Understanding London Forces and Molecular Interactions

This page explores the fundamental concepts of intermolecular forces and their various manifestations. The content focuses on three main types of molecular interactions and their effects on physical properties.

Definition: London forces are universal intermolecular forces present between all molecules, resulting from temporary electron distribution fluctuations.

Highlight: Every molecule exhibits London forces, which form the basis for molecular attractions.

Example: When electrons create an instantaneous dipole in one molecule, it induces a dipole in nearby molecules, leading to attraction.

Vocabulary: Permanent dipole-dipole interactions occur specifically between polar molecules due to uneven electron distribution.

Definition: Hydrogen bonding represents a special type of permanent dipole-dipole interaction, occurring when hydrogen is attached to highly electronegative atoms (O, N, or F) with lone electron pairs.

The relationship between these forces and boiling points is particularly significant, with hydrogen bonding typically resulting in higher boiling points due to stronger intermolecular attractions.