# Kinetic and Mechanistic Studies on the Interaction of Glycyl-L-alanine, Glycyl-L-asparagine, and Glycyl-L-tyrosine with Hydroxopentaaquarhodium(III) Ion

Authors: Biplab K. Bera; Sumon Ray; Subala Mondal; Parnajyoti Karmakar; Arup Mandal; Subhasis Mallick; Alak K. Ghosh
Journal: Journal of Chemistry
 (2013)

---

## Abstract

The kinetics of the interaction of three glycine-containing dipeptides, namely, glycyl-L-alanine (L1-L′H), glycyl-L-asparagine (L2-L′H), and glycyl-L-tyrosine (L3-L′H) with [Rh(H2O)5OH]2+
has been studied spectrophotometrically in aqueous medium as a function of the molar concentration of [Rh(H2O)5OH]2+, [dipeptide], pH, and temperature at constant ionic strength. Reactions were studied at pH 4.3, where the substrate complex exists predominantly as the hydroxopentaaqua species and dipeptides as the zwitterion. The reaction has been found to proceed via two parallel paths: both processes are ligand dependent. The rate constant for the processes are k1~10-3s-1 and k2~10-5s-1. The activation parameters for both the steps were evaluated using Eyring’s equation. The low ΔH1≠ and large negative value of ΔS1≠ as well as ΔH2≠ and ΔS2≠ indicate an associative mode of activation for both the aqua ligand substitution processes for both the parallel paths. The product of the reaction has been characterized by IR and ESI-mass spectroscopic analyses.


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## Body

## 1. Introduction

The continued interest in platinum-based antitumor compounds is stimulated by the fact that certain tumors are resistant to the clinically used drugscis-platin and carboplatin. As work progressed, different Pt(II) amine complexes and their derivatives as well as complexes of other 4d and 5d metal ions with nucleic acid constituents [1, 2] were studied. Complexes of other metal ions specially ruthenium, rhodium, iridium, and palladium have also been reported to have considerable antibacterial power [3–5]. It is reported that ruthenium complexes are an order of magnitude less toxic than cis-platin [6, 7]. The novel rhodium(III) and iridium(III) complexes are characterized as potential anticancer agents in respect to their cytotoxicity [8]. Meridional rhodium(III) polypyridyl complexes of the type mer-[RhX3(DMSO)(pp)] (X=Cl, pp=phen, dpq, dppz; X=Br, pp=phen) represent a promising class of potent cytostatic agents for the treatment of lymphoma and leukemia [9].It is now established [10] that cis-platin at first hydrolyses in the biological condition and the aqua variety is the active species. Some of the hydrolyzed products are also responsible for toxicity. Thus, it is expected that aqua complexes if used directly will be less toxic. In order to examine the bioactivity of rhodium(III) complexes, studies on the interaction of rhodium(III) with pyridine-2-aldoxime [11], DL-methionine [12], L-cysteine [13], and adenosine [14] have already been reported. In the present paper we report the results on the interaction of three glycine containing dipeptides glycyl-L-alanine (L1-L′H), glycyl-L-aspergine (L2-L′H) and glycyl-L-tyrosine (L3-L′H) with the title complex.  Obtained results are investigated for the kinetic tuning of the interaction of such ligands via electronic and steric effects. This work describes the detailed kinetic and mechanistic studies of aqua ligand substitution from hydroxopentaaquarhodium(III) ion by the dipeptide which is a model dipeptide. This work is also interesting from kinetic view point because of its parallel reaction paths.


## 2. Experimental

[Rh(H2O)6](ClO4)3 was prepared as per the literature method [15] and characterized by chemical analysis and spectroscopic data [16] (λmax=396 nm, ε=62 dm3 mol−1 cm−1; λmax=311 nm, ε=67.4  dm3 mol−1 cm−1). The reactant complex [Rh(H2O)5(OH)](ClO4)2 [complex A] was obtained in situ (yield ~ 90%) by adjusting the pH to 4.3. Higher proportions of complex could not be obtained as the solution becomes turbid at higher pH. The reaction product of dipeptides and complex A was (substituted complex: complex C, complex D, and complex E) prepared by mixing the reactants in different ratios, namely, 1 : 1, 1 : 2, 1 : 3, 1 : 5, and 1 : 10, and equilibrating the mixtures at 60°C for 72 h. The absorption spectra of all these mixtures (Figure 1) for each of complex C, complex D, and complex E show identical λmax with almost same absorbance indicating the complete complexation. But λmax for complex C–Eare 224 nm, 226 nm, and 239 nm, respectively.Figure 1
Spectra of the starting complex (A), glycyl-L-alanine (L1-L′H) substituted complex (C),  glycyl-L-aspergine (L2-L′H) substituted complex (D), and glycyl-L-tyrosine (L3-L′H)  substituted complex (E); [complex A] = 2.5 × 10−4 mol dm−3, [dipeptide] = 7.5 × 10−3 mol dm−3,  pH = 4.3,  cell used = 1 cm quartz.


