Research Article | Open Access
Tatiana M. Savankova, Lev G. Akselrud, Lyudmyla I. Ardanova, Alexey V. Ignatov, Eugeni I. Get’man, Roman E. Gladyshevskii, Stanislav N. Loboda, "Synthesis, Crystal Structure Refinement, and Electrical Conductivity of Pb(8−x)Na2Smx(VO4)6O(x/2)", Journal of Chemistry, vol. 2014, Article ID 263548, 7 pages, 2014. https://doi.org/10.1155/2014/263548
Synthesis, Crystal Structure Refinement, and Electrical Conductivity of Pb(8−x)Na2Smx(VO4)6O(x/2)
Solid solutions of Pb(8−x)Na2Smx(VO4)6O(x/2) were studied using X-ray diffraction analysis including Rietveld refinement and scanning electron microscopy and by measuring their electrical conductivity. Crystal structure of the solid solutions was refined and the solubility region was determined for samarium substitution for lead under the scheme . The influence of degree of substitution on the electrical conductivity of solid solutions was established.
Compounds with the apatite-type structure M10(ZO4)6X2 (where M = Na+, K+,Ca2+, Sr2+, Ba2+, Pb2+, Cd2+, Eu3+,Y3+, La3, etc.; Z = Si4+, Ge4+, P5+, V5+, As5+, S6+, Cr6+, etc.; X = OH−, F−, Cl−, Br−, I−, O2−, vacancy, etc.) are characterized by different properties and may be used as bioactive, laser and luminescent materials, sensors, solid electrolytes, adsorbents, and catalysts [1–4], among other uses. The apatite structure features two structurally nonequivalent positions M(1) and M(2), present in a ratio of 4 : 6 in the formula unit. The M(1) position (4f position) is surrounded by nine oxygen atoms of VO4 tetrahedra. The position of M(2) (6h position) is surrounded by six oxygen atoms of VO4 tetrahedra and one atom X (2a position) located in the channel of the structure. The central axis of triangles formed by ions in position M(2) coincides with axis. Repetition of this structure along the axis results in formation of channels, along which anions (X) can be located .
This structure makes isomorphous substitutions possible by different elements in different sites. Formation of solid solutions changes not only the nature of chemical bonding and interatomic distances but the physical and chemical properties of the substances as well. Accordingly, the synthesis and study of solid solutions with the apatite structure are a way to produce new functional materials with improved physical and chemical characteristics and to address one of the fundamental problems of modern chemistry, that of establishing the correlation between composition, structure, and property.
Substitutions of rare earth elements for alkaline earth elements in compounds with apatite structure have been well-studied (e.g., [6–8]). However, despite the fact that the value of ionic radius of lead is close to the radii of alkaline earth ions, there is no information about the substitution of rare earth elements for lead in the systems Pb(10−x)Lnx(ZO4)6(OH)(2−x)Ox in the literature. Possibly, this is due to the presence of the stereochemically active lone electron pairs on lead atoms, which prevent substitution under the scheme Pb2+ + OH−→ Ln3+ + O2−. However, substitutions 2Pb2+ + □ → 2Sm3+ + O2− apparently are possible for Pb8Na2(VO4)6 as well as for previously described Pb8Na2(PO4)6 . This is due to absence of OH− groups in the structure and a smaller number of unshared electron pairs in lead atoms compared to Pb10(VO4)6(OH)2. Advantages of Pb-Na systems are twofold. Substantially lower temperature of synthesis for lead sodium apatite [10, 11] compared to alkaline earth apatite-type compounds  simplifies the method of synthesis and promotes the production of fine grains. Additionally, the structural channels of these lead apatite compounds are free, which would be expected to favor oxygen conductivity according to the substitution scheme presented previously. Thus, we anticipate that Ln3+ substitutions are feasible in Pb-Na apatites.
