Startseite Magnetic iron oxide/clay nanocomposites for adsorption and catalytic oxidation in water treatment applications
Artikel Open Access

Magnetic iron oxide/clay nanocomposites for adsorption and catalytic oxidation in water treatment applications

  • Ganjar Fadillah , Septian Perwira Yudha , Suresh Sagadevan , Is Fatimah EMAIL logo und Oki Muraza
Veröffentlicht/Copyright: 8. September 2020
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Open Chemistry
Aus der Zeitschrift Open Chemistry Band 18 Heft 1

Abstract

Physical and chemical methods have been developed for water and wastewater treatments. Adsorption is an attractive method due to its simplicity and low cost, and it has been widely employed in industrial treatment. In advanced schemes, chemical oxidation and photocatalytic oxidation have been recognized as effective methods for wastewater-containing organic compounds. The use of magnetic iron oxide in these methods has received much attention. Magnetic iron oxide nanocomposite adsorbents have been recognized as favorable materials due to their stability, high adsorption capacities, and recoverability, compared to conventional sorbents. Magnetic iron oxide nanocomposites have also been reported to be effective in photocatalytic and chemical oxidation processes. The current review has presented recent developments in techniques using magnetic iron oxide nanocomposites for water treatment applications. The review highlights the synthesis method and compares modifications for adsorbent, photocatalytic oxidation, and chemical oxidation processes. Future prospects for the use of nanocomposites have been presented.

Keywords: iron oxide; magnetic; nanomaterials; photocatalyst

1 Introduction

Water treatment has continued to be a required technology in many industries, because water contamination and pollution have become major environmental problems worldwide. This has created a great demand for an effective water treatment technology, and adsorption and photocatalysis are the most popular techniques due to their ease of handling. They are also more economical than other techniques. Research work in nanoscale science and engineering has suggested that nanomaterials have a great potential to improve the capability of these techniques to reduce water contaminants. Magnetic materials, especially iron oxide nanoparticles, have been known since ancient times to have characteristic properties for specified applications, including for water treatment [1]. Magnetite and maghemite (Fe3O4, γ-Fe2O3) are the most commonly studied materials due to the outstanding properties they exhibit on a nanometric scale, including high specific surface area, superparamagnetism, and so on [2,3,4]. The nanoscale dimensions of the materials can be developed by enhancing and functionalizing their surfaces for use in environmental and biomedical applications. In addition, magnetic nanocomposites have been developed for sensor, adsorption, catalytic, and photocatalytic environmental applications.

Magnetic iron oxide nanoparticles (MNPs) may be good candidates for use in the development of high-capacity adsorbents and photocatalysts. With their saturation magnetization, magnetic iron oxide-based nanocomposites provide a cost-effective approach for adsorption and photocatalysis through their reusability and ease of recovery. A material’s selectivity or affinity for a specified contaminant can be enhanced by modifying its surface and combining it with features of solid supports. By the scheme, and as conducted in biomedical and biological applications of MNPs, material properties can be tailored by setting synthesis parameters [4,5].

Some solid supports have been reported as magnetic nanoparticle supports, such as zeolite, MCM-41, biochar, carbon nanotube, and mesoporous silica. Among potential supports and materials that can be combined with magnetic properties and MNPs, clay and clay minerals have received interest. Clays have a high adsorption capacity, which corresponds to the high surface area resulting from their layer structure and a net negative charge on their structure, which attracts and holds cations, such as heavy metals and cationic molecules. There are three basic classes of clay, which are as follows: kaolinite, micas (for example, illite), and smectites (for example, montmorillonite) [6,7]. Clays, especially natural clays, are attractive and low-cost materials due to their porosity, high specific surface area, and capacity to adsorb organic molecules and ions. At the time of writing, increasing attention on the use of magnetic iron oxide/clay nanocomposites (MICNCs) was evident in the SCOPUS database (Figure 1).

Figure 1 The popularity of using MICNCs for the photodegradation of organic molecules (keywords: magnetic iron oxide/clays; source: www.scopus.com, 2012–2019).
Figure 1

The popularity of using MICNCs for the photodegradation of organic molecules (keywords: magnetic iron oxide/clays; source: www.scopus.com, 2012–2019).

The physicochemical properties of MICNCs depend on their source, the kind of clay they contain, and the parameters governing their synthesis [8,9,10,11]. The layer silicate structure, cation exchange capacity, and pore size distribution of nanocomposites affect critical features for specified purposes in water treatment. To understand variability in nanocomposite formation and the implications for the use of nanocomposites as engineered materials, this review has presented an overview of our present knowledge regarding the influence of source material, synthesis method, and parameters in production technologies on MICNCs.

2 Synthesis of MICNCs

Clay minerals have been defined as hydrated phyllosilicates, which are abundant in sedimentary rocks. The basic unit of phyllosilicates, including clay minerals, is based on interconnected SiO44− tetrahedrons, with three apical oxygen atoms from each tetrahedron shared with another tetrahedron, making the fourth apical oxygen vertically positioned upon the sheet [12,13]. In this respect, the basic structure is Si2O52− with hexagonal symmetry. In some clays, the tetrahedral position can be occupied by aluminum atoms, which deform the tetrahedral sheet and decrease its symmetry to a level lower than hexagonal.

The tetrahedron forms sheets with X (O, OH)6 octahedrons, which share not only vertexes but also half of their edges. Octahedrons are tagged together by the octahedron plane perpendicularly to [001], so that three anions (O− or OH−) form a lower layer, and three anions are in the upper layer and in between the octahedral cations (X). The occupation of structural positions in the octahedral sheet generates trioctahedral sheet silicates in which each O or OH is surrounded by three divalent cations, like Fe(ii) or Mg(ii), and dioctahedral sheet silicates in which each O or OH ion is surrounded by two trivalent cations, mostly Al(iii). Clay can be divided into two major classes according to the combination of tetrahedral and octahedral sheets, type 1:1 (layers t-o) and type 2:1 (layers t-o-t).

