1. Structure and Bonding in Organic Chemistry
Hybridization
Van der waals INTERACTIONS
Hydrogen bonding
SUBMITTED BY
SUKHMEET KAUR

2. Hybridization
The intermixing of orbitals and having slightly energies and the redistribution of their energies to form a new orbitals having identical shapes and equivalent energies is known as hybridization.
New orbital thus formed are called hybrid orbitals.

3. Features of Hybridization
Only those orbitals which have approximately equal energies and belong to the same atom undergo hybridization.
Number of hybrid orbitals produced is equal to the number of atomic orbitals which undergo hybridization.
The hybridization orbitals have equivalent energies and identical shapes.

4. Types of Hybridization
Tetrahedral or sp3-hybridization.
Trigonal or sp2-hybridization.
Diagonal or sp-hybridization.

5. sp3 Orbital Hybridization
Promote an electron from the 2s to the 2p orbital 2s

6. sp3 Orbital Hybridization

7. sp3 Orbital Hybridization
Mix together (hybridize) the 2s orbital and the three 2p orbitals 2s 2p

8. Tetrahedral Geometry

9. sp3 Hybridization 4 Regions of electron Density

10. Hybridization of 1 s and 3 p Orbitals – sp3

11. Each of the four hybrid orbitals has one-fourth s-character and three-fourth p-character.
This type of orbitals are formed when carbon atoms form only single bonds with other atoms.
One of the lobes of an sp3 orbital is larger than other, it can overlap better with another when it forms a bond therefore sp3 hybrid orbitals forms stronger bonds then formed by unhybridised s or p orbitals.

12. Structure of Methane
tetrahedral bond angles = 109.5° bond distances = 110 pm

13. sp3 is Tetrahedral Geometry Methane

15. Orbital Depiction of Ethane, C2H6 the s bond

16. sp2 Orbital Hybridization
Promote an electron from the 2s to the 2p orbital 2s

17. sp2 Orbital Hybridization
2p 2p
2s 2s

18. sp2 Orbital Hybridization
Mix together (hybridize) the 2s
orbital and two of the three 2p orbitals 2p 2s

19. sp2 Orbital Hybridization
3 equivalent half-filled sp2 hybrid orbitals plus 1 p orbital left unhybridized 2p
2 sp2 2s

20. sp2 Orbital Hybridization
2 of the 3 sp2 orbitals are involved in s bond to hydrogen's; the other is involved in a s bond in a
s bond to carbon p
2 sp2

21. The sp2 hybrid orbitals has one-third s-character and two-third p-character.
This type of orbitals are formed when carbon atoms form only double bonds with other atoms.

23. Orbital Depiction of Ethane, C2H6 the s bond

24. sp2 Hybridization 3 Regions of Electron Density

25. Hybridization of 1 s and 2 p Orbitals – sp2

26. An sp2 Hybridized Atom

27. The p bond Overlap of 2 parallel p Orbitals

28. Ethylene CH2=CH2

29. Views of Ethylene, C2H4

30. sp Orbital Hybridization
Promote an electron from the 2s to the 2p orbital 2s

31. sp Orbital Hybridization
2s s 2p 2p

32. sp Orbital Hybridization
Mix together (hybridize) the 2s orbital and one of the three 2p orbitals 2s

33. sp Orbital Hybridization

34. sp Hybridization 2 Regions of Electron Density

35. The sp Orbital

36. The sp hybrid orbitals has one-half s-character and one- half p-character.
This type of orbitals are formed when carbon atoms form only triple bonds with other atoms.

37. Acetylene, C2H2, 1 s bond 2 perpendicular p bonds

38. Intermolecular forces
1. Van der Waal’s forces
(attraction between partial + charge on one molecule & partial - charge on another molecule)
>

39. Factors influencing vander waals forces
Number of electrons in the molecule
Size of the molecule
Molecular shape
CH3-CH2-CH2-CH2-CH3
n-pentane
Larger surface area; greater magnitude of Vander Waals forces.

40. CH3 |
CH3-C-CH3
neo-pentane
Lesser surface area; lesser magnitude of vander waals forces.
Temperature and pressure