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Advances in Materials Science and Engineering
Volume 2012 (2012), Article ID 748098, 15 pages
The Role of pH in PEG-b-PAAc Modification of Gadolinium Oxide Nanostructures for Biomedical Applications
1Center for Technologies against Cancer (CTC), Tokyo University of Science, 2669 Yamazaki Noda, Chiba 278-0022, Japan
2Department of Materials Science and Technology, Tokyo University of Science, 2641 Yamazaki Noda, Chiba 278-8510, Japan
Received 6 February 2012; Accepted 26 June 2012
Academic Editor: Dachamir Hotza
Copyright © 2012 Eva Hemmer et al. This is an open access article distributed under the Creative Commons Attribution License, which permits unrestricted use, distribution, and reproduction in any medium, provided the original work is properly cited.
Upconversion and near-infrared emitting Gd2O3:Er3+,Yb3+ nanostructured phosphors (nanoparticles and nanorods) for applications in bioimaging have been synthesized by precipitation methods and hydrothermal treatment. Variation of the material synthesis conditions (additives and pH) allows controlling particle size (40 nm to μm range) and rod aspect ratio (5 to 18). It was shown that PEG-b-PAAc (poly(ethylene glycol) poly(acrylic acid) block polymer) is suitable to provide the required chemical durability, dispersion stability, and noncytotoxic behaviour for biomedical applications, where the coating of Gd2O3 with a protecting and biocompatible layer is essential in order to prevent the release of toxic Gd3+ ions. Physicochemical properties of the Gd2O3:Er3+,Yb3+ nanostructures modified with PEG-b-PAAc have been investigated by TG-DTA, FT-IR, and DLS revealing a strong influence of modification conditions, namely, pH of the reaction media, on the nature of the PEG-b-PAAc layer.
Optical imaging techniques for biomedical applications on the basis of fluorescent probes are recently attracting increasing attention. However, drawbacks of commonly used dyes and markers are the poor photostability in case of organic dyes, toxicity of quantum dots and, most severe, autofluorescence from the biological tissue, high absorption by haemoglobin as well as light scattering when ultraviolet (UV) or visible (VIS) light is used as excitation source . Upconverting phosphors, like lanthanide (Ln) containing inorganic compounds emitting light in the visible and near-infrared (NIR) range when excited with NIR light, are interesting candidates to overcome those problems. Rare-earth oxides like yttrium oxide doped with erbium and ytterbium ions, Y2O3:Er3+,Yb3+, absorb NIR light at 980 nm and efficiently emit light of higher energy in the red or green range of the visible spectrum. Besides this upconversion process, the emission of NIR light under 980-nm excitation is of special interest. This is due to the reduced absorption by haemoglobin and scattering when compared to light of shorter wavelengths (UV-VIS), which is absorbed within micrometers to a millimetre of tissue thickness . The resulting deeper penetration depth into biological tissue enables the noninvasive investigation of tissue in deeper areas. Hilderbrand et al. report optical imaging using upconverting Y2O3 nanoparticles modified with poly(acrylic acid), poly(ethylene glycol), and a NIR emitting fluorophore . Amine-modified rare-earth doped and codoped Y2O3 nanocrystals and nanorods for biomedical applications are described by Das and Tan . Besides oxides, applications of LaF3:Ln3+  or NaYF4:Ln3+  nanoparticles as upconverting and NIR emitting phosphors in bioimaging are reported. In recent years, NIR-NIR bioimaging systems based on Er3+-doped Y2O3 nanoparticles have been developed in the group of K. Soga. The development of a NIR-IFBI (near-infrared in vivo fluorescence bioimaging) system using an InGaAs-CCD to detect the emitted light in the NIR wavelength region makes those phosphors promising candidates as biomarkers . Besides the outstanding optical properties, magnetic properties of lanthanides are remarkable and make Ln-based inorganic (nano)structures promising candidates for applications as contrast agents in magnetic resonance imaging (MRI). Recently, the combination of luminescence showing lanthanide ions with a paramagnetic matrix, like Fe3O4  or Gd2O3 [8–10], is of growing interest because both, the possibility of multicolour marking and time resolution of the luminescence and the high spatial resolution of MRI, could improve the efficiency of modern biomarkers. Therefore, we have recently investigated the suitability of gadolinium oxide nanostructures doped with Er3+ and Yb3+ ions as NIR-NIR fluorescent biomarkers, which may also be suitable as contrast agent in MRI. With regard to the application of metal and metal oxide nanostructures in biomedicine and bioimaging, surface modification is essential in order to provide the required biocompatibility and dispersability, for example, in ionic aqueous media. For example, functionalisation of nanoparticles with amino or carboxylic acids [11, 12], capping of quantum dots with biomolecules , coating with silica  and modification with polymers like poly(vinyl alcohol) , dextran, chitosan, or poly(ethylene glycol) are widely-used. Poly(ethylene glycol) (PEG) is chemically inert, provides terminal hydroxyl groups that can be used as anchors for functional groups, is nontoxic and highly solvent in water . Further, grafting of nanostructures with PEG results in enhanced stability of suspensions due to steric repulsion. Surface modification with PEG (so-called PEGylation) is applied for quantum dots , metal [18, 19], and metal oxide [20, 21] nanostructures. PEG-b-PAAc (poly(ethylene glycol) poly(acrylic acid) block polymer) has been chosen because of the electrostatic adsorption of the poly(acrylic acid) group (PAAc) of the coblock polymer on the positively charged surface of the ceramic nanostructures .
