Open Access

Zinc Oxide Coating Effect for the Dye Removal and Photocatalytic Mechanisms of Flower-Like MoS2 Nanoparticles

Nanoscale Research Letters201712:221

https://doi.org/10.1186/s11671-017-2005-0

Received: 9 February 2017

Accepted: 16 March 2017

Published: 23 March 2017

Abstract

Flower-like MoS2 nanoparticles (NPs) consist of ultra-thin MoS2 nanosheets are synthesized via a facile one-pot hydrothermal method. The MoS2/ZnO p-n heterostructure is formed by coating n-type ZnO on the surface of flower-like MoS2 NPs through the seed-mediate route and post-annealing treatment. The effects for the dye removal and photocatalytic performances after ZnO coating are systematically investigated. The results demonstrated that the coating of ZnO nanoparticles has a positive promotion to the photodegrading properties while negative effect on the adsorption capacity of the MoS2/ZnO heterostructures. The related mechanisms on the relationship of adsorption capacity and photocatalysis are discussed in detail.

Keywords

Molybdenum disulfide Zinc oxide Absorbance Photocatalyst p-n heterostructure

Background

Synthetic dyes are massively produced and widely used in many areas nowadays, while most of them are the hazardous materials in the wastewater. Because they are environmentally harmful and not quite prone to degradation, the daily life and health of human beings are imperceptibly influenced by these synthetic dyes [1]. Therefore, the development of efficient methodology or technology to decompose these synthetic dyes becomes emergency issues for environment remediation. Various reports demonstrated that adsorption and photocatalytic degradation are the conventional, effective, and economical methodologies in wastewater purification and environmental protection over the past decades [24].

From a technical point of view, semiconductor-based photocatalysts with excellent photoelectric properties have always been the candidates for environmental remediation and clean energy, including metallic oxides (TiO2, ZnO, Fe2O3) [510], metallic sulfides (CdS, MoS2, CdSe) [1114], and metallic phosphides (InP, Ni2P) [15, 16]. Among those photocatalysts, the two-dimensional (2D) transition-metal dichalcogenides (TMDs) have received an increasing attention for the strong anisotropy of their electrical, chemical, mechanical and thermal properties. Molybdenum disulfide (MoS2) is one of the most studied examples in recent years [1719]. Interestingly, MoS2 has enormous potential application value in the field of low-cost adsorbents and environmental friendly photocatalysts because of its tunable band gap (1.29–1.9 eV) and morphology [20].

In fact, the MoS2-based composite photocatalysts that are coupled with TiO2, ZnO, CdS, or reduced graphene oxide (RGO) have been reported recently [11, 2124]. For example, the P-doped 2D-2D ZnO/MoS2 nanocomposites show excellent photocatalytic activity in methyl blue degradation [22]. The P-doped ZnO nanosheets were prepared through conventional chemical vapor transportation and condensation (CVTC) method, and the 2D MoS2 was prepared via liquid exfoliation method, then the ZnO nanosheets/MoS2 hybrid photocatalysts were formed by ultrasonically handling and magnetically stirring. This was a complicated preparation process, and the ZnO and MoS2 will be in loose contact with each other only by physically mixing, which is not beneficial for the efficient transfer of energy and carriers. In addition, most of the previous studies on MoS2-based composite photocatalysts reveal that the enhanced photocatalytic performance could be attributed to the synergetic effect of effective light-response, p-n heterojunctions, and large surface areas. However, there are scarcely researches that focused on the influence of the coating effect to the relationship between adsorption capacity and photocatalysts. Indeed, the adsorption and desorption equilibrium between the dyes and the photocatalysts before light illumination show positive promotion effect on the photodegradation process. It has been reported that strong surface adsorption performance is beneficial for the effective degradation of organic dyes during the photocatalytic reaction [25, 26]. For example, the BiOI microspheres have more effective surface adsorption than random BiOI nanoplatelets, which lead to more excellent performance for the degradation of tetracycline hydrochloride (TC) [27].

Therefore, the relationship of adsorption and photocatalysts need to be understood before the application. Good adsorption ability means the organic dyes tend to be in closer contact with the photocatalysts, which is beneficial for the transmission of photogenerated carriers from photocatalysts to organic dye molecules. Strong surface adsorption ability portends more active sites for the photodegrading reaction as well [3]. Moreover, different components will lead to dual removal mechanisms between surface adsorption and photocatalytic degradation in the process of organic dye removal. For instance, the composite photocatalysts combining TiO2 with highly adsorptive multi-walled carbon nanotubes (MWCNT) demonstrated high removal rate of methyl orange (MO) dyes in aqueous solutions [28].

