OJICOpen Journal of Inorganic Chemistry2161-7406Scientific Research Publishing10.4236/ojic.2015.54011OJIC-60150ArticlesChemistry&Materials Science Synthesis, Characterization and Antibacterial Activity of Mixed Ligand (HL) Complexes Mn(ll), Co(ll), Ni(ll), Zn(ll), Cd(ll) and Hg(ll) with Azide (N<sub>3</sub><sup style="margin-left:-6px;">-</sup>) assimS. Sultan1*SajedM. Lateaf1DhuhaK. Rashid1Department of Chemistry, College of Education for pure Sciences, Ibn Al-Hiatham, University of Baghdad, Baghdad, Iraq* E-mail:ja.sultan@yahoo.com(ASS);31082015050410211112 June 2015accepted 5 October 8 October 2015© Copyright 2014 by authors and Scientific Research Publishing Inc. 2014This work is licensed under the Creative Commons Attribution International License (CC BY). http://creativecommons.org/licenses/by/4.0/

The complexes of mixed ligand (HL) as primary ligand with azide ion (N 3 -) as co-ligand with Mn(ll), Co(ll), Ni(ll), Zn(ll), Cd(ll) and Hg(ll) were prepared via reaction metal (ll) chloride salt with ligand (HL) and sodium azide (NaN 3) using 1:2:2 mole ratio in ethanol solvent, respectively. The complexes of mixed ligand (HL) were characterized by elemental microanalysis (C.H.N), atomic absorption chloride content, molar conductance, magnetic susceptibility, melting point, FTIR and UV-Vis spectral data. The anti bacterial activity with four kinds of bacteria, Staphylococcus aureus, Bacillus, Escherichia coli and Pseudomonas aureus was studied.

4-Aminoantipyrine Glyoxylic Acid Sodium Azide Schiff Base Azido Mixed Ligand1. Introduction

The chemistry of Schiff bases metal complexes is of interest because these species display a variety of reactivity mode and they possess catalytic and biological activity [1] . Metal complexes of nitrogen-oxygen chelating agents derived from 4-aminoantipyrine Schiff bases have been studied extensively due to their pronounced applications in biological, clinical, analytical and pharmacological areas [2] -[4] .

4-Aminoantipyrine, an antipyretic agent [5] is one of the pyrazole derivatives. Numerous synthetic compounds containing pyrazole moiety have been focused in the field of medicinal chemistry [6] because of their pharmacological, photographic, catalytic and liquid crystals applications [7] [8] . Glyoxylic acid and its derivatives play important roles in natural processes participating in the glyoxylate cycle which functions in plants and some microorganisms [9] . It has been widely used in organic synthesis for the manufacture of intermediate products in pharmaceutical [10] . The spectrophotometric methods are usually based on the reactivity of the aldehyde group [11] [12] . Azido-mixed ligand complexes particular interest has been focused on the azido ligand not only for its efficiency in ferromagnetic or antiferromagnatic coupling but also for its diversity in co- ordination modes, m-1, 1, (end-on EO), m-1, 3 (end-end, EE), m-1, 1, 1, m-1, 1, 3 or still other modes and polymetric bridging network, and a large number of azido-bridged complexes with different dimensionalities and various topologies have been reported in the literature [13] [14] . Polynuclear complexes and coordination polymer in which paramagnetic metal ions are bridged by short ligands have attracted great attention in recent years. The studies focusing on better understanding fundamental magnetic applications, a large number of a zide- bridged transition metal complexes, have been reported [15] .

2. Experimental

All chemicals were purchased from BDH, and used without further purifications.

2.1. Instrumentation

FTIR spectra were recorded in KBr on Shimadzu-8300 Spectrophotometer in the range of (4000 - 400 cm−1). The electronic spectra in H2O were recorded using the UV-Visible spectrophotometer type (spectra 190 - 900 nm) CECIL, England, with quartz cell of (1 cm) path length. The melting point was recorded on Gallen kamp Melting point Apparatus.

The Conductance Measurements were recorded on W. T. W. conductivity Meter. The metal contents of the complexes were determined by atomic absorption (A. A.) technique using a Shimadzu PR-5 with Orphic Printer atomic absorption spectrophotometer. Balance Magnetic Susceptibility model MSB-MLI was conducted for measuring the magnetic susceptibility.

