Structural characterization of the catalystsIn this work, a carbon-based catalyst, named EA-x, was prepared via EDTA thermal polymerization, where x is the synthesis temperature. To determine the structural information of the carbon skeleton structure and functional group, a series of structural characterization experiments on these samples (EA-x) were first conducted, including the Fourier transform infrared spectroscopy (FTIR), carbon-13 cross polarization/magic angle spinning nuclear magnetic resonance (13C CP/MAS NMR), thermogravimetric analysis (TGA), and time-of-flight secondary ion mass spectrometry (TOF−SIMS).The FTIR spectra of the pristine EDTA and as-prepared catalysts (EA-x, x = 200, 240, 260, 300, 350 and 400) are shown in Fig. 1a and Supplementary Figs. 1 and 2. In Supplementary Fig. 1, the FTIR spectrum of EA-200 (blue line) is consistent with that of pristine EDTA. Specifically, the peak centered at 3000 cm−1 is ascribed to the stretching vibration of C−H, while the peak located at 1700 cm−1 is assigned to the stretching of C=O14. The peaks located at 1413 cm−1 and 1320 cm−1 are ascribed to COO−, and the peaks located at 1213 cm−1 and 1140 cm−1 are attributed to the absorption vibration mode of C−N32. The absorption bands at 1087 cm−1, 1050 cm−1 and 1010 cm−1 are ascribed to C−C stretching vibrations33. For EA-260 (black line in Fig. 1a), an increase in the peak at 3350 cm−1 compared to EA-200 (blue line in Fig. 1a) indicates the formation of −NH, suggesting that the secondary amine was produced by the cleavage reaction3. Simultaneously, the intensity of the C−H peak decreases, accompanied by a redshift to 2941 cm−1. This observation suggested the transformation of methylene group into a double-bond conjugated structure34. Compared with that of EA-200, the C=O characteristic peak of EA-260 shifts from 1700 cm−1 to 1736 cm−1, demonstrating the formation of cycloketone components3. The peak at 1650 cm−1 is attributed to C=N and C=C3. Compared with those of EA-200, the intensities of the −COO−, C−C, and C−N peaks of EA-260 decreased, which indicates the destruction of the carboxyl group and the breakage of the alkane chain. Since the vibrational mode of the acid anhydride was not observed in the FTIR spectrum of EA-260, carboxylic acid polymerization was excluded. When the synthesis temperature reached 400 °C (EA-400, red line in Fig. 1a), almost all the infrared absorption vibrational peaks disappeared, and the peak at 1638 cm−1 was attributed to C=C or C=N on the aromatic ring. The infrared peak is derived in the second order, and the derivative result is integrated to obtain the relative content of the corresponding functional groups. The relative content of the obtained functional groups is shown in Fig. 1b, and it can be intuitively seen that with increasing reaction temperature, the number of unsaturated bonds (C=C, C=N) first increases and then decreases, and the sample synthesized at 260 °C (EA-260) has the maximum content of unsaturated bonds (source data).Fig. 1: Chemical structure of the catalysts.a FTIR spectra of EA-200, EA-260, and EA-400. b The change trend of the functional group content with synthesis temperature. The peaks of the FTIR spectra of different samples were fitted to obtain the corresponding second derivative spectra. Then, the derived second derivative spectra were used to determine the exact location of the absorption and shoulder peaks in the original spectrum, and the peak area of each subpeak was calculated using the fitted smoothed spectrum of the original spectrum and compared for analysis. 