Introduction

Exploitation of the photothermal effect, specifically to enhance the production of synthetic fuels via gas-phase heterogeneous CO2 hydrogenation, relies upon the nonradiative decay processes of photogenerated electron−hole pairs to simultaneously drive thermochemical and photochemical reactions on the surface of nanostructured materials. Unlike traditional photocatalysis, which is limited to the use of higher-energy photons, photothermal catalysis can theoretically utilize the full wavelength range of the solar spectrum to facilitate surface chemical reactions1,2,3,4,5,6,7,8,9,10,11,12.

Optimizing the photonic efficiency of these reactions requires control over the thermal relaxation processes that create high local temperatures and drive surface thermochemical reactions, and the electron−hole generation and separation processes that facilitate surface photochemical reactions7. While these two processes appear to be antithetical, requiring one to be optimized at the expense of the other, both are expected to benefit from materials that provide high optical absorption strength over the entire solar spectral wavelength range.

Achieving peak photothermal performance would require the use of black, high surface area nanostructures capable of concurrent thermochemical and photochemical hydrogenation of CO2 to value-added products. Unfortunately, no such materials currently exist.

Our approach to this problem focuses attention on stoichiometric indium oxide (In2O3). In its pristine form, In2O3 is a pale yellow thermal insulator with a wide electronic bandgap, absorbing light mainly in the ultraviolet wavelength range and thereby minimizing its ability to function as a photothermal CO2 hydrogenation catalyst13,14,15,16,17,18.

Pale yellow In2O3 can, however, be turned pitch black via thermal hydrogenation at 400 °C. This reduction reaction converts stoichiometric In2O3 into an oxygen-deficient, nonstoichiometric form, In2O3−x. This black In2O3−x is shown to be a CO2 hydrogenation catalyst possessing both photothermal and photochemical activity, thereby dramatically transcending the activity and selectivity performance of pale-yellow In2O3 and, indeed, any other known form of cubic indium oxide13,14,15,16,19.

In brief, we discover that black indium oxide, a nonstoichiometric/stoichiometric heterostructure, denoted In2O3−x/In2O3, can enable the photothermal reverse water gas shift reaction (RWGS) under ambient conditions with 100% selectivity. Compared to pale yellow In2O3, with its CO production rate of 0.78 μmol h−1 m−2 (19.64 μmol g−1 h−1) in light, black In2O3−x/In2O3 can drive the reaction at 1874.62 μmol h−1 m−2 (23,882.75 μmol g−1 h−1), approximately three orders of magnitude greater than both stoichiometric In2O3 and about three orders of magnitude larger than the best reported RWGS rate of all known indium-oxide-based photocatalysts (Supplementary Fig. 1). The estimated turnover frequency (TOF) is 2.44 s−1, which is higher than most photocatalysts and photothermal catalysts for CO2 hydrogenation (Supplementary Table 1). The fact that this synthesis of black indium oxide is straightforward and amenable to scaling speaks well for its application as an industrial photothermal RWGS catalyst.

Results

Black indium oxide—synthesis and characterization

The as-prepared indium oxide nanocrystals (S1) devoid of hydroxide groups was synthesized via thermal dehydroxylation of In(OH)3 nanocrystals at 700 °C for 5 h in air. As-prepared S1 was subsequently treated with hydrogen at different temperatures (i.e., 200, 300 and 400 °C) for 1 h to form In2O3−x/In2O3 with different x values, labeled S2, S3 and S4, respectively.

Powder X-ray diffraction (PXRD) patterns of all samples are shown in Fig. 1a. These patterns reveal the presence of the phase pure cubic bixbyite structure type In2O3 and are devoid of metallic indium, indicating that the black color created during hydrogenation is intrinsic to the indium oxide itself. The cubic bixbyite In2O3 is a fluorite-type structure In2O3 with one fourth of the anions missing indicates a periodic structure that produces 25% structural vacancies20. The grain sizes calculated from the width of the strongest PXRD peak at 30.6° were found to be 20.6, 30.9, 33.0 and 36.3 nm for S1 through S4, respectively, which confirmed slight size growth with increasing temperature of the hydrogenation.

Fig. 1: Structural and morphological information for In2O3−x/In2O3 materials S1, S2, S3, S4.
figure 1

a PXRD patterns of S1−S4. b High-resolution O1s core level XPS spectrum of S4. c, d HRTEM and STEM images of S4 at different magnifications. A dashed green circle indicates an amorphous phase, yellow arrow indicates the measured lattice spacing and the red square indicates the imaged position.

