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. 2022 Sep 3;12:15038. doi: 10.1038/s41598-022-18922-1

Preparation and DFT studies of chiral Cu (I)-complexes of biphenyl bisoxazolines and their application in enantioselective Kharasch–Sosnovsky reaction

Saadi Samadi 1,✉, Hamid Arvinnezhad 1, Sirwan Mansoori 1, Hadi Parsa 1
PMCID: PMC9440904  PMID: 36057728

Abstract

Effect of a range of t-butyl perbenzoates bearing electron-withdrawing and electron-donating substitutions on the phenyl ring and HZSM-5 as a porous additive at 0 °C in enantioselective allylic C–H bond oxidation of cyclic and acyclic olefins in the presence of Cu (I)-(S,aS,S) complexes of biphenyl bisoxazoline ligands, produced easily through the chelation-induced process, were investigated. The enantioenriched allylic esters were obtained in reasonable times with excellent enantioselectivities and yields using electron-withdrawing substituted peresters in the presence of Cu (I)-(S,aS,S)-1a complex, containing phenyl groups at the stereogenic centers of the oxazoline moieties. To reach a better insight on geometry, chemical activity, enantioselectivity, and thermodynamic stability of the Cu (I)-BOX complexes, DFT calculations with B3LYP-D3/6-31G (d, p) level of theory were applied to them. Moreover, NBO analysis was used to illustrate interactions between orbitals.

Subject terms: Asymmetric catalysis, Homogeneous catalysis, Organic chemistry, Stereochemistry, Asymmetric synthesis

Introduction

Over the last two decades, chiral bisoxazoline (BOX) ligands, mainly prepared from the reaction of various dicarboxylic acids and a range of chiral β-amino alcohols, have great attracted increasing attention as promising ligands in numerous catalytic asymmetric transformations1–11. It has been shown that an effective arrangement for high asymmetric induction can be achieved owing to the existence of stereogenic centers adjacent to the active catalytic site. Furthermore, both great diversity in amino alcohols and diacid structures lead to a wide range of BOX ligands with unique features. On the other hand, literature surveys have implied that the introduction of an additional chiral element in the ligand backbone is capable of effectively controlling asymmetric induction12–17. It has demonstrated that the combination of a biaryl backbone and chiral oxazoline rings at ortho-position leads to a mixture of atropisomeric diastereomers of BOX ligands bearing a chiral axis close to the stereogenic centers of the oxazoline moieties18–25. However, separation of the diastereomers is always a tedious and time-consuming process, and also the maximum theoretical yield of the resulting atropisomers is only 50%. These drawbacks can be ingeniously overcome by using a biphenyl backbone containing only two ortho oxazoline moieties. Such a BOX ligand scaffold exists as an equilibrium mixture of two axis-unfixed atropisomers that are able to readily rotate around C–C bond between Ph–Ph, and one of them tend to be selectively coordinated to a metal ion such as Cu (I), Ag (I), Pd (II), and Zn (II) through chelation-induced process12–15,26. It is obvious that during such a dynamic kinetic resolution process, the more stable BOX complex can be obtained in a theoretical yield of 100% due to rotation around the biphenyl axis. According to our earlier study15 and also Ikeda group12,14, it was found that the selective complexation of an equilibrium mixture of biphenyl bisoxazoline 1 with Cu (I) results in the Cu (I)-(S,aS,S) complex as almost the only complex that can catalyze allylic oxidation and cyclopropanation with high enantioselectivity (Scheme 1).

Scheme 1.

Scheme 1

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Resolution of (S,aS,S)-bipheny bisoxazoline complex through chelation-induced process.

Enantioselective copper-catalyzed allylic C-H bond oxidation of olefins with peresters (Kharasch–Sosnovsky reaction) has been known as a powerful strategy to prepare chiral allylic esters by introducing a new stereogenic center containing oxygen substituent close to an intact C=C27–49. Previous studies have shown that this asymmetric transformation is considerably improved by inorganic porous additives15,18,50. Therefore, based on the above-mentioned and in continuation of our research group studies to tune the best condition15,18,49–52, enantioselective allylic C–H bond oxidation of alkenes was evaluated with different substituted t-butyl perbenzoates as an oxidant in the presence of inorganic porous additives, using the copper complexes of biphenyl BOX ligands 1 bearing phenyl and isopropyl groups at the stereogenic centers of the oxazoline moiety. Furthermore, to evaluation the thermodynamic stability and catalyst activity of the chiral biphenyl BOX Cu-complexes, density functional theory (DFT) calculations were performed.

