Hui
Li‡
a,
Wenqi
Zheng‡
a,
Xinyi
Liu
a,
Jiashi
Li
a,
Lianbing
Wen
a,
Fujie
Tang
b and
Wei-Tao
Liu
*a
aPhysics Department, State Key Laboratory of Surface Physics, Key Laboratory of Micro and Nano Photonic Structures [Ministry of Education (MOE)], Fudan University, Shanghai 200433, China. E-mail: wtliu@fudan.edu.cn
bPen-Tung Sah Institute of Micro-Nano Science and Technology, Institute of Artificial Intelligence, Laboratory of AI for Electrochemistry (AI4EC), Tan Kah Kee Innovation Laboratory (IKKEM), Xiamen University, Xiamen, 361005, China
First published on 10th April 2025
The dissociation of water on TiO2 surfaces, marked by the presence of TiOH groups, is pivotal for environmental and energy applications involving TiO2. Yet characterizing these surface groups has remained a challenge. Here, we employ in situ sum-frequency vibrational spectroscopy (SFVS) to unveil the vibrational signatures of surface TiOH and undercoordinated Ti–O groups in the Ti–O vibrational frequency range, offering a clear structural indicator of TiO2 hydroxylation. Our findings confirm the spontaneous dissociation of water molecules on TiO2 surfaces, a process significantly enhanced by structural defects such as oxygen vacancies. Through methanol titration experiments, we gain molecular-level insights into the adsorption/desorption dynamics, estimating a ∼70% TiOH coverage on amorphous TiO2 under ambient conditions. This work not only deepens our understanding of TiO2/water interactions but also lays the groundwork for future SFVS investigations into these interfaces.
Previously, we have implemented SFVS to explore lattice vibrations of various oxides such as crystalline/amorphous silicon oxides and crystalline titanium oxides,19–21 which provided unique insights into interfacial chemistry from the oxide perspective. In this work, we investigated lattice vibrations from amorphous and polycrystalline anatase TiO2 surfaces in the ambient atmosphere, in correlation with water adsorption and dissociation processes. Besides undercoordinated surface Ti–O bonds, we further identified resonances from Ti–O–H vibrations, which are well separated from water OH stretching and bending vibrations, and can serve as an unambiguous signature of chemisorbed OH groups on TiO2. In conjunction with the titration study between methanol and water, we monitored the adsorption and dissociation of atmospheric water on TiO2 and deduced a typical coverage of TiOH being ∼70% under ambient conditions. With ultraviolet (UV) irradiation and annealing treatments that converted the amorphous TiO2 to polycrystalline phase, the results again underscored the key role of structural defects in water dissociation, as previously shown for single crystalline TiO2 surfaces.20,21 These vibrational signatures can serve as direct indicators of the TiO2 surface hydroxylation status to be monitored in situ, paving the way for a wholistic understanding of the TiO2/water interaction as combined with complementary spectroscopic information.
The SFVS experiments were carried out with a femtosecond broadband laser system. Briefly, a Ti:sapphire amplifier (Spitfire ACE, Spectra Physics) produces ∼7 W of 800 nm, 35 fs pulses at a 2 kHz repetition rate. 35% of the 800 nm beam passed through a beam-splitter to pump an optical parameter amplifier, followed by a difference frequency generation stage (TOPAS-C, Spectra Physics). The rest of the light was either used to generate a narrowband beam of approximately 3 nm bandwidth by passing through an interference filter (LL01-808-25, Semrock) or reflected from a Bragg filter (N013-14-A2, OptiGrate) to generate a narrowband beam of approximately 0.5 nm bandwidth. The broadband IR and narrowband 800 nm pulses overlapped at the sample surface with incident angles of 57° and 30° (or 45°), respectively. The SF signal was collected along the reflected direction using a spectrograph (Acton SP300i, Princeton Instruments) and a CCD camera (PyLoN: 400BR eXcelon, Princeton Instruments). All SFVS measurements were conducted under ambient conditions at room temperature. The relative humidity (RH) of the environment was maintained at 40%.
