# Luminescence and Morphological Kinetics of  Functionalized ZnS Colloidal Nanocrystals

Authors: Prabha Sana; Lubna Hashmi; M. M. Malik
Journal: ISRN Optics
 (2012)

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## Abstract

This paper reports functionalized zinc sulphide (ZnS) semiconductor nanocrystals (quantum dots, approx., 2.5 nm) which are an important building block in self-assembled nanostructures. ZnS is functionalized by organic stabilizer Thio glycolic acid (TGA). The samples have been synthesized by colloidal technique at relatively low temperature (below 100°C) at an atmospheric pressure of 10−3 torr. Manganese (Mn) doping ions have been incorporated (doped) in ZnS host lattice and observed its effect on growth morphology and optical properties of ZnS colloidal nanocrystals. By XRD, SEM, TEM, and PL, the obtained cubic phase nanosized TGA-capped ZnS materials were characterized. The morphology of ZnS obtained at different temperatures are analyzed by SEM. The crystallite size of the ZnS nanoparticles was estimated from the X-ray diffraction pattern by using Scherrer’s formula (approximately 2.5 nm) which is confirmed by TEM. The estimated bandgap value of ZnS NC’s by (αhύ)2 versus hύ
plot was 4.89 eV. Gaussian fitting curve in photoluminescence (PL) spectra indicated room temperature emission wavelength range from 300 to 500 nm in undoped and Mn-doped ZnS, with different emission peak intensities, and suggested the wide band emission colours in visible and near UV region which has wider applications in optical devices.


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## Body

## 1. Introduction

Zinc sulfide (ZnS), group II-VI compound semiconductor, is having great interest for its practical applications in optoelectronics and photonics [1–9]. Because of its wide bandgap (3.73 eV), it has a high index of reflection and a high transmittance in the visible range, particularly suitable for host material for a large variety of dopants. It has been extensively studied for a variety of applications like optical coatings, field effect transistors, optical sensors, electroluminescence, phosphors, and other light emitting materials [10–12]. Photoluminescence properties of ZnS have received special attention because of emission in different visible bands due to dopant ions in host matrices. The blue luminescence of ZnS host and orange luminescence due to the 4T1-6A1 transition of Mn2+ ions excited via energy transfer from the host ZnS have been reported by various researchers [13, 14]. At nanoregime, the potential advantages have been occurred in ZnS due to the spatial confinement of photoexcited electrons and holes that modify its optical and other related properties. Many research works have been carried out on these materials at nanoscale [15, 16]. A variety of methods have been reported for the preparation of nano-ZnS. These methods include soft solution synthesis, sol-gel synthesis, chemical vapor deposition, hydrothermal conditions, microwave irradiation, and so forth [17–27]. These novel routes for synthesis of optoelectronic materials are an integral aspect of material chemistry and physics. The colloidal synthesis route is another novel method of synthesis and is a developing area in the field of research. In this technique, concentration of reagent, capping agent to precursor ratio, pH, time, and temperature play important role to control the morphology and size of the ZnS nanoparticle. The stoichiometric molar ratio of sodium sulfide to zinc acetate is favorable to produce the cubic ZnS phase with fine nanoparticles. In the present context, the colloidal technique has been successfully employed for the preparation of TGA- (Thio-glycolic acid-) capped manganese-doped and undoped ZnS nanomaterials. This paper reports the ZnS QD’s of size approximately 2.5 nm with varying morphologies, depending on the concentration of dopant ion and temperature. The photoluminescence emission spectra of TGA-capped manganese- (Mn2+-) doped and undoped ZnS colloidal nanocrystals suggests the wide band emission colours in visible and near UV region.


## 2. Experimental Details

### 2.1. Synthesis of ZnS Nanoparticles

The chemicals, thio glycolic acid (TGA), zinc acetate, and sodium sulfide obtained from Aldrich and Merck chemicals. For preparation of TGA-capped ZnS, 100 mL solution of 10.3 mmole TGA in deionized water has been taken in a three-necked round bottom (RB) flask and stirred upto 1 hour. Afterwards, 100 mL of 10.26 mmole aqueous solution of zinc acetate Zn(CH3COO)2 was added in the TGA solution. The pH of resultant solution was maintained up to 11.5 in addition of 5 mL of 1 N NaOH aqueous solution and then the round bottom flask kept on stirring for 12 hours in vacuum atmosphere of relative pressure 10−3 torr at room temperature. After 12 hours, freshly prepared 100 mL of a 10.26 mmole aqueous solution of sodium sulfide Na2S was injected slowly in the round bottom flask. This leads to a milky white precipitate in the flask, further stirred 2 hours upto 80°C.


