Influence of the Preparation Technique on the Magnetic Characteristics of ε-Fe2O3-Based Composites

Abstract

ε-Fe₂O₃ is an iron(III) oxide polymorph attracting an increasing interest due to its unique magnetic properties combining extremely high coercivity and relatively large saturation magnetization. We review existing methods for the ε-Fe₂O₃ synthesis focusing on synthesis speed, repeatability, manufacturability and purity of the final product. Samples of ε-Fe₂O₃ have been synthesized using the two methods that appear the most promising: silica gel impregnation and microemulsion. In both cases, ε-Fe₂O₃ and α-Fe₂O₃ are present in the final product as attested by X-ray diffraction patterns and magnetic properties (maximum coercive force at 300 K~1 Tesla). Two different precursors, iron(III) nitrate and iron(II) sulfate, have been used in the silica gel impregnation method. Somewhat surprisingly, iron sulfate proved superior yielding ε-Fe₂O₃ content of 69% in the total iron oxide product, compared to 25% for iron nitrate under the same synthesis conditions. These results pave the way for modifying the existing ε-Fe₂O₃ synthesis methods aiming to increase the content of the epsilon phase in the final product and, consequently, improve its physicochemical properties.

1. Introduction

Iron(III) oxide (Fe₂O₃) is one of the most commonly used metal oxides for various applications. The polymorphic nature of Fe₂O₃ has been known for a very long time, and nowadays, the existence of five (alpha, beta, gamma, epsilon, and zeta) Fe₂O₃ crystalline polymorphs has been established [1,2].

The most stable and widespread are alpha and gamma polymorphs found in nature as the minerals hematite and maghemite, respectively. Beta and zeta polymorphs are metastable and do not exist in natural conditions [2,3,4]. The Epsilon phase, once also believed to be metastable, has been increasingly found in rocks [5,6] and in man-made materials [7,8,9]. Of all Fe₂O₃ polymorphs, only ε-Fe₂O₃ is characterized by a combination of unique magnetic properties, primarily high coercivity and small particle size in the nanometer range.

ε-Fe₂O₃ polymorph was discovered in 1934 [10]. Despite notable differences between the obtained material and both hematite and maghemite, its characteristic properties took many decades to establish. In 1946, an X-ray diffraction spectrum of Fe₂O₃ synthesized at high temperatures was reported [11]. This spectrum did not correspond to either α-Fe₂O₃ or Fe₃O₄, which is a stable phase at temperatures above 1700 K in an inert atmosphere [11]. Below 1600 K, some of the ε-Fe₂O₃ nanoparticles appeared to be converted into the more stable α-Fe₂O₃, while at higher temperatures, all Fe₂O₃ polymorphs were converted into Fe₃O₄. Only much later, in 1963, was this new structure named and characterized [12].

Tronc et al. [13] have proposed that ε-Fe₂O₃ is a non-collinear four-sublattice ferrimagnet, likely to be piezoelectric, with three octahedrally and one tetrahedrally coordinated sublattices, arranged in such a way that Fe spins in the tetrahedral sublattice are canted with respect to those in octahedral ones. However, the magnetic structure of ε-Fe₂O₃ is still debated. The initial assessment [13] has been challenged, suggesting that at 300 K, no spin canting occurs in the tetrahedral sublattice, and the net magnetization of ε-Fe₂O₃ is simply due to uncompensated magnetic moment of spins in the tetrahedral and one of the octahedral sublattices, while the moments of two other octahedral sublattices mutually cancel [14]. Furthermore, ε-Fe₂O₃ exhibits rich and not yet fully understood magnetic behavior at cryogenic temperatures [14,15,16].

