GEN CHEM 3rd Quarter

Melting (or freezing) curve - The curve on a phase diagram which represents the transition between the liquid and solid states.

Vaporization (or condensation) curve - The curve on a phase diagram which represents the transition between the gaseous and liquid states.

Sublimation (or deposition) curve - The curve on a phase diagram which represents the transition between the gaseous and solid states.

Triple point - The point on a phase diagram at which the three states of matter coexist, combination of pressure and temperature at which all three phases of matter are at equilibrium.

Critical point - The point in temperature and pressure on a phase diagram where the liquid and gaseous phases of a substance merge together into a single phase. The temperature and pressure corresponding to this are known as the critical temperature and critical pressure.

critical temperature and critical pressure - The temperature and pressure corresponding to the critical point.

Normal melting and boiling points - Melting and boiling points when the pressure is 1 atm.

Liquefied petroleum gas or liquid petroleum gas (LPG or LP gas) - also referred to as simply propane or butane, are flammable mixtures of hydrocarbon gases used as fuel in heating appliances, cooking equipment, and vehicles.

phase diagram - is a graphical representation of the physical states of a substance under different conditions of temperature and pressure.

Phase diagrams - are plots of pressure (usually in atmospheres) versus temperature (usually in degrees Celsius or Kelvin)

green line - divides the solid and liquid phases, and represents melting (solid to liquid) and freezing (liquid to solid) points.

blue line - divides the liquid and gas phases, and represents vaporization (liquid to gas) and condensation.

red line - divides the solid and gas phases, and represents sublimation (solid to gas) and deposition

supercritical fluid - Beyond the temperature of the critical point, the merged single phase

Phase - homogenous part of a system in contact w/ other parts of the system.

Condensed Phases (fluids, solid)

Intramolecular forces - forces that holds atoms together in a molecule.

Intermolecular forces - attractive forces between molecule.

Diffusion - process which a gas, enters a container w/ another gas and two mix to form a uniform mixture.

Effusion - process in which gas through a small hole in its current container into another container

KMT - model word to explain the behavior used of matter. (Kinetic Molecule Theory).

Johannes Van Der Waals (1837-1923) - working on the theory of ideal gases of close recognized the existence of some type of weak force or particles that are very close to each other.

IMF - molecules interact and have a great influence on one another.

Fluid- gas or a liquid, a substance that can flow.

Surface - measure of the elastic force in the surface of a liquid, amount of energy required to Stretch or increase the surface of a liquid by a unit area,

Capillary Action - tendency of a liquior to rise in narrow tubes or to be drawn into small openings.

Viscosity - measure of fluid resistance to flow

Vapor - gaseous substance that exist naturally as a liquid or solid of normal temperature.

Vaporization - change of phase from liquid to vapor (gaseous phase).

vapor pressure of a liquid - equilibrium pressure of vapor above its liquid, pressure exerted by the vapor above the surface of the liquid in a closed temperature.

Boiling Point- the boiling point of a liquid when the external pressure is 1atm is called the normal boiling point.

Molar Heat of Vaporization (AH Vap) - energy required to vaporize, 1 mole of a liquid at given temperature.

Ethyl Alcohol - water have very low vapor pressures, both liquid have the strong dipole-dipole interaction called hydrogen bonding.

Acetone - popular but does not have H-bonding, it's vapor pressure is of Intermediate value.

Pentane - nonpolar substance, and its vapor pressure is high compared to those of water and ethyl alcohol.

Crystal or crystalline solid - solid material whose components, such as atom molecules or ions

Ion - atom or group of atoms that has a net positive or negative charge.

ionic Crystal - solid that consists of positively and negatively charge ion held together by electrostatic forces.

Electrostatic bonding - attraction between oppositively charged ions in a chemical compound.

Ionic bond - electrostatic force that hold ions together in an ionic compound.

Network solid or covalent - network crystal solid that may be a chemical compound in which atom are bonded by covalent bond.

Molecular Crystal - solid composed of molecules held together by Vander Waals forces.

Covalent bond - one or more pairs of electron are shared by two atoms.

Nature of solute and Solvent - general rule of solutions -like dissolve like".

Polar liquids - dissolve polar compound and nonpolar liquids dissolve nonpolar compounds.

Polar Compound - compound either ionic or Covalent, that have a permanent dipole moment.

Nonpolar Compound - covalent compound have no permanent dipole moment.

Saturated Solution - there is maximum amount of solute that can be dissolved in a given amount of solvent in a given temperature.

Super Saturated - more than the maximum amount of salute.

Unsaturated - less than maximum amount of solute.