# Structural and Optical Properties of Calcium Titanate Prepared from Gypsum

Authors: Massaud Mostafa; Z. A. Alrowaili; M.M. Al Shehri; M. Mobarak; Ahmed M. Abbas
Journal: Journal of Nanotechnology
 (2022)

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## Abstract

Ceramic materials have been used in various human health-related applications for considerable time. One of the important applications of ceramic materials is in electronics. Our work focuses on calcium titanate (CaTiO3). CaTiO3 is typically created via sintering. Gypsum particles is used to form calcium hydroxide, which is then combined with titanium dioxide to form rutile crystals. Thereafter, calcination is performed at 900°C, 1000°C, and 1100°C for 2 h. X-ray diffraction is employed to track the evolution of the CaTiO3 phase. Scanning electron microscopy is used to characterize the morphologies of the different preparation steps. As the calcination temperature increases from 900°C to 1000°C, the crystallite size of CaTiO3 increases from 35 nm to 45 nm. Furthermore, the energy gaps of the CaTiO3 powders obtained after calcination at 900°C and 1000°C are 5.32 eV and 5.43 eV, respectively, and their particle sizes are 150–200 nm and 200–300 nm, respectively.


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## Body

## 1. Introduction

The general formula of perovskites is ABO3 (A is a rare or alkaline earth metal and B is a first-row transition metal). Calcium titanate (CaTiO3), which is considered as the “founding father” of the perovskite family of titanium-based perovskite-type oxide photocatalysts [1–7], is attracting increasing attention. CaTiO3 is a chemically stable n-type semiconductor with a broad bandgap of 3–3.5 eV [8]. Ca ions are located at the corners (1/2, 1/2, 1/2), Ti at the body center (0, 0, 0), and oxygen at the face center (1/2, 0, 0; 0, 12, 0; 0, 0, 1/2) [9]. CaTiO3 is an alkaline earth metal titanate composed of earth-abundant nontoxic elements. It is fabricated using various methods [10], e.g., solid-state, coprecipitation, mechanochemical, sol-gel, hydrothermal, and solvothermal processes. Among these, the sol-gel process is the most widely used method. CaTiO3 exhibits excellent qualities as a multifunctional material, including optical properties, high dielectric constant, ferroelectricity, chemical stability, small dielectric loss, low cost, and environmental friendliness [11]. Several properties of CaTiO3 have been explored owing to its broad applications. CaTiO3 shows electrical properties when it is applied to electronic devices such as capacitors and thermistors. Hence, it has been extensively explored as an electroceramic material. In addition, it is known as a microwave ceramic owing to its dielectric response in the microwave spectrum. The photocatalytic activity and dynamic efficiency of CaTiO3 have been investigated in decomposing organic dye waste in aquatic environments and water splitting for H2 production, CO2 reduction, and other applications. CaTiO3 has been developed as an implant material for biomedical applications in composites with hydroxyapatite [12]. Furthermore, it is a good substitute for the commercial titanium dioxide (TiO2) catalyst in photocatalytic applications. The property of volume growth caused by water absorption is observed in rocks containing clay minerals and anhydrite. Rock swelling is a term used to describe this phenomenon. The origin of swelling in anhydrite is chemical, and it depends on the transformation of anhydrite into gypsum [13]. The solid-solid reaction of CaO or Ca(OH)2 with TiO2 at a specific molar content is the basic principle of the synthesis of CaTiO3 perovskite material [14]. Calcium can be obtained from a low-cost source such as gypsum. Aside from the benefits of using gypsum as a low-cost calcium source, this research attempted to manufacture CaTiO3 perovskite material from gypsum and test it on a laboratory scale as a simple and low-cost ceramic material.The goal of this study was to synthesize CaTiO3 using a sol-gel technique with calcium hydroxide (Ca(OH)2) and TiO2 as starting materials and ethanol as the dispersion medium. Gypsum rock samples were collected from a specified site in Gebel Elba National Park in southeastern Egypt, as shown in Figure 1, and Ca(OH)2 was obtained from treated gypsum rocks. The gels disintegrated into CaTiO3 precipitates. Crystalline CaTiO3 powders were obtained by calcining the precipitate at 900°C, 1000°C, and 1100°C for 2 h. Transmission electron microscopy (TEM), X-ray diffraction (XRD), and scanning electron microscopy (SEM) were performed to study the microstructural and morphological behavior of dried CaTiO3 sol-gel powders.Figure 1
Site map of the collected gypsum samples (Gabal Elbah) [15].


