# Sol-Gel Synthesis and Characterization of Cubic Bismuth Zinc Niobium Oxide Nanopowders

Authors: Ganchimeg Perenlei; Peter C. Talbot; Wayde N. Martens
Journal: Journal of Nanomaterials
 (2014)

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## Abstract

Bismuth zinc niobium oxide (BZN) was successfully synthesized by a diol-based sol-gel reaction utilizing metal acetate and alkoxide precursors. Thermal analysis of a liquid suspension of precursors suggests that the majority of organic precursors decompose at temperatures up to 150°C, and organic free powders form above 350°C. The experimental results indicate that a homogeneous gel is obtained at about 200°C and then converts to a mixture of intermediate oxides at 350–400°C. Finally, single-phased BZN powders are obtained between 500 and 900°C. The degree of chemical homogeneity as determined by X-ray diffraction and EDS mapping is consistent throughout the samples. Elemental analysis indicates that the atomic ratio of metals closely matches a Bi1.5ZnNb1.5O7 composition. Crystallite sizes of the BZN powders calculated from the Scherrer equation are about 33–98 nm for the samples prepared at 500–700°C, respectively. The particle and crystallite sizes increase with increased sintering temperature. The estimated band gap of the BZN nanopowders from optical analysis is about 2.60–2.75 eV at 500-600°C. The observed phase formations and measured results in this study were compared with those of previous reports.


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## Body

## 1. Introduction

Bismuth oxide based pyrochlore materials are of interest for decoupling capacitors, wireless communications, and low-fired high-frequency filter applications due to their dielectric properties. For these applications, the material is required to have a low sintering temperature and chemical compatibility with the metal electrodes such as silver or copper during cofiring. The dielectric properties of pyrochlore materials strongly depend on the chemical composition and sintering conditions [1].One of the main representatives of bismuth oxide based pyrochlore compounds is bismuth zinc niobium oxide, Bi2O3-ZnO-Nb2O5 (BZN). There are two basic phases in the BZN system: cubic structure Bi1.5ZnNb1.5O7 (α phase) and monoclinic structure Bi2Zn2/3Nb4/3O7 (β phase). Several studies have reported synthesis of various forms of cubic BZN compounds using a variety of synthetic techniques [2–4]. Conventional solid state reaction is the most commonly employed synthesis strategy to prepare both thin film and bulk crystal BZN materials [5, 6]. This technique does not require expensive starting materials and the synthesis process is relatively simple which includes repeated mixing and heating. The main shortcoming of this procedure is that it requires high sintering temperatures (above 950°C) for an extended period of time which leads to a formation of heterogeneous multiphase particles with large crystal sizes due to the lack of stoichiometric control [7].In order to overcome this problem, a number of methods have been used to lower the sintering temperature of the BZN. Firing aids such as CuO and SiO2-B2O3 have been used in the BZN powders synthesis process which have lowered the sintering temperature to 900°C and 800°C, respectively [8, 9]. However, it has been reported that the additives may influence the properties of the final products [10].Other synthetic techniques, generally called wet-chemical, involve the reaction of precursor solutions to prepare the BZN compounds (below 800°C). Depending on the precursor solutions and solvents, this technique is referred to as a metallo-organic deposition route or aqueous solution-gel route [11–14]. The final powders are found to be phase pure and homogeneous with smaller particle and crystallite sizes compared to those obtained by solid state reaction, as expected for lower crystallization and sintering temperatures.The purpose of this research was to prepare chemically homogeneous, phase pure cubic BZN powders with small size at low sintering temperature. To this end, a diol-based sol-gel reaction from an alkoxide route has been successfully employed. During the synthesis process, thermal decomposition studies were carried out to determine the approximate temperature when the phase formation occurred. Crystal structure, elemental homogeneity, and crystallite sizes of the powder samples prepared at different temperatures were thoroughly studied utilizing various techniques. The band gap values of the powders were estimated from the optical absorption data to examine its photocatalytic capabilities.


