Roles of Hydrogen Bonding in Proton Transfer to κ^P,κ^N,κ^P-N(CH₂CH₂PⁱPr₂)₂-Ligated Nickel Pincer Complexes

Abstract

The nickel PNP pincer complex (^iPrPNP)NiPh (^iPrPNP = κ^P,κ^N,κ^P-N(CH₂CH₂PⁱPr₂)₂) was prepared by reacting (^iPrPNP)NiBr with PhMgCl or deprotonating [(^iPrPN^HP)NiPh]Y (^iPrPN^HP = κ^P,κ^N,κ^P-HN(CH₂CH₂PⁱPr₂)₂; Y = Br, PF₆) with KO^tBu. The byproducts of the PhMgCl reaction were identified as [(^iPrPN^HP)NiPh]Br and (^iPrPNP′)NiPh (^iPrPNP′ = κ^P,κ^N,κ^P-N(CH=CHPⁱPr₂)(CH₂CH₂PⁱPr₂)). The methyl analog (^iPrPNP)NiMe was synthesized from the reaction of (^iPrPNP)NiBr with MeLi, although it was contaminated with (^iPrPNP′)NiMe due to ligand oxidation. Protonation of (^iPrPNP)NiX (X = Br, Ph, Me) with various acids, such as HCl, water, and MeOH, was studied in C₆D₆. Nitrogen protonation was shown to be the most favorable process, producing a cationic species [(^iPrPN^HP)NiX]⁺ with the NH moiety hydrogen-bonded to the conjugate base (i.e., Cl^–, HO^–, or MeO^–). Protonation of the Ni–C bond was observed at room temperature with (^iPrPNP)NiMe, whereas at 70 °C with (^iPrPNP)NiPh, both resulting in [(^iPrPN^HP)NiCl]Cl as the final product. Protonation of (^iPrPNP)NiBr was complicated by site exchange between Br^– and the conjugate base and by the degradation of the pincer complexes. Indene, which lacks hydrogen-bonding capability, was unable to protonate (^iPrPNP)NiPh and (^iPrPNP)NiMe, despite being more acidic than water and MeOH. Neutral and cationic nickel pincer complexes involved in this study, including (^iPrPNP′)NiBr, (^iPrPNP)NiPh, (^iPrPNP′)NiPh, (^iPrPNP)NiMe, [(^iPrPN^HP)NiPh]Y (Y = Br, PF₆, BPh₄), [(^iPrPN^HP)NiPh]₂[NiCl₄], [(^iPrPN^HP)NiMe]Y (Y = Cl, Br, BPh₄), [(^iPrPN^HP)NiBr]Br, and [(^iPrPN^HP)NiCl]Cl, were characterized by X-ray crystallography.

Introduction

The advances of metal–ligand bifunctional catalysis have provided the momentum for the recent surge in developing base metal-catalyzed (de)hydrogenation reactions.¹⁻⁹ The key to the success of these reactions is often attributed to ligand participation in proton-transfer steps, which helps activate substrates while deemphasizing the roles that metals need to play. One particularly effective and popular ligand system has the general formula HN(CH₂CH₂PR₂)₂ (abbreviated here as ^RPN^HP),¹⁰ which is commonly referred to as PNP pincer when the ligand adopts the meridional coordination mode. Over the past few years, Ni,¹¹⁻¹⁴ Co,^11,15−21 Fe,²²⁻³⁰ and Mn complexes³¹⁻³³ bearing the PNP pincer ligands or their deprotonated form [N(CH₂CH₂PR₂)₂]⁻ (abbreviated here as ^RPNP) have been successfully produced, many of which have shown excellent catalytic activity for hydrogenation,^{16,21,25−42} dehydrogenation,^{16,22,34,35,43−52} and related transfer hydrogenation reactions.^20,53 Although the presence of the NH group is not always necessary,⁵³ especially for the reduction of olefins^12,16 and CO₂,⁵⁴⁻⁵⁶ its function in many (de)hydrogenation processes has been well established.^{16,26,38,44,57} As illustrated by a generalized mechanism for carbonyl reduction (Scheme 1; for clarity, other ligands are removed), H⁺/H^– transfer from nitrogen/metal to the O=C bond generates the alcohol product and an amido complex, which activates H₂ to close the catalytic cycle. The reverse process, namely, alcohol dehydrogenation, proceeds via H⁺/H^– transfer from the alcohol molecule to the amido complex. Although the key features have been captured, the missing piece of the mechanistic picture is an adduct of the alcohol molecule and the amido species linked by a hydrogen-bonding interaction. According to density functional theory calculations,^34,43,58 such an intermediate represents a local minimum in energy and plays a critical role in H₂ activation (for hydrogenation) or elimination (for dehydrogenation).^57,59 Isolation or even spectroscopic observation of this specific intermediate has proven to be challenging or may not even be possible, yet understanding its bonding and reactivity is essential for the further development of the catalytic reactions.

Scheme 1. Hydrogen Transfer in (De)Hydrogenation Reactions Catalyzed by PNP Pincer Complexes.

In this work, we chose the nickel PNP pincer system as the platform to probe the hydrogen-bonding interaction in question. We simplified the research problem by focusing on the protonation of (^iPrPNP)NiX (X = Br, Ph, Me) with various Brønsted acids, including methanol and water (eq 1). In particular, products resulting from methanol protonation should mimic the alcohol adduct depicted in Scheme 1. In addition to examining different acids, we varied the nickel-bound ligand X with an objective to study its effect on the protonation reaction.

1

Results and Discussion

Synthesis and Characterization of Nickel Phenyl Complexes

The synthesis of the nickel bromide complex (^iPrPNP)NiBr (1) was already reported by the Arnold group in 2011.¹¹ We thus turned our initial attention to the target phenyl complex (^iPrPNP)NiPh (2). Group 10 metal phenyl complexes supported by a pincer ligand are often readily prepared by treating the corresponding metal halide complexes with PhLi⁶⁰⁻⁶³ or PhMgX (X = Cl, Br).⁶⁴⁻⁶⁶ Applying this synthetic strategy to the nickel PNP pincer system is, however, nontrivial. The room-temperature reaction of 1 with PhLi did not go to completion unless more than 3 equiv of PhLi were added, in which case a complicated mixture was obtained. Similar phenomena were observed when Ph₂Zn was employed in place of PhLi. Using PhMgCl as the source of the phenyl group also resulted in multiple products but needed only 1 equiv of the Grignard reagent to fully convert 1. Fortunately, the solubility difference of the products in pentane made separation possible (see Experimental Section for details). In addition to the anticipated complex 2, a cationic nickel phenyl complex [(^iPrPN^HP)NiPh]Br ([2^H]Br) and a neutral nickel phenyl complex bearing a dehydrogenated PNP pincer ligand (complex 2′) were isolated (eq 2). Control experiments indicated that when exposed to air, both 1 and 2 decomposed rapidly, resulting in a mixture of a cationic species, a complex with a dehydrogenated PNP pincer ligand, and other unidentified species. Efforts were thus made to avoid contact with oxygen and moisture during the synthesis of 2. Unfortunately, [2^H]Br and 2′ remained present in the crude product.

2

Schneider and co-workers have previously mentioned low selectivity for the reaction between [(^iPrPN^HP)PdCl]PF₆ and a phenyl Grignard reagent.⁶⁷ They have therefore developed an alternate route to [(^iPrPN^HP)PdPh]PF₆ using (TMEDA)PdPhI (TMEDA = Me₂NCH₂CH₂NMe₂), ^iPrPN^HP, and AgPF₆. Additionally, they have shown that deprotonation of [(^iPrPN^HP)PdPh]PF₆ by KO^tBu provides the neutral phenyl complex (^iPrPNP)PdPh in good yield. We found that this strategy could also be successfully implemented using (TMEDA)NiPhI as the starting material for the synthesis of [(^iPrPN^HP)NiPh]PF₆ ([2^H]PF₆) and 2 (Scheme 2). Alternatively, 2 could be isolated from deprotonation of [2^H]Br with KO^tBu.

Scheme 2. Independent Synthesis of Complex 2.

To confirm the formation of 2′, a nickel bromide complex supported by the dehydrogenated PNP pincer ligand (complex 1′; see Scheme 3) was prepared first following the procedure established for the dehydrogenation of (^tBuPNP)CoCl,¹⁹ although the isolated yield was low (8%). Synthesis of 2′ from 1′ and PhMgCl was relatively straightforward, reflecting higher stability of 1′ and 2′ toward oxygen and moisture. Previous studies of (^iPrPNP)Ru(PMe₃)H have suggested that the PNP pincer ligand, when dehydrogenated, can be restored in the presence of H₂ (1 bar).^68,69 In our work, exposing a 95:5 mixture of 1 and 1′ (in C₆D₆) to 2 bar of H₂ over a period of 5 days showed no sign of hydrogenation of 1′ to 1. The phenyl complex 2′ also resisted hydrogenation under similar conditions.

Scheme 3. Independent Synthesis of Complex 2′.

The nickel phenyl complexes described above were characterized by NMR spectroscopy and elemental analysis. Consistent with the symmetries of the molecules, 2 displays two sets of CH₃ resonances in its ¹H and ¹³C{¹H} NMR spectra, whereas 2′, [2^H]Br, and [2^H]PF₆ each show four different sets of CH₃ resonances. The higher symmetry of 2 is further manifested by the observation of only one carbon resonance for the CH groups of the pincer ligand. In contrast, two pincer CH resonances are located for 2′, [2^H]Br, and [2^H]PF₆. As expected, the ³¹P{¹H} NMR spectrum of 2′ displays an AB quartet for the two inequivalent phosphorus nuclei with a large coupling constant of 259.7 Hz.

