# Aqueous Medium Synthesis Route for Randomly Stacked Molybdenum Disulfide

Authors: Pravas Kumar Panigrahi; Amita Pathak
Journal: Journal of Nanoparticles
 (2013)

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## Abstract

Synthesis of poorly crystalline, randomly oriented rag-like structures of molybdenum disulfide has been reported starting from aqueous solutions of ammonium molybdate, and thioacetamide in presence of sodium dodecyl sulfate via calcination of the amorphous precipitates, obtained through acidification of thein situ generated intermediate of ammonium tetrathiomolybdate. X-ray photoelectron spectroscopy, UV-visible spectroscopy, and X-ray diffraction of the calcined samples reveal the formation of single-phase MoS2, while the amorphous precipitates have been found to be a mixture of Mo2S5, MoS3, and a trace amount of H2MoS4. Highly folded and disordered layers of rag-like MoS2 have been confirmed through high-resolution transmission electron microscopy. The electrical conductivity for the cold pressed pellet of the MoS2 sample is found to be significantly higher than that of 2H-MoS2 and increases further on annealing.


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## Body

## 1. Introduction

Molybdenum disulfide (MoS2) is a hexagonal layer structured material. The MoS2 layers, each of which consists of a layer of molybdenum atoms sandwiched between two layers of sulfur atoms, are connected by weak van der Waals force. Due to the weak interactions between the sheets of sulfur atoms, MoS2 exhibits excellent lubrication property [1, 2]. It also finds applications as electrode in high-density lithium batteries [3], solar cells [4] in form of thin films, and as intercalation host to produce new materials [5, 6]. From a catalytic point of view, MoS2 possesses outstanding properties towards methanation of CO with hydrogen [7] and hydrodesulfurization reaction for removal of sulfur compounds from crude oil [8, 9]. It has been found that the catalytic activity of MoS2 strongly depends on the number of coordinatively unsaturated sites [10]. Thus, the catalytic activity of MoS2 is influenced by the particle size as well as the number of layers, demonstrating that the morphology is also an important parameter for such applications.Till date, MoS2 powders with different morphologies have been synthesized through a wide range of methods, such as thermal decomposition of ammonium tetrathiomolybdate or amorphous MoS3 [11, 12], reaction of stoichiometrically mixed molybdenum and sulfur powders in vacuum at high temperature [13], and gas-phase reactions of molybdenum oxides with H2S under reducing atmosphere [14, 15]. There are also reports on the use of other high-energy sources like laser [16], electron beam [17], and γ-radiation [18] for the synthesis of nanotubes, fullerene-like, and other curved nanostructures of MoS2. As an alternative to these methods, which require high temperatures/pressures and/or sophisticated instrumentations, solution-based synthesis routes have been developed [19–21] and have gained popularity due to their simplicity and convenience. For example, hydrothermal/solvothermal processes have been carried out at different temperatures (100–300°C) and incubation periods (12 h–3 days) by various research groups [22–25] to obtain fine powders of MoS2 with a variety of crystallinity. Among these reports, Li et al. [23] observed MoS2 nanoparticles with short range stacking of layers, when a solution containing (NH4)2Mo3S13 and hydrazine was treated hydrothermally at 180°C for 16 h. Sonochemical method [26] has also been explored to produce MoS2. Alternatively, Bezverkhy et al. [27] have synthesized highly dispersed MoS2 by using (NH4)2MoS4 and N2H4·H2O via aqueous medium precipitation method. The same group has also reported the formation of single layered MoS2 with short fringes, when processed in presence of an organic surfactant in the reaction mixture [28]. Similarly, Hu et al. [29] have prepared the ball-like MoS2 nanoparticles on calcining the amorphous molybdenum sulfide (MoSx), obtained through precipitation from the solution of Na2MoO4 and thioacetamide in water and alcohol. Recently, Wu et al. [30] have reported the preparation of poorly crystalline MoS2 nanospheres through calcination of MoS3 precursor obtained through precipitation in an aqueous medium in presence of polyethylene glycol.Considering the technical simplicity and versatility of the precipitation synthesis approaches, we have described here an aqueous solution-based precipitation route for the preparation of poorly crystalline MoS2 with randomly stacked layers using commonly available starting reagents. Unlike most of the previous reports, the composition of the precursor powders has been studied by XRD, XPS, and thermal analysis. The present paper also includes the optical and electrical studies of the calcined powders, which have not been widely reported for the poorly crystalline MoS2 nanostructures, prepared and studied so far in the literature.


## 2. Experimental

### 2.1. Synthesis

The preparation of MoS2 was carried out through modification of the method described in literature [31]. All the chemicals were purchased and used as received. To start, 30 mL of 0.008 M ammonium molybdate ((NH4)6Mo7O24·4H2O, Merck India, 98%) solution was taken, and sodium dodecyl sulfate (SDS) of 10 times of cmc (critical micelle concentration) was added to it under constant stirring to obtain a clear solution. Then, 9.60 mL of 0.23 M sodium dithionite (Na2S2O4, BDH, England, 98% pure) solution and 45 mL of 0.20 M thioacetamide (CH3CSNH2, Spectrochem India, 99%) solution were added into the former solution and were thoroughly mixed together by stirring. The solution mixture was heated (~90°C) over a water bath to obtain a clear reddish yellow color solution. Acidification of this solution with concentrated HCl (pH < 1) led to a dark brown colored precipitate. The precipitate was isolated using a centrifuge and was washed with water for several times. Drying of the precipitate gave rise to brownish black powders, which were calcined at 400°C for 2 h under argon atmosphere to obtain the black powders of MoS2.


### 2.2. Characterization

The optical absorption spectrum of the reddish yellow colored solution of the intermediate as well as the ethanol dispersion of the calcined powders were studied at room temperature using Shimadzu UV-1601 UV-visible spectrophotometer. The phase and structure analyses of the virgin and the calcined powders were carried out on X’pert Pro 3040/60 high-resolution X-ray diffractometer using Cu Kα radiation (λ = 1.5418 Å´). X-ray photoelectron spectra (XPS), using VG Microtech ESCA2000 Multilab apparatus, was obtained for the virgin and the calcined powders for determining the oxidation states of Mo and S in the respective samples. Thermal analysis of the dried precipitate was performed at the heating rate of 6°C per min under dynamic argon using Perkin-Elmer Pyris Diamond TG/Differential thermal analyzer and alumina as the reference. Transmission electron microscope of model JEOL2010 (UHR) was used to study the microstructure of the calcined powders. The FTIR spectrum of the precursor sample was taken on a Perkin Elmer Fourier transform analyzer (FTIR spectrometer RXI). Electrical conductivity measurement was carried out on pressed pellet of the as-prepared calcined powders of MoS2 using a computer-controlled HIOKI LCR HITESTER at an AC signal of 1.0 V. The surfaces of the pellets were coated with silver paint for electrical contact. Finally, the electrical connection of the pellet to the apparatus was made through nickel electrode and put in a temperature controlled furnace. The hydrodynamic size of the synthesized MoS2 sample was measured by using 90 Plus Particle Size Analyzer (made by Brookhaven Instruments). The BET (Brunauer-Emmett-Teller) specific surface area of the calcined sample was measured through nitrogen adsorption isotherms at 77 K by using Quantachrome Instruments (Autosorb-1, Model no. ASI-C-9).