Many combinations and substitutions of the layers affect the negative charges of the main structure. Clay minerals are classified according to the following criteria: (i) type of layer (1:1 or 2:1), (ii) type of interlayer (water or interlayer cation), (iii) layer charge, (iv) type of octahedral sheet (di- or trioctahedral), and (v) chemical composition. In an analogous structure, layered double hydroxides (LDHs) have been designated as “anionic clay” and have a general formula expressed as [M2+1−xM3+x(OH)2]x+Ax/nn−·mH2O, where M2+ and M3+ represent, respectively, di- and trivalent metal cations; An− represents a charge anion n; x represents the molar ratio between di- and trivalent cations M2+/(M2+ + M3+); and m represents the number of water molecules. These criteria affect the synthesis procedure and variables. Table 1 shows the clay minerals, specific procedures, and synthesis parameters of various MICNCs. In general, there are two main synthesis procedures, co-precipitation and the intercalation of MNPs into a clay structure.

Table 1

Clay minerals, specific procedures, and synthesis parameters of MICNCs

Clay mineralMNP precursorMethodSynthesis conditionNotes Ref.
Natural bentonite from Slovakia Not mentionedCo-precipitationIron oxide is precipitated at 20°C and 85°CComposites have a high specific surface area. The highest magnetization is 46.22 emu/g, present at a 1:1 ratio of bentonite to iron[14]
BentoniteFeCl3 and FeSO4Co-precipitationIron oxide precipitation is followed by drying at 100°C for 3 h in airComposites have good adsorption of Cd, Zn, Cu, and Ni[15]
Montmorillonite from GreeceFeCl3·6H2OCo-precipitation and acetic acid treatmentMontmorillonite is mixed with FeCl3·6H2O and NaOH, followed by exposure to glacial acetic acidComposites have a saturation magnetization of 4.1 emu/g and more basal spacing than montmorillonite d001[16]
KaolinFe2+ and Fe3+ImpregnationIron oxide nanoparticles are dispersed into a kaolin suspension in the presence of chitosanComposites have a good adsorption capability for ciprofloxacin[16]
Saponite and palygorskiteFe3O4ImpregnationFe3O4 slurry is adsorbed by saponite and palygorskite, followed by drying at 60–80°CComposites have a good ability to adsorb the surfactant from water[17]
Natural bentonite from SlovakiaFeSO4·7H2O and FeCl3·6H2OCo-precipitationBentonite/iron oxide weight ratios of 1:1 and 5:1 with co-precipitation temperatures of 20°C and 85°CMagnetic iron oxide/bentonite composites have a magnetization of about 35–42 emu/g, and iron oxide is formed as the γ-Fe2O3 phase[14]
Natural bentonite from ShanghaiFeSO4–HNO3Pillarization–co-precipitation Montmorillonite is pillared with Al, prior to MNP co-precipitation[18]
Natural bentonite from EthiopiaFeCl3·6H2O–FeSO4·7H2OCo-precipitation–oxidationThe FeCl3·6H2O–FeSO4·7H2O precursor solution is co-precipitated into activated bentonite, followed by drying at 100°C[19]
Fe3O4/activated montmorilloniteFeCl3·6H2O and FeCl2·4H2OCo-precipitationA 30% ammonia solution is added dropwise to the iron solution (nFe2+:nFe3+ = 1:1.8) at 363 K with constant stirring to adjust the pH to 9–10, so that Fe2+/Fe3+ ions are precipitated. Mt powder is then added, and the solution is stirred for 4 hThe material has significantly improved in the adsorptivity for MB[20]
Diatomite FeCl3·6H2OSolvothermalThe MNP precursor is prepared by mixing FeCl3·6H2O with ethylene glycol, followed by the addition of CH3COONa·3H2O. The mixture is kept in an autoclave for 8 h at 200°CComposites have a saturation magnetization of 26.89 emu/g[21]
IlliteFeCl3·6H2OSolvothermalComposites have a saturation magnetization of 35.39 emu/g[21]
Natural bentonite from SlovakiaFeSO4·7H2O and FeCl3·6H2O (with the molar ratio of Fe3+/Fe2+ = 2)Co-precipitation is followed by drying at 70°CIron oxide is in the γ-Fe2O3 phase[22]
MontmorilloniteFeCl3·6H2O–FeCl2·4H2OPillarization The precursor of the oligomer of iron oxide is formed by mixing Fe(iii) and Fe(ii) solution with ammonia. Montmorillonite is intercalated by cetyltrimethylammonium ions in combination with tetraethyl orthosilicateMNPs are homogeneously distributed and generally spherical in shape, and particle sizes are around 10–15 nm[23]
Montmorillonite SWy-2FeCl2·4H2OPillarization–impregnationMontmorillonite is pillared with Ti, followed by Fe impregnationThe specific saturation magnetization is influenced by the temperature of calcination[24]
Natural bentonite from ArgentinaFe(NO3)2Pillarization The intercalation of oligomer ferrous hydroxide is followed by calcination at 500°CIncreasing basal spacing d001 of bentonite was obtained significantly [25]
Montmorillonite K10FeCl2·4H2OPillarization The intercalation of oligomer ferrous hydroxide is followed by calcination at 400°C for 2 hIncreasing basal spacing d001 of montmorillonite from 1.25 to 1.5 Å was identified[26]
Natural bentonite from East Java, Indonesia FeCl3Pillarization The intercalation of oligomer ferrous hydroxide is followed by calcination at 400°C for 4 hThe process increased the basal spacing d001 of montmorillonite from 1.49 to 1.69 Å[27]
K10 montmorilloniteFeCl2·4H2OCo-precipitation–hydrothermal The precipitate is obtained by mixing montmorillonite suspension and FeCl2·4H2O–NH4OH and keeping the mixture in an autoclave at 140°C for 5 hDispersed spherical Fe3O4 nanoparticles in the 10–45 nm size range are coated on the surface of the montmorillonite[28]
MontmorilloniteFeSO4·7H2O–FeCl3Co-precipitation–hydrogel formationAfter magnetic iron oxide montmorillonite is obtained, the graft copolymerization of acrylamide is performed using potassium persulfate as a free radical initiator and N,N′-methylenebisacrylamide as a cross-linking agentThe magnetic nanocomposite has hydrophilicity and the ability to swell[29]
Laponite FeSO4·7H2O–FeCl3Co-precipitation–hydrogel formationFe3+:Fe2+ at a molar ratio of 2:1 is co-precipitated into a laponite suspension by the addition of NH4OH at 70°C for 2 h. Hydrogel is formed via a cross-linking reaction using ammonium persulfate and N,N,N′,N′-tetramethylethylenediamineThe magnetic nanocomposite has hydrophilicity and the ability to swell[30]
SepioliteFeCl2·4H2OHydrothermal The precursor of FeCl2·4H2O solution is heated in an autoclave at 140°C for 4 h in a mixture with NH4OH and sepiolite suspension. Then, the precipitate is dried at 60°C for 24 h[31]
KaolinFeCl3·6H2O–FeSO4·7H2OCo-precipitationThe precursor of FeCl3·6H2O–FeSO4·7H2O solution is stirred at 70°C for 2 h in a mixture with NaOH and a suspension of kaolin. The precipitate is dried at 115°CComposites have well-distributed Fe3O4 nanoparticles, ranging in size from 5.76 to 18.2 nm with a good adsorption capability[32]
KaoliniteFeSO4·7H2OCo-precipitation–microwave irradiationFeSO4·7H2O precursor solution is stirred in a mixture with NaOH and subjected to microwave irradiation (700 W, 2450 MHz) for 10 min. The formed FexOy NPs are mixed with a kaolinite suspension while stirring, and the mixture is dried completely at 40°CFexOy phases–maghemite (γ-Fe2O3) in a mixture with magnetite (Fe3O4) phase are formed and anchored on the edges of the kaolinite[33]
KaoliniteFeCl3·6H2O and FeSO4·7H2O Co-precipitation FeCl3·6H2O: FeSO4·7H2O in a molar ratio of 2:1 is mixed with NH4OH and slowly added to kaolinite. The mixture is stirred for 5 h, followed by drying at 70°C for 24 h[34]
HaloysiteFeCl3·6H2O and FeSO4·7H2OCo-precipitation A suspension of HNT is mixed with FeCl3·6H2O–FeSO4·7H2O, followed by the dropwise addition of NH3H2O solution at 60°C in N2HNT–Fe3O4 has good magnetic properties with a saturation magnetization of 27.91 emu/g at a magnetic field of about 9,000 Oe[35]
Pristine HNTFe(NO3)3⋅9H2OWet impregnationA pristine HNT suspension is stirred with Fe(NO3)3⋅9H2O, followed by the rapid removal of the solvent at 80°C The preparation is calcined for 1 h at 200°C under high-purity argon flow[36]
Magnetic and anionic–cationic modified montmorillonite (Fe3O4–cetyltrimethylammonium chloride–sodium eicosenoate/CTMAC/SEIA-Mt)FeCl3–FeCl2Co-precipitation–surfactant modificationMontmorillonite is intercalated using CTMA and SEIA, prior to co-precipitation using FeCl3–FeCl2 precursor solutionThe material has a great adsorption capacity for the removal of the MB dye and a saturation magnetization of 19.84 emu/g[37]

