New Spectroelectrochemical Insights into Manganese and Rhenium Bipyridine Complexes as Catalysts for the Electrochemical Reduction of Carbon Dioxide

This study aimed to demonstrate the behavior of different complexes using IR spectroelectrochemistry (SEC), a technique that combines IR spectroscopy with electrochemistry. Four different Mn and Re catalysts for electrochemical CO2 reduction were studied in dry acetonitrile. In the case of Mn(apbpy)(CO)3Br (apbpy = 4(4-aminophenyl)-2,2′-bipyridine), SEC suggested that a very slow catalytic reduction of CO2 also occurs in acetonitrile in the absence of proton donors, but at rather negative potentials. In contrast, the corresponding Re(apbpy)(CO)3Br clearly demonstrated slow catalytic conversion at the first reduction potential. Switching to saturated CO2 solutions in a mixture of acetonitrile and 5% water as a proton donor, the SEC of Mn(apbpy)(CO)3Br displayed a faster catalytic behavior.


Introduction
The constant increase in CO 2 concentration in the atmosphere and the depletion of fossil fuels have raised serious worldwide environmental and energy-related concerns [1].Thus, one of the most prominent contemporary research topics is the conversion of CO 2 into fuels using green, eco-friendly approaches and sustainable methodologies.Solar energy is a perfect engine that fits these requirements for driving the chemical conversion of CO 2 (employing it as an energy vector in a carbon-based cycle), to be used as a raw starting material for fuel production [2].Although direct artificial photosynthesis is conceptually attractive [3,4], its real-world application is still not optimal, and parallel approaches are actively being explored.An instantaneous and clean way of capturing the sun's power is its direct conversion into electric energy using photovoltaic cells.The possible exploitation of this energy for the electrochemical reduction of CO 2 into chemicals with higher energy content has attracted several researchers, resulting in the exponential growth of the number of papers that have lately appeared in this field.
The present contribution illustrates recent results of the spectroelectrochemical technique applied to the study of CO 2 reduction using selected Mn and Re organometallic complexes.Cyclic voltammetry (CV) is a relatively rapid technique (one can envisage that the scan rate dictates the time scale of the experiments, which usually last a fraction of a second), whereas SEC is a slower technique (with a time scale in the order of minutes); however, the production of reduced/oxidized species in higher quantities enables the recording of their spectroscopic properties.SEC has been proven to be a very versatile technique, tested in different conditions and with different substrates and catalysts, assisting, in certain circumstances, with the interpretation of reduction mechanisms and the identification of intermediates.For example, in 2012, SEC was used to investigate CO 2 reduction on a gold surface, making it possible to propose a reduction mechanism for CO 2 in working conditions [5].SEC has also been used several times to determine the mechanism of carbon dioxide reduction with different complexes and different metals.With Ru metal used for molecular and cluster catalysts, SEC is a fundamental technique employed for observing CO 2 reduction products (CO, CO 3  2− , and HCOO − ), as well as another two not fully identified carboxylate species [6,7].The literature also reports examples of catalysts containing Co and Ni metals complexes, in which SEC has been used to identify intermediates, with interesting results [8,9].Similarly, for complexes based on Mn and Re and with bipyridine-type structures, such as those used in this study, SEC has been used for discovering both radical intermediates and CO 2 reduction products, in agreement with those previously reported [10,11].
We explored the activities of Re and Mn catalysts bearing bipyridine-like (bpy) units towards the electrochemical and photochemical reduction of CO 2 [1,[12][13][14].Complexes 1-4 (Scheme 1) were synthesized here, following a previously reported procedure [15,16]; their electrochemical behavior is herein described in different conditions, as are their SEC properties and new insights into the overall mechanism.Cyclic voltammetry (CV) of Mnbpy derivatives usually presents two subsequent chemically irreversible reductions [17], but only the second one, and only when in the presence of proton sources, is active toward CO 2 conversion.Complex 1, when chemically bonded to an electrode surface via 4(4aminophenyl)-2,2 -bipyridine functionality (apbpy), shows extremely interesting catalytic properties in water, with a turnover number (TON) of up to 164,000 [12,13].In contrast, Re-bpy complexes typically initially undergo a reversible reduction followed by a second irreversible and catalytically active reduction, even in the absence of proton donors.In very rare cases (and in kinetically much slower systems), Re-bpy derivatives can exhibit catalytic activities even at the first reduction peak, in a so-called slow regime [18].We herein demonstrate via SEC that Re complex 2 is catalytically active at the initial reduction.SEC experiments were employed as a powerful tool to elucidate the mechanism details of CO 2 reduction [10,19,20] in the case of analogous Mn and Re derivatives [14,[21][22][23][24].The SEC experiments and properties of the complexes are herein studied in a homogeneous phase for the first time.
Molecules 2023, 28, x FOR PEER REVIEW 2 of 15 however, the production of reduced/oxidized species in higher quantities enables the recording of their spectroscopic properties.SEC has been proven to be a very versatile technique, tested in different conditions and with different substrates and catalysts, assisting, in certain circumstances, with the interpretation of reduction mechanisms and the identification of intermediates.For example, in 2012, SEC was used to investigate CO2 reduction on a gold surface, making it possible to propose a reduction mechanism for CO2 in working conditions [5].SEC has also been used several times to determine the mechanism of carbon dioxide reduction with different complexes and different metals.With Ru metal used for molecular and cluster catalysts, SEC is a fundamental technique employed for observing CO2 reduction products (CO, CO3 2− , and HCOO − ), as well as another two not fully identified carboxylate species [6,7].The literature also reports examples of catalysts containing Co and Ni metals complexes, in which SEC has been used to identify intermediates, with interesting results [8,9].Similarly, for complexes based on Mn and Re and with bipyridine-type structures, such as those used in this study, SEC has been used for discovering both radical intermediates and CO2 reduction products, in agreement with those previously reported [10,11].
