Efficient and Stable Luminescence from Mn2+ in Core and Core-Isocrystalline Shell CsPbCl3 Perovskite Nanocrystals.

There has been a growing interest in applying CsPbX3 (X = Cl, Br, I) nanocrystals (NCs) for optoelectronic application. However, research on doping of this new class of promising NCs with optically active and/or magnetic transition metal ions is still limited. Here we report a facile room temperature method for Mn2+ doping into CsPbCl3 NCs. By addition of a small amount of concentrated HCl acid to a clear solution containing Mn2+, Cs+, and Pb2+ precursors, Mn2+-doped CsPbCl3 NCs with strong orange luminescence of Mn2+ at ∼600 nm are obtained. Mn2+-doped CsPbCl3 NCs show the characteristic cubic phase structure very similar to the undoped counterpart, indicating that the nucleation and growth mechanism are not significantly modified for the doping concentrations realized (0.1 at. % - 2.1 at. %). To enhance the Mn2+ emission intensity and to improve the stability of the doped NCs, isocrystalline shell growth was applied. Growth of an undoped CsPbCl3 shell greatly enhanced the emission intensity of Mn2+ and resulted in lengthening the radiative lifetime of the Mn2+ emission to 1.4 ms. The core-shell NCs also show superior thermal stability and no thermal degradation up to at least 110 °C, which is important in applications.

Introduction

Doping transition metals (i.e., Mn2+, Ni2+, Co2+) in nanoparticles has received significant research interest.[1−4] Fascinating new properties (e.g., optical and magnetic) can be introduced by intentional incorporating dopant ions into nanoparticles. Mn2+-doped II–VI (CdSe, CdS, ZnSe) quantum dots (QDs), as a representative, have been studied extensively in recent years.[5−7] The intense luminescence of Mn2+ combined with the large absorption cross section of QDs make these Mn2+-doped II–VI quantum dots promising for a wide range of applications.[8−11] For example, luminescent Mn2+-doped ZnSe QDs show emission that is detuned from the QDs’ absorption, making these highly luminescent QDs promising for application in solar cells.[11] In addition, another interesting aspect of Mn2+-doped QDs is their unique magneto-optical behavior resulting from interaction of photogenerated charge carriers in the QDs with the high magnetic moment of Mn2+ (3d5) ions.[12,13]

Recently, all-inorganic CsPbX3 (X = Cl, Br, I) perovskite nanocrystals have emerged as a very promising group of materials with nearly unity quantum yield in a broad spectral range covering the visible spectrum.[14−17] Particular attention is presently given to new synthesis routes for this group of materials aimed at a better control of their optical properties (emission color, efficiency) as well as the chemical and temperature stability.[18−21] A promising avenue to improve control over the optical properties is doping these NCs with luminescent ions, but so far studies on doping of lead halide perovskite NCs with optically active ions are limited. Two recent papers reveal the possibility of doping Mn2+ with CsPbCl3 NCs at elevated temperature (180 °C) via a hot-injection method.[22,23] Here, we report an alternative synthesis method allowing successful synthesis of Mn2+-doped CsPbCl3 NCs at room temperature. Creating a high chemical potential for Mn2+ in solution by mixing a reactive Mn2+ precursor with a Cs+ and Pb2+ precursor in toluene, followed by the addition of a small amount of HCl acid, results in Mn2+-doped CsPbCl3 NCs showing intense yellow/orange emission. A thermodynamically controlled doping mechanism is proposed to explain the doping process. In a next step, an undoped CsPbCl3 shell is grown which greatly enhances the luminescence quantum yield and stability of the doped CsPbCl3:Mn2+ NCs.

Experimental Section

Chemicals

All the chemicals were obtained from Sigma-Aldrich and used as received without further purification. The chemicals’ specifications are CsAc (cesium acetate, 99.9%), PbAc2·3H2O (lead acetate, 99.99%), MnAc2·4H2O (manganese acetate, 99.9%), and HCl acid (hydrochloric, 37 wt % in water).

