Skip to main content

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.

Controlling hot electron flux and catalytic selectivity with nanoscale metal-oxide interfaces

Abstract

Interaction between metal and oxides is an important molecular-level factor that influences the selectivity of a desirable reaction. Therefore, designing a heterogeneous catalyst where metal-oxide interfaces are well-formed is important for understanding selectivity and surface electronic excitation at the interface. Here, we utilized a nanoscale catalytic Schottky diode from Pt nanowire arrays on TiO2 that forms a nanoscale Pt-TiO2 interface to determine the influence of the metal-oxide interface on catalytic selectivity, thereby affecting hot electron excitation; this demonstrated the real-time detection of hot electron flow generated under an exothermic methanol oxidation reaction. The selectivity to methyl formate and hot electron generation was obtained on nanoscale Pt nanowires/TiO2, which exhibited ~2 times higher partial oxidation selectivity and ~3 times higher chemicurrent yield compared to a diode based on Pt film. By utilizing various Pt/TiO2 nanostructures, we found that the ratio of interface to metal sites significantly affects the selectivity, thereby enhancing chemicurrent yield in methanol oxidation. Density function theory (DFT) calculations show that formation of the Pt-TiO2 interface showed that selectivity to methyl formate formation was much larger in Pt nanowire arrays than in Pt films because of the different reaction mechanism.

Introduction

Understanding the mechanisms of energy dissipation and electronic excitation at solid–gas interfaces on heterogeneous catalyst is important for various energy conversion applications to improve energy efficiency1,2,3,4. In particular, through exothermic catalytic reactions on a metal catalyst surface, non-adiabatic energy dissipation leads to the flow of energetic electrons with an energy of 1–3 eV (i.e., reaction-induced hot electrons) from a chemical energy conversion process; this flow of electrons operates on a femtosecond time scale before atomic vibrations dissipate the energy by adiabatic process5,6,7,8,9. However, because of the extremely short lifetime by thermalization (i.e., within a few femtoseconds via electron–electron or electron–phonon scattering) and mean free path of hot electrons in metal catalysts, directly detecting catalytically excited hot electrons before relaxation has been challenging3,8,10. Recently, metal–semiconductor Schottky nanodiodes, composed of a metal catalyst film deposited on a semiconductor substrate, have emerged as a powerful strategy for quantitative real-time detection of hot electron transfer excited on catalyst surface by exothermic chemical reactions11,12,13. When the potential barrier formed at the metal–semiconductor junctions (i.e., the Schottky barrier) is lower than the energy of the chemically excited electrons (1–3 eV) by catalytic reaction, the Schottky barrier allows excited hot electrons to irreversibly transport through the metal–semiconductor junction. Once hot electrons arrive at the semiconductor by transfer, these electrons cannot go back to the metal catalyst, leading to the irreversible and one-way hot electron transfer from the metal catalyst to the semiconductor. Therefore, metal–semiconductor catalytic nanodiodes allow the quick capture of energetic hot electrons before thermalization; the detected current is known as chemicurrent5,9,14.

In heterogeneous catalysis, one of the key strategies for enhancing the reaction rate and selectivity is the use of catalytically active metal nanoparticles supported on an oxide support, forming a metal-oxide interface15,16,17. Strong metal-support interaction (SMSI) effect, in which the encapsulation of metal nanoparticles by reducible oxide-support overlayers can affect the catalytic behavior of metal nanoparticles (i.e., migration of oxide support onto the active metal surface) was discovered by Tauster et al.18,19. Matsubu et al.20 also showed that adsorbate-functionalized encapsulation of metal nanoparticles by the reducible oxide support (e.g., TiO2 and Nb2O5) can influence the selectivity of CO2 hydrogenation in heterogeneous Rh catalysts (i.e., adsorbate-mediated SMSI effect) and these results were proved by observing changes in pre-treatment through in situ diffuse-reflectance infrared Fourier transform spectroscopy and in situ scanning transmission electron microscopy (TEM)20. Studies of low-temperature CO oxidation on gold nanoparticles on a TiO2 support catalyst exhibits that the metal-oxide interface along its perimeter can dramatically change the catalytic activity21,22. Therefore, it can be seen that the formation of metal-oxide interface in heterogeneous catalyst plays an important role in altering the catalytic reaction.

In contrast to one-path reactions such as CO or hydrogen oxidation, the research on selectivity for achieving the desired product molecule in multi-path reactions is a challenging issue; this is the ultimate goal of a heterogeneous catalyst for green chemistry4,20,23,24,25. Among the various multi-path reactions, the gas-phase methanol oxidation reaction, which produces CO2 and methyl formate by full oxidation and partial oxidation of methanol, is an important transformation process for the conversion of energy and chemical synthesis26. The partial oxidation of methanol to methyl formate is an especially efficient and environmentally benign way of producing valuable chemicals. Furthermore, it has been demonstrated that the oxidation state or chemical composition of the metal catalyst can affect the selectivity to methyl formate under methanol oxidation27,28,29. Recently, it was found that the quantity of hot electrons generated in the methanol oxidation reaction is affected by the selectivity of methyl formate production using a Pt film/TiO2 catalytic nanodiode30. In addition, previous studies have revealed that the partial oxidation of methanol increases when the metal-oxide interfacial sites (i.e., Pt/FeO and Au/TiO2) are formed by using theoretical calculation and surface science techniques31,32. Therefore, the smart design of heterogeneous catalysts can improve the selectivity of metal catalysts on reducible oxide supports (e.g., Pt nanoparticles or nanowires on oxide support substrate) by engineering the metal-oxide interface8.

In this study, to demonstrate the effect of metal-oxide interface on selectivity and reaction-induced hot electrons (i.e., chemicurrent), we fabricated a Schottky nanodiode with Pt nanowires on a TiO2 support forming nanoscale Pt-TiO2 interface that was exposed on the gas-phase reaction environment. Using the fabricated Pt nanowires/TiO2 catalytic nanodiode, we report the in situ detection of charge flow as steady-state chemicurrent generated by gas-phase catalytic methanol oxidation on the Pt nanowire catalysts supported on TiO2. To find the dynamics of reaction-induced hot electrons on the metal-oxide interface, the results of partial oxidation selectivity and chemicurrent on Pt nanowires/TiO2 were compared with the results of the Pt film/TiO2 Schottky nanodiode whose metal-oxide interface was not exposed to the environment of the gas-phase chemical reaction. We showed that formed nanoscale Pt-TiO2 interface gives rise to the higher selectivity of methyl formate, thereby hot electrons were excited much more on the Pt-TiO2 interface, as the hot electron generation was affected by selectivity under methanol oxidation. Comparing the simulation results by density functional theory (DFT) from the two models of Pt nanorod on TiO2(110) and Pt(111), we could support the increase in selectivity at the Pt-TiO2 interface due to the difference of activation barrier.

Results

Detection of hot electrons on Pt nanowires/TiO2 nanodiodes

The metal-oxide interface was fabricated on the catalytic Schottky nanodiodes by depositing the two-dimensional Pt nanowire arrays on the surface of TiO2 using lithography, thus creating a well-defined nanoscale interface between the platinum and the titanium dioxide. A previous study on lithographically fabricated Pt nanowire arrays on oxide support found strong oxide support dependence for both TOF and the activation energy of the CO oxidation reaction33,34. Thus, in this study, the Pt nanowire arrays were chosen to form the metal-oxide interface, because these nanowires can be deposited on the TiO2, while sustaining the electrical connection for the fabrication of Schottky nanodevices when exposing the well-defined Pt-TiO2 interface to the reaction environment. A scheme of the fabricated catalytic nanodiode is presented in Fig. 1a, where the two-dimensional Pt nanowire arrays were deposited on the thin-film TiO2 surface, forming a Pt nanowires/TiO2 catalytic nanodiode. The figure in the inset shows that methanol oxidation occurs at the metal-oxide interface formed by the deposition of Pt nanowires on a TiO2 surface. The Schottky nanodevice was well-constructed, the width of the Pt nanowires was 20 nm, and the pitch of the nanowire arrays was 50 nm, as shown in scanning electron microscopy (SEM) image.

Fig. 1: Detection of hot electrons generated on Pt nanowires/TiO2 nanodiode.
figure 1

a Schematic of hot electron generation on the Pt nanowires/TiO2 catalytic nanodiode during exothermic methanol oxidation. Methanol oxidation occurs, and CO2 and methyl formate are produced at the Pt-TiO2 interface formed by the bonding of Pt nanowires and TiO2. In this process, non-adiabatic energy dissipation occurs and hot electrons are generated on the nanodiode surface. SEM image of Pt nanowire arrays with a width of 20 nm and a pitch of 50 nm. b Energy band diagram for Schottky nanodiode of the Pt nanowires supported on TiO2. Hot electrons excited from the surface chemical reaction can be detected as a steady-state chemicurrent by charge transfer if their excess chemical energy is large enough to overcome the Schottky barrier of the Pt-TiO2 junction. c TEM image of the transferred Pt nanowire arrays on TEM grid with a width of 20 nm. d Current–voltage (IV) curves for the Pt nanowires/TiO2 catalytic nanodiode. The solid line is a fit of the obtained IV curve to the thermionic emission theory. The obtained Schottky barrier height was 0.85 eV. e Current density associated with the methanol oxidation measured on the Pt nanowires/TiO2 with increased reaction temperature. The differences in the magnitude of the currents measured with and without catalytic reaction were associated with reaction-induced hot electrons generated on the catalytic nanodiode (i.e., net chemicurrent).

