# Optical and Morphological Properties of ZnO- and TiO2-Derived Nanostructures Synthesized via a Microwave-Assisted Hydrothermal Method

Authors: Nosipho Moloto; Siyasanga Mpelane; Lucky M. Sikhwivhilu; Suprakas Sinha Ray
Journal: International Journal of Photoenergy
 (2012)

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## Abstract

A microwave-assisted hydrothermal method was used to synthesize ZnO and TiO2 nanostructures. The experimental results show that the method resulted in crystalline monodispersed ZnO nanorods that have pointed tips with hexagonal crystal phase. TiO2 nanotubes were also formed with minimum bundles. The mechanism for the formation of the tubes was validated by HRTEM results. The optical properties of both ZnO and TiO2 nanostructures showed characteristics of strong quantum confinement regime. The photoluminescence spectrum of TiO2 nanotubes shows good improvement from previously reported data.


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## Body

## 1. Introduction

The fabrication of size- and shape-controlled nanoparticles and their assembly into materials still poses a challenge in the area of nanosciences. It is well recognized that the shape of the nanoparticles plays a crucial role in determining their resultant properties [1–5]. One of the difficulties associated with the synthesis of anisotropic nanoparticles is the control of growth through variation of the reaction parameters [6–10]. Factors such as concentration, temperature, pH, capping agent and the reaction time are critical parameters that influence the size and the morphology of the nanoparticles. Apart from these factors, altering a synthetic strategy can also introduce surprising results. Herein we report on the syntheses of ZnO and TiO2 nanoparticles using a microwave-assisted method. Their optical and morphological properties are also investigated.ZnO has attracted much attention because of its outstanding physical properties. It is an II-VI semiconductor that has a direct wide band gap of 3.37 eV and a large excitonic-binding energy (60 meV). Because of these properties, ZnO has found use in various technological applications including transparent conducting electrodes for solar cells, photocatalysis, surface acoustic devices, UV lasers, and as chemical and biological sensors [11–15]. Various methods such as the sol-gel method, hydrothermal process, chemical vapour deposition, and the single-source precursor method have been employed to synthesize different ZnO nanostructures [16–19]. Though similar to ZnO, TiO2 has been found to be particularly very effective in photocatalytic water splitting and has been employed in this capacity as an active layer in photovoltaics as well as an electrode in photoelectrolysis cells where it has been known to enhance the efficiency of electrolytic splitting of water into hydrogen and oxygen [20]. TiO2 is a semiconductor with a structurally dependent band gap (anatase −3.20 eV and rutile –3.03 eV) [21]. TiO2 has been prepared via several techniques such as the sol-gel, hydrothermal process, and pulse laser deposition [22–24].Although the sol-gel method is widely accepted for the preparation of both ZnO and TiO2 nanostructures, the calcinations process is essential and can cause further particle growth, induce phase transformation, and result in lower specific surface area. The method also results in the incorporation of impurities and poor crystallinity [25]. In this context, the use of the microwave assisted method is expected to be an alternative to the sol-gel technique. The most notable effect of microwave irradiation is the heating effect. In microwave heating, unlike in conventional heating, heat is generated within the material itself instead of heat supplied from external sources. As a result of this internal and volumetric heating, thermal gradients and flow of heat during microwave processing are quite different from those observed in conventional heating. This heating mechanism also results in the reduction of the reaction time. The optical and morphological properties of ZnO and TiO2 synthesized using the microwave-assisted method are hereby reported.


## 2. Experimental

### 2.1. Reagents

Titania (TiO2, P25 Degussa), zinc oxide, potassium hydroxide, hydrogen peroxide, and methanol were all purchased from Merck, South Africa. The potassium hydroxide (KOH) and hydrogen peroxide (H2O2) were diluted accordingly to obtain the desired concentration.


### 2.2. Synthesis of ZnO-Derived Nanostructures

About 0.045 mol of ZnO powder was added to 20 mL of 30% hydrogen peroxide. The solution was then placed in Teflon container and heated in a microwave oven with a maximum power of 1200 W, at a pressure of 30 bars for 15 min. The resultant particles were then washed several times with deionised water and dried in a conventional oven at 100°C for 5 h.


### 2.3. Synthesis of the TiO2-Derived Nanostructures

In a typical synthesis, 22 g of TiO2 powder was added to a 200 mL of 18 M potassium hydroxide. The solution was then placed in Teflon container and heated in a microwave oven with a maximum power of 1200 W, at a pressure of 22 bars for 15 min. The resultant particles were then washed several times with deionised water until the conductivity of the solution was below 100 μS/cm and finally dried in a conventional oven at 100°C for 5 h.


