The binary aluminum scandium clusters AlxScy with x + y = 13: when is the icosahedron retained?

Geometrical and electronic structures of the 13-atom clusters AlxScy with x + y = 13, as well as their thermodynamic stabilities were investigated using DFT calculations. Both anionic and neutral isomers of AlxScy were found to retain an icosahedral shape of both Al13 and Sc13 systems in which an Al atom occupies the endohedral central position of the icosahedral cage, irrespective of the number of Al atoms present. Such a phenomenon occurs to maximize the number of stronger Al–Al and Sc–Al bonds instead of the weaker Sc–Sc bonds. NBO analyses were applied to examine their electron configurations and rationalize the large number of open shells and thereby high multiplicities of the mixed clusters having more than three Sc atoms. The SOMOs are the molecular orbitals belonged to the irreducible representations of the symmetry point group of the clusters studied, rather than to the cluster electron shells. Evaluation of the average binding energies showed that the thermodynamic stability of AlxScy clusters is insignificantly altered as the number y goes from 0 to 7 and then steadily decreases when y attains the 7–13 range. Increase of the Sc atom number also reduces the electron affinities of the binary AlxScy clusters, and thus they gradually lose the superhalogen characteristics with respect to the pure Al13.


Introduction
During the last four decades, a very large number of both experimental and theoretical studies on atomic clusters were reported with the aim to understand their novel physical and chemical properties as well as to emphasize their abilities to be used for new promising technological applications. 1 The atomic clusters possessing high symmetry geometries have oen attracted more attention, in part due to the fact that they are expected to have an enhanced stability along with appealing features. In particular they can be considered as building blocks for assembled nanostructured materials. 1,2 Especially, many investigations found that various clusters formed by 13 atoms, including both homonuclear and heteronuclear derivatives, exist in an icosahedral shape and have interesting physicochemical properties that could lead to signicant applications. 3 For instance, to adjust the overall valence state and thereby the chemical behavior of the silicon doped aluminum Al 12 Si icosahedron, it is possible to substitute the Si atom by another dopant such as B, P and Ca, to form the superhalogen Al 12 B, super alkali metal Al 12 P, and superchalcogen Al 12 Ca, respectively. 4 Of the main group element clusters, only the aluminum clusters at this size, Al 13 , in both neutral and anionic states, are icosahedra formed by 13 homonuclear atoms, [5][6][7] that are one of the most well-known and inspiring example for superatomic clusters. 1 The anion Al 13 À exhibits 40 valence electrons in a closed shell structure and thus emerges as a magic cluster with an enhanced thermochemical stability. For its part, the neutral Al 13 , having one valence electron less than the anion Al 13 À , has a very high electron affinity exceeding those of halogen atoms and has been regarded as a superhalogen. 8,9 Stimulated by the existence of the icosahedral Al 13 , many similar structures were found by doping of various hetero-atoms into aluminum hosts. 3 A previous study using photoelectron spectroscopy combined with theoretical calculations pointed out that an icosahedral anion Al 12 Li À can be composed by replacing a surface Al atom of the icosahedron Al 13 À by a Li atom. 10 For the doped aluminum Al 12 X 2À , while the beryllium, X ¼ Be, sits at the center of an aluminum icosahedral cage due to its small atomic radius, the remaining dopants with X being an alkaline earth metal having larger atomic radius, favor its attachment outside at the surface. [11][12][13] Although the aluminum doped boron clusters B 12 Al favor a quasi-planar shape, 14 it was also found that other dopants which belong to the same group IIIA as aluminum including B and Ga, can substitute the Al atom(s) at the center of icosahedral cage Al 13 . 15,16 An investigation of the cationic clusters Al 12 X + , with X being a tetravalent atom including C, Si, Ge, Sn, and Pb, showed that except for the low symmetry structure of Al 12 C + , the remaining structures of Al 12 X + prefer an icosahedral shape. The Si and Ge atoms are encapsulated at the central position of the icosahedra Al 12 Si + and Al 12 Ge + , respectively, whereas for the Al 12 Sn + and Al 12 Pb + , the dopant substitutes an aluminum atom on a vertex of the icosahedral framework. 17 Moreover, a recent study on singly and doubly silicon doped aluminum clusters reported that both neutral and cationic states of Al 11 Si 2 keep on favoring the icosahedral shape with one Si dopant embedded at the central position, whereas the remaining Si atom substitutes an external Al position of the icosahedron Al 13 . 