# Synthesis, Characterization, and Antibacterial Studies of Pd(II) and Pt(II) Complexes of Some Diaminopyrimidine Derivatives

Authors: Peter A. Ajibade; Omoruyi G. Idemudia
Journal: Bioinorganic Chemistry and Applications
 (2013)

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## Abstract

Pd(II) and Pt(II) complexes of trimethoprim and pyrimethamine were synthesized and characterized by elemental analysis, UV-Vis, FTIR, and NMR spectroscopy. The complexes are formulated as four coordinate square planar species containing two molecules of the drugs and two chloride or thiocyanate ions. The coordination of the metal ions to the pyrimidine nitrogen atom of the drugs was confirmed by spectroscopic analyses. The complexes were screened for their antibacterial activities against eight bacterial isolates. They showed varied activities with the active metal complexes showing more enhanced inhibition than either trimethoprim or pyrimethamine. The Pd(II) complexes of pyrimethamine showed unique inhibitory activities againstP. aeruginosa and B. pumilus, and none of the other complexes or the drugs showed any activity against these bacteria isolates. The MIC and MBC determinations revealed that these Pd(II) complexes are the most active. Structure activity relationship showed that Pt(II) complexes containing chloride ions are more active, while for Pd(II) complexes containing thiocyanate ions showed more enhanced activity than those containing chloride ions.


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## Body

## 1. Introduction

The discovery of potent group of pyrimidines with pronounced antagonistic effect on folic acid in cultures ofLactobacilli[1] led to the development of pyrimethamine and trimethoprim. Pyrimethamine was developed through brilliant feet of organic synthesis guided by biochemical considerations [2]. Additional modifications led to the synthesis of trimethoprim that inhibits bacterial dihydrofolate reductase like other diaminopyrimidines and its consequence selection as antibacterial agent [3–5]. Trimethoprim is a broad-spectrum antimicrobial and also exhibits antiparasitic activities [6]. Due to intensive use and misuse, resistance has emerged against trimethoprim [7].Development of antimicrobial drugs was hailed as one of the great medical success story of the twentieth century [8]. At present, resistance against antimicrobial agents have become public health problem worldwide [9–15]. In the search for novel drugs against drug resistant diseases, the use of metal complexes has received tremendous attention [16–24] and resulted in a variety of exciting and invaluable drugs such as cis-platin [24]. Research are being undertaken in fields such as cancer [25–27], diabetes [28–32], arthritis [33], magnetic resonance imaging [34], metal-mediated antibiotics, antibacterial, antiviral, antiparasitic and radiosensitizers [35–38]. In continuation of our efforts [39–44] to develop metal-based therapeutics agents, the synthesis, characterization, and antibacterial studies of trimethoprim and pyrimethamine are presented.


## 2. Experimental

### 2.1. Materials and Physical Measurements

All reagents and solvents were of analytical grade and used without further purification. Elemental analyses were carried out on a Perkin-Elmer elemental analyzer. Melting point determination was obtained with the Gallenkamp melting point apparatus. Molar conductivity measurement (10−3 M solutions in dimethylformamide) was obtained on the CON 6/TDS 6 conductivity/TDS Meter. FTIR spectra of the complexes were recorded as KBr pellets on a Perkin-Elmer paragon 2000 FT-IR spectrophotometer in the range 4000–370 cm−1. Electronic spectra of the complexes were recorded on a Perkin-Elmer Lambda 25 spectrophotometer. The 1H spectra in DMSO-d6 were performed and recorded on a Varian-NMR-vnmr s400 MHz spectrometer at 25°C, using high-power proton decoupling, and pulse sequence: s2pul. Proton chemical shifts in DMSO-d6 were referenced to DMSO-d6 (1H-NMR, δ(DMSO) = 2.49 ppm). Chemical shifts for proton resonances are reported relative to tetramethylsilane. PtCl2(COD)2 and PdCl2(CH3CN)2 were prepared according to literature procedures [45, 46].


### 2.2. Synthesis of Metal Complexes of the Type [M(L)2Cl2]

A solution containing 1 mmol of the respective metal salts (PtCl2(COD)2, 0.260 g) and (PdCl2(CH3CN)2, 0.374 g) was added to colorless solutions of trimethoprim (2 mmol, 0.508 g) or pyrimethamine (2 mmol, 0.497 g) in 50 mL of methanol. The mixture was refluxed for 4 h and cooled to room temperature, and the solvent was removed in vacuo. The solid product was dried over CaCl2.


### 2.3. Synthesis of Metal Complexes of the Type [M(L)2(NCS)2]

A solution containing 1 mmol of the respective metal salts (PtCl2(COD)2, 0.260 g) and (PdCl2(CH3CN)2, 0.374 g) was added to colorless solutions of trimethoprim (2 mmol, 0.508 g) or pyrimethamine (2 mmol, 0.497 g) in 50 mL of methanol. The mixture was refluxed for 1 h, followed by the addition of a colourless solution of NH4NCS (2 mmol, 0.152 g) in methanol and refluxed further for 3 h and cooled to room temperature, and the solvent was removed in vacuo. The solid product was dried over CaCl2.


### 2.4. Antibacterial Studies

The antimicrobial activity of the synthesized compounds as well as their free ligands was studied by the zone of inhibition technique [47, 48] using Staphylococcus aureus (ATCC 6538), Streptococcus faecalis (ATCC 29212), Bacillus cereus (ATCC 10702), gram(−) Escherichia coli (ATCC 8739), Klebsiella pneumonia (ATCC 4352), Proteus vulgaris (ATCC 6830),Pseudomonas aeruginosa(ATCC 19582), and Bacillus pumilus(ATCC 14884) typed cultures as obtained from American Type Culture Collection (ATCC). The macrobroth dilution technique [49, 50] was used to determine the MIC. The MIC was taken as the lowest concentration of the tested complexes that shows no visible bacterial growth [51]. Samples of organisms were taken from plates which were used for the MIC test that were with no visible growth and subcultured by way of streaking onto a freshly prepared Mueller Hinton agar medium. MBC was carried out with the method of Olorundare et al. [52] and was taken as the lowest concentration of antibiotic at which all bacteria are killed. These plates were incubated at 35–37°C for 24 h and results taken as the MBC.


