Metal-Ion-Doped Manganese Halide Hybrids with Tunable Emission for Advanced Anti-Counterfeiting

Stimuli-responsive luminescent materials have received great attention for their potential application in anti-counterfeiting and information encryption. Manganese halide hybrids have been considered an efficient stimuli-responsive luminescent material due to their low price and adjustable photoluminescence (PL). However, the photoluminescence quantum yield (PLQY) of PEA2MnBr4 is relatively low. Herein, Zn2+- and Pb2+-doped PEA2MnBr4 samples are synthesized, and show an intense green emission and orange emission, respectively. After doping with Zn2+, the PLQY of PEA2MnBr4 is elevated from 9% to 40%. We have found that green emitting Zn2+-doped PEA2MnBr4 could transform to a pink color after being exposed to air for several seconds and the reversible transformation from pink to green was achieved by using heating treatment. Benefiting from this property, an anti-counterfeiting label is fabricated, which exhibits excellent “pink-green-pink” cycle capability. Pb2+-doped PEA2Mn0.88Zn0.12Br4 is acquired by cation exchange reaction, which shows intense orange emission with a high QY of 85%. The PL of Pb2+-doped PEA2Mn0.88Zn0.12Br4 decreases with increasing temperature. Hence, the encrypted multilayer composite film is fabricated relying on the different thermal responses of Zn2+- and Pb2+-doped PEA2MnBr4, whereby the encrypted information can be read out by thermal treatment.


Introduction
Counterfeiting and forgery are an ever-growing global issue, causing serious financial losses to governments, companies and individuals. Over the last few decades, counterfeit products have been widely found in daily consumer goods, diplomas, medicines and banknotes [1][2][3]. Information security, including encryption and anticounterfeiting, is becoming an important task that needs to be urgently accomplished. The development of advanced anti-counterfeiting technologies is the only way to solve this dilemma. Due to the merit of visual identifiability and easy operation, luminescent anti-counterfeiting is considered to provide ideal security elements [4,5].
However, the current luminescent materials are easy to mimick due to their monotony response to the excitation light. Stimuli-responsive luminescent materials and multi-mode excited luminescent materials as new kinds of advanced anti-counterfeiting luminescent materials have attracted much attention. Multi-mode excited luminescent materials show multicolor emissions under multiple excitation modes (PL, upconversion luminescence, and long-lasting luminescence), which is hard to mimick [6,7]. However, multi-mode excited luminescent materials usually contain expensive rare earth elements and require different excitation light sources, which is severely restricted by non-portable testing tools. Stimuliresponsive luminescent materials will change their optical properties, including spectra and lifetime, in response to external stimuli such as light, [8] electricity [9], temperature [10,11], force [12], and gases [13]. So far, various organic and inorganic luminescent materials, including organic dyes [14], quantum dots [15][16][17], and transition metal complexes [9], have been used as stimuli-responsive PL materials, but most of these materials suffer from complicated and tedious synthesis and unsatisfactory PL properties.
Due to the low toxicity, low price, and high abundance of Mn 2+ , manganese halide hybrids have been considered as an efficient luminescent material [35][36][37]. Besides, Mn 2+ is stable in an ambient environment. The emission spectrum of manganese halide hybrids can be tuned by the crystalline field of Mn 2+ ions. The tetrahedral coordination Mn 2+ emits a green color with a narrow full width at half-maximum (FWHM), whereas the octahedral coordination Mn 2+ exhibits orange emission with a broad FWHM [35][36][37]. For Mn-based material, its emission can be adjusted by the ratio of reactants due to this unique luminescent property, which is conducive to a color-changing application. Zang et al. synthesized green emitting 0D organic metal halide C 6 N 2 H 16 MnBr 4 , which could be transformed into the non-emissive hydrated phase C 6 N 2 H 16 MnBr 4 (H 2 O) 2 by uptake of water molecules [3]. The reversible color changing was due to the change in the coordination environment. Rewritable PL paper has been constructed relying on this reversible structure transformation, which showed excellent cycle capability. Chen and co-workers found that tetrahedron and trigonal bipyramid could be converted to each other as well. Specifically, green emitting [MnBr 2 (dppeO 2 )] n could transform to [MnBr 2 (dppeO 2 )(DMF)] n upon exposure to DMF vapor, and reversible conversion could be realized by heating treatment [38]. Han et al. reported a tunable pure-color red/green/blue emission in cesium manganese bromides nanocrystals (NCs) by modulating their crystal field strengths. Redemitting CsMnBr 3 NCs could transform into green-emitting Cs 3 MnBr 5 NCs by adding isopropanol. Furthermore, after contact with water, either CsMnBr 3 NCs or Cs 3 MnBr 5 NCs could transform into blue-emitting Cs 2 MnBr 4 ·2H 2 O NCs, while Cs 2 MnBr 4 ·2H 2 O NCs could transform into the mixture of CsMnBr 3 and Cs 3 MnBr 5 phase during dehydration treatment. [39]. Compared to other Mn-based halide materials, PEA 2 MnBr 4 can be regarded as a good candidate for the stimuli-responsive luminescent materials, which does not involve complicated ligands and shows complete reversal transformation. Tang and co-workers prepared a new organic-inorganic hybrid PEA 2 MnBr 4 single-crystal, and they found that PEA 2 MnBr 4 possessed humidity chromism characteristics (it emitted green and pink emission at the water-desorption state and water-adsorption state, respectively) [40]. Due to the visible chromism, this PEA 2 MnBr 4 was used as a marker to check water content (0.02 and 0.05 vol%) in toluene. However, the PLQY of PEA 2 MnBr 4 was relatively low and the cycle stability was unsatisfactory.