The co-precipitation method is based on the chemical reaction used to produce magnetic nanoparticles in aqueous clay mineral dispersions, so the nucleation and growth of nanoparticles occur in situ in an aqueous dispersion of clay minerals, as described in Figure 2. The synthesis of nanocomposites by co-precipitation involves mixing clay mineral with MNP precursors under alkaline condition to form a sol–gel system. NH4OH and/or NaOH are commonly used to create the alkaline condition, which directly produces the precipitate of the composite [14,33,34]. The interaction between MNPs produced from clay minerals in a sol–gel system can be intensified using several methods, such as heating in a reflux system or microwave-irradiation. As the precipitate is created, drying or calcination can be conducted, which influences the iron oxide phase and magnetization properties through various processes. Synthesis using Slovakian bentonite has shown that a higher drying temperature (85°) successfully produces the γ-Fe2O3 phase with a magnetization of 35–42 emu/g, while at a lower temperature (20°C), iron oxide presents in the oxo-hydroxide phase (goethite) and has a low magnetization (8–15 emu/g). The combination of co-precipitation and oxidation can also be conducted to find a homogeneous MNP phase [18,38]. Instead of using iron salt as a precursor, an aqueous oxidation using NaNO3 as an oxidant has been used to form Fe3O4 nanoparticles (Fe3O4 NPs). The homogeneous phase of iron oxide can be obtained by conducting precipitation and oxidation under N2 flow and the use of ultrasound-irradiation for the intensification.

Figure 2 Schematic representation of the co-precipitation method.
Figure 2

Schematic representation of the co-precipitation method.

Pillarization is another method of nanocomposite formation (Figure 3). In pillarization, MNPs are formed through the intercalation of polyoxocations or iron oxide oligomer precursors on to the interlayer structure of smectite clay, followed by calcination. For example, Tirelli reported the use of the oligomer trinuclear acetate–hydroxo iron(iii) nitrate, which was obtained through the slow titration of Fe(ii) in alkaline conditions as an MNP precursor [39]. As with the pillarization of other metal oxides, the intercalation of the oligomer into a clay suspension was conducted by stirring vigorously. Mixing iron salt with urea also creates oligomers [26]. The success of clay pillarization can be identified by determining the basal spacing d001, using the basal spacing d001 of smectite clay as a reference.

Figure 3 Schematic representation of clay pillarization.
Figure 3

Schematic representation of clay pillarization.

