# Alkali Cation Potential and Functionality in the Nanoporous Prussian Blue Analogues

Authors: Yutaka Moritomo; Hiroshi Tanaka
Journal: Advances in Condensed Matter Physics
 (2013)

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## Abstract

Cation and/or molecule transfer within nanoporous materials is utilized in lithium-ion secondary battery, ion exchange, hydrogen storage, molecular sensors, molecular filters, and so on. Here, we performedab initio total energy calculation to derive the alkali cation potential in the Prussian blue analogues, AxM[Fe(CN)6]yzH2O (A=Li, Na, K, Rb, and Cs; M=Co, Ni, Mn, and Cd), with jungle-gym-type nanoporous framework. The potential curves of larger cations, that is, K+, Rb+ and Cs+, exhibit a barrier at the window of the host framework, while those of the smaller cations, that is, Li+ and Na+, exhibit no barrier. We will discuss the useful functionalities observed in the Prussian blue analogues, that is, (a) battery properties mediated by Li+ intercalation/de-intercalation, (b) electrochromism mediated by Na+ transfer in all solid device, and (c) the elimination of Cs+ from aqueous solution by precipitation, in terms of the alkali cation potentials.


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## Body

## 1. Introduction

Nanoporous materials are attracting the increasing interest of material scientists because the materials are utilized in lithium-ion battery, ion exchange, hydrogen storage, molecular sensors, and molecular filters, and so on. To further improve the functionality, we need to comprehend the cation and molecular routes and their potential within the host framework. Among the nanoporous materials, the Prussian blue analogues,AxM[Fe(CN)6]yzH2O (A and M are alkali metal and transition metal, resp.), are attracting current interest of material scientists because they exhibit useful functionalities, such as battery properties mediated by Li+ intercalation [1–8], electrochromism mediated by Na+ intercalation [9–16], and the elimination of Cs+ from aqueous solution by precipitation [17]. The Prussian blue analogue is the oldest complex compound that the human being synthesized. The compound is easily synthesized from cheap and ubiquitous source materials and, hence, has great advantage for commercial use of the above-mentioned functionalities.The Prussian blue analogue,AxM[Fe(CN)6]yzH2O, consists of a three-dimensional (3D) cyano-bridged transition metal framework (M[Fe(CN)6]y) and guests (A+ and H2O), as schematically shown in Figure 1. A part of the waters (ligand water: H2Ol) locates at the [Fe(CN)6] vacancies and coordinates to the transition metal. The residual waters (zeolite water: H2Oz) and alkali cations (A+) locate in the nanocubes of the host framework. Most of the Prussian blue analogues exhibit the face-centered cubic structure (Fm3_m; Z=4) [18].Figure 1
Schematic structure of the Prussian blue analogue,AxM[Fe(CN)6]yzH2O (A and M are alkali metal and transition metal, resp.). Transition metal and iron (small spheres) are alternatively bridged by the cyano groups (sticks). Large spheres represent the guest alkali cations. Water molecules are omitted for simplicity.The framework size of the nanocube can be finely-controlled by the substitution ofM, whose ionic size (rM) changes from rM=0.061 nm for Fe2+ to 0.083 nm for Mn2+. As shown in Figure 2(a), the magnitude of a increases linearly with rM as [nm] = 0.891 + 2rM [nm] in (Cs,Rb)xMII[FeIII(CN)6]y (M=Co, Fe, Ni, Cu, Zn, Mn, and Cd) [18]. Incidentally, the lattice property of the host framework systematically changes with the framework size (=a/2). For example, the magnitude and sign of the thermal expansion coefficient (β=dlna/dT) systematically change from positive to negative with increase in a (Figure 2(b)). The behavior was explained by the steric hindrance effect of the rotational fluctuation of the [Fe(CN)6] units [18]. The rotational fluctuation is suppressed in the small-a compounds, causing the conventional positive thermal expansion.(a) Lattice constant (a) against ionic radius (rM) of transition metal in the Prussian blue analogues. (b) Thermal expansion coefficient (β=dlna/dT) against a in the Prussian blue analogues. Solid line in (a) is the result of the least-squares fitting. Data were cited from [18].
(a)
(b)Historically, cation transfer within the Prussian blue analogues is interpreted in terms of the hydrated radius (rH) [19–22] rather than the ionic radius (rA). This is because the Prussian blue analogues contain considerable amount of zeolite water, and hydration energy is needed to form a bare cation at the liquid-solid interface. Actually, Tieke’s group [21, 22] reported that self-assembled films of the Prussian blue analogues are permeable to smaller hydrated ions such as Cs+ (rH=0.119 nm) and K+ (rH=0.125 nm), whereas they block larger hydrated ions such as Na+ (rH=0.184 nm). These films, however, consist of microcrystals with considerable [Fe(CN)6] vacancies (y~0.67). This suggests that the hydrated ions migrate along the vacancies and/or grain boundaries. Recently, Moritomo et al. [23] electrochemically synthesized a thin film of Na0.76Co[Fe(CN)6]0.902.9H2O (y=0.9) with fewer vacancies. In addition, the film consists of crystalline large rod-shaped grains and has few grain boundaries. They observed that the intercalation of Na+ (rA=0.118 nm) is much faster than those of K+ (rA=0.151 nm) and Rb+ (rA=0.161 nm) in this film. This suggests that the cation transfer within the Prussian blue framework should be interpreted in terms of rA of the bare cation: Li+ (rA=0.092 nm), Na+ (0.118 nm), K+ (0.151 nm), Rb+ (0.161 nm), and Cs+ (0.174 nm).In this paper, we performedab initiototal energy calculation in the Prussian blue analogues, AxM[Fe(CN)6]yzH2O (A = Li, Na, K, Rb, and Cs; M = Co, Ni, Mn, and Cd). The alkali cation potentials of larger K+, Rb+, and Cs+ exhibit a potential barrier at the window of the host framework, while those of the smaller Li+ and Na+ exhibit no barrier. We will discuss the useful functionalities observed in the Prussian blue analogues, that is, (a) battery properties mediated by Li+ intercalation/de-intercalation, (b) electrochromism mediated by Na+ transfer in all solid device, and (c) the elimination of Cs+ from aqueous solution by precipitation, in terms of the alkali cation potentials.