We explored the activities of Re and Mn catalysts bearing bipyridine-like (bpy) units towards the electrochemical and photochemical reduction of CO2 [1,[12][13][14].Complexes 1-4 (Scheme 1) were synthesized here, following a previously reported procedure [15,16]; their electrochemical behavior is herein described in different conditions, as are their SEC properties and new insights into the overall mechanism.Cyclic voltammetry (CV) of Mnbpy derivatives usually presents two subsequent chemically irreversible reductions [17], but only the second one, and only when in the presence of proton sources, is active toward CO2 conversion.Complex 1, when chemically bonded to an electrode surface via 4(4-aminophenyl)-2,2′-bipyridine functionality (apbpy), shows extremely interesting catalytic properties in water, with a turnover number (TON) of up to 164,000 [12,13].In contrast, Re-bpy complexes typically initially undergo a reversible reduction followed by a second irreversible and catalytically active reduction, even in the absence of proton donors.In very rare cases (and in kinetically much slower systems), Re-bpy derivatives can exhibit catalytic activities even at the first reduction peak, in a so-called slow regime [18].We herein demonstrate via SEC that Re complex 2 is catalytically active at the initial reduction.SEC experiments were employed as a powerful tool to elucidate the mechanism details of CO2 reduction [10,19,20] in the case of analogous Mn and Re derivatives [14,[21][22][23][24].The SEC experiments and properties of the complexes are herein studied in a homogeneous phase for the first time.Complexes 3 and 4 of the present set were selected for comparison, considering the promising and relatively high TON values observed for the electrochemical conversion of CO2 in a homogeneous solution.Complex 3 possessed a push-and-pull substituent group on the bpy ligand, resulting in a net negligible shift in the reduction potential with respect to the Mn-bpy complex without substituents, whereas good catalytic activities were recorded in both the CV and constant potential electrolysis (CPE) experiments.Complex 4, bearing a strong electron-donor ligand, showed a shift in reduction processes to more negative potentials, with improvements in the catalytic activity [16].We selected these two different methodologies to enhance the catalytic behavior of the catalysts, and tested them in SEC experiments.The four complexes, which are promising catalysts [15,16] (see Table 1), were studied in comparative tests under SEC conditions.Complexes 3 and 4 of the present set were selected for comparison, considering the promising and relatively high TON values observed for the electrochemical conversion of CO 2 in a homogeneous solution.Complex 3 possessed a push-and-pull substituent group on the bpy ligand, resulting in a net negligible shift in the reduction potential with respect to the Mn-bpy complex without substituents, whereas good catalytic activities were recorded in both the CV and constant potential electrolysis (CPE) experiments.Complex 4, bearing a strong electron-donor ligand, showed a shift in reduction processes to more negative potentials, with improvements in the catalytic activity [16].We selected these two different methodologies to enhance the catalytic behavior of the catalysts, and tested them in SEC experiments.The four complexes, which are promising catalysts [15,16] (see Table 1), were studied in comparative tests under SEC conditions.1) at the first reduction potential showed conversion of the original ν(CO) bands (2026, 1933, and 1922 cm −1 ) into four ν(CO) bands (1973,1931,1878, and 1852 cm −1 ).This behavior is typical for the formation of a Mn-Mn dimer, which has recently been demonstrated by Daasbjerg [23] to proceed, for the similar Mn(bpy)(CO) 3 Br complex, via its 2e − reduction involving an extremely rapid Br − release, and the subsequent rapid chemical reaction between the penta-coordinated anion and the neutral Mn complex.The second reduction of 1, which occurred at more negative potentials, split the dimer [10,[25][26][27][28], leading to the monomeric penta-coordinated anion [Mn(apbpy)(CO) 3 ] − This anion exhibits two ν(CO) bands, at 1909 and 1811 cm −1 (two wider, almost degenerate vibration modes) (Figure 2).The overall mechanism is briefly summarized in Scheme 2.
Molecules 2023, 28, x FOR PEER REVIEW 3 of 15 CV of Mn(apbpy)(CO)3Br (1) in dry acetonitrile (MeCN) displayed two chemically irreversible reductions at Ep = −1.21V and Ep = −1.41V vs. Ag/AgCl [15].In situ SEC spectra of 1 (Figure 1) at the first reduction potential showed conversion of the original ν(CO) bands (2026,1933, and 1922 cm −1 ) into four ν(CO) bands (1973,1931,1878, and 1852 cm −1 ).This behavior is typical for the formation of a Mn-Mn dimer, which has recently been demonstrated by Daasbjerg [23] to proceed, for the similar Mn(bpy)(CO)3Br complex, via its 2e − reduction involving an extremely rapid Br ‾ release, and the subsequent rapid chemical reaction between the penta-coordinated anion and the neutral Mn complex.The second reduction of 1, which occurred at more negative potentials, split the dimer [10,[25][26][27][28], leading to the monomeric penta-coordinated anion [Mn(apbpy)(CO)3] − This anion exhibits two ν(CO) bands, at 1909 and 1811 cm −1 (two wider, almost degenerate vibration modes) (Figure 2).The overall mechanism is briefly summarized in Scheme 2.   No significant difference was observed when the SEC experiments (first and second reduction) were performed with the solution saturated with carbon dioxide.Only when the reduction potential was changed to more negative values, behind the second reduction peak of 1, did the band of dissolved CO2 at 2342 cm −1 decrease (Figure S1) and bands at 1684 and 1643 cm −1 increase.These two bands are a ributed to the formation of the HCO3 −- /CO3 2− system that usually appears after CO2 reduction [10,29].Although we cannot completely exclude a direct reduction in CO2, the potential applied (−1.75 V vs. Ag/AgCl) is not sufficiently negative to reduce pure CO2-saturated solution in dry acetonitrile [15]; therefore, these observations suggest a slow catalytic process not evident in faster CV experiments.To the best of our knowledge, this is the first a empt to perform reduction and SEC procedures on Mn complexes at this negative potential in the absence of proton donors.In the relatively short SEC process time (albeit much longer with respect to CV), it is possible to assert that the two bands at 1909 and 1811 cm −1 partially lose intensity, but at the same time, the bands at 1684 and 1643 cm −1 sharply increase (Figure S1), which can be interpreted by a slow catalytic process, with probable catalyst decomposition over a longer time and at such negative potentials.
SEC performed at the second reduction peak (i.e., −1.41 V), but employing acetonitrile solution containing 5% of water, exhibited typical catalytic CO2 reduction (Figure 3), a decrease in the CO2 absorption band at 2343 cm −1 , and increases in bands of HCO3 − /CO3 2− Scheme 2. Summary of the overall mechanism of [Mn(bpy-type)(CO) 3 Br] complexes leading to the Mn anion, the active catalyst in electrochemical CO 2 reduction.
No significant difference was observed when the SEC experiments (first and second reduction) were performed with the solution saturated with carbon dioxide.Only when the reduction potential was changed to more negative values, behind the second reduction peak of 1, did the band of dissolved CO 2 at 2342 cm −1 decrease (Figure S1) and bands at 1684 and 1643 cm −1 increase.These two bands are attributed to the formation of the HCO 3 − /CO 3 2− system that usually appears after CO 2 reduction [10,29].Although we cannot completely exclude a direct reduction in CO 2 , the potential applied (−1.75 V vs. Ag/AgCl) is not sufficiently negative to reduce pure CO 2 -saturated solution in dry acetonitrile [15]; therefore, these observations suggest a slow catalytic process not evident in faster CV experiments.To the best of our knowledge, this is the first attempt to perform reduction and SEC procedures on Mn complexes at this negative potential in the absence of proton donors.In the relatively short SEC process time (albeit much longer with respect to CV), it is possible to assert that the two bands at 1909 and 1811 cm −1 partially lose intensity, but at the same time, the bands at 1684 and 1643 cm −1 sharply increase (Figure S1), which can be interpreted by a slow catalytic process, with probable catalyst decomposition over a longer time and at such negative potentials.SEC performed at the second reduction peak (i.e., −1.41 V), but employing acetonitrile solution containing 5% of water, exhibited typical catalytic CO 2 reduction (Figure 3), a decrease in the CO 2 absorption band at 2343 cm −1 , and increases in bands of HCO 3 − /CO 3 2− at 1684 and 1643 cm −1 .Other bands showed a trend similar to that presented in Figure 2, i.e., the reduction of the dimer [Mn(apbpy)(CO) 3 ] 2 into a monomeric anion.These results agree with previous observations from cyclic voltammetry and exhaustive electrolysis experiments [15], demonstrating electrocatalysis in the presence of proton donors.