### 2.1. Product Analysis

The composition of the product in the reaction mixture was determined by Job’s   method of continuous variation (Figure2). The metal-ligand ratio was found to be 2 : 1.Figure 2
Job’s plot for reaction of complexA with glycyl-L-alanine (L1-L′H) at the wavelength 224 nm.[Rh(H2O)5(OH)]2+ and dipeptides were mixed in 2 : 1 molar ratio at pH 4.3, and the products were obtained. The IR spectra of all the product complexes, in the KBr disc, show strong bands in the region ~3414–3094 cm−1, together with medium bands at 1609, 559, and 398 cm−1. The asymmetric -COO− stretching frequency (νasym) of the zwitterionic forms of amino acids occurs at 1580–1660 cm−1 when the group is coordinated to metals, where as a noncoordinated -COO− group has the νasym (COO−) stretching at lower frequency [17]. The band at 1609 cm−1 is therefore due to the νasym (COO−) of the metal bound carboxyl group. The presence of strong stretching band at ~3414 cm−1 indicates that the product contains aqua or hydroxyl ligands. The bands at 559 and 398 cm−1 are assigned to ν(Rh–N) and ν(Rh–O) bond formation, respectively [18]. An intense band of the ν(C=O)amide at 1693 cm−1 in the noncoordinated peptide undergoes a bathochromic shift of ~84 cm−1 in the IR spectrum upon complexation. This is probably due to the involvement of the peptide nitrogen (because of the deprotonation that has taken place) in bonding with Rh(III), which lowers the bond order of the ν(C=O)amide group due to resonance stabilization.The aqueous solution’s of [Rh(H2O)5(OH)]2+ and glycyl-L-alanine (L1-L′H) were mixed in a 2 : 1 molar ratio, and the mixture was thermostated at 60°C for 48 hours and used for ESI-MS measurement. The ESI mass spectra of the resulting solution are shown in Figure 3.Figure 3
ESI-mass spectrum of the substituted hydroxopentaaquarhodium(III) ion by glycyl-L-alanine.It is clear from this spectrum that the ion atm/z 246.18 (minor peak) has become the parent ion species in the mixture solution, and this is tentatively attributed to (glycyl-L-alanine + 2Rh3+ + 6H2O + 2HO−)2+. The parent ion is shown in Figure 4.Figure 4
Plausible structure of the parent ion from the ESI-mass spectrum.


## 2.1. Product Analysis

The composition of the product in the reaction mixture was determined by Job’s   method of continuous variation (Figure2). The metal-ligand ratio was found to be 2 : 1.Figure 2
Job’s plot for reaction of complexA with glycyl-L-alanine (L1-L′H) at the wavelength 224 nm.[Rh(H2O)5(OH)]2+ and dipeptides were mixed in 2 : 1 molar ratio at pH 4.3, and the products were obtained. The IR spectra of all the product complexes, in the KBr disc, show strong bands in the region ~3414–3094 cm−1, together with medium bands at 1609, 559, and 398 cm−1. The asymmetric -COO− stretching frequency (νasym) of the zwitterionic forms of amino acids occurs at 1580–1660 cm−1 when the group is coordinated to metals, where as a noncoordinated -COO− group has the νasym (COO−) stretching at lower frequency [17]. The band at 1609 cm−1 is therefore due to the νasym (COO−) of the metal bound carboxyl group. The presence of strong stretching band at ~3414 cm−1 indicates that the product contains aqua or hydroxyl ligands. The bands at 559 and 398 cm−1 are assigned to ν(Rh–N) and ν(Rh–O) bond formation, respectively [18]. An intense band of the ν(C=O)amide at 1693 cm−1 in the noncoordinated peptide undergoes a bathochromic shift of ~84 cm−1 in the IR spectrum upon complexation. This is probably due to the involvement of the peptide nitrogen (because of the deprotonation that has taken place) in bonding with Rh(III), which lowers the bond order of the ν(C=O)amide group due to resonance stabilization.The aqueous solution’s of [Rh(H2O)5(OH)]2+ and glycyl-L-alanine (L1-L′H) were mixed in a 2 : 1 molar ratio, and the mixture was thermostated at 60°C for 48 hours and used for ESI-MS measurement. The ESI mass spectra of the resulting solution are shown in Figure 3.Figure 3
ESI-mass spectrum of the substituted hydroxopentaaquarhodium(III) ion by glycyl-L-alanine.It is clear from this spectrum that the ion atm/z 246.18 (minor peak) has become the parent ion species in the mixture solution, and this is tentatively attributed to (glycyl-L-alanine + 2Rh3+ + 6H2O + 2HO−)2+. The parent ion is shown in Figure 4.Figure 4
Plausible structure of the parent ion from the ESI-mass spectrum.


