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Article

Engineering of Iron-Based Magnetic Activated Carbon Fabrics for Environmental Remediation

by
Hai Haham
1,
Judith Grinblat
1,
Moulay-Tahar Sougrati
2,
Lorenzo Stievano
2 and
Shlomo Margel
1,*
1
Institute of Nanotechnology and Advanced Materials, Department of Chemistry, Bar-Ilan University, Ramat-Gan 52900, Israel
2
Institute Charles Gerhardt (UMR 5253 CNRS), Université Montpellier 2, CC 1502, Place E. Bataillon, Montpellier 34095, Cedex 5, France
*
Author to whom correspondence should be addressed.
Materials 2015, 8(7), 4593-4607; https://doi.org/10.3390/ma8074593
Submission received: 4 June 2015 / Revised: 30 June 2015 / Accepted: 10 July 2015 / Published: 22 July 2015
(This article belongs to the Section Advanced Materials Characterization)
Browse Figures
Versions Notes

Abstract

:
Magnetic Fe3O4, Fe and Fe/Pd nanoparticles embedded within the pores of activated carbon fabrics (ACF) were prepared by impregnation of the ACF in iron acetylacetanoate (Fe(acac)3) ethanol solution, followed by thermal decomposition of the embedded iron precursor at 200, 400 and 600 °C in an inert atmosphere. The effect of the annealing temperature on the chemical composition, shape, crystallinity, surface area, pore volume, and magnetic properties of the various functionalized ACF was elucidated. The Fe nanoparticles within the ACF were also doped with tinier Pd nanoparticles, by impregnation of the Fe/ACF in palladium acetate ethanol solution. The potential use of the functionalized ACF for removal of a model azo-dye, orange II, was demonstrated. This study illustrated the enhanced removal of the dye from an aqueous solution according to the following order: Fe/Pd/ACF > Fe/ACF > ACF. In addition, the enhanced activity of Fe3O4/ACF in the presence of increasing concentrations of H2O2 (Fenton catalysts) was also illustrated.

Graphical Abstract

1. Introduction

Zerovalent Iron (Fe) and iron oxides (IO) are among the most useful ferromagnetic and ferrimagnetic elements. Fe has the highest magnetic moment at room temperature, a high Curie temperature, and is significantly cheaper than other ferromagnetic elements such as nickel and cobalt [1]. In addition to their unique magnetic properties, IO and Fe nanoparticles are chemically reactive and therefore are good candidates for many environmental remediation applications [2,3].
Previous studies have shown that in the presence of hydrogen peroxide, IO generates free hydroxyl radicals (·OH) that degrade most organic pollutants quickly and non-selectively [4]. Fe nanoparticles were reported to be efficient in the transformation of a wide variety of common organic contaminants such as organic dyes [5], chlorinated organic solvents [6] and fire retardants [7]. Furthermore, Fe nanoparticles doped with an appropriate catalytic metal such as Pd, Pt or Ni demonstrate enhanced elimination activity on many classes of organic pollutants such as azo-dyes and polychlorinated biphenyls [6,8,9].
Preserving the stability of Fe nanoparticles is considered a major challenge, since Fe nanoparticles get oxidized rapidly in water and air, resulting in loss or decrease of magnetism and dispersibility [1,10,11]. To overcome this phenomenon, Fe nanoparticles are usually protected by a protection layer made of polymers [12] carbon [13,14,15], silica [10] or alumina [16]. Previous research showed the efficiency of air-stable iron/carbon (Fe/C) nanomaterials in the removal of heavy metal ions and chlorinated hydrocarbons from water [17,18,19,20]. Such combinations of Fe nanoparticles with the advantages of carbon materials [21], e.g., porous structure and large surface area [22,23], may hold a great potential for adsorptive-reactive water treatment processes [18,24,25,26].
Disposal of dye-contaminated wastewater is a major environmental challenge faced by the textile, dyeing, printing, ink, and related industries [27,28,29]. Dyes are known pollutants that reduce light penetration into water, have an inhibiting effect on photosynthesis, and some are considered toxic and even carcinogenic [30,31].
The present manuscript presents a surfactant-free synthesis which combines the advantages of carbon materials, Fe3O4 and Fe nanoparticles for environmental applications. Iron oxides and Fe nanoparticles were prepared in situ within the pores of activated carbon fabrics (ACF) of a large surface area (1300 m2·g−1) by thermal decomposition of iron acetylacetanoate, Fe(acac)3, embedded in ACF at 200, 400 or 600 °C in an inert atmosphere. The chemical composition, surface area, crystallinity, and magnetic properties of the various functionalized ACF were controlled as a function of the annealing temperature. Doping of the Fe/ACF with smaller Pd nanoparticles was accomplished by reduction of Pd2+ ions onto the Fe nanoparticles embedded within the ACF. The removal rate of a model azo-dye, orange II, by the pristine ACF, Fe3O4/ACF, Fe/ACF, and Fe/Pd/ACF was also studied.

2. Experimental Part

2.1. Materials

All reagents were purchased from commercial sources and used without further purification, as follows: iron (III) acetylacetanoate, Fe(acac)3, (>99.9%), orange II (>85%) and ethanol (Sigma-Aldrich, Rehovot, Israel). Palladium acetate, Pd(acet)2, (>95%) (Sterm-Chemicals, Newburyport, MA, USA). Large surface area porous ACF (areal density: 170 g·m−2; thickness: 0.6 mm; surface area: 1300 m2·g−1) (Kynol, Hamburg, Germany).

2.2. Synthesis of Iron Oxides and Fe Nanoparticles within the ACF

ACF (240 mg) were cleaned with water and then dried at 120 °C for 30 min. The washed ACF was soaked in 10 mL of 1% Fe(acac)3 ethanol solution and then heated at 70 °C for 30 min for the removal of entrapped air and, thereby, enhancing the adsorption of the iron precursor within the ACF pores. After evaporation of the ethanol and cooling to room temperature, the impregnated ACF was soaked in distilled water in order to remove excess reagents, and then annealed at 200, 400 or 600 °C for 4 h in Ar, for the thermal decomposition of the absorbed Fe(acac)3. The obtained functionalized ACF were then extensively washed from excess reagents with ethanol and then dried.

