Sulfur-doped carbon dots synthesis under microwave irradiation as turn-off fluorescent sensor for Cr(III)

Abstract

This study synthesized a facile and high sensitive fluorescent probe based on sulfur-doped carbon dots (S-CDs) using a one-step microwave irradiation method. The probe exhibited a strong blue emission and a high quantum yield (QY) of 36.40%. In the detection, the presence of trivalent chromium (Cr(III)) strongly quenched the PL intensity of S-CDs by the inner filter effect (IFE) quenching mechanism of Cr(III) on the S-CDs. The S-CDs exhibited good sensitivity to turn-off Cr(III) detection with a linear range concentration of 0–45 μM and a detection limit of 0.17 μM. Furthermore, the proposed method has been successfully applied for Cr(III) detection in natural water samples with the 93.68–106.20% recoveries.

Introduction

Carbon dots (CDs) are carbon-based nanoparticles that have unique photoluminescent properties such as high photostability (Zhi et al. 2018), good solubility in water, easily modified with specific functional groups for various field applications (Karakoti et al. 2015; Farshbaf et al. 2018). In addition, CDs provide superior prospects both in cost-effectiveness and environmental friendliness (Pudza et al. 2020). Currently, carbon dots applications have tremendous concerns, e.g., metal sensing (Chahal et al. 2020; Khan et al. 2017; Zhang et al. 2016), tunable photoluminescence (Zheng et al. 2020), biosensor (Madrakian et al. 2017; Zhang and Guo 2021), bioimaging (Zan et al. 2018), bio-labeling (Liu et al. 2019), biomedicine (Shaikh et al. 2018), photocatalytic energy conversion (Fernando et al. 2015), and as nanocarriers for gene delivery (Zuo et al. 2015). In metal sensing, carbon dots can detect metal by quenching or turning it off. This causes a decrease in the intensity of PL carbon dots on the addition of metal (Khan et al. 2017).

The method for synthesizing carbon dots is generally divided into top-down and bottom-up (Zuo et al. 2015). Synthesis of carbon dots by breaking down large particles into nanoparticle-sized particles is called the top-down method, like oxidation (Misra et al. 2018; Tan et al. 2019), electrochemical (Ahirwar et al. 2017), laser ablation (Thongpool et al. 2012; Kang et al. 2020). In contrast, the bottom-up method is a method of arranging atoms or molecules to form the desired nanometer-sized particles like hydrothermal (Chahal et al. 2020), solvothermal (Zheng et al. 2020), pyrolysis (Li et al. 2020), microwave, and sonochemical assisted (Ashritha et al. 2021). The microwave method is a common bottom-up method for synthetic CDs due to being simple, fast, cost-efficient, and environmentally friendly (Ang et al. 2020). This method works by vibrating the carbon chain to undergo rearrangement (Guan et al. 2020).

This work synthesized carbon dots from succinic acid and sodium thiosulfate using a one-step microwave irradiation method. Succinic acid and sodium thiosulfates are biocompatible carbon and oxygen-rich building blocks in chemical synthesis (Prathumsuwan et al. 2018). Succinic acid comprises mainly the carboxylic functionalize group and can be produced from Actinobacillus succinogenes through Broth fermentation (Lin et al. 2010). Meanwhile, Sulfur (S) is often used to improve the properties of optical carbon dots because of the similar electronegativity with carbon but a larger atomic radius than a carbon atom. Six valence electrons in each S atom can modify the electronic structure of CDs. Under certain conditions, zero-length bonds can be formed between the CDs and the target biomolecules from the disulfide covalent bonds (Karakoti et al. 2015). Therefore, the presence of S together with carboxylic acid functionality made S-CDs negatively charged and bright blue luminescent (Ding et al. 2020). The purpose of this study is to identify whether the naturally present functional groups in succinic acid’s precursor and S will impact the optical properties of CDs and their sensing applications for presenting Cr(III) in water.

