Plan
Comptes Rendus
no. 6-7

Geomaterials (Mineralogy)
Iron oxides: From molecular clusters to solid. A nice example of chemical versatility
[Oxydes de fer : du complexe moléculaire au solide. Un bel exemple de versatilité chimique]

Présenté par : Written on invitation of the Editorial Board

Jean-Pierre Jolivet1  ; Elisabeth Tronc1 ; Corinne Chanéac1
1 Chimie de la matière condensée, UMR–CNRS 7574, université Pierre-et-Marie-Curie, 4, place Jussieu, 75252 Paris cedex 05, France
Comptes Rendus. Géoscience, Volume 338 (2006) no. 6-7, pp. 488-497.

Résumés

This overview features the chemical background on condensation phenomena of iron cations in aqueous solution. The formation of molecular clusters or nanosized solid phases is interpreted with illustrative mechanisms building a bridge between solution chemistry and solid-state chemistry. Iron chemistry gives a very nice example of chemical versatility.

Cette revue sur les oxydes de fer formés en solution aqueuse met en évidence les phénomènes de condensation entre complexes hydroxylés. La formation des polycations et des différentes phases solides sous forme de particules de taille nanométrique est interprétée selon des mécanismes qui permettent de comprendre comment s'effectue la condensation et, de ce point de vue, la chimie du fer offre un superbe exemple de versatilité chimique.

Métadonnées
Reçu le :
Accepté le :
Publié le :
DOI : 10.1016/j.crte.2006.04.014
Keywords: Iron oxides, Precipitation, Condensation in solution, Olation, Oxolation
Mot clés : Oxydes de fer, Précipitation, Condensation en solution, Olation, Oxolation
Jean-Pierre Jolivet 1 ; Elisabeth Tronc 1 ; Corinne Chanéac 1

1 Chimie de la matière condensée, UMR–CNRS 7574, université Pierre-et-Marie-Curie, 4, place Jussieu, 75252 Paris cedex 05, France 
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Jean-Pierre Jolivet; Elisabeth Tronc; Corinne Chanéac. Iron oxides: From molecular clusters to solid. A nice example of chemical versatility. Comptes Rendus. Géoscience, Volume 338 (2006) no. 6-7, pp. 488-497. doi : 10.1016/j.crte.2006.04.014. https://comptes-rendus.academie-sciences.fr/geoscience/articles/10.1016/j.crte.2006.04.014/

Version originale du texte intégral

1 Introduction

Iron is an important element in environment, because it is abundant in the Earth's crust. It is present in soils, essentially as oxides [9], and easily mobilized in natural waters under the form of molecular complexes and colloids. Dissolution of ferric oxides in natural conditions (including acid-base and redox phenomena, microbial mediation, and photochemistry) is of major importance in the cycling of iron [46]. Iron oxides are also present in living organisms (e.g., plants, bacteria, molluscs, birds, animals and humans). Ferrous complexes are the active centre of haemoglobin and ferredoxins, and various biomineralization processes involve ferrous and ferric species for the regulation of iron concentration in organism (ferritin) or, in various occurrences, to produce different oxides, such as goethite, lepidocrocite, magnetite and green rusts. Goethite, lepidocrocite and magnetite are the mains constituents of radulas of limpets and chitons, magnetite is synthesised by magnetotactic bacteria for their guidance and orientation in various aqueous media and in sediments [32]. Of course, the iron oxides are also of high interest in various technological fields, such as metallurgy, coloured pigments, magnetic materials, catalysts... [9].

The structural chemistry of iron oxi(hydroxi)des is very rich, as shown by the large number of structural types for ferrous, ferric and mixed-valent compounds that exist (Fig. 1) [9,58]. Almost all these phases can be formed from solutions giving rise to a puzzling chemistry [9,20,34], and because of the great diversity of physicochemical conditions in the environment (acidity, redox conditions, bacterial activity, temperature, salinity, presence of organic or inorganic ligands...), practically all the iron oxide phases can be found in the natural environment. The high versatility of iron chemistry in aqueous medium comes essentially from two factors: the occurrence of two oxidation states, stable on a large range of acidity, and the high reactivity of iron complexes towards acid-base and condensation phenomena.

Fig. 1

The different phases of iron oxyhydroxides formed as a function of hydroxylation ratio and the composition in the ferrous–ferric system.

Représentation des différentes phases des oxyhydroxydes de fer formés en fonction du taux d'hydroxylation et de la composition dans le système ferreux–ferrique.

