Acidities and basicities of carboxylic acids. Correlations between core-ionization energies, proton affinities, and gas-phase acidities

1978 ◽  
Vol 100 (17) ◽  
pp. 5459-5466 ◽  
Author(s):  
S. R. Smith ◽  
T. D. Thomas
Keyword(s):  
Gas Phase ◽  
Carboxylic Acids ◽  
Proton Affinities ◽  
Ionization Energies

scholarly journals Crystal Phase Effects on the Gas‐Phase Ketonization of Small Carboxylic Acids over TiO 2 Catalysts

ChemSusChem ◽  
2021 ◽  
Author(s):  
Egor V. Fufachev ◽  
Bert M. Weckhuysen ◽  
Pieter C. A. Bruijnincx
Keyword(s):  
Gas Phase ◽  
Carboxylic Acids ◽  
Crystal Phase

S-Acylation of aliphatic and aromatic thiols with carboxylic acids and their esters over solid acid catalysts in the gas phase at temperatures above 200°C

2013 ◽  
Vol 464-465 ◽  
pp. 332-338 ◽  
Author(s):  
Sayoko Nagashima ◽  
Hitomi Yamazaki ◽  
Kentaro Kudo ◽  
Satoshi Kamiguchi ◽  
Teiji Chihara
Keyword(s):  
Gas Phase ◽  
Carboxylic Acids ◽  
Solid Acid ◽  
Solid Acid Catalysts ◽  
Acid Catalysts ◽  
Aromatic Thiols

Redshift or Adduct Stabilization—A Computational Study of Hydrogen Bonding in Adducts of Protonated Carboxylic Acids

2009 ◽  
Vol 15 (2) ◽  
pp. 239-248 ◽  
Author(s):  
Solveig Gaarn Olesen ◽  
Steen Hammerum
Keyword(s):  
Hydrogen Bond ◽  
Hydrogen Bonds ◽  
Bond Strength ◽  
Bond Length ◽  
Carboxylic Acids ◽  
Computational Study ◽  
Proton Affinities ◽  
Oh Groups ◽  
Hydrogen Bond Strength ◽  
Length Changes

It is generally expected that the hydrogen bond strength in a D–H•••A adduct is predicted by the difference between the proton affinities (Δ PA) of D and A, measured by the adduct stabilization, and demonstrated by the infrared (IR) redshift of the D–H bond stretching vibrational frequency. These criteria do not always yield consistent predictions, as illustrated by the hydrogen bonds formed by the E and Z OH groups of protonated carboxylic acids. The Δ PA and the stabilization of a series of hydrogen bonded adducts indicate that the E OH group forms the stronger hydrogen bonds, whereas the bond length changes and the redshift favor the Z OH group, matching the results of NBO and AIM calculations. This reflects that the thermochemistry of adduct formation is not a good measure of the hydrogen bond strength in charged adducts, and that the ionic interactions in the E and Z adducts of protonated carboxylic acids are different. The OH bond length and IR redshift afford the better measure of hydrogen bond strength.

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