The pillarization of smectite is advantageous, because it increases its basal spacing and pore distribution, bringing it from micro- to macroporosity. To facilitate the formation of MNPs in the clay structure, montmorillonite that has been pillared with another metal oxide, such as aluminum, silica, or titanium oxide, can be used [23,24,40]. Increasing the specific surface area and pore volume through pillarization using aluminum oxide facilitates the distribution of MNPs, which enhances the adsorption mechanism in contribution for the Photo-Fenton oxidation process of the dye. Measuring saturation magnetization has shown that decreasing the loading of Fe3O4 NPs decreases particle size and saturation magnetization. This trend is analogous with the relationship between the saturation magnetization and coercivity (Hc) of Fe3O4 NPs. A higher Fe3O4 nanoparticle size reflects a higher saturation magnetization and Hc. The low magnetization of materials with a smaller particle size is due to the formation of a magnetically disordered surface as a result of the large surface-to-volume ratio. However, the saturation magnetization values of these composites are still acceptable (23.5–81.2 emu/g), though they are less than those of Fe3O4 nanoparticles (82.7 emu/g). The magnetization, a higher specific surface area, and a resultant lower particle size of the composite for RhB decolorization enhance its adsorption capability and photocatalytic activity [18]. The composite’s iron loading, magnetization, and temperature of calcination significantly affect the size of MNPs [24,40]. In addition, the use of titanium-pillared montmorillonite as a support for MNPs has shown that increasing the temperature of calcination increases particle size and saturation magnetization [24].

Kaolinite is a 1:1 clay structure that has a small capacity for cation exchange and does not swell. Its structure has rarely been reported to involve the intercalation of metal oxides or their precursors. This different structure means that MNPs/kaolinite materials are mainly prepared using the co-precipitation method, which is also used in the production of halloysite, pristine halloysite, and halloysite nanotubes (HNTs), which are within the kaolin–serpentine class of clay. MNPs in the composite could be formed via a similar synthesis route as bentonite, which is produced by mixing precursors with a kaolinite suspension or preparing them separately before their dispersion into the suspension. The combination of co-precipitation and hydrothermal processes for nanoparticle formation has also been reported to produce homogeneously distributed nanoparticles. Different mechanisms of MNP growth have been reported, from impregnation methods to the use of pristine HNTs [36].

The structure of pristine HNTs consists of gibbsite octahedral sheet groups (Al–OH) on the internal surface and siloxane groups (Si–O–Si) on the external surface. This structure results in a negatively charged outer surface and a positively charged inner lumen in solutions with a pH of less than 8.5. The impregnation method applies a charged iron oxide precursor at the outer surface of HNTs. As the precursor on the outer surface is exposed to acetic acid vapor, iron acetate precursor species are formed. Calcination converts these species into smaller sized nanoparticles. Figure 3 shows the nanoparticle formation on the HNT surface.

LDHs are characterized as a porous clay with the potential to form nanocomposites, and their layers and ionic structures have different characteristics. The crystalline structure of LDHs consists of positively charged layers [M2+1−xM3+x(OH)2]x+ similar to the layered structure of brucite (Mg(OH)2) and an interlayered negative region composed of anions and water molecules, An−x/n·mH2O. As a result of this different ionic condition, magnetic nanocomposite formation with LDH usually involves anionic surfactants in the intercalation step [41]. Though the formation of magnetic nanocomposites with hydrotalcite (HT) can be identified by the increasing basal spacing of the interlayered structure, they are mostly synthesized using the co-precipitation method. The formation of magnetic HT reported by Miranda (2014), Lulu (2014), and Zolfaghar (2012) are examples of this method, as are hydrothermal and solvothermal syntheses [41,42,43,44].

Through the co-precipitation method, MNPs are dispersed in the interlayer space of the clay structure, but scanning electron microscope and transmission electron microscope analyses have shown that they are mostly distributed on to the clay surface. Generally, the pH, the temperature, and the concentration of the alkali and iron oxide precursors are critical factors in the synthesis. These factors significantly affect the nucleation and growth of particles. For example, MNPs will have different sizes and surface properties when synthesized from different iron-to-clay mass ratios and at different temperatures of nucleation.

Surface modification has been used to influence MICNCs’ ability to adapt to various pH conditions and hydrophobicities of the treated solution. The formation of hydrogels, hydrophobic magnetic nanocomposites, and surfactant-modified magnetic nanocomposites are three major techniques that have been widely reported. The hydrophobicity of MICNCs can be increased through the formation of Fe3O4–CTMAC/SEIA–Mt. In this process, prior to co-precipitation, montmorillonite is intercalated using cetyltrimethylammonium and sodium eicosenoate. The interlayer space was increased through the use of CTMA as a cationic surfactant. The electrostatic attraction of clay platelets may create an exfoliated composite system, meaning that the surfactant breaks the parallel arrangement. A multi-arrangement consists of monolayers, bilayers, and pseudo trilayers, and a paraffinic structure may be created. In addition, the use of CTMA as a cationic surfactant with SEIA as an anionic surfactant has been proposed as a way to stabilize the hydrophobic interaction of organic molecules at the surface [33].

The hydrogel formation of MICNCs from laponite and montmorillonite has been reportedly conducted by cross-linking the polymerization method [29,30]. As iron oxide/montmorillonite is produced, the hydrogel form is synthesized through the in situ graft copolymerization of acrylamide using potassium persulfate as a free radical initiator and N,N′-methylenebisacrylamide as a cross-linking agent. Polymerization agents were mixed with the nanocomposite suspension. Similarly, MNPs in laponite have been subjected to the cross-linking reaction through the use of ammonium persulfate as a radical initiator with N,N,N′,N′-tetramethylethylenediamine reagent to form poly(N-isopropylacrylamide) hydrogel. Hydrogels have a better solubility, pH stability, and mechanical and diffusion properties, which create a viscous, suspended treated solution with a highly concentrated contamination.

3 Application of MICNCs in water and wastewater treatments

In water treatment, MICNCs have been widely used for the removal of pollutants from aqueous solution, either by adsorption, photooxidation, or by chemical oxidation processes. The reduction and removal of contaminants, including chemical constituents, such as dye, heavy metals, and other organic pollutants from water, have been reported.

