An Electrochemical System for Forming Periodic Precipitation Bands of Cu-Fe-Based Prussian Blue Analogues

We propose a novel electrochemical system to form precipitation patterns of Cu-Fe-based Prussian blue analogues (Cu-Fe PBA) in agarose gels, using an applied voltage to produce reactant ions. The spatiotemporal evolution, spatial distribution, and crystallite morphologies of the precipitates were investigated by visual inspection, Fe Kα intensity distribution measurements, and optical and scanning electron microscope observations. The precipitation patterns and their evolution depended on the applied voltage. Multicolored periodic precipitation bands were stochastically formed under cyclic alternating voltage (4 V for 1 h and then 1 V for 4 h per cycle). The distances between adjacent bands were randomly distributed (0.30 ± 0.25 mm). The sizes and shapes of the crystallites generated in the gel were position-dependent. Almost cubic but fairly irregular crystallites (0.1–0.8 μm) were formed in the periodic bands, whereas definitely cube-shaped crystallites (1–3 μm) appeared close to the anode. These cube-like reddish-brown crystallites were assigned to Cu-FeII PBA. In some periodic bands, plate-like blue crystallites (assigned to Cu(OH)2) were also present. Future issues for applications of the observed periodic banding were discussed.


Introduction
Liesegang bands (periodic precipitation bands of slightly soluble inorganic compounds in gels) are formed spontaneously when a precipitation reaction is coupled to the mass transport of reagents in a sample tube filled with hydrogels [1][2][3]. A typical setup for observing Liesegang bands is illustrated in Figure 1a. In this setup, two electrolytes are loaded in separate columns in a single sample tube. The longer gel column is placed at the bottom, where a continuous precipitation zone (sometimes called the "turbulent zone" [4]) and Liesegang bands form. The shorter column on top (in the form of a gel or aqueous solution) has a higher electrolyte concentration. These electrolytes are denoted as the "inner" and "outer" electrolytes, respectively.
Since its discovery in 1896 [1], Liesegang banding has been continuously investigated. Today, it still attracts considerable interest as a self-organization phenomenon [5], having the potential for the spontaneously creation of complex materials and functional devices [4,6,7]. However, only limited systems have been reported for forming Liesegang bands [2]. To develop the applications of periodic banding in material science and engineering, it is important to widely explore systems in which Liesegang-band-like precipitation patterns could form.
From a technological point of view, it is important to control the spacing between the adjacent Liesegang bands. A powerful approach to change precipitation patterns is the use of an electric field [2,3]. In fact, the spacing of Liesegang bands has been reported to show a significant dependence on the direction and strength of direct current fields [2,[8][9][10][11] and alternating current fields passing through the system [2,12]. A schematic  [1,4,5], (b) previously reported setup to examine the effects of electric field on Liesegang bands [8,10,11], and (c) currently proposed setup to observe precipitation patterns formed by electrochemical processes. The arrows in (a) and (b) indicate the direction of movement of reactant ions supplied from the outer electrolyte column. Note that the ion movement in (c) is different, reflecting changes in the supply of reactant ions.
In this study, we propose a new electrochemical system for producing periodic precipitation patterns with interesting features. Although the proposed setup ( Figure 1c) appears similar to that in Figure 1b, the processes occurring within these systems are quite different. Instead of diffusion from the outer electrolyte column, the reactant ions (Cu 2+ and [Fe(CN)6] 4-) are produced at the electrodes through electrochemical reactions. Specifically, in a tube containing agarose gel, Cu 2+ and [Fe(CN)6] 4-ions are generated at the anode and cathode, respectively, when the applied voltage exceeds the sum of the overpotential of the electrodes (typically around 0.5 V in aqueous solutions at 25 °C [13]) and the potentials of the electrode reactions (Cu 2+ + 2e -= Cu + 0. cates Fe(CN)6 vacancies, i.e., defects arising from missing Fe(CN)6 moieties (x = 2, y = z = 1, and n = 0 for Cu-Fe II PBA with no Fe(CN)6 vacancies, whereas x = 1, y = z = 1, and n = 0 for Cu-Fe III PBA with no Fe(CN)6 vacancies). Crucially, the concentrations of the reactant ions can be controlled in situ by varying the voltage of the electrodes.
