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Interaction of Proline with Cu<sup>+</sup> and Cu<sup>2+</sup> Ions in the Gas PhaseGab Yong Lee*Department of Life Chemistry, Catholic University of Daegu, Gyeongsan 712‐702, Korea(Received March 3, 2009)INTRODUCTIONCopper ions are the most important transitionmetals involved in several biological processes ofliving systems, including oxidation, dioxygentransport, and charge transfer.1 The study of interactionsbetween the metal ion and amino acids hasattracted considerable attention from experimental2-6and theoretical6-11 viewpoints. Thermochemicalinformation on interactions between the metal ion and biological
Interaction of Proline with Cu+ and Cu2+ Ions in the Gas PhaseGab Yong Lee*Department of Life Chemistry, Catholic University of Daegu, Gyeongsan 712‐702, Korea(Received March 3, 2009)INTRODUCTIONCopper ions are the most important transitionmetals involved in several biological processes ofliving systems, including oxidation, dioxygentransport, and charge transfer.1 The study of interactionsbetween the metal ion and amino acids hasattracted considerable attention from experimental2-6and theoretical6-11 viewpoints. Thermochemicalinformation on interactions between the metal ion and biological
Journal of the Korean Chemical Society. 2009. Jun, 53(3): 257-265
Copyright © 2009, The Korean Chemical Society
  • Received : March 03, 2009
  • Published : June 20, 2009
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Gab-Yong Lee

Abstract
The structures and metal affinities of the binding configurations of Cu + and Cu 2+ to proline have been investigated using the hybrid three-parameter Density Functional Theory(DFT/B3LYP). We found that the metal-proline bonding and the energy ordering of several conformers were very different in Cu + -proline and Cu 2+ -proline. For Cu + -proline, the ground state structure was found to have a bidentated coordination in which Cu + was coordinated to the carbonyl oxygen and imino group nitrogen of neutral proline. On the contrary, the ground state structure of Cu 2+ -proline involves chelation between the two oxygens of the carboxylate group in a zwitterionic proline. The metal ion affinity of proline of the most stable Cu + -proline complex was calculated as 76.0 kcal/mol at 6-311++G(d,p) level, whereas the Cu 2+ ion affinity of proline was calculated as 258.5 kcal/mol.
Keywords
INTRODUCTION
Copper ions are the most important transition metals involved in several biological processes of living systems, including oxidation, dioxygen transport, and charge transfer. 1 The study of nteractions between the metal ion and amino acids has attracted considerable attention from experimental 2 - 6 and theoretical 6 - 11 viewpoints. Thermochemical information on interactions between the metal ion and biological molecules is essential as it can help us understand the role of the metal in several essential biochemical processes. The thermochemical properties can be obtained in the gaseous state where solvent effects are absent.
Proline is a constituent of collagen and plays an important role in enzymes and peptide hormone. 12 Proline has an imino group within the pyrrolidine ring, therefore making conformation more rigid than for other amino acids.
The binding energies for Cu + complexes with 20 commonly found α-amino acids in natural peptides have been determined in the gas phase. 13 Hoyau and Ohanessian have studied Cu + ion affinities for glycine, serine, and cystein by using an extensive theoretical method. 14 The results showed that the most favorable structure for Cu + -glycine involves metal chelation between the carbonyl oxygen and amino nitrogen of glycine. The effects of metal ions(Li + , Na + , K + , Mg 2+ , Ca 2+ , Ni 2+ , Cu 2+ , and Zn 2+ ) on the structures and ion affinities of arginine-metal complexes have been studied by Remko et al . 15 The results confirmed that the strongest affinity to arginine is exhibited by the Cu 2+ cation.
On the other hand, the interaction of proline with Cu + has been investigated using ab initio methods by Hoyau and Ohanessian. 16 Marino et al . 17 have observed the Cu + and Cu 2+ preferred binding sites on α-alanine and their affinity values for this amino acid by density functional theory calculations. The results showed that the two ions both demonstrate stable complexes with α-alanine but stability order of the metalated complexes and the binding sites are different depending on the nature of the cation. Bertrán et al . 18 have reported the results of a study of the ifferent nature in bonding of glycine with Cu + and Cu 2+ ions by theoretical calculations.
