Yue Hua,
Salah Ahmed Sarhan Al-Shujaaa,
Bin Zhenc,
Yaping Zhang*ab,
Xianggao Li
a and
Yaqing Feng*a
aSchool of Chemical Engineering and Technology, Tianjin University, Tianjin 300072, China. E-mail: zhypin126@126.com; yqfeng@tju.edu.cn
bSchool of Materials and Environment, Beijing Institute of Technology, Zhuhai, Zhuhai 519085, China
cCollege of Chemistry and Chemical Engineering, Tianjin University of Technology, Tianjin 300384, China
First published on 10th June 2021
Electrophoretic display (EPD) is a type of flexible display which has attracted wide attention. In this work, blue nanosized crystals of cobalt aluminum oxide (CoAl2O4) were precipitated on silica nanoparticles, and then the nanocomposites were coated with an ionic liquid polymer (PIL) to give blue electrophoretic particles. The blue nanocomposites (SCAs) formed possess an excellent spherical structure, and the average diameter is about 188 nm. The porous silica matrix presents a relative light density, and the blue CoAl2O4 pigment offers excellent color. The outside ionic liquid polymer supplies the PIL/SCAs with a light density of 1.7915 g cm−3, excellent hydrophobicity and dispersion stability in the electrophoretic liquid. The fabricated single-particle EPD prototypes show a response time of 165 ms in the EPD cell with a 0.2 mm thickness, which is much faster than the commercial EPDs, and this is probably because of the unique composite structure.
Electrophoretic particles are the key component of the electrophoretic display, and their color and electrophoretic property have a remarkable affect on the display properties. At present, organic pigments are usually used to color the electrophoretic particles.3–5 Organic pigments provide almost all types of color series and have a suitable low density for electrophoretic systems. However, decomposition of organic pigments in organic electrophoretic liquid often leads to a short service lifetime of EPDs.
Inorganic pigments usually possess excellent optical, electrical and chemical properties and have a long service lifetime.6,7 However, the finite existing color series and large density limit their application in EPDs. The large density of the inorganic pigment makes it very easy to sediment out in the suspension fluid. Use of electrophoretic particles with a hollow structure have been proposed to decrease the density,8,9 but their poor mechanical strength cannot be neglected. An inorganic pigment coated with polymer is another option for reducing its apparent density, which in addition favors the improvement of the dispersion stability.10–12 At the moment, polymers are mostly coated onto the surface of particles through weak physical interaction, which leads to a swelling problem and affects their lifetime badly. Meanwhile, general polymer coatings always offer poor surface charge performance and show a low responding speed in electric fields.13
In this work, blue inorganic nanocrystals are precipitated on the surface of silica nanospheres to obtain blue inorganic pigments. Next, the inorganic pigments are modified by a silane coupling agent, which further reacts with the ionic liquid monomer to achieve electrophoretic particles coated with ionic liquid polymers. The porous silica nanoparticles have a relatively low density, excellent mechanical strength, and rich surface hydroxyl groups for reacting with the silane coupling agent. The ionic liquid polymer coating would offer light density, good dispersion stability and suitable electrophoretic property.
Another method was an in situ method using a sol–gel process and reverse microemulsion. Firstly, n-hexane (35.80 g), n-hexanol (19.62 g), Triton X-100 (30.00 g) and methylamine aqueous solution (20 wt%, 3 mL) were mixed together under vigorous stirring to give a reverse microemulsion solution. Then, an n-hexane solution of TEOS (10 wt%, 30 mL) was added dropwise. As the TEOS moved from the oil-phase into the water-core of the reverse micelles, the sol–gel process started. After reacting at 35 °C for 60 min, an aqueous solution containing 0.3291 g of Co(NO3)3·6H2O and 0.8483 g of Al(NO3)3·9H2O was added into the reaction system. The CoAl2O4 precursors formed and were deposited on the surface of the silica particles as the reaction proceeded. Lastly, the composite precursors were collected and calcined at 1000 °C for 120 min to give the blue CoAl2O4/SiO2 nanoparticles (SCAs-2).
