Xinxin Xinga,
Yuxiu Lia,
Dongyang Denga,
Nan Chenb,
Xu Liua,
Xuechun Xiaoac and
Yude Wang*bc
aSchool of Materials Science and Engineering, Yunnan University, 650091, Kunming, People's Republic of China
bDepartment of Physics, Yunnan University, 650091, Kunming, People's Republic of China. E-mail: ydwang@ynu.edu.cn; Fax: +86-871-65153832; Tel: +86-871-65035570
cYunnan Province Key Lab of Micro-Nano Materials and Technology, Yunnan University, 650091, Kunming, People's Republic of China
First published on 10th October 2016
The aim of this paper is to develop easily manufactured and highly sensitive gas sensors for VOCs (volatile organic compounds) detection. Macro-/mesoporous 5 at% Al-doped ZnO (AZO) and Ag-AZO composite powders were prepared by a one-step solution combustion method and used to fabricate gas sensors. Both powders showed the same macro-/mesoporous morphology but have different grain sizes and separated silver phase due to the fast growth of ZnO and the reduction of Ag+. The capability of Ag-AZO was investigated for VOCs detection, including n-butanol, methanol, acetone, ethanol, isopropanol and formaldehyde. It is found that the added Ag greatly increases the gas response towards different VOCs. Particularly 2.5 at% Ag-AZO shows the most superior gas sensing performance to 100 ppm VOCs at an operating temperature of 240 °C, which is also the optimum operating temperature of other sensors. The results may be attributed to the synergistic effects of these doped and composite elements, the amount of adsorbed oxygen and the macro-/mesoporous morphology.
Zinc oxide (ZnO) has attracted much attention when applied as a gas sensing material, on account of its environmental friendliness, low cost, good compatibility, multiple morphology and so on.6–9 However, traditional semiconductor ZnO has the shortcomings of fast recombination of electron–hole pairs,10 few gas transmission paths11 and poor selectivity and gas response12 when it is utilized as a gas sensing material. Several efforts have been made in order to overcome these limitations, such as doping metal elements,13 noble metal-functionalized semiconductors,14 introducing heterostructures15 and heat treatment16 to form more active sites and structures with large surface area, and facilitate gas transmission and reaction on the surface of the materials. It has been proven that metal-doped ZnO exhibits good selectivity and high gas response to objective gas, high electrical conductivity and different lattice constants,17–19 which are good factors to improve gas sensing performance. AZO (Al-doped ZnO) as metal-oxide nanocomposites showed great sensing properties for the detection of objective gases.13,20–22 Moreover, AZO shows the highest conductivity when compared with Li-, Ca-, In-, N- and P-doped ZnO,19 making it practical for future application and a promising candidate in gas detection.
On this basis, some properties of Ag and Al co-doped ZnO have been discussed,23–25 and Ag has been proven to have a function to improve gas sensor properties due to its catalytic activity.14 In this paper, the amount of Al was reduced to improve conductivity, and Ag was added to form Ag-AZO macro-/mesoporous composite powders. We synthesized Ag-AZO powders using a self-sustained solution combustion method to obtain large specific surface area and hierarchically porous morphology, which were propitious for the flow of gases and the contact between active sites and the surface of the material. The gas sensing performances of these powders were investigated by detecting gas response of fabricated sensors towards VOCs (including n-butanol, methanol, acetone, ethanol, isopropanol and formaldehyde). It is found that 2.5 at% Ag-AZO shows better sensing properties to all VOCs at 240 °C compared with AZO and other samples with different atomic ratios of Ag (1 at%, 1.5 at%, 2 at% and 3 at% Ag-AZO). In the end, a possible mechanism of the influence of doped Al and added Ag, in the formation of a porous structure and high sensing performance was also proposed.
Ag-AZO was synthesized on the basis of 5 at% Al-ZnO (AZO). AgNO3 was added to the precursor solution ([Al3+]/[Zn2+] = 5%) and the amount of AgNO3 was calculated according to atomic molar ratios [Ag+]/[Zn2+] = 0%, 1%, 1.5%, 2%, 2.5% and 3%. The following steps were consistent with the abovementioned steps. Finally, the corresponding samples were labeled and named as x at% Ag-AZO (x = 1, 1.5, 2, 2.5 and 3).
