# Interaction of Small Zinc Complexes with Globular Proteins and Free Tryptophan

Authors: Joann M. Butkus; Shelby O’Riley; Balwant S. Chohan; Swarna Basu
Journal: International Journal of Spectroscopy
 (2016)

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## Abstract

A series of eight water soluble anionic, cationic, and neutral zinc(II) complexes were synthesized and characterized. The interaction of these complexes with bovine serum albumin (BSA), human serum albumin (HSA), lysozyme, and free tryptophan (Trp) was investigated using steady-state fluorescence spectroscopy. Static and dynamic fluorescence quenching analysis based on Stern-Volmer kinetics was conducted, and the decrease in fluorescence intensity of the Trp residue(s) can be ascribed predominantly to static quenching that occurs when the Zn complex binds to the protein and forms a nonfluorescent complex. The role played by the nature of the ligand, the metal, and complex charge in quenching Trp fluorescence was investigated. The binding association constants (Ka) ranged from 104 to 1010 M−1 and indicate that complexes with planar aromatic features have the strongest affinity for globular proteins and free Trp. Complexes with nonaromatic features failed to interact with these proteins at or in the vicinity of the Trp residues. These interactions were studied over a range of temperatures, and binding was found to weaken with the increase in temperature and was exothermic with a negative change in entropy. The thermodynamic parameters suggest that binding of Zn complexes to the proteins is a highly spontaneous and favorable process.


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## Body

## 1. Introduction

Zinc(II) is one of the most important metal ions found in proteins and metalloenzymes, including alcohol dehydrogenase, carbonic anhydrase, carboxypeptidase A, matrix metalloproteinase, and thermolysin [1–5]. Zinc proteins play a vital role in the biosynthesis and metabolism of a number of bioactive peptides and have been implicated in various disease states including cancer, arthritis, and multiple sclerosis [6].Structurally, biological zinc is found ligated by a shell of hydrophilic side chains, involving O, N, and S donors, in 4-, 5-, or 6-coordinate geometry. The most common donor protein-derived ligands tend to be His, Cys, Asp, Glu, and water molecules. This hydrophilic shell is often embedded within a larger shell made up of hydrophobic side chains [7–9]. Regardless of the common qualitative features of the Zn binding site, much effort has been devoted to understanding the role of the specific pattern of Zn ligation and the protein matrix in regulating reactivity.Albumin proteins bind and transport a wide diversity of ions and molecules with very high affinity [10–13]. Human serum albumin (HSA) accounts for 60% of serum proteins and is the most abundant protein in the circulatory system [14–17]. Bovine serum albumin (BSA) is a homologous globular protein and its sequence is 76% identical to that of HSA. For many drugs and exogenous metal complexes, binding to serum albumin is a critical determinant of their distribution, pharmacokinetics, and potency [18–20].In this work, several small Zn(II) complexes with varying O, N, and S donor ligands, including some that are novel, were synthesized and characterized. The interaction of these complexes with BSA, HSA, lysozyme, and free tryptophan (Trp) was investigated using steady-state fluorescence spectroscopy to gain information on the binding mode, binding order, affinity, efficiency, and mechanism of fluorescence quenching. The information could potentially lead to better structure-based drug design and development of highly selective ligands as tags for precise and accurate quantification of proteins, which will ultimately lead to new and more effective therapeutic approaches [21, 22].The dominant fluorophore in these proteins is Trp, a residue that has an emission maximum that is sensitive to the polarity of the surrounding environment. HSA contains 585 amino acids, with a single intrinsic Trp residue at position 214. BSA consists of a chain of 580 amino acids, with two Trp residues at positions 134 and 212. Fluorescence quenching constants and thermodynamic parameters (ΔH, ΔS, and ΔG) for the interaction were calculated using Stern-Volmer kinetics and a Van’t Hoff analysis.The interaction of Zn complexes with lysozyme is included since it is a very well characterized protein, containing six Trp residues that are located in the substrate binding sites and are essential for enzymatic activity. It is expected that each of the Trp residues will be affected differently depending on their location and environment and so contributing independently to the inherent fluorescence intensity [23–30]. Steady-state fluorescence studies have shown that most of the lysozyme emissions are due to Trp-62 and Trp-108, residues that are buried deep in the active site [26, 30]. Lysozyme has many physiological and pharmaceutical functions, one of which is to bind and transport drugs. The inclusion of free Trp is to illustrate the affinity of the Zn complexes for this particular amino acid, with its indole functional group, irrespective of the surrounding environment. The experimental results have allowed us to discuss the type, degree, and nature of the interactions taking place between the protein and the Zn complexes, with particular consideration to polarity, hydrophobicity, and molecular charge.


## 2. Experimental

### 2.1. Materials and Methods

Unless otherwise mentioned, all chemicals and reagents were of analytical grade (Sigma-Aldrich, Alfa Aesar, TCI, VWR). The solvents either were HPLC-grade or were dried and distilled using conventional methods and stored under an argon atmosphere [31, 32]. Nanopure water was used for all of the experiments. Zn(II) complexes are relatively stable in air; however, many of the ligands are air/moisture sensitive; therefore, all synthetic procedures were conducted using Schlenk techniques, and by default all compounds were stored in sealed vials under argon. The three proteins and free Trp were purchased (Sigma-Aldrich) and used without further purification. Stock solutions of proteins, Trp, and the Zn complexes were prepared in 50 mM Tris-HCl (pH 7.4) buffer solution.


### 2.2. Physical Measurements

FTIR data for solid samples (as KBr disks) and neat liquid samples were obtained on a Jasco 4000 IR spectrometer. The IR spectral peaks were calibrated with polystyrene and are reported in wavenumbers. Relative intensities of the key bands in a spectrum are indicated (w = weak, m = medium, s = strong, vs = very strong, and br = broad). Elemental analyses were performed at the UMass-Amherst Microanalysis Center, or by QTI/Intertek, Whitehouse, NJ. Samples for microanalysis were ground to a fine powder and vacuum desiccated over phosphorus pentoxide for at least four days prior to analysis. UV-vis experiments for characterization of the Zn complexes and determination of protein concentration were carried out using a Cary 4000 UV-vis spectrophotometer. Fluorescence spectra were obtained at room temperature using a Perkin-Elmer LS50B Spectrometer. The fluorescence emission spectra were corrected for wavelength dependent sensitivity using a calibration curve that was generated using five commercial spectral fluorescence standards (BAM-F001 to F005, Sigma-Aldrich) [33].For the fluorescence quenching experiments, the concentration of the protein, or free Trp, was held constant at 0.1μM and the concentration of each Zn complex was varied from 0 μM to 21.0 μM,via preparation of individual samples. The concentration range was adjusted according to whether quenching was more clear at higher or lower concentrations. The excitation wavelength was 280 nm, the emission wavelength was 345 nm for the proteins and 363 nm for Trp, and both the excitation and emission slit widths were kept constant at 4.0 nm. Fluorescence spectra were obtained at 25°C, 35°C, and 45°C. Spectra have been smoothed for presentation purposes.


### 2.3. Data Analysis

The dynamic quenching constants were determined using the Stern-Volmer relationship as shown in the following equation [24, 34]:(1)F0F=1+KSVQ,where F0 and F correspond to the fluorescence intensities of the protein in the absence and presence of quencher, respectively. [Q] is the concentration of the quencher. KSV is the Stern-Volmer quenching constant. KSV is related to the lifetime of the system according to the following equation:(2)KSV=kqτ0,where kq is the bimolecular quenching constant and τ0 is the lifetime of unquenched fluorophore. The value of τ0 is short for free Trp (2.7 ns) but longer in a protein environment. This value is dependent on the location within the protein, the extent of solvent exposure, and the vicinity of various side chains [35–37]. The static quenching constant, also known as the binding constant, Ka, and binding site number, n, were calculated from the following equation [24, 34]:(3)log⁡F0-FF=log⁡Ka+nlog⁡Q.The change in Gibb’s free energy, ΔG, was calculated using (4), where R is the gas constant and T is the temperature (K). Changes in entropy (ΔS) and enthalpy (ΔH) were determined using Van’t Hoff plot, based on the following:(4)ΔG=-RTln⁡Ka,(5)ln⁡K=-ΔHRT+ΔSR.Finally, the possibility of Forster type long-range energy transfer (FRET) from the Trp residues was explored using previously published protocols, and the Forster distances, R0, were calculated using the relevant spectroscopic properties of the participating molecules [38, 39].