## 2.1. Synthesis

The preparation of MoS2 was carried out through modification of the method described in literature [31]. All the chemicals were purchased and used as received. To start, 30 mL of 0.008 M ammonium molybdate ((NH4)6Mo7O24·4H2O, Merck India, 98%) solution was taken, and sodium dodecyl sulfate (SDS) of 10 times of cmc (critical micelle concentration) was added to it under constant stirring to obtain a clear solution. Then, 9.60 mL of 0.23 M sodium dithionite (Na2S2O4, BDH, England, 98% pure) solution and 45 mL of 0.20 M thioacetamide (CH3CSNH2, Spectrochem India, 99%) solution were added into the former solution and were thoroughly mixed together by stirring. The solution mixture was heated (~90°C) over a water bath to obtain a clear reddish yellow color solution. Acidification of this solution with concentrated HCl (pH < 1) led to a dark brown colored precipitate. The precipitate was isolated using a centrifuge and was washed with water for several times. Drying of the precipitate gave rise to brownish black powders, which were calcined at 400°C for 2 h under argon atmosphere to obtain the black powders of MoS2.


## 2.2. Characterization

The optical absorption spectrum of the reddish yellow colored solution of the intermediate as well as the ethanol dispersion of the calcined powders were studied at room temperature using Shimadzu UV-1601 UV-visible spectrophotometer. The phase and structure analyses of the virgin and the calcined powders were carried out on X’pert Pro 3040/60 high-resolution X-ray diffractometer using Cu Kα radiation (λ = 1.5418 Å´). X-ray photoelectron spectra (XPS), using VG Microtech ESCA2000 Multilab apparatus, was obtained for the virgin and the calcined powders for determining the oxidation states of Mo and S in the respective samples. Thermal analysis of the dried precipitate was performed at the heating rate of 6°C per min under dynamic argon using Perkin-Elmer Pyris Diamond TG/Differential thermal analyzer and alumina as the reference. Transmission electron microscope of model JEOL2010 (UHR) was used to study the microstructure of the calcined powders. The FTIR spectrum of the precursor sample was taken on a Perkin Elmer Fourier transform analyzer (FTIR spectrometer RXI). Electrical conductivity measurement was carried out on pressed pellet of the as-prepared calcined powders of MoS2 using a computer-controlled HIOKI LCR HITESTER at an AC signal of 1.0 V. The surfaces of the pellets were coated with silver paint for electrical contact. Finally, the electrical connection of the pellet to the apparatus was made through nickel electrode and put in a temperature controlled furnace. The hydrodynamic size of the synthesized MoS2 sample was measured by using 90 Plus Particle Size Analyzer (made by Brookhaven Instruments). The BET (Brunauer-Emmett-Teller) specific surface area of the calcined sample was measured through nitrogen adsorption isotherms at 77 K by using Quantachrome Instruments (Autosorb-1, Model no. ASI-C-9).