## 2.1. Materials and Physical Measurements

All reagents and solvents were of analytical grade and used without further purification. Elemental analyses were carried out on a Perkin-Elmer elemental analyzer. Melting point determination was obtained with the Gallenkamp melting point apparatus. Molar conductivity measurement (10−3 M solutions in dimethylformamide) was obtained on the CON 6/TDS 6 conductivity/TDS Meter. FTIR spectra of the complexes were recorded as KBr pellets on a Perkin-Elmer paragon 2000 FT-IR spectrophotometer in the range 4000–370 cm−1. Electronic spectra of the complexes were recorded on a Perkin-Elmer Lambda 25 spectrophotometer. The 1H spectra in DMSO-d6 were performed and recorded on a Varian-NMR-vnmr s400 MHz spectrometer at 25°C, using high-power proton decoupling, and pulse sequence: s2pul. Proton chemical shifts in DMSO-d6 were referenced to DMSO-d6 (1H-NMR, δ(DMSO) = 2.49 ppm). Chemical shifts for proton resonances are reported relative to tetramethylsilane. PtCl2(COD)2 and PdCl2(CH3CN)2 were prepared according to literature procedures [45, 46].


## 2.2. Synthesis of Metal Complexes of the Type [M(L)2Cl2]

A solution containing 1 mmol of the respective metal salts (PtCl2(COD)2, 0.260 g) and (PdCl2(CH3CN)2, 0.374 g) was added to colorless solutions of trimethoprim (2 mmol, 0.508 g) or pyrimethamine (2 mmol, 0.497 g) in 50 mL of methanol. The mixture was refluxed for 4 h and cooled to room temperature, and the solvent was removed in vacuo. The solid product was dried over CaCl2.


## 2.3. Synthesis of Metal Complexes of the Type [M(L)2(NCS)2]

A solution containing 1 mmol of the respective metal salts (PtCl2(COD)2, 0.260 g) and (PdCl2(CH3CN)2, 0.374 g) was added to colorless solutions of trimethoprim (2 mmol, 0.508 g) or pyrimethamine (2 mmol, 0.497 g) in 50 mL of methanol. The mixture was refluxed for 1 h, followed by the addition of a colourless solution of NH4NCS (2 mmol, 0.152 g) in methanol and refluxed further for 3 h and cooled to room temperature, and the solvent was removed in vacuo. The solid product was dried over CaCl2.


## 2.4. Antibacterial Studies

The antimicrobial activity of the synthesized compounds as well as their free ligands was studied by the zone of inhibition technique [47, 48] using Staphylococcus aureus (ATCC 6538), Streptococcus faecalis (ATCC 29212), Bacillus cereus (ATCC 10702), gram(−) Escherichia coli (ATCC 8739), Klebsiella pneumonia (ATCC 4352), Proteus vulgaris (ATCC 6830),Pseudomonas aeruginosa(ATCC 19582), and Bacillus pumilus(ATCC 14884) typed cultures as obtained from American Type Culture Collection (ATCC). The macrobroth dilution technique [49, 50] was used to determine the MIC. The MIC was taken as the lowest concentration of the tested complexes that shows no visible bacterial growth [51]. Samples of organisms were taken from plates which were used for the MIC test that were with no visible growth and subcultured by way of streaking onto a freshly prepared Mueller Hinton agar medium. MBC was carried out with the method of Olorundare et al. [52] and was taken as the lowest concentration of antibiotic at which all bacteria are killed. These plates were incubated at 35–37°C for 24 h and results taken as the MBC.


## 3. Results and Discussion

Pd(II) and Pt(II) complexes, trimethoprim and pyrimethamine, have been synthesized and characterized by elemental analysis, UV-Vis, FTIR, and1H and 13C-nmr spectroscopy. Conductivity measurements on the complexes showed that they are nonelectrolyte in solution. Generally all the complexes are insoluble both in polar and nonpolar solvents except polar coordinating solvents such as DMSO and DMF. The analytical data for the complexes are presented in Table 1 and proposed structures in Figure 1.Table 1
Analytical data and some physical properties of the metal complexes.
Analytical Data (%)
Complexes
Molecular formulae
Colour
C
H
N
Yield (%)
M.P (°C)
Cond. µS
Found (calc.)
Found (calc.)
Found      (calc.)
[Pd(tmp)2Cl2]
C28H36N8Cl2O6Pd
Orange
43.94 (44.37)
5.13 (4.79)
15.47 (14.78)
91
248–250
11.42
[Pd(tmp)2(SCN)2]
C30H36N10O6S2Pd
Yellow
44.42 (44.86)
3.97 (4.52)
17.01 (17.44)
92
242–245
9.03
[Pt(tmp)2Cl2]
C28H26N8Cl2O6Pt
Pale yellow
40.10 (39.72)
3.79 (4.29)
13.72 (13.24)
92
135–137
10.13
[Pt(tmp)2(SCN)2]
C30H36N10O6S2Pt
Pale yellow
40.94 (40.40)
4.22 (4.07)
16.27 (15.70)
88
167–171
7.02
[Pd(pyrm)2Cl2]
C24H26N8Cl4Pd
Orange
43.65 (42.72)
4.26 (3.88)
16.69 (16.61)
90
259–261
15.62
[Pd(pyrm)2(SCN)2]
C26H26N10Cl2S2Pd
Orange
43.46 (43.37)
3.76 (3.64)
19.66 (19.45)
92
80–82
40.80
[Pt(pyrm)2Cl2]
C24H26N8Cl4Pt
Pale yellow
37.99 (37.76)
3.88 (3.43)
14.93 (14.68)
89
200–202
39.80
[Pt(pyrm)2(NCS)2]
C26H26N10Cl2S2Pt
Pale yellow
39.90 (38.62)
3.77 (3.24)
16.98 (17.32)
97
180-181
52.80Proposed structures for the metal complexes.
(a)
(b)
(c)
(d)


