# Synthesis and Characterization of PVA-Assisted Metal Oxide Nanomaterials: Surface Area, Porosity, and Electrochemical Property Improvement

Authors: Buzuayehu Abebe; H. C. Ananda Murthy; Enyew Amare Zereffa
Journal: Journal of Nanomaterials
 (2020)

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## Abstract

The poly(vinyl alcohol)-assisted sol-gel-self-propagation route has been used for the synthesis of porous binary metal oxide nanocomposites (BMONCs) and ternary metal oxide nanocomposites (TMONCs). The effects of synthesis techniques, precursor’s type, amount of PVA loading, and precursor’s percentage were studied. The optical, chemical bonding, crystallinity, morphological, textural, and electrochemical properties of the synthesized materials were characterized by UV-vis-DRS/UV-vis, FT-IR, XRD, SEM/EDX and TEM/HRTEM/SAED, BET, and CV/EIS techniques, respectively. The porous nature of the materials was confirmed by SEM, BET, and SAED analytical techniques. Using XRD and TEM analysis, the approximate particle size of the materials was confirmed to be in the nanometer range (~7-70 nm). The EDX and HRTEM analysis was confirming the presence of predictable composition and actuality of the composites, respectively. Moving from bare ZnO to ternary nanocomposites, the great morphological, surface area, and electrochemical property enhancement was confirmed. The charge transfer capability order was obtained to be ZnO/Fe2O3/Mn2O3 > ZnO/Fe2O3 > ZnO/Mn2O3 > ZnO. The respective approximate electron transfer resistance value is 7, 25, 61, and 65 Ω. Therefore, this work can improve the toxicity towards solvent used, surface area to volume ratio, and aggregation/agglomeration problem and also enhance the charge transfer capability due to the heterojunction.


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## Body

## 1. Introduction

With the rapid development of industrial society, increasing environmental safety threats pose a major concern. Nowadays, metal oxides have been vigorously applied as an environmental waste management system [1]. Among several metal oxides, ZnO was reported to be less production cost, higher light absorption efficacy, and less toxic properties [2, 3]. However, the dissolution in acidic solution, photocorrosion in alkaline solution under UV irradiation [4], fast electron-hole recombination during the photocatalytic reaction, and agglomeration are the obvious drawbacks of ZnO [5]. Among several efficient efforts applied to reduce the mentioned drawbacks, developing ZnO-based heterojunction with different bandgap materials was obtained to be one of the preferences [6]. Depending on the magnetic property, stability, and high surface area to volume ratio property, iron and manganese oxides are reported to be promising materials [7–9].Iron oxide utilizes efficient absorption of visible light during the formation of heterojunction with ZnO photocatalyst. As reported [10, 11], it can absorb approximately 20% of the solar spectrum. Depending on the applied temperature, among different crystalline polymorphs of Fe2O3 Viz. hematite (α-Fe2O3), β-Fe2O3, maghemite (γ-Fe2O3), ε-Fe2O3, and ζ-Fe2O3, the α-Fe2O3 phase is the most stable and simple to be formed. The pathway for the formation of α-Fe2O3 follows γ-Fe2O3 → ε-Fe2O3 → α-Fe2O3 [12]. Among different crystalline polymorphs of manganese oxides, the Mn2O3 is cheap and environmentally safe [13]. Both in the amorphous and crystalline state, α-Mn2O3 uses a wide range of applications [14]. Manganese oxide also has low charge transfer resistance and multitudinous defect properties. In the nanosized range, α-Fe2O3 and α-Mn2O3 can enhance the adsorption capacity during heterojunction [15]. A significant surface area enhancement from single ZnO to ternary materials was also proven in the author’s earlier work [16]. In addition to single ZnO, this work compares additional two binary metal oxide composites with the ternary composite materials. Furthermore, the presence of good electrochemical improvement due to the formation of heterojunction was also proven.Among several bottom-up synthesis approaches, depending on the price, time, easiness, and harmfulness, the sol-gel and coprecipitation techniques are feasible [17, 18]. In advance, when being applied, toxic solvents, especially that are suggested under the severe human health risk phrase category of the Global Harmonized System (GHS) Hazard and Precautionary (H&P), are cancer-causing and also have mutagenic properties [19]. As reported [20], the nontoxic solvents like water can give equivalent morphology and crystalline size. Furthermore, due to high surface energy and large surface area, metal oxides can aggregate/agglomerate easily. Among different techniques used to avoid the aggregation/agglomeration of the NPs, the polymer matrix as a capping agent is one of the preferences [21]. Due to several properties, poly(vinyl alcohol) (PVA) polymer has been reported to be efficient [22]. As reported [23, 24], 500°C is the optimum temperature to remove unwanted impurities including the PVA polymer after acting as a capping agent.Therefore, considering all the mentioned aspects, this work was aimed at synthesizing single, BMONC, and TMONC materials using a simple and green sol-gel-self-propagation technique. The physical properties of the synthesized materials were characterized byUV-vis-diffuse reflectance spectroscopy (UV-vis-DRS), Fourier-transform infrared spectroscopy (FT-IR), X-ray powder diffraction (XRD), scanning electron microscopy/energy-dispersive X-ray spectroscopy (SEM/EDX) and transmission electron microscopy/high-resolution transmission electron microscopy/selected area electron diffraction (TEM/HRTEM/SAED), Brunauer-Emmett-Teller (BET), and cyclic voltammetry/electrical impedance spectroscopy (CV/EIS) analytical techniques. The techniques are confirming the presence of an enhanced surface area, porosity, and electrochemical improvement.


