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. 2011 Jun 22;2011:531946. doi: 10.1155/2011/531946

Lanthanide Complexes of Substituted β-Diketone Hydrazone Derivatives: Synthesis, Characterization, and Biological Activities

W H Hegazy 1, 2,2,*, I H Al-Motawaa 1
PMCID: PMC3135049  PMID: 21799665

Abstract

A series of β-diketone hydrazone derivatives have been synthesized through condensation of β-diketone with aromatic aldehydes followed by reaction with phenylhydrazine. The structure of the ligands and intermediates are well defined through elemental and spectroscopic analyses. These hydrazones are potential ligands toward lanthanide metal ions. New complexes of trivalent Scandium, Yttrium, Lanthanum, and Cerium have been synthesized. The composition of these complexes is discussed on the basis of elemental analyses, IR, magnetic moments, and thermal analyses. The prepared complexes were screened for antibacterial and antifungal properties and have exhibited potential activity.

1. Introduction

Metal complexes of Schiff bases occupy a central role in coordination chemistry for analytical, physical, and biochemical purposes [1–19]. Many complexation process of β-diketones Schiff bases and/or hydrazones with lanthanide metal ions have been synthesized and characterized by elemental analysis, DTA-TG,X-ray, IR, fluorescence, UV spectra,and molar conductance [20–31].Biochemical activities of some complexes were reported [15].

The present investigation deals with the preparation of some new β-diketone dihydrazone derivatives (L1–L12) and their mononuclear Sc(III), Y(III), La(III), and Ce(III) complexes. The prepared ligands were characterized by elemental analysis, IR, 1H NMR, and mass spectra. Elemental analysis, IR, magnetic susceptibility measurements, TG, and conductivity measurements characterize the prepared complexes. The antibacterial activities of the prepared complexes were assessed against Gram-positive bacteria B. subtilis and S. aureus and Gram-negative bacteria E. coli and S. typhi. Prepared complexes were also screened for their antifungal activities against two fungi (A. niger and C. albicans).

2. Results and Discussion

The synthesized ligands L1–L12 were characterized by their physical properties, elemental analyses, IR Spectra, 1H NMR, and mass spectra. The data are given in Tables 1–4, respectively. Figure 1 represents tautomerization of the ligands.

Table 1.

Physical properties and elemental analyses of the ligands.

Color Yield% MP/°C Elemental analyses found (calc.)
%C %H %N
L1·4H2O
C24H23N4F
460.46		 Yellow 81 213 62.88 (61.65) 6.95 (6.75) 12.23 (12.36)
L2·7H2O
C24H23N4Cl
530.8		 Yellow 83 238 54.49 (54.40) 7.00 (6.74) 10.60 (11.36)
L3
C24H23N4Br
447.36		 Yellow 80 188 64.43 (63.69) 5.14 (500) 12.51 (11.37)
L4
C24H23N5O
397.41		 Orange-red 79 163 69.60 (69.73) 5.30 (5.57) 16.50 (16.95)
L5·3H2O
C29H23N4F
502		 Dark-green 88 225 69.31 (68.87) 6.17 (6.17) 11.15 (10.67)
L6·3H2O
C29H25N4Cl
518.88		 Light-pink 74 216 67.18 (66.64) 5.97 (5.22) 10.81 (10.41)
L7
C29H23N4Br
509.43		 Light-pink 74 20 68.42 (69.13) 4.95 (5.26) 10.99 (10.17)
L8·3H2O
C29H25N5O2
530		 Orange 67 231 65.78 (65.05) 5.86 (5.25) 13.23 (13.31)
L9
C34H27N4F
510.59		 Pale-beige 70 138 80.00 (80.90) 5.32 (5.32) 10.97 (10.95)
L10
C34H27N4Cl
527.04		 Beige 88 143 77.48 (76.61) 5.15 (4.82) 10.63 (9.99)
L11
C34H27N4Br
571.47		 Beige 65 173 71.46 (71.46) 4.75 (5.31) 9.80 (9.72)
L12
C34H27N5O2
537.58		 Orange 70 190 75.00 (74.25) 5.03 (5.22) 13.03 (12.65)
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Table 4.

m/z values (relative intensities) of the main fragments of the ligands.