Concerning the crystal structure of ε-Fe₂O₃, Tronc et al. [13] have demonstrated that it occupies an intermediate position between γ-Fe₂O₃ and α-Fe₂O₃ in several respects, for example, the arrangement of anions and the proportion of four-coordinated cations. The formation of ε-Fe₂O₃ occurred during the heat treatment of γ-Fe₂O₃ particles dispersed in silicon dioxide. γ-Fe₂O₃ particles are resistant to heating as long as the matrix or shell prevents their sintering, which, depending on the degree of agglomeration, leads to the formation of ε-Fe₂O₃ or α-Fe₂O₃. Consequently, in order to obtain ε-Fe₂O₃, it is necessary to limit the size of particles formed during the synthesis of metastable phases. This approach appears promising for obtaining high purity ε-Fe₂O₃ and potentially can be used to obtain other currently unknown polymorphs of iron oxide under various temperature conditions.

Recently, ε-Fe₂O₃-like phases have been found in a number of natural [5,6] and man-made materials [7,8,9]. For example, Dejoie et al. [7] have detected the ε-Fe₂O₃ polymorph in the ceramics of the Song Dynasty (960–1279) manufactured in Jian Yao-type kilns. This suggests that the formation of Fe₂O₃ polymorphs is associated with thermal transformations of iron-containing materials in the oxidizing atmosphere.

Due to the outstanding magnetic properties of ε-Fe₂O₃, this polymorph can be used in various applications. First of all, its high coercivity ε-Fe₂O₃ makes it a promising candidate for a recording medium. Investigation of the effect of high-frequency resonance in the ε-Fe₂O₃ phase [17,18] shows the possibility of its applications in electronic devices intended for high-speed wireless communication, for effective suppression of electromagnetic interference and stabilization of the electromagnetic transmittance [18,19,20]. ε-Fe₂O₃ possesses both spontaneous magnetization and polarization, so it can be used as an advanced magnetoelectric material with possible applicability in various electric/magnetic field-tunable devices [21] or in biomedicine for the targeted delivery of drugs (under the action of a magnetic field), including colloidal solutions of magnetic nanoparticles (MNPs). For example, during transdermal procedures, in particular, based on the use of microneedles [22]. Synthetic and biogenic MNPs based on various ferrimagnetic iron oxides (Fe₃O₄, γ-Fe₂O₃, and ε-Fe₂O₃) have low toxicity and, therefore, are used in preparations for theranostics [23].

The present work carries out a review of the most promising synthesis methods of ε-Fe₂O₃, the most efficient synthesis methods of this polymorph are selected, and the physical properties of samples of this material are obtained and studied.

2. Synthesis Methods for ε-Fe₂O₃

Several methods for synthesizing high-purity ε-Fe₂O₃ have been considered: sol-gel method, silica gel impregnation method, microemulsion method, chemical vapor deposition (CVD), thin film deposition methods, and thermal decomposition method.

The sol-gel method makes it possible to synthesize ε-Fe₂O₃ in a silica gel matrix, which is necessary to limit the maximum sizes of nanoparticles during annealing. To obtain the sol, tetraethoxysilane (TEOS) is used as a silica nanocomposite precursor. Iron nitrate serves as a source of iron for the formation of an oxide phase, which subsequently turns into ε-Fe₂O₃ upon annealing [24]. With the help of TEOS, a shell for iron oxide particles is formed, which is necessary to limit particle size during growth. The processes of hydrolysis and condensation proceed in an acidic hydroethanolic medium at a molar ratio of TEOS:H₂O:EtOH = 1:6:6, pH ≈ 0.9. The reactions are self-catalyzed by nitric acid formed during the hydrolysis of iron nitrate. Gelation at room temperature occurs in 20 days; after that, the gel is dried for 14 h at 60–80 °C. The obtained red-brown translucent glassy material is crushed in an agate mortar and then subjected to heat treatment in air with temperature increasing in steps of 100 °C, followed by 3-h annealing and slowly cooling at each temperature, from 300 °C to 1100 °C.

Using this method, samples of ε-Fe₂O₃-SiO₂ composite nanoparticles with an average diameter of 25 nm have been obtained [24]. The properties of samples depend on the synthesis conditions, varying from superparamagnetic to ferrimagnetic at 300 K for the samples annealed at 1000 °C and 1100 °C. Néel temperature of the ε-Fe₂O₃ phase was found to be 510 K, and the coercive force at 300 K was about 20 kOe. At the same time, ε-Fe₂O₃ remained stable up to about 1300 °C.