## 2. Material and Methods

### 2.1. Synthesis of Single, Binary, and Ternary Metal Oxides

The common analytical grade reagents and characterization technique details were present as supplementary materials (S). The single, binary, and ternary nanomaterials were synthesized following the sol-gel-self-propagation process. In detail, the PVA polymer was dissolved in distilled water while stirring on a magnetic stirrer at ~115°C for about 15 minutes [25]. After cooling at room temperature, the Zn, Mn, and Fe salt precursors (18 : 5 : 5 molar ratio, respectively) were added to form a 0.01 mol L−1 aqueous metal salt solution. The sol formed was aged for two days to form a gel and dried in an oven at 110°C. At the final drying process, the unintentional self-propagation process took place and a highly porous product was formed. The dried gel was grounded and calcined at 500°C for 3 hours. The detailed procedure is also reported on the author’s earlier works [16, 26] and shown in Figure S1. The same protocol was used for the synthesis of binary metal oxides by mixing two different metal salt precursors.To synthesize single (ZnO, Fe2O3, and Mn2O3), binary, and ternary metal oxides without PVA, except the first procedure used to dissolve the polymer, the same protocols were followed. However, due to the absence of the polymer, no self-propagation process occurred at the final drying period. Single ZnO was synthesized using a zinc nitrate salt precursor. The synthesized PVA-assisted BMONCs (PVA-BMONCs) were coded as PVA-BMO1 and PVA-BMO2 for Zn-Fe and Zn-Mn oxides, respectively. The respective BMONCs synthesized without PVA were coded as BMO1 and BMO2 (see Table S1 and S2). The synthesized TMONCs without PVA using the sol-gel (M1) and coprecipitation (M2) techniques were coded as TMOM1 and TMOM2, respectively, whereas the PVA-assisted TMONCs (PVA-TMONCs) using zinc nitrate (P1) and zinc acetate (P2) precursors were coded as PVA-TMOP1 and PVA-TMOP2, respectively (see Table S3).


## 2.1. Synthesis of Single, Binary, and Ternary Metal Oxides

The common analytical grade reagents and characterization technique details were present as supplementary materials (S). The single, binary, and ternary nanomaterials were synthesized following the sol-gel-self-propagation process. In detail, the PVA polymer was dissolved in distilled water while stirring on a magnetic stirrer at ~115°C for about 15 minutes [25]. After cooling at room temperature, the Zn, Mn, and Fe salt precursors (18 : 5 : 5 molar ratio, respectively) were added to form a 0.01 mol L−1 aqueous metal salt solution. The sol formed was aged for two days to form a gel and dried in an oven at 110°C. At the final drying process, the unintentional self-propagation process took place and a highly porous product was formed. The dried gel was grounded and calcined at 500°C for 3 hours. The detailed procedure is also reported on the author’s earlier works [16, 26] and shown in Figure S1. The same protocol was used for the synthesis of binary metal oxides by mixing two different metal salt precursors.To synthesize single (ZnO, Fe2O3, and Mn2O3), binary, and ternary metal oxides without PVA, except the first procedure used to dissolve the polymer, the same protocols were followed. However, due to the absence of the polymer, no self-propagation process occurred at the final drying period. Single ZnO was synthesized using a zinc nitrate salt precursor. The synthesized PVA-assisted BMONCs (PVA-BMONCs) were coded as PVA-BMO1 and PVA-BMO2 for Zn-Fe and Zn-Mn oxides, respectively. The respective BMONCs synthesized without PVA were coded as BMO1 and BMO2 (see Table S1 and S2). The synthesized TMONCs without PVA using the sol-gel (M1) and coprecipitation (M2) techniques were coded as TMOM1 and TMOM2, respectively, whereas the PVA-assisted TMONCs (PVA-TMONCs) using zinc nitrate (P1) and zinc acetate (P2) precursors were coded as PVA-TMOP1 and PVA-TMOP2, respectively (see Table S3).


## 3. Results and Discussion

### 3.1. XRD Analysis

The XRD diffraction pattern of the synthesized nanomaterials that confirms the crystallinity and composition of single, BMONC, and TMONC materials are shown in Figure1. All the diffraction angles with its corresponding crystal planes are corresponding to ZnO (ICSD: 00-036-1451, P63mc (#186-1) space group) (Figure 1). For single Fe2O3, the diffraction angles with its corresponding crystal planes are consistent with hematite, α-Fe2O3 (ICSD: 00-033-0664, R-3c (#167-1) space group) (see Figure S2(a)). Furthermore, for single Mn2O3, the diffraction angles with its corresponding crystal planes are consistent with α-Mn2O3 (ICSD: 24342, PBCA space group) (Figure S2(b)). The structure of stable ZnO, α-Mn2O3, and α-Fe2O3 that was developed using the VESTA 3D visualization program software depending on the AMCSD search result is given in Figures 2(a)–2(c), respectively.Figure 1
XRD patterns of ZnO, PVA-BMO1, PVA-BMO2, and PVA-TMOP1 nanomaterials.Figure 2
The polyhedral style crystal structures of (a) ZnO, (b) Fe2O3, and (c) Mn2O3 (red is for O atoms).
(a)(b)(c)The particle size optimizations for BMONCs with and without PVA are given in FigureS2(a) and (b). For the TMONCs, the particle size optimizations using different methods and salt precursors are given in Figure S2c. Further particle size optimizations using different amounts of PVA and precursor percentages were also present in [16]. For the BMONCs and TMONCs, except for peak intensity reduction and width widening, no diffraction peaks for Fe2O3 and Mn2O3 were found. Most probably, this is due to the small percentage of iron and manganese oxides. The nonshifting of peak position may also indicate the absence of any structural distortion on the ZnO crystal lattice attributed to Fe3+ or Mn3+ ion inclusion [27]. This means Fe2O3 and Mn2O3 are present as a separate phase through forming only a local heterojunction [27]. Loading a higher percentage of iron or/and manganese precursors above the optima may also degrade the structure of ZnO [28]. Furthermore, due to the presence of ionic radius differences between zinc and iron or/and manganese oxides, instead of doping, the formation of heterojunction was recommended [29].A reasonable surface area enhancement for PVA-BMONCs and PVA-TMONCs was observed compared to single ZnO, BMONCs, and TMONCs (TableS1-3). In advance, compared to the PVA-BMONCs, the PVA-TMONCs are showing enhanced surface area results. The XRD data and the respective size of the particles were calculated using Debye–Scherrer’s formula:
(1)D=Kλβcosθ,where λ is the wavelength of X-ray radiation (for Cu 0.15418 nm), K is constant, β is the full width at half maximum (FWHM), and θ is the diffracting angle.