Re(apbpy)(CO) 3 Cl
CV of the rhenium complex 2 (Figure 4) showed an initial reversible reduction at E 1/2 = −1.28V, and a second irreversible reduction at E p = −1.74V vs. Ag/AgCl.SEC of 2 showed that the reduction mechanism significantly differed from that observed for Mn analogue 1.
On the reduction at the first peak (Figure 5), the original three ν(CO) bands (2021, 1915, and 1897 cm −1 ) shifted to lower wavenumbers (1997, 1886, and 1866 cm −1 ), but the characteristics of the three-band spectrum, and consequently, the coordination symmetry, remained unchanged.Only a low-energy shift in the CO bands due to the electrostatic effect of the electron uptake is evident in Figure 5, indicating quantitative conversion of the neutral species into the chemically stable radical anion.Hence, the single-electron reduction product remained hexacoordinated, and no dimerization took place, in contrast to Mn complex 1.After the electrolysis at the first peak (Figure 5), the bands of the double-electron reduction product also appeared, due to the close potentials of the first and second reduction peaks.Development of the bands of the double-electron reduction product continued during reduction at the second peak (Figure 6); as a result, the spectrum consisted of two main bands at 1986 cm −1 and 1850 cm −1 (two wider, almost degenerate vibrations), corresponding to the anion [Re(apbpy)(CO) 3 ] − .
Molecules 2023, 28, x FOR PEER REVIEW 5 of 15 at 1684 and 1643 cm −1 .Other bands showed a trend similar to that presented in Figure 2, i.e., the reduction of the dimer [Mn(apbpy)(CO)3]2 into a monomeric anion.These results agree with previous observations from cyclic voltammetry and exhaustive electrolysis experiments [15], demonstrating electrocatalysis in the presence of proton donors.