[M]+ [A]+ [B]+ [C]+ [D]+ [E]+ [F]+ [G]+
L1 386 (11) 281 (20) 263 (19.0) 173 (18.1) 131 (10.40) 118 (31) 92 (12.6) 77 (100)
L2 402 (0.28) 297 (4.12) 263 (1.01) 173 (6.07) 131 (3.74) 118 (40) 92 (15.54) 77 (100)
L3 447 (0.12) 342 (1.34) 263 (0.79) 173 (8.90) 131 (2.61) 118 (29.64) 92 (23.06) 77 (100)
L4 413
(8)		 308 (12.7) 263 (41.1) 173 (11.3) 131 (12.7) 118 (28) 92
(53)		 77 (100)
L5 448 (1.11) 343 (6.1) 325 (13.1) 234 (16.2) 131 (4.4) 118 (13.5) 92
(7.7)		 77
(97)
L6 464 (26.0) 359 (22.27) 324 (0.19) 233 (4.64) 131 (0.82) 118 (2.57) 92 (3.67) 77 (100)
L7 509
18.9		 404
—		 325
13.1		 234
12.5		 131
1.0		 118
13.5		 92
7.7		 77
97.3
L8 475 (8.6) 370 (2.4) 324 (25.9) 233 (4.4) 131 (1.3) 118 (1.0) 92
—		 77
(62)
L9 510
(8)		 405
—		 386
—		 295 (40.2) 193 (11.6) 180 (4.2) 154 (1.1) 77 (72.6)
L10 527 (3.24) 422
—		 387 (2.8) 296
—		 194 (12.3) 181
—		 155 (2.03) 78
(84)
L11 571 (7.11) 466
—		 386
—		 295
32.9		 193
8.6		 180
25.7		 154
—		 77
81.4
L12 537 [M+1]+ (10) 432
(8)		 386
—		 297 (90) 193 (28) 180
(4)		 154 (29) 77
(31)
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Figure 1.

Figure 1

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Tautomerization of the ligands.

The elemental analyses of the ligands, Table 1, were found in good agreement with the calculated data (±0.9%).

The infrared spectra of the ligands show broad bands in the region 3449.46–3208.93 cm−1 assigned to N–H stretching vibrations, strong-intensity bands in the region 1601.2–1594.04 cm−1 assigned to C=N stretching vibrations, strong-intensity bands in the region 1502.21–1442.31 cm−1 assigned to interaction (coupling) between C–N stretching and N–H bending vibrations of the C–H–N group, and medium-intensity bands in the region 1376.13–1320.88 cm−1 assigned to N=N asymmetric stretching vibrations of the azoform of the ligands which formed as a result of the azo-hydrazo tautomerism [21]. Substitutions at the ortho- and parapositions enhance the mesomeric effect, which activate azo-hydrazo tautomerism. Weak intensity bands in the region 1281.66–1182.83 cm−1 are assigned to N–H inplane bending vibrations. Medium intensity bands in the region 1109.24–1060.85 cm−1 are assigned to N–N stretching vibrations. It is notable that no bands around 1700 cm−1 are observed which confirms the condensation of C=O groups of the Knövenagel condensation with phenylhydrazine [31, 32]. Two medium-intensity bands corresponding to C=C stretching vibrations of the aromatic rings are shown around 1600 and 1500 cm−1. Selected infrared data of the new ligands are listed in Table 2.

Table 2.

Selected infrared data of the ligands (cm−1).

υ(N–H) υ(C=N) υ(C–N)
δ(N–H)		 υ(N=N) δ(N–H) υ(N–N)
L1 3431 1600 1456 1373 1222 1072
L2 3430 1598 1443 1376 1249 1071
L3 3421 1598 1487 1375 1247 1072
L4 3433 1601 1442 1375 1192 1080
L5 3447 1598 1502 1365 1226 1098
L6 3429 1596 1497 1364 1221 1070
L7 3449 1594 1454 1359 1211 1066
L8 3346 1597 1444 1346 1240 1060
L9 3430 1595 1446 1346 1182 1109
L10 3448 1594 1445 1320 1260 1089
L11 3441 1595 1446 1359 1251 1072
L12 3408 1594 1451 1360 1281 1067
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The 1H NMR chemical shifts and coupling constants of DMSO-d6 are given in Table 3 suggesting the existence of two tautomeric forms except for ligands L9–L12. Two sets of signals are observed for the methyl group for ligands L1–L8. The resonance of the CH groups of the azoform is readily detectable for all ligands, whereas the peaks of the two NH groups of the hydrazoform (L1–L8) are broad in the case of L1–L5. The above IR and NMR spectroscopic features point to an azo-hydrazo tautomerism for ligands L1–L8 as shown below. Steric hindrance as well as electrondonating properties of the two phenyl groups prevent hydrazoform.