Former investigation of the cytotoxicity of Gd2O3:Er3+,Yb3+ towards macrophages revealed a toxic effect in case of bare nanostructures. However, viability could be improved by modifying the surface of the nanostructures with PEG-b-PAAc [23, 24]. The cytotoxic effect on macrophages observed in case of bare nanostructures was deduced to the poor chemical durability of Gd2O3 under acidic conditions as found inside macrophages. The result is the release of toxic Gd3+ ions inducing cell death. Surface modification provided the required chemical durability of Gd2O3 reducing the Gd3+ release from nanostructures uptaken by macrophages. Firstly, variations of modification conditions (e.g., ultrasonic treatment versus stirring, modification time, and temperature) showed a strong effect on grafting rate, acidic resistivity, and -potential. Changes in FT-IR spectra in the wavenumber range from 500 to 1000 cm−1 in dependence from modification conditions led us propose the formation of a “gadolinium-PEG-b-PAAc-complex” on the gadolinium oxide nanostructure surface. The pH value of the PEG-b-PAAc solution that is used for modification is in the range of 3.5 to 4.0, thus, corresponds to the critical range for chemical instability of Gd2O3. Consequently, a partial dissolution of Gd2O3 and an exposition of free Gd3+ on the nanostructure surface under acidic conditions are expected. In contrast, under basic conditions, most Gd3+ species are covered by OH− groups reducing the interaction with the PAAc group of the polymer.
In order to clarify the influence of modification conditions, potential formation of a “gadolinium-PEG-b-PAAc-complex” and to optimize modification conditions, we investigated the relationship between modification pH and physical as well as chemical properties of Gd2O3:Er3+,Yb3+ modified with PEG-b-PAAc in more detail.
2. Results and Discussion
2.1. Material Synthesis and Characterization
Nanoscale Gd2O3 doped with Er3+ and Yb3+ ions was prepared by two different approaches, hydrothermal treatment and precipitation methods. This allows the variation of the morphology, such as spherical particles or rod-like structures. As shown by Wang and Li, the hydrothermal process easily provides various lanthanide hydroxide, Ln(OH)3, nanostructures including nanoparticles, nanotubes, nanosheets, or fullerene-like nanoparticles . Herein, pH of the reaction mixture  as well as complexing agents  play an important role on the control over the aspect ratio of the Ln(OH)3 nanorods. Ln2O3 nanostructures can be obtained by a postthermal treatment, whereas shape and morphology are kept constant. We observed similar formation of nanorods with various aspect ratios by hydrothermal treatment of an aqueous gadolinium nitrate solution (doped with each 1 mol% Er3+ and Yb3+). Prior to the hydrothermal treatment (200°C, 6 hrs), the solutions were activated with either an aqueous potassium hydroxide () or ammonia solution. The variety of shape and aspect ratio of the obtained nanostructures (annealed at 900°C for 30 min) is shown in the scanning electron micrographs in Figure 1.
Activation of the Ln solution with 4.5 mL 1 M results in nanorods with a homogeneous size distribution and an aspect ratio of approximately 12 (Rods12, Figure 1(a) ). The influence of the alkali concentration on morphology was investigated by adding 0.1 to 5.0mL ammonia solution prior to the hydrothermal treatment. At low ammonia concentrations ( mL, pH = 6.6–6.8) platelets of inhomogeneous size distribution (length and width : several 100 nm to 2 μm) are formed (Figures 1(b) and 1(c)). An increase in the ammonia concentration induces the formation of nanorods. A bimodal size distribution is obtained after activation with 0.35 mL ammonia (pH = 7.1, Figure 1(d)). Nanorods of 90 nm in width and an average length of 1.7 μm, resulting in an average aspect ratio of 18 are found. But also larger rod-like structures of approximately 400 nm in width and 4.2 μm in length with an average aspect ratio of 11 are observed. Larger nanorods ( up to 4.5 μm, ~400–500 nm, aspect ratio ~7–9) are obtained in case of 0.5 mL ammonia (pH = 8.7, Figure 1(e)). Further increase in the amount of ammonia reduces the size of the nanostructures: the addition of 1.0 mL ammonia (pH = 9.2) results in nanorods of up to 1.5 μm in length and 100 nm in width (average aspect ratio: 11) (Figure 1(f)). Further decrease in size is observed for the addition of 2 mL ammonia (pH = 10.3, average nm, nm, aspect ratio: 6) (Figure 1 (g)). Almost no changes in morphology are observed at even higher ammonia concentrations (2 mL5 mL, pH = 10.3–10.9, Figures 1(h) and 1(i)). Comparing Figures 1(f) and 1(j), which both show powders obtained by activation with 1 mL ammonia, the influence of the mixing order becomes obvious. Generally, 0.1 to 5 mL ammonia solution was added to the aqueous Ln solution. In contrast, powders shown in Figure 1(j) have been prepared by adding an aqueous lanthanide solution ( mL) to a diluted ammonia solution (1 mL ammonia in 20 mL H2O) during rigorous stirring. The latter case results in a much more homogeneous size distribution with an average length of 660 nm and width of 160nm (average aspect ratio: 4-5, Rods5 ). Hence, precipitation by adding the Ln solution into a diluted alkaline (precipitant) solution under stirring induces a more homogenous precipitation process, which results in the uniform growth of nanorods with a monodispersed size distribution during the hydrothermal treatment.
