## Introduction

High-entropy alloys (HEAs) with five or more elemental species have been successfully synthesized and have attracted extensive attention due to their unique physical properties and potential applications1,2,3. Compared with HEAs, it is more difficult to yield the formation of high entropy ceramics including oxides, carbides, nitrides et al. owing to their larger heats of formation. Since 2015, the family of high entropy materials has been expanded when the first entropy-stabilized oxides (HEOs) were reported by Rost et al.4. HEOs, a kind of multicationic equiatomic oxides, were then found to have a variety of interesting and unexpected characteristics5. Inspired from this discovery, several kinds of high-entropy oxides with different crystal structures were then reported one after another, such as perovskite oxide6,7, spinel oxide8, and fluorite oxide9,10,11. Quite recently, new entropy-stabilized single-phase fluorite oxides (HEFO) Hf0.25Zr0.25Ce0.25Y0.25O2–δ11 and Ce0.2Zr0.2Hf0.2Sn0.2Ti0.2O212 were also synthesized by using high-energy ball milling. However, rigorous synthetic conditions, including the long reaction time (6–24 h), ultra-high temperature (1500–1800 °C), and uniaxial high pressure, limit its application in catalysis.

Fluorite oxide-supported noble metals including SACs are widely used as heterogeneous catalysts with superior catalytic performances for mitigating critical pollutants (e.g., CO, CH4, HCs, and NOx) from engine emissions. A wide range of hosts (metal oxides, N-doped C, zeolites, MOFs, etc.) are known for their ability to stabilize single atoms13. Recent advances in synthetic strategies for SACs are generally dominated by wet-chemistry approaches including defect engineering, spatial confinement, and coordination design strategies14,15. Mechanochemistry scenarios, which have attracted more interest because of their quick, quantitative, and solvent-free properties compared with wet-chemistry approaches, however, have always been a great challenge for fabricating atomically dispersed metal sites16,17,18. In addition, the successful assembly of metal single atoms on conventional carriers often requires a very careful control of synthesis conditions, such as low temperature19,20, low metal loading21,22, grafting of N-rich organic linkers23,24, etc. Therefore, fabricating sintering-resistant SACs with intrinsically thermodynamic stability on high-entropy supports by using a solvent-free synthetic strategy is highly desirable.

Herein, we present a mechanochemical-assisted synthesis of Pd single atoms substituted on HEFO by simple mechanical milling followed by the calcination of metal precursors. The unique trait of HEFO can be validated by the formation of isolated Pd atoms on Pd1@HEFO, as well as the presence of Pd agglomeration with CeO2 as an alternative carrier under the same preparation conditions. A series of characterizations including high-resolution transmission electron microscopy (HRTEM), energy-dispersive X-ray spectroscopy (EDS) mapping, extended X-ray absorption fine structure (EXAFS), and diffuse reflectance infrared Fourier transform spectroscopy (DRIFTS) measurements are employed to unravel the existence of high-entropy phase and isolated Pd atoms in Pd1@HEFO. The catalytic activity of CO oxidation, as well as the resistance to thermal and hydrothermal degradation are then compared for Pd1@HEFO and Pd@CeO2 catalysts to prove the advantages of HEFO as the catalyst carrier.

## Results

### Synthesis and characterizations

As illustrated in Fig. 1, six metal salt precursors (Ce, Zr, Hf, Ti, La, and Pd) are first mixed with fumed silica by ball milling. The resultant mixture is pyrolyzed at 900 °C in air to achieve the silica-templated metal oxide complex. Finally, Pd1@HEFO catalyst is obtained after etching silica with NaOH. It should be noted that the molar ratios of Ce, Zr, Hf, Ti, and La are approximately 1:1:1:1:1 confirmed by both EDS and inductively coupled plasma (ICP) results listed in Supplementary Table 1. The high surface-area HEFO is synthesized through the same steps without the addition of Pd precursor; Pd@CeO2 counterpart is prepared by the same method; the single-phase CeO2, TiO2, ZrO2, La2O3, and HfO2 are obtained from facile pyrolysis of their corresponding metal salts at 900 °C.

