# Synthesis of Bismuth Ferrite Nanoparticles via a Wet Chemical Route at Low Temperature

Authors: Yongming Hu; Linfeng Fei; Yiling Zhang; Jikang Yuan; Yu Wang; Haoshuang Gu
Journal: Journal of Nanomaterials
 (2011)

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## Abstract

Nanoparticles (NPs) of multiferroic bismuth ferrite (BiFeO3) with narrow size distributions were synthesized via a wet chemical route using bismuth nitrate and iron nitrate as starting materials and excess tartaric acid and citric acid as chelating agent, respectively, followed by thermal treatment. It was found that BiFeO3 NPs crystallized at ~350∘C when using citric acid as chelating agent. Such crystallization temperature is much lower than that of conventional chemical process in which other types of chelating agent are used. BiFeO3 NPs with different sizes distributions show obvious ferromagnetic properties, and the magnetization is increased with reducing the particle size.


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## Body

## 1. Introduction

In recent years, much research interest has been drawn to bismuth ferrite (BiFeO3, abbreviated as BFO), which is known to be the only multiferroic compound that exhibits simultaneous ferroelectric and G-type antiferromagnetic orders over a broad range above room temperature (Curie temperature >800°C, Neel temperature = 370°C) [1–6]. As a partially covalent oxide, BFO has a rhombohedrally distorted perovskite structure belonging to a space group of R3c [7]. Nevertheless, it exhibits weak magnetism at room temperature due to a spiral magnetic spin cycloid with a periodicity of ~62 nm [4]. So far, most studies on BFO have been performed on two-dimensional epitaxial thin films grown on various substrates [8–11], where epitaxial strain is manifested so as to alter some important properties including crystal lattice structure, polarization, and magnetization. However, more recent approaches are focusing on polycrystals as well as substrate-free nanostructures such as low-dimensional nanostructures, especially zero-dimensional materials like nanoparticles (NPs) [12–17]. Meanwhile, studies on finite size effect of BFO have been carried out by different authors and some interesting properties (e.g., shift of Neel temperature, gas sensing properties, etc.) have been reported [18–22].Previous studies have demonstrated that synthesis of BFO NPs through a traditional solid-state method produces poor reproducibility and causes formation of coarser powders as well as Bi2O3/Bi2Fe4O9 impurity phase [4]. Up to date, several chemical routes (e.g. hydrothermal treatment, mechanochemical synthesis method, and sol-gel methodology, etc.) have been successfully employed for fabricating BFO nanoparticles. However, these approaches have certain shortcomings such as impurities in the final products. Ghosh et al. reported a ferrioxalate precursor method to synthesize BFO NPs through solutions of some specific salts at a temperature of 600°C [23]. Despite the efforts made through enhancing sintering temperature to avoid impurities, a small amount of Bi2O3 was found in the final product. Han et al. have accomplished the morphologies tunable synthesis of bismuth ferrites using hydrothermal method [24]. The resulting size of BFO NPs was sometimes large (up to several hundred nanometers) although no impurities were found in the final products. Using the same method, Chen et al. prepared pure phase BFO nanocrystallites at 200°C using KOH concentration of 4 M. In this study, impurity phases of Bi2Fe4O9 and Bi25FeO40 were easily formed with only a slight change in the KOH concentration [25]. Selbach et al. synthesized BFO NPs through a modified Pechini method using nitrates as metal precursors [26]. Although pure phase BFO was obtained in this study, contaminant produced by decomposition of the precursor was present. Ghosh et al. synthesized nanosized bismuth ferrite using a soft chemical route with tartaric acid as a template material and nitric acid as an oxidizing agent [27]. However, the crystallinity of the resulting BFO NPs was unsatisfactory and the existence of an impure Bi2O3 amorphous phase in the host at low temperature product of 400°C was evident. To deal with the issues mentioned above, our recent research suggests that excess tartaric acid and/or citric acid to be added in the solution so that the crystallinity of BFO NPs can be improved. Herein, we reported a general wet chemical route for synthesizing uniform BFO NPs at about 350°C. To our best knowledge, this is the lowest temperature employed in the literature for BFO fabrication with the exception of certain high pressure techniques such as hydrothermal or solvothermal methods. In addition, the magnetic properties were also investigated for BFO NPs with different size distributions.


