Journal of Chemistry

Volume 2013 (2013), Article ID 370637, 9 pages

http://dx.doi.org/10.1155/2013/370637

Research Article

XPS-Characterization of Heterometallic Coordination Compounds with Optically Active Ligands

Yenny Ávila-Torres,¹ Lázaro Huerta,² and Noráh Barba-Behrens¹

¹Departamento de Química Inorgánica, Facultad de Química, Universidad Nacional Autónoma de México, C. U., Coyoacán, 04510 Mexico, DF, Mexico

²Instituto de Investigaciones en Materiales, Universidad Nacional Autónoma de México, C. U., Coyoacán, 04510 Mexico, DF, Mexico

Received 14 March 2013; Revised 9 May 2013; Accepted 23 May 2013

Academic Editor: Tsun-Ren Chen

Copyright © 2013 Yenny Ávila-Torres et al. This is an open access article distributed under the Creative Commons Attribution License, which permits unrestricted use, distribution, and reproduction in any medium, provided the original work is properly cited.

Abstract.

The heterometallic optical complexes [Cu₂Co(S,S(+)cpse)₃(H₂O)₃]·4H₂O (1) and [Cu₂Ni(S,S(+)cpse)₃(H₂O)₃]·10H₂O (2) were obtained from the mononuclear copper(II) compound by the addition of nickel(II) or cobalt(II) chlorides, where (H₂cpse) is the acetyl amino alcohol derivative N-[2-hydroxy-1(R)-methyl-2(R)-phenylethyl]-N-methylglycine. In comparison with the homotrinuclear copper(II) compound [Cu₃(S,S(+)cpse)₃(H₂O)₃]·8H₂O reported previously, the substitution of a copper(II) atom by one cobalt(II) ion gave place to a heterotrinuclear compound 1, which presents ferromagnetic-antiferromagnetic behaviour. When substituting a copper(II) by a nickel(II) ion, the trinuclear compound 2 showed an antiferromagnetic coupling. The magnetic behaviour of the heterotrinuclear compounds is driven by the nature of the metal ion which was introduced in the copper(II) triangular array. The ligand and its coordination compounds were characterized by IR, UV-Vis-NIR. Their chemical was confirmed by photoelectron spectroscopy (XPS).

1. Introduction

Investigation of novel inorganic-organic compounds mixed represents one of the most active areas of materials science and chemical research. The structural diversity of compounds bearing with more than one metal ion may give place to potential applications in research fields such as electrical conductivity, magnetism, photomechanism, host-guest chemistry, ion exchange, shape specificity, and catalysis [1, 2].

Mixed metal states can allow access to several electronic states and cooperative effects between them [3]. There is a particular emphasis on heterobimetallic complexes, and much of this research has been directed towards transition metal clusters. High-spin multiplicity in a polymetallic entity could be stabilized without imposing ferromagnetic interactions between the nearest magnetic centers. To achieve this, two high local spins are aligned in the same direction due to antiferromagnetic interactions with a small spin located between them [4–6].

Chiral ligands have been used in the formation of an extended homochiral two-dimensional (2D) sheet, which, in turn, leads to a conglomerate structure, constructed through the homochiral stacking of the 2D sheets [7]. Also, such photochemical switches controlled by photoisomerization can be used in the formation of cholesteric phases on nematic hosts and helical pitches [8]. In the technological field, chiral magnet may participate in the process for storage information and gas storage [9, 10].

The d-block metal ions are borderline acids, having a strong tendency to coordinate with N-donors as well as O-donors [11]. The acetyl pseudoephedrine derivative S,S(+)H₂cpse is a flexible enantiomerically pure ligand, with three potential coordination sites: the nitrogen which is an atom, and the carboxylic and the alcohol groups and (Figure 1).

Figure 1: Structures for (S,S(+)H₂cpse).

In this work, we present the synthesis of the heterotrinuclear compounds [Cu₂Ni(S,S(+)cpse)₃(H₂O)₃]·10H₂O 1 and [Cu₂Co(S,S(+)cpse)₃(H₂O)₃]·4H₂O 2. The trinuclear bimetallic compounds are product of deprotonation of the OH group in the mononuclear copper(II) compound [Cu(S,S(+)Hcpse)₂]·2H₂O, which gives place to an oxo-bridge between the metal ions [12]. They were spectroscopically characterized by IR, electronic absorption, atomic absorption, EPR, and magnetic susceptibility at variable temperature. Photoemission spectroscopy provided direct electronic information about core-level states at higher binding energies. The heterometallic compounds were spectroscopically compared with trinuclear copper(II) compound [Cu₃(S,S(+)cpse)₃(H₂O)₃]·8.5 reported previously [13]. This characterization allowed us to understand structural similarities between homometallic and heterometallic compounds. Finally, it is considered that these results contributed significantly to the structural elucidation and the electronic structure of coordination compounds [14–16].