## 3. Results and Discussions

### 3.1. Analysis of the Precursor Precipitate

To understand the chemistry involved in the formation of precursor precipitate, the composition of the reddish yellow colored precursor solution obtained on heating the solution mixture over a water bath was characterized by UV-visible spectroscopy (Figure1). This optical absorption spectrum shows two absorption peaks centered at ~307 and 465 nm corresponding to the tetrathiomolybdate ions (MoS42-) [32, 33]. These ions possibly get formed as an intermediate on heating the solution of heptamolybdate (Mo7O246-) and thioacetamide through exchange of oxygen atoms in molybdate ions by sulfur. The possible reaction involved can be written as follows:
(1)Mo7O246-+28CH3CSNH2+4H2O⟶7MoS42-+8H++28CH3CONH2Figure 1
Optical absorption spectrum of the precursor solution containingMoS42- ions.Acidification of the solution containing tetrathiomolybdate ions with concentrated HCl led to brownish black colored precipitate of the sulfides. The composition of this as-precipitated precursor was investigated through analyzing the oxidation states of Mo and S in the samples by X-ray photoelectron spectroscopy. The survey spectra (not shown) showed the peaks for carbon, an impurity in the vacuum system, and oxygen in addition to the elements of interest (i.e., Mo and S). The deconvoluted and curve-fitted spectra shown in Figure2(a) corroborated to seven peaks centered at 225.2, 227.6, 230.2, 232.6, 233.5, 235.6, and 237.1 eV corresponding to Mo and S species present in the sample. The peak at 227.6 eV may be attributed to the 2s binding energy of S in elemental state [34]. The peak around 225.2 eV, which has a lower shift of 2.4 eV with respect to 2s binding energy of free S, originates from the sulfur bonded to Mo. The rest of the peaks can readily be fitted into three groups, 230.2 and 233.5 eV, 232.6 and 235.6 eV, 233.5 and 237.1 eV, representing the 3d doublets, 3d5/2 and 3d3/2, respectively, of various oxidation states of Mo.XPS spectra (a) for Mo, after and before curve peak fitting, and (b) for S in the as-precipitated precursor sample obtained after acidification of ATM solution.
(a)
(b)It is reported that, for any oxidation state of Mo, the 3d doublet (i.e.,3d5/2 and 3d3/2) has an energy separation of ~3.1 eV and a characteristic 3d5/2 : 3d3/2 peak intensity ratio of 3 : 2 [35]. Furthermore, the 3d5/2 and 3d3/2 binding energies of all the oxidation states of Mo show a higher shift in comparison to the respective binding energy values for elemental Mo, that is, 228 and 231.1 eV [36]. The peak pair (230.2 eV and 233.5 eV), which has a shift from 3d doublet of elemental Mo, higher than that of Mo (IV) in MoS2 (1.6 eV) and lower than that for Mo (VI) in MoS3 (4.2 eV), can be, respectively, assigned to 3d5/2 and 3d3/2 (i.e., the 3d doublet) binding energies of Mo (V) species in Mo2S5. The 3d doublet binding energies at 232.6 and 235.6 eV in Figure 2(a) may appear due to Mo (VI) species in MoS3. However, the higher energy shift of this peak pair from that of elemental Mo than the expected value of 4.2 eV and close proximity of the binding energies of the respective 3d doublets (i.e., 3d5/2 and 3d3/2) of MoS3 and MoO3 led us to believe that the XPS peak pair at 232.6 and 235.6 eV may be partially contributed by 3d doublet for the Mo (VI) species in MoO3. This trace amount of MoO3 may be formed during the handling of the sample in ambient atmosphere. The lone peak at 237.1 eV matches well with the respective 3d3/2 binding energy of Mo (VI) species in H2MoS4 [35], whereas its 3d5/2 counterpart of 3d doublet, with binding energy at 233.8 eV, may have merged with the broad peak at 233.5 eV. The insoluble compound, H2MoS4, which may be resulted from one of the acidification subreactions, eventually produces MoS3 with liberation of H2S on heating above 190°C.Figure2(b) shows the XPS spectra for S in the as-precipitated virgin precursors obtained after acidification of ATM solution. The figure indicates the presence of three major peaks with their maxima at 162.9, 166.8, and 168.9 eV. The broad peak at 162.9 eV has a lower binding energy value compared to that of the S 2p doublet (i.e., 164.1 eV and 165.2 eV for S 2p3/2 and S 2p1/2, resp.) in elemental sulfur [35]. However, this value is higher than the expected XPS peak positions for 2p doublet for S in MoS2 (i.e., 161.7 eV and 162.7 eV for S 2p3/2 and S 2p1/2, resp.). In consistency with the previous literature, the peak at 162.9 eV is thus assigned to the binding energy of S 2p in MoS3 [37]. On the other hand, the XPS peaks of S located at around 166.8 and 168.9 eV show higher binding energy values compared to that of S in zero oxidation state. These peaks possibly appeared due to the presence of bisulfite (with S in +4 oxidation state) and bisulfate (with S in +6 oxidation state) residue in the precipitate. The bisulfite and bisulfate ions are possibly produced from aqueous solution of sodium dithionite in presence of oxygen [38]. Nevertheless, it is difficult to ascertain the identity of Mo2S5 and H2MoS4 from the XPS analysis of sulfur because of nonavailability of relevant XPS data in the literature. However, on the basis of Mo 3d peak analysis, it can be predicted that the brownish black uncalcined samples, which get formed during the acidification of the intermediate ammonium tetrathiomolybdate (ATM) solution, could be a mixture of amorphous MoS3, Mo2S5, elemental S, and a small amount of H2MoS4. The plausible set of reactions (2)–(4) can be written as follows [39–41]:
(2)MoS42-+2H+⟶MoS3↓+H2S↑(3)2MoS42-+4H+⟶Mo2S5↓+2H2S↑+S↓(4)MoS42-+2H+⟶H2MoS4⟶MoS3↓+H2S↑The simultaneous thermogravimetric (TG), differential thermogravimetric (DTG), and differential thermal analysis (DTA) of the as-precipitated brownish black powders, shown in Figure3, supported the XPS results. The TG curve shows an initial weight loss of ~2.8% below 150°C, possibly corresponding to the removal of adsorbed water from the sample. The temperature region between 150 and 600°C in the TG curve can be divided into four distinct stages corresponding to various reactions involved in the decomposition process. The weight loss of ~22.7% associated with the endothermic effect in the stage-I region (150–240°C) could be taken as a collective effect due to loss of occluded vapors of H2S, HCl, and the by-product elemental sulfur formed due to reaction (3) along with the conversion of MoS3 to Mo2S5 [42] as per the following reaction:
(5)2MoS3→190-220°CMo2S5+S↑Figure 3
Thermograms for the decomposition of the as-precipitated precursor sample.The stage-II (240–390°C) involves the endothermic decomposition of Mo2S5 to amorphous MoS2 and an additional exothermic effect [41] for the transformation MoS2 (amorphous) → MoS2 (crystalline) in the sample. As a result, the overall thermal effect in DTA curve for stage-II is a small exothermic, which may be superimposed on a small endothermic peak. The weight loss (~9%) in the TG curve, in the corresponding region, matches well with the expected loss of sulfur during the conversion as follows:
(6)Mo2S5→△S↑+MoS2(amorphous)⟶MoS2(Crystalline)The stage-III (390–430°C) and IV (430–600°C), exothermic and endothermic effects, respectively, represent the oxidation of MoS2 to MoO2 and MoO2 to Mo2O3, respectively [42]. The formation of MoO2 may occur due to the oxygen impurities present in argon (carrier gas for the instrument) and subsequent conversion to Mo2O3 at higher temperature due to local deficiency of oxygen.Finally, the degree of crystallinity of the dried as-precipitated precursor powders was studied by X-ray diffraction (XRD), which shows a broad and diffused diffraction spectrum (Figure4) indicating the sample to be predominantly amorphous. The solitary peak centered at ~2θ = 13.4° may be due to some amount of crystalline materials present in the sample. Of the sulfide compounds of molybdenum, MoS3 are reported to be amorphous [12, 43]. However, Mo2S5, whose crystallinity nature is unknown given to the unavailability of any information in JCPDS database, may be responsible for the broad peak in Figure 4.Figure 4
XRD pattern of the as-precipitated precursor powders.


