Journal of Inorganic Chemistry

Journal of Inorganic Chemistry / 2014 / Article

Research Article | Open Access

Volume 2014 |Article ID 769573 | 10 pages |

Copper(II) Complexes of 2-(Methylthiomethyl)anilines: Spectral and Structural Properties and In Vitro Antimicrobial Activity

Academic Editor: Roman Boča
Received23 Dec 2013
Accepted13 Feb 2014
Published16 Apr 2014


Copper(II) complexes of 2-(methylthiomethyl)anilines (1a1f) have been obtained and characterized by elemental analyses, IR, electronic spectra, conductivity, and X-ray crystallography. The complexes (2a2f) have the structural formula [CuCl2L] with the bidentate ligand coordinating through sulfur and nitrogen. The single crystal X-ray diffraction data reveal that the copper complex (2f) has a tetragonally distorted octahedral structure with long Cu–Cl equatorial bonds. Magnetic susceptibility measurements indicate the availability of one unpaired electron in the complexes and the conductivity measurements in DMF show their behaviour as nonelectrolytes. The solid reflectance spectra and the electronic spectra of the complexes in DMSO were determined. The ligands and their copper complexes were screened for in vitro antimicrobial activity against S. aureus, B. subtilis, E. coli, and C. albicans. The methoxysubstituted complex (2c) showed more promising antibacterial activity against S. aureus and B. subtilis than other compounds at the concentration tested.

1. Introduction

The alkylthioalkylated anilines have found application as intermediates in production of many organic compounds [13] including dyes, rubber, and herbicides [4]. They act as coordinating ligands due to the presence of the aniline nitrogen and the thioether sulfur in their moiety. The hard-borderline and soft nature of the nitrogen and sulfur, respectively, in alkylthioalkylated anilines permits the formation of stable complexes between them and metal ions under mild nonextreme reacting conditions. Donor groups commonly found in many known biologically active compounds and ligands used in pharmaceutical synthesis include the nitrogen, oxygen, sulfur, and chlorine atoms. Such biopotent organic compounds with their metal complexes are being explored for their activity against a wide range of microorganisms. Sulfur-containing ligands and complexes have been explored for biological activity and practical application [57]. Some metal complexes of SN ligands were investigated and reported. Copper(II) complexes CuX2(N–SMe) (X = Cl, Br) obtained from alcohol solution at 0°C were not very stable [8]. Ni(II) complexes of 2-methylthiomethylaniline [8] and 8-methylthioquinoline [9] have the composition NiX2(N–SMe)2 (X = Cl, Br [8]; X = Cl, Br, I, NCS [9]). The Pd(II) and Pt(II) complexes of these ligands, on being heated in dimethylformamide were S-demethylated to yield the thiolo-bridged complexes M2Cl2(N–S)2. Complexes MX2(N–SMe) and [M(N–SMe)2](ClO4)2 (M = Pd, Pt, Cu, Hg) were derived with 2-(2-methylthioethyl)pyridine [10] and 2-methylthiomethylpyridine [11]. The structural, spectroscopic, and biological studies of alkylthioalkylated anilines and their copper complexes are less investigated in comparison to their sulfonamide analogues. Copper ions are biologically relevant in living systems as Cu(I)/Cu(II) cuproproteins which transport molecular oxygen and act as good catalysts in related oxidation-reduction processes. Here, the spectral, structural, and antimicrobial properties of copper(II) complexes of 2-(methylthiomethyl)anilines are reported with the spectral property and antimicrobial activity of the complexes compared to their corresponding ligands.

2. Materials and Methods

2.1. Materials and Physical Measurements

The reagents and solvents used in the experimental procedures were of analytical grade and used without further purification. The elemental analysis was carried out on Elementar Analysensysteme varioMICRO V1.6.2 GmbH. 1H and 13C NMR spectra of the ligands were obtained in CDCl3 relative to the residual proton in the solvent on Bruker Avance 400 MHz NMR spectrometer. The midinfrared spectra (400–4000 cm−1) were determined as solids on PerkinElmer Spectrum 100 ATR-FTIR spectrometer. Far-infrared spectra (30–700 cm−1) were obtained in nujol mulls held between polyethene discs and recorded on Perkin Elmer Spectrum 400 FTIR/FIR spectrometer. The electronic spectra (250–1100 nm) of ligands and complexes were measured in DMF using PerkinElmer Lambda 25 UV/VIS Spectrometer. The solid reflectance spectra of the copper complexes (300–1500 nm) were obtained on Shimadzu UV-3100 UV-VIS-NIR Spectrometer. Conductivity measurements of the complexes were taken at room temperature on AZ 86555 conductivity instrument. A Gouy balance was used to determine the room temperature magnetic moments of the powdered samples employing Hg(II) tetrathiocyanatocobaltate(II) as a calibrant and diamagnetic corrections were made from Pascal’s constants.

