Download PDF

Applied Nanoscience

, Volume 4, Issue 4, pp 449–454 | Cite as

Photoluminescence enhancement of hexagonal-phase ZnS:Mn nanostructures using 1-thioglycolic acid

Open Access
Original Article
First Online:
Received:
Accepted:

Abstract

Hexagonal wurtzite ZnS:Mn2+ nanostructures were synthesized at lower temperature (80 °C) by chemical method in an air atmosphere using 1-thioglycolic acid (TGA) as a stabilizing agent. It is a simple, highly efficient and energy-saving method for large-scale synthesis of hexagonal ZnS:Mn2+ nanoparticles at lower temperature. Structural and optical properties of the samples were investigated. An optimum concentration of TGA was selected through optical PL study.

Keywords

Nanoball Nanorod Surface defect TGA Luminescence 

Introduction

Zinc sulfide is one of the II–VI group compound mostly found in two structural polymorphs—cubic sphalerite or hexagonal wurtzite. It is a wide band gap material with unique properties in applications such as photocatalysts, solar cells, display panels, optical sensors and single electron transistors (Karar et al. 2004; Mu et al. 2005). It is the best host material for a large variety of dopants (Sooklal et al. 1996). Bhargava et al. (1994a, b) reported the first observation of optical properties of Mn2+ doped ZnS nanocrystals. It is well known that the cubic phase (zinc blende) of ZnS is stable at room temperature, while the hexagonal phase (wurtzite) is a high-temperature form. The equilibrium phase transformation between cubic and hexagonal phases occurs at about 1,296 K (Yu and Yoshimura 2002). Since the inherent crystal structures of ZnS have an important effect on its physical and chemical properties (Moore et al. 2004; Jiang et al. 2003), the preparation of ZnS with controllable phase is vital to its practical applications. Current research work is focused on nanosize particles and devices, because the particles display unique properties in the orange region and therefore have a lot of potential properties.

Mn2+ usually occupies substitutional sites in the Zn lattice as a divalent ion, and the excitation and decay of this ion produce an orange luminescence at approximately 590 nm (Bhargava et al. 1994a; Sapra et al. 2003). This emission peak is generally associated with a transition between 4T1 and 6A1 energy levels. In addition, electron paramagnetic resonance (EPR) technique has been widely used to obtain an insight into the local crystal field effects and symmetry around Mn2+ ions (Borse et al. 1999). The observed Mn2+ spectral features were used to explain the changes in the optical properties of the material. Manganese-doped ZnS nanoparticles have been synthesized using different methods such as laser ablation, certain physical methods, solution growth, and other different chemical techniques (Soo et al. 1994). In this study, hexagonal ZnS:Mn2+ nanostructures were synthesized by chemical method using thioglycolic acid and its structural and photoluminescence properties were studied. It is a simple energy-saving method to synthesize hexagonal ZnS:Mn2+ at lower temperatures.

Experimental

Materials

To synthesize Mn-doped ZnS nanoparticles, the following materials were used. Zinc acetate (Zn (CH3COO)2·2H2O), manganese chloride (MnCl2·4H2O) and sodium sulfide (Na2S·xH2O) obtained from Nice Chemical company were used as precursors. Thioglycolic acid (TGA) was obtained from Aldrich Company. The chemical reagents used were analytical reagent grade without further purification. All the glasswares used in this experimental work were acid washed. Ultrapure water was used for all dilutions and sample preparation.

Synthesis of Mn-doped ZnS nanoparticles

In a typical synthesis, 0.5 M of Zn (CH3COO)2·2H2O in 50 ml de-ionized water and different amounts of (5–25 ml) thioglycolic acid (TGA) in 50 ml de-ionized water were dissolved. Then, 4 % of manganese chloride in 25 ml was added. The optimum concentration of Mn was selected from the previous work (Murugadoss et al. 2010a). Subsequently, the Na2S (50 ml) was added drop wise to the above mixture. For each experiment, the molar amounts of Zn(CH3COO)2 and Na2S used were equal. The pH value of the colloidal solution was reduced from 6 to 2 with respect to concentration of the TGA from 5, 20, 15, 20 and 25 ml, respectively. During the whole reaction process, the reactants were vigorously stirred under air atmosphere at 80 °C. After 30 min, the colloidal solution was kept for 1 week at room temperature. Then, the formed nanoparticles were separated from the colloidal solution by centrifuging. The collected precipitate was washed several times by de-ionized water and ethanol and then dried at 120 °C in an air atmosphere.

