# Comparison of Urea and Citric Acid Complexing Agents and Annealing Temperature Effect on the Structural Properties ofγ- and α-Alumina Nanoparticles Synthesized by Sol-Gel Method

Authors: A. Rajaeiyan; M. M. Bagheri-Mohagheghi
Journal: Advances in Materials Science and Engineering
 (2013)

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## Abstract

A sol-gel method based on the Pechini process was used to synthesize different phases of alumina nanoparticles using a polymeric precursor with Aluminum nitrate.  The  emphasis  was  on investigating  the effect of two different complexing agents, urea and citric acid, on the structural properties, particle size, and phase transformation during the heat treatment that was studied by XRD, TEM, SEM, BET, and FT-IR spectroscopy. The obtained results showed that particles do get fused together at high temperatures, and also the size of particles increases with the increase of annealing temperature. It was concluded that the size ofα-alumina synthesized by urea was 10–15 nm, whereas the sample with citric acid yielded α-powder with particle size of 200 nm. Also, the resulting powder prepared by urea exhibited larger surface area (84.2 m2/gm−1) compared to citric acid (39.92 m2/gm−1) at 750∘C.


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## Body

## 1. Introduction

Among various ceramics, alumina (Al2O3) or sapphire, especially nanosized alumina, is one of the most important ceramic materials with exceptional properties such as high melting point, high temperature stability, high chemical inactivity, great hardness, and large band gap energy. Due to its excellent properties, it has many applications both as structural and functional materials such as heterogeneous catalyst or catalyst support, abrasive and adsorbent, cutting tool, and microelectronic and medical devices like surgical implants [1–4].Alumina exists in a number of metastable transition phases as well as the thermodynamically stableα-Al2O3 or corundum. These metastable alumina structures can be divided into two broad categories: a face-centered cubic arrangement of oxygen anions including γ-, η-, θ-, and δ-alumina, and a hexagonal close-packed arrangement of oxygen anions consisting of α-, κ-, and Χ-alumina [5–7]. In the past decades, nanotechnology has become a key area in the development of science and engineering. Nanostructural materials have structural domains with diameters between 1 and 100 nm. They are used potentially for many applications since the reduction of grain size to the nanometer scale can improve their physical and mechanical properties. Recently, much attention has been paid to the synthesis of nanocrystalline ceramics such as alumina ceramics. Among the physical and chemical methods devised for preparation of nanoscaled materials, synthesis from atomic or molecular precursors such as sol-gel route can give better control of particle size and homogeneity in particle distribution. It is a relatively simple processing technology that has been considered in the last three decades. Sol-gel enables materials to be mixed on a molecular level and bring out a solution, either as a colloidal gel, or as a polymerized macromolecular network [8, 9]. Metal alkoxides are typical precursors, which undergo various forms of hydrolysis and polycondensation reactions. However, these metal alkoxide precursors have some disadvantages such as costs, flammability, moisture sensitivity, and toxicity. To overcome these problems, an alternative method for the production of fine powder is Pechini’s method. Pechini processing involves the dissolution of metal salts in a mixture of a weak hydroxyl carboxylic acid as citric acid and a poly hydroxyl alcohol such as ethylene glycol. When the solution is heated at a certain temperature usually lower than 100°C, a viscous organic precursor develops which can then be converted to the oxide by post-heating. Many preparation parameters like pH, nature of salt and solute concentration, type of solvent, temperature, and drying conditions have to be judiciously controlled to obtain desired nanoparticles [9, 10].A few number of papers discuss the effect of sol-gel process parameter on physical properties ofα-alumina nanoparticle. Kim et al. [11] studied aluminum nitrate precursor as compared to aluminum sulfate precursor. They conclude that the size of alumina nanoparticles obtained using aluminum nitrate precursor was smaller than that obtained using aluminum sulfate precursor, and the particles obtained from aluminum nitrate precursor have elongated shape, while those obtained from aluminum sulfate precursor have spherical shape. It was also observed that the temperature for complete transformation to α-Al2O3 is lower in the case of using aluminum nitrate precursor as compared to aluminum sulfate precursor. Li et al. [12] investigated the molar ratio of citric acid to metal nitrate (C/N) in the sol-gel process which played an important role in phase transition and morphology controlling of alumina. Their results showed that the increasing molar ratio of C/N was found to be in favor of γ- to α-Al2O3 phase transition, whereas the precursor with C/N = 1 yielded a relatively well dispersed ultrafine γ-Al2O3 powder. Sharma et al. [13] demonstrated the critical role of pH in the sol-gel synthesis of alumina nanopowder. According to their results, by increasing the pH value from 2.5 to 12, the particle size increases from 75 to 750 nm. Also, the morphology of nanoparticle can be altered by changing pH of alumina sol. In another research [14], alumina nanopowder was synthesized by two different drying methods: (1) calcined at different temperatures and (2) by supercritical drying. They successfully obtained the hexagon sheet nano-γ-alumina particles with average size around 5–10 nm and more homogeneous dispersibility with the assistance of supercritical drying. While they had hard agglomerate nanoparticles in the first drying method that the phase transformation strongly depends on calcined temperature.In the Pechini method, chelating occursbetween complex cations and acid like citric acid, which is one of the leading basic chemical reactions as shown in Figure1.Figure 1
Chelating between complex cations and acid like citric acid.It seems that what makes difference in the performance of these material is the difference in the strength of bond formation with central atom of complex. So, various complexing agents behave differently, which should be considered. In this paper, we compared two different complexing agents (urea and citric acid) in the synthesis of alumina nanoparticle via sol-gel processing and Pechini’s method. They are the most commonly used agents that is the reason why we have chosen them. These agents contain carboxylate or amine groups which are essential for the water-soluble complex precursor synthesis route. Citric acid contains carboxylate group, while urea contains aliphatic amine group. So they would behave differently in the methods of synthesis according to their ability in bond formation in complexes [15–18].