Synthesis of Mn2+-Doped CsPbCl3 NCs

Equimolar amount of the acetates CsAc and PbAc2 with a variable amount of MnAc2 were stirred in 5 mL of toluene at room temperature (∼293 K) under N2 atmosphere. Oleic acid (OA) and oleylamine (OLAM) were chosen as ligands. A colorless clear solution was achieved after ∼15 min of stirring. Subsequently, the HCl acid in water was added under vigorous stirring. A white suspension formed, and the suspension was centrifuged at low speed (1500 rpm) to remove large particles, agglomerates, and acid residues (water). The larger particles precipitated at the bottom of the vial. The supernatant which contains the NCs was collected and stored at 0 °C for 15 min followed by centrifuging, now at a higher speed (3500 rpm) to precipitate the NCs. After removing the supernatant, the NCs were redissolved in 3 mL of toluene and centrifuged again at low temperature (0 °C). The supernatant was discarded and followed by addition of 1 mL of toluene, resulting in a stable colloidal dispersion of Mn2+-doped CsPbCl3 NCs.

In a typical synthesis, 0.1 mmol of CsAc, 0.1 mmol of PbAc2·3H2O, and 0.005 mmol of MnAc2 (5 at. %) were mixed in 5 mL of toluene and stirred with 0.045 mL of OA and 0.075 mL OLAM to get a clear solution. Concentrated HCl acid (0.1 mL) was injected under vigorous stirring. The successful doping of CsPbCl3 NCs was evidenced by the observation of the characteristic emission of Mn2+ under excitation with a 365 nm UV lamp. The average chemical yield is around 70% and was determined by weighing the final reaction product and comparing this to the expected weight for 0.1 mmol of the product.

Shell Growth

For growth of an undoped CsPbCl3 shell around the Mn2+-doped NCs, a coating precursor solution was prepared by dissolving 0.01 mmol of CsAc and PbAc2 in 5 mL of toluene with 0.01 mL of OA and OLAM. Separately, a clear crude solution of NCs was made by redissolving dried Mn2+-doped CsPbCl3 NCs (∼0.01 mmol) and oleylammonium chloride (∼0.01 mmol) in 1 mL of toluene. To this crude solution, the coating precursor solution was slowly added. To achieve different shell thicknesses, the amount of coating solution was increased from 0 to 0.3 mL with the increment of 0.05 mL.

Characterization

A variety of techniques was used to characterize the doped CsPbCl3 NCs and to investigate the doping process. To determine the crystal structure and phase purity, X-ray diffraction (XRD) patterns were recorded by using a PW 1729 Philips diffractometer, operating at 40 kV and 20 mA and using Cu Kα radiation (λ = 1.5418 Å). For XRD analysis, the sample plates were prepared by evaporating the NCs films on the silicon wafer. Transmission electron microscopy (TEM) images were made with a FEI TECNAI T12, operating at 120 kV and a Talos F200X, operating at 200 kV. The samples for TEM imaging were prepared by dipping a carbon-coated copper mesh TEM grid into a toluene solution of NCs. The excess liquid was evaporated under vacuum. Elemental analysis was used to determine the Mn/Pb elemental ratio using a PerkinElmer Optima 8300 inductively coupled plasma-optical emission spectrometer (ICP-OES). To this end, samples were dissolved in concentrated HCl acid overnight, followed by dilution with 5% HNO3 acid.

Absorption spectra were obtained with a double beam PerkinElmer Lambda 950 UV/vis/IR spectrophotometer. Luminescence (emission and excitation) spectra and photoluminescence (PL) decay curves were measured using an Edinburgh Instruments FLS920 spectrofluorometer equipped with a 450 W xenon lamp as excitation source and a 0.22 m double grating monochromator for excitation (Bentham DTMS300, 1200 lines/mm grating, blazed at 300 nm for excitation). Emission spectra (380–700 nm) were recorded with a single 0.22 m monochromator (500 nm blazed grating), and the emitted light was detected by a Hamamatsu R928 photomultiplier tube (PMT). Decay curves of the Mn2+ emission were recorded in the same setup using the third harmonic of a 10 Hz pulsed Nd:YAG laser as the excitation source (pulse width: 10 ns, λex = 355 nm) and a Hamamatsu R928 photomultiplier tube (PMT) for light detection. The samples for optical analysis were prepared by dissolving the crude NCs mixture in toluene and transferring the solution to the quartz cuvette.