2.2. Crystallographic Measurements

Crystallography data were collected at −73°C using a Bruker KAPPA APEX II diffractometer equipped with a graphite monochromator and a molybdenum fine focus sealed X-ray tube as source of X-ray (Mo- radiation, = 0.71073 Å) and an Oxford Cryostream 700 system for sample temperature control. Bruker APEX II software was used for instrument control. The structures of the compounds were solved and refined using SHELXL-97 software package [1315]. Numerical absorption corrections were done and all nonhydrogen atoms were refined anisotropically. The positions and temperature parameters of the hydrogen atoms were fixed to the adjacent atoms. Diagrams and publication materials were generated using ORTEP [16]. Crystal size (mm), 0.06 × 0.06 × 0.17; chemical formula (per unit cell), C8H10Cl2CuN2O2S; formula weight, 332.68; sum formula per unit cell, C16H20Cl4Cu2N4O4S2; formula weight, 665.40; monoclinic; P21/c; unit cell parameters: (Å) 5.5999(2), (Å) 27.2688(9), (Å) 7.6550(2), (°) 90.00, (°) 97.8850(10), (°) 90.00; 3), 1157.89(6); Z, 4; (K), 200(2); calc (Mg/m3), 1.908; absorption coefficient (mm−1), 2.512; absorption correction (min., max.), 0.6705, 0.8721; (000), 668; range for data collection (°), 2.79–27.99; limiting indices, , , ; reflections collected, 11213; unique reflections (int), 3530 (0.0232); completeness to , 27.99 (99.9%); refinement method, full-matrix least-squares on ; data/restraints/parameters, 2798/0/162; goodness-of-fit on , 1.080; final indices [], , w; indices (all data), , w = 0.0601; largest difference in peak and hole (e A−3), 0.383 and −0.337.

2.3. Antimicrobial Susceptibility Procedure

The ligands (1af) and copper complexes (2af) were screened in vitro for their antibacterial activity against Staphylococcus aureus ATCC 6538, Bacillus subtilis (subsp. spizizenii) ATCC 6633, and Escherichia coli ATCC 8739 and for antifungal activity against Candida albicans ATCC 2091. Ampicillin (AMP) and ketoconazole (KTZ) were, respectively, used as positive controls for the antibacterial and antifungal tests. All the growth media (Mueller Hinton agar (MHA), agar bacteriological, potato dextrose agar (PDA), and nutrient broth) were prepared in double-distilled water according to standard procedure. Sterile saline was prepared by dissolving 0.85 g saline in double-distilled water and making up to 100 mL. McFarland solution (0.5 turbidity standard) was prepared by adding 0.5 mL of 1% barium chloride to 99.5 mL of 1% sulphuric acid [17]. Agar disc diffusion method was employed to determine the susceptibility of the microorganisms to the test compounds [18, 19]. The preparation of the agar plates, culturing of the microbial strains, and the inoculation of the plates followed described procedure [20, 21]. Each microbial inoculum was standardized by reference to 0.5 McFarland turbidity standard [17]. Stock solutions (100 mg/mL) of ampicillin and ketoconazole were also prepared and diluted to lower concentrations [21].

2.3.1. Agar Disc Diffusion Method

The sterile assay disks were kept in sealed containers at 5°C and allowed to equilibrate to room temperature before use. The test compounds, namely, ligands (1a2f) and complexes (2a2f) were dissolved in DMF. Known concentrations of test solutions were delivered on to sterile assay disks of 6 mm diameter each using a micropipette; the quantity taken was 250 μg per disc. 125 μg of Ampicillin and ketoconazole was measured on separate disks and allowed to dry under the laminar flow. Six disks were placed on each inoculated agar plate containing the appropriate growth medium and incubated for 24 h (bacteria) and 60 h (fungus) at 37°C. The diameter of zone of inhibition of the microbial growth by each compound was thereafter measured. The tests were carried out in triplicate and the mean values are recorded in Table 5.

2.4. Synthesis of Ligands and Complexes

The ligands, 4-R-2-(methylthiomethyl)anilines (1a1f), were prepared according to reported procedure [2]. Appropriate aniline (10.7 mmol) and dimethyl sulfide (15.00 mmol) in dichloromethane were vigorously stirred at room temperature. -chlorosuccinimide (15.0 mmol) was added in small portions. The mixture was stirred for 10 min; triethylamine (15.0 mmol) was added and the mixture was heated at reflux for 12 h. The organic layer was extracted with 10% NaOH (25 mL) and dried over anhydrous magnesium sulfate. Solvent was removed in vacuo to give the crude which was purified by column chromatography on silica gel 60 (0.040–0.063 mm) using hexane: ether (4 : 1 vol/vol) as the eluent. Fractions were collected in test tubes in 30 mL portions and value of each fraction was determined on TLC plate (silica gel 60 F254). Fractions with similar values were combined and dried in vacuo to remove the solvent and the NMR spectra obtained to identify the desired product (Scheme 1).


The copper(II) complexes (2a2f) were prepared by adding equimolar amounts of cupric chloride dihydrate (0.65 mmol) in ethanol (2 mL) to a stirred solution of the ligand (0.65 mmol) in ethanol or a mixture of ethanol/dichloromethane (2 mL). The mixture was further stirred for 1 h and the resulting solid precipitates were filtered off, washed with cold ethanol, and dried under vacuum (Scheme 1).

