Crystal Structure and Electronic Properties of Bulk and Thin Film Brownmillerite Oxides

Crystal Structure and Electronic Properties of Bulk and Thin Film Brownmillerite Oxides

Joshua Young jy346@drexel.edu Department of Materials Science and Engineering, Drexel University, Philadelphia, PA 19104, USA Department of Materials Science and Engineering, Northwestern University, Evanston, IL 60208, USA    James M. Rondinelli jrondinelli@northwestern.edu Department of Materials Science and Engineering, Northwestern University, Evanston, IL 60208, USA Materials Science Division, Argonne National Laboratory, Argonne, Illinois 60439, USA
July 26, 2019
Abstract

The equilibrium structure and functional properties exhibited by brownmillerite oxides, a family of perovskite-derived structures with alternating layers of O octahedra and O tetrahedra, viz., ordered arrangements of oxygen vacancies, is dependent on a variety of competing crystal-chemistry factors. We use electronic structure calculations to disentangle the complex interactions in two ferrates, SrFeO and CaFeO, relating the stability of the equilibrium (strain-free) and thin film structures to both previously identified and newly herein proposed descriptors. We show that cation size and intralayer separation of the tetrahedral chains provide key contributions to the preferred ground state. We show the bulk ground state structure is retained in the ferrates over a range of strain values; however, a change in the orientation of the tetrahedral chains, i.e., a perpendicular orientation of the vacancies relative to the substrate, is stabilized in the compressive region. The structure stability under strain is largely governed by maximizing the intraplane separation of the ‘dipoles’ generated from rotations of the FeO tetrahedra. Lastly, we find that the electronic band gap is strongly influenced by strain, manifesting as an unanticipated asymmetric-vacancy alignment dependent response. This atomistic understanding establishes a practical route for the design of novel functional electronic materials in thin film geometries.

I Introduction

The family of brownmillerite oxides (general formula O or O) are highly studied for use in ionic conducting and anion insertion applications.Kendall et al. (1995); Boivin and Mairesse (1998); Rolle et al. (2005); Shaula et al. (2006); Orera and Slater (2010); Antipov et al. (2004); Sullivan and Greaves (2012); Tarasova et al. (2013) Their structure type can be thought of as an O perovskite with one-sixth of the oxygen atoms removed, creating parallel rows of ordered anion vacancies along the [110] crystallographic direction; this results in alternating layers of corner-connected O tetrahedra and O octahedra (Figure 1a). While cooperative distortions and octahedral rotations are well understood in perovskites, the presence of tetrahedral layers in the brownmillerites adds additional structural complexity and possible degrees of freedom for both structure and electronic function design. In addition to rotations of the octahedra, each tetrahedral chain can ‘twist’ in a “left-handed” or “right-handed” sense, resulting in two different types of chains related by mirror symmetry (Figure 1b). Furthermore, these different chains can be ordered relative to each other within the brownmillerite unit cell, resulting in a variety of structures displaying different space group symmetries.

Figure 1: The removal of chains of oxygen atoms (colored in black) from the O perovskite structure (a) results in the vacancy ordered O brownmillerite structure (b), which consists of alternating layers of O tetrahedra and O octahedral along the direction. The undistorted rows of O tetrahedra can then ‘twist’ to create left- or right-handed chains (colored blue and red, respectively).

When the tetrahedra and octahedra are not rotated, the structure displays the space group (Figure 2a); this aristotype may be used as a high symmetry reference phase for which subsequent structural analyses are made. Alternatively, the structure can be imagined as having disordered left- and right-handed chains (i.e. the chains display either incommensurate ordering or no long range order); some structures, such as SrCoFeO and SrMnGeO,Battle et al. (1988); Abakumov et al. (2003) display this phase at ambient conditions, while others become disordered at high temperature (including CaAlO and CaFeO).Lazic et al. (2008); Krüher and Kahlenberg (2005) Each of the three low-symmetry bulk hettotypes display two-dimensional sheets of corner-connected octahedra, which rotate out-of-phase along the direction. This rotation transforms like the irreducible representation (irrep) of the phase.

Along the axis, however, the allowed displacements of the oxygen atoms are constrained by the ‘handedness’ and ordering of the tetrahedral chains, which ultimately control the final symmetry of the brownmillerite structure (see the discussion in Section III). The tetrahedral chains can cooperatively rotate in a variety of ways, each described by a different irrep of . When the tetrahedra rotate into either all left- or all right-handed chains the structure displays the polar space group owing to the irrep (Figure 2b). If there is a racemic mixture of both types of chains, the structure becomes centrosymmetric, with different relative orderings generating different symmetries. Alternating chains of different handedness within each tetrahedral layer is described by the irrep and yields the centrosymmetric structure (Figure 2c), while alternation between layers (given by ) gives the centric structure (Figure 2d). Because the left- and right-handed chains are related by symmetry and differ only by small atomic displacements, the formation energies for the different polymorphs are nearly degenerate and should form with equal probability. However, each of the aforementioned ordering types is seen experimentally in various members of the brownmillerite family, and the driving force behind the preferred type in different chemistries is not completely understood.

Figure 2: The hypothetical high symmetry brownmillerite structure (a) is defined as having no octahedral or tetrahedral rotations, and has the space group. Relative ordering of tetrahedral chains results in three different low-symmetry structures. If all chains are of the same handedness, the structure is polar (b); alternation of left- and right-handed chains within each layer results in centric (c), while alternation between each layer gives centric (d). The -site cations are omitted from the low-symmetry structures for clarity.