The energy band diagram for real-time detection of hot electron flux as steady-state chemicurrent under methanol oxidation on Pt nanowires/TiO2 catalytic nanodiode is illustrated in Fig. 1b. Here, a Au/Ti film layer for the ohmic contact electrodes of the nanodiodes on both sides is deposited by electron beam evaporation. As a probe reaction, methanol oxidation showing two reaction products (i.e., CO2 and methyl formate production by full oxidation and partial oxidation of methanol reactant, respectively) was chosen, as it is an exothermic reaction with low temperature that is stable for maintaining the electrical properties of the catalytic nanodiode. When methanol oxidation, as an exothermic catalytic reaction, occurs in the catalyst, hot electrons were generated by non-adiabatic electronic excitation (i.e., chemical energy conversion) and only energetic electrons can be detected through the Schottky barrier formed at the metal–semiconductor junction as the electric current (i.e., chemical reaction-induced current flow).

To characterize the microstructure of Pt nanowires using TEM, the fabricated Pt nanowires were directly transferred onto a TEM grid in the same way that they were transferred to the nanodiodes for TEM sampling, as shown in Fig. 1c. Larger Pt nanowires with a width of 200 nm were observed between smaller Pt nanowires with a width of 20 nm. The formation of larger Pt nanowires was influenced by the topographical template required to control the long-range order of self-assembled block copolymer patterns35,36. Thus, we confirmed that the fabricated catalytic nanodiode was well designed, and that the junction formed between the Pt nanowire arrays and TiO2 was stable.

To investigate the electrical properties and rectifying behavior of the fabricated Pt nanowires/TiO2 catalytic nanodiode, current–voltage (IV) curves were plotted. As shown in Fig. 1d, by fitting the IV curve of the nanodiode to the thermionic emission equation, a Schottky barrier of 0.85 eV was obtained, which was similar to that of the device based on Pt film (see Supplementary Note 1 for details). Thus, the effect of Schottky barrier height on the hot electron detection can be excluded by showing a similar Schottky barrier to that of the Pt film (i.e., about 0.87 and 0.85 eV for Pt film/TiO2 and Pt nanowires/TiO2, respectively). Recently, the detection of excited hot electrons as a steady-state chemicurrent under the catalytic oxidation of CO or hydrogen was demonstrated by using metal catalyst/TiO2 Schottky nanodiodes and a clear correlation was found between catalytic activity and reaction-induced hot electron flux10,37,38,39,40,41. In this study, the chemically excited hot electrons generated by methanol oxidation were enough to irreversibly overcome the Schottky barrier at the Pt nanowire arrays/TiO2 junction when the excess chemical energy was higher than the Schottky barrier height of the nanodiode (i.e., obtained sufficient energy) and could be detected as a current of hot electron flow.

The fabrication procedure of patterned Pt nanowire arrays on a TiO2 support with self-assembled block copolymer is shown in Supplementary Fig. 1. Bulk Au nanowires, 200 nm, were printed on the Pt nanowires to prevent electrical shorts from defects in the Pt nanowires (Supplementary Fig. 2a). As the bulk Au nanowires were much larger than the Pt nanowire arrays, the Au nanowire arrays had no effect on the catalytic reaction. Moreover, X-ray photoelectron spectroscopy (XPS) was used to demonstrate the chemical composition of Pt nanowires on TiO2, showing that the oxidation state was maintained in a metallic state (Supplementary Fig. 2b). In addition, X-ray diffraction (XRD) patterns of the Pt nanowires deposited on silicon wafer exhibited the polycrystalline nature of the transferred Pt nanowires (Supplementary Fig. 2c). To demonstrate the area density effect of the metal-oxide interface, nanodiodes were fabricated by depositing Pt nanowire arrays with widths of 15, 20, and 50 nm on a TiO2 support; the morphology of these deposited Pt nanowire arrays and Pt film was confirmed by SEM (Supplementary Fig. 3a–d).

We monitored the electric current signals flowing across the Pt nanowires/TiO2 Schottky contact at the open circuit by ammeter during reaction conditions (methanol 1–4 Torr and O2 to 760 Torr) and non-reactive conditions (pure O2 760 Torr) at elevated temperatures. The stable steady-state current signals on a Pt nanowires/TiO2 Schottky nanodiode by catalytic methanol oxidation with elevated reaction temperatures are shown in Fig. 1e, where the measured electric current increased as the reaction activity increased with rising temperature. Under a pure oxygen environment (760 Torr of O2), there was a weak thermoelectric current caused by the difference in electrical potential between the two electrodes (i.e., Seebeck effect)41. A definite deviation between the currents measured with and without catalytic reaction was observed and the difference in magnitude of the currents was clearly associated with hot electron generation from the catalytic methanol oxidation on the Pt-TiO2 interface. Therefore, this result suggests that chemicurrent measurement by using the Pt nanowires/TiO2 catalytic nanodiodes can indeed be used to monitor the surface chemical reaction at the metal-oxide interface in a quantitative and sensitive manner. Pt nanowires/TiO2 catalytic nanodiodes exhibit good thermal stability, showing a stable steady-state chemicurrent due to electrical stability under oxygen-rich conditions (see Supplementary Note 2 and Supplementary Figs. 47 for details).

Effect of metal-oxide interface on selectivity

Recently, it was observed that selectivity of partial oxidation in the methanol oxidation reaction exhibited a significant increase when the Pt-TiO2 interface was formed, which was well supported by theoretical calculations42,43. Thus, in this study, to find the metal-oxide interface effect on selectivity and reaction-induced hot electron, the results of Pt nanowire/TiO2 were compared with a Pt film/TiO2 without an exposed metal-oxide interface. We calculated turnover frequency (TOF) for CO2 and methyl formate production from the slope of the turnover number with reaction time carried out in a batch reactor system (Supplementary Fig. 8a). The selectivity to methyl formate formation was then calculated from the ratio of formation rate of methyl formate to CO2; the selectivity to produce methyl formate decreases with increasing temperature, which is similar to the tendency in our previous results of Pt film/TiO2 catalytic nanodiode (Supplementary Fig. 8b). The decline of selectivity with rising temperature was a result of the higher activation energy for full oxidation pathway than partial oxidation26. All TOF and selectivity were obtained in methanol conversion of less than 10%. As shown in Fig. 2a, the total TOF value (i.e., the sum of the TOFs of CO2 and methyl formate production) was similar for Pt nanowires/TiO2 and Pt film/TiO2. Through this, it can be seen that the Pt-TiO2 interface formed from Pt nanowires/TiO2 does not affect the total reactivity. Unlike the TOF results, surprisingly, Pt nanowires/TiO2 showed much higher selectivity toward methyl formate formation than Pt film/TiO2; these results clearly indicate that the Pt-TiO2 interface affects the selectivity of the chemical reaction, which is similar to previously reported results (Fig. 2b)43. Therefore, this indicates that when the Pt-TiO2 interface was formed, CO2 production was reduced and methyl formate production was increased, resulting in significant increase in selectivity, whereas total TOF was similar in both systems; thus, it can be said that Pt nanowires/TiO2 was a more efficient catalyst for selective reaction producing methyl formate than Pt film/TiO2. All the TOF values obtained from Pt film/TiO2 and Pt nanowires/TiO2, and the calculated selectivity are shown in Supplementary Tables 1 and 2, respectively. There have been previous studies to increase catalytic performance by increasing coverage degree of metal nanocatalyst at interfacial sites when metal nanoparticles were supported by TiO244,45,46. In addition, earlier catalytic studies on two-dimensional Pt nanowire arrays deposited on reducible support (e.g., CeO2 and ZrO2) demonstrated increased catalytic activity on Pt nanowires with nanoscale metal-oxide interfaces than in Pt film or Pt(111) single crystal surface33. Therefore, in this study, we conclude that much-improved selectivity in our two-dimensional TiO2 supported Pt nanowire arrays is associated with the nanoscale interfacial sites formed between Pt nanowires and TiO2.

Fig. 2: Selectivity and hot electron generation on nanodiodes.
figure 2

Comparison of a total reactivity and b partial oxidation selectivity under methanol oxidation for two Schottky nanodiodes of Pt film and Pt nanowires supported on TiO2 at different temperatures. c Plot of selectivity according to methanol conversion on the catalytic nanodiodes of Pt film/TiO2 and Pt nanowires/TiO2 measured at 343 K. d Chemicurrent yield associated with the efficiency for hot electron flow obtained from the Pt film/TiO2 and Pt nanowires/TiO2 catalytic nanodiodes during methanol oxidation reaction. e Selectivity to methyl formate and f chemicurrent yield under methanol oxidation on the Schottky nanodiodes with different oxide support or stack order of nanowires. All results were obtained under methanol 4 Torr and O2 to 760 Torr.

