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Vol.:(0123456789)1 3 Journal of Thermal Analysis and Calorimetry (2020) 140:2131–2142 https://doi.org/10.1007/s10973-019-08896-0 Physicochemical and photocatalytic properties of tin dioxide supported onto silica gel S. Khalameida1 · V. Sydorchuk1 · S. Levytska1 · N. Shcherban2 Received: 27 March 2019 / Accepted: 6 October 2019 / Published online: 15 November 2019 © Akadémiai Kiadó, Budapest, Hungary 2019 Abstract The samples containing 1–10% tin dioxide supported onto silica gel have been synthesized via precipitation or thermolysis of tin tetrachloride. The prepared samples have been characterized using DTA–TG, XRD, Raman and UV–Vis spectroscopy, TPD of ammonia, and low-temperature nitrogen adsorption–desorption. The supported samples have been tested as photo- catalysts in the process of rhodamine B degradation under visible irradiation. It has been established that the deposited phase is uniformly dispersed on the surface. Redshift of band gap is observed for the supported samples. Unlike a bulk SnO2, the supported samples exhibit photocatalytic activity under visible irradiation. Keywords Tin dioxide · Silica gel · Photocatalysis · DTA–TG · UV–Vis spectroscopy Introduction Tin dioxide SnO2 is a versatile material since it has wide numerous applications in a bulk and deposited state as cata- lyst, ion-exchanger, and material for gas sensors [1–3]. Being a semiconductor by its nature, it is a promising photocatalyst for processes of organic pollutants degradation [4–6]. The efficiency of these applications is determined by crystal and porous structure, surface design, and electronic character- istics of SnO2. The main disadvantages of tin dioxide as a photocatalyst are (i) large band gap (3.4–4.0 eV [1, 4, 6]); as a result, this material is active only under UV irradia- tion; (ii) preferably, a microporous structure, whereby a large portion of the surface is inaccessible for large molecules of organic substrates and diffusion difficulties slow down the photocatalytic transformations. There are several ways to overcome these shortcomings. Among them, introduc- tion of intrinsic (structural) and extrinsic (dopant) defects in “white” oxides results in the band gap narrowing and mani- festation of activity under visible irradiation [7]. The use of mechano- and sonochemical processes for these purposes simultaneously optimizes the porosity, creating a meso- macroporous structure (the most suitable structure for most adsorption and catalytic processes) as it was demonstrated for different perovskites and SnO2 [4, 5]. Another approach can be the deposition of an active phase onto the surface of mesoporous supports as it was shown for TiO2 [8–10], BaTiO3 [11], and heteropolycompounds [12, 13]. However, this method practically was not investigated for the prepara- tion of supported photocatalysts based on tin dioxide. The exceptions are the papers on photodegradation of rhodamine B (RhB) under UV irradiation using tin dioxide supported on porcine bone and SBA-15 [14, 15]. In the first case, it has been showed that about 97.3% of RhB can be decom- posed (based on bleaching of RhB solution degree) when the composition SnO2/porcine bone as a photocatalyst was used, while only 51.5% of RhB can be degraded using pure SnO2 nanoparticles. In the second case, the rate constant of RhB photocatalytic degradation is 3.8 × 10−5 s−1; in the third case, the rate constant achieves value of 1.5 × 10−4 s−1. Therefore, the possibility of pollutants photodegradation under visible irradiation using SnO2 embedded into structure of support, as it was done for titania [8–10] and mixed oxides [11, 16], was not studied. At the same time, it is known that deposition of tin diox- ide onto silica promotes to improvement of its catalytic per- formance in acid-catalyzed and oxidation processes [17–21]. Several methods for deposition of SnO2 on porous supports are known from the literature: sol–gel [22], polymeric [20], * S. Khalameida svkhal@ukr.net 1 Institute for Sorption and Problems of Endoecology, NAS of Ukraine, Naumova Street 13, Kiev 03164, Ukraine 2 L.V. Pysarzhevsky Institute of Physical Chemistry, NAS of Ukraine, Nauky Ave. 31, Kiev 03028, Ukraine http://crossmark.crossref.org/dialog/?doi=10.1007/s10973-019-08896-0&domain=pdf 2132 S. Khalameida et al. 1 3 template [21], and impregnation [17]. We used the simplest of them, namely impregnation of commercial silica gel and subsequent precipitation or thermolysis of prepared precur- sors. Silica being a dielectric was chosen as a support. The aim of this work is the study of crystal and porous