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High-resolution X-ray photoelectron spectroscopy (XPS) of In 3d and Auger LMM 3d electronic transitions served to establish the oxidation state of indium as In(III) (Supplementary Fig. 2). The O 1s core level XPS spectra for all samples could be fit with just two peaks at ~529.2 and ~531.8 eV. These peaks corresponded to lattice oxygen (OI, InO6) and the unsaturated lattice oxygen that generated by the formation of oxygen vacancy (OII, InO6−x), with the latter population increasing with the temperature of the hydrogenation process, as consistent with the following reaction: In2O3 + xH2 → In2O3−x + xH2O (Supplementary Fig. 2d).

Since XPS is a surface-sensitive characterization technique, the value of x can be further calculated based on the concentration of oxygen vacancies. As a result, the chemical formulae for S2−S4 are estimated to be In2O2.8, In2O2.7 and In2O2.63, respectively. The absence of a diagnostic hydroxide O 1s XPS peak supports this reaction pathway, rather than an alternative H2 homolysis involving the injection of protons and charge-balancing electrons into the lattice with the concomitant formation of Brønsted hydroxides, In2O3 + xH2 → H2xIn2O3.

The thermogravimetric analysis has been performed to simulate the synthetic process of S1 (2In(OH)3 → In2O3 + 3H2O) and indicates a very similar value of the weight change (84.94%) for S1 to the theoretical stoichiometric In2O3 (83.7%), where the very slight excess can be attributed to absorbed water (Supplementary Fig. 3a). Similar measurements were conducted to simulate the synthetic process of S2−S4 (Supplementary Fig. 3b−d) with the observed weight changes of 99.35%, 99.19%, and 98.63%, and indicates the overall formulas of In2O2.98, In2O2.97 and In2O2.95, respectively. Such minor overall weight change confirmed the formation of [O] and the hydrogenation process is a surface treatment and result in the formation of In2O3−x/In2O3 heterostructures.

The Brunauer−Emmett−Teller (BET)-specific surface areas of S1–S4 paralleled the monotonic trend of increasing nanocrystal size, registering at 25.15, 15.30, 14.74 and 12.74 m2 g−1, respectively, with a pore diameters ranging from 29 to 64 nm (Supplementary Fig. 4).

High-resolution transmission electron microscopy (HRTEM) were employed to investigate the morphology of all samples. The HRTEM images shown in Supplementary Fig. 5 indicate highly crystalline nanomaterials for S1–S3 with the typical (222) facet lattice spacing of ~0.292 nm. By contrast, the images for S4 show the formation of what appear to be amorphous regions, and which seem to be associated with the increased loss of surface O. Lattice regions observed in these images have an average spacing of ~0.296 nm (Fig. 1c and Supplementary Fig. 6). The STEM image also confirmed the imaged nanocrystal is not overlapping with others (Fig. 1d). The average particle sizes of S1 and S4 are calculated as 28.8 and 44.9 nm, respectively (Supplementary Fig. 6e–g).

The optical reflectance spectra (UV-Vis-NIR) for S1–S4 show a trend of gradually increasing absorption, broadening and red shifting of the ultraviolet absorption edge into the visible region with higher temperatures of the hydrogenation (Supplementary Fig. 7). The bandgap of all samples can be then calculated as 2.66, 2.62, 2.54 and 2.36 eV for S1, S2, S3 and S4, respectively.

Raman spectra were also recorded for S1−S4. In particular, the mode around 132.3 cm−1 is ascribed to the totally symmetrical stretching mode of InO6 octahedral building blocks21. With increasing values of x on passing from S1 to S4, this mode undergoes a notable redshift (from 132.3 to 130.0 cm−1) and broadening (full-width half maximum increased from 3.24 to 6.21 cm−1) (Supplementary Fig. 8)22,23. The broadening of peaks also confirmed the amorphization of the surface of black indium oxide. The observed peaks at 132.3, 308.1, 366.5, 497.0 cm−1 can be assigned to the phonon vibration modes of the bcc form of In2O3, while the peak at 366.5 cm−1 most likely is associated with the oxygen vacancy which we believe could be considered as the unsaturated lattice oxygen (InO6−x)24. The ratio between InO6 (132.3 cm−1) and InO6−x (366.5 cm−1) exhibits a monotonically increasing trend from S1 to S4 and implies an increasing concentration in [O]. Further Raman spectroscopy with different beam intensities were conducted over S3 and S4 to study their photothermal effects. The Raman signal located at ~308 cm−1 has been assigned to a vibrational/phonon mode of an InO6 site and is used as the probe/reference signal. The resulting Raman signals for S4 exhibit blue shift with increasing beam intensities (0.00110, 0.00055, 0.00028, and 0.00011 mW μm−2) gradually shift from 304.18 to 302.90, 302.68 and 300.63 cm−1 and indicates an increasing trend of photothermal local temperatures. On the contrary, no significant shift can be observed from S3 and implies minor photothermal effects.