2. Experimental Section

2.1. General Remarks

IR spectra in the range 4000–400 cm⁻¹ were recorded on a Nicolet FT-IR 740 spectrophotometer using KBr pellets. Electronic spectra (diffuse reflectance), were measured on a Cary 5E Uv-Vis-NIR spectrophotometer over the range 250–2500 nm (40000–4000 cm⁻¹). Elemental analyses were performed on a Fisons EA 1108 elemental analyser. The relationship between metal ions was performed in AA Varian model Spectra AA 20 plus calibrated using SPEX standards for each metal. All experiments were run 10 times to reduce random errors; the reported data are the average values with errors below 0.5%. Magnetic susceptibility measurements were carried out with a pendulum-type magnetometer (MANICS DSM8) equipped with an Oxford CF 1200 S helium continuous-flow cryostat working in the temperature range 300–4 K in a magnetic field of 1.5 T. Diamagnetic corrections were estimated using Pascal constants. The chemical analysis was obtained using X-ray photoelectron spectroscopy (XPS), with VG Microtech ESCA2000 Multilab UHV system, KαX-ray source (h = 1486.6 eV), and CLAM4 MCD analyzer. XPS spectrum was obtained at 55° from the normal surface in the constant pass analyzer energy mode (CAE), E₀ = 50 and 20 eV for survey and high resolution narrow scan. Peak positions were referenced to the background silver 3d5/2 core level at 368.20 eV, having a FWHM of 1.10 eV, Au 4f7/2 in 84.00 eV, and C 1s hydrocarbon groups in 285.00 eV central peak position. The XPS spectra were fitted with the program SDP v 4.1 [17]. The XPS error is considering a detection limit estimated to be 0.1% in mass and uncertain propagation. For deconvolution analysis the uncertain was estimated at 5%. The valence band (VB) energy zone was obtained.

2.2. Materials

The metal salts CoCl₂·6H₂O, NiCl₂·6H₂O, Cu (OAc)₂·H₂O, and methanol (J. T. Baker) were used without further purification.

The synthesis of the ligand N-[2-hydroxy-1(S)-methyl-2(S)-phenylethyl]-N-methylglycine (S,S(+)H₂cpse) 2 and [Cu(S,S(+)Hcpse)₂]·2H₂O compound was carried out as previously described [18].

2.3. Synthesis of Compound [Cu(S,S(+)Hcpse)₂]·2H₂O

Cu (CH₃COO)₂2H₂O (249.3 mg, 0.125 mmol) was added to a solution of S,S(+)H₂cpse (479 mg, 2.13 mmol) in methanol (20 mL). The mixture was stirred for 15 minutes. A blue precipitate appeared immediately, yield 77.8%. Anal. Calcd. for C₂₄H₃₆CuN₂O₇: C%, 55.98; H%, 6.58; N%, 5.27. Found: C%, 54.58; H%, 6.87; N%, 5.30. IR (KBr /cm⁻¹): 1612 ( COO⁻), 1392 ( COO⁻) Δ = 220 cm⁻¹ [17].

2.4. Synthesis of Compound [Cu₂Co(S,S(+)cpse)₃(H₂O)₃]·4H₂O  (1)

To a solution in MeOH (20 mL) of [Cu(S,S(+)Hcpse)₂]·2H₂O (502 mg, 1 mmol), 2 equivalents of NaOH (82 mg) and CoCl₂6H₂O (0.238 g, 1 mmol) were added. A green-gray solid was obtained over a period of one week, yield 47.8%. Anal. Calcd for C₃₆H₅₆Cu₂CoN₃O₁₃: C, 46.75; H, 6.10; N, 4.54. Exp.: C, 46.45; H, 6.71; N, 4.52. Atomic absorption: Cu : Co 1.78 : 1.22 (13.4598%–8.1445%). IR (KBr /cm⁻¹): 1632 ( COO⁻) and 1383 ( COO⁻), Δ = 249 cm⁻¹.

