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Chapter 9: Problem 46

Is it possible to "trap" a resonance structure of a compound for study? Explain.

Short Answer

Expert verified
No, it is not possible to 'trap' a resonance structure of a compound for study. This is because resonance structures are a theoretical representation and do not physically exist. The compound exists as a hybrid of all possible resonance structures simultaneously.

Step by step solution

01

Understanding Resonance Structures

Resonance structures are ways of drawing Lewis structures to represent the electron configuration in a molecule. These structures are a theoretical construct, and molecules do not switch between them. Instead, the actual structure of the molecule is a resonance hybrid of these resonance forms.
02

Delocalized Electrons and Resonance Hybrids

In a molecule, the location of certain electrons (shared electrons between atoms) is not fixed. We call these electrons 'delocalized'. They are not associated with a single pair of atoms but move within the whole molecule. This behavior makes the concept of resonance structures necessary. The molecule does not oscillate between the resonance forms. Instead, it exists as a resonance hybrid of these forms.
03

The Theoretical Nature of Resonance Structures

This concept is theoretical and helps us understand the nature of molecular structures better. Since resonance is a theoretical concept, we can't 'trap' one resonance structure because the molecule exists as a weighted average or hybrid of all potential resonance forms.

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Most popular questions from this chapter

What is a polar covalent bond? Name two compounds that contain one or more polar covalent bonds.

What is lattice energy and what role does it play in the stability of ionic compounds?

Summarize the essential features of the Lewis octet rule. The octet rule applies mainly to the second period elements. Explain.

Classify these bonds as ionic, polar covalent, or covalent, and give your reasons: (a) the SiSi bond in \(\mathrm{Cl}_{3} \mathrm{SiSiCl}_{3},\) (b) the \(\mathrm{SiCl}\) bond in \(\mathrm{Cl}_{3} \mathrm{SiSiCl}_{3},\) (c) the CaF bond in \(\mathrm{CaF}_{2},\) (d) the \(\mathrm{NH}\) bond in \(\mathrm{NH}_{3}\).

Give three examples of compounds that do not satisfy the octet rule. Write a Lewis structure for each.
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