## 2. Experimental

### 2.1. Synthesis

The starting solution was prepared by dissolving 0.1 M aluminum nitrate nonahydrate (Al(NO3)3·9H2O) in 100 mL deionized water and 100 mL ethanol to form a clear solution. The required amount of ethylene glycol and citric acid was added to the solution and heated at 40°C under vigorous magnetic stirring. The molar ratio of complexing agent and ethylene glycol to metal ions was 3 : 1 in the solution. Ethylene glycol functions as a spacer to modulate the distance between metal ions, preventing metal oxide particles from aggregation during earlier stages of organics removal. The aim of the polymeric organic net by esterification is to reduce any segregation of the cations. Then, the solution was continuously stirred for 4 hours and kept at a temperature of 80°C under reflux system until it turned to a yellowish sol. Then, the sol was heated in the oil bath at 100°C for 21 hours. With evaporation of the solvents, a transparent stick gel was gained. The beaker containing the aerogel was placed on a hot plate at 120°C. It was concurrently heated from the top by infrared lamp radiation. During heating, the solution in the beaker was evaporated, and the gel started to swell and bubble. After 3 hours, a dried brownish xerogel was formed. The sol-gel precursors obtained were dried at 200°C in an oven and then grinded into a powder. Subsequently, the powder was put into the porcelain crucible and calcined in a muffle furnace at different temperatures (750, 1000, and 1250°C) for 1 hour. In the next step, with maintaining all experiment conditions, we used urea as complexing agent instead of citric acid. To get an accurate comparison, the molar ratio of materials used in the second experiment was same as the first experiment; that is, we used 0.1 mol Aluminum nitrate nonahydrate (Al(NO3)3·9H2O) dissolved in 100 mL deionized water and 100 mL ethanol. Like the previous experiment, the molar ratio of urea as complexing agent and ethylene glycol to metal ions was three to one in the solution. In this condition, at the heating step of the aerogel, the sample suddenly foamed up and caught fire, leaving a finely black-colored powder.


### 2.2. Characterization

To identify phases and their crystallinity, powder X-ray diffraction (XRD) studies were carried out by D8 Advance Bruker diffractometer using CuKα (λ = 0.15406 nm), radiation in the 2θ range from 20° to 70°. The average crystallite size (D) was calculated using Scherrer’s formula [19],
(1)D=Kλβcosθ,
where β is the full width at half maximum (FWHM) of the corresponding XRD peak at radiant. K = 0.9 is correction factor, λ is X-ray wavelength (λ = 0.15406 nm), and θ is the Bragg diffraction angle. Scanning electron microscopy (Leo 430I) and transmission electron microscopy (LEO (912 AB)) were used to observe and analyze the morphology and the particle size of the powders. The different absorption bands corresponding to the gel and additives were determined by Fourier transform infrared spectra analysis (FT-IR) using KBr disk technique with a Perkin Elmer-RXI with k = 4000−400 cm−1. The specific surface areas were calculated by the Brunauer-Emmett-Teller (BET) equation using the data in the P/P0 range of 0.09–0.3 and outgas temperature of 200°C. The specific surface area (SSA) was converted into particle size assuming that the particles are closed spheres with smooth surface and uniform size using
(2)DBET=6×103dthSBET,
where dth is the theoretical density of the material under consideration, DBET is the average particle size in nm, and SBET is the specific surface area expressed in m2 gm−1 [16].