Another degree of freedom appears for the brownmillerite structures when when they are grown as a thin film, e.g., via molecular beam epitaxy or pulsed laser deposition, owing to the constraints imposed by epitaxial strain. In this thin film case, the oxygen-deficient layers can order parallel or perpendicular to the substrate (this is shown in Figure 3a and 3b, respectively, with the pseudocubic orientation shown in Figure 3c and 3d). Although different strain states will stabilize one orientation over the other, it is not always clear which will be preferred and why. In (La,Sr)CoO, for example, tensile strain stabilizes perpendicular ordering while compressive strain stabilizes parallel ordering;Klenov et al. (2003); Gazquez et al. (2013) however, the opposite effect is observed in strained CaFeO.Inoue et al. (2010)

In this work, we seek to disentangle the structural and energetic effects operative in brownmillerite oxides through an investigation of bulk and epitaxially strained SrFeO and CaFeO using first-principles density functional theory calculations. The SrFeO and CaFeO members are experimentally known to be stable in the ordered brownmillerite phase up to high temperatures (approximately 1200 K for SrFeO and 920 K for CaFeO);Schmidt and Campbell (2001); Krüger et al. (2009) at ambient conditions, SrFeO displays the Pbcm ordering,Auckett et al. (2012, 2013) while CaFeO exhibits the Pnma structure.Krüger et al. (2009) Additionally, they both contain only Fe cations and display G-type antiferromagnetic ordering with high Néel temperatures (700 and 720 K, respectively).Takeda et al. (1968, 1969); Schmidt and Campbell (2001) The indirect band gap of both compounds is approximately 2.0 eV, owing to a - to X-point transition.Galakhov et al. (2010)

Figure 3: When brownmillerite structures are placed under epitaxial strain, the oxygen deficient layers can order (a) parallel or (b) perpendicular to the substrate, with the pseudocubic orientations shown in (c) and (d), respectively.

We find that, in agreement with experimental results of the bulk phases, the Pbcm and Pnma phase are the lowest energy (and thus equilibrium) structures for SrFeO and CaFeO, respectively. Furthermore, we find that the parallel (or perpendicular) ordering is preferred under tensile (or compressive) strain; additionally, this switch occurs due to which ordering maximizes the intralayer tetrahedral chain distance under a specific strain state, analogously to the bulk phases. Finally, we report that the band gap of these materials is heavily influenced by epitaxial strain owing to strain-induced changes to the intralayer bond angles. Although strain is well known to influence the band gap via control of the octahedral rotations in O perovskites, the alternating octahedra-tetrahedra layers in the brownmillerites allow for a more complex coupling between the two. We show that, similar to the O perovskites, an alteration of the –O– bond angles causes this response; unlike perovskites, however, it is the angle between the tetrahedrally and octahedrally coordinated irons which controls the band gap. The band gap of the compounds in the parallel orientation increases under increasing tensile strain, but decreases in the perpendicular orientation, a discrepancy that arises from how the response of the out-of-plane lattice parameter to strain affects this bond angle differently in the two orientations.

Figure 4: The three characteristic angles of the O brownmillerite structure (a). Rotations of the tetrahedral chains, of the octahedral network, and between the tetrahedral and octahedral layers are given by , , and , respectively. These three angles are also sufficient to describe the case when the tetrahedral chains order parallel to the substrate under biaxial strain. In the perpendicular orientation (b), however, the changes in the out-of-plane lattice parameter owing to the strain state splits the octahedral and tetrahedral rotation angles.

Ii Computational Methods

All investigations were performed using density functional theory as implemented in the Vienna ab-initio Simulation Package (VASP).Hohenberg and Kohn (1964); Kresse and Hafner (1993); Kresse and Furthmüller (1996) We used projector augmented-wave (PAW) potentials with the PBEsol functional, with valence electron configurations of for Ca, for Sr, for Fe, and for O.Blöchl (1994); Perdew et al. (2008) A plane-wave cutoff of 500 eV and a 757 Monkhorst-Pack mesh was used during the structural relaxations.Monkhorst and Pack (1976) We applied a Hubbard correction of 5 eV using the Dudarev formalism to treat the correlated Fe states; we also enforced a G-type anti-ferromagnetic collinear spin ordering on the Fe atoms.Dudarev et al. (1998) Symmetry-adapted mode decompositions were performed using the ISODISTORT tool, part of the ISOTROPY software suite.Campbell et al. (2006) Atomic structures were visualized using VESTA.Momma and Izumi (2011)

To simulate the application of epitaxial strain by growth on a cubic [001] terminated perovskite substrate with a square surface net, we fix the and lattice parameters to be equal and allow the out-of-plane axis and ions to fully relax (adopted from the approach of Ref. 32). The , , and phases of CaFeO and the and phases of SrFeO, in both the parallel and perpendicular orientation were strained from -3% to 3% in increments of 1%. Because of the difference in size and equilibrium volume of the CaFeO and SrFeO unit cells, application of the same percent strain results in different pseudocubic lattice parameters (a) for the two structures; for this reason, we report the strain in terms of rather than in terms of percentage.

