Dynamics of self-reorganization explains passivation of silicate glasses


Understanding the dissolution of silicate glasses and minerals from atomic to macroscopic levels is a challenge with major implications in geoscience and industry. One of the main uncertainties limiting the development of predictive models lies in the formation of an amorphous surface layer––called gel––that can in some circumstances control the reactivity of the buried interface. Here, we report experimental and simulation results deciphering the mechanisms by which the gel becomes passivating. The study conducted on a six-oxide borosilicate glass shows that gel reorganization involving high exchange rate of oxygen and low exchange rate of silicon is the key mechanism accounting for extremely low apparent water diffusivity (10−21 m2 s−1), which could be rate-limiting for the overall reaction. These findings could be used to improve kinetic models, and inspire the development of new molecular sieve materials with tailored properties as well as highly durable glass for application in extreme environments.


In nature, silicate glasses and minerals dissolve incongruently by various interrelated processes such as water diffusion in the solid, ion exchange, hydrolysis, condensation, and precipitation of secondary phases1,2,3,4,5,6. The global dissolution kinetics of the primary solid depends on its composition, its structure, and also on the fluid properties (e.g., pH, composition, and flow rate)7. As a result, the less-soluble elements will form new phases on the reacting surface, either by dissolution–reprecipitation3,4,6 or by local rearrangement8,9. These phases can be amorphous or crystalline, dense, or porous10. These products change the solution composition; this can affect both the driving force for further dissolution and the mass transfer between the bulk solution and the reactive surface1,6. To date, the role of surface layers remains insufficiently understood to derive rate laws that can accurately predict the fate of silicate phases in various natural or engineered environments10,11. This is, however, an important need in many fields: in geochemistry to calculate the budget of some elements in the rivers and in the oceans, for the geological sequestration of CO2, for the safety assessment of geological disposal of nuclear waste, etc. In the case of borosilicate glass used to confine nuclear wastes, several hypotheses are still under debate to account for the 3–5 orders-of-magnitude decrease of the dissolution rate measured in confined environments: (i) saturation of the solution in silica thereby decreasing the chemical driving force for the dissolution reaction12, (ii) pore closure within the gel layer limiting the transport of aqueous species9, (iii) water diffusion in the pristine solid13, (iv) diffusion of dissolved silica through the gel layer leading to higher concentrations at the reaction front2, and more recently (v) slow mobility of water molecules in the gel due to their confinement in constricted micropores14,15. The reasons why so many hypotheses are still under consideration are that high-resolution and high-sensitivity analytical tools available to investigate reacting buried interfaces are limited, and the composition and properties of alteration layers depend on many intrinsic and environmental parameters, complicating any attempt of a general theory5,16.

Here, we propose an approach based on three experiments with isotopically tagged water molecules to study their mobility and their reactivity in a passivating gel formed on International Simple Glass (ISG), a six-oxide borosilicate reference glass17, as well as molecular dynamics (MD) simulations and continuum-scale modeling to support experimental findings. Although isotopes have been used previously to investigate glass or mineral alteration mechanisms6,18,19,20,21, another approach relying on the quantification of the passivating properties of the alteration layer is proposed here. The first experiment studies the dynamics of water in a gel formed during a 1-year-long alteration of ISG glass monoliths, and the second and the third experiments explore the dynamics of self-reorganization of a young and a mature gel, respectively. All the gels have been obtained by alteration of ISG at 90 °C, pH 7 in a solution initially saturated with respect to amorphous silica and containing K (called reference conditions in the following). It was demonstrated in a previous study that these conditions lead to the formation of a micrometer thick, uniform, and chemically homogeneous, passivating gel layer free of secondary phases14. Monoliths tested in experiments 1 and 3 come from the experiment described in Gin et al.14, whereas experiment 2 is a short-term experiment conducted in similar conditions. From this study, we infer that hydrolysis–condensation reactions within the gel strongly affect the transport of water molecules and thereby limit glass dissolution.


Water dynamics in a mature gel

For the first experiment, we have selected a passivating gel formed by ISG glass alteration in the reference conditions. In this medium, after 1 year, the glass dissolution rate dropped by a factor 1000 relative to the initial dissolution rate and a 1.5-µm-thick gel-like material formed on the glass surface (Fig. 1). Note that this value is more accurate than that estimated in a previous study14 due to a larger number of data points giving a long-term trend. This film was partly characterized in a previous study22 and its characterization was completed by the assessment of water content, speciation, and mean pore size22,23 (Table 1 and Supplementary Note 1). This experiment therefore probes a uniform, 1.5-µm-thick amorphous gel formed by reorganization of the Al–Zr–silicate glassy network following the release of B, Na, and Ca and the incorporation of some K supplied by the leachate14. In this material, pore size is of the order of 1 nm. Six pieces of this altered glass were subsequently immersed at 25 °C in H218O (18O/16O ~ 7) for various durations up to 3 months and the oxygen isotopic profiles were recorded by time-of-flight secondary ion mass spectrometry (ToF-SIMS). Complementary analyses were carried out to validate the analytical protocol and verify the accuracy of the 18O/16O measurements (Supplementary Note 2).