In spite of various theoretical studies of amino acid complexes of copper ions, no effort has been reported to estimate the different nature of bonding in Cu + and Cu 2+ with proline.
Cu + possesses a closed-shell system with a d 10 ground state, while Cu 2+ possesses an open-shell system with a d 9 ground state. Therefore, these two copper ions are associated with very different chemistries. In this paper, we report the differences between Cu + and Cu 2+ with regard to their proline complexes.
COMPUTATIONAL METHODS
The Density Functional Theory(DFT) calculations were performed at the B3LYP level 19 , 20 with a 6-311++G(d,p) internal basis set for all atoms using the Gaussian 03 program. 21 It is shown that the density functional method provides accurate results for many transition metal-containing systems. 22 - 24 Unrestricted open shell methods were used to calculate the Cu 2+ system
The equilibrium geometries for all the structures were fully optimized without any symmetry restrictions. Harmonic frequencies were also calculated to confirm that all the stationary points orresponded to true minima on the potential energy surface. The stationary structures were obtained by verifying that all of the harmonic frequencies are real. The natural atomic charges were calculated in order to analyze the nature of the bonding for complexes of copper with proline.
Copper ion affinities were calculated as the negative value of the enthalpy change(ΔH) associated with the following reaction:
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RESULTS AND DISCUSSION
The conformational behavior of amino acids is essential to understand their dynamic role in protein formation. 25 Therefore, extensive structural studies have been performed on amino acids in their natural solid state. However, amino acids have a zwitterionic structure in their solid state. Consequently, to obtain the neutral structure of amino acids, studies should be performed in the gas phase. Proline is the only natural amino acid that contains a secondary amino group as part of a flexible five-membered ring.
number of experimental studies on the structure of the proline have been conducted in the condensed phase; 26 - 28 these studies include an x-ray diffraction analysis of the zwitterionic ring conformation, because of the high melting point of proline and associated low-vapor pressure. To date, no experimental structure of neutral proline has been reported. Ramek et al . 29 located 10 distinct conformers of proline at the 6-311++G ** RHF level, and Stepanian et al . 30 determined 15 stable minima on the PES of proline using DFT. Czinki and Csazar 31 reported that proline has 18 possible stable conformers at high levels of ab initio electronic-structure theory. . 1 shows the numbering of the 8 conformers of neutral proline, which reflects the relative energies of the distinct conformers obtained at DFT optimized geometries in this study.
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Optimized structures at the B3LYP/6-311++G(d,p) level of eight neutral prolines numbered according to their relative energy order. Hydrogen bond lengths are in Å.
As shown in . 1 , the optimized geometries of proline are classified according to the type of intramolecular hydrogen bond(N...H–O, N–H... O=C, and N–H...O–H) and the nature of the bent configuration of the pyrrolidine ring(pucker-up and pucker-down).
Conformer 1 was found to be at the global minimum. The next stable structure is conformer 2. However, the energy difference between the global and first local minimum(2) is only 0.5 kcal/mol. Further, the only difference between conformers 1 and 2 is the pucker position of the pyrrolidine ring. These two conformers are stabilized relative to conformers 3 and 4 because the N...H–O hydrogen bonds are more favorable to the secondary amine in proline (1.88 or 1.90Å in conformers 1 and 2 versus 2.4 or 2.2 Å in conformers 3 and 4). This leads to conformers 1 and 2 being more stable than conformers 3 and 4. In contrast to simpler amino acids such as glycine and alanine, only a few low-energy conformers exist on the PES of neutral proline. Conformer pairs 1/2 and 3/4 are the only ones that have relative energies of less than 2 kcal/mol relative to the global minimum conformer 1. For the zwitterionic form, we have considered only the complexes formed by proline with the copper ion.
The optimized structures for eight low-energy conformers of Cu + -proline and Cu 2+ -proline are shown in . 2 and 3 , respectively; In addition, calculated energies, including the natural atomic charges of metal, are listed in 1 .
