Tuning the Porosity of Supraparticles.

Supraparticles consisting of nano- or microparticles have potential applications as, for example, photonic crystals, drug carriers, or heterogeneous catalysts. To avoid the use of solvent or processing liquid, one can make supraparticles by evaporating droplets of aqueous suspensions from super-liquid-repellent surfaces. Herein, a method to adjust the porosity of supraparticles is described; a high porosity is desired, for example, in catalysis. To prepare highly porous TiO2 supraparticles, polymer nanoparticles are co-dispersed in the suspension. Supraparticles are formed through evaporation of aqueous suspension droplets on superamphiphobic surfaces followed by calcination of the sacrificial polymer particles. The increase of porosity of up to 92% resulted in enhanced photocatalytic activity while maintaining sufficient mechanical stability.

Supraparticles are agglomerates of primary nano- or microparticles with a typical size from a few 10 μm to several 100 μm. For simplicity, we call the all primary particles nanoparticles in the following. As agglomerates, supraparticles assemble nanoparticles into larger entities, making handling and recovery easier, while reducing the hazards associated with the high mobility of the primary nanoparticles.[1] As an entity, such a superstructure can combine functionalities of the nanoparticles, e.g., high specific surface area, intrinsic material property, catalytic activity. Moreover, supraparticles may exhibit improved functions due to the synergism, coupling, and colocalization, which exceed the performance of simple sum function of primary building blocks.[2] Therefore, supraparticles have attracted considerable attention and shown specific structure and potential applications,[3,4] such as absorber materials in chromatography, for heterogeneous catalysis,[5] for making photonic crystals,[6] drug carriers,[7] or energy production and storage materials.[8,9]

A variety of fabrication methods has been developed. Most of the supraparticles are prepared in solution,[10]e.g., by kinetics/thermodynamics-controlled growth or template-based synthesis. For kinetics/thermodynamics-controlled growth methods, the self-assembly of nanoparticles is triggered by weak interactions such as hydrogen bonding, solvophobic interactions, and dipole–dipole interactions.[11−16] Instead, in template-based synthesis the assembly is controlled by using a template such as emulsions, mini-emulsions, block copolymer structures, or droplets prepared through microfluidics.[17−20] While being suitable for large-scale production, these approaches depend on chemicals, especially for size and composition engineering, which need to be separated from the supraparticles and disposed of afterward. These chemicals may harm the environment and their use consumes energy. Therefore, developing simple strategies to reduce or completely avoid the use of solvent, emulsifiers, templates, or any other processing liquid is desirable.

Recently, evaporation-induced self-assembly has been introduced as a promising strategy for the fabrication of supraparticles. Supraparticles are prepared by evaporation of sessile dispersion droplets on superhydrophobic surfaces.[21,22] On simple hydrophobic surfaces, a deposited dispersion droplet will have the shape of a spherical cap. The contact line will be mostly pinned during evaporation. Pinning leads to contact angles below 90° and to a higher evaporation rate of water near the contact line. As a result, liquid flows from the center of the droplet toward the contact line. This flow pattern inside the droplet leads to the formation of a ring- or doughnut-like structure of the final deposit.[23−25] On superhydrophobic surfaces, however, the apparent contact angle of water droplets is above 150°, leading to an almost spherical droplet shape with small contact area between the droplet and substrate. As a consequence, the evaporation of water is isotropic, ensuring that the droplet will maintain a spherical morphology during the evaporation process, since water molecules can also evaporate into the porous structure of the superhydrophobic substrate. This symmetric evaporation leads to an almost spherical shape of the supraparticle. In addition, it avoids temperature-induced Marangoni flow in the evaporating droplet.[26] As the evaporation process could be easily controlled, Velev etal. were able to produce opalescent supraparticles by forming colloidal crystals inside.[21,27] Colloidal crystals are formed when nanoparticles repel each other even at a very high nanoparticle density in the later stage of drying. In contrast, irregular porous packings are favored when particles are not as stably dispersed and attract each other at some stage.[22,28−33]

A limitation of superhydrophobic surfaces is the restriction to use aqueous electrolyte solutions. Nonpolar liquids or surfactant solutions cannot remain in the Cassie state and impale into the structures. Furthermore, the supraparticles are sometimes not easy to release from the substrate.