The structures of 2, 2′, [2^H]Br, and [2^H]PF₆ were further established by X-ray crystallography. The dehydrogenated PNP pincer ligand in 2′ is evident from a relatively short C(1)–C(2) distance of 1.392(3) Å (Figure 1 and Table 1), which is best described as a C=C bond.^13,19 Its C(3)–C(4) bond [1.462(3) Å], although shorter than the C(1)–C(2) [1.517(2) Å] and C(3)–C(4) [1.514(2) Å] bonds in 2 (Figure 2), is most consistent with a single bond. The phenyl group in 2 and 2′ adopts a conformation almost perpendicular to the coordination plane; the dihedral angles between the least-square planes P(1)–P(2)–N(1)–Ni and C(17) through C(22) were measured to be 76.34(4) and 75.60(5)° for 2 and 2′, respectively. The sum of angles about the nitrogen (∑N) is 354.05° for 2 and 359.49° for 2′, suggesting that the nitrogen lone-pair electrons are delocalized into the neighboring π-system and/or nickel. The cations of [2^H]Br (Figure 3) and [2^H]PF₆ (Figure 4) are almost structurally identical to each other with only slight differences in Ni–P bond lengths and P–Ni–P angle (Table 1). Like 2 and 2′, the phenyl group in [2^H]Br and [2^H]PF₆ is nearly perpendicular to the coordination plane, presumably to minimize the steric clash with the isopropyl groups. The Ni–N bonds of [2^H]Br [1.985(2) Å] and [2^H]PF₆ [1.999(3) Å] are substantially longer than those of 2 [1.8932(11)Å] and 2′ [1.9139(14) Å], which reflects the difference between an amine and an amido donor. Perhaps the most notable structural feature of [2^H]Br is the hydrogen-bonding interaction (Table S1) between the NH group and the counterion, bromide [NH···Br = 3.370(3) Å]. It is interesting to note that weaker hydrogen bonds also exist in [2^H]PF₆ between the NH moiety and the fluorine atoms of PF₆^– [NH···F = 3.021(7) Å] (Figure 4 and Table S1). The extent of hydrogen-bonding interaction in the solid state was probed by IR spectroscopy, which showed a broad band at 3351 cm^–1 for [2^H]Br and a sharp band at 3249 cm^–1 in the case of [2^H]PF₆, both assigned to the N–H bond stretch.

Figure 1.

Oak Ridge thermal ellipsoid plot (ORTEP) drawing of (^iPrPNP′)NiPh (2′) at the 50% probability level. Hydrogen atoms except those attached to the pincer backbone are omitted for clarity.

Table 1. Selected Bond Lengths (Å) and Angles (deg) for the Nickel Phenyl Complexes.

	(iPrPNP)NiPh (2)	(iPrPNP′)NiPh (2′)	[(iPrPNHP)NiPh]Br ([2H]Br)	[(iPrPNHP)NiPh]PF6 ([2H]PF6)	[(iPrPNHP)NiPh]BPh4 ([2H]BPh4)a	[(iPrPNHP)NiPh]2[NiCl4] ([2H]2[NiCl4])b
Ni–N(1)	1.8932(11)	1.9139(14)	1.985(2)	1.999(3)	1.997(2)	1.9806(18)
Ni–C(17)	1.9163(13)	1.9066(16)	1.909(3)	1.900(3)	1.903(2)	1.906(2)
Ni–P(1)	2.1513(4)	2.1743(5)	2.1801(8)	2.1960(6)	2.1780(8)	2.1812(5)
Ni–P(2)	2.1492(4)	2.1675(5)	2.1769(8)	2.1960(6)	2.1827(7)	2.1760(6)
C(1)–C(2)	1.517(2)	1.392(3)	1.511(4)	1.521(3)	1.512(4)	1.518(3)
C(3)–C(4)	1.514(2)	1.462(3)	1.514(4)	1.521(3)	1.518(4)	1.506(4)
P(1)–Ni–P(2)	172.006(15)	171.250(19)	173.87(3)	168.05(4)	174.55(3)	172.04(2)
C(17)–Ni–N(1)	179.22(5)	178.21(7)	179.71(12)	175.85(13)	178.88(11)	177.26(9)
dihedral anglec	76.34(4)	75.60(5)	75.45(8)	84.99(2)	75.43(7)	79.92(5)

^a[2^H]BPh₄ crystallizes as [2^H]BPh₄·3/2THF.

^b[2^H]₂[NiCl₄] crystallizes as [2^H]₂[NiCl₄]·4C₆D₆·1/2H₂O.

^cAngle between the least-square planes P(1)–P(2)–N(1)–Ni and C(17) through C(22).

Figure 2.

ORTEP drawing of (^iPrPNP)NiPh (2) at the 50% probability level. Hydrogen atoms are omitted for clarity.

Figure 3.

ORTEP drawing of [(^iPrPN^HP)NiPh]Br ([2^H]Br) at the 50% probability level. Hydrogen atoms except the one attached to the nitrogen are omitted for clarity.

Figure 4.

ORTEP drawing of [(^iPrPN^HP)NiPh]PF₆ ([2^H]PF₆) at the 50% probability level. Hydrogen atoms except the one attached to the nitrogen are omitted for clarity. The PF₆ counterion is disordered in the fluorine atoms.

Synthesis of the cationic nickel phenyl complex devoid of hydrogen bonds is possible. This was accomplished by a salt metathesis reaction between [2^H]Br and NaBPh₄, as illustrated in eq 3. The product [2^H]BPh₄, when recrystallized in tetrahydrofuran (THF)-pentane, provides a structure without hydrogen-bonding interaction (Figure 5) despite the fact that THF molecules are present in the crystal lattice. In contrast, our previous crystallographic analysis of an iron PNP pincer complex trans-(^iPrPN^HP)Fe(CO)Br₂ showed that a co-crystallized THF molecule was hydrogen-bonded to the NH group.²⁵ Nevertheless, the lack of hydrogen bonds in [2^H]BPh₄ appears to have a negligible impact on key angles and distances (Table 1) as well as the orientation of the phenyl group. One might have anticipated that without the N–H···X interaction, the nitrogen is less amido like, resulting in a longer Ni–N bond. The IR spectrum of [2^H]BPh₄ (solid) shows a sharp N–H stretching band at 3181 cm^–1, further supporting that hydrogen bonds are absent in this molecule.

3

Figure 5.

ORTEP drawing of [(^iPrPN^HP)NiPh]BPh₄ ([2^H]BPh₄) at the 50% probability level. THF molecules (co-crystallized with [2^H]BPh₄) and all hydrogen atoms except the one attached to the nitrogen are omitted for clarity.

Because the reaction of 1 with PhMgCl (eq 2) involves two different halides, there is a possibility that the counterion for the cationic phenyl complex could be a mixture of Br^– and Cl^–. However, both elemental analysis and X-ray study (barring selective crystallization of one compound) support the [2^H]Br formulation. Pure [2^H]Cl, which was obtained from protonation of 2 by HCl (eq 4), gives similar but distinctively different NMR spectra. In particular, the NH resonance is shifted from 5.35 ppm for [2^H]Br (in CD₃CN) to 6.25 ppm for [2^H]Cl, consistent with a stronger hydrogen bond formed by a more electronegative halide. The equilibrium for the halide exchange (eq 5, approached from both directions) apparently lies far from the [2^H]Br/MgCl₂ side, likely driven by the more negative Gibbs free energy of formation for MgCl₂.⁷⁰

4

5

The aforementioned cationic nickel phenyl complexes are soluble in polar solvents, such as acetonitrile and acetone. In benzene, the ones with a strong hydrogen-bonding interaction ([2^H]Cl and [2^H]Br) are sparsely soluble, whereas the ones with weak or no hydrogen-bonding interaction ([2^H]PF₆ and [2^H]BPh₄) are insoluble. Interestingly, a concentrated solution of [2^H]Cl in C₆D₆ left under an argon atmosphere for 2 weeks yielded some single crystals, which were analyzed by X-ray crystallography as [2^H]₂[NiCl₄] (Figure 6). As summarized in Table 1, the structural parameters of the cation are virtually the same as those of other cationic nickel phenyl complexes. The chlorides of [NiCl₄]^2– are all hydrogen-bonded, two with the NH moieties [NH···Cl = 3.327(2) Å] (Table S1) and the other two with co-crystallized water molecules [OH···Cl = 3.321(5) Å].

Figure 6.

ORTEP drawing of [(^iPrPN^HP)NiPh]₂[NiCl₄] ([2^H]₂[NiCl₄]) at the 50% probability level. Co-crystallized C₆D₆ and H₂O molecules and all hydrogen atoms, except the one attached to the nitrogen, are omitted for clarity.

In solution, the rotation of the phenyl group appears to be restricted, as judged by NMR spectroscopy. Complex [2^H]PF₆ or [2^H]BPh₄ dissolved in CD₃CN exhibited two different resonances for the ortho carbons. Although [2^H]Cl or [2^H]Br in CD₃CN showed only one ortho carbon resonance as a triplet, the solution in C₆D₆ gave a ¹H NMR spectrum with two aromatic hydrogen resonances attributable to the ortho hydrogens.

