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Stable magnesium peroxide at high pressure

  • Scientific Reports volume 5, Article number: 13582 (2015)
  • doi:10.1038/srep13582
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Rocky planets are thought to comprise compounds of Mg and O as these are among the most abundant elements, but knowledge of their stable phases may be incomplete. MgO is known to be remarkably stable to very high pressure and chemically inert under reduced condition of the Earth’s lower mantle. However, in exoplanets oxygen may be a more abundant constituent. Here, using synchrotron x-ray diffraction in laser-heated diamond anvil cells, we show that MgO and oxygen react at pressures above 96 GPa and T = 2150 K with the formation of I4/mcm MgO2. Raman spectroscopy detects the presence of a peroxide ion (O22−) in the synthesized material as well as in the recovered specimen. Likewise, energy-dispersive x-ray spectroscopy confirms that the recovered sample has higher oxygen content than pure MgO. Our finding suggests that MgO2 may be present together or instead of MgO in rocky mantles and rocky planetary cores under highly oxidized conditions.


Oxygen and magnesium are the first and second most abundant elements in the Earth’s mantle1; thus knowledge of stable phase relations in the Mg-O system as a function of thermodynamic parameters is necessary input information for reconstructing Earth-like planetary interiors. For example, ferropericlase (MgO with a relatively low Fe content) is the second most abundant mineral on Earth owing to its remarkable thermodynamic stability in the Fm3m crystal structure (up to 500 GPa and at least 5000 K for pure MgO)2,3. This is why ferropericlase has been assumed in gas giant cores4,5 as well as in extrasolar terrestrial mantles6,7. However, planet-harboring stars vary in chemical composition8, which likely affects the composition of planetary building blocks and exoplanet mineralogy9. Therefore, Earth-like mantle mineralogy should not be assumed for terrestrial exoplanets. Elevated oxygen contents have been observed in planet-host stars10, which may affect the stability of MgO and favor other solid phases in the Mg-O system11,12. For example, magnesium peroxide (MgO2) have been synthesized at near-ambient conditions and at high oxygen fugacities in the pyrite-type (Pa3) structure11. However, Pa3 MgO2 is thermodynamically unstable and readily decomposes to MgO and O2 upon heating to 650 K at ambient pressure11. The intrinsic instability of MgO2 is attributed to the strong polarizing effect of the Mg2+ ion possessing high charge density in a relatively small ionic radius13. This is why the stability of Group II peroxides increases down the Group: beryllium peroxides are not known13, while Ca, Sr and Ba form increasingly more stable peroxides at ambient conditions14,15. Therefore, using empirical considerations on chemical pressure16,17 MgO2 may be expected to become stable under high pressure conditions. Indeed, ab initio simulations found that I4/mcm MgO2 becomes stable at P > 116 GPa (Ref. 12) and 0 K. Here, we report on the synthesis of I4/mcm MgO2 in a laser-heated diamond anvil cell (DAC). MgO2 may be an abundant mineral in highly oxidized terrestrial exoplanets. Our finding also suggests that the Mg-Fe-Si-O system likely has more unexpected chemistry at high pressure.


Two types of chemical precursors were loaded in DACs to study the MgO-O2 phase diagram in the 0–160 GPa pressure range (see Table 1 and Methods). In type-A experiments we put two 4 μm thick MgO disks in the sample cavity which was subsequently filled with liquefied oxygen (Fig. 1, inset). In type-B runs we used commercially available magnesium peroxide complex (24–28% Pa3 MgO2, 42–46% MgO, ~30% Mg) mixed with submicron Au powder serving as a laser absorber. The mixture was loaded without pressure medium.