Table 3.

1HNMR spectroscopic data of the ligands (δ/ppm).

2 CH3 groups of azoform (d, 3H) 2 CH3 groups of hydrazoform (d, 3H) 2 CH groups of azoform (d, 2H) NH groups of hydrazoform (D2O exchangeable, s, 1H) Aromatic + methylenic protons (m)
L1 1.588 2.50 3.41 broad 7.12–7.50
L2 1.61 2.50 3.36 broad 6.85–7.75
L3 1.60 2.495 3.39 broad 6.70–7.60
L4 2.00 2.44 3.52 broad 6.71–7.54
L5 2.24 2.49 3.85 broad 6.56–7.63
L6 1.37 2.50 4.00 4.80, 7.77 6.91–7.25
L7 1.436 2.50 3.34 4.83, 7.98 6.83–7.68
L8 1.45 2.50 3.34 4.79, 8.21 7.06–7.77
L9 — — 3.45 — 6.42–7.97
L10 — — 3.40 — 6.62–7.95
L11 — — 3.50 — 6.50–7.12
L12 — — 3.38 — 7.39–8.23
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The mass spectroscopic fragmentation pathway of the ligands is shown in Scheme 1. The molecular ions in the mass spectra and their relative abundances are given in Table 4.

Scheme 1.

Scheme 1

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The general route of fragmentation of ligands.

Reaction of the ligands  L 1-2, L 4-5, L 7–9, and L12 with Sc(NO3)3·xH2O, Y(NO3)3·6H2O, Ce(NO3)3·6H2O, and La(NO3)3·6H2O were performed in ethanol. The complexes show 1 : 1 metal-to-ligand ratio as indicated by their elemental analyses. Their physical properties, magnetic moments, and elemental analyses are listed in Table 5. The results are in agreement with the postulated formulae (±1%). Complexes of ligands 3, 6, 10, and 11 cannot be separated in the solid state.

Table 5.

Physical properties, magnetic moments, and elemental analyses of complexes.