Ion doping has been regarded as an effective method to optimize the properties of Mn-based materials [36,37,41]. Here, we report on the synthesis of Zn 2+ -and Pb 2+ -doped PEA 2 MnBr 4 by the direct hot-injection method and cation-exchange method, respectively. Zn 2+ -doped PEA 2 MnBr 4 exhibits a strong green PL band centered at 528 nm with a PLQY of 40%, and it can transform to a pink color after being exposed to air for several sec-onds. The reversible color change from pink to green can be realized after the heating treatment. Benefiting from this property, the anti-counterfeiting label and trademark were fabricated, which exhibited excellent "pink-green-pink" cycle capability. The Pb 2+ -doped PEA 2 Mn 0.88 Zn 0.12 Br 4 shows broad-band orange emission originating from the 4 T 1 -6 A 1 transition of octahedrally coordinated Mn 2+ ions with a high QY of 85%. It's worth noting that different from the Zn 2+ -doped PEA 2 MnBr 4 , the Pb 2+ counterpart is stable in air and its PL decreases with increasing temperature. Utilizing the different thermal-responsive properties of Zn 2+ -and Pb 2+ -doped PEA 2 MnBr 4 , we have fabricated the encrypted multilayer composite film containing both Zn 2+ -and Pb 2+ -doped PEA 2 MnBr 4 . The encrypted information was concealed by the brighter orange fluorescence of Pb 2+ -doped PEA 2 Mn 0.88 Zn 0.12 Br 4 at the upper layer and it could be read out by thermal treatment.
Synthesis of PEA 2 MnBr 4 : 0.2 mmoL of MnAc 2 , 80 µL PEA, 0.3 mL DBSA, 0.2 mL OTAc and 5 mL ODE was placed into a 10 mL three-necked flask. Then, the flask was subjected to vacuum-nitrogen three times and heated to 80 • C to dissolve. After that, the flask was heated to 140 • C, and 150µL TMSBr was injected into the flask. 5 s later, the solution was cooled by an ice-water bath. The crude solution was centrifugated at 5000 rpm for 3 min. After centrifugation, the precipitate was washed with xylene twice and dried under vacuum.
Synthesis of PEA 2 Mn 0.88 Zn 0.12 Br 4 : The synthetic procedure of PEA 2 Mn 0.88 Zn 0.12 Br 4 was similar to that of pure PEA 2 MnBr 4 , except for the addition of ZnAc 2 . The new additions of MnAc 2 and ZnAc 2 are 0.0294 and 0.0066 g, respectively.
Synthesis of Pb 2+ -doped PEA 2 Mn 0.88 Zn 0.12 Br 4 by cation exchange method: 0.0037 g PbBr 2 and 0.0109 g TOAB were dissolved in 0.2 mL xylene to form a lead bromide precursor. Then, the lead bromide precursor was dropped into 3 mL of PEA 2 Mn 0.88 Zn 0.12 Br 4 solution (0.124 g PEA 2 Mn 0.88 Zn 0.12 Br 4 in 5 mL xylene). The solution was stirred for 10 min at room temperature. Then, the solution was subjected to centrifuge at 5000 rpm for 5 min. 5 mL of Xylene was added to the precipitate, and then centrifuged at 5000 rpm for 5 min. After that, hexane was added to wash the precipitate.
Synthesis of multilayer fluorescent composite films: 5 g of EVA was dissolved in 45 g of xylene to obtain a polymer solution. 0.2 mmol PEA 2 Mn 0.88 Zn 0.12 Br 4 was dispersed into 2 mL polymer solution. The mixture was screen-printed on the glass substrate to print the pattern. Next, the polymer solution was spun onto the glass substrate to completely cover the pattern. Then, 0.2 mmol product of Pb 2+ -doped PEA 2 Mn 0.88 Zn 0.12 Br 4 was dispersed into 2 mL polymer solution and spun onto the glass substrate as the upper layer. The glass was placed on the hot plate to observe the encryption and decryption process.
Characterization: The PL and PLE spectra were conducted by a FLS920P spectrometer (Edinburgh Instruments, Livingston, UK). The absolute PLQYs and time-resolved PL decays of the samples were measured by a fluorescence spectrometer (FLS920P, Edinburgh Instruments, UK). The Fourier transform infrared (FTIR) spectrum was conducted Nanomaterials 2023, 13, 1890 4 of 15 on a Thermo-Nicole iS50 FTIR spectrometer with an attenuated total reflection detector (Bruker, Bremen, Germany). The inductively coupled plasma optical emission spectrometry (ICP-OES) measurements were measured by an ICP Optima 8300 (PerkinElmer, Waltham, MA, USA). X-ray photoelectron spectroscopy (XPS) was recorded on a Thermo Scientific K-Alpha spectrometer (Thermo, Waltham, MA, USA). The X-ray diffraction (XRD) measurements were measured on a Rigaku Smart Lab 9 kW (Rigaku Corporation, Tokyo, Japan). Scanning electron microscope (SEM) images were acquired using ZEISS Sigma 500 (ZEISS, Jena, Germany).

Results and Discussion
PEA 2 MnBr 4 micro-sized powders were prepared by the hot-injection method (see details in the Materials and Methods Section). We found that the carboxylic acid ligands have an important influence on the composition of products. The X-ray diffraction (XRD) patterns of products prepared by different carboxylic acid ligands are shown in Figure 1. When oleic acid (OA) is used, the impurity phase not belonging to PEA 2 MnBr 4 appears. Instead, most of the diffraction peaks of the product synthesized by dodecylbenzene sulfonic acid (DBSA) are consistent with the main peaks in ICSD 13,856, demonstrating that DBSA facilitates the acquisition of the PEA 2 MnBr 4 phase. This may be because DBSA ligands have an aromatic ring structure and they can stabilize the PEA 2 MnBr 4 phase by π-π stacking interaction with β-phenylethylamine (PEA) molecules. The strong acidity of DBSA may have a tight connection with Mn 2+ , which may further strengthen the stability of the PEA 2 MnBr 4 phase. However, the DBSA possesses large steric hindrance, which offers incomplete protection of PEA 2 MnBr 4 , causing low PLQY and a small amount of impurity at 32.2 • , 37.1 • , and 38.5 • . In order to elevate the PLQY and acquire the pure phase of the PEA 2 MnBr 4 , a small amount of octanoic acid (OTAc) with a short carbon-chain was added to further passivate the surface of PEA 2 MnBr 4 . As shown in Figures 1 and S1, the product prepared by DBSA and OTAc possesses a pure phase structure, and the PLQY is elevated from 3% to 9%. decays of the samples were measured by a fluorescence spectrometer (FLS920P, Edinburgh Instruments, UK). The Fourier transform infrared (FTIR) spectrum was conducted on a Thermo-Nicole iS50 FTIR spectrometer with an attenuated total reflection detector (Bruker, Bremen, Germany). The inductively coupled plasma optical emission spectrometry (ICP-OES) measurements were measured by an ICP Optima 8300(PerkinElmer, Waltham, MA, USA). X-ray photoelectron spectroscopy (XPS) was recorded on a Thermo Scientific K-Alpha spectrometer (Thermo, Waltham, MA, USA). The X-ray diffraction (XRD) measurements were measured on a Rigaku Smart Lab 9 kW (Rigaku Corporation, Tokyo, Japan). Scanning electron microscope (SEM) images were acquired using ZEISS Sigma 500 (ZEISS, Jena, Germany).