Photoluminescence quantum yield (PL QY) determination was done using Lumogen Red 305 with a PL QY 95% in toluene as a first reference. With this reference, the PL QY of CsPbBr1.5 I1.5 nanocrystals (λem = 598 nm) was determined under 443 nm excitation. Next, the PL QY of Mn2+-doped CsPbCl3 NCs was determined by comparison with the second reference (CsPbBr1.5 I1.5 nanocrystals) using 380 nm excitation. The absorption coefficients of all the samples were carefully tuned to the range 0.02–0.1.

Results and Discussion

Synthesis and Luminescence of CsPbCl3/Mn2+ NCs

To investigate the formation of the CsPbCl3 NCs, the reaction product was analyzed using a variety of techniques to determine size, crystal structure, and chemical composition. In Figure (a) the X-ray diffraction (XRD) patterns for doped and undoped CsPbCl3 NCs are shown. The XRD pattern shows a number of diffraction peaks at angles that are characteristic of the CsPbCl3 perovskite structure. The positions for diffraction peaks calculated from the unit cell parameters are marked by filled blue circles and match the position observed. There is no difference between the XRD pattern for the doped (nominal concentration: 10 at. % Mn, actual Mn2+ concentration ∼1 at. %) and undoped CsPbCl3 NCs. The width of the peaks reflects a small crystallite size. However, due to the close resemblance of diffraction peaks of the tetragonal phase of CsPbCl3 and the cubic phase (Supporting Information, Figure S1) coupled with the broadness of the diffraction peaks, further study is still needed to confirm the phase of the product. To determine the size and size distribution, TEM images were recorded. Figure (b) shows TEM images of CsPbCl3 NCs on a TEM grid that was dipped into a NCs’ solution. On the grid, areas with a high density of NCs are observed where the NCs are ordered. It is believed that, during evaporation of the solvent, self-assembly of the cubic CsPbCl3 NCs takes place, resulting in the highly ordered pattern. From analysis of the size of NCs, the average size (length of the edge of squares) was determined to be 7 nm. In Figure S2 the size distribution obtained from the analysis of 100 NCs is shown (Supporting Information Figure S2 (C1)). For 7 nm CsPbCl3 NCs, weak quantum confinement effects can be expected, as the exciton Bohr radius in CsPbCl3 is ∼2.5 nm.[14] Elemental analysis was done to determine the actual Mn2+ concentration in the NCs, as it is often observed that the fraction of dopant ions incorporated is lower than the nominal concentration of dopants added to the reaction mixture. A series of samples was prepared with different nominal Mn2+ concentrations (5 at. % to 25 at. %, relative to Pb2+). The Mn2+ concentrations in the CsPbCl3:Mn2+ NCs after careful washing were determined with ICP-AES, and the results are shown in Table S1 of the Supporting Information. The concentration of Mn2+ incorporated is about 10 times less than the concentration in the reaction mixtures and seems to saturate around just above 2 at. % Mn2+ for the presently used synthesis protocol. The fraction of dopant ions incorporated is typically much lower than the nominal concentration added and is determined by kinetic and thermodynamic effects, which are less favorable for incorporation of the chemically different dopant ion than for the host cation.[24,25] For example, for Mn2+ incorporation in ZnSe NCs, the actual Mn2+ concentration was found to be around 10% of the Mn2+ concentration added and to saturate at 3 at. % Mn2+.[26] Similar observations have been reported for ZnS:Mn2+.[27] Extensive research on Mn2+ incorporation in CdSe QDs has provided more insight into the role of both kinetic and thermodynamic factors controlling dopant incorporation, and under extreme circumstances (very high Mn2+ concentration in the presence of extra host anions), concentrations of 30 at. % Mn2+ were realized.[28] It can be expected that with different synthesis methods also for CsPbCl3 NCs, higher Mn2+ doping levels are possible.

Figure 1

Structure characterization of as-prepared undoped and Mn-doped CsPbCl3 NCs. (a) XRD pattern of undoped and doped samples.(b) TEM image of Mn2+-doped (nominal concentration: 10 at. %, actual concentration ∼1 at. %) CsPbCl3 NCs.

