Molecular Orbital Theory
electrons
as
waves
constructive
~
~
+
+
t
+
N
=
=
MO
°
the electron
whenever
is
between it favors
in
t
←
F-
e
←
-
-
e
→
t
net
→
F
force
=
attractive
F
destructive
✓
+
favors bonding
,
←
F
\
bonding
,
F
F
→
,
=
"
'
-
+
t
-
anti
=
.
E
+
e-
←
F
example
:
F
F
→
←
→
OH
F
does
-
Ha
+
HB
Ho
not
-
electrons
are
favor bonding
low energy
t
exothermic
Ha
as
\
Isa
bonding
e-
anti
-
,
BE ABO
2-
bonding
=
=
=
I
usually single
SB
bonding
Gs
-
Bond order
bonding
l
Jeasytogodon.nl
11
-
releases energy
as they form a bond
'
-
e
-
HB
anti
l
MO
\ node
high
Ha
bonding
outside
H,
=
-
.
.
F
e-
+
→
,
,
bond
MO
MO
example
-
Hz
:
Ha
-
Ha
-
HB
Bond order
1
✓
2
electrons
for
H
=
=
'T
-
÷
ISB
ISA
Gio :*
n
,
-
Els
example
:
He ,
Hez
He
He
Bond order
ff
Qs*
'
.
.
2
=
=
o ✓
no
bond
so
this molecule does
not exist !
It
11
IS
IS
11
oisoistx
o
IS
example
:
Liz
Liz
L;
L;
L;
-
→
-
%*
I
as
)
71
→
/
1
q;
u
25
Li
25
IS
Li
BO
=
'
Is electrons do not
25
(
l
=
participate
orbitals would overlap
orbital )
Is
025
IS
only
Is Is
I
Zpx
2Pa
spy
in
#
-
€p-
-
,
,§"
phase
Ozp
=
t
thigh probability
'
.
out
of
side
-
phase
At
+
side
%*
node
constructive
a
=
.
destructive
+
head
-
If
Thp*
=
head overlap
T2px
-
z
bonding
I
=
overlap
+
.
02ps
,
Tlzpx Tlzpy
,
:
-
anti
-
bonding