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Structure of alumina glass


The fabrication of novel oxide glass is a challenging topic in glass science. Alumina (Al2O3) glass cannot be fabricated by a conventional melt–quenching method, since Al2O3 is not a glass former. We found that amorphous Al2O3 synthesized by the electrochemical anodization of aluminum metal shows a glass transition. The neutron diffraction pattern of the glass exhibits an extremely sharp diffraction peak owing to the significantly dense packing of oxygen atoms. Structural modeling based on X-ray/neutron diffraction and NMR data suggests that the average Al–O coordination number is 4.66 and confirms the formation of OAl3 triclusters associated with the large contribution of edge-sharing Al–O polyhedra. The formation of edge-sharing AlO5 and AlO6 polyhedra is completely outside of the corner-sharing tetrahedra motif in Zachariasen’s conventional glass formation concept. We show that the electrochemical anodization method leads to a new path for fabricating novel single-component oxide glasses.


Oxide glasses, e.g., window glass, fiber glass, optical glass, and the cover glass of a smart phone are indispensable materials in our daily life. However, the fabrication of a novel single-component oxide glass is challenging particularly when a conventional melt–quenching method is used because the glass forming ability is governed by the viscosity of a high-temperature melt. Indeed, Angell proposed the concept of “fragility” to understand the relationship between the viscosity and the glass forming ability1. The basic idea behind the formation of covalent glass is the corner-sharing tetrahedral motif proposed by Zachariasen in 19322. Sun classified single-component oxides into glass formers, glass modifiers, and intermediates3. SiO2, B2O3, P2O5, and As2O3 are typical glass formers, in which the cation–oxygen coordination number is 3 or 4 and the glass network is formed by corner-sharing oxygen atoms. Alkali and alkali earth oxides are typical glass modifiers; they cannot form glass, but they can modify the network formed by a network former by breaking cation–oxygen bonds in the network and/or occupy voids4,5. Alumina (Al2O3) can be considered as an intermediate, because it can be both a glass former and a glass modifier in binary oxide glasses, although Al2O3 cannot solely form glass.

Al2O3 has many applications, e.g., in cements, substrates of electronic materials, and high-temperature crucibles. As mentioned above, it is impossible to prepare Al2O3 glass by the melt–quenching method; hence, sol–gel methods were used to prepare amorphous samples for studying optical properties6,7 and behaviors at high temperatures8. Another approach is the fabrication of thin films, such as the highly ductile amorphous Al2O3 thin films that have recently been reported9. However, the structure of amorphous Al2O3 is still largely unknown owing to a very limited number of structural studies. Lamparter and Kniep reported the formation of AlO4 tetrahedra with corner-sharing oxygen atoms as confirmed by neutron and X-ray diffraction measurements with the aid of the reverse Monte Carlo (RMC)10 modeling technique11. Hashimoto et al. reported the average Al–O coordination number of 4.7 determined by 27Al nuclear magnetic resonance (NMR) spectroscopic measurements12, whereas Lee and Ryu confirmed the formation of OAl3 triclusters by 17O NMR measurements13. Shi et al. have recently reported the comparison between amorphous Al2O3 and liquid Al2O3, and they concluded on the basis of molecular dynamics (MD) and empirical potential structure refinement (EPSR)14 simulations based on diffraction data15 that the Al–O coordination number is increased in amorphous Al2O3.

In this study, we have found that amorphous Al2O3 synthesized by the anodization of aluminium metal shows a glass transition by differential thermal analysis (DTA). We have performed 27Al solid-state NMR and high-energy X-ray and neutron diffraction measurements. Moreover, we constructed a structural model for the glass by a combined MD–RMC modeling technique to understand the structure of single-component intermediate oxide glass, because it is expected that the glass structure is inconsistent with Zachariasen’s rules.


Preparation of alumina glass

The Al2O3 sample was prepared according to our previous report12. High-purity (99.99%) aluminium sheets were immersed in 1.25 mol dm−3 NaOH for 20 s at 60 °C, washed with tap water, immersed in 3.9 mol dm−3 HNO3 for 60 s, and finally washed with deionized water to remove surface native oxides and contaminants. Constant-voltage anodization was performed for 80 V in 0.3 mol dm−3 H2CrO4 electrolyte for 2 h at 40 °C. After anodization, the sample was carefully washed with deionized water to remove residual electrolyte. A stepwise voltage reduction from formation voltage to ~ 60 V was performed in the same electrolyte to reduce barrier layer thickness. To detach the alumina from the aluminium substrates, anodic polarization was applied in a mixed solution of 1:4 vol% of perchloric acid (60%) and ethanol (99.5%) for 1 min at ~ 70 V. The detached sample was carefully washed with deionized water, dried at room temperature, and crushed into powder by an agate mortar. To remove physisorbed water, the powder sample was heat-treated at 300 °C for 4 h at a heating rate of 5 °C min−1 and were subsequently cooled in the furnace, as previously reported.

Density measurement

The density measurement was performed on a helium pycnometer (AccuPyc 1340TC, Shimadzu-Micromeritics). Before the measurement, the sample was dried for 24 h at room temperature in vacuum.