To more clearly show the selectivity differences and assess these differences on Pt nanowires/TiO2 and Pt film/TiO2, the selectivity according to methanol conversion at 343 K was plotted, as shown in Fig. 2c. We divided the regions for each section of conversion, calculated the TOF for each CO2 and methyl formate production, then calculated selectivity and compared them in Pt nanowires/TiO2 and Pt film/TiO2. The selectivity of each catalyst according to methanol conversion was almost constant, which means that the reaction kinetics of methanol oxidation were constant within this comparable methanol conversion region. In addition, when comparing selectivity obtained from Pt nanowires/TiO2 and Pt film/TiO2, it was found that Pt nanowires/TiO2 with Pt-TiO2 interface showed higher selectivity in all methanol conversion regions. Plots of selectivity vs. conversion measured at 353 K were also shown in the Supplementary Fig. 9 and higher selectivity was observed for Pt nanowires/TiO2 catalyst in all conversion regions at this temperature. Through this comparison of selectivity according to conversion, it can be seen that the metal-oxide interface plays a critical role in enhancing selectivity within the comparable methanol conversion region.

Efficiency comparison of hot electron generation

To elucidate the unique electronic structures of the nanoscale metal-oxide interface, we calculated the efficiency of the hot electrons produced by the chemical reaction using the chemicurrent and reactivity results. As the measured current of reaction-induced hot electron is linearly proportional to the reactivity30,47, the chemicurrent generated by the catalytic methanol oxidation on the catalytic nanodiode can be described as Eq. (1)

$$I = \alpha qAN_{{\mathrm{Pt}}}{\mathrm{TOF}}$$
(1)

where α is the chemicurrent yield, q is the elementary charge, A is the active area of the Pt catalyst, NPt is the number of Pt sites per mm2, and TOF is the rate of methanol oxidation10. Therefore, we can obtain the chemicurrent yield, which is the probability of non-adiabatic electronic excitation forming one molecule of the product during a chemical reaction (i.e., the number of hot electrons captured per unit chemical reaction on the nanodiode surface). As shown in Fig. 2d, the chemicurrent yield, the efficiency of hot electron generation on the catalyst surface was compared for two cases. There was a reasonable chemicurrent density in Pt film/TiO2 nanodiode, but it can be said that the reaction occurred completely on the Pt surface in the Pt film because the interfacial sites were not exposed to the methanol oxidation environment. In the Pt film/TiO2, the thickness of the Pt film was 5 nm, making the effect of the substrate negligible (see Supplementary Note 3 for details). Selectivity was low in Pt film without Pt-TiO2 interface (Fig. 2b, c), which resulted in a smaller hot electron excitation than in Pt nanowires/TiO2 nanodiode. In addition, all the experimental results (e.g., TOF, chemicurrent density, and chemicurrent yield) were calibrated to the surface area of Pt. The number of Pt sites for nanowire arrays was calculated by geometrical assumptions (e.g., the Pt nanowire was considered to be rectangular and standing upright on a planar oxide support); therefore, the surface area effect of nanowires can be excluded. As demonstrated by the previous results in the Pt film/TiO2 nanodiode, there is a significant influence of selectivity to chemicurrent yield (i.e., as selectivity to methyl formate increased, the generation of hot electrons was enhanced); due to this fact, the chemicurrent yield of Pt nanowires/TiO2 was higher than Pt film/TiO2, owing to the higher selectivity of Pt nanowires/TiO2 that have an exposed Pt-TiO2 interface. We note that in our previous research, we found that hot electrons are generated much more in the reaction to methyl formate than CO230 and it can be concluded that enhanced hot electron excitation obtained on Pt nanowires/TiO2 indeed originates from their improved selectivity on nanoscale Pt-TiO2 interfacial sites. Recently, we fabricated a Schottky nanodiode that formed a Pt/CoO interface and reported a significant increase in catalytic activity and hot electron excitation by hydrogen oxidation48,49. Thus, the improved partial oxidation selectivity when Pt nanowires were supported on TiO2 can be attributed to the Pt-TiO2 interfacial sites formed in the nanodiode, and owing to this increased selectivity, the efficiency of hot electron excitation was enhanced. Hence, the most striking finding of these results was that the Pt-TiO2 interface could promote the partial oxidation reaction to form methyl formate and thereby enhance the hot electron generation on the catalyst. Furthermore, from the observation of change in the chemicurrent yield according to the partial pressure of methanol (i.e., according to product formation), we can also demonstrate that the efficiency of hot electron excitation was greatly affected by selectivity to methyl formate, not total activity (see Supplementary Note 4 and Supplementary Figs. 10 and 11 for details). In addition, for reliable comparison between the interface effects in multi-path reactions and those in one-path reactions, we carried out comparative experiments and examined the results of TOF and chemicurrent for the Pt nanowires/TiO2 and the Pt film/TiO2 in a hydrogen oxidation reaction whose product is only water. In the hydrogen oxidation reaction (i.e., hydrogen 4 Torr and oxygen to 760 Torr), the change in activity and the efficiency of hot electron excitation by the Pt-TiO2 interface did not appear (Supplementary Note 5 and Supplementary Figs. 12 and 13), which indicates that selectivity is the key factor in influencing chemicurrent yield.

Control experiments changing stack order and oxide support

To further demonstrate the effect of the Pt-TiO2 interface, we conducted further control experiments that changed the stack order or composition of supported nanowires. This involved fabricating TiO2 nanowires/Pt inverse structure with TiO2 nanowires deposited on Pt thin film and Pt nanowires/SiO2 structure, and obtaining the selectivity and chemicurrent yield, as shown in Fig. 2e, f. We obtained and compared all the reaction data (e.g., TOF and selectivity) at each nanodiode by measuring the reaction rate at low methanol conversion (i.e., <10%) under a kinetically controlled regime (Supplementary Fig. 14). As shown in Supplementary Fig. 15a, we fabricated the inverse structure of TiO2 nanowire arrays on the Pt film/TiO2 diode with exactly the same size and period of nanowires with width of 20 nm (i.e., TiO2 nanowires (width 20 nm)/Pt film/TiO2 inverse catalytic nanodiode) to form the inverse TiO2-Pt interface. The device was constructed, as shown in Supplementary Fig. 15b, and the Schottky barrier height was 0.88 eV, which was similar to the Pt film/TiO2 and Pt nanowires/TiO2. Under methanol 4 Torr and oxygen to 760 Torr, the steady-state chemicurrent was measured, and the stability of the device under reaction condition was confirmed by checking the unchanged electrical properties (Supplementary Fig. 15c, d). As the width of the TiO2 nanowire arrays on Pt film was the same as the previous Pt nanowire arrays on the TiO2 structure, the ratio of interface to metal site was also the same for both structures (i.e., Pt nanowires (width 20 nm)/TiO2 and TiO2 nanowires (width 20 nm)/Pt film/TiO2). For this reason, the selectivity of the inverse structure was similar to those of the previous structure in which the Pt nanowires were on the TiO2 with the same width, as shown in Fig. 2e. As the selectivity in Pt nanowires/TiO2 and TiO2 nanowires/Pt was almost the same, the chemicurrent yields in both systems were also similar (Fig. 2f). Therefore, whether the Pt nanowires were on TiO2 or the TiO2 nanowires were on the Pt film, the same amount of interface ratio could not affect the selectivity or hot electron generation; if the same ratio of metal-oxide interfacial sites formed, it can be seen that the stack order had little effect on the chemical reaction and hot electron excitation was hardly affected. This control experiment in depositing TiO2 nanowires on the Pt film indicates that the nanoscale Pt-TiO2 interface plays an important role in determining selectivity and hot electron generation in methanol oxidation.

Instead of the Pt-TiO2 interface, the catalytic reaction experiment was carried out after depositing the Pt nanowire arrays on a non-reducible SiO2 support known to have little metal-support interface effect50,51. In the structure where the Pt nanowires were placed on the SiO2 support, the selectivity to produce methyl formate was not high, coming close to that of the Pt film/TiO2 (Fig. 2e). Hence, the shape and size effect of the Pt nanowires could be excluded from the results of similar selectivity for Pt nanowires/SiO2 and Pt film. Unlike on other oxide supports, previously reported results also showed similar activity to Pt nanowire arrays on SiO2 supports and to both Pt film and single Pt(111) crystals33. Through this control experiment in which Pt nanowires were deposited on SiO2, which is a non-reducible support, it was found that the Pt-TiO2 interface has a greater effect on selectivity improvement than the Pt-SiO2 interface. Pt nanowires may have exhibited different selectivity when deposited on SiO2 and TiO2 supports due to the difference in Lewis acidity between the two oxide supports52.

