Question

what type or types of intermolecular forces exists or exist in the molecule below? ccl4
london dispersion forces only
dipole dipole only
h bonding only
london dispersion forces, dipole dipole, & h bonding
dipole dipole, & h bonding
london dispersion forces & dipole dipole
ionic bonding only
london dispersion forces & ionic bonding
none of these

Explanation:

1. London - Dispersion Forces: All molecules have London - dispersion forces. These forces arise from temporary dipoles caused by the motion of electrons. In $CCl_4$, the large number of electrons (carbon has 6 and each chlorine has 17, so a total of $6 + 4\times17=74$ electrons) leads to significant London - dispersion forces.
2. Dipole - Dipole Forces: Although each $C - Cl$ bond is polar due to the electronegativity difference between carbon (2.5) and chlorine (3.0), the $CCl_4$ molecule is tetrahedral and symmetric. The bond dipoles cancel each other out, making the molecule non - polar overall. So, there are no permanent dipole - dipole forces.
3. Hydrogen Bonding: Hydrogen bonding occurs when a hydrogen atom is bonded to a highly electronegative atom ($N$, $O$, or $F$). Since $CCl_4$ has no hydrogen atoms, there is no hydrogen bonding.
4. Ionic Bonding: $CCl_4$ is a covalent compound formed by the sharing of electrons between carbon and chlorine atoms, so there is no ionic bonding.

Answer:

A. London Dispersion forces only