The characterization of the new ligand (L) is achieved by 1H and 13C-NMR spectra were recorded by using a Bruker 300 MHZ (Switzerland). Chemical Shift of all 1H and 13C-NMR spectra were recorded in δ(ppm) unit downfield from internal reference tetramethylsilane (TMS), using D2O as a solvent. Elemental analysis for carbon, hydrogen was performed using a Euro Vector EA 3000 A Elemental Analysis (Italy).

2.2. Synthesis of Ligand and Complexes2.2.1. Synthesis of Ligand (1,5-Diemthyl-3-oxo-2-phenyl-2,3-dihydro-1H-pyrazol-4-ylimino) (HL)

A solution of (4-AAP) (0.203 g, 1 mmole) in ethanol (20 ml), and a few drop of 48% of HBr, was added to a solution of (Glyoxylic acid) (0.074 g, 1 mmol) in ethanol (10 ml). The mixture was refluxed for (6 hr) with stirring. The resulting was an orange solution allowed to cool and dried at room temperature, then washed with ethanol and re-crystallization to the precipitate with methanol/H2O to give orange crystals during (24 hr), m.p. (128 - 132)˚C.

2.2.2. Synthesis of [Co(HL)<sub>2</sub>(N<sub>3</sub>)<sub>2</sub>]∙2H<sub>2</sub>O Complex

A solution of (HL) (0.518 g, 2 mmole) in ethanol (5 ml) and a solution of NaN3 (0.13 g, 2 mmol) in ethanol (5 ml) were added to a stirred solution of CoCl2∙6H2O (0.238 g, 1 mmol) in ethanol (5 ml). The resulting mixture was stirred for (1 hr). Then the mixture was filtered and dried then the precipitate was washed with an excess of ethanol and dried at room temperature during (24 hr). A pale green crystals were obtained, m.p. (116 - 121)˚C. A similar method was used to prepare of Mn(II), Ni(II), Zn(II), Cd(II) and Hg(II) mixed ligand complexes.

3. Results and Discussion3.1. Characterization of Ligand (HL)

In this study, new Schiff base ligand (HL) type (NOO) donor atoms was synthesized according to the used method shown in Scheme 1.

Spectroscopic methods [FT-IR, UV-Vis, 1H NMR, 13C NMR] along with melting point and elemental microanalysis C.H.N. were used to characterization the new ligand (HL).

Scheme 1. Synthesis route of ligand (HL).

3.1.1. <sup>1</sup>H NMR Spectral Data

The 1H-NMR spectrum of ligand (HL) shows single peaks attributed to two methyl groups appeared at range (d1.06 - d2.91) ppm. The strong signal obtained at (d3.35) ppm. due to DMSO-d6. The weak peak at (d8.14) ppm was attributed to proton of azomethine group (-N=CH-). Single weak peak attributed to proton of (-COOH) appeared at (d9.30) ppm. The multiple chemical shifts around (6.98 - 7.47) ppm may assigned to aromatic protons. The two weak signals at d(3.04) and d(3.14) ppm refer to water molecule of DMSO [16] .

3.1.2. <sup>13</sup>C NMR Spectral Data

13C NMR spectrum of ligand (HL) shows chemical shifts at (15.54) ppm and (18.35) ppm refer to C5 and C6 for two CH3 group respectively. The chemical shifts at (61.79) ppm and (88.32) ppm were attributed to C3 and C4 of C=C in 4-AAP ring respectively. Signals related to aromatic carbon (C7 - C12) were detected at range (126.04 - 130.89) ppm. The chemical shift of C1 for carboxylic group appeared as expected downfield at (170.25) ppm. The two chemical shift at (165.51) ppm and (135.47) ppm were attributed to C2 for azomethine group (-N=CH-) and C13 to C=O for 4-AAP respectively. Finally, the chemical shift at (40.86) ppm is due to DMSO d6 [17] .

3.2. Characterization of Mixed Ligand (HL) Complexes with Azide

The complexes of mixed ligand, (HL) as primary ligand with azide ion as co-ligand with Mn(II), Co(II), Ni(II), Zn(II), Cd(II) and Hg(II) were prepared via reaction metal (II) chloride salt with ligand (HL) and sodium azide (NaN3) using 1:2:2 mole ratio in ethanol solvent respectively. The method of this synthesis shows in Scheme 2 and Scheme 3.

