Hybridization
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Transcript Hybridization
Hybridization
A Blending of Orbitals
Methane
CH4
Sometimes called “natural gas, ” methane is
used to heat homes.
Shape of Methane
Tetrahedral geometry
109.5o angle between bonds
Carbon’s atomic orbitals
4 valence electrons
Outermost orbitals: 2s, 2px, 2py, 2pz
How can this happen?
2 possibilities
Maybe our quantum mechanical model
of atomic orbitals is totally wrong.
OR
Maybe carbon is doing something else
with its orbitals to form this compound.
Hybridization occurs
A mathematical blending of orbitals
Number of atomic orbitals blended =
number of hybrid orbitals produced
Result: Identical orbitals
– New shape
– New orientation in space
sp3 hybridization
s + px + Py + pz = 4 sp3 orbitals
Sp3 hybridization on carbon
4 identical sp3
orbitals
109.5o between
orbitals
Tetrahedral
orientation
Bonds form when orbitals overlap
Sigma bonds: end to end overlap of
orbitals
What happens in ethene?
C2H4
Properties
Double bond
between carbons
Trigonal planar
geometry around C
120o bond angles
Sp2 hybridization occurs
S + px + py = 3 sp2 orbitals
1 unused p orbital left over
Bonding in ethene
Sigma bond: end to
end overlap
Pi bond: side to
side overlap
Putting ethene together
Carbon-carbon double bond = 1 sigma
bond and 1 Pi bond
4 C-H sigma bonds
Trigonal planar
geometry results
What happens in ethyne?
C2H2
Linear geometry
What type of hybridization is involved?
What hybrid and atomic orbitals can it
use?
What types and numbers of bonds are
present in the molecule?