### 2.4. Synthesis and Characterization of Zn Complexes

A series of eight water soluble Zn(II) complexes with varying donor atoms and ligand types were synthesized.Complex
1
, Na
2
[Zn(EDTA)]·2H
2
O, Zinc(II) Ethylenediaminetetraacetate Disodium Dehydrate. The zinc salt was synthesized in a slightly modified manner to that reported in the literature [40]. Na2(EDTA)·2H2O (10.83 g, 29.1 mmol) dissolved in 50 mL of water was added to a solution of ZnCl2 (3.96 g, 29.1 mmol) dissolved in 30 mL of water. The solution was neutralized by adding 4.89 g (58.2 mmol) of NaHCO3 and then adjusted to pH 7.0 with a few drops of 3 M HCl and heated to 80°C for 5 min. The solution was then left to concentrate in the open air at room temperature overnight. Addition of 20 mL of absolute ethanol produced a white colored crystalline material which was filtered and driedin vacuo for two days. The product was recrystallized twice from a 1 : 1 water-ethanol mixture, filtered, and driedin vacuo for a further six days to give a final yield of 10.52 g (83%): CHN microanalysis, Anal Calcd (found) for ZnC10H12N2O8·Na2·2H2O: C, 27.57 (27.28); H, 3.70 (3.35); N, 6.43 (6.38). IR (cm−1): ν(C-H) 2950m, ν(C=O) 1605vs, 1400s, 930s, ν(C-N) 1130m.Complex
2
, Zn-Pr-Pr, N,N′-Dimethyl-N-N′-bis(2-sulfanylpropyl)propylenediamine Zinc(II). The ligand N,N′-dimethyl-N,N′-bis(2-sulfanylpropyl)propylenediamine was synthesized according to the published procedures [41]. The ligand (2.390 g, 9.56 mmol) in 30 mL of 1 : 1 ethanol-methanol solvent mix was placed in a 200 mL round bottom flask in an ice bath, under an argon atmosphere, and stirred for 15 min. To this NaH (0.500 g, 20.83 mmol) was added and the solution was stirred for another 20 min under an argon atmosphere. Zn(OAc)2·2H2O (1.966 g, 8.96 mmol) was dissolved in ethanol (80 mL) under an argon atmosphere and added dropwise to the ligand. The whole mixture was allowed to stir for 15 hrs and then was concentrated on a rotary evaporator to 80 mL. The solution was filtered through a fine glass frit funnel, and the filtrate further reduced in volume to 50 mL. Diethyl ether (20 mL) was added to the solution and left in a −20°C freezer overnight. The white colored crystalline precipitate that formed was filtered, washed with diethyl ether, and driedin vacuo to yield 1.72 g (61%) of the zinc product: CHN microanalysis, Anal Calcd (found) for ZnC11H24N2S2: C, 41.10 (40.48); H, 7.71 (7.15); N, 8.93 (9.22). IR (KBr, cm−1): 1650, 1465, 1455, 1438, 1408, 1362, 1292, 1143, 1042, 1007, 985.Complex
3
, (Zn(pya
2
tn)Cl
2
), N,N′-Bis(2-pyridylmethylene)-1,3-diaminopropyl Zinc(II) Chloride. The complex was synthesized in a manner analogous to that reported for the Ni(II) complex [42, 43]. The Schiff base ligand (pya2tn) was derived from 2 equivalents of pyridine-2-carboxaldehyde and 1 equivalent of 1,3-diamino-2-propanol in isopropyl alcohol. The zinc complex was madein situ by dropwise addition of the ligand to a hot solution of ZnCl2 (1 equivalent) dissolved in absolute ethanol. The very pale yellow solution was concentrated on a rotary evaporator to 80 mL. Upon cooling, a pale yellow colored crystalline material appeared. This product was filtered, recrystallized from 10 : 1 water-isopropyl alcohol solvent mixture, and driedin vacuo for eight days to give a yield of 11.26 g (58%): CHN microanalysis, Anal Calcd (found) for ZnC15H16N4Cl2: C, 46.36 (46.02); H, 4.15 (3.98); N, 14.42 (14.22). IR (cm−1): ν(C-C, 4 bands, m) 1590 to 1440, ν(C-N) 1650s, ν(C-C) 1010s, ν(C-H) 790s.Complex
4
, (Zn(pya
2
tn-OH)Cl
2
), N,N′-Bis(2-pyridylmethylene)1,3-diamino-2-propanol Zinc(II) Chloride. The ligand was synthesized according to the modification of the published procedures [43, 44]. The Schiff base ligand (pya2tn) was derived from 2 equivalents of pyridine-2-carboxaldehyde and 1 equivalent of 1,3-diamino-2-propanol. The resulting yellow colored oil was crystallized by the addition of absolute ethanol to the neat oil. The zinc complex is made by the addition of the Schiff base ligand dissolved in absolute ethanol to a refluxing solution of ZnCl2 (1 equivalent), absolute ethanol, and 2,2-dimethoxypropane. The solution was then cooled to give a pale-beige colored crystalline material. The product was filtered, recrystallized from 10 : 1 water-methanol solvent mixture, and driedin vacuo for four days to give a yield of 17.11 g (71%): CHN microanalysis, Anal Calcd (found) for ZnC15H16N4Cl2O: C, 44.53 (44.27); H, 3.99 (3.91); N, 13.85 (13.67). IR (cm−1): ν(C-C, 4 bands) ν(O-H) 3400s broad, 1600 to 1430, ν(C-N) 1650s, ν(C-C) 1000s, ν(C-H) 780s.Complex
5
, Zn-sal-Ph-Cl
2
, Bis(N-salicylideneaniline) Zinc(II) Chloride. The ligand (5-L) and the zinc complex were synthesized in a manner analogous to that reported for the bis(N-phenylsalicylaldimine) nickel complex [45–47]. The salicylideneaniline ligand is commercially available from Sigma-Aldrich; however, for economic reasons, we chose to synthesize the ligand in-house according to generic procedures [48, 49]. In a 100 mL round bottomed flask, 2.20 mL (24.1 mmol) of aniline in 25 mL water was added to 2.95 mL (27.8 mmol) of salicylaldehyde in 20 mL of water. The flask was kept at room temperature and the solution was vigorously stirred for six hours. The yellow colored precipitate that formed was filtered off, washed with ice-cold water, and dried undervacuo to give a yellow colored precipitate, yield 4.32 g (91%). The complex was made by dropwise addition of 1.47 g (10.8 mmol) ZnCl2 in 40 mL methanol to a mixture of 4.24 g (21.6 mmol) salicylideneaniline in 40 mL methanol. The mixture was refluxed for three hours and then cooled. The yellow-orange colored precipitate that formed was filtered off, washed with ethanol, and driedin vacuo, to yield 4.76 g (83%) of product: Anal Calcd (found) for ZnC26H22N2O2Cl2: C, 58.84 (59.17); H, 4.18 (4.44); N, 5.28 (5.21). IR (KBr, cm−1): ν(O-H) 3430w, ν(C-H) 2910, ν(C-N) 1600s, ν(C-C) 1540s.Complex
6
, Zn-sal-NH
2
, Bis(salicylaldehyde hydrazone) Zinc(II). The ligand, the nickel complex, and the zinc complex have been known since the early 1970s [50]. The ligand is commercially available but is custom-synthesized and thus very expensive. The high cost led us to synthesize the ligand in-house, according to generic procedures [48, 50–52]. The synthesis involves a condensation of salicylaldehyde with hydrazine. The reaction is highly exothermic; therefore, the synthesis is carried outvia slow addition of a dilute solution of the salicylaldehyde to a dilute solution of hydrazine hydrate. The order of addition and dilute nature of the reagents also prevents side-reactions from occurring (i.e., prevents formation of salicylaldehyde azine). The ligand was synthesized by slowly adding 3.30 mL (31.1 mmol) of salicylaldehyde in 40 mL of a 1 : 1 ethanol/water mixture to a stirring solution of 2.15 mL (about 34 mmol) of hydrazine hydrate (50–60% solution) in 40 mL of water. The solution was then refluxed for an hour, and upon cooling the resulting pale yellow product was filtered off, washed with cold ethanol, and driedin vacuo to give a yield of 4.15 g (98%) product. The complex was made by adding 3.32 g (15.1 mmol) zinc acetate dihydrate in 40 mL of a 1 : 1 dichloromethane-methanol mixture to a stirring solution of the salicylaldehyde hydrazone ligand (4.12 g, 30.3 mmol) in 40 mL methanol. The mixture was refluxed for five hours and then cooled. The bright yellow colored precipitate was filtered off, washed with ethanol and diethyl ether, and then driedin vacuo to give a yield of 3.94 g (78%) product: Anal Calcd (found) for ZnC14H14N4O2: C, 50.09 (49.77); H, 4.20 (4.39); N, 16.69 (16.62). IR (KBr, cm−1): ν(O-H) 3505w, ν(N-H) 3295s, ν(C-N) 1605s, ν(C-O) 1540s.Complex
7
, Zn-(dien)
2
·ZnCl
4
, [Bis(dien)zinc(II)] Zinc(II) Tetrachloride. The complex was synthesized in a similar manner to that reported in literature [53]. ZnCl2 (2.181 g, 16 mmol) in 40 mL anhydrous methanol was added dropwise to a stirring solution of diethylenetriamine (dien, 1.729 mL, 16 mmol) in 40 mL anhydrous methanol, at room temperature. The mixture was then heated and stirred at 60°C for three hours. Upon cooling, the resulting off-white colored precipitate was filtered and driedin vacuo to yield 3.48 g (91%) of product: CHN microanalysis, Anal Calcd (found) for Zn2C8H26N6Cl4: C, 20.06 (19.97); H, 5.47 (6.11); N, 17.55 (17.34). IR (KBr, cm−1): ν(N-H) 3330s, 3265s, 3225s, ν(C-H) 2940m, 2882m, ν(C-N) 1072s, 1028s.Complex
8
, (Zn(en)
3
Cl
2
·H
2
O), Tris(ethylenediamine)-zinc(II) Chloride. The synthesis was based on the published reports [54, 55]. In a round bottomed flask, under argon and with stirring, 5.83 mL (87 mmol) ethylenediamine was added to a solution of ZnCl2 (3.95 g, 29.0 mmol) in methanol (60 mL). The mixture was stirred overnight, reduced in volume on a rotary evaporator to 30 mL, and then filtered. The filtrate was allowed to evaporate for two days at room temperature to yield a white colored precipitate, which was filtered, washed with cold ethanol and diethyl ether, and then driedin vacuo: IR (KBr, cm−1): ν(N-H) 3500s broad, 3250s broad, 1600s, ν(C-H) 3000s, 1470s, ν(C-N) 1170m, 1060s.


## 2.1. Materials and Methods

Unless otherwise mentioned, all chemicals and reagents were of analytical grade (Sigma-Aldrich, Alfa Aesar, TCI, VWR). The solvents either were HPLC-grade or were dried and distilled using conventional methods and stored under an argon atmosphere [31, 32]. Nanopure water was used for all of the experiments. Zn(II) complexes are relatively stable in air; however, many of the ligands are air/moisture sensitive; therefore, all synthetic procedures were conducted using Schlenk techniques, and by default all compounds were stored in sealed vials under argon. The three proteins and free Trp were purchased (Sigma-Aldrich) and used without further purification. Stock solutions of proteins, Trp, and the Zn complexes were prepared in 50 mM Tris-HCl (pH 7.4) buffer solution.


