The document by A.K. Gupta discusses hybridization in chemistry, detailing types such as sp3, sp2, and sp along with their geometries and bond formation properties. It describes how hybrid orbitals are formed and their roles in sigma and pi bond creation, particularly in molecules like methane and ethene. The document emphasizes the importance of hybridization in understanding chemical bonding and molecular structure.

1. Hybridization
Class XI
A.K.Gupta, PGT Chemistry
KVS ZIET Bhubaneswar

2. What is hybridization?
Hybridisation (or hybridization) is the
concept of mixing atomic orbitals into
new hybrid orbitals (with different
energies, shapes, etc., than the
component atomic orbitals) suitable for
the pairing of electrons to form chemical
bonds in valence bond theory.
A.K.Gupta, PGT Chemistry, KVS ZIET BBSR

3. Types of hybridisation
sp3
C
↑↓ ↑↓ ↑ ↑
1s 2s 2p 2p 2p
C*
↑↓ ↑ ↑ ↑ ↑
1s 2s 2p 2p 2p
C*
↑↓ ↑ ↑ ↑ ↑
1s sp3 sp3 sp3 sp3
C atom ground state
C atom excited state
C atom sp3 hybridized
A.K.Gupta, PGT Chemistry, KVS
ZIET BBSR

4. sp3 Hybridization
A.K.Gupta, PGT Chemistry, KVS
ZIET BBSR

5. sp3 Hybridization
A.K.Gupta, PGT Chemistry, KVS
ZIET BBSR

6. Bonding in Methane (CH4)
A.K.Gupta, PGT Chemistry, KVS
ZIET BBSR

7. Summary
 sp3 hybridization occurs when a C has 4
attached groups
sp3 hybrid orbital has 25% s and 75% p
character
the 4 sp3 hybrids point towards the corners
of a tetrahedron at 109.28o to each other
each sp3 hybrid orbital is involved in σ bond
foprmation.
A.K.Gupta, PGT Chemistry, KVS
ZIET BBSR

8. Formation of Sigma Bond
A.K.Gupta, PGT Chemistry, KVS
ZIET BBSR

9. hybrid orbitals – sp, sp2, or sp3
A.K.Gupta, PGT Chemistry, KVS
ZIET BBSR

10. A.K.Gupta, PGT Chemistry, KVS
ZIET BBSR

11. A.K.Gupta, PGT Chemistry, KVS
ZIET BBSR

12. Formation of s bond
A.K.Gupta, PGT Chemistry, KVS
ZIET BBSR

13. sp2 Hybridization
A.K.Gupta, PGT Chemistry, KVS ZIET BBSR

14. A.K.Gupta, PGT Chemistry, KVS ZIET BBSR

15. Formation of  bond
A.K.Gupta, PGT Chemistry, KVS
ZIET BBSR

16. Remaining p orbitals from sp or sp2
s bond
A.K.Gupta, PGT Chemistry, KVS
ZIET BBSR

17. A.K.Gupta, PGT Chemistry, KVS
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18. A.K.Gupta, PGT Chemistry, KVS ZIET BBSR

19. Formation of  bond
Planar molecule (each carbon is trigonal planar)
with  cloud above and below the plane
 bond hinders free rotation about the carbon-to-
carbon bond
A.K.Gupta, PGT Chemistry, KVS ZIET BBSR

20.  sp2 hybridization occurs when a C has 3
attached groups
sp2 hybrid orbital has 33% s and 67% p
character
the 3 sp2 hybrids point towards the corners of a
triangle at 120o to each other
each sp2 hybrid orbital is involved in a σ bond
formation and the remaining p orbital forms the
 bond
a double bond as a σ+  bond
Summary
A.K.Gupta, PGT Chemistry, KVS ZIET BBSR

21. Bonding in Ethene (H2C=CH2)
A.K.Gupta, PGT Chemistry, KVS ZIET BBSR

22. sp Hybridization
A.K.Gupta, PGT Chemistry, KVS
ZIET BBSR
Pure p
orbital
Sp hybrid
orbital

23. Bonding in Acetylene
A.K.Gupta, PGT Chemistry, KVS ZIET BBSR

24. sp Hybridization
A.K.Gupta, PGT Chemistry, KVS
ZIET BBSR

25. Bonding in Acetylene
A.K.Gupta, PGT Chemistry, KVS
ZIET BBSR

26. Summary
 Sp hybridization occurs when a C has 2
attached groups
sp hybrid orbital has 50% s and 50% p
character
the 2 sp hybrids are oriented at an angle of
180o to each other
each sp hybrid orbital is involved in a σ bond
formation and the remaining two p orbital
forms two  bonds
a triple bond = one σ + two  bonds
A.K.Gupta, PGT Chemistry, KVS
ZIET BBSR

27. Bond formation from
hybridization
• Single bond
- sigma bond
• Double bond
– sigma bond + pi bond
• Triple bond
– sigma bond + pi bond + pi bond
How are the two pi bonds in the triple bond oriented?
end-to-end
side-to-side
A.K.Gupta, PGT Chemistry, KVS
ZIET BBSR

28. 1
2
3
4
5
6
7
What is the hybridization in each carbon atom?
sp3 – 2, 5
tetrahedral
sp2 – 1, 3, 4
trigonal planar
sp – 6, 7
linear
= Oxygen atom
= Carbon atom
= Hydrogen atom

29. What is the hybridization in each carbon atom?
1
2
3
4
A.K.Gupta, PGT Chemistry, KVS ZIET BBSR

30. Draw the Lewis dot structure –
C3H4
Remember to chain the carbon atoms and fill
the octet of the center carbon atom in the
chain first.
You should have come up with one of these structures:
H:C:C:::C:H
H
H
..
..
C::C::C
H
H
..
..
H
H
..
..
A.K.Gupta, PGT Chemistry, KVS
ZIET BBSR

31. Thanks