3.1 Adsorption

The use of MICNCs for the treatment of water and wastewater via adsorption is more dominant than photocatalysis and advanced oxidation processes (AOPs). The combination of the adsorptive properties of clay minerals with the magnetic properties of MNPs to produce novel MICNC adsorbents is a promising technique for the removal of pollutants from water. Table 2 shows various MICNCs along with their target contaminants and removal processes. The next section discusses each process in brief detail.

Table 2

MICNCs used for adsorption

MICNCsContaminantSaturation magnetization/Ms (emu/g)Isotherm of adsorptionRemoval capacityRef.
Fe3O4/ZnAl–LDHCr(vi)Not presentedLangmuir197.1[45]
MNPs/bentoniteLa3+, Eu3+, and Yb314.0°Langmuir18.4 mg/g for La(iii), 26.1 mg/g for Eu(iii), and 71.4 mg/g for Yb(iii)[46]
Fe3O4/montmorilloniteMethylene blue (MB)Not presentedLangmuir59.9[20]
Graphene/magnetite/montmorilloniteMB63.48Langmuir225.0[47]
Fe3O4/Al-pillared bentoniteHg(ii)22.08Dubinin–Radushkevich (D–R)26.2 mg g−1[48]
Fe3O4 NPs/diatomite and Fe3O4 NPs/illite PO43−35.39Langmuir11.9 mg/g for Fe3O4 NPs/diatomite and 5.48 mg/g for Fe3O4 NPs/illite[21]
Fe3O4/bentoniteEnrofloxacin27.57Not presented 180.0 mg/g[49]
Chitosan/clay/magnetiteCu(ii) and As(V)AdsorptionCu(ii) and As(v) of 17.2 and 5.9 mg g−1 in the initial concentration ranges of 16–656.0 and 17–336.0 mg L−1, respectively[38]
Fe2O3–palygorskiteFenarimolAdsorption 27.8 mg/g[50]
Fe3O4–sepioliteBisphenol APhoto-FentonMaximum removal of 12.0 mg/g at room temperature[51]
Di(2-thylhexly)phosphoric acid–immobilized magnetic GMZ bentoniteEu(iii)Adsorption 40.5 mg/g[52]
Fe3O4/HNTMethylene blue (MB), neutral red (NR), and methyl orange (MO)37.3, 30.6, and 2.5 mg/g for MB, NR, and MO, respectively[35]
Sodium dodecyl sulfate-modified BiOBr/magnetic bentoniteTetracycline and ciprofloxacinPhotocatalysis18.5 mg/g for TC and 34 mg/g for CP [53]
REC–Fe3O4MB and NRAdsorption8.6 mg MB, 16.0 mg NR[54]
Fe3O4/sepioliteAtrazine 31.82Langmuir 15.9[55]
Fe3O4/HNTCr(vi)29.53Not presented38.6[56]
Fe3O4/bentoniteCr(iii)Not presentedLangmuir11.7[57]
Fe3O4/saponiteMalachite green, Congo red, and indigo carmine, Not presentedLangmuir159.1 mg/g for MG, 73.1 mg/g for CR, and 110.3 mg/g for IC[58]
Magnetic bentonite/carboxymethyl chitosan/sodium alginate hydrogel beadsCu(ii) 18.86 emu/gLangmuir56.8 mg/g[59]
MnFe2O4/bentoniteAcid redNot presentedNot presented23.5 mg/g[60]
Fe3O4/kaoliniteCopper, lead, cadmium, chromium, and nickel38.2LangmuirCu2+ = 106.0 mg/g[61]
Pb2+ = 98.0 mg/g
Cd2+ = 100.0 mg/g
Cr2+ = 97.0 mg/g
Ni2+ = 95.2 mg/g
Magnetic attapulgite–biochar composite (MABC)Oxytetracycline31.46Langmuir33.3 mg/g[62]
Fe3O4/bentoniteCd(ii)Not presentedLangmuir63.3 mg/g[14]
Iron oxide–HT modified with the surfactant dodecyl sulfate (DS) and β-cyclodextrin (β-CD) PHE, p-nitrophenol (PNP), and PCSNot presentedLangmuirPHE = 216.1 mg/g PNP = 255.6 mg/g PCS = 272.5 mg/g  [63]
γ-Fe2O3/halloysite Ag nanoparticles18 Langmuir67.9 mg/g[64]
Magnetic and anionic–cationic modified montmorillonite (Fe3O4–CTMAC/SEIA–Mt)Methylene blue 19.84Langmuir211 mg/g[37]
Fe3O4/halloysiteNaphthol green BNot presentedLangmuir11.2 mg/g[65]
Polyethylenimine functionalized magnetic montmorillonite clay (MMT–Fe3O4–PEI)Cr(vi)59.81Langmuir62.9 mg/g[28]
Fe3O4/sepioliteSafranin31.8Langmuir18.5 mg/g[66]
Magnetic core-shell dodecyl sulfate intercalated layered double hydroxide (Fe3O4@DS-LDH)MB and MO25FreundlichMB = 225.0 mg/g[67]
MO = 221.0 mg/g
CTAB-modified Fe3O4/montmorillonite2,6-Dichlorophenol and p-nitrophenol5.4Langmuir 200 mg/g for 2,6-dichlorophenol and 125.0 mg/g for p-nitrophenol[67]
Fe3O4/montmorilloniteMBNot presentedLangmuir 223.0 mg/g[25]
Montmorillonite–Cu(ii)/Fe(iii) oxidesHumic acid3.9Langmuir 98.0 mg/g[68]
Clay/polyaniline/Fe3O4MB36.52Langmuir184.0 mg/g[69]
O,O′-bis(2-aminopropyl)polypropyleneglycol-γ-Fe2O3/montmorilloniteMO26.79.8 mg/g[70]
Fe3O4/bentoniteCo(ii)Not presentedLangmuir10.7 mg/g [71]
Fe2O3/bentonitePicloramNot presentedLangmuir[72]