We present the main aspects of iron chemistry in aqueous medium involving condensation phenomena and leading to the formation of clusters or nanoparticles. The main factors orienting the crystallization process of ferrous, ferric and mixed-valent solids are examined.

2 Hydroxylation and condensation mechanisms in aqueous solution

Like many transition elements in water, the iron cations form hexacoordinated aquo complexes, [Fe(OH2)6]z+, in which the polarization of coordinated water molecules is strongly dependent on the formal charge (oxidation state) and size of the cation. This makes the ferric aquo complexes strongly more acidic than ferrous complexes; therefore hydroxylation of the cations occurs on very distinct ranges of pH: hydroxylation of Fe(II) cation occurs at room temperature around pH 7–9 while it ranges from pH 1 to pH 4–5 for Fe(III) cation [2].

Hydroxylated complexes are not stable as ‘monomeric’ species in solution; they condense via two basic mechanisms, depending on the nature of the coordination sphere of the cations [20]. In all cases, condensation involves a substitution mechanism induced by the nucleophilic character of hydroxo ligand. For aquohydroxo complexes, [M(OH)h(OH2)6−h](z−h)+, condensation proceeds by elimination of a water molecule and formation of hydroxo bridges (olation mechanism):

Because of the high lability of coordinated water molecules, olation is more often a very fast reaction. For oxohydroxo complexes, [MOa(OH)b](z−2a−b)+, there is no water molecule as ligand in the coordination sphere of the complexes, and therefore there is no leaving group. Condensation can only proceed in this case via a two-step associative mechanism allowing the formation of a water molecule as leaving group and leading to the formation of oxo bridges (oxolation mechanism):

The hydroxylation rate, h, of the complexes represents their functionality towards condensation and it controls the type and structure of condensed species. h is obviously a function of the pH of the medium. Its also depends on the characteristics of the cation such as size, formal charge and electronegativity. As long as h<z (z is the formal charge of the cation), condensation in solution is always limited and forms molecular polycationic species containing at maximum around twenty metal atoms. That is well exemplified for various cations, for instance Cr(III), Al(III) [20], but the formation of ferrous polycationic species is poorly documented. As for many divalent elements in solution, a compact tetrameric polycation [Fe4(OH)4(OH2)12]4+ may form above pH 6 (Fig. 2) at the first stage of hydroxylation (h=1) [2] but, to our knowledge, no structural evidence has so far been reported. In such a tetrameric polycation, the hydroxo ligands tend to be tri-coordinated, because they are weakly polarized by divalent cations and their basicity remains high. The chemistry of ferric species is extremely complicated in comparison to that of other trivalent elements (Al, Cr). Due to their high reactivity, ferric complexes condense very rapidly and it is difficult to stop the process at molecular level, i.e. polycationic species. The control of the reactivity requires the use of very strong complexing polydentate ligands able to coordinate the cation by more than one bond. Many polycationic ferric species have nicely been obtained for instance with various polycarboxylate or amino ligands [29,31,44,48]. It is interesting to observe that, at variance with chromium and aluminium polycations, ferric ions are more often bound by oxo than hydroxo brigdes. This seems to result from the higher electronegativity of iron than that of chromium and aluminium.

Fig. 2

Schematic formation of the ferrous polycation [Fe4(OH)4(OH2)12]4+ from complexes in solution.

Schéma de la formation du polycation ferreux [Fe4(OH)4(OH2)12]4+ à partir de complexes en solution.

3 Formation of solid phases

The precursor of the solid is always a zero-charge aquo hydroxo complex. One may understand the extremely different crystal chemistry of the two cations Fe(II) and Fe(III) not only from the functionality of the precursor, but also from the process involved in its formation, for instance by addition of a base or by thermolysis at temperature in the range 60–100 °C in acidic medium.

3.1 Ferrous compounds

Zero-charge ferrous complexes [Fe(OH)2(OH2)4]0 formed at pH > 6–7 under anaerobic conditions lead to the hydroxide Fe(OH)2. Like the hydroxides of many divalent elements, Fe(OH)2 has the brucite structure. It is easy to understand how this structural type is formed (Fig. 3) [20]. As there is no structural relationship between the compact tetramers (Fig. 2) and the hydroxide, the nuclei of the solid phase seems to be planar tetramers [M4(OH)8(OH2)8]0 formed by olation from neutral zero-charge dimers. Because of the bifunctionality of the precursor [Fe(OH)2(OH2)4]0, these planar tetrameric species can further condense and the growth of nuclei, always by olation, must take place rapidly in the plane and leads to the layered brucite-type structure. This example shows very well that the polycations eventually formed during the hydroxylation process are not building blocks for the solid phase. The change in acidity of the medium leads to an important change in the structure of the condensed species during the lowering of their charge. As a rule, there is no structural relationship between the solid and the polycations formed at lower hydroxylation stages.