3. Results and Discussion

The synthesis route for the copper complexes is shown in Scheme 1. The complexes are stable solids in air, with varying shades of green colouration, and their structures were established from their elemental analyses, infrared and electronic spectra and X-ray crystallography. The results of the elemental analysis are in good agreement with the calculated values of 1 : 1 metal to ligand combination for the copper complexes. The complexes are completely soluble in DMF and DMSO, partially soluble in other polar solvents such as water, acetonitrile, and methanol but are completely insoluble in nonpolar organic solvents. Low molar conductance values between 27.2 and 38.3 Ω−1 cm2 mol−1 obtained for the complexes in DMF indicate they are nonelectrolytes [22] and the nature of chlorine to metal bonds can be described as coordinative. The summary of the analytical data and other physical properties of the complexes are recorded in Table 1.

ComplexesMolecular formulaColourM. pt.
% found (calculated)Yield

Molar conductanceb

2MT 1aC8H11NSoil62.87 (62.70)7.08 (7.23)9.27 (9.14)19.61 (20.92)80
4Me-2MT 1bC9H13NSPale brown65-6663.12 (64.62)7.87 (7.83)8.09 (8.37)18.11 (19.17)69
4MeO-2MT 1cC9H13NOSoil57.97 (58.98)7.92 (7.15)7.51 (7.64)17.32 (17.50)26
4Cl-2MT 1dC8H10NSClPale brown69-7051.84 (51.19)5.51 (5.37)7.38 (7.46)16.49 (17.08)78
4Br-2MT 1eC8H10NSBrPale brown68-6941.25 (41.39)4.22 (4.34)5.89 (6.03)13.42 (13.81)62
4-NO2-2MT 1fC8H10N2O2SYellow70–7347.58 (47.39)5.30 (5.22)13.74 (13.82)16.01 (15.82)33
CuCl2(2MT)   2a c Cu(C8H11NS)Cl2 Green153–15533.30 (33.40)3.97 (3.85)4.86 (4.87)10.93 (11.15)912.3027.929.4
CuCl2(4Me-2MT)   2b Cu(C9H13NS)Cl2 Brown158–16036.19 (35.83)4.09 (4.34)4.56 (4.64)10.45 (10.63)891.9532.228.6
CuCl2(4MeO-2MT)   2c Cu(C9H13NOS)Cl2 Brown147–14934.09 (34.02)4.19 (4.12)4.30 (4.41)9.58 (10.09)891.7638.329.6
CuCl2(4Cl-2MT )  2d c Cu(C8H10ClNS)Cl2 Green158–16030.10 (29.83)2.86 (3.13)4.31 (4.35)9.90 (9.95)752.1229.528.5
CuCl2(4Br-2MT)   2e Cu(C8H10NSBr)Cl2 Green170–17226.35 (26.21)2.41 (2.75)3.86 (3.82)8.38 (8.75)792.2128.532.9
CuCl2(4NO2-2MT)   2f Cu(C8H10N2O2S)Cl2 Green146–14829.68 (28.88)2.91 (3.03)8.50 (8.42)9.73 (9.64)731.8727.231.5

Measured at room temperature, 298 K.
bMolar conductance of 10−3 M solution at 298 K, values given in  cm2 mol−1.
cReference [12].
3.1. NMR Spectra

The NMR shifts for the protons and carbon atoms of the respective ligands are shown in (Scheme 2, Table 2). The proton NMR spectra of the ligands can be classified into three distinct classes; the thiomethyl (–CH3) and methylene (–CH2) protons appear as singlet peaks and resonate in the ranges 1.97–2.02 δ and 3.59–3.70 δ, respectively. The broad singlet peaks found between 3.81 and 4.76 δ are due to amine (–NH2) protons and the peaks downfield in the region 6.58–7.96 δ which appear as multiplets are due to the aromatic protons. The ligands with the methyl or methoxy group show additional singlet peak due to methyl (–CH3) protons at 2.25 δ or methoxy (–OCH3) protons at 3.73 δ.

Ligands(C)1(C)2H (C)3H (C)4H (C)5H (C)6H (C)7H (C)8H9H (C)10

2MT(144.96)(121.19)7.05 d (130.49)6.76 t (117.96)7.14 t (128.21)6.71 d (116.15)3.71 s (35.14)2.01 s (14.32)4.06 s
4Me-2MT(142.62)(121.61)6.85 s (131.23)— (127.44)6.93 d (128.98)6.62 d (116.52)3.67 s (35.48)2.02 s (14.63)3.95 s 2.25 s (35.60)
4MeO-2MT(138.64)(123.71)6.70 d (116.46)— (152.21)6.64 s (113.45)6.64 d (117.41)3.64 s (35.48)1.99 s (14.57)3.81 s 3.73 s (55.56)
4Cl-2MT(143.85)(122.84)6.98 s (130.18)— (123.14)7.04 d (128.23)6.58 d (117.53)3.59 s (35.20)1.97 s (14.66)4.07 s
4Br-2MT(144.24)(109.72)7.13 s (132.83)— (123.47)7.18 d (130.99)6.60 d (117.82)3.60 s (35.00)1.98 s (14.57)4.08 s
4NO2-2MT(151.60)(119.95)7.96 s (126.68)— (138.42)8.02 d (125.08)6.67 d (114.76)3.70 s (34.94)2.00 s (14.57)4.76 s

