Solubility of Compounds Experiment

Flashcards covering key concepts related to the solubility of compounds and intermolecular forces discussed in the chemistry lecture.

Electronegativity

The tendency of an atom to attract a bonding pair of electrons.

Intermolecular Forces

Forces that mediate interaction between molecules, including dipole-dipole, ion-dipole, London dispersion, and hydrogen bonds.

Hydrogen Bonds

Strong intermolecular forces formed when a hydrogen atom bonded to a highly electronegative atom is attracted to another electronegative atom.

Dipole-Dipole Interactions

Attractions between the positive end of one polar molecule and the negative end of another polar molecule.

London Dispersion Forces

Weak intermolecular forces arising from temporary dipoles in molecules due to electron movement.

Solubility Principle

The principle stating that 'like dissolves like', meaning polar solvents dissolve polar solutes better than nonpolar solutes.

Ion-Dipole Interactions

Attractions between an ion and a polar molecule, significant in the solubility of ionic compounds in polar solvents.

Polar Molecule

A molecule with a net dipole moment due to the presence of polar bonds that do not cancel each other out.

Nonpolar Molecule

A molecule that has no net dipole moment; its charge distribution is symmetrical.

Lewis Structure

A diagram that represents the bonding between atoms of a molecule and the lone pairs of electrons.

Molecular Geometry

The three-dimensional arrangement of the atoms in a molecule.

Solute

The substance that is dissolved in a solvent to form a solution.

Solvent

The substance in which the solute is dissolved to form a solution.