Thank you for visiting nature.com. You are using a browser version with limited support for CSS. To obtain the best experience, we recommend you use a more up to date browser (or turn off compatibility mode in Internet Explorer). In the meantime, to ensure continued support, we are displaying the site without styles and JavaScript.

# In situ identification of the metallic state of Ag nanoclusters in oxidative dispersion

## Abstract

Oxidative dispersion has been widely used in regeneration of sintered metal catalysts and fabrication of single atom catalysts, which is attributed to an oxidation-induced dispersion mechanism. However, the interplay of gas-metal-support interaction in the dispersion processes, especially the gas-metal interaction has not been well illustrated. Here, we show dynamic dispersion of silver nanostructures on silicon nitride surface under reducing/oxidizing conditions and during carbon monoxide oxidation reaction. Utilizing environmental scanning (transmission) electron microscopy and near-ambient pressure photoelectron spectroscopy/photoemission electron microscopy, we unravel a new adsorption-induced dispersion mechanism in such a typical oxidative dispersion process. The strong gas-metal interaction achieved by chemisorption of oxygen on nearly-metallic silver nanoclusters is the internal driving force for dispersion. In situ observations show that the dispersed nearly-metallic silver nanoclusters are oxidized upon cooling in oxygen atmosphere, which could mislead to the understanding of oxidation-induced dispersion. We further understand the oxidative dispersion mechanism from the view of dynamic equilibrium taking temperature and gas pressure into account, which should be applied to many other metals such as gold, copper, palladium, etc. and other reaction conditions.

## Introduction

Sintering is a longstanding problem in heterogeneous catalysis leading to deactivation after the long-term operation at high temperatures1,2,3. Many regeneration methods are developed to redisperse the sintered metal catalysts, such as oxidation–reduction, chlorination–oxychlorination, thermal treatment with halohydrocarbons, etc2,4,5,6. Among those, oxidative dispersion is one widely adopted process for the regeneration of used industrial catalysts6,7,8,9,10,11. It has been shown that sintered metal catalysts can break apart into highly dispersed oxide segments during oxidation and are then reactivated by reduction, yielding metal nanoclusters with restored activity4. Beyond catalyst regeneration, oxidative dispersion has recently been employed as one important route to fabricate single-atom catalysts (SACs) and oxidation treatment of supported metal catalysts in the oxidative atmosphere such as air, O2, and water vapor produces SACs of Pt, Pd, Rh, Ag, etc12,13,14,15,16,17,18. Hence, oxidative dispersion is of paramount importance for the fabrication and regeneration of highly/atomically dispersed catalysts with remarkable activity.

Dispersion under oxidizing conditions is a common phenomenon reported in catalysts of Rh/CeO2, Pt/CHA(siliceous chabazite), Ru/CeO2, Ag/MnOx, Pt/FeOx, etc6,12,13,19,20. The consensus on the oxidative dispersion process includes the formation of mobile metal oxide species from large metal particles and capture of these species on the support surface, which are regarded as the most crucial steps in the so-called oxidation-induced dispersion mechanism as revealed by in situ electron microscopy and/or in situ spectroscopy21,22,23,24,25,26,27,28. For example, Nagai et al. ascribed the redispersion of Pt nanoparticles to the formation of Pt oxide species as observed in O2 at 873 K by in situ X-ray absorption spectroscopy (XAS)22. Nevertheless, the underlying mechanism yet needs to be fully depicted. It is well known that the oxidation of metals is strongly dependent on both oxidant partial pressure and temperature. The high temperature applied in catalyst treatments, in general, does not favor the oxide formation, particularly for metals with small heat of formation of an oxide such as Au, Ag, Pd, etc29,30,31. Thus, more detailed investigation by in situ characterization is highly demanded in order to provide new and deep insights into the dynamic mechanism for the oxidative dispersion of supported metal catalysts.

In this work, we performed a state-of-the-art study for the dynamic dispersion of Ag aggregates i.e., nanowires (NWs) and nanoparticles (NPs) supported on Si3N4 surfaces upon heating in O2 using a combination of ex situ, quasi in situ, and in situ characterization techniques including near-ambient pressure XPS (NAP-XPS), near-ambient pressure photoemission electron microscopy (NAP-PEEM), and environmental scanning (transmission) electron microscopy (ESEM/ESTEM). The oxidative dispersion of Ag aggregates has been unambiguously observed, which occurs via the formation of mobile metallic Ag nanoclusters rather than Ag oxide species, and remarkably enhances their catalytic reactivity in CO oxidation. Chemisorption of oxygen from mbar O2 atmosphere is an essential driving force for the dispersion of nearly-metallic Ag nanoclusters under in situ conditions, verified by both experimental evidence and density functional theory (DFT) calculations. The dynamic dispersion of Ag during the reaction and its correlation to the catalytic reactivity is further demonstrated for CO oxidation reaction.

## Results

### Ex situ characterization of oxidation-induced dispersion of AgNWs

Well-defined AgNWs32 were drop-casted onto a Si3N4 thin film (50 nm thick) grown on a Si(100) wafer, denoted as Ag/Si3N4 (see “Methods” and Fig. 1a). The as-prepared AgNWs (Fig. 1b) show an average length of 20 μm with 80 nm in diameter. Thermal treatment in 1 mbar O2 at 673 K results in the dispersion of all AgNWs into ultra-small Ag clusters on the Si3N4 surface (denoted as Ag/Si3N4-O-673), rather than sintered aggregates. The small size makes them nearly invisible under SEM imaging as shown by Fig. 1c. High angle annular dark-field (HAADF)-STEM imaging further reveals the highly dispersed sub-nm Ag nanoclusters (Agn) with a significant number of atomic clusters and single atoms (marked by yellow arrows in Fig. 1d and supplementary Fig. 1).