Fig. 3

Possible pathway of the formation of ferrous hydroxide Fe(OH)2 from complexes in solution.

Chemin réactionnel possible pour la formation de l'hydroxyde ferreux Fe(OH)2 à partir de complexes en solution.

In the solid state or in aqueous suspension, the ferrous phases are very sensitive to oxidation. Various phases (green rusts, magnetite, goethite, lepidocrocite, and feroxyhyte) can be formed, depending on the conditions, as discussed below.

3.2 Ferric compounds

The behaviour of ferric species in solution exemplifies very well the complexity of their structural chemistry. Hydroxylation of ferric ions in solution by addition of base at room temperature (pH > 3) leads quasi instantaneously to 2-line ferrihydrite, a poorly defined highly hydrated phase exhibiting only two broad bands in its X-ray diffraction pattern [18,45]. Due to its poor structural organization, ferrihydrite is thermodynamically unstable. It transforms into different crystalline phases via different pathways depending on the acidity of the medium. At 5⩽pH⩽8, ferrihydrite transforms into very small particles of haematite, α-Fe2O3 [8]. The solubility of the solid being very low (around 10−10 mol l−1), the transformation can proceed only by dehydration in situ and local rearrangement. This explains the formation of an oxide and the very small size of crystalline domains. When the solubility of ferrihydrite is higher (pH < 4 or pH  > 8), the transformation can proceed more easily via a dissolution–crystallization process, leading to goethite, α-FeOOH. In contrast with aluminium, ferric hydroxide Fe(OH)3 does not exist and has never been identified. Growth of goethite by dissolution–crystallization process may be interpreted as taking place from the planar tetramer [M4(OH)12(OH2)4]0. Condensation of these species by olation can lead directly to embryos of double chains of octahedra, characteristic of the structure of goethite (Fig. 4). The chains connect by oxolation because of the relative kinetics of each reaction. Connection between the double chains occurs through tri-coordinated oxygen atoms forming μ3-O bridges, and hydrogen bonds between the chains. Complexing ligands such as silicate and especially phosphate delay or hinder the transformation of ferrihydrite into crystalline phases [12,37,40,41]. This is for instance the case in very old soils in New Zealand (200 000 years!) or in living organisms, in ferritin nanoparticles in which iron(III) is stocked.

Fig. 4

Possible pathway of the formation of goethite α-FeOOH and electron micrograph of particles. From [20].

Chemin réactionnel possible de formation de la goethite α-FeOOH et cliché de microscopie électronique des particules. D'après [20].

Haematite forms by thermolysis of acidic ferric solutions at 90–100 °C (pH ⩽ 3), [9,34]. In these conditions, oxolation is facilitated and leads to oxide [20]. Very small particles of 6-line ferrihydrite form initially at low concentration of chloride (C<10−3moll−1, ∼3 nm in diameter) [9,18,45]. This phase is better organized than 2-line ferrihydrite and transforms into haematite during thermolysis. It is interesting to observe that the size of haematite particles increases strongly when the acidity of the medium increases. The role of the acidity is to facilitate oxide crystallization and to favour the dissolution–crystallization process leading to particle growth (Fig. 5). At high concentration of chloride, akaganeite, β-FeOOH, is first formed instead of ferrihydrite [5,35]. Chloride anions are not included at stoichiometry in the channels of the structure and they seem to be the template allowing the specific organization of the goethite-like double chains of octahedrons (Fig. 1). This metastable phase is slowly transformed into haematite during thermolysis and large (micronic) polycrystalline particles with various morphologies are obtained depending on the nature of anions [3,33,47].

Fig. 5

Electron micrographs of haematite particles obtained by thermolysis at 95 °C of ferric nitrate solutions and variation of the particle size as a function of the pH of solutions. From [17].

Clichés de microscopie électronique de particules d'hématite obtenues par thermolyse à 95 °C de solutions de nitrate ferrique et variation de la taille des particules en fonction du pH des solutions. D'après [17].