s: singlet; d: doublet; t: triplet.
3.2. Infrared Spectra

Selected infrared bands of the ligands and copper complexes are recorded in Table 2. The vibrational frequencies in the 2MT ligands (1a1f) were characterized by those observed in primary amines [23]. The N–H symmetric and asymmetric stretches were found between 3320 and 3400 cm−1, respectively; NH2 scissor was in the range 1590–1600 cm−1 and C–N stretching frequency was seen around 1280 cm−1. The band expected from the thioether group due to C–S–C bend (around 1100 cm−1) and that due to C–S stretch between 650 and 780 cm−1 was not observed as they are weak bands and were masked by vibrations associated with the benzene ring [24]. There was no deprotonation of the amine hydrogen atoms upon complexation as two N–H stretches were observed, shifted to lower energies by 100–200 cm−1. The N–H bends were similarly shifted to lower frequencies (cm−1) in the complexes. The shift to lower frequency of these vibrational modes after chelation is a result of the electron density of the nitrogen being directed to the metal ion, leaving the amino protons less tightly bound to the nitrogen [25]. Copper to ligand vibrations were seen in the far infrared region; Cu–N was observed in the range 425–450 cm−1 [26] and the vibrations due to Cu–Cl stretches consist of a mixture of medium and intense bands in the complexes between 268 and 365 cm−1 [27, 28]. In the crystal structure of complex (2f) below, the arrangement of the ligand atoms around the Cu2+ center includes two chloride ions, one of them terminally bonded, while the other is linked to two other adjacent copper centres in a bridging mode. Frequencies between 268 and 303 cm−1 are assigned as Cu–Cl for equatorial bonds [29]. Bands close to 320 cm−1 were assigned to Cu–S stretches [30].

3.3. The Crystallographic Structure of [Cu(4NO2-2MT)] (2f)

A single crystal of (2f) was grown by the slow evaporation of a mixture of DMSO/EtOH solution (2 : 1 vol/vol). The atom numbering scheme and the selected bond distances and angles are listed in Table 3. The four corners of the square plane of (2f) are occupied by the aniline nitrogen (N1), thioether sulfur (S1), and two chloride ions (Cl1, Cl2) which have cis arrangement to each other. One chlorido ligand (Cl1) is terminally bonded, while the other (Cl2) is bonded to two other copper ions in adjacent molecules as a bridging ligand giving rise to an octahedral arrangement around each copper center. Hence the complex has a monomer formula of CuLCl2 (where L is the ligand) and the ORTEP drawing is shown in Figure 1. The presence of chloride bridges between the adjacent molecules results in a “ladder-like” polymeric structure seen in Figure 2. The bond distances for Cu1–N1 and Cu1–S1 which are 2.075(18) and 2.321(6) Å, respectively, fall within the expected ranges [31, 32] and the Cu1–S1 distance is typical of equatorially bound thioether sulfur [3340]. Cu–Cl lengths are observed at 2.255(6) Å (Cu1–Cl1 terminal bond), 2.318(5) Å (Cu1–Cl2 in the basal bond), 2.690(5) Å (Cu1–Cl2 bridging bond), and 2.932(5) Å (Cu1–Cl2 bridging bond). The longer distances observed for Cu1–Cl2 bonds are within the acceptable range for Cu–Cl distances for axial bonds in previously reported copper(II) octahedral compounds [32, 4143]. The Cu–Cu distance of 3.532 Å is normal for distorted octahedral structures [25]. The bond angles for the basal ligands trans to each other are 176.82° and 163.90° for N1–Cu1–Cl1 and S1–Cu1–Cl2, respectively. L(basal)–Cu–L(apical) angles which are ideally 90° range from 85.39° to 105.45°, the greater deviation being from S1–Cu1–Cl2 bond angle.

Compoundv (N–H)δ NH2v (C–N)v (Cu–L) (cm−1)Electronic spectra aλ max, nm ( , mol−1 dm3 cm−1)

L–H (1a)3424, 335216181272    259, 300
2a3294, 321716091251430, 398, 364, 327, 295, 274  259, 298, 322, 430, 925
  Solid353, 400, 706
L–CH3 (1b)3420, 334616251275  259, 306
2b3276, 322115991259446, 405, 335, 321, 294, 268259, 303, 330, 430, 916
Solid354, 450, 754
L–OCH3 (1c)3409, 334116261293  259, 319, 360
2c3256, 320216171272430, 364, 338, 303, 271259, 286, 336, 447, 595, 885
Solid352, 403, 479, 786
L–Cl (1d)3399, 330716251275275, 316
2d3261, 322116091244439, 398, 322, 297, 272261, 309, 335, 430, 936
Solid364, 405, 782
L–Br (1e)3398, 331716241275272, 312
2e3259, 321916071244437, 393, 341, 322, 293, 281262, 308, 333, 430, 920
Solid348, 425, 795
L–NO2 (1f)3450, 334716391278258, 295, 392
2f3267, 322216201250425, 380, 365, 323, 294, 271263, 301, 381, 399, 428, 925
Solid367, 450, 765

