Why is there a greater degree of separation in a dipole-dipole interaction? My textbook says this:


  Electrostatic forces between two ions decrease by the factor $\frac{1}{d^2}$ as their separation distance, $d$, increases. Dipole–dipole forces, however, vary as  $\frac{1}{d^4}$. Because of the higher power of $d$ in the denominator, the attractive forces diminish with increasing $d$ much more rapidly than does  $\frac{1}{d^2}$. As a result, dipole forces are effective only over very short distances.


Now mathematically I understand why this is true, but I don't understand why this is the case in reality. Can someone shed some light on this?
Like I answered my other question, this is in some ways very similar. Since electrostatic attractions are so strong, it is decreases less at a longer distances. The $+$ &amp; $-$ are attracted together so strongly. 

Dipole-dipole attractions aren't strong attractions, electrostatic attractions are stronger, since they are created by ionic bonding. Dipole-dipole occur in covalent bonding. Thus dipole-dipole attractions decrease with increasing distance faster.

This is just a piece of the whole picture.



Check the refs: 1, 2, 3. They provide more in depth detail to the entire picture.