2.5. Synthesis of Compound [Cu₂Ni(S,S(+)cpse)₃(H₂O)₃]·10H₂O (2)

To a solution in MeOH (20 mL) of [Cu(S,S(+)Hcpse)₂]·2H₂O (502 mg, 1 mmol), 2 equivalents of NaOH (82 mg) and NiCl₂·6H₂O (245 mg, 1 mmol) were added. A pale green precipitate was obtained over a period of one week, yield 58.5%. Anal. Calcd for C₃₆H₇₄Cu₂NiN₃O₂₂: C, 39.78; H, 6.86; N, 3.87. Exp.: C, 39.2; H, 5.36; N, 3.88. Atomic absorption Cu : Ni 1.92 : 1.08 (15.6278%–8.7689%). IR (KBr /cm⁻¹): 1623 ( COO⁻) and 1377 ( COO⁻), Δ = 246 cm⁻¹.

3. Results and Discussion

3.1. Heterotrinuclear Compounds 1 and 2

When reacting the copper(II) mononuclear [Cu(S,S(+)Hcpse)₂]·2H₂O (obtained as previously described) [17] in basic conditions, with cobalt(II) or nickel(II) chlorides, the corresponding heterotrinuclear compounds [Cu₂Co(S,S(+)cpse)₃(H₂O)₃]·4H₂O (1) and [Cu₂Ni(S,S(+)cpse)₃(H₂O)₃]·9H₂O (2) were obtained.

In these compounds the ligand is coordinated by the nitrogen atom, the carboxylic group and the alcohol group, as observed from their IR spectra [19], where the corresponding stretching bands are shifted to lower energies upon coordination to the metal ions (Table 1). The  (C–OH)st. is not observed due to deprotonation of the OH group and the bridging oxygen coordination to the metal centres.

Table 1: Selected IR bands for the ligand and its coordination compounds.

Coordinate compound and ligand
(COO⁻)–

(cm⁻¹)
(–COO⁻)

(cm⁻¹)

(cm⁻¹)
(C–OH)st 

(cm⁻¹)

S,S(+)H₂cpse¹⁸
1638
1385
—
1040

Cu₃(S,S(+)cpse)₃(H₂O)₃·8.5H₂O
1631
1385
246
—

Cu₂Co(S,S(+)cpse)₃(H₂O)₃·4H₂O (1)
1632
1383
249
—

Cu₂Ni(S,S(+)cpse)₃(H₂O)₃·10H₂O (2)
1623
1377
246
—

In the electronic spectrum of [Cu₂Co(S,S(+)cpse)₃(H₂O)₃]·4H₂O 1, there are bands corresponding to = (F)← (F) = 5933 cm⁻¹, = (F)← (F) = 8770 cm⁻¹, and = (F)← (F) = 16222 cm⁻¹ for the cobalt(II) ion in a square-based pyramid geometry; the latter is a broad band which is superimposed with the expected transition for the copper(II) ion at ca. 14000 cm⁻¹ [20]. Additionally, there is a CT M-L band at 31336 cm⁻¹ (Figure 2). The spectrum was compared with the corresponding mononuclear compounds. The contribution of the copper(II) and cobalt(II) metal ions is observed in the electronic transitions.

Figure 2: Electronic spectra for (a) [Cu₂Co(S,S(+)cpse)₃(H₂O)₃]·4H₂O (1), (b) [Cu(S,S(+)cps)₂]·2H₂O, and (c) [Co(S,S(+)cps)₂]·2H₂O synthetized previously.

The reflectance spectrum of the [Cu₂Ni(S,S(+)cpse)₃(H₂O)₃]·10H₂O compound 2 shows transitions in the near infrared that were assigned for a nickel(II) in a square-based pyramidal geometry, ← at 5218 cm⁻¹ and ← at 7047 cm⁻¹; the rest of the expected transitions are overlapped with the copper(II) transition at 14285 cm⁻¹, in the same region as for the trinuclear copper(II) [Cu₃(S,S(+)cpse)₃(H₂O)₃]·8H₂O (Figure 3).

Figure 3: The UV-Vis-NIR electronic spectra for (a) [Cu₂Ni(S,S(+)cpse)₃(H₂O)₃]10H₂O (2), (b) [Ni(S,S(+)cps)₂]·2H₂O [17] and (c) [Cu(S,S(+)cps)₂]·2H₂O [17].