13C CP/MAS NMR spectra of EA-200 (c), EA-260 (d), and (e) EA-400 Inset: Three chemical structures inferred separately from the analysis. All the illuminations were based on the research. f The thermogravimetric curve of EDTA and possible reactions in the corresponding temperature range; ①to ⑤ show the synthesis temperatures of the five catalyst samples. Source data are provided as a Source Data file.Figure 1c–e and Supplementary Fig. 3 show the 13C CP/MAS NMR spectra of these carbon-based catalysts. The 13C spectra of EA-200 and EA-240 show five signals like those of pristine EDTA, indicating that both the EA-200 and EA-240 still maintain the EDTA structure (Fig. 1c and Supplementary Fig. 3a). Specifically, the peak at 53.2 ppm corresponds to saturated carbon atoms connected to carbon and nitrogen atoms, while the peaks at 58.46 and 61.46 ppm corresponds to saturated carbon atoms connected to carboxyl groups4. The chemical shifts at δ = 168.81 ppm and 174.58 ppm correspond to the carbon on the carboxyl group4. The signals in the 13C NMR spectra of EA-260 and EA-300 can be deconvoluted into nine carbon components, a to i, which can be classified as edge-saturated carbon linkers (methyl or methylene) produced by breaking C−C or C−N bonds (a–d), unsaturated pyrazine conjugated systems (e, f), and C=O or C=N in carbocyclic structures (g, h), respectively (Fig. 1d and Supplementary Fig. 3b)35,36. All these structural features suggested that EDTA undergoes cleavage, decarboxylation and dehydration reactions, producing secondary amines as intermediate substrates for further condensation reactions during thermal polymerization at 260 °C (Supplementary Fig. 4). Ultimately, a pyrazine ring bearing a double-bond conjugated carbonyl structure was synthesized from compound EA-260. The 13C NMR spectrum of EA-400 shows two signals ascribed to the aromatic π-conjugated structure (Fig. 1e). This suggested that at 400 °C, due to further carbonization, the saturated carbon linker and amide structure were destroyed and polymerized to form an aromatic π-conjugated system.Thermogravimetric analysis (TGA) of EDTA was performed to elucidate the pyrolysis characteristics of EDTA across a temperature range of 50 to 400 °C. As depicted in Fig. 1f and Supplementary Fig. 5, the pyrolysis process can be divided into three stages. The first stage (stage I), between 50 °C and 243 °C, exhibited negligible weight reduction. Subsequently, the following stage (stage II) occurs from 243 °C to 261 °C, during which EDTA undergoes rapid pyrolysis, resulting in a significant mass reduction of 70%. The weight loss process at this stage and the substantial decrease in the number of −COOH groups and C−N bonds illustrated in the results of IR and NMR may be attributed to decarboxylation and cracking reactions during this phase, and the presence of amide structures indicates the potential for dehydration condensation reactions. Beyond 261 °C (stage III), the pyrolysis action becomes weaker, with the total weight loss reaching 83% at 400 °C.Furthermore, based on the TGA curve, we investigated the various structures of the carbon-based catalysts at five specific temperatures (①to ⑤ for 200 °C, 240 °C, 260 °C, 350 °C, and 400 °C, respectively, in Fig. 1f), and the molecular weight distributions of these samples were determined by gel permeation chromatography (GPC). As shown in Supplementary Fig. 6, with increasing temperature, the molecular weight increases, and the molecular weight distribution becomes wider. Specifically, the molecular weight distribution of EA-260 ranged from 8.2 × 104 g/mol to 5.1 × 106 g/mol, with a peak molecular weight of 8.5 × 104 g/mol, indicating substantial polymerization of EDTA.The hydrogen component transformation of EDTA during thermal polymerization was elucidated by nuclear magnetic resonance (1H NMR) analysis (Supplementary Fig. 7). The peak at 2.77 ppm observed in the spectrum of EA-200 (black line) corresponds to the methylene proton of ethylenediamine in EDTA. Furthermore, the signal at 3.48 ppm is attributed to the protons of the ethylenediamine methylene grafted to the β ammonium groups37. However, the absence of methylene protons in EA-260, EA-350 and EA-400 indicates complete dehydrogenation or cleavage of the C−N bond at synthesis temperatures exceeding 260 °C. Simultaneously, as the synthesis temperature increases, the number of branched methylene hydrogen molecules in β ammonium shifts toward the low magnetic field region due to the α-carbon electron drawing effect37.To characterize the structure of EA-x, TOF−SIMS of EA-x (x = 200, 260, 350 and 400) was performed. The TOF−SIMS of EA-200 showed that the largest monomer fragment (positive