### 2.4. Structural Characterization

#### 2.4.1. X-Ray Diffraction

XRD patterns on powdered samples were measured on a Phillips X’Pert materials research diffractometer using secondary graphite monochromated Cu Kα radiation (λ=1.54060 Å) at 40 kV/50 mA. Measurements were taken using a glancing angle of incidence detector at an angle of 2°, for 2θ values over 10°–80° in steps of 0.05° with a scan speed of 0.01° 2θ·s−1.


#### 2.4.2. Electron Microscopy

The samples were characterized using field emission scanning electron microscopy (FE-SEM) (Leo, Zeiss), operated at 3–10 kV electron potential difference and equipped with a semiconductor detector that allows for detection of energy dispersive X-rays (EDX). The samples were prepared by placing a thin layer of powder on a carbon tape. The high resolution transmission electron microscopy (HRTEM) was carried out on a Joel JEM-2100 microscopy with a LAB6 filament. The measurements were carried out at 200 kV with a beam spot size of 20–200 nm in TEM mode. The samples were prepared by placing a drop of particles suspended in methanol on a holey carbon-coated copper grid.


### 2.5. Optical Characterization

#### 2.5.1. Absorption Spectroscopy

A Perkin Elmer Lambda 75S UV-VIS-NIR Spectrophotometer with double grating and double monochromator for high absorbance measurements was used to carry out the optical measurements. The powders were suspended in methanol and placed in quartz cuvettes (1 cm, path length). The band edges of the samples were determined from absorption spectrum by extrapolation.


#### 2.5.2. Emission Spectroscopy

A Perkin Elmer LS55 with a xenon lamp (150 W) and a 152 P photo multiplier tube as a detector was used to measure the photoluminescence of the particles. The samples were suspended in methanol and placed in quartz cuvettes (1 cm path length) for spectral analysis.


## 2.1. Reagents

Titania (TiO2, P25 Degussa), zinc oxide, potassium hydroxide, hydrogen peroxide, and methanol were all purchased from Merck, South Africa. The potassium hydroxide (KOH) and hydrogen peroxide (H2O2) were diluted accordingly to obtain the desired concentration.


## 2.2. Synthesis of ZnO-Derived Nanostructures

About 0.045 mol of ZnO powder was added to 20 mL of 30% hydrogen peroxide. The solution was then placed in Teflon container and heated in a microwave oven with a maximum power of 1200 W, at a pressure of 30 bars for 15 min. The resultant particles were then washed several times with deionised water and dried in a conventional oven at 100°C for 5 h.


## 2.3. Synthesis of the TiO2-Derived Nanostructures

In a typical synthesis, 22 g of TiO2 powder was added to a 200 mL of 18 M potassium hydroxide. The solution was then placed in Teflon container and heated in a microwave oven with a maximum power of 1200 W, at a pressure of 22 bars for 15 min. The resultant particles were then washed several times with deionised water until the conductivity of the solution was below 100 μS/cm and finally dried in a conventional oven at 100°C for 5 h.


## 2.4. Structural Characterization

### 2.4.1. X-Ray Diffraction

XRD patterns on powdered samples were measured on a Phillips X’Pert materials research diffractometer using secondary graphite monochromated Cu Kα radiation (λ=1.54060 Å) at 40 kV/50 mA. Measurements were taken using a glancing angle of incidence detector at an angle of 2°, for 2θ values over 10°–80° in steps of 0.05° with a scan speed of 0.01° 2θ·s−1.


### 2.4.2. Electron Microscopy

The samples were characterized using field emission scanning electron microscopy (FE-SEM) (Leo, Zeiss), operated at 3–10 kV electron potential difference and equipped with a semiconductor detector that allows for detection of energy dispersive X-rays (EDX). The samples were prepared by placing a thin layer of powder on a carbon tape. The high resolution transmission electron microscopy (HRTEM) was carried out on a Joel JEM-2100 microscopy with a LAB6 filament. The measurements were carried out at 200 kV with a beam spot size of 20–200 nm in TEM mode. The samples were prepared by placing a drop of particles suspended in methanol on a holey carbon-coated copper grid.


## 2.4.1. X-Ray Diffraction

XRD patterns on powdered samples were measured on a Phillips X’Pert materials research diffractometer using secondary graphite monochromated Cu Kα radiation (λ=1.54060 Å) at 40 kV/50 mA. Measurements were taken using a glancing angle of incidence detector at an angle of 2°, for 2θ values over 10°–80° in steps of 0.05° with a scan speed of 0.01° 2θ·s−1.