18 Similarly, another study of Al 12 X clusters at both neutral and cationic states, with dopant X being a pentavalent atom including P, As, Sb and Bi, also showed that the P atom prefers to be at the center of the Al 12 icosahedron whereas the rest of the dopants favor occupancy of a vertex site due to their larger size. 19 Previous studies on transition metal doped aluminum clusters also reported that an icosahedral structure can be composed by 12 aluminum atoms plus a transition metal dopant such as Co, Ni, Cu, and Zn. The atomic radius of the latter seems small enough to allow its position at the center of such a cage. 10,11,[20][21][22] A combined theoretical and experimental study on Al n V clusters 23 showed that the anionic Al 12 V À prefers a distorted icosahedral shape in which the vanadium atom occupies a convex capped site. Interestingly, Kumar and Kawazoe carried out a study using density functional theory (DFT) calculations on a doping of a Cu atom into Al 12 and discovered a perfect icosahedral Cu@Al 12 possessing a high spin state with a 3 m B magnetic moment. 22 A subsequent theoretical study found that the Al 12 Cu could play as a stable building block to form ionic salts, as shown from stable dimers, trimers, and tetramers of the Al 12 CuM 3 complex. 24 On the other hand, it appears that an icosahedral structure based on the elements of the main group IVA can be also obtained upon doping of an impurity atom onto a 12 tetravalent atom system. A theoretical study indicated that the most stable isomers of the Ge 12 M x clusters, with M ¼ Li, Na, Be, Mg, B and Al with x going from À1 to +1 and each containing 50 valence electrons, prefer a high symmetry icosahedron. 25 Particularly for the anion Ge 12 Li À , the lithium dopant was found at the central position of the icosahedral cage instead of on its surface as in the case of Al 12 Li À . 25 Goicoechea and McGrady carried out a theoretical investigation of endohedrally transition metal doped silicon MSi 12 and germanium MGe 12 clusters, and found that while MSi 12 have a hexagonal prism or a bicapped pentagonal prism shape, some MGe 12 with M being Cr, Mn, Fe, Cu, Zn, Ag, and Cd, tend to favor an icosahedral form. 26 Similarly, many icosahedra bearing an endohedrally doped metal such as tin MSn 12 and lead MPb 12 were also found from both theoretical and experimental approaches. [27][28][29][30][31] Previous investigations also demonstrated that many pure clusters formed by 13 transition metal atoms in both neutral and ionic states exist in ideal or distorted icosahedral shape, including the rst-row transition metal clusters such as Sc 13 , Ti 13 , V 13 , Cr 13 , Mn 13 and Fe 13 and heavier transition metal clusters such as Y 13 , Hg 13 , Zr 13 , Lu 13 and Hf 13 . 32-34 A characteristic difference of the latter from the main group element clusters is that most of the transition metal icosahedra possess very high total spin and thereby large magnetic moments, due to their unpaired nd electrons. Along with the homonuclear icosahedra, it was found that many doped transition metal clusters favor an icosahedral shape. Datta et al. reported from DFT calculations that the most stable isomers of vanadium doped cobalt clusters Co 13Àm V m , with m ¼ 1-4, adopt an icosahedral geometry, unlike the hexagonal symmetry preference of the pure Co 13 clusters. 35 Other theoretical studies also demonstrated that an icosahedral 13-atom structure can be formed by endohedrally doping a transition metal atom into a coinage metal cluster Cu 12 and Ag 12 . [36][37][38][39] In particular, doping of a Cr atom into Cu 12 as well as Ag 12 was shown to form a Kondo-like system that enhances the thermodynamic stability of both resulting CrCu 12 and CrAg 12 icosahedra but quenches the large magnetic moment of the dopant simultaneously. 37,39 Of the transition metal clusters possessing icosahedral geometry, the scandium-based clusters could deserve more attention because of their formal similarities with aluminumbased clusters in terms of valence electrons. As a matter of fact, the scandium element belongs to group IIIB and also has 3 valence electrons (3d 1 4s 2 ). Additionally, both Sc 13 and Al 13 are characterized by a perfect icosahedral structure. However, unlike the anion Al 13 À having a closed shell electronic structure and the neutral Al 13 exhibiting a doublet ground state, both anionic and neutral states of Sc 13 are known to exist in very high spin ground states, with the total spin magnetic moments of 18 and 19 m B , respectively. 32,40 A previous theoretical investigation of the singly aluminum doped scandium clusters Sc n Al, with n ¼ 1-8, 12, showed that the Sc n Al isomers prefer an Al substitution at a Sc position of a structure of the corresponding Sc n+1 size. In fact, the resulting doped cluster Sc 12 Al exists in a high spin state along with an icosahedral shape in which the Al dopant is put into the center. 41 Surprisingly, despite such a formal association between Sc and Al, an understanding of the geometric structure and electronic properties of the mixed Sc-Al clusters is still limited; they have not much been investigated so far. In this context, we set out to perform a detailed and systematic investigation on the binary Al-Sc clusters Al x Sc y with x + y ¼ 13, at both anionic and neutral states using DFT method, with the purpose of gaining deeper insights into the structural and electronic features of these intriguing systems. A question of interest is as to whether the icosahedral geometry, ideal or distorted, remains predominant following atomic mixture, and the identity of the central atom.

