The synthesis of clay minerals has been studied for decades in an attempt to better understand their formation in natural environments and more recently to obtain clay minerals with controlled compositions and properties. Even though nontronite has been synthesized successfully since 1935, the process is not a straightforward and has been poorly documented. In the present review concerning the synthesis of nontronite and other Fe-rich smectites, the experiments attempted in the past are discussed critically in light of the most recent data. Most notably, the application of relationships established recently, thanks to synthetic smectitic series, have allowed us to refine the chemical compositions of some nontronites synthesized previously.

Smectites are common clay minerals occurring in various types of soils and sediments (e.g.Wilson, 2013). Smectites are relatively important among clay minerals because of their large specific surface areas (due to their small particles size, generally <1 µm) and ion-exchange properties. These specific physical and chemical properties make them unique and lead to a great variety of applications (Zhou, 2010).

Smectites are found the world over, but they occur only rarely as large, mono-mineralic deposits with homogeneous chemical compositions. Mineral syntheses in the laboratory have been performed to obtain clay minerals with controlled compositions and properties (see reviews by Kloprogge et al., 1999; Zhang et al., 2010). For smectites, most such syntheses were devoted to trioctahedral and Al-rich smectites (Kloprogge et al., 1999; Zhang et al., 2010). The present study is devoted exclusively to the synthesis of nontronite and other Fe-rich smectites. Natural Fe-rich smectites are generally neoformed authigenic clays occurring in various environments: weathered rocks and soils, oceanic sediments and hydrothermal deposits (see an extended review of smectite paragenesis by Wilson, 2013). The formation temperatures of these natural smectites range between 2–3°C for authigenic nontronites in deep-sea sediments and ∼150°C for hydrothermal deposits (Wilson, 2013). Nontronite can also form from late-stage magmatic, granitic fluids at higher temperatures than those of hydrothermal origin (Oyawoye & Hirst, 1964). Similarly, Meunier et al. (2008) described post-magmatic nontronites formed when the residual liquids are concentrated in the diktytaxitic voids of basaltic rocks. The interest in Fe-smectites was recently reinforced by their widespread detection on the surface of Mars (Poulet et al., 2005; Mustard et al., 2008; Carter et al., 2013, 2015) and generated discussion concerning their origin (Wray et al., 2009; Milliken & Bish, 2010; Meunier et al., 2012; Carter et al., 2013; Ehlmann et al., 2013; Berger et al., 2014; Mangold et al., 2016). In natural Fe-rich smectites, Si, Al3+ and to a lesser degree Fe3+, occupy tetrahedral sites, while Mg2+, Fe2+, Fe3+ and Al3+ commonly occupy octahedral sites. Heterovalent substitutions create a negative charge (tetrahedral charge due to R3+ for Si tetrahedral substitutions, and octahedral charge due to R2+ for R3+ octahedral substitutions). Due to the great variability in their chemical composition, the structural formulae of smectites range between those of dioctahedral [4(Si4–xR3+x)6(R3+2–yR2+y)O10(OH)2M+x+y] and trioctahedral [4(Si4–xR3+x) 6(R2+3–yR3+y)O10(OH)2M+x–y]. The most common smectite end-members are montmorillonite [4(Si4)6(Al2−yMg-R2+y)O10(OH)2M+y], beidellite [4(Si4–xAlx)6(Al-R3+)2O10(OH)2M+x], nontronite [4(Si4–x (Al-Fe3+)x6((Fe3+-Al)2–y (Fe2+-Mg)y))O10(OH)2M+x+y], and saponite [4(Si4–xAlx)6(Mg-Fe2+)3O10(OH)2M+x+y], where M+ is an exchangeable interlayer cation and 4( ) and 6( ) refer to tetrahedral and octahedral sites, respectively (Brigatti et al., 2013). Many natural Fe3+- rich smectites are generally intermediate between tetrahedrally charged smectites (beidellite – nontronite series : 4(Si4−x(Al-Fe3+))6(Al,Fe3+)2O10(OH)2M+x), and octahedrally charged smectites (montmorillonite and Fe3+-montmorillonite series : 4(Si4) 6((Al-Fe3+)2−yR2+y) O10(OH)2M+y) (R2+ being Mg or Fe). Natural Fe2+-rich smectites are generally saponites: 4(Si4−xAlx)6(R2+3)O10(OH)2M+x, (R2+ being Mg and Fe). Numerous theoretical Fe-smectitic end-members can be thus defined, such as 4(Si4–xFe3+x)6(Al2) O10 (OH)2M+x (only theoretical, see below), 4(Si4–xAlx)6(Fe3+2)O10 (OH)2M+x (nontronite), 4(Si4–xFe3+x) 6(Fe3+2)O10(OH)2M+x (ferric nontronite), 4(Si4)6(Fe3+2–x Mgx)O10(OH)2M+x (ferric montmorillonite), 4(Si4–x Fe3+x) 6(Mg3)O10(OH)2M+x, (ferric saponite), 4(Si4–x Alx)6(Fe2+3)O10(OH)2M+x (ferrous saponite), etc. Numerous questions arise when establishing the structural formulae for natural Fe-rich smectites: what is the extent of substitution of the main octahedral cations Al, Fe and Mg? How are Al3+ and Fe3+ distributed between the octahedral and tetrahedral sites, and, in particular, what is the amount of tetrahedral Fe? Infrared (IR) and Mössbauer spectroscopy, among other techniques, is often used to constrain the structural formulae of natural clay minerals (e.g.Goodman et al., 1976; Bonnin et al., 1985; Cardile & Johnston, 1985; Slonimskaya et al., 1986; Madejová et al., 1994; Gaudin et al., 2004a, 2004b; Gates, 2005; Cashion et al., 2008; Kaufhold et al., 2017). However, interpretation of spectroscopic features is generally not unambiguous.

