What is wrong with this molecular view of a sodium chloride solution? What would make the picture correct?
In the figure given smaller particles are water molecules and bigger particles are NaCl molecules when solid NaCl is put into water there is a clash between the attractive forces that hold Na + and Cl - particles together.and the attractive forces occuring between the particles of Na+ and Cl-and water molecule .
Hence the attractive forces occurring between the water molecules and particles of NaCl overcome the attractive forces that hold Na+ and Cl- particles together .
NaCl(solid) + H2O -> Na+(aqueous) + Cl-(aqueous) + H2O
On addition to water the Na+ section of NaCl is attracted to the oxygen side of the water molecules, while the Cl- side is attracted to the hydrogens' side of the water molecule.
This causes the sodium chloride to split in water, and the NaCl dissolves into separate Na+ and Cl- atoms. A hydration shell is formed around them which prevents Na+ and Cl- to form ionic bonds.
Thus we say the salt is dissolved.