# Effect of Tetramethylammonium Hydroxide on Nucleation, Surface Modification and Growth of Magnetic Nanoparticles

Authors: Ângela L. Andrade; José D. Fabris; José D. Ardisson; Manuel A. Valente; José M. F. Ferreira
Journal: Journal of Nanomaterials
 (2012)

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## Abstract

Nanoparticles of magnetite (Fe3O4) were obtained by reacting ferric chloride with sodium sulphite, through the reduction-precipitation method. The effects of adding tetramethylammonium hydroxide (TMAOH) during or after the precipitation of the iron oxide were studied in an attempt to obtain well-dispersed magnetite nanoparticles. Accordingly, the following experimental conditions were tested: (i) precipitation in absence of TMAOH (sample Mt), (ii) the same as (i) after peptizing with TMAOH (Mt1), (iii) TMAOH added to the reaction mixture during the precipitation of magnetite (Mt2). Analyses with transmission electron microscopy (TEM), X-ray diffraction, Mössbauer spectroscopy, attenuated total reflectance Fourier transform infrared spectroscopy (ATR-FTIR), zeta potential, and magnetization measurements up to 2.5 T revealed that magnetite was normally formed also in the medium containing TMAOH. The degree of particles agglomeration was monitored with laser diffraction and technique and inspection of TEM images. The relative contributions of Néel and Brownian relaxations on the magnetic heat dissipation were studied by investigating the ability of suspensions of these magnetite nanoparticles to release heat in aqueous and in hydrogel media. Based on ATR-FTIR and zeta potential data, it is suggested that the surfaces of the synthesized magnetite particles treated with TMAOH become coated with (CH3)4N+ cations.


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## Body

## 1. Introduction

Studying fundamental properties of synthetic analogous magnetite (Fe3O4) nanoparticles keeps drawing much scientific attention and technological interest mainly due to their actual and many potential uses on data storage [1, 2], biolabeling, and on the separation of biomolecules [3, 4]. Most of those applications require chemically stable and uniformly sized nanoparticles that will be well dispersed in liquid media. Usually, a protection layer on the particle surface is necessary to ensure their chemical stability and improve their dispersion ability,in order to increase the surface area to volume ratios. Fe3O4 nanoparticles are inherently unstable and tend to spontaneously aggregate to minimize their high surface energies.Stable concentrated suspensions of magnetic nanoparticles in either organic or inorganic solvents are known as magnetic fluids or ferrofluids [5]. Magnetic fluids were firstly synthesized in 1964, by Papell [6]. They behave as a functional fluid and have increasingly found technological applications in a variety of fields, such as electronic packing, mechanical engineering, aerospace, and bioengineering [7]. Over the recent years, new ferrofluids and their derivatives have been developed for medical diagnosis and therapeutic practices in oncology, specifically, in these cases, for materials with magnetic ferrofluid hyperthermia (MFH) [8, 9], and for many other biomedical technologies [10–13].Hyperthermia is a physical phenomenon that fundaments a medical practice in cancer therapy. The practice consists in selectively heating the malignant tumor, by placing the magnetocaloric material closely to or in direct contact with the affected internal organ of human body. Those organs tend to have fewer blood vessels and are less oxygenated than health ones. Consequently, they are more sensible and die when the local temperature goes above 43°C.The heat dissipation from magnetic particles is caused by the delay of the relaxation of the magnetic moment through either the rotation within the particle (Néel) or the rotation of the particle itself (Brownian), when they are exposed to an AC-magnetic field with magnetic field reversal times shorter than the magnetic relaxation times of the particles [14]. In 2009, Suto et al. [14] showed that the relative contribution between Néel and Brownian relaxations varies depending upon the particle size. Differently from the Brownian relaxation, the heat dissipated through Néel relaxation is not influenced by viscosity of the medium. For example, if the viscosity of the medium is high or if the rotational degree of freedom of the particle restricted, the heat dissipated may either diminish or even completely seize. It is always necessary to determine the relative simultaneous contribution of heat from Néel and Brownian relaxations, to estimate the possible minimum and maximum heat that could be generated with in vivo experiments.Berger et al. [15] have successfully prepared a ferrofluid of Fe3O4 by reacting iron (II) and iron (III) ions in an aqueous ammonia solution with the addition of tetramethylammonium hydroxide (TMAOH), in order to chemically stabilize the magnetic nanoparticles in a colloidal suspension. Cheng et al. [16] have synthesized ferrofluids of magnetite by coprecipitating iron (II) and iron (III) ions in an aqueous solution alkalinized with TMAOH. According to Jolivet et al. [17], TMAOH acts as a surfactant to nanoparticles by absorbing the cationic species at the surface OH groups thus creating an electrostatic repulsion layer surrounding the particles keeping them apart. On the other hand, a number of earlier studies by Yang et al. [18–23] on hydrothermal synthesis of TiO2 [18–22] and α-Al2O3 nanoparticles [23] confirmed that TMAOH plays a very active peptizing role, enhancing the state of dispersion and the crystallinity of the synthesized materials.In the present work, Fe3O4 nanoparticles were synthetized via precipitation of partially reduced ferric chloride with sodium sulfide, in an alkaline solution. The effects of adding TMAOH either during the precipitation or after the synthesis of magnetite on the characteristics of the nanoparticles and on the colloidal stability of the suspensions will be discussed in this report.


