Abstract
To develop new fluorescent and afterglow materials, Mn2+ and Eu3+ co-doped ZnO–GeO2 glasses and glass ceramics were prepared by a sol–gel method and their optical properties were investigated by measuring luminescence, excitation and afterglow spectra, and luminescence quantum yield (QY). Under UV irradiation at 254 nm, some glasses and all of the glass ceramics showed green luminescence peaking at 534 nm due to the 4T1 → 6A1 transition of tetrahedrally coordinated Mn2+ ions. The strongest luminescence was observed in a glass ceramic of 0.1MnO–0.3Eu2O3–25ZnO–75GeO2 heat treated at 900 °C, with QY of 49.8%. All of the green-luminescent glasses and glass ceramics showed green afterglow, and the afterglow lasting for more than 60 min was obtained in a glass ceramic heat treated at 900 °C. It is considered that the Eu3+ ions may behave as electron trapping centers to be associated with the occurrence of the green afterglow due to the Mn2+ ions in the co-doped system.
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1 Introduction
The research and development of phosphor materials are prosperous. Red (such as Y(P,V)O4:Eu3+ and (Y,Ga)BO3:Eu3+), green (such as Zn2SiO4:Mn2+ and (Y,Gd)BO3:Tb3+), and blue (such as BaMgAl10O17:Eu2+ and CaMgSi2O6:Eu2+) inorganic phosphors are typical ones used for optical displays such as cathode-ray tubes (CRTs), liquid crystal displays (LCDs), and plasma display panels (PDPs). In recent years, new displays such as organic electroluminescence displays have begun to be used practically, but the demand for thermally-stable inorganic phosphors is still large. Moreover, there is great interest in rare earth (RE) activated oxide glasses in the field of waveguide photonics [1, 2], and the sol–gel method is suitable to obtain these new optically functional materials.
Transition metal and rare earth ions serve as luminescence centers in inorganic oxide compounds. The Mn2+ ion shows strong luminescence, the color of which can be changed over the range 490–750 nm depending on host materials [3, 4], and a number of Mn-containing phosphors have been investigated. A typical phosphor of this type is Zn2SiO4:Mn2+ which shows clear and high luminosity green luminescence under UV or electronic excitation, and it has been used for first stage type color displays of CRTs and PDPs [5]. The Eu3+ and Eu2+ ions have been used for luminescence centers of red and blue inorganic phosphors, respectively, as mentioned above. Thus, Mn2+, Eu3+, and Eu2+ ions will serve as good luminescence centers in doped systems.
Moreover, new optical characteristics are expected in the Mn and Eu ions co-doped system; for example, strong upconversion luminescence due to both Mn2+ and Eu3+ ions was observed in co-doped ZnS nanoparticles [6], and white light-emitting Mn2+ and Eu2+ co-doped Ba3MgSi2O8 phosphors were synthesized through combustion process [7]. Long-lasting afterglow has also been reported in transition metal ions (like Mn2+)- and RE ions (such as Eu2+ and Dy3+)-doped systems [8, 9] and in an Mn and Eu co-doped system [10]. Almost all of those phosphors were heated or sintered under reducing atmospheres to reduce the selected rare earth ion (for example Eu3+ and Eu2+), but those with heat treatment in the air were only limited.
In the present study, we prepared ZnO–GeO2 glasses and glass ceramics co-doped with Mn2+ and Eu3+ ions by a sol–gel method. Optical properties of these materials were investigated by measuring luminescence, excitation and afterglow spectra, and luminescence quantum yield (QY). Especially, green, long-lasting afterglow due to Mn2+ ions was observed in the co-doped system.
2 Experimental
Mn2+ and Eu3+ co-doped ZnO–GeO2 glasses and glass ceramics were prepared by a sol–gel method. A starting solution consisted of tetraethoxygermanium (Ge(OC2H5)4) as a precursor of germanium dioxide, (CH3COO)2Zn·2H2O as a precursor of zinc oxide, C2H5OH and n-C4H9OH as solvents, H2O, and CH3COOH as the catalyst, with the molar ratio Ge(OC2H5)4:(CH3COO)2Zn·2H2O:C2H5OH:n-C4H9OH:H2O:CH3COOH = 1:0.33:10:10:1:0.1. To this solution, Mn(NO)3·6H2O and Eu(C5H7O2)3 as dopants were added in order to obtain oxides with final compositions of xMnO–yEu2O3–25ZnO–75GeO2 (x = 0.1–2.0, y = 0.05–2.0). The resulting solution was continuously stirred in a closed Teflon container for 1.5 h at room temperature to prepare sol solution. To obtain dried gels, the sol solution was placed in a lid-free Teflon container and kept at 70 °C under drying atmosphere for 2 weeks, and then at 100 °C for 1 week. The dried gels were heat treated at 630 °C to obtain glasses, and at 700–1,000 °C to obtain glass ceramics. These heat-treatment processes were carried out under the air.
