B.
Arab-Chapelet
*a,
P. M.
Martin
b,
S.
Costenoble
a,
T.
Delahaye
a,
A. C.
Scheinost
c,
S.
Grandjean
a and
F.
Abraham
d
aCEA, DEN, DRCP, SERA/ Laboratoire de Conversion des Actinides et Radiolyse, BP 17171, F-30207 Bagnols sur Cèze Cedex, France. E-mail: benedicte.arab-chapelet@cea.fr
bCEA, DEN, DEC, 13108 St Paul Lez Durance, France
cHelmholtz-Zentrum Dresden-Rossendorf, Institute of Resource Ecology, D-01314 Dresden, Germany
dUniv. Lille Nord de France, Unité de Catalyse et de Chimie du Solide, UCCS, UMR CNRS 8181, ENSCL-USTL, BP 90108, 59652 Villeneuve d'Ascq Cedex, France
First published on 2nd March 2016
Mixed actinide(III,IV) oxalates of the general formula M2.2UIV1.8AnIII0.2(C2O4)5·nH2O (An = Pu or Am and M = H3O+ and N2H5+) have been quantitatively precipitated by oxalic precipitation in nitric acid medium (yield >99%). Thorough multiscale structural characterization using XRD and XAS measurements confirmed the existence of mixed actinide oxalate solid solutions. The XANES analysis confirmed that the oxidation states of the metallic cations, tetravalent for uranium and trivalent for plutonium and americium, are maintained during the precipitation step. EXAFS measurements show that the local environments around U+IV, Pu+III and Am+III are comparable, and the actinides are surrounded by ten oxygen atoms from five bidentate oxalate anions. The mean metal–oxygen distances obtained by XAS measurements are in agreement with those calculated from XRD lattice parameters.
With the ongoing nuclear transition towards 4th generation reactors, France has initiated a project called ASTRID (Advanced Sodium Technological Reactor for Industrial Demonstration), which is a French prototype of a sodium-cooled FNR.1 Although the main objective of this project is to assess the ability of fast reactors to burn plutonium isotopes, spurred on by the French Bataille Act, it will also be of great interest to evaluate minor actinide (MA = Np, Am or Cm) partitioning and transmutation.2 Two types of transmutation are currently considered: homogeneous and heterogeneous.3 In homogeneous mode, MAs are directly added to the fuel to form MA-MOX.4 Only a small percentage of MAs will be included in the fuel to avoid changing the core neutronics. In the heterogeneous mode, minor actinides are introduced into a UO2 based matrix located in the core periphery as a minor actinide bearing blanket (MABB).5,6 This last option is preferred due to its low influence on the core behavior and the higher quantity of MAs transmuted. Among the MAs, americium has been given priority due to its high radiotoxicity after Pu recycling and its proportion in spent fuel, with the irradiation of U1−xAmxO2±δ pellets called Am bearing blankets (AmBB).
FNR MOX fuel integrates higher quantities of Pu than is in the MOX currently used in PWR or AmBB blankets, and so fuel fabrication routes based on pulverulent precursors for fuel pelletization steps should be modified. Conventional fuel fabrication7 is currently based on multistep powder metallurgy processes, which involve mixtures of simple oxides, ball milling, pelletizing and reactive sintering, and could be limited for several reasons.
These methods, due to the number of steps, generate large quantities of very fine, and thus contaminating, particles. Also, they can lead to very significant chemical and microstructural heterogeneities in the sintered MOX or AmBB that may be accentuated by the presence of a miscibility gap in the U–Pu–O phase diagram or the higher oxygen potential of the americium oxides compared to UO2.