Spectroscopic methods [FT-IR, UV-Vis, A. A.] along with molar conductivity, elemental microanalysis C.H.N, Chloride content, magnetic susceptibility, melting point were used to characterize the prepared mixed ligand complexes. All mixed ligand complexes are stable in solution and soluble in methanol, ethanol, acetone, DMSO and DMF solvents. Some physical properties were listed in Table 1. Elemental microanalysis C.H.N, metal and chloride analysis are in a good agreement with calculated values, Table 2.

3.2.1. Molar Conductance

The molar conductance values, Table 1, of the soluble mixed ligand complexes in DMSO solvent in 10−3 M solution at room temperature refer to non-electrolytic nature [18] .

3.2.2. Magnetic Susceptibility

The magnetic susceptibility for all complexes were measured at room temperature and the effective magnetic moment (μeff) values [19] were listed in Table 3.

3.2.3. FT-IR Spectral Data

The IR spectra of mixed ligand complexes Co(II), Ni(II), Zn(II), Cd(II), and Hg(II), exhibited band at (1616) cm−1, (1624) cm−1, (1614) cm−1, (1616) cm−1, and (1635) cm−1, respectively, refers to stretching frequency uC=O of 4-AAP ring, which was shifted to lower frequency when its comparison with that of the free ligand (HL), showing that the coordination between oxygen atom of this group with metal ion has happened [20] . The IR spectrum of mixed ligand complex of Mn(II), showed no change in position of the stretching frequency of uC=O ring when it compare of free ligand, indicating that the oxygen atom of (C=O) ring wasn’t involved in coordination with Mn(II). The detected bands at (1593) cm−1, (1591) cm−1, (1593) cm−1, (1591) cm−1, (1591) cm−1, and (1591) cm−1 in the IR spectra of all mixed ligand complexes refer to stretching frequency of imine

Scheme 2. Synthesis route of mixed ligand complexes for Co(II), Ni(II), Zn(II), Cd(II) and Hg(II).

Scheme 3. Synthesis route of mixed ligand (HL) complex for [Mn(HL)2(N3)2(H2O)2]∙H2O.

Some physical properties and molar conductance (M.C) of mixed ligand (HL) complexes
ComplexesM.wt g/molYield %ColourM. P. ˚CM.C ohm−1∙cm2∙mol−1
[Mn(HL)2(N3)2(H2O)]∙H2O71178Dark green10012.22
[Co(HL)2(N3)2]∙2H2O69791Pale green1209.42
[Ni(HL)2(N3)2]∙3H2O714.792Pale olive12215.58
[Zn(HL)2(N3)2]∙3H2O721.488Pale orangedec. 108 - 1127.97
[Cd(HL)2(N3)2]∙2H2O750.489Pale orange1039.21
[Hg(HL)2(N3)2]∙3H2O856.692Pale orange1029.16
 Elemental microanalysis of mixed ligand (HL) complexes
ComplexesFound, (cal cu.)%
CHNMCl
[Mn(HL)2(N3)2(H2O)]∙H2O(43.88) 43.06(4.50) 3.85(23.62) 23.84(7.73) 7.26Nil
[Co(HL)2(N3)2(H2O)2]∙H2O(44.76) 44.03(4.01) 4.26(24.10) 23.67(8.46) 8.01Nil
[Ni(HL)2(N3)2]∙3H2O(43.65) 42.86(4.47) 3.82(23.50) 22.64(8.21) 7.75Nil
[Zn(HL)2(N3)2]∙3H2O(43.24) 42.75(4.43) 4.68(23.28) 22.85(9.06) 8.42Nil
[Cd(HL)2(N3)2]∙2H2O(41.57) 40.82(3.99) 3.52(22.38) 23.04(14.97) 14.62Nil
[Hg(HL)2(N3)2]∙3H2O(36.42) 35.86(3.73) 3.25(19.61) 19.18(23.41) 22.94Nil
 Magnetic susceptibility and m<sub>eff</sub>. (B.M) of some mixed ligand (HL) complexes
Complexes*Xg ´ 10−6XM ´ 10−6XA ´ 10−6meff. (B.M)Suggested structure
[Mn(HL)2(N3)2(H2O)2]∙H2O18.5713204.6512971.035.56Octahedral
[Co(HL)2(N3)2]∙2H2O14.089815.3810049.04.88Octahedral
[Ni(HL)2(N3)2]∙3H2O4.503217.883451.502.86Octahedral