### 3.2. Analysis of the Calcined Sample

XRD pattern of the sample, obtained on calcinations of the as-precipitated powders at 400°C in argon atmosphere for 2 h, shows broad but distinct XRD peaks (Figure5). All the XRD peaks are indexed to the respective dhkl values of the hexagonal cell of bulk MoS2 with lattice parameters a=3.159 Å and c=12.162 Å (according to JCPDS Card no. 37-1492). The d002 line for the calcined powders is observed at 2θ=13.70°, which indicates a shift towards lower angle with respect to bulk 2H-MoS2. The observed shift may be attributed to lattice expansion of ~6.2% along c-axis due to induction of crystal defects or strains owing to the curvature of the layers [30]. This prediction is substantiated by larger ca. “c” value of the sample (a=3.105 Å and c=12.911 Å) compared to that reported for 2H-MoS2. The diffraction pattern is comparable with the scan reported by Wildervanck and Jellinek for MoS2 prepared through the decomposition of MoS3 [12]. The average crystallite size is found to be about 33 Å in c-direction (corresponding to approximately six MoS2 layers) and 78 Å in a-direction. The calculations of dimensions and number of layers have been carried out in the standard manner [44] by using full width at half maximum (FWHM) of the well-defined diffraction peaks. Furthermore, the broadening of the dhkl lines gives an indication of the formation of poorly crystalline MoS2 powders.Figure 5
XRD pattern of the MoS2 sample after calcination at 400°C for 2 h.Finally, the purity and composition of the calcined powders were analyzed by XPS. The peak pair (229.1 and 232.3 eV) in Figure6(a) represents the 3d doublet (i.e., 3d5/2 and 3d3/2, resp.) of the Mo (IV) species in MoS2, while the peak centered at 226.6 eV can be assigned to S 2s binding energy in MoS2. Figure 6(b) shows two peaks centered at 161.9 and 163.1 eV corresponding to the S 2p doublet, that is, 2p3/2 and 2p1/2, respectively in MoS2 [35]. The small peak of insignificant intensities beyond 163.1 eV may be attributed to some impurities associated with sulfur. Thus, the XPS studies indicate the formation of pure MoS2 through heat treatment of the precursor precipitate, obtained on acidification of ATM solution.XPS spectra, before and after curve peak fitting, (a) for Mo and (b) for S in MoS2 sample, obtained after calcination at 400°C for 2 h.
(a)
(b)The detailed microstructure of the calcined MoS2 sample is analyzed by transmission electron microscopy. Low-resolution transmission electron micrograph (TEM) of the sample (Figure 7(a)) indicated the formation of typical lamellar structures of MoS2 analogous to that observed by Chianelli et al. [45], who termed them as rag-like structures. Peng et al. also reported similar type of rag structures, which were synthesized under drastic conditions of hydrothermal reaction [24]. At higher magnification, these structures (Figure 7(b)) reveal the presence of different number of lattices ranging from 3 to 11. The low stacking and random orientation of the lattices, characteristics of rag-like structures, are also supported by the broad XRD peaks (Figure 5). At still higher resolution, the image (Figure 7(c)) indicates the existence of edge dislocations (in the encircled domains of the image) in the microstructure of the sample. This type of defects generally induced nonuniformity in d-spacing between the lattices [46], which is justified by the measured fringe widths, that is, 0.54, 0.61, and 0.7 nm, at different location of the image. This observation further demonstrates the formation of highly folded and disorder stacking character of rag-like structures [12]. However, the average width of the lattice fringes measured from the image is found to be ~0.62 nm, which is in close agreement with the characteristic d002 plane of the 2H-MoS2 crystal. The selected area electron diffraction (SAED) patterns of the sample (Figure 7(d)) show diffused diffraction rings, which are indexed by matching the d-values of the MoS2 crystal in the JCPDS card 37-1492 with those calculated from measurement of the ring radii. The observed diffraction rings can be attributed to coherent diffraction by aggregate of partially crystalline nanoparticles.Morphological analysis of the as-obtained MoS2 product obtained after calcination at 400°C for 2 h; (a) low-resolution image; (b), (c) high resolution images showing clear view of lattice fringes; (d) electron diffraction pattern of a selected area.
(a)
(b)
(c)
(d)Finally, the hydrodynamic size of synthesized MoS2 powders was measured, which is found to be around 299.3 nm. Since the measured size for the particles is higher than that observed from TEM image, it can be indicated that there is presence of aggregation in the sample [47].Based on the previous literature, it has been proposed that the formation of the poorly crystalline rag structures of MoS2 may be due to the presence of some amount of SDS residue in the precipitated precursor powders, which is evident from its FTIR spectra (Figure 8(a)). The appearance of typical infrared peaks at 2919 and 2850 cm−1 (asymmetric and symmetric –CH2 vibration), 1221 cm−1 (C–C skeletal vibration), 1074 and 633 cm−1 (SO42-), and 722 cm−1 (C–O stretching vibration) gives enough indication of the existence of SDS in the sample [48]. This is also confirmed by comparing the observed FTIR peaks with those obtained from pure SDS (Figure 8(b)). According to the previous reports, the precipitates, obtained through low-temperature reactions in the presence of long chain surfactants, such as cetyltrimethylammonium bromide (CTAB) or polyethylene glycol (PEG), were found to be contaminated with surfactants even after extensive washing [22, 30]. These adsorbed surfactants were believed to be decomposed under heat treatment, resulting in the abnormal expansion of interlayer gaps. Drawing similarity with the report, it can thus be predicted that the thermal decomposition of the carbonaceous compound (i.e., SDS) adsorbed on the precursor precipitate obtained through the present preparation procedure prevents the regular stacking of the layers of molybdenum sulfide and induces faulted stacking in the structures of the synthesized MoS2.Figure 8
FTIR spectra of (a) the as-precipitated virgin precursor powders and (b) pure SDS.Further verification of the role of SDS in the formation of poorly crystalline MoS2 powders with highly folded and disorder stacking layered structure has been performed by carrying out the XRD and microscopy analysis of the MoS2 sample obtained in the absence of SDS (Figure 9). The XRD pattern in Figure 9(a) displays X-ray diffraction pattern similar to that shown in Figure 5. However, the 2θ values for the (002) diffraction peak position for MoS2 samples prepared in absence of SDS (Figure 9(a)) and in presence of SDS (Figure 5) are found to be at 2θ≈ 14.0 and 13.4, respectively, compared to that for bulk 2H-MoS2 (2θ≈ 14.40°) (according to standard data in JCPDS Card no. 37-1492). This relatively higher downward shift of the (002) peak in case of sample prepared in presence of SDS indicates the larger lattice expansion along c-axis, which can be ascribed to the folding and randomness in the stacking of the MoS2 layers [30]. This finding is also supported by the TEM images of the samples. The TEM image of the MoS2 sample obtained in absence of SDS indicates the formation of agglomerations of some irregularly shaped coarse particles in contrast to that represented in Figure 7 (for MoS2 sample obtained in the presence of SDS).(a) XRD pattern and (b) TEM image of MoS2 sample obtained on calcination (at 400°C for 2 h) of the precipitate prepared in absence of SDS.
(a)
(b)


