# Effect of Fe Doping on Photocatalytic Dye-Degradation and Antibacterial Activity of SnO2 Nanoparticles

Authors: T. Preethi; K. Senthil; M. P. Pachamuthu; R. Balakrishnaraja; B. Sundaravel; N. Geetha; Stefano Bellucci
Journal: Adsorption Science & Technology
 (2022)

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## Abstract

A simple hydrothermal method is utilized to synthesize iron-doped tin oxide nanoparticles (Fe-SnO2 NPs) at various doping concentrations. The structural characterization using XRD, Raman, and FTIR measurements confirmed the incorporation of Fe ions into the SnO2 lattice without any deviation in the tetragonal crystal system of SnO2 nanoparticles. SEM and HRTEM images show the spherical-shaped nanoparticles with agglomeration. The values of interplanar spacing (d-value) calculated from the HRTEM lattice are consistent with the XRD results. Further, optical analysis revealed a red shift in the optical absorption band and a decrease in the band gap energy with an increase in Fe-dopant concentration. The decrease of PL emission peak intensity with Fe doping revealed the generation of singly charged oxygen vacancies. The H2O2-assisted photocatalytic degradation efficiency of Fe-SnO2 NPs investigated against crystal violet dye indicated an efficiency of 98% for 0.05 M Fe-SnO2 NPs within 30 minutes under visible light illumination. In addition, the effects of pH, scavengers, and reusability of the catalyst are tested. The antibacterial behavior of Fe-SnO2 NPs against Escherichia coli is examined by using the colony count method, and the inhibition rate was found to be 49, 65, 70, and 78% for pure, 0.01, 0.03, and 0.05 M Fe-SnO2 NPs, respectively.


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## Body

## 1. Introduction

Globally, the release of effluents into the environment has been increased due to rapid industrialization, which may cause adverse effects on the ecological and aquatic environment. Dyes are a major source of pollution since they are utilized in a variety of sectors, including food, cosmetics, plastic, leather, paper, and textiles. The presence of complex aromatic structures in the dyes makes them difficult to degrade, which may cause color changes, odor changes, excessive nutrients, biocontamination, and underoxygenation in the aquatic environment [1, 2]. Therefore, it is highly essential to remove these contaminants from wastewater to achieve a concentration below the level accepted for environmentally safe disposal. Adsorption [3–5], biodegradation [6], photocatalysis [7, 8], ultrasound-assisted method [9], and ozonation [10] are the procedures used to remove these contaminants from wastewater. Among these methods, considerable attention has been paid on photocatalytic degradation due to its ability to produce highly reactive radicals for efficient removal of contaminants [11]. Semiconducting metal oxide nanoparticles, especially SnO2, have gained significant attention due to their unique properties such as good photochemical stability, high oxidizing power, cost effectiveness, and environment friendly nature [12]. Although it has several advantages, the main drawback of using SnO2 nanoparticles for photocatalytic degradation is faster recombination rate of electron-hole pairs. The promising solution to overcome this problem is to introduce a metal dopant into the SnO2 lattice, which will increase the visible light absorption ability by decreasing the band gap of SnO2. Baig et al. observed that doping SnO2 nanoparticles with Zn and Y increased their photocatalytic efficiency towards methylene blue [13, 14]. Sathishkumar and Geethalakshmi have reported the synthesis of Cu:SnO2 nanoparticles with improved antibacterial and photocatalytic activity under ultraviolet light [15]. Ragupathy and Sathya have shown Ni doping in SnO2 nanoparticles by chemical precipitation method for increasing the photocatalytic degradation of brilliant green dye to a considerable extent [16]. The effect of Fe doping and surfactant on the photocatalytic behavior of SnO2 nanoparticles is studied by Sujatha et al. [17]. Among the various transition metal atoms, Fe seems to be a suitable dopant. The presence of half-filled electronic structure in Fe tends to narrow down the band gap by forming new intermediate energy levels, and electron-hole pair recombination rate is minimized by the trapped photogenerated electrons [18, 19]. Hence, in this study, pure and Fe-SnO2 NPs are synthesized at various Fe concentrations (0.01, 0.03, and 0.05 M) by using a simple surfactant-free hydrothermal technique. The structure, surface morphology, composition, optical, photocatalytic dye-degradation, and antibacterial properties are investigated systematically. The investigations revealed an enhancement in the photocatalytic degradation efficiency and antibacterial activity with increasing Fe-dopant concentration.


## 2. Experimental Procedures

### 2.1. Fe-SnO2 Nanoparticle Synthesis

Tin (IV) chloride pentahydrate (SnCl4·5H2O) and ferric chloride hexahydrate (FeCl3.6H2O) are used as metal precursors; sodium hydroxide (NaOH) is used as a precipitating agent; methyl alcohol (CH3OH) and double deionized water are used for washing of the obtained precipitates. Double-distilled water is used as a solvent for all the synthesis process. All the chemicals are utilized with no further purification. SnCl4·5H2O (0.4 M) and FeCl3.6H2O at various concentrations (0.01, 0.03, and 0.05 M) are dissolved in 50 mL of double-deionized water in a conventional synthesis. The pH of precursor solution was adjusted to 10 by adding NaOH solution, and final solution is agitated at room temperature for 30 min. The contents are then transferred to an autoclave and hydrothermally treated for 24 h at 150°C. After the completion of reaction, the autoclave is allowed to cool down to room temperature. To eliminate unreacted chemicals, the precipitate is centrifuged and washed many times with double-distilled water and methyl alcohol. Final solid is dehydrated for 12 h at 80°C and heated for 3 h at 600°C.


### 2.2. Characterization Techniques

The crystalline structures of Fe-SnO2 NPs are analyzed using an X-ray diffractometer (Inel Equinox 2000). WITec Alpha 300 Raman spectrometer is used for Raman and photoluminescence measurements at different excitation wavelengths 532 and 355 nm, respectively. A Fourier transform infrared spectrophotometer [Shimadzu-Japan 00719 (A221355)] is used to screen the surface functional groups of the nanoparticles. A scanning electron microscope (SEM-Leo 440i) is used to examine the surface morphology and composition. A high-resolution transmission electron microscope (JEM-2100 Plus, JEOL-Japan) is employed to obtain the lattice images and SAED patterns. The optical absorption spectra are recorded using a UV-visible spectrophotometer (Edinburgh Instruments FLS 980) with Xenon lamp as a light source.