Re(apbpy)(CO)3Cl
CV of the rhenium complex 2 (Figure 4) showed an initial reversible reduction at E1/2 = −1.28V, and a second irreversible reduction at Ep = −1.74V vs. Ag/AgCl.SEC of 2 showed that the reduction mechanism significantly differed from that observed for Mn analogue 1.On the reduction at the first peak (Figure 5), the original three ν(CO) bands (2021, 1915, and 1897 cm −1 ) shifted to lower wavenumbers (1997, 1886, and 1866 cm −1 ), but the characteristics of the three-band spectrum, and consequently, the coordination symmetry, remained unchanged.Only a low-energy shift in the CO bands due to the electrostatic effect of the electron uptake is evident in Figure 5, indicating quantitative conversion of the neutral species into the chemically stable radical anion.Hence, the single-electron reduction product remained hexacoordinated, and no dimerization took place, in contrast to Mn complex 1.After the electrolysis at the first peak (Figure 5), the bands of the doubleelectron reduction product also appeared, due to the close potentials of the first and second reduction peaks.Development of the bands of the double-electron reduction product continued during reduction at the second peak (Figure 6); as a result, the spectrum consisted of two main bands at 1986 cm −1 and 1850 cm SEC experiments performed under CO2 revealed the catalytic activity of complex 2. Figure 7 clearly shows that carbon dioxide is catalytically reduced at potentials of the first reduction peak of the complex.The decrease in the CO2 concentration in the solution (band at 2342 cm −1 ) and the formation of the products (HCO3 − /CO3 2− , bands around 1685 and 1645 cm −1 ) take place simultaneously with the reductive transition of 2 to 2 ‾ .The results thus show that although 2 ‾ does not lose a Cl atom to form the penta-coordinated complex in the CV time scale, the coordination bond is labilized, and the halide can be substituted by solvent or substrate (CO2).The labilized coordination site plays a key role SEC experiments performed under CO 2 revealed the catalytic activity of complex 2. Figure 7 clearly shows that carbon dioxide is catalytically reduced at potentials of the first reduction peak of the complex.The decrease in the CO 2 concentration in the solution (band at 2342 cm −1 ) and the formation of the products (HCO 3 − /CO 3 2− , bands around 1685 and 1645 cm −1 ) take place simultaneously with the reductive transition of 2 to 2 − .The results thus show that although 2 − does not lose a Cl atom to form the penta-coordinated complex in the CV time scale, the coordination bond is labilized, and the halide can be substituted by solvent or substrate (CO 2 ).The labilized coordination site plays a key role in the catalytic mechanism.Indications that the catalytically active complex does not necessarily need to be formed through the second reduction of a bipyridine-tricarbonyl complex have previously been posited for similar complexes [14].Complex 2 is a clear example, demonstrated by a relatively rapid technique such as SEC, that exhibits catalytic activity when reduced only at the initial single-electron step.
Molecules 2023, 28, x FOR PEER REVIEW 7 of 15 in the catalytic mechanism.Indications that the catalytically active complex does not necessarily need to be formed through the second reduction of a bipyridine-tricarbonyl complex have previously been posited for similar complexes [14].Complex 2 is a clear example, demonstrated by a relatively rapid technique such as SEC, that exhibits catalytic activity when reduced only at the initial single-electron step.The metal-halogen bond (M-X) is much weaker in Mn complex 1 than in Re complex 2. For example, whereas complex 1 does not normally release Br -in MeCN solution at r.t., rapid solvolysis of the Mn-Br bond in MeCN has been observed in the Mn complex carrying a bpy ligand modified with a hydroxyphenyl moiety [21], even at open circuit potentials.
The kinetics of the halogen-releasing process are greatly enhanced in Mn complexes whenever the corresponding reduced species are considered, accounting for the chemically irreversible and the reversible first reduction steps of 1 and 2, respectively.DFT relaxed geometry scans of 1 ‾ and 2 ‾ as a function of M-X distances (Figure 8) clearly show that the radical anion Mn complex 1 ‾ has a much higher propensity to release the halogen than the Re counterpart 2 ‾ .This is confirmed by the fact that the Mn-Br distance of the optimized geometry 1 ‾ is 0.294 Å longer than that of 1, while the Re-Cl bond of 2 -is only 0.052 Å longer than that of 2 (see the Supplementary Materials for details).The metal-halogen bond (M-X) is much weaker in Mn complex 1 than in Re complex 2. For example, whereas complex 1 does not normally release Br -in MeCN solution at r.t., rapid solvolysis of the Mn-Br bond in MeCN has been observed in the Mn complex carrying a bpy ligand modified with a hydroxyphenyl moiety [21], even at open circuit potentials.

