Naima Munira,
Sara Masooda,
Faroha Liaqata,
Muhammad Nawaz Tahirb,
Sammer Yousufc,
Saima Kalsoomd,
Ehsan Ullah Mughale,
Sajjad Hussain Sumrrae,
Aneela Maalik*f and
Muhammad Naveed Zafar*a
aDepartment of Chemistry, Quaid-i-Azam University, Islamabad-45320, Pakistan. E-mail: mnzafar@qau.edu.pk; Tel: +923314503061
bDepartment of Physics, University of Sargodha, Sargodha-40100, Pakistan
cH. E. J. Research Institute of Chemistry, International Centre for Chemical and Biological Sciences, University of Karachi, 75270, Pakistan
dCentre for Interdisciplinary Research in Basic Sciences (CIRBS), International Islamic University, Islamabad, Pakistan
eDepartment of Chemistry, University of Gujrat, Gujrat-50700, Pakistan
fDepartment of Chemistry, COMSATS University Islamabad, Islamabad Campus, Park Road, Islamabad-45550, Pakistan. E-mail: aneela.maalik@comsats.edu.pk; Tel: +923335490834
First published on 21st November 2019
The present research work describes the synthesis of five new ligands containing pyridinium amine, [H2L1][OTf]2–[H2L5][I]2 from two new precursors, [P3Et][I] and [P2Me][CF3SO3]. The structure elucidations of the compounds were confirmed by multinuclear NMR (1H, 13C), FT-IR and by single crystal XRD techniques. Theoretical DFT studies were carried out to get better insight into the electronic levels and structural features of all the molecules. These synthesized new Pro-PYE ligands [H2L1][OTf]2–[H2L5][I]2 were found to be significantly active as co-catalysts for Pd(CH3CO2)2 toward Heck–Mizoroki coupling reactions with wide substrate scope in the order of [H2L1][OTf]2 ≫ [H2L2][OTf]2 > [H2L3][OTf]2 > [H2L4][OTf]2 > [H2L5][I]2.
The catalytic cycle of Heck–Mizoroki C–C cross coupling involves both oxidative addition as well as reductive elimination reaction. This coupling method is an appropriate synthetic route for synthesis of substituted olefins. High electronic density around the palladium via appropriate electron rich ligand facilitates oxidative addition (the key rate determining step) of various aliphatic or aromatic halides in the coupling reaction.19–21 Various palladium complexes have been used to catalyze above reaction.22–24 However, the much easier way is to use a mixture of suitable ligand and palladium precursor.25,26 In this regard, five new H-PYE ligands, [H2L1][OTf]2–[H2L5][I]2, were synthesized (Schemes 1–3) from two ligand precursors [P3Et][I] and [P2Me][CF3SO3]. These ligands were found to act as co-catalysts for Pd(OAc)2 and significantly enhanced their catalytic activity in Mizoroki–Heck coupling reactions under diverse reaction conditions. The molecular structures of all new compounds were characterized by using various spectroscopic and computational techniques.
Royal yellow solid, yield 56%, mp: 156 °C. 1H NMR (300 MHz, DMSO-d6), J (Hz), δ (ppm): 9.28 (dd, 1H, J = 1.8, Py-H), 8.65 (dd, 1H, J = 1.8, Py-H), 8.19–8.07 (m, 2H, Py-H), 4.75 (q, 2H, J = 7.2, CH2), 1.49 (t, 3H, J = 7.2, CH3). 13C NMR (75 MHz, DMSO-d6), J (Hz), δ (ppm): 147.5, 144.7, 141.21, 127.87, 122.60, 62.31, 15.96. FT-IR (KBr, cm−1): 3069, 2956, 1600, 1357, 1272, 1153, 1065.
Colorless solid, yield 95%, mp: 161 °C. 1H NMR (300 MHz, DMSO-d6), J (Hz), δ (ppm): 9.16 (dd, 1H, J = 1.5, Py-H), 8.62–8.56 (m, 1H, Py-H), 8.37 (dd, 1H, Py-H), 8.12–8.07 (m, 1H, Py-H) 4.33 (s, 3H, CH3). 13C NMR (75 MHz, DMSO-d6), J (Hz), δ (ppm): 148.6, 147.4, 129.9, 126.5, 123.2, 119.0, 47.8. FT-IR (KBr, cm−1): 3097, 1617, 1309, 1260, 1142, 1028.