Mineral synthesis in the laboratory was of interest in preparing Fe-rich smectites with unique crystal-chemistry:

  1. for better interpretation of their spectroscopic features (see Andrieux & Petit, 2010; Petit et al. 2015, 2016; Baron et al., 2016a), for IR spectroscopy in both the mid- and near-IR regions, and, for Mössbauer spectroscopy (Baron et al., 2017).

  2. to better constrain the conditions of formation of smectite, e.g. the synthesis temperature of nontronite was given as 340°C (Ewell & Insley, 1935), 200°C (Hamilton & Furtwängler, 1951), 90–100°C (Tomita et al., 1993) and 3–20°C (Harder, 1976), revealing the wide temperature range suitable for nontronite formation. Farmer et al. (1991, 1994) and Farmer (1997) suggested that the widespread occurrence of ferruginous beidellites in Vertisols under Mediterranean and subtropical climates was linked to the presence of ferrous Fe, cyclic oxidizing and reducing conditions and alkaline pH (Farmer et al. 1991, 1994; Farmer, 1997). Thus, to understand better the formation of Fe-beidellite in Vertisols, Farmer et al. (1991, 1994) and Farmer (1997) performed syntheses of Al-Fe-Mg smectites at temperatures of 23–95°C.

  3. to obtain materials of interest for many applications such as in catalysis (e.g.Zen et al., 1996; Liu et al., 2014; Li et al., 2015), degradation or retention of organic compounds (e.g.Gupta et al., 2006; Hofstetter et al., 2006; Neumann et al., 2009), reduction of mobility of heavy metals (e.g.Jaisi et al., 2009; Yang et al., 2012; Ilgen et al., 2012), liquid crystals (e.g.Michot et al., 2008, 2009, 2013; Paineau et al., 2013; MacGregor-Ramiasa et al., 2015) or potentially for geological disposal of high-level nuclear waste (Nagase et al., 1999).


Ewell & Insley (1935) were the first to report the synthesis of nontronite (Table 1) along with kaolinite and beidellite, to better understand the conditions of formation of natural clay minerals. The synthesis was performed from an Fe2O3-2SiO2 starting gel obtained from solutions (2 FeCl3 + 2SiNa2O3 + NaOH 10%). The gel was washed and aged at 340°C for 6 days. Some nontronite, identified by X-ray diffraction (XRD) camera films from powdered samples, mixed with hematite and a hydrous Fe silicate (not studied) were obtained. After removing hematite, the chemistry of the nontronite-hydrous Fe silicate (50% each) mixture, established by chemical analysis, was: 4(Si3.8Fe0.2)6Fe2 (ferric nontronite). The Fe hydrous silicate probably had a greater Si/Fe ratio than that of nontronite. The same ageing from a mixture of Fe2O3 and SiO2 gels yielded hematite and cristobalite instead of nontronite.

Hamilton & Furtwängler (1951) used a starting gel with a SiO2/Fe2O3/Na2O ratio of 4/1/0.25. 0.25 g of gel was aged for 24 h at temperatures between 175 and 350°C, in 3 cm3 of water. The most favourable temperature was 200°C. The structural formula of the ferric nontronite synthesized, determined using XRD, differential thermal analysis (DTA) and chemical analyses, was Si4Fe1.78O10(OH)2Na0.33, not balanced but clearly in accordance with the chemical composition of ferric nontronite. Caillère et al. (1953, 1955) performed syntheses of Fe-rich smectites by adding droplets (one drop per 20 s) of diluted solutions of Si(OH)4 (<10 mg L−1), Mg, Fe2+, and Fe3+ chlorides (10–50 mg L−1) to boiling water at pH fixed between 8.5 and 9.5 by addition of small quantities of acid or base. After ∼1 month, 25–125 mg of solids was obtained. From XRD, DTA and chemical analyses, the synthesized smectites were classified as “saponites” by the authors, and had ∼0.4–0.6 tetrahedral Fe3+, with the octahedral sheet containing 1.0 Fe3+, 1.1 Mg and 0.16 Fe2+ atoms per half unit cell (phuc). Syntheses performed at pH = 7–7.5 produced expanding chlorites. When Al was added, synthesis performed at pH = 8–9 produced a smectite with the following composition: 4(Si3.33Al0.15Fe3+0.52)6(Fe3+2.06Mg0.21), with some Mg possibly being exchangeable.