## 2. Experimental Procedure

### 2.1. Reagents

All chemicals used, such as iron (III) chloride hexahydrate, FeCl3·6H2O (Riedel-de Haen, France); sodium sulfite, Na2SO3 (Sigma–Aldrich, Japan); ammonium hydroxide, NH4OH (Fluka, Germany); 25% aqueous tetramethylammonium hydroxide solution, C4H13NO·5H2O (TMAOH) (Aldrich, Germany, Japan) and hydrochloric acid, HCl (Sigma-Aldrich) were of analytical grade and used as received.


### 2.2. Synthesis of Iron Oxide Nanoparticles

Samples of Fe3O4 nanoparticles were obtained via the reduction-precipitation method, following the procedure described in details elsewhere [24]. In one of them, the iron ions solution was alkalinized with ammonium hydroxide and the particles were peptized with TMAOH. In the other, the iron ions solution was directly alkalinized with the peptizing agent (TMAOH), as described below.


#### 2.2.1. Alkalinizing with Ammonia

30 mL of a FeCl3.6H2O stock solution containing 0.5 mol L−1 (dissolved in 0.5 mol L−1 HCl), 20 mL of a Na2SO3 stock solution with 1 mol L−1, and 50.8 mL of a NH4OH solution diluted to a total volume of 800 mL were used. Just after mixing Fe3+ and SO3-2, the color of the solution changed from yellow to red and, after few minutes, the yellow color reappeared. A diluted ammonia solution was then quickly poured into the mixture under vigorous stirring; a black precipitate was then formed. Stirring continued for an additional 30 min. The pH of the solution was monitored to be maintained at 10.0 ± 0.1. The suspension containing the precipitated powder was centrifuged at 2,000 rpm for 3 min; the supernatant was discarded. This procedure was repeated for five times by redispersing the resultant cakes in distilled water, each time. The as-obtained precipitate sample was labeled Mt. The Mt nanoparticles were peptized with TMAOH. Typically, 1 mL of 25 mass% TMAOH solution was added to each centrifuge tube containing an amount of wet cake corresponding to about 1 g of dry powder and re-dispersed by stirring with a thin glass rod until obtaining homogeneous suspensions. These suspensions were then dried to obtain the powders for the different measurements. This sample peptized with TMAOH was labeled Mt1.


#### 2.2.2. Alkalinizing with TMAOH

In this case, magnetite nanoparticles were synthesized in the same way as described above, but alkalinizing was made by quickly pouring 25 mass% TMAOH solution until a pH of about 10.0 ± 0.1 was obtained. A precipitate was formed. The mixture was stirred for further 30 min. The obtained suspension was centrifuged at 2,000 rpm for 3 min, and the supernatant was discarded. This procedure was repeated five times by redispersing the resultant cakes in distilled water. The centrifuged cakes were dried to obtain the powders to be used for further characterization. The obtained solid sample, precipitated in medium containing TMAOH, was labeled Mt2.


