CHEM2311 Lecture 9: Intermolecular Forces

A set of vocabulary flashcards covering key concepts related to intermolecular forces, including definitions and explanations pivotal for understanding the topic.

Dipole Moment

A measure of charge separation within a bond or molecule, represented as a vector indicating both direction and magnitude.

Molecular Dipole

The vector sum of all bond dipole moments and the lone pair electrons in a molecule, which reflects both magnitude and direction of dipole moments.

Intermolecular Forces (IMFs)

Attractive and repulsive forces between two or more molecules, affecting properties such as boiling point and solubility.

Hydrogen Bonding

The strongest intermolecular force, requiring a very polar bond to a hydrogen atom, involving H-bond donors and acceptors.

London Dispersion Forces (LDF)

Weak intermolecular forces that arise from temporary dipole moments in non-polar molecules due to the influence of neighboring molecules.

Polarizability

The extent to which electrons can be displaced by a positive charge; in polarizable atoms, electrons move more freely towards positive charges.

Solubility

The extent to which a solute dissolves into a solvent, generally summarized by the rule 'like dissolves like'.

Dipole-Dipole Interactions

Attractive forces that occur between polar molecules, influencing physical properties such as boiling points.

Bond Dipole

A measure of the polarity of a bond; it indicates the separation of charge within the bond.

Lone Pairs

Pairs of valence electrons that are not involved in bonding, affecting molecular dipoles and polar characteristics.