For luminescence spectral measurements, samples were powdered sufficiently using an agate mortar and a pestle. Luminescence, excitation, and afterglow spectra were recorded on a fluorescence spectrometer (Hitachi F-4500) with an Xe lamp as an excitation source; luminescence from the illuminated surface of the sample was collected at the right angle to the direction of the excitation light. Decay curves were recorded similarly, after 254-nm irradiation for 5 min with a handy UV lamp. QY values were obtained by an absolute photoluminescence quantum yield measurement system (Hamamatsu C9920-02) under excitation at 254 nm with an Xe lamp as an excitation source. X-Ray diffraction (XRD) patterns were recorded on an X-ray diffractometer (Rigaku RINT-2200) with CuKα radiation.
3 Results and discussion
All samples heat treated at 630 °C were amorphous (glasses). Figure 1 shows luminescence spectra of xMnO–yEu2O3–25ZnO–75GeO2 glasses under UV excitation at 254 nm. A green luminescence spectrum peaking at 534 nm is due to the 4T1 → 6A1 transition of tetrahedrally coordinated Mn2+ ions [11–13]. On the other hand, red luminescence spectra peaking at 592, 612, 650, and 700 nm are due to the 5D0 → 7F1, 5D0 → 7F2, 5D0 → 7F3, and 5D0 → 7F4 transitions of Eu3+ ions, respectively, and these luminescence are quite weak compared with the green one. The strongest red luminescence was due to the hypersensitive transition 5D0 → 7F2 of Eu3+ ions [14–16]. According to the parity selective rule of the electronic transition, if the Eu3+ ion was in a non-central symmetric site, the 5D0 → 7F2 transition could be observed much stronger than that of the 5D0 → 7F1 transition [15]. Therefore, it is thought that Eu3+ ions occupied in a site with lower local site symmetry in the present glass samples. Neither green nor red luminescence was observed in the glasses with x ≥ 1.0. Green luminescence becomes dominant in the glasses with y ≤ 0.4, but red luminescence does in the glasses with y ≥ 0.5. Excitation spectra for 612-nm luminescence of Eu3+ are shown in Fig. 2. Absorption bands due to Eu3+ ions were observed in the sample with (x, y) = (0.1, 0.5) which showed red luminescence from Eu3+ ions as shown in Fig. 1. An Eu3+ absorption band at around 530 nm in Fig. 2 is located at almost the same wavelength as the green luminescence from Mn2+ in Fig. 1. Therefore, it is believed that the Eu3+ ions could absorb the emission energy from Mn2+ and red luminescence became dominant with increasing the Eu3+ concentration in the glass samples.
Figure 3 shows luminescence spectra of xMnO–yEu2O3–25ZnO–75GeO2 glass ceramics under UV excitation at 254 nm. Results of XRD measurements show that these glass ceramics consist of rhombohedral Zn2GeO4 and hexagonal GeO2 (Fig. 4). All of these glass ceramics heat treated at 800–1,000 °C showed strong green luminescence due to the 4T1 → 6A1 transition of the Mn2+ ion, regardless of the value of y. The glass ceramics heat treated at 800 °C show weak, red luminescence around 610 nm due to the Eu3+ ion, however this red luminescence was not observed in the spectra of glass ceramics heat treated at 900 and 1,000 °C. Moreover, unlike the glasses, the glass ceramics with x ≥ 1.0 showed green luminescence, but those intensities are weak, therefore the concentration quenching is believed to start to occur at x = 1.0. It is considered that Eu3+ ions existing in the grain boundary were aggregated to clusters in host lattice upon crystallization of host matrix, resulting in the concentration quenching.
