Bronsted Acid and Bases, pKa, C-A-R-I-O, Lewis Acid and Bases

Question 1

Arrhenius Acid

Answer 1

Substance when add an water, increase the concentration of H3O+ in solution

Question 2

Arrhenius Base

Answer 2

Substance when add to water, increase the concentration of OH- ion in solution

Question 3

Bronsed Lowry Acid

Answer 3

Anything that releases proton

Question 4

Bronsted Lowry Base

Answer 4

Anything that accepts proton

Question 5

Conjugate Acid

Answer 5

Product that result when a base accept a proton

Question 6

Conjugate Base

Answer 6

Product that results when a base gains a proton

Question 7

What does equilibrium always favor?

Answer 7

Equilibrium always favor formation of weaker acid and base

Question 8

Why does equilibrium favor the weak acid and weak base?

Answer 8

The weaker acid and the weaker base are the most stable species due to their lower potential energies.

Question 9

What determines the strength of a bronsted acid?

Answer 9

how much they can dissociate in solution to release H+ and their conjugate base

Question 10

How do you tell the strength of an acid based on their pKa?

Answer 10

Lower the pKa, stronger the acid

Question 11

What type of strength relationship is between acid/base and conjugate acid/conjugate base?

Answer 11

Inverse relationship.
The stronger the acid, the weaker its conjugate base.
The stronger the base, the weaker its conjugate acid

Question 12

Why does acid/base have in inverse relationship of strength than its conjugate pairs?

Answer 12

If an acid is strong, it will readily donate its hydrogen. Thus, its conjugate acid, the substance that results from the loss of proton, did not hold the proton very well, thus weak.

Question 13

How does charge affect acid strength?

Answer 13

The more positively charged an atom is, the stronger its acidity is. There is more hydronium ion, making the compound more acidic.

Question 14

How does electronegative affect acid strength?

Answer 14

Atom Effect - Electronegativity: The proton that is attached to a more electronegative atom is more negative

Question 15

How does atomic size affect acid strength?

Answer 15

The proton that is attached to a bigger atom is more acidic.

Question 16

How does resonance effect affect acid strength?

Answer 16

The acid with a conjugate base that is stabilized by resonance structure will be more acidic

Question 17

How does inductive effect affect acid strength?

Answer 17

The proton that is near an electron withdrawing group (EWG) is more acidic.
Number and Distance of EWG: As the number of EWG increase, the more acidic the proton
As the distance of the EWG from the acid proton increase, the less acidic

Question 18

How does orbital effect affect acid strength?

Answer 18

As the s character of the hybridized carbon increases, the more acidic the attached proton is

Question 19

What is a lewis acid?

Answer 19

Substance that accept electron pairs

Question 20

Lewis Bases

Answer 20

Substances that donate electron pairs

Question 21

What is an electrophile?

Answer 21

Molecule that forms a bond by accepting a lone pair from another molecule (nucleophile)

Usually positively charge so it’s “electron-loving”

Question 22

What is a nucleophile?

Answer 22

An atom or molecule that form a bond by donating a pair of electrons.

A nucleophile wants to seek a positively charged nucleus to form a bond with its negatively charged polar. Therefore, nucleophile always initiate bonding with electrophile. Usually neutral or negatively charged.