group (-N=CH-) which were shifted to lower frequency when it compare with that of free ligand showing that the coordination with the metal ions was occurred via nitrogen atom of imine group (-N=CH-) [21] . The IR spectra of all mixed ligand complexes exhibited new strong splited band or new strong singlate band which wasn’t observed in the IR spectrum of free ligand (HL), this band was located at (2123 cm−1, 2058 cm−1) Mn(II), (2123 cm−1, 2102 cm−1) Co(II), (2121 cm−1, 2036 cm−1) Ni(II), (2125 cm−1, 2036 cm−1) Hg(II), (2065) cm−1 for Zn(II) and Cd(II), which was attributed to stretching frequency uasy.. While the new band at (1311) cm−1 for Mn(II) Co(II) and at (1317) cm−1 for Zn(II), Cd(II) and at (1313) cm−1 for Hg(II), was attributed to stretching frequency usy. [22] . These values of uasy. and usy. suggest the coordination between azide ion and metal ion. Further, the two bands observed at (1419) cm−1 and (1369) cm−1 in the IR spectrum of free ligand which are assigned to uasy. (COO−) and usy. (COO−) respectively, parically no or slightly change on these frequencies at complexation was observed, indicating noninvolvement of this group in coordination with metal ion [23] . In the IR spectra of mixed ligand complexes of Mn(II), Co(II), Ni(II), Zn(II), Cd(II), and Hg(II) abroad band was observed around (3464) cm−1 to (3390) cm−1 which was assigned to hydrate water molecules [24] , while the presence of coordinated water (aqua) in the structure of Mn(II) complex was suggested by a broad band at (3390) cm−1 and weak band at (931) cm−1 in the IR spectrum of Mn(II) complex, which refer to uO-H and δO-H for H2O coordination molecules [25] . The stretching frequency of uC=O for carboxylate group in IR spectra for all mixed complexes appeared as overlap with band of uC=O ring or as a weak band around (1735) cm−1. Two bands in the region (545 - 505) cm−1 and (505 - 445) cm−1 typical for the presence of M-N and M-O in the IR spectra for all mixed ligand complexes as new bands [26] . These Two bands were not present in the spectrum of free ligand (HL). Other bands in the IR for all complexes were listed in Table 4. These observation in the IR spectra of free ligand and its mixed complexes indicate that the ligand (HL) coordinate with Co(II), Ni(II), Zn(II), Cd(II), and Hg(II) via oxygen atom of (C=O) ring and nitrogen atom of imine group (-N=CH-), behaving bidentate ligand. But its behaves as monodentate ligand when it coordinate with Mn(II) via nitrogen atom of imine group (-N=CH-) only. While the azide ion coordinates with metal ion in all mixed ligand complexes as terminal ligand. According to these fact, the primary oxidation states of the metal ions Mn(II), Co(II), Ni(II), Zn(II), Cd(II), and Hg(II) ware satisfied by the presence of azide ion present inside the coordination sphere, that was proved by molar conductance values which were a good evidence for non-elec- trolytic complexes.

3.2.4. UV-Vis Spectral Data

The electronic spectral data for all mixed ligand complexes are summarized in Table 5, together with electronic