## 2. Materials and Methods

First, the raw material was collected from gypsum stones washed using distilled water and then ground with a heavy grinder. Next, the small stone pieces were milled using a ball-milling machine to obtain gypsum powder with the chemical formula of CaSO4.2H2O. Commercially available rutile titanium dioxide (TiO2) was used to synthesize CaTiO3 powders via combustion. Calcium sulfate (CaSO4) powder was obtained by calcining the gypsum powder at 500°C to evaporate H2O particles. Then, the powder was mixed with potassium hydroxide (KOH) for 1 h using a magnetic stirrer at a temperature of 80°C. The mixture was filtered to obtain Ca(OH)2. Figure 2 shows the preparation steps.Figure 2
Preparation of CaTiO3 powders via the sol-gel technique.The sol-gel method was used to produce CaTiO3 powder from Ca(OH)2 powder and TiO2. These were added to distilled water and stirred for 2 h at 80°C to obtain all reactants in the form of a gel. The gel was dried at 70°C for 20 h to obtain a powder, which was sintered at 900°C, 1000°C, and 1100°C for 2 h. The final powder was pressed into pellets and sintered at 1000°C. The powder samples were characterized using XRD, SEM, and TEM, as shown in Figure 3.Figure 3
Block diagram of the sol-gel preparation method.


### 2.1. Measurements

All prepared particles were characterized by XRD. Particles were observed with a Zeiss LEO 912 OMEG operated at 100 kV accelerating voltage. Crystal structures of the particles were measured with an X-ray diffractometer (Rigaku RU-200A) operated at 40 kV and 30 mA with CuKα radiation using a monochromator. Optical properties of the nanoparticles were studied by a UV-visible spectrophotometer (UV2300II). The Fourier transmission infrared (FTIR) spectra of the samples were recorded by using FTIR (Shimadzu, model DF 803) in the wave range 400–4000 cm. Scanning electron microscopy (JEOL, JSM 5500LV) and transmission electron microscopy (JEOL, JEM 1010) were employed to reveal the microstructure of the synthesized powders, whereas the elemental analysis was studied using energy dispersive spectroscopy (Oxford Instruments, ISIS Link).


## 2.1. Measurements

All prepared particles were characterized by XRD. Particles were observed with a Zeiss LEO 912 OMEG operated at 100 kV accelerating voltage. Crystal structures of the particles were measured with an X-ray diffractometer (Rigaku RU-200A) operated at 40 kV and 30 mA with CuKα radiation using a monochromator. Optical properties of the nanoparticles were studied by a UV-visible spectrophotometer (UV2300II). The Fourier transmission infrared (FTIR) spectra of the samples were recorded by using FTIR (Shimadzu, model DF 803) in the wave range 400–4000 cm. Scanning electron microscopy (JEOL, JSM 5500LV) and transmission electron microscopy (JEOL, JEM 1010) were employed to reveal the microstructure of the synthesized powders, whereas the elemental analysis was studied using energy dispersive spectroscopy (Oxford Instruments, ISIS Link).


