Review :
acetone
alkylchloride , 5
X
S+
g- Il
R Cl - +
A +
H20 -
why won't this rxn work ? for this to work ,
carbon and the alky need
to form a bond They . are both S positively charged They
. cannot bond .
The C-OH bond does not have an issue due to opposing s charges.
to make this work we must approach stepwise.
i ⑧
XOmgBr
.
s
R-mg-Br + +
note :
we have
St
method to create
new carbon bonds.
Carbon is rarely Polarized and is therefore very stable .
the inversion of polarity on the alkyl group is significant.
>
-
the Gringard reactants
by Viktor Gringard (1912) .
atom Xp the electronegativity of the atom dictates the rxn ,
C 2 5 .
are responsible for the reverse polarity.
Cl 3 I the nucleophile carbon attacks the electrophilic
.
3 4
⑧ .
Ketone.
Mg 1 3 the
.
then Grighard reagents behave as nucleophiles.
R-H HO-mgX
R-mg-Br H20
+ + +
O O
ROMgBrRoh
Il
R-mg-Br c -
=
+ O =
0
note that due to high stability CO2 is not used as a
reactant ,
but we can react it using Grigand reactions.
O
then
RUR"
R CEN [H30Jt
R-mg- Br + > + NH3 +
HOMgBr
-
- .
↑
similar to
above.
they also work for alkyl Lithiums .
HzC-Br - HzC-Li LiBr +
5- s + Zi
,transition metals :
a metal with an empty or incomplete or f
-
orbital in one or more of its oxidation states (incomplete shell) .
+
there are no known oxidation states of Zinc where it is not
full and it behaves like the p-block (and the rest of the
elements in the column are not transition metals .
chemistry acossiated with transition metals :
i. complexed compounds
-
11 ·
organic chemistry reagents
..
III .
magnetism , colour ,
reactivity.
metals are viewed as electropositive where the ligands
are electron donors. multiple ligands can bind depending on
oxidation state. predominately interested in carbon-based ligands.
Zeise's Salt (1827) ferrocene (1957)
"
"sandwich compound
Ko
IClipI -
Fe-
the geometry of the metal complex is attributed to steric factors for each
lig and to spatially separate . We also consider non-bonding / lone electrons.
for common geometries ,
lone pairs , angles , and coordination numbers ,
refer to the USEPR theory chart.
of relavent orbitals
view
:
MM
S
#
Py PX Pz
lone phase) middle two phases ,
on named axis.
of axises. bonding happens on axis .
#
, Y
·
dxy , tzg dxztzg diz ,
tz dz , eg dx -
y , eg
bonding off the axises two phases. , bonding on axises two phases. ,
tfield
a l
theory part 1 :
degeneracy :
the same energy.
...... Seg off axis
- - - -
. E
4
- axis.
degenerate
ya-stug
all on
dXy
versus. low Spin
⑭spin determining high spin
:
versus low
Metic
- - spin complexes comes to the quantification
id"
of the Pauli-Exclusion principle and
the Aufbau Principle , and by the
field splitting energy , .
8
theSpin is also controlled by the type of lig and bonded to the metal .
[Fe(H20)] has a high spin configuration with 5 delections. [Fe(col] has a
low spin configuration with 6 delections.
bonding and overlap not all orbitals !
- can overlap They must have the
correct symmetery (o ,
it , 8 ,
eg , tzg etc) Spatial overlap (the ability to occupy
, , the
same region of space) and similar energies.
,
O ⑭0 & moderate
/
m momia ⑭mox
L
/I
best overlap
/I
worst overlap
⑭
ju dXY PY
overlap results
in a it bond.
&
e bonds
:
any Lewis base can be a Ligand .
The donation of a lewis
base to a lewis adid does not get a charge another way . to depict this is by
the use of an arrow indicating a covalent bond.
H H H
F H
Fi
F F
N
# -N
Fun H
, ,
⑦
=
>
-
F B - -N H
-
- -
#H # H # H
Yindicates ionic (wrong Y dative bond
, A reminder about bonding and overlap :
MMMMMMMM the in-phase combination ,
s orbital
-- M
*
>
out-phases , antibonding ,
o
3
M + C un
&
*
#
men also
+ >
- mm un
*
-M
#
Shr the promotion of an electron
~
.