## 2. Experimental

All of the reagents were of analytical grade and used without further purification. Following a typical procedure, bismuth nitrate [Bi(NO3)3·5 H2O] and iron nitrate [Fe(NO3)3·9 H2O] were weighed in stoichiometric proportions and dissolved in deionized water to make a solution with an independent concentration of 0.2 M before adding 20 mL diluted nitric acid (65~68% HNO3) to the mixture. Then 10 g of citric acid (C6H8O7) were added to the solutions as chelating agent. The light-yellow-colored solution was heated under vigorous stirring until no liquid was left in the beaker to form gel deposit. Each beaker with solid deposit was kept in the oven at 150°C for another 2~3 h. Subsequently, powders were quarterly divided and calcined in the oven for 2 h at 350, 450, and 550°C, respectively, to obtain well-crystallized BFO NPs with controllable sizes. For comparison, another group of powders were synthesized by modifying a typical soft chemical route by using excess tartaric acid as chelating agents [27].The gel (intermediate product) was subjected to thermal analysis in order to determine the subsequent sintering temperature with simultaneous Thermogravimetric Analysis & Differential Scanning Calorimetry (TG-DSC) system (NETZSCH STA 449 C Jupiter). After heat treatment, the sample was characterized using X-ray diffraction (XRD) with a Bruker AXS D8 ADVANCE X-ray diffractometer with Cu Kα radiation (λ=0.154178nm). Fourier transformation infrared (FT-IR) spectra were obtained on a Perkin-Elmer Spectrum one FT-IR spectrometer at a resolution of 4 cm−1 with an HgCdTe detector. Transmission electron microscopy (TEM) images and high-resolution transmission electron microscopy (HRTEM) images were obtained on a JEOL 2011 transmission electron microscope at an acceleration voltage of 200 kV. Magnetization measurements were taken on a LakeShore Vibrating Sample Magnetometry (VSM) system.