1 shows that the most favorable structure of Cu + -proline corresponds to the Cu + ion interacting with the imino nitrogen atom on the pyrrolidine ring with a pucker-down position and with the carbonyl oxygen on the carboxylate group, as observed in structure 3. In this conformer, the Cu + –O and Cu + –N bond lengths are 2.090 and 2.043Å, respectively. A similar result was found for the copper-glycine complex 14 , 18 and for the copper–α-alanine complex. 17 The second most favorable structure, complex 4, possesses 0.9 kcal/mol more energy and has the same type of chemical coordination, although it has the pucker-up form of a pyrrolidine ring. For the zwitterionic conformers (structure 1 and 2), . 2 shows that the Cu + -O distances are quite different(1.90 and 2.91Å); thus, it can be deduced that proline acts as a monodentate ligand. This unsymmetrical coordination may be due to the hydrogen bond between the oxygen and the amino hydrogen. However, in the Cu 2+ -proline complexes, the Cu 2+ -O distances between the metal cation and the two oxygens are very similar(1.96 and 1.99 Å). This trend is also shown in analogous M + -COO– coordination with alkali metal cations. 7 Thus, we attribute the difference between Cu + and Cu 2+ cations to the fact that Cu + tends to undergo an unsymmetrical interaction to minimize the repulsion between the occupied d orbitals of metal and the lone pairs of oxygens.
On the other hand, the most favorable structure of the Cu 2+ -proline has a zwitterionic bonding arrangement, wherein binding occurs between the two carboxylate oxygens and the cation. To further investigate the nature of bonding, the natural population analyses were performed by the natural bond orbital(NBO) method. NBO calculations were carried out for the optimized structures of copper-proline complexes. The calculated natural atomic charges are shown in 1 . As shown in 1 , the natural charge on the Cu + ion is reduced by about 0.13|e|, whereas the charge on the Cu 2+ is reduced by about 0.68|e|. This means that in the Cu 2+ -proline complex, the ligand transfers a large amount of electrons to the cation. This result suggests that in comparison with the binding of Cu + to proline, that of Cu 2+ to proline involves a higher contribution of charge transfer rather than electrostatic effects.
Relative energies of Cu+-proline and Cu2+-proline complexes(in kcal/mol) and natural atomic charges of the metal cation at B3LYP/6-311++G(d,p) level
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Relative energies of Cu+-proline and Cu2+-proline complexes(in kcal/mol) and natural atomic charges of the metal cation at B3LYP/6-311++G(d,p) level
. 2
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Optimized structures at B3LYP/6-311++G(d,p) level of theory of Cu+-proline complexes. Distances are in Å.
. 3
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Optimized structures at B3LYP/6-311++G(d,p) level of theory of Cu2+-proline complexes. Distances are in Å.
For the zwitterionic isomers, namely, structures 1 and 2, the distances between the cation Cu 2+ and the two oxygens are more similar than those obtained for Cu + -proline. This difference is due to the smaller metal-ligand repulsion in the Cu 2+ -proline system, which favors the symmetrical position of the metal cation. Moreover, the intramolecular hydrogen bond, present in Cu + -proline; that is, the O---H–N distance increases significantly. It is also noteworthy that, in the bicoordinated conformers 3 ~ 8, Cu 2+ –O and Cu 2+ –N distances were found to be shorter than the corresponding Cu + –O and Cu + –N distances. As mentioned above, this result is due to the repulsion effect between the filled d orbitals of Cu + and the lone pairs of the ligand heteroatoms. 17
1 shows that the energy ordering of the different conformers obtained for the Cu 2+ -proline is very different from the ordering for Cu + -proline. For the Cu + -proline system, the order is structures 3 < 4 < 2 < 1 < 5 < 6 < 7 < 8, whereas for Cu 2+ -proline, the order is structures 1 < 2 < 3 < 4 < 5 < 6 < 7 < 8. Thus, the ground state structure of Cu 2+ -proline corresponds to that of conformer of zwitterionic structure 1 and not to that of structure 3 as found for Cu + -proline. This observation is in good agreement with the experimental results that show that Cu 2+ has some affinity to the C-terminal carboxylate group. 32 , 33 In other words, the most stable conformer comprises the Cu 2+ ion interacting with zwitterionic proline through the carboxylate group in a bidentate manner, unlike the case of the Cu + ion. A similar result is obtained for group 1 metal ions(Li + , Na + and K + ) binding with proline. 34
