Question

missed this? watch iwe: determining whether a molecule is polar. read section 10.8. you can click on

part a

classify each of the following molecules as polar or nonpolar
drag the items into the appropriate bins.

ch₃oh ch₂cl₂ co₂ h₂co

polar nonpolar

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Explanation:

• For \( \text{CH}_3\text{OH} \): It has a bent shape around the oxygen atom due to the lone pairs. The \( \text{O}-\text{H} \) and \( \text{C}-\text{O} \) bonds are polar, and the molecule's asymmetry leads to an overall dipole moment, so it is polar.
• For \( \text{CH}_2\text{Cl}_2 \): The \( \text{C}-\text{Cl} \) bonds are more polar than \( \text{C}-\text{H} \) bonds. The molecule is tetrahedral but not symmetrical in terms of bond polarities (since \( \text{Cl} \) and \( \text{H} \) have different electronegativities), resulting in a net dipole moment, so it is polar.
• For \( \text{CO}_2 \): It is a linear molecule (\( \text{O}=\text{C}=\text{O} \)). The individual \( \text{C}=\text{O} \) bond dipoles cancel each other out due to the symmetry of the linear shape, so it is non - polar.
• For \( \text{H}_2\text{CO} \) (formaldehyde): It has a trigonal planar shape. The \( \text{C}=\text{O} \) bond is polar, and the molecule is not symmetrical enough (the \( \text{C}-\text{H} \) and \( \text{C}=\text{O} \) bonds have different polarities) to cancel the dipole moment, so it is polar.

Answer:

Polar: \( \text{CH}_3\text{OH} \), \( \text{CH}_2\text{Cl}_2 \), \( \text{H}_2\text{CO} \)
Non - polar: \( \text{CO}_2 \)