# Controlled Synthesis of Water-Soluble NaYF4:Yb3+, Er3+ Nanoparticles with Surfactant Dependent Properties

Authors: Junwei Zhao; Tiekun Jia; Xiaofeng Wang; Xianggui Kong
Journal: Journal of Nanomaterials
 (2014)

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## Abstract

Water-soluble NaYF4:Yb3+, Er3+ nanoparticles (NPs) are successfully prepared by a solvothermal reaction using branched polyethylenimine (PEI) with different chain lengths as the surfactants in a water/diethylene glycol (DEG) mixed solution. It is shown that the size of NaYF4 NPs prepared with high molecular weight PEI (HPEI) is smaller than that of the NPs prepared with low molecular weight (LPEI), while small-sized NPs exhibit more intense upconversion luminescence intensities than large-sized NPs in the same excitation power of 980 nm. It is found that HPEI is conducive to the formation of smaller NP with high crystallinity. Small-sized NaYF4:Yb3+, Er3+ NPs with intense upconversion luminescence and improved crystallinity were related to their growth process. A possible growth mechanism of the samples is proposed. The results of this study can provide new insights into the controlled synthesis of novel NPs.


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## Body

## 1. Introduction

In recent years, the upconversion luminescence of rare-earth fluoride NPs has attracted great research interest of the research groups in the world due to their potential applications in various fields, such as photodetectors and fluorescent labels or imaging probes [1–7]. Compared with downconversion fluorescent nanomaterials, upconversion luminescence NPs have many conceivable advantages in the field of biomedicine [8–10]. The upconversion luminescence nanomaterials have achieved considerable results, but many biomedicine experiments are still proof of concept [11]. In order to carry out their widespread application in biomedical fields, the upconversion luminescence NPs should be small enough and water soluble and exhibit high fluorescent intensity. Synthesis of upconversion luminescence nanomaterials with high crystal quality, uniform particle size distribution, and adjustable spectrum is still a challenge. Fluoride matrix materials show some unique advantages because of their low phonon frequencies observed in the crystal lattice [12]. Rare-earth ion-doped fluoride under 980 nm near-infrared (NIR) excitation can reduce the multiphonon relaxation process; thereby activating ions have a long-lived excited state, improving the luminescence intensity of the materials. So far, NaYF4 has been considered the most effective matrix for upconversion luminescence [3, 12]. Therefore, it is important to develop efficient and convenient methods to synthesize NaYF4:Yb, Er NPs with high quality and monodispersion for various biomedical applications.Over the past few years, many research groups have made great efforts to explore the feasible synthesis methods of upconversion luminescence NPs. Many chemical synthesis technologies, including coprecipitation [13–15], thermal decomposition [16–18], and hydrothermal synthesis [19, 20], have been demonstrated to synthesize lanthanide-doped upconversion luminescence NPs. However, most of these synthesized methods of NPs are in an organic solvent or at high temperature and usually require heat after treatment or produce toxic byproducts [1]. In our previous work, we have used ethylenediaminetetraacetic acid disodium salt (EDTA) and sodium citrate as the surfactants to synthesize NaYF4 NPs [21, 22]; however, these NPs are difficult to disperse in water for a long time due to the lack of sufficient hydrophilic groups on the NP surface.In this work, water-soluble NaYF4:Yb3+, Er3+ NPs are successfully prepared via a solvothermal method using branched PEI with different chain lengths as the surfactants. The influence of surfactant chain length on the size, crystallinity, and upconversion luminescence of NaYF4:Yb3+, Er3+ NPs was discussed in detail. All the obtained NPs exhibit strong upconversion fluorescence under 980 nm excitation. A possible growth mechanism of the samples is proposed. These nanocrystals have great potential for use in biology and medicine as fluorescent labels or imaging probes.