Complex (formula weight) Color MP/°C Yield% μ eff. BM found (calc.) Elemental analyses found (calc.)
%C %H %N
Sc[C24H25N7O10F] (635.51) White 255 60 — 46.27 (45.35) 3.70 (3.93) 15.14 (15.43)
Ce[C24H27N7O11F] (747.9) Yellow 302 64 2.31 (2.54) 36.81 (35.50) 3.95 (3.61) 13.11 (13.10)
Sc[C24H29N8O6Cl]NO3 (667.54) White 308 72 — 44.06 (43.14) 5.13 (4.34) 18.26 (18.87)
Y[C24H33N5O7](NO3)3·3H2O (831.86) Yellow-orange 288 78 — 35.81 (34.62) 3.87 (4.69) 14.07 (13.46)
Ce[C24H33N5O7](NO3)3·8H2O (973.12) Gray 294 77 2.26 (2.54) 30.81 (29.60) 4.35 (5.04) 12.45 (11.51)
Y[C29H29N7O11F] (757.01) White 313 62 — 45.22 (45.97) 3.74 (3.83) 13.22 (12.95)
Sc[C29H31N5O6Br]NO3 (731.95) Yellow 289 54 — 46.92 (44.54) 4.74 (4.23) 11.35 (12.48)
La[C29H31N5O6Br](NO3)2 (887.91) White 301 81 — 37.92 (39.19) 3.74 (3.49) 10.46 (11.04)
Y[C29H28N9O11]·0.5H2O (775.95) Yellow 296 58 — 45.88 (44.85) 4.21 (3.74) 15.99 (16.24)
La[C29H35N5O7](NO3)3 (889.98) Yellow-white 293 87 — 40.15 (39.10) 4.21 (3.93) 13.42 (12.58)
Sc[C34H35N4O4F](NO3)3·7H2O (938.83) White 314 60 — 42.15 (43.46) 5.31 (5.22) 10.70 (10.44)
Y[C38H39N7O11F] (877) White 287 65 — 52.15 (52.00) 4.85 (4.47) 10.90 (11.18)
La[C34H33N6O9F](NO3)·4H2O (960.85) Black 299 76 — 43.55 (42.42) 4.99 (4.27) 11.11 (10.20)
Ce[C34H37N4O5F](NO3)3·H2O (944) Yellow-white 301 66 2.42 (2.54) 43.31 (43.22) 4.58 (3.91) 12.21 (10.38)
Sc[C34H35N5O6](NO3)3·H2O (857.79) White 305 79 — 48.22 (47.57) 3.86 (4.38) (13.05) 14.31
Y[C38H39N8O13] (903.69) White 317 79 — 51.60 (50.44) 4.27 (4.31) 14.04 (12.39)
La[C34H37N5O7](NO3)3·3H2O (1011.91) White 306 63 — 42.20 (43.83) 3.99 (3.22) 10.16 (11.85)
Ce[C34H33N6O11](NO3)·H2O (935.0) Brown 288 72 2.37 (2.54) 45.27 (43.63) 4.38 (3.52) 10.44 (11.90)
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To achieve an idea about the groups involved in complex formation as well as the influence of the electrical field of the central metal ion on the change distribution within the ligand, the spectra of the complexes were carefully compared with those of the ligands.

The IR spectra of all complexes exhibit broad bands around 3748.80–3413.39 cm−1, which are attributed to O–H stretching vibrations of the associated water molecules that may be water of hydration or coordinated molecules. N–H and O–H stretching vibrations of complexes are overlapped for eight complexes. The N–H stretching vibrations of the other ten complexes show shifts to wave numbers differing from those of the free ligand (~315–45 cm−1). Red chemical shifts are observed (~7–60 cm−1) which are attributed to C=N stretching vibrations. Positive chemical shifts (~10–75 cm−1) is also detected for the C=N stretching vibrations and N–H inplane bending vibrations. Red shifts for complexes compared with ligands (~6–35 cm−1), (~5–91 cm−1), and (~7–50 cm−1) are seen for N=N stretching vibrations, N–H inplane bending vibrations, and N–N stretching vibrations, respectively. All these shifts in infrared spectra of the complexes compared with those of the ligands suggest coordination through the two lone pairs of electrons of the two sp2 nitrogen atoms of the hydrazoform as a bidentate ligand forming two stable six-membered rings. The infrared spectral data of the complexes are listed in Table 6.

Table 6.

Selected infrared data of complexes (cm−1).

Complexes υ(O–H) υ(N–H) υ(C=N) υ(C–N) + δ(N–H) υ(N=N) δ(N–H) υ(N–N)
Sc-L1 3425 overlap 1598 1503 1365 1225 1079
Ce-L1 3427 overlap 1596 1499 1397 1248 1069
Sc-L2 3445 3208 1613 1493 1360 1281 1067
Y-L4 3445 3300 1610 1503 1381 1227 1097
Ce-L4 3611 overlap 1648 1457 1372 1228 1157
Y-L5 3748 overlap 1609 1505 1382 1235 1156
Sc-L7 3450 3331 1596 1490 1382 1235 1072
La-L7 3423 overlap 1606 1499 1379 1253 1089
Y-L8 3455 3395 1597 1512 1345 1224 1062
La-L8 3538 3342 1594 1511 1382 1246 1105
Sc-L9 3500 3448 1617 1492 1365 1242 1113
Y-L9 3540 3116 1592 1444 1361 1210 1168
La-L9 3523 overlap 1609 1494 1383 1211 1020
Ce-L9 3413 3115 1591 1489 1356 1208 1168
Sc-L12 3435 overlap 1594 1491 1360 1290 1067
Y-L12 3427 overlap 1596 1499 1379 1248 1069
La-L12 3430 3430 1603 1496 1383 1347 1106
Ce-L12 3500 3412 1653 1492 1383 1299 1087
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The thermograms of the complexes show a loss of hygroscopic water molecules from 85 to 105°C. The anhydrous complexes show thermal stability up to 130°C. Removal of coordinated water molecules takes place at 130–260°C. The coordinated water molecules are found to be one for complexes Sc-L 1, two for complexes Ce-L 1, Y-L 5, three for complexes Sc-L 7, La-L 7, La-L 9, and Ce-L 12, four for complexes Sc-L 9 and Sc-L 12, and five for complexes Y-L 4, Ce-L 4, Y-L 4, Ce-L 9, and La-L 12. TG shows no coordinated water molecules in the complexes Sc-L 2, Y-L 8, Y-L 9, and Y-L 12.