### 3.2. UV-vis-DRS and UV-vis Studies

The optical properties of the nanopowder and its aqueous solution were characterized by UV-vis-DRS and UV-vis techniques, respectively. The percent reflectance versus wavelength along with the Kubelka–Munk (K–M) plots of ZnO powder is given in Figure3. ZnO and the optimized PVA-BMO1, PVA-BMO2, and PVA-TMOP1 nanocomposites are showing a characteristic absorption edge near to 380 nm (Figure 3(a)). Compared to the other, pure ZnO is showing high reflectance in the visible region. In fact, due to its wide bandgap energies (3.17 eV), it only responds to the UV region. However, for the binary and ternary composites, the reflectance in the visible region is reduced. Compared to ZnO, PVA-TMO1 and PVA-TMOP1 have low reflectance (~45%). This enhanced optical activity for the composites is due to the increased porosity/surface imperfection [30].Figure 3
(a) DRS plots of ZnO, PVA-BMO1, PVA-BMO2, and PVA-TMOP1; the respective direct (b); and indirect (c) Kubelka–Munk plots.
(a)(b)(c)In the parabolic band structure, the bandgap energy,Eg, and the absorption coefficient of a direct bandgap semiconductor α are related through
(2)αℏν1/n=Aℏν−Eg,where ℏ is Planck’s constant, ν is the photon’s frequency, and A is the slope in the linear region. Taking the K–M scattering coefficient S as a constant concerning the wavelength, and using the remission function in Equation (2), the following expression was derived:
(3)FRℏν2=Aℏν−Eg,where FR is equal to K/S, the molar absorption coefficient K is equal to 1−R2, the scattering factor S is equal to 2R, and R is the reflectance of the materials and is defined as %R/100.As shown in Figures3(b) and 3(c), the direct and indirect bandgap energies of the ZnO, PVA-BMO1, PVA-BMO2, and PVA-TMOP1 materials were measured by the extrapolation of the linear portion of the direct K–M function plots. The result shows the presence of nonnoticeable bandgap change. As shown in Figure S3(a) and (b), the nonobvious bandgap change was also further confirmed on UV-vis analysis conducted for optimized PVA-TMOP1 nanocomposites during the PVA amount and precursor percentage particle size optimization [16]. This may be due to the nonincorporation of either Fe0/Mn0 or Fe3+/Mn3+ ions in the ZnO crystalline lattice as confirmed on the XRD pattern [31]. The formation of this type of couple/heterojunction between metal oxides can enhance the charge transfer property. Furthermore, compared to single ZnO, the observed slight bandgap tuning (blue shift) for the composite could be attributed to the confinement effects [32].


### 3.3. FT-IR Analysis

The FTIR technique that gives the chemical bonding information of single, binary, and ternary nanomaterials is shown in Figure4. The calcined (C) and uncalcined (U) PVA-BMONCs and PVA-TMONCs are also given in Figure S4(a)-(c). The common broad absorption band around ~3600 and ~1650 cm-1 is due to the stretching vibration of chemisorbed hydroxyl groups and physisorbed water molecules. Due to interatomic vibration, semiconductor metal oxides exhibit a strong absorption band below 1000 cm-1. Due to two transverse optical stretching modes, the FT-IR spectrum of ZnO shows a characteristic absorption band in the range of 400-550 cm−1. These absorption peaks correlated with the TO-phonon and the LO-phonon frequency [33]. The shape, number, and wavenumber position of the bands are dependent on the chemical composition, morphology, and crystal structure of the materials. This means if the morphology of the materials changed from spherical (zero) dimension to one, two, or three-dimensional morphology, the broadness and splitting were also found to increase [34, 35]. For the crystalline ZnO, within the range of 400-550 cm−1, the two absorption peaks were observed. For PVA composites, only one peak was observed.Figure 4
FT-IR spectra of ZnO, PVA-BMO1, PVA-BMO2, and PVA-TMOP1 nanomaterials.Comparing the spectra of ZnO and calcined PVA composites with uncalcined PVA composites, one distinctive peak appeared around ~1400 cm−1 is due to the -CH2 bending vibration of PVA [36, 37]. Furthermore, the wavenumber shift and intensity difference were also observed. As reported [38], the source for the other peaks is expected to be from intermediate impurities created during synthesis. The absorption peaks appeared at ~1640 and ~1400 cm−1 are most probably either due to C=C and C-C stretching, respectively, or from the symmetric and asymmetric stretching vibration of the C=O/C-O group. The absorption peaks appeared at ~3000 cm−1 are due to the symmetric and asymmetric stretching vibration of CH2 [39, 40]. The absorption bands appeared at ~1300 and ~940 cm−1 were ascribed to symmetric C-H and bending vibration of the –CH3 group, respectively. The peak at ~1100 cm−1 is identified as CO (H) and CO (C) vibrations. Comparing the broad absorption band of ZnO with PVA composites, shifting of PVA composite peaks towards lower wavenumber was observed. The observed shift for both calcined and uncalcined PVA composites indicates surface passivation influences of PVA during synthesis. Indirectly, this indicates the presence of hydrogen bonds between the PVA (O-H group) and metal oxide surface [41].


