# Structural Characterization and Magnetic Properties of Undoped and Ti-Doped ZnO Nanoparticles Prepared by Modified Oxalate Route

Authors: Ekane Peter Etape; Josepha Foba-Tendo; Lambi John Ngolui; Beckley Victorine Namondo; Fomogne Cyrille Yollande; Marius Borel Nguefack Nguimezong
Journal: Journal of Nanomaterials
 (2018)

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## Abstract

Ti-doped zinc oxide and pure zinc oxide nanoparticles were synthesized by a modified oxalate route usingAverrhoa carambola fruit juice as a natural source of oxalate. The characteristics of the precursors have been investigated by FTIR, TGA, and XRD. The results from the investigation revealed that the precursors are zinc oxalate and Ti-doped zinc oxalate which readily decompose at 450°C. The as-prepared precursors were calcined at 450°C for 4 hours, and the decomposition products have been characterized by XRD, SEM, EDX, and VSM. XRD results revealed crystallinity with hexagonal wurtzite structure, while the average grain size was found to be 26 nm for Ti-doped ZnO and 29 nm for ZnO, using calculations based on Debye-Scherrer equation. Furthermore, the morphological studies by SEM showed particle agglomeration, while the presence of Ti3+ in the zinc oxide lattice is indicated by EDS analysis. Finally the hysteresis loop from VSM results shows that Ti-doped ZnO exhibits ferromagnetism.


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## Body

## 1. Introduction

The magnetic properties of nanomaterials used in semiconductors seem to result from their ability to manipulate electron spins. These properties have been exploited in dilute magnetic semiconductor materials [1]. Zinc oxide is one of such materials that have received special interest because it has both charge and spin degrees of freedom in a single matrix, which lead to the interplay of functionalities (magnetic and electronic). Also the oxalates from the 3d metals such as zinc are isomorphous in nature, which enables the enhancement of physical properties of oxide semiconductors by doping the precursor in the course of synthesis [2–6]. Many research groups that have worked on doping with transition metals have used zinc oxide as a good host material for realizing wide band-gap dilute magnetic semiconductors. Furthermore, some special interest in titanium has been shown because neither titanium nor its oxides are ferromagnetic, but calculations of the electronic structure of Ti-doped ZnO have confirmed experimentally [7] and indicated the likelihood of titanium to order ferromagnetically in ZnO. However, to generate Ti-doped ZnO with good functional properties for industrial scale production, control of purity, morphology, size, and size distribution, and relatively simple and cost effective synthetic methods are required.Several methods have been used for ZnO synthesis such as chemical precipitation in water solution [8], hydrothermal synthesis [9], sol-gel process [10], precipitation from microwave [11], and thermal evaporation [12] process. These methods have given products with particles differing in shape, size, and spatial structure. Metallurgical processes obtained zinc oxide from roasting of zinc ores as reported by the international organization for standardization (SIO). This method of synthesis is called the direct (American) process or the indirect (French) process where zinc is melted in a furnace and vaporized at 910°C. This method was popularized by Le Claire in 1844, and the products consisted of agglomerations with average particle size ranging from 0.1 to a few microns [13]. The high temperatures involved make the process costly and this has encouraged the use of other methods operating at relatively lower temperatures. Also there is the mechanochemical process [14] which is cheap and simple, works at low temperature, and yields nanoparticles at an industrial scale, but uniform grinding of particles to the required size leads to longer processing time and greater quantity of impurities. The sol-gel methods reported have attracted a lot of interest in view of their simplicity, low cost, reliability, reproducibility, and relatively mild conditions of synthesis which make easy surface modification of zinc oxide with selected organic compounds. Benhebal et al., 2013, [15] produced zinc oxide powder by sol-gel method from zinc acetate dihydrate and oxalic acid, using ethanol as solvent. The zinc oxide obtained had a hexagonal wurtzite structure with the particles having a spherical shape, but the use of organic solvents makes the method relatively cost ineffective and environmentally questionable. Controlled precipitation is a widely used method for the generation of zinc and other metal oxide nanoparticles [16]. The method is fast and spontaneous, with the possibility of controlling particle size, but breaking down agglomerates remains a drawback [17]. Hong et al., 2006 [18], and Lanje et al. [19], 2013, reported on a cost effective and simple precipitation process for the synthesis of zinc oxide which could be used in the large scale production of pure zinc oxide particles. The microemulsion method [20] operates at low temperature 140°C and generates hexagonal (wurtzite) structure; particles morphology: needle (L: 150–200 nm, D: ~55 nm), nanocolumns (L: 80–100 nm, D: 50–80 nm), spherical shape (~45 nm). However, the conditions of the process (temperature, substrates, and ratio of two-phase components) affect the size of the particles and the location of their phases.The modified solvothermal method using oxalate precursor has many advantages (it is cost effective and simple and produces pure and homogeneous nanoparticles [6]). However, a precipitation process which makes use of a natural source of precipitating agent could be more cost effective and environmentally appropriate. We have developed some special interest in the implementation of an environmentally friendly process which involves the use of renewable material sources such as fruit juices. Some of the fruit juices, likeAverrhoa carambola, are very rich in organic acid (namely, oxalic acid), which can serve as ligand species for the precipitation of precursors for metal oxides. The concept is being developed and has proven to be an efficient one [21, 22]. In this paper, we follow the steps of our previous work [21, 22] and report for the first time the synthesis of doped metal oxide (Ti-doped ZnO) by a relatively low temperature method which involves the pyrolysis of a precursor by a coprecipitation route in aqueous solution using an oxalate ligand from a natural source (A. carambola fruit juice) as the precipitating agent. The nanoparticles have been characterized by powder X-ray diffraction, thermogravimetry, Fourier Transform Infrared (FTIR) spectroscopy, and scanning electron microscopy coupled to an EDAX, and magnetic properties have also been investigated.


## 2. Experimental

### 2.1. Materials and Methods

Titanium trichloride (20% in 3% Hydrochloric acid) (Alfa Aesar, Germany) and zinc chloride (MERCK) were of analytical grade and were used without further purification.Averrhoa carambolajuice (source of the precipitating agent) processed as described elsewhere [21] was also used.