## 3. Results and Discussion

### 3.1. XRD Characterization

Figure4 shows the XRD patterns obtained at different steps during the preparation of CaTiO3. Broad XRD peaks suggest the presence of nanocrystalline particles. The XRD patterns were used to calculate the crystallite sizes and strain were using Scherrer’s formula and the Williamson–Hall equation. The results are given in Table 1.Figure 4
XRD patterns obtained at different CaTiO3 preparation steps.Table 1
Crystal size values derived using the average Scherrer, Scherrer straight line, and Williamson–Hall methods.
MaterialScherrer (nm)Williamson–Hall (nm)StrainCaSO4.2H2O4045.42.2 × 10−3CaSO468.7608.5 × 10−5Ca(OH)239.940.21.5 × 10−3CaTiO3 (900°C)35.430.21.006 × 10−6CaTiO3 (1000°C)45.2467.3 × 10−4Figure4(a) shows the XRD patterns of gypsum (CaSO4⋅2H2O). XPert HighScore was used to analyze the XRD results to obtain the Miller indices and crystallographic parameters of mineral gypsum, as given in Table 1.Figure4(b) shows the XRD patterns for CaSO4. The Match software was used to identify CaSO4 peaks. Figure 4(c) shows the main compounds present in the three analyzed Ca(OH)2 samples. The peaks are assigned to KOH (α) in addition to Ca(OH)2. This may be because KOH and CaSO4 did not fully react. This indicates that the reactants may need to be stirred for longer than 2 h. However, this step of the preparation was not returned because of the expectation that KOH will evaporate during calcination.(1)CaSO4+2KOH⟶CaOH2+K2SO4.In this reaction, calcium sulfate joins with potassium hydroxide, a base. The OH− from the base joins to form calcium hydroxide, while the SO4− and K+ ions join to form potassium sulfate. A chemical filter paper is used to separate calcium hydroxide and remove potassium sulfate, as shown in Figure 2.The XRD patterns were analyzed to assess the crystal structure. Figure4(d) shows the XRD patterns of the CaTiO3 powder produced after calcination at 900°C for 2 h. The diffraction patterns of CaTiO3 are consistent with the JCPDS card (no. 22-0153). A few minor peaks (denoted by β) are caused by TiO2 impurities, which are associated with an incomplete reaction. In addition, we assume an orthorhombic phase because of the Pbnm space group. The crystallographic variables obtained from the XRD analysis are given in Table 2.Table 2
Crystallographic parameters of different materials.
MaterialCrystal systemSpace groupSpace group numbera=bA˙cA˙c/aα=Y(°)β(°)GypsumMonoclinic12/a155.66.511.1690118.4CaSO4OrthorhombicBmmb636.9926.240.899090Ca(OH)2OrthorhombicBmmb1364.582.950.699090CaTiO3 (900°C)OrthorhombicPbnm1364.582.950.469090CaTiO3 (1000°C)CubicIm-3m2294.474.4719090The XRD patterns were analyzed to assess the crystal structure. Figure4(e) shows the XRD results of the CaTiO3 powder produced via calcination at 1000°C for 2 h. The diffraction patterns are consistent with the JCPDS card (no. 22-0153). Additionally, a few small peaks (denoted by β) are due to the presence of TiO2 impurities, indicating an incomplete reaction. The Pbnm space group indicates the orthorhombic phase. The crystallographic parameters obtained from the XRD analysis are given in Table 2.Figure4(f) shows the XRD patterns of the powder produced via calcination at 1100°C for 2 h. These patterns show that CaTiO3 is not formed. This may be because the bonds between Ca(OH)2 and TiO2 are destroyed at a high temperature. The XRD patterns show calcium (Ca) ions and TiO. We can assume that the phase of the Ca ions is cubic with the Im-3m space group. The crystallographic parameters obtained from the XRD analysis are given in Table 2.The expected reaction may be as follows:(2)CaOH2+TiO2⟶Ca+TiO+2H2O↑.Understanding the tolerance factor aids in the development of novel perovskite compounds. Goldschmid’s tolerance factort was used to classify the synthesis of perovskite-type compounds:(3)t=rA+rO2rB+rO,where rA, rB, and rO are the effective ionic radii of A and B sites and the oxygen ion sites, respectively, where rCa2+=1.48Å, rTi4+=0.745Å, and rO2−=1.21Å indicate radii values. A site and B site cations’ bonding requirements in the ABO3 perovskite is measured quantitatively by the tolerance factor which reflects the distortion structure that contains the octahedral rotation and tilt. As the substituent radii Ca2+ion is at A site and radii Ti4+ion at B site, the tolerance factor calculated values of the CaTiO3 is 0.972. Hence, the general the structures tend to be in the perovskite structure as the calculated tolerance factor t ∼ 1 [16].The cubic structure of CaTiO3 is shown in Figure 5(b), with Ca ions occupying the A site, Ti ions occupying the B site, and O representing the oxygen anion [17–19]. However, with CaTiO3 calcined at 900 C, the perovskite structure deviates from cubic symmetry and transitions to orthorhombic phase, as given in Table 2, in order to fit the Ca2+ cations, which are smaller in size than the ideal ions for site ”A.” The tolerance factor is used to calculate the degree of distortion in the ideal cubic structure (t).Figure 5
(a) Ideal cubic perovskite structure for ABO3 (cyan, BO6 units; yellow, A atoms) (Reprinted with permission from reference [18]-[11] copyright from Elsevier). (b) Illustration of the crystal structure of CaTiO3.
(a)(b)