## 2. Experimental Procedure

### 2.1. Materials

All starting materials used in this experiment were of analytical grade (≥99.9%), purchased from Aldrich (Australia), and used according to the required stoichiometric ratio to prepare cubic BZN structure. Our synthesis process was adapted from the method reported by Singh et al. [12]. Firstly, bismuth acetate (Bi(CH3COO)3) was added to a mixture of organic solvents consisting of 1,3-propanediol (CH2(CH2OH)2) and dried glacial acetic acid (C2H4O2), which was stirred at 60°C. Subsequently, zinc acetate dihydrate (Zn(CH3COO)2·2H2O) was added to the mixture and completely dissolved at 100°C. Niobium ethoxide (Nb(OC2H5)5) was then added dropwise to the mixture to prevent precipitation due to its high reactivity. The mixture was continuously stirred at 60°C overnight. The final product obtained was a yellowish-white, translucent solution, and referred to as a liquid suspension. The synthesis was conducted in an argon glovebox due to the moisture sensitivity of alkoxide reagent. The pH of the mixture was adjusted to 6.0–6.5 with 1 : 1 ratio of organic solvents in order to achieve homogeneous polymeric gels. In subsequent experiments, the liquid suspension was slowly heated at a rate of 2°C min−1 and thermally treated at 350°C for 1 h in a box furnace. The sample was subdivided before further heating at 5°C min−1 to enable the subdivided samples to be annealed at different temperatures in the range of 400–900°C for 1 h.


### 2.2. Characterization

A small amount of the liquid suspension was placed on an open platinum crucible and heated from room temperature to 1000°C in air. A TA Instruments Q500 Thermogravimetric Analysis (TGA) was used for this experiment and a heating rate of 5°C min−1 was adopted. Infrared Emission Spectroscopy (IES) analysis was carried out on a Nicolet Nexus FTS-60A FT-IR spectrometer modified via replacement of the infrared source with an emission cell. A small amount of sample was placed on the top of a platinum nail surface in a nitrogen-purged cell during heating. Temperature control of  ±2°C at the operating temperature of the samples was achieved by using a Eurotherm Model 808 proportional temperature controller attached to the thermocouple. Techniques such as X-ray diffraction (XRD) and backscattered scanning electron microscopy (SEM) combined with Energy-dispersive X-ray spectroscopy (EDS) were used for phase determination and elemental analysis of the powder samples. XRD patterns were collected in Bragg-Brentano geometry using a Philips PANalytical X’Pert PRO X-Ray Diffractometer. The incident X-rays were produced from a PW3373/00 Co X-ray tube operating at 40 kV and 40 mA, providing Kα1 wavelength of 1.7903 Å. Diffraction patterns were collected from 5.0–90° (2θ) with either 0.01 or 0.02 step size, on a spun stage. A LaB6  standard powder was also used as a size/strain standard to calibrate instrumental broadening of diffraction peaks. Secondary electron and backscattered electron images of the surface of powder samples were captured by a Zeiss Sigma FE-SEM and EDS, operating at 20 kV. All samples were coated with gold before analysis to minimize excessive electron buildup. Elemental ratios of the samples were analyzed by Inductively Coupled Plasma with Optical Emission Spectrometers (ICP-OES) analysis. A PerkinElmer Optima 8300 DV Inductively Coupled Plasma Optical Emission Spectrometer was used for this experiment. To dissolve the samples in acid, a known amount of lithium borate was mixed with powders and fused in platinum crucibles. The fusion products were then dissolved in a mixture of 5% of nitric acid and 0.5% hydrofluoric acid. Ultraviolet and Visible (UV-Vis) was used for light absorption analysis from which the band gaps of the samples were calculated. Spectra were recorded on a UV-Vis-NIR Cary 5000 Stheno spectrometer in the 200 to 800 nm region.