Iii Results and Discussion

iii.1 Polyhedral Rotation Definitions

To characterize the brownmillerite structures, we consider three types of rotation angles: the angle between (i) the FeO tetrahedra (), (ii) the FeO octahedra (), and (iii) the tetrahedra and octahedra (). We report these angles as , where the definition of ( = , , or ) is shown in Figure 4; in this case, a larger angle indicates a larger distortion of the relative bond away from 180. In the bulk case, and the case of parallel orientation of vacancies under strain, these three angles are sufficient to describe the structure (Figure 4a). In the perpendicular orientation, however, the applied strain and response of the out-of-plane lattice parameter now affect the tetrahedra and octahedra in different ways. To capture this, we divide and into two unique angles defined by in-plane (i.p.) and out-of-plane (o.o.p.) components (Figure 4b).

SrFeO ( = 3.8 D, =0.976)
Symmetry (meV/f.u.) (Å) (Å) (Å) () () () (Å) () (eV)
I2bm 12.6 5.501 15.402 5.659 24.48 3.70 15.41 5.0977 18.79 2.19
0 5.503 15.407 11.311 24.54 4.43 15.39 5.0988 19.07 2.15
22.7 5.499 15.413 5.659 24.49 3.64 15.31 5.0971 19.03 2.09
CaFeO ( = 1.7 D, =0.923)
Symmetry (meV/f.u.) (Å) (Å) (Å) () () () (Å) () (eV)
16.7 5.381 14.617 5.579 27.92 6.538 20.34 5.0173 11.16 2.16
23.3 5.386 14.627 11.155 28.16 4.909 19.90 5.0476 10.85 2.13
Pnma 0 5.397 14.632 5.561 27.23 8.032 20.45 4.9941 10.73 2.07
Table 1: The energetics and structure of bulk SrFeO and CaFeO. The tolerance factor () is defined by Equation 2 in the text. The energy difference between the different tetrahedral chain ordering structures is given as ; each energy is given as the difference in meV between that phase and the lowest energy phase for each compound normalized to the number of formula units. The , , and lattice parameters are given in Angstroms. The rotations of the tetrahedra, octahedra, and between the octahedra and tetrahedra are given in degrees as , , and , respectively; each is defined in Figure 4. The average intralayer separation of tetrahedral chains is (defined in Figure 5), and the deviation in the bond lengths of an octahedra is given by . The band gap () of each structure is given in eV.

iii.2 Bulk Phases

We first investigated the bulk phases of SrFeO and CaFeO with the three tetrahedral chain orderings shown in Figure 2. The main results are summarized in Table 1. In the case of SrFeO, we found that centrosymmetric is the lowest energy structure, followed by , with being the highest. In CaFeO, we found the structure to be lowest in energy, followed by and . Each polymorph is separated from the other two by a small amount of energy (, Table 1), indicating that the formation of a right- or left-handed tetrahedral chain may be equally probable. Furthermore, the lattice parameters, rotation angles, and band gaps vary only slightly between orderings. Between the two chemistries, CaFeO has a smaller unit cell and larger rotation angles than SrFeO, which is due to the smaller size of the Ca cation.

Experimentally, the structure of SrFeO has been highly contested. Initial structure refinements on powder samples ambiguously supported assignment of both completely disordered tetrahedral chains (space group ) or pure left- or right-handed ordering (space group ); this material was thus theorized to display symmetry locally, but with random ordering taking place over longer length scales. This was challenged, however, by transmission electron microscopy results showing clear intralayer alternation of tetrahedral chains.D’Hondt et al. (2008) Additionally, more recent neutron diffraction experiments on single crystals grown by the floating zone method have indicated that is indeed the preferred structure type for SrFeO. Auckett et al. (2012, 2013) Furthermore, all of these recent experiments are supported by the aforementioned results of our ab initio calculations; the small energy difference between the and structures, however, indicate that intergrowths of the phases is not out of the question. In contrast to the ambiguity of SrFeO, the structure of CaFeO is well known to form in the phase,Krüger et al. (2009) again in agreement with our theoretical results.

What factors lead to and stabilize the preferred ground state in different brownmillerite compounds? In 2005, Abakumov et al. put forth the idea that the twisting of tetrahedral chains away from the undistorted 180 orientation creates local dipole moments, with larger rotations producing larger dipoles.Abakumov et al. (2005) Hadermann and Abakumov et al. further suggested that the distance (i.e., the length of the axis) between the tetrahedral layers is also an important factor to consider.Hadermann et al. (2007) Parsons et al. then recognized that each tetrahedral ordering scheme distorts the octahedra in different ways; the fact that the octahedra are not connected out-of-plane (along ) causes the apical oxygen atoms to displace more than the equatorial ones, which creates a ‘shearing’ effect from this non-rigid rotation. Generally, the phase causes the least octahedral (elastic) distortion, followed by , with causing the most. They then rationalized these arguments into a “structure map” relating the observed phase of different brownmillerites to these factors, followed by a classification of several known compounds into this scheme.Parsons et al. (2009) Although these observations have been key in building an understanding of structural trends in brownmillerite oxides, and are corroborated by some recently synthesized brownmillerite phases (such as CaCrO),Arevalo-Lopez and Attfield (2015)discrepancies in this structure map show there are additional effects which should be considered. CaFeCoO and CaCoO, for example, both display the rather than the structure-map predicted structure.Ramezanipour et al. (2010); Zhang et al. (2014)