Powder X-ray diffraction (PXRD) (Fig. 2a) is performed to demonstrate the crystalline structure of HEFO and its corresponding single metal oxides. The cubic CeO2 (c-CeO2), monoclinic ZrO2 (m-ZrO2), monoclinic HfO2 (m-HfO2), tetragonal TiO2 (t-TiO2), and tetragonal La2O3 (t-La2O3) are observed for the single metal oxides, respectively. Interestingly, HEFO exhibits only five obvious broad peaks centered at 30.2, 34.8, 50.2, 60.1, and 62.6°, corresponding to (111), (200), (220), (311), and (222) planes of a single cubic phase. The absence of diffraction peaks indexed to m-ZrO2, m-HfO2, t-TiO2, and t-La2O3 indicates that Zr, Hf, Ti, and La are all incorporated into c-CeO2 to form a new high-entropy (CeZrHfTiLa)Ox solid solution (HEFO). Moreover, Zr4+, Hf4+, and Ti4+ except for La3+ have a smaller ion radius than Ce4+, thus resulting in an obvious shift of diffraction peaks of HEFO to a higher 2θ value compared with c-CeO2. The structural and chemical uniformity of HEFO is further evidenced by high-resolution TEM (HRTEM) and fast Fourier transfer (FFT, Fig. 2j) images, which show well-defined lattice fringes without the secondary phases. In addition, EDS-mapping results show the highly homogeneous dispersion of randomly-distributed five metal signals including Ce, Zr, Hf, Ti, and La (Fig. 2c–i), which also unambiguously suggests the formation of the high-entropy cubic phase of HEFO on nanometer scale. N2 adsorption–desorption isotherm and corresponding pore size distribution (Supplementary Figs. 1 and 2) of HEFO exhibit the emergency of rich porosity due to removal of hard-template SiO2 with a high specific surface area of 162.1 m2 g−1 (Supplementary Table 2). This porous structure of HEFO makes it a suitable candidate to be a catalyst carrier. The surface components of HEFO is mainly dominated by Zr4+, Hf4+, Ti4+, Ce4+, and La3+ shown by X-ray photoelectron spectroscopy (XPS, Supplementary Fig. 3) analysis, which indicates partial removal of oxygen in (CeZrHfTiLa)Ox (x < 2) crystal after incorporation of La compared with c-CeO2. The schematic model of cubic HEFO is then constructed (Fig. 2k) based on the above results, where the Ce atoms in c-CeO2 is randomly populated by Zr, Hf, Ti, and La atoms.

After introducing 0.5–2 wt% Pd during the synthesis of HEFO, the HEFO crystalline phase is well retained without the appearance of any additional diffraction peaks in Fig. 2b. More importantly, the absence of diffraction peaks ascribed to Pd species and the shift of diffraction peaks with the increases of Pd loading (Fig. 2b) suggests that a large portion of Pd may be incorporated into the HEFO sublattice for the  formation of (PdyCeZrHfTiLa)Ox solid solution. After the introduction of Pd with different weight loading, the surface area and pore volume of Pd1@HEFO-x slightly decrease compared with pristine HEFO carrier (Supplementary Table 2). Fortunately, the surface area, pore size distribution and crystalline structure of Pd1@HEFO stay almost unchanged after both thermal and hydrothermal treatment (Supplementary Figs. 1, 2, and 4). The EDS-mapping results of Pd1@HEFO in Fig. 3a–h suggest the uniform element distribution of Pd, Ce, Zr, Hf, Ti, and La. More importantly, the agglomeration and sintering of Pd species are not observed in Pd1@HEFO (Fig. 3b), indicating the possible existence of isolated Pd sites. The HRTEM image in Fig. 3i only depicts randomly oriented lattice spacing belonging to the HEFO phase. Consistent with EDS-mapping and HRTEM results, FFT pattern in Fig. 3i (inset) again reveals the diffraction rings from (111), (200), (220), (311), and (222), attributed to the face-centered cubic (CeZrHfTiLa)Ox solid solution structure without diffraction rings ascribed to any Pd species. The above results confirm the existence of isolated Pd atoms, but the microenvironment of Pd still requires further exploration. In addition, TEM images of HEFO and Pd1@HEFO (Supplementary Fig. 5) display similar morphologies and the grains size distributions for both are centered at around 4 nm. This suggests that the morphology and particle size of HEFO will not change after the introduction of Pd. Furthermore, the chemical state of Pd in Pd1@HEFO is then investigated by XPS analysis, and the obtained binding energy (Supplementary Fig. 6) is the characteristic of electron-deficient Pd4+25,26,27. This formation of electron-deficient Pd4+ may be attributed to the electron transfer from Pd to M through Pd–O–M bonds (M = Ce, Zr, Hf, Ti, and La) in (PdyCeZrHfTiLa)Ox solid solution.