## 2.1. Materials

All starting materials used in this experiment were of analytical grade (≥99.9%), purchased from Aldrich (Australia), and used according to the required stoichiometric ratio to prepare cubic BZN structure. Our synthesis process was adapted from the method reported by Singh et al. [12]. Firstly, bismuth acetate (Bi(CH3COO)3) was added to a mixture of organic solvents consisting of 1,3-propanediol (CH2(CH2OH)2) and dried glacial acetic acid (C2H4O2), which was stirred at 60°C. Subsequently, zinc acetate dihydrate (Zn(CH3COO)2·2H2O) was added to the mixture and completely dissolved at 100°C. Niobium ethoxide (Nb(OC2H5)5) was then added dropwise to the mixture to prevent precipitation due to its high reactivity. The mixture was continuously stirred at 60°C overnight. The final product obtained was a yellowish-white, translucent solution, and referred to as a liquid suspension. The synthesis was conducted in an argon glovebox due to the moisture sensitivity of alkoxide reagent. The pH of the mixture was adjusted to 6.0–6.5 with 1 : 1 ratio of organic solvents in order to achieve homogeneous polymeric gels. In subsequent experiments, the liquid suspension was slowly heated at a rate of 2°C min−1 and thermally treated at 350°C for 1 h in a box furnace. The sample was subdivided before further heating at 5°C min−1 to enable the subdivided samples to be annealed at different temperatures in the range of 400–900°C for 1 h.


## 2.2. Characterization

A small amount of the liquid suspension was placed on an open platinum crucible and heated from room temperature to 1000°C in air. A TA Instruments Q500 Thermogravimetric Analysis (TGA) was used for this experiment and a heating rate of 5°C min−1 was adopted. Infrared Emission Spectroscopy (IES) analysis was carried out on a Nicolet Nexus FTS-60A FT-IR spectrometer modified via replacement of the infrared source with an emission cell. A small amount of sample was placed on the top of a platinum nail surface in a nitrogen-purged cell during heating. Temperature control of  ±2°C at the operating temperature of the samples was achieved by using a Eurotherm Model 808 proportional temperature controller attached to the thermocouple. Techniques such as X-ray diffraction (XRD) and backscattered scanning electron microscopy (SEM) combined with Energy-dispersive X-ray spectroscopy (EDS) were used for phase determination and elemental analysis of the powder samples. XRD patterns were collected in Bragg-Brentano geometry using a Philips PANalytical X’Pert PRO X-Ray Diffractometer. The incident X-rays were produced from a PW3373/00 Co X-ray tube operating at 40 kV and 40 mA, providing Kα1 wavelength of 1.7903 Å. Diffraction patterns were collected from 5.0–90° (2θ) with either 0.01 or 0.02 step size, on a spun stage. A LaB6  standard powder was also used as a size/strain standard to calibrate instrumental broadening of diffraction peaks. Secondary electron and backscattered electron images of the surface of powder samples were captured by a Zeiss Sigma FE-SEM and EDS, operating at 20 kV. All samples were coated with gold before analysis to minimize excessive electron buildup. Elemental ratios of the samples were analyzed by Inductively Coupled Plasma with Optical Emission Spectrometers (ICP-OES) analysis. A PerkinElmer Optima 8300 DV Inductively Coupled Plasma Optical Emission Spectrometer was used for this experiment. To dissolve the samples in acid, a known amount of lithium borate was mixed with powders and fused in platinum crucibles. The fusion products were then dissolved in a mixture of 5% of nitric acid and 0.5% hydrofluoric acid. Ultraviolet and Visible (UV-Vis) was used for light absorption analysis from which the band gaps of the samples were calculated. Spectra were recorded on a UV-Vis-NIR Cary 5000 Stheno spectrometer in the 200 to 800 nm region.