Measured by quasi in situ XPS (Fig. 1e), the pristine Ag/Si3N4 surface shows Ag 3d5/2 binding energy (BE) of 368.3 eV which is characteristic of metallic silver33, whereas the Ag/Si3N4-O-673 sample presents a significant upshift of Ag 3d5/2 by +1.7 eV to 370.0 eV. Both Si 2p and N 1s spectra of the two samples remain unchanged (Supplementary Fig. 2), suggesting the high stability of the Si3N4 film under the treatment condition. It is well known that Ag oxides usually have a similar or even lower Ag 3d BE compared to Ag metal12. Therefore, the upshift of Ag 3d BE in Ag/Si3N4-O-673 is not caused by the change of oxidation state, but more likely due to size effect34,35. It has been validated that the screening of core holes in ultra-small metal nanoclusters becomes limited which results in an upshift of core-level BEs36,37,38,39. Hence, the upshift of Ag 3d BE is ascribed to the decreasing size of Ag aggregates from micrometer to sub-nanometer. Meanwhile, considering the surface sensitivity of XPS, Ag 3d peak intensity of the Ag/Si3N4-O-673 sample also increases drastically, reflecting the gain of Ag surface area (surface-to-bulk ratio) during the transformation of AgNWs to highly dispersed Ag nanoclusters. To quantify, the peak area ratio of Ag 3d5/2 to Si 2p (denoted as Ag/Si ratio) was derived and used as a representative for the dispersion degree of Ag nanostructures on Si3N4. As illustrated in Fig. 1f, both Ag/Si ratio and Ag 3d5/2 BE reflect the Ag dispersion degree for a given coverage (referred to Ag loadings on Si3N4 substrate), suggesting the high dispersion of AgNWs after the O2 treatment as proved by the SEM/STEM results (Fig. 1b–d).

Regarding the oxidation state of silver, it is unable to distinguish oxide or metallic state using XPS core-levels12,33. Alternatively, Auger Parameters (AP, α) (see the description of Auger parameter in the Supplementary Discussion) defined as the sums of Auger kinetic energy (KE) and photoelectron BE are often used to identify the chemical state of elements including Cu, Ag, Zn, etc37,40,41. Auger spectra of Ag MNN are shown in supplementary Fig. 2, and the sums of Ag 3d5/2 BE and Ag MNN KE were given in Fig. 1f. AP value for pristine Ag/Si3N4 is about 726.4 eV as characteristic for metallic Ag12,40, while that of Ag/Si3N4-O-673 shows a lower value of 723.6 eV reflecting its nature of Ag oxides (e.g., Ag2O)12 after the O2 treatment. Overall, we can thus establish a criterion by using Ag/Si ratio and Ag 3d5/2 BE as indications for Ag dispersion degree, and AP value to describe the oxidation state. To further validate the universality of this dynamic dispersion of Ag on different supports, we have performed additional experiments on a variety of oxides including SiO2/Si(100), Al2O3(0001), and SrTiO3(110) substrates. The upshift of Ag 3d BE and the increase in the Ag 3d peak intensity were observed on all the substrates (supplementary Fig. 3), which is similar to that on the Si3N4 surface (Supplementary Discussion).

### Reversible oscillation of Ag dispersion upon cyclic oxidation–reduction treatments

Cyclic oxidation–reduction treatments (Fig. 2a) were performed to investigate the dispersion-aggregation of Ag nanostructures in an alternative O2 and H2 atmosphere. Quasi in situ Ag 3d XPS spectra (Fig. 2b) and Ag MNN Auger spectra (supplementary Fig. 4) as well as ex situ SEM images (Fig. 2d) reveal good reversibility of Ag dispersion upon the oxidation–reduction cycles. The deduced Ag/Si ratio, Ag 3d5/2 BE, and AP values are presented in Fig. 2c, and an oscillation of Ag dispersion and oxidation states is clearly demonstrated. After the first oxidation treatment (1 bar O2 at 673 K for 1 h), a highly dispersed state of silver oxide (AgOx) nanoclusters was identified at room temperature. The increasing Ag/Si ratio and the upshift of Ag 3d5/2 BE are characteristic of the high dispersion state, and the lower AP value infers its oxide nature. The ultra-small AgOx nanoclusters are likely below 1 nm making them invisible under SEM imaging (Fig. 2d, II).

The subsequent reduction (0.1 bar H2 at 573 K for 1 h) leads to strong sintering as indicated by the decreasing Ag/Si ratio and the downshift of Ag 3d5/2 BE. The reduction to metallic Ag state is verified by the higher AP value. The sintered Ag metal particles show a size range of 10–200 nm measured by SEM (Fig. 2d, III). The re-oxidation (Fig. 2d, IV) can repeatedly disassemble the aggregated Ag particles into ultra-small AgOx clusters. The results indicate that the oxidative dispersion behavior does not rely on the morphology of Ag aggregates, no matter of NWs or NPs. The second reduction shows a good reproducibility yielding metallic Ag aggregates after the H2 treatment. The observed reversible oscillation of Ag dispersion during redox cycles opens the feasibility to control the dispersion of Ag catalysts via oxidation/reduction pretreatments.

Solely based on quasi in situ XPS and ex situ EM results, we can demonstrate oxidative dispersion of μm-scale metallic AgNWs into sub-nm AgOx clusters through 1 mbar–1 bar O2 treatment at 673 K. These ex situ observations are seemingly in line with the previous understanding for the oxidation-induced dispersion mechanism. However, our in situ experiments disproved this “common sense” and further revealed the role of oxygen atmosphere as discussed in the following section.

