ISRN NanotechnologyVolume 2012 (2012), Article ID 879480, 6 pagesdoi:10.5402/2012/879480

Research Article

Preparation and Ethanol Sensing Properties of ZnO Nanoparticles via a Novel Sol-Gel Method

A. Ahmadi Daryakenari,¹ M. Ahmadi Daryakenari,² Y. Bahari,¹ and H. Omivar²

¹Materials and Energy Research Center, P.O. Box 31787-316, Karaj, Iran²Amirkabir University of Technology, 424 Hafez Ave, P.O. Box 15875-4413, Tehran, Iran

Received 26 October 2011; Accepted 8 December 2011

Academic Editors: R. Alexandrescu and D. Tsoukalas

Copyright © 2012 A. Ahmadi Daryakenari et al. This is an open access article distributed under the Creative Commons Attribution License, which permits unrestricted use, distribution, and reproduction in any medium, provided the original work is properly cited.

Abstract.

ZnO nanoparticles were prepared using a novel sol-gel method. Chemical reactions were carried out between zinc acetate and methanol under ambient conditions using monoethanol amine (MEA) as surfactant and subsequent heating at . The powders were calcined, pressed into pellets, and presintered. The properties of the product were characterized by X-ray diffraction (XRD), scanning electron microscopy (SEM), and Fourier transform infrared (FTIR) spectra. For gas sensing experiment, ethanol was used as testing gas. The gas sensing results showed that the maximum value for detecting of 1000 ppm ethanol vapor was 25 at an operating temperature of .

1. Introduction

Oxide semiconductor nanostructures have been widely investigated in recent years because of their excellent properties [1] and application in novel optical, electrical, and mechanical devices such as photovoltaic solar cells, luminescence, biomedicine, photocatalysis, light-emitting diodes (LEDs), varistors, and optoelectronic nanodevices [2–6].

ZnO is an n-type II–VI semiconductor with wide band gap of 3.37 eV, large exciton binding energy (~60 meV), strong emission, large saturation velocity (~3.2 × 107 cm/s), and high breakdown voltage [7, 8]. These properties make it a promising material for optoelectronic devices in the ultraviolet (UV) and blue region of the electromagnetic spectrum [9], optical or display devices, solar cells [9, 10] catalysis [11], cantilevers production, piezoelectric applications [6], superficial acoustic waves (SAW) [12], and humidity [11] and gas sensors [13]. Furthermore, ZnO has high transparency, chemical and thermal stability, high conductance, and it is nontoxic, inexpensive, and one of the few oxides that exhibit quantum confinement effects in an experimentally accessible size range [2, 3]. ZnO nanostructures which can come in different shapes such as nanowires, nanobelts, nanorods, nanotubes, and nanoparticles can exhibit interesting physical and chemical properties not found in other nanostructures [14, 15]. ZnO in pure and doped form has been intensively studied, and ZnO gas sensor elements have been prepared and studied in different forms, mostly as thin films, thick films, single crystals, wintered pellets, and hetero junctions while not many have been reported in the bulk form [16, 17]. Various methods have been used for the production of ZnO nanostructures, such as vapor-liquid-solid (VLS) method, reaction-vapor deposition, physical vapor deposition, pulsed-laser deposition, thermal evaporation, metal organic chemical vapor deposition (MOCVD), which utilize expensive equipment and are energy consuming (the working temperature is higher than 400°C) and chemical solution routs like sol-gel, coprecipitation, hydrothermal, and template-based methods [15, 18, 19]. In comparison with bulk ZnO, nanocrystalline ZnO gas sensors have drawn interest due to their application in detecting hydrogen [19], pollutants and toxic gases [13], organic compounds [20, 21], alcohols [19, 22, 23], moisture [11, 24], and so forth. The aim of the present work is to synthesize and characterize the novel sol-gel-prepared ZnO nanoparticles and to investigate the ethanol sensing properties of such nanoparticles.

