1
.
allylic lone pair
-
Compound contains C = C bond
V
Atoms Connected to the called
vinylic positions >
-
vinylic positions are
allylic positions
vinylic positions allylic positions
>
- >
-
:
not allylicG EX . ·
...
J I all have a it next to a lone pair
Lone pairs are not next to c= c f are not
allylic Lone pairs (next to C= c or
any other doubleon(
↳ :
& Z
↓ ↑O
G:
① Q I
. G 0
09/07 Ch3 .
sec 3 1-3 2 .
.
conjugate Conjugate
Intro to Acid + Bases Base Acid It
- I
Bases transfer of
: a Proton (Proton acceptor HHH + H-H
Acid : Proton donor (Acid =
Away Acid (donor) Base (accepta
conjugate Base :
What remains of the acid (on product Side Cons Acid
.
Coni . base
Conjugate
j H
Acid : What formed after the base accepted a proton H
base
3 2 flow of Electron
.
Density : Curved Arrow Notation
-
i HH
Not the same arrows used in resonance structures &
↳ arrows arc used as tools I do not represent the real physical process
In the reaction above the arrows DO represent
,
an actual physical process.
-
There's a flow of electron density that causes a proton to be transferred from one reagent to another >
- curved arrow
↳ show a
1 Proton transfer
A-
B: H A + -
-> B -
H + A! Reaction Mechanism
-
can
only happen if its abase >
-
acid proton transfer
↳
Acids don't lose protons wort the participation of a base
, 09/10 Klein Ch3 sec 3 3-3 6
.
.
Bronsted -
lowry Acidity Comparing pKa values
:
Using PKa to Compare Acidity
HA+ H20 - A+ HyOt
acid base
&
equilibrium = Kea
Key
=H
O - large Product concentrations
Small ProductConcentrations
- Keat
I large Small Product Concentrationas
Product Concentrations
=
Keq71
Ka =
Key (HO] =S
A
very strong acids can have
extremely large ka (often very small or
very large
pKa -logka =
Using pka to compare Basicity
-weakest acid has strongest base stronger weaker
-
Using pka to predict position of Equilibrium - OH
·
Ea will
always favor weaker acid/base H0H HO-
base Acid cons Acid Consbase
Pla 14 0
=
.
PKa = 1S
I product acidpla-reactant acid pica
Kea If =
14)
kea 1048 104
-
= =
3 4 factors Affecting
.
Stability of Anions
the
comparing structures w/ no net charge (HAvcHB) = W/ Net Charge (HAvs HBt
HAA :
If A is very stable unattractive
-
relatively
If A is a weak base-HA will be a strong Acid
If A is
very Unstable >
-
Very reactive comparing energy involved in deprotonating various acids
H D
Chy NHs H20
Pa J significant a
Pka = 50 Pka 38
=
Oka : 14 trends on periodic table
↓ ↓ -Charge localized
M
CH5 HO- Increasing En Increasing size
-less stable anion
-
Stronger base
lessimportant more important)
: j
Very unstable relatively Stable N
↑ Charge delocalized
1 mor stable anion
-
less
highly
-
reactive reactive : -
Weaker base
-
Strong base Weak base
.
allylic lone pair
-
Compound contains C = C bond
V
Atoms Connected to the called
vinylic positions >
-
vinylic positions are
allylic positions
vinylic positions allylic positions
>
- >
-
:
not allylicG EX . ·
...
J I all have a it next to a lone pair
Lone pairs are not next to c= c f are not
allylic Lone pairs (next to C= c or
any other doubleon(
↳ :
& Z
↓ ↑O
G:
① Q I
. G 0
09/07 Ch3 .
sec 3 1-3 2 .
.
conjugate Conjugate
Intro to Acid + Bases Base Acid It
- I
Bases transfer of
: a Proton (Proton acceptor HHH + H-H
Acid : Proton donor (Acid =
Away Acid (donor) Base (accepta
conjugate Base :
What remains of the acid (on product Side Cons Acid
.
Coni . base
Conjugate
j H
Acid : What formed after the base accepted a proton H
base
3 2 flow of Electron
.
Density : Curved Arrow Notation
-
i HH
Not the same arrows used in resonance structures &
↳ arrows arc used as tools I do not represent the real physical process
In the reaction above the arrows DO represent
,
an actual physical process.
-
There's a flow of electron density that causes a proton to be transferred from one reagent to another >
- curved arrow
↳ show a
1 Proton transfer
A-
B: H A + -
-> B -
H + A! Reaction Mechanism
-
can
only happen if its abase >
-
acid proton transfer
↳
Acids don't lose protons wort the participation of a base
, 09/10 Klein Ch3 sec 3 3-3 6
.
.
Bronsted -
lowry Acidity Comparing pKa values
:
Using PKa to Compare Acidity
HA+ H20 - A+ HyOt
acid base
&
equilibrium = Kea
Key
=H
O - large Product concentrations
Small ProductConcentrations
- Keat
I large Small Product Concentrationas
Product Concentrations
=
Keq71
Ka =
Key (HO] =S
A
very strong acids can have
extremely large ka (often very small or
very large
pKa -logka =
Using pka to compare Basicity
-weakest acid has strongest base stronger weaker
-
Using pka to predict position of Equilibrium - OH
·
Ea will
always favor weaker acid/base H0H HO-
base Acid cons Acid Consbase
Pla 14 0
=
.
PKa = 1S
I product acidpla-reactant acid pica
Kea If =
14)
kea 1048 104
-
= =
3 4 factors Affecting
.
Stability of Anions
the
comparing structures w/ no net charge (HAvcHB) = W/ Net Charge (HAvs HBt
HAA :
If A is very stable unattractive
-
relatively
If A is a weak base-HA will be a strong Acid
If A is
very Unstable >
-
Very reactive comparing energy involved in deprotonating various acids
H D
Chy NHs H20
Pa J significant a
Pka = 50 Pka 38
=
Oka : 14 trends on periodic table
↓ ↓ -Charge localized
M
CH5 HO- Increasing En Increasing size
-less stable anion
-
Stronger base
lessimportant more important)
: j
Very unstable relatively Stable N
↑ Charge delocalized
1 mor stable anion
-
less
highly
-
reactive reactive : -
Weaker base
-
Strong base Weak base
