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Chapter 6: Problem 24

Why are resonance structures used to model certain molecules?

Short Answer

Expert verified
Resonance structures are used to model molecules in cases where a single Lewis structure cannot fully represent the electron configuration of a molecule. The true structure of the molecule, the resonance hybrid, is a blend of all valid resonance structures and provides a more accurate depiction of the molecule's electronic state.

Step by step solution

01

Definition of Resonance Structures

Resonance structures are multiple Lewis structures that represent the same molecule or ion. They are drawn to depict the delocalization of electrons in certain molecules.
02

Necessity of Resonance Structures

Some molecules cannot be adequately represented by a single Lewis structure. The 'real' structure of the molecule is a hybrid of the possible resonance structures. This hybrid, called the resonance hybrid, represents an average of the resonance forms, and provides a more accurate depiction of electron distribution.
03

Example of Resonance Structures

A classic example of resonance can be found in the carbonate ion (CO3 2-). Its resonance hybrid is far more accurately depicted by three equivalent resonance structures rather than a single one.

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Most popular questions from this chapter

What determines the electron distribution between two atoms in a bond?

Why do electron pairs around a central atom stay as far apart as possible?

Draw Lewis structures for the following polyatomic ions. a. \(\mathrm{CO}_{3}^{2-}\) b. \(\mathrm{O}_{2}^{2-}\) c. \(\mathrm{PO}_{4}^{3-}\)

Predict whether the bonds between the following pairs of elements are ionic, polar covalent, or nonpolar covalent. a. \(\mathrm{Na}-\mathrm{F}\) b. \(\mathrm{H}-\mathrm{I}\) c. \(\mathrm{N}-\mathrm{O}\) d. \(\mathrm{Al}-\mathrm{O}\) e. \(\mathrm{S}-\mathrm{O}\) f. \(\mathrm{H}-\mathrm{H}\)

What type of bond results if two atoms share six electrons?
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