[Co(dmgBF 2) 2(H 2O) 2] 1 (where dmgBF 2 = difluoroboryldimethylglyoximato) was used to synthesize [Co(dmgBF 2) 2(H 2O)(py)]0.5(CH 3) 2CO 2 (where py = pyridine) in acetone. The formulation of complex 2 was confirmed by elemental analysis, high resolution MS, and various spectroscopic techniques. The complex [Co(dmgBF 2) 2(solv)(py)] (where solv = solvent) was readily formed in situ upon the addition of pyridine to complex 1. A spectrophotometric titration involving complex 1 and pyridine proved the formation of such a species, with formation constants, log K = 5.5, 5.1, 5.0, 4.4, and 3.1 in 2-butanone, dichloromethane, acetone, 1,2-difluorobenzene/acetone (4: 1, v/v), and acetonitrile, respectively, at 20 °C. In strongly coordinating solvents, such as acetonitrile, the lower magnitude of K along with cyclic voltammetry, NMR, and UV-visible spectroscopic measurements indicated extensive dissociation of the axial pyridine. In strongly coordinating solvents, [Co(dmgBF 2) 2(solv)(py)] can only be distinguished from [Co(dmgBF 2) 2(solv) 2] upon addition of an excess of pyridine, however, in weakly coordinating solvents the distinctions were apparent without the need for excess pyridine.

The coordination of pyridine to the cobalt(II) centre diminished the peak current at the E pc value of the Co I/0 redox couple, which was indicative of the relative position of the reaction equilibrium. Herein we report the first experimental and theoretical 59Co NMR spectroscopic data for the formation of Co(I) species of reduced cobaloximes in the presence and absence of py (and its derivatives) in CD 3CN. From spectroelectrochemical studies, it was found that pyridine coordination to a cobalt(I) metal centre is more favourable than coordination to a cobalt(II) metal centre as evident by the larger formation constant, log K = 4.6 versus 3.1, respectively, in acetonitrile at 20 °C. Eduard kraft torrent download. The electrosynthesis of hydrogen by complexes 1 and 2 in various solvents demonstrated the dramatic effects of the axial ligand and the solvent on the turnover number of the respective catalyst. Introduction The production and use of clean, renewable and high-energy-density sources are growing in demand to circumvent the use of fossil fuels, thus reducing the effects of carbon dioxide emissions and global warming. Hydrogen has been suggested as the leading candidate – and its production through the reduction of water appears to be a convenient solution for long-term storage and accessibility.

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Traditionally, noble metals of the platinum group metal series have been employed as catalytic centres in hydrogen production; – however, the high cost associated with these metals has led to searches for viable catalysts based on cheap and abundant first-row transition metals, such as nickel and cobalt. – Cobaloximes essentially mimic the active centre of hydrogenases, and are a promising class of compounds for the production of hydrogen in acidic media. – In addition to cobaloximes, – numerous cobalt-containing complexes exist for the catalytic reduction of protons to produce hydrogen. These include cobalt porphyrin derivatives, macrocyclic complexes of [14]diene-N 4 and [14]tetraene-N 4 (tetraazamacrocycles), imine/oximes, polypyridyl compounds, – bis(iminopyridine), phosphine coordinated complexes, and dithiolene (dithiolate)-containing complexes (), however, cobaloximes still continue to generate a lot of interest due to their high activity towards electrocatalytic proton reduction.,,–. Examples of some cobalt-containing complexes employed in the electrocatalytic reduction of protons. The most plausible route in the catalytic evolution of hydrogen involves the formation of a Co(I) species from either a Co(III) or Co(II) precursor., Recent studies have been geared towards studying the Co(I) intermediate through NMR spectroscopy, X-ray absorption spectroscopy (XAS), and high frequency electron paramagnetic resonance (HFEPR) techniques.