DTA measurement

The differential thermal analysis (DTA) experiment was performed on a Rigaku Thermo plus EVO apparatus. The sample was dried at a heating rate of 10 °C min−1 to 300 °C for 4 h and cooled in the furnace. After reaching 50 °C, the sample was heat-treated at a heating rate of 10 °C min−1 to 1350 °C.

NMR measurements

The 27Al magic angle spinning (MAS) nuclear magnetic resonance (NMR) experiment was performed on a JEOL JNM-ECA800 (18.79 T) spectrometer at a 27Al Larmor frequency of 208.58 MHz. The sample was packed in zirconia rotors and spun at 20 kHz using a 3.2 mm HXMAS probe. The 27Al chemical shift δiso in parts per million (ppm) was referenced to an external 1 mol dm−3 AlCl3 solution (− 0.1 ppm). The 27Al single-pulse MAS spectrum was obtained using 6/π pulses (0.67 us) with a recycle delay of 1 s and 512 scans. The spectrum was decomposed into three components, and fitting parameters, namely, the average isotropic chemical shift (\(\overline{{{\varvec{\updelta}}}_{\mathbf{i}\mathbf{s}\mathbf{o}}}\)), the width of the Gaussian distribution of δiso (ΔCS), and the average quadrupolar coupling constant (\(\overline{{\mathbf{C}}_{\mathbf{Q}}}\)), were determined using the “Dmfit” program16 applying a simple Czjzek model. The errors of fitting values for δiso and other parameters were < 0.04% and < 0.3%, respectively. The average NAl–O was determined using the following equation: \(\overline{{{\varvec{N}}}_{{\varvec{A}}{\varvec{l}}-\mathbf{O}}}=\sum {\varvec{N}}{{\varvec{A}}}_{{\varvec{N}}}\), where N and AN represent the number of oxygen atoms around a given aluminium atom and the relative ratio of the corresponding peak area, respectively.

Diffraction measurements

The high-energy X-ray diffraction experiment was performed at the BL04B2 beamline at the SPring-8 synchrotron radiation facility, using a two-axis diffractometer dedicated to the study of disordered materials17. The energy of the incident X-rays was 61.4 keV. The raw data were corrected for polarization, absorption, and the background, and the contribution of Compton scattering was subtracted by using standard data analysis software17. The neutron diffraction measurement was conducted on a high intensity total diffractometer, NOVA18, installed at BL21 of the Materials and Life Science Experimental Facility at the J-PARC spallation neutron source. The wavelength range of the incident neutron beam was 0.12 Å < λ < 8.3 Å. The glass sample was transferred into vanadium-nickel null alloy cell 6 mm in diameter. The observed scattering intensity for the sample was corrected for instrumental background, attenuation of the sample and cell, and then normalized by the incident beam profile. All corrected data were normalized to give a Faber–Ziman19 total structure factor S(Q). A Lorch20 modification function was used in Fourier transform.

Structure modelling

We combined MD simulation with NVT ensemble–reverse Monte Carlo (RMC) modelling for structure modelling. The MD simulation was performed using the LAMMPS package21 and RMC modellings were performed using the RMC ++code22.

In the case of l-Al2O3, we used the Born–Mayer-type pair potential in the MD simulation given as


Here, e is the elementary charge and Bij and Rij are the parameters accounting for the repulsion of ionic cells. qAl =  + 3 and qO =  − 2 are the charges of Al3+ and O2–, respectively. The Bij values of 2.3708 × 10−16 J (Al–O), 2.4031 × 10−16 J (O–O) and zero (Al–Al) and the Rij values of 0.29 Å (Al–O and O–O) and zero (Al–Al) are found in Ref.23. A random configuration composed of 10,000 atoms was prepared with respect to the experimental density (0.08630 Å−3). This configuration was heated to 5000 K and treated above 50,000 steps. Subsequentry, the configuration was cooled to 2400 K at a cooling rate of 1.3 K/ps. Eventually, the system was equilibrated at 2400 K for 100,000 steps. The long-range Coulomb interactions were calculated with standard Ewald summation and the simulation used periodic boundary conditions. A time step of 1 fs was used in the Verlet algorithm.

For g-Al2O3, the starting configuration, which contain 10,000 particles (Al, 4000: O, 6000) for g-Al2O3 was created using hard-sphere Monte Carlo (HSMC) simulation. The atomic number density is 0.09007 Å−3. The r-spacing for the calculations of the partial pair-distribution functions was set to 0.075 Å. Two kinds of constraints were applied: the closest atom–atom approach and the coordination number. The first one can avoid unreasonable spikes in the partial pair-distribution functions. The second forces aluminium atoms to coordinate to averaged 4.6 oxygen atoms within a cut off distance of 2.50 Å. After the HSMC simulation, RMC simulation was conducted to reproduce the X-ray S(Q) and neutron S(Q) data. Following the RMC simulations, the atomic configuration was optimized by MD simulation. The MD simulation was performed using pairwise additive interatomic terms of the form