In accordance with the atomic absorption, elemental analysis, ultraviolet-infrared visible diffuse reflectance, and infrared spectroscopy, it is proposed that the heterotrinuclear compounds present a similar structure to that of [Cu₃(S,S(+)cpse)₃(H₂O)₃]·8H₂O reported previously [12]. This structure corresponds to three metal ions in a square pyramidal geometry; each of them coordinated with one molecule of the S,S(+)cpse ligand and to a water molecule in the apical position. The metal centres are bridged by an oxygen atoms from the deprotonated OH group. In Figure 4 is shown the chemical structure for the heterometallic compounds. The supramolecular structure for [Cu₃(S,S(+)cpse)₃(H₂O)₃]·8H₂O presents interesting arrangements in the crystalline cell, due to the stabilization of a Δ isomer. In this system the S,S(+)cpse and the metal ions contributed to the chirality (Figure 4).

(a)

(b)

(c)

Figure 4: (a) Structure of the homotrinuclear [Cu₃(S,S(+)cpse)₃(H₂O)₃]·8H₂O compound, Δ isomer. Proposed structures for (b) [Cu₂Co(S,S(+)cpse)₃(H₂O)₃]·4H₂O (1) and (c) [Cu₂Ni(S,S(+)cpse)₃(H₂O)₃]·10H₂O (2).

In order to further corroborate the structure of the heterometallic compounds, a XPS study was performed for the three compounds. It compared the Survey XPS spectra of heterometallic compounds [Cu₂Co(S,S(+)cpse)₃(H₂O)₃]·4H₂O (1) [Cu₂Ni(S,S(+)cpse)₃(H₂O)₃]·10H₂O (2) with those of [Cu₃(S,S(+)cpse)₃(H₂O)₃]·8H₂O (Figure 5). The electronic structure is similar to these compounds. It is observed that there are contributions for Cu 2p to [Cu₃(S,S(+)cpse)₃(H₂O)₃]·8H₂O; Cu 2p and Co 2p for [Cu₂Co(S,S(+)cpse)₃(H₂O)₃]·4H₂O (1); and Cu 2p and Ni 2p for [Cu₂Ni(S,S(+)cpse)₃(H₂O)₃]·10H₂O (2).

Figure 5: Survey XPS spectra of the homometallic and heterometallic compounds. (a) [Cu₃(S,S(+)cpse)₃(H₂O)₃]·8H₂O, (b) [Cu₂Co(S,S(+)cpse)₃(H₂O)₃]·4H₂O (1), and (c) [Cu₂Ni(S,S(+)cpse)₃(H₂O)₃]·10H₂O (2).

In XPS interpretation, the general rule is that the BE of the central atom increases as the electronegativity of the attached atoms or groups increases [21]. The difference on electronegativities when substituting copper(II) by cobalt(II) or nickel(II) is not significant, but the charge transfer between metal ions is observed.

In the XPS valence band spectra for these compounds mainly two peaks are observed. The first one with a single fine structure at a binding energy of 2–8 eV originates from photoemission out of the d⁹ ground state configuration of copper(II), for which the photo-hole is screened by a charge transfer from the ligand O2p electrons towards the Cu (labelled by d⁹→d⁹L with L meaning the hole in the O2p ligand states L). For the three compounds there exists a contribution of copper(II). However, heterometallic compounds 1 and 2 present an additional contribution from the cobalt(II), Co 3d (1 eV), and nickel(II) Ni 3d (2 eV) (Figure 6). In the crystalline structure for [Cu₃(S,S(+)cpse)₃(H₂O)₃]·8H₂O there exists a stable six-membered ring (Cu1-O-Cu2-O-Cu3-O-Cu1) in a chair conformation (Figure 7). For this arrangement there is a higher electronic delocalization between metal ions and the oxygen atoms from of the ligand. For the heterometallic compounds this electronic delocalization is also expected. In consequence, the effect on their charge transfer is observed which is a shift to positive energy at Fermi level. The second one appears at about 14 eV and presents contributions of the ligand.

Figure 6: XPS valence band spectra of (a) [Cu₃(S,S(+)cpse)₃(H₂O)₃]·8H₂O, (b) [Cu₂Co(S,S(+)cpse)₃(H₂O)₃]·4H₂O (1), and (c) [Cu₂Ni(S,S(+)cpse)₃(H₂O)₃]·10H₂O (2).