Fig. 1

Experiment from which pieces studied in experiment 1 and 3 were taken. This initial experiment was conducted in the so-called “reference conditions” (90 °C, pH90 °C 7, 160 mg L−1 of Si and 6 g L−1 of K). The image displays the reactor, the sample holders, and a few glass pieces. More details are provided in Gin et al.14. Experiment 2, although conducted on new fresh glass pieces corresponds to the early stages of the initial experiment. a Time evolution of the equivalent thickness of altered glass calculated from B concentration in solution. A few data points deviate from the overall trend because of the low concentration of B and the high dilution factor (11) prior to ICP-OES analyses. b Glass dissolution rate derived from the correlation displayed in a. Error bars represent s.d.

Table 1 Main features of the pristine and altered glass

Figure 2a shows that, for all contacting durations, 18O exchanged with 16O in the gel and penetrated up to the reactive interface, which was well defined by a sharp change in the B concentration (Fig. 2b). Moreover, the measurable increase of 18O in the gel is observed even at the shortest contacting time (3 min) and its concentration significantly increases with time. We also note that all 18O/16O profiles are mostly flat with a slight but significant increase in the 200 nm near the reactive interface, likely due to the greater number of exchangeable O atoms in this less-mature area. According to the mean value of the O isotopic ratio measured in the gel, the time evolution of the percentage of exchanged O atoms was calculated assuming that only O from molecular water and silanols could exchange (Fig. 2c). It is found that only ~0.2% of these supposedly mobile O atoms had exchanged quickly (≤3 min). This fraction increases with time but remains below 6% even after 3 months (Table 2).

Fig. 2

Water mobility in the gel. Water mobility is recorded by time-dependent isotopic and elemental ToF-SIMS profiles (experiment 1). For a and b, only lines are displayed for a better readability, and the analytical step is 7 nm. a Quantitative 18O/16O profiles in the gel for the different contacting durations. The mean value of the O isotopic ratio in the pristine glass (2.2 × 10−3) is within uncertainty of the natural abundance (2.05 × 10−3). b Normalized boron profiles for the same durations. The alteration front, given by the normalized concentration of 0.5 is located at 1574 ± 20 nm. The shifts between the different profiles give the analytical error of the technique, which is small. For a given contacting time, the B profile is well anti-correlated with the 18O/16O profile, indicating that some tagged water molecules reached the glass dissolution front at all tested durations. Some B is retained in the gel as evidenced by the B concentration on the gel side of the gel/pristine glass interface, which does not fall to zero. This likely corresponds to undissolved glass clusters15. c Evolution of the mean value of the oxygen isotopic ratio within the gel as a function of contacting time with the H218O solution. Error bars are calculated from uncertainites on natural abundance in the pristine glass

Table 2 Fraction of exchanged mobile O

A model for water diffusion in passivating gel

The results from experiment 1 are consistent with a pore network made of a few deeply penetrating open channels and a large amount of dead-end or closed pores in which water molecules and silanols cannot exchange easily (Fig. 3). The basic assumption is that water molecules randomly explore the open porosity, and react with (Si, Al, and Zr)–O–Si bonds to open (by hydrolysis reactions) and close (by condensation reactions) pores within the gel. A model was developed according to these hypotheses (Supplementary Note 3). In this approach, the gel is assumed to contain spherical pores with a single mean pore radius. Some fraction of the pores are connected in aggregates that run from the solution/gel interface to the gel/pristine glass interface and are thus treated as cylinders for simplicity. The diffusion coefficient of water in connected pores (exchange mode 1), Dc, is derived from a fit to the O isotopic profile recorded at 3-min contacting time using the Crank solution of Fick’s second law for a one-dimensional Cartesian case (Supplementary Fig. 4). Although the exact value cannot be determined, a value ≥10−11 m2 s−1 is expected to account for the flat experimental profile. Owing to the fast diffusion in connected pores, these pores rapidly equilibrate with the 18O-enriched solution and can serve as a continuous source of 18O that diffuses through the gel, via gel reorganization, to reach closed pores. The diffusion coefficient for water diffusion out of the connected pores and into the gel (exchange mode 2), Dd, was calculated using an approximation to the Crank solution of Fick’s second law in cylindrical geometry (see full derivation in Supplementary Information 3). This analysis led to values of Dd that decreased with time following a power law (Supplementary Fig. 5), which could be indicative of a decrease in water diffusivity through the gel due to self-reorganization. Dd decreased to ~10−21 m2 s−1 within 24 h and reached 6 × 10−23 m2 s−1 after 3 months. Because isotopic equilibration was not achieved even after 3 months, it is likely that water diffusion could slow down further with time.

