Chapter 3

Question 1

what is a Bronsted-Lowry Acid?

Answer 1

a Bronsted-Lowry acid is a proton donor

Question 2

what is a Bronsted-Lowry Base?

Answer 2

a Bronsted-Lowry Base is a proton acceptor

Question 3

which one is the acid, the base, the conjugate acid, and the conjugate base?

Answer 3

Question 4

what is a reaction mechanism?

Answer 4

a reaction mechanism is how the reaction occurs in terms of the (real!) motion of electrons

Question 5

What is Keq? (also formula?)

Answer 5

Keq is the equilibrium constant of a reaction. It describes the moment when the rate of the forward reaction equals the rate of the reverse reaction, in terms of the concentrations of products and reactants.

Keq = [products]

​ [reactants]

Question 6

what is Ka? (also formula)

Answer 6

Ka is another way of expressing Keq

Ka = [products]without water

[reactants]

Question 7

what’s the equation for pKa?

Answer 7

pKa = -log(Ka)

Question 8

are lower or higher pKa values more acidic?

Answer 8

lower

Question 9

a stronger acid generates a ___________ conjugate base

Answer 9

weaker

Question 10

a weaker acid generates a ____________ conjugate base

Answer 10

stronger

Question 11

a stronger base generates a _________ conjugate acid

Answer 11

weaker

Question 12

a weaker base generates a ___________ conjugate acid

Answer 12

stronger

Question 13

the equilibrium of a reaction will always favor the __________ acid

Answer 13

weaker

Question 14

the equilibrium of a reaction will always favor the ___________ base

Answer 14

stronger

Question 15

what does this symbol mean?

Answer 15

the position of equilibrium favors the right side

Question 16

a weaker acid has a _________ pKa value

Answer 16

higher

Question 17

a stronger acid has a __________ pKa value

Answer 17

lower

Question 18

reaction equilibrium will favor the side where the pKa (of the acid) is __________

Answer 18

higher

Question 19

why are some reaction equilibriums written —> or <— ?

Answer 19

because they essentially proceed in only one direction

(because of a vast different in pKa of the acids)

Question 20

the ___________ base indicates the side the reaction will favor

Answer 20

more stable

Question 21

a more stable conjugate base indicates a _______ acid, which will drive the reaction _________

Answer 21

stronger

towards the conjugate base

Question 22

conjugate bases frequently bear a __________ charge (proton ________)

Answer 22

negative

donor

Question 23

conjugate acids frequently bear a __________ charge (proton ________)

Answer 23

positive

acceptor

Question 24

How do you determine which base is more stable?

Answer 24

ARIO-S

A: ATOM: more massive atoms bearing a negative charge are more stable

more electronegative atoms bearing a negative charge are more stable

(mass > electronegativity)

R: RESONANCE: resonance makes more stable

I: INDUCTION: induction from nearby electronegative atoms makes a base more stable

O: ORBITAL: smaller orbitals are more stable when bearing an electron

S: STERICALLY HINDERED: the less bulky (# of different connections) base is more stable

Question 25

a Lewis acid is an \_\_\_\_\_\_\_\_\_\_\_\_

Answer 25

electron acceptor

Question 26

a Lewis Base is an \_\_\_\_\_\_\_\_\_\_\_

Answer 26

electron donor

Question 27

when do we use Lewis acids/bases?

Answer 27

to discuss acid-base reactions that _do not involve hydrogen_ as an active part of the reaction

Question 28

which base is more stable?: explain A

Answer 28

a more massive atom can distribute the - charge over the whole atom, making it more stable mass \> (dominant effect) electronegativity a more electronegative atom is more stable when bearing a - charge (electron)

Question 29

which base is more stable?: explain R

Answer 29

resonance structures are more stable because the charges are delocalized (spread out over entire molecule)

Question 30

which base is more stable?: explain I

Answer 30

induction from nearby (highly electronegative) atoms helps to create a more stable base electronegative atoms induce a stronger partial charge, helping to make the area near the electron more positive, so that it can hold the electron more strongly

Question 31

which base is more stable?: explain O

Answer 31

smaller orbitals are more stable when bearing an electron because the electron's orbital is closer to the nucleus

Question 32

which base is more stable?: explain S

Answer 32

the less bulky base is more stable the less bulky (less sterically hindered) based can accommodate more solvent reactions and is therefore more stable (tert-butanol is more bulky)

Question 33

define sterically hindered

Answer 33

a sterically hindered compound can accommodate _fewer_ solvent reactions sterically hindered --\> less stable (tert-butanol is more sterically hindered)