Yufei
Xia
a,
Jian
Chen
a,
Yan-gai
Liu
*a,
Maxim S.
Molokeev
bc,
Ming
Guan
a,
Zhaohui
Huang
a and
Minghao
Fang
a
aSchool of Materials Science and Technology, Beijing Key Laboratory of Materials Utilization of Nonmetallic Minerals and Solid Wastes, National Laboratory of Mineral Materials, China University of Geosciences, Beijing, 100083, China. E-mail: liuyang@cugb.edu.cn
bLaboratory of Crystal Physics, Kirensky Institute of Physics, SB RAS, Krasnoyarsk 660036, Russia
cDepartment of Physics, Far Eastern State Transport University, Khabarovsk 680021, Russia
First published on 23rd November 2015
A series of apatite solid solution phosphors Ca2+xLa8−x(SiO4)6−x(PO4)xO2:Eu2+ (x = 0,2,4,6) were synthesized by a conventional high-temperature solid-state reaction. The phase purity was examined using XRD, XPS and XRF. The crystal structure information, such as the concentration, cell parameters and occupation rate, was analyzed using a Rietveld refinement, demonstrating that the Eu2+ activated the Ca2La8(SiO4)6O2 and Ca8La2(PO4)6O2 to form continuous solid solution phosphors. Different behaviors of luminescence evolution in response to structural variation were verified among the series of phosphors. Two kinds of Eu2+ ion sites were proved using low temperature PL spectra (8k) and room temperature decay curves. The substitution of large La3+ ions by small Ca2+ ions induced a decreased crystal field splitting of the Eu2+ ions, which caused an increase in emission energy from the 5d excited state to the 4f ground state and a resultant blue-shift from 508 nm to 460 nm. Therefore, with the crystal structure evolution, the emitted color of the series of phosphors could be tuned from green to blue by adjusting the ratio of Ca/La.
The crystal field strength and coordination environment have great influences on the outermost electron transition of the Eu2+ ion, the most frequently used activator in phosphors, because the active electronic level is not shielded against the surrounding ligands,8–10 indicating that Eu2+ ions can emit light from the ultraviolet to the infrared with broadband emitting fluorescence.11,12 It is well known that apatite structure compounds (space group P63/m), with a general chemical formula of the form A10(XO4)6Z2 (A = Ca2+,Ba2+,Ce3+,La3+,Y3+, etc., X = P5+,As5+,Si4+, etc., and Z = O2−,F−,Cl−,OH−, etc.),13 contain two kinds of cation sites: the 9-fold coordinated 4f sites with C3 point symmetry and the 7-fold coordinated 6 h sites with a CS point symmetry, which are suitable for the substitution of various rare-earth-metal ions.14–16 Consequently, due to their adjustable structures, and excellent thermal and physicochemical stabilities, apatite compounds have become highly efficient host materials for the luminescence of various rare earth ions and have aroused widespread attention.17–19 As discussed above, the coordination environment of the Eu2+ site is anticipated to be changed via chemical composition variation among solid solution phosphors.20 Thus, the emitted color can be controlled by doping Eu2+ ions into a series of apatite solid solution hosts which are expected to display adjustable emission spectra in a wide range to meet the requirements of multi-color phosphors.
In this study, the coordination environment variation of the Eu2+ ion has been realized by the replacement of Ca2+ ions with La3+ ions and resulted in crystal splitting decreases of the Eu2+ ion, a series of color tunable solid solution phosphors Ca2+xLa8−x(SiO4)6−x(PO4)xO2:Eu2+ (x = 0,2,4,6) were successfully prepared by a high-temperature solid-state reaction. Moreover, it's worth noting that the replacement of [PO4]3− with the [SiO4]4− tetrahedron was introduced into the solid solution to realize the charge compensation because of the different valences between Ca2+–La3+ and also that the Ca4La6(SiO4)4(PO4)2O2:Eu2+ and Ca6La4(SiO4)2(PO4)4O2:Eu2+ phosphors were synthesized for the first time.
The phase purity was demonstrated by XRD, XPS and XRF, and the crystal structure information was analyzed base on Rietveld refinement results. In addition, the relationship between the crystal structure evolutions, the PLE and PL spectra at normal and low temperatures, the lifetimes and the temperature dependence spectra have been discussed in detail.
X-ray photoelectron spectroscopy (XPS) measurements were collected using a Kratos Axis Ultra DLD, employing an MCP stack & delay-line photoelectron detector with scanned & snapshot spectroscopy modes. X-ray Fluorescence (XRF) measurements were measured by utilizing a Rigaku ZSX Primus II X-ray fluorescence spectrograph. The photoluminescence emission (PL) and the photoluminescence excitation (PLE) spectra at 298k and 8k were measured using a Hitachi F-4600 fluorescence spectrophotometer (Japan) equipped with a 150 W Xe lamp as the excitation source. The temperature-dependent luminescence properties were measured on the same spectrophotometer which was assembled with a computer-controlled electric furnace and a self-made heating attachment. The morphology was observed using high-resolution transmission electron microscopy (HRTEM; JEM-21000, JEOL, Japan). The room-temperature luminescence decay curves were obtained from a spectrofluorometer (Horiba, Jobin Yvon TBXPS) using a tunable pulse laser radiation (nano-LED) for the excitation.
