Ting Zhang,
Ai Du*,
Chuanxiang Chen,
Xiujie Ji,
Bin Zhou,
Jun Shen and
Zhihua Zhang
Shanghai Key Laboratory of Special Artificial Microstructure Materials and Technology, School of Physics Science and Engineering, Tongji University, Shanghai 200092, China. E-mail: duai@tongji.edu.cn; Tel: +86 21 6598 6071
First published on 22nd October 2019
A ZnGa2O4:Cr3+-based aerogel was prepared by using polyacrylic acid (PAA) as a dispersant and propylene oxide (PO) as a crosslinking agent via CO2 supercritical drying. The results of BET and SEM show that there is a certain degree of macroporosity (d > 50 nm) in the aerogel. It has a dendritic structure and the interior is relatively loose. EDS mapping illustrates that the elements Zn, Ga, and Cr are evenly distributed in the aerogel. In addition, the diffuse reflectance spectra and the emission spectrum of samples with different calcination temperatures were also characterized. Both demonstrated, when the calcination temperature is greater than 600 °C, that the sample crystallizes and has a significant emission, which is consistent with the XRD and TG-DSG results. Finally, the ZnGa2O4:Cr3+-based aerogel also exhibits excellent long afterglow performance and high photocatalytic performance with 80.1% methylene blue (MB) degradation at 20 min.
As a good luminescent material matrix, it shows various emission colors when doped with different transition metal ions or rare earth ions, such as Cr3+, Mn2+, Eu3+ or Ce3+.2,3,13–15 The near-infrared luminescence of Cr3+ was reported as early as 1988, but the Cr3+ doped with ZnGa2O4 near-infrared luminescent material was rarely reported. The first report on near infrared-persistent luminescence in Cr3+ doped ZnGa2O4 by Bessière et al. in 2011.16 ZnGa2O4:Cr3+ is a bright red emitting long-lasting phosphor when ultraviolet excited with the emission range of 650–750 nm.
The reported ZnGa2O4:Cr3+ is mostly synthesized by high temperature solid state method. This method produces large particles, irregular morphology and sinter clustering. The researchers focused on finding a way to synthesize ZnGa2O4:Cr3+ at low temperatures and even in solution. Under this condition, it is beneficial to adjust the shape of the material and control its size. The sol–gel method gives an excellent control over the stoichiometry, introducing dopant easily and allowing lower processing temperature compared to other methods.13 The citrate sol–gel technique is the most common. But its only can obtained nanopowders instead of monolith. And the sample density is larger, the pores are less and the pore size is small.
A new sol–gel method for preparation of ZnGa2O4:Cr3+ long afterglow materials. In this paper, PAA and PO are used as a dispersant and a crosslinking agent to prepare a ZnGa2O4:Cr3+-based (with ZnO as the skeleton) aerogel. ZnGa2O4:Cr3+ has potential application value in bioprobe technology due to its excellent near-infrared long afterglow luminescence. The ZnGa2O4:Cr3+-based aerogel prepared by this method has more macropores, can be used as a drug carrier because of its sustained release effect. Also, monolith ZnGa2O4:Cr3+-based aerogel have a significant role in the field of hypervelocity particle capture. When space debris or comet particles impact this aerogel, as the depth of penetration increases, the aerogel heated temperature gradually decreases. Thus creating a temperature gradient on the track. Therefore, according to the difference of luminous intensity, the heating temperature at each position of the track can be derived. This is of great significance for solving the thermal interaction between hypervelocity particles and aerogels.
![]() | ||
Fig. 1 (a) The appearance, (b) SEM picture and (c) the N2 adsorption–desorption isotherms of ZnGa2O4:Cr3+-based aerogel, inset is the pore size distribution. |
![]() | ||
Fig. 2 The (a) TEM picture of ZnGa2O4:Cr3+-based aerogel and EDS mapping images of (b) Zn, (c) Ga and (d) Cr element. |
Fig. 3 shows the XRD patterns of the samples with various calcined temperatures. It can be seen that the aerogel exhibits nanocrystalline properties after calcination at least 600 °C, and the sample calcined at 500 °C is amorphous. The peaks of the curves in the Fig. 3 correspond to No. 30-1240 in the JCPDS document, indicating that the sample is a cubic crystal spinel structure. The sample has crystallized at 600 °C and a broad diffraction peak appears. As the calcination temperature increases, the diffraction peaks gradually become stronger and sharper. We attribute it to an increase of crystallinity. It can be seen from Fig. S2† that the crystallization temperature of the reference sample increased from 600 °C to 700 °C.