To demonstrate the Lewis acid/base properties of these two oxide supports in a methanol oxidation reaction environment, we investigated the charge transfer from the adsorbate to the support surface when reactant methanol molecule was adsorbed on TiO2 and SiO2 support by using DFT calculation (see Supplementary Note 6 and Supplementary Figs. 16 and 17 for calculation details). As shown in Supplementary Fig. 17, when the methanol was adsorbed on two oxide surfaces, the electron density on the methanol basis was calculated (with a negative sign indicating a loss of electrons), yielding −0.07 when adsorbed on the TiO2 surface and +0.01 when adsorbed on the SiO2 surface. This result implies that when the adsorption of methanol occurs on the two oxide surfaces, electron transfer from methanol to surface occurs on the TiO2 surface (i.e., Lewis acid) and electron transfer from surface to methanol occurs a little on the SiO2 surface (i.e., Lewis base). Therefore, through this Bader charge analysis, it was found that the Lewis acidity of TiO2 is stronger than that of the surface of SiO2 when methanol oxidation reaction occurs. Therefore, when Pt nanowires were deposited on the TiO2 support, which has a higher Lewis acidity than SiO2, it showed higher partial oxidation selectivity. A previous study also indicated that the selectivity of methyl formate production in the methanol oxidation reaction increased as the Lewis acidity of the oxide support increased when the metal catalyst was introduced to the oxide support53. As a result, it has been confirmed that the Pt-SiO2 interface had little metal-support interface effect compared to the Pt-TiO2 interface, due to the different acid/base properties of SiO2 and TiO2. Hence, the increase in selectivity only when Pt nanowires were deposited on TiO2, which was reducible support (i.e., strong Lewis acidity), rather than non-reducible SiO2, lends strong evidence to the claim that catalytic reactions occur mainly at nanoscale Pt-TiO2 interface sites.

Change of selectivity and efficiency of hot electron

Because of a lack of definitive experimental evidence, the fundamental role and effect of metal-oxide interfacial sites are still debated. To prove this hypothesis, it is necessary to observe the change in selectivity according to the ratio of the Pt-TiO2 interfacial sites. The change in selectivity as a function of the density of the metal-oxide interface provides evidence that the reaction primarily occurs at interfacial sites of metal-support when reducible oxides are used as supports for metal nanocatalysts15,54. Recently, we found a shift in catalytic activity when controlling the concentration of the metal-oxide interface under H2 oxidation and CO oxidation, indicating that higher catalytic activity was observed when more metal-oxide interfaces were created55,56. Moreover, a previous study also reported that higher butanol production selectivity was achieved by generating more metal-oxide interfaces, as the density of Pt nanoparticles on oxide support increases by changing the Langmuir–Blodgett surface pressure57. In addition, when Pt, Pd, and Ni nanocatalysts were supported by oxide, there was a previous study in which the CO oxidation reactivity increased as the size of the nanocatalysts decreased, since the ratio of interfacial sites (i.e., perimeter and corner atoms) increased as the particle size decreased17. Therefore, to further investigate the effect of the metal-oxide interface ratio, we fabricated a nanodiode based on Pt nanowire arrays with width of 15 nm; the ratio of interface to metal sites of these nanowire arrays was higher than the earlier Pt nanowire arrays with width of 20 nm. In other words, a higher ratio of Pt-TiO2 interface to metal sites could be modeled by decreasing the width of Pt nanowires. Concurrently, we fabricated the Pt nanowire arrays by increasing the width to 50 nm and depositing it on the TiO2 support to produce a catalytic nanodevice. To further observe the selectivity and hot electron excitation changes according to the width control of Pt nanowires, both the selectivity and chemicurrent yield were measured as the width of the nanowires was changed (see Supplementary Note 7 and Supplementary Figs. 18 and 21 for details).

Figure 3a–c represent the SEM image of the fabricated nanowire arrays of Pt nanowires (width 15 nm)/TiO2, Pt nanowires (width 20 nm)/TiO2, and Pt nanowires (width 50 nm)/TiO2, respectively. The selectivity and quantity of hot electron generation from methanol 4 Torr and oxygen to 760 Torr in each nanodiode were compared according to the width of Pt nanowires by adding the results from the fabricated devices (Fig. 3d, e). All the current density measured under methanol oxidation and non-reactive conditions is shown in Supplementary Fig. 22. As shown in Fig. 3d, compared to Pt film, selectivity increased when Pt nanowires were deposited on TiO2 support and it was confirmed that selectivity was enhanced as the width of the Pt nanowires decreased. As the width of Pt nanowires on TiO2 was reduced from 50 nm to 15 nm, the ratio of Pt-TiO2 interface to metal increased, which enhanced selectivity to methyl formate formation, owing to the increased ratio of interfacial sites. In addition, when comparing selectivity according to methanol conversion, the selectivity trend according to the width of nanowires was clearly shown in all methanol conversion regions (Supplementary Fig. 23).

Fig. 3: Selectivity and chemicurrent yield on nanowire arrays with different widths.
figure 3

SEM images of a Pt nanowires/TiO2 with a width of 15 nm, b Pt nanowires/TiO2 with a width of 20 nm, and c Pt nanowires/TiO2 with a width of 50 nm. Scale bars are 200 nm. d Selectivity to methyl formate under methanol oxidation on the Schottky nanodiodes at different temperatures with different widths. e Chemicurrent yield for methanol oxidation on the catalytic nanodiodes of width 15 (Pt nanowires/TiO2 with a width of 15 nm), width 20 (Pt nanowires/TiO2 with a width of 20 nm), width 50 (Pt nanowires/TiO2 with a width of 50 nm), and Pt film (Pt film/TiO2) measured both at 333 and 343 K. All results were obtained under methanol 4 Torr and O2 to 760 Torr.

As shown in Fig. 3e, when comparing the chemicurrent yield detected in catalytic nanodevices as a function of the width of Pt nanowires, it can be seen that the chemicurrent yield increased (i.e., higher efficiency for reaction-induced hot electron excitation) as the width of nanowires decreased, owing to the enhanced selectivity by the increased ratio of interfacial sites. Therefore, we can conclude that as the width of the Pt nanowires decreased, higher selectivity to methyl formate was observed due to the increased ratio of Pt-TiO2 interface, thereby enhancing hot electron excitation in catalytic nanodiodes. In all nanodiodes, the Schottky barrier height was obtained by fitting each IV curve to thermionic emission theory, as shown in Supplementary Table 3. As mentioned earlier, this Schottky barrier acts as a filter for hot electron transfer, and only energetic electrons whose excess chemical energy by energy conversion is higher than the Schottky barrier height can be detected on this metal–semiconductor nanodiode. Here, despite the higher Schottky barrier height in the Pt nanowires/TiO2 nanodiode with width of 15 nm (i.e., ~1.02 and 0.85 eV for Pt nanowires (width 15 nm)/TiO2 and Pt nanowires (width 20 nm)/TiO2, respectively), the higher hot electron detection indicates that the enhanced selectivity owing to the increased Pt-TiO2 interface concentration has a significant effect on hot electron excitation, neglecting the decrease in hot electron transfer due to the increased barrier. Therefore, as the structure exhibiting smaller width has a higher ratio of metal-oxide interface to metal sites, it exhibits higher partial oxidation selectivity to form methyl formate, thereby increasing reaction-induced hot electron excitation in methanol oxidation. The width dependence of selectivity of these TiO2 supported nanowires indicates that the selective partial oxidation reaction primarily occurs at the metal-oxide interface. Thus, the well-controlled width of oxide supported nanowires through our lithography technique can easily tune the ratio of metal-oxide interface, which changed the catalytic reaction significantly.

DFT calculations for two possible pathways

To gain further insight into the enhanced selectivity of methyl formate on Pt-TiO2 interface compared to Pt film, we performed DFT calculations on the Pt nanorod model on TiO2(110). Two possible reaction pathways toward CO2 and methyl formate formation are laid out in Supplementary Fig. 24, and detailed mechanisms, including all elementary steps and associated energetics are presented in Supplementary Table 4, following previously suggested mechanisms30,58. First, as shown in Supplementary Fig. 24, methanol is oxidized to formaldehyde, which can further oxidize to form CO2 or undergo C–C coupling to form methyl formate. As the reaction of the formaldehyde intermediate determines which product is produced between methyl formate and CO226, we considered the reaction channel from formaldehyde in two catalysts to compare the selectivity in the methanol oxidation reaction. The free energetics from formaldehyde to both products are presented in Fig. 4a, b. To initiate the reaction, methanol preferred to adsorb on the Ti top site of TiO2, whereas oxygen preferred the Pt sites in the present Pt-TiO2 interfacial structure. Thus, the reaction would mainly take place by transferring the protons from adsorbates on the Ti sites to oxygen (or OH) on Pt. However, once *CH2O loses its proton to *OH (*CH2O + *OH → *HCO + *H2O), *HCO prefers and moves to the Pt sites. Consequently, the final reaction CO + O → CO2 occurs above the Pt sites.

