Bambesiwe M. Mayab,
Mokae F. Bamboc,
Seyed Saeid Hosseiniad,
Unathi Sidwabaa,
Edward N. Nxumaloa and
Ajay K. Mishra*efg
aInstitute for Nanotechnology and Water Sustainability (iNanoWS), College of Science, Engineering and Technology, University of South Africa, Florida Campus, Johannesburg, South Africa
bMintek Analytical Chemistry Division, Private Bag X3015, Randburg 2125, South Africa
cDSI/Mintek Nanotechnology Innovation Centre, Advanced Materials Division, Private Bag X3015, Randburg 2125, South Africa
dDepartment of Chemical Engineering, Vrije Universiteit Brussel, Pleinlaan 2, 1050 Brussels, Belgium
eDepartment of Medicine and Chemical Engineering, Hebei University of Science and Technology, Shijiazhuang, 050018, China. E-mail: ajaykmishraedu@gmail.com
fAcademy of Nanotechnology and Waste Water Innovations, Johannesburg, South Africa
gDepartment of Chemistry, School of Applied Sciences, KIIT Deemed University, Odisha, India
First published on 11th April 2022
Heavy metal contamination remains a major threat to the environment. Evaluating the concentrations of heavy metals in water environments is a crucial step towards a viable treatment strategy. Non-cadmium photo-luminescent I–III–VI ternary QDs have attracted increasing attention due to their low toxicity and extraordinary optical properties, which have made them popular in biological applications. Recently, ternary I–III–VI-QDs have gained growing interest as fluorescent detectors of heavy metal ions in water. Here, we review the research progress of ternary I–III–VI QDs for the fluorescence detection of heavy metal ions in water. First, we summarize the optical properties and synthesis methodologies of ternary I–III–VI QDs. Then, we present various detection mechanisms involved in the fluorescence detection of heavy metal ions, which are mostly attributed to direct interaction between these unique QDs and the metal ions, seen in the form of fluorescence quenching and fluorescence enhancement. We also display the potential applications in environmental remediation such as water treatment and associated challenges of I–III–VI QDs in the fluorescence detection of Cu2+ and other metal ions.
The contamination of water systems by inorganic pollutants such as heavy metals remains a major concern. Copper (Cu), manganese (Mn), cobalt (Co) and zinc (Zn) are among the few heavy metals essential for human health, although they become toxic at high concentrations.1 Other metals like mercury (Hg), lead (Pb) and cadmium (Cd) are non-essential and toxic.2,3 These pollutants contaminate water streams which are used for irrigation purposes and agricultural land even at trace concentrations, posing a high health risk to the people consuming the water and agricultural products. Moreover, these pollutants are not biodegradable therefore they are persistent in water streams and agricultural land. The prolonged exposure of humans to these metals can cause various diseases, e.g. brain damage, kidney dysfunction, organ failure, and bone disorder.4,5 Hence, the World Health Organisation (WHO) and the United States Environmental Protection Agency (USEPA) have established maximum concentration levels for some of these metals of concern.6 Thus, it is imperative to detect these pollutants to protect the environment and prevent diseases. Additionally, the proper evaluation of the amounts of heavy metals present in the water environments is a crucial step towards the formation of a viable treatment plan.
The analysis of heavy metal ions in water requires highly sensitive and selective technologies that can easily integrate with microfluidic media. Atomic absorption spectroscopy (AAS), inductively coupled plasma optical emission spectroscopy (ICP-OES), and mass spectroscopy (ICP-MS) are among the most common analytical techniques for the determination of heavy metals.7,8 They show excellent sensitivity, and some are with multi-element analysis capability (i.e. ICP-OES and ICP-MS). However, they are expensive and often involve sample preparation methods which can be complex, time-consuming, and error prone.
Nano-based material sensing has emerged as a key role player in the field of heavy metal ion detection.9–16 Since these materials are in the nanoscale, their unique chemical and physical properties such as large surface area, chemical affinity, and surface activity can aid the sensing processes.17,18 Among the nano-sensing systems, quantum dot (QD)-based fluorescent probes have gained popularity due to their efficient small catalytic sizes which help to display low detection limits, fast response time, high specificity,19–21 anti-pathogenic effects (e.g. virucidal22 and bactericidal properties23,111) and high influx membrane-based antifouling metal-doping effects.24,110 Also, they exhibit optical properties such as high photoluminescence quantum yield (PLQY), photoluminescence (PL) spectra from the ultraviolet-visible to the near-infrared and high photostability, which make them ideal fluorescence sensors25 as well as photodegradation, and photodynamic therapeutic agents.23 As sensors, their detection strategy is based on compromising or enhancing their fluorescence properties upon exposure to the analyte, which can be seen with changes in intensity, PL lifetime, and emission peak position at varying concentrations of the analyte.26
In the past years, QD nanomaterials have been employed for water treatment purposes in the form of sensors (for inorganic and organic targets), photocatalysts27 and microbial inhibitory agents.23 Among these nanomaterials, several II–VI based (CdSe, CdS) QDs28,29,117,118 and ZnS QD based fluorescent sensors30,31 were designed for screening of heavy metal ions. However, ternary I–III–VI QD probes are still the least explored in this field. Ternary I–III–VI QDs have been receiving growing interest mainly because of their attractive optical and electronic properties and offering of safer alternatives compared to II–VI and IV–VI (PbSe) QDs.32–34 This makes them popular in biological applications,35–39 water treatments and biocompatible solar cells applications.37,40,41 Specifically, this safety advantage has been extended by demonstrating the analytical potential of I–III–VI QDs as heavy metal ion detectors in water.42–44 The comprehensive review on the biological,35,36 photocatalysis/disinfections23 and energy45 applications of QD materials have been previously reported by several authors and thus will not be covered in this review. Thus, this review aims at presenting the research progress on I–III–VI ternary QDs as fluorescent detectors for heavy metal ions in water. The detection mechanisms based on the direct interaction between the QDs and metal ions, evident by fluorescence quenching and fluorescence enhancement are fully described. Also, the potential in real water treatment applications together with challenges and future prospects of these materials is fully elucidated.