Results and Discussion
PEA2MnBr4 micro-sized powders were prepared by the hot-injection method (see details in the Experimental Section). We found that the carboxylic acid ligands have an important influence on the composition of products. The X-ray diffraction (XRD) patterns of products prepared by different carboxylic acid ligands are shown in Figure 1. When oleic acid (OA) is used, the impurity phase not belonging to PEA2MnBr4 appears. Instead, most of the diffraction peaks of the product synthesized by dodecylbenzene sulfonic acid (DBSA) are consistent with the main peaks in ICSD 13,856, demonstrating that DBSA facilitates the acquisition of the PEA2MnBr4 phase. This may be because DBSA ligands have an aromatic ring structure and they can stabilize the PEA2MnBr4 phase by π-π stacking interaction with β-phenylethylamine (PEA) molecules. The strong acidity of DBSA may have a tight connection with Mn 2+ , which may further strengthen the stability of the PEA2MnBr4 phase. However, the DBSA possesses large steric hindrance, which offers incomplete protection of PEA2MnBr4, causing low PLQY and a small amount of impurity at 32.2°, 37.1°, and 38.5°. In order to elevate the PLQY and acquire the pure phase of the PEA2MnBr4, a small amount of octanoic acid (OTAc) with a short carbon-chain was added to further passivate the surface of PEA2MnBr4. As shown in Figures 1 and S1, the product prepared by DBSA and OTAc possesses a pure phase structure, and the PLQY is elevated from 3% to 9%. For further elevating the PLQY, Zn 2+ -doped PEA2MnBr4 was prepared by following the procedure of PEA2MnBr4 except adding ZnAc2 into the solution. Here, the feed ratios of Zn 2+ ([Zn]/([Zn] + [Mn]) mass ratio) were 5%, 15%, 25%, 35%, and 50%. After being calibrated by inductively coupled plasma optical emission spectrometer (ICP-OES) elemental analysis, the actual ratios of Zn 2+ were 4.6%, 12.3%, 23.6%, 32.9%, and 45.7%, respectively (Table S1). The PL spectra of PEA2MnBr4 with different Zn 2+ ratios are shown in Figure 2a. The PL intensity of Zn 2+ -doped PEA2MnBr4 first increases with increasing Zn 2+ concentration and reaches the maximum value at the Zn 2+ ratio of 15% For further elevating the PLQY, Zn 2+ -doped PEA 2 MnBr 4 was prepared by following the procedure of PEA 2 MnBr 4 except adding ZnAc 2 into the solution. Here, the feed ratios of Zn 2+ ([Zn]/([Zn] + [Mn]) mass ratio) were 5%, 15%, 25%, 35%, and 50%. After being calibrated by inductively coupled plasma optical emission spectrometer (ICP-OES) elemental analysis, the actual ratios of Zn 2+ were 4.6%, 12.3%, 23.6%, 32.9%, and 45.7%, respectively (Table S1). The PL spectra of PEA 2 MnBr 4 with different Zn 2+ ratios are shown in Figure 2a. The PL intensity of Zn 2+ -doped PEA 2 MnBr 4 first increases with increasing Zn 2+ concentration and reaches the maximum value at the Zn 2+ ratio of 15% (PEA 2 Mn 0.88 Zn 0.12 Br 4 ). Further increasing the substitution ratio results in a decline of PL intensity. As shown in Figure 2b,c, the PEA 2 Mn 0.88 Zn 0.12 Br 4 shows much more intense green emission compared with the undoped PEA 2 MnBr 4 . The PEA 2 Mn 0.88 Zn 0.12 Br 4 possesses a high PLQY of 40% (PEA2Mn0.88Zn0.12Br4). Further increasing the substitution ratio results in a decline of PL intensity. As shown in Figure 2b,c, the PEA2Mn0.88Zn0.12Br4 shows much more intense green emission compared with the undoped PEA2MnBr4. The PEA2Mn0.88Zn0.12Br4 possesses a high PLQY of 40% compared to 9% for the pristine PEA2MnBr4. The improvement of PLQY is caused by the mitigation of concentration quenching. Because Zn 2+ ions prefer to form a tetragonal coordination, Zn 2+ ions can replace Mn 2+ ions to inhibit the concentration quenching of Mn 2+ ions, thus leading to high QY. XRD patterns of the undoped PEA2MnBr4 and PEA2Mn0.88Zn0.12Br4 are displayed in Figure S2. All the diffraction peaks of PEA2Mn0.88Zn0.12Br4 move to a larger angle compared to that of undoped PEA2MnBr4, demonstrating that the interplanar crystal spacing is reduced. This is because the ionic radius of Mn 2+ (0.80 Å) is slightly larger than that of Zn 2+ (0.74 Å). Replacing Mn 2+ with smaller Zn 2+ leads to lattice contraction.
X-ray photoelectron spectroscopy (XPS) was carried out to analyze the electron density around the ions in PEA2MnBr4 and PEA2Mn0.88Zn0.12Br4 ( Figure S3). Both the PEA2MnBr4 and PEA2Mn0.88Zn0.12Br4 show strong characteristic Mn 2p and Br 3d peaks. Only the PEA2Mn0.88Zn0.12Br4 shows the Zn 2p peak located at 1022.6 eV, proving the presence of Zn 2+ in PEA2Mn0.88Zn0.12Br4. Besides, the binding energies of Mn 2p are reduced from 641.5 eV and 653.7 eV to 641.2eV and 653.4eV after Zn 2+ doping. Introducing Zn 2+ ions leads to the lattice contraction, which increases the electron density around the Mn 2+ ions, thus resulting in a decrease in Mn 2+ ion binding energy [42]. All the above characterizations suggest that Zn 2+ ions have been successfully doped into the PEA2MnBr4.
In addition, scanning electron microscope SEM measurement was also performed to investigate the effect of Zn 2+ doping on the morphology. As shown in Figure S4, both the PEA2MnBr4 and PEA2Mn0.88Zn0.12Br4 show irregular morphology. However, after doping with Zn 2+ , the particle size becomes smaller and the particles are more uniform than the pristine one, demonstrating that Zn 2+ doping can retard the reaction speed and homogenize particle size distribution.
