancement.The evaluation of the photocatalytic performance of the photocatalysts was primarily determined by their efficiency in separating photogenerated electron-hole pairs.Therefore, we carried out photoluminescence (PL) testing.Figure 5b shows that g-C3N4 has a significant fluorescence peak at 450 nm, indicating a high rate of electron-hole pair recombinations after irradiation.In contrast, the fluorescence intensity of FCNBs notably decreased, suggesting that the incorporation of Fe can effectively suppress carrier recombination and enhance photocatalytic activity.We carried out an in-depth study of the light-induced electron transfer process and enhanced photocatalytic activity using electrochemical impedance spectroscopy (EIS) and photocurrent testing.The objective of this study is to explore the charge transfer resistance and efficiency in photogenerated electron-hole pairs' separation.A comparison of the Nyquist plots of g-C3N4 and FCNBs in Figure 6a reveals that the arc radius of FCNBs is significantly smaller, the charge transfer resistance is reduced, and the electron transfer rate is accelerated.In addition, Figure 6b illustrates that the photocurrent intensity of FCNBs surpasses that of g-C3N4, indicating a substantial enhancement in the separation of the photogenerated electron-hole pairs.

Photocatalytic Activity Measurement
The study investigated the degradation of OTC in the presence of visible light using the prepared materials.Figure 7a illustrates the OTC photodegradation process for differ-ent photocatalyst systems.Prior to visible-light irradiation (300 W xenon lamp), a dark reaction was conducted for 30 min to ensure catalyst adsorption saturation.The figure clearly demonstrates that, in the absence of any photocatalyst, OTC photodegradation is minimal, indicating the high stability of OTC under visible light.After 60 min of visiblelight irradiation, g-C 3 N 4 only degraded 37% of the OTC.In contrast, FCNBs achieved a photocatalytic efficiency of 82.5% within the same timeframe, which is superior to the similarly reported g-C 3 N 4 catalyst at present (Table S4).This indicates that the introduction of iron notably augmented the photocatalytic properties of the composites.We increased the amount of FCNB from 30 to 50 mg to conduct a photodegradation experiment, and compared the effects of different amounts of the catalyst on the photodegradation performance.As shown in S2a, the OTC degradation efficiency of 50 mg FCNB within 60 min is 84.9%, indicating that the degradation efficiency increases with an increase in the amount of catalyst.In addition, we carried out an in-depth study of the prepared samples to analyze the reaction kinetic properties of the photocatalytic degradation of OTC and applied Equation ( 1) to calculate the apparent rate constant (k) [29]: where k is the apparent rate constant, t is the light irradiation time, C is the concentration at irradiation time t, and C 0 is the concentration at adsorption equilibrium.

Photocatalytic Mechanism
To delve deeper into the photocatalytic degradation mechanism, active radical trapping experiments were performed by using hydroquinone (BQ) and isopropanol (IPA) as a trap for the superoxide anion radical (•O 2− ) and hydroxyl radical (•OH), and disodium ethylenediamine tetraacetate (EDTA-2Na) as a hole-trapping agent [30].We conducted an The plot of ln(C 0 /C) versus time (t) demonstrates linearity in the kinetic analysis (Figure 7b), affirming that its degradation process adheres to first-order kinetics.The k for g-C 3 N 4 is calculated as 0.0055 min −1 .In contrast, the k value for FCNBs was determined to be 0.0205 min −1 , which is 3.7 times greater than that of g-C 3 N 4 , underscoring the significantly enhanced degradation rate of the composite photocatalyst.In practical applications, the reusability and stability of composite materials are paramount.Consequently, cycling tests for OTC photocatalytic degradation were conducted on FCNBs to assess their reusability.In addition, we tested the photocatalytic degradation of OTC under the full solar spectrum with other conditions remaining unchanged.The results show that the photodegradation efficiency of the sample is 85.0%, as shown in Figure S2b.As depicted in Figure 7c, after four cycles, the degradation efficiency of the catalyst exhibited no notable decline, highlighting the excellent stability of FCNBs during photocatalytic degradation.We carried out SEM and XRD tests on the materials after the degradation test, as shown in Figure S3a,b.The considerable photodegradation efficiency of OTC makes FCNB an excellent material for the photocatalytic degradation of OTC.