Result and discussion

Chiral atropisomeric BOX ligands 1a and 1b were prepared according to our previous study15. In this procedure, at first, inexpensive starting material anthranilic acid 2 was converted to biphenyl dicarboxylic acid backbone 3 using Cu (I) through homo-coupling of aryldiazonium salts53. Treatment of the obtained dicarboxylic acid 3 with oxalyl chloride using a catalytic amount of DMF resulted in diacyl chloride that was then reacted with two individual (S)-amino alcohol 5a and 5b, prepared from the reduction of the corresponding chiral amino acids 4a and 4b54, to form (S,aS,S) and (S,aR,S)-bishydroxylamides 6a and 6b. As expected, the S,aS,S isomer15, the more stable one, is mainly formed during the crystallization of the equilibrium mixture. It seems that this process, which is known as crystallization induced asymmetric transformation55, is mainly directed by hydrogen bonding. Cyclization of the bishydroxylamides 6a and 6b using p-TsCl, DMAP, and Et3N at ambient temperature resulted in an equilibrium mixture of the (S,aS,S) and the (S,aR,S) atropisomeric ligands 1a and 1b in 95% and 85% yields, respectively (Scheme 2).

Scheme 2.

Scheme 2

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Preparation of bipheny bisoxazoline ligands 1.

The 1HNMR spectra of the resulting ligands have demonstrated two sets of signals for the rotatory diastereomers with different ratios. In the case of the ligand bearing phenyl groups (1a), the observed ratio of (S,aS,S) to (S,aR,S) was 61:39, while for the ligand bearing isopropyl groups (1b), it was 80: 20. These ratios indicate that one of the two possible diastereomers has more preference to the other, which can be attributed to the steric congestion of the R groups on the oxazoline rings. On the basis of the behavior of such scaffolds, in order to obtain enantiomerically pure complexes, Cu(CH3CN)4PF6 was added to the conformational mixture. Upon addition of the Cu salt, one of the both possible diastereomeric complexes, the (S,aS,S) isomer, was predominantly formed through the chelation-induced process. It can be deduced that one of the two diastereomers converts to another by rotation around the internal C–C bond, resulting in a stable Cu-isomeric complex. In the 1H NMR spectrum of the obtained complex, one set of signals was mainly observed. Comparison of the 1H NMR spectra of the Cu (I)-1a complex with the ligand 1a, for example, clearly showed that three of six triplets signals in the ligand 1a, which are around at δ = 3.83–5.27 ppm, were disappeared. Such a distinct decline in the number of signals was also observed in the 13CNMR spectra of the Cu (I)-1a complex. Although the absolute configuration of the resulting complex has been determined as (S,aS,S) by NOE14,15, attempts to achieve suitable crystals for X-ray single crystallographic analysis to assign the exact stereochemistry were failed.