### 2.2. Synthesis of Manganese-Doped ZnS Nanoparticles

Same procedure was adopted to prepare Mn-doped TGA-capped ZnS, where 50 mL aqueous solution of 1.03 mmole Mn(CH3COO)2 was added in RB flask. Further, the same procedure was adopted as mentioned in Section 2.1. To observe the temperature and time effect on growth morphology of ZnS, aliquots at temperature 40°C and 80°C were taken. Subsequently, the prepared samples were centrifuged at 5000 rpm and washed several times with deionized water, later precipitates were collected for further characterization.


### 2.3. Morphological and Optical Characterization

The Mn incorporated ZnS was observed by transmission electron microscopy (TEM) (TECNAI-20 G2) at 200 kV and the morphology of the Mn-doped ZnS nanostructures was observed using scanning electron microscope (SEM) JEOL/EO Version-1 model JSM-6390 using stable suspension. The X-ray diffraction patterns of different samples were recorded using a Rigaku Mini Flex 2 Desktop using Kb filter CuKα  (λ=1.54148Å´)  radiation at 15 mA and 30 kV X-ray diffractometer. Room temperature UV-Visible absorption spectra were obtained by UV/Vis spectrophotometer model number 117 Systronics with wavelength range 200 nm to 800 nm, photoluminescence spectra were studies with LS-55, Perkin Elmer Photoluminescence Spectrophotometer.


## 2.1. Synthesis of ZnS Nanoparticles

The chemicals, thio glycolic acid (TGA), zinc acetate, and sodium sulfide obtained from Aldrich and Merck chemicals. For preparation of TGA-capped ZnS, 100 mL solution of 10.3 mmole TGA in deionized water has been taken in a three-necked round bottom (RB) flask and stirred upto 1 hour. Afterwards, 100 mL of 10.26 mmole aqueous solution of zinc acetate Zn(CH3COO)2 was added in the TGA solution. The pH of resultant solution was maintained up to 11.5 in addition of 5 mL of 1 N NaOH aqueous solution and then the round bottom flask kept on stirring for 12 hours in vacuum atmosphere of relative pressure 10−3 torr at room temperature. After 12 hours, freshly prepared 100 mL of a 10.26 mmole aqueous solution of sodium sulfide Na2S was injected slowly in the round bottom flask. This leads to a milky white precipitate in the flask, further stirred 2 hours upto 80°C.


## 2.2. Synthesis of Manganese-Doped ZnS Nanoparticles

Same procedure was adopted to prepare Mn-doped TGA-capped ZnS, where 50 mL aqueous solution of 1.03 mmole Mn(CH3COO)2 was added in RB flask. Further, the same procedure was adopted as mentioned in Section 2.1. To observe the temperature and time effect on growth morphology of ZnS, aliquots at temperature 40°C and 80°C were taken. Subsequently, the prepared samples were centrifuged at 5000 rpm and washed several times with deionized water, later precipitates were collected for further characterization.


## 2.3. Morphological and Optical Characterization

The Mn incorporated ZnS was observed by transmission electron microscopy (TEM) (TECNAI-20 G2) at 200 kV and the morphology of the Mn-doped ZnS nanostructures was observed using scanning electron microscope (SEM) JEOL/EO Version-1 model JSM-6390 using stable suspension. The X-ray diffraction patterns of different samples were recorded using a Rigaku Mini Flex 2 Desktop using Kb filter CuKα  (λ=1.54148Å´)  radiation at 15 mA and 30 kV X-ray diffractometer. Room temperature UV-Visible absorption spectra were obtained by UV/Vis spectrophotometer model number 117 Systronics with wavelength range 200 nm to 800 nm, photoluminescence spectra were studies with LS-55, Perkin Elmer Photoluminescence Spectrophotometer.