As reported previously , spherical nanostructures can be obtained by precipitation methods without further hydrothermal treatment. Particles of inhomogeneous morphology and size ( nm to 1 μm, Figure 2(a)) are obtained by alkaline precipitation (AP) using sodium carbonate, Na2CO3, as precipitation agent (ParticlesAP). Enzymatic precipitation (EP) results in smaller particles of less than 100 nm in diameter (ParticlesEP). In EP, the enzyme urease is used in order to decompose urea at room temperature providing , which reacts as precipitant . Due to the reduced particle size and the absence of any surfactant during synthesis a high tendency for the formation of agglomerations is observed (Figure 2(b)). In order to avoid agglomeration and to improve homogeneity of the nanoparticles, surfactant-free and surfactant-assisted homogeneous precipitation (HP) of Gd2O3 was affected as originally described by Matijević and Hsu . The obtained nanoparticles are not agglomerated and show a diameter of approximately 300 nm (Figure 2(c)). However, by the proposed surfactant-free method, morphology control is difficult, may result in inhomogeneous morphology and size distribution as reported in literature . We observed the formation of flake-like structures (FlakesHP) of about 2 μm in length and 1.5 μm in width (Figure 2(d)). Those flakes are built up by smaller particles, which were similarly reported by Park et al. and which were assigned to strong bonds between the aggregates due to thermal decomposition of the precursor gadolinium carbonate . The growth of flake-like structures can be overcome by the addition of PEG-6000 or CTAB (cetyltrimethylammonium bromide)  resulting in smaller nanoparticles when compared to the surfactant-free method with diameters of about 150–120 nm (ParticlesHP-PEG, Figure 2(e), ParticlesHP-CTAB, Figure 2(f)). Water at 85°C is highly active for diffusion processes, which drives the growth of particles. When CTAB or PEG is added into the solution, diffusion processes are inhibited and the formation of agglomerations can be suppressed. Further, reduced agglomeration is ascribed to the adsorption of CTAB molecules on the formed hydroxide precipitates by Zhu et al. describing the formation of Nd(OH)3 nanoparticles by microemulsion method using CTAB for morphology control . Hereby, adsorption of CTAB molecules on the surface planes of the formed lanthanide hydroxide can inhibit the aggregation of nanoparticles. Moreover, an increase in particle size with increasing stirring time is reported. This is deduced to an enhanced Brownian motion of the microemulsion droplets, leading to increased interaction between droplets and therefore easy aggregation. In agreement with this, we observed a more likely formation of flake-like agglomerations of Gd2O3:Er3+,Yb3+ when the reaction time exceeds 30min even in presence of CTAB. In contrast to observations by Zhu et al., but in agreement with Yue et al. , CTAB concentrations in the range of 0.3 to 33.3 mmol/L had no influence on size or morphology of the resultant material.
Scheme 1 gives an overview of the used synthesis routes and variations as well as the morphology and size of the resultant nanostructures.
2.1.2. Crystallinity and Phase
Powder X-ray diffraction (XRD) analysis on powders obtained by hydrothermal treatment revealed crystalline gadolinium hydroxide, Gd(OH)3, when 0.35 mL or a higher volume of ammonia solution was added (pH ≥ 7.1, Figure 3(a)). In analogy with the changes in morphology, different XRD patterns are obtained for powders prepared at lower ammonia concentrations. Patterns recorded for powders obtained by addition of 0.1 or 0.2 mL ammonia solution (pH: 6.6–6.8) show peaks that do not match with the characteristic pattern for Gd(OH)3. However, we could not doubtlessly determine the obtained phase. The formation of crystalline Gd(OH)3 at pH higher than 7 is in agreement with the stability of lanthanide hydroxides in alkaline solution, but instability in acid solutions in which they dissolve as the corresponding cations . Independent from alkaline concentration, all as-prepared powders could be transformed into the oxide phase, Gd2O3, by post-thermal treatment at 900°C for 30 min (Figure 3(b), graphs B and C). In fact, those high temperatures (900°C) are not necessary for transformation of Gd(OH)3 into Gd2O3. Lower annealing temperatures, such as 600°C, are sufficient to induce crystallization of the oxide phase (Figure 3(b), graph A). The reason for the postthermal treatment at such high temperatures is that at least 900°C are necessary for the elimination of residual hydroxyl or carbonate groups which may quench the photoluminescence of Gd2O3:Er3+,Yb3+.
