The document discusses hybridization in methane and ethylene. It explains that carbon atoms in methane are sp3 hybridized, forming 4 identical hybrid orbitals that overlap to make single sigma bonds. Carbon atoms in ethylene are sp2 hybridized, where the first bond is a sigma bond from overlap of the sp2 hybrid orbitals. The second bond is a pi bond formed from side-to-side overlap of the unhybridized p orbital. A double bond consists of one sigma bond and one pi bond. Triple bonds contain one sigma bond and two pi bonds, using the two unhybridized p orbitals.

1. Hybridization

2. Sp 3 Hybridization in methane
When you make sp3 hybrid orbitals all 4 atomic orbitals
become hybridized to yield 4 identical hybrid orbitals.
H1s
H1s
H1s
H1s

3. Formation of a single bond (sigma bond)
Each C in ethylene is sp2 hybridized
The first bond forms from the head on
overlap of the sp2 hybrid orbitals

4. Formation of a single bond (sigma bond)
Each C in ethylene is sp2 hybridized
The first bond forms from the head on
overlap of the sp2 hybrid orbitals
Hybrid orbitals that come together in a head
on collision will always form a sigma bond

5. Formation of a single bond (sigma bond)
Each C in ethylene is sp2 hybridized
The first bond forms from the head on
overlap of the sp2 hybrid orbitals
Single bonds are
H1s
called sigma bonds H1s
(σ)
σ bond
H1s H1s
How does the double bond form?

6. Formation of a double bond (pi bond)
The second bond is formed from the side-
to-side overlap of the unchanged p orbital
σ bond

7. Formation of a double bond (pi bond)
The second bond is formed from the side-
to-side overlap of the unchanged p orbital
σ bond

8. Formation of a double bond (pi bond)
The second bond is formed from the side-
to-side overlap of the unchanged p orbital
σ bond

9. Formation of a double bond (pi bond)
The second bond is formed from the side-
to-side overlap of the unchanged p orbital
σ bond

10. Formation of a double bond (pi bond)
The second bond is formed from the side-
to-side overlap of the unchanged p orbital
σ bond

11. Formation of a double bond (pi bond)
The second bond is formed from the side-
to-side overlap of the unchanged p orbital
Double bonds occur from the combination
of one sigma bond and one pi bond (π)
π bond
σ bond
π bond

12. Sp Hybridization
When you make sp hybrids, two atomic p orbitals
(Pz and Py) remain unchanged
The sp hybrid π
orbitals will form pz
sigma bonds
σ sp sp σ
The p orbitals
are available
for further π π
bonding
Two P orbitals available two pi bonds
triple bond can be formed (1 σ and 2 π)