The proposed setup could expand the applications of precipitation patterning in material science and engineering because the electrodes are used as the ion sources, so various changes can be made to the reactant ion concentrations during the experiment to yield different precipitation patterns. For instance, pulsatile concentration changes are easily achievable by tuning the voltage of the power supply. Such tuning is capable of generating diverse precipitation patterns. Moreover, because the electrodes are generally made of metals, their microfabrication is relatively easy. This workability could expand the use of periodic banding for micro-and nanotechnology, which was opened up by Grzybowski's group using a wet stamping technique (WETS) [4,6,7].
It should be noted that Cu-Fe PBA have attracted significant attention as interesting functional materials for electrodes [15,16], hydrogen storage [17], and CO2 adsorption [18]. Generally, the properties of Prussian blue analogues (PBA) are strongly influenced by the Fe(CN)6 vacancies, which are correlated with the crystal structure, crystallite morphology, and preparation processes [19][20][21][22]. Interestingly, the sizes and shapes of Mn-Fe-based PBA (Mn-Fe PBA) crystallites in Liesegang bands have been reported to depend on the band position [23]. Therefore, if Liesegang band-like periodic patterns of Cu-Fe PBA form in the proposed setup, they have the potential to be used for producing Cu-Fe PBA crystallites varying in size and shape (i.e., having different functional properties) simultaneously, and, subsequently, the periodic bands of interest could be cut out and examined/applied specifically. This possibility is interesting for applications in material science and engineering.
Considering the abovementioned novelty and potential applicability, herein, we report the patterning of precipitates formed using the setup shown in Figure 1c, as well as their crystallite morphologies.

Reagents
Analytical reagent grade K3[Fe(CN)6], K4[Fe(CN)6]•3H2O, and CuCl2•2H2O were obtained from Wako Pure Chemical Industries (Osaka, Japan). Agarose for electrophoresis (gel strength: 1800-2300 g/cm 3 ) was purchased from Kanto Chemical (Tokyo, Japan). All chemicals were used without further purification. All aqueous solutions were prepared using deionized water that had been purified from tap water using a cartridge water purifier (G-10, Organo, Tokyo, Japan). Note that the density of the employed agarose sol was very high in order to suppress gel shrinkage on the application of a voltage. Using a Pasteur pipette, the prepared sol was transferred to plastic straws (4 mm diameter and 50 mm long), whose bottoms had been plugged by Cu rods, which were used as the cathodes (HIKARI, CM395-4; 4 mm diameter and ~20 mm long). Because the sol was viscous and solidified quickly (within 1000 s), it did not leak from the bottoms of the straws. Plastic straws were employed as sample holders because they are simple to process and use, low-cost, highly transparent to X-rays, and allow the easy introduction of viscous samples [24]. The hot sol in the straw was allowed to cool to 25 °C, thus forming a solidified gel. The height of the gel column in the sample tube was ~40 mm.

Preparation of gel samples and optical microscope observation
Another Cu rod (HIKARI, CM395-3; 3 mm diameter and ~20 mm long) was placed atop the gel as an anode. This Cu rod was narrower than that at the tube bottom. Because it did not fit tightly inside the straw, the Cu anode maintained contact with the gel surface even when the electric field caused the gel sample to contract. The cathode and anode were connected to a programmable power supply (1696B, B&K Precision, Yorba Linda, CA, USA). During voltage application at 25 °C for 100 h, the precipitation patterns formed in the sample tube were monitored using a digital camera (IXY650, Canon, Japan). The formed patterns were further monitored for 50 h without voltage application, and, thus, the total observation time was 150 h. The period of voltage application of 100 h was chosen because the precipitation patterns showed almost no further changes after ~90 h of constant voltage application. Additional monitoring for 50 h was conducted, because under cyclic alternating voltage conditions, the precipitation patterns sometimes changed noticeably even after the application of voltage had stopped (as shown later).