CT: charge transfer.
3.4. Magnetic Moment and Electronic Spectra

The magnetic moments of copper(II) complexes (2a–2f) are recorded in Table 1. The magnetic moments between 1.76 and 2.30 B. M. obtained for the complexes suggest the presence of one electron in the d9 copper(II) configuration. The increase from the spin-only value of 1.73 B. M could be due to spin orbit coupling or orbital contribution from the unpaired electron in the ground state [44]. The electronic spectra of the ligands and copper(II) complexes in DMSO are recorded in Table 2. The spectra of the ligands (1a–1f) consist of two high energy bands found in the range 250–320 nm arising from transitions of the phenyl ring; the ligands (1c) and (1f) show an additional band close to 360 and 390 nm, respectively, due to intraligand charge transitions of their methoxy and nitro groups. The electronic spectra of the copper(II) complexes in DMSO similarly show the transitions which are slightly shifted to shorter wavelengths as a result of decrease in conjugation of the system after complexation. Ligand to metal charge transfer transitions are observed; the band in the region 320–390 nm is assigned as NCu, while that between 400 and 450 nm is associated with S()Cu [25]. In the solid reflectance spectra of the complexes in Figure 3(a), two high energy bands due to charge transfer transitions are found near 350 and 400 nm, while the broad band in the range 700–800 nm is assigned to dd transition [25]. The description of the dd band of the complexes changes in DMSO (Figure 3(b)) and a broad low-energy band is observed in the near-infrared between 880 and 920 nm. The shift to lower energies, by approximately 100 nm, is indicative of geometry change in the complexes as a result of probable coordination of DMSO to copper(II). From the crystal structure, the Cu–Cl distance in the bridging bonds is long and could imply a possible replacement of the axial binding site through the bridging chlorido ligand by the high coordinating DMSO molecule. Previous studies on electronic spectra of similar copper(II) complexes in DMF suggested the coordination of the solvent molecule to the metal ion resulting in distorted octahedral or tetragonal structures [19]. The large bandwidth in the electronic spectra can be attributed to Jahn-Teller distortion which is commonly observed in octahedral Cu(II) complexes.

3.5. Antimicrobial Susceptibility Testing

The results for the disc diffusion susceptibility tests recorded in Table 4 shows the inhibitory activity of each ligand was improved upon chelation to copper ion. The higher activity of the complexes could be due to the increased lipophilicity conferred on the complex by the copper ion. It was also observed that the pure metal salt solution has an inhibitory effect on the microbial growth and it shows a measure of biological activity. In this study, the gram-positive bacteria were more susceptible to the test compounds than the gram-negative E. coli and the fungus C. albicans. Among the ligands and complexes screened, those with electron donating groups are seen to inhibit the microbial growth better than the electron withdrawing groups. The compounds with the methoxy moiety (1c) and (2c) demonstrate more inhibitory activity than other compounds (2b) with a methyl group showing a similar though less pronounced activity.



; ** ; *** .

CompoundDiameter of zonesa of inhibition (mm)
B. subtilis S. aureus E. coli C. albicans

AMP 125  g/disk403823
KTZ 125  g/disk23

250  g disc−1 sample concentration, disc diameter 6 mm.
bNI: No inhibition.

4. Conclusion

The copper(II) complexes (2a2f) formed in a 1 : 1 ligand to metal reaction stoichiometry and were characterized by the elemental analysis, IR and X-ray crystallography. A change in the structure of the complexes in the solid state is suspected as a result of the coordination of DMSO to the copper(II). Screening of the ligands and their copper complexes for in vitro antimicrobial activity against S. aureus, B. subtilis, E. coli, and C. albicans was carried out using agar disk diffusion as well as microbroth dilution techniques. The methoxy complex (2c) showed promising antibacterial activityagainst S. aureus and B. subtilis, while E. coli was not susceptible to any of the compounds at the concentration tested.

5. Extra Material

CCDC 888074 contains the supplementary crystallographic data for compound [CuCl2(4NO2-2MT)] (2f) (see Supplementary Material available online at Copies of these data can be obtained free of charge from the Cambridge Crystallographic Data Centre via

Conflict of Interests

The authors declare that there is no conflict of interests.


One of the authors (Temitope E. Olalekan) thanks the Organization of Women in Science for the Developing World (OWSDW) for providing a Research Fellowship and Rhodes University for academic bursary.

Supplementary Materials

The four corners of the square plane are occupied by the aniline nitrogen (N1), thioether sulfur (S1) and two chloride ions (Cl1, Cl2) which have cis arrangement to each other. One chlorido ligand (Cl1) is terminally bonded while the other (Cl2) is bonded to two other copper ions in adjacent molecules as a bridging ligand giving rise to an octahedral arrangement around each copper center. The presence of chloride bridges between the adjacent molecules results in a ‘ladder-like’ polymeric structure. The bond distances for Cu1–N1 and Cu1–S1 are 2.075(18) and 2.321(6) Å respectively. Cu–Cl lengths are observed at 2.255(6) Å (Cu1–Cl1 terminal bond), 2.318(5) Å (Cu1–Cl2 in the basal bond), 2.690(5) Å (Cu1–Cl2 bridging bond) and 2.932(5) Å (Cu1–Cl2 bridging bond). The Cu–Cu distance of 3.532 Å is normal for distorted octahedral structures. The bond angles for the basal ligands trans to each other are 176.82° and 163.90° for N1–Cu1–Cl1 and S1–Cu1–Cl2 respectively.