## 3. Results and Discussions

### 3.1. Growth Mechanism of ZnS

Zinc acetate dissociates into zinc ions (Zn2+) and acetate (Ac-) ions in aqueous solution. Similarly, manganese acetate and sodium sulfide dissociate into their respective cation and anions. Sodium being more reactive than zinc and manganese readily forms sodium acetate. ZnS nuclei form due to the reaction between Zn2+ and S2- ions, which subsequently grow by consuming more ions from the solution. To prevent further agglomeration to control the size, a repulsive force must be added between the particles to balance the attractive force. This is achieved by adsorbing organic molecules over nanoparticles inducing steric hindrance by employing TGA as the stabilizing agent. Thiol group of TGA gets attached to the surface of ZnS nanoparticles and prevents further agglomeration to control the size of nanoparticle, shown in Figure 1.Figure 1
Schematic representation of stabilization of ZnS nanoparticles by thio glycolic acid (TGA).


### 3.2. Structural Analysis

Structural analysis was made on the TGA-capped ZnS nanomaterial by colloidal synthesis process. The X-ray diffractogram in Figures2(a) and 2(b) indicated the polycrystalline nature of both undoped and Mn-doped ZnS materials. The prominent peaks corresponding to (111), (220), and (311) plane reflected to ZnS, which were observed at 2θ value 28.8, 48.0, and 56.9, respectively, agreed with JCPDS Card number 80-0020. It reveals face-centered cubic ZnS having zinc blend structure with preferential orientation in the (111) direction. The lattice parameter was estimated and the values of “a” was 5.40 [28]. The XRD peaks are broadened due to nanocrystalline nature of particles because nanocrystals have lesser lattice planes compared to bulk, which contributes to the broadening of the peaks in the diffraction pattern [29, 30]. From the width of the XRD peak broadening, the mean crystalline size was calculated using Scherrer’s equation: D=0.9λ/βcosθ, where λ is the X-ray wavelength (Cu Kα radiation 1.541 Å), θ is the diffraction angle, and β is the half-width of the diffraction peak. The mean crystal sizes of doped and undoped ZnS nanoparticles are calculated to be 2.5 nm. This is consistent with the estimated size of nanocrystals in TEM images. No apparent difference is observed in the XRD peak shape and broadening of ZnS nanoparticles before and after Mn2+ doping. The electron microscope studies have been made for TGA-capped Mn2+-doped ZnS nanoparticles, shown in Figure 3(a). The nano-ZnS fringes are observed clearly and comparable with the XRD data. The electron diffraction pattern of nano-ZnS shows diffraction rings assigned to (111), (220), and (311) planes. In the TEM images, Figure 3(b), the shape of these nanoparticles is spherical. The average size of the nanoparticle is in the range of 2-3 nm, which is also a supportive data for this research and comparable with XRD result.X-Ray diffraction patterns: (a) ZnS, (b) doped ZnS.
(a)(b)TEM images of doped ZnS nanoparticles: (a) bright field image with diffraction pattern (b) dark field image.
(a)(b)


### 3.3. Growth Mechanism of Undoped ZnS Nanocrystals

Growth process of nanostructures or microstructures is basically depending on nanoparticle aggregation. The aggregation of nanoparticles may provide zero, one, two, or three dimensional structures of various shapes. The kinetics of aggregation depends on the growth rate of nanoparticles in the solution and ions concentration. In our case, the aggregation of ZnS nanoparticles of initial size 2.5 nm (by TEM analysis) provides the spherical-shaped morphology of size 300 to 500 nm. Morphological analysis of aggregated nanoparticles of TGA-capped undoped ZnS (synthesized at 40°C) is presented in SEM micrograph Figure4(a). The as prepared undoped ZnS sample shows size distribution approximately 300 nm to 500 nm. With increased synthesis temperature 80°C, the sizes of ZnS nanostructure have been increased, it became approximately 400 to 800 nm shown in Figure 4(b). The size variations of spherical nanostructures with increased time and temperature is clearly observed. Schematic representation of the growth process of ZnS spherical nanostructure is shown in Figure 4. This growth process is based on Ostwald repining [31], which suggests that nanocrystal size increases with increasing reaction time and temperature because when the free atoms in solution are supersaturated, the free atoms have a tendency to condense on the surface of larger particles. Therefore, all smaller particles shrink, while larger particles grow, and overall the average size increase.SEM image TGA-capped ZnS; (a) at 40°C and (b) 80°C.
(a)(b)(c)


