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

To determine the total number of valence electrons in CCl4, we need to add the number of valence electrons of each atom. Carbon has 4 valence electrons (group 14) and chlorine has 7 valence electrons (group 17). Since there are 4 chlorine atoms, the total number of valence electrons in CCl4 is: Total valence electrons = 1 x 4 (C) + 4 x 7 (Cl) = 4 + 28 = 32 valence electrons

To draw the Lewis structure of CCl4, we need to arrange the atoms in a way that the central atom (carbon) is surrounded by 4 chlorine atoms. Carbon is the central atom because it has the least electronegative element. Then, connect each chlorine atom to the central carbon atom with single bonds. After forming these bonds, if any valence electrons remain, distribute them as lone pairs on the surrounding atoms. Finally, check if the octet rule is fulfilled for all the atoms. The Lewis structure of CCl4 is represented as follows: Cl | Cl - C - Cl | Cl In this structure, each carbon-chlorine bond consists of 2 electrons, and thus the octet rule is fulfilled for all atoms in the molecule.

To describe the electron configuration around the central carbon atom, we must find the hybridization of the carbon atom. Carbon has four sigma bonds with four chlorine atoms in the CCl4 molecule, so it has tetrahedral electron pair geometry. This corresponds to sp3 hybridization for the central carbon atom. So, carbon has one s orbital and three p orbitals that hybridize to form four sp3 orbitals.

The bond between carbon and chlorine atoms in the CCl4 molecule is a single covalent bond formed due to the sharing of two electrons between them (one electron from the carbon atom and one electron from the chlorine atom). Thus, the C-Cl bond has a sigma bond character.

The molecular geometry of CCl4 is determined by the arrangement of the atoms in the molecule. Since carbon has four sp3 hybrid orbitals, the four chlorine atoms are arranged tetrahedrally around the central carbon atom. The bond angle between the C-Cl bonds is approximately 109.5 degrees. In conclusion, the local electron model helps describe the bonding in CCl4 as having a central carbon atom with sp3 hybridization, a single sigma bond between carbon and chlorine atoms, and a tetrahedral molecular geometry with bond angles of 109.5 degrees.