#### 2.1.1. Synthesis and Thermal Decomposition of Zinc and Titanium-Doped Zinc Oxalates

Zinc and titanium-doped zinc complexes (ZZ and ZT, where Z = Zn and T = Ti) were prepared from zinc chloride and titanium chloride usingAverrhoa carambolajuice as the source of the precipitating agent. 0.04 M solution of the various metal ions (Zn2+ and Ti3+) was prepared by dissolving the appropriate amount of the metal chloride in 200 mL of distilled water. The metal ion solutions were then mixed in appropriate Zn2+ : Ti3+ ratios (see Table 1) and stirred to homogenize.Averrhoa carambolafruit juice (see Table 1, for volumes) was poured into a 400 mL round bottom flask and maintained under magnetic stirring at ambient temperature. The metal ion solution was slowly added to the juice while stirring at room temperature and the mixture stirred for a further four hours. The solutions obtained (white for ZZ and greenish for ZT) were aged for eight (08) hours, filtered, washed successively with distilled water and ethanol, and then dried in an oven at 80°C for one hour. The decomposition products zinc oxide and titanium-doped zinc oxide (ZZd and ZTd, resp.) were obtained by calcination of the precursors zinc oxalate and titanium-doped zinc oxalate (ZZ and ZT resp.). ZZ and ZT were placed in ceramic combustion boat holders and maintained into a preheated muffle oven for four hours at 450°C under air. Table 1 gives a quantitative and qualitative description of the various samples prepared, and the flow chart of the synthesis is shown in Figure 1.Table 1
Quantitative and qualitative description of the various samples prepared.
Code 0.04 M ZnCl2 (mL) 0.04 M TiCl3 (mL) A. carambola juice (mL) ZZ 100 0 200 ZT 88 12 200Figure 1
Flow diagram for the synthesis route of the materials.


#### 2.1.2. Characterization Techniques

Fourier Transform Infrared (FTIR) spectra were recorded from 4000 to 400 cm−1 on a PerkinElmer Spectrum Two Universal Attenuated Total Reflectance Fourier Transform Infrared (UATR-FTIR) spectrometer, while thermogravimetric analysis (TGA) was obtained using a Pyris 6 PerkinElmer TGA 4000 thermal analyzer. The TGA analysis was conducted between 30 and 900°C under nitrogen atmosphere at a flow rate of 20 mL/min and a temperature ramp of 10°C/min, while the XRD diffractogram of the precursors and the decomposition products were recorded on a Bruker D8 advance X-ray diffractometer using a Cu Kα radiation source (λ = 0.15406 nm, 40 kV, and 40 mA). Scans were taken over the 2θ range from 10°C to 100°C in steps of 0.01°C at room temperature in open quartz sample holders. The phases were identified with the help of a Bruker DIFFRAC plus evaluation software in combination with the ICDD (International Centre for Diffraction Data) powder diffraction database. The surface morphology of the samples was examined by a Scanning Electron Microscope (SEM) JEOL JSM-5600 while the elemental analysis was carried out using the same machine fitted with an EDAX DX-4 microanalysis system with an energy dispersive spectrometer (EDX). Prior to examination, samples were prepared by mounting about 0.5 mg of powder onto a 5 mm × 5 mm double sided carbon tape, on an aluminum stub. The powder was then sputter-coated for 40 seconds with gold. The magnetic measurement was performed on the commercial vibrating sample magnetometer (VSM) Lakeshore (model 73009). The magnetic hysteresis loops were measured at room temperature with maximal applied magnetic field up to 0.95 T. Magnetic field sweep rate was kept at 5 Oe/s so that the measurement of the hysteresis loop with maximum field of 0.989 t was taken from an interval of three hours. The saturation magnetization, coercivity, and remanent magnetization are obtained from hysteresis loop.


## 2.1. Materials and Methods

Titanium trichloride (20% in 3% Hydrochloric acid) (Alfa Aesar, Germany) and zinc chloride (MERCK) were of analytical grade and were used without further purification.Averrhoa carambolajuice (source of the precipitating agent) processed as described elsewhere [21] was also used.


### 2.1.1. Synthesis and Thermal Decomposition of Zinc and Titanium-Doped Zinc Oxalates

Zinc and titanium-doped zinc complexes (ZZ and ZT, where Z = Zn and T = Ti) were prepared from zinc chloride and titanium chloride usingAverrhoa carambolajuice as the source of the precipitating agent. 0.04 M solution of the various metal ions (Zn2+ and Ti3+) was prepared by dissolving the appropriate amount of the metal chloride in 200 mL of distilled water. The metal ion solutions were then mixed in appropriate Zn2+ : Ti3+ ratios (see Table 1) and stirred to homogenize.Averrhoa carambolafruit juice (see Table 1, for volumes) was poured into a 400 mL round bottom flask and maintained under magnetic stirring at ambient temperature. The metal ion solution was slowly added to the juice while stirring at room temperature and the mixture stirred for a further four hours. The solutions obtained (white for ZZ and greenish for ZT) were aged for eight (08) hours, filtered, washed successively with distilled water and ethanol, and then dried in an oven at 80°C for one hour. The decomposition products zinc oxide and titanium-doped zinc oxide (ZZd and ZTd, resp.) were obtained by calcination of the precursors zinc oxalate and titanium-doped zinc oxalate (ZZ and ZT resp.). ZZ and ZT were placed in ceramic combustion boat holders and maintained into a preheated muffle oven for four hours at 450°C under air. Table 1 gives a quantitative and qualitative description of the various samples prepared, and the flow chart of the synthesis is shown in Figure 1.Table 1
Quantitative and qualitative description of the various samples prepared.
Code 0.04 M ZnCl2 (mL) 0.04 M TiCl3 (mL) A. carambola juice (mL) ZZ 100 0 200 ZT 88 12 200Figure 1
Flow diagram for the synthesis route of the materials.