## 2.2. Physical Measurements

FTIR data for solid samples (as KBr disks) and neat liquid samples were obtained on a Jasco 4000 IR spectrometer. The IR spectral peaks were calibrated with polystyrene and are reported in wavenumbers. Relative intensities of the key bands in a spectrum are indicated (w = weak, m = medium, s = strong, vs = very strong, and br = broad). Elemental analyses were performed at the UMass-Amherst Microanalysis Center, or by QTI/Intertek, Whitehouse, NJ. Samples for microanalysis were ground to a fine powder and vacuum desiccated over phosphorus pentoxide for at least four days prior to analysis. UV-vis experiments for characterization of the Zn complexes and determination of protein concentration were carried out using a Cary 4000 UV-vis spectrophotometer. Fluorescence spectra were obtained at room temperature using a Perkin-Elmer LS50B Spectrometer. The fluorescence emission spectra were corrected for wavelength dependent sensitivity using a calibration curve that was generated using five commercial spectral fluorescence standards (BAM-F001 to F005, Sigma-Aldrich) [33].For the fluorescence quenching experiments, the concentration of the protein, or free Trp, was held constant at 0.1μM and the concentration of each Zn complex was varied from 0 μM to 21.0 μM,via preparation of individual samples. The concentration range was adjusted according to whether quenching was more clear at higher or lower concentrations. The excitation wavelength was 280 nm, the emission wavelength was 345 nm for the proteins and 363 nm for Trp, and both the excitation and emission slit widths were kept constant at 4.0 nm. Fluorescence spectra were obtained at 25°C, 35°C, and 45°C. Spectra have been smoothed for presentation purposes.


## 2.3. Data Analysis

The dynamic quenching constants were determined using the Stern-Volmer relationship as shown in the following equation [24, 34]:(1)F0F=1+KSVQ,where F0 and F correspond to the fluorescence intensities of the protein in the absence and presence of quencher, respectively. [Q] is the concentration of the quencher. KSV is the Stern-Volmer quenching constant. KSV is related to the lifetime of the system according to the following equation:(2)KSV=kqτ0,where kq is the bimolecular quenching constant and τ0 is the lifetime of unquenched fluorophore. The value of τ0 is short for free Trp (2.7 ns) but longer in a protein environment. This value is dependent on the location within the protein, the extent of solvent exposure, and the vicinity of various side chains [35–37]. The static quenching constant, also known as the binding constant, Ka, and binding site number, n, were calculated from the following equation [24, 34]:(3)log⁡F0-FF=log⁡Ka+nlog⁡Q.The change in Gibb’s free energy, ΔG, was calculated using (4), where R is the gas constant and T is the temperature (K). Changes in entropy (ΔS) and enthalpy (ΔH) were determined using Van’t Hoff plot, based on the following:(4)ΔG=-RTln⁡Ka,(5)ln⁡K=-ΔHRT+ΔSR.Finally, the possibility of Forster type long-range energy transfer (FRET) from the Trp residues was explored using previously published protocols, and the Forster distances, R0, were calculated using the relevant spectroscopic properties of the participating molecules [38, 39].


## 2.4. Synthesis and Characterization of Zn Complexes

A series of eight water soluble Zn(II) complexes with varying donor atoms and ligand types were synthesized.Complex
1
, Na
2
[Zn(EDTA)]·2H
2
O, Zinc(II) Ethylenediaminetetraacetate Disodium Dehydrate. The zinc salt was synthesized in a slightly modified manner to that reported in the literature [40]. Na2(EDTA)·2H2O (10.83 g, 29.1 mmol) dissolved in 50 mL of water was added to a solution of ZnCl2 (3.96 g, 29.1 mmol) dissolved in 30 mL of water. The solution was neutralized by adding 4.89 g (58.2 mmol) of NaHCO3 and then adjusted to pH 7.0 with a few drops of 3 M HCl and heated to 80°C for 5 min. The solution was then left to concentrate in the open air at room temperature overnight. Addition of 20 mL of absolute ethanol produced a white colored crystalline material which was filtered and driedin vacuo for two days. The product was recrystallized twice from a 1 : 1 water-ethanol mixture, filtered, and driedin vacuo for a further six days to give a final yield of 10.52 g (83%): CHN microanalysis, Anal Calcd (found) for ZnC10H12N2O8·Na2·2H2O: C, 27.57 (27.28); H, 3.70 (3.35); N, 6.43 (6.38). IR (cm−1): ν(C-H) 2950m, ν(C=O) 1605vs, 1400s, 930s, ν(C-N) 1130m.Complex
2
, Zn-Pr-Pr, N,N′-Dimethyl-N-N′-bis(2-sulfanylpropyl)propylenediamine Zinc(II). The ligand N,N′-dimethyl-N,N′-bis(2-sulfanylpropyl)propylenediamine was synthesized according to the published procedures [41]. The ligand (2.390 g, 9.56 mmol) in 30 mL of 1 : 1 ethanol-methanol solvent mix was placed in a 200 mL round bottom flask in an ice bath, under an argon atmosphere, and stirred for 15 min. To this NaH (0.500 g, 20.83 mmol) was added and the solution was stirred for another 20 min under an argon atmosphere. Zn(OAc)2·2H2O (1.966 g, 8.96 mmol) was dissolved in ethanol (80 mL) under an argon atmosphere and added dropwise to the ligand. The whole mixture was allowed to stir for 15 hrs and then was concentrated on a rotary evaporator to 80 mL. The solution was filtered through a fine glass frit funnel, and the filtrate further reduced in volume to 50 mL. Diethyl ether (20 mL) was added to the solution and left in a −20°C freezer overnight. The white colored crystalline precipitate that formed was filtered, washed with diethyl ether, and driedin vacuo to yield 1.72 g (61%) of the zinc product: CHN microanalysis, Anal Calcd (found) for ZnC11H24N2S2: C, 41.10 (40.48); H, 7.71 (7.15); N, 8.93 (9.22). IR (KBr, cm−1): 1650, 1465, 1455, 1438, 1408, 1362, 1292, 1143, 1042, 1007, 985.Complex
3
, (Zn(pya
2
tn)Cl
2
), N,N′-Bis(2-pyridylmethylene)-1,3-diaminopropyl Zinc(II) Chloride. The complex was synthesized in a manner analogous to that reported for the Ni(II) complex [42, 43]. The Schiff base ligand (pya2tn) was derived from 2 equivalents of pyridine-2-carboxaldehyde and 1 equivalent of 1,3-diamino-2-propanol in isopropyl alcohol. The zinc complex was madein situ by dropwise addition of the ligand to a hot solution of ZnCl2 (1 equivalent) dissolved in absolute ethanol. The very pale yellow solution was concentrated on a rotary evaporator to 80 mL. Upon cooling, a pale yellow colored crystalline material appeared. This product was filtered, recrystallized from 10 : 1 water-isopropyl alcohol solvent mixture, and driedin vacuo for eight days to give a yield of 11.26 g (58%): CHN microanalysis, Anal Calcd (found) for ZnC15H16N4Cl2: C, 46.36 (46.02); H, 4.15 (3.98); N, 14.42 (14.22). IR (cm−1): ν(C-C, 4 bands, m) 1590 to 1440, ν(C-N) 1650s, ν(C-C) 1010s, ν(C-H) 790s.Complex
4
, (Zn(pya
2
tn-OH)Cl
2
), N,N′-Bis(2-pyridylmethylene)1,3-diamino-2-propanol Zinc(II) Chloride. The ligand was synthesized according to the modification of the published procedures [43, 44]. The Schiff base ligand (pya2tn) was derived from 2 equivalents of pyridine-2-carboxaldehyde and 1 equivalent of 1,3-diamino-2-propanol. The resulting yellow colored oil was crystallized by the addition of absolute ethanol to the neat oil. The zinc complex is made by the addition of the Schiff base ligand dissolved in absolute ethanol to a refluxing solution of ZnCl2 (1 equivalent), absolute ethanol, and 2,2-dimethoxypropane. The solution was then cooled to give a pale-beige colored crystalline material. The product was filtered, recrystallized from 10 : 1 water-methanol solvent mixture, and driedin vacuo for four days to give a yield of 17.11 g (71%): CHN microanalysis, Anal Calcd (found) for ZnC15H16N4Cl2O: C, 44.53 (44.27); H, 3.99 (3.91); N, 13.85 (13.67). IR (cm−1): ν(C-C, 4 bands) ν(O-H) 3400s broad, 1600 to 1430, ν(C-N) 1650s, ν(C-C) 1000s, ν(C-H) 780s.Complex
5
, Zn-sal-Ph-Cl
2
, Bis(N-salicylideneaniline) Zinc(II) Chloride. The ligand (5-L) and the zinc complex were synthesized in a manner analogous to that reported for the bis(N-phenylsalicylaldimine) nickel complex [45–47]. The salicylideneaniline ligand is commercially available from Sigma-Aldrich; however, for economic reasons, we chose to synthesize the ligand in-house according to generic procedures [48, 49]. In a 100 mL round bottomed flask, 2.20 mL (24.1 mmol) of aniline in 25 mL water was added to 2.95 mL (27.8 mmol) of salicylaldehyde in 20 mL of water. The flask was kept at room temperature and the solution was vigorously stirred for six hours. The yellow colored precipitate that formed was filtered off, washed with ice-cold water, and dried undervacuo to give a yellow colored precipitate, yield 4.32 g (91%). The complex was made by dropwise addition of 1.47 g (10.8 mmol) ZnCl2 in 40 mL methanol to a mixture of 4.24 g (21.6 mmol) salicylideneaniline in 40 mL methanol. The mixture was refluxed for three hours and then cooled. The yellow-orange colored precipitate that formed was filtered off, washed with ethanol, and driedin vacuo, to yield 4.76 g (83%) of product: Anal Calcd (found) for ZnC26H22N2O2Cl2: C, 58.84 (59.17); H, 4.18 (4.44); N, 5.28 (5.21). IR (KBr, cm−1): ν(O-H) 3430w, ν(C-H) 2910, ν(C-N) 1600s, ν(C-C) 1540s.Complex
6
, Zn-sal-NH
2
, Bis(salicylaldehyde hydrazone) Zinc(II). The ligand, the nickel complex, and the zinc complex have been known since the early 1970s [50]. The ligand is commercially available but is custom-synthesized and thus very expensive. The high cost led us to synthesize the ligand in-house, according to generic procedures [48, 50–52]. The synthesis involves a condensation of salicylaldehyde with hydrazine. The reaction is highly exothermic; therefore, the synthesis is carried outvia slow addition of a dilute solution of the salicylaldehyde to a dilute solution of hydrazine hydrate. The order of addition and dilute nature of the reagents also prevents side-reactions from occurring (i.e., prevents formation of salicylaldehyde azine). The ligand was synthesized by slowly adding 3.30 mL (31.1 mmol) of salicylaldehyde in 40 mL of a 1 : 1 ethanol/water mixture to a stirring solution of 2.15 mL (about 34 mmol) of hydrazine hydrate (50–60% solution) in 40 mL of water. The solution was then refluxed for an hour, and upon cooling the resulting pale yellow product was filtered off, washed with cold ethanol, and driedin vacuo to give a yield of 4.15 g (98%) product. The complex was made by adding 3.32 g (15.1 mmol) zinc acetate dihydrate in 40 mL of a 1 : 1 dichloromethane-methanol mixture to a stirring solution of the salicylaldehyde hydrazone ligand (4.12 g, 30.3 mmol) in 40 mL methanol. The mixture was refluxed for five hours and then cooled. The bright yellow colored precipitate was filtered off, washed with ethanol and diethyl ether, and then driedin vacuo to give a yield of 3.94 g (78%) product: Anal Calcd (found) for ZnC14H14N4O2: C, 50.09 (49.77); H, 4.20 (4.39); N, 16.69 (16.62). IR (KBr, cm−1): ν(O-H) 3505w, ν(N-H) 3295s, ν(C-N) 1605s, ν(C-O) 1540s.Complex
7
, Zn-(dien)
2
·ZnCl
4
, [Bis(dien)zinc(II)] Zinc(II) Tetrachloride. The complex was synthesized in a similar manner to that reported in literature [53]. ZnCl2 (2.181 g, 16 mmol) in 40 mL anhydrous methanol was added dropwise to a stirring solution of diethylenetriamine (dien, 1.729 mL, 16 mmol) in 40 mL anhydrous methanol, at room temperature. The mixture was then heated and stirred at 60°C for three hours. Upon cooling, the resulting off-white colored precipitate was filtered and driedin vacuo to yield 3.48 g (91%) of product: CHN microanalysis, Anal Calcd (found) for Zn2C8H26N6Cl4: C, 20.06 (19.97); H, 5.47 (6.11); N, 17.55 (17.34). IR (KBr, cm−1): ν(N-H) 3330s, 3265s, 3225s, ν(C-H) 2940m, 2882m, ν(C-N) 1072s, 1028s.Complex
8
, (Zn(en)
3
Cl
2
·H
2
O), Tris(ethylenediamine)-zinc(II) Chloride. The synthesis was based on the published reports [54, 55]. In a round bottomed flask, under argon and with stirring, 5.83 mL (87 mmol) ethylenediamine was added to a solution of ZnCl2 (3.95 g, 29.0 mmol) in methanol (60 mL). The mixture was stirred overnight, reduced in volume on a rotary evaporator to 30 mL, and then filtered. The filtrate was allowed to evaporate for two days at room temperature to yield a white colored precipitate, which was filtered, washed with cold ethanol and diethyl ether, and then driedin vacuo: IR (KBr, cm−1): ν(N-H) 3500s broad, 3250s broad, 1600s, ν(C-H) 3000s, 1470s, ν(C-N) 1170m, 1060s.