where the terms represent Coulomb, van der Waals, and repulsion energy, respectively. Here, rij is the interatomic distance between atoms i and j, D is a standard force constant 4184 JÅ−1 mol−1, qi is the effective charge on atom i (qAl = 1.17, qO = − 0.78). The repulsive radius Ai values are 0.7852 Å (Al), 1.8215 Å (O); the softness parameter Bi values are 0.034 Å (Al), 0.138 Å (O); and the van del Waals coefficient Ci values are 36.82 Å3kj1/2mol−1/2 (Al), 90.61 Å3kj1/2mol−1/2 (O). The parameters Ai, Bi, Ci can be found in Ref.24. The optimization of the atomic configuration was performed by minimizing the energy using the conjugate gradient method. We confirmed that these parameters are in better agreement with diffraction data; in particular, a very sharp principal peak (PP) in SN(Q) for the glass was very well reproduced, while the parameters reported in Ref.23 underestimated the PP.

After the MD simulations, both configurations were refined by additional RMC simulations while constraining the Al–O coordination number, and the partial pair-distribution functions, gij(r), within the first coordination shell to avoid unfavorable artifacts.

As a reference, we constructed three-dimensional structure model of g-SiO2 by combined MD–RMC simulation. The MD simulation of SiO2 glass was performed employing Born–Mayer type pair potentials, where the values qSi and qO are + 2.4 and − 1.2; the Bij values were 21.39 × 10−16 J (Si–O), 0.6246 × 10−16 J (O–O) or zero (Si–Si); the Rij values were 0.174 Å (Si–O), 0.362 Å (O–O) or zero (Si–Si)25. As the initial atomic configuration, 9000 atoms (Si, 3000: O, 6000) were randomly distributed in a cubic cell with respect to the experimental number density (0.06615 Å−3). The simulation temperature was maintained at 4000 K for 20,000 time steps, then the temperature was reduced to 300 K over 200,000 time steps. Finally, the system was equilibrated at 300 K for 50,000 time steps. After the MD simulation, the obtained atomic configuration was refined by additional RMC simulation. In the RMC refinement, the MD results for the Si–O coordination number and the bond angle distribution for O–Si–O, and the partial pair-distribution functions within the first coordination distance were used as constraints. The cut off distance for the constraints for coordination of silicon and O–Si–O bond angle distribution was set to 1.90 Å.

Topological analyses

The bond angle distribution B(θ) was calculated as the number of bonds between θ and θ + Δθ, which is dependent on the solid angle ΔΩ  sinθ subtended at that value of θ. Thus, each bond angle distribution was plotted as B(θ)/sinθ to compensate for the effect of ΔΩ. The primitive26,27 (Al–O)n ring size distributions for the g- and l-Al2O3 were calculated using the R.I.N.G.S. code28,29. The void analysis was conducted employing the pyMolDyn code30 with a cutoff distance of rc = 2.50 Å.

Results and discussion

Figure 1a shows a DTA curve for an Al2O3 sample. Sharp intense and broad weak exothermic peaks at ~ 830 and ~ 1150 °C, respectively, are observed. The former peak is assigned to the crystallization of γ-alumina from the amorphous phase and the latter peak is assigned to the phase transition from γ- to α-alumina31. Note that the slight baseline shift to the endothermic direction is observed in the low temperature region around 500 °C (inset of Fig. 1a), owing to glass transition, showing that the sample is Al2O3 glass (g-Al2O3). The starting point of the shift, i.e., the glass transition temperature, is determined to be ~ 470 °C. In general, common glass‐forming oxides have a ratio of glass transition temperature to melting point (Tg/Tm) of ~ 0.6732. On the other hand, the present g-Al2O3 shows a Tg/Tm of ~ 0.32 (743 K/2345 K), which is extremely lower than that of general glass-forming oxides. The extraordinarily wide gap between Tg and Tm shows the low glass forming ability of alumina to maintain the deeply supercoiling state without the formation of crystal nucleus from the Tm = 2072 °C to Tg =  ~ 470 °C for realizing the glassy state.

Figure 1
figure 1

(a) DTA curve recorded at a heating rate of 10 °C min−1 for g-Al2O3. (b) 27Al solid state NMR spectrum for g-Al2O3.

Figure 1b shows a typical 27Al single-pulse MAS NMR spectrum normalized by the total peak area. This spectrum consists of three broad peaks located at around ~ 64, ~ 36, and ~ 7 ppm, which are assigned to four- (AlO4), five- (AlO5), and six-fold (AlO6) oxygen-coordinated polyhedra, respectively12. This spectrum is decomposed into the three components and the fitting result (dotted curve) is in good agreement with the measured data (solid curve). The fractions of AlO4, AlO5, and AlO6 are 37.5, 52.1, and 10.3%, respectively, and the average coordination number is determined to be 4.73. The values obtained here are slightly different from those of our previous report12; this variation depends on the resolution of the NMR equipment used. More precise values are obtained in the current study owing to the higher-resolution spectra obtained under higher magnetic fields. This precise local structural information is used as a constraint for the MD–RMC modeling as follows.

