Synthesis and Spectral, Thermal and Antimicrobial Investigation of Mixed Ligand Metal Complexes of N-Salicylidene Aniline and 1,10-Phenanthroline

Abstract

Coordination compounds of Co(II), Cu(II), Y(III), Zr(IV) and La(III) ions were synthesized from the N-salicylidene aniline (L) derived from the condensation of aniline with salicylaldhyde and 1,10-phenanthroline (phen) as a secondary mixed ligand. L, phen and their complexes were characterized using various physiochemical methods, such as elemental analyses (CHN), Fourier-transform infrared spectroscopy (FT-IR), molar conductance (Λ), magnetic susceptibility (μeff), proton nuclear magnetic resonance (¹H NMR), ultraviolet–visible spectroscopy (UV–Vis) and thermogravimetric analysis (TG/DTG). The analytical and spectroscopic data supporting the chemical formulas of the metal complexes and chelation of L and phen with the metal ions forming octahedral complexes. FT-IR spectra demonstrated that L chelated with metal ions as a bidentate ligand via the oxygen atom of the phenolic group with a band in the range 3378–3437 cm⁻¹ and the nitrogen atom of the azomethine group at 1612 cm⁻¹. In addition, phen chelated through two nitrogen atoms in the range 1525–1565 cm⁻¹. The ¹H NMR results confirmed the IR assumption that the ligand connected to the metal ions via the phenolic’s oxygen atom. The molar conductance measurements of the complexes revealed high values of the electrolytic nature of these complexes in the range of 90.40–125.80 S cm² mol⁻¹. Thermal analysis (TG/DTG) was used to differentiate between coordinated and hydrated water molecules and the thermal stability of the complexes. Finally, the anti-microbial activities of the complexes were investigated against fungi (Candida albicans), Gram-negative bacteria (Escherichia coli and Salmonella typhimurium) and Gram-positive bacteria (Staphylococcus aureus and Micrococcus sp.) using the disc diffusion method. The La(III) complex was significant against C. albicans compared with all other compounds and reference standard control.

1. Introduction

Schiff base ligands contain N, O donor atoms that may be used in the reduction reaction of ketones, and oxidation of organic compounds, dyes, pigments, catalysts and polymers [1,2,3]. Schiff base chelated with metal ions forms stable complexes employed in biological, analytical, agricultural, industrial, and medicinal applications [3,4]. There are imine or azomethine groups in a number of natural, naturally derived, and synthetic substances. Such compounds are demonstrated to be crucial to their biological functions [5,6,7,8,9,10]. The first-row transition metals, in particular cobalt and copper, are significant to biology because they are linked to a variety of proteins that are crucial for vital physiological functions [11,12,13,14,15]. The prolate-shaped N-salicylidene anilines (Scheme 1A) belong to the class of liquid crystals with rod- and disc-shaped structural units [16,17,18,19,20] that have undergone extensive study and are employed in a wide range of scientific, technological, industrial domains and possess mesomorphism that have photochromic properties [21,22,23]. Some metals, such as Co, Ni, Cu, Rh, Pd and Pt, combine with N-salicylidene anilines, and the resulting complexes modify the geometric structure of molecules and exhibit smectic mesomorphism [24,25,26]. Phen (Scheme 1B) is a powerful nitrogen donor ligand that effectively chelates metal ions to form stable complexes and has supplemental features for complexes due to it possessing heteroaromatic and aromatic groups [27,28].

The objectives of this research were to investigate the effects of changing atomic volume, atomic mass, and oxidation state of Co(II), Cu(II), Y(III), Zr(IV) and La(III) on the biological activity of the parent ligand (L) in presence of phen. These unique electolytic mononuclear metal complexes have been subjected to spectroscopic characterization using spectroscopic techniques, such as FT-IR, UV-Vis, ¹H NMR, CHN, molar conductivity, magnetic susceptibility studies and thermal analyses. These compounds’ antimicrobial efficacy has been assessed in vitro against bacteria and fungi, as well as statistical analysis of the antimicrobial data.