Fig. 4: Calculated activation barrier for Pt nanorod on TiO2(110) compared with Pt(111).
figure 4

Optimized free-energy profiles for a methyl formate and b the CO2 formation path with reaction barriers (ΔG‡). Barriers with red and blue indicate the RDS of each path for Pt nanorod structure on TiO2(110) and Pt(111), respectively. c Schematic drawing showing formation of CO2 and methyl formate in methanol oxidation on Pt nanorod/TiO2(110). Species marked with an asterisk (*) are adsorbed on the surface. The gray, blue, brown, red, and yellow balls indicate Pt, Ti, C, O, and H, respectively.

As the selectivity is determined by the activation barrier in the reaction determining steps (RDSs), we calculated the reaction energy barriers for CO2 and methyl formate on the Pt nanorods on TiO2(110) modeling Pt nanowires supported on TiO2. The Pt-TiO2 energetics were then compared to our previous calculation on a three-atomic-layer of Pt(111) surface, representing the reaction on the Pt film surface (Supplementary Table 5)30. As shown in Fig. 4a, on Pt-TiO2(110), the largest barrier step for the methyl formate formation was the last dehydration step (*CH3OCOH2 + *OH → *CH3OCOH + *H2O) with a low barrier of 0.16 eV. In the case of Pt(111), the RDS (i.e., the C–C coupling step) was different, with a much higher barrier of 0.64 eV. The altered RDS was attributed to the different adsorption configuration of CH2O that is needed for C–C coupling and has changed in the respective sites, as shown in Supplementary Fig. 25. In other words, on Pt(111), C and O are simultaneously adsorbed on the surface, requiring the rupture of the metal-C bonding for C-C coupling, whereas on Pt-TiO2(110) only O is bonded to the surface with an easy rotation of the methyl group for the coupling reaction.

The RDS in the CO2 formation path on both Pt-TiO2(110) and Pt(111) is the last C–O coupling step (CO + O → CO2), but the activation barrier was much larger on Pt-TiO2(110) (1.24 eV) than on Pt(111) (0.86 eV). This intriguing result could be attributed to a change in the reaction mechanism; on Pt(111), the reaction occurs via the Langmuir–Hinshelwood mechanism (*CO + *O → CO2(g)), whereas on the interfacial Pt sites of the Pt-TiO2(110), the reaction follows the Eley–Rideal mechanism (CO(g) + *O → CO2(g)) where CO desorbs first and then forms a new bond with adsorbed O. The binding energy of CO2 on the TiO2 surface was calculated, because the lower production of CO2 may be due to the adsorption of CO2 on TiO2. As shown in Supplementary Fig. 26, the binding energy of CO2 on the TiO2 surface was −0.21 eV, which is an energy level that can be sufficiently desorbed even at room temperature59; thus, the reason for the adsorption of CO2 on the TiO2 cannot be the low production of CO2. In addition, in the theoretical calculation on the Pt nanorod/TiO2(110) model, HCO, which is the intermediate before CO2 is generated, prefers adsorption to the Pt surface and CO2 generation occurs at the Pt site; thus, CO2 adsorption in TiO2 can also be excluded. Furthermore, as mentioned above, since the reaction mechanism in which CO2 was generated by methanol oxidation was revealed by DFT calculation as an Eley–Rideal mechanism (CO(g) + *O → CO2(g)) in the Pt nanorod/TiO2(110) model, there was no state in which CO2 was adsorbed during the methanol oxidation reaction. Thus, the experimentally observed enhanced selectivity toward methyl formate over CO2 on the Pt nanorod on TiO2(110) compared to thin Pt film can be understood by the much lower activation barrier to form methyl formate (0.64 for Pt(111) → 0.16 eV for Pt-TiO2(110)), as well as the increased activation barrier to form CO2 (0.86 for Pt(111) → 1.24 eV for Pt-TiO2(110)). The pathways in which CO2 and methyl formate were generated in Pt nanorod/TiO2(110) investigated by theoretical simulation are shown in Fig. 4c. Here, CO2 was generated on the Pt surface and methyl formate formed by reacting the intermediate present on TiO2 with OH present on Pt, and the importance of the Pt-TiO2 interface to improve the selectivity of methyl formate production could be theoretically proven. Hence, we can prove the experimental results of the reduced CO2 production and increased methyl formate production in Pt nanowires/TiO2 compared to Pt film/TiO2 (Fig. 2b, c). We note that a similar effect, changing activation barriers when the interfacial sites formed, was also demonstrated in the previous combined theory and experimental studies for Pt-NiO and Pt-CoO interfaces49,60. Therefore, all these results can point to the conclusion of selectivity enhancement on metal-oxide interfacial sites in Pt nanowires/TiO2, as these theoretical calculation results demonstrate the increased barrier for CO2 generation and the decreased barrier for methyl formate production. As hot electrons generated by non-adiabatic electronic excitation by exothermic catalytic reaction are excited states, it is challenging to directly calculate the transfer of excited hot electrons through DFT calculation and compare them in these two systems. However, we note that our earlier DFT calculations30 show the relationship between the generation of methyl formate and hot electron generation. In this study, it was found that the selectivity of methyl formate formation was enhanced when the Pt/TiO2 interface was formed, which was due to the difference in the activation barrier confirmed by theoretical calculations. Our quantitative comparison between the selectivity of methyl formate and CO2 on Pt-TiO2 and that of Pt(111) via DFT calculations, the enhanced hot electron generation on Pt-TiO2 interface can be rationalized. These are important findings, because these works are the first visualization of the unique electronic property of the metal-oxide perimeter in oxide supported-metal nanowires obtained by real-time measurement of excited hot electrons from the exothermic surface chemical reaction.

Discussion

In this study, we have investigated the metal-oxide interface effect on partial oxidation selectivity using a newly designed Schottky nanodiode composed of two-dimensional Pt nanowire arrays deposited on TiO2, and the changed selectivity influenced the magnitude of reaction-induced hot electron flow excited by methanol oxidation. Compared to Pt films on TiO2 where the interface was not exposed to the reaction environment, the Pt-TiO2 interface was exposed to the gaseous environment when the Pt nanowire arrays were placed on TiO2. The effect of the metal-oxide interface can be identified by comparing the selectivity in these two structures. We observed that the formation of the nanoscale Pt-TiO2 interface showed that selectivity to methyl formate formation was much larger in Pt nanowire arrays than in Pt films. As the efficiency of hot electron excitation by exothermic catalytic reaction was attributed to selectivity, the chemicurrent yield showed much higher in Pt nanowire arrays than on Pt film owing to enhanced selectivity, confirming the role of metal-oxide interfacial sites in enhancing selectivity and reaction-induced electron transfer. Calculation of the activation barrier by DFT calculation in two models of Pt nanorod/TiO2(110) and Pt(111) revealed barrier differences due to different molecular adsorption orientations and reaction mechanisms in the two models, which indicates improved selectivity at the Pt-TiO2 interface. This study is the first to directly observe the reaction-induced electronic excitation at the nanoscale metal-oxide interface, which was made possible by the real-time detection of hot electrons excited by catalytic reaction in the newly designed Pt nanowires/TiO2 system. Thus, this technique for using the catalytic nanodiodes provides a powerful and highly sensitive tool for studying the processes of charge transfer at the metal-oxide interface excited by surface chemical reaction. These studies demonstrate that the presence of nanoscale metal-oxide interfaces alters selectivity, thereby influencing reaction-induced electron transfer in heterogeneous catalysts. Tuning the materials and architectures of nanowires catalysts gives rise to the important control mechanism of chemical reaction and hot electron generation.

Methods

Fabrication of master molds for nanowire transfer printing

Cylinder forming polystyrene-block-poly(dimethylsiloxane) (PS-b-PDMS) block copolymers with molecular weights (MWs) of 36 kg/mol (SD36) and 48 kg/mol (SD48), which form 15- and 20 nm-wide lines, and hydroxyl-terminated PDMS brush polymer with a MW of 5 kg/mol were purchased from Polymer Source, Inc. (Canada). Surface-patterned Si substrates with a width of 1 μm and a period of 1.2 µm were fabricated using KrF photolithography followed by reactive ion etching and used as guiding substrates for the self-assembly of block copolymers. The hydroxyl-terminated PDMS solution dissolved in heptane solvent with a 2 wt% was spin-coated on the pre-patterned Si substrate. After spin casting, the sample was thermal annealed at 150 °C and then washed with heptane, to remove unattached polymer residues. SD36 and SD48 block copolymers were dissolved in a mixed solvent of toluene, heptane, and PGMEA (1 : 1 : 1 by volume) with a 0.6–0.8 wt% polymer solution. The SD36 and SD48 polymer solutions were spin-cast on the prepared substrates, respectively, and solvent-annealed with toluene vapor for 6–10 h in the chamber at room temperature to form well-ordered line/space patterns. After the annealing process, the samples were etched by CF4 plasma followed by O2 plasma treatment to obtain oxidized line/space PDMS nanostructures. To form Pt nanowires with 50 nm width and 200 nm pitch, the master mold was fabricated using KrF photolithography followed by reactive ion etching process.

