# Crystallisation and crystal surface

It is my understanding that if you put table salt (as an example of polar compound) in water, the Na+ and Cl- ions will freely move through the solution. They will make the solution conductive and will independently travel through it to carry electric current.

Now the thing is, if you dry the solution, how come every Na+ finds it's Cl- to recombine into NaCl? How come there are no lonely Na+ and Cl- pairs who couldn't find their mate in time, before the solution dried completely? Can someone give me a better understanding of how do polar solutions work?

• $\ce{NaCl}$ doesn't exist as molecules, it exists as unit cells with particular crystal arrangements. May 9 '17 at 11:02
• @PrittBalagopal Thanks for the input, but the question then still stands: How come there are not leftover ions that didn't fit in the crystal grid? May 9 '17 at 11:07
• Crystal surface is different than interior. There is no unit cell there. May 9 '17 at 14:22
• @TomášZato Have you consider the fact that both ions have a charge and they are strongly attracting each other? If the solution dries up it mea the concentration goes up, so it is even easier to find each other when they are packed in a small place.
– Greg
May 9 '17 at 17:10