which of the following molecules would most likely exhibit dipole - dipole interactions? check all that apply. no₂ co pcl₃ so₂ hcl

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# Brief Explanations:
- **For $NO_2$**:
  - $NO_2$ has a bent molecular geometry. The $N - O$ bonds are polar (due to the difference in electronegativity between $N$ and $O$). The overall molecule has a net dipole moment, so it can exhibit dipole - dipole interactions.
- **For $CO$**:
  - The $C - O$ bond is polar (since $O$ is more electronegative than $C$). The molecule has a net dipole moment (because it is a heteronuclear diatomic molecule), so it can exhibit dipole - dipole interactions.
- **For $PCl_3$**:
  - $PCl_3$ has a trigonal pyramidal geometry. The $P - Cl$ bonds are polar (due to the difference in electronegativity between $P$ and $Cl$). The overall molecule has a net dipole moment, so it can exhibit dipole - dipole interactions.
- **For $SO_2$**:
  - $SO_2$ has a bent molecular geometry. The $S - O$ bonds are polar (due to the difference in electronegativity between $S$ and $O$). The overall molecule has a net dipole moment, so it can exhibit dipole - dipole interactions.
- **For $HCl$**:
  - The $H - Cl$ bond is polar (since $Cl$ is more electronegative than $H$). The molecule has a net dipole moment (because it is a heteronuclear diatomic molecule), so it can exhibit dipole - dipole interactions.

# Answer:
$NO_2$, $CO$, $PCl_3$, $SO_2$, $HCl$

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