Fabrication of n-type TiO2 support for catalytic nanodiodes

A 200 nm titanium film was deposited by electron beam evaporation with a titanium target using a patterned aluminum shadow mask (4 × 6 mm2) on a 4 inch 500 nm SiO2-covered p-type Si (100) wafer. After its deposition, the titanium film was thermally oxidized in air at 470 °C for 2.5 h, forming an n-type TiO2 film; the sheet resistance was checked during annealing. The electrode with a 50 nm Ti and a 150 nm Au thin film was deposited sequentially through a second shadow mask (5 × 5 mm2) on both sides by electron beam evaporation. The Ti layer was deposited to form ohmic contact with the n-type TiO2 surface and the Au layer created the two Ohmic electrodes for the catalytic nanodiodes. At room temperature, all the metal films were deposited with 10 kV of DC voltage in a high-vacuum chamber with a base pressure of 2 × 10−8 Torr, which was evacuated using rotary and turbomolecular pumps. The deposition rate of metal was 0.2 Å s−1 until a thin film of 5 nm was deposited for adhesion on the surface and the deposition rate was then gradually increased to 1.0 Å s−1 until reaching the final thickness of the metal film.

Solvent-assisted nanotransfer printing of Pt nanowire arrays on TiO2 support

Poly(methyl methacrylate) (PMMA; MW = 100 kg/mol) was purchased from Sigma Aldrich, Inc. and dissolved in a mixed solvent of toluene, acetone, and heptane with four wt% (4.5 : 4.5 : 1 by volume). The surface of the master molds was treated with a hydroxyl-terminated PDMS brush to enable the release of the polymer replica film from the master molds. After surface treatment, a PMMA polymer solution was spin-coated onto the master molds. A polyimide (PI) adhesive film (3M, Inc.) was then attached to the top surface of PMMA and smoothly detached from the master mold with the inverted surface topography. Pt nanowires were fabricated by obliquely angled deposition using an e-beam evaporator. The fabricated Pt nanowires/PMMA/PI adhesive film was exposed to a mixed solvent vapor of acetone and heptane (1 : 1 by volume) at 55 °C for 20–30 s then immediately brought into contact with the TiO2 surface of a nanodiode. After the transfer process, the PMMA replica was removed by dipping it into the toluene solvent baths. In addition, to facilitate the movement of hot electrons generated at the interface between Pt nanowires and TiO2, catalytic-inert Au nanowires with a width of 200 nm and a period of 1.2 µm were also transferred to the fabricated nanodiodes in a mesh type by sequential printing using the same method.

Measurement of reaction rates and chemicurrent

Catalytic methanol oxidation reactions were performed in an ultrahigh vacuum chamber (1 L) with a base pressure of 1 × 10−8 Torr, which was evacuated using rotary and turbomolecular pumps. After isolating with a gate valve, the catalytic reaction was carried out in a batch reactor system filled with a mixture of 1, 2, or 4 Torr of methanol and O2 to atmospheric pressure (760 Torr) at room temperature. To inject the methanol vapor into the reaction chamber, the methanol reactant was purified by three cycles of freeze–pump–thawing. All the reactant gas mixtures were recirculated through the reaction line using a Metal Bellows circulation pump at a rate of 2 L/min. After 0.5 h of recirculation to reach equilibrium at room temperature, a gas chromatograph (DS 6200) equipped with a thermal conductivity detector, for detection of CO2 product, and a flame ionization detector, for detection of methanol reactant and methyl formate product, were used to separate the gases for analysis. The reaction rates were reported as TOF in units of product molecules produced per Pt surface site pert second, and the number of Pt sites for nanowire arrays was calculated by geometrical assumptions. The Pt nanowire was assumed to be rectangular and standing upright on a planar oxide support similar to previous study33. The signals of electric current for the chemicurrent generated on the catalytic Schottky nanodiode were obtained using a Keithley Instrumentation 2400 SourceMeter at open circuit. Two gold wires were connected to make contact with the two electrical contact pads on either side (Au/Ti layer). The electric current flowing across the Schottky junction was then measured at reactive conditions (1–4 Torr of methanol and O2 to equal 760 Torr) and at non-reactive conditions (760 Torr of pure O2).

Characterization of fabricated catalytic nanodiodes

The crystalline phases of the Pt nanowire arrays were revealed using XRD patterns (Rigaku D/MAX-2500) taken at a 2θ scan range of 20–90°, scan speed of 4° min−1, and step size of 0.01 Å using Cu Kα radiation. The chemical oxidation states of the Pt nanowires (Pt 4 f) before and after catalytic reaction were identified using XPS (Thermo VG Scientific Sigma Probe spectrometer with an X-ray source of Al K-alpha (1486.3 eV)) with an energy resolution of 0.5 eV full width at half maximum under ultrahigh vacuum conditions with a base pressure of 10−10 Torr. Field-emission SEM (Magellan 400) and TEM (FEI Titan G2 Cubed 60-300) were used to observe the morphological structures of the Pt nanowires. IV characteristics of the Pt nanowires/TiO2 catalytic nanodiodes were obtained using a Keithley Instrumentation 2400 SourceMeter under various gas conditions (mixtures of 1–4 Torr of methanol with O2 to equal 760 Torr). By fitting the obtained IV characteristics to the thermionic emission equation, a series resistance, Schottky barrier height, and ideality factor could be obtained.

Simulation methods

DFT calculations were carried out using the VASP code with the Perdew–Burke–Ernzerhof functional61,62. The projector augmented wave method was used to describe the potentials of the atoms63. Geometries were optimized until the force on each atom was less than 0.05 eV/Å with a cutoff energy of 400 eV. As shown in Supplementary Fig. 16, to simulate the Pt-TiO2 structure, a (4 × 3) unit cell was used for rutile TiO2(110), which contains two layers of TiO2, and a Pt nanorod three layers high and three atoms wide is bonded on top of the TiO2(110) surface21. The bottom layer of TiO2 was fixed to their bulk position and all of the Pt atoms are allowed to relax in the Z-direction. K-points were sampled using a 2 × 1 × 1 Monkhorst–Pack grid. To model the Pt film, a three-atomic-layer (3 × 3) of Pt(111) surface unit cell with the bottom layer fixed was used. Spacing of more than 15 Å in the z-direction was applied. The Gibbs free energies were calculated using ΔG = ΔEads + ΔEZPE − TΔS (T = 300 K), where ΔEads, ΔEZPE, and ΔS represent the changes in adsorption energy, zero-point energy, and entropy, respectively. The DFT + U corrections were applied to the metal d states to correct the on-site Coulomb interaction, and the U-value was set at 4.0 eV64. The climbing image nudged elastic band method was employed to calculate the activation barriers65. The Bader charge analysis was performed to estimate the amount of charge transfer after methanol adsorption on Pt-TiO2 and Pt-SiO266. Negative sign indicates the loss of electrons.

Data availability

The data that support the findings of this study are available from the corresponding author upon reasonable request.

References

  1. Somorjai, G. A., Frei, H. & Park, J. Y. Advancing the frontiers in nanocatalysis, biointerfaces, and renewable energy conversion by innovations of surface techniques. J. Am. Chem. Soc. 131, 16589–16605 (2009).

    CAS  PubMed  Article  Google Scholar 

  2. Wodtke, A. M. Electronically non-adiabatic influences in surface chemistry and dynamics. Chem. Soc. Rev. 45, 3641–3657 (2016).

    CAS  PubMed  Article  Google Scholar 

  3. Park, J. Y., Kim, S. M., Lee, H. & Nedrygailov, I. I. Hot-electron-mediated surface chemistry: toward electronic control of catalytic activity. Acc. Chem. Res. 48, 2475–2483 (2015).

    CAS  PubMed  Article  Google Scholar 

  4. Somorjai, G. A. & Park, J. Y. Molecular factors of catalytic selectivity. Angew. Chem. Int. Ed. 47, 9212–9228 (2008).

    CAS  Article  Google Scholar 

  5. Nienhaus, H. Electronic excitations by chemical reactions on metal surfaces. Surf. Sci. Rep. 45, 1–78 (2002).

    CAS  Article  ADS  Google Scholar 

  6. Hasselbrink, E. How non-adiabatic are surface dynamical processes? Curr. Opin. Solid State Mater. Sci. 10, 192–204 (2006).

    CAS  Article  ADS  Google Scholar 

  7. Wodtke, A. M., Matsiev, D. & Auerbach, D. J. Energy transfer and chemical dynamics at solid surfaces: the special role of charge transfer. Prog. Surf. Sci. 83, 167–214 (2008).

    CAS  Article  ADS  Google Scholar 

  8. Park, J. Y., Baker, L. R. & Somorjai, G. A. Role of hot electrons and metal–oxide interfaces in surface chemistry and catalytic reactions. Chem. Rev. 115, 2781–2817 (2015).

