Which of the following pairs represent resonance structures? (LO 7.13) (a)(b)(c)

Verified step by step guidance

1. Identify the definition of resonance structures: Resonance structures are different Lewis structures for the same molecule that show the same arrangement of atoms but different arrangements of electrons.
2. Examine each pair of structures to ensure they have the same molecular formula and connectivity of atoms. This means the skeleton of the molecule should remain unchanged.
3. Check if the only differences between the structures are in the placement of electrons, such as lone pairs or pi bonds. The positions of atoms should not change.
4. Verify that the total number of electrons in each structure is the same, ensuring that the structures are valid Lewis structures.
5. Determine if the structures can be interconverted by moving electrons, such as shifting a double bond or moving a lone pair to form a double bond, without breaking any single bonds.

Key Concepts

Resonance Structures

Resonance structures are different Lewis structures for the same molecule that depict the same arrangement of atoms but differ in the distribution of electrons. These structures are used to represent delocalized electrons within certain molecules, where the actual structure is a hybrid of all possible resonance forms. Understanding resonance is crucial for predicting the stability and reactivity of molecules.

Lewis Structures

Lewis structures are diagrams that represent the bonding between atoms in a molecule and the lone pairs of electrons that may exist. They provide a visual representation of the molecule's structure, showing how valence electrons are arranged. Mastery of drawing Lewis structures is essential for identifying resonance structures, as it allows for the visualization of electron distribution.

Delocalization of Electrons

Delocalization of electrons refers to the phenomenon where electrons are not associated with a single atom or bond but are spread over multiple atoms. This occurs in resonance structures, where the electrons can be shared among several bonds, leading to increased stability. Recognizing delocalization is important for understanding the behavior of molecules in chemical reactions and their overall stability.