After monitoring the formed pattern, the gel sample was pulled out of the straw and repeatedly immersed in deionized water (~200 mL) until the water no longer showed the characteristic yellow color of unreacted [Fe(CN)6] 3-ions. This soaking process typically took 3 days. The gel sample was then placed in the straw one more time and plugged at both ends by styrene-resin stoppers covered with Parafilm. The repacked gel sample was examined using an optical microscope (SKM-S31C-PC, Saitoh Kougaku, Japan) and then mounted on a handmade holder (acrylic resin, 80 mm × 30 mm × 10 mm (h × w × d)) for Xray fluorescence (XRF) experiments.
For comparison, the conventional setup (illustrated in Figure 1a) was also used to produce precipitation patterns of Cu-Fe PBA in agarose gels (1.0-2.0 mass% agarose). In this case, gel columns containing [Fe(CN)6] 3-and [Fe(CN)6] 4-ions were separately prepared in glass tubes (4 mm diameter and 60 mm long) in a similar manner to the above description. These gel columns were employed as the inner electrolyte gels, their height was ~35 mm, and the concentration of [Fe(CN)6] 3-or [Fe(CN)6] 4-therein was 0.010-0.100 M. For the outer electrolyte gel containing Cu 2+ ions, CuCl2•2H2O powder was dissolved in deionized water at 25 °C. After adding 1.0 mass% agarose, the mixture was vigorously stirred at 98 °C for 30 s to prepare a uniform Cu 2+ sol (0.100-0.500 M). This sol was poured over the inner electrolyte ([Fe(CN)6] 3-/[Fe(CN)6] 4-) gel columns using a Pasteur pipette, and it solidified into a gel (height: ~20 mm) within 1000 s.

Fe Kα intensity distribution measurements reparation of gel samples and optical microscope observation
Laboratory XRF experiments were conducted using a homemade setup, the details of which have been provided previously [25]. Briefly, the excitation source was Cu Kα1 Xrays from an 18 kW generator (RU-300, Rigaku, Tokyo, Japan) operating at 40 kV and 60 mA, and the beam was focused to within 0.5 mm in the horizontal direction by an SiO2 (101 1) Johansson-type crystal monochromator. The sample tube mounted on the holder was placed perpendicular to the incident X-ray beam, which had a linear shape, on a computer-controlled X-Z stage. The XRF signals from the sample tube were detected using a silicon PIN detector (XR-100CR, Amptek, Bedford, MA, USA), and the data were collected for 90 s using a multichannel analyzer (MCA8000A, Amptek).
The distribution of Fe Kα intensity from the sample tube in the X-direction was monitored at 25 °C by moving the sample tube in the same direction in 0.5 or 1.0 mm increments. After subtracting the constant background from the Fe Kα peak, the integrated intensities over 6214-6647 eV were used to determine the Fe Kα intensity distribution. In situ time-resolved Fe Kα distributions as the precipitation patterns evolved (as reported in previous studies [25][26][27][28][29][30]) were not measured because the Fe Kα intensity from the unreacted [Fe(CN)6] 3-ions was too strong to allow the examination of the distribution of Cu-Fe PBA formed in the tube.

SEM observation of crystallites in the precipitation patterns
After the XRF measurements, the gel sample was pulled out of the sample tube and cut into ~1 mm-thick sections. The sections were allowed to dry for a few days in the ambient laboratory environment, stuck on double-sided adhesive carbon tape, and mounted on the aluminum stub of the field-emission scanning electron microscope (SEM; SU8220, Hitachi, Japan). SEM observation was conducted at 2.0 kV at working distances of 3.3-3.9 mm. Several images were acquired with a gradual increase in magnification to observe the crystallites formed in the gel sample. Figure 2 shows the typical precipitation patterns of Cu-Fe PBA formed in the conventional setup (Figure 1a). It was found that the Cu-Fe PBA tended to produce a continuous precipitation band in agarose gels, regardless of preparation conditions such as the initial electrolyte concentration and density of the agarose gels. Similar trends have also been reported for Co-Fe-based PBA (Co-Fe PBA) [25,26] and Prussian blue [23,25,27], whereas Mn-Fe PBA tend to generate periodic (Liesegang) bands [28,29]. The color of the precipitates depends on the oxidation states of Fe: reddish-brown for Cu-Fe II PBA con   As shown in Figure 3, a continuous band formed near the gel boundary immediately after adding the outer electrolyte (Cu 2+ ) sol. This band expanded monotonously with time in the inner electrolyte gel (according to the elapsed time indicated at the right of each image) without generating Liesegang bands.  After 40 h, a wide region on the anode side became green. Typically, aqueous Cu 2+ ions give a blue color in gel/solution, but they could appear green when mixed with [Fe(CN)6] 3-ions, which give a yellow color ( Figure 5). Thus, the green color in the sample tube suggests the accumulation of aqueous Cu 2+ ions without generating Cu-Fe III PBA, which is typically ocher (Figure 2b). These images were acquired after ~300 s of the addition of the Cu 2+ gel. When seen from above, the blue Cu 2+ gel appears green.