The data was collected at -73°. Numerical absorption corrections were done. All non-hydrogen atoms were refined anisotropically. The positions and temperature factors of the hydrogen atoms bonded to the N1, the amine nitrogen coordinated to the copper, were refined independently. The positions of all other hydrogen atoms were fixed by the positions of the atoms to which these were bonded but the isotropic temperature parameters were refined independently.

R1 = 0.0262 for 2366 Fo > 4sig(Fo) and 0.0354 for all 2798 data, wR2 = 0.0601, GooF = S = 1.080, Electron density synthesis with coefficients Fo-Fc, Highest peak 0.38 at 0.2249 0.3582 0.2013 [0.74 A from C6], Deepest hole -0.34 at 0.3433 0.4676 0.9741 [0.54 A from Cu1].

  1. Supplementary Material


  1. H. L. Holland, F. M. Brown, A. Kerridge, and C. D. Turner, “Biotransformation of organic sulfides. Part. 10. Formation of chiral ortho- and meta-substituted benzyl methyl sulfoxides by biotransformation using Helminthosporium species NRRL 4671,” Journal of Molecular Catalysis B: Enzymatic, vol. 6, no. 5, pp. 463–471, 1999. View at: Publisher Site | Google Scholar
  2. J. P. Chupp, T. M. Balthazor, M. J. Miller, and M. J. Pozzo, “Behavior of benzyl sulfoxides toward acid chlorides. Useful departures from the Pummerer reaction,” Journal of Organic Chemistry, vol. 49, no. 24, pp. 4711–4716, 1984. View at: Google Scholar
  3. P. G. Gassman and H. R. Drewes, “Selective ortho formylation of aromatic amines,” Journal of the American Chemical Society, vol. 96, no. 9, pp. 3002–3003, 1974. View at: Google Scholar
  4. J. Whysner, L. Verna, and G. M. Williams, “Benzidine mechanistic data and risk assessment: species- and organ-specific metabolic activation,” Pharmacology and Therapeutics, vol. 71, no. 1-2, pp. 107–126, 1996. View at: Publisher Site | Google Scholar
  5. H. Stunzi, “Can chelationbe important in the antiviral activity of isatin β-thiosemicarbazones?” Australian Journal of Chemistry, vol. 35, no. 6, pp. 1145–1155, 1982. View at: Google Scholar
  6. M. J. M. Campbell, “Transition metal complexes of thiosemicarbazide and thiosemicarbazones,” Coordination Chemistry Reviews, vol. 15, no. 2-3, pp. 279–319, 1975. View at: Google Scholar
  7. S. Padhyé and G. B. Kauffman, “Transition metal complexes of semicarbazones and thiosemicarbazones,” Coordination Chemistry Reviews, vol. 63, pp. 127–160, 1985. View at: Google Scholar
  8. L. F. Lindoy, S. E. Livingstone, and T. N. Lockyer, “S-dealkylation and S-alkylation reactions of metal chelates of sulfur ligands,” Inorganic Chemistry, vol. 6, no. 4, pp. 652–656, 1967. View at: Google Scholar
  9. L. F. Lindoy, S. E. Livingstone, and T. N. Lockyer, “Sulphur-nitrogen chelating agents. I. Metal complexes of 8-methylthioquinoline,” Australian Journal of Chemistry, vol. 19, no. 8, pp. 1391–1400, 1966. View at: Publisher Site | Google Scholar
  10. P. S. K. Chia, S. E. Livingstone, and T. N. Lockyer, “Sulphur-nitrogen chelating agents. II. Metal complexes of 2-(2-methylthioethyl)pyridine,” Australian Journal of Chemistry, vol. 19, no. 10, pp. 1835–1845, 1966. View at: Publisher Site | Google Scholar
  11. P. S. K. Chia, S. E. Livingstone, and T. N. Lockyer, “Sulphur-nitrogen chelating agents. III. Metal complexes of 2-(methylthiomethyl)pyridine,” Australian Journal of Chemistry, vol. 20, no. 2, pp. 239–255, 1967. View at: Publisher Site | Google Scholar
  12. K. Kratzl, H. Fostel, and R. Sobczak, “Metallkomplexe einiger o-methylthiomethyaniline (metal complexes of o-methylthiomethylaniline),” Monatshefte für Chemie, vol. 9, no. 103, p. 677, 1972. View at: Google Scholar
  13. G. M. Sheldrick, “A short history of SHELX,” Acta Crystallographica A: Foundations of Crystallography, vol. 64, no. 1, pp. 112–122, 2007. View at: Publisher Site | Google Scholar
  14. G. M. Sheldrick, “Crystal structure refinement incorporating chemical information,” in Electron Crystallography, D. L. Dorset, S. Hovmöller, and X. Zou, Eds., vol. 347 of NATO ASI Series, pp. 219–220, 1997. View at: Publisher Site | Google Scholar
  15. G. M. Sheldrick and T. R. Schneider, “SHELXL: high-resolution refinement,” Methods in Enzymology, vol. 277, pp. 319–343, 1997. View at: Publisher Site | Google Scholar