In 2021, samples of ε-Fe₂O₃ with a high coercivity (>1 T) were synthesized using the sol-gel method [25]. The formation of the ε-Fe₂O₃ phase apparently followed γ → ε → α pathway. The highest ε-Fe₂O₃ content, of up to 90% in the mixture as calculated from Mössbauer spectra measured at room temperature, was achieved for the sample heat-treated at 1000 °C for 10 h. The magnetic properties of the samples range from superparamagnetism to a ferrimagnetic behavior, and a two-step magnetic transition typical for ε-Fe₂O₃ [14,15,16] was observed in the range of 80–150 K.

The silica gel impregnation method is a modification of the sol-gel method, in which a silica gel is used as the SiO₂ matrix, allowing to exclude the long-term sol-gel stage from the synthesis process. Silica gel is impregnated with iron sulfate solutions of various concentrations, followed by drying (4 h at 180 °C) and high-temperature annealing in a muffle furnace (4 h at 400–900 °C). Using this method, it is possible to synthesize stable nanoparticles with a diameter of 20 nm, a Néel temperature of 470 K and a coercive force of about 9 kOe [26,27,28,29,30].

The microemulsion method is based on mixing two microemulsions formed with cetyltrimethylammonium bromide (CTAB) and octane-based butanol-1 (oil phase). A solution of Ba(NO₃)₂ and Fe(NO₃)₃ salts was placed in an aqueous phase within the reverse micelles of the first microemulsion, and a solution of was placed inside the second one. Microemulsions are mixed, and then TEOS is added to the solution, all operations being carried out with rapid stirring until the mixture reaches homogeneity. The desired material is separated by centrifugation, heated to 900–1100 °C, and maintained at this temperature for 4 h [31,32].

Samples synthesized by this method contained rod-shaped ε-Fe₂O₃ nanoparticles with geometric dimensions of 100–140 × 20–40 nm, Neel temperature of 480 K and coercive force of 20 kOe.

Chemical vapor deposition is implemented using a microwave torch discharge, which is initiated in argon on a hollow nozzle-shaped electrode. ε-Fe₂O₃ is deposited on the walls of the reaction chamber (quartz tube) from a flowing gas mixture consisting of vapors of iron pentacarbonyl (Fe(CO)₅) and hydrogen peroxide (H₂O₂) [33]. In such a system, ε-Fe₂O₃ precipitates at a rate of about 1 g/h and, immediately after being removed from the reaction chamber, can be stored in air as a powder. Due to the flow system, this method can work continuously, but it has a significant drawback – the final product contains a significant amount of γ-Fe₂O₃ and α-Fe₂O₃ impurities.

The thin film deposition methods can be based either on atomic layer deposition (ALD) or pulsed laser deposition (PLD).

To implement the ALD process, FeCl₃ powder placed in a reactor in an open boat at 158 °C and deionized water in a container outside of the reactor are used as precursors [34]. Nitrogen is used as a carrier gas to purge the reactor after each cycle. Thin films of ε-Fe₂O₃ are deposited on a silicon or borosilicate glass substrate at temperatures from 210 °C to 360 °C, having a thickness of about 260 nm and a coercive force of 1.6 kOe.

Epitaxial films of ε-Fe₂O₃ have been obtained by PLD from a Fe₂O₃ target on GaN substrates using a KrF laser [35,36]. The growth of ε-Fe₂O₃ takes place in an oxygen atmosphere at a pressure of 20 Pa and a substrate temperature of 750–850 °C. For the obtained films, the correlation between the crystal structure and magnetic properties, dependence of the coercive force on the thickness, and mechanism of films nucleation and formation have been investigated.

The method of thermal decomposition consists of annealing a nontronite clay mineral (Garfield, Washington, DC, USA) followed by separation of the iron oxide phase by leaching of silicates. The coarsely ground material was heated to 900 °C at an arbitrary rate and then to 970 °C at a rate of 0.5 °C/min and maintained at this temperature for 30 h. After annealing, iron oxide was isolated by leaching the silicate phases with sodium hydroxide solution for 5 days at 70 °C. After filtration and thorough washing with water and a solution of acetic acid, a brown powder was obtained. This method can be used to obtain crystalline ε-Fe₂O₃ in the form of a precipitate or in the form of nanoparticles in a palladium matrix during the internal oxidation of the Pd₉₆Fe₄ alloy [37].

