Structure-specific synthesis processes are of key importance to the growth of polymorphic functional compounds such as TiO2, where material properties strongly depend on structure as well as chemistry. The robust growth of the brookite polymorph of TiO2, a promising photocatalyst, has been difficult in both powder and thin-film forms due to the disparity of reported synthesis techniques, their highly specific nature, and lack of mechanistic understanding. In this work, we report the growth of high-fraction (~95%) brookite thin films prepared by annealing amorphous titania precursor films deposited by pulsed laser deposition. We characterize the crystallization process, eliminating the previously suggested roles of substrate templating and Na helper ions in driving brookite formation. Instead, we link phase selection directly to film thickness, offering a novel, generalizable route to brookite growth that does not rely on the presence of extraneous elements or particular lattice-matched substrates. In addition to providing a new synthesis route to brookite thin films, our results take a step towards resolving the problem of phase selection in TiO2 growth, contributing to the further development of this promising functional material.


TiO2 can form in many structures, the most prominent of which are the naturally-occurring rutile, anatase and brookite polymorphs depicted in Fig. 1, although many other synthetically prepared structures have been reported1,2. Rutile, the ground state, and anatase are by far the most common and find many applications3,4, from paint pigments to transparent conductors and photocatalysts. Brookite is seeing renewed interest5,6,7, with a rutile/brookite mixture serving as effective photocatalysts and outperforming Degussa P25 (an anatase/rutile mixture commonly used to degrade organic pollutants) at degrading both rhodamine B and methyl orange. Furthermore, through surface engineering, brookite can become either oxidative or reductive8 depending on the exposed surface ((201) or (210) respectively), adding versatility as a catalyst. However, the synthesis of high-quality brookite has proven much more difficult than that of rutile and anatase, motivating us to study its formation in the form of a functionally-relevant thin film.

Figure 1
Figure 1

Crystal structures of TiO2 rutile (tetragonal, P42/mmm), brookite (orthorhombic, Pbca) and anatase (tetragonal, I41/amd) polymorphs.

Designing a synthesis route to a metastable phase such as brookite requires the knowledge of both equilibrium and non-equilibrium reactions that could occur9. Although phase diagrams of the bulk Ti-O system under standard conditions are established, phase selection during synthesis is not merely a matter of bulk equilibrium thermodynamics, as evidenced by the ubiquity of metastable, non-equilibrium synthesis products, which include anatase and brookite. As reported in similar ionic systems, synthesis routes to various stable and metastable phases can be driven by finite-size effects10, nucleation kinetics11,12, bulk and surface off-stoichiometry13,14 and others15,16. Table 1 lists several proposed stabilization mechanisms for the common TiO2 polymorphs, as well as the conditions driving their transformations. In the case of brookite, it appears that the most efficient reactions leading to the bulk material are crystallization by sol-gel and hydrothermal techniques in the presence of Na or some other alkali ion spectators17,18. However, there is no established mechanistic understanding of these synthesis routes. Moving further beyond bulk synthesis, the growth of materials as thin-films opens the door to high-energy synthesis methods such as sputtering and pulsed laser deposition (PLD). Although thin films of brookite have been obtained by vapour deposition on lattice-matched substrates19,20,21,22 (Table 2), the non-equilibrium growth of high-purity brookite on amorphous substrates has been largely unexplored.

Table 1 Formation mechanisms reported for some metastable TiO2 polymorphs.
Table 2 Vapour deposition of phase pure brookite reported in the literature.

The lack of a clear and consistent mechanistic understanding of brookite growth explains the wide variety of hydrothermal and sol-gel synthesis approaches found in literature3,4. Some reports find that high concentrations of NaOH lead to the best brookite samples23, while others use a combination of inorganic and organic precursors to produce phase pure brookite24, and others report pure brookite based on a delicate balance between Cl ion concentration, pH, and the necessity of the [Ti(OH)2(Cl)2(OH2)2]0 salt as a brookite precursor25. One common thread between these recipes is the use of some ionic complexing agent (Na+, C2O4 2−, or Cl) to favor the structural selection of brookite in large quantities. However, vapour deposition processes inspired by the proposed growth mechanisms do not consistently lead to the same results26.

One of the reasons for the discrepancies between solution-based and vapour-based results, and the difficulty of synthesizing brookite via the vapour phase, and in particular by physical vapour deposition (PVD), could be the delicate balance of thermodynamic forces favoring each polymorph10, which is difficult to transfer precisely between growth techniques. Another possibility is that helper species present during hydrothermal or sol-gel growth (e.g. Na+, C2O4 2−, Cl) are not typically used during PVD growth, limiting the accessible pathways to the ones without these helper species. As a result, to date synthesis of pure brookite by vapour deposition has relied on highly specific stabilization mechanisms, namely substrate lattice-matching, to produce any thickness of thin-film brookite. The first study to produce brookite via vapour deposition22 relied on plasma-enhanced chemical vapour deposition (PECVD) with titanium tetra-isopropoxide (a common precursor used in TiO2 hydrothermal growth) vapour on (100)-oriented silicon substrates. Other works19,21 have reported lattice-matched brookite growth on (110) yttria-stabilized zirconia (YSZ) by plasma-enhanced atomic layer deposition (PEALD) and metal-organic chemical vapour deposition (MOCVD), reporting an in-plane orientation of [001]brookite//[001]YSZ and an out-of-plane orientation of [120]brookite//[110]YSZ. In one case, a brookite nanorod film was reported20 grown by matrix-assisted pulsed laser evaporation (MAPLE), using a target made from a suspension of solution-synthesized brookite nanorods frozen in liquid nitrogen, onto (100) Si substrates. Furthermore, of the brookite formation studies on amorphous glass substrates27,28, the highest brookite fraction reported to date is 45 ± 15%27 with the remaining film composed of rutile and anatase. Thus, despite the relative abundance of synthesis routes yielding brookite from solution, there remains no established mechanism reported for the formation of high-fraction brookite on general, non-lattice-matched or amorphous substrates.