### 3.3. Study of the Properties of the Synthesized MoS2 Sample

In order to study the optical property of the calcined powders, UV-visible absorption was taken at room temperature after dispersion in ethanol. The spectra in Figure10 depict two weak bands centered at ~675 and 617 nm (marked by arrows), and a strong and very broad band with the maxima centered at ~400 nm. The first two peaks correspond to exciton A and B of MoS2, respectively. These exciton energy values are found to be red shifted in comparison to the respective exciton energy values assigned to the bulk 2H-MoS2 (654.3 and 593.3 nm) but are comparable to the respective values for nested IF-like structures (667 and 616.3 nm) at 175 K [49]. Furthermore, the observed UV-visible spectral pattern is found similar to that reported by Liao et al. [50] for MoS2 fibers synthesized through a low-temperature soft chemical route. It can thus be inferred that the curved nanostructures of the synthesized sample may be responsible for the observed optical spectrum of the synthesized MoS2 sample.Figure 10
Optical absorption spectrum of the as-obtained MoS2 sample.For studying the semiconducting behavior of the prepared MoS2 samples, two pellets were prepared by pressing MoS2 powders. One of the pellets was heated at 400°C for 4 h in argon atmosphere before carrying out the electrical measurement. The plots of log of conductivity (log σ) versus inverse of temperature (1/T) at different frequencies (such as 100, 200, 500, and 1000 kHz) are shown in Figures 11(a) and 11(b) for the MoS2 pellets, before and after heat treatment, respectively. Both of the samples exhibit typical semiconductor behaviors, that is, increase in the electrical conductivity with rise in temperature. In the low frequency range (below 1 kHz), the electrical conductivity for both heat-treated and virgin MoS2 pellets is found to be frequency independent and comparable to the DC conductivity values. The conductivity (in both, heat-treated and virgin pellets) is, however, observed to increase beyond the frequency range of 1 kHz. The frequency dependence of conductivity can be given by the following equation [51]:
(7)σ=σdc+σac=σdc+Aωn,
where A and n are materials parameters (0<n<1), σdc is “DC conductivity” or frequency independent part,  σac and ω are AC conductivity and angular frequency, respectively.Variation of conductivity with temperature at different frequencies for pressed pellets of MoS2; (a) before heat treatment and (b) after heat treatment.
(a)
(b)Further, from Figure11, the plots of log σ versus (1/T) are observed to undergo a change in slope beyond 373 K for both the samples. Relatively less significant rise in electrical conductivities of the samples at temperatures below 373 K is probably due to σac part being the major contributor to the total measured conductivity for the sample, owing to the fact that AC conductivity of semiconductors is only weakly dependent on temperature compared to σdc [52]. At intermediate and higher temperature range, the σdc part possibly contributes significantly, and thus the samples shows a noticeable rise in conductivity with temperature. Similar nonlinear dependence of log conductivity on (1/T) for MoS2 has been reported by Sienicki [53], who showed that log σ for MoS2 varied exponentially with reciprocal of temperature (1/T) at higher temperatures.In addition, the conductivity measured at room temperature (303 K) for the heat-treated pellet (1.13 × 10−2 S m−1) is found to be 16 times higher than that of the virgin pellet (6.88 × 10−4 S m−1). This significant improvement in σac may be due to the densification of the heat-treated pellet through grain growth at higher temperature. The activation energies (Ea) of the samples were also calculated from the slope of the logσ versus 1/T curve at a frequency of 1000 kHz using Arrhenius equation. Contrary to the trend of σ, the Ea values for heat-treated pellet (0.259 eV) and virgin pellet (0.258 eV) were found to be comparable.Finally, the BET surface area of the calcined sample has been determined by using BET surface area measurement instrument, which is found to be 35 m2/g. In spite of the low surface area value, based on some previous studies [10, 54, 55] and the morphological analysis, the synthesized MoS2 sample in the present technique, however, may be predicted to exhibit better catalytic activity. According to the studies by Tanaka and Okuhara [54], the difference in catalytic activity of layered transition metal chalcogenides such as MoS2 is not accounted for by BET surface area or pore structure but depends on the morphology, in particular on the ratio of basal and edge planes. This fact was also vindicated by the experimental observation by Iwata et al. [10] and Uzcanga et al. [55]. For example, Iwata et al. [10] claimed that the poorly crystalline MoS2 sample with highly bent multilayered structure provides larger number of catalytically active sites than the well-crystallized sample in spite of having surface area as low as 10 m2/g. This improvement in catalytic property was ascribed to the high content of edges and defects induced in the MoS2 layers of the synthesized sample. Uzcanga et al. [55] also anticipated enhanced catalytic performance for the sonochemically prepared MoS2 powders compared to that of the conventionally prepared sample, even though the former sample displayed lower surface area.