## 2.4.2. Electron Microscopy

The samples were characterized using field emission scanning electron microscopy (FE-SEM) (Leo, Zeiss), operated at 3–10 kV electron potential difference and equipped with a semiconductor detector that allows for detection of energy dispersive X-rays (EDX). The samples were prepared by placing a thin layer of powder on a carbon tape. The high resolution transmission electron microscopy (HRTEM) was carried out on a Joel JEM-2100 microscopy with a LAB6 filament. The measurements were carried out at 200 kV with a beam spot size of 20–200 nm in TEM mode. The samples were prepared by placing a drop of particles suspended in methanol on a holey carbon-coated copper grid.


## 2.5. Optical Characterization

### 2.5.1. Absorption Spectroscopy

A Perkin Elmer Lambda 75S UV-VIS-NIR Spectrophotometer with double grating and double monochromator for high absorbance measurements was used to carry out the optical measurements. The powders were suspended in methanol and placed in quartz cuvettes (1 cm, path length). The band edges of the samples were determined from absorption spectrum by extrapolation.


### 2.5.2. Emission Spectroscopy

A Perkin Elmer LS55 with a xenon lamp (150 W) and a 152 P photo multiplier tube as a detector was used to measure the photoluminescence of the particles. The samples were suspended in methanol and placed in quartz cuvettes (1 cm path length) for spectral analysis.


## 2.5.1. Absorption Spectroscopy

A Perkin Elmer Lambda 75S UV-VIS-NIR Spectrophotometer with double grating and double monochromator for high absorbance measurements was used to carry out the optical measurements. The powders were suspended in methanol and placed in quartz cuvettes (1 cm, path length). The band edges of the samples were determined from absorption spectrum by extrapolation.


## 2.5.2. Emission Spectroscopy

A Perkin Elmer LS55 with a xenon lamp (150 W) and a 152 P photo multiplier tube as a detector was used to measure the photoluminescence of the particles. The samples were suspended in methanol and placed in quartz cuvettes (1 cm path length) for spectral analysis.


## 3. Results and Discussions

### 3.1. Morphological Properties

The XRD patterns of the as-synthesized ZnO and TiO2 are shown in Figures 1(a) and 1(b), respectively. The diffraction peaks in Figure 1(a) could be indexed to a hexagonal phase ZnO (JCPDS 36–1451). The slight broadening of the peaks is ascribed to size effect. The diffraction pattern of titania depicted in Figure 1(b), revealed the presence of both rutile (JCPDS 88-1175) and anatase (JCPDS 84-1286) phase. Two broad peaks belonging to neither rutile nor anatase were also detected. These peaks could be indexed to a titanate structure, Ti4O7. The titanate structures containing potassium ions, KTiO2(OH), have been previously observed and this was attributed to the intercalation of potassium ions into TiO2 framework [26]. In the current study, the use of microwave resulted in the formation of a titanate structure (Ti4O7) without potassium ions. This clearly shows that the intercalation of potassium ions is dependent on the time and method of processing. The crystallinity of the TiO2 sample is slightly poorer when compared to that of ZnO and this is probably due to the difference in particle size and shape.X-ray diffractograms of (a) ZnO and (b) TiO2.
(a)(b)The morphologies of ZnO and TiO2 nanostructures are depicted in Figure 2 and Figure 3, respectively. The SEM micrograph in Figure 2(a) shows rod-like nanostructures with pointed tips. The TEM image in Figure 2(b) confirms the morphology as that of pointed-tip rods. The particles have a very high aspect ratio. The averaged particle size was found to be 36 nm. The HRTEM depicted in Figure 2(c) shows a crystalline particle indicated by the presence of the lattice fringes with the lattice spacing (d=0.28 nm) that could be indexed to a (100) crystal plane of hexagonal ZnO. This is in agreement with the observed crystal phase in Figure 1(a). The sketch in Figure 2(d) shows the perceived geometry of the particle with the rod growth occurring along the (100) plane as corroborated by the HRTEM.(a) SEM, (b) TEM, (c) HRTEM micrographs of ZnO and (d) sketch illustrating the shape of ZnO.
(a)(b)(c)(d)(a) SEM, (b) TEM, (c) HRTEM micrographs of TiO2 and (d) formation mechanism of TiO2 nanotubes.
(a)(b)(c)(d)The SEM image of TiO2 in Figure 3(a) shows entangled nanotubular structures. The TEM confirms the morphology to be tubular rather than wires. The tubes show narrow size distribution with the diameters being approximately 25 nm. The HRTEM shown in Figure 3(c) shows a single tube with crystal fringes indexed to the anatase phase. The sizes of the walls of the tube appear to be asymmetrical. This is to be expected as various authors have suggested the formation of the tubes as a mere rolling up of the TiO2 sheets (Figure 3(d)) [26, 27]. This growth mechanism is clearly supported and confirmed in this case by the HRTEM image in Figure 3(c).