In this work, we report a simple, substrate agnostic synthesis route that produces a high fraction of the brookite phase in a thin film by PLD of amorphous TiO2 and subsequent annealing. We characterize the growth process and resulting films through 2D synchrotron X-ray diffraction (XRD), 2D micro-Raman spectroscopy, high resolution transmission electron microscopy (HRTEM), energy dispersive X-ray spectroscopy (EDS) and first-principles calculations to confirm the presence of brookite and discuss the possible mechanisms leading to its formation. We are able to produce thin films with more than 90% brookite, document the interplay of brookite with the more common rutile and anatase polymorphs, and eliminate a number of reaction mechanisms previously proposed on the basis of sol-gel and hydrothermal growth results. Specifically, we investigate the proposed role of Na in promoting brookite growth as it migrates into the growing film from the substrate26,29,30, and demonstrate that contrary to previous reports17,18, brookite growth does not depend on the presence of Na. Instead, the nucleation and growth of brookite appears to rely on processing and structural properties such as film thickness.



Based on a variety of hydrothermal and sol-gel brookite synthesis recipes, a common claim is that the presence of sodium during TiO2 growth promotes the formation of the brookite phase17,18. To investigate the thermodynamic feasibility of this claim, we evaluate the thermodynamics of sodium incorporation into various known TiO2 phases. This analysis follows by analogy to the recently reported role of alkali ions in the formation of MnO2 polymorphs through the stabilization of off-stoichiometric intermediate products13. To identify possible off-stoichiometric intermediates, we examine the formation of partially sodiated NaxTiO2+y compounds, with Na+ incorporated into the Ti-O matrices of each phase (rutile, brookite, and anatase, as well as the bronze, layered, and postspinel structures) which are known to form in the Na-TiO2 space31, so that the NaxTiO2+y phases may template the growth of a particular Ti-O framework. To enumerate the NaxTiO2+y structures that may play a role in such a mechanism, we consider Na+ incorporation either through the partial reduction of Ti4+ to Ti3+, or the formation of Ti4+ vacancies (equivalent to the incorporation of Na2O). Note, we do not consider the incorporation of purely interstitial Na2O as none of the TiO2 polymorphs contain interstitial sites large enough for such defects. We then evaluate the stability of these structures by comparing their energies to that of all known phases in the NaxTiO2 and Na2yTiO2+y spaces, regardless of Ti-O framework.

The low-temperature, low-pressure thermodynamics of NaxTiO2+y compounds, shown as heats of formation in Fig. 2(a) and (b), do not support the previously hypothesized role of sodium in brookite formation, at least via the formation of a bulk-sodiated intermediate. In the case of Na+ intercalation alongside Ti4+/3+ reduction, the stabilized phases are TiO2-bronze at low sodium content, post-spinel at intermediate sodiation, and layered-TiO2 at high sodiation. These results are consistent with both reported crystal structures in this space31, and the observation that small levels of sodiation appear to favor the TiO2-bronze phase26. Similarly, Na2O incorporation is most favorable in the TiO2-bronze phase, and generally leads to the well-known Na2Ti3O7 titanate structure, which is not topotactically related to any of the TiO2 polymorphs we consider. While these results are obtained for zero-temperature conditions, the large difference in Na-defect energies seen in Fig. 2 would make the entropic stabilization of sodiated brookite over the competing phases highly unlikely. Of course, it is possible that the role of sodium in previous experiments was not to influence the relative stability of TiO2-phases through bulk incorporation – for example, sodium may selectively influence the surface energies of specific TiO2 polymorphs, thereby affecting their relative nucleation kinetics, analogous to the role of Mg2+ ions in influencing CaCO3 polymorphism12. While we expect that the impact of surface sodium on the relative surface energies of the TiO2 polymorphs would be limited to 0.1 J/m2,13 a rigorous analysis of sodiated TiO2 interfaces would be necessary to ascertain the exact behavior of interfacial Na, and falls outside the scope of this work. Nonetheless, our analysis suggests that sodium may not be essential to brookite formation, motivating our further experimental study of brookite growth in both sodium-containing and sodium-free media.

Figure 2
Figure 2

Computed low-temperature free energies of (a) NaxTiO2 and (b) Na2yTiO2+y compounds, with Ti-O frameworks constrained to those of known TiO2 phases, as a representative sample of structure selection in the NaxTiO2+y chemical space. The dotted lines denote the global thermodynamic equilibrium in each composition space.

Observation of brookite in films on different substrates

Amorphous TiO2 films deposited on a variety of amorphous substrates, and annealed as described in the methods section, consistently produce crystalline films with varying quantities of brookite and anatase, and sometimes rutile, regardless of whether the substrate is sodium-free (pure fused silica (a-SiO2) or Si with thermally-grown oxide) or sodium-containing glass (Corning Eagle XG (EXG) with low Na content, or soda-lime-silicate (SLS) with high Na content). Na clearly plays no role in the brookite formation on the Na-free substrates. We detail below the identification of various titania phases in a typical film deposited on low-Na EXG glass. Notably, we find no evidence of Na migration into that film. If sodium incorporation were indeed favorable, sodium migration from the substrate would have produced sodiated TiO2 26,29,30. We find the fraction of brookite produced in this process is controlled by the thickness of the film and the time and temperature of the anneal, rather than the substrate and the presence of Na+.