### 3.1. Infrared Spectra

The FTIR spectra of the ligands and metal complexes were compared and assigned on careful comparison. The N—H stretching frequencies of the pyrimidine NH2 in the free trimethoprim shifted slightly in the metal complexes. It was observed in the same region, 3332–3461 cm−1, as in the free ligands. The slight shift is ascribed to hydrogen bonding and other noncovalent interactions in the metal complexes. The coordination of the metal ions to trimethoprim affected the v(C=N) stretching vibrations. The v(C=N) that occur at 1635 cm−1 in the free trimethoprim ligand shifted to lower frequencies in all the complexes confirming that the metal ions are coordinated directly to the pyrimidine nitrogen atom. Strong vibrations at 2111 and 2120 cm−1 in [Pd(tmp)2(NCS)2] and [Pt(tmp)2(NCS)2], respectively, are due to v(NCS) stretching vibrations and may be attributed to the presence of the thiocyanate ion in the coordination sphere of these complexes [53]. The band observed in the complexes in the region 542−502 cm−1 was attributed to v(Pd—N) and v(Pt—N) [54].Pyrimethamine possesses four potential coordination sites. A comparison of the spectra of pyrimethamine and the metal complexes showed that the bands due to symmetrical and asymmetrical stretching modes of NH2 in the spectrum of pyrimethamine undergo only very slight changes in the complexes. This indicates that the metal ions bond preferentially to pyrimethamine through the nitrogen atom of pyrimidine. The absorption band at 1629 cm−1 in the spectrum of the pyrimethamine is attributed to the v(C=N) of the pyrimidine ring. It shifted to 1612, 1619, 1639, and 1632 cm−1, in [Pd(pyrm)2Cl2], [Pd(pyrm)2(NCS)2], [Pt(pyrm)2Cl2], and [Pt(pyrm)2(NCS)2], respectively, which is a good indication that pyrimethamine is coordinated to Pd(II) and Pt(II) ions through the N(1) atom of the pyrimidine ring. The appearance of a prominent absorption bands observed at 2112 and 2107 cm−1 in the complexes [Pd(pyrm)2(NCS)2] and [Pt(pyrm)2(NCS)2], but absent in the free ligand one has is due to v(NCS) stretching frequency of the thiocyanate ion [55].
(1)M=PdorPt.


### 3.2. Electronic Spectra of the Complexes

The effect of complexation on the splitting of the d orbital is more marked for Pd(II) and Pt(II), and consequently their complexes are diamagnetic and majority of them are square planar. The electronic spectra of Pd(II) and Pt(II) complexes like any other square planar complexes can be assigned easily. However, the situation is complicated in the Pt(II) series by the expectation that the d-p transitions will occur at comparable energies to LMCT transitions, and a clear distinction between these two types of transition may be difficult. Pt(II) complexes of trimethoprim do not show any absorption band in the visible region of their electronic spectra, but the Pd(II) complexes display weak absorption bands at around 440 nm which is assigned to1B1g←1A1g and 1A2g←1A1g d-d transition of a four coordinate palladium complexes [56]. The absorption band in [Pd(tmp)2Cl2] is stronger than that of the [Pd(tmp)2(NCS)2], and this can be attributed to the more intense orange colour of [Pd(tmp)2Cl2] as compared to that of yellow [Pd(tmp)2(NCS)2]. The palladium complexes of pyrimethamine show absorption bands at 553 nm, and another absorption band in the region 450–480 nm in both complexes corresponding to 1B1g←1A1g and 1A2g←1A1g low spin allowed d-d transition [56], respectively. The d-d transition in the platinum complexes is not seen, and this can be evident from its pale yellow colour which makes the MLCT bands dominant, as compared to the deep orange colour of palladium [57]. All the four complexes display high energy absorption band around 300 nm which can be attributed to typical charge transfer transitions in the complexes [56, 57] confirming the square planar geometries proposed for the metal complexes.


