3.1-3.6 Notes

London Dispersion Forces

Intermolecular forces resulting from temporary, fluctuating dipoles, often the strongest net force between large molecules.

Polarizability

The ability of a molecule's electron cloud to be distorted, increasing with the number of electrons and size of the electron cloud.

Dipole-Induced Dipole Interactions

Attractive forces between a polar molecule and a nonpolar molecule, dependent on the polarizability of the nonpolar molecule.

Dipole-Dipole Interactions

Forces present between polar molecules, influenced by the magnitudes of their dipoles and their relative orientation.

Ion-Dipole Forces

Strong attractive forces between ions and polar molecules, typically stronger than dipole-dipole forces.

Hydrogen Bonding

A strong intermolecular interaction occurring when hydrogen is covalently bonded to electronegative atoms (N, O, F) and interacts with another electronegative atom.

Properties of Solids

Determined by the strengths and types of intermolecular forces, affecting vapor pressure, boiling point, and melting point.

Ionic Solids

Characterized by strong interactions between ions, resulting in low vapor pressures, high melting and boiling points, and brittleness.

Covalent Network Solids

Solids formed by covalently bonded atoms in a three-dimensional network, exhibiting high melting points and rigidity.

Molecular Solids

Composed of distinct molecules held together by weak intermolecular forces, generally having low melting points and not conducting electricity.

Metallic Solids

Good conductors of electricity and heat due to free valence electrons, malleable and ductile, with properties influenced by interstitial atoms in alloys.

Crystalline Solids

Solids with particles arranged in a regular three-dimensional structure, limiting particle motion.

Amorphous Solids

Solids lacking a regular arrangement of particles, with limited motion and no overall translation.

Liquid Properties

Particles are in close contact and continually moving, influenced by intermolecular forces and temperature.

Gas Properties

Particles are in constant motion with minimal intermolecular forces, resulting in no definite volume or shape.

Ideal Gas Law

The relationship between pressure (P), volume (V), temperature (T), and number of moles (n) of an ideal gas, expressed as PV = nRT.

Partial Pressure

The pressure exerted by an individual gas in a mixture, independent of other gases, contributing to total pressure.

Deviations from Ideal Gas Law

Occur due to high pressure, low temperature, nonzero molecular volume, and intermolecular attractions affecting gas behavior.