Concept:Boiling point elevation is heavily dependent on the strength of attractions between separate molecules in a liquid.
Formula:$$ \text{B.P.} \propto \text{Intermolecular Force Strength} $$
Solution:- Intermolecular Hydrogen Bonding creates strong, pervasive electrostatic linkages between multiple separate molecules across the entire liquid volume, requiring massive thermal energy to break apart, raising the boiling point dramatically.
- Intramolecular H-bonding occurs strictly within a single molecule (e.g., ortho-nitrophenol). Because the molecule is busy bonding with itself, it interacts less strongly with neighboring molecules, generally leading to a lower boiling point.
Why other options are incorrect:London dispersion and dipole-induced forces are relatively weak compared to genuine Intermolecular Hydrogen bonding.
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