structure, electronic characteristics of the supported SnO2/ SiO2 compositions of different SnO2 content and influence of these physicochemical properties on their photocatalytic activity under visible irradiation. Experimental Reagents and materials Silica gel KSKG (China) was used as a support. In order to increase the mesopore size, it was also subjected to hydro- thermal treatment (HTT) in a vapor phase at 150 °C for 3 h [23, 24]. Tin tetrachloride SnCl4·5H2O was used as a source of tin, aqueous ammonia solution—as a precipitant. Preparation of supported SnO2/SiO2 compositions Samples of SnO2/SiO2-supported compositions with differ- ent tin dioxide content, designated as XSn, where X = 1, 3, 5, 7 and 10, (the number in the sample designation corresponds to SnO2 content in mass%), were synthesized by deposition of tin dioxide on silica gel granules using incipient wetness impregnation. For this purpose, a fraction (0.5–2 mm) of silica gel was impregnated with an appropriate amount of SnCl4·5H2O aqueous solution, held for 1 h, then treated with 1 M NH4OH solution to form an insoluble SnO2, then dried at 110 °C and calcined in air at 450 and 550 °C (2 h). This is precipitation method (designation of samples − XSn- prec). In another procedure, the stage of precipitation using NH4OH was absent. This is thermolysis method (designation of samples − XSn-therm). For the purpose of activation, a precipitated sample containing 5% SnO2 was also milled in air for 0.5 h at 300 rpm (sample 5Sn-mill). For comparison, the supported sample was also prepared by direct dry milling of mixture of 5% SnO2 and silica gel under the same condi- tions (sample 5Sn-mill-mix). Milling was carried out using a planetary ball mill Pulverisette-7, premium line (Fritsch Gmbh) with a vessel of silicon nitride. Twenty-five balls from S3N4 with a 10 mm diameter (total ball mass − 40 g) were used as working bodies. Physicochemical measurements The crystal structure of the supported samples was studied by means of X-ray powder diffraction (XRD) using Philips PW 1830 diffractometer with CuKα radiation. The curves of DTA and TG were recorded using the Derivatograph-C apparatus (F. Paulik, J. Paulik, L. Erdey) in the temperature range of 20–1000 °C at a heating rate of 10° min−1. The ini- tial sample mass was about 200 mg, and the sensitivity was 50 mg. Raman spectra were recorded using spectrograph of Renishaw system (Ar laser, 514 nm). Strength (H0) and acid sites concentration in SnO2/SiO2 catalysts were deter- mined using an indicator method and the back titration of n-butylamine by hydrochloric acid in the presence of bro- mothymol blue, respectively, as well as using temperature- programmed desorption (TPD) of ammonia [19]. The porous structure of the initial silica gel and supported samples was studied using nitrogen adsorption–desorption technique. The isotherms were obtained using an automatic gas adsorption analyzer ASAP 2405 N (“Micromeritics Instrument Corp”) after outgassing the catalysts at 150 °C for 2 h. The specific surface area S, mesopore volume Vme, and micropore vol- ume Vmi were calculated from these isotherms using BET, BJH, and t-plot methods, respectively. The total pore volume VΣ was determined by impregnation of the samples, which were preliminarily driedat 150 °C, with liquid water (so- called incipient wetness method [25]). Macropore volume Vma was calculated as the difference between VΣ and sorp- tion pore volume Vs. The latter one was determined from the isotherms at nitrogen relative pressure close to 1.0. The mesopore size dme was calculated from the curves of pore size distribution (PSD) plotted using the desorption branches of isotherms. Diffuse reflectance UV–Vis spec- tra of the powders were registered on Lambda 35 UV–Vis spectrometer (PerkinElmer Instruments). The band gap was determined using Planks formula. Photocatalytic testing Photocatalytic degradation was performed in a glass reac- tor under visible irradiation. LED Cool daylight lamp, Philips (100 W) possessing emission spectra exclusively in the visible range with a broad maximum in the region of 500–700 nm and a local maximum around 440 nm, was used as an irradiation source. The dye rhodamine B (RhB) in the form of 1.5 × 10−5 mol L−1 solution was used as a pollutant [16]. The main absorption bands λmax in the spectra of substrate is 553 nm. The catalyst dose was 1 g L−1 (80 mg of catalysts and 80 mL of solution). Duration of dark adsorption to establish of equilibrium was 60 min. The initial solution and solutions after dye adsorption and degradation for 30–600 min were analyzed spectrophotometrically at λmax (Lambda 35, Perkin Elmer Instruments) after centrifugation of the reaction mixture (10 min at 8000 rpm). The calculation of photodegrada- tion rate Kd was based on the temporal changes of the dye concentration after reaching the adsorption equilibrium. The total organic carbon (TOC), which is a measure of dye 2133Physicochemical and photocatalytic properties of tin dioxide supported onto silica gel 1 3 mineralization [26], for selected solutions, was determined using a Shimadzu TOC analyzer (model 5050A). Results and discussion Thermogravimetric measurements In order to determine the temperature of thermodestruc- tion of SnCl4·5H2O resulting in tin dioxide formation, the DTA–TG curves for bulk salt as well as for compo- sitions precursors prepared on its basis were registered. Obviously, SnCl4·5H2O is decomposed in air according to Eq. (1): Theoretical mass loss for this process is 54.1% w/w. Experimental value of mass loss calculated from DTA–TG curves of bulk SnCl4·5H2O is 55.5% w/w. At the same time, this process takes place in a wide temperature range—from 100 to 450 °C (Fig. 1a). It can be divided into two stages: (i) sharp stage at 100–200 °C with an intensive endoeffect at about 150 °C when mass loss is 47.9% w/w (crystallization water) and (ii) slow stage at 200–450 °C when mass loss is 7.6% w/w. It should be noted that simi- lar curves were obtained for hydrous copper, cobalt, and manganese chlorides [27]. On the other hand, there is an endoeffect at 20–200 °C with a maximum at 115 °C, which is accompanied by release of water from the pores, for the initial porous silica and supported samples, namely their precursors (Fig. 1b, c, respectively). These endoeffects are characteristic for porous materials including supported compositions based on porous carriers [11–13, 16, 28, 29]. Therefore, the first stage of SnCl4·5H2O decomposition for supported precursors is over- lapped with removal of this physically bound water from the pores of silica gel. At the same time, removal of surface OH groups additionally occurs on the second stage which is the characteristic for silica [23]. This value is 0.72% w/w (Table 1). Therefore, mass loss in the range of 200–450 °C for precursors is determined by the tin chloride decomposi- tion process and the removal of hydroxyl groups. The first component depends on the precursor composition, i.e., content of SnCl4, and the second one is approximately constant—about 0.72% w/w: where X—SnO2 content in composition. It can be seen that Δm200–450_therm values, determined from the experimental data (Table 1, column 6), are (1)SnCl4 ⋅ 5H2O = SnO2 + 4HCl + 3H2O (2) Δm200−450_therm = X ⋅ 7.6∕100 + (1 − X) ⋅ 0.72∕100 (%w/w), well-consistent with those ones calculated by the formula (2). Precursors, prepared with a precipitation stage, contain tin dioxide and ammonium chloride which are formed in the pores of silica gel according to the equation: In line with it, mass loss in the range of 200–450 °C for these precursors is determined by the ammonium chloride sublimation [30] and the removal of hydroxyl groups both for silica gel and precipitated tin dioxide [1, 4, 5]. The NH4Cl content in the products of the reaction (3) is about 58.6% w/w and mass loss in the range of 200–450 °C for precipitated SnO2 is 4.86% [4]. Therefore, total mass loss in the range of 200–450 °C for the precursors prepared via precipitation can be calculated as follows: The experimental data presented in column 7 of Table 1 are in a good agreement with those ones calculated by the formulas (2) and (4). Based on the results of thermogravimetric measure- ments, the first calcination temperature of precursors was determined as 450 °C. The second calcination temperature of 550 °C was chosen since content of surface OH groups was reduced by 11% compared with the samples calcined at 450 °C for silica gel as shown in [21] and by 8% for tin diox- ide xerogel [4] according to the data of DTA–TG. Therefore, use of the samples calcined at these temperatures makes it possible to establish the influence of the content of OH groups on the photocatalytic activity. It should also be noted that the indicated values of temperature (450 and 550 °C) correspond to optimal conditions for regeneration of oxide catalysts using oxygen and air, respectively [31]. Crystal structure Crystal structure of tin dioxide in composition is formed during calcinations of precursors. XRD patterns for some supported samples as well as for pure SnO2 calcined at 550 °C are depicted in Fig. 2. As can be seen, positions of the diffraction peaks corresponding to the planes (110), (101), (200), and (211) are