## 2.Ab Initio Total Energy Calculation

### 2.1. Method of Calculation

Theab initio total energy calculation was performed for an ideal Prussian blue lattice, that is, AM[Fe(CN)6] (A = Li, Na, K, Rb, and Cs; M = Co, Ni, Mn, and Cd), using the program package WIEN2k [24] for the full potential linear augmented wave (FLAPW) method. We employed a potential based on the generalized gradient approximation (GGA) proposed by Perdew et al. [25]. We confirmed that the final results are nearly independent of the approximation of the potential. The alkali cation potential corresponds to the total energy difference ΔE against the alkali cation coordinate (z). In order to move the A+ ion, tetragonal space group (Imm2: Z=2) was adopted instead of the actual cubic space group (Fm3_m; Z=4).z=0 corresponds to the window position, as z=±1/4 does to the nanocube center.In the Mn and Co compounds, the actual lattice parameters, that is, Na1.32Mn[Fe(CN)6]0.83·3.6H2O (a=1.056601 nm) [26] at 340 K and K0:34Co[Fe(CN)6]0:75·6H2O (a=0.93440 nm) [27] at 90 K, were adopted (see Tables 1 and 2). The magnitude of a(=1.05561 nm) for M = Mn is much larger than that (=0.93440 nm) for M = Co. In the Ni (a = 1.02915 nm) and Cd (a=1.0755 nm) compounds, we used the same atomic coordinates as M=Mn.Table 1
Structural parameters used in theab initio total energy calculation of AMn[Fe(CN)6] (A = Li, Na, K, Cs, and Rb). The lattice constants are a = b = 0.74730 nm and c = 1.056601 nm.
Atom
Site
g
x
y
z
Fe
2a
1
0
0
0
Mn
2a
1
0
0
1/2
C
8e
1
0.32461
0.67539
1/2
C
2a
1
0
0
0.82461
C
2a
1
0
0
0.17539
N
8e
1
0.20884
0.79116
1/2
N
2a
1
0
0
0.70884
N
2a
1
0
0
0.29116
A
2b
1
1/2
0
zTable 2
Structural parameters used in theab initio total energy calculation of ACo[Fe(CN)6] (A = Li, Na, K, Cs, and Rb). The lattice constants are a = b = 0.66072 nm and c = 0.93440 nm.
Atom
Site
g
x
y
z
Fe
2a
1
0
0
0
Co
2a
1
0
0
1/2
C
8e
1
0.31995
0.68005
1/2
C
2a
1
0
0
0.82461
C
2a
1
0
0
0.17539
N
8e
1
0.20464
0.79536
1/2
N
2a
1
0
0
0.70464
N
2a
1
0
0
0.29536
A
2b
1
1/2
0
z


### 2.2. Results and Discussion

Figure3 shows total energy difference ΔE of (a) AMn[Fe(CN)6] and (b) ACo[Fe(CN)6] against cation coordinate (z). The profile of the alkali cation potential is determined by the short-range atomic repulsive interaction as well as the long-range electrostatic interaction. In both materials, the potential curves for K+, Rb+, and Cs+ exhibit a barrier at z=0. The heights of the potential barrier (Δ) steeply decrease with the decrease in rA. The Δ-values (>0.3 eV) for K+, Rb+, and Cs+ are much higher than the thermal energy (=0.03 eV) at room temperature, indicating that ionic migration is impossible. On the other hand, the potential curves for Li+ and Na+ have no barrier at z=0, indicating that these cations rapidly migrate within the host framework. Reflecting the smaller a-value of ACo[Fe(CN)6], the Δ-rA curve of ACo[Fe(CN)6] shifts toward the higher energy side (see Figure 4).Total energy difference ΔE of (a) AMn[Fe(CN)6] and (b) ACo[Fe(CN)6] against cation coordinate (z). z=0 corresponds to the window position, as z=±1/4 does to the nanocube center.
(a)
AxMn[Fe(CN)6] a=1.05561 nm
(b)
A
xCo[Fe(CN)6] a=0.93440 nmFigure 4
Potential barrier (Δ) at the window against ionic radius (rA) of alkali cation in AM[Fe(CN)6] (M = Co, Ni, Mn, and Cd).The Li+ and Na+ potential curves of AMn[Fe(CN)6] (see Figure 2(a)) exhibit local minima at the square window (z=0). Similar trend is observed in the Na+ potentials of ACo[Fe(CN)6] (see Figure 3(b)). These observations suggest that the central position (z=±1/4) of the nanocube is not the potential minima. The nanocube consists of four [Fe(CN)6]3- and four M2+, and, hence, the resultant electrostatic potential has Td symmetry. Then, the potential minimum is considered to be at the tetrahedral site toward the four [Fe(CN)6]3−. Consistently, Moritomo et al. [26] performed structural analysis of Na1.32Mn[Fe(CN)6]0.83·3.6H2O at 300 K and found that Na+ randomly occupies the tetrahedral site. The small ionic radius is considered to be a necessary condition for the tetrahedral displacement, since the larger ions feel short-range atomic repulsive interaction from the host framework. Actually, no displacement of K+ is observed in K0:34Co[Fe(CN)6]0:75·3.6H2O and K0:34Co[Fe(CN)6]0:75·2.7H2O [27]. Even though the tetrahedral site is beyond the investigated route, the actual Li+ and Na+ route seems to be window center → tetrahedral site → window center. We emphasize that the potential barrier in this route is further suppressed as compared with the route, window center → nanocube center → window center.