### 3.4. BET Analysis

For an efficient environmental west management system, the surface-active sites and optimized pore volume of the synthesized materials are important [42]. The BET plots of single, binary, and ternary metal oxides are given in Figure S5-8. Furthermore, the combined BET plots of ZnO, PVA-BMO1, PVA-BMO2, and PVA-TMOP1 are also given in Figure 5. As seen in BET plots, the nanomaterials have a resemblance to the cylindrical pore shape model. The BET data is treated according to a BET adsorption isotherm linear equation:
(4)P/Pon1−P/Po=C−1nmCPPo+1nmC,where Po is the saturated vapor pressure of N2 gas in Pa; P is the partial vapor pressure of N2 gas in Pa; n is the volume of N2 gas adsorbed at standard temperature and pressure (STP) in mL; nm is the BET monolayer capacity; C is the dimensionless constant related to the enthalpy of N2 gas adsorption on the single, BMONC, and TMONC adsorbent.Figure 5
BET plots of ZnO (a), PVA-BMO1 (c), PVA-BMO2 (b), and PVA-TMOP1 (d) (inset: the respective BJH pore size distributions).According to the BET theory, the value ofC has a close relationship with the shape of the isotherms. For defining the BET monolayer capacity of the nanocomposites, the value of C should be ≥80 [43]. As seen from Table S4-6, the values of C for ZnO, Mn2O3, BMO1, BMO2, and PVA-BMO1 are <80 and the C values for the other are >80. For PVA-BMO1, PVA-TMOM1, and PVA-TMOP1, since their slope is 0, it is not possible to define the value of C. The specific surface area in m2·g–1 is calculated as
(5)as=nmLσmm×22400,where as is the BET-specific surface area of the single, BMONCs, and TMONCs of mass m in grams, L is the Avogadro constant (6.022×1023 mol−1), σm is the molecular adsorptive cross-sectional area occupied by N2 gas molecule in the complete monolayer (equal to 0.162 nm2 for N2 gas), and the 22400 is the volume occupied by 1 mole of N2 gas at STP, in mL.Among six types of adsorption isotherms that are characteristic of porous materials (types I-VI) [44], the appearances of the synthesized materials look like a typical IV isotherm with an H3 hysteresis loop. High adsorption capacities and sharp inflection at a high relative pressure (P/P0>0.8) signifying the coexistence of mesopore and macropore size distribution [45]. The sharp capillary condensation step between 0.40 and 0.85 for PVA-TMOP2 reflects the presence of a narrow pore size distribution.The relatively large surface area and narrow mesoporous channels provide enough space and facilitate the rapid adsorption of molecules. The pore size distributions of the synthesized materials were expressed in terms of the Barrett-Joyner-Halenda (BJH) curve. According to the IUPAC classification, materials that have a pore size diameter of <2.0 nm is categorized as microporous, in the range between 2.0 and 50.0 nm as mesoporous, and >50.0 nm as macroporous [43, 46, 47]. As seen in Table S4-6, for all single, BMONCs, and TMONCs, the average pore size distribution is in the range of 9–43 nm. This indicates the materials have mesoporous pore size distribution properties. Except for Fe2O3, the sizes of mesopores in the architecture of all materials look uniform; the difference is only in intensity. The appearance of the peaks>60 nm indicates the presence of some macroporous size distribution (see Figure S5-8 inset) [45]. Therefore, the materials have meso-macropore size distribution properties, yet the mesoporous type is dominant. The pore size curve shows a relatively wide distribution for PVA-TMOP1, which is consistent with the SEM result. Compared to single, BMONCs, and TMONCs, the PVA-TMOP1 is showing enhanced surface area and optimized pore volume.


### 3.5. SEM-EDX Analysis

For morphological and microstructure properties of synthesized materials, the SEM analysis was studied. The SEM images of ZnO, BMO1, BMO2, TMOM1, TMOM2, and PVA-TMOP2 nanomaterials are given in FigureS9(a)-(f), respectively, whereas the SEM images and the respective EDX spectra of PVA-BMO1, PVA-BMO2, and PVA-TMOP1 are given in Figures 6(a)–6(c). The morphology of BMONCs and TMONCs shows greater crystallinity compared to PVA-BMONCs and PVA-TMONCs. This is consistent with the XRD pattern result of the materials. Furthermore, as seen on SEM images, BMONCs and other TMONCs have high agglomeration/aggregation properties than PVA-BMONCs and PVA-TMONCs.Figure 6
SEM images and the respective EDX spectra of (a) PVA-TMOP1, (b) PVA-BMO1, and (c) PVA-BMO2 nanocomposites.
(a)(b)(c)Also, as confirmed on the N2 adsorption study, the porosity of PVA-BMO1 and PVA-TMOP1 is more visible than the others (see Figures 6(a) and 6(b)). To confirm the presence of Zn, Mn, Fe, and O compositions, which are not detected on the SEM images and XRD pattern, the EDX analysis was conducted. The result showed the presence of the expected Zn, Mn, Fe, and O elements. However, S in PVA-TMOP1, Cl and N in PVA-BMO1, and C and S in PVA-BMO2 present as impurities. The source for these impurities is most probably from the standard used during analysis [48, 49].


### 3.6. TEM Analysis

The TEM morphology of the optimized PVA-TMOP1, PVA-BMO1, and PVA-BMO2 NCs is shown in Figures7–9, respectively. As seen in Figure 7(a) of the PVA-TMOP1 image, agglomerates with a size ranging from 7 to 30 nm were observed. The particle size diameter for PVA-BMO1 and PVA-BMO2 composites is in the range of 20–70 and 30–60 nm, respectively. This is in agreement with the obtained approximate particle size from each XRD pattern. The TEM analysis also confirmed the porous nature of the composite, which is in good agreement with BET and SEM analysis. Between the agglomerates of PVA-TMOP1, PVA-BMO1, and PVA-BMO2 NCs, the oriented attachment that usually occurs between metal oxides was also detected. During oriented attachment, the presence of fission as a driving force and the particles were found to share a common crystallographic orientation [50, 51].Figure 7
(a) TEM image of PVA-TMOP1; (b) SAED ring (inset: XRD pattern of PVA-TMOP1); (c) HRTEM image; images (2), (3), (4), and (5) for ZnO (d) and Mn2O3 (e) are the magnified, FFT, IFFT, and profile of IFFT image of (1), respectively.
(a)(b)(c)(d)(e)Figure 8
(a) TEM image of PVA-BMO1, (b) HRTEM image, (c) SAED ring, and (d) the magnified (2), FFT (3), IFFT (4), and profile of IFFT (5) image of (1) for ZnO.
(a)(b)(c)(d)Figure 9
(a) TEM image of PVA-BMO2, (b) HRTEM image, (c) SAED ring, and (d) the magnified (2), FFT (3), IFFT (4), and profile of IFFT (5) image of (1) for Mn2O3.
(a)(b)(c)(d)The output from the lattice fringe analysis is given in Figures7(d) and 7(e) for PVA-TMOP1 and Figures 8(d) and 9(d) for PVA-BMO1 and PVA-BMO2, respectively. Figure 7(c) shows the magnified HRTEM image of PVA-TMOP1. From characteristic lattice fringes that appeared on the HRTEM image, the d-spacing value for (002) plane of ZnO was found to be 0.28 nm. The d-spacing value of 0.34 nm is matching to (221) plane of α-Mn2O3 [52, 53]. Yet, the lattice fringes for α-Fe2O3 were not found on the HRTEM image which is possibly due to the highly dispersed states of it. The lattice fringes of α-Fe2O3 were also not detected on the PVA-BMO1. Furthermore, as seen in Figure 9(d), the d-spacing value of ~0.343 nm is corresponding to (221) atomic plane of α-Mn2O3. In advance, unlike that of PVA-BMO1 and PVA-TMOP1 (Figures 7(a) and 8(a)), the presence of two different morphologies in Figure 9(a) clearly shows the existence of two different components.The occurrence of stacking faults on the surface of the NPs suggests the semicrystalline nature of the nanocomposites (see the IFFT (4) images of Figures7–9). The selected area electron diffraction (SAED) rings of PVA-TMOP1, PVA-BMO1, and PVA-BMO2 are given in Figures 7(b), 8(c), and 9(c), respectively. The obtained approximate interplanar spacing of the diffraction rings from SAED ring matches with XRD pattern of the respective composites. The SAED pattern, especially on PVA-TMOP1, indicates the presence of porous regions on the samples. The presence of several bright diffraction spots on the rings, especially for PVA-BMO1 and PVA-BMO2, confirms the crystallinity of the ZnO, whereas the spots present out of the ring most probably is due to the α-Fe2O3 or/and α-Mn2O3 [54].