Figure 3 shows background-subtracted, integrated 2D XRD spectra of TiO2 films, 58 nm and 52 nm thick, on Na-free fused SiO2 and Na-containing EXG glass substrates respectively, obtained after annealing. The strong brookite signature in films on both Na-containing and Na-free substrates is evident from the XRD peak at Q = 2.166 Å−1. This result shows that films of the same thickness that are annealed under the same conditions can produce similar mixed phase brookite and anatase films regardless of the presence of Na in the substrate. These are examples of high-fraction brookite films (>70% brookite), where the fraction is quantified from the optical and Raman maps as discussed below.

Figure 3
Figure 3

Room temperature XRD patterns of TiO2 films grown on a-SiO2 and EXG substrates annealed following a protocol similar to that shown in Fig. 4. Optical images of these films appear in Fig. S3. The brookite and anatase phases appear in similar proportions in films on both substrates.

To explore the annealing process and progression of the crystalline phases, we use in-situ XRD during annealing. Figure 4 shows the in-situ XRD evidence from a 65-nm TiO2 (measured by HRTEM) film on amorphous EXG glass annealed in N2 according to the annealing profile shown in gray. Brookite is tracked by the (121) peak at Q = 2.166 Å−1 which provides a clear signature because it is strong and isolated from the other polymorph peaks. Anatase is tracked by its (101) peak at Q = 1.787 Å−1, which is very strong but close to a moderately strong brookite peak. This particular film has a relatively low fraction of brookite (<20%) which makes the anatase identification unambiguous in XRD (an example 2D XRD spectrum can be seen in Fig. S1). Here we observe the crystallization of brookite and anatase TiO2 phases at ~290 °C. When the experiment is repeated, we consistently observe that the anatase and brookite polymorphs form concurrently. The polymorphs quickly achieve their final steady-state phase fractions, as evidenced by the lack of change in peak area after 200 secs. In contrast to crystallization from solution, which is often dominated by one polymorph at a time32, the concurrent formation of two separate polymorphs here suggests independent nucleation events, likely at different locations of the substrate. There is minimal transformation of the two phases after formation. Gibbs’ phase rule suggests that there can only be one polymorph at equilibrium in the film at a time, so the persistence of a two-polymorph thin film suggests slow coarsening kinetics, which is likely due to limited transport kinetics in thin films.

Figure 4
Figure 4

The integrated peak areas for brookite (121) [blue] and anatase (101) [green] on a 65-nm film, grown on EXG, as a function of time and temperature during the anneal indicated by the gray line. Both polymorphs crystallize at ~290 °C.

Figure 5 shows optical and Raman images of the mixed-phase brookite/anatase film in Fig. 6. Figure 5a is an optical image, with clear contrast evident on the micron length scale. The lighter regions, labeled B, are characterized by the Raman spectrum in Fig. 5b which matches the brookite spectrum in the RRUFF database (RRUFFID R050591)33. The darker regions, labeled A, yield the Raman spectrum in Fig. 5c, which matches anatase (RRUFFID R070582)33. With the Raman shift tuned to 319 cm−1 (brookite) and 144 cm−1 (primarily anatase), the laser is scanned over the region marked by the red square in Fig. 5a, and the 2D maps in Fig. 5d and e, respectively, are obtained. The shapes evident in the optical image, which presumably result from refractive index contrast (n rutile = 2.72, n brookite = 2.64, n anatase = 2.53)34, are replicated in the Raman maps, giving an unambiguous polymorph identification. The optical contrast therefore provides a quick and convenient “first-cut” polymorph identification method, which can then be confirmed with Raman or electron microscopy. From the 2D Raman maps or the optical images, it is easy to convert the A and B areas to polymorph fractions, which for this film is 50% brookite to 50% anatase. Associating the area with a volume phase fraction assumes the surface structures permeate the film.

Figure 5
Figure 5

(a) Optical image (100x magnification) of a 65-nm TiO2 film on EXG glass. Regions marked B yield the Raman spectrum for brookite in (b), while those marked A yield the anatase spectrum in (c). The 2D Raman maps at 319 cm−1 (d) and 144 cm−1 (e) show that the color variations in the optical image correlate with a particular polymorph. The brookite:anatase ratio in this film is 50:50 and no rutile is observed. The dotted lines in (b) and (c) indicate the wavenumber range over which the Raman intensity maps in (d) and (e), respectively, are acquired.

Figure 6
Figure 6

HRTEM image of a 50-nm TiO2 film on EXG glass annealed following a protocol similar to that shown in Fig. 4. The selected area electron diffraction patterns in the insets indicate that the grain on the left is anatase and on the right, is brookite. The S-shaped grain boundary is approximately 20 nm wide.

Cross-sectional TEM analysis in Fig. 6 shows that the grains do indeed occupy the entire film thickness and can be considered columnar on a micron-scale. Figure 6 also provides further phase confirmation by the electron diffraction shown in the insets. The TEM image shows an anatase-brookite grain boundary, which changes curvature from the top of the film to the bottom. This S-shape extends over a 20-nm range perpendicular to the boundary. Due to a balance of forces indicated by the point of inflection, boundary mobility and further grain growth are significantly reduced, again suggesting that phase stability is kinetically limited35. The in-situ XRD studies in Fig. 4 also suggest a rapid settling into a particular morphological configuration after a rapid nucleation, shown by the plateau in intensity after crystallization. Further experiments are needed to understand the details of the nucleation and growth of the polymorphs and the nature of the phase boundary.