Superamphiphobic surfaces overcome these limitations for supraparticle fabrication, since they repel not only water but also nonpolar liquids, surfactant, or protein solutions. Droplets on such surfaces have high contact angle (CA > 150°) and roll off easily (tilting angle <10°), while the interfacial area between liquid and solid is extremely small (≪V2/3).[34−36] In addition, the highly porous superamphiphobic surface leads to an almost radially symmetric evaporation, like in levitated droplets. Furthermore, the release of dried supraparticles from the substrate is facilitated because their adhesion to superamphiphobic surfaces is usually lower than to superhydrophobic surfaces.[36]

Preparation of supraparticles on superamphiphobic surfaces not only avoids the expensive purification from a continuous aqueous phase and the migration and aging effects resulting from slow phase separation between particles and stabilizers, but also facilitates producing supraparticles with various sizes, compositions, and architectures by simple alternations of particle concentrations without consuming additional chemicals and energy. Porosity is a critical parameter for supraparticles, which has a great influence on the performance in practical applications, such as heterogeneous catalysis, absorber materials, and drug carriers.[5−7] For many applications, one needs highly porous supraparticles to facilitate diffusion of analytes or reactants. Porosity can be increased by allowing the dispersed particles to aggregate partially. If the nanoparticles attract each other in the later stage of the evaporation, they tend to form a more porous structure rather than forming a dense packing. Porosity achieved in this way is, however, limited: during the last stage of evaporation, strong compressive capillary forces act on the nanoparticle aggregates, leading to densification of loose agglomerates.

Herein, we propose a method to increase the porosity of supraparticles and circumvent the limit set by capillary compression. We prepared TiO2 supraparticles with hierarchical porosity by first constructing TiO2–polystyrene (PS) binary supraparticles on superamphiphobic surfaces and then removing the PS phase by calcination. By regulating the concentration and droplet volume of the mixed particle dispersions, the size of the spherical TiO2 supraparticles could be controlled. The porosity of superparticles is related to the volumetric ratio of TiO2 to PS. We demonstrate that the hierarchical porous structures of the TiO2 supraparticles enhance photocatalytic performance in degrading rhodamine B (RhB). Our approach for regulating the inner structure of supraparticles will allow optimizing them for specific applications.

Results and Discussion

Fabrication of Porous Supraparticles

Highly porous supraparticles were fabricated by first depositing a droplet of a binary nanoparticle suspension on a superamphiphobic surface (Figure a). While water evaporates and the volume of the droplet decreases, the confinement leads to concentration of nanoparticles inside the droplet. The droplets we use were nearly spherical at the beginning because their radius r ≈ 770 μm was lower than the capillary constant of κ = 2.7 mm. During the evaporation, the scaled radius r/κ decreases further, leading to an even more precise spherical shape. A solid binary supraparticle with spherical shape is formed. Then a calcination process was applied to remove the polymer components, forming supraparticles with highly porous structures. The evaporation was conducted on nanofilament-based superamphiphobic surfaces, which were prepared by hydrolysis of silane (Figure b).[37,38] The obtained superamphiphobic surface exhibits good liquid repellent properties with roll-off angles for water and hexadecane droplets (V = 5 μL) of 4° and 8°, leading to a highly spherical-shaped droplet (Figure c,d). Such liquid repellency ensures the formation of nearly spherical droplets of nanoparticle suspension.

Figure 1

Surface-mediated fabrication of highly porous supraparticles. (a) Schematic illustration of porous supraparticle formation mediated by droplet evaporation and postcalcination. (b) SEM image of the nanofilaments forming the superamphiphobic substrate. (c, d) Side view images of 5 μL water and hexadecane droplets on the surface.

