One-Pot Synthesis and Characterization of CuCrS2/ZnS Core/Shell Quantum Dots as New Blue-Emitting Sources

In this paper, we introduce a new blue-emitting material, CuCrS2/ZnS QDs (CCS QDs). To obtain bright and stable photoluminescent probes, we prepared a core/shell structure; the synthesis was conducted in a one-pot system, using 1-dodecanethiol as a sulfur source and co-ligand. The CCS QDs exhibited a semi-spherical colloidal nanocrystalline shape with an average diameter of 9.0 nm and ZnS shell thickness of 1.6 nm. A maximum photoluminescence emission peak (PL max) was observed at 465 nm with an excitation wavelength of 400 nm and PLQY was 5% at an initial [Cr3+]/[Cu+] molar ratio of one in the core synthesis. With an off-stoichiometric modification for band gap engineering, the CCS QDs exhibited slightly blue-shifted PL emission spectra and PLQY was 10% with an increase in initial molar ratio of 2.0 (462 nm PL max). However, when the initial molar ratio exceeded two, the CCS QDs exhibited a lower photoluminescence quantum yield of 4.5% with 461 nm of PL max at the initial molar ratio of four due to the formation of non-emissive Cr2S3 nanoflakes.


Introduction
Colloidal semiconductor nanocrystals, also called quantum dots (QDs), have been extensively investigated over the past three decades since the report on the synthesis of high-quality colloidal CdE (E = S, Se, and Te) in 1993 [1]. Due to the quantum confinement effect, the fluorescence wavelength of QDs can be tuned simply through the control of their size, shape, and composition. Although many studies have reported cadmium-based QDs due to their high quantum yield (QY) and full color tunability from blue to red [2], recently, Cd-free QDs are an emerging research area due to their inherent toxicity [3]. To apply the QDs to optoelectronic devices and biological area, the QDs should be less toxic and exhibit high performance such as high QY and stability.
Among QDs with various compositions, copper-based ternary QDs can be alternative sources for Cd-based QDs because they are less toxic and provide prominent optical properties. In particular, CuInS 2 (CIS) QDs have been extensively investigated under bio-labelling [4], bio-sensing [5][6][7], gas sensors [8], light-emitting diodes (LEDs) [9], and solar cells [10]. They exhibit a high QY with the introduction of ZnS shells for surface passivation as high as over 50-80%, and the emission color can be tuned from green to near-infrared by controlling the size and Cu/In ratio [11][12][13]. However, because CIS QDs cannot be applied for the blue emission region of display applications, other alternatives for blue-emissive QDs with high QY and stability need to be investigated.
Several studies have been published related to blue-emissive QDs synthesis and characterization. For instance, Lesnyak et al. reported a method of blue-emitting ZnSe 1-x Te x alloy nanocrystals in an aqueous condition with a maximum photoluminescence (PL) wavelength at 425 nm and PL quantum efficiency (PLQE) of 20% [14]. In addition, Gao et al. prepared bulk-like ZnSe QDs as blue LEDs with a maximum PL peak at 446 nm, and PL quantum yield (PLQY) of~100%, and external quantum efficiency (EQE) of 12.2% [15]. Additionally, Ji et al. fabricated strontium-doped CsPbCl 3 superlattices for ultra-stable violet-emissive perovskite QDs (PQDs) with high PLQY of 82.4% [16]. However, their work required a significantly complex preparation process, such as various state precursors (solid and gas states), or an extremely careful step-by-step protocol for uniform and high-quality colloidal QDs. Accordingly, for commercialization, a simpler and more economic method for synthesis should be developed [17].
CuCrS 2 is a Cu-based p-type semiconductor with optical band gap of approximately 2.48 eV. CuCrS 2 has been frequently investigated in the thermoelectric field [18]; however, it has not been synthesized at nanoscales or as QDs for fluorescent probes. In this study, we prepared new blue-emitting CuCrS 2 /ZnS (CCS) QDs through a simple one-pot heating method with 1-dodecanethiol as a sulfur precursor and co-ligand. For band gap engineering, we used the off-stoichiometric modification method by varying the molar ratio of [Cr 3+ ]/[Cu + ] to induce blue shifting of the PL emission peak.