For the pellet fabrication of MOX and AmBB intended to be irradiated in FNRs and thus promote the transition to 4th generation reactors, it would be advantageous to develop new non-proliferative synthesis routes, which allow the obtaining of precursor powders of homogeneous mixed oxide that could be directly pelletized and sintered.8–10 Using actinides from spent fuel dissolution purified in nitric acid media, these synthesis routes are based on a co-conversion step, which permits the quantitative transfer of the actinides from solution into mixed actinide oxides. Various co-conversion methods such as the oxalate precipitation route have been investigated. Since the 1990s, several works have provided evidence that this process, based on the precipitation of an oxalate compound followed by its thermal treatment into an oxide, is a particularly convenient route for actinide co-conversion into mixed oxalate compounds, suitable as the precursors of mixed actinide oxides.11–17 Thus, oxalic precipitation of different actinide(IV)–actinide(III) oxalates characterized by different crystallographic structures and morphologies can be achieved. Moreover, a strong relationship between the microstructure and properties of the mixed actinide oxides and the morphology and crystallographic structure of the oxalate precursors has been established.18,19 The influence of oxide morphology during the fuel pellet formation is an important factor in the process, and therefore, the thorough structural characterization of the mixed oxalate precursor is a key step. Up until now, there is only one structural determination from single-crystal X-ray diffraction data concerning mixed actinide(IV)–actinide(III) oxalate compounds.20 In many works U(IV)–Ln(III) systems are considered as good structural analogs of An(IV)/An(III) systems due to their similar ionic radii.21–23 Consequently, the structure of precipitated actinide oxalates14,16,18 has often been identified by comparison with the structural data of a three mixed U(IV)–Ln(III) oxalate series, named hexagonal, triclinic and tetragonal, with the formula M2+xUIV2−xLnIIIx(C2O4)5·nH2O for the first and M1−xLnIII1−xUIVx(C2O4)2·nH2O for the last two,24–26 where M is a monovalent cation. These three structural series are characterized by a mixed crystallographic site which accommodates both U(IV) and Ln(III) ions despite their charge difference. The charge compensation due to the substitution of the trivalent cation for the tetravalent cation, or vice versa, is ensured by the presence of single-charged cations, M, located in the interspaces of the structure.
This article aims to present multiscale characterizations combining X-ray Absorption Spectroscopy (XAS) and powder X-Ray Diffraction (XRD) measurements performed on mixed U(IV)–An(III) (An(III) = Pu or Am) oxalates.
Lanthanide nitrate salts (Aldrich, 99.9% Reagent Grade Ln(NO3)3·6H2O, Ln = Ce, Nd or Gd) were used when appropriate to prepare Ln(III) solutions to simulate An(III) solutions in pseudo-active experiments, considering the analogies between Ln(III) and An(III) ions.21–23
The resulting crystallized powders, whose color depends on the elements involved, were filtered off and dried at room temperature.
For XAS measurements, samples were fabricated using a standard method for transmission geometry/configuration: ∼2 mg of mixed oxalate or oxide powder was mixed with 15 mg of cellulose using an agate mortar. The resulting mixture was pelletized and then confined in two independent sealed sample holders.
Silicon was added to all samples as an internal standard to calibrate the angular positions of the observed XRD lines. Actinide oxalates were mixed with an epoxy resin to prevent contamination spreading and their diffraction patterns were compared with the recently built M+–U(IV)–Ln(III) oxalate structures database20,24–26 to detect isomorphic similitude.
The refinement of the lattice parameters was carried out using the “pattern matching” option of the Fullprof software28 where only the profile parameters (cell dimensions, peak shapes, background, zero point correction and asymmetry) were refined. The peak shape was described by a pseudo-Voigt function with an asymmetry correction at low angles.
The hydrazinium content was determined by colorimetric analysis after dissolution of the precipitated solids in concentrated nitric acid solution. In a 1 M nitric medium, hydrazinium cations react with dimethylamino-4-benzaldehyde to form a yellow complex characterized by the presence of a peak around 455 nm.
To determine the oxidation states of U, Pu and Am cations, XANES spectra were compared to data collected on several reference compounds at the same beam line (BM20) using the same experimental set-up. The reference compounds were U+IVO2 for uranium, Am+IVO2 for americium,33 Pu+IVO2 and Pu+IIIF3 for plutonium31 and the data were collected at U-LIII, Am-LIII and Pu-LIII, respectively.