The [VDoIm][Br] ionic liquid was synthesized by a previously reported method.14 The [VDoIm][Br] (0.64 mmol), 0.2 g of VSCAs and 0.32 mmol of divinylbenzene were added into deionized water, and the reaction was initiated with 0.16 mmol K2S2O8 at 70 °C. After reacting for 180 min, the nanoparticles were washed with acetone, and then dried to give blue PIL/SCAs nanoparticles.
The first idea was to coat the blue CoAl2O4 nanocrystals onto silica nanoparticles by post-coprecipitation. The silica nanoparticles were prepared previously, and then the Co2+ and Al3+ ions were coprecipitated onto the surface of the silica nanoparticles with the assistance of alkalis, such as ammonia and urea. As shown in Fig. 1(a), the prepared silica nanoparticles possess a monodisperse spherical structure. After the coprecipitation, SEM of the obtained SCAs was performed and the resulting images are shown in Fig. 1(b) and (c), and it can be seen that the silica nanoparticles have been corroded. Even at low concentrations, both ammonia and urea would damage the structure of the silica spheres.
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Fig. 1 The SEM images of silica nanoparticles (a), the SCAs-1 post-coprecipitated with ammonia (b) and urea (c), and the samples obtained by direct coupling of the silica sols with ions (d). |
In previous work, the formation of the silica nanoparticles in a reverse microemulsion has been studied in detail.14 The monodisperse silica sols and gels formed successively in the polar microreactors dispersed in a nonpolar solvent, with assistance of alkali. Coprecipitation of Al3+ ions and Co2+ ions on silica nanoparticles was also performed under alkaline conditions. Immediately, coupling of the sol–gel process of silica precursors with the coprecipitation of Al3+ ions and Co2+ ions was proposed. Therefore, Co2+ and Al3+ ions were directly added into the reaction system during the formation of silica sols. Unfortunately, it was found in that the products obtained were tiny particles with an average diameter of 20–50 nm (Fig. 1(d)), which was obviously much less than that of the silica nanoparticles. This occurred because the addition of electrolytes (Co2+ and Al3+ ions) destroyed the framework of the silica sols, and the silica nanospheres broke into tiny particles.15,16
In order to introduce the CoAl2O4 nanocrystals into the silica nanoparticles, the most effective time to add the Al3+ ions and the Co2+ ions into the system should be considered. To have the best chance of combining silica spheres with the pigment CoAl2O4, the detailed formation process of the matrix silica nanoparticles was studied. It was found that during the formation process, silica nanoparticles with a stable structure could form when the reaction in the micelles lasted for at least 60 min. If the metal ions were added into the reaction system after this time, then it was more likely that the reaction would work. Hence, a reverse microemulsion containing a Co2+ and Al3+ aqueous solution was added into the system after the initial reaction had progressed for 75 min. After the addition of the reverse microemulsion containing Co2+ and Al3+ ions, the reaction system was sampled as the reaction time proceeded. After washing and calcination, the blue particles were collected. The SEM images of the samples are shown in Fig. 2. It can be observed that when the coprecipitation goes on for 30 min, the particles formed possess a spherical structure, and the average diameter is about 188 nm (the inset shown in Fig. 2(a)). As the reaction time continues, the average diameter of the particles showed no obvious change, whereas a sintering problem happened between the particles. This was probably because the further hydrolysis of the silica sols and ions caused the formation of the bonds between the particles.
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Fig. 2 The SEM images of the samples during the formation of SCAs-2. (a) 30 min, (b) 45 min, (c) 60 min, and (d) 90 min. The inset in (a) is statistical particle size distribution of the SCAs-2. |
The FTIR spectra and XRD patterns of the inorganic composite precursors and SCAs-2 are shown in Fig. 3. As shown in Fig. 3(A), after calcination, the characteristic peaks, such as 2983 cm−1 and 2935 cm−1, 1520 cm−1, 1468 cm−1, 1388 cm−1, disappear, and the characteristic peaks of free water and hydroxyl at 3550–3300 cm−1 and 1635 cm−1, respectively, decrease remarkably. At the same time, the amorphous inorganic composite became crystalline. The XRD pattern of the SCAs-2 is shown in Fig. 3(B). The diffraction peaks at 36.52°, 31.02°, 44.62°, 59.22°, and 65.10° were assigned to the lattice planes of 311, 220, 400, 511 and 440, respectively. This illustrated the formation of the spinel CoAl2O4 phase.