## 3. Measurements

All the spectral scanning and kinetic measurements were done in a Shimadzu UV-VIS spectrophotometer (UV-2450 PC), with a thermoelectric cell temperature controller (model TCC-240A with an accuracy of ± 0.1°C). IR spectra (KBr disc, 4000–300 cm−1) were measured in Perkin-Elmer FTIR model RX1 infrared Spectrophotometer. ESI-mass spectra were recorded using a micromass Q-Tof micromass spectrometer in positive ion mode. The pHs of the solutions were adjusted with HClO4/NaOH and measured with a Sartorius pH meter (model PB11) with an accuracy of ± 0.01.The progress of the reaction was monitored by the absorbance measurements at different intervals of time with a Shimadzu spectrophotometer (UV-2450 PC) attached to a thermoelectric cell temperature controller (TCC-240A) at 224 nm. The conventional mixing technique was followed, and pseudo first order conditions were employed throughout.The plots ofln(A∞-At) (where At and A∞ are absorbance at time t and at infinite time or after the completion of the reaction) against time (Figure 5) were found to be nonlinear, curved at the initial stage and subsequently linear in nature indicating that the reactions proceed via two steps mechanism. From the limiting linear portion of the curve, the values of k2(obs) were obtained. The k1(obs) values were obtained from the slopes of lnΔ (the meaning of Δ is shown in Figure 5) versus time when t is small (Figure 6). The reported rate data represented as an average of duplicate runs were reproducible within ±4%.Figure 5
A typical plot ofln(A∞-At) versus time. [complex A] = 2.5 × 10−4 mol dm−3, [L1-L′H] = 7.5 × 10−3 mol dm−3, pH = 4.3, and temperature = 60°C; Δ=X-Y is difference in absorbances between two steps at different time interval.Figure 6
Plot oflnΔ versus time. [complex A] = 2.5 × 10−4 mol dm−3, [L1-L′H] = 7.5 × 10−3 mol dm−3, pH = 4.3, and temperature = 60°C.


## 4. Results and Discussion

From thepKa values [19] of the dipeptides, it is clear that, at pH 4.3, the major species involved in the kinetic processes are the zwitterionic forms of the dipeptides.On the other hand, the ionization of [Rh(H2O)6]3+ may be given as
(1)[Rh(H2O)6]3+⇌Kc(1)[Rh(H2O)5OH]2++H+,[Rh(H2O)5OH]2+⇌Kc(2)[Rh(H2O)4(OH)2]++H+.
The pKc(1) and pKc(2) values of [Rh(H2O)6]3+ are 3.6 and 4.7, respectively, at 25°C [20]. Other reports on the pKc(1) value are 3.2, 3.4, and 3.45 (references are given in [20]). With an increase in pH, the proportion of the more labile hydroxopentaaquarhodium(III) ion increases. The hydroxide ligand increases the water exchange rate of [Rh(H2O)5OH]2+ relative to [Rh(H2O)6]3+. In the studied pH range, dipeptides exist mainly as the dipolar ion. As the pH increases, the proportion of the more reactive anionic form increases, and since the ligating capability of the deprotonated ligand is always higher than its dipolar ion form, the rate increases with pH as expected. The pH range chosen in the present study is 3.0 to 4.3, where the active species involved in the reaction is L1-L′H. At pH higher than 4.5, precipitation of Rh3+ takes place.At constant temperature, pH (4.3), and fixed concentration of complex (A), the ln(A∞-At) versus time (t) plot for different ligand concentrations indicates a two-step process. Both are dependent on the incoming ligand concentration, and with increasing ligand concentration, a limiting rate is observed. Job’s method of complexation indicates a 2 : 1 metal-ligand ratio in the product complex. This is possible only when a bridged complex is formed. The rate constant for such a process can be evaluated assuming Scheme 1, where, L, the ligand reacts with both of the Rh centers [(1) and (2)] in a parallel fashion. In the starting complex, there are two equivalent rhodium(III) centers. Now, the ligand has two donor centers. As rhodium(III) is a borderline center, during the ligation, two donor centers attack in two parallel speeds (k1~10-3s-1 and k2~10-5s-1), which is shown in Section 5.Scheme 1