Characterization
For the morphology characterization, a high-resolution transmission electron microscope (HR-TEM, Tecnai, FEI) was employed, with an accelerated voltage of 300 kV and resolution of 1.4 Å. To characterize the composition and crystal structure of synthesized QDs, a high-resolution X-ray photoelectron spectroscope (HR-XPS, Nexa, Thermofisher, Waltham, MA, USA) and high-resolution X-ray diffractometer (HR-XRD, Smartlab, Rigaku) with Al Kα X-ray and 3 kW Cu X-ray sources were employed, respectively. To characterize the optical properties of QDs, UV/Vis/NIR spectrophotometry (UV-Vis, V-770, Jasco) and spectrofluorometry (PL, Nanolog, Horiba) were utilized. In addition, fluorescence lifetime decay was measured with a time-resolved photoluminescence spectroscope (TRPL, Easylife, PTI).

Synthesis of CuCrS 2 /ZnS QDs in the One-Pot System
To synthesize CuCrS 2 cores with a [Cr 3+ ]/[Cu + ] molar ratio of 1.0, 20 mL of ODE, 5 mL of OAm (~10 mmol), 0.375 mmol of Cu(OAc), and 0.375 mmol Cr(NO 3 ) 3 ·9H 2 O were mixed in a 100 mL three-neck round-bottomed flask; then, the mixture was degassed at 120 • C for 10 min. After degassing, 5 mL of DDT (~20 mmol) was added to the solution, which was then heated to 230 • C. Thereafter, it was stored for 1 h to form monomers and proceed with nucleation. After core synthesis, the solution was cooled down to room temperature; for a simultaneous ZnS shelling process, 4 mmol of Zn(OAc) 2 ·H 2 O and 5 mL of OAm were added to the mixture and it was heated again to 120 • C for further degassing. Subsequently, 1 mL of DDT (~4 mmol) was injected, followed by heating up to 240 • C. After heating, the mixture was maintained at that temperature for 15 min for ZnS shelling onto the CuCrS 2 core. For the purification step of the synthesized QDs, a small amount of toluene was added into the flask to dissolve the prepared QDs, and they were centrifuged at 5000 rpm for 5 min to remove larger particles and undesirable side-products. After removing by-products, they were precipitated by introducing an excess amount of acetone and performing centrifugation. After the QDs were precipitated, they were washed using the precipitation and re-dispersion method. Briefly, they were re-dispersed into a small amount of toluene, followed by precipitation with the addition of an excess amount of ethyl acetate. Subsequently, they were centrifuged at 5000 rpm for 5 min. This process was conducted one more time. After QDs were washed, they were dried overnight at 60 • C in a pre-heated vacuum oven. To compare the composition effect to the band gap of the QDs, we conducted the same process with only a change in the molar ratio of  Figure 1 shows a schematic diagram of CCS QDs synthesis. TEM analysis was conducted to investigate their morphological structure and the particle size. As shown in Figure 2a,b, the pure CuCrS 2 nanocrystals and 1.0 CCS QDs exhibited an approximate spherical shape with mean diameters of 8.96 and 12.12 nm, respectively, and the ZnS shell thickness was confirmed to be approximately 1.6 nm by comparing the core and core/shell mean diameters. We clearly observed the lattice structure of the nanocrystals, showing that the 1.0 CCS QDs had high crystallinity ( Figure 2c).