We now seek to explain the stability of these materials’ preferred ground state phase in terms of local structure. The tetrahedral chain ordering configuration preferred by the ground state can be summarized as a complex competition between two primary energetic factors: (i) separation of the tetrahedral chains (i.e., minimization of electrostatic repulsion) and (ii) distortion of the nominally regular O octahedra (minimization of elastic strain energy). The three different ordering schemes shown in Figure 2 better maximize either factor (i) or (ii), at the expense of the other. Following the approach of Zhang et al.,Zhang et al. (2014) we can assign a magnitude to the local dipole generated by the tetrahedral rotations (, Table 1, given in units of Debye). In compounds with large , factor (i) becomes the quantity of interest to maximize; rather than considering the separation along , however, we quantify this by defining the average intralayer separation of the tetrahedral chains as (shown in Figure 5). Competing with this is factor (ii), i.e., the regularity in the octahedra. We use the averaged sum-of-squares difference between the measured bond lengths () and the average bond length () in the octahedra to quantify this:

(1)

For small values of , factor (ii) becomes the critical quantity to optimize, and minimizing becomes more important than maximizing .

Figure 5: The intralayer chain separation in the brownmillerite structure. The average separation distance is given by , which is defined as the average of the two distances between Fe atoms of different chains ( and ).

Interestingly, we found that although SrFeO has smaller rotations, it has a larger chain dipole ( = 3.8 D) than CaFeO ( = 1.7 D); generally, one would expect smaller rotations to generate a smaller dipole. This is due to the fact that the electric polarization generated by the apical oxygen atoms tends to cancel that from the equatorial oxygen atoms in the tetrahedra; however, the smaller rotations of the octahedra in SrFeO means this cancellation happens to a lesser degree, increasing . Again, at large values of , the need to separate the dipoles, factor (i), overcomes the need to have regular octahedra, factor (ii). SrFeO therefore exhibits the structure, which allows for the best average in-plane separation (, Table 1) of the large dipoles. In CaFeO, the larger octahedral rotations distort the octahedra more in the presence of tetrahedral chains; this, in combination with the small chain dipole, therefore gives more importance to the phase which keeps the octahedra most regular (, Table 1). In this case, that is the structure.

Another approach to understanding these energetic competitions is to consider the the Goldschmidt tolerance factor.Goldschmidt (1926) This quantity is given by:

(2)

where , , and is the radius of the -site atom, -site atom, and oxide anion, respectively.111Although this is generally intended for use in perovskites, it is also applicable to perovskite-derived structures such as these brownmillerites. An ideal undistorted (cubic or tetragonal) structure will have =1; the further the tolerance factor deviates from 1, the more the structure is likely to distort, and the larger the octahedral rotations will be. In CaFeO (=0.923), the phase least distorts the octahedra (as reflected in in Table 1), and is therefore the most stable. As increases, the need to maximize the separation between dipoles overcomes the steric packing driving force for octahedral rotations and hence they decrease; because best maximizes this distance ( in Table 1), it is the preferred phase for the larger SrFeO (=0.976).

Finally, despite the structural differences between the bulk SrFeO and CaFeO phases, the DFT-PBEsol (indirect -X) band gap remains nominally the same ( 2.10 eV) across changes in chemistry and tetrahedral ordering. This is due to the fact that O states make up the top of the valence band, while the bottom of the conduction band is made up of Fe states, making the band gap largely independent of -site chemistry. A more detailed analysis of the changes in the electronic gap is given for the thin film cases below.

Figure 6: Energy of the different tetrahedral chain ordered SrFeO (left) and CaFeO (right) structures as a function of epitaxial strain (top panels). In both cases, the parallel vacancy ordering (filled symbols) is stabilized under tensile strain, while perpendicular (empty symbols) is stabilized under compressive. This change in stabilization occurs at the point where either the parallel or perpendicular phase maximizes the average intralayer tetrahedral chain separation (, middle panels) and minimizes the octahedral distortion effect (, bottom panels).

iii.3 Strained Phases

We next investigated the crystal and electronic structure of SrFeO and CaFeO under epitaxial strain. As mentioned previously, we must now consider the orientation of the vacancies as another degree of freedom (i.e., whether the vacancy layers are parallel or perpendicular to the substrate, Figure 3), in addition to tetrahedral chain rotation and ordering. First, we find that when SrFeO is constrained to a substrate, it retains the ground state in both parallel (filled symbols) and perpendicular (empty symbols) substrate-vacancy orientations (Figure 6a, top), a fact that can be explained using the same arguments presented for the bulk phase. However, we also find that the perpendicular configuration of oxygen-deficient layers is stabilized over the parallel arrangement under small amounts of compressive strain. This is due to the fact that increasing compressive strain decreases the intralayer separation between tetrahedral chains if the vacancies are ordered parallel to the substrate (i.e., becomes more energetically unfavorable), but increases if the vacancies are perpendicular. The strain value at which the perpendicular ordering becomes more stable exactly coincides with the values at which the intralayer separation becomes greater (Figure 6a, middle) and the octahedral distortions become smaller (Figure 6a, bottom) than that of the parallel ordering.

