Domanda del libro di testo
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
Tro6th EditionChemistry: A Molecular ApproachISBN: 9780137832217
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TOC.tableOfContents
- 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
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Capitolo 10, Problema 118
Calculate the heat of atomization (see previous problem) of C2H3Cl, using the average bond energies in Table 10.3.
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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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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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02:19
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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01:50Bond Energy
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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02:08Molecular Formula
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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 heat of atomization is the heat required to convert a molecule in the gas phase into its constituent atoms in the gas phase. The heat of atomization is used to calculate average bond energies. Without using any tabulated bond energies, calculate the average C–Cl bond energy from the following data: the heat of atomization of CH4 is 1660 kJ/mol, and the heat of atomization of CH2Cl2 is 1495 kJ/mol.
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Domanda del libro di testo
List the following gas-phase ion pairs in order of the quantity of energy released when they form from separated gas-phase ions. List the pair that releases the least energy first. Na+ F-, Mg2+F-, Na+O2-, Mg2+O2-, Al3+O2-.
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