To understand the origin of emissions in PEA2Mn0.88Zn0.12Br4, excitation power dependent PL measurements were performed. As shown in Figure S5, the PL intensity is linearly increased with the excitation power density. The origin of the emission can be estimated using the power-law equation, [43]. which is defined as IPL = nL k , where IPL represents the PL intensity; L is the excitation power; coefficient k relates to the recombination mechanism; and n represents the emission efficiency. Here, the fitted k value is 1.1, which represents a free exciton mechanism. We have also measured the PL spectra under different excitation wavelengths. As shown in Figure S5b, all the PL spectra were fixed at the peak of 528 nm as the excitation wavelength changed from 350 to 490 nm. The independence of excitation wavelength demonstrates that the source of this green emission is attributed to the same excited state-Mn 2+ emission center ( 4 T1 − 6 A1).
Interestingly, green-emitting PEA2Mn0.88Zn0.12Br4 becomes pink after being placed in air for several seconds and the pink color can convert back to the green color by thermal  Figure S2. All the diffraction peaks of PEA 2 Mn 0.88 Zn 0.12 Br 4 move to a larger angle compared to that of undoped PEA 2 MnBr 4 , demonstrating that the interplanar crystal spacing is reduced. This is because the ionic radius of Mn 2+ (0.80 Å) is slightly larger than that of Zn 2+ (0.74 Å). Replacing Mn 2+ with smaller Zn 2+ leads to lattice contraction.
X-ray photoelectron spectroscopy (XPS) was carried out to analyze the electron density around the ions in PEA 2 MnBr 4 and PEA 2 Mn 0.88 Zn 0.12 Br 4 ( Figure S3). Both the PEA 2 MnBr 4 and PEA 2 Mn 0.88 Zn 0.12 Br 4 show strong characteristic Mn 2p and Br 3d peaks. Only the PEA 2 Mn 0.88 Zn 0.12 Br 4 shows the Zn 2p peak located at 1022.6 eV, proving the presence of Zn 2+ in PEA 2 Mn 0.88 Zn 0.12 Br 4 . Besides, the binding energies of Mn 2p are reduced from 641.5 eV and 653.7 eV to 641.2 eV and 653.4 eV after Zn 2+ doping. Introducing Zn 2+ ions leads to the lattice contraction, which increases the electron density around the Mn 2+ ions, thus resulting in a decrease in Mn 2+ ion binding energy [42]. All the above characterizations suggest that Zn 2+ ions have been successfully doped into the PEA 2 MnBr 4 .
In addition, scanning electron microscope SEM measurement was also performed to investigate the effect of Zn 2+ doping on the morphology. As shown in Figure S4, both the PEA 2 MnBr 4 and PEA 2 Mn 0.88 Zn 0.12 Br 4 show irregular morphology. However, after doping with Zn 2+ , the particle size becomes smaller and the particles are more uniform than the pristine one, demonstrating that Zn 2+ doping can retard the reaction speed and homogenize particle size distribution.
To understand the origin of emissions in PEA 2 Mn 0.88 Zn 0.12 Br 4 , excitation power dependent PL measurements were performed. As shown in Figure S5, the PL intensity is linearly increased with the excitation power density. The origin of the emission can be estimated using the power-law equation, [43]. which is defined as I PL = nL k , where I PL represents the PL intensity; L is the excitation power; coefficient k relates to the recombination mechanism; and n represents the emission efficiency. Here, the fitted k value is 1.1, which represents a free exciton mechanism. We have also measured the PL spectra under different excitation wavelengths. As shown in Figure S5b, all the PL spectra were fixed at the peak of 528 nm as the excitation wavelength changed from 350 to 490 nm. The independence of excitation wavelength demonstrates that the source of this green emission is attributed to the same excited state-Mn 2+ emission center ( 4 T 1 − 6 A 1 ).
Interestingly, green-emitting PEA 2 Mn 0.88 Zn 0.12 Br 4 becomes pink after being placed in air for several seconds and the pink color can convert back to the green color by thermal treatment or vacuum treatment (Figure 3a). This color-changing phenomenon was associated with water adsorption and desorption, which can be confirmed by the Fourier transform infrared (FTIR) spectra results (Figure 3b). The stretching vibration peak belonging to water can be found at 3400 cm −1 . A similar phenomenon has also been observed in PEA 2 MnBr 4 single crystal [40]. Tang et al. believed that green and red emissions originated from tetradentate Mn 2+ and trigonal bipyramid Mn 2+ , respectively [40]. However, detailed structure characterization was not given. Color-changing phenomenon upon contact with water was also found in C 6 N 2 H 16 MnBr 4 . Zang et al. attributed the state of water molecules adsorption to octahedron coordination geometry [3]. In order to further verify the change in the structure, we have performed XRD measurements at high temperature (120 • C) and room temperature (25 • C) (Figure 3c). Strangely, the high temperature XRD pattern of the sample was similar to the room temperature XRD pattern, except that several diffraction peaks (20.9 • , 22.4 • and 27.9 • ) in the high temperature XRD are stronger than that in room temperature XRD. Because no new diffraction peak appears, the presence of red emission cannot be accurately determined. The absence of red-emitting sample diffraction peaks may be caused by the following two reasons: first, the amount of the red-emitting sample is low; second, the crystallinity of the red-emitting sample is poor or the diffraction peaks of the red-emitting sample are much like those of the green-emitting sample. Han et al. also found that it was hard to distinguish the red-emitting CsMnBr 3 phase by powder XRD when a small amount of red-emitting CsMnBr 3 mixed with green-emitting Cs 3 MnBr 5 NCs [39]. treatment or vacuum treatment (Figure 3a). This color-changing phenomenon was associated with water adsorption and desorption, which can be confirmed by the Fourier transform infrared (FTIR) spectra results (Figure 3b). The stretching vibration peak belonging to water can be found at 3400 cm −1 . A similar phenomenon has also been observed in PEA2MnBr4 single crystal [40]. Tang et al. believed that green and red emissions originated from tetradentate Mn 2+ and trigonal