2. Experimental Section

2.1. Materials and Instrumments

The highest purity analytical grade chemicals were used for all applications. Salicylaldhyde, aniline, phen, ethanol absolute, dimethylformamide (DMF), dimethyl sulfoxide (DMSO), cobalt chloride hexahydrate, copper chloride dihydrate, yttrium chloride hexahydrate, zirconium chloride octahydrate, lanthanum chloride heptahydrate, potassium chromate, concentrated sulfuric acid and silver nitrate from sigma, Aldrich and Fluka Chemical Co. All glasswares were submerged in a chromatic solution (K₂Cr₂O₇ + concentrated H₂SO₄) before being thoroughly washed with bidistiled water and dried in an oven at 100 °C.

The range of 4000–400 cm⁻¹ of the FT-IR spectra in KBr discs was recorded by using FT-IR 460 PLUS Spectrophotometer. DMSO-d6 was employed as the solvent to acquire the ¹H NMR spectra on a Varian Mercury VX-300 NMR Spectrometer. UV-3101PC Shimadzu completed the electronic spectra. The absorption spectra were recorded as DMSO solutions. Shimadzu TGA-50H was used for implementation. TG-DTG measurements were performed in an environment of N₂ at temperatures ranging from ambient °C to 1000 °C, and the sample mass was meticulously weighed out in an aluminum crucible. To quantify the M percent content, three analytical methods were used. This purposeful experiment included complexmetric titration, thermogravimetry by converting the solid products into metal oxide, and atomic absorption utilizing a spectrometer type PYE-UNICAM SP 1900 equipped with the appropriate lamp [29,30]. The percent of CHN was carried out using a Perkin Elmer 2400 CHN elemental analyzer. Melting points were measured on a Buchi device. With a Gouy balance and Hg[Co(CSN)₄] as the signing material, the magnetic susceptibilities of the powdered materials were investigated on a Sherwood scientific magnetic scale. Using CONSORT K410, the molar conductance of 1 × 10⁻³ M solutions of the ligands and their complexes in DMF was examined. Each experiment used freshly made solutions and was conducted at room temperature.

2.2. Preparation of N-Salicylidene Aniline (L)

Light yellow solid compound (L) was obtained by the reaction of 20 mmol aniline (1.82 mL) with 10 mmol of salicylaldhyde (2.08 mL) (Scheme 2) using absolute ethanol and refluxed with constant stirring for 5 h in presence of 1 mL glacial acetic acid and concentrated to 8 mL in a water bath and allowed to cool at 0 °C. The formed precipitate was filtered off and dried over anhydrous CaCl₂.

2.3. Synthesis of Metal Complexes

The dark green solid complex [Co(L)(phen)(H₂O)₂]Cl₂.6H₂O (1) was created by combining 1 mmol of L (0.197 g) with 1 mmol of phen (0.198 g) in 20 mL of ethanol. After 10 min of stirring the mixture, we added 1 mmol (0.237 g) of CoCl₂·6H₂O in 20 mL ethanol dropwise and refluxed for 6 h. The dark green precipitate was dried over anhydrous CaCl₂ under vacuum. Dark brown complex [Cu(L)(phen)(H₂O)₂]Cl₂ (2), dark blue [Y(L)(phen)(H₂O)₂]Cl₃·5H₂O (3), green [ZrO(L)(phen)(H₂O)]Cl₂ (4) and yellow [La(L)(phen)(H₂O)₂]Cl₃ (5) were made in a similar way to that previously described, using ethanol. CoCl₂.6H₂O, YCl₃.6H₂O, ZrOCl₂.8H₂O, LaCl₃.7H₂O, respectively in 1:1:1 (L:phen:M) molar ratio.