## 2. Experimental Section

### 2.1. Materials

All reagents were of analytical grade. Ln(NO3)3·6H2O (Ln = Y, Yb, and Er) stock solution was freshly prepared by the reaction of Ln2O3 with dilute nitric acid. Deionized water was prepared using a Millipore Milli-Q Purification System; its resistivity is more than 18.2 MΩ. The different molecular weight PEI polymers were purchased from Sigma-Aldrich. The molecular structure of PEI is shown in Figure 1. PEI stock solution (5 wt%) was prepared by diluted PEI with deionized water.Figure 1
The molecular structure of branched PEI.


### 2.2. Synthesis of Water-Soluble NaYF4:Yb3+, Er3+ NPs

In a typical procedure for the preparation of NaYF4: 20 mol% Yb3+, 2 mol% Er3+ NPs, a PEI solution (5 mL, 5 wt%) was added to a mixture of Ln(NO3)3·6H2O aqueous solution (2.5 mL, 0.2 mol/L, lanthanide ion molar ratio, and Y/Yb/Er = 78 : 20 : 2), NaCl aqueous solution (2.5 mL, 0.2 mol/L), and DEG (20 mL) with vigorous stirring for 1 h. An aqueous solution of NH4F was then added slowly to the above mixture with vigorous stirring for 1 h and the pH value of the system was adjusted to 7.5 using NaOH and HCl solutions. Then the prepared precursor solution was transferred to a 50 mL autoclave with polytetrafluoroethylene lining. The reaction autoclave was placed in a digital type heating furnace to heat to 180°C temperature and maintained at the temperature for several hours before natural cooling to room temperature. Finally, NaYF4:Yb3+, Er3+ precipitation can be separated out by centrifugation (6500 rpm, 10 min). The separated precipitation was washed with deionized water and ethanol for three times, respectively. The obtained NaYF4:Yb3+, Er3+ NPs were dried in vacuum at 60°C for 24 hours.


### 2.3. Characterization

The structure and morphology of NaYF4:Yb3+, Er3+ NPs were characterized by means of X-ray powder diffractometer (XRD), scanning electron microscopy (SEM, Hitachi, S-4800), and the Fourier transform infrared (FT-IR) spectra (Perkin-Elmer 580B infrared spectrophotometer). The operation voltage and the current of a Brucker D8-advance X-ray diffractometer with CuKα radiation (λ = 1.5418 Å) when testing the samples were 40 kV and 40 mA, respectively. The 2θ angle ranges from 15 to 60° with step of 0.021 and counting time of 0.2 s. All parameters during XRD data collection were kept constant. The upconversion emission spectra of NaYF4:Yb3+, Er3+ phosphors were acquired using a Jobin-Yvon LabRam Raman spectrometer system equipped with 1800 and 600 grooves/mm holographic gratings, respectively, and a Peltier air-cooled CCD detector. The dry powder samples were excited by a CW semiconductor diode laser at 980 nm. The maximal excitation power used in the experiment was about 760 mW with a focusing area of about 0.03 mm2. The upconversion luminescence spectra were measured under identical conditions in order to compare their relative emission intensities.


## 2.1. Materials

All reagents were of analytical grade. Ln(NO3)3·6H2O (Ln = Y, Yb, and Er) stock solution was freshly prepared by the reaction of Ln2O3 with dilute nitric acid. Deionized water was prepared using a Millipore Milli-Q Purification System; its resistivity is more than 18.2 MΩ. The different molecular weight PEI polymers were purchased from Sigma-Aldrich. The molecular structure of PEI is shown in Figure 1. PEI stock solution (5 wt%) was prepared by diluted PEI with deionized water.Figure 1
The molecular structure of branched PEI.