### In situ observation of oxidative dispersion

In order to elucidate the dynamic process of the Ag dispersion, we performed NAP-XPS studies on Ag/Si3N4 in 1 mbar O2 during heating from 300 to 700 K (Fig. 3a). No obvious change in XPS Ag 3d spectra was observed in a range of 300–600 K. The slight increase of Ag 3d peak intensity is ascribed to the removal of carbon residuals on the sample surface (see C 1s spectra in Supplementary Fig. 5). Further increasing temperature to 700 K results in a sharp increase of Ag/Si ratio along with a prominent BE shift of Ag 3d5/2 from 368.1 to 370.2 eV (Fig. 3b), which serves as a clear indication for the dispersion of AgNWs into small Ag clusters.

Direct imaging of dynamic dispersion of AgNWs was performed in situ using ESEM in 1 mbar O2 at 673 K (Fig. 3c and Supplementary Video 1). Initially, intact AgNWs were observed on Si3N4 surface at t = 0 min. Subsequently, the dispersion of AgNWs occurs at t = 15 min, along with the spread-out of Ag nanoclusters (<1 nm) to the free substrate surface resulting in the invisibility of Ag under SEM (t = 30 min). The dispersion sustains with increasing time and eventually leads to a nearly complete disappearance of AgNWs at t = 45 min. Similarly, the dispersion process was further confirmed by NAP-PEEM42 (Supplementary Fig. 6), which was conducted at 873 K in O2 ambience up to 0.1 mbar. The bright contrast of AgNWs in PEEM images is due to the low surface work function of metallic Ag43. When exposed to O2, part of NW was observed to become dark and the darkening gradually extended to the whole NW (Supplementary Fig. 6), indicating the diffusion of silver atoms from NWs to the bared substrate surface43. Both in situ spectroscopic and microscopic measurements provide a clear picture of the high dispersion of AgNWs at elevated temperatures driven by O2.

### Role of oxygen: surface oxygen adsorption vs. bulk oxidation

It has been well accepted that bulk oxidation with a high oxidation degree is the key step in the dispersion of metal particles in O2 at elevated temperatures6,11,14,20,44,45. However, whether bulk oxidation is necessary for oxidative dispersion of supported metal catalysts still requires to be validated. To this end, we performed NAP-XPS studies of AgNWs on Si3N4 under different conditions in the following sequence: I, pristine Ag/Si3N4 under UHV at room temperature; II, 1 mbar O2 at 700 K; III, UHV at 700 K; IV, 1 mbar O2 at 700 K; V, 1 mbar O2 at 450 K; VI, 1 mbar O2 at 300 K. All XPS core-level and Auger peaks were measured in situ at the treatment temperatures and under the certain environments as presented in Fig. 4a, b, and the corresponding Ag/Si ratios and AP values were displayed in Fig. 4c.

The results show that calcinating at 700 K in 1 mbar O2 (condition II) leads to a significant increase in Ag/Si ratio indicating the dispersion of AgNWs. The AP value remains at 726.0 eV (errors in the range from −0.3 to 0.3 eV due to the broad Ag Auger peaks) that strongly infers a metallic state of dispersed Ag species under in situ condition (700 K, 1 mbar O2). This can be rationalized by the Ag-O phase diagram showing that oxides are prone to decompose into metallic phase at 700 K in 1 mbar O229. It suggests that the formation of bulk oxide with a high oxidation degree is not necessary for stabilizing highly dispersed metallic species. To our best knowledge, it is the first evidence that elucidates the dispersion in the form of nearly-metallic clusters rather than bulk oxide (with a high oxidation degree) during oxidative dispersion. A similar metallic state of dispersed Ag species was also observed on the SiO2/Si(100) surface in O2 at elevated temperatures, verifying a universal phenomenon for SiO2 and other oxides (Supplementary Fig. 7).

After removing mbar O2 to UHV condition (condition III), sintering of dispersed Ag nanoclusters occurs, forming aggregated particles as indicated by the smaller Ag/Si ratio. In absence of O2 atmosphere, the gain of surface energy favors the sintering of Ag metal particles, e.g., Ostwald ripening, which suggests that adsorbed oxygen species from the O2 atmosphere play a critical role in stabilizing highly dispersed Ag nanoclusters. Previous surface science studies on Ag foils and Ag single crystals indicated that adsorbed oxygen species are formed at Ag surfaces at high temperature in O246,47,48, rather than producing bulk oxides (Ag2O). Hence, chemisorption of oxygen on metallic Ag surface is suggested as a possible driving force for the dynamic dispersion of AgNWs/aggregates into sub-nm Ag clusters during the oxidative dispersion. The reversibility of adsorption-driven dispersion-aggregation is further proved by re-exposure of the sintered Ag aggregates to O2 at 700 K (Fig. 4c IV). During the entire process, nearly-metallic state of Ag is preserved as indicated by the constant AP value of 726.0 eV for all four states (I, II, III, and IV).

The cooling process of highly dispersed Ag nanoclusters in 1 mbar O2 from 700 to 300 K was further investigated by changing from condition IV to VI. Cooling down in 1 mbar O2 to 450 and 300 K results in a prominent downshift of AP value to 724.6 eV suggesting the formation of AgOx upon cooling in O2 (Fig. 4c, IV–VI). Meanwhile, the constant Ag/Si ratio (Fig. 4c, IV–VI) reveals that the high dispersion of Ag nanoclusters is still preserved at low temperatures. Therefore, we can depict an overall picture of dynamic dispersion of AgNWs in 1 mbar O2 by two independent processes: (1) surface oxygen adsorption-driven dispersion of AgNWs to Ag nanoclusters at 700 K, and (2) oxidation of readily dispersed Ag nanoclusters to bulk-like AgOx nanoclusters with a high oxidation degree during cooling to 300 K. Our in situ characterizations allow to conclude that the chemisorption of oxygen on metallic silver is the driving force for Ag dispersion whereas the bulk oxide with a high oxidation degree is only the result upon cooling in O2.