### 2.1.2. Characterization Techniques

Fourier Transform Infrared (FTIR) spectra were recorded from 4000 to 400 cm−1 on a PerkinElmer Spectrum Two Universal Attenuated Total Reflectance Fourier Transform Infrared (UATR-FTIR) spectrometer, while thermogravimetric analysis (TGA) was obtained using a Pyris 6 PerkinElmer TGA 4000 thermal analyzer. The TGA analysis was conducted between 30 and 900°C under nitrogen atmosphere at a flow rate of 20 mL/min and a temperature ramp of 10°C/min, while the XRD diffractogram of the precursors and the decomposition products were recorded on a Bruker D8 advance X-ray diffractometer using a Cu Kα radiation source (λ = 0.15406 nm, 40 kV, and 40 mA). Scans were taken over the 2θ range from 10°C to 100°C in steps of 0.01°C at room temperature in open quartz sample holders. The phases were identified with the help of a Bruker DIFFRAC plus evaluation software in combination with the ICDD (International Centre for Diffraction Data) powder diffraction database. The surface morphology of the samples was examined by a Scanning Electron Microscope (SEM) JEOL JSM-5600 while the elemental analysis was carried out using the same machine fitted with an EDAX DX-4 microanalysis system with an energy dispersive spectrometer (EDX). Prior to examination, samples were prepared by mounting about 0.5 mg of powder onto a 5 mm × 5 mm double sided carbon tape, on an aluminum stub. The powder was then sputter-coated for 40 seconds with gold. The magnetic measurement was performed on the commercial vibrating sample magnetometer (VSM) Lakeshore (model 73009). The magnetic hysteresis loops were measured at room temperature with maximal applied magnetic field up to 0.95 T. Magnetic field sweep rate was kept at 5 Oe/s so that the measurement of the hysteresis loop with maximum field of 0.989 t was taken from an interval of three hours. The saturation magnetization, coercivity, and remanent magnetization are obtained from hysteresis loop.


## 2.1.1. Synthesis and Thermal Decomposition of Zinc and Titanium-Doped Zinc Oxalates

Zinc and titanium-doped zinc complexes (ZZ and ZT, where Z = Zn and T = Ti) were prepared from zinc chloride and titanium chloride usingAverrhoa carambolajuice as the source of the precipitating agent. 0.04 M solution of the various metal ions (Zn2+ and Ti3+) was prepared by dissolving the appropriate amount of the metal chloride in 200 mL of distilled water. The metal ion solutions were then mixed in appropriate Zn2+ : Ti3+ ratios (see Table 1) and stirred to homogenize.Averrhoa carambolafruit juice (see Table 1, for volumes) was poured into a 400 mL round bottom flask and maintained under magnetic stirring at ambient temperature. The metal ion solution was slowly added to the juice while stirring at room temperature and the mixture stirred for a further four hours. The solutions obtained (white for ZZ and greenish for ZT) were aged for eight (08) hours, filtered, washed successively with distilled water and ethanol, and then dried in an oven at 80°C for one hour. The decomposition products zinc oxide and titanium-doped zinc oxide (ZZd and ZTd, resp.) were obtained by calcination of the precursors zinc oxalate and titanium-doped zinc oxalate (ZZ and ZT resp.). ZZ and ZT were placed in ceramic combustion boat holders and maintained into a preheated muffle oven for four hours at 450°C under air. Table 1 gives a quantitative and qualitative description of the various samples prepared, and the flow chart of the synthesis is shown in Figure 1.Table 1
Quantitative and qualitative description of the various samples prepared.
Code 0.04 M ZnCl2 (mL) 0.04 M TiCl3 (mL) A. carambola juice (mL) ZZ 100 0 200 ZT 88 12 200Figure 1
Flow diagram for the synthesis route of the materials.


## 2.1.2. Characterization Techniques

Fourier Transform Infrared (FTIR) spectra were recorded from 4000 to 400 cm−1 on a PerkinElmer Spectrum Two Universal Attenuated Total Reflectance Fourier Transform Infrared (UATR-FTIR) spectrometer, while thermogravimetric analysis (TGA) was obtained using a Pyris 6 PerkinElmer TGA 4000 thermal analyzer. The TGA analysis was conducted between 30 and 900°C under nitrogen atmosphere at a flow rate of 20 mL/min and a temperature ramp of 10°C/min, while the XRD diffractogram of the precursors and the decomposition products were recorded on a Bruker D8 advance X-ray diffractometer using a Cu Kα radiation source (λ = 0.15406 nm, 40 kV, and 40 mA). Scans were taken over the 2θ range from 10°C to 100°C in steps of 0.01°C at room temperature in open quartz sample holders. The phases were identified with the help of a Bruker DIFFRAC plus evaluation software in combination with the ICDD (International Centre for Diffraction Data) powder diffraction database. The surface morphology of the samples was examined by a Scanning Electron Microscope (SEM) JEOL JSM-5600 while the elemental analysis was carried out using the same machine fitted with an EDAX DX-4 microanalysis system with an energy dispersive spectrometer (EDX). Prior to examination, samples were prepared by mounting about 0.5 mg of powder onto a 5 mm × 5 mm double sided carbon tape, on an aluminum stub. The powder was then sputter-coated for 40 seconds with gold. The magnetic measurement was performed on the commercial vibrating sample magnetometer (VSM) Lakeshore (model 73009). The magnetic hysteresis loops were measured at room temperature with maximal applied magnetic field up to 0.95 T. Magnetic field sweep rate was kept at 5 Oe/s so that the measurement of the hysteresis loop with maximum field of 0.989 t was taken from an interval of three hours. The saturation magnetization, coercivity, and remanent magnetization are obtained from hysteresis loop.


## 3. Results and Discursion

### 3.1. FTIR

Figure2 Shows the FTIR spectra of oxalate precursors synthesized by coprecipitation usingA. Carambolafruit juice as precipitating agent. The spectra of the precursors (ZZ and ZT) are very similar with weak IR bands occurring around 3363 cm−1 corresponding to the stretching vibrations of the -OH group associated with the presence of water of crystallization. The presence of the water of crystallization is confirmed by the H-O-H bending vibration observed at 737 cm−1. The Infrared bands observed below 1700 are assigned to the oxalate vibrational modes [21, 22] (the sharp intense peaks at 1620 cm−1 are attributed to the asymmetric stretching vibrations of the OCO group, while those around 1450–1300 cm−1 are attributed to the asymmetric (C=O) and symmetric (C-O) stretching vibrations in the OCO group). The sharp medium intense peaks at 826 cm−1 and 737 cm−1 confirm the bonding of metal oxygen (M-O) (indicating the presence of Zn2+ and Ti3+ bonded to the oxalate ion) and are assigned to (Vo-c=o + δZn-O) and (δTi-O + Vo-c=o). Moreover, the absence of the free IR VC=O, vibration expected at 1735–1705 cm−1, suggests that the entire carboxylate group of the oxalate is engaged in the formation of the coordination compound. On incorporating Ti+3 into the ZnO lattice sites, shifting of bands to lower wavenumbers is observed. This may be as a result of the bond weakening (increase in bond length) [23].Figure 2
FTIR of the precursors: zinc complex (ZZ) and titanium-doped zinc complex (ZT).


