alexa Facile Sensor for Heavy Metals Based on Thiol-Capped CdTe Quantum Dot

ISSN: 2380-2391

Journal of Environmental Analytical Chemistry

  • Research Article   
  • J Environ Anal Chem 2018, Vol 5(1): 232
  • DOI: 10.4172/2380-2391.1000232

Facile Sensor for Heavy Metals Based on Thiol-Capped CdTe Quantum Dot

Souad A Elfeky*
National Institute of Laser Enhanced Science, Cairo University, Giza, Egypt
*Corresponding Author: Souad A Elfeky, National Institute of Laser Enhanced Science, Cairo University, Giza, Egypt, Tel: +201110199538, Email: [email protected]

Received Date: Feb 26, 2018 / Accepted Date: Mar 07, 2018 / Published Date: Mar 13, 2018

Abstract

Background: Semiconductor Quantum Dots (QDs) have gained much attention in different fields of application due to exclusive photochemical reactions. They achieved a big triumph in supramolecular chemistry. A highly sensitive and specific nanosensor was reported in this study using QDs coated with acid for sensing Heavy Metal (HM) ions in water. Few relevant patents to the topic have been reviewed and cited in this article.
Methods: The Mercaptopropionic Acid (MPA)-capped CdTe QDs were prepared through a hydrothermal route and characterized by TEM, FTIR, UV/Vis, fluorescence and XRD techniques. Sensing of HM ions was performed in Deionized Water (DW) by titration of their respective salts with CdTe/MPA.
Results: TEM revealed that the QDs size diameter was in the range of 4 ± 0.2 nm. FTIR, UV/Vis, and fluorescence confirmed the structure and spectroscopic classification of QDs. XRD showed that CdTe/MPA crystals were cubic. Based on the fact that the QDs fluorescence possibly quench by HM ions, an easy process for HM detection was anticipated. The QDs response showed a direct correlation to the concentration of HM. The synthesized QDs had potential for detecting the HM ions with higher selectivity to Mercury ions (Hg2+) in water compared with Lead (Pb2+) and Barium (Ba2+). The optimum sensor sensitivity was achieved at pH 8.
Conclusion: HM ions quenching CdTe/MPA fluorescence in a concentration-dependent manner. The method presented in this manuscript is novel, economical and convenient for realistic applications.

Keywords: Nanosensors; CdTe; Mercury; Lead; Barium

Abbreviations

QDs: Quantum Dots; HM: Heavy Metal; MPA: Mercaptopropionic Acid; MAA: Mercaptoacetic Acid; NCs: Nanocrystals; DW: Deionized Water; FTIR: Fourier Transform Infrared.

Introduction

In the current time, fluorescent QDs have been used in different applications because of their amazing optical properties they are better than organic dyes [1]. QDs Nanocrystals (NCs), turn out to be essential in the industrial field due to their exclusive electronic and spectroscopic characteristics. They achieved great success in supramolecular chemistry [2]. QDs get their importance from the quantum confinement of the excited electrons and holes. This confinement gives rise to unique electronic and optical characteristics that are different from those in bulk semiconductors [3]. Moreover, surface modification of the QDs can enhance their optical properties [4] by obstructing non-radiative electron/hole (e-/h+) recombination [5]. The photostability of QDs can be improved by increasing traps sites on the surface. The generation of new traps on the surface of the QD leads to the appearance of new emission bands. For the previous motives, semiconductor QDs has great achievements in analytical applications [6]. Some literature studied the application of thiolcapped QDs in metal ion sensing [7] and significant success was achieved [8]. Schematic illustration of the effect of HM ions in quenching QD fluorescence is presented in Scheme 1.

environmental-analytical-chemistry-QDs-fluorescence

Scheme 1: Quenching of QDs fluorescence upon HM ion complexation.

For instance, Mercaptoacetic Acid (MAA) capped CdS QDs used for Mercury(II) sensing [9], thioglycolic acid capped CdTe QDs applied to Lead(II) sensing [10]. CdTe QDs was applied before for selective sensing of Cu2+ [11]. A great interest is paid towards sensitive sensors of analytes that have an environmental impact. Monitoring HMs in aqueous media has great significance due to their dangerous effect on the ecosystem.

Mercury is well known for its toxic environmental impact. Mercury comes up from natural or industrial sources. It damages microorganisms and aquatic environment at low concentrations. Consuming water polluted with Mercury causes serious disorders in addition to neurological damage [12]. Consequently, developing good sensitive and selective fluorescent sensor to identify the Mercury ion at low concentration in the aqueous medium is of great interest.