## 2.2. Synthesis of Water-Soluble NaYF4:Yb3+, Er3+ NPs

In a typical procedure for the preparation of NaYF4: 20 mol% Yb3+, 2 mol% Er3+ NPs, a PEI solution (5 mL, 5 wt%) was added to a mixture of Ln(NO3)3·6H2O aqueous solution (2.5 mL, 0.2 mol/L, lanthanide ion molar ratio, and Y/Yb/Er = 78 : 20 : 2), NaCl aqueous solution (2.5 mL, 0.2 mol/L), and DEG (20 mL) with vigorous stirring for 1 h. An aqueous solution of NH4F was then added slowly to the above mixture with vigorous stirring for 1 h and the pH value of the system was adjusted to 7.5 using NaOH and HCl solutions. Then the prepared precursor solution was transferred to a 50 mL autoclave with polytetrafluoroethylene lining. The reaction autoclave was placed in a digital type heating furnace to heat to 180°C temperature and maintained at the temperature for several hours before natural cooling to room temperature. Finally, NaYF4:Yb3+, Er3+ precipitation can be separated out by centrifugation (6500 rpm, 10 min). The separated precipitation was washed with deionized water and ethanol for three times, respectively. The obtained NaYF4:Yb3+, Er3+ NPs were dried in vacuum at 60°C for 24 hours.


## 2.3. Characterization

The structure and morphology of NaYF4:Yb3+, Er3+ NPs were characterized by means of X-ray powder diffractometer (XRD), scanning electron microscopy (SEM, Hitachi, S-4800), and the Fourier transform infrared (FT-IR) spectra (Perkin-Elmer 580B infrared spectrophotometer). The operation voltage and the current of a Brucker D8-advance X-ray diffractometer with CuKα radiation (λ = 1.5418 Å) when testing the samples were 40 kV and 40 mA, respectively. The 2θ angle ranges from 15 to 60° with step of 0.021 and counting time of 0.2 s. All parameters during XRD data collection were kept constant. The upconversion emission spectra of NaYF4:Yb3+, Er3+ phosphors were acquired using a Jobin-Yvon LabRam Raman spectrometer system equipped with 1800 and 600 grooves/mm holographic gratings, respectively, and a Peltier air-cooled CCD detector. The dry powder samples were excited by a CW semiconductor diode laser at 980 nm. The maximal excitation power used in the experiment was about 760 mW with a focusing area of about 0.03 mm2. The upconversion luminescence spectra were measured under identical conditions in order to compare their relative emission intensities.