## 3. Results and Discussion

### 3.1. Zinc Complexes

The series of small water soluble Zn(II) complexes (Figure1) represent molecules that vary in charge (neutral, anionic, and cationic) and degree of hydrophilicity by virtue of the nature of ligands. Complexes1,6,7, and8 have been previously synthesized [40, 50, 53–55]. The remaining complexes (2,3,4, and5) are novel. All characterization data, including IR spectroscopy, UV-vis spectroscopy, and elemental microanalysis are consistent with the formulations and structures given for each complex.Figure 1
Zn(II) complexes used in this study: Complex1 is a dianion; Complexes2–6 are neutral; Complexes7 and8 are dications.1. Na2[Zn(EDTA)]·2H2O,2. Zn-Pr-Pr,3. Zn(pya2tn)Cl2,4. Zn(pya2tn-OH)Cl2,5. Zn-sal-Ph-Cl2,6. Zn-sal-NH2,7. Zn-(dien)2·ZnCl4, and8. Zn(en)3·2Cl·H2O [EDTA = ethylenediaminetetraacetate, Pr-Pr = N,N′-dimethyl-N,N′-bis(2-sulfanylpropyl)propylenediamine, tn = trimethylenediamine, pya = Schiff base ligand derived from pyridine-2-carboxaldehyde and 1,3-diaminopropane (pya2tn), sal-Ph = N-salicylideneaniline, sal-NH2 = salicylaldehyde hydrazine, dien = diethylenetriamine, and en = ethylenediamine].Complex1 is a dianion, with the [EDTA]4− chelate coordinating through the two amines and four carboxylates (N2O4 donor ligand) and adopting octahedral geometry. Complexes2 and6 are neutral in charge, with a four-coordinate ligand donor set of N2S2 and N2O2, respectively, and adopt a pseudotetrahedral structure. Complexes3,4, and5 are also neutral in charge. Complexes3 and4 possess a N4Cl2 donor ligand set, while Complex5 contains a N2O2Cl2 donor ligand set. Complexes3 and4 adopt an octahedral geometry with the coordinating chloridestrans to each other, similar to related nickel complexes [42–47]. The most significant difference between the Schiff base Complexes3 and4 is the presence of a hydroxyl group on the NN′ propyl strap. It is expected that this additional feature will enhance the solubility of Complex4 in polar solvents. Complexes7 and8 are alicyclic dications, each with an N6 donor ligand set and octahedral geometry [53, 55, 56]. Both are very soluble in polar solvents and make for an interesting comparison with Zn complexes that possess planar aromatic rings.


### 3.2. Absorption and Emission Spectra of Zn Complexes

The absorption spectra for the eight Zn complexes are shown in Figure2. No peaks were observed above 375 nm for these complexes, confirming the absence of any d-d transition. Complexes3–6 possess absorption band(s) in the visible domain, leading to the observed yellow coloration of these compounds. These bands between 215 nm and 325 nm correspond to intraligand π→π∗ and n→π∗ transitions, stemming from the phenyl or pyridyl conjugated rings [57]. Complexes3,4, and6 have measurable absorbance around 280 nm, with Complexes3 and4 being the strongest absorbers (molar extinction coefficient, ε280 ≈ 10,000 to 15,000 M−1 cm−1). ε280≈700 M−1 cm−1 for Complex6, while the other complexes have extinction coefficients at this wavelength lower than 150 M−1 cm−1.Figure 2
Absorption spectra of the eight zinc complexes. Samples were at 3.0 × 10−4 M, with the exception of Complexes3 and4, which were measured at 3.0 × 10−5 M.Characterization of the absorption spectra is important for two reasons. First, there may be the possibility of coexcitation of the complex when the protein (or Trp) is excited at 280 nm for fluorescence experiments. Second, if there is an overlap between the emission spectra of the proteins and Trp and the complex, Forster’s long-range energy transfer (FRET) may occur. In order to determine whether or not coexcitation of the complex would require spectral corrections, the fluorescence spectra of each of the eight complexes were obtained following excitation at 280 nm, as shown in Figure3(a).Figure 3
(a) Emission spectra of the eight Zn complexes (3.0 × 10−5 M). (b) Emission spectra of BSA (1.0 × 10−5 M) and Complex5 (2.1 × 10−5 M). λexc = 280 nm. Excitation and emission slit widths were both set at 4.0 nm.
(a)
(b)With the exception of Complex5 (solid line), none of the complexes emitted at 345 nm, including the complexes that exhibited strong absorption at 280 nm (Complexes3,4, and6). It is worth noting that the highest concentration of each Zn complex added in an experimental series was 2.1 × 10−5 M. Therefore, the contribution to the fluorescence intensity when the proteins (and Trp) were excited in the presence of the complex was very small (Figure 3(b)).Given that Complexes3,4, and6 exhibited strong absorption at 280 nm and Complex5 was emitted weakly at 345 nm, this could affect the absorption and subsequent emission by the proteins (and Trp) and a correction for the inner-filter effect would become necessary. However, the correction is really not necessary if the absorbance of the complex is less than 0.02, which is the case for Complex6 over the range of concentrations used in this study [58]. For Complexes3 and4, the absorbance exceeds 0.02 and the observed fluorescence, Fobs, was corrected for the inner-filter effect using the following equation [34, 59]:(6)Fcorr=Fobs×10OD280+OD345/2the corrected fluorescence intensity, Fcorr, was determined by taking into account the absorbance value of the quencher at 280 nm (OD280) and at 345 nm (OD345). The corrected intensity was then used to determine the Stern-Volmer constant (KSV) and binding constant (Ka) using (1)–(3). This correction was carried out for all Zn complexes, including the ones that were weakly absorbent at 280 nm (and the emission wavelengths).