### 2.3. Photocatalytic Dye-Degradation and Antibacterial Activity

The catalytic activity of the Fe-SnO2 samples are investigated by monitoring the decomposition of dye in the presence of H2O2 under visible light illumination using 125 W mercury vapour lamp. The degradation efficiency is investigated by analysing the absorption maximum of the dye by using a UV-visible spectrophotometer (Shimadzu UV 1800). Antibacterial activity of the synthesized samples is investigated by using colony count method against gram-negative Escherichia coli bacterial strain.


## 2.1. Fe-SnO2 Nanoparticle Synthesis

Tin (IV) chloride pentahydrate (SnCl4·5H2O) and ferric chloride hexahydrate (FeCl3.6H2O) are used as metal precursors; sodium hydroxide (NaOH) is used as a precipitating agent; methyl alcohol (CH3OH) and double deionized water are used for washing of the obtained precipitates. Double-distilled water is used as a solvent for all the synthesis process. All the chemicals are utilized with no further purification. SnCl4·5H2O (0.4 M) and FeCl3.6H2O at various concentrations (0.01, 0.03, and 0.05 M) are dissolved in 50 mL of double-deionized water in a conventional synthesis. The pH of precursor solution was adjusted to 10 by adding NaOH solution, and final solution is agitated at room temperature for 30 min. The contents are then transferred to an autoclave and hydrothermally treated for 24 h at 150°C. After the completion of reaction, the autoclave is allowed to cool down to room temperature. To eliminate unreacted chemicals, the precipitate is centrifuged and washed many times with double-distilled water and methyl alcohol. Final solid is dehydrated for 12 h at 80°C and heated for 3 h at 600°C.


## 2.2. Characterization Techniques

The crystalline structures of Fe-SnO2 NPs are analyzed using an X-ray diffractometer (Inel Equinox 2000). WITec Alpha 300 Raman spectrometer is used for Raman and photoluminescence measurements at different excitation wavelengths 532 and 355 nm, respectively. A Fourier transform infrared spectrophotometer [Shimadzu-Japan 00719 (A221355)] is used to screen the surface functional groups of the nanoparticles. A scanning electron microscope (SEM-Leo 440i) is used to examine the surface morphology and composition. A high-resolution transmission electron microscope (JEM-2100 Plus, JEOL-Japan) is employed to obtain the lattice images and SAED patterns. The optical absorption spectra are recorded using a UV-visible spectrophotometer (Edinburgh Instruments FLS 980) with Xenon lamp as a light source.


## 2.3. Photocatalytic Dye-Degradation and Antibacterial Activity

The catalytic activity of the Fe-SnO2 samples are investigated by monitoring the decomposition of dye in the presence of H2O2 under visible light illumination using 125 W mercury vapour lamp. The degradation efficiency is investigated by analysing the absorption maximum of the dye by using a UV-visible spectrophotometer (Shimadzu UV 1800). Antibacterial activity of the synthesized samples is investigated by using colony count method against gram-negative Escherichia coli bacterial strain.


## 3. Results and Discussion

### 3.1. XRD Analysis

The XRD diffraction patterns of synthesized pure and Fe-SnO2 NPs at different concentrations (0.01, 0.03, and 0.05 M) are shown in Figure 1. The XRD peaks detected in the XRD pattern of pure samples (Figure 1(a)) correspond well to the standard JCPDS data # 41-1445, confirming the formation of a tetragonal crystalline structure. The peaks observed at 26.50°, 33.89°, 37.85°, 51.74°, 54.70° 57.72°, 61.73°, 64.74°, 65.92°, and 71.25° correspond to the crystal planes (110), (101), (200), (211), (220), (002), (310), (112), (301), and (202), respectively. The XRD patterns of Fe-SnO2 NPs are identical to those of pure SnO2 NPs, with a modest shift in peak position and a reduction in the intensity. The decrease in peak intensity as the Fe-dopant concentration increases suggests that dopant ions have been incorporated into the SnO2 lattice effectively. The observed shift in peak positions is due to the substitution of Fe ions with smaller ionic radii (0.063 nm) in the site of Sn (0.069 nm) [17]. Besides, the XRD patterns do not reveal any other impurities or secondary-phase peaks, indicating that the synthesized samples are in pure crystalline form. The calculated mean crystalline sizes of the particles are found to be 9.38, 4.48, 4.88, and 4.87 nm for pure and (0.01, 0.03, and 0.05 M) Fe-SnO2 NPs, respectively. The strain generated by Fe-dopant ions in the host lattice can be attributed to the reduction in crystalline size for the Fe-doped samples. Baig et al., Segueni et al., and Rao et al. reported the similar results for Fe-SnO2 samples [19–21].Figure 1
XRD patterns of (a) pure, (b) 0.01 M, (c) 0.03 M, and (d) 0.05 M Fe-SnO2 NPs.


### 3.2. Raman Analysis

The typical vibrational modes of the Brillouin zone of SnO2 are represented by using group theory [22].
(1)Г=A1g+A2g+B1g+B2g+Eg+2A2u+2B1u+4Eu.The Raman modesB1g, Eg, A1g, and B2g observed at wavenumbers 123, 473, 634, and 773 cm–1, respectively, are active and caused by the vibration of oxygen atoms when Sn atoms are not in vibration. The Raman spectra (Figure 2(a)) of pure SnO2 NPs exhibit three active modes at 485, 631, and 776 cm–1 related to Eg, A1g, and B2g vibrations, respectively [23]. The modes A1g (631 cm–1) and B2g (776 cm–1) are caused by asymmetric stretching of Sn-O, but the mode Eg (485 cm–1) is caused by the vibration of two oxygen atoms along the c-axis but in the reverse direction, and it is highly susceptible to oxygen vacancies. In addition, the presence of three fundamental Raman modes confirms the formation of tetragonal rutile structure in SnO2 NPs. From the Raman spectra of Fe-SnO2 NPs (Figures 2(b)–2(d)), it is observed that the intensity of Eg, A1g, and B2g mode diminishes on increasing the Fe-dopant concentration, and the B2g mode observed at 776 cm-1 is completely vanished at 0.05 M Fe-SnO2 NPs. This supports the XRD results by indicating that Fe ions are integrated into the SnO2 lattice. The similar observation of a decrease in peak intensity of the B2g mode has been observed by Jayapandi et al. [24] and Othmen et al. [25] for La-doped and Fe-doped SnO2 NPs, respectively.Figure 2
Raman spectra of (a) pure, (b) 0.01 M, (c) 0.03 M, and (d) 0.05 M Fe-SnO2 NPs.


