Hybrid orbitals

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

1. Hybridization occurs to minimize the energy of a molecule and achieve more effective overlapping of atomic orbitals.
2. $sp^3$ hybridization involves one s orbital and three p orbitals combining to form four equivalent $sp^3$ hybrid orbitals, seen in molecules like methane (CH$_4$).
3. $sp^2$ 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$_4$).
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$_2$).
5. The type of hybridization affects molecular shape, bond angles, and bond strength.

Review Questions

• What is the significance of hybridizing atomic orbitals?
• How does $sp^3$ hybridization differ from $sp^2$ and $sp$ hybridizations in terms of geometry?
• Give an example of a molecule that exhibits $sp^2$ hybridization.

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.

Valence Shell Electron Pair Repulsion (VSEPR) Theory: A model used to predict molecular shape based on repulsion between electron pairs around a central atom.