Herein, we prepared the MoS2/ZnO heterostructures by coating the tunable ZnO layers onto the surface of flower-like MoS2 nanoparticles with facile methods. The adsorption and photocatalytic abilities of MoS2 NPs have been investigated before and after ZnO coating. The adsorption results illustrate MoS2 is the main contributor to the adsorption capacity, which is non-selective adsorption to the organic dyes. After ZnO coating, the adsorption capacity is decreasing and the photocatalytic ability is increasing. And hence the relationship between the surface adsorption and photocatalytic degradation was discussed in detail.

Methods

Materials and Chemicals

Sodium molybdate dehydrate (Na2MoO4 · 2H2O), thiourea (CS(NH2)2), and ethanol (C2H5OH) were purchased from Sinopharm Chemical Reagent Co., Ltd. Ammonia (NH3 · H2O, 25%) and zinc acetate (Zn(CH3COO)2), Rhodamine B (RhB), methyl blue (MB), Rhodamine 6G (Rh6G), and methyl orange (MO) were purchased from Shanghai Jingchun Chemical Reagent Co., Ltd. All the used reagents were analytically pure (AR) without any further purification.

Synthesis of MoS2 Nanoparticles

In a typical process, 93.75 mg of Na2MoO4 · 2H2O and 185 mg of thiourea was dispersed into 30 ml of H2O by rigorous stirring for 5 min. Then, 1 ml of concentrated hydrochloric acid (35% wt.) was added into the solution with stirring to form a homogenous mixture. The mixture was transferred into a 50-ml Teflon-lined autoclave after another 5 min continuous stirring. Finally, the sealed autoclave was placed into the oven and kept for 24 h at 200 °C. The precipitate was centrifuged and sequentially washed by H2O for several times. The as-synthesized products were dried (60 °C, 12 h) for further measurement.

Synthesis of MoS2/ZnO Heterostructural Photocatalyst

Fifteen milligrams of as-synthesized MoS2 nanoparticles were dispersed in a flask containing 22.5 ml of H2O under stirring. Then, 12.5 ml of Zn(CH3COO)2 solution with certain concentration (0.01, 0.02, 0.03, 0.05, and 0.1 M) were added into the mixture and subsequently heated to 40 °C. And then 4 ml of ammonia (5% wt) was added dropwise into the above mixture. After 1 h, the mixture was centrifuged at 5000 rpm. The precipitate was washed to remove the CH3COO and dried, and the final as-obtained powders were annealed under vacuum at 200 °C for 2 h. The theoretical mass proportion can be calculated as MoS2/ZnO (3:2), MoS2/ZnO (3:4), MoS2/ZnO (3:6), MoS2/ZnO (3:10), and MoS2/ZnO (3:20).

Adsorption and Photocatalytic Degradation Test

For the adsorption tests, 10 mL of organic dyes (RhB, MB, MO, and Rh6G) in aqueous solution with different concentrations were added into the quartz tube with 5 mg of the as-prepared samples. The suspension was homogenized by sonication and placed in the dark environment with continuous vigorous stirring. The adsorption/desorption equilibrium curves were measured at 5-min intervals by the UV-vis spectra on the Shimadzu UV-2550 spectrophotometer. The photocatalytic performances of MoS2/ZnO heterostructures were characterized by investigating the degradation of RhB with 10 mg/L. The preliminary homogenized solutions were illuminated under the simulated sunlight environment after reaching the adsorption/desorption equilibrium. The light source is mercury and tungsten mixed light lamp (300 W). And the corresponding UV-vis spectra were measured at 15 min intervals.

Characterization

Scanning electron microscopy (SEM) was carried out on a FEI Nova 400 NanoSEM at accelerating voltage of 20 kV. Transmission electron microscopy (TEM), high-resolution TEM (HRTEM) images, and energy-dispersive X-ray spectroscopy (EDX) were performed on a JEOL JEM-2100F transmission electron microscope at 200 kV. The X-ray diffraction (XRD) patterns were recorded in a PANalytical X'Pert PRO X-ray diffractometer with Co Ka radiation. X-ray photoelectron spectroscopy (XPS) analysis was performed on a Thermo Fisher ESCALAB 250Xi system equipped with a monochromatic Al Ka (1486.6 eV) as the radiation source.