2.3. Doping Pd Nanoparticles onto the Fe/ACF

Deposition of tinier Pd nanoparticles onto the Fe nanoparticles embedded within the ACF pores was accomplished by reduction of Pd2+ onto the Fe surface, as reported previously [9,32]. Briefly, 200 mg of the Fe/ACF were immersed in 10 mL of 0.1% Pd(acet)2 ethanol solution. After agitation at room temperature for 10 min, the Fe/ACF were washed from excess reagents with ethanol and then dried.

2.4. Characterization of the Various ACF

The thermal behavior of Fe(acac)3 was measured by Thermo Gravimetric Analysis (TGA) and Differential Scanning Calorimeter (DSC) (STAR-1 System, Mettler Toledo, Columbus, OH, USA) in an inert atmosphere at a heating rate of 5 °C·min−1. Surface morphology was characterized by FEI, Magellan 400 L high-resolution scanning electron microscopy (HRSEM) (JEOL, JSM-840, Tokyo, Japan) of iridium-coated samples. X-ray diffraction (XRD) patterns were recorded using an X-ray diffractometer (model D8 Advance, Bruker AXS, Ness Ziona, Israel) with Cu Ka radiation. 57Fe Mössbauer studies were performed using a conventional constant acceleration spectrometer. The velocity calibration was performed using a room temperature α-Fe absorber, and the isomer shift values are given relative to α-Fe. The collected spectra were least-square fitted by appropriate combinations of Lorentzian profiles corresponding to non-equivalent iron environments. Cross-section samples were characterized by high-resolution transmission electron microscope (HRTEM) (JEOL-2100, JEOL, Tokyo, Japan) operating at 200 kV. The HRTEM is integrated with a digital scanning transmission electron microscope (STEM) comprising annular dark and bright field detectors and with a Noran System Six energy-dispersive X-ray spectrometer (EDS) system for elemental analysis. For structural analysis, nanobeam electron diffraction (NBD) and selected area electron diffraction (SAED) techniques were used. Cross-section samples were prepared using focused ion beam (FIB, FESEM; FEI, Helios 600, Hillsboro, OR, USA). For this purpose, a protective layer of platinum was deposited on top of the analyzed material surface. C, H, N and O analysis of the various ACF was performed using an elemental analysis instrument (model FlashEA1112 Instruments, Thermoquast, Austin, TX, USA). Fe and Pd concentrations were determined by inductive coupled plasma (ICP) (ULTIMA-2, HORIBA-Jovin-Yivon, Kyoto, Japan) measurements after dissolving the Fe3O4, Fe and Fe/Pd compounds embedded within the ACF in concentrated HCl solution. The surface area of the pristine and the various functionalized ACF were measured by N2 adsorption-desorption isotherms and calculated according to Brunauer–Emmet–Teller (BET) method [33] (NOVA 3200E Quantachrome, Pale Lane, UK). Total pore volume values of the pristine and functionalized ACF were calculated by measuring the maximum amount of condensed N2 adsorbed into the ACF in pressure equilibrium. Knowing the density of the adsorbate, one can calculate the volume it occupies and, consequently, the total pore volume of the various ACF [34]. Room temperature magnetization measurements were performed using Microsense V-VSM vibrating scanning magnometer (VSM) (Microsense, Lowell, MA, USA) with field ranging from −10,000 to 10,000 Oe. Raman spectroscopy (HORIBA Jobin Yvon, Kyoto, Japan) measurements were carried out using an Ar ion laser (power = 10 mW and wavelength = 632.8 nm). The exposure and data acquisition times were 20 and 2 s, respectively. Spectrophotometric measurements were performed using a Cary 100 UV–visible spectrophotometer (Agilent Technologies Inc., Santa Clara, CA, USA).

2.5. Environmental Activity

In order to study the use of Fe3O4/ACF as a Fenton catalyst for decomposition of orange II room temperature kinetics experiments were performed. For this purpose, in each tube a piece of 2 × 1 cm2 of Fe3O4/ACF was agitated in 25 mL of 20 mg·L−1 orange II aqueous solution, in the absence and presence of H2O2 (1%, 2% and 3% w·v−1). After each time interval, 0.5 mL of the solution was removed from the solution. The concentration of orange II was then determined by measuring its absorbance at 484 nm. Similar experiments in the absence of H2O2 were also carried out with the pristine ACF, Fe/ACF and Fe/Pd/ACF. The results of each experiment represent the average of four repetitions with maximal standard deviation of 4%.