## 3.1. Analysis of the Precursor Precipitate

To understand the chemistry involved in the formation of precursor precipitate, the composition of the reddish yellow colored precursor solution obtained on heating the solution mixture over a water bath was characterized by UV-visible spectroscopy (Figure1). This optical absorption spectrum shows two absorption peaks centered at ~307 and 465 nm corresponding to the tetrathiomolybdate ions (MoS42-) [32, 33]. These ions possibly get formed as an intermediate on heating the solution of heptamolybdate (Mo7O246-) and thioacetamide through exchange of oxygen atoms in molybdate ions by sulfur. The possible reaction involved can be written as follows:
(1)Mo7O246-+28CH3CSNH2+4H2O⟶7MoS42-+8H++28CH3CONH2Figure 1
Optical absorption spectrum of the precursor solution containingMoS42- ions.Acidification of the solution containing tetrathiomolybdate ions with concentrated HCl led to brownish black colored precipitate of the sulfides. The composition of this as-precipitated precursor was investigated through analyzing the oxidation states of Mo and S in the samples by X-ray photoelectron spectroscopy. The survey spectra (not shown) showed the peaks for carbon, an impurity in the vacuum system, and oxygen in addition to the elements of interest (i.e., Mo and S). The deconvoluted and curve-fitted spectra shown in Figure2(a) corroborated to seven peaks centered at 225.2, 227.6, 230.2, 232.6, 233.5, 235.6, and 237.1 eV corresponding to Mo and S species present in the sample. The peak at 227.6 eV may be attributed to the 2s binding energy of S in elemental state [34]. The peak around 225.2 eV, which has a lower shift of 2.4 eV with respect to 2s binding energy of free S, originates from the sulfur bonded to Mo. The rest of the peaks can readily be fitted into three groups, 230.2 and 233.5 eV, 232.6 and 235.6 eV, 233.5 and 237.1 eV, representing the 3d doublets, 3d5/2 and 3d3/2, respectively, of various oxidation states of Mo.XPS spectra (a) for Mo, after and before curve peak fitting, and (b) for S in the as-precipitated precursor sample obtained after acidification of ATM solution.
(a)
(b)It is reported that, for any oxidation state of Mo, the 3d doublet (i.e.,3d5/2 and 3d3/2) has an energy separation of ~3.1 eV and a characteristic 3d5/2 : 3d3/2 peak intensity ratio of 3 : 2 [35]. Furthermore, the 3d5/2 and 3d3/2 binding energies of all the oxidation states of Mo show a higher shift in comparison to the respective binding energy values for elemental Mo, that is, 228 and 231.1 eV [36]. The peak pair (230.2 eV and 233.5 eV), which has a shift from 3d doublet of elemental Mo, higher than that of Mo (IV) in MoS2 (1.6 eV) and lower than that for Mo (VI) in MoS3 (4.2 eV), can be, respectively, assigned to 3d5/2 and 3d3/2 (i.e., the 3d doublet) binding energies of Mo (V) species in Mo2S5. The 3d doublet binding energies at 232.6 and 235.6 eV in Figure 2(a) may appear due to Mo (VI) species in MoS3. However, the higher energy shift of this peak pair from that of elemental Mo than the expected value of 4.2 eV and close proximity of the binding energies of the respective 3d doublets (i.e., 3d5/2 and 3d3/2) of MoS3 and MoO3 led us to believe that the XPS peak pair at 232.6 and 235.6 eV may be partially contributed by 3d doublet for the Mo (VI) species in MoO3. This trace amount of MoO3 may be formed during the handling of the sample in ambient atmosphere. The lone peak at 237.1 eV matches well with the respective 3d3/2 binding energy of Mo (VI) species in H2MoS4 [35], whereas its 3d5/2 counterpart of 3d doublet, with binding energy at 233.8 eV, may have merged with the broad peak at 233.5 eV. The insoluble compound, H2MoS4, which may be resulted from one of the acidification subreactions, eventually produces MoS3 with liberation of H2S on heating above 190°C.Figure2(b) shows the XPS spectra for S in the as-precipitated virgin precursors obtained after acidification of ATM solution. The figure indicates the presence of three major peaks with their maxima at 162.9, 166.8, and 168.9 eV. The broad peak at 162.9 eV has a lower binding energy value compared to that of the S 2p doublet (i.e., 164.1 eV and 165.2 eV for S 2p3/2 and S 2p1/2, resp.) in elemental sulfur [35]. However, this value is higher than the expected XPS peak positions for 2p doublet for S in MoS2 (i.e., 161.7 eV and 162.7 eV for S 2p3/2 and S 2p1/2, resp.). In consistency with the previous literature, the peak at 162.9 eV is thus assigned to the binding energy of S 2p in MoS3 [37]. On the other hand, the XPS peaks of S located at around 166.8 and 168.9 eV show higher binding energy values compared to that of S in zero oxidation state. These peaks possibly appeared due to the presence of bisulfite (with S in +4 oxidation state) and bisulfate (with S in +6 oxidation state) residue in the precipitate. The bisulfite and bisulfate ions are possibly produced from aqueous solution of sodium dithionite in presence of oxygen [38]. Nevertheless, it is difficult to ascertain the identity of Mo2S5 and H2MoS4 from the XPS analysis of sulfur because of nonavailability of relevant XPS data in the literature. However, on the basis of Mo 3d peak analysis, it can be predicted that the brownish black uncalcined samples, which get formed during the acidification of the intermediate ammonium tetrathiomolybdate (ATM) solution, could be a mixture of amorphous MoS3, Mo2S5, elemental S, and a small amount of H2MoS4. The plausible set of reactions (2)–(4) can be written as follows [39–41]:
(2)MoS42-+2H+⟶MoS3↓+H2S↑(3)2MoS42-+4H+⟶Mo2S5↓+2H2S↑+S↓(4)MoS42-+2H+⟶H2MoS4⟶MoS3↓+H2S↑The simultaneous thermogravimetric (TG), differential thermogravimetric (DTG), and differential thermal analysis (DTA) of the as-precipitated brownish black powders, shown in Figure3, supported the XPS results. The TG curve shows an initial weight loss of ~2.8% below 150°C, possibly corresponding to the removal of adsorbed water from the sample. The temperature region between 150 and 600°C in the TG curve can be divided into four distinct stages corresponding to various reactions involved in the decomposition process. The weight loss of ~22.7% associated with the endothermic effect in the stage-I region (150–240°C) could be taken as a collective effect due to loss of occluded vapors of H2S, HCl, and the by-product elemental sulfur formed due to reaction (3) along with the conversion of MoS3 to Mo2S5 [42] as per the following reaction:
(5)2MoS3→190-220°CMo2S5+S↑Figure 3
Thermograms for the decomposition of the as-precipitated precursor sample.The stage-II (240–390°C) involves the endothermic decomposition of Mo2S5 to amorphous MoS2 and an additional exothermic effect [41] for the transformation MoS2 (amorphous) → MoS2 (crystalline) in the sample. As a result, the overall thermal effect in DTA curve for stage-II is a small exothermic, which may be superimposed on a small endothermic peak. The weight loss (~9%) in the TG curve, in the corresponding region, matches well with the expected loss of sulfur during the conversion as follows:
(6)Mo2S5→△S↑+MoS2(amorphous)⟶MoS2(Crystalline)The stage-III (390–430°C) and IV (430–600°C), exothermic and endothermic effects, respectively, represent the oxidation of MoS2 to MoO2 and MoO2 to Mo2O3, respectively [42]. The formation of MoO2 may occur due to the oxygen impurities present in argon (carrier gas for the instrument) and subsequent conversion to Mo2O3 at higher temperature due to local deficiency of oxygen.Finally, the degree of crystallinity of the dried as-precipitated precursor powders was studied by X-ray diffraction (XRD), which shows a broad and diffused diffraction spectrum (Figure4) indicating the sample to be predominantly amorphous. The solitary peak centered at ~2θ = 13.4° may be due to some amount of crystalline materials present in the sample. Of the sulfide compounds of molybdenum, MoS3 are reported to be amorphous [12, 43]. However, Mo2S5, whose crystallinity nature is unknown given to the unavailability of any information in JCPDS database, may be responsible for the broad peak in Figure 4.Figure 4
XRD pattern of the as-precipitated precursor powders.