The magnetic moments of complexes given in Table 7 suggest diamagnetic characters for Sc(III), Y(III), and La(III) complexes whereas Ce(III) complexes have paramagnetic characters ranging from 2.42–2.26 J·T−1 [33] being consistent with mononuclear complexes and free from antiferromagnetism. The deviation of the values from the theoretical value suggests that the 4f electron participate in the bond formation of the metal to the ligand.

Table 7.

Thermogravimetric results of the complexes.

Complexes Hygroscopic water Coordinated water
T/°C % Weight loss No. of water molecule T/°C % Weight loss No. of water molecule
found calc found calc
Sc[L1(NO3)3 (H2O)] — — — — 130–235 2.62 2.78 1
Ce[L1(NO3)3 (H2O)2] — — — — Up to 220 4.89 4.72 2
Sc[L2(NO3)2 (NH3)2]NO3 — — — — — — — —
Y[L4(H2O)5](NO3)3·3H2O 92 6.18 6.49 3 130–210 9.20 10.82 5
Ce[L4(H2O)5](NO3)3·8H2O 90 14.20 12.80 8 130–210 10.20 9.25 5
Y[L5(NO3)3 (H2O)2] — — — — 160–210 3.99 4.78 2
Sc[L7(NO3)(H2O)3](NO3)2 — — — — 170–220 6.42 7.38 3
La[L7(NO3)(H2O)3](NO3)2 — — — — 180–240 6.49 6.08 3
Y[L8(NO3)3 (NH3)]·0.5H2O 98 1.13 1.16 0.5 — — — —
La[L8(H2O)5](NO3)3 — — — — 190–250 11.63 10.11 5
Sc[L9(H2O)4](NO3)3·7H2O 90 14.60 13.42 7 140–210 6.22 7.67 4
Y[L9(NO3)3 (C2H5OH)2] — — — — — — — —
La[L9(NO3)2 (H2O)3](NO3)·4H2O 85 7.00 7.49 4 130–160 5.58 5.62 3
Ce[L9(H2O)5](NO3)3·H2O 105 2.47 1.95 1 160–220 8.95 9.73 5
Sc[L12(H2O)4](NO3)3·H2O 100 2.05 2.10 1 160–260 9.19 8.39 4
Y[L12(NO3)3 (C2H5OH)2] — — — — — — — —
La[L12(H2O)5](NO3)3·3H2O 95 4.00 5.37 3 130–160 11.70 10.95 5
Ce[L12(NO3)2(H2O)3](NO3)·H2O 100 2.17 1.95 1 130–220 5.20 5.86 3
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The thermogravimetric results given in Table 7 and the elemental analyses suggest that Sc-L2 and Y-L8 complexes complete their coordination sphere by ammonia molecules, Y-L9 complete its coordination sphere by ethanol molecules and Sc-L1, Ce-L1, Y-L4, Ce-L4, Y-L5, Sc-L7, La-L7, La-L8, Sc-L9, Ce-L9, La-L9, Sc-L12, La-L12, and Ce-L12 complexes complete their coordination sphere by water molecules. Y-L12 complex complete its coordination sphere by ammonia and ethanol molecules.

Conductivity measurements using conductivity meter of platinum electrodes for mmol concentrations of complex solutions in DMF at 25°C show that Sc-L1, Ce-L1, Y-L5, Y-L8, Y-L9, and Y-L12 are neutral, whereas other complexes measure ~213.42–197.63 cm3·Ohm−1·mol−1, suggesting the presence of free nitrate anions.