Formation of multicolored patterns at constant voltage in the electrochemical setup
After 65 h, the reddish-brown band, which was not periodic but continuous, propagated toward the anode by ~3.5 mm in the direction of movement of the [Fe(CN)6] 4-ions, and the green color at the anode side deepened. The reason why the precipitate front propagated only toward the anode side is not clear currently. However, one possible cause is that, on voltage application, [Fe(CN)6] 3-ions (as well as [Fe(CN)6] 4-ions generated from the cathode) become depleted near the cathode over time as a result of their transport to the anode side, thus preventing the precipitation of Cu-Fe PBA near the cathode (such depletion is less expected at the anode side).
After 90 h, the pattern was well-developed and showed almost no further changes, even after stopping the voltage application at 100 h (compare the images taken at 90 and 135 h). Interestingly, the characteristic yellow color of [Fe(CN)6] 3-ions still remained near the cathode after 90 h, suggesting that (1) the constant voltage application of 2 V only moved [Fe(CN)6] 3-ions slowly, and, hence, (2) diffusion contributed significantly to ion transport, nucleation, and crystallization in the sample tube.
The last image in Figure 4 was obtained after removing the unreacted ions. The yellow color disappeared, but the reddish-brown band persisted. Interestingly, the characteristic blue color of aqueous Cu 2+ ions also remained over a wide area at the anode side (right side), suggesting that the Cu 2+ ions formed sparingly soluble Cu(OH)2 precipitates. The formation of Cu(OH)2 precipitates in the sample tube is possible because OHions could be generated by a side reaction at the cathode (2H O + 2e → H + 2OH ) and then migrate to the anode side under the influence of the static electric field to react with Cu 2+ ions. Note also that the ocher color characteristic to Cu-Fe III PBA was not observed. The absence of this color strongly suggests that [Fe(CN)6] 3-ions are less reactive with aqueous Cu 2+ ions than [Fe(CN)6] 4-and OHions in the proposed electrochemical setup. It should be noted that Cu-Fe PBA can be also formed on the Cu electrodes. Figure  6a shows significant amounts of deposits at the cathode and anode after 100 h at 2 V. These deposits were firmly bonded to the electrodes, and, hence, the electrodes required polishing with sandpaper of different grades (#120, #240, and #400) after the experiments. Moreover, Figure 6b shows that the boundary between the [Fe(CN)6] 3-gel and Cu rod is sufficiently reactive to form a small amount of reddish-brown compounds (probably Cu-Fe II PBA) without voltage application. This reactivity can be explained as follows. At the boundary without an applied voltage, the ions forming Cu-Fe II PBA (Cu   Meanwhile, the reddish-brown and green colors generated at 4 V were deeper than those generated at 2 V, suggesting greater amounts of Cu-Fe II PBA precipitates and aqueous Cu 2+ -related compounds, respectively. Moreover, compared to the behavior observed at 2 V, band propagation to the anode side was considerably suppressed at 4 V, and the resultant band was narrower (2 mm vs. 3.5 mm (approximate values)). This finding suggests that an increase in the applied voltage from 2 to 4 V is effective in restricting the broadening of the Cu-Fe II PBA precipitation band.