3. Results and Discussion

3.1. Characterization of The Functionalized ACF

Large surface area porous ACF were functionalized with various iron-based nanoparticles for water clean-up applications. A scheme describing the synthetic route of the various nanoparticles is illustrated in Figure 1.
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Figure 1. Illustration of the synthetic route of the iron-based functionalized ACF.
Figure 1. Illustration of the synthetic route of the iron-based functionalized ACF.
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A TGA thermogram (Figure 2A) of Fe(acac)3 indicates that this precursor starts to decompose at 186 °C with 76% weight loss between 186–680 °C. The DSC curve of Fe(acac)3 (Figure 2B) is compatible with the TGA behavior displaying an endothermic decomposition peak around 186 °C, as reported in the literature [35]. We also noticed almost a complete thermal decomposition of Fe(acac)3 after 4 h of heating at 200 °C in an inert atmosphere.
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Figure 2. TGA (A) and DSC (B) thermograms of Fe(acac)3 obtained by heating the Fe precursor at a rate of 5 °C·min−1 in inert atmosphere.
Figure 2. TGA (A) and DSC (B) thermograms of Fe(acac)3 obtained by heating the Fe precursor at a rate of 5 °C·min−1 in inert atmosphere.
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Figure 3 exhibits HRSEM images of the non-functionalized (pristine) and the various-functionalized ACF. This figure clearly shows that the annealing temperature of the Fe(acac)3/ACF strongly influences the morphology, structure, and distribution of the formed nanoparticles within the various ACF pores. HRSEM image of the pristine ACF (Figure 3A) shows a distinct porous texture. Thermal decomposition of Fe(acac)3/ACF at 200 °C (Figure 3B) resulted in a non-homogenous film coating on the ACF. This film coating is probably generated from agglomerated nanoparticles. Thermal decomposition of the Fe(acac)3/ACF at 400 °C (Figure 3C) and 600 °C (Figure 3D) exhibit the formation of well-defined nanoparticles embedded within the ACF pores.
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Figure 3. HRSEM images of pristine ACF before impregnation with the Fe(acac)3 (A); and after impregnation, followed by thermal annealing at 200 °C (B); 400 °C (C); and 600 °C (D) in inert atmosphere according to the experimental section.
Figure 3. HRSEM images of pristine ACF before impregnation with the Fe(acac)3 (A); and after impregnation, followed by thermal annealing at 200 °C (B); 400 °C (C); and 600 °C (D) in inert atmosphere according to the experimental section.
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The crystalline and non-crystalline nature of the various-functionalized ACF was investigated by XRD (Figure 4) and Mössbauer spectroscopy (Figure 5). Thermal decomposition of Fe(acac)3 within the ACF at 200 °C in Ar resulted in a flat XRD pattern (Figure 4A), indicating the amorphous state of the formed iron phases. Room temperature 57Fe Mössbauer spectrum of the same sample (Figure 5A) presents a single quadrupole doublet (blue) which may be attributed to ill-defined paramagnetic IO species [13,36]. The isomer shift and quadrupole splitting of this doublet (0.39 and 0.77 mm·s−1, respectively) are characteristic to high-spin Fe3+ in oxygen environment [37]. Since many possible nano-sized trivalent iron oxides polymorphs (e.g., α-Fe2O3, β-Fe2O3, etc.) provide similar hyperfine parameters [38], this iron phase is marked for simplicity as “IIO” (ill-defined iron oxide), as shown in Table 1.
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Figure 4. XRD patterns of Fe(acac)3/ACF annealed at 200 °C (A); 400 °C (B); and 600 °C (C) for 4 h in Ar prepared as described in the experimental section.
Figure 4. XRD patterns of Fe(acac)3/ACF annealed at 200 °C (A); 400 °C (B); and 600 °C (C) for 4 h in Ar prepared as described in the experimental section.
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Materials 08 04593 g005 1024
Figure 5. Mössbauer spectra of Fe(acac)3/ACF annealed at 200 °C (A); 400 °C (B); and 600 °C (C) for 4 h in Ar prepared as described in the experimental section.
Figure 5. Mössbauer spectra of Fe(acac)3/ACF annealed at 200 °C (A); 400 °C (B); and 600 °C (C) for 4 h in Ar prepared as described in the experimental section.
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Thermal decomposition of Fe(acac)3 within the ACF at 400 °C in Ar resulted in an XRD pattern with diffraction profiles at 2θ 30.3 (220), 35.4 (311), 43.4 (400), 53.8 (422), 57.5 (511) and 62.5 (440) (Figure 4B). Such pattern corresponds to the spinel structure of Fe3O4 or γ-Fe2O3. Mössbauer spectrum of the same sample (Figure 5B) distinguishes Fe3O4 from γ-Fe2O3, showing evidence of partially oxidized Fe3O4. This Mössbauer spectrum is fitted with three spectral components; two magnetic sextets (orange and green) and one paramagnetic quadrupole doublet (blue). The two sextets have isomer shifts of 0.67 and 0.38 mm·s−1, hyperfine fields 450 and 489 kOe and an intensity ratio of about 1:2, respectively. The first sextet is typical for Fe2.5+ sites in Fe3O4 whereas the second sextet is characteristic to Fe3+ in both Fe3O4 and γ-Fe2O3. The observed intensity ratio indicates a large excess of Fe3+ compared to pure Fe3O4, indicating the presence of a mixture of Fe3O4 and γ-Fe2O3. Indeed, the stoichiometry parameter xm = 0.2 (defined as xm = Fe2+/Fe3+) is characteristic of partially oxidized magnetite with nominal formula Fe2.8O4. Finally, the paramagnetic doublet is similar to that observed at 200 °C, and can be attributed to the ill-defined IO species mentioned above.Table 1 summarizes the composition of the iron species obtained after annealing of the Fe(acac)3/ACF at 400 °C, as follows: 65.2% Fe3O4 and 34.8% IIO. Recapping the XRD and Mössbauer data suggests that the nanoparticles obtained within the ACF are mainly composed of FCC Fe3O4 with a unit cell parameter of 8.37 Å.
Table
Table 1. Mössbauer spectroscopy parameters and phase composition of the Fe(acac)3/ACF annealed at 200 °C (A, B), 400 °C (C, D) and 600 °C (E, F) for 4 h in Ar. IS, QS, LW and H are isomer shift (relative to α-Fe), quadrupole splitting, linewidth, and hyperfine field, respectively.
Table 1. Mössbauer spectroscopy parameters and phase composition of the Fe(acac)3/ACF annealed at 200 °C (A, B), 400 °C (C, D) and 600 °C (E, F) for 4 h in Ar. IS, QS, LW and H are isomer shift (relative to α-Fe), quadrupole splitting, linewidth, and hyperfine field, respectively.
Temp (°C)IS (mm·s−1)QS (mm·s−1)LW (mm·s−1)H (kOe)Composition (wt.%)
2000.390.770.470100 IIO
4000.3800.5448965.2 Fe3O4
0.6700.54450
0.380.880.62034.8 IIO
6000.391.151.02067.1 Fe
0.290.020.6550119.2 Fe3O4
0.530.110.65473
000.3533513.8 IIO
Annealing of the Fe(acac)3/ACF at 600 °C in Ar resulted in the formation of α-Fe, easily identified by the XRD pattern shown in Figure 4C. In fact, the peaks at 2θ = 45.1 (110), 65.7 (200) and 83.3 (211) match the crystal plane of cubic BCC structure of α-Fe with a unit cell parameter of 2.84 Å. Mössbauer spectrum of the same sample (Figure 5C) displays the dominant magnetic sextet of α-Fe (red) centered at 0.01 mm·s−1. In addition to α-Fe, less-intense magnetically split components at higher fields indicate the presence of Fe3O4. Also in this case, a minor paramagnetic quadrupole doublet with the hyperfine parameters of IO is present, probably representing ill-defined amorphous IO. The hyperfine parameters of these components are summarized in Table 1. The iron species composition, as presented in Table 1, is 67.1%, 19.2% and 13.8% for α-Fe, Fe3O4 and IIO, respectively. These findings indicate that the obtained Fe/ACF contains mainly α-Fe phase.