Due to crystallization of gadolinium hydroxide in the hexagonal lattice ( Å, Å, Å) no templates are required to synthesize elongated structures. Consequently, the hydrothermal treatment leads to a rod-like morphology of Gd2O3:Er3+, Yb3+. The anisotropic growth is governed by crystal chemistry and chemical potential in solution [35–38]. The chemical potential is tuneable by pH value of the reaction mixture, whereas a higher chemical potential favours the one-dimensional growth. As a result nanorods are obtained at addition of at least 0.35 mL ammonia, while at lower ammonia amount (lower pH) the 1-dimensional growth is less supported resulting in plate-like structures (Figures 1(b) and 1(c)). For higher OH− concentrations lower aspect ratios are expected as explained in the formation mechanism of 1-dimensional Ln(OH)3 structures proposed by Wang and Li [36, 37] and Yang et al. . In agreement with the proposed formation mechanism we observe a strengthening of the (110) peak in the XRD pattern of Gd(OH)3:Er3+,Yb3+ obtained by addition of 0.35 mL ammonia solution ((ammonia)=0.35 mL: I(110)/I(101)=2.4; (ammonia)=5mL: I(110)/I(101)=0.8). This strengthening represents the favoured growth direction along the c-axis, resulting in the high aspect ratio of 18 observed in SEM (Figure 1(d)). With an increasing amount of ammonia inducing a reduced aspect ratio (/) this strengthening is less pronounced.
As-prepared powders from hydrothermal synthesis consist of crystalline Gd(OH)3. In contrast, precipitation methods always lead to amorphous powders requiring a postthermal treatment to induce crystallization. X-ray diffraction patterns recorded on annealed powders obtained by enzymatic, alkaline, and CTAB-assisted homogeneous precipitation confirm the crystallization of Gd2O3:Er3+,Yb3+ (Figure 3(c)). Crystal sizes determined by Scherrer equation increase from 31 nm (ParticlesEP) to 43 nm (ParticlesHP-CTAB) to 61 nm (ParticlesAP). A crystal size of 38 nm was determined for the FlakesHP. Even though the particles are not single crystals, but are built up by several crystallites, the smaller calculated crystal size in case of ParticlesEP reflects the trend for a smaller average particle size observed in SEM.
2.1.3. Optical Properties
With regard to potential applications as luminescent biomarkers, optical properties of Gd2O3:Er3+,Yb3+ were investigated . All samples show the characteristic Er3+ f-f transition peaks for upconversion emission under 980 nm excitation. Green emission corresponds to (525 nm) and (561 nm) transitions. The red emission band is referred to the (660 nm, 677 nm) transition (Figure 4(a)). Enhanced emission intensity and peak resolution are observed for nanoparticles when compared to nanorods. This may be due to different powder densities or carbonate or hydroxide impurities. Figure 4(a) also shows the emission spectra recorded in the NIR wavelength range with a peak of maximum intensity at 1540 nm, which can be assigned to the transition of Er3+. As mentioned earlier, NIR emission is particularly interesting with regard to new NIR-based bioimaging devices .
As the interpretation of the emission intensities is not trivial, we here discuss the relation between the red (660 nm, ) and the green (560 nm, ) ratio of the emission spectra. Comparing the red-to-green ratio of particles obtained by enzymatic, alkaline, and CTAB-assisted homogeneous precipitation, ParticlesEP and ParticlesHP-CTAB (–150 nm) show a higher red-to-green ratio than ParticlesAP ( nm to μm) (Figure 4(b)). In fact, a stronger phonon interaction of the rare-earth ions is known to be often found for smaller particle size resulting in the increased emission of red light [40, 41]. With increasing particle size the specific surface area decreases compared to the volume. Hence, there are less Ln3+ that are affected on the surface. Thus, rare-earth ions doped into larger ParticlesAP show less phonon interaction and consequently the ratio between red and green light shifts towards the green range. A further aspect taking influence on the red-to-green ratio is the hydroxyl content in the investigated powders. In general, upconversion emission efficiency from lanthanide ions doped into a ceramic host is strongly influenced by organic ligands or solvent molecules, such as groups with high energy vibrational mode (OH, NH2) located close to the light-emitting lanthanide ions resulting in quenching of the upconversion emission . In order to determine the hydroxyl content, FT-IR spectra were recorded on the samples. As obvious from the obtained spectra (Figures 4(c) and 4(d)) the hydroxyl content in ParticlesHP-CTAB and ParticlesEP is higher than in ParticlesAP. The broad band in the range 1200–1700 cm−1 recorded on ParticlesAP indicates the presence of water molecules on the nanoparticle surface, but the hydroxyl content in the structures is lower compared to ParticlesHP-CTAB and ParticlesEP. The sharp peak at 880 cm−1 is associated to  originating from the use of Na2CO3 as precipitant in alkaline precipitation method. In general, the red light emitting 4F9/2 state is mainly produced by quenching of the green light emitting 4S3/2 state . Accordingly, the higher content in OH− groups leads to quenching of the green emission while the red emission is maintained. This then results in the observed higher red-to-green ratio of ParticlesEP and ParticlesHP-CTAB compared to ParticlesAP. On the other hand, even though Rods12 show much higher hydroxyl content than Rods5, the red-to-green ratio is enhanced in case of Rods5. The lower red-to-green ratio in case of Rods12 cannot be explained by the residual hydroxyl content, however, we suggest the higher content in residual carbonate groups (1400 cm−1, 1510 cm−1) and the presence of water molecules (peak at 1630 cm−1 associated with H–O–H bending of water ) determined in Rods12 to be the reason for the stronger quenching effect.