## 3. Results and Discussion

Thermal analysis of a liquid suspension was started from room temperature and completed at 1000°C. Figure1 shows the dTG/TG analysis results. A large exothermic dTG peak were obtained at 80 and 145°C, which corresponds to about 83% of the total mass loss. This large mass loss was due to the evaporation of water and residual organic solvents contained within the precursor solution. The thermal decomposition study revealed that two small dTG peaks were observed at about 250 and 330°C. This slow and constant mass decay consisted of about 4% mass loss. The dTG/TG curves show that the main decomposition of the organic precursors occurred just before 150°C and continuously occurred until 330°C.Figure 1
TG/dTG curves of the liquid suspension.This result was quite similar to Wang’s reported experimental work [11]. However, there was a weak exothermic peak obtained at about 545°C, which was not observed in this experimental result. Other authors’ works on thermal decomposition of the BZN powders showed that there were significant weight losses observed above 500°C [13, 14]. From this experiment result, no other significant mass loss was observed from the TG curve as the temperature was increased up to 1000°C, indicating limited or no volatility of bismuth or other metals. This result suggested that the majority of the organic precursors decomposed before the gel sample formed at about 200°C, and continued until 350°C, which resulted in the formation of organic free metal oxide powders.TGA analysis on the liquid suspension was further confirmed by IES analysis. Figure2 shows that the sample consisted of residual organic compounds which were completely lost before the dried powder formed at 350°C. In the IES spectra, the C–C and C–O stretches were observed between 1000 cm−1 and 1300 cm−1. Two peaks were also found at 2700 cm−1 and 2800 cm−1 which were due to either –O–CH3 or –O–CH2–O– groups. Moreover, –CH2 and –CH3 bands were clearly observed in the spectra at 2850–2950 cm−1 and 1450–1475 cm−1, respectively. These were due to CH2(CH2OH)2 and CH3COOH species in the precursor solution.Figure 2
IES spectra of the liquid suspension heated from 200 to 400°C.As expected, when the sample was heated to 200–250°C, the above mentioned bands were observed in the spectrum but significantly declined in intensity at 300°C. However, the spectra were relatively featureless after the sample was heated above 350°C, presumably due to the formation of the metal oxides. Such metal oxides were expected to show features in their vibrational spectrum below the 500 cm−1 limit of the instrument. The IES result suggested that the organic groups from the precursors, as well as water from the reaction, completely evaporated from the liquid suspension as temperature was increased. Thus, organic free metal oxide powders formed from 350°C onwards. The backscattered SEM micrograph and EDS mapping images of the powder samples prepared at 400°C are shown in Figure 3. It can be seen from the SEM micrographs that the particles of the powders had sizes ranging from 0.5 to 3 μm. The SEM backscattering image in Figure 3(a) also shows some uneven elemental distribution in the sample indicating some phase separation. Elemental analysis on several areas confirmed that the bismuth and niobium atoms were not completely uniformly distributed. The EDS mapping image in Figure 3(b) also confirmed this observation. The distribution of bismuth, niobium and oxygen atoms were even throughout the sample. However, zinc atoms predominated in some areas creating small pockets of impurities. This indicated that the sample contained two or more phases; one mainly consisting of bismuth and niobium atoms, and another which was rich in zinc.Backscattered SEM (a) and EDS mapping (b) images of the powder sample prepared at 400°C (Bi: blue, Nb: green, Zn: purple, and O: red).
(a)
(b)Figure4 shows SEM micrographs and elemental mapping of the BZN powder samples prepared at 900°C. It can be seen in Figure 4(a) that much bigger microcrystalline particles were present in this sample when compared to particles obtained at lower temperature. Elemental distribution of each metal atom on the surface of the particles looked relatively homogeneous. However, the color differences in the EDS mapping in Figure 4(b) clearly showed the presence of small amounts of impurities. These impurities were maybe due to excess of unreacted metals such as zinc or bismuth that were rejected from the BZN particles.Backscattered SEM (a) and EDS mapping (b) images of the BZN powders prepared at 900°C (Bi: purple, Nb: light blue, and Zn: yellow).
(a)
(b)XRD patterns of the powder samples prepared between 350 and 900°C are shown in Figure5. The XRD pattern obtained from the sample prepared at 350°C indicated that the sample contained large amounts of an amorphous phase in addition to a crystalline phase. The obtained pattern matched closely that of orthorhombic bismuth niobium oxide, Bi7.84Nb0.16O12.16. The XRD pattern was unchanged when the sample was reheated at 400°C. This suggested that two binary oxides were formed during low temperature sintering processes. ICP-OES analysis was carried out on the sample and gave as a result: Bi7.84Nb1.61ZnO14.786. The difference between the ICP-OES and the XRD pattern suggested that the amorphous phase might be niobium zinc oxide, Nb1.45ZnO2.625.Figure 5