Interestingly, a sharp line structure appeared in the green region after 40 h at 4 V ( Figure 7). This structure remained in the same location and was distinguishable after removing the unreacted ions. As discussed in a previous study concerning Mn-Fe PBA precipitates in water-glass gels [29], these light-colored band-in-band structures can form in slightly soluble precipitates when there is a local shortage of the constituent compounds. Thus, the line structure in Figure 7 suggests again the coexistence of slightly soluble precipitates, such as Cu(OH)2, in the blue region of the gel sample after removing unreacted ions.
In addition, occasionally, the gel sample shrunk during the application of a constant voltage of 4 V, mainly at the cathode side. At higher voltages, such shrinkage occurred more frequently and prevented detailed observations. Additionally, at higher voltages, (1) the yellow color near the cathode rapidly disappeared without the formation of the reddish-brown band (e.g., within 40 h at 8 V), and (2) the contact between the cathode and gel was frequently lost because of the formation of bubbles (possibly H2) on the cathode. Meanwhile, at applied voltages below 2 V, the reddish-brown color of the band formed in the sample tube was very light, even after 100 h, suggesting that the concentration of generated Cu-Fe II PBA was very low. Thus, in the current setup, the applied constant voltages used to examine the precipitation patterns in detail were limited from 2 to 4 V. Figure 8 shows the spatiotemporal evolution of a typical multicolored pattern formed in the sample tube under applying a cyclic alternating voltage: i.e., 4 V for 1 h and then 1 V for 4 h per cycle for a total of 20 cycles. In this cyclic voltage sequence, few reactant ions will be produced at 1 V, and diffusion should exert a stronger effect on the residual ions, thus stimulating the formation of wide, diffuse precipitation patterns. In contrast, the stronger electric field at 4 V should have a greater influence on the reactant ions, thus producing narrow, thick precipitation bands, as suggested by the constant voltage experiments. After 15 h of cyclic voltage application (3 cycles), the wide region at the anode side became slightly green. However, no marked reddish-brown band was observed, which is unlike the observations obtained at constant voltages of 2 and 4 V (see Figures 4 and 7). After 40 h (8 cycles), several short, faint, and reddish-brown bands were formed near the cathode (~10 mm from the cathode surface). After 65 h (13 cycles), the number of thin reddish-brown bands increased. It should be noted that the formation of these periodic bands was stochastic, having a probability of ~50 %; in the other ~50% of cases, an almost continuous band was formed (Figure 9). During the stochastic formation of the periodic bands, the green region became deeper in color, and this trend continued throughout the voltage application up to 100 h. Interestingly, even after stopping the voltage application, These stochastically formed periodic bands showed the following common features.

Formation of multicolored periodic bands under cyclic alternating voltage in the electrochemical setup
(1) The periodic bands were formed within a relatively narrow region (< 5 mm). (2) The number of the residual bands after removing unreacted ions was within 12 ± 5. (3) The spaces between the adjacent bands were within 0.30 ± 0.25 mm after removing unreacted ions (details will be discussed later). (4) The positions of the periodic bands were maintained over the observation time, similar to the unusual Liesegang bands previously found in a Co-Fe PBA system [30]. (5) After removing unreacted ions, several periodic bands became blue instead of reddish-brown, strongly suggesting the presence of Cu(OH)2 precipitates (as already suggested in Figures 4 and 7). Figure 10a provides an enlarged image of the multicolored periodic bands after removing unreacted ions (bottom image in Figure 8) together with 0.5 mm graduations for ease of comparison. These periodic bands are numbered from n = 1 (the cathode side) to 15 (the anode side). Their positions (Xn, n = 1-15) were measured using the graduations with an accuracy of ± 0.05 mm to determine the band spacing dn = Xn+1 -Xn, which is plotted in Figure 10b.
