C.W. BAKER HIGH SCHOOL

Core V Review

Prepared by K. Schmidt/M. Foster

 

 

I.Matter- anything that has mass and volume

 

A.   Properties = characteristics

1.     physical - can be described without changing identity of material

                         a.extensive – depend on sample size

                           b.intensive – independent of sample size

2.     chemical – changes the identity of material

 

B.    States (Phases) of Matter

1.     Solid (vibrational motion)

a.      amorphorous – No geometric patterns (glass, wax)

b.     crystalline – regular geometric patterns

 

2.     Liquid (vibrational and rotational motion)

a.      vapor pressure – when liquids evaporate in a closed system

b.     boiling point – when atmospheric pressure = vapor pressure

c.     “Normal” Boiling Point – boiling point at 1 atm pressure.

 

3.     Gas ( vibrational, rotational, and translational motion)

a.      maximum entropy

b.     maximum potential energy

c.     weakest bonds (Van der Waals)

 

C.   Phase Changes

 

 

        D. Classification

1.     Elements- CAN NOT be broken down!

2.     Compounds- CAN be broken down chemically

3.     Mixtures – physical combinations of elements or compounds

a.      heterogeneous  – different properties throughout

Examples:

 

b.     homogeneous -same properties throughout (SOLUTIONS)

Examples:

 

II. Solution Chemistry

 

A.   Solubility- determines how much solute will dissolve in a given amount of solvent.

1.    “like dissolves like” – polar solvents dissolve polar solutes, non-polar solvents dissolve non-polar solutes.

2.             solubility curves – region above the curve is supersaturated, the curve is saturated, region below the curves is unsaturated (see reference table G)

 

B.    Concentration units

 

Molarity  =     moles of solute

                     Liters of solution

 

C.   Colligative Properties – adding a solute to a pure solvent will:

1.     elevate the boiling point

2.     lower the freezing point

3.     lower the vapor pressure

4.     electrolytic solutes (i.e. salts) will have a greater effect on collegative properties than nonelectrolytic solutes like sugar.

 

   III. Energy

 

          A. Forms

1.     Kinetic – motion, KE = ½ mv2

a.     Temperature measures AVE. kinetic energy!!!!!

2.     Potential – positional, stored

3.     Heat – always flows from high temp to low temp.

 

 

          B. Calorimetry

 

                   Heat =(mass of water)(change of temp)(specific heat)

                    Q = m x  DT  x  C

 

IV. Gases

 

        A. Kinetic Molecular Theory (Ideal Gas Model)

               - continuous motion

               - volume is negligible

