Intermolecular Forces and Properties

Reactant

Catalyst

Product

Solvent

High charge density leading to increased lattice energy

Larger atomic radii decreasing ion-dipole interactions

Smaller ion sizes reducing crystal defect formation

Lower hydration enthalpy for larger ions

Differences in lattice energy due to varying ion charges and sizes

The phase at room temperature between various salts

The difference in melting points between salts

The color change when each salt is dissolved in water

London dispersion forces

Hydrogen bonding

Dipole-dipole forces

Ion-dipole forces

The compound forms covalent bonds with water molecules.

The compound precipitates out of the solution.

The water molecules form an alloy with the compound.

The compound dissociates into its ions.

The strong hydrogen bonding between the polar molecules and the solvent molecules make it easier for the molecular compound to dissolve in polar solvents.

The strong dipole-dipole interactions between the polar molecules and the solvent molecules make it easier for the molecular compound to dissolve in polar solvents.

The weak van der Waals interactions between the polar molecules and the solvent molecules make it difficult for the molecular compound to dissolve in nonpolar solvents.

The strong covalent bonding between the polar molecules and the solvent molecules make it easier for the molecular compound to dissolve in polar solvents.

Mn^2+

Co^2+

Fe^2+

Ni^2+

Molecular solid with hydrogen bonding interactions

Ionic solid with an endothermic dissolution process

Nonpolar molecular solid with induced dipole forces

Ionic solid with an exothermic dissolution process

Generally increases both Ksp value and solubility.

Decreases soluble salt content without affecting Ksp value.

Increases Ksp but has no direct relationship with soluble salt content.

Generally decreases both Ksp values ​​and solubility.

A solution that contains the maximum amount of solute that can dissolve at a given temperature.

A solution with less solute than can be dissolved at a specific temperature

A homogeneous mixture where the particles are evenly mixed and the solute is uniformly distributed within the solvent.

A solution where more solute than can normally be dissolved in the solvent is present.