The FT-IR spectral data (cm<sup>−1</sup>) of ligand (HL) and its mixed complexes
CompoundsuO-HuC=O ringuC=O carbox.uN=C imineuCOO− asy.uCOO− sy.u asy.u sy.uC=C arom.uC-H arom.uC-C aliph.uC-H aliph.uM-NuM-O
(HL)342116451724160814191369--1586293911972900--
[Mn(HL)2(N3)2(H2O)2]∙H2O33901647Overlap1593141713692123 205813111570306411902927543505
[Co(HL)2(N3)2]∙H2O34421616Overlap1591142113712123 210213111573Overlap11972935505445
[Ni(HL)2(N3)2]∙3H2O3390162417351593141713632121 203613111575Overlap1168Overlap545475
[Zn(HL)2(N3)2]∙3H2O346416141735159114171373206513171560306611412933542445
[Cd(HL)2(N3)2]∙2H2O34461616Overlap159114191375206513171558306411882930505460
[Hg(HL)2(N3)2]∙3H2O33461635Overlap1591141713692125 203613131558306411882900505453
 Electronic spectral data of ligand (HL) and its mixed complexes
Compoundlnmu− (cm−1)(emaxmolar−1∙L∙cm−1)Electronic transitionSuggested structure
(HL)27636,2311885p ® p*-
34628,901614n ® p*
36227,624500n ® p*
[Mn(HL)2(N3)2(H2O)2]∙H2O29733,6702370Intra-ligandOh
34528,9862042Intra-ligand
35927,8551324Intra-ligand
47521,0532086A1g ® 4T2g(G)
63815,674416A1g ® 4T1g(G)
79412,59476A1g ® 4Eg(D)
[Co(HL)2(N3)2]∙2H2O28634,9652304Intra-ligandoh
34528,9862034Intra-ligand
36227,6241228Intra-ligand
65015,387134T1g ® 4A2g
87911,37744T1g ® 4T2g
[Ni(HL)2(N3)2]∙3H2O28135,5872218Intra-ligandOh
34728,8181152Intra-ligand
36527,397842Intra-ligand
42623,4743233A1g ® 3T2g(P)
79215,942103A1g ® 3T1g
87911,37723A1g ® 3T2g
[Zn(HL)2(N3)2]∙3H2O28634,9652278Intra-ligandOh
34528,9861489Intra-ligand
35428,249962Intra-ligand
[Cd(HL)2(N3)2]∙2H2O28634,9652276Intra-ligandOh
34528,9861485Intra-ligand
35428,249960Intra-ligand
[Hg(HL)2(N3)2]∙3H2O28435,2112274Intra-ligandOh
34528,9862085Intra-ligand
35428,2491266Intra-ligand

transitions and suggested geometries. The electronic spectra for all mixed ligand complexes displayed three absorption peaks in the ultraviolet region. The first peak at range (281 - 297) nm (35587 - 33670) cm−1 (emax = 2370 - emax = 2218) mol−1∙L∙cm−1, the second peak at (345, 347) nm (28986, 28818) cm−1 (emax = 1152 - emax = 2278) mol−1∙L∙cm−1, the third peak at (354 - 365) nm (28249 - 27397) cm−1 (emax = 842 - emax = 1324) mol−1∙L∙cm−1 were attributed to intra-ligand p → p*, n → p*, and n → p*, respectively [25] which exhibited bath chromic shift or hypsochromic shift when it comparison with that of free ligand (HL).

3.2.5. [Mn(HL)<sub>2</sub>(N<sub>3</sub>)<sub>2</sub>(H<sub>2</sub>O)<sub>2</sub>]∙H<sub>2</sub>O

The UV-Vis spectrum of Mn(II) complex, displayed three additional absorption peaks. The first peak at (475) nm (21053) cm−1 (emax = 208) mol−1∙L∙cm−1, the second peak at (638) nm (15674) cm−1 (emax = 41) mol−1∙L∙cm−1, the third peak at (794) nm (12594) cm−1 (emax = 7) mol−1∙L∙cm−1 were attributed to (d-d) spin-forbidden electronic transition type 6A1g → 4T2g(G), 6A1g → 4T1g(G), and 6A1g → 4Eg(D), confirming octahedral geometry about Mn(II) [27] .

3.2.6. [Co(HL)<sub>2</sub>(N<sub>3</sub>)<sub>2</sub>]∙2H<sub>2</sub>O

The electronic spectrum of Co(II) complex, showed two additional absorption peaks. The first peak at (650) nm (15,387) cm−1 (emax = 13) mol−1∙L∙cm−1, and the second peak at (879) nm (11377) cm−1 (emax = 4) mol−1∙L∙cm−1 were attributed to (d-d) spin-allowed electronic transition type 4T1g → 4A2g, and 4T1g → 4T2g, respectively, characteristic octahedral geometry around Co(II) [28] .

