AP®︎ Chemistry: Topic 8.6 Flashcards

Stronger acids have weaker, more stable conjugate bases; stronger bases have weaker conjugate acids.

Hydrogens bonded to electronegative atoms or in acidic groups are most likely to transfer as H+.

Weaker H-X bonds give stronger acids; for hydrogen halides, acidity increases down the group.

More electronegative atoms stabilize negative charge in the conjugate base, increasing acid strength.

Electron-withdrawing atoms pull electron density through sigma bonds, stabilizing nearby negative charge.

Delocalizing negative charge over multiple atoms stabilizes the conjugate base and strengthens the acid.

Stronger oxyacids have more electron-withdrawing central atoms or higher oxidation states, weakening the O-H bond.

HCl, HBr, HI, HNO3, HClO4, and the first proton of H2SO4 dissociate essentially completely in water.

Organic acids containing a COOH group that are weak acids because their conjugate bases are resonance-stabilized.

COOH compounds are more acidic than ROH compounds because carboxylate ions are resonance-stabilized but alkoxides are not.

Alkali metal hydroxides and Ca(OH)2, Sr(OH)2, Ba(OH)2 dissociate completely to produce OH-.

Resonance-stabilized conjugate bases of carboxylic acids that are weak bases and can accept H+.

Alkyl groups increase amine basicity by donating electron density to nitrogen's lone pair.

Ammonia, amines, and carboxylate ions are weak bases that only partially react with water.