The formation of single Pd atoms is further confirmed by atomic-resolution TEM image (Fig. 4a) and the corresponding Pd EDS-mapping image (Fig. 4b). The absence of Pd atoms outside HEFO lattice (Fig. 4a) and around 6.44% surface Pd atoms determined by CO chemisorption (0.0644 μmol CO/μmol Pd, Supplementary Table 1) together indicate that the Pd atoms have been incorporated into both surface and bulk HEFO phase in Pd1@HEFO, consistent with the reported phenomena that single platinum-group metal atoms prefer to substitute cerium atoms of CeO2 rather than adsorb on its surface28. To confirm the electronic structure and coordination state of Pd in Pd1@HEFO, the X-ray absorption near-edge structure (XANES) and EXAFS measurements are performed at the Pd K-edge. XANES spectra show that the Pd K-edge absorption edge for Pd1@HEFO located between that of Pd foil and PdO (Fig. 4d), revealing the valence state of Pd is between 0 and +2, which is lower than +4 of the surface Pd from XPS. This is probably attributed to the fact that the surface Pd atoms are more likely to be contacted with oxygen and be oxidized at high temperatures. Fourier-transformed k3-weighted EXAFS spectra (Fig. 4e and Supplementary Table 3) exhibit the obvious Pd–Pd (bond length = 2.74 Å) and Pd–O–Pd (bond lengths = 3.06 and 3.44 Å) features for Pd foil and PdO references, respectively, which are both absent in Pd1@HEFO. As an alternative, the bond lengths at 3.01 and 3.26 Å corresponding to Pd–O–Zr and Pd–O–M (M = Ce/La) are identified in Pd1@HEFO (Supplementary Table 3), illustrating the existence of isolated Pdx+ (0 < x < 2) in proximity to Zr, Ce, or La atoms29,30,31. The wavelet transform plot (Fig. 4f) of Pd1@HEFO shows the wavelet transform maximum at ~10 Å−1, which corresponds to the Pd–O–Zr and Pd–O–M (M = Ce/La) bonding by comparing Pd foil and PdO counterparts and the intensity maxima of Pd–O–Ti at ca. 7 Å−1 and Pd–O–Hf at above 12 Å−132,33. Moreover, no intensity maxima corresponding to Pd−Pd and Pd–O–Pd is found, which matches well with the EXAFS fitting results in R space. Consequently, a possible schematic model of Pd1@HEFO (220) is shown in Fig. 4c.

