Ines Ennajeh*a,
Samuel Georgesb,
Youssef Ben Smidaa,
Abderrahmen Guesmiac,
Mohamed Faouzi Zida and
Habib Boughazalaa
aUniversité de Tunis El Manar, Laboratoire de Matériaux et Cristallochimie, Faculté des Sciences, El Manar II, 2092, Tunis, Tunisia. E-mail: inesnajeh@gmail.com
bLaboratoire d'Electrochimie et de Physicochimie des Matériaux et des Interfaces LEPMI, UMR 5279, CNRS: Grenoble INP, Université de Savoie, Université Joseph Fourier, BP75, 38402 Saint Martin d'Hères, France
cUniversité de Tunis El Manar, Institut Préparatoire aux Etudes d'Ingénieurs d'El Manar, El Manar II, 2092 Tunis, Tunisia
First published on 22nd April 2015
A new triple molybdate K0.13Na3.87MgMo3O12 was synthesized by solid state reaction. The crystal structure has been determined by single X-ray diffraction and the electrical conductivity measured by impedance spectroscopy. The title compound crystallizes in the monoclinic space group C2/c with a = 12.9325 (8) Å, b = 13.5537 (9) Å, c = 7.1627 (6) Å, β = 112.212 (9)°, V = 1162.33 (14) Å3 and Z = 4. The final agreement factors are R = 0.0241, wR (F2) = 0.0584, S(F2) = 1.22. The magnesium–molybdate 3D-framework belongs to the alluaudite type. The structure is formed by infinite chains composed of edge-sharing (Mg/Na)2O10 dimmers, which are linked together via bridging MoO4 tetrahedra, yielding to a three-dimensional framework enclosing two distinct types of hexagonal tunnels in which Na+ and K+ cations reside. The structural model is validated by bond valence sum (BVS) and charge distribution (CD) methods. Ball milling is used as mechanical means to reduce the particles sizes of the synthesized powder. At the optimal sintering temperature of 650 °C, a relative density of 81% was obtained. The microstructures were characterized by scanning electron microscopy. The compound undergoes a phase transformation at 528 °C accompanied by an abrupt increase of the electrical conductivity. Above this phase transition, the electrical conductivity reaches 10−2 S cm−1. Thus K0.13Na3.87Mg(MoO4)3 may be considered as a promising compound for developing new materials with high ionic conductivity.
In this work, we report the synthesis, structure and ionic conductivity of a new triple molybdate K0.13Na3.87Mg(MoO4)3 with an alluaudite-type structure. The structural study showed that the title compound presents a three-dimensional framework with large hexagonal tunnels containing the alkaline cations. The proposed structural model based on a careful investigation of the single crystal X-ray diffraction data is supported by charge-distribution (CHARDI) analysis and bond-valence-sum (BVS) calculations. The correlation between the X-ray refinement and the validation results is discussed. The thermal stability of the molybdate was investigated. The electrical properties of the ceramics shaped from the powders have been studied using complex impedance spectroscopy. Correlation attempts between the electrical behaviour and the microstructure of the samples were made.
Relative densities were calculated from accurate measurements of the pellet size and weight, with comparison to the theoretical density deduced from the crystal structure.
Crystal and X-ray analysis data of the title compound are summarized in Table 1. The atomic coordinates, equivalent isotropic displacement parameters and selected interatomic distances are listed in Tables 2 and 3. The structure graphics were drawn with diamond 2.1 supplied by Crystal Impact.20
Empirical formula | K0.13Na3.87Mg(MoO4)3 |
Formula weight (g mol−1) | 598.18 |
Crystal system, space group | Monoclinic, C2/c |
Unit cell dimensions (Å) | a = 12.9325 (8), b = 13.5537 (9), c = 7.1627 (6), β = 112.212 (9)° |
