acids and bases

Bronsted Lowry Acid

proton donator

Bronsted Lowry Base

proton acceptor

CA

Base + H+

CB

Acid - H+

amphiopiotic

can donate or accept H+ depending on conditions (ex. water)

acidic

[H+] >[OH-]

basic

[H+]

flow of electron density

high e- density --> low e- density

arrows indicate

a flow of e- density and a shift of H+

strong acid / base dissociates

completly

weak acid/base dissociates

ka =

[products] / [reactants]

big ka

strong acid, products dominate (same as small pka)

small ka

weak acid, reactants dominate (same as big pka)

pka =

-log ka

big pka

weak acid, reactants dominate (same as small ka)

small pka

strong acid, products dominate (same as big ka)

equilibrium always favors

side with weaker acid and stronger base

stability of orbitals

sp > sp2 > sp3

(O) a neg. charge is more stable if it

is held closely to the pos. nucleus

induction (definition)

the withdrawal of e- density away from a neg. charge region of a structure thus spreading out the charge

neg. charge is drawn to

EN atoms and bigger atoms

equil will favor _____ base

more stable

what you are protonating is the

base

what you are deprotecting is the

acid

if equil favors product

suitable reagent

if equil favors reactants

not suitable reagent

leveling effect

water can be an acid or a base

___ more stable --> equil favors products --> suitable reagent

CB

___ more stable --> equil favors reactants --> not suitable reagent

Base

counter ions

spectator ions

counterions always ___ but never ____

always present but never chemically involved

counterions necessary to

balance overall charge of a solution

solvating effect is used to explain

slight differences in pka when ARIO analysis of two bases are identical

solvating effects (def.)

the more solvent molecules that can be around base, the more stable the base will be

_____ prevents solvent molecules from getting to the atom

branching

lewis acid

accepts and shares pair of e-

lewis base

donates and shares pair of e-