### DFT study in oxidative dispersion mechanism

We proposed a DFT-based model to understand the O2 adsorption-induced dispersion. The equation for this model is described in the “Methods” section (Eq. (1)). The competing mechanism among cohesive energy (Ecoh, metal-metal interaction), adhesion energy (Eadh, metal-support interaction), and gas adsorption energy (Eads, metal-gas interaction) has been considered thoroughly, the sum of which constitutes the formation energy of the NP/cluster on the support under in situ conditions. The difference of the averaged formation energy/atom between the sintered NP and the dispersed cluster $$({\Delta}E_{\mathrm{for}})$$, thus determines the dynamic dispersion, and the positive $${\Delta}E_{\mathrm{for}}$$ favors the dispersion.

Considering the very large average sizes of the sintered NPs in this work (over 100 nm), we used the cohesive energy/atom of bulk Ag $$(E_{\mathrm{{coh}}}^{\mathrm{{bulk}}})$$ to represent the NP’s Ecoh (set α in Eq. (1) to be 12), which is −2.79 eV in our calculation. Ag3 and Ag8 clusters were used as the models for the cluster calculations, the $$E_{\mathrm{{coh}}}^{\mathrm{{clu}}}$$ of which are calculated to be −1.21 and −1.86 eV, respectively. Thus, in their freestanding states, ΔEfor are −1.58 and −0.93 eV, respectively (Fig. 4d). When supported on the surface, the averaged Eadh/atom of the sintered NP is neglectable because the ratio of the interface to volume for such a large particle is very small. On the other hand, the averaged Eadh/atom of Ag3 and Ag8 clusters are calculated to be −0.96 and −0.56 eV on the supported Si3N4(0001) surface (Supplementary Figs. 8, 9), respectively. Consequently, $${\Delta}E_{\mathrm{for}}$$ becomes −0.62 and −0.37 eV, respectively, which are still negative, suggesting that the addition of metal-support interaction is insufficient to disperse Ag NPs into nanoclusters. This thus explains the aggregated state of Ag particles under UHV condition during in situ experiments in Fig. 4c, III when O2 is removed from the atmosphere.

When O2 adsorption is involved, the reaction condition effects (temperature and gas pressure) are considered through the calculation of gas adsorption coverage θi by using a DFT-based thermodynamic adsorption isotherm described in the methods section49,50,51. We used the gas coverage of O2 on three low-index surfaces ($$\theta ^{111},\;\theta ^{110},\;\theta ^{100}$$) to estimate θi of the sintered NP because a nanosized Ag particle is normally composed of these surfaces (supplementary Fig. 10). The results show that O2 barely adsorbs on the three surfaces at 673 K even with an O2 pressure of 1 bar due to the small adsorption energies ($$E_{\mathrm{ads}}^{111} = - 0.40$$ eV, $$E_{\mathrm{ads}}^{110} = - 0.38$$ eV, $$E_{\mathrm{ads}}^{100} = - 0.76$$ eV). On the contrary, associative O2 and dissociative O atoms adsorb stably at the Ag3-Si3N4 ($$E_{\mathrm{ads}}^{\mathrm{clu}} = - 2.24\;{\mathrm{eV}}$$) and Ag8-Si3N4 ($$E_{\mathrm{ads}}^{\mathrm{clu}} = - 3.97\;{\mathrm{eV}}$$) interfaces, which leads to $$\theta ^{\mathrm{clu}} = 1$$ for both models at 673 K under either 1 mbar O2 or 1 bar O2. The averaged $$E_{\mathrm{ads}}^{\mathrm{clu}}$$/atom is −0.75 and −0.50 eV, respectively, which eventually makes $${\Delta}E_{\mathrm{for}}$$ positive (0.13 eV for both models, Fig. 4d). Compared to the sintered NP, dispersed nanoclusters have more contact with the support surface and the O2 gas environment. Neither the support effect nor the O2 adsorption could cause the dispersion of Ag NPs observed in our experiments, but the combined effects are enough to pry the lever.

### Dynamic dispersion during CO oxidation reaction

The dynamic dispersion of Ag nanostructures during the reaction was further verified for CO oxidation11,48,52,53,54 and the impact on their catalytic activity was investigated. In situ ESEM images (Fig. 5a) show the dynamic dispersion of AgNWs under reaction conditions of 5% CO/95% O2 at 1 mbar. The dispersion of AgNWs initially occurs at 623 K and reaches a highly dispersed state at 673 K. The highly dispersed Ag nanoclusters remain in the reaction gases during cooling. The catalytic test was further performed in a home-built flow reactor with an online mass spectrometer to the outlet for product analysis (see Supplementary Methods). The reactivity for catalytic CO oxidation reaction was present in Fig. 5b and Supplementary Fig. 11, and a hysteresis phenomenon was clearly identified upon heating and cooling cycle, as the result of the dynamic structure evolution of Ag during the reaction. The highly dispersed Ag nanoclusters formed during reaction exhibit an enhanced activity especially at low temperature, higher than the initial state of AgNWs upon heating. A similar reactivity at 623 K indicates the structural transformation from NWs to nanoclusters which is consistent with the in situ ESEM observations. The time-on-stream stability test displayed in Fig. 5c further reveals excellent durability of the highly dispersed Ag/Si3N4 catalyst under the reaction condition (at 673 K) up to 35 h (also see Supplementary Discussion). Our results thus prove the long-term stability of dispersed nearly-metallic Ag nanoclusters in O2-rich reaction environments, and opens up a new route for the fabrication of highly dispersed catalysts during the reaction.