### 3.3. FTIR Analysis

The bonding nature of the synthesized Fe-SnO2 nanoparticles was identified by FTIR and displayed in Figure 3. The major peak appearing in the region of 441-445 cm–1 can be associated with the stretching mode of O–Sn–O bonding [26]. Remarkably, this stretching mode is shifted towards higher wavenumber (~450 cm–1) when the dopant concentration is increased. The vibrational bands appearing in the regions 550-557 cm–1 and 592-598 cm–1 were ascribed to Sn–O and Sn–O–Sn stretching vibrations, respectively [27, 28]. Further, the peak found in all samples around 638-642 cm–1 could be related to the O–Sn–O functional group, which confirmed the formation of SnO2 NPs [17].Figure 3
FTIR spectra of (a) pure, (b) 0.01 M, (c) 0.03 M, and (d) 0.05 M Fe-SnO2 NPs.


### 3.4. Morphology and Elemental Composition Analysis

Figure4 shows the morphological structure and elemental composition of the Fe-SnO2 nanoparticles studied with SEM and EDS analysis, respectively. The SEM micrograph obtained from pure SnO2 sample (Figure 4(a)) indicates the irregular distribution of particles which are agglomerated. With increasing Fe-dopant concentration, the agglomeration rate increases further (Figures 4(b)–4(d)), and this increase in agglomeration is mainly attributed to the higher surface free energy and larger surface area of the nanoparticles which have the tendency to agglomerate because of the stronger attractive forces exhibited by the surface atoms. The presence of Sn, O, and Fe as important trace elements were confirmed by EDS spectra corresponding to Figures 4(a) and 4(d). The calculated weight percent of the observed elements is shown in the EDS spectra inset tables.Figure 4
SEM micrographs of (a) pure, (b) 0.01 M, (c) 0.03 M, and (d) 0.05 M Fe-SnO2 NPs and EDS spectra of pure and 0.05 M Fe-SnO2 NPs.


### 3.5. HRTEM and SAED Analysis

The formation of spherical shaped nanoparticles with agglomeration was observed in the HRTEM image (Figure5(a)) of the 0.05 M Fe-SnO2 NPs sample. The interplanar spacing (dhkl) is calculated from the HRTEM lattice image shown in Figure 5(b). In addition, the calculated value of dhkl (0.3375 nm) is almost very close to the values obtained from the XRD data (0.3359 nm) and JCPDS data (0.3347 nm). Notably, the SAED pattern (Figure 5(c)) indicates the polycrystalline nature of the synthesized Fe-SnO2 NPs and having tetragonal crystal structure.Figure 5
(a) HRTEM image, (b) HRTEM lattice image, and (c) SAED pattern obtained from the 0.05 M Fe-SnO2 NPs.
(a)
(b)
(c)


### 3.6. UV-Visible Absorption Spectroscopy

Figure6 shows the UV-visible absorption spectra in the 250–500 nm wavelength region. In the near-UV range, the optical absorption spectrum of pure SnO2 NPs revealed a broad absorption band. With increasing Fe-dopant level, a red shift in the absorption band has been observed, and this shift in the absorption band provides a proof for the integration of dopants in the host lattice. The Tauc’s plots presented in Figure 6 were used to estimate the values of band gap. The estimated values are 3.36, 2.85, 2.77, and 2.58 eV for pure, 0.01, 0.03, and 0.05 M Fe-SnO2 NPs, respectively. Further, the vacancies or defects due to the absence of oxygen created by the Fe dopants in the host are responsible for the blue shift noticed in band gap energy. The quantum confinement effect cannot be treated as the reason for band gap reduction, since the crystallite size reduction does not increase the band gap here. Thus, the oxygen vacancies are considered as the sole reason for the band gap reduction in the present work [29].Figure 6
Optical absorption spectra and Tauc’s plot of (a) pure, (b) 0.01 M, (c) 0.03 M, and (d) 0.05 M Fe-SnO2 NPs.


### 3.7. Photoluminescence Spectroscopy

The recorded photoluminescence spectra are shown in Figure7. In the spectra, there are two peaks: a weak band (≈359 nm) and a strong band (≈650 nm) are noticed. The photogenerated electron-hole pairs undergo radiative recombination, resulting in weak band emission. The electrons in the deep level energy states undergo radiative recombination, and the holes generated in the valence band due to photoexcitation produce electrons in deep level states. The photoexcited holes in the valence band produce a strong emission in the visible region. Further, the intensity of PL emission peak decreases on increasing the Fe concentration, which is indicating the trapping of electron-hole pairs by oxygen vacancies, and leads to the creation of singly ionized oxygen vacancies with the accumulation of Fe+ ions [19]. The lower the intensity of PL emission peak, the lower will be the electron-hole recombination rate, which is favorable for photocatalytic activity, and hence, it is expected that the 0.05 M Fe-SnO2 NPs sample will give efficient results towards the degradation of dye molecules when compared to other samples.Figure 7
PL spectra of (a) pure, (b) 0.01 M, (c) 0.03 M, and (d) 0.05 M Fe-SnO2 NPs.