### 3.4. Growth Mechanism of Doped ZnS Nanocrystals

Morphological analysis by SEM of TGA-capped manganese-doped ZnS nanoparticles has been shown in Figure5 at two synthesized temperature 40°C and 80°C. SEM micrograph shows colloidal microsphere of size 1 to 3 μm, synthesized at 40°C temperature. These colloidal microspheres are self-assembly of nanoparticles. Schematic representation of self-assembly of Mn-doped ZnS nanoparticles into colloidal sphere with SEM micrograph is shown in Figure 5(a). As the synthesis temperature increased, the colloidal sphere started to disappear and growths of one dimensional nanorod have been observed on the surface of colloidal sphere. Schematic representations of growth of one-dimensional nanorods from colloidal sphere and SEM micrograph are shown in Figure 5(b). SEM image shows the approximately 4 μm length and 200 nm diameter of Mn-doped ZnS nanorods. The growth process of colloidal sphere to 1D structure was demonstrated by Botsan’s, Denk and Chua in 1972 [32]. They suggested the possibility of presence of impurity ions on the surface of colloidal sphere, which could enhance secondary nucleation by adsorbing at defect on existing crystal surface. By initiating crack propagation, crystal prone to disintegration and secondary nucleation may take place, the growth occurs from the impurity ion which is present on the surface. As the time and temperature increase the growth of secondary nucleation increases, the colloidal sphere simultaneously starts to disintegrate. The morphology transformation of colloidal sphere into one-dimensional nanorods of as prepared Mn2+-doped TGA-capped ZnS material sample has been observed. The impurity ion Mn2+ adsorbed at defect on existing ZnS crystal surface, responsible for the one-dimensional growth, and also diffused in the interstitial site of ZnS which modified the optical emission spectra of ZnS material. Therefore, the doping ion (manganese) has greatly affected the growth of nanostructures as well as their optical properties.SEM micrograph of doped ZnS; (a) at 40°C and (b) 80°C.
(a)(b)


### 3.5. The Quantum Size Effect and Bandgap Calculation

The UV-visible absorption spectra of Mn2+-doped ZnS nanoparticles in Figure 6(a), at 40°C and 80°C, exhibit absorption band edge at 235 and 253 nm, respectively, resulting from quantum confinement effect. It suggests large blue shift of the absorption from that of 320 nm (3.73 eV) for bulk ZnS crystals at room temperature [33, 34]. Thus, the bandgap of doped ZnS has been enlarged. Since the crystallite size of doped ZnS nanoparticles is approximately similar to Bohr radius of exciton in bulk ZnS crystal, a quantum confinement effect is expected to occur within these crystals, exhibiting an enlargement of the optical bandgap. The optical bandgap has been estimated by (αhύ)2 versus hύ plots, where the optical absorption coefficients (α) were calculated using the following equation:(1)T=(1-R)exp⁡⁡(-αt),
where T is transmittance, R is reflectance, and t is the thickness of the sample. The absorption coefficient (α) is related to the incident photon energy as follows:(2)αhυ=k(hυ-Eg)n/2,
where k is a constant, Eg is the optical bandgap of bulk ZnS, and n is a constant equal to 1 for direct bandgap semiconductors and 4 for indirect bandgap materials. Plots of hυ versus (αhυ)2 in Figure 6(b) are linear at the absorption edge, which means that the mode of transition in these nanomaterials has a direct nature. The bandgap energy Eg can be obtained from an extrapolation of the straight-line portion of the (αhυ)2 versus hυ plot to zero absorption coefficient value [35]. (αhυ)2 versus hυ plot provides the estimated bandgap 5.2 eV and 4.89 eV for Mn2+-doped ZnS nanoparticles at synthesized temperatures 40°C and 80°C, respectively. The bandgap energy clearly shifts to a lower wavelength (higher energy) with decreasing synthesis temperature at time. This can be attributed to a quantum confinement effect in nanosize particles. The approximate bandgap 4.9 eV has been estimated for particle size of 2.5 nm by Bruse equation [36], which is similar to the bandgap calculated by hν versus (αhν)2 plots, proved the direct optical bandgap of as-prepared nano-ZnS.(a) UV-visible absorption graph, (b)hυ versus (αhυ)2 plot.
(a)(b)