FTIR spectra of the ZnGa2O4:Cr3+-based aerogel calcined at various temperatures are shown in Fig. 4(a). The broad band at 3430 cm−1 is due to the stretching vibration of H2O, indicating the existence of water absorbed in the samples. PAA commonly used as both a water absorbing agent and a dispersing agent. In this experiment, the aerogel prepared by using PAA as a dispersing agent is also easy to absorb water. The band at 1600 cm−1 represents the stretching vibrations of COO− groups of PAA. It shows that the sample contains impurities and the organic matter is not completely decomposed. The band between 1000 cm−1 to 1300 cm−1 is due to the vibration of the NO3− group. With the increasing of temperature, the above mentioned bands became weaker. Since the aerogel is based on ZnO, the Zn–O adsorption peak (589 cm−1) appears in the infrared spectrum of all samples. When the temperature reaches 600 °C, another adsorption peak appear at 420 cm−1 (Ga–O), which also indicating the formation of ZnGa2O4 nanocrystals. Unlike ZnGa2O4:Cr3+-based aerogel, there is no Zn–O (∼589 cm−1) adsorption peak (Fig. S3(a)†) in the uncalcined reference sample. When the temperature reached 700 °C, two adsorption peaks appeared at ∼586 cm−1 (Zn–O) and ∼420 cm−1 (Ga–O), indicating the formation of ZnGa2O4 nanocrystals. Fig. 4(b) shows TG-DSG results of the aerogel. The decrease in mass within 100 °C is attributed to the evaporation of adsorbed moisture. In the range of 100 °C to 360 °C, it can be seen slight weight loss due to decomposition of some organic groups. The strong exothermic peak at 410 °C accompanied weight loss is mainly due to the decomposition of PAA and some residual organic matter. The sample at 600–800 °C is in the endothermic process and the mass remains unchanged, indicating the formation of ZnGa2O4 nanocrystals. The crystallinity of the sample increases and the particles gradually increase during this process. However, an exothermic peak appeared at 900 °C should attribute to loss of ZnO during firing. The vapor pressure of ZnO is relatively high.15 But as shown in Fig. S3(b),† there is no excess ZnO in reference sample, so there is no exothermic peak at 900 °C.
![]() | ||
Fig. 4 (a) FTIR spectra as a function of calcined temperature; (b) TG-DSG result of the ZnGa2O4:Cr3+-based aerogel before calcined. |
UV-visible diffuse reflectance spectra and the photoluminescence emission spectrum of the samples are shown in Fig. 5. The spectra of the samples both present two additional absorption bands at 550 nm and 430 nm which attributed to 4A2 (4F)–4T2 (4F) and 4A2 (4F)–4T1 (4F) transitions of Cr3+, respectively.19,20 The third peak is about 260 nm, we attribute this band to the spin-allowed 4A2 (4F)–4T1 (4P) absorption transition of Cr3+. Three excitation peaks attributed to three d–d absorption bands of Cr3+.21 From Fig. S4(a),† the UV-visible diffuse reflectance spectra of reference sample is the same as ZnGa2O4:Cr3+-based aerogel. It can be seen from the PL emission spectrum that the sample starts to glow after being calcined at 600 °C. This is consistent with the XRD results. Therefore, the UV-visible spectrum of the sample calcined at 500 °C cannot be excited. The higher the calcination temperature, the greater the luminous intensity. It can be seen from the Fig. 5(b) that the sample has a broad emission peak with a peak value of 696 nm. This typical emission peak is attributed to the 2E–4A2 transition of Cr3+ in the ZnGa2O4 luminescent matrix.22 The emission peak at 713 nm is ascribed to the short-range perturbations of the octahedral sites surrounding Cr3+. These perturbations are caused by crystal defects and can manifest in the form of separate bands.23,24 Fig. S4(b)† illustrates that the reference sample starts to glow after being calcined at 700 °C. Unlike ZnGa2O4:Cr3+-based aerogel, ZnGa2O4:Cr3+ aerogels not have the emission peaks at 696 nm and 713 nm, but a large span of light-emitting region at 700–950 nm. However, if aerogels are used in the field of hypervelocity particle capture, we prefer that materials emit red light instead of infrared. This makes it easy to observe the tracks with a microscope.