Morphology and Crystal Structure of CuCrS2/ZnS QDs
CCS QDs were synthesized in an organic solvent via a simple heating process. Figure  1 shows a schematic diagram of CCS QDs synthesis. TEM analysis was conducted to investigate their morphological structure and the particle size. As shown in Figure 2a,b, the pure CuCrS2 nanocrystals and 1.0 CCS QDs exhibited an approximate spherical shape with mean diameters of 8.96 and 12.12 nm, respectively, and the ZnS shell thickness was confirmed to be approximately 1.6 nm by comparing the core and core/shell mean diameters. We clearly observed the lattice structure of the nanocrystals, showing that the 1.0 CCS QDs had high crystallinity ( Figure 2c).  In addition, to analyze the crystal structure of the CCS QDs, we employed thin film and powder XRD techniques ( Figure 2d). The XRD pattern of CuCrS 2 core showed weak and broad peaks at 33.13 • , 36.17 • , 49.46 • , and 51.89 • indicating the (102), (104), (108), and (110) phases of hexagonal CuCrS 2 , respectively [19]. The absence of a (101) phase at around 30 • was probably attributed to the partial release of Cu atoms at the washing step for XRD analysis. On the other hand, when the ZnS shell was coated onto the CuCrS 2 core (Figure 1d interpolation graph), the (101) phase was observed, and every peak shifted slightly toward the smaller 2θ because the lattice parameter (a = 5.345 Å) of ZnS with a zinc blended structure is larger than that (a = 3.483 Å) of CuCrS 2 [20]. To characterize the elemental composition and chemical oxidation state of the CCS QDs, we conducted XPS analysis for the pure CuCrS 2 core and 1.0 CCS QDs. In addition, to analyze the crystal structure of the CCS QDs, we employed thin film and powder XRD techniques (Figure 2d). The XRD pattern of CuCrS2 core showed weak and broad peaks at 33.13°, 36.17°, 49.46°, and 51.89° indicating the (102), (104), (108), and (110) phases of hexagonal CuCrS2, respectively [19]. The absence of a (101) phase a around 30° was probably attributed to the partial release of Cu atoms at the washing step for XRD analysis. On the other hand, when the ZnS shell was coated onto the CuCrS2 cor ( Figure 1d interpolation graph), the (101) phase was observed, and every peak shifted slightly toward the smaller 2θ because the lattice parameter (a = 5.345 Å) of ZnS with zinc blended structure is larger than that (a = 3.483 Å) of CuCrS2 [20]. To characterize th elemental composition and chemical oxidation state of the CCS QDs, we conducted XP analysis for the pure CuCrS2 core and 1.0 CCS QDs. Figure 3 shows the XPS results of the pure CuCrS2 core and 1.0 CCS QDs. As shown in Figure 3b, which depicts the result of the CCS QDs XPS survey analysis, the Zn 2p peak was clearly observed with the disappearance of Cu 2p and Cr 2p peaks, which indicated the successful ZnS shell coating onto the CuCrS2 core. The N 1s peak in Figure 2a resulted from unwashed OAm on the surface of the CuCrS2 core. For deeper evaluation, high-res olution XPS analysis was also conducted.    In addition, to analyze the crystal structure of the CCS QDs, we employed thin film and powder XRD techniques (Figure 2d). The XRD pattern of CuCrS2 core showed weak and broad peaks at 33.13°, 36.17°, 49.46°, and 51.89° indicating the (102), (104), (108), and (110) phases of hexagonal CuCrS2, respectively [19]. The absence of a (101) phase at around 30° was probably attributed to the partial release of Cu atoms at the washing step for XRD analysis. On the other hand, when the ZnS shell was coated onto the CuCrS2 core (Figure 1d interpolation graph), the (101) phase was observed, and every peak shifted slightly toward the smaller 2θ because the lattice parameter (a = 5.345 Å) of ZnS with a zinc blended structure is larger than that (a = 3.483 Å) of CuCrS2 [20]. To characterize the elemental composition and chemical oxidation state of the CCS QDs, we conducted XPS analysis for the pure CuCrS2 core and 1.0 CCS QDs. Figure 3 shows the XPS results of the pure CuCrS2 core and 1.0 CCS QDs. As shown in Figure 3b, which depicts the result of the CCS QDs XPS survey analysis, the Zn 2p peak was clearly observed with the disappearance of Cu 2p and Cr 2p peaks, which indicated the successful ZnS shell coating onto the CuCrS2 core. The N 1s peak in Figure 2a resulted from unwashed OAm on the surface of the CuCrS2 core. For deeper evaluation, high-resolution XPS analysis was also conducted.    [21] and Cr(III) 2p 3/2 and 2p 1/2 at 576.57 and 586.25 eV [22], respectively. In addition, the CuCrS 2 QDs core did not provide any unwanted state, such as Cu(II) or Cr(VI). Moreover, after the ZnS shell was formed, Zn 2p and S 2p spectra exhibited reasonably good spinorbital coupling, indicating successful ZnS shell coating onto the CuCrS 2 core. Interestingly, as shown in Figure 4c, some undesirable peaks appeared at 162.97 and 167.85 eV, indicating a S-S bond [23] and sulfate salt (SO 4 2− ) state [24], in S 2p of the CuCrS 2 core, respectively. The SO 4 2− salt peaks might be attributed to the oxidizing activity of nitrate salts in Cr(NO 3 ) 3 with DDT, as a sulfur source, which probably results in the formation of SO 4 2− in the CuCrS 2 core level [25]. As proof, when the ZnS shell was coated, undesired peaks did not appear in the S 2p survey, which indicated that no other states were formed when nitrate salt was not present in the ZnS shell coating.