In situ X-ray absorption spectroscopy measurements of S1 under a 3.5% H2/He atmosphere at 400 °C for 2 h indicated partial reduction of In(III) via a shift of the white line peak to lower binding energies (Supplementary Fig. 9). No further shift was observed after an additional 2 h of reductive treatment; however, ex situ measurements of S4 showed more extensive reduction of In(III), resulting in slightly reduced intensity throughout XANES region of the spectrum. There is no sign of metallic indium formation in these spectra, however, which supports the trapping of conduction electrons in mid-gap oxygen vacancy states predominates over the reduction of In(III). Fitting of the Fourier-transformed EXAFS spectra in Supplementary Fig. 10 revealed a slightly lower In–O coordination number of 5.3 relative to the nominal value of 6 (Supplementary Table 2).

In an attempt to delve more deeply into the origin and cause of the aforementioned amorphization processes, an in situ high-resolution environmental transmission electron microscopy (HRETEM) study was performed on stoichiometric In2O3 nanocrystals under conditions simulating the aforementioned hydrogenation process (Fig. 2). A reference image of a stoichiometric In2O3 nanocrystal was obtained after annealing and stabilization at 400 °C under an N2 atmosphere for 20 min (Fig. 2a). When exposed to an H2 atmosphere for increasing time periods, the birth and growth of amorphous regions in the nanocrystal can be observed (Fig. 2b−d). The H2-induced removal of O atoms from stoichiometric In2O3 resulted in nonstoichiometric In2O3−x domains, and thus causing the formation of amorphous phase as illustrated in Fig. 2e, f. The density functional theory calculations performed to analyze the effect of this amorphization process suggests an expansion of the adjacent lattice, proof of which will require atomic resolution TEM (Supplementary Fig. 11 and Supplementary Table 3). The simulated electronic band structures for the simulated In2O3 are shown in Supplementary Figs. 12 and 13.

Fig. 2: In situ high-resolution environmental transmission electron microscopy (HRETEM) observations of the In2O3 + xH2 → In2O3−x + xH2O process.
figure 2

High-resolution images of a stoichiometric In2O3 nanocrystal (S1) at 400 °C a under an N2 atmosphere and then switched to an H2 atmosphere for the following times: b 5 min, c 10 min and d 20 min. Scale bars are the same for all images, green squares indicate the formation of an amorphous phase. Graphical representation of the e original and f treated In2O3, wherein blue region, pink dots, yellow dots and yellow circles represent amorphous phase, In atoms, O atoms and [O], respectively.

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Black indium oxide—photocatalyst evaluation

It has thus far been established that the black color of hydrogenated In2O3 stems from the nucleation and growth of amorphous domains of nonstoichiometric In2O3−x in crystalline stoichiometric In2O3. Hereafter, black indium oxide will be denoted In2O3−x/In2O3. The strong, broad optical absorption of In2O3−x/In2O3 across the entire wavelength range of the solar spectrum increases the likelihood that black indium oxide will function as an effective catalyst for the photothermal hydrogenation of CO2. To this end, the photocatalytic activity of black indium oxide on a borosilicate film support was evaluated in a batch reactor. Isotopically labeled 13CO2 was used to confirm hydrogenation products originated from carbon dioxide and not adventitious carbon contamination (Supplementary Fig. 14).

The photocatalytic hydrogenation activity of CO2 by samples S1−S4, normalized to their specific surface area, was observed to monotonically increase: 0.78, 1.77, 2.96, 1874.62 μmol h−1 m−2. This increase paralleled the degree of nonstoichiometry. Notably, the only product observed was CO (Fig. 3a). The S4 sample exhibited the largest conversion rate, being 2403 times higher than that of S1 with TOF of 2.44 s−1. The reason for such an impressive photo-enhancement can be attributed to the much stronger solar energy harvesting ability and photothermal effects of S4 compared to the other samples (Supplementary Figs. 7a and 8), which results in a larger photothermal effect and correspondingly higher catalytic performance. Based on the enclosed thermocouple, the temperatures of S1−S3 are lower than 50 °C, and about 160 °C for S4. The local temperatures of all samples can be estimated from the conversion of CO2 to CO (yield, ppm), where S4 is found to be 262 °C in contrast to S1−S3 which are found to have much lower local temperatures (Supplementary Fig. 15). These results illustrate photocatalysis and photothermal catalysis can be achieved with light irradiation and in this case serve to shift the reaction equilibrium equivalent to one corresponding to 262 °C.