ion) was identified as EDTA (positive ion) with m/z = 293 (Supplementary Fig. 8). The TOF−SIMS spectra of EA-260 and EA-350 exhibit similar secondary ion fragment compositions; moreover, based on the above analysis, the fragment structure, i.e., m/z = 127, is derived as N-ethyl-2-piperazinone (Supplementary Fig. 9). The characteristic fragment structure at m/z = 159 in the TOF−SIMS spectrum of EA-400 was simulated and defined as 2-methyl-8-hydroxyl-quinoxaline (Supplementary Fig. 10).The local electronic structure and chemical structure of EA-x were investigated by X-ray absorption spectroscopy (XAS) and X-ray photoelectron spectroscopy (XPS). As depicted in Supplementary Fig. 11, no discernible peaks corresponding to elements other than C, N and O were detected in survey XPS spectra of EA-x (x = 200, 240, 260, 350 and 400). Concurrently, the inductively coupled plasma optical emission spectrometry (ICP-OES) analysis of the EA-x sample revealed an absence of detectable signals associated with metallic elements (The specific elements measured are detailed in Supplementary Table 2). Supplementary Figs. 12a and 13a show the XPS spectra of C 1 s of EA-x (x = 200, 240, 260, 350 and 400), and the peaks of EA-200 centered at 284.8 eV, 286.1 eV, and 288.6 eV are attributed to graphitic carbon (C−C/C=C), C−N/C−O, and C=O, respectively22. As the temperature increased, the intensity of the C−C/C=C peak increased, while the intensities of the C−N/C−O peak and the C=O peak decreased. This suggests that the pyrolysis process destroys the carboxyl group and C−N, providing unsaturated bonds for polymerization. The peak at 284.8 eV observed in the C K-edge XAS spectrum of EA-200 is attributed to the π*, which is a typical out-of-plane C=C bond related to interlayer bonding, and the peak located at 288.1~288.4 eV is attributed to 1 s → σC=O/C−O* (Supplementary Fig. 14)38. The σC=O/C−O* peaks of EA-260 and EA-400 are negatively shifted, which is due to the participation of endogenous oxygen in autooxidation, the formation of carbon oxides by the original carbon species, and the increase in delocalized π bonds in the aromatic carbon layer38. As demonstrated in the N K-edge region of EA-200, the peak located at 407.2 eV is ascribed to 1 s → σN−C* (Supplementary Fig. 15). In the N K-edge XAS spectrum of EA-260, two new signals at 399.4 and 402.5 eV are attributed to the 1 s → π* transitions of heterocyclic aromatic nitrogen atoms (πC=N−C*) and sp3 N−C bridges between triazine groups (πN−C*), respectively38. These results indicate the formation of nitrogen species in prominent triazine-like structures from EA-200 to EA-260, which is beneficial for charge conduction39. From the XPS N 1 s spectrum in Supplementary Figs. 12b and 13b, the transition from C3−N to C=N−C and C−N−H can be observed, which proves the cleavage of C−N bonds on EDTA and the generation of pyrazine structures from EA-200 to EA-400. A negative shift of the peak attributed to C3−N indicates a decrease in the electron density of nitrogen, which may be attributed to the C3−N group being adjacent to the conjugated carbonyl structure. The O K-edge XAS and O 1 s XPS spectra further reveal the changes in surface oxygen species during continuous heat treatment (Supplementary Figs. 12c, 13c and 16). Compared to those of EA-200, no new features are observed in the O K-edge XAS spectra of EA-260 and EA-400 (Supplementary Fig. 16). The peak at 532.7 eV is attributed to the 1 s → π* transition in the carbonyl structure38. In addition, the peak at 539 eV is attributed to the O 1 s → σC−O* transition, which gradually decreases from EA-200 to EA-400. These conclusions are also supported by the XPS O 1 s peak (Supplementary Figs. 12c and 13c).Next, electron microscopy was used to characterize the morphology and microstructure of the as-synthesized catalysts (EA-200, EA-260 and EA-400). As revealed in Fig. 2a, the transmission electron microscopy (TEM) image of EA-200 shows its block-shaped amorphous morphology. The spherical aberration corrected transmission electron microscopy (AC-TEM) image of EA-200 illustrates that EA-200 has a similar structure to EDTA