1
antibonding orbital
*
into an
&: 11 1
from a -bonding one
through
- the energy of a photon
1 1V
1 ---- --
-
-
---- IV ----
o .
au mu au
acetone
alkylchloride , 5
X
S+
g- Il
R Cl - +
A +
H20 -
why won't this rxn work ? for this to work ,
carbon and the alky need
to form a bond They . are both S positively charged They
. cannot bond .
The C-OH bond does not have an issue due to opposing s charges.
to make this work we must approach stepwise.
i ⑧
XOmgBr
.
s
R-mg-Br + +
note :
we have
St
method to create
new carbon bonds.
Carbon is rarely Polarized and is therefore very stable .
the inversion of polarity on the alkyl group is significant.
>
-
the Gringard reactants
by Viktor Gringard (1912) .
atom Xp the electronegativity of the atom dictates the rxn ,
C 2 5 .
are responsible for the reverse polarity.
Cl 3 I the nucleophile carbon attacks the electrophilic
.
3 4
⑧ .
Ketone.
Mg 1 3 the
.
then Grighard reagents behave as nucleophiles.
R-H HO-mgX
R-mg-Br H20
+ + +
O O
ROMgBrRoh
Il
R-mg-Br c -
=
+ O =
0
note that due to high stability CO2 is not used as a
reactant ,
but we can react it using Grigand reactions.
O
then
RUR"
R CEN [H30Jt
R-mg- Br + > + NH3 +
HOMgBr
-
- .
↑
similar to
above.
they also work for alkyl Lithiums .
HzC-Br - HzC-Li LiBr +
5- s + Zi
,transition metals :
a metal with an empty or incomplete or f
-
orbital in one or more of its oxidation states (incomplete shell) .
+
there are no known oxidation states of Zinc where it is not
full and it behaves like the p-block (and the rest of the
elements in the column are not transition metals .
chemistry acossiated with transition metals :
i. complexed compounds
-
11 ·
organic chemistry reagents
..
III .
magnetism , colour ,
reactivity.
metals are viewed as electropositive where the ligands
are electron donors. multiple ligands can bind depending on
oxidation state. predominately interested in carbon-based ligands.
Zeise's Salt (1827) ferrocene (1957)
"
"sandwich compound
Ko
IClipI -
Fe-
the geometry of the metal complex is attributed to steric factors for each
lig and to spatially separate . We also consider non-bonding / lone electrons.
for common geometries ,
lone pairs , angles , and coordination numbers ,
refer to the USEPR theory chart.
of relavent orbitals
view
:
MM
S
#
Py PX Pz
lone phase) middle two phases ,
on named axis.
of axises. bonding happens on axis .
#
, Y
·
dxy , tzg dxztzg diz ,
tz dz , eg dx -
y , eg
bonding off the axises two phases. , bonding on axises two phases. ,
tfield
a l
theory part 1 :
degeneracy :
the same energy.
...... Seg off axis
- - - -
. E
4
- axis.
degenerate
ya-stug
all on
dXy
versus. low Spin
⑭spin determining high spin
:
versus low
Metic
- - spin complexes comes to the quantification
id"
of the Pauli-Exclusion principle and
the Aufbau Principle , and by the
field splitting energy , .
8
theSpin is also controlled by the type of lig and bonded to the metal .
[Fe(H20)] has a high spin configuration with 5 delections. [Fe(col] has a
low spin configuration with 6 delections.
bonding and overlap not all orbitals !
- can overlap They must have the
correct symmetery (o ,
it , 8 ,
eg , tzg etc) Spatial overlap (the ability to occupy
, , the
same region of space) and similar energies.
,
O ⑭0 & moderate
/
m momia ⑭mox
L
/I
best overlap
/I
worst overlap
⑭
ju dXY PY
overlap results
in a it bond.
&
e bonds
:
any Lewis base can be a Ligand .
The donation of a lewis
base to a lewis adid does not get a charge another way . to depict this is by
the use of an arrow indicating a covalent bond.
H H H
F H
Fi
F F
N
# -N
Fun H
, ,
⑦
=
>
-
F B - -N H
-
- -
#H # H # H
Yindicates ionic (wrong Y dative bond
, A reminder about bonding and overlap :
MMMMMMMM the in-phase combination ,
s orbital
-- M
*
>
out-phases , antibonding ,
o
3
M + C un
&
*
#
men also
+ >
- mm un
*
-M
#
Shr the promotion of an electron
~
.
1
antibonding orbital
*
into an
&: 11 1
from a -bonding one
through
- the energy of a photon
1 1V
1 ---- --
-
-
---- IV ----
o .
au mu au