Koop & Harris (1967) obtained nontronite and aegirine (a Na-clinopyroxene, NaFeSi2O6) as by products when studying the synthesis of grunerite (Fe2+-amphibole). Syntheses were performed for 82–92 days in a furnace inducing a thermal gradient into the autoclave (425–400°C at the base; 395–365°C at the top), the pressure being 1.6 kbar and the pO2 greater than that of the magnetite-quartz-fayalite buffer. Silica came from chips of quartz and iron from the autoclave liner, the solution being 0.1 N NaOH. Aegirine and nontronite were identified using XRD, at the base and at the top of the autoclave, respectively.

Harder (1976, 1978) studied the synthesis of Fe3+-clay minerals from ferrous amorphous gels. Very dilute solutions of monomeric silica (near 20 ppm SiO2) and FeSO4 (0.3–20 ppm Fe) and sometimes Al (0.3–2 ppm Al) and/or Mg (300–1200 ppm Mg) were used. Reducing conditions were obtained by the addition of 0.03, 0.1 and 0.3% of Na-dithionate. Amorphous starting hydroxide-silica precipitates were obtained by an increase in the pH of starting solutions, or by a change in Eh. Syntheses were performed at 3–20°C for 3–30 days. The pH was fixed between 8 and 8.5 by NaOH. Successful syntheses of Fe clays were obtained for reducing conditions only. Trioctahedral TO clays were synthesized from starting solutions having a low Si/Fe ratio, while poorly crystallized TOT clays were obtained for high Si/Fe ratios. Nontronite (mainly dioctahedral Fe3+ smectite) and lembergite (mainly trioctahedral Fe2+ smectite) were identified on the basis of the d0¯6¯3¯3 XRD values. Chemical analyses suggested that the synthetic products were not monomineralic. Harder (1978) then concluded that the synthesis of Fe3+-nontronite was possible only if: Fe2+ cations were present in solutions, there was a high pH and Eh < 0, inducing better crystallinity of these smectites.

Decarreau & Bonnin (1986) synthesized at 75°C, a ferric nontronite from a ferrous starting gel, Si4Fe2+3O11.nH2O, with stoichiometry corresponding to trioctahedral ferrous smectite, obtained by mixing FeSO4 and SiO2Na2O solutions. The starting gel was first aged for 15 days under reducing conditions by bubbling hydrogen gas in the synthesis vessel. Only a very poorly crystallized ferrous stevensite was identified by XRD. After 15 days of spontaneous oxidation in contact with air, a strictly ferric nontronite was synthesized as was confirmed by Mössbauer spectroscopy. The chemical analyses corresponded to the following structural formula: Si4Fe3+2.95O10(OH)2Na0.05. This structural formula is probably invalid due to the amount of Fe3+ which is too great. Accordingly, from Mössbauer spectroscopy at 4 K, at the end of the synthesis, one third of Fe was located in an amorphous Fe oxide (or oxyhydroxide) phase. This amorphous Fe oxide was linked intimately to nontronite layers and was issued from the oxidation reaction of the ferrous stevensite: [Fe2+3-stevensite] → [Fe3+2-nontronite] + ½ Fe2O3.

The synthesis of a ferric nontronite under oxidizing conditions was managed by Decarreau et al. (1987) using a ferric starting gel with stoichiometry corresponding to a dioctahedral smectite: 4(Si4)6(Fe3+2)O11. This gel was obtained from sodium-silicate and ferric sulfate solutions. Syntheses were performed for 1 month at 75 and 100°C and for 12 days at 150°C. The XRD and X-ray absorption fine structure (EXAFS) data showed that the synthetic product obtained at 75°C looked like germs with dioctahedral TOT structure. At 100 and 150°C, ferric nontronites were obtained. The structural formula, determined from chemical analyses of the synthetic product, was 4(Si4)6(Fe3+1.83)O10(OH)2Ca0.26. This structural formula probably does not actually correspond to the nontronite synthesized, and the presence of an excess of silica was suggested. From the increase in the crystallinity of nontronites vs. the synthesis temperature, the time necessary to obtain nontronite was evaluated to be of the order of 10 y at 25°C and 200 y at 2°C.