and a clear edge with 0.193 nm and 0.328 nm crystal lattices, corresponding to the (604) and (−213) planes of the monoclinic structure of EDTA (Fig. 2b)40. From the TEM image of EA-260, a flower-like morphology can be observed (Fig. 2c). The AC-TEM image of EA-260 shows that its surface contains of triazine-like carbocyclic rings, and the lattice spacing measured from the AC-TEM image is 0.26 nm which can be indexed to the (110) of the in-plane pyrazine ring unit (Fig. 2d and Supplementary Fig. 17). The X-ray diffraction (XRD) pattern of EA-260 shows a broad peak at 2θ = 17.5° corresponding to the in-plane structural stacking (100) pattern (Supplementary Fig. 18a)41, which is consistent with the TEM results. As shown in Fig. 2e, the edges of the EA-400 particles are curled. The regular graphene-like aromatic system stacking with a lattice spacing of 0.21 nm, which is related to the (100) graphite-like plane, on the local surface can be clearly observed in the AC-TEM image of EA-400 (Fig. 2f). The HAADF-STEM image of EA-400 also shows a clear edge at 0.33 nm belonging to the (002) plane of graphite (Supplementary Figs. 19 and 20)3.Fig. 2: Lattice structure of the catalysts.a HRTEM image of EA-200 showing the blocky morphology; scale: 100 nm. b AC-TEM image of EA-200; scale: 5 Å. The morphology of EA-200 exhibits an EDTA-like atomic arrangement. c HRTEM image of EA-260; scale: 200 nm. d AC-TEM image of EA-260; scale: 2 nm. Inset: Spherical aberration magnified image. EA-260 has a triazine atomic arrangement; scale: 5 Å. e HRTEM image of EA-400; scale: 500 nm. f AC-TEM image of EA-400; scale: 2 nm. Inset: Spherical aberration magnified local image. EA-400 has a graphene-like atomic arrangement; scale: 5 Å.Cyclic voltammetry (CV) was chosen to qualitatively determine the band configuration for various catalysts6. As illustrated in Supplementary Fig. 21, the redox potential derived from the CV curve decreases as the synthesis temperature increases27. At high synthesis temperatures (above 350 °C), a large loss of the structure of oxygen-containing electron-deficient groups (e.g., acyl, carboxyl) leads to a decrease in the oxidizing capacity of the material. Moreover, the results shown in Fig. 3a reveal that the energy band positions of EA-200, EA-240 and EA-260 satisfy the thermodynamic conditions of the WOR and ORR. Similar results were also acquired from the XPS valence spectra of these samples (Supplementary Fig. 22).Fig. 3: Photoelectrochemical properties of the catalysts.a The band diagram derived from the cyclic voltammetry curves. b Transient photocurrent response curves and c Nyquist plots for the EIS spectra of EA-200, EA-240, EA-260, EA-350, and EA-400. Exact data is provided in the source data. d Transient photovoltage spectra of EA-200, EA-240, EA-260, EA-350 and EA-400. e Comparison of the intensity-time curves obtained by extracting a fixed frequency f = 60 Hz from the wavelet transform graph of the TPV curves.Electrochemical tests and transient photovoltage (TPV) analysis were performed to investigate the charge behavior of diverse catalysts. The transient photocurrent response (TPR) curves in Fig. 3b show that EA-260 possesses the best charge separation efficiency among all samples. At the beginning of illumination, the current signal rapidly increases and then gradually decreases to a stable state. This phenomenon indicates that the separation process between electrons and holes is extremely rapid and is accompanied by a redistribution of surface charges on the catalyst. The electrochemical impedance spectroscopy (EIS) curves in Fig. 3c show that EA-260 has the smallest semicircle radius (source data), revealing that it has the lowest charge transfer resistance. The presence of double-bond conjugated carbonyl structures reduce the band width, greatly promoting the generation of charge carriers. Simultaneously, the n-π transition of carbonyl groups promotes carrier separation. TPV was conducted to study the interfacial charge transfer behavior of these five carbon-based catalysts42. The results are presented in Fig. 3d and the Supplementary Table 1, revealing that EA-260 