Ryohei Oka,
Yusuke Shobu,
Fumiya Aoyama,
Takashi Tsukimori and
Toshiyuki Masui*
Department of Chemistry and Biotechnology, Graduate School of Engineering, Tottori University, 4-101, Koyama-cho Minami, Tottori 680-8552, Japan. E-mail: masui@chem.tottori-u.ac.jp; Fax: +81-857-31-5264; Tel: +81-857-31-5264
First published on 4th December 2017
Reddish-brown SrY2−xCexO4 (0 ≤ x ≤ 1.2) solid solutions were synthesized by a citrate sol–gel method as novel environmentally friendly inorganic pigments. The powders obtained were characterized by X-ray powder diffraction (XRD), UV-vis diffuse reflectance spectra and CIE L*a*b*Ch° chromatic coordinate measurements. All SrY2−xCexO4 (0 ≤ x ≤ 1.2) samples were obtained in a single-phase form and the lattice volume increased on increasing the Ce3+ concentration. The reddish-brown pigments exhibited optical absorption due to the 4f–5d allowed transition of Ce3+. The absorption bands observed in the wavelength region of 400 and 550 nm were due to the Ce3+ ions in the ideal octahedral Y3+ site and those in the longer wavelength region above 600 nm were attributed to the transition of Ce3+ in the distorted octahedral Y3+ site. The samples gradually became reddish on increasing the Ce3+ content. The most reddish colour was obtained in SrYCeO4 (a* = +21.8).
Because of this situation, we focused on a trivalent cerium (Ce3+) ion as a red colouring source. As an example of a popular Ce3+-containing material, Ce3+-doped yttrium aluminium garnet, (Y, Ce)3Al5O12 (YAG:Ce3+), has been well known as a yellow-emitting phosphor widely used in white light emitting diodes. YAG:Ce3+ absorbs the visible lights in the wavelength region of 410 to 500 nm,28–30 which is attributed to the 4f–5d allowed transition. The absorption wavelength due to the Ce3+ ions depends on the host crystal structure, because the energy level of the 5d orbital of Ce3+ is strongly affected by the crystal field strength around the Ce3+ ions. In the case of a phosphor, the amount of Ce3+ is about 1 mol% to prevent concentration quenching, but it is considered that colouring of the sample can be seen by further increasing the Ce3+ concentration. Furthermore, it is expected that strong reddish colour will be obtained if Ce3+ is doped at a high concentration in the Y3+ site in the lattice with a stronger crystal field.
In this study, we selected SrY2O4 as a host material, because this compound is composed of non-toxic elements. SrY2O4 belongs to the CaFe2O4-related structure, and it crystallizes into an orthogonal structure with space group Pnma. Four formula units for a total of 28 atoms are contained in the SrY2O4 structure. All of the constituent atoms occupy 4c sites according to the Wyckoff notation.31 The Sr2+ and Y3+ ions are coordinated by eight and six O2− ions, respectively. Y3+ occupies two non-equivalent sites Cs symmetry, where one Y(1) site is nearly a regular octahedron but the other Y(2) one is much distorted.32 Since it has been reported that high calcination temperature is necessary for the synthesis of SrY2O4 by a solid-state reaction,33,34 SrY2−xCexO4 (0 ≤ x ≤ 1.2) pigments were synthesized using a citrate sol–gel method. The optical and colour properties of the samples were evaluated as novel environmentally friendly inorganic reddish-brown pigments.
The morphology of the SrYCeO4 particles was investigated by using field-emission-type scanning electron microscopy (FE-SEM; JEOL, JSM-6701F). The optical reflectance spectra were measured with a UV-vis spectrometer (Shimadzu, UV-2550 with an integrating sphere attachment) with barium sulphate as a reference. The colour properties of the samples were evaluated in terms of the CIE L*a*b*Ch° system using a chromometer (Konika-Minolta, CR-300). The L* parameter indicates the brightness or darkness of a colour relative to a neutral grey scale, and the a* (the red-green axis) and b* (the yellow-blue axis) parameters express the colour qualitatively. Chroma parameter (C) represents the colour saturation of the pigments and is calculated according to the following formula: C = [(a*)2 + (b*)2]1/2. The parameter h° ranges from 0 to 360°, and is calculated with the formula, h° = tan−1(b*/a*). X-ray photoelectron spectra measurements (XPS; ULVAC-PHI, PHI5000 VersaProbe II) using Mg-Kα radiation were carried out to investigate the oxidation state of the cerium ion on the surface of the as-synthesized and the calcined SrYCeO4 samples.
