Tomasz
Jaroń
ab,
Wojciech
Grochala
*ac and
Roald
Hoffmann
*b
aDepartment of Chemistry, University of Warsaw, Pasteur 1, 02-093 Warsaw, Poland. E-mail: wg22@cornell.edu; Fax: +48 22 8225996 ext. 276; Tel: 48 22 8220211
bDepartment of Chemistry and Chemical Biology, Cornell University, Ithaca, NY 14853-1301, USA. E-mail: rh34@cornell.edu; Fax: +1 607 2555707; Tel: +1 607 2553419
cInterdisciplinary Center for Mathematical and Computational Modeling, University of Warsaw, Pawińskiego 5a, 02-106 Warsaw, Poland
First published on 3rd January 2006
We theoretically examine four hypothetical ternary lanthanide hydrides, CsLnIIH3 and Cs2LnIIH4, where LnII = Yb, Tm. We optimize their crystal unit cells in the BaTiO3 and K2NiF4 structures, respectively, and compute their electronic band structures. Our calculations indicate that the novel hydrides should be unstable with respect to decomposition into binaries (CsH and LnIIH2); ternaries would form only under elevated pressure (>7–22 GPa). We predict that significant perturbation of the electronic and magnetic properties of CsYbIIH3 and Cs2YbIIH4 will take place via a progressive exchange of f14 YbII for f13 TmII, while promoting magnetic ordering and valence fluctuations. Analysis of the phonon dispersion for these hydrides suggests that metallic forms of doped CsLnIIH3 and Cs2LnIIH4 would exhibit substantially high Debye temperatures of ∼1800 K. This is likely to prompt moderate-TC superconductivity in these as yet unknown materials.
YbII and EuII, the most prominent representatives of stable divalent lanthanide cations, are often compared to closed shell CaII and SrII, respectively, in terms of ionic radius.5 A nice series of isomorphic compounds of YbII and CaII, and those of EuII and SrII, are known; examples include YbBeF4 and CaBeF4, EuLiF3 and SrLiF3, and—among the hydrides—Yb4Mg3H146 and Yb4Mg4Co3H197 (and their Ca analogues), Eu6Mg7H268 and inverse perovskite EuLiH3 (and their Sr analogues). In all these compounds, binary components of divalent Yb and Eu (i.e., EuF2, YbH2etc.) formally serve as Lewis bases, while donating their ligands to the stronger and smaller Lewis acids (MgII, BeII).
TmII (ionic radius, R, of 1.17 Å in the octahedral environment), an electron-deficient analogue of YbII, is virtually isomorphic with YbII (R = 1.16 Å)9 and with CaII (R = 1.14 Å). However, because of the enormous reducing properties of TmII,10 its compounds are scarce, and very difficult to preserve in the presence of traces of O2 or humidity.
Prompted by the existence of MICaX3 and MI2CaX4, where MI = Cs, Rb and X = H or F,11 of ternary lanthanide salts such as the perovskites CsYbF3,12 CsYbI3 and RbTmI3,13 and driven by the fluoride-hydride analogy,14 we examine theoretically and attempt to predict the possible existence and selected properties of CsLnIIH3 and Cs2LnIIH4 where LnII = Yb, Tm. In these hypothetical compounds, and in contrast to all known ternary hydrides containing divalent lanthanide cations, LnH2 would formally serve as a Lewis acid while accepting hydride anion from the very strong base (CsH). Here, our interest in ternary hydrides of divalent lanthanides has origin in (i) anticipated involvement of f orbitals in bonding, i.e. a mixing of LnII (4f) and H (1s) orbitals (moderate ‘covalence’), (ii) large values of electronic density of 4f states in the vicinity of the Fermi level, and (iii) concomitant consequences of hole- and electron-doping for electronic and magnetic properties of the stoichiometric compounds of LnII, and possible promotion of superconductivity.
