Study on the Photocatalytic Properties of Flower-Shaped SnO2

Using cetyltrimethylammonium bromide (CTAB) as the surfactant from the precursors of SnCl2·2H2O, the flower-shaped nano composite of tin oxide (SnO2) is prepared by the simple eco-friendly hydrothermal method. We can see that the as-prepared SnO2 sample has a rutile phase crystal structure with regular-shaped nanosheets, and the nanosheets were cross-assembled to form nanoflowers. The band gap of the as-prepared SnO2 sample is 2.26 eV, which is close to the calculated energy gap of 2.58 eV based on density functional theory. The sample is used to degrade the organic dye, and this preliminary application study indicates that the as-prepared SnO2 sample has good stability and reusability in the visible light assisted degradation of methyl orange. Through capture experiments, it is determined that electrons and holes play a major role in the degradation process. The reaction mechanism is also analyzed to indicate the internal relationship between the as-prepared SnO2 samples and its photocatalytic properties.


Introduction
At present, water pollution is a direct threat to human survival, and it is a big problem that must be addressed. In water pollution control, wastewater containing dyes is a challenge for wastewater treatment due to its variety, high toxicity, severe environmental impact, and difficulty in degradation [1]. Photocatalytic technology is an efficient, energysaving, and non-cross-contaminating method to break down organic pollutants contained in dyes in wastewater into non-toxic or less-toxic small molecules [2]. Therefore, the preparation of excellent photocatalysts is very important in the treatment of wastewater containing dyes. SnO 2 is an inexpensive, non-toxic, high electron mobility, and high photosensitivity compound, which has attracted wide attention in basic research and practical applications, such as photocatalysts, gas sensors, solar cells, electrode materials, and so on [3]. By modulating the morphology of the SnO 2 nanocrystals, the physical and chemical properties can be manipulated [4]. In recent years, various morphologies of SnO 2 have been prepared, including nanorods, nanowires, nanobelts, and nanoflowers [5][6][7][8]. Three-dimensional SnO 2 hierarchical nanostructures are beneficial to improving its performance, due to a low density, high porosity, high specific surface area, and so on [9]. Acharyulu et al. synthesized TiO 2 /SnO 2 hollow spheres via a hydrothermal process and the samples can be used for photocatalytic mineralization of methylene blue (MB), methyl orange (MO), rhodamine B (RhB), and Congo red (CR) dyes under UV exposure [10]. Lei et al. proposed a facile route to prepare a novel Fe 2 O 3 /SnO 2 heterojunction structure, in which the nanobelt arrays grown on iron foil naturally form a Schottky-type contact and provide a direct pathway for the photogenerated excitons, with a degradation rate constant of the Fe 2 O 3 /SnO 2 film of approximately 12 times that α-Fe 2 O 3 nanobelt arrays [11]. Xu et al. synthesized SnO 2 @ZnO hierarchical nanostructures by a simple two-step microwave-assistant hydrothermal method, and remarkably enhanced the photocatalytic degradation of a MB aqueous solution under visible light irradiation [12]. Bezzerrouk et al. synthesized SnO 2 thin film via an ultrasonic spray pyrolysis technique in the inner wall of a glass tube, with the SnO 2 thin film presenting the best MB degradation efficiency compared to the other processes [13].
In this work, we used a simple method to synthesize hierarchical flower-like SnO 2 nanostructures by the hydrothermal method. The properties of the product are investigated by using X-ray diffraction (XRD), scanning electron microscopy (SEM), transmission electron microscopy (TEM), X-ray photoelectron spectrum (XPS), as well as Raman and ultraviolet-visible (UV-Vis) spectra. In addition, the experiment shows that the SnO 2 product exhibits a high catalytic activity, good stability, and reusability for degradation of MO under visible light.

Synthesis of SnO 2
In this paper, the chemical precursors were all analytical grade. SnO 2 was prepared by a facile one-step hydrothermal method as follows: 1 g SnCl 2 ·2H 2 O was first dissolved in 40 mL deionized water ultrasonically for 5 min, and stirred for 30 min to form the precursor solution; 1.6467 g CTAB was dissolved in 40 mL deionized water, with ultrasonic treatment for 15 min; and 0.7293 g NaOH was added and stirred for 30 min. After being fully dissolved, we added the precursor solution. The mixture solution was stirred for 60 min, and then transferred to a 100 mL Teflon-lined stainless-steel autoclave and kept at 140 • C for 12 h. After the reaction, the precipitate was washed with anhydrous ethanol and deionized water for several times. Finally, light-yellow SnO 2 powder was obtained after drying at 80 • C for 8 h. ( Figure S1 shows the SnO 2 product synthesis procedure).