### 3.2. Thermal Analysis (TGA/DTG)

The thermal decomposition of zinc oxalate (ZZ) and Ti-doped zinc oxalate (ZT) precursors was carried out within the same temperature range of 30–650°C (as shown in Figure3). The decomposition of Tix-Zni-xC2O4 occurs in two steps (Figure 3(a)). The initial step is the dehydration process which takes place in two steps. The first step occurred in the temperature range 30–125°C (1) and the second step in the range 125–220°C (2). The dehydration steps for both the pure and the doped ZnC2O4 occurred within the same temperature range although the doped sample started dehydrating at a lower temperature, which revealed the relative instability of the doped crystal [23]. The measured weight loss for the first segment of the first step is about 4.5% of the total weight resulting in the elimination of half a molecule of water. The measured weight loss for the second segment of the first step is about 13.71%, which results in the elimination of one and a half molecules of water.Figure 3 (a)
Thermogram of Ti-doped zinc oxalate (ZT) (b)
Thermogram of zinc oxalate (ZZ)The total weight of water of crystallization in the pure sample (19.02%) decreases (to 18.51%) following the incorporation of Ti+3 in the zinc oxalate crystal. This shows that on introducing titanium ion, water of crystallization decreases. The reduction in the water of crystallization could be attributed to H-bonding between the particles (on introducing Ti as dopant, the lattice contracts leading to a decrease in particle size and reduction in the H-bonding between the particles). (1)Tix-Zn1-xC2O4·2H2O⟶Tix-Zn1-xC2O4·32H2O+12H2O(2)Tix-Zn1-xC2O4·32H2O⟶Tix-Zn1-xC2O4+32H2OThe second step, like the first, has also two segments. The first segment occurred in the temperature range 230–430°C and corresponds to the decomposition of the anhydrous doped oxalate, eliminating carbon monoxide (3). The last segment is the decarboxylation process, which occurred in the temperature range 430–650°C and constitutes the decomposition of the carbonate to the corresponding metal oxides (4). (3)TixZn1-xC2O4⟶TixZn1-xCO3+CO(4)TixZn1-xCO3⟶TixZn1-xO+CO2Looking at the DTG, there is no apparent difference in the thermal decomposition patterns of the pure and the Ti added sample (ZT). Just like the Ti free sample (ZZ), the thermogram of ZT shows two well defined weight loss steps. Cong et al. [2] and Ahmad et al. [24] made similar observations for Mn-Zn oxalate. The first (19.29%) around 125–220°C is attributed to the loss of two molecules of water of crystallization (cf. 19.23%), while the second (36.80%) found between 400 and 480°C is attributed to the release of one molecule of each of CO2 and CO (cf. 39.45%) giving a difference of 2.65%. The difference suggests that decomposition of ZT is not actually complete at 450°C. This observation could be attributed to the more stable TiCO3 which holds back some proportion of CO2. A closer view of the thermogram (TGA and DTG) for ZT reveals a little weight loss portion around 600°C which could accounts for the complete decomposition of ZT to ZTd. However calcinations of both ZZ and ZT at 450°C for 4 hours gives the final decomposition products (ZZd and ZTd).


