Intermolecular Forces and Properties of Mixtures

These flashcards cover the key concepts related to intermolecular forces, their properties, and behaviors in solutions.

Intermolecular Forces

Forces/attractions between separate molecules that influence properties like solubility and boiling point.

Covalent Bond

A strong bond where individual atoms are held together to form a single molecule.

Polarity

A phenomenon arising from an unequal distribution of electrons in a covalent bond, leading to positive and negative poles.

Ionic Bond

A bond characterized by a large difference in electronegativity, resulting in a complete transfer of electrons.

Dipole Moment

A measure of the polarity of a molecule, calculated as the vector sum of individual bond dipoles.

Hydrogen Bond

A strong dipole-dipole interaction occurring between a hydrogen atom bonded to highly electronegative atoms (N, O, F) and another electronegative atom.

London Dispersion Forces

Weak intermolecular forces arising from temporary dipoles due to electron motion; present in all molecules.

Solvation

The process of solute molecules dissolving in a solvent, surrounded by solvent molecules.

Hydrophobic Effect

The tendency of nonpolar substances to aggregate in aqueous solutions to minimize their exposure to water.

Colligative Properties

Changes in physical properties of a solvent as a result of adding a solute, independent of the solute's identity.

Freezing Point Depression

The lowering of a solvent's freezing point due to the presence of solute particles.

Boiling Point Elevation

The raising of a pure solvent's boiling point as a result of solute addition.

Electrostatic Potential Maps

Visual depictions of dipole moments and polarity distributions in molecules.

Partition Coefficient (LogP)

A measure of a compound's hydrophobicity or hydrophilicity by its partitioning between two immiscible solvents.

Molarity (M)

A concentration measure representing the number of moles of solute per liter of solution.