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Article

Synthesis and Broadband Spectra Photocatalytic Properties of Bi2O2(CO3)1−xSx

by
Junping Ding
1,2,
Huanchun Wang
1,3,
Haomin Xu
1,
Lina Qiao
1,
Yidong Luo
1,
Yuanhua Lin
1,* and
Cewen Nan
1
1
State Key Laboratory of New Ceramics and Fine Processing, School of Materials Science and Engineering, Tsinghua University, Beijing 100084, China
2
China Astronaut Research and Training Center, Beijing 100094, China
3
High-Tech Institute of Xi’an, Xi’an 710025, China
*
Author to whom correspondence should be addressed.
Materials 2018, 11(5), 791; https://doi.org/10.3390/ma11050791
Submission received: 31 March 2018 / Revised: 29 April 2018 / Accepted: 3 May 2018 / Published: 14 May 2018
(This article belongs to the Special Issue Novel Photoactive Materials)
Browse Figures
Versions Notes

Abstract

:
High efficiency photocatalyst Bi2O2(CO3)1−xSx was synthesized conveniently with chemical bath precipitation using Bi2O2CO3 as the precursor. The microstructures of the samples are systematically characterized by X-ray diffraction (XRD), scanning electron microscopy (SEM), high resolution transmission electron microscopy (HRTEM), X-ray photoelectron spectroscopy (XPS), ultraviolet photoelectron spectroscopy (UPS) and UV-Vis spectroscopy; the optical and photocatalytic properties are carefully tested as well. The content of S, which was tuned through the controlling of the precipitation process, was verified to have an intense effect over the photocatalytic properties. A nearly saturated S ratio and the best photocatalytic performance were observed in specimens with the most S content. Our study reveals that, with negligible influence of the morphology and crystal structure, Bi2O2(CO3)1−xSx possessed a broadened optical absorption regionfromultraviolet to visible light, and enhanced photocatalytic activity in comparison to precursor Bi2O2CO3 in photocatalytic degradation of Congo Red aqueous solution.

1. Introduction

Semiconductor photocatalysis has attracted increasing attention because of the capability of harvesting the solar energy to eliminate environmental pollutants [1,2,3,4,5,6,7]. Among various semiconductors, some Aurivillius type bismuth-based oxide semiconductor materials such as BiOX (X = Cl, Br, I), BiVO4 and Bi2WO6 have been widely used in photocatalysis [8,9,10,11,12,13,14].
Bismuth-based layered-structure compounds have a unique crystal structure and band structure. Hybridisation between 6s electrons of Bi and 2p electrons of O form chemical bonds which are stronger than those between Bi and other nonmetallic atoms (such as chalcogen), leading to a particularly stable (Bi-O)+ layer. A series of Bi-based layered-structural photocatalytic materials of various band gap widths from 3.2 eV (e.g., BiOCl [15]) to 1.12~1.5 eV (e.g., Bi2O2S [16,17]) can be obtained by combining the (Bi-O)+ layer with different anion layers. In addition, p-type (BiCuSO or the like) or n-type (Bi2O2CO3, etc.) semiconductor materials can be obtained by adjusting the anion layer. Therefore, the different Bi-based oxide composite structure can not only control and broaden the range of light absorption of the catalyst, but also may form a hetero structure such as p-n junction.
Recently, Bi2O2CO3, which is a member of the Aurivillius-type family and composed of [Bi2O2]2+ layers interleaved by CO32− layers [18,19], has attracted growing concern because of its photocatalytic ability to decompose organic pollutants in liquid phase and NO in gaseous phase [20,21,22]. Its unique layered structure, resulting in a large internal electrostatic field and asymmetric polarization effect, contributes to the separation of photogenerated electron-hole pairs [23,24]. However, the application of Bi2O2CO3 in photodegradation is strongly limited by its large band gap (~3.3 eV). To overcome this limitation, many methods have been developed, such as the fabrication of heterojunctions such as BiVO4/Bi2O2CO3, Bi2S3/Bi2O3/Bi2O2CO3 [25,26,27], noble metal deposition [28], elemental doping [29], and morphological modulation [30].
In this paper, we have synthesized S-doped Bi2O2(CO3)1−xSx by chemical bath precipitation, using Bi2O2CO3 as the precursor, through the controlling of the precipitation process to have an intense effect over the photocatalytic properties. A nearly saturated S ratio and the best photocatalytic performance were observed in specimens with the most S content. With a negligible influence of the morphology and crystal structure, the optical absorption of Bi2O3CO3 was extended from the ultraviolet (UV) to the visible region. The photocatalytic degradation of Congo Red showed that Bi2O2(CO3)1−xSx exhibited enhanced photoactivity in comparison to the precursor powder.

