Draw the Lewis Dot Structure for CCl4: Determine the Electron Geometry and Molecular Shape of This Molecule. Is This Molecule Polar or Nonpolar?

To draw the Lewis dot structure for CCl₄, follow these steps:

1. Count the total number of valence electrons: Carbon (C) has 4 valence electrons, and each chlorine (Cl) atom has 7 valence electrons. Since there are 4 chlorine atoms, the total number of valence electrons is 4 (from C) + 4 × 7 (from Cl) = 32 electrons.
2. Place the least electronegative atom in the center: Carbon is less electronegative than chlorine, so it will be the central atom.
3. Connect the outer atoms to the central atom with single bonds: Draw a single bond between the carbon atom and each chlorine atom. This uses up 8 electrons (4 bonds × 2 electrons).
4. Distribute the remaining electrons: Place the remaining 24 electrons around the chlorine atoms to complete their octets. Each chlorine atom will have 3 lone pairs.

The Lewis dot structure for CCl₄ is as follows:

    Cl
    |
Cl—C—Cl
    |
    Cl

Electron Geometry: The electron geometry of CCl₄ is tetrahedral. This is because there are 4 electron domains around the central carbon atom (4 bonding pairs).

Molecular Shape: The molecular shape of CCl₄ is also tetrahedral. Since there are no lone pairs on the central atom, the electron geometry and molecular shape are the same.

Polarity: CCl₄ is a nonpolar molecule. Although the C-Cl bonds are polar, the molecule is symmetrical, and the dipole moments cancel out, resulting in a nonpolar molecule.