Fig. 3

A model for water diffusion in passivating gels. Conceptual model for interpreting water diffusion in passivating gel (left) and the corresponding mathematical model used to determine the water diffusion coefficients (right). The gel is assumed to contain spherical pores with mean pore radius, r, and a fraction of the pores are connected in aggregates that run from the solution/gel interface to the gel/pristine glass interface and are thus treated as cylinders with mean separation distance, <rc>. Exchange modes 1 and 2 with diffusion coefficients Dc and Dd, respectively, are illustrated in red

To summarize, the gel behaves as a molecular sieve for water molecules with a few open pathways allowing rapid diffusion and many closed pores that reduce water diffusivity by at least eight orders of magnitude. This raises two questions: (i) do simulations at the pore scale support the idea that water diffusivity can be ≥10−11 m2 s−1 in open but narrow channels of the order of 1-nm width, and (ii) is there any experimental evidence that the gel undergoes hydrolysis and condensation reactions once it is formed, as was indirectly seen in mesoporous silica?24

In order to address the first question, water diffusion coefficients D in amorphous silica micropores of diameter ranging from 0.5 to ~4 nm were evaluated by MD simulations with reactive potentials25,26 (Supplementary Note 4). Pure silica was selected as reliable potentials have been developed for the silica-water system and as the actual gels are made of more than 90% of SiO2 (Table 1). D values are plotted as a function of the radial distance from the center of the cylindrical pores (Fig. 4a). An unconstrained bulk diffusivity of ~2.5 × 10−9 m2 s−1 27,28 is attained only at the center of the largest pore. While similar results have been obtained with non-reactive potentials29 with controlled addition of silanols, the use of reactive potentials in this work allows for dissociation of water, proton exchange, and formation of surface silanols. Close to the wall, water molecules form hydrogen bonds with oxygen in the silanols and other oxygen from the glass (Fig. 4a, b). The formation of hydrogen bonds of water with relatively immobile species in the glass leads to lowering of water diffusivity by an order of magnitude for water molecules that are closer to the pore wall. These slow water layers induce a drag on other water molecules and reduce diffusivity in the center, especially in smaller pores. If the pore diameter is large enough, water molecules at the center of the pore are hydrogen bonded only to the nearby mobile ones and hence have a diffusivity closer to that of water in bulk. These results show that, as long as the pores remain open and larger than 0.5 nm in diameter, water diffusion is not dramatically affected by interactions with pore walls. This important result supports the idea that the value of Dc derived from the modeling of the isotopic tracing experiments corresponds to water diffusion in open but constricted micropores, whereas Dd is tied to diffusion between closed pores limited by bond breaking.

Fig. 4

Water diffusivity in amorphous silica micropores. a Self-diffusion coefficient of water as a function of distance from the center of the pore in cylinder pores of amorphous silica with diameters of 0.5, 0.9, 1.6, and 3.6 nm from reactive force field-based molecular dynamics simulations. At the center of the pore, diffusing water molecules do not see the reactive sites in the wall and are relatively less constrained. The inner walls of the pore are oxygen terminated with atomic-scale roughness and reaction with water results in changes in the surface structure. Water molecules have been observed to diffuse up to a nanometer into the silica structure beyond the surface and further change the surface structure. The dashed lines corresponding to the color of the curves represent the approximate location of the pore wall. b Mean water diffusion coefficients at the pore wall and at the center of the pore for various pore sizes. In-between figures a and b, a snapshot of the 0.9-nm pore system with a section of the silica structure removed to show water in the pore. The silica structure is shown as the gray block and water on either side is shown as molecules inside the transparent blob