2. Experimental

All the reagents used in our experiments were prepared from MERC with 99.0% purification. Zinc acetate dihydrate (Zn (CH₃COO)₂ 2H₂O) was used as zinc source. Methanol and MEA were applied as solvent and surfactant, respectively. The molar ratio of MEA to zinc acetate dihydrate was maintained at 1.0, and the concentration of zinc acetate was adjusted at 0.5 mol/L. First, zinc acetate dihydrate was dissolved in a mixture of methanol and MEA at room temperature. After vigorous stirring using a magnetic bar for 1 h, the solution became homogeneous and clear and allowed to age for 24 h. Then the aged solution was heated at 200°C for 3 h. The remaining black sediment at the bottom of the container is our green nanoparticle (GNP). Next, the GNP calcined at 500°C (which determined by TG/DTA analysis), and a white powder was obtained (calcined nanoparticle (CNP)). For evaluating sensor properties, pellets (diameter 13 mm and thickness 1.5 mm) were prepared from the CNP using hydraulic press and applying 2 tones for 2 min and subsequently presintering at 400°C for 1 h. The gas sensing properties were evaluated at various concentrations of ethanol gas and several operating temperatures, from 300°C to 400°C, by measuring the changes of resistance of the sensor in air and in gas.

The crystal structure of GNP was characterized by X-ray diffraction (XRD) (Philips, Model PW3710, ). The XRD pattern of GNP is represented in Figure 1. All the diffraction peaks could be indexed to hexagonal wurtzite ZnO according to standard JCPDS card no. 36-1451,  nm,  nm with high crystallinity. By applying the Debye-Scherrer formula , where is the main crystallite size, λ is the wavelength of the X-ray radiation (1.54), k is a constant to be taken as 0.9, β is the full width at half maximum height of the peak (FWHM), and θ is the diffraction angle, resulting in the 21 nm crystallite size for the as-prepared GNP.

Figure 1: XRD pattern of GNP. All the peaks can be assigned to ZnO.

Because the XRD pattern could not detect the noncrystalline materials, it should be noted that since in, this study, we used organic solvents and a surfactant, There is some possibility that they still remain in the black sediment and are not completely removed.

The IR spectrum of GNP (Figure 2) exhibits absorption peaks. The broad absorption band centered at 3438 cm⁻¹ is attributed to the band O–H stretching vibrations, and the band at 1557 cm⁻¹ is primarily due to the bending vibration of N–H. The band at 1422 cm⁻¹ is attributed to the bending mode (H–C–H). The bands around 1281, 1021, and 546 cm⁻¹ are related to the vibration of C–N, C–O, and Zn–O, respectively. Hence, the FTIR data confirms the presence of organic compounds. The suggestion for such reactions could be as Scheme 1 [25].

Scheme 1

Figure 2: The FT-IR spectra of GNP.

Figure 3 shows the TG/DTA curve of GNP. There is no significant weight loss before 200°C since our working temperature was at 200°C. At this temperature, thermal decomposition begins gradually, and the sharp peak in DTA graph is attributed to the elimination and decomposition of zinc alkoxide by organic compounds.

Figure 3: (a) TG, (b) DTA graph of GNP.

A weight loss of about 20 wt% is observed before 475°C is reached. At this point, all organic compounds have volatilized such that the molecule will be stable and its weight nearly constant as illustrated in the DTA graph.

The XRD patterns of the CNP and pellets are represented in Figure 4. In comparison with Figure 2, there is no change in diffraction peaks. Therefore, a zinc oxide (without organic compounds) with the same crystal structure is established. By applying the Debye-Scherrer formula, the main crystallite size would be 39 nm for CNP and 42 nm for pellets. The growth of crystallite size is easily attributed to the relatively high temperature of calcinations and following press.

Figure 4: (a) The XRD patterns of the CNP and (b) pellets.

Figure 5(a) shows the SEM image of GNP. Most of the particles have a size less than 80 nm with relatively good distribution and near spherical morphology. The SEM image of pellets is shown in Figure 5(b). Pellets have a small growth (less than 10 nm) in size, but their morphologies totally transferred to spherical.

(a)

(b)

Figure 5: SEM image of (a) GNP and (b) pellets.

The sensitivity of pellets in the experiment to the ethanol gas could be defined as where is the sample resistance measured in the air and is sample resistance under ethanol gas.

