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# The elusive abnormal CO2 insertion enabled by metal-ligand cooperative photochemical selectivity inversion

## Abstract

Direct hydrogenation of CO2 to CO, the reverse water–gas shift reaction, is an attractive route to CO2 utilization. However, the use of molecular catalysts is impeded by the general reactivity of metal hydrides with CO2. Insertion into M–H bonds results in formates (MO(O)CH), whereas the abnormal insertion to the hydroxycarbonyl isomer (MC(O)OH), which is the key intermediate for CO-selective catalysis, has never been directly observed. We here report that the selectivity of CO2 insertion into a Ni–H bond can be inverted from normal to abnormal insertion upon switching from thermal to photochemical conditions. Mechanistic examination for abnormal insertion indicates photochemical N–H reductive elimination as the pivotal step that leads to an umpolung of the hydride ligand. This study conceptually introduces metal-ligand cooperation for selectivity control in photochemical transformations.

## Introduction

Selectivity control is a key issue for CO2 functionalization to added value products. The products from CO2 reduction can range from oxalic acid (1-electron) to carbon monoxide or formic acid (2-electron), formaldehyde (4-electron), and methanol (6-electron) all the way to hydrocarbons1. The primary industrial C1 building block CO is a particularly attractive target. In nature, CO2 reduction to CO is catalyzed by the enzyme [NiFe] carbon monoxide dehydrogenase ([NiFe]-CODH), which contains a nickel capped [Fe4S4Ni]-cluster as active site1. The proposed mechanism comprises CO2 binding to nickel followed by formation of a hydroxycarbonyl bridged {Ni(CO2H)Fe} intermediate as selectivity deriving step upon electron and proton transfer. Alternatively, CO2 insertion into a Ni–H bond has also been discussed2. In analogy, metallocarboxylate (MCO2H/M) species are also proposed as the key intermediates for synthetic CO-selective molecular catalysis, yet rarely detected3,4,5,6,7,8. Such systems are generally electro- or photochemically driven1,9,10,11,12 as direct hydrogenation by reverse water–gas shift (RWGS) is endothermic (see equation 1).

$${\mathrm{CO}}_{\mathrm{2}} + {\mathrm{H}}_{\mathrm{2}} \to {\mathrm{CO}} + {\mathrm{H}}_{\mathrm{2}}{\mathrm{O}}\,({\mathrm{\Delta }}_{\mathrm{r}}{\mathrm{H}}^0 = + 42.2\,{\mathrm{kJ}} \cdot {\mathrm{mol}}^{ - 1})$$
(1)

Photo-driven direct RWGS would be a highly desirable alternative to (photo)electrocatalysis. But this route also faces a major kinetic challenge, which disfavors CO formation: CO2 hydrogenation via molecular hydride catalysts generally leads to formic acid (or methanol) instead of CO13,14,15,16. This selectivity is a consequence of the normal CO2 insertion into M–H bonds giving formates (MO2CH)17. In contrast, the alternative formation of the hydroxycarbonyl (MCO2H) isomer has never been directly observed and is therefore referred to as abnormal CO2 insertion13.

Nickel pincer complexes were recently studied both as [NiFe]-CODH models and in catalytic CO2 hydrogenation to formate18,19,20,21. Inspired by the biological and synthetic precedence, we here report the photo-driven inversion of the CO2 insertion selectivity into a Ni–H bond representing an example of abnormal CO2 insertion. The selectivity is defined by photoinduced trans N–H reductive elimination as an application of metal-ligand cooperativity in photocatalysis.

## Results

### Thermal vs. photochemical CO2 insertion

Nickel(II) hydride complex [NiH(PNP)] (1, PNP = N(CHCHPtBu2)2) can be prepared from the previously reported bromide [NiBr(PNP)] with LiAlH422. As expected, the reaction of 1 with CO2 (1–10 bar) at room temperature (r.t.) gives formate complex [Ni(O2CH)(PNP)] (2, Fig. 1) as the product of normal insertion. However, the reaction is sluggish and takes several days for completion even at p(CO2) = 10 bar. In contrast to this thermal reactivity, bulk photolysis of 1 (λexc > 305 nm, Supplementary Fig. 15) in benzene or THF under CO2 (1 bar) at r.t. results in full conversion of 1 within a few hours (Fig. 1). A quantum yield around ΦP = 5% was estimated actinometrically using a ferrioxalate assay (Supplementary Fig. 37). Importantly, the abnormal insertion product [NiII(CO2H)(PNP)] (3) is formed as the main product in ~ 70% spectroscopic and isolated yield with no indication for formate 2. In the solid state, the bond metrics of the {NiCO2H} entity (Fig. 2) resemble the other previously reported nickel hydroxycarbonyl complex, which was not obtained directly from CO218. Besides 3, small amounts (ca. 20%) of the hydrocarbonate complex [Ni(OCO2H)(PNP)] (4, Fig. 2) and trace quantities of nickel(I) complex [Ni(CO)(PNP)] (5, Fig. 2) are observed by nuclear magnetic resonance (NMR) and electron paramagnetic resonance (EPR) spectroscopy (Supplementary Figs. 28, 29), respectively, as the only side products. Kinetic monitoring of the photolysis (Fig. 3a) indicates slow underlying conversion of 3 to 4 by CO extrusion and CO2 insertion as the source of hydrocarbonate and carbonyl side products. Accordingly, photolysis of isolated 3 under argon gives the hydroxy complex [Ni(OH)(PNP)] (6, Fig. 2) in high yield within competitive timescales and 6 selectively inserts CO2 to hydrocarbonate 4 (Fig. 4a, Supplementary Fig. 16).