In surface water, the ratio of Cr(III) to hexavalent chromium varies widely. Generally, Cr(III) is a positive ion that forms hydroxides and complexes. Approximately 25% of Cr(III) of the available daily intake (2–8 g) is absorbed for metabolism, but Cr(III) compounds are cytotoxic. They might cause chromosomal damage in enormous amounts (Tumolo et al. 2020). Thus, selective and sensitive determination of chromium is important. Several methods have been used to detect Cr(III) in water, such as inductively coupled plasma atomic emission spectrometry (ICP-AES) (Liang et al. 2003), flame atomic absorption spectrometry (EAAS) (Sperling et al. 1992), X-ray fluorescence spectrometry (Inui et al. 2011) and electrochemical methods (Prabhakaran et al. 2020). However, several of these methods requires expensive costs and a complex procedure because the sample must be pre-treated, so that it takes a long time and is less efficient if applied. In addition, the method of using a colorimetric method based on nanoparticles has also been developed for a long time. One example is the synthesis of gold nanoparticles functionalized with mercaptobenzoic acid (Zhang et al. 2020). However, this nanoparticle is a bit tough to synthesize, so that a better method is needed.

Therefore, the synthesis of S-CDs from succinic acid as a precursor and sodium thiosulfate as an S source is an excellent alternative method for detecting Cr(III). Cr(III) is considered as a quencher for the mechanism of S-CDs fluorescence via IFE. In IFE, the quencher absorption spectrum overlaps with the CDs’ excitation and/or emission (Lee et al. 2020; Tan et al. 2020; Panigrahi and Mishra 2019).

Methods

Materials

All chemicals were of analytical grade. Succinic acid (C₄H₆O₄), quinine hemisulfate salt monohydrate (C₄₀H₅₂N₄O₉S), lead(II) nitrate (Pb(NO₃)₂), rubidium chloride (RbCl), and cesium chloride (CsCl) were obtained from Sigma-Aldrich (USA). Chromium(III) nitrate nonahydrate (Cr(NO₃)₃·9H₂O) was purchased from Alfa Aesar (USA). Nickel(II) nitrate hexahydrate (Ni(NO₃)₂·6H₂O) and magnesium nitrate hexahydrate (Mg(NO₃)₂·6H₂O) were procured from Showa (Japan). Sodium thiosulfate pentahydrate (Na₂S₂O₃·5H₂O) was purchased from Shimakyu’s pure chemicals (Japan) and copper(II) sulfate pentahydrate (CuSO₄·5H₂O) was purchased from Choneye pure chemicals. Sodium hydroxide (NaOH) was purchased from Honeywell Fluka (Germany). Iron(II) chloride tetrahydrate (FeCl₂·4H₂O) and other metals were purchased from Merck (USA). Ultrapure water was obtained from a Milli-Q Reference purification system (18.2 MΏ cm, 25 °C).

Synthesis of the S-CDs

The S-CDs were synthesized by microwave irradiation method according to previous reported method with small modification (Nemati et al. 2018a). Typically, succinic acid (0.5 g) and sodium thiosulfate (0.35 g) were dissolved with deionized water (15 mL) in crucible porcelain 50 mL. A domestic microwave irradiated the mixture solution at 700 W for 5.5 min. After irradiation, the resulting solid was dissolved in 10 mL for further centrifugation at 10,000 rpm for 30 min. This step is purposed to remove the insoluble material of S-CDs. The obtained supernatant was filtered by a micropore membrane filter (0.22 µm). Thus, the solution containing S-CDs was kept for further analysis. The synthesis of S-CDs and their application as turn-off sensor for Cr(III) is depicted in Fig. 1.

Fig. 1

S-CDs synthesis process for Cr(III) detection

Characterization of S-CDs

S-CDs morphology was performed by transmission electron microscopy (TEM) on a JEOL JEM-2010 with an accelerating voltage of 200 kV. The surface of S-CDs was characterized by attenuated total reflectance-Fourier transform infrared (ATR-FTIR) spectrometer (Perkin Elmer, USA). PHI Hybrid Quantera conducted X-ray photoelectron spectroscopy (XPS) measurement. Characterization of the nature of the material was conducted by x-ray diffraction (XRD). The PL spectra were observed by FP-750 Spectrofluorometer (Jasco, Japan). All measurements were performed in 10 mm quartz microcells, at room temperature. Ultraviolet–visible (UV–Vis) absorption spectra were obtained with Spectrophotometer Lambda 265 (Perkin Elmer, USA).