Synthesis and Characterization of Nickel Methyl Complexes

Complex (^iPrPNP)NiMe (3) has been previously prepared by treating [(^iPrPN^HP)NiBr]Br with 2.5 equiv of MeLi.⁷¹ Our attempts to repeat this synthesis were, however, unsuccessful; other synthetic routes (for analogous complexes^65,72−78) were thus pursued. Under the conditions used for the synthesis of 2 (eq 2), 1 reacted sluggishly with MeMgBr, as inferred by the persistent green characteristic of 1. Extending the reaction time (from 1 to 17 h) eventually led to the disappearance of the green color, although NMR analysis of the crude product revealed a very complicated mixture. A more successful route involved the reaction of 1 with MeLi in diethyl ether (eq 6), which was previously used for the synthesis of (^CyPNP)NiMe bearing cyclohexyl groups as the phosphorus substituents.¹² The isolated material was confirmed as the desired compound 3 although contaminated with a small amount of byproduct 3′. The percentage of 3′ varied from batch to batch (5–20%), likely due to the high sensitivity of 3 toward the adventitious O₂ present during the synthesis. The amount of cationic nickel methyl species was negligible (<1%). The ³¹P{¹H} NMR spectrum of the isolated material shows a singlet at 68.81 ppm for 3 (in C₆D₆) along with a small AB quartet at 62.71 and 49.86 ppm (J_AB = 275.4 Hz) for 3′. As expected for 3, the nickel-bound methyl group appears in the upfield region, featuring triplets at −0.59 (J_P–H = 8.6 Hz) and −26.32 ppm (J_P–C = 25.6 Hz) for the proton and carbon resonances, respectively.

6

Cationic nickel methyl complexes [3^H]Br and [3^H]Cl were prepared by generating 3 in situ followed by protonation with MeOH (Scheme 4). Instead of bearing MeO^– as the counterion, the isolated products contain the original halide hydrogen-bonded to the NH moiety (vide infra). The byproduct LiOMe is presumably stabilized by MeOH through solvation. The halide can be removed via a salt metathesis reaction with NaBPh₄, as demonstrated by a successful synthesis of [3^H]BPh₄ from 1.

Scheme 4. Synthesis of Cationic Nickel Methyl Complexes.

The ¹H and ¹³C{¹H} NMR spectra of [3^H]Cl, [3^H]Br, and [3^H]BPh₄ (in CD₃CN) show more splittings than 3 (in C₆D₆) due to reduced symmetry. Chemical shifts for the three cations differ only slightly. The most significantly shifted resonances are the NH hydrogen observed as a broad triplet ([3^H]Cl, 5.61 ppm; [3^H]Br, 4.92 ppm; [3^H]BPh₄, 3.57 ppm) and NiCH₃ carbon also seen as a triplet ([3^H]Cl, −24.27 ppm; [3^H]Br, −24.04 ppm; [3^H]BPh₄, −23.73 ppm). The trend for the NH chemical shifts can be rationalized by the extent of hydrogen-bonding interaction, which follows the order [3^H]Cl > [3^H]Br > [3^H]BPh₄.

The four nickel methyl complexes (3, [3^H]Cl, [3^H]Br, and [3^H]BPh₄) in their solid state were studied by X-ray crystallography (Figure 7). As summarized in Table 2, there is very little structural variation in the cation of [3^H]Cl, [3^H]Br, and [3^H]BPh₄. Similar to the phenyl series, an hydrogen-bonding interaction (Table S1) is present between the NH moiety and Cl^–/Br^– [NH···Cl = 3.140(2) Å, NH···Br = 3.010(16) Å] but absent when the counterion is BPh₄^–. This was further supported by IR spectroscopy, which revealed a very broad N–H stretching band for [3^H]Cl (3393 cm^–1) and [3^H]Br (3399 cm^–1), whereas a relatively sharp band for [3^H]BPh₄ (3189 cm^–1). Compared to the neutral methyl complex 3, the Ni–N and Ni–P bonds of the cationic species are elongated by 0.09–0.11 and 0.02–0.05 Å, respectively. Without the proton, the amido nitrogen of 3 is nearly flat (∑N = 353.05°), similar to that of the phenyl complex 2 (∑N = 354.05°) but less planar than that observed for the complexes supported by the dehydrogenated PNP pincer ligand (2′, ∑N = 359.49°; 1′, ∑N = 359.1 or 359.7°; see Supporting Information for details). Interestingly, the related palladium complexes (^iPrPNP)PdX (X = Cl, ∑N = 337.4°; X = Me, ∑N = 345.7°)⁶⁷ as well as the nickel bromide complex 1 (∑N = 348.30 or 348.35°)¹¹ were reported to have a more pyramidal amido nitrogen.

Figure 7.

ORTEP drawings of nickel methyl complexes at the 50% probability level. Hydrogen atoms except the one attached to the nitrogen are omitted for clarity.

Table 2. Selected Bond Lengths (Å) and Angles (deg) for Nickel Methyl Complexes.

	(iPrPNP)NiMe (3)	[(iPrPNHP)NiMe]Cl ([3H]Cl)	[(iPrPNHP)NiMe]Br ([3H]Br)	[(iPrPNHP)NiMe]BPh4 ([3H]BPh4)
Ni–N(1)	1.8943(17)	1.9897(13)	1.9866(14)	2.0081(12)
Ni–C(17)	1.968(2)	1.9488(17)	1.9756(18)	1.9608(15)
Ni–P(1)	2.1471(6)	2.1806(4)	2.1737(4)	2.1814(4)
Ni–P(2)	2.1504(6)	2.1744(4)	2.1810(5)	2.1976(4)
C(1)–C(2)	1.516(3)	1.518(2)	1.517(2)	1.519(2)
C(3)–C(4)	1.519(3)	1.520(2)	1.518(2)	1.517(2)
P(1)–Ni–P(2)	169.25(2)	172.998(17)	172.966(18)	173.884(16)
C(17)–Ni–N(1)	171.23(10)	178.10(8)	178.10(8)	177.49(6)

Protonation of the Nickel PNP Pincer Complexes

Since the nickel halide complexes lack acid-labile Ni–C bonds, for simplicity, their protonation reactions were investigated first (Scheme 5). As anticipated, adding 1 equiv of HCl (2 M solution in Et₂O) to the chloride complex 4 provided [4^H]Cl quantitatively as a result of nitrogen protonation. No hydride species was observed during the reaction. Protonation of the metal is likely to be kinetically and thermodynamically unfavorable,⁷⁹⁻⁸¹ as it would require a geometric reorganization at nickel and a formal oxidation of Ni(II) to Ni(IV). The product [4^H]Cl was synthesized independently by mixing NiCl₂ with ^iPrPN^HP and was characterized by NMR spectroscopy and elemental analysis. IR studies showed that the N–H stretching band was too broad to be accurately located. An N–H···Cl interaction is observed in the crystal structure (NH···Cl = 3.109(8) and 3.152(8) Å for the two independent molecules, Table S1). Furthermore, [4^H]Cl displays a broad proton resonance at 7.88 ppm (in CDCl₃) or 9.79 ppm (in C₆D₆), which is in the region for an NH group participating in strong hydrogen-bonding interaction.⁸² Protonation of the bromide complex 1 in C₆D₆ with HBF₄·Et₂O also yielded a cationic complex exclusively. The NH resonance of the product ([1^H]BF₄) was found at 4.44 pm, implying weak hydrogen-bonding interaction. By comparison, the NH resonance of [1^H]Br, which forms hydrogen bonds between the NH group and the bromide (NH···Br = 3.331(15) and 3.301(15) Å for the two independent molecules), appears at 8.74 ppm (in C₆D₆). Protonation of 1 with 1 equiv of HCl is more complicated because of facile Cl^–/Br^– exchange at the nickel and NH sites. Comparing the NMR data of the cationic complexes described in this study (nine total) suggests that for these cationic species, the ³¹P chemical shift is primarily determined by what is bound to nickel. This allowed us to determine the ratio of [4^H]X/[1^H]X to be 2:1, consistent with the notion that nickel forms a stronger bond with a harder donor atom (i.e., Cl as opposed to Br).^83,84

Scheme 5. Protonation of Nickel Halide Complexes.

Complex 1 is surprisingly sensitive to water. When treated with 5 equiv of degassed H₂O, the solution of 1 in C₆D₆ exhibited a broad ³¹P resonance at 66.53 ppm (85%) along with a sharp ³¹P resonance at 50.15 ppm (15%). Assuming that the former is a weighted average of the chemical shifts of 1 (68.33 ppm) and its protonated form [1^H]⁺ (58.2 ppm), we estimated 15% of 1 being converted to [1^H]OH (Scheme 6) or perhaps [1^H]OH(H₂O)_n, in which a more elaborate hydrogen-bonding network is established with water. The resonance at 50.15 ppm is tentatively assigned to an isomer of [1^H]OH with a Br^–/OH^– swap. Isolating this minor species was not possible because the mixture decomposed readily by releasing the free PNP pincer ligand (−1.04 ppm). It is possible that the nickel hydroxide species forms a dimer bridged by the OH groups. In fact, related nickel hydroxide complexes bearing a pincer ligand are known to be unstable.^85,86

Scheme 6. Reaction of 1 with H₂O.

The reaction of 1 with MeOH (1–10 equiv) was quite similar, forming products consistent with [(^iPrPN^HP)NiBr]OMe and its isomer [(^iPrPN^HP)NiOMe]Br as well as the free PNP pincer ligand. The ¹H NMR spectrum of the reaction mixture also displayed an emerging triplet at −19.16 ppm (J_P–H = 62.0 Hz), suggesting the formation of a nickel hydride species. It is possible that [(^iPrPN^HP)NiOMe]Br proceeds via β-hydride elimination to yield [(^iPrPN^HP)NiH]Br.⁸⁷

Nickel–carbon bonds are susceptible to cleavage by acids.⁸⁸ Complex 2 specifically may undergo protonation of the phenyl group in parallel with or in competition with protonation of the nitrogen atom. Considering that a coordinating anion such as Cl^– is needed to stabilize nickel following phenyl protonation, we used HCl as the acid for the protonation study. Judging from the NMR spectra, the reaction between 2 and HCl (2 M solution in Et₂O) in a 1:1 stoichiometry led rapidly and cleanly to [2^H]Cl (Scheme 7). There was no evidence suggesting that a neutral or cationic nickel chloride complex was produced. Phenyl protonation would eventually take place if 2 equiv of HCl were initially added to 2; however, this process was shown to be extremely slow at room temperature, converting ∼50% of the newly formed [2^H]Cl to [4^H]Cl over a period of 3 weeks. Raising the temperature to 70 °C accelerated the second protonation step, resulting in full conversion to [4^H]Cl within 24 h. As one might have expected, using a substoichiometric amount of HCl (e.g., 0.5 equiv) generated a mixture of 2 and [2^H]Cl. Interestingly, the phosphorus resonances of these two species are significantly broad, presumably due to a rapid interconversion. In an attempt to test if [4^H]Cl was generated via elimination of Ph–H from [2^H]Cl followed by protonation of the resulting nickel chloride complex 4, pure [2^H]Cl was dissolved in C₆D₆ and CD₃CN (for easier detection of benzene) and then heated to 70 °C. In both cases, no Ph–H elimination was observed after monitoring the samples for 3 days.