Lead ion (Pb2+), causes a severe damage to human health and the environment [13]. It is found in the environment and its toxicity to animals comes from its non-degradable nature. Lead-poisoning results in severe neurotoxic effects mainly in children. Inductively coupled plasma mass spectrometry is the conventional method used in Lead detection [14]. This is expensive method and requires complicated sample preparation. Therefore, developing a sensitive sensor for detection of Pb2+ in the environment has a great significance.

Barium is a trace element and cannot be found alone in the environment [15]. Some compounds which occur in nature such as Barium sulfate and Barium carbonate contain Barium. Barium at high doses excites arterial muscle and causes vasoconstriction [16]. Barium can cause death, the time between Barium consumption and death toxicity depend on the quantity and the solubility of the Barium compound. Thus death can happen in a few hours or a few days. The lethal oral dose is between 3 and 4 g [17].

Only a few workers have reported the presence of Mercury(II) [18] and Lead(II) ions using semiconductor QDs [18]. However, these methods require complex reaction condition, in addition to the high cost and low yield where no work reported the sensing Barium(II) using semiconductor QDs. This study illustrates a facile preparation of the MPA capped CdTe QDs for application in sensing Hg(II), Pb(II) and Ba(II). This method is straightforward, responsive and economic and can be applied at room temperature conditions.

Materials and Methods

All chemicals were purchased from Sigma Aldrich-UK.

Synthesis of CdTe/MAA NCs

MPA-capped CdTe QDs were synthesized in DW according to the procedure described by Zheng [19] with slight modifications. In brief, NaHTe solution, prepared by adding Te and NaBH4 powder to CdCl2 solution under an inert condition in the presence of MPA. Cd2+:Te2-:MPA molar ratio was 1.0:0.5:2.0. Then, pH of the solution was adjusted to 9.0-9.5 using 1 M NaOH solution. After that, the reaction mixture was heated (100°C) and refluxed to get MPA-capped CdTe QDs. Absolute ethanol was added to separate the MPA-capped CdTe QDs. This process was (precipitation by ethanol) repeated for three cycles to purify the product.

Characterization

• Absorption spectra were recorded using a Perkin-Elmer Lambda 20 spectrometer.

• FTIR spectra recorded with FT/IR-4600 spectrometer (JASCO, Japan).

• CdTe/MPA crystal structure was studied using the X-ray diffractometer system X'Pert³Powder (PANalytical, The Netherlands).

• Fluorescence spectra were recorded with the Perkin Elmer LS 55 fluorescence spectrometer

• Microscopic imaging was acquired by JOEL USA transmission electron microscope.

Sensing of HM ions

The luminescent MPA-capped QDs were dissolved in DW; concentration of QDs is 1.0 mg L-1 [16]. The stock solutions of metal ions were prepared by dissolving their respective salts (HgCl2, PbCl2, BaCl2) in DW, the used concentration of Hg2+, Pb2+, and Ba2+ ions is ranging from 0.4-3.6 ppm. A stock solution of 244 μM from each HM was prepared in DW and 5 μL was titrated (9 times) to 3 ml of MPA/ CdTe (1 mgL-1) in DW. In pH effect experiment, HCl (1 N) and NaOH (1 M) were used to adjust the pH to the proposed value using JENWAY 3505 pH meter. Origin 8 software was used for data processing, statistical analysis, and KSV calculations.

Results and Discussion

Characterization of MPA-capped CdTe QDs

Fourier Transform Infrared (FTIR) spectrometry is a great tool to describe the atoms on the surface. FTIR spectrometry is the unsurpassed technique to chase the surface modification of the synthesized chemical species [20].

Figure 1 shows the FTIR spectra of (a) free MPA and (b) MPAcapped CdTe QDs. The IR absorption bands at 3034 cm−1 (νOH, COOH), 2550–2650 cm−1 (νS–H), 1710 cm−1 (νC=O), 1400 cm−1 (νCOOH), and 1277 cm−1 (νC–O) are for MPA. The bands at 3410 cm−1 (νOH, COOH), 1380–1555 cm−1 (νs COOH) and 1290 cm−1 (νC– O) are for MPA-capped CdTe QDs. MPA-capped CdTe QDs and free MPA FTIR illustrated the presence of carboxyl and carbonyl groups absorption peaks. This confirms the coexistence of these groups on the shell of the CdTe QDs. The missing of S–H (2550–2650 cm−1) vibration peak in MPA-capped CdTe QDs may be due to the covalent bonding between thiols and Cd atom on the QDs surface. These results agree with Zhang [21] who found that the sulfhydryl group band at 2567 cm−1 lost in the FTIR spectrum of MPA-capped QDs.

environmental-analytical-chemistry-FTIR-spectrum

Figure 1: FTIR spectrum of (a) MPA (b) MPA-capped CdTe QDs.