### 2.3. Characterization Techniques

For transmission electron microscopy analysis (TEM), a drop of the suspension of the magnetite sample was placed onto a copper mesh coated with an amorphous carbon film and then dried in an evacuated desiccator. TEM micrographs were recorded on a transmission electron microscope (Hitachi, 9000 NA, Japan) and the particle size was measured with the software Image J. The crystalline phases were determined by X-ray powder diffraction (XRD) analysis (Rigaku Geigerflex D/Max, C Series; CuKα radiation; 2θ angle range 20°–70°; step 0.02 s−1) after evaporation of the liquid carrier. Phases were identified by comparing the experimental X-ray patterns with standard files compiled by the International Centre for Diffraction Data. The Rietveld structural refinement was performed with FULLPROF 2010 program. Mössbauer spectra were collected in constant acceleration transmission mode with a ~50 mCi 57Co/Rh gamma-ray source. Spectra at 298 K and 100 K were obtained with a spectrometer equipped with a transducer (CMTE model MA250) controlled by a linear function driving unit (CMTE model MR351). Values of Mössbauer isomer shifts are quoted relatively to α-Fe. The experimental reflections were fitted to Lorentzian functions by least-square fitting with software NORMOS-90 (this NORMOS package was developed by R. A. Brand, Laboratorium für Angewandte Physik, Universität Duisburg, D-47048, Duisburg-Germany).The ATR–FTIR data were collected with a FT-IR model Mattson Galaxy S-7000, 32 scans, and resolution of 4 cm−1.The determination of zeta potential (ξ) was performed on a COULTER DELSA 440SX, by using a stock suspension of the ground material in deionized water, prepared and homogenized by ultrasonication for 15 min. Drops of this stock suspension were then added to an aqueous solution of KCl 10-3mol L−1 for the zeta potential measurements. The pH of the measuring solution was varied and adjusted to several values, in the pH range of 3.5 to 10.5, by using 10-3mol L−1aqueous solutions of KOH and HNO3.The agglomerate grain sizes in suspension were determined by dynamic light scattering (DSL) using a Zetasizer Nano ZS instrument (Malvern Instruments Ltd., UK) that allows specific measurements of thez-average diameter (defined as the intensity-weighted average hydrodynamic diameter of the particles being measured). An aliquot of a stock suspension of the ground material in deionized water was prepared and homogenized by ultrasonication for 5 min. The used water was purified by passing through a 0.22 μm Millipore filter. The z-average diameter was calculated as the average of six measurements.The DC magnetic measurements were performed on powder samples (100–150 mg) using a vibrating sample magnetometer (VSM) with a cryogen-free magnet (cryogenic-cryofree), at the University of Aveiro, Portugal. Typical hysteresis curves were obtained at 300 ± 0.1 K with a magnetic field varying between −2.5 and 2.5 T. The magnetic parameters such as saturation magnetization (Ms), coercivity (Hc), and retentivity (Mr) were obtained from the VSM results.Heat dissipation experiments were carried out by transfering the suspensions with dispersed magnetite in both water and hydrogel into a test tube. This tube was placed at the center of a three-loop coil of the VSM equipment, consisting of a power supply (Nova Star 5 kW RF Power Supply, Ameritherm, Inc, Scottsville, NY, USA) and a heating station (Induction atmospheres). The sample concentration was approximately 2 mg mL−1 in water and 2 mg g−1 in polyvinyl alcohol hydrogel. In the hydrogel dispersed samples, rotation of particles was restricted and the magnetic moment relaxed only through Néel relaxation. The temperature of the magnetic suspension was measured with an optical fiber thermometer. Results were taken as the mean of triplicate measurements.The polyvinyl alcohol hydrogel was based on the method earlier proposed by Hyon et al. [25], with minor modifications. A homogeneous polyvinyl alcohol (PVA) solution with a PVA concentration of 15 wt% was obtained by heating the mixture of PVA and a mixed water/dimethyl sulfoxide (DMSO) solvent at 140°C for 2 hrs. The mixing ratio of water to DMSO was kept to 20/80 by weight. Then the casted PVA was placed in a freezer at −20°C for 24 h.


## 2.1. Reagents

All chemicals used, such as iron (III) chloride hexahydrate, FeCl3·6H2O (Riedel-de Haen, France); sodium sulfite, Na2SO3 (Sigma–Aldrich, Japan); ammonium hydroxide, NH4OH (Fluka, Germany); 25% aqueous tetramethylammonium hydroxide solution, C4H13NO·5H2O (TMAOH) (Aldrich, Germany, Japan) and hydrochloric acid, HCl (Sigma-Aldrich) were of analytical grade and used as received.


## 2.2. Synthesis of Iron Oxide Nanoparticles

Samples of Fe3O4 nanoparticles were obtained via the reduction-precipitation method, following the procedure described in details elsewhere [24]. In one of them, the iron ions solution was alkalinized with ammonium hydroxide and the particles were peptized with TMAOH. In the other, the iron ions solution was directly alkalinized with the peptizing agent (TMAOH), as described below.


### 2.2.1. Alkalinizing with Ammonia

30 mL of a FeCl3.6H2O stock solution containing 0.5 mol L−1 (dissolved in 0.5 mol L−1 HCl), 20 mL of a Na2SO3 stock solution with 1 mol L−1, and 50.8 mL of a NH4OH solution diluted to a total volume of 800 mL were used. Just after mixing Fe3+ and SO3-2, the color of the solution changed from yellow to red and, after few minutes, the yellow color reappeared. A diluted ammonia solution was then quickly poured into the mixture under vigorous stirring; a black precipitate was then formed. Stirring continued for an additional 30 min. The pH of the solution was monitored to be maintained at 10.0 ± 0.1. The suspension containing the precipitated powder was centrifuged at 2,000 rpm for 3 min; the supernatant was discarded. This procedure was repeated for five times by redispersing the resultant cakes in distilled water, each time. The as-obtained precipitate sample was labeled Mt. The Mt nanoparticles were peptized with TMAOH. Typically, 1 mL of 25 mass% TMAOH solution was added to each centrifuge tube containing an amount of wet cake corresponding to about 1 g of dry powder and re-dispersed by stirring with a thin glass rod until obtaining homogeneous suspensions. These suspensions were then dried to obtain the powders for the different measurements. This sample peptized with TMAOH was labeled Mt1.


