Location via proxy:   [ UP ]  
[Report a bug]   [Manage cookies]                
Skip to main content
PMC home page
Sensors (Basel, Switzerland) logoLink to Sensors (Basel, Switzerland)
. 2018 Feb 27;18(3):701. doi: 10.3390/s18030701

Synthesis of ZnMn2O4 Nanoparticles by a Microwave-Assisted Colloidal Method and their Evaluation as a Gas Sensor of Propane and Carbon Monoxide

Juan Pablo Morán-Lázaro 1,*, Erwin Said Guillen-López 2, Florentino López-Urias 3, Emilio Muñoz-Sandoval 3, Oscar Blanco-Alonso 4, Héctor Guillén-Bonilla 5, Alex Guillén-Bonilla 1, Verónica María Rodríguez-Betancourtt 6, Marciano Sanchez-Tizapa 2, María de la Luz Olvera-Amador 7
PMCID: PMC5876874  PMID: 29495427

Abstract

Spinel-type ZnMn2O4 nanoparticles were synthesized via a simple and inexpensive microwave-assisted colloidal route. Structural studies by X-ray diffraction showed that a spinel crystal phase of ZnMn2O4 was obtained at a calcination temperature of 500 °C, which was confirmed by Raman and UV-vis characterizations. Spinel-type ZnMn2O4 nanoparticles with a size of 41 nm were identified by transmission electron microscopy. Pellet-type sensors were fabricated using ZnMn2O4 nanoparticles as sensing material. Sensing measurements were performed by exposing the sensor to different concentrations of propane or carbon monoxide at temperatures in the range from 100 to 300 °C. Measurements performed at an operating temperature of 300 °C revealed a good response to 500 ppm of propane and 300 ppm of carbon monoxide. Hence, ZnMn2O4 nanoparticles possess a promising potential in the gas sensors field.

Keywords: ZnMn2O4, nanoparticles, microwave, gas sensor

1. Introduction

The excessive emission of polluting and toxic gases, such as propane (C3H8) and carbon monoxide (CO), in urban and rural areas because of human activities such as transportation, production, landfill, and livestock farming has generated many public health concerns as well as environmental concerns over global warming. In this sense, resistive sensors based on semiconductor metal oxides have been widely used for the detection of several gases and vapors. These types of gas sensors have been used because they are cheap, easy to operate, and chemically stable in harsh conditions. The operational principle of these sensors is based on changes of the electrical conductivity when a reaction occurs between pre-adsorbed oxygen molecules, or the material itself, and a reducing or oxidizing gas [1]. Most of these sensors are based on binary metal oxides, such as SnO2 [2,3,4], ZnO [5,6], and TiO2 [7,8]. More recently, ternary compounds such as NiSb2O6 [9], CuSb2O6 [10], MgSb2O6 [11], LaCoO3 [12], ZnM2O4 (M = Fe, Co, Cr) [13], and MFe2O4 (M = Co, Ni) [14], have also been used. Ternary metallic oxides with a particle size on the nanometric scale display significant responses when they are exposed to reducing or oxidizing gases. As is already known, when the particle size is reduced to a nanometric size, the surface area-to-volume ratio increases, favoring the adsorption of a gas on the sensor [15]. Also, it has been reported that the gas response depends on the morphology of the material, the gas concentration, and the operational temperature [12,16,17,18]. In fact, some common issues of resistive sensors based on metallic oxides are the low response and the high operating temperature; therefore, the search for new materials without these problems is an important research topic.

Among the spinel-type oxides, the zinc manganite (ZnMn2O4) is a compound that possesses a normal spinel structure, where the divalent Zn cation occupies the tetrahedral site and the trivalent Mn cation occupies the octahedral site in the cubic spinel structure. ZnMn2O4 is an interesting compound that has been widely used as an electrode for Li-ion batteries due to its low cost and being environmentally friendly [19,20,21,22,23,24]. Also, this material has been used as a supercapacitor [25,26,27,28,29] and thermistor [30] due to its structural, physical, and chemical properties. It has been reported that zinc manganite shows strong catalytic activity [31,32,33,34,35]; therefore, this material could perform well as a gas sensor. To date, ZnMn2O4 has been little studied in the gas sensors field. Nassar et al. [36] developed a chemical sensor based on ZnMn2O4 nanostructures, which exhibited high sensitivity to omeprazole and lansoprazole drugs. Sorita and Kawano [37] used the oxide as ann electrode in a CO sensor based on a zirconia galvanic cell, obtaining a response of 9.68 at 2000 ppm of CO at 400 °C. Na et al. [38], as well as Panmatarith and Innoi [39], studied the response of sensors made from ZnO–ZnMn2O4 nanostructures to substances like ethanol, ammonia, carbon monoxide, propane, hydrogen peroxide, etc.

In regard to the synthesis of nanometric ZnMn2O4, several routes have been commonly employed: polymer-pyrolysis [23], solid-state reaction [24], sol-gel [31], co-precipitation [33], hydrothermal [29,40], and solvothermal methods [41]. Reports on the synthesis of ZnMn2O4 nanoparticles using a microwave-assisted route are still limited. Recently, Brahma et al. [42] obtained ZnMn2O4 nanoparticles using a three-step process that included microwave irradiation, centrifugation, and washing.

In this work, nanoparticles of the ternary compound ZnMn2O4 were synthesized using a microwave-assisted colloidal route without the use of a centrifugation and washing [9,10,43,44]. It is noteworthy to mention that microwave irradiation provides a rapid evaporation of the solvent from the precursor solutions, shortening the reaction times [45]. The ZnMn2O4 nanoparticles were characterized by means of thermogravimetric analysis (TGA), X-ray powder diffraction (XRD), Raman and UV-vis spectroscopies, and transmission electron microscopy (TEM). In addition, the performance of zinc manganite nanoparticles as a sensor of C3H8 and CO was evaluated.