Further investigation related to the morphology and the structure of the Fe/ACF was obtained by cross-section TEM analysis. For this purpose, the Fe/ACF sample was coated with a protective layer of Pt and then sliced by FIB. Figure 6A,B show that the Fe/ACF cross-section comprising two populations of nanoparticles that vary in size and shape according to their location; at the surface of the ACF and within the ACF core. The line-scan profile of the elemental Fe from the surface of the ACF into its core (Figure 6C) is consistent with the observations by STEM (Figure 6A) and the elemental mapping (Figure 6B), indicating the presence of two populations of nanoparticles, as mentioned above. Additional selected area electron diffraction (SAED) of the Fe/ACF (Figure 6D) shows reflections matching the interplanar spacing of d110, d220 and d211 of α-Fe (α-Fe, a = 2.86 Å, BCC, PDF# No. 04-007-9753).
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Figure 6. (A) A cross-section STEM micrograph of the Fe/ACF coated with a protective layer of Pt, as described in the experimental section; (B) elemental mapping of the Fe nanoparticles within the ACF; (C) Elemental line-scan profile (red arrow) displaying spatial distribution of the Fe (green) of the cross-section Fe/ACF; (D) Selected area electron diffraction of the Fe/ACF.
Figure 6. (A) A cross-section STEM micrograph of the Fe/ACF coated with a protective layer of Pt, as described in the experimental section; (B) elemental mapping of the Fe nanoparticles within the ACF; (C) Elemental line-scan profile (red arrow) displaying spatial distribution of the Fe (green) of the cross-section Fe/ACF; (D) Selected area electron diffraction of the Fe/ACF.
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TEM micrograph of the nanoparticles at the surface of the ACF (Figure 7A) exhibits wide distributed nanoparticles with average diameter 85 ± 20 nm, depending on the pore size. The data obtained from the HRTEM suggests for these nanoparticles a structure of α-Fe nanoparticle coated with a thin IO layer, as shown in Figure 7B. Figure 7C shows magnified lattice fringes obtained from the area marked by the white square in Figure 7B which match the interplanar spacing d110 of BCC α-Fe (d = 0.203 nm). In addition, a nanobeam diffraction (NBD) pattern shows the sets of reflections which can be uniquely indexed on the basis of the BCC structure of α-Fe (Figure 7D). Recapping the observed HRTEM data indicate Fe nanoparticles coated with a thin layer of IO at the surface of the ACF.
The magnetic properties of the functionalized ACF were studied by room temperature VSM magnetization loops, as shown in Figure 8 and summarized in Table 2. The magnetization loops of Fe3O4/ACF and Fe/ACF display ferromagnetic response with magnetization saturations (Ms) of 2.00 and 3.25 emu·g−1 and coercivity values of 270 and 80 Oe, respectively. It should be noted that the relatively low Ms values of the Fe3O4/ACF and Fe/ACF compared to the reported bulk values of the Fe3O4 and Fe [1], arise from the non-magnetic carbon content, as reported previously [39]. The IIO/ACF magnetization loop displays a magnetic response which is proportional to the applied magnetic field, thus shows no Ms. Supporting this observation, the Mössbauer analysis suggests a paramagnetic phase within the IIO/ACF (Figure 5).
The pristine ACF, IIO/ACF, Fe3O4/ACF, and Fe/ACF differ in the Fe content, surface area, and pore volume as shown in Table 2. The Fe content of the various functionalized ACF is 11.9%, 10.7% and 9.7% for IIO/ACF, Fe3O4/ACF and Fe/ACF, respectively. Surface area values of the various ACF decreased from 1292 for the pristine ACF to 572, 718 and 880 m2·g−1 for the IIO/ACF, Fe3O4/ACF and Fe/ACF, respectively. The same trend was also observed for the total pore volume values that decreased from 0.70 for the pristine ACF to 0.32, 0.40 and 0.52 cm3·g−1 for the IIO/ACF, Fe3O4/ACF and Fe/ACF, respectively. These results arise two main observations: First, the obtained nanoparticles fill the ACF pores and thus decrease the surface area and pore volume of the pristine ACF. Second, the surface area and pore volume increase with the annealing temperature (e.g., 0.32, 0.40 and 0.52 cm3·g−1 for 200, 400 and 600 °C, respectively). This observation is consistent with the increase in nanoparticle density with increasing temperature, as illustrated in the HRSEM images shown in Figure 3.
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Figure 7. Cross-section TEM and HRTEM analysis of the Fe/ACF samples: (A) TEM micrograph of the Fe/ACF surface; (B) HRTEM image of a thin IO layer (white arrow) coating the α-Fe nanoparticle; (C) Magnified HRTEM image of the area marked by the white square (inset B) displaying lattice fringes of α-Fe; (D) NBD taken from 4 nm diameter displaying sets of reflections matching the structure of α-Fe.
Figure 7. Cross-section TEM and HRTEM analysis of the Fe/ACF samples: (A) TEM micrograph of the Fe/ACF surface; (B) HRTEM image of a thin IO layer (white arrow) coating the α-Fe nanoparticle; (C) Magnified HRTEM image of the area marked by the white square (inset B) displaying lattice fringes of α-Fe; (D) NBD taken from 4 nm diameter displaying sets of reflections matching the structure of α-Fe.
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Figure 8. Room temperature magnetization loops of IIO/ACF, Fe3O4/ACF and Fe/ACF obtained as described in the experimental part. A magnified magnetization loop of the IIO/ACF is also presented in the right inset.
Figure 8. Room temperature magnetization loops of IIO/ACF, Fe3O4/ACF and Fe/ACF obtained as described in the experimental part. A magnified magnetization loop of the IIO/ACF is also presented in the right inset.
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Table
Table 2. A comparison between the chemical/physical properties of the pristine ACF, IIO/ACF, Fe3O4/ACF, and Fe/ACF obtained according to the experimental section.
Table 2. A comparison between the chemical/physical properties of the pristine ACF, IIO/ACF, Fe3O4/ACF, and Fe/ACF obtained according to the experimental section.
SampleFe (wt.%)Composition (%)Ms (emu·g−1)Coercivity (Oe)Surface Area (m2·g−1)Pore Volume (cm3·g−1)Raman (Id/Ig)
ACF––––12920.701.23
IIO/ACF11.9100 IIO––5720.321.29
Fe3O4/ACF10.765.2 Fe3O4
34.8 IIO		2.002757180.401.31
Fe/ACF9.767.1 Fe
13.8 IIO
19.2 Fe3O4		3.25808800.521.36
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Figure 9. Raman spectra the pristine ACF, IIO/ACF, Fe3O4/ACF and Fe/ACF obtained as described in the experimental section.
Figure 9. Raman spectra the pristine ACF, IIO/ACF, Fe3O4/ACF and Fe/ACF obtained as described in the experimental section.
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The Raman spectra of pristine ACF and of the various functionalized ACF are presented in Figure 9. All of the ACF possess two main peaks around 1330 cm−1 (D band) and 1580 cm−1 (G band). The G band is associated with the E2g stretching vibrations in the basal-plane of graphite [40,41], while the D band is explained as a disorder-induced lattice distortion, or an amorphous C background signal [42]. A comparison between the intensity ratios of the D band (Id) and the G band (Ig) shows an increase of Id/Ig from 1.23 for the pristine ACF to 1.29, 1.31, 1.36 for the IIO/ACF, Fe3O4/ACF and Fe/ACF, respectively (Table 2). This probably indicates that increasing the annealing temperature leads to a slight increase in the content of amorphous carbon compared to graphitic carbon.

