# XPS-Characterization of Heterometallic Coordination Compounds with Optically Active Ligands

Authors: Yenny Ávila-Torres; Lázaro Huerta; Noráh Barba-Behrens
Journal: Journal of Chemistry
 (2013)

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## 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).


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## Body

## 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 (hν = 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)2·2H2O (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 ν/cm−1): 1612 (νas COO−), 1392 (νs COO−) Δν = 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 CoCl2·6H2O (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 ν/cm−1): 1632 (νas COO−) and 1383 (νs COO−), Δν = 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 ν/cm−1): 1623 (νas COO−) and 1377 (νs COO−), Δν = 246 cm−1.


## 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 (hν = 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)2·2H2O (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 ν/cm−1): 1612 (νas COO−), 1392 (νs COO−) Δν = 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 CoCl2·6H2O (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 ν/cm−1): 1632 (νas COO−) and 1383 (νs COO−), Δν = 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 ν/cm−1): 1623 (νas COO−) and 1377 (νs COO−), Δν = 246 cm−1.


## 3. Results and Discussion

### 3.1. Heterotrinuclear Compounds1 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 v (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
ν
as(COO−)–(cm−1)
ν
s(–COO−) (cm−1)
Δ
ν (cm−1)
ν(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 ν1 = A42′′(F)←A4′(F) = 5933 cm−1, ν2 = E4′(F)←A42′(F) = 8770 cm−1, and ν3 = E4′(F)←A42′(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, E3′←E3 at 5218 cm−1 and A32←E3 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) 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).
(a)
(b)
(c)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 Figure8, 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 theN 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.ForO 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 for1 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 (4A2) 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 g 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 ofχMT versus T (300–4 K), show a change in the slope.  It involves an increase in χMT as temperature is lowered, followed by a rapid drop at temperatures <13.75 K. The drop in χMT 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 ofχMT versus T 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 g∥>g⊥>ge (2.0023) suggest that the un pair electron is localized in dx2-y2 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 R parameter (g2-g1/g3-g2) 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 plotχMT versus T, 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 J=-4.9 cm−1, g=1.696,
(1)xMT=Ng2β23k×6exp(J/KT)+6exp(2J/KT)+30exp(2J/KT)1+3exp(J/KT)+3exp(2J/KT)+5exp(3J/KT).Figure 14
Temperature dependence ofχMT versus T for [Cu2Ni(S,S(+)cpse)3(H2O)3]·9H2O (2). The solid line shows the theoretical susceptibility calculated by (1).


## 3.1. Heterotrinuclear Compounds1 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 v (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
ν
as(COO−)–(cm−1)
ν
s(–COO−) (cm−1)
Δ
ν (cm−1)
ν(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 ν1 = A42′′(F)←A4′(F) = 5933 cm−1, ν2 = E4′(F)←A42′(F) = 8770 cm−1, and ν3 = E4′(F)←A42′(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, E3′←E3 at 5218 cm−1 and A32←E3 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) 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).
(a)
(b)
(c)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 Figure8, 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 theN 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.ForO 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 for1 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 (4A2) 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 g 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 ofχMT versus T (300–4 K), show a change in the slope.  It involves an increase in χMT as temperature is lowered, followed by a rapid drop at temperatures <13.75 K. The drop in χMT 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 ofχMT versus T 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 g∥>g⊥>ge (2.0023) suggest that the un pair electron is localized in dx2-y2 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 R parameter (g2-g1/g3-g2) 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 plotχMT versus T, 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 J=-4.9 cm−1, g=1.696,
(1)xMT=Ng2β23k×6exp(J/KT)+6exp(2J/KT)+30exp(2J/KT)1+3exp(J/KT)+3exp(2J/KT)+5exp(3J/KT).Figure 14
Temperature dependence ofχMT versus T 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.



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*Source: 370637-2013-07-02.xml*