The mass density of g-Al2O3 is 3.05 g cm−3, which corresponds to the atomic number density of 0.0901 Å−3. This value is smaller than 4.00 g cm-3 of α-Al2O3 and slightly larger than 2.92 g cm−3 of l-Al2O333. Note that the density of γ-Al2O3 is 3.59 g cm−3, which is between those of g-Al2O3 and α-Al2O3. This trend is very different from SiO2, in which the density of glass (2.20 g cm−3) is comparable to those of α-cristobalite (2.30 g cm−3) and β-cristobalite (2.20 g cm−3), implying that a large density difference between the glass and crystal in Al2O3 indicates a low glass forming ability in single-component oxide glasses.

Figure 2 shows neutron and X-ray total structure factors, SN,X(Q), for g-Al2O3 together with the results of MD–RMC simulation. For comparison, the results of silica glass (g-SiO2)5 and liquid alumina (l-Al2O3) at 2400 K33 are also shown. All the experimental SN,X(Q) data are well reproduced by the MD–RMC simulations. The first sharp diffraction peak (FSDP)34, which is from pseudo35 (quasi36) Bragg planes (successive small cages37) created along a void, is observed at Q = 1.52 Å−1 for g-SiO2, a typical glass forming oxide, whereas the FSDP observed at Q ~ 2 Å−1 is not prominent in g-Al2O3, suggesting the formation of a densely packed structure with a small void volume. In addition, g-Al2O3 shows an extraordinarily sharp PP38 in the neutron S(Q), but no PP is observed in the X-ray S(Q) owing to the small weighting factor of O–O correlations for X-rays, because PP reflects the packing of oxygen atoms39. Therefore, the extraordinarily sharp PP in the neutron S(Q), nearly twice sharper than those of l-Al2O3 and g-SiO2, suggests the extremely high packing fraction of oxygen atoms manifested by the high density of g-Al2O3. A similar behavior is found in the neutron diffraction data of g-SiO2 under a high pressure40. Both the overall profiles of SN,X(Q) for l-Al2O3 are broader than those for g-Al2O3, but the SX(Q) data of both l-Al2O3 and g-Al2O3 are more identical, suggesting that O–O correlations are different between g-Al2O3 and l-Al2O3.

Figure 2
figure 2

(a) Neutron total structure factors, SN(Q), together with the results of the MD–RMC simulations for g-Al2O3, l-Al2O333, and g-SiO25. (b) X-ray total structure factors, SX(Q), together with the results of the MD–RMC simulations for g-Al2O3, l-Al2O333, and g-SiO25. Coloured curve, experimental data; black broken curve, MD-RMC model. Successive curves are displaced upward by 2 for clarity.

The neutron and X-ray total correlation functions, TN,X(r), for g-Al2O3, l-Al2O333, and g-SiO25 are shown in Fig. 3. The first peak observed at 1.81 Å in TN,X(r) for g-Al2O3 is assigned to the Al–O correlations. The second peak observed around 2.8 Å in TN(r) and that around 3.2 Å in TX(r) are assigned to the O–O and Al–Al correlations, respectively. Longer Al–O distances relative to g-SiO2 and the asymmetric Al–O correlation peak with a tail of ~ 2.4 Å indicate the formation of distorted AlOn polyhedra with a coordination number higher than 4. The average Al–O coordination number calculated using the area of the first correlation peak of TN(r) is 4.6 ± 0.2, which is in agreement with the NMR result of 4.73 (37.5% of AlO4; 52.1% of AlO5; and 10.3% of AlO6) and larger than 4.4 in l-Al2O3. Such a larger coordination number, which is often observed in nonglass-forming high-temperature oxide melts37,41, cannot be observed in the typical glass-forming oxides. The overall profile for g-Al2O3 is similar to that for l-Al2O3, but the Al–O and O–O correlation peaks for g-Al2O3 are sharper than those for l-Al2O3, as apparently observed in TN(r). This behavior suggests that the packing of oxygen atoms in glass could differ from that in high-temperature liquid.

Figure 3
figure 3

(a) Neutron total correlation functions, TN(r), for g-Al2O3, l-Al2O333, and g-SiO25. (b) X-ray total correlation functions, TX(r), or g-Al2O3, l-Al2O333, and g-SiO25. Upper and lower panel data were obtained by Fourier transform with Qmax = 25 and 18 Å−1, respectively. Note that the Al–Al correlation peak is not legibly marked owing to its small weighting factor for neutrons.

Figure 4a shows the partial structure factors, Sij(Q), derived from the MD–RMC models for g-Al2O3 and l-Al2O3 together with those for g-SiO2. All the Sij(Q) give a positive peak at the FSDP position in g-SiO2, but there is no positive peak at the expected FSDP position in g-Al2O3. It is confirmed that the PP comprises the sum of positive correlations of A–A and X–X and negative correlations of A–X. As can be seen in Fig. 2b the PP is absent because the positive correlations of A–A and X–X are completely canceled by the A–X correlations in the SX(Q) of g-SiO2 and g- and l-Al2O3. On the other hand, the contribution of the X–X correlations at PP position is largely enhanced in the SN(Q) (see Fig. 2a) due to large weighting factors of O–O correlations for neutrons. The positive O–O PP for g-Al2O3 is sharper than that for l-Al2O3, resulting in the exceptionally sharp PP observed in the SN(Q) for g-Al2O3. Both the absence of the FSDP as mentioned above and the sharp PP in the SN(Q) mainly originated from the O–O correlations allow us to expect the formation of the dense oxygen packing in g-Al2O3. The partial pair distribution functions, gij(r), derived from the MD–RMC models for g-Al2O3 and l-Al2O3 together with those for g-SiO2 are shown in Fig. 4b. g-SiO2 shows very prominent sharp Si–Si, Si–O, and O–O correlation peaks, whereas Al–Al, Al–O, and O–O correlation peaks are broader for g-Al2O3. Note that both the Al–O and O–O correlation peaks for l-Al2O3 are broader than those for g-Al2O3, whereas the Al–Al correlation peak in the former is identical to the latter. This trend is consistent with the finding that the difference in SX(Q) between l-Al2O3 and g-Al2O3 is very small.