It is well known that Liesegang bands tend to follow an empirical scaling law, the socalled spacing law, irrespective of the electrolyte pair and the geometry of the system: Xn+1/Xn = 1+ p, where p > 0 for most systems [1−5]. This law can also be described as , indicating that the dn value increases monotonically with n (for p > 0).  Figure 10b indicates that the obtained dn values did not increase monotonically, thus failing to obey the spacing law, but were rather randomly distributed around an average value (0.30 mm) with a broad dispersion (± 0.25 mm), as mentioned before. It is not surprising that the dn values disobey the spacing law because the mechanism to form periodic bands in the current setup (Figure 1c) is fundamentally different from that in the conventional setup used to examine Liesegang banding (Figure 1a). Note that the average dn value (0.30 mm) is comparable to its dispersion value (± 0.25 mm). Under this situation, the periodic bands can easily overlap one another to form almost continuous bands (as found in Figure 9c and 9d), particularly when relatively broad bands (such as the bands of n = 1-4 in Figure 10a) form stochastically. Thus, Figure 10 implies that the expansion of the band spaces is effective for generating periodic bands with higher probability. The related experimental issues will be discussed later. Figure 11 shows the Fe Kα intensity distribution of the gel sample having multicolored periodic bands (shown in Figures 8 and 10) formed under the cyclic alternating voltage. The horizontal axis indicates the distance from the periodic band of n = 1 (X), where X > 0 is on the anode side. The vertical axis is the relative Fe Kα intensity. As already shown in previous studies [27,28], the Fe Kα distributions of gel samples forming PBA precipitates provide a good estimate of the Fe elemental distributions. Because the current XRF experiments were conducted after removing the unreacted [Fe(CN)6] 3-ions, the measured Fe Kα distribution should approximate the distribution of the Cu-Fe PBA formed in the gel sample. Figure 11. Fe Kα intensity distribution of the multicolored pattern formed under the cyclic alternating voltage, obtained after removing the unreacted ions. An image of the gel sample is displayed at the top to facilitate comparison with the periodic bands.

Fe Kα intensity distribution of the pattern formed under cyclic alternating voltage
The Fe Kα intensity was relatively strong in regions close to the electrodes (X = -9.0 and 26.0 mm). This result is consistent with the fact that considerable amounts of deposits (probably Cu-Fe II PBA) were present at the electrodes ( Figure 6). Interestingly, a strong Fe Kα intensity (~125 in Figure 11) was also observed in the reddish-brown periodic bands on the cathode side (n = 2-4 in Figure 10a, named "main bands" hereafter) with a sharp peak at X = 0.5 mm (± 0.25 mm: this uncertainty is due to the focus size of incident X-rays), strongly suggesting that Cu-Fe II PBA specifically accumulated in the main bands. Such highly localized precipitation is expected to cause the depletion of reactant ions (and, thus, also Cu-Fe PBA) nearby. Indeed, the Fe Kα intensity around the main bands was low, resulting in a broad valley-like structure around X = 3.0 mm. This broad valley-like region is where the blue periodic bands (n ≥ 12) are located. This finding supports the hypothesis that the blue bands mainly consist of Cu(OH)2 instead of Cu-Fe PBA, as indicated by the blue color itself. Except for the main bands, other reddish-brown periodic bands (denoted "non-main reddish-brown (RB) bands" hereafter) did not have very strong Fe Kα intensities, although a weak peak in the distribution was found at X = 2.0 mm, corresponding to the position of non-main RB bands of n = 7-9. Therefore, it is likely that the non-main RB bands did not contain significant quantities of Cu-Fe II PBA.
Note that the Fe Kα intensities of the wide blue region (8.0 < X < 23.0 mm) are comparable to those of the non-main RB bands. Thus, to our surprise, Cu-Fe PBA (reddishbrown or ocher in color) should be also present in the blue region. The amount there is estimated to be ~2/5 of that in the main bands, based on the Fe Kα intensities (50 vs. 125 (approximate values)). Additional explanation of this interesting feature is given in the next section. Figure 12 shows the optical microscopy images (×1000) of the gel sample having multicolored periodic bands formed under the cyclic alternating voltage (the corresponding Fe Kα distribution is shown in Figure 11). The positions where the images were acquired are indicated in the uppermost panel. Many reddish-brown crystallites (sizes: approximately1-10 μm) are visible in Figure  12, not only in regions close to the electrodes (Figure 12a and 12e, where the crystallite sizes were relatively large) and the main bands (Figure 12b) but also in the blue region (Figure 12c and 12d). This finding strongly suggests that micrometer-sized Cu-Fe II PBA crystallites (which are too small to be visible to the naked eye) were generated over a wide region in the gel sample on the application of the cyclic alternating voltage. The existence of these crystallites in the blue region can explain the non-negligible Fe Kα intensities at 5.0 < X < 23.0 mm in Figure 11. On the other hand, the approximately flat Fe Kα distribution in the blue region suggests an even probability of Cu-Fe II PBA crystallite formation there. The mechanism that generated these widely dispersed crystallites remains unclear at present and requires future research.