It is worth noting that the unique way to form lepidocrocite, γ-FeOOH, a ferric oxyhydroxide isostructural with boehmite γ-AlOOH, is the oxidation of Fe(OH)2 by air in suspension at pH around 7 [9]. Oxidation occurs at the minimum of solubility of ferric complexes ruling out a dissolution–crystallization process for the structural transformation. It presumably results from solid-state reaction involving local rearrangements of chains of octahedrons forming the corrugated planes of the oxyhydroxide phase. Fragmentation of initial ferrous hydroxide particles forms lath-shaped particles. If oxidation proceeds around pH 7–8 but very fast with H2O2, feroxyhyte, δ-FeOOH, is obtained without any structural rearrangement, even if stacking defects and tetrahedral cations are the more often present [9]. Like lepidocrocite, feroxyhyte is never formed from ferric species. It seems that ferrous ions are oxidized in situ and the hydroxide sheets are simultaneously partially deprotoned, leading to feroxyhyte as the memory of ferrous hydroxide.

3.3 Ferric-ferrous mixed phases: green rusts and magnetite

The presence of ferrous and ferric ions simultaneously in solution orients the condensation process to the formation of specific phases, namely the green rusts, of hydrotalcite structural type, and magnetite or maghemite, of spinel structural type. The formation of these mixed phases depends on many factors such as the iron concentration, pH and especially the composition of the system defined as x=[Fe3+/(Fe2+ + Fe3+)] (Fig. 1). These phases are of high importance because green rusts are reactive intermediate products in aqueous corrosion of iron and are abundantly found in reductomorphic soils. Spinel oxides are ferrimagnetic materials usable for many technological applications. All these phases can have a more or less broad range of composition, x. For green rusts, x is near of 0.33 while x is equal to 0.66 for magnetite. A special feature of these phases lies in the fact that electrons are mobile at room temperature into spinel structure leading to a Fe2.5+ state for octahedral cations, while there is no such electron hopping through the bi-dimensional framework of green rusts.

3.3.1 Green rusts

For x⩽0.66 and {[OH−]/[Fetotal]} = 2 (pH ≈ 8), hydroxylation of the mixture forms a green rust (GR), a phase derived from brucite structure of Fe(OH)2 in which Fe2+ and Fe3+ ions fill the octahedral sites giving a positive charge to the brucitic sheets (Fig. 1). This positive charge is balanced by anion intercalation and there are in fact several structural families depending on the nature of the intercalated anions. The structural prototype is a carbonated phase, pyroaurite [Mg6Fe2(OH)16]CO3⋅3 H2O. With chloride or carbonate anions, green rust of type 1 with a variable Fe(II)–Fe(III) composition is formed, while tetrahedral anions (sulphate, arsenate...) form green rust of type 2 with the unique composition Fe(II)/Fe(III) = 2 [14,16,39]. The study of the progressive alkalization of Fe(II) and Fe(III) mixtures in the presence of sulphate ions, forming the phase [FeII4FeIII2(OH)12]SO4⋅8H2O for x=0.33, gives an interesting insight into the mechanism of formation [42] (see also Ruby's paper in this issue [43]). During the coprecipitation of ferric and ferrous ions, this phase forms following a heterogeneous crystallization process, because the two ions precipitate successively. Up to pH 4, purely ferric and poorly ordered hydroxysulphate forms on which, at higher pH, hydroxylated ferrous ions adsorb inducing the crystallization of GR phase. Crystallization proceeds according to dissolution–crystallization, allowing the incorporation of sulphate anions into the structure. Surprisingly, the end of the formation of GR is not marked by an equivalent point in the pH titration curve. By raising pH up around 10, the equivalent point corresponds exactly to the transformation into magnetite and ferrous hydroxide, showing the metastability of GR against hydroxylation. It is interesting to note that GR phases can be formed following different pathways: a partial oxidation of ferrous hydroxide, a coprecipitation of ferric and ferrous ions, and a chemical, electrochemical or biological reduction of lepidocrocite [36]. GRs appear as a turn-plate in many redox processes involving iron corrosion or transformation in natural environment [6,15,16,49].

There is a very close structural relation between ferrous hydroxide, green rusts and feroxyhyte. Continuity could be expected in the formation of these phases by hydroxylation of cations in solution, but such continuity does not exist. The reason seems to come from kinetic and electronic reasons. For mixtures with an x ratio higher than 0.33, electron mobility between ferrous and ferric ions drives the spinel crystallization as seen below. Precipitation of ferric ions alone forms goethite and feroxyhyte is obtained only from very fast oxidation of ferrous hydroxide. There is a chromium phase, CrOOH, with a structure very similar to that of feroxyhyte, obtained by thermolysis at 90 °C of acidic solutions. This phase probably results from the chemical inertness of Cr3+ ions towards substitution reactions and, consequently, olation and oxolation reactions are kinetically equivalent [20] so that two-dimensional growth of planes occurs instead chains for goethite (Fig. 4). In fact, ferric ions in solution seem to be too reactive towards condensation and the δ-FeOOH phase cannot be formed directly by precipitation.