## 3. Results and Discussion

### 3.1. Structure and Morphology

In order to study the molecular weight of PEI on the effect of sample, we on purpose synthesized four samples using different synthetic conditions. The synthetic conditions and characteristics of samples prepared via the solvothermal route are listed in Table1. The structure and crystallinity of the products were characterized by XRD. Figure 2 shows the XRD patterns of the NaYF4: 20 mol% Yb3+, 2 mol% Er3+ NPs prepared with different solvothermal time using HPEI and LPEI, respectively. As can be seen from Figure 2, all diffraction peaks of the four samples coincide with the standard face-centered cubic structure data (JCPDS card number 77-2042). No additional diffractions of impurities are observed. Assuming a homogeneous strain across crystallites, the average size of microcrystallites can be estimated from the full width half maximum (FWHM) values of diffraction peaks using the Debye-Scherrer formula [23]. The average sizes of the samples L1, L2, H1, and H2 are 58 nm, 64 nm, 40 nm, and 45 nm, respectively. The diffraction peaks of the as-prepared samples show different intensity. After treatment of the precursors under the same solvothermal conditions, the intensity of the XRD diffractograms of the NPs synthesized with HPEI is stronger and the particle size is smaller, compared with that of the NPs synthesized with LPEI. The different intensity of the XRD diffractograms of the four samples should be related to their different crystallinity. This is similar to the results previously published for synthesis of anatase Titania using the hydrothermal technique [24].Table 1
The synthesis conditions and characteristics of the samples prepared via the solvothermal method.
Sample number
Molecular weight
Solvothermal time (h)
Sample size (nm)
L1
2000
3 h
58 nm
L2
2000
5 h
64 nm
H1
25000
3 h
40 nm
H2
25000
5 h
45 nmFigure 2
XRD patterns of the as-prepared samples. All the samples are prepared under the conditions according to Table1.Figure3 shows the SEM images of the NaYF4: 20 mol% Yb3+, 2 mol% Er3+ NPs prepared according to the synthesis conditions in Table 1. As can be seen from Figure 3, the NPs synthesized with LPEI exhibited a spherical shape with an average size of about 60 nm. The NPs exhibit rough surface and nonuniform size distribution (see Figures 3(a) and 3(b)), which represent a low degree of crystallinity [21]. On using HPEI, the size of the obtained NPs with regular shape and uniform size is about 42 nm. When the solvothermal time reached 5 h, the crystallinity of the NaYF4 NPs was further improved, as evidenced by the more regular shape and the smoother surface (see Figure 3(d)). Moreover, the size of the NPs prepared with HPEI is smaller than that of the NPs prepared with LPEI via the same solvothermal treatment process. The average size estimated from the SEM images is in agreement with the estimated value from the XRD patterns. The XRD spectrum data and the SEM image data complement each other well.SEM images of the NaYF4: 20 mol% Yb3+, 2 mol% Er3+ NPs prepared under different conditions: (a) LPEI, 3 h; (b) LPEI, 5 h; (c) HPEI, 3 h; (d) HPEI, 5 h.
(a)
(b)
(c)
(d)Figure4 shows the FT-IR spectra of the NaYF4:Yb3+, Er3+ NPs. The strong absorption bands at 3500 and 3300 cm−1 of the NaYF4:Yb3+, Er3+ NPs are the result of the NH vibrations [25]. The weak absorption bands of 2928 and 2853 cm−1 result from the asymmetrical and symmetrical stretching vibration of the CH2 groups, respectively [26]. The absorption bands of 1650 and 1550 cm−1 are attributed to in-plane vibrations of the NH bonds [25]. The peaks at about 1450 cm−1 arised from vibrations of the C–C groups [26]. The presence of free amine groups on the surface of the nanoparticles is of extreme importance since these can bond with the ligand molecule (e.g., antibody) necessary for additional functionalization of the nanoparticle. The obtained NPs can be dispersed in water for two weeks without obvious precipitation due to the presence of sufficient hydrophilic groups on the NP surface (see Figure 5).Figure 4
FT-IR spectra of the NaYF4:Yb3+, Er3+ NPs.Figure 5
The photographs of the as-prepared NaYF4:Yb3+, Er3+/Tm3+ NPs (sample H2) dispersed in aqueous solution under white light and 980 nm excitation.