### Mechanistic examinations

In agreement with the experimental findings, thermal normal insertion was computed to be slow and strongly favored over endergonic abnormal insertion both thermodynamically and kinetically (Fig. 1). Mechanistic examinations were conducted to rationalize this photochemical selectivity inversion. Photolysis of the [NiD(PNP)] isotopologue under CO2 results in almost quantitative transfer of the deuterium label to the hydroxy proton of 3, thus confirming the hydride ligand as the primary hydrogen source (Supplementary Fig. 25). The reaction rate exhibits first-order dependence in 1 and photon flux, respectively, but is independent from CO2 pressure between 1 and 10 bar (Supplementary Figs. 2025). Therefore, the photochemistry of 1 in the absence of CO2 was first studied. Hydride H/D exchange with TEMPO-D (2,2,6,6-tetramethylpiperidinyldeuteroxide; 10 equiv.) is observed only under photolytic conditions (Supplementary Fig. 19). In contrast, H/D scrambling with tBuOD is obtained neither in the dark nor upon photolysis, suggesting homolytic rather than heterolytic Ni–H photoactivation. Accordingly, photolysis of 1 in benzene or THF under argon (Fig. 4b) gives [Ni(PNP)] (7) as the only detectable product by NMR and EPR spectroscopy upon comparison with an analytically pure sample prepared by reduction of [NiBr(PNP)] with Mg (Supplementary Figs. 17 and 30). Liberation of H2 was confirmed by gas chromatography headspace analysis (Supplementary Fig. 18). The rhombic g-tensor (gx = 2.29, gy = 2.25, gz = 2.01) and 14N superhyperfine interaction (Az = 34 MHz) of 7 are in agreement with nickel(I) and some spin delocalization onto the pincer ligand, which is confirmed by density functional theory (DFT) computations (ρNi = 91%; Supplementary Fig. 42). In analogy to other nickel(I) complexes with similar spectroscopic features20,23,24,25, the molecular structure of 7 (Fig. 2) reveals T-shaped nickel coordination.

The observation of the photoreduction products 7 and 5 raises the question about the role of nickel(I) for abnormal insertion, e.g, via a radical chain mechanism. 7 reacts with equimolar amounts of CO2 in the dark and under photochemical conditions to one diamagnetic compound (Fig. 4b). NMR spectroscopic characterization of the 13CO2 isotopologue is in agreement with the formation of a dinuclear CO2-bridged (δ(13C) = 237 ppm) NiII/NiII complex, in analogy with a related nickel(I) pincer complex20. In the current case, the product [(PNP)NiII(1κC,2κ2O,O′-CO2)NiII(κ2P,N-PNP)] (8) bears one tridentate (δ(31P) = 67.8 ppm) and one bidentate pincer ligand (δ(31P) = 72.2 and 4.8 ppm), respectively, presumably as a consequence of increased steric pressure. At 1 bar CO2, 8 subsequently eliminates CO and inserts CO2 (Fig. 4b) to the dinuclear carbonate bridged complex [(PNP)NiII(OC(O)O)NiII(PNP)] (9, Fig. 2). In the presence of 1 (without irradiation) this reactivity of 7 with CO2 remains unchanged. Importantly, 1 is not consumed under these conditions disfavoring a radical chain mechanism for abnormal insertion with photochemically produced 7 as chain propagator. Photolysis of mixtures of 1 and 7 ([7]0 = 0–1.3 [1]0) under CO2 (1 bar) gives rising amounts of binuclear (9) vs. mononuclear (3) products with increasing [7]0 (Fig. 3b). In fact, the consumption of 1 even slows with increasing [7]0. This rate retardation and the diverging selectivities strongly suggest that nickel(I) complex 7 is not an intermediate in abnormal CO2 insertion.

### Time-resolved spectroscopy

Transient spectroscopy was employed to further rationalize the photochemistry of 1. Pump-probe IR-spectroscopy (λexc = 400 nm, THF) reveals an instantaneous bleach of the Ni–H stretching vibration at 1845 cm–1 and simultaneous shift of vibrational modes of the vinylic PNP ligand backbone ~1500–1520 cm–1 (Fig. 3c–e). The absence of other transient signals within the experimental window (1260–1900 cm–1) for both Ni–H/D isotopomers is consistent with the population of a dissociative state or at least strong weakening of the metal-hydride bond upon excitation (Supplementary Figs. 32, 33, 35). Ground state repopulation can be modeled with a biexponential fit. The immediately formed excited state shows a lifetime of τ1 = 1.3 ps. The timescale of the subsequent spectral evolution (τ2 = 12 ps) is consistent with vibrational cooling in the electronic ground state of 1. Although full relaxation is observed for the IR spectrum, transient UV/Vis spectroscopy (Fig. 3f–h, Supplementary Fig. 34; λexc = 400 nm, THF) reveals the evolution of a band at around 450 nm within the same timescale (τ2 ≈ 13 ps) that is persistent on the timescale of the pump-probe experiment (τ3 1 ns) and does not originate from nickel(I) complex 7 (Supplementary Fig. 31). The absence of IR-bands assignable to this product is attributed to low quantum yields (<5%). Notably, a weak feature at 450 nm is also observed in the stationary UV/Vis spectrum after bulk photolysis of 1 (Supplementary Fig. 31). Importantly, the rapid rate of all photoprocesses well below the timescale of diffusion exclude bimolecular reactivity of an excited state of 1 with CO2, which is in line with the rate independence of abnormal insertion from p(CO2). Instead, 1 apparently forms a photoproduct with low quantum yield that presumably is a common intermediate for photoreduction to 7 or, alternatively, abnormal insertion in the presence of CO2.

### Trapping experiments

The timescales of the photoprocesses and the retention of the Ni–D label upon reaction with CO2 support an intramolecular rearrangement to the photoproduct, yet not to nickel(I) as suggested by the kinetics. Further information about the photointermediate was obtained from variation of the reaction conditions. Irradiation of 1 in the presence of only one equivalent of CO2 gave a new product in ~20% isolated yield (Fig. 4c). Spectroscopic and crystallographic characterization reveal the formation of the unusual, dinuclear complex [(PNP)NiII(1κC,2κ2O,O’-CO2)NiII(κ2P,C-tBu2PCHCHNHCHCH2PtBu2)] (10, Fig. 2). This product is also obtained upon photolysis of solutions of 1 and 3 under argon suggesting trapping of the photointermediate by 3 at low CO2 concentrations. The formation of 10 can be rationalized by O–H oxidative addition of 3 to a nickel(0) photoproduct and subsequent olefin migrative insertion. Initial photoinduced N–H reductive elimination to nickel(0) is further supported by a trapping experiment with CO. Photolysis under CO gives the nickel(0) complex [(CO)3Ni{κP-HN(CHCHPtBu2)2}] (11, Fig. 2) almost selectively (Fig. 4c). Thermal reductive elimination under CO is also observed26, yet on considerably slower timescales compared with the photolytic conditions. Reductive elimination photoreactivity is frequently observed for metal hydrides27. Surprisingly, the almost fully released pincer ligand of 11 favors the divinylamine over imine tautomer, in line with the selective transfer of the Ni–D deuteride label to the hydroxy group of 3. In contrast, cooperative participation of the vinylic backbone, should lead to C–H/D scrambling, which is not observed22.