Scheme 7. Protonation of 2 by HCl.

Treatment of 2 with a weak acid, such as MeOH or H₂O, provided a rapidly equilibrated mixture of 2 and a cationic nickel phenyl complex. As illustrated by the NMR titration of 2 with MeOH (Figure 8), >10 equiv of MeOH are required for complete protonation of 2. Unlike the bromide complex 1, the mixture of 2 and H₂O (5 equiv) in C₆D₆ showed no sign of degradation to the free PNP pincer ligand. This can be explained by the fact that the phenyl group is unable to dissociate from nickel (or protonated by H₂O). Hydrogen-bonding interaction is critical to the protonation process. Because our reactions were carried out in C₆D₆, pK_a values measured in dimethyl sulfoxide cannot be used to predict the extent of protonation. For instance, indene (pK_a = 20.1),⁸⁹ which is more acidic than MeOH (pK_a = 29.0) and H₂O (pK_a = 31.4)⁹⁰ but lacks hydrogen-bonding capability, failed to protonate 2.

Figure 8.

³¹P{¹H} NMR spectra of 2 (in C₆D₆) with various amounts of MeOH added.

Replacing the phenyl group with a more basic methyl group should enhance the reactivity of the Ni–C bond toward acids. Indeed, protonation of complex 3 by HCl (2 M solution in Et₂O) was shown to proceed via two different routes (Scheme 8): nitrogen protonation first (route 1) or methyl protonation first (route 2). With a large excess of HCl (>2 equiv), 3 was fully converted to [4^H]Cl with a concomitant release of CH₄. When 3 was treated with only 1 equiv of HCl, [3^H]Cl was obtained as the major product (75%) along with 4 observed as the minor product (25%). Control experiments showed that CH₄ elimination from [3^H]Cl was not feasible even at 70 °C, ruling out the possibility that 4 was generated from [3^H]Cl. A separate NMR experiment established a rapid protonation of [3^H]Cl by HCl to give [4^H]Cl and CH₄. Evidently, [4^H]Cl is more acidic than [3^H]Cl because the equilibrium in eq 7 heavily favors [3^H]Cl and 4 (tested from both directions). Given these results, one might propose that 3 undergoes nitrogen protonation first, followed by methyl protonation to yield [4^H]Cl (route 1), which in turn reacts with the remaining 3 to give [3^H]Cl and 4. However, this mechanism would require protonation of the [3^H]Cl methyl group by HCl and protonation of the 3 nitrogen atom by [4^H]Cl to be faster than direct methyl protonation of 3 by HCl, which seems unlikely. It was noted that adding 2 equiv of HCl to 3 in C₆D₆ caused a color change of the solution from orange to yellow (for [4^H]Cl) via a transient green color (for 4). This further supports the viability of route 2 by which methyl protonation precedes nitrogen protonation, although it is still kinetically less competitive than route 1. The protonation study was also carried out using 0.5 equiv of HCl, which yielded a mixture of 3, [3^H]Cl, and 4. In contrast to the sharp phosphorous resonance attributed to 4, the spectral lines for 3 and [3^H]Cl appeared quite broad, implying a rapid process that allows these two species to interconvert.

7

Scheme 8. Two Parallel Pathways for the Protonation of 3 by HCl.

Complex 3 behaves similarly to phenyl complex 2 when reacting with weak acids. Addition of MeOH or H₂O to a solution of 3 in C₆D₆ resulted in partial protonation of 3 to a cationic nickel methyl species. NMR titration experiments indicated that a complete protonation of 3 was accomplished with ∼7 equiv of MeOH (Figure S49), supporting the notion that 3 is more basic than 2. The protonation result is not surprising, given the success of making cationic nickel methyl complexes from in situ generated 3 dissolved in MeOH (Scheme 4). Once again, despite being more acidic than MeOH and H₂O, indene exhibited no reactivity toward 3.

Conclusions

In this work, we have shown the propensity of (^iPrPNP)NiX (X = Br, Ph, Me) to undergo nitrogen protonation, even in the presence of a weak Brønsted acid, such as water or MeOH. The reaction is primarily driven by the hydrogen-bonding interaction formed between the NH group and the conjugate base. Halides, which could come from the employed Brønsted acid (e.g., HCl) or the starting pincer complex (e.g., (^iPrPNP)NiBr), appear to form the strongest interaction with the NH group. Thus, the synthesis of (^iPrPNP)NiPh and (^iPrPNP)NiMe from (^iPrPNP)NiBr is always plagued by the formation of a cationic byproduct bearing N–H···Br bonds (eq 2), likely due to nitrogen protonation by adventitious water, followed by OH^–/Br^– exchange. Similarly, the degradation of (^iPrPNP)NiBr in the presence of water (Scheme 6) or MeOH is initiated by nitrogen protonation and facilitated by the exchange of the nickel-bound Br^– with OH^– or MeO^–. The nitrogen protonation and halide exchange steps can, however, be utilized to make [(^iPrPN^HP)NiMe]X (X = Cl, Br) from (^iPrPNP)NiX and MeLi following MeOH addition (Scheme 4). The Ni–C bond in (^iPrPNP)NiPh and (^iPrPNP)NiMe becomes labile only when a strong acid, such as HCl, is added, and in the former case, an elevated temperature of 70 °C is required to cleave the Ni–C_sp2 bond (Scheme 7). We believe our results have important implications in the understanding of the stability of catalysts containing an ^RPN^HP- or ^RPNP-type pincer ligand, especially for reactions that either use or generate alcohols and for processes that contain water and/or halides. Our future work in this area will be focused on other PNP pincer systems to examine the generality of our observations. As far as catalytic reactions are concerned, it will also be interesting to see if replacing the nitrogen with a less electronegative donor (e.g., phosphorus) can improve the stability of the catalysts.

Experimental Section

General Comments

Unless otherwise noted, all organometallic/inorganic compounds were prepared and handled under an argon atmosphere using standard Schlenk and inert-atmosphere box techniques. Dry and oxygen-free solvents (THF, CH₂Cl₂, diethyl ether, toluene, and pentane) were collected from an Innovative Technology solvent purification system and used throughout the experiments. Acetone-d₆ was purchased from Cambridge Isotope Laboratories (CIL) and used as received. Benzene-d₆ (purchased from CIL) was dried over Na-benzophenone and distilled under an argon atmosphere. Acetonitrile-d₃ (purchased from CIL), acetonitrile, and acetone were dried over CaH₂ and distilled under an argon atmosphere. Methanol was dried over 4 Å molecular sieves and then degassed by bubbling argon through it for 30 min to 1 h. All other reagents were used as received from commercial sources. ^iPrPN^HP,^91,92 (^iPrPNP)NiBr (1),¹¹ and [(^iPrPN^HP)NiBr]Br ([1^H]Br)¹¹ were prepared as described in the literature. ¹H, ¹³C{¹H}, and ³¹P{¹H} NMR spectra were recorded on a Bruker Avance 400 MHz spectrometer. Chemical shift values in ¹H and ¹³C{¹H} NMR spectra were referenced internally to the residual solvent resonances. Assignments were made based on DEPT-135 and ¹H–¹³C HSQC spectra. ³¹P{¹H} NMR spectra were referenced externally to 85% H₃PO₄ (0 ppm). Infrared spectra were recorded on a Thermo Scientific Nicolet 6700 Fourier transform infrared (FT-IR) spectrometer or a PerkinElmer Spectrum Two FT-IR spectrometer equipped with a smart orbit diamond-attenuated total reflectance (ATR) accessory.

Synthesis of (^iPrPNP)NiPh (2), [(^iPrPN^HP)NiPh]Br ([2^H]Br), and (^iPrPNP′)NiPh (2′) from (^iPrPNP)NiBr (1) and PhMgCl

Under an argon atmosphere, a 2.0 M solution of PhMgCl in THF (500 μL, 1.0 mmol) was added dropwise to a Schlenk flask (flask #1) containing a solution of 1 (443 mg, 1.0 mmol) in 5 mL of THF chilled at 0 °C. The resulting mixture was warmed to room temperature, stirred at that temperature for 1 h, and then filtered into Schlenk flask #2, from which the solvent was removed under vacuum. The residue in flask #2 was treated with 10 mL of pentane, resulting in a suspension, which was filtered into Schlenk flask #3. The filtrate (in flask #3) was dried under vacuum to give 2 as a yellow solid (219 mg, 50% yield). The solid left in flask #2 was rinsed with pentane (collected in Schlenk flask #4) until the pentane wash was colorless. The combined pentane washes in flask #4 were dried under vacuum to yield a yellow solid. Recrystallization of this solid with pentane or acetone at −25 °C yielded orange-yellow rod-shaped crystals of 2′ (20 mg, 5% yield). The solid obtained after exhaustive pentane washes (in flask #2) was dissolved in acetone and then filtered through a pad of Celite to give a pale yellow solution. This solution was dried under vacuum, and the residue was suspended in a minimum amount of toluene. Several drops of acetone were added to the toluene suspension until a clear solution was obtained. The toluene–acetone solution was carefully layered with pentane and kept at −25 °C to yield colorless plate-shaped crystals of [2^H]Br (147 mg, 28% yield).