Figure 4
figure 4

(a) Partial structure factors, Sij(Q), for g-Al2O3, l-Al2O3, and g-SiO2. (b) Partial pair distribution functions, gij(r), for g-Al2O3, l-Al2O3, and g-SiO2. A = Si or Al and X = O.

Table 1 shows coordination number distributions and polyhedral connections in g-Al2O3, l-Al2O3, and g-SiO2. For a typical glass-forming oxide, g-SiO2, the number of oxygen atoms around a Si atom (NA–X) is 4, the number of Si atoms around an oxygen atom (NX–A) is 2, and the SiO4 polyhedra are connected via 100% corner-sharing, which is definitely in accordance with Zachariasen’s conventional glass formation concept. On the other hand, for g-Al2O3, more than 50% of the cations have NA–X ≥ 5 and most of the oxygen atoms are connected with three Al atoms, showing the formation of OAl3 triclusters and a significant number of OAl4 tetraclusters. In addition, a significant fraction of edge-sharing AlOn polyhedral units are observed in g-Al2O3. These features are completely inconsistent with Zachariasen’s rules. The fractions of AlO5 and AlO6 units, OAl3 triclusters and OAl4 tetraclusters, and edge-sharing AlOn polyhedra are all characteristic features of a non-glass-forming behavior.

Table 1 Coordination number distributions and polyhedral connections in g-Al2O3, l-Al2O3, and g-SiO2.

To obtain the characteristic real space atomic arrangement of intermediate oxide glass, we analyzed the bond angle distribution. Figure 5a shows the bond angle distributions of g-Al2O3 and l-Al2O3 together with those of g-SiO2. The O–Si–O distribution has a well-defined peak at 109° attributable to the formation of regular SiO4 tetrahedra. The Si–Si–Si distribution has a broad peak at around 109°, suggesting the formation of SiSi4 hyper-tetrahedra42. The Si–O–Si distribution shows a peak at 165° attributable to the formation of the corner-sharing network. On the other hand, the bond angle distributions of g- and l-Al2O3 show completely different behaviors. The O–Al–O distributions of g-Al2O3 and l-Al2O3 shows peak at ~ 95 and ~ 180°, suggesting that AlOn polyhedra are octahedral and are rather similar to those in non-glass-forming liquids, O–Zr–O in l-ZrO237 and O–Er–O in l-Er2O341. The Al–O–Al distributions has two peaks at 97 (edge-sharing) and 120° (OAl3 tricluster) of g-Al2O3, which become a broad single peak in l-Al2O3 owing to highly densely packed structure. Both the O–Al–O and Al–O–Al distributions of g-Al2O3 are slightly different from the results recently reported by Shi et al., because they do not have neutron diffraction data15. The most striking difference between g-SiO2 and g-/l-Al2O3 is the A–A–A distribution. The Si–Si–Si distribution suggests the formation of SiSi4 hyper-tetrahedra probably associated with the prominent FSDP, but the Al–Al–Al distribution shows two peaks at ~ 60° and ~ 115°, suggesting that the distribution of Al atoms is due to a typical dense random packing43, which cannot give rise to an FSDP in the diffraction data. The O–O–O distributions of g-Al2O3 and l-Al2O3 are also very different from that of g-SiO2 and suggest that the distributions of oxygen atoms are dense also due to the random packing. Moreover, it is suggested that the oxygen packing fraction of g-Al2O3 increases owing to the higher mass density in the glass in comparison with the liquid (see Table 1). Indeed, the distribution peak of g-Al2O3 is sharper than that of l-Al2O3. Both the O–O–Al and O–A–Al distributions of g-Al2O3 and l-Al2O3 are also different from the O–O–Si and O–S–Si distributions in g-SiO2.

Figure 5
figure 5

(a) Bond angle distributions for g-Al2O3, l-Al2O3, and g-SiO2. (b) Primitive ring size distributions for g-Al2O3, l-Al2O3, and g-SiO2. A = Si or Al and X = O.

To understand the topology of g-Al2O3 and l-Al2O3, we calculated the primitive ring size distribution and compared it with the g-SiO2 data in Fig. 5b. g-SiO2 shows a broad ring size distribution from threefold to ninefold rings, which is topologically disordered according to Gupta and Cooper44. Both g-Al2O3 and l-Al2O3 show broad ring size distributions that are nearly identical, but they have large fractions of small rings, e.g., twofold rings (edge-sharing) and threefold rings, which is a signature of the low glass forming ability of Al2O3.