Results and Discussion

The morphology of the as-obtained naked MoS2 nanoparticles are characterized by SEM and TEM. The representative SEM image is shown in Fig. 1a, in which the surface of flower-like MoS2 nanoparticles consisted of several or even single layers of ultra-thin MoS2 nanosheets. The average size of individual flower-like MoS2 nanoparticle is about 200 nm. As shown in Fig. 1c, high-resolution TEM image demonstrates that the thickness of MoS2 monolayer is ca. 0.7 nm, and the nanosheets consisted of about two to five layers, which could be indexed well with the theoretical thickness of MoS2 monolayer (S–Mo–S unit cell) [29, 30]. The EDX spectra of as-obtained MoS2 nanoparticles are shown in Fig. 1b, the elements of Mo, S, C, and Cu could be found. The structure of the naked MoS2 nanoparticles is further characterized by XRD (Fig. 1d), all the characteristic peaks can be assigned to the molybdenite-2H phase of MoS2 (JCPDS card no. 37–1492). The above results reveal the successful synthesis of MoS2 NPs.
Fig. 1

The SEM (a) and TEM (c) images of as-obtained naked MoS2. (Inset of Fig. 1c shows the HRTEM) and (b, d) are the EDX and XRD spectrum

Subsequently, the MoS2/ZnO heterostructures with different concentrations of zinc precursor are prepared. The detailed microstructural characterizations are presented in Fig. 2a–e, which show that the ZnO nanoparticles were successfully deposited on the surface of MoS2. Along with the increase of the concentration of Zn2+, both of the sizes and coverage area of ZnO nanoparticles are increased gradually. Compared with the uncoated MoS2 nanoparticles (Additional file 1: Figure S1), the morphology of MoS2/ZnO (3:2) shows no significant change because only a few ZnO nanoparticles are coated on the surface of MoS2 (Fig. 2a). When the Zn2+ is increased to 0.02 M, some small ZnO particles appeared (as marked by the red circle in Fig. 2b). When the Zn2+ concentration further increases to 0.03 M, most of MoS2 are coated by ZnO nanoparticles, the uncovered area of MoS2 was marked with red cycle in Fig. 2c. In addition, the size of ZnO nanoparticles grew much larger than 0.02 M. In Fig. 2d, the SEM image of MoS2/ZnO (3:10) shows that all the surface of MoS2 was covered with ZnO nanoparticles and the ZnO nanoparticles presented as triangle-shape. When the Zn2+ concentration elevated to 0.1 M, the ZnO particles with spindle-like structure that appeared on the surface of MoS2 nanosheets are observed. The TEM images of MoS2/ZnO are shown in Fig. 2a′–e′, displaying the gradual change of morphology during the ZnO coating process. From the corresponding high-resolution TEM images (inset), the (101) and (100) crystal planes of ZnO were observed, revealing the successful formation of ZnO nanoparticles on the surface of MoS2. The EDX and XRD techniques are employed for furtherly characterizing the elemental composition of as-obtained MoS2/ZnO heterostructure (MoS2/ZnO (3:10)). The EDX spectroscopy in Fig. 2f reveals the elements of Mo, S, Zn, C, and O. The XRD diffraction (Fig. 2g) peaks of MoS2/ZnO along with the JCPDS card for hexagonal ZnO (36–1451) and the diffraction signals of MoS2 are hardly observed, except for (002) plane (marked by “▲”), because the diffraction signals of ZnO is too strong and concealed the diffraction signals of MoS2. No other additional peaks corresponding to impurities are found, indicating the purity of the sample.
Fig. 2

The SEM and TEM images of MoS2/ZnO with different mass proportion: (3:2) (a, a′), (3:4) (b, b′), (3:6) (c, c′), (3:10) (d, d′), and (3:20) (e, e′). Inset in (b′, c′, d′, e′) are the corresponding HRTEM images. The EDX (f) and XRD (g) spectra results from MoS2/ZnO (3:10)

The element valence in the naked MoS2 and MoS2/ZnO heterostructures (MoS2/ZnO (3:10)) are characterized by XPS. The full survey spectrum in Fig. 3a reveals the co-presence of Mo, S, O, C, and Zn elements. In the high-resolution XPS spectra of Mo 3d (Fig. 3b), two peaks are located at 232.4 and 229.2 eV, which could be attributed to Mo 3d 3/2 and Mo 3d 5/2 of Mo4+ in MoS2, respectively. The peak at 226.5 eV is indexed to S 2s. The peak positioned at the binding energy of 161.7 and 163.1 eV in S 2p spectra (Fig. 3c) are indexed to S2− ions in the Mo–S bonding of the molybdenite-2H phase of MoS2, respectively. After coating with ZnO, the binding energies of 232.3, 229.1, 161.4, and 162.8 eV can be ascribed to Mo 3d 3/2, Mo 3d 5/2, S 2p 1/2, and S 2p 3/2, respectively (Fig. 3e, f). And the main peaks of Zn 2p at 1044.8 and 1021.7 eV are characteristic peaks of the Zn 2p 1/2 and Zn 2p 3/2 of ZnO, respectively (Fig. 3d). The asymmetric peaks at 235.4 eV could be indexed to Mo (VI) 3d, indicating the oxidation of a small amount of Mo [13, 31]. The TEM, XRD, and XPS results illustrate the successful preparation of MoS2/ZnO heterostructures.
Fig. 3

a The survey XPS spectra of naked MoS2 (blue line) and MoS2/ZnO heterostructure (MoS2/ZnO (3:10), red line). The high-resolution spectra of b Mo 3d, S 2s and c S 2p peaks for the MoS2 and the main satellite peaks of d Zn 2p, e Mo 3d, S 2s, and f S 2p for the MoS2/ZnO (3:10), respectively