### 4.1. Calculation ofk1 Value for the A→B Step

The rate constant for the first phase of the reactionA→B was calculated from the absorbance data using the Weyh and Hamm [21] equation
(2)(A∞-At)=a1exp(-k1(obs)t)+a2exp(-k2(obs)t),
where a1 and a2 are constants that depend upon the rate constants and extinction coefficients.Values ofa2exp(-k2(obs)t) at different times (when t is small) were obtained from the linear portion of the curve (Figure 5) extended to t equals zero; that is,
(3)a2exp(-k2(obs)t)=(A∞-At)limiting.
Therefore, values of (A∞-At)-a2exp(-k2(obs)t) were calculated from X and Y values (Figure 5) at different t;
(4)Δ=a1exp(-k1(obs)t),
or
(5)lnΔ=constant-k1(obs)t.A similar procedure was applied for each ligand concentration in the2.50×10-3 mol dm−3 to 7.50×10-3 mol dm−3 range using the experimental conditions specified in Table 1. The k1(obs) values were collected in Table 1.Table 1
10
3
k
1
(
obs
) (s−1) values for different dipeptide concentrations at different temperatures; [Complex A] = 2.5 × 10−4 mol dm−3, pH = 4.3, ionic strength = 0.1 mol dm−3 NaClO4.
Ligand
Temperature (°C )
103 [Ligand] (mol dm−3)
2.50
3.75
5.00
6.25
7.50
L1-L′H
50
2.23
2.77
3.07
3.37
3.69
55
2.75
3.32
3.81
4.14
4.33
60
3.19
3.95
4.42
4.47
5.15
65
3.77
4.67
5.16
5.62
6.09
L2-L′H
50
0.52
0.69
0.81
0.92
1.01
55
0.72
0.93
1.10
1.23
1.35
60
0.98
1.28
1.47
1.64
1.82
65
1.27
1.59
1.85
2.08
2.27
L3-L′H
50
1.53
1.90
2.15
2.33
2.46
55
2.03
2.49
2.83
3.05
3.15
60
2.57
3.11
3.45
3.66
3.80
65
3.21
3.83
4.27
4.52
4.69The rate increases with an increase in[L1-L′H] and reaches a limiting value (Figure 7). The limiting rate is probably due to the completion of outer-sphere association complex formation. Since the metal ion reacts with its immediate environment, further change in [L1-L′H] beyond the saturation point will not affect the reaction rate. The outer-sphere association complex may be stabilized through H-bonding [25, 26].Figure 7
Plots ofk1(obs) (s−1) versus [L1-L′H] at different temperatures, A=50, B=55, C=60, and D=65°C.Based on the experimental findings, the following (6) and (7) may be proposed for the step A→B:
(6)A+(L-L′H)+A⇌KE,KE′A·(L-L′H)·A.
Outer-sphere association complex
(7)A·(L-L′H)·A⟶k1B(Rh(1)).
Based on the above scheme, a rate expression can be derived for the A→B  step
(8)d[B]dt=k1KE[Rh(H2O)5(OH)2+]T[dipeptide](1+KE[dipeptide]),
or
(9)d[B]dt=k1(obs)[[Rh(H2O)5(OH)]2+]T,
where T stands for total concentration of Rh(III). We can then write
(10)k1(obs)=k1KE[dipeptide]1+KE[dipeptide],
where k1 is the rate constant for the A→B step, that is, the rate constant for the interchange of outer-sphere complex to the inner-sphere complex; KE is the outer-sphere association equilibrium constant.The equation can be represented as(11)1k1(obs)=1k1+1k1KE[dipeptide].The plot of1/k1(obs) against 1/[dipeptide] should be linear with an intercept of 1/k1 and slope 1/k1KE. This was found to be the case at all temperatures studied. The k1 and KE values were calculated from the intercept and slope (Figure 8) and are collected in Table 3.Figure 8
Plot of1/k1(obs) (s) versus 1/[L1-L′H], A=50, B=55, C=60, and D=65°C.


### 4.2. Calculation ofk2 Value for Step A→B

The rate constants for this path were calculated from the latter linear portions of the graphs and are collected in Table2. This is again dependent on [dipeptide] and shows a limiting value at higher ligand concentrations. The intermediate here is also possibly stable through H-bonding between coordinated water and the approaching dipeptide. When two paths are parallel, then two rates are overlapping. When we are calculating the k1 (~10−3 s−1), the contribution from k2 (10−5 s−1) is negligible; and when we are calculating k2, the k1 path is already completed. Thus, there is no problem in calculating both the rate constants.Table 2
10
5
k
2
(
obs
) (s−1) values for different dipeptide concentrations at different temperatures; [Complex A] = 2.5 × 10−4 mol dm−3, pH = 4.3, ionic strength = 0.1 mol dm−3 NaClO4.
Ligand
Temperature (°C )
103 [Ligand] (mol dm−3)
2.50
3.75
5.00
6.25
7.50
L1-L′H
50
2.91
3.41
3.69
3.86
3.98
55
4.39
5.17
5.75
6.03
6.19
60
6.91
8.43
9.22
9.75
10.03
65
10.86
12.66
14.97
16.43
16.71
L2-L′H
50
2.71
3.08
3.34
3.50
3.57
55
4.22
4.93
5.38
5.71
5.99
60
6.37
7.69
8.55
9.09
9.26
65
9.98
12.50
13.51
14.29
16.10
L3-L′H
50
2.79
3.22
3.51
3.65
3.76
55
4.24
5.00
5.56
5.85
6.06
60
6.58
8.06
8.85
9.35
9.62
65
10.64
12.50
14.29
15.87
16.13Table 3
Thek1,k2,KE, and KE′ values for different dipeptide concentration at different temperatures;     [Complex A] = 2.5 × 10−4 mol dm−3, pH = 4.3, ionic strength = 0.1 mol dm−3 NaClO4.
Ligand
Temperature (°C)
103k1 (s−1)
K
E (dm3 mol−1)
105k2 (s−1)
K
E
′ (dm3 mol−1)
L1-L′H
50
5.25
295
4.92
330
55
6.15
309
7.94
433
60
7.26
315
13.38
498
65
8.51
319
23.93
580
L2-L′H
50
1.88
154
4.29
348
55
2.37
173
7.51
479
60
3.06
189
12.01
511
65
3.66
209
21.60
683
L3-L′H
50
3.55
304
4.60
359
55
4.50
331
7.82
428
60
5.08
413
12.85
475
65
6.21
429
22.31
616Thek2 and KE′ are calculated in a manner similar to (11), and data are collected in Table 3.Based on the experimental findings, a two-step interchange associative mechanism is proposed for the substitution processes for both the paths. In the first step, an outer-sphere association complex is formed between the ligand and the two rhodium(III) centers, which is stabilized by the H-bonding between the incoming dipeptide and the coordinated aqua molecules. Now the interchange of the ligand from the outer sphere to the inner sphere occurs.Both the paths of the final phase of substitution reaction are the chelation step to give the product complex (P) which is independent of dipeptide concentration.