## 2.1. Method of Calculation

Theab initio total energy calculation was performed for an ideal Prussian blue lattice, that is, AM[Fe(CN)6] (A = Li, Na, K, Rb, and Cs; M = Co, Ni, Mn, and Cd), using the program package WIEN2k [24] for the full potential linear augmented wave (FLAPW) method. We employed a potential based on the generalized gradient approximation (GGA) proposed by Perdew et al. [25]. We confirmed that the final results are nearly independent of the approximation of the potential. The alkali cation potential corresponds to the total energy difference ΔE against the alkali cation coordinate (z). In order to move the A+ ion, tetragonal space group (Imm2: Z=2) was adopted instead of the actual cubic space group (Fm3_m; Z=4).z=0 corresponds to the window position, as z=±1/4 does to the nanocube center.In the Mn and Co compounds, the actual lattice parameters, that is, Na1.32Mn[Fe(CN)6]0.83·3.6H2O (a=1.056601 nm) [26] at 340 K and K0:34Co[Fe(CN)6]0:75·6H2O (a=0.93440 nm) [27] at 90 K, were adopted (see Tables 1 and 2). The magnitude of a(=1.05561 nm) for M = Mn is much larger than that (=0.93440 nm) for M = Co. In the Ni (a = 1.02915 nm) and Cd (a=1.0755 nm) compounds, we used the same atomic coordinates as M=Mn.Table 1
Structural parameters used in theab initio total energy calculation of AMn[Fe(CN)6] (A = Li, Na, K, Cs, and Rb). The lattice constants are a = b = 0.74730 nm and c = 1.056601 nm.
Atom
Site
g
x
y
z
Fe
2a
1
0
0
0
Mn
2a
1
0
0
1/2
C
8e
1
0.32461
0.67539
1/2
C
2a
1
0
0
0.82461
C
2a
1
0
0
0.17539
N
8e
1
0.20884
0.79116
1/2
N
2a
1
0
0
0.70884
N
2a
1
0
0
0.29116
A
2b
1
1/2
0
zTable 2
Structural parameters used in theab initio total energy calculation of ACo[Fe(CN)6] (A = Li, Na, K, Cs, and Rb). The lattice constants are a = b = 0.66072 nm and c = 0.93440 nm.
Atom
Site
g
x
y
z
Fe
2a
1
0
0
0
Co
2a
1
0
0
1/2
C
8e
1
0.31995
0.68005
1/2
C
2a
1
0
0
0.82461
C
2a
1
0
0
0.17539
N
8e
1
0.20464
0.79536
1/2
N
2a
1
0
0
0.70464
N
2a
1
0
0
0.29536
A
2b
1
1/2
0
z


## 2.2. Results and Discussion

Figure3 shows total energy difference ΔE of (a) AMn[Fe(CN)6] and (b) ACo[Fe(CN)6] against cation coordinate (z). The profile of the alkali cation potential is determined by the short-range atomic repulsive interaction as well as the long-range electrostatic interaction. In both materials, the potential curves for K+, Rb+, and Cs+ exhibit a barrier at z=0. The heights of the potential barrier (Δ) steeply decrease with the decrease in rA. The Δ-values (>0.3 eV) for K+, Rb+, and Cs+ are much higher than the thermal energy (=0.03 eV) at room temperature, indicating that ionic migration is impossible. On the other hand, the potential curves for Li+ and Na+ have no barrier at z=0, indicating that these cations rapidly migrate within the host framework. Reflecting the smaller a-value of ACo[Fe(CN)6], the Δ-rA curve of ACo[Fe(CN)6] shifts toward the higher energy side (see Figure 4).Total energy difference ΔE of (a) AMn[Fe(CN)6] and (b) ACo[Fe(CN)6] against cation coordinate (z). z=0 corresponds to the window position, as z=±1/4 does to the nanocube center.
(a)
AxMn[Fe(CN)6] a=1.05561 nm
(b)
A
xCo[Fe(CN)6] a=0.93440 nmFigure 4
Potential barrier (Δ) at the window against ionic radius (rA) of alkali cation in AM[Fe(CN)6] (M = Co, Ni, Mn, and Cd).The Li+ and Na+ potential curves of AMn[Fe(CN)6] (see Figure 2(a)) exhibit local minima at the square window (z=0). Similar trend is observed in the Na+ potentials of ACo[Fe(CN)6] (see Figure 3(b)). These observations suggest that the central position (z=±1/4) of the nanocube is not the potential minima. The nanocube consists of four [Fe(CN)6]3- and four M2+, and, hence, the resultant electrostatic potential has Td symmetry. Then, the potential minimum is considered to be at the tetrahedral site toward the four [Fe(CN)6]3−. Consistently, Moritomo et al. [26] performed structural analysis of Na1.32Mn[Fe(CN)6]0.83·3.6H2O at 300 K and found that Na+ randomly occupies the tetrahedral site. The small ionic radius is considered to be a necessary condition for the tetrahedral displacement, since the larger ions feel short-range atomic repulsive interaction from the host framework. Actually, no displacement of K+ is observed in K0:34Co[Fe(CN)6]0:75·3.6H2O and K0:34Co[Fe(CN)6]0:75·2.7H2O [27]. Even though the tetrahedral site is beyond the investigated route, the actual Li+ and Na+ route seems to be window center → tetrahedral site → window center. We emphasize that the potential barrier in this route is further suppressed as compared with the route, window center → nanocube center → window center.


## 3. Battery Properties Mediated by Li+ Intercalation/Deintercalation

### 3.1. Experiment

Thin films of Li0.68Na0.04Ni[Fe(CN)6]0.68·5.1H2O (M = Ni), Li0.71Na0.13Co[Fe(CN)6]0.71·3.8H2O (M = Co), Li1.24Mn[Fe(CN)6]0.81·3.0H2O (M = Mn), and Li0.96Na0.88Cd[Fe(CN)6]0.96·4.8H2O (M = Cd) were synthesized by electrochemical deposition of the Na compounds on an indium tin oxide (ITO) transparent electrode and subsequent electrochemical substitution of Li+ for Na+. In the M = Ni, Co, and Cd compounds, [5] only the Fe site exhibits the redox reaction (Fe2+⟷ Fe3+), and, hence, a part of the Na sites is replaced by Li+. By contrast, two-electron reaction (Fe2+⟷ Fe3+ and Mn2+⟷ Mn3+) takes place in the M = Mn compound [5, 6]. As a result, all the Na sites can be replaced by Li+. Chemical compositions of the films were determined by the inductively coupled plasma (ICP) method and CHN organic elementary analysis (Perkin-Elmer 2400 CHN Elemental Analyzer). Details of the synthesis and characterization are described elsewhere [5].The charge/discharge properties of the thin films were measured against Li in a beaker-type cell. The electrolyte was ethylene carbonate (EC)/diethyl carbonate (DEC) solution containing 1 mol/L LiClO4. The cutoff voltage was from 2.0 to 4.2 V. The thickness and active areas of the films were ~1 μm and 1-2 cm2, respectively. The mass of each film was measured with a conventional electronic weighing machine after the film was carefully removed from the substrate with a microspatula. The experimental error of the mass is 10%. The current density was set to be the same for the charge/discharge process.