3.3.2 Magnetite

Magnetite Fe3O4 is easily obtained by coprecipitation of aqueous Fe3+ and Fe2+ ions with x=0.66. Iron ions are distributed into the octahedral (Oh) and tetrahedral (Td) sites of the fcc stacking of oxygen according to [Fe3+]Td[Fe3+Fe2+]OhO4. Magnetite is characterized by a fast electron hopping between the iron cations on the octahedral sublattice. Crystallization of spinel is quasi-immediate at room temperature and electron transfer between Fe2+ and Fe3+ ions plays a fundamental role in the process. In effect, maghemite, γ-Fe2O3, ([Fe3+]Td[Fe3+5/3V1/3]OhO4 where V stands for a cationic vacancy) does not form directly in solution by precipitation of ferric ions, but a small proportion of Fe2+ (⩾10 mol %) induces the crystallization of all the iron into spinel [24,54]. All Fe2+ ions are incorporated into the early precipitate, a Fe2+-ferrihydrite forming a short-range ordered, mixed valence material exhibiting fast electron hopping. Electron mobility brings about local structure rearrangements and drives spinel ordering. Besides this topotactic process, crystallization of spinel can also proceed by dissolution–crystallization, resulting in two families of non-stoichiometric spinel particles ([FeIII]Td[FeIII1+2z/3FeII1−zVz/3]OhO4) with very different mean size [24,54]. The relative importance of these two pathways depends on the Fe2+ level in the system and the end products of the coprecipitation are single phase only for 0.60⩽x⩽0.66. The comparison with the cases where M2+ is different from Fe2+ emphasizes the role of electron mobility between Fe2+ and Fe3+ ions in the crystallization process. With other divalent cations, intervalence transfers are negligible and a spinel ferrite forms only by dissolution–crystallization [27]. With x=0.66, corresponding to stoichiometric magnetite, the mean particle size is finely monitored in the range 2–12 nm by the conditions of precipitation, pH and ionic strength [25,28,57].

Nanoparticles of magnetite are very sensitive to oxidation and transform into maghemite, γ-Fe2O3. The high reactivity is obviously due to the high surface-to-volume ratio, but aerial oxidation is not the only way to go to maghemite. Due to the high electron mobility in the bulk, magnetite nanoparticles give rise to an interesting surface chemistry. Different interfacial ionic and/or electron transfers depending on the pH of the suspension can be involved in the transformation. In basic medium, the oxidation of magnetite proceeds by oxygen reduction at the surface of particles (electron transfer only) and coordination of oxide ions, while in acidic medium and anaerobic conditions, surface Fe2+ ions are desorbed as hexaaquo complexes in solution (electron and ion transfer) according to [21]:

[Fe3+]Td[Fe2.5+2]OhO4+2H+→0.75[Fe3+]Td[Fe3+5/3V1/3]OhO4+Fe2++H2O
In both cases, the oxidation of Fe2+ ions is correlated with the migration of cations through the lattice framework, creating cationic vacancies in order to keep the charge balance, as represented in Scheme 1.

Scheme 1

Sketches of the oxidation of magnetite into maghemite in acidic suspension: (a) by protonation of a surface oxygen atom, a mobile electron is localized on a superficial octahedral iron ion; (b) in these acidic conditions (pH around 2), the iron (II) ion formed is released as a soluble hexaaquocation leaving an excess of positive charge inside the particle; (c) the excess of charge is compensated by moving a ferric ion towards the surface in order to create a cationic vacancy in the lattice. The net balance of elimination of Fe(II) ions is the oxidation of material and diffusion of cationic vacancies towards the interior of particles.