### 3.2. Possible Growth Mechanism

As discussed above, the size of the NaYF4 NPs synthesized with HPEI is smaller than that of the NPs synthesized with LPEI under the same solvothermal conditions. This can be understood from the growth mechanism of crystals. The process of precipitation from a liquid phase to a solid phase is inevitable when using wet chemical synthesis of bulk and NPs [27]. The formation process of NPs includes the production of the nucleation, growth, and final shaping. Therefore, in order to understand the intrinsic factors which influence the size of NPs, it is needed to start studying nucleation mechanism of NPs. For a solute, any solution has certain solubility; thereby the excess solute will inevitably lead to the occurrence of the precipitation and formation of a crystal in solution. Therefore, to obtain the NPs in solution, the solute must reach supersaturation and then the nucleation occurs. The nucleation rate is one of the key factors to determine the size of NPs. The high nucleation rate is conducive to the formation of small-sized NPs because their subsequent growth process can be hindered by the solution since the rapid nucleation consumes more reactants [21, 24]. In our case, the PEI-Ln complex in the initial stage begins to form; the incorporation of anions into the PEI-Ln complex has a significant effect on nucleation rate. In the nucleation stage the Ln ions which are released slowly from the PEI-Ln complex reacted with F anions, transferring them into the NaYF4 crystal nucleuses. In our previous report, we have reported the effect of the difference of chelate constant between EDTA and sodium citrate on the nucleation rate and then the size of NPs [21]. However, the chelate constant or chelating ability of PEI is almost not influenced by the degree of polymerization [28]. In this work, the PEI surfactants with different chain lengths are composed of the same monomer. Therefore, the nucleation rate is almost the same since the weight percentage of HPEI in precursors is the same as that of LPEI. In other words, the effect of the nucleation rate was not the determinant of the size difference of the as-prepared NPs. The particle growth stages followed the nucleation process. When the solute concentration decreased to a critical level, the nucleation process is stopped and the particles continue to grow by adding the reactive ions until reaching a new equilibrium concentration of the precipitated species [27]. In the growth stage, crystal nuclei are to form the primary particles which serve as growth center of NPs [21]. The ions that continually diffuse to the surface of the growing crystal, subsequently, incorporate into the lattice structure. Therefore, the diffusion rate of ions is another key factor to control the size and shape of the growing crystal. In water/DEG solution, the diffusion rate of the ions was slow due to the high viscosity of DEG. It is a reason for the synthesis of small-sized NPs. However, the influence of water/DEG solution is almost exactly the same for the four samples because of the same solvent. On the other hand, it is more important that PEI molecules as chelating ligands were bonded with rare-earth ions to form the PEI-Ln complex which reduced the diffusion rate of cations in solution to deposit on crystal surfaces. The later conditions make the size difference possible during the growth of NPs. It is well known that the degree of polymerization of HPEI is higher than that of LPEI. The chain length of the HPEI like a tail is longer than that of LPEI. Therefore, the diffusion rate of the cations bound to HPEI molecules in solution is slower than that of the cations bound to LPEI molecules, with the result that the growth rate of the NaYF4 NPs prepared with HPEI is slower than that of the NPs prepared with LPEI. Finally, the size of NaYF4 NPs prepared with HPEI is smaller than that of the NPs prepared with LPEI. As we all know, ideal perfect crystals with well crystallinity would grow exceedingly slowly. That would be difficult to achieve since real crystals always have relatively few disruptions in their lattice structure. The only thing we can do is to reduce the crystallite defects to improve the crystal quality. During the growth stage, the slower the diffusion rate of ions is, the better the crystallinity is. Therefore, in this work the reason that the crystallinity of small-sized NaYF4 seems to be higher than that of the biggest ones under the same solvothermal conditions is the slow growth rate of them.In addition, the size of the as-prepared NPs is increasing with increasing solvothermal time when using the same molecular weight PEI molecules. It is reported that temperature has a certain influence on the stability of crystal nucleus [29]. As the crystal nucleus stability decreases, the nucleation rate of nonoxide crystals decreases with increasing the temperature [29]. As discussed above, the low nucleation rate leads to the increasing size of NPs. This is the reason that the particle size of obtained NaYF4 NPs was increased with increasing the temperature.


### 3.3. Upconversion Photoluminescence of the NaYF4:Yb3+, Er3+ NPs

Figure6 shows the upconversion photoluminescence spectra of the four dry powder samples prepared with different solvothermal conditions according to Table 1. Several distinct green and red emission bands centered at 520, 540, and 650 nm were observed. The green and red emission bands could be assigned to (2H11/2, 4S3/2) → 4I15/2 and 4F9/2 → 4I15/2 transitions of the Er3+ ions in the NaYF4 NPs, respectively. In spite of the degree of polymerization of PEI, the relative upconversion luminescence intensity of samples under solvothermal treatment for 5 h is higher than that of samples under solvothermal treatment for 3 h, which is similar to the previous report [22]. Surprisingly, the upconversion luminescence intensity of the small-sized NaYF4:Yb3+, Er3+ NPs prepared with HPEI is stronger than that of the large-sized NaYF4:Yb3+, Er3+ NPs prepared with LPEI undergoing the same solvothermal treatment process. The observed phenomena are opposite to the common phenomenon. Generally, the NPs with large size exhibit the strong luminescence due to the reduced nonradiative relaxation [22, 30]. This opposite phenomenon in this research is probably related to the difference between HPEI and LPEI. The luminescence difference of samples prepared by different precursors has been reported in previous work [31, 32]. As discussed above, the PEI ligands influence the growth processes of the NPs. The difference in the chain length of PEI leads to a different diffusion rate. Therefore, it is suggested that the samples with the smallest size particle probably have the higher crystallinity because they exhibit the highest relative emission intensity.Figure 6
Upconversion luminescence spectra of the dried power NaYF4:Yb3+, Er3+ samples prepared with different solvothermal conditions according to Table 1 (λex = 980 nm, power = 760 mW): (a) LPEI, 3 h; (b) LPEI, 5 h; (c) HPEI, 3 h; (d) HPEI, 5 h.


