Final answer:
The intermolecular forces in salt are ionic bonds, while water molecules exhibit hydrogen bonds, dipole-dipole interactions, and London dispersion forces. These forces determine the properties of salt and water, such as boiling point and solubility
Step-by-step explanation:
Intermolecular Forces in Salt and Water
The intermolecular forces involved in salt (ionic compounds) and water (H2O) molecules have a significant impact on their physical properties, such as melting points, boiling points, and solubility. In salt molecules, the primary intermolecular force is the strong ionic bond between the positively charged cations and negatively charged anions. In water molecules, the primary intermolecular forces are hydrogen bonds, along with dipole-dipole interactions and London dispersion forces.
Hydrogen bonding in water is particularly strong due to the highly polar nature of the molecule, where the oxygen atom has a partial negative charge, and the hydrogen atoms have a partial positive charge.
The extensive hydrogen bonding in water leads to its high surface tension, viscosity, and relatively high boiling point compared to other substances of similar molecular weight. The dissolution of salt in water is facilitated by ion-dipole interactions between the ions and the polar water molecules, which help to break apart the ionic lattice of the salt and separate the ions into the solution.
Temperature effects on intermolecular forces can be observed in the changes in properties such as surface tension and viscosity. With an increase in temperature, the kinetic energy of the water molecules increases, reducing the strength of hydrogen bonding, hence decreasing surface tension and viscosity. Conversely, lowering the temperature diminishes kinetic energy, which enhances the intermolecular attractions, increasing these properties.