## Discussion

Dynamic dispersion of AgNWs into sub-nm Ag clusters on Si3N4 surface has been observed using combined ex situ and in situ characterization techniques. By altering oxidizing/reducing treatments, we can reversibly switch between highly dispersed Ag nanoclusters (0.7 nm) and aggregated Ag particles (20–100 nm). Based on ex situ characterizations, we readily observed the formation of dispersed silver oxides at room temperature after the high-temperature treatment in O2, which is in line with the commonly accepted “oxidation dispersion” scenario. However, as Fig. 6 summarized, our in situ studies directly demonstrated a transitional state of nearly-metallic Ag during dispersion that overturn this common concept and depict an overall scenario of dynamic dispersion under O2 environment consisting of oxygen adsorption-induced dispersion of Ag in a nearly-metallic state at 700 K and oxidation of readily dispersed Ag nanoclusters to Ag oxide nanoclusters during cooling to 300 K. We provide solid evidence for the fact that formation of bulk oxide with a high oxidation degree is not necessary in oxidative dispersion, but a result during cooling in O2. Chemisorption of oxygen on nearly-metallic Ag rather than bulk oxidation is proved as the driving force to disperse Ag aggregates and stabilize ultra-small Ag clusters under in situ conditions. Correctly understanding the role of O2 environment played in oxidative dispersion is of great significance in predicting and controlling the dynamics of dispersion/redispersion of supported metal catalysts under reaction conditions. It also opens up a new route to stabilize metal nanoclusters in a realistic reaction atmosphere, and benefits the fabrication of highly/atomically dispersed catalyst during reaction.

## Methods

### Sample preparation and treatment

AgNWs were synthesized via a polyol method and then purified by a novel dynamic agitation-induced centrifugal filtration32. Si3N4 film (50-nm thick) grown on Si(100) single crystals were purchased from Prmat (Shanghai) Technology Co., Ltd. The inert Si3N4 films are nearly free of surface defects55 and remain stable under reaction conditions (see Supplementary Discussion). AgNWs in ethanol solution were drop-casted onto the Si3N4 substrate (denoted as Ag/Si3N4). We prepared three kinds of samples with different Ag densities (high, medium, and low). To acquire strong Auger spectra, samples with high NW density were used and shown in Fig. 4. Samples with medium AgNW density were used to get an obvious change of Ag/Si ratio during various treatments, also to make XPS peak intensity strong enough, shown in Figs. 13. Samples with low density were used in electron microscopy (SEM, STEM, PEEM) to observe the process easily. The effect of surface concentration in our experiments was excluded by SEM results (Supplementary Fig. 16). Ex situ treatments were performed in 1 mbar O2, 1 bar O2, or 100 mbar H2 at elevated temperatures in a high-pressure reactor (SPECS, HPC-20) (denoted as Ag/Si3N4-x-y, x is the atmosphere and y is the temperature).

### Scanning transmission electron microscopy

AC-STEM was performed on a JEM ARM200F (JEOL, Japan), equipped with a thermal-field emission gun and a Cs-corrector. The microscope was operated at 80 kV to minimize the beam damage. For the high angle annular dark-field (HAADF) imaging, the convergence angle of ~23 mrad and collection angle range of 68–174 mrad were adapted for the incoherent atomic number imaging.

### In situ NAP-XPS

Surface chemistry of Ag/Si3N4 was characterized in a lab-based near-ambient pressure X-ray photoelectron spectroscopy (SPECS EnviroESCA). Spectra were obtained using monochromatic Al Kα irradiation (1486.7 eV) of an Al anode operated at 50 W. A pass energy of 40 eV with a step of 0.05 eV and a dwell time of 0.1 s were typically used for acquiring the core-level spectra.

### Quasi in situ XPS

Quasi in situ XPS measurements were carried out with a spectrometer equipped with an Mg Kα X-ray source operated at 300 W. The background pressure was in the range of 10−9 mbar. Ex situ treatments were performed in the high-pressure reactor (SPECS, HPC-20). After each treatment, the sample was transferred to the analysis chamber for XPS measurements without exposure to air. All quasi in situ XPS spectra were collected under UHV (10−9–1010 mbar) at room temperature.

### In situ ESEM

In situ SEM imaging was performed in a commercial ESEM (FEI Quanta 650) equipped with a commercial heating stage and a gas feeding unit. The accelerating voltage was 20 kV with an objective lens aperture of 30 μm. During heating, low magnification was used to locate the targeted area due to thermal drift, and high magnification imaging (×20,000) was conducted when the temperature is stable.

### In situ NAP-PEEM

PEEM experiments were performed on a newly developed NAP-PEEM system, which enables high-resolution PEEM imaging in gases with pressures up to 1 mbar. A tunable deep ultraviolet (DUV) laser with wavelength between 175 and 210 nm was used as an excitation source. The sample was heated up by a specially design laser heater, and the sample temperature was measured by an infrared thermometer. The in situ PEEM imaging was conducted by first heating the sample to a specific temperature and then dosing O2 with increasing pressures.

### Catalytic testing

The sample was prepared by drop-casting of AgNWs onto Si3N4/Si(100) surfaces (10 mm × 10 mm) with a silver loading of 1 μg. The catalytic test was performed in a home-built cell reactor (setup details see Supplementary Methods) in a gas flow of 10 ml/min 5% CO/95% O2 at atmospheric pressure. The reaction product (CO2, m/z 44) was monitored by an online mass spectrometer (SRS RGA) to the outlet of the reactor. The cell reactor was repeatedly purged and flushed with the reaction gas for >6 h to achieve a clean background. All catalysts were pre-reduced in 5% H2 at 100 °C for 30 min before catalytic measurements.