The priority parameter for ε-Fe₂O₃ is the coercive force, while methods should be selected to optimize for speed and final product purity. Based on the data summarized in Table 1, we used the microemulsion method and the silica gel impregnation method to synthesize ε-Fe₂O₃. The silica gel impregnation method is simple, fast, and low-cost. The microemulsion method is more complicated but is characterized by the absence of other iron oxide polymorphic modifications and the highest fraction of ε-Fe₂O₃ in the final product. The SiO₂ matrix used in these methods can be removed by etching.

3. Materials and Methods

Silica gel impregnation method. Silica gels with different physicochemical characteristics (Silipor 300, Silipor 075 (Vekton, Russia), Superico (Merck Millipore, Burlington, Massachusetts, MA, USA)) have been purchased and used as is to create the SiO₂ matrix. Silica gels were impregnated with 1-molar solutions of either iron(II) sulfate or iron(III) nitrate (99%, Vekton, Russia), followed by drying for 4 h at 110 °C. Sequential repetition of impregnation and drying processes has resulted in an increase in ε-Fe₂O₃ concentration in the final product. The dried samples were subjected to high-temperature annealing at 900 °C.

The microemulsion method combines microemulsion and sol-gel technologies. First, two reverse microemulsions were prepared using 9.7 mM CTAB, 39 mM butanol-1 (99%, Vekton, Russia) and 330 mM deionized water in 110 mM isooctane (99%, Vekton, Russia). The reverse micelles of the first microemulsion contained an aqueous solution of salts: 0.74 mM Fe(NO₃)₃ (99%, Vekton, Russia) and 0.074 mM Ba(NO₃)₂ (99%, Vekton, Russia), and the second contained 30 mM aqueous ammonia (99%, Vekton, Russia). The second microemulsion was then added dropwise to the first one with rapid stirring. 6.7 mM TEOS (99%, Vekton, Russia) was added to the resulting solution, followed by stirring for 20 h at a speed of 300 rpm. After 20 h of stirring, a gel was formed, which was successively washed with chloroform and methanol, and a precipitate was separated by centrifugation. The precipitate has then been annealed at 1000 °C. Synthesis procedures and obtained samples are summarized in Table 2. Samples obtained using the silica gel impregnation method are named according to the used silica gel and the precursor (Iron Sulphate—S or Iron Nitrate—N): Superico—SUP and SUP-2, Silipor 75–S75, Silipor 300—S300S, S300S-2, S300N. Three samples obtained by the microemulsion method under the same synthesis conditions are designated ME-A, ME-B, and ME-M, respectively.

X-ray diffractograms of the samples prepared with the silica gel impregnation method have been recorded using a Bruker D2 Phaser (Bruker, Billerica, MA, USA) automatic powder diffractometer. The experiment conditions were: X-ray tube radiation – CoKα₁₊₂, wavelengths λ_CoKα1 = 1.78900 Å and λ_CoKα2 = 1.79283 Å, tube operation mode 30 kV/10 mA, position-sensitive detector, reflection geometry, Bragg-Brentano focusing scheme, sample rotation speed 20 rpm, diffraction angle interval 2θ = 5–80°, scan step 0.02°, exposure at a point 1 s. Diffractograms for the samples synthesized with the microemulsion method have been analyzed using a Bruker D8 Discover diffractometer (Bruker, Billerica, MA, USA) in the parallel beam mode with linear focusing, slit width 0.6 mm, a position-sensitive detector with 2.1 aperture, theta-two-theta scanning mode, exposure at a point 2 s. Phase identification has been carried out with the PDXL2 software package (Rigaku, Version 2.0.2, Tokyo, Japan) using the Powder Diffraction File (PDF-2, 2020) powder diffraction database.