### Computational examinations

This mechanistic picture was further probed by DFT computations (Fig. 5). The trans-NH reductive elimination product [Ni0(HPNP)] (A) was found at ΔG = 33.2 kcal mol–1 relative to parent 1 and close to a THF solvent adduct, [(THF)Ni0(HPNP)] (A, ΔG = 35.9 kcal mol–1). In contrast to the NiII and NiI complexes 1 and 7, respectively, TD-DFT predicts several electronic transitions with high oscillator strength in the range 400–450 nm both for A and A (Supplementary Fig. 40), as was found by transient UV/Vis spectroscopy (Fig. 3f). Anagostic hydrogen bonding of the amine proton indicates high basicity of the metal ion. For the unproductive oxidative addition back to parent 1, which fully proceeds on the singlet potential energy surface, a sizable barrier (TS A/1 : ΔG = 13.8 kcal mol–1, Supplementary Fig. 45) was found that is in agreement with a persistent photoproduct on the (ps) timescale of the transient spectroscopy experiments. Carbon dioxide binding stabilizes A by 7.0 kcal mol–1 giving side-on CO2 complex [Ni0(CO2)(HPNP)] (B). Alternatively, explicit solvent modeling produced intermediate [Ni0(CO2)(THF-HPNP)] (C) within 2.6 kcal mol–1. Anagostic N–H bonding (B) is in C replaced by a hydrogen bridge to THF. Such a structure could not be found for A, indicating reduced metal basicity upon binding of the π-acceptor CO2. Furthermore, nitrogen is directly bound to the metal in C more closely resembling the {Ni(PNP)} fragment of final product 3. This observation suggests structural flexibility of the pincer at low energetic cost. Proton coupled electron transfer to the CO2 ligand would then complete the reaction sequence. Several intra- and intermolecular routes are conceivable and were found computationally with kinetically competitive barriers below unproductive N–H oxidative addition (TS A/1 ). However, such values should be treated with caution without experimental benchmarking owing to the known difficulties for DFT to reliably describe proton transfer reactions with considerable charge buildup and possible direct solute–solvent interactions28. We therefore prefer to correlate intermediates B/C with the free energy for deprotonation of 3 in THF, which is experimentally accessible upon reaction with a reference base (Supplementary Figs. 26, 27), defining an energetic upper limit for N-to-O proton transfer. Assuming that the proton mobility is sufficient within a [H(THF)xNi(CO2)(PNP)] (D) ion pair the pKip of 3 (20.6) is used, placing D at 35.4 kcal mol–1 well below TS A/1 , which further supports the proposed mechanism.

In summary, a mechanism that evolved from kinetic, spectroscopic, labeling, and chemical trapping experiments supported by DFT calculations explains the photochemical selectivity inversion. Photochemical excitation populates a dissociative state leading to rate-determining conversion to a photoproduct with an overall quantum yield ~5%. Trapping with CO, 3 and 1, respectively, the exclusion of nickel(I) as relevant intermediate, the retention of the Ni–D label, the photochemical timescales and the computed UV/Vis spectroscopic signatures all support the nickel(0) assignment for the immediate photoproduct as a result of intramolecular N–H reductive elimination. Hydroxycarbonyl formation presumably follows CO2 coordination to nickel(0) and proton coupled electron transfer. Hydrogen atom transfer of the photointermediate with 7 can explain the abnormal insertion rate retardation in the presence of added nickel(I) (Fig. 6).

This model implies the notion that the inversion of the CO2 insertion selectivity from normal to abnormal relies on the photochemical umpolung reaction of the hydride ligand to an N–H proton. As a consequence of this electron transfer, the reduced metal center becomes the most basic site and is subject to electrophilic attack by the substrate CO2. This mechanistic picture therefore in several ways expresses an application of metal-ligand cooperation (MLC), which is currently extensively exploited as a strategy for catalyst design29. On one hand, photochemical transfer of the two reducing equivalents stored within the Ni–H bond to the metal presumably drives the overall endergonic abnormal CO2 insertion. On the other hand, the pincer ligand acts as a proton relay and intramolecular proton coupled electron transfer from the amine likely facilitates the CO2 two-electron reduction to the hydroxycarbonyl isomer. Hence, MLC might similarly emerge as a valuable conception for photocatalysis.

## Methods

### Synthesis and characterization

[NiH{N(CHCHPtBu2)2}] (1). [NiBr{N(CHCHPtBu2)2}] (208 mg, 0.420 mmol, 1.00 eq) and LiAlH4 (16 mg, 0.422 mmol, 1.00 eq) are dissolved in 6 mL of THF. After stirring at room temperature for 30 mins, the solvent of the orange solution is removed in vacuo. The orange residue is extracted with pentanes and the resulting solution is filtered over Celite to yield a yellow solution. The solvent is removed in vacuo and the yellow solid is washed with 7 × 2 mL MeOH at 0 °C. The residue is dissolved in 10 mL of pentanes and filtered. After removal of the solvent in vacuo, the yellow solid is dissolved in a minimal amount of pentanes and recrystallized at −36 °C. The supernatant solution is decanted, and again recrystallized at −36 °C. The yellow crystalline material is dried in vacuo to yield 106 mg (0.255 mmol, 61%) of 1. Crystals suitable for X-ray diffraction are obtained by crystallization from pentanes at −36 °C. 31P{1H} NMR (121 MHz, C6D6) δ: 86.2 ppm. 1H NMR (300 MHz, C6D6) δ: 7.20 (ABXX’B’A’, N = │3JA-X + 4JA-X’│ = 18.3 Hz, 3JA-B = 5.0 Hz, 4JH-H = 1.9 Hz, Hz, 2 H, NCH), 4.09 (ABXX’B’A’, N = │2JA-X + 4JA-X’│ = 1.8 Hz, 3JA-B = 5.1 Hz, 4JH-H = 1.8 Hz, 2 H, PCH), (A18XX’A’18, N = │3JA-X + 5JA-X│ = 6.7 Hz, 36 H, PtBu), −18.52 (tp, 2JP-H = 59.4 Hz, 4JH-H = 2.0 Hz, 1 H, NiH) ppm. 13C{1H} NMR (75 MHz, C6D6) δ: 160.8 (AXX’A’, N = │2JA-X + 3JA-X’ │ = 11.8 Hz, NCH), 83.0 (AXX’A’, N = │1JA-X + 3JA-X’│ = 15.8 Hz, PCH), 33.8 (A2XX’A’2, N = │1JA-X + 3JA-X’ │ = 11.1 Hz, PCMe3), 29.8 (A6XX’A’6, N = │2JA-X + 4JA-X’ │ = 2.9 Hz, PCMe3) ppm. IR (KBr): ṽ = 1834.3 cm−1. Anal. Calcd. For C40H41NNiP2 (416.20): C, 57.72; H, 9.93; N, 3.37. Found: C, 57.48 H, 9.80; N, 3.41. MS (LIFDI): m/z (%) 415.1 (100).