Mn
The kinetics of the halogen-releasing process are greatly enhanced in Mn complexes whenever the corresponding reduced species are considered, accounting for the chemically irreversible and the reversible first reduction steps of 1 and 2, respectively.DFT relaxed geometry scans of 1 − and 2 − as a function of M-X distances (Figure 8) clearly show that the radical anion Mn complex 1 − has a much higher propensity to release the halogen than the Re counterpart 2 − .This is confirmed by the fact that the Mn-Br distance of the optimized geometry 1 − is 0.294 Å longer than that of 1, while the Re-Cl bond of 2 − is only 0.052 Å longer than that of 2 (see the Supplementary Materials for details).
rying a bpy ligand modified with a hydroxyphenyl moiety [21], even at open circuit potentials.
The kinetics of the halogen-releasing process are greatly enhanced in Mn complexes whenever the corresponding reduced species are considered, accounting for the chemically irreversible and the reversible first reduction steps of 1 and 2, respectively.DFT relaxed geometry scans of 1 ‾ and 2 ‾ as a function of M-X distances (Figure 8) clearly show that the radical anion Mn complex 1 ‾ has a much higher propensity to release the halogen than the Re counterpart 2 ‾ .This is confirmed by the fact that the Mn-Br distance of the optimized geometry 1 ‾ is 0.294 Å longer than that of 1, while the Re-Cl bond of 2 -is only 0.052 Å longer than that of 2 (see the Supplementary Materials for details).The three original ν(CO) bands (2026, 1932, and 1921 cm −1 ) were converted at the first single-electron reduction (Figure 10) into four bands of the dimer (1974,1932,1878, and 1854 cm −1 ).The coincidence of the bands of the original complex and of the single-electron reduction product at 1932 cm −1 caused a poorly distinguishable spectral change in this region.The second reduction (Figure 11) led to the anionic species [Mn(bpy-4,4′-CF3-NMe2)(CO)3] ‾ with the characteristic two-band spectrum (1917, 1816 (wide) cm −1 ) in the carbonyl region.A small band at 2047 cm −1 appeared as transient, and could be a ributed to solvent-substituted species [Mn(bpy-4,4′-CF3-NMe2)(CO)3(MeCN)] + , whose formation can be facilitated due to an electron-transfer catalytic (ETC) effect, as observed in similar [21].The three original ν(CO) bands (2026, 1932, and 1921 cm −1 ) were converted at the first single-electron reduction (Figure 10) into four bands of the dimer (1974,1932,1878, and 1854 cm −1 ).The coincidence of the bands of the original complex and of the single-electron reduction product at 1932 cm −1 caused a poorly distinguishable spectral change in this region.The second reduction (Figure 11) led to the anionic species [Mn(bpy-4,4 -CF 3 -NMe 2 )(CO) 3 ] −1 with the characteristic two-band spectrum (1917, 1816 (wide) cm −1 ) in the carbonyl region.A small band at 2047 cm −1 appeared as transient, and could be attributed to solvent-substituted species [Mn(bpy-4,4 -CF 3 -NMe 2 )(CO) 3 (MeCN)] + , whose formation can be facilitated due to an electron-transfer catalytic (ETC) effect, as observed in similar complexes [21].
reduction product at 1932 cm −1 caused a poorly distinguishable spectral change in this region.The second reduction (Figure 11) led to the anionic species [Mn(bpy-4,4′-CF3-NMe2)(CO)3] ‾ with the characteristic two-band spectrum (1917, 1816 (wide) cm −1 ) in the carbonyl region.A small band at 2047 cm −1 appeared as transient, and could be a ributed to solvent-substituted species [Mn(bpy-4,4′-CF3-NMe2)(CO)3(MeCN)] + , whose formation can be facilitated due to an electron-transfer catalytic (ETC) effect, as observed in similar complexes [21].SEC experiments with carbon dioxide-saturated solution showed that no CO2 reduction takes place during electrolysis at potentials of the first reduction wave, and the spectral change (Figure S2) resembles that under argon.Carbon dioxide reduction starts only at the potential of the second reduction peak (Figure S5, see bands HCO3 − /CO3 2− at 1685 and 1647 cm −1 ), similarly to that observed for compound 1.