Off white solid, yield 70%, mp: 165 °C. 1H NMR (300 MHz, DMSO-d6), J (Hz), δ (ppm): 11.06 (s, 2H, NH), 8.48–8.46 (d, 4H, J = 7.2, py- H), 7.96–7.91 (d, 1H, J = 7.7, py-H), 7.84–7.82 (d, 4H, J = 6.3, py-H), 6.96–6.94 (d, 2H, J = 8.1, py-H), 4.07 (s, 6H, CH3).13C NMR (75 MHz, DMSO-d6),J (Hz),δ (ppm): 152.6, 151.1, 145.1, 143.2, 112.9, 109.7, 45.8. FT-IR (KBR, cm−1): 3296, 3080, 1638, 1581, 1365, 1278, 1199, 1025.
Brown crystalline solid, yield 78%, mp: 180 °C.1H NMR (300 MHz, DMSO-d6), J (Hz),δ (ppm): 9.11 (s, 2H, NH), 8.18–8.15 (d, 2H, J = 6.9, py-H), 7.93–7.91 (d, 2H, J = 6.9, py-H), 7.21–7.19 (m, 2H, py-H), 6.75–6.73 (m, 2H,py-H), 3.81 (s, 6H, CH3), 3.71–3.69 (d, 2H, J = 6, cy-H), 1.75–1.73 (d, 2H, J = 7.8, cy-H), 1.53–1.49 (d, 2H, J = 9.3, cy-H), 1.45–1.37 (m, 4H, cy-H).13C NMR (75 MHz, DMSO-d6), J (Hz),δ (ppm): 156.5, 144.3, 142.5, 110.4, 106.3, 56.2, 44.4, 31.5, 24.3. IR (KBR, cm−1): 3360, 3053, 2943, 1646, 1588, 1375, 1296, 1169, 1058.
Brown solid, yield 60%, mp: 232 °C. 1H NMR (300 MHz, DMSO-d6), J (Hz),δ (ppm): 8.26 (t, 2H, J = 6.6, NH), 8.24–8.18 (dd, 2H, J = 6.9, py-H), 7.99–7.37 (m, 2H, py-H), 7.03–7.00 (d, 1H, J = 7.5, py-H), 6.53–6.45 (dd, 1H, J = 8.4, py-H), 3.99 (s, CH3, 6H), 3.66 (s, 1H, cy-H), 3.54–3.50 (d, 1H, J = 3.6, cy-H), 2.49–2.25 (m, 2H, cy-H), 1.88–1.86 (d, 2H, J = 6 cy-H), 1.66–1.65 (d, 2H, J = 3, cy-H), 1.19–1.17 (d, 2H, J = 5.1, cy-H). 13C NMR (75 MHz, DMSO-d6), J (Hz), δ (ppm): 159.1, 153.3, 147.7, 143.2, 112.7, 43.2, 32.8, 24.5.
Dark brown solid, yield 70%; mp: 205 °C. 1H NMR (300 MHz, DMSO-d6), J (Hz),δ (ppm): 8.28 (t, 2H, J = 5.7, NH), 8.09–8.03 (m, 4H, Py-H), 7.42–7.39 (d, 4H, J = 9, Py-H), 7.05–6.99 (m, 2H, Py-H), 3.79 (d, 6H, J = 4.8, CH3), 3.67 (d, 4H, J = 4.5, CH2). 13C NMR (75 MHz, DMSO-d6), J (Hz),δ (ppm):153.2, 143.5, 142.4, 123.3, 118.9, 113.2, 111.5, 42.2, 40.7. IR (KBr, cm−1): 3325, 3086, 2952, 1649, 1591, 1348, 1243, 1159, 1025.
Fawn yellow solid, yield 48%; mp: 304 °C. 1H NMR (300 MHz, DMSO-d6), J (Hz),δ (ppm): 8.28 (s, 1H, N–H), 8.19 (s, 1H, Py-H), 8.04 (s, 1H, Py-H), 7.40 (d, 1H, Py-H), 7.03 (s, 1H, Py-H), 4.22 (q, 2H, J = 5.1, CH2), 3.68 (s, 2H, CH2), 1.31 (t, 3H, J = 7.2, CH3). IR (KBr, cm−1): 3205, 3016, 2970, 1642, 1536, 1364, 1217, 1173, 1063.
