Hybrid Orbitals Formation

Hybridization Concepts

• Four atomic electron orbitals (one s and three p orbitals) combine to create the sp3 hybrid orbital.
• The sp3 hybrid orbital is composed of 25% s orbital energy and 75% p orbital energy.
• Four sp3 orbitals are formed to minimize electron pair repulsion, creating a more stable arrangement compared to individual orbitals.
• The distinctive shape resulting from the combination of s and p orbital energies is tetrahedral.

Effects of Hybridization

• The distribution of s orbital energy influences the shape and orientation of the lobes in the resulting hybrid orbital, affecting bond angles around the atom.
• Sigma bonds are stronger and shorter compared to pi bonds.
• In ethylene (H2C=CH2), one pi bond is formed from the sideways overlap of unhybridized p orbitals.

Types of Hybridization

• In sp3 hybridization, the hybrid orbitals formed are designated as sp3 orbitals.
• Molecules like ethylene (C2H4) exhibit sp2 hybridization.
• A triple bond, such as in acetylene (C2H2), comprises two pi bonds and one sigma bond.
• A hybrid orbital formed by combining s and d orbitals typically exhibits a trigonal bipyramidal shape.

Hybridization in Specific Molecules

• In ethane (C2H6), the carbon atoms are sp3 hybridized.
• The hybridization of an atom in a molecule is determined by its electron geometry and the number of bonding and lone pairs around it.
• When a carbon atom forms a double bond, one of the sp2 hybrid orbitals is used to form the sigma bond, while the remaining p orbitals contribute to the pi bond.

Geometrical Arrangement

• sp3 hybrid orbitals form a tetrahedral arrangement in molecules, resulting in a bond angle of approximately 109.5 degrees.