Hybridization-2

Bonding in Molecules
Part-III: Hybridization-II
(Remedial Teaching Lecture-1)
Prepared by
D. R. Shinde
Associate Professor in Chemistry
Department of Chemistry
P.D.E.A’s.
Prof. Ramkrishna More
Arts, Commerce and Science College Akurdi,
Pune-411044

In this part we Will learn
Types of Hybridization-Involving s, p and d
Orbitals
Examples to explain Hybridization-Involving
s, p and d Orbitals
Shapes and bond angels in molecules with
Hybridization-Involving s, p and d Orbitals
05/08/2020
D. R. Shinde, Asociate Prof., P.D.E.A's. Prof Ramkrishna More
College, Akurdi, Pune
2

Types of Hybridization-
Involving s, p and d
Orbitals
i. One s + two p + one d orbital - form two
dsp2 hybrid orbitals
ii. One s + three p + one d orbital - form five
iii. One s + three p + two d orbital - form six
d2sp3 hybrid orbitals
iv. One s + three p + three d orbital - form
seven d3sp3 hybrid orbitals
05/08/2020
3

 1. dsp2 hybridization : One s, two p and one d orbitals of same atom having nearly
same energy mix with each other to form four dsp2 hybrid orbitals.
• Four dsp2 hybrid orbitals are oriented at the corners
of the square plane.
• This gives angle between two hybrid orbitals 90˚
• There are five types of d orbitals (dxy, dxz, dyz, dx
2
– y
2
and dz
2). From these dx
2
– y
2 have suitable geometry and
orientation hence it take part in dsp2 hybridization
+
+
S orbital pz and px
orbital orbitals
dx
2
-y
2 orbital
-
-
z
x
-
x
y
05/08/2020
College, Akurdi, Pune 4

Example: [Ni(CN)4]2-: In this complex, Ni(II) ion is central metal ion which undergo
dsp2 hybridization.
 Outer most shell Electronic configuration of ‘Ni (atomic number 28)’ ion is 3d8 4s2, 4p0
 In Complex Ni loss two electron from 4s orbital to form ‘Ni(II)’ ion.
Thus, electronic configuration of Ni(II) ion is 3d8 4s0 4p0
↑↓ ↑↓ ↑↓ ↑↓ ↑↓ ↑↓ ↑↓ ↑↓ ↑↓
 During complex formation, Ni(II) ion undergoes excitation, where two unpaired electrons in 3d orbital
pair with each other 3d8 4s0 4p0
↑↓ ↑↓ ↑↓ ↑↓ ↓ ↑↓ ↑↓ ↑↓ ↑↓
 Thus, one of the 3d i.e. 3dx
2
-y
2 orbital, 4s
orbital and two 4p orbitals are empty. They
undergo dsp2 hybridization to form four dsp2
hybrid orbitals. 3d8 4s0 4p0
↑↓ ↑↓ ↑↓ ↑↓ ↓ ↑↓ ↑↓ ↑↓ ↑↓
dsp2 hybridization05/08/2020
5

 Each CN- ion donate its pair electron to Ni(II) ion to form coordinate bond. The electrons
from the CN- are accommodated in empty hybrid orbitals of Ni(II) ion.
The C of CN- ion consists of lone pair of electron on C atom which is
used for bonding.
:
CN
: +
Four empty dsp2 hybrid orbitals
Lone pair of CN- ion
• Square planar geometry of
[Ni(CN)4]2- complex ion
• Bond angle is 90˚
05/08/2020
6

 2. dsp3 hybridization : One s, three p and one d
orbitals of same atom having nearly same energy mix with
each other to form four dsp3 hybrid orbitals. As such it is
result of sp2 and dp hybridization.
• There are five types of d orbitals
(dxy, dxz, dyz, dx
2
– y
2 and dz
2). From
these dz
2 have suitable geometry and
orientation hence it take part in dsp2
hybridization.
+
S orbital pz, Px and px
orbital orbitals
dz
2 orbital
+-
-
z
x
y
pz and dz
2 orbital
-
-
05/08/2020
7

-
-
Orbitals in
Trigonal plane
Orbitals along vertical
axis, Perpendicular to
trigonal plane
+
-
-
Axial orientation of
two dp hybrid orbitals
Trigonal planar
orientation of three
sp2 hybrid orbitals
Example: PCl5 Molecule
In PCl5 Molecule central P has dsp3 hybridization AO’s
 Ground state outer most
shell Electronic configuration
of P (At. No. 15) is
3d0
3s2 3p3
↑↓ ↑↓ ↑↓ ↑↓ ↓↑↓ ↑↓ ↑↓ ↑↓
05/08/2020
8