    CAS  PubMed  Article  Google Scholar 

  9. Gergen, B., Nienhaus, H., Weinberg, W. H. & McFarland, E. W. Chemically induced electronic excitations at metal surfaces. Science 294, 2521–2523 (2001).

    CAS  PubMed  Article  ADS  Google Scholar 

  10. Lee, H., Nedrygailov, I. I., Lee, C., Somorjai, G. A. & Park, J. Y. Chemical‐reaction‐induced hot electron flows on platinum colloid nanoparticles under hydrogen oxidation: impact of nanoparticle size. Angew. Chem. Int. Ed. 54, 2340–2344 (2015).

    CAS  Article  Google Scholar 

  11. Karpov, E. G. & Nedrygailov, I. Nonadiabatic chemical-to-electrical energy conversion in heterojunction nanostructures. Phys. Rev. B 81, 205443 (2010).

    Article  ADS  CAS  Google Scholar 

  12. Hashemian, M., Palacios, E., Nedrygailov, I., Diesing, D. & Karpov, E. Thermal properties of the stationary current in mesoporous Pt/TiO2 structures in an oxyhydrogen atmosphere. ACS Appl. Mater. Interfaces 5, 12375–12379 (2013).

    CAS  PubMed  Article  Google Scholar 

  13. Diesing, D. & Hasselbrink, E. Chemical energy dissipation at surfaces under UHV and high pressure conditions studied using metal–insulator–metal and similar devices. Chem. Soc. Rev. 45, 3747–3755 (2016).

    CAS  PubMed  Article  Google Scholar 

  14. Nienhaus, H. et al. Electron-hole pair creation at Ag and Cu surfaces by adsorption of atomic hydrogen and deuterium. Phys. Rev. Lett. 82, 446 (1999).

    CAS  Article  ADS  Google Scholar 

  15. Ro, I., Resasco, J. & Christopher, P. Approaches for understanding and controlling interfacial effects in oxide-supported metal catalysts. ACS Catal. 8, 7368–7387 (2018).

    CAS  Article  Google Scholar 

  16. Sun, Y. N. et al. The interplay between structure and CO oxidation catalysis on metal‐supported ultrathin oxide films. Angew. Chem. Int. Ed. 49, 4418–4421 (2010).

    CAS  Article  Google Scholar 

  17. Cargnello, M. et al. Control of metal nanocrystal size reveals metal-support interface role for ceria catalysts. Science 341, 771–773 (2013).

    CAS  PubMed  Article  ADS  Google Scholar 

  18. Tauster, S., Fung, S. & Garten, R. L. Strong metal-support interactions. Group 8 noble metals supported on titanium dioxide. J. Am. Chem. Soc. 100, 170–175 (1978).

    CAS  Article  Google Scholar 

  19. Tauster, S., Fung, S., Baker, R. & Horsley, J. Strong interactions in supported-metal catalysts. Science 211, 1121–1125 (1981).

    CAS  PubMed  Article  ADS  Google Scholar 

  20. Matsubu, J. C. et al. Adsorbate-mediated strong metal–support interactions in oxide-supported Rh catalysts. Nat. Chem. 9, 120–127 (2017).

    CAS  PubMed  Article  Google Scholar 

  21. Green, I. X., Tang, W., Neurock, M. & Yates, J. T. Spectroscopic observation of dual catalytic sites during oxidation of CO on a Au/TiO2 catalyst. Science 333, 736–739 (2011).

    CAS  PubMed  Article  ADS  Google Scholar 

  22. Haruta, M., Kobayashi, T., Sano, H. & Yamada, N. Novel gold catalysts for the oxidation of carbon monoxide at a temperature far below 0 °C. Chem. Lett. 16, 405–408 (1987).

    Article  Google Scholar 

  23. Ye, R., Zhao, J., Wickemeyer, B. B., Toste, F. D. & Somorjai, G. A. Foundations and strategies of the construction of hybrid catalysts for optimized performances. Nat. Catal. 1, 318–325 (2018).

    Article  Google Scholar 

  24. Gross, E., Liu, J. H.-C., Toste, F. D. & Somorjai, G. A. Control of selectivity in heterogeneous catalysis by tuning nanoparticle properties and reactor residence time. Nat. Chem. 4, 947–952 (2012).

    CAS  PubMed  Article  Google Scholar 

  25. Lee, I., Delbecq, F., Morales, R., Albiter, M. A. & Zaera, F. Tuning selectivity in catalysis by controlling particle shape. Nat. Mater. 8, 132–138 (2009).

    CAS  PubMed  Article  ADS  Google Scholar 

  26. Wittstock, A., Zielasek, V., Biener, J., Friend, C. & Bäumer, M. Nanoporous gold catalysts for selective gas-phase oxidative coupling of methanol at low temperature. Science 327, 319–322 (2010).

    CAS  PubMed  Article  ADS  Google Scholar 

  27. Eren, B. et al. Structure of the clean and oxygen-covered Cu (100) surface at room temperature in the presence of methanol vapor in the 10–200 mTorr pressure range. J. Phys. Chem. B 122, 548–554 (2017).

    PubMed  Article  CAS  Google Scholar 

  28. Zugic, B. et al. Dynamic restructuring drives catalytic activity on nanoporous gold–silver alloy catalysts. Nat. Mater. 16, 558–564 (2017).

    CAS  PubMed  Article  ADS  Google Scholar 

  29. Wang, H. et al. Influence of size-induced oxidation state of platinum nanoparticles on selectivity and activity in catalytic methanol oxidation in the gas phase. Nano Lett. 13, 2976–2979 (2013).

    CAS  PubMed  Article  ADS  Google Scholar 

  30. Lee, S. W. et al. Intrinsic relation between hot electron flux and catalytic selectivity during methanol oxidation. ACS Catal. 9, 8424–8432 (2019).

    CAS  Article  Google Scholar 

  31. Chen, Z. et al. Understanding the dual active sites of the FeO/Pt (111) interface and reaction kinetics: density functional theory study on methanol oxidation to formaldehyde. ACS Catal. 7, 4281–4290 (2017).

    CAS  Article  Google Scholar 

  32. Farnesi Camellone, M. et al. Molecular understanding of reactivity and selectivity for methanol oxidation at the Au/TiO2 interface. Angew. Chem. Int. Ed. 52, 5780–5784 (2013).

    Article  CAS  Google Scholar 

  33. Contreras, A., Yan, X.-M., Kwon, S., Bokor, J. & Somorjai, G. Catalytic CO oxidation reaction studies on lithographically fabricated platinum nanowire arrays with different oxide supports. Catal. Lett. 111, 5–13 (2006).

    CAS  Article  Google Scholar 

  34. Contreras, A., Grunes, J., Yan, X.-M., Liddle, A. & Somorjai, G. Fabrication of 2-dimensional platinum nanocatalyst arrays by electron beam lithography: ethylene hydrogenation and CO-poisoning reaction studies. Top. Catal. 39, 123–129 (2006).

    CAS  Article  Google Scholar 

  35. Kim, J. M. et al. Eliminating the trade‐off between the throughput and pattern quality of sub‐15 nm directed self‐assembly via warm solvent annealing. Adv. Funct. Mater. 25, 306–315 (2015).

    CAS  Article  Google Scholar 

  36. Jung, Y. S. & Ross, C. A. Orientation-controlled self-assembled nanolithography using a polystyrene−polydimethylsiloxane block copolymer. Nano Lett. 7, 2046–2050 (2007).

    CAS  PubMed  Article  ADS  Google Scholar 

  37. Goddeti, K. C., Lee, H., Jeon, B. & Park, J. Y. Enhancing hot electron collection with nanotube-based three-dimensional catalytic nanodiode under hydrogen oxidation. Chem. Commun. 54, 8968–8971 (2018).

    CAS  Article  Google Scholar 

  38. Jeon, B., Lee, H., Goddeti, K. C. & Park, J. Y. Hot electron transport on three-dimensional Pt/mesoporous TiO2 Schottky nanodiodes. ACS Appl. Mater. Interfaces 11, 15152–15159 (2019).

    CAS  PubMed  Article  Google Scholar 

  39. Park, J. Y., Renzas, J., Hsu, B. B. & Somorjai, G. A. Interfacial and chemical properties of Pt/TiO2, Pd/TiO2, and Pt/GaN catalytic nanodiodes influencing hot electron flow. J. Phys. Chem. C 111, 15331–15336 (2007).

    CAS  Article  Google Scholar 

  40. Park, J. Y., Lee, H., Renzas, J. R., Zhang, Y. & Somorjai, G. A. Probing hot electron flow generated on Pt nanoparticles with Au/TiO2 Schottky diodes during catalytic CO oxidation. Nano Lett. 8, 2388–2392 (2008).

    CAS  PubMed  Article  ADS  Google Scholar 

  41. Lee, H. et al. Graphene–semiconductor catalytic nanodiodes for quantitative detection of hot electrons induced by a chemical reaction. Nano Lett. 16, 1650–1656 (2016).