3.2. Doping of The Fe/ACF with Tinier Pd Nanoparticles

Attachment of smaller Pd nanoparticles onto the surface of the Fe nanoparticles was conducted in order to enhance the environmental activity of the Fe/ACF towards organic pollutants. The deposition of the tinier Pd nanoparticles onto the Fe nanoparticles embedded within the ACF pores was verified qualitatively and quantitatively by HRSEM and ICP measurements. Figure 10 shows HRSEM images of the Fe/ACF (A) and Fe/Pd/ACF (B), illustrating the smaller Pd nanoparticles coating onto the Fe nanoparticles which are embedded within the carbon pores. The measured diameter of the Pd nanoparticles varied from 5 to 14 nm as shown in Figure 9C. The Pd content, as measured by ICP, is 0.9 wt.%.
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Figure 10. HRSEM images of the Fe/ACF (A); and the Fe/Pd/ACF (B) prepared as described in the experimental section.
Figure 10. HRSEM images of the Fe/ACF (A); and the Fe/Pd/ACF (B) prepared as described in the experimental section.
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3.3. Environmental Activity-Proof of Concept

3.3.1. Activity of The Fe3O4/ACF in Absence or Presence of H2O2

The activity of Fe3O4/ACF as a Fenton catalyst was studied in room temperature on orange II as a model environmental contaminant (Figure 11A). The removal rate of orange II from an aqueous solution by the Fe3O4/ACF containing 1%, 2% and 3% w/v H2O2, is significantly higher than that of the pristine ACF and Fe3O4/ACF in absence of H2O2. For example, 60 min after initiating the reaction, 84%, 92% and 98% of the initial amount of orange II was reduced by the Fe3O4/ACF+1%, 2% and 3% H2O2, compared to 48% by the Fe3O4/ACF and 52% by the pristine ACF (Figure 11B). As expected, the degradation rate of orange II increases with H2O2 concentration. This is because the H2O2 concentration is directly related to the content of ·OH radicals generated in the Fenton reaction. We assume that in this study, as reported previously [43], orange II is totally mineralized by the Fenton reaction.
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Figure 11. (A) Chemical structure and elimination rate at room temperature of orange II by Fenton reaction; (B) elimination rate at room temperature of orange II by the Fe/ACF and Fe/Pd/ACF.
Figure 11. (A) Chemical structure and elimination rate at room temperature of orange II by Fenton reaction; (B) elimination rate at room temperature of orange II by the Fe/ACF and Fe/Pd/ACF.
Materials 08 04593 g011

3.3.2. Activity of Fe/ACF and Fe/Pd/ACF

The activity of Fe/ACF and Fe/Pd/ACF was also studied in room temperature on orange II as a model environmental contaminant (Figure 11B). Both Fe/ACF and Fe/Pd/ACF showed enhanced elimination activity compared to the pristine ACF. As shown in Figure 10B, only 5 min after initiation of the reaction, 68% of the initial amount of orange II was reduced by the Fe/Pd/ACF, compared to 30% and 10% by the Fe/ACF and the pristine ACF, respectively.
We assume that the Fe/Pd/ACF combines the advantageous properties of Fe, Pd and carbon matrix. Previous research have shown that Fe nanoparticles induce the cleavage of azo-bond compounds into amine products that are more amenable to mineralization in biological treatment processes [44]. Moreover, the attachment of an appropriate catalytic metal to Fe, such as Pd in this case, increases degradation rates on azo-compouds [45]. Finally, the adsorptive properties of the carbon matrix, as reported previously [3,24], enable the Fe/Pd/ACF to work in adsorptive-reactive manner. Future research will seek to fully clarify the adsorptive and reactive mechanism and potential use of the Fe/Pd/ACF.