Component | Result | Unit | Intensity | Spectral lines of the element |
---|---|---|---|---|
O | 23.5 | Mass% | 0.0745 | O-KA |
Si | 3.17 | Mass% | 3.064 | Si-KA |
P | 8.04 | Mass% | 20.233 | P-KA |
Ca | 18.7 | Mass% | 35.581 | Ca-KA |
La | 42.5 | Mass% | 6.245 | La-LA |
Eu | 1.55 | Mass% | 0.5759 | Eu-LA |
Fig. 2a displays the crystal structure of the 2 × 2 × 2 unit cells of Ca4La6(SiO4)4(PO4)2O2, which is chosen as the representative. Obviously, Ca4La6(SiO4)4(PO4)2O2 has a layered structure and contains two kinds of cation sites: the inner-laminar site labeled M(I) with the local symmetry C3 and the inter-laminar site labeled M(II) with the local symmetry Cs.22 The two kinds of different coordination environment of the cation sites are displayed in Fig. 2b and c. The M(I) site at the 4f site (C3) was surrounded by 9 oxygen atoms to form a mono-caped square antiprism, which was connected with tetrahedral PO4/SiO4 groups, and the M(II) site at the 6 h site (CS) formed a pentagonal bipyramid with the surrounding 7 oxygen atoms and these bipyramids were connected with each other through a vertex. Theoretically, both the Ca2+ ion and the La3+ ion are uniformly distributed in the two kinds of cationic sites,23 illustrating that the ratio of Ca/La is easily changed by adjusting the proportion of raw materials.
The four XRD patterns were analyzed using the Rietveld refinement. The observed (×), calculated (red) and difference (gray) XRD profiles for the refinements of Ca2+xLa8−x(SiO4)6−x(PO4)xO2 (x = 0,2,4,6) are shown in Fig. 3a–d. The main refinement parameters of the processing and refinement results are presented in Table 2. The results of the refinement further demonstrate that the series of solid solution phosphors are single phase without any impurity or secondary phases. On the other hand, the ranges of the weighted profile R-factor (Rwp) and the R-Bragg factor (RB) are 10.038%–11.012% and 1.792%–2.777%, respectively, indicating that the crystal structures of these phosphors match well with the starting model (Ca2La8(SiO4)6) after the refinement and that the results are believable and publishable. Meanwhile, we also refined the concentration of these samples while obtaining the high-quality XRD data. According to these refinement results, the calculated formula are Ca2.87(2)La7.13(2)(SiO4)6O2, Ca4.47(2)La5.53(2)(SiO4)3.53(2)(PO4)2.47(2)O2, Ca5.52(2)La3.48(2)(SiO4)1.48(2)(PO4)4.52(2)O2 and Ca8.28(2)La1.72(2)(PO4)6O2, demonstrating that the refined concentrations are highly consistent with the suggested formula and that the coordination environment variation is mainly caused by the replacement of a Ca2+ with a La3+ ion. Moreover, according to the XRD data and the Rietveld refinement, no additive superstructure peaks were detected, this feature proves that the Ca2+ ions and the La3+ ions were randomly mixed at the atomic level.24 In addition, the unit lattice parameters and the unit cell volumes of the as-prepared phosphors are given in Fig. 4. The high linear fitting coefficients (0.99334–0.99796) proved the crystal structure evolution of this continuous solid solution. The lattice parameters and unit cell volumes show linear decreases and are proportional to the value of x, which is attributed to the substitution of the large La3+ ions by small Ca2+ ions, suggesting that the coordination environment of the cations become more unconsolidated as x increases.25
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Fig. 3 (a–d) Powder XRD patterns (×) of the Ca2+xLa8−x(SiO4)6−x(PO4)xO2:0.02Eu2+ (x = 0,2,4,6) samples with the corresponding Rietveld refinement (red) and residuals (gray). |
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Fig. 4 The refined unit cell parameters (a, c) and cell volume (v) of Ca2+xLa8−x(SiO4)6−x(PO4)xO2:0.02Eu2+ (x = 0,2,4,6). |
Compound | x = 0 | x = 2 | x = 4 | x = 6 |