Computational methods
All standard electronic structure calculations in this study are carried out using the Gaussian 09 package. 42 The possible isomers of each cluster are searched for using different approaches. In the rst step, a stochastic genetic algorithm 43 is used to generate the possible structures of each size Al x Sc y with x + y ¼ 13. This algorithm has been used in previous studies and shown to be highly efficient for systems containing different components. 18,[44][45][46] Another way of generating the initial isomers is a manual substitution by a Sc-atom at all Al positions of the well-known icosahedron Al 13 to generate the Al 12 Sc structures, and successively for the following sizes with more Sc atoms. The search also includes the shapes of other 13-atom clusters that have previously been reported. Geometry optimizations are rst carried out to generate the rst initial set of isomers using the popular hybrid B3LYP functional in combination with the small LANL2DZ basis set. 47 The local energy minima identied with relative energies of <5 eV with respect to the corresponding lowest-lying isomer of each size are then reoptimized at various spin states using the same functional but with the larger 6-311+G(d) basis set. 48 Harmonic vibrational frequencies are subsequently calculated at this level to conrm the identity of the true local minima obtained, as well as to evaluate their zero-point energy corrections.
The lower-lying isomers of the neutral 13-atom clusters Al x -Sc y that have 39 valence electrons each, are then obtained from the corresponding anionic isomers upon removal of an electron and then geometrically optimized at different spin states. Moreover, a natural bond orbital (NBO) analysis is performed to examine the electronic conguration and thereby to rationalize the chemical bonding and magnetic properties of the clusters considered by using the NBO 3.1 program implemented in Gaussian 09. The total and local electron densities are dened as the difference between the numbers of spin-up and spindown electrons occupying the molecular/atomic orbitals of the cluster/atom.

Lower-lying isomers of binary Al-Sc clusters in both anionic and neutral states
Since there is a large number of local minima located on the potential energy surface of each size considered in different spin states, we only present here the lowest-lying isomers whose relative energies are close to the corresponding most stable structure, being <1 eV in relative energy. The shapes of Al x Sc y equilibrium structures in both anionic and neutral states, their spin states, and their relative energies obtained at the B3LYP/6-311+G(d)+ZPE level are shown in Fig. 1-3.
As for a convention, the S.x.y.Z label is used to denote the isomers in which S ¼ a and n stand for an anionic state and its corresponding neutral with a similar geometrical shape, respectively, x being the number of Al atoms and y the number of Sc atoms, and Z ¼ A, B, C. referring to the isomers with an increasing relative energy. Accordingly, the notation a.x.y.A invariably refers to the most stable anionic isomer (A) of the a.x.y series, and the n.x.y.A to its corresponding neutral.
Calculated results reveal an interesting discovery about geometrical features. All the lowest-lying Al x Sc y isomers in both anionic and neutral states, irrespective of the number x of Al atoms, have an icosahedral shape in which an Al atom is invariably situated at the cage center, whereas the remaining Al and Sc atoms form the corresponding icosahedron in different positions.