bipyramid Mn 2+ , respectively [40]. However, detailed structure characterization was not given. Color-changing phenomenon upon contact with water was also found in C6N2H16MnBr4. Zang et al. attributed the state of water molecules adsorption to octahedron coordination geometry [3]. In order to further verify the change in the structure, we have performed XRD measurements at high temperature (120 °C) and room temperature (25 °C) (Figure 3c). Strangely, the high temperature XRD pattern of the sample was similar to the room temperature XRD pattern, except that several diffraction peaks (20.9°, 22.4° and 27.9°) in the high temperature XRD are stronger than that in room temperature XRD. Because no new diffraction peak appears, the presence of red emission cannot be accurately determined. The absence of red-emitting sample diffraction peaks may be caused by the following two reasons: first, the amount of the red-emitting sample is low; second, the crystallinity of the red-emitting sample is poor or the diffraction peaks of the red-emitting sample are much like those of the green-emitting sample. Han et al. also found that it was hard to distinguish the red-emitting CsMnBr3 phase by powder XRD when a small amount of red-emitting CsMnBr3 mixed with green-emitting Cs3MnBr5 NCs [39]. We can deduce that the red emission originates from octahedron coordination geometry based on the following results of Pb 2+ doping. To get further insights into the PL mechanism, photoluminescence excitation (PLE) spectra were carried out. As shown in Figure 4, the PLE spectrum monitored at 528 nm is in coincidence with that monitored at 640 nm, demonstrating that energy transfer takes place from the tetrahedron Mn 2+ to the octahedron Mn 2+ . A similar energy transfer process of Mn 2+ has also been observed in [Mn(dppeO 2 ) 3 ] − [MnBr 4 ]. [38]. The crystal field strengths around Mn 2+ can be calculated according to the PLE spectrum. Here, the Racah parameter (B and C) and crystal field strength (Dq) of Zn 2+ -doped and undoped samples are shown in Table S2. After doping with Zn 2+ , the crystal field strength increases, which is due to the lattice contraction. We can deduce that the red emission originates from octahedron coordination geo etry based on the following results of Pb 2+ doping. To get further insights into the mechanism, photoluminescence excitation (PLE) spectra were carried out. As shown Figure 4, the PLE spectrum monitored at 528 nm is in coincidence with that monitored 640 nm, demonstrating that energy transfer takes place from the tetrahedron Mn 2+ to t octahedron Mn 2+ . A similar energy transfer process of Mn 2+ has also been observed [Mn(dppeO2)3] − [MnBr4]. [38]. The crystal field strengths around Mn 2+ can be calculat according to the PLE spectrum. Here, the Racah parameter (B and C) and crystal fi strength (Dq) of Zn 2+ -doped and undoped samples are shown in Table S2. After dopi with Zn 2+ , the crystal field strength increases, which is due to the lattice contraction. We further monitored the PL evolution of hydrated PEA2Mn0.88Zn0.12Br4 at high te perature (140 °C) and dehydrated PEA2Mn0.88Zn0.12Br4 in different humidity environmen Upon heating, the intensity of the green PL peak increases significantly and the red em sion drops as time goes on ( Figure S6a). After heating for 12 s, the red emission complet disappears. Further prolonging the time to 20 s, the green emission drops as well. Hen the thermal treatment time should be 12-20 s. For the cooling process, the green-emitti PEA2Mn0.88Zn0.12Br4 was exposed to air with different humidity. The evolution of PL sp tra during the cooling process was contrary to the heating process. The correspondi response time is about 100 s at a relative humidity of 38% RH. It is worth noting that t response time is related to the humidity, which is extended at relatively lower humidi The corresponding color coordinates of color changing during the heating and cooli process are labeled and shown in Figures S6c,d. The heating-cooling cycle stability was further tested. As shown in Figure S7, t emission peak, intensity, and FWHM are well maintained after 60 heating-cooling cycl which is much better than the PEA2MnBr4 single crystal [40]. To further verify the prac cability of the PEA2Mn0.88Zn0.12Br4 film, a series of images were captured at different ti intervals. Here, the green channel and red channel of the images were extracted via Ima J software to study the change of color ( Figure 5). The color index (It) can be calculated the intensity of the red channel (It(R)) and green channel (It(G)) ( = (G)/ (R)+ (G Also, a time-dependence curve could be drawn according to the following equation −ln[(1− )/(1− 0)] = kt. Correspondingly, the change rates of the heating process and co ing process can be obtained, which are 0.025 min −1 and −0.006 min −1 , respectively. For t anti-countering application, the letters "H", "B", and "T" were successfully coated on t paper, which exhibited reversible changes in green and pink emissions during the heati and cooling process. As shown in Figure 6, the "H", "B", and "T" still exhibit a brig We further monitored the PL evolution of hydrated PEA 2 Mn 0.88 Zn 0.12 Br 4 at high temperature (140 • C) and dehydrated PEA 2 Mn 0.88 Zn 0.12 Br 4 in different humidity environments. Upon heating, the intensity of the green PL peak increases significantly and the red emission drops as time goes on ( Figure S6a). After heating for 12 s, the red emission completely disappears. Further prolonging the time to 20 s, the green emission drops as well. Hence, the thermal treatment time should be 12-20 s. For the cooling process, the green-emitting PEA 2 Mn 0.88 Zn 0.12 Br 4 was exposed to air with different humidity. The evolution of PL spectra during the cooling process was contrary to the heating process. The corresponding response time is about 100 s at a relative humidity of 38% RH. It is worth noting that the response time is related to the humidity, which is extended at relatively lower humidity. The corresponding color coordinates of color changing during the heating and cooling process are labeled and shown in Figure S6c,d.