One important detail to note is that SrFeO has a relatively large pseudo-cubic lattice parameter (); only with some of the largest commercially available substrates can it be placed under tensile strain and have the parallel orientation be stabilized. Many experimental observations agree with our prediction of the energetic stability of vacancy orientation. Growth of SrFeO near the transition point, such as on SrTiO ( = 3.91 Å) shows a competition between the two orientations,Shimakawa et al. (2010) whereas growth on larger substrates stabilizes the parallel orientation, such as on KTaO ( = 3.99 Å).Inoue et al. (2008)

When CaFeO is placed under epitaxial strain, the phase remains lowest in energy, while the and structures become much closer in energy and strongly compete. As with SrFeO, the tetrahedral layers in CaFeO switch to a perpendicular orientation under compressive strain, and parallel under tensile (Figure 6b, top). Once again, this occurs due to the perpendicular orientation maximizing the distance between intralayer tetrahedral chains and minimizing octahedral distortions, , under compression (Figure 6b, middle and bottom). Although the phase minimizes octahedral shearing as in the bulk phase, the very small differences in between the strained phases means that it cannot be the only controlling feature; instead there is a complex interplay between the various structural descriptors which produces the observed ground state. The fact that CaFeO has a smaller pseudo-cubic lattice parameter than SrFeO means that the parallel phase is experimentally accessible with much more modest strain. Experimental results on thin films of CaFeO show that the vacancies order perpendicularly when grown on LaSrAlO (LSAO, = 3.75 Å) and LaAlO ( = 3.79 Å), but order parallel on LSAT ( = 3.87 Å) and SrTiO ( = 3.91 Å), again in agreement with these theoretical results.Rossell et al. (2004); Inoue et al. (2010) Interestingly, the stabilization of the perpendicular phase under compressive strain and parallel phase under tensile strain does not hold across all brownmillerite oxide chemistries; in the cobaltates, for example, the trend is reversed.

We next look at the structural evolution of these compounds under strain. For the structures with the parallel orientation, there are only the three bond angles defined previously to consider (Figure 4). Under increasing tensile strain, the FeO tetrahedral chains become less distorted (decreasing Fe-O-Fe bond angle), while the octahedral network and connections between the tetrahedral and octahedral layers, becomes more distorted (increasing Fe-O-Fe bond angle). It should come as no surprise that this trend holds across all three types of ordered phases, as they are all very structural similar with the exception of the relative orientation of tetrahedral chains (Figure 7). Additionally, the chemistry of the -site, although influencing the magnitude of the tilts, does not affect this trend.

Figure 7: The effect of strain on the tilt angles (as defined in Figure 4) of the different SrFeO (left) and CaFeO (right) structures with both parallel and perpendicular vacancy orientation.

When the oxygen-deficient layers reorient to become perpendicular to the substrate, there are now two more angles to consider. In the previous geometries, only one angle of the tetrahedra and octahedra had to be considered owing to the fact that the equatorial oxygen atoms of each were in the plane of epitaxial strain. Now these same atoms are oriented such that they are affected by both the plane of epitaxial strain and the strain-induced changes to the out-of-plane lattice parameter. In order to get a full understanding of the structural distortions in this case, we separate the tetrahedral and octahedral angles into in-plane and out-of-plane components. In this perpendicular orientation, increasing tensile strain increases the out-of-plane component of the octahedral and tetrahedral angles, while decreasing the in-plane component, as well as the angle between the layers.

Finally, the band gap of both materials is strongly influenced by strain, ranging from 1.8 eV to 2.6 eV for SrFeO (Figure 8a) and 1.6 eV to 2.5 eV for CaFeO (Figure 8b). In both compounds, increasing tensile strain results in an increase of the band gap for the parallel orientation of vacancies, but interestingly, a decrease in the perpendicular orientation. This is due to how an increase in the lattice parameters influences the connectivity of the tetrahedrally and octahedral coordinated iron atoms (i.e., ). For the films with the parallel vacancy orientation, deviates further away from 180 as tensile strain increases; this results in decreased overlap of the Fe -orbitals and O -orbitals, giving a higher band gap. Figures 8c and 8d show, as an example, the difference in the band gap of parallel-oriented SrFeO at 2% (2.43 eV) and -2% (2.00 eV). The opposite effect occurs in the perpendicular case, where a decrease in provides better overlap and thus a smaller band gap through increased bandwidth.

Figure 8: The band gap of (a) SrFeO and (b) CaFeO are strongly influenced by epitaxial strain; the electronic gap for thin films structures with vacancies ordered parallel to the substrate (filled symbols) increases as tensile strain increases, but decreases in the perpendicular orientation (empty symbols). This electronic structure response occurs owing to the manner in which strain affects the angle between the tetrahedral and octahedral layers. The structure of SrFeO with vacancies parallel to the substrate, for example, has a 0.3 eV larger band gap under (c) 2% tensile strain when compared to (d) 2% compressive strain as seen by the change in the atom-resolved densities of states.