Re(bpy-4,4′-NMe2)(CO)3Cl
CV of Re complex 4 (Figure 12) exhibited a single chemically irreversible doubleelectron reduction at Ep = −1.82V, and another much more negative reduction (ligandcentered) at Ep = −2.60V vs. Ag/AgCl.The two single-electron reduction steps were merged in the case of complex 4 into the one double-electron peak observed in CV [16].However, a carefully controlled spectroelectrochemical reduction revealed that the reduction steps could be distinguished according to spectral changes.The first spectral change during the reduction process resembled that observed for single-electron reduction of complex 2. Original carbonyl bands (2014, 1903, 1883 cm −1 ) were shifted to lower wavelengths (1998, 1982, 1864 cm −1 , Figure 13).Continued reduction at only slightly more negative potential (two merged reduction steps) (Figure 14) produced an anion ([Re(bpy-4,4′-NMe2)(CO)3] ‾ ) with the ν(CO) bands at 1986 and 1862 (wide) cm −1 , similarly to what was observed for the analogous rhenium complex 2. SEC experiments with carbon dioxide-saturated solution showed that no CO 2 reduction takes place during electrolysis at potentials of the first reduction wave, and the spectral change (Figure S2) resembles that under argon.Carbon dioxide reduction starts only at the potential of the second reduction peak (Figure S5, see bands HCO 3 − /CO 3 2− at 1685 and 1647 cm −1 ), similarly to that observed for compound 1.

Re(bpy-4,4 -NMe 2 )(CO) 3 Cl
CV of Re complex 4 (Figure 12) exhibited a single chemically irreversible doubleelectron reduction at E p = −1.82V, and another much more negative reduction (ligandcentered) at E p = −2.60V vs. Ag/AgCl.The two single-electron reduction steps were merged in the case of complex 4 into the one double-electron peak observed in CV [16].However, a carefully controlled spectroelectrochemical reduction revealed that the reduction steps could be distinguished according to spectral changes.The first spectral change during the reduction process resembled that observed for single-electron reduction of complex 2. Original carbonyl bands (2014, 1903, 1883 cm −1 ) were shifted to lower wavelengths (1998, 1982, 1864 cm −1 , Figure 13).Continued reduction at only slightly more negative potential (two merged reduction steps) (Figure 14) produced an anion ([Re(bpy-4,4 -NMe 2 )(CO) 3 ] − ) with the ν(CO) bands at 1986 and 1862 (wide) cm −1 , similarly to what was observed for the analogous rhenium complex 2. tion steps could be distinguished according to spectral changes.The first spectral change during the reduction process resembled that observed for single-electron reduction of complex 2. Original carbonyl bands (2014, 1903, 1883 cm −1 ) were shifted to lower wavelengths (1998, 1982, 1864 cm −1 , Figure 13).Continued reduction at only slightly more negative potential (two merged reduction steps) (Figure 14) produced an anion ([Re(bpy-4,4′-NMe2)(CO)3] ‾ ) with the ν(CO) bands at 1986 and 1862 (wide) cm −1 , similarly to what was observed for the analogous rhenium complex 2.  In the presence of CO2, the CV peak current significantly increased, suggesting reactivity with the reduced species (orange curve in Figure 12).The spectroelectrochemical reduction of 4 in a solution saturated with CO2 produced bands at 1684 and 1646 cm −1 (HCO3 − /CO3 2− ) simultaneously, with decreases in the CO2 band at 2342 cm −1 .The original spectrum of the complex remained almost unchanged (Figure 15).This result indicated that a different SEC mechanism of electrocatalytic carbon dioxide reduction was observed: it began at the first double-electron reduction potential of complex 4, and the catalytic cycle restored the original neutral complex 4. In the presence of CO2, the CV peak current significantly increased, suggesting reactivity with the reduced species (orange curve in Figure 12).The spectroelectrochemical reduction of 4 in a solution saturated with CO2 produced bands at 1684 and 1646 cm −1 (HCO3 − /CO3 2− ) simultaneously, with decreases in the CO2 band at 2342 cm −1 .The original spectrum of the complex remained almost unchanged (Figure 15).This result indicated that a different SEC mechanism of electrocatalytic carbon dioxide reduction was observed: it began at the first double-electron reduction potential of complex 4, and the catalytic cycle restored the original neutral complex 4. In the presence of CO 2 , the CV peak current significantly increased, suggesting reactivity with the reduced species (orange curve in Figure 12).The spectroelectrochemical reduction of 4 in a solution saturated with CO 2 produced bands at 1684 and 1646 cm −1 (HCO 3 − /CO 3 2− ) simultaneously, with decreases in the CO 2 band at 2342 cm −1 .The original spectrum of the complex remained almost unchanged (Figure 15).This result indicated that a different SEC mechanism of electrocatalytic carbon dioxide reduction was observed: it began at the first double-electron reduction potential of complex 4, and the catalytic cycle restored the original neutral complex 4. In order to prove the possible influence of a different solvent on the reduction mechanism, the SEC reductions of 1-4 were repeated using dimethylacetamide (DMA)/0.1 M Bu4NPF6 as a solvent.In the case of compounds 1-3, these experiments did not reveal any essential differences in the mechanism of the reduction and generated reduced species (Figures S4-S9).However, the reduction of complex 4 in DMA directly proceeded in one double-electron step to the anion ([Re(bpy-4,4′-NMe2)(CO)3] ‾ (Figure S10).The single-electron intermediate observed in the acetonitrile solution was not detected in the DMA solutions.The reason could have been a different substitution equilibrium chloride/solvent for the 1e ‾ reduced intermediate, and consequently, a different intrinsic reduction mechanism (EEC vs. ECE).The principal ν(CO) frequencies observed experimentally from SEC in solvents (acetonitrile and dimethylacetamide) are summarized in Table 2.