For the size x ¼ 12 Al 12 Sc À , a.12.1.A, formed by capping the Sc atom on a vertex of the bicapped pentagonal prism framework, is only 0.05 eV lower in energy than the icosahedral structure a.12.1.B in which the Sc atom is placed on a surface position of the icosahedron. However, such a relative energy gap is too small to be meaningful, and therefore both isomers can be considered as energetically degenerate. DFT results also point out some energetic degeneracies with small energy gaps of <0.1 eV for most of the (x, y) combination of the series of Al x Sc y with y > 2. These isomers have an icosahedral framework with different positions of Sc atoms on the surface and in different spin states. As stated above, a remarkable feature of Al x Sc y structures is that an Al atom is consistently found at the center regardless of the number of Al atoms. The fact that the Sc atoms occupy surface positions of the icosahedron can be understood by the smaller atomic radius of aluminum which favors the Al atom to occupy a position inside the cage. This is in agreement with a previous experimental study on the argon physisorption ability of the rst row transition metals, 49 showing that the transition metal doped clusters Al n TM + are able to attach one argon atom up to a critical cluster size n crit , with n crit ¼ 16 for TM ¼ V, Cr and n crit ¼ 19-21 for TM ¼ Ti, and undergo a geometrical transition in going from exohedrally to endohedrally doped clusters in which the transition metal atom becomes, from n crit , located inside an aluminum cage. Furthermore, this feature can be rationalized on the basis of the strength of the homo-and heteronuclear bonds between Al and Sc atoms. According to DFT calculations, the bond energies of the Al 2 , AlSc and Sc 2 dimers, also obtained at the B3LYP/6-311+G(d) level, amount to 1.2, 0.6, and 0.5 eV, respectively. Although bond energies of the dimers are expected to differ from the energies of corresponding bonds in the clusters, this result shows that in the cluster the bond between two Al atoms is much stronger than the Al-Sc and Sc-Sc bonds. In a Al x Sc y cage structure both Al and Sc atoms are arranged in such a way of favoring formation of a maximum number of strong bonds, along with a minimum number of weak bonds. Accordingly, the Al atom thus prefers to occupy the icosahedral center in order to maximize the possible number of Al-Al and Al-Sc bonds.

Electron conguration and multiplicity
Along with a consistent possession of an icosahedral shape, another typical feature is that the Al x Sc y ground electronic states are associated with high number of unpaired electrons. The search for the most stable isomers is carried out for all plausible electron spin state for each cluster composition, and the multiplicity of Al x Sc y tends to gradually increase with an increasing number of Sc atoms. For a small number of Sc atoms, y ¼ 0-3, the most stable structures of Al 12 Sc, Al 11 Sc 2 and Al 10 Sc 3 and their anions keep the lowest spin states alike the Al 13 cluster, that are singlet state for species having an even number of electrons and doublet state for those having an odd number of electrons. A competition between the low and high spin states begins to occur at the size of four Sc atoms, namely the Al 9 Sc 4 . For y ¼ 10-13, both anionic and neutral Al x Sc y structures are more stable at very high spin state in which each has nine or more unpaired electrons, approaching that of the pure scandium Sc 13 . Indeed, the most stable isomer of the latter has the highest spin states with 18 and 19 open shells for both anionic and neutral states, respectively. Fig. 4 displays the variation of the multiplicity of the binary clusters considered.
In order to rationalize the high spin states of Al x Sc y clusters and obtain a deeper understanding of their electronic structures, we now analyze the natural bond orbitals of the anions.
Each 13-atom Al x Sc y À anion has 40 valence electrons, as each of the Al and Sc atoms has three valence electrons. For Al 13 À , all of its 40 valence electrons contribute to the shell molecular orbitals resulting in a closed electron shell of [1S 2 1P 6 1D 10 2S 2 2P 6 1F 14 ], without any unpaired electron, as shown in Fig. 5. Similarly, the Al 12 Sc À , Al 11 Sc 2 À , and Al 10 Sc 3 À anions also have the same closed electron conguration of [1S 2 1P 6 1D 10 2S 2 2P 6 1F 14 ] without open shell. The clusters having up to three Sc atoms do not have any Sc-Sc bond for the reason described above, as their geometrical structures seen in Fig. 1.
In these cases, the isolation of Sc atoms around an Al environment results in a quenching of its spin upon formation of the Al-Sc bonds. In order to understand how the Al x Sc y clusters come to possess high multiplicity upon increase of the Sc atom number going from four up to thirteen, we would start examining the electron conguration of the pure Sc 13 cluster which is characterized by the highest spin multiplicity as a special reference case, and the other binary clusters with a reduced number of Sc atoms, going down to Al 9 Sc 4 , are subsequently examined.