The resulting Cu-(S,aS,S)-BOX complexes 1a and 1b were evaluated in the enantioselective allylic oxidation of a range of olefins using different substituted t-butyl perbenzoate 7 bearing both electron-withdrawing and electron-donating groups on the phenyl ring. To obtain the optimum condition, the asymmetric reaction was studied by employing cyclohexene as the substrate and t-butyl p-nitroperbenzoate 7a in the presence of catalytic amounts of Cu-1a or 1b complexes, which is generated in situ from a slight excess of ligands 1a or 1b and a variety of copper (I) and (II) salts such as Cu(CH3CN)4PF6, CuOTf, Cu(OTf)2, CuI, CuCl2, CuO, CuSO4, Cu(OAc)2, Cu2O, and Cu(NO3)2. The reaction was also examined in a range of temperatures from − 10 to room temperature in different polar to non-polar solvents such as acetonitrile, acetone, chloroform, dichloromethane, toluene, and n-hexane. Moreover, the effect of additives such as phenylhydrazine as a reductant agent that reduces Cu (II) into Cu (I), and also inorganic porous materials such as molecular sieves 4 Å, MCM-41, SBA-15 and HZSM-5 were investigated. The results showed that the corresponding enantiomerically enriched allylic ester 8a, (S)-2-cyclohexenyl-p-nitrobenzoate, could be obtained in high enantioselectivity (93% ee) and excellent yield (98%) in a reasonable time (39 h) when the reaction was carried out at room temperature in CH3CN, in the presence of 3.2 mol% of Cu(CH3CN)4PF6-1a complex as a catalyst, 5 μL phenylhydrazine and 5 mg HZSM-5 (Table 1, entry 1). As it can be seen in Table 1 and Fig. 1, conducting the reaction in the presence of Cu(CH3CN)4PF6-1a gave higher enantioselectivites than Cu(CH3CN)4PF6-1b. It was also found that the best results could be achieved when the peresters containing electron-withdrawing substitutions, especially p-nitro (7a), p-iodo (7b), and also o-iodo (7d) substitutions, were used (Table 1, entries 1–6). The reaction using electron donating groups such as Me (7 h) and OMe (7i) was slower and gave allylic esters in lower yields and ee values (Table 1, entries 8 and 9).

Table 1.

Effect of stereochemistry of the BOX ligand and substitution on the perester on asymmetric allylic oxidation of cyclohexene.

graphic file with name 41598_2022_18922_Tab1_HTML.jpg

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Figure 1.

Figure 1

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Comparison of the chiral ligands 1a and 1b in ee, yield and reaction time.

According to literature49,56–65, the proposed reaction mechanism take places by complexation of the (S,aS,S)-biphenyl BOX ligand 1a with Cu (I) to form the chiral catalyst, which is assumed that mainly coordinated with cyclohexene (Scheme 3). Addition of the t-butyl p-nitroperbenzoate 7a initiates the reaction through a catalytic cycle involving change in the copper oxidation state. In the first step, cyclohexene is substituted by the perester 7a. Following that, in the oxidative-addition step, crypto-tert-butoxyl radical is formed through concerted cleavage of oxygen–oxygen bond of the perester 7a and also oxidation of copper (I) into copper (III). In the next step, cyclohexene again coordinates to the copper, and then, in the limiting step, the tert-butoxo group, which is bonded to the copper complex, selectively removes a prochiral allylic hydrogen of the cyclohexene in an intramolecular process. Thereafter, elimination of a tert-butyl alcohol leads to the key intermediate. Subsequently, carboxyl attacks the Si-face of cyclohexnyl and through a pericyclic rearrangement including the migration of π-bond and a stereospecific reductive-elimination, gives (S)-2-cyclohexenyl-p-nitrobenzoate-catalyst complex. Eventually, enantioenriched (S)-2-cyclohexenyl-p-nitrobenzoate is released by replacing with cyclohexene, and as a result, the Cu (I)- cyclohexene is reproduced.

Scheme 3.

Scheme 3

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A rational mechanism of enantioselective allylic oxidation of cyclohexene using tert-butyl p-nitrobenzoperoxoate, catalyzed by Cu (I)-(S,aS,S)-1a complex.

It was observed that the reaction rate in the case of ortho substituted peresters was slower than para; however, enantioselectivities and yields were not significantly different (Table 1, cf. entries 1–3 and 4–6). Therefore, under optimum conditions, allylic oxidation of other olefinic substrates with peresters 7a, b and d were also investigated. Similarly, ligand 1a gave better results than 1b, and also p-nitroperbenzoate 7a was the best oxidant (Table 2, entries 1–9). This discrepancy in the enantioselectivity may be attributed to the interaction between generated allyl radicals and the phenyl substituents in ligand 1a at the transition states51,66. In case of acyclic olefins, the reaction times were longer, and yields and ee values were also inferior, although the best results were obtained in the presence of p-iodoperbenzoate 7b (Table 2, entries 10–12). It seems that due to more conformational flexibility of the acyclic olefins compared with the cyclic ones, both re-face and Si-face can be attacked32. Cyclopentene and cyclooctene afforded the corresponding enantioenriched allylic esters 9 and 10 in longer times with lower enantioselectivities and yields in comparison to cyclohexene (Table 2, entries 1–6). However, in the case of 1,5-cyclooctadiene the best results were obtained. In other words, not only the reaction was completed in shorter times, but enantioselectivity and yield of the obtained chiral ester 11 were also excellent (Table 2, entries 7–9).