2. Materials and Methods

2.1. ZnMn2O4 Synthesis

ZnMn2O4 nanoparticles were prepared by a microwave-assisted colloidal method, using as starting reagents: Zinc nitrate hexahydrate (Zn(NO3)2·6H2O, Sigma-Aldrich 98%, St. Louis, MO, USA), manganese(II) nitrate tetrahydrate (Mn(NO3)2·4H2O, Aldrich 99%, St. Louis, MO, USA), dodecylamine (C12H27N, Aldrich 98%, St. Louis, MO, USA), and ethanol (C2H6O, Hycel 96%, Zapopan, Jalisco, Mexico). Three solutions were prepared using 5 mL of ethanol as solvent: (i) A 5 mmol solution of zinc nitrate; (ii) a 10 mmol solution of manganese nitrate; (iii) a 16.2 mmol solution of dodecylamine. All the solutions were stirred at ~300 rpm for 20 min at room temperature. Afterwards, the zinc nitrate solution was slowly added under stirring to the dodecylamine solution. Subsequently, the manganese solution was added dropwise to the zinc + dodecylamine mixture, producing a brownish solution with pH = 2. To prevent gelation of the solution, 8 mL of ethanol were added. The final solution was kept under stirring at ~300 rpm for 24 h at room temperature. After that, microwave radiation was applied for periods of 2 min for about 4 h until the solvent was removed. A black viscous material was obtained. For our purposes, a kitchen-type microwave oven (Whirlpool WM1311S, Benton Harbor, MI, USA) was used, operating at low power (~300 W). The resulting material was dried in air at 200 °C for 8 h using a muffle (Terlab TE-M20DR, Zapopan, Jalisco, Mexico). The calcination of the resulting black powder was carried out at different temperatures in the range from 300 to 600 °C for 5 h, at a heating rate of 100 °C/h. The synthesis process is depicted in Figure 1.

Figure 1.

Figure 1

Open in a new tab

Schematic representation of the synthesis of ZnMn2O4 nanoparticles.

2.2. Characterization of ZnMn2O4 Powders

The thermal decomposition of the precursor powder, as a function of temperature, was followed at a rate of 10 °C/min by means of a thermogravimetric analysis using a PerkinElmer TGA 4000 device in an atmosphere of air. The crystal structure of the calcined samples was analyzed by the XRD technique using a PANalytical Empyrean equipment operated at 45 kV and 40 mA, with CuKα and λ = 1.546 Å. The XRD data were collected at room temperature in a 2θ range from 10° to 70° with steps of 0.02°. The main Raman vibrational modes of the zinc manganite were obtained using a Thermo Scientific DXR confocal Raman microscope (λ = 633 nm). The Raman spectrum was recorded from 100 to 800 cm−1 at room temperature, using an exposure time of 60 s and a laser power of 5 mW. The absorbance was measured with a Shimadzu UV3600 spectrophotometer in the range 200–800 nm. The ZnMn2O4 nanoparticles were analyzed by TEM and high-resolution transmission electron microscopy (HRTEM) using a FEI Tecnai-F30 system operated at an acceleration voltage of 300 kV.

2.3. Gas Sensitivity Tests

Pellet-type sensors based on ZnMn2O4 nanoparticles were used for the detection of C3H8 and CO. For the fabrication of the pellets, with a thickness of ~100 µm and a diameter of 12 mm, the ZnMn2O4 powder calcined at 500 °C was compacted with a uniaxial force of 10 tons for 5 min using a manual pressure machine (Simplex Ital Equip). The pellet was placed in a vacuum chamber at a vacuum level of 10−3 torr, partial pressure and gas concentration within the chamber were controlled using a TM20 Leybold detector. The electrical resistance of the ZnMn2O4 sensor exposed to the gases was measured using a digital multimeter (Keithley 2001, Cleveland, OH, USA). A gas sensing system such as the one shown in Figure 2 was used. The sensor response has been usually defined as β = Ra/Rg for reducing gases, where Ra is the resistance in the air and Rg is the resistance in the sampled gas [46,47,48].

Figure 2.

Figure 2

Open in a new tab

Schematic of the system used for gas sensitivity measurements.

3. Results and Discussion

3.1. Thermogravimetric Analysis

Figure 3 shows a typical TGA curve obtained from the precursor material. The weight loss of 1.5% observed in the range of 51 to 156 °C could be due to the evaporation of physically absorbed water molecules. The following 14.6% weight loss, from 156 to 310 °C, is attributed to the thermal decomposition of dodecylamine molecules existing in the dried precursor. Finally, the small weight loss observed from 310 to 800 °C is probably due to the complete desorption of nitrate ions [49]. Based on this analysis, a temperature of 500 °C was chosen for the calcination treatment of the sample to ensure complete crystallization.

Figure 3.

Figure 3

Open in a new tab

TGA curve of the precursor powder of ZnMn2O4.

3.2. XRD Results

Figure 4 shows the crystallinity evolution of the ZnMn2O4 powder samples calcined at temperatures from 300 to 600 °C. For the samples annealed at 300 and 400 °C, the main peaks corresponding to ZnMn2O4 were identified using the JCPDF file No. 24-1133; at 500 and 600 °C, a small peak located at 36.9° completely proved the formation of the ZnMn2O4 spinel structure. An additional feature of the diffractograms at these temperatures was the well-defined narrow peaks that were observed, indicating the high crystallinity of these zinc manganite samples. The crystallite size of the sample calcined at 500 °C was calculated from the most intense peak located at 36.4° using Scherrer´s equation [50], giving a value of 26.6 nm.