iii.4 Comparison to Perovskite Oxides

The fact that O octahedra in perovskite oxides form a flexible corner-connected network (Figure 1a) allows them to easily rotate in space about the different crystallographic axes. The size of these rotations directly affect the magnitude of the –O– bond angles, which in turn impacts many electronic and magnetic properties. Although there are 15 distinct ways in which the octahedra can cooperatively rotate while retaining connectivity (as identified by Glazer),Glazer (1972) the vast majority exhibit either an orthorhombic or rhombohedral tilt pattern (given by or in Glazer notation, respectively). A high degree of control over the electronic structure can be achieved by using epitaxial strain (or chemical substation, as captured by ) to control these rotations, owing primarily to the strong coupling between the lattice and electronic degrees of freedom in perovskites (Figure 9a);Vailionis et al. (2011); Rondinelli and Spaldin (2011); Rondinelli et al. (2012); Johnson-Wilke et al. (2013) as mentioned previously, buckling of the –O– bond away from a linear 180 configuration (i.e., increasing the magnitude of the octahedral rotations) decreases the overlap between the O and metal orbitals, thereby increasing the band gap in insulating compounds or inducing bandwidth-driven metal-insulator transitions.Eng et al. (2003); Amat et al. (2014); Filip et al. (2014); Aschauer and Spaldin (2014); Li et al. (2015); Imada et al. (1998)

Figure 9: The effect of different stress stimuli (ionic size or chemical pressure [captured by ] and epitaxy) on various structure descriptors, which combine to produce the equilibrium crystal structure in (a) perovskite and (b) brownmillerite oxides.

As we have shown, the distinct alternating tetrahedral and octahedral layers in brownmillerites allows for many more structural degrees of freedom than perovskites. Application of the same forces (chemical pressure and epitaxial strain) now affects the interlayer separation of tetrahedra (i.e., lattice parameter), as well as the rotations (connectivity) of the different polyhedra (given by , , and ); each of these in turn influences the octahedral distortions (), the intralayer dipole separation (), and the magnitude of the local tetrahedral dipoles (). The balance of these different factors, which is shown schematically in Figure 9b, is then what governs the equilibrium structure—the tetrahedral chain ordering and, for the case of thin films, the orientation of the vacancies relative to the substrate.

A feature implicitly indicated in Figure 9 is that the electronic properties of these oxides are also a structural consequence; hence, control over the structural descriptors makes it possible to control the electronic response. Indeed, the band gaps of the brownmillerites are highly sensitive to rotations of the polyhedra; like the perovskites, the gap opens as the rotations increase owing to a change in orbital overlap. Unlike perovskites, however, it is not solely a single –O– bond angle controlling the electronic structure, which is due to the breaking of the structural topology by the oxygen-vacant (tetrahedral) layers. For the brownmillerite oxides, it is the out-of-plane angle between the O tetrahedra and O octahedra, given by (or, alternatively, –O–), that controls the gap and band edge character. Furthermore, strain affects the band gap of parallel or perpendicularly oriented brownmillerites in completely opposite (asymmetric) ways owing to the response of to the biaxial strain state. Although strain has been used to control functional properties in perovskites, it appears to induce even more interesting responses in brownmillerites owing to the additional structural degrees of freedom present.

Iv Conclusion

Using first principles density functional theory calculations, we investigated the brownmillerite compounds SrFeO and CaFeO. These anion deficient materials offer many more degrees of freedom than the related perovskite structures, increasing the structural complexity greatly. The symmetry of these structures is determined by the relative ordering of left- and right-handed tetrahedral chains; which ordering scheme preferred, however, is determined by the interplay of several structural factors. Although previous studies have attempted to characterize the various members of this family, here we clearly demonstrate how the tolerance factors, polarizations generated by rotations of FeO tetrahedra, distortions of FeO octahedra, and intralayer chain separation interact to produce the observed equilibrium phases.

Furthermore, we show the crystal and electronic structure of these phases are highly tunable using epitaxial strain. We find that under compressive strain, the preferred ordering of vacancies (tetrahedral FeO chains) changes from parallel to perpendicular when the separation between the change becomes better maximized. The rotation angles are also strongly influenced, resulting in a increase (or decrease) in the band gap for the parallel (or perpendicular) orientation. While this study is by no means comprehensive in scope, we hope that the framework presented here encourages the consideration of additional structural metrics (especially intralayer separation) in future studies and helps provide greater insight into this complex family of materials. We can now harness this knowledge and understanding of the atomistic mechanisms behind the coupling of the crystal and electronic structure in brownmillerites to design electronic function and realize new materials platforms for thin film devices.

V Acknowledgments

We wish to thank members of the Materials Theory and Design Group, as well as D. Fong, for useful discussions. J.Y. and J.M.R. were supported by the U.S. DOE, Office of Basic Energy Sciences (BES), DE-AC02-06CH11357. DFT calculations were performed on hardware supported by Drexel’s University Research Computing Facility, and the CARBON cluster at the Center for Nanoscale Materials (Argonne National Laboratory, also supported by DOE-BES DE-AC02-06CH11357) under allocation CNM39812.