## 3.1. Structure and Morphology

In order to study the molecular weight of PEI on the effect of sample, we on purpose synthesized four samples using different synthetic conditions. The synthetic conditions and characteristics of samples prepared via the solvothermal route are listed in Table1. The structure and crystallinity of the products were characterized by XRD. Figure 2 shows the XRD patterns of the NaYF4: 20 mol% Yb3+, 2 mol% Er3+ NPs prepared with different solvothermal time using HPEI and LPEI, respectively. As can be seen from Figure 2, all diffraction peaks of the four samples coincide with the standard face-centered cubic structure data (JCPDS card number 77-2042). No additional diffractions of impurities are observed. Assuming a homogeneous strain across crystallites, the average size of microcrystallites can be estimated from the full width half maximum (FWHM) values of diffraction peaks using the Debye-Scherrer formula [23]. The average sizes of the samples L1, L2, H1, and H2 are 58 nm, 64 nm, 40 nm, and 45 nm, respectively. The diffraction peaks of the as-prepared samples show different intensity. After treatment of the precursors under the same solvothermal conditions, the intensity of the XRD diffractograms of the NPs synthesized with HPEI is stronger and the particle size is smaller, compared with that of the NPs synthesized with LPEI. The different intensity of the XRD diffractograms of the four samples should be related to their different crystallinity. This is similar to the results previously published for synthesis of anatase Titania using the hydrothermal technique [24].Table 1
The synthesis conditions and characteristics of the samples prepared via the solvothermal method.
Sample number
Molecular weight
Solvothermal time (h)
Sample size (nm)
L1
2000
3 h
58 nm
L2
2000
5 h
64 nm
H1
25000
3 h
40 nm
H2
25000
5 h
45 nmFigure 2
XRD patterns of the as-prepared samples. All the samples are prepared under the conditions according to Table1.Figure3 shows the SEM images of the NaYF4: 20 mol% Yb3+, 2 mol% Er3+ NPs prepared according to the synthesis conditions in Table 1. As can be seen from Figure 3, the NPs synthesized with LPEI exhibited a spherical shape with an average size of about 60 nm. The NPs exhibit rough surface and nonuniform size distribution (see Figures 3(a) and 3(b)), which represent a low degree of crystallinity [21]. On using HPEI, the size of the obtained NPs with regular shape and uniform size is about 42 nm. When the solvothermal time reached 5 h, the crystallinity of the NaYF4 NPs was further improved, as evidenced by the more regular shape and the smoother surface (see Figure 3(d)). Moreover, the size of the NPs prepared with HPEI is smaller than that of the NPs prepared with LPEI via the same solvothermal treatment process. The average size estimated from the SEM images is in agreement with the estimated value from the XRD patterns. The XRD spectrum data and the SEM image data complement each other well.SEM images of the NaYF4: 20 mol% Yb3+, 2 mol% Er3+ NPs prepared under different conditions: (a) LPEI, 3 h; (b) LPEI, 5 h; (c) HPEI, 3 h; (d) HPEI, 5 h.
(a)
(b)
(c)
(d)Figure4 shows the FT-IR spectra of the NaYF4:Yb3+, Er3+ NPs. The strong absorption bands at 3500 and 3300 cm−1 of the NaYF4:Yb3+, Er3+ NPs are the result of the NH vibrations [25]. The weak absorption bands of 2928 and 2853 cm−1 result from the asymmetrical and symmetrical stretching vibration of the CH2 groups, respectively [26]. The absorption bands of 1650 and 1550 cm−1 are attributed to in-plane vibrations of the NH bonds [25]. The peaks at about 1450 cm−1 arised from vibrations of the C–C groups [26]. The presence of free amine groups on the surface of the nanoparticles is of extreme importance since these can bond with the ligand molecule (e.g., antibody) necessary for additional functionalization of the nanoparticle. The obtained NPs can be dispersed in water for two weeks without obvious precipitation due to the presence of sufficient hydrophilic groups on the NP surface (see Figure 5).Figure 4
FT-IR spectra of the NaYF4:Yb3+, Er3+ NPs.Figure 5
The photographs of the as-prepared NaYF4:Yb3+, Er3+/Tm3+ NPs (sample H2) dispersed in aqueous solution under white light and 980 nm excitation.


