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

First, draw the Lewis structure of CCl4. The Lewis structure is a representation of the molecule showing the arrangement of atoms and the distribution of valence electrons. To draw the Lewis structure for CCl4: 1. Find the number of valence electrons for each atom. Carbon has 4 valence electrons, and each Chlorine atom has 7 valence electrons. 2. Combine all valence electrons (4 for carbon + 7x4 for four chlorines = 32 electrons). 3. Place the carbon atom in the center and arrange the four chlorine atoms around it. 4. Distribute the valence electrons following the octet rule: 8 electrons for each chlorine atom (forming single bonds with the carbon atom) and 8 electrons for the carbon atom (forming one bond with each chlorine atom). 5. Check that each atom has a complete octet.

Next, determine the electron-pair geometry of CCl4. The electron-pair geometry is the arrangement of electron pairs around the central atom. In this case, the central atom is carbon, and it is surrounded by four electron pairs, each of them shared with a chlorine atom. According to the VSEPR (Valence Shell Electron Pair Repulsion) theory, these electron pairs will repel each other and be arranged as far away from each other as possible, resulting in a tetrahedral geometry.

Now, identify the molecular geometry. Molecular geometry is the arrangement of atoms in a molecule. Since the carbon atom in CCl4 is surrounded by four chlorine atoms and has no lone pairs, the molecular geometry is similar to the electron-pair geometry, also tetrahedral.

Finally, describe the sigma (σ) and pi (π) bonding in CCl4 using the localized electron model. In the localized electron model, bonds are described as either sigma (head-on overlap of atomic orbitals) or pi (side-on overlap of atomic orbitals). In CCl4, the carbon atom has four single bonds with chlorine atoms. In each C-Cl bond, an sp3 hybrid orbital from the carbon atom and a singly occupied atomic p-orbital from the chlorine atom overlap, resulting in the formation of four sigma (σ) bonds. There are no pi (π) bonds in CCl4. In conclusion, the localized electron model helps describe the bonding in CCl4 as follows: The bonds are formed by four sigma (σ) bonds, with the electron-pair geometry and molecular geometry both being tetrahedral.