The change in droplet shape during the evaporation process was tracked with a side view camera (IDS uEye USB camera). After depositing 2 μL of TiO2–PS binary mixture (0.1 vol % of nanoparticles, volume ratio of TiO2 to PS is 1:5) onto the superamphiphobic surface, it takes about 24 min to evaporate the water (22 °C at 40% relative humidity, Figure a). The suspension evaporated at a constant contact angle without contact line pinning until the end of the process. The droplet as well as the finally obtained supraparticle had a sphere-like shape, in agreement with what has been observed before.[36,39] Picknett and Bexon calculated the evaporation rate of water droplets in still air, while assuming that diffusion of water molecules in air is rate-limiting.[40] They showed that the volume V2/3 of a sessile droplet evaporating at a constant contact angle decreases linearly with time asHere, V0 is the initial volume of the droplet and α is the evaporation speed. In our experiment, a linear decrease of V2/3 was observed for both nanoparticle suspension and pure water droplets (Figure S1). The evaporation speed in the presence of nanoparticles in the droplet was similar (α = 972 ± 10 μm2/s) to that of a pure water droplet (α = 905 ± 8 μm2/s) evaporating under the same conditions. This similar evaporation speed indicates that no significant accumulating of nanoparticles at the interface occurs.

Figure 2

Supraparticles obtained after evaporation (22 °C at 40% relative humidity, the volume ratio of TiO2 to PS is 1:5) and calcination (500 °C). (a) Evaporation of a binary colloidal dispersion droplet on a superamphiphobic surface. SEM images of the surface (b) and the inner part (c) of TiO2–PS binary supraparticles obtained after evaporation. Inset in (b) shows the whole binary supraparticle. (d, e) SEM images of the surface (d) and the inner part (e) of highly porous TiO2 supraparticles achieved after calcination. Inset in (d) shows the whole porous supraparticle.

SEM images (Figure b inset) confirm the spherical morphology of the obtained supraparticles. Small TiO2 and large PS nanoparticles are randomly distributed on the surface (Figures b and S2a). This is due to the size and shape polydispersity of the TiO2 nanoparticles, which prevent the formation of a crystalline-like structure. To further characterize the distribution of building blocks in the microsphere, we cut the binary supraparticles in half (with a WEDO leather knife) and imaged the internal structure with SEM. Both colloids are homogeneously distributed inside the supraparticle without a large degree of segregation (Figures c and S2b).

After removing the PS phase by calcination, a highly porous superstructure was formed (Figure d,e). The retained TiO2 supraparticles maintained the spherical morphology and their size even after removing about 83% (vol %) solid of the binary supraparticles (Figure d inset). Randomly distributed macropores are formed on the surface of the supraparticle after removing PS (Figures d and S2c). By cutting the obtained TiO2 supraparticles in half the homogeneously distributed macropores left by the PS particles are visible (Figures e and S2d). The macropores inside supraparticles are mostly interconnected to each other especially for the case of higher PS content (Figure S3). This interconnectivity is essential for applications to allow reactants to diffuse into and out of the supraparticles.

Control of the Structure of Porous Supraparticles

The final size of supraparticles can be precisely controlled by the initial droplet volume and the concentration of the components in suspension. First, we evaporated 2 μL of droplets with different volume contents of nanoparticles (0.1%, 0.2%, 0.3%, 0.4%, 0.5%, and 1%). Second, we prepared supraparticles using the same volume ratio (0.1%) but with different droplet volumes (0.3, 0.5, 1, 2, 5, 10, 40, and 100 μL). The diameter of supraparticles prepared ranged from 70 to 900 μm (Figures S4 and S5). Even larger particles can in principle be prepared. However, when the diameter of the droplet approaches the capillary length (γ/gρ)1/2, the droplets are deformed to an oblate shape by gravity (Figure S6). Here, γ and ρ are the surface tension and density of the suspension and g = 9.81 m/s2 is the standard acceleration of free fall.