Samples have been characterized using remanence measurements in the 1.8–300 K range carried out using a SQUID magnetometer MPMS 3 (Quantum Design, San Diego, CA, USA) in the vibrating sample mode. Isothermal remanent magnetization (IRM) has been acquired in a 5 T field at 1.8 K after cooling in a zero magnetic field (zero field cooling, ZFC) and in a strong magnetic field (5 T, field cooling, FC), respectively. IRM decay curves in the zero field were then measured quasi-continuously during warming to 300 K at the 1.5 K/min rate in the MPMS temperature sweeping mode. IRM (5 T), acquired at 300 K, was measured at the same rate during the cooling-warming cycle between 300 and 1.8 K in a zero field.

To assess the samples’ behavior at high temperatures, the AC magnetic susceptibility (driving field frequency 976 Hz, amplitude 200 A/m) has been measured as a function of temperature up to 700 °C (973 K) in air, using an MFK-1FA Kappabridge (AGICO, Brno, Czech Republic) equipped with a CS4 furnace. This experiment requires about 150–200 mg of material in powder form, and therefore measurements have been performed for the samples synthesized with the silica gel impregnation method only. The microemulsion method didn’t provide an insufficient amount of the material during a single synthesis cycle for the susceptibility measurements.

Hysteresis loops have been measured in a maximum field (7 T, 295 K) using the MPMS 3 in the vibrating sample mode with a logarithmic field increment of 400 points per loop. To obtain coercivity of remanence (H_cr) values, IRM acquired in a 5 T has been remagnetized by the magnetic field of opposite sign up to 3 T, and the respective remagnetization curves have been measured using the same instrument.

4. Results and Discussion

4.1. X-ray Diffractograms

X-ray diffractograms (Figure 1) show lines belonging to ε-Fe₂O₃ and hematite phases. For samples synthesized with the silica gel impregnation method, the crystalline lattice parameters (Table 3) of both polymorphs correspond reasonably well to the data from the literature. For ε-Fe₂O₃: a = 5.098(2) Å, b = 8.785(3) Å, and c = 9.468(2) Å [15]; a = 5.095 Å, b = 8.789 Å, and c = 9.437 Å [38] and for α-Fe₂O₃: a = 5.0345 Å and c = 13.749 Å [39]. However, in samples synthesized with the microemulsion method, the ε-Fe₂O₃ lattice appears slightly deformed in the ab plane so that the parameter a is some 1–2% lower than the values reported in the literature and found for samples synthesized with the silica gel impregnation method in this study. It should be noted that the hematite phase in these samples also shows lattice parameters slightly smaller than reference values. This may indicate that iron oxides are squeezed to some extent in the silicate matrix. The relative fraction of ε-Fe₂O₃ phase in the total iron oxide content varies widely, from ~25% in the sample prepared with nitrate precursor to >70% in the sample prepared under the same conditions but with the sulfate precursor.

4.2. Magnetic Properties

Temperature dependences of AC magnetic susceptibility are shown in Figure 2. All samples except S300N show strong Hopkinson peaks associated with the magnetic transition of the ε-Fe₂O₃ phase and much weaker but still noticeable peaks just below the hematite Néel temperature. The transition temperature of the ε-Fe₂O₃ phase lies in the 225–230 °C (498–503 K) range, close to the maximum values reported in the previous studies [24,40,41,42,43,44,45,46]. The S300N sample (Figure 2c) is notable in that it does not exhibit Hopkinson peaks associated with the magnetic transitions, although the transition temperature of the ε-Fe₂O₃ phase for this sample is similar to others. The different AC susceptibility behavior of this sample may be due to a smaller grain size of both ε-Fe₂O₃ and hematite phases.

Figure 3 illustrates the low-temperature remanence behavior and hysteresis loops measured at 295 K for two samples that show coercivities in excess of 1 Tesla, as expected for the ε-Fe₂O₃ phase [24,44,46,47,48,49,50].

Coercivity, magnetization and remanence values are listed in Table 4. Remanent magnetization acquired at 1.8 K shows a complex behavior that is characterized by:

• The rapid decrease between 1.8 K and 60–70 K;

• Increase between 60–70 K and 150 K;

• The relatively gradual decrease between 150 K and room temperature.