As seen in Table 2, many modifications have been attempted to enhance the adsorption capability of MICNCs, mainly through surface functionalization. The application of surfactants, polymers, and other compounds containing functional groups on to nanocomposites is effective for attracting the adsorbate. To describe the adsorption behavior, studies have adopted isotherm models, including the Langmuir, Freundlich, and Dubinin–Radushkevich models. As seen in Table 2, the Langmuir isotherm model is the most representative for almost all kinds of adsorbates. The Langmuir isotherm model represents the monolayer adsorption occurring on an energetically uniform surface, on which adsorbed molecules are not interactive. The equilibrium is attained once the monolayer is completely saturated. Contrary to Langmuir, the Freundlich model describes adsorption on an energetically heterogeneous surface, on which adsorbed molecules are interactive. In a different approach, the Dubinin–Radushkevich (D–R) model was constructed, based on the assumption that the adsorption performance is preferable when it occurs in micropores by pore-filling rather than layer-by-layer surface coverage. The D–R model can generally be applied to adsorption that occurs via a van der Waals interaction, for example, the adsorption of Hg(ii) by Fe3O4/Al-pillared bentonite [44]. Three main mechanisms for the adsorption of organic compounds have been identified, which are as follows:

  • a. π–π interactions are those that are available for surface-modified MICNCs, especially by the surfactant. In addition, hydrogen bond formation between MICNCs and double bonds of the adsorbate are usually both present together [37,62]. In a study on the adsorption of oxytetracycline by MABC, adsorption kinetics and Fourier-transform infrared spectroscopy revealed the π–π interaction mechanism. The enthalpy of adsorption at 12.50 kJ/mol represents the physical adsorption interaction dominantly. Moreover, positive values of ΔS° revealed an increasing randomness at the solid–solution interface during the adsorption process. Similarly, the hydrophobic interaction in phenol (PHE), CRE, and p-cresol (PCS) adsorption was presumably from the hydrogen bonds between the dodecyl sulfate/β-cyclodextrin (DS/β-CD) cavity contained in Fe/HT–dodecyl sulfate/β-cyclodextrin (DS/β-CD)Fe/HT–DS/β-CD and the phenolic compounds forming inclusion complexes, which promote selective adsorption.

  • b. Hydrogen bonding corresponds to the interaction between the hydrogen of the hydroxyl group (–C(O)–OH) in dyes or organic compounds and the oxygen atoms in the tetrahedral layer of the montmorillonite surface. Hydrogen bonding dominates when there is an adsorbate electrophilic element in the functional group, such as the nitrogen in, for example, –N(C2H5)2 or the oxygen atom.

  • c. Lewis interaction occurs when the nitrogen atom in the dye or organic molecule, which acts as the Lewis base, combines with the Al3+ and Fe3+ ions on the MICNC surface, which act as the Lewis acid. This molecular dynamic of this interaction is simulated by Ouachtak for the adsorption of rhodamine B and has also been found in the adsorption of picloram herbicide by pillared montmorillonite [73].

A schematic representation of the possible interaction between adsorbate and MICNCs is presented in Figure 5.

Figure 4 Schematic representation of the possible mechanism in adsorption using MICNCs.
Figure 4

Schematic representation of the possible mechanism in adsorption using MICNCs.

Figure 5 Montmorillonite (Mt.)-supported iron shifts base complexes as a catalyst.
Figure 5

Montmorillonite (Mt.)-supported iron shifts base complexes as a catalyst.

In previous research work, FTIR analysis has revealed that the interaction between iron oxide and pillared montmorillonite occurs through the nitrogen of the pyridine ring as a result of the replacement of OH groups from the coordination sphere of iron. As shown in Figure 6, the interaction involves the formation of a bridge complex between COO− ions, nitrogen atoms in pyridine groups, and iron(iii) centers, such as those previously proposed [72].

Figure 6 Schematic representation of the photocatalysis mechanism over MNPs.
Figure 6

Schematic representation of the photocatalysis mechanism over MNPs.

3.2 Photocatalytic and catalytic degradation of organic pollutants

MNPs are capable of oxidizing in AOPs. Traditional AOPs based on hydroxyl radicals (˙OH) and sulfate radicals (SO4˙−) produce strong oxidation radicals for the degradation of organic pollutants in water [74]. Electron excitation in MNPs activates the formation of radicals when MNPs are exposed to a small amount of energy, such as when undergoing thermal treatment. MICNCs are common catalyst carriers with high specific surface areas and good thermal stability and ion-exchange performance. They support the adsorption mechanism via oxidation over a heterogeneous catalyst. Zong et al. (2020) used magnetic clay with persulfate to degrade atrazine. In their study, Fe3O4 was loaded on sepiolite clay to catalyze potassium persulfate (K2S2O8) and hydrogen peroxide (H2O2), generating SO4˙2− and ˙OH for atrazine removal [75]. The composite maintained a good catalytic activity and stability during four consecutive runs. The quenching experiments showed that SO4˙2−/˙OH and ˙OH were the dominant radical species in the two systems.

The photocatalytic activity of MNPs arises from the semiconductor properties of Fe2O3 and Fe3O4. As semiconducting materials, both oxides are promising visible light-driven photocatalysts due to the band gap energy range. Moreover, iron oxides have a low cost and an excellent chemical stability, besides being easy to produce and environment-friendly. They also absorb most visible light. For example, γ-Fe2O3 absorbs light up to 600 nm, collects up to 40% of solar spectrum energy, and is one of the cheapest semiconductor materials. However, the stability of iron oxide photocatalysts is more or less at a pH of more than 3, and depending on the chemical environment, iron oxides may easily lose activity due to corrosion and aggregation.