exhibits the highest charge extraction (A), indicating superior surface charge separation efficiency and photogenerated charge. These findings are consistent with those obtained through EIS and TPR analyses. Furthermore, the charge decay constant (τ) of EA-260, which is associated with charge recombination, is much greater than that of EA-350 and EA-400, indicating a longer lifetime for surface photogenerated charges. The results are shown in the Supplementary Table 1 shows the surface effective electron numbers (ne = Aτ/tmax) of the five catalysts, revealing that EA-260 has the highest ne and potential for excellent photocatalytic capacity. The electron transfer dynamics of the catalysts were further studied using fast Fourier transform (FFT) and continuous wavelet transform (CWT) methods27. The FFT and CWT results of the TPV relaxation curve of the EA-x catalysts are shown in Supplementary Figs. 23–26. As shown in Supplementary Fig. 24, the amount of charge at all velocities in EA-260 is greater than that in the other EA-x samples (x = 200, 240, 350 and 400). As shown in Fig. 3e and Supplementary Figs. 25 and 26, the time-intensity spectra of EA-x were compared at seven increasing frequencies. When considering low-speed electrons, the interface charge transfer rate of EA-260 (t1) is much faster than that of the other samples (t2 to t5). When higher-velocity electrons are considered, the surface migration efficiency of all EA-x tends to be consistent. These results indicate that EA-260 can accelerate charge transfer and continuously generate carriers that are delivered to the reaction site owing to the presence of double-bond conjugated carbonyl structures.Catalytic properties of the catalystsThe photocatalytic performance of EA-x (x = 200, 240, 260, 280, 300, 350 and 400) was evaluated in air using a 420 nm light emitting diode (LED). As depicted in Fig. 4a and Supplementary Fig. 27, none of the samples exhibited the production of H2O2 during the initial 4 h incubation in the dark. During the subsequent 12-hour period of exposure to light, both EA-200 and EA-400 demonstrated a lack of photocatalytic activity in the production of H2O2. The EA catalysts synthesized through calcination at temperatures between 240 °C and 350 °C exhibit the production of H2O2. Among them, EA-260 possesses the greatest amount of photogenerated H2O2, reaching 31.46 ± 2.39 mM after 12 h of light irradiation (source data). A six-day continuous cycle experiment was conducted to evaluate the high-performance retention of EA-260. As depicted in Fig. 4b, the performance of EA-260 reached a H2O2 production of 52.66 ± 2.07 mM after 24 h of illumination on the sixth day, indicating the stability of the catalyst (source data). The apparent quantum efficiency (AQE) versus the UV−Vis absorption diagram revealed that the AQE of EA-260 calculated from the yield of H2O2 was 12.67 ± 2.02 % at 420 nm (source data), while the light absorbance increased with increasing carbonization (Fig. 4c and Supplementary Fig. 28). Supplementary Fig. 29 shows the photocatalytic performance test under different gas atmospheres. The rate of photocatalytic H2O2 production by EA-260 under N2 decreased to 602.2 ± 138.4 μmol g−1 h−1, while the rate of photocatalytic H2O2 production increased to 4001.46 ± 232.6 μmol g−1 h−1 in saturated O2 condition. Thus, O2 is the primary reactant in the H2O2 production process. Using 5,5-dimethyl-1-pyrroline N-oxide (DMPO) as a radical spin-trapping agent, in situ EPR was performed to investigate the radicals produced through photochemical activation of different reactants. As shown in Fig. 4d (upper panel), the signals attributed to ·OH were observed, indicating that H2O was oxidized to ·OH by photogenerated holes over EA-260. In the methanol solution, ·O2− signals were observed in the in situ EPR spectra, indicating that O2 was reduced by the electrons photogenerated on EA-260 (Fig. 4d, bottom). The WOR transfer electron numbers of EA-200, EA-260 and EA-400 were investigated electrochemically. As shown in Supplementary Fig. 30, the WOR electron transfer numbers of EA-200 and EA-260 are approximately 2.14 and 2.22 (2e− WOR), respectively. However, the WOR electron transfer number of EA-400 is 3.79, suggesting a 4e− WOR route (H2O is converted to O2) on EA-400.Fig. 4: Photocatalytic properties of the catalysts.a Photocatalytic H2O2 evolution activity of EA-200, EA-240, EA-260, EA-350, and EA-400; The H2O2 production rates of EA-200 and EA-400 are both zero, and the performance curves of the two samples overlap. b Photocatalytic H2O2 evolution cycles of the EA-260. c AQE versus the UV-vis absorption spectrum of EA-260. Error bars represent the standard deviations of three replicate measurements in a–c. d In situ EPR spectra of the EA-260 photocatalytic system in the dark and after 30 min of visible light irradiation. DMPO-·OH: The test is performed in 200 μL of 1 mg/mL of the EA-260 in H2O, with the addition of 200 μL of DMPO solution at a concentration of 100 mM for ·OH capture. DMPO-·O2−: The test was performed in 200 μL of 1 mg/mL EA-260 in methanol, with the addition of 200 μL of DMPO solution at a concentration of 100 mM for ·O2− capture. Exact data of photocatalytic performance is provided in the source data.To investigate the intermediate species and active sites involved in the photocatalytic H2O2 production process, in situ diffuse reflectance infrared fourier transform spectroscopy (in situ DRIFT spectroscopy) was performed on EA-260. As displayed in Fig. 5a, b and Supplementary Fig. 31, the DRIFTs of EA-260 acquired through the adsorption of O2 and water vapor for 30 minutes in the dark were subjected to background subtraction. To emphasize the spectral evolution trend, noise reduction and differential processing were adopted for in situ DRIFT. After 10 min of light exposure, the downward signal that increases with time appears at approximately 3500 cm−1, suggesting consumption of the adsorbed H2O molecules, and the observation of C−O−H at 1326 cm−1 revealed the conversion of C=O into C−O−H. Additionally, the signal appeared at 1723 cm−1 attributed to the C=O from pyrazinone gradually increased along with increasing illumination (from 10 min to 70 min). Meanwhile, the increase in the downward signal of C=OH+ at 1670 cm−1 confirms the pivotal sites in the photocatalytic process of accessing carbonyl groups6. The peaks at 1629 cm−1, 1580 cm−1 and 1530 cm−1 are attributed to C=N, C=NH*, and N−H vibrations, respectively34,43, indicating that the N atoms may serve as potential water adsorption sites or a vibration modes caused by changes in the distribution of electrons on the C=N functional group due to changes in the surrounding electronic environment. In addition, the formation of intermediate species (*OOH and *HOOH), which occur in the two-step single-electron ORR was observed at 1223 cm−1 and 1285 cm−1, respectively43. As shown in Fig. 5c, from the in situ DRIFT spectroscopy, the above information regarding the intermediates involved in the ORR and WOR was observed, as well as the reaction sites on the catalyst. Specifically, the C=O (1723 cm−1) and C=N (1629 cm−1) functional groups served as adsorption sites (3500 cm−1) for H2O molecules, leading to WOR. It is also possible to adsorb protons directly on C=O or C=N. The ORR occurred subsequent to the formation of C−O−H or C−N−H (1326 cm−1 and 1530 cm−1) species.Fig. 5: In situ structural evolution of the catalysts.a, b In situ DRIFTS spectra of EA-260 under illumination conditions in a flow of H2O and O2 for 70 min; the baseline for DRIFTS is EA-260 with 30 minutes of oxygen and water vapor in the dark, allowing the surface of EA-260 to adsorb reactants first. Local spectrum of in situ DRIFTS (a ranging from 4000 cm−1 to 2800 cm−1 and b ranging from 1900 cm−1 to 1000 cm−1). The spectra of these time intervals were differentially processed (subtracting the infrared spectra measured at 5 minutes from all the infrared spectra measured at that time to highlight the changes in the infrared peaks). c Key reaction sites and intermediate information of the WOR and ORR observed in in situ DRIFTS spectra.To investigate the influence of H2O on the photocatalytic production of H2O2, the photocatalytic performance of EA-260 was evaluated under