### 3.8. Photocatalytic Dye Degradation

The photocatalytic efficiency of Fe-SnO2 NPs to degrade crystal violet dye is performed by using H2O2-assisted photocatalytic process. H2O2 is a well-known photooxidant in waste water treatment since it creates hydroxyl radicals that degrade harmful pollutants when illuminated with visible light, hence enhancing the photocatalytic efficacy [12]. Initially, a required ppm of CV dye solution is prepared, and then, the certain amount of Fe-SnO2 sample (20 mg) is added to the dye solution, and 30 minutes of stirring is done to achieve equilibrium in adsorption-desorption process. Under continuous stirring, an appropriate amount of H2O2 (0.5 mL) is added into the dye solution under visible light irradiation. The dye degradation efficiency of the synthesized nanoparticles is elucidated by measuring the absorbance using UV-visible spectrophotometer at regular intervals. Figures 8(a)–8(d) show the absorption spectra taken at regular time intervals during the crystal violet dye-degradation using pure and 0.01 M, 0.03 M, and 0.05 M Fe-SnO2 NPs, respectively. It is observed that the intensity of characteristic absorption peak corresponding to crystal violet decreases slowly with increasing time, and the degradation is noticed clearly from the variation in the dye color. With increasing dopant concentration, the degradation time reduces monotonically. The crystal violet dye was completely degraded after 30 minutes of light illumination for the 0.05 M Fe-SnO2 NPs, which could be due to the efficient separation of electron-hole pairs as the dopant concentration is increased, as evidenced by the PL analysis, which showed reduced PL intensity with increasing Fe-dopant concentration, implying a lower electron-hole recombination rate. The efficiency of degradation is computed from the following equation reported in [30].
(2)DegradationEfficiency=1−AA0×100.Figure 8
Optical absorption spectra depicting the degradation of crystal violet dye using (a) pure, (b) 0.01 M, (c) 0.03 M, (d) 0.05 M Fe-SnO2 NPs, and (e) efficiency vs. time graph.
(a)
(b)
(c)
(d)
(e)The degradation efficiency vs. time curves of the pure and Fe-SnO2 NPs are shown in Figure 8(e). For 0.05 M Fe-SnO2 NPs, a maximum degradation efficiency of 98% is observed in 30 minutes. To study the role of light source in degradation process, a blank test is carried out without using the light source for 0.05 M Fe-doped SnO2 sample, and the result showed only 7% degradation efficiency in 30 minutes. From this result, it is clear that the synthesized Fe-SnO2 NPs acts as efficient photocatalyst in the presence of both H2O2 and light source. Thus, we have successfully synthesized Fe-SnO2 NPs having 98% efficiency to degrade crystal violet dye within 30 min of visible light irradiation even in the presence of less catalyst (20 mg) and H2O2 (0.5 mL), whereas the other literature reported low efficiency even after longer irradiation time. A detailed comparison of the results obtained in the present work is compared with previously reported literatures and tabulated in Table 1. These comparisons revealed that the photocatalyst efficiency to degrade dye molecules can be increased by adding H2O2. In general, the mechanism behind the photocatalytic dye degradation process can be explained as follows.Table 1
Comparison of catalytic dye degradation efficiency of the present work with the previously reported literature.
Material
Dye
Light source
Efficiency (%)
Time (min)
Reference
Fe:SnO2
Methylene blue
Visible light (500 W)
43
120
Ref [17]
Fe:SnO2 (CTAB)
25
Fe:SnO2 (SDS)
28
Fe:SnO2 (Triton)
49
Fe:TiO2
Methyl orange
Visible light (250 W)
69
Ref [18]
Fe:SnO2
Visible light (500 W)
87.2
200
Ref [19]
Ni:SnO2
Brilliant green
Sunlight
97.54
105
Ref [16]
Fe:SnO2
Crystal violet
Visible light (125 W) + H2O2
98.23
30
Present workWhen a photon with energy higher than the band gap excites the photocatalyst, the electrons are elevated into the conduction band from the valence band, and holes are generated. These generated electrons form superoxide radicals by reacting with dissolved oxygen, whereas the produced holes transform OH- into ˙OH radicals. The mechanism can be described by using the following equations:
(3)Fe−SnO2NPs+hυ⟶Fe−SnO2NPs+e–+h+,e–+O2⟶⋅O2–,h++OH–⟶.OH,CV+⋅O2–,⋅OH⟶CO2+H2O.H2O2 has played an important role in the photocatalytic reaction because it acts as an electron acceptor, absorbing photon energy, and forming hydroxyl radicals. As a result, the probability of electron-hole recombination rate will be reduced. The produced superoxide radical anions and hydroxyl radicals are expected to be responsible to breakdown the dye molecules [31].


#### 3.8.1. Effect of Scavengers on Degradation Efficiency

In order to identify the active species which govern the degradation process, the reaction is carried out in the presence of 0.5 mM ethylene diamine tetra acetic acid (EDTA), isopropyl alcohol (IPA), and ascorbic acid (AA) as holes (h+), hydroxyl radical (⋅OH), and superoxide radical anions ⋅O2– scavengers, respectively. Figure 9 shows the degradation efficiency of Fe-SnO2 NPs while using different scavengers, and the results suggest that efficiency is in the order of No scavengers > IPA > AA > EDTA. The very feeble role of hydroxyl radical in degradation process is identified from the slight reduction in efficiency while using hydroxyl radical scavenger (IPA). The minimum degradation efficiency of 5% and 21% is observed while using EDTA and AA, respectively. This strongly indicates that the holes and superoxide radical anions play a significant role in the degradation of crystal violet dye.Figure 9
Effect of different radical scavengers on degradation of crystal violet dye.


#### 3.8.2. Effect of pH on Degradation of Crystal Violet Dye

The degradation efficiency of nanoparticles depends on pH of the dye solution, since it controls the production of hydroxyl radicals during the degradation process. To study the effect of pH, we have varied the pH of dye solution from 2 to 10 by using 1 M NaOH and HCl solutions. After adjusting the pH, the dye solution containing an appropriate amount of 0.05 M Fe-doped SnO2 nanoparticles is stirred for 30 min in dark to obtain an equilibrium between the catalyst and dye molecules. In this stage, H2O2 (0.5 mL) is added and stirred continuously under visible light illumination. UV-visible absorption spectra were taken at regular time interval to study its degradation efficiency. The degradation efficiency increases while increasing the pH of dye solution as shown in Figure 10, and the results clearly indicated a maximum degradation efficiency of 98% for the nanoparticles in the basic medium (pH=10). In the basic medium, the charge on the surface of Fe-doped SnO2 nanoparticles tends to be negative which attracts the cationic crystal violet dye via electrostatic force of attraction [2].Figure 10
Effect of pH on the degradation of crystal violet dye using 0.05 M Fe-SnO2 NPs.