The mobility of electrons on the octahedral sublattice renews the surface ferrous ions allowing the reaction to go to completion. The oxidation in acidic medium (pH ≈ 2) does not lead to noticeable size variation. This reaction is apparently reversible. Adsorption of ferrous ions on maghemite particles by raising the pH proceeds so that the composition of magnetite (x=0.66) is reached and all iron ions appear as ‘spinel iron’ by Mössbauer spectroscopy [50–52]. In fact, there is no migration of iron ions towards the interior of particles. Electrons (and presumably protons) are injected into the particle from the ferrous hydroxide adsorbed layer. This layer crystallizes as spinel and the reaction stops when equal populations of Fe3+ and Fe2+ in the octahedral sublattice are reached. Similar electron transfers occur during adsorption of ferric ions on magnetite [4] or reduction of silver or platinum ions in suspension by magnetite, leading to a mixture of nanoparticles of maghemite and silver or platinum [23].

Maghemite particles resulting from oxidation of magnetite can easily form very stable and concentrated aqueous dispersions. In acidic medium and at low ionic strength, maghemite nanoparticles carry a high positive charge density and so are well dispersed in water, forming sols practically free from aggregation [22,26,38]. The formation of such stable sols is a key step to the preparation of magnetic materials such as ferrofluids [1,10,11,13,30]. The dispersion of particles in organic or inorganic matrices enabled the synthesis of various magnetic composite materials well-suited for studies on magnetism of nanoparticles, including measurements on unique particle [56]. Thermal treatment of silica-based composites led to the formation of a less common phase of iron oxide. Silica glass composites were prepared by polymerizing silicic acid or alkoxysilanes inside the aqueous sol of maghemite [7]. Hydrolysis and condensation of silanols take place in situ, forming a gel and a transparent monolithic glass after drying at room temperature (Fig. 6).

Fig. 6

Transmission electron microscopy image of γ-Fe2O3–18wt% silica composite.

Cliché de microscopie électronique en transmission du composite silice–γ-Fe2O3 18% en masse.

The silica matrix acts as an anti-sintering agent that stabilizes the maghemite particles against the thermal transformation into haematite. In composites with sufficiently low particle concentration, no transformation occurs as long as the matrix prevents the migration and coalescence of particles, that is, up to around 1000 °C, the temperature at which the glass softens or starts crystallizing. By heating at 1200 °C, the matrix partly crystallizes into cristobalite and the major iron oxide phase is the rarely observed polymorph ɛ-Fe2O3 [55]. The particles are spherical in shape (Fig. 7) and correspond to a few tens of maghemite nanoparticles in volume. ɛ-Fe2O3 isotype with kappa alumina, is ferrimagnetic with a high coercivity [19]. It is probably piezoelectric.

Fig. 7

TEM micrograph of silica composite heated at 1200 °C and crystal structure of ɛ-Fe2O3.

Cliché de microscopie électronique en transmission du composite silicique chauffé à 1200 °C et structure de ɛ-Fe2O3.

At 1400 °C, the crystallization of the matrix is complete and iron oxide is transformed into haematite in the form of crystals larger than those of ɛ-Fe2O3 by at least one order of magnitude. All observations indicate that ɛ-Fe2O3 forms as a result of the sintering of a limited number of γ-Fe2O3 nanoparticles. With powdered uncoated particles, the γ→α-Fe2O3 transformation starts below 300 °C and is generally complete at 400 to 500 °C [53]. In powders, the surface component in the total free energy of the transformation of iron oxide particles can be eliminated, so the free energy of the system can be minimized and the thermodynamically stable phase (haematite) is obtained. In the composites, when the diffusion of particles is limited, the decrease in surface area allows us to lower the free energy of the system, but the surface component remains important, so that the minimum in free energy cannot be reached and a metastable phase forms. It could be possible that a careful control of the thermal treatments allows one to observe a series of phases intermediate between γ- and α-Fe2O3, like for alumina. Many other phases could also be synthesized such as for instance β-Fe2O3 of bixbyite β-Mn2O3 structural type (Fig. 8). This phase, antiferromagnetic (TN≈120K), results from dehydroxylation of β-FeOOH (akaganeite) in vacuum at 170 °C or from solid-state reaction at 400 °C between NaCl and Fe2(SO4)3 [59].

Fig. 8

Crystal structure of β-Fe2O3.

Structure cristalline de β-Fe2O3.

4 Conclusions

This overview emphasizes the high versatility of aqueous iron chemistry. It shows how to control the crystalline structure and offers many possibilities for tailoring materials for a wide range of utilizations. The careful control of the size and degree of dispersion of the particles in composite materials may reveal unexpected phenomena.

Acknowledgements

The authors wish to thank their collaborators P. Belleville, P. Prené, L. Vayssières, and J. Hernandez. Prof. J.-M. Génin (LCPME, ‘Université Henri-Poincaré, Nancy, France) is gratefully acknowledged for fruitful discussions.

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