### 3.3. Fluorescence Quenching by Zn Complexes

Proteins with different numbers and locations of Trp residues were studied. The observed fluorescence quenching is a result of the interaction between the ligand bound to the Zn in the complex, the Trp residue(s) of the protein, and its immediate vicinity in the protein. The extent of quenching as determined by a decrease in total fluorescence and calculated binding constants depends on the protein and the nature of the ligand. Three major factors are typically involved in fluorescence quenching: (i) the hydrophobicity of the ligand, (ii) the charge of the complex, and (iii) the immediate environment of the Trp residue in the protein. The globular proteins in this study have complex structures, and so many types of interactions are possible between the protein and the Zn complex, including van der Waals, electrostatic, hydrophobic, and hydrogen bonding [39].A typical fluorescence quenching series is shown in Figure4. BSA has a strong fluorescence emission with a broad peak around 345 nm upon excitation at 280 nm. The fluorescence intensity of BSA decreases in the presence of Complex5, indicating a significant interaction between the complex and protein. An isoemissive point was observed at 410 nm and the emission intensity increased with complex concentration at 450 nm. This phenomenon has no effect on the quenching of the protein and the interaction leading to the quenching. There is no shift in the emission maximum of the proteins (and Trp) when they were quenched by Complexes3,4,5, and6. The degree of fluorescence quenched in each of the combinations of fluorophore and Zn complex studied is summarized in Table 1.Table 1
Percent decrease in fluorescence intensity of fluorophore (1.0 × 10−5 M) at the highest quencher concentration (21 μM) at 25°C. Fluorescence intensity was measured at 345 nm.
3
4
5
6
BSA
21.8
—
29.6
4.291
HSA
19.6
16.0
34.6
—
Lyso
23.7
15.2
11.0
—
Trp
—
39.1
—
—
Charge
0
0
0
0
1Decrease at 1.8 × 10−5 M. Quenching reversed at quencher concentrations higher than 1.8 × 10−5 M.Figure 4
Typical fluorescence quenching spectra, showing quenching of BSA by Complex5 over a concentration range of 0.0 to 21.0 μM of the complex. An isoemissive point was observed at 410 nm.The Zn Complexes1,2,7, and8 did not quench the fluorescence of any protein or free Trp. These complexes are nonaromatic and possess no planar structural features. Complexes1,7, and8 adopt octahedral geometry, and Complex2 adopts tetrahedral geometry. The complexes do vary in charge: Complex1 is a dianion, Complexes7 and8 are dications, and Complex2 is neutral. The overall trend in the type of complexes that quench these proteins and Trp and those that do not is similar to the data obtained from a series of small Ni(II) complexes, where complexes with aromatic ligands displayed very strong interactions, and the nonaromatic nickel complexes showed no affinity towards the proteins [41].The quenching of BSA by Complex6 proceeded to a lesser extent than all other combinations. With this complex, quenching was reversed at concentrations higher than 1.8 × 10−5 M, which can be explained using Le Chatelier’s Principle, where the equilibrium shifts to the reactants when an excess of the complex is formed. As discussed later, the quenching was predominantly static in nature and due to the formation of a nonfluorescent complex. Equation (7) illustrates the equilibrium reaction:(7)Protein+Zncomplex⟷Protein-ZncomplexIn the case of free Trp, only Complex4 was found to be interacting. This complex, in addition to the planar aromatic features, possess hydroxyl (-OH or -NH2) groups that are capable of H-bonding interactions with the Trp residues. While Complex6 features readily accessible amines (-NH2) that are capable of forming significant H-bonding contacts, this complex only weakly interacted with BSA. The structural features of the ligand itself are important when considering these protein-complex interactions, particularly when there is a possibility of forming H-bonds with Trp and other amino acid residues within the immediate protein environment. It appears that the environment around Trp is also a significant factor, since the Zn complexes interacted more readily with the proteins when compared to just free Trp.The results reported here clearly show that aromatic complexes with planar structural features have a very high affinity for these globular proteins and free Trp, whereas nonaromatic complexes with octahedral geometry fail to interact with these systemsvia the Trp environment. The interaction is more likely if the complexes are neutral. Interestingly, ligands, such as N,N′-dimethyl-N-N′-bis(2-sulfanylpropyl)propylenediamine, that generate small square planar complexes, with Ni(II), for instance, interact to a much greater extent [41], but when in tetrahedral geometry (in2, e.g.) the complexes fail to interact with the proteins studied.The underlying mechanism of the interaction of Zn complexes with these proteins was studied by measuring the intrinsic fluorescence intensity of protein before and after the addition of the complexes. Quenching can be classified as either dynamic or static quenching. Static quenching occurs as a result of the formation of a relatively less-fluorescent ground state complex between the fluorophore and the quencher, whereas dynamic quenching results from a collisional process between the fluorophore and the quencher. In order to determine the fluorescence quenching mechanism, the Stern-Volmer equation was used to process the collected data. A plot ofF0/F against [quencher] is typically linear when dynamic quenching occurs ((1) and (2)) as is usually the case for gas-phase and liquid-phase systems, where kq or τ0 is large. In the case of the proteins and free Trp, τ0 is expected to be small (10−8 to 10−9 s) [41, 60].There are three approaches taken to distinguish between static quenching and dynamic quenching. First, for dynamic quenching, the maximum value ofkq is around 2.0 × 1010 M−1 s−1 [38, 61, 62]. Second, an indication that the quenching may be static is the upward curvature in dynamic quenching plots [24, 30, 60]. Thirdly, if both the binding constant, Ka, and the bimolecular quenching constant, kq, decrease with temperature, then the quenching is taken to be static. For the Zn complexes investigated, values for kq were in the order of 1011 to 1012 M−1 s−1, as summarized in Table 2. In the case of similar Ni(II) complexes, values for kq were found to be in the order of 1012 to 1013 M−1 s−1 [41]. The dynamic quenching plots for these complexes (not shown) displayed very slight upward curvature at high complex concentrations, thus lowering the R2 values. Similar upward curvature has been observed with complexes containing nickel as well as chromium(III) and molybdenum(VI) [60, 63]. Finally, both the binding constants and Stern-Volmer constants decreased with temperature, as described in a later section. These observations clearly show that static quenching predominates due to the formation of a ground state complex between the protein and Zn complex.Table 2
Summary of the Stern-Volmer constant,KSV, and the bimolecular quenching constant, kq, for BSA, HSA, lysozyme, and free Trp.
Complex
BSA
HSA
Lysozyme
Free Trp
K
S
V/M−1 (×104)
k
q/M−1 s−1 (×1012)
K
S
V/M−1 (×104)
k
q/M−1 s−1 (×1012)
K
S
V/M−1 (×104)
k
q/M−1 s−1 (×1012)
K
S
V/M−1 (×104)
k
q/M−1 s−1 (×1012)
3
1.3
1.3
1.4
1.4
1.5
1.5
—
—
4
—
—
0.94
0.94
0.69
0.69
3.0
3.0
5
2.0
2.0
2.4
2.4
0.62
0.62
—
—
6
0.22
0.22
—
—
—
—
—
—For static quenching, the apparent binding constant (Ka) for the interaction between the Zn complexes and proteins was determined using double logarithmic plots based on (3), and the results are summarized in Table 3. The value of n is associated with binding constant and implies a direct relation between the binding constant and number of binding sites. The data illustrates that smaller complexes (such as3,4, and5) exhibit moderate to strong binding interactions with HSA and lysozyme. Static quenching plots for the three proteins with Complex5 are shown in Figure 5.Table 3
Summary of binding constant,Ka, binding site number, n, and ΔG for BSA, HSA, lysozyme, and free tryptophan at 25°C.
Complex
BSA
HSA
Lysozyme
Free Trp
K
a/M−1
n
Δ
G/kJ mol−1
K
a/M−1
n
Δ
G/kJ mol−1
K
a/M−1
n
Δ
G/kJ mol−1
K
a/M−1
n
Δ
G/kJ mol−1
3
1.2 × 105
1.0
−29
7.7 × 1010
2.5
−56
6.2 × 104
1.0
−27
—
—
—
4
—
—
—
2.0 × 106
2.5
−66
3.7 × 104
1.0
−26
1.2 × 105
1.0
−29
5
1.1 × 106
1.0
−35
5.0 × 106
1.5
−38
1.7 × 107
2.0
−41
—
—
—
6
9.6 × 104
1.0
−28
—
—
—
—
—
—
—
—
—Figure 5
The Stern-Volmer plots for the static quenching of BSA (■), HSA (●), and lysozyme (▲) by Complex5 at 25°C. R2 values: BSA 0.974, HSA 0.986, and lysozyme 0.965.The calculatedKa values correlate extremely well with the extent of fluorescence quenching. There is also a strong correlation between Ka and the large negative values obtained for ΔG, as shown in Table 3. The calculated ΔG values confirm that binding is a spontaneous process and are similar to values observed in other studies involving BSA, HSA, and lysozyme [17, 39, 41, 60, 61, 64–66].The absence of any significant binding and quenching between BSA and lysozyme with complexes such as4 (with BSA) and6 (with lysozyme) is most likely due to the H-bonding interactions that arise from the presence of a -OH group in4 and -NH2 groups in6. This results in significantly strong interactions between the complex and the polar amino acids in the immediate vicinity of the Trp residue(s) in the protein.