#### 3.8.3. Reusability and Stability of Fe-SnO2 NPs

It is important to study the reusability and stability of the catalyst to identify its practical applicability. The catalyst was collected and dried after each cycle and was reused for the next cycle. Figure11 indicates that the Fe-doped SnO2 nanoparticles showed only a slight variation in degradation efficiency of crystal violet dye from 98% to 96% after five cycles. This result confirms that the synthesized Fe-doped SnO2 nanoparticles are stable when reused.Figure 11
Recycling ability and stability of 0.05 M Fe-SnO2 nanoparticles.


### 3.9. Antibacterial Activity

Antibacterial activity of the synthesized pure and Fe-SnO2 NPs against Escherichia coli was studied by using colony count method. This method is particularly advantageous when the nanoparticle suspension offers less diffusion through the medium. In this method, bacterial strains are grown in a nutrient broth medium overnight at a temperature of 37°C in an orbital shaker. Further, the number of colony forming unit (CFU) is adjusted to 1×102 cells/mL by using a 75 mM saline solution. 100 μL of the above medium is spread on the nutrient agar plates using L-rod, and same quantity of the aqueous nanoparticle suspension is also spread over the bacterium inoculated plates and incubated at 37°C for 24 h. Here, the plates without the nanoparticle suspension is used as a control. The number of colonies formed is counted, and the percentage of inhibition is found by using the formula
(4)%Inhibition=Control–TestTest∗100.The obtained antibacterial activity of pure and Fe-SnO2 NPs at different concentrations is depicted in Figure 12. The inhibition rate of pure, 0.01 M, 0.03 M, and 0.05 M Fe-SnO2 NPs against gram-negative bacteria Escherichia coli is found to be 49, 65, 70, and 78%, respectively. Notably, the observed inhibition rate shows the nanoparticle diffusion into a thin cell wall having many lipopolysaccharides and a few peptidoglycan layers.Figure 12
Antibacterial potential of pure and Fe-SnO2 NPs.The mechanism involved in the antibacterial activity of Fe-SnO2 NPs is assumed to be influenced by the generated reactive oxygen species, viz., H2O2, superoxide, and hydroxyl radicals, which will penetrate through the bacterial cell membrane, damage DNA, and protein, which will finally inhibit bacterial growth. For Fe-SnO2 NPs, the increased antibacterial action can be attributed to their smaller particle size, as evidenced by XRD and FESEM analysis, which leads to the generation of a large number of reactive oxygen species on the surface of bacterial cells, resulting in intracellular component leakage and cell death [32, 33]. To check the reliability of the obtained results, a triplicate of the experiment is carried out. Similar types of enhancement in antibacterial activity of doped SnO2 NPs have been reported previously by Manjula and Selvan and Amutha et al. [34, 35].


## 3.1. XRD Analysis

The XRD diffraction patterns of synthesized pure and Fe-SnO2 NPs at different concentrations (0.01, 0.03, and 0.05 M) are shown in Figure 1. The XRD peaks detected in the XRD pattern of pure samples (Figure 1(a)) correspond well to the standard JCPDS data # 41-1445, confirming the formation of a tetragonal crystalline structure. The peaks observed at 26.50°, 33.89°, 37.85°, 51.74°, 54.70° 57.72°, 61.73°, 64.74°, 65.92°, and 71.25° correspond to the crystal planes (110), (101), (200), (211), (220), (002), (310), (112), (301), and (202), respectively. The XRD patterns of Fe-SnO2 NPs are identical to those of pure SnO2 NPs, with a modest shift in peak position and a reduction in the intensity. The decrease in peak intensity as the Fe-dopant concentration increases suggests that dopant ions have been incorporated into the SnO2 lattice effectively. The observed shift in peak positions is due to the substitution of Fe ions with smaller ionic radii (0.063 nm) in the site of Sn (0.069 nm) [17]. Besides, the XRD patterns do not reveal any other impurities or secondary-phase peaks, indicating that the synthesized samples are in pure crystalline form. The calculated mean crystalline sizes of the particles are found to be 9.38, 4.48, 4.88, and 4.87 nm for pure and (0.01, 0.03, and 0.05 M) Fe-SnO2 NPs, respectively. The strain generated by Fe-dopant ions in the host lattice can be attributed to the reduction in crystalline size for the Fe-doped samples. Baig et al., Segueni et al., and Rao et al. reported the similar results for Fe-SnO2 samples [19–21].Figure 1
XRD patterns of (a) pure, (b) 0.01 M, (c) 0.03 M, and (d) 0.05 M Fe-SnO2 NPs.


## 3.2. Raman Analysis

The typical vibrational modes of the Brillouin zone of SnO2 are represented by using group theory [22].
(1)Г=A1g+A2g+B1g+B2g+Eg+2A2u+2B1u+4Eu.The Raman modesB1g, Eg, A1g, and B2g observed at wavenumbers 123, 473, 634, and 773 cm–1, respectively, are active and caused by the vibration of oxygen atoms when Sn atoms are not in vibration. The Raman spectra (Figure 2(a)) of pure SnO2 NPs exhibit three active modes at 485, 631, and 776 cm–1 related to Eg, A1g, and B2g vibrations, respectively [23]. The modes A1g (631 cm–1) and B2g (776 cm–1) are caused by asymmetric stretching of Sn-O, but the mode Eg (485 cm–1) is caused by the vibration of two oxygen atoms along the c-axis but in the reverse direction, and it is highly susceptible to oxygen vacancies. In addition, the presence of three fundamental Raman modes confirms the formation of tetragonal rutile structure in SnO2 NPs. From the Raman spectra of Fe-SnO2 NPs (Figures 2(b)–2(d)), it is observed that the intensity of Eg, A1g, and B2g mode diminishes on increasing the Fe-dopant concentration, and the B2g mode observed at 776 cm-1 is completely vanished at 0.05 M Fe-SnO2 NPs. This supports the XRD results by indicating that Fe ions are integrated into the SnO2 lattice. The similar observation of a decrease in peak intensity of the B2g mode has been observed by Jayapandi et al. [24] and Othmen et al. [25] for La-doped and Fe-doped SnO2 NPs, respectively.Figure 2
Raman spectra of (a) pure, (b) 0.01 M, (c) 0.03 M, and (d) 0.05 M Fe-SnO2 NPs.


