Written by the Fiveable Content Team • Last updated September 2025
Written by the Fiveable Content Team • Last updated September 2025
Definition
Hybrid orbitals are atomic orbitals that combine to form new orbitals, which can explain the geometry of covalent bonding. These hybridized orbitals have different shapes and energies than the original atomic orbitals.
5 Must Know Facts For Your Next Test
Hybridization occurs to minimize the energy of a molecule and achieve more effective overlapping of atomic orbitals.
$sp^3$ hybridization involves one s orbital and three p orbitals combining to form four equivalent $sp^3$ hybrid orbitals, seen in molecules like methane (CH$_4$).
$sp^2$ hybridization involves one s orbital and two p orbitals forming three equivalent $sp^2$ hybrid orbitals, resulting in trigonal planar geometry as seen in ethene (C$_2$H$_4$).
$sp$ hybridization combines one s orbital and one p orbital to form two $sp$ hybrid orbitals, leading to linear geometry found in acetylene (C$_2$H$_2$).
The type of hybridization affects molecular shape, bond angles, and bond strength.
Review Questions
Related terms
Sigma Bond ($\sigma \text{ bond}$): A covalent bond formed by the direct overlap of atomic or hybrid orbitals along the internuclear axis.
Pi Bond ($\pi \text{ bond}$): A type of covalent bond formed by the side-to-side overlap of unhybridized p-orbitals above and below the internuclear axis.