Module 2: Acids and Bases

Question 1

four main factors, in the following priority order, that affect the stability of the conjugate base

Answer 1

1. Atom
2. Resonance
3. Induction
4. Orbital

Question 2

the acidity of H-A increases as the percent s-character of A increases

Answer 2

hybridization effects

Question 3

measure of a compound’s affinity for a proton

Answer 3

basicity

Question 4

Any species that is electron deficient and capable of accepting an electron also a?

Answer 4

lewis acid

Question 5

The acidity relies on the stability of the?

Answer 5

conjugate base

Question 6

Down the periodic table, the ___________________ determines the acidity

Answer 6

atomic size

Question 7

acids that the net charge may be zero (+), or (-)

Answer 7

bronsted-lowry acids

Question 8

The tendency of an acid to donate a proton

Answer 8

acid strength

Question 9

these are more electronegative than p orbitals

Answer 9

s orbitals

Question 10

Electron donor

Answer 10

lewis base

Question 11

these contains a proton

Answer 11

all bronsted-lowry acids

Question 12

this always favors formation of the weaker acid and base

Answer 12

equilibrium

Question 13

the acidity of H-A inccreases both left-to-right across a row and down a column of the periodic table

Answer 13

element effects

Question 14

this shows how greatly the acidity varied for different functional groups.

Answer 14

pKa table

Question 15

this is the characteristic of a particular compound, which indicates the tendency of the compound to give up its proton.

Answer 15

pKa

Question 16

Electron acceptor

Answer 16

lewis acid

Question 17

the lewis acid is also called a ________________ or electron-rich

Answer 17

nucleophile

Question 18

Proton acceptor

Answer 18

bronsted-lowry base

Question 19

Increase the concentration of H+ions when dissolved in water

Answer 19

arrhenius acid

Question 20

the acidity of H-A increases with the presence of electron-withdrawing groups in A

Answer 20

inductive effects

Question 21

Increase the concentration of OH-ions when dissolved in water

Answer 21

arrhenius base

Question 22

this is used to describe the acidity (concentration of positively charged hydrogen ions) of a solution

Answer 22

pH scale

Question 23

The more readily the compound donates a proton, the?

Answer 23

stronger the acid

Question 24

these contain a lone pair of electrons or a pi bond

Answer 24

all bronsted-lowry base

Question 25

bases that the net charge may be zero or (-)

Answer 25

bronsted-lowry bases

Question 26

The use of curved arrows to show simple proton-transfer reactions.

Answer 26

The Lewis Definition

Question 27

Proton donor

Answer 27

bronsted-lowry acid

Question 28

the acidity of H-A increases when the conjugate base A is resonance stabilized

Answer 28

resonance effects

Question 29

An acid can be deprotonated by the conjugate base of any acid having a?

Answer 29

higher pKa

Question 30

from left to right, acidity increases as the electronegativity _________________

Answer 30

increases

Question 31

The ______________ the electronegativity, the stronger the inductive effect

Answer 31

stronger

Question 32

Structural effects on acidity and basicity of organic molecules

Answer 32

The Brønsted–Lowry Definition

Question 33

a lewis acid is also called an ________ or electron deficient

Answer 33

electrophile

Question 34

the closer the electronegative atom to the hydrogen, the stronger the?

Answer 34

acid

Question 35

this is due to differences in electronegativity (EN), the intrinsic ability of an atom to attract the shared electrons in a covalent bond

Answer 35

bond polarity

Question 36

a weaker conjugate base means a more?

Answer 36

stable conjugate base

Question 37

this is broader and more encompassing than the Bronsted-Lowry definition because it is not limited to substances that donate or accept protons only.

Answer 37

lewis definition of acids and bases

Question 38

these are structurally the same as Brønsted–Lowry bases. Both have an available electron pair—a lone pair or an electron pair in a π bond.

Answer 38

lewis bases

Question 39

measure of the tendency of a compound to give up a proton

Answer 39

acidity

Question 40

the stronger the acid, the weaker its?

Answer 40

conjugate base