Table 1: Experiments description.
Figure 1: X-ray diffraction (XRD) pattern of the A1 sample before laser heating (black line), at high temperature (red line) and quenched to 300 K (blue line).
Figure 1

Arrows mark new peaks that appear at high temperature. A thermal shift of the MgO peaks is seen at T = 2150 K indicating a uniform heating of the sample. Miller indices correspond to the indexed tetragonal unit cell. Expected positions of I4/mcm MgO2 Bragg reflections12 are shown by red ticks. Blue bars correspond to MgO. Oxygen peaks are not resolved. The wavelength is 0.3344 Å. The inset shows the experimental assemblage of type-A runs.

X-ray diffraction

Figure 1 shows representative XRD patterns of the run A1 at 96 GPa before heating, at 2150 K, and after quenching. Oxygen peaks were weak and not resolved in the integrated pattern before laser-heating. Six new peaks appear upon heating and become clearly seen in the XRD pattern of the quenched sample. Indexing the new peaks reveals a tetragonal unit cell with a = 4.000(1) Å, c = 4.743(5) Å. The new peaks show a good match with the expected positions of the predicted I4/mcm MgO2 Bragg reflections12 (shown as red ticks in Fig. 1). Rietveld refinement of the new phase was not possible due to its spotty diffraction texture and because low intensity peaks could not be resolved (Supplementary Fig. S1).

In the experiments with type-B precursors MgO, ε-O2, and Au were the only phases observed in XRD patterns after it was heated to T > 2000 K in the pressure range of 5–70 GPa. Bragg peaks that can be assigned to Pa3 MgO2 were completely absent in the reaction products suggesting that the precursor had decomposed to MgO and O2. Indeed, the presence of pure oxygen in the quenched sample was confirmed with Raman spectroscopy. Noteworthy, we did not observe elemental Mg (neither hcp at P < 50 GPa nor bcc at P > 50 GPa) in the reaction products. Magnesium likely reacts with oxygen as the latter gets liberated upon Pa3 MgO2 decomposition at high temperature.

Laser heating of the B2 sample to T > 2000 K at P = 134 GPa provided more information on the high pressure chemistry of the Mg-O system. We were very curious to note that new peaks form a powder-type texture in XRD images (Fig. 2), indicating the presence of a large number of randomly oriented crystallites. Surprisingly, the spotty texture is now built by MgO and ζ-O2. Indexing the most clearly resolved new peaks again yields a tetragonal unit cell with a = 3.925 (1) Å, c = 4.613 (6) Å. Moreover, the obtained Miller indices reproduce that of the tetragonal phase synthesized in the A1 run (Fig. 1) suggesting that the exact same phase has been produced in the A1 and B2 runs. Given the large yields of the new phase as well as the polycrystalline sample texture, Rietveld method can be applied to test and refine the theoretically predicted I4/mcm MgO2. According to the prediction by Zhu et al. (Ref. 12), magnesium occupies a 4a Wyckoff position (0, 0, 0.25) and oxygen is located in 8 h (x, x + 0.5, 0), which leaves only the x fractional coordinate of oxygen to refine. The refined x = 0.1285(13), and the predicted x = 0.126 agrees to within 2σ; thus the refined structural model may be considered identical to the predicted one. Figure 3 compares the experimental XRD pattern with the synthetic XRD of the Rietveld-refined I4/mcm MgO2.

Figure 2: XRD image of I4/mcm MgO2 powder synthesized at 134 GPa (seen as dark grey vertical lines) in rectangular coordinates (cake).
Figure 2

Red and violet ticks correspond to the positions of I4/mcm MgO2 and MgO, respectively. Green ticks represent some reflections of ζ-O2 (high angle Bragg reflections are not shown). White labels are Miller indices of the indexed tetragonal phase. Part of this XRD pattern (2θ = 9–13.5) was used to Rietveld refine the predicted structure of I4/mcm MgO2. The x-ray wavelength is 0.3344 Å.