The heating-cooling cycle stability was further tested. As shown in Figure S7, the emission peak, intensity, and FWHM are well maintained after 60 heating-cooling cycles, which is much better than the PEA 2 MnBr 4 single crystal [40]. To further verify the practicability of the PEA 2 Mn 0.88 Zn 0.12 Br 4 film, a series of images were captured at different time intervals. Here, the green channel and red channel of the images were extracted via Image J software to study the change of color ( Figure 5). The color index (I t ) can be calculated by the intensity of the red channel (I t (R)) and green channel (I t (G)) (I t = I t (G)/I t (R) + I t (G)). Also, a time-dependence curve could be drawn according to the following equation y = −ln[(1 − I t )/(1 − I t0 )] = kt. Correspondingly, the change rates of the heating process and cooling process can be obtained, which are 0.025 min −1 and −0.006 min −1 , respectively. For the anti-countering application, the letters "H", "B", and "T" were successfully coated on the paper, which exhibited reversible changes in green and pink emissions during the heating and cooling process. As shown in Figure 6, the "H", "B", and "T" still exhibit a bright green color at high temperature after 60 cycles, demonstrating excellent stability in the anti-counterfeiting application. green color at high temperature after 60 cycles, demonstrating excellent stability in the anti-counterfeiting application.  Based on the above analysis, the variable structure of PEA2MnBr4 can be attributed to its unique 0D structure. The isolated [MnBr4] 2− tetrahedron is vulnerable to the external environment. According to the hard and soft acids and bases (HSAB) principle, the O green color at high temperature after 60 cycles, demonstrating excellent stability in the anti-counterfeiting application.  Based on the above analysis, the variable structure of PEA2MnBr4 can be attributed to its unique 0D structure. The isolated [MnBr4] 2− tetrahedron is vulnerable to the external environment. According to the hard and soft acids and bases (HSAB) principle, the O Based on the above analysis, the variable structure of PEA 2 MnBr 4 can be attributed to its unique 0D structure. The isolated [MnBr 4 ] 2− tetrahedron is vulnerable to the external environment. According to the hard and soft acids and bases (HSAB) principle, the O belongs to a hard base while Mn 2+ is a hard acid. Hence, Mn 2+ ions prefer to bind to H 2 O to form the octahedron configuration. Because Pb-Br tends to form the octahedron structure, [PbBr 6 ] 4− has a strong inducement effect on the transformation of [MnBr 4 ] 2− . In order to acquire highly emitting and stable octahedron PEA 2 MnBr 4 , Pb 2+ doping was introduced. Firstly, Pb 2+ -doped PEA 2 Mn 0.88 Zn 0.12 Br 4 was synthesized in colloidal solution by introducing PbAc 2 into an Mn precursor. Although a bright orange emitting product can be acquired, the product is not uniform ( Figure S8a). XRD measurement was performed to identify the impurity. As shown in Figure S8b, these strong diffraction peaks at 14.0 • , 20.9 • , and 27.9 • can be indexed to PEA 2 ZnBr 4 (CCDC 258591), suggesting that phase separation takes place due to the different activity of the Pb 2+ , Mn 2+ and Zn 2+ ions. In order to address the activity issue, cation exchange reaction was performed. We have tried several different combinations (PEA 2 MnBr 4 and PEA 2 PbBr 4 , PEA 2 PbBr 4 and MnAc 2 , PEA 2 PbBr 4 and MnBr 2 , PEA 2 MnBr 4 and PbBr 2 ) ( Figure S9) and found that the PLQYs were not high except for the combination of PEA 2 Mn 0.88 Zn 0.12 Br 4 and PbBr 2 ( Figure S10). Hence, we have chosen the reaction of PEA 2 Mn 0.88 Zn 0.12 Br 4 and PbBr 2 to prepare PEA 2 Mn 0.88 Zn 0.12 Br 4 with different Pb-doping concentrations. The actual concentrations of Pb 2+ in the final products were determined by ICP and shown in Table S3. The PL spectra of PEA 2 Mn 0.88 Zn 0.12 Br 4 with different Pb 2+ -doping ratios are shown in Figure 7. The highest PL intensity is acquired at the Pb 2+ ratio of 9.1%. Actually, the PLQY of the product is as high as 85%. With the Pb 2+ ratio changed from 6.3% to 16.7%, the lifetime becomes longer, which is consistent with the PLQY result ( Figure S11). Firstly, Pb 2+ -doped PEA2Mn0.88Zn0.12Br4 was synthesized in colloidal solution by introducing PbAc2 into an Mn precursor. Although a bright orange emitting product can be acquired, the product is not uniform ( Figure S8a). XRD measurement was performed to identify the impurity. As shown in Figure S8b, these strong diffraction peaks at 14.0°, 20.9°, and 27.9° can be indexed to PEA2ZnBr4 (CCDC 258591), suggesting that phase separation takes place due to the different activity of the Pb 2+ , Mn 2+ and Zn 2+ ions. In order to address the activity issue, cation exchange reaction was performed. We have tried several different combinations (PEA2MnBr4 and PEA2PbBr4, PEA2PbBr4 and MnAc2, PEA2PbBr4 and MnBr2, PEA2MnBr4 and PbBr2) ( Figures S9) and found that the PLQYs were not high except for the combination of PEA2Mn0.88Zn0.12Br4 and PbBr2 ( Figure S10). Hence, we have chosen the reaction of PEA2Mn0.88Zn0.12Br4 and PbBr2 to prepare PEA2Mn0.88Zn0.12Br4 with different Pb-doping concentrations. The actual concentrations of Pb 2+ in the final products were determined by ICP and shown in Table S3. The PL spectra of PEA2Mn0.88Zn0.12Br4 with different Pb 2+ -doping ratios are shown in Figure 7. The highest PL intensity is acquired at the Pb 2+ ratio of 9.1%. Actually, the PLQY of the product is as high as 85%. With the Pb 2+ ratio changed from 6.3% to 16.7%, the lifetime becomes longer, which is consistent with the PLQY result ( Figure S11). PLE spectra were carried out to investigate the PL mechanism. As shown in Figure  7d, the energy levels of 4 T1(P) and 4 E(D) maintain at 6% substitution while energy levels of low energy excited states ( 4 A1, 4 E(D), 4 T2(G), 4 T1(G)) disappear. As the Pb 2+ concentration changes to 9.1%, the discrete energy levels of 4 T1(P) and 4 E(D) merge together and another peak located at 414 nm appears. According to previous studies [36,44], this newly PLE spectra were carried out to investigate the PL mechanism. As shown in Figure 7d, the energy levels of 4 T 1 (P) and 4 E(D) maintain at 6% substitution while energy levels of low energy excited states ( 4 A 1 , 4 E(D), 4 T 2 (G), 4 T 1 (G)) disappear. As the Pb 2+ concentration changes to 9.1%, the discrete energy levels of 4 T 1 (P) and 4 E(D) merge together and another peak located at 414 nm appears. According to previous studies [36,44], this newly appeared peak is assigned to the lead-halide units, indicating that the electronic structure of Pb 2+doped PEA 2 Mn 0.88 Zn 0.12 Br 4 is related to the interaction between [MnBr 6 ] 4− units and [PbBr 6 ] 4− units. Further increasing the Pb 2+ doping concentration, the intensity of the PLE peak decreases.
