Departamento de Química Física y Analítica

Universidad de Oviedo, 33006-Oviedo, Spain

email: victor@carbono.quimica.uniovi.es

Several important differences appear, from the point of view of AIM theory, between gas phase molecules and crystalline solids:

- atomic basins in solids have well defined boundaries and encompasse a finite volume;
- whereas ring and cage CPs are rare in most organic molecules, they are quite abundant in crystals;
- as a consequence of the above, the molecular graph of a solid can be very complicated and, what is more important, it gives only a very poor image of the topological properties of the electronic density.

In this report we discuss some of the most significant features of
the topology of the electronic density in 120 alkali-halide perovskites
*AMX3* (*A*: Li, Na, K, Rb, Cs;
*M*: Be, Mg, Ca, Sr, Ba, Zn; *X*: F, Cl, Br, I).
This work is part of an ongoing effort to determine and analyze the
structural and chemical stability of the *AmMnXo* compounds.
Consequently, one of our motivations in applying AIM theory to the
analysis of the perovskites was to determine whether a connection
between stability and electronic density topology exists or not.

The *ab initio* Perturbed Ion (aiPI)
[6,7]
method has been used to determine the best geometry for each crystal.
Best available Slater Type function (STO) basis sets have been used for
all ions. The unrelaxed hard Coulomb hole formalism (uCHF) has been used to
estimate the correlation energy [8],
but the crystal wavefunction has been obtained at the Hartree-Fock level,
not being modified by the correlation estimation procedure.
All coulomb interactions have been integrated exactly. Interionic exchange
and projection operators, on the other hand, have been accounted for neighbors
up to 25 bohr away.

The perovskite structure [Cubic, Pm3m, *A* at (1/2,1/2,1/2),
*M* at (0,0,0), and *X* at (1/2,0,0),
See Fig. 1]
fixes all geometrical parameters but one: the cell side length *a*.
We have optimized *a* for all the 120 compounds using a simplex
method.

The ionic wavefunctions obtained from a final aiPI calculation at the
optimal geometry have been used in the `critic` program
[9]
to determine the crystal wavefunction for each crystal. Ions up to 3
cell side lengths contribute to the wavefunction at any point.
The program implements a new algorithm to locate automatically all
critical points (CP's) of the electronic density. The algorithm
works by first determining the irreducible zone of the Wigner-Seitz
cell (IWSZ). The IWSZ is the smallest polyhedron that reproduces the
complete crystal by the exhaustive application of the space group
symmetry. Vertices of the IWSZ are guaranteed to be CP's. Similarly,
every edge and face of the IWSZ contains at least one CP, and further
CP's could be found within the IWSZ. The search algorithm explores the
corresponding 1-D, 2-D and 3-D regions. Every time a new CP is found in
a region, the region is splitted into two or more new ones and a
further search is performed on each. As for the searching criterion, we
have found that minimizing the square of the density gradient is
far more efficient and less error prone than other navigation
techniques based on the gradient and hessian of the function.

The automatic routine has worked remarkably well in most crystals. Early runs that included an insuficient number of ions in the evaluation of the wavefunction were unable to locate some CP's in some crystals. Once this problem was solved, the only failures of the automatic procedure were: (a) false positives of points that showed rather large gradients and that were easily discarded by inspection; and (b) remarkably, Wyckoff's 3c position, which is a CP fixed by symmetry (see below), was considered doubtful in some crystals by the automatic discard criteria. Morse relationships and similarities between compounds have been analyzed to make sure that all CP's were found in each case.

Fig. 1 Crystallographic (balls and sticks) and Wigner-Seitz (transparent box) unit cells of the cubic perovskites. Dark grey balls represents

After analyzing all 120 halide perovskites, we have found that the
electronic density can be classified into one of seven differents
*topological schemes* (i.e. seven different arrangements of critical
points). Seven may appear to be a large number for a group of apparently
quite similar compounds. On the other hand, we have performed some numerical
experiments by placing two-electron imaginary ions, represented as
single 1s Slater type orbitals, in the ionic sites. By independently
varying the three orbital exponents we were able to generate a rather
large number of topological schemes, including the seven actually
obtained for the halide perovskites. This numerical experiment proved
that the physical limitation of the ion sizes effectively reduces to a
large extent the possible topological schemes.

The seven topological schemes can be organized into three families
according to the character of Wyckoff's 3c position: (a) 3c is a
bond CP in the **B** family; (b) a ring point in the
**R** family; and (c) a cage point in the **C** family.
The special positions of the Pm3m group have been included in
Table 1, and the number and positions of the
CP's in the seven topological schemes have been summarized in
Table 2.