Figure 3: XRD of the type-B precursor laser-heated to T > 2000 K at 134 GPa.
Figure 3

Red bars represent positions and intensities of Bragg reflections of the Rietveld refined I4/mcm MgO2. Dark blues bars correspond to MgO. The peak marked with an asterisk belongs to oxygen. Inset: Rietveld refinement of the MgO2 crystal structure. Grey bars approximate positions of the strongest ζ-O2 peaks. Green curve represents the calculated intensities of the refined structure (Icalc). Black line is the intensity difference curve (Iobs − Icalc). Calculated residuals after background subtraction are Rexp = 0.138, Rwp = 0.265. The x-ray wavelength is 0.3344 Å.

Raman spectroscopy was applied to characterize I4/mcm MgO2, albeit the increased fluorescent background of diamond anvils typical at pressures exceeding 100 GPa. On top of this, oxygen becomes metallic at pressure above 96 GPa18 and may screen reaction products from the probe laser radiation. First, we used density-functional perturbation theory (DFT) to compute spectral position and intensities of I4/mcm MgO2 Raman bands in the 90–150 GPa pressure range. Group theory for the I4/mcm MgO2 allows 5 Raman active vibrations (2Eg + B1g + A1g + B2g). Our DFT calculations suggest that B2g and A1g modes should have observable intensities with A1g being the most intense as it may also be anticipated from earlier Raman studies of solid peroxides19. Figure 4A shows Raman spectra of A2 at 104 GPa collected from an area containing I4/mcm MgO2 as established by XRD. The O2 vibron was also observed in Raman spectra collected from the laser-heated spot. Since both ε- and ζ-O2 have a rich Raman spectrum20 at frequencies lower than 900 cm−1 it is difficult to use this spectral region for a reliable identification of the I4/mcm MgO2. Luckily, the position of A1g band is predicted in the 1060–1175 cm−1 spectral range at 90–150 GPa according to our DFT calculations. Based on this comparison, the high-frequency mode at 1037 cm−1 may be assigned to the O-O stretching vibration in the peroxide ion. Raman shift of the high-frequency band is in agreement with the positions of A1g band in H2O2 (Ref. 21) and BaO2 (Ref. 22) confirming the assignment.

Figure 4
Figure 4

(A) Raman spectra of MgO + O2 reaction products collected with 488, 532, and 660 nm excitations. Oxygen Raman spectra collected outside of the laser-heated region is shown for comparison. Dark blue vertical ticks correspond to the computed Raman modes of I4/mcm at 100 GPa (A1g and B2g modes may have observable intensities, according to our DFT computations). The 1037 cm−1 peak that can be assigned to the A1g mode in I4/mcm MgO2 is marked by an arrow. (B) Pressure dependencies of O-O symmetric stretching vibration (A1g). Red circles represent positions of the high-frequency mode observed in the A2 sample. Green circles correspond to the positions of the A1g band in Pa3 MgO2 measured in this study and in Ref. 19 (green open circle at 1 atm.). Blue triangles are positions of the A1g mode in BaO2. Black circles are computed frequencies of the A1g mode in I4/mcm MgO2.

Raman spectra of I4/mcm MgO2 were followed on A2 decompression run. In Fig. 4B the pressure-frequency dependence of the A1g band of I4/mcm MgO2 is compared with that in BaO2 (Ref. 22) and Pa3 MgO2 (this study and Ref. 19). We could only trace the high-frequency band down to 50 GPa, and then at 0–10 GPa because of the overlap with the overtone of oxygen L2 peak (2υL2)20. Expectedly, the pressure dependence of the frequency O-O symmetric stretching in Pa3 MgO2 is similar to that in I4/mmm BaO2. The DFT-computed frequencies of the A1g in I4/mcm MgO2 also have a similar slope in the 90–150 GPa pressure range. However, the measured pressure dependence of the high-frequency band in the synthesized sample is less steep. Interestingly, at 1 bar the position of high-frequency band (857 cm−1) is almost identical to the position of A1g mode in Pa3 MgO2 (864 cm−1) (Ref. 19) suggesting that the recovered product is likely Pa3 MgO2. Overall, our data provide spectroscopic evidence for the peroxide ion in the synthesized material and that the material containing peroxide ion is preserved to ambient conditions.