Furthermore, MD simulations were performed to obtain ISG glass and gel structures and analyzed the bottleneck and interstitial site density to understand available sites for water diffusion (Fig. 5 and Supplementary Note 4). Two gel structures were simulated from the glass. The first type of gel structure, called “Na-removed” in the following was obtained by removing Na atoms only from the ISG structure. The second type, chemically closer to the actual gel, and called “gel” in the following was prepared by removing all Na and B, 30% of Ca, and the free oxygen ions, i.e., oxygen ions that are not bonded to any other atom within a distance of 2.5 Å. The structures were generated using classical MD simulations with recently developed partial charge composition dependent potentials. A zoomed-in region of the 24,000 atoms simulation cell is shown in Fig. 5b. A Voronoi–Delaunay tetrahedron analysis30,31 was performed to find the bottleneck size and interstitial site and density distributions. The results, which represent the available bottlenecks for water molecule diffusion, are shown in Fig. 5a. In the bulk glass structure, the density of bottlenecks with size larger than the size of a water molecule is relatively small. The density increases in the Na-removed structure. In the gel structure, the density of bottlenecks and bottlenecks with larger sizes are much higher, and both contribute to provide channels for water diffusion. The density of bottleneck size with 1.28-Å radius (about the size of a water molecule) is 1.2, 2.2, and 2.8/nm3 for ISG, Na-removed, and gel, respectively. These results are consistent with a recent MD study showing that a silica gel structure has randomly connected pores with certain pore size distributions that form channels for water diffusion32. Overall, this study at the nanometer scale suggests that the release of mobile species during glass alteration creates narrow channels in which water diffuses slightly slower than in the bulk, but not slow enough to account for the extremely low values derived from the 18O-tracing experiments (<10−21 m2 s−1). Moreover, the release of mobile species leads to a reorganization of the silicate network which might affect the diffusion pathways.

Fig. 5

Bottleneck distribution in International Simple Glass and gel. a Bottleneck density distribution with bottlenecks larger than 1.28-Å radius for bulk ISG, Na-depleted ISG, and ISG gel structures. The inset shows a tetrahedron with a water molecule in the bottleneck (side face) and interstitial (center of the tetrahedron) sites. b Snapshot of a zoomed-in region of an ISG glass structure from MD simulations showing glass-forming network made up of [SiO4] (yellow), [AlO4] (blue), [BO4] and [BO3] (brown), and [ZrO6] (green) and charge compensator or network modifier elements, Na (pink) and Ca (golden). Oxygen atoms are displayed in red (see also Supplementary Fig. 6)

Role of gel restructuring on passivation

To address the second question, i.e., whether the gel undergoes hydrolysis and condensation reactions once it is formed, two experiments were conducted in the reference conditions, one focused on the early stages of gel formation (experiment 2), and the other focused on a mature gel (experiment 3). For experiment 2, two solutions were prepared: solution S1 with natural water (18O/16O = 2 × 10−3) and solution S2 with 18O-enriched water so that 18O/16O = 0.24. Three polished pieces of unaltered ISG were first altered in solution S1 for 3 days, after which one piece was withdrawn for ToF-SIMS depth-profiling analysis, while the other two were transferred to solution S2 for an additional 4 or 10 days of alteration. Overall, O isotopic ratios were recorded in gels formed after 3, 7, and 13 days of alteration (Fig. 6). The gel thickness obtained from the B profiles was 500, 600, and 740 nm at day 3, 7, and 13, respectively (Fig. 6a). As expected, the gel analyzed after 3 days had the O isotopic signature of natural water. Importantly, no enrichment of 29Si was noticed in the gel (Fig. 6b, inset), confirming previous results indicating that, in silica-saturated and near-neutral pH conditions, Si from the glass does not dissolve, diffuse, and redeposit14.

Fig. 6

Dynamics of self-reorganization of a young gel. Dynamics is monitored by ToF-SIMS depth profiling (experiment 2). a Experimental protocol: piece 1 (orange) was altered for 3 days in solution S1 only, piece 2 (green) was altered 3 days in solution S1 followed by 4 days in solution S2, and piece 3 (blue) is similar to piece 2 but the alteration duration in solution S2 was 10 days. b Normalized B profiles showing the position of the alteration front at the three considered durations. The inset displays the 29Si/28Si ratio in the gel of piece 1. Although the glass is altered in a solution highly enriched in 29Si, the gel keeps the isotopic signature of the glass. c Oxygen isotopic profiles in the three gels. Contrary to Si, O in the gel displays an isotopic signature close to that of the solution. For ToF-SIMS profiles, only lines are displayed for a better readability, and the analytical step is 7 nm

When in contact with solution S2, the glass continued to alter but the isotopic signature of the gel originally formed in solution S1 increased to a mean value of 0.15, which is very close to that recorded in the 100 nm of a new gel formed between days 3 and 7. From 7 to 13 days, the 18O/16O ratio increased further in the part of the gel formed in natural water by an amount that is beyond the noise of the signal (0.15 → 0.17) as well as in the gel formed between day 3 and 7 (0.13 → 0.18). According to the O speciation in the gel (Table 1), and assuming that water molecules and silanols exchange first, a mass balance analysis indicates that 62% of the bridging O of the gel network was hydrolyzed and exchanged between days 3 and 7 and this figure increased to 70% at day 13. This is direct evidence that the young gel undergoes hydrolysis and condensation reactions that allow for isotopic exchange. Because Si atoms of the gel do not exchange with Si species in solution, it must be concluded that all the Si−O bonds of a given Si atom in the gel are not broken simultaneously. An alternative explanation, whereby all Si−O bonds are hydrolyzed, H4SiO4(aq) is released in pore water, and then quickly condenses has been ruled out in a previous study14.