(Å3)/Z | 1162.33 (14)/4 |
Calculated density (g cm−3) | 3.418 |
Crystal size (mm) | 0.16 × 0.14 × 0.12 |
μ(MoKα) (mm−1) | 3.490 |
θ range (deg) for data collection | 2.3° ≤ θ ≤ 27° |
Miller index ranges | −16 ≤ h ≤ 16, −1 ≤ k ≤ 17, −9 ≤ l ≤ 9 |
Measured reflections | 2712 |
Independent reflections | 1261 (Rint = 0.0272) |
No. of variables | 97 |
R[F2 > 2σ(F2)] | 0.0241 |
wR(F2) | 0.0584 |
GooF = S | 1.23 |
Δρmax/Δρmin (e Å−3) | 0.81/−0.66 |
Atom | x | y | z | U*eq (Å) | Occ, (<1) |
---|---|---|---|---|---|
Mo1 | 0.0000 | 0.21604 (3) | 0.7500 | 0.01849 (13) | |
Mo2 | 0.23694 (3) | 0.60958 (2) | 0.12685 (5) | 0.02006 (11) | |
Mg1 | 0.21624 (11) | 0.34005 (10) | 0.12690 (19) | 0.0161 (3) | 0.50 |
Na1 | 0.21624 (11) | 0.34005 (10) | 0.12690 (19) | 0.0161 (3) | 0.50 |
Na2 | 0 | 0.23648 (18) | 0.25 | 0.0250 (5) | |
Na3 | 0.5 | 0.5 | 0.5 | 0.0412 (7) | |
Na4 | 0 | 0.4915 (2) | 0.75 | 0.0440 (11) | 0.87 |
K1 | 0 | 0.4915 (2) | 0.75 | 0.0440 (11) | 0.13 |
O1 | 0.6702 (3) | 0.0051 (3) | 0.6099 (5) | 0.0434 (9) | |
O2 | 0.3951 (3) | 0.3654 (2) | 0.2540 (5) | 0.0387 (8) | |
O3 | 0.3789 (3) | 0.5894 (2) | 0.1839 (5) | 0.0306 (7) | |
O4 | 0.4566 (3) | 0.7802 (2) | 0.5302 (4) | 0.0265 (6) | |
O5 | 0.3261 (3) | 0.8305 (2) | 0.1080 (4) | 0.0314 (7) | |
O6 | 0.2769 (3) | 0.8203 (3) | 0.6735 (4) | 0.0326 (7) |
Mo1O4 | Mo2O4 | Mg1O6 | |||
---|---|---|---|---|---|
Mo1–O2i | 1.758 (3) | Mo2–O3 | 1.745 (3) | Na3–O3 | 2.523 (3) |
Mo1–O2ii | 1.758 (3) | Mo2–O1v | 1.759 (3) | Na3–O3xi | 2.523 (3) |
Mo1–O4iii | 1.771 (3) | Mo2–O5vi | 1.765 (3) | Na3–O2xi | 2.543 (3) |
Mo1–O4iv | 1.771 (3) | Mo2–O6vii | 1.781 (3) | Na3–O2 | 2.543 (4) |
Na3–O3xii | 2.686 (4) | ||||
Na3–O3xiii | 2.686 (4) |
Na3O6 | Na2O6 | K1O8 | |||
---|---|---|---|---|---|
Na3–O3 | 2.523 (3) | Na2–O4iv | 2.393 (3) | K1–O1i | 2.684 (4) |
Na3–O3xi | 2.523 (3) | Na2–O4xv | 2.393 (3) | K1–O1ii | 2.684 (4) |
Na3–O2xi | 2.543 (3) | Na2–O5xv | 2.447 (3) | K1–O1xiv | 2.749 (4) |
Na3–O2 | 2.543 (4) | Na2–O5iv | 2.447 (3) | K1–O1xv | 2.749 (4) |
Na3–O3xii | 2.686 (4) | Na2–O3iv | 2.468 (4) | K1–O4iv | 3.093 (4) |
Na3–O3xiii | 2.686 (4) | Na2–O3x | 2.468 (4) | K1–O4iii | 3.093 (4) |
K1–O5iviii | 3.192 (4) | ||||
K1–O5xvi | 3.192 (4) |
The structural model is validated by the two structural tools, Bond Valence Sum BVS21,22 and Charge Distribution analysis CD.23–25
Both BVS and CD show adequate valences (V) and charges (Q) of all the cation sites. The structural model is thus validated, as shown by the dispersion factor of 3.1% which measures the deviation of the computed charges (Q) with respect to the formal oxidation numbers. The Bond Valence computation and Charge Distribution analysis are summarized in Table 4.
Cation | q(i)sof(i) | Q(i) | V(i) | CN(i) | ECoN(i) |
---|---|---|---|---|---|
Mo1 | 6 | 6.040 | 5.946 | 4 | 3.998 |
Mo2 | 6 | 5.987 | 5.913 | 4 | 3.992 |
Mg1 | 2 | 2.032 | 1.573 | 6 | 5.922 |
Na1 | 1 | 1.016 | 1.678 | 6 | 5.922 |
Na2 | 1 | 1.001 | 1.068 | 6 | 5.962 |
Na3 | 1 | 0.985 | 0.841 | 6 | 6.081 |
M1 | 1 | 0.951 | 0.645 | 8 | 6.212 |
Rietveld analysis was performed in the 10–70° range using the single crystal structure data (Fig. 2). In fact, the crystal data and the structure refinement details were obtained from Crystal X-ray diffraction, the purpose of the Rietveld refinement is only to show the purity of powder and to show that there are no other additional peaks due to the presence of impurity. The Rietveld refinement was carried out using Topas Academic software,26 allowed a Quantitative Phase Analysis (QPA) and led to a weight proportion of 100% of K0.13Na3.87Mg(MoO4)3. In addition, the background is linear: this is an indicator of the good crystallinity of the powder.
