Use the localized electron model to describe the bonding in \(\mathrm{CCl}_{4}\).

We first need to determine the electron configurations for both Carbon (C) and Chlorine (Cl) atoms: - Carbon (C) - Atomic number: 6 Electron configuration: \(1s^2 2s^2 2p^2\) - Chlorine (Cl) - Atomic number: 17 Electron configuration: \(1s^2 2s^2 2p^6 3s^2 3p^5\)

Next, we need to determine the valence electrons of Carbon and Chlorine atoms: - Carbon (C) - Valence electrons: 4 - Chlorine (Cl) - Valence electrons: 7

We can now calculate the total number of electrons in the CCl4 molecule. Carbon contributes 4 electrons, and each Chlorine atom contributes 7 electrons: Total electrons = (1 x 4) + (4 x 7) = 4 + 28 = 32 electrons

Using the localized electron model, we can now determine the structure of the CCl4 molecule: 1. Place Carbon (C) in the center as it has the lowest electronegativity among the atoms. 2. Arrange the Chlorine atoms (Cl) around the Carbon atom (tetrahedral geometry). 3. Distribute the remaining electrons around the Chlorine atoms as lone pairs to complete their octet. Now, regarding the CCl4 molecule: - Carbon (C) forms 4 single covalent bonds with each Chlorine atoms. So, ∠Cl-C-Cl bond angle = 109.5° (tetrahedral arrangement) - Each Carbon-Chlorine bond is a sigma bond formed by overlapping atomic orbitals between Carbon and Chlorine. In conclusion, the bonding in carbon tetrachloride (CCl4) using the localized electron model is characterized by a central carbon atom covalently bonded to four surrounding chlorine atoms in a tetrahedral geometry with ∠Cl-C-Cl bond angles of 109.5°.