All the ligands, [H2L1][OTf]2–[H2L5][I]2, were synthesised by the melt reaction between respective ligand precursor and corresponding amine. In these ligands, NH peak appeared in the range of 9–11 ppm that indicated the conversion of all primary amines to secondary amines. In aliphatic region, N-alkylated protons showed peaks for methyl and ethyl between 4.24–3.70 ppm in all ligands. Similarly carbon NMR showed these peaks between 62.3–47.8 ppm. The aromatic protons and their carbon atoms showed the respective peaks in their standard region. The peaks for cyclohexyl group appeared between 1.17–3.71 ppm for [H2L2][OTf]2 and [H2L3][OTf]2. In FT-IR spectra, the broad peaks appeared between 3296-3205 cm−1 for ν(N–H). While peaks of δ(N–H) appeared at 1581–1591 cm−1 in [H2L1][OTf]2–[H2L5][I]2. Peaks of aromatic region ν(C–H) ranges 3101–3016 cm−1 while skeleton vibrations or peaks due to breathing vibrations of aromatic ring were observed around the following frequencies; 1600, 1560, 1500, 1460 cm−1.30 In aliphatic region, the characteristic stretching band ν(C–H) appeared at 2970–2943 cm−1 and bending vibrations associated with δ(C–H) present in the particular range of 1436–1459 cm−1. Signals appeared for both secondary CN and primary C–N stretch in the region of 1690–1590 cm−1 and 1350–1280 cm−1 respectively. Peaks between 1350–1225 cm−1 were assigned to both asymmetric and symmetric ν(SO), while signals between 828–863 cm−1 were designated to ν(S–O). Sharp peak associated with ν(C–F) observed in the range of 1025–1063 cm−1.
A comparison of proton and carbon NMR spectra of [H2L1][OTf]2 and [H2L2][OTf]2 reveals that B type resonance structure is predominant for [H2L2][OTf]2 unlike in [H2L1][OTf]2 as shown in Fig. 2. The 1H and 13C NMR (DMSO-d6) spectra for [H2L2][OTf]2 indicated the chemical equivalence in solution form of both pyridinium groups on NMR timescale. This lead to the appearance of only one signal for the both methyl groups at 3.81 ppm in 1H NMR and 44.4 ppm in 13C NMR spectra. Similarly, only one signal for NH appeared in 1H NMR spectrum at 9.11 ppm. Though the individual atoms making up each of the pairs C2/C3 and C1/C4 (as well as their symmetry related pairs) within each pyridinium group were found unequal and we observed separate signals in each case. Such as, for C2/C2, C3/C3, C1/C1 and C4/C4 in the 13C NMR spectrum, separate singlet signals were observed at 144.35, 142.46, 110.37, and 106.31 ppm, respectively. This situation most likely result because of the conformational changes that equilibrate the positions of each of the pairs of atoms, C2/C3, C1/C4, C2/C3 and C1/C4, were slow on the NMR timescale. Whereas the 1H and 13C NMR (DMSO-d6) spectra of [H2L1][OTf]2 showed the chemical equivalence of both pyridinium groups and the pairs of atoms C1/C4 and C2/C3 (and the corresponding pairs of atoms in the second pyridinium ring) in solution on NMR timescale. The interaction possibility of the N1 and N1 lone pairs in [H2L1][OTf]2 with the head pyridine ring resulting in reduction of the N1/C5 and N1/C5 π-interactions is one possible explanation for this different behavior. Hence rotation about the N1–C5 bond became rapid on the NMR timescale.
Crystals suitable for single crystal XRD analysis were successfully grown for both precursors. [P3Et][I] crystals were grown from its acetone solution through slow evaporation method. The ORTEP depiction of [P3Et][I] is shown in Fig. 3. The crystal structure of [P3Et][I] confirms the successful ethylation of pyridine nitrogen. It also reveals that iodide acts as counter anion as well as replacement of o-chloro with iodo group. Crystals of [P2Me][CF3SO3] were prepared through slow evaporation process from its methanol solution. The ORTEP depiction of [P2Me][CF3SO3] is shown in Fig. 4 that shows successful methylation on nitrogen.