## 3.3. FTIR Analysis

The bonding nature of the synthesized Fe-SnO2 nanoparticles was identified by FTIR and displayed in Figure 3. The major peak appearing in the region of 441-445 cm–1 can be associated with the stretching mode of O–Sn–O bonding [26]. Remarkably, this stretching mode is shifted towards higher wavenumber (~450 cm–1) when the dopant concentration is increased. The vibrational bands appearing in the regions 550-557 cm–1 and 592-598 cm–1 were ascribed to Sn–O and Sn–O–Sn stretching vibrations, respectively [27, 28]. Further, the peak found in all samples around 638-642 cm–1 could be related to the O–Sn–O functional group, which confirmed the formation of SnO2 NPs [17].Figure 3
FTIR spectra of (a) pure, (b) 0.01 M, (c) 0.03 M, and (d) 0.05 M Fe-SnO2 NPs.


## 3.4. Morphology and Elemental Composition Analysis

Figure4 shows the morphological structure and elemental composition of the Fe-SnO2 nanoparticles studied with SEM and EDS analysis, respectively. The SEM micrograph obtained from pure SnO2 sample (Figure 4(a)) indicates the irregular distribution of particles which are agglomerated. With increasing Fe-dopant concentration, the agglomeration rate increases further (Figures 4(b)–4(d)), and this increase in agglomeration is mainly attributed to the higher surface free energy and larger surface area of the nanoparticles which have the tendency to agglomerate because of the stronger attractive forces exhibited by the surface atoms. The presence of Sn, O, and Fe as important trace elements were confirmed by EDS spectra corresponding to Figures 4(a) and 4(d). The calculated weight percent of the observed elements is shown in the EDS spectra inset tables.Figure 4
SEM micrographs of (a) pure, (b) 0.01 M, (c) 0.03 M, and (d) 0.05 M Fe-SnO2 NPs and EDS spectra of pure and 0.05 M Fe-SnO2 NPs.


## 3.5. HRTEM and SAED Analysis

The formation of spherical shaped nanoparticles with agglomeration was observed in the HRTEM image (Figure5(a)) of the 0.05 M Fe-SnO2 NPs sample. The interplanar spacing (dhkl) is calculated from the HRTEM lattice image shown in Figure 5(b). In addition, the calculated value of dhkl (0.3375 nm) is almost very close to the values obtained from the XRD data (0.3359 nm) and JCPDS data (0.3347 nm). Notably, the SAED pattern (Figure 5(c)) indicates the polycrystalline nature of the synthesized Fe-SnO2 NPs and having tetragonal crystal structure.Figure 5
(a) HRTEM image, (b) HRTEM lattice image, and (c) SAED pattern obtained from the 0.05 M Fe-SnO2 NPs.
(a)
(b)
(c)


## 3.6. UV-Visible Absorption Spectroscopy

Figure6 shows the UV-visible absorption spectra in the 250–500 nm wavelength region. In the near-UV range, the optical absorption spectrum of pure SnO2 NPs revealed a broad absorption band. With increasing Fe-dopant level, a red shift in the absorption band has been observed, and this shift in the absorption band provides a proof for the integration of dopants in the host lattice. The Tauc’s plots presented in Figure 6 were used to estimate the values of band gap. The estimated values are 3.36, 2.85, 2.77, and 2.58 eV for pure, 0.01, 0.03, and 0.05 M Fe-SnO2 NPs, respectively. Further, the vacancies or defects due to the absence of oxygen created by the Fe dopants in the host are responsible for the blue shift noticed in band gap energy. The quantum confinement effect cannot be treated as the reason for band gap reduction, since the crystallite size reduction does not increase the band gap here. Thus, the oxygen vacancies are considered as the sole reason for the band gap reduction in the present work [29].Figure 6
Optical absorption spectra and Tauc’s plot of (a) pure, (b) 0.01 M, (c) 0.03 M, and (d) 0.05 M Fe-SnO2 NPs.


## 3.7. Photoluminescence Spectroscopy

The recorded photoluminescence spectra are shown in Figure7. In the spectra, there are two peaks: a weak band (≈359 nm) and a strong band (≈650 nm) are noticed. The photogenerated electron-hole pairs undergo radiative recombination, resulting in weak band emission. The electrons in the deep level energy states undergo radiative recombination, and the holes generated in the valence band due to photoexcitation produce electrons in deep level states. The photoexcited holes in the valence band produce a strong emission in the visible region. Further, the intensity of PL emission peak decreases on increasing the Fe concentration, which is indicating the trapping of electron-hole pairs by oxygen vacancies, and leads to the creation of singly ionized oxygen vacancies with the accumulation of Fe+ ions [19]. The lower the intensity of PL emission peak, the lower will be the electron-hole recombination rate, which is favorable for photocatalytic activity, and hence, it is expected that the 0.05 M Fe-SnO2 NPs sample will give efficient results towards the degradation of dye molecules when compared to other samples.Figure 7
PL spectra of (a) pure, (b) 0.01 M, (c) 0.03 M, and (d) 0.05 M Fe-SnO2 NPs.


