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Valence Bond Theory and Hybridization
In valence bond theory, bonds result from the pairing of unpaired electrons from the valence shell atomic orbitals
σ bond
: cylindrically symmetric about the bond axis; no nodal plane along the bond axis
𝜋 bond
: electron density in 2 lobes with a single nodal plane along the bond axis
Single bond
: 𝜋 bond
Double bond
: σ bond + 𝜋 bond
Molecules can’t rotate around a double bond
Triple bond
: σ bond + 𝜋 bond + 𝜋 bond
Electron Promotion and Hybridization of Atomic Structures
Electron promotion
serves to increase the number of unpaired electrons
If you have an empty orbital you can promote one of your electrons to that orbital
The hybrid orbitals only differ in their orientation in space
Energy for the initial electron promotion comes from bonding
(# of bonded atoms) + (# of lone pairs) = # of hybrid orbitals
2 hybrid orbitals
= sp
3 hybrid orbitals
= sp²
4 hybrid orbitals
= sp³
Exception: single-bonded terminal atoms
Don’t hybridize single-bonded terminal atoms
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