Final answer:
The identification of hybrid orbitals involves using VSEPR theory to predict electron-pair geometry, mixing the necessary atomic orbitals to form equivalent hybrid orbitals, and utilizing these hybrid orbitals to create sigma bonds, with remaining orbitals possibly forming pi bonds.
Step-by-step explanation:
The step-by-step process of identifying hybrid orbitals involves the following steps:
- Determine the electron-pair geometry of the molecule using the Valence Shell Electron Pair Repulsion (VSEPR) theory.
- Based on the electron-pair geometry, decide how many atomic orbitals must mix to form the required set of hybrid orbitals.
- Mix the relevant atomic orbitals (s and p, or s, p, and d) to create a new set of equivalent hybrid orbitals that correspond in number to the domains of electron density.
- Assign the electrons from the atom to the hybrid orbitals, starting with the lowest energy orbitals.
- Use the hybrid orbitals to form sigma (σ) bonds with adjacent atoms, while any unhybridized orbitals may form pi (π) bonds.
For instance, in sp hybridization (like in BeCl₂), one s orbital and one p orbital from beryllium mix to form two sp hybrid orbitals arranged 180° apart, conducive to a linear molecular geometry. Similarly, sp² hybridization involves mixing one s and two p orbitals to form three equivalent sp² hybrids at 120° to each other, indicative of trigonal planar geometry. The sp³ hybridization involves one s and three p orbitals to yield four sp³ hybrids, suitable for tetrahedral geometry.