Characterization

The X-ray diffraction patterns of the products were recorded using X-ray diffractometer (XRD, X’pert PRO) with Cu Kα radiation (λ = 1.54060 Å) at room temperature. The crystallite size was estimated using the Scherrer’s equation D = (0.9 λ)/(βcosθ) from the full width at half maximum of the major XRD peak. The morphology and interior structure of the products were analyzed using TEM (Technai 20G2, FEI). The optical absorption spectra of the particles in de-ionized water were recorded using UV-1650PC SHIMADZU spectrophotometer. The photoluminescence measurements were performed on a RF-5301PC spectrophotometer. Electron spin resonance (ESR) spectrum of the powder of the ZnS:Mn2+ was measured on an ESR spectrometer (Bruker EMX Plus) at room temperature.

Results and discussion

Structural and morphological study

The crystal structures of the samples were investigated through the XRD study. Figure 1 shows the XRD pattern of the ZnS:Mn2+ with capped TGA. The XRD pattern reveals the formation of perfectly indexed highly crystalline hexagonal wurtzite phase (JCPDS, card no. 80-0007) of ZnS:Mn2+ nanoparticles. Previous research work (Murugadoss 2011), no observed hexagonal phase for Mn doped (up to 20 %) and surfactants capped ZnS:Mn (Biswas et al. 2005). However, a phase transition (cubic to hexagonal wurtzite) is detected only for the annealing sample (ZnS:Mn) at higher temperatures (Biswas et al. 2005). The broadening of the diffraction peaks indicates the nanocrystalline nature of the sample. Actually, in the presence of the organic compound (TGA), it contains both a thiol (mercaptan) and a carboxylic acid, the free energy difference between the hexagonal and cubic phase might have increased toward their normal value, and as a result, the cubic phase gets favored over the hexagonal phase. This is the reverse of the reaction reported in the literature regarding the transformation of cubic ZnS to hexagonal wurtzite phase in the presence of some organic molecules (Murakoshi et al. 1998). However, an exact mechanism behind the formation of hexagonal nanorods by stabilizer is not clear and needs further study. Along with the main diffraction peaks some low-intensity impurity peaks are detected in Fig. 1. It may be due to the formation of MnS in the colloidal form.
Open image in new window
Fig. 1

X-ray diffraction analysis of TGA (15 ml) capped ZnS:Mn2+ nanoparticles

The morphology of the samples was investigated through the transmission electron microscopic images (Fig. 2a–f). This reveals the formation of nanoballs and nanorods along with very tiny particles. The formation of complex structure (nanoballs and rods) may be due to the presence of TGA. At the suitable temperature (80 °C) the thiol and carboxylic molecules come out of the layered complex structure, resulting in the aggregation or assemblage by the seeds (very small size nanoparticles) as shown in Fig. 2. Figure 2a, b shows the formation of the nanoballs (~100 nm) by the assemblage of very small size nanoparticles (<5 nm). The sizes of the nanoballs varied within 100–150 nm range. Figure 2c shows a complete formation of the isolated nanoball. Well-shaped hexagonal structured ZnS:Mn (Fig. 2d, e) nanorods were also obtained along with nanoballs and very small size particles. It may be because of the stabilization of the synthesized particles in the colloidal form for long time (for 15 days) with the presence of the TGA. Additionally, it should be pointed out that the tiny size of as-synthesized ZnS particles made it easy for cubic ZnS to transform into hexagonal ZnS at low temperatures (Qadri et al. 1999). Consequently, the capping agent TGA can be used as a simple, highly efficient, and energy saving method for large-scale synthesis of hexagonal ZnS:Mn nanoparticles.The diameters and lengths of the nanorods varied within 50–100 nm and 1–1.5 μm, respectively. In addition, very small size (>20 nm dia.) nanorods are detected (Fig. 2e). Corresponding SAED pattern of the sample is shown in Fig. 2f. It shows six rings corresponding to (1 0 2), (1 1 0), (1 0 3), (2 0 0), (1 1 2) and (2 0 1) phases of the hexagonal structure.
Open image in new window
Fig. 2