However, the relative proportion of these features is different for different samples. For the sample synthesized with the silica gel impregnation method, loss of magnetization between 1.8 K and 70 K is far more prominent than the following rebound, while the opposite pattern is observed for the sample synthesized with the microemulsion method. For both samples, remanence acquired at 300 K exhibits notable irreversibility during the zero-field cooling-warming cycle, losing 15–20% of its value after the cycle. In addition, both the low- and room-temperature remanence curves show weak but discernible features around 240 K, likely due to the Morin transition in hematite [51]. This is somewhat lower than the transition temperature in bulk hematite [52]. However, the Morin transition temperature is known to decrease significantly with grain size [53,54,55,56], implying the fine (<100 nm) size of the hematite particles in these samples.

Apart from the behavior described above, which seems to be characteristic of the ε-Fe₂O₃ phase, a feature that can be viewed as a collapse of the remanent magnetization signal has been observed in some samples (Figure 4). Remanence acquired at 1.8 K drops suddenly around 250 K to small, sometimes near-zero, values (Figure 4a). The hysteresis loop at 295 K (Figure 4b) becomes strongly wasp-waisted due to coexisting soft and hard magnetic phases. The coercive force then appears to be controlled by a soft phase, while the coercivity of remanence H_cr is due to the hard one. At the same time, the remanence signature between 1.8 K and 200 K in this sample (Figure 4c) resembles that measured for the samples containing stable ε-Fe₂O₃ phase (Figure 3), though the coercivity values at 200 K are still considerably lower. All this suggests that, unlike others, samples showing remanence collapse close to room temperature contain a significant fraction of ε-Fe₂O₃ particles at the verge of superparamagnetism. The lower coercivity at 200 K further indicates that stable ε-Fe₂O₃ particles may also have a smaller size than in other samples.

Remanence measurements presented here are of particular interest in studies of natural and some man-made materials, such as archaeological ceramics. Standard methods used in the physics of magnetic materials may fail in this case since they employ field measurements, and the signal of the ferromagnetic (sensu lato) phases usually present in a concentration <1% concentration will be masked by an overwhelmingly large contribution from the paramagnetic matrix. Therefore, reference data for carefully prepared and thoroughly characterized synthetic ε-Fe₂O₃ are tantamount to the correct interpretation of measurements made on natural samples. Until now, remanence curves for ε-Fe₂O₃ between 2 K and 300 K have only been reported for the material prepared with the sol-gel method, the precursor being iron(III) and yttrium nitrates with an approximate Fe:Y atomic ratio of 4:3 [42]. Their M_r (300 K, 5 T) cooling curve closely resembles those reported in this study, while the FC (2 K, 5 T) curve shows fast decay below 50 K and gradually flattens above that temperature, similar to S300N sample behavior below 200 K in our study. At the same time, we have observed a more variable shape of zero-field decay curves for remanence acquired at 1.8 K. This must be related to fine details of the material synthesis and resulting properties and deserves further study.

5. Conclusions

Existing methods for the synthesis of ε-Fe₂O₃ iron(III) oxide polymorph have been reviewed. The two most promising methods have been chosen: silica gel impregnation and microemulsion. These methods were used to synthesize samples of silica-iron oxide composite. The iron oxide phase in the final product contains 25.3% to 70% ε-Fe₂O₃ by weight, the rest being hematite (α-Fe₂O₃). The samples are characterized by a relatively high coercive force reaching ~ 1 Tesla at 300 K, Curie temperatures of 225–230 °C (498–503 K) characteristic of the ε-Fe₂O₃ phase, and also Néel temperatures of ~680 °C (953 K) and the Morin phase transition at ~240 K, characteristic of hematite. A comparison of two different iron salts used as precursors in the silica gel impregnation method has shown that iron(II) sulfate is clearly superior to iron(III) nitrate yielding 69% of ε-Fe₂O₃ per total iron oxide mass versus 25.3%, respectively. The substantial hematite content in the samples synthesized by the microemulsion method may indicate that the synthesis parameters are not optimal, and further research in this area is needed. It is also necessary to work out and optimize the process of etching the SiO₂ matrix to obtain high-purity samples of ε-Fe₂O₃.