Mizutani et al. (1991) synthesized Fe nontronites from suspensions obtained by adding to a SiNa2O3-FeSO4 solution (Fe/Si = 0.75 and 1.5), a NaOH 5 M solution and 10 g L−1 of Na-dithionite. Syntheses were performed at 150 and 200°C for 50 h. At 150°C, and with a Si/Fe ratio of 0.75, the nontronite obtained was pure and well crystallized, but still contained 3.5% of Fe2+ detected by Mössbauer spectroscopy.

Tomita et al. (1993) showed that smectites may form by reaction of volcanic glass with NaOH, under 1 atm. pressure at 90–100°C. Experiments were carried out for 3–10 days, using various glass/NaOH ratios. An Fe-Al-Mg beidellite (Fe/Al = 0.7, Mg/Al = 0.5) was synthesized for a low glass/NaOH ratio, while zeolites or zeolite-smectite mixtures were formed in other cases. The beidellite synthesized was not well crystallized, regardless of the time of the experiments. A b crystallographic parameter of 9.2 Å was measured from dotted electron diffraction patterns, suggesting an ordered stacking of beidellite layers.

Farmer et al. (1991, 1994) performed experiments from 23 to 95°C for 4–13 weeks. The pH was near 8–8.5 using a Ca(OH)2-CaCO3 buffer. The starting materials were obtained mixing various amounts of Si(OH)4, AlCl3, FeCl2 and (MgCl2 + KCl) solutions. Initial reducing conditions were obtained by addition of hydrazine, and oxidation occurred during syntheses by air diffusion. For syntheses performed at 23°C, Mg-free allophanes were identified by XRD and IR data. At 89°C allophane formed from the (Fe-Mg)-free starting product. Smectites were obtained from the initial products having Fe/Al ratios >1 and when the amount of Si in solution was >280 µmole L−1. The synthesized smectite particles containing Mg, obtained in Ca + K solutions, exhibited randomly stacked layers. For the experiments without Mg, Al-Fe smectites were synthesized with layer stacking which depended on the cations occurring in solution: ordered for Ca and random for Na or K. Farmer (1997) carried out similar syntheses, without Mg, but using successive redox cycles for 10–13 weeks: reduction by adding large amounts of hydrazine, followed by oxidation for ∼15 days due to air diffusion. Initial precipitates resembled allophanes and no smectite was synthesized for starting materials with Al/Fe > 3.5. Smectites with a constant chemistry were synthesized for 2.5 < Al/Fe < 3.5; the chemical analyses suggested excess Al and Fe, said to be in the interlayer space. For a starting material with a Si/Al/Fe ratio of 15/5/2, the smectite synthesized had the following structural formula: 4(Si3.41Al0.59)6(Al1.18Fe0.82)O10(OH)2Ca0.295. Farmer et al. (1994) concluded that the main crystallization process of synthetic Al/Fe smectites occurred during or after Fe oxidation.

Grauby et al. (1994) studied the heterovalent octahedral Fe3+/Mg substitution via the hydrothermal synthesis at 200°C of a smectite series from starting gels having the 4(Si4)6(Fe3+(2–2x/3)Mgx)O11 theoretical stoichiometry, with x varying from 0 to 3. The starting gels were obtained from sodium metasilicate and Mg and Fe3+ chlorides. After combining XRD, IR, Mössbauer and transmission/analytical electron microscopy (TEM-AEM) data, those authors showed that the Fe-smectites synthesized had a small tetrahedral charge increasing from 0 to 0.17 e/huc when 6Fe3+ increased from 0.3 to 1.88 while the 6Mg increased from 0.08 to 2.43 (for O10(OH)2). The b crystallographic parameter was correlated linearly to the amounts of 6Mg or 6Fe, following Vegard's law (Table 2). The simultaneous occurrence in IR spectra of bands due to 3Mg-OH, Mg2+Fe3+-OH and 2Fe3+-OH stretching vibrations proved the segregation of 6Mg and 6Fe3+ cations in trioctahedral and dioctahedral local environments, respectively, within each smectite layer.

Using the procedure of Decarreau & Bonnin (1986), i.e. preparing the starting material under anaerobic conditions and oxidation occurring during synthesis by air diffusion into the reactors, Lajarige et al. (1998) synthesized Al-Fe beidellites in which some Fe remained as Fe2+. Those authors performed two syntheses at 200°C for 41 days using the same starting gel with the following stoichiometry: Si4Al1.33FeO11. According to XRD, IR and Mössbauer data, two different Al-Fe beidellites were obtained: 4(Si3.7Al0.3)6(Al1Fe3+0.97Fe2+0.03)O10(OH)2Na0.33 and 4(Si3.74Al0.26)6(Al1.06Fe3+0.8Fe2+0.2)O10(OH)2Na0.33.