Attempts were made to grow the single crystals of all the ligands but [H2L3][OTf]2–[H2L5][I]2 were successfully grown and analyzed. [H2L3][OTf]2 was crystallized out in Pbcn space group from dichloromethane and ether (50:50) solution. ORTEP diagram is shown in Fig. 4. Crystal structure analysis confirms the attachment of two pyridinium rings to the cyclohexyl diamine and triflate is acting as counter anion. Cyclohexyl group adopts chair conformation with two substitutions at consecutive axial and equatorial positions show transoid geometry. Due to steric repulsion, the two substituted arms of cyclohexyl group shows torsion C7N1C5N2 angle of 171.8°.(Fig. 5).
[H2L4][OTf]2 was crystallized out in the space group P21/c in methanol and acetone solution. ORTEP depiction is shown in Fig. 6(A). Examination of crystal structure shows that there is torsion angle of 180.0° (N1–C1–C2–N3). Fig. 6(B) presents the hydrogen bonding that exists with NH–O distance of 2.92 Å (N1 and O2). These distances are within the normal range of NH–O bond lengths 2.81–3.04 Å.31. [H2L5][I]2 was crystallized out in the space group R in dichloromethane solvent. ORTEP depiction is shown in Fig. 7. Crystal structure cell coordinates reveal the presence of monoclinic system. The X-ray crystal structure confirms that two pyridinium rings are attached to nitrogen atoms of bidentate ethylene diamine. The two pyridinium amine groups beside ethylene unit adopt transoid geometry due to N1C1C1N1 torsion angle of precise 180° in both [H2L4][OTf]2 and [H2L5][I]2.
Fig. 6 (A) ORTEP depiction of [H2L4][OTf]2, (B) wire frame work of [H2L4][OTf]2 showing hydrogen bonding. |
The wire frame work structures of [H2L3]+2–[H2L5]+2 are shown in Fig. 8(A). It reveals that the bond lengths of [H2L3][OTf]2–[H2L5][I]2 are in accordance with the resonance form B in Fig. 8(B). The bond length of C5–N1 is 1.347 Å in [H2L3][OTf]2. Similarly [H2L4][OTf]2 and [H2L5][I]2 C2–N1 bond distances are 1.338 Å and 1.331 Å respectively that correspond to exocyclic carbon double bond nitrogen.
Fig. 8 (A) Wire framework of [H2L3]2+–[H2L5]2+ showing important bond distances, (B) resonance forms of [H2L3][OTf]2–[H2L5][I]2. |
A number of structural parameters have been obtained from semi-empirical studies on conformers with minimum energy. The energy of the frontier molecular orbitals is also instrumental in obtaining the values of chemical hardness (η), chemical potential (χ) and electrophilicity index (ω) using the eqn (1)–(3);33,34 where I and A are the ionization potential and electron affinity of a molecule, shown in Tables 1 and 2.
η = (I − A)/2 | (1) |
χ = −(I + A)/2 | (2) |
ω = χ2/2η | (3) |
Ligands | Values (eV) | Ionization energies (eV per molecule) | Electron affinity (eV per molecule) | Band gap (eV per molecule) |
---|---|---|---|---|
[P3Et][I] | HOMO = −8.15, LUMO = −0.47 | −8.15 | −0.47 | −7.67 |
[P2Me][CF3SO3] | HOMO = −9.39, LUMO = −2.27 | −9.39 | −2.27 | −7.12 |
[H2L1][OTf]2 | HOMO = −14.69, LUMO = −6.77 | −14.69 | −6.77 | −8.22 |
[H2L2][OTf]2 | HOMO = −14.50, LUMO = −6.12 | −14.50 | −6.12 | −8.38 |
[H2L3][OTf]2 | HOMO = −9.49, LUMO = −2.55 | −9.49 | −2.55 | −6.94 |
[H2L4][OTf]2 | HOMO = −9.15, LUMO = −2.33 | −9.15 | −2.33 | −6.82 |
[H2L5][I]2 | HOMO = −14.82, LUMO = −6.75 | −14.82 | −6.75 | −8.07 |
Ligands | Chemical hardness (η) | Chemical potential (χ) | Electrophilicity index (ω) |
---|---|---|---|
[P3Et][I] | −4.31 | 4.31 | −2.15 |
