The main bands and their assignments are listed in Table 2. In the IR spectra of macrocyclic Cu(II) complexes, a medium intensity band due to υ_(C=N) was shifted towards lower side about 20–33 cm⁻¹ compared to the ligand spectra and was appeared in the range of 1598–1573 cm⁻¹ [21]. The appearance of a lower intensity band in the region of 524–505 cm⁻¹ corresponds to the υ_(M–N) vibration supports the fact that the ligands coordinate to the metal ions through the nitrogen of C=N group in all the complexes [22–24]. A band present in the range of 318–302 cm⁻¹ in the spectra of 1.1, 1.2, 1.3, 1.4 and 1.6 complexes indicating the presence of two chlorides in trans position around copper center [17,25]. The presence of chloride ions in 1.1, 1.2, 1.3, 1.4 and 1.6 complexes are detected by the addition of silver nitrate reagent leading to the formation of white precipitate. However, in the case of complex 1.5, this band is not observed indicating chloride ions are not in the coordination sphere. The coordination of the nitrate groups have been confirmed in the complexes 2.1, 2.2, 2.3, 2.4 and 2.6 by the band in the region of 230–240 cm⁻¹ may be assigned [9] to υ_(M–O) of the ONO₂ group [26]. The additional bands observed around ~1410, 1300 and 1020 cm⁻¹ [25] were obtained in the spectra of the nitrato complexes, which consistent [26] with the monodentate nature of the nitrato group [25,27,28]. The absence of these bands was observed in case of complex 2.5 indicating nitrate groups are not in the coordination sphere. The macrocyclic Cu(II) compounds (1.2 and 1.6) contain a broad band in the region 3505– 3374 cm⁻¹ due to the presence of lattice water molecules[18,22].

The EPR spectra of the Cu(II) complexes have been recorded at room temperature as well as at liquid nitrogen temperature and their g_ll and g_⊥ values have been calculated. The observed data show that g_ll = 2.085–2.219 and g_⊥ = 2.018–2.046 (Table 3). The values of g_ll and g_⊥ are closer to 2 and g_ll > g_⊥. This suggests that the unpaired electron is in the d_x2-y2 orbital and hence, ²B₁ is the ground state. It should be noted that for an ionic environment g_ll > 2.3, while for a covalent environment g_ll < 2.3. The copper complexes show g_ll < 2.3 indicating their considerable covalent character [9,29]. The g values are related by the expression G = (g_ll − 2)/(g_⊥ − 2) which suggests an exchange interaction between copper centers in the polycrystalline solid. According to Hathway [30] if G > 4, the exchange interaction is negligible. In the present case, the axial symmetry parameter, G, lies in the range 4.025–5.896, which indicates no considerable exchange interaction in these solid complexes.

The magnetic moment of all the Cu(II) complexes at room temperature lie in the range of 1.86–1.98 B.M. given in Table 1, corresponding to one unpaired electron. This indicates that these complexes are monomeric in nature and the absence of metal-metal interaction [17]. The electronic spectra of the complexes [Cu(L)X₂](X = Cl⁻, NO₃ ⁻) display two characteristic bands in the region 21226–22801 cm⁻¹ and 16008–18348 cm⁻¹ these may be assigned to ²B_1g→²E_g and ²B_1g→²A_1g transitions respectively. The third band assigned to ²B_1g→²B_2g transition band is usually not observed as a separate band in the tetragonal field. Therefore, it may be concluded that all the [Cu(L)X₂] complexes show distorted octahedral structure (Scheme) [31]. The complexes [Cu(L)]X₂ display broad band in the region 18181–18457 cm⁻¹ and 13065–13524 cm⁻¹ corresponding to transitions ²B_1g→²E_g and ²B_1g→²A_1g which suggests the square planar geometry [19].

Thermograms of TGA and DTA of macrocyclic Cu(II) compounds were recorded in nitrogen atmosphere at a heating rate of 10 °C/min. In the thermogram of complexes [Cu(TBACD)Cl₂]·2H₂O (1.2) and [Cu(TBAHD)Cl₂]·2H₂O (1.5), the initial weight loss of 15.36% (Calcd 15.28%) and 14.45% (Calcd 14.37%) at 70–110 °C corresponding to loss of two lattice held water molecules [18,22]. This fact was further supported by their DTA curves, which contain endothermic peaks in the temperature range 90–125 °C. The TGA decomposition curve, a peak corresponding to the loss of organic moiety in the temperature range of 238–252 °C was observed. On the other hand, the thermograms of other macrocyclic Cu(II) compounds showed only a single decomposition curve in the region 220–260 °C corresponding to the loss of organic moiety. Above 455 °C, organic moieties in macrocyclic Cu(II) compounds were decomposed leading to the formation of copper oxide.

In the mass spectra of respective macrocyclic Cu(II) complexes, molecular ion peaks, were observed at different m/z (M⁺/[M + Na]⁺) values. The molecular ion peaks and isotopic pattern of Cu(II) complexes shows different m/z values with different intensities. The mass spectra contain molecular ion peaks at m/z 511 (M⁺, complex 1.1), 517 (M⁺, complex 1.2), 507 (M⁺, complex 1.3), 543 (M⁺, complex 1.4), 483 (M⁺, complex 1.5), 517 (M⁺, complex 1.6), 563 (M⁺, complex 2.1), 586 ([M + Na]⁺, complex 2.1), 533 (M⁺, complex 2.2), 560 (M⁺, complex 2.3), 583 ([M + Na]⁺, complex 2.3), 595 (M⁺, complex 2.4), 535 (M⁺, complex 2.5), and 565 (M⁺, complex 2.6). This data is in good agreement with the respective molecular formulae.