References

  • Kendall et al. (1995) K. R. Kendall, C. Navas, J. K. Thomas,  and H.-C. zur Loye, Solid State Ionics 82, 215 (1995).
  • Boivin and Mairesse (1998) J. C. Boivin and G. Mairesse, Chem. Mater. 10, 2870 (1998).
  • Rolle et al. (2005) A. Rolle, R. N. Vannier, N. V. Giridharan,  and F. Abraham, Solid State Ionics 176, 2095 (2005).
  • Shaula et al. (2006) A. L. Shaula, Y. V. Pivak, J. C. Waerenborgh, P. Gaczyñski, A. A. Yaremchenko,  and V. V. Karton, Solid State Ionics 177, 2923 (2006).
  • Orera and Slater (2010) A. Orera and P. R. Slater, Chem. Mater. 22, 675 (2010).
  • Antipov et al. (2004) E. V. Antipov, A. M. Abakumov, A. M. Alekseeva, M. G. Rozova, J. Hadermann, O. I. Lebedev,  and G. Van Tendeloo, Phys. Status Solidi A 201, 1403 (2004).
  • Sullivan and Greaves (2012) E. Sullivan and C. Greaves, Mater. Res. Bull. 47, 2541 (2012).
  • Tarasova et al. (2013) N. A. Tarasova, Y. V. Filinkova,  and I. E. Animitsa, Russ. J. Electrochem. 49, 45 (2013).
  • Battle et al. (1988) P. D. Battle, T. C. Gibb,  and P. Lightfoot, J. Solid State Chem. 76, 334 (1988).
  • Abakumov et al. (2003) A. M. Abakumov, A. M. Alekseeva, M. G. Rozova, E. V. Antipov, O. I. Lebedev,  and G. V. Van Tendeloo, J. Solid State Chem. 174, 319 (2003).
  • Lazic et al. (2008) B. Lazic, H. Krüher, V. Kahlenberg, J. Konzett,  and R. Kaindl, Acta Cryst. B64, 417 (2008).
  • Krüher and Kahlenberg (2005) H. Krüher and V. Kahlenberg, Acta Cryst. B61, 656 (2005).
  • Klenov et al. (2003) D. O. Klenov, W. Donner, B. Foran,  and S. Stemmer, Appl. Phys. Lett. 82, 3427 (2003).
  • Gazquez et al. (2013) J. Gazquez, S. Bose, M. Sharma, M. A. Torija, S. J. Pennycook, C. Leighton,  and M. Varela, APL Mater. 1, 012105 (2013).
  • Inoue et al. (2010) S. Inoue, M. Kawai, N. Ichikawa, H. Kageyama, W. Paulus,  and Y. Shimakawa, Nature Chem. 2, 213 (2010).
  • Schmidt and Campbell (2001) M. Schmidt and S. J. Campbell, J. Solid State Chem. 156, 292 (2001).
  • Krüger et al. (2009) H. Krüger, V. Kahlenberg, V. Petříček, F. Phillipp,  and W. Wertl, J. Solid State Chem. 182, 1515 (2009).
  • Auckett et al. (2012) J. E. Auckett, A. J. Studer, N. Sharma,  and C. D. Ling, Solid State Ionics 225, 432 (2012).
  • Auckett et al. (2013) J. E. Auckett, A. J. Studer, E. Pellegrini, J. Ollivier, M. R. Johnson, H. Schober, W. Miiller,  and C. D. Ling, Chem. Mater. 25, 3080 (2013).
  • Takeda et al. (1968) T. Takeda, Y. Yamaguchi, S. Tomiyoshi, M. Fukase, M. Sugimoto,  and H. Yamamoto, J. Phys. Soc. Jpn. 24, 446 (1968).
  • Takeda et al. (1969) T. Takeda, Y. Yamaguchi, J. Watanabe, S. Tomiyoshi,  and H. Yamamoto, J. Phys. Soc. Jpn. 26, 1320 (1969).
  • Galakhov et al. (2010) V. R. Galakhov, E. Z. Kurmaev, K. Kuepper, M. Neumann, J. A. McLeod, A. Moewes, I. A. Leonidov,  and V. L. Kozhevnikov, J. Phys. Chem. C 114, 5154 (2010).
  • Hohenberg and Kohn (1964) P. Hohenberg and W. Kohn, Phys. Rev. 136, B864 (1964).
  • Kresse and Hafner (1993) G. Kresse and J. Hafner, Phys. Rev. B 47, 558 (1993).
  • Kresse and Furthmüller (1996) G. Kresse and J. Furthmüller, Comput. Mater. Sci. 6, 15 (1996).
  • Blöchl (1994) P. E. Blöchl, Phys. Rev. B 50, 17953 (1994).
  • Perdew et al. (2008) J. P. Perdew, A. Ruzsinszky, G. I. Csonka, O. A. Vydrov, G. E. Scuseria, L. A. Constantin, X. Zhou,  and K. Burke, Phys. Rev. Lett. 100, 136406 (2008).
  • Monkhorst and Pack (1976) H. J. Monkhorst and J. D. Pack, Phys. Rev. B 13, 5188 (1976).
  • Dudarev et al. (1998) S. L. Dudarev, G. A. Botton, S. Y. Savrasov, C. J. Humphreys,  and A. P. Sutton, Phys. Rev. B 57, 1505 (1998).
  • Campbell et al. (2006) B. J. Campbell, H. T. Stokes, D. E. Tanner,  and D. M. Hatch, J. Appl. Cryst. 39, 607 (2006).
  • Momma and Izumi (2011) K. Momma and F. Izumi, J. Appl. Cryst. 44, 1272 (2011).
  • Zayak et al. (2006) A. T. Zayak, X. Huang, J. B. Neaton,  and K. M. Rabe, Phys. Rev. B 74, 094104 (2006).
  • D’Hondt et al. (2008) H. D’Hondt, A. M. Abakumov, J. Hadermann, A. S. Kalyuzhnaya, M. G. Rozova, E. V. Antipov,  and G. V. Van Tendeloo, Chem. Mater. 20, 7188 (2008).