Nagase et al. (1999) synthesized Fe-smectites at 100 and 200°C for 24 h from hydrous oxides obtained by mixing acidic sodium silicate, FeCl3 and MgCl2 solutions, precipitated at pH = 9.9 (pH adjusted using NaOH). Smectites were identified by XRD for a narrow pH range only between 12.0 and 12.4. When the pH was <12, an amorphous phase was detected and when the pH was >13 a mixture of aegirine and hematite was produced. From TEM-energy dispersive X-ray spectroscopy (EDS) data, the Si/Fe/Mg ratio of clay particles was 4/1.65/0.3.

Decarreau et al. (2008) synthesized hydrothermally (75–150°C, 4 weeks) high-charge ferric nontronite, and characterized accurately for the first time the ferric end-member of nontronite using XRD, IR, Mössbauer and X-ray absorption near-edge spectroscopy (XANES) data. The synthesis was performed from a silico-ferrous starting gel, Si2FeNa2O6.nH2O, produced by mixing sodium metasilicate and ferrous chloride solutions. The pH was adjusted to 12.5 by NaOH. Regardless of the synthesis temperature, the nontronite synthesized had the same structural formula: 4(Si3.25Fe3+0.75)6Fe3+2O10(OH)2Na+075. The crystallinity of these nontronites increased with synthesis temperature, and their expandability moved from smectite to vermiculite-like behaviour. Aegirine, mixed with a poorly crystallized ferric nontronite, was synthesized at 200°C using the same starting gel at pH from 10 to 12 (Decarreau et al., 2004).

Andrieux & Petit (2010) were the first to synthesize Al-Fe3+ smectites within a wide compositional range, without Mg, following the 4(Si4–x(Fe3+-Al)x)6(Fe3+2–yAly)O10(OH)2Nax structural formula. These Al-Fe3+ smectites were characterized carefully by coupling XRD, IR and TEM-EDS data (Petit et al., 2015). The tetrahedral charge (x) ranged from 0.3 to 0.5 e/huc (0.75 for the ferric end-member) and occurred essentially by means of Al-for-Si substitutions, with tetrahedral Fe3+ being ∼0.1 for most of the Fe-rich Al-Fe3+ smectites. The octahedral Al (y) ranged from 0 to 1.88. The windows of experimental conditions to crystallize such smectites are narrow. Temperatures up to 150°C and high pH (∼12) are suitable for the formation of the Fe3+-rich smectites (nontronite), while higher temperatures (200°C) and lower pH (down to 7) are suitable for the most Al-rich smectites (Fe3+-beidellites). For intermediate compositions, both the pH and temperature of synthesis should be adjusted in parallel to favour crystallization of pure smectite. Outside these windows, admixtures or other phases were obtained.

Baldermann et al. (2014) synthesized Mg-Fe2+ saponites under reducing conditions (0.05 mass% of Na dithionite) at 120 and 180°C, over periods of 2, 5 and 7 days, the final pH being near 12.6. Initial precipitates were obtained from solutions of Na orthosilicate (Na4SiO4), Fe (II) sulfate (FeSO4·6H2O) and Mg chloride salts (MgCl2·6H2O) with molar Si:Fe:Mg ratios of 4:0:2, 4:1:1, 4:1.5:0.5, 4:1.75:0.25, and 4:1.82:0.18. The initial pH was adjusted to 8.5 with NaOH. The smectites synthesized were characterized by XRD, FTIR and TEM-EDS. The Fe2+/Fe3+ ratios of clay particles were measured using electron energy-loss spectroscopy (EELS). The saponites synthesized were more or less mixed with by products (antigorite, nontronite, brucite, ferrihydrite, opal CT). The tetrahedral charge of the saponites synthesized, arising from Si for Fe3+ substitutions, was between 0.03 and 0.26 electrons (for O10(OH)2), and the octahedral sheet always contained Mg, Fe2+ and Fe3+ cations, the 6(Fe2+/Fe3+) ratio being ∼10. Baldermann et al. (2014) suggested that a complete octahedral substitution may exist in ferrous saponites between Mg and (Fe2+ + Fe3+) cations. Surprisingly, IR spectra of the synthesized saponites exhibited mainly dioctahedral Fe3+-OH-Fe3+ features, probably due to possible oxidation of the samples.

Petit et al. (2016) synthesized a series of Fe3+-Ga3+ smectites in order to study the IR spectral features of these smectites. Syntheses were performed at 180°C for 18 days from starting gels using Fe3+ and Ga nitrates and Na metasilicate. Six smectites were synthesized with intermediate chemistries ranging from the Ga to the Fe end-members. The layer charge, due to Si-Ga substitution only, decreased from 0.76 to 0.52 electrons per O10(OH)2 when the amount of octahedral Fe3+ increased. Tetrahedral Fe3+ occurred for the nontronite ferric end-member only, and was 0.45 electrons per O10(OH)2.