Figure 7: Chair conformation for the [Cu₃(S,S(+)cpse)₃(H₂O)₃]8H₂O structure.

In Figure 8, the binding energies for copper 2p3/2, 2p1/2, nickel 2p3/2, 2p1/2, and cobalt 2p3/2, 2p1/2 levels in the three compounds are shown: [Cu₃(S,S(+)cpse)₃(H₂O)₃]8H₂O, [Cu₂Co(S,S(+)cpse)₃(H₂O)₃]4H₂O (1), and [Cu₂Ni(S,S(+)cpse)₃(H₂O)₃]·10H₂O (2) synthesized in this work. For copper on [Cu₃(S,S(+)cpse)₃(H₂O)₃]·8H₂O compound 2p3/2 was found at 932.54 eV (charge transfer shake-up satellite peak at 942.80) and 2p1/2 in 952.48 eV (charge transfer satellite peak at 962.71 eV). The compounds 1 and 2 present similar peaks to those of the homotrinuclear copper(II) compound in the expected region for copper(II); therefore this behaviour suggests electronic similarities between the trinuclear compounds. The compounds 1 and 2 spectra for cobalt (781.53 eV, charge transfer satellite peak at 786.87 and 2p1/2 in 797.42 eV, charge transfer satellite peak at 802.96 eV) and nickel (855.20 eV, charge transfer satellite peak at 861.22 and 2p1/2 in 872.87 eV, charge transfer satellite peak at 879.47 eV) were compared with CoO [22] and NiO. The satellites were used as a finger print for the recognition of high-spin cobalt(II) and nickel(II). This behaviour is consistent with a 3d⁸ nickel(II) ion and 3d⁷ cobalt(II) ion. No evidence of other nickel(II) and cobalt(II) transitions was observed from their spectra. Hence this suggests that in these compounds the metal ions do not contain different oxidation states other than 2⁺ [23].

Figure 8: XPS spectra of Cu 2p, Ni 2p, Co 2p, and N 1s core level. Compared with the XPS spectra of the homotrinuclear and heterotrinuclear compounds (1) and (2).

The observed binding energy of the N 1s XPS transition, at 399.93 eV, is in agreement with the reported values for organic amines coordinated with metal atoms in solid state [15]. The nitrogen atom shows a similar electronic behaviour in all studied compounds (Figure 8).

The XPS core level spectrum for [Cu₃(S,S(+)cpse)₃(H₂O)₃]·8H₂O of the C 1s region shows the following order: (C–CH₂) 285.00, (C–CH₃) 285.67, (CH₃–N) 285.96 eV, (CH₂–N) 286.46, (C–O–M; M = metal ion) 287.20 eV, and (C=O) 289.09 eV. The binding energy depends on the specific environment where the functional groups are located. In this context, it is found that C–C is after of C–N and C–O. The increase in bond polarity leads shifted to higher energy. These contributions for C1s level show coordination of the ligand towards metal by nitrogen and oxygen atoms (Figure 9).

Figure 9: XPS spectra for C 1s core level in [Cu₃(S,S(+)cpse)₃(H₂O)₃]·8H₂O for compounds 1 and 2.

For O 1s core level the binding energy corresponding to (O–Cu–O) 530.79 eV, (C=O) 531.67 eV, (C–O) 532.38 eV, (H₂O–Cu) 533.36, and satellite at 532.50 eV are shown. The allocations were realized for trinuclear copper(II) compound. For compound 1 contributions for O–Co–O and compound 2 O–Ni–O are additionally observed (Figure 10). Contributions due to H₂O molecule are correlated with the amount of molecules outside the coordination sphere: compound 2 > trinuclear copper(II) compound > compound 1.

Figure 10: XPS spectra O1s core level for [Cu₃(S,S(+)cpse)₃(H₂O)₃]·8H₂O and compounds 1 and 2.

3.2. Magnetic Properties of the Trinuclear Compounds for 1 and 2

To investigate the magnetic interactions in the heterotrinuclear compounds, EPR spectra and the magnetic susceptibilities of powdered samples were measured from 4 to 300 K.

