ap chem unit 3 terms

intermolecular forces

Forces of attraction or repulsion between molecules.

London dispersion forces

Weak intermolecular forces due to temporary, fluctuating dipoles in molecules.

dipole-dipole

Attractive forces between polar molecules due to their dipole moments.

hydrogen bonding

Strong type of dipole-dipole interaction that occurs between molecules containing a hydrogen atom bonded to a highly electronegative atom. (H with N, O, or F)

dipole-induced dipole

Interaction between a polar molecule and a nonpolar molecule that induces a dipole in the nonpolar molecule.

ion-induced dipole

Attraction between an ion and a nonpolar molecule that creates a dipole in the nonpolar molecule.

ion-dipole

Attractive forces between an ion and a polar molecule.

vapor pressure

Pressure exerted by a vapor in equilibrium with its liquid or solid phase.

ionic solids

Solids composed of ions held together by ionic bonds, characterized by high melting points.

covalent network solids

Solids where atoms are bonded by covalent bonds in a continuous network.

molecular solids

Solids comprised of molecules held together by intermolecular forces.

metallic solids

Solids composed of metal atoms held together by metallic bonds.

temperature

A measure of the average kinetic energy of the particles in a substance.

pressure

Caused by gas particles colliding with the container

total pressure

The sum of all partial pressures in a mixture of gases.

partial pressure

The pressure that a single gas in a mixture contributes to the total pressure.

mole fraction

The ratio of the number of moles of a component to the total number of moles in a mixture.

kinetic molecular theory

A theory that explains the behavior of gases in terms of the motion of their particles.

molarity

The concentration of a solution expressed as the number of moles of solute per liter of solution.

heterogeneous mixtures

Mixtures that are not uniform in composition and can be separated easily.

homogeneous mixtures

Mixtures that are uniform in composition and have a consistent appearance.

distillation

A process to separate components of a mixture based that are miscible based on differences in boiling points.

miscible

Describes liquids that can mix in any proportion without separating.

chromatography

A technique for separating mixtures based on differences in their movement through a stationary phase. (polarity, size, specific ions, boiling point, etc)

stationary phase

The phase in chromatography that does not move, used to separate compounds.

mobile phase

The phase in chromatography that moves and carries the sample through the stationary phase.

thin layer chromatography

A chromatography technique using a thin layer of adsorbent on a plate for separation.

column chromatography

A technique where the stationary phase fills a column through which the mobile phase flows.

spectroscopy

The study of the interaction between matter and electromagnetic radiation.

electromagnetic spectrum

The range of all types of electromagnetic radiation. (gamma rays, x-rays, UV, visible light, IR, microwaves, radio waves)

photoelectric effect

The phenomenon where electrons are emitted from a material when it is exposed to light.

spectrophotometry

An analytical method used to measure the intensity of light absorbed by a sample.

beer-lambert law

A linear relationship between absorbance and concentration of an absorbing species.