The photodegradation performances of MoS2/ZnO heterostructures are investigated by the degradation of RhB dyes as a model experiment under illumination of simulated sunlight. Figure 4a shows the comparison of photocatalytic activity of bare control, pure ZnO nanoparticles, and as-obtained MoS2/ZnO heterostructures. All the curves are normalized after reaching the adsorption/desorption equilibrium. The results demonstrated that 68.3% of the RhB dyes can be degraded after 90 min light irradiation at the presence of pure ZnO. In contrast, MoS2/ZnO heterostructures show enhanced photocatalytic performance and more than 91.4% of the RhB can be degraded. Moreover, the photocatalytic properties show increasing tendency from MoS2/ZnO (3:4) to MoS2/ZnO (3:6) and reach the highest at MoS2/ZnO (3:10). However, the MoS2/ZnO (3:20) heterostructures show decreased photocatalytic abilities than MoS2/ZnO (3:10), which could be attributed to high mass percentage of ZnO (with poor photodegradation performance), and finally decreased the total degradation performance of MoS2/ZnO heterostructures. Generally, the reaction kinetics of photocatalytic degradation is followed by the pseudo first-order rate model: [6].
Fig. 4

a The comparison degradation performance of MoS2/ZnO (3:4), MoS2/ZnO (3:6), MoS2/ZnO (3:10), MoS2/ZnO (3:20) heterostructures, and pure ZnO: the curves are normalized after the adsorption/desorption equilibrium in dark for 30 min. b The corresponding kinetic characters of photocatalytic degradation

$$ - \ln \left( C/{C}_0\right) = k t $$
(1)

where k is the photodegradation rate. In Fig. 4b, the k value increased 3.7 times from 1.26 × 10−2 min−1 for pure ZnO nanoparticles to 4.71 × 10−2 min−1 for MoS2/ZnO (3:10) heterostructure. And the photodegradation rate of the MoS2/ZnO (3:4), MoS2/ZnO (3:6), and MoS2/ZnO (3:20) are 2.88 × 10−2 min−1, 3.29 × 10−2 min−1, and 3.01 × 10−2 min−1, respectively. The enhanced photodegradation activities of the as-obtained MoS2/ZnO heterostructures could be attributed to the p-n heterojunction that formed between MoS2 and ZnO at the contact interface, and the induced high separation rate of photogenerated electrons and holes.

The schematic illustrations of photocatalysis mechanisms are shown in Fig. 5, when the n-type semiconductor ZnO contact with the p-type semiconductor MoS2, the highest occupied conduction band (CB) and the valence band (VB) of ZnO situate below the energy band of MoS2 after reaching the same Fermi level due to the different work functions of the MoS2 (5.39 eV) [32, 33] and ZnO (4.7 eV) [29, 34]. Then, the photogenerated electrons at the CB of MoS2 can overcome the barrier and transfer to the CB of ZnO; meanwhile, the photogenerated holes will be in a position to transfer from the VB of ZnO to the VB of MoS2. Consequently, the photogenerated electron-hole pairs are separated efficiently at the contact interfaces of MoS2 and ZnO, thus, improving the photocatalytic abilities of the heterostructural catalysts finally.
Fig. 5

Schematic illustration of MoS2/ZnO heterostructures and the charge transfer process occurring between MoS2 and ZnO at the interface

