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.10 - Chemical Bonding I: The Lewis Model
Tro5th EditionChemistry: A Molecular ApproachISBN: 9780134874371
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Table of contents
- Ch.1 - Matter, Measurement & Problem Solving93
- Ch.2 - Atoms & Elements94
- Ch.3 - Molecules and Compounds103
- Ch.4 - Chemical Reactions and Chemical Quantities44
- Ch.5 - Introduction to Solutions and Aqueous Solutions69
- Ch.6 - Gases97
- Ch.7 - Thermochemistry85
- Ch.8 - The Quantum-Mechanical Model of the Atom48
- Ch.9 - Periodic Properties of the Elements73
- Ch.10 - Chemical Bonding I: The Lewis Model76
- Ch.11 - Chemical Bonding II: Molecular Shapes, VSEPR & MO Theory70
- Ch.12 - Liquids, Solids & Intermolecular Forces41
- Ch.13 - Solids & Modern Materials40
- Ch.14 - Solutions76
- Ch.15 - Chemical Kinetics90
- Ch.16 - Chemical Equilibrium56
- Ch.17 - Acids and Bases121
- Ch.18 - Aqueous Ionic Equilibrium127
- Ch.19 - Free Energy & Thermodynamics78
- Ch.20 - Electrochemistry87
- Ch.21 - Radioactivity & Nuclear Chemistry60
- Ch.22 - Organic Chemistry115
Chapter 10, Problem 112
Calculate the heat of atomization (see previous problem) of C2H3Cl, using the average bond energies in Table 10.3.
Verified step by step guidance1
Identify the bonds present in the molecule \( \text{C}_2\text{H}_3\text{Cl} \). These include \( \text{C=C} \), \( \text{C-H} \), and \( \text{C-Cl} \) bonds.
Determine the number of each type of bond in the molecule. For \( \text{C}_2\text{H}_3\text{Cl} \), there is 1 \( \text{C=C} \) bond, 3 \( \text{C-H} \) bonds, and 1 \( \text{C-Cl} \) bond.
Look up the average bond energies for each type of bond from Table 10.3. For example, \( \text{C=C} \) might be 614 kJ/mol, \( \text{C-H} \) might be 413 kJ/mol, and \( \text{C-Cl} \) might be 328 kJ/mol.
Calculate the total energy required to break all the bonds in one mole of \( \text{C}_2\text{H}_3\text{Cl} \) by multiplying the number of each type of bond by its respective bond energy and summing them up.
The heat of atomization is the total energy calculated in the previous step, as it represents the energy required to break all bonds in the molecule to form individual atoms.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Heat of Atomization
The heat of atomization is the amount of energy required to break all the bonds in a molecule to form individual gaseous atoms. It is a crucial concept in thermochemistry, as it helps quantify the stability of a compound. The heat of atomization can be calculated using bond energies, which represent the average energy needed to break specific bonds in a molecule.
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Heat Capacity
Bond Energies
Bond energies are the average energies required to break specific types of chemical bonds in a molecule. These values are typically derived from experimental data and are essential for calculating the heat of atomization. In the context of C2H3Cl, one would use the bond energies of C-H, C-C, and C-Cl bonds to determine the total energy needed to separate the molecule into its constituent atoms.
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Molecular Structure
Understanding the molecular structure of a compound, such as C2H3Cl, is vital for calculating the heat of atomization. The arrangement of atoms and the types of bonds present influence the overall bond energies. A clear grasp of the molecular geometry and the connectivity of atoms allows for accurate calculations of the energy required to break all bonds in the molecule.
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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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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.
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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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