Photocatalytic Mechanism
To delve deeper into the photocatalytic degradation mechanism, active radical trapping experiments were performed by using hydroquinone (BQ) and isopropanol (IPA) as a trap for the superoxide anion radical (•O 2− ) and hydroxyl radical (•OH), and disodium ethylenediamine tetraacetate (EDTA-2Na) as a hole-trapping agent [30].We conducted an in-depth study on the role of these actives in the photocatalytic degradation process.As seen in Figure 7d, the introduction of IPA had no discernible impact on the degradation rate of OTC, suggesting that •OH had an insignificant effect on the degradation of OTC.However, the addition of BQ (10 mM) and EDTA-2Na (10 mM) led to a significant decrease in the degradation rate of OTC, highlighting the key role of •O 2− and h + in the degradation process.
Furthermore, the Tauc diagram (Figure S4a) of g-C 3 N 4 and FCNBs was obtained through UV-vis spectrum calculations, revealing band gaps of 2.92 eV and 2.48 eV for g-C 3 N 4 and FCNBs, respectively.By combining this with the Mott-Schottky curves (Figure S4b,c), the band structure of g-C 3 N 4 and FCNBs can be deduced (Figure S4d).The conduction band potential (E CB ) of FCNBs is −0.55 V vs. NHE, which is lower than the O 2 /•O 2− potential (−0.33 V vs. NHE).This indicates that the photoelectrons on the CB of FCNBs are conducive to the reduction in •O 2− .The valence band potential (E VB ) of FCNBs is 1.93 V vs. NHE, which is lower than that of H 2 O/•OH (2.69 V vs. NHE).It can be inferred that holes (h + ) cannot oxidize OH − to •OH but directly oxidize OTC instead, based on these findings.This suggests that the influence of •OH on photocatalytic performance is negligible, consistent with the results of the capture experiment [31].
To explain how FCNBs degrade OTC, a tenable photocatalytic process is put forth (Figure 8).Under the given light conditions, electrons in the g-C 3 N 4 material move to the conduction band through the valence band and then migrate to the iron state, improving the separation efficiency of electron-hole pairs.The h + remaining in the valence band can oxidize contaminants.Subsequently, the photogenerated electrons may be captured by oxygen molecules to generate a potent oxidizing species •O 2 − , which decomposes antibiotics into smaller molecular species.Additionally, the incorporation of iron considerably boosts the absorption of visible light and enhances solar utilization.In conclusion, the improved photocatalytic degradation performance of FCNBs can be attributed to the increased light harvesting and higher electron-hole pair separation efficiency.
oxygen molecules to generate a potent oxidizing species •O2 − , which decomposes an otics into smaller molecular species.Additionally, the incorporation of iron consider boosts the absorption of visible light and enhances solar utilization.In conclusion, th proved photocatalytic degradation performance of FCNBs can be attributed to th creased light harvesting and higher electron-hole pair separation efficiency.

Possible Degradation Pathway of OTC by FCNBs
The degradation intermediates of OTC were detected using LC-MS in order to e date its degradation pathway.Figure S5 and Table S5 present the potential intermedi while Figure 9 illustrates two plausible main degradation pathways.In the first path OTC undergoes dehydroxylation and deamidation, resulting in the formation of P2 = 382.9),which is subsequently further degraded to P3 (m/z = 279.1)through fragm tion.Further dehydroxylation leads to the generation of P4 (m/z = 262.9).In the se pathway, dehydration converts OTC into P1 (m/z = 443.1),which then decomposes fragments into P5 (m/z = 244.2) via deamidation, demethylation, and dehydration cesses.Subsequently, P5 is converted to P6 (m/z = 232.2) through deoxidation react Finally, both P4 and P6 undergo additional decomposition steps, yielding lower-mo lar-weight substances such as P7 (m/z = 110.1),P8 (m/z = 142.0),P9 (m/z = 178.0), and (m/z = 192.0).These small molecules eventually degrade into CO2 and H2O after unde ing further degradation steps.

