What is the difference between an ion-induced dipole attraction and just an ion-dipole attraction? By what I've read, an ion-induced dipole attraction is a weak attraction that results when the approach of an ion creates a dipole in a non-polar atom or in a non-polar molecule by disturbing the arrangement of electrons in the non-polar species. So this is a dispersion/van-der-Waal force, I believe?  

On the other hand, an ion-dipole attraction is a weak attraction that results when the approach of an ion interacts with the dipole in a polar atom or in a polar molecule. And so this wouldn't be a van-der-Waal force would it?  



If what I said above happens to be true, does the same apply with dipole-induced dipole forces and just dipole-dipole forces?

In this scenario, a dipole-induced dipole attraction would be a weak attraction that results when the approach of an dipole (polar covalent bond) creates a dipole in a non-polar atom or in a non-polar molecule by disturbing the arrangement of electrons in the non-polar species. So this is a dispersion/van-der-Waal force too, right?

And a dipole-dipole attraction would be a weak attraction that results when the approach of an dipole that already exists  in a polar bond attracts with another dipole in another polar atom or in polar molecule.
It is useful to note the definition of a van der Waal force: weak electric forces attracting neutral molecules to each other in gas thus causing a gas to deviate from an ideal gas.

So, there are three types of these forces


Dipole-dipole force
Dipole-induced dipole force
London dispersion force


It becomes clear that forces involving ions do not fit van de Waals forces as the molecules involved must be neutral. 

An ion-induced dipole force is not a dispersion force, either (as dispersion forces are a subset of van der Waals), and with ion-dipole forces, ion-induced dipole forces have a category of it's own

A dipole-induced dipole force is a van der Waal force but not a dispersion force