various H2O concentrations in acetonitrile, and saturated O2 was introduced into the testing system. As demonstrated in Fig. 6a, no H2O2 was detected in pure acetonitrile after 6 h of illumination. Upon the addition of 1% H2O to the system, the rate of H2O2 production reaches 120.96 ± 16.50 μmol g−1 h−1 (source data). With the increasing volume fraction of H₂O, the yield of H₂O₂ increases proportionally. Therefore, H2O is a necessary reactant for the formation of H2O2. To investigate whether the WOR affects the ORR in the photocatalytic system of EA-260, the ORR electron transfer number was examined under various conditions. As shown in Fig. 6b, the ORR electron transfer number of EA-260 tested in acetonitrile containing 0.0025 g/L H2O is 0.4 (single-electron ORR process). However, the calculated number of transferred electrons of the ORR is close to 2 (Fig. 6c, two-electron ORR process) in acetonitrile containing 0.1 g/L H2O (the detailed calculation is shown in Supplementary Note 1). Therefore, it can be inferred that the WOR reaction should first be performed on EA-260, and the resulting protons should be used for the ORR reaction (Supplementary Fig. 32).Fig. 6: Photocatalytic mechanism of EA-260.a Catalytic performance of EA-260 in acetonitrile. The H2O content was controlled to test the change in the photocatalytic performance of EA-260 under the condition of trace H2O. Here, 15.0 mg of catalyst was added to 20 mL of acetonitrile. Different volume fractions of H2O (1%, 2%, 3%, 4%, and 5%) and saturated O2 were introduced before illumination of the system, while the other conditions remained unchanged. The amount of H2O2 was measured after 6 h of light exposure. b Rotating ring-disk electrode (RRDE) i-t curves of EA-260 under dark and light conditions (λ ≥ 420 nm) in an O2-saturated 0.1 M TBAP acetonitrile solution (40 mL) containing 2.5 mg/L H2O and c O2-saturated 0.1 M TBAP acetonitrile solution (40 mL) containing 100 mg/L H2O; d free energy diagrams of H2O2 photocatalytic production though cascaded single WOR−1e− ORR pathway (See Supplementary Data 2 for details) and e the models of the molecular structure of the catalyst during the reaction; f free energy diagrams of H2O2 photocatalytic production though cascaded dual WOR−2e− ORR pathway (See Supplementary Data 3 for details); and g models of the molecular structure of the catalyst during the reaction. Source data are provided as a Source Data file.To verify the detailed reaction mechanism of H2O2 production on the asymmetric units of EA-260, density functional theory (DFT) calculations were conducted. In the first step, the H+ adsorption energies on the N and O atoms of EA-260 were calculated to determine the possible active sites (H2O adsorption sites). As shown in Supplementary Fig. 33, H+ adsorption on the N atom of EA-260 is calculated at 2.21 eV, higher than that of O sites (1.26 eV with an O−H distance of 0.98 Å) (see Supplementary Fig. 33 and Supplementary Data 1). Thus, the WOR mainly occurs on the O atom of EA-260. Based on the experimental results discussed above, DFT calculations of the two proposed reaction mechanisms were conducted (Fig. 6d–g). As shown in the free energy diagram (Fig. 6d, e), the procedure comprises one electron (1e−) transfer mechanism featuring a single ·OH intermediate and H+, followed by an end-on (Pauling type) O2 adsorption configuration and a two-step 1e− ORR (Supplementary Data 2)44. Specifically, C=O groups have the ability to undergo n-π transitions when exposed to light, leading to the transfer of electrons from non-bonding σ orbitals to the π anti-bonding orbitals, resulting in the formation of a triplet biradical. Simultaneously conjugation stabilizes the existence of free radicals (Supplementary Figs. 34 and 35)45,46,47. Subsequently, the H2O molecule is adsorbed onto the O atom of EA-260 (the ΔG of H2O adsorption is calculated to be 0.20 eV), leading to a single-electron WOR with an energy barrier of 1.06 eV (source data), which is the rate-determining step (RDS). The WOR process in this stage is in accordance with the previously discussed first-order reaction (Fig. 6a). Then O2 is