Characterization Data of 2

¹H NMR (400 MHz, C₆D₆, δ): 7.70 (d, ³J_H–H = 7.2 Hz, ArH, 2H), 7.11 (t, ³J_H–H = 7.4 Hz, ArH, 2H), 6.95 (t, ³J_H–H = 7.0 Hz, ArH, 1H), 3.23–3.15 (m, NCH₂, 4H), 1.84–1.79 (m, PCH(CH₃)₂, 4H), 1.76–1.71 (m, PCH₂, 4H), 1.07–0.98 (m, PCH(CH₃)₂, 24H). ¹³C{¹H} NMR (101 MHz, C₆D₆, δ): 156.09 (t, J_P–C = 28.6 Hz, ArC), 140.88 (s, ArC), 125.76 (s, ArC), 120.97 (s, ArC), 59.10 (s, NCH₂), 25.06 (t, J_P–C = 9.8 Hz, PCH₂), 23.33 (t, J_P–C = 11.1 Hz, PCH(CH₃)₂), 18.30 (s, CH₃), 17.48 (s, CH₃). ³¹P{¹H} NMR (162 MHz, C₆D₆, δ): 64.40 (s). Anal. Calcd for C₂₂H₄₁NP₂Ni: C, 60.03; H, 9.39; N, 3.18. Found: C, 59.75; H, 9.47; N, 3.18.

Characterization Data of [2^H]Br

¹H NMR (400 MHz, CD₃CN, δ): 7.33 (d, ³J_H–H = 7.6 Hz, ArH, 2H), 6.92 (t, ³J_H–H = 7.4 Hz, ArH, 2H), 6.75 (t, ³J_H–H = 7.2 Hz, ArH, 1H), 5.35 (t, broad, ³J_H–H = 11.0 Hz, NH, 1H), 3.18–3.03 (m, NCH₂, 2H), 2.45–2.34 (m, NCH₂, 2H), 2.22–2.15 (m, PCH(CH₃)₂, 2H), 2.10–2.00 (m, PCH(CH₃)₂ + PCH₂, 6H), 1.28–1.23 (m, PCH(CH₃)₂, 12H), 1.06–0.95 (m, PCH(CH₃)₂, 12H). ¹³C{¹H} NMR (101 MHz, CD₃CN, δ): 144.64 (t, J_P–C = 29.4 Hz, ArC), 138.67 (t, J_P–C = 3.5 Hz, ArC), 127.32 (s, ArC), 122.78 (s, ArC), 51.99 (t, J_P–C = 4.5 Hz, NCH₂), 23.75 (t, J_P–C = 11.9 Hz, PCH(CH₃)₂), 22.98 (t, J_P–C = 9.4 Hz, PCH₂), 22.67 (t, J_P–C = 13.1 Hz, PCH(CH₃)₂), 18.43 (s, CH₃), 18.33 (s, CH₃), 17.68 (s, CH₃), 17.27 (s, CH₃). ³¹P{¹H} NMR (162 MHz, CD₃CN, δ): 48.41 (s). ³¹P{¹H} NMR (162 MHz, C₆D₆, δ): 48.44 (s). Selected data from ATR-IR (solid): ν_N–H = 3351 cm^–1 (broad). Anal. Calcd for C₂₂H₄₂NP₂BrNi: C, 50.71; H, 8.12; N, 2.69. Found: C, 50.84; H, 7.93; N, 2.50.

Characterization Data of 2′

¹H NMR (400 MHz, C₆D₆, δ): 7.71 (d, ³J_H–H = 7.2 Hz, ArH, 2H), 7.42 (d, J = 42.8 Hz, CH, 1H), 7.14 (t, ³J_H–H = 7.2 Hz, ArH, 2H), 6.96 (t, ³J_H–H = 7.2 Hz, ArH, 1H), 3.41 (br, CH, 1H), 3.14 (dt, ³J_P–H = 18.4 Hz, ³J_H–H = 6.9 Hz, NCH₂, 2H), 2.09–1.99 (m, PCH(CH₃)₂, 2H), 1.76–1.66 (m, PCH(CH₃)₂, 2H), 1.30 (dt, ²J_P–H = 9.2 Hz, ³J_H–H = 4.0 Hz, PCH₂, 2H), 1.23 (dd, ³J_P–H = 13.8 Hz, ³J_H–H = 6.9 Hz, CH₃, 6H), 1.14 (dd, ³J_P–H = 15.4 Hz, ³J_H–H = 7.5 Hz, CH₃, 6H), 0.95–0.89 (m, CH₃, 12H). ¹³C{¹H} NMR (101 MHz, C₆D₆, δ): 167.67 (dd, J_P–C = 22.4 and 4.8 Hz, CH), 153.92 (dd, J_P–C = 30.4 and 29.2 Hz, ArC_ipso), 139.59 (t, J_P–C = 3.2 Hz, ArC), 126.14 (t, J_P–C = 2.1 Hz, ArC), 121.22 (t, J_P–C = 2.0 Hz, ArC), 65.80 (d, J_P–C = 40.8 Hz, CH), 55.13 (dd, J_P–C = 7.4 and 2.6 Hz, NCH₂), 24.28 (d, J_P–C = 18.7 Hz, PCH₂), 23.43 (dd, J_P–C = 25.8 and 1.2 Hz, PCH(CH₃)₂), 22.79 (dd, J_P–C = 19.6 and 1.9 Hz, PCH(CH₃)₂), 18.25 (d, J_P–C = 3.7 Hz, CH₃), 18.06 (d, J_P–C = 4.2 Hz, CH₃), 17.71 (d, J_P–C = 0.9 Hz, CH₃), 17.36 (s, CH₃). ³¹P{¹H} NMR (162 MHz, C₆D₆, δ): 58.97 (AB, J_AB = 259.7 Hz), 48.51 (AB, J_AB = 259.7 Hz). Anal. Calcd for C₂₂H₃₉NP₂Ni: C, 60.30; H, 8.97; N, 3.20. Found: C, 61.20; H, 9.02; N, 2.79.

Synthesis of (^iPrPNP′)NiBr (1′)

Under an argon atmosphere, 1 (111 mg, 0.25 mmol) and 1,4-benzoquinone (27 mg, 0.25 mmol) were mixed with 3 mL of toluene at room temperature and stirred for 24 h. The resulting black suspension was filtered, and the solvent in the filtrate was removed under vacuum. The product was extracted into pentane (5 mL × 3). Green crystals of 1′ were obtained from a concentrated pentane solution kept at −25 °C (8.5 mg, 8% yield). ¹H NMR (400 MHz, C₆D₆, δ): 6.76 (ddd, J = 45.1, 4.9, and 1.5 Hz, CH, 1H), 3.32–3.30 (m, CH, 1H), 2.79 (dt, ³J_P–H = 21.2 Hz, ³J_H–H = 6.8 Hz, NCH₂, 2H), 2.25–2.15 (m, PCH(CH₃)₂, 2H), 2.00–1.90 (m, PCH(CH₃)₂, 2H), 1.64 (dd, ³J_P–H = 16.0 Hz, ³J_H–H = 6.8 Hz, PCH(CH₃)₂, 6H), 1.41 (dd, ³J_P–H = 15.2 Hz, ³J_H–H = 7.2 Hz, PCH(CH₃)₂, 6H), 1.30 (dd, ³J_P–H = 13.6 Hz, ³J_H–H = 7.2 Hz, PCH(CH₃)₂, 6H), 0.94–1.02 (m, PCH(CH₃)₂ + PCH₂, 8H). ¹³C{¹H} NMR (101 MHz, C₆D₆, δ): 168.50 (dd, J_P–C = 22.9 and 4.4 Hz, CH), 68.25 (d, J_P–C = 40.9 Hz, CH), 57.44 (dd, J_P–C = 8.7 and 2.0 Hz, NCH₂), 25.15 (dd, J_P–C = 25.2 and 2.5 Hz, PCH(CH₃)₂), 23.86 (dd, J_P–C = 19.2 and 2.4 Hz, PCH(CH₃)₂), 22.23 (d, J_P–C = 19.3 Hz, PCH₂), 19.16 (d, J_P–C = 3.9 Hz, CH₃), 19.02 (d, J_P–C = 4.2 Hz, CH₃), 18.05 (s, CH₃), 17.78 (s, CH₃). ³¹P{¹H} NMR (162 MHz, C₆D₆, δ): 63.58 (AB, J_AB = 299.2 Hz), 57.87 (AB, J_AB = 299.2 Hz). Anal. Calcd for C₁₆H₃₄NP₂BrNi: C, 43.58; H, 7.77; N, 3.18. Found: C, 43.82; H, 7.96; N, 3.12.

Independent Synthesis of (^iPrPNP′)NiPh (2′) from (^iPrPNP′)NiBr (1′)

Under an argon atmosphere, a 2.0 M solution of PhMgCl in THF (50 μL, 0.10 mmol) was added dropwise to a solution of 1′ (37 mg, 0.084 mmol) in 5 mL of THF chilled at 0 °C. The resulting mixture was stirred at room temperature for 1 h, after which the solvent was removed under vacuum. The residue was dissolved in pentane and filtered through a pad of Celite. The filtrate was pumped to dryness, giving the desired product as a yellow solid (17 mg, 46%).