The porosity of supraparticles can be adjusted in two ways: macro-pore size and volume ratio of the inorganic phase. The macro-pore size is adjustable by controlling the diameter of PS nanoparticles. As shown in Figure S7, interconnected pores could be achieved by reducing the diameter of PS particles from 1.25 μm to 572 nm (Figure S7a–c) and 270 nm (Figure S7d–f) and keeping the volume ratio of TiO2 to PS at 1:5. Macropores are still formed on the surface and the inner part. The pore size agreed with the PS nanoparticle size used in each case.

We also modulated the porosity of porous supraparticles by regulating the volume ratio of TiO2 to PS in nanoparticle suspension. The volume ratio (R) was set to 1:1, 1:3, 1:5, 1:7, and 1:9. By SEM (Figure ) we observed that the number and density of macropores correlate with R. Likewise, the density of pores inside the porous supraparticles also increased. The interlayer of TiO2 between macropores becomes thinner and thinner with increasing R. Without PS particles, mesopores are formed by the interstitial space between the TiO2 nanoparticles. Since TiO2 nanoparticles tend to attract each other at short distance, they do not form a crystalline close packing but a more porous packing. When adding PS particles, macropores are formed. Interconnection of macropores will occur if neighboring PS particles contact with each other before the calcination process. Such contacts will become more likely when the R of TiO2 to PS in the nanoparticle suspension decreases. Table S1 shows the volume fraction of PS particles in the final supraparticles as derived from supraparticle size and added amount of PS templates. With R decreasing, PS particles in the binary supraparticles reach but do not exceed a volume fraction of 49.4%. This volume fraction corresponds to the minimum density of a jammed packing, indicating that PS particles form such a jammed configuration during the drying process. In such a minimal jammed packing configuration, each particle should on average contact seven immediate neighbors, resulting in a corresponding number of interconnections between macropores in the final porous supraparticles.[41,42] The lowest volume ratio of TiO2 to PS we could reach was 1:9. This means even after removing 90% of the solid phase in the binary supraparticles, the remaining TiO2 still preserved the spherical morphology of the supraparticles. The porosity of the final porous supraparticles obtained in each case was calculated based on the initial TiO2 volume in the droplet and the size of the supraparticle. Pure TiO2 (R = 1:0) supraparticles have a porosity of 66%. With increasing of the PS volume ratio, the porosity gradually increased to 74.8%, 83.4%, 89.5%, 91.6%, and 92.1%, respectively (Figure S8). The porosity of the supraparticles would be hard to measure directly, since typical experimental methods such as gas sorption/desorption would fail for the combination of micro- and macropores. However, since only the inorganic phase remains after the calcination process, the porosity of supraparticles can simply be calculated based on the TiO2 volume in the original droplet and the diameter of the final TiO2 supraparticles. These results demonstrate that the structural parameters of the porous supraparticles, such as size, macropore size, and porosity, can be easily determined by defining the evaporation conditions. Therefore, preparation of highly porous supraparticles can be carried out in a finely controllable manner.

Figure 3

SEM images for the surface of binary supraparticles (1), the porous surface (2) and inner structure (3) after calcination of supraparticles. The volume ratios of TiO2 to PS equal 1:1 (a1, a2, a3), 1:3 (b1, b2, b3), 1:5 (c1, c2, c3), 1:7 (d1, d2, d3), and 1:9 (e1, e2, e3), respectively; the diameter of PS particles was about 1.25 μm.