Figure 4.

Figure 4

Open in a new tab

XRD patterns of the ZnMn2O4 precursor powder after calcination at different temperatures.

3.3. Raman Spectroscopy

Raman spectra of the ZnMn2O4 powders calcined at 500 and 600 °C are shown in Figure 5. According to group theory, ten Raman active modes (2A1g + 3B1g + 1B2g + 4Eg) are expected for the tetragonal spinel structure of AMn2O4 (A = Zn, Mg, Mn), with a space group of I41/amd [51,52]. The Raman spectrum of the powder treated at 500 °C exhibited five Raman vibrational modes, which are the typical modes of the zinc manganite [53,54,55]. It was interesting that eight of the 10 allowed modes were observed for the sample calcined at 600 °C. In this spectrum, a small increase of the intensity and a slight shift of the vibrational modes were observed in contrast with the ones from the spectrum of the sample calcined at 500 °C. The differences between these spectra could be explained by the crystallinity of the ZnMn2O4 samples, as was confirmed by XRD. According to the literature, it was assumed that modes above 600 cm−1 were due to the oxygen motion in the tetrahedral AO4 sites, and the low-frequency modes by the octahedral BO6 sites [56]; however, this assumption requires further study.

Figure 5.

Figure 5

Open in a new tab

Raman spectra of the ZnMn2O4 powder calcined at 500 and 600 °C.

3.4. UV-Vis Analysis

The optical-absorbance spectrum of the ZnMn2O4 powder calcined at 500 °C is shown in Figure 6. The ZnMn2O4 exhibited an absorption band between the 250 and 600 nm. This absorption behavior is characteristic of the ZnMn2O4 spinel and is in agreement with previous reports [57,58,59]. In order to calculate the band gap energy, Tauc´s formula was used [60,61]. The bang gap energy was determined by extrapolating the linear part of the graph of (αhv)n versus hv up to energy axis at α = 0, where α is the optical absorption coefficient, and n = ½ for indirect transitions and = 2 for direct transitions (see inset of Figure 6). The band gap for the ZnMn2O4 was of 1.58 eV, considering a direct transition.

Figure 6.

Figure 6

Open in a new tab

UV-vis spectrum of ZnMn2O4 nanoparticles.

3.5. TEM Analysis

Figure 7a,b show TEM and HRTEM images of the zinc manganite powder calcined at 500 °C. The TEM image confirmed the presence of nanoparticles with different size and irregular shapes (Figure 7a). HRTEM further revealed that the nanoparticles were of crystalline nature with an inter-planar d-spacing of 4.87 Å, corresponding to the (101) plane of the ZnMn2O4 spinel structure (Figure 7b). Figure 7c shows the particle size distribution of the ZnMn2O4 nanoparticles. The particles were in the range from 10 to 70 nm, with a representative particle size of ~41 nm and a standard deviation of ±13.1 nm. Concerning to the formation mechanism of the nanoparticles, it is known that in colloidal media, nanoparticles are formed by a mechanism of nucleation and growth [62,63]. The formation of ZnMn2O4 nanoparticles should be produced through these mechanisms, where the nucleation could occur when the manganese nitrate solution was added to the zinc–dodecylamine solution and the particle growth during the agitation of the solution [44]. The dodecylamine also plays an important role in the size and morphology formation of inorganic materials [44,46].

Figure 7.

Figure 7

Open in a new tab

(a) TEM and (b) HRTEM images of ZnMn2O4 nanoparticles; (c) particle size distribution for the zinc manganite.

3.6. Gas Sensing Performance

In order to know the capacity of ZnMn2O4 for its possible application as a gas sensor, the oxide was studied in C3H8 and CO atmospheres. Figure 8 shows the results obtained in propane atmospheres at different concentrations (1–500 ppm) and operating temperatures (100, 200, and 300 °C).

Figure 8.

Figure 8

Open in a new tab

Sensing response of the ZnMn2O4 nanoparticles as a function of (a) C3H8 concentration and (b) operation temperature.

According to these results, the pellets of ZnMn2O4 are clearly sensitive to C3H8 at the given temperature. As expected, the response of the material also increases as the temperature and concentration of propane increase. The good response of the oxide is due to the increase in the number of molecules of the gas that react with the oxygen present on the surface of the pellets. In addition, due to the effect of temperature (when it is increased), there are changes in the electrical resistance [12], causing an increase in the response of the material. Several authors have reported that temperature plays a key role in increasing the efficiency of a material like the one used in this work [9,10,11,12]. In particular, at 100 °C, the oxide showed a poor response: 1.19 at 500 ppm. In contrast, at 200 °C, a slight increase was obtained: 1.88 at the same concentration of propane (see Figure 8a,b). The low response at 100 and 200 °C is due to the fact that the thermal energy is not enough to produce the oxygen desorption reaction [10,17], causing no significant changes in the electrical resistance of the material during the detection test. In contrast, upon increasing the temperature to 300 °C, the response of the pellets increased considerably to 4.23 at 500 ppm of C3H8 (see Figure 8a). The good response obtained at this temperature is attributed to the fact that during the adsorption of propane, it subsequently reacts with the oxygen present on the surface of the material [9,10], inducing a high interaction between the gas and the surface of the zinc manganite pellets. The mechanism that involves detection in propane atmospheres has not been fully studied. However, it has been suggested in the literature that C3H8 molecules react with chemisorbed O− species, producing CO2, water vapor, and an electron release to the material’s surface [64], causing the changes in the material’s electrical resistance shown in Figure 8a,b. Other authors have studied the chemical interaction between the surface of a material and the molecules of the C3H8, suggesting some chemical processes that involve the adsorption–desorption of propane, and obtaining results such as those presented in this work [11,65,66].