We show the atomic configuration of the glass obtained from the MD–RMC model in Fig. 6a to understand the structure of g-Al2O3. It is easily recognized that the assembly of two-membered rings (edge-sharing polyhedra) forms a lattice-like structure (black dotted line). The O–O atomic distance, which is the diagonal of one square, is ~ 2.3–2.7 Å, which is nearly consistent with the periodicity of ~ 2.3 Å estimated from the peak position of the PP observed in the SN(Q) for g-Al2O3. Therefore, we conclude that, in addition to the large fraction of corner-sharing OAl3 triclusters associated with the formation of octahedral AlOn polyhedra, the larger fraction of edge-sharing AlOn polyhedra for g-Al2O3 (19.3%) than for l-Al2O3 (17.6%) must be the origin of the exceptionally sharp PP observed in the SN(Q) for g-Al2O3. We show the OAl3 triclusters (red) and OAl4 tetraclusters (yellow) in Fig. 6b. Such a cluster network can be found in g-SiO2 at a high pressure of 200 GPa45, but it is possible to fabricate such a glass structure at ambient pressure through the electrochemical anodization process under high electric field46,47. The voids (highlighted in green) of g-Al2O3 are shown in Fig. 6c. The void volume ratio of g-SiO2 according to our previous study is 32%5, whereas those in g-Al2O3 and l-Al2O3 is only 4.5% and 5.5%, respectively, indicating that a highly densely packed structure is formed in them. The dense-random-packing-like bond angle distribution (see Fig. 5a) with significantly octahedral AlOn polyhedra is very different from that of conventional oxide glass but rather similar to that of metallic glass in which icosahedra is highly distorted owing to geometric frustration48.

Figure 6
figure 6

(a) Atomic configuration of g-Al2O3 (stick bonds schematic). (b) Atomic configuration of g-Al2O3 (schematic of the OAl3 triclusters (red) and OAl4 tetraclusters (yellow)). (c) Atomic configuration of g-Al2O3 with voids. Pink and red circles represent Al and O atoms, respectively, and green regions show the voids.

The electrochemically prepared g-Al2O3 has many features that are completely outside of Zachariasen’s rules. Regardless of the dense oxygen packing structure with a large fraction of edge-sharing polyhedral motifs, g-Al2O3 can stably exist as glass. The electrochemical anodization technique can be regarded as a powerful tool for our questing for novel intermediate oxide glasses with an extremely dense structure, and the comprehensive understanding of the atomic structure of the glasses will give new insights into the fabrication of novel glass materials.


  1. Angell, C. A. Formation of glasses from liquids and biopolymers. Science 267, 1924–1935 (1995).

    ADS  CAS  PubMed  Article  Google Scholar 

  2. Zachariasen, W. H. The atomic arrangement in glass. J. Am. Chem. Soc. 54, 3841–3851 (1932).

    CAS  Google Scholar 

  3. Sun, K.-H. Fundamental condition of glass formation. J. Am. Ceram. Soc. 30, 277–281 (1947).

    CAS  Article  Google Scholar 

  4. Greaves, G. N. EXAFS and the structure of glass. J. Non-Cryst. Solids 71, 203–217 (1985).

    ADS  CAS  Article  Google Scholar 

  5. Onodera, Y. et al. Origin of the mixed alkali effect in silicate glass. NPG Asia Mater. 11, 75 (2019).

    ADS  CAS  Article  Google Scholar 

  6. Hu, B., Yao, M., Xiao, R., Chen, J. & Yao, X. Optical properties of amorphous Al2O3 thin films prepared by a sol–gel process. Ceram. Int. 40, 14133–14139 (2014).

    CAS  Article  Google Scholar 

  7. Nasu, H., Hirota, D., Inoue, K., Hashimoto, T. & Ishihara, A. Luminescent properties of amorphous Al2O3 prepared by sol–gel method. J. Ceram. Soc. Jpn. 116, 835–836 (2008).

    CAS  Article  Google Scholar 

  8. Mavrič, A., Fanetti, M., Mali, G. & Valant, M. High-temperature stabilization of bulk amorphous Al2O3. J. Non-Cryst. Solids 499, 363–370 (2018).

    ADS  Article  CAS  Google Scholar 

  9. Frankber, E. J. et al. Highly ductile amorphous oxide at room temperature and high strain rate. Science 366, 864–869 (2019).

    ADS  Article  CAS  Google Scholar 

  10. McGreevy, R. L. & Pusztai, L. Reverse Monte Carlo simulation: A new technique for the determination of disordered structures. Mol. Simul. 1, 359–367 (1988).

    Article  Google Scholar 

  11. Lamparter, P. & Kniep, R. Structure of amorphous Al2O3. Physica B 234–236, 405–406 (1997).

    ADS  Article  Google Scholar 

  12. Hashimoto, H., Yazawa, K., Asoh, H. & Ono, S. NMR spectroscopic analysis of the local structure of porous-type amorphous alumina prepared by anodization. J. Phys. Chem. C 121, 12300–12307 (2017).