### 3.6. Emission Spectra Analysis

Room temperature photoluminescence (PL) emission spectra of undoped and Mn-doped ZnS were taken. Doped ZnS nanoparticles were prepared from a solution with Mn/Zn molar ratio 0.01 at 80°C. The excitation wavelength 250 nm (4.9 eV) for both doped and undoped sample was blue shifted, from excitation wavelength 332 nm (3.73 eV) corresponding to the bandgap energy of bulk ZnS host. This blue shift in ZnS nanocrystals is a reflection of the bandgap increase owing to the quantum confinement effect. Photoluminescence (PL) emission spectrum with Gaussian fitting for undoped ZnS has been shown in Figure7(a). Two characteristic bands of undoped ZnS with emission wavelengths at 353 and 464 nm were observed. PL emission wavelength at 353 nm (ultraviolet color) contributed to near-band-edge emission originates from the recombination of free excitons of ZnS nanocrystalline size regime. PL emission peak at 464 should be assigned to stoichiometric vacancies (defect states) or interstitial impurities, possibly at the surface in the ZnS nanoparticles [37–39]. Gaussian fitting curve with less intense blue emission at 419 nm is attributed to the sulphur vacancies. The comparative intensity of emission wavelength shows the less interstitial S2- ions, vacancies, and surface defects present in the ZnS nanocrystals. The photoluminescence emission band at approximately 590 nm (2.1 eV; yellowish orange) is the characteristic emission of Mn2+ ions in ZnS crystals, which can be attributed to 4T1 (excited) to 6A1 (ground) transition of the Mn2+ ions in Td symmetry. Emission occurs through energy transfer from the excited state of the ZnS host lattice to the d electrons of Mn2+ [40, 41]. This clearly suggests that the emission at 590 nm (2.1 eV) arises from Mn2+ ions, incorporated into the ZnS nanocrystals and not from Mn2+ ions of MnS nanocrystals. It is important to note that the Mn2+ ions in MnS nanocrystals have two emission peaks at 1.66 and 1.8 eV. Therefore, the presence of Mn2+ emission at 590 nm indicates that the Mn2+ ions occupy the Zn2+ ion site. More aspects of Mn2+ incorporation in ZnS host lattice have been made by Kennedy et al. [42] stated that there are two types of Mn in ZnS:Mn nanocrystallites. One is located inside the crystal or very close to another Mn. The other type of Mn is located at or near the surface. The latter shows the unusual fluorescence of interest. Sooklal et al. [43] reported that Mn2+ incorporated into the ZnS lattice led to Mn2+-based orange emission while ZnS with surface-bound Mn2+ yielded ultraviolet emission. In present investigation, emission at 590 nm due to Mn2+ in ZnS host lattice is not observed shown Figure 7(b), indicating that the Mn2+ ions were not occupied the Zn2+ ion site. The intensity of the UV emission at 353 nm which was observed in undoped ZnS in Figure 7(a) was reduced and this band edge emission shifts in the region 375–461 nm for Mn-incorporated ZnS [44, 45], as shown in Figure 7(b). Hu and Zhang [46] explained that this red-shift may come from the quantum confinement effect in nanoparticles, which leads to the change of the field surrounding the dopant ions [47]. Gaussian fitting for Mn-incorporated ZnS has been shown in Figure 7(b). Four characteristic bands of Mn:ZnS with emission wavelengths at 375 nm, 402 nm, 423 nm, and 461 nm were observed. Emission peaks at 402 nm and 423 nm attributed to sulfur vacancies, while surface-bound Mn2+ yielded ultraviolet emission peak at 375 nm, which clearly supports our argument for the morphology variation due to dopant ion. There is another important effect that needs to be observed, that the increased intensity of intense blue emission at 461 nm in case of doped ZnS nanoparticle may be confirming that the incorporation of the Mn ions into the ZnS lattice resulted in activation of surface defect sites and had an effect on the emission as well as growth of ZnS nanostructures.Photoluminescence (PL) spectrum of (a) undoped ZnS and (b) Mn doped ZnS nanoparticles.
(a)(b)


## 3.1. Growth Mechanism of ZnS

Zinc acetate dissociates into zinc ions (Zn2+) and acetate (Ac-) ions in aqueous solution. Similarly, manganese acetate and sodium sulfide dissociate into their respective cation and anions. Sodium being more reactive than zinc and manganese readily forms sodium acetate. ZnS nuclei form due to the reaction between Zn2+ and S2- ions, which subsequently grow by consuming more ions from the solution. To prevent further agglomeration to control the size, a repulsive force must be added between the particles to balance the attractive force. This is achieved by adsorbing organic molecules over nanoparticles inducing steric hindrance by employing TGA as the stabilizing agent. Thiol group of TGA gets attached to the surface of ZnS nanoparticles and prevents further agglomeration to control the size of nanoparticle, shown in Figure 1.Figure 1
Schematic representation of stabilization of ZnS nanoparticles by thio glycolic acid (TGA).


