Make a sketch showing the location and geometry of the p orbitals in the nitrite ion, NO2-. Describe the bonding in this ion using a localized valence bond model for s bonding and a delocalized MO model for p bonding.

Key Concepts

p Orbitals and Their Geometry

P orbitals are dumbbell-shaped regions of space where the probability of finding an electron is high. In the context of the nitrite ion (NO2-), there are three p orbitals oriented at right angles to each other, with two of them involved in bonding. The geometry of these orbitals is crucial for understanding how they overlap with s orbitals to form bonds.

Localized Valence Bond Theory

Localized valence bond theory describes how atoms in a molecule form bonds by sharing pairs of electrons in overlapping atomic orbitals. In the nitrite ion, the s bonding involves the overlap of the nitrogen's s orbital with the oxygen's p orbitals, resulting in sigma bonds. This model emphasizes the localized nature of electron pairs in specific bonds.

Delocalized Molecular Orbital Theory

Delocalized molecular orbital (MO) theory explains how electrons are not confined to individual bonds but are spread over several atoms in a molecule. In the nitrite ion, the p electrons are delocalized across the nitrogen and oxygen atoms, leading to resonance structures that contribute to the overall bonding character. This model provides a more comprehensive view of the bonding in polyatomic ions.