### Equation for the adsorption-induced dispersion model

Equation (1) is the formula we used to estimate the energy difference per atom between a sintered NP and dispersed clusters on the support under the O2 gas conditions.

$${\Delta}E_{\mathrm{for}} = \frac{\alpha }{{12}}E_{\mathrm{coh}}^{\mathrm{bulk}} + \left( {\frac{{E_{\mathrm{adh}}^{\mathrm{par}}}}{{N_{\mathrm{par}}}} + \frac{{\mathop {\sum }\nolimits_{i = 1}^{N_{\mathrm{surf}}} \theta ^iE_{\mathrm{ads}}^i}}{{N_{\mathrm{par}}}}} \right) - E_{\mathrm{coh}}^{\mathrm{clu}} - \left( {\frac{{E_{\mathrm{adh}}^{\mathrm{clu}}}}{{N_{\mathrm{clu}}}} + \frac{{\theta ^{\mathrm{clu}}E_{\mathrm{ads}}^{\mathrm{clu}}}}{{N_{\mathrm{clu}}}}} \right)$$
(1)

The first term in Eq. (1) is the cohesive energy per atom of the sintered NP, in which $$E_{\mathrm{coh}}^{\mathrm{bulk}}$$ is the cohesive energy of a bulk Ag atom, α represents for the average coordination number of a sintered NP, and 12 is the coordination number of bulk Ag. The support effect and the O2 adsorption effect on the sintered NP are considered in the second term, in which $$E_{\mathrm{adh}}^{\mathrm{par}}$$ is the adhesion energy of the NP on the support, θi is the adsorption coverage of O2 at the ith surface site, $$E_{\mathrm{ads}}^i$$ is the corresponding adsorption energy, $$N_{\mathrm{surf}}$$ is the number of surface sites, and $$N_{\mathrm{par}}$$ is the number of atoms of the NP. The third term ($$E_{\mathrm{coh}}^{\mathrm{clu}}$$) is the cohesive energy of the dispersed cluster averaged to each atom. The support effect and the O2 adsorption effect on the dispersed cluster are considered in the fourth term, in which $$E_{\mathrm{adh}}^{\mathrm{clu}}$$ is the adhesion energy of the cluster on the support, $$\theta ^{\mathrm{clu}}$$ is the adsorption possibility, $$E_{\mathrm{ads}}^{\mathrm{clu}}$$ is the corresponding adsorption energy, and $$N_{\mathrm{clu}}$$ is the number of atoms of the cluster. If the formation energy difference per atom $${\Delta}E_{\mathrm{for}}$$ is larger than zero, the dispersion of the nanoclusters is preferred. The DFT settings can be found in the Supplementary Information.

The O2 coverage (θ) at a given adsorption site was described using the Langmuir adsorption isotherm. The formula is shown below,

$$\theta = PK/(1 + PK)$$
(2)

where P is the gas pressure, K is the equilibrium constant calculated as below:

$$K = {\mathrm{exp}}\left( { - \frac{{{\Delta}G}}{{RT}}} \right) = {\mathrm{exp}}\left( { - \frac{{E_{\mathrm{ads}} - T\left( {S_{\mathrm{ads}} - S_{\mathrm{gas}}} \right)}}{{RT}}} \right)$$
(3)

where R is the gas constant, T is the temperature, $$E_{\mathrm{ads}}$$ is the gas adsorption energy obtained from DFT calculations, $$S_{\mathrm{ads}}$$ and $$S_{\mathrm{gas}}$$ are the entropy of adsorbed O2 and gas-phase O2, respectively. In this work, $$S_{\mathrm{ads}}$$ was set to be 0 and $$S_{\mathrm{gas}}$$ was obtained from the thermodynamic table (https://www.nist.gov/srd).

## Data availability

The data that support the plots within this paper and other findings of this study are available from the corresponding author upon reasonable request due to the data are of large amount.

## References

1. Campbell, C. T., Parker, S. C. & Starr, D. E. The effect of size-dependent nanoparticle energetics on catalyst sintering. Science 298, 811–814 (2002).

2. Argyle, M. D. & Bartholomew, C. H. Heterogeneous catalyst deactivation and regeneration: A review. Catalysts 5, 145–269 (2015).

3. Hansen, T. W., Delariva, A. T., Challa, S. R. & Datye, A. K. Sintering of catalytic nanoparticles: Particle migration or ostwald ripening? Acc. Chem. Res. 46, 1720–1730 (2013).

4. Morgan, K., Goguet, A. & Hardacre, C. Metal redispersion strategies for recycling of supported metal catalysts: a perspective. ACS Catal. 5, 3430–3445 (2015).

5. Sa, J. et al. Redispersion of gold supported on oxides. ACS Catal. 2, 552–560 (2012).

6. Moliner, M. et al. Reversible transformation of Pt nanoparticles into single atoms inside high-silica chabazite zeolite. J. Am. Chem. Soc. 138, 15743–15750 (2016).

7. Birgerssona, H., Boutonnet, M. & Lars, E. S. J. Deactivation and regeneration of spent three-way automotive exhaust gas catalysts (TWC). Top. Catal. 30, 433–437 (2004).

8. Nishihata, Y. et al. Self-regeneration of a Pd-perovskite catalyst for automotive emissions control. Nature 418, 164–167 (2002).

9. Ganzler, A. M. et al. Tuning the structure of platinum particles on ceria in situ for enhancing the catalytic performance of exhaust gas catalysts. Angew. Chem. Int. Ed. 56, 13078–13082 (2017).