Possible Degradation Pathway of OTC by FCNBs
The degradation intermediates of OTC were detected using LC-MS in order to elucidate its degradation pathway.Figure S5 and Table S5 present the potential intermediates, while Figure 9

Conclusions
Graphene carbon nitride materials modified with iron were successfully synthesized using a homogeneous mixture of urea and chlorophyll iron sodium salt via chemical vapor-phase co-precipitation.Fe is uniformly dispersed within the internal structure of g-C3N4 through chemical coordination with the g-C3N4 matrix.Furthermore, Fe functions as

Conclusions
Graphene carbon nitride materials modified with iron were successfully synthesized using a homogeneous mixture of urea and chlorophyll iron sodium salt via chemical vaporphase co-precipitation.Fe is uniformly dispersed within the internal structure of g-C 3 N 4 through chemical coordination with the g-C 3 N 4 matrix.Furthermore, Fe functions as an electron trap, thereby improving the separation efficiency of the generation of electronhole pairs through light.The composite demonstrates efficient and stable photocatalytic degradation activity during the decomposition of OTC, making it a promising material for mitigating antibiotic contamination in the environment.

Scheme 1 .
Scheme 1. Flow chart for the synthesis of FCNBs.

Figure 1 .
Figure 1.SEM image (a) and the magnified SEM image (b) of FCNBs.

Figure 1 .
Figure 1.SEM image (a) and the magnified SEM image (b) of FCNBs.

Figure 1 .
Figure 1.SEM image (a) and the magnified SEM image (b) of FCNBs.

Figure 2 .
Figure 2. TEM image (a), the magnified TEM image of a single structural unit (b), and elemental mapping (c-e) of FCNBs.

Figure 2 .Scheme 1 .
Figure 2. TEM image (a), the magnified TEM image of a single structural unit (b), and elemental mapping (c-e) of FCNBs.

Figure 6 .
Figure 6.EIS Nyquist plots (a) and transient photocurrent density response (b) of nanosized and g-C 3 N 4 and FCNBs.

Materials 2024 , 13 Figure 7 .
Figure 7. Photocatalytic activities (a) and kinetic fit (b) of the g-C3N4 and FCNBs for OTC photodegradation; (c) cycle runs for OTC photodegradation on FCNBs; (d) effect of different scavengers on the photodegradation of OTC compared to FCNBs.

Figure 7 .
Figure 7. Photocatalytic activities (a) and kinetic fit (b) of the g-C 3 N 4 and FCNBs for OTC photodegradation; (c) cycle runs for OTC photodegradation on FCNBs; (d) effect of different scavengers on the photodegradation of OTC compared to FCNBs.

Figure 8 .
Figure 8.The possible photocatalytic mechanism of FCNBs for oxytetracycline degradation.

Figure 8 .
Figure 8.The possible photocatalytic mechanism of FCNBs for oxytetracycline degradation.

13 Figure 9 .
Figure 9.The possible degradation pathways of OTC.

Figure 9 .
Figure 9.The possible degradation pathways of OTC.
: SEM image of FCNBs; Figure S2: Photocatalytic activities of (a) 50 mg FCNBs, (b) 30 mg FCNBs in full solar spectrum of light; Figure S3: (a) XRD image and (b) SEM image of FCNBs after photocatalytic activity measurement; Figure S4: (a) Tauc curves of FCNBs and g-C 3 N 4 , Mott-Schottky curves of (b) g-C 3 N 4 and (c) FCNBs, (d) the band structure of g-C 3 N 4 and FCNBs; Figure S5: MS spectra of OTC solution after 60 min degradation; Table