[P2Me][CF3SO3] | −5.83 | 5.83 | −2.91 |
[H2L1][OTf]2 | −10.73 | 10.73 | −5.36 |
[H2L2][OTf]2 | −10.31 | 10.31 | −5.15 |
[H2L3][OTf]2 | −6.02 | 6.02 | −3.01 |
[H2L4][OTf]2 | −5.74 | 5.74 | −2.87 |
[H2L5][I]2 | −10.78 | 10.78 | −5.39 |
The reactivity of a compound can also be gauged from the HOMO and LUMO orbitals energy difference (ΔEH−L); a larger band gap indicates lower reactivity and higher chemical hardness.35,36 The greater is the energy of HOMO, greater would be ionization potential and thus more is the ability of a molecule to donate an electron pair. While LUMO has the ability to accept electron density via back bonding from transition metal that is associated with electron affinity of molecule.37,38 The pictorial representations of all the frontier molecular orbitals (HOMO–LUMO) were acquired. HOMO–LUMO of [P3Et][I] and [H2L1][OTf]2 are shown in Fig. 9 and 10. The important bond lengths of optimized structures and XRD structures of compounds [H2L3][OTf]2–[H2L5][I]2 are compared in Tables 3–5. It shows good agreement between the computed and experimental values for all the compounds. Slight divergences in some bond lengths can be attributed to the choice of computational method, and the basis set used.35–39
Concerned atoms | Experimental | Calculated | Concerned atoms | Experimental | Calculated |
---|---|---|---|---|---|
C1–C2 | 1.35 | 1.38 | N2–C1 | 1.36 | 1.35 |
C2–C3 | 1.39 | 1.38 | C5–N1 | 1.35 | 1.39 |
C3–C4 | 1.36 | 1.39 | N1–C7 | 1.46 | 1.46 |
C4–C5 | 1.41 | 1.41 | C7–C8 | 1.53 | 1.54 |
C5–N2 | 1.36 | 1.37 | C8–C9 | 1.53 | 1.53 |
N2–C6 | 1.47 | 1.48 | C7–C7 | 1.54 | 1.55 |
Atom no | Experimental | Calculated | Atom no | Experimental | Calculated |
---|---|---|---|---|---|
C1–N1 | 1.46 | 1.48 | C5–C6 | 1.34 | 1.38 |
N1–C2 | 1.34 | 1.34 | C6–N2 | 1.36 | 1.35 |
C2–C3 | 1.40 | 1.41 | N2–C7 | 1.46 | 1.48 |
C3–C4 | 1.36 | 1.39 | N2–C2 | 1.36 | 1.38 |
C4–C5 | 1.39 | 1.38 | C1–C1 | 1.51 | 1.52 |
Concerned atoms | Experimental | Calculated | Concerned atoms | Experimental | Calculated |
---|---|---|---|---|---|
C1–N1 | 1.46 | 1.45 | C5–C6 | 1.32 | 1.38 |
N1–C2 | 1.33 | 1.39 | C6–N2 | 1.36 | 1.36 |
C2–C3 | 1.39 | 1.41 | N2–C7 | 1.49 | 1.49 |
C3–C4 | 1.36 | 1.39 | C7–C8 | 1.46 | 1.52 |
C4–C5 | 1.37 | 1.38 | C5–C6 | 1.32 | 1.38 |
Entry | Base | Pd(OAc)2 (mol) | Pd(OAc)2:L | Temperature (°C) | Solvent | Yield (%) |
---|---|---|---|---|---|---|
a Conditions: 3 h except entry 20, styrene (1.4 eq.) versus halobenzene. Isolated yields were based on aryl halide. | ||||||
1 | K2CO3 | — | 0:1 without catalyst | 100 | DMA | No reaction |
2 | K2CO3 | 0.1 | 1:1 | 100 | DMA | 83 |
3 | K2CO3 | 0.05 | 1:1 | 100 | DMA | 80 |
4 | K2CO3 | 0.01 | 1:1 | 100 | DMA | 78 |
5 | K2CO3 | 0.001 | 1:1 | 100 | DMA | 50 |
6 | K2CO3 | 0.01 | 1:1 | 80 | Hexane | 43 |
7 | K2CO3 | 0.01 | 1:1 | 110 | Toluene | 47 |
8 | K2CO3 | 0.01 | 1:1 | 100 | H2O | 56 |
9 | K2CO3 | 0.01 | 1:1 | 75 | DMF | 68 |
10 | K2CO3 | 0.01 | 1:1 | 100 | DMF | 84 |
11 | Na2CO3 | 0.01 | 1:1 | 100 | DMF | 80 |
12 | Cs2CO3 | 0.01 | 1:1 | 100 | DMF | 78 |
13 | NEt3 | 0.01 | 1:1 | 100 | DMF | 41 |
14 | Pyridine | 0.01 | 1:1 | 100 | DMF | 46 |
15 | CH3COONa | 0.01 | 1:1 | 100 | DMF | 86 |
16 | CH3COONa | 0.01 | 1:1 | 25 | DMF | 53 |
17 | CH3COONa | 0.01 | 1:1 | 50 | DMF | 63 |
18 | CH3COONa | 0.01 | 1:1 | 75 | DMF | 72 |
19 | CH3COONa | 0.01 | 1:1 | 130 | DMF | 93 |
20 | CH3COONa | 0.01 | 1:0 without ligand | 130 | DMF | 6 |
21 | CH3COONa | 0.01 | 1:2 | 130 | DMF | 54 |