Synthesis of (TMEDA)Ni(Ph)I

This compound was prepared following a procedure similar to the one used for the synthesis of (TMEDA)Ni(Ph)Cl.⁹³ Under an argon atmosphere, a solution of TMEDA (280 μL, 1.9 mmol) in iodobenzene (2.2 mL, 20 mmol) was added to a Schlenk flask containing Ni(COD)₂ (420 mg, 1.5 mmol). The resulting mixture was stirred at room temperature for 6 h, followed by layering with pentane (10 mL). The mixture was then allowed to stand at room temperature overnight, resulting in a precipitate, which was collected by filtration, washed with pentane (10 mL × 3), and dried under vacuum. The product was isolated as a pink solid (500 mg, 88% yield). ¹H NMR (400 MHz, THF-d₈, δ): 7.47 (br, ArH, 2H), 6.62 (br, ArH, 2H), 6.43 (br, ArH, 1H), 2.58–2.13 (m, CH₃ + CH₂, 16H). ¹³C{¹H} NMR (101 MHz, THF-d₈, δ): 146.32 (br, ArC), 139.63 (s, ArC), 124.65 (s, ArC), 121.05 (s, ArC), 61.11 (br, NCH₂), 57.39 (br, NCH₂), 49.51 (br, CH₃), 48.68 (br, CH₃). Anal. Calcd for C₁₂H₂₁N₂INi: C, 38.04; H, 5.59; N, 7.39. Found: C, 37.25; H, 5.68; N, 7.31.

Synthesis of [(^iPrPN^HP)NiPh]PF₆ ([2^H]PF₆)

Under an argon atmosphere, a solution of ^iPrPN^HP (159 mg, 0.52 mmol) in 5 mL of THF was added dropwise to (TMEDA)Ni(Ph)I (197 mg, 0.52 mmol) dissolved in 20 mL of THF. The resulting mixture was stirred at room temperature for 30 min, giving a yellow precipitate. The solid was collected by filtration, washed with diethyl ether (5 mL × 3), and dried under vacuum. The isolated complex (268 mg, 0.47 mmol) was dissolved in 20 mL of CH₂Cl₂, followed by dropwise addition of a solution of AgPF₆ (143 mg, 0.56 mmol) in 10 mL of CH₂Cl₂. The resulting suspension was stirred at room temperature for 15 min and then filtered, and the solid was washed with diethyl ether (5 mL × 2). The filtrate combined with the ether wash was concentrated under vacuum to ∼3 mL, and the product precipitated after adding diethyl ether and pentane (5 mL each). The precipitate was collected by filtration, washed with diethyl ether (5 mL × 2), and dried under vacuum. The desired product was isolated as a yellow solid (238 mg, 78% yield over two steps). ¹H NMR (400 MHz, CD₃CN, δ): 7.31 (d, ³J_H–H = 7.6 Hz, ArH, 2H), 6.96 (t, ³J_H–H = 7.4 Hz, ArH, 2H), 6.79 (t, ³J_H–H = 7.4 Hz, ArH, 1H), 3.62 (t, broad, ³J_H–H = 13.8 Hz, NH, 1H), 3.22–3.09 (m, NCH₂, 2H), 2.58–2.45 (m, NCH₂, 2H), 2.30–2.18 (m, PCH(CH₃)₂, 2H), 2.18–2.06 (m, PCH(CH₃)₂ + PCH₂, 4H), 1.97–1.88 (m, PCH₂, 2H), 1.31–1.21 (m, PCH(CH₃)₂, 12H), 1.05–0.98 (m, PCH(CH₃)₂, 12H). ¹H NMR (400 MHz, acetone-d₆, δ): 7.38 (d, ³J_H–H = 7.2 Hz, ArH, 2H), 6.96 (t, ³J_H–H = 7.4 Hz, ArH, 2H), 6.77 (t, ³J_H–H = 7.4 Hz, ArH, 1H), 4.42 (t, broad, ³J_H–H = 11.8 Hz, NH, 1H), 3.41–3.27 (m, NCH₂, 2H), 2.77–2.66 (m, NCH₂, 2H), 2.35–2.23 (m, PCH(CH₃)₂ + PCH₂, 4H), 2.20–2.15 (m, PCH(CH₃)₂, 2H), 2.10–2.02 (m, PCH₂, 2H), 1.38–1.33 (m, PCH(CH₃)₂, 6H), 1.32–1.26 (m, PCH(CH₃)₂, 6H), 1.11–1.04 (m, PCH(CH₃)₂, 12H). ¹³C{¹H} NMR (101 MHz, acetone-d₆, δ): 143.42 (t, J_P–C = 29.3 Hz, ArC), 138.59–138.53 (m, ArC), 138.40–138.33 (m, ArC), 127.64 (s, ArC), 123.16 (t, J_P–C = 1.7 Hz, ArC), 52.52 (t, J_P–C = 4.5 Hz, NCH₂), 23.93 (t, J_P–C = 12.0 Hz, PCH(CH₃)₂), 22.95 (t, J_P–C = 9.0 Hz, PCH₂), 22.50 (t, J_P–C = 13.0 Hz, PCH(CH₃)₂), 18.38 (s, CH₃), 18.01 (s, CH₃), 17.34 (s, CH₃), 17.31 (s, CH₃). ³¹P{¹H} NMR (162 MHz, acetone-d₆, δ): 46.42 (s, PⁱPr₂), −143.72 (sept, ¹J_P–F = 708.2 Hz, PF₆). ³¹P{¹H} NMR (162 MHz, CD₃CN, δ): 47.64 (s, PⁱPr₂), −142.84 (sept, ¹J_P–F = 706.6 Hz, PF₆). Selected data from ATR-IR (solid): ν_N–H = 3249 cm^–1. Anal. Calcd for C₂₂H₄₂NP₃F₆Ni: C, 45.08; H, 7.22; N, 2.39. Found: C, 45.02; H, 7.18; N, 2.41.

Independent Synthesis of (^iPrPNP)NiPh (2) from [(^iPrPN^HP)NiPh]Br ([2^H]Br) or [(^iPrPN^HP)NiPh]PF₆ ([2^H]PF₆)

From [2^H]Br: Under an argon atmosphere, a solution of KO^tBu (5.6 mg, 0.050 mmol) in 3 mL of THF kept at −78 °C was added to [2^H]Br (26 mg, 0.050 mmol) suspended in 5 mL of THF, which was also chilled at −78 °C. The resulting mixture was stirred at that temperature for 15 min. The volatiles were removed under vacuum and the product was extracted with pentane (5 mL × 3). Complex 2 was isolated as a yellow solid after removing pentane under vacuum (14.8 mg, 67% yield). From [2^H]PF₆: Under an argon atmosphere, a solution of KO^tBu (16 mg, 0.14 mmol) in 5 mL of THF was added to [2^H]PF₆ (82 mg, 0.14 mmol) suspended in 10 mL of THF, which was chilled at −78 °C. The resulting suspension was stirred at that temperature for 15 min. The volatiles were removed under vacuum and the product was extracted with pentane (5 mL × 3). Complex 2 was isolated as a yellow solid after removing pentane under vacuum (29 mg, 47% yield).

Synthesis of [(^iPrPN^HP)NiPh]BPh₄ ([2^H]BPh₄)

Under an argon atmosphere, a solution of NaBPh₄ (82 mg, 0.24 mmol) in 2 mL of CH₃OH was added dropwise to [2^H]Br (100 mg, 0.19 mmol) dissolved in 2 mL of CH₃OH. The mixture was stirred at room temperature for 30 min, giving a yellow precipitate. The solid was filtered off, washed with diethyl ether (5 mL × 2), and dried under vacuum. The desired product was isolated as a yellow solid (87 mg, 60% yield). ¹H NMR (400 MHz, CD₃CN, δ): 7.32–7.28 (m, ArH, 10H), 7.00 (t, ³J_H–H = 7.4 Hz, ArH, 8H), 6.94 (t, ³J_H–H = 7.2 Hz, ArH, 2H), 6.85 (t, ³J_H–H = 7.0 Hz, ArH, 4H), 6.77 (t, ³J_H–H = 7.2 Hz, ArH, 1H), 3.77 (t, broad, ³J_H–H = 10.4 Hz, NH, 1H), 3.17–3.03 (m, NCH₂, 2H), 2.52–2.42 (m, NCH₂, 2H), 2.24–2.16 (m, PCH(CH₃)₂, 2H), 2.13–2.01 (m, PCH(CH₃)₂ + PCH₂, 4H), 1.92–1.83 (m, PCH₂, 2H), 1.29–1.19 (m, PCH(CH₃)₂, 12H), 1.03–0.96 (m, PCH(CH₃)₂, 12H). ¹³C{¹H} NMR (101 MHz, CD₃CN, δ): 164.68 (q, ¹J_B–C = 49.5 Hz, ArC), 143.52 (t, J_P–C = 29.5 Hz, ArC), 138.63 (t, J_P–C = 2.2 Hz, ArC), 138.44 (t, J_P–C = 3.5 Hz, ArC), 136.62 (q, J_B–C = 1.2 Hz, ArC), 127.54 (br, ArC), 126.50 (q, J_B–C = 2.7 Hz, ArC), 123.05 (t, J_P–C = 2.0 Hz, ArC), 122.67 (s, ArC), 52.13 (t, J_P–C = 4.5 Hz, NCH₂), 23.82 (t, J_P–C = 12.1 Hz, PCH(CH₃)₂), 22.86 (t, J_P–C = 9.0 Hz, PCH₂), 22.47 (t, J_P–C = 13.1 Hz, PCH(CH₃)₂), 18.27 (s, CH₃), 17.98 (s, CH₃), 17.30 (s, CH₃), 17.23 (s, CH₃). ³¹P{¹H} NMR (162 MHz, CD₃CN, δ): 47.72 (s). Selected data from ATR-IR (solid): ν_N–H = 3181 cm^–1. Anal. Calcd for C₄₆H₆₂NBP₂Ni·1.5C₄H₈O (crystals grown from THF–pentane): C, 71.90; H, 8.59; N, 1.61. Found: C, 71.28; H, 8.25; N, 1.87.