2.4. Antimicrobial Investigation

Five standard microbial strains, two Gram-negative bacteria (Escherichia coli ATCC 10536 and Salmonella typhimurium ATCC 14028), two Gram-positive bacteria (Staphylococcus aureus ATCC 6538 and Micrococcus sp. TCC 10240) and one fungi (Candida albicans ATCC 10231) were obtained as pure cultures from the microbial collection of the School of Agricultural, Forestry, Food and Environmental Sciences (SAFE), University of Basilicata, Potenza, Italy. The antimicrobial activity of the tested samples was determined at the Laboratory of Phytopathology, SAFE, University of Basilicata by using the disc diffusion method according to Clinical Laboratory and Standards Institute Guidelines [31,32] (CLSI, 2012). The microbial strains were inoculated into Mueller-Hinton broth and incubated at 35 °C until it reached a turbidity equivalent to or greater than that of the 0.5 McFarland standard. The turbidity of the suspension was adjusted with sterile saline to achieve a turbidity equivalent to that of a 0.5 McFarland standard. Sterile Mueller–Hinton agar plates were poured aseptically. A sterile cotton swab should ideally be dipped into the modified suspension within 15 min of altering the inoculum suspension’s turbidity. The swab should be turned around many times and firmly pressed against the interior tube wall above the fluid level. By doing this, the swab’s extra inoculum will be removed. By streaking the swab across the whole sterile agar surface of a Mueller-Hinton agar plate’s dried surface, the plate is infected. To ensure an evenly distributed inoculum, streak the plate two more times while rotating it by about 60 degrees each time. The rim of the agar is swabbed as a last step. Before using the drug-impregnated discs, the lid may be left open for 3 to 5 min, but no longer than 15 min, to allow any excess surface moisture to be absorbed. To ensure full contact with the agar surface, sterile filter paper discs of about 5 mm in diameter that were impregnated with 8 L of the test samples were placed on the plates. The diameter of the inhibitory zones was determined after the plates were inverted and incubated at 37 °C for 16 to 20 h [31,33,34]. Inhibition of microbial growth was calculated in relation to the positive control. Using the equation, the compounds’ activity index percent was calculated. The whole experiment was carried out twice with three replicates, and the obtained data are illustrated as mean values ± SDs.

$$\% Activity Index=\frac{Zone of inhibition by test compound \left(diametre\right)}{Zone of inhibition by standard \left(diametre\right)}\times 100$$

(1)

3. Results and Discussion

The physical characteristics and the analytical data of our complexes are mentioned in

Table 1. Elemental analysis and Physico-analytical data for L, Phen and their complexes.

Compounds M.Wt. (M.F.)	Yield%	Mp/°C	Color	(Calcd.) Found (%)					Λ (S cm2 mol−1)
				C	H	N	Cl	M
L 197 (C13H11NO)	-	50 (49–51)	Light-yellow	(79.18) 79.01	(5.58) 5.52	(7.10) 6.89	-	-	1.45
Phen 198.23 (C12H10N2O)	-	100	White	(72.64) 72.59	(5.04) 4.87	(14.12) 14.03	-	-	5.00
(1) 650.933 (CoC25H35N3O9Cl2)	90.02	>300	Dark-green	(46.08) 45.92	(5.37) 5.24	(6.45) 6.19	(10.90) 10.88	(9.05) 8.99	95.80 (94.81–96.80)
(2) 547.56 (CuC25H23N3O3Cl2)	88.22	213 (212–214)	Dark-brown	(54.78) 54.72	(4.20) 4.14	(7.67) 7.62	(12.94) (12.88)	(11.60) 11.52	90.40 (88.60–92.21)
(3) 698.4 (YC25H33N3O8Cl3)	91.34	220 (219–221)	Dark-blue	(42.95) 42.83	(4.72) 4.57	(6.01) 5.86	(15.24) 15.18	(12.72) 11.69	120.51 (119.20–121.83)
(4) 573.334 (ZrC25H21N3O3Cl2)	85.69	>300	Green	(52.32) 52.22	(3.66) 3.56	(7.32) 7.22	(12.36) 12.25	(15.91) 15.81	93.70 (92.69–94.71)
(5) 658.4 (LaC25H23N3O3Cl3)	89.12	>300	Yellow	(45.56) 45.41	(3.49) 3.40	(6.37) 6.31	(16.15) 16.11	(21.09) 21.02	125.80 (124.90–126.70)

, and, according to the obtained data, the complexes are formed of 1:1:1 (L:phen:Metal) stoichiometry. All the complexes are hydrates except Zr(IV) complex with high melting points, air-stable at room temperature and insoluble in most organic solvents but soluble in DMF and DMSO mediums. The molar conductance measurements in 10⁻³ M DMF of 1, 3, 4 and 5 complexes are in 90.40–125.80 Ω cm² mol⁻¹ range; these high values revealed the electrolytic nature of these complexes [35,36]. Qualitative data demonstrated the existence of chloride within the complex sphere.