attributed to tetragonal modifica- tion of cassiterite/rutile (JCPDS N 41-1445). The intensity of all the peaks is predictably increased with an increase in the content of tin dioxide. The reflexes also differ in width, which is a measure of crystallinity (crystallite size Dhkl), and I110/I101 ratio. Since reflex with maximal intensity (110) is overlapped with halo characteristic for amorphous silica, calculation of crystallites size was performed using reflex attributed to the plane (101) (D101). These parameters are determined by SnO2 content in composition and calcinations (3)SnCl4 + 4NH3 + 2H2O = SnO2 + 4NH4Cl (4) Δm200−450_prec = X ⋅ 58.6∕100 + X ⋅ 4.86∕100 + (1 − X) ⋅ 0.72∕100 2134 S. Khalameida et al. 1 3 Fig. 1 a DTA, TG, DTG curves for SnCl4·5H2O. b DTA, TG, DTG curves for the initial silica gel. c DTA, TG, DTG curves for a precursor containing 10% SnCl4 Mass loss/% 0 12 24 36 48 60 200 400 Temperature/°C 600 800 TG DTG DTG/mg min–1 DTG/mg min–1 DTG/mg min–1 DTA/µV mg–1 DTA/µV mg–1 DTA/µV mg–1 DTA 0.20.6 0.5 0.4 0.3 0.2 0.1 0.0 – 0.1 0.0 – 0.2 – 0.4 – 0.6 – 0.8 – 1.0 – 1.2 Mass loss/% Temperature/°C Mass loss/% Temperature/°C 0.0 – 0.1 – 0.2 0 1 2 3 4 5 6 200 400 600 800 0.0 – 0.1 – 0.2 0 1 2 3 4 5 6 7 200 400 600 800 TG DTG DTA TG DTG DTA 0.45 0.40 0.35 0.30 0.25 0.20 0.15 0.10 0.05 0.45 0.40 0.35 0.30 0.25 0.20 0.15 0.10 0.05 0.50 (a) (b) (c) 2135Physicochemical and photocatalytic properties of tin dioxide supported onto silica gel 1 3 temperature which is also quite expected (Table 2). Thereby, D101 value is increased as a result of enrichment of the com- position with tin dioxide and an elevation in the calcinations temperature. On the other hand, calculated crystallite size for the supported samples is 2–3 times smaller than for bulk SnO2 calcined at 450–550°C. It indicates well-dispersion of the deposited phase on the support surface as it was pre- viously observed for supported titania [8–10] as well as for mixed oxide compositions [11, 32]. A feature of the supported samples also is an increase in I110/I101 value (Table 2, column 5) compared to that for pure SnO2 prepared under the same conditions as well as described in the literature [1, 6, 33]. It can also be seen that this value is larger for the samples prepared via precipitation and decreases when calcinations temperature is elevated. This parameter characterizes the surface orientation of defined planes which can be very important for catalytic processes [34, 35] including photocatalytic transformation [36]. Particularly, the ratio of different crystallographic planes (surface content) and, as a result, catalytic proper- ties, could be changed by various types of treatment for vanadium–molybdenum oxides [35, 37]. These are so-called structural-sensitive reactions [1, 36]. Raman spectra confirm low crystallinity for deposited SnO2 phase which can be seen from the comparison of the spectra registered for bulk and supported tin dioxide (Fig. 3) As can be seen (Fig. 3, spectra b, c), there are low-inten- sity bands centered at 795 and 590 cm−1 which attributed to SnO2 nanoparticles with a size less than 10 nm [17, 38, 39]. Besides, broad bands at 300–550 cm−1, which can be a Table 1 Results of thermogravimetric measurements for some SnO2/ SiO2 samples N Synthesis conditions Temperature of effect from DTG curve/°C Δm20–200/% w/w Δm200–450/% w/w Δm450–550/% w/w 1 Initial silica gel 113 3.71 0.72 0.19 2 3Sn without precipitation 110 3.88 0.93 0.20 3 5Sn without precipitation 115 3.60 1.13 0.21 4 5Sn with precipitation 118 4.11 3.94 0.26 5 7Sn without precipitation 113 3.69 1.31 0.22 6 10Sn without precipitation 118 3.53 1.48 0.24 7 10Sn with precipitation 121 4.55 6.88 0.29 8 Precipitated SnO2 128 13.01 4.86 0.48 1200 900 600 300 0 3300 2200 1100 0 3300 2200 1100 0 3300 2200 1100 0 17700 11800 5900 0 10 15 20 25 30 35 40 45 50 55 60 a b c d e 110 2θ/° 101 In te ns ity /a .u . Fig. 2 XRD patterns for the supported samples after calcinations at 450 °C: 3Sn_prec (a), 5Sn_therm (b), 5Sn_prec (c), 10 Sn_prec (d), bulk precipitated SnO2 (e) Table 2 Some parameters of crystal structure Sample Method of prepara- tion Temperature/°C D101/nm I110/I101 3Sn Precipitation 450 5.0 1.69 550 5.8 1.55 5Sn Precipitation 450 6.0 1.88 550 7.1 1.70 Thermolysis 450 7.3 1.58 550 10.0 1.50 7Sn Precipitation 450 7.5 1.55 550 8.8 1.45 10Sn Precipitation 450 10.4 1.52 550 11.0 1.40 Thermolysis 550 11.2 1.34 100Sn Precipitation 450 12.0 1.05 550 15.6 1.11 2136 S. Khalameida et al. 1 3 superposition of several bands characteristic for tin dioxide [39], are presented in Fig. 3 (spectra b and c). Similar spectra were also obtained