### 3.4. Nature of the Interaction between the Proteins and Zn Complexes

The observed fluorescence emission of these proteins arises from Trp, tyrosine (Tyr), and phenylalanine (Phe) residues. Phe has a very low quantum yield, and the fluorescence of Tyr is almost totally quenched when it is ionized or close to an amino group, a carboxyl group, or a Trp. Thus, the fluorescence of these proteins is dominated by Trp emission. Fluorescence quenching of Trp residues occurs when there is significant interaction with hydrophobic ligands, which is either promoted or stabilized by additional amino acid residues in the immediate environment [41, 66]. BSA has two tryptophan residues: Trp-134 residue is near the surface of the protein surrounded by negatively charged (Glu), polar uncharged (Ser), and hydrophobic (Tyr, Val) amino acid residues. Trp-212 is in a hydrophobic pocket and surrounded by hydrophobic residues (Tyr, Leu, and Phe). HSA contains a lone Trp-214 found in a pocket, surrounded by only hydrophobic residues (Tyr, Val). In lysozyme, there are six tryptophans in various environments, some of which are surrounded by positively charged amino acids (Lys, Arg) [62].The interaction of Zn complexes with free Trp is relatively strong (Ka > 105 M−1) but is limited to Complex4. This Zn complex possesses functional groups that can H-bond to Trp and/or possess a highly labile ligand. H-bonding can lead to a very strong interaction overall; such nonhydrophobic contacts are thermodynamically favored and play a major role in generating the high Ka values. For Complex4, there is a possibility that monodentate chloride ligands are displaced in aqueous solution, which would allow free Trp to interact directly with the Zn atom through the nucleophilic O and/or N donor atoms.The interaction with lysozyme is limited to the octahedral Complexes3,4, and5. A variety of interactions are possible between lysozyme and3: Trp-28, Trp-62, Trp-63, and Trp-111 residues are close to amphiphilic amino acids, such as Lys and Arg, while Trp-108 and Trp-123 residues are close to hydrophobic Val and Ile, respectively. Complex3 is comprised of planar aromatic ligands, with minimal flexibility in the equatorial plane due to the five membered chelate rings, and, unlike Complex4, there is no possibility of forming H-bond contacts with Trp or nearby residues. The result is strong and significant interactions with lysozyme.Complexes3 and4 are both similar in structure except for the OH group on the ligand of4. Both are octahedral in geometry with the two chlorides in the axial positions and neutral in charge. Both complexes bind to HSA, but only3 binds to BSA. This observation is similar to what was observed with the analogous nickel complexes [41]. Trp-134 in BSA has a polar amino acid (Ser) in its vicinity. It is possible that a H-bonding interaction could be occurring between this residue and Complex4, in addition to the H-bonding involving Trp. The H-bonding interaction is stronger than any stacking interaction that would be expected between Tyr (or Trp) and the pyridinium group(s) in the complex. The H-bonding between the OH group in Complex4 and the Ser (and/or Trp) residue is also stronger than the hydrophobic interactions promoted by the Leu and Val residues in the vicinity of Trp-134 [62]. This situation also results in the absence of fluorescence quenching when Complex4 is added to BSA. However, BSA does have an additional residue (Trp-212) in a very similar buried hydrophobic environment to the Trp-214 in HSA. This Trp-212 residue has no polar residues in its immediate vicinity, and so one might expect some fluorescence quenching to occur albeit reduced in the case of BSA, though why no quenching was detected remains unclear. HSA does not have polar residues near its Trp-214, so the hydrophobic interactions predominate, leading to fluorescence quenching and strong binding. The binding of Complex4 to HSA (Ka~106) is weaker than that of Complex3 (Ka~1010), providing a binding site number of 1.5, which could be due to an interaction between Complex4 with a nearby tyrosine residue, through either stacking or hydrogen bonding.The values for the number of binding sites (n) varied from 1 to 2.5, as calculated from (3). In the case of BSA, the values for n were all equal to 1.0. This indicates that there is one set of binding sites in the proximity of the fluorophore in BSA for Zn complexes and that the key contact is predominantly a hydrophobic interaction. For interactions with HSA, the value of n ranged from 1.5 to 2.5 for the strongly binding Complex3 (Ka = 7.7 × 1010 M−1). A binding site number of 1.0 is typical when static quenching of proteins occurs as a result of hydrophobic interactions alone. The presence of two binding sites in HSA raises the possibility that multiple quencher complexes may be involved and that nonhydrophobic forces have a very important role to play in these close contacts.The temperature dependence of theKa and kq values indicates the nature of quenching. The Ka values can also be used to determine the signs of enthalpy and entropy changes that occur during association of the fluorophore with quencher. The decrease in the binding constants indicates that the protein-complex interactions are weakening as the temperature is raised. This observation eliminates the dynamic quenching mechanism, since dynamic quenchers do not physically bind to the target, and the Stern-Volmer constant increases with temperature. Thus, the most probable quenching mechanism is initiated by protein-complex formation rather than dynamic collision. For example, with Complex5, the binding constant Ka decreased for BSA, HSA, and lysozyme, but there was no quenching of lysozyme at 45°C. There was little to no quenching at higher temperatures with Complexes3,4, and6, with the exception of Trp, where quenching occurred at all three temperatures with Complex4. In the cases where there was little quenching, the bimolecular quenching constant, kq, decreased with temperature, which is the opposite of what is expected in the case of dynamic quenching. Van’t Hoff plots were generated using (5), and changes in enthalpy (ΔH) and entropy (ΔS) were calculated and summarized in Table 4. Van’t Hoff plots for BSA and HSA with Complex5 are presented in Figure 6.Table 4
Changes in enthalpy (ΔH) and entropy (ΔS) for the interaction of the proteins (and Trp) with Zn complexes.
4
5
Δ
H kJ mol−1
Δ
S J mol−1 K−1
Δ
H kJ mol−1
Δ
S J mol−1 K−1
BSA
—
—
−175
−468
HSA
—
—
−207
−564
Lysozyme1
—
—
−150
−365
Trp
−244
−716
—
—
1Lysozyme did not quench at 45°C so the data is based on measurements at 25°C and 35°C only.Figure 6
Van’t Hoff plots for BSA and HSA with Complex5. R2 values: BSA 0.9631, HSA 0.9896.The combination of highKa values (>104 M−1) and negative ΔH values clearly shows that the binding process is highly spontaneous and exothermic. The exothermic interaction is consistent with “bond formation” or binding, which results in the product being lower in energy. This data also confirms that the binding weakens with increasing temperature and the value for Ka decreases. According to Le Chatelier’s principle, exothermic reactions favor reactants as the temperature increases. Negative values for both ΔH and ΔS show that the interaction between these Zn complexes and the proteins is a result of van der Waals forces and H-bonding and drives the reaction forward [61]. Wu and coworkers reported negative entropy values for HSA and a positive entropy value for BSA [38, 67]. In our previous study with a dioxo-Mo(VI) complex, negative values for both ΔH and ΔS for BSA, HSA, lysozyme, and tryptophan were reported [63].The possibility of Forster’s long-range resonance energy transfer (FRET), which occurs over a distance of 2–10 nm, was investigated. In order for this type of quenching to occur, the emission spectrum of the donor (protein or Trp) must have some overlap with the absorption spectrum of the acceptor (Zn complex). The absorption spectra of Complexes5 and6 do display (Figure 2 and highlighted in Figure 7) some overlap with the emission spectra of the proteins and Trp.Figure 7
Fluorescence emission spectrum of 1.0 × 10−5 M BSA (solid line) and the absorption spectra of 1.0 × 10−5 M Complex5 (dotted line) and Complex6 (dashed line) showing minor spectral overlap.The spectral overlap integral between the protein emission and complex absorbance was calculated to be in the order of 10−15–10−16 L·cm3·mol−1 due to the low molar absorptivity of these complexes, and Forster distances (r0, the distance at which 50% energy transfer occurs) are less than 2 nm (Table 5); thus, one can rule out quenching due to FRET. Taking the temperature dependence and magnitude of kq, it is clear that static quenching is predominant in these systems. The Forster distances are in good agreement with what we have reported for the dioxo-Mo(VI) complex and with other reports in the literature [39, 63].Table 5
Summary of the FRET analysis for the overlap (J) between the absorption spectrum of Complexes 5 and 6 and the emission spectra of BSA, HSA, and lysozyme and the Forster distance (R0) for the combinations that showed fluorescence quenching.
5
6
J (L·cm3/mol)
R
0 (nm)
J (L·cm3/mol)
R
0 (nm)
BSA
1.46 × 10−15
1.73
5.89 × 10−16
1.49
HSA
1.49 × 10−15
1.74
—
—
Lysozyme
4.87 × 10−16
1.26
—
—Molecular modeling studies (Gaussian, Docking) are currently underway to pinpoint and determine optimal binding and the energetic contribution that accompanies the interaction between Trp residues and their protein environment in HSA, BSA, and lysozyme with this series of Zn complexes.


## 3.1. Zinc Complexes

The series of small water soluble Zn(II) complexes (Figure1) represent molecules that vary in charge (neutral, anionic, and cationic) and degree of hydrophilicity by virtue of the nature of ligands. Complexes1,6,7, and8 have been previously synthesized [40, 50, 53–55]. The remaining complexes (2,3,4, and5) are novel. All characterization data, including IR spectroscopy, UV-vis spectroscopy, and elemental microanalysis are consistent with the formulations and structures given for each complex.Figure 1
Zn(II) complexes used in this study: Complex1 is a dianion; Complexes2–6 are neutral; Complexes7 and8 are dications.1. Na2[Zn(EDTA)]·2H2O,2. Zn-Pr-Pr,3. Zn(pya2tn)Cl2,4. Zn(pya2tn-OH)Cl2,5. Zn-sal-Ph-Cl2,6. Zn-sal-NH2,7. Zn-(dien)2·ZnCl4, and8. Zn(en)3·2Cl·H2O [EDTA = ethylenediaminetetraacetate, Pr-Pr = N,N′-dimethyl-N,N′-bis(2-sulfanylpropyl)propylenediamine, tn = trimethylenediamine, pya = Schiff base ligand derived from pyridine-2-carboxaldehyde and 1,3-diaminopropane (pya2tn), sal-Ph = N-salicylideneaniline, sal-NH2 = salicylaldehyde hydrazine, dien = diethylenetriamine, and en = ethylenediamine].Complex1 is a dianion, with the [EDTA]4− chelate coordinating through the two amines and four carboxylates (N2O4 donor ligand) and adopting octahedral geometry. Complexes2 and6 are neutral in charge, with a four-coordinate ligand donor set of N2S2 and N2O2, respectively, and adopt a pseudotetrahedral structure. Complexes3,4, and5 are also neutral in charge. Complexes3 and4 possess a N4Cl2 donor ligand set, while Complex5 contains a N2O2Cl2 donor ligand set. Complexes3 and4 adopt an octahedral geometry with the coordinating chloridestrans to each other, similar to related nickel complexes [42–47]. The most significant difference between the Schiff base Complexes3 and4 is the presence of a hydroxyl group on the NN′ propyl strap. It is expected that this additional feature will enhance the solubility of Complex4 in polar solvents. Complexes7 and8 are alicyclic dications, each with an N6 donor ligand set and octahedral geometry [53, 55, 56]. Both are very soluble in polar solvents and make for an interesting comparison with Zn complexes that possess planar aromatic rings.


## 3.2. Absorption and Emission Spectra of Zn Complexes

The absorption spectra for the eight Zn complexes are shown in Figure2. No peaks were observed above 375 nm for these complexes, confirming the absence of any d-d transition. Complexes3–6 possess absorption band(s) in the visible domain, leading to the observed yellow coloration of these compounds. These bands between 215 nm and 325 nm correspond to intraligand π→π∗ and n→π∗ transitions, stemming from the phenyl or pyridyl conjugated rings [57]. Complexes3,4, and6 have measurable absorbance around 280 nm, with Complexes3 and4 being the strongest absorbers (molar extinction coefficient, ε280 ≈ 10,000 to 15,000 M−1 cm−1). ε280≈700 M−1 cm−1 for Complex6, while the other complexes have extinction coefficients at this wavelength lower than 150 M−1 cm−1.Figure 2
Absorption spectra of the eight zinc complexes. Samples were at 3.0 × 10−4 M, with the exception of Complexes3 and4, which were measured at 3.0 × 10−5 M.Characterization of the absorption spectra is important for two reasons. First, there may be the possibility of coexcitation of the complex when the protein (or Trp) is excited at 280 nm for fluorescence experiments. Second, if there is an overlap between the emission spectra of the proteins and Trp and the complex, Forster’s long-range energy transfer (FRET) may occur. In order to determine whether or not coexcitation of the complex would require spectral corrections, the fluorescence spectra of each of the eight complexes were obtained following excitation at 280 nm, as shown in Figure3(a).Figure 3
(a) Emission spectra of the eight Zn complexes (3.0 × 10−5 M). (b) Emission spectra of BSA (1.0 × 10−5 M) and Complex5 (2.1 × 10−5 M). λexc = 280 nm. Excitation and emission slit widths were both set at 4.0 nm.
(a)
(b)With the exception of Complex5 (solid line), none of the complexes emitted at 345 nm, including the complexes that exhibited strong absorption at 280 nm (Complexes3,4, and6). It is worth noting that the highest concentration of each Zn complex added in an experimental series was 2.1 × 10−5 M. Therefore, the contribution to the fluorescence intensity when the proteins (and Trp) were excited in the presence of the complex was very small (Figure 3(b)).Given that Complexes3,4, and6 exhibited strong absorption at 280 nm and Complex5 was emitted weakly at 345 nm, this could affect the absorption and subsequent emission by the proteins (and Trp) and a correction for the inner-filter effect would become necessary. However, the correction is really not necessary if the absorbance of the complex is less than 0.02, which is the case for Complex6 over the range of concentrations used in this study [58]. For Complexes3 and4, the absorbance exceeds 0.02 and the observed fluorescence, Fobs, was corrected for the inner-filter effect using the following equation [34, 59]:(6)Fcorr=Fobs×10OD280+OD345/2the corrected fluorescence intensity, Fcorr, was determined by taking into account the absorbance value of the quencher at 280 nm (OD280) and at 345 nm (OD345). The corrected intensity was then used to determine the Stern-Volmer constant (KSV) and binding constant (Ka) using (1)–(3). This correction was carried out for all Zn complexes, including the ones that were weakly absorbent at 280 nm (and the emission wavelengths).