## 3.2. Structural Analysis

Structural analysis was made on the TGA-capped ZnS nanomaterial by colloidal synthesis process. The X-ray diffractogram in Figures2(a) and 2(b) indicated the polycrystalline nature of both undoped and Mn-doped ZnS materials. The prominent peaks corresponding to (111), (220), and (311) plane reflected to ZnS, which were observed at 2θ value 28.8, 48.0, and 56.9, respectively, agreed with JCPDS Card number 80-0020. It reveals face-centered cubic ZnS having zinc blend structure with preferential orientation in the (111) direction. The lattice parameter was estimated and the values of “a” was 5.40 [28]. The XRD peaks are broadened due to nanocrystalline nature of particles because nanocrystals have lesser lattice planes compared to bulk, which contributes to the broadening of the peaks in the diffraction pattern [29, 30]. From the width of the XRD peak broadening, the mean crystalline size was calculated using Scherrer’s equation: D=0.9λ/βcosθ, where λ is the X-ray wavelength (Cu Kα radiation 1.541 Å), θ is the diffraction angle, and β is the half-width of the diffraction peak. The mean crystal sizes of doped and undoped ZnS nanoparticles are calculated to be 2.5 nm. This is consistent with the estimated size of nanocrystals in TEM images. No apparent difference is observed in the XRD peak shape and broadening of ZnS nanoparticles before and after Mn2+ doping. The electron microscope studies have been made for TGA-capped Mn2+-doped ZnS nanoparticles, shown in Figure 3(a). The nano-ZnS fringes are observed clearly and comparable with the XRD data. The electron diffraction pattern of nano-ZnS shows diffraction rings assigned to (111), (220), and (311) planes. In the TEM images, Figure 3(b), the shape of these nanoparticles is spherical. The average size of the nanoparticle is in the range of 2-3 nm, which is also a supportive data for this research and comparable with XRD result.X-Ray diffraction patterns: (a) ZnS, (b) doped ZnS.
(a)(b)TEM images of doped ZnS nanoparticles: (a) bright field image with diffraction pattern (b) dark field image.
(a)(b)


## 3.3. Growth Mechanism of Undoped ZnS Nanocrystals

Growth process of nanostructures or microstructures is basically depending on nanoparticle aggregation. The aggregation of nanoparticles may provide zero, one, two, or three dimensional structures of various shapes. The kinetics of aggregation depends on the growth rate of nanoparticles in the solution and ions concentration. In our case, the aggregation of ZnS nanoparticles of initial size 2.5 nm (by TEM analysis) provides the spherical-shaped morphology of size 300 to 500 nm. Morphological analysis of aggregated nanoparticles of TGA-capped undoped ZnS (synthesized at 40°C) is presented in SEM micrograph Figure4(a). The as prepared undoped ZnS sample shows size distribution approximately 300 nm to 500 nm. With increased synthesis temperature 80°C, the sizes of ZnS nanostructure have been increased, it became approximately 400 to 800 nm shown in Figure 4(b). The size variations of spherical nanostructures with increased time and temperature is clearly observed. Schematic representation of the growth process of ZnS spherical nanostructure is shown in Figure 4. This growth process is based on Ostwald repining [31], which suggests that nanocrystal size increases with increasing reaction time and temperature because when the free atoms in solution are supersaturated, the free atoms have a tendency to condense on the surface of larger particles. Therefore, all smaller particles shrink, while larger particles grow, and overall the average size increase.SEM image TGA-capped ZnS; (a) at 40°C and (b) 80°C.
(a)(b)(c)