Measurement of quantum yield

The QY of synthesized S-CDs was measured by plotting the absorbance versus PL intensity of both S-CDs and quinine sulfate in 0.1 M H₂SO₄ (QY = 0.54) as reference. The excitation wavelength was conducted at 320 nm and the QY calculation refers to the QY equation (Xu et al. 2020) based on Eq. (1):

$${\text{QY}}_{{\text{s}}} = {\text{QY}}_{{\text{r}}} \frac{{I_{{\text{s}}} A_{{\text{r}}} \eta_{{\text{s}}}^{2} }}{{I_{{\text{r}}} A_{{\text{s}}} \eta_{{\text{r}}}^{2} }}$$

(1)

subscripts “s” and “r” stand for sulfur-doped carbon dots and reference quinine sulfate, respectively. “I” corresponds to the integrated PL intensity, “A” corresponds to the absorbance measured at the excited wavelength and “η” refers to the solvent refractive index.

Sensitivity and selectivity of Cr(III)

To evaluate the range detection of S-CDs towards Cr(III), the series of Cr(III) concentration were mixed with 10 µL S-CDs solution (0.02 mg/mL), respectively. Then, the mixture solution was diluted to 3 mL with deionized water. The solution was mixed thoroughly and kept at room temperature for 5 min. Afterward, the PL intensity was measured at excitation wavelength 320 nm and emission wavelength 407 nm. To describe the PL quenching profile of S-CDs with Cr(III) presence, the plot of I₀/I versus C was performed according to the Stern–Volmer equation (Ghanem et al. 2020) based on Eq. (2):

$$\frac{{I_{0} }}{I} = 1 + K_{{{\text{SV}}}} \left[ C \right]$$

(2)

where I₀ refers to the initial PL intensity, I represents the PL intensity with the presence of Cr(III), K_SV denotes the Stern–Volmer quenching constant, and C refers to the added concentration of metal ions.

To assess selectivity, different kinds of metal ions, e.g. Cr(III), Cs(I), K(I), Li(I), Mn(II), Na(I), Rb(I), Hg(II), Se(IV), Ni(II), Pb(II) and Fe(III) were tested with the S-CDs. 10 μL S-CDs (0.02 mg/mL) and 60 μL of metal ion (0.01 M) was transferred to vial, respectively. Then, the mixture solution was diluted to 3 mL with deionized water. The solution was mixed thoroughly and left to react at room temperature for 5 min, and then recorded the associated PL intensity. To validate the feasibility of S-CDs under environmental conditions, the S-CDs were applied in Taichung city in two different water samples (river water and tap water). A 0.22 µm syringe filter filtered the water sample to reduce the insoluble materials and each sample (1 mL) was spiked with a known concentration of Cr(III) and S-CDs 10 µL (0.02 mg/mL).

Result and discussions

Optimization of S-CDs synthesis

The synthesis of S-CDs was conducted by a microwave irradiation method using succinic acid as precursor and sodium thiosulfate as sulfur sources. The S-CDs synthesized has good solubility in water. A factorial design using three factors and two levels has been done to produce the S-CDs with the highest quantum yield and good optical properties. These factors are microwave power, time irradiation, and the amount of sodium thiosulfate, while succinic acid was 0.22 g for each experiment. The QY was determined by a plot of integrated PL intensity versus the absorbance of S-CDs and quinine sulfate (Additional file 2: Fig. S1). Quinine sulfate was used as fluorescent standard due to similar PL excitation and emission wavelength with the S-CDs synthesized. Thus, the highest QY for S-CDs was obtained 36.40% at the microwave power 700 W, the time irradiation 5.5 min and the amount of sodium thiosulfate 0.35 g (Additional file 1: Table S1). The microwave irradiation method provides an effective, efficient, and convenient method for synthesizing S-CDs. The microwave method could increase the particle size uniformity of carbon dots (Lin et al. 2019). Particle size could be attributed to the change rate of non-radiative radiation and relaxation mechanisms. Wherein an increase in particle size causes a decrease in quantum efficiency (Dijken et al. 2001). In addition, adding S as surface passivation can increase the QY due to its catalytic ability on the surface of S-CDs (Lin et al. 2019).

S-CDs characterization

TEM image of synthesized S-CDs is displayed in Fig. 2a. The result showed that S-CDs were spherical in shape and distributed within the range of 1.5–5.0 nm (Fig. 2b). The XRD spectra indicated the degree of crystallinity of the S-CDs synthesized showed sharp peaks around 25.47°–28.06°. These peaks correspond to graphite’s (002) plan (Nemati et al. 2018a; Wang et al. 2019; Pakhira et al. 2016). The other sharp peak appeared at 13.93° and broad peaks appeared at 18.12° and 23.56°, which indicated highly disorder carbon atoms and confirmed the amorphous nature of carbon dots (Du et al. 2014; Bian et al. 2018). Thus, the synthesized S-CDs contained a structure of carbon, both crystalline and amorphous phases.