Meanwhile, when we measured the photocatalytic performance of MoS2/ZnO, it can be found that the surface adsorption plays an important influence in photocatalytic degradation process. It can be seen that 99% of RhB dyes can be absorbed by naked MoS2 nanoparticles before the light illumination (Fig. 6a), while 27.7% of RhB dyes are absorbed when using the MoS2/ZnO (3:10) heterostructures as the photocatalysts (Fig. 6b). Thus, we measured the absorption capacities of different samples in dark environment for 30 min. The comparative absorbance of all the samples was carried out in Fig. 6c. It can be seen that the MoS2/ZnO photocatalysts exhibit decreased adsorption capacity along with the increasing of the concentration of Zn precursor. Obviously, the ZnO coating can prevent the MoS2 to adsorb the dyes. The adsorption abilities of MoS2/ZnO photocatalysts are better than pure ZnO nanoparticles (12%, red dotted line in Fig. 6c). Furthermore, the naked MoS2 after annealing treatment show decreased adsorption abilities, only 89% of the RhB dyes were adsorbed. The reason may be resulted from the surface morphologic change of the flower-like MoS2 nanoparticles (Additional file 1: Figure S1) that decreases the adsorption sites. The corresponding Brunauer-Emmett-Teller specific surface areas (S BET ) of MoS2 nanoparticles before and after annealing were investigated by nitrogen adsorption (Beishide, 3H-2000PS2). In contrast, the S BET for flower-like MoS2 nanoparticles is about 54.7 m2/g, which is much larger than that of MoS2 nanoparticles after annealing treatment with a surface area of 13.2 m2/g (Additional file 1: Figure S2). The reason was largely attributed to the morphologic change of MoS2 nanoparticles, resulting in the decrease of the adsorption capacities to MG dyes finally.
Fig. 6

The UV-vis absorption spectra of naked MoS2 (a) and MoS2/ZnO (3:10) (b) heterostructures before light irradiation. c The comparison absorbance of all the samples and the corresponding absorbance percentage of RhB dyes: (a) blank RhB, (b) pure ZnO, (c) MoS2 before annealing, (d) MoS2 after annealing, (e) MoS2/ZnO (3:2), (f) MoS2/ZnO (3:4), (g) MoS2/ZnO (3:6), (h) MoS2/ZnO (3:10), and (i) MoS2/ZnO (3:20)

The selective adsorption to organic dyes is also a critical factor for the photocatalytic performance of catalyst. As the main contributor to the adsorption capacity of the MoS2/ZnO heterostructures, the adsorptive capacity of the naked MoS2 was further measured with different organic dyes, including RhB, Rh6G, MB, and MO. The as-selective dyes are very stable in routine environment. In addition, different concentrations of organic dyes (5, 10, and 20 mg/L) are tested. Additional file 1: Figure S3 displays the relationship between the adsorption time and concentrations. It is found that the adsorption process can be finished in 5 min, and there is no continued adsorption with prolonging adsorption time. The experiment results are in agreement with the report that the adsorption equilibrium can be reached in a relatively quick process of about 5 min [30]. The adsorption capacity is calculated based on the experimental dates and according to the mass balance relationship: [35].
$$ {Q}_{eq}=\left({C}_0-{C}_{eq}\Big) V/ m\right) $$
(2)
where Q eq is the amount of dye adsorbed onto the naked MoS2, and C 0 and C eq are the initial and equilibrated dyes concentrations, respectively. V is the volume of solution, and m is the mass of the adsorbent. Figure 7 shows the isotherms for dyes adsorption on the as-obtained naked MoS2 nanoparticles. All the adsorption isotherms that fitted to the experimental dates are modeled using the Langmuir and Freundlich isotherm (Table 1) [2]. The theoretical Langmuir and Freundlich isothermal parameters can be represented by the following Eqs. 3 and 4 [36, 37].
Fig. 7

The adsorption isotherms for a RhB, b MB, c MO, and d Rh6G on the as-obtained naked MoS2 nanoparticles

Table 1

Equilibrium Parameters for the Adsorption of RhB, MB, MO and Rh6G onto naked MoS2

 

Langmuir Fit

Freundlich Fit

 

\( {Q}_e=\frac{Q_{\max }{K}_L{C}_e}{1+{K}_L{C}_e} \)

\( {Q}_e={K}_F{C_e}^{\raisebox{1ex}{$1$}\!\left/ \!\raisebox{-1ex}{$\mathrm{n}$}\right.} \)

Dyes

Q max (mg/g)

K L (L/mg)

R 2

K F (mg1–1/n  L1/n  g−1)

n

R 2

RhB

55.22

6.43

0.98506

38.65

4.03

0.8628

MB

28.43

20.15

0.95061

23.10

5.99

0.9741

MO

18.65

0.80

0.97768

8.70

3.46

0.9999

Rh6G

18.79

10.25

0.99207

14.55

7.39

0.9794

Q e (mg/g) is the amount of dyes adsorbed onto the adsorbent at equilibrium, Q max (mg/g) is the maximum amount of adsorption, K L (L/mg) is the Langmuir adsorption equilibrium constant, K F (mg1–1/n  L1/n  g−1) is the Freundlich constant representing the adsorption capacity, n (dimensionless) is the constant depicting the adsorption intensity

$$ {Q}_{eq}=\frac{Q_{\max }{K}_L{C}_{eq}}{1+{K}_L{C}_{eq}} $$
(3)
$$ {Q}_{eq}={K}_F{C_{eq}}^{\raisebox{1ex}{$1$}\!\left/ \!\raisebox{-1ex}{$ n$}\right.} $$
(4)