Elemental analyses, conductivity measurements, magnetic susceptibility measurements, and thermogravimetry of the complexes reinforce each other; suggesting octahedral geometry with coordination number 6 for the complexes Sc-L1, Sc-L2, Sc-L7, La-L7, Y-L8, Sc-L9, and Sc-L12, whereas they suggest distorted pentagonal bipyramid structure with coordination number 7 for other complexes [34].

In the light of the above discussion, representative structures of the complexes may be as follow:

The metal complexes and standard drugs (ampicillin, tetracycline, and salicylic acid) were tested for their antimicrobial activity at a concentration of 60 μg mL−1 in DMF using the paper disc diffusion method [35, 36]. The diameter of the susceptibility zones was measured, and the results are given in Table 8. The susceptibility zones measured were the clear zones around the discs inhibiting the microbial growth. It is clear that Scandium(III) complexes are more active towards bacterium, yeast, and fungi. Because of the relatively large positive charge density on Scandium atom, it is partially shared with the donor nitrogen atoms of the ligands, and there is π-electron delocalization over the whole chelate ring [36, 37]. This in turn, increases its permeation through the lipoid layers of the microorganism membranes. Other factors such as solubility, conductivity, and dipole moment may also increasing activity [36, 37]. Representative structures of the complexes are given in Figure 2.

Table 8.

Antimicrobial activity data for the complexes*.

Complex B. subtilis S. aureus E. coli S. typhi A. niger C. albicans
Sc-L1 15 7 10 6 + ++
Ce-L1 9 — 7 — + +
Sc-L2 10 6 6 11 ++ ++
Y-L4 7 7 7 7 + +
Ce-L4 6 — 7 6 + ++
Y-L5 10 7 6 8 — +
Sc-L7 11 10 10 12 + +
La-L7 6 — — 6 — —
Y-L8 6 8 8 8 + +
La-L8 6 7 6 6 + —
Sc-L9 12 11 12 12 + +
Y-L9 14 9 13 9 + +
La-L9 6 — — — + +
Ce-L9 7 6 6 6 + +
Sc-L12 17 10 10 15 ++ +++
Y-L12 11 11 10 8 + ++
La-L12 11 7 7 — — ++
Ce-L12 12 9 10 7 ++ +++
Ampicillin 18 16 15 14 — —
Tetracycline 16 15 17 17 — —
Salicylic Acid — — — — ++++ ++++
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*Inhibition zone diameter (% inhibition): +, 6–9 mm (33–50%); ++, 10–12 mm (55–67%); +++, 13–15 mm (72–83%); ++++, 16–18 mm (89–100%).

Percentage inhibition values were relative to inhibition zone (18 mm) with 100% inhibition.

Figure 2.

Figure 2

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Representative structures of the complexes.

3. Methodology

3.1. Chemicals and Equipments

The required 3-benzylidene-2,4-pentanedione, 3-benzylidene-1-phenyl-1,3-butandione, and 3-benzyllidene-1,3-diphenyl-1,3-propanedione were synthesized as described previously [32]. The Schiff bases were prepared by condensation with phenylhydrazine (BDH, England) in dry absolute ethanol(Riedel-de Haën) in presence of HCl (Riedel-de Haën) as a catalyst [31]. Sc(NO3)3·xH2O 99%, Y(NO3)3·6H2O 99%, Ce(NO3)3·6H2O 99%, and La(NO3)3·6H2O 97% were purchased from BDH. 4-chloro-benzaldehyde 97% (Fluka), 4-fluorobenzaldehyde 98% (BDH), 4-nitrobenzaldehyde 98% (BDH), 4-bromobenzaldehyde 99% (BDH), 1,3-diphenyl-1,3-propandion 98% (BDH), phenyl-1,3-butanedion 99% (BDH), and acetylacetone 99% (WINLAB) were also used. All other solvents used were of the ANALAR grade. Elemental analyses were performed at King Saud University, Saudi Arabia. Melting points were recorded on a Gallenkamp melting point apparatus. IR spectra were recorded on Perkin Elmer (spectrum 1000) FT-IR spectrometer using KBr pellets at the chemistry department, College of Science, King Fahd University for Petroleum and Minerals Saudi Arabia. Proton NMR spectra were recorded using JEOl EX-270 MHz (DMSO-d6) with TMS as an internal reference. Mass spectra were recorded with the aid of GCMS-QP 1000 EX Shimadzu spectrophotometer at 70 eV using a direct insertion probe at 25–300°C at the Microanalytical Centre, Cairo University, Egypt. Thermogravimetric analyses were measured under nitrogen flow rate: 30 cm3 min−1 using a Shimadzu TGA-60H thermobalance from room temperature up to 1000°C at the chemistry department, college of Science, King Faisal University Saudi Arabia. The magnetic susceptibilities were measured using a Sherwood Scientific Ltd. Magnetic susceptibility balance (England).