### 3.2. SEM Characterization

Figure5(a) shows the SEM micrographs of gypsum powder; the particles are either rectangular or rod shaped. Figure 5(b) shows the SEM micrographs of Ca(OH)2; the particles are either rectangular or rod shaped.Figures6(c) and 6(d) show the microstructures of CaTiO3 obtained after calcination at 900°C and 1000°C, respectively. We can deduce that this substance appears foamy. The microstructures of the particles are almost nonexistent. All of the CaTiO3 powders had an ultra-agglomeration powder, and because of the chemically active particles, they agglomerate quickly. This is why it was so difficult to achieve greater magnifications, as we had previously done with gypsum and calcium hydroxide samples, where increased magnification resulted in visual blurring at higher magnifications.Figure 6
SEM micrograph of (a) gypsum, (b) Ca(OH)2, (c) CaTiO3 obtained after calcination at 900°C, and (d) CaTiO3 obtained after calcination at 1000°C.
(a)(b)(c)(d)


### 3.3. TEM Characterization

Figures7(a) and 7(b) show the TEM micrographs of CaTiO3 powders obtained after calcination at 900°C and 1000°C, respectively, and a spherical morphology is observed. Figures 6(c) and 6(d) show the length distribution histograms of these powders. In the CaTiO3 powder obtained after calcination at 900°C, the size of most particles is 150–200 nm, and there are a few agglomerated particles. The average particle size of the CaTiO3 powder obtained after calcination at 1000°C is 200–300 nm.Figure 7
TEM micrographs of CaTiO3 obtained after calcination at (a) 900°C and (b) 1000°C. Length distribution histograms of CaTiO3 obtained after calcination at (c) 900°C and (d) 1000°C.
(a)(b)(c)(d)


### 3.4. Optical Properties

The UV-vis absorbance spectra (at room temperature) of CaTiO3 powders are shown in Figure 8. The wavelength of the spectra is 200–800 nm. The absorption decreases rapidly for a wavelength of 200–250 nm but remains almost constant for 250–800 nm.Figure 8
UV-vis absorbance spectra of CaTiO3 obtained after calcination at 900°C and 1000°C.Wood and Tauc [20] demonstrated the relationship between the absorption curve and energy gap of a material. The bandgap values were obtained by extrapolating the linear region of the curve. According to this method, the energy dependence of the gap and optical absorbance can be expressed as follows:(4)hvα=hv−Egopt2,where α is the absorbance, h is Planck’s constant, m is the frequency, and Egopt is the bandgap of a material.Figure9 shows the calculated bandgaps for CaTiO3 powders obtained after calcination at 900°C and 1000°C, which are 5.32 and 5.43 eV, respectively.Figure 9
Energy gaps for CaTiO3 obtained after calcination at 900°C and 1000°C.Egap values were measured in previous research, and the results were calculated by extrapolating the linear section of the curve using linear regression to arrive at Egap values of about 3.51 eV [21]. An increase in the bandgap may be identified for the current CaTiO3 when compared to previous works, which can be due to the existence of TiO2 secondary phase, which can cause defects such as distortions along CaO linkages, which result in localized electronic levels in the band gap.


