Summary
Summary Lone pairs and shapes of molecules
- Institution
- PEARSON (PEARSON)
Shows different shapes of molecules that occur when central atoms have different numbers of bonds and electron pairs.
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I. ONE PAIRS & SHAPETYPES OF BONDS
ELECTRON PAIR REPULSION THEORY
•
The shape of a molecule is determined by the covalent : shared pair of
electrons ( ≥ 1)
electron pairs surrounding the central atom .
↳ only ionic :
referring to the outer shells .
giving or
accepting
electrons between
•
Based on the fact pairs of electrons repel
metal and non -
meta
other electron pairs ( to minimise repulsion )
TRIGONAL PLANAR TETRAHEDRAL
0 ◦
double bond treated 0
120% [ ] 120°
as
single /I
µ 5 ]II / angle 109.5°
• all 120° around central 109.5° ◦
all bond
atom ''
-
0
0¥70
'
CO32
- -
0%11
◦
0
-
0 •
dative bond treated
as
regular bond
"
.
• all 120°
- .
o
1 EFFECTS OF LONE PAIRS
dative bond .
The extra repulsion decreases all bond
angles by 2.5°
TRIGONAL B/ PYRAMIDAL lone pair
in
three bonding
-
CI
""
H -
Ñ -
H
pairs
jf%fp bonding pairs lone pair
-
fine one
- .
, µ ,
-
bond angle 90° to
107° H 107° -
based on tetrahedral
} 90
/ g• Cl
atoms above / below ↳ pyramidal , 109-5-2.5
a
-
bond angle 120° to
= 107°
atoms on planar / =
trigonal
OCTAHEDRAL -
two lone pairs
:O
.
two
bonding pairs
-
.
F F It 109-5-(2.5×2)=104.50
F%%
H
six bonding pairs
-
-
.
-
all bond angles
-
V
-
shaped / bent
90° < ( on the central plane .
And tag above and below)
F 90°
F F are .
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