Ra (resistance in air) values of pure ZnO and 2.5 at%, 5 at%, 7.5 at% Al-ZnO-based gas sensors were tested at first, and the results are list in Table 1. As we all know, the smaller the Ra is, the more favorable it is for the application of gas sensors. Therefore, in the following tests, we added Ag on the basis of 5 at% Al-ZnO because of its lowest resistance in air. Ra values of 1%, 1.5%, 2%, 2.5% and 3% Ag-AZO-based gas sensors changed a little compared with that of the AZO-based gas sensor. n-Butanol, methanol, acetone, ethanol, isopropanol and formaldehyde were chosen as six types of VOCs to evaluate gas sensing properties of the Ag-AZO-based gas sensors.
Materials based gas sensor | Operating temperature (°C) | Ra (kΩ) (resistance in air) |
---|---|---|
ZnO | 240 | 1123 |
2.5% Al-ZnO | 240 | 1157 |
5% Al-ZnO (AZO) | 240 | 12 |
7.5% Al-ZnO | 240 | 30 |
1% Ag-AZO | 240 | 14 |
1.5% Ag-AZO | 240 | 22 |
2% Ag-AZO | 240 | 33 |
2.5% Ag-AZO | 240 | 19 |
3% Ag-AZO | 240 | 36 |
Samples | ZnO/AZO | Average grain size of ZnO/AZO (nm) | Average grain size of Ag (nm) | |
---|---|---|---|---|
a (Å) | c (Å) | |||
ZnO | 3.2549 | 5.2141 | 73.8 | — |
5% Al-ZnO (AZO) | 3.2524 | 5.2109 | 50.0 | — |
1% Ag-AZO | 3.2527 | 5.2077 | 18.4 | 45.0 |
1.5% Ag-AZO | 3.2582 | 5.2140 | 17.6 | 46.5 |
2% Ag-AZO | 3.2520 | 5.2086 | 21.4 | 33.4 |
2.5% Ag-AZO | 3.2544 | 5.2095 | 19.8 | 52.5 |
3% Ag-AZO | 3.2537 | 5.2119 | 24.9 | 38.1 |
The surface morphology and structure of the as-prepared samples were investigated by SEM. A coral-like structure can be observed in Fig. 2 and it does not change when Ag is added. The coral-like structure consists of interconnected channels with the diameter size ranging from several nanometers to ten micrometers forming a hierarchical macro-/mesoporous architecture. This type of structure provides an easy way for the flow of air and contact between objective gas and active sites, which is used to improve gas sensing performance.
TEM was employed to analyze morphology characteristics and grain size of AZO and 2.5 at% Ag-AZO. The macro-/mesoporous structure can be evidently observed in Fig. 3, which confirms the SEM results. These mesopores consist of self-assembled nanoparticles with diameters ranging from 4 to 38 nm, which are irregular crystal nanoparticles. The energy for self-assembly of nanoparticles is derived from the heat produced by combustion. The diameter of crystalline grains of 2.5 at% Ag-AZO, shown in Fig. 3(b), is smaller than that of AZO, as shown in Fig. 3(a). Therefore, the TEM results are in good agreement with the XRD conclusions and the data listed in Table 1. The crystalline grains were found to grow irregularly, producing more defects on the surface of the nanoparticles, which can provide more adsorbed oxygen to promote gas sensing performance.31
Nitrogen adsorption–desorption isotherms were investigated to analyze the hierarchically porous structure of the as-prepared AZO and 2.5 at% Ag-AZO powders. The insets in Fig. 4(a) and (b) calculated by the BJH method indicates that the pore diameter of AZO ranges from 1.3 to 109.2 nm with a maximum at 3.8 nm, and that of 2.5 at% Ag-AZO ranges from 1.3 to 102.7 nm with a maximum at 13.2 nm, illustrating that the pore sizes are distributed over a wide range. Hysteresis loops located between the adsorption and desorption branches at P/P0 ranging from 0.45–0.95 exhibit the existence of mesopores (about 2–50 nm in diameter) formed by self-assembled nanoparticles.8,16 This indicates that the inner architectures of these hierarchically porous samples are not solid, but full of pore structure. The loop observed at high relative pressure (above 0.9) illustrates the existence of macropores (>50 nm in diameter), which can be directly observed in the images of SEM and TEM. The BET specific surface area of AZO and x at% Ag-AZO where (x = 1, 1.5, 2, 2.5 and 3) are 45.59, 39.83, 46.17, 41.55, 40.13 and 43.85 m2 g−1, respectively, which provides enough surface area to promote the contact between gas and active sites on the surface of the prepared samples.