### 3.5. Fourier-Transform Infrared Spectroscopy Analysis

Fourier-transform infrared spectroscopy (FTIR) analyses were performed for CaTiO3 powders obtained after calcination at 900°C and 1000°C. The results are shown in Figure 10. The band at 570 cm−1 is assigned as the signature peak of the CaTiO3 bond. The absorption peak at 460 cm−1 is due to the bending mode of the Ti-O-Ti bond. The absorption peak at 567 cm−1 is characterized as Ti-O stretching vibration. This implies the existence of TiO6 octahedra and the formation of a CaTiO3 perovskite-type structure [22]. For the CaTiO3 powder obtained at 1000°C, the broad bands observed above 3644 cm−1 and 3429 cm−1 are related to the superposition of the vibration band of the hydroxyl group and the stretching vibration of the adsorbed OH group.Figure 10
FTIR spectra of CaTiO3 obtained after calcination at 900°C and 1000°C.


## 3.1. XRD Characterization

Figure4 shows the XRD patterns obtained at different steps during the preparation of CaTiO3. Broad XRD peaks suggest the presence of nanocrystalline particles. The XRD patterns were used to calculate the crystallite sizes and strain were using Scherrer’s formula and the Williamson–Hall equation. The results are given in Table 1.Figure 4
XRD patterns obtained at different CaTiO3 preparation steps.Table 1
Crystal size values derived using the average Scherrer, Scherrer straight line, and Williamson–Hall methods.
MaterialScherrer (nm)Williamson–Hall (nm)StrainCaSO4.2H2O4045.42.2 × 10−3CaSO468.7608.5 × 10−5Ca(OH)239.940.21.5 × 10−3CaTiO3 (900°C)35.430.21.006 × 10−6CaTiO3 (1000°C)45.2467.3 × 10−4Figure4(a) shows the XRD patterns of gypsum (CaSO4⋅2H2O). XPert HighScore was used to analyze the XRD results to obtain the Miller indices and crystallographic parameters of mineral gypsum, as given in Table 1.Figure4(b) shows the XRD patterns for CaSO4. The Match software was used to identify CaSO4 peaks. Figure 4(c) shows the main compounds present in the three analyzed Ca(OH)2 samples. The peaks are assigned to KOH (α) in addition to Ca(OH)2. This may be because KOH and CaSO4 did not fully react. This indicates that the reactants may need to be stirred for longer than 2 h. However, this step of the preparation was not returned because of the expectation that KOH will evaporate during calcination.(1)CaSO4+2KOH⟶CaOH2+K2SO4.In this reaction, calcium sulfate joins with potassium hydroxide, a base. The OH− from the base joins to form calcium hydroxide, while the SO4− and K+ ions join to form potassium sulfate. A chemical filter paper is used to separate calcium hydroxide and remove potassium sulfate, as shown in Figure 2.The XRD patterns were analyzed to assess the crystal structure. Figure4(d) shows the XRD patterns of the CaTiO3 powder produced after calcination at 900°C for 2 h. The diffraction patterns of CaTiO3 are consistent with the JCPDS card (no. 22-0153). A few minor peaks (denoted by β) are caused by TiO2 impurities, which are associated with an incomplete reaction. In addition, we assume an orthorhombic phase because of the Pbnm space group. The crystallographic variables obtained from the XRD analysis are given in Table 2.Table 2
Crystallographic parameters of different materials.