[NiD{N(CHCHPtBu2)2}] (1-D). [NiBr{N(CHCHPtBu2)2}] (150 mg, 0.303 mmol, 1.00 eq) and LiAlD4 (13 mg, 0.310 mmol, 1.02 eq) are dissolved in 6 mL of THF. After stirring at room temperature for 30 mins, the solvent of the orange solution is removed in vacuo. The orange residue is extracted with pentanes and the resulting solution is filtered over Celite to yield a yellow solution. The solvent is removed in vacuo and the yellow solid is washed with 7 × 2 mL MeOH at 0 °C. The residue is dissolved in 10 mL of pentanes and filtered. After removal of the solvent in vacuo, the yellow solid is dissolved in a minimal amount of pentanes and recrystallized at −36 °C. The supernatant solution is decanted, and again recrystallized at −36 °C. The yellow crystalline material is dried in vacuo to yield 69 mg (0.165 mmol, 55%) of 1-D. 2H NMR (46 MHz, C6H6) δ: −17.50 (t, 2JH-P = 9.0 Hz, NiD) ppm. IR (THF-d8): ṽ = 1318, 1333 cm−1.

[Ni(OCHO){N(CHCHPtBu2)2}] (2). Complex 1 (2.0 mg, 4.8 µmol, 1.00 eq) is dissolved in 0.3 mL of THF-d8 and filled into a medium wall precision pressure/vacuum valve NMR tube. The sample is degassed by three freeze–pump–thaw cycles. A total of 10 atm CO2 pressure (≥99.5% purity, no further purification) is applied. After 14 days, nearly complete conversion of 1 to 2 is detected. 31P{1H} NMR (203 MHz, THF-d8) δ: 56.1 ppm. 1H NMR (500 MHz, THF-d8) δ: 7.25 (t, 4JH-P = 3.4 Hz, 1 H, OCOH), 6.49 (ABXX’B’A’, N = │3JA-X + 4JA-X’│ = 19.1 Hz, 3JA-B = 5.5 Hz, 2 H, NCH), 4.09 (ABXX’B’A’, N = │2JA-X + 4JA-X’│ = 2.0 Hz, 3JA-B = 5.5 Hz, 2 H, PCH), 1.51 (A18XX’A’18, N = │3JA-X + 5JA-X’│ = 6.8 Hz, 36 H, PtBu) ppm. 13C{1H} NMR (126 MHz, THF-d8) δ: 168.3 (t, 3JC-P = 1.1 Hz, OCOH), 162.9 (AXX’A’, N = │2JA-X + 3JA-X’ │ = 11.0 Hz, NCH), 83.0 (dd, 1JC-P = 19.6 Hz, 3JC-P = 18.7 Hz, PCH), 35.8 (A2XX’A’2, N = │1JA-X + 3JA-X’ │ = 8.5 Hz, PCMe3), 29.0 (A6XX’A’6, N = │2JA-X + 4JA-X’ │ = 2.8 Hz, PCMe3) ppm.

[Ni(CO2H){N(CHCHPtBu2)2}] (3). A solution of 1 (20 mg, 0.048 mmol, 1.00 eq) in benzene (6 mL) is degassed by three pump–freeze–thaw cycles and set under 1 atm of CO2 (≥99.5% purity, no further purification). The reaction mixture is photolyzed (λexc > 305 nm) for 8 hours, followed by washing with 5 × 2 mL of benzene and 5 × 2 mL of pentanes. The product is dissolved in THF and dried in vacuo to yield 3 (15 mg, 0.035 mmol, 73%) as a yellow solid. Crystals suitable for X-ray diffraction are obtained by diffusion of pentanes into a solution of 3 in THF. 31P{1H} NMR (162 MHz, THF-d8) δ: 66.2 ppm. 1H NMR (400 MHz, THF-d8) δ: 9.51 (br, 1 H, CO2H), 6.49 (ABXX’B’A’, N = │3JA-X + 4JA-X’│ = 18.4 Hz, 3JA-B = 5.3 Hz, 2 H, NCH), 4.02 (ABXX’B’A’, N = │2JA-X + 4JA-X’│ = 2.0 Hz, 3JA-B = 5.2 Hz, 2 H, PCH), 1.37 (A18XX’A’18, N = │3JA-X + 5JA-X’│ = 6.7 Hz, 36 H, PtBu) ppm. 13C{1H} NMR (126 MHz, THF-d8) δ: 203.6 (t, 2JC-P = 31.1 Hz, CO2H), 161.1 (AXX’A’, N = │2JA-X + 3JA-X’ │ = 10.7 Hz, NCH), 82.4 (AXX’A’, N = │1JA-X + 3JA-X’ │ = 18.6 Hz, PCH), 35.9 (A2XX’A’2, N = │1JA-X + 3JA-X’ │ = 10.2 Hz, PCMe3), 29.3 (A6XX’A’6, N = │2JA-X + 4JA-X’ │ = 2.7 Hz, PCMe3) ppm. IR (KBr): ṽ = 2645, 1584, 1565 cm−1. Anal. Calcd. For C41H41NO2NiP2 (460.20): C, 54.81; H, 8.98; N, 3.04. Found: C, 54.92 H, 8.98; N, 2.91. MS (LIFDI): m/z (%) 459.0 (100).

[Ni(OCO2H){N(CHCHPtBu2)2}] (4). A solution of [Ni(OH){N(CHCHPtBu2)2}] (6) in THF-d8 is degassed by three pump–freeze–thaw cycles set under 1 atm CO2 ( ≥ 99.9993% purity, purification by passing through P4O10, Drierite and cooling to −40 °C) in a J-Young NMR tube. Crystals of 4 suitable for X-ray diffraction are obtained by diffusion of pentanes on a THF solution. 31P{1H} NMR (162 MHz, THF-d8) δ: 54.6 ppm. 1H NMR (400 MHz, THF-d8) δ: 9.28 (br, 1 H, OCO2H), 6.47 (ABXX’B’A’, N = │3JA-X + 4JA-X’│ = 19.1 Hz, 3JA-B = 5.5 Hz, 2 H, NCH), 3.88 (ABXX’B’A’, N = │2JA-X + 4JA-X’│ = 2.0 Hz, 3JA-B = 5.4 Hz, 2 H, PCH), 1.48 (A18XX’A’18, N = │3JA-X + 5JA-X’│ = 6.8 Hz, 36 H, PtBu) ppm. 13C{1H} NMR (126 MHz, THF-d8) δ: 163.0 (AXX’A’, N = │2JA-X + 3JA-X’ │ = 11.1 Hz, NCH), 158.9 (s, OCO2H), 82.2 (AXX’A’, N = │1JA-X + 3JA-X’ │ = 18.8 Hz, PCH), 35.7 (A2XX’A’2, N = │1JA-X + 3JA-X’ │ = 8.6 Hz, PCMe3), 29.0 (A6XX’A’6, N = │2JA-X + 4JA-X’ │ = 2.9 Hz, PCMe3) ppm. Evaporation of a solution of 4 results in CO2 elimination and clean reformation of 6.