The ATHENA software32 was used for extracting EXAFS oscillations. The experimental EXAFS spectra collected on the (U,Pu) and (U,Am) mixed oxalate samples were Fourier-transformed using a Hanning window over the full k space range available for each edge: 2.6–13.5 Å−1 for U and Am LIII; 2.6–12.8 Å−1 for Pu-LII. Curve fitting of the EXAFS spectra was performed simultaneously on k1, k2 and k3-weighted data in an R-space between 1.5 and 4.4 Å using the ARTEMIS software.32 Phases and amplitudes for the interatomic scattering paths were calculated with the ab initio code FEFF8.40.34 Spherical 7.5 Å clusters of atoms built using the hexagonal crystallographic structure (space group = P6/3mmc) determined by Chapelet-Arab et al.24 were used for the FEFF8.40 calculations. The cell parameters used for theoretical calculations are those determined experimentally in this work by X-ray diffraction. In this crystallographic structure, each cation (U, Pu and Am) is surrounded by five oxalate ions (C2O4). Three single-scattering (two-legged) paths are then used in the EXAFS fitting process. These three paths correspond to 10 oxygen atoms (O1) located at ∼2.46 Å, 10 carbon atoms at ∼3.29 Å and 10 oxygen atoms (O2) at ∼4.52 Å. These mean distances have been obtained by averaging the different distances given by the crystallographic structure for each coordination shell. Furthermore, two three-legged and one four-legged multiple-scattering paths, based on their relatively high magnitudes, were included to fit the spectra. The three-legged paths are Abs-C(1)–O-Abs (Abs representing the absorbing atoms) and Abs-O(2)–C-Abs. The four legged one is Abs-C–O(1)–C-Abs. Without the addition of these three multiple-scattering paths the third coordination corresponding to O(2) atoms cannot be properly fitted as its relative amplitude is lower relative to these paths. Due to the reduced spectral domain available for Pu-LII, it was not necessary to consider the three-legged path Abs-C–O(1)-Abs during the fit. Furthermore, in order not to limit the introduction of free parameters, the N and σ2 values for each multiple-scattering path were not individually fitted but linked to the values used for the included single-scattering paths. Only the distances were fitted because, as mentioned for the single-scattering paths, the distances obtained are an average of the different equivalent contributions. As often employed for An LIII/LII31–37 the amplitude factor (S02) was set at 0.90 for U-LIII and Am-LIII and 1.0 for Pu-LII. The shift in threshold energy (ΔE0) was varied as a global parameter. The goodness of fit is estimated using the Rfactor.32
System | U(IV) | An(III) or Ln(III) | AnIII/(AnIII + UIV) (%) | ||
---|---|---|---|---|---|
Experimental method | [U(IV)] (mol L−1) | Experimental method | [An(III)] or [Ln(III)] (mol L−1) | ||
U(IV)–Ce(III) | TIMS | 3.19 × 10−3 | ICP/AES | 3.4 × 10−4 | 9.6 ± 0.9 |
U(IV)–Nd(III) | TIMS | 3.53 × 10−3 | ICP/AES | 3.8 × 10−4 | 9.7 ± 0.9 |
U(IV)–Gd(III) | TIMS | 3.33 × 10−3 | ICP/AES | 3.8 × 10−4 | 10.3 ± 1.0 |
U(IV)–Pu(III) | TIMS | 2.77 × 10−3 | TIMS | 2.7 × 10−4 | 8.8 ± 0.2 |
U(IV)–Am(III) | TIMS | 3.38 × 10−3 | TIMS | 4.1 × 10−4 | 10.8 ± 0.3 |
For each U(IV)–An(III)/Ln(III) (An(III) = Pu or Am and Ln(III) = Ce, Nd or Gd) oxalic co-precipitation experiment, the resulting solid was characterized from the powder diffraction pattern (Fig. 2) by analogy with uranium(IV)–lanthanide(III)24–26 and uranium(IV)–plutonium(III)20 oxalates whose structures were solved using single-crystal X-ray diffraction data. Isomorphic similitudes have been detected and permit the identification of the precipitation of a homeotype single-phase mixed U(IV)–An(III)/Ln(III) oxalate characterized using the general formula M2+xUIV2−xAn/LnIIIx(C2O4)5·nH2O (M = single charged cation which can be H3O+ and/or N2H5+). This mixed oxalate crystallizes in a hexagonal symmetry and its structural arrangement is based on a mixed crystallographic site which can accept either a tetravalent cation or a trivalent one, with the charge balance being ensured by monovalent cations (H3O+ and/or N2H5+) located in the cavities of the structure. The crystal network is built on honeycomb-like hexagonal rings leading to a three-dimensional structure. Considering the U(IV)–An(III)/Ln(III) pairs (An(III) = Pu or Am and Ln(III) = Ce, Nd or Gd) and a similar An(III)/(U(IV) + An(III)) ratio close to 10% for all compounds, no modification of the global structure of the precipitate is observed.