Based on the physicochemical and the spectral studies the tentative structures proposed for the complexes are shown in Scheme 1.

Twelve chemically synthesized Cu(II) macrocyclic complexes were tested in vitro for their antibacterial activity against five test bacteria namely S. aeruginosa, S. epidermidis, B. pumilus, B. megaterium and P. aeruginosa. The minimum inhibitory concentrations of complexes were determined by liquid dilution method. The minimum inhibitory concentration at which no growth was observed was taken as the MIC values. All the complexes of the tested series possessed good antibacterial activity against both gram-positive bacteria and gram-negative bacteria. The higher antibacterial activity of the copper complexes is may be due to the change in structure due to coordination and chelating tends to make metal complexes act as more powerful and potent bactereostatic agents, thus inhibiting the growth of the bacteria. Six complexes out of twelve (1.4, 1.5, 1.6, 2.4, 2.5 & 2.6) were most potent against both gram-positive as well as gram-negative bacteria. However, complexes 1.1, 1.2, 1.3, 2.1, 2.2 & 2.3 were also showed noticeable MIC ranging from 1–16 μg/mL against S. aeruginosa, B. pumilus and B. megaterium (Table 5). The gram positive were much more susceptible to the series as compared to gram-negative bacteria. The twelve Cu (II) complexes were also compared with two commercial antibiotics namely Linezoid and Cefaclor. The six complexes 1.4, 1.5, 1.6, 2.4, 2.5 & 2.6 registered better antibacterial in comparison with commercial antibiotics. The activity of these complexes is due to the presence of thio group in the coordinated ligands. Comparison of MIC values (in μg/mL) of Cu(II) macrocyclic complexes and standard drugs against different bacteria are given in Figure 1.

The metal salts CuCl₂·2H₂O and Cu(NO₃)₂·3H₂O were purchased from E. Merck. All the chemicals used were of AR grade and were procured from Aldrich. All solvents used were of AR grade. Six macrocyclic ligands viz. 7,8,9,18,19,20-hexahydrodibenzo[g,p] [1,2,4,5,10,11,13,14]- octaazacyclooctadecine-8,19-dione [HBOADO], 7,8,17,18-tetrahydrodibenzo[f,n] [1,2,4,9,11,12]- hexaazacyclohexadecine-8,17-dione [TBACD], 7,8,9,10,19,20,21,22-octahydrodibenzo[c,m] [1,6,11,16]-tetraazacycloicosine [OBACI], 7,8,9,18,19,20-hexahydrodibenzo[g,p] [1,2,4,5,10,11,13,14]-octaazacyclooctadecine-8,19-dithione [HBOADT], 7,16-dihydrodibenzo[e,l] [1,3,8,10]-tetraazacyclo tetradecine-7,16-dithione [DBACDT] and 7,8,17,18-tetrahydrodibenzo[f,n] [1,2,4,9,11,12]-hexaazacyclohexadecine-8,17-dithione [TBAHD] were synthesized according to the procedure reported by shanker et al. [32]. Gram positive microorganisms like Staphylococcus aeruginosa (ATCC-29213), Staphylococcus epidermidis (MTCC-2639), Bacillus pumilus (MTCC-1456), Bacillus megaterium (MTCC-428) and gram negative microorganism like Pseudomonas aeruginosa (ATCC-27853) from IMTECH, Chandigarh were used for antibacterial studies.

The elemental analyses were obtained by using a Perkin-Elmer-2400 CHN elemental analyzer. The complexes were analyzed for Cu(II) content gravimetrically by literature procedures (Vogel AI (1989) Vogel’s text book of quantitative chemical analysis, 5th edition Longman, Amsterdam) after decomposing the organic matter with a mixture of HNO₃ and HCl and evaporating the residue to dryness with concentrated H₂SO₄. UV-Vis spectra were recorded on Shimadzu UV-160A spectrophotometer, EPR spectra were recorded on Varian E-112X-Q band EPR Spectrometer. IR spectra in KBr pellets on Perkin-Elmer-283 spectrophotometer. LC-ESI MS was used to obtain mass spectra. Gouy balance calibrated with Hg[Co(NCS)₄] was used for the determination of magnetic susceptibilities of complexes in solid state at room temperature. Thermograms were recorded on mettler-TA-2000C model. TG-DSC equilibrated at 25 ± 0.05 °C. The electrical conductivities of 10⁻³ M solutions in dichloromethane were performed using Digisun Digital conductivity meter model DL-909.

To a stirred solution of the respective copper salts (0.519 g, 0.003 mol) dissolved in methanol (~20 mL) in a round-bottomed flask, methanolic solution (~25 mL) of ligand (0.003 mol., viz. 1.17 g of HBOADO, 1.038 g of TBACD, 1.116 g of OBACI, 1.26 g of HBOADT, 1.044 g of DBACDT, 1.134 g of TBAHD respectively) were added with the help of a dropping funnel. The reaction mixture was stirred magnetically. The resulting solution was concentrated to 5 mL under reduced pressure and a few mL of diethyl ether was added to initiate the crystallization. The resulting precipitate was separated by suction filtration, washed several times with diethyl ether, dried in vacuo and was recrystallized using dichloromethane and diethyl ether solvent mixture.