The translationally invariant crystals are topologically equivalent to the 3-torus and, consequently, all topological schemes must satisfy Morse invariant relationships:

n - b + r - c = 1

and

n>=1, b>=3, r>=3, c>=1,

where n represents the total number of nuclei in the unit cell,
b the number of bonds, r the number of rings, and c the number
of minima or cages. On the other hand, the topological
schemes can be easily organized in terms of the
*total number of symmetrically different* CP: **T**.
All topological schemes found for the perovskites can be uniquely
identified by giving the family and value of **T**. Furthermore,
every scheme has a different **T**, except **B10**
and **C10**.

A single scheme, **B10**, forms the **B** family. The
scheme presents three different bond CP's: b4,
b1 and b2, corresponding to *A*-*A*, *M*-*X*, and *A*-*X*
bonds, respectively. The existence of the *A*-*A* bond is the most
distinctive aspect of the **B10** scheme, and it is the
consequence of two combined factors: a very large *A* to *X*
size ratio, and a large cell side length a due to the large
size of *M*. This is an unusual combination and, in consequence,
only two out of the 120 crystals belong to this scheme:
CsSrF3 and CsBaF3.

The **C** family comprises three topological schemes,
all of them having an even number of different CP's:
**C8**, **C10**, and **C12**.
The **R** family comprises three topological schemes,
all of them having an odd number of different CP:
**R9**, **R11**, and **R13**.
Both families maintain a close relationship and exhibit identical
mechanisms in going from the simplest to the most complex
scheme. Accordingly, the **C10** and **R11**
schemes are obtained from the **C8** and **R9**
ones, respectively,
by adding both a bond and a ring point at
Wyckoff's 12i position.
The addition of both a ring and a cage point at the 8g
position originates the **C12** and **R13**
schemes.

We see here a simple mechanism for increasing the complexity of a topological scheme: add new CP's in pairs, each new point being of a type with different sign in the Morse sum. Either bonds and rings, or rings and cages would do the trick. If both types of CP's appear in the same Wyckoff's position, or in two positions with identical multiplicity, the invariance required by the Morse relation is automatically fulfilled.

The **C8** and **R9** schemes, the simplest in
their respective families, present just two types of bond
CP's. The bond at Wyckoff's 6e position lies in the edges of the
cubic unit cell and constitutes a bond between the divalent metal
and the halide: *M*-*X*. The bond point in 12j, on the other
hand, represents an *A*-*X* bond. The other four schemes of the
**C** and **R** families also show a *X*-*X* bond
occupying the 12i position.

**R** is the most frequent family. Both, **R** and
**C**, families
show a decreasing number of ions in passing from the simplest
to the most complex topological scheme. The actual number of
crystals belonging to each scheme is: 21 (**C8**),
27 (**R9**), 15 (**C10**), 25 (**R11**),
12 (**C12**), and 18 (**R13**).

Wyckoff Symmetry Symmetry Position 1a Oh m3m (0,0,0) 1b Oh m3m (1/2,1/2,1/2) 3c D4h 4/mm.m (0,1/2,1/2) 3d D4h 4/mm.m (1/2,0,0) 6e C4v 4m.m (x,0,0) 6f C4v 4m.m (x,1/2,1/2) 8g C3v .3m (x,x,x) 12h C2v mm2.. (x,1/2,0) 12i C2v m.m2 (0,x,x) 12j C2v m.m2 (1/2,x,x) 24k Cs m.. (0,y,z) 24l Cs m.. (1/2,y,z) 24m Cs ..m (x,x,z) 48n C1 1 (x,y,z)

Wyckoff CsSrF3 KCaF3 LiCaF3 KMgF3 LiZnCl3 CsBeI3 LiBeI3 1a n:Sr n:Ca n:Ca n:Mg n:Zn n:Be n:Be 1b n:Cs n:K n:Li n:K n:Li n:Cs n:Li 3c b4 c1 r2 c1 r2 c1 r2 3d n:F n:F n:F n:F n:Cl n:I n:I 6e b1 b1 b1 b1 b1 b1 b1 6f --- --- c3 --- c3 --- c3 8g c2 c2 c2 c2 c2 c2 c2 --- --- --- --- --- r4 r4 --- --- --- --- --- c4 c4 12h r5 --- --- --- --- --- --- 12i c5 --- --- r3 r3 r3 r3 --- --- --- b3 b3 b3 b3 12j b2 b2 b2 b2 b2 b2 b2 24k --- --- --- --- --- --- --- 24l --- --- --- --- --- --- --- 24m r1 r1 r1 r1 r1 r1 r1 48n --- --- --- --- --- --- --- SchemeB10 C8 R9 C10 R11 C12 R13