3.1. FT-IR Spectra

To monitor the complexation of the transition metal ions by the organic ligand, FT-IR spectroscopy can be a useful analytical technique. To verify the mixed ligand’s mechanism of binding to the appropriate metal ions in the complexes, the FT-IR spectra of L and phen were compared to those of the metal complexes (Figure S1). We initially paid attention to the vibrations of the metal complexes, phenolic and azomethine groups because this supports the mechanism that was hypothesized for the interaction between L and the metal cations. The broad and medium intensity bands observed in the range 3378–3437 cm⁻¹ (

Table 2. Infrared wavenumber (cm⁻¹) of L, phen and their complexes.

L	phen	(1)	(2)	(3)	(4)	(5)	Assignments
3426 mbr	3380 sbr	3433 mbr	3426 mbr	3378 mr	3390 mbr	3437 ms	ν(O–H); H2O
1612 vs		1600 vs	1605 vs	1601 s	1600 vs	1602 sh	ν(C=N) of azomethine group
	1586 ms	1526 m	1527 ms	1565 w	1526 m	1525 m	ν(C=N) pyridine ring
		758 s 663 vw	756 s 621 w	726 w 657 m	756 s 652 sh	721 vs 630 m	ν(M–O) and ν(M–N)

Keys: s = strong, w = weak, v = very, m = medium, br = broad, sh = shoulder, ν = stretching.

) in FT-IR spectra of complexes are assigned to O–H stretching vibrations of the phenolic group, lattice and coordinated water [11,12,13,14,37]. The chelation mode and structures of complexes are shown in Scheme 3. According to the provided information, v(Zr=O) is a medium band at 846 cm⁻¹ [38]. The vibrational mode v(C=N) of azomethine group for L was visible at 1612 cm⁻¹; this band shifted to lower frequencies around 1600 cm⁻¹ in all metal complexes, which indicates chelation with the metal [13,14]. Phen was matched with metal ions through the two nitrogen atoms and displayed bidentate ligand behavior, as evidenced by the free phen peak at 1586 cm⁻¹. After chelation, this peak shifted to lower values at 1525–1565 cm⁻¹ [37,38]. The decrease of v(C=N) resulted from the decrease in the stretching force constant of the C=N bond as a consequence of the coordination of the nitrogen atom of the azomethine group to the metal ions [39,40,41,42]. New bands with varying intensities at 758, 663 cm⁻¹ for complex (1), at 756, 621 cm⁻¹ for complex (2), at 726, 657 cm⁻¹, for complex (3), at 756, 652 cm⁻¹ for complex (4) and at 721, 630 cm⁻¹ for complex (5), which are absent in the spectra of L and phen indicate the chelation of L and phen with metal ion [43,44,45].

3.2. Electronic Spectra and Magnetic Moment Measurements

UV–visible spectral data for L, phen and their mixed complexes were recorded in the wavelength range 200–800 nm in DMSO solvent. The intra-ligand transitions (π–π* and n–π*) for L were accountable at 270, 302, 318 and 340 nm (Figure S2) and

Table 3. UV-Vis. spectra of L, phen and their complexes.