XRD patterns of the powder samples at various temperatures.Phase transformation occurred as the sintering temperature was increased. Low temperature intermediate oxides directly converted to the singe-phased crystals from 500°C onwards. This phase was identified as cubic BZN compound (JCPDS PDF, 00-054-0971). The elemental analysis of the powder sample was carried out by ICP-OES and the result suggested that the atomic ratio was closely matched with cubic Bi1.5ZnNb1.5O7 composition. The observed phase transformation from intermediate oxides to the single-phased BZN in this study is slightly different from those of other reported works [11–14]. The cubic BZN powders formed at 450°C straight from the precursor gels, and then fully crystallized at 550-600°C [11–14]. In another work, a small amount of residual amorphous phase was obtained besides BZN [14]. Other reports suggested that the cubic BZN phase was obtained at about 500°C [11, 13]; however, there was a small amount of Bi2O3 also present. This was because Bi2O3 phase was first formed at 400°C in those studies.Nonetheless, the crystals of the BZN powder samples obtained in this study between 500 and 700°C were phase pure with broad peak widths, indicating small and/or disordered crystallites. The crystallite sizes of the powders were calculated from the Scherrer equation using selected diffraction peaks. The calculated sizes of the powders were 33, 72 and 98 nm for 500, 600 and 700°C, respectively. This result was similar with reported values of 30–90 nm at 450–700°C [11]. However, it was relatively larger than that obtained by another group reporting 13–36 nm at 500–700°C [14].Similarly, the XRD patterns of the powders prepared at higher temperatures, 800–900°C, were also identified as cubic BZN compound. However, small amounts of impurities were found to co-exist with the main BZN phase. Other research has suggested that the low temperature BZN phase might have a composition of Bi1.5Zn0.5Nb1.5O6.8 which undergoes a peritectoid decomposition at about 700°C to high temperature phases of Bi1.5ZnNb1.5O7  and BiNbO4 [15]. In this study, however, the small impurity observed at high temperatures corresponds to ZnO [16]. With increasing temperature, the peak widths significantly narrowed, indicating the formation of larger crystals.The UV-Vis spectra of the powder samples heated at different temperatures of 350–600°C are shown in Figure6. The band gaps of each sample can be estimated from the optical reflectance data to evaluate the direct transition between the valence band and the conduction band. Approximate band gaps of 2.25–2.29 eV were estimated form the absorbance spectra of mixed intermediate oxides obtained at 350–400°C. The optical band gap values estimated from extrapolation to zero of absorption versus photon energy plot, and those increased when the sample was prepared at higher temperatures.Figure 6
UV-Vis spectra of the powder samples at various temperatures.The optical band gaps of the single-phased BZN powders formed at 500 and 600°C were 2.60 and 2.75 eV, respectively. This result was slightly larger than the reported value by Zanetti et al. (3.0-3.1 eV at 500–700°C) [13]. The optical analysis result showed that the band gaps of the samples widened when the powders were prepared at high temperatures of above 600°C. Such wide band gap values might be caused by the effect of bigger crystallite size due to the high sintering temperature. This study also suggests that the phase pure BZN powders have an optical absorption at wavelengths of 450 nm, indicating that this nanostructured material can be responsive only to the UV/Vis light region.


## 4. Conclusion

A diol-based sol-gel synthesis method was successfully employed for the preparation of phase pure cubic BZN nanopowders. Thermal analysis results showed that most decomposition in the precursors occurred up to 150°C, and it was completed before 350°C. The results also indicated that organic free powders were obtained at 350–400°C. Low temperature intermediate oxides were examined by elemental analysis and found to be a mixture of bismuth niobium oxide and niobium zinc oxide. These oxides then directly transformed to the single-phased BZN with increasing temperature. This finding was contrary to that of sol-gel methods in the literature, where a different phase mixture was obtained at low temperature. However, our result was similar to that reported for a solid state method, where the mixture of phases before BZN formation was comparable to ours. Measured crystallite sizes and band gaps of the BZN powders obtained from this study are in close agreement with the reported values. The optical study suggested that the BZN compound may be photoactive in the UV/Vis light region.



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*Source: 695973-2014-11-05.xml*