x | Lattice volume/nm3 |
---|---|
0 | 0.410 |
0.2 | 0.411 |
0.4 | 0.413 |
0.6 | 0.414 |
0.8 | 0.418 |
1.0 | 0.420 |
1.2 | 0.422 |
The Rietveld analysis of the XRD data of the SrY2−xCeO4 (x = 0, 0.2, and 1.0) samples was carried out to determine the site occupancy of the Y(1) and the Y(2) sites. The Rietveld refinement profiles of the samples are shown in Fig. 2, and the detailed crystallographic data and structure refinement parameters are summarized in Tables 2 and 3, respectively. Fig. 3 shows the crystal structure of SrY2O4 illustrated using the VESTA program based on the crystallographic data from the Rietveld refinement.37 As seen in Table 2, the low R-factors were obtained for all the SrY2−xCexO4 (x = 0, 0.2, and 1.0) samples. The Rietveld refinements revealed that the Ce3+ concentrations at the Y(1) site gradually increased from 16 to 64 mol%, while that in the Y(2) site increased from 4 to 36 mol% as x increased from 0.2 to 1, as seen in Table 3. Therefore, in the SrY2−xCexO4 structure, Ce3+ ions occupied both Y(1) and Y(2) sites. Although each Y site is coordinated by six oxide anions, one Y(1) site is located in the ideal octahedral coordination environment and the other Y(2) site is significantly distorted, as shown in Fig. 3. This difference of structural distortion of two non-equivalent Y sites affects the Ce3+ occupancy. In fact, the occupancy ratio, Ce2/Ce1, was 0.25 for SrY1.8Ce0.2O4 (x = 0.2), while it was 0.56 for SrYCeO4 (x = 1). These results indicate that the Ce3+ ions were preferentially located in the energetically favoured ideal octahedral Y(1) site when the Ce3+ concentration was low, and suggest that the distorted Y(2) site were also begun to be occupied when the Ce3+ concentration was increased and the solubility in the Y(1) sites were saturated.
x = 0 | x = 0.2 | x = 1 | |
---|---|---|---|
a Crystal symmetry: orthorhombic, space group: Pnma, number of formula units per unit cell: Z = 4. | |||
Cell data | |||
a (nm) | 1.007815(7) | 1.008700(5) | 1.01202(1) |
b (nm) | 0.340805(2) | 0.341514(2) | 0.345788(4) |
c (nm) | 1.191426(8) | 1.193350(7) | 1.20445(1) |
V (nm3) | 0.409217(5) | 0.411091(4) | 0.421491(8) |
R factor | |||
Rwp | 3.398 | 4.785 | 6.478 |
Rp | 2.536 | 3.474 | 4.370 |
Re | 2.662 | 2.716 | 3.119 |
S | 1.277 | 1.761 | 2.163 |
RF | 1.456 | 3.781 | 3.701 |
SrY2O4 (x = 0)b | |||||
---|---|---|---|---|---|
Atom | Occupancy | x | y | z | Uiso (nm2) |
a All atoms are placed at general 4c positions.b At refinement of SrY2O4, isotropic atomic displacement parameters (Uiso) of four oxygen atoms were constrained to be equal.c Because of the disordering of Y and Ce atoms, the fractional coordinate and Uiso were constraint to the same values, respectively. In order to refine the occupation ratio of Ce atoms, Uiso parameters of Sr, Y and O atoms were fixed to the respective values of each atoms at non-doped SrY2O4. | |||||
Sr | 1 | 0.24722(9) | 1/4 | 0.64940(9) | 0.000087(2) |
Y1 | 1 | 0.0775(1) | 1/4 | 0.38967(7) | 0.000067(3) |
Y2 | 1 | 0.5762(1) | 1/4 | 0.61230(7) | 0.000086(3) |
O1 | 1 | 0.2861(5) | 1/4 | 0.3235(4) | 0.0001303 |
O2 | 1 | 0.3729(5) | 1/4 | 0.0193(5) | 0.0001303 |
O3 | 1 | 0.4852(5) | 1/4 | 0.7820(4) | 0.0001303 |
O4 | 1 | 0.07423(6) | 1/4 | 0.0767(4) | 0.0001303 |
SrY1.8Ce0.2O4 (x = 0.2)c | ||||
---|---|---|---|---|
Atom | Occupancy | x | y | z |
Sr | 1 | 0.2483(1) | 1/4 | 0.64917(1) |
Y1 | 0.84(1) | 0.0772(1) | 1/4 | 0.3891(1) |
Y2 | 0.96 | 0.5780(2) | 1/4 | 0.6125(1) |
Ce1 | 0.16 | 0.0772 | 1/4 | 0.3891 |
Ce2 | 0.04 | 0.5780 | 1/4 | 0.6125 |
O1 | 1 | 0.2871(8) | 1/4 | 0.3236(7) |
O2 | 1 | 0.3742(7) | 1/4 | 0.0188(7) |
O3 | 1 | 0.4822(8) | 1/4 | 0.7832(6) |
O4 | 1 | 0.078(1) | 1/4 | 0.0770(6) |
SrYCeO4 (x = 1)c | ||||
---|---|---|---|---|
Atom | Occupancy | x | y | z |
Sr | 1 | 0.2509(3) | 1/4 | 0.6482(2) |
Y1 | 0.36(1) | 0.0746(2) | 1/4 | 0.3880(2) |
Y2 | 0.64 | 0.5844(3) | 1/4 | 0.6118(2) |
Ce1 | 0.64 | 0.0746 | 1/4 | 0.0746 |
Ce2 | 0.36 | 0.5844 | 1/4 | 0.5844 |
O1 | 1 | 0.278(2) | 1/4 | 0.319(1) |
O2 | 1 | 0.374(1) | 1/4 | 0.012(2) |
O3 | 1 | 0.487(1) | 1/4 | 0.787(1) |
O4 | 1 | 0.086(2) | 1/4 | 0.079(1) |
Fig. 3 Crystal structure obtained by the Rietveld analysis for SrY2O4 (a), and the octahedral coordination environment of Y(1)O6 and Y(2)O6 in SrY2O4 (b). |
Fig. 4 shows the FE-SEM images of the SrYCeO4 (x = 1) sample at different magnifications. Since it was synthesized at a high temperature of 1300 °C, the primary particles melted to form large secondary particles.