[Ni(CO){N(CHCHPtBu2)2}] (5). A solution of [Ni{N(CHCHPtBu2)2}] 7 (10 mg, 0.024 mmol, 1.00 eq) in THF (0.5 mL) is degassed by three freeze–pump–thaw cycles and set under 1 atm of CO in a J-Young NMR tube. The solution is shaken at r.t. for 30 mins and the solvent is evaporated. The black residue is dissolved in pentanes and filtrated. Evaporation of the solvent and drying in vacuo gives 9 mg (0.020 mmol, 83%) of 5 as black solid. Crystals suitable for X-ray diffraction are obtained by crystallization from Et2O at −36 °C. IR (KBr): ṽ = 1910.1 (CO) cm−1. MS (LIFDI): m/z (%) 414.1 (55), 442.1 (45). For EPR characterization see Supplementary Figs. 28, 29.

[Ni(OH){N(CHCHPtBu2)2}] (6). [NiBr{N(CHCHPtBu2)2}] (24 mg, 0.048 mmol, 1.00 eq), KOH (30 mg, 0.535 mmol, 11.15 eq) and 15-crown-5 (10 µL, 0.051 mmol, 1.06 eq) are filled in a J-Young NMR tube and dissolved in 1 mL THF. The solution is warmed to 70 °C for 2 days. After evaporation of the solvent, the orange solid is extracted with pentanes and filtered over celite. The solvent is evaporated and the orange powder is dissolved in pentanes and recrystallized at −36 °C. Removal of the solvent and drying in vacuo yields red, crystalline 6 (14 mg, 0.033 mmol, 69%). Crystals suitable for X-ray diffraction are obtained by crystallization from pentanes at −36 °C. 31P{1H} NMR (162 MHz, THF-d8) δ: 50.3 ppm. 1H NMR (400 MHz, THF-d8) δ: 6.62 (ABXX’B’A’, N = │3JA-X + 4JA-X’│ = 18.8 Hz, 3JA-B = 5.4 Hz, 2 H, NCH), 3.88 (ABXX’B’A’, N = │2JA-X + 4JA-X’│ = 1.9 Hz, 3JA-B = 5.3 Hz, 2 H, PCH), 1.37 (A18XX’A’18, N = │3JA-X + 5JA-X’│ = 6.6 Hz, 36 H, PtBu), −4.88 (t, 3JH-P = 5.6 Hz, OH) ppm. 13C{1H} NMR (126 MHz, THF-d8) δ: 162.8 (AXX’A’, N = │2JA-X + 3JA-X’ │ = 11.8 Hz, NCH), 81.2 (AXX’A’, N = │1JA-X + 3JA-X’ │ = 18.3 Hz, PCH), 35.2 (A2XX’A’2, N = │1JA-X + 3JA-X’ │ = 8.6 Hz, PCMe3), 29.3 (A6XX’A’6, N = │2JA-X + 4JA-X’ │ = 2.9 Hz, PCMe3) ppm. IR (Nujol): ṽ = 3643.8 cm−1. Anal. Calcd. For C40H41NONiP2 (132.19): C, 55.58; H, 9.56; N, 3.24. Found: C, 55.50 H, 9.46; N, 3.12. MS (LIFDI): m/z (%) 431.2 (100).

[Ni{N(CHCHPtBu2)2}] (7). [NiBr{N(CHCHPtBu2)2}] (80 mg, 0.162 mmol, 1.00 eq) and magnesium powder (78 mg, 3.21 mmol, 19.8 eq) are suspended in 5 mL THF and stirred for 30 mins at room temperature accompanied by a color change to orange. The solvent is evaporated, and the residue is dissolved in pentanes and filtered over celite. The solution is dried in vacuo and the orange powder is dissolved in a minimum amount of pentanes and recrystallized at –36 °C. The mother liquor is decanted after 3 days and this procedure is repeated two times, giving 42 mg (0.101 mmol, 62%) of 7 as orange crystals. Crystals suitable for X-ray diffraction are obtained by crystallization from pentanes at −36 °C. 1H NMR (400 MHz, C6D6) δ: 7 (br, tBu), −62 (br, CH) ppm. Anal. Calcd. For C20H40NP2Ni (415.19): C, 57.86; H, 9.71; N, 3.37. Found: C, 57.59 H, 9.48; N, 3.27. MS (LIFDI): m/z (%) 414.1 (100).