## 3.4. Growth Mechanism of Doped ZnS Nanocrystals

Morphological analysis by SEM of TGA-capped manganese-doped ZnS nanoparticles has been shown in Figure5 at two synthesized temperature 40°C and 80°C. SEM micrograph shows colloidal microsphere of size 1 to 3 μm, synthesized at 40°C temperature. These colloidal microspheres are self-assembly of nanoparticles. Schematic representation of self-assembly of Mn-doped ZnS nanoparticles into colloidal sphere with SEM micrograph is shown in Figure 5(a). As the synthesis temperature increased, the colloidal sphere started to disappear and growths of one dimensional nanorod have been observed on the surface of colloidal sphere. Schematic representations of growth of one-dimensional nanorods from colloidal sphere and SEM micrograph are shown in Figure 5(b). SEM image shows the approximately 4 μm length and 200 nm diameter of Mn-doped ZnS nanorods. The growth process of colloidal sphere to 1D structure was demonstrated by Botsan’s, Denk and Chua in 1972 [32]. They suggested the possibility of presence of impurity ions on the surface of colloidal sphere, which could enhance secondary nucleation by adsorbing at defect on existing crystal surface. By initiating crack propagation, crystal prone to disintegration and secondary nucleation may take place, the growth occurs from the impurity ion which is present on the surface. As the time and temperature increase the growth of secondary nucleation increases, the colloidal sphere simultaneously starts to disintegrate. The morphology transformation of colloidal sphere into one-dimensional nanorods of as prepared Mn2+-doped TGA-capped ZnS material sample has been observed. The impurity ion Mn2+ adsorbed at defect on existing ZnS crystal surface, responsible for the one-dimensional growth, and also diffused in the interstitial site of ZnS which modified the optical emission spectra of ZnS material. Therefore, the doping ion (manganese) has greatly affected the growth of nanostructures as well as their optical properties.SEM micrograph of doped ZnS; (a) at 40°C and (b) 80°C.
(a)(b)


## 3.5. The Quantum Size Effect and Bandgap Calculation

The UV-visible absorption spectra of Mn2+-doped ZnS nanoparticles in Figure 6(a), at 40°C and 80°C, exhibit absorption band edge at 235 and 253 nm, respectively, resulting from quantum confinement effect. It suggests large blue shift of the absorption from that of 320 nm (3.73 eV) for bulk ZnS crystals at room temperature [33, 34]. Thus, the bandgap of doped ZnS has been enlarged. Since the crystallite size of doped ZnS nanoparticles is approximately similar to Bohr radius of exciton in bulk ZnS crystal, a quantum confinement effect is expected to occur within these crystals, exhibiting an enlargement of the optical bandgap. The optical bandgap has been estimated by (αhύ)2 versus hύ plots, where the optical absorption coefficients (α) were calculated using the following equation:(1)T=(1-R)exp⁡⁡(-αt),
where T is transmittance, R is reflectance, and t is the thickness of the sample. The absorption coefficient (α) is related to the incident photon energy as follows:(2)αhυ=k(hυ-Eg)n/2,
where k is a constant, Eg is the optical bandgap of bulk ZnS, and n is a constant equal to 1 for direct bandgap semiconductors and 4 for indirect bandgap materials. Plots of hυ versus (αhυ)2 in Figure 6(b) are linear at the absorption edge, which means that the mode of transition in these nanomaterials has a direct nature. The bandgap energy Eg can be obtained from an extrapolation of the straight-line portion of the (αhυ)2 versus hυ plot to zero absorption coefficient value [35]. (αhυ)2 versus hυ plot provides the estimated bandgap 5.2 eV and 4.89 eV for Mn2+-doped ZnS nanoparticles at synthesized temperatures 40°C and 80°C, respectively. The bandgap energy clearly shifts to a lower wavelength (higher energy) with decreasing synthesis temperature at time. This can be attributed to a quantum confinement effect in nanosize particles. The approximate bandgap 4.9 eV has been estimated for particle size of 2.5 nm by Bruse equation [36], which is similar to the bandgap calculated by hν versus (αhν)2 plots, proved the direct optical bandgap of as-prepared nano-ZnS.(a) UV-visible absorption graph, (b)hυ versus (αhυ)2 plot.
(a)(b)