3.2. Preparation of the Ligands

Condensation of substituted {p-F(1), p-Cl(2), p-Br(3), and p-NO2(4)} 3-benzylidene-2, 4-pentanedione (I), 3-benzylidene-1-phenyl-1,3-butandione (II), and 3-benzyllidene-1,3-diphenyl-1,3-propanedione (III) with phenylhydrazine (see equation below) was performed by refluxing 20 mmol solution of the carbonyl compounds (I1 = 4.124, I2 = 4.453, I3 = 5.342, I4 = 4.662 g), (II1 = 5.363, II2 = 5.690, II3 = 6.581, II4 = 5.903 g), and (III1 = 6.604, III2 = 6.932, III3 = 7.822, III4 = 7.140 g) with 40 mmol phenylhydrazine (3.93 cm3) in 30 cm3 absolute ethanol in presence of 5 cm3 concentrated HCl as a catalyst for 18–24 h. The solution was then cooled to room temperature and added in portions with continuous stirring to crushed ice prepared from bidistilled water. The resulting yield was filtered, washed with water, and recrystallized from ethanol until constant melting point. Color, MP., yield, and elemental analyses are given in Table 1.

3.3. General Procedure for the Complexes

A solution containing 5 mmol of ligand in 40 cm3 ethanol was refluxed with a solution of 7 mmol of Sc(III), Y(III), La(III), and Ce(III) nitrates for about 12 h after adjusting the pH using ammonia (1 : 1) or Thiel Buffer [38] solution, cooled to room temperature, filtered, washed with ethanol and water, recrystallized from ethanol, and dried on air. The physical properties of the prepared complexes were very stable under ordinary conditions.

3.4. Antimicrobial Studies

3.4.1. Preparation of the Discs

The complex (60 μg) in DMF (0.01 cm3) was mounted on a paper disc (prepared from blotting paper (5 mm diameter)) with the help of micropipette. The discs were left at room temperature till dryness and then applied on the microorganism-grown agar plates.

3.4.2. Preparation of Agar Plates

Minimal agar was used for the growth of specific microbial species. The preparation of agar plates for B. subtilis, S. aureus, E. coli, and S. typhi (bacteria) utilized nutrient agar (2.30 g; obtained from Panreac Quimica SA, Spain) suspended in freshly distilled water (100 cm3) and potato dextrose agar medium (3.9 g/100 cm3; obtained from Merck) for A. niger and C. albicans (fungi). This was allowed to soak for 15 min and then boiled on a water bath until the agar was completely dissolved. The mixture was autoclaved for 15 min at 120°C, then poured into previously washed and sterilized Petri dishes, and stored at 30°C for inoculation.

3.4.3. Procedure of Inoculation

Inoculation was done with the help of platinum wire loop, which was heated to red-hot in a flame, cooled and then used for the application of the microbial strains.

3.4.4. Application of the Discs

Sterilized forceps were used for the application of the paper disc on previously inoculated agar plates. When the discs were applied, they were incubated at 37°C for 24 h for bacteria and yeast and at 28°C for 48 h for fungi. The zone of inhibition around the disc was then measured in millimeters [35].

Acknowledgment

The authors wish to express their deep thanks to the King Abdul-Aziz City for Science and Technology (KACST), Riyadh, Saudi Arabia for providing support to this scientific research.

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