For compounds of TmII (an open-shell f13 configuration with large magnetic moment) we have always done spin-polarized calculations (SP). Calculations without spin polarization (‘metallic’ or ‘antiferromagnetic’ polymorph) always yielded a larger energy per unit cell (by about 0.5 eV per Tm atom) than for those with polarized spins (‘ferromagnetic’ polymorph). At the same time, calculations without spin polarization typically result in minor changes in the unit cell vectors (for example, compare results for Cs2TmH4: SP a = b = 4.601 Å, c = 15.696 Å, no SP a = b = 4.616 Å, c = 15.613 Å).
We have also performed supplementary VASP16 calculations for several Yb- and Tm-containing compounds (see the electronic supplementary information (ESI)†). Here we could use dense k-point sampling of 11 × 11 × 11 (CsLnH3), and 11 × 11 × 6 (Cs2LnH4). We tested two types of pseudopotentials: those which explicitly involve f electrons on Ln atoms (PBA set) and those which do not; it turned out that optimizations with VASP (pseudopotentials without f electrons) and CASTEP (pseudopotentials with f electrons) yielded only minor differences in unit cell vectors for CsYbH3 and Cs2YbH4.
For phonon dispersion and phonon DOS calculations we have used the PHONON17 code as implemented in the MEDEA package. PHONON uses VASP-preoptimized unit cells in order to determine vibrations of the crystal lattice. To speed up the time-demanding frequency calculations we used norm-conserving pseudopotentials which do not explicitly involve f electrons on Ln atoms.
Compound | CsYbH3 | CsTmH3 | CsCaH3 | CsCaD3 exp. | Cs2YbH4 | Cs2TmH4 | Cs2CaH4 | Cs2CaD4 exp. |
---|---|---|---|---|---|---|---|---|
a = b/Å | 4.609 | 4.609 | 4.619 | 4.617 | 4.609 | 4.601 | 4.615 | 4.597 |
c/Å | 4.609 | 4.609 | 4.619 | 4.617 | 15.531 (0.148) | 15.696 (0.146) | 15.558 (0.149) | 15.528 (0.149) |
Our GGA-PBA calculations predict a cubic unit cell constant of 4.609 Å for CsYbH3 and 4.609 Å as well for CsTmH3; the deviation from the experimental value for CsCaD3 (4.617 Å) is very small (<0.01 Å) and slightly negative; in fact small positive deviations (ca. +0.03 to 0.04 Å) are expected based on comparison of the crystal radii (see the previous section). The difference between calculated and experimental cubic unit cell constants for CsCaD3 is as small as 0.002 Å.
Our result is entirely within the limitations of the computational method utilized (we note slightly positive deviations for smaller energy cutoffs). The calculated unit cell constant of 4.609 Å for CsYbH3 also matches well the experimental value of 4.61 Å for CsYbF3; indeed, the close hydride–fluoride analogy has been pointed out to apply for similar compounds.14 For CsTmH3, the environment of TmII is predicted to be that of an ideal octahedron; the Jahn–Teller (JT) distortion apparently does not influence the coordination shell of the f13 cation, similar to the crystal structure of CsTmCl3.18 This feature points to the relatively ionic character of Tm–H bonding.
For Cs2YbH4, slight deviations from regular octahedral coordination of YbII are predicted, with four equivalent longer equatorial Ln–H distances of 2.305 Å and two shorter apical distances of 2.301 Å. This effect is of course slightly larger for ferromagnetic (f13) Cs2TmH4 (equatorial 2.300 Å, apical 2.286 Å). An inverse JT effect is computed to be small for the inner transition metal f13 configuration of TmII (the ratio of apical to equatorial Tm–H distances is 0.994), in agreement with experimental data for similar compounds of TmII (the analogous ratio being 0.986 for KTmI3,19 and 1.006 for Cs2TmCl420).
The fractional z atomic coordinate for an apical H(0,0,z) atom (which quantitatively determines the distortion of the {LnH6} octahedron), has been predicted to be 0.146 for Cs2TmH4, via 0.148 for Cs2YbH4, up to 0.149 for Cs2CaH4, always close to the experimental value of 0.149 for Cs2CaD4.
The predicted unit cell vectors are very similar for hydrides of YbII and for isostructural compounds of TmII (identical for CsLnH3, and within 1% deviation for Cs2LnH4). This should facilitate formation of solid solutions for analogous compounds of these Ln metals, i.e., ease of electronic doping.