Energy-dispersive x-ray spectroscopy

Mapping the extracted sample with an energy-dispersive x-ray spectroscopy (EDS) revealed that the laser-heated area has higher oxygen content (36 ± 2 at% Mg, 64 ± 3 at% O) than the area that was not subjected to high temperatures (Fig. 5). Detailed chemical characterization, however, was not possible because unreacted MgO is mixed with the oxygen-rich phase in the laser-heated area. Nevertheless, EDS analysis provides independent evidence for MgO2 in the recovered sample.

Figure 5: Electron microscope images of the extracted sample (run A2).
Figure 5

(A) SEM micrograph. Laser-heated area is shown with a dashed circle. (B) Energy-dispersive x-ray spectroscopy image. Color intensity is proportional to the element abundance. The laser-heated area (white dashed line) has higher oxygen content. The white scale bar corresponds to 15 μm.


Bragg peaks of MgO2 were sharp in quenched samples right after the synthesis which allowed for a reliable volume determination with small σ values (Supplementary Table S1). On decompression, however, XRD peaks become broad probably due to the phase instability and volume measurements were less certain. Decompressed samples were mapped with the x-ray beam in order to find the best quality XRD, but only relative variations in Bragg peaks intensities were revealed. The new phase was still observed in XRD of the sample B2 decompressed down to 75 GPa. P-V data obtained on the sample B2 decompression is marked with an asterisk in the Supplementary Table S1. At P < 75 GPa the XRD peaks become too broad and start overlapping with peaks from other materials precluding identification of the MgO2 phase. Therefore, it remains unclear what physicochemical transformations occurred in the synthesized phase at P < 75 GPa. However, at 1 bar the laser-heated area of the recovered sample (A2) (Supplementary Fig. S2) shows a Raman signature of a peroxide ion with the Raman shift identical to that in Pa3 MgO2.

Figure 6 shows a fit of the I4/mcm MgO2 P-V data collected upon compression (red line) and decompression (blue line) to the room temperature third-order Birch-Murnaghan equation of state (EOS). Sample annealing was not performed upon decompression which resulted in less precise P-V information. We also computed the I4/mcm MgO2 volume in the 70–150 GPa pressure range (Supplementary Table S2). The EOS parameters are reported in the Supplementary Table S3. The theoretically computed volumes are systematically 1.1% larger than the experimental ones in the 100–150 GPa pressure range, which is within the computational uncertainty.

Figure 6: The 300 K third-order Birch-Murnaghan EOS of I4/mcm MgO2.
Figure 6

Red line is EOS fit to the experimental data from runs A1, A2 (red circles), and B2 (red triangles) collected upon compression. Blue line is EOS fit to the experimental data collected on decompression (B2* in the Supplementary Table S1). The pressure error bar is based on the reported uncertainty of the MgO EOS (A-runs) and the maximum pressure difference between MgO and Au pressure gauges (B-runs). Green diamonds and green line are the DFT EOS of I4/mcm phase. Black dashed line is the sum of the unit cell volumes of MgO and O2 (taken with proper coefficients as dictated by the synthesis reaction and the number of formula units in the MgO and O2 unit cells). Inset: Experimental pressure-composition phase diagram of the Mg-O system as determined in this work. Stable phases are shown with thick solid lines.