Photocatalytic Testing
In this work, MO was selected as the target pollutant to evaluate the photocatalytic activity. Specifically, 50 mg of the catalyst was added to a 10 mg/L MO solution, and these solutions were stirred in the dark for 30 min to make the photocatalyst reach the adsorption-desorption equilibrium of MO. The light source used for photodegradation of the MO solution was a 500 W xenon lamp. The degradation reaction was carried out under stirring conditions at various times points: 0, 20, 40, 60, 80, 100, and 120 min. A 5 mL solution was taken out each time for centrifugation to completely precipitate, and then their respective supernatants were taken. The corresponding absorbance ABS value (absorption wavelength is 300 nm-600 nm) was tested using an ultraviolet spectrophotometer, with a residual degradation ratio of MO: η = C t /C 0 , where C 0 (mg/L) and C t (mg/L) represent the initial concentration of the dye and the mass concentration of the dye solution at time t, respectively. Additionally, a SnO 2 adsorption study was carried out in the contaminated solutions for 2 h, and a pollutant circulation photolysis study was carried out for 10 h under visible light.

Materials Characterization
The crystal phases of the as-prepared SnO 2 products were characterized by XRD and the results are shown in Figure 1a. The scan range is from 10 • to 75 • . By comparing the SnO 2 PDF standard card (JADES: 71-0652), the 2θ values at 26.5 • , 34 • , 37.8 • , 51.9 • , 54.8 • , 64.7 • , and 65.9 • correspond to the crystalline planes (110), (101), (200), (211), (220), (310), and (301), which can determine the crystal structure of the SnO 2 is in the rutile phase based on the 71-0652 file of the JCPDS [14,15]. However, there are two miscellaneous peaks generated around 32 • and 50.1 • , which may result from SnO generated during the preparation process.  Figure 1c, corresponds to the (310) surface of SnO 2 . Besides the two peaks at 32 • and 50.1 • , there is no other obvious impurity peaks, and the diffraction peaks are sharp and strong, which is basically consistent with the results of the standard card, indicating that the synthesized SnO 2 sample has good crystallinity. process. Figure 1d exhibits the high-resolution transmission electron microscopy (HRTEM) image of the as-prepared SnO2. The visible lattice fringe with an interplanar crystal spacing of 0.289 nm, shown in Figure 1b, is assigned to the (112) plane of SnO, which can confirm the source of the XRD peaks at 32° and 50.1°. The lattice fringe of the crystal spacing of 0.336 nm, shown in Figure 1c, corresponds to the (310) surface of SnO2. Besides the two peaks at 32° and 50.1°, there is no other obvious impurity peaks, and the diffraction peaks are sharp and strong, which is basically consistent with the results of the standard card, indicating that the synthesized SnO2 sample has good crystallinity.  Figure 2 displays the SEM images of the as-prepared SnO2 sample, and the product has a flower-shaped morphology. The general morphology of the SnO2 product is shown in Figure 2e-h, and we can see that the products have a high yield and uniformity. As shown in Figure 2d, the SnO2 presents a uniform, flower-like architecture, with a diameter of approximately 8-9 μm. As we can see from Figure 2a-d, the SnO2 nanoflowers are constructed by a lot of nanosheets, which are self-assembled densely together and the surface is very smooth.  Figure 2 displays the SEM images of the as-prepared SnO 2 sample, and the product has a flower-shaped morphology. The general morphology of the SnO 2 product is shown in Figure 2e-h, and we can see that the products have a high yield and uniformity. As shown in Figure 2d, the SnO 2 presents a uniform, flower-like architecture, with a diameter of approximately 8-9 µm. As we can see from Figure 2a-d, the SnO 2 nanoflowers are constructed by a lot of nanosheets, which are self-assembled densely together and the surface is very smooth.
Furthermore, the chemical compositions and valence states of the SnO 2 samples were analyzed by XPS. High-resolution XPS analysis was performed for each element and calibrated using the C 1s standard carbon peak. Figure 3a shows the wide range of XPS spectra of the as-prepared SnO 2 product. In Figure 3b,c, no peaks other than Sn, O, and C can be identified. The presence of a C element was observed, which may be due to the pollution of the sample surface by carbon materials. Figure 3b shows the XPS spectra of O 1s. The peak at 530.45 eV corresponds to O 1s, and the binding energy indicates that the oxygen atoms exist as O 2− species in the product. Figure 3c shows the high-resolution XPS spectra of Sn 3d, in which the peaks at 486.35 eV and 494.8 eV are from Sn 3d 5/2 and Sn 3d 3/2 , respectively. The result is in agreement with the reported values in the literature [16]. XPS results confirmed that the synthesized product is pure SnO 2 in terms of elements. Thus, the SnO 2 flower-like nanostructures were determined to be successfully synthesized through the above analysis. Furthermore, the chemical compositions and valence states of the SnO2 samples were analyzed by XPS. High-resolution XPS analysis was performed for each element and calibrated using the C 1s standard carbon peak. Figure 3a shows the wide range of XPS spectra of the as-prepared SnO2 product. In Figure 3b,c, no peaks other than Sn, O, and C can be identified. The presence of a C element was observed, which may be due to the pollution of the sample surface by carbon materials. Figure 3b shows the XPS spectra of O 1s. The peak at 530.45 eV corresponds to O 1s, and the binding energy indicates that the oxygen atoms exist as O 2− species in the product. Figure 3c shows the high-resolution XPS spectra of Sn 3d, in which the peaks at 486.35 eV and 494.8 eV are from Sn 3d5/2 and Sn 3d3/2, respectively. The result is in agreement with the reported values in the literature [16]. XPS results confirmed that the synthesized product is pure SnO2 in terms of elements. Thus, the SnO2 flower-like nanostructures were determined to be successfully synthesized through the above analysis.
