Final answer:
The molecule among the options that does not have a dipole moment is CCl4. It is nonpolar because the symmetric tetrahedral geometry allows the individual bond dipole moments to cancel out, resulting in no overall dipole moment d) CCI4.
Step-by-step explanation:
The molecule that does not have a dipole moment among the given options is CCl4 (tetrachloromethane). Each of the carbon-chlorine bonds in CCl4 is polar due to the difference in electronegativity between carbon and chlorine. However, because the molecule has a tetrahedral geometry with four equivalent C-Cl bonds pointing in symmetric directions, the individual bond polarities cancel each other out, resulting in a nonpolar molecule with no net dipole moment.
On the other hand, molecules like CH3Cl, CH2Cl2, and CHCl3 have dipole moments because their shapes do not allow for the complete cancellation of their bond dipoles. For instance, chloromethane (CH3Cl) is a tetrahedral molecule with three slightly polar C-H bonds and a more polar C-Cl bond. The bond moments do not cancel out and result in a molecule with a considerable dipole moment.