Author Contributions

Conceptualization, D.O.T. and K.G.G.; methodology, D.O.T., K.G.G., A.K. and L.S.; validation, I.K.K. and V.V.L.; investigation, D.O.T., K.G.G., A.K. and L.S.; resources, A.K., I.K.K., L.S. and V.V.L.; writing—original draft preparation, D.O.T. and A.K.; writing—review and editing, K.G.G., I.K.K. and V.V.L.; supervision, K.G.G.; project administration, I.K.K.; funding acquisition, V.V.L. All authors have read and agreed to the published version of the manuscript.

Institutional Review Board Statement

Not applicable.

Informed Consent Statement

Not applicable.

Data Availability Statement

Not applicable.

Acknowledgments

The study of the crystal structure, magnetic properties, and other measurements was carried out at the resource centers “X-ray diffraction methods of research”, “Center for Diagnostics of Functional Materials for Medicine, Pharmacology and Nanoelectronics”, and “Geomodel” of the Science Park of St. Petersburg University.

Conflicts of Interest

The authors declare no conflict of interest.

Footnotes

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Figures and Tables

Figure 1. X-ray diffractograms: (a) Sample S300S-2; (b) Sample S300N; (c) Sample ME-B. PDF-2 (International Center for Diffraction Data, 2020) cards: Hematite 01-080-2377; ε-Fe2O3 01-076-3272; Cristobalite 01-077-1317; Quartz 01-083-0539; Tridymite 01-086-0681.

Figure 2. AC susceptibility temperature dependences: (a) Sample SUP; (b) Sample S300S-2; (c) Sample S300N.

Figure 2. AC susceptibility temperature dependences: (a) Sample SUP; (b) Sample S300S-2; (c) Sample S300N.

Figure 3. (a) Low-temperature remanence decay curve, Sample ME-B; (b) Hysteresis loop and backfield demagnetization curve measured at 295 K, Sample ME-B; (c) Low-temperature remanence decay curve, Sample SUP-2; (d) Hysteresis loop and backfield demagnetization curve measured at 295 K, Sample SUP-2.

Figure 3. (a) Low-temperature remanence decay curve, Sample ME-B; (b) Hysteresis loop and backfield demagnetization curve measured at 295 K, Sample ME-B; (c) Low-temperature remanence decay curve, Sample SUP-2; (d) Hysteresis loop and backfield demagnetization curve measured at 295 K, Sample SUP-2.

Figure 4. Illustration of the collapse of magnetic signal in ε-Fe2O3, sample S300N: (a) Low-temperature remanence behavior between 1.8 K and 300 K; (b) Hysteresis loop and backfield demagnetization curve measured at 295 K; (c) Low-temperature remanence behavior between 1.8 K and 200 K; (d) Hysteresis loop and backfield demagnetization curve measured at 200 K.

Figure 4. Illustration of the collapse of magnetic signal in ε-Fe2O3, sample S300N: (a) Low-temperature remanence behavior between 1.8 K and 300 K; (b) Hysteresis loop and backfield demagnetization curve measured at 295 K; (c) Low-temperature remanence behavior between 1.8 K and 200 K; (d) Hysteresis loop and backfield demagnetization curve measured at 200 K.

Table 1

Main characteristics of the methods for the synthesis of ε-Fe₂O₃.