a–e TEM micrographs of TGA capped ZnS:Mn2+ nanoparticles with different magnification and SAED pattern (f)

Optical study

UV–Visible spectrophotometry is one of the basic techniques to study the quantum confinement effects. Figure 3 shows the UV–Visible absorption spectra of the ZnS:Mn2+ (4 %) nanoparticles stabilized by thioglycolic acid (5–25 ml). The characteristic absorption peaks of the samples were appeared in the range 250–350 nm. The peak position reflects the band gap of the nanoparticles. The obtained peaks are centered at 292 nm. As seen in Fig. 3, the peak position has no change with respect to the TGA concentrations. However, a strong absorption is observed for 5 ml of TGA. The absorption peaks are significantly blue-shifted from the bulk ZnS (345 nm). It dictates the reduction of the particles size in the nanoscale. This shifting is due to quantum confinement effect (Deshpande et al. 2009). It is well known that the fundamental absorption can be used to determine the nature and value of the optical band gap of the nanoparticles. The band gap of all the samples is calculated using a simple wave–energy equation:
$$ E_{\text{gn}} = h\nu = hc/\lambda $$
(1)
where h is the Planck’s constant, c is the light velocity and λ is the absorption wavelength. From the band gap value, the size (R) of nanoparticles can be calculated by the Brus model (Brus 1991)
$$ E_{g} \left( {\text{nano}} \right)-E_{g} \left( {\text{bulk}} \right) = h^{2} /8R^{2} \left( {1/m_{\hbox{e}} + 1/m_{\hbox{h}}} \right)-1.8e^{2} /\left( {4\pi \varepsilon_{\alpha } \varepsilon_{0} R} \right) $$
(2)
where Ebulk and Enano are the band gap energies of bulk and nanosized semiconductors, respectively, h is the Planck’s constant, me and mh are the effective masses of electron and hole, respectively, ε α is the dielectric constants of the material (ε α  = 8.3) and ε0 is the permittivity of vacuum. Here, me = 0.19m0 and mh = 0.8m0, where m0 is the free electron mass and e is the charge of electron (in coulomb). The calculated particles size is 3.7 nm.
Open image in new window
Fig. 3

UV–Visible absorption spectra of TGA capped (5–25 ml) ZnS:Mn2+ nanoparticles

Figure 4a depicts the PL spectra of the ZnS:Mn2+ nanoparticles stabilized by different amounts (5–25 ml) of TGA. The PL spectra show two emission bands, one is the strong orange emission band located at about 580 nm from intraconfigurational d–d transitions 4T1−6A1 in Td symmetry which are in principle spin forbidden by the S = 0 and parity selection rules; the other is a weak and broad blue band centered at about 445 nm, which is considered to be associated with defects (Murugadoss et al. 2010b). The narrow orange emission indicates the particles are highly homogeneous. Figure 4b shows a plot between the concentrations of TGA versus PL intensity. As seen in Fig. 4b, a maximum PL intensity is observed for lower concentration of stabilizer (TGA, at 5 ml), and after that, it is decreased.
Open image in new window
Fig. 4

a PL spectra of TGA capped (5–25 ml) ZnS:Mn2+ nanoparticles and b corresponding concentration versus PL intensity

At higher concentrations of TGA (>5 ml), the pH of the colloidal solution is suddenly reduced (<4). Hence, the PL intensity of ZnS:Mn is significantly decreased. It dictates that the increase of the surface defect or decomposition of the sample is due to increase of the carboxylic acid by increasing TGA concentration. The ZnS:Mn/TGA (~5 ml) gave an enhanced PL efficiency [the ratio of intensity of the orange emission (I1) to blue emission (I0)] as shown in Fig. 4b. The increasing efficiency indicates the improvement of homogeneous ZnS:Mn2+ growth and declining surface defect. The role of the stabilizer is not only to tailor crystalline structure but also to control the size in the nanoscale. In addition, the PL enhancement indicates elimination of the surface defect completely by TGA.