Studying the improvement in the process of Decarreau et al. (2008), Baron (2016) successfully synthesized nontronites from starting gels prepared using FeCl2, FeSO4, or FeCl3 salts. The size of the nontronite particles was more homogeneous when hydrated gels rather than dehydrated powders were used as the starting materials (Fig. 1). Baron (2016) also synthesized hydrothermally nontronite using a microwave furnace. For conditions of 150°C over 6 days, no difference in the yield or in the crystal chemistry of the nontronites synthesized could be detected between microwave and classical furnace experiments as observed by Baron et al. (2016b) for trioctahedral Ni-Mg 1:1 (nepouite–lizardite) or 2:1 (pimelite–kerolite) synthetic series (220°C – 2 days). The microwave hydrothermal synthesis method is of more interest though, because it is easier to increase the reactor capacity and maintain uniform heating.

Baron et al. (2016a) were able to synthesize at 150°C a chemical series of strictly ferric nontronites with various tetrahedral charges across a range of initial aqueous pH values between 11 and 14 obtained by addition of NaOH. This series was characterized accurately using XRD, IR and TEM-EDS analyses. The permanent layer charge of synthetic nontronites, due to Fe3+-for-Si tetrahedral substitutions only, ranged from 0.43 to as high as 1.54 per O10(OH)2. Despite the unusual values of the layer charge, synthetic Ca-saturated nontronite layers showed expansion after ethylene glycol solvation. The increase in tetrahedral Fe3+ was correlated with the increase in the end-of-synthesis pH measured at 25°C (Baron et al., 2016a). The same trend was observed with the data recalculated for 150°C (Fig. 2). High pH values induced a strong increase in SiO2 in solution via anionic aqueous Si species ratios (i.e. H3SiO4(aq) and H2SiO42−(aq)), favouring the incorporation of Fe3+ in the tetrahedral sites of synthetic nontronites.


Thanks to recent syntheses of ferric nontronites and Al-Fe3+ and Ga-Fe3+ smectites, chemical series of Fe-rich smectites exhibiting large and continuous chemical variations were available (Andrieux & Petit, 2010; Baron et al., 2016a; Petit et al., 2016). Careful characterization of these synthetic smectites allowed us to establish robust correlations between XRD and IR data, and crystal-chemistry (Table 2). Petit et al. (2015) and Baron et al. (2016a) showed that the b lattice parameters measured by XRD, and the positions of FTIR bands, are linearly correlated with the amounts of octahedral and tetrahedral Al and Fe in the synthetic smectite (Table 2). In light of these relations, when XRD and/or spectroscopic data are available in the literature, the structural formulae for all synthetic Fe-rich smectite can be determined (or reconsidered). As an example, for the Decarreau & Bonnin (1986) ferric nontronites obtained in partly reducing conditions, both the XRD and IR independent data are consistent and led to small values for tetrahedral Fe3+ (0.13 and 0.17 atoms per O10 (OH)2, respectively) (Table 1). Decarreau et al. (1986) were aware that the layer charge of the synthetic nontronites was particularly low, but they hypothesized that it was due to the occurrence of empty octahedral sites.

Farmer et al. (1991) synthesized smectites from starting gels with various Si/Al/Fe/Mg ratios. Using the available IR data and the relationships determined from chemical series (Table 2), the amounts of 4Fe3+ and/or 6Fe3+ in the synthetic smectites (for which no structural formulae were given) could be determined. For the 6/2/2/0 and 6/2/4/0 gels, the 6Fe3+ value was between 1.2 and 1.5 atoms (per O 10(OH) 2) and for the 6/0/4/0 gel, the 4Fe3+ value was 0.73, remarkably close to the 0.75 of the nontronite synthesized by Decarreau et al. (2008) under similar conditions.

Using the synthetic nontronite series with various tetrahedral charges described above (Baron et al., 2016a), Baron et al. (2017) refined Mössbauer parameters (isomer shifts (δ) and quadrupoles splitting (Δ)) for tetrahedral and octahedral Fe3+ at ambient temperature and 77 K, using the ratio of the four possible local tetrahedral cationic environments around an octahedral Fe3+ (i.e. 4Si, 3Si-Fe3+, 2Si-2Fe3+). The Mössbauer spectra at ambient temperature and 95 K of a synthetic ferric nontronite given by Mizutani et al. (1991) were decomposed using the Baron et al. (2017) method (Fig. 3). A 4Fe3+ value of 0.7 atoms (per O10 (OH) 2) was found. This value appears consistent with the synthesis conditions and all of the available data described by Mizutani et al. (1991).