2.2. Surface Modification with PEG-b-PAAc
ParticlesHP-CTAB and Rods5 were chosen for modification with PEG-b-PAAc. An aqueous suspension of those nanostructures was stirred at 35°C for 24 hrs after the addition of an aqueous PEG-b-PAAc solution, whose pH was set to 3.7, 5.0, 6.5, or 8.0.
The -potential of bare Gd2O3:Er3+,Yb3+ nanostructures dispersed in distilled water  decreases from +21.8 mV (ParticlesHP-CTAB) and +18.5 mV (Rods5) to −35.74 mV (ParticlesHP-CTAB) and −30.0 mV (Rods5) when the pH of the dispersion increases from 5 to 12. The isoelectric point was found to be at pH=8.6 (ParticlesHP-CTAB) and 8.4 (Rods5). Modification with PEG-b-PAAc is based on the electrostatic adsorption of the poly(acrylic acid) group (PAAc) of the coblock polymer on the positively charged surface of the nanostructures. Previously [23, 28], nanostructures have been modified by addition of a PEG-b-PAAc solution of pH 3.7. Under those conditions surface charge is sufficiently positive to ensure the electrostatic adsorption as shown by -potential measurements. An increase in pH of the nanostructure suspension results in a decrease of the surface charge reaching the isoelectrical point at pH ~ 8.5. As a consequence, reduced adsorption rate is expected in case of modification using PEG-b-PAAc solutions of higher pH.
2.2.1. FT-IR Spectroscopy
FT-IR spectra recorded on bare and modified ParticlesHP-CTAB and Rods5 are presented in Figure 5. All spectra show an adsorption peak at 545 cm−1, which is assigned to the metal-oxygen bonds in gadolinium oxide. In case of modified samples, a broad band due to O–H groups in the range of 3500 cm−1 and a shoulder at 1640 cm−1 assigned to H–O–H bending of water result from the modification in aqueous medium. Peaks at 2900 and 1100 cm−1 can be assigned to C–H asymmetric stretching and C–O–C stretching in PEG . Peaks of less intensity are observed at 1347 and 950 cm−1, which are due to CH2 wagging motion as well as CH2 rocking vibrations . Those peaks are also observed in the FT-IR spectrum recorded on pure PEG-b-PAAc (provided in supporting information). This confirms the presence of PEG-b-PAAc on the surface of Gd2O3:Er3+,Yb3+ nanostructures. The sharp and intensive peak at 1730 cm−1 observed for pure PEG-b-PAAc, originating from carboxylic acidic groups (–COOH), disappears in spectra recorded on modified samples. Instead, two bands at 1523 and 1406 cm−1 appear. Those are related to carboxylate (–COO−) stretches  giving a further confirmation for surface modification.
With decreasing modification pH intensities of the peaks assigned to C–H, C–O–C, as well as –COO- increase. This increase indicates a higher amount of PEG-b-PAAc on the nanostructure surface. Further, in case of pH 5 or lower a splitting of the peak at 1406 cm−1 into two peaks at 1419 and 1453 cm−1 is observed (marked with an asterisk). Investigating the formation of complex of copper with poly(acrylic acid), Allan et al. report peaks at a similar wavenumber range (1554, 1451, and 1413 cm−1) and assign them to the υ(COO−) group, which has complexed to the copper ion . Hence, formation of a gadolinium-PEG-b-PAAc-complex (Scheme 2) is proposed to be the origin of the here observed peak splitting. While the peak intensity of bands, which are characteristic for the polymer, is increasing with decreasing pH, the Gd–O band is less pronounced and broadened. Reference measurements on gadolinium acetate tetrahydrate (FT-IR spectrum provided in Supplementary Material available online at doi: 10.1155/2012/748098) reveal a broad band at wavenumber range 850 to 550 cm−1. The exhibition of such a band is a potential reason for the broadening observed in the spectra recorded on samples modified with PEG-b-PAAc solutions of pH 5 or lower and supports the suggested complex formation.