Compound | CsYbH3 | CsTmH3 | Cs2YbH4 | Cs2TmH4 |
---|---|---|---|---|
ΔH/eV per molecule | 0.27 | 0.55 | 0.19 | 0.47 |
ΔV/Å3 per molecule | −6.02 | −5.30 | −5.66 | −3.85 |
p/GPa | 7.3 | 16.7 | 5.3 | 19.7 |
Ternary Tm and Yb hydrides are predicted to be thermodynamically unstable with respect to decomposition to binary hydrides, and it is not expected that vibrational zero-point correction and entropy effects—typically small for solid reagents—will easily reverse this trend. Diamagnetic forms of TmII compounds are computed to have higher electronic energy than their magnetically ordered (ferromagnetic) polymorphs, in agreement with the strong magnetism of unpaired f electrons. In the following sections we will discuss exclusively ferromagnetic compounds of TmII.
The enthalpy of the reactions of synthesis of ternary hydrides is positive for all ternaries studied, while the associated volume change is computed to be negative (Table 2). This suggests that hydrides might form from binaries at elevated pressure. A rough estimate of the formation pressure can be obtained from the “common tangent” method, as a ratio of reaction enthalpy to the volume change. The estimated formation pressures—listed in Table 2—range from 5 to 20 GPa.23
Our conclusion is that ternary hydrides of TmII and YbII could be synthesized at increased pressures, and at relatively low temperatures up to 200 °C (to avoid decomposition of fragile CsH) and with rather small H2 overpressure (to avoid formation of compounds of trivalent lanthanides, especially for compounds of divalent Tm, strong reducing agents). Some of these ternary phases might be quenchable upon decompression to 1 atm.
The band structure of Cs/Yb(Tm) hydrides (see ESI†) consists of: (i) very narrow filled subvalence bands originating from 5s2 (at about −52 eV) and 5p6 (at about −24 eV) states of Yb(Tm), and from 5s2 (at about −23 eV) and 5p6 (at about −10 eV) states of Cs, (ii) a filled ‘hydride band’ at −6 to −2.5 eV, (iii) a very narrow 4f valence band and (iv) a very broad set of bands constituting the conducting band. In the analysis to come we will omit the sub-valence bands, i.e. set (i).
The CASTEP software does not allow direct atomic identification of a given segment of the density of states, only decomposition by angular momentum type—s, p, d, or f. Nevertheless an atomic assignment can be made, both by the energy range in which the density is found, and also by computing the disposition in space of the states in a given energy interval.
The ‘hydride band’ (ii) is visibly split from the valence band (iii) for all ternary hydrides studied (by some 3 eV) and it is composed predominantly of H (1s) states (Fig. 1), with a little contribution from lanthanide s, p and d states; in turn, the valence 4f band contains very little contribution from H (1s) states, which might point to an ionic formulation of the hydrides studied, to be written formally as CsILnII(H−)3 and (CsI)2LnII(H−)4. The ‘hydride band’ is usually split in several separate bands, some of which show significant dispersion (up to 3 eV). This cannot be due to direct H⋯H interactions, as the hydrides are far apart (usually at >3.2 Å). The band width in the hydride band is due to interactions between H ions and lanthanide and alkali centers; the title hydrides are not as ionic as one might think.
![]() | ||
Fig. 1 Band structure and DOS for CsYbH3 (upper left), CsTmH3 (upper right), Cs2YbH4 (lower left) and Cs2TmH4 (lower right). Focus is on hydride, f and conduction bands. |
The set of bands (iii) originating from 4f states either gives rise to a single and large peak in the DOS (as for diamagnetic f14 YbII) or is split equally into two bands separated by some 2 eV (as for ferromagnetic f13 TmII). This description of f electrons in these phases is unsatisfactory; unfortunately it is common to all first-principles calculations within the independent electron approximation.24,25
The broad conduction band, or rather, the set of interpenetrating bands (with a collective width of up to 9.5 eV for CsLnIIH3 and of only 3 eV for Cs2LnIIH4) is built of s, p and d states, predominantly coming from Yb, but in some part also from the alkali metal. For Yb hydrides, the bottom of the (formally empty) conduction band is remarkably close (0.25–0.5 eV) to the uppermost part of the (formally filled) valence band. For Tm compounds, however, the broad conduction band penetrates through (and for CsTmH3 even 0.5 eV below) the narrow 4f band, thus closing the direct band gap.