The optical properties of the NCs were explored by recording emission and excitation spectra for CsPbCl3 NCs doped with Mn2+. Figure shows the typical absorption, emission, and excitation spectra of Mn2+-doped (10 at. %) CsPbCl3 NCs. In the emission spectrum, two distinctive peaks can be seen, namely, a narrow peak located at 405 nm with fwhm 11 nm and a broad band with a maximum around 600 nm. The narrow band at 405 nm is assigned to the intrinsic exciton emission of CsPbCl3 NCs while the broader emission peak at 600 nm (fwhm: ∼100 nm) is assigned to a 3d5 intraconfigurational Mn2+ transition (4T1 → 6A1).[2,22,23] The excitation spectra both of the exciton emission at 405 nm and of the Mn2+ emission at 600 nm very closely follow the absorption spectrum. The spectra have a sharp onset at 400 nm followed by a first maximum around 385 nm, a weak second maximum around 360 nm, and a third maximum around 337 nm. The fine structure observed is typical for nanoparticles where discrete energy levels that emerge at the band edges give rise to discrete transitions and fine structure in the absorption/excitation spectra. For the II–VI (e.g., CdSe) and IV–VI (e.g PbSe) QDs, this fine structure has been extensively investigated, and theoretical calculations on peak positions and absorption strengths have been compared with experimental spectra to gain insight into the energy level structures of the QDs. For the perovskite NCs, energy level calculations explaining the fine structure are in progress. The observation of the exciton absorption peaks in the excitation spectrum of the Mn2+ emission provides strong evidence for the incorporation of Mn2+ in the CsPbCl3 NCs. Clearly, exciton absorption by the CsPbCl3 NCs is followed by energy transfer to Mn2+ and bright yellow/orange emission from the Mn2+ ions. The fact that exciton to Mn2+ energy transfer is observed shows the successful incorporation of Mn2+ in the CsPbCl3 NCs.

Figure 2

Absorption, excitation, and emission spectra of Mn2+-doped (10 at. % nominal concentration) CsPbCl3 NCs. The inset shows a photograph of a vial with a colloidal dispersion of undoped (left) and Mn-doped (right) CsPbCl3 sample under excitation of 365 nm UV light. The Mn2+ concentration indicated is the nominal concentration; the actual Mn2+ concentration in the NCs is much lower (see Table S1 of the Supporting Information).

It is interesting to investigate the incorporation mechanism for this room temperature synthesis. In the formation mechanism of NCs, ligands play an important role. To investigate the role of the ligands, we systematically varied the concentrations of both oleic acid (OA) and oleylamine (OLAM). Surface passivation by ligands is crucial and influences colloidal stability, quantum yield, and doping efficiency. In the present case, a ligand combination of OA and OLAM is used. This is essential to obtain a clear solution of the precursors (CsAc, PbAc2, and MnAc2), which is important for achieving a stable colloidal solution of NCs. Furthermore, the long chain amine can play an important role in regulating the crystallization process of the NCs, while the steric repulsion provided by oleic acid is integral to preventing the irreversible coagulation. The presence of ligands is crucial in forming a stable colloidal solution of NCs. However, a stable bond between Mn2+ ions and ligands will hinder the effective incorporation of Mn2+. These considerations reflect the trade-off between colloidal stability and successful incorporation of Mn2+ ions. To optimize the synthesis, the added volume of OA was varied from 0.015 to 0.125 mL while keeping the added volume of OLAM fixed at 0.015 mL, and the added OLAM volume was varied from 0.015 to 0.15 mL while keeping the volume of OA fixed at 0.045 mL. The variations of the emission spectra as a function of OA or OLAM volume are shown in Figure a and 3b. The results show a strong dependence of the relative Mn2+ emission intensity, especially on the OA concentrations. The relative intensity of the Mn2+ emission is expected to increase with Mn2+ concentration in the CsPbCl3 NCs. The Mn2+ concentrations were determined using ICP, and the results are collected in Table S1 of the Supporting Information. Indeed, the Mn2+ concentration shows the same trends as the Mn2+ emission intensity, which means that a decrease in the Mn2+ emission intensity can be explained by a lower concentration on Mn2+ in the NC, except for the highest Mn2+ concentrations, where concentration quenching starts to play a role (vide infra). For OA added volumes higher than 0.045 mL, a very rapid decrease in the Mn2+ concentration is observed. The added volume of OLAM also affects the relative intensity of the Mn2+ emission. For an OA volume of 0.045 mL, the highest relative Mn2+ emission intensity is observed for 0.075 mL of OLAM.

