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2. negative charge on the more electronegative atom makes it more stable! so if you have negative charge on O and C, the negative charge on O is more stable!
3. Carbon isn't very electronegative! so it doesn't stabilize a negative charge very well!
4. Since the negative charge on resonance structures, spread out on molecule, it makes the molecule more stable compare to molecule that looks a like but has no resonance structure! ex. propene is more acidic than propane!
5. EN is a more important FACTOR than resonance in acid strength. ex. one molecule has resonance but only CH and another molecule no resonance but OH! OH is more stable.
6. to see which acid is stronger compare there Conjugate bases.
7. The more resonance structures you can draw the more stable the conjugate base!
8. inductive effect (delocalize the negative charge): The closer or high in number the electronegative atom is to the negative charge the more stable conjugate base and the more acidic the acid is.
9. EN: - < =< ≡ sp3<sp2<sp (delocalize the negative charge!)(as S character increases, effective EN increases!)
10. The more substituded they are the more electron donator they are! and negative charges repel each other!
(as atoms become more EN, it falls in love with lone pair more, so wants to kick out the H!)
(- < =< ≡ Acidic!)
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