We further used Raman spectroscopy and XRD to characterize the TiO2 films.13,24 Both Raman and XRD spectra of the as-grown sample showed no characteristic peaks of crystalline TiO2, indicating amorphous nature (Fig. 1e and f, black curves). (The Raman signals observed at 300 cm−1 and 517 cm−1, as well as the diffraction peak at 33°, were all due to the Si substrate.) After annealing at 400 °C, the sample turned into the anatase phase, characterized by prominent Raman peaks at 140 and 632 cm−1 (Fig. 1e, red curve).13 Meanwhile, the XRD analysis of the annealed sample showed four distinct peaks at 25.4°, 33°, 38°, and 48.2°, corresponding to anatase (101), (004), and (200), and the peak at 33° was from Si (200) (Fig. 1f, red curve).24
To further verify our assignment of both surface modes, we conducted UV and annealing treatments of the TiO2 surface. First, we irradiated an as-grown sample surface with UV light, which is known to promote the water dissociation on TiO2 surfaces under ambient conditions.28–30 The contrasting spectra before (black) and after (purple) UV irradiation of the as-grown TiO2 film are shown in Fig. 2b. The UV irradiation caused a notable increase in the intensity of the 1060 cm−1 mode, in accordance with its assignment to the TiOH species. Besides, the low-frequency intensity grew after the treatment, possibly contributed from UV-generated free carriers.31 Next, we annealed the as-grown samples at 400 °C for 4 hours, which would remove adsorbed water molecules and hydroxyl groups from the TiO2 surfaces.32,33 As shown in Fig. 2b (red), the 1060 cm−1 peak intensity of the annealed sample decreased drastically, which again is consistent with our assignment. This 1060 cm−1 band can therefore characterize the dissociated TiOH species on TiO2.
Meanwhile, the SF signal near ∼900 cm−1 grew appreciably upon annealing (Fig. 2b, red), showing a strong peak at 870 cm−1, closely resembling the surface phonon mode on single crystalline anatase (101) (Fig. 2b, grey dashed curve, adopted from ref. 20). This is consistent with the Raman and XRD results shown above (Fig. 1e and f), that the thermal annealing treatment converted the amorphous sample to the (poly)crystalline anatase phase. Such conversion underscored our assignment of the low-frequency mode to the vibration of surface Ti–O bonds. Overall, the TiO2 samples exhibited multiple peaks near ∼900 cm−1, with the single crystalline sample dominated by the peak at ∼870 cm−1, and amorphous samples by the peak at ∼900 cm−1. The higher frequency on the amorphous surface possibly arose from the structural variation in Ti–O bond length, Ti–O–Ti bonding angle, and/or the localization of the vibrational mode. Collectively, the UV and thermal annealing treatments agreed with our assignment of the spectral features. Fig. 2d schematically summarizes the structural changes of the amorphous TiO2 surface upon UV and annealing treatments.
It is noted that, in contrast to the amorphous TiO2 surface, our previous study on the single crystalline anatase (101) surface did not observe TiOH resonance under ambient conditions.20 Even for the annealed (poly)crystalline sample, the UV irradiation afterwards could not restore the TiOH signal (Fig. 2c). Overall, since annealing (UV irradiation) would reduce (increase) the amount of structural defects, the corresponding drop (increase) in the TiOH signal intensity upon the above treatments emphasizes that surface structural defects, including oxygen vacancies (VO) and others, are crucial in promoting the auto-dissociation of water in the ambient atmosphere.
Upon exposure to methanol, spectra in the C–H stretching vibrational frequency range showed major resonance bands centered at 2850–2870 cm−1, 2960–2980 cm−1, and 2990–3050 cm−1 (Fig. 3a, see details in the ESI†). Some of the modes appeared as dips due to their interference with the non-resonant background of the TiO2 surface.20,35 These modes can be assigned to the CH3 symmetric stretching mode (r+), its Fermi resonance mode with the bending overtone (FR-r+), antisymmetric stretching and/or OH stretching mode from physisorbed methanol molecules,22 respectively. Meanwhile, we observed notable SF responses at the lower frequency sides of the methanol r+ and FR-r+ peaks, marked by dashed lines in Fig. 3a, which was absent on single crystalline TiO2 surfaces including anatase (101) (presented in the inset of Fig. 3a) and rutile (110), (001), and (100).22 According to the literature,16,36 these modes arise from the CH3 symmetric stretching of methoxy species (CH3O) dissociated from methanol. Observation of these modes indicated the auto-dissociation of methanol on the amorphous TiO2 film. Again, this showcases the essential role played by TiO2 structural defects in methanol dissociation. Fig. 3b illustrates the time-dependent magnitudes of the fitted amplitudes of methanol r+ and FR-r+ modes, as well as the methoxy r+ mode (magnified by 4 times for clarity). The background colour of Fig. 3b was matched that of the corresponding SF spectrum in Fig. 3a to guide the eye. It was seen that all three amplitudes rose simultaneously and reached the maxima at t = 2–3 minutes, then diminished at t ≈ 5 minutes. The same adsorption/desorption processes were repeatable for multiple cycles.