### 3.2. Results

Figure5 shows the charge/discharge curves of thin-film electrodes at various rates (v). The discharge capacities at low v (=0.1–1 C) coincides with the ideal value within the experimental error (~10%). In all the compounds, the discharge curves show plateaus at ~3.4 V. This plateau is ascribed to the reduction process at the Fe site (Fe3+ → Fe2+) [5]. The plateau structure is discernible even at high v (<30 C). The capacities at 100 C are 0.66 (M = Ni), 0.31 (Co), 0.62 (Mn), and 0.74 (Cd) of those at 1 C.Charge/discharge curve of thin-film electrodes of (a) Li0.68Na0.04Ni[Fe(CN)6]0.68·5.1H2O, (b) Li0.71Na0.13Co[Fe(CN)6]0.71·3.8H2O, (c) Li1.24Mn[Fe(CN)6]0.81·3.0H2O, and (d) Li0.96Na0.88Cd[Fe(CN)6]0.96·4.8H2O against Li at various rate (v). The discharge curve at v was measured after the charge process at v.
(a)
M
=
Ni
(b)
M
=
Co
(c)
M
=
Mn
(d)
M
=
CdThe Mn compound (Figure5(c)) shows rather complicated behaviors. In the discharge curve, two additional plateaus are observed at 3.8 V and 3.6 V. These plateaus are probably ascribed to the reduction process at the Mn site (Mn3+ → Mn2+) [5, 6]. The oxidization (charge) process of the Mn compound is as follows. At the initial stage (Li1.24Mn2+[Fe2+(CN)6]0.81·3.0H2O), the valence state is Mn2+ and Fe2+. In the first plateau at 3.4 V, the Fe site is selectively oxidized to become Li0.44Mn2+ [Fe3+(CN)6]0.81·3.0H2O. In the second plateau at 3.8 V, parts of the Mn sites are oxidized to become Mn2.44+ [Fe3+(CN)6]0.81·3.0H2O. Recently, Matsuda and Moritomo [28] found that thin film of Na1.32Mn[Fe(CN)6]0.83·3.5H2O exhibits a high capacity of 114 mAh/g and an average operating voltage of 3.3 V against Na with a good cyclability. The electrolyte was propylene carbonate (PC) solution containing 1 mol/L NaClO4. Thus, the Mn compound exhibits reversible intercalation/deintercalation of Li+ and Na+ in organic solvent.


### 3.3. Interrelation with the Alkali Cation Potential

Generally speaking, the alkali cation intercalation process in the Li+ and Na+ secondary batteries can be divided into the transfer process from the electrolyte to host framework and the migration process within the host framework. The former process usually accompanies the desolvation process and is complicated. In the latter process, the bare cation migrates toward the collective electrode with feeling the alkali cation potential. The latter process is essential for the capacity and rate properties of the active material. In the Prussian blue analogues, Li+ and Na+ rapidly migrate within the host framework as their potential barrier (Δ) is lower than or comparable to the thermal energy (Figure 3). This is the reason why the Prussian blue analogues work as the active material in Li+ and Na+ secondary batteries.On the other hand, the migration of K+ and Rb+ is impossible as Δ is much higher than the thermal energy. Actually, Moritomo et al. [23] reported that K+ and Rb+ cannot intercalate into the AxCo[Fe(CN)6]0.902.9H2O film from aqueous solution, whereas Na+ can intercalate into the film. Of course, the alkali cation intercalation process is mainly governed by the transfer process from the electrolyte to the host framework. Nevertheless, the migration process plays a significant role even in the following case. They investigated the effect of the dipping of the film into an aqueous solution containing K+ or Rb+ and found that the procedure blocks the intercalation of Na+. This behavior is explained by the clogging of the cation routes at the surface region, as discussed in the next section.


## 3.1. Experiment

Thin films of Li0.68Na0.04Ni[Fe(CN)6]0.68·5.1H2O (M = Ni), Li0.71Na0.13Co[Fe(CN)6]0.71·3.8H2O (M = Co), Li1.24Mn[Fe(CN)6]0.81·3.0H2O (M = Mn), and Li0.96Na0.88Cd[Fe(CN)6]0.96·4.8H2O (M = Cd) were synthesized by electrochemical deposition of the Na compounds on an indium tin oxide (ITO) transparent electrode and subsequent electrochemical substitution of Li+ for Na+. In the M = Ni, Co, and Cd compounds, [5] only the Fe site exhibits the redox reaction (Fe2+⟷ Fe3+), and, hence, a part of the Na sites is replaced by Li+. By contrast, two-electron reaction (Fe2+⟷ Fe3+ and Mn2+⟷ Mn3+) takes place in the M = Mn compound [5, 6]. As a result, all the Na sites can be replaced by Li+. Chemical compositions of the films were determined by the inductively coupled plasma (ICP) method and CHN organic elementary analysis (Perkin-Elmer 2400 CHN Elemental Analyzer). Details of the synthesis and characterization are described elsewhere [5].The charge/discharge properties of the thin films were measured against Li in a beaker-type cell. The electrolyte was ethylene carbonate (EC)/diethyl carbonate (DEC) solution containing 1 mol/L LiClO4. The cutoff voltage was from 2.0 to 4.2 V. The thickness and active areas of the films were ~1 μm and 1-2 cm2, respectively. The mass of each film was measured with a conventional electronic weighing machine after the film was carefully removed from the substrate with a microspatula. The experimental error of the mass is 10%. The current density was set to be the same for the charge/discharge process.