### 3.3. XRD/EDS/SEM Characterization

#### 3.3.1. X-Ray Diffraction

Figures4 and 5 show, respectively, the room temperature powder X-ray diffraction spectra for the oxalate precursors (ZZ and ZT) and the decomposition products (ZZd and ZTd). All the reflections in the pattern could be indexed to the zinc oxalate (JCPDS card number 25-1029), Table 2, and monophasic zinc oxide hexagonal wurtzite structure (JCPDS card number 36-1451), Table 3, respectively. The diffraction patterns for sample ZZ and ZT are virtually indifferent and matched perfectly with JCPDS card number 25-1029 for zinc oxalate dehydrate. This is in conformity with FTIR results which indicated the presence of water of hydration. The peaks in the spectra of both ZZd and ZTd matched perfectly with JCPDS card number 36-1451 for hexagonal wurtzite ZnO structure, shown in Table 3. (No impurity peaks were observed as no peak from the patterns of the decomposed sample ZTd matched JCPDS card number 84-1286 for TiO2 anatase phase and JCPDS card number 75-1753 rutile phase.) However, the diffraction peaks of Ti-doped ZnO are shifted to lower angles with respect to those of ZnO, which suggests some changes in the ZnO matrix resulting from the substitution of Ti for some Zn. The substitution is confirmed by the EDS spectrum shown in Figure 6, which shows that the composition of ZTd to be Ti, Zn, and O. Therefore, for the dopant proportion, Ti did not bring any change in the crystal structure of ZnO since there was complete incorporation of Ti into the ZnO structure by substituting for some of the Zn. This phenomenon was earlier observed by other groups for Ti-doped ZnO nanoparticle [25] and films [2], and they attributed the shift in 2θ values to a distortion of the ZnO crystallite when Ti substitutes for Zn since Ti4+ radius is lower than that of Zn2+. Therefore, the formula of ZTd and ZZd could be written as Zn0.958Ti0.042O and ZnO, respectively. The crystallite size was estimated from X-ray line broadening studies using (101) reflections with the help of the Debye-Scherer’s equation (5) and was found to be 29 nm and 26 nm for pure and doped ZnO, respectively.(5)D=kλβcos⁡θ,where D is the crystallite size, k is the correction factor that accounts for the shape of the particles, λ is the wavelength of the XRD beam (here λ = 0.15406 nm), β is the full width at half maximum (FWHM) of the peak, and θ is the Bragg’s diffraction angleTable 2
PXRD data for the precursors (ZZ and ZT) indexed with JCPDS card number 25-1029 for zinc oxalate dehydrate.
JCPDS no. 25-1029 ZZ/ZT h k l d  (Å) Intensity 2θ d  (Å) Intensity −202 4.77 100 18.27 4.85 100 002 3.6 35 22.83 3.89 31 −113 2.65 35 33.38 2.67 16 021 2.55 25 35.12 2.54 24 022 2.22 30 40.53 2.24 21 221 2.03 18 43.67 2.07 16 023 1.88 25 48.43 1.87 19Table 3
PXRD data for the decomposition products (ZZd and ZTd) indexed with JCPDS card number 36-1451 for wurtzite ZnO.
JCPDS no. 36-1451 ZnO wurtzite structure ZZd ZTd 2θ h k l 2θ Relative intensity 2θ Relative intensity 31.749 100 31.8 71.7 32.307 58.85 34.228 002 34.46 50.94 34.82 48.83 36.257 101 36.3 100 36.6 100 47.257 102 47.62 19.81 48.02 26.68 110 56.66 19.81 57.15 46.72 103 62.94 18.87 63.25 38.71Figure 4
XRD of the precursors: zinc oxalate (ZZ) and Ti-doped zinc oxalate (ZT).Figure 5
XRD of the decomposition products of the zinc complex (ZZd) and the titanium-doped zinc complex (ZTd).Figure 6
The EDS of the decomposition products, zinc oxide (ZZd), and the titanium-doped zinc oxide (ZTd).
(a) (b)The SEM images of ZZd (ZnO) and ZTd (Ti-doped ZnO) are shown in Figures7(a) and 7(b). A high degree of particle agglomeration is observed, which is in agreement with literature [2]. The SEM images for the calcined products at 450°C for 4 hours are shown in Figures 7(c) and 7(d). On the one hand, ZZd (ZnO) is present as regular polyhedral particles with the hexagonal shape of the wurtzite structure observed in PXRD, while, on the other hand, ZTd (Ti-doped ZnO) shows spherical particulates with some level of agglomeration and an average agglomerate size of about 2 μm in width and 4 μm in length. The fact that agglomerates showed sizes in the range of 2 μm indicates that the particulates are in the nanometer range which conforms to the XRD results.Figure 7 (a)
SEM image of ZZd (ZnO) (b)
SEM image of ZTd (Ti-doped ZnO) (c)
SEM image of calcined, ZZd (ZnO) (d)
SEM image of calcined, ZTd (Ti-doped ZnO)


### 3.4. Vibrating Sample Magnetometry (VSM)

The magnetic behavior of the nanoparticles was investigated by plotting the magnetic moment as a function of the applied magnetic field measured at a temperature of 5 k while the magnitudes of the magnetic properties obtained from the hysteresis loop are shown in Table4. The observed curve shows a hysteresis (Figure 8), which indicates the existence of ferromagnetic ordering in the sample. The solid solution shows saturated magnetization (Ms) of 6.89 emu/g, remnant magnetization (Mr) of 7.93 emu/g at room temperature, and a coercive force (Hc) of ZTd of 1.500 (Oe) which could be attributed to the tiny nature of the as-prepared ZTd particles [26, 27]. The squareness (remanence ratio) Mr/Ms for the sample was determined and the value obtained was 0.012.Table 4
The magnitudes of the magnetic properties obtained from the hysteresis loop.
Hysteresis loop Upward part Downward part Average Parameter “definition” H c Oe −9999.000 - 9996.000 - 1.500 Coercive field, field at whichM//H change sign M r emu - 11.181 E - 6 4.673 E - 6 7.927 E - 6 Remanent magnetization:M at H=0 S 0.016 0.008 0.012 Squareness:Mr/Ms S ∗ 1.005 1.013 1.009 1 - ( M r / H c ) (1 slope at Hc) M s emu 689.246 E - 6 - 615.022 E - 6 652.134 E - 6 Saturation magnetization: maximumM measured M at Hmax emu - 615.022 E - 6 6899.246 E - 6 652.134 E - 6 M at the maximum field Permeability, CGS-slope [ur] 984.957 E - 3 985.307 E - 3 985.132 E - 3 Permeability calculated from slope in CGS (unit less) requires correct volume in sample dimensions H s Oe - 9999.00 - 9996.00 9997.50 Saturation field, field at whichM reaches 0.95Ms H m a x Oe 10002.000 - 9999.000 10000.500 MaximumH measuredFigure 8 (a)
Magnetization versus the applied field plot at room temperature for the obtained power Ti-doped ZnO (ZTd) (b)
Zoomed-in image of Figure8(a)The experimental magnetic moment was calculated using the equation(6)η=Mw×Ms5585.Mw is the molecular weight of the sample while Ms is the saturation magnetization (emu/g) [28]. The value of the magnetic moment obtained was 0.1004 emu for 4.2% Ti-doped ZnO compared with saturation magnetic moment of about 0.15 μβ/Ti atom at room temperature for 5% Ti-doped ZnO [4]. Similar existence of ferromagnetism has been observed earlier in Fe-doped ZnO [29] and Mn-doped ZnO [30].The particle size of 26 nm obtained was less than the critical nanoparticle size (100 nm); consequently the nanoparticles form single domains with all the spins aligned in the same direction and uniformly magnetized. Furthermore, because there are no domain walls to move, the magnetization will be reversed through spin rotation rather than through the motion of domain walls which results in large coercivity of the nanoparticles. However observed coercivity (magnetic field required to bring the magnetization back to zero) of 1.500 (Oe) is relatively small suggesting that the nanoparticles are spherical. This observation is in conformity with the SEM results which suggested that the Ti-doped ZnO nanoparticles were spherical. At such low coercivity, the ferromagnetic nanoparticles with possible coexistence of paramagnetism behave like paramagnetic atoms with giant spins, and as the coercivity turns to zero, the nanoparticles become super magnetic [20, 31].