for samples containing 5–10% of SnO2 incorporated into structure of dealuminated zeolite ß [18]. It should be noted that there are no bands for amorphous silica in this range [40]. Porous structure Parameters of porous structure for initial silica gel and supported samples were calculated from nitrogen adsorp- tion–desorption isotherms, examples of which are shown in Fig. 4. All of them belong to type IV according to IUPAC classification which is characteristic for mesoporous materi- als. The curves of pore size distribution PSD (inset of Fig. 4) also indicate it. Thus, initial silica gel contains mesopores with a size in the range of 2–14 nm and maximum on PSD curve about 7.8 nm but does not contain micro- and macropores (Table 3). Deposition of tin dioxide on siliceous surface predictably leads to some decrease in the specific surface area, total pore volume and mesopore volume but their size remains almost the same (inset of Fig. 4, Table 3, columns 7). Silica gel subjected to HTT has a smaller specific sur- face area but larger mesopores, namely 9.8 nm. Therefore, the supported sample based on the hydrothermally treated silica gel also has a smaller specific surface area and larger mesopores. Maximum reduction in the specific surface area 4000 3000 2000 1000 0 750 500 250 0 1000 750 500 250 0 500 1000 Raman shift/cm–1 1500 2000 0 a In te ns ity /a .u . b c Fig. 3 Raman spectra for bulk tin dioxide (a) and supported samples containing 5 (b) and 10% (c) of SnO2 Fig. 4 Nitrogen adsorption– desorption isotherms and PSD curves for the initial silica gel and some supported samples 700 a/ cc g –1 dv /d r 600 500 400 300 200 100 0 0.0 0.2 0.4 0.6 0.8 P/P0 1.0 0 5 10 15 r /nm 20 0.035 0.030 0.025 0.020 0.015 0.010 0.005 0.000 Initial silica gel 1Sn-prec 5Sn-prec 5Sn-mill 2137Physicochemical and photocatalytic properties of tin dioxide supported onto silica gel 1 3 and pore volume is observed for the milled sample 5Sn- mill (Fig. 4, Table 3, column 4) which is consistent with the results obtained for a milled silica gel of different porous structure [23, 41]. UV–Vis spectra Diffuse reflectance UV–Vis spectra for some supported samples with different SnO2 content are presented in Fig. 5. One can see that they differ in the position of the absorp- tion edge λ and the magnitude of absorption in the visible region. It is important that significant redshift of absorption Table 3 Parameters of porous structure of supported samples Sample Method of preparation Temperature/°C S/m2 g−1 VΣ/cm3 g−1 Vme/cm3 g−1 dme/nm SiO2 – – 371 0.97 0.98 7.8 1Sn Precipitation 450 365 0.92 0.92 7.8 Thermolysis 450 367 0.93 0.92 7.8 3Sn Thermolysis 450 362 0.90 0.90 7.8 550 359 0.91 0.90 7.8 5Sn Thermolysis 450 357 0.93 0.92 7.9 550 355 0.94 0.93 7.9 Precipitation 450 360 0.91 0.91 7.8 Precipitation 550 354 0.90 0.89 7.8 5Sn-HTT Precipitation 450 320 0.90 0.89 9.5 5Sn-mill Precipitation – 198 0.50 0.48 7.9 5Sn-mill-mix Precipitation – 301 0.74 0.73 7.8 7Sn Thermolysis 450 350 0.90 0.89 8.1 550 345 0.89 0.89 8.0 10Sn Thermolysis 450 344 0.88 0.87 8.1 550 340 0.87 0.87 8.1 Fig. 5 UV–Vis spectra for some supported samples 1.0 0.5 0.4 1Sn-prec 10Sn-prec 5Sn-prec 5Sn-therm 0.3 0.2 350 400 450 K – M in de x K – M in de x 0.9 0.8 0.7 0.6 0.5 0.4 0.3 0.2 0.1 200 300 400 500 Wavenumber/nm Wavenumber/nm 2138 S. Khalameida et al. 1 3 edge is observed for the supported samples compared with bulk SnO2. Thus, λ is 364–341 nm for bulk tin dioxide [4, 5], while its value is shifted toward 407–356 nm for the precipi- tated samples containing 1–10% SnO2 (Table 4). It cor- responds to narrowing the band gap Eg from 3.64 eV for bulk SnO2 [4, 5] to 3.05–3.48 eV for the supported sam- ples (Table 4, columns 4, 5). Such an effect was earlier described for silica supported TiO2 photocatalysts [8, 9] and for SnO2–TiO2 solid solution embedded into SBA-15 structure [42]. But it was not observed for deposited SnO2, as a rule [15, 21, 42]. Similar spectrum is given only in the paper [18] for sample containing 10% SnO2 incorporated into the structure of dealuminated ß zeolite. However, the authors do not discuss it. Moreover, co-precipitated (but not supported) SnO2–SiO2 samples prepared by a sol–gel method and additionally calcined at 800 °C showed red- shift in UV–Vis spectra with an increase in SnO2 content from 1 to 10% [43]. It is noteworthy that observed redshift of absorption edge for the precipitated samples is significantly larger than for the samples prepared via thermolysis (Fig. 5, Table 4). An observed redshift effect can be associated with different surface orientations of deposited crystallites compared to crystallites