The EPR spectrum at 115 K for [Cu₂Co(S,S(+)cpse)₃(H₂O)₃]4H₂O (1) corresponds to a high-spin d⁷ configuration either in an orbitally nondegenerate ground state (⁴A ₂) or in an orbitally degenerate ground state (⁴T₁) in which the orbital levels are separated by spin-orbit coupling. The orbital angular moment is quenched, and the combined effects of crystal field symmetry and mixture of excited terms through second-order spin-orbit may lead to a splitting the two doublets. The resonance absorption features appear at value ~5.6, 3.4 and splitting ~2.09. Hyperfine structure resolved in both ~5.6 and ~2.09 regions corresponds to a coupling for the cobalt(II) I = 7/2. However, the EPR spectra depicted in Figure 11 show the overlap signals for copper(II) and cobalt(II) for pentacoordinate complexes of high spin.

Figure 11: EPR spectrum for [Cu₂Co(S,S(+)cpse)₃(H₂O)₃]·4H₂O (1).

The plot of versus (300–4 K), show a change in the slope. It involves an increase in as temperature is lowered, followed by a rapid drop at temperatures <13.75 K. The drop in below 17 K suggests the presence of a weak intermolecular antiferromagnetic interaction, but after 17 K the ferromagnetic behaviour is shown (Figure 12). This compound presents a magnetic moment of 8.15 B.M. at 298 K, per all metallic atoms, which is indicating the contribution of the copper(II) and cobalt(II) atoms.

Figure 12: Temperature dependence of versus for [Cu₂Co(S,S(+)cpse)₃(H₂O)₃]4H₂O (1).

For compound [Cu₂Ni(S,S(+)cpse)₃(H₂O)₃]10H₂O (2), in the EPR spectrum at 115 K (2.0023) suggest that the un pair electron is localized in dx ²-y ² orbital of Cu(II) ions and the spectral features are characteristics of axial symmetry. The complex under study may have square pyramidal geometry in the copper(II) atoms. The value of parameter ( ) is indicating ²B₁ as ground state; thus less than one. For nickel(II) with S = 1 signals around of 1000 G are expected (Figure 13). The magnetic moment of five coordinated Cu(II)-Cu(II)-Ni(II) complexes at room temperature of 6.15 B.M is representing antiferromagnetic behaviour between metal centres.

Figure 13: EPR spectrum for [Cu₂Ni(S,S(+)cpse)₃(H₂O)₃]·9H₂O (2).

The plot versus , between 300–4 K, is depicted in Figure 14. It shows an antiferromagnetic behaviour. The experimental data were fitted with the expression derived from the Hamiltonian (1) which corresponds to a triangular array of Cu-Cu-Ni spins: the best fit parameters being  cm⁻¹, ,

Figure 14: Temperature dependence of versus for [Cu₂Ni(S,S(+)cpse)₃(H₂O)₃]9H₂O (2). The solid line shows the theoretical susceptibility calculated by (1).

4. Conclusions

Cobalt-copper and nickel-copper trinuclear heterometallic compounds, with the chiral ligand (S,S(+)cpse), were studied by photoelectron spectroscopy (XPS). The found core levels for Cu 2p, Ni 2p, Co 2p, C 1s, O 1s, and N 1s led to the the identification the chemical structure in correspondence with the crystalline structure for homotrinuclear copper(II) compound. In the valence band, the effects due to charge transfer between the metal ions and the ligand were found. These results were in agreement with the spectroscopic and analytical characterization (IR, UV-V is reflectance diffuse, elemental analysis, and atomic absorption). The substitution of a copper(II) atom by one the cobalt(II) ion gave place to a heterometallic compound 1, which is ferromagnetic-antiferromagnetic magnetic transition. The substitution of a copper(II) atom by one the nickel(II) atom in compound 1, showed an antiferromagnetic coupling. The magnetic behaviour of the heterotrinuclear compounds is driven by the nature of the metal ion which was introduced in the copper(II) triangular array.

Acknowledgments

The authors would like to thank CONACyT for student fellowships to Yenny Ávila-Torres, Ramón Vicente (Universitat de Barcelona) for magnetic measurements, Israel Betancourt (IIM-UNAM) for academic support, and Rosalinda Contreras (CINVESTAV) for synthesis of chiral ligands, and Horacio López Sandoval (F.Q. UNAM), and the financial support by DGAPA (Grant IN212210 to Noráh Barba-Behrens) is acknowledged.

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