At high temperatures, sulfur vapor is predominantly in the form of S₂(g) molecules. (a) Assuming that the molecular orbitals for third-row diatomic molecules are analogous to those for second-row molecules, construct an MO diagram for the valence orbitals of S₂(g).

Key Concepts

Molecular Orbital Theory

Molecular Orbital (MO) Theory describes the behavior of electrons in molecules by combining atomic orbitals to form molecular orbitals. These orbitals can be bonding, antibonding, or non-bonding, and they help predict the stability, magnetic properties, and electronic configurations of molecules. Understanding MO theory is essential for constructing MO diagrams, which visually represent the energy levels and occupancy of these orbitals.

Valence Orbitals

Valence orbitals are the outermost orbitals of an atom that are involved in chemical bonding. In diatomic molecules like S2, the valence orbitals of each sulfur atom combine to form molecular orbitals. For sulfur, the relevant valence orbitals include the 3s and 3p orbitals, which will interact to form the molecular orbitals that dictate the electronic structure of the S2 molecule.

Diatomic Molecules and Their Orbitals

Diatomic molecules consist of two atoms bonded together, and their molecular orbitals are formed from the combination of the atomic orbitals of the constituent atoms. For sulfur (S2), the molecular orbitals are constructed by considering the symmetry and energy levels of the 3s and 3p orbitals. The arrangement of these orbitals in an MO diagram helps in understanding the bond order, stability, and reactivity of the molecule.