I'm having trouble understanding exactly what intermolecular forces occur in ionic compounds.
What I understand is that ionic compounds are held together by electrostatic interactions between opposite charged ions and that they aren't "finite" in the way covalent molecules are, and therefore they do not have intermolecular forces.
However, while my textbook says that only covalent molecules have van der Waals forces, my professor said that all compounds, even ionic compounds have London dispersion interactions.
Isn't London dispersion a van der Waals force? How does that work?