Synthesis of [(^iPrPN^HP)NiPh]Cl ([2^H]Cl)

At room temperature under an argon atmosphere, a 2.0 M solution of HCl in diethyl ether (75 μL, 0.15 mmol) was added dropwise to 2 (54 mg, 0.12 mmol) dissolved in 5 mL of diethyl ether. The resulting suspension was stirred for 30 min. The volatiles were then removed under vacuum, and the residue was washed with pentane (5 mL × 3). After drying under vacuum, the product was isolated as a greenish yellow solid (57 mg, 97% yield). ¹H NMR (400 MHz, CD₃CN, δ): 7.34 (d, ³J_H–H = 6.0 Hz, ArH, 2H), 6.91 (t, ³J_H–H = 7.4 Hz, ArH, 2H), 6.74 (t, ³J_H–H = 7.0 Hz, ArH, 1H), 6.25 (t, broad, ³J_H–H = 10.0 Hz, NH, 1H), 3.14–3.04 (m, NCH₂, 2H), 2.46–2.36 (m, NCH₂, 2H), 2.21–1.97 (m, PCH(CH₃)₂ + PCH₂, 8H), 1.30–1.22 (m, PCH(CH₃)₂, 12H), 1.08–1.02 (m, PCH(CH₃)₂, 6H), 1.01–0.95 (m, PCH(CH₃)₂, 6H). ¹³C{¹H} NMR (101 MHz, CD₃CN, δ): 145.18 (t, J_P–C = 29.6 Hz, ArC), 138.82 (t, J_P–C = 3.0 Hz, ArC), 127.31 (s, ArC), 122.76 (s, ArC), 52.13 (t, J_P–C = 4.7 Hz, NCH₂), 23.81 (t, J_P–C = 11.9 Hz, PCH(CH₃)₂), 23.07 (t, J_P–C = 9.2 Hz, PCH₂), 22.72 (t, J_P–C = 13.0 Hz, PCH(CH₃)₂), 18.55 (s, CH₃), 18.41 (s, CH₃), 17.83 (s, CH₃), 17.34 (s, CH₃). ³¹P{¹H} NMR (162 MHz, CD₃CN, δ): 48.76 (s). ³¹P{¹H} NMR (162 MHz, C₆D₆, δ): 48.92 (s). Selected data from ATR-IR (solid): ν_N–H = 3360 cm^–1 (broad).

Synthesis of (^iPrPNP)NiMe (3)

At room temperature under an argon atmosphere, a 1.6 M solution of MeLi in diethyl ether (188 μL, 0.30 mmol) was added dropwise to a solution of 1 (111 mg, 0.25 mmol) in 5 mL of diethyl ether, resulting in a color change from dark green to orange. After the addition, the reaction mixture was stirred at room temperature for another 5 min. The volatiles were removed under vacuum, and the residue was extracted with pentane (5 mL × 2). The pentane extracts were concentrated under vacuum, giving 3 as an orange solid (72 mg, 76% yield). The ³¹P{¹H} NMR spectrum suggested that the product was contaminated with a small amount (∼5%) of the dehydrogenated species, (^iPrPNP′)NiMe (3′). ¹H NMR (400 MHz, C₆D₆, δ): 3.23–3.15 (m, NCH₂, 4H), 1.94–1.87 (m, PCH(CH₃)₂, 4H), 1.75–1.71 (m, PCH₂, 4H), 1.27–1.21 (m, PCH(CH₃)₂, 12H), 1.11–1.06 (m, PCH(CH₃)₂, 12H), −0.59 (t, ³J_P–H = 8.6 Hz, NiCH₃, 3H). ¹³C{¹H} NMR (101 MHz, C₆D₆, δ): 58.75 (t, broad, NCH₂), 25.19 (t, J_P–C = 9.8 Hz, PCH₂), 23.64 (t, J_P–C = 10.3 Hz, PCH(CH₃)₂), 19.25 (t, J_P–C = 2.1 Hz, PCH(CH₃)₂), 17.85 (s, PCH(CH₃)₂), −26.32 (t, ²J_P–C = 25.6 Hz, NiCH₃). ³¹P{¹H} NMR (162 MHz, C₆D₆, δ): 68.81 (s). Elementary analyses were unsatisfactory despite repeated trials. This is likely due to the extremely high sensitivity of this compound toward even a trace amount of O₂. Coincidently, the data matched those of 3 with two oxygen atoms incorporated. Anal. Calcd for C₁₇H₃₉NO₂P₂Ni (3 + O₂): C, 49.78; H, 9.58; N, 3.42. Found: C, 49.62; H, 9.86; N, 3.42.

Characterization Data of 3′

Selected ¹H NMR data (400 MHz, C₆D₆, δ): 7.47 (dd, J = 41.8 and 5.0 Hz, CH, 1H), −0.35 (t, ³J_P–H = 8.6 Hz, NiCH₃, 3H). ³¹P{¹H} NMR (162 MHz, C₆D₆, δ): 62.71 (AB, J_AB = 275.4 Hz), 49.86 (AB, J_AB = 275.4 Hz).

Synthesis of [(^iPrPN^HP)NiMe]Br ([3^H]Br)

At room temperature under an argon atmosphere, a 1.6 M solution of MeLi in diethyl ether (188 μL, 0.30 mmol) was added dropwise to a solution of 1 (111 mg, 0.25 mmol) in 5 mL of diethyl ether. After addition, the mixture was stirred at room temperature for another 5 min. The volatiles were removed under vacuum, and the residue was treated with 3 mL of methanol, which resulted in the formation of a small amount of black particles. The reaction mixture was stirred at room temperature for 15 min, and methanol was removed under vacuum. The residue was suspended in 20 mL of toluene (or 3 mL acetonitrile) and filtered through a pad of Celite to remove the black particles. The filtrate was pumped to dryness, washed with pentane (5 mL × 3), and dried under vacuum. The desired product was isolated as a yellow solid (60 mg, 52% yield). ¹H NMR (400 MHz, CD₃CN, δ): 4.92 (t, broad, NH, 1H), 3.11–2.94 (m, NCH₂, 2H), 2.34–2.20 (m, PCH(CH₃)₂ + NCH₂, 6H), 1.98–1.93 (m, PCH₂, 4H), 1.36–1.24 (m, PCH(CH₃)₂, 24H), −0.57 (t, ³J_P–H = 9.0 Hz, NiCH₃, 3H). ¹³C{¹H} NMR (101 MHz, CD₃CN, δ): 51.87 (t, J_P–C = 4.7 Hz, NCH₂), 25.11 (t, J_P–C = 11.3 Hz, PCH(CH₃)₂), 23.14 (t, J_P–C = 12.4 Hz, PCH(CH₃)₂), 23.00 (t, J_P–C = 9.3 Hz, PCH₂), 19.44 (t, J_P–C = 1.5 Hz, PCH(CH₃)₂), 19.34 (t, J_P–C = 2.2 Hz, PCH(CH₃)₂), 18.43 (s, PCH(CH₃)₂), 17.91 (s, PCH(CH₃)₂), −24.04 (t, J_P–C = 23.8 Hz, NiCH₃). ³¹P{¹H} NMR (162 MHz, CD₃CN, δ): 51.69 (s). ³¹P{¹H} NMR (162 MHz, C₆D₆, δ): 51.86 (s). Selected data from ATR-IR (solid): ν_N–H = 3399 cm^–1 (broad). Anal. Calcd for C₁₇H₄₀NP₂BrNi: C, 44.48; H, 8.78; N, 3.05. Found: C, 44.58; H, 8.71; N, 3.07.

Synthesis of (^iPrPNP)NiCl (4)

Under an argon atmosphere, a 1.6 M solution of n-BuLi in hexanes (750 μL, 1.2 mmol) was added dropwise to a chilled (−78 °C) solution of ^iPrPN^HP (305 mg, 1.0 mmol) in 5 mL of THF. The reaction mixture was stirred first at −78 °C for 30 min and then at room temperature for 1.5 h. In a separate flask, a mixture of NiCl₂ (194 mg, 1.5 mmol) and 15 mL of THF was stirred at room temperature for 2 h and then cooled to −78 °C. The lithiated ligand ^iPrPNP was slowly added while the temperature was maintained at −78 °C. The resulting suspension was stirred at −78 °C for 30 min and then at room temperature for 16 h. The volatiles were removed under vacuum, and the residue was treated with 20 mL of pentane and then filtered through a pad of Celite. The filtrate was concentrated under vacuum and recrystallized at −25 °C. The desired product was isolated as dark green crystals (73 mg, 18% yield). The ³¹P{¹H} NMR spectrum suggested that the product was contaminated with a small amount (∼2%) of the dehydrogenated species, (^iPrPNP′)NiCl (4′). ¹H NMR (400 MHz, C₆D₆, δ): 2.59–2.49 (m, NCH₂, 4H), 2.10–2.01 (m, PCH(CH₃)₂, 4H), 1.55–1.50 (m, PCH(CH₃)₂, 12H), 1.38–1.33 (m, PCH₂, 4H), 1.16–1.11 (m, PCH(CH₃)₂, 12H). ¹³C{¹H} NMR (101 MHz, C₆D₆, δ): 60.70 (t, J_P–C = 6.5 Hz, NCH₂), 23.59 (t, J_P–C = 10.0 Hz, PCH(CH₃)₂), 22.03 (t, J_P–C = 10.7 Hz, PCH₂), 19.17 (t, J_P–C = 1.9 Hz, CH₃), 17.76 (s, CH₃). ³¹P{¹H} NMR (162 MHz, C₆D₆, δ): 66.09 (s). Anal. Calcd for C₁₆H₃₆NP₂ClNi: C, 48.22; H, 9.10; N, 3.51. Found: C, 48.14; H, 9.30; N, 3.47.

