Hydrogen bonding and dipole moment

Why this is asked: Net dipole moment is a vector sum of bond dipoles, not a scalar one — CO₂'s two C=O dipoles cancel exactly in its linear geometry (μ=0), while bent H₂O's don't. The classic trap: o-nitrophenol's intramolecular hydrogen bond makes it more volatile than p-nitrophenol, whose hydrogen bonding is intermolecular — having H-bonds isn't enough, the question is whether they're within or between molecules.

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