[{N(CHCHPtBu2)2}Ni(1κC,2O,O’-13CO2)Ni{κ2P,N-N(CHCHPtBu2)2}] (8). Complex 7 (5.0 mg, 0.012 mmol, 1.00 eq) is dissolved in 0.5 mL C6D6 in a J-Young NMR tube and 300 µL (0.012 mmol, 1.00 eq) 13CO2 are added with a syringe. The solution is kept at room temperature for 24 h. 31P{1H} NMR (162 MHz, C6D6) δ: 72.2 (dd, 5JP-P = 8.7 Hz, 3JP-C = 2.4 Hz, 1 P, (PNP)NiCO2Ni(PN)), 67.8 (d, 2JP-C = 29.1 Hz, 2 P, (PNP)NiCO2Ni(PN)), 4.77 (d, 5JP-P = 8.6 Hz, 1 P, non-coordinating pincer arm) ppm.1H NMR (400 MHz, C6D6) δ: 8.23 (ddd, 3JH-P = 42.4 Hz, 4JH-P = 5.5 Hz, 3JH-H = 5.5 Hz, 1 H, NCH non-coordinating pincer arm), 6.86 (ABXX’B’A’, N = │3JA-X + 4JA-X’│ = 18.4 Hz, 3JA-B = 5.2 Hz, 2 H, NCH), 6.43 (dd, 3JH-P = 20.8 Hz, 2JH-H = 10.5 Hz, 1 H, NCH coordinating pincer arm), 4.69 (dd, 2JH-H = 10.5 ppm, 2JH-P = 6.4 Hz, 1 H, PCH coordinating pincer arm), 3.95 (m, 2 H, PCH), 3.40 (dd, 2JH-P = 4.8 Hz, 2JH-H = 4.8 Hz, 1 H, PCH non-coordinating pincer arm), 1.60 (m, 36 H, PtBu), 1.47 (d, 3JH-P = 13.6 Hz, 18 H, PtBu coordinating pincer arm), 1.25 (d, 3JH-P = 10.9 Hz, 18 H, PtBu non-coordinating pincer arm) ppm. 13C{1H} NMR (101 MHz, C6D6) δ: 236.7 (t, 2JC-P = 29.1 Hz, 3JC-P = 2.4 Hz, CO2), 165.8 (dd, 2JC-P = 23.0 Hz, 3JC-P = 13.7 Hz, NCH non-coordinating pincer arm), 160.9 (AXX’A’, N = │2JA-X + 3JA-X’│ = 10.4 Hz, NCH), 149.8 (d, 2JC-P = 14.1 Hz, NCH), 96.4 (d, 1JC-P = 18.8 Hz, PCH), 82.3 (AXX’A’, N = │1JA-X + 3JA-X’│ = 18.6 Hz, PCH), 74.9 (d, 1JP-C = 47.5, PCH non-coordinating pincer arm), 36.0 (A2XX’A’2, N = │1JA-X + 3JA-X’ │ = 10.3 Hz, PCMe3), 35.0 (d, 1JC-P = 20.9 Hz, PCMe3), 32.4 (d, 1JC-P = 19.5 Hz, PCMe3), 30.0 (d, 2JC-P = 14.3 Hz, PCMe3), 29.7 (br, PCMe3), 28.9 (d, 1JC-P = 4.1 Hz, PCMe3), 30.0 (d, 2JC-P = 14.3 Hz, PCMe3) ppm. Assignment of signals is based on selectively decoupled 1H{31P} and 2D NMR spectra. MS (LIFDI): m/z (%) 872.3 (100).

[{N(CHCHPtBu2)2}Ni(OC(O)O)Ni{N(CHCHPtBu2)2}] (9). Complex 7 (3.2 mg, 0.008 mmol, 1.00 eq) and 3 µL O(SiMe3)2 as internal standard are dissolved in 0.5 mL THF-d8. The solution is degassed by three pump–freeze–thaw cycles and 1 atm CO2 (≥99.9993% purity, purification by passing through P4O10, Drierite and cooling to −40 °C) is applied. The solution is stirred at room temperature for 11 days. Crystals suitable for X-ray diffraction are obtained by crystallization from pentanes at −36 °C. 31P{1H} NMR (162 MHz, THF-d8) δ: 49.2 ppm. 1H NMR (400 MHz, THF-d8) δ: 6.31 (ABXX’B’A’, N = │3JA-X + 4JA-X’│ = 17.9 Hz, 3JA-B = 5.6 Hz, 4 H, NCH), 3.80 (d, 3JH-H = 5.6 Hz, 4 H, PCH), 1.50 (A18XX’A’18, N = │3JA-X + 5JA-X’│ = 6.7 Hz, 72 H, PtBu), ppm. 13C{1H} NMR (126 MHz, C6D6) δ: 162.5 (s, OC(O)O) ppm. MS (LIFDI): m/z (%) 889.3 (100, 13CO32–-isotopologue).

[{N(CHCHPtBu2)2}Ni(1κC,2 κ2O,O’-CO2)Ni{κ2P,C-tBu2PCHCHNHCHCH2PtBu2)}] (10). Synthesis from 1 and CO2: Complex 1 (30 mg, 0.072 mmol, 1.00 eq) is dissolved in 3 mL benzene and 1.8 mL CO2 (0.074 mmol, 1.03 eq, ≥99.9993% purity, purification by passing through P4O10, Drierite and cooling to −40 °C) are added by syringe. The solution is photolyzed (λexc > 305 nm) over night and the solvent is evaporated. The residue is dissolved in pentanes, filtered, and the solvent is evaporated. The residue is suspended in 1 mL acetonitrile and diethyl ether is added dropwise until the solid is dissolved completely. Repeated crystallization at –36 °C and subsequent drying in vacuo gives orange 10 (7 mg, 0.008 mmol, 22%). Crystals suitable for X-ray diffraction are obtained by crystallization from pentanes at −36 °C. Synthesis from 1 and 3: 3 (1.5 mg, 3.3 µmol, 1.00 eq) and 1 (1.4 mg, 3.4 µmol, 1.03 eq) are dissolved in 0.5 mL THF and filled in a J-Young NMR tube and the sample is photolyzed (λexc > 305 nm). 31P{1H} NMR (203 MHz, C6D6) δ: 66.2 (d. 2JP-P = 197.3 Hz, 1 P, (PNP)NiCO2Ni(PC)), 65.0 (d. 2JP-P = 197.1 Hz, 1 P, (PNP)NiCO2Ni(PC)), 36.8 (d, 4JP-P = 7.4 Hz, 1 P, (PNP)NiCO2Ni(PC)), 17.1 (d, 4JP-P = 7.2 Hz, 1 P, non-coordinating pincer arm) ppm. 1H NMR (500 MHz, C6D6) δ: 6.96 (m, 2 H, NCH), 6.48 (ddd, 2JH-P = 27.2 Hz, 3JH-H = 9.6 Hz, 4JH-H = 7.5 Hz, 1 H, PCH), 4.37 (dd, 4JH-P = 7.4 Hz, 4JH-H = 7.4 Hz, 1 H, NH), 4.02 (m, 2 H, PCH), 3.52 (d, 3JH-H = 9.6 Hz, 1 H, NCH), 2.92 (dddd, 3JH-H = 12.4 Hz, 3JH-P = 6.1 Hz, 3JH-H = 1.9 Hz, 3JH-H = 1.9 Hz, 1 H, NCHCH2), 2.72 (ddd, 2JH-H = 14.3 Hz, 2JH-P = 5.9 Hz, 3JH-H = 2.1 Hz, 1 H, NCHCHH), 1.73 (m, 9 H, PtBu), 1.68 (m, 9 H, PtBu), 1.59 (m, 9 H, PtBu), 1.51 (m, 9 H, PtBu), 1.50 (d, 3JH-P = 12.9 Hz, 9 H, PtBu), 1.47 (d, 3JH-P = 13.1 Hz, 9 H, PtBu), 1.47 (NCHCHH, detected by 1H,1H COSY NMR), 1.32 (d, 3JH-P = 10.7 Hz, 9 H, PtBu), 1.19 (d, 3JH-P = 10.9 Hz, 9 H, PtBu) ppm. 13C{1H} NMR (126 MHz, C6D6) δ: 228.3 (dt, 2JC-P = 28.5 Hz, 3JC-P = 3.0 Hz, NiCO2Ni), 160.7 (dd, 3JC-P = 13.9 Hz, 2JC-P = 7.3 Hz, NCH), 160.7 (dd, 3JC-P = 14.0 Hz, 2JC-P = 7.1 Hz, NCH), 149.0 (d, 2JC-P = 7.3 Hz, NCH), 82.6 (dd, 1JC-P = 33.3 Hz, 3JC-P = 9.4 Hz, PCH), 82.4 (dd, 1JC-P = 32.5 Hz, 3JC-P = 9.5 Hz, PCH), 68.0 (dd, 1JC-P = 50.7 Hz, PCH), 36.2 (dd, 1JC-P = 13.8, 3JC-P = 6.0 Hz, PCMe3), 35.9 (dd, 1JC-P = 14.0, 3JC-P = 5.8 Hz, PCMe3), 35.8 (dd, 1JC-P = 14.2, 3JC-P = 6.0 Hz, PCMe3), 35.4 (dd, 1JC-P = 14.2, 3JC-P = 6.4 Hz, PCMe3), 35.0 (d, 1JC-P = 21.4, PCMe3), 34.6 (d, 1JC-P = 24.4, PCMe3), 33.2 (dd, 2JC-P = 30.4 Hz, 2JC-P = 4.1 Hz, NCHNi), 32.6 (d, 1JC-P = 22.9 Hz, PCMe3), 31.2 (d, 1JC-P = 21.6 Hz, PCMe3), 30.5 (d, 2JC-P = 12.7 Hz, PCMe3), 30.2 (dd, 2JC-P = 3.9 Hz, 4JC-P = 1.8 Hz, PCMe3), 30.1 (dd, 2JC-P = 3.8 Hz, 4JC-P = 1.8 Hz, PCMe3), 39.9 (d, 1JC-P = 13.3 Hz, PCMe3), 29.7 (d, 2JC-P = 5.0 Hz, 2xPCMe3), 29.7 (dd, 2JC-P = 3.7 Hz, 4JC-P = 1.8 Hz, PCMe3), 29.6 (dd, 2JC-P = 3.7 Hz, 4JC-P = 1.6 Hz, PCMe3), 29.4 (d, 1JC-P = 26.9 Hz, CH2) ppm. IR (THF-d8): ṽ = 1526.4, 1611.3, 3333.5 cm−1. MS (LIFDI): m/z (%) 873.4 (50), 1392.5 (50).