2.2.2. TG-DTA Analysis
For further determination of the amount of PEG-b-PAAc on the surface of the nanostructures, TG-DTA analysis was performed from 20 to 900°C (under air). Endothermic peaks in the range of 40 to 80°C in the DTA curves (not shown here) are assigned to the loss of absorbed water on the nanostructure surface. Exothermic peaks in the range of 350 to 390°C are assigned to the combustion of organic groups, namely, PEG-b-PAAc. Herein, a shift of the exothermic peaks to lower temperatures is observed with increasing modification pH. TG curves (not shown here) show a two-step mass loss at equivalent temperatures with main mass loss in the temperature range from 200 to 500°C, which is taken as representative for the grafting rate with PEG-b-PAAc (Table 1) . In analogy to DTA characteristics, changes with modification pH. With increasing modification pH the temperature range for is broadened and less sharp. The grafting rate (/residual mass) is decreasing from 0.31 (pH = 3.7) to 0.08 (pH = 8) in case of ParticlesHP-CTAB and from 0.67 (pH = 3.7) to 0.09 (pH = 8) in case of Rods5. Those data support the trend observed by FT-IR spectra, revealing that the surface modification is less pronounced when carried out at higher pH. This observation can also be deduced to modification conditions approaching the isoelectric point of Gd2O3:Er3+,Yb3+ nanostructures as observed by -potential measurements ( ~ 8.5), which hinders the electrostatic adsorption of PEG-b-PAAc at high pH.
Comparing the grafting rate at pH 3.7, Rods5 exhibit a higher PEG-b-PAAc content than ParticlesHP-CTAB. However, the grafting rate of Rods5 drops significantly at a modification pH 5.0 (grafting rate ~0.18). A similar drop is shifted to pH 6.5 in case of ParticlesHP-CTAB (grafting rate ~0.17). This is in agreement with our observation in FT-IR spectroscopy (Figure 5). Spectra recorded on ParticlesHP-CTAB modified at pH 5.0 and 3.7 show the characteristic peak splitting for complex formation at 1419 and 1453 cm−1. On the other hand, the same peak splitting is shifted towards a modification pH of 3.7 in case of Rods5.
2.2.3. Chemical Durability
For applications of Gd2O3:Er3+,Yb3+ nanostructures in biomedicine, protection from dissolution of Gd2O3 inducing the formation of toxic Gd3+ ions in acidic media (as found inside macrophages) is an essential task of the PEG-b-PAAc layer. Therefore, chemical durability of nanostructures modified at pH 3.7 and 8 has been investigated, and the recorded graphs are presented in Figure 6.
Dissolution of lanthanide oxides in acidic solutions under pH less than 6.4 is well known. The pH of a suspension of lanthanide oxides reaches a saturation value of about 6.4 almost immediately after addition of the oxides into an acidic solution due to their dissolution . Accordingly, Gd3+ ions start to be released from insufficiently coated Gd2O3 (modification pH 8) resulting in an increase in pH reaching around 6 after 4hrs. Results of FT-IR spectroscopy and TG-DTA in dependence on modification pH revealed a higher PEG-b-PAAc content in case of modification pH 3.7. The slight increase in pH of the suspension of nanostructures modified at pH 3.7 indicates a starting dissolution of Gd2O3. However, the presence of sufficient polymer chains from surface modification enables the reaction between those free ions and the polymer chains (COO−). As the released ions are trapped by the polymer and further dissolution is stopped, pH reaches a saturation value of around 3.9. In agreement with the formation of a complex between Gd3+ on the nanostructure surface and COO− in the PAAc chain at low modification pH, nanostructures modified at pH 3.7 show sufficient chemical durability, while the PEG-b-PAAc layer provided by modification at pH 8 cannot fulfil acidic resistance requirements.
2.2.4. Size Distribution and Dispersion Stability in Aqueous Medium
The size distribution of bare and PEG-b-PAAc modified nanostructures dispersed in water is displayed in Figures 7(a) and 7(b). Bare nanostructures tend to aggregate to larger agglomerates of several 100 nm to micrometer size. On the other hand, data obtained for modified nanostructures suggest that PEG-b-PAAc modified nanostructures are well dispersed in aqueous solutions. The hydrodynamic mean diameters are 200 and 260 nm for ParticlesHP-CTAB modified at pH 3 and 8. Analogous diameters for Rods5 are 170 nm (pH = 3) and 200 nm (pH = 8).
The capability of PEG-b-PAAc modification to avoid agglomeration of the nanostructures in aqueous media is also reflected in their dispersion stability. Dispersion stability of the nanostructures was investigated by adsorption measurements in a spectrophotometer. Results are presented in Figures 7(c) and 7(d). Accordingly, dispersion stability of ParticlesHP-CTAB in distilled water is improved by PEG-b-PAAc modification. In case of bare nanostructures, absorbance decreases linearly to around 85% within 2 hrs. In contrast, suspensions of PEG-b-PAAc modified ParticlesHP-CTAB and Rods5 remain stable with more than 90% absorbance after 2 hrs. The slightly concave decay of the curve recorded on ParticlesHP-CTAB modified at pH 3 indicates even better stability than the convex shaped curve recorded for a modification pH of 8. For Rods5, both modified samples exhibit a concave shaped curve indicating good dispersion stability.