adsorbed on the H+ generated from the WOR in the end-on (Pauling type) O2 adsorption configuration (Fig. 6e and Supplementary Fig. 36)44,48. O2 is first reduced to ·OOH, with a calculated energy barrier of −1.15 eV, and then further reduced to HOOH, with a calculated energy barrier of −1.66 eV. This result is consistent with the 1e− ORR process observed in our experiments (Fig. 6b). When considering a high H2O content, the second mechanism was illustrated in Fig. 6f, g. As shown in Fig. 6g, two molecules of H2O are adsorbed on the O atoms of two adjacent units of EA-260. The adsorption energy of the first H2O molecule is calculated as 0.20 eV, and that of the second H2O molecule is calculated as 0.03 eV (source data). After WOR (ΔG = 1.96 eV), two H+ remain on the oxygen. O2 is adsorbed onto the H+ generated from the WOR on EA-260, and the side-on (Yeager-type) configuration prevents the cleavage of the O=O bond and facilitates the one-step 2e− ORR (Fig. 6g and Supplementary Data 3)44,48. Sufficient supply of H+ (at a high H2O concentration) promotes the one-step 2e− ORR with an energy barrier of −3.68 eV, which verifies the experimental results (Fig. 6c). The presence of a double-bond conjugated carbonyl group on EA-260 serves as both a water adsorption site and facilitates the generation of protons through the oxidation of water molecules adsorbed under illumination. These protons are safeguarded by the conjugated structure of the molecule. Finally, we evaluated O2 adsorption and direct activation during the initial stage of the ORR, and performed DFT calculations of the ORR on the C atom of EA-260 (Supplementary Data 4). As shown in Supplementary Fig. 37, when adsorbed on the C atom of EA-260, the side-on (Yeager-type) O2 adsorption configuration tends to break the O=O bond, hindering the 2e− ORR44,48. This is consistent with experimental results indicating that the catalytic system produces no H2O2 without water (Fig. 6a). To confirm the proposed reaction mechanism, Fukui function calculations were performed to evaluate the activity of each point reaction. As shown in Supplementary Fig. 38 and Supplementary Table 3, in the simulated monomer structure of EA-260, the electronegativity on the O2 and O3 atoms is relatively higher (E+(O2) = 0.053 e eV, E+(O₃) = 0.03965 e eV), and the CCD values also indicate that the O2 and O3 atoms are more likely to undergo nucleophilic reactions and be reduced (CCD(O₂) = 0.0396 e, CCD(O₂) = 0.0286 e). Hence, in the photocatalytic system of EA-260, the predominant mechanism is the two-step 1e− ORR process under low H2O content conditions, whereas under high H2O content conditions, a one-step, 2e− ORR process is favored.In the next study, we further confirmed that the double-bond conjugated carbonyl structure is the key and universal feature of the active site of metal-free photocatalysts for H2O2 photoproduction. Five small-molecule organics were selected as model catalysts (Fig. 7a–e), and their catalytic activities for the photocatalytic production of H2O2 were examined under the same conditions. As shown in Fig. 7f, the production of H2O2 in cyclohexanone and 2-phenyl-1,4-benzoquinone was detected under light (H2O2 formation rates of 502 ± 67.6 and 136 ± 34.1 μmol g−1 h−1 for cyclohexanone and 2-phenyl-1,4-benzoquinone catalysts, respectively), but no H2O2 was detected in the inositol, 5-phenyl-1,3-cyclohexadidione and 1,4-cyclohexadidione catalytic systems (source data). Hence, it can be deduced that small molecules containing double-bond conjugated carbonyl structures possess the capability to generate H2O2 through photocatalysis.Fig. 7: Verification of the key feature for the active site.Five selected small molecules used as model catalysts: a Cyclohexanone octahydrate, b 1,4-cyclohexanedione, c 2-phenyl-1,4-benzoquinone, d 5-phenyl-1,3-cyclohexanedione, and e inositol. All materials were used directly without further processing. f The H2O2 evolution rate over these five model materials (a–e) under visible light (λ ≥ 420 nm). Error bars represent the standard deviations of three replicate measurements. Source data are provided as a Source Data file.
