Textbook Question
A compound composed of only carbon and chlorine is 85.5% chlorine by mass. Propose a Lewis structure for the compound.
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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 108
The azide ion, N3-, is a symmetrical ion, all of whose contributing resonance structures have formal charges. Draw three important contributing structures for this ion.
Verified step by step guidance1
Identify the total number of valence electrons in the azide ion, \( \text{N}_3^- \). Nitrogen has 5 valence electrons, and there are three nitrogen atoms, plus one extra electron due to the negative charge, giving a total of 16 valence electrons.
Distribute the electrons to form bonds between the nitrogen atoms. Start by connecting the three nitrogen atoms in a linear arrangement: \( \text{N} - \text{N} - \text{N} \).
Assign electrons to form double or triple bonds between the nitrogen atoms to satisfy the octet rule for each atom, while keeping the total number of electrons at 16.
Calculate the formal charge for each nitrogen atom in each resonance structure using the formula: \( \text{Formal Charge} = \text{Valence Electrons} - \text{Non-bonding Electrons} - \frac{1}{2} \times \text{Bonding Electrons} \).
Draw the three resonance structures, ensuring that the sum of the formal charges equals the overall charge of the ion, which is -1.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Resonance Structures
Resonance structures are different ways of drawing a molecule or ion that represent the same arrangement of atoms but differ in the distribution of electrons. For the azide ion (N3-), these structures help illustrate how the electrons can be delocalized across the molecule, contributing to its overall stability. Each resonance structure must obey the rules of valence and maintain the same number of electrons.
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Resonance Structures
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 non-bonding electrons, and half the number of bonding electrons. It helps in determining the most stable resonance structure, as structures with formal charges closer to zero are generally more favorable. In the case of the azide ion, understanding formal charges is crucial for drawing accurate resonance structures.
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Symmetry in Ions
Symmetry in ions refers to the uniform distribution of charge and structure, which can influence the stability and reactivity of the ion. The azide ion (N3-) is symmetrical, meaning its resonance structures will reflect this symmetry, leading to equivalent contributions from each structure. Recognizing symmetry helps predict the behavior of the ion in chemical reactions and its interactions with other species.
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Related Practice
Textbook Question
A compound composed of only carbon and hydrogen is 7.743% hydrogen by mass. Propose a Lewis structure for the compound.
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Textbook Question
Draw the Lewis structure for each compound. c. H3AsO4
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Textbook Question
Calculate ΔHrxn for the combustion of octane (C8H18), a component of gasoline, by using average bond energies and then calculate it using enthalpies of formation from Appendix IIB. What is the percent difference between your results? Which result would you expect to be more accurate?
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Textbook Question
Calculate the heat of atomization (see previous problem) of C2H3Cl, using the average bond energies in Table 9.3.
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