The AlSc 12
À cluster. The most stable isomer of the AlSc 12 À anion is characterized by twelve (12) open shells, corresponding to a 13-et multiplicity. Therefore, 28 valence electrons ll the cluster shell orbitals resulting from an electron conguration of [1S 2 1P 6 1D 10 2S 2 2P 6 1F 2 SOMO 12 ] (cf. Fig. 6).  This is conrmed by the results of the local and total unpaired electrons derived from the NBO calculation, as represented in Table 2. Again, the ten SOMOs combination lead to MOs that belong to the A and E irreducible representations of a C 5V point group. The electron conguration of the Al 2  Similarly, the electron conguration based on the symmetry point group and spin multiplicity of the remaining anions can concisely be expressed in the same way as follows: The Al 3 Sc 10 À cluster (C 5v , 11-et The symmetries, spin multiplicities, and electron congurations of all anionic Al x Sc y À clusters are also summarized in     . In general, in the open shell systems of Al x Sc y À , with y ¼ 4-13, the unpaired electrons are mostly distributed on the Sc atoms located at the cage vertexes. Moreover, the spatial orbitals of the SOMOs are neither the shell molecular orbitals nor the individual AOs of any Sc atoms of the Al x Sc y À clusters, but rather the MOs that belong to the irreducible representations of the corresponding point group, depending on the geometrical symmetry of the cluster considered. As shown in Table 4, the calculation results show that all the d electrons of Sc atoms take part in cluster bonding in the Al 12 Sc À , Al 11 Sc 2 À , and Al 10 Sc 3 À clusters while the Al x Sc y À clusters contain unpaired d electrons when x is larger than three. In the clusters Al 12 Sc À , Al 11 Sc 2 À , and Al 10 Sc 3 À the Sc atoms are far apart from each other, their d electrons rather participate in formation of bonds with the Al atoms. For the Al x Sc y À (x > 3) clusters, the Sc atoms are located next to each other (see Fig. 1 and 2) and their 3d unpaired electrons are not bonded but having parallel spins that create a magnetism.
In the cluster Al 9 Sc 4 À , each of the Sc (10) and Sc (12) atoms, which are next to each other, has 0.8 unpaired electrons and these unpaired electrons mainly belong to their d AOs (see Tables 1 and 2). Therefore, it can be concluded that they do not use their single electron d AOs to form bonds with each other.
In the cluster Al 8 Sc 5 À , the Sc (9) , Sc (10) atoms are the neighbors of Sc (12) and Sc (11) ones, respectively, at a distance of 2.970Å, 0.148Å closer than the distance to the Sc (13) atom. Tables 1 and  2 show that each of the Sc (9) , Sc (10) , Sc (11) and Sc (12) atoms have $0.75 single electrons that mainly belong to their d AOs. Therefore, we can also conclude that these Sc atoms do not use their unpaired d electron to form bonds with each other.
In the Al 7 Sc 6 , the six Sc atoms next to each other forming a ring with equal Sc-Sc distance of 3.043Å. Tables 1 and 2 show that each Sc atom has $0.7 unpaired electrons and these unpaired electrons mainly belong to their d AOs.
In the case of Al 6 Sc 7 À , Al 5 Sc 8 À , we observe the same phenomenon as in previous clusters having four or more Sc atoms. Although the number of Sc atoms increases, there are still enough Al atoms in the alternative positions of the Sc atoms and their magnetism does not increase. A leap in the magnetic property is observed in subsequent clusters from Al 3 Sc 10 À , Al 2 Sc 11 À to Al 1 Sc 12 À , in which the number of Al atoms becomes sufficiently small that all the Sc atoms are located in positions next to each other with similar distance and do not use their d AOs for bonding to each other. Therefore, they exhibit 10, 10 and 12 unpaired electrons, respectively.
A special case involves the Sc 13 À where no Al atom is present and all Sc atoms do not use their d AOs, and some of their s and p AOs for bonding. As a result, the cluster is exceptionally magnetic, bearing up to 18 unpaired electrons.