![]() | ||
Fig. 5 (a) The UV-visible diffuse reflectance spectra and (b) the PL emission spectrum of the ZnGa2O4:Cr3+-based aerogels with different calcination temperatures. |
Since the luminescence intensity of the samples calcined at 800 °C is the highest, we have characterized its PL decay properties and as shown in Fig. 6(a). When the excitation light is removed, the fluorescence intensity drops to 1/e of the maximum fluorescence intensity I0 at the time of excitation, which is called the fluorescence lifetime τ. The bi-exponential represents two types of radiation channels, one is the emission between the conduction band and the valence band, and the other is the defect emission. The decay curves can be well fitted with a bi-exponential equation as given in the following expression:
![]() | (1) |
τ = (A1τ12 + A2τ22)/(A1τ1 + A2τ2) | (2) |
The fitting data is shown in Table 1. The decay process of the long-lasting phosphorescence can be divided into two parts: the fast process and the slow process. And the decay time is mainly determined by the slow part. Fig. 6(b) illustrates the energy levels involved in the energy transfer mechanism between ZnGa2O4 and Cr3+ and the subsequent emission from Cr3+. The sample is excited by 254 nm UV light (high energy), and the incident photon is absorbed by the ZnGa2O4 (host), causing the electron to directly transition from the valence band to the conduction band. Electrons are transferred from the conduction band to the corresponding trap and captured due to thermal radiation and conduction band assist. The electron traps and hole traps are the energy states of storing excited electrons and holes, the energy can be stored for a period of time. However, after UV irradiation stopped, some electrons will break free from the shallow trap and transfer to the 4T1 energy level of Cr3+. The electrons trapped in the trap center transfer part of the energy to the Cr3+, causing the electrons of Cr3+ to excite from the ground state (4A2) to the three excited state levels of 2E, 4T1, and 4T2. The excited Cr3+ electrons return to the ground state by emitting photons of different energy.13,25 This produces a near-infrared long afterglow phenomenon which attribute to the sustained energy transfer of the host ZnGa2O4.26
A1 | τ1 (s) | A2 | τ2 (s) | τ (s) | R2 |
---|---|---|---|---|---|
7359.79 | 2.69 | 1430.79 | 36.06 | 26.81 | 0.98 |
The degradation of methylene blue (MB) dye was measured as a function of irradiation time of ZnGa2O4:Cr3+-based aerogels, and samples with different calcination temperatures was also tested for comparison. The sample without calcination exhibits high photocatalytic performance with 80.1% MB degradation at 20 min, much better than other materials. In addition, it can be seen that the adsorption effect of aerogel is also very good. After 40 minutes in the dark room, the adsorption rate reached 40%. However, the degradation rate of the calcined sample is slower and more uniform. The experimental results show that the heat treatment has a great influence on the photocatalytic and adsorption properties. As the calcination temperature gradually increases, the characteristic surface area of aerogels decrease and the particle volume increases, resulting in a decrease in catalytic activity. The morphology of the samples after calcined were characterized by SEM, as shown in Fig. 7. Obviously, the morphology changes from porous loose dendrites to dense spherical stacked structures. The pore structure almost disappears and the clusters are very tightly bound. This may be due to structural collapse of the sample during calcination. The SEM images are consistent with the conclusion obtained by photocatalytic. To support this conclusion, we characterized the N2 adsorption–desorption isotherms of calcined samples with different temperatures, as shown in Fig. 8. As the temperature increases, the specific surface area of the samples is 84.3 m2 g−1, 61.6 m2 g−1, 48.9 m2 g−1, 30.7 m2 g−1 (Table 2). Compared with Fig. 1(c), it is much reduced, once again proving this conclusion. In addition, photocatalytic and long-lasting luminescence are significantly associated. In the ZnGa2O4 host, a part of photo-generated electrons and holes recombine to release energy in the form of photoluminescence. And some of them can be trapped by lattice defects, impurities or Cr3+. The photo-generated electrons and holes are trapped to slow down the recombination process, which will enhance charge transfer and photocatalytic activity. On the other hand, after stopping the UV irradiation, some electrons and holes break free from the trap. Transferring part of the energy to Cr3+ and then emitting long-lasting light. It can be seen that the relationship between photocatalytic and long afterglow properties is mutually inhibited. As the calcination temperature increases, the luminescence intensity increases and the photocatalytic efficiency decreases.27
![]() | ||
Fig. 7 Photocatalytic effect of ZnGa2O4:Cr3+-based aerogels at different calcination temperatures; the SEM images of the samples after (a) 500 °C, (b) 600 °C, (c) 700 °C and (d) 800 °C calcination. |
Before calcined | 500 °C | 600 °C | 700 °C | 800 °C | |
---|---|---|---|---|---|
Surface area (m2 g−1) | 420.3 | 84.3 | 61.6 | 48.9 | 30.7 |
Average pore size (nm) | 14.6 | 36.7 | 35.7 | 40.7 | 36.0 |
Footnote |
† Electronic supplementary information (ESI) available. See DOI: 10.1039/c9ra08303k |
This journal is © The Royal Society of Chemistry 2019 |