QDs core did not provide any unwanted state, such as Cu(II) or Cr(VI). Moreover, after the ZnS shell was formed, Zn 2p and S 2p spectra exhibited reasonably good spin-orbital coupling, indicating successful ZnS shell coating onto the CuCrS2 core. Interestingly, as shown in Figure 4c, some undesirable peaks appeared at 162.97 and 167.85 eV, indicating a S-S bond [23] and sulfate salt (SO4 2− ) state [24], in S 2p of the CuCrS2 core, respectively. The SO4 2− salt peaks might be attributed to the oxidizing activity of nitrate salts in Cr(NO3)3 with DDT, as a sulfur source, which probably results in the formation of SO4 2− in the Cu-CrS2 core level [25]. As proof, when the ZnS shell was coated, undesired peaks did not appear in the S 2p survey, which indicated that no other states were formed when nitrate salt was not present in the ZnS shell coating.

Band Gap Engineering of CuCrS2/ZnS QDs
To prepare the true-blue-emissive probe, we conducted band gap engineering of CCS QDs using a simple stoichiometric modification method by varying the molar ratio of [Cr 3+ ]/[Cu + ]. Then, the results were analyzed with UV-Vis and PL spectrometers. It is well known that the band gap of CIS QDs is significantly affected by the stoichiometry of the metal ions because the valence band (VB) of QDs is related to the copper vacancy level [26]. When copper vacancy decreases (Cu-deficient state CIS QDs), the ground state of VB of QDs is lowered due to the decrease in the Cu vacancy level, causing the band gap to broaden or increase [27,28]. Therefore, we employed this strategy to prepare the true-blueemissive CCS QDs. Interestingly, the pure CuCrS2 exhibited a less-or non-emissive optical property after washing. Therefore, every subsequent experimental comparison was conducted through a ZnS shelling process with the same protocol. The optical band gap of prepared samples was calculated using the following Tauc plot equation with the direct transition method.
where E is the optical band gap of samples, α is an absorption coefficient of each sample, and hv is the photon energy. Then, relative PLQY was calculated using the Stern-Volmer equation:

Band Gap Engineering of CuCrS 2 /ZnS QDs
To prepare the true-blue-emissive probe, we conducted band gap engineering of CCS QDs using a simple stoichiometric modification method by varying the molar ratio of [Cr 3+ ]/[Cu + ]. Then, the results were analyzed with UV-Vis and PL spectrometers. It is well known that the band gap of CIS QDs is significantly affected by the stoichiometry of the metal ions because the valence band (VB) of QDs is related to the copper vacancy level [26]. When copper vacancy decreases (Cu-deficient state CIS QDs), the ground state of VB of QDs is lowered due to the decrease in the Cu vacancy level, causing the band gap to broaden or increase [27,28]. Therefore, we employed this strategy to prepare the trueblue-emissive CCS QDs. Interestingly, the pure CuCrS 2 exhibited a less-or non-emissive optical property after washing. Therefore, every subsequent experimental comparison was conducted through a ZnS shelling process with the same protocol. The optical band gap of prepared samples was calculated using the following Tauc plot equation with the direct transition method.
where E is the optical band gap of samples, α is an absorption coefficient of each sample, and hv is the photon energy. Then, relative PLQY was calculated using the Stern-Volmer equation: where Q is the quantum yield, I is the integration of PL emission spectrum, and A is the absorbance of materials. The subscript r and f refer to the reference material and sample, respectively.
