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Ch.9 - Molecular Geometry and Bonding Theories
Brown - Chemistry: The Central Science 14th Edition
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Tutti i libri di testoBrown 14th EditionCh.9 - Molecular Geometry and Bonding TheoriesProblema 63
Capitolo 9, Problema 63

(c) Is the p bond in NO2- localized or delocalized?

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Step 1: Understand the concept of localized and delocalized bonds. A localized bond is a bond that is confined between two atoms. A delocalized bond, on the other hand, is a bond in which the electrons are not confined to two adjacent bonding atoms, but actually spread over three or more atoms.
Step 2: Draw the Lewis structure of NO2-. The Lewis structure of NO2- (Nitrite ion) is a resonance structure. It consists of nitrogen (N) bonded to two oxygen (O) atoms. One of the oxygen atoms has a single bond with nitrogen and the other oxygen atom has a double bond with nitrogen. However, these bonds keep switching between the two oxygen atoms, creating a resonance structure.
Step 3: Identify the p bond in the structure. In the Lewis structure of NO2-, the p bond is the second bond in the double bond between the nitrogen and one of the oxygen atoms.
Step 4: Determine whether the p bond is localized or delocalized. Since the double bond in NO2- is part of a resonance structure and can switch between the two oxygen atoms, the p bond is not confined to just two atoms. Therefore, the p bond in NO2- is delocalized.

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Bonding in Molecules

In molecular chemistry, bonding refers to the interactions that hold atoms together in a molecule. There are two primary types of bonds: localized bonds, where electrons are shared between specific atoms, and delocalized bonds, where electrons are spread over multiple atoms. Understanding these concepts is crucial for analyzing the structure and stability of molecules like NO2-.
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Resonance Structures

Resonance structures are different ways of drawing a molecule that can represent the same arrangement of atoms but differ in the distribution of electrons. In the case of NO2-, resonance indicates that the p bond can be represented as being shared between the nitrogen and both oxygen atoms, suggesting that the bond is delocalized rather than confined to a single pair of atoms.
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Molecular Orbital Theory

Molecular Orbital Theory explains how atomic orbitals combine to form molecular orbitals, which can be occupied by electrons. This theory helps in understanding the nature of bonding in molecules, including whether bonds are localized or delocalized. In NO2-, the presence of degenerate molecular orbitals allows for the delocalization of p electrons, contributing to the overall stability of the ion.
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