Figure 3

Emission spectrum of as-prepared CsPbCl3:Mn2+ NCs samples formed under different reaction conditions at 297 K. All spectra are normalized to the absorption at 365 nm, which makes a direct comparison of the efficiencies of the emission possible. (a) PL emission spectrum as a function of OA volume (λex = 365 nm). (b) PL emission spectrum as a function of OLAM volume (λex = 365 nm). (c) PL emission spectrum as a function of HCl volume (λex = 365 nm). (d) Emission spectrum of Mn2+-doped CsPbCl3 NCs with 5 at. % ∼ 25 at. % Mn2+ in the reaction mixture. The Mn2+ concentrations indicated are nominal concentration; the actual Mn2+ concentration in the NCs is much lower and depends strongly on the synthesis conditions (see Table S1 of the Supporting Information).

To understand the variation in incorporation efficiency for different added OLAM/OA volumes, the doping mechanism needs to be considered. Given the present reaction conditions, the doping resembles diffusion doping that was recently shown to be effective in incorporating Mn2+ in CdSe.[29] This doping process is largely thermodynamically controlled. Dopant incorporation is driven by a high chemical potential of the dopant in solution which will be further internalized from the surface layer and subsequently diffuses inward. In our synthesis, metal acetate salts are the initial metal precursors. When metal acetate salts are dissolved in toluene with oleic acid and oleylamine, acetate ligands will be replaced by oleate ligands and form dissolvable metal-oleate complexes. Initially, after addition of the hydrochloric acid, the carboxylate groups of the oleate ligand are protonated, which results in a massive increase in the concentration of active metal monomers. Consequently, the chemical potential of metal ions (e.g., Cs+, Pb2+, Mn2+) in bulk solution is substantially increased and provides a strong driving force for the crystallization of CsPbCl3. In the presence of excess Cl– (from the addition of concentrated HCl) a Cl– surface layer allows for binding of Mn2+ to the surface, followed by inward diffusion. Given that there is an activation energy for inward diffusion, the Mn2+ incorporation is expected to be slow at room temperature and the Mn2+ concentration in the surface layer can be expected to be higher than in the core of the NCs.

Second, since the doping and crystallization process are initiated by protonation of metal-oleate complex, it is expected that H+ ions are of prime importance to determine PL properties. The influence of varying volume of HCl added is depicted in Figure c. A strong increase in the Mn2+ emission intensity is observed when the volume of HCl acid increases from 0.01 to 0.1 mL. Increasing the concentration of H+ will facilitate the formation of reactive metal monomer, resulting in a higher chemical potential difference of metal ions in solution and nanocrystals. In addition, the higher Cl– concentration will result in surface adsorption of Cl–, and adsorption of Mn2+ at the Cl– rich surface will be followed by internalization of Mn2+ through cation diffusion. Thus, excess Cl– will decrease the chemical potential of dopant ions in the host lattice, enlarging the driving force for Mn2+ incorporation. Again, similar observations were made for Mn2+ diffusion doping of CdSe, where the anion (Se2–) concentration in solution was shown to be crucial for successful Mn2+ doping.[29] With further increase of the amount of HCl acid, the emission intensity of Mn2+ decreases. The reduction of Mn2+ emission intensity suggests that H2O from halide acid may affect the incorporation of Mn2+ while also the chemical stability of the NCs may be reduced at the highest HCl concentrations. The optimum concentration (under the presently optimized reaction conditions) is 0.10 mL of concentrated HCl.

Based on the observations discussed above, the optimized synthesis conditions for further NCs synthesis are HCl: 0.1 mL, OA: 0.045 mL, and OLAM: 0.075 mL. The observation of Mn2+ emission indicates that energy transfer from the exciton to Mn2+ ions occurs. However, it still cannot rule out the possibility that a large fraction of the Mn2+ ions are only surface bound and not (statistically) incorporated in the nanocrystal lattice. The fact that for a 1–2 at. % Mn2+ content (on average 30–60 Mn2+ ions per CsPbCl3 NC) exciton emission is still observed indicates that energy transfer to Mn2+ is not highly efficient. For Mn2+ in the center of the NC, where the exciton wave function has the higher amplitude, more efficient energy transfer is expected. The observation of exciton emission indicates that the concentration of Mn2+ is relatively higher closer to the surface of the NC, where the overlap with the exciton wavelengths is weaker. The relative intensity of the exciton emission is observed to vary between samples that were prepared under identical conditions and is also affected by the washing procedure. The trends observed in Figure are however reproducible and provide information on the optimum conditions for Mn2+ incorporation for the present synthesis protocol.

