# Why do some ionic compounds have some solubility in water; why do ionic compounds have high melting and boiling points?

Boiling, or dissolution, requires that these strong forces of attraction be disrupted. For sodium chloride, these intramolecular or interparticle interactons, are compensated for by the making of ion-dipole bonds when sodium chloride dissolves in water, and the water dipoles solvate the individual ions; we write $N {a}^{+} \left(a q\right)$ to represent this, a shorthand for ${\left[N a {\left(O {H}_{2}\right)}_{6}\right]}^{+}$. Dissolution of sodium chloride is VERY SLIGHTLY endothermic; what does this say with regard to thermodynamics of of $N {a}^{+} \left(a q\right)$ and $C {l}^{-} \left(a q\right)$ formation?