ESR study

The presence of Mn2+ ions in ZnS lattice nanostructure can be confirmed by ESR spectrum. The ESR spectrum (Fig. 5) of ZnS:Mn2+ nanostructure shows six lines which is attributed to (∆M I  = 0 and ∆M S  = ±1) allowed transitions of the Mn2+ ions (I = 5/2). For lower Mn concentrations, these lines are accompanied by smaller ones between them which are assigned to (∆M I  = 0 and ∆M S  = ±1) forbidden transitions. The appearance of the well-resolved hyperfine structure together with the less intense lines between them (at approximately g = 2) proves that many Mn ions are at nearly cubic symmetry (Sooklal et al. 1996; Hoffman et al. 1998). As the Mn2+ ion is affected by other Mn2+ ions that are randomly distributed around it, the Mn–Mn interactions should result in a reduction of the electron spin–nuclear spin interactions in an individual Mn ion (Ji et al. 2003).
Open image in new window
Fig. 5

ESR spectrum of ZnS:Mn2+ (5 ml) nanoparticles

Conclusions

In summary, the hexagonal wurtzite ZnS:Mn2+ nanostructures (nanoballs and nanorods) were successfully synthesized by simple chemical method and studied using XRD, TEM, UV–Vis and PL. It is a simple, highly efficient and energy-saving method for large-scale synthesis of hexagonal ZnS:Mn2+ nanoparticles at lower temperature. The experimental results demonstrated that as-prepared ZnS:Mn2+/TGA nanostructures have an excellent optical property. An optimum concentration of the TGA was selected as 5 ml (since it shows enhanced PL intensity) and it tailored the structure of the ZnS:Mn2+. The presence of Mn2+ ions was confirmed by ESR study. The intense emission was observed for Mn-doped ZnS nanoparticles using TGA, which will be useful for fabrication of optoelectronic devices.