Discussion and Conclusions
IR spectroelectrochemistry has been used to highlight the catalytic behavior of four bpy complexes of Mn and Re.The CV of Mn complex 1 and that of Re complex 2 exhibited irreversible and reversible first chemical reductions, respectively.The corresponding SEC experiments clearly indicated that at the first reduction, 2 was already catalytically active in the CO2 conversion.Only at more negative potentials did 1 display an unprecedented In order to prove the possible influence of a different solvent on the reduction mechanism, the SEC reductions of 1-4 were repeated using dimethylacetamide (DMA)/0.1 M Bu 4 NPF 6 as a solvent.In the case of compounds 1-3, these experiments did not reveal any essential differences in the mechanism of the reduction and generated reduced species (Figures S4-S9).However, the reduction of complex 4 in DMA directly proceeded in one double-electron step to the anion ([Re(bpy-4,4 -NMe 2 )(CO) 3 ] − (Figure S10).The singleelectron intermediate observed in the acetonitrile solution was not detected in the DMA solutions.The reason could have been a different substitution equilibrium chloride/solvent for the 1e − reduced intermediate, and consequently, a different intrinsic reduction mechanism (EEC vs. ECE).The principal ν(CO) frequencies observed experimentally from SEC in both solvents (acetonitrile and dimethylacetamide) are summarized in Table 2.

Discussion and Conclusions
IR spectroelectrochemistry has been used to highlight the catalytic behavior of four bpy complexes of Mn and Re.The CV of Mn complex 1 and that of Re complex 2 exhibited irreversible and reversible first chemical reductions, respectively.The corresponding SEC experiments clearly indicated that at the first reduction, 2 was already catalytically active in the CO 2 conversion.Only at more negative potentials did 1 display an unprecedented very slow catalytic activity, which was greatly enhanced by the presence of 5% water as a proton donor.The higher lability of the M-X bond in 1 − with respect to 2 − has been interpreted using DFT calculations.Complexes 3 and 4 showed analogue catalytic activities, with the latter characterized by an overlapped 2e first reduction, partially resolved by SEC.In dimethylacetamide solutions, 4 was reduced by two electrons, and SEC could not discriminate the individual steps.These results highlight the suitability and effectiveness of SEC in investigating such catalytic processes, in a time scale slightly longer than that of CV.