I–III–VI ternary QDs are derived from II–VI binary QDs by replacing the divalent cation with one monovalent and one trivalent cation to synthesize less toxic QDs with similar excellent optical properties. Unlike II–VI and IV–VI binary QDs, most ternary QDs do not exhibit a sharp exciton peak but rather an absorption band edge. This is a known feature of ternary QDs, which is associated with surface defects on the crystal structure, making it a challenge to determine the size-dependent bandgap.53 Considering this challenge, Mao et al.47 demonstrated a theoretical calculation of the I–III–VI band gap using Tauc law from the absorption band edge of the semiconductor material.
(Ahν) α(hν − Eg) 1/2 for hν < Eg | (1) |
In the equation, hν is the energy of the absorbed photons, Eg is the bandgap of the semiconductor material and A is the absorption band edge.47
The photoluminescence (PL) characteristic features of I–III–VI ternary QDs include broad full width at half maximum (FWHM) (i.e. between 80–120 nm) of the PL peak, large stokes shift and slow PL lifetimes compared to binary QDs.35,37,40,53 These features mainly arise due to their various defects. For example, in CuInS2 core QDs defects such as Cu vacancies (VCu), indium–copper (In–Cu) antisite defects and sulfur (S) vacancy defect may occur. Additionally, the varied molecularity and mole ratios in Cu, In and S precursors involved in the synthesis are also contributors to these features.40 Time-resolved PL (TRPL) spectra are often measured to recognize the PL lifetimes in the recombination process during emission. TRPL of ternary I–III–VI QDs reveals multiple emission states (Fig. 1) which arise from surface-related states due to dangling bonds, donor–acceptor pairs (DAP) involving surface defects (DAPsurf), or intrinsic defects (DAPint).55,56 Furthermore, some ternary I–III–VI QDs revealed DAPsurf and DAPint as the dominating components contributing towards their emission.43,56,57
Fig. 1 Photoluminescence mechanisms in AgInS2/ZnS QDs [reprinted with permission from ref. 55 Royal Society of Chemistry]. |
In another case, Mao et al.53 investigated the PL behavior of AgInS2 core and AgInS2/ZnS core/shell QDs. The results showed the reduction of surface defects with an increase in the particle size of the core QDs and further reduction of surface defects after ZnS shell coating. The PL spectra showed two deconvolution peaks relative to the QD emission peak, where peak 1 (in shorter wavelengths) was attributed to surface defects and peak 2 (at longer wavelengths) was attributed to intrinsic trap states. Intrinsic trap states are known to easily form in I–III–VI compounds between interstitial atoms which are responsible for donor–acceptor transitions. The results revealed a decrease in the emission intensity at peak 1 and an increase in peak 2 when the particle size increased with time. The same result was observed after the ZnS coating, which leads to higher PLQY. The reduced surface defects at an increased size are attributed to the fact that larger particles exhibit reduced surface to volume ratio which leads to fewer surface defects.53
In other reports, Li et al.62 enhanced the poor photoluminescence properties of CuInS2 core QDs by coating with cadmium sulfide (CdS) shell. An initial blue-shift followed by a red-shift in PL peak of CuInS2 core QDs with continuous CdS shell growth was reported. This was attributed to the lower conduction band of CdS compared to ZnS. PLQY increased from 5–10% to 86% after the growth of CdS shell and PL lifetime studies revealed that the non-radiative rates were largely reduced after coating of the core QDs with the shell.62 The coating of silica on CuInS2/ZnS core/shell QDs revealed enhanced stability but the PLQY was slightly reduced.66 Furthermore, stability was maintained when CuInS2/ZnS QDs were coated with ZnGa2O4.67 Rao et al.68 presented the self-passivation of Al2O3 on CuInS2/ZnS QDs to improve photostability. The Al2O3 passivation prevented the oxidation of sulfur on the surface of the QD after irradiation, suggesting that it improved photostability of the CuInS2/ZnS core/shell QD.68