### 3.7. CV and EIS Studies

The electrochemical property of ZnO, PVA-BMO1, PVA-BMO2, and PVA-TMOP1 was characterized by EIS and CV analytical techniques. The CV plots of these materials at different scan rates are given in FigureS10-12(a) and (b). With increasing the scan rate, the oxidation peak shifts towards more positive potential and a slight increment in redox peak current was observed. As reported [4], the presence of ZnOH42− reduction peaks at a lower frequency for ZnO indicates the formation of photocorrosion. Its absence on the composites confirms the prevention of photocorrosion due to the enhancement of quantum efficiency and stability of the photocatalyst. For electrochemical improvement contrast, the CV plot of ZnO with the two binary and ternary nanocomposites at a scan rate of 30 mV S−1 is depicted in Figure S10-12(c). At the upper potential, the PVA-BMO1, PVA-BMO2, and PVA-TMOP1 CV curves show a greater current rise over the ZnO curve. This enhanced current response for the composites indicates the presence of an improved electron transport between the electrolyte medium and the electrode of the composite [55]. The electron transport potential order was determined to be PVA-TMOP1 > PVA-BMO1 > PVA-BMO2 > ZnO. This obvious electron transport potential result for the composite is due to the formation of heterojunction between metal oxides. As confirmed on the SEM images, this may also be due to the porous nature of the nanocomposites.The linear relationship plotted between the oxide peak current (Ip) versus the scan rate (υ) is drawn as seen in Figure S10-12(d). The well-fitting of the linear plots for PVA-BMO1 and PVA-TMOP1 shows the adsorption controlled electrocatalytic process. Nonfitting of the PVA-BMO2 linear plot indicates the diffusion-dependent electrocatalytic process. The combined CV plots of ZnO, PVA-BMO1, PVA-BMO2, and PVA-TMOP1 are given in Figure 10(a). Compared to the other, the PVA-TMOP1 CV curve shows a greater electrochemical oxidation process.Figure 10
(a) CV plots of ZnO (i), PVA-BMO1 (iii), PVA-BMO2 (ii), and PVA-TMOP1 (iv); (b) the respective EIS spectra (inset: their magnified EIS plots).
(a)(b)To further understand the electrochemical properties of ZnO, PVA-BMO1, PVA-BMO2, and PVA-TMOP1 materials, the EIS test was conducted. As seen in FigureS10-12(e) and Figure 10(b), the Nyquist plot was used to understand the resistance properties of the material. The semicircular portion at a higher frequency is equal to the electron transfer resistance Rct at the contact interface of the electrode and electrolyte solution [56]. As seen in the combined EIS plots in Figure 10(b), the semicircular diameter of PVA-TMOP1 is much smaller than the other. This indicates that the PVA-TMOP1 has a higher electron transfer capability.The value ofRct is equal to the diameter of the semicircle [57]. The approximate Rct value of ZnO, PVA-BMO1, PVA-BMO2, and PVA-TMOP1 was determined to be 65, 25, 61, and 7 Ω, respectively. The result shows that the charge transfer capability is in the order of PVA-TMOP1 > PVA-BMO1 > PVA-BMO2 > ZnO. As confirmed on the TEM image, the increased conductivity of the composites may be due to the formation of heterojunction between the metal oxides and the porous nature of the materials. In advance, increasing the heterojunction to the ternary PVA-TMOP1 is showing enhanced charge transfer capability. As reported [58], this is most probably due to the more negative band position values of the composites compared to ZnO. The linear portion at lower frequencies is known as the Warburg resistance, which is related to ion transport/diffusion from the electrolyte to the surfaces of the electrode.


## 3.1. XRD Analysis

The XRD diffraction pattern of the synthesized nanomaterials that confirms the crystallinity and composition of single, BMONC, and TMONC materials are shown in Figure1. All the diffraction angles with its corresponding crystal planes are corresponding to ZnO (ICSD: 00-036-1451, P63mc (#186-1) space group) (Figure 1). For single Fe2O3, the diffraction angles with its corresponding crystal planes are consistent with hematite, α-Fe2O3 (ICSD: 00-033-0664, R-3c (#167-1) space group) (see Figure S2(a)). Furthermore, for single Mn2O3, the diffraction angles with its corresponding crystal planes are consistent with α-Mn2O3 (ICSD: 24342, PBCA space group) (Figure S2(b)). The structure of stable ZnO, α-Mn2O3, and α-Fe2O3 that was developed using the VESTA 3D visualization program software depending on the AMCSD search result is given in Figures 2(a)–2(c), respectively.Figure 1
XRD patterns of ZnO, PVA-BMO1, PVA-BMO2, and PVA-TMOP1 nanomaterials.Figure 2
The polyhedral style crystal structures of (a) ZnO, (b) Fe2O3, and (c) Mn2O3 (red is for O atoms).
(a)(b)(c)The particle size optimizations for BMONCs with and without PVA are given in FigureS2(a) and (b). For the TMONCs, the particle size optimizations using different methods and salt precursors are given in Figure S2c. Further particle size optimizations using different amounts of PVA and precursor percentages were also present in [16]. For the BMONCs and TMONCs, except for peak intensity reduction and width widening, no diffraction peaks for Fe2O3 and Mn2O3 were found. Most probably, this is due to the small percentage of iron and manganese oxides. The nonshifting of peak position may also indicate the absence of any structural distortion on the ZnO crystal lattice attributed to Fe3+ or Mn3+ ion inclusion [27]. This means Fe2O3 and Mn2O3 are present as a separate phase through forming only a local heterojunction [27]. Loading a higher percentage of iron or/and manganese precursors above the optima may also degrade the structure of ZnO [28]. Furthermore, due to the presence of ionic radius differences between zinc and iron or/and manganese oxides, instead of doping, the formation of heterojunction was recommended [29].A reasonable surface area enhancement for PVA-BMONCs and PVA-TMONCs was observed compared to single ZnO, BMONCs, and TMONCs (TableS1-3). In advance, compared to the PVA-BMONCs, the PVA-TMONCs are showing enhanced surface area results. The XRD data and the respective size of the particles were calculated using Debye–Scherrer’s formula:
(1)D=Kλβcosθ,where λ is the wavelength of X-ray radiation (for Cu 0.15418 nm), K is constant, β is the full width at half maximum (FWHM), and θ is the diffracting angle.


