Consider the H2+ ion. (a) Sketch the molecular orbitals of the ion and draw its energy-level diagram.

Key Concepts

Molecular Orbitals

Molecular orbitals (MOs) are formed by the linear combination of atomic orbitals (LCAO) when atoms bond together. In the case of diatomic molecules like H2+, the MOs can be classified as bonding or antibonding. Bonding MOs lower the energy of the system and stabilize the molecule, while antibonding MOs increase energy and destabilize it. Understanding the arrangement and energy levels of these orbitals is crucial for predicting the stability and properties of the ion.

Energy-Level Diagram

An energy-level diagram visually represents the relative energies of molecular orbitals in a molecule or ion. In the case of H2+, the diagram will show the bonding molecular orbital (σ) at a lower energy level and the antibonding molecular orbital (σ*) at a higher energy level. The placement of electrons in these orbitals, according to the Aufbau principle and Hund's rule, helps determine the overall stability and magnetic properties of the ion.

H2+ Ion Characteristics

The H2+ ion is a simple molecular ion consisting of two hydrogen nuclei and one electron. Its unique characteristics arise from the presence of only one electron, which allows for a straightforward analysis of its molecular orbitals. The ion's behavior can be understood through quantum mechanics, particularly in how the single electron occupies the bonding molecular orbital, leading to a net attractive force between the nuclei, thus influencing its stability and energy.