Over the years, doping of QDs has been extensively explored.58,69–72 Doping is a process that involves introducing atoms to QDs to achieve additional properties. For instance, Guo et al.73 reported enhanced PLQY when Zn2+ was incorporated into CuInS2 core QDs to form quaternary CuInZnS QDs. The author also demonstrated the inhibition of the emission blue-shift during ZnS shell growth on CuInS2 QDs when Zn ions were intentionally introduced into the CuInS2 core QDs. This action inhibited the cation-exchange process occurring between Zn and the cations (Cu2+/In3+) during ZnS shell formation.73 In other reports, doping I–III–VI ternary QDs with Mn2+ or Gd3+ introduced a magnetic property which resulted in negligible decreases in PLQY and their application in fluorescence/magnetic resonance imaging studies.70,74,75
On the other hand, Sharma et al.56 demonstrated the effect of increasing Zn quantities on AgInZnS QDs of the same size to separate the size effect from the composition effect. The study showed a gradual decrease in the PL lifetime at increased Zn amounts, while the surface defects decay components increased from 22 to 57% at increased Zn amounts, which was an opposite result to Komarala's report.60 In addition, the slow decay component was reduced from 21 to 3% at increased Zn amounts, an indication that the surface-related traps involving dangling bonds were reduced. The study also gave insight into the changes in non-radiative (knr) and radiative recombination (krad) rates at varied PLQY. The PLQY of AgInZnS nanocrystals (NCs) increased with increased Zn amounts (x = 1 to x = 0.7), while higher Zn amounts (x = 0.3) reduced the PLQY. The average PL lifetime (τ), and PLQY values of the NCs were used to determine the non-radiative (knr) and radiative (krad) recombination rates (Table 1) using equations below.56
(2) |
AgInZnS(x) | PLQY (%) | τ (ns) | krad (s−1) | knr (s−1) |
---|---|---|---|---|
1 | 40.4 | 2518 | 0.16 × 106 | 0.24 × 106 |
0.7 | 70.6 | 1647 | 0.43 × 106 | 0.18 × 106 |
0.3 | 53.0 | 1017 | 0.52 × 106 | 0.46 × 106 |
The results showed that Zn initially increased PL lifetime where non-radiative surface decays were reduced and the radiative sites within the NCs were increased, then higher Zn quantities increased the non-radiative surface decays.56
Although organic synthesis produces high-quality QDs, it might not be suitable for all applications. For example, biological applications require the material to be biocompatible, hydrophilic, and non-toxic. Therefore, it is imperative to change the organically soluble QDs to water-soluble without losing their optical properties. This can be achieved through ligand–exchange with hydrophilic ligands, silica shell coating as well as encapsulation with amphiphilic ligands. A desirable ligand of interest is usually thiols with water-soluble functional groups such as carboxylic groups. Thiol binds to the surface of the QDs and the water-soluble groups on the surface make it soluble in aqueous media. An example of such ligands is 11-mercaptoundecanoic acid (MUA), which was reported to be biocompatible and low in toxicity.46 Mao et al.46 reported ligand exchange of DDT-stabilized AgInS2/ZnS QDs with MUA ligand. The process involved the dispersion of QDs with MUA in chloroform under sonification. The absorption and PL spectrums were like those obtained for DDT-stabilized QDs with emission peaks positioned at 809 nm. A time-resolve study was carried out, where biexponential function showed a decrease for both r1 (fast decay) and r2 (slow decay) components which led to a decrease in the PL decay average (rave) from 349.4 to 324 ns. This was attributed to the decreased stability of the QD surface due to the exchange of the ligands. Regardless, the rave value was still higher than that obtained for II–IV binary QDs.46 Although water-soluble QDs can be produced through ligand–exchange, a decrease of 5–35% in PLQY usually occurs.78,83,84 This decrease has been attributed to the surface traps due to poorly coated QD surface after passivation. Besides, the reactions involve long reaction times and then transfer to water-soluble means additional synthesis steps which can be tedious. Nonetheless, the synthesis of organic soluble QDs requires high temperatures, large quantities of organic solvent, and sometimes make use of unstable and hazardous precursors which are not ideal for green synthesis. Therefore, a lot of attention has been paid to direct aqueous synthesis of ternary QDs.