### 2.2.2. Alkalinizing with TMAOH

In this case, magnetite nanoparticles were synthesized in the same way as described above, but alkalinizing was made by quickly pouring 25 mass% TMAOH solution until a pH of about 10.0 ± 0.1 was obtained. A precipitate was formed. The mixture was stirred for further 30 min. The obtained suspension was centrifuged at 2,000 rpm for 3 min, and the supernatant was discarded. This procedure was repeated five times by redispersing the resultant cakes in distilled water. The centrifuged cakes were dried to obtain the powders to be used for further characterization. The obtained solid sample, precipitated in medium containing TMAOH, was labeled Mt2.


## 2.2.1. Alkalinizing with Ammonia

30 mL of a FeCl3.6H2O stock solution containing 0.5 mol L−1 (dissolved in 0.5 mol L−1 HCl), 20 mL of a Na2SO3 stock solution with 1 mol L−1, and 50.8 mL of a NH4OH solution diluted to a total volume of 800 mL were used. Just after mixing Fe3+ and SO3-2, the color of the solution changed from yellow to red and, after few minutes, the yellow color reappeared. A diluted ammonia solution was then quickly poured into the mixture under vigorous stirring; a black precipitate was then formed. Stirring continued for an additional 30 min. The pH of the solution was monitored to be maintained at 10.0 ± 0.1. The suspension containing the precipitated powder was centrifuged at 2,000 rpm for 3 min; the supernatant was discarded. This procedure was repeated for five times by redispersing the resultant cakes in distilled water, each time. The as-obtained precipitate sample was labeled Mt. The Mt nanoparticles were peptized with TMAOH. Typically, 1 mL of 25 mass% TMAOH solution was added to each centrifuge tube containing an amount of wet cake corresponding to about 1 g of dry powder and re-dispersed by stirring with a thin glass rod until obtaining homogeneous suspensions. These suspensions were then dried to obtain the powders for the different measurements. This sample peptized with TMAOH was labeled Mt1.


## 2.2.2. Alkalinizing with TMAOH

In this case, magnetite nanoparticles were synthesized in the same way as described above, but alkalinizing was made by quickly pouring 25 mass% TMAOH solution until a pH of about 10.0 ± 0.1 was obtained. A precipitate was formed. The mixture was stirred for further 30 min. The obtained suspension was centrifuged at 2,000 rpm for 3 min, and the supernatant was discarded. This procedure was repeated five times by redispersing the resultant cakes in distilled water. The centrifuged cakes were dried to obtain the powders to be used for further characterization. The obtained solid sample, precipitated in medium containing TMAOH, was labeled Mt2.