I4/mcm MgO2 can be synthesized in the mixture of MgO with O2 at 96 GPa indicating a thermodynamic stability of MgO2 at this pressure, which is close to the theoretically predicted pressure of 116 GPa (Ref. 12), especially if one keeps in mind that the theoretical prediction was done at zero temperature. We therefore conclude that I4/mcm MgO2 is a thermodynamically stable phase in the high pressure phase diagram of the Mg-O system (Fig. 6, inset). The thermodynamic stability of I4/mcm MgO2 at P > 96 GPa is not surprising as heavier Group II elements, strontium and barium, form stable peroxides with CaC2-type (I4/mmm) crystal structure at ambient pressure with the O-O bond parallel to the c axis and 2 MO2 (M = Sr, Ba) formula units in the unit cell14. The O-O chemical bond length in MgO2 is 1.454 (1) Å at 96 GPa, which is comparable to that of SrO2 (1.483 Å) and BaO2 (1.493 Å) at standard conditions14. I4/mcm MgO2, however, has 4 formula units in the unit cell and the O-O bond is parallel to the ab plane diagonal (Supplementary Fig. S3A,B).

Taking into account that Fm3m MgO has 4 formula units and C2/m oxygen (ε−, ζ−) has 8 O2 molecules in the unit cell we calculated the volume of MgO + 1/2 O2 as a function of pressure using the reported MgO and O2 EOS18,23 (Fig. 6, dashed curve). It is apparent that I4/mcm MgO2 is denser than the reactants in the studied pressure range. Interestingly, the reaction of MgO with O2 at P > 96 GPa promotes an 8-fold coordination of Mg2+ at much lower pressures than expected for Fm3m to Pm3m (NaCl-type to CsCl-type) transition in pure MgO (500 GPa)2,3,12. In the I4/mcm phase of MgO2, there is a covalently bonded peroxo-group O22−, ionically bonded with Mg2+ ions. The arrangement of Mg2+ and O22− ions is topologically identical to the CsCl structure type (Supplementary Fig. S3B,C).

In situ XRD at T = 2150 K (Fig. 1) demonstrates that MgO2 is stable at high temperature. Thus, MgO2 may be present together or instead of MgO in highly oxidized planetary interiors. Overall, the case of I4/mcm MgO2 shows that even the most inert planetary-forming minerals may be prone to chemical transformations.


Materials and samples

Diamond anvils with culets of 200, 300/100, and 300/80 μm were used to access the 100–160 GPa pressure range. Rhenium foils (200 μm thick) were indented to a thickness of 30–40 μm and then laser-drilled to create holes (30–100 μm in diameter) serving as sample chambers. Two types of chemical precursors were loaded in DAC to study the MgO-O2 phase diagram in the 0–160 GPa pressure range (see Table 1 and Fig. 1, inset). Magnesium oxide (99.85%) available from Alfa-Aesar was used for the type-A experiments. Before sample loadings magnesia was annealed at 1293 K for 12 hours to get rid of any adsorbed water. Two MgO disks were made by compressing the magnesia powder to a thickness of 4–5 μm and were stacked in the gasket hole. The remaining volume of the sample chamber was filled with liquefied zero-grade oxygen (99.8%, Matheson Gas Products) at approximately 77 K. In type-B experiments we used magnesium peroxide complex available from Sigma-Aldrich (24–28% Pa3 MgO2, 42–46% MgO, ~30% Mg). The magnesium peroxide complex was mixed with submicron gold powder and loaded in the sample chambers with no pressure medium.

Synthesis and characterization

All XRD experiments were performed at the undulator beamline at 13ID-D GeoSoilEnviroCARS, APS, using the online double-sided laser-heating system24. Oxygen exhibits strong near-infrared absorption at P > 10 GPa25,26,27 which allowed coupling the 1064 nm laser-heating radiation directly to oxygen in type-A experiments. Moreover, at P > 96 GPa oxygen turns metallic18,20,28 boosting the laser-heating efficiency. Finite element calculations reveal that diamond-sample interface remains at near-ambient temperatures almost independent of the sample and pressure medium, owing to diamond’s remarkable thermal conductivity29,30. Accordingly, no sign of etching was found on diamond anvils under an optical microscope after the experiments. In type-B runs, laser-heating radiation was coupled to the gold powder.