## 3.2. Analysis of the Calcined Sample

XRD pattern of the sample, obtained on calcinations of the as-precipitated powders at 400°C in argon atmosphere for 2 h, shows broad but distinct XRD peaks (Figure5). All the XRD peaks are indexed to the respective dhkl values of the hexagonal cell of bulk MoS2 with lattice parameters a=3.159 Å and c=12.162 Å (according to JCPDS Card no. 37-1492). The d002 line for the calcined powders is observed at 2θ=13.70°, which indicates a shift towards lower angle with respect to bulk 2H-MoS2. The observed shift may be attributed to lattice expansion of ~6.2% along c-axis due to induction of crystal defects or strains owing to the curvature of the layers [30]. This prediction is substantiated by larger ca. “c” value of the sample (a=3.105 Å and c=12.911 Å) compared to that reported for 2H-MoS2. The diffraction pattern is comparable with the scan reported by Wildervanck and Jellinek for MoS2 prepared through the decomposition of MoS3 [12]. The average crystallite size is found to be about 33 Å in c-direction (corresponding to approximately six MoS2 layers) and 78 Å in a-direction. The calculations of dimensions and number of layers have been carried out in the standard manner [44] by using full width at half maximum (FWHM) of the well-defined diffraction peaks. Furthermore, the broadening of the dhkl lines gives an indication of the formation of poorly crystalline MoS2 powders.Figure 5
XRD pattern of the MoS2 sample after calcination at 400°C for 2 h.Finally, the purity and composition of the calcined powders were analyzed by XPS. The peak pair (229.1 and 232.3 eV) in Figure6(a) represents the 3d doublet (i.e., 3d5/2 and 3d3/2, resp.) of the Mo (IV) species in MoS2, while the peak centered at 226.6 eV can be assigned to S 2s binding energy in MoS2. Figure 6(b) shows two peaks centered at 161.9 and 163.1 eV corresponding to the S 2p doublet, that is, 2p3/2 and 2p1/2, respectively in MoS2 [35]. The small peak of insignificant intensities beyond 163.1 eV may be attributed to some impurities associated with sulfur. Thus, the XPS studies indicate the formation of pure MoS2 through heat treatment of the precursor precipitate, obtained on acidification of ATM solution.XPS spectra, before and after curve peak fitting, (a) for Mo and (b) for S in MoS2 sample, obtained after calcination at 400°C for 2 h.
(a)
(b)The detailed microstructure of the calcined MoS2 sample is analyzed by transmission electron microscopy. Low-resolution transmission electron micrograph (TEM) of the sample (Figure 7(a)) indicated the formation of typical lamellar structures of MoS2 analogous to that observed by Chianelli et al. [45], who termed them as rag-like structures. Peng et al. also reported similar type of rag structures, which were synthesized under drastic conditions of hydrothermal reaction [24]. At higher magnification, these structures (Figure 7(b)) reveal the presence of different number of lattices ranging from 3 to 11. The low stacking and random orientation of the lattices, characteristics of rag-like structures, are also supported by the broad XRD peaks (Figure 5). At still higher resolution, the image (Figure 7(c)) indicates the existence of edge dislocations (in the encircled domains of the image) in the microstructure of the sample. This type of defects generally induced nonuniformity in d-spacing between the lattices [46], which is justified by the measured fringe widths, that is, 0.54, 0.61, and 0.7 nm, at different location of the image. This observation further demonstrates the formation of highly folded and disorder stacking character of rag-like structures [12]. However, the average width of the lattice fringes measured from the image is found to be ~0.62 nm, which is in close agreement with the characteristic d002 plane of the 2H-MoS2 crystal. The selected area electron diffraction (SAED) patterns of the sample (Figure 7(d)) show diffused diffraction rings, which are indexed by matching the d-values of the MoS2 crystal in the JCPDS card 37-1492 with those calculated from measurement of the ring radii. The observed diffraction rings can be attributed to coherent diffraction by aggregate of partially crystalline nanoparticles.Morphological analysis of the as-obtained MoS2 product obtained after calcination at 400°C for 2 h; (a) low-resolution image; (b), (c) high resolution images showing clear view of lattice fringes; (d) electron diffraction pattern of a selected area.
(a)
(b)
(c)
(d)Finally, the hydrodynamic size of synthesized MoS2 powders was measured, which is found to be around 299.3 nm. Since the measured size for the particles is higher than that observed from TEM image, it can be indicated that there is presence of aggregation in the sample [47].Based on the previous literature, it has been proposed that the formation of the poorly crystalline rag structures of MoS2 may be due to the presence of some amount of SDS residue in the precipitated precursor powders, which is evident from its FTIR spectra (Figure 8(a)). The appearance of typical infrared peaks at 2919 and 2850 cm−1 (asymmetric and symmetric –CH2 vibration), 1221 cm−1 (C–C skeletal vibration), 1074 and 633 cm−1 (SO42-), and 722 cm−1 (C–O stretching vibration) gives enough indication of the existence of SDS in the sample [48]. This is also confirmed by comparing the observed FTIR peaks with those obtained from pure SDS (Figure 8(b)). According to the previous reports, the precipitates, obtained through low-temperature reactions in the presence of long chain surfactants, such as cetyltrimethylammonium bromide (CTAB) or polyethylene glycol (PEG), were found to be contaminated with surfactants even after extensive washing [22, 30]. These adsorbed surfactants were believed to be decomposed under heat treatment, resulting in the abnormal expansion of interlayer gaps. Drawing similarity with the report, it can thus be predicted that the thermal decomposition of the carbonaceous compound (i.e., SDS) adsorbed on the precursor precipitate obtained through the present preparation procedure prevents the regular stacking of the layers of molybdenum sulfide and induces faulted stacking in the structures of the synthesized MoS2.Figure 8
FTIR spectra of (a) the as-precipitated virgin precursor powders and (b) pure SDS.Further verification of the role of SDS in the formation of poorly crystalline MoS2 powders with highly folded and disorder stacking layered structure has been performed by carrying out the XRD and microscopy analysis of the MoS2 sample obtained in the absence of SDS (Figure 9). The XRD pattern in Figure 9(a) displays X-ray diffraction pattern similar to that shown in Figure 5. However, the 2θ values for the (002) diffraction peak position for MoS2 samples prepared in absence of SDS (Figure 9(a)) and in presence of SDS (Figure 5) are found to be at 2θ≈ 14.0 and 13.4, respectively, compared to that for bulk 2H-MoS2 (2θ≈ 14.40°) (according to standard data in JCPDS Card no. 37-1492). This relatively higher downward shift of the (002) peak in case of sample prepared in presence of SDS indicates the larger lattice expansion along c-axis, which can be ascribed to the folding and randomness in the stacking of the MoS2 layers [30]. This finding is also supported by the TEM images of the samples. The TEM image of the MoS2 sample obtained in absence of SDS indicates the formation of agglomerations of some irregularly shaped coarse particles in contrast to that represented in Figure 7 (for MoS2 sample obtained in the presence of SDS).(a) XRD pattern and (b) TEM image of MoS2 sample obtained on calcination (at 400°C for 2 h) of the precipitate prepared in absence of SDS.
(a)
(b)