Operando diffuse reflectance infrared Fourier transform spectroscopy (DRIFTS) upon CO adsorption in Fig. 5a is then employed to examine the coordination environment of Pd in Pd1@HEFO and Pd@CeO2. To strengthen the CO adsorption on Pd sites, HEFO, Pd1@HEFO, and Pd@CeO2 are reduced in situ at 250 °C in the DRIFTS cell before exposure to CO flow. For HEFO, the absence of FTIR bands in Fig. 4a suggests the surface of HEFO is not capable of adsorbing CO molecules. In comparison, CO frequencies between 2200 and 2000 cm−1 are clearly seen in Pd1@HEFO, which is assignable to CO molecules linearly adsorbed on single-atom Pd species34,35. The bridge and hollow-CO bands are not seen in Pd1@HEFO, indicating that Pd are atomically dispersed on the HEFO host, which agrees with HAADF-STEM and EXAFS results34,36. However, the bridge and hollow-CO peaks are obviously observed for Pd@CeO2 because of the aggregation of Pd species, thus further validating the importance of hosts for the formation of isolated Pd species37. The obvious agglomeration of Pd in Pd@CeO2 can be also evidenced by EDS-mapping results (Supplementary Fig. 7) and existence of the metallic Pd phase from PXRD pattern (Supplementary Fig. 8), in agreement with the bridge and hollow-CO peaks of DRIFTS. The chemical states of Pd in Pd@CeO2 and Pd1@HEFO are both dominated by Pd4+ based on XPS results (Supplementary Fig. 6), which suggests their similar Pd–O coordination number though totally different Pd microenvironment. As is well known, the phase stabilization is a process determined by combination of the enthalpy (H) and entropy (S) effects, which are temperature- and composition-dependent. Compared with the Pd@CeO2, Pd1@HEFO with enhanced compositional complexity provides a higher molar configurational entropy, especially for equimolar cations, which then potentially decreases the Gibbs free energy according to the equation (ΔG = ΔH−TΔS). This means that the formation of (PdyCeZrHfTiLa)Ox solid solution is an entropy-dominated process, whereas the decreased configuration entropy induces the dissociation of (PdyCe)Ox as an enthalpy-driven process. To prove this hypothesis, the PXRD patterns of Pd@ZrO2, Pd@La2O3, Pd@HfO2, Pd@TiO2, ternary Pd@CeZrTiOx, and quaternary Pd@CeZrHfTiOx samples synthesized by the same method are also collected (Supplementary Fig. 8). The diffraction peaks ascribed to metallic Pd and/or PdO can be observed, further confirming the importance of the high configurational entropy on stabilizing the Pd single atoms. We also synthesized the Pd/HEFO-p (single Pd atoms dispersed on HEFO carrier) by a post-deposition method, where the single-atom structure can be confirmed by XRD pattern and CO-DRIFTS spectra in Supplementary Fig. 9. Unfortunately, the sintering and aggregation of Pd on HEFO can be obviously observed in Pd/HEFO-p-900 after post-treatment at 900 °C, which might be ascribed to the excessive Pd density on HEFO surface.

