Question

take a look at the lewis structures of the molecules below. based on shape and polarity of the bonds, select the molecules that are polar. :\ddot{\text{cl}} - \text{be} - \ddot{\text{cl}}: shape: linear \ddot{\text{o}} = \ddot{\text{s}} = \ddot{\text{o}} shape: bent :\text{c} \equiv \text{o}: shape: linear

Explanation:

• For \(Cl - Be - Cl\): The molecule has a linear shape. The \(Be - Cl\) bonds are polar, but due to the symmetry of the linear shape, the bond dipoles cancel each other out. So, this molecule is non - polar.
• For \(O = S = O\): The molecule has a bent shape. The \(S - O\) bonds are polar. In a bent shape, the bond dipoles do not cancel each other. So, this molecule is polar.
• For \(C\equiv O\): The molecule has a linear shape. The \(C - O\) bond is polar. Since there is only one bond (and no symmetry to cancel the dipole), this molecule is polar.

Answer:

\(O = S = O\) (Shape: Bent), \(C\equiv O\) (Shape: Linear)