## 3.3. Fluorescence Quenching by Zn Complexes

Proteins with different numbers and locations of Trp residues were studied. The observed fluorescence quenching is a result of the interaction between the ligand bound to the Zn in the complex, the Trp residue(s) of the protein, and its immediate vicinity in the protein. The extent of quenching as determined by a decrease in total fluorescence and calculated binding constants depends on the protein and the nature of the ligand. Three major factors are typically involved in fluorescence quenching: (i) the hydrophobicity of the ligand, (ii) the charge of the complex, and (iii) the immediate environment of the Trp residue in the protein. The globular proteins in this study have complex structures, and so many types of interactions are possible between the protein and the Zn complex, including van der Waals, electrostatic, hydrophobic, and hydrogen bonding [39].A typical fluorescence quenching series is shown in Figure4. BSA has a strong fluorescence emission with a broad peak around 345 nm upon excitation at 280 nm. The fluorescence intensity of BSA decreases in the presence of Complex5, indicating a significant interaction between the complex and protein. An isoemissive point was observed at 410 nm and the emission intensity increased with complex concentration at 450 nm. This phenomenon has no effect on the quenching of the protein and the interaction leading to the quenching. There is no shift in the emission maximum of the proteins (and Trp) when they were quenched by Complexes3,4,5, and6. The degree of fluorescence quenched in each of the combinations of fluorophore and Zn complex studied is summarized in Table 1.Table 1
Percent decrease in fluorescence intensity of fluorophore (1.0 × 10−5 M) at the highest quencher concentration (21 μM) at 25°C. Fluorescence intensity was measured at 345 nm.
3
4
5
6
BSA
21.8
—
29.6
4.291
HSA
19.6
16.0
34.6
—
Lyso
23.7
15.2
11.0
—
Trp
—
39.1
—
—
Charge
0
0
0
0
1Decrease at 1.8 × 10−5 M. Quenching reversed at quencher concentrations higher than 1.8 × 10−5 M.Figure 4
Typical fluorescence quenching spectra, showing quenching of BSA by Complex5 over a concentration range of 0.0 to 21.0 μM of the complex. An isoemissive point was observed at 410 nm.The Zn Complexes1,2,7, and8 did not quench the fluorescence of any protein or free Trp. These complexes are nonaromatic and possess no planar structural features. Complexes1,7, and8 adopt octahedral geometry, and Complex2 adopts tetrahedral geometry. The complexes do vary in charge: Complex1 is a dianion, Complexes7 and8 are dications, and Complex2 is neutral. The overall trend in the type of complexes that quench these proteins and Trp and those that do not is similar to the data obtained from a series of small Ni(II) complexes, where complexes with aromatic ligands displayed very strong interactions, and the nonaromatic nickel complexes showed no affinity towards the proteins [41].The quenching of BSA by Complex6 proceeded to a lesser extent than all other combinations. With this complex, quenching was reversed at concentrations higher than 1.8 × 10−5 M, which can be explained using Le Chatelier’s Principle, where the equilibrium shifts to the reactants when an excess of the complex is formed. As discussed later, the quenching was predominantly static in nature and due to the formation of a nonfluorescent complex. Equation (7) illustrates the equilibrium reaction:(7)Protein+Zncomplex⟷Protein-ZncomplexIn the case of free Trp, only Complex4 was found to be interacting. This complex, in addition to the planar aromatic features, possess hydroxyl (-OH or -NH2) groups that are capable of H-bonding interactions with the Trp residues. While Complex6 features readily accessible amines (-NH2) that are capable of forming significant H-bonding contacts, this complex only weakly interacted with BSA. The structural features of the ligand itself are important when considering these protein-complex interactions, particularly when there is a possibility of forming H-bonds with Trp and other amino acid residues within the immediate protein environment. It appears that the environment around Trp is also a significant factor, since the Zn complexes interacted more readily with the proteins when compared to just free Trp.The results reported here clearly show that aromatic complexes with planar structural features have a very high affinity for these globular proteins and free Trp, whereas nonaromatic complexes with octahedral geometry fail to interact with these systemsvia the Trp environment. The interaction is more likely if the complexes are neutral. Interestingly, ligands, such as N,N′-dimethyl-N-N′-bis(2-sulfanylpropyl)propylenediamine, that generate small square planar complexes, with Ni(II), for instance, interact to a much greater extent [41], but when in tetrahedral geometry (in2, e.g.) the complexes fail to interact with the proteins studied.The underlying mechanism of the interaction of Zn complexes with these proteins was studied by measuring the intrinsic fluorescence intensity of protein before and after the addition of the complexes. Quenching can be classified as either dynamic or static quenching. Static quenching occurs as a result of the formation of a relatively less-fluorescent ground state complex between the fluorophore and the quencher, whereas dynamic quenching results from a collisional process between the fluorophore and the quencher. In order to determine the fluorescence quenching mechanism, the Stern-Volmer equation was used to process the collected data. A plot ofF0/F against [quencher] is typically linear when dynamic quenching occurs ((1) and (2)) as is usually the case for gas-phase and liquid-phase systems, where kq or τ0 is large. In the case of the proteins and free Trp, τ0 is expected to be small (10−8 to 10−9 s) [41, 60].There are three approaches taken to distinguish between static quenching and dynamic quenching. First, for dynamic quenching, the maximum value ofkq is around 2.0 × 1010 M−1 s−1 [38, 61, 62]. Second, an indication that the quenching may be static is the upward curvature in dynamic quenching plots [24, 30, 60]. Thirdly, if both the binding constant, Ka, and the bimolecular quenching constant, kq, decrease with temperature, then the quenching is taken to be static. For the Zn complexes investigated, values for kq were in the order of 1011 to 1012 M−1 s−1, as summarized in Table 2. In the case of similar Ni(II) complexes, values for kq were found to be in the order of 1012 to 1013 M−1 s−1 [41]. The dynamic quenching plots for these complexes (not shown) displayed very slight upward curvature at high complex concentrations, thus lowering the R2 values. Similar upward curvature has been observed with complexes containing nickel as well as chromium(III) and molybdenum(VI) [60, 63]. Finally, both the binding constants and Stern-Volmer constants decreased with temperature, as described in a later section. These observations clearly show that static quenching predominates due to the formation of a ground state complex between the protein and Zn complex.Table 2
Summary of the Stern-Volmer constant,KSV, and the bimolecular quenching constant, kq, for BSA, HSA, lysozyme, and free Trp.
Complex
BSA
HSA
Lysozyme
Free Trp
K
S
V/M−1 (×104)
k
q/M−1 s−1 (×1012)
K
S
V/M−1 (×104)
k
q/M−1 s−1 (×1012)
K
S
V/M−1 (×104)
k
q/M−1 s−1 (×1012)
K
S
V/M−1 (×104)
k
q/M−1 s−1 (×1012)
3
1.3
1.3
1.4
1.4
1.5
1.5
—
—
4
—
—
0.94
0.94
0.69
0.69
3.0
3.0
5
2.0
2.0
2.4
2.4
0.62
0.62
—
—
6
0.22
0.22
—
—
—
—
—
—For static quenching, the apparent binding constant (Ka) for the interaction between the Zn complexes and proteins was determined using double logarithmic plots based on (3), and the results are summarized in Table 3. The value of n is associated with binding constant and implies a direct relation between the binding constant and number of binding sites. The data illustrates that smaller complexes (such as3,4, and5) exhibit moderate to strong binding interactions with HSA and lysozyme. Static quenching plots for the three proteins with Complex5 are shown in Figure 5.Table 3
Summary of binding constant,Ka, binding site number, n, and ΔG for BSA, HSA, lysozyme, and free tryptophan at 25°C.
Complex
BSA
HSA
Lysozyme
Free Trp
K
a/M−1
n
Δ
G/kJ mol−1
K
a/M−1
n
Δ
G/kJ mol−1
K
a/M−1
n
Δ
G/kJ mol−1
K
a/M−1
n
Δ
G/kJ mol−1
3
1.2 × 105
1.0
−29
7.7 × 1010
2.5
−56
6.2 × 104
1.0
−27
—
—
—
4
—
—
—
2.0 × 106
2.5
−66
3.7 × 104
1.0
−26
1.2 × 105
1.0
−29
5
1.1 × 106
1.0
−35
5.0 × 106
1.5
−38
1.7 × 107
2.0
−41
—
—
—
6
9.6 × 104
1.0
−28
—
—
—
—
—
—
—
—
—Figure 5
The Stern-Volmer plots for the static quenching of BSA (■), HSA (●), and lysozyme (▲) by Complex5 at 25°C. R2 values: BSA 0.974, HSA 0.986, and lysozyme 0.965.The calculatedKa values correlate extremely well with the extent of fluorescence quenching. There is also a strong correlation between Ka and the large negative values obtained for ΔG, as shown in Table 3. The calculated ΔG values confirm that binding is a spontaneous process and are similar to values observed in other studies involving BSA, HSA, and lysozyme [17, 39, 41, 60, 61, 64–66].The absence of any significant binding and quenching between BSA and lysozyme with complexes such as4 (with BSA) and6 (with lysozyme) is most likely due to the H-bonding interactions that arise from the presence of a -OH group in4 and -NH2 groups in6. This results in significantly strong interactions between the complex and the polar amino acids in the immediate vicinity of the Trp residue(s) in the protein.