Fig. 2 X-ray diffraction patterns of U90(IV)–An/Ln10(III) oxalate co-precipitates compared to the X-ray diffraction pattern calculated from the uranium oxalate hydrate, (NH4)2U2(C2O4)5·nH2O single crystal data;24 (a) example of Fullprof fit results obtained for U(IV)–Am(III) oxalate. Si is used as internal standard. |
The diffraction patterns are very similar and characteristic of the hexagonal M2+xUIV2−xAn/LnIIIx(C2O4)5·nH2O compounds.20,24
It is interesting to note that the lattice parameters evolve along the actinide/lanthanide series (Table 2). The decrease in the lattice parameters from Ce(III) to Gd(III) for the hexagonal structure is in agreement with the decreasing ionic radii along the lanthanide series22 (Table 2). Considering the possible effect of alpha radiolysis and the slight difference of the An(III)/(U(IV) + An(III)) ratios (8.8% for Pu and 10.8% for Am), a relevant comparison of the lattice parameters of structures based on those trivalent actinides adjacent on the periodic table is not practicable. XRD analysis shows that mixed oxalate compounds characterized by a similar hexagonal structure are obtained when, starting from (N2H5+,H3O+)2UIV2(C2O4)5·nH2O,18 tetravalent uranium is substituted by a trivalent lanthanide or actinide (An/Ln(III)/(U(IV) + An/Ln(III) ∼ 10%). Considering the lattice parameters determined for the U(IV)–Nd(III) and U(IV)–Am(III) systems, a slight discrepancy is observed from the data previously published.18 This difference is more important for the a parameter, which corresponds to the hexagonal cycles.
System | a (Å) | c (Å) | AnIII/(AnIII + UIV) (%) | Reference |
---|---|---|---|---|
U90(IV)–Ce10(III) | 19.225(2) | 12.745(2) | 9.6 ± 0.9 | This work |
U90(IV)–Nd10(III) | 19.222(3) | 12.738(2) | 9.7 ± 0.9 | This work |
U90(IV)–Nd10(III) | 19.205(2) | 12.74(2) | 10 ± 1 | 18 |
U90(IV)–Gd10(III) | 19.183(2) | 12.707(3) | 10.3 ± 1.0 | This work |
U90(IV)–Pu10(III) | 19.193(2) | 12.730(2) | 8.8 ± 0.2 | This work |
U90(IV)–Am10(III) | 19.245(2) | 12.760(2) | 10.8 ± 0.3 | This work |
U90(IV)–Am10(III) | 19.203(8) | 12.74(1) | 10 ± 1 | 18 |
Water molecules and hydrazinium and oxonium cations located in these hexagonal cavities are very labile and their composition partially depends on the chemical conditions of the precipitation and the storage conditions of the precipitates. Moreover, the decomposition of hydrazinium cations leads to the formation of ammonium cations, which can participate in the charge balance in the hexagonal mixed oxalate and modify the lattice parameters.39
In the U(IV)–An(III)/Ln(III) precipitated solids, hydrazinium cations were quantified in order to study the balance charge mechanisms during the partial substitution of tetravalent uranium by a trivalent lanthanide or actinide. Very similar contents were obtained except for the uranium–americium compound (Table 3). Then a general formula of (N2H5+)1.2(H3O+)1UIV1.8An/LnIII0.2(C2O4)5·nH2O can be suggested. These results show that the balance charge during the partial substitution of tetravalent uranium by a trivalent lanthanide or actinide is ensured by the same mixture of hydrazinium and oxonium cations. Concerning the U(IV)–Am(III) precipitate, radiolysis could be responsible for the partial decrease of hydrazinium contents in the solid phase.
System | General formula M2+xUIV2−xAn/LnIIIx(C2O4)5·nH2O | ||||
---|---|---|---|---|---|
UIV | Ln/AnIII | N2H5+ | H3O+ | H2O | |
U90(IV)–Ce10(III) | 1.81 | 0.19 | 1.2 | 1.0 | 5.4 |
U90(IV)–Nd10(III) | 1.81 | 0.19 | 1.2 | 1.0 | 5.3 |
U90(IV)–Gd10(III) | 1.79 | 0.21 | 1.2 | 1.0 | 6.0 |
U90(IV)–Pu10(III) | 1.82 | 0.18 | 1.1 | 1.1 | 5.5 |
U90(IV)–Am10(III) | 1.78 | 0.22 | 0.8 | 1.4 | 5.1 |
Thermogravimetric experiments were carried out on the different mixed U(IV)–An(III)/Ln(III) compounds and led to the determination of the complete general formula of each mixed U(IV)–An(III)/Ln(III) oxalate (Table 3). The different thermogravimetric curves are very close which indicates that very similar mechanisms are implied during thermal decomposition for each mixed U(IV)–An(III)/Ln(III) oxalate (Fig. 3). Qualitatively, the thermal conversion of the different mixed U(IV)–An(III)/Ln(III) oxalates into oxides proceeds through dehydration and hydrazinium cation decomposition steps (between 20 and around 300 °C) followed by the oxalate ligand decomposition step (between 300 and 700 °C) leading to the mixed oxide formation. These decomposition steps are quite similar to those previously reported for the (N2H5+)2UIV2(C2O4)5·nH2O oxalate decomposition.40 Finally, no significant difference is observed in the chemical formula derived from the TGA experiments which confirms also the existence of the same mechanism of oxalic co-precipitation for all U(IV)–An(III)/Ln(III) pairs (An(III) = Pu or Am and Ln(III) = Ce, Nd or Gd).
