Textbook Question
Write a Lewis structure that obeys the octet rule for each molecule or ion. Include resonance structures if necessary and assign formal charges to each atom. b. CO32– c. ClO– d. NO2–
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Ch.9 - Chemical Bonding I: The Lewis Model
Tro4th EditionChemistry: A Molecular ApproachISBN: 9780134112831
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Table of contents
- Ch.1 - Matter, Measurement & Problem Solving107
- Ch.2 - Atoms & Elements100
- Ch.3 - Molecules, Compounds & Chemical Equations127
- Ch.4 - Chemical Quantities & Aqueous Reactions114
- Ch.5 - Gases103
- Ch.6 - Thermochemistry92
- Ch.7 - Quantum-Mechanical Model of the Atom50
- Ch.8 - Periodic Properties of the Elements89
- Ch.9 - Chemical Bonding I: The Lewis Model84
- Ch.10 - Chemical Bonding II: Molecular Shapes & Valence Bond Theory74
- Ch.11 - Liquids, Solids & Intermolecular Forces60
- Ch.12 - Solids and Modern Material50
- Ch.13 - Solutions90
- Ch.14 - Chemical Kinetics111
- Ch.15 - Chemical Equilibrium65
- Ch.16 - Acids and Bases135
- Ch.17 - Aqueous Ionic Equilibrium145
- Ch.18 - Free Energy and Thermodynamics92
- Ch.19 - Electrochemistry100
- Ch.20 - Radioactivity and Nuclear Chemistry68
- Ch.21 - Organic Chemistry121
Chapter 9, Problem 68
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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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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