2. Results and Discussion

2.1. Synthetic Bi2O2(CO3)1−xSx

Figure 1 shows the XRD(X-ray diffraction) pattern of the Bi2O2CO3 powder prepared by hydrothermal method, together with a reference pattern of tetragonal Bi2O2CO3 (JCPDS: 41−1488). No second phase can be found, and the sharp peaks indicate well-developed crystallinity. The preparation process of Bi2O2CO3 can be summarized in Equations (1)–(3). CO32− forms through a hydrolysis reaction between (NH2)2CO and H2O. Bi2O3 is also strongly hydrolyzed with water to produce (Bi2O2)2+. The produced (Bi2O2)2+ and CO32− then react to generate Bi2O2CO3.
(NH2)2CO + 2H2O → 2NH3+ + CO32−
Bi2O3 + 2H2O →(Bi2O2)2+ + 2OH+
(Bi2O2)2+ + CO32−→Bi2O2CO3
In addition, the percentage of crystallinity and the BET (Brunauer–Emmett–Teller) specific surface area of the samples with a S:Bi2O2CO3 ratio n equals to 0, 0.01, 0.02, 0.05, 0.10 and 0.20 (marked as M0, M1, M2, M5, M10 and M20, respectively) are shown in Table 1. There are no significant changes in their percentage of crystallinity, while samples of M5 and M10 displaylarger specific surface areas than that of other samples, which could lead to theexposure of more active sites for the photocatalytic experiment. The scanning electron microscopy (SEM) photograph and the high resolution transmission electron microscopy (HRTEM) images of the powder are shown in Figure 2 and Figure 3. The morphology of the particles are nano-sized flakes of about 60–80 nm in thickness. In addition, the crystallinity of different samples calculated from the XRD results shows that S doping introduced defects in the Bi2O2CO3 and thus caused crystallinity change.
The XRD patterns of the samples prepared by the Na2S chemical bath precipitationare shown in Figure 4a. All diffraction peaks are consistent with Bi2O2CO3, indicating that chemical bath precipitation did not introduce a significant second phase. The intensity of the diffraction peak does not obviously decrease, and the products still have good crystallinity. The position of the (013) diffraction peak for different samples are shown in Figure 4b. No obvious influence of Na2S chemical precipitation on the crystal structure of Bi2O2CO3 can be found because the position of the peak (013) did not show an apparent shift according to XRD results.
X-ray photoelectron spectroscopy (XPS) was utilized toobtain insights into the valence states and surface chemical compositions details of Bi2O2(CO3)1−xSx. As shown in Figure 5a, the XPS spectrum of Bi-4f shows two peaks at 159.05 and 164.35 eV, which belong to Bi-4f7/2 and Bi-4f5/2 energy levels, respectively. These two peaks are characteristic features of trivalent Bi in Bi2O2(CO3)1−xSx [31]. The two peaks at 284.7 eV and 288.8 eV in Figure 5b show that the existence form of C is CO32− [32]. In Figure 5c, the two peaks are at 530.5 eV and 531 eV, which belong to O energy levels in B-O and CO32−, respectively [33]. In Figure 5d, the peak of S-2p is at the range of 158–166 eV, which shows that the existence form of S is S2− [17]. On the other hand, the Bi-4f peak of M20 apparently shifts compared to M0 (Figure 5a), which proves that S takes place of CO32− partially [34].