4. Conclusions

Fe3O4/ACF, Fe/ACF and Fe/Pd/ACF were engineered by thermal decomposition of iron acetylacetonate supported on ACF at different temperatures in an inert atmosphere. The physical and chemical properties of the various functionalized ACF were found to be significantly dependent on the annealing temperature of the Fe(acac)3/ACF. The potential use of these magnetic fabrics for environmental use was demonstrated with a model azo-dye, orange II. This study illustrated the potential environmental utility of Fe3O4/ACF in the presence of increasing concentrations of H2O2. In addition, the catalytic activity of the Fe/Pd/ACF compared to Fe/ACF was also demonstrated. In future research we will examine the catalytic removal efficiency of the various iron-based ACF on a diverse set of contaminants. Of special interest is the Fe/Pd/ACF. The catalytic performances, as well as the mechanistic activity, will be thoroughly studied.

Acknowledgments

The authors thank to Amit Kohn and Rajesh Chalasani from the Department of Materials Engineering and Ilse-Katz Institute for Nanoscale science and technology, Ben-Gurion Univeristy of the Negev, Beer-Sheva, Israel for the magnetic measurements. We thank also Michal Kolitz-Domb for English editing and proofreading. Finally, we thank to the BSF for funding part of this study.

Author Contributions

This study was designed, directed and coordinated by Hai Haham and Shlomo Margel. Shlomo Margel, as the principal investigator, provided conceptual and technical guidance for all aspects of the project. Judith Grinblat performed and analyzed all of the HRTEM characterizations. Moulay-Tahar Sougrati and Lorenzo Stievano performed and analyzed the data from the MÖssbauer measurements. The manuscript was written by Hai Haham and Shlomo Margel, and commented on by all authors.

Conflicts of Interest

The authors declare no conflict of interest.