## 3.1. FTIR

Figure2 Shows the FTIR spectra of oxalate precursors synthesized by coprecipitation usingA. Carambolafruit juice as precipitating agent. The spectra of the precursors (ZZ and ZT) are very similar with weak IR bands occurring around 3363 cm−1 corresponding to the stretching vibrations of the -OH group associated with the presence of water of crystallization. The presence of the water of crystallization is confirmed by the H-O-H bending vibration observed at 737 cm−1. The Infrared bands observed below 1700 are assigned to the oxalate vibrational modes [21, 22] (the sharp intense peaks at 1620 cm−1 are attributed to the asymmetric stretching vibrations of the OCO group, while those around 1450–1300 cm−1 are attributed to the asymmetric (C=O) and symmetric (C-O) stretching vibrations in the OCO group). The sharp medium intense peaks at 826 cm−1 and 737 cm−1 confirm the bonding of metal oxygen (M-O) (indicating the presence of Zn2+ and Ti3+ bonded to the oxalate ion) and are assigned to (Vo-c=o + δZn-O) and (δTi-O + Vo-c=o). Moreover, the absence of the free IR VC=O, vibration expected at 1735–1705 cm−1, suggests that the entire carboxylate group of the oxalate is engaged in the formation of the coordination compound. On incorporating Ti+3 into the ZnO lattice sites, shifting of bands to lower wavenumbers is observed. This may be as a result of the bond weakening (increase in bond length) [23].Figure 2
FTIR of the precursors: zinc complex (ZZ) and titanium-doped zinc complex (ZT).


## 3.2. Thermal Analysis (TGA/DTG)

The thermal decomposition of zinc oxalate (ZZ) and Ti-doped zinc oxalate (ZT) precursors was carried out within the same temperature range of 30–650°C (as shown in Figure3). The decomposition of Tix-Zni-xC2O4 occurs in two steps (Figure 3(a)). The initial step is the dehydration process which takes place in two steps. The first step occurred in the temperature range 30–125°C (1) and the second step in the range 125–220°C (2). The dehydration steps for both the pure and the doped ZnC2O4 occurred within the same temperature range although the doped sample started dehydrating at a lower temperature, which revealed the relative instability of the doped crystal [23]. The measured weight loss for the first segment of the first step is about 4.5% of the total weight resulting in the elimination of half a molecule of water. The measured weight loss for the second segment of the first step is about 13.71%, which results in the elimination of one and a half molecules of water.Figure 3 (a)
Thermogram of Ti-doped zinc oxalate (ZT) (b)
Thermogram of zinc oxalate (ZZ)The total weight of water of crystallization in the pure sample (19.02%) decreases (to 18.51%) following the incorporation of Ti+3 in the zinc oxalate crystal. This shows that on introducing titanium ion, water of crystallization decreases. The reduction in the water of crystallization could be attributed to H-bonding between the particles (on introducing Ti as dopant, the lattice contracts leading to a decrease in particle size and reduction in the H-bonding between the particles). (1)Tix-Zn1-xC2O4·2H2O⟶Tix-Zn1-xC2O4·32H2O+12H2O(2)Tix-Zn1-xC2O4·32H2O⟶Tix-Zn1-xC2O4+32H2OThe second step, like the first, has also two segments. The first segment occurred in the temperature range 230–430°C and corresponds to the decomposition of the anhydrous doped oxalate, eliminating carbon monoxide (3). The last segment is the decarboxylation process, which occurred in the temperature range 430–650°C and constitutes the decomposition of the carbonate to the corresponding metal oxides (4). (3)TixZn1-xC2O4⟶TixZn1-xCO3+CO(4)TixZn1-xCO3⟶TixZn1-xO+CO2Looking at the DTG, there is no apparent difference in the thermal decomposition patterns of the pure and the Ti added sample (ZT). Just like the Ti free sample (ZZ), the thermogram of ZT shows two well defined weight loss steps. Cong et al. [2] and Ahmad et al. [24] made similar observations for Mn-Zn oxalate. The first (19.29%) around 125–220°C is attributed to the loss of two molecules of water of crystallization (cf. 19.23%), while the second (36.80%) found between 400 and 480°C is attributed to the release of one molecule of each of CO2 and CO (cf. 39.45%) giving a difference of 2.65%. The difference suggests that decomposition of ZT is not actually complete at 450°C. This observation could be attributed to the more stable TiCO3 which holds back some proportion of CO2. A closer view of the thermogram (TGA and DTG) for ZT reveals a little weight loss portion around 600°C which could accounts for the complete decomposition of ZT to ZTd. However calcinations of both ZZ and ZT at 450°C for 4 hours gives the final decomposition products (ZZd and ZTd).