10. Dessal, C. et al. Atmosphere-dependent stability and mobility of catalytic Pt single atoms and clusters on γ-Al2O3. Nanoscale 11, 6897–6904 (2019).

11. Zhang, Z. et al. Thermally stable single atom Pt/m-Al2O3 for selective hydrogenation and CO oxidation. Nat. Commun. 8, 16100 (2017).

12. Huang, Z. et al. Catalytically active single-atom sites fabricated from silver particles. Angew. Chem. Int. Ed. 51, 4198–4203 (2012).

13. Jeong, H. et al. Fully dispersed Rh ensemble catalyst to enhance low-temperature activity. J. Am. Chem. Soc. 140, 9558–9565 (2018).

14. Spezzati, G. et al. Atomically dispersed Pd-O Species on CeO2(111) as highly active sites for low-temperature CO oxidation. ACS Catal. 7, 6887–6891 (2017).

15. Wang, A., Li, J. & Zhang, T. Heterogeneous single-atom catalysis. Nat. Rev. Chem. 2, 65–81 (2018).

16. Jones, J. et al. Thermally stable single-atom platinum-on-ceria catalysts via atom trapping. Science 353, 150–154 (2016).

17. Wang, F. et al. Resolving the puzzle of single-atom silver dispersion on nanosized γ-Al2O3 surface for high catalytic performance. Nat. Commun. 11, 529 (2020).

18. Liu, K. et al. Strong metal-support interaction promoted scalable production of thermally stable single-atom catalysts. Nat. Commun. 11, 1263 (2020).

19. Lang, R. et al. Non defect-stabilized thermally stable single-atom catalyst. Nat. Commun. 10, 234 (2019).

20. Aitbekova, A. et al. Low-temperature restructuring of CeO2-supported Ru nanoparticles determines selectivity in CO2 catalytic reduction. J. Am. Chem. Soc. 140, 13736–13745 (2018).

21. Maurer, F. et al. Tracking the formation, fate and consequence for catalytic activity of Pt single sites on CeO2. Nat. Catal. 3, 824–833 (2020).

22. Nagai, Y. et al. In situ redispersion of platinum autoexhaust catalysts: an on-line approach to increasing catalyst lifetimes? Angew. Chem. Int. Ed. 47, 9303–9306 (2008).

23. Ferré, G. et al. Exploiting the dynamic properties of Pt on ceria for low-temperature CO oxidation. Catal. Sci. Technol. 10, 3904–3917 (2020).

24. DeRita, L. et al. Structural evolution of atomically dispersed Pt catalysts dictates reactivity. Nat. Mater. 18, 746–751 (2019).

25. Kibis, L. S. et al. Redox and catalytic properties of RhxCe1–xO2−δ solid solution. J. Phys. Chem. C 121, 26925–26938 (2017).

26. Gao, Y. et al. Aggregation and redispersion of silver species on alumina and sulphated alumina supports for soot oxidation. Catal. Sci. Technol. 7, 3524–3530 (2017).

27. Gardini, D., Christensen, J. M., Damsgaard, C. D., Jensen, A. D. & Wagner, J. B. Visualizing the mobility of silver during catalytic soot oxidation. Appl. Catal. B 183, 28–36 (2016).

28. Ikemoto, S. et al. Reversible low-temperature redox activity and selective oxidation catalysis derived from the concerted activation of multiple metal species on Cr and Rh-incorporated ceria catalysts. Phys. Chem. Chem. Phys. 21, 20868–20877a (2019).

29. Li, W., Stampfl, C. & Scheffler, M. Why is a noble metal catalytically active? The role of the O-Ag interaction in the function of silver as an oxidation catalyst. Phys. Rev. Lett. 90, 256102 (2003).

30. Ketteler, G. et al. In situ spectroscopic study of the oxidation and reduction of Pd(111). J. Am. Chem. Soc. 127, 18269–18273 (2005).

31. Tsai, H. C. et al. Instability of gold oxide Au2O3. Surf. Sci. 537, L447–L450 (2003).

32. Wang, H., Tang, H., Liang, J. & Chen, Y. Dynamic agitation-induced centrifugal purification of nanowires enabling transparent electrodes with 99.2% transmittance. Adv. Funct. Mater. 28, 1804479 (2018).

33. Schon, G. ESCA studies of Ag, Ag2O and AgO. Acta Chem. Scand. 27, 2623–2633 (1973).

34. Luo, K., Clair, T. P. S., Lai, X. & Goodman, D. W. Silver growth on TiO2(110) (1 × 1) and (1 × 2). J. Phys. Chem. B 104, 3050–3057 (2000).

35. Guo, D., Guo, Q., Zheng, K., Wang, E. & Bao, X. Initial growth and oxygen adsorption of silver on Al2O3 film. J. Phys. Chem. C 111, 3981–3985 (2007).

36. Mao, B. et al. A near ambient pressure XPS study of subnanometer silver clusters on Al2O3 and TiO2 ultrathin film supports. Phys. Chem. Chem. Phys. 16, 26645–26652 (2014).

37. Moretti, G. The Wagner plot and the Auger parameter as tools to separate initial- and final-state contributions in X-ray photoemission spectroscopy. Surf. Sci. 618, 3–11 (2013).

38. Bagus, P. S., Wieckowski, A. & Freund, H. Initial and final state contributions to binding-energy shifts due to lattice strain: validation of Auger parameter analyses. Chem. Phys. Lett. 420, 42–46 (2006).

39. Fu, Q. & Wagner, T. Interaction of nanostructured metal overlayers with oxide surfaces. Surf. Sci. Rep. 62, 431–498 (2007).

40. Aspromonte, S. G., Mizrahi, M. D., Schneeberger, F. A., Lopez, J. M. R. & Boix, A. V. Study of the nature and location of silver in Ag-exchanged mordenite catalysts. Characterization by spectroscopic techniques. J. Phys. Chem. C 117, 25433–25442 (2013).