  16. L. J. Farrugia, “ORTEP-3 for windows—a version of ORTEP-III with a graphical user interface (GUI),” Journal of Applied Crystallography, vol. 30, no. 5, p. 565, 1997. View at: Google Scholar
  17. J. McFarland, “The nephelometer: an instrument for estimating the number of bacteria in suspensions used for calculating the opsonic index and for vaccines,” Journal of American Medical Association, vol. 49, no. 14, pp. 1176–1178, 1907. View at: Google Scholar
  18. A. W. Bauer, W. M. Kirby, J. C. Sherris, and M. Turck, “Antibiotic susceptibility testing by a standardized single disk method,” American Journal of Clinical Pathology, vol. 45, no. 4, pp. 493–496, 1966. View at: Google Scholar
  19. J. L. Rios, M. C. Recio, and A. Villar, “Screening methods for natural products with antimicrobial activity: a review of the literature,” Journal of Ethnopharmacology, vol. 23, no. 2-3, pp. 127–149, 1988. View at: Google Scholar
  20. S. M. Finegold and E. J. Baron, Bailey and Scott’s Diagnostic Microbiology, C. V. Mosby Co., St. Louis, Mo, USA, 7th edition, 1986.
  21. J. H. Jorgensen and J. D. Turnidge, “Susceptibility test methods: dilution and disk diffusion methods,” in Manual of Clinical Microbiology, P. R. Murray, E. J. Baron, J. H. Jorgensen, M. L. Landry, and M. A. Pfaller, Eds., vol. 1, pp. 1152–1172, American Society for Microbiology, Washington, DC, USA, 9th edition, 2007. View at: Google Scholar
  22. W. J. Geary, “The use of conductivity measurements in organic solvents for the characterisation of coordination compounds,” Coordination Chemistry Reviews, vol. 7, no. 1, pp. 81–122, 1971. View at: Google Scholar
  23. P. J. Kruger and D. W. Smith, “Amino group stretching vibrations in primary aliphatic amines,” Canadian Journal of Chemistry, vol. 45, no. 14, pp. 1611–1618, 1967. View at: Publisher Site | Google Scholar
  24. K. Nakamoto, Infrared and Raman Spectra of Inorganic and Coordination Compounds, Part I: Theory and Applications in Inorganic Chemistry, John Wiley & Sons, New York, NY, USA, 1984.
  25. R. J. H. Clark, “Metal-halogen stretching frequencies in inorganic complexes,” Spectrochimica Acta, vol. 21, no. 5, pp. 955–963, 1965. View at: Google Scholar
  26. J. A. Lee-Thorp, J. E. Rüede, and D. A. Thornton, “The infrared spectra (3500-150 cm−1) of aniline complexes of cobalt(II), nickel(II), copper(II) and zinc(II) halides,” Journal of Molecular Structure, vol. 50, no. 1, pp. 65–71, 1978. View at: Google Scholar
  27. I. S. Ahuja, D. H. Brown, R. H. Nuttall, and D. W. A. Sharp, “The preparation and spectroscopic properties of some aniline complexes of transition metal halides,” Journal of Inorganic and Nuclear Chemistry, vol. 27, no. 5, pp. 1105–1110, 1965. View at: Google Scholar
  28. G. F. Svatos, C. Curran, and J. V. Quagliano, “Infrared absorption spectra of inorganic coordination complexes. V. The N-H stretching vibration in coordination compounds,” Journal of the American Chemical Society, vol. 77, no. 23, pp. 6159–6163, 1955. View at: Google Scholar
  29. E. W. Ainscough, E. N. Baker, A. M. Brodie, and N. G. Larsen, “Copper co-ordination to thioether ligands. Spectroscopic studies of dimeric copper(II) complexes of 2-(3,3-dimethyl-2-thiabutyl)pyridine and the crystal structure of di-μ-bromo-bis{bromo[2-(3,3-dimethyl-2-thiabuty1)pyridine-NS]copper(II))},” Journal of the Chemical Society, Dalton Transactions, no. 10, pp. 2054–2058, 1981. View at: Publisher Site | Google Scholar
  30. K. Nakamoto, Infrared and Raman Spectra of Inorganic and Coordination Compounds, John Wiley & Sons, New York, NY, USA, 3rd edition, 1978.
  31. L. Escriche, M. Sanz, J. Casabó, F. Teixidor, E. Molins, and C. Miravitlles, “Closely related macrocyclic and acyclic tridentate, pyridine derivatives, containing sulphur, and their complexes. Crystal structures of {dichloro-3,10-dithia-16-azabicyclo[10.3.1]hexadeca-1(16),12,14-triene} copper(II) and [2,6-bis(ethyithiomethyl)pyridine]dichlorocopper(II),” Journal of the Chemical Society, Dalton Transactions, no. 9, pp. 1739–1743, 1989. View at: Publisher Site | Google Scholar