Fig. 3 TG plot analyses of U(IV)–An(III)/Ln(III) mixed oxalates under Ar: ■ U(IV)–Pu(III); ▲ U(IV)–Am(III); ◆ U(IV)–Ce(III); ● U(IV)–Nd(III); U(IV)–Gd(III). |
The following investigations by EXAFS and XANES experiments aim at unambiguously determining the oxidation states stabilized in the oxalate compounds and precisely investigating the U(IV)–An(III)/Ln(III) oxalate solid solutions.
In fact only the non-substituted U(IV) hexagonal structure has been totally determined.24 For the substituted U(IV)–An(III)/Ln(III) oxalate single crystals only a subcell with as = a/√3, and cs = c/2 is observed and only an average structure in this subcell has been determined for the mixed U(IV)–Pu(III) oxalate (NH4)2.7PuIII0.7UIV1.3(C2O4)5·nH2O.20 Thus, occupation of different sites with different environments for U(IV) and An(III)/Ln(III) atoms in the actual structure cannot be ruled out. In the (NH4+)2UIV2 (C2O4)5·nH2O hexagonal structure, U(IV) is coordinated by 10 oxygens from five bidentate oxalate ligands24 but in Ln(III) and An(III) oxalates the metals are coordinated by six oxygens from three oxalate ligands and three water molecules.41,42 It is therefore essential to ensure that Ln(III) and An(III) have the same environment in the substituted compounds as U(IV).
XANES spectra collected at Am LIII and Pu LIII edges are shown in Fig. 5a and b respectively. For the (U,Am) sample, the E0 and WL positions are located at 18513.1(5) eV and 18517.1(5) eV respectively. Both positions are clearly shifted to lower energies compared to AmO2 with 18514.5(5) and 18521.5(5) eV for the E0 and WL positions, respectively. The 4.4(5) eV difference between the WL positions is in very good agreement with the value of 4 eV observed between the WL positions of AmIVO2 and AmIII2O3 by Nishi et al.43 Based on this comparison, the +III state of americium in the (U,Am) mixed oxalate is evidenced. Concerning the (U,Pu) sample, both the E0 (18058.9(5) eV) and the WL (18062.8(5) eV) Pu-LIII XANES positions are slightly below the positions reported for PuIIIF331 which are equal to 18059.3(5) eV and 18063.3(5) eV for the E0 and the WL, respectively. Moreover, similarly to americium, a 4.3(5) eV shift to lower energy compared to the WL maximum reported for PuIVO2 (18067.1(5) eV)33 is observed.
Based on these results, we can come to a conclusion on the accuracy of the formulations (UIV,AnIII) and (UIV,LnIII).
Fig. 6 (a) Hexagonal unit cell based on resolved (U,Nd) structure.24 ( Actinide/lanthanide cations, and oxygen and carbon atoms in the C2O4 group, and monovalent cations and oxygen atoms in water molecules). (b) EXAFS data at uranium LIII edge. (c) Fourier transformations of EXAFS shown in (b). |
The three FT are almost identical indicating that a similar environment is observed around uranium cations for the three samples.
EXAFS fit results for (U,Am) and (U,Pu) oxalate samples are displayed in Fig. 6–8, and associated metric values are given in Tables 4 and 5. The experimental data are very well reproduced by the fits as illustrated by the low Rfactor values obtained. For each sample, the three coordination shells corresponding to single-scattering paths (O1, C and O2), and coordination numbers equal to ∼10 (by taking into account uncertainties) are systematically obtained for both cations. This result is in very good agreement with the structure including five oxalate ions (C2O4) around U+IV, Pu+III and Am+III cations in the mixed (U0.9Pu0.1) and (U0.9Am0.1) oxalates. The same values of the Debye–Waller factors around both U and Am in the (U,Am) sample compared to values observed in (U,Pu) sample were measured. As the data were collected at 15 K, these similar σ2 values illustrate that a similar structural disorder is observed in the two mixed oxalates.
