The ion - dipole attractions between the Na+ and the polar water molecule and the ion - dipole attractions between the Cl- and the polar water molecule contribute to the dissolution of sodium chloride in water.
Further Explanation:
Sodium chloride is an ionic compound. The electrostatic attraction between its positive charged ions (Na+) and negatively charged ions (Cl-) holds the crystal lattice together.
Water is a polar molecule. Polar molecules have a net dipole moment due to the differences in electronegativity of the atoms in the molecule and the geometry of the molecule as well. Since oxygen is more electronegative than hydrogen, it pulls the shared electrons towards itself. The part of the molecule where oxygen is, gains a partial negative charge, since the shared electrons spend more time in this region than near hydrogen. The hydrogen side of the molecule, then becomes mostly electron-deficient giving it a partial positive charge.
In the dissolution of sodium chloride in water, the ion - ion attractions of the salt is weakened as it absorbs heat. Then, polar water molecules start to surround individual Na+ or Cl- ions by orienting themselves accordingly: the partial negative side of water are attracted to the Na+ and the H side of the water molecule is attracted to the Cl- ions. With enough water molecules surrounding the each ion, the ion - dipole attractions formed overcome the ion - ion attraction of the salt.
Learn More
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Keywords: dissolution, intermolecular forces