We then acquired Ti–O spectra under the same conditions to track the changes of the TiO2 surface structure. The low-frequency mode near ∼900 cm−1 did not exhibit notable changes upon methanol adsorption/desorption (see Fig. S3 in the ESI†). In contrast, the high-frequency band from TiOH groups evolved in close correlation with the methanol response, as shown in Fig. 3c. The black dotted curve represents the spectrum before methanol adsorption. Within the first 2–3 minutes, the intensity of the TiOH band dropped rapidly in accordance with the methanol adsorption, showing the titration behaviour between methanol and water. Meanwhile, the band split into two bands at ∼1000 and 1070 cm−1, respectively (see details in the ESI†). After t ≈ 3 minutes, upon methanol desorption, the TiOH band started to increase but at a much slower pace, and eventually recovered to the initial profile in about 20 minutes. By analysing the time-dependent TiOH spectra, we found that all spectra could be fitted with two bands around 990–1010 cm−1 and 1060–1070 cm−1, respectively. According to ref. 37, the frequency of the R–O–H bending mode is affected by the hydrogen bonding (H-bonding) environment. The stronger the H-bonding it senses, the higher the R–O–H bending frequency becomes. We therefore attribute the bands near 1000 cm−1 and 1060 cm−1 to weak and strong H-bonded TiOH groups, respectively. Fig. 3d displays the time-dependent amplitudes of the two modes extracted from fitting (solid curves), as well as their combined amplitude for reference (dot curve). The amplitudes were all normalized to their respective values at t = 0 minute.
With both CH and TiOH spectra available, we now discuss the microscopic picture underlying the titration procedure. Before introducing methanol molecules, the TiO2 surface is covered by both molecular water17 and dissociated OH groups (Fig. 3e). Upon the introduction of methanol vapor (t = 0–2 minute), both physisorption and chemisorption of methanol would occur. Fig. 3e (left panel ①) presents the typical physisorption scheme of methanol molecules, which could replace physisorbed water molecules on both surface Ti and bridging oxygen (Obr) sites. Accordingly, we observed the increase of the r+ and FR-r+ amplitudes of methanol molecules. Although physisorbed methanol molecules could not directly replace TiOH groups, they would weaken the overall surface H-bonding network, as methanol cannot form as many H-bonds as water per molecule. This agreed with the trend observed in Fig. 3d, that when the intensities of both strong and weak H-bonded TiOH groups dropped within the first few minutes, the former dropped more rapidly than the latter due to the overall weakened surface H-bonding network.
For the chemisorption of methanol, it involves the dissociation of methanol molecules into methoxy groups via the reaction with surface terminal hydrogen groups, described by CH3OH (g) + Ti–OH → CH3O–Ti + H2O (g) (Fig. 3e, right panel ①).12 Meanwhile, as mentioned earlier, the strong H-bonded TiOH groups dropped more rapidly than weak H-bonded ones (Fig. 3d). This may also be contributed by the proton transfer process involved in the above reaction facilitated by the H-bonding network.38 In addition, as we previously observed on anatase (101), the configuration energy of surface VO could be lower upon the adsorption of methanol.20 This could further facilitate the methanol dissociation in a “self-catalysis” manner as demonstrated in ref. 39, that a methanol molecule would auto-dissociate on the surface VO site.
We could further estimate the coverage of TiOH groups based on the above results. By assuming a one-to-one conversion between methoxy and desorbed TiOH species, we derived that the coverage of TiOH is about 72.5% ± 14.5% under ambient conditions (1 atm, RH = 40%, see details in the ESI†). This value is greater than that predicted for pristine crystalline surfaces,5 for example, 20–30% on rutile (110),6 but is close to the 75% found by SXRD on heavily reduced anatase (101) in the ambient atmosphere.11
At 3–5 minutes, the methanol started to desorb. The physisorbed methanol molecules could simply leave the surface (Fig. 3e, left panel ② and ③). For chemisorbed methoxy species, they are usually assumed to be hydrolysed by water via CH3O–Ti + H2O (g) → CH3OH (g) + Ti–OH.40 However, this reaction would lead to TiOH formation, yet the TiOH intensity hardly increased during the same period of time. Such an observation suggested that, in our case, the methoxy desorption could also occur via processes other than hydrolysis. One possibility is that the chemisorbed methoxy could recombine with neighbouring protons on Obr sites and desorb from the surface (Fig. 3e, right panel ②). Meanwhile, the slow recovery of the TiOH signal in comparison to the rapid rise of the methoxy signal (upon adsorption) is in accordance with the fact that methoxy adsorbs more favorably than water.
Footnotes |
† Electronic supplementary information (ESI) available. See DOI: https://doi.org/10.1039/d5cp00400d |
‡ These authors contributed equally to this work. |
This journal is © the Owner Societies 2025 |