### 3.2. Optical Properties

Zinc oxide is a direct band gap semiconductor with bulk band gap energy of 3.37 eV (368 nm). The optical properties are shown in Figure4(a). The band edge is a function of the composition, size, and shape of the nanocrystal. The absorption spectrum has a band edge at 350 nm. The band edge is blue-shifted from bulk band edge of 368 nm. This is indicative of quantum confinement of the exciton within the ZnO nanocrystal and this is characteristic of nanoparticles. Another impressive feature of semiconductor nanoparticles is their ability to emit light. Upon excitation with wavelength shorter or equivalent to the absorption onset, an electron is promoted from the valence band to the conduction band, and upon relaxation a phonon of light is emitted. The emission spectrum of ZnO depicted in Figure 4(a) shows a relatively narrow Gaussian-distributed curve signifying a monodispersed particles population. The wavelength at maximum emission (420 nm) is red-shifted from the first absorption peak by a stoke shift of approximately 80 nm. The sharpness and the intensity of the peak suggest that the particles are very stable and have very few surface traps. The Stoke shift for the ZnO is particularly large. Stokes shift is well known both in the molecular spectroscopy and in the spectroscopy of the nanoparticles. It is known that this kind of shift (so-called Frank-Condon shift) is due to vibrational relaxation of the excited nanoparticles to the ground state [28].Absorption and emission spectra of (a) ZnO and (b) TiO2.
(a)(b)The absorption spectrum of TiO2 nanotubes in Figure 4(b) shows an absorption band edge at 371 nm. This peak is blue-shifted from the bulk band edge of 388 nm. Similarly to ZnO, this suggests strong quantum confinement of the excitons. The photoluminescence spectrum of TiO2 usually shows poor characteristics probably because the hydrothermal and sol-gel methods usually used to synthesize the nanostructures do not make use of the surface-passivating ligands resulting in formation of surface traps as well as high bundle formation in the case of nanotubes [28]. The emission spectrum for TiO2 nanotubes depicted in Figure 3(b) shows a narrow, sharp Gaussian peak with high intensity. The emission maximum located at 400 nm is red-shifted from the absorption band edge. The characteristics of the observed emission spectrum are indicative of minimum bundle formation as validated by the SEM and TEM. The use of microwave as the heating source compared to the conventional heating method used in hydrothermal processes results in short synthetic time as well as high energy system that can limit the formation of bundles.


## 3.1. Morphological Properties

The XRD patterns of the as-synthesized ZnO and TiO2 are shown in Figures 1(a) and 1(b), respectively. The diffraction peaks in Figure 1(a) could be indexed to a hexagonal phase ZnO (JCPDS 36–1451). The slight broadening of the peaks is ascribed to size effect. The diffraction pattern of titania depicted in Figure 1(b), revealed the presence of both rutile (JCPDS 88-1175) and anatase (JCPDS 84-1286) phase. Two broad peaks belonging to neither rutile nor anatase were also detected. These peaks could be indexed to a titanate structure, Ti4O7. The titanate structures containing potassium ions, KTiO2(OH), have been previously observed and this was attributed to the intercalation of potassium ions into TiO2 framework [26]. In the current study, the use of microwave resulted in the formation of a titanate structure (Ti4O7) without potassium ions. This clearly shows that the intercalation of potassium ions is dependent on the time and method of processing. The crystallinity of the TiO2 sample is slightly poorer when compared to that of ZnO and this is probably due to the difference in particle size and shape.X-ray diffractograms of (a) ZnO and (b) TiO2.
(a)(b)The morphologies of ZnO and TiO2 nanostructures are depicted in Figure 2 and Figure 3, respectively. The SEM micrograph in Figure 2(a) shows rod-like nanostructures with pointed tips. The TEM image in Figure 2(b) confirms the morphology as that of pointed-tip rods. The particles have a very high aspect ratio. The averaged particle size was found to be 36 nm. The HRTEM depicted in Figure 2(c) shows a crystalline particle indicated by the presence of the lattice fringes with the lattice spacing (d=0.28 nm) that could be indexed to a (100) crystal plane of hexagonal ZnO. This is in agreement with the observed crystal phase in Figure 1(a). The sketch in Figure 2(d) shows the perceived geometry of the particle with the rod growth occurring along the (100) plane as corroborated by the HRTEM.(a) SEM, (b) TEM, (c) HRTEM micrographs of ZnO and (d) sketch illustrating the shape of ZnO.
(a)(b)(c)(d)(a) SEM, (b) TEM, (c) HRTEM micrographs of TiO2 and (d) formation mechanism of TiO2 nanotubes.
(a)(b)(c)(d)The SEM image of TiO2 in Figure 3(a) shows entangled nanotubular structures. The TEM confirms the morphology to be tubular rather than wires. The tubes show narrow size distribution with the diameters being approximately 25 nm. The HRTEM shown in Figure 3(c) shows a single tube with crystal fringes indexed to the anatase phase. The sizes of the walls of the tube appear to be asymmetrical. This is to be expected as various authors have suggested the formation of the tubes as a mere rolling up of the TiO2 sheets (Figure 3(d)) [26, 27]. This growth mechanism is clearly supported and confirmed in this case by the HRTEM image in Figure 3(c).