### 4.3. Effect of pH on Reaction Rate

The reaction was studied at five different pH values (3.0, 3.3, 3.6, 4.0, and 4.3). Thek1(obs) and k2(obs) values increased with increase in pH at fixed concentration of (2.5×10-4 mol dm−3 of [complex A], 7.50×10-3 mol dm−3 [L1-L′H]) and 0.1 mol dm−3 ionic strength. The 103k1(obs) values at 60°C were 2.59, 3.17, 3.81, 4.46 and 5.15 s-1, and 105k2 values were 3.63, 5.14, 7.02, 8.17, and 10.03 s-1 at 3.0, 3.3, 3.6, 4.0, and 4.3, respectively. The enhancement in rate may be explained based on the acid dissociation equilibria of the reactants. A rate expression for path 1 may be given as follows:
(12)k(obs)=K1KEKc(1)Ka[dipeptide]t[H+]×([H+]3+[H+]2(Ka+Kc(1))+[H+]×(Kc(1)Ka+Kc(1)Kc(2)+Kc(1)KaKE[dipeptide]t)+Kc(1)Kc(2)Ka{[H+]3})-1,
where k1 and KE are rate constant and outer-sphere association equilibrium constant, and also Kc(1), Kc(2), and Ka are acid dissociation constants of [Rh(H2O)6]3+, [Rh(H2O)4(OH)]2+, and for the ligand –COOH, respectively. Further study of the substitution reaction was followed at pH 4.3 to avoid complications caused by adding an additional parameter [H+] to the rate equation. At pH 4.3, the complex exists mainly in the hydroxopentaaqua form, and the contribution due to the hexaaqua species is negligible. With increasing pH, the complex also changes its form from aqua to hydroxoaqua, and the hydroxide ligand increases the water exchange rate constant of [Rh(H2O)5(OH)]2+ relative to [Rh(H2O)6]3+. However, the dipeptide acts as a buffer during the reaction.


### 4.4. Effect of Temperature on the Reaction Rate

The reaction was studied at four different temperatures for different ligand concentrations, and the results are listed in Tables1 and 2. The activation parameters for both the paths were evaluated from the linear Eyring’s plots and were collected in Table 4. The low ΔH≠ values were in support of the ligand participation in the transition state for both the steps. The high negative ΔS≠ values suggest a more compact transition state, where both the incoming and departing ligands are attached in the transition state, and this is also in support of the assumption of a ligand participated transition state.Table 4
Comparison of activation parameters for the interaction of different ligands with the complex in aqueous medium at pH = 4.3.
Ligands
Δ
H
1
≠(kJ mol−1)
Δ
S
1
≠
(J K−1 mol−1)
Δ
H
2
≠(kJ mol−1)
Δ
S
2
≠ (J K−1 mol−1)
Reference
L-Arginine
56.9
±
3.8
-
105
±
12
89.1
±
2.9
-
54
±
9
[22]
L1-L′H
26.1
±
0.3
-
209
±
1
91.3
±
2.9
-
45
±
9
This work
L2-L′H
37.2
±
0.7
-
183
±
2
94.7
±
3.1
-
36
±
9
This work
L3-L′H
29.4
±
2.8
-
201
±
8
93.1
±
1.6
-
40
±
5
This work
Glycyl-glycine
26.7
±
0.3
-
207
±
1
92.4
±
1.3
-
42
±
4
[23]
Glycyl-L-glutamine
34.7
±
1.3
-
189
±
4
94.1
±
1.1
-
37
±
3
[24]
Glycyl-L-valine
22.0
±
1.2
-
220
±
4
90.7
±
3.2
-
47
±
10
[24]