References

  1. Huber, D.L. Synthesis, Properties, and Applications of Iron Nanoparticles. Small 2005, 1, 482–501. [Google Scholar] [CrossRef] [PubMed]
  2. Rusevova, K.; Kopinke, F.D.; Georgi, A. Nano-sized Magnetic Iron Oxides as Catalysts for Heterogeneous Fenton-like Reactions-influence of Fe(II)/Fe(III) Ratio on Catalytic Performance. J. Hazard. Mater. 2012, 241–242, 433–440. [Google Scholar] [CrossRef] [PubMed]
  3. Sunkara, B.; Zhan, J.; Kolesnichenko, I.; Wang, Y.; He, J.; Holland, J.E.; McPherson, G.L.; John, V.T. Modifying Metal Nanoparticle Placement on Carbon Supports Using an Aerosol-based Process, with Application to The Environmental Remediation of Chlorinated Hydrocarbons. Langmuir 2011, 27, 7854–7859. [Google Scholar] [CrossRef] [PubMed]
  4. Shin, S.; Yoon, H.; Jang, J. Polymer-encapsulated Iron Oxide Nanoparticles as Highly Efficient Fenton Catalysts. Catal. Commun. 2008, 10, 178–182. [Google Scholar] [CrossRef]
  5. Shahwan, T.; Abu Sirriah, S.; Nairat, M.; Boyacı, E.; Eroğlu, A.E.; Scott, T.B.; Hallam, K.R. Green Synthesis of Iron Nanoparticles and Their Application as A Fenton-like Catalyst for The Degradation of Aqueous Cationic and Anionic Dyes. Chem. Eng. J. 2011, 172, 258–266. [Google Scholar] [CrossRef]
  6. Lien, H.L.; Zhang, W. Nanoscale Iron Particles for Complete Reduction of Chlorinated Ethenes. Colloids Surf. A 2001, 191, 97–105. [Google Scholar] [CrossRef]
  7. Shih, Y.; Tai, Y. Reaction of Decabrominated Diphenyl Ether by Zerovalent Iron Nanoparticles. Chemosphere 2010, 78, 1200–1206. [Google Scholar] [CrossRef] [PubMed]
  8. Cheng, R.; Zhou, W.; Wang, J.L.; Qi, D.; Guo, L.; Zhang, W.X.; Qian, Y. Dechlorination of Pentachlorophenol Using Nanoscale Fe/Ni Particles: Role of nano-Ni and Its Size Effect. J. Hazard. Mater. 2010, 180, 79–85. [Google Scholar] [CrossRef] [PubMed]
  9. Nagpal, V.; Bokare, A.D.; Chikate, R.C.; Rode, C.V.; Paknikar, K.M. Reductive Dechlorination of Gamma-hexachlorocyclohexane Using Fe-Pd Bimetallic Nanoparticles. J. Hazard. Mater. 2010, 175, 680–687. [Google Scholar] [CrossRef] [PubMed]
  10. Lu, A.H.; Salabas, E.L.; Schüth, F. Magnetic Nanoparticles: Synthesis, Protection, Functionalization, and Application. Angew. Chem. Int. Ed. 2007, 46, 1222–1244. [Google Scholar] [CrossRef] [PubMed]
  11. Kim, D.K.; Zhang, Y.; Voit, W.; Rao, K.V.; Muhammed, M. Synthesis and Characterization of Surfactant-Coated Superparamagnetic Monodispersed Iron Oxide Nanoparticles. J. Magn. Magn. Mater. 2001, 225, 30–36. [Google Scholar] [CrossRef]
  12. He, Q.; Yuan, T.; Wei, S.; Haldolaarachchige, N.; Luo, Z.; Young, D.P.; Khasanov, A.; Guo, Z. Morphology- and Phase-controlled Iron Oxide Nanoparticles Stabilized with Maleic Anhydride Grafted Polypropylene. Angew. Chem. Int. Ed. 2012, 51, 8842–8845. [Google Scholar] [CrossRef] [PubMed]
  13. Amara, D.; Felner, I.; Nowik, I.; Margel, S. Synthesis and Characterization of Fe and Fe3O4 Nanoparticles by Thermal Decomposition of Triiron Dodecacarbonyl. Colloids Surf. A 2009, 339, 106–110. [Google Scholar] [CrossRef]
  14. Boguslavsky, Y.; Margel, S. Synthesis and Characterization of Poly(divinylbenzene)-coated Magnetic Iron Oxide Nanoparticles as Precursor for The Formation of Air-stable Carbon-coated Iron Crystalline Nanoparticles. J. Colloid Interface Sci. 2008, 317, 101–114. [Google Scholar] [CrossRef] [PubMed]
  15. Zhang, X.; Alloul, O.; Zhu, J.; He, Q.; Luo, Z.; Colorado, H.A.; Haldolaarachchige, N.; Young, D.P.; Shen, T.D.; Wei, S.; et al. Iron-core Carbon-shell Nanoparticles Reinforced Electrically Conductive Magnetic Epoxy Resin Nanocomposites with Reduced Flammability. RSC Adv. 2013, 3, 9453. [Google Scholar] [CrossRef]
  16. Jay, F.; Gauthier, V.; Dubois, S. Iron Particles Coated with Alumina: Synthesis by A Mechanofusion Process and Study of the High-temperature Oxidation Resistance. J. Am. Ceram. Soc. 2006, 89, 3522–3528. [Google Scholar] [CrossRef]
  17. Gupta, V.K.; Agarwal, S.; Saleh, T.A. Chromium Removal by Combining the Magnetic Properties of Iron Oxide with Adsorption Properties of Carbon Nanotubes. Water Res. 2011, 45, 2207–2212. [Google Scholar] [CrossRef] [PubMed]
  18. Zhang, D.; Wei, S.; Kaila, C.; Su, X.; Wu, J.; Karki, A.B.; Young, D.P.; Guo, Z. Carbon-stabilized Iron Nanoparticles for Environmental Remediation. Nanoscale 2010, 2, 917–919. [Google Scholar] [CrossRef] [PubMed]
  19. Qiu, B.; Wang, Y.; Sun, D.; Wang, Q.; Zhang, X.; Weeks, B.L.; O’Connor, R.; Huang, X.; Wei, S.; Guo, Z. Cr(Vi) Removal by Magnetic Carbon Nanocomposites Derived from Cellulose at Different Carbonization Temperatures. J. Mater. Chem. A 2015, 3, 9817–9825. [Google Scholar] [CrossRef]
  20. Zhu, J.; Wei, S.; Gu, H.; Rapole, S.B.; Wang, Q.; Luo, Z.; Haldolaarachchige, N.; Young, D.P.; Guo, Z. One-pot Synthesis of Magnetic Graphene Nanocomposites Decorated with Core@double-shell Nanoparticles for Fast Chromium Removal. Environ. Sci. Technol. 2012, 46, 977–985. [Google Scholar] [CrossRef] [PubMed]
  21. Zhu, J.; Chen, M.; Qu, H.; Wei, H.; Guo, J.; Luo, Z. Positive and Negative Magnetoresistance Phenomena Observed in Magnetic Electrospun Polyacrylonitrile-based Carbon Nanocomposite. RSC Adv. 2014, 2, 715–722. [Google Scholar] [CrossRef]
  22. Chen, L.; Wang, H.; Wei, H.; Guo, Z.; Khan, M.A.; Young, D.P.; Zhu, J. Carbon Monolith with Embedded Mesopores and Nanoparticles as A Novel Adsorbent for Water Treatment. RSC Adv. 2015, 5, 42540–42547. [Google Scholar] [CrossRef]
  23. Wang, Y.; Wei, H.; Lu, Y.; Wei, S.; Wujcik, E.; Guo, Z. Multifunctional Carbon Nanostructures for Advanced Energy Storage Applications. Nanomaterials 2015, 5, 755–777. [Google Scholar] [CrossRef]
  24. Mezohegyi, G.; van der Zee, F.P.; Font, J.; Fortuny, A.; Fabregat, A. Towards Advanced Aqueous Dye Removal Processes: A Short Review on the Versatile Role of Activated Carbon. J. Environ. Manag. 2012, 102, 148–164. [Google Scholar] [CrossRef] [PubMed]