### Catalytic performance

The oxidation of CO, a key reaction in automotive emission abatement, has been extensively investigated in the past decades38,39,40,41. Therefore, the light-off curves of CO oxidation are measured to evaluate the catalytic efficiency of our as-obtained samples. As depicted in Fig. 5d, HEFO exhibits an inferior catalytic activity of CO oxidation with a high onset temperature of 230 °C. After doping 1 wt% Pd, Pd1@HEFO shows a dramatically enhanced reactivity with the onset temperature as low as ~80 °C and complete CO oxidation at 170 °C. In comparison, the onset temperature and T100 over Pd@CeO2 are 223 and 253 °C, respectively, much higher than those of Pd1@HEFO. It is generally accepted that metal on reducible carrier (CeO2) follows a Mars–van Krevelen reaction mechanism, where CO adsorbed on metals reacts with active lattice O from CeO2 to form oxygen vacancies42,43. Therefore, the reducibility of the surface lattice O from the carrier plays an important role in catalytic CO oxidation. For Pd@CeO2, the only reduction peak observed at around 250 °C is assigned to the reduction of Pd–O–Pd (PdOx) and the surface lattice oxygen in CeO244,45. In contrast, the surface lattice O of HEFO in the vicinity of Pd (Pd–O–M) is easier to be activated for Pd1@HEFO compared with Pd–O–Pd for Pd@CeO2, which offers a reduction temperature centered at 160 °C. The enhanced reducibility of the surface lattice O in Pd1@HEFO should be the main cause for its higher catalytic activity. Moreover, XPS spectra of O 1 s in Fig. 5c show that the ratio of the surface chemisorbed oxygen (Oβ, 530.4 eV) to the support’s lattice oxygen (Oα, 528.8 eV) of Pd1@HEFO is about twofold higher than that of Pd@CeO2, which might be ascribed to the existence of more under-coordinated metal cations due to the incorporation of Pd into HEFO46,47, consistent with the surface concentration of Ce3+ in Supplementary Fig. 10. These as-formed under-coordinated sites, namely oxygen vacancies, in Pd1@HEFO would render more habitation for O2 dissociation adsorption41. Combined CO-TPR with O 1s XPS results, the improved reducibility of partial surface lattice oxygen in vicinity of Pd and enhanced oxygen vacancies in Pd1@HEFO should be the main cause for its superior catalytic performance. The apparent activation energies (Ea) of Pd@CeO2 and Pd1@HEFO were calculated, as shown in Fig. 5e. Pd1@HEFO has an Ea value of 43.40 kJ/mol, which is much lower than that of Pd@CeO2 (72.21 kJ/mol), further identify the advantage of Pd1@HEFO catalyst. As shown in Fig. 5f, the cycled measurement of CO oxidation over Pd1@HEFO and time-on-stream test at 170 °C (inset) reveal the outstanding stability of Pd1@HEFO. Since water vapor is usually present in vehicle exhaust, we thereafter examine the hydrothermal stability of both Pd@CeO2 and Pd1@HEFO catalysts by treating them at 750 °C for 10 h before the activity test. After hydrothermal treatment, the textural and structural properties of Pd1@HEFO–HA remain almost unchanged (Supplementary Table 2 and Fig. 5). Correspondingly, all elements are still uniformly dispersed without agglomeration and sintering of Pd species from the EDS-mapping result in Supplementary Fig. 11. More importantly, the absence of the bridge and hollow-CO peaks further validates that single-atom Pd in Pd1@HEFO–HA is stable under hydrothermal conditions (Supplementary Fig. 12). Consequently, the complete conversion temperature of CO barely changes after the hydrothermal treatment in Fig. 5d and even 10 vol% H2O in the feed gas (Pd1@HEFO-H2O, Supplementary Fig. 13). The increase of low-temperature catalytic activity of Pd1@HEFO–HA and Pd1@HEFO-H2O (Supplementary Fig. 13) is probably ascribed to the formation of activated surface chemisorbed oxygen (Oβ) on HEFO, reported in the previous study41. However, the catalytic activity of Pd@CeO2–HA obviously decreases compared with its fresh counterpart due to the existence sintering of Pd species, evidenced by the decreased linear-CO and increased bridge and hollow-CO peaks of Pd@CeO2–HA (Supplementary Fig. 12). In addition, Pd1@HEFO not only exhibits better thermal and hydrothermal stability than Pd@CeO2 in this work, but also shows better or comparable performance relative to other reported representative catalysts of CO oxidation20,41,48,49. More importantly, Pd1@HEFO exhibits simultaneously outstanding oxidation activities of CO, C3H6, and NO at a high gas-hourly space velocity (GHSV) of 200,000 mL gcat−1 h−1 (Supplementary Fig. 14a), although the T100 of CO oxidation shifts to ca. 260 °C due to the co-presence of C3H6 and NO at a high GHSV. The catalytic performance of Pd1@HEFO is comparable to Pt/CeO2–SiAlOx regarded as a candidate of diesel oxidation catalyst (DOC)50 and Pt/CeO240. Moreover, no obvious deactivation of CO, C3H6, and NO oxidation can be observed over Pd1@HEFO even after 10 h of reaction in Supplementary Fig. 14b, implying that Pd1@HEFO shows a good DOC activity and stability. PXRD patterns of Pd1@HEFO treated in H2 at different temperatures (Supplementary Fig. 15) suggest that Pd atoms in Pd1@HEFO are not stable in reductive atmosphere. As a result, our Pd1@HEFO is more suitable for the oxidation reaction under the oxygen-rich conditions, such as catalytic destruction of pollutions emitted from diesel engines. These illustrate that our Pd1@HEFO possesses not only outstanding low-temperature CO oxidation activity but also excellent resistance to hydrothermal degradation as a candidate of DOC, thus possibly tolerating the harsh conditions during exhaust treatment of diesel engines.

## Discussion

In summary, we have developed a solid-state strategy to synthesize a sintering-resistant Pd single-atom catalyst stabilized on HEFO (Pd1@HEFO). The as-synthesized single-atom Pd catalyst displays not only superior CO oxidation activity but also outstanding resistance to thermal and hydrothermal degradation compared with Pd@CeO2 counterpart prepared using the same method. The choice of host in this work plays a paramount role on the synthesis of single-atom Pd catalysts, which can only be realized with HEFO as the carrier because of its maximum configurational entropy. This trait induces Pd to be incorporated into the HEFO sublattice during the mechanochemical-assisted preparation process, and the above process cannot be accomplished with CeO2 as an alternative carrier. This work provides a solvent-free entropy-driven methodology for the synthesis of SACs and may guide the development of next-generation SACs.