Similar trends were obtained when the pellets of ZnMn2O4 were exposed to atmospheres of CO at different concentrations (1–300 ppm) and working temperatures (100, 200, and 300 °C). The results obtained are shown in Figure 9a,b.

Figure 9.

Figure 9

Open in a new tab

Response of the ZnMn2O4 sensor as a function of: (a) CO concentration and (b) working temperature.

As was the case in propane atmospheres, the zinc manganite pellets showed changes in electrical resistance when the CO molecules contacted the surface of the material. The increase in response to this atmosphere clearly depends on the increase in operating temperature and the concentration of CO. It is known that when a semiconductor metal oxide, like the ZnMn2O4, is exposed to a gas at a moderate temperature, its electrical resistance is altered due to the reaction of the gas with pre-adsorbed oxygen species [67]. Hence, when performing the tests at 100, 200, and 300 °C, the adsorbed CO reacts with the oxygen present, as a result of temperature, causing an increase in the sensitivity of the material. Therefore, the response obtained in CO was estimated at 1.13 and 1.25 for 300 ppm of CO at temperatures of 100 and 200 °C, respectively (see Figure 9a,b). The maximum response in CO was of 1.55, which corresponds to a concentration of 300 ppm of CO at a temperature of 300 °C (see Figure 9a). Recently, it has been reported in the literature that the increase in the response of a material such as the one used in this work is associated with the increase of oxygen desorption at elevated temperatures [11,12,65]. According to Barsan and Weimar [68], the nature of the adsorbed oxygen species on a semiconductor gas sensor depends on the working temperature: Below 150 °C, the molecular O2− species are present; above 150 °C, the ionic O− and O2− species are found. In addition, it is known that the formation of ionic species at high temperatures increases the gas–solid interaction because of the higher reactivity of these species; therefore, the gas response is improved [10,11,17], as happened in this work (see Figure 9).

Considering our results, the zinc manganite was sensitive, as expected, to both changes in C3H8 and CO concentrations, and operation temperatures. In fact, the high sensitivity of the ZnMn2O4 sensor was mainly due to the nanometric particle size, since the surface-to-volume ratio of the nano-sized semiconductor is very high; therefore, more active sites increase the sensor response [1,2,18]. In particular, our propane sensitivity results were compared with similar metal oxides, showing that we have succeeded in obtaining a better response. For example, the SnO2 and undoped ZnO thin films exhibited a maximum sensitivity of 0.7 and 2.3, respectively; both sensitivities were measured at 300 °C in 300 ppm of C3H8 [69,70]. The oxide ZnSb2O6 showed a maximum sensitivity of 1.2 in 300 ppm of C3H8 at 250 °C [71].

4. Conclusions

Zinc manganite nanoparticles were successfully synthesized via a microwave-assisted colloidal route. This simple and economical synthesis process can be extended for the synthesis of nanoparticles of many other simple and complex compounds. Single-phase ZnMn2O4 was found at 500 °C with an optical band-gap energy of 1.58 eV. Eight Raman vibrational modes were registered from zinc manganite. ZnMn2O4 nanoparticles with an average particle size of 41 nm were obtained. Test sensors based on these nanoparticles exhibited a good response to C3H8 and CO at an operating temperature of 300 °C. Based on the results of this work, the ZnMn2O4 nanoparticles can be considered a promising new material for the sensing of relatively low concentrations of propane.

Acknowledgments

E.S. Guillen-López is grateful to the National Council of Science and Technology of Mexico (CONACYT) for his M.Sc. scholarship. The authors are grateful to LINAN-IPICYT for the TEM and SEM analysis. The authors also acknowledge the support from PRODEP (project No. 511-6/17-7354, Fortalecimiento de Cuerpos Académicos Convocatoria 2017) and the Maestría en Ciencias Físico Matemáticas (CUValles). Thanks are owed to Mtro. Sergio Oliva for the XRD measurements.

Author Contributions

J.P.M.-L. and E.S.G.-L. conceived and designed the experiments; E.S.G.-L., H.G.-B. and M.L.O.-A. performed the experiments; F.L.-U. and E.M.-S. analyzed the data; O.B.-A. and V.M.R.-B. contributed reagents/materials/analysis tools; J.P.M.-L. and M.S.-T. wrote the paper, and A.G.-B. surveyed related works.

Conflicts of Interest

The authors declare no conflict of interest.

