Chemistry Unit 5 - PBOM

Absolute Zero

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Lowest possible temperature

Alloy

Homogeneous mix containing least one metal

Avogadro's Law

Gases at same temp, pressure & vol have same # of molecules or particles

Bolling Point

Temp which liquid undergoes phase change from liquid to gas

Bolling Point Elevation

BP of a solution is higher than BP of pure solvent

Colloid

A heterogeneous mix made of tiny particles suspended in another material

Compound

Two or more elements chemically combined

Concentrated

Having relatively large amount of substance present in a unit amount of mixture

Concentration

Measure of the amount of solute present in a unit amount of mixture

Cooling Curve

Diagram showing phase changes for a substance as it loses energy gas phase all the way to solid phase

Deposition

Phase change from gas to solid

Element

Pure substance composed of one species of atoms

Energy

The capacity to do work

Evaporation

Phase change from liquid to gas

Extensive (property)

Physical property that depends on sample size or amount

Freezing Point Depression

The freezing point/melting point of solution is lower than the freezing point/melting point of pure solvent

Heat

From of energy measured in Joules (J)

Heat of Fusion

Energy required to change 1g of a substance from solid to liquid

Heat of Vaporization

Energy required to change 1g of a substance from liquid to gas

Heat Transfer

Energy transferred from a substance with more (hotter) to a substance with less (cooler)

Heating Curve

Diagram showing phase change for a substance as it gains energy goes solid phase to gas phase

Heterogeneous

Matter consisting of more than one pure substance

Homogeneous

A sample of matter consisting of more than one pure substance that do not vary within sample

Insoluble

Refers to a substance that does not dissolve in a solvent to any significant degree

Intensive (property)

Physical property that does NOT depend on sample size or amount

Kinetic Energy

Energy of motion energy; associated with a change in temp

Kinetic Molecular Theroy (KMT)

model used to explain behavior of gases in terms of the motion of their particles

Lattice

The unique crystal structure associated with any given solid

Matter

Anything having mass and takes up space

Melting Point

Temp at which phase change between solid and liquid occurs

Miscible

Two liquids are considered “miscible” or sizable if shaking them results in single liquid phase

Mixture

Two or more pure substances PHYSICALLY combined

Molarity

Measure of concentration: M = moles of solute/liters of solution

Normal Bolling Point

Temp at which a phase change between liquid and gas occurs at 1 atm or 101.3 kPa; Vapor pressure = atmospheric pressure

Percent Composition (mass or vol)

% comp = (part/whole) ×100

Sublimation

Phase change from solid to gas

Suspension

A heterogeneous mixture in which relatively large particles are suspended in

Temperature

Measure of average kinetic energy

Tyndall Effect

Light passing through a colloid is scattered by suspended particles (light beam becomes clearly visible)

Vapor Pressure

Upward pressure of a vapor in equilibrium with its liquid