## 3.3. Study of the Properties of the Synthesized MoS2 Sample

In order to study the optical property of the calcined powders, UV-visible absorption was taken at room temperature after dispersion in ethanol. The spectra in Figure10 depict two weak bands centered at ~675 and 617 nm (marked by arrows), and a strong and very broad band with the maxima centered at ~400 nm. The first two peaks correspond to exciton A and B of MoS2, respectively. These exciton energy values are found to be red shifted in comparison to the respective exciton energy values assigned to the bulk 2H-MoS2 (654.3 and 593.3 nm) but are comparable to the respective values for nested IF-like structures (667 and 616.3 nm) at 175 K [49]. Furthermore, the observed UV-visible spectral pattern is found similar to that reported by Liao et al. [50] for MoS2 fibers synthesized through a low-temperature soft chemical route. It can thus be inferred that the curved nanostructures of the synthesized sample may be responsible for the observed optical spectrum of the synthesized MoS2 sample.Figure 10
Optical absorption spectrum of the as-obtained MoS2 sample.For studying the semiconducting behavior of the prepared MoS2 samples, two pellets were prepared by pressing MoS2 powders. One of the pellets was heated at 400°C for 4 h in argon atmosphere before carrying out the electrical measurement. The plots of log of conductivity (log σ) versus inverse of temperature (1/T) at different frequencies (such as 100, 200, 500, and 1000 kHz) are shown in Figures 11(a) and 11(b) for the MoS2 pellets, before and after heat treatment, respectively. Both of the samples exhibit typical semiconductor behaviors, that is, increase in the electrical conductivity with rise in temperature. In the low frequency range (below 1 kHz), the electrical conductivity for both heat-treated and virgin MoS2 pellets is found to be frequency independent and comparable to the DC conductivity values. The conductivity (in both, heat-treated and virgin pellets) is, however, observed to increase beyond the frequency range of 1 kHz. The frequency dependence of conductivity can be given by the following equation [51]:
(7)σ=σdc+σac=σdc+Aωn,
where A and n are materials parameters (0<n<1), σdc is “DC conductivity” or frequency independent part,  σac and ω are AC conductivity and angular frequency, respectively.Variation of conductivity with temperature at different frequencies for pressed pellets of MoS2; (a) before heat treatment and (b) after heat treatment.
(a)
(b)Further, from Figure11, the plots of log σ versus (1/T) are observed to undergo a change in slope beyond 373 K for both the samples. Relatively less significant rise in electrical conductivities of the samples at temperatures below 373 K is probably due to σac part being the major contributor to the total measured conductivity for the sample, owing to the fact that AC conductivity of semiconductors is only weakly dependent on temperature compared to σdc [52]. At intermediate and higher temperature range, the σdc part possibly contributes significantly, and thus the samples shows a noticeable rise in conductivity with temperature. Similar nonlinear dependence of log conductivity on (1/T) for MoS2 has been reported by Sienicki [53], who showed that log σ for MoS2 varied exponentially with reciprocal of temperature (1/T) at higher temperatures.In addition, the conductivity measured at room temperature (303 K) for the heat-treated pellet (1.13 × 10−2 S m−1) is found to be 16 times higher than that of the virgin pellet (6.88 × 10−4 S m−1). This significant improvement in σac may be due to the densification of the heat-treated pellet through grain growth at higher temperature. The activation energies (Ea) of the samples were also calculated from the slope of the logσ versus 1/T curve at a frequency of 1000 kHz using Arrhenius equation. Contrary to the trend of σ, the Ea values for heat-treated pellet (0.259 eV) and virgin pellet (0.258 eV) were found to be comparable.Finally, the BET surface area of the calcined sample has been determined by using BET surface area measurement instrument, which is found to be 35 m2/g. In spite of the low surface area value, based on some previous studies [10, 54, 55] and the morphological analysis, the synthesized MoS2 sample in the present technique, however, may be predicted to exhibit better catalytic activity. According to the studies by Tanaka and Okuhara [54], the difference in catalytic activity of layered transition metal chalcogenides such as MoS2 is not accounted for by BET surface area or pore structure but depends on the morphology, in particular on the ratio of basal and edge planes. This fact was also vindicated by the experimental observation by Iwata et al. [10] and Uzcanga et al. [55]. For example, Iwata et al. [10] claimed that the poorly crystalline MoS2 sample with highly bent multilayered structure provides larger number of catalytically active sites than the well-crystallized sample in spite of having surface area as low as 10 m2/g. This improvement in catalytic property was ascribed to the high content of edges and defects induced in the MoS2 layers of the synthesized sample. Uzcanga et al. [55] also anticipated enhanced catalytic performance for the sonochemically prepared MoS2 powders compared to that of the conventionally prepared sample, even though the former sample displayed lower surface area.


## 4. Conclusions

We have reported a simple aqueous solution-based precipitation route for the preparation of rag-like structures of MoS2 using some easily available laboratory reagents. As all of the reagents used are fairly soluble in water, there is less possibility of having impurities in the final products. The acidification of ATM solution with concentrated HCl resulted in the formation of a mixture of amorphous MoS3 and Mo2S5 with small amount of elemental sulfur and H2MoS4, as evident from XPS and thermal analysis. However, XRD patterns indicated the formation of pure but poorly crystalline MoS2 phase on calcining the as-precipitated samples at 400°C for 2 h in argon atmosphere. The calcined powders were found to be composed of significantly folded and randomly oriented S-Mo-S layers of MoS2 as visible from high-resolution TEM images. This observation was supported by the red shifting of the exciton peak positions in UV-visible spectrum of solid MoS2. The unique morphologies of the prepared MoS2 sample may be applied as a potential catalyst for hydrodesulfurization reactions. The electrical conductivity of MoS2 sample was found to increase on annealing.



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*Source: 671214-2013-04-18.xml*