References

  • 1.Yamazoe N. New approaches for improving semiconductor gas sensors. Sens. Actuators B Chem. 1991;5:7–19. doi: 10.1016/0925-4005(91)80213-4. [DOI] [Google Scholar]
  • 2.Xu C., Tamaki J., Miura N., Yamazoe N. Grain size effects on gas sensitivity of porous SnO2-based elements. Sens. Actuators B Chem. 1991;3:147–155. doi: 10.1016/0925-4005(91)80207-Z. [DOI] [Google Scholar]
  • 3.Kolmakov A., Klenov D.O., Lilach Y., Stemmer S., Moskovits M. Enhanced gas sensing by individual SnO2 nanowires and nanobelts functionalized with Pd catalyst particles. Nano Lett. 2005;5:667–673. doi: 10.1021/nl050082v. [DOI] [PubMed] [Google Scholar]
  • 4.Kolmakov A., Zhang Y., Cheng G., Moskovits M. Detection of CO and O2 using tin oxide nanowire sensors. Adv. Mater. 2003;15:997–1000. doi: 10.1002/adma.200304889. [DOI] [Google Scholar]
  • 5.Ahn M.-W., Park K.-S., Heo J.-H., Park J.-G., Kim D.-W., Choi K.J., Lee J.-H., Hong S.-H. Gas sensing properties of defect-controlled ZnO-nanowire gas sensor. Appl. Phys. Lett. 2009;93:263103. doi: 10.1063/1.3046726. [DOI] [Google Scholar]
  • 6.Shishiyanu S.T., Shishiyanu T.S., Lupan O.I. Sensing characteristics of tin-doped ZnO thin films as NO2 gas sensor. Sens. Actuators B Chem. 2005;107:379–386. doi: 10.1016/j.snb.2004.10.030. [DOI] [Google Scholar]
  • 7.Tang H., Prasad K., Sanjinés R., Lévy F. TiO2 anatase thin films as gas sensors. Sens. Actuators B Chem. 1995;26:71–75. doi: 10.1016/0925-4005(94)01559-Z. [DOI] [Google Scholar]
  • 8.Kim H.-J., Lee J.-H. Highly sensitive and selective gas sensors using p-type oxide semiconductors: Overview. Sens. Actuators B Chem. 2014;192:607–627. doi: 10.1016/j.snb.2013.11.005. [DOI] [Google Scholar]
  • 9.Rodríguez Betancourtt V.-M., Guillén Bonilla H., Flores Martínez M., Guillén Bonilla A., Moran Lazaro J.P., Guillen Bonilla J.T., González M.A., Olvera Amador M.d.l.L. Gas sensing properties of NiSb2O6 micro- and nanoparticles in propane and carbon monoxide atmospheres. J. Nanomater. 2017;2017:1–9. doi: 10.1155/2017/8792567. [DOI] [Google Scholar]
  • 10.Guillén-Bonilla A., Rodríguez-Betancourtt V.M., Guillén-Bonilla J.T., Sánchez-Martínez A., Gildo-Ortiz L., Santoyo-Salazar J., Morán-Lázaro J.P., Guillén-Bonilla H., Blanco-Alonso O. A novel CO and C3H8 sensor made of CuSb2O6 nanoparticles. Ceram. Int. 2017;43:13635–13644. doi: 10.1016/j.ceramint.2017.07.073. [DOI] [Google Scholar]
  • 11.Guillén-Bonilla H., Flores-Martínez M., Rodríguez-Betancourtt V.M., Guillén-Bonilla A., Reyes-Gómez J., Gildo-Ortiz L., Olvera-Amador M.L., Santoyo-Salazar J. A novel gas sensor based on MgSb2O6 nanorods to indicate variations in carbon monoxide and propane concentrations. Sensors. 2016;16:177. doi: 10.3390/s16020177. [DOI] [PMC free article] [PubMed] [Google Scholar]
  • 12.Gildo-Ortiz L., Guillén-Bonilla H., Santoyo-Salazar J., Olvera M.L., Karthik T.V.K., Campos-González E., Reyes-Gómez J. Low-temperature synthesis and gas sensitivity of perovskite-type LaCoO3 nanoparticles. J. Nanomater. 2014;2014:1–8. doi: 10.1155/2014/164380. [DOI] [Google Scholar]
  • 13.Niu X., Du W., Du W. Preparation and gas sensing properties of ZnM2O4 (M = Fe, Co, Cr) Sens. Actuators B Chem. 2004;99:405–409. doi: 10.1016/j.snb.2003.12.007. [DOI] [Google Scholar]
  • 14.Wang Z., Liu X., Lv M., Chai P., Liu Y., Meng J. Preparation of ferrite MFe2O4 (M = Co, Ni) ribbons with nanoporous structure and their magnetic properties. J. Phys. Chem. B. 2008;112:11292–11297. doi: 10.1021/jp804178w. [DOI] [PubMed] [Google Scholar]
  • 15.Yamazoe N. Toward innovations of gas sensor technology. Sens. Actuators B Chem. 2005;108:2–14. doi: 10.1016/j.snb.2004.12.075. [DOI] [Google Scholar]
  • 16.Lingmin Y., Xinhui F., Lijun Q., Lihe M., Wen Y. Dependence of morphologies for SnO2 nanostructures on their sensing property. Appl. Surf. Sci. 2011;257:3140–3144. doi: 10.1016/j.apsusc.2010.11.013. [DOI] [Google Scholar]
  • 17.Gildo-Ortiz L., Reyes-Gómez J., Flores-Álvarez J.M., Guillén-Bonilla H., Olvera M.d.l.L., Betancourtt V.R., Verde-Gómez Y., Guillén-Cervantes A., Santoyo-Salazar J. Synthesis, characterization and sensitivity tests of perovskite-type LaFeO3 nanoparticles in CO and propane atmospheres. Ceram. Int. 2016;42:18821–18827. doi: 10.1016/j.ceramint.2016.09.027. [DOI] [Google Scholar]
  • 18.Yamazoe N., Sakai G., Shimanoe K. Oxide semiconductor gas sensors. Catal. Surv. Asia. 2003;7:63–75. doi: 10.1023/A:1023436725457. [DOI] [Google Scholar]
