Module 6 Defintions

Amorphous solids

Solids in which the particles are arranged in a random fashion.

Colligative properties

Physical properties of solvents that depend on the concentration of the solute and the identity of the solvent but not on the identity of the solute.

Colloids

Heterogeneous mixtures that appear to be homogeneous one-phase mixtures, composed of particles too small to be seen with the naked eye.

Condensation

The process of gas being converted to liquid.

Critical point

The temperature above which a substance cannot exist in the liquid phase.

Critical pressure

The lowest pressure required for the substance to exist as a liquid at the critical point.

Crystalline solids

Solids in which the particles are arranged in orderly, repeating geometric patterns.

Electrolytes

Ionic or very polar compounds that dissolve to form solutions of ions which conduct an electric current.

Fluids

Substances like liquids and gases that have no fixed shape and can flow.

Ionization

The splitting of molecules to form ions.

Molality

A term which expresses concentration in moles of solute present per kilogram of solvent.

Molarity

A term which expresses concentration in moles of solute present per liter of solution.

Nonelectrolytes

Compounds that dissolve to form solutions of molecules which do not conduct an electric current.

Phase

Any state of matter such as solid, liquid, or gas.

Strong electrolytes

Solutes that ionize completely.

Sublimation

The conversion of a solid directly to the gas state.

Surface tension

The force that causes a liquid in contact with a gas to assume the least amount of surface area, acting like a thin elastic sheet.

Triple point

The temperature and pressure at which solid, liquid, and gas phases can coexist.

Vapor pressure

Pressure exerted by vapor molecules above a liquid.

Weak electrolytes

Solutes that only partially ionize.