## 2.1. Synthesis

The starting solution was prepared by dissolving 0.1 M aluminum nitrate nonahydrate (Al(NO3)3·9H2O) in 100 mL deionized water and 100 mL ethanol to form a clear solution. The required amount of ethylene glycol and citric acid was added to the solution and heated at 40°C under vigorous magnetic stirring. The molar ratio of complexing agent and ethylene glycol to metal ions was 3 : 1 in the solution. Ethylene glycol functions as a spacer to modulate the distance between metal ions, preventing metal oxide particles from aggregation during earlier stages of organics removal. The aim of the polymeric organic net by esterification is to reduce any segregation of the cations. Then, the solution was continuously stirred for 4 hours and kept at a temperature of 80°C under reflux system until it turned to a yellowish sol. Then, the sol was heated in the oil bath at 100°C for 21 hours. With evaporation of the solvents, a transparent stick gel was gained. The beaker containing the aerogel was placed on a hot plate at 120°C. It was concurrently heated from the top by infrared lamp radiation. During heating, the solution in the beaker was evaporated, and the gel started to swell and bubble. After 3 hours, a dried brownish xerogel was formed. The sol-gel precursors obtained were dried at 200°C in an oven and then grinded into a powder. Subsequently, the powder was put into the porcelain crucible and calcined in a muffle furnace at different temperatures (750, 1000, and 1250°C) for 1 hour. In the next step, with maintaining all experiment conditions, we used urea as complexing agent instead of citric acid. To get an accurate comparison, the molar ratio of materials used in the second experiment was same as the first experiment; that is, we used 0.1 mol Aluminum nitrate nonahydrate (Al(NO3)3·9H2O) dissolved in 100 mL deionized water and 100 mL ethanol. Like the previous experiment, the molar ratio of urea as complexing agent and ethylene glycol to metal ions was three to one in the solution. In this condition, at the heating step of the aerogel, the sample suddenly foamed up and caught fire, leaving a finely black-colored powder.


## 2.2. Characterization

To identify phases and their crystallinity, powder X-ray diffraction (XRD) studies were carried out by D8 Advance Bruker diffractometer using CuKα (λ = 0.15406 nm), radiation in the 2θ range from 20° to 70°. The average crystallite size (D) was calculated using Scherrer’s formula [19],
(1)D=Kλβcosθ,
where β is the full width at half maximum (FWHM) of the corresponding XRD peak at radiant. K = 0.9 is correction factor, λ is X-ray wavelength (λ = 0.15406 nm), and θ is the Bragg diffraction angle. Scanning electron microscopy (Leo 430I) and transmission electron microscopy (LEO (912 AB)) were used to observe and analyze the morphology and the particle size of the powders. The different absorption bands corresponding to the gel and additives were determined by Fourier transform infrared spectra analysis (FT-IR) using KBr disk technique with a Perkin Elmer-RXI with k = 4000−400 cm−1. The specific surface areas were calculated by the Brunauer-Emmett-Teller (BET) equation using the data in the P/P0 range of 0.09–0.3 and outgas temperature of 200°C. The specific surface area (SSA) was converted into particle size assuming that the particles are closed spheres with smooth surface and uniform size using
(2)DBET=6×103dthSBET,
where dth is the theoretical density of the material under consideration, DBET is the average particle size in nm, and SBET is the specific surface area expressed in m2 gm−1 [16].