[(CO)3Ni{κP-HN(CHCHPtBu2)2}] (11). A solution of 1 (9.69 mM, 0.5 mL) in THF-d8 and O(SiMe3)2 as internal standard are filled into a J-Young NMR tube, degassed by three pump–freeze–haw cycles and 1 atm of CO applied. The sample is photolyzed (λexc > 305 nm) for 90 minutes. Crystals of 11 suitable for X-ray diffraction are obtained by crystallization from acetonitrile at −36 °C. 31P{1H} NMR (162 MHz, THF-d8) δ: 39.3 (PNi(CO)3), −5.2 ppm. 1H NMR (400 MHz, THF-d8) δ: 8.10 (dd, 3JH-H = 12.3 Hz, 3JH-H = 12.3 Hz, 1 H, NH), 6.92 (dddd, 3JH-P = 24.8 Hz, 3JH-H = 13.0 Hz, 3JH-H = 10.8 Hz, 4JH-H = 2.4 Hz, 1 H, NCHCHPNi(CO)3), 6.88 (ddd, 3JH-P = 18.1 Hz, 3JH-H = 11.6 Hz, 3JH-H = 9.5 Hz, 1 H, NCH), 4.74 (dd, 3JH-H = 9.5 Hz, 2JH-P = 4.8 Hz, 1 H, PCH), 4.46 (dd, 3JH-H = 10.7 Hz, 2JH-P = 2.4 Hz, 1 H, HCPNi(CO)3), 1.24 (d, 3JH-P = 13.3 Hz, 18 H, tBu2PNi(CO)3), 1.23 (d, 3JH-P = 12.3 Hz, 18 H, PtBu 2 ) ppm. 13C{1H} NMR (101 MHz, THF-d8) δ: 198.5 (d, 2JC-P = 3.8 Hz, Ni(CO)3), 145.5 (d, 2JC-P = 5.8 Hz, NCH), 145.0 (d, 2JC-P = 20.4 Hz, NCH), 95.3 (d, 1JC-P = 17.1 Hz, PCH), 84.9 (d, 1JC-P = 30.7 Hz, PCH), 35.9 (d, 1JC-P = 35.9 Hz, PCMe3), 31.9 (d, 1JC-P = 16.3 Hz, PCMe3), 29.7 (d, 2JC-P = 13.8 Hz, PCMe3), 29.2 (d, 2JC-P = 7.1 Hz, PCMe3) ppm. IR (Nujol): ṽ = 3316.5, 2062.7, 1987.9 cm−1. MS (LIFDI): m/z (%) 443.4 (100). Evaporation in vacuo results in CO loss and reformation of 1.

### Data availability

Detailed descriptions of experimental and spectroscopic methods and results are available within this paper and its supplementary information files. For NMR spectra of the compounds in this article, see Supplementary Figs 114. For quantum chemical methods and results see Supplementary Figs. 3847 and Supplementary Tables 118. The crystallographic data CCDC-1561988–1561994, CCDC-1574302, and CCDC-1574303 can be obtained free of charge from the Cambridge Crystallographic Data Centre (www.ccdc.cam.ac.uk/data_request/cif). All other data are available from the authors upon reasonable request.

## References

1. 1.

Appel, A. M. et al. Frontiers, opportunities, and challenges in biochemical and chemical catalysis of CO2 fixation. Chem. Rev. 113, 6621–6658 (2013).

2. 2.

Volbeda, A. & Fontecilla-Camps, J. C. Structural bases for the catalytic mechanism of Ni-containing carbon monoxide dehydrogenases. Dalton Trans. 3443–3450 (2005).

3. 3.

Hammouche, M. et al. Chemical catalysis of electrochemical reactions. Homogeneous catalysis of the electrochemical reduction of carbon dioxide by iron(“0”) porphyrins. Role of the addition of magnesium cations. J. Am. Chem. Soc. 113, 8455–8466 (1991).

4. 4.