## 3.2. Possible Growth Mechanism

As discussed above, the size of the NaYF4 NPs synthesized with HPEI is smaller than that of the NPs synthesized with LPEI under the same solvothermal conditions. This can be understood from the growth mechanism of crystals. The process of precipitation from a liquid phase to a solid phase is inevitable when using wet chemical synthesis of bulk and NPs [27]. The formation process of NPs includes the production of the nucleation, growth, and final shaping. Therefore, in order to understand the intrinsic factors which influence the size of NPs, it is needed to start studying nucleation mechanism of NPs. For a solute, any solution has certain solubility; thereby the excess solute will inevitably lead to the occurrence of the precipitation and formation of a crystal in solution. Therefore, to obtain the NPs in solution, the solute must reach supersaturation and then the nucleation occurs. The nucleation rate is one of the key factors to determine the size of NPs. The high nucleation rate is conducive to the formation of small-sized NPs because their subsequent growth process can be hindered by the solution since the rapid nucleation consumes more reactants [21, 24]. In our case, the PEI-Ln complex in the initial stage begins to form; the incorporation of anions into the PEI-Ln complex has a significant effect on nucleation rate. In the nucleation stage the Ln ions which are released slowly from the PEI-Ln complex reacted with F anions, transferring them into the NaYF4 crystal nucleuses. In our previous report, we have reported the effect of the difference of chelate constant between EDTA and sodium citrate on the nucleation rate and then the size of NPs [21]. However, the chelate constant or chelating ability of PEI is almost not influenced by the degree of polymerization [28]. In this work, the PEI surfactants with different chain lengths are composed of the same monomer. Therefore, the nucleation rate is almost the same since the weight percentage of HPEI in precursors is the same as that of LPEI. In other words, the effect of the nucleation rate was not the determinant of the size difference of the as-prepared NPs. The particle growth stages followed the nucleation process. When the solute concentration decreased to a critical level, the nucleation process is stopped and the particles continue to grow by adding the reactive ions until reaching a new equilibrium concentration of the precipitated species [27]. In the growth stage, crystal nuclei are to form the primary particles which serve as growth center of NPs [21]. The ions that continually diffuse to the surface of the growing crystal, subsequently, incorporate into the lattice structure. Therefore, the diffusion rate of ions is another key factor to control the size and shape of the growing crystal. In water/DEG solution, the diffusion rate of the ions was slow due to the high viscosity of DEG. It is a reason for the synthesis of small-sized NPs. However, the influence of water/DEG solution is almost exactly the same for the four samples because of the same solvent. On the other hand, it is more important that PEI molecules as chelating ligands were bonded with rare-earth ions to form the PEI-Ln complex which reduced the diffusion rate of cations in solution to deposit on crystal surfaces. The later conditions make the size difference possible during the growth of NPs. It is well known that the degree of polymerization of HPEI is higher than that of LPEI. The chain length of the HPEI like a tail is longer than that of LPEI. Therefore, the diffusion rate of the cations bound to HPEI molecules in solution is slower than that of the cations bound to LPEI molecules, with the result that the growth rate of the NaYF4 NPs prepared with HPEI is slower than that of the NPs prepared with LPEI. Finally, the size of NaYF4 NPs prepared with HPEI is smaller than that of the NPs prepared with LPEI. As we all know, ideal perfect crystals with well crystallinity would grow exceedingly slowly. That would be difficult to achieve since real crystals always have relatively few disruptions in their lattice structure. The only thing we can do is to reduce the crystallite defects to improve the crystal quality. During the growth stage, the slower the diffusion rate of ions is, the better the crystallinity is. Therefore, in this work the reason that the crystallinity of small-sized NaYF4 seems to be higher than that of the biggest ones under the same solvothermal conditions is the slow growth rate of them.In addition, the size of the as-prepared NPs is increasing with increasing solvothermal time when using the same molecular weight PEI molecules. It is reported that temperature has a certain influence on the stability of crystal nucleus [29]. As the crystal nucleus stability decreases, the nucleation rate of nonoxide crystals decreases with increasing the temperature [29]. As discussed above, the low nucleation rate leads to the increasing size of NPs. This is the reason that the particle size of obtained NaYF4 NPs was increased with increasing the temperature.