Q e is the amount of dyes adsorbed onto the adsorbent at equilibrium, Q max is the maximum amount of adsorption, K L is the Langmuir adsorption equilibrium constant, K F is the Freundlich constant representing the adsorption capacity, and n is the constant depicting the adsorption intensity. The maximum adsorption capacities calculated from the experimental date for RhB, MB, MO, and Rh6G are 55.2, 28.4, 18.6, and 18.8 mg/g, respectively. The results reveal that the naked MoS2 has a non-selective adsorption to the organic dyes with perfect adsorption capacities. From the nonlinear-curve-fitting results (R 2), we can see that the Langmuir isotherm present well with the experimental dates than that of Freundlich isotherm for RhB (0.9851 > 0.8628) and Rh6G (0.9921 > 0.9794), while the adsorption value is concurred with agreement with the Freundlich model than Langmuir model from the regression coefficient R 2 of MB (0.9506 < 0.9741) and MO (0.9921 < 0.9999). For the comparison, the absorption capacity of pure ZnO particles is tested. The corresponding effect of contact time and concentration is shown in Additional file 1: Figure S4a. The maximum adsorption amount is only 2.4 mg/g (R 2 = 0.9985) from the Langmuir model fitting result in the Additional file 1: Figure S4b.

From the adsorption isotherm studies, we can draw the conclusion that the pure ZnO nanoparticles has a poor adsorption to RhB dyes, which decreased the adsorption capacity of MoS2/ZnO heterostructures. MoS2 nanoparticles act as the main adsorption substrate in the heterostructural system and show perfect and non-selective adsorption capacity to the organic dyes. The Langmuir and Freundlich modeled results can be confirmed that the organic dyes inhibited monolayer adsorption on the surface of MoS2 nanoparticles and further indicated that the homogeneous nature of MoS2 surface has a same adsorption capacity of all the surfaces [36]. Moreover, the adsorption intensity (1/n) gives an indication of the favorability of adsorption. When the n > 1 (or 10 > 1/n > 1), it represents favorable adsorption condition [38, 39]. The calculated values of n are listed in Table 1, confirming the favorable adsorption condition of dyes on the surface of MoS2 nanoparticles.

Conclusions

In summary, the naked flower-like MoS2 nanoparticles are synthesized successfully via a hydrothermal method. The MoS2/ZnO heterogeneous photocatalysts are synthesized and formed as p-n heterojunction. The coating of ZnO nanoparticles shows positive promotion to the photodegrading properties while negative effect on the adsorption capacity of the MoS2/ZnO heterostructures. The MoS2/ZnO (3:10) heterostructures showed 3.7 times than pure ZnO for the decomposition of RhB dyes. The adsorption property of naked MoS2 was further investigated with RhB, MB, MO, and Rh6G. The adsorption relationship was described with Langmuir and Freundlich isotherm, showing that the adsorption of dye molecules on the surface of MoS2 is monolayer adsorption and it is favorable for the adsorption of organic dyes in our study. We envision that the MoS2/ZnO photocatalysts will become a potential candidate in the field of environmental remediation.

Declarations

Acknowledgements

This work was supported by the National Natural Science Foundation of China (51171132 and 11375134), Hong Kong Scholars Program, Young Chenggang Project of Wuhan City (2013070104010011), China Postdoctoral Science Foundation (2014 M550406), Natural Science Foundation of Jiangsu Province (BK20160383), the Fundamental Research Funds for the Central Universities, and Wuhan University.

Authors’ Contributions

QYT completed all the experiments and wrote the manuscript. SLY, JL, and WJY assisted with the manuscript preparation. WW, FR, and CZJ conceived the study, revised the manuscript, and supervised the work. All authors read and approved the final manuscript.

Competing Interests

The authors declare that they have no competing interests.

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Authors’ Affiliations

(1)
School of Printing and Packaging and School of Physics and Technology, Wuhan University
(2)
Suzhou Research Institute of Wuhan University

