Observe the statements.
1) Dipole-Dipole interaction energy between rotating polar molecules is proportional to $\frac{1}{r^6}$[r = distance between polar molecules]
2) London forces are always attractive and interaction energy is inversely proportional to $\frac{1}{r^6}$ [r = distance between two particles]
3) Dipole-Dipole interaction energy between stationary polar molecules is proportional to $\frac{1}{r^3}$
4) The order of thermal energy is “solid < liquid < gas”.
The correct statements are

Dipole dipole interaction energy between stationary polar molecules is proportional to 1/r³ and that between the rotating polar molecules is proportional to 1/r⁶ where r is the distance between the molecules .

London dispersion forces are always attractive and operate only over very short distance. The energy of interaction varies as $\frac{1}{{\left(\mathrm{distance} \mathrm{between} \mathrm{two} \mathrm{interacting} \mathrm{particles}\right)}^6}$

Solid < liquid < gas. This is because solid absorb energy to change into a liquid which further absorbs energy to change into a gas.