in bulk SnO2 (Table 2, increase in I110/I101 ratio from 1.05–1.10 to 1.34–1.88). It is in a good agreement with the results described for TiO2 in [30]; UV–Vis spectroscopy measurements of anatase crystals with different surface orientations have revealed differ-ences in the band gap indicating the upward shift in the conduction band minimum for anatase (101) and (100) compared to (001) surfaces. A feature of the spectrum for 5Sn-prec-450 is the pres- ence of another absorption edge in the long-wavelength region—about 540 nm (selected fragment in Fig. 5). As a result, the occurrence of an additional level in the forbidden zone of SnO2 is possible. Similarly, a new metastable surface phase exhibits with much reduced band gap from that one of bulk TiO2 (about 2 eV) on the rutile TiO2 (011) surface [36]. Photocatalytic tests It is well-known that the photocatalytic properties of semi- conductors depend on their electronic characteristics, crystal and porous structure, specific surface area and degree of hydroxylation, and therefore, adsorption capacity toward the substrate [7, 26]. It is also natural that the first stage of Table 4 Electronic and photocatalytic properties of the supported samples *n.d not done N SnO2 content/% Preparation conditions λ/nm Eg/eV a/% Kd 105/s−1 Bleaching degree/% 1 1Sn Precipitation, 450 °C 392 3.16 40 5.6 84 2 3Sn Precipitation, 450 °C 399 3.11 45 7.2 88 3 5Sn Precipitation, 450 °C 407 3.05 56 9.1 92 4 5Sn Precipitation, 550 °C 388 3.20 40 7.0 84 5 5Sn Thermolysis, 450 °C 375 3.31 44 6.1 80 6 5Sn Thermolysis, 550 °C 365 3.40 37 5.1 76 7 5Sn Precipitation, 450 °C, SiO2 treated via HTT *n.d – 33 3.9 63 8 5Sn Precipitation, 450 °C MChT *n.d – 32 3.1 68 9 5Sn Precipitation, 450 °C + SiO2 MChT *n.d – 37 0.1 11 10 7Sn Precipitation, 450 °C 367 3.38 41 5.8 82 11 10Sn Precipitation, 450 °C 364 3.41 25 3.1 59 12 10Sn Thermolysis, 450 °C 356 3.48 36 2.0 44 13 100Sn Precipitation, 450 °C 341 3.64 30 – – 0.30 dV H C l/d T 0.25 0.20 0.15 0.10 0.05 0.00 0 100 200 300 400 500 600 700 1.0 T C D s ig na l/a .u . 0.8 0.6 0.4 0.2 0.0 Temperature/°C Fig. 6 NH3-TPD profile for the sample 5Sn_prec-450 2139Physicochemical and photocatalytic properties of tin dioxide supported onto silica gel 1 3 catalysis is the adsorption of reagents on the catalyst surface. Based on the fact that the tested dye has a basic nature, it was important to evaluate the acidic properties of the photocata- lyst surface. Using the indicator method, it was established that the supported samples have concentration of acid sites within 1.58–1.68 mmol g−1 or 4.3–4.6 μmol m−2. The value of Gammet function H0 is about − 3, i.e., acid sites are weak. At the same time, ammonia TPD profile obtained for the sample 5Sn_prec-450 (Fig. 6) shows the value of acid sites concentration equal to 1.51 mmol g−1 which is close to the above indicated range. Temperature of the maximum is at 172 °C which also corresponds to weak acid sites. It should be noted that similar results were obtained for SnO2–SiO2 xerogels containing 3–9% w/w of tin dioxide [44], while content of acid sites for bulk SiO2 and SnO2 is 1.10 and 0.38 mmol g−1 or 3.0 and 6.5 μmol m−2, respectively. As can be seen, the supported samples have close acidity val- ues, but higher than the values based on the additivity rule. Therefore, the difference in RhB adsorption during dark stage a (%), determined as the ratio of optical density of RhB solution before and after dark stage, depends primarily on the value of the specific surface area and, possibly, on the surface content of (110) plane (I110/I101 ratio). At the same time, band gap (namely < 3.26 eV) and absorption value in the region with wavelength > 380 nm for the photocatalyst determine its activity under visible irradia- tion [7]. As shown in Table 4, some of the prepared samples (namely NN 1-4) meet these conditions. Consequently, the appearance of an electron–hole pair on the catalyst surface due to the action of photons of visible light is possible in this case. It results in initiation of a conventional photocatalytic process. As a result, these samples showed high activity in the process of RhB degradation. The latter is evidenced by the character of the changes in the RhB spectrum during its degradation in the presence of the samples of different activity (Fig. 7a, b). The similar spectra were also obtained for other photocatalysts. It should be noted that bulk pre- cipitated SnO2 prepared under the same conditions does not show noticeable activity when it is exposed to visible light [4] which is associated with a high band gap value (3.41 eV) and minimal absorption in