MIDTERM 02 - Structural Effects on Acidity and Basicity
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Substance that increases the concentration of H+ ions
Arrhenius acid
Substance that increases the concentration of OH- ions
Arrhenius base
Is a substance that donates a proton to another substance
Bronsted-Lowry acid
Is a substance that accepts a proton
Bronsted-Lowry base
Formed by removing a proton from the acid
Conjugate base
Formed by adding a proton to the base
Conjugate acid
A substance capable of acting as either an acid or a base
Amphiprotic
Is a measure of the tendency of a compound to lose a proton
Acidity
Is a measure of a compound’s affinity for a proton
Basicity
Ka; the higher the Ka, the stronger the acid
Acid-dissociation constant
Kb; the higher the Kb, the stronger the base
Base-dissociation constant
Is a substance that accepts an electron pair
Lewis acid
Is a substance that donates an electron pair
Lewis base
Other name for Lewis acids
Electrophiles
Other name for Lewis bases
Nucleophiles
Are organic compounds that contain a hydrogen atom bonded to an electronegative oxygen
Organic acids
Shift in electron density through charge polarization transmitted through sigma bonds
Inductive effect
Stabilizes conjugate base
Electron-withdrawing groups
Destabilizes conjugate base
Electron-donating groups
Results from the presence of bulky groups and results to congestion and twisting of bonds
Steric effect