Although Na2S chemical precipitation had no obvious influence on the crystal structure of Bi2O2CO3, the powder color was changed from white to yellow, and the color became darker as S: Bi2O2CO3 molar ratio n increased. The UV-Vis diffuse reflectance spectra are shown in Figure 6. Bi2O2CO3 has a strong absorption of UV light with wavelengths less than 360 nm and weak absorption to 400 nm~500 nm-wavelength-visible light due to defects and oxygen vacancy, which also explained the fact that Bi2O2CO3 could display visible light photocatalytic activity with the bandgap of 3.2 eV. With the introduction of S, the light absorption behaviour was significantly changed from M1 to M20. In particular, the absorption of visible light increased by about one order of magnitude. The band gap of Bi2O2CO3 without sulfur is fitted as 3.27 eV, and the introduction of S leads to the emergenceof a narrow band gapby lowering the conduction band position and meanwhile generating impurity levels [35,36]. The adsorption edge is around 380 nm. With the increase of S content, defects and oxygen vacancies increase, possibly due to point defects, and the fitted narrow band gap decreases from 3.25 to 2.20 eV. Energy levels of the valence band maximum (EVB) were measured by the ultraviolet photoelectron spectrometer at UV intensity 500 nW and energy levels of the conduction band minimum (ECB) were calculated by the bandgap. As shown in Figure 7, valence band edge position and conduction band edge position become more negative after the incorporation of sulfur into Bi2O2CO3.
The SEM observation showed that chemical bath treatment had little influence on the morphology of the Bi2O2CO3 particles. EDS (energy dispersive spectroscopy) elemental mapping in Figure 8 revealed the homogeneous distribution of S on the particle surface, and no obvious segregation and aggregation can be seen among the particles. The quantitative elemental analysis results are shown in Table 2. The S content in samples M1~M20 increases with the increase of S: Bi2O2CO3 molar ratio n, but the S atom percentage (referring to Bi-content) is obviously smaller than n and becomes stable as n is greater than 0.10. This is consistent with the calculations about the surface adsorption of Bi2O2CO3 by Chang [34], who suggested that S2− can be adsorbed in the oxygen vacancy of the (001) plane via the chemical bonding and reduce the surface energy. The calculation of the density of states near the Fermi level shows that the doping of S can introduce a new energy level in the energy band and reduce the band gap. The electron state density near the Fermi surface is more diffusive, which favours the migration of electrons and therefore improves the photocatalytic performance.