  • 19.Zhang G., Yu L., Wu H.B., Hoster H.E., Lou X.W. Formation of ZnMn2O4 ball-in-ball hollow microspheres as a high-performance anode for lithium-ion batteries. Adv. Mater. 2012;24:4609–4613. doi: 10.1002/adma.201201779. [DOI] [PubMed] [Google Scholar]
  • 20.Courtel F.M., Duncan H., Abu-Lebdeh Y., Davidson I.J. High capacity anode materials for Li-ion batteries based on spinel metal oxides AMn2O4 (A = Co, Ni, and Zn) J. Mater. Chem. 2011;21:10206–10218. doi: 10.1039/c0jm04465b. [DOI] [Google Scholar]
  • 21.Zhou L., Wu H.B., Zhu T., Lou X.W. Facile preparation of ZnMn2O4 hollow microspheres as high-capacity anodes for lithium-ion batteries. J. Mater. Chem. 2012;22:827–829. doi: 10.1039/C1JM15054E. [DOI] [Google Scholar]
  • 22.Xiao L., Yang Y., Yin J., Li Q., Zhang L. Low temperature synthesis of flower-like ZnMn2O4 superstructures with enhanced electrochemical lithium storage. J. Power Sources. 2009;194:1089–1093. doi: 10.1016/j.jpowsour.2009.06.043. [DOI] [Google Scholar]
  • 23.Yang Y., Zhao Y., Xiao L., Zhang L. Nanocrystalline ZnMn2O4 as a novel lithium-storage material. Electrochem. Commun. 2008;10:1117–1120. doi: 10.1016/j.elecom.2008.05.026. [DOI] [Google Scholar]
  • 24.Bai Z., Fan N., Sun C., Ju Z., Guo C., Yang J., Qian Y. Facile synthesis of loaf-like ZnMn2O4 nanorods and their excellent performance in Li-ion batteries. Nanoscale. 2013;5:2442–2447. doi: 10.1039/c3nr33211j. [DOI] [PubMed] [Google Scholar]
  • 25.Sahoo A., Sharma Y. Synthesis and characterization of nanostructured ternary zinc manganese oxide as novel supercapacitor material. Mater. Chem. Phys. 2015;149:721–727. doi: 10.1016/j.matchemphys.2014.11.032. [DOI] [Google Scholar]
  • 26.Huang T., Zhao C., Qiu Z., Luo J., Hu Z. Hierarchical porous ZnMn2O4 synthesized by the sucrose-assisted combustion method for high-rate supercapacitors. Ionics. 2017;23:139–146. doi: 10.1007/s11581-016-1817-8. [DOI] [Google Scholar]
  • 27.Guo N., Wei X.Q., Deng X.L., Xu X.J. Synthesis and property of spinel porous ZnMn2O4 microspheres. Appl. Surf. Sci. 2015;356:1127–1134. doi: 10.1016/j.apsusc.2015.08.185. [DOI] [Google Scholar]
  • 28.Gao Y., Zheng M., Pang H. Achieving high-performance supercapacitors by constructing porous zinc-manganese oxide microstructures. Energy Technol. 2015;3:820–824. doi: 10.1002/ente.201500067. [DOI] [Google Scholar]
  • 29.Guan Y., Feng Y., Mu Y., Fang L., Zhang H., Wang Y. Ultra-tiny ZnMn2O4 nanoparticles encapsulated in sandwich-like carbon nanosheets for high-performance supercapacitors. Nanotechnology. 2016;27:1–11. doi: 10.1088/0957-4484/27/47/475402. [DOI] [PubMed] [Google Scholar]
  • 30.Guillemet-Fritsch S., Chanel C., Sarrias J., Bayonne S., Rousset A., Alcobe X., Martinez Sarriòn M.L. Structure, thermal stability and electrical properties of zinc manganites. Solid State Ionics. 2000;128:233–242. doi: 10.1016/S0167-2738(99)00340-9. [DOI] [Google Scholar]
  • 31.Talebi R. Simple synthesis and characterization of zinc manganite nanoparticles: Investigation of surfactants effect and its photocatalyst application. J. Mater. Sci.: Mater. Electron. 2017;28:3774–3779. doi: 10.1007/s10854-016-5987-y. [DOI] [Google Scholar]
  • 32.Deraz N.M., Abdeltawab A.A., Selim M.M., El-Shafey O., El-Asmy A.A., Al-Deyab S.S. Precipitation–deposition assisted fabrication and characterization of nano-sized zinc manganite. J. Ind. Eng. Chem. 2014;20:2901–2904. doi: 10.1016/j.jiec.2013.11.026. [DOI] [Google Scholar]
  • 33.Juibari N.M., Eslami A. Investigation of catalytic activity of ZnAl2O4 and ZnMn2O4 nanoparticles in the thermal decomposition of ammonium perchlorate. Therm. Anal. Calorim. 2017;128:115–124. doi: 10.1007/s10973-016-5906-8. [DOI] [Google Scholar]
  • 34.Bessekhouad Y., Robert D., Weber J.-V. Photocatalytic activity of Cu2O/TiO2, Bi2O3/TiO2 and ZnMn2O4/TiO2 heterojunctions. Catal. Today. 2005;101:315–321. doi: 10.1016/j.cattod.2005.03.038. [DOI] [Google Scholar]
  • 35.Bessekhouad Y., Trari M. Photocatalytic hydrogen production from suspension of spinel powders AMn2O4 (A = Cu and Zn) Int. J. Hydrogen Energy. 2002;27:357–362. doi: 10.1016/S0360-3199(01)00159-8. [DOI] [Google Scholar]
  • 36.Nassar M.Y., El-Moety E.A., El-Shahat M.F. Synthesis and characterization of a ZnMn2O4 nanostructure as a chemical nanosensor: A facile and new approach for colorimetric determination of omeprazole and lansoprazole drugs. RSC Adv. 2017;7:43798–43811. doi: 10.1039/C7RA08010G. [DOI] [Google Scholar]