EDS analysis of Ti, O and Na is shown in Fig. 7 of two films grown on EXG and annealed in a manner similar to the film in Fig. 4. The TiO2 stoichiometry is confirmed by EDS and there is no change in stoichiometry at or near the grain boundary (<0.35 at%). There is no evidence of Na migration into the film, nor into the grain boundary. There is a clear accumulation of Na in the substrate near the substrate film/interface, however.

Figure 7
Figure 7

(a,b) Elemental EDS map and plot trace across the substrate/film interface of the film shown in Fig. 4. (c,d) Elemental EDS map and plot trace showing an anatase/brookite phase boundary in the film shown in Fig. 6. Na (green) is below the detection limit in the TiO2 films and accumulates near the film-substrate interface.

Film thickness and polymorph fraction

We have reproduced the results described above in many films made on different amorphous substrates that are Na-containing (EXG and SLS) and Na-free (a-SiO2 and Si with 100 nm of thermal oxide). Figure 8 shows the results of a phase fraction analysis of a set of samples annealed with the standard protocol described in the methods section using maximum temperature hold times of 0 or 1 minute at 400 °C. (The set includes only films annealed in the same oven to keep the processing variables as similar as possible. In particular, it excludes the film in Fig. 4, where the in-situ anneal was used to establish a protocol that would yield brookite.) There is a thickness gradient across most films, which allows the observed phase fraction to be correlated to the thickness of the film in that region. The data in Fig. 8 represent 10 different depositions, with the different classes of substrate denoted by the symbol shape. Each deposition yields several entries on the plot because the film thickness varies across the sample. At each thickness, there are four color-coded points representing the brookite, anatase, rutile and amorphous fractions, averaged over an area approximately 150 µm × 150 µm. One striking feature is that films with brookite as the major phase (above 70% and up to 95%) are clustered in the thickness range of 45 to 65 nm. At the lowest thicknesses, below ~30 nm, anatase is the major phase. Between 30 nm and 45 nm, brookite as the dominant crystalline phase is accompanied by the presence of an amorphous component. This transition corresponds with the size-dependent stabilization order identified by Ranade et al.10 for TiO2 crystallites in solution. Rutile is absent or a minor phase for most of our films; examples of rutile-containing films are given in Figs S2 and S3.

Figure 8
Figure 8

Phase fraction of brookite (blue), rutile (red) and anatase (green) polymorph or amorphous component (gray) in TiO2 films as a function of thickness. Na-free a-SiO2 and Si/SiO2 (circles), low-Na EXG (squares) and high-Na SLS (diamonds) substrates are represented. The uncertainty in thickness is ±5 nm for d <50 nm and ±3 nm for d >50 nm.


Synthetic routes to brookite TiO2 via solution growth suggest that the presence of Na+ cations is a driver of the formation of the brookite phase. However, we observe that sodium is not critical to the formation of brookite, on the basis of first-principles calculations, which show that addition of Na into the system does not favor brookite, and because brookite thin film growth occurs independent of the presence or absence of sodium from the substrate. Our analysis suggests it is possible to synthesize brookite TiO2 films by PLD on a wide range of substrates, independent of substrate composition and orientation, such as Na-free SiO2.

By characterizing the conditions favoring the formation of the brookite phase, we find with this annealing protocol and amorphous films, that brookite preferentially forms in a film thickness range of 45–65 nm, with anatase appearing at smaller film thicknesses. This trend of brookite formation in an intermediate size regime is analogous to the intermediate-size stabilization of brookite in solution growth10, although the mechanistic relationship between solid-liquid surface energies relevant to phase selection in nanoparticles, and thickness effects in thin films is not clear. The in-situ x-ray study tracking the annealing of the as-deposited amorphous films shows that after an initial crystalline phase forms, few if any transformations occur. This result suggests that phase selection likely occurs during single, independent nucleation events, which can be controlled through annealing rates and final annealing temperatures to possibly achieve phase-pure brookite thin films without the need for assisted growth methods such as epitaxy.

In summary, we synthesize high-phase-fraction (~95%) brookite TiO2 thin films by PLD on both sodium-free and sodium-containing amorphous substrates and identify an ideal thickness region for forming the brookite phase with this annealing protocol. We track the formation of the brookite, anatase, and rutile phases via Raman mapping, TEM and in-situ XRD and trace their predominance to the processing conditions used, eliminating the previously hypothesized role of Na incorporation as a mechanism for brookite stabilization in thin films. Our results suggest that instead, phase selection in the films is dictated by a single nucleation event, which can be controlled through film processing and structure.



To model the thermodynamics of possible growth mechanisms we use density functional theory (DFT) as implemented in the Vienna Ab-Initio Simulation Package (VASP)36, relying on the SCAN exchange-correlation functional37, projector augmented wave method38, and a reciprocal space discretization of 25 Å−1. We choose the SCAN functional as it was recently demonstrated to generally produce accurate results in phase selection among polymorphs in similar systems14, and accurate formation energies for titanium oxides in our own benchmarking.