## 3.2. Results

Figure5 shows the charge/discharge curves of thin-film electrodes at various rates (v). The discharge capacities at low v (=0.1–1 C) coincides with the ideal value within the experimental error (~10%). In all the compounds, the discharge curves show plateaus at ~3.4 V. This plateau is ascribed to the reduction process at the Fe site (Fe3+ → Fe2+) [5]. The plateau structure is discernible even at high v (<30 C). The capacities at 100 C are 0.66 (M = Ni), 0.31 (Co), 0.62 (Mn), and 0.74 (Cd) of those at 1 C.Charge/discharge curve of thin-film electrodes of (a) Li0.68Na0.04Ni[Fe(CN)6]0.68·5.1H2O, (b) Li0.71Na0.13Co[Fe(CN)6]0.71·3.8H2O, (c) Li1.24Mn[Fe(CN)6]0.81·3.0H2O, and (d) Li0.96Na0.88Cd[Fe(CN)6]0.96·4.8H2O against Li at various rate (v). The discharge curve at v was measured after the charge process at v.
(a)
M
=
Ni
(b)
M
=
Co
(c)
M
=
Mn
(d)
M
=
CdThe Mn compound (Figure5(c)) shows rather complicated behaviors. In the discharge curve, two additional plateaus are observed at 3.8 V and 3.6 V. These plateaus are probably ascribed to the reduction process at the Mn site (Mn3+ → Mn2+) [5, 6]. The oxidization (charge) process of the Mn compound is as follows. At the initial stage (Li1.24Mn2+[Fe2+(CN)6]0.81·3.0H2O), the valence state is Mn2+ and Fe2+. In the first plateau at 3.4 V, the Fe site is selectively oxidized to become Li0.44Mn2+ [Fe3+(CN)6]0.81·3.0H2O. In the second plateau at 3.8 V, parts of the Mn sites are oxidized to become Mn2.44+ [Fe3+(CN)6]0.81·3.0H2O. Recently, Matsuda and Moritomo [28] found that thin film of Na1.32Mn[Fe(CN)6]0.83·3.5H2O exhibits a high capacity of 114 mAh/g and an average operating voltage of 3.3 V against Na with a good cyclability. The electrolyte was propylene carbonate (PC) solution containing 1 mol/L NaClO4. Thus, the Mn compound exhibits reversible intercalation/deintercalation of Li+ and Na+ in organic solvent.


## 3.3. Interrelation with the Alkali Cation Potential

Generally speaking, the alkali cation intercalation process in the Li+ and Na+ secondary batteries can be divided into the transfer process from the electrolyte to host framework and the migration process within the host framework. The former process usually accompanies the desolvation process and is complicated. In the latter process, the bare cation migrates toward the collective electrode with feeling the alkali cation potential. The latter process is essential for the capacity and rate properties of the active material. In the Prussian blue analogues, Li+ and Na+ rapidly migrate within the host framework as their potential barrier (Δ) is lower than or comparable to the thermal energy (Figure 3). This is the reason why the Prussian blue analogues work as the active material in Li+ and Na+ secondary batteries.On the other hand, the migration of K+ and Rb+ is impossible as Δ is much higher than the thermal energy. Actually, Moritomo et al. [23] reported that K+ and Rb+ cannot intercalate into the AxCo[Fe(CN)6]0.902.9H2O film from aqueous solution, whereas Na+ can intercalate into the film. Of course, the alkali cation intercalation process is mainly governed by the transfer process from the electrolyte to the host framework. Nevertheless, the migration process plays a significant role even in the following case. They investigated the effect of the dipping of the film into an aqueous solution containing K+ or Rb+ and found that the procedure blocks the intercalation of Na+. This behavior is explained by the clogging of the cation routes at the surface region, as discussed in the next section.


## 4. Electrochromism Mediated by Na+ Transfer in All Solid Device

### 4.1. Experiment

Thin films of Na0.72Ni[Fe(CN)6]0.68·5.1H2O and Na0.79Co[Fe(CN)6]0.90·2.9H2O were synthesized by electrochemical deposition on an ITO transparent electrode and subsequent electrochemical treatment. The electrolyte was aqueous solution containing of 1 mol/L NaCl. The Ni-Fe film was transparent, while the Co-Fe film was dark purple. Chemical compositions of the films were determined by the ICP method and CNH organic elementary analysis (Perkin-Elmer 2400 CHN Elemental Analyzer). Details of the synthesis procedure and characterization were described in the literatures [12, 13].The all-solid electrochromic device [14, 15] was made by connecting the surfaces of the Na0.72Ni[Fe(CN)6]0:68·5.1H2O (560 nm) and Na0.79Co[Fe(CN)6]0:90·2.9H2O (320 nm) films without any electrolytes. The thickness of the films was determined by the cross-sectional scanning electron micrographs. The scanning probe microscope (SEM) images indicate that the Ni-Fe film consists of spherical grains, ~50 nm in diameter, whereas the Co-Fe film consists of pyramidal grains, 100 × 100 nm2 in area. The compositions after the short circuit are Na0.46Ni[Fe(CN)6]0:68·5.1H2O and Na1.03Co[Fe(CN)6]0:90·2.9H2O, respectively. The Na+ concentrations were estimated by IR spectra. Thus, the short circuit of the device induces the Na+ transfer between the films. Before each measurement, the device was short circuited for several minutes.


### 4.2. Results

Figure6(a) shows the I-t curves of the device under periodic rectangular voltage on the M = Ni side. The compositions after the short circuit are Na0.46Ni[Fe(CN)6]0:68·5.1H2O and Na1.03Co[Fe(CN)6]0:90·2.9H2O, respectively. At 0.6 V, the magnitude of the positive current gradually decreases with t. The 0.6 V voltage changes the compositions into Na0.31Ni[Fe(CN)6]0:68·5.1H2O and Na1.53Co[Fe(CN)6]0:90·2.9H2O, respectively. The Ni-Fe film becomes dense yellow, while the Co-Fe film becomes more transparent. These color changes is ascribed to the valence change of the constituent transition metals. We note that the total current flow (=0.16 e/Ni site) in this process is comparable to the Na+ transfer (=0.15) of the Ni-Fe film. Reversely, the application of −0.6 V on the Ni-Fe side induces negative current. The −0.6 V voltage changes the compositions into Na0.62Ni[Fe(CN)6]0:68·5.1H2O and Na0.81Co[Fe(CN)6]0:90·2.9H2O, respectively. The Ni-Fe film becomes transparent, while the Co-Fe film becomes dark purple. We confirmed that the electrochromism is reversible for the periodic rectangular voltage by more than 100 cycles.(a) Current density (I) of ITO/Na0.72Ni[Fe(CN)6]0 : 68·5.1H2O (560 nm)/Na0.79Co[Fe(CN)6]0:90·2.9H2O (320 nm)/ITO device against time (t) under periodic rectangular voltage (V) on the M = Ni side. (b) I-t curves at 0.6 V of the device before and after the K+-treatment.
(a)
ITO/Ni-Fe/Co-Fe/ITO
(b)Figure6(b) shows the I-t curves of the device at +0.6 V on the M = Ni side before and after dipping the films in an aqueous solution containing K+ (K+-treatment) Before the K+ treatment, the magnitude of I rapidly decreases and eventually becomes nearly zero at ~10 s. This clearly indicates that the device is not a resistor and the electrons cannot pass through the cyanide/cyanide interface. In other words, the Na+ transfer between the films is a necessary condition for the current flow. The K+ treatment significantly suppresses the magnitude of I, indicating that the treatment blocks the Na+ transfer between the films.


