Domanda del libro di testo
Calculate the heat of atomization (see previous problem) of C2H3Cl, using the average bond energies in Table 10.3.
Ch.10 - Chemical Bonding I: The Lewis Model
Tro5th EditionChemistry: A Molecular ApproachISBN: 9780134874371
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TOC.tableOfContents
- Ch.1 - Matter, Measurement & Problem Solving117
- Ch.2 - Atoms & Elements106
- Ch.3 - Molecules and Compounds128
- Ch.4 - Chemical Reactions and Chemical Quantities56
- Ch.5 - Introduction to Solutions and Aqueous Solutions84
- Ch.6 - Gases112
- Ch.7 - Thermochemistry96
- Ch.8 - The Quantum-Mechanical Model of the Atom60
- Ch.9 - Periodic Properties of the Elements86
- Ch.10 - Chemical Bonding I: The Lewis Model91
- Ch.11 - Chemical Bonding II: Molecular Shapes, VSEPR & MO Theory85
- Ch.12 - Liquids, Solids & Intermolecular Forces51
- Ch.13 - Solids & Modern Materials48
- Ch.14 - Solutions93
- Ch.15 - Chemical Kinetics114
- Ch.16 - Chemical Equilibrium68
- Ch.17 - Acids and Bases137
- Ch.18 - Aqueous Ionic Equilibrium154
- Ch.19 - Free Energy & Thermodynamics91
- Ch.20 - Electrochemistry105
- Ch.21 - Radioactivity & Nuclear Chemistry74
- Ch.22 - Organic Chemistry141
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Capitolo 10, Problema 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.
Guida verificata passo dopo passo1
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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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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01:42
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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01:53Formal Charge
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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06:17Ion Formation
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