### 3.3. NMR Spectroscopy of the Metal Complexes

1H-nmr spectra data of the trimethoprim complexes in d6-DMSO shows the presence of some of the proton signals as compared to that of the free trimethoprim ligand [58, 59]. The proton NMR of [Pt(tmp)2(NCS)2] showed three major peaks at the aromatic region integrating for only three protons at δ(ppm) 7.68, 7.46, and 6.61 ppm assigned to (s, 1H, H-4a, J = 1.2 Hz), (s, 1H, H-5b), and (s, 1H, H-1b), respectively. The protons of the methyl in the methoxyl group which are equivalent can be observed as a single peak at δ(ppm) 1.77 ppm integrated for three protons. In [Pd(tmp)2(NCS)2] four major peaks can also be observed in the aromatic region but only two of the peaks which are integrated for one proton each was successfully assigned at delta values of 8.25 and 7.96 ppm ascribed to (s, 1H, H-4a) and (s, 1H, H-5b), respectively. The 1H-nmr spectrum of [Pt(tmp)2Cl2] could not be resolved but the 13C-nmr gave useful information for the formation of the Pd(II) complex. The coordinations of the two different metals and their contributions in [Pt(tmp)2(NCS)2] and [Pd(tmp)2(NCS)2] can be seen from the slight shift of the proton nmr signals assigned in their spectra.1H and 13C-nmr spectra of pyrimethamine [60] were compared to those of the complexes. There was a significant shift in the chemical shift values upon complexation. The 1H-nmr spectra of [Pt(pyrm)2Cl2] in DMSO-d6 solutions showed chemical shift at δ(ppm) 7.51 (s, 1H, H-5b), 7.26 (s, 1H, H-3b), 6.75 (s, 1H, H-6b), and 6.55 (s, 1H, H-2b). The aliphatic region showed multiple signals between 2.20 and 1.00 ppm which support the presence of an ethyl group of the pyrimethamine ligand, integrating for five protons. In [Pt(pyrm)2(NCS)2], the chemical shift was observed at δ(ppm) 7.53 (s, 2H, H-5b, 3b), 7.28 (s, 1H, H-6b), and 6.98 (s, 1H, H-2b). Once again, the aliphatic region showed multiple signals between 2.20 and 1.00 ppm which support the presence of an ethyl group integrating for five protons. The two amino groups of pyrimethamine exhibit characteristic shifts which can be seen as a broad peak at chemical shift value at around 4.00 ppm in both complexes.The13C-nmr spectra of the metal complexes of trimethoprim were compared with that of free trimethoprim ligand [61] with a significant shift in the area that has been affected by the coordination to the metal ions. The signal at 155.91 ppm in the ligand has been shifted upfield to a value of 153.60 ppm in [Pt(tmp)2Cl2] assigned to C(2a, C6a), both of C=N carbon atom of the pyrimidine ring of trimethoprim. Other 13C-nmr signal of trimethoprim were observed at 136.69 ppm assigned to the quaternary carbon C(5a, C5b), 106.59 ppm C(1b, 5b), 60.99 ppm assigned to C7a, the peaks at 56.64 and 32.99 ppm assigned to C(2b, 3b, 4b) and CH3 bonded to the oxygen of the methoxyl. The 13C-nmr of [Pt(tmp)2(NCS)2] and [Pd(tmp)2(NCS)2] both have more peaks than that of the [Pt(tmp)2Cl2], probably due to the presence of a thiocyanate group NCS in the coordination sphere of these complexes. The resonance at 162.77 and 160.68 ppm in [Pt(tmp)2(NCS)2] and at 163.10 and 160.51 ppm in [Pd(tmp)2(NCS)2] corresponding to C=N (C2a, C6a) of the trimethoprim ligand shifted downfield and this can be ascribed to the coordination of the metal to the nitrogen of the pyrimidine ring. The quaternary carbon C5a, C5b chemical shift occurs at 155.94 and 153.53 ppm in [Pt(tmp)2(NCS)2] and at 154.83 and 153.72 ppm in [Pd(tmp)2(NCS)2]. The presence of a peak at 135 ppm in both complexes is an indication that the thiocyanate ions are present in the complex and coordinate through the nitrogen. The high intensity peaks at 56.67 and 56.68 ppm in [Pt(tmp)2(NCS)2] and [Pd(tmp)2(NCS)2] were assigned to the methoxyl carbon, the peaks at 60.85 ppm in [Pt(tmp)2(NCS)2] and 60.84 ppm in [Pd(tmp)2(NCS)2] were assigned to methylene C7a, and lastly the peaks at 33.19 and 33.58 ppm were assigned to the CH3 of the aliphatic region.The13C-nmr for both platinum complexes of pyrimethamine gave more information in assigning the necessary signals and affirming the probable structure of the complexes. In the spectra of [Pt(pyrm)2Cl2], the singlet resonance at 163.83 is assigned to carbon atom of C=N of the pyrimidine ring; there was a significant upfield shift which is probably due to the effect of coordination to the Pt(II) ion. The peak at 159.43 ppm was assigned to C5a. The phenyl ring carbon C1b–C6b can be seen in the range of 133.58–107.10 ppm. The aliphatic region consists of two peaks at 26.44 and 13.59 ppm assigned to the methylene and the methyl groups, respectively, from the ethyl of the pyrimethamine ligand. [Pt(pyrm)2(NCS)2] show a similar trend in the 13C-nmr spectrum; the singlet peak at 164.34 ppm was assigned to C(2a) of the pyrimethamine. The thiocyanate carbon is observed at 134.02 ppm [62, 63]. The carbons of the pyrimethamine phenyl ring were found in the range of 133.34–107.65 ppm. The aliphatic region consists of complex peaks at between 29.93 and 25.62 ppm, indicative of the presence of a methylene group.