## 2.3. Characterization Techniques

For transmission electron microscopy analysis (TEM), a drop of the suspension of the magnetite sample was placed onto a copper mesh coated with an amorphous carbon film and then dried in an evacuated desiccator. TEM micrographs were recorded on a transmission electron microscope (Hitachi, 9000 NA, Japan) and the particle size was measured with the software Image J. The crystalline phases were determined by X-ray powder diffraction (XRD) analysis (Rigaku Geigerflex D/Max, C Series; CuKα radiation; 2θ angle range 20°–70°; step 0.02 s−1) after evaporation of the liquid carrier. Phases were identified by comparing the experimental X-ray patterns with standard files compiled by the International Centre for Diffraction Data. The Rietveld structural refinement was performed with FULLPROF 2010 program. Mössbauer spectra were collected in constant acceleration transmission mode with a ~50 mCi 57Co/Rh gamma-ray source. Spectra at 298 K and 100 K were obtained with a spectrometer equipped with a transducer (CMTE model MA250) controlled by a linear function driving unit (CMTE model MR351). Values of Mössbauer isomer shifts are quoted relatively to α-Fe. The experimental reflections were fitted to Lorentzian functions by least-square fitting with software NORMOS-90 (this NORMOS package was developed by R. A. Brand, Laboratorium für Angewandte Physik, Universität Duisburg, D-47048, Duisburg-Germany).The ATR–FTIR data were collected with a FT-IR model Mattson Galaxy S-7000, 32 scans, and resolution of 4 cm−1.The determination of zeta potential (ξ) was performed on a COULTER DELSA 440SX, by using a stock suspension of the ground material in deionized water, prepared and homogenized by ultrasonication for 15 min. Drops of this stock suspension were then added to an aqueous solution of KCl 10-3mol L−1 for the zeta potential measurements. The pH of the measuring solution was varied and adjusted to several values, in the pH range of 3.5 to 10.5, by using 10-3mol L−1aqueous solutions of KOH and HNO3.The agglomerate grain sizes in suspension were determined by dynamic light scattering (DSL) using a Zetasizer Nano ZS instrument (Malvern Instruments Ltd., UK) that allows specific measurements of thez-average diameter (defined as the intensity-weighted average hydrodynamic diameter of the particles being measured). An aliquot of a stock suspension of the ground material in deionized water was prepared and homogenized by ultrasonication for 5 min. The used water was purified by passing through a 0.22 μm Millipore filter. The z-average diameter was calculated as the average of six measurements.The DC magnetic measurements were performed on powder samples (100–150 mg) using a vibrating sample magnetometer (VSM) with a cryogen-free magnet (cryogenic-cryofree), at the University of Aveiro, Portugal. Typical hysteresis curves were obtained at 300 ± 0.1 K with a magnetic field varying between −2.5 and 2.5 T. The magnetic parameters such as saturation magnetization (Ms), coercivity (Hc), and retentivity (Mr) were obtained from the VSM results.Heat dissipation experiments were carried out by transfering the suspensions with dispersed magnetite in both water and hydrogel into a test tube. This tube was placed at the center of a three-loop coil of the VSM equipment, consisting of a power supply (Nova Star 5 kW RF Power Supply, Ameritherm, Inc, Scottsville, NY, USA) and a heating station (Induction atmospheres). The sample concentration was approximately 2 mg mL−1 in water and 2 mg g−1 in polyvinyl alcohol hydrogel. In the hydrogel dispersed samples, rotation of particles was restricted and the magnetic moment relaxed only through Néel relaxation. The temperature of the magnetic suspension was measured with an optical fiber thermometer. Results were taken as the mean of triplicate measurements.The polyvinyl alcohol hydrogel was based on the method earlier proposed by Hyon et al. [25], with minor modifications. A homogeneous polyvinyl alcohol (PVA) solution with a PVA concentration of 15 wt% was obtained by heating the mixture of PVA and a mixed water/dimethyl sulfoxide (DMSO) solvent at 140°C for 2 hrs. The mixing ratio of water to DMSO was kept to 20/80 by weight. Then the casted PVA was placed in a freezer at −20°C for 24 h.