## 3.2. UV-vis-DRS and UV-vis Studies

The optical properties of the nanopowder and its aqueous solution were characterized by UV-vis-DRS and UV-vis techniques, respectively. The percent reflectance versus wavelength along with the Kubelka–Munk (K–M) plots of ZnO powder is given in Figure3. ZnO and the optimized PVA-BMO1, PVA-BMO2, and PVA-TMOP1 nanocomposites are showing a characteristic absorption edge near to 380 nm (Figure 3(a)). Compared to the other, pure ZnO is showing high reflectance in the visible region. In fact, due to its wide bandgap energies (3.17 eV), it only responds to the UV region. However, for the binary and ternary composites, the reflectance in the visible region is reduced. Compared to ZnO, PVA-TMO1 and PVA-TMOP1 have low reflectance (~45%). This enhanced optical activity for the composites is due to the increased porosity/surface imperfection [30].Figure 3
(a) DRS plots of ZnO, PVA-BMO1, PVA-BMO2, and PVA-TMOP1; the respective direct (b); and indirect (c) Kubelka–Munk plots.
(a)(b)(c)In the parabolic band structure, the bandgap energy,Eg, and the absorption coefficient of a direct bandgap semiconductor α are related through
(2)αℏν1/n=Aℏν−Eg,where ℏ is Planck’s constant, ν is the photon’s frequency, and A is the slope in the linear region. Taking the K–M scattering coefficient S as a constant concerning the wavelength, and using the remission function in Equation (2), the following expression was derived:
(3)FRℏν2=Aℏν−Eg,where FR is equal to K/S, the molar absorption coefficient K is equal to 1−R2, the scattering factor S is equal to 2R, and R is the reflectance of the materials and is defined as %R/100.As shown in Figures3(b) and 3(c), the direct and indirect bandgap energies of the ZnO, PVA-BMO1, PVA-BMO2, and PVA-TMOP1 materials were measured by the extrapolation of the linear portion of the direct K–M function plots. The result shows the presence of nonnoticeable bandgap change. As shown in Figure S3(a) and (b), the nonobvious bandgap change was also further confirmed on UV-vis analysis conducted for optimized PVA-TMOP1 nanocomposites during the PVA amount and precursor percentage particle size optimization [16]. This may be due to the nonincorporation of either Fe0/Mn0 or Fe3+/Mn3+ ions in the ZnO crystalline lattice as confirmed on the XRD pattern [31]. The formation of this type of couple/heterojunction between metal oxides can enhance the charge transfer property. Furthermore, compared to single ZnO, the observed slight bandgap tuning (blue shift) for the composite could be attributed to the confinement effects [32].


## 3.3. FT-IR Analysis

The FTIR technique that gives the chemical bonding information of single, binary, and ternary nanomaterials is shown in Figure4. The calcined (C) and uncalcined (U) PVA-BMONCs and PVA-TMONCs are also given in Figure S4(a)-(c). The common broad absorption band around ~3600 and ~1650 cm-1 is due to the stretching vibration of chemisorbed hydroxyl groups and physisorbed water molecules. Due to interatomic vibration, semiconductor metal oxides exhibit a strong absorption band below 1000 cm-1. Due to two transverse optical stretching modes, the FT-IR spectrum of ZnO shows a characteristic absorption band in the range of 400-550 cm−1. These absorption peaks correlated with the TO-phonon and the LO-phonon frequency [33]. The shape, number, and wavenumber position of the bands are dependent on the chemical composition, morphology, and crystal structure of the materials. This means if the morphology of the materials changed from spherical (zero) dimension to one, two, or three-dimensional morphology, the broadness and splitting were also found to increase [34, 35]. For the crystalline ZnO, within the range of 400-550 cm−1, the two absorption peaks were observed. For PVA composites, only one peak was observed.Figure 4
FT-IR spectra of ZnO, PVA-BMO1, PVA-BMO2, and PVA-TMOP1 nanomaterials.Comparing the spectra of ZnO and calcined PVA composites with uncalcined PVA composites, one distinctive peak appeared around ~1400 cm−1 is due to the -CH2 bending vibration of PVA [36, 37]. Furthermore, the wavenumber shift and intensity difference were also observed. As reported [38], the source for the other peaks is expected to be from intermediate impurities created during synthesis. The absorption peaks appeared at ~1640 and ~1400 cm−1 are most probably either due to C=C and C-C stretching, respectively, or from the symmetric and asymmetric stretching vibration of the C=O/C-O group. The absorption peaks appeared at ~3000 cm−1 are due to the symmetric and asymmetric stretching vibration of CH2 [39, 40]. The absorption bands appeared at ~1300 and ~940 cm−1 were ascribed to symmetric C-H and bending vibration of the –CH3 group, respectively. The peak at ~1100 cm−1 is identified as CO (H) and CO (C) vibrations. Comparing the broad absorption band of ZnO with PVA composites, shifting of PVA composite peaks towards lower wavenumber was observed. The observed shift for both calcined and uncalcined PVA composites indicates surface passivation influences of PVA during synthesis. Indirectly, this indicates the presence of hydrogen bonds between the PVA (O-H group) and metal oxide surface [41].