## 4.1. Calculation ofk1 Value for the A→B Step

The rate constant for the first phase of the reactionA→B was calculated from the absorbance data using the Weyh and Hamm [21] equation
(2)(A∞-At)=a1exp(-k1(obs)t)+a2exp(-k2(obs)t),
where a1 and a2 are constants that depend upon the rate constants and extinction coefficients.Values ofa2exp(-k2(obs)t) at different times (when t is small) were obtained from the linear portion of the curve (Figure 5) extended to t equals zero; that is,
(3)a2exp(-k2(obs)t)=(A∞-At)limiting.
Therefore, values of (A∞-At)-a2exp(-k2(obs)t) were calculated from X and Y values (Figure 5) at different t;
(4)Δ=a1exp(-k1(obs)t),
or
(5)lnΔ=constant-k1(obs)t.A similar procedure was applied for each ligand concentration in the2.50×10-3 mol dm−3 to 7.50×10-3 mol dm−3 range using the experimental conditions specified in Table 1. The k1(obs) values were collected in Table 1.Table 1
10
3
k
1
(
obs
) (s−1) values for different dipeptide concentrations at different temperatures; [Complex A] = 2.5 × 10−4 mol dm−3, pH = 4.3, ionic strength = 0.1 mol dm−3 NaClO4.
Ligand
Temperature (°C )
103 [Ligand] (mol dm−3)
2.50
3.75
5.00
6.25
7.50
L1-L′H
50
2.23
2.77
3.07
3.37
3.69
55
2.75
3.32
3.81
4.14
4.33
60
3.19
3.95
4.42
4.47
5.15
65
3.77
4.67
5.16
5.62
6.09
L2-L′H
50
0.52
0.69
0.81
0.92
1.01
55
0.72
0.93
1.10
1.23
1.35
60
0.98
1.28
1.47
1.64
1.82
65
1.27
1.59
1.85
2.08
2.27
L3-L′H
50
1.53
1.90
2.15
2.33
2.46
55
2.03
2.49
2.83
3.05
3.15
60
2.57
3.11
3.45
3.66
3.80
65
3.21
3.83
4.27
4.52
4.69The rate increases with an increase in[L1-L′H] and reaches a limiting value (Figure 7). The limiting rate is probably due to the completion of outer-sphere association complex formation. Since the metal ion reacts with its immediate environment, further change in [L1-L′H] beyond the saturation point will not affect the reaction rate. The outer-sphere association complex may be stabilized through H-bonding [25, 26].Figure 7
Plots ofk1(obs) (s−1) versus [L1-L′H] at different temperatures, A=50, B=55, C=60, and D=65°C.Based on the experimental findings, the following (6) and (7) may be proposed for the step A→B:
(6)A+(L-L′H)+A⇌KE,KE′A·(L-L′H)·A.
Outer-sphere association complex
(7)A·(L-L′H)·A⟶k1B(Rh(1)).
Based on the above scheme, a rate expression can be derived for the A→B  step
(8)d[B]dt=k1KE[Rh(H2O)5(OH)2+]T[dipeptide](1+KE[dipeptide]),
or
(9)d[B]dt=k1(obs)[[Rh(H2O)5(OH)]2+]T,
where T stands for total concentration of Rh(III). We can then write
(10)k1(obs)=k1KE[dipeptide]1+KE[dipeptide],
where k1 is the rate constant for the A→B step, that is, the rate constant for the interchange of outer-sphere complex to the inner-sphere complex; KE is the outer-sphere association equilibrium constant.The equation can be represented as(11)1k1(obs)=1k1+1k1KE[dipeptide].The plot of1/k1(obs) against 1/[dipeptide] should be linear with an intercept of 1/k1 and slope 1/k1KE. This was found to be the case at all temperatures studied. The k1 and KE values were calculated from the intercept and slope (Figure 8) and are collected in Table 3.Figure 8
Plot of1/k1(obs) (s) versus 1/[L1-L′H], A=50, B=55, C=60, and D=65°C.