22 | CH3COONa | 0.01 | 2:1 | 130 | DMF | 56 |
All the other synthesized ligands, [H2L2][OTf]2–[H2L5][I]2, were compared with [H2L1][OTf]2 and the results are shown (Table 7). [H2L1][OTf]2 presented maximum coupled product comparatively. The reason can be associated with the extensive delocalization of electrons in the in situ generated L1 (Fig. 11) that binds with palladium acetate. This conjugation in ligand can make amido nitrogen electron rich that in turn increases the electronic density on palladium catalyst that eventually speeds up the rate of oxidative addition of bromobenzene, thus activating the catalyst towards coupling reaction.
Entry | Ligands | %Yield |
---|---|---|
a Conditions: 3 h, 130 °C, styrene (1.4 eq.) versus halobenzene, Pd(OAc)2:L = 1:1, DMF (2 mL), ligand loading (0.01 mol), Pd(OAc)2 loading (0.01 mol) and NaOAc (4.3 mmol, 3.1 eq.). Isolated yield based on aryl halide. | ||
1 | [H2L1][TfO]2 | 93 |
2 | [H2L2][TfO]2 | 83 |
3 | [H2L3][TfO]2 | 81 |
4 | [H2L4][TfO]2 | 79 |
5 | [H2L5][I]2 | 77 |
Alkyl substituted ligands, [H2L2][OTf]2–[H2L5][I]2, were found less active comparatively. Nevertheless, they showed coupled product in the range of 77 to 83% owing to the inductive effect of ethyl and hexyl groups. The minor variations in product yield can be related to the steric of N-alkylated group of varying degree around the donor amido nitrogen. This catalytic activity order of co-catalysts can also be related with their EHOMO values i.e., greater is the energy of HOMO, greater would be the electron donation from ligand to Pd(II) thus more would be the stability of in situ generated active catalyst.
Substrates with a different range of electron withdrawing to electron donating substituent were coupled under optimum conditions to test the substrate scope of best catalyst system ([H2L1][OTf]2/Palladium acetate). As expected, more activated aryl iodides couple more effectively than aryl bromides and aryl chloride (Table 8, entry 1–8). The high reactivity of aryl iodides are due to small dissociation energy of C–I bond and ease of activation towards Pd(0) catalyst in oxidative addition step.40 Generally coupling of aryl chlorides demand high catalyst loading with low yield of coupled product.41
Entry | RC6H4X | R'CHCH2 | Yield (%) | Time (h) |
---|---|---|---|---|
a Conditions: 130 °C, styrene (1.4 eq.) versus halobenzene, Pd(OAc)2:L = 1:1, NaOAc (4.3 mmol, 3.1 eq.), DMF (2 mL), ligand loading 0.01, Pd(OAc)2 loading (0.01 mol%). Isolated yield based on aryl halide. | ||||
1 | ClC6H5 | C6H5CHCH2 | 67 | 6 |
2 | 4-ClC6H4CH3 | C6H5CHCH2 | 65 | 7 |
3 | 4-ClC6H4NO2 | C6H5CHCH2 | 72 | 6 |
4 | 4-ClC6H4COCH3 | C6H5CHCH2 | 70 | 6 |
5 | I–C6H5 | C6H5CHCH2 | 98 | 4 |
6 | 4-IC6H4CH3 | C6H5CHCH2 | 95 | 5 |
7 | BrC6H5 | C6H5CHCH2 | 93 | 4 |
8 | 4-BrC6H4CH3 | C6H5CHCH2 | 89 | 6 |
9 | 4-BrC6H4OCH3 | C6H5CHCH2 | 87 | 6 |
10 | 4-BrC6H4NO2 | C6H5CHCH2 | 96 | 4.5 |
11 | 4-BrC6H4CHO | C6H5CHCH2 | 92 | 4 |
12 | 4-BrC6H4COCH3 | C6H5CHCH2 | 94 | 4 |
13 | 1-BrC10H7 | C6H5CHCH2 | 85 | 16 |
14 | BrC6H5 | CH2CHCO2C2H5 | 96 | 3.5 |
15 | 4-BrC6H4CH3 | CH2CHCO2C2H5 | 94 | 4 |
16 | 4-BrC6H4OCH3 | CH2CHCO2C2H5 | 93 | 4 |
17 | 4-BrC6H4NO2 | CH2CHCO2C2H5 | 98 | 3 |
18 | 4-BrC6H4CHO | CH2CHCO2C2H5 | 97 | 2 |
19 | 4-BrC6H4COCH3 | CH2CHCO2C2H5 | 98 | 2 |
20 | 1-BrC10H7 | CH2CHCO2C2H5 | 92 | 12 |