Synchrotron XRD was collected in situ at high temperature and high pressure in the diamond anvil cells to determine the onset of chemical and physical transformations with the x-ray beam (37.077 keV) focused to 4 μm spot size. Temperature was measured spectroradiometrically (Supplementary Fig. S4) simultaneously with XRD and calculated using the T-Rax software (C. Prescher). Temperature uncertainty of 150 K was assumed, typical of laser-heating DAC experiments24,31.

Mapping quenched samples with a step size of 5 (A runs) or 2 (B runs) μm to find areas with less O2 or Au, but with MgO was necessary for a careful indexing of the new phase XRD and to minimize the effect of pressure gradients across the sample chamber. MgO was present in both type-A and type-B experiments allowing consistent P-V measurements across the A- and B-runs. Tange et al.32 MgO pressure scale was preferred as it is based on several pressure-scale-free MgO thermodynamic data sets and allowed for minimal discrepancies with Au EOS33 in type-B experiments at 150–160 GPa. The maximum pressure differences observed between the MgO32 and Au33 EOS were on the order of 3–6 GPa (at 150 GPa), which was taken into account upon the I4/mcm MgO2 EOS fitting.

2D XRD patterns were integrated using the DIOPTAS software34. Manual background subtraction was done in Fityk (Ref. 35). Preliminary Bragg peaks indexing was performed with Dicvol06 (Ref. 36). GSAS/EXPGUI (Ref. 37, 38) was used for Rietveld refinement in accordance with the guidelines provided in Ref. 39, 40. Oxygen spotty reflections overlapping with the continuous lines produced by the new phase were masked. Also, we did not use the region of 2θ >13° where the background scattering is not uniformly distributed in the azimuth range of 0 to 360°. Scaling factors and unit cell parameters were refined first. Subsequently, peak profiles were fit with the pseudo-Voigt function and, at last, we refined the oxygen fractional coordinate (x in the 8 h position) of I4/mcm MgO2. Crystal structures were visualized with the use of VESTA 3 (Ref. 41). The 300 K third-order Birch-Murnaghan EOS was obtained using a (sigma)volume-weighted fitting procedure was performed as implemented in the EoSFit7GUI42.

Raman characterization of the quenched samples was performed in the Geophysical Laboratory. Solid-state lasers with 488, 532, and 660 nm lines focused to 3–4 μm were used as excitation sources. Backscattered Raman radiation was analyzed by a single-stage grating spectrograph equipped with a CCD array detector. The spectral resolution was 4 cm−1.

Our XRD and Raman data does not allow ruling out the formation of rhenium oxides at the gasket edge. However, the possible synthesis of rhenium oxides did not affect the careful characterization of I4/mcm MgO2. The tightly-focused x-ray beam allowed us analyzing reaction products within the laser-heated region and without sampling of the near-gasket regions. Likewise, Raman spectra assigned to the I4/mcm MgO2 were collected in a sample area shielded from Re by the oxygen rim (Supplementary Figure S2). At the same time, Raman data collected from the oxygen rim near the gasket had revealed only spectroscopic signatures of oxygen itself (Fig. 4A).

Energy-dispersive x-ray spectroscopy (EDS) analysis was performed on a dual beam focused ion beam/scanning electron microscope (FIB/SEM Zeiss Auriga 40) equipped with an Oxford X-Max 80 mm2 large-area silicon drift detector at the accelerating voltage of 5 kV in the Geophysical Laboratory. The analyzed sample was coated with Ir (~5 nm) to prevent specimen charging. Pyrope and the ENEL20 glass were used as standards for oxygen and magnesium, respectively.

Density functional theory (DFT) within the Perdew-Burke-Ernzerhof (PBE) generalized gradient approximation (GGA)43 as implemented in the VASP code44, was used for structural and vibrational analysis. For the structural relaxation, we used the all-electron projector-augmented wave (PAW) method45 and the plane wave basis set with the 600 eV kinetic energy cutoff; the Brillouin zone was sampled by Г-centered meshes with the resolution 2π × 0.06 A−1. The phonon frequencies were calculated using the finite displacement approach as implemented in the Phonopy code46. The Raman intensities were obtained by computing the derivative of the macroscopic dielectric tensor with respect to the normal mode coordinate47.

