CHEM 1112 Lecture Notes - Lecture 1: Intermolecular Force, London Dispersion Force, Hydrogen Bond
Document Summary
Fundamental difference between states of matter > distance between particles: gas. Particles have freedom of motion: far apart from one another. Particles are clustered with one another and take shape of one another. Has extremely weak bonds or no bonds at all. Particles free to move relative to each other: close together. Particles in fixed positions: close together. Solids and liquids = condensed phases: b/c particles are closer together. Substance"s state is in at a specific temperature depends on: ke of particles, strength of attractions b/w particles. Intramolecular forces that hold compounds together are extremely stronger than intermolecular attractions: intermolecular forces are strong enough to control physical properties (i. e. boiling and melting points, vapor pressures, and viscosities) Collectively known as van der waals forces van der waals forces. Strength makes it possible for ionic substances to dissolve in polar solvents: example: salt in water.
