Question

Study the following sketch of a molecular orbital (MO) in a homonuclear diatomic molecule. This MO was formed by combining one 3 s atomic orbital from each atom. The dark dots in this sketch are the nuclei. Now use the sketch to complete the table below.

Answer 1

The question relates to the creation of molecular orbital energy diagrams for homonuclear diatomic molecules using Molecular Orbital Theory, involving the combination of atomic orbitals to form bonding and antibonding molecular orbitals.

Step-by-step explanation:

The question covers the topic of Molecular Orbital (MO) Theory, particularly focusing on molecular orbital energy diagrams for homonuclear diatomic molecules. The student is asked to complete a table based on a provided sketch of a MO formed by combining two 3s atomic orbitals. A molecular orbital diagram is a visual representation of the relative energy levels of the atomic and molecular orbitals, showing how atomic orbitals combine to form bonding (lower energy) and antibonding (higher energy) molecular orbitals. According to MO Theory, the number of molecular orbitals formed equals the number of atomic orbitals interacting. We populate these molecular orbitals with electrons following the Pauli exclusion principle and Hund's rule, filling the orbitals in order of increasing energy.

Answer 2

Based on the molecular orbital (MO) sketch formed by combining one 3s atomic orbital from each atom in a homonuclear diatomic molecule, the bonding MO is occupied by two electrons, while the antibonding MO is unoccupied.

Step-by-step explanation:

In the provided MO sketch, the bonding MO is represented by the region between the nuclei where the electron density is concentrated, indicated by the absence of nodes. According to the Pauli exclusion principle, each orbital can accommodate a maximum of two electrons with opposite spins. Therefore, the bonding MO is occupied by two electrons. On the other hand, the antibonding MO has a node between the nuclei, resulting in reduced electron density in that region. Since the sketch indicates no electrons in the antibonding MO, it remains unoccupied.

Understanding the electronic configuration of molecular orbitals is crucial for predicting the stability and properties of diatomic molecules. In this case, the occupation of the bonding MO by two electrons signifies the formation of a stable bond between the two atoms, contributing to the molecule's overall stability. The absence of electrons in the antibonding MO further supports the stability, as an occupied antibonding MO would lead to a less stable molecular configuration.

In conclusion, the MO sketch provides insights into the electronic structure of a homonuclear diatomic molecule. The occupation of the bonding and antibonding MOs determines the stability of the molecule, with a fully occupied bonding MO contributing to stability, while an occupied antibonding MO would indicate reduced stability. This understanding is fundamental in the study of molecular properties and behavior.

Question

How does the occupation of the bonding and antibonding molecular orbitals influence the stability and properties of homonuclear diatomic molecules, and what implications does this have for the overall behavior of such molecules in chemical reactions and interactions?