Table 2.

Enantioselective allylic oxidation of cyclic and acyclic olefins using BOX ligands 1a and 1b.

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In the following, to gain a greater insight in to the structure of the copper complexes 1a and 1b, catalytic activity, enantioselectivity, thermodynamic stability, and interactions between orbitals, DFT calculations were carried out using the B3LYP method at 6–31 (d,p) basis set level and CPCM as the method of solvent. Moreover, the Van der Waals interactions were considered to correct DFT energies. A suitable way to investigate the thermodynamic stability of isomers is the comparison between their Gibbs free energy values67–69. Thermochemistry results of the isomeric complexes containing phenyl group (Cu (I)-1a) showed that the Cu (I)-(S,aS,S)-isomeric complex has more negative free energy by 3.48 kcal/mol than the (S,aR,S) isomer, which means that the (S,aS,S)-complex is more stable than another one. Moreover, the equilibrium constant, which indicates the population of each isomer, was calculated to be K = 355.73, at ∆Go = − 3.48 kcal/mol that again confirms the more preferred of the (S,aS,S) isomeric complex than the (S,aR,S) isomer (Fig. 2). Similarly, the difference Gibbs free energy between the isomeric complexes containing isopropyl group (Cu (I)-1b) displayed that the (S,aS,S) complex is 3.05 kcal/mol more negative than another one, and the equilibrium constant at ∆Go = − 3.05 kcal/mol is 172.15, which again showed that the (S,aS,S) complex is almost the only formed product (Figure S46). All of these results are in good agreement with the experimental results, where the complexation of the mixture of the free ligands with Cu(CH3CN)4PF6 showed mainly one set of signals in the 1HNMR and 13CNMR spectra. Based on the NMR observations, the absolute configuration of the main complex was assigned as (S,aS,S)14,15.

Figure 2.

Figure 2

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Gibbs free energy and equilibrium constant values for Cu (I)-1a complexes.

It was calculated that the relative population of the (S,aS,S) isomeric complexes Cu (I)-1a and Cu (I)-1b are 99.72% and 99.42%, respectively (Fig. 2 and S46). It can be deduced that regardless of the type of substitution at the stereogenic centers, the Cu (I)-(S,aS,S) diastereomer is more stable than the other one. The optimized geometric structures of the Cu (I)-(S,aS,S)-1a and Cu (I)-(S,aR,S)-1a have obviously shown that the (S,aR,S)-isomer confronts with steric hindrance caused by phenyl groups, which are in the equatorial position and have eclipsed form to each other. It is thought that the eclipsed form does not allow the PF6− group to be at the best distance and orientation from the Cu (I), thus the Cu (I)-(S,aR,S)-1a complex has more energy level than the (S,aS,S) isomer (Fig. 3). On the contrary, in the Cu (I)-(S,aS,S)-1a, the phenyl substitutions are placed in the axial position and anti-form to each other, so, due to lack of constraint, the PF6− group can easily close to the Cu (I) and stabilize it more effectively than the eclipse form (Fig. 3). Therefore, in line with the experimental observation, the major formed isomeric complex would be the (S,aS,S) isomer15,18,19,24.

Figure 3.

Figure 3

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Optimized structures of the Cu (I)-(S,aS,S) and (S,aR,S)-1a complexes in CHCl3.

Natural Bond Orbital (NBO) analysis is a convenient method to simplify the analysis of intra and intermolecular interactions between filled and virtual orbitals in molecules70,71. Therefore, NBO calculation was used at the B3LYP/6-31G(d,p) level to determine stabilization energy (E(2))72,73, and to specify partial charge on the selected atoms, as well. Then the highest values of E(2), namely the strongest interactions, were selected to examine interactions in the Cu (I)-(S,aS,S)-1a and Cu (I)-(S,aS,S)-1b complexes. As expected, the stabilization energies, E(2), have shown that the nitrogen atoms have a main role in coordination with the Cu (I). In the Cu (I)-(S,aS,S)-1a complex, the highest interaction energy between the donor orbital (the nitrogen lone pair) and the acceptor antibonding orbital (the lone pair star on the Cu (I) metal) is 55.39 kcal/mol. While, this energy in the case of Cu (I)-(S,aS,S)-1b complex is lower (44.62 kcal/mol). The stabilization energies for other types of interactions are listed in Table 3.