Microscopic observation of the pattern formed under cyclic alternating voltage
At position b in Figure 12 (the main band, n = 2), the crystallites are visible against the reddish-brown background, suggesting that finer Cu-Fe II PBA crystallites (< 1 μm) also contribute to the main bands. The ratio of the quantities of larger crystallites (particles in Figure 12b, 1-10 μm) to smaller crystallites (reddish-brown background in Figure 12b, < 1 μm) in the main bands was estimated as follows. A comparison between Figures 12b  and 12d shows that the numbers of large crystallites in the main bands and the blue region are comparable. As mentioned above concerning the Fe Kα distribution, the amount of Cu-Fe II PBA in the blue region (where most of the crystallites are larger ones) is ~2/5 of that in the main bands. Thus, approximately 1 -2/5 = 3/5 of the Cu-Fe II PBA is expected to exist as smaller crystallites in the main bands. In other words, the ratio of the quantities of larger and smaller crystallites is ~2/3, suggesting a dominance of smaller crystallites in the main bands. Figure 13 shows SEM images of the gel sample having multicolored periodic bands formed under the cyclic alternating voltage (other results related to the same sample are shown in Figures 8, 10-12). Figure 13a, 13b, and 13c were obtained for the periodic bands of n = 1 (the non-main RB band), 2 (the main band), and 12 (the blue band), respectively. For comparison, a region close to the anode is also shown in Figure 13d.

SEM observation of the pattern formed under cyclic alternating voltage
As shown in Figure 13d, the precipitates close to the anode consisted of crystallites that were definitely cubic, which is characteristic of PBA [23]. In accordance with the relatively high Fe Kα intensity in Figure 11 (i.e., a large amount of Cu-Fe PBA), there were numerous crystallites. The crystallite sizes (1-3 μm on each side) are somewhat smaller than those of Mn-Fe PBA crystallites formed in agarose gels in the conventional setup for Liesegang banding (3-10 μm on each side) [23]. Despite the different (but comparable) sizes, the image in Figure 13d is very similar to the SEM images acquired previously for precipitation bands of Mn-Fe PBA in agarose gels [23,31]. Figure 13b shows an SEM image of the precipitates formed in the main band of n = 2. These precipitates also consisted of cube-like crystallites, even though their sizes were considerably smaller (0.1-0.8 μm on each side) and the shapes were not perfectly cubic, suggesting the existence of many defects. These small crystallites can be considered to form the reddish-brown background observed in Figure 12b.
The somewhat irregular shapes of the crystallites in Figure 13b are disappointing if one expects well-defined PBA crystallites with few defects for use as electrodes [15,16,20] or magnets [19]. However, if used as adsorbents or catalysts for ions and molecules, smaller PBA crystallites with many defects would be advantageous because of their inherently large surface area. Indeed, the importance of defects (i.e., porosity) has been reported in several studies on the adsorption/catalytic properties of PBA [17,18,[20][21][22]32] Figure 13a shows an SEM image of the precipitates formed in the non-main RB band of n = 1. Interestingly, in addition to the cube-like crystallites, there were also plate-like crystallites (indicated by white circles). This finding strongly suggests that the non-main RB bands consisted of two types of crystallites (i.e., plate-like Cu(OH)2 and cube-like Cu-Fe PBA). Figure 13c shows an SEM image of the precipitates formed in the blue band of n = 12. Unlike in the other images, this image shows only a few cube-like crystallites, as expected. Instead, plate-like crystallites were dominant, and there were even laminates of these The position-dependent size and shape of the crystallites formed in the proposed setup, as shown in Figure 13, suggest the potential applications of the electrochemically periodic banding phenomenon for selective preparation of PBA, as mentioned in the introduction. However, unfortunately, the current periodic banding occurred stochastically (having a probability of ~50%), and some byproducts were also present. To establish the electrochemical banding system(s) having practical application in material science and engineering, better control over the periodic bands is required, especially concerning the (1) amounts, sizes, and shapes of crystallites, (2) amounts of byproducts formed, (3) spacing between bands, and (4) reproducibility.
