VSEPR Theory & Hybridization

1. Made by:-
Sauhard Singhal

2. The shape of the molecule is determined by
repulsions between all of the electron
present in the valance shell.
Electron pairs in the valence shell of the
central atom repel each other and align
themselves to minimize this repulsion.
Lone pair electrons takes up more space
round the central atom than a bondpair.
Lone pair attracted to one nucleus, but
bond pair is shared by two nuclei.
The minimum repulsions to the state
minimum energy and maximum stability of
the molecule.

3. Lone pair -Lone pair  Lone
pair -Bond pair  Bond
pair-Bond pair

4. Triple bond >double bond
>single bond

5. Presence of lone pairs on the central atom
causes slight distortion of the bond angles
from the ideal shape.
The magnitude of repulsions between
bonding pairs of electrons depends on the
electronegativity difference between the
central atom &the other atoms .

6. Determine the central atom.
Draw the electron dot structure and bar
diagram
Find arrangement of electron pairs.
Find arrangement of bonding pairs.
Determine the geometry based on of
bonding pairs.

7. BONDED PAIRS OF ELECTRONS
ONLY

8. There are two electron pairs in the valance
shell of Beryllium. [1s2 2s2 ]
Molecular geometry-Linear arrangement
H HBe

9. Three electron pairs in the valance shell of
Boron. [1s2 2s2 2p1 ]
Molecular geometry- Trigonal Planar
arrangement
B
F
F
F

13. BONDED PAIRS AS WELL AS LONE
PAIRS OF ELECTRONS

15. Molecular geometry- V-Shaped or Bent
shape
Electron pairarrangement- Tetrahetral
Repulsions between Lonepair- Lonepair ,
Lonepair -Bondpair is possible.
It causes slight distortion from 109⁰28′ to
104⁰27′

18. 102⁰30′

22. It fails to predict the shapes of isoelectronic
species[CH4&NH4
+] and transition metal
compounds.
This model does not take relative sizes of
substituents .
Unable to explain atomic orbitals overlap.

24. Concise Inorganic chemistry-J.D.LEE[Fifth
edition]-Black well publishing.
Chemistry-Raymond chang.
Pictures from Wikipedia- free encyclopedia-
www. Wikipedia.org.
Pictures from Google Images.
Thanks to my Teachers &
friends

26. The intermixing of two or more pure atomic
orbital's of an atom with almost same energy to
give same number of identical and degenerate
new type of orbital's is known as hybridization.
The new orbital's formed are also known as
hybrid orbital's.
During hybridization, the atomic orbital's with
different characteristics are mixed with each
other.

27. sp
sp2
sp3
sp3d
sp3d2
sp3d3

28. Intermixing of one 's' and one 'p'
orbital's of almost equal energy
to give two identical and
degenerate hybrid orbital's is
called 'sp' hybridization.
These sp-hybrid orbital's are
arranged linearly at by making
180 ⁰ of angle.
They possess 50% 's' and 50% 'p'
character.

29. Intermixing of one 's' and two
'p' orbital's of almost equal
energy to give three identical
and degenerate hybrid orbital's
is known as sp2 hybridization.
The three sp2 hybrid orbital's
are oriented in trigonal planar
symmetry at angles of 120 ⁰ to
each other.
The sp2 hybrid orbital's have
33.3% 's' character and 66.6%
'p' character.

30. In sp3 hybridization, one 's'
and three 'p' orbital's of almost
equal energy intermix to give
four identical and degenerate
hybrid orbital's.
These four sp3 hybrid orbital's
are oriented in tetrahedral
symmetry with 109 ⁰ 28' angle
with each other.
The sp3 hybrid orbital's have
25% ‘s’ character and 75% 'p'
character.

31. In sp3d hybridization, one 's', three 'p'
and one 'd' orbital's of almost equal
energy intermix to give five identical and
degenerate hybrid orbital's, which are
arranged in trigonal bipyramidal
symmetry.
Among them, three are arranged in
trigonal plane and the remaining two
orbital's are present above and below the
trigonal plane at right angles.
The sp3d hybrid orbital's have 20% 's',
60% 'p' and 20% 'd' characters.

32. Intermixing of one 's', three 'p' and two
'd' orbital's of almost same energy by
giving six identical and degenerate
hybrid orbital's is called sp3d2
hybridization.
These six sp3d2 orbital's are arranged in
octahedral symmetry by making 90 ⁰
angles to each other. This arrangement
can be visualized as four orbital's
arranged in a square plane and the
remaining two are oriented above and
below this plane perpendicularly.

33. In sp3d3 hybridization, one 's', three 'p'
and three 'd' orbital's of almost same
energy intermix to give seven sp3d3
hybrid orbital's, which are oriented in
pentagonal bipyramidal symmetry.
Five among the sp3d3 orbital's are
arranged in a pentagonal plane by
making 72⁰ of angles. The remaining are
arranged perpendicularly above and
below this pentagonal plane.

34. ē Pair
Hybridizatio
n
Shape
2 sp linear
3 sp2 trigonal planar
4 sp3 tetrahedral, pyramidal, or
bent
5 sp3d
trigonal bipyramidal,
trigonal planar, or linear
6 sp3d2 octahedral, square planar,
or linear

35. THANK YOU