Table 3.

E(2) parameter on selected atoms of the Cu (I)-(S,aS,S)-complexes using NBO calculation.

Cu (I)-(S,aS,S)-1b complex Cu (I)-(S,aS,S)-1a complex
Donor Acceptor E(2) (kcal/mol) Donor Acceptor E2(kcal/mol)
LP (1) N 33 LP*(6) Cu 37 44.62 LP (1) N 33 LP*(6) Cu 37 55.39
LP (1) N 36 LP*(6) Cu 37 44.62 LP (1) N 36 LP*(6) Cu 37 55.39
CR (2) P 38 LP*(7) Cu 37 11.83 LP*(1) P 60 LP*(7) Cu 37 11.81
LP*(1) P 38 LP*(7) Cu 37 14.24 CR (2) P 60 LP*(7) Cu 37 10.54
LP*(2) P 38 LP*(6) Cu 37 13.60 LP*(2) P 60 LP*(6) Cu 37 14.92
LP (3) F 39 LP*(6) Cu 37 14.62 LP (3) F 61 LP*(6) Cu 37 12.70
LP (3) F 39 LP*(7) Cu 37 12.76 LP (3) F 61 LP*(7) Cu 37 11.00
LP (3) F 44 LP*(6) Cu 37 14.62 LP (3) F 66 LP*(6) Cu 37 12.70
LP (3) F 44 LP*(7) Cu 37 12.74 LP (3) F 66 LP*(7) Cu 37 11.00
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In addition, the comparison of the length bond between the nitrogen atom and the Cu (I) fragment of the two mentioned complexes have shown that the complex Cu (I)-(S,aS,S)-1a possess fewer length bond (1.4 pm). It seems that this slight difference caused a dramatic increase (10.77 kcal/mol) in E(2) energy (Table 3 and Fig. 4).

Figure 4.

Figure 4

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Bond lengths and partial charges on selected atoms in the Cu (I)-(S,aS,S)-1a and -1b complexes.

In the following, to compare the chemical activity of the complexes, the HOMO–LUMO energy gaps of the (S,aS,S) complexes were calculated74,75. In fact, the lower the HOMO–LUMO gap, the higher the chemical activity. The HOMO–LUMO gap values for the Cu (I)-(S,aS,S)-1a- and -1b complexes are 3.31 eV and 3.28 eV, respectively (Fig. 5). The Cu (I)-1b complex possesses a very slightly lower (30 meV) band-gap energy than the Cu (I)-1a complex. Although analyzing the HOMO–LUMO gaps indicates a very little higher chemical activity in favor of the Cu (I)-1b complex, it seems that the formation of enantiomerically enriched allylic esters is controlled by steric hindrance. In addition, the large electron density on the Cu (I) fragment reveals that this metal ion plays a significant role in the HOMO orbital.

Figure 5.

Figure 5

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HOMO–LUMO energy gaps of the Cu (I)-(S,aS,S)-1a and Cu (I)-(S,aS,S)-1b complexes.

As it was explained, in the Cu (I)-(S,aS,S)-1b complex, the steric congestion caused by the isopropyl substitutes is more than the phenyl groups in the Cu (I)-(S,aS,S)-1a complex, and as a result, the N-Cu–N bond angle has to become a little smaller in the Cu (I)-(S,aS,S)-1b complex than the one in another complex. Although this help the steric repulsion arising from the isopropyl groups decrease to some extent, yet the PF6− group has to approach to the Cu (I) atom with a slight tilt angle (Ф). In contrast, in the Cu (I)-(S,aS,S)-1a complex, there is no significant steric congestion; the PF6− group can approach to the Cu (I) atom with a little tilt (Fig. 6). Therefore, it seems that the reactants, olefin and perester, can properly close to the Cu (I)-(S,aS,S)-1a complex and generate chiral allylic esters with higher enantioselectivities than the other complex.