Table 3

MICNCs for the photocatalytic degradation of organic compounds

MaterialMsProcessTarget compoundDegradation efficiency (%)MNP sizeRef.
Sepiolite/Fe3O4Not givenAOP using K2S2O8Atrazine57.8[75]
Fe3O4/rectorite30.28Wet peroxidationp-Chlorophenol98[76]
Magnetite/HNTsNot givenAOP using NaIO4Pentachlorophenol 8915–30[36]
Fe3O4/montmorillonite27.57AOP using K2S2O8Enrofloxacin9030–150[49]
Fe3O4/montmorillonite78AOP using permonosulfateBisphenol A (BPA)99.345–58 [77]
TiO2/montmorillonite/Fe3O423.96PhotocatalysisMB9445–60[78]
Fe3O4/montmorilloniteNot givenPhotocatalysisBrilliant orange X-GN79.1 (under visible light exposure)Not given[78]
Fe/montmorillonite41 emu/gPhotocatalysisRhB79<10[79]
Fe3O4/palygorskite44.11PhotocatalysisTetracycline72.920–50 [80]
Sepiolite/Fe3O4Not givenPhotocatalysisDiuron 925–20[81]
Sepiolite/Fe3O4Not givenPhotocatalysisBPA872–50[51]
Polypyrrole/HNTs/Fe3O4/Ag/Co nanocompositeNot givenPhotocatalysisMB9110–20[82]
Fe2O3–Fe3O4/montmorilloniteNot givenPhotocatalysisMethyl orange98.810–80[83]
Maghemite/montmorillonite45.61PhotocatalysisPhenol9925–30[84]

Drawbacks of using these oxides in photocatalysis arise from the recombination of separated photo-induced electron–hole pairs due to a low band gap energy. The formation of oxides in nanosize, in combination with the supporting form, has proven effective in improving the separation efficiency of photo-induced electron–hole pairs. According to the method given in Figure 7, as MNP and MICNC photocatalysts are exposed by photons, electrons are excited from the valence band (VB) to the conductance band (CB), leading to the formation of a hole (h+) in the VB. The interaction between h+ and e− in each CB and VB with OH and O2 from the reaction system or solvent produces radicals for further oxidation.

Figure 7 Mechanism of the photocatalytic degradation of organic molecules using iron oxide/clay nanocomposites.
Figure 7

Mechanism of the photocatalytic degradation of organic molecules using iron oxide/clay nanocomposites.

Wang et al. (2017) reported that the formation of Fe2O3–Fe3O4 nanocomposites supported by montmorillonite increased the band gap energy [83]. Fe2O3–Fe3O4/Mt has a band gap energy of 2.85 eV, while pure Fe2O3–Fe3O4 has a band gap energy of 2.14 eV. Increasing the band gap energy increases the photocatalytic degradation of Fe2O3–Fe3O4/Mt by methyl orange which is higher compared to the pure one. The composite shows a 1.61-fold degradation rate, compared to pure Fe2O3–Fe3O4, and 98.8% recoverability by magnetic separation. Figure 4 shows a schematic representation of the photocatalytic degradation of organic molecules by MNP and MICNC photocatalysts.

Bledowski et al. reported that the redox potential of the CB of Fe2O3 is around 0.2 eV and that because the band gap energy of MICNCs is 2.85 eV, the VB is located at 3.15 eV. The CB has a lower redox potential than the formation of superoxide anion radicals (O2˙−) [E0(O2/O2˙−) = −0.33 eV. The spontaneous formation of O2˙− and HOO˙− arises, because O2 interacts with excited electrons. Moreover, the interaction of the electron hole with H2O to produce HO˙ occurs, because the VB has a higher potential reduction than the oxidation of water [E0 (H2O/˙OH) = 2.38 V] [86]. These generated radicals are effective oxidants for the degradation of dyes and organic compounds. A further oxidation reaction releases CO2, H2O, NO3−, and SO3− upon completion. In addition, fast degradation can be achieved through the addition of an oxidant, mainly H2O2. Interactions between H2O2 and the surface of MICNCs are mainly initiated by the following chain of reactions:

H2O2+≡Fe(II)→≡Fe3+OH+OH−≡Fe3++H2O2→≡Fe3+(H2O2)≡Fe3+(H2O2)→(≡Fe2+⋅O2H)(≡Fe2+⋅O2H)→≡Fe2++HO2˙/HO2˙−

In addition, ˙OH, HO2˙/HO2˙− ions are generated through the reactions, which are responsible for the reversible conversion between Fe2+ and Fe3+. Furthermore, modifications on to iron oxide/clay have been reported concerning the catalyst and photocatalyst stabilization and surface modification to improve hydrophobicity.

Electronic features of dispersed Fe have been studied by Bao et al. [76], who showed that the amount and location of iron oxide nanoparticles in MICNCs are critical parameters in determining the shape, size, and crystal structure of nanoparticles, which correlate with their magnetization. It was concluded that the zero valence and large surface area of iron oxide nanoparticles create a high level of photocatalytic activity. The larger specific surface area facilitates an intensive interaction in the oxidation mechanism, and the calcination process creates a particle size uniformity and a strong interaction of iron oxide with the clay support. The strengthened interaction of iron oxide with a silica–alumina framework in the clay support reduces iron leaching, giving it a stable activity for consecutive usage as shown by the Fenton-like phenol degradation. Increasing calcination temperature increases particle size, and at certain temperatures, it affects iron oxide agglomeration and phase change [84].

Visible light sensitization is a popular and efficient photocatalysis mechanism that saves energy. The materials doping with Ag, Co, and TiO2 in small portions significantly enhance photocatalytic activity through the inhibition of electron recombination [78,82]. As photocatalysts have good capability in the visible light region, this photocatalytic process could be sunlight-driven.

4 Physicochemical character of MICNCs

Specific surface area and pore distribution are important parameters in adsorbent and photocatalyst applications for water treatment [60]. The higher specific surface area provides more adsorption sites for interacting with target molecules. The Brunauer–Emmett–Teller approach calculated from the N2 adsorption/desorption isotherm data is a generally acceptable method for this calculation. However, specific surface area and pore size distribution are not the most influential parameters for removal efficiency, as surface hydrophobicity and hydrophilicity also play roles in the interaction [27].