References

  1. Bhargava RN, Gallagher D, Hong X, Nurmikko A (1994a) Optical properties of manganese-doped nanocrystals of ZnS. Phys Rev Lett 72:416–419CrossRefGoogle Scholar
  2. Bhargava RN, Gallagher D, Welker T (1994b) Doped nanocrystals of semiconductors—a new class of luminescent materials. J Lumin 60–61:275–280CrossRefGoogle Scholar
  3. Biswas S, Kar S, Chaudhuri S (2005) Optical and magnetic properties of manganese-incorporated zinc sulfide nanorods synthesized by a solvothermal process. J Phys Chem B 109:17526–17530CrossRefGoogle Scholar
  4. Borse PH, Srinivas D, Shinde RF, Date SK, Vogel W, Kulkarni SK (1999) Effect of Mn2+ concentration in ZnS nanoparticles on photoluminescence and electron-spin-resonance spectra. Phys Rev B 60:8659–8664CrossRefGoogle Scholar
  5. Brus LE (1991) Quantum crystallites and nonlinear optics. Appl Phys A 53:465–474CrossRefGoogle Scholar
  6. Deshpande A, Shah P, Gholap RS, Gupta NM (2009) Interfacial and physico-chemical properties of polymer-supported CdS–ZnS nanocomposites and their role in the visible-light mediated photocatalytic splitting of water. J Colloid Interface Sci 333:263–268CrossRefGoogle Scholar
  7. Hoffman DM, Hofstaetter A, Lei U, Meyer BK, Gounio G (1998) EPR and ENDOR investigations on CdS:Mn nanocrystals. J Cryst Growth 184(185):383–387CrossRefGoogle Scholar
  8. Ji TH, Jain WB, Fang JY (2003) The first synthesis of Pb1−xMnxSe nanocrystals. J Am Chem Soc 125:8448–8449CrossRefGoogle Scholar
  9. Jiang Y, Meng XM, Liu J, Hong ZR, Lee CS, Lee ST (2003) ZnS nanowires with wurtzite polytype modulated structure. Adv Mater 15:1195–1198CrossRefGoogle Scholar
  10. Karar N, Raj S, Singh F (2004) Properties of nanocrystalline ZnS:Mn. J Cryst Growth 268:585–589CrossRefGoogle Scholar
  11. Moore D, Ronning C, Ma C, Wang ZL (2004) Wurtzite ZnS nanosaws produced by polar surfaces. Chem Phys Lett 385:8–11CrossRefGoogle Scholar
  12. Mu J, Gu D, Xu Z (2005) Effect of annealing on the structural and optical properties of non-coated and silica-coated ZnS:Mn nanoparticles. Mater Res Bull 40:2198–2204CrossRefGoogle Scholar
  13. Murakoshi K, Hosokawa H, Tanaka N, Saito M, Wada Y, Sakata T, Mori H, Yanagida S (1998) Phase transition of ZnS nanocrystallites induced by surface modification at ambient temperature and pressure confirmed by electron diffraction. Chem Commun 1998:321–322CrossRefGoogle Scholar
  14. Murugadoss G (2011) Synthesis, optical, structural and thermal characterization of Mn2+ doped ZnS nanoparticles using reverse micelle method. J Lumin 131:2216–2223CrossRefGoogle Scholar
  15. Murugadoss G, Rajamannan B, Ramasamy V (2010a) Synthesis, characterization and optical properties of water-soluble ZnS:Mn2+ nanoparticles. J Lumin 130:2032–2039CrossRefGoogle Scholar
  16. Murugadoss G, Rajamannan B, Ramasamy V (2010b) Synthesis and photoluminescence study of PVA-capped ZnS:Mn2+ nanoparticles. Dig J Nanomater Biostruct 5:339–345Google Scholar
  17. Qadri SB, Skelton EF, Hsu D, Dinsmore AD, Yang J, Gray HF, Ratna BR (1999) Size-induced transition-temperature reduction in nanoparticles of ZnS. Phys Rev B 60:9191–9193CrossRefGoogle Scholar
  18. Sapra S, Nanda J, Anand A, Bhat SV, Sarma DD (2003) Optical and magnetic properties of manganese-doped zinc sulfide nanoclusters. J Nanosci Nanotechnol 3:392–400CrossRefGoogle Scholar
  19. Soo YL, Ming ZH, Huang SW, Kao YH, Bhargava RN, Gallagher D (1994) Local structures around Mn luminescent centers in Mn-doped nanocrystals of ZnS. Phys Rev B 50:7602–7607CrossRefGoogle Scholar
  20. Sooklal K, Cullum BS, Angel SM, Murphy CJ (1996) Photophysical properties of ZnS nanoclusters with spatially localized Mn2+. J Phys Chem 100:4551–4555CrossRefGoogle Scholar
  21. Yu SH, Yoshimura M (2002) Shape and phase control of ZnS nanocrystals: template fabrication of wurtzite ZnS single-crystal nanosheets and ZnO flake-like dendrites from a lamellar molecular precursor ZnS·(NH2CH2CH2NH2)0.5. Adv Mater 14:296–300CrossRefGoogle Scholar

Copyright information

© The Author(s) 2013

Open AccessThis article is distributed under the terms of the Creative Commons Attribution License which permits any use, distribution, and reproduction in any medium, provided the original author(s) and the source are credited.

Authors and Affiliations

  1. 1.Centre for Nanoscience and TechnologyAnna UniversityChennaiIndia
  2. 2.Department of PhysicsAnnamalai UniversityChidambaramIndia

Personalised recommendations