Fig. 2 Proposed mechanisms for analyte interaction with the NP samples [reprinted with permission from ref. 89 American Chemical Society]. |
Fluorescence mechanism A assumes the attack of surface ligand by a metal ion, resulting in detachment of the ligand. This destabilizes the QD, leading to reduced fluorescence.90 Mechanism B suggests direct interaction with the host QD, which could result in cation exchange with the metals in the QD.42,43,89,91 Mechanism C involves forming passivating layers with QDs surface, which cover surface defects and enhance fluorescence.44,89,92,93
Fluorescence quenching can also be a result of the inner filter effect (IFE) which occurs when a species absorbs excited/emitted light during the detection process. This can be seen in the overlap of the absorption spectra of the absorber and the excitation spectra of the fluorophore.21 IFE is not categorized as a major quenching process since it does not involve radiative and non-radiative transitions in fluorescence measurements.101 Therefore, other mechanisms besides IFE could be attributed to the quenching. Moreover, IFE has been reported to enhance the sensitivity compared to other mechanisms because the changes in the absorbance of sensors can transform exponentially into fluorescence intensity changes.102–104
Fig. 3 (A) PL intensity of the CuInS2/ZnS/TGA QDs in addition of various concentration of Co2+. Inset: The extent of the quenching (F0/FI) versus the concentration of Co2+. (B) UV-vis absorption spectra (a and b) and PL spectra (c and d) of QDs solution in the absence (a and c) and presence (b and d) of Co2+. Inset: the photo of QDs solutions in the absence (left) and presence (right) of Co2+ in natural light. (C) UV-vis absorption spectra of mixture of Co2+ and TGA (a), mixture of Co2+ and thioglycerol (b), and mixture of QDs and Co2+ in the absence (c) and presence (d) of excess carboxyl. Inset: The photo of the mixture solutions of TGA (left) and thioglycerol (right) with Co2+ respectively in natural light [reprinted with permission from ref. 90 copyright 2013 Elsevier]. |
Fig. 4 Schematic representation for the coordination of Co2+ ions and CuInS2/ZnS/TGA QDs [reprinted with permission from ref. 90 copyright 2013 Elsevier]. |
Anand et al.105 and Gore et al.106 speculated TGA–metal complexes were either due to interaction between the metal ion and the carbonyl group or sulfur group respectively.105,106 Therefore, absorbance spectra of Co2+ ions exposed to TGA and Co2+ ions exposed to thioglycerol were investigated to determine the interaction. The results showed two peaks centered at 370 nm and 470 nm for Co2+–TGA solution and similar spectra with slight shifts were observed for Co2+–thioglycerol solution, which was attributed to the presence of carbonyl groups in the TGA solution. The similar spectra indicated that the interaction between Co2+ and TGA was indeed through the sulfur group and not the carbonyl group (Fig. 3C).
The effect of temperature on the fluorescence intensity of the QDs with Co2+ ions was studied to confirm the type of quenching. During dynamic quenching, the quenching constant increased while in static quenching, the constant decreased with a rise in temperature. The data was analyzed using the Stern–Volmer equation and the results revealed an inversely proportional relationship with temperature, confirming static quenching mechanism.90
Establishing the type of quenching gave insight into the binding involved in the quenching. Thus, IFE was identified as the partial contributor towards the quenching of the QDs upon exposure to Co2+ ions. This could be confirmed by the overlap in the excitation wavelength of the QDs at 365 nm with the absorption spectra of the QDs-Co2+ solution (Fig. 3B). This indicated that less light entered the QDs when excited at 365 nm, thus reducing the fluorescence because changes in absorbance could exponentially transfer to the resulting fluorescence properties.90
Fig. 5 (A) The fluorescence spectra of AgInZnS–graphene oxide (GO) nanocomposite after addition of different Cu2+ concentrations of sample 1 to 16 i.e. 0, 10, 30, 60, 100, 150, 200, 250, 300, 350, 400, 500, 550, 650, 750, 850 μM, respectively. (B) TEM images of AgInZnS–GO NC in absence and (C) presence of Cu2+ ions (850 μM) [reprinted with permission from ref. 99 copyright 2016 Elsevier]. |
Parani et al.100 reported GSH capped AgInS2–ZnS QDs for the detection of Cr(III) ions. The PL intensity of the QDs was quenched with increased Cr3+ ion concentration between 0.025 μM and 10 μM, accompanied with gradual red-shifting of the PL peak from 623 nm to 630 nm (Fig. 6A). The quenching behaviour was attributed to the aggregation of the QD after addition of Cr3+ ions, seen in the TEM image (Fig. 6B). The authors proposed that the aggregation was due to the attachment of Cr3+ ion onto the surface GSH; since Cr3+ is a hard acid, it binds to oxygen and nitrogen rich ligands, GSH being rich in these, a Cr3+–GSH complex forms on the surface. FTIR analysis showed significant shifting of the COO− peaks to higher wavenumbers after addition of Cr3+ ions, confirming that the Cr3+−GSH interaction occurred through the GSH carboxylate group likely by electrostatic interaction. Furthermore, the Cr3+–GSH complex formation resulted in reduced electrostatic repulsion between the QDs hence the aggregation. As a result, an imperfect QD surface was initiated which facilitated non-radiative recombination hence the quenched PL100.