Binary superlattice thin films could be seen as an alternative approach to create highly porous materials with a comparable internal microstructure. By using larger PS particles for the formation of the lattice structure and filling of the voids with TiO2 nanoparticles, one could create inverse opals of TiO2 after calcination.[43,44] In this case, the achievable porosity would even be higher due to the closer packing of the PS spheres. Tuning of the porosity in this case would be possible via variation of the size ratios of PS and TiO2 particles. Therefore, one would expect that the catalytic activity of both systems should in principle be similar. The main advantages of the supraparticles are (1) the simple way of fabrication (just placing a droplet and letting it evaporate), (2) tuning of porosity is more simple (no need for different PS particle sizes but just varying concentration), and (3) the final product comes without supporting substrate. This offers more flexibility in handling and application scenarios. The supraparticles in dispersion are highly mobile and can be easily transferred, concentrated, or diluted as required. The size of the spherical supraparticles can range from a few tens of micrometers to a few millimeters. Therefore, they can readily be adopted in existing application systems (such as drug carriers and catalysts in reaction vessels).

Mechanical Properties

To evaluate the potential benefit of the highly porous supraparticles for practical applications, the mechanical stability and photocatalytic activity were further investigated. The fracture force of single supraparticles with different porosity was measured with a home-built force-sensing system, which allowed particle compression between two parallel glass plates equipped with a force sensor and a stepper motor.[45] For the pure mesoporous TiO2 supraparticles without macropores, the fracture force for a single particle was ∼175 mN (Figure S8). With the introduction of macropores, the mechanical stability was significantly reduced. With increasing porosity, the fracture force further decreased. For supraparticles with a porosity higher than 85%, the fracture force decreased to about 4–5 mN. Even though these highly porous particles are more fragile, even for the supraparticles with the largest porosity (92%), the fracture force is still about 600 000 times larger than the gravitational force (Figure S9). This means that a densely packed bed of such particles could reach a height of 76 m before the lowermost particles would start to break. Therefore, even the supraparticles with the largest porosity prepared by our method are stable enough for practical use.

Photocatalytic Efficiency

TiO2 is commonly used as photocatalyst for degradation of organic dyes, splitting of water, decontamination, photosynthesis, etc.[46−49] Improvement in its photocatalytic activity without using chemical modification is of great importance. The photodegradation performance of the TiO2 supraparticles with different porosities was investigated to evaluate the effect of macropores. Rhodamine B, a typical organic dye, was chosen as a model compound for photocatalytic degradation. The process was conducted by irradiation with UV-A light (power: 0.3 ± 0.01 mW/cm2). As shown in Figure a, after 22 h of irradiation, the organic dye in solution containing the largest porosity TiO2 supraparticles is nearly completely degraded (∼97%, 72% of the degradation was contributed by TiO2 supraparticles). The photocatalytic activity of the porous supraparticles increased with increasing porosity (Figure b,c). The photocatalytic activity of supraparticles with the largest porosity reached about 2.7 times of that of mesoporous supraparticles without macropores. We attribute the enhancement of photocatalytic activity to the existence of macropores, making it much easier for the organic dye to diffuse into supraparticles, increasing the effectively available surface area for photocatalytic reaction. For catalytic reactions, which do not depend on light, the effect is probably even more pronounced. For photocatalysis, the inner part of the supraparticles is not effective because light is absorbed in the outer shell. These results show that the introduction of macropores can improve the catalytic property of the supraparticles. Our method is therefore a promising approach for the production of highly porous supraparticles with enhanced properties in an environmentally friendly manner.

Figure 4

Porosity-dependent photocatalytic efficiency enhancement and supraparticles prepared from different materials. (a) Optical image of rhodamine B (RhB)/supraparticle solutions after exposure to UV-A for 22 h. (b) Relationship between degradation of RhB and irridation time for supraparticles with different porosity. (c) Relationship between photocatalytic efficiency and porosity. (d, e) SEM images of binary TiO2–Au and ZnO–Au porous supraparticles made from TiO2/Au/PS (40:1:200) and ZnO/Au/PS (40:1:200) ternary suspensions. (F) SEM image of a ternary TiO2–ZnO–Au porous supraparticle fabricated from a TiO2/ZnO/Au/PS (20:20:1:200) quaternary suspension. Insets are optical images of the hybrid supraparticles.