    CAS  Article  Google Scholar 

  13. Lee, S. K. & Ryu, S. Probing of triply coordinated oxygen in amorphous Al2O3. J. Phys. Chem. Lett. 9, 150–156 (2018).

    CAS  PubMed  Article  Google Scholar 

  14. Soper, A. Empirical potential Monte Carlo simulation of fluid structure. Chem. Phys. 202, 295–306 (1996).

    CAS  Article  Google Scholar 

  15. Shi, C. et al. The structure of amorphous and deeply supercooled liquid alumina. Front. Mater. 6, 38 (2019).

    ADS  Article  Google Scholar 

  16. Massiot, D. et al. Modelling one- and two-dimensional solid-state NMR spectra. Magn. Reson. Chem. 40, 70–76 (2002).

    CAS  Article  Google Scholar 

  17. Ohara, K., Onodera, Y., Murakami, M. & Kohara, S. Structure of disordered materials under ambient to extreme conditions revealed by synchrotron x-ray diffraction techniques at SPring-8: Recent instrumentation and synergic collaboration with modelling and topological analyses. J. Phys. Condens. Matter 33, 383001 (2021).

    ADS  CAS  Article  Google Scholar 

  18. Otomo, T. et al. Fundamental research of hydrogen storage mechanism with high-intensity total diffractometer. KENS Rep. 17, 28–36 (2011).

    Google Scholar 

  19. Faber, T. E. & Ziman, J. M. A theory of the electrical properties of liquid metals. Philos. Mag. 11, 153–173 (1965).

    ADS  CAS  Article  Google Scholar 

  20. Lorch, E. Neutron diffraction by germania, silica and radiation-damaged silica glasses. J. Phys. C Solid State Phys. 2, 229–237 (1969).

    ADS  Article  Google Scholar 

  21. Plimpton, S. Fast parallel algorithms for short-range molecular dynamics. J. Comput. Phys. 117, 1–19 (1995).

    ADS  CAS  MATH  Article  Google Scholar 

  22. Gereben, O., Jóvári, P., Temleitner, L. & Pusztai, L. A new version of the RMC++ Reverse Monte Carlo programme, aimed at investigating the structure of covalent glasses. J. Optoelectron. Adv. Mater. 9, 3021–3027 (2007).

    CAS  Google Scholar 

  23. Hoang, V. V. Molecular dynamics study on structure and properties of liquid and amorphous Al2O3. Phys. Rev. B 70, 134204 (2004).

    ADS  Article  CAS  Google Scholar 

  24. Matsui, M. A transferable interatomic potential model for crystals and melts in the system CaO-MgO-Al2O3-SiO2. Miner. Mag. 58A, 571 (1994).

    Article  Google Scholar 

  25. Onodera, Y. et al. Structure and properties of densified silica glass: Characterizing the order within disorder. NPG Asia Mater. 12, 85 (2020).

    ADS  CAS  Article  Google Scholar 

  26. Goetzke, K. & Klein, H. J. Properties and efficient algorithmic determination of different classes of rings in finite and infinite polyhedral networks. J. Non-Cryst. Solids 127, 215–220 (1991).

    ADS  CAS  Article  Google Scholar 

  27. Yuan, X. & Cormack, A. N. A computational multiscale strategy to the study of amorphous materials. Comput. Mater. 24, 343–360 (2002).

    CAS  Article  Google Scholar 

  28. Roux, S. L. & Jund, P. Ring statistics analysis of topological networks: New approach and application to amorphous GeS2 and SiO2 systems. Comput. Mater. Sci. 49, 70–83 (2010).

    Article  Google Scholar 

  29. Roux, S. L. & Jund, P. Erratum: Ring statistics analysis of topological networks: New approach and application to amorphous GeS2 and SiO2 systems [Comput. Mater. Sci. 49 (2010) 70–83]. Comput. Mater. Sci. 50, 1217 (2011).

    Article  Google Scholar 

  30. Heimbach, I. et al. pyMolDyn: Identification, structure, and properties of cavities/vacancies in condensed matter and molecules. J. Comput. Chem. 38, 389–394 (2017).

    CAS  PubMed  Article  Google Scholar 

  31. Abe, T., Uchiyama, T. & Otuska, T. Heat-decomposition process of the anions incorporated into anodic oxide films of aluminum. Kinzoku Hyomen Gijutsu 27, 15–19 (1976).

    CAS  Google Scholar 

  32. Sakka, S. & Mackenzie, J. D. Relation between apparent glass transition temperature and liquids temperature for inorganic glasses. J. Non-Cryst. Solids 6, 145–162 (1971).

    ADS  CAS  Article  Google Scholar 

  33. Skinner, L. B. et al. Joint diffraction and modeling approach to the structure of liquid alumina. Phys. Rev. B 87, 024201 (2013).

    ADS  Article  CAS  Google Scholar 

  34. Price, D. L. et al. Intermediate-range order in glasses and liquids. J. Phys. C Solid State Phys. 21, L1069–L1072 (1988).