## 3.8. Photocatalytic Dye Degradation

The photocatalytic efficiency of Fe-SnO2 NPs to degrade crystal violet dye is performed by using H2O2-assisted photocatalytic process. H2O2 is a well-known photooxidant in waste water treatment since it creates hydroxyl radicals that degrade harmful pollutants when illuminated with visible light, hence enhancing the photocatalytic efficacy [12]. Initially, a required ppm of CV dye solution is prepared, and then, the certain amount of Fe-SnO2 sample (20 mg) is added to the dye solution, and 30 minutes of stirring is done to achieve equilibrium in adsorption-desorption process. Under continuous stirring, an appropriate amount of H2O2 (0.5 mL) is added into the dye solution under visible light irradiation. The dye degradation efficiency of the synthesized nanoparticles is elucidated by measuring the absorbance using UV-visible spectrophotometer at regular intervals. Figures 8(a)–8(d) show the absorption spectra taken at regular time intervals during the crystal violet dye-degradation using pure and 0.01 M, 0.03 M, and 0.05 M Fe-SnO2 NPs, respectively. It is observed that the intensity of characteristic absorption peak corresponding to crystal violet decreases slowly with increasing time, and the degradation is noticed clearly from the variation in the dye color. With increasing dopant concentration, the degradation time reduces monotonically. The crystal violet dye was completely degraded after 30 minutes of light illumination for the 0.05 M Fe-SnO2 NPs, which could be due to the efficient separation of electron-hole pairs as the dopant concentration is increased, as evidenced by the PL analysis, which showed reduced PL intensity with increasing Fe-dopant concentration, implying a lower electron-hole recombination rate. The efficiency of degradation is computed from the following equation reported in [30].
(2)DegradationEfficiency=1−AA0×100.Figure 8
Optical absorption spectra depicting the degradation of crystal violet dye using (a) pure, (b) 0.01 M, (c) 0.03 M, (d) 0.05 M Fe-SnO2 NPs, and (e) efficiency vs. time graph.
(a)
(b)
(c)
(d)
(e)The degradation efficiency vs. time curves of the pure and Fe-SnO2 NPs are shown in Figure 8(e). For 0.05 M Fe-SnO2 NPs, a maximum degradation efficiency of 98% is observed in 30 minutes. To study the role of light source in degradation process, a blank test is carried out without using the light source for 0.05 M Fe-doped SnO2 sample, and the result showed only 7% degradation efficiency in 30 minutes. From this result, it is clear that the synthesized Fe-SnO2 NPs acts as efficient photocatalyst in the presence of both H2O2 and light source. Thus, we have successfully synthesized Fe-SnO2 NPs having 98% efficiency to degrade crystal violet dye within 30 min of visible light irradiation even in the presence of less catalyst (20 mg) and H2O2 (0.5 mL), whereas the other literature reported low efficiency even after longer irradiation time. A detailed comparison of the results obtained in the present work is compared with previously reported literatures and tabulated in Table 1. These comparisons revealed that the photocatalyst efficiency to degrade dye molecules can be increased by adding H2O2. In general, the mechanism behind the photocatalytic dye degradation process can be explained as follows.Table 1
Comparison of catalytic dye degradation efficiency of the present work with the previously reported literature.
Material
Dye
Light source
Efficiency (%)
Time (min)
Reference
Fe:SnO2
Methylene blue
Visible light (500 W)
43
120
Ref [17]
Fe:SnO2 (CTAB)
25
Fe:SnO2 (SDS)
28
Fe:SnO2 (Triton)
49
Fe:TiO2
Methyl orange
Visible light (250 W)
69
Ref [18]
Fe:SnO2
Visible light (500 W)
87.2
200
Ref [19]
Ni:SnO2
Brilliant green
Sunlight
97.54
105
Ref [16]
Fe:SnO2
Crystal violet
Visible light (125 W) + H2O2
98.23
30
Present workWhen a photon with energy higher than the band gap excites the photocatalyst, the electrons are elevated into the conduction band from the valence band, and holes are generated. These generated electrons form superoxide radicals by reacting with dissolved oxygen, whereas the produced holes transform OH- into ˙OH radicals. The mechanism can be described by using the following equations:
(3)Fe−SnO2NPs+hυ⟶Fe−SnO2NPs+e–+h+,e–+O2⟶⋅O2–,h++OH–⟶.OH,CV+⋅O2–,⋅OH⟶CO2+H2O.H2O2 has played an important role in the photocatalytic reaction because it acts as an electron acceptor, absorbing photon energy, and forming hydroxyl radicals. As a result, the probability of electron-hole recombination rate will be reduced. The produced superoxide radical anions and hydroxyl radicals are expected to be responsible to breakdown the dye molecules [31].


### 3.8.1. Effect of Scavengers on Degradation Efficiency

In order to identify the active species which govern the degradation process, the reaction is carried out in the presence of 0.5 mM ethylene diamine tetra acetic acid (EDTA), isopropyl alcohol (IPA), and ascorbic acid (AA) as holes (h+), hydroxyl radical (⋅OH), and superoxide radical anions ⋅O2– scavengers, respectively. Figure 9 shows the degradation efficiency of Fe-SnO2 NPs while using different scavengers, and the results suggest that efficiency is in the order of No scavengers > IPA > AA > EDTA. The very feeble role of hydroxyl radical in degradation process is identified from the slight reduction in efficiency while using hydroxyl radical scavenger (IPA). The minimum degradation efficiency of 5% and 21% is observed while using EDTA and AA, respectively. This strongly indicates that the holes and superoxide radical anions play a significant role in the degradation of crystal violet dye.Figure 9
Effect of different radical scavengers on degradation of crystal violet dye.


### 3.8.2. Effect of pH on Degradation of Crystal Violet Dye

The degradation efficiency of nanoparticles depends on pH of the dye solution, since it controls the production of hydroxyl radicals during the degradation process. To study the effect of pH, we have varied the pH of dye solution from 2 to 10 by using 1 M NaOH and HCl solutions. After adjusting the pH, the dye solution containing an appropriate amount of 0.05 M Fe-doped SnO2 nanoparticles is stirred for 30 min in dark to obtain an equilibrium between the catalyst and dye molecules. In this stage, H2O2 (0.5 mL) is added and stirred continuously under visible light illumination. UV-visible absorption spectra were taken at regular time interval to study its degradation efficiency. The degradation efficiency increases while increasing the pH of dye solution as shown in Figure 10, and the results clearly indicated a maximum degradation efficiency of 98% for the nanoparticles in the basic medium (pH=10). In the basic medium, the charge on the surface of Fe-doped SnO2 nanoparticles tends to be negative which attracts the cationic crystal violet dye via electrostatic force of attraction [2].Figure 10
Effect of pH on the degradation of crystal violet dye using 0.05 M Fe-SnO2 NPs.


### 3.8.3. Reusability and Stability of Fe-SnO2 NPs

It is important to study the reusability and stability of the catalyst to identify its practical applicability. The catalyst was collected and dried after each cycle and was reused for the next cycle. Figure11 indicates that the Fe-doped SnO2 nanoparticles showed only a slight variation in degradation efficiency of crystal violet dye from 98% to 96% after five cycles. This result confirms that the synthesized Fe-doped SnO2 nanoparticles are stable when reused.Figure 11
Recycling ability and stability of 0.05 M Fe-SnO2 nanoparticles.