  • 37.Sorita R., Kawano T. A highly selective CO sensor: Screening of electrode materials. Sens. Actuators B Chem. 1996;36:274–277. doi: 10.1016/S0925-4005(97)80081-0. [DOI] [Google Scholar]
  • 38.Na C.W., Park S.-Y., Chung J.-H., Lee J.-H. Transformation of ZnO Nanobelts into single-crystalline Mn3O4 nanowires. ACS Appl. Mater. Interfaces. 2012;4:6565–6572. doi: 10.1021/am301670x. [DOI] [PubMed] [Google Scholar]
  • 39.Panmatarith T., Innoi S. Vapour sensing characteristics of ZnO-ZnMn2O4 ceramics using the visual basic-based measurement system. Suranaree J. Sci. Technol. 2009;16:235–243. [Google Scholar]
  • 40.Courtel F.M., Abu-Lebdeh Y., Davidson I.J. ZnMn2O4 nanoparticles synthesized by a hydrothermal method as an anode material for Li-ion batteries. Electrochim. Acta. 2012;71:123–127. doi: 10.1016/j.electacta.2012.03.108. [DOI] [Google Scholar]
  • 41.Song M.S., Cho Y.J., Yoon D.Y., Nahm S., Oh S.H., Woo K., Ko J.M., Cho W.I. Solvothermal synthesis of ZnMn2O4 as an anode material in lithium ion battery. Electrochim. Acta. 2014;137:266–272. doi: 10.1016/j.electacta.2014.05.126. [DOI] [Google Scholar]
  • 42.Brahma S., Liu C.-P., Shivashankar S.A. Microwave irradiation assisted, one pot synthesis of simple and complex metal oxide nanoparticles: A general approach. J. Phys. D: Appl. Phys. 2017;50:1–5. doi: 10.1088/1361-6463/aa82e2. [DOI] [Google Scholar]
  • 43.Morán-Lázaro J.P., Blanco O., Rodríguez-Betancourtt V.M., Reyes-Gómez J., Michel C.R. Enhanced CO2-sensing response of nanostructured cobalt aluminate synthesized using a microwave-assisted colloidal method. Sens. Actuators B Chem. 2016;226:518–524. doi: 10.1016/j.snb.2015.12.013. [DOI] [Google Scholar]
  • 44.Blanco O., Morán-Lázaro J.P., Rodríguez-Betancourtt V.M., Reyes-Gómez J., Barrera A. Colloidal synthesis of CoAl2O4 nanoparticles using dodecylamine and their structural characterization. Superficies y Vacío. 2016;29:78–82. [Google Scholar]
  • 45.Mirzaei A., Neri G. Microwave-assisted synthesis of metal oxide nanostructures for gas sensing application: A review. Sens. Actuators B Chem. 2016;237:749–775. doi: 10.1016/j.snb.2016.06.114. [DOI] [Google Scholar]
  • 46.Morán-Lázaro J.P., López-Urías F., Muñoz-Sandoval E., Blanco-Alonso O., Sanchez-Tizapa M., Carreon-Alvarez A., Guillén-Bonilla H., Olvera-Amador M.d.l.L., Guillén-Bonilla A., Rodríguez-Betancourtt V.M. Synthesis, characterization, and sensor applications of spinel ZnCo2O4 nanoparticles. Sensors. 2016;16:2162. doi: 10.3390/s16122162. [DOI] [PMC free article] [PubMed] [Google Scholar]
  • 47.Wang C., Yin L., Zhang L., Xiang D., Gao R. Metal oxide gas sensors: Sensitivity and influencing factors. Sensors. 2010;10:2088–2106. doi: 10.3390/s100302088. [DOI] [PMC free article] [PubMed] [Google Scholar]
  • 48.Qu F., Jiang H., Yang M. Designed formation through a metal organic framework route of ZnO/ZnCo2O4 hollow core–shell nanocages with enhanced gas sensing properties. Nanoscale. 2016;8:16349–16356. doi: 10.1039/C6NR05187A. [DOI] [PubMed] [Google Scholar]
  • 49.Zhou X., Feng W., Wang C., Hu X., Li X., Sun P., Shimanoe K., Yamazoe N., Lu G. Porous ZnO/ZnCo2O4 hollow spheres: Synthesis, characterization, and applications in gas sensing. J. Mater. Chem. 2014;2:17683–17690. doi: 10.1039/C4TA04386C. [DOI] [Google Scholar]
  • 50.Xiong H., Zhang Y., Liew K., Li J. Catalytic performance of zirconium-modified Co/Al2O3 for Fischer–Tropsch synthesis. J. Mol. Catal. A: Chem. 2005;231:145–151. doi: 10.1016/j.molcata.2004.12.033. [DOI] [Google Scholar]
  • 51.Malavasi L., Galinetto P., Mozzati M.C., Azzoni C.B., Flor G. Raman spectroscopy of AMn2O4 (A = Mn, Mg and Zn) spinels. Phys. Chem. Chem. Phys. 2002;4:3876–3880. doi: 10.1039/b203520k. [DOI] [Google Scholar]
  • 52.Tortosa M., Manjón F.J., Mollar M., Marí B. ZnO-based spinels grown by electrodeposition. J. Phys. Chem. Solids. 2012;73:1111–1115. doi: 10.1016/j.jpcs.2012.04.002. [DOI] [Google Scholar]
  • 53.Samanta K., Dussan S., Katiyar R.S., Bhattacharya P. Structural and optical properties of nanocrystalline Zn1−xMnxO. Appl. Phys. Lett. 2007;90:261903. doi: 10.1063/1.2751593. [DOI] [Google Scholar]
  • 54.Li H., Song B., Wang W.J., Chen X.L. Facile synthesis, thermal, magnetic, Raman characterizations of spinel structure ZnMn2O4. Mater. Chem. Phys. 2011;130:39–44. doi: 10.1016/j.matchemphys.2011.04.072. [DOI] [Google Scholar]