The purpose of this work, therefore, was to study the substitution of samarium (Sm3+) for lead in lead sodium vanadate Pb8Na2(VO4)6. It is known that vanadates with apatite structure form and sinter at much lower temperatures than phosphate apatites. Vanadate apatites also have up to an order of magnitude greater electrical conductivity compared with phosphate apatites . Since conductivity determination is part of the characterization we report here, vanadate apatites are advantageous for this study.
2. Experimental Procedure
A series of samples Pb(8−x)Na2Smx(VO4)6O(x/2) with the values of = 0, 0.05, 0.10, 0.15, 0.20, 0.25, 0.30, 0.40, 0.50, and 0.60 have been investigated. Reagents that have been used are PbCO3 (99.99% pure) and NH4VO3 (99.5%) from Alfa Aesar and Na2CO3 (99.8%) and Sm2O3 (99.99%) from Acros Organics. Powders were weighed on an analytical balance, mixed, and then ground for 20 minutes in an agate mortar. Then, the mixture was transferred into alumina crucibles and calcined for one hour at 300°C and 500°C each and then at 600°C. Samples were analyzed by X-ray diffraction after every 5-6 hours of calcination at 600°C, which was carried out until a consistent phase composition was attained. The synthesis was completed in 67 hours at 600°C. XRD analysis was conducted on a Rigaku Ultima IV diffractometer (CuKα-radiation, Ni-filter) with the scanning rate of 2° (2) per minute.
Phase composition analysis was carried out using the PDXL software. The unit cell parameters were calculated by the least squares method based upon 17 clearly displayed peaks with the angular scan rate of counter 1° per minute (). Silicon was added to samples as an internal standard. Rietveld refinement was then used to determine the crystalline structure by powder diffraction data. The angular range chosen for calculations was from 15 to 140° (). The angle increment and scanning rate were 0.02°and 0.3° per minute, respectively. The refinement was carried out using WinCSD software . The reliability factors and for compositions with and 0.15 were equal to 0.055, 0.097 and 0.048, 0.088, respectively. Infrared absorption spectra were recorded in the wave number range from 4000 to 400 cm−1 with a Bruker-Optics infrared spectrometer with Fourier transformer, using KBr pellets compressed at a pressure of 700 MP (mass ratio 1 : 200). The grain size and composition, as well as elemental distribution on the grain surfaces, have been studied using a JSM-6490LV scanning electron microscope with INCA Penta FETx3 (OXFORD Instruments) energy dispersion spectrometer.
To measure electrical conductivity, the powders were pressed into the pellets with diameter of 0.8 cm at a pressure of 120 MPa and sintered at 600°C for 50 hours. Silver was used as electrodes. Resistivity measurements were carried out with a LCR DE-5000 meter at 100 kHz frequency while heating the samples from 300 to 600°C with a rate of 2°/min.
3. Results and Discussion
Powder diffraction analyses show that only apatite diffraction lines are present in the composition range (Figure 1(a)). In addition to peaks corresponding to the apatite structure, the peaks corresponding to a SmVO4 phase are found in the diffraction patterns of the samples with composition in the apatite formula. For , the intensity of the SmVO4 lines increases as the proportion of Sm2O3 in the mixture of initial components increases. Thus, based on the samples’ phase composition data, the replacement of samarium for lead in the Pb-Na apatite structure occurs in the range . The refinement of the location of the single-phase region boundary was carried out using the “disappearing phase” method by plotting the absolute intensity of hkl = 200 line of the SmVO4 phase as a function of value (Figure 1(b)). Extrapolating the resulting straight line to a zero-intensity value for the SmVO4 peak, the limit of substitution of samarium for lead was found at .
Incorporation of samarium into apatite structure is confirmed by the unit cell parameters presented in Table 1. This data shows a decrease of the unit cell parameter (by 0.017 Å with the precision 0.001-0.002 Å) and within the error (by 0.004 Å) as the samarium content increases due to the smaller ionic radius of Sm3+ (1.132 Å) compared to the radius of Pb2+ (1.350 Å), using the ionic radii of Shannon for coordination number 9 .