Thermodynamic stability
The inherent thermodynamic stability of the 13-atom clusters Al x Sc y are now evaluated through the examination of average binding energies (E b ) which can conventionally be dened in eqn (1) and (2): Particularly for the anionic Sc 13 À , the E b can be dened by eqn (3): where E(Al), E(Al À ), E(Sc), E(Sc À ), E(Al x Sc y ), and E(Al x Sc y À ) are the total energies of the Al-atom, the anion Al À , the Sc-atom, the anion Sc À , the neutral Al x Sc y , and the anion Al x Sc y À , respectively. Since the electron affinity of the Al atom (EA(Al) ¼ 0.43 eV) 50 is larger than that of the Sc atom (EA(Sc) ¼ 0.19 eV), 51 the total energy of the anion Al À is thus used to calculate the average binding energy instead of that of the anion Sc À . All these energies are obtained from DFT calculations and the plots of E b depicted in Fig. 7a illustrate their evolution. There is no signicant change of E b values of the anions Al x Sc y À whereas those values of the neutral structures increase when y goes from 0 to 4. For y ¼ 4-7, the E b values of the anions slightly decrease whereas those of neutrals continue to increase, even slightly. However, when the Sc atom number is greater than seven, the E b of both anionic and neutral states steadily decrease, and attains the lowest value at y ¼ 13, corresponding to the value of the pure scandium cluster Sc 13 . In order to interpret such a trend, the total Al-Al, Al-Sc and Sc-Sc bond order within each cluster are analyzed using NBO calculations. The bond order for each of the bonds connecting two atoms, including Al-Al, Al-Sc, and Sc-Sc in the clusters can be calculated as half of the difference between the electron occupancies in the corresponding bonding and anti-bonding orbitals. The total bond order for each of the bonds involved are thus summed up in the total Al-Al, Al-Sc and Sc-Sc bond orders. The values of bond orders, NBO charges of the central atom of the icosahedral cage are listed in the Table 3. In going from Al 13 À to Al 7 Sc 6 À , the Al-Al bond order decreases, whereas the Al-Sc and Sc-Sc bond orders increase, and the total bond order of each cluster remains relatively high. Therefore, the energy needed to break all the bonds in a cluster to form the constituent atoms is high as compared to that in other clusters. It is worth noting again that the Al-Al bond is markedly stronger than those made between Sc and Sc (cf. above). Nevertheless, the Sc-Sc bond order in the Sc 2 dimer amounts to 2.3, being much larger as compared to that of the Al-Al dimer. 52 From the size Al 6 Sc 7 À onward to AlSc 12 À and nally Sc 13 À , the Al-Al bond order of Al x Sc y is going close to zero, and this makes their average binding energies much lower as compared to those the Al x Sc y clusters having y < 7. Consequently, the average binding energy tends to decrease from Al 6 Sc 7 À to Al 1 Sc 12 À and to Sc 13 À and this could attribute to a substantial decrease in the Al-Sc bond order in these sizes. Fig. 7a also shows the E b values of all anionic Al x Sc y À clusters that are obviously higher than those of the neutral counterparts, and this proves that the neutral tends to receive an electron to form the more stable anionic state. This feature can be observed more closely by examining the computed electron affinities shown in Fig. 7b. Starting from the superhalogen Al 13 with a very large electron affinity, EA(Al 13 ) ¼ 3.2 eV, the substitution of one to ve Al atoms in Al 13 by a corresponding number of Sc atoms rapidly reduces this parameter, down to a value of 1.6 eV at Al 8 Sc 5 . When the Sc atom number increases from 5 to 13, the electron affinity turns out to slightly decrease and takes the lowest value of 1.3 eV at the pure Sc 13 . Such a reduction is no doubt due to the low electron affinity of the transition metal atom. Thus, substitution of Al atoms in Al 13 by Sc atoms makes the binary clusters losing their superhalogen characteristic.

Concluding remarks
In the present theoretical study, the geometrical and electronic structures of the 13-atom clusters Al x Sc y , with x + y ¼ 13, were investigated using DFT calculations. Geometry optimizations remarkably pointed out that all the most stable isomers of Al x Sc y , in both anionic and neutral states, retain the icosahedral shape in which the Al atom is favored to occupy the central location, irrespective of the Al atom number. The Sc atoms are consistently located at the vertexes of an icosahedral cage. The icosahedral shape is thus retained, even with some slight geometric distortions. The perfect icosahedral shape is kept only for the Al 13 , Sc 13 and AlSc 12 sizes. The electron congurations of the clusters considered, in their ground state, have been established and rationalized along with the spin multiplicities. NBO analyses revealed that the unpaired electrons are mostly distributed on the Sc atoms and the SOMOs are the molecular orbitals belonging to the irreducible representations of the symmetry point group of the corresponding cluster. Thermodynamic stabilities were also examined through the average binding energy per atom in each size. The stable geometrical structure, the unpaired electron and thereby multiplicity, and the average binding energy follow some clear trends as follows: (i) The scandium atoms prefer to be located on exohedral sites of icosahedron nearby the aluminum atoms in order to