Fig. 3: Photocatalytic evaluation of black indium oxide.
figure 3

a Photocatalytic CO2 hydrogenation in a batch reactor. Conditions: H2/CO2 ratio = 1:1, light intensity = ~20 suns, no external heating and measurement time = 30 min. b Catalytic performance for S4 in a flow reactor at different temperatures, both with and without light irradiation; inset is the enlarged view of the catalytic performance for 200, 225 and 250 °C. c Stability test for S4 in a flow reactor at 300 °C with light irradiation for 70 h. Conditions for flow measurement: atmospheric pressure, H2/CO2 ratio = 1:1 with a flow rate of 1 mL min−1 and light intensity of ~8 suns.

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To further evaluate the performance of black indium oxide under more practical conditions, S1 and S4 were tested at 200 °C in a flow reactor with and without light irradiation. As shown in Fig. 3b, S4 (0.10 and 0.14 μmol h−1 m−2) was much more active towards CO production from CO2 than S1−S3 (ranging from 0.01 to 0.03 and 0.015 to 0.039 μmol h−1 m−2) both thermocatalytically and photocatalytically (Supplementary Fig. 16a). Increasing temperature causes the CO rates for S4 to continually increase. At 300 °C S4 displayed CO production rates of 160.99 and 38.54 μmol h−1 m−2. There is a notable photo-enhancement in the CO rate of about 417% under light compared to dark reaction conditions, which is about four times higher than that of the best reported cubic In2O3-based photocatalyst13. The significant photo-enhancement could be caused by the photothermal catalysis. Interestingly, a minor amount of methanol can also be detected in between 250 and 275 °C with light; the detected methanol rates are 1.14 and 1.48 μmol h−1 m−2, respectively (Supplementary Fig. 16b, c). Formation of methanol at such low H2 concentrations implies a strong hydrogenation ability of black indium oxide. The photoaction behavior of S3 and S4 was examined in a multiwavelength LED photoreactor and exhibited very different catalytic performance (Supplementary Fig. 16d−f). Relative to the activity in the dark, the less photoactive S3 is able to exhibit an increase of 8.8% and 7.7% with irradiation from the UV and blue LEDs, respectively and much less with the green (2.1%) and red (2.2%) LEDs. In stark contrast, S4 exhibits a much stronger photo-enhancement under UV, blue, green or red LEDs (42.6%, 41.0%, 35.9% and 35.2%, respectively). A 70-h photo-stability test for S4 in the flow reactor at 300 °C showed a decrease in activity of only 5% (Fig. 3c). The spent sample of the stability test was probed by PXRD and HRTEM and no obvious change can be identified (Supplementary Fig. 17).

How does black indium oxide function as a photocatalyst?

We now know that black indium oxide, formed by the thermal hydrogenation of pale yellow indium oxide, is best described as a heterostructure comprising amorphous domains of nonstoichiometric indium oxide In2O3−x interfaced with crystalline regions of stoichiometric indium oxide In2O3, which we denote In2O3−x/In2O3. We also know that the amorphous phase was caused by the loss of surface oxygen from the In2O3 phase.

To study the dynamics of photoexcited electrons, in situ photoconductivity measurements under vacuum and experimental conditions for S1 and S4 were performed and shown in Fig. 4a, b and Supplementary Fig. 18. It is known that, among metal oxides systems, In2O3 exhibits very long photocurrent relaxation times (minutes to hours), a quality known as persistent conductivity25,26. The measurements display photocurrent saturation and decay process lifetimes on the order of minutes. The much faster photo-saturation of the excited electrons for S4 implies a stronger optical absorbance for S4 than S1. While the light was off, the photocurrents of S1 and S4 slowly decayed, with S4 requiring a much longer decay time than S1, which implies a higher population of oxygen vacancy traps for photoelectrons. Furthermore, the longer lifetime of the detected photoelectrons also implies a higher probability for the photoexcited electrons to participate in the reaction and thereby results in a better catalytic performance for S4. The same trend was observed under vacuum conditions, and the resulting I−V plot further confirmed the prolonged lifetime of photoexcited electrons for S4. Moreover, the observed photocurrent is consistent with the observed photocatalytic activity of black indium oxide for CO2 hydrogenation.