References

  1. Forgacs E, Cserháti T, Oros G (2004) Removal of synthetic dyes from wastewaters: a review. Environ Int 30:953View ArticleGoogle Scholar
  2. Travlou NA, Kyzas GZ, Lazaridis NK, Deliyanni EA (2013) Functionalization of graphite oxide with magnetic chitosan for the preparation of a nanocomposite dye adsorbent. Langmuir 29:1657View ArticleGoogle Scholar
  3. Chen C, Ma W, Zhao J (2010) Semiconductor-mediated photodegradation of pollutants under visible-light irradiation. Chem Soc Rev 39:4206View ArticleGoogle Scholar
  4. Kyzas GZ, Siafaka PI, Lambropoulou DA, Lazaridis NK, Bikiaris DN (2014) Poly(itaconic acid)-grafted chitosan adsorbents with different cross-linking for Pb(II) and Cd(II) uptake. Langmuir 30:120View ArticleGoogle Scholar
  5. Liu J, Yang S, Wu W, Tian Q, Cui S, Dai Z, Ren F, Xiao X, Jiang C (2015) 3D flower-like α-Fe2O3@TiO2 core-shell nanostructures: general synthesis and enhanced photocatalytic performances. ACS Sustain Chem Eng 3:2975View ArticleGoogle Scholar
  6. Wu W, Zhang S, Xiao X, Zhou J, Ren F, Sun L, Jiang C (2012) Controllable synthesis, magnetic propertiesand enhanced photocatalytic activity of spindle-like mesoporous iron oxide/ZnO core-shell heterostructures. ACS Appl Mater Interfaces 4:3602View ArticleGoogle Scholar
  7. Sun L, Wu W, Yang S, Zhou J, Hong M, Xiao X, Ren F, Jiang C (2014) Template and silica interlayer tailorable synthesis of spindle-like multilayer α-Fe2O3/Ag/SnO2 ternary hybrid architectures and their enhanced photocatalytic activity. ACS Appl Mater Interfaces 6:1113View ArticleGoogle Scholar
  8. Tian Q, Wu W, Sun L, Yang S, Lei M, Zhou J, Liu Y, Xiao X, Ren F, Jiang C (2014) Tube-like ternary α-Fe2O3@SnO2@Cu2O sandwich heterostructures: synthesis and enhanced photocatalytic properties. ACS Appl Mater Interfaces 6:13088View ArticleGoogle Scholar
  9. Wu W, Jiang C, Roy VAL (2015) Recent progress on magnetic iron oxide-semiconductors composite nanomaterials as promising type of photocatalyst. Nanoscale 7:38Google Scholar
  10. Wu Z, Yang S, Wu W (2016) Shape control of inorganic nanoparticles from solution. Nanoscale 8:1237View ArticleGoogle Scholar
  11. Tian Q, Wu W, Liu J, Wu Z, Yao W, Ding J, Jiang C (2017) Dimensional heterostructures of 1D CdS/2D ZnIn2S4 composited with 2D graphene: designed synthesis and superior photocatalytic performance. Dalton Trans 46:2770View ArticleGoogle Scholar
  12. Zhai T, Fang X, Li L, Bando Y, Golberg D (2010) One-dimensional CdS nanostructures: synthesis, properties, and applications. Nanoscale 2:168View ArticleGoogle Scholar
  13. Zhou W, Yin Z, Du Y, Huang X, Zeng Z, Fan Z, Liu H, Wang J, Zhang H (2013) Synthesis of few-layer MoS2 nanosheet-coated TiO2 nanobelt heterostructures for enhanced photocatalytic activities. Small 9:140View ArticleGoogle Scholar
  14. Wu Y, Xu M, Chen X, Yang S, Wu H, Pan J, Xiong X (2016) CTAB-assisted synthesis of novel ultrathin MoSe2 nanosheets perpendicular to graphene for the adsorption and photodegradation of organic dyes under visible light. Nanoscale 8:440View ArticleGoogle Scholar
  15. Zeng G, Qiu J, Hou B, Shi H, Lin Y, Hettick M, Javey A, Cronin SB (2015) Enhanced photocatalytic reduction of CO2 to CO through TiO2 passivation of InP in ionic liquids. Chem-Eur J 21:13502View ArticleGoogle Scholar
  16. Popczun EJ, McKone JR, Read CG, Biacchi AJ, Wiltrout AM, Lewis NS, Schaak RE (2013) Nanostructured nickel phosphide as an electrocatalyst for the hydrogen evolution reaction. J Am Chem Soc 135:9267View ArticleGoogle Scholar
  17. Chhowalla M, Shin H, Eda G, Li L, Loh K, Hua Z (2013) The chemistry of two-dimensional layered transition metal dichalcogenide nanosheets. Nature Chem 5:263View ArticleGoogle Scholar
  18. Lu Q, Yu Y, Ma Q, Chen B, Zhang H (2016) 2D transition-metal-dichalcogenide-nanosheet-based composites for photocatalytic and electrocatalytic hydrogen evolution reactions. Adv Mater 28:1917View ArticleGoogle Scholar
