chapter9.CO#ntbondng- wavefunction spherically symmetric distribution
centered on the nucleus > Which is
Hi'=HH+→bonaoraer¥
1-12=1-1:H → bond order -_ 1
ground
-
state
attire center and reduces exponentially
at larger distances Tetrahedral
largest Hez=H:H → bond order-_ 0
molecular orbital theory
-
electrons lnamolecule
are not assigned -10 Individual chemical bonds between
" "" " " " e " " " M " " " "
µ µ
of the atom "
atoms ,bu+ are treated as moving
under the influence
\ / Li -2=1; Lit→ bond
- order
__1z
molecule -
both atoms are the same element, the same orbitals w '" overlap H -
C -
C -
H
mononuclear diatomic Liz =L ; :L; → bond order=/
and form molecular orbitals /
together
H 1µg
orbital describes the attractive interactions between the atomic orbitals ottwoormoreatomsina
bonding
-
molecule Bez → bond order -_ 0
hybridization →
internuclear axis
-
Imaginary straight-line that connects the nuclei of atoms bounded to eachother in a molecule Betz→ bond order-_ 1/2
between two atoms and helps -10 raise
orbital molecular orbital that weakens the chemical bond
antibonding
-
"
*
" " " " "" " " "" "" " " "" "
" " " ""
"
"
" " """ " " " "" " "" " " " ""
ZPO Cz double bond (
internuclear distance the distance between two nuclei lnamoleoule
4-20-1=2 diamagnetic
-
,
,
paramagnetic unpaired electron 2%0 Nz Triple bond (6-21)=3
-
.
, diamagnetic
Molecular Orbitals
diamagnetic
-
all electrons are paired .
250
(
-
Oz double bond ,(
6-22-7=2 , paramagnetic
broken down by photons ; interaction of with
photo dissociation chemical -
compound is one or more photons
one + argetmaeaue.no, , ,m,+ea+o×,s,b,eugn+ Zpz f single bond,
,
spatial arrangement of atoms within molecules
N/A
cis-trans Isomerism
-
Nez bond
(6-21)=0
[
no ,
' "
HC CH
3 Less stable
3 12 31
c=c nodal plane
*
¥⇐¥
'
qq.FI#&q--*-
"
①
wB€→¥BEaB%
- N
E€→
srihybrid molecular orbital /
( antibonding)
localized framework -7
¥¥¥%⇐⇐ sa*nybnd ¥Y+*Ba#→"Éq% %qq•q
↳ % " mains
•
•
straight
associated
lines
with particular atoms
molecular orbital •
located between atoms
I bonding)
E€€¥Ñ¥ ¥ "
Sp×d hybrid bondangieofoisa little less than 109°
1
H O H bond angle
- - is 90°
delocalized IT framework -7
¥ ¥ ¥ ¥¥?§¥µ •g ←
Correct bond combine Aoson central atom -10 form hybrid AO 's
angle →
bonding
•
non
sitetranedral SN bond angle is 1800
•
circles
120°
.
5111=3 bond angle is •
associated with all atomslnamolealle
514=4 bond angle is 109.5° •
Located above and below atoms
5111=5 bond angle are 90° and 120°
H H
E ±¥¥¥Ñ%:¥B•E¥a•g
514=6 bond 900
'
angle is
Sp trigonal planar • •
• ⇐÷→ t
Spz
1-1 1 Hoo C •
C • H
⇐EÉ¥±⇐¥.;io•¥#É?a%-¥É.*E;T -B - - - - - - -* a
:
• •
•
1%2 0
B. °
•
C
•
H
T
H
⇐ ¥ i•±É☒→¥ ¥?TM¥• •gµ•⇐ •
H••• IT framework G) Sigma framework
→£⇐¥¥÷s* .