Figure 5 shows excitation spectra for green luminescence in the xMnO–yEu2O3–25ZnO–75GeO2 glass ceramics. In all samples, strong and broad excitation bands were observed at 250 and 310 nm. Undoped and Mn-doped GeO2 show a broad absorption band around 250 nm, therefore, it is thought that the 250-nm excitation band in Fig. 5 is a host absorption band or a charge transfer (CT) band associated with Mn2+ [17–19]. The 310-nm broad absorption band was not observed in the excitation spectra of GeO2 and MnO–ZnO–SiO2 [19, 20]. Thus, it is considered that the 310-nm absorption band is due to the host material of Zn2GeO4 [13].
Strong luminescence was observed in the samples with x = 0.1, and their QY values are shown in Fig. 6. In the samples that showed red luminescence due to the Eu3+ ion, QY values were too weak to measure. Large QY values were obtained in the samples heat treated at 900 °C, with the maximum QY value of 49.8% in the glass ceramic with y = 0.3.
The longest afterglow was observed in the glass ceramic heat treated at 900 °C, the spectra of which were measured at the average interval of 4 min up to 60 min after 254-nm UV irradiation for 5 min as shown in Fig. 7a. The afterglow could be observed by naked eyes for several minutes under irradiation by a commercially available fluorescent lamp. Such a long afterglow has not been observed in Eu3+-undoped MnO–ZnO–GeO2 glass ceramics [13]. Figure 7b shows decay curves of the 534-nm afterglow for 0.1MnO–0.3Eu2O3–25ZnO–75GeO2 glasses and glass ceramics with high QY values.
Thus, it is considered that Eu3+ ions may play some roles in trapping the excitation energy and transferring it to Mn2+ ions in MnO–Eu2O3–ZnO–GeO2 glass ceramics in the present study. The energy transfers from Eu2+ or various vacancies to Mn2+ in long-lasting afterglow have been well known and possible mechanisms for these energy transfers reported [10, 12], however, we could not detect experimentally the existence of Eu2+ ions or vacancies in the present samples. Therefore, it is considered that Eu3+ ions in our samples, Mn2+ and Eu3+ co-doped ZnO–GeO2 glasses and glass ceramics, may become electron trapping centers. Previous studies [8–10, 12] and the above results lead to a possible mechanism of long-lasting afterglow of Mn2+ in this study as shown in Eqs. 1–4.
During UV irradiation (Eqs. 1 and 2), the photo-oxidization of Mn2+ would occur and an excited electron e − would be generated. These electrons would be trapped at Eu3+ and an Eu2+-liked energy trapping species, (Eu3+)−, would be produced.
After stopping UV irradiation (Eqs. 3 and 4), the trapped electron would be released from (Eu3+)− with thermal excitation and recombine with (Mn2+)+, then green long-lasting afterglow from Mn2+ would be emitted.
4 Conclusions
ZnO–GeO2 glasses and glass ceramics co-doped with Mn2+ and Eu3+, xMnO–yEu2O3–25ZnO–75GeO2, were prepared by the sol–gel method. Under excitation at 254 nm, the glasses with y ≤ 0.4 showed green luminescence peaking at 534 nm due to the 4T1 → 6A1 transition of tetrahedrally coordinated Mn2+ ions, and those with y ≥ 0.4 showed red luminescence peaking at 592, 612, 650, and 700 nm due to the 5D0 → 7FJ (J = 1, 2, 3, 4) transitions of Eu3+ ions, regardless of the value of x. All of the glass ceramics show green luminescence; the strongest luminescence is observed in a 0.1MnO–0.3Eu2O3–25ZnO–75GeO2 glass ceramic heat treated at 900 °C with luminescence quantum yield of 49.8%. The 534-nm green afterglow due to the Mn2+ ion was observed in all of the green-luminescent glasses and glass ceramics, while no afterglow was observed in the red-luminescent glasses. The long afterglow lasting for more than 60 min is obtained in a glass ceramic heat treated at 900 °C. In these glasses and glass ceramics, the Eu3+ ions may behave as electron trapping centers to be associated with the occurrence of the green afterglow.
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Sanada, T., Seto, H., Morimoto, Y. et al. Luminescence and long-lasting afterglow in Mn2+ and Eu3+ co-doped ZnO–GeO2 glasses and glass ceramics prepared by sol–gel method. J Sol-Gel Sci Technol 56, 82–86 (2010). https://doi.org/10.1007/s10971-010-2278-6
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DOI: https://doi.org/10.1007/s10971-010-2278-6