## 3. Results and Discussion

### 3.1. Structural Properties

Figures2(a)–2(c) show comparative XRD patterns of the as-synthesized powder obtained with citric acid and urea calcined at different temperatures. It was found that the phase transformation strongly depends on calcined temperature. As shown by the XRD pattern at 750°C, there are broad peaks which are indications of crystallite structure formation and nanosized dimension [20]. At this temperature for the sample obtained from urea, Figure 2(a)(B) indicates the formation of poorly crystallized alumina, as broad peaks indexed for γ-Al2O3. Indeed, at this temperature, aqueous amorphous Al2O3 phase exists which is also seen in [21], which is introduced as a precursor of gamma alumina. But for the sample obtained from citric acid, diffraction peaks attributed to γ-alumina appeared. The broadness of peaks implies a low crystallization [14]. The black color of powder at this temperature shows the existence of organic materials, also confirmed XRD pattern so that these compounds have prevented the formation of crystal structure.XRD patterns of Al2O3 nanopowder prepared with complexing agent. (A) Citric acid and (B) urea calcined at temperatures of (a) 750°C, (b) 1000°C, and (c) 1250°C.
(a)
750°C
(b)
1000°C
(c)
1250°CWith the increase of calcination temperature up to 1000°C, crystallinity ofγ-Al2O3 improved. The γ-Al2O3 crystallized in a defective spinel lattice with aluminum located in tetragonal position. Such a lattice is unstable and should transform into stable form at high temperatures. At 1000°C, weak peaks of δ-Al2O3 were observed, which is an essential intermediate phase for the transformation of gamma to alpha at higher temperatures [22]. At this temperature in the case of using urea, characteristic peaks of α-Al2O3 appear with a rather weak intensity, which indicate the starting point of γ- to α-Al2O3 transition.It can be seen that the phase transformation temperature to alpha phase is lower in the case of urea precursor compared to citric acid precursor. It was reported that NH4NO3 is formed during the preparation of alumina from aluminum nitrate and urea according to the following chemical reactions [23]:
(3)2Al(NO3)3+3NH2–CO–NH2+(x+6)H2O⟶Al2O3·xH2O+6NH4NO3+3CO2(4)2Al(NO3)3+4NH2–CO–NH2+(x+7)H2O⟶Al2O3·xH2O+6NH4NO3+2NH3+4CO2(5)2Al(NO3)3+7NH2–CO–NH2+(x+14)H2O⟶Al2O3·xH2O+6NH4NO3+4(NH4)4CO3+3CO2
After that, NH4NO3 decomposes and releases a large amount of energy during calcination, leading to the decrease of temperature for the complete transformation of γ- to α-alumina [24]. Single-phase α-Al2O3 was completely formed after calcinations at 1250°C for both samples. The diffraction pattern was extremely sharp indicating the existence of a highly crystalline material. Since all the organic materials were burnt off during calcination at elevated temperatures, the powder was completely white. Table 1 shows weight loss of powders after calcination temperatures.Table 1
Weight loss of powders versus annealing temperatures.
Complexing agent
Weight lossT = 750°C
Weight lossT = 1000°C
Urea
86%
89%
Citric acid
90%
92%


### 3.2. Particle Size and Specific Surface Area

The XRD parameters and the calculated crystallite sizes using Scherrer’s formula are presented in Table2. Irrespective of the preparation conditions, all the samples exhibited a crystallite size of around 6.5–8.5 nm at 1000°C and 28–38 nm at 1250°C. Table 3 shows the BET surface area of powders and the particle size calculated from (2) using alumina density of 3.98 g/cm3. A large particle size calculated from surface area compared to the crystallite size measured by XRD illustrates the rate of agglomeration of the particles. The surface area was higher for the urea complexing agent (84.2) compared to citric acid (39.92) which is in agreement with the size of nanoparticle, as the particle size becomes small, the specific surface area is increased. From Table 3, it is indicated that upon annealing, due to the increased grain growth during the phase transformation from γ-Al2O3 to α-Al2O3, a substantial reduction in surface area had occurred.Table 2
Summary of XRD measurements for Al2O3 samples.
Complexing agent
h
k
l
2θ (deg)
Intensity(cps)
d (Å) Lattice distance
FWHM(deg)
D (nm) Crystalite size
Identification with(hkl) value
Citric acid
T = 1000°C
440
67.08
712
1.39
1.14
8.60
γ-Al2O3; Cubic
400
45.86
528
1.97
1.19
7.50
γ-Al2O3; Cubic
311
37.56
426
2.39
1.17
7.40
γ-Al2O3; Cubic
T = 1250°C
113
43.44
3346
2.08
0.29
30.50
α-Al2O3; Hexagonal
104
35.23
3031
2.54
0.28
31.00
α-Al2O3; Hexagonal
116
57.59
2774
1.59
0.32
28.87
α-Al2O3; Hexagonal
012
25.62
1885
3.46
0.27
30.53
α-Al2O3; Hexagonal
Urea
T = 1000°C
440
67.11
705
1.39
1.153
8.60
γ-Al2O3; Cubic
400
45.96
499
1.97
0.999
8.90
γ-Al2O3; Cubic
311
37.52
446
2.39
1.3
6.70
γ-Al2O3; Cubic
104
35.23
289
2.54
0.227
38.24
α-Al2O3; Hexagonal
113
43.519
180
2.07
0.303
29.40
α-Al2O3; Hexagonal
106
57.57
155
1.59
0.255
37.02
α-Al2O3; Hexagonal
T = 1250°C
113
43.48
3608
2.07
0.29
30.72
α-Al2O3; Hexagonal
104
35.28
3334
2.54
0.27
31.23
α-Al2O3; Hexagonal
116
57.63
2980
1.59
0.32
29.14
α-Al2O3; Hexagonal
012
25.0
2386
3.46
0.26
32.00
α-Al2O3; HexagonalTable 3
BET surface area of powders and the particle size versus annealing temperatures.
Complexing agent
S
BET (m2/g) T = 750°C
D
BET (nm) T = 750°C
S
BET (m2/g) T = 1250°C
D
BET (nm) T = 1250°C
Urea
84.2
18
17.4
87
Citric acid
39.92
38
—
—