## 3.4. BET Analysis

For an efficient environmental west management system, the surface-active sites and optimized pore volume of the synthesized materials are important [42]. The BET plots of single, binary, and ternary metal oxides are given in Figure S5-8. Furthermore, the combined BET plots of ZnO, PVA-BMO1, PVA-BMO2, and PVA-TMOP1 are also given in Figure 5. As seen in BET plots, the nanomaterials have a resemblance to the cylindrical pore shape model. The BET data is treated according to a BET adsorption isotherm linear equation:
(4)P/Pon1−P/Po=C−1nmCPPo+1nmC,where Po is the saturated vapor pressure of N2 gas in Pa; P is the partial vapor pressure of N2 gas in Pa; n is the volume of N2 gas adsorbed at standard temperature and pressure (STP) in mL; nm is the BET monolayer capacity; C is the dimensionless constant related to the enthalpy of N2 gas adsorption on the single, BMONC, and TMONC adsorbent.Figure 5
BET plots of ZnO (a), PVA-BMO1 (c), PVA-BMO2 (b), and PVA-TMOP1 (d) (inset: the respective BJH pore size distributions).According to the BET theory, the value ofC has a close relationship with the shape of the isotherms. For defining the BET monolayer capacity of the nanocomposites, the value of C should be ≥80 [43]. As seen from Table S4-6, the values of C for ZnO, Mn2O3, BMO1, BMO2, and PVA-BMO1 are <80 and the C values for the other are >80. For PVA-BMO1, PVA-TMOM1, and PVA-TMOP1, since their slope is 0, it is not possible to define the value of C. The specific surface area in m2·g–1 is calculated as
(5)as=nmLσmm×22400,where as is the BET-specific surface area of the single, BMONCs, and TMONCs of mass m in grams, L is the Avogadro constant (6.022×1023 mol−1), σm is the molecular adsorptive cross-sectional area occupied by N2 gas molecule in the complete monolayer (equal to 0.162 nm2 for N2 gas), and the 22400 is the volume occupied by 1 mole of N2 gas at STP, in mL.Among six types of adsorption isotherms that are characteristic of porous materials (types I-VI) [44], the appearances of the synthesized materials look like a typical IV isotherm with an H3 hysteresis loop. High adsorption capacities and sharp inflection at a high relative pressure (P/P0>0.8) signifying the coexistence of mesopore and macropore size distribution [45]. The sharp capillary condensation step between 0.40 and 0.85 for PVA-TMOP2 reflects the presence of a narrow pore size distribution.The relatively large surface area and narrow mesoporous channels provide enough space and facilitate the rapid adsorption of molecules. The pore size distributions of the synthesized materials were expressed in terms of the Barrett-Joyner-Halenda (BJH) curve. According to the IUPAC classification, materials that have a pore size diameter of <2.0 nm is categorized as microporous, in the range between 2.0 and 50.0 nm as mesoporous, and >50.0 nm as macroporous [43, 46, 47]. As seen in Table S4-6, for all single, BMONCs, and TMONCs, the average pore size distribution is in the range of 9–43 nm. This indicates the materials have mesoporous pore size distribution properties. Except for Fe2O3, the sizes of mesopores in the architecture of all materials look uniform; the difference is only in intensity. The appearance of the peaks>60 nm indicates the presence of some macroporous size distribution (see Figure S5-8 inset) [45]. Therefore, the materials have meso-macropore size distribution properties, yet the mesoporous type is dominant. The pore size curve shows a relatively wide distribution for PVA-TMOP1, which is consistent with the SEM result. Compared to single, BMONCs, and TMONCs, the PVA-TMOP1 is showing enhanced surface area and optimized pore volume.


## 3.5. SEM-EDX Analysis

For morphological and microstructure properties of synthesized materials, the SEM analysis was studied. The SEM images of ZnO, BMO1, BMO2, TMOM1, TMOM2, and PVA-TMOP2 nanomaterials are given in FigureS9(a)-(f), respectively, whereas the SEM images and the respective EDX spectra of PVA-BMO1, PVA-BMO2, and PVA-TMOP1 are given in Figures 6(a)–6(c). The morphology of BMONCs and TMONCs shows greater crystallinity compared to PVA-BMONCs and PVA-TMONCs. This is consistent with the XRD pattern result of the materials. Furthermore, as seen on SEM images, BMONCs and other TMONCs have high agglomeration/aggregation properties than PVA-BMONCs and PVA-TMONCs.Figure 6
SEM images and the respective EDX spectra of (a) PVA-TMOP1, (b) PVA-BMO1, and (c) PVA-BMO2 nanocomposites.
(a)(b)(c)Also, as confirmed on the N2 adsorption study, the porosity of PVA-BMO1 and PVA-TMOP1 is more visible than the others (see Figures 6(a) and 6(b)). To confirm the presence of Zn, Mn, Fe, and O compositions, which are not detected on the SEM images and XRD pattern, the EDX analysis was conducted. The result showed the presence of the expected Zn, Mn, Fe, and O elements. However, S in PVA-TMOP1, Cl and N in PVA-BMO1, and C and S in PVA-BMO2 present as impurities. The source for these impurities is most probably from the standard used during analysis [48, 49].