In order to further internalize surface bound dopant ions, surface passivation by isocrystalline core–shell (ICS) growth was adopted. Several reports have confirmed that solution epitaxial growth of additional layers of host material can efficiently internalize surface-bound dopant ions, hence enhancing the relative intensity of dopant emission.[30−32] For growing a CsPbCl3-shell layer, 0.01 mmol of the purified Mn2+-doped CsPbCl3 NCs was redispersed in 1 mL of toluene. This was followed by slow addition of a specific volume of a solution consisting of Pb2+ and Cs+ precursors for overgrowth with a CsPbCl3 shell under vigorous stirring. The samples obtained after additional shell growth will be referred to as Cx (x represents sample number, C1 is the original NCs without any modification, higher numbers correspond to a thicker shell). Figure presents the evolution of PL QY of an as-prepared sample with that of NCs with different isocrystalline shell thicknesses. The details of PL QY determination can be found in the Experimental Section. As can be seen from Figure , a general trend of an increase in PL QY of the Mn2+ emission is observed with increasing shell thickness. The highest PL quantum yield is measured for sample C7. The high PL QY (39%) reflects successful incorporation of surface bound Mn2+ ions by overgrowth of a CsPbCl3 shell. Successful growth of additional layers of CsPbCl3 is also supported by a slight red shift of the exciton emission peak of CsPbCl3 NCs (Supporting Information Figure S3). Additionally, the shape of the emission peak of CsPbCl3 NCs is largely unaffected without any broadening. This confirms that the process of continued growth on existing CsPbCl3 NCs is dominant (Supporting Information, Figure S3). TEM images of samples C1 and C7 were shown in Figure S2 and reveal a clear increase of the average size of NCs after shell coating (from 7 to 8.5 nm).

Figure 4

Effect of ICS growth on the relative PL QY and integrated area under the Mn2+ luminescence decay curves for Mn2+-doped CsPbCl3 NCs. Blue line: evolution of PL QY as a function of shell thickness (λex = 380 nm). The inset shows a photograph of samples C1 to C7 (left to right) under excitation with a 365 nm UV lamp (Please note that the NCs concentration of each sample is different, decreasing from left to right). Red line: Evolution of integrated area under the Mn2+ emission decay curves for samples C1 to C7 (λex = 355 nm, λem = 600 nm).

Further evidence for the beneficial influence of ICS growth on the luminescence efficiency can be obtained from luminescence lifetime measurements. Luminescence decay curves of the Mn2+ emission are shown in Figure S4 of the Supporting Information. The Mn2+ emission decay curve of the as-prepared samples does not show monoexponential decay behavior. A multiexponential fitting has to be used, and a biexponential fit gives a reasonably good agreement, with lifetimes of 0.15 and 0.78 ms. Upon overgrowth of an additional CsPbCl3 shell, a clear lengthening of the decay lifetime of the Mn2+ emission is observed. This is explained by a reduction of Mn2+ ions close to surface quenching sites. It is well-known that luminescent ions close to the surface experience faster decay as a result of energy transfer to surface defects. This results in a faster and also nonexponential decay, as the nonradiative decay rate varies between luminescent ions at varying distances from quenching sites. A transformation of the Mn2+ emission decay curve from multiexponential to monoexponential is observed as the undoped CsPbCl3 layer thickness increases. This is consistent with efficient incorporation of Mn2+ ions by additional shell growth, which effectively removes Mn2+ ions at the NC surface by overcoating with an undoped isocrystalline CsPbCl3 shell. For the thickest CsPbCl3 shell, a monoexponential decay curve with a 1.4 ms decay time is observed. The 1.4 ms Mn2+ lifetime is the radiative lifetime and is in the millisecond range that is expected for the spin- and parity-forbidden 4T1–6A1 transition within the 3d5 configuration of Mn2+. The evolution of integration area under the decay curve, which is a good indicator for the relative PL QY, runs parallel to the PL QY determined by the double reference method. The final PL QY of 40% is high and can possibly be further improved by optimizing the synthesis conditions. The high PL QY makes these Mn2+-doped NCs promising for application as efficient emitters in optical devices.