### 3.3. SEM and TEM Observations

The effect of complexing agents on the structure of nanoparticles can be clearly seen from the SEM and TEM images. Figures3 and 4 present SEM image of nanoparticles calcined at 750°C and 1250°C prepared by urea and citric acid, respectively. Figure 5 shows a comparison in TEM images between the particle as produced from urea and citric acid at 1250°C. Electronic Microscopic images reveal that hard agglomeration occurred at high temperatures, and the size distribution of nanoparticle is mostly uniform. Due to the agglomeration, the determination of the average diameter was hard because individual particle boundaries were not clearly distinguishable. But with more accuracy the size of particles before hard agglomeration is possible to estimate. From TEM images, the size of particles produced with citric acid is about 200 nm, and those prepared from urea are about 10–15 nm. Probably due to using the urea and spontaneous combustion process, the particles did not have any chance for growth and had smaller size. In order to study the effect of calcinations temperature on the size of particles, TEM image of nanoalumina obtained from urea calcined at 750°C is also shown in Figure 6. At this temperature, due to presence of organic compounds in powder, there is an opaque background so that the particles are not properly observed and are consistent with black color of powder and XRD diagrams at 750°C. With a smaller-scale image, extremely fine particles with a size of about 6–8 nm can be seen which become larger with increasing temperature as shown in Figure 6(b).SEM images of Al2O3 nanoparticles prepared by urea calcined at (a) 750°C and (b) 1250°C.
(a)
750°C
(b)
1250°CSEM image of Al2O3 nanoparticles prepared by citric acid calcined at (a) 750°C and (b) 1250°C.
(a)
750°C
(b)
1250°CTEM images of Al2O3 nanoparticles prepared with complexing agent. (a) Citric acid and (b) urea calcined at 1250°C for 1 hour.
(a)
Citric acid
(b)
UreaTEM images of Al2O3 nanoparticles prepared with urea at 750°C at different scales of the microscope image.
(a)
Urea (750°C)
(b)
Urea (750°C)
(c)
Urea (750°C)
(d)
Urea (750°C)From SEM images, it can be observed that the particles have elongated shape. It seems that the open structure of the gelatinous precipitate formed from precursor allowed alumina crystallites agglomeration freely, resulting in the evolution of the typical morphology, namely, elongated structure [24, 25].