Likewise, those aryl halides with electron donating substituents like methoxy, methyl or naphthyl and electron neutral group such as –H showed less reactivity than aryl halide containing electron withdrawing substituents such as nitro, aldo and keto groups (Table 8, entry 1–13). The more electron deficient quaternary carbon of aryl halide better would be the rate of oxidative addition reaction. Similar trend was shown by ethyl acrylate for the above mentioned aryl halides activated to different degrees. However the yield of all coupled products with ethyl acrylate was comparatively more than styrene (Table 8, entry 14–18). The reason can be attributed to the greater polarization of the alkene with more electron-withdrawing adjacent carbonyl group in ethyl acrylate. This polarization enhances the insertion of ethyl acrylate into aryl–palladium bond during catalytic cycle. Moreover, as explained earlier, out of 3.1 eq. sodium acetate, 1.1 eq. of sodium acetate was used for catalytic reaction however remaining 2 eq. of sodium acetate was used to in situ deprotonate the ligand leading to the formation of an effective complex with ligand.
Efforts to synthesize pure palladium complexes with all the ligands, [H2L1][OTf]2–[H2L5][I]2 were proved to be futile owing to strong trans influence by in situ generated deprotonated ligands. The resulted mixtures were attempted to be purified by various analytical techniques but was proved in vain. To full fill the urge of identifying the actual nature of catalyst, standard mercury test was performed. 150 to 300 equivalent of Hg(0) compared to catalytic system was added in the catalytic reactor during coupling reaction. The yield of coupled product was not affected in this test reaction. This result clearly confirmed the in situ generation of homogeneous palladium catalysts and heterogeneous Pd(0) catalysts were not obtained by any opponent way.42,43
The plausible catalytic cycle of one of the reactions between iodobenzene and styrene under the best reaction conditions (mentioned in Table 8) shown in Fig. 12 involved pre-activation of catalyst followed by oxidative addition of palladium in benzene to iodide bond of iodobenzene, Pd(II) π-complex formation, migratory insertion of styrene in palladium and carbon bond, relief of torsional strain with the elimination of beta hydride, another π-complex formation with stilbene and generation of Pd(0) catalyst with reductive elimination. Sodium acetate plays a vital role in regeneration of catalyst.44
Fig. 12 The catalytic cycle showing the role of reagents, ligands and etc., under the best reaction conditions. |
Herein, we performed the critical comparison (mentioned in Table 9) of the catalytic activity (entry 1 to 5)45a–e of this work in entry 6 related to Heck coupling of chlorobenzene and styrene with literature showed that this catalyst is potentially the trademark for the coupling of chlorobenzene with styrene. It gave 67% yield in 6 hours at 130 °C with 1 mol%. The problem with catalysts in entries 1 and 2 catalysts is utilization of too much time for catalytic conversion of chlorobenzene to coupled product. The catalyst in entry 3 yields 70% coupled product in just 85 minutes at 120 °C but with much high catalyst amount i.e. 10 mol%. The best one seems to be in entry 4; utilizes less catalyst at the cost of 20 °C more temperature comparatively. The catalyst in entry 5 is useless for chlorobenzenes. Whereas with respect to catalyst shown in entry 4, our catalysts showed more substrate scope for chlorobenzenes.