Smectite end-members are rarely found in nature and this is the case for ferric nontronite and Al-beidellite end-members 4(Si4 –xR3+x)6(R3+)2O10(OH)2M+x,R3+ being exclusively Fe or Al, respectively. The Al-beidellite end-member has been synthesized many times in the past (e.g. Kloprogge et al., 1999; Zhang et al., 2010), but always with a rather small tetrahedral charge value (x) and without focus on the tailoring of the charge. The ferric nontronite end-member was synthesized with a wide range of tetrahedral charges (x) per O10(OH)2: x = 0.2–0.3 in Ewell & Insley (1935) and Decarreau et al. (1986, 1987); x = 0.7 in Hamilton & Furtwängler (1951), Farmer et al. (1991), Mizutani et al. (1991) and Decarreau et al. (2008), and x varying from 0.43 to 1.54 in Baron et al. (2016a). The latter authors demonstrated that the amount of 4Fe3+ in synthetic nontronites is pH dependent. The various tetrahedral charges for synthetic nontronites reported in the literature, when the values are robust, are probably due to the pH conditions of the synthesis.

The Fe3+ substitutes easily for Si in tetrahedral sites when it is the only M3+ cation used for synthesis (Table 1). When competition exists between Al and Fe3+, Al occurs predominantly in tetrahedral sites and Fe3+ appears only when the Fe3+/Al ratio is very high (Table 1). Indeed, Decarreau & Petit (2014) showed that the distribution of Al3+ and Fe3+ between octahedral and tetrahedral sites of dioctahedral smectites is controlled by a partition coefficient, Kd:  
which had a very small value (<0.02) for smectites synthesized at 200°C. Consequently, the nontronite end-member 4(Si4–xAlx)6(Fe3+)2O10(OH)2M+x is theoretical because some tetrahedral Fe necessarily exists for this Fe-rich smectite, although 4Fe3+ would be very difficult to detect for Fe3+/(Fe3++Al) ratios of <0.6 (Decarreau & Petit, 2014). For the same reason the 4Fe3+-beidellite end-member 4(Si4–xFe3+x)6(Al)2O10(OH)2M+x is theoretical.




Grauby et al. (1994) showed that a continuous octahedral solid solution exists between the ferric nontronite (4(Si4–xFe3+x)6Fe3+2O10(OH)2M+x) and ferric saponite (4(Si4–xFe3+x)6(Mg3)O10(OH)2M+x) end-members, with no chemical gap, unlike that which was suggested by Weaver & Pollard (1973) from the chemistry of natural smectites. This solid solution series implies a mixing of local di- and trioctahedral sites occupancies forming small domains within layers which were revealed accordingly by FTIR spectroscopy through OH-stretching bands due to the occurrence of Mg and Fe3+ neighbouring octahedral cations (see above).  
Baldermann et al. (2014) proposed the possibility of a complete octahedral substitution rate between Mg and (Fe3+ + Fe2+) in saponites. The Mg- and Fe-richest saponite end-members synthesized by Baldermann et al. (2014) had (Mg2.3Fe2+0.42Fe3+0.04) and (Mg0.26Fe2+2.26Fe3+0.21) octahedral compositions, respectively.  
Although many syntheses of Fe smectites were performed under partly reducing conditions, the occurrence of some octahedral Fe2+, generally measured using Mössbauer spectroscopy, has rarely been reported (Mizutani et al., 1991; Lajarige et al., 1998). The composition of the octahedral sheet was reported by Mizutani et al. (1991) to be 6(Fe3+1.9Fe2+0.1) and by Lajarige et al. (1998) to be 6(Al1.06Fe3+0.8Fe2+0.2). Only a small 6Fe2+6Fe3+ range was then explored experimentally, probably because it is difficult to prevent the oxidation of Fe during experiments or even after syntheses (Baldermann et al., 2014).  

In the ternary Fe3+/Al/Mg diagram of Güven (1988), a large chemical gap between beidellite and nontronite was suggested for natural dioctahedral smectites. These natural dioctahedral smectites very often contain Mg (Gates, 2005) and the octahedral Al-Fe3+ solid solution is complete only as long as Mg is present in the system (Gaudin et al., 2004a,b). Andrieux & Petit (2010) and Petit et al. (2015) showed that a complete Al-Fe3+ octahedral solid solution does exist along the join Al (beidellite)–Fe3+ (nontronite) [4(Si4–x(Al-Fe3+)x)6(Al-Fe3+)2O10(OH)2M+x], with no Mg. Similarly, Ga3+ can substitute easily for Fe3+ in the octahedral sheet of dioctahedral smectites forming a complete solid solution (Petit et al., 2016). Moreover, for these two binary Al-Fe3+ and Ga-Fe3+ smectitic solid solutions, combination bands in IR spectra (Fig. 4) revealed that octahedral cations are always distributed randomly (see Petit et al. (2015) and Petit et al. (2016), for Al-Fe3+ and Ga-Fe3+, respectively).