### 3.4. FT-IR Spectra

Plots (a) and (b) in Figure7 illustrate the infrared spectrum of the powders annealed at 750, 1000, and 1250°C for each complexing agent that shows similar features. At 750°C, a broad band around 3500 cm−1 and an absorption one at 1635 cm−1 are observed, which are assigned to bending and stretching vibration of hydroxylate group (O–H) in the adsorbed water, respectively [26]. It can be seen that the infrared spectra tend to possess a double-peak at ~800 cm−1 and ~600 cm−1 that are assigned to aluminium ions in octahedral and tetrahedral environment and indicating the presence of γ-phase at this temperature [27, 28]. The low intensity of these peaks indicates that it is at the beginning of gamma phase formation. With increasing temperature up to 1000°C, these broad bands divided into two clear distinct peaks represent that the γ-phase formation is complete at this temperature [27, 28]. This is in agreement with the presence of γ-alumina diffraction peaks observed in the XRD pattern at 750°C and 1000°C. At 1250°C, sharp absorption peaks at 450, 600, and 650 cm−1 and the other with less intensity at 780 cm−1 appear which are identified to be the characteristics absorption bands of α-Al2O3 with a corundum structure that is built up only on octahedral AlO6 [12]. The high intensity of these peaks is proportional to the XRD pattern at 1250°C. Absorption at ~2350 cm−1 that increases with temperature is stretching the vibration ofHCO3-group, related to the atmospheric H2O and CO2 adsorbed on the metallic cations [29]. In the pattern Figure 6(a) at 750°C, the peak centered at ~1390 cm−1 indicates thatNO3-disappears by increasing temperature [27], and the one at 2341 cm−1 is related to CO2 absorption from the surrounding environment by metal cations that did not remove even with increasing temperature [28].FT-IR spectrums of Al2O3 nanopowders prepared with complexing agent. (a) Citric Acid and (b) urea calcined at various temperatures.
(a)
Citric acid
(b)
Urea


## 3.1. Structural Properties

Figures2(a)–2(c) show comparative XRD patterns of the as-synthesized powder obtained with citric acid and urea calcined at different temperatures. It was found that the phase transformation strongly depends on calcined temperature. As shown by the XRD pattern at 750°C, there are broad peaks which are indications of crystallite structure formation and nanosized dimension [20]. At this temperature for the sample obtained from urea, Figure 2(a)(B) indicates the formation of poorly crystallized alumina, as broad peaks indexed for γ-Al2O3. Indeed, at this temperature, aqueous amorphous Al2O3 phase exists which is also seen in [21], which is introduced as a precursor of gamma alumina. But for the sample obtained from citric acid, diffraction peaks attributed to γ-alumina appeared. The broadness of peaks implies a low crystallization [14]. The black color of powder at this temperature shows the existence of organic materials, also confirmed XRD pattern so that these compounds have prevented the formation of crystal structure.XRD patterns of Al2O3 nanopowder prepared with complexing agent. (A) Citric acid and (B) urea calcined at temperatures of (a) 750°C, (b) 1000°C, and (c) 1250°C.
(a)
750°C
(b)
1000°C
(c)
1250°CWith the increase of calcination temperature up to 1000°C, crystallinity ofγ-Al2O3 improved. The γ-Al2O3 crystallized in a defective spinel lattice with aluminum located in tetragonal position. Such a lattice is unstable and should transform into stable form at high temperatures. At 1000°C, weak peaks of δ-Al2O3 were observed, which is an essential intermediate phase for the transformation of gamma to alpha at higher temperatures [22]. At this temperature in the case of using urea, characteristic peaks of α-Al2O3 appear with a rather weak intensity, which indicate the starting point of γ- to α-Al2O3 transition.It can be seen that the phase transformation temperature to alpha phase is lower in the case of urea precursor compared to citric acid precursor. It was reported that NH4NO3 is formed during the preparation of alumina from aluminum nitrate and urea according to the following chemical reactions [23]:
(3)2Al(NO3)3+3NH2–CO–NH2+(x+6)H2O⟶Al2O3·xH2O+6NH4NO3+3CO2(4)2Al(NO3)3+4NH2–CO–NH2+(x+7)H2O⟶Al2O3·xH2O+6NH4NO3+2NH3+4CO2(5)2Al(NO3)3+7NH2–CO–NH2+(x+14)H2O⟶Al2O3·xH2O+6NH4NO3+4(NH4)4CO3+3CO2
After that, NH4NO3 decomposes and releases a large amount of energy during calcination, leading to the decrease of temperature for the complete transformation of γ- to α-alumina [24]. Single-phase α-Al2O3 was completely formed after calcinations at 1250°C for both samples. The diffraction pattern was extremely sharp indicating the existence of a highly crystalline material. Since all the organic materials were burnt off during calcination at elevated temperatures, the powder was completely white. Table 1 shows weight loss of powders after calcination temperatures.Table 1
Weight loss of powders versus annealing temperatures.
Complexing agent
Weight lossT = 750°C
Weight lossT = 1000°C
Urea
86%
89%
Citric acid
90%
92%