  19. Wang F, Shifa T, Zhan X, Huang Y, Liu K, Cheng Z, Jiang C, He J (2015) Recent advances in transition-metal dichalcogenide based nanomaterials for water splitting. Nanoscale 7:19764View ArticleGoogle Scholar
  20. Mak K, Lee C, Hone J, Shan J, Heinz T (2010) Atomically thin MoS2: a new direct-gap semiconductor. Phys Rev Lett 105:136805View ArticleGoogle Scholar
  21. Hu K, Hu X, Xu Y, Sun J (2010) Synthesis of nano-MoS2/TiO2 composite and its catalytic degradation effect on methyl orange. J Mater Sci 45:2640View ArticleGoogle Scholar
  22. Liu Y, Xie S, Li H, Wang X (2014) A highly efficient sunlight driven ZnO nanosheet photocatalyst: synergetic effect of P-doping and MoS2 atomic layer loading. ChemCatChem 6:2522Google Scholar
  23. Min Y, He G, Xu Q, Chen Y (2014) Dual-functional MoS2 sheet-modified CdS branch-like heterostructures with enhanced photostability and photocatalytic activity. J Mater Chem A 2:2578View ArticleGoogle Scholar
  24. Li Y, Wang H, Xie L, Liang Y, Hong G, Dai H (2011) MoS2 nanoparticles grown on graphene: an advanced catalyst for the hydrogen evolution reaction. J Am Chem Soc 133:7296View ArticleGoogle Scholar
  25. Zhou Q, Zhong YH, Chen X, Liu JH, Huang XJ, Wu YC (2014) Adsorption and photocatalysis removal of fulvic acid by TiO2-graphene composites. J Mater Sci 49:1066View ArticleGoogle Scholar
  26. Tachikawa T, Takai Y, Tojo S, Fujitsuka M, Majima T (2006) Probing the surface adsorption and photocatalytic degradation of catechols on TiO2 by solid-state NMR spectroscopy. Langmuir 22:893View ArticleGoogle Scholar
  27. Hao R, Xiao X, Zuo X, Nan J, Zhang W (2012) Efficient adsorption and visible-light photocatalytic degradation of tetracycline hydrochloride using mesoporous BiOI microspheres. J Hazard Mater 209:137View ArticleGoogle Scholar
  28. Saleh TA, Gupta VK, Colloid J (2012) Photo-catalyzed degradation of hazardous dye methyl orange by use of a composite catalyst consisting of multi-walled carbon nanotubes and titanium dioxide. Interf Sci 371:101View ArticleGoogle Scholar
  29. Fang Y, Sha J, Wang Z, Wan Y, Xia W, Wang Y (2011) Behind the change of the photoluminescence property of metal-coated ZnO nanowire arrays. Appl Phys Lett 98:033103View ArticleGoogle Scholar
  30. Hao Y, Man C, Hu ZB (2010) Effective removal of Cu (II) ions from aqueous solution by amino-functionalized magnetic nanoparticles. J Hazard Mater 184:392View ArticleGoogle Scholar
  31. Wang PP, Sun H, Ji Y, Li W, Wang X (2014) Three-dimensional assembly of single-layered MoS2. Adv Mater 26:964Google Scholar
  32. Fontana M, Deppe T, Boyd AK, Rinzan M, Liu AY, Paranjape M, Barbara P (2013) Electron-hole transport and photovoltaic effect in gated MoS2 Schottky junctions. Sci. Rep. 3Google Scholar
  33. Choi S, Shaolin Z, Yang W, Korean J (2014) Layer-number-dependent work function of MoS2 nanoflakes. Phys Soc 64:1550Google Scholar
  34. Cornil D, Van Regemorter T, Beljonne D, Cornil J (2014) Work function shifts of a zinc oxide surface upon deposition of self-assembled monolayers: a theoretical insight. Phys Chem Chem Phys 16:20887View ArticleGoogle Scholar
  35. Yang S, Wu Z, Huang L, Zhou B, Lei M, Sun L, Tian Q, Pan J, Wu W, Zhang H (2014) Significantly enhanced dye removal performance of hollow tin oxide nanoparticles via carbon coating in dark environment and study of its mechanism. Nanoscale Res Lett 9:1View ArticleGoogle Scholar
  36. Malik P (2004) Dye removal from wastewater using activated carbon developed from sawdust: adsorption equilibrium and kinetics. J Hazard Mater 113:81View ArticleGoogle Scholar
  37. Parida SK, Mishra BK, Colloid J (1996) Adsorption of styryl pyridinium dyes on silica gel. Interf Sci 182:473View ArticleGoogle Scholar
  38. Vijayakumaran V, Arivoli S (2012) Equilibrium and kinetic modeling on the removal of malachite green from aqueous solution using odina wodier bark carbon. J Mater Environ Sci 3:525Google Scholar
  39. Ho Y, McKay G (1998) Sorption of dye from aqueous solution by peat. Chem Eng J 70:115View ArticleGoogle Scholar

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