The attraction basin of a
nucleus is made out of all the points such that a trajectory that starts
at the point and moves upward in the gradient field of the electronic
density ends in the nucleus. The interior of an attraction basin is then
a 3-dimensional region of the crystal with no other CP but the nucleus itself.
All non-nuclear CP's lie, therefore, on the 2-dimensional zero-flux
boundaries of the
different attraction basins of the crystal. The latter are called atomic
surfaces. The set of CP's situated on the atomic surface of
a given nucleus is said to be *related* to it. Despite
the general shape an atomic surface may display, its set of related CP's
induce a homeomorphism between the surface and a polyhedron. This relation is
established as follows: each cage point on the surface is defined as a vertex
of the associated polyhedron. Every bond point is mapped into a face, made up
of all the gradient lines ending up at that point. Last, but not least, to
each ring point we associate an edge, defined by the two only gradient lines
that die at it. If we draw onto the atomic surface all the vertices and edges of
the associated polyhedron, we may compare the actual atomic surfaces with the
ideal (planar faces and linear edges) mapped polyhedron. Though symmetry, when
present, is a very powerful means of assuring planarity and linearity of
the actual faces and edges, it is not uncommon that large curvatures do
appear in some cases.

It is interesting no note that physicists and chemists tend to think of atoms in crystals as to slightly deformed spheres. Spheres, however, do not fill the three dimensional space without gaps and are thus inappropriate approximations to the attraction basins shape in crystals. The ideal polyhedra just defined do represent a much better approach, but we have to keep in mind that in passing from curved faces and edges to linear representations some fictitious facets may appear, that is, facets that are not associated to a bond point.

The attraction basins of LiCaF3, a crystal with **R9** topology,
are depicted in Fig. 2.
We can see that the basin of Li is a rounded rhombododecahedron.
Each rhomb is associated to a Li-F bond.
The F basin only has six real
faces: four concave rhombi related to Li-F bonds, and two large and curved
squares corresponding to Ca-F bonds. In a polyhedral approximation,
every curved square would appear as a smaller square with four trapezoids
connected to it by an edge each. Were they real, the trapezoids of the
F basin would represent F-F bonds, that do not exist in
**R9**. To avoid face to face contact
between two neighbor F basins, this implying F-F bond,
the Ca basins develop nearly bidimensional
*wings* that perfectly envelop the F
basins. Apart from those wings, the Ca basin could
be described as a slightly engrossed cube. A similar behavior is
observed in **C8** and **B10** crystals.

The **C10**, **R11**, **C12**, and **R13** schemes, on the
other hand, do not suffer from this circumstance, and the face that separates
two neighbor *X* ions is a true bond. Accordingly, the *M* basin
is topologically equivalent to a cube: the basins show more or less acute
spikes on the cube vertices for **C10** and **R11**
(see Fig. 3),
and a round,
nearly spherical, shape for **C12** and **R13**
(see Fig. 4).

It is an important observation that the topological schemes having
the smallest numbers of symmetrically different CP's are the most
complicated ones in the geometrical sense. Contrarily, the schemes with
**T**=12 and **T**=13 are the simplest ones and present shapes
easily related to the classical concept of spherical cations. In all
cases the anion basin stretches to fill in the gap between cations.

Fig. 2 Attraction basins of the ions in LiCaF3, a crystal having

Fig. 3 Attraction basins of
the ions in LiZnCl3, a crystal having **R11** topological scheme.
Different colors are used for each ion: golden (Zn), green (Cl) and
fuchsia (Li).
The figure was created with `critic`
[9] and rendered with
`geomview` [13].

Fig. 4 Attraction basins of
the ions in LiBeI3, a crystal having **R13** topological scheme.
Different colors are used for each ion: golden (Be), green (F) and
fuchsia (Li).
The figure was created with `critic`
[9] and rendered with
`geomview` [13].