 Excited state, outer most
shell Electronic Configuration
of P (At. No. 15) is
3d1
3s1 3p3
↑↓ ↑↓ ↑↓ ↑↓ ↓↑↓ ↑↓ ↑↓ ↑↓
of P in hybridized state is
3d0dsp3 hybrid orbitals
↑↓ ↑↓ ↑↓ ↑↓ ↓↑↓ ↑↓ ↑↓ ↑↓
dsp3 hybridization
-
-
Five dsp3 hybrid Orbitals
on P atom in excited state
When reaction starts between P and Cl2 gas, P atom
undergoes excitation. One electron from 3s orbital is
promoted to the higher energy 3d orbital.
 In excited state P atom undergoes dsp3 hybridization
05/08/2020
9

Cl (17) ground and excited state
Outer shell electronic configuration:
↑↓ ↑↓ ↑↓ ↑
3s2 3px
2 3py
2 3pz
1
Cl atom has half filled 3pz orbital which take part in
bonding. It form axial overlap with half filled hybrid orbital
of P atom to form P-Cl sigma bond
 Thus, in excited state P consists of five half filled hybrid
orbitals which take part in bonding with chlorine.
05/08/2020
10

-
-
pz orbital of 5 Cl atom
-
+5
Hybrid orbitals of P atom
-
-
-
-
-Process of orbital overlap to form P-Cl sigma bonds
 PCl5 Molecule:
 i) Structure – Trigonal Bipyramidal,
ii) Cl - P – Cl Bond angle - 120˚ in trigonal
plane and 90 ˚ between trigonal plane
and vertical axis.
PCl5 molecule
P
Cl
90˚
120˚
05/08/2020
11

 3. d2sp3 hybridization:
One s, three p and two d
orbitals of same atom
having nearly same energy
mix with each other to form
six d2sp3 hybrid orbitals. As
such it is result of dsp2 and
dp hybridization.dsp2 hybridization
s + px + py +
dx
2-y
2 orbitals
dp hybridization
Pz + dz
2
-
-
S orbital pz and px orbitals dx
2
-y
2 orbital
-
x
y
-
-
z
x
y
dz
2 orbital
Four dsp2
hybrid orbitals Two dphybrid
orbitals
05/08/2020 D. R. Shinde, Asociate Prof., P.D.E.A's. Prof Ramkrishna More
12

• Six d2sp3 hybrid orbitals are oriented at the corners of
the octahedron.
• This gives angle between two adjutant hybrid orbitals
90˚
-
-
Octahedrondsp2 hybrid orbitals dp hybrid orbitals
-
-
+
x
y
Z
05/08/2020
13

Example of d2sp3 hybridization od AO’s: S in SF6 Molecule
In SF6 Molecule central S has d2sp3 hybridized AO’s
 Ground state, outer most
of S (At. No. 16) is
3d0
3s2 3p4
↑↓ ↑↓ ↑↓ ↑↓ ↓↑↓ ↑↓ ↑↓ ↑↓
of S is
3d2
3s2 3p3
↑↓ ↑↓ ↑↓ ↑↓ ↓↑↓ ↑↓ ↑↓ ↑↓
of S in hybridized state is
3d0Six d2sp3 hybrid orbitals
↑↓ ↑↓ ↑↓ ↑↓ ↓↑↓ ↑↓ ↑↓ ↑↓
d2sp3 hybridization
 When reaction stats between S and F2 gas, S atom undergoes excitation. One electron
from 3s and one electron from 3p orbital is promoted to the higher energy 3d orbital.
 In excited state S atom undergoes d2sp3 hybridization
05/08/2020
14

F (9) ground and excited state
Outer shell electronic configuration:
↑↓ ↑↓ ↑↓ ↑
2s2 2px
2 2py
2 2pz
1
F atom has half filled 2pz orbital which take part in
bonding. It form axial overlap with half filled hybrid orbital
of S atom to form S-F sigma bond.
 Thus, in excited state S consists of six half filled hybrid
orbitals which take part in bonding with Fluoride.
-
-
05/08/2020
15

-
-Process of orbital overlap to form S-F sigma bonds
 SF6 Molecule:
 i) Structure –
Square planar Bipyramidal,
ii) F – S – F Bond angle - 90˚
6
pz orbital of 6 F atom
-
Hybrid orbitals of ‘S’ atom
-
-
-
-
S
F
05/08/2020
16

Sr.
No
Pure Orbitals
used for
hybridization
Hybridi-
zation
Geometry Bond
Angle
Example
1
s, two p
and one d
dsp2 Square
Planar
90˚
[Ni(CN)4]2-
[PtCl4]
2
s, three p
and one d
dsp3 Trigonal
bipyramidal
120˚ and
90˚ PCl5
3
s, three p and
two d
d2sp3 Octahedral 90˚ SF6
Summery
05/08/2020
17

05/08/2020
18

Hybridization-2

Recommended

Recommended

More Related Content

What's hot

What's hot (20)

Similar to Hybridization-2

Similar to Hybridization-2 (20)

Recently uploaded

Recently uploaded (20)

Hybridization-2