## 3.2. Optical Properties

Zinc oxide is a direct band gap semiconductor with bulk band gap energy of 3.37 eV (368 nm). The optical properties are shown in Figure4(a). The band edge is a function of the composition, size, and shape of the nanocrystal. The absorption spectrum has a band edge at 350 nm. The band edge is blue-shifted from bulk band edge of 368 nm. This is indicative of quantum confinement of the exciton within the ZnO nanocrystal and this is characteristic of nanoparticles. Another impressive feature of semiconductor nanoparticles is their ability to emit light. Upon excitation with wavelength shorter or equivalent to the absorption onset, an electron is promoted from the valence band to the conduction band, and upon relaxation a phonon of light is emitted. The emission spectrum of ZnO depicted in Figure 4(a) shows a relatively narrow Gaussian-distributed curve signifying a monodispersed particles population. The wavelength at maximum emission (420 nm) is red-shifted from the first absorption peak by a stoke shift of approximately 80 nm. The sharpness and the intensity of the peak suggest that the particles are very stable and have very few surface traps. The Stoke shift for the ZnO is particularly large. Stokes shift is well known both in the molecular spectroscopy and in the spectroscopy of the nanoparticles. It is known that this kind of shift (so-called Frank-Condon shift) is due to vibrational relaxation of the excited nanoparticles to the ground state [28].Absorption and emission spectra of (a) ZnO and (b) TiO2.
(a)(b)The absorption spectrum of TiO2 nanotubes in Figure 4(b) shows an absorption band edge at 371 nm. This peak is blue-shifted from the bulk band edge of 388 nm. Similarly to ZnO, this suggests strong quantum confinement of the excitons. The photoluminescence spectrum of TiO2 usually shows poor characteristics probably because the hydrothermal and sol-gel methods usually used to synthesize the nanostructures do not make use of the surface-passivating ligands resulting in formation of surface traps as well as high bundle formation in the case of nanotubes [28]. The emission spectrum for TiO2 nanotubes depicted in Figure 3(b) shows a narrow, sharp Gaussian peak with high intensity. The emission maximum located at 400 nm is red-shifted from the absorption band edge. The characteristics of the observed emission spectrum are indicative of minimum bundle formation as validated by the SEM and TEM. The use of microwave as the heating source compared to the conventional heating method used in hydrothermal processes results in short synthetic time as well as high energy system that can limit the formation of bundles.


## 4. Conclusion

Highly crystalline ZnO nanorods and TiO2 one-dimensional structures were successfully synthesized via the microwave-assisted hydrothermal method. The structural properties of ZnO indicated the predominance of a hexagonal phase and growth of pointed nanorods in (100) direction. A mixed crystal phase was detected for TiO2 with anatase, rutile, and Ti4O7 present. The morphology was found to be tubular with diameters of approximately 25 nm. The difference in crystallinity of the two materials is ascribed to materials different size and morphology. There was also less formation of bundles thought to be as a result of the evenly distributed heat generated by the microwave. The optical properties of both ZnO and TiO2 nanostructures showed characteristics of strong quantum confinement regime. The photoluminescence spectrum of TiO2 nanotubes show good improvement from previously reported data.



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*Source: 189069-2012-02-29.xml*