However, this small change (0.017 and 0.004 Å for parameters and , resp.) requires explanation, since the difference in the ionic radii is significant (0.218 Å). To explain what causes this phenomenon, a comparison of the values for the unit cell parameters for Pb10(VO4)6(OH)2, Na2Pb8(VO4)6, and K2Pb8(VO4)6 with apatite structure has been done (Table 2). As can be seen from the table, replacement of the alkali metals for lead results in significant reduction in values of the unit cell parameters not only in case of sodium but surprisingly in case of potassium as well, although the radius of K+ (1.550 Å) is larger than the ionic radius of Pb2+ (1.350 Å). Replacement of alkaline metals for lead in the structure of Pb10(VO4)6(OH)2 reduces the size of the apatite unit cells so significantly that the partial replacement of samarium (smaller in size than lead) for lead has almost no effect on the values of the unit cell parameters.
The reason for this, which is related to the reason for the lack of substitution in the systems Pb(10−x)Lnx(ZO4)6(OH)(2−x)Ox, lies in the electronic structure of lead. Unlike alkaline earth elements apatites, in lead apatites (Pb10(ZO4)6(OH)2), stereochemically active lone electron pairs experience repulsive forces from OH− ions, located in the structural channels. The substitution under the cheme Pb2+ + OH− → Na+ + □ results in decreasing the number of OH− ions and the number of lone electron pairs in the structure, thereby decreasing repulsion and promoting a more compact structure. Indeed, minimal Pb-O distances 2.210 and 2.218 Å  in the vanadates Pb8Na2(VO4)6 and Pb8K2(VO4)6 are significantly less than the 2.35 Å Pb-O distance in Pb10(VO4)6(OH)2 . Thus, in this case, the change in cell parameters is primarily influenced not by the size of the structural units but by the nature of the chemical bond. Rietveld method crystal structure refinement has established that sodium and samarium ions in Pb(8−x)Na2Smx(VO4)6O(x/2) occupy half of the M(1) position and lead ions occupy the second half of M(1) position. Position M(2) is fully occupied by the lead ions. These findings are in agreement with previous work  for Pb8Na2 (VO4)6. The average interatomic distances Pb(2)-O(1–3), V-O, and Pb(2)-Pb(2) do not change substantially as values increase and only Pb(1)-O(1–3) decreases from 2.800(4) to 2.777(4) due to the substitution of smaller samarium ions into the Pb(1) position according to crystal structure refinement (Table 3).
Note: data are given for the solid solution with and ; hence, interatomic distances for the intermediate compositions will be within an error.|
IR spectra of Pb8Na2(VO4)6 and a solid solution Pb7.8Na2Sm0.2(VO4)6O0.1 in the wave number range from 1000 to 400 cm−1 are shown in Figure 2. The absorption bands at 760, 819, and 845 cm−1 and bands at 416, 466, and 514 cm−1 can be assigned to ν3 and ν4 vibrations of ions [11, 12, 16]. As a result of substitution of samarium for lead, frequency of the ν4 band increases by 2-3 cm−1 and frequency of the ν3 (819 cm−1) band increases by 3 cm−1. Furthermore, the spectrum of the solid solution has an additional band at 444 cm−1 not detected previously in studies on nonmodified lead apatite [11, 12]. However, in studies of substitutions in Ca10−xLax(PO4)6(OH)y  and Sr10−xEux(PO4)6(OH)2−xOx , additional bands were detected in this frequency region and were assigned to vibrations of La-O and Eu-O, respectively.
Therefore, the band at 444 cm−1 can be assigned to vibrations of Sm-O.
Scanning electron microscopy of the synthesized compounds (e.g., Figure 3) shows that the elements are uniformly distributed over the surface of the powder particles. Available irregularity related to its relief.