2.2. Ultraviolet-Visible Light Photocatalytic Properties of Bi2O2(CO3)1−xSx

The photocatalytic activity of Bi2O2(CO3)1−xSx was characterised by photocatalytic degradation of Congo Red. As is shown in Figure 9, the introduction of S could improve the photocatalytic activity of Bi2O2CO3 under visible light and UV light. We measured the dye adsorption before switching on the light and normalized the concentrations, which made initial values of c/c0 equal to 1 for all samples. The operation temperature used was around 0 °C. With pure Bi2O2CO3, the Congo Red degrades by 41.6% under the irradiation of visible light for 3h, and by 46.1% under that of UV light, respectively. With the increase of molar ratio of S: Bi2O2CO3 from 0.01 to 0.1, the degradation rate increases to 64.2% and 70.1%, respectively. The further increase of n, however, cannot further remarkably increase the degradation rate. At the highest molar ratio of S(0.2), the photocatalytic activity of Congo Red was 65.3% and 71.4%, respectively, which was 1.57 and 1.55 times higher than that of Bi2O2CO3, respectively. The photo-degradation behavior of CR by use of Bi2O2(CO3)1−xSx obeys pseudo-first-order kinetics. This can be fitted by the Langmuir–Hinshewood model of ln(C0/C) = kt + A, where k is the reaction rate constant, t is the degradation time and the intercept A is the initial value of ln(C0/C), which means the dark adsorption of substrates. The k value of M1, M2, M5, M10 and M20 under UV light is 4.3 × 10−3 min−1, 5.5 × 10−3 min−1, 6.1 × 10−3 min−1, 6.8 × 10−3 min−1 and 6.9 × 10−3 min−1, respectively. The k value under visible light is 3.0 × 10−3 min−1, 3.5 × 10−3 min−1, 4.7 × 10−3 min−1, 5.5 × 10−3 min−1 and 5.9 × 10−3 min−1, respectively. The strong visible light sensitivity indicates higher utilization efficiency of solar light, making Bi2O2(CO3)1−xSx a superior photocatalyst than the commercial P25 TiO2, which has been reported to be hardly able to respond to visible light [37,38].
Chang’s theoretical calculations [34] suggest that S can be easily captured and adsorbed by oxygen vacancies on the surface of Bi2O2CO3 as formed S2− can partially substitute CO32− without forming a second phase, introducing a bend built-in electric field. At the same time, their experiments also confirmed that Bi2O2(CO3)1−xSx had higher conductivity and better carrier transport performance. The photoluminescence (PL) spectra of different S-substituted Bi2O2(CO3)1−xSx (Figure 10) show that samples M10 and M20 displayed weaker electron holes and recombination, indicating that the introduction of S can effectively suppress the carrier recombination. The stronger light absorption contributed by the smaller band gap means more photo-induced electron hole generation, and those electron holes showed better separation according to PL spectra. It is worthnoting that M20 has astronger light absorption and smaller bandgap than thatof M10, but that they presentnearly the same photocatalytic activity, which may be caused by the smaller specific surface area (Table 1) and slightlyweaker separation (Figure 10) of M20. Thus, all the three factors helped enhance the photocatalytic performance of Bi2O2CO3 in our samples under UV and visible light irradiation.

3. Materials and Methods

3.1. Preparation of the Precursor Powder Bi2O2CO3 via Hydrothermal Method

Three grams of urea (≥99.0%, Beijing Modern Orient Fine Chemistry Co. Ltd., Beijing, China) was dissolved in 60 mL of deionized water in a Teflon hydrothermal tank. 4.65 g Bi2O3 powder (99.99%, Aladdin Industrial Corporation, Shanghai, China) was then introduced into the solution. The hydrothermal tank was then tightly closed and kept in an oven at 180 °C for 12 h. After cooling down to room temperature, the precipitate was separated and washed with deionized water and ethanol several times and then dried in the oven at 70 °C.

3.2. Preparation of Bi2O2(CO3)1−xSx by Chemical Bath Precipitation

Five suspensions of Bi2O2CO3 were prepared, each by dispersing 2.04 g of Bi2O2CO3 powder in 50 mL of deionized water with the help of ultrasonic stirring for 10 min. A certain amount (S:Bi2O2CO3 ratio n, equals to 0.01, 0.02, 0.05, 0.10 and 0.20, respectively) of 0.5 mol/L Na2S (≥98.0%, Shanghai Tongya Chemical Technology Co. Ltd., Shanghai, China) solution was introduced into the respective suspensions. After 8 h of further magnetic stirring at room temperature, the precipitates were separated and washed several times with deionized water and ethanol and dried at 70 °C. As-treated powders were numbered as M1, M2, M5, M10 and M20, respectively.

3.3. Characterization

Powder X-ray diffraction (XRD) was completed on a diffractometer (D8-Advance, Bruker, Billerica, MA, USA)using monochromatized Cu Kα (λ = 0.15418 nm) radiation with scanning speed of 3°/min. The morphologyof the sampleswerecarried out on a scanning electron microscope (JSM-7001F, JEOL, Tokyo, Japan) operating at a 5 kV and a field emissionelectron microscope (JEM-2100F, JEOL). The surface areas of specimens were tested on a automated gas sorption anslyser (Quantachrome, autosorb iQ2). The X-ray photoelectron spectroscopic (XPS) measurements were performed on a Thermo Fisher ESCALAB 250Xi instrument. A UV-Vis-NIR spectrometer (Lambda 950, PerkinElmer, Waltham, MA, USA) was used to measure UV-Vis diffuse reflectance spectra (DRS). Energy levels of the valence band maximum (EVB) were measured by the ultraviolet photoelectron spectrometer (AC-2, RIKEN KEIKI, Tokyo, Japan).