Experiment 3 explored the behavior of a mature gel. This gel resulted from the alteration of ISG that altered 1625 days in the reference conditions (Fig. 1). A piece of 1625 d was immersed for 1 month in a solution at 90 °C, pH 7, saturated with respect to amorphous silica, and spiked with 18O, so that 18O/16O = 0.24. The O isotopic ratio was then recorded by ToF-SIMS depth profiling (Fig. 7). The shape of the O profile in the gel is similar to that obtained in tracing experiment 1 conducted at room temperature (Fig. 2a) but the 18O enrichment is much higher due to a greater reactivity at 90 °C than at room temperature20. In experiment 3, 21.1% of all O atoms available in the gel have been exchanged after 1 month. This value is close to the fraction of mobile O calculated from the budget of water molecules and silanols (28.4%, Table 1). However, experiment 1 demonstrated that a large faction of mobile O atoms are not easily accessible. To exchange these atoms between close and dead-end pores, network reorganization is necessary. This means that a total exchange of mobile O would necessarily be associated to some exchange of the O from the network, resulting in a higher 18O/16O ratio than that at equilibration. As a consequence, the mean 18O/16O obtained here (5.3 × 10−2) suggests that a fraction of mobile O and bridging O of the gel network were exchanged, although the exact amounts are unknown.

Fig. 7

Dynamics of reorganization of a mature gel. Oxygen isotopic ratio and B profiles recorded by ToF-SIMS depth profiling on a piece altered 1625 days (experiment 3) in the initial experiment and then placed 1 month in similar conditions (90 °C, pH90 °C 7, silica-saturated solution) with water spiked with 18O (18O/16O = 0.24). During this 1-month experiment, the oxygen isotopic signature of the gel raised from natural abundance to 0.125 on average, leading to a fraction of exchanged O of 21.1%

According to experiments 2 and 3, it is shown that both an early-formed and a mature gel could undergo hydrolysis and condensation reactions, suggesting that the gel reorganization is a continuous process affecting the pore connectivity and thus the mobility of water molecules. Although more research is needed to determine the kinetic constant and the activation energy of each type of reaction involving O, our results show that the consumption of water molecules in the exchange with silanols and bridging oxygens affects the flux of water molecules reaching the pristine glass surface. Indeed, a simple calculation based on the results of experiment 1 estimates that the flux of water molecules through the 1-year-old passivating gel is decreased by approximately four orders of magnitude compared to a non-passivating gel formed in a Si-free solution (Supplementary Note 4). Previous studies proposed that hydrolysis, diffusion, and redeposition of Si were the key processes leading to the densification of the outer part of the gel, thereby closing open pores formed by the release of mobile species and eventually stopping further glass corrosion simply by preventing water molecules from reaching the pristine glass surface9,33,34. This paradigm must be revised as the present work shows that gel reorganization could be a continuous phenomenon involving a high reactivity of O and low mobility of Si. The simplistic idea that the gel is a rigid, strain-relaxed, and porous structure once formed, either totally inherited from the glassy network or re-precipitated, must also be revised, as its passivating properties mostly depend on reactions between water molecules and (Si, Al, and Zr)−O−Si bonds with bonding oxygen of the network. It is also expected that both the topology of the pore network and its dynamics of maturation depend on parameters such as glass composition, solution composition and pH, and temperature. Adjustment of these parameters––especially the relative proportion of low-strength bonds (e.g., Si−O−B) that might lead to rapid reorganization but also to extensive dissolution and high-strength bonds (e.g., Si−O−Zr)––could lead to the development of new materials, for instance, for controlled drug release or the fabrication of glasses resistant to extreme conditions. For nuclear glass, the design of a smart engineered barrier supplying the glass surface with elements rending the gel dense and chemically-and-radiation-resistant might contribute to improving the safety demonstration of geological repositories and eventually public acceptance.


Glass and experimental design

ISG glass was prepared by MoSci Corporation (Rolla, MO, USA)17. Pieces were cut and polished to optical grade. The alteration experiment dedicated to the formation of the passivating gels studied in experiment 1 and 3 of the present work was conducted with 16 pieces placed in perfluoroalkoxy (PFA) vessel, in controlled conditions: (90 ± 1) °C, pH90 °C 7 ± 0.2, 6 g L−1 K, and 160 ± 10 mg L−1 of 29Si corresponding to the saturation of amorphous silica. The reader is referred to Gin et al.35 for more details about this experiment. In this initial experiment, glass alteration was monitored by solution sampling. Samples were diluted and analyzed by inductively coupled plasma-optical emission spectroscopy (ICP-OES, Thermo Scientific ICAP 6300 DUO). Several pieces were withdrawn during the course of the initial experiment: one after 363 days for running experiment 1 of the present study and another after 1625 days for experiment 3.