We can define topological ionic radii as the
distance from the nucleus to the surface of its attraction basin. It
is evident from Figs. 2 to 4
that such topological
radii do depend strongly on the direction being analyzed. Not all
directions are equally important from the chemical point of view:
the directions that contain
bonds are the most significant ones for the crystal stability. In
this way, the b1 CP, that represents a *M*-*X* bond, provides
estimated ionic radii for *M* and *X*, that we will designate
as R(M) and R1(X), respectively. Similarly, the b2 CP
represents an *A*-*X* bond, and provides the R(A) and R2(X) radii.
The b3 CP, found in many crystals, corresponds to a *X*-*X* bond
and gives R3(X).

We have found, after some initial surprise, that the ratio of ionic
radii along the *M*-*X* and *A*-*X* bond lines
completely determines the topological scheme exhibited by the crystal.
To show this we
have prepared Fig. 5, in which we have plotted the ratio
R(M)/R1(X) * versus* the ratio R(A)/R2(X), every crystal being
represented by a symbol different for each type of topological scheme.

It is observed that the **C** and **R**
topological families are decided according to the value of R(A)/R2(X).
If the *A* ion is larger than about 0.88 times the
*X* ion in the *A*-*X* bond line, the crystal belongs to the
**C** family, and it belongs to the **R** family if it is smaller.

The R(M)/R(X) ratio, on the other hand, is in control of the
topological complexity within each family: the larger *M* is
in comparison to *X*, the simpler the topological scheme appears.

It is interesting to notice that althought the topological radii behave similarly to Shannon's empirical radii, only the topological values provide an exact criterion to predict the topological family.

Fig. 5 The topological schemes are determined by the ratio of topological radii R(A)/R2(X) and R(M)/R1(X).

The integration on the ionic basins is computationally quite
demanding. The algorithm implemented in the
`critic` program [9]
involves sampling a number of rays defined by its (theta,phi)
spherical coordinates. The position of the basin surface is determined
along each ray, and a Gaussian quadrature is used to integrate with
respect to the radial coordinate for each ray. Site symmetry is used
to improve the performance of this method. A grid of
40x40x60 points on (theta,phi,r) has been used in
this work. This grid produces an accuracy better than 0.01 Å3 in
the integrated total volume of the cell, and better than 0.001 a.u. in
the cell total charge.

All perovskites behave clearly as ionic compounds, as indicated by the
topological charges (See Table IV).
The charge of the alkaline ions is very close to
the nominal **+1** value, the halides have an average charge
**Q**(*X*)=-0.95, and the alkaline earth ions vary from
**Q**(Be)=1.95 to
**Q**(Zn)=1.8.
The variability of the charge in the alkaline ions, on the other hand,
increases as we descend the Periodic Table, effect that is not
observed neither on the halides nor on the alkaline earth ions.

Several interesting facts are observed in analyzing the
average ionic radii (See Fig. 6).
First of all, the ionic size increases, within each group of ions,
with the atomic number, as it should be the case if we want to claim
any physical meaning for the topological property.
Secondly, the dispersion of ionic
radii increases, within each group of ions, as we descend in the
periodic table, following the trend of the empirical
scale of polarizabilities.
With regard to the differences between groups,
the alkaline earth ions present a rather constant radii along different
compounds,
with the noticeable exception of Ba, and halide ions
exhibit a greater variability. The most interesting fact is, however,
the large variability of radii observed for the alkaline ions, even
larger than that found for the halides, in sharp contradiction with the
polarizabilities of both groups. This circumstance suggests that the
variability of **R**(*A*) has a different origin that the
variability of **R**(*M*) and **R**(*X*). It appears that the
*A* ions are weakly binded and easily vibrate
within the cage made up of *M* and
*X* ions.

Ion charge Ion charge Ion charge be 1.9541 li 0.9970 f -0.9630 mg 1.8908 na 0.9914 cl -0.9466 zn 1.8113 k 0.9896 br -0.9490 ca 1.8634 rb 0.9852 i -0.9499 sr 1.8321 cs 0.9990 ba 1.8256Fig. 6 Average ionic radii as obtained after the volume of the attraction basin.

On a more fundamental basis, the stability of the crystal should be
addressed with respect to: (a) solid state reactions producing
compounds of different stoichiometry;
and (b) the existence of crystals with the same *AMX3* stoichiometry
but a different crystalline structure.
To our knowledge there is neither experimental nor theoretical
data regarding the thermodynamic stability of perovskites but for a
handful of compounds.

The relation between the topology of the energetic hypersurfaces connecting several crystalline structures has been previously investigated for the alkali halides [14]. Based on the definition of topological ionic radii we were able to establish a single criterion that exactly predicted the stability of the B1 and B2 structures, defined in terms of the properties of the Gibbs free energy. The relation between phase transitions and topological structure of the perovskites, albeit very interesting, is beyond the scope of this work.