Figure 6.

Figure 6

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Steric repulsion caused by phenyl and isopropyl substitutions.

To investigate the enantioselectivity and yields of the allylic oxidation reaction, DFT calculations of the key reaction intermediate stage (the mechanism proposed in Scheme 3) were performed at the B3LYP-D3/6-31G (d,p) level of theory for cyclohexene and 1-hexene reactants and para-nitrobenzoate as the perester of the reaction in acetonitrile. To this end, our selected conformers not only must have minimum energy but also must follow a pericyclic rearrangement similar to the key intermediate stage. The computational results indicate that this intermediate is more stable thermodynamically when the oxygen atom attacks the cyclohexyl group from the Si-face side than the Re-face side by − 3.06 kcal/mol (Fig. 7). Based on the optimized geometry structures, in the Si-face intermediate the nucleophile (i.e., oxygen atom) can easily approach the double bond, on the contrary, in the Re-face intermediate the oxygen cannot simply get close to the double bond due to the existence of steric hindrance between the oxazoline ring (in red) of the catalyst and cyclohexyl group (in green) (Fig. 7A). Therefore, to reduce repulsive interactions, the cyclohexnyl group has to get away from the oxazoline moiety so that the oxygen atom can get close to the double bond (Fig. 7B). In this situation, although the Re-face intermediate can avoid undesirable interactions to some degree, it remains unstable thermodynamically compared to the Si-face intermediate (Fig. 7C).

Figure 7.

Figure 7

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Steric hindrance and Gibbs free energies of the Si-face and Re-face of the key reaction intermediate containing cyclohexene reactant. To better visibility, some atoms of biphenyl backbone are not shown.

On the other hand, since acyclic compounds are very flexible, they can find a variety of geometries; consequently, they can get rid of the steric congestion caused by the oxazoline ring well. Accordingly, for the intermediate bearing 1-hexenyl group, the steric congestion does not make a significant difference between energy levels of the Si-face and Re-face in the key reaction intermediate stage. As a result, the ee and yield of products would be very low compared to the cyclic compounds. Albeit conformational search indicates a slight preference (by − 0.05 kcal/mol) for the Re-face intermediate (Fig. 8A), in this conformer, the orientation of the nucleophile (i.e., oxygen atom) is opposite to the double bond; thereby, the para-nitro benzoate group must have a significant amount of rotation to perform the desired reaction. According to our initial condition for intermediates, having an appropriate orientation between the nucleophile and electrophile is essential for a pericyclic rearrangement. Therefore, the Gibbs free energy difference between Si-face and Re-face intermediates containing favorable orientation is − 1.38 kcal/mol in favor of the Si-face intermediate (Fig. 8B,C).

Figure 8.

Figure 8

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Geometries and Gibbs free energies of the Si-face and Re-face of the key reaction intermediate containing 1-hexene reactant. To better visibility, some atoms of biphenyl backbone are not shown.

Most importantly, the difference in enantiomeric excesses and yields of the cyclic and acyclic products is due to the difference in steric congestion that these reactants encounter in the key reaction intermediate stage. In the case of the 1-hexene reactant, the 1-hexenyl group can avoid the steric congestion caused by the oxazoline ring, thus the difference in thermodynamic stability between Re- and Si-face conformers are very close to each other (1.38 kcal/mol). For that reason, enantiomeric excess and yields of its products would be lower compared to the rigid structure of the intermediate containing cyclohexene, in which related ∆Go is − 3.08 kcal/mol. These results are in line with the experimental data in Table 2.

Another factor that is effective in the low yields of acyclic compounds is their non-symmetric geometries, leading to a diversity of intermediates via coordinating different carbon types to the copper catalyst. Hence, the nucleophile can attack a variety of carbons, produce a range of products, and as a result, reduce the yield and ee of the products.