First, achieving the above objectives requires a deeper understanding of the observed periodic banding. As a starting point, theoretical models of Liesegang bands may be useful. Modern theoretical models for Liesegang banding can be approximately classified into pre-or post-nucleation models, depending on the sequence of elementary events [1][2][3]5,[33][34][35][36]. Pre-nucleation models assume that the precipitation bands are formed as a result of repeated cycles of the supersaturation, nucleation, and depletion of the reaction products. In these models, the crystallites are formed by rapid nucleation and crystallization triggered by supersaturation, and, hence, they should be relatively small in size and irregular in shape [23]. In contrast, post-nucleation models assume the competitive growth of small particles of reaction products (including crystallites). According to these models, the crystallites in Liesegang bands must be relatively large in size because most of them have undergone Ostwald ripening [23]. Overall, the sizes and shapes of the crystallites in Liesegang bands can be used to identify the dominant formation processes: small and irregular crystallites are likely formed according to the pre-nucleation models, whereas relatively large crystallites indicate the dominance of the post-nucleation processes.
Although the mechanisms of Liesegang banding and the current electrochemical banding are different, the correlation between the dominant processes in precipitation banding and the sizes and shapes of the resultant crystallites should remain valid. The SEM image in Figure 13b is more consistent with pre-nucleation models, i.e., rapid nucleation and crystallization triggered by supersaturation were dominant in forming the main bands. Nevertheless, this suggestion is qualitative and tentative, and more quantitative and comprehensive models are required.
Second, the optimal experimental conditions to produce well-controlled periodic bands should be further explored. Conventional precipitation banding of PBA in gels (using the setup in Figure 1a) is known to be dependent on the experimental conditions, including the gel type, gel density [29], and presence of magnetic fields [37]. The precipitation patterns formed using the proposed electrochemical setup should be examined while varying these factors (as well as the initial concentration of [Fe(CN)6] 3-and the gel length). The optimal external potential, including voltage, period, and number of cycles for cyclic alternating voltage application, should be also explored further. Additionally, variation in the sizes, materials, and shapes of the electrodes may also have interesting effects on the banding.
Third, the reaction products formed in the periodic bands, blue region in the gel, and anode and cathode regions should be more comprehensively characterized. For instance, the defect concentration in the Cu-Fe PBA crystallites formed in these regions should be measured quantitatively and separately. In addition, the local structure(s) around the Cu atoms and the crystallinity could be investigated by X-ray absorption fine structure spectroscopy and X-ray diffractometry, respectively. The adsorption properties of the Cu-Fe PBA crystallites generated by the proposed system should also be compared to those prepared by conventional methods. Additionally, the characteristics and distribution of the byproducts must be studied.
Fourth, simple and effective methods should be developed for cleaning the electrodes. As shown in Figure 6a, considerable deposits accumulated on the electrodes, which could pose a serious problem when applying this method to microscale fabrication processes.
Fifth, the extension of the electrochemical experiments to other PBA systems may expand the potential applications. Co-Fe PBA and Ni-Fe-based PBA could be easily produced using the current setup after substituting Co and Ni anodes for the Cu anode, respectively.

Conclusions
We have proposed a simple and novel electrochemical setup for producing precipitation patterns in hydrogels. On the application of a cyclic alternating voltage, this setup can produce periodic precipitation bands containing cube-like reddish-brown (possibly Cu-Fe II PBA) crystallites (albeit stochastically), of which the formation was not observed in conventional setup for Liesegang banding. This new approach for periodic banding utilizing electrochemical processes has many interesting features, and the associated potential applications in material science and engineering merit further investigation.