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17 notecards = 5 pages (4 cards per page)

Viewing:

Chapter 2 - Acids and Bases

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