## 3. Results and Discussion

The TG/DSC curves of the precipitated and dried powders are carried out and shown in Figure1. Since tartaric acid and citric acid can form different chelate compounds with Bi3+ and Fe3+ ions (as schematically shown in Figures 4(a) and 4(b)), different thermal behaviors were observed from the curves. There are four weight-loss segments in both Figures 1(a) and 1(b). It can be seen that the first and last segments are due to the evaporation of crystalline water and the crystallization process of BFO. The major mass loss of the two intermediate segments in tartaric acid precursor are derived from volatilization of excess tartaric acid, decomposition of chelate complex, and a small amount of nitrate. However, in the citric acid precursor, this loss is caused by the decomposition process only. The analysis results provided us a detailed guide to our subsequent heat treatment process, which showed that citric acid precursor has a relatively lower crystallization temperature (indicated by red arrows in Figure 1), that is, nearly 100°C lower than that of the tartaric acid precursor. More importantly, to our best knowledge, a crystallize temperature of about 350°C is far lower than those reported in the literature.TG-DSC curves of the gel reminders acquired by using (a) tartaric acid and (b) citric acid as chelating agent.
(a)(b)XRD measurements were performed to characterize the crystal structure of the calcined powders. As shown in Figure2, all the XRD patterns can be indexed to pure rhombohedral perovskite structure, which are in good agreement with the powder data of JCPDS Card number 20-169. After heat treatment at 350°C, the sample from citric acid precursor begins to generate pure phase BFO while another sample from tartaric acid precursor is still of amorphous feature. It is clear that the crystallization of BFO completed at a temperature of 350°C for citric acid precursor while 450°C for tartaric acid precursor, which is in good line with the TG-DSC analysis. Meanwhile, the particle size of BFO changed remarkably after further heat treatment. Calcined at temperatures above 450°C, well-crystallized and pure phase BFO can be obtained for either precursor. As discussed in early literatures, the grain sizes of BFO NPs grow up with increasing the temperature in soft chemical routes [21, 26]. This can be also confirmed by the peak sharpening of XRD curves (data not shown).XRD patterns of BiFeO3 samples synthesized by wet chemical route using different chelating agents followed by calcination at 350°C, 450°C and 550°C, respectively. (a) Tartaric acid and (b) citric acid.
(a)(b)The morphology of the calcined BFO nanoparticles was examined on TEM. Typical TEM images are shown in Figure3. It is clear that the spherical NPs formed from both precursors are sufficiently fine and uniform on copper grid, and the particle sizes are about 12 and 4 nm, respectively. Hardly any aggregation could be found in our samples compared with traditional approaches. The corresponding selected area electron diffraction patterns (as shown in Figures 3(c) and 3(f)) suggest that our NPs are well crystallized, and both can be indexed to pure BFO rhombohedral crystal structure. The HRTEM image of individual BFO NP (Figure 3(b)) clearly shows an interplanar spacing of 2.778 Å, corresponding to the (110) crystal planes. Furthermore, we can acquire NPs with an average particle size of about 4, 12, 30, and 80 nm through keeping the calcination temperatures at 350, 450, 550, and 650°C, respectively.Figure 3
TEM images of BiFeO3 NPs at low and high magnification, and corresponding SAED patterns: (a), (b), and (c) for nanoparticles from tartaric acid and calcined at 450°C, while (d), (e), and (f) for NPs from citric acid and calcined at 350°C.Figure 4
FTIR spectra of BiFeO3 precursors formed by tartaric acid (a) and citric acid (b), respectively.Figure4 shows the FTIR spectra of BiFeO3 precursors using tartaric acid and citric acid as chelating, respectively. As shown, eight characteristic IR peaks appeared for BFO precursor (tartaric acid), while four characteristic IR peaks together with some weak peaks appeared for BFO precursor using citric acid as chelating.  Both samples have two sharp and one wide IR peaks, which correspond to the stretching vibrations of C=O and –OH. The IR wide peaks located at 3466 cm-1 in (a) and (b) were assigned to the stretching vibrations of structural hydroxyl (OH) groups, and the intense peaks at 1628–1672 cm-1 were assigned to the stretching vibrations of C=O (corresponding to the groups of tartaric and citric acid). The IR peaks located at 1374 cm-1 were attributed to the symmetry bending vibration of C–H. In addition, a sharp IR peak located at 1278 cm-1 was assigned to the stretching vibration of single bond of C–O for tartaric acid precursor sample, while it cannot be observed for citric acid precursor sample. The IR peaks below 1000 cm-1 (such as 492, 806, and 902 cm-1 for tartaric acid precursor, 477, 551, 613, 858, and 910 cm-1 for citric acid precursor) were corresponding to the vibrations bonds of Bi–O or Fe–O, respectively.A possible mechanism for the formation of BFO NPs was proposed based on previous analysis (as shown in Figure5). Firstly, Bi(NO3)3·5 H2O and Fe(NO3)3·9 H2O along with chelating agents were added to the deionized water and formed the complex of Bi and Fe (Figures 5(a) and 5(b)). Secondly, sol-like precursor and irregular particles come into being followed by aqueous solution were dried (which can be inferred from FRIR spectra of BFO precursors using tartaric and citric acid as chelating, as shown in Figure 4). Finally, the precursor decomposed and BFO NPs started to generate accompanied by the calcination stage under different temperature. It is believed that the chelating compounds plays an important role in controlling shape and size of particles and the decomposition temperatures of the precursor will partially determine the crystallization temperature of BFO NPs in our synthesis. The investigations show that the grain size of the BFO NPs increases with increasing calcination temperature, implying a facile way to BFO NPs with controllable sizes. The geometry of the grains becomes more complicated with higher temperature, a result of better crystallization under high temperature. Higher temperatures cause the grains to grow much bigger so that we can obtain sharper monocrystal SAED image as shown in Figure 6.Schematic for different chelating complex formed by tartaric acid (a) and citric acid (b), where purple stands for Bi, blue for Fe, red for oxygen, and gray for carbon atoms. (c) Possible formation processes of BiFeO3 NPs under wet chemical environment using tartaric acid and citric acid as chelating agents, respectively.
(a)(b)(c)Figure 6
TEM image of BiFeO3 NPs calcined at 650°C and the corresponding SAED pattern (inset), indicated by the black square.The magnetization hysteresis loops of BFO NPs samples with three different particle sizes were measured over±1T at room temperature, as shown in Figure 7. All loops exhibit a finite exchange bias field and vertical asymmetry with visibly greater saturation magnetizations compared to what has been reported previously [21]. This could be a result of uniform particle sizes and the additional lattice strains caused by the large amount of surfaced atoms from small grain size [28]. According to the theory of BFO’s ferromagnetism, magnetization drops as its grain size increases [21]. As the calcination temperature raises, the magnetization of BFO NPs with diameters of 12 and 30 nm decreases as expected. One possible explanation may be that some grains may not have spontaneous magnetic moments and therefore fail to contribute to the magnetization. The possibility of superparamagnetic behaviors in BFO NPs can be ruled out from the finite coercivity and the finite exchange bias field at room temperature (varies within 60 to 90 Oe), which confirms the ferromagnetic order as well as spin pinning at the ferromagnetic—antiferromagnetic interfaces [28]. The magnetization is nearly linear with the external magnetic field for the sample heat treatment at 650°C, which means the NPs has almost lost its ferromagnetic property (the result is not shown here). This finding matches well with what have been found previously, that is, crystallites larger than 62 nm display bulk lattice parameters and hence do not present any ferromagnetic property, namely, the hysteresis loop.Figure 7
Magnetization hysteresis loops of BiFeO3 NPs with different particle size distributions. (a) 4 nm, (b) 12 nm, and (c) 30 nm.


## 4. Conclusions

In summary, pure phase BFO NPs with an average diameters ranging from 4 to 30 nm were synthesized by a simple soft chemical route using citric acid as chelating agent followed by calcination at a relatively low temperature. TG/DSC, XRD, and TEM were used to confirm the phase and size distribution of the nanoparticles and VSM was utilized to measure the size-dependent magnetic behaviors of the as-prepared nanoparticles. Precursors of the nanoparticles in the experiments as well as the formation mechanism are proposed. This method avoids using traditional high temperature and therefore could be easily extended to other systems.



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*Source: 797639-2010-08-15.xml*