Fig. 6 (A) The PL spectra of GSH capped AgInS2–ZnS QDs after addition of different Cr3+ concentrations. (B) TEM images of GSH capped AgInS2–ZnS QDs after addition of Cr3+ ions [reprinted with permission from ref. 100 IOP Publishing]. |
Scheme 1 Schematic illustration for the fluorescence quenching of DTAB-capped AIZS QDs by Cu2+ ions [reprinted with permission from ref. 107 copyright 2017 Elsevier]. |
The authors also displayed this mechanism in sodium dodecylsulfate (SDS)-capped AgInZnS QDs. The zeta potential of the QDs was −36.8 mV, demonstrating that the negatively charged QDs bonded with Cu2+ through electrostatic interactions which resulted in the electron transfer from the QD to the Cu2+. This aided the reduction of Cu2+ to Cu+, which was also confirmed by XPS analysis.108
Later, an optical fiber nanoprobe based on (SDS)-capped AgInZnS QDs was developed for the detection of Cu2+ ions. The QDs were deposited on silica optical fiber ends using polyvinylalcohol (PVA) as an entrapment matrix. The PL intensity of the QDs was reduced after the addition of Cu2+ ions, while the average lifetime of the QDs decreased from 500 ns to 325 ns. The reduced PL decay could be due to the reduced radiative pathways facilitated by some electrons being transferred to Cu2+ ions.109
Liu et al.44 reported fluorescence detection of Cu2+ ions using MPA-capped CuInS2 QDs. The PL quenching of the QDs upon exposure to Cu2+ was attributed to the formation of either Cu2S precipitate or isolated Cu+ ions on the surface of the MPA capped QDs. This was facilitated by the reduction of Cu2+ to Cu+ through electron transfer from QDs to Cu2+ ions. In addition, the QD–Cu2+ mixture was exposed with EDTA, a Cu2+ extracting agent. No changes in the PL spectra was observed, indicating that the quenching reaction could not be reversed, suggesting that static quenching could also be involved. Modifying the QDs with Cd2+ played a profound role in improving the sensitivity, detection range and limit. In this reaction, the quenching might be due to the Cu2+ adsorption on the surface of Cd modified QDs, which changed the original surface state (CuInS2–Cd-SR), inducing the non-radiative recombinations and thus reducing the radiative emission (Scheme 2).44
Scheme 2 Cu2+ and Cd2+ ion detection process using CuInS2 QDs [reprinted with permission from ref. 44 Royal Society of Chemistry]. |
Recently, Jiao et al.43 reported GSH capped CuInZnS/ZnS (CIZS/ZnS) QD fluorescent probe for the detection of Cu2+ ions via cation exchange. The results showed PL quenching accompanied by red-shifted emission peaks at increased Cu2+ ions concentrations (Fig. 7).
Fig. 7 PL spectra of the CIZS/ZnS QDs in the presence of different amounts of Cu2+ ions [reprinted with permission from ref. 43 copyright 2019 Elsevier]. |
The chemical compositions of QDs in the absence and presence of Cu2+ ions revealed a decrease in In and Zn content from 55.0% to 54.3% and 37.5% to 33.7% at increased Cu2+ concentrations, respectively, as shown in Table 2. Since ZnS has a wider bandgap than CuInS2, the replacement of Zn with Cu2+ resulted in a redshift of the absorbance and PL spectra. In addition, the cation-exchange of Zn and In in the QD core at different degrees occurs because although In is a harder Lewis acid than Zn, it is more difficult to exchange it with Cu2+ (weaker Lewis acid) due to In2S3 exhibiting a lower ksp value than ZnS and Cu2S. Thus, In would exchange at a lower degree than Zn. PL lifetime studies displayed a decrease in lifetimes at increased Cu2+ ion concentrations from 413 ns to 289 ns (100 μm Cu2+ ions). This suggested a change in the recombination processes of the QDs, which was an indication of increased non-radiative surface defects, hence the decrease in the PL intensity.43
[Cu2+] detection (μM) | 0 | 0.1 | 1 | 10 | 100 |
---|---|---|---|---|---|
Cu content (%) | 7.52 | 7.65 | 7.77 | 8.13 | 12 |
Zn content (%) | 37.5 | 37.4 | 37.3 | 36.9 | 33.7 |
In content (%) | 55.0 | 55.0 | 54.9 | 54.9 | 54.3 |
Han et al.91 displayed GSH capped AgInZnS for the detection of Cu2+ ions. The fluorescence intensity of the QDs also decreased with increase Cu2+ ion concentration with a gradual redshift in the emission peak (Fig. 8). These results suggest possible cation exchange interaction between Cu2+ ions and the cations in the QD core, as seen in other publications.42,43
Fig. 8 PL spectra quenching spectra of AIZS QDs with different concentrations of Cu2+ [reprinted with permission from ref. 91 Royal Society of Chemistry]. |