For experiment 1, the 363-day piece withdrawn in the initial experiment was dried, broken into six pieces, and then placed at (25 ± 2) °C in a solution spiked with H218O, so that 18O/16O = 7 ± 3. These pieces of altered glass were sampled after various durations and analyzed by ToF-SIMS.

Experiment 2 devoted to study the dynamics of the early stages of gel reorganization was performed with fresh ISG pieces at (90 ± 1) °C, pH90 °C 7 ± 0.2, 3 g L−1 K using isotopically natural water in the first 3 days, and in 18O-enriched water between day 3 and 13, so that 18O/16O = 0.24 ± 0.05.

ToF-SIMS analyses were performed by Tescan Analytics, Fuveau, France using a ToF-SIMS5 spectrometer (IonTof––Münster, Germany). The analytical procedure was optimized to minimize exchange between pore water and air humidity and quantify oxygen isotopic ratio in the gel. Details are provided in Supplementary Note 2. A pulsed 25 keV 0.1-pA Bi3++ primary ion source was employed over a rastered area of 50 μm × 50 μm (beam size ≤ 3 μm). Depth profiling was performed using a 2-keV Cs+ sputter beam with a 45° incidence to the glass surface, giving a 195-nA target current over a 200-μm x 200-μm area. A flood gun was used to compensate the charging effect on the surface. Negative ion depth profiles were recorded. These conditions provide a step of 7 nm, similar in the gel and in the glass. Data acquisition and post-processing analyses were performed using the SurfaceLab 6 software. A profilometer was used to measure the crater depth at the end of the analysis. Data are displayed as a function of depth considering the same sputtering rate in the alteration layer and pristine glass.

Molecular dynamics

Molecular dynamics (MD) simulations of water diffusion in amorphous silica micropores were performed with reactive dissociable water potentials25,26 and the LAMMPS package36. Reactive force field-based MD simulations were used previously to study the gel and gel/water interfaces32,37. The Hole program38 was used to determine the location and smoothness of the pore walls. NVT simulations at 298 K were performed for all the systems: 8 ns for the 0.5 and 1-nm pore systems, 4 ns for the 2-nm pore system, and 2 ns for the 4-nm pore system. The diffusion coefficients were calculated as the average of the diffusion coefficient in the radial direction over the length of the pore. See Supplementary Note 4 for more details.

Data availability

The data that support the findings of this study are available from the corresponding author upon request.


  1. 1.

    Frugier, P. et al. SON68 nuclear glass dissolution kinetics: current state of knowledge and basis of the new GRAAL model. J. Nucl. Mater. 380, 8–21 (2008).

    ADS  Article  CAS  Google Scholar 

  2. 2.

    Grambow, B. & Muller, R. First-order dissolution rate law and the role of surface layers in glass performance assessment. J. Nucl. Mater. 298, 112–124 (2001).

    ADS  Article  CAS  Google Scholar 

  3. 3.

    Hellmann, R. et al. Nanometre-scale evidence for interfacial dissolution-reprecipitation control of silicate glass corrosion. Nat. Mater. 14, 307–311 (2015).

    ADS  Article  PubMed  CAS  Google Scholar 

  4. 4.

    Putnis, A. Mineral replacement reactions: from macroscopic observations to microscopic mechanisms. Mineral. Mag. 66, 689–708 (2002).

    Article  CAS  Google Scholar 

  5. 5.

    Ruiz-Agudo, E. et al. Control of silicate weathering by interface-coupled dissolution-precipitation processes at the mineral-solution interface. Geology 44, 567–570 (2016).

    ADS  Article  CAS  Google Scholar 

  6. 6.

    Geisler, T. et al. The mechanism of borosilicate glass corrosion revisited. Geochim. Cosmochim. Acta 158, 112–129 (2015).

    ADS  Article  CAS  Google Scholar 

  7. 7.

    Vienna, J. D., Ryan, J. V., Gin, S. & Inagaki, Y. Current understanding and remaining challenges in modeling long-term degradation of borosilicate nuclear waste glasses. Int. J. Appl. Glass Sci. 4, 283–294 (2013).

    Article  Google Scholar 

  8. 8.

    Casey, W. H., Westrich, H. R., Banfield, J. F., Ferruzzi, G. & Arnold, G. W. Leaching and reconstruction at the surfaces of dissolving chain-silicate minerals. Nature 366, 253–256 (1993).