---|---|---|---|---|
Sp.Gr. | P63/m | P63/m | P63/m | P63/m |
a, Å | 9.6559(1) | 9.5948(6) | 9.5325(4) | 9.4606(2) |
b, Å | 9.6559(1) | 9.5948(6) | 9.5325(4) | 9.4606(2) |
c, Å | 7.1529(1) | 7.0882(5) | 7.0206(4) | 6.9356(1) |
α, ° | 90 | 90 | 90 | 90 |
β, ° | 90 | 90 | 90 | 90 |
γ, ° | 120 | 120 | 120 | 120 |
V, Å3 | 577.56(2) | 565.12(8) | 552.49(6) | 537.59(2) |
2θ-Interval, | 10–110 | 10–110 | 10–110 | 10–110 |
R wp, % | 10.038 | 11.012 | 10.135 | 10.065 |
R exp, % | 1.311 | 1.299 | 1.287 | 1.325 |
R B, % | 2.268 | 2.168 | 1.792 | 2.777 |
As shown in Fig. 5a–d, the linear change in the crystal structure of these solid solution phosphors was further verified by HRTEM and fast Fourier transform (FFT) images. Both the HRTEM and FFT images illustrate that no significant structural defects appeared in the selected areas of these single-phase samples and that good crystallinity was obtained. Moreover, the lattice fringe measurements with the d spacings of 0.315 nm, 0.837 nm, 0.354 nm, and 0.353 nm could be assigned to the planes (210), (010), (021) and (021) for Ca2+xLa8−x(SiO4)6−x(PO4)xO2:0.02Eu2+ (x = 0,2,4,6). The measured d spacing in different orientations could be transformed into the same d spacing value of (021) according to the classic Bragg equation.24 Therefore, the normalized d spacings of (021) were calculated to be 0.358 nm, 0.356 nm, 0.354 nm and 0.353 nm. Consequently, the decrease of the d spacings is well consistent with the refinement results, indicating the existence of structural evolution in the series of solid solutions.
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Fig. 5 HRTEM and FFT images for Ca2+xLa8−x(SiO4)6−x(PO4)xO2:0.02Eu2+ with different x values, x = 0 (a), x = 2 (b), x = 4 (c) and x = 6 (d). |
The effective ionic radii of the Ca2+ ions are 1.18 (CN = 9) and 1.06 Å (CN = 7) and the effective ionic radii of the La3+ ions are 1.21 (CN = 9) and 1.10 Å (CN = 7). Theoretically, considering the similar ionic radius and valence, the Eu2+ ion (RCN=9 = 1.3, RCN=7 = 1.2) is expected to substitute the La3+ and Ca2+ sites in the Ca2+xLa8−x(SiO4)6−x(PO4)xO2 (x = 0,2,4,6) crystal structure.26 Therefore, four kinds of emitting blocks will be included in the host: Ca(I), Ca(II), La(I) and La(II). The occupation rates of Ca(I), Ca(II), La(I), and La(II), reflecting the distribution of Ca2+ ions and La3+ ions in the two cationic sites, have been refined and displayed in Table 3. When the content of Ca2+ ions increases, the occupation rate of La(II) is decreased faster than that of La(I) and the M(II) site is totally occupied by Ca2+ ions while the chemical formula is Ca8La2(PO4)6O2 (x = 6), which shows similar results to the previous studies.16,26 The phenomenon can be explained as follows: the Eu2+ ion located at the M(II) site that is connected with a free oxygen ion, results in a very short Eu–O distance due to the small sum of the electrostatic bond strength of the cations toward the free oxygen ion. Thus, it must be very unfavorable for the (6 h) sites to be occupied by a cation with a large radius in these compounds.27
Sites | x = 0 | x = 2 | x = 4 | x = 6 |
---|---|---|---|---|
Ca1 | 0.12(2) | 0.20(2) | 0.43(1) | 0.714(7) |
La1 | 0.88(2) | 0.80(2) | 0.57(1) | 0.286(7) |
Ca2 | 0.53(1) | 0.81(1) | 0.983(7) | 1.000(6) |
La2 | 0.47(1) | 0.19(1) | 0.017(7) | 0.000(6) |
Fig. 6c and d display the low temperature (8k) PLE and PL spectra of Ca2La8(SiO4)6O2:0.02Eu2+ and Ca8La2(PO4)6O2:0.02Eu2+. The PL spectra of Ca2La8(SiO4)6O2:0.02Eu2+ can be separated into two components with peaks at 526 nm and 576 nm, and the PL spectra of Ca8La2(PO4)6O2:0.02Eu2+ obviously contains two components with peaks at 460 nm and 625 nm. The results further demonstrate that there are two kinds of cation sites included in the series of apatite phosphors which could be occupied by the Eu2+ ion.