Conclusion

In summary, asymmetric copper catalyzed allylic C-H bond oxidation of cyclic and acyclic alkenes with a series of substituted t-butyl perbenzoates in the presence of (S,aS,S)-atropisomeric BOX ligands 1a and 1b (which can be easily obtained from a mixture of their S, R epimers, through the chelation-induced process) and porous inorganic additives was studied. It was revealed that at room temperature in CH3CN in a combination of ligand Cu(CH3CN)4PF6-1a and additives of PhNHNH2 and porous HZSM-5, peresters containing electron withdrawing groups at phenyl ring led to the corresponding chiral allylic esters with an excellent level of enantioselectivities and chemical yields in relatively short times. The DFT results of the Cu (I)-BOX complexes provided a deeper understanding of more thermodynamic stability of the (S,aS,S) complexes than their (S,aR,S) isomers. It can be inferred that due to the less sterically congestion of Cu (I)-(S, aS, S)-1a complex, the reactants are able to easily place in the appropriate position, leading to enantioenriched allylic esters with higher enantioselectivity compared to the Cu (I)-(S,aS,S)-1b complex. Finally, it turns out that enantiomeric excess of the cyclic products is controlled by steric hindrance arose from oxazoline moiety of the copper catalyst and incoming reactants in the key reaction intermediate stage.

Experimental

Typical procedure for the synthesis of bishydroxylamides 6a and 6b

In a 25 mL flame dried, 2-necked flask, under nitrogen, biphenyl dicarboxylic acid 3 (0.48 g, 2.0 mmol) was dissolved in 6 mL dichloromethane. Then, the reaction was cooled to 0 °C, and then oxalyl chloride (0.84 mL, 8 mmol) was added slowly followed by 3 drops of DMF. After stirring the mixture for 4 h at room temperature, evaporation of the solvent in vaccuo gave diacyl chloride as a light yellow solid (0.56 g, 99%). The obtained diacyl chloride was dissolved in 6 mL CH2Cl2, and at 0 °C, slowly added to a solution of (S)-phenyl glycinol 5a (0.6 g, 2.4 mmol) and Et3N (0.67 mL) in 6 mL CH2Cl2 during 30 min. The mixture was allowed to warm to room temperature and stirred overnight. Monitoring the reaction by TLC (90:10 EtOAc/n-hexane) showed two compounds (S,aS,S)- and (S,aR,S)-6a. After the reaction was completed, it was washed with brine (10 mL) and the organic layer was separated, and then the aqueous layer was extracted with EtOAc (3 × 15 mL). The combined organic layer was dried over MgSO4 and concentrated in vaccuo. Purification of the residue by silica gel column chromatography (eluent: EtOAc/n-hexane; 80–100: 20–0) gave a white solid 6a in 95% yield. Compound 6b was prepared according to the same procedure in 98% yield15,18.

Typical procedure for the synthesis of ligands 1a and 1b

In order to cyclization of 6a, under nitrogen atmosphere, in an oven-dried round-bottom flask bishydroxylamide 6a (1 mmol, 0.48 g, 1 equiv) was dissolved in CH2Cl2 and 4-(dimethylamino) pyridine (0.01 g, 0.1 mmol, 0.1 equiv) was added. After cooling to 0 °C, Et3N (0.6, 4.4 mmol, 4.4 equiv), and a solution of p-TsCl (0.38 g, 2 mmol, 2 equiv) in 2 mL of dichloromethane were added. The mixture was stirred at ambient temperature for 18 h and then washed with saturated aqueous NH4Cl (10 mL). The aqueous layer was extracted with CH2Cl2 (3 × 10 mL), and the combined organic layers washed with 10 mL saturated NaHCO3 (aq), dried with Na2SO4 and evaporated under vaccuo. Purification of the resulting light yellow oil by column chromatography (n-hexane/EtOAc; 90:10); resulted in pure light yellow 1a (95%); (61 (S,aS,S): 39 (S,aR,S)). Ligand 1b was synthesized by the similar protocol in 85% yield; (80 (S,aS,S): 20 (S,aR,S) 15,18.

General procedure for the synthesis of the Cu (I)-1-complex

Under nitrogen atmosphere, 1 equiv of Cu(CH3CN)4PF6 (0.018 mmol, 6.6 mg) was added to ligand 1 (0.02 mmol) dissolved in 1 mL of chloroform-d and stirred at room temperature for 3 h. Monitoring the reaction by TLC revealed a single new spot14,15.