We evaluate the effect of sodium incorporation into titania polymorphs (i) as accompanied by reduction of Ti, and (ii) as a neutral Na2O defect. We enumerate likely phases in the TiO2 NaTiO2 and TiO2 Na2Ti3O7 spaces respectively, including all known sodiated titania structures (bronze, post spinel, layered, sodium titanate) as well as the common TiO2 polymorphs of interest here (rutile, brookite, anatase). In the case of Na+ intercalation, we consider both isolated defects and symmetrically distinct orderings on the possible interstitial sublattices in each phase, and obtain the lowest energy configuration across all NaxTiO2 compositions. To access the Na2Odefect thermodynamics, we enumerate dilute Na2O in TiO2 defect configurations, formed by creating a Ti4+ vacancy and charge compensating it with 4 Na+ ions, over all likely configurations of the sodium ions. In all cases, to correct the well-known problem of reproducing the energy of rutile versus brookite and anatase39, brookite and anatase phases are shifted to +0.007 meV/TiO2 and +0.023 meV/TiO2 with respect to pure rutile respectively, based on experimentally-obtained enthalpies of the three phases10. While no similar correction enthalpies are known for the bronze, post spinel, and layered phases, no enthalpy shift of these phases within expected DFT error ranges changes which phase is stabilized in both the Na and Na2O cases.

Film deposition and annealing

Using PLD, we deposit amorphous TiO2 films on Corning Eagle XG glass (EXG, MTI corporation), soda-lime silicate microscope slides (SLS, Corning 0215), fused quartz (aSiO2, GM associates), and p-type silicon with a 100-nm-thick thermal oxide (MTI corporation). According to the specification sheets, EXG glass has 0.1 wt. % alkali content, SLS has 14% Na2O and the fused quartz and p-Si substrates are Na-free. Before deposition, substrates are cleaned with a 1% solution of Liqui-Nox (Cole-Palmer)/deionized water and rinsed in deionized water followed by five-minute ultrasound baths in acetone and then in isopropyl alcohol. Substrates are then dried with compressed nitrogen and stored in a warming oven at 120 °C in ambient atmosphere, until being transferred to the vacuum chamber for deposition.

The films are deposited at room temperature in a vacuum chamber with base pressure near 5 × 10−7 Torr, purged with ultra-high purity oxygen for five minutes, and then held at 1.0 mTorr during deposition. Substrates are typically 2 cm × 3 cm and are held stationary at a target-to-substrate distance of 12 cm. This distance produces a thickness variation of about 30% across an individual sample, which is useful to investigate the polymorph fraction as a function of thickness. The ceramic target (99.998% TiO2, Materion) is rotated during deposition to obtain uniform ablation. The output energy from the Lambda Physik KrF excimer laser (λ = 248 nm, ~10 ns pulse duration, and 10 Hz repetition rate) is 150 mJ. The laser energy on the target is 60 mJ giving a laser fluence of 0.54 Jcm−2. To ensure repeatability, we deposit films in two different chambers at NREL and OSU using similar deposition conditions. The substrates are large enough that they can be cleaved into four sub-samples so that the same amorphous precursor can be processed or analyzed in different ways.

After deposition, the amorphous TiO2 films are annealed in one of two ways. For in-situ XRD characterization, the anneal occurs in the sample holder in the SSRL beamline according to protocols like that shown in Fig. 4 (0.25 L min−1 flowing N2 with a heating rate of approximately 60 °C min−1 and a cooling rate of approximately 110 °C min−1). Otherwise, the anneal occurs in an AET Thermal RX Series Rapid Thermal Processing system under flowing N2 with a flow rate of approximately 10 L min−1. The peak temperature and processing times are chosen to be near those found at SSRL to produce the brookite and anatase polymorphs. The standard protocol is to ramp to 340 °C at 50 °C min−1, then to 400 °C at 20 °C min−1, hold at 400 °C for 0 or 1 min, and cool to ambient at 110 °C min−1. The films depicted in Fig. 8 have hold times of 0 or 1 minute; the hold time was not a strong influence.

Optical Spectroscopy

Because the substrate is not rotated during deposition, a thickness variation in the TiO2 films is visible as a color gradation in the reflected light. The thickness is quantified using reflection and transmission spectroscopy. Spectra are acquired in the range 250 to 1000 nm using a UV-enhanced xenon light source, a diffraction grating double monochromator and a Si photodetector. With the light beam focused to ~1 mm diameter, reflection (R) and transmission (T) spectra are acquired in 3–4 different locations across each cleaved sample. The spectra exhibit the intensity modulation characteristic of thin-film interference. T, R and the interference-free transmission40 T/(1-R) ≈ exp(-αd) are fit using established models41 with film thickness and film index of refraction as fit parameters, and standard Sellmeier coefficients to give the wavelength-dependent refractive index for the substrate42. The evolution of the optical spectra (see Fig. S4) make clear the relative thickness, however, even if the absolute thickness has some error. Optically determined thicknesses are consistent with those measured by cross-sectional TEM on selected samples.

Raman Spectroscopy

Micro-Raman spectroscopy is performed using a Horiba Jobin-Yvon LabRam800 with 532-nm laser excitation and a beam of about 1 µm in diameter. Data are processed using the LabSpec 5.0 software suite. After background subtraction, peaks are fit with Gaussian functions to identify peak position, amplitude, width, and compared to reference spectra reported in the RRUFF database33 for polymorph identification. 2D micro-Raman mapping is performed by inserting a motorized mirror in the laser beam line allowing the laser to be positioned and scanned across the sample, with the detector tuned to the desired wavelength range indicated between the dashed lines in Figs 5b,c, and S4f–h. Optical images are acquired using the Raman system optical microscope, which has 10x, 20x, 50x and 100x objective lenses. Polymorph fraction is calculated from 2D Raman maps or from corresponding 100x optical images over an area of approximately 150 µm × 150 µm.

