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Chapter 17: Problem 2

Why is a resonance hybrid representation of \(\mathrm{NO}_{3}^{-}\) better than just a single structure?

Short Answer

Expert verified
A resonance hybrid representation of \(\mathrm{NO}_{3}^{-}\) is better than a single structure because it accurately depicts the reality that all three nitrogen-oxygen bonds are equivalent. Each bond is neither a single nor a double bond, but rather an average of the two. This understanding is fundamental to the concept of resonance in chemistry.

Step by step solution

01

Understanding Resonance

Resonance in chemistry refers to a situation where a molecule or an ion could be represented by multiple equivalent Lewis structures. The actual structure is an average of all possible structures and is referred to as a resonance hybrid.
02

Lewis Structures of \(\mathrm{NO}_{3}^{-}\)

The nitrogen (N) atom in Nitrate (\(\mathrm{NO}_{3}^{-}\)) can form three bonds, one with each of the three oxygen (O) atoms. Each oxygen atom also has one lone pair of electrons. A single Lewis structure would depict one of the oxygen atoms as double bonded to the Nitrogen, and the others as single bonded. This, however, is misleading because it inaccurately suggests that one of the bonds is stronger than the others.
03

Resonance Hybrid Representation of \(\mathrm{NO}_{3}^{-}\)

A resonance hybrid combines all the possible resonant structures of a molecule or ion. In the case of Nitrate (\(\mathrm{NO}_{3}^{-}\)), there are three possible structures. Each shows a double bond with one of the oxygen atoms and single bonds with the rest. By averaging these structures, each N-O bond is portrayed as one-and-one-third bonds 鈥� neither single nor double but in-between. This depiction is more accurate as it correctly portrays all N-O bonds as equivalent.

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Most popular questions from this chapter

How was the \(\mathrm{N}-\mathrm{O}\) bond order of \(4 / 3\) calculated for \(\mathrm{NO}_{3}^{-}\) ?

Why can \(\mathrm{C}, \mathrm{N}, \mathrm{O}\) and \(\mathrm{F}\) accommodate only eight electrons (sum of the bonding and lone-pair electrons)?

Why can atoms in the third (or greater) period accommodate more than eight electrons (sum of the bonding and nonbonding electrons)?
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