Answer:
Option B
Explanation:
Ion-ion interaction is dependent on the square of distance.
i.e, ion-ion interaction $\propto \frac{1}{r^{2}}$
Similarly,
ion-dipole interaction $\propto \frac{1}{r^{3}}$
London forces $\propto \frac{1}{r^{6}}$
and dipole -dipole interactions $\propto \frac{1}{r^{3}}$
Superficially it seems as both ion dipole interaction and hydrogen bonding vary with inverse cube of distance between the molecules but when we look at the exact expressions of field (force) created in two situations it comes as
$|E| or |F|= \frac{2|P|}{4\pi \epsilon_{0}r^{3}}$
(In case of ion-dipole interaction)
and $F=\frac{2q^{2}r-4q^{2}a}{4\pi \epsilon_{0}r^{3}}$
( In case of dipole-dipole interaction)
From the above it is very clear , the ion-dipole interaction is the better answer as compared to dipole -dipole interaction , i.e hydrogen bonding