The metal ion affinities(MIAs) were computed for the eight investigated binding arrangements of Cu + and Cu 2+ , as listed in 2 . The MIAs were computed as the enthalpy difference between the corresponding complex and the sum of Cu 2+ and the most stable conformer of the free proline. As shown in 2 , there is a significant difference between the MIA values of Cu + and Cu 2+ . The MIA values of the Cu 2+ ion are much larger than those of Cu + . This large difference may be due to the Cu 2+ ion possessing a greater charge than the Cu + ion. No experimental value for Cu 2+ ions is available in the literature for comparison with the value calculated in this paper. Cerda and Wesdemiotis 13 have reported experimental results on the affinity of copper(I) to various amino acids. However, no absolute values were reported. With regard to the theoretical studies performed thus far, Fleming et al . 35 have reported absolute MIAs for alkali earth metal ions(Be 2+ , Mg 2+ , Ca 2+ ) bound to proline. With the DFT(B3LYP/6-311++G ** ) method, these affinities were determined as follows: Be 2+ = 301.52 kcal/mol, Mg 2+ =184.29 kcal/mol, and Ca 2+ =139.95 kcal/mol. As shown in 2 , the MIAs of the Cu 2+ ion are larger than those of Mg 2+ and Ca 2+ , and are smaller than those of Be 2+ . The MIA of the most stable Cu + -proline conformer is calculated as 76.0 kcal/mol. This MIA value is larger than the values for alkali metal ions(Li + = 64.21 kcal/mol, Na + = 47.32 kcal/mol and K + = 34.62 kcal/mol) 34 bound to proline.
On the other hand, the MIAs calculated in this study for the most stable Cu + -proline and Cu 2+ -proline are larger than the corresponding values for the copper-glycine complexes 18 (Cu + =68.1 kcal/mol and Cu 2+ =214.8 kcal/mol at CCSD(T) level) and for the copper–α-alanine complexes 17 (Cu + =68.2 kcal/mol and Cu 2+ =220.7 kcal/mol at BHandHLYP level). No experimental data have been reported absolute values of the copper ion affinity to amino acids. The only experimental study 13 shows that the relative Cu + affinity of proline is larger than that of the glycine by 4.8 kcal/mol, and is larger than that of the α-alanine by 3.1 kcal/mol. The result in this study is in good agreement with this experimental trend.
Metal ion affinities of Cu+-proline and Cu2+-proline at B3LYP/6-311++G(d,p) level(in kcal/mol)
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Metal ion affinities of Cu+-proline and Cu2+-proline at B3LYP/6-311++G(d,p) level(in kcal/mol)
CONCLUSION
A study of the metal-proline bonding for several modes of coordination of Cu + and Cu 2+ with proline is reported. The Cu + ion has a tendency to bind to proline in a electrostatic interaction arrangement through the carbonyl oxygen and imino nitrogen atom. In contrast, Cu 2+ tends to bind to proline by means of a charge-transfer mechanism through the two carboxylate oxygens of proline in a zwitterionic form. For the Cu 2+ -proline, the obtained energy ordering of the different conformers is very different from that determined for the single positive Cu + -proline system. The ground state structure of Cu 2+ -proline is zwitterionic in nature, as observed from the interaction of the metal cation with the COO group of the zwitterionic proline. Thus, the proline favors the interaction of the Cu 2+ cation with the carboxylate group as compared to other coordination modes. The calulated MIA shows that the Cu + ion affinity is larger than the alkali metal ion affinity bound to proline and the affinity of Cu 2+ ion is larger than that of Mg 2+ and Ca 2+ , but smaller than that of Be 2+ . The Cu + ion affinity of proline is larger than that of the glycine and α-alanine.
This work was conducted during a sabbatical year at the Catholic University of Daegu.
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