Question

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

Explanation:

• 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:

\(NO_2\), \(CO\), \(PCl_3\), \(SO_2\), \(HCl\)