With respect to potential biomedical applications we further investigated the dispersion stability of ParticlesHP-CTAB and Rods5 without and with PEG-b-PAAc modification in an aqueous sodium chloride solution. Therefore, 1.5 mL of a 0.3 M NaCl solution were added to 2.5 mL of the nanostructure dispersion resulting in an overall saline concentration of 0.1 M. The increase in solution ionic strength is expected to increase the hydrodynamic diameter of the dispersed nanostructures, resulting in unstable, highly agglomerated dispersions . Thus, as obvious from Figures 7(e) and 7(f), the increase of the ionic strength results in immediate aggregation of the dispersed (unmodified) nanostructures. However, surface modification with PEG-b-PAAc effectively improves the dispersion stability (blue and red graphs) and suppresses agglomeration under such conditions.
Figure 8 summarizes the relationship between modification pH and physicochemical properties of PEG-b-PAAc modified ParticlesHP-CTAB and Rods5. There is a clear trend of enhanced surface modification with decreasing pH indicated by an increase in grafting rate determined from TG graphs and an increased COO- peak area in FT-IR spectra. Further, FT-IR data suggest the formation of a gadolinium-PEG-b-PAAc-complex in case of modification under acidic conditions (pH < 5). With regard to biomedical applications, acidic durability of nanostructures is improved by modification at low pH, which is evident from the lack of increase in pH during the chemical durability test.
Erbium and ytterbium doped gadolinium oxide (Gd2O3:Er3+,Yb3+) spherical as well as rod-like nanostructures have been synthesized by precipitation methods and hydrothermal treatment. Variation of the precipitation conditions allows the control of aspect ratio and particle size ranging from 5 to 18, respectively, 40 nm to micrometer range. The poor chemical durability of gadolinium oxide under acidic conditions induces cell death when incubated with macrophages, which must be overcome prior to applications in biomedicine. Surface modification with PEG-b-PAAc provides a protecting layer. Herein, variation of the modification pH takes strong influence on grafting rate and bonding characteristics between the Gd2O3 surface and the PEG-b-PAAc layer as observed by TG-DTA analysis and FT-IR spectroscopy. It was shown that a modification pH in the acidic range results in higher grafting rate when compared to basic modification conditions. The formation of a gadolinium-PEG-complex between Gd3+ on the nanostructure surface and COO- groups in the PAAc chain in case of low modification pH improves the surface properties such as acidic durability and dispersion stability of the nanostructures. Further, the obtained acidic durability ensures the reduced release of toxic Gd3+ ions providing good biocompatibility and making the investigated system a promising candidate for future bioimaging applications.
4. Experimental Section
4.1. Material Synthesis
Starting materials like lanthanide nitrates (Ln = Gd, Er, Yb), urea, urease enzyme, PEG-6000 (poly(ethylene glycol), Mw = 6000), CTAB (cetyltrimethylammonium bromide), KOH (potassium hydroxide), ammonia (25 wt% aqueous solution), Na2CO3 (sodium carbonate), and PEG-b-PAAc (poly(ethylene glycol)-b-poly(acrylic acid) block copolymer, Mw = 5000/3200) were purchased from usual commercial sources and were used without further purification.
For the alkaline precipitation, 1.81 g (4 mmol) Gd(NO3)36H2O were dissolved in 100 mL distilled water. To obtain Gd2O3 particles doped with 1 mol% of Er3+ and Yb3+ 18.2 mg (0.041 mmol) Er(NO3)35H2O and 14.7 mg (approx. 0.041 mmol) Yb(NO3)3xH2O were added to the gadolinium nitrate solution. An aqueous Na2CO3 solution ( mol/L, mL) was added to the lanthanide nitrate solution and stirred at room temperature for 2hrs. For the homogeneous precipitation, 758.3 mg (1.68 mmol) Gd(NO3)36H2O and 1 mol% Er(NO3)35H2O (7.5 mg, 0.017 mmol), respectively, 1 mol% Yb(NO3)3xH2O (6.1 mg, approx. 0.017 mmol) were dissolved in 300 mL H2O. Additionally, as a surfactant either 30 g (5 mmol) PEG-6000 or 1–10 mmol CTAB were added, followed by stirring for 50 min at room temperature. 9.01 g (150 mmol) urea was added to the pure Ln- or Ln-surfactant-solution and the mixture was kept stirring for 10 min. For precipitation, the mixture was stirred at 85°C for 30 min. In case of the enzymatic precipitation 1.35 g (3 mmol) Gd(NO3)36H2O and 1 mol% Er(NO3)35H2O (13.4 mg, 0.030 mmol), respectively, 1 mol% Yb(NO3)3xH2O (10.9 mg, approx. 0.030 mmol) were dissolved in 200 mL H2O and 18.02 g (300 mmol) urea were added. This solution was added to an aqueous urease enzyme solution (22.5 mg urease enzyme in 100 mL H2O) to initiate precipitation. The mixture was stirred at room temperature for 2 hrs. In the hydrothermal synthesis, the concentration of gadolinium nitrate was set to 0.05 mol/L at a total volume of 30 mL. Therefore, in a first approach 677 mg (1.5 mmol) Gd(NO3)36H2O and 6.8mg (0.015 mmol) Er(NO3)35H2O and 5.5 mg (approx. 0.015 mmol) Yb(NO3)3xH2O were dissolved in 25.5 mL H2O. The obtained solution was transferred into teflon liners ( mL) and activated with 4.5 mL 1 M aqueous KOH solution. In a second approach, 677 mg (1.5 mmol) Gd(NO3)36H2O and 6.8 mg (0.015 mmol) Er(NO3)35H2O and 5.5 mg (approx. 0.015 mmol) Yb(NO3)3xH2O were dissolved in (30–y) mL H2O (, and 5.0 mL) and the mixture was activated by addition of z mL (, and 5.0 mL) of aqueous ammonia hydroxide (25 wt%) resulting in solutions with a pH value of 6.6, 6.8, 7.1, 8.7, 9.2, 10.3, 10.3 and 10.9. Alternatively, the lanthanide nitrates were dissolved in 9 mL H2O and quickly added to an aqueous ammonia solution (1 mL 25wt% ammonia solution +20 mL H2O) under rigorous stirring. After enclosing the teflon liners in steel autoclaves, the autoclaves were placed in a furnace, respectively, wrapped into a heating mantle system (equipped with a thermocouple K:Class:2 by Toho and a program temperature controller TXN700 by AS ONE) and heated to a temperature of 200°C that was kept for 6 to 12 hrs. The obtained powders were collected by centrifugation, washed two times with distilled water, and dried at 80°C for at least 12 hrs. Crystalline oxide powders were obtained by postthermal treatment at 900°C (30 min).