The final agreement factors are RB: 4.689%; Rexp: 0.9; Rexp: 8%; Rp: 4.64%; Rwp: 7.44%.
The asymmetric unit of K0.13Na3.87Mg(MoO4)3 (Fig. 3) consists of MgO6 octahedra, two MoO4 tetrahedra and four alkali cation sites ensuring the charge compensation.
The structure can be described as a three-dimensional framework composed of pairs of edge-sharing (Mg,Na)2O10 dimmers, linked via vestige to Mo2O4 tetrahedra to form polyhedral infinite layers parallel to the (100) plane (Fig. 4).
The junction between layers is ensured by Mo1O4 tetrahedra. The 3-D framework shows two kinds of hexagonal tunnels along the c direction in which site Na+ and K+ (Fig. 5).
Fig. 5 Projection of K0.13Na3.87Mg(MoO4)3 structure according to (001) direction, showing tunnels where monovalent cations are located. |
The Mo(1)O4 tetrahedron shares his four oxygen summits with four different Mg2O10 dimmers belonging to two adjacent layers. The Mo(2)O4 tetrahedron shares only three oxygen with three Mg2O10 units, the other one being free. The magnesium coordination has a very distorted octahedral geometry, as evidenced by the Mg–O bond distances which vary between 2.169 (4) and 2.292 (3) Å. The O–Mg–O bond angles vary between 82.60 (2)° and 174.75 (2)°. This distortion is probably due to the rigidity of [MoO4] units surrounding the Mg atom (Fig. 6).
The two types of hexagonal channels along [001] are shown in Fig. 7.
The largest distance in the tunnel (a) (about 5.844 Å) is more than twice of the radii of the ions, thus more favorable to cationic displacement. Second, larger tunnels (b), with bottleneck widths varying from 6.433 to 7.991 Å, were larger than twice of the radii of the ions (2 × (rNa+ + rO2−) = 2 × (1.02 + 1.35)) and thus more favourable to Na+ displacement. The framework of the title compound is thus of open character and the isotropic motion of cations through the tunnels seems to be feasible. This factor led us to study the ionic conduction.
Fig. 9 shows the evolution, versus milling time, of the relative density of the pellets obtained after sintering at 650 °C. The relative density reaches 81% of the theoretical density after 60 minutes of milling. There is no more significant increase of the density after additional milling sequences. Adding Small amounts of powders (CuO, ZnO, …) may improve the sintering process and increase the final relative density, but some complex mechanisms are usually observed and the best conductivity is not always obtained for the highest relative density.29 Accordingly and to limit the pollution contribution of the milling apparatus on the electrical properties, the sample with 81% of the theoretical density was selected for the electrical characterization.
Fig. 9 Evolution of the relative density of K0.13Na3.87Mg(MoO4)3 pellets sintered at 923 K as a function of the initial powder planetary ball milling time. |
The densification of the sample observed with the increased milling time is confirmed by the SEM micrographs, of the polished and thermally etched faces (50 °C below the sintering temperature) of K0.13Na3.87Mg(MoO4)3 pellets presented in Fig. 10.
Fig. 10 SEM micrographs of sintered K0.13Na3.87Mg(MoO4)3 pellets with different relative densities: (a) 73% and (b) 81%. |
In spite of a significant decrease of the mean grain size (approximately from 20 to 10 μm), a small increase of the relative density is obtained (8%). The geometric factor k of the obtained sample with 81% of relative density was 0.38 cm−1.
The complex impedance spectroscopy measurements were carried out with a frequency response analyzer (HP 4192A) from 5 Hz to 13 MHz with a signal amplitude of 0.05 V in air. The electrical measurements were made with the sample of 81% of the theoretical density in the temperature range 250–620 °C. Due to the relatively low density, the measured conductivity is only the lower limit of the intrinsic conductivity but the trend is certainly representative of the true behavior.
Fig. 11 show the Impedance spectra recorded at different temperatures after stabilization.