### 4.3. Interrelation with the Alkali Cation Potential

The alkali cation intercalation of the present device is governed by the migration process within the host framework because the device has no electrolyte region. In the Prussian blue analogues, Na+ rapidly migrates is within the host framework as Δ is lower than or comparable to the thermal energy (Figure 3). This is the reason why the device made by the Prussian blue analogues exhibits a rapid electrochromism.On the other hand, the migration of K+ is impossible as Δ is much higher than the thermal energy. At the K+ treatment, a part of Na+ in the surface region is exchanged for the larger K+. K+ cannot migrate into the inner part of the host framework or clogs the cation routes at the surface region. The clogged K+ further blocks the intercalation of the smaller Na+. This mechanism explains well why the K+ treatment significantly suppresses the Na+ transfer between the films.


## 4.1. Experiment

Thin films of Na0.72Ni[Fe(CN)6]0.68·5.1H2O and Na0.79Co[Fe(CN)6]0.90·2.9H2O were synthesized by electrochemical deposition on an ITO transparent electrode and subsequent electrochemical treatment. The electrolyte was aqueous solution containing of 1 mol/L NaCl. The Ni-Fe film was transparent, while the Co-Fe film was dark purple. Chemical compositions of the films were determined by the ICP method and CNH organic elementary analysis (Perkin-Elmer 2400 CHN Elemental Analyzer). Details of the synthesis procedure and characterization were described in the literatures [12, 13].The all-solid electrochromic device [14, 15] was made by connecting the surfaces of the Na0.72Ni[Fe(CN)6]0:68·5.1H2O (560 nm) and Na0.79Co[Fe(CN)6]0:90·2.9H2O (320 nm) films without any electrolytes. The thickness of the films was determined by the cross-sectional scanning electron micrographs. The scanning probe microscope (SEM) images indicate that the Ni-Fe film consists of spherical grains, ~50 nm in diameter, whereas the Co-Fe film consists of pyramidal grains, 100 × 100 nm2 in area. The compositions after the short circuit are Na0.46Ni[Fe(CN)6]0:68·5.1H2O and Na1.03Co[Fe(CN)6]0:90·2.9H2O, respectively. The Na+ concentrations were estimated by IR spectra. Thus, the short circuit of the device induces the Na+ transfer between the films. Before each measurement, the device was short circuited for several minutes.


## 4.2. Results

Figure6(a) shows the I-t curves of the device under periodic rectangular voltage on the M = Ni side. The compositions after the short circuit are Na0.46Ni[Fe(CN)6]0:68·5.1H2O and Na1.03Co[Fe(CN)6]0:90·2.9H2O, respectively. At 0.6 V, the magnitude of the positive current gradually decreases with t. The 0.6 V voltage changes the compositions into Na0.31Ni[Fe(CN)6]0:68·5.1H2O and Na1.53Co[Fe(CN)6]0:90·2.9H2O, respectively. The Ni-Fe film becomes dense yellow, while the Co-Fe film becomes more transparent. These color changes is ascribed to the valence change of the constituent transition metals. We note that the total current flow (=0.16 e/Ni site) in this process is comparable to the Na+ transfer (=0.15) of the Ni-Fe film. Reversely, the application of −0.6 V on the Ni-Fe side induces negative current. The −0.6 V voltage changes the compositions into Na0.62Ni[Fe(CN)6]0:68·5.1H2O and Na0.81Co[Fe(CN)6]0:90·2.9H2O, respectively. The Ni-Fe film becomes transparent, while the Co-Fe film becomes dark purple. We confirmed that the electrochromism is reversible for the periodic rectangular voltage by more than 100 cycles.(a) Current density (I) of ITO/Na0.72Ni[Fe(CN)6]0 : 68·5.1H2O (560 nm)/Na0.79Co[Fe(CN)6]0:90·2.9H2O (320 nm)/ITO device against time (t) under periodic rectangular voltage (V) on the M = Ni side. (b) I-t curves at 0.6 V of the device before and after the K+-treatment.
(a)
ITO/Ni-Fe/Co-Fe/ITO
(b)Figure6(b) shows the I-t curves of the device at +0.6 V on the M = Ni side before and after dipping the films in an aqueous solution containing K+ (K+-treatment) Before the K+ treatment, the magnitude of I rapidly decreases and eventually becomes nearly zero at ~10 s. This clearly indicates that the device is not a resistor and the electrons cannot pass through the cyanide/cyanide interface. In other words, the Na+ transfer between the films is a necessary condition for the current flow. The K+ treatment significantly suppresses the magnitude of I, indicating that the treatment blocks the Na+ transfer between the films.


## 4.3. Interrelation with the Alkali Cation Potential

The alkali cation intercalation of the present device is governed by the migration process within the host framework because the device has no electrolyte region. In the Prussian blue analogues, Na+ rapidly migrates is within the host framework as Δ is lower than or comparable to the thermal energy (Figure 3). This is the reason why the device made by the Prussian blue analogues exhibits a rapid electrochromism.On the other hand, the migration of K+ is impossible as Δ is much higher than the thermal energy. At the K+ treatment, a part of Na+ in the surface region is exchanged for the larger K+. K+ cannot migrate into the inner part of the host framework or clogs the cation routes at the surface region. The clogged K+ further blocks the intercalation of the smaller Na+. This mechanism explains well why the K+ treatment significantly suppresses the Na+ transfer between the films.