Typical procedure for asymmetric Kharasch–Sosnovsky reaction

Under a nitrogen atmosphere, at room temperature, a 10 mL flame dried schlenk flask was charged with dried acetonitrile (2 mL), Cu(CH3CN)4PF6 (10 mg, 0.027 mmol) and chiral ligand 1a (14 mg, 0.032 mmol) and stirred for 2 h. Then, phenyl hydrazine (5 μL, 0.05 mmol) and HZSM-5 (5 mg) were added. After a few minutes, cyclohexene (2.5 mmol, 0.25 mL) was added slowly, and the reaction mixture was cooled to 0 °C, and tert-butyl-p-nitrobenzoperoxoate 7a15,18,50–52 (0.85 mmol, 0.203 g) was added portionwise, and then stirred at 0 °C until complete disappearance of 7a (TLC). After that, 5 mL 10% NH4OH was added to the mixture and extracted with EtOAc (3 × 5 mL). A yellow residue was obtained after evaporation of the solvent. Column chromatography of the obtained residue on silica gel afforded (S)-2-cyclohexenyl-p-nitrobenzoate as a white solid (98%, 93% ee). The bisoxazoline ligand was also recovered in 92% yield15,18,50–52,76–80.

Computational method

In this study, the phenyl and isopropyl group substitutions were selected to examine the effect of aryl and alkyl groups on the isomeric complexes. First structures were drawn using Spartan software81 and gauss view 682, and then Gaussian 983 and Gaussian 16 were employed for DFT calculations. Both frequency and optimization calculations were carried out with the B3LYP method at 6-31G (d,p) basis set level and CPCM as the method for chloroform solvent. The basis set was selected based on two factors: computational cost and an excellent agreement between computational and experimental results. In addition, long-range van der Waals interactions are taken into account using the Grimm’s D3 dispersion correction for complexes (i.e. B3LYP-D3/6-31G (d,p) level of theory) to make the DFT energies of complexes more accurate. Different conformers of complexes with C1 and C2 symmetries were designed and optimized at the 6-31G (d,p) basis set level. The selection criterion for determining the stable conformers was the Gibbs free energy of the systems and not the symmetry of the molecules. All frequencies were done without imaginary frequency. The absence of imaginary frequencies in the computational outputs indicates that all optimized structures are at their minimum energy in the potential energy surfaces diagram. Moreover, Gibbs free energies were calculated to determine the thermodynamic stability of the complexes. In the case of intermediates containing 1-hexenyl groups, different conformers, including cis and trans forms of the 2-hexenyl group, were investigated to find global minimums. In addition, to determine the relative amounts of each isomer at equilibrium, equilibrium constant (Keq) at the 298.15 K, one atmosphere pressure and 1.98 × 10–3 kcal/(K mole) as gas constant, were calculated84.

Supplementary material

Supplementary material (included materials and characterization methods, the typical procedure for the synthesis of 5 and 7–14, and Figure S46 and geometry optimized coordinates of compounds) associated with this article can be found in the online version.

Supplementary Information

Supplementary Information. (3.4MB, pdf)

Acknowledgements

The authors are grateful to the University of Kurdistan Research Councils and the Iran National Science Foundation (Project No: 4003026) for providing financial support for this research.

Author contributions

S.S.: Conceived and designed the experiments; Performed the experiments; Analyzed and interpreted the data; Wrote the paper. H.A.: Performed the experiments; Analyzed and interpreted the data; Wrote the paper. S.M.: Designed and performed the calculations, analyzed and interpreted the computational results; wrote the computational part of the manuscript. H.P.: Revised and commented on the computational part; performed part of calculations; provided a high-performance computer for calculations. All authors read and approved the final manuscript.

Data availability

The generated and analyzed data during the current study is supplied in this manuscript and supplementary material.

Competing interests

The authors declare no competing interests.

Footnotes

Publisher's note

Springer Nature remains neutral with regard to jurisdictional claims in published maps and institutional affiliations.

Supplementary Information

The online version contains supplementary material available at 10.1038/s41598-022-18922-1.

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Supplementary Materials

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Data Availability Statement

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