Fig. 11 Experimental and calculated impedance spectra of K0.13Na3.87Mg(MoO4)3 recorded at different temperatures. |
The semicircles were fitted using an equivalent electrical circuit composed of a resistor R, connected in parallel with a constant phase element, CPE. The CPE contribution is an empirical impedance function of the type:
(1) |
(2) |
ρ = R/k; ε0εR = Ck | (3) |
The refined parameters of R//CPE electrical models are given in Table 5 for different temperatures from 290 °C to 460 °C. At low temperature, highly depressed (±32°) and well defined semicircles are observed, indicating rather heterogeneous electrical properties. Given the porosity content (19%), one would expect in this high frequency contribution an interfacial part (grain boundaries or other microstructural effects). However, no reliable deconvolution can be obtained from the high frequency semicircle. Moreover, the capacitances obtained from the impedance spectra are in the range commonly observed for bulk ionic mobility. Without references values of Ck and ω0 (Table 5), we assume that this high frequency contribution is mainly due to the bulk ionic mobility, with probably a grain boundary part, as observed in other ionic conductors.30 At low temperature, the low frequency signals indicating electrochemical interfacial processes associated to the electrode contribution are not observed. The large inductive effect observed at high temperature is instrumental. It is almost constant in the measurement thermal range. It is negligible at low temperature when the resistance of the sample is high, and becomes prevalent at high temperature when the measured resistance is low (and capacity high), especially above the phase transition. This effect is well known for our measurement setup and is not a problem for the determination of the electrical parameters from the impedance spectra.31
T (°C) | ρ = R/k (104 Ω cm) ± 0.1 | Ck (10−12 F cm−1) ± 0.1 | β (°) ± 1 | ω0 (104 rad s−1) ± 0.1 | σ (10−7 S cm−1) ± 0.1 |
---|---|---|---|---|---|
290 | 402.8 | 12.6 | 31 | 2.1 | 2.4 |
320 | 173.9 | 11.4 | 32 | 5.0 | 5.7 |
350 | 69.4 | 10.3 | 33 | 14.1 | 14.4 |
390 | 18.7 | 8.96 | 34 | 62.5 | 53.4 |
420 | 7.4 | 7.84 | 36 | 182.8 | 135.1 |
460 | 2.2 | 6.74 | 38 | 741.5 | 454.5 |
Above 500 °C, the high frequency semicircles are no longer observed. The spectra consist in a strong inductive effect concealing the bulk polarisation. At high temperature, a low frequency contribution indicates the presence of exchanges with the gas phase, and then the existence of significant ionic conductivity in the ceramic. At 620 °C, a fit of the low frequency part of the impedance spectra (Fig. 11) to a R//CPE circuit gives C = 2.7 × 10−3 F, ω0 = 19 rad s−1. These values, typical for electrode reactions, provide a confirmation of the existence of ionic mobility.
Based on the structure analysis provided in this paper and on previous reports about neighbouring phases,32 the ionic conductivity observed in K0.13Na3.87MgMo3O12 is most probably due to monovalent Na+ and K+ cations anisotropic mobility.
The temperature dependence of the electrical conductivity of K0.13Na3.87Mg(MoO4)3 is shown in Fig. 12 in an Arrhenius plot. A high conductivity jump of about two orders of magnitude in the Arrhenius plot is observed above 528 °C. The transition temperature correlates with DTA data (Fig. 8). The peaks at 528 °C and 483 °C respectively on heating and cooling on the DTA curve were then attributed to an order/disorder type phase transition, accompanied with a strong increase of the ionic conductivity. This kind of conductivity increase in fast ionic conductors is usually attributed to a first-order superionic phase transition.33,34 Below and above the transition temperature, linear evolutions are observed with activation energies of 1 and 0.7 eV respectively. These values are compatible with cationic conductivity mechanisms.31
Fig. 12 Arrhenius plots of conductivity of K0.13Na3.87Mg(MoO4)3 and differential thermal Analysis (DTA) curve. |
At 580 °C, the conductivity was found to be 3.8 × 10−2 S cm−1. Typical conductivity values of molybdates reach 10−4 S cm−1.35–37 Among this family of materials, the experimental values obtained for K0.13Na3.87Mg(MoO4)3 are high. They are comparable to that conductivity of superionic conductors.38,39 The title compound K0.13Na3.87Mg(MoO4)3 can be considered as a promising solid electrolyte due to the observed high conductivity.
Footnote |
† CCDC 1045308. For crystallographic data in CIF or other electronic format see DOI: 10.1039/c5ra02276b |
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