Question

determine whether each molecule is polar or nonpolar. drag the appropriate items to their respective bins. nonpolar polar

Explanation:

• \(SF_{6}\): It has an octahedral molecular geometry. The symmetric distribution of \(S - F\) bonds (all \(F\) atoms are equivalent in this symmetric structure) leads to the cancellation of bond dipoles. So, it is non - polar.
• \(CF_{2}Cl_{2}\): It has a tetrahedral electron - pair geometry. But \(C - F\) and \(C - Cl\) bonds have different electronegativity differences. The bond dipoles do not cancel out (since \(F\) and \(Cl\) are not the same atoms), so it is polar.
• \(SiCl_{4}\): It has a tetrahedral molecular geometry. The four \(Si - Cl\) bonds are symmetrically arranged. The bond dipoles cancel each other out, making it non - polar.
• \(PCl_{3}\): It has a trigonal pyramidal molecular geometry. The \(P - Cl\) bond dipoles do not cancel (due to the lone pair on \(P\) which distorts the symmetry), so it is polar.

Answer:

• Nonpolar: \(SF_{6}\), \(SiCl_{4}\)
• Polar: \(CF_{2}Cl_{2}\), \(PCl_{3}\)