X-Ray Diffraction

XRD is performed using the Stanford Synchrotron Radiation Lightsource (SSRL) Beamline 11–3 with an X-ray energy of 12.7 keV. The x-ray beam dimensions are 3 mm by 0.1 mm. Two-dimensional scattering data are collected using a Rayonex charge-coupled device and in a grazing incidence geometry with the x-ray beam held at an incident angle of 3°. Images are calibrated using a LaB6 standard and integrated between 10° < χ < 170° (χ is the polar angle) using GSAS-II43. The background due to the amorphous substrate is subtracted using the CrystalMaker software package.

Transmission Electron Microscopy

TEM micrographs are acquired with an FEI Co. Talos F200X transmission electron microscope with scanning capabilities operating at an accelerating voltage of 200 keV. Specimens for TEM are prepared from deposited films via in-situ focused ion beam lift-out methods44 using an FEI Co. Helios Nanolab 600i SEM/FIB DualBeam workstation. Specimens are ion milled at 2 keV and 77 pA to remove Ga ion beam damage and achieve a final thickness of approximately 80 nm. Structural characterization is conducted by acquiring selected area electron diffraction (SAED) patterns on an FEI Co. Ceta 16 M pixel CMOS camera at a camera length of 410 mm. Platinum from the FIB is used to calibrate the camera constant, allowing SAED reflections to be accurately measured and indexed. Chemical mapping is performed in the TEM using the Super-X energy-dispersive X-ray spectroscopy (EDS) system equipped with four windowless silicon drift detectors, allowing for high count rates and chemical sensitivity to 1 atomic percent.

All data needed to evaluate the conclusions in the paper are present in the paper and the Supplementary Materials. Additional data related to this paper may be requested from the authors.

Data availability

All datasets are available from the corresponding author upon reasonable request.

Additional information

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


  1. 1.

    Liu, Q.-J. et al. Structural, elastic, electronic and optical properties of various mineral phases of TiO2 from first-principles calculations. Phys. Scripta 89, 075703 (2014).

  2. 2.

    Buckeridge, J. et al. Polymorph engineering of TiO2: demonstrating how absolute reference potentials are determined by local coordination. Chem. Mater. 27, 3644–3851 (2015).

  3. 3.

    Hanaor, D. A. H. & Sorrell, C. C. Review of the anatase to rutile phase transformation. J. Mater. Sci. 46, 855–874 (2011).

  4. 4.

    Chen, X. & Mao, S. S. Titanium dioxide nanomaterials: synthesis, properties, modifications, and applications. Chem. Rev. 107, 2891–2959 (2007).

  5. 5.

    Di Paola, A., Bellardita, M. & Palmisano, L. Brookite, the least known TiO2 photocatalyst. Catalysts 3, 36–73, https://doi.org/10.3390/catal3010036 (2013).

  6. 6.

    Balaganapathi, T., KaniAmuthan, B., Vinoth, P. & Thilakan, P. Synthesis, characterization and dye adsorption studies of porous brookite and mixed brookite with rutile TiO2 using PEG assisted sol-gel synthesis process. Mater. Res. Bull. 91, 114–121 (2017).

  7. 7.

    Vequizo, J. J. M. et al. Trapping-induced enhancement of photocatalytic activity on brookite TiO2 powders: comparison with anatase and rutile TiO2 powders. ACS Catalysis 7, 2644–2651 (2017).

  8. 8.

    Lin, H. et al. Synthesis of high-quality brookite TiO2 single-crystalline nanosheets with specific facets exposed: tuning catalysts from inert to highly reactive. J. Am. Chem. Soc. 134, 8328–8331 (2012).

  9. 9.

    Jansen, M. A concept for synthesis planning in solid-state chemistry. Angew. Chem. Int. Ed. 3746-3766 (2002).

  10. 10.

    Ranade, M. R. et al. Energetics of nanocrystalline TiO2. Proc. Nat. Acad. Sci. USA 99, s.2 6476–6481 (2002).

  11. 11.

    Baumgartner, J. et al. Nucleation and growth of magnetite from solution. Nat. Mater. 12, 310–314 (2013).

  12. 12.

    Sun, W., Jayaraman, S., Chen, W., Persson, K. A. & Ceder, G. Nucleation of metastable aragonite CaCO3 in seawater. Proc. Nat. Acad. Sci. USA 112(11), 199–3204 (2015).

  13. 13.

    Kitchaev, D. A. & Ceder, G. Evaluating structure selection in the hydrothermal growth of FeS2 pyrite and marcasite. Nat. Commun. 7, 13799, https://doi.org/10.1038/ncomms13799 (2016).

  14. 14.

    Kitchaev, D. A., Dacek, S. T., Sun, W. & Ceder, G. Thermodynamics of phase selection in MnO2 framework structures through alkali intercalation and hydration. J. Am. Chem. Soc. 139, 2672–2681 (2017).

  15. 15.

    Sun, W., Dacek, S. T., Ong, S. P., Hautier, G., Jain, A., Richards, W. D., Gamst, A. C., Persson, K. A. & Ceder, G. The thermodynamic scale of inorganic crystalline metastability. Sci. Adv. 2(11), p.e1600225 (2016).

