Abstract:A series of homobimetallic manganese cofacial porphyrin-corrole dyads were synthesized and investigated as to their electrochemistry, spectroelectrochemistry, and ligand binding properties in nonaqueous media. Four dyads were investigated, each of which contained a Mn(III) corrole linked in a face-to-face arrangement with a Mn(III) porphyrin. The main difference between compounds in the series is the type of spacer, 9,9-dimethylxanthene, anthracene, dibenzofuran, or diphenylether, which determines the distance… Show more
“…The quasireversible (slow) electron transfer for the Mn III/II reduction process in CH 2 Cl 2 and C 2 H 4 Cl 2 (as indicated by a Δ E p ≫ 60 mV and the lack of a well-defined reoxidation) and the faster electron transfer for the first oxidation under the same solution conditions (Δ E p = 80 to 100 mV) is consistent with not only the different sites of electron transfer (i.e., a ligand-centered oxidation and a metal-centered reduction) as assigned above but also the possible presence of a coupled chemical reaction on reduction. The larger Δ E p value associated with a slow metal-centered reduction is also consistent for what has been reported for the Mn III/II process of many porphyrins − and also other Mn III macrocycles. − …”
Section: Resultssupporting
confidence: 89%
“…A summary of the measured oxidation and reduction potentials for (Ph)DPPMn in these solvents containing 0.1 M TBAPF6 is given in Table 2 and examples of cyclic voltammograms are shown in Figure 5, where three types of current-voltage curves are seen for reduction. The first is in CH2Cl2 and C2H4Cl2 where the reduction peak is broad and no clear reoxidation peak is observed, perhaps due to the formation of dimers in solution as seen in the solid state 10 and also in the gas phase as seen by the ESI-MS results in Figures S4 and S5 Mn III/II process of many porphyrins [38][39][40] and also other Mn III macrocycles. [41][42][43] It is also worth noting that, with the exception of CH2Cl2 and C2H4Cl2, the cathodic peak currents for the first reduction (ipc) are essentially the same as the anodic peak currents for the first oxidation (ipa), consistent with the same number of electrons transferred in each step.…”
Section: Resultsmentioning
confidence: 99%
“…It should also be noted that a dimerization detectable during reduction but not oxidation can be rationalized by the different sites of electron transfer; i.e., an electron is added to the manganese center during reduction, while electron abstraction takes place on the (Ar)DPP ring during oxidation. It should also be noted that ring-centered redox processes are typically rapid (reversible) electron transfers, while Mn III -centered reductions would be slower as is often observed for Mn III reductions at the metal center. − ,− …”
Section: Resultsmentioning
confidence: 99%
“…It should also be noted that ring centered redox processes are typically rapid (reversible) electron 21 transfers while Mn III -centered reductions would be slower as is often observed for Mn III reductions at the metal center. [16][17][18][38][39][40][41][42][43] Figure 12. Cyclic voltammograms of (a) (Ph)DPPMn and (b) (Mes)DPPMn at 10 -3 M in CH2Cl2 containing 0.1 M TBAPF6 before and after the addition of 2.0 eq TFA.…”
Section: Scheme 1 Possible Products Of Dimer Dissociationmentioning
A series of "N2O2-type" manganese dipyrrin-bisphenols (DPP), formulated as (Ar)DPPMn, where Ar = pentafluorophenyl (F5Ph), phenyl (Ph) or mesityl (Mes), were electrochemically and spectroscopically characterized in nonaqueous media with and without added anions in the form of tetrabutylammonium salts (TBAX where X = ClO4 -, PF6 -, BF4 -, F -, Cl -, OHor CN -). Two major one-electron reductions are observed under most solution condition, the first of which is assigned as a Mn III/II process and the second as electron addition to the π-ring system as confirmed by spectroelectrochemistry. Each Mn III complex also exhibits one or two one-electron oxidations, the exact number depending upon the positive potential limit of the electrochemical solvent. The two oxidations are separated by 580-590 mV in CH3CN, 0.1 M TBAPF6 and are assigned as π-ring centered electron transfers to stepwise form a (Ar)DPPMn III π-cation radical and dication under these solution conditions. Comparisons are made between redox properties of (Ar)DPPMn and manganese(III) porphyrins, corroles and corrolazines each of which contains an innocent trianionic complexing ligand. The redox behavior and spectroscopic properties of [(Ar)DPPMn] n where n = 0, -1 or +1 are also compared to that of other structurally related [(Ar)DPPM] n complexes under similar solution conditions where M = Co II , Cu II , B III or Au III .