MaterialCrystal systemSpace groupSpace group numbera=bA˙cA˙c/aα=Y(°)β(°)GypsumMonoclinic12/a155.66.511.1690118.4CaSO4OrthorhombicBmmb636.9926.240.899090Ca(OH)2OrthorhombicBmmb1364.582.950.699090CaTiO3 (900°C)OrthorhombicPbnm1364.582.950.469090CaTiO3 (1000°C)CubicIm-3m2294.474.4719090The XRD patterns were analyzed to assess the crystal structure. Figure4(e) shows the XRD results of the CaTiO3 powder produced via calcination at 1000°C for 2 h. The diffraction patterns are consistent with the JCPDS card (no. 22-0153). Additionally, a few small peaks (denoted by β) are due to the presence of TiO2 impurities, indicating an incomplete reaction. The Pbnm space group indicates the orthorhombic phase. The crystallographic parameters obtained from the XRD analysis are given in Table 2.Figure4(f) shows the XRD patterns of the powder produced via calcination at 1100°C for 2 h. These patterns show that CaTiO3 is not formed. This may be because the bonds between Ca(OH)2 and TiO2 are destroyed at a high temperature. The XRD patterns show calcium (Ca) ions and TiO. We can assume that the phase of the Ca ions is cubic with the Im-3m space group. The crystallographic parameters obtained from the XRD analysis are given in Table 2.The expected reaction may be as follows:(2)CaOH2+TiO2⟶Ca+TiO+2H2O↑.Understanding the tolerance factor aids in the development of novel perovskite compounds. Goldschmid’s tolerance factort was used to classify the synthesis of perovskite-type compounds:(3)t=rA+rO2rB+rO,where rA, rB, and rO are the effective ionic radii of A and B sites and the oxygen ion sites, respectively, where rCa2+=1.48Å, rTi4+=0.745Å, and rO2−=1.21Å indicate radii values. A site and B site cations’ bonding requirements in the ABO3 perovskite is measured quantitatively by the tolerance factor which reflects the distortion structure that contains the octahedral rotation and tilt. As the substituent radii Ca2+ion is at A site and radii Ti4+ion at B site, the tolerance factor calculated values of the CaTiO3 is 0.972. Hence, the general the structures tend to be in the perovskite structure as the calculated tolerance factor t ∼ 1 [16].The cubic structure of CaTiO3 is shown in Figure 5(b), with Ca ions occupying the A site, Ti ions occupying the B site, and O representing the oxygen anion [17–19]. However, with CaTiO3 calcined at 900 C, the perovskite structure deviates from cubic symmetry and transitions to orthorhombic phase, as given in Table 2, in order to fit the Ca2+ cations, which are smaller in size than the ideal ions for site ”A.” The tolerance factor is used to calculate the degree of distortion in the ideal cubic structure (t).Figure 5
(a) Ideal cubic perovskite structure for ABO3 (cyan, BO6 units; yellow, A atoms) (Reprinted with permission from reference [18]-[11] copyright from Elsevier). (b) Illustration of the crystal structure of CaTiO3.
(a)(b)


## 3.2. SEM Characterization

Figure5(a) shows the SEM micrographs of gypsum powder; the particles are either rectangular or rod shaped. Figure 5(b) shows the SEM micrographs of Ca(OH)2; the particles are either rectangular or rod shaped.Figures6(c) and 6(d) show the microstructures of CaTiO3 obtained after calcination at 900°C and 1000°C, respectively. We can deduce that this substance appears foamy. The microstructures of the particles are almost nonexistent. All of the CaTiO3 powders had an ultra-agglomeration powder, and because of the chemically active particles, they agglomerate quickly. This is why it was so difficult to achieve greater magnifications, as we had previously done with gypsum and calcium hydroxide samples, where increased magnification resulted in visual blurring at higher magnifications.Figure 6
SEM micrograph of (a) gypsum, (b) Ca(OH)2, (c) CaTiO3 obtained after calcination at 900°C, and (d) CaTiO3 obtained after calcination at 1000°C.
(a)(b)(c)(d)