To characterize the optical properties of the prepared CCS QDs, we conducted UV-Vis and PL measurements. As shown in Figure 5a, the optical band gap of the CCS QDs increased with the increase in the molar ratio of [Cr 3+ ]/[Cu + ] (2.61 eV for 1.0 CCS to 2.74 eV for 4.0 CCS). However, in the PL spectra (Figure 5b), a negligible blue shift in the maximum PL emission peak was observed, from 465 nm (1.0 CCS QDs) to 462 nm (2.0 CCS QDs) and 461 nm (4.0 CCS QDs). In Table 1, the optical properties of CCS QDs at different [Cr 3+ ]/[Cu + ] molar ratios are given. The 2.0 CCS QDs showed the highest PLQY, but further increase in molar ratio of [Cr 3+ ]/[Cu + ] caused a drastic decrease in the PLQY with a negligible blue shift. Fluorescence lifetime decay information is also presented in Table 1. The lifetime decay was fitted with a bi-exponential decay function (Figure 5c), and the decay times were obtained as 8.11 ns, 10.42 ns, and 8.2 ns for 1.0, 2.0, and 4.0 CCS QDs (Figure 5c), respectively. In addition, the photostability of CCS QDs were evaluated; it was found that CCS QDs showed good photostability under 365 nm light irradiation (Figure 5d), indicating that the core was well passivated by the ZnS shell.
absorbance of materials. The subscript r and f refer to the reference material and sample, respectively.
To characterize the optical properties of the prepared CCS QDs, we conducted UV-Vis and PL measurements. As shown in Figure 5a, the optical band gap of the CCS QDs increased with the increase in the molar ratio of [Cr 3+ ]/[Cu + ] (2.61 eV for 1.0 CCS to 2.74 eV for 4.0 CCS). However, in the PL spectra (Figure 5b), a negligible blue shift in the maximum PL emission peak was observed, from 465 nm (1.0 CCS QDs) to 462 nm (2.0 CCS QDs) and 461 nm (4.0 CCS QDs). In Table 1, the optical properties of CCS QDs at different [Cr 3+ ]/[Cu + ] molar ratios are given. The 2.0 CCS QDs showed the highest PLQY, but further increase in molar ratio of [Cr 3+ ]/[Cu + ] caused a drastic decrease in the PLQY with a negligible blue shift. Fluorescence lifetime decay information is also presented in Table 1. The lifetime decay was fitted with a bi-exponential decay function (Figure 5c), and the decay times were obtained as 8.11 ns, 10.42 ns, and 8.2 ns for 1.0, 2.0, and 4.0 CCS QDs (Figure  5c), respectively. In addition, the photostability of CCS QDs were evaluated; it was found that CCS QDs showed good photostability under 365 nm light irradiation (Figure 5d), indicating that the core was well passivated by the ZnS shell.   Figure 6 shows results of the TEM analysis of the 2.0 and 4.0 CuCrS2 core. As shown in Figure 6a,b, some flake-shaped nanocrystals were observed. CuCrS2 consists of a series of alternating S-Cr-S triple layers perpendicular to the hexagonal c-axis in addition to an interlayer of copper atoms. S atoms form a distorted cubic close packing, whereas Cr atoms occupy tetragonal sites between the layers [29]. When the CuCrS2 core is synthesized, if the Cr 3+ concentration is increased, c-axis-aligned Cr2S3 intermediates can be formed   Figure 6 shows results of the TEM analysis of the 2.0 and 4.0 CuCrS 2 core. As shown in Figure 6a,b, some flake-shaped nanocrystals were observed. CuCrS 2 consists of a series of alternating S-Cr-S triple layers perpendicular to the hexagonal c-axis in addition to an interlayer of copper atoms. S atoms form a distorted cubic close packing, whereas Cr atoms occupy tetragonal sites between the layers [29]. When the CuCrS 2 core is synthesized, if the Cr 3+ concentration is increased, c-axis-aligned Cr 2 S 3 intermediates can be formed more easily, and these intermediates might undergo crystal growth during the synthesis, exhibiting a nanoflake shape. Therefore, more Cr 3+ will cause unnecessary Cr 2 S 3 nanoflakes. Without a ZnS shelling process, the copper atoms might be easily removed when washing, resulting in less-or non-emissive nanocrystals. This could be observed after synthesis of the CuCrS 2 core without the ZnS shell. In this step, the unstable Cu atoms were washed out with the solvent and green precipitates were observed. Furthermore, CuCrS 2 nanocrystals with [Cr 3+ ]/[Cu + ] ratios of 2.0 and 4.0 were investigated using high-resolution XPS analysis to compare the impurity peak intensities, such as SO 4 2− in the CuCrS 2 QDs core level.