Since the lead oxide can sublime in the synthesis, elemental microanalysis by scanning electron microscopy was performed on 20 samples each of compositions and (Table 4). The experimental results are in satisfactory agreement with the calculated values. The analytical error in these measurements is comparable to those reported in  for compounds with apatite structure studied by the same method. In addition, the elemental composition data obtained by the crystal structure refinement (Table 4) is consistent with the results of microanalysis; if sublimation of lead oxide did take place, it was only to a minor extent.
|Elemental composition was determined using Rietveld crystal structure refinement.|
To evaluate electrical conductivity of the synthesized apatites, was plotted against 1/T. Two such plots for compositions with and are given in Figure 5. In contrast to , in which for Pb8Na2(VO4)6 only one linear plot was obtained in the temperature range 350–456°C, we have determined the conductivity of Pb8Na2(VO4)6 in the temperature range 300–600°C. Four plots were obtained, yielding activation energy values 0.49, 1.61, 4.84, and 1.41 eV in the temperature ranges 300–440, 440–480, 480–530, and 530–600°C, respectively (Table 5). The values of activation energy and electrical conductivity for unmodified Pb8Na2(VO4)6 in the temperature range of 300–440°C (Table 6) do not differ significantly from the results on conductivity obtained in  (0.37·10−5, 0.67·10−5, and 1.30·10−5 at 350, 400, and 450°C and activation energy 0.59 eV). The activation energies for Pb8Na2(VO4)6 ranges in the temperatures 440–480 and 530–600°C are 1.61 and 1.41 eV and belong to the range 1.21–2.07 eV also found for the solid solution Pb8K2−xNax(PO4)6 with the apatite structure having a cationic conductivity . However, the activation energy in the temperature range 480–530°C is significantly higher (4.84 eV) and is not typical of cationic conductivity. Somewhat lower activation energy (3.85 eV) and a similar dependence of the electrical conductivity on temperature were previously described for compounds with the apatite structure Pb4.8Bi1.6Na3.6(PO4)6 .
|Temperature ranges are given for Pb8Na2(VO4)6 (); they are approximately the same for other compositions.|
On the basis of its crystal structure study at 900 K, such large activation energy for ionic conductivity is thought to result from the transfer of sodium cations from their positions at normal conditions to the center of the channel. The cationic conductivity in Pb4.8Bi1.6Na3.6(PO4)6 was found within the entire temperature range.
As the replacement of samarium for lead takes place, activation energy varies depending on the value of and on temperature. Thus, in the temperature range 300–440°C, activation energy gradually increases with increasing (Table 5). At higher temperatures, the most significant change in activation energy, about 30–100%, takes place with the substitution of lead by 0.62 wt. % (at ). In the temperature range of 440–480°C it first decreases significantly from 1.61 to 0.98 eV and then gradually increases to 1.49 eV with increasing content of samarium. In the temperature range of 530–600°C, the opposite takes place; activation energy initially rises sharply from 1.41 to 2.89 eV and then gradually decreases to 1.06 eV. Finally, in the temperature range of 480–530°C the activation energy decreases from the greatest magnitude of 4.84 to 2.44–2.49 eV.
The electrical conductivity of synthesized apatites (Table 6) decreases by 50% to 80% throughout almost the entire temperature range in going from pure Pb apatite () to a Sm substitution of and then increases as samarium content increases (Table 6). In the temperature range 450–500°C, the conductivity for the limiting composition () is twice as much as that of Pb8Na2(VO4)6.
The substitution of samarium for lead in Pb(8−x)Na2Smx(VO4)6O(x/2) occurs in the region . Conductivity decreases sharply by 50% to 80% with initial Sm substitution for Pb (from to ) and then increases with x over the entire temperature range. Conductivity for the limiting composition of the solid solution () is approximately twice as much as it is in Pb8Na2(VO4)6 over the temperature range 450–500°C. These results may be of practical importance in the application of the modified solid solutions of lead sodium vanadate as solid electrolytes and luminescent materials.
Conflict of Interests
The authors declare that there is no conflict of interests regarding the publication of this paper.
The authors are grateful to Dr. Steven Losh for editorial help.
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