Figure 6 describes the sensitivity changes of pellets versus operating temperature at the concentration of 1000 ppm of ethanol gas. It could be observed that sensitivity will increase with increasing temperature from 300°C to 370°C where sensitivity reaches a maximum value of 25 at 370°C. After that, the sensitivity suddenly decreases to 19 at 390°C. Since sensitivity is related to both and , the sudden decrease may be attributed to two reasons.

Figure 6: Sensitivity of pellets in various temperatures.

First is the widely accepted phenomenon of chemisorptions when an n-type semiconductor gas sensor presented in air. Chemisorption of oxygen molecules could happen on the surface in the form of , , and ions by capturing electrons from the conductance band, since the electronegativity of oxygen molecules is higher than semiconductor. As a result, an electron-depleted space-charge layer in the surface region of the particle will be produced (Figure 7). Takata et al. found that the stable oxygen ions were below 100°C, between 100 and 300°C, and above 300°C [26].

Figure 7: Electron-depleted layer model (d is distance from surface and is depth of depletion layer).

Therefore, oxygen adsorption plays an important role in the resistance of pellets, and the amounts of such chemisorbed oxygen species depend strongly on the temperature.

Before 370°C, air resistance increases with increasing temperature. Since the oxygen species capture conduction electrons from the materials, this leads to a decrease in the electron concentration [22], and the depletion layer becomes larger because of the higher concentration of the adsorbed oxygen. But above 370°C, the decrease in occurs since the adsorption reaction is exothermic and the reaction () will proceed to the left. This causes the reduction of the trapped electrons from the conductance band [27] and the enlargement of the depletion layer.

The next reason could be attributed to . In the presence of the test gas (R), chemisorption of gas molecules to the surface will result in RO molecules. As the temperature increases to 370°C, there is greater adsorption of RO molecules (since the RO molecules leave the surface and the active sites remain free for the other gas molecules). As a result, charging of electrons in the conduction band occurs, the depletion layer becomes smaller, and the drops which is followed by an increase in the sensitivity. The reaction is expressed as follows [22, 28]: Here the testing gas is ethanol, and therefore, where the subscripts gas and ads, mean gas and adsorbed respectively.

After that, the physisorption rate of R molecules will decrease. Therefore, fewer electrons will be charged in the conduction band and the larger depletion layer causes an increase in .

The effect of ethanol concentration on sensitivity at 370°C is described in Figure 8. As would be expected, the sensitivity will be enhanced by presenting further ethanol concentration. The slope of the curve drops and the sensitivity will reach a saturation value in the large ethanol concentration due to the fact that the active sites of surface will be occupied by more ethanol molecules until the surface is completely covered by gas molecules.

Figure 8: Relationship between the ethanol concentration and sensitivity.

Figure 9 shows the effect of ethanol concentration on both response time (the time in which the gas resistance reaches 90% of its maximum value) and recovery time (the time in which the air resistance reaches 90% of its maximum value after removing the gas). By providing more ethanol gas, it can be expected that the depletion layer would be tightened since more electrons will charge in the conductance band according to (5). As a result, response time will be reduced. Similar description is applicable for recovery time.

Figure 9: Relationship between ethanol concentration and both response and recovery time.

3. Conclusion

In summary, ZnO nanoparticles were synthesized using the sol-gel technique. The minimum temperature for calcination of GNP was determined at 475°C by TG-DTA curve. The CNP was pressed to pellets and presintered at 400°C. Crystallite size for pellets was determined to be 42 nm from XRD. SEM image showed that the majority of particles have a size less than 90 nm with relatively good distribution and near-spherical morphology. In the ethanol sensing experiment, sensitivity reached a maximum value of 25 at 370°C and then decreased to 19 at 390°C for 1000 ppm of ethanol concentration. By increasing the concentration of ethanol, the sensitivity was enhanced and both response and recovery time dropped. Therefore, sol-gel-prepared ZnO pellets have been shown to demonstrate excellent sensing properties.

Acknowledgment

The authors would like to thank the Electrochemistry Laboratory of the Materials and Energy Research Center for its support.

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