## 3. Results and Discussion

Centrifuging the just formed precipitate, still in aqueous suspension, in order to finally obtain the Mt2 sample, at 2,000 rpm for 3 min was found to be enough condition to separate the solid particles from the liquid phase, whereas for the corresponding Mt1 sample, centrifugation even at 12,000 rpm for 6 min was insufficient to separate the two phases. This suggests that Mt2 particles are coarser and/or strongly agglomerated than Mt1.The obtained Mt, Mt1, and Mt2 samples were black in color and exhibited magnetic behavior, as it could be observed from their response to the magnetic field of a small hand magnet. The Mt1 suspension kept their colloidal characteristics for up to 5 months with negligible sedimentation in this ferrofluid. Contrarily, the Mt2 sample was completely sedimented when the ferrofluid flask was in rest for 1 h, evidencing again the coarser and/or aggregated nature of its particles.Thez-average diameter of the Mt, Mt1, and Mt2 samples in water was as follows: 243.7 ± 18.59, 85.86 ± 2.736, and 1,906 ± 495.8 nm, respectively. The large individual or aggregated grains, as observed for sample Mt2, explains the reason by which it sedimented even faster than the Mt1 sample. The Mt1 ferrofluid is also much better dispersed than Mt and Mt2.Figure1 shows TEM images of Mt, Mt1, and Mt2 nanoparticles. The mean particle size diameters for the samples Mt, Mt1, and Mt2 were found to be about 5.7 ± 2.9 nm, 5.8 ± 2.7 nm, and 9.7 ± 6.4 nm, respectively. The mean size of the particles/aggregates is larger in the case of Mt2 sample. The higher tendency of particles in sample Mt2 to be aggregated can be explained by the bigger particle sizes but also by their higher crystallinity (Figure 2), well favored by the addition of the peptizing agent (TMAOH). Larger particles of well-crystallized magnetite in which the bulk properties supersede surface properties, and they are expected to magnetically attract more strongly each other. Hosono et al. [26] suggested that the bigger particles could be a consequence of higher concentration of charged ions in the solution since agglomeration between particles occurs by shrinkage of electric double layer. Moreover, the role of the ionic strength on the particle size also is largely dependent on the nature of the electrolyte. The smallest cations being the best screening ions, their influence on the surface charge is highest. The surface of iron oxides is negatively charged at pH > PZC (point of zero charge). These characteristics explain the strong influence of NH4+ on reducing particle sizes, as compared to the [N(CH3)4]+ cations, and also on preventing particles aggregation. This interpretation is in line with that of Bacri et al. [27, 28], who proposed a decreasing stability of the iron oxide nanoparticles as a consequence of a decrease of the electrical double layer thickness around the particles, driven by the increased ionic strength of the media upon adding TMAOH.TEM micrograph of samples: Mt, Mt1, and Mt2.
(a)
(b)
(c)Figure 2
X-ray diffraction patterns of samples: Mt, Mt1, Mt2, and magnetite (ICDD file no. 019-0629).The crystalline structure of the synthesized iron oxide species analyzed by powder XRD (Figure2) shows that Fe3O4 was identified in these Mt, Mt1, and Mt2 samples. The most intense reflections for this phase were registered at 2θ = 30.095°, 35.423°, 43.053°, 57.22° and 62.76°, corresponding to the planes of (220), (311), (400), (511), and (440), respectively, of the iron oxide spinel. The peaks in the diffractograms match well with the PDF data for magnetite from the powder diffraction file (PDF) from International Centre for Diffraction Data (ICDD) card number  019-0629. The average particle sizes for Mt, Mt1, and Mt2 magnetites, from breadths of reflection 311, estimated with Scherrer equation were 11, 10, and 13 nm, respectively [29]. From routine powder XRD data only, it may be difficult to differentiate the coexisting maghemite (γFe2O3) and magnetite (Fe3O4) in a same sample since structure is cubic with relatively close unit cell dimension. The diffraction patterns for both phases are quite similar. Therefore, one might presume that magnetite and maghemite are components of the obtained ferromagnetic phases, as oxidation processes could not be totally avoided during chemical synthesis and solid powder washings and handling in air. Results in Figure 2 confirm that the sample Mt that has not been in contact with the peptizing agent exhibits the lowest degree of crystallinity as it can be drawn from the noisy background and from the broader diffraction peaks. Contrarily, the Mt2 sample that has been synthesized from the very beginning in presence of TMAOH presents the sharpest XRD diffraction peaks, which is in good consistence with its coarser morphology (Figure 1). When the peptizing agent was added to the precipitated Mt sample, it promoted a better dispersion of the partially amorphous nanoparticles and enhanced the degree of spatial arrangement of the matter, thus increasing the crystallinity. This effect was reportedly proposed for other systems [18–23]. These results suggest that, in the case of Mt2, the [(CH3)4N]+ cations are prone to readily adsorb specifically onto the surface of the early nuclei being formed, as schematized in Figure 3, hindering some of them to achieve the critical size for growing. Under this perspective, a smaller number of effective nuclei would be formed, explaining the greater size of the resulting nanoparticles in the case of Mt2 sample.Figure 3
Peptization exerted by tetramethyl ammonium cations adsorbed onto the surface of magnetic nanoparticles thus, creating repulsive forces and enabling the particle growing species to be added to the surface in an organized manner.Mössbauer spectra obtained at variable temperatures (Figure4) reveal that these nanosized particles do contain ferric iron oxides in small particle sizes, more clearly for samples Mt and Mt2.Mössbauer spectra of Mt, Mt1, and Mt2 at (a) RT, and ( b) 80 K.