    ADS  Article  CAS  Google Scholar 

  9. 9.

    Cailleteau, C. et al. Insight into silicate-glass corrosion mechanisms. Nat. Mater. 7, 978–983 (2008).

    ADS  Article  PubMed  CAS  Google Scholar 

  10. 10.

    Daval, D. et al. Dynamics of altered surface layer formation on dissolving silicates. Geochim. Cosmochim. Acta 209, 51–69 (2017).

    ADS  Article  CAS  Google Scholar 

  11. 11.

    White, A. F. & Brantley, S. L. The effect of time on the weathering of silicate minerals: why do weathering rates differ in the laboratory and field? Chem. Geol. 202, 479–506 (2003).

    ADS  Article  CAS  Google Scholar 

  12. 12.

    Neeway, J., Abdelouas, A., Grambow, B. & Schumacher, S. Dissolution mechanism of the SON68 reference nuclear waste glass: New data in dynamic system in silica saturation conditions. J. Nucl. Mater. 415, 31–37 (2011).

    ADS  Article  CAS  Google Scholar 

  13. 13.

    Ferrand, K., Abdelouas, A. & Grambow, B. Water diffusion in the simulated French nuclear waste glass SON 68 contacting silica rich solutions: experimental and modeling. J. Nucl. Mater. 355, 54–67 (2006).

    ADS  Article  CAS  Google Scholar 

  14. 14.

    Gin, S. et al. Origin and consequences of silicate glass passivation by surface layers. Nat. Commun. 6 (2015). https://doi.org/10.1038/ncomms7360.

  15. 15.

    Gin, S. et al. Atom-probe tomography, TEM and ToF-SIMS study of borosilicate glass alteration rim: a multiscale approach to investigating rate-limiting mechanisms. Geochim. Cosmochim. Acta 202, 57–76 (2017).

    ADS  Article  CAS  Google Scholar 

  16. 16.

    Gin, S. et al. The controversial role of inter-diffusion in glass alteration. Chem. Geol. 440, 115–123 (2016).

    ADS  Article  CAS  Google Scholar 

  17. 17.

    Gin, S. et al. An international initiative on long-term behavior of high-level nuclear waste glass. Mater. Today 16, 243–248 (2013).

    Article  CAS  Google Scholar 

  18. 18.

    Valle, N. et al. Elemental and isotopic (29Si and 18O) tracing of glass alteration mechanisms. Geochim. Cosmochim. Acta 74, 3412–3431 (2010).

    ADS  Article  CAS  Google Scholar 

  19. 19.

    McGrail, B. P. et al. The structure of Na2O-Al2O3-SiO2 glass: impact on sodium ion exchange in H2O and D2O. J. Non-Cryst. Solids 296, 10–26 (2001).

    ADS  Article  CAS  Google Scholar 

  20. 20.

    Doremus, R. H. Diffusion of water in silica glass. J. Mater. Res. 10, 2379–2389 (1995).

    ADS  Article  CAS  Google Scholar 

  21. 21.

    Neeway, J. J. et al. Ion-exchange interdiffusion model with potential application to long-term nuclear waste glass performance. J. Phys. Chem. C 120, 9374–9384 (2016).

    Article  CAS  Google Scholar 

  22. 22.

    Collin, M. et al. Structure of international simple glass and properties of passivating layer formed in circumneutral pH conditions. npj Mater. Degrad. 2 (2018).

  23. 23.

    Collin, M., Fournier, M., Charpentier, T., Moskura, M. & Gin, S. Do alkalis affect the passivation of silicate glass? npj Mater. Degrad. In Press (2018). https://doi.org/10.1038/s41529-018-0036-3.

  24. 24.

    Gouze, B., Cambedouzou, J., Parres-Maynadie, S. & Rebiscoul, D. How hexagonal mesoporous silica evolves in water on short and long term: Role of pore size and silica wall porosity. Microporous Mesoporous Mater 183, 168–176 (2014).

    Article  CAS  Google Scholar 

  25. 25.

    Mahadevan, T. S. & Garofalini, S. H. Dissociative water potential for molecular dynamics simulations. J. Phys. Chem. B 111, 8919–8927 (2007).

    Article  PubMed  CAS  Google Scholar 

  26. 26.

    Mahadevan, T. S. & Garofalini, S. H. Dissociative chemisorption of water onto silica surfaces and formation of hydronium ions. J. Phys. Chem. C 112, 5694–5694 (2008).

    Article  CAS  Google Scholar 

  27. 27.

    Holz, M., Heil, S. R. & Sacco, A. Temperature-dependent self-diffusion coefficients of water and six selected molecular liquids for calibration in accurate 1H NMR PFG measurements. Phys. Chem. Chem. Phys. 2, 4740–4742 (2000).