  16. 16.

    De Yoreo, J. J. et al. Crystallization by particle attachment in synthetic, biogenic, and geologic environments. Science 349, aaa6760, https://doi.org/10.1126/science.aaa6760 (2015).

  17. 17.

    Keesmann, I. Zur hydrothermalen synthese von brookit. Z. Anorg. Allg. Chem. 346, 30–43 (1966).

  18. 18.

    Cargnello, M., Gordon, T. R. & Murray, C. B. Solution-phase synthesis of titanium dioxide nanoparticles and nanocrystals. Chem. Rev. 114, 9319–9345 (2014).

  19. 19.

    Kim, D.-H., Kim, W.-S., Kim, S. & Hong, S.-H. Brookite TiO2 thin film epitaxially grown on (110) YSZ substrate by atomic layer deposition. Appl. Mater. Interfaces 6, 11817–11822 (2014).

  20. 20.

    Manera, M. G. et al. Enhancement of the optically activated NO2 gas sensing response of brookite TiO2 nanorods/nanoparticles thin films deposited by matrix-assisted pulsed-laser evaporation. Sens. Actuators, B 161, 869–879 (2012).

  21. 21.

    Wang, W. et al. Synthesis and characterization of structural and optical properties of heteroepitaxial brookite TiO2 single crystalline films. Scripta Mater. 115, 75–79 (2016).

  22. 22.

    Srivatsa, K. M. K., Bera, M. & Basu, A. Pure brookite titania crystals with large surface area deposited by plasma enhanced chemical vapour deposition technique. Thin Solid Films 516, 7443–7446 (2008).

  23. 23.

    Bokhimi, X., Morales, A., Aguilar, M., Toledo-Anonio, J. A. & Pedraza, F. Local order in titania polymorphs. Int. J. Hydrogen Energy 26, 1279–1287 (2001).

  24. 24.

    Kuznetsova, I. N., Blaskov, V., Stambolova, I., Znaidi, L. & Kanaev, A. TiO2 pure phase brookite with preferred orientation synthesized as a spin-coated film. Mater. Lett. 59, 3820–3823 (2005).

  25. 25.

    Pottier, A., Chanéac, C., Tronc, E. & Jolivet, J.-P. Synthesis of brookite TiO2 nanoparticles by thermolysis of TiCl4 in strongly acidic aqueous media. J. Mater. Chem. 11, 1116–1121 (2001).

  26. 26.

    Chimupala, Y. et al. Synthesis and characterization of mixed phase anatase TiO2 and sodium-doped TiO2(B) thin films by low pressure chemical vapour deposition (LPCVD). RSC Adv. 4, 48507 (2014).

  27. 27.

    Moret, M. P., Zallen, R., Vijay, D. P. & Desu, S. B. Brookite-rich titania films made by pulsed laser deposition. Thin Solid Films 366, 8–10 (2000).

  28. 28.

    Sharma, A. K., Thareja, R. K., Willer, U. & Schade, W. Phase transformation in room temperature pulsed laser deposited TiO2 thin films. Appl. Surf. Sci. 206, 137–148 (2003).

  29. 29.

    Rudmann, D., Brémaud, D., Zogg, H. & Tiwari, A. N. Na incorporation into Cu(In, Ga)Se2 for high-efficiency flexible solar cells on polymer foils. J. Appl. Phys. 97, 084903 (2005).

  30. 30.

    Rockett, A. et al. Na in selenized Cu(In, Ga)Se2 on Na-containing and Na-free glasses: distribution, grain structure, and device performances. Thin Solid Films 372, 212–217 (2000).

  31. 31.

    Belsky, A., Hellenbrandt, M., Karen, V. L. & Luksch, P. New developments in the Inorganic Crystal StructureDatabase (ICSD): accessibility in support of materials research and design. Acta Cryst. B 58, 364–369 (2002).

  32. 32.

    Nielsen, M. H., Aloni, S. & De Yoreo, J. J. In situ TEM imaging of CaCO3 nucleation reveals coexistence of direct and indirect pathways. Science 345(6201), 1158–1162 (2014).

  33. 33.

    Lafuente, B., Downs, R. T., Yang, H. & Stone, N. The power of databases: the RRUFF project in Highlights in Mineralogical Crystallography, Armbruster, T. and Danisi, R. M., eds Berlin, Germany, W. De Gruyter, 1–30 (2015).

  34. 34.

    Rocquefelte, X., Goublin, F., Koo, H.-J., Whangbo, M.-H. & Jobic, S. Investigation of the origin of the empirical relationship between refractive index and density on the basis of first principles calculations for the refractive indices of various TiO2 phases. Inorg. Chem. 43, 2246–2251 (2004).

  35. 35.

    Rahaman, M. N. Grain growth and microstructure control in Ceramic Processing and Sintering. 540–619, (CRC Press, 2003).

  36. 36.

    Kresse, G. & Furthmuller, J. Efficient iterative schemes for ab initio total-energy calculations using a plane-wave basis set. Phys. Rev. B54, 11169–11186 (1996).

  37. 37.

    Sun, J., Ruzsinszky, A. & Perdew, J. P. Strongly constrained and appropriately normed semilocal density functional. Phys. Rev. Lett. 115, 036402 (2015).

  38. 38.

    Kresse, G. & Joubert, D. From ultrasoft pseudopotentials to the projector augmented-wave method. Phys. Rev. B 59, 1758–1775 (1999).

  39. 39.