EXAFS | XRD | ||||
---|---|---|---|---|---|
Edge | Coordination shell | N | R (Å) | σ 2 (Å2) | R (Å) |
For multiple-scattering paths, values with a star (*) correspond to the parameters fixed during the fit and are calculated using the correspond single-scattering paths. The XRD corresponds to the values calculated using the cell parameters given in Table 2. | |||||
U-LIII | O (1) | 10.5(5) | 2.46(1) | 0.005(1) | 2.46 |
C | 9.2(5) | 3.28(2) | 0.003(1) | 3.28 | |
O (2) | 10(2) | 4.50(2) | 0.011(2) | 4.52 | |
C → O(1) | 20* | 3.45(2) | 0.004* | 3.51 | |
O(2) → C | 20* | 4.58(2) | 0.008* | 4.59 | |
C → O(1) → C | 10* | 4.51(2) | 0.008* | 4.53 | |
ΔE0 (eV) | 3.0(5) | ||||
R factor (k1; k2; k3) | 0.004; 0.006; 0.011 | ||||
Pu-LII | O (1) | 10.4(5) | 2.53(1) | 0.007(1) | 2.46 |
C | 10.0(5) | 3.32(1) | 0.004(1) | 3.28 | |
O (2) | 10(2) | 4.55(2) | 0.004(1) | 4.52 | |
O(2) → C | 20* | 4.55(2) | 0.004* | 4.59 | |
C → O(1) → C | 10* | 4.55(2) | 0.005* | 4.53 | |
ΔE0 (eV) | 3.0(5) | ||||
R factor (k1; k2; k3) | 0.003; 0.004; 0.008 |
EXAFS | XRD | ||||
---|---|---|---|---|---|
Edge | Coordination shell | N | R (Å) | σ 2 (Å2) | R (Å) |
For multiple-scattering paths, values with a star (*) correspond to the parameters fixed during the fit and are calculated using the corresponding single-scattering paths. The XRD corresponds to the values calculated using the cell parameters given in Table 2. | |||||
U–LIII | O (1) | 10.8(5) | 2.46(1) | 0.006(1) | 2.46 |
C | 9.6(5) | 3.28(2) | 0.005(1) | 3.29 | |
O (2) | 10(2) | 4.50(2) | 0.012(2) | 4.52 | |
C → O(1) | 20* | 3.45(2) | 0.004* | 3.51 | |
O(2) → C | 20* | 4.60(2) | 0.008* | 4.55 | |
C → O(1) → C | 10* | 4.49(2) | 0.004* | 4.51 | |
ΔE0 (eV) | 3.1(5) | ||||
R factor (k1; k2; k3) | 0.010; 0.012; 0.015 | ||||
Am–LIII | O (1) | 10.4(5) | 2.50(1) | 0.007(1) | 2.46 |
C | 10.0(5) | 3.32(1) | 0.007(1) | 3.29 | |
O (2) | 10(2) | 4.54(2) | 0.004(1) | 4.52 | |
C → O(1) | 20* | 3.54(2) | 0.007* | 3.51 | |
O(2) → C | 20* | 4.59(2) | 0.006* | 4.55 | |
C → O(1) → C | 10* | 4.62(2) | 0.006* | 4.51 | |
ΔE0 (eV) | 0.3(5) | ||||
R factor (k1; k2; k3) | 0.003; 0.005; 0.012 |
For each compound, the only significant differences observed between the two actinides are systematically shorter distances around uranium than around Pu or Am. These differences could be explained by the difference in ionic radii between U+IV and trivalent Pu and Am, but these values are unknown for such cations that are ten-coordinated. Nevertheless, based on values available for americium(III) and uranium(IV) cations for a coordination number (CN) of 9 (Am+III = 1.162 Å (ref. 23) and U+IV = 1.05 Å (ref. 22)), the Am+III–O bond distance would be significantly longer (about 0.11 Å) than the U+IV–O bond. Similar values would be observed for Pu+III–O and Am+III–O distances as Pu and Am have very similar ionic radii (Am+III = 1.162 Å (ref. 23) and Pu+III = 1.165 Å (ref. 23) for CN = 9). But, as shown in Tables 4 and 5 the differences with U+IV–O determined by EXAFS in this work are only 0.04 Å and 0.07 Å for americium(III) and plutonium(III), respectively.
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