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Chapter 6: Problem 8

What are resonance structures? What is a resonance hybrid?

Short Answer

Expert verified
Resonance structures are different valid Lewis structures for the same molecule showing electron delocalization and do not change atom positions. A resonance hybrid is the actual electron distribution representation, averaging all resonance structures.

Step by step solution

01

Definition of Resonance Structures

Resonance structures are different Lewis structures for the same molecule that have the same arrangement of atoms but a different arrangement of electrons. They are used to represent the delocalization of electrons within molecules, where the electron distribution cannot be represented by a single Lewis structure alone.
02

Illustration of Resonance Structures

To illustrate resonance structures, draw all possible structures where double bonds, lone pairs, and charges can move around the molecule without altering the positions of the atoms. The real structure is a blend of these resonance structures.
03

Explanation of Resonance Hybrid

A resonance hybrid is the actual structure of the molecule, which is an average of all the resonance structures. It more accurately represents the electron distribution within a molecule and often involves partial bonds and charges rather than full ones represented in each individual resonance structure.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Understanding Lewis Structures
To comprehend the foundation of many chemistry concepts, we must start with the basics of Lewis structures. Lewis structures, named after the chemist Gilbert N. Lewis, are diagrams that show the distribution of valence electrons among the atoms in a molecule. Here's what you need to know to draw a Lewis structure:

  • Identify the total number of valence electrons in the molecule.
  • Arrange the atoms with the least electronegative atom in the center (except for hydrogen).
  • Draw single bonds between atoms to form a skeletal structure.
  • Distribute the remaining electrons to satisfy the octet rule (duet for hydrogen).
  • Double or triple bonds may be necessary if single bonds do not suffice to balance the remaining electrons.

It's essential to practice Lewis structures as they serve as the starting point in understanding more complex concepts like resonance structures in chemistry. Remember that the aim is to represent all valence electrons and fulfill the octet rule for each atom, where applicable.
Delving into Electron Delocalization
Electron delocalization is a key concept that emerges from understanding Lewis structures. In certain molecules, electrons are not confined to a single bond or atom, but instead, they are spread across multiple atoms. This phenomenon leads to structures that have more stability than what would be predicted if the electrons were localized.

  • Electron delocalization typically occurs in conjugated systems where p-orbitals overlap, creating a delocalized pi system through which electrons can move.
  • This can lead to molecules having more than one valid Lewis structure, known as resonance structures.
  • Delocalization is associated with lower energy and increased stability of the molecule.

By recognizing where electron delocalization is likely to occur, you not only predict the possible resonance structures but also gain insights into the molecule's reactivity and properties.
Resonance Hybrid: The Real Molecular Structure
A resonance hybrid is the actual representation of a molecule's structure, considering all possible arrangements of its electrons as shown by its resonance structures. Here's the crux:

  • The resonance hybrid uses partial bonds or charges to reflect the electron delocalization across the molecule.
  • Resonance hybrids do not 'switch' between forms; rather, the actual state of the molecule is an average of its resonance forms.
  • Representing a molecule as a resonance hybrid helps chemists understand and predict the strengths of bonds and the stability of the molecule.

It's important to emphasize that a resonance hybrid is not something that oscillates between forms. Instead, it is a more accurate depiction of molecular structure, which allows for a better understanding of molecular behavior.

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Most popular questions from this chapter

Which statement best captures the fundamental idea behind VSEPR theory? Explain what is wrong with the statements you do not choose. \begin{equation}\begin{array}{l}{\text { a. The angle between two or more bonds is determined primarily by }} \\ {\text { the repulsions between the electrons within those bonds and other }} \\ {\text { (lone pair) electrons on the central atom of a molecule. Each of these electron groups }} \\ {\text { (bonding electrons or lone pair electrons)lowers its potential energy by maximizing }} \\ {\text { its separation from other electron groups, thus determining the geometry of the molecule. }} \\ {\text { b. The angle between two or more bonds is determined primarily by the repulsions between }} \\\ {\text { the electrons within those bonds. Each of these bonding electrons lowers its potential energy }} \\ {\text { by maximizing its separation from other electron groups, thus determining the geometry }} \\ {\text { of the molecule }} \\ {\text { c. The geometry of a molecule is determined by the shapes of the overlapping orbitals }} \\ {\text { that form the chemical bonds. Therefore, to determine the geometry of a molecule, }} \\ {\text { you must determine the shapes of the orbitals involved in bonding.}}\end{array}\end{equation}

Write a Lewis structure that obeys the octet rule for each molecule or ion. Include resonance structures if necessary and assign formal charges to each atom. \begin{equation} \mathrm { a. } {SeO}_{2} \quad \text { b. } \mathrm{CO}_{3}^{2-} \quad \text { c. } \mathrm{ClO}^{-} \quad \text { d. } \mathrm{NO}_{2}^{-} \end{equation}

A molecule with the formula AB3 has a trigonal planar geometry. How many electron groups are on the central atom?

Name and draw the five basic electron geometries, and state the number of electron groups corresponding to each. What constitutes an electron group?

Write the Lewis structure for each molecule. a. \(\mathrm{NF}_{3} \quad\) b. HBr \(\quad\) c. \(\mathrm{SBr}_{2} \quad\) d. \(\mathrm{CCl}_{4}\)
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