    CAS  PubMed  Article  ADS  Google Scholar 

  42. Hervier, A., Baker, L. R., Komvopoulos, K. & Somorjai, G. A. Titanium oxide/platinum catalysis: charge transfer from a titanium oxide support controls activity and selectivity in methanol oxidation on platinum. J. Phys. Chem. C 115, 22960–22964 (2011).

    CAS  Article  Google Scholar 

  43. Yoon, S. et al. Specific metal–support interactions between nanoparticle layers for catalysts with enhanced methanol oxidation activity. ACS Catal. 8, 5394–5398 (2018).

    Article  CAS  Google Scholar 

  44. Xu, M. et al. Insights into interfacial synergistic catalysis over Ni@TiO2–x catalyst toward water–gas shift reaction. J. Am. Chem. Soc. 140, 11241–11251 (2018).

    CAS  PubMed  Article  Google Scholar 

  45. Xu, M. et al. TiO2–x-modified Ni nanocatalyst with tunable metal–support interaction for water–gas shift reaction. ACS Catal. 7, 7600–7609 (2017).

    CAS  Article  Google Scholar 

  46. Liu, N. et al. Auδ−–Ov–Ti3+ interfacial site: catalytic active center toward low-temperature water gas shift reaction. ACS Catal. 9, 2707–2717 (2019).

    CAS  Article  Google Scholar 

  47. Hervier, A., Renzas, J. R., Park, J. Y. & Somorjai, G. A. Hydrogen oxidation-driven hot electron flow detected by catalytic nanodiodes. Nano Lett. 9, 3930–3933 (2009).

    CAS  PubMed  Article  ADS  Google Scholar 

  48. Lee, H. et al. Enhanced hot electron generation by inverse metal–oxide interfaces on catalytic nanodiode. Faraday Dicuss. 214, 353–364 (2019).

    CAS  Article  ADS  Google Scholar 

  49. Lee, H. et al. Boosting hot electron flux and catalytic activity at metal–oxide interfaces of PtCo bimetallic nanoparticles. Nat. Commun. 9, 2235 (2018).

    PubMed  PubMed Central  Article  ADS  CAS  Google Scholar 

  50. An, K. et al. Enhanced CO oxidation rates at the interface of mesoporous oxides and Pt nanoparticles. J. Am. Chem. Soc. 135, 16689–16696 (2013).

    CAS  PubMed  Article  Google Scholar 

  51. Baker, L. R. et al. Furfuraldehyde hydrogenation on titanium oxide-supported platinum nanoparticles studied by sum frequency generation vibrational spectroscopy: acid–base catalysis explains the molecular origin of strong metal–support interactions. J. Am. Chem. Soc. 134, 14208–14216 (2012).

    CAS  PubMed  Article  Google Scholar 

  52. Hanukovich, S., Dang, A. & Christopher, P. Influence of metal oxide support acid sites on Cu-catalyzed nonoxidative dehydrogenation of ethanol to acetaldehyde. ACS Catal. 9, 3537–3550 (2019).

    CAS  Article  Google Scholar 

  53. Yang, Z. -Y., Wojtaszek-Gurdak, A., Yang, C. -M. & Ziolek, M. Enhancement of selectivity in methanol oxidation over copper containing SBA-15 by doping with boron species. Catal. Today 356, 122–131 (2020).

  54. Bunluesin, T., Putna, E. & Gorte, R. A comparison of CO oxidation on ceria-supported Pt, Pd, and Rh. Catal. Lett. 41, 1–5 (1996).

    CAS  Article  Google Scholar 

  55. Lee, S. W., Song, J. T., Kim, J., Oh, J. & Park, J. Y. Enhanced catalytic activity for CO oxidation by the metal–oxide perimeter of TiO2/nanostructured Au inverse catalysts. Nanoscale 10, 3911–3917 (2018).

    CAS  PubMed  Article  Google Scholar 

  56. Qadir, K. et al. Tailoring metal–oxide interfaces of inverse catalysts of TiO2/nanoporous-Au under hydrogen oxidation. Chem. Commun. 51, 9620–9623 (2015).

    CAS  Article  Google Scholar 

  57. Kennedy, G., Melaet, Grm, Han, H.-L., Ralston, W. T. & Somorjai, G. A. In situ spectroscopic investigation into the active sites for crotonaldehyde hydrogenation at the Pt nanoparticle–Co3O4 interface. ACS Catal. 6, 7140–7147 (2016).

    CAS  Article  Google Scholar 

  58. Xu, B., Haubrich, J., Baker, T. A., Kaxiras, E. & Friend, C. M. Theoretical study of O-assisted selective coupling of methanol on Au (111). J. Phys. Chem. C. 115, 3703–3708 (2011).

    CAS  Article  Google Scholar 

  59. Nørskov, J. K., Studt, F., Abild-Pedersen, F. & Bligaard, T. Fundamental Concepts in Heterogeneous Catalysis (Wiley, 2014).

  60. Kim, J. et al. Adsorbate-driven reactive interfacial Pt-NiO1−x nanostructure formation on the Pt3Ni (111) alloy surface. Sci. Adv. 4, eaat3151 (2018).

    PubMed  PubMed Central  Article  ADS  CAS  Google Scholar 

  61. Kresse, G. & Furthmüller, J. Efficiency of ab-initio total energy calculations for metals and semiconductors using a plane-wave basis set. Comput. Mater. Sci. 6, 15–50 (1996).

    CAS  Article  Google Scholar 

  62. Perdew, J. P., Burke, K. & Ernzerhof, M. Generalized gradient approximation made simple. Phys. Rev. Lett. 77, 3865 (1996).

    CAS  PubMed  Article  ADS  Google Scholar 

  63. Blöchl, P. E. Projector augmented-wave method. Phys. Rev. B 50, 17953 (1994).

    Article  ADS  Google Scholar 

  64. Dudarev, S., Botton, G., Savrasov, S., Humphreys, C. & Sutton, A. Electron-energy-loss spectra and the structural stability of nickel oxide: An LSDA + U study. Phys. Rev. B 57, 1505 (1998).

    CAS  Article  ADS  Google Scholar 

  65. Henkelman, G., Uberuaga, B. P. & Jónsson, H. A climbing image nudged elastic band method for finding saddle points and minimum energy paths. J. Chem. Phys. 113, 9901–9904 (2000).

    CAS  Article  ADS  Google Scholar 

  66. Tang, W., Sanville, E. & Henkelman, G. A grid-based Bader analysis algorithm without lattice bias. J. Phys. Condens. Matter 21, 084204 (2009).

    CAS  PubMed  Article  ADS  Google Scholar 

Download references

Acknowledgements

This work was supported by the Institute for Basic Science (IBS) [IBS-R004]. Y.J. acknowledges support through the National Research Foundation of Korea from the Korean Government (NRF-2019M3D3A1A01069099 & 2016M3D1A1021147).

Author information

Authors and Affiliations

Authors

Contributions

S.W.L. and J.Y.P. planned and designed the experiments. S.W.L. performed the central measurements and analysis. S.W.L. and H.L. fabricated the nanodevices and carried out the chemicurrent and catalytic activity measurements. W.P. and Y.J. performed the DFT calculations. J.K., G.R.L., and Y.S.J. fabricated the nanowire-based diode. All authors discussed the results and contributed to the manuscript.

Corresponding authors

Correspondence to Yousung Jung, Yeon Sik Jung or Jeong Young Park.

Ethics declarations

Competing interests

The authors declare no competing interests.

Additional information

Peer review information Nature Communications thanks Bin Wang 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.

Supplementary information

Rights and permissions

Open Access This article is licensed under a Creative Commons Attribution 4.0 International License, which permits use, sharing, adaptation, distribution and reproduction in any medium or format, as long as you give appropriate credit to the original author(s) and the source, provide a link to the Creative Commons license, and indicate if changes were made. The images or other third party material in this article are included in the article’s Creative Commons license, unless indicated otherwise in a credit line to the material. If material is not included in the article’s Creative Commons license and your intended use is not permitted by statutory regulation or exceeds the permitted use, you will need to obtain permission directly from the copyright holder. To view a copy of this license, visit http://creativecommons.org/licenses/by/4.0/.

Reprints and Permissions

About this article

Verify currency and authenticity via CrossMark

Cite this article

Lee, S.W., Kim, J.M., Park, W. et al. Controlling hot electron flux and catalytic selectivity with nanoscale metal-oxide interfaces. Nat Commun 12, 40 (2021). https://doi.org/10.1038/s41467-020-20293-y

Download citation

  • Received:

  • Accepted:

  • Published:

  • DOI: https://doi.org/10.1038/s41467-020-20293-y

Comments

By submitting a comment you agree to abide by our Terms and Community Guidelines. If you find something abusive or that does not comply with our terms or guidelines please flag it as inappropriate.

Search

Quick links

Nature Briefing

Sign up for the Nature Briefing newsletter — what matters in science, free to your inbox daily.

Get the most important science stories of the day, free in your inbox. Sign up for Nature Briefing