Method	Shape of ε-Fe2O3	Matrix/Substrate	Associated Polymorphs	Max. Annealing T, °C	Duration of One Synthesis Cycle, h	Particle Size, nm	Neel T, °C	Coercive Force, kOe	Ref.
Sol-gel	NPs	SiO2/-	α-Fe2O3	1100	528	25	510	4–6	[24,25]
Silica gel impregnation	NPs	SiO2/-	α-Fe2O3	900	30	20–80	470	9	[26,27,28,29,30]
Microemulsion	NPs	SiO2/-	-	1100	40	20–100	480	10–20	[31,32]
CVD	NPs	-	γ-Fe2O3α-Fe2O3	n/a	1 *	n/a	n/a	n/a	[33]
Thin film deposition	Thin film	-/GaN	γ-Fe2O3α-Fe2O3	800	36+	10–30	n/a	1,6–15	[34,35,36]
Thermal decomposition	Crystal	Pd/-	α-Fe2O3unidentified phase	970	168	50–200	n/a	n/a	[37]

* For the synthesis of 1 g of NPs.

Table 2

Synthesis parameters of all samples.

№	Sample	Synthesis Method	Precursors	Matrix	AnnealingTemperature, °C
1	SUP	Silica gelImpregnation	FeSO4	Chromatographic Superico silicagel	900
2	SUP-2
3	S75	Silica gelImpregnation	FeSO4	Silipor 075	900
4	S300S	Silica gelImpregnation	FeSO4	Silipor-300	900
5	S300S-2			Silipor-300
6	S300S-2 at 200 K			Silipor-300
7	S300N	Silica gelImpregnation	Fe(NO3)3	Silipor-300	900
8	S300N at 200 K			Silipor-300
9	ME-A	Microemulsion	TEOSFe(NO3)3Ba(NO3)2	SiO2 formed during the synthesis process	1000
10	ME-B
11	ME-M

Table 3

Results of X-ray analysis.

Sample	ε-Fe2O3				Hematite (α-Fe2O3)
	Content, %	a (Å)	b (Å)	c (Å)	Content, %	a (Å)	c (Å)
SUP	61	5.094(2)	8.797(4)	9.482(2)	39	5.0377(5)	13.7539(16)
SUP-2	58.8	5.0992(13)	8.784(2)	9.485(2)	41.2	5.0367(4)	13.7512(12)
S75	38.6	5.0945(15)	8.784(3)	9.486(2)	61.4	5.0382(3)	13.7534(11)
S300S	73.1	5.098(2)	8.795(4)	9.490(3)	26.9	5.0392(14)	13.768(4)
S300S-2	69.0	5.086(3)	8.799(5)	9.493(3)	31.0	5.0368(3)	13.7504(11)
S300-N	25.3	5.084(12)	8.82(2)	9.507(12)	74.7	5.043(2)	13.771(7)
ME-A	60.9	5.057(4)	8.796(3)	9.465(3)	39.1	5.03077(19)	13.7360(7)
ME-B	39.2	5.048(4)	8.797(3)	9.467(3)	60.8	5.0310(2)	13.7363(8)
ME-M	37.2	4.951(4)	8.863(6)	9.473(5)	62.8	5.0294(5)	13.727(2)

Table 4

Coercivity, magnetization, and remanence of synthesized samples.

Sample	M (7 T, 300 K), Am2/kg	Mr (300 K, 7 T loop), Am2/kg	Mr (300 K, 5 T), Am2/kg	ZFC (1.8 K, 5 T), Am2/kg	FC (1.8 K, 5 T), Am2/kg	µ0·Hc, mT	µ0·Hcr, mT
SUP	3.842	1.227	1.209	1.026	0.9691	1121	1734
SUP-2	3.595	1.13	1.113	1.405	1.545	1089	1742
S75	2.222	0.7528	0.7337	0.7668	0.9171	1243	2047
S300S	2.735	0.7513	0.7014	1.073	1.212	4.96	23.3
S300S-2	2.925	0.5294	0.5292	0.6499	0.7830	1.71	1617
S300S-2 at 200 K	3.158	0.8410	0.8411	1.040	1.211	576	1834
S300N	1.874	0.3042	0.2856	0.7179	0.8422	50.3	1190
S300N at 200 K	2.097	0.4292	0.4327	0.7336	0.8799	256	1666
ME-A	1.647	0.4844	0.4774	0.4204	0.4340	896	2160
ME-B	1.751	0.5838	0.5793	0.4799	0.4643	1070	2143
ME-M	0.7439	0.1577	0.1560	0.1935	0.2047	342	2130

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