The electronic density at the Fermi level consists mainly of rather localized 4f electrons (Fig. 2) with no contribution from H 1s states.
![]() | ||
Fig. 2 Electronic density (in blue) at the Fermi level (EF ± 0.03 eV) for CsYbH3 (upper left), CsTmH3 (upper right), Cs2YbH4 (lower left) and Cs2TmH4 (lower right). Density isovalue 0.012 e Å−3. |
![]() | ||
Fig. 3 Phonon band structure (left) and phonon DOS (right) for CsYbH3; PHONON/VASP calculation. H's contribution to phonon DOS is in black, Yb's one in red, Cs's one in blue. |
The unit cell of CsYbH3 contains 5 atoms, so there are 15 degrees of freedom: 12 vibrational and 3 translational ones. Three phonon bands are seen in the highest frequency range of the spectrum (30.9–37.7 THz, 128–156 meV, 1030–1260 cm−1).27 They are degenerate at the zone center (recollect, the cell is cubic), and correspond to the Yb–H stretching modes. Six other modes are seen in the moderate-frequency range (11.0–21.9 THz, 46–90 meV, 370–730 cm−1). These are the Ln–H–Ln bending modes, which also show significant amplitude of H motions. The last set of three phonons is centered at low frequency (3.07 THz, 13 meV, 120 cm−1). These are deformational modes of the lattice, with predominant contribution from heavy elements (Yb, Cs). The remaining three lowest-frequency motions correspond to translations of the entire lattice; their calculated wavenumbers (at the zone center, Γ) are close to zero within narrow error margin, as expected. The dispersion of Ln–H stretching modes is significant (∼7 THz, 29 meV, 230 cm−1); that of Ln–H bending modes is even larger (∼10.8 THz, 45 meV, 360 cm−1).
The phonon density of states is composed of a single narrow and intense peak originating from the lowest-frequency phonons; a low dispersion, broad band coming from moderate-frequency phonons; and a double peak of moderate intensity marking the highest energy range of the spectrum.28
In the first section we have considered the ‘static’ crystal structure of lanthanide hydrides, and we have pointed to minor structural distortions predicted for the Cs2LnIIH4 compounds. We think that dynamic inversion of the Jahn–Teller effect (a set of local two short and four long Ln–H bonds transforms into two long and four short bonds) is undoubtedly within vibrational amplitude of H atoms, at least within the Born–Oppenheimer approximation. Interestingly, such fluctuating transformation of a JT species should decrease the anisotropy of electron density around the lanthanide cation, in particular for compounds of TmII.
In a simplistic chemical picture, PdHx≈1.0 is formally a mixed valence system, Pd0PdIIH−12.32 A molecular mixed-valence systems can be either localized, delocalized (i.e., intermediate valence), or an intermediate case between the two.33 These three classes of molecular mixed-valence systems may naturally be compared to, respectively, insulating, metallic and superconducting mixed-valence solids.34 In this picture, the electronic wavefunction of a system (be it a solid or a molecule) is most affected by motions of nuclei when the vibrational zero-point energy (ZPE) of metal–ligand–metal stretching (or of the highest-energy optical phonon in solids) is close to the energy barrier for the electron transfer (EB) between the metal centers (Fig. 4).
![]() | ||
Fig. 4 The double-well PES for a mixed-valence compound for three different zero-point vibrational energy situations: (A) a separated (localized) mixed valence compound; (B) a fluctuating valence species; (C) an intermediate (delocalized) valence compound. Solid state analogues are likely to be (A) insulators, (B) superconductors, (C) ‘normal’ metals. Case (D) illustrates the postulated explanation for the inverse isotope effect observed experimentally for palladium hydride (PdH, PdD, PdT). |
When the ZPE is too small, the system is localized (insulating, Fig. 4A). When the ZPE is too large, the system is delocalized (‘simple’ metal) and two distinct oxidation states cannot be recognized in the molecular (crystal) structure (Fig. 4C). We suggest that when the ZPE is close to EB, strong electron–phonon coupling dramatically influences the shape of the wavefunction and superconductivity may arise (Fig. 4B).
