1. Acids and Bases Arrhenius Bronsted-Lowry Lewis

2. Definitions of Acids/Bases

3. Measuring Acid Strength Ka

4. Acid Strength defined by pK a

5. Dissociation in H 2 O Arrhenius Acid forms H 3 O + Bronsted-Lowry Acid donates a H +

6. Resonance Stabilization

7. Stronger Acid Controls Equilibrium

8. Reaction Described with Arrows HCl donates a proton H 2 O accepts a proton

10. Equilibrium Reactions

11. Draw the Conjugate Acid and Base

12. Propanol is a Base

13. Draw the Conjugate Acid and Base

14. Propanol is an Acid

15. Some Acid-Base Reactions

17. The Effect of Resonance on pKa

18. Identify the Acid and Base

19. Equilibrium Favors Reactants

20. Carboxylic Acids can be Separated from non-acidic Compounds

21. Lewis Acids and Bases

22. Formation of a new bond

23. Lewis Base = Nucleophile Lewis Acid = Electrophile

24. Draw the Acid-Base Complexes

27. Draw Arrows

29. Identify the Conjugate Base (i.e. Which H is most acidic?)

30. By deprotonating one of the H b protons, one can distribute the charge onto three atoms and give a major resonance structure with the charge on the Oxygen (the third structure).