Compounds	Peak		Assignment	ε (M−1cm−1)x 104	10 Dq		CFSE#	μeff (B.M)	Postulated Structure
	nm	cm−1			cm−1	kJ/mol
L	270	37,037	π → π *	0.600
	302	33,112	n → π *	0.800
	318	31,446	n → π *	0.723
	340	29,411	n → π *	0.769
Phen	273	41,152	π → π *	1.500
	310	36,630	n → π *	2.000
	350	28,571	n → π *	0.400
(1)	275	36,363	π → π *	0.912	16,528	198	198+2p	5.11	octahedral
	300	33,333	n → π *	1.300
	316	31,645	n → π *	0.812
	338	29,585	n → π *	0.500
	475	21,052	CT	0.423
	605	16,528	4T1g → 41g	0.350
(2)	245	41,666	π → π *	1.320	17,241	206	206+4p	1.70	octahedral
	286	34,965	n → π *	0.780
	397	25,188	n → π *	0.387
	460	21,739	CT	0.312
	580	17,241	2B1g → 2E1g	0.200
(3)	250	40,000	π → π *	1.600					octahedral
	275	34,129	π → π *	0.800
	310	32,258	n → π *	0.750
	318	22,123	n → π *	0.900
	340	29,411	n → π *	0.950
	480	20,833	CT	0.500
(4)	247	40,485	π → π *	1.200
	265	37,735	π → π *	1.620
	346	28,901	n → π *	0.200
	465	21,505	CT	0.450
(5)	244	40,983	π → π *	2.230					octahedral
	275	36,363	π → π *	1.330
	320	31,250	n → π *	1.230
	345	28,985	n → π *	1.450
	467	21,413	CT	0.650

[11,12]. In addition, phen shows bands at 273, 310 and 350 nm, which may be assigned to π–π* and n–π* transitions [13,14,37,38]. The shifting of the absorption bands of π–π* and n–π* to higher or lower frequencies indicates the formation of complexes. For our complexes, the presence of new peaks in the range 460–480 nm may be assigned to ligand–metal charge transfer [46]. Co(II) complex’s electronic spectrum exhibits an absorption band at 16,528 cm⁻¹, which equates to ⁴T_1g (F) → ⁴T_1g (P) transitions, and a noticeable magnetic moment estimate of 5.11 B.M, demonstrating that the complex seems to have a high spin octahedral with 10 dq 198 kJ/mole and CFSE 198+2p [45,46]. The band observed at 17,241 cm⁻¹ for Cu(II) complex may be assigned to ²B_1g → ²E_g transition [11,12,13,14,47,48], the magnetic moment of the complex at 1.70 B. M, which was within the typical range for octahedral Cu(II) complexes with 10 dq 206 kJ/mole and CFSE 206+4p [47]. No d–d transitions were noticed for the complexes Y(III), Zr(IV), and La(III) since these complexes are diamagnetic as expected given their electron configuration (d⁰). Complexes’ molar absorptivity (ε), as determined by their electronic spectra, was published (Table 3) utilizing the following equation: A = εcl, where c = 1 × 10⁻³ M and l is the length of the cell (1 cm).

3.3. ¹HNMR Spectra

In d6-dimethylsulfoxide (DMSO) solution, the ¹H NMR spectra of L, phen and their complexes were recorded using tetramethylsilane (TMS) as an internal reference (Figure S3)

Table 4. H NMR values (ppm) and tentative assignments for L, phen and their complexes.

L	Phen	(1)	(2)	(3)	(4)	(5)	Assignments
2.48	-	1.98–2.51	1.25–2.50	2.51	1.99–2.53	2.50	δH, –CH aliphatic
-	3.37	4.35	3.37	3.36	4.17	3.33	δH, H2O
6.96–8.95	7.26–8.81	7.11–8.95	7.54	7.31–8.96	7.02–8.50	7.00–8.96	δH, –CH aromatic
13.09	-	13.01	13.00	13.02	14.87	13.00	δH, –OH

. The ¹H NMR spectrum of L and phen ligand showed a band at δ: 2.48 corresponding to N=CH aliphatic and at δ: 6.96–8.96 ppm for–CH aromatic [49]. Figure S3 demonstrates a singlet (OH) at δ: 13.09 ppm, which may be assigned to the phenolic OH [50]. It is implied that L is coordinated through the oxygen atom of the phenolic proton since the phenolic proton OH is observable in the spectra of the complexes with chemical shift. Due to the presence of water molecules in the complexes, the ¹H NMR spectra for all of the complexes reveal a distinct signal in the interval of 3.36–4.35 ppm [50,51]. All signals from the free ligands are evident in the complexes’ spectra when compared to L, phen, with some changes resulting from the ligand’s interaction with the metal.