Characterization Data of 4′

Selected ¹H NMR data (400 MHz, C₆D₆, δ): 6.72 (ddd, J = 45.2, 5.2, and 1.2 Hz, CH, 1H), 3.28 (t, J = 3.8 Hz, CH, 1H), 2.76 (dt, ³J_P–H = 21.2 Hz, ³J_H–H = 6.8 Hz, NCH₂, 2H). ³¹P{¹H} NMR (162 MHz, C₆D₆, δ): 60.87 (AB, J_AB = 307.8 Hz), 55.02 (AB, J_AB = 307.8 Hz).

Synthesis of [(^iPrPN^HP)NiMe]Cl ([3^H]Cl)

At room temperature under an argon atmosphere, a 1.6 M solution of MeLi in diethyl ether (188 μL, 0.30 mmol) was added dropwise to a solution of 4 (100 mg, 0.25 mmol) in 5 mL of diethyl ether. After addition, the mixture was stirred at room temperature for 5 min. The volatiles were removed under vacuum, and the residue was treated with 3 mL of methanol, which resulted in the formation of a small amount of black particles. The reaction mixture was stirred for 15 min, and methanol was removed under vacuum. The resulting solid was treated with 3 mL of acetonitrile and filtered through a pad of Celite to remove the black particles. The filtrate was pumped to dryness, and the residue was washed with pentane (5 mL × 3) and then dried under vacuum. The product was isolated as a yellow solid (75 mg, 72% yield). ¹H NMR (400 MHz, CD₃CN, δ): 5.61 (br, NH, 1H), 3.06–2.96 (m, NCH₂, 2H), 2.30–2.21 (m, PCH(CH₃)₂ + NCH₂, 6H), 1.37–1.25 (m, PCH₂ + PCH(CH₃)₂, 28H), −0.58 (t, ³J_P–H = 8.8 Hz, NiCH₃, 3H). ¹³C{¹H} NMR (101 MHz, CD₃CN, δ): 51.91 (t, J_P–C = 4.7 Hz, NCH₂), 25.03 (t, J_P–C = 11.2 Hz, PCH(CH₃)₂), 23.09 (t, J_P–C = 12.4 Hz, PCH(CH₃)₂), 22.96 (t, J_P–C = 9.8 Hz, PCH₂), 19.41 (br, PCH(CH₃)₂), 19.27 (t, J_P–C = 2.4 Hz, PCH(CH₃)₂), 18.37 (s, PCH(CH₃)₂), 17.87 (s, PCH(CH₃)₂), −24.27 (t, J_P–C = 23.9 Hz, NiCH₃). ³¹P{¹H} NMR (162 MHz, CD₃CN, δ): 51.85 (s). ³¹P{¹H} NMR (162 MHz, C₆D₆, δ): 51.97 (s). Selected data from ATR-IR (solid): ν_N–H = 3393 cm^–1 (broad). Anal. Calcd for C₁₇H₄₀NP₂ClNi: C, 49.25; H, 9.72; N, 3.38. Found: C, 48.04; H, 9.59; N, 3.31.

Synthesis of [(^iPrPN^HP)NiMe]BPh₄ ([3^H]BPh₄)

At room temperature under an argon atmosphere, a 1.6 M solution of MeLi in diethyl ether (188 μL, 0.30 mmol) was added dropwise to a solution of 1 (111 mg, 0.25 mmol) in 5 mL of diethyl ether. After addition, the mixture was stirred at room temperature for another 5 min. The volatiles were removed under vacuum, and the residue was treated with 3 mL of methanol, which resulted in the formation of a small amount of black particles. A solution of NaBPh₄ (103 mg, 0.30 mmol) in 3 mL of methanol was then added dropwise, and the resulting suspension was stirred at room temperature for 30 min, after which methanol was removed under vacuum. The residue was suspended in 3 mL of acetonitrile and filtered through a pad of Celite to remove the black particles. The filtrate was pumped to dryness, washed with pentane (5 mL × 3), and dried under vacuum. The desired product was isolated as a yellow solid (115 mg, 66% yield). ¹H NMR (400 MHz, CD₃CN, δ): 7.29–7.25 (br, ArH, 8H), 7.00 (t, ³J_H–H = 7.4 Hz, ArH, 8H), 6.84 (t, ³J_H–H = 7.2 Hz, ArH, 4H), 3.57 (t, broad, ³J_H–H = 11.6 Hz, NH, 1H), 3.08–3.00 (m, NCH₂, 2H), 2.37–2.19 (m, PCH(CH₃)₂ + NCH₂, 6H), 2.03–1.98 (m, PCH₂, 2H), 1.84–1.75 (m, PCH₂, 2H), 1.34–1.22 (m, PCH(CH₃)₂, 24H), −0.53 (t, ³J_P–H = 8.8 Hz, NiCH₃, 3H). ¹³C{¹H} NMR (101 MHz, CD₃CN, δ): 164.72 (q, ¹J_B–C = 49.6 Hz, ArC), 136.66 (br, ArC), 126.52 (q, J_B–C = 2.8 Hz, ArC), 122.69 (s, ArC), 51.89 (t, J_P–C = 4.5 Hz, NCH₂), 25.09 (t, J_P–C = 11.3 Hz, PCH(CH₃)₂), 22.93 (t, J_P–C = 12.2 Hz, PCH(CH₃)₂), 22.88 (t, J_P–C = 9.1 Hz, PCH₂), 19.30 (br, PCH(CH₃)₂), 19.07 (t, J_P–C = 1.9 Hz, PCH(CH₃)₂), 18.36 (s, PCH(CH₃)₂), 17.64 (s, PCH(CH₃)₂), −23.73 (t, J_P–C = 23.7 Hz, NiCH₃). ³¹P{¹H} NMR (162 MHz, CD₃CN, δ): 51.24 (s). Selected data from ATR-IR (solid): ν_N–H = 3189 cm^–1. Anal. Calcd for C₄₁H₆₀NBP₂Ni: C, 70.51; H, 8.66; N, 2.01. Found: C, 70.70; H, 8.80; N, 2.04.

Synthesis of [(^iPrPN^HP)NiCl]Cl ([4^H]Cl)

Under an argon atmosphere, a solution of the ligand ^iPrPN^HP (380 mg, 1.25 mmol) in 5 mL of THF was added to NiCl₂ (161 mg, 1.24 mmol) suspended in 10 mL of THF. The resulting mixture was stirred at room temperature for 24 h. The solvent was then removed under vacuum, and the residue was extracted with CH₂Cl₂ (10 mL × 3). The combined CH₂Cl₂ fractions were concentrated under vacuum, layered with diethyl ether, and kept at −25 °C for crystallization. The product was isolated as orange crystals (73 mg, 14% yield). ¹H NMR (400 MHz, CDCl₃, δ): 7.88 (br, NH, 1H), 3.06 (tt, J = 19.2 and 3.9 Hz, NCH₂, 2H), 2.41–2.17 (m, PCH(CH₃)₂ + PCH₂ + NCH₂, 8H), 1.69–1.60 (m, PCH(CH₃)₂ + PCH₂, 8H), 1.58–1.54 (m, PCH(CH₃)₂, 6H), 1.54–1.46 (m, PCH(CH₃)₂, 6H), 1.44–1.39 (m, PCH(CH₃)₂, 6H). ¹³C{¹H} NMR (101 MHz, CDCl₃, δ): 54.97 (t, J_P–C = 5.0 Hz, NCH₂), 24.34 (t, J_P–C = 11.2 Hz, PCH(CH₃)₂), 23.73 (t, J_P–C = 12.6 Hz, PCH(CH₃)₂), 20.53 (t, J_P–C = 9.3 Hz, PCH₂), 19.45 (s, CH₃), 18.92 (s, CH₃), 18.06 (s, CH₃), 17.95 (s, CH₃). ³¹P{¹H} NMR (162 MHz, CDCl₃, δ): 55.25 (s). ³¹P{¹H} NMR (162 MHz, C₆D₆, δ): 55.40 (s). For both solid and solution samples, the ν_N–H band was absent from the IR spectra. Anal. Calcd for C₁₆H₃₇NP₂Cl₂Ni: C, 44.18; H, 8.57; N, 3.22. Found: C, 44.18; H, 8.57; N, 3.24.

Protonation of Nickel PNP Pincer Complexes with an Acid

Under an argon atmosphere, a neutral nickel pincer complex (1–4, 0.010 or 0.020 mmol) was dissolved in ∼0.5 mL of C₆D₆ and placed in a J. Young NMR tube. To the solution was added an appropriate amount of acid (HCl as a 2.0 M solution in Et₂O, HBF₄·Et₂O, H₂O, or MeOH), as described in the Results and Discussion section. The progress of the reaction was monitored by ¹H and ³¹P{¹H} NMR spectroscopy.

Supporting Information Available

The Supporting Information is available free of charge on the ACS Publications website at DOI: 10.1021/acsomega.8b00777.

• Complete characterization data, including structural parameters of the compounds characterized by X-ray diffraction (PDF)

• X-ray crystallographic information for 1′, [1^H]Br, 2, 2′, [2^H]Br, [2^H]PF₆, [2^H]BPh₄·3/2THF, [2^H]₂[NiCl₄]·4C₆D₆·1/2H₂O, 3, [3^H]Cl, [3^H]Br, [3^H]BPh₄, [4^H]Cl, and (TMEDA)NiPhI (CIF)

The authors declare no competing financial interest.