Textbook Question
How important is the resonance structure shown here to the overall structure of carbon dioxide? Explain.
Ch.10 - Chemical Bonding I: The Lewis Model
Tro6th EditionChemistry: A Molecular ApproachISBN: 9780137832217
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Table of contents
- Ch.1 - Matter, Measurement & Problem Solving118
- Ch.2 - Atoms & Elements106
- Ch.3 - Molecules and Compounds131
- Ch.4 - Chemical Reactions and Chemical Quantities56
- Ch.5 - Introduction to Solutions and Aqueous Solutions82
- Ch.6 - Gases114
- Ch.7 - Thermochemistry96
- Ch.8 - The Quantum-Mechanical Model of the Atom60
- Ch.9 - Periodic Properties of the Elements90
- Ch.10 - Chemical Bonding I: The Lewis Model89
- Ch.11 - Chemical Bonding II: Molecular Shapes, VSEPR & MO Theory85
- Ch.12 - Liquids, Solids & Intermolecular Forces51
- Ch.13 - Solids & Modern Materials47
- Ch.14 - Solutions90
- Ch.15 - Chemical Kinetics115
- Ch.16 - Chemical Equilibrium68
- Ch.17 - Acids and Bases136
- Ch.18 - Aqueous Ionic Equilibrium153
- Ch.19 - Free Energy & Thermodynamics93
- Ch.20 - Electrochemistry106
- Ch.21 - Radioactivity & Nuclear Chemistry74
- Ch.22 - Organic Chemistry140
Chapter 10, Problem 73
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.
Verified step by step guidance1
insert step 1> Identify the formal charge formula: Formal charge = (Valence electrons) - (Non-bonding electrons) - (Bonding electrons/2).
insert step 2> Calculate the formal charges for each atom in N2O with nitrogen as the central atom: Consider the possible Lewis structures and calculate the formal charges for nitrogen and oxygen.
insert step 3> Calculate the formal charges for each atom in OF2 with oxygen as the central atom: Consider the possible Lewis structures and calculate the formal charges for oxygen and fluorine.
insert step 4> Compare the formal charges: The most stable structure is the one where the formal charges are minimized and closest to zero.
insert step 5> Explain the stability: In N2O, having nitrogen as the central atom results in a more stable structure with minimized formal charges, whereas in OF2, oxygen as the central atom results in minimized formal charges, explaining the observed structures.
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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 all atoms. A lower formal charge on an atom generally indicates a more stable configuration.
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Formal Charge
Molecular Geometry
Molecular geometry refers to the three-dimensional arrangement of atoms within a molecule. The central atom's position and the surrounding atoms influence the overall shape, which can affect the molecule's reactivity and properties. Understanding molecular geometry is crucial for predicting how atoms will bond and interact in different compounds.
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Central vs. Terminal Atoms
In a molecule, central atoms are typically bonded to multiple other atoms, while terminal atoms are usually bonded to only one other atom. The choice of which atom is central can affect the distribution of electrons and the overall stability of the molecule. In the case of N2O and OF2, the central atom's identity influences the formal charge calculations, leading to different preferred structures.
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Related Practice
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.
Textbook Question
What are the formal charges of the atoms shown in red?
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Textbook Question
Use formal charges to identify the better Lewis structure.
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.
Textbook Question
Write a Lewis structure that obeys the octet rule for each ion. Include resonance structures if necessary and assign formal charges to each atom. a. ClO3- b. ClO4- c. NO3- d. NH4+