3.2.7. [Ni(HL)<sub>2</sub>(N<sub>3</sub>)<sub>2</sub>]∙H<sub>2</sub>O

The UV-Vis spectrum of Ni(II) complex, displayed three additional absorption peaks. The first peak at (426) nm (23,474) cm−1 (emax = 323) mol−1∙L∙cm−1, the second peak at (792) nm (15942) cm−1 (emax = 10) mol−1∙L∙cm−1, the third peak at (879) nm (11,377) cm−1 (emax = 2) mol−1∙L∙cm−1 were due to (d-d) spin-allowed electronic transition type 3A1g → 3T1g(P), 3A1g → 3T1g, and 3A1g → 3T2g, respectively, which were a good agreement for octahedral geometry of Ni(II) complexes [29] .

3.2.8. [Zn(HL)<sub>2</sub>(N<sub>3</sub>)<sub>2</sub>]∙3H<sub>2</sub>O, [Cd(HL)<sub>2</sub>(N<sub>3</sub>)<sub>2</sub>]∙2H<sub>2</sub>O, and Hg(HL)<sub>2</sub>(N<sub>3</sub>)<sub>2</sub>]∙3H<sub>2</sub>O

The electronic spectra of Zn(II), Cd(II), and Hg(II), respectively show no absorption peaks in the visible region, indicating (d10-system) for Zn(II), Cd(II), and Hg(II), that is mean no d-d electronic transition happened [27] .

3.3. Biological Activity of the Ligand (HL) and Mixed Ligand Complexes

Indicating that the new ligand and its mixed ligand complexes exhibited antibacterial activity against four kinds of bacterial: Staphylococcus aureus, Bacillus, Escherichia coli, and Pseudomonad aureus respectively, in Table 6, Figure 1 and Figure 2. The enhanced activity of the complexes can be explained on the bases of Overtone’s concept and Tweedy’s chelation theory [30] [31] .

Showed the inhibition circle diameter in millimeter for the bacteria after 24 hour in cubation paid (37˚C) for ligand (HL) and its mono and mated complexes
CompoundsE. coliPesudomonasBacillusStaphylococcus
DMSO57-5
Ligand (HL)13141211
[Mn(HL)2(N3)2(H2O)2]∙H2O-11-15
[Co(HL)2(N3)2]∙2H2O14--11
[Ni(HL)2(N3)2]∙3H2O1310-11
[Zn(HL)2(N3)2]∙3H2O13112111
[Cd(HL)2(N3)2]∙2H2O16163218
[Hg(HL)2(N3)2]∙3H2O26112612
 Inhibition diameter for ligands and complexes E. coli = Escherichia coli, Staph = Staphylococcus aureus Inhibition diameter for ligands and complexes Pse = Pesudomonas, Bacil = Bacillus4. Conclusions and the Proposed Molecular Structure for All Prepared Complexes

According to the characterization data for new Schiff base (HL) derived from 4-aminoantipyrine with glyoxylic acid, and its mixed ligand complexes based Schiff base liagnd HL primary ligand and azide ion (co-ligand), by FT-IR, UV-Vis, atomic absorption, 1H NMR, 13C NMR, magnetic susceptibility, molar conductivity, elemental microanalysis, chloride content alonge with melting point, we found that:

1) The Schiff base (HL) in mixed ligand complexes behaved bidentatc ligand through its azomethine nitrogen, oxygen atom of C=O group of five member ring with the central metal ions: Co(II), Ni(II), Zn(II), Cd(II) and Hg(II) forming complexes with molecular formula: [M(HL)2(N3)2]∙mH2O where: (MII = Co, Cd; m = 2), (MII = Ni, Zn, Hg; m = 3), except in Mn(II) complex, Schiff base (HL) behaved monodentatc ligand via azomethine nitrogen forming complex with molecular formula [Mn(HL)2(N3)2]∙H2O.

2) The octahedral geometrical structure was suggested for all prepared complexes based on the characterization data for all technique.

3) The antibacterial study showed that the complexes were more toxic to the strain of bacteria taken under study than the Schiff base ligand (HL).

Cite this paper

Jassim S.Sultan,Sajed M.Lateaf,Dhuha K.Rashid, (2015) Synthesis, Characterization and Antibacterial Activity of Mixed Ligand (HL) Complexes Mn(ll), Co(ll), Ni(ll), Zn(ll), Cd(ll) and Hg(ll) with Azide (N3 ). Open Journal of Inorganic Chemistry,05,102-111. doi: 10.4236/ojic.2015.54011

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