41. Wagner, C. Auger parameter in electron spectroscopy for the identification of chemical species. Anal. Chem. 47, 1201–1203 (1975).

42. Ning, Y. et al. A near ambient pressure photoemission electron microscope (NAP-PEEM). Ultramicroscopy 200, 105–110 (2019).

43. Huang, W. & Bao, X. Adsorption and reaction of CO and O2 on the Ag/Pt(110) surface studied by photoemission electron microscopy. Chin. Sci. Bull. 46, 998–1001 (2001).

44. Kwak, J. H. et al. Coordinatively unsaturated Al3+ centers as binding sites for active catalyst phases of platinum on γ-Al2O3. Science 325, 1670–1673 (2009).

45. Homeyer, S. T. & Sachtler, W. M. H. Oxidative redispersion of palladium and formation of PdO particles in Nay: an application of high-precision TPR. Appl. Catal. 54, 189–202 (1989).

46. Pettinger, B., Bao, X., Wilcock, I. C., Muhler, M. & Ertl, G. Surface-enhanced Raman scattering from surface and subsurface oxygen species at microscopically well-defined Ag surfaces. Phys. Rev. Lett. 72, 1561–1564 (1994).

47. Rocha, T. C. et al. The silver-oxygen system in catalysis: new insights by near ambient pressure X-ray photoelectron spectroscopy. Phys. Chem. Chem. Phys. 14, 4554–4564 (2012).

48. Qu, Z., Huang, W., Cheng, M. & Bao, X. Restructuring and redispersion of silver on SiO2 under oxidizing/reducing atmospheres and its activity toward CO oxidation. J. Phys. Chem. B 109, 15842–15848 (2005).

49. Zhu, B., Xu, Z., Wang, C. & Gao, Y. Shape evolution of metal nanoparticles in water vapor environment. Nano Lett. 16, 2628–2632 (2016).

50. Zhang, X. et al. Reversible loss of core–shell structure for Ni–Au bimetallic nanoparticles during CO2 hydrogenation. Nat. Catal. 3, 411–417 (2020).

51. Yuan, W. et al. Visualizing H2O molecules reacting at TiO2 active sites with transmission electron microscopy. Science 367, 428–430 (2020).

52. Fu, Q. et al. Interface-confined ferrous centers for catalytic oxidation. Science 328, 1141–1144 (2010).

53. Schlögl, R. Heterogeneous catalysis. Angew. Chem. Int. Ed. 54, 3465–3520 (2015).

54. Lamoth, M. et al. Supported Ag nanoparticles and clusters for CO oxidation: size effects and influence of the silver–oxygen interactions. ACS Appl. Nano. Mater. 2, 2909–2920 (2019).

55. Bocanegra, M. H. & Matovic, B. Dense and near-net-shape fabrication of Si3N4 ceramics. Mater. Sci. Eng. A 500, 130–149 (2009).

## Acknowledgements

This work was financially supported by the National Natural Science Foundation of China (Nos. 21688102, 21825203, 21872145, and 21773287), the National Key R&D Program of China (Nos. 2016YFA0200200 and 2017YFB0602205), Strategic Priority Research Program of the Chinese Academy of Sciences (No. XDB17020000), and B.Y. acknowledges the Foundation of Dalian Institute of Chemical Physics (DICP I201943). B.Z. thanks for the Youth Innovation Promotion Association, CAS, and the financial support of Key Research Program of Frontier Sciences, CAS, Grant No. ZDBS-LY-7012. All calculations were performed at National Supercomputing Center in Guangzhou (NSCC-GZ), Shanghai, and Tianjin.

## Author information

Authors

### Contributions

R.L. and Q.F. performed the sample preparation, XPS experiments, and surface data analysis. Y.N. and R.M. contributed to the NAP-PEEM experiments and surface data analysis. X.X. and B.Y. conducted the ESEM/STEM characterizations and catalytic test. P.D. and M.L. assisted with the catalytic test and data analysis. B.Z., X.L., and Y.G. conducted the DFT calculations. H.W., J.L., and Y.C. prepared the AgNWs. Q.F. and X.B. directed the project. All the authors discussed the results and wrote the manuscript together.

### Corresponding authors

Correspondence to Yi Gao, Bing Yang, Qiang Fu or Xinhe Bao.

## Ethics declarations

### Competing interests

The authors declare no competing interests.

Peer review information Nature Communications thanks Zhen-Yu Tian, and the other, anonymous, reviewer(s) for their contribution to the peer review of this work. Peer reviewer reports are available.

Publisher’s note Springer Nature remains neutral with regard to jurisdictional claims in published maps and institutional affiliations.

## Rights and permissions

Reprints and Permissions

Li, R., Xu, X., Zhu, B. et al. In situ identification of the metallic state of Ag nanoclusters in oxidative dispersion. Nat Commun 12, 1406 (2021). https://doi.org/10.1038/s41467-021-21552-2

• Accepted:

• Published:

• DOI: https://doi.org/10.1038/s41467-021-21552-2

• ### Ultrasmall Ag nanoclusters anchored on NiCo-layered double hydroxide nanoarray for efficient electrooxidation of 5-hydroxymethylfurfural

• Jing Jin
• Yingyan Fang
• Junfeng Liu

Science China Materials (2022)

• ### Effect of the Ag–CeO2 interaction and the nature of pore structure on the catalytic activities of different Ag–CeO2/mesoporous-SiO2 catalysts on the reduction of 4-nitrophenol

• Kumer Saurav Keshri
• Biswajit Chowdhury

Journal of Porous Materials (2022)