### 3.4. Antibacterial Screening of the Metal Complexes

The complexes showed varied antibacterial activities against both gram-positive and gram-negative bacterial isolates (Table2). The highest zone of inhibition of 34 mm was recorded for [Pd(tmp)2Cl2] B. cereus. All Pd and Pt complexes of trimethoprim are active against E. coliand P. vulgaris. Their zones of inhibition varied between 28 and 32 mm as against 16 mm shown by trimethoprim drug. Trimethoprim and all its complexes are inactive against P. aeruginosaand B. pumilus. Of all the trimethoprim complexes, [Pd(tmp)2(NCS)2] appear to be the least active, inhibiting only E. coli, S. faecalis, and P. vulgaris. It must also be noted that, it might be least active but it is the only complex of trimethoprim that shows a zone of inhibition of 27 mm against S. faecalis whereas the other three complexes did not show any visible inhibition. For the trimethoprim complexes, the structure activity relationship showed that both Pd(II) and Pt(II) complexes containing chloride ions are the most active. They are active against two gram positive bacteria and three gram negative bacteria isolates with the Pt complexes, [Pt(tmp)2Cl2], showing relatively higher zones of inhibition against five bacteria isolates than the Pd(II) complex, [Pd(tmp)2Cl2]. It must be noted however that high zone of inhibition may not reveal for certain that a particular compound is a stronger antibacterial agent since this may be attributed to factors such as the rate of diffusion of the antibacterial agents and the amount of bacterial isolates present in a certain amount of agar solution [64].Table 2
Zone of inhibition exhibited by metal complexes at 40 mg/mL (mm).
Complexes
E.  coli
P.  aeruginosa
S.  aureus
S.   faecalis
B.  cereus
B. pumilus
K.  pneumonia
P.  vulgaris
[Pd(tmp)2Cl2]
30.0
NI
29.0
NI
32.0
NI
26.0
32.0
[Pd(tmp)2(NCS)2]
28.0
NI
NI
27.0
NI
NI
NI
28.0
[Pt(tmp)2Cl2]
32.0
NI
32.0
NI
34.0
NI
30.0
28.0
[Pt(tmp)2(NCS)2]
30.0
NI
25.0
NI
32.0
NI
NI
30.0
[Pd(pyrm)2Cl2]
NI
30
12
NI
NI
21
14
NI
[Pd(pyrm)2(NCS)2]
NI
33
29
NI
NI
20
33
NI
[Pt(pyrm)2Cl2]
14
NI
20
26
NI
NI
NI
NI
[Pt(pyrm)2(NCS)2]
20
NI
18
NI
28
NI
NI
30
Pyrimethamine
11
NA
13
12
10
NA
15
12
Trimethoprim
15.0
NA
12.0
18.0
17.0
NA
20.0
16.0
NI: no inhibition; NA: not applicable.The inhibition of the bacteria isolates by the pyrimethamine complexes are relatively fewer than those of complexes of trimethoprim (Table2). However, the results showed that Pd(II) complexes of pyrimethamine, [Pd(pyrm)2Cl2] and [Pd(pyrm)2(NCS)2], have zones of inhibition of 30 and 33 mm against P. aeruginosa and 14 and 33 mm against B. pumilus. None of the complexes of trimethoprim and neither trimethoprim nor pyrimethamine showed any visible activity against these bacteria isolates. The highest zones of inhibition of 33 mm were observed for [Pd(pyrm)2(NCS)2] against P. aeruginosa and K. pneumonia. Pyrimethamine inhibited the growth of six bacteria isolates whereas three of its metal complexes inhibited four bacteria isolates while [Pt(pyrm)2Cl2] inhibited only three bacteria isolates. In the trimethoprim metal complexes, the complexes containing the chloride ions are generally showed better antibacterial activities than those with NCS ions. In the pyrimethamine metal complexes, the NCS ion is the anion of choice for enhanced activity. The minimum inhibition concentrations (MICs) and minimum bactericidal concentrations (MBCs) of the compounds were evaluated and presented in Tables 3 and 4, respectively. It shows that the Pd(II) complexes of pyrimethamine are more active than the Pt(II) complexes of either trimethoprim or pyrimethamine. The lowest MIC values of 0.31 mg/mL were recorded for the Pd complexes: [Pd(pyrm)2Cl2] against K. pneumoniaand [Pd(pyrm)2(NCS)2] against S. aureus. The complexes also have MIC values of 0.63 mg/mL against S. aureus and B. pumilus for [Pd(pyrm)2Cl2] while [Pd(pyrms)2(NCS)2] values are against B. pumilusand K. pneumonia. Their MBC values against these bacteria isolates are also the lowest indicating their high antibacterial activities.Table 3
MIC values (mg/mL) of the metal complexes on selected bacteria.
Complexes
E.  coli
P.  aeruginosa
S.  aureus
S.   faecalis
B.  cereus
B. pumilus
K.  pneumonia
P.  vulgaris
[Pd(pyrm)2Cl2]
NI
5.0
0.63
NI
NI
0.63
0.31
NI
[Pd(pyrm)2(NCS)2]
NI
5.0
0.31
NI
NI
0.63
0.63
NI
[Pt(pyrm)2Cl2]
20.0
NI
10.0
5.0
NI
NI
NI
NI
[Pt(pyrm)2(NCS)2]
10.0
NI
10.0
NI
5.0
NI
NI
5.0
[Pd(tmp)2Cl2]
20.0
NI
10.0
NI
5.0
NI
5.0
10.0
[Pd(tmp)2(NCS)2]
10.0
NI
NI
10.0
NI
NI
NI
NI
[Pt(tmp)2Cl2]
20.0
NI
10.0
NI
10.0
NI
5.0
10.0
[Pt(tmp)2(NCS)2]
20.0
NI
10.0
NI
10.0
NI
NI
5.0
Pyrimethamine
20.0
NA
20.0
20.0
10.0
NA
20.0
10.0
Trimethoprim
20.0
NA
10.0
20.0
10.0
NA
10.0
10.0Table 4
MBC values (mg/mL) of the metal complexes on selected bacteria.
Complexes
E.  coli
P.  aeruginosa
S.  aureus
S.   faecalis
B.  cereus
B. pumilus
K.  pneumonia
P.  vulgaris
[Pd(tmp)2Cl2]
>20.0
NI
20.0
NI
5.0
NI
10.0
20.0
[Pd(tmp)2(NCS)2]
10.0
NI
NI
>20.0
NI
NI
NI
NI
[Pt(tmp)2Cl2]
20.0
NI
>20.0
NI
10.0
NI
10.0
>20.0
[Pt(tmp)2(NCS)2]
>20.0
NI
10.0
NI
>20.0
NI
NI
20.0
[Pd(pyrm)2Cl2]
NI
10.0
2.5
NI
NI
2.5
0.31
NI
[Pd(pyrm)2(NCS)2]
NI
10.0
0.63
NI
NI
1.25
2.50
NI
[Pt(pyrm)2Cl2]
20.0
NI
10.0
10.0
NI
NI
NI
NI
[Pt(pyrm)2(NCS)2]
>20.0
NI
20.0
NI
10.0
NI
NI
20.0
Pyrimethamine
>20.0
NA
>20.0
>20.0
>20.0
NA
20.0
>20.0
Trimethoprim
>20.0
NA
20.0
>20.0
20.0
NA
20.0
20.0