In order to clarify the effect of the as-prepared SnO2 products on the fluctuation of chemical bonds, the molecular vibration information of the specimens was characterized by a Raman spectrometer and the result is shown in Figure 3d. For the as-prepared nanoflower SnO2, the main peaks are concentrated at 621.177 cm −1 and 675.25 cm −1 . The peak at 621.177 cm −1 is attributed to the A1g vibration mode of SnO2 with a tetragonal rutile structure. The peak at 675.25 cm −1 is induced by the size effect of the very small SnO2 nanocrystals and in fact it does not appear in bulk SnO2. PL measurement is powerful to study the recombination rate of the e − and h + pair in the samples, and the recombination rate of the e − and h + pair is proportional to the PL intensity. Figure 3e shows the emission spectra of the as-prepared SnO2 products, and the PL spectrum is carried out in the wavelength range of 350-800 nm using an excitation wavelength of 325 nm. The as-prepared SnO2 products show bands located at 497 nm and 528 nm. The stronger peak is present at 497 nm, which is due to the recombination of the electron-hole pairs, and the peak value in the spectra maybe also related to the lifetime of the excited electrons before recombination. The stronger the emission intensity of the PL spectrum, the larger the recombination rate of the electrons and holes, and then the lower the photocatalytic rate [17].   Figure 3f shows the UV-Vis absorption spectrum of the as-prepared SnO2. As we ca see from Figure 3f, the spectrum of the as-prepared SnO2 shows the highest peak at abou 290 nm, which indicate the as-prepared SnO2 can be excited by a small part of the visibl spectrum, and it is mainly excited by ultraviolet light. Further, to investigate the band ga of SnO2, the UV-Vis diffuse reflectance spectrum (DRS) was obtained with the help of th Kubelka-Munk formula (Equation (S1)) [18], indicating that the SnO2 displayed a ban gap value of 2.26 eV. Moreover, the valence band (VB) and conduction band (CB) positio was obtained from (Equations (S2)-(S4)), as proposed by Ralph G. Pearson in 1988 [19 Thus, the ECB values of SnO2 was calculated to be 0.65 eV, while the corresponding EV values was 2.91 eV, respectively.
From Figure 3f, we can see the band gap of the as-prepared SnO2 is 2.26 eV, whic indicates that the material is a wide band gap semiconductor material. However, the band gap is much shorter than those of 3.2 and 3.6 eV reported by other teams [20,21]. We ca infer that the as-prepared SnO2 may effectively degrade pollutants, because the wave length range of the samples with a narrow band gap is generally wide. In order to clarify the effect of the as-prepared SnO 2 products on the fluctuation of chemical bonds, the molecular vibration information of the specimens was characterized by a Raman spectrometer and the result is shown in Figure 3d. For the as-prepared nanoflower SnO 2 , the main peaks are concentrated at 621.177 cm −1 and 675.25 cm −1 . The peak at 621.177 cm −1 is attributed to the A 1g vibration mode of SnO 2 with a tetragonal rutile structure. The peak at 675.25 cm −1 is induced by the size effect of the very small SnO 2 nanocrystals and in fact it does not appear in bulk SnO 2 . PL measurement is powerful to study the recombination rate of the e − and h + pair in the samples, and the recombination rate of the e − and h + pair is proportional to the PL intensity. Figure 3e shows the emission spectra of the as-prepared SnO 2 products, and the PL spectrum is carried out in the wavelength range of 350-800 nm using an excitation wavelength of 325 nm. The asprepared SnO 2 products show bands located at 497 nm and 528 nm. The stronger peak is present at 497 nm, which is due to the recombination of the electron-hole pairs, and the peak value in the spectra maybe also related to the lifetime of the excited electrons before recombination. The stronger the emission intensity of the PL spectrum, the larger the recombination rate of the electrons and holes, and then the lower the photocatalytic rate [17]. Figure 3f shows the UV-Vis absorption spectrum of the as-prepared SnO 2 . As we can see from Figure 3f, the spectrum of the as-prepared SnO 2 shows the highest peak at about 290 nm, which indicate the as-prepared SnO 2 can be excited by a small part of the visible spectrum, and it is mainly excited by ultraviolet light. Further, to investigate the band gap of SnO 2 , the UV-Vis diffuse reflectance spectrum (DRS) was obtained with the help of the Kubelka-Munk formula (Equation (S1)) [18], indicating that the SnO 2 displayed a band gap value of 2.26 eV. Moreover, the valence band (VB) and conduction band (CB) position was obtained from (Equations (S2)-(S4)), as proposed by Ralph G. Pearson in 1988 [19]. Thus, the E CB values of SnO 2 was calculated to be 0.65 eV, while the corresponding E VB values was 2.91 eV, respectively.
From Figure 3f, we can see the band gap of the as-prepared SnO 2 is 2.26 eV, which indicates that the material is a wide band gap semiconductor material. However, the band gap is much shorter than those of 3.2 and 3.6 eV reported by other teams [20,21]. We can infer that the as-prepared SnO 2 may effectively degrade pollutants, because the wavelength range of the samples with a narrow band gap is generally wide.