Cambrea et al.89 fabricated three AgInZnS NPs of different Zn:Ag:In mole ratios with identical non-specific ligand dodecylamine. The Zn:Ag:In mole ratios for NP1, NP2 and NP3 were 0:1:1, 0.6:0.7:0.7 and 1.2:0.4:0.4 respectively. The study focused on determining metal ion specificity detection based on the interaction of the metal ion with the core NP containing different metal mole ratios. The study showed a different response to all three NPs for each metal ion. For example, NP3 dissolved in CHCl3 and CH3CN was selective towards Cu2+ ions compared to Fe2+ and Co2+, as seen in the complete quenching of the PL peak at 500 nM (Fig. 9). In addition, the quenched PL peak maximum was seen at a longer wavelength indicating a redshift. On the other hand, NP1 showed complete quenching when exposed to dichromate while chromate had the least quenching effect even though both solutions were of chromium in the same valency state of +6. NP2 was significantly quenched by Hg2+ ions at 500 nM, whereas it was one of the least reactive analytes in NP1 and NP3. The report highlighted that most metal ions at mM ranges caused precipitates to form in quenched NP solution, which could be linked to fluorescence mechanism A (Fig. 2). However, since all metal ions responded differently to all the three NPs, the quenching mechanism might involve other interactions other than the cation exchange (fluorescence mechanism B), as shown in Fig. 2. Particularly, Cu2+ ion detection by NP3 could be partly attributed to cation exchange indicating direct interaction of the core NP with Cu2+ ions. These suspicions are based on the red-shift PL peak apart from the PL decrease also seen in the detection of the other metals. Since NP3 contains the highest amounts of Zn, it is most likely to experience cation exchange reactions between Zn and In in the QD and Cu2+ ions interaction than the other two NPs. However, further investigations are required to confirm this possibility.89
Fig. 9 PL spectra of NP3 in CHCl3/CH3CN with 500 nM (∼1 ppm) of Fe2+, Co2+ and Cu2+ metal ions [reprinted with permission from ref. 89 American Chemical Society]. |
Xiong et al.42 reported the synthesis of GSH-capped AgInS2/ZnS core/shell QDs via microwave irradiation route. The core/shell material displayed quenched and red-shifted emission after the addition of Cu2+ ions (Fig. 10). This could be due to the replacement of Zn2+ with Cu2+ ions, forming a CuS layer on the QD surface, thus inducing the non-radiative recombinations.42 The red-shifted emission is not surprising since ZnS (3.54 eV) has a wider bandgap than CuS (1.97 eV).116
Fig. 10 PL spectra of AgInS2/ZnS NCs (0.02 mg mL−1) exposed to different amounts of Cu2+. Inset: the correlation curve of I0/Ii as a function of the concentration of Cu2+ from 0.1 μM to 10 μM [reprinted with permission from ref. 42 Royal Society of Chemistry]. |
Several interactive routes that result in quenching may have been reported but a clear attribution of interactions remains a challenge, which leads to the suspicion that the interaction could be most likely a combination of interactive routes in some cases. For example, some authors reported the detection of Hg2+ using Cd based QDs through quenching via a combination of interaction mechanisms. The detection was attributed to both cation exchange between the QDs and the Hg2+ as well as ligand detachment from the QD surface.112,113 Future studies need to consider all possible pathways to obtain detailed information on the interactions involved in the detection process.
The study on the three AgInZnS NPs (of different metal ratios) for the detection of heavy metal ions revealed an increase in PL on exposure to Cd2+ ions for all the NPs (Fig. 11A).89 This is not surprising because core QDs are expected to have surface defects since they are bare. Thus, the addition of Cd2+ fills the defect sites and enhance the PL by reducing the non-radiative recombinations.89 Similar results were seen in MPA capped CuInS2 QDs (Fig. 11B),44 where the exposure to Cd2+ improved the PL intensity but PL quenching occurred at higher concentrations indicating saturation of the surface traps.44 MPA capped AgInZnS QDs (Fig. 12) also revealed continuous increase in PL intensity with increased Cd2+ concentrations due to surface defect passivation, which was verified by the prolonged fluorescence lifetimes and increased PLQY.92 The average lifetime and PLQY of the AgInZnS QDs increased from 262.55 ns to 292.33 ns and 41% to 49% respectively after the addition of 290 μM Cd2+. The AgInZnS QDs exhibited a zeta potential of −44 mV suggesting that Cd2+ ions adsorbed onto the negatively charged QD surface through electrostatic interactions, which passivated the surface trap state of the QDs. As a result, the PLQY was enhanced and the fluorescence lifetime were elongated.92 Recently, aggregation induced emission enhancement (AIEE) was seen in L-cysteine capped Zn–Ag–In–S quaternary QDs when exposed to Cd2+.93 The PL enhancement of the Zn–Ag–In–S QDs was accompanied by blue-shifted PL peaks and aggregation of the QDs (Fig. 13A). This was attributed to the binding of Cd2+ to thiol anions on the QD surface, leading to weakened electrostatic repulsion between the QDs and passivation of surface defects, TEM images (Fig. 13B and C) show the well dispersed Zn–Ag–In–S QDs and aggregated QDs when exposed Cd2+. Furthermore, macroscopic floc formation was seen at high Cd2+ concentrations. The weakened electrostatic repulsion can be confirmed by the reduced negative charge after Cd2+ addition from −38.8 mV to −27.4 mV. The blue-shifted PL peaks at increased Cd2+ concentrations are suspected to be due to the diffusion of Cd2+ in the Zn–Ag–In–S QD broadening the band gap. The possible mechanism responsible for AIEE is shown in Fig. 13D.93