For PdH, electron transfer between Pd centers is greatly affected by motions of the hydride ligand.32 Hydrogen is the lightest ligand available to chemistry; here the ZPE can reach as much as 0.25 eV (for molecular H2). In cases when the ZPE for the proton isotope is larger than EB, and since the (classical) amplitude of vibrations—and also the vibrational zero point energy—decreases as the atomic mass increases for three isotopes of H, inverse isotope effect might indeed occur (Fig. 4D).
The case of PdH (small TC because of large energy of hydrogen motions (!), and concomitant easy mixing of d orbitals on Pd centers linked by H) brings to mind an idea for increasing the EB value by (i) involving in the electronic transport such orbitals, which are deeper lying (in energy) and more contracted than the 4d set of Pd (in this contribution we want to use 4f electrons), or by (ii) increasing the separation of the metal centers.35 It might allow a reversal of the atypical isotope effect, and also larger TC values by hydride superconductors. CsTmH3 and Cs2TmH4, which have a nearly filled yet significantly contracted f-shell, seem promising in terms of possible heavy-fermion superconductivity via appropriate chemical doping to these compounds; if EB proves to be too large, external pressure might be applied to bring these systems back towards the metal–insulator transition.
Cs2TmH4 (f13 TmII) is a quite formal analogue of other important systems with a nearly filled electron shell, namely Ln2CuO4 and Nd2CuO4 (d9 CuII). The latter two are parent (undoped) compounds of, respectively, hole-doped (La2−xBaxCuO4) and electron-doped (Nd2−xCexCuO4) oxocuprate superconductors. Simultaneously, CsTmH3 perovskite (f13 TmII) may be treated as a distant sibling of BaBiO3, with a distorted perovskite structure (s1 BiIV). The latter becomes Ba1−xKxBiO3, a regular perovskite superconductor, upon hole-doping.36
Thus, in terms of a formal electron count on the transition metal, Cs2TmII1−xYbIIxH4 would be equivalent to NdIII2−xCeIVxCuII/IO4, while Cs1−x□xTmII/IIIH3 (where □ stands for a vacancy)37 would be analogous to Ba1−xKxBiIV/VO3.38
We expect that tuning the transition between the f13 and f14 electron count39 within the LnH2 sublattice may bring Cs2TmII1−xYbIIxH4 and CsTmII1−xYbIIxH3 towards the anticipated metal/insulator borderline. At this stage, it is impossible to evaluate correctly from first principles whether these quaternary lanthanide hydrides will exhibit genuine heavy-fermion superconductivity, or plain ‘valence fluctuations’ (commonly observed for compounds of Yb, Tm, Eu, Sm, and also Ce and Tb).40,41 The consequences for the electronic and magnetic properties of novel hydride phases of the interplay of strong magnetism of 4f electrons and of the varying electron count (at the edge of the f shell closure), should be probed experimentally.
The estimated Debye temperature of CsYbH3 is substantial, ∼1800 K, while DOS below the Fermi level rises very steep, due to narrowness of the 4f electron band. The BCS theory predicts that these features alone are likely to prompt low-TC superconductivity in as yet unknown hole-doped hydrides of YbII, despite rather small involvement of H states into the DOS at the Fermi level of these compounds. Ultra-high pressure experiments constitute another prospective path of research. External pressure is an independent experimental variable which might enforce larger mixing of hydride 1s states into the quasi-valence 4f electrons and thus provoke larger involvement of the former in the electronic transport in these compounds. In this way a moderate-TC superconductivity could be achieved while making use of strong electron–phonon coupling of the states at the Fermi level with the high-frequency H-based phonons.
Footnote |
† Electronic supplementary information (ESI) available: Full DOS for CsYbH3 and VASP results. See DOI: 10.1039/b514773e |
This journal is © The Royal Society of Chemistry 2006 |