Fig. 2

a TEM image of S-CDs. b diameter distribution of particle. c FTIR spectrum of the S-CDs. d XPS spectrum of S-CDs

The FTIR spectra (Fig. 2c) presented the surface functionalities of S-CDs corresponding to succinic acid. Both the S-CDs and succinic acid were similar functional peaks, except the absorption peak at 665 cm⁻¹ in the S-CDs demonstrated C–S/C–S–C bending (Ouyang et al. 2019; Nemati et al. 2018a; Gupta and Nandi 2017). In addition, the peaks at 1122 cm⁻¹ and 1051 cm⁻¹ could be described as C–S and present of SO₃, respectively (Sun et al. 2016; Ding et al. 2014). Meanwhile, the peaks at 3430 cm⁻¹ and 2933 cm⁻¹ attributed to the broad absorption of O–H and C–H stretching vibration, respectively (Başoğlu et al. 2020; Lin et al. 2019). The peak of C=O representing carboxylic acid, and the C–O stretching vibration was indicated at 1692 cm⁻¹ at 1309 cm⁻¹ (Chandra et al. 2013). The peak at 1411 cm⁻¹ demonstrated C–O–H in-plane blending (Mitra et al. 2013). The FTIR spectra indicated that succinic precursors doped with S could be successfully prepared by microwave method.

The three peaks in the XPS spectrum characterized by C1s, O1s, and S2p, respectively, indicate that C, O, and S contained atomic percentage ratio of C:O:S = 62.3:36.2:1.5 in the S-CDs synthesis (Fig. 2d). The high-resolution of XPS spectra showed the C1s spectrum at 284.5 assigned to C–C/C=C and the subsequent peaks at 285.5, 286.3, and 288.3 eV (Additional file 3: Fig. S2a) assigned to C–OH (hydroxyl), C–S, and C=O (carboxyl), respectively (Nemati et al. 2018b; Chandra et al. 2013). The two peaks at 532.1 and 535.6 eV in the O1s spectrum assigned C = O/COOH groups and OH (Additional file 3: Fig S2b). According to Fig. S2c, there were two main peaks of the S2p spectrum centered at 163.7 and 168.8 eV. The first centered peaks at 163.2 and 164.3 eV could be associated with 2p3/2 and 2p1/2 of the –C–S– covalent bond due to their spin–orbit couplings (Ding et al. 2014; Nemati et al. 2018b). The next peak could be deconvoluted into three peaks at 167.6, 168.5, and 169.3 eV, refer to the –C–SOx– (x = 2, 3, 4) species (Ding et al. 2014; Gupta and Nandi 2017). Therefore, The FTIR and XPS approved the presence of C–C/C = C, C = O, –OH, –COOH, C–S, and C-SOx surface functional group in the S-CDs synthesis.

Optical properties

The optical properties of S-CDs were conducted by UV–Vis and fluorescence techniques. As shown in Fig. 3a, there were two unique absorption peaks of the S-CDs spectrum. The peak at 255 nm corresponded to π–π* transition of C=C, and the peak 320 nm corresponded to n → π* transition of C=O (Ouyang et al. 2019; Nemati et al. 2018c; Başoğlu et al. 2020). Under a 365 UV lamp, the S-CDs solution emitted a blue color (Fig. 3a inset). Figure 3b shows the photoluminescence (PL) emission spectra of S-CDs dependent on the excitation wavelength. There were two regions of fluorescence emitted according to fluorescence excitation. When the fluorescence excited from 300 to 340, the fluorescence emission displayed a red shift from 405 to 414 nm. Meanwhile, the fluorescence emission demonstrated a red shift from 446 to 504 nm when the fluorescence excitation was 350–480. Then, the fluorescence emission-dependent excitation wavelength resulted in the highest emission at 407 nm upon excitation by 320, giving rise to a blue emission. This color is due to the S doping of the CDs (Ding et al. 2014). Otherwise, the lowest emission at 504 nm upon excitation by wavelength 480 nm. Furthermore, there is no fluorescence emitted at fluorescence excited more than 480 nm.

