Honors Chemistry Second Semester Final Reveiw

Stoichiometry

The study of quantitative relationships in chemical equations.

Mole Ratio

Ratio between the number of moles of any two substances in a balanced chemical equation.

Limiting Reactant

“Limits” the amount of product that can be produced.

Percent Yield

Measures the efficiency of a chemical equation.

Kinetic molecular theory

Defines the behavior of ideal gasses.

Properties of gasses

Mass, may be compressed, fills containers, diffusion, and pressure

Charles’ Law

Volume, temperature, and directly proportional

Boyle’s Law

Pressure, volume, and indirectly proportional

Gay - Lussac’s Law

Pressure, temperature, and directly proportional

Mixture

A combination of two or more substances in which each pore substance retains its individual chemical properties.

Heterogeneous Mixture

Does not have a uniform composition and in which the individual substances remain distinct.

Homogenous Mixture

Has a constant composition throughout.

Suspension

Mixtures containing particles that sifil out if left undisturbed.

Colloid

Mixtures of intermediate sized particles (between 1nm and 1000nm) and do not settle.

Tyndall Effect

Disperse colloid particles scatter light.

Soluble

A substance that dissolves in a solvent.

Insoluble

A substance that doesn't dissolve.

Miscible

Two liquids that dissolve into one another in any proportion.

Immiscible

Two liquids that can be mixed but separate shortly after.

Concentration

Measurement of how much solute is dissolved in a specific amount of solvent or solution.

Molarity

Number of moles of solute dissolved per liter of solution (M)

Molality

Volume of a solution changes with temperature altering the molality, masses do not change so sometimes it's more useful to use mass.

Forces of Attraction

Attractive forces within and between particles hold these particles together.

Dispersion Forces

Weak forces that result from temporary shifts in density of electrons in electron clouds. they exist between particles.

Dipole

A region of the atom with a charge.

Dipole - Dipole Forces

Attractions between oppositely charged regions of polar molecules. The difference in electronegativity causes one side to hug electrons closer.

Hydrogen Bonds

Special Dipole - Dipole attractions that occur between molecules that contain a Hydrogen atom directly bonded to a small, highly electronegative atom with at least one lone pair of electrons. The strongest force.

Solvation

Interaction of a solvent with the dissolved solute.

Dissociation

The process of an ionic solid separating into its individual ions.

Hydration

When solvent is H2O.

Solubility

The amount of solute that dissociates in a given solvent under specific conditions.

Saturated

Contains the maximum amount of solute possible at a given T and P

Unsaturated

Contains less the maximum (at a given T and P)

Supersaturated

Contains more than the maximum amount possible (at a given T and P)

Colligative Properties

A property that depends on the concentration of the solute particles, but is independent of their nature.

Semipermeable

Material that only allows certain substances to pass through.

Osmosis

Movement of solvent from low concentration of solute to high.

Osmotic Pressure

Pressure required to move solvent (equalizes the amount of water).

Vapor Pressure Reduction

Results when some molecules of pure liquids leave the liquid surface and enter the gaseous state (vaporization).

Boiling Point Elevation

Solvation forces prevent solvent from gaining sufficient energy to vaporize.

Freezing Point Depression

Solvation forces prevent solvent particles from loosing too much energy.

Thermochemistry

Energy and chemical change. The study of heat (energy) changes that occur during chemical reactions and phase changes.

Energy

The ability to do work or produce heat.

Potential Energy

Energy due to the composition or position of an object.

Kinetic Energy

Energy of motion.

Law of Conservation of Energy

In any chemical reactions or physical process, energy can be converted form one form to another, but its neither created or destroyed.