These results are considered to be due to the existence of two non-equivalent octahedral Y sites of different coordination environments in the crystal structure of SrY2O4. As mentioned above, Y(1) site is located in the ideal octahedral coordination environment and the other Y(2) site is significantly distorted,31 as illustrated in Fig. 3. The band structure models of the ideal Y(1) and the distorted Y(2) sites in the SrY2−xCexO4 (0 ≤ x ≤ 1.2) samples are illustrated schematically in Fig. 6. The valence band (VB) and the conduction band (CB) consist of O2p and Y3d orbitals, respectively. When the Ce3+ ions are doped into the SrY2O4 lattice, the 4f and 5d energy levels of Ce3+ are introduced between VB (O2p orbital) and CB (Y3d orbital). Since the crystal field energy around the Ce3+ ions in the distorted Y(2) site is stronger than that in the ideal Y(1) site, the 5d orbital energy splitting of Ce3+ in the Y(2) site is also larger than that in the Y(1) site. As already discussed, the Ce3+ preferentially occupies the ideal Y(1) in the low Ce3+ concentration sample, and the Y(2) occupancy was increased with increasing the Ce3+ concentration.
Fig. 6 Band structure models of the ideal octahedral Y(1) site (a) and the distorted Y(2) site (b) in the SrY2−xCexO4 (0 ≤ x ≤ 1.2) pigments. |
Accordingly, the optical absorption at 600 nm and longer wavelengths was observed in the samples with high Ce3+ concentration.
x | L* | a* | b* | C | h° |
---|---|---|---|---|---|
0 | 98.2 | −0.24 | +1.69 | 1.71 | 98.1 |
0.2 | 83.3 | +1.78 | +36.3 | 36.3 | 87.2 |
0.4 | 68.6 | +10.2 | +45.3 | 46.4 | 77.3 |
0.6 | 68.4 | +10.5 | +43.3 | 44.6 | 76.4 |
0.8 | 57.3 | +20.4 | +44.1 | 48.6 | 65.2 |
1.0 | 49.1 | +21.8 | +42.2 | 47.5 | 62.7 |
1.2 | 42.8 | +19.7 | +36.5 | 41.5 | 61.6 |
The colour of the samples after the thermal and chemical stability tests were evaluated using the colorimeter. The colour coordinate data are summarized in Table 5. Unfortunately, the heat resistance of this sample was low, and the colour degradation was observed after heating the present SrYCeO4 pigment at 300 °C and above in air. On the other hand, the SrYCeO4 pigment has chemical stability. The colour was almost unchanged after the leaching test in the acetic acid and ammonium bicarbonate solutions.
Pigment | L* | a* | b* | C | h° |
---|---|---|---|---|---|
As synthesized | 49.1 | +21.8 | +42.2 | 47.5 | 62.7 |
300 °C in air | 94.5 | −0.33 | +3.12 | 3.14 | 96.0 |
500 °C in air | 95.4 | −0.94 | +3.41 | 3.54 | 105 |
4% CH3COOH | 49.3 | +17.5 | +41.1 | 44.7 | 66.9 |
4% NH4HCO3 | 46.7 | +18.7 | +40.6 | 44.7 | 65.3 |
In order to investigate the reason for the color degradation after the heating in air, oxidation state of the cerium ions of the SrYCeO4 samples was identified by the XPS measurement before and after the heat resistance tests. The Ce (3d3/2) and Ce (3d5/2) XPS obtained from the SrYCeO4 sample before and after the heat resistance tests are shown in Fig. 8. In addition to the binding energy peaks for Ce3+ at 884.2 (V′) and 902.4 (U′) eV, four peaks corresponding to Ce4+ species on the surface of the non-treatment sample were observed at 881.1 (V), 897.4 (V′′′), 899.8 (U) and 914.5 (U′′′) eV.40,41 The labels U and V refer to the Ce (3d3/2) and Ce (3d5/2) spin–orbit components. The intensities of two peaks assigned to Ce3+ decreased with increasing the calcination temperature, in comparison with those of the as-synthesized sample. Therefore, the colour degradation will be caused by the oxidation of Ce3+ to Ce4+.
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