Photocatalysis Performance
In order to evaluate the photocatalytic activity of the as-prepared SnO 2 , the photocatalytic performance of the aqueous MO solution was tested in the presence of the synthesized SnO 2 product under visible light irradiation. The results are shown in Figure 4a. The blank test shows that light has little influence on the MO aqueous solution. However, when the solution is irradiated for 120 min in the presence of the as-prepared SnO 2 product, the solution has almost no color. By processing the data, we obtained that the degradation rate of the as-prepared SnO 2 to MO is 90.6%.  Further, kinetic curves were provided, with correlation coefficients (r 2 ) over the valu of 0.90, to study the photocatalytic process of the MO, indicating that all catalysts matc the pseudo-first-order kinetic model in Figure 4b. The stability and reusability of the as prepared SnO2 products were investigated by reusing the products. From Figure 4c, w can see that the activity of the as-prepared SnO2 products did not decrease significantl after five cycles of MO photo degradation under visible light irradiation.

Reaction Mechanism
In order to study the degradation mechanism of the as-prepared SnO2 products, free radical-capture experiments were carried out. In the photocatalytic process, because th super-oxide radicals (•O2 − ), holes (h + ), and hydroxide radicals (•OH − ) are considered a the most active intermediate free-radical species, they can directly transfer the radical un paired electrons from the valence band maximum (VBM) to the identified lowest unoccu pied molecular orbital (LUMO) [22]. These kinds of radical scavenger experiments on th degradation of MO are carefully carried out to inspect the underlying photo-degradatio Further, kinetic curves were provided, with correlation coefficients (r 2 ) over the value of 0.90, to study the photocatalytic process of the MO, indicating that all catalysts match the pseudo-first-order kinetic model in Figure 4b. The stability and reusability of the as-prepared SnO 2 products were investigated by reusing the products. From Figure 4c, we can see that the activity of the as-prepared SnO 2 products did not decrease significantly after five cycles of MO photo degradation under visible light irradiation.