## 4.2. Calculation ofk2 Value for Step A→B

The rate constants for this path were calculated from the latter linear portions of the graphs and are collected in Table2. This is again dependent on [dipeptide] and shows a limiting value at higher ligand concentrations. The intermediate here is also possibly stable through H-bonding between coordinated water and the approaching dipeptide. When two paths are parallel, then two rates are overlapping. When we are calculating the k1 (~10−3 s−1), the contribution from k2 (10−5 s−1) is negligible; and when we are calculating k2, the k1 path is already completed. Thus, there is no problem in calculating both the rate constants.Table 2
10
5
k
2
(
obs
) (s−1) values for different dipeptide concentrations at different temperatures; [Complex A] = 2.5 × 10−4 mol dm−3, pH = 4.3, ionic strength = 0.1 mol dm−3 NaClO4.
Ligand
Temperature (°C )
103 [Ligand] (mol dm−3)
2.50
3.75
5.00
6.25
7.50
L1-L′H
50
2.91
3.41
3.69
3.86
3.98
55
4.39
5.17
5.75
6.03
6.19
60
6.91
8.43
9.22
9.75
10.03
65
10.86
12.66
14.97
16.43
16.71
L2-L′H
50
2.71
3.08
3.34
3.50
3.57
55
4.22
4.93
5.38
5.71
5.99
60
6.37
7.69
8.55
9.09
9.26
65
9.98
12.50
13.51
14.29
16.10
L3-L′H
50
2.79
3.22
3.51
3.65
3.76
55
4.24
5.00
5.56
5.85
6.06
60
6.58
8.06
8.85
9.35
9.62
65
10.64
12.50
14.29
15.87
16.13Table 3
Thek1,k2,KE, and KE′ values for different dipeptide concentration at different temperatures;     [Complex A] = 2.5 × 10−4 mol dm−3, pH = 4.3, ionic strength = 0.1 mol dm−3 NaClO4.
Ligand
Temperature (°C)
103k1 (s−1)
K
E (dm3 mol−1)
105k2 (s−1)
K
E
′ (dm3 mol−1)
L1-L′H
50
5.25
295
4.92
330
55
6.15
309
7.94
433
60
7.26
315
13.38
498
65
8.51
319
23.93
580
L2-L′H
50
1.88
154
4.29
348
55
2.37
173
7.51
479
60
3.06
189
12.01
511
65
3.66
209
21.60
683
L3-L′H
50
3.55
304
4.60
359
55
4.50
331
7.82
428
60
5.08
413
12.85
475
65
6.21
429
22.31
616Thek2 and KE′ are calculated in a manner similar to (11), and data are collected in Table 3.Based on the experimental findings, a two-step interchange associative mechanism is proposed for the substitution processes for both the paths. In the first step, an outer-sphere association complex is formed between the ligand and the two rhodium(III) centers, which is stabilized by the H-bonding between the incoming dipeptide and the coordinated aqua molecules. Now the interchange of the ligand from the outer sphere to the inner sphere occurs.Both the paths of the final phase of substitution reaction are the chelation step to give the product complex (P) which is independent of dipeptide concentration.


## 4.3. Effect of pH on Reaction Rate

The reaction was studied at five different pH values (3.0, 3.3, 3.6, 4.0, and 4.3). Thek1(obs) and k2(obs) values increased with increase in pH at fixed concentration of (2.5×10-4 mol dm−3 of [complex A], 7.50×10-3 mol dm−3 [L1-L′H]) and 0.1 mol dm−3 ionic strength. The 103k1(obs) values at 60°C were 2.59, 3.17, 3.81, 4.46 and 5.15 s-1, and 105k2 values were 3.63, 5.14, 7.02, 8.17, and 10.03 s-1 at 3.0, 3.3, 3.6, 4.0, and 4.3, respectively. The enhancement in rate may be explained based on the acid dissociation equilibria of the reactants. A rate expression for path 1 may be given as follows:
(12)k(obs)=K1KEKc(1)Ka[dipeptide]t[H+]×([H+]3+[H+]2(Ka+Kc(1))+[H+]×(Kc(1)Ka+Kc(1)Kc(2)+Kc(1)KaKE[dipeptide]t)+Kc(1)Kc(2)Ka{[H+]3})-1,
where k1 and KE are rate constant and outer-sphere association equilibrium constant, and also Kc(1), Kc(2), and Ka are acid dissociation constants of [Rh(H2O)6]3+, [Rh(H2O)4(OH)]2+, and for the ligand –COOH, respectively. Further study of the substitution reaction was followed at pH 4.3 to avoid complications caused by adding an additional parameter [H+] to the rate equation. At pH 4.3, the complex exists mainly in the hydroxopentaaqua form, and the contribution due to the hexaaqua species is negligible. With increasing pH, the complex also changes its form from aqua to hydroxoaqua, and the hydroxide ligand increases the water exchange rate constant of [Rh(H2O)5(OH)]2+ relative to [Rh(H2O)6]3+. However, the dipeptide acts as a buffer during the reaction.