## 3.1. Infrared Spectra

The FTIR spectra of the ligands and metal complexes were compared and assigned on careful comparison. The N—H stretching frequencies of the pyrimidine NH2 in the free trimethoprim shifted slightly in the metal complexes. It was observed in the same region, 3332–3461 cm−1, as in the free ligands. The slight shift is ascribed to hydrogen bonding and other noncovalent interactions in the metal complexes. The coordination of the metal ions to trimethoprim affected the v(C=N) stretching vibrations. The v(C=N) that occur at 1635 cm−1 in the free trimethoprim ligand shifted to lower frequencies in all the complexes confirming that the metal ions are coordinated directly to the pyrimidine nitrogen atom. Strong vibrations at 2111 and 2120 cm−1 in [Pd(tmp)2(NCS)2] and [Pt(tmp)2(NCS)2], respectively, are due to v(NCS) stretching vibrations and may be attributed to the presence of the thiocyanate ion in the coordination sphere of these complexes [53]. The band observed in the complexes in the region 542−502 cm−1 was attributed to v(Pd—N) and v(Pt—N) [54].Pyrimethamine possesses four potential coordination sites. A comparison of the spectra of pyrimethamine and the metal complexes showed that the bands due to symmetrical and asymmetrical stretching modes of NH2 in the spectrum of pyrimethamine undergo only very slight changes in the complexes. This indicates that the metal ions bond preferentially to pyrimethamine through the nitrogen atom of pyrimidine. The absorption band at 1629 cm−1 in the spectrum of the pyrimethamine is attributed to the v(C=N) of the pyrimidine ring. It shifted to 1612, 1619, 1639, and 1632 cm−1, in [Pd(pyrm)2Cl2], [Pd(pyrm)2(NCS)2], [Pt(pyrm)2Cl2], and [Pt(pyrm)2(NCS)2], respectively, which is a good indication that pyrimethamine is coordinated to Pd(II) and Pt(II) ions through the N(1) atom of the pyrimidine ring. The appearance of a prominent absorption bands observed at 2112 and 2107 cm−1 in the complexes [Pd(pyrm)2(NCS)2] and [Pt(pyrm)2(NCS)2], but absent in the free ligand one has is due to v(NCS) stretching frequency of the thiocyanate ion [55].
(1)M=PdorPt.


## 3.2. Electronic Spectra of the Complexes

The effect of complexation on the splitting of the d orbital is more marked for Pd(II) and Pt(II), and consequently their complexes are diamagnetic and majority of them are square planar. The electronic spectra of Pd(II) and Pt(II) complexes like any other square planar complexes can be assigned easily. However, the situation is complicated in the Pt(II) series by the expectation that the d-p transitions will occur at comparable energies to LMCT transitions, and a clear distinction between these two types of transition may be difficult. Pt(II) complexes of trimethoprim do not show any absorption band in the visible region of their electronic spectra, but the Pd(II) complexes display weak absorption bands at around 440 nm which is assigned to1B1g←1A1g and 1A2g←1A1g d-d transition of a four coordinate palladium complexes [56]. The absorption band in [Pd(tmp)2Cl2] is stronger than that of the [Pd(tmp)2(NCS)2], and this can be attributed to the more intense orange colour of [Pd(tmp)2Cl2] as compared to that of yellow [Pd(tmp)2(NCS)2]. The palladium complexes of pyrimethamine show absorption bands at 553 nm, and another absorption band in the region 450–480 nm in both complexes corresponding to 1B1g←1A1g and 1A2g←1A1g low spin allowed d-d transition [56], respectively. The d-d transition in the platinum complexes is not seen, and this can be evident from its pale yellow colour which makes the MLCT bands dominant, as compared to the deep orange colour of palladium [57]. All the four complexes display high energy absorption band around 300 nm which can be attributed to typical charge transfer transitions in the complexes [56, 57] confirming the square planar geometries proposed for the metal complexes.