## 3.3. TEM Characterization

Figures7(a) and 7(b) show the TEM micrographs of CaTiO3 powders obtained after calcination at 900°C and 1000°C, respectively, and a spherical morphology is observed. Figures 6(c) and 6(d) show the length distribution histograms of these powders. In the CaTiO3 powder obtained after calcination at 900°C, the size of most particles is 150–200 nm, and there are a few agglomerated particles. The average particle size of the CaTiO3 powder obtained after calcination at 1000°C is 200–300 nm.Figure 7
TEM micrographs of CaTiO3 obtained after calcination at (a) 900°C and (b) 1000°C. Length distribution histograms of CaTiO3 obtained after calcination at (c) 900°C and (d) 1000°C.
(a)(b)(c)(d)


## 3.4. Optical Properties

The UV-vis absorbance spectra (at room temperature) of CaTiO3 powders are shown in Figure 8. The wavelength of the spectra is 200–800 nm. The absorption decreases rapidly for a wavelength of 200–250 nm but remains almost constant for 250–800 nm.Figure 8
UV-vis absorbance spectra of CaTiO3 obtained after calcination at 900°C and 1000°C.Wood and Tauc [20] demonstrated the relationship between the absorption curve and energy gap of a material. The bandgap values were obtained by extrapolating the linear region of the curve. According to this method, the energy dependence of the gap and optical absorbance can be expressed as follows:(4)hvα=hv−Egopt2,where α is the absorbance, h is Planck’s constant, m is the frequency, and Egopt is the bandgap of a material.Figure9 shows the calculated bandgaps for CaTiO3 powders obtained after calcination at 900°C and 1000°C, which are 5.32 and 5.43 eV, respectively.Figure 9
Energy gaps for CaTiO3 obtained after calcination at 900°C and 1000°C.Egap values were measured in previous research, and the results were calculated by extrapolating the linear section of the curve using linear regression to arrive at Egap values of about 3.51 eV [21]. An increase in the bandgap may be identified for the current CaTiO3 when compared to previous works, which can be due to the existence of TiO2 secondary phase, which can cause defects such as distortions along CaO linkages, which result in localized electronic levels in the band gap.


## 3.5. Fourier-Transform Infrared Spectroscopy Analysis

Fourier-transform infrared spectroscopy (FTIR) analyses were performed for CaTiO3 powders obtained after calcination at 900°C and 1000°C. The results are shown in Figure 10. The band at 570 cm−1 is assigned as the signature peak of the CaTiO3 bond. The absorption peak at 460 cm−1 is due to the bending mode of the Ti-O-Ti bond. The absorption peak at 567 cm−1 is characterized as Ti-O stretching vibration. This implies the existence of TiO6 octahedra and the formation of a CaTiO3 perovskite-type structure [22]. For the CaTiO3 powder obtained at 1000°C, the broad bands observed above 3644 cm−1 and 3429 cm−1 are related to the superposition of the vibration band of the hydroxyl group and the stretching vibration of the adsorbed OH group.Figure 10
FTIR spectra of CaTiO3 obtained after calcination at 900°C and 1000°C.


## 4. Conclusions

CaTiO3 was successfully prepared from gypsum using a sol-gel method and characterized via TEM, XRD, and SEM. XRD analysis confirmed the presence of the pure crystalline CaTiO3 phase after calcination at 900°C and 1000°C for 2 h, along with unreacted TiO2 particles. According to TEM observations, the CaTiO3 powder obtained after calcination at 900°C had a particle size of 150–200 nm and exhibited agglomeration of nanoparticles. The CaTiO3 powder obtained after calcination at 1000°C had a particle size of 200–300 nm. SEM observations showed that CaTiO3 particles did not have a specific microstructure. The energy gaps for CaTiO3 powders obtained after calcination at 900°C and 1000°C were 5.32 eV and 5.43 eV, respectively. Infrared bands were analyzed to identify the functional groups of CaTiO3. The bands at approximately 570 cm−1 were due to the signature peak of the CaTiO3 bond. The band at 567 cm−1 was due to Ti-O stretching vibration. Furthermore, the bands close to 460 cm−1 were attributed to the Ti-O-Ti bending mode.



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