Actually, considering the valence state and the previous results,16,29 the blue emission band observed in the PL spectrum of Ca2La8(PO4)6O2:0.02Eu2+ is attributed to the substitution of a Ca2+ ion by a Eu2+ ion. According to the report by Van Uitert, to further demonstrate the relationship between emission peaks and emission centers, the possible crystallographic site may be investigated theoretically by the following equation:30
![]() | (1) |
The emission wavelengths of the Ca2+xLa8−x(SiO4)6−x(PO4)xO2:0.02Eu2+ (x = 0,2,4,6) PL spectra show a wide blue shift from 508 nm to 460 nm with the increase of the x value which is dependent on the crystal field strength variation. The structural model of the cation substitution around the Eu2+ ion sites is depicted in Fig. 7. In this regard, the crystal field splitting of the Eu2+ ions can be determined as obeying:17,32,33
![]() | (2) |
In addition, as shown in Table 4, the stokes shifts were estimated to be 6135 cm−1–5985 cm−1 and the full width at half-maximum (FWHMs) of the PLE spectra decrease from 142 nm to 113 nm with the increase in x. The crystal-field splitting of the Eu2+ ions was estimated to be 22230 cm−1–18
190 cm−1, which is calculated by the gap between the first and the last component peaks of the PLE spectra. All the computations further demonstrate the decrease of the crystal field splitting.37
x Values | λ ex range (nm) | FWHM of λex (nm) | λ em (nm) | Stokes shift (cm−1) | Crystal field splitting (cm−1) |
---|---|---|---|---|---|
0 | 250–450 | 142 | 508 | 6135 | 22![]() |
2 | 250–450 | 127 | 500 | 6082 | 20![]() |
4 | 250–450 | 118 | 478 | 6039 | 19![]() |
6 | 250–400 | 113 | 460 | 5985 | 18![]() |
Furthermore, Fig. 8 presents the room temperature decay curves of the Eu2+ ion luminescence in the Ca2+xLa8−x(SiO4)6−x(PO4)xO2:0.02Eu2+ (x = 0,2,4,6) series. All of the decay curves can be well fitted with a second order exponential equation:
I(t) = A1 exp(−t/τ1)+A2 exp(−t/τ2) | (3) |
τ* = (A1τ12 + A2τ22)/(A1τ1 + A2τ2) | (4) |
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Fig. 8 Room temperature decay curves of the Ca2+xLa8−x(SiO4)6−x(PO4)xO2:0.02Eu2+ (x = 0,2,4,6) phosphors. |
The effective decay times were calculated to be 745.34, 468.61, 384.15 and 353.33 ns with x = 0, 2, 4 and 6, respectively. One can see that the decay times decrease with the increasing Ca2+ ion content. Due to the phase structures becoming more unconsolidated compared to the original Ca2La8(SiO4)4:0.02Eu2+ phase, the increasing possibility of energy transfer among the Eu2+ ions increases the possible non-radiative transition and leads to the decreasing lifetime values.32,38 Also the two decay components (τ1 and τ2) proved that the Eu2+ occupied two different Ca2+ sites.13
The temperature dependence experiment proved that the thermal stability is consistent with the crystal structure evolution in the as-prepared series phosphors, and the peak emission intensity that normalized to 25 °C values was depicted in Fig. 9. As shown in Fig. 9, the emission intensity of all the samples decreases with the increase in temperature. Additionally, the thermal stability gradually decreases with the increasing x values, this phenomenon can be explained by the neighboring-cation effect.39,40 The replacement of large La3+ ions by small Ca2+ ions makes the distances between the Eu2+ activator ion and the neighboring cations become smaller, as demonstrated by the refined cell parameters and cell volume, resulting in a larger coulombic force following the inverse-square law41,42 and the decrease of the thermal quenching barrier height. Thus, the thermal stability becomes lower when the replacement occurs.
Luminescence efficiency is an important technological parameter for the application of phosphors. The internal quantum efficiency (QE) of the Ca2+xLa8−x(SiO4)6−x(PO4)xO2:0.02Eu2+ (x = 0,2,4,6) phosphors was measured and calculated following:12
![]() | (5) |
The CIE coordinates and the digital photos of the Ca2+xLa8−x(SiO4)6−x(PO4)xO2:0.02Eu2+ (x = 0,2,4,6) phosphors under 365 nm excitation are displayed in Fig. 10. The calculated CIE coordinates are (0.2099, 0.4884) for x = 0, (0.2167, 0.3585) for x = 2, (0.1955, 0.2992) for x = 4 and (0.1846, 0.1851) for x = 6. Obviously, both the digital photos and the coordinates demonstrate that the emitted color of the solid solution phosphors Ca2+xLa8−x(SiO4)6−x(PO4)xO2:0.02Eu2+ (x = 0,2,4,6) can be adjusted in the wide range from green to blue by changing the ratio of Ca/La.
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Fig. 10 The CIE coordinates and the digital photos of the Ca2+xLa8−x(SiO4)6−x(PO4)xO2:0.02Eu2+ (x = 0,2,4,6) phosphors. |
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