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Fig. 3 (A) The FTIR spectra of the composite precursors (a), and SCAs-2 (b). (B) The XRD patterns of the composite precursors (a), and SCAs-2 (b), and the inset is a photograph of the SCAs-2. |
The element analysis was carried out using XPS, and aluminum, cobalt, oxygen and silicon, elements were all found, as shown in Fig. 4. The silicon element came from silica, and the cobalt and aluminum have valences of +2 and +3, respectively. This proves that silica and aluminum cobalt oxide were formed. In addition, the atomic percent of silicon (2p), aluminum (2p) and cobalt (2p) were 21.5%, 1.4% and 1.0%, respectively. This proves that the mass ratio of CoAl2O4 to silica was equal to 11%, which was close to the set value.
The TEM images of the SCAs-2 are shown in Fig. 5. This also proved that the SCAs-2 had a spherical shape. In the magnified image (inset of Fig. 5), it was also seen that tiny spinel CoAl2O4 particles gathered on the surface of the SCAs-2, giving them a bright blue color. The density of the samples was determined using the density bottle method. For the CoAl2O4 particles prepared under the same reaction conditions, its density was 6.2354 g cm−3. Compared with CoAl2O4, the density of SCAs-2 was reduced dramatically to 2.3414 g cm−3. This proved that the existence of the silica matrix dramatically decreased the density of the SCAs-2.
As the preparation process has shown, as the surface modification proceeds, some of the hydroxyl groups on the surface of the SCAs-2 reacted with triethoxyvinylsilane, and the following anchored vinyl groups polymerized with the vinyl groups of the ionic liquids, until the PIL/SCAs were generated. When compared with the FTIR spectrum of the SCAs-2 (Fig. 3(A)), the FTIR spectrum of the modified SCAs-2 shown in Fig. 6(A) shows some characteristic peaks of [VDoIm][Br]. The peaks at 1630 cm−1, 1606 cm−1, and 1448 cm−1, 1412 cm−1 were assigned to the stretching vibration of imidazole ring and benzene ring, respectively, and 3065 cm−1 and 3024 cm−1 were assigned to the unsaturated C–H bond. The peaks at 2925 cm−1 and 2854 cm−1 were assigned to the saturated C–H bond, and 2959 cm−1 was assigned to the methylene group.
After surface modification, the density of the prepared VCSAS and PIL/SCAs was reduced further to 1.9668 g cm−3 and 1.7915 g cm−3, respectively. This was because of the introduction of organic components. The dispersion stability of the electrophoretic particles in dispersant largely depended on the density of the electrophoretic particles.17,18 According to the density value of the PIL/SCAs, its deviation from the solvent density was smaller than 0.5 g cm−3, which means that the density of the prepared nanoparticles is close to that of the solvent and is therefore suitable for use as an electrophoretic liquid. In addition, the surface modification showed an evident influence on the surface property of the SCAs-2. As shown in Table 1, the wetting angle value of the PIL/SCAs was much bigger than that of the SCAs-2, which indicated that the VSCAs showed a lower hydrophilicity. For the SCAs-2, the plentiful hydroxyl groups on the surface helped them to easily disperse in water because of the formation of hydrogen bonds. By comparison, after surface modification, some of hydroxyl groups were consumed, and the ionic liquid polymers were introduced. The long alkyl groups of the ionic liquid polymers covered the surface of the particles. All these factors result in the much higher hydrophobicity of the PIL/SCAs. Furthermore, the long alkyl groups of the ionic liquids could also help to mitigate the agglomeration of PIL/SCAs dispersed in the hydrophobic electrophoretic liquid.
The morphology of the prepared VSCAs and PIL/SCAs were also observed using SEM, and the images obtained, showing the spherical structure of the particles, are displayed in Fig. 7. The TEM images (Fig. 8) proved the spherical structure and the existence of the organic ionic liquid polymer which coats the particle surface, and the thickness of the ionic liquid polymer on the surface of PIL/SCAs was about several nanometers. In addition, the XRD patterns of the VSCAS and PIL/SCAs showed that the surface modification of SCAs would not affect the crystal structure of the CoAl2O4, as shown in Fig. 6(B). It was also found that the blue color of the SCAs did not change during the surface modification.