    Article  CAS  Google Scholar 

  28. 28.

    Wang, J. H. Self-diffusion coefficients of water. J. Phys. Chem. 69, 4412–441 (1965).

    Article  CAS  Google Scholar 

  29. 29.

    Bourg, I. C. & Steefel, C. I. Molecular dynamics simulations of water structure and diffusion in silica nanopores. J. Phys. Chem. C 116, 11556–11564 (2012).

    Article  CAS  Google Scholar 

  30. 30.

    Malavasi, G., Menziani, M. C., Pedone, A. & Segre, U. Void size distribution in MD-modelled silica glass structures. J. Non-Cryst. Solids 352, 285–296 (2006).

    ADS  Article  CAS  Google Scholar 

  31. 31.

    Mansas, C. et al. Drivers of water transport in glass: chemical or topological effect of the glass network? J. Phys. Chem. C 121, 16201–16215 (2017).

    Article  CAS  Google Scholar 

  32. 32.

    Rimsza, J. M. & Du, J. C. Interfacial structure and evolution of the water-silica gel system by reactive force-field-based molecular dynamics simulations. J. Phys. Chem. C 121, 11534–11543 (2017).

    Article  CAS  Google Scholar 

  33. 33.

    Cailleteau, C., Devreux, F., Spalla, O., Angeli, F. & Gin, S. Why do certain glasses with a high dissolution rate undergo a low degree of corrosion? J. Phys. Chem. C 115, 5846–5855 (2011).

    Article  CAS  Google Scholar 

  34. 34.

    Jollivet, P. et al. Investigation of gel porosity clogging during glass leaching. J. Non-Cryst. Solids 354, 4952–4958 (2008).

    ADS  Article  CAS  Google Scholar 

  35. 35.

    Gin, S. et al. The fate of silicon during glass corrosion under alkaline conditions: a mechanistic and kinetic study with the International Simple Glass. Geochim. Cosmochim. Acta 151, 68–85 (2015).

    ADS  Article  CAS  Google Scholar 

  36. 36.

    Plimpton, S. LAMMPS website. http://lammps.sandia.gov/ (2003).

  37. 37.

    Rimsza, J. M., Yeon, J., van Duin, A. C. T. & Du, J. C. Water interactions with nanoporous silica: comparison of ReaxFF and ab initio based molecular dynamics simulations. J. Phys. Chem. C 120, 24803–24816 (2016).

    Article  CAS  Google Scholar 

  38. 38.

    Smart, O. S., Goodfellow, J. M. & Wallace, B. A. The pore dimensions of gramicidin-A. Biophys. J. 65, 2455–2460 (1993).

    Article  PubMed  PubMed Central  CAS  Google Scholar 

  39. 39.

    Iacovino, K. Glass density Calc. v3.2. www.kaylaiacovino.com/tools-for-petrologists (2017).

Download references


This work was supported as part of the Center for Performance and Design of Nuclear Waste Forms and Containers, an Energy Frontier Research Center funded by the U.S. Department of Energy, Office of Science, and Basic Energy Sciences under Award # DE-SC0016584. The authors are grateful to Géraldine Parisot for technical support.

Author information




S.G. led the study and wrote the paper, M.C., P.J., and M.F. ran the experiments, L.D. conducted the ToF-SIMS analyses, T.M. and J.D. performed the MD simulations, and S.K. and Y.M. developed the diffusion model.

Corresponding author

Correspondence to Stéphane Gin.

Ethics declarations

Competing interests

The authors declare that they have no competing interests.

Additional information

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

Electronic supplementary material

Rights and permissions

Open Access This article is licensed under a Creative Commons Attribution 4.0 International License, which permits use, sharing, adaptation, distribution and reproduction in any medium or format, as long as you give appropriate credit to the original author(s) and the source, provide a link to the Creative Commons license, and indicate if changes were made. The images or other third party material in this article are included in the article’s Creative Commons license, unless indicated otherwise in a credit line to the material. If material is not included in the article’s Creative Commons license and your intended use is not permitted by statutory regulation or exceeds the permitted use, you will need to obtain permission directly from the copyright holder. To view a copy of this license, visit http://creativecommons.org/licenses/by/4.0/.

Reprints and Permissions

About this article

Verify currency and authenticity via CrossMark

Cite this article

Gin, S., Collin, M., Jollivet, P. et al. Dynamics of self-reorganization explains passivation of silicate glasses. Nat Commun 9, 2169 (2018). https://doi.org/10.1038/s41467-018-04511-2

Download citation


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.


Nature Briefing

Sign up for the Nature Briefing newsletter — what matters in science, free to your inbox daily.

Get the most important science stories of the day, free in your inbox. Sign up for Nature Briefing