Is the molecule CF2Cl2 polar or nonpolar? Explain.

To determine whether CF₂Cl₂ is polar or nonpolar, we need to consider its molecular geometry and the electronegativity of its constituent atoms.

CF₂Cl₂, also known as dichlorodifluoromethane, has a tetrahedral shape. Carbon (C) is at the center, bonded to two fluorine (F) atoms and two chlorine (Cl) atoms. The electronegativity values of fluorine (3.98) and chlorine (3.16) indicate that fluorine is more electronegative than chlorine.

In this molecule, the C-F bonds are polar because fluorine attracts the bonding electrons more strongly than carbon. Similarly, the C-Cl bonds are also polar, but they are less polar than the C-F bonds due to the lower electronegativity of chlorine.

Despite the presence of polar bonds, the symmetry of the CF₂Cl₂ molecule plays a crucial role. The two C-F bonds and the two C-Cl bonds are arranged symmetrically around the central carbon atom. This symmetry results in the bond dipoles opposing each other and effectively canceling out.

Ultimately, due to this symmetrical arrangement leading to a cancellation of dipole moments, CF₂Cl₂ is considered to be a nonpolar molecule. In summary, while CF₂Cl₂ has polar bonds, its overall molecular geometry means that the dipole moments do not result in a net dipole moment, classifying it as nonpolar.