    ADS  Article  Google Scholar 

  35. Uchino, T., Harrop, J. D., Taraskin, S. N. & Elliott, S. R. Real and reciprocal space structural correlations contributing to the first sharp diffraction peak in silica glass. Phys. Rev. B 71, 014202 (2005).

    ADS  Article  CAS  Google Scholar 

  36. Gaskell, P. H. & Wallis, D. J. Medium-range order in silica, the canonical network glass. Phys. Rev. Lett. 76, 66–69 (1996).

    ADS  CAS  PubMed  Article  Google Scholar 

  37. Kohara, S. et al. Atomic and electronic structures of an extremely fragile liquid. Nat. Commun. 5, 5892 (2014).

    ADS  CAS  PubMed  Article  Google Scholar 

  38. Salmon, P. S., Martin, R. A., Mason, P. E. & Cuello, G. J. Topological versus chemical ordering in network glasses at intermediate and extended length scales. Nature 435, 75–78 (2005).

    ADS  CAS  PubMed  Article  Google Scholar 

  39. Salmon, P. S. & Zeidler, A. Ordering on different length scales in liquid and amorphous materials. J. Stat. Mech. Theory E 2019, 114006 (2019).

    MathSciNet  MATH  Article  CAS  Google Scholar 

  40. Zeidler, A. et al. High-pressure transformation of SiO2 glass from a tetrahedral to an octahedral network: A joint approach using neutron diffraction and molecular dynamics. Phys. Rev. Lett. 113, 135501 (2014).

    ADS  PubMed  Article  CAS  Google Scholar 

  41. Koyama, C. et al. Very sharp diffraction peak in nonglass-forming liquid with the formation of distorted tetraclusters. NPG Asia Mater. 12, 43 (2020).

    CAS  Article  Google Scholar 

  42. Shi, R. & Tanaka, H. Distinct signature of local tetrahedral ordering in the scattering function of covalent liquids and glasses. Sci. Adv. 5, 3194 (2019).

    ADS  Article  CAS  Google Scholar 

  43. Howe, M. A., McGreevy, R. L., Pusztai, L. & Borzsák, I. Determination of three body correlations in simple liquids by RMC modelling of diffraction data II. Elemental liquid. Phys. Chem. Liq. 25, 205–241 (1993).

    CAS  Article  Google Scholar 

  44. Gupta, P. K. & Cooper, A. R. Topologically disordered networks of rigid polytopes. J. Non-Cryst. Solids 123, 14–21 (1990).

    ADS  CAS  Article  Google Scholar 

  45. Murakami, M. et al. Ultrahigh-pressure form of SiO2 glass with dense pyrite-type crystalline homology. Phys. Rev. B 99, 045153 (2019).

    ADS  CAS  Article  Google Scholar 

  46. Hoar, T. P. & Mott, N. F. A mechanism for the formation of porous anodic oxide films on aluminium. J. Phys. Chem. Solids 9, 97–99 (1959).

    ADS  CAS  Article  Google Scholar 

  47. O’Sullivan, J. P., Wood, G. C. & Mott, N. F. The morphology and mechanism of formation of porous anodic films on aluminium. Proc. R. Soc. Lond. A 317, 511–543 (1970).

    ADS  CAS  Article  Google Scholar 

  48. Hirata, A. et al. Geometric frustration of icosahedron in metallic glass. Science 341, 376–379 (2013).

    ADS  CAS  PubMed  Article  Google Scholar 

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Part of this study was financially supported by the Light Metal Education Foundation of Japan and the JSPS Grant-in-Aid for Transformative Research Areas (A) "Hyper-Ordered Structures Science" (Grant Numbers 20H05881 and 20H05878) and JSPS KAKENHI (Grant Number 19K05648). We thank Prof. Hidetaka Asoh and Mr. Yuki Fujita for supporting the sample preparation and for helpful discussion. NMR experiments were supported by NIMS microstructural characterization platform as a program of "Nanotechnology Platform" of the Ministry of Education, Culture, Sports, Science and Technology (MEXT), Japan. The synchrotron radiation experiments were performed at BL04B2 of SPring-8 with the approval of the Japan Synchrotron Radiation Research Institute (JASRI) (Proposal No. 2016B0134). The neutron diffraction experiment at the Materials and Life Science Experimental Facility of the Japan Proton Accelerator Research Complex (J-PARC) was performed as the S-type project of High Energy Accelerator Research Organization (KEK) (Proposal No. 2014S06).

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Authors and Affiliations



S.K. and H.H. formulated the research project. H.H. prepared the materials. H.H. and K.Y. performed NMR measurements. H.H. and H.S. performed thermal analysis. Y.O. preformed neutron diffraction measurements and analyzed the measured data. S.K. and K.O. performed high-energy X-ray diffraction measurements and analyzed the measured data. Y.O. S.T., and S.K. performed MD–RMC modelling. Y.O., S.K., and M.M. analyzed the structural model. H.H., Y.O., and S.K. wrote the paper with the input of all the authors.

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Correspondence to Hideki Hashimoto or Shinji Kohara.

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Hashimoto, H., Onodera, Y., Tahara, S. et al. Structure of alumina glass. Sci Rep 12, 516 (2022).

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