## 3.3. NMR Spectroscopy of the Metal Complexes

1H-nmr spectra data of the trimethoprim complexes in d6-DMSO shows the presence of some of the proton signals as compared to that of the free trimethoprim ligand [58, 59]. The proton NMR of [Pt(tmp)2(NCS)2] showed three major peaks at the aromatic region integrating for only three protons at δ(ppm) 7.68, 7.46, and 6.61 ppm assigned to (s, 1H, H-4a, J = 1.2 Hz), (s, 1H, H-5b), and (s, 1H, H-1b), respectively. The protons of the methyl in the methoxyl group which are equivalent can be observed as a single peak at δ(ppm) 1.77 ppm integrated for three protons. In [Pd(tmp)2(NCS)2] four major peaks can also be observed in the aromatic region but only two of the peaks which are integrated for one proton each was successfully assigned at delta values of 8.25 and 7.96 ppm ascribed to (s, 1H, H-4a) and (s, 1H, H-5b), respectively. The 1H-nmr spectrum of [Pt(tmp)2Cl2] could not be resolved but the 13C-nmr gave useful information for the formation of the Pd(II) complex. The coordinations of the two different metals and their contributions in [Pt(tmp)2(NCS)2] and [Pd(tmp)2(NCS)2] can be seen from the slight shift of the proton nmr signals assigned in their spectra.1H and 13C-nmr spectra of pyrimethamine [60] were compared to those of the complexes. There was a significant shift in the chemical shift values upon complexation. The 1H-nmr spectra of [Pt(pyrm)2Cl2] in DMSO-d6 solutions showed chemical shift at δ(ppm) 7.51 (s, 1H, H-5b), 7.26 (s, 1H, H-3b), 6.75 (s, 1H, H-6b), and 6.55 (s, 1H, H-2b). The aliphatic region showed multiple signals between 2.20 and 1.00 ppm which support the presence of an ethyl group of the pyrimethamine ligand, integrating for five protons. In [Pt(pyrm)2(NCS)2], the chemical shift was observed at δ(ppm) 7.53 (s, 2H, H-5b, 3b), 7.28 (s, 1H, H-6b), and 6.98 (s, 1H, H-2b). Once again, the aliphatic region showed multiple signals between 2.20 and 1.00 ppm which support the presence of an ethyl group integrating for five protons. The two amino groups of pyrimethamine exhibit characteristic shifts which can be seen as a broad peak at chemical shift value at around 4.00 ppm in both complexes.The13C-nmr spectra of the metal complexes of trimethoprim were compared with that of free trimethoprim ligand [61] with a significant shift in the area that has been affected by the coordination to the metal ions. The signal at 155.91 ppm in the ligand has been shifted upfield to a value of 153.60 ppm in [Pt(tmp)2Cl2] assigned to C(2a, C6a), both of C=N carbon atom of the pyrimidine ring of trimethoprim. Other 13C-nmr signal of trimethoprim were observed at 136.69 ppm assigned to the quaternary carbon C(5a, C5b), 106.59 ppm C(1b, 5b), 60.99 ppm assigned to C7a, the peaks at 56.64 and 32.99 ppm assigned to C(2b, 3b, 4b) and CH3 bonded to the oxygen of the methoxyl. The 13C-nmr of [Pt(tmp)2(NCS)2] and [Pd(tmp)2(NCS)2] both have more peaks than that of the [Pt(tmp)2Cl2], probably due to the presence of a thiocyanate group NCS in the coordination sphere of these complexes. The resonance at 162.77 and 160.68 ppm in [Pt(tmp)2(NCS)2] and at 163.10 and 160.51 ppm in [Pd(tmp)2(NCS)2] corresponding to C=N (C2a, C6a) of the trimethoprim ligand shifted downfield and this can be ascribed to the coordination of the metal to the nitrogen of the pyrimidine ring. The quaternary carbon C5a, C5b chemical shift occurs at 155.94 and 153.53 ppm in [Pt(tmp)2(NCS)2] and at 154.83 and 153.72 ppm in [Pd(tmp)2(NCS)2]. The presence of a peak at 135 ppm in both complexes is an indication that the thiocyanate ions are present in the complex and coordinate through the nitrogen. The high intensity peaks at 56.67 and 56.68 ppm in [Pt(tmp)2(NCS)2] and [Pd(tmp)2(NCS)2] were assigned to the methoxyl carbon, the peaks at 60.85 ppm in [Pt(tmp)2(NCS)2] and 60.84 ppm in [Pd(tmp)2(NCS)2] were assigned to methylene C7a, and lastly the peaks at 33.19 and 33.58 ppm were assigned to the CH3 of the aliphatic region.The13C-nmr for both platinum complexes of pyrimethamine gave more information in assigning the necessary signals and affirming the probable structure of the complexes. In the spectra of [Pt(pyrm)2Cl2], the singlet resonance at 163.83 is assigned to carbon atom of C=N of the pyrimidine ring; there was a significant upfield shift which is probably due to the effect of coordination to the Pt(II) ion. The peak at 159.43 ppm was assigned to C5a. The phenyl ring carbon C1b–C6b can be seen in the range of 133.58–107.10 ppm. The aliphatic region consists of two peaks at 26.44 and 13.59 ppm assigned to the methylene and the methyl groups, respectively, from the ethyl of the pyrimethamine ligand. [Pt(pyrm)2(NCS)2] show a similar trend in the 13C-nmr spectrum; the singlet peak at 164.34 ppm was assigned to C(2a) of the pyrimethamine. The thiocyanate carbon is observed at 134.02 ppm [62, 63]. The carbons of the pyrimethamine phenyl ring were found in the range of 133.34–107.65 ppm. The aliphatic region consists of complex peaks at between 29.93 and 25.62 ppm, indicative of the presence of a methylene group.