Reaction Mechanism
In order to study the degradation mechanism of the as-prepared SnO 2 products, freeradical-capture experiments were carried out. In the photocatalytic process, because the super-oxide radicals (•O 2 − ), holes (h + ), and hydroxide radicals (•OH − ) are considered as the most active intermediate free-radical species, they can directly transfer the radical unpaired electrons from the valence band maximum (VBM) to the identified lowest unoccu-pied molecular orbital (LUMO) [22]. These kinds of radical scavenger experiments on the degradation of MO are carefully carried out to inspect the underlying photo-degradation mechanism. A total of 0.3 mmol nitrogen (N 2 ), 0.3 mmol potassium iodide (KI), 0.3 mmol argentum nitricum (AgNO 3 ), and 0.3 mmol isopropanol (IPA) were added to the reaction system as the scavenger of •O 2 − , h + , e − , and •OH − , respectively. Figure 5a shows the change in the degradation kinetics in the presence of those above scavengers. We can see that under visible light irradiation, e − , •OH − , and h + play predominant roles in the reaction.

Reaction Mechanism
In order to study the degradation mechanism of the as-prepared SnO2 products, freeradical-capture experiments were carried out. In the photocatalytic process, because the super-oxide radicals (•O2 − ), holes (h + ), and hydroxide radicals (•OH − ) are considered as the most active intermediate free-radical species, they can directly transfer the radical unpaired electrons from the valence band maximum (VBM) to the identified lowest unoccupied molecular orbital (LUMO) [22]. These kinds of radical scavenger experiments on the degradation of MO are carefully carried out to inspect the underlying photo-degradation mechanism. A total of 0.3 mmol nitrogen (N2), 0.3 mmol potassium iodide (KI), 0.3 mmol argentum nitricum (AgNO3), and 0.3 mmol isopropanol (IPA) were added to the reaction system as the scavenger of •O2 − , h + , e − , and •OH − , respectively. Figure 5a shows the change in the degradation kinetics in the presence of those above scavengers. We can see that under visible light irradiation, e − , •OH − , and h + play predominant roles in the reaction. The reaction mechanism of the as-prepared SnO2 products in the degradation of MO dyes is showed in Figure 5b. When MO and the as-prepared SnO2 solutions are irradiated with visible light, because the band gap of the as-prepared SnO2 is 2.26 eV, the SnO2 product absorbs energy and the electrons in the valence band (VB) are excited to jump to the conduction band (CB), and photogenic holes h + are left. Because the nanoparticles are in The reaction mechanism of the as-prepared SnO 2 products in the degradation of MO dyes is showed in Figure 5b. When MO and the as-prepared SnO 2 solutions are irradiated with visible light, because the band gap of the as-prepared SnO 2 is 2.26 eV, the SnO 2 product absorbs energy and the electrons in the valence band (VB) are excited to jump to the conduction band (CB), and photogenic holes h + are left. Because the nanoparticles are in the aqueous phase and h + have strong oxidability, the H 2 O molecules adsorbed on the surface of the tin oxide can be oxidized to (•OH − ) with high activity and can be directly degraded by reaction with MO. The reduction potential of the photocatalyst at the conduction band (0.65 eV) is lower than the reduction potential of O 2 (−0.33 eV); so, the (•O 2 − ) production conditions cannot be met. The (•O 2 − ) cannot effectively decompose the organic dye, which is consistent with the captured experimental results. With their powerful oxidability, h + and (•OH − ) can effectively decompose the organic dyes [23]. The main equations are shown in (Equations (S5)-(S7)). Furthermore, due to the high surface area of the as-prepared SnO 2 , there are numerous active sites, which is good for adsorbing the active group.