Fujita, E., Furenlid, L. R. & Renner, M. W. Direct XANES evidence for charge transfer in Co-CO2 complexes. J. Am. Chem. Soc. 119, 4549–4550 (1997).

5. 5.

Feller, M. et al. Reductive cleavage of CO2 by metal-ligand-cooperation mediated by an iridium pincer complex. J. Am. Chem. Soc. 138, 6445–6454 (2016).

6. 6.

Sato, S., Morikawa, T., Kajino, T. & Ishitani, O. A highly efficient mononuclear iridium complex photocatalyst for CO2 reduction under visible light. Angew. Chem. Int. Ed. 52, 988–992 (2013).

7. 7.

Garg, K. et al. Striking differences in properties of geometric isomers of [Ir(tpy)- (ppy)H]+: experimental and computational studies of their hydricities, interaction with CO2, and photochemistry. Angew. Chem. Int. Ed. 54, 14128–14132 (2015).

8. 8.

Bourrez, M. et al. Pulsed-EPR evidence of a manganese(II) hydroxycarbonyl intermediate in the electrocatalytic reduction of carbon dioxide by a manganese bipyridyl derivative. Angew. Chem. Int. Ed. 126, 240–243 (2014).

9. 9.

Rakowski DuBois, M. & DuBois, D. L. Development of molecular electrocatalysts for CO2 reduction and H2 production/oxidation. Acc. Chem. Res. 42, 1974–1982 (2009).

10. 10.

Schneider, J., Jia, H., Muckerman, J. T. & Fujita, E. Thermodynamics and kinetics of CO2, CO, and H+ binding to the metal centre of CO2 reduction catalysts. Chem. Soc. Rev. 41, 2036–2051 (2012).

11. 11.

Constentin, C., M. Robert, M. & Savéant, J.-M. Current issues in molecular catalysis illustrated by iron porphyrins as catalysts of the CO2-to-CO electrochemical conversion. Acc. Chem. Res. 48, 2996–3006 (2015).

12. 12.

Berardi, S. et al. Molecular artificial photosynthesis. Chem. Soc. Rev. 43, 7501–7519 (2014).

13. 13.

Jessop, P. G., Ikariya, T. & Noyori, R. Homogeneous hydrogenation of carbon dioxide. Chem. Rev. 95, 259–272 (1995).

14. 14.

Jessop, P. G., Joó, F. & Tai, C.-C. Recent advances in the homogeneous hydrogenation of carbon dioxide. Coord. Chem. Rev. 248, 2425–2442 (2004).

15. 15.

Wang, W.-H., Himeda, Y., Muckerman, J. T., Manbeck, G. F. & Fujita, E. CO2 hydrogenation to formate and methanol as an alternative to photo- and electrochemical CO2 reduction. Chem. Rev. 115, 12936–12973 (2015).

16. 16.

Alberico, E. & Nielsen, M. Towards a methanol economy based on homogeneous catalysis: methanol to H2 and CO2 to methanol. Chem. Commun. 51, 6714–6725 (2015).

17. 17.

Fan, T., Chen, X. & Lin, Z. Theoretical studies of reactions of carbon dioxide mediated and catalysed by transition metal complexes. Chem. Commun. 48, 10808–10828 (2012).

18. 18.

Yoo, C., Kim, J. & Lee, Y. Synthesis and reactivity of nickel(II) hydroxycarbonyl species, NiCOOH-κC. Organometallics 32, 7195–7203 (2013).

19. 19.

Yoo, C. & Lee, Y. Carbon dioxide binding at a Ni/Fe center: synthesis and characterization of Ni(η1-CO2C) and Ni-μ-CO2C2 O,O′-Fe. Chem. Sci. 8, 600–605 (2017).

20. 20.

Yoo, C. & Lee, Y. A T-shaped nickel(I) metalloradical species. Angew. Chem. Int. Ed. 56, 9502–9506 (2017).

21. 21.

Chakraborty, S., Bhattacharya, P., Dai, H. & Guan, H. Nickel and iron pincer complexes as catalysts for the reduction of carbonyl compounds. Acc. Chem. Res. 48, 1995–2003 (2015).

22. 22.

Schneck, F., Finger, M., Tromp, M. & Schneider, S. Chemical non-innocence of an aliphatic PNP pincer ligand. Chem. Eur. J. 23, 33–37 (2017).

23. 23.

Zimmermann, P. & Limberg, C. Activation of small molecules at nickel(I) moieties. J. Am. Chem. Soc. 139, 4233–4242 (2017).

24. 24.

Ingleson, M. J. et al. Influence of the d-electron count on CO binding by three-coordinate [(tBu2PCH2SiMe2)2N]Fe, -Co, and –Ni. Inorg. Chem. 47, 407–409 (2008).

25. 25.

Rettenmeier, C., Wadepohl, H. & Gade, L. H. Electronic structure and reactivity of nickel(I) pincer complexes: their aerobic transformation to peroxo species and site selective C–H oxygenation. Chem. Sci. 7, 3533–3542 (2016).

26. 26.

Liang, L.-C. et al. Divergent carbonylation reactivity preferences of nickel complexes containing amido pincer ligands: migratory insertion versus reductive elimination. Organometallics 31, 700–708 (2012).

27. 27.

Perutz, R. N. & Procacci, B. Photochemistry of transition metal hydrides. Chem. Rev. 116, 8506–8544 (2016).

28. 28.

Ho, J. & Coote, M. L. A universal approach for continuum solvent pK a calculations: are we there yet? Theor. Chem. Acc. 125, 3–21 (2010).

29. 29.

Khusnutdinova, J. R. & Milstein, D. Metal-ligand cooperation. Angew. Chem. Int. Ed. 54, 12236–12273 (2015).

## Acknowledgements

This work was supported by grants from the European Research Council (ERC Grant Agreement 646747) and the Deutsche Forschungsgemeinschaft (CRC 1073, Project C07).

## Author information

Authors

### Contributions

F.S. planned and performed all synthetic work and characterization (except transient spectroscopy) supervised by S.S. A.C.S. assisted the EPR spectroscopic examinations and C.W. the crystallographic characterizations. M.F. carried out the quantum chemical study. J.A. carried out the transient spectroscopy experiments supervised by D.S. The paper was co-written by F.S. and S.S. and all authors discussed the results and commented on the manuscript.

### Corresponding author

Correspondence to Sven Schneider.

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Schneck, F., Ahrens, J., Finger, M. et al. The elusive abnormal CO2 insertion enabled by metal-ligand cooperative photochemical selectivity inversion. Nat Commun 9, 1161 (2018). https://doi.org/10.1038/s41467-018-03239-3

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