Anhydrides experience even weaker resonance stabilization, since the resonance is split between two carbonyl groups, and are more reactive than esters and amides.
12.
This occurs typically in compounds such as resonance stabilization are usually very strong, or superbases, which cannot exist in a water solution due to the acidity of water.
13.
When adjacent to the phenyl ring the amine group,-NH 2-, is in resonance stabilization and therefore becomes more acidic and a result less reactive as a base.
14.
The resonance stabilization of thiophene is 29 kcal / mol ( 121 kJ / mol ) compared to 20 kcal / mol ( 84 kJ / mol ) for the oxygen analogue furan.
15.
Where Q is the measure of reactivity of monomer via resonance stabilization, and e is the measure of polarity of monomer ( molecule or radical ) via the effect of functional groups on vinyl groups.
16.
This intermediate tends to revert to the amide form, expelling the attacking group, since the amide form is usually favored by free energy, ( presumably due to the strong resonance stabilization of the peptide group ).
17.
The recombination of the electron and hole, i . e . the decay of the exciton, is limited by resonance stabilization due to the overlap of the electron and hole wave functions, resulting in an extended lifetime for the exciton.
18.
In another variation the reagent is the imidazole 1, 1'- thiocarbonyldiimidazole ( TCDI ), for example in the total synthesis of pallescensin B . TCDI is especially good to primary alcohols because there is no resonance stabilization of the xanthate because the nitrogen lonepair is involved in the aromatic sextet.
19.
Thus, while most organic acids are deprotonated by the ionization of a polar hydrogen oxygen bond, usually accompanied by some form of resonance stabilization ( resulting in a carboxylate ion ), uric acid is deprotonated at a nitrogen atom and uses a tautomeric hydroxy group as an electron-withdrawing group to increase the p " K " 1 value.
20.
Secondly, since many types of compounds can function as an acid and a base, then what is the point of their K a when you might not even be using water as the solvent ? ( Granted, I am in chapter 1 of my organic chemistry book and it only devotes only 7 pages to the following topics : " Arrhenius Acids / Bases, Bronsted-Lowry Acids / Bases & acid Strength, acid-dissociation constant, base strength, structural effects on Acidity including electronegativity, size, & resonance stabilization, Lewis Acids / Bases " and I finally ditched my chemistry book and taught myself from Wikipedia and am getting every question right on practice tests ! ) If I'm wrong, then please correct me because I absolutely loved the explanation of acids / bases under this Solvent-system definition and that's why I'm so curious to resolve my anxiety.