In order to explore the structure of the PIL/SCAs, the N2 physisorption isotherms of the samples were then carried out. The N2 adsorption–desorption isotherms of the samples (Fig. 9(A)) were type III hysteresis curves with a wide pore size distribution (Fig. 9(B)). The lack of isotherm plateauing from P/P0 = 0.95 to 1.0 in the samples was because there was a combination of large mesopores, macropores (pores > 50 nm), and interparticle voids.19 The pore volume and specific surface area of the silica nanoparticles prepared in a closed system reported previously were 0.415 cm3 g−1 and 22.745 m2 g−1, respectively, whereas the calculated pore volume and specific surface area of the SCAs-2 were 0.321 cm3 and 22.373 m2 g−1. Compared with the silica nanoparticles prepared in the similar system reported previously,14 the SCAs-2 had a similar pore structure and negligible reduction of pore volume and specific surface area. It was concluded that the introduction of CoAl2O4 did not affect the mesoporous structure of the silica matrix. After surface modification, the N2 adsorption–desorption isotherms of the samples did not obviously change, whereas the pore volume and specific surface area of VSCAs and PIL/SCAs shrank gradually. This was because the modified layers occupied part of the pore wall and the surface of the silica matrix. This had the effect that the silica matrix and the surface modification greatly reduced the density of the SCAs-2, and made the particles suitable for use in electrophoretic fluids.
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Fig. 9 The N2 adsorption–desorption isotherms (A), and the pore size distribution curves (B) of the silica nanoparticles. |
Sample | Y | x | y | Zeta potential/mV | Mobility/cm2 V−1 s−1 | Response time/ms |
---|---|---|---|---|---|---|
a The display properties of the EPDs were evaluated under an electric field of 20 V μm−1. | ||||||
SCAs-2 | 46.41 | 0.2142 | 0.1831 | 0.32 | 4.98 × 10−8 | — |
VSCAs | 46.36 | 0.2234 | 0.1947 | — | — | — |
PIL/SCAs | 45.77 | 0.2251 | 0.1977 | 4.13 | 6.17 × 10−7 | 165 |
In this research, the prepared PIL/SCAs were employed as blue particles to fabricate a single particle prototype EPD. In the fabricated prototype EPD, it was obvious to see that the blue electrophoretic particles swam in the cell and showed blue images. The surface zeta potentials and mobility values of the SCAs-2 and PIL/SCAs in the electrophoretic liquids were determined and are shown in Table 2. Compared with SCAs, the surface zeta and mobility value of PIL/SCAs were obviously improved, and these probably benefited from the ionic liquid polymer on the surface. In the fabricated prototypes with a thickness of 0.2 mm, the response time of the PIL/SCAs is 167 ms. For the modified titania particles reported previously20,21 and commercial EPDs with a close response distance, the response times were all greater than 260 ms, which was much longer than that of the PIL/SCAs. It was probably that the low density and ionic liquid polymer coating of the PIL/SCAs which endowed them the excellent property. The low density decreased their gravitational sedimentation and favored their mobility. The ionic liquid polymer coating not only favored the hydrophobicity and dispersity stability, but also helped to enrich the trace polar impurities around the particles, such as water.22,23 The polar impurities favored the ionization effect and aided the mobility. With the assistance of electric field, the response time of the prototype EPDs were tested and the results are shown in Table 2. As demonstrated in Table 2, the response property of the applied electric field of the prepared PIL/SCAs was faster than that of the commercial EPDs and the SCAs-2, and this was probably because of the special ionic liquid chains on the surface.14
At the same time, TiO2 nanoparticles were used as the opposite white particles and a blue-white dual-particle prototype EPD was fabricated. A clear white image and a blue image could be displayed, but the response time became longer and the quality of the blue image became lighter. This was probably due to the more complicated interactions between the particles and the hiding power of PIL/SCAs.
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