Hybridization
Carbon configuration
Carbon in excited state can form 4 bonds
Hybrid orbital= an orbital created by the combination of
atomic orbitals in the same atom
1 orbital s + 3 orbitals p= sp3
Form 4 hybrid orbitals with a tetrahedral arrangement
Energy changes occurring in
hybridization
Hybridization of an s orbital with all three p
orbitals (px , py, and pz) results in four
sp3 hybrid orbitals. sp3 hybrid orbitals are
oriented at bond angle of 109.5 degrees from
each other. This 109.5 degree arrangement
gives tetrahedral geometry
C in alkanes has a
methane
3
sp
hybridation
ethane
sp3 Hybridization in Methane
Carbon's 2s and all three of its 3p orbitals
hybridize to form four sp3 orbitals. These
orbitals then bond with four hydrogen atoms
through sp3-s orbital overlap, creating
methane. The resulting shape is tetrahedral,
since that minimizes electron repulsion.
sp2 hybridization
Hybridization of an s orbital with two p orbitals
(px and py) results in three sp2 hybrid orbitals
that are oriented at 120o angle to each other.
Sp2 hybridization results in trigonal geometry.
1 orbital s + 2 p =
2
3sp
Form 3 hybrid orbitals with a 120° angle
With orbital p remained this C can arrange a
double bond characteristic of alkenes (ethene)
sp2 Hybridization in Ethene
These hybridized orbitals align themselves in the
trigonal planar structure.
For each carbon, two of these sp orbitals bond
with two 1s hydrogen orbitals through s-sp
orbital overlap.
The atoms that form the double bond cannot move in space unlike the
single one.
The double bond is very reactive and it can produce alkanes or alcohol
by way of the addition reaction
sp Hybridization
In it, the 2s orbital and one of the 2p orbitals
hybridize to form two sp orbitals, each
consisting of 50% s and 50% p character.
The front lobes face away from each other and
form a straight line leaving a 180° angle
between the two orbitals
1 orbital s + 1 p = 2sp
Form 2 hybrid orbitals with a 180° angle
Two orbitals direct perpendicularly remain available.
So the molecule can form a triple bond
The triple bond is characteristic of alkynes like ethine
Sigma bond= covalent bond formed by overlap of atomic orbitals along the bond
axis
Pi bond= a bond formed by the overlap of p orbitals on adjacent atoms,
perpendicular to any sigma bond
sp Hybridization in Ethyne
The first bond consists of sp-sp orbital overlap
between the two carbons. Another two bonds
consist of s-sp orbital overlap between the sp
hybridized orbitals of the carbons and the 1s
orbitals of the hydrogens.