As the approach presented here is mainly controlled by the evaporation of droplets on superamphiphobic surfaces, our method can easily be adopted to fabricate highly porous supraparticles from other materials in an environmental friendly manner. Figure d–f shows the highly porous binary and ternary suprapaticles (TiO2–Au, ZnO–Au, TiO2–ZnO-Au) fabricated by mixing two functional materials or adding noble metal nanoparticles in the droplet. Again we maintain spherical morphology and evenly distributed macropores spanning a network from the surface to the inner core. Moreover, other supraparticles, e.g., ZnO, SiO2, and TiO2–ZnO, can also be obtained by using the same method (Figure S10). These results confirmed the possibility of our approach for integrating multiple functions into a single supraparticle for optimized applications.

Conclusions

In conclusion, we fabricate highly porous surpraparticles based on evaporation of droplets of suspensions on superamphiphobic surfaces. Taking advantage of the liquid repellency of the superamphiphobic surface, we suppress contact line pinning during the evaporation, leading to the formation of spherical multicomponent supraparticles that can be easily released from the surface. To increase the porosity of the supraparticles, we add sacrificial polymer nanoparticles. After formation of supraparticles these polymer nanoparticles are burned away to create interconnected pores. The structures of the obtained porous supraparticles (particle size, pore size, porosity, and component distribution) are finely adjustable by regulating droplet volume, dispersion concentration, choice of primary particles, and sacrificial particles. The flexibility of our approach has the potential to expand applications of supraparticles in research areas such as absorber materials in chromatography, heterogeneous catalysts, and drug carriers.

Experimental Methods

Materials

Methyltrichlorosilane (TCMS, 99%), TiO2 nanoparticles (P25, mixture of anatase and rutile), and hexadecane (reagentPlus, 99%) were purchased from Aldrich. 1H,1H,2H,2H-Perfluorodecyltrichlorosilane (PFDTS, 96%) was purchased from Alfa Aesar; n-hexane (95%) from Fisher Chemical. Toluene, acetone, and ethanol absolute were provided by VWR Chemicals. Ultrapure water with a resistivity of 18.2 MΩ·cm was produced using a Sartorius Arium 611 VF water purification system. Glass slides of 26 × 76 mm2 in size were provided by Menzel-Gläser, Germany. Polystyrene particles (negative charged, with a −COOH group on the surface) with diameters of 270 nm, 572 nm, and 1.25 μm were prepared using surfactant-free emulsion polymerization[50] and purified by several cycles of centrifugation and redispersion in ultrapure water.

Fabrication of a Silicone Nanofilaments Based Superamphiphobic Surface

The superamphiphobic surfaces were prepared by the grow-from method.[37,38] Glass slides were first cleaned with toluene, acetone, absolute ethanol under ultrasonication, and dried by nitrogen flow. Then the substrates were treated with an oxygen plasma (Diener Electronic Femto, 30 W for 2 min). Five activated glass slides were immersed in 360 mL of toluene with 166 ppm water in a reaction chamber. Subsequently, 250 μL of TCMS was added to initiate the growth of silicone nanofilaments, and the chamber was sealed. After 12 h of reaction, the silicone nanofilament-grafted glass slides were rinsed with hexane and dried under a nitrogen flow. To achieve superamphiphobicity, the substrate is modified with 1H,1H,2H,2H-perfluorodecyltrichlorosilane. For the modification of PFDTS, the silicone nanofilaments were further activated with oxygen plasma (120 W for 2 min). Then the activated substrates were immersed in a mixture of 180 μL of PFDTS and 120 mL of hexane for 30 min. After the modification, the substrates were rinsed with hexane and dried under nitrogen flow. The obtained nanofilament-coated glass was homogeneous over a large area, and the micropores and overhangs formed by the silicone fibers endowed the surface with its nonwettability. Water droplets possess a static contact angle over 161° (Figure c) with a sliding angle of about 4°, while hexadecane droplets have a contact angle around 156° (Figure d) with a sliding angle about 8° at a volume of 5 μL.

