Show how a hydrogen 1s atomic orbital and a fluorine 2p...

Show how a hydrogen 1$s$ atomic orbital and a fluorine 2$p$ atomic orbital overlap to form bonding and antibonding molecular orbitals in the hydrogen fluoride molecule. Are these molecular orbitals $\sigma$ or $\pi$ molecular orbitals?

Key Concepts

Atomic Orbitals

Atomic orbitals are regions in an atom where electrons are most likely to be found. They are characterized by specific shapes (such as spherical or dumbbell-shaped) and energy levels, determined by quantum mechanics. These orbitals serve as the fundamental building blocks for describing electron distributions in isolated atoms.

Molecular Orbital Theory

Molecular orbital theory explains how atomic orbitals combine to form molecular orbitals that are spread over the entire molecule. It utilizes the linear combination of atomic orbitals (LCAO) approach to predict the electron distribution, energies, and bonding characteristics within a molecule.

Orbital Overlap

Orbital overlap refers to the region where two atomic orbitals from different atoms merge to form a molecular orbital. The extent and type of overlap, which depend on the orientation and symmetry of the participating atomic orbitals, are crucial in determining whether the resulting molecular orbital has bonding or antibonding character.

Bonding and Antibonding Orbitals

Bonding orbitals are formed by the constructive interference of overlapping atomic orbitals, which results in an increased electron density between the nuclei and a stabilizing effect on the molecule. Antibonding orbitals, on the other hand, arise from destructive interference, leading to a node between the nuclei and a higher energy, destabilizing effect.

Sigma (?) and Pi (?) Molecular Orbitals

Sigma (?) molecular orbitals are generated by head-on overlapping of atomic orbitals along the internuclear axis, resulting in a cylindrical distribution of electron density that is symmetric around the bond axis. In contrast, pi (?) molecular orbitals are formed by the side-to-side overlap of atomic orbitals, which creates electron density above and below the plane of the nuclei. The type of orbital formed depends on the orientation of the participating atomic orbitals relative to the internuclear axis.

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