front 1 ![]() Label the Bronsted Lowry acid, base, conjugate acid and conjugate base. | back 1 ![]() |
front 2 ![]() Label the Bronsted Lowry acid, base, conjugate acid and conjugate base. | back 2 ![]() |
front 3 ![]() Use curved arrow notation to show the movement of electrons in the Lewis Acid-Base Reaction | back 3 ![]() |
front 4 ![]() Use curved arrow notation to show the movement of electrons in the Bronsted Lowry Acid-Base Reaction | back 4 ![]() |
front 5 ![]() Label the Bronsted Lowry acid, base, conjugate acid and conjugate base. Then determine in which direction equilibrium is favored. | back 5 ![]() |
front 6 ![]() Determine in which direction equilibrium is favored. | back 6 ![]() |
front 7 ![]() Determine in which direction equilibrium is favored. | back 7 ![]() |
front 8 ![]() Determine in which direction equilibrium is favored. | back 8 ![]() |
front 9 ![]() Rank the following in order of increasing acidity | back 9 ![]() *Elemental Effect Electronegativity when comparing CH4, NH3, and CH3OH Polarizability when comparing CH3OH and HCl |
front 10 ![]() Rank the following in order of increasing basicity | back 10 ![]() Negatively charged ions are stronger bases compared to their neutral counterparts When comparing H2O and NH3, H2O is a stronger acid, because the conjugate base (OH-) is more stable than (NH2-) because oxygen is more electronegative than nitrogen. Since OH- is the more stable conjugate base, it is a stronger acid, and thereby the weakest base. |
front 11 ![]() Rank these compounds in order of increasing acidity | back 11 ![]() |
front 12 ![]() Rank these compounds in order of increasing acidity | back 12 ![]() Elemental Effect (CH3 vs NH2) Elemental Effect (NH2 vs OH) Resonance Effect (OH vs. CO2H) |
front 13 ![]() Rank these compounds in order of increasing acidity | back 13 ![]() Resonance Effect (OH vs CO2H) Elemental Effect (CO2H vs HF) Positively charged ions are stronger acids than neutral counterparts |
front 14 ![]() Circle the most acidic proton on each compound | back 14 ![]() A. Inductive Effect B. Elemental Effect (Eliminates C-H and N-H), (Sulfur is more polarizable than Oxygen) C. Elemental Effect (Eliminates C-H), Resonance Effect (Eliminates O-H group) |
front 15 ![]() Circle the most acidic proton on each compound | back 15 ![]() A. Elemental Effect (Fluorine electronegativity) B. Hybridization Effect (increase percent s character, closer to the nucleus, more stable) |
front 16 ![]() Draw the products for the Lewis Acid and Base Reaction. Identify the electrophile and nucleophile | back 16 ![]() |
front 17 ![]() Draw the products for the Lewis Acid and Base Reaction. Identify the electrophile and nucleophile | back 17 ![]() |