  • 55.Hadzic B., Romcevic N., Romcevic M., Kuryliszyn-Kudelska I., Dobrowolski W., Wróbel R., Narkiewicz U., Sibera D. Raman study of surface optical phonons in ZnO(Mn) nanoparticles. J. Alloy. Compd. 2014;585:214–219. doi: 10.1016/j.jallcom.2013.09.132. [DOI] [Google Scholar]
  • 56.Zhang T., Yue H., Qiu H., Zhu K., Zhang L., Wei Y., Du F., Chen G., Zhang D. Synthesis of graphene-wrapped ZnMn2O4 hollow microspheres as high performance anode materials for lithium ion batteries. RSC Adv. 2015;5:99107–99114. doi: 10.1039/C5RA16667E. [DOI] [Google Scholar]
  • 57.Zhang P., Li X., Zhao Q., Liu S. Synthesis and optical property of one dimensional spinel ZnMn2O4 nanorods. Nanoscale Res. Lett. 2011;6:1–8. doi: 10.1186/1556-276X-6-323. [DOI] [PMC free article] [PubMed] [Google Scholar]
  • 58.Javed Q., Wang F., Toufiq A.M., Rafiq M.Y., Iqbal M.Z., Kamran M.A. Preparation, characterizations and optical property of single crystalline ZnMn2O4 nanoflowers via template-free hydrothermal synthesis. J. Nanosci. Nanotechnol. 2013;13:2937–2942. doi: 10.1166/jnn.2013.7389. [DOI] [PubMed] [Google Scholar]
  • 59.Zhao L., Li X., Zhao J. Fabrication, characterization and photocatalytic activity of cubic-like ZnMn2O4. Appl. Surf. Sci. 2013;268:274–277. doi: 10.1016/j.apsusc.2012.12.078. [DOI] [Google Scholar]
  • 60.Misho R.H., Murad W.A. Band gap measurements in thin films of hematite Fe2O3, pyrite FeS2 and troilite FeS prepared by chemical spray pyrolysis. Sol. Energy Mater. Sol. Cells. 1992;27:335–345. doi: 10.1016/0927-0248(92)90095-7. [DOI] [Google Scholar]
  • 61.Rani S., Sanghi S., Agarwal A., Seth V.P. Study of optical band gap and FTIR spectroscopy of Li2O·Bi2O3·P2O5 glasses. Spectrochim. Acta A. 2009;74:673–677. doi: 10.1016/j.saa.2009.07.023. [DOI] [PubMed] [Google Scholar]
  • 62.LaMer V.K., Dinegar R.H. Theory, production and mechanism of formation of monodispersed hydrosols. J. Am. Chem. Soc. 1950;72:4847–4854. doi: 10.1021/ja01167a001. [DOI] [Google Scholar]
  • 63.Vekilov P.G. What determines the rate of growth of crystals from solution? Cryst. Growth Des. 2007;7:2796–2810. doi: 10.1021/cg070427i. [DOI] [Google Scholar]
  • 64.Gildo-Ortiz L., Guillén-Bonilla H., Reyes-Gómez J., Rodríguez-Betancourtt V.M., Olvera-Amador M.d.l.L., Eguía-Eguía S.I., Guillén-Bonilla A., Santoyo-Salazar J. Facile synthesis, microstructure, and gas sensing properties of NdCoO3 nanoparticles. J. Nanomater. 2017;2017:1–10. doi: 10.1155/2017/8174987. [DOI] [Google Scholar]
  • 65.Kerlau M., Reichel P., Bârsan N., Weimar U., Delsarte-Guéguen S., Merdrignac-Conanec O. Detection of propane by “GaON” thick-film gas sensors. Sens. Actuators B Chem. 2007;122:14–19. doi: 10.1016/j.snb.2006.05.001. [DOI] [Google Scholar]
  • 66.Bahrami B., Khodadadi A., Kazemeini M., Mortazavi Y. Enhanced CO sensitivity and selectivity of gold nanoparticles-doped SnO2 sensor in presence of propane and methane. Sens. Actuators B Chem. 2008;133:352–356. doi: 10.1016/j.snb.2008.02.034. [DOI] [Google Scholar]
  • 67.Barsan N., Simion C., Heine T., Pokhrel S., Weimar U. Modeling of sensing and transduction for p-type semiconducting metal oxide based gas sensors. J. Electroceram. 2010;25:11–19. doi: 10.1007/s10832-009-9583-x. [DOI] [Google Scholar]
  • 68.Barsan N., Wiemar U. Conduction model of metal oxide gas sensors. J. Electroceram. 2001;7:143–167. doi: 10.1023/A:1014405811371. [DOI] [Google Scholar]
  • 69.Gómez-Pozos H., González-Vidal J.L., Alberto-Torres G., Olvera M.L., Castañeda L. Physical characterization and effect of effective surface area on the sensing properties of tin dioxide thin solid films in a propane atmosphere. Sensors. 2014;14:403–415. doi: 10.3390/s140100403. [DOI] [PMC free article] [PubMed] [Google Scholar]
  • 70.Gómez-Pozos H., González-Vidal J.L., Torres G.A., Rodríguez-Baez J., Maldonado A., Olvera M.L., Acosta D.R., Avendaño-Alejo M., Castañeda L. Chromium and ruthenium-doped zinc oxide thin films for propane sensing applications. Sensors. 2013;13:3432–3444. doi: 10.3390/s130303432. [DOI] [PMC free article] [PubMed] [Google Scholar]
  • 71.Guillen-Bonilla H., Rodríguez-Betancourtt V.M., Guillén-Bonilla J.T., Reyes-Gómez J., Gildo-Ortiz L., Flores-Martínez M., Olvera-Amador M.L., Santoyo-Salazar J. CO and C3H8 sensitivity behavior of zinc antimonate prepared by a microwave-assisted solution method. J. Nanomater. 2015;16:450. [Google Scholar]

Articles from Sensors (Basel, Switzerland) are provided here courtesy of Multidisciplinary Digital Publishing Institute (MDPI)

RESOURCES