(a)
(b)These magnetic nanoparticles in a liquid medium experience reorientations of the magnetization vector, in single anisotropic magnetic domains (Néel relaxation time,τN) but also due to viscous rotation of the particle (Brownian relaxation time, τB) [30, 31].The global magnetic relaxation times (τ) of colloids are the sum of the Néel and Brownian relaxation rates, which is given by [31, 32]
(1)1τ=1τB+1τN.These relaxations explain the obtained Mössbauer spectra with a relatively intense central Fe3+ doublet along with a magnetic sextet, as it was more clearly observed for samples Mt and Mt2. However, lowering the sample temperature tends to progressively block the relaxations effect and promote the magnetic ordering. The coexistence of these two major spectral contributions, that is, superparamagnetic and magnetically ordered patterns, in different proportions, means that particle sizes distributions are different in each case. From Mössbauer data only, the sample Mt does contain higher proportion of smaller particles than in Mt2, but sample Mt1 contains the highest proportion of bigger particles of all three. The corresponding hyperfine field distributions clearly reflect these trends. The 80 K probability profile for sample Mt1 is considerably narrower than for the other two samples. Values of hyperfine magnetic fields at maximum probability for all these magnetic samples steadily increase on going from 297 K to 80 K, following values well around those expected for maghemite (γFe2O3).The apparent contradiction with evidences from hyperthermic measurements that point to sample Mt2 as the sample containing bigger particles than Mt and Mt1 is explained by assuming that the Brownian relaxation rate in sample Mt2, with more strongly aggregated nanoparticles, is much slower so to produce a more significant hyperthermic effect. However, Mössbauer spectra are necessarily collected with the solid sample. In this condition, the global relaxation time is only influenced by the Néel relaxation, for which magnitude, particularly for samples Mt and Mt2, would be comparable or below the time-scale window for Mössbauer spectroscopy, or ~10−7 s.A Mössbauer spectrum results from the hyperfine coupling arising from extranuclear electric and magnetic fields that influence the energy levels of the probe nucleus. The fast fluctuation of the magnetization vector between easy directions in the monodomain nanosystem, relatively to the lifetime decay of the57Fe 14.4 keV Mössbauer level, would lead to an electric quadrupole coupling, resulting in a spectral superparamagnetic doublet. Particles aggregation that is promoted by coating their surface with surfactant or polymerizing organic materials may be enough to change the hyperthermic behavior of the material but not necessarily the hyperfine structure of the solid material. Aggregates of fine particles may present typical hyperthermic behavior as of bigger particles, essentially due to the increasing Brownian reorientation energy in the colloidal medium, but their hyperfine structure still accounts for local interactions at the atomic nuclear level in the superparamagnetic state of the solid material.Figure5 compares the ATR–FTIR spectra of the TMAOH and of the Mt, Mt1, and Mt2 samples. The ATR–FTIR spectrum of the TMAOH shows a strong band at 1490 cm−1, assigned to the asymmetric methyl deformation mode, δasym(CH3). A smaller one assigned to the symmetrical methyl deformation mode δsym(CH3) appears near to 1430 cm−1. A single band appeared at 950 cm−1 is attributed to the υasym(C–N) mode which is generally observed in the domain 900–1000 cm−1 [33]. The Mt sample shows a band at 550 cm−1. Since magnetite has an inverse spinel-type structure, it shows bands indicating the vibrations MT–O–MO (ν1 ≈ 600–550 cm−1), where MT and MO correspond to the metal occupying tetrahedral and octahedral positions, respectively [34–36]. The ATR–FTIR spectra of the Mt1 and Mt2 samples also show the band at 550 cm−1 characteristic of magnetite and the characteristic vibration of Fe-O in maghemite (γ-Fe2O3) at 690 cm−1[37–39], as well as the transmittance bands typical of TMAOH, proving that the peptizing agent has been strongly adsorbed at the surface of the nanoparticles.Figure 5
ATR-FTIR spectra of TMAOH, Mt, Mt1, and Mt2.Zeta potential data are a powerful tool being extensively used to evaluate the effects of the presence of surface-active agents in different systems. In the present work, this technique was also used to help evaluating the influence of added TMAOH on the solid/liquid interface properties of magnetite nanoparticles. Results presented in Figure6 show that the pH values corresponding to the isoelectric points (pHIEP) of the Mt and Mt1 samples were found to be about 6.4 and 6.8, respectively. This is in good agreement with the reported data in the scientific literature for magnetite [40, 41]. In the Mt2 sample, the  pHIEP was about 7.3. The increase in pHIEP of the Mt1 and Mt2 samples, with respect to that determined for Mt sample, indicates that [(CH3)4N]+ cations were specifically adsorbed onto the surface of the synthesized iron oxide species [42]. This specific adsorption is partially driven by the negative charge exhibited by magnetite above its  pHIEP (6.4) and has been apparently more extensive when the peptizing agent was added during the precipitation. Thus, the adsorbed [(CH3)4N]+ ions tend to decrease the negative charge of the iron oxide powder at alkaline pH range.Figure 6