visible region for this sample. It is well-known that RhB photodegradation in the pres- ence of tin dioxide can occur by two pathways [4–6]: as de- ethylation process in a stepwise manner (with the formation of three intermediates from RhB to Rh110) or as a direct cleavage of the chromophore rings. A gradual blueshift of the band at 553 nm on the spectrum of the RhB solution is observed in the first case and the reduction in its intensity without shift takes place in the second case. As shown in Fig. 7a, b, mixed mechanism is realized in this case as it was described earlier for doped and milled SnO2 [4, 5]: (i) decrease of the intensity band at 553 nm occurs for 60 min which corresponds to direct degradation of RhB [16]; (ii) shift of this band toward 498–500 nm for 180 min which is accompanied by complete de-ethylation of RhB to Rh110; (iii) decrease in intensity of the band at 498–500 nm which is associated with degradation of Rh110 with cleavage of the chromophore rings (for duration > 180 min). The photocatalytic tests showed that the degradation of RhB under visible irradiation (as dye bleaching) using the supported samples proceeds according to first-order kinetic equation (Fig. 8) with a correlation coefficient R2 = 0.93–0.99, which is agreed with literature data [4–6, 16]. The photodegradation rate constants Kd were calculated from the slopes of the plots ln(D/D0) − τ (where D and D0 are values of optical density of RhB solution after time τ and dark adsorption, respectively). One can see (Table 4) that photocatalytic activity, the measure of which is the Kd magnitude, for the precipitated samples is increased with an increase in SnO2 content up to 5% and decreased with a further increase in its content up to 10%. In general, it corre- lates with the electronic characteristics of the photocatalysts: 0.3 D 0.2 0.1 0.0 400 500 600 0.30 0.25 0.20 0.15 0.10 0.05 0.00 200 300 400 500 Wavenumber/nm 600 700 0 1800 s 3600 s 7200 s 10,800 s 18,000 s 27,000 s 36,000 s 0 1800 s 3600 s 7200 s 10,800 s 18,000 s 27,000 s 36,000 s RhB initial D Wavenumber/nm (a) (b) Fig. 7 a Spectra of RhB depending on degradation time in the pres- ence of 5Sn_prec_450. b Spectra of RhB depending on degradation time in the presence of 3Sn_prec_450 2140 S. Khalameida et al. 1 3 the samples containing 1–5% SnO2 have Eg = 3.05–3.20 eV, i.e., less than 3.26 eV and absorption in visible region for them is 25–40%, while these parameters are 3.35–3.41 eV and 15–20%, respectively, for samples containing 7–10% SnO2 (Table 4). Therefore, generation of an electron–hole pair is possible in the first case. Moreover, the number of active sites should be increased with an increase in SnO2 content. In the second case, the samples also exhibit suffi- cient photocatalytic activity. The latter can be explained as follows. The spectrum of RhB absorption is overlapped in a wide region with the emission spectrum of a lamp—illumi- nation source; the maxima are located at 553 and 565 nm, respectively. Therefore, the absorption of visible light and the direct excitation of RhB molecules are very likely. Sub- sequent injection of an electron from the excited RhB mol- ecules into the conduction band of a photocatalyst occurs. It is so-called photosensitization contributing the initiation of photocatalytic process [26, 45]. Obviously, this mechanism determines the photocatalytic activity of the samples pos- sessing Eg > 3.26 eV, although it can also contribute to the activityof the samples with Eg < 3.26 eV. For the most active sample, namely containing 5% SnO2, the influence of preparation conditions on the photocatalytic activity was studied. One can see that the samples prepared via thermolysis have lower activity, and it is directly related to the larger Eg value and lower absorption for visible irra- diation (Table 4). An increase in calcinations temperature for the samples prepared via precipitation and thermolysis from 450 to 550 °C results in a slight decrease in activity. It can be explained by a decrease in concentration of the sur- face OH groups which influence on photocatalytic processes. As mentioned above, their content according to TG data is reduced by approximately 10% in this temperature range. It is also important to evaluate the effect of other phys- icochemical characteristics on photocatalytic properties. Particularly, it is difficult to associate an increase in crys- tallite size D101, which is observed with increasing SnO2 content (Tables 2, 4), with activity. Here, it is important to have an actual increase in the content of the active phase, as established for 5.8–17.7% of SnO2 embedded into