Question

question 15 (1 point)
which of the following molecules is non - polar?
co₂
co
cf₃cl
co₃²⁻
you can use this periodic table during the quiz.
however, as stated in the course outline, and in
the orientation session, this quiz is not open book.
you cannot access course material while you write
the quiz. nor can you google your answers, work as
a group, use a cheat sheet, etc.

Explanation:

• For \(CO_2\): It has a linear shape (\(O = C=O\)). The bond dipoles (due to the difference in electronegativity between \(C\) and \(O\)) are equal in magnitude and opposite in direction. So, they cancel each other out, making \(CO_2\) non - polar.
• For \(CO\): There is a significant electronegativity difference between \(C\) and \(O\). The bond dipole does not cancel (since there is only one bond dipole in a diatomic molecule), so \(CO\) is polar.
• For \(CF_3Cl\): The molecule has a tetrahedral electron - pair geometry. The bond dipoles ( \(C - F\) and \(C - Cl\) bonds have different electronegativity differences) do not cancel each other. The \(C - F\) bonds are more polar than \(C - Cl\) bonds, and the overall dipole moment is non - zero, so it is polar.
• For \(CO_3^{2-}\): Although it has a trigonal planar shape, the central \(C\) is bonded to \(O\) atoms. The \(C - O\) bond dipoles do not cancel exactly (due to the negative charge and the nature of resonance in the carbonate ion, there is an overall dipole moment), so it is polar.

Answer:

\(CO_2\)