) ( :S 'h91e bond
.CM#0fe*+rnszinan+ib-ondngorb-ag)gYYeY' %
-
number electrons
of
bonding orbitals
shares a
single pair
bond order in
?⃝
centered on the nucleus > Which is
Hi'=HH+→bonaoraer¥
1-12=1-1:H → bond order -_ 1
ground
-
state
attire center and reduces exponentially
at larger distances Tetrahedral
largest Hez=H:H → bond order-_ 0
molecular orbital theory
-
electrons lnamolecule
are not assigned -10 Individual chemical bonds between
" "" " " " e " " " M " " " "
µ µ
of the atom "
atoms ,bu+ are treated as moving
under the influence
\ / Li -2=1; Lit→ bond
- order
__1z
molecule -
both atoms are the same element, the same orbitals w '" overlap H -
C -
C -
H
mononuclear diatomic Liz =L ; :L; → bond order=/
and form molecular orbitals /
together
H 1µg
orbital describes the attractive interactions between the atomic orbitals ottwoormoreatomsina
bonding
-
molecule Bez → bond order -_ 0
hybridization →
internuclear axis
-
Imaginary straight-line that connects the nuclei of atoms bounded to eachother in a molecule Betz→ bond order-_ 1/2
between two atoms and helps -10 raise
orbital molecular orbital that weakens the chemical bond
antibonding
-
"
*
" " " " "" " " "" "" " " "" "
" " " ""
"
"
" " """ " " " "" " "" " " " ""
ZPO Cz double bond (
internuclear distance the distance between two nuclei lnamoleoule
4-20-1=2 diamagnetic
-
,
,
paramagnetic unpaired electron 2%0 Nz Triple bond (6-21)=3
-
.
, diamagnetic
Molecular Orbitals
diamagnetic
-
all electrons are paired .
250
(
-
Oz double bond ,(
6-22-7=2 , paramagnetic
broken down by photons ; interaction of with
photo dissociation chemical -
compound is one or more photons
one + argetmaeaue.no, , ,m,+ea+o×,s,b,eugn+ Zpz f single bond,
,
spatial arrangement of atoms within molecules
N/A
cis-trans Isomerism
-
Nez bond
(6-21)=0
[
no ,
' "
HC CH
3 Less stable
3 12 31
c=c nodal plane
*
¥⇐¥
'
qq.FI#&q--*-
"
①
wB€→¥BEaB%
- N
E€→
srihybrid molecular orbital /
( antibonding)
localized framework -7
¥¥¥%⇐⇐ sa*nybnd ¥Y+*Ba#→"Éq% %qq•q
↳ % " mains
•
•
straight
associated
lines
with particular atoms
molecular orbital •
located between atoms
I bonding)
E€€¥Ñ¥ ¥ "
Sp×d hybrid bondangieofoisa little less than 109°
1
H O H bond angle
- - is 90°
delocalized IT framework -7
¥ ¥ ¥ ¥¥?§¥µ •g ←
Correct bond combine Aoson central atom -10 form hybrid AO 's
angle →
bonding
•
non
sitetranedral SN bond angle is 1800
•
circles
120°
.
5111=3 bond angle is •
associated with all atomslnamolealle
514=4 bond angle is 109.5° •
Located above and below atoms
5111=5 bond angle are 90° and 120°
H H
E ±¥¥¥Ñ%:¥B•E¥a•g
514=6 bond 900
'
angle is
Sp trigonal planar • •
• ⇐÷→ t
Spz
1-1 1 Hoo C •
C • H
⇐EÉ¥±⇐¥.;io•¥#É?a%-¥É.*E;T -B - - - - - - -* a
:
• •
•
1%2 0
B. °
•
C
•
H
T
H
⇐ ¥ i•±É☒→¥ ¥?TM¥• •gµ•⇐ •
H••• IT framework G) Sigma framework
→£⇐¥¥÷s* .
) ( :S 'h91e bond
.CM#0fe*+rnszinan+ib-ondngorb-ag)gYYeY' %
-
number electrons
of
bonding orbitals
shares a
single pair
bond order in
?⃝