The thermal stability of NCs is another issue, especially for applications in high-power LEDs where on-chip phosphors reach temperatures between 150 and 200 °C. To gain insight on the quenching behavior of NCs with different shell thicknesses at elevated temperature, the thermal stabilities of C1–Mn2+:CsPbCl3 and C7–Mn2+:CsPbCl3 (both in toluene, boiling point: 111 °C) were tested using a thermal cycling experiment. By monitoring the luminescence intensity of the Mn2+ emission band for successive heating and cooling cycles, we studied the temperature dependent luminescent behavior. The thermal cycling experiments were conducted between 30 °C and 110 °C. Emission spectra was taken every 10 °C under 365 nm illumination. During the measurement, the temperature of the sample was gradually increased to 110 °C and allowed to cool down to 30 °C. Both heating and cooling were done in a controlled manner (heating and cooling rate: ∼10 °C/min).

The temperature dependent luminescence characteristics of C1–Mn2+:CsPbCl3 (no CsPbCl3 shell) and C7–Mn2+:CsPbCl3 (thickest CsPbCl3 shell) are plotted in Figure . Upon raising the temperature, the peak intensity of the uncoated CsPbCl3:Mn2+ sample shows a continuous decrease (Figure a, emission spectra are shown in Figure S5), losing nearly 50% of peak intensity at 110 °C.

Figure 5

Temperature dependent PL behavior. (a) Peak emission intensity of sample C1–Mn2+: CsPbCl3 NCs (no shell overgrowth) and C7–Mn2+:CsPbCl3 NCs (overcoated) as a function of temperature. (b) Temperature dependent emission spectra for C7–Mn2+:CsPbCl3 NCs.

After the first heating cycle, the uncoated CsPbCl3:Mn2+ sample suffered an ∼15% permanent peak intensity loss (see Figure a). A much superior temperature stability is observed for the emission from the core–shell sample C7. A nearly constant PL intensity is observed when temperature varies from 30 to 110 °C (see also Figure a and Figure S6). In fact, a small increase in emission intensity is observed upon heating. This increase can be explained by thermal annealing of defects. Defects reduce the emission intensity. The nonequilibrium defect concentration, for example defects at the interface between the core and isocrystalline shell, can be reduced by annealing. A beneficial effect of annealing is generally observed for (nano)crystalline luminescent materials and can explain the presently observed increase in emission intensity during and after the heat treatment. The superior thermal stability of the Mn2+ emission for the CsPbCl3:Mn2+ after overgrowth with an undoped CsPbCl3 shell is explained by efficient passivation from thermally induced quenching sites located at the surface. Furthermore, it is also interesting to note a small shift of the emission wavelength of the Mn2+ emission during the heating cycle. As shown in Figure b, the emission shifts to higher energies (blue shift) when the temperature increases from 30 to 110 °C, which is fully reversible upon cooling. The reason for the temperature dependent emission wavelength is lattice expansion at high temperature.[33] Lattice expansion results in a larger Mn2+–ligand distance and thus a smaller crystal field splitting. The 3d5 Tanabe–Sugano diagram shows that the emission maximum shifts to higher energies (shorter wavelengths) for stronger crystal fields. The stabilization of the doped CsPbCl3 NCs is important for the applicability of ICS growth.

Conclusions

In summary, Mn2+-doped CsPbCl3 perovskite NCs were synthesized by a facile room temperature method. Following addition of a small volume of concentrated HCl acid to a clear solution containing Mn2+, Cs+, and Pb2+ precursors, monodisperse Mn2+-doped CsPbCl3 NCs showing bright orange Mn2+ emission were obtained. For the used doping levels (up to 25 at. % relative to Pb), no substantial changes of the NC size and shape were observed. Several important synthesis parameters, e.g. ligand volume and ratio, HCl volume, and Mn2+ concentration, were optimized to achieve highly efficient Mn2+ emission. Overgrowth with an undoped CsPbCl3 shell strongly improves the photoluminescence quantum yield of the Mn2+ emission (up to 40%) and also improves the thermal stability (no thermal quenching up to 110 °C). Overall, the presently reported room temperature synthesis method enables us to achieve highly luminescent NCs and provides new insights in the development of new doping strategies for perovskite NCs.