Covalent bonding occurs when two atoms share electrons to achieve a more stable electron configuration, typically forming molecules. This type of bond usually happens between nonmetals and results in the formation of strong, stable compounds. The shared electrons allow each atom to attain a full ou...
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
.CM#0fe*+rnszinan+ib-ondngorb-ag)gYYeY' %
-
number electrons
of
bonding orbitals
shares a
single pair
bond order in
?⃝
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