3.4. Thermal Analysis (TG and DTG)

The thermogravimetric analyses (TG and DTG) for L, phen and their complexes were done. The TG data and their assignments are summarized in

Table 5. The maximum temperature T_max (°C) and weight loss for L, phen and their complexes.

Compounds	Decomposition	Tmax (°C)	Weight Loss (%)		Lost Species
			Calc.	Found
L	First step	200	100.00	99.68	2C4H2 + H2O + 0.5N2 + 2.5C2H2
	Total loss		100.00	99.68
phen	First step	95	9.08	8.98	H2O
	Second step	278	90.92	90.87	2C4H2 + 2C2H2 + N2
	Total loss		100	100
(1)	First step	41	16.59	16.22	6H2O
	Second step	172,258	52.55	52.64	6C2H2 + C2N2 + H2O + 2C4H2 + 0.5O2
	Third step	330,432,657	15.67	15.80	CH4 + 0.5Cl2 + 0.5N2 + HCl
	Total loss		84.81	84.66
	Residue		15.19	15.34	CoO + 2C
(2)	First step	175,288	25.57	25.51	2H2O + 4C2H2
	Second step	495	62.83	62.80	4C4H2 + CO + 2HCl + 1.5N2 + 0.5H2
	Total loss		88.40	88.31
	Residue		11.60	11.69	Cu
(3)	First step	85	12.89	12.85	5H2O
	Second step	150,283	49.81	49.79	2H2O + 12C2H2
	Third step	475,810	19.41	19.40	3HCl + 0.5H2 + 2NO + NO2 + 0.5H2O
	Total loss		82.11	82.04
	Residue		17.89	17.96	0.5Y2O3 + C
(4)	First step	220	17.44	17.40	3C4H2
	Second step	530	52.70	52.80	2C4H2 + CO + 2HCl + 3NH3
	Total loss		70.14	70.20
	Residue		29.86	29.80	ZrO2 + 4C
(5)	First step	174	5.47	5.40	2H2O
	Second step	428,506	67.95	67.88	9C2H2 + C2N2 + CO + HCN + 1.5Cl2
	Total loss		73.42	73.28
	Residue		26.58	26.72	La + 3C

and displayed in Figure S4. The results of thermal study showed good consistency with the molecular formula obtained from the elemental analysis data. The TG of L advanced through one step with an estimated mass loss of 99.68% (calc: as 100.00%) at T_max 200 °C corresponding to 2C₄H₂ + H₂O + 0.5N₂ + 2.5C₂H₂. The literature review reported the thermal degradation of phen at T_max 95 °C with loss weight 8.98% (calc: 9.08%) to loss H₂O. The second step with T_max 278 °C and weight loss of 90.87% (calc: 90.92%) corresponded to the loss of 2C₄H₂ + 2C₂H₂ + N₂ with activation energy 117.83 kJ/mole [52,53]. Complexes (1) and (3) have nearly identical thermal behavior and break down with three stages: The first one corresponds to the loss of lattice water molecules at T_max 41 and 85 °C. The second decompostion stage at T_max 172, 285 and 150, 283 °C with loss of 6C₂H₂ + C₂N₂ + H₂O + 2C₄H₂ + 0.5O₂ and 2H₂O + 12C₂H₂, respectively. The third step involves decomposition at 330, 432, 657 and 475, 810 °C maxima (Table 5). According to TG curve complexes (2), (4) and (5) are thermally stable up to 170 °C and then decompose in two steps: The first one of degradation matches to loss of 2H₂O + 4C₂H₂, 3C₄H₂ and 2H₂O with a mass loss of 25.51% (calc 25.57%), 17.40% (calc 17.44%) and 5.40% (calc 5.47%). The second step corresponds to loss of 4C₄H₂ + CO + 2HCl + 1.5N₂ + 0.5H₂, 2C₄H₂ + CO + 2HCl + 3NH₃ and 9C₂H₂ + C₂N₂ + CO + HCN + 1.5Cl₂ with T_max 495, 530, 428 and 506 °C.