## 4.4. Effect of Temperature on the Reaction Rate

The reaction was studied at four different temperatures for different ligand concentrations, and the results are listed in Tables1 and 2. The activation parameters for both the paths were evaluated from the linear Eyring’s plots and were collected in Table 4. The low ΔH≠ values were in support of the ligand participation in the transition state for both the steps. The high negative ΔS≠ values suggest a more compact transition state, where both the incoming and departing ligands are attached in the transition state, and this is also in support of the assumption of a ligand participated transition state.Table 4
Comparison of activation parameters for the interaction of different ligands with the complex in aqueous medium at pH = 4.3.
Ligands
Δ
H
1
≠(kJ mol−1)
Δ
S
1
≠
(J K−1 mol−1)
Δ
H
2
≠(kJ mol−1)
Δ
S
2
≠ (J K−1 mol−1)
Reference
L-Arginine
56.9
±
3.8
-
105
±
12
89.1
±
2.9
-
54
±
9
[22]
L1-L′H
26.1
±
0.3
-
209
±
1
91.3
±
2.9
-
45
±
9
This work
L2-L′H
37.2
±
0.7
-
183
±
2
94.7
±
3.1
-
36
±
9
This work
L3-L′H
29.4
±
2.8
-
201
±
8
93.1
±
1.6
-
40
±
5
This work
Glycyl-glycine
26.7
±
0.3
-
207
±
1
92.4
±
1.3
-
42
±
4
[23]
Glycyl-L-glutamine
34.7
±
1.3
-
189
±
4
94.1
±
1.1
-
37
±
3
[24]
Glycyl-L-valine
22.0
±
1.2
-
220
±
4
90.7
±
3.2
-
47
±
10
[24]


## 5. Mechanism and Conclusion

Each dipeptide has one carboxyl group and one amino group at the opposite ends of the molecule. Because of neutrality of the amide group, the two terminal groups are the most effective bonding sites for metal coordination, but steric requirements preclude the simultaneous coordination of three groups to the same metal ion. Also tetra coordination complex formation may be possible when two metal ions are participated.The complex of dipeptides such as glycyl-glycine with various metal ions has been studied. The metal ions, which are able to promote amide deprotonation, are the most interesting in this field. A literature survey [27] shows that Pd(II), Cu(II), and Ni(II) are most effective in this respect. There are reports of Fe(II) and Fe(III) induced deprotonation of the amide groups [28, 29].Dipeptide may coordinate to Rh(III) ion in four way:(1)
monodentate coordination through carboxylate-O to give 1 : 1 and 1 : 2 products;(2)
bidentate coordination involving amino-N and carbonyl-O is expected to occur at low pH where amide deprotonation is difficult [30];(3)
tridentate coordination involving terminal carboxylate-O, amide-N, and amino-N groups gives rise to two fused five-membered rings. This has been observed with Cu(II), Pd(II), and Ni(II) complexes [27] in slightly alkaline medium;(4)
tetradentate coordination involving amino-N, carbonyl-O, peptide-N, and carboxylate-O gives a 2 : 1 (metal : ligand) five-membered chelated product of high stability [31]. This type of chelation occurs [32] at and above pH 4.As the substrate is a hydroxopentaaqua complex at experimental pH 4.3 and Job’s method also confirms the formation of a 2 : 1 product, so the first three possibilities are ruled out. At first, the dipeptide binds to the rhodium center through carboxylate-O− and peptide-O which shows high affinity for Rh(III), a borderline acid. The carboxylate-O− has more electron density, and so it reacts at a faster rate than the other.The interaction of dipeptide with the title rhodium complex proceeds via two distinct parallel substitution steps of aqua molecules (k1~10-3s-1 and k2~10-5s-1). Each step proceeds via an associative interchange activation. At the outset of each step outer-sphere association complex results, which is stabilized through H-bonding and is followed by an interchange from the outer-sphere to the inner-sphere complex. The outer-sphere association equilibrium constants, a measure of the extent of H-bonding for each step at different temperatures, are evaluated (Table 3). The activation parameters for both the steps suggest an associative mode of activation for the substitution process. The ΔH1≠ and ΔH2≠ values and negative ΔS1≠ and ΔS2≠ values imply a good degree of ligand participation in the transition state.But for amino acids, the mechanism of substitution of aqua ligands in ion [Rh(H2O)5(OH)]2+ can be explained in terms of rapid outer-sphere association complex formation, followed by two consecutive steps; the first is dependent on ligand concentration, and second is the chelation, that is, ring closure step, which is independent of ligand concentration.From a comparison of the dipeptides used, it can be concluded that the variation in size and bulkiness of the entering dipeptides reflects their properties as nucleophiles. The differences in reactivity of the selected dipeptides is obvious, and their reactivity follows the orderL2-L′H < Gly-glut. < L3-L′H < Gly-gly. < L1-L′H < Gly-val. The sensitivity of the reaction rate towards the donor properties of the entering ligands is in line with that expected for an associative mode of activation. In addition, donor effects (present in different R group of dipeptide) were more important than steric effect due to the presence of water molecules in the hydroxopentaaquarhodium complex. Also the entering dipeptide was stabilized by hydrogen bonding with water molecules of hydroxopentaaquarhodium complex. For the three dipeptides with increasing donor effects, reactivity increases which is reflected in their rate constant values. Also, from ESI-MS measurement, a chelated product in the final step is proposed.Based on the previous facts, a plausible mechanism for the substitution has been proposed as shown in Figure9.Figure 9
Proposed mechanism for the interaction of dipeptide with the complexA.



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*Source: 801362-2013-09-11.xml*