Fig. 11 (A) PL spectra of NP2 in the presence of Cd2+ ions. As the amount of Cd2+ is increased the fluorescence increases by an order of magnitude [reprinted with permission from ref. 89 American Chemical Society]. (B) The relationship between the PL intensity of CuInS2 QDs and the concentration of Cd2+. Inset: the plot of [Cd2+]/I versus the concentration of Cd2+ [reprinted with permission from ref. 44 Royal Society of Chemistry]. |
Fig. 12 PL spectra of AgInZnS QDs with increased concentrations of Cd2+; inset shows images of AgInZnS QDs without (left) and with 290 μM Cd2+ under UV light irradiation [reprinted with permission from ref. 92 copyright 2021 Elsevier]. |
Fig. 13 (a) PL spectra of Zn–Ag–In–S QDs without and with Cd2+ of different concentrations added (from 25 μM to 2 mM). (b) TEM image of ZAIS QDs. Inset: HRTEM image of the sample (top); size distribution histogram of QDs (bottom). (c) TEM image of ZAIS QDs after adding Cd2+ of 2 mM. (d) Illustration of possible mechanism of Cd2+-triggered AIEE of ZAIS QDs [reprinted with permission from ref. 93 Royal Society of Chemistry]. |
QDs | Analyte | Detection scheme | Detection mechanism | Detection range | LOD | Reference | Sample type |
---|---|---|---|---|---|---|---|
MPA-capped CuInS2 | Cu2+ | PL quenching | Electron transfer | 0.2–10 μM | 0.10 μM | 44 | Tap and pound water |
Cd2+ modified MPA-capped CuInS2 | Cu2+ | PL quenching | Electron transfer | 0.1–10 μM | 0.037 μM | ||
MPA-capped CuInS2 | Cd2+ | PL enhancement | Surface passivation | 0.8–7.2 μM | 0.19 μM | ||
DTAB-capped AgInZnS | Cu2+ | PL quenching | Electron transfer | 0.05–10 μM | 15 nM | 101 | — |
SDS-capped AgInZnS | Cu2+ | PL quenching | Electron transfer | 0–340 μM | 27.3 nM | 102 | — |
AgInZnS-GO | Cu2+ | PL quenching | Binding with ligands | 0–850 μM | 0.18 nM | 97 | — |
Optical fiber SDS capped AgInZnS | Cu2+ | PL quenching | Electron transfer | 2.45–800 nM | 2.45 nM | 103 | Lake water |
GSH-capped CuInZnS/ZnS | Cu2+ | PL quenching | Cation-exchange | 0.02–20 μM | 6.7 nM | 43 | River water |
GSH-capped AgInZnS | Cu2+ | PL quenching | Cation-exchange | 0–35 μM | 100 nM | 91 | — |
AgInZnS | Cu2+ | PL quenching | Cation-exchange | Not mentioned | Not mentioned | 89 | — |
AgInZnS | Hg2+ | PL quenching | Cation-exchange | Not mentioned | Not mentioned | ||
AgInZnS | Cd2+ | PL enhancement | Surface passivation | Not mentioned | Not mentioned | ||
AgInZnS | Cr6+ | PL quenching | Cation-exchange | Not mentioned | Not mentioned | ||
GSH-capped AgInS2/ZnS | Cu2+ | PL quenching | Cation-exchange | Not mentioned | Not mentioned | 42 | — |
TGA-capped CuInS2/ZnS | Co2+ | PL quenching | Inner filter effect | 0.3012–90.36 μM | 0.16 μM | 90 | — |
MSA capped AgInS2 | Pb2+ | PL quenching | Not mentioned | 0–90 nM | 16.44 nM | 57 | — |
GSH AgInS2–ZnS | Cr3+ | PL quenching | Binding with ligands | 0.025–10 μM | 0.51 nM | 100 | — |
MPA AgInZnS | Cd2+ | PL enhancement | Surface passivation | 0.1–290 μM | 37.8 nM | 92 | Lake water |
L-Cysteine Zn–Ag–In–S | Cd2+ | PL enhancement | AIEE | 25 μM to 2 mM | 1.56 μM | 93 | Tap and lake water |
Zinc doped AgInS2 (AgInZnS) QDs synthesized via an emulsion solvent route with DTAB as amphiphilic ligand were reported by Liu et al.107 XPS analysis confirmed the formation of the QDs by identifying the valences of Ag, In, Zn, and S to be 1+, 3+, 2+, and 2−. However, Cu (2p) peak corresponding to Cu+ was also identified when the QDs were exposed to Cu2+ ions. This confirmed the electron-induced PL quenching resulting in the reduction of Cu2+ to Cu+. A detection range of 0.05–10 μM and LOD of 15 nM were achieved. The probe displayed a rapid response time of one minute and a sequence of QDs, Tris–HCl buffer, and Cu2+ ions yielded the best results. No further quenching occurred at a concentration higher than 10 μM indicating saturated surface traps. Other metal ions had no significant influence on the PL intensity but Fe3+ interference was eliminated by adding FeF63−.107
Liu et al.108 displayed a wider detection range of 0–340 μM with SDS capped AgInZnS QDs at longer response times of 10 minutes. The importance of the probe concentration was stressed since a high concentration might allow little analyte to interact compromising sensitivity while a low concentration would offer limited sites to adsorb. As a result, an optimum concentration of 0.5 mg mL−1 was established. The reported zeta potential value of −36.8 mV suggested an electrostatic interaction between the QD and Cu2+ existed, aiding the electron transfer from QDs to Cu2+ ions. Additionally, the use of different Cu2+ ion sources (i.e. CuCl2, CuN03) did not affect the PL intensity at the same concentration (340 μM).108
A wider detection range of 0–850 μM was achieved with AgInZnS–graphene oxide nanocomposite with a response time of one minute.99 The AgInZnS–GO–Cu2+ interaction triggered particle size increase due to the R–COO–Cu2+–COOR complex formation, which quenched the PL of the NC. This result was seen in the obvious red-shifted emission after the addition of Cu2+, while also confirmed by TEM images illustrating a size of 5.7 nm and 21.7 nm before and after the addition of Cu2+ ions respectively. The NC revealed weak binding interactions with other metal ions because only slight changes in PL intensity were seen.99