  32. S. B. Sanni, H. J. Behm, P. T. Beurskens et al., “Copper(II) and zinc(II) co-ordination compounds of tridentate bis(benzimidazole)pyridine ligands. Crystal and molecular structures of bis[2,6-bis(1′-methylbenzimidazol-2′-yl)pyridine]copper(II) diperchlorate monohydrate and (acetonitrile)[2,6-bis(benzimidazol-2′-yl)pyridine](perchlorato)copper(II) perchlorate,” Journal of the Chemical Society, Dalton Transactions, no. 6, pp. 1429–1435, 1988. View at: Publisher Site | Google Scholar
  33. M. Vaidyanathan, R. Balamurugan, U. Sivagnanam, and M. Palaniandavar, “Synthesis, structure, spectra and redox of Cu(II) complexes of chelating bis(benzimidazole)—thioether ligands as models for electron transfer blue copper proteins,” Journal of the Chemical Society, Dalton Transactions, no. 23, pp. 3498–3506, 2001. View at: Google Scholar
  34. P. C. Burns and F. C. Hawthorne, “Tolbachite, CuCl2, the first example of Cu2+ octahedrally coordinated by Cl,” American Mineralogist, vol. 78, no. 1-2, pp. 187–189, 1993. View at: Google Scholar
  35. J. G. Gilbert, A. W. Addison, A. Y. Nazarenko, and R. J. Butcher, “Copper(II) complexes of new unsymmetrical NSN thioether ligands,” Inorganica Chimica Acta, vol. 324, no. 1-2, pp. 123–130, 2001. View at: Publisher Site | Google Scholar
  36. M. D. Glick, D. P. Gavel, L. L. Diaddario, and D. B. Rorabacher, “Structure of the 14-membered macrocyclic tetrathia ether complex of copper(II). Evidence for undistorted geometries in blue copper protein models,” Inorganic Chemistry, vol. 15, no. 5, pp. 1190–1193, 1976. View at: Google Scholar
  37. E. N. Baker and G. E. Norris, “Copper co-ordination to thioether ligands: crystal and molecular structures of bis(2,5-dithiahexane)copper(II) bis(tetrafluoroborate) and bis(3,6-dithiaoctane)copper(I) tetrafluoroborates,” Journal of the Chemical Society, Dalton Transactions, no. 9, pp. 877–882, 1977. View at: Publisher Site | Google Scholar
  38. R. Louis, Y. Agnus, and R. Weiss, “Binuclear copper(II) “face to face” inclusion complex of a macrotricyclic ligand,” Journal of the American Chemical Society, vol. 100, no. 11, pp. 3604–3605, 1978. View at: Google Scholar
  39. B. Cohen, C. C. Ou, R. A. Lalancette, W. Borowski, J. A. Potenza, and H. J. Schugar, “Crystal and molecular structure of di-μ-chloro-bis[chloro(5,8-dithiadodecane)copper(II)], [Cu(BuSCH2CH2SBu)Cl2]2,” Inorganic Chemistry, vol. 18, no. 2, pp. 217–220, 1979. View at: Google Scholar
  40. G. R. Brubaker, J. N. Brown, M. K. Yoo, R. A. Kinsey, T. M. Kutchan, and E. A. Mottel, “Crystal and molecular structures of (1,8-bis(2-pyridyl)-3,6-dithiaoctane)copper(I) hexafluorophosphate and perchlorato(1,8-bis(2-pyridyl)-3,6-dithiaoctane)copper(II) perchlorate: stereodynamics of the copper(II)-copper(I) couple,” Inorganic Chemistry, vol. 18, no. 2, pp. 299–302, 1979. View at: Google Scholar
  41. B. K. Santra, P. A. N. Reddy, M. Nethaji, and A. R. Chakravarty, “Structural model for the CuB site of dopamine β-hydroxylase: crystal structure of a copper(II) complex showing N3OS coordination with an axial sulfur ligation,” Inorganic Chemistry, vol. 41, no. 5, pp. 1328–1332, 2002. View at: Publisher Site | Google Scholar
  42. B. K. Santra, P. A. N. Reddy, M. Nethaji, and A. R. Chakravarty, “Structural model for the CuB site of dopamine β-hydroxylase and peptidylglycine α-hydroxylating monooxygenase: crystal structure of a copper(II) complex showing N3OS coordination and axial sulfur ligation,” Journal of the Chemical Society, Dalton Transactions, no. 24, pp. 3553–3555, 2001. View at: Google Scholar
  43. R. D. Willett, G. Pon, and C. Nagy, “Crystal chemistry of the 4,4′-dimethyl-2,2′bipyridine/copper bromide system,” Inorganic Chemistry, vol. 40, no. 17, pp. 4342–4352, 2001. View at: Publisher Site | Google Scholar
  44. B. N. Figgis and J. Lewis, “The magneto chemistry of chelates,” in Modern Coordination Chemistry, J. Lewis and R. G. Wilkins, Eds., Interscienc, New York, NY, USA, 1960. View at: Google Scholar

Copyright © 2014 Temitope E. Olalekan 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.

2223 Views | 508 Downloads | 3 Citations
 PDF  Download Citation  Citation
 Download other formatsMore
 Order printed copiesOrder