## 3.3. XRD/EDS/SEM Characterization

### 3.3.1. X-Ray Diffraction

Figures4 and 5 show, respectively, the room temperature powder X-ray diffraction spectra for the oxalate precursors (ZZ and ZT) and the decomposition products (ZZd and ZTd). All the reflections in the pattern could be indexed to the zinc oxalate (JCPDS card number 25-1029), Table 2, and monophasic zinc oxide hexagonal wurtzite structure (JCPDS card number 36-1451), Table 3, respectively. The diffraction patterns for sample ZZ and ZT are virtually indifferent and matched perfectly with JCPDS card number 25-1029 for zinc oxalate dehydrate. This is in conformity with FTIR results which indicated the presence of water of hydration. The peaks in the spectra of both ZZd and ZTd matched perfectly with JCPDS card number 36-1451 for hexagonal wurtzite ZnO structure, shown in Table 3. (No impurity peaks were observed as no peak from the patterns of the decomposed sample ZTd matched JCPDS card number 84-1286 for TiO2 anatase phase and JCPDS card number 75-1753 rutile phase.) However, the diffraction peaks of Ti-doped ZnO are shifted to lower angles with respect to those of ZnO, which suggests some changes in the ZnO matrix resulting from the substitution of Ti for some Zn. The substitution is confirmed by the EDS spectrum shown in Figure 6, which shows that the composition of ZTd to be Ti, Zn, and O. Therefore, for the dopant proportion, Ti did not bring any change in the crystal structure of ZnO since there was complete incorporation of Ti into the ZnO structure by substituting for some of the Zn. This phenomenon was earlier observed by other groups for Ti-doped ZnO nanoparticle [25] and films [2], and they attributed the shift in 2θ values to a distortion of the ZnO crystallite when Ti substitutes for Zn since Ti4+ radius is lower than that of Zn2+. Therefore, the formula of ZTd and ZZd could be written as Zn0.958Ti0.042O and ZnO, respectively. The crystallite size was estimated from X-ray line broadening studies using (101) reflections with the help of the Debye-Scherer’s equation (5) and was found to be 29 nm and 26 nm for pure and doped ZnO, respectively.(5)D=kλβcos⁡θ,where D is the crystallite size, k is the correction factor that accounts for the shape of the particles, λ is the wavelength of the XRD beam (here λ = 0.15406 nm), β is the full width at half maximum (FWHM) of the peak, and θ is the Bragg’s diffraction angleTable 2
PXRD data for the precursors (ZZ and ZT) indexed with JCPDS card number 25-1029 for zinc oxalate dehydrate.
JCPDS no. 25-1029 ZZ/ZT h k l d  (Å) Intensity 2θ d  (Å) Intensity −202 4.77 100 18.27 4.85 100 002 3.6 35 22.83 3.89 31 −113 2.65 35 33.38 2.67 16 021 2.55 25 35.12 2.54 24 022 2.22 30 40.53 2.24 21 221 2.03 18 43.67 2.07 16 023 1.88 25 48.43 1.87 19Table 3
PXRD data for the decomposition products (ZZd and ZTd) indexed with JCPDS card number 36-1451 for wurtzite ZnO.
JCPDS no. 36-1451 ZnO wurtzite structure ZZd ZTd 2θ h k l 2θ Relative intensity 2θ Relative intensity 31.749 100 31.8 71.7 32.307 58.85 34.228 002 34.46 50.94 34.82 48.83 36.257 101 36.3 100 36.6 100 47.257 102 47.62 19.81 48.02 26.68 110 56.66 19.81 57.15 46.72 103 62.94 18.87 63.25 38.71Figure 4
XRD of the precursors: zinc oxalate (ZZ) and Ti-doped zinc oxalate (ZT).Figure 5
XRD of the decomposition products of the zinc complex (ZZd) and the titanium-doped zinc complex (ZTd).Figure 6
The EDS of the decomposition products, zinc oxide (ZZd), and the titanium-doped zinc oxide (ZTd).
(a) (b)The SEM images of ZZd (ZnO) and ZTd (Ti-doped ZnO) are shown in Figures7(a) and 7(b). A high degree of particle agglomeration is observed, which is in agreement with literature [2]. The SEM images for the calcined products at 450°C for 4 hours are shown in Figures 7(c) and 7(d). On the one hand, ZZd (ZnO) is present as regular polyhedral particles with the hexagonal shape of the wurtzite structure observed in PXRD, while, on the other hand, ZTd (Ti-doped ZnO) shows spherical particulates with some level of agglomeration and an average agglomerate size of about 2 μm in width and 4 μm in length. The fact that agglomerates showed sizes in the range of 2 μm indicates that the particulates are in the nanometer range which conforms to the XRD results.Figure 7 (a)
SEM image of ZZd (ZnO) (b)
SEM image of ZTd (Ti-doped ZnO) (c)
SEM image of calcined, ZZd (ZnO) (d)
SEM image of calcined, ZTd (Ti-doped ZnO)


## 3.3.1. X-Ray Diffraction

Figures4 and 5 show, respectively, the room temperature powder X-ray diffraction spectra for the oxalate precursors (ZZ and ZT) and the decomposition products (ZZd and ZTd). All the reflections in the pattern could be indexed to the zinc oxalate (JCPDS card number 25-1029), Table 2, and monophasic zinc oxide hexagonal wurtzite structure (JCPDS card number 36-1451), Table 3, respectively. The diffraction patterns for sample ZZ and ZT are virtually indifferent and matched perfectly with JCPDS card number 25-1029 for zinc oxalate dehydrate. This is in conformity with FTIR results which indicated the presence of water of hydration. The peaks in the spectra of both ZZd and ZTd matched perfectly with JCPDS card number 36-1451 for hexagonal wurtzite ZnO structure, shown in Table 3. (No impurity peaks were observed as no peak from the patterns of the decomposed sample ZTd matched JCPDS card number 84-1286 for TiO2 anatase phase and JCPDS card number 75-1753 rutile phase.) However, the diffraction peaks of Ti-doped ZnO are shifted to lower angles with respect to those of ZnO, which suggests some changes in the ZnO matrix resulting from the substitution of Ti for some Zn. The substitution is confirmed by the EDS spectrum shown in Figure 6, which shows that the composition of ZTd to be Ti, Zn, and O. Therefore, for the dopant proportion, Ti did not bring any change in the crystal structure of ZnO since there was complete incorporation of Ti into the ZnO structure by substituting for some of the Zn. This phenomenon was earlier observed by other groups for Ti-doped ZnO nanoparticle [25] and films [2], and they attributed the shift in 2θ values to a distortion of the ZnO crystallite when Ti substitutes for Zn since Ti4+ radius is lower than that of Zn2+. Therefore, the formula of ZTd and ZZd could be written as Zn0.958Ti0.042O and ZnO, respectively. The crystallite size was estimated from X-ray line broadening studies using (101) reflections with the help of the Debye-Scherer’s equation (5) and was found to be 29 nm and 26 nm for pure and doped ZnO, respectively.(5)D=kλβcos⁡θ,where D is the crystallite size, k is the correction factor that accounts for the shape of the particles, λ is the wavelength of the XRD beam (here λ = 0.15406 nm), β is the full width at half maximum (FWHM) of the peak, and θ is the Bragg’s diffraction angleTable 2
PXRD data for the precursors (ZZ and ZT) indexed with JCPDS card number 25-1029 for zinc oxalate dehydrate.
JCPDS no. 25-1029 ZZ/ZT h k l d  (Å) Intensity 2θ d  (Å) Intensity −202 4.77 100 18.27 4.85 100 002 3.6 35 22.83 3.89 31 −113 2.65 35 33.38 2.67 16 021 2.55 25 35.12 2.54 24 022 2.22 30 40.53 2.24 21 221 2.03 18 43.67 2.07 16 023 1.88 25 48.43 1.87 19Table 3
PXRD data for the decomposition products (ZZd and ZTd) indexed with JCPDS card number 36-1451 for wurtzite ZnO.
JCPDS no. 36-1451 ZnO wurtzite structure ZZd ZTd 2θ h k l 2θ Relative intensity 2θ Relative intensity 31.749 100 31.8 71.7 32.307 58.85 34.228 002 34.46 50.94 34.82 48.83 36.257 101 36.3 100 36.6 100 47.257 102 47.62 19.81 48.02 26.68 110 56.66 19.81 57.15 46.72 103 62.94 18.87 63.25 38.71Figure 4
XRD of the precursors: zinc oxalate (ZZ) and Ti-doped zinc oxalate (ZT).Figure 5
XRD of the decomposition products of the zinc complex (ZZd) and the titanium-doped zinc complex (ZTd).Figure 6
The EDS of the decomposition products, zinc oxide (ZZd), and the titanium-doped zinc oxide (ZTd).
(a) (b)The SEM images of ZZd (ZnO) and ZTd (Ti-doped ZnO) are shown in Figures7(a) and 7(b). A high degree of particle agglomeration is observed, which is in agreement with literature [2]. The SEM images for the calcined products at 450°C for 4 hours are shown in Figures 7(c) and 7(d). On the one hand, ZZd (ZnO) is present as regular polyhedral particles with the hexagonal shape of the wurtzite structure observed in PXRD, while, on the other hand, ZTd (Ti-doped ZnO) shows spherical particulates with some level of agglomeration and an average agglomerate size of about 2 μm in width and 4 μm in length. The fact that agglomerates showed sizes in the range of 2 μm indicates that the particulates are in the nanometer range which conforms to the XRD results.Figure 7 (a)
SEM image of ZZd (ZnO) (b)
SEM image of ZTd (Ti-doped ZnO) (c)
SEM image of calcined, ZZd (ZnO) (d)
SEM image of calcined, ZTd (Ti-doped ZnO)