## 3.3. Upconversion Photoluminescence of the NaYF4:Yb3+, Er3+ NPs

Figure6 shows the upconversion photoluminescence spectra of the four dry powder samples prepared with different solvothermal conditions according to Table 1. Several distinct green and red emission bands centered at 520, 540, and 650 nm were observed. The green and red emission bands could be assigned to (2H11/2, 4S3/2) → 4I15/2 and 4F9/2 → 4I15/2 transitions of the Er3+ ions in the NaYF4 NPs, respectively. In spite of the degree of polymerization of PEI, the relative upconversion luminescence intensity of samples under solvothermal treatment for 5 h is higher than that of samples under solvothermal treatment for 3 h, which is similar to the previous report [22]. Surprisingly, the upconversion luminescence intensity of the small-sized NaYF4:Yb3+, Er3+ NPs prepared with HPEI is stronger than that of the large-sized NaYF4:Yb3+, Er3+ NPs prepared with LPEI undergoing the same solvothermal treatment process. The observed phenomena are opposite to the common phenomenon. Generally, the NPs with large size exhibit the strong luminescence due to the reduced nonradiative relaxation [22, 30]. This opposite phenomenon in this research is probably related to the difference between HPEI and LPEI. The luminescence difference of samples prepared by different precursors has been reported in previous work [31, 32]. As discussed above, the PEI ligands influence the growth processes of the NPs. The difference in the chain length of PEI leads to a different diffusion rate. Therefore, it is suggested that the samples with the smallest size particle probably have the higher crystallinity because they exhibit the highest relative emission intensity.Figure 6
Upconversion luminescence spectra of the dried power NaYF4:Yb3+, Er3+ samples prepared with different solvothermal conditions according to Table 1 (λex = 980 nm, power = 760 mW): (a) LPEI, 3 h; (b) LPEI, 5 h; (c) HPEI, 3 h; (d) HPEI, 5 h.


## 4. Conclusions

Water-soluble NaYF4:Yb3+, Er3+ NPs are successfully prepared by a solvothermal reaction using PEI with different chain lengths as the surfactants in a water/DEG mixture. HPEI may favour the formation of small-sized NPs with a high degree of crystallinity. The size of NaYF4:Yb3+, Er3+ NPs prepared with HPEI is smaller than that of the NPs prepared with LPEI, while small-sized NPs exhibit more intense relative UC luminescence intensities than large-sized NPs under the excitation of 980 nm NIR light. It is suggested the upconversion luminescence properties and the improved crystallinity of small-sized NPs should be related to the growth process controlled by the chain length of PEI. The obtained NPs have great potential for use in biology and medicine as fluorescent labels or imaging probes.



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*Source: 821706-2014-03-31.xml*