Textbook Question
Draw the Lewis structure (including resonance structures) for methyl azide (CH3N3). For each resonance structure, assign formal charges to all atoms that have formal charge.
2220
views
Ch.10 - Chemical Bonding I: The Lewis Model
Tro6th EditionChemistry: A Molecular ApproachISBN: 9780137832217
Not the one you use?Change textbookSelect a different textbook
Table of contents
- Ch.1 - Matter, Measurement & Problem Solving90
- Ch.2 - Atoms & Elements94
- Ch.3 - Molecules and Compounds103
- Ch.4 - Chemical Reactions and Chemical Quantities46
- Ch.5 - Introduction to Solutions and Aqueous Solutions65
- Ch.6 - Gases100
- Ch.7 - Thermochemistry85
- Ch.8 - The Quantum-Mechanical Model of the Atom51
- Ch.9 - Periodic Properties of the Elements79
- Ch.10 - Chemical Bonding I: The Lewis Model70
- Ch.11 - Chemical Bonding II: Molecular Shapes, VSEPR & MO Theory68
- Ch.12 - Liquids, Solids & Intermolecular Forces44
- Ch.13 - Solids & Modern Materials42
- Ch.14 - Solutions77
- Ch.15 - Chemical Kinetics88
- Ch.16 - Chemical Equilibrium57
- Ch.17 - Acids and Bases121
- Ch.18 - Aqueous Ionic Equilibrium126
- Ch.19 - Free Energy & Thermodynamics80
- Ch.20 - Electrochemistry87
- Ch.21 - Radioactivity & Nuclear Chemistry61
- Ch.22 - Organic Chemistry114
Chapter 10, Problem 77
What are the formal charges of the atoms shown in red?
Verified step by step guidance1
Identify the red atoms in the given molecular structure.
Determine the number of valence electrons for each red atom in its elemental state.
Count the number of electrons assigned to each red atom in the molecule, considering both lone pairs and bonding electrons (each bond counts as one electron for the atom in question).
Use the formal charge formula: \( \text{Formal Charge} = \text{Valence Electrons} - \text{Non-bonding Electrons} - \frac{1}{2} \times \text{Bonding Electrons} \).
Calculate the formal charge for each red atom using the formula and the values obtained in the previous steps.
Verified video answer for a similar problem:
This video solution was recommended by our tutors as helpful for the problem above.
Video duration:
2mWas this helpful?
Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Formal Charge
Formal charge is a theoretical charge assigned to an atom in a molecule, calculated based on the number of valence electrons, the number of bonds, and the number of non-bonding electrons. It helps in determining the most stable structure of a molecule by minimizing the formal charges across the atoms. The formula for calculating formal charge is: Formal Charge = Valence Electrons - (Non-bonding Electrons + 1/2 Bonding Electrons).
Recommended video:
Guided course
01:53
Formal Charge
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 arrangement of electrons and help in understanding the distribution of formal charges. Drawing accurate Lewis structures is essential for determining the formal charges of atoms within a molecule.
Recommended video:
Guided course
04:28Lewis Dot Structures: Ions
Valence Electrons
Valence electrons are the electrons in the outermost shell of an atom that are involved in forming bonds with other atoms. The number of valence electrons determines an atom's reactivity and its ability to form bonds. Understanding the concept of valence electrons is crucial for calculating formal charges and predicting the behavior of atoms in chemical reactions.
Recommended video:
Guided course
02:12Transition Metals Valence Electrons
Related Practice
Textbook Question
In N2O, nitrogen is the central atom and the oxygen atom is terminal. In OF2, however, oxygen is the central atom. Use formal charges to explain why.
1716
views
Textbook Question
What are the formal charges of the atoms shown in red?
410
views
Textbook Question
Write the Lewis structure for each molecule (octet rule not followed). b. NO2
826
views
Textbook Question
Write the Lewis structure for each molecule (octet rule not followed). a. BBr3 b. NO c. ClO2
829
views
2
comments
Textbook Question
Draw the Lewis structure (including resonance structures) for the acetate ion (CH3COO-). For each resonance structure, assign formal charges to all atoms that have formal charge.
1572
views