Theoretical Calculation
In order to indicate the internal relationship between the photocatalytic activity and electronic structure of the as-prepared SnO 2 products, the electronic structures of the pure SnO 2 were calculated based on density functional theory (DFT), and the exchange interaction and related potential between the electrons were rectified by Becke's Three Parameter Hybrid Functional using the LYP Correlation Functional (B3LYP). The band structure, the total, and part of the density of states (TDOS/PDOS) of the rutile-type SnO 2 are shown in Figure 6.
In order to indicate the internal relationship between the photocatalytic activity electronic structure of the as-prepared SnO2 products, the electronic structures of the p SnO2 were calculated based on density functional theory (DFT), and the exchange in action and related potential between the electrons were rectified by Becke's Three Par eter Hybrid Functional using the LYP Correlation Functional (B3LYP). The band struct the total, and part of the density of states (TDOS/PDOS) of the rutile-type SnO2 are sho in Figure 6. In Figure 6a, the Fermi level is shown with a dashed line and assigned a zero on energy scale. The occupied state below the Fermi energy is the valence band, and the occupied state lying above the Fermi energy is the conduction band. The conduction b minimum and the valence band maximum are located at the same G point, which dem strate that SnO2 is a direct band-gap semiconductor. The Fermi level is close to the vale band, which means that the conductivity of SnO2 is lower. The calculated band gap v is 2.58 eV, which is less than the experimental value of 3.6 eV [24], but is very close to UV-Vis spectrum-measured band gap of the as-prepared SnO2 of 2.26 eV. The exci electrons in the valence band transfer to the conduction band through some dista which may inhibit the recombination of electrons and holes. The band gap value ca used to show the performance of the excited electrons. If the band gap of catalyst is sm when the matched or greater energy of the electromagnetic wave is close to the cata surface, the electron-hole pairs can be easily generated, which is good for the dye ph catalytic degradation. That is maybe the reason why the MO can be degraded under ble light by our as-prepared SnO2; in other reports, the dye degradation is under ultr olet light. Figure 6b shows the DOS and PDOS of the rutile-type SnO2. There are three par the total density state, from the −20 eV to −15.00 eV region, which is far from the Fe In Figure 6a, the Fermi level is shown with a dashed line and assigned a zero on the energy scale. The occupied state below the Fermi energy is the valence band, and the unoccupied state lying above the Fermi energy is the conduction band. The conduction band minimum and the valence band maximum are located at the same G point, which demonstrate that SnO 2 is a direct band-gap semiconductor. The Fermi level is close to the valence band, which means that the conductivity of SnO 2 is lower. The calculated band gap value is 2.58 eV, which is less than the experimental value of 3.6 eV [24], but is very close to the UV-Vis spectrum-measured band gap of the as-prepared SnO 2 of 2.26 eV. The exciting electrons in the valence band transfer to the conduction band through some distance, which may inhibit the recombination of electrons and holes. The band gap value can be used to show the performance of the excited electrons. If the band gap of catalyst is small, when the matched or greater energy of the electromagnetic wave is close to the catalyst surface, the electron-hole pairs can be easily generated, which is good for the dye photocatalytic degradation. That is maybe the reason why the MO can be degraded under visible light by our as-prepared SnO 2 ; in other reports, the dye degradation is under ultraviolet light. Figure 6b shows the DOS and PDOS of the rutile-type SnO 2 . There are three parts of the total density state, from the −20 eV to −15.00 eV region, which is far from the Fermi level, and is dominated by the O 2s 2 states. Due to the deep-level orbital role, the analysis of this region is unnecessary. Generally, the electrical properties of a semiconductor are determined by the electron states near the Fermi surface, and only the electrons near the Fermi surface can possibly jump into the nearby empty states. The −8.00 eV to 0 eV region is dominated by O 2p states and a few Sn 5s, Sn 5p states, and especially around the Fermi energy level, the DOS is mainly from the O 2p states. The conduction band is mainly dominated by Sn 5s Sn 5p and a few O 2p.

Conclusions
In this work, flower-shaped SnO 2 was successfully synthesized by a one-step hydrothermal method. The XRD, Raman, and SEM examinations revealed that the as-prepared SnO 2 products possess pure-phase, good crystallinity. In the visible light range, the degradation rate of MO was 90.6%, and the SnO 2 can keep a high degradation efficiency after five cycles, which indicate its potential application in eliminating organic pollutants. Through free-radical-capture experiments, we found that the electrons and holes play major roles in the degradation process. The band gap of the as-prepared SnO 2 measured by the UV-Vis spectrum was 2.26 eV, which is close to the calculated band gap value of 2.58 eV based on DFT. Such a flower-shaped structure is also expected to present good performance in gas sensing.
Author Contributions: T.S., X.C. conceived and prepared the flower-shaped SnO 2 ; X.C., J.D., J.N. and X.W. implemented the photocatalytic testing; T.S., X.C., Y.C. and H.K. analyzed the data and wrote original draft; F.Z., T.S. and X.C. provided funding acquisition; F.Z. and W.Z. revised the data and papers. All authors participated in analysis of the data and discussions of the results, as well as editing the manuscript. All authors have read and agreed to the published version of the manuscript.