## 3.6. Emission Spectra Analysis

Room temperature photoluminescence (PL) emission spectra of undoped and Mn-doped ZnS were taken. Doped ZnS nanoparticles were prepared from a solution with Mn/Zn molar ratio 0.01 at 80°C. The excitation wavelength 250 nm (4.9 eV) for both doped and undoped sample was blue shifted, from excitation wavelength 332 nm (3.73 eV) corresponding to the bandgap energy of bulk ZnS host. This blue shift in ZnS nanocrystals is a reflection of the bandgap increase owing to the quantum confinement effect. Photoluminescence (PL) emission spectrum with Gaussian fitting for undoped ZnS has been shown in Figure7(a). Two characteristic bands of undoped ZnS with emission wavelengths at 353 and 464 nm were observed. PL emission wavelength at 353 nm (ultraviolet color) contributed to near-band-edge emission originates from the recombination of free excitons of ZnS nanocrystalline size regime. PL emission peak at 464 should be assigned to stoichiometric vacancies (defect states) or interstitial impurities, possibly at the surface in the ZnS nanoparticles [37–39]. Gaussian fitting curve with less intense blue emission at 419 nm is attributed to the sulphur vacancies. The comparative intensity of emission wavelength shows the less interstitial S2- ions, vacancies, and surface defects present in the ZnS nanocrystals. The photoluminescence emission band at approximately 590 nm (2.1 eV; yellowish orange) is the characteristic emission of Mn2+ ions in ZnS crystals, which can be attributed to 4T1 (excited) to 6A1 (ground) transition of the Mn2+ ions in Td symmetry. Emission occurs through energy transfer from the excited state of the ZnS host lattice to the d electrons of Mn2+ [40, 41]. This clearly suggests that the emission at 590 nm (2.1 eV) arises from Mn2+ ions, incorporated into the ZnS nanocrystals and not from Mn2+ ions of MnS nanocrystals. It is important to note that the Mn2+ ions in MnS nanocrystals have two emission peaks at 1.66 and 1.8 eV. Therefore, the presence of Mn2+ emission at 590 nm indicates that the Mn2+ ions occupy the Zn2+ ion site. More aspects of Mn2+ incorporation in ZnS host lattice have been made by Kennedy et al. [42] stated that there are two types of Mn in ZnS:Mn nanocrystallites. One is located inside the crystal or very close to another Mn. The other type of Mn is located at or near the surface. The latter shows the unusual fluorescence of interest. Sooklal et al. [43] reported that Mn2+ incorporated into the ZnS lattice led to Mn2+-based orange emission while ZnS with surface-bound Mn2+ yielded ultraviolet emission. In present investigation, emission at 590 nm due to Mn2+ in ZnS host lattice is not observed shown Figure 7(b), indicating that the Mn2+ ions were not occupied the Zn2+ ion site. The intensity of the UV emission at 353 nm which was observed in undoped ZnS in Figure 7(a) was reduced and this band edge emission shifts in the region 375–461 nm for Mn-incorporated ZnS [44, 45], as shown in Figure 7(b). Hu and Zhang [46] explained that this red-shift may come from the quantum confinement effect in nanoparticles, which leads to the change of the field surrounding the dopant ions [47]. Gaussian fitting for Mn-incorporated ZnS has been shown in Figure 7(b). Four characteristic bands of Mn:ZnS with emission wavelengths at 375 nm, 402 nm, 423 nm, and 461 nm were observed. Emission peaks at 402 nm and 423 nm attributed to sulfur vacancies, while surface-bound Mn2+ yielded ultraviolet emission peak at 375 nm, which clearly supports our argument for the morphology variation due to dopant ion. There is another important effect that needs to be observed, that the increased intensity of intense blue emission at 461 nm in case of doped ZnS nanoparticle may be confirming that the incorporation of the Mn ions into the ZnS lattice resulted in activation of surface defect sites and had an effect on the emission as well as growth of ZnS nanostructures.Photoluminescence (PL) spectrum of (a) undoped ZnS and (b) Mn doped ZnS nanoparticles.
(a)(b)


## 4. Conclusions

ZnS and ZnS:Mn nanoparticles were prepared using a colloidal synthesis method with thioglycolic acid (TGA) as a surface stabilizing agent to prevent surface dangling bonds and agglomeration of in ZnS nanocrystals. The ZnS nanocrystal size was controlled by the synthesis temperature. Temperature ranges from 40°C to 80°C have been used in synthesis process to observe the effect on optical bandgap and morphology of ZnS nanocrystals. The prepared samples were highly transparent (>80%) in the visible region. The absorption edge of doped ZnS samples was demonstrated narrow grain size distribution. The effect of dopant ions Mn2+ is observed on growth morphology and optical behavior ZnS nanostructures. It was found that the surface bound Mn2+ ion in ZnS nanocrystals provides ultraviolet emission. XRD reveals the formation of face-centred cubic ZnS quantum dots with grains size approximately 2.5 nm for both undoped and Mn-doped ZnS, this result was confirmed by TEM. These materials show strong emission, are highly transparent in the visible range, and may be useful in fabrication of flat panel display devices.



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*Source: 621908-2012-02-02.xml*