Estimating the Acidity of Transition Metal Hydride and Dihydrogen Complexes by Adding Ligand Acidity Constants

• Published in: Journal of the American Chemical Society Vol. 136; no. 5; pp. 1948 - 1959
• Main Author: Morris, Robert H
• Format: Journal Article
• Language: English
• Published: United States American Chemical Society 05.02.2014
• Subjects: Acetonitriles - chemistry; Acids - chemistry; Coordination Complexes - chemistry; Ferrous Compounds - chemistry; Hydrogen - chemistry; Hydrogen Bonding; Ligands; Metallocenes; Models, Chemical; Solvents - chemistry; Transition Elements - chemistry
• ISSN: 0002-7863; 1520-5126
• DOI: 10.1021/ja410718r

A simple equation (pK a THF = ∑A L + C charge + C nd + C d6) can be used to obtain an estimate of the pK a of diamagnetic transition metal hydride and dihydrogen complexes in tetrahydrofuran, and, by use of conversion equations, in other solvents. It involves adding acidity constants A L for each of the ligands in the 5-, 6-, 7-, or 8-coordinate conjugate base complex of the hydride or dihydrogen complex along with a correction for the charge (C charge = −15, 0 or 30 for x = +1, 0 or −1 charge, respectively) and the periodic row of the transition metal (C nd = 0 for 3d or 4d metal, 2 for 5d metal) as well as a correction for d6 octahedral acids (C d6 = 6 for d6 metal ion in the acid, 0 for others) that are not dihydrogen complexes. Constants A L are provided for 13 commonly occurring ligand types; of these, nine neutral ligands are correlated with Lever’s electrochemical ligand parameters E L. This method gives good estimates of the over 170 literature pK a values that range from less than zero to 50 with a standard deviation of 3 pK a units for complexes of the metals chromium to nickel, molybdenum, ruthenium to palladium, and tungsten to platinum in the periodic table. This approach allows a quick assessment of the acidity of hydride complexes found in nature (e.g., hydrogenases) and in industry (e.g., catalysis and hydrogen energy applications). The pK a values calculated for acids that have bulky or large bite angle chelating ligands deviate the most from this correlation. The method also provides an estimate of the base strength of the deprotonated form of the complex.