## 5. Elimination of Cs+ from Aqueous Solution by Precipitation

### 5.1. Experiment

The Cs+ elimination performance from the aqueous solution was investigated for manganese and cobalt ferricyanides by the precipitation method [17]. We investigated the Cs+ concentrations in aqueous solution before and after the precipitation treatment. In the high concentration region (>1 ppm), a Cs standard aqueous solution (1000 ppm Cs+ in 0.5 mol/L HNO3) was used as the Cs source, and the Cs+ concentrations were determined by mass spectroscopy inductively coupled plasma (MS-ICP) method. In the low concentration region (≪1 ppm), the radioactive 137Cs+ was used as the Cs source, and the Cs+ concentrations were determined by the radioactivity of the solution.The precipitation treatment was schematically shown in Figure7. Ci. and Cf are the initial and final Cs+ concentrations, respectively. First, 5 mmol/L MnIICl2 (CoIICl2a) and 5 mmol/L mmol/L K3[FeIII(CN)6] were added to the aqueous solution. Then, the solution was mixed, agitated for 5 min, and ultrasonicated for 5 min. The precipitates in the solution were separated and collected with a cyclotron separator. Cf was determined after the percolation treatment of the solution with a 0.2 μm polytetrafluoroethylene (PTFE) filter.Figure 7
Schematic illustration of precipitation treatment. 5 mmol/LMIICl2 (M = Co and Mn) and 5 mmol/L mmol/L K3[FeIII(CN)6] were added to the aqueous solution, and, then, the precipitates were removed. Ci. and Cf are the initial and final Cs+ concentrations, respectively.


### 5.2. Results and Discussion

Figure8 shows the Cs concentration before (filled circles) and after (open circles) the precipitation treatment. In the manganese ferricyanide (open circles), the simple precipitation procedure eliminates Cs+ from the aqueous solution by 4 or 5 orders. We emphasize that the manganese ferricyanide exhibits an excellent performance even at low Cs+ concentration in the ppt (=10−6 ppm) region.Figure 8
Cs+ concentration before (filled circles) and after (open symbols) the precipitation treatment with 5 mmol/L K3[FeIII(CN)6] and 5 mmol/L MnIICl2. (CoIICl2). Open circle and squares are for manganese and cobalt ferricyanides, respectively.We investigated the structure and the grain size of the precipitates from 5 mmol/L K3[FeIII(CN)6] and 5 mmol/L MnIICl2. The X-ray powder diffraction patterns were obtained at BL02B2 beamline [29] at SPring-8. The X-ray powder diffraction patterns revealed that the precipitates belong to the face-centered cubic. The lattice constants (a) are distributed from 1.056 to 1.060 nm, which are close to the value (=1.05561 nm [22]) of Na1.32Mn[Fe(CN)6]0.83·3.6H2O. This observation suggests that the precipitates are manganese ferricyanide, CsxMn[Fe(CN)6]y. We further estimated the domain size (~300 nm) by Scherrer’s equation. Thus, manganese ferricyanide imprisons Cs+ into large domain (~300 nm) and, hence, can isolate them from the environment for a long time.


### 5.3. Interrelation with the Alkali Cation Potential

First, let us investigate the Cs+ site by the Rietveld analysis (Rietan-FP [30]) of the precipitates from the 100 ppm Cs+ solution. We neglect H+ in the structural analysis. We refined the occupancies (g) of Cs, Fe(CN)6, and Oz. The obtained parameters were listed in Table 3. The estimated oxygen concentration (z=2.9) is reasonable. We found that 85% of the nanocubes were occupied by Oz. The residual rooms are comparable to the Cs concentration (=15%). This structural analysis indicates that the Cs+ is trapped at the nanocube center of the host framework.Table 3
Structural parameters of Cs0.31Mn[Fe(CN)6]0.79·2.9H2O obtained the Rietveld analysis with the (Fm3_m; Z = 4) model. The reliable parameters were Rwp=6.4%, RI=8.0%, and S=2.29. The lattice constant is a=1.06057(2) nm. Ol and Oz are ligand and zeolite oxygens, respectively.
Atom
Site
g
x
y
z
B (A2)
Cs
8c
0.155(2)
1/4
1/4
1/4
2.33(5)
Fe
4a
0.79(1)
0
0
0
2.33
Mn
4b
1
1/2
1/2
1/2
2.33
C
24e
0.79
0.201(1)
0
0
4.47(17)
N
24e
0.79
0.304(1)
0
0
4.47
Ol
24e
0.21
0.201
0
0
4.47
Oz
32f
0.200(4)
0.2
0.2
0.2
4.47The Cs+ capture process within the host framework is inseparable with the crystallization process from the aqueous solution of Cs+, [FeIII(CN)6]3−, and MnII. In this sense, the Cs+ capture performance is determined by the crystallization energy or, more precisely, the energy difference between CsMnII[FeIII(CN)6] and MnII[FeIII(CN)6]2/3 + Cs+ + 1/3[FeIII(CN)6]3−. What we can say from the alkali cation potential (Figure 3) is that the captured Cs+ is hard to escape from the nanocube due to the high-Δ at the surrounding windows. This partly explains the excellent performance of manganese ferricyanide.Here, let us crudely discuss the interrelation between Δ and the crystallization energy. Roughly speaking, the magnitude of Δ is a measure of the short-range atomic repulsive interaction between Cs+ and the host framework. Then, the smaller Δ becomes, the larger the crystallization gain by the Cs+ capture becomes. Δ of the Mn (a=1.05561 nm) compound is ~1 eV smaller than that of the Co (a=0.93440 nm) compound (see Figure 4). This trend is consistent with the higher performance in MnII-[FeIII(CN)6] as compared with CoII-[FeIII(CN)6] (see Figure 8). In addition, Omura and Moritomo [17] systematically investigated the Cs+ capture performance in MII-[FeIII(CN)6] (M = Fe, Ni, Cu, Zn, Co, and Mn) and found a positive correlation with the ionic radium (rM) of MII. This positive correlation is also interpreted in terms of the crystallization gain by the Cs+ capture.