Additional Information

How to cite this article: Lobanov, S. S. et al. Stable magnesium peroxide at high pressure. Sci. Rep. 5, 13582; doi: 10.1038/srep13582 (2015).


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The study was supported by the Deep Carbon Observatory, the National Science Foundation (EAR-1114313, EAR-1015239, EAR-1128867, DMR-1231586), DARPA (Grants No. W31P4Q1210008 and No. W31P4Q1310005), the Government of Russian Federation (grants 14.A12.31.0003 and 14.B25.31.0032), and Foreign Talents Introduction and Academic Exchange Program (No. B08040), National Natural Science Foundation China (No. 21473211). Portions of this work were performed at GeoSoilEnviroCARS (Sector 13), Advanced Photon Source (APS), Argonne National Laboratory. GeoSoilEnviroCARS is supported by the National Science Foundation - Earth Sciences (EAR-1128799) and Department of Energy- GeoSciences (DE-FG02-94ER14466). This research used resources of the Advanced Photon Source, a U.S. Department of Energy (DOE) Office of Science User Facility operated for the DOE Office of Science by Argonne National Laboratory under Contract No. DE-AC02-06CH11357. Calculations were performed on XSEDE facilities and on the cluster of the Center for Functional Nanomaterials, Brookhaven National Laboratory, which is supported by the DOE-BES under contract no. DE-AC02-98CH10086. N.H. was supported by Army Research Office (No. W911NF-13-1-0231). Maddury Somayazulu and other co-workers at the Geophysical Laboratory are thanked for their comments on earlier versions of this manuscript.

Author information


  1. Geophysical Laboratory, Carnegie Institution of Washington, Washington, DC 20015, USA

    • Sergey S. Lobanov
    • , Nicholas Holtgrewe
    •  & Alexander F. Goncharov
  2. V.S. Sobolev Institute of Geology and Mineralogy SB RAS, Novosibirsk 630090, Russia

    • Sergey S. Lobanov
  3. Department of Geosciences, Department of Physics and Astronomy, Stony Brook University, Stony Brook, NY 11794, USA

    • Qiang Zhu
    •  & Artem R. Oganov
  4. Howard University, 2400 Sixth Street NW, Washington, DC 20059, USA

    • Nicholas Holtgrewe
  5. Center for Advanced Radiation Sources, University of Chicago, Chicago, IL 60632, USA

    • Clemens Prescher
    •  & Vitali B. Prakapenka
  6. Moscow Institute of Physics and Technology, 9 Institutskiy lane, Dolgoprudny city, Moscow Region, 141700, Russian Federation

    • Artem R. Oganov
  7. School of Materials Science, Northwestern Polytechnical University, Xi’an, 710072, China

    • Artem R. Oganov
  8. Key Laboratory of Materials Physics, Institute of Solid State Physics, CAS, Hefei, 230031, China

    • Alexander F. Goncharov
  9. University of Science and Technology of China, Hefei, 230026, China

    • Alexander F. Goncharov
  10. Skolkovo Institute of Science and Technology, Skolkovo Innovation Center, 5 Nobel St., Moscow 143026, Russia

    • Artem R. Oganov


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S.S.L., A.F.G. and A.R.O. designed the study. S.S.L., N.H. and A.F.G. performed the experimental work with an active assistance of C.P. and V.B.P. Theoretical calculations were performed by Q.Z. and A.R.O. All authors discussed the results and the implications. S.S.L. analyzed the data and wrote the paper.

Competing interests

The authors declare no competing financial interests.

Corresponding author

Correspondence to Sergey S. Lobanov.

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