3.5. Antimicrobial Investigation

The antimicrobial property of L, phen, and their metal complexes versus distinct bacterial and fungal species was assessed utilizing the disc diffusion method. Generally, the findings shown in Figure 1 illustrated that the prepared complexes have promising antifungal and antibacterial properties. Following the revelation that chelating compounds can suppress the development of bacteria when complexed with a variety of metals, the antibacterial properties of transition metal complexes have been specifically explored in great detail. The created compounds were discovered to have exceptional bactericidal properties. However, it is intriguing to note that, as shown in

Table 6. The inhibition diameter zone (mm) and the activity index (%) values for L, Phen and their complexes.

Tested Compounds	Tested Microbial Species
	G(+ve) Bacteria				G(−ve) Bacteria				Fungi
	S. aureus		M. luteus		E. coli		Salm. typhi		C. albicans
	D.Iz a (mm)	AI b (%)	D.Iz (mm)	AI (%)	D.Iz (mm)	AI (%)	D.Iz (mm)	AI (%)	D.Iz (mm)	AI (%)
L	8 ±0.17	32	10 ±0.08	34.48	8 ±0.12	23.52	8 ±0.14	25	9 ±0.19	50
Phen	8 ±0.39	32	9 ±0.24	31.03	8 ±0.13	35.52	7 ±0.31	21.87	8 ±0.36	44.44
(1)	9 NS ±0.50	36	10 ±0.41	34.48	9 NS ±0.42	26.47	8 ±0.21	25	9 ±0.44	50
(2)	9 NS ±0.48	36	10 ±0.20	34.48	9 NS ±0.35	26.47	8 ±0.29	25	9 ±0.59	50
(3)	9 NS ±0.59	36	11 NS ±0.32	37.93	9 NS ±0.52	26.47	8 ±0.40	25	11 NS ±0.70	61.11
(4)	8 ±0.18	32	10 ±0.27	34.48	8 ±0.23	23.52	7 ±0.28	21.87	10 NS ±0.66	55.55
(5)	9 NS ±0.64	36	11 NS ±0.35	37.93	9 NS ±0.55	26.47	8 ±0.33	25	12 +1 ±0.37	66.66
Ciprofloxacin (control)	25 ±0.3	100	29 ±0.2	100	34 ±1.11	100	32 ±0.98	100	0	0
Nystatin (control)	0	0	0	0	0	0	0	0	18 ±0.42	100
DMSO (control)	0	0	0	0	0	0	0	0	0	0
DMF (control)	0	0	0	0	0	0	0	0	0	0

^(a) D.Iz (mm): the diameter of inhibition zone in millimeters. ^(b) AI (%): the activity index for the tested compounds. ^(c) (DMF) dimethyl formamide and (DMSO) dimethyl sulfoxide, ⁺¹ significant and ^NS not significant.

, when biological activity undergoes complexation with the metal ions, it increases in comparison to the examined standards.

Regarding the antifungal activity, complex (5) possesses significant activity against C. albicans compared to L and phen. On the basis of chelation theory, this increased activity of the metal complexes can be explained [54,55]. The permeability of the cell membrane and the lipid composition of the studied microbial cells’ cell walls enable the easier passage of soluble compounds through the cell, which is a significant aspect of assessing an antimicrobial agent’s efficacy [54,55]. This suggests that chelation may facilitate metal complex diffusion across the lipid layer of the cell membrane to the site of action [56,57,58,59,60]. Table 6 and Figure 2 provide measurements of the compounds’ activity indices.

4. Conclusions

The chelation of oxygen, nitrogen of L and nitrogen of phen has been shown through the complexation process with Co(II), Cu(II), Y(III), Zr(IV) and La(III) which supported by spectroscopic data. The new mixed metal complexes have been characterized using spectroscopic and physicochemical techniques. The data supported the proposed coordination of six coordinated metal ions with distorted octahedral geometry formed by the ligands. The indicated molecular formulae of the complexes were supported by thermal studies, which also served to assess the stability of the compounds. In addition, the molar conductance statistics indicate that all complexes are electrolytic with chloride ions as counter ions. The antibacterial activity of each generated complex and the two parent ligands has been tested against a variety of food- and phytopathogen-causing microorganisms. In addition, complex (5) demonstrated significant activity against C. albicans compared to the parent ligands L and phen and other complexes.