Fig. 3

a UV–Vis absorption corresponding to emission at 407 nm and excitation at 320 nm (inset: photographs of S-CDs under UV light and daylight). b PL emission spectra of S-CDs dependent excitation wavelengths

The changing of emission wavelengths at different excitation wavelengths was related to functional groups on the surface, and the various sizes of S-CD particles (Lin et al. 2019; Jayaweera et al. 2019). The S is the one that has a strong electron affinity, which causes the increase in electron density in the intrinsic state of the S-CDs (Kang et al. 2020). The surface functional group of the S-CDs will act as an emission trap. The electronic structure of the carbon dots might be modulated by S through inputting the S energy levels between π and π* of carbon to produce multi-emission peaks (Feng et al. 2018). In addition, different functional groups provide different energy levels. It was possible due to the ability of each functional group to supply electrons to the CDs. On the other hand, the change in S-CD particle size resulted in a localized state associated with discrete sp² at the Lowest Unoccupied Molecular Orbital (LUMO) and Highest Occupied Molecular Orbital (HOMO) levels (Ouyang et al. 2019; Kang et al. 2020). When the particles get smaller, there was a larger energy gap between the 2 levels, which caused the electrons in the HOMO to need more a lot of energy to get excited into the LUMO. The electronic transitions in these localized states were responsible for the redshift of the fluorescence emission wavelength (Ouyang et al. 2019; Feng et al. 2018).

Photostability of the S-CDs

Four critical factors were observed to evaluate the stability of the S-CDs. These were: the effect of various ionic strength concentrations, different temperatures, different time exposure to ultraviolet light (under UV light 365 nm), and the effect of various pH. The effect of ionic strength on PL intensity was studied with a range concentration of NaCl solution from 0 to 200 mM. The PL intensity was stable even at high NaCl concentration (Additional file 4: Fig. S3a), which indicated the high colloid stability possessed by S-CDs against the attractive forces of the particles (Jayaweera et al. 2019; Nemati et al. 2018c). This showed that the PL intensity was independent of ionic strength. Under environmental conditions, the PL intensity remained unchanged because the primary mechanism was not disturbed by the presence of ions. In contrast, increasing temperatures resulted in a decrease in PL intensity (Additional file 4: Fig. S3b). Increased temperature indicates diminishing fluorescence caused by non-radiant heat, leading to reduced radiation emissions.

To ensure photostability of S-CDs was conducted by continuous UV irradiation using UV light 365 nm for 120 min. Additional file 4: Fig. S3c demonstrated a decrease in PL intensity after 60 min and 120 min of exposure by 14% and 21%, respectively. In traditional fluorescent dyes such as Rhodamine 6G, the reduction in PL intensity after 120 min of continuous exposure was almost 54% (Madjene et al. 2021). This shows that the S-CDs were more resistant to photobleaching. Furthermore, to determine the effect of pH on PL intensity, it was carried out in the pH value from 1 to 12. The most vigorous PL intensity occurred at pH 3 (Additional file 4: Fig. S3d). An increase in pH value resulted in a decrease in PL intensity, but an increase in PL intensity returned to pH 6. A similar pattern occurred in the pH between 6 and 10. The pH-dependent PL intensity was related to the protonation/deprotonation of the carboxyl (–COOH) and hydroxyl groups (–OH) on the S-CD surface (Huang et al. 2015). Therefore, the unique PL intensity characteristics as a function of pH provided a good direction for determining metal ions, especially in acidic environments (Issa et al. 2020).

Sensitivity and selectivity of S-CDs towards Cr(III)

The fluorescence quenching refers to Stern–Volmer, which is expressed by Eq. 2. While the limit of detection was calculated using 3δ/m, where the standard deviation of the blank signal was denoted by δ and m refers to the slope of the linear correlation. As shown in Fig. 4a, the S-CDs’ PL intensity demonstrated a significant decrease with the increasing concentration of Cr(III) from 0 to 200 µM compared to the other metal ions. A good linear correlation (R², 0.995) was showed between quenching efficiency I₀/I and concentration Cr(III) in a range of 0–45 µM (Fig. 4b), and the limit of detection (LOD) was calculated to be 0.17 µM.

Fig. 4

a Changes in PL emission spectra of S-CDs with different concentrations of Cr(III) and b The Stern–Volmer curve, insert: linear curve in the Cr(III) concentration range of 0–45 µM

Several metal ions were prepared to evaluate the selectivity of S-CDs towards Cr(III). These ions included Cr(III), Na(I), Li(I), Cs(I), K(I), Mn(II), Rb(I), Hg(II), Se(IV), Ni(II), Pb(II) and Fe(III) with a concentration of 200 µM for each ion and they were tested with 10 µl S-CDs solution (0.02 mg/mL). Figure 5 shows the PL intensity was quenched by the presence of Cr(III), about 95% of the initial PL intensity of S-CDs. These results confirmed that the S-CDs have high selectivity towards Cr(III) compared to other metals.