The morphology and size of the prepared QDs were studied by the TEM. The image in Figure 2a shows that the MPA-capped QDs are dispersed and mostly spherical particles. HRTEM in Figure 2b reveals that the average crystal size is 4 ± 0.2 nm.

environmental-analytical-chemistry-TEM-HRTEM

Figure 2: (a) TEM, (b) HRTEM (c) XRD of MPA/CdTe QDs.

The XRD wide diffraction peak at 2θ=26.7 of the prepared CdTe QDs (Figure 2c) can be indexed to the (200) reflection for cubic CdTe complying with the standard pattern (JCPDS card 75- 2083). The broad peak indicates the occurrence of small size nanoparticles [22,23].

From the XRD data, the diameter of the MPA/CdTe QDs can be calculated using Scherrer formula [24] as shown in equation (1):

d=Kλ/βcos θ (1)

Where, d=crystal size, K=Scherrer constant (0.89), λ=wavelength of the X-ray radiation (0.15418 nm for Cu Kα) and β=full width at half maximum of diffraction peaks measured at 2θ.

From equation (1), the calculated QDs crystal size is 3.5 nm. The calculated size usually 10-15% less than the size of particles that appears under electron microscopy as the X-ray coherent scattering applies to the internal side of the crystal and does not include margins.

The absorption and emission of MPA-capped CdTe QDs were measured by UV–visible absorption spectrometry and fluorescence spectroscopy as shown in Figure 3. The absorption peak of the MPAcapped CdTe nanoparticles is noticed at 520 nm and the fluorescence emission is found at 545 nm (λex=400 nm). In fact CdTe NCs generally have no luminescent properties until they are stabilized with mercapto compounds as mentioned by Wei-Heng in his patent entitled: Water soluble nanocrystalline QDs [25].

environmental-analytical-chemistry-fluorescence-spectrum

Figure 3: Absorption and fluorescence spectrum of CdTe QDs and MPA-capped CdTe QDs.

Effect of pH on the CdTe/MPA sensitivity to HM

The pH has a significant effect on the fluorescence intensity of the system. In addition, the pH affects the solubility of the QDs and its interaction in the system. Kotov [26] mentioned in his patent that CdTe luminescence displays strong sensitivity to the pH of the media. He also explained that the variation of pH will change the electrostatic attraction between CdTe and metals. The pH in the range between 4 and 11 was studied to select the optimum sensitivity pH. From Figure 4, it is obvious that maximum sensitivity of CdTe/MPA was at pH 8 for all the tested HM ions.

environmental-analytical-chemistry-Normalized-fluorescence

Figure 4: Normalized fluorescence of MPA-capped CdTe QDs (λmax 546.4 nm) at different pH values, HM Concentration=3.6 ppm.

The previous study also confirmed that the optimum sensitivity of QDs to HM was at pH 8 [16]. The QDs sensitivity decrease in the acidic medium may be due to the dissociation of Cd2+– MPA–QDs as the surface binding thiolates protonated in acidic medium [27]. The fluorescence intensity enhanced with increasing the pH increase up to 8. This can be ascribed to the deprotonation of MPA thiol group at higher pH, as a consequence, the covalent bond between thiol and Cd atom at the surface of QDs becomes stronger. Thus, the increase of pH maintains carboxylic acid group negative charge and promotes the interaction with HM ions [28]. At pH>8, the fluorescence intensity decreases due to hydration of the QD surface. Furthermore, hydroxides of HM ions are precipitated at high pH values.