In practice, several factors influence intensive adsorption, such as pH, adsorbent/catalyst dosage, time of treatment, and so on. For example, pH determines the efficiency of surface–adsorbate bonding, which is an important step in adsorption, and it depends on the zeta potential of the adsorbent surface. The zeta potential is correlated with saturation magnetization. Measurements of zeta potential in solutions under the influence of magnetic fields have shown that increasing the field greatly influences the adsorption of dyes and metals, with larger field strengths creating more adsorption [25,49]. Magnetic fields exert much influence on the adsorption of dyes, as shown by their increase of removal and adsorption capacity. In addition, increasing nanoparticle size increases saturation magnetization [87]. Nanoparticle size analysis can be carried out using transmission electron microscopy (Table 3).

Szabo concluded that the lamellar sizes and cation exchange capacities of clay minerals affect MNP growth and magnetization. Comparing the formation of MNPs in laponite with their formation in montmorillonite showed that the size effect and greater amount of aggregation in laponite composites were related to the dominance of the maghemite phase due to the greater contribution of attractive dipolar interactions between magnetic nanocrystals [87]. Compared to laponite, montmorillonite sheets accommodated the formation of nanoparticles, while in the laponite, formed particles had the tendency to produce highly exfoliated clay lamellae. Thus, MNPs in laponite have a higher saturation magnetization than MNPs in montmorillonite. Saturation magnetization data have shown that the following factors significantly influence the properties of MICNCs:

  • a. MNP content and phase.

  • b. Average particle size of MNPs, size distribution, and aggregation state.

  • c. Specific surface area and the porous structure of clay.

  • d. Homogeneous/heterogeneous dispersion of iron oxide crystals in the clay matrix.

Figure 8 shows the effect of the iron content in iron oxide on montmorillonite-based MICNCs with saturation magnetization recapitulated from several references. In general, the higher the iron content in MICNCs, the higher the saturation magnetization. Higher particle sizes and the formation of more aggregates tend to give a higher saturation magnetization, and a higher calcination temperature enhances saturation magnetization [24,79]. The MNP size depends on the amount of iron precursors and the growth of iron oxide crystallite. As the growth of nanoparticles occurs in the layers of the clay structure, layer charge, and porous and surface structure are crucial factors that suppress nanoparticle formation. Nanoparticle formation is also controlled by temperature, especially in the synthesis of iron oxide-pillared clay, as a phase change from γ-Fe2O3 to α-Fe2O3 may occur, which affects magnetization properties. α-Fe2O3 decreases magnetization, while the presence of zerovalent iron (Fe0) in MICNCs increases magnetization [84,88].

Figure 8 Effect of the iron content on saturation magnetization in montmorillonite-based MICNCs.
Figure 8

Effect of the iron content on saturation magnetization in montmorillonite-based MICNCs.

Surface characteristics, including hydrophobicity, pore distribution, pore radius, and nanoparticle distribution, are critical parameters in the proposed MICNC interactions in the adsorption mechanism. Theoretically, higher specific surface areas provide more space for adsorption. The data presented in Table 1 show that the insertion of MNPs into clay structure oxides changes the specific surface area of the composite. As with magnetization, iron content influences porous distribution and thus, the specific surface area of the composite. However, dispersion method, including pillarization, co-precipitation, and impregnation, is a more important factor than the iron content. The MNPs are distributed as metal oxide pillars in the pillarization method, while co-precipitation and impregnation position nanoparticles in the interlayer or at the edge of silica or alumina layers [27,88]. The cation exchange capacity and surface area of raw clay, as well as the layered structure, calcination temperature, and dispersion method, strongly influence the specific surface area of the composite. As there are so many additional factors, there is no strict relationship between magnetization and the specific surface area of MICNCs.

The terms recoverability and sustainability of the adsorbent and photocatalyst materials are proven by reusability. In most reported works, the durability of the materials until a minimum of five cycles with less reduction of removal activity has been presented. However, in photocatalytic applications, electronic transition may affect changes in the electronic state of MNPs in a nanocomposite. X-ray photoelectron spectroscopy is an effective method for predicting the change in speciation.

5 Future of MICNCs

MICNC syntheses and applications in water and wastewater treatments have been well studied and have been used in various ways to deal with pollutant-containing water. Research work has shown that incorporating functional MNPs into clay structures has resulted in stable adsorbent, catalyst, and photocatalyst materials, which have increased recoverability and sustainability in the treatment process. However, to our knowledge, research work has not addressed large-scale applications of this technology. Thus, we have recommended that researchers study large-scale production and implementation, including the following:

  • a. Research works should address the technical form of materials in large-scale processes. Although the adsorption capability of MICNCs has been discussed, findings have been limited to a laboratory setting. Modeling and simulation have shown that the performance of materials on a larger scale may vary from that on a smaller scale due to changes in material activity and the economic cost of the process.

  • b. Studies should recalculate the economic availability of technologies using MICNCs. The main factors for redesigning systems and technology in water and wastewater treatments are pH and the chemical and biological stability of the water treated.

  • c. Consideration should be given to potential secondary pollution and further treatment.

  1. Conflict of interest: Authors declare no conflict of interest.

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Received: 2020-06-07
Revised: 2020-07-13
Accepted: 2020-07-17
Published Online: 2020-09-08

© 2020 Ganjar Fadillah et al., published by De Gruyter

This work is licensed under the Creative Commons Attribution 4.0 International License.

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  159. Advancing biodiesel production from microalgae Spirulina sp. by a simultaneous extraction–transesterification process using palm oil as a co-solvent of methanol
  160. Topical Issue on Applications of Mathematics in Chemistry
  161. Omega and the related counting polynomials of some chemical structures
  162. M-polynomial and topological indices of zigzag edge coronoid fused by starphene
https://doi.org/10.1515/chem-2020-0159
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iron oxide; magnetic; nanomaterials; photocatalyst
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Artikel in diesem Heft

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  160. Topical Issue on Applications of Mathematics in Chemistry
  161. Omega and the related counting polynomials of some chemical structures
  162. M-polynomial and topological indices of zigzag edge coronoid fused by starphene
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