Preparation and Modulation of Hierarchical Porous TiO2 Supraparticles

Hierarchical porous TiO2 supraparticles were prepared by calcination of TiO2/PS binary supraparticles that were fabricated on a superamphiphobic surface. First, 2 μL of binary mixture of TiO2 and PS particles with the concentration equal to 0.1% (vol) were dropped onto a silicone nanofilament-based superamphiphobic surface with the help of an Eppendorf Research Plus pipet (equipped with epT.I.P.S. LoRetention Reloads tips). Then water evaporated at 22 °C and relative humidity (RH) was equal to 40%. The binary TiO2/PS supraparticles formed after evaporation were released by slightly inclining and shaking. Supraparticles were collected on a weighing paper and then transferred into a bottle vial. The binary supraparticles are stable for collection and handling without attrition. However, when immersing them in water, they tend to disintegrate, since the particles are hydrophilic and there are no strong interactions between TiO2 and PS. In some cases, trace amounts of the nanofilaments were left behind at the supraparticle surface (Figure S11) since the nanofilaments may still have a few hydrophilic points that can pin the contact line. The binary TiO2/PS supraparticles were put into a muffle furnace and calcinated at 500 °C for 3 h to remove the PS and form pure TiO2 supraparticles with hierarchical porosity. The final TiO2 supraparticles showed improved stability and did not disintegrate when immersed in water. The final size of supraparticles could be adjusted by the volume content of nanoparticles (range 0.1–1%) and the initial volumes (0.3–100 μL). Meanwhile, the porosity and the size of macropores can also be regulated with the volume ratio of TiO2 to PS and the size of template PS. It is worth noting that the transformation temperature of anatase to rutile is around 500–800 °C. Choosing 500 °C for calcination did not cause any detectable crystal transformation, while complete removal of the organic component is ensured (Figure S12).

Photocatalytic Activity

To measure the photocatalytic activity of TiO2 supraparticles, 2 mg of TiO2 SPs with different porosities were placed into 8 mL vials containing a RhB solution (10 μg/mL, 5 mL) separately. The supraparticles formed a monolayer on the bottom and did not shield each other. Then the mixtures were radiated from the bottom side with a UV-A light (UV source: LQ-400, Dr. Gröbel UV-Elektronik GmbH) for a certain time at a power of 0.3 ± 0.01 mW/cm2. The photodegradation process was conducted without stirring. As a control group, 5 mL of RhB solution without TiO2 SPs and 5 mL of RhB solution with 2 mg of pure TiO2 SPs without macroporous were irradiated with the UV-A light under the same conditions.

Characterization

The morphology of the silicone nanofilaments and supraparticles was imaged by scanning electron microscopy (low voltage LEO 1530 Gemini, Germany). The samples were sputter-coated with a 5 nm layer of Pt using a BalTec MED 020 modular high-vacuum coating system prior to avoid charging. Static and sliding angles of 5 μL water and hexadecane droplets on the nanofilament-based superamphiphobic surface were measured with a goniometer, Dataphysics OCA35 (Data Physics Instruments GmbH, Germany). UV–vis adsorption spectra were taken from a PerkinElmer Lambda 25 UV–vis spectrometer with Suprasil QS 1 mm cuvettes. The water concentration in toluene was evaluated using a Karl Fischer coulometer (Mettler Toledo C20 Compact KF coulometer). Optical micrographs were taken by an optical microscope (Carl Zeiss Axiotech Vario 100HD). TEM images of TiO2 nanoparticles with and without calcination were taken by transmission electron microscopy (JEOL JEM-1400). Powder XRD measurement was performed on a Bruker D8 ADVANCE Twin X-ray diffractometer with Cu Kα radiation.