## 3.4. Vibrating Sample Magnetometry (VSM)

The magnetic behavior of the nanoparticles was investigated by plotting the magnetic moment as a function of the applied magnetic field measured at a temperature of 5 k while the magnitudes of the magnetic properties obtained from the hysteresis loop are shown in Table4. The observed curve shows a hysteresis (Figure 8), which indicates the existence of ferromagnetic ordering in the sample. The solid solution shows saturated magnetization (Ms) of 6.89 emu/g, remnant magnetization (Mr) of 7.93 emu/g at room temperature, and a coercive force (Hc) of ZTd of 1.500 (Oe) which could be attributed to the tiny nature of the as-prepared ZTd particles [26, 27]. The squareness (remanence ratio) Mr/Ms for the sample was determined and the value obtained was 0.012.Table 4
The magnitudes of the magnetic properties obtained from the hysteresis loop.
Hysteresis loop Upward part Downward part Average Parameter “definition” H c Oe −9999.000 - 9996.000 - 1.500 Coercive field, field at whichM//H change sign M r emu - 11.181 E - 6 4.673 E - 6 7.927 E - 6 Remanent magnetization:M at H=0 S 0.016 0.008 0.012 Squareness:Mr/Ms S ∗ 1.005 1.013 1.009 1 - ( M r / H c ) (1 slope at Hc) M s emu 689.246 E - 6 - 615.022 E - 6 652.134 E - 6 Saturation magnetization: maximumM measured M at Hmax emu - 615.022 E - 6 6899.246 E - 6 652.134 E - 6 M at the maximum field Permeability, CGS-slope [ur] 984.957 E - 3 985.307 E - 3 985.132 E - 3 Permeability calculated from slope in CGS (unit less) requires correct volume in sample dimensions H s Oe - 9999.00 - 9996.00 9997.50 Saturation field, field at whichM reaches 0.95Ms H m a x Oe 10002.000 - 9999.000 10000.500 MaximumH measuredFigure 8 (a)
Magnetization versus the applied field plot at room temperature for the obtained power Ti-doped ZnO (ZTd) (b)
Zoomed-in image of Figure8(a)The experimental magnetic moment was calculated using the equation(6)η=Mw×Ms5585.Mw is the molecular weight of the sample while Ms is the saturation magnetization (emu/g) [28]. The value of the magnetic moment obtained was 0.1004 emu for 4.2% Ti-doped ZnO compared with saturation magnetic moment of about 0.15 μβ/Ti atom at room temperature for 5% Ti-doped ZnO [4]. Similar existence of ferromagnetism has been observed earlier in Fe-doped ZnO [29] and Mn-doped ZnO [30].The particle size of 26 nm obtained was less than the critical nanoparticle size (100 nm); consequently the nanoparticles form single domains with all the spins aligned in the same direction and uniformly magnetized. Furthermore, because there are no domain walls to move, the magnetization will be reversed through spin rotation rather than through the motion of domain walls which results in large coercivity of the nanoparticles. However observed coercivity (magnetic field required to bring the magnetization back to zero) of 1.500 (Oe) is relatively small suggesting that the nanoparticles are spherical. This observation is in conformity with the SEM results which suggested that the Ti-doped ZnO nanoparticles were spherical. At such low coercivity, the ferromagnetic nanoparticles with possible coexistence of paramagnetism behave like paramagnetic atoms with giant spins, and as the coercivity turns to zero, the nanoparticles become super magnetic [20, 31].


## 4. Conclusion

Pure nanocrystalline ZnO (29 nm) and Ti-doped ZnO (26 nm) dilute magnetic semiconductors have been successfully synthesized by a modified oxalate process for the first time, usingAverrhoa carambola fruit juice as the source of the precipitating agent. The precursors were identified as the expected metal oxalates, and the decomposition products were found to be pure ferromagnetic nanoparticles.Our results demonstrate that not only the proposed modified coprecipitation technique, by using a precipitating agent extract fromA. Carambola juice, is simple, environmentally friendly, low-cost, controllable, but it can also be applied to prepare spherical Ti-doped ZnO magnetic nanoparticles and possibly a wide variety of mixed metal oxides useful in many applications.



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*Source: 9072325-2018-03-22.xml*