“…The quasireversible (slow) electron transfer for the Mn III/II reduction process in CH 2 Cl 2 and C 2 H 4 Cl 2 (as indicated by a Δ E p ≫ 60 mV and the lack of a well-defined reoxidation) and the faster electron transfer for the first oxidation under the same solution conditions (Δ E p = 80 to 100 mV) is consistent with not only the different sites of electron transfer (i.e., a ligand-centered oxidation and a metal-centered reduction) as assigned above but also the possible presence of a coupled chemical reaction on reduction. The larger Δ E p value associated with a slow metal-centered reduction is also consistent for what has been reported for the Mn III/II process of many porphyrins − and also other Mn III macrocycles. − …”
Section: Resultssupporting
confidence: 89%
“…A summary of the measured oxidation and reduction potentials for (Ph)DPPMn in these solvents containing 0.1 M TBAPF6 is given in Table 2 and examples of cyclic voltammograms are shown in Figure 5, where three types of current-voltage curves are seen for reduction. The first is in CH2Cl2 and C2H4Cl2 where the reduction peak is broad and no clear reoxidation peak is observed, perhaps due to the formation of dimers in solution as seen in the solid state 10 and also in the gas phase as seen by the ESI-MS results in Figures S4 and S5 Mn III/II process of many porphyrins [38][39][40] and also other Mn III macrocycles. [41][42][43] It is also worth noting that, with the exception of CH2Cl2 and C2H4Cl2, the cathodic peak currents for the first reduction (ipc) are essentially the same as the anodic peak currents for the first oxidation (ipa), consistent with the same number of electrons transferred in each step.…”
Section: Resultsmentioning
confidence: 99%
“…It should also be noted that a dimerization detectable during reduction but not oxidation can be rationalized by the different sites of electron transfer; i.e., an electron is added to the manganese center during reduction, while electron abstraction takes place on the (Ar)DPP ring during oxidation. It should also be noted that ring-centered redox processes are typically rapid (reversible) electron transfers, while Mn III -centered reductions would be slower as is often observed for Mn III reductions at the metal center. − ,− …”
Section: Resultsmentioning
confidence: 99%
“…It should also be noted that ring centered redox processes are typically rapid (reversible) electron 21 transfers while Mn III -centered reductions would be slower as is often observed for Mn III reductions at the metal center. [16][17][18][38][39][40][41][42][43] Figure 12. Cyclic voltammograms of (a) (Ph)DPPMn and (b) (Mes)DPPMn at 10 -3 M in CH2Cl2 containing 0.1 M TBAPF6 before and after the addition of 2.0 eq TFA.…”
Section: Scheme 1 Possible Products Of Dimer Dissociationmentioning
A series of "N2O2-type" manganese dipyrrin-bisphenols (DPP), formulated as (Ar)DPPMn, where Ar = pentafluorophenyl (F5Ph), phenyl (Ph) or mesityl (Mes), were electrochemically and spectroscopically characterized in nonaqueous media with and without added anions in the form of tetrabutylammonium salts (TBAX where X = ClO4 -, PF6 -, BF4 -, F -, Cl -, OHor CN -). Two major one-electron reductions are observed under most solution condition, the first of which is assigned as a Mn III/II process and the second as electron addition to the π-ring system as confirmed by spectroelectrochemistry. Each Mn III complex also exhibits one or two one-electron oxidations, the exact number depending upon the positive potential limit of the electrochemical solvent. The two oxidations are separated by 580-590 mV in CH3CN, 0.1 M TBAPF6 and are assigned as π-ring centered electron transfers to stepwise form a (Ar)DPPMn III π-cation radical and dication under these solution conditions. Comparisons are made between redox properties of (Ar)DPPMn and manganese(III) porphyrins, corroles and corrolazines each of which contains an innocent trianionic complexing ligand. The redox behavior and spectroscopic properties of [(Ar)DPPMn] n where n = 0, -1 or +1 are also compared to that of other structurally related [(Ar)DPPM] n complexes under similar solution conditions where M = Co II , Cu II , B III or Au III .
“…Dyads with one cobalt(III) corrole and a noncobalt containing porphyrin showed a poor selectivity towards water formation . Similarly, dimanganese porphyrin–corrole dyads and heterobimetallic (M)‐porphyrin–Co‐corrole dyads (with M=Fe, Mn; Figure ) showed only insufficient selectivities.…”
In this Concept article we present the syntheses and application of homo and heterodinuclear "Pacman" compounds. This architecture implies that two metal coordination fragments are brought in close vicinity to each other via a covalent linkage to either support energy transfer between the two units or cooperative transformation of a substrate. Nature has shown that the combination of metal fragments, in particular two different metals, can dramatically improve the efficiency of small molecule activation. We exemplify this strategy for the activation of water, dioxygen and carbon dioxide. Furthermore, we present artificial systems in which a positive effect on the catalytic performance because of the combination of two (different) metal centers could be observed. Thus, Pacman-type compounds are very well suited as structural and functional models for their biological counterparts.
Four metalloporphyrin dimers linked by bridging amide‐bonded xanthene moieties and that contain either MnIII, CoII, NiII, or CuII metal centers were synthesized. Various spectroscopic, electrochemical, and spectroelectrochemical methods were used to study trends in their properties. Their electronic structure and optical properties were analyzed through a comparison of the electronic absorption and magnetic circular dichroism (MCD) spectral data with the results of time‐dependent (TD)‐DFT calculations.
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