## 3.4. Antibacterial Screening of the Metal Complexes

The complexes showed varied antibacterial activities against both gram-positive and gram-negative bacterial isolates (Table2). The highest zone of inhibition of 34 mm was recorded for [Pd(tmp)2Cl2] B. cereus. All Pd and Pt complexes of trimethoprim are active against E. coliand P. vulgaris. Their zones of inhibition varied between 28 and 32 mm as against 16 mm shown by trimethoprim drug. Trimethoprim and all its complexes are inactive against P. aeruginosaand B. pumilus. Of all the trimethoprim complexes, [Pd(tmp)2(NCS)2] appear to be the least active, inhibiting only E. coli, S. faecalis, and P. vulgaris. It must also be noted that, it might be least active but it is the only complex of trimethoprim that shows a zone of inhibition of 27 mm against S. faecalis whereas the other three complexes did not show any visible inhibition. For the trimethoprim complexes, the structure activity relationship showed that both Pd(II) and Pt(II) complexes containing chloride ions are the most active. They are active against two gram positive bacteria and three gram negative bacteria isolates with the Pt complexes, [Pt(tmp)2Cl2], showing relatively higher zones of inhibition against five bacteria isolates than the Pd(II) complex, [Pd(tmp)2Cl2]. It must be noted however that high zone of inhibition may not reveal for certain that a particular compound is a stronger antibacterial agent since this may be attributed to factors such as the rate of diffusion of the antibacterial agents and the amount of bacterial isolates present in a certain amount of agar solution [64].Table 2
Zone of inhibition exhibited by metal complexes at 40 mg/mL (mm).
Complexes
E.  coli
P.  aeruginosa
S.  aureus
S.   faecalis
B.  cereus
B. pumilus
K.  pneumonia
P.  vulgaris
[Pd(tmp)2Cl2]
30.0
NI
29.0
NI
32.0
NI
26.0
32.0
[Pd(tmp)2(NCS)2]
28.0
NI
NI
27.0
NI
NI
NI
28.0
[Pt(tmp)2Cl2]
32.0
NI
32.0
NI
34.0
NI
30.0
28.0
[Pt(tmp)2(NCS)2]
30.0
NI
25.0
NI
32.0
NI
NI
30.0
[Pd(pyrm)2Cl2]
NI
30
12
NI
NI
21
14
NI
[Pd(pyrm)2(NCS)2]
NI
33
29
NI
NI
20
33
NI
[Pt(pyrm)2Cl2]
14
NI
20
26
NI
NI
NI
NI
[Pt(pyrm)2(NCS)2]
20
NI
18
NI
28
NI
NI
30
Pyrimethamine
11
NA
13
12
10
NA
15
12
Trimethoprim
15.0
NA
12.0
18.0
17.0
NA
20.0
16.0
NI: no inhibition; NA: not applicable.The inhibition of the bacteria isolates by the pyrimethamine complexes are relatively fewer than those of complexes of trimethoprim (Table2). However, the results showed that Pd(II) complexes of pyrimethamine, [Pd(pyrm)2Cl2] and [Pd(pyrm)2(NCS)2], have zones of inhibition of 30 and 33 mm against P. aeruginosa and 14 and 33 mm against B. pumilus. None of the complexes of trimethoprim and neither trimethoprim nor pyrimethamine showed any visible activity against these bacteria isolates. The highest zones of inhibition of 33 mm were observed for [Pd(pyrm)2(NCS)2] against P. aeruginosa and K. pneumonia. Pyrimethamine inhibited the growth of six bacteria isolates whereas three of its metal complexes inhibited four bacteria isolates while [Pt(pyrm)2Cl2] inhibited only three bacteria isolates. In the trimethoprim metal complexes, the complexes containing the chloride ions are generally showed better antibacterial activities than those with NCS ions. In the pyrimethamine metal complexes, the NCS ion is the anion of choice for enhanced activity. The minimum inhibition concentrations (MICs) and minimum bactericidal concentrations (MBCs) of the compounds were evaluated and presented in Tables 3 and 4, respectively. It shows that the Pd(II) complexes of pyrimethamine are more active than the Pt(II) complexes of either trimethoprim or pyrimethamine. The lowest MIC values of 0.31 mg/mL were recorded for the Pd complexes: [Pd(pyrm)2Cl2] against K. pneumoniaand [Pd(pyrm)2(NCS)2] against S. aureus. The complexes also have MIC values of 0.63 mg/mL against S. aureus and B. pumilus for [Pd(pyrm)2Cl2] while [Pd(pyrms)2(NCS)2] values are against B. pumilusand K. pneumonia. Their MBC values against these bacteria isolates are also the lowest indicating their high antibacterial activities.Table 3
MIC values (mg/mL) of the metal complexes on selected bacteria.
Complexes
E.  coli
P.  aeruginosa
S.  aureus
S.   faecalis
B.  cereus
B. pumilus
K.  pneumonia
P.  vulgaris
[Pd(pyrm)2Cl2]
NI
5.0
0.63
NI
NI
0.63
0.31
NI
[Pd(pyrm)2(NCS)2]
NI
5.0
0.31
NI
NI
0.63
0.63
NI
[Pt(pyrm)2Cl2]
20.0
NI
10.0
5.0
NI
NI
NI
NI
[Pt(pyrm)2(NCS)2]
10.0
NI
10.0
NI
5.0
NI
NI
5.0
[Pd(tmp)2Cl2]
20.0
NI
10.0
NI
5.0
NI
5.0
10.0
[Pd(tmp)2(NCS)2]
10.0
NI
NI
10.0
NI
NI
NI
NI
[Pt(tmp)2Cl2]
20.0
NI
10.0
NI
10.0
NI
5.0
10.0
[Pt(tmp)2(NCS)2]
20.0
NI
10.0
NI
10.0
NI
NI
5.0
Pyrimethamine
20.0
NA
20.0
20.0
10.0
NA
20.0
10.0
Trimethoprim
20.0
NA
10.0
20.0
10.0
NA
10.0
10.0Table 4
MBC values (mg/mL) of the metal complexes on selected bacteria.
Complexes
E.  coli
P.  aeruginosa
S.  aureus
S.   faecalis
B.  cereus
B. pumilus
K.  pneumonia
P.  vulgaris
[Pd(tmp)2Cl2]
>20.0
NI
20.0
NI
5.0
NI
10.0
20.0
[Pd(tmp)2(NCS)2]
10.0
NI
NI
>20.0
NI
NI
NI
NI
[Pt(tmp)2Cl2]
20.0
NI
>20.0
NI
10.0
NI
10.0
>20.0
[Pt(tmp)2(NCS)2]
>20.0
NI
10.0
NI
>20.0
NI
NI
20.0
[Pd(pyrm)2Cl2]
NI
10.0
2.5
NI
NI
2.5
0.31
NI
[Pd(pyrm)2(NCS)2]
NI
10.0
0.63
NI
NI
1.25
2.50
NI
[Pt(pyrm)2Cl2]
20.0
NI
10.0
10.0
NI
NI
NI
NI
[Pt(pyrm)2(NCS)2]
>20.0
NI
20.0
NI
10.0
NI
NI
20.0
Pyrimethamine
>20.0
NA
>20.0
>20.0
>20.0
NA
20.0
>20.0
Trimethoprim
>20.0
NA
20.0
>20.0
20.0
NA
20.0
20.0


## 4. Conclusions

We report the synthesis, characterization, and antibacterial studies of Pd(II) and Pt(II) complexes of trimethoprim and pyrimethamine. The complexes formulated as four coordinate square planar species consisting of two molecules of either trimethoprim or pyrimethamine and two chloride or thiocyanate ions. The complexes were characterized by elemental analysis, electronic, FTIR, and NMR spectroscopy. Spectroscopic analyses confirmed the coordination of the metal ions to the drug through the pyrimidine nitrogen atom. The antibacterial screening of the complexes showed varied activities but they are more active than the drugs. The MIC and MBC determinations revealed that the Pd(II) metal complexes are the most active.



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*Source: 549549-2013-03-12.xml*