## 3.8.1. Effect of Scavengers on Degradation Efficiency

In order to identify the active species which govern the degradation process, the reaction is carried out in the presence of 0.5 mM ethylene diamine tetra acetic acid (EDTA), isopropyl alcohol (IPA), and ascorbic acid (AA) as holes (h+), hydroxyl radical (⋅OH), and superoxide radical anions ⋅O2– scavengers, respectively. Figure 9 shows the degradation efficiency of Fe-SnO2 NPs while using different scavengers, and the results suggest that efficiency is in the order of No scavengers > IPA > AA > EDTA. The very feeble role of hydroxyl radical in degradation process is identified from the slight reduction in efficiency while using hydroxyl radical scavenger (IPA). The minimum degradation efficiency of 5% and 21% is observed while using EDTA and AA, respectively. This strongly indicates that the holes and superoxide radical anions play a significant role in the degradation of crystal violet dye.Figure 9
Effect of different radical scavengers on degradation of crystal violet dye.


## 3.8.2. Effect of pH on Degradation of Crystal Violet Dye

The degradation efficiency of nanoparticles depends on pH of the dye solution, since it controls the production of hydroxyl radicals during the degradation process. To study the effect of pH, we have varied the pH of dye solution from 2 to 10 by using 1 M NaOH and HCl solutions. After adjusting the pH, the dye solution containing an appropriate amount of 0.05 M Fe-doped SnO2 nanoparticles is stirred for 30 min in dark to obtain an equilibrium between the catalyst and dye molecules. In this stage, H2O2 (0.5 mL) is added and stirred continuously under visible light illumination. UV-visible absorption spectra were taken at regular time interval to study its degradation efficiency. The degradation efficiency increases while increasing the pH of dye solution as shown in Figure 10, and the results clearly indicated a maximum degradation efficiency of 98% for the nanoparticles in the basic medium (pH=10). In the basic medium, the charge on the surface of Fe-doped SnO2 nanoparticles tends to be negative which attracts the cationic crystal violet dye via electrostatic force of attraction [2].Figure 10
Effect of pH on the degradation of crystal violet dye using 0.05 M Fe-SnO2 NPs.


## 3.8.3. Reusability and Stability of Fe-SnO2 NPs

It is important to study the reusability and stability of the catalyst to identify its practical applicability. The catalyst was collected and dried after each cycle and was reused for the next cycle. Figure11 indicates that the Fe-doped SnO2 nanoparticles showed only a slight variation in degradation efficiency of crystal violet dye from 98% to 96% after five cycles. This result confirms that the synthesized Fe-doped SnO2 nanoparticles are stable when reused.Figure 11
Recycling ability and stability of 0.05 M Fe-SnO2 nanoparticles.


## 3.9. Antibacterial Activity

Antibacterial activity of the synthesized pure and Fe-SnO2 NPs against Escherichia coli was studied by using colony count method. This method is particularly advantageous when the nanoparticle suspension offers less diffusion through the medium. In this method, bacterial strains are grown in a nutrient broth medium overnight at a temperature of 37°C in an orbital shaker. Further, the number of colony forming unit (CFU) is adjusted to 1×102 cells/mL by using a 75 mM saline solution. 100 μL of the above medium is spread on the nutrient agar plates using L-rod, and same quantity of the aqueous nanoparticle suspension is also spread over the bacterium inoculated plates and incubated at 37°C for 24 h. Here, the plates without the nanoparticle suspension is used as a control. The number of colonies formed is counted, and the percentage of inhibition is found by using the formula
(4)%Inhibition=Control–TestTest∗100.The obtained antibacterial activity of pure and Fe-SnO2 NPs at different concentrations is depicted in Figure 12. The inhibition rate of pure, 0.01 M, 0.03 M, and 0.05 M Fe-SnO2 NPs against gram-negative bacteria Escherichia coli is found to be 49, 65, 70, and 78%, respectively. Notably, the observed inhibition rate shows the nanoparticle diffusion into a thin cell wall having many lipopolysaccharides and a few peptidoglycan layers.Figure 12
Antibacterial potential of pure and Fe-SnO2 NPs.The mechanism involved in the antibacterial activity of Fe-SnO2 NPs is assumed to be influenced by the generated reactive oxygen species, viz., H2O2, superoxide, and hydroxyl radicals, which will penetrate through the bacterial cell membrane, damage DNA, and protein, which will finally inhibit bacterial growth. For Fe-SnO2 NPs, the increased antibacterial action can be attributed to their smaller particle size, as evidenced by XRD and FESEM analysis, which leads to the generation of a large number of reactive oxygen species on the surface of bacterial cells, resulting in intracellular component leakage and cell death [32, 33]. To check the reliability of the obtained results, a triplicate of the experiment is carried out. Similar types of enhancement in antibacterial activity of doped SnO2 NPs have been reported previously by Manjula and Selvan and Amutha et al. [34, 35].


## 4. Conclusion

Pure and Fe-SnO2 NPs at different molar concentrations are synthesized by the hydrothermal method. The structural studies confirmed the successful incorporation of Fe ions into the Sn lattice of SnO2 NPs without the formation of any other secondary phases. SEM micrographs revealed the formation of irregularly shaped particles with agglomeration. EDS analysis confirmed the presence of Fe, Sn, and O as major trace elements. The PL emission peaks seen in the visible region confirm the presence of intrinsic defects such as oxygen vacancies and tin interstitials. H2O2-assisted photocatalytic degradation of crystal violet dye using Fe-SnO2 NPs has shown increased efficiency with the increase of Fe-dopant concentration, and a maximum efficiency of 98% was observed for 0.05 M Fe-SnO2 NPs. The radical scavenger studies indicated that the holes and superoxide radicals played major roles while the hydroxide radicals played a relatively minor role in the degradation process. The investigations on the role of pH of the dye solution revealed a maximum degradation efficiency when the pH value is 10. The synthesized Fe-SnO2 NPs showed excellent stability and almost constant dye degradation efficiency even after 5 cycles when reused. The antibacterial activity of Fe-SnO2 NPs investigated against gram-negative Escherichia coli by using the colony count method shown the promising potential of the synthesized nanoparticles as antibacterial agents.



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*Source: 9334079-2022-05-09.xml*