Fig. 5

The quenching of S-CDs when added different metal ions

Table 1 shows the comparison between the feasibility of Cr(III) detection in this study and other related results, including linear detection range and LOD.

Table 1 Comparison of different sensing methods for detection of Cr(III)

Possible mechanism of Cr(III) detection

To evaluate the quenching mechanism by Cr(III), the absorbance spectra of the presence of Cr(III) with S-CDs were matched with PL excitation spectra and PL emission spectra from S-CDs (Fig. 6a). There was a good spectral overlap in the excitation and emission of S-CDs with the absorption spectrum of Cr(III). This phenomenon could occur through the IFE process due to the overlap of the quencher absorption spectrum with excitation called the primary inner-filter effect and/or the emission of CDs called the secondary inner-filter effect (Lee et al. 2020; Tan et al. 2020; Panigrahi and Mishra 2019). Thus, IFE involved primary and secondary quenching mechanisms on the S-CDs surface in the presence of Cr(III). IFE was considered the quenching fluorescence mechanism rather than the fluorescence resonant energy transfer process due to the excellent overlap between the quencher absorption spectrum and CDs’ excitation and emission spectra (Zhao et al. 2018; Al-Hashimi et al. 2020). The PL intensity of S-CDs was reduced by adding Cr(III) to the S-CDs solution. In this phenomenon, Cr(III) would absorb the emission light of S-CDs, but the excitation light would be constant since the addition of Cr(III) into the S-CDs solution. Therefore, the emission PL intensity of S-CDSs would be a turn-off (Shahbazi and Zare-Dorabei 2019; Mousavi et al. 2020). Figure 6b shows no difference in absorption spectrum S-CDs both in absence Cr(III) and presence Cr(III). This confirmed the impossibility of forming the ground-state complex between S-CDs and Cr(III).

Fig. 6

a UV–Vis absorption spectra of S-CDs with the presence of Cr(III) versus excitation and emission spectra of S-CDs. b UV–Vis absorption spectra for Cr(III), S-CDs, and S-CDs with Cr(III)

Based on energy perspective, the band gaps values between S-CDs and S-CDs with Cr(III) were calculated using the Tauc plot equation (Aziz et al. 2019) as formulated in Eq. 3:

$$(\alpha h\upsilon ) = k(h\upsilon - E_{{\text{g}}} )^{\gamma }$$

(3)

where hʋ is the photon energy, α is coefficient of absorption, E_g is the band gap, ƴ is the index for the responsible electronic transition (αhʋ)² indicated a direct allowed electron transition of ½), and k is the parameter dependent on the inter-band transition. As shown by Additional file 5: Fig. S4a and S4b, Cr(III) in S-CDs indicated a reduction in band gap energy. S-CDs’ absorption causes the absorption edge to shift in the direction of low photon energy (Aziz et al. 2019). In addition, the lower band gap was related to the charge of metal ions on the surface of CDs (Murugan et al. 2019).

Application of S-CDs on water samples for Cr(III) detection

Experiments in two water sources were carried out to investigate the visibility of S-CDs for Cr (III) detection. Three known concentrations of Cr(III) were respectively introduced to the water sample. The results showed an increase in the concentration of Cr(III) quenched on the PL intensity of each water sample. As shown in Table 2, the percentage of water sample recovery is in the range of 93.68–106.20, while the relative standard deviation (RSD) ranges from 0.20 to 0.74. These results support that S-CDs have the feasibility of being applied as a sensor to detect Cr(III) in water in actual environmental conditions.

Table 2 Cr(III) detection in water samples (n = 3)

Conclusion

In summary, we have developed the water-soluble S-CDs fluorescent sensor to detect Cr(III) in water samples. A microwave irradiation method was adopted to prepare S-CDs using succinic acid as a precursor, and sodium thiosulfate as a source of S. The PL intensity of S-CDs was effectively quenched by the presence of Cr(III) due to the IFE of Cr(III) on S-CDs. Therefore, the proposed method was successfully used to detect Cr(III) in actual water samples, which can be considered for analyzing Cr(III) in other samples. Our present work provides the advantage of simplicity, saving time, low cost, and selectivity.