3.4. Photocatalytic Test

The photocatalytic activity of the prepared Bi2O2(CO3)1−xSx powder samples was evaluated by photodegrading Congo Red (CR, 100 mg/L) aqueous solution.The reason we chose this concentration is because it is proper to evaluate the change of the color. 0.16 g photocatalyst powder specimen was dispersed into 80 mL CR solution and stirred in the dark for 2 h to reach theadsorption–desorption equilibrium between the photocatalysts and organic dye molecules. Magnetic stirringanda cooling-water bath were held continuously to prevent thermal effect during the degradation process and tokeep the uniformity. A 5W LED with emission wavelength of 365 ± 5 nm and a 300 W xenon lamp with 420 nm cut-off filters were used as the UV (365~800 nm) and visible light sources (420~800 nm), respectively.The incident light source was placed above the aqueous solution vertically, and the illumination intensity for UV and visible lights at upper surface of the solution were about 78 mW/cm2 and 132 mW/cm2. The photocatalytic processes were conducted under constant temperature, using ice water to cool the system. At the end of regular time intervals, 3 mL suspension was collected and centrifuged, and the residual CR concentrationin the supernatant fluid was analyzed by UV-vis spectrophotometer (UV−3100, Hitachi, Tokyo, Japan).

4. Conclusions

AnNa2S chemical bath treatment of Bi2O2CO3 did not generate a second phase. It is shown that the introduction of S can effectively broaden the optical absorption range, although it does not apparently change the crystal structure of Bi2O2CO3. The electrons at the top of the valence band in Bi2O2(CO3)1−xSx can be excited by shorter wavelengths of sunlight, forming photo-generated electron-hole pairs. This may be due to the formation of chemical bonds between the S2− and vacancies on the surface of Bi2O2CO3 crystal, which can affect the surface properties.
Bi2O2(CO3)1−xSx can improve the catalytic performance of visible and UV regions to a certain extent by the introduction of S in Bi2O2CO3 by chemical bath. This is because the introduction of S can effectively suppress the carrier recombination and improve the carrier transport performance. However, S can be introduced only into the surface of Bi2O2CO3 by chemical bath at room temperature, and the improvement of catalytic performance is limited.

Author Contributions

Y.L. and J.D. designed the project; J.D. conducted the most experiments; L.Q. and H.X. performed party of the experiments; J.D. and H.W. together wrote and revised the manuscript with input from all the authors. C.N. and Y.L. took part in discussing and the revision of the manuscript.

Acknowledgments

This work was supported by National Natural Science Foundation of China (no. 51221291, no. 51328203 and 51532003).

Conflicts of Interest

The authors declare no conflict of interest.