## 3.2. Particle Size and Specific Surface Area

The XRD parameters and the calculated crystallite sizes using Scherrer’s formula are presented in Table2. Irrespective of the preparation conditions, all the samples exhibited a crystallite size of around 6.5–8.5 nm at 1000°C and 28–38 nm at 1250°C. Table 3 shows the BET surface area of powders and the particle size calculated from (2) using alumina density of 3.98 g/cm3. A large particle size calculated from surface area compared to the crystallite size measured by XRD illustrates the rate of agglomeration of the particles. The surface area was higher for the urea complexing agent (84.2) compared to citric acid (39.92) which is in agreement with the size of nanoparticle, as the particle size becomes small, the specific surface area is increased. From Table 3, it is indicated that upon annealing, due to the increased grain growth during the phase transformation from γ-Al2O3 to α-Al2O3, a substantial reduction in surface area had occurred.Table 2
Summary of XRD measurements for Al2O3 samples.
Complexing agent
h
k
l
2θ (deg)
Intensity(cps)
d (Å) Lattice distance
FWHM(deg)
D (nm) Crystalite size
Identification with(hkl) value
Citric acid
T = 1000°C
440
67.08
712
1.39
1.14
8.60
γ-Al2O3; Cubic
400
45.86
528
1.97
1.19
7.50
γ-Al2O3; Cubic
311
37.56
426
2.39
1.17
7.40
γ-Al2O3; Cubic
T = 1250°C
113
43.44
3346
2.08
0.29
30.50
α-Al2O3; Hexagonal
104
35.23
3031
2.54
0.28
31.00
α-Al2O3; Hexagonal
116
57.59
2774
1.59
0.32
28.87
α-Al2O3; Hexagonal
012
25.62
1885
3.46
0.27
30.53
α-Al2O3; Hexagonal
Urea
T = 1000°C
440
67.11
705
1.39
1.153
8.60
γ-Al2O3; Cubic
400
45.96
499
1.97
0.999
8.90
γ-Al2O3; Cubic
311
37.52
446
2.39
1.3
6.70
γ-Al2O3; Cubic
104
35.23
289
2.54
0.227
38.24
α-Al2O3; Hexagonal
113
43.519
180
2.07
0.303
29.40
α-Al2O3; Hexagonal
106
57.57
155
1.59
0.255
37.02
α-Al2O3; Hexagonal
T = 1250°C
113
43.48
3608
2.07
0.29
30.72
α-Al2O3; Hexagonal
104
35.28
3334
2.54
0.27
31.23
α-Al2O3; Hexagonal
116
57.63
2980
1.59
0.32
29.14
α-Al2O3; Hexagonal
012
25.0
2386
3.46
0.26
32.00
α-Al2O3; HexagonalTable 3
BET surface area of powders and the particle size versus annealing temperatures.
Complexing agent
S
BET (m2/g) T = 750°C
D
BET (nm) T = 750°C
S
BET (m2/g) T = 1250°C
D
BET (nm) T = 1250°C
Urea
84.2
18
17.4
87
Citric acid
39.92
38
—
—


## 3.3. SEM and TEM Observations

The effect of complexing agents on the structure of nanoparticles can be clearly seen from the SEM and TEM images. Figures3 and 4 present SEM image of nanoparticles calcined at 750°C and 1250°C prepared by urea and citric acid, respectively. Figure 5 shows a comparison in TEM images between the particle as produced from urea and citric acid at 1250°C. Electronic Microscopic images reveal that hard agglomeration occurred at high temperatures, and the size distribution of nanoparticle is mostly uniform. Due to the agglomeration, the determination of the average diameter was hard because individual particle boundaries were not clearly distinguishable. But with more accuracy the size of particles before hard agglomeration is possible to estimate. From TEM images, the size of particles produced with citric acid is about 200 nm, and those prepared from urea are about 10–15 nm. Probably due to using the urea and spontaneous combustion process, the particles did not have any chance for growth and had smaller size. In order to study the effect of calcinations temperature on the size of particles, TEM image of nanoalumina obtained from urea calcined at 750°C is also shown in Figure 6. At this temperature, due to presence of organic compounds in powder, there is an opaque background so that the particles are not properly observed and are consistent with black color of powder and XRD diagrams at 750°C. With a smaller-scale image, extremely fine particles with a size of about 6–8 nm can be seen which become larger with increasing temperature as shown in Figure 6(b).SEM images of Al2O3 nanoparticles prepared by urea calcined at (a) 750°C and (b) 1250°C.
(a)
750°C
(b)
1250°CSEM image of Al2O3 nanoparticles prepared by citric acid calcined at (a) 750°C and (b) 1250°C.
(a)
750°C
(b)
1250°CTEM images of Al2O3 nanoparticles prepared with complexing agent. (a) Citric acid and (b) urea calcined at 1250°C for 1 hour.
(a)
Citric acid
(b)
UreaTEM images of Al2O3 nanoparticles prepared with urea at 750°C at different scales of the microscope image.
(a)
Urea (750°C)
(b)
Urea (750°C)
(c)
Urea (750°C)
(d)
Urea (750°C)From SEM images, it can be observed that the particles have elongated shape. It seems that the open structure of the gelatinous precipitate formed from precursor allowed alumina crystallites agglomeration freely, resulting in the evolution of the typical morphology, namely, elongated structure [24, 25].