## 3.4. Nature of the Interaction between the Proteins and Zn Complexes

The observed fluorescence emission of these proteins arises from Trp, tyrosine (Tyr), and phenylalanine (Phe) residues. Phe has a very low quantum yield, and the fluorescence of Tyr is almost totally quenched when it is ionized or close to an amino group, a carboxyl group, or a Trp. Thus, the fluorescence of these proteins is dominated by Trp emission. Fluorescence quenching of Trp residues occurs when there is significant interaction with hydrophobic ligands, which is either promoted or stabilized by additional amino acid residues in the immediate environment [41, 66]. BSA has two tryptophan residues: Trp-134 residue is near the surface of the protein surrounded by negatively charged (Glu), polar uncharged (Ser), and hydrophobic (Tyr, Val) amino acid residues. Trp-212 is in a hydrophobic pocket and surrounded by hydrophobic residues (Tyr, Leu, and Phe). HSA contains a lone Trp-214 found in a pocket, surrounded by only hydrophobic residues (Tyr, Val). In lysozyme, there are six tryptophans in various environments, some of which are surrounded by positively charged amino acids (Lys, Arg) [62].The interaction of Zn complexes with free Trp is relatively strong (Ka > 105 M−1) but is limited to Complex4. This Zn complex possesses functional groups that can H-bond to Trp and/or possess a highly labile ligand. H-bonding can lead to a very strong interaction overall; such nonhydrophobic contacts are thermodynamically favored and play a major role in generating the high Ka values. For Complex4, there is a possibility that monodentate chloride ligands are displaced in aqueous solution, which would allow free Trp to interact directly with the Zn atom through the nucleophilic O and/or N donor atoms.The interaction with lysozyme is limited to the octahedral Complexes3,4, and5. A variety of interactions are possible between lysozyme and3: Trp-28, Trp-62, Trp-63, and Trp-111 residues are close to amphiphilic amino acids, such as Lys and Arg, while Trp-108 and Trp-123 residues are close to hydrophobic Val and Ile, respectively. Complex3 is comprised of planar aromatic ligands, with minimal flexibility in the equatorial plane due to the five membered chelate rings, and, unlike Complex4, there is no possibility of forming H-bond contacts with Trp or nearby residues. The result is strong and significant interactions with lysozyme.Complexes3 and4 are both similar in structure except for the OH group on the ligand of4. Both are octahedral in geometry with the two chlorides in the axial positions and neutral in charge. Both complexes bind to HSA, but only3 binds to BSA. This observation is similar to what was observed with the analogous nickel complexes [41]. Trp-134 in BSA has a polar amino acid (Ser) in its vicinity. It is possible that a H-bonding interaction could be occurring between this residue and Complex4, in addition to the H-bonding involving Trp. The H-bonding interaction is stronger than any stacking interaction that would be expected between Tyr (or Trp) and the pyridinium group(s) in the complex. The H-bonding between the OH group in Complex4 and the Ser (and/or Trp) residue is also stronger than the hydrophobic interactions promoted by the Leu and Val residues in the vicinity of Trp-134 [62]. This situation also results in the absence of fluorescence quenching when Complex4 is added to BSA. However, BSA does have an additional residue (Trp-212) in a very similar buried hydrophobic environment to the Trp-214 in HSA. This Trp-212 residue has no polar residues in its immediate vicinity, and so one might expect some fluorescence quenching to occur albeit reduced in the case of BSA, though why no quenching was detected remains unclear. HSA does not have polar residues near its Trp-214, so the hydrophobic interactions predominate, leading to fluorescence quenching and strong binding. The binding of Complex4 to HSA (Ka~106) is weaker than that of Complex3 (Ka~1010), providing a binding site number of 1.5, which could be due to an interaction between Complex4 with a nearby tyrosine residue, through either stacking or hydrogen bonding.The values for the number of binding sites (n) varied from 1 to 2.5, as calculated from (3). In the case of BSA, the values for n were all equal to 1.0. This indicates that there is one set of binding sites in the proximity of the fluorophore in BSA for Zn complexes and that the key contact is predominantly a hydrophobic interaction. For interactions with HSA, the value of n ranged from 1.5 to 2.5 for the strongly binding Complex3 (Ka = 7.7 × 1010 M−1). A binding site number of 1.0 is typical when static quenching of proteins occurs as a result of hydrophobic interactions alone. The presence of two binding sites in HSA raises the possibility that multiple quencher complexes may be involved and that nonhydrophobic forces have a very important role to play in these close contacts.The temperature dependence of theKa and kq values indicates the nature of quenching. The Ka values can also be used to determine the signs of enthalpy and entropy changes that occur during association of the fluorophore with quencher. The decrease in the binding constants indicates that the protein-complex interactions are weakening as the temperature is raised. This observation eliminates the dynamic quenching mechanism, since dynamic quenchers do not physically bind to the target, and the Stern-Volmer constant increases with temperature. Thus, the most probable quenching mechanism is initiated by protein-complex formation rather than dynamic collision. For example, with Complex5, the binding constant Ka decreased for BSA, HSA, and lysozyme, but there was no quenching of lysozyme at 45°C. There was little to no quenching at higher temperatures with Complexes3,4, and6, with the exception of Trp, where quenching occurred at all three temperatures with Complex4. In the cases where there was little quenching, the bimolecular quenching constant, kq, decreased with temperature, which is the opposite of what is expected in the case of dynamic quenching. Van’t Hoff plots were generated using (5), and changes in enthalpy (ΔH) and entropy (ΔS) were calculated and summarized in Table 4. Van’t Hoff plots for BSA and HSA with Complex5 are presented in Figure 6.Table 4
Changes in enthalpy (ΔH) and entropy (ΔS) for the interaction of the proteins (and Trp) with Zn complexes.
4
5
Δ
H kJ mol−1
Δ
S J mol−1 K−1
Δ
H kJ mol−1
Δ
S J mol−1 K−1
BSA
—
—
−175
−468
HSA
—
—
−207
−564
Lysozyme1
—
—
−150
−365
Trp
−244
−716
—
—
1Lysozyme did not quench at 45°C so the data is based on measurements at 25°C and 35°C only.Figure 6
Van’t Hoff plots for BSA and HSA with Complex5. R2 values: BSA 0.9631, HSA 0.9896.The combination of highKa values (>104 M−1) and negative ΔH values clearly shows that the binding process is highly spontaneous and exothermic. The exothermic interaction is consistent with “bond formation” or binding, which results in the product being lower in energy. This data also confirms that the binding weakens with increasing temperature and the value for Ka decreases. According to Le Chatelier’s principle, exothermic reactions favor reactants as the temperature increases. Negative values for both ΔH and ΔS show that the interaction between these Zn complexes and the proteins is a result of van der Waals forces and H-bonding and drives the reaction forward [61]. Wu and coworkers reported negative entropy values for HSA and a positive entropy value for BSA [38, 67]. In our previous study with a dioxo-Mo(VI) complex, negative values for both ΔH and ΔS for BSA, HSA, lysozyme, and tryptophan were reported [63].The possibility of Forster’s long-range resonance energy transfer (FRET), which occurs over a distance of 2–10 nm, was investigated. In order for this type of quenching to occur, the emission spectrum of the donor (protein or Trp) must have some overlap with the absorption spectrum of the acceptor (Zn complex). The absorption spectra of Complexes5 and6 do display (Figure 2 and highlighted in Figure 7) some overlap with the emission spectra of the proteins and Trp.Figure 7
Fluorescence emission spectrum of 1.0 × 10−5 M BSA (solid line) and the absorption spectra of 1.0 × 10−5 M Complex5 (dotted line) and Complex6 (dashed line) showing minor spectral overlap.The spectral overlap integral between the protein emission and complex absorbance was calculated to be in the order of 10−15–10−16 L·cm3·mol−1 due to the low molar absorptivity of these complexes, and Forster distances (r0, the distance at which 50% energy transfer occurs) are less than 2 nm (Table 5); thus, one can rule out quenching due to FRET. Taking the temperature dependence and magnitude of kq, it is clear that static quenching is predominant in these systems. The Forster distances are in good agreement with what we have reported for the dioxo-Mo(VI) complex and with other reports in the literature [39, 63].Table 5
Summary of the FRET analysis for the overlap (J) between the absorption spectrum of Complexes 5 and 6 and the emission spectra of BSA, HSA, and lysozyme and the Forster distance (R0) for the combinations that showed fluorescence quenching.
5
6
J (L·cm3/mol)
R
0 (nm)
J (L·cm3/mol)
R
0 (nm)
BSA
1.46 × 10−15
1.73
5.89 × 10−16
1.49
HSA
1.49 × 10−15
1.74
—
—
Lysozyme
4.87 × 10−16
1.26
—
—Molecular modeling studies (Gaussian, Docking) are currently underway to pinpoint and determine optimal binding and the energetic contribution that accompanies the interaction between Trp residues and their protein environment in HSA, BSA, and lysozyme with this series of Zn complexes.


## 4. Conclusion

The synthesis and characterization of a series of Zn(II) complexes with different types of ligands containing N, S, and O donor atoms are reported. Fluorescence spectroscopy and Stern-Volmer kinetics were used to study the interaction of the Zn complexes with human and bovine serum albumin and lysozyme proteins. The addition of the complexes causes the intrinsic fluorescence of Trp residues to quench by varying amounts depending on the nature of complex. The Zn complexes possessing planar aromatic ligands exhibit exceptionally strong interactions and much greater fluorescence quenching, particularly with the Trp residues located in hydrophobic environments. Static quenching was found to be the predominant form of quenching in these systems, generating binding constants over a wide range (104–1010 M−1). The thermodynamic parameters, as estimated from the Stern-Volmer plots and Gibbs’ free energy values, suggest that the binding of Zn complexes to the proteins is a highly spontaneous process. In the case of BSA the binding reaction was mainly driven by hydrophobic interactions. For HSA, lysozyme, and free Trp, the thermodynamic parameters suggest a combination of forces at play. The fluorescence studies described may provide an approach in evaluating the molecular mechanism of metal-based chemicals on serum proteins.



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