In order to investigate the effect of Pb 2+ doping on the structure of the products, XRD was carried out (Figure 8). At low-doping concentration (6.3-16.7%), all of the peaks are still in coincidence with the patterns of PEA 2 MnBr 4 and the diffraction peak positions shift to a smaller angle with the increasing doping concentration. Because the ionic radius of the Pb 2+ ion is larger than that of Mn 2+ , doping Pb 2+ ions leads to lattice expansion. As we discussed, the preservation of the PEA 2 MnBr 4 XRD pattern indicates that the content of the octahedron Mn 2+ is small. In addition, the intensities of several peaks (20.9 • , 22.4 • and 27.9 • ) decrease while the intensity of peaks located at 13.9 • , 20.8 • , and 27.8 • is nearly unchanged as the doping concentration increases. Combined with the above high-temperature XRD analysis, these unchanged peaks may belong to the octahedron Mn 2+ and these decreased peaks come from tetrahedron Mn 2+ . Further increasing to 66.7% substitution, PEA 2 PbBr 4 appears and pure PEA 2 PbBr 4 is acquired at 88.9% substitution. For PEA 2 PbBr 4 , the highest PLQY (3.2%) is obtained at 95.2% substitution (Figure 7a), which is much less than the Pb 2+ -doped PEA 2 Mn 0.88 Zn 0.12 Br 4 . FTIR was performed to study the influence of the Pb 2+ doping effect. As shown in Figure 8b, the peak belonging to the stretching vibration of H 2 O shifts from 3400 cm −1 to 3450 cm −1 after doping with Pb 2+ , demonstrating that its coordination environment changes. When PEA 2 Mn 0.88 Zn 0.12 Br 4 is exposed to air, H 2 O molecules can coordinate with Mn 2+ , changing the configuration of Mn 2+ from tetrahedron to octahedron. Due to this coordination, the electron cloud density of O reduces, leading to the decrease in the H-O bond strength. However, when Pb 2+ is introduced into the lattice, these unstable tetrahedrons Mn 2+ will transform to octahedrons Mn 2+ due to the inducive effect. In other words, the H 2 O molecules are no longer involved in the coordination of octahedron Mn 2+ . The chemical composition and electronic states of Pb 2+ -doped PEA 2 Mn 0.88 Zn 0.12 Br 4 were further studied by XPS. As shown in Figure S12 In order to explain the influence of the Pb 2+ doping effect, the photophysical process of Pb 2+ -doped PEA 2 Mn 0.88 Zn 0.12 Br 4 is depicted in Figure 9. The high PLQY of Pb 2+ -doped PEA 2 Mn 0.88 Zn 0.12 Br 4 is mainly caused by the following three aspects: 1. energy transfer paths are optimized from tetrahedron Mn 2+ to Pb 2+ then to octahedron Mn 2+ . 2. the removement of H 2 O reduces the nonradiative recombination, forming perfect [MnBr 6 ] 4− . 3. Pb 2+ doping inhibits the concentration quenching of Mn 2+ . As we discussed, the content of the [MnBr 6 ] 4− is low in Pb 2+ -doped PEA 2 Mn 0.88 Zn 0.12 Br 4 when the Pb 2+ doping ratio is below 20%, but intense orange emission belonging to octahedron Mn 2+ is observed. This can be understood by the PLE results. Both the red emission and green emission possess the same PLE spectrum, demonstrating that energy transfer occurs from tetrahedron Mn 2+ to octahedron Mn 2+ . Interestingly, the discrete energy levels of 4 T 1 (P) and 4 E(D) become merged together as the Pb 2+ concentration increases. According to the previous study [44], a quasi-continuous conduction band can be formed and spin-forbidden transition is further broken due to the merge of high energy states, which have less constraint on electron transitions, leading to increasement of the density of excitons in excited states. Besides, the transition of lead-halide units is also found in the PLE spectrum, which is placed under the energy levels of 4 T 1 (P) and 4 E(D). This newly appeared energy level of lead-halide precludes the energy absorption and transfer of the low energy states ( 4 A 1 , 4 E(D), 4 T 2 (G), 4 T 1 (G)) and directly transfers the energy to the 4 T 1 (G). It is well known that H 2 O could easily introduce de-excitation channels for the excited state, causing severe PL decay. The removal of H 2 O can reduce the nonradiative recombination process, leading to effective radiative recombination. In addition, Pb/Mn alloying also dilutes the Mn 2+ concentration, inhibiting the concentration quenching of Mn 2+ . All these factors optimize the energy transfer path and increase the density of excitons, thus leading to high PLQY. In order to explain the influence of the Pb 2+ doping effect, the photophysical process of Pb 2+ -doped PEA2Mn0.88Zn0.12Br4 is depicted in Figure 9. The high PLQY of Pb 2+ -doped PEA2Mn0.88Zn0.12Br4 is mainly caused by the following three aspects: 1. energy transfer paths are optimized from tetrahedron Mn 2+ to Pb 2+ then to octahedron Mn 2+ . 2. the removement of H2O reduces the nonradiative recombination, forming perfect [MnBr6] 4− . 3. Pb 2+ doping inhibits the concentration quenching of Mn 2+ . As we discussed, the content of the [MnBr6] 4− is low in Pb 2+ -doped PEA2Mn0.88Zn0.12Br4 when the Pb 2+ doping ratio is below 20%, but intense orange emission belonging to octahedron Mn 2+ is observed. This can be understood by the PLE results. Both the red emission and green emission possess the same PLE spectrum, demonstrating that energy transfer occurs from tetrahedron Mn 2+ to octahedron Mn 2+ . Interestingly, the discrete energy levels of 4 T1(P) and 4 E(D) become merged together as the Pb 2+ concentration increases. According to the previous study [44], a quasicontinuous conduction band can be formed and spin-forbidden transition is further broken due to the merge of high energy states, which have less constraint on electron transitions, leading to increasement of the density of excitons in excited states. Besides, the transition of lead-halide units is also found in the PLE spectrum, which is placed under the energy levels of 4 T1(P) and 4 E(D). This newly appeared energy level of lead-halide precludes the energy absorption and transfer of the low energy states ( 4 A1, 4 E(D), 4 T2(G), 4 T1(G)) and directly transfers the energy to the 4 T1(G). It is well known that H2O could easily introduce de-excitation channels for the excited state, causing severe PL decay. The removal of H2O can reduce the nonradiative recombination process, leading