Fig. 4: Characterization of electronic properties and surface H2 and H2-CO2 chemistry of the samples S1 and S4.
figure 4

a Photocurrent saturation and decay plot acquired at ~200 °C with a 1:1 ratio of CO2/H2 and under a 100 W LED white lamp. b Corresponding in situ I−V plot. In situ DRIFTS spectra of S4 obtained c under H2 at room temperature and d under both H2 and CO2 (1:1) with increased temperatures. The collected DRIFTS spectra are subtracted by the background signal of S4 obtained under He.

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In addition, we know that oxygen vacancies [O] and the associated charge-balancing electrons in In2O3−x, arising from the removal of oxygen from In2O3, cause the color of the material to change from pale yellow to black. The oxygen vacancies [O] and coordinately unsaturated indium In′ sites and oxygen O′ sites in In2O3−x will exist as mid-gap defect states in the bandgap of In2O3 27,28. These states will be respectively situated near the oxide-based valence band and indium-based conduction band, with the charge-balancing electrons occupying mid-gap states, as shown in Supplementary Fig. 12e−g. Together, they give rise to optical absorption throughout much of the solar spectral wavelength range.

With this information, we can begin to understand how and why the In2O3−x/In2O3 heterostructure is well-equipped for photothermal CO2 hydrogenation reactions. Absorption of light across the solar spectral wavelength range causes local heating of In2O3−x/In2O3 that enables thermochemical conversion of CO2 to CO. Formed via the absorption of light, photogenerated electrons and holes can separate across the interface between In2O3 and In2O3−x, thereby promoting the photochemical conversion of CO2.

The in situ DRIFTS measurements performed under H2 atmosphere at room temperature revealed homolytic H2 dissociation over black indium oxide (Fig. 4c). The weak peaks around 2900−3700 cm−1 and 1100−1200 cm−1 can be associated with protonated indium oxide species (In-OH+)29. The similarity of these peak positions to those described for In-OH bonds in previous reports, and the disappearance of such peaks on heating above 100 °C, further confirmed the presence of protonated In-O (Supplementary Fig. 19a). The rising baseline in the near infrared spectral range could be caused by free electrons in the conduction band, generated by the homolytic splitting of H2 30. The absence of indium hydrides in the region of 1100−4000 cm−1 implies homolysis of H2, which is different from the former study over In2O3−x(OH)y that exhibited heterolysis of H2 31.

To further confirm the proposed homolytic H2 splitting mechanism on In2O3−x, solid-state 1H MAS NMR spectroscopy was utilized to detect the H-related species in S4 before and after exposure to H2 at room temperature (Supplementary Fig. 19b). The absence of hydride peak and formation of new peaks at 9.51, 6.91 and 5.66 ppm match well with those of the reference material, In2O3−x(OH)y, leading support to the H2 homolysis pathway (Supplementary Fig. 20a).

While under a CO2 atmosphere at temperatures ranging from 25 to 100 °C, gaseous CO2 fingerprint modes are observed at 3500−3800 cm−1 and 2300−2400 cm−1. Two new peaks are also observed at 680 and 825 cm−1, and likely signal the activation of absorbed CO2 (Supplementary Fig. 19c, d)18,32,33 via the insertion of CO2 into O vacancies (Supplementary Fig. 20b).

Insight into the reaction pathway of CO2 hydrogenation has been obtained via in situ DRIFTS under both H2 and CO2 gases (1:1 ratio) (Fig. 4d). Similar to the DRIFTS results obtained under CO2, the results favor a reaction pathway involving the insertion and regeneration of [O], where the ɑ and β peaks at 825 and 680 cm−1 can be associated with In-O groups originating from the activation and insertion of CO2 (Supplementary Fig. 20c)34,35.

Discussion

While CO2 hydrogenation can be driven thermally in the ground electronic state, how can one rationalize the much greater efficiency of the reaction in the excited state?

The relative positions of the valence and conduction bands in the electronic band diagram of In2O3/In2O3−x, shown in Fig. 5, were obtained via UV-Vis-NIR (Supplementary Fig. 7) and ultraviolet photoelectron spectroscopy (UPS) (Supplementary Fig. 21). One can deduce that following absorption of solar light, photogenerated electrons and holes in the In2O3 CB can respectively relax to the mid-gap unsaturated In(III)′ and [O] vacancy states near the CB edge and unsaturated O′ near the VB edge in In2O3−x27. These states can also be directly populated by band gap excitation and the relaxation of electrons and holes in In2O3−x.