The fluorescence response of MPA-capped CdTe QDs to different Hg2+, Ba2+ and Pb2+ concentrations at pH 8 is illustrated in Figure 5. Figure 5 displays the fluorescence emission spectra of MPA-capped CdTe QDs containing various concentrations of (a) Hg2+, (b) Ba2+ and (c) Pb2+ respectively. Fluorescence intensity was regularly quenched by adding more HMs, this may be due to the change on the surface of QDs after HM addition. Fluorescence quenching of CdTe QDs as a response to HM addition can be explained in view of electron transfer from MPA to Hg2+, Ba2+or Pb2+ [29]. The QD sensing to HM was patented before by Wu [30] who found that QD fluorescence emission energy transfer can detect the presence and the quantity of the HM.

environmental-analytical-chemistry-MPA-capped

Figure 5: MPA-capped CdTe QDs (QDs (1 mg L-1, λex=400 nm) fluorescence quenching in the presence of Hg2+ (a), Ba2+ (b) and Pb2+ (c) at various concentrations and pH 8.

Comparing the QDs sensing results of different HMs, it was found that the used HMs quench the fluorescence of QDs in a concentrationdependent manner. Similar results were obtained by Ming [31] who found that L-cysteine modified CdTe QD fluorescence intensity changes in relationships with Mercury concentration. In this study, when increasing the concentrations of Hg2+, Ba2+ and Pb2+, the fluorescence intensity MPA-capped QDs gradually reduced to 4%, 22% and 54% (respectively) of the initial intensity after the primary sharp decline, while the fluorescence of Ba2+ treated QDs continues on decreasing till getting the plateau. Numerous quenching approaches have been anticipated to describe QDs fluorescence quenching by metal ions. Some mechanisms such as inner filter effect, ion binding interaction, electron transfer process, and non-radiative recombination pathway are capable of explaining the quenching phenomena [32,33]. From the results, there was no obvious shift in emission wavelength (emission band centered 545 nm with the excitation 400 nm) by adding more concentration from HM ions. Thus, it is suggested that the quenching in this system is ascribed to enhancing non-radiative recombination of excited electrons (e-) and holes through the effective electron transfer from MPA to HM ions [34].

It was reported that ion sensitivity and selectivity depend on the function groups of the QDs surface [34]. It is known that mercapto acids molecules have high tendency as chelating agents for Hg2+ than other HM ions [35]. In our study, the ion sensitivity was in the following order Hg(II)>Ba(II)>Pb(II). A patent entitled “Sensors using AIGaN/GaN high electron mobility transistors” invented by Fan [35], also used thioglycolic acid as a chelating ligand and sensor binding site for HM detection in solution. From the results, it is obvious that QDs fluorescence quenching boosted by increasing HM concentration that can be represented by the Stern–Volmer relationship which is given by the following equation (2):

I0/I=1+KSV[HM] (2)

I0/I=fluorescence intensities of QDs in the absence and presence of HM, respectively. HM=heavy metal concentration, KSV=Stern–Volmer constant [36].

The slope of the I0/I versus the concentration curve (Figure 6) is the Stern-Volmer constant KSV [37]. Table 1 illustrates the KSV, Standard Error (SE) and R-square (R2) values for CdTe/MPA QDs interaction with the used HM.

HM KSV SE R2
Hg(II) 23.1 2.4 0.9
Ba(II) 4.5 0.58 0.85
Pb(II) 0.96 0.03 0.99

Table 1: KSV, SE and R2 values for CdTe/MPA QDs interaction with Hg(II), Ba(II) and Pb(II).

environmental-analytical-chemistry-Stern-Volmer

Figure 6: Stern-Volmer plot for the quenching of CdTe/MPA QDs (1.0 mg L-1) by HM at λmax 546.4 nm and pH 8.

Conclusion

The HM ions quench the fluorescence of the MPA-capped CdTe QDs in a concentration-dependent manner. The quenching was found to be relative to the amount of HM ions that can be described by the Stern–Volmer relationship. The MPA-capped CdTe shows a higher affinity for Hg2+ than other used HM ions. The optimum sensor sensitivity was achieved at pH 8.

Acknowledgement

The author is very grateful to the University of Cairo and University of Bath (Chemistry Department) for supporting this research.

Conflict of Interest

The author declares that there is no conflict of interest regarding the publication of this paper.

References

Citation: Elfeky SA (2018) Facile Sensor for Heavy Metals Based on Thiol-Capped CdTe Quantum Dot. J Environ Anal Chem 5: 232. Doi: 10.4172/2380-2391.1000232

Copyright: © 2018 Elfeky SA. This is an open-access article distributed under the terms of the Creative Commons Attribution License, which permits unrestricted use, distribution, and reproduction in any medium, provided the original author and source are credited.

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