  25. Mall, I.D.; Srivastava, V.C.; Agarwal, N.K.; Mishra, I.M. Adsorptive Removal of Malachite Green Dye from Aqueous Solution by Bagasse Fly Ash and Activated Carbon-kinetic Study and Equilibrium Isotherm Analyses. Colloids Surf. A 2005, 264, 17–28. [Google Scholar] [CrossRef]
  26. Zhu, J.; Pallavkar, S.; Chen, M.; Yerra, N.; Luo, Z.; Colorado, H.A.; Lin, H.; Haldolaarachchige, N.; Khasanov, A.; Ho, T.C.; et al. Magnetic Carbon Nanostructures: Microwave Energy-assisted Pyrolysis vs. Conventional Pyrolysis. Chem. Commun. 2013, 49, 258–260. [Google Scholar] [CrossRef] [PubMed]
  27. Yagub, M.T.; Sen, T.K.; Afroze, S.; Ang, H.M. Dye and Its Removal from Aqueous Solution by Adsorption: Review. Adv. Colloid Interface Sci. 2014, 209, 172–184. [Google Scholar] [CrossRef] [PubMed]
  28. Janoš, P. Sorption of Basic Dyes onto Iron Humate. Environ. Sci. Technol. 2003, 37, 5792–5798. [Google Scholar] [CrossRef] [PubMed]
  29. Liu, F.; Chung, S.; Oh, G.; Seo, T.S. Three-Dimensional Graphene Oxide Nanostructure for Fast and Efficient Water-Soluble Dye Removal. ACS Appl. Mater. Inter. 2011, 4, 922–927. [Google Scholar] [CrossRef] [PubMed]
  30. Wang, S.; Boyjoo, Y.; Choueib, A.; Zhu, Z.H. Removal of Dyes from Aqueous Solution Using Fly Ash and Red Mud. Water Res. 2005, 39, 129–138. [Google Scholar] [CrossRef] [PubMed]
  31. Gong, J.L.; Wang, B.; Zeng, G.M.; Yang, C.P.; Niu, C.G.; Niu, Q.Y.; Zhou, W.J.; Liang, Y. Removal of Cationic Dyes from Aqueous Solution Using Magnetic Multi-wall Carbon Nanotube Nanocomposite as Adsorbent. J. Hazard. Mater. 2009, 164, 1517–1522. [Google Scholar] [CrossRef] [PubMed]
  32. Huang, Q.; Liu, W.; Peng, P.; Huang, W. Reductive Dechlorination of Tetrachlorobisphenol A by Pd/Fe Bimetallic Catalysts. J. Hazard. Mater. 2013, 262, 634–641. [Google Scholar] [CrossRef] [PubMed]
  33. Brunauer, S.; Emmett, P.; Teller, E. Adsorption of Gases in Multimolecular Layers. J. Am. Chem. Soc. 1936, 407, 309–319. [Google Scholar] [CrossRef]
  34. Barrett, E.P.; Joyner, L.G.; Halenda, P.P. The Determination of Pore Volume and Area Distributions in Porous Substance: I. Computations from Nitrogen Isotherms. J. Am. Chem. Soc. 1951, 1896, 373–380. [Google Scholar] [CrossRef]
  35. Song, Q.; Ding, Y.; Wang, Z.L.; Zhang, Z.J. Tuning The Thermal Stability of Molecular Precursors for The Nonhydrolytic Synthesis of Magnetic MnFe2O4 Spinel Nanocrystals. Chem. Mater. 2007, 19, 4633–4638. [Google Scholar] [CrossRef]
  36. Mero, O.; Sougrati, M.T.; Jumas, J.C.; Margel, S. Engineered Magnetic Core–shell SiO2/Fe Microspheres and “medusa-like” Microspheres of SiO2/iron Oxide/carbon Nanofibers or Nanotubes. Langmuir 2014, 30, 9850–9858. [Google Scholar] [CrossRef] [PubMed]
  37. Menil, F. Systematic Trends of The 57Fe Mössbauer Isomer Shifts in (FeOn) and (FeFn) Polyhedra. Evidance of A New Correlation Between The Isomer Shift and The Inductive Effect of The Competing bondT-X (Fe ). J. Phys. Chem. Solids 1985, 46, 763–789. [Google Scholar] [CrossRef]
  38. Tuček, J.; Tuček, P.; Čuda, J.; Filip, J.; Pechoušek, J.; Machala, L.; Zbořil, R. Iron(III) Oxide Polymorphs and Their Manifestations in In-field 57Fe Mössbauer Spectra. In Mossbauer Spectroscopy in Materials Science-2012, Proceedings of The International Conference MSMS-12, Olomouc, Czech Republic, 11–15 June 2012; Tuček, J., Machala, L., Eds.; American Institute of Physics: Melville, NY, USA, 2012; pp. 56–74. [Google Scholar]
  39. Gu, H.; Ding, D.; Sameer, P.; Guo, J.; Yerra, N.; Huang, Y.; Luo, Z.; Ho, T.C.; Haldolaarachchige, N.; Young, D.P. Microwave Assisted Formation of Magnetic Core-Shell Carbon Nanostructure. ECS Solid State Lett. 2013, 2, M65–M68. [Google Scholar] [CrossRef]
  40. Tuinstra, F. Raman Spectrum of Graphite. J. Chem. Phys. 1970, 53, 1126–1130. [Google Scholar] [CrossRef]
  41. Reich, S.; Thomsen, C. Raman Spectroscopy of Graphite. Philos. Trans. A Math. Phys. Eng. Sci. 2004, 362, 2271–2288. [Google Scholar] [CrossRef] [PubMed]
  42. Lu, Y.; Zhu, Z.; Liu, Z. Carbon-encapsulated Fe Nanoparticles from Detonation-induced Pyrolysis of Ferrocene. Carbon 2005, 43, 369–374. [Google Scholar] [CrossRef]
  43. Feng, J.; Hu, X.; Yue, P.L. Degradation of Azo-dye Orange II by a Photoassisted Fenton Reaction Using A Novel Composite of Iron Oxide and Silicate Nanoparticles as A Catalyst. Ind. Eng. Chem. Res. 2003, 42, 2058–2066. [Google Scholar] [CrossRef]
  44. Fan, J.; Guo, Y.; Wang, J.; Fan, M. Rapid Decolorization of Azo Dye Methyl Orange in Aqueous Solution by Nanoscale Zerovalent Iron Particles. J. Hazard. Mater. 2009, 166, 904–910. [Google Scholar] [CrossRef] [PubMed]
  45. Bokare, A.D.; Chikate, R.C.; Rode, C.V.; Paknikar, K.M. Iron-nickel Bimetallic Nanoparticles for Reductive Degradation of Azo Dye Orange G in Aqueous Solution. Appl. Catal. B 2008, 79, 270–278. [Google Scholar] [CrossRef]

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MDPI and ACS Style

Haham, H.; Grinblat, J.; Sougrati, M.-T.; Stievano, L.; Margel, S. Engineering of Iron-Based Magnetic Activated Carbon Fabrics for Environmental Remediation. Materials 2015, 8, 4593-4607. https://doi.org/10.3390/ma8074593

AMA Style

Haham H, Grinblat J, Sougrati M-T, Stievano L, Margel S. Engineering of Iron-Based Magnetic Activated Carbon Fabrics for Environmental Remediation. Materials. 2015; 8(7):4593-4607. https://doi.org/10.3390/ma8074593

Chicago/Turabian Style

Haham, Hai, Judith Grinblat, Moulay-Tahar Sougrati, Lorenzo Stievano, and Shlomo Margel. 2015. "Engineering of Iron-Based Magnetic Activated Carbon Fabrics for Environmental Remediation" Materials 8, no. 7: 4593-4607. https://doi.org/10.3390/ma8074593

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