Fig. 5: Illustration of the electronic band structure.
figure 5

The In2O3−x/In2O3 heterostructure showing the In(III)′, [O] electron-trapping and O′ hole-trapping mid-gap energy states near the CB and VB edges, respectively. Included also in the diagram is the outcome of photoexcitation and relaxation of electrons and holes involving valence, conduction and mid-gap energy states.

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To simulate the formation of surface O vacancies and the reactivity for CO2 hydrogenation, a model In2O3 (110) surface is used in these calculations (Supplementary Fig. 22). Six possible positions for O vacancies are considered as shown in Supplementary Fig. 23. The calculated energies in Supplementary Table 4 support that the proposed reaction pathways could still occur under solar irradiation conditions. To expand, proton insertion weakens the C−O bond of the adsorbed CO2 at an oxygen vacancy, which enables the formation of CO, thereby reforming In2O3. Subsequent abstraction of O from In2O3 by protons to form H2O, reforming the O vacancy and In2O3−x, thereby completes the catalytic cycle. The simulated reaction pathway is represented by the scheme shown in Supplementary Fig. 20d.

Black indium oxide has been found to outperform all known indium-oxide-based photocatalysts based on its activity, selectivity and stability. The calculated turnover frequency of 2.44 s−1 is higher than most of the reported photocatalysts and photothermal catalysts in the prior art. It exhibits 100% selectivity towards CO at 300 °C and able to be operated stably for more than 70 h. Its ease of synthesis via hydrogenation of commercially available, pale-yellow indium oxide and shelf-life of more than 9 months (Supplementary Fig. 24) make it highly amenable to scaling for use as an industrial photothermal catalyst.

In this context, the question of cost always arises. For indium, as for all metals, cost depends upon market demand and availability. To amplify on this point, the concentration of terrestrial indium is 0.050 ppm; this concentration is greater than those of silver, which is not considered to be in short supply. With improvements in extraction technology, indium can also be obtained as a by-product from different base metals that include zinc, lead, tin and copper.

The increasing number of geographical locations bearing discovered indium-containing ore deposits, and the positive financial gains of mining companies stemming from greater demand for indium, has encouraged new investments in mining, thereby providing confidence in the stability of indium supply. While still costly at $200−$300 per kg, there currently exist 3000 to 4000 tonnes of stored and commercially available indium, which would suggest that it can sustain great growth in its use without suffering limitations of supply.

Thus, it will be interesting to see whether black indium oxide proves to be a technologically and commercially viable industrial RWGS photocatalyst.

Methods

Chemicals

Indium(III) chloride (98%) was purchased from Sigma Aldrich and commercial In2O3 nanocrystal was purchased from Alfa Aesar.

Synthesis of In(OH)3 nanocrystals

In a typical synthesis of indium hydroxide, indium(III) chloride (3.6 g, 16.2 mmol, 98%) was dissolved in a 3:1 solution (72 mL) of anhydrous ethanol (Commercial Alcohols) and deionized water. In a separate beaker, a 3:1 mixture of ethanol and ammonium hydroxide was prepared by combining aqueous ammonium hydroxide (18 mL, Caledon, 28–30%) and of anhydrous ethanol (54 mL). The solutions were rapidly combined, resulting in the immediate formation of a white precipitate. The resulting suspension was then immediately immersed in a preheated oil bath at 80 °C and stirred for 30 min. The suspension was then removed from the oil bath and allowed to cool to room temperature. The precipitate was separated via centrifugation and washed five times with deionized water. The precipitate was sonicated between washings to ensure adequate removal of any trapped impurities and then dried overnight at 60 °C in a vacuum oven.

Synthesis of In2O3 and hydrogenated samples

The pale yellow In2O3 nanocrystal (S1) was obtained via thermal treatment of In(OH)3 nanocrystal in air at 700 °C for 5 h. The hydrogenated samples (S2−S4) were synthesized via treating S1 in tube furnace with 10%H2/Ar at a flow rate of 120 sccm. The temperatures for treatment were set as 200, 300 and 400 °C for 1 h with an increasing temperature rate of 5 °C per min. When the hydrogenation process was finished, the sample was naturally cooled down to room temperature.