Chemistry

I mean, are they still there, or they dissapear due to the attractions between sodium and chlorine ions and the water molecules?

Keep in mind the polarity of water requires that the sodium is bound to the oxygen atom and the chloride is bound to the hydrogen atoms. It will disrupt hydrogen bonding to some degree, but it won't eliminate it entirely unless you form a defined complex in which no hydrogen bonding is likely.

>>8552214
A high-schooler will tell you "nothing, they are still there", a chemist will tell "they assume a slightly different energy state/orbit", a physicist will tell you "we don't know" and a researcher computational quantum electron theory will simulate an approximation for you.

tl;dr: Your question is loaded and non-trivial.

>>8552237
Come on, we know that solvation is ethalpically favorable and entropically unfavorable, which is highly suggestive that the energetic states available to the solvent are decreased when things are dissolved in it.

What's exactly happening is still very vague, yes, but don't pretend that we don't have any idea what's happening.

>>8552237
What would a physical chemist say?