Nontronites and Fe3+-beidellites were synthesized over a wide range of temperatures (3 < T < 350°C), generally within few days (Table 1). For a given synthesis time, an increase in synthesis temperature leads to an increase in the crystal order of the smectites (Decarreau et al., 2008). The transformation rate of starting materials (mainly co-precipitated gels) is time- and temperature-dependent and, for low-temperature syntheses, amorphous and/or unreacted products were observed for short synthesis times (Harder, 1976, 1978; Farmer et al., 1991).

Many syntheses used starting gels containing Fe2+ or Mg cations, partly on the basis of previous results showing that it was easy to synthesize trioctahedral M2+-smectites (Strese & Hofmann, 1941). But syntheses of Fe smectites were also performed successfully under strictly oxidizing conditions and without Mg (Table 1). Nevertheless the kinetics of synthesis seems to be greater when the starting gel contains Fe2+: a relatively well crystallized ferric nontronite was synthesized at 75°C over 15 days from a ferrous gel (Decarreau et al., 1986) while with a ferric gel, at the same temperature, only the beginning of crystallization of a ferric nontronite was observed after 1 month of synthesis (Decarreau et al., 1987). However, the pH was not the same and the two experiments were not directly comparable.

When ferrous starting gels were used, generally, smectites synthesized in oxidizing conditions contained only ferric iron (Table 1). Under partial anaerobic conditions, Fe2+ cations might remain in synthesized smectites and the oxidation process is rather slow (Mizutani et al., 1991; Lajarige et al., 1998). These results suggest that the occurrence of Fe2+ in natural smectites does not necessary result from a long exposure time under reducing conditions.


In the Si, Fe3+, Na, H2O system, three silicate minerals may form: ferripyrophyllite, ferric nontronite and aegirine. True ferripyrophyllite has never been synthesized (Lantenois et al., 2007), while Grauby (1993) synthesized a 2:1 ferric silicate similar to ferripyrophyllite (that author synthesized a non-swelling layered Si-Fe3+ mineral with a 9–10 Å XRD reflection). Aegirine is a common by-product of nontronite syntheses (Kopp, 1967; Nagase et al., 1999; Baron, 2016). Baron (2016) studied the evolution at 150°C of a starting gel with a Si2FeNa2O6 composition at pH 12 and 13.3 from 1–183 days. For experiments at pH 13.3, during the first 15 days, a high-charge ferric nontronite was synthesized which disappeared progressively and was replaced by the aegirine + hematite paragenesis in long-time syntheses. In this chemical system, nontronite appears as a metastable phase, kinetically favoured, aegirine being the true stable silicate phase. In the Si, Fe3+, K, H2O system, the ferric mica appeared as the stable silicate phase, probably because the potassic equivalent to aegirine does not exist (Baron, 2016). The calcic equivalent to aegirine does not exist either. Farmer et al. (1994) and Tomita et al. (1993) observed dotted electron diffraction patterns characteristic of a 3D stacking for Fe-rich smectites synthesized with Ca available in solution: Ca(OH)2 was used as a pH buffer by Farmer et al. (1994) and Ca coming from the dissolution of the starting volcanic glass by Tomita et al. (1993). Similar syntheses performed with NaOH or KOH by Farmer et al. (1994) produced Fe-smectite particles giving electron diffraction patterns with continuous rings typical of turbostratic stacking layers as commonly observed for other synthesized smectites and for smectite in general. Unfortunately, not enough data are available, notably concerning syntheses with long duration times, to be able to evaluate the comparative ‘stability’ of the Fe-smectite synthesized vs. the interlayer cation.


Eight decades of synthesis of nontronite and other Fe-rich smectites have shown that smectite can form at rather low temperatures, typically from ambient to 200°C, under various redox conditions, from either Fe2+ or Fe3+ starting gels. The purity of the sample and the structural Fe3+ content in the smectite is controlled by pH and temperature conditions. The octahedral homovalent Al3+-Fe3+ substitution in smectites is complete and continuous, while the tetrahedral Fe3+ content depends on the Al3+/Fe3+ ratio of the smectite. Many experimental investigations are still needed to explore and fine-tune the Fe2+-Fe3+ octahedral solid solution in smectite as well as to study the possible role of organic matter in smectite crystallization and in the crystal chemistry of the smectite formed.

This review has provided evidence of the crucial importance of detailed characterization of the samples synthesized. Very often, the use of multiple analytical techniques is required. Among them, both XRD and IR spectroscopy are required at least to characterize samples in a known chemical system. Mössbauer spectroscopy is appropriate for detecting and quantifying the amounts of Fe2+, but not of tetrahedral Fe3+, in smectites. XANES offers promise as a means of measuring tetrahedral Fe3+ (Decarreau et al., 2008) and deserves to be evaluated with chemical series of synthetic nontronites with various known 4Fe3+, such as the chemical series of Baron et al. (2016a) described above.

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