On the other hand, perovskites are usually prepared by melting
a mixture of *MX2* and *AX* crystals in 1:1
stoichiometric proportions and slowly
cooling whereas the *AMX3* crystal is simultaneously grown and
extracted according to the Czochralski procedure.
Even though, to the better of our
knowledge, there is no systematic study on the energetics of the above
reaction, most of the 120 *AMX3* compounds have never been referred
to in the literature, which suggests that most of the perovskites are
unstable with respect to *MX2+AX*.

To address this problem we have determined the energy of the reaction:

*MX2*(s) + *AX*(s) ---> *AMX3*(s)

as

E = *E(AMX3)* - *E(MX2)* - *E(AX)*

where *E(compound)* is the aiPI total energy.
The fluorite structure
[Cubic, Fm3m, *M(+2)* at (0,0,0), *X(-1)* at (1/4,1/4,1/4)]
has been assumed for the *MX2* compounds, and the rock-salt structure
has been assumed for the *AX* compounds. Even though perovskite,
fluorite and rock-salt are not necessarily the most stable structures
of the three types of compounds, the difference should not be very
large nor it should modify the general trends for the whole set of
crystals.

Fig. 7 represents the reaction energy
together with the topological scheme for the 120 *AMX3* compounds.
The first thing to notice is that the crystal stability is dominated by
the identity of the *M(+2)* cation: Ba, Sr, and most
Ca perovskites are unstable, whereas most Zn and Mg,
and all Be perovskites are stable. For a given *M(+2)*,
stability is favored by having large *A(+1)* ions. The role of
*X(-1)* is more complex, but it is seen that fluorides are
different to the other
halides, either more or less stable, the chlorides, bromides and
iodides behaving rather similarly.

It is very interesting to observe in Fig. 7 that all
crystals having **R9** and **B10**,
and most crystals having **C8** topological schemes, are
unstable. Contrarily, all **C12** and most **R13**
crystals are stable. It appears that the existence of bizarre
features, like wings, in the attraction basins works against the
stability of the crystal. Alternatively, we can argue that the
formation of *X*-*X* bonds is important to stabilize the structure.
This sheds new light to the question of what is simple and what is
complex in relation to the topological structure of the electronic
density. The simple
enumeration of critical points would suggests that those topological
schemes having smallest values for **T** are the simplest ones. The
shape of the attraction basins is simpler, however, in the schemes of
large **T** and, as the analysis of the above reaction indicates,
those schemes are more favored in energetic terms.

The above results refer to the difference between quantum mechanical total energies. It corresponds, thermodynamically, to null temperature and pressure. We have investigated the role of thermal effects, up to about 900 K, on the perovskite stability and have found interesting but small effects that do not modify the general trends discussed above.

Fig. 7 Stability of the perovskite structure with respect to the decomposition into

Ionic radii along the bond paths follow systematic trends in passing from one crystal to another, even though the ionic radius of an ion in a crystal do strongly depend on the direction being considered.

Ionic basins have, essentially, a polyhedral shape, even though faces and
edges present very large curvatures in some cases.
The type and number of CP's in the unit cell is limited by the Morse
relations. The type and number of CP's in the surface
of an ionic basin is limited by the Euler relation. Both, together with
the space group symmetry, posse strict requirements on the shape of
the ionic basins. This point of view helps to explain some of the
bizarre features exhibited by the basins in some cases, particularly
the nearly bidimensional wings of the *M(+2)* basins in the
**C8**, **R9** and **B10** topological schemes.

We have found a suggestive connection between the topological
properties of the electronic density and the chemical stability of
the perovskites. In particular, we have found that the crystal tends
to be more stable, with respect to the decomposition into *MX2*
and *AX*, when there are *X*-*X* bonds and the attraction
basins of the ions are free of strange features like wings and spikes.
This view is in agreement with previous work
[14] relating the phase stability of the
B1 and B2 alkali halides to the ratios of ionic radii obtained
through topological arguments.

As a final remark, the Atoms in Molecules theory may be used to give a rigorous foundation to important historical concepts like ionicity, index of coordination, coordination polyhedron or volume of an atom or an ion in a solid. Several interesting mappings between atoms and polyhedra can be built, some of which have been examined and exploited in this work. We think that there is room in solid state thinking for the new tools and concepts emerged from AIM, and that a judicious use of them, will give new ways to correlate chemical behavior and chemical structure in solids.

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