SCH 102
Dr. Solomon Derese 136
sp2
sp2
d
sp2sp2
pzpz
p
p
Hybridization
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Hybridization of Carbon: A Detailed Explanation with Examples, Lecture notes of Chemistry
Hybridization is the combination of two or more atomic orbitals to form the same number of hybrid orbitals, each having the same shape and energy.
Typology: Lecture notes
2021/2022
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sp 2 sp 2 d sp 2 sp 2 p z p z p p
Hybridization
Hybridization of Carbon
A typical C-H has a bond strength of 100 Kcal/mol Net-Energy change = (400-97) Kcal/mol = 300 Kcal/mol In the excited state carbon has four unpaired electrons and can form four bonds with hydrogen.
Methane - sp
3
Hybridized
What is the nature of the four C-H bonds in methane? Since excited carbon uses two kinds of orbitals ( 2 s and 2 p) for bonding purpose, we might expect methane to have two kinds of C-H bonds. In fact this is not the case. A large amount of evidence show that all four C-H bonds in methane are identical in terms of their length and strength.
Each bond in CH 4 is formed by overlap of an sp 3 hybrid orbital of carbon with a 1 s orbital of hydrogen. These four bonds point to the corners of a tetrahedron. **H H H H C . . . .
109 0 A 0 Bond strength = 104 Kcal/mol**
The tetrahedral shape of an sp 3 hybridized carbon
Ethane (C 2
H
6 ) – sp 3 Hybridization C C H H H H H H We can picture the ethane molecule by assuming that the two carbon atoms bond to each other by sigma overlap of an sp 3 hybrid orbital from each carbon.
**C C H H H H H H 109 0 109 0
0 A 0 A Structure of Ethane**
Ethylene (C
2
H
4
)-sp
2
Hybridization
H
H H
H
sp
2
hybridization of a carbon
ground state excited state sp 2 hybridized state 2p z sp 2 2s 2p 2s 2p unhybridized p orbital
sp 2 sp 2 d sp 2 sp 2 p z pz p p d Bond are formed by end-on overlap of two sp 2 hybrid orbitals. p bond are formed by side-by-side overlap of two 2 p orbitals. The electron density in a p bond is farther from the two nuclei, p bonds are usually weaker and therefore more easily broken than d bonds.
Planar shape
trans = The substituents are on opposite side of the double bond. cis = The substituents are on the same side of the double bond.
Examples C C H Cl Cl H C C Cl Cl H H cis - 1,2-dichloroethene trans - 1,2-dichloroethene