Variation of zeta potential of samples: Mt, Mt1, and Mt2.Magnetization curves obtained for Mt, Mt1, and Mt2 samples at 300 K are presented in Figure7. The curves indicate a superparamagnetic behavior, for all these samples, as evidenced by zero coercivity and remanence on the magnetization loop. The saturation magnetization (MS) was obtained from moment versus magnetic field (B) curves. For the Mt sample, the saturation magnetization value is 70.7 emu g−1, being higher than values reported in the literature (46.3 emu g−1) for samples prepared by the same method [43], whereas for peptized samples Mt1 and Mt2 with TMAOH the corresponding values are 62.8 and 63.2 emu g−1. The magnetic saturation values of magnetite nanoparticles are experimentally determined to be in the range of 30–50 emu g−1, which is lower than the bulk value, 90 emu g−1 [44]. Similar values have been obtained for Mt sample. It was expected that the saturation magnetization was higher for samples Mt1 and Mt2, as they have a higher degree of crystallinity and, in the case of Mt2, a larger particle size. The differences between the saturation magnetization between the samples with and without TMAOH can be ascribed to the previous presumption that magnetite and maghemite are both present in these peptized powders with TMAOH.Figure 7
Magnetization curves of samples: Mt, Mt1, and Mt2.The magneto caloric behavior, influencing the heating ability of magnetite samples Mt, Mt-1, and Mt-2, is shown in Figure8. For each experiment, the temperature rising was measured for every 1 min up to an accumulated time of 20 min and then every 5 min up to 1 h. Superparamagnetic particles generate heat by conversion of magnetic energy into thermal energy caused by the delay in magnetic relaxation. According to the Néel model, the magnetic moment originally locked along the crystal easy axis rotates away from that axis, tending to align with the external field. The Néel mechanism is analogous to the hysteresis loss in multidomain magnetic particles whereby there is an internal friction due to the movement of the magnetic moment in an external field that results in heat generation. In the Brownian mode, the whole particle rotates in the direction of the field with the moment locked along the crystal axis. The heat generated through Néel or Brownian relaxation in an applied AC magnetic field depends on the size of the nanoparticles. Smaller nanoparticles generate heat preferentially by the Néel modell.Temperature-time curves of the samples Mt, Mt1, and Mt2 dispersed in (a) water and (b) PVA hydrogel.
(a)
(b)The amount of heat generated by pure water and hydrogel in 220 Oe AC magnetic fields was measured to obtain any contribution of water and hydrogel in the increase of temperature by the dispersed nanoparticles. The whole contribution of both pure water and gel was discounted from the final temperature value for each ferrofluid.The results of heat dissipation experiments of the samples Mt, Mt1, and Mt2 dispersed in water and hydrogel are shown in Figure8. The ΔTmax values for magnetite nanoparticles dispersed in water and hydrogel were determined from the gradients of temperature-time curves obtained by exposing the samples to an AC magnetic field strength of 220 Oe at frequency of 198 kHz. Results are summarized in Table 1.Table 1
TheΔTmax values of the magnetite samples dispersed in water and hydrogel under 220 Oe AC magnetic field.
Sample
Δ
T
max
Water
Hydrogel
Mt
23
12
Mt1
11
6
Mt2
19
8TheΔTmax values for dispersed samples Mt, Mt1, and Mt2 in hydrogel were roughly 52, 54, and 42% less than that of the sole sample dispersed in water. The reduction in heat dissipation was attributed to the inhibition of particle rotation. In other words, particles should have an average Brownian magnetic relaxation time (TB) less than room temperature (RT) and narrow particle size distribution. This suggested that the fraction of the particles that generated heat through Brownian rotation was comparatively large. The sample with an average diameter below 13 nm had large fraction of particles dissipating heat through Néel relaxation losses. On the other hand, the sample with average diameter larger than 13 nm had large fraction of particles dissipating heat through Brownian relaxation [14]. Furthermore, these results suggested that it is important to analyze the relative contributions of Néel and Brownian relaxations losses to formulate the appropriate strategy for effective in vivo treatments. And also, it could be concluded that the samples with blocking temperature below RT are more suitable for a reliable in vivo MFH treatment. Thus, to derive at the appropriate sample for in vivo experiments, similar study on size-classified particles with TB less than RT and narrow size distribution should be pursued.Hyperthermia is a cancer therapy that consists in heating selectively tumour in focusing organ zones. Those zones have fewer blood vessels and are less oxygenated than health ones. Consequently, they are more sensible and can die if the local temperature increases above 43°C. Thus, a temperature variation ofΔTmax = 11°C would be sufficient to produce therapeutical effects.


## 4. Conclusions

Tetramethylammonium hydroxide (TMAOH) was revealed to be an effective peptizing agent for magnetite manoparticles in ferrofluid systems based on. The [(CH3)4N]+ cations specifically adsorbed onto the surface of the synthesized iron oxide species give rise to repulsive stabilization forces that enable the particle growing species to be added to the surface in a more organized manner. Accordingly, when TMAOH is added during precipitation as in the case of Mt2 samples it promotes the formation of larger particles having a higher degree of crystallinity, including magnetite and  maghemite. The addition of TMAOH after the magnetite has been synthesized promotes the colloidal stability of the nanoparticles and enhances the transformation of the amorphous material into more ordered crystalline phases.



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*Source: 454759-2012-08-02.xml*