    Curnan, M. T. & Kitchin, J. R. Investigating the energetic ordering of stable and metastable TiO2 polymorphs using DFT plus U and hybrid functionals. J. Phys. Chem. C 119, 21060–21071 (2015).

  40. 40.

    Hishikawa, Y. et al. Interference-free determination of the optical absorption coefficient and the optical gap of amorphous silicon thin films. Jpn. J. Appl. Phys. 30, 1008–1014 (1991).

  41. 41.

    Ventura, S. D., Birgin, E. G., Martinez, J. M. & Chambouleyron, I. Optimization techniques for the estimation of the thickness and the optical parameters of thin films using reflectance data. J. Appl. Phys. 97, 043512 (2005).

  42. 42.

    Polyanskiy, M. N. Refractive IndexDatabase. RefractiveIndex.INFO. https://refractiveindex.info (2017).

  43. 43.

    Toby, B. H. & Von Dreele, R. B. GSAS-II: the genesis of a modern open-source all purpose crystallography software package. J. Appl. Cryst. 46, 544–549 (2013).

  44. 44.

    Giannuzzi, L. A. & Stevie, F. A. A review of focused ion beam milling techniques for TEM specimen preparation. Micron 30, 197–204 (1999).

  45. 45.

    Swamy, V. et al. Finite-size and pressure effects on the Raman spectrum of nanocrystalline anatase TiO2. Phys. Rev. B 71, 184302 (2005).

  46. 46.

    Buonsanti, R. et al. Nonhydrolytic synthesis of high-quality anisotropically shaped brookite TiO2 nanocrystals. J. Am. Chem. Soc. 130, 11223–11233 (2008).

  47. 47.

    Zhang, H. & Banfield, J. F. Understanding polymorphic phase transformation behavior during growth of nanocrystalline aggregates: insights from TiO2. J. Phys. Chem. B 104, 3481–3487 (2000).

  48. 48.

    Penn, R. L. & Banfield, J. F. Oriented attachment and growth, twinning, polytypism, and formation of metastable phases: insights from nanocrystalline TiO2. Am. Mineral. 83, 1077–1082 (1998).

Download references


This work was supported as part of the Center for Next Generation Materials by Design: Incorporating Metastability, an Energy Frontier Research Center funded by the U.S. Department of Energy, Office of Science, Basic Energy Sciences under Award #DE-AC36-08GO28308. Use of the Stanford Synchrotron Radiation Lightsource, SLAC National Accelerator Laboratory, was supported by the U.S. Department of Energy, Office of Basic Energy Sciences under Contract No. DE-AC02-76SF00515. DK acknowledges computational resources provided by the Extreme Science and Engineering Discovery Environment (XSEDE), which is supported by National Science Foundation grant number ACI-1548562. We thank Okan Agirseven and Ryan Lance for assistance with measurements, and Vladan Stevanovich for early contributions to the project.

Author information


  1. Department of Physics, Oregon State University, Corvallis, OR, 97331, USA

    • James E. S. Haggerty
    •  & Janet Tate
  2. Applied Energy Programs, SLAC National Accelerator Laboratory, Menlo Park, CA, 94025, USA

    • Laura T. Schelhas
    •  & Michael F. Toney
  3. Department of Materials Science and Engineering, Massachusetts Institute of Technology, Cambridge, MA, 02139, USA

    • Daniil A. Kitchaev
  4. Department of Metallurgical and Materials Engineering, Colorado School of Mines, Golden, CO, 80401, USA

    • John S. Mangum
    •  & Brian P. Gorman
  5. National Renewable Energy Laboratory, Golden, CO, 80401, USA

    • Lauren M. Garten
    • , John D. Perkins
    •  & David S. Ginley
  6. Materials Science Division, Lawrence Berkeley National Laboratory, Berkeley, CA, 94720, USA

    • Wenhao Sun
    •  & Gerbrand Ceder
  7. Department of Materials Science and Engineering, UC Berkeley, Berkeley, CA, 94720, USA

    • Wenhao Sun
    •  & Gerbrand Ceder
  8. Stanford Synchrotron Radiation Lightsource, SLAC National Accelerator Laboratory, Menlo Park, CA, 94025, USA

    • Kevin H. Stone
    •  & Michael F. Toney


  1. Search for James E. S. Haggerty in:

  2. Search for Laura T. Schelhas in:

  3. Search for Daniil A. Kitchaev in:

  4. Search for John S. Mangum in:

  5. Search for Lauren M. Garten in:

  6. Search for Wenhao Sun in:

  7. Search for Kevin H. Stone in:

  8. Search for John D. Perkins in:

  9. Search for Michael F. Toney in:

  10. Search for Gerbrand Ceder in:

  11. Search for David S. Ginley in:

  12. Search for Brian P. Gorman in:

  13. Search for Janet Tate in:


D.G., J.T., L.S., L.G., M.T., and J.P. originated the research. J.H. and L.G. synthesized the films, J.H. and L.S. conducted the experiments, L.S. and K.S. performed X-ray diffraction, JH measured the Raman and optical spectra, J.M. and B.G. did the TEM and EDS characterization. D.K. performed the computational analysis with contributions from W.S. and G.C. The manuscript was primarily written by J.T., J.H., D.K., L.S. and J.M. All authors contributed to discussions of data and manuscript review.

Competing Interests

The authors declare that they have no competing interests.

Corresponding author

Correspondence to Janet Tate.

Electronic supplementary material

About this article

Publication history




Issue Date




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.