## Methods

### Synthesis of HEFO and Pd1@HEFO

Ce(OOCCH3)3 (AR, ACROS, USA), ZrCl4 (98%+, Alfa Aesar, USA), HfCl4 (97.0%, ACROS, USA), La(NO3)3 (AR, ACROS, USA), TiOSO4 (99.0%, ACROS, USA), K2PdCl6.xH2O (99.9%, ALDRICH, USA), and fumed silica (99.9%, ALDRICH, USA) equaled to the total weights of the above five metal precursors were massed and added to a commercially available 25 mL screw-capped zirconia vial reactor along with five zirconia balls. The reactor was placed in a high-speed vibrating ball miller (1800 rounds min−1, 300 W motor power) and the mixtures were ball milled twice for 30 min each time. The resulting powder product (Pd@CeZrHfTiLaOx@SiO2) was pyrolyzed at 900 °C with a heating rate of 2 °C min−1 for 4 h under air in a tube furnace and cooled down the room temperature, to obtain the sample named as Pd1@HEFO@SiO2, and then it was stirred in 2.5 M NaOH for 8 h at room temperature and then washed with deionized water, repeating the process four times to remove the silica template, followed by drying at vacuum conditions at 40 °C overnight, finally achieved the porous Pd1@HEFO samples. Pd1@HEFO with different Pd loading (0.5, 1.0, 1.5, and 2.0 wt% Pd) were prepared according to the same above steps, denoted as Pd1@HEFO-0.5, Pd1@HEFO-1.0, Pd1@HEFO-1.5, Pd1@HEFO-2.0, respectively. Pd1@HEFO-1.0 was chosen to be as the representative sample to investigate the role of HEFO on the formation of the stabled Pd SACs, which was further briefly labeled as Pd1@HEFO. HEFO sample was prepared by the same steps as Pd1@HEFO, without K2PdCl6. Pd@CeO2, Pd@ZrO2, Pd@HfO2, Pd@TiO2, Pd@La2O3, Pd@CeZrTiOx, and Pd@CeZrHfTiOx were also prepared by the same steps as Pd1@HEFO. Pd1@HEFO and Pd@CeO2 samples were treated under 10 vol% water vapor in N2 at 750 °C for 10 h and named as Pd1@HEFO–HA and Pd@CeO2–HA. Pd1@HEFO sample was also treated under 2 vol% H2 in He at 250 °C for 2 h and named as Pd1@HEFO-H2.

### Synthesis of Pd/HEFO-p

The post-deposition of Pd atoms onto HEFO was obtained by the following typical steps: 0.5 g the pre-synthesized HEFO powder was dispersed in deionized water with rigorous stirring. An appropriate amount of H2PdCl6 (K2PdCl6 dissolved in diluted hydrochloric acid, corresponding to a Pd loading of 0.5 wt%) solution was added dropwise into the HEFO solution under magnetically stirring51. After continuing stirring for 5 h and followed by aging for 5 h, the suspension was filtered and washed with deionized water for several times, and dried at 60 °C under vacuum52 and then calcined at 300 and 900 °C in air for 2 h, respectively, denoted as Pd/HEFO-p and Pd/HEFO-p-900.

### Characterizations

X-ray diffraction (XRD) data were recorded on a PANalytical Empyrean diffractometer with a Cu-Kα radiation source in the 2θ range of 20–80°. The nitrogen adsorption and desorption isotherms were measured at 77 K under a Gemini VII surface-area analyzer. Samples were degassed for 6 h under N2 at 160 °C prior to the measurement. High-resolution transmission electron microscopy (HRTEM), high-angle annular dark-field scanning transmission electron microscopy (HAADF-STEM) and the corresponding energy-dispersive X-ray spectroscopy (EDS) were conducted on an aberration-corrected Titan S 80-300 (FEI) with an accelerating 300 kV voltage.