4.2. Surface Modification
For surface modification with PEG-b-PAAc, Gd2O3:Er3+,Yb3+ nanostructures were dispersed in water ( mg/mL) and sonicated for 30 min at room temperature. An aqueous PEG-b-PAAc solution was added into the nanostructure dispersion, resulting in final concentrations of 0.6 mg/mL Gd2O3:Er3+,Yb3+ and 1.2 mg/mL PEG-b-PAAc. The mixtures were stirred at 35°C for 24 hrs. In order to investigate the influence of pH during modification process, the pH of the initial aqueous PEG-b-PAAc solution (pH = 3.7) was adjusted by addition of NaOH to values of approximately 5.0, 6.5, and 8.0 before adding the mixture into the nanostructure dispersion, followed by stirring for 24 hrs at 35°C. The obtained surface modified powders were collected by centrifugation, washed at least three times with distilled water, and dried at room temperature. For the investigation of the dispersion stability and for dynamic light scattering (DLS) measurements, PEG-6000 assisted modification with PEG-b-PAAc was achieved at pH 3.0 and 8.0. Therefore, PEG-6000 was added to the Gd2O3:Er3+,Yb3+ suspension and sonicated for 10 min prior to the addition of the PEG-b-PAAc solution (pH = 3.0 or 8.0). The final concentrations of PEG-6000 and PEG-b-PAAc were both 0.6 mg/mL. The obtained surface modified powders were collected by centrifugation, washed at least three times with distilled water, and redispersed into distilled water without further drying.
4.3. Material Characterization
The crystalline phase of the samples was determined by powder XRD with a ULTIMA III diffractometer (Rigaku) using CuKα radiation. Crystal sizes were determined by Scherrer equation = /(FWMH cos()) with and nm. Morphology of the obtained powders was investigated by scanning electron microscope (S-4200, Hitachi). For FT-IR spectroscopy, samples were mixed with KBr and spectra of the powders were recorded under vacuum conditions using a JASCO FT/IR-6500 spectrometer. TG-DTA graphs were recorded by use of DTG-60 Simultaneous DTA-TG apparatus with FC-60A gas flow controller by Shimadzu with a heating rate of 10 K/min and an air flow of 50 mL/min. Surface charge of the nanostructures was determined with a Delsa Nano Submicron Particle Size and Zeta Potential analyzer by Beckman Coulter using the disposable cell for zeta potential unit. Nanostructures were suspended ( mg/mL) in either distilled water (pH = 5.2) or an aqueous NaOH solution with an adjusted pH in the range 5 to 12. Zeta-potential was calculated from the mobility by the equipment’s software using the Smoluchowski model. In order to investigate chemical durability under acidic conditions as-prepared or PEG-modified nanostructures were added into an aqueous HCl solution with an initial pH of 3 ((Gd2O3:Er3+,Yb3+) = 0.2 mg/mL). Under rigorous stirring, the time-dependent change of pH was recorded by use of an Auto Titrator Com-1600 (Hiramura). Dispersion stability of an aqueous suspension of bare and modified (PEG-6000 assisted modification) Gd2O3:Er3+,Yb3+ nanostructures was investigated by absorbance measurements with a V-630 Spectrophotometer by JASCO. The size distribution of PEG-b-PAAc modified powders (PEG-6000 assisted modification) in distilled water was measured by DLS using a Dynamic Light Scattering Particle Size Analyzer LB-550 by Horiba.
The authors thank Dr. Lionel Vayssieres (WPI Center for Materials NanoArchitectonics (MANA), National Institute for Materials Science (NIMS), Tsukuba, Japan) for scientific discussion and provision of the zeta-potential equipment.
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