A molecule with formula C4H3NO has the connectivity shown in the figure. After the Lewis structure of the molecule is completed, how many of each of the following are there in the molecule:
a. single bonds,
b. double bonds,
c. triple bonds,
d. nonbonding pairs? [Sections 8.3 and 8.5]

Key Concepts

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 help visualize how atoms are connected and the distribution of electrons, which is crucial for determining the number of single, double, and triple bonds, as well as nonbonding pairs.

Types of Chemical Bonds

Chemical bonds can be classified into single, double, and triple bonds based on the number of shared electron pairs between atoms. A single bond involves one pair of shared electrons, a double bond involves two pairs, and a triple bond involves three pairs. Understanding these types is essential for analyzing the connectivity in a molecule.

Nonbonding Electron Pairs

Nonbonding electron pairs, also known as lone pairs, are pairs of valence electrons that are not involved in bonding. They play a significant role in determining the geometry and reactivity of a molecule. Identifying these pairs is important for accurately completing the Lewis structure and understanding the overall electron distribution.