nanoflakes. Without a ZnS shelling process, the copper atoms might be easily removed when washing, resulting in less-or non-emissive nanocrystals. This could be observed after synthesis of the CuCrS2 core without the ZnS shell. In this step, the unstable Cu atoms were washed out with the solvent and green precipitates were observed. Furthermore, CuCrS2 nanocrystals with [Cr 3+ ]/[Cu + ] ratios of 2.0 and 4.0 were investigated using highresolution XPS analysis to compare the impurity peak intensities, such as SO4 2− in the Cu-CrS2 QDs core level.  Figure 7 shows the XPS results for CuCrS2 core nanocrystals at different [Cr 3+ ]/[Cu + ] molar ratios. The Cu(I) 2p and Cr(III) 2p XPS spectra exhibited no meaningful change with increases in Cr 3+ concentration (Figure 7d-g). The only difference was observed in the S 2p results. With increase in the Cr 3+ molar ratio, the unwanted peak intensity at approximately 163 eV was also stronger in the S 2p analysis (Figure 7a-c), indicating that the disulfide bond formation might be improved [30,31]. The S 2p spin-orbital couples (S 2p1/2 and S 2p3/2) showed good agreement with a peak area ratio of approximately 2.0, indicating a typical S 2p orbital state [32]. This phenomenon probably resulted from Cr2S3 crystal growth with stacking, forming the nanoflakes. The increased Cr 3+ concentration might accelerate the kinetics of Cr2S3 monomers, forming needless nanoflakes, as observed in the TEM analysis results ( Figure 6). Due to these factors, the CCS QDs with high Cr 3+ precursors exhibited a lower PLQY with a negligible blue shift.   (Figure 7d-g). The only difference was observed in the S 2p results. With increase in the Cr 3+ molar ratio, the unwanted peak intensity at approximately 163 eV was also stronger in the S 2p analysis (Figure 7a-c), indicating that the disulfide bond formation might be improved [30,31]. The S 2p spin-orbital couples (S 2p 1/2 and S 2p 3/2 ) showed good agreement with a peak area ratio of approximately 2.0, indicating a typical S 2p orbital state [32]. This phenomenon probably resulted from Cr 2 S 3 crystal growth with stacking, forming the nanoflakes. The increased Cr 3+ concentration might accelerate the kinetics of Cr 2 S 3 monomers, forming needless nanoflakes, as observed in the TEM analysis results ( Figure 6). Due to these factors, the CCS QDs with high Cr 3+ precursors exhibited a lower PLQY with a negligible blue shift.

Conclusion
We have introduced new blue-light-emissive CuCrS2/ZnS (CCS) quantum (QDs), which yielded a mean diameter of 12.1 nm with a ZnS shell with 1.6 nm thick The optical band gap and PLQY were confirmed to be 2.61 eV and 5% with 400/46 PLE/PL max at the initial molar ratio [Cr 3+ ]/[Cu + ] of 1.0, respectively. For obtaining blue-emissive QDs, the stoichiometric modification method was employed; it was f