## 3.6. TEM Analysis

The TEM morphology of the optimized PVA-TMOP1, PVA-BMO1, and PVA-BMO2 NCs is shown in Figures7–9, respectively. As seen in Figure 7(a) of the PVA-TMOP1 image, agglomerates with a size ranging from 7 to 30 nm were observed. The particle size diameter for PVA-BMO1 and PVA-BMO2 composites is in the range of 20–70 and 30–60 nm, respectively. This is in agreement with the obtained approximate particle size from each XRD pattern. The TEM analysis also confirmed the porous nature of the composite, which is in good agreement with BET and SEM analysis. Between the agglomerates of PVA-TMOP1, PVA-BMO1, and PVA-BMO2 NCs, the oriented attachment that usually occurs between metal oxides was also detected. During oriented attachment, the presence of fission as a driving force and the particles were found to share a common crystallographic orientation [50, 51].Figure 7
(a) TEM image of PVA-TMOP1; (b) SAED ring (inset: XRD pattern of PVA-TMOP1); (c) HRTEM image; images (2), (3), (4), and (5) for ZnO (d) and Mn2O3 (e) are the magnified, FFT, IFFT, and profile of IFFT image of (1), respectively.
(a)(b)(c)(d)(e)Figure 8
(a) TEM image of PVA-BMO1, (b) HRTEM image, (c) SAED ring, and (d) the magnified (2), FFT (3), IFFT (4), and profile of IFFT (5) image of (1) for ZnO.
(a)(b)(c)(d)Figure 9
(a) TEM image of PVA-BMO2, (b) HRTEM image, (c) SAED ring, and (d) the magnified (2), FFT (3), IFFT (4), and profile of IFFT (5) image of (1) for Mn2O3.
(a)(b)(c)(d)The output from the lattice fringe analysis is given in Figures7(d) and 7(e) for PVA-TMOP1 and Figures 8(d) and 9(d) for PVA-BMO1 and PVA-BMO2, respectively. Figure 7(c) shows the magnified HRTEM image of PVA-TMOP1. From characteristic lattice fringes that appeared on the HRTEM image, the d-spacing value for (002) plane of ZnO was found to be 0.28 nm. The d-spacing value of 0.34 nm is matching to (221) plane of α-Mn2O3 [52, 53]. Yet, the lattice fringes for α-Fe2O3 were not found on the HRTEM image which is possibly due to the highly dispersed states of it. The lattice fringes of α-Fe2O3 were also not detected on the PVA-BMO1. Furthermore, as seen in Figure 9(d), the d-spacing value of ~0.343 nm is corresponding to (221) atomic plane of α-Mn2O3. In advance, unlike that of PVA-BMO1 and PVA-TMOP1 (Figures 7(a) and 8(a)), the presence of two different morphologies in Figure 9(a) clearly shows the existence of two different components.The occurrence of stacking faults on the surface of the NPs suggests the semicrystalline nature of the nanocomposites (see the IFFT (4) images of Figures7–9). The selected area electron diffraction (SAED) rings of PVA-TMOP1, PVA-BMO1, and PVA-BMO2 are given in Figures 7(b), 8(c), and 9(c), respectively. The obtained approximate interplanar spacing of the diffraction rings from SAED ring matches with XRD pattern of the respective composites. The SAED pattern, especially on PVA-TMOP1, indicates the presence of porous regions on the samples. The presence of several bright diffraction spots on the rings, especially for PVA-BMO1 and PVA-BMO2, confirms the crystallinity of the ZnO, whereas the spots present out of the ring most probably is due to the α-Fe2O3 or/and α-Mn2O3 [54].


## 3.7. CV and EIS Studies

The electrochemical property of ZnO, PVA-BMO1, PVA-BMO2, and PVA-TMOP1 was characterized by EIS and CV analytical techniques. The CV plots of these materials at different scan rates are given in FigureS10-12(a) and (b). With increasing the scan rate, the oxidation peak shifts towards more positive potential and a slight increment in redox peak current was observed. As reported [4], the presence of ZnOH42− reduction peaks at a lower frequency for ZnO indicates the formation of photocorrosion. Its absence on the composites confirms the prevention of photocorrosion due to the enhancement of quantum efficiency and stability of the photocatalyst. For electrochemical improvement contrast, the CV plot of ZnO with the two binary and ternary nanocomposites at a scan rate of 30 mV S−1 is depicted in Figure S10-12(c). At the upper potential, the PVA-BMO1, PVA-BMO2, and PVA-TMOP1 CV curves show a greater current rise over the ZnO curve. This enhanced current response for the composites indicates the presence of an improved electron transport between the electrolyte medium and the electrode of the composite [55]. The electron transport potential order was determined to be PVA-TMOP1 > PVA-BMO1 > PVA-BMO2 > ZnO. This obvious electron transport potential result for the composite is due to the formation of heterojunction between metal oxides. As confirmed on the SEM images, this may also be due to the porous nature of the nanocomposites.The linear relationship plotted between the oxide peak current (Ip) versus the scan rate (υ) is drawn as seen in Figure S10-12(d). The well-fitting of the linear plots for PVA-BMO1 and PVA-TMOP1 shows the adsorption controlled electrocatalytic process. Nonfitting of the PVA-BMO2 linear plot indicates the diffusion-dependent electrocatalytic process. The combined CV plots of ZnO, PVA-BMO1, PVA-BMO2, and PVA-TMOP1 are given in Figure 10(a). Compared to the other, the PVA-TMOP1 CV curve shows a greater electrochemical oxidation process.Figure 10
(a) CV plots of ZnO (i), PVA-BMO1 (iii), PVA-BMO2 (ii), and PVA-TMOP1 (iv); (b) the respective EIS spectra (inset: their magnified EIS plots).
(a)(b)To further understand the electrochemical properties of ZnO, PVA-BMO1, PVA-BMO2, and PVA-TMOP1 materials, the EIS test was conducted. As seen in FigureS10-12(e) and Figure 10(b), the Nyquist plot was used to understand the resistance properties of the material. The semicircular portion at a higher frequency is equal to the electron transfer resistance Rct at the contact interface of the electrode and electrolyte solution [56]. As seen in the combined EIS plots in Figure 10(b), the semicircular diameter of PVA-TMOP1 is much smaller than the other. This indicates that the PVA-TMOP1 has a higher electron transfer capability.The value ofRct is equal to the diameter of the semicircle [57]. The approximate Rct value of ZnO, PVA-BMO1, PVA-BMO2, and PVA-TMOP1 was determined to be 65, 25, 61, and 7 Ω, respectively. The result shows that the charge transfer capability is in the order of PVA-TMOP1 > PVA-BMO1 > PVA-BMO2 > ZnO. As confirmed on the TEM image, the increased conductivity of the composites may be due to the formation of heterojunction between the metal oxides and the porous nature of the materials. In advance, increasing the heterojunction to the ternary PVA-TMOP1 is showing enhanced charge transfer capability. As reported [58], this is most probably due to the more negative band position values of the composites compared to ZnO. The linear portion at lower frequencies is known as the Warburg resistance, which is related to ion transport/diffusion from the electrolyte to the surfaces of the electrode.


## 4. Conclusion

Developing an efficient technique is the current necessity for the environmental waste management system. The novel sol-gel-self-propagation technique was developed for the synthesis of porous materials. Compared to the coprecipitation, the sol-gel technique gave a better surface area to volume ratio result. The zinc nitrate precursor is giving good self-propagation progression than the zinc acetate salt precursor. The porous nature of the material was confirmed by SEM and BET analysis; in advance, this is confirmed from the SAED ring. Using the XRD pattern and TEM analysis, the particle size of the synthesized materials was confirmed to be in the nanorange (~7-70 nm). The EDX and HRTEM analyses were used for the compositional investigation of the nanomaterials. The improvements in charge transfer synergy from single-binary-ternary were verified through CV and EIS techniques. The result shows the charge transfer capability to be in the order of ternary > binary > single. The efficiency of these porous materials will also be tested for the photocatalytic degradation of dye.



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*Source: 6532835-2020-09-29.xml*