## 5.1. Experiment

The Cs+ elimination performance from the aqueous solution was investigated for manganese and cobalt ferricyanides by the precipitation method [17]. We investigated the Cs+ concentrations in aqueous solution before and after the precipitation treatment. In the high concentration region (>1 ppm), a Cs standard aqueous solution (1000 ppm Cs+ in 0.5 mol/L HNO3) was used as the Cs source, and the Cs+ concentrations were determined by mass spectroscopy inductively coupled plasma (MS-ICP) method. In the low concentration region (≪1 ppm), the radioactive 137Cs+ was used as the Cs source, and the Cs+ concentrations were determined by the radioactivity of the solution.The precipitation treatment was schematically shown in Figure7. Ci. and Cf are the initial and final Cs+ concentrations, respectively. First, 5 mmol/L MnIICl2 (CoIICl2a) and 5 mmol/L mmol/L K3[FeIII(CN)6] were added to the aqueous solution. Then, the solution was mixed, agitated for 5 min, and ultrasonicated for 5 min. The precipitates in the solution were separated and collected with a cyclotron separator. Cf was determined after the percolation treatment of the solution with a 0.2 μm polytetrafluoroethylene (PTFE) filter.Figure 7
Schematic illustration of precipitation treatment. 5 mmol/LMIICl2 (M = Co and Mn) and 5 mmol/L mmol/L K3[FeIII(CN)6] were added to the aqueous solution, and, then, the precipitates were removed. Ci. and Cf are the initial and final Cs+ concentrations, respectively.


## 5.2. Results and Discussion

Figure8 shows the Cs concentration before (filled circles) and after (open circles) the precipitation treatment. In the manganese ferricyanide (open circles), the simple precipitation procedure eliminates Cs+ from the aqueous solution by 4 or 5 orders. We emphasize that the manganese ferricyanide exhibits an excellent performance even at low Cs+ concentration in the ppt (=10−6 ppm) region.Figure 8
Cs+ concentration before (filled circles) and after (open symbols) the precipitation treatment with 5 mmol/L K3[FeIII(CN)6] and 5 mmol/L MnIICl2. (CoIICl2). Open circle and squares are for manganese and cobalt ferricyanides, respectively.We investigated the structure and the grain size of the precipitates from 5 mmol/L K3[FeIII(CN)6] and 5 mmol/L MnIICl2. The X-ray powder diffraction patterns were obtained at BL02B2 beamline [29] at SPring-8. The X-ray powder diffraction patterns revealed that the precipitates belong to the face-centered cubic. The lattice constants (a) are distributed from 1.056 to 1.060 nm, which are close to the value (=1.05561 nm [22]) of Na1.32Mn[Fe(CN)6]0.83·3.6H2O. This observation suggests that the precipitates are manganese ferricyanide, CsxMn[Fe(CN)6]y. We further estimated the domain size (~300 nm) by Scherrer’s equation. Thus, manganese ferricyanide imprisons Cs+ into large domain (~300 nm) and, hence, can isolate them from the environment for a long time.


## 5.3. Interrelation with the Alkali Cation Potential

First, let us investigate the Cs+ site by the Rietveld analysis (Rietan-FP [30]) of the precipitates from the 100 ppm Cs+ solution. We neglect H+ in the structural analysis. We refined the occupancies (g) of Cs, Fe(CN)6, and Oz. The obtained parameters were listed in Table 3. The estimated oxygen concentration (z=2.9) is reasonable. We found that 85% of the nanocubes were occupied by Oz. The residual rooms are comparable to the Cs concentration (=15%). This structural analysis indicates that the Cs+ is trapped at the nanocube center of the host framework.Table 3
Structural parameters of Cs0.31Mn[Fe(CN)6]0.79·2.9H2O obtained the Rietveld analysis with the (Fm3_m; Z = 4) model. The reliable parameters were Rwp=6.4%, RI=8.0%, and S=2.29. The lattice constant is a=1.06057(2) nm. Ol and Oz are ligand and zeolite oxygens, respectively.
Atom
Site
g
x
y
z
B (A2)
Cs
8c
0.155(2)
1/4
1/4
1/4
2.33(5)
Fe
4a
0.79(1)
0
0
0
2.33
Mn
4b
1
1/2
1/2
1/2
2.33
C
24e
0.79
0.201(1)
0
0
4.47(17)
N
24e
0.79
0.304(1)
0
0
4.47
Ol
24e
0.21
0.201
0
0
4.47
Oz
32f
0.200(4)
0.2
0.2
0.2
4.47The Cs+ capture process within the host framework is inseparable with the crystallization process from the aqueous solution of Cs+, [FeIII(CN)6]3−, and MnII. In this sense, the Cs+ capture performance is determined by the crystallization energy or, more precisely, the energy difference between CsMnII[FeIII(CN)6] and MnII[FeIII(CN)6]2/3 + Cs+ + 1/3[FeIII(CN)6]3−. What we can say from the alkali cation potential (Figure 3) is that the captured Cs+ is hard to escape from the nanocube due to the high-Δ at the surrounding windows. This partly explains the excellent performance of manganese ferricyanide.Here, let us crudely discuss the interrelation between Δ and the crystallization energy. Roughly speaking, the magnitude of Δ is a measure of the short-range atomic repulsive interaction between Cs+ and the host framework. Then, the smaller Δ becomes, the larger the crystallization gain by the Cs+ capture becomes. Δ of the Mn (a=1.05561 nm) compound is ~1 eV smaller than that of the Co (a=0.93440 nm) compound (see Figure 4). This trend is consistent with the higher performance in MnII-[FeIII(CN)6] as compared with CoII-[FeIII(CN)6] (see Figure 8). In addition, Omura and Moritomo [17] systematically investigated the Cs+ capture performance in MII-[FeIII(CN)6] (M = Fe, Ni, Cu, Zn, Co, and Mn) and found a positive correlation with the ionic radium (rM) of MII. This positive correlation is also interpreted in terms of the crystallization gain by the Cs+ capture.


## 6. Summary

We performed anab initiototal energy calculation to derive the alkali cation potential in the Prussian blue analogues, AxM[Fe(CN)6]yzH2O (A = Li, Na, K, Rb, and Cs; M = Co, Ni, Mn, and Cd). We discussed the interrelation between the alkali cation potential and the functionalities observed in the Prussian blue analogues, that is, (a) battery properties mediated by Li+ intercalation/deintercalation, (b) electrochromism mediated by Na+ transfer in all solid device, and (c) elimination of Cs+ from aqueous solution by precipitation.



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*Source: 539620-2013-03-20.xml*