## 3.4. FT-IR Spectra

Plots (a) and (b) in Figure7 illustrate the infrared spectrum of the powders annealed at 750, 1000, and 1250°C for each complexing agent that shows similar features. At 750°C, a broad band around 3500 cm−1 and an absorption one at 1635 cm−1 are observed, which are assigned to bending and stretching vibration of hydroxylate group (O–H) in the adsorbed water, respectively [26]. It can be seen that the infrared spectra tend to possess a double-peak at ~800 cm−1 and ~600 cm−1 that are assigned to aluminium ions in octahedral and tetrahedral environment and indicating the presence of γ-phase at this temperature [27, 28]. The low intensity of these peaks indicates that it is at the beginning of gamma phase formation. With increasing temperature up to 1000°C, these broad bands divided into two clear distinct peaks represent that the γ-phase formation is complete at this temperature [27, 28]. This is in agreement with the presence of γ-alumina diffraction peaks observed in the XRD pattern at 750°C and 1000°C. At 1250°C, sharp absorption peaks at 450, 600, and 650 cm−1 and the other with less intensity at 780 cm−1 appear which are identified to be the characteristics absorption bands of α-Al2O3 with a corundum structure that is built up only on octahedral AlO6 [12]. The high intensity of these peaks is proportional to the XRD pattern at 1250°C. Absorption at ~2350 cm−1 that increases with temperature is stretching the vibration ofHCO3-group, related to the atmospheric H2O and CO2 adsorbed on the metallic cations [29]. In the pattern Figure 6(a) at 750°C, the peak centered at ~1390 cm−1 indicates thatNO3-disappears by increasing temperature [27], and the one at 2341 cm−1 is related to CO2 absorption from the surrounding environment by metal cations that did not remove even with increasing temperature [28].FT-IR spectrums of Al2O3 nanopowders prepared with complexing agent. (a) Citric Acid and (b) urea calcined at various temperatures.
(a)
Citric acid
(b)
Urea


## 4. Conclusion

Different phases of alumina nanoparticles with elongated and uniform structure were synthesized by sol-gel method using aluminum nitrate and two different complexing agents: urea and citric acid. The following was found.(a)
According to XRD patterns, using the citric acid lowers the formation temperature ofγ-Al2O3. So concerning citric acid, this phase is formed at T = 750°C while regarding urea, it formed at T = 1000°C, this is confirmed by IR spectra.(b)
Urea has reduced the phase transition temperature to Alpha-Al2O3 so that at 1000°C low intensity δ- and α-peaks are observed in the case of using urea, and it may be due to the formation of NH4NO3, which is decomposed with releasing large amounts of energy during annealing. But for citric acid just peaks of γ is observed. So we introduce urea as a fuel of reaction at high temperatures.(c)
With increasing temperature up to 1250°C, high intensity and sharp peaks ofα-alumina are observed for both samples that shows very high crystallization at this temperature and is consistent with FT-IR spectra at 1250°C.(d)
According to electron microscope images, the size of alumina nanoparticles obtained using urea (10–15 nm) was so smaller and more uniform than those obtained using citric acid (200 nm), and their BET surface areas are 84.2 and 39.92 m2/g, respectively.(e)
Due to lower molecular weight of urea compared to citric acid, the remaining powder prepared by urea was more than the powder prepared by citric acid, so we suggest urea instead of citric acid in commercial and industrial applications.



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*Source: 791641-2013-10-23.xml*