Skip to main content
Ch. 1 - Remembering General Chemistry: Electronic Structure and Bonding (Part 2)
Bruice - Organic Chemistry 8th Edition
Bruice8th EditionOrganic ChemistryISBN: 9780135213711Not the one you use?Change textbook
All textbooksBruice 8th EditionCh. 1 - Remembering General Chemistry: Electronic Structure and Bonding (Part 2)Problem 55b
Chapter 2, Problem 55b

Draw a Lewis structure for each of the following:
b. HNO2

Verified step by step guidance
1
Step 1: Determine the total number of valence electrons in the molecule. Hydrogen (H) has 1 valence electron, nitrogen (N) has 5 valence electrons, and oxygen (O) has 6 valence electrons. Add these together, considering there are two oxygen atoms in HNO₂.
Step 2: Identify the central atom. In this case, nitrogen (N) is the central atom because it is less electronegative than oxygen and can form multiple bonds.
Step 3: Connect the atoms with single bonds. Place hydrogen (H) bonded to nitrogen (N), and connect nitrogen to each oxygen atom with single bonds. This forms the basic skeleton of the molecule.
Step 4: Distribute the remaining valence electrons as lone pairs around the oxygen atoms to satisfy their octet rule. If there are still electrons left, place them on the nitrogen atom.
Step 5: Check the formal charges on each atom. If necessary, adjust the structure by forming a double bond between nitrogen and one of the oxygen atoms to minimize formal charges and achieve a more stable structure.

Verified video answer for a similar problem:

This video solution was recommended by our tutors as helpful for the problem above.
Video duration:
7m
Was this helpful?

Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

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 use dots to represent valence electrons and lines to represent bonds between atoms. Understanding how to draw Lewis structures is essential for visualizing molecular geometry and predicting reactivity.
Recommended video:
Guided course
04:12
Drawing the Lewis Structure for N2H4.

Valence Electrons

Valence electrons are the outermost electrons of an atom and are crucial in determining how atoms bond with each other. The number of valence electrons influences the molecule's structure and stability. For HNO2, knowing the valence electrons of hydrogen, nitrogen, and oxygen is necessary to accurately depict its Lewis structure.
Recommended video:
Guided course
03:40
Valence Electrons of Transition Metals

Formal Charge

Formal charge is a concept used to determine the distribution of electrons in a molecule and assess the most stable Lewis structure. It is calculated by comparing the number of valence electrons in the free atom to the number of electrons assigned to it in the Lewis structure. Minimizing formal charges across a molecule often leads to a more stable configuration.
Recommended video:
Guided course
01:34
Calculating formal and net charge.
Related Practice
Textbook Question

What is the hybridization of all the atoms (other than hydrogen) in each of the following?

What are the bond angles around each atom?

i. H3O+

j. H2C═O

1
views
Textbook Question

Draw the condensed structure of a compound that contains only carbon and hydrogen atoms and that has

a. three sp3 hybridized carbons.

b. one sp3 hybridized carbon and two sp2 hybridized carbons.

c. two sp3 hybridized carbons and two sp hybridized carbons.

1
views
Textbook Question

Draw a Lewis structure for each of the following:

d. NH2O−

Textbook Question

Predict the approximate bond angles:

c. the C—N—H bond angle in (CH3)2NH

d. the C—N—C bond angle in (CH3)2NH

1
views
Textbook Question

Rank the bonds from most polar to least polar.

b. C—Cl, C—I, C—Br

2
views
Textbook Question

Rank the bonds from most polar to least polar.

c. H—O, H—N, H—C

3
views