Materials and Methods
Synthesis.The reagents were purchased from Sigma-Aldrich and used without further purification.The ligand 4-(4-aminophenyl)-2,2 -bipyridine was synthesized through a multistep reaction, following the slight modification of previously published procedures [30].First, 4.1 g of 4-nitrobenzaldehyde was added to 50 mL of EtOH, and the mixture was heated at 70 • C until all the solid was dissolved.Subsequently, 3.1 g of sodium pyruvate dissolved in 15 mL of H 2 O was slowly added, and the mixture was cooled on ice.Then, 25 mL of NaOH 0.5 M was slowly added, and the mixture was left on ice for a further 2.5 h.HCl 2 M was added dropwise to the mixture until neutrality was achieved, and the solution was filtered.The solid, 4-(4-nitrophenyl)-2-oxo-3-butenoic acid, was washed with ethanol and air-dried.After that, 3.0 g of the acid, 4.4 g of pyridinium iodide, and 8.3 g of NH 4 OAc were added to 90 mL of water.The suspension was heated at reflux for 6 h.The resulting ammonium salt of 4-(4-nitrophenyl)-6-carboxylate-2,2 -bipyridine was washed with water and acetone, air-dried, and finally heated under vacuum until gas evolution (CO 2 ) ceased and a black solid formed.The black solid was dissolved in EtOAc, activated charcoal was added, and the suspension was refluxed for 20 min.After this procedure, the solution was filtered over Celite, and the solvent was removed under vacuum.The dried yellowish solid, 4-(4-nitrophenyl)-2,2 -bipyridine, was dissolved in 30 mL of EtOH, mixed with 0.30 g of 10% Pd/C, 3.7 mL of hydrazine was added at 50%, and finally, flask was heated at reflux for two hours.After a second addition of hydrazine (2 mL) and a further 30 min of refluxing, the liquid mixture was filtered over Celite; the solid was dissolved in CH 2 Cl 2 and transferred into a separation funnel, and water was added.The organic solution was then dried through contact with anhydrous Na 2 SO 2 , and the solvent was removed under vacuum.The desired ligand, 4-(4-aminophenyl)-2,2 -bipyridine, was obtained with an overall yield of 40%. 1 H-NMR: ((CD 3 ) 2 CO) 8.71 (s, 1H), 8.70 (dm, 1H, J = 5.0 Hz), 8.60 (d, 1H, J = 7.9 Hz), 7.92 (td, 1H, J = 7.8 Hz, J = 1.8 Hz), 7.63 (d, 2H, J = 8.8 Hz), 7.60 (dd, 1H, J = 5.3 Hz, J = 2.0 Hz), 7.41 (ddd, 1H, J = 7.9 Hz, J = 5.0 Hz, J = 1.2 Hz), 6.83 (d, 2H, 8.8 Hz), 5.07 (s, 2H).
Mn complex 1 was obtained by mixing equimolar quantities of the ligand 4-(4aminophenyl)-2,2 -bipyridine and the carbonyl complex Mn(CO) 5 Br in diethyl ether and refluxing for 4 h.The resulting yellow solid was washed with clean diethyl ether and left to dry under an inert atmosphere.Re complex 2 was obtained by mixing an equimolar amount of 4-(4-aminophenyl)-2,2 -bipyridine and Re(CO) 5 Cl in toluene and refluxing for 4 h.The resulting solid was first washed with clean toluene and then with petroleum ether and left to dry under an inert atmosphere.Re and Mn carbonyl complexes 3 and 4 were synthesized through a similar procedure by reacting the corresponding substituted bipyridines with the Re(CO) 5 Cl or Mn(CO) 5 Br precursors, following a similar synthetic approach as previously reported [15,16].The ligand and the complexes were characterized using 1 H NMR spectroscopy.NMR spectra were recorded with a JEOL EX 400 spectrometer ( 1 H operating frequency 400 MHz) at 298 K; data were treated using Jeol Delta Software. 1 H chemical shifts were relative to TMS (δ = 0 ppm) and referenced against solvent residual peaks.
Cyclic Voltammetry.Cyclic voltammetry experiments were performed using a 1 mM solution of the complexes under study with a Biologic 300SP potentiostat.A singlecompartment cell was employed, equipped with a glassy carbon electrode (GCE, Ø = 1 mm) as the working electrode, a Pt counter electrode, and a Ag/AgCl (KCl 3 M) reference electrode.Acetonitrile (MeCN) and dimethylacetamide (DMA) solvents were freshly distilled over calcium hydride.Tetrabutylammonium hexafluorophosphate (Bu 4 NPF 6 , Sigma-Aldrich, Saint Louis, MI, USA, 98%) was recrystallized three times from ethanol solutions and used as the supporting electrolyte (0.1 M).Ar-and CO 2 -saturated conditions were achieved by purging gases for 5 min before the experiment.
Spectroelectrochemistry. Spectroelectrochemical experiments were performed using a Nicolet iS50 NIR-FTIR spectrometer equipped with an optically transparent thin-layer electrode (OTTLE) cell, employing Pt working and counter electrodes and a Ag wire as the pseudoreference electrode [31,32].The spectra were collected during a slow (5 mV/s)

Scheme 1 .
Scheme 1. Sketch of the complexes under study.

Scheme 1 .
Scheme 1. Sketch of the complexes under study.

1 Figure 1 .
Figure 1.IR spectroelectrochemical response on the first reduction of 1 in MeCN/0.1 M Bu4NPF6.Arrows up and down represent increases and decreases in the absorption bands, respectively.

Figure 1 . 1 Figure 2 .
Figure 1.IR spectroelectrochemical response on the first reduction of 1 in MeCN/0.1 M Bu 4 NPF 6 .Arrows up and down represent increases and decreases in the absorption bands, respectively.Molecules 2023, 28, x FOR PEER REVIEW 4 of 15

Figure 3 .
Figure 3. IR spectroelectrochemical response on the second reduction of 1 in MeCN/0.1 M Bu4NPF6/5% H2O under CO2 (*: distorted due to strong absorption of the MeCN/water mixture as a solvent).

Figure 3 .Figure 3 .
Figure 3. IR spectroelectrochemical response on the second reduction of 1 in MeCN/0.1 M Bu 4 NPF 6 /5% H 2 O under CO 2 (*: distorted due to strong absorption of the MeCN/water mixture as a solvent).

Figure 7 .
Figure 7. IR spectroelectrochemical response on the first reduction of 2 in MeCN/0.1 M Bu4NPF6 under CO2 (*: artefact due to strong absorption of solvent).

Figure 7 .
Figure 7. IR spectroelectrochemical response on the first reduction of 2 in MeCN/0.1 M Bu 4 NPF 6 under CO 2 (*: artefact due to strong absorption of solvent).

Figure 8 .
Figure 8. Relaxed geometry scan for 1 ‾ (black squares) and 2 ‾ (red circles) as a function of M-X distances in acetonitrile as the solvent.

Figure 8 .
Figure 8. Relaxed geometry scan for 1 − (black squares) and 2 − (red circles) as a function of M-X distances in acetonitrile as the solvent.

Figure
Figure Cyclic voltammetry of 3 in MeCN/0.1 M TBAPF 6 under Ar (violet line) and under CO 2 (black line).