Calculate the heat of atomization (see previous problem) of C2H3Cl, using the average bond energies in Table 10.3.

Verified step by step guidance

1. 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.
2. 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.
3. 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.
4. 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.
5. 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.

Key Concepts

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.

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.

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.