SBA- 15 under UV irradiation [15]. At the same time, surface exposition of certain crystallographic planes can affect the dye adsorption and through it on photocatalytic activity. On the contrary, the dependence of the activity on the specific surface area was precisely established earlier [1, 7]. At the same time, the tested samples have close S values (Table 3). In order to reduce the specific surface area of the support, and therefore the supported sample, silica gel was subjected to HTT. Photocatalyst prepared on the basis of a hydrother- mally treated support showed significantly lower activity (Table 4, sample 7). Finally, an attempt to activate the most effective cata- lyst (sample 3) by milling, as was done for bulk SnO2 [5], was made. As shown in Table 4 (sample 8), positive effect was not achieved. Furthermore, the samples prepared via milling of tin dioxide and silica gel mixture (without pre- liminary deposition of SnO2 on silica gel) was practically inactive, although the adsorption of RhB was quite large (sample 9). It can be explained as follows. Under milling, SnO2 (semiconductor) is partially (sample 8) or completely (sample 9) coated by a silica layer (dielectric). As a result, the active sites of SnO2 are blocked. Taking into account a large excess of silica in relation to SnO2, as well as the dif- ference in the hardness of the components (Mohs hardness of amorphous silica and SnO2 is 5 and 6.5, respectively) [46, 47], “smearing” of amorphous silica on SnO2 nano- crystallites is possible. Similar results were described when “core–shell” particles were formed during dry milling of cerium and molybdenum oxides mixtures [48]. As shown in Table 4 (column 8) bleaching degree of RhB under visible irradiation for the most active sample reaches 88–92% which is comparable with ones obtained in [14] for the same dye using the SnO2/porcine bone photocatalyst but under UV irradiation. At the same time, the mineraliza- tion degree of a dye is even more important indicator for evaluating of the photocatalyst efficiency [26]. This param- eter, calculated as the degree of total organic carbon (TOC) reduction, is 40 and 75% for sample containing 5% SnO2 calcined at 450 °C and prepared via thermolysis and pre- cipitation, respectively. Conclusions Using thermogravimetric analysis, it has been established that hydrous tin tetrachloride is transformed into tin dioxide in silica gel pores at 450 °C. The choice of the temperature of the precursor transformation into the oxide composition 0.5 In /D /D 0 0.0 – 0.5 – 1.0 – 1.5 – 2.0 – 2.5 – 3.0 – 3.5 – 4.0 0 5000 10000 τ /s 15,000 20,000 25,000 30,000 35,000 40,000 SnO2 bulk 1Sn/SiO2 5Sn/SiO2 10Sn/SiO2 Fig. 8 Kinetic curves of RhB degradation for some tested samples 2141Physicochemical and photocatalytic properties of tin dioxide supported onto silica gel 1 3 is based on these results. Also, it has been estimated the degree of surface dehydroxylation within the range of 450–550 °C. Deposition of 1–10% tin dioxide onto silica gel contributes to its dispersion on the surface; crystallite size of SnO2 is decreased from 12 nm for a bulk sample to 5–10 nm (depending on SnO2 content) for the supported samples. Besides, surface re-orientation of the crystallites occurs: content of (110) plane, expressed as I110/I101 ratio, is increased by 45–80%. Moreover, narrowing the band gap from 3.64 eV for bulk SnO2 to 3.05–3.48 eV for the samples containing 1–10% SnO2 is observed. As a result, the sup- ported samples, in contrast to the bulk SnO2, exhibit photo- catalytic activity under visible irradiation. The precipitated samples are more effective compared with the samples pre- pared by thermolysis. An increase in calcinations tempera- ture decreases the photocatalytic activity due to a reduction in the specific surface area and surface dehydroxylation. 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Publisher’s Note Springer Nature remains neutral with regard to jurisdictional claims in published maps and institutional affiliations. https://doi.org/10.1007/s10973-019-08479-z https://doi.org/10.1007/s10973-019-08479-z https://doi.org/10.1002/masy.200850519 https://doi.org/10.1002/masy.200850519 Physicochemical and photocatalytic properties of tin dioxide supported onto silica gel Abstract Introduction Experimental Reagents and materials Preparation of supported SnO2SiO2 compositions Physicochemical measurements Photocatalytic testing Results and discussion Thermogravimetric measurements Crystal structure Porous structure UV–Vis spectra Photocatalytic tests Conclusions References
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