Entry | Reactions | Halo-benzene (mmol) | Ligands (L), Pd(OAc)2 mol% | Solvent (ml), base | Time (h) | T (°C) | Y (%) | Ref. |
---|---|---|---|---|---|---|---|---|
a TBAI = tetrabutylammonium iodide, TEA = triethylamine, NMP = N-methyl-2-pyrrolidone. | ||||||||
1 | C6H5Cl + styrene | 1 | DMF, K2CO3 | 12 | 60 | 62 | 45a | |
2 | C6H5Cl + styrene | 0.5 | Pd(OAc)2: Dave-Phos (2:6) 2 | 1,4- dioxane, TBAE | 24 | 80 | 99 | 45b |
3 | C6H5Cl + styrene | 1 | K2CO3, DMF | 85 min | 120 | 70 | 45c | |
4 | C6H5Cl + styrene | 1.5 | NMP, Ca(OH)2 | 6 | 150 | 62 | 45d | |
5 | C6H5Cl + styrene | 1 | NMP, K2CO3 | 2.5 | 120 | Trace | 45e | |
6 | C6H5Cl + styrene | 400 | Pd (OAc)2:[H2L1][TfO]2 (1:1) | DMF, NaOAc | 6 | 130 | 67 | This work |
7 | C6H5I + styrene | 1 | DMF, K2CO3 | 12 | 60 | 98 | 45a | |
8 | C6H5I + styrene | 1 | DMF, Na2CO3 | 20 | 145 | 95 | 45f | |
9 | C6H5I + styrene | 1 | DMF, K2CO3 | 20 | 130 | 90 | 45g | |
10 | C6H5I + styrene | 1 | DMF, Et3N | 40 min | 120 | 97 | 45h | |
11 | C6H5I + styrene | 1 | NMP, K2CO3 | 2.5 | 120 | 96 | 45c | |
12 | C6H5I + styrene | 400 | Pd (OAc)2:[H2L1][TfO]2 (1:1) | DMF, NaOAc | 4 | 130 | 98 | This work |
13 | C6H5Br + alkyl acrylate | 1 | DMF, Na2CO3 | 20 | 145 | 92 | 45f | |
14 | C6H5Br + alkyl acrylate | 1 | H2O, K2CO3 | 5 | 50 | 95 | 45i | |
15 | C6H5Br + alkyl acrylate | 400 | Pd (OAc)2:[H2L1][TfO]2 (1:1) | DMF, NaOAc | 3.5 | 130 | 96 | This work |
We observed a probable limitation of our new catalytic system entry 12 as it was not found to be the best for the Heck coupling of iodobenzenes with styrene. The published literature 45c,h (entry 10 and 11) proved it inferior to them with respect to catalyst loading but it still looks reasonable when compared to entries 7–9 (ref. 45a,f,g) of the above table.
The comparison of our result with literature with regard to the Heck coupling of bromobenzene with alkyl acrylate (entries 13–15) 45f,i,j suggested that the catalyst system generated in this work (entry 19) proved to be an excellent attempt specially with respect to very less time utilization (3.5 hours). Likhar et al.,45f got 92% of coupled product with 0.01 mol% but in 20 h and at 145 °C. In 2017, Abdol R. Hajipour45i synthesized highly active catalyst and got 95% yield at only 50 °C but using more time than our catalytic system i.e. 5 hours. Wang et al., 45j used 0.005 mol% of catalyst but with only 4% yield. The other remarkable feature of our catalyst (entry 16) was the use of 400 mmol of halobenzene transformed into 96% of coupled product compared to literature (1 mmol) (Table 9).
Footnote |
† Electronic supplementary information (ESI) available. CCDC 1955342, 1955343, 1955344, 1955349 and 1961686. For ESI and crystallographic data in CIF or other electronic format see DOI: 10.1039/c9ra07912b |
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