The detection of Cu2+ at the nanomolar range was later reported by Liu et al.,109 using a fluorometric optical fiber nanoprobe based on SDS-capped AgInZnS QDs. A detection range of 2.45–800 nM and LOD of 2.45 nM were reported. Electron transfer was put forward as a possible mechanism. PL lifetime studies supported the possibility where average lifetimes decreased from 500 ns to 325 ns for QDs in the presence and absence of Cu2+ respectively. Furthermore, the detection could be carried out in the presence of Fe3+ by adding FeF63−. Applications in real water samples produced recoveries between 95.7–100.5%.109
A few authors revealed GSH capped QD based fluorescent probes towards the detection of Cu2+ ions through cation exchange mechanism.42,43,91 CuInZnS/ZnS core/shell QDs synthesized with a 1/1 Cu/Zn mole ratio exhibited an emission peak at 607 nm. The emission intensity decreased while red-shifted emission from 607 nm to 646 nm was observed with increased Cu2+ ion concentration. The probe claimed detection between 0.02–20 μM with an LOD of 6.7 nM. Other metal ions (of the same concentration as Cu2+) had no significant change upon their addition and no emission shifts were observed. GSH offers a variety of functional groups on the surface that helps resist pH variation and maintain QD stability. As a result, the probe responded to wide pH ranges (6–10). The strategy was applied in real water samples. Recoveries between 98.07–102.4% were achieved, which were comparable to ICP-AES results of the same sample.43 AgInZnS QDs were quenched with slight red-shifted emission when exposed to Cu2+ ions. The QDs displayed a good linear relationship between quenching efficiency and Cu2+ ion concentration, thus a detection range and LOD of 0–35 μM and 100 nM were established respectively.91 In another development, AgInS2/ZnS core/shell QDs experienced the replacement of Zn2+ with Cu2+ forming a CuS layer on the QD surface. This detection scheme was supported by the gradual quenching and red-shifted emission between 0.1–10 μM.42
AgInZnS NPs synthesized with different metal mole ratios (1 = no Zn, 2 = low Zn, 3 = high Zn) were applied to Cu2+ detection.89 A direct interaction was assumed between the QDs and Cu2+ resulting to a significant quenching and red-shifted emission with the NP at Zn concentrations as low as 500 nM. The results suggested a cation-exchange mechanism between the Zn and In in the NP and Cu2+ ions.89
In the case of Hg2+ ions, a significant reduction in the PL intensity of AgInZnS NPs with low Zn (NP2) was seen at 500 nM, which was the opposite of NPs with high (NP3) and no Zn (NP1). This means greater interaction occurred between NP2 and Hg than the other two NPs. On the other hand, NP1 showed complete quenching when exposed to 500 nM dichromate and little quenching with chromate at the same concentration, suggesting that ion size or overall charge may influence selectivity.89
In another development, GSH capped AgInS2/ZnS QDs displayed PL quenching and red-shifted emission when exposed to increased concentrations of Cr3+, which was attributed to Cr3+–GSH complex formation on the QD surface resulting in aggregation.100 A linear relationship between quenching efficiency and Cr3+ concentration was seen between 0.025 μM and 10 μM with a LOD of 0.51 nM. The effect of different metal cations across the periodic table towards the PL response of the QDs was investigated. The studies revealed almost 85% of PL quenching of the QDs and lower degree of quenching for Pb2+, Cu2+, Ni2+ and Hg2+, while other metal ions exhibited negligible effect on the PL intensity of the QDs. Cr3+ ions were selectively detected by adding Na2S to mask the interfering metal ions (i.e. Pb2+, Cu2+, Ni2+ and Hg2+) which have a greater affinity to sulfides. Results showed that the addition of the Na2S prevented the PL quenching of the QDs in the presence of the interfering metal ions, leaving the quenching due to Cr3+ unaffected. In addition, Cr3+ were selectively detected by the QDs among a mixture of the interfering metal ions.100
The interaction of Co2+ ions with TGA capped CuInS2/ZnS QDs resulted in the formation of a TGA–Co2+–TGA due to the detachment of the TGA molecule on the QDs, leading to quenching of QDs.100 The quenching was partly attributed to IFE. A good linear relationship between quenching efficiency and Co2+ concentration was seen between the range of 0.3012–90.36 μM with an LOD of 0.16 μM.100 Furthermore, mercaptosuccinic acid (MSA) capped AgInS2 core QDs showed potential in the detection of Pb2+ ions. The addition of Cd2+, Zn2+, K+, and Mn2+ at increased concentrations had little effect on PL intensity of QDs but Pb2+ produced a gradual decrease at the same concentrations. A good linear relationship between PL efficiency and Pb2+ ion concentration was seen between 0 – 90 nM with a detection limit of 16.44 nM.57
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