The X-ray absorption spectra (XAS) were collected on the beamline BL01C1 in National Synchrotron Radiation Research Center (NSRRC), with electron energy of 1.5 GeV and a beam current between 100 and 200 mA, and XAS data were collected at treatment temperatures. The radiation was monochromatized by a Si (111) double-crystal monochromator. XANES and EXAFS data reduction and analysis were processed by Athena software. More details on the fitting process are given in the figure legend or table footnote.

In situ diffuse reflectance infrared Fourier transform spectra (DRIFTS) were collected at 30 °C with a Thermo Nicolet 6700 spectrometer equipped with a mercury cadmium telluride (MCT) detector accumulated at a resolution of 4 cm−1 in 100 scans. Fifty milligrams of samples were preconditioned in situ at 400 °C under He (99.999%) for 30 min and then cooled to 250 °C to be reduced for 30 min in 5 vol% H2/N2 (30 mL min−1). Finally, the sample was cooled to 30 °C prior to recording the background spectra and exposed to 1 vol% CO/N2 flow until no change of the spectrum, and the CO adsorption spectrum was collected after purging in He.

X-ray photoelectron spectroscopy (XPS) measurements were performed with a Kratos XSAM-800 Kα instrument. Peak fitting was performed using CasaXPS software (v 2.3.18). The C 1s peak (284.6 eV) was used for the calibration.

The pulse CO chemisorption was measured by Micromeritics AutoChem II 2920. Hundred milligrams of sample was reduced in H2 at 400 °C for 1 h and then the sample was cleaned by He for 1 h with a flow rate of 30 ml min−1. Then, the CO was injected (11.10 μmol/pluse) into the catalyst in a flow of He until the amount of CO uptake was saturated. The exposed Pd atoms were evaluated from the amount of CO consumption assuming 1 molecule of CO adsorbed per surface Pd atom32.

CO temperature-programmed reduction (CO-TPR) experiments were conducted by the FTIR spectrometer (Antaris IGS, Nicolet). The powder catalyst put in flow reactor device. Fifty milligrams of sample was put in a fixed bed quartz and pretreated at 450 °C (10 °C min−1) in He for 1 h and then cooled down to room temperature. Then the sample was heated to 500 °C (5 °C min−1) under an atmosphere of 1 vol% CO in He (200 mL min−1).

O2-temperature-programmed desorption (O2-TPD) experiments were performed on a PX200 apparatus equipped with a TCD. Fifty milligrams of the sample was pretreated in a flow of N2 (20 mL min−1) at 400 °C for 30 min and then cooled to 80 °C. The adsorption was carried out by 5 vol% O2–95 vol% N2 (30 mL min−1) at 80 °C for 30 min. Then the samples were swept at 80 °C for 60 min by He. The desorption was detected from 80 to 400 °C with a heating rate of 5 °C min−1.

### CO oxidation activity measurement

CO oxidation reaction was performed in the same manner as our previous work5. The outlet concentrations of CO and CO2 were analyzed using an on-line gas chromatograph (Buck Scientific 910) equipped with a dual molecular sieve/porous polymer column (Alltech CTR1) with a thermal conductivity detector.

The apparent activation energy was calculated using the Arrhenius law (k = Aexp(−Ea/RT)). Ea was obtained from the slope of the linear plot of ln(k) versus 1000/T and the value of k was calculated using the following equation:

$$k = (V \times X)/m$$

Where, V is the total gas flow (mL·s−1) at temperature T (K), X is the CO conversion (%), and m is the catalyst mass in the reactor (g). In this work, the weights of Pd1@HEFO and Pd@CeO2 are both 10 mg.

### DOC catalytic activity measurement

The DOC catalytic activity evaluation of Pd1@HEFO was performed according to the previous work49. A catalyst loading of 150 mg at a gas-hourly space velocity (GHSV) of 200,000 mL gcat−1 h−1 with the total gas flow rate of 500 ml min−1 was used. The outlet flows of CO, C3H6, NO, and NO2 were analyzed using a Nicolet Antaris IGS-6700 gas analyzer (Thermo Fisher Scientific, USA).