  • Abakumov et al. (2005) A. M. Abakumov, A. S. Kalyuzhnaya, M. G. Rozova, E. V. Antipov, H. J.,  and G. V. Van Tendeloo, Solid State Sci. 7, 801 (2005).
  • Hadermann et al. (2007) J. Hadermann, A. M. Abakumov, H. D’Hondt, A. S. Kalyuzhnaya, M. G. Rozova, M. M. Markina, M. G. Mikheev, N. Tristan, R. Klingeler, B. Büchner,  and E. V. Antipov, J. Mater. Chem. 17, 692 (2007).
  • Parsons et al. (2009) T. G. Parsons, H. D’Hondt, J. Hadermann,  and H. M. A., Chem. Mater. 21, 5527 (2009).
  • Arevalo-Lopez and Attfield (2015) A. M. Arevalo-Lopez and J. P. Attfield, Dalton Trans.  (2015).
  • Ramezanipour et al. (2010) F. Ramezanipour, J. E. Greedan, A. P. Grosvenor, J. F. Britten, L. M. D. Cranswick,  and V. O. Garlea, Chem. Mater. 22, 6008 (2010).
  • Zhang et al. (2014) J. Zhang, H. Zheng, C. D. Malliakas, J. M. Allred, Y. Ren, Q. Li, T.-H. Han,  and J. F. Mitchell, Chem. Mater. 16, 7172 (2014).
  • Goldschmidt (1926) V. M. Goldschmidt, Naturwissenschaften 14, 477 (1926).
  • (41) Although this is generally intended for use in perovskites, it is also applicable to perovskite-derived structures such as these brownmillerites.
  • Shimakawa et al. (2010) Y. Shimakawa, S. Inoue, M. Haruta, M. Kawai, K. Matsumoto, A. Sakaiguchi, N. Ichikawa, S. Isoda,  and H. Kurata, Cryst. Growth Des. 10, 4713 (2010).
  • Inoue et al. (2008) S. Inoue, M. Kawai, Y. Shimakawa, M. Mizumaki, N. Kawamura, T. Watanabe, Y. Tsujimoto, H. Kageyama,  and K. Yoshimura, Appl. Phys. Lett. 92, 161911 (2008).
  • Rossell et al. (2004) M. D. Rossell, O. I. Lebedev, G. V. Van Tendeloo, N. Hayashi, T. Terashima,  and M. Takano, J. Appl. Phys. 95, 5145 (2004).
  • Glazer (1972) A. M. Glazer, Acta. Cryst. B28, 3384 (1972).
  • Vailionis et al. (2011) A. Vailionis, H. Boschker, W. Siemons, E. P. Houwman, D. H. A. Blank, G. Rijnder,  and G. Koster, Phys. Rev. B 88, 064101 (2011).
  • Rondinelli and Spaldin (2011) J. M. Rondinelli and N. A. Spaldin, Adv. Mater. 23, 3363 (2011).
  • Rondinelli et al. (2012) J. M. Rondinelli, S. J. May,  and J. W. Freeland, MRS Bull. 37, 261 (2012).
  • Johnson-Wilke et al. (2013) R. L. Johnson-Wilke, D. Marincel, S. Zhu, M. P. Warusawithana, A. Hatt, J. Sayre, K. T. Delaney, R. Engel-Herber, C. M. Schlepütz, J.-W. Kim, V. Gopalan, N. A. Spaldin, D. G. Schlom, P. J. Ryan,  and S. Trolier-McKinstry, Phys. Rev. B 88, 174101 (2013).
  • Eng et al. (2003) H. W. Eng, P. W. Barnes, B. M. Auer,  and P. M. Woodward, J. Solid State Chem. 175, 94 (2003).
  • Amat et al. (2014) A. Amat, E. Mosconi, E. Ronca, C. Quarti, P. Umari, M. K. Nazeeruddin, M. Grätael,  and F. D. Angelis, Nano Lett. 14, 3608 (2014).
  • Filip et al. (2014) M. Filip, G. E. Eperon, H. J. Snaith,  and F. Giustino, Nature Commun. 5, 5757 (2014).
  • Aschauer and Spaldin (2014) U. Aschauer and N. A. Spaldin, J. Phys.: Condens. Matter 26, 122203 (2014).
  • Li et al. (2015) H. Li, I. E. Castelli, K. S. Thygesen,  and K. W. Jacobsen, Phys. Rev. B 91, 045204 (2015).
  • Imada et al. (1998) M. Imada, A. Fujimori,  and Y. Tokura, Rev. Mod. Phys. 70, 1039 (1998).
Comments 0
Request Comment
You are adding the first comment!
How to quickly get a good reply:
  • Give credit where it’s due by listing out the positive aspects of a paper before getting into which changes should be made.
  • Be specific in your critique, and provide supporting evidence with appropriate references to substantiate general statements.
  • Your comment should inspire ideas to flow and help the author improves the paper.

The better we are at sharing our knowledge with each other, the faster we move forward.
""
The feedback must be of minimum 40 characters and the title a minimum of 5 characters
   
Add comment
Cancel
Loading ...
244083
This is a comment super asjknd jkasnjk adsnkj
Upvote
Downvote
""
The feedback must be of minumum 40 characters
The feedback must be of minumum 40 characters
Submit
Cancel

You are asking your first question!
How to quickly get a good answer:
  • Keep your question short and to the point
  • Check for grammar or spelling errors.
  • Phrase it like a question
Test
Test description