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Materials 11 00791 g001 550
Figure 1. XRD pattern of hydrothermal synthesised Bi2O2CO3.
Figure 1. XRD pattern of hydrothermal synthesised Bi2O2CO3.
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Materials 11 00791 g002 550
Figure 2. SEM photograph of hydrothermal synthesised Bi2O2CO3.
Figure 2. SEM photograph of hydrothermal synthesised Bi2O2CO3.
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Materials 11 00791 g003 550
Figure 3. HRTEM images of M0 (a); (b) and M20 (c); (d).
Figure 3. HRTEM images of M0 (a); (b) and M20 (c); (d).
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Materials 11 00791 g004 550
Figure 4. (a) XRD patterns of Bi2O2(CO3)1−xSx prepared by chemical bath precipitation; (b) the position of the (013) diffraction.
Figure 4. (a) XRD patterns of Bi2O2(CO3)1−xSx prepared by chemical bath precipitation; (b) the position of the (013) diffraction.
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Materials 11 00791 g005 550
Figure 5. XPS spectra of M0, M1, M2, M5, M10 and M20, Bi-4f (a); C−1s (b); O−1s (c); and S-2p (d).
Figure 5. XPS spectra of M0, M1, M2, M5, M10 and M20, Bi-4f (a); C−1s (b); O−1s (c); and S-2p (d).
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Materials 11 00791 g006 550
Figure 6. (a) UV-Vis diffuse reflectance spectra of the synthesized Bi2O2(CO3)1−xSx; (b) band gap fitting with K-M relation.
Figure 6. (a) UV-Vis diffuse reflectance spectra of the synthesized Bi2O2(CO3)1−xSx; (b) band gap fitting with K-M relation.
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Materials 11 00791 g007 550
Figure 7. Energy levels of the conduction band minimum (ECB, red) and the valence band maximum (EVB, black) calculated at theoretical pH = 0 (V is voltage; NHE is normalhydrogen electrode potential).
Figure 7. Energy levels of the conduction band minimum (ECB, red) and the valence band maximum (EVB, black) calculated at theoretical pH = 0 (V is voltage; NHE is normalhydrogen electrode potential).
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Materials 11 00791 g008 550
Figure 8. EDS element mapping details of M20 particles.
Figure 8. EDS element mapping details of M20 particles.
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Figure 9. Degradation of Congo Red under the irradiation of (a,c) UV, and (b,d) visible light, with Bi2O2(CO3)1−xSx; (e) the degradation rate as a function of n (=S:Bi2O2CO3).
Figure 9. Degradation of Congo Red under the irradiation of (a,c) UV, and (b,d) visible light, with Bi2O2(CO3)1−xSx; (e) the degradation rate as a function of n (=S:Bi2O2CO3).
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Materials 11 00791 g010 550
Figure 10. Photoluminescence spectra of Bi2O2(CO3)1−xSx.
Figure 10. Photoluminescence spectra of Bi2O2(CO3)1−xSx.
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Table
Table 1. Surface area and percentage of crystallinity of the Bi2O2CO3 and M1~M20 powders.
Table 1. Surface area and percentage of crystallinity of the Bi2O2CO3 and M1~M20 powders.
M0M1M2M5M10M20
Surface area (m2/g)0.9170.9730.9801.6661.8230.966
Percentage of crystallinity (%)--74.43 ± 0.9665.62 ± 0.6174.14 ± 0.8877.31 ± 0.7579.87 ± 1.75
Table
Table 2. EDS quantitative results of the M0~M20 powders.
Table 2. EDS quantitative results of the M0~M20 powders.
M0M1M2M5M10M20
C K43.7843.8843.9044.1144.3044.41
O K45.5345.3045.3045.2745.1745.10
S K--0.040.060.110.240.29
Bi M10.6910.7810.7410.5110.2910.20
x00.0070.0110.0210.0470.057

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MDPI and ACS Style

Ding, J.; Wang, H.; Xu, H.; Qiao, L.; Luo, Y.; Lin, Y.; Nan, C. Synthesis and Broadband Spectra Photocatalytic Properties of Bi2O2(CO3)1−xSx. Materials 2018, 11, 791. https://doi.org/10.3390/ma11050791

AMA Style

Ding J, Wang H, Xu H, Qiao L, Luo Y, Lin Y, Nan C. Synthesis and Broadband Spectra Photocatalytic Properties of Bi2O2(CO3)1−xSx. Materials. 2018; 11(5):791. https://doi.org/10.3390/ma11050791

Chicago/Turabian Style

Ding, Junping, Huanchun Wang, Haomin Xu, Lina Qiao, Yidong Luo, Yuanhua Lin, and Cewen Nan. 2018. "Synthesis and Broadband Spectra Photocatalytic Properties of Bi2O2(CO3)1−xSx" Materials 11, no. 5: 791. https://doi.org/10.3390/ma11050791

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