to effective radiative recombination. In addition, Pb/Mn alloying also dilutes the Mn 2+ concentration, inhibiting the concentration quenching of Mn 2+ . All these factors optimize the energy transfer path and increase the density of excitons, thus leading to high PLQY. We have also studied the stability of the Pb 2+ -doped PEA2Mn0.88Zn0.12Br4. To our surprise, Pb 2+ -doped PEA2Mn0.88Zn0.12Br4 show excellent stability under the ambient environment, which still possesses 80% of the original PL intensity after 25 days. However, the thermal stability is totally different from the PEA2Mn0.88Zn0.12Br4. As shown in Figure S13, the PL intensity decreases sharply as the temperature increases, which is common in luminescent semiconductors. For example, the PL intensity only retains 20% of the original after heating the sample to 160 °C. The different fluorescent temperature-dependencies of PEA2Mn0.88Zn0.12Br4 and Pb 2+ -doped PEA2Mn0.88Zn0.12Br4 offer great opportunities for information encryption. Multilayer fluorescent composite films were fabricated for the application of information encryption. As shown in Figure 10, patterns of bird, rabbit, and butterfly composed of PEA2Mn0.88Zn0.12Br4 layer are screen printed on a substrate. After that, the Pb 2+ -doped PEA2Mn0.88Zn0.12Br4 solution is spin-coated on the surface of the PEA2Mn0.88Zn0.12Br4 layer to form a uniform film. The composite film exhibits strong or- We have also studied the stability of the Pb 2+ -doped PEA 2 Mn 0.88 Zn 0.12 Br 4 . To our surprise, Pb 2+ -doped PEA 2 Mn 0.88 Zn 0.12 Br 4 show excellent stability under the ambient environment, which still possesses 80% of the original PL intensity after 25 days. However, the thermal stability is totally different from the PEA 2 Mn 0.88 Zn 0.12 Br 4 . As shown in Figure S13, the PL intensity decreases sharply as the temperature increases, which is common in luminescent semiconductors. For example, the PL intensity only retains 20% of the original after heating the sample to 160 • C. The different fluorescent temperature-dependencies of PEA 2 Mn 0.88 Zn 0.12 Br 4 and Pb 2+ -doped PEA 2 Mn 0.88 Zn 0.12 Br 4 offer great opportunities for information encryption. Multilayer fluorescent composite films were fabricated for the application of information encryption. As shown in Figure 10, patterns of bird, rabbit, and butterfly composed of PEA 2 Mn 0.88 Zn 0.12 Br 4 layer are screen printed on a substrate. After that, the Pb 2+ -doped PEA 2 Mn 0.88 Zn 0.12 Br 4 solution is spin-coated on the surface of the PEA 2 Mn 0.88 Zn 0.12 Br 4 layer to form a uniform film. The composite film exhibits strong orange emission under UV light at room temperature. When the temperature increases from 20 to 160 • C, the orange emission upper film gradually decreases and the patterns of the bird, rabbit, and butterfly with green emission appear. Finally, when the composite film is heated at 160 • C for 5 s, clear patterns of bird, rabbit, and butterfly are observed. Therefore, in this multilayer composite, the encrypted information can be read out by using a simple heating treatment. Besides, such color-changing PL behaviors can be repeated more than 10 times ( Figure S14), demonstrating excellent cycle performance. This indicates that these luminescent materials can be used in document security. At room temperature the information is concealed. When we want to read the information, we can simply heat the document using a hair dryer. After the document cools to room temperature, the information can be hidden again.

Conclusions
In summary, we have fabricated Zn 2+ -doped PEA2MnBr4 and Pb 2+ -doped PEA2Mn0.88Zn0.12Br4, which possess different PL properties. For PEA2Mn0.88Zn0.12Br4, the reversible structural transformation was responsible for the color-changing phenomenon, which was due to the desorption and absorption of coordinating water. Anti-counterfeiting labels and trademarks have been constructed by taking advantage of this property, which exhibited excellent "pink-green-pink" cycle capability. Pb 2+ -doped PEA2Mn0.88Zn0.12Br4 was synthesized by the cation exchange reaction, which possessed high-efficiency orange emission. Compared to PEA2Mn0.88Zn0.12Br4, the Pb 2+ -doped PEA2Mn0.88Zn0.12Br4 was stable in the air, but its PL intensity decreased with the increase in temperature. Multilayer fluorescent composite films were fabricated by spin-coating of Pb 2+ -doped PEA2Mn0.88Zn0.12Br4 with strong orange emission onto the PEA2Mn0.88Zn0.12Br4 with weak pink emission, where the information was recorded onto the PEA2Mn0.88Zn0.12Br4 film. The encrypted information could be read out by using a simple heating treatment. In addition, the composite films showed excellent cycle stability.

Conclusions
In summary, we have fabricated Zn 2+ -doped PEA 2 MnBr 4 and Pb 2+ -doped PEA 2 Mn 0.88 Zn 0.12 Br 4 , which possess different PL properties. For PEA 2 Mn 0.88 Zn 0.12 Br 4 , the reversible structural transformation was responsible for the color-changing phenomenon, which was due to the desorption and absorption of coordinating water. Anti-counterfeiting labels and trademarks have been constructed by taking advantage of this property, which exhibited excellent "pink-green-pink" cycle capability. Pb 2+ -doped PEA 2 Mn 0.88 Zn 0.12 Br 4 was synthesized by the cation exchange reaction, which possessed high-efficiency orange emission. Compared to PEA 2 Mn 0.88 Zn 0.12 Br 4 , the Pb 2+ -doped PEA 2 Mn 0.88 Zn 0.12 Br 4 was stable in the air, but its PL intensity decreased with the increase in temperature. Multilayer fluorescent composite films were fabricated by spin-coating of Pb 2+ -doped PEA 2 Mn 0.88 Zn 0.12 Br 4 with strong orange emission onto the PEA 2 Mn 0.88 Zn 0.12 Br 4 with weak pink emission, where the information was recorded onto the PEA 2 Mn 0.88 Zn 0.12 Br 4 film. The encrypted information could be read out by using a simple heating treatment. In addition, the composite films showed excellent cycle stability.

Data Availability Statement:
The data related with this work are not publicly available but can be obtained upon reasonable request from the corresponding author.

Conflicts of Interest:
The authors declare no conflict of interest.