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Fig. 4 N2 absorption–desorption isotherms of (a) AZO and (b) 2.5% Ag-AZO. The insets are the pore-size distribution calculated by the BJH method from the desorption. |
X-ray photoelectron spectroscopy (XPS) was used to analyze surface compositions and chemical states of AZO and 2.5 at% Ag-AZO. In Fig. 5(a), Zn 2p spectra of 2.5 at% Ag-AZO reveal two peaks located at 1044 (Zn 2p1/2) and 1021 eV (Zn 2p3/2) with the splitting distance of 23 eV, which illustrates that Zn exists as Zn2+.32 The Ag 3d spectra of 2.5 at% Ag-AZO shows two peaks of Ag 3d3/2 and Ag 3d5/2 with the splitting of the 3d doublet of 6 eV attributed to metallic silver,14,33 which is in concert with the XRD result. In Fig. 5(c) and (d), the Al 2p peak can be fitted to two peaks with reference to Al–OH and Al–O bonds in the samples.34 The data are around 74.53 and 73.57 eV for 2.5 at% Ag-AZO and 74.76 and 73.93 eV for AZO. The Al–OH bond is formed due to the adsorbed H2O reacting with O2 on the surface of the powder. The Al–O bond is formed by Al3+ (exchanging the Zn2+ in the bulk) combining with the lattice oxygen. The added Ag does not change the existing form of Al. No trace of Al–Al bonds located at around 72.7 eV can be found in the XPS result.35 From Fig. 5(e) and (f), the low binding energy component located at 530.6 eV is attributed to O2− ions in the crystal lattice of wurtzite-type ZnO surrounded by Zn (or doped Al) atoms, and the high binding energy component located at 531.8 eV is attributed to surface adsorbed Ox− ions like O−, O2− and O2−.36–38 O2 combines with one electron to form O2−, and then O2− combines with one electron to form O−.39 However, only the surface-adsorbed Ox− can react with gas. So the improvement of the area of the Ox− peak can directly affect the gas sensing performance.
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Fig. 5 High-resolution spectra of (a) Zn 2p, (b) Ag 3d, (c) Al 2p and (e) O 1s of 2.5% Ag-AZO. High-resolution spectra of (d) Al 2p and (f) O 1s of AZO. |
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Fig. 6 Gas response of pure ZnO, AZO and x at% Ag-AZO-based gas sensors towards 100 ppm (a) n-butanol, (b) methanol, (c) acetone, (d) ethanol, (e) isopropanol and (f) formaldehyde. |
Materials | Concentration (ppm) | Temperature (°C) | Sensitivity | Ref. | |||||
---|---|---|---|---|---|---|---|---|---|
n-Butanol | Methanol | Acetone | Ethanol | Isopropanol | Formaldehyde | ||||
Meso-/macroporous Co3O4 | 1000 | 120 | 27.7 | 13.0 | 16.8 | 22.0 | 19.0 | 7.2 | 16 |
Co3O4 nanosheets | 300 | 100 | 767 | 94 | 234 | 15 | 353 | 36.4 | 40 |
Nanoporous TiO2 | 500 | 370 | 7.56 | 9.86 | 25.97 | 11.19 | 5.35 | 3.53 | 41 |
ZnO hollow spheres | 500 | 385 | 292 | 25.4 | — | 97.3 | 146 | 12.3 | 42 |
Porous flower-like SnO2 | 260 | 100 | — | 5.1 | 5.7 | 6.4 | — | — | 43 |
Pt–SnO2 nanocomposite | 100 | 50 | 44.2 | 2.7 | — | 8.3 | — | — | 44 |
Magnetron-sputtered CuO NPs | 500 | 200 | — | 3.2 | — | 5.6 | — | — | 45 |
Microporous Co3O4@C | 100 | 170 | — | 11 | 7.8 | 14.7 | — | — | 46 |
Er–SnO2 nanobelts | 100 | 230 | — | — | 4.8 | 5.3 | — | 9 | 47 |
Au–WO3 nanofibers | 100 | 250 | 229.7 | 8.1 | 22.3 | 90.8 | — | — | 48 |
Macro-/mesoporous Ag-AZO | 100 | 240 | 994.8 | 448.42 | 336.56 | 444.04 | 437.37 | 87.66 | This work |
As a typical n-type metal oxide, the gas response (Ra/Rg) of the ZnO-based gas senor shows a rise when reducing gas is injected into the testing equipment. The same type of response and recovery curves are shown in Fig. 7, indicating that the added Ag-AZO maintains the n-type semiconducting characteristic. The 2.5 at% Ag-AZO-based gas sensor was tested towards 100 ppm different VOCs at the optimum operating temperature of 240 °C. One can observe that the response and recovery time of this sensor have been marked out. The response times (time needed to reach 90% of the adsorption platform) towards n-butanol, methanol, acetone, ethanol, isopropanol and formaldehyde were calculated as 66, 18, 69, 36, 26 and 47 s, respectively, and the recovery times (time need to return to 10% above the original response in air) were 25, 8, 13, 12, 9 and 5 s, correspondingly. All of these results illustrate that the 2.5 at% Ag-AZO-based gas sensor reveals relatively quick response and recovery times to VOCs.
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Fig. 7 Typical response and recovery times of the 2.5 at% Ag-AZO-based gas sensor to 100 ppm (a) n-butanol, (b) methanol, (c) acetone, (d) ethanol, (e) isopropanol and (f) formaldehyde. |
Afterwards, in order to analyze the effect of gas concentrations on gas sensitivities, n-butanol was chosen as the objective gas because the gas sensor has the highest gas response towards n-butanol, which can be more convenient to observe and analyze. As an example, the sensing property of the 2.5 at% Ag-AZO-based gas sensor was tested towards 1–100 ppm n-butanol at the optimum operating temperature of 240 °C. Dynamic response and recovery curves to n-butanol of different concentrations (1–100 ppm) are shown in Fig. 8(a). Even at a low detection limit of 1 ppm, the gas response is about 14.66, which indicates its good sensitivity towards low-concentration VOCs. When concentration reaches 100 ppm, it shows an excellent gas response, as high as 996.48. The injection of n-butanol results in a rise of gas response and every adsorption platform returns to its baseline value after the gas is released. As shown in Fig. 8(b), with the enhancement of gas concentration, gas response shows a corresponding improvement. These phenomena indicate that the adsorption towards n-butanol by Ag-AZO-based gas sensors is reversible.
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Fig. 8 (a) Dynamic sensing properties for 2.5% Ag-AZO to n-butanol from 1 to 100 ppm at 240 °C. (b) Gas responses to different concentrations of n-butanol of 2.5% Ag-AZO at 240 °C. |
In practice, long-term stability is one of the key problems to determine the practical application of gas sensors.49 To detect the stability of the 2.5 at% Ag-AZO-based gas sensor, we conducted the test at the optimum operating temperature of 240 °C to three randomly selected VOCs, including n-butanol, methanol and acetone. In Fig. 9, one can observe a downward trend of gas responses towards the three types of VOCs. In the first few days, the gas responses decayed sharply and then tended to be stable with slight swings in the rest of the time. The possible reasons for the oscillation can be explained as follows. For one thing, the core of this kind of gas sensor is welded above bakelite base through four platinum wires, which are utilized for the output of electric current and signal. During the long-term stability test conducted at 240 °C the strength of the metal wires decreased. Once the gas sensor is in use it is inevitable that it will suffer bumps and vibrations. When the welding points are not firm enough, the stability of this sensor will be affected. For another point, Ag is added to improve the selectivity and sensitivity of gas sensors, but the main disadvantage is that Ag atoms easily migrate in the electric field and the environment of high temperature and high humidity.50 Moreover, the grain size is considered as one of the most important parameters to affect the stability of the gas sensor. The grain size might grow during the experiment, which can change the resistance of the sensor and further influence the stability.51 In addition to these reasons, numerous factors closely influence the stability performance of sensors, such as structural transformation, phase transformation, poisoning, degradation of contacts and heaters, bulk diffusion, errors in design, change of humidity, fluctuations of temperature in the surrounding atmosphere and interference effects.52 The prepared gas sensors are barely satisfactory in their long-term stability performance, which is an unfavorable factor needing to be overcome for its application in the long run.
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Fig. 9 Long-term stability of the 2.5% Ag-AZO-based gas sensor towards 100 ppm n-butanol, methanol and acetone tested once a day for 30 days. |
Based on the abovementioned results, the enhancement of gas sensing properties is related to the following issues. For one thing, the special microstructure of the prepared samples synthesized by a self-sustained solution combustion method exhibits abundant pore structure, which is better for gas circulation and provides sufficient surface area. Moreover, the excellent gas response can be attributed to the increased amount of absorbed Ox− ions (for example O−, O2− and O2−) influenced by Al doping. A large number of electrons are released when the positions of Zn2+ are replaced by Al3+ ions,13,53 resulting in the improvement of conductivity. The possible mechanism is as follows:
Al2O3 + ZnO → ZnZn + 2AlZn+ + 3OOx + (1/2)O2(g) + 2e | (1) |
These descriptive electrons are easily captured by the adsorbed oxygen to form Ox− ions,39 which play an important role to enhance the gas sensing property.4,9–12 The decrease of free electrons may increase resistance of the gas sensor. On the contrary, when gas sensors are exposed to VOCs, Ox− ions can react with these reducing gases with the release of captured electrons, resulting in the decrease of resistance.14,31 The reaction process is as follows:
VOCs + Ox → CO2 + H2O + e | (2) |
Thus, the testing atmosphere switching between VOCs and air can cause a distinct change in conductivity of the sensors, which can directly enhance gas sensing performance. Fig. 10 graphically displays the mechanism of the entire reaction.
As has been reported in ref. 14, 54 and 55, Ag nanoparticles can prominently enhance the gas sensing property of metal semiconductor materials like ZnO and SnO2. The work function of AZO (5 at% Al-doped ZnO) has been studied.56 The energy band structure of metal Ag and AZO before and after contact are displayed in Fig. 11. In Fig. 11(b), the electrons flow across the interface which evidently increases the electron concentration on the AZO surface, because the electrons transfer from a metal having a lower work function (Wm) to a semiconductor with a higher work function (Ws). Once the Ag-functionalized AZO-based gas sensor is exposed to air, the oxygen will capture electrons from the surface of AZO to form Ox−, as observed in the XPS results, leading to an increase in resistance. Ox− can react with VOCs and break the VOC molecules into H2O and O2, releasing electrons back to the conduction band of ZnO, which is the same as the process in Fig. 10. The released electrons will lead to a decrease in resistance of the gas sensor.14,57,58 Therefore, the resistance of the gas sensor is greatly influenced by Ag and Ox−, which can strongly affect the gas response of the gas sensor by switching the resistance between air and objective gas. Thus, we can obtain gas sensors with high sensitivity.
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Fig. 11 Schematic of the energy band structure of the Ag-functionalized AZO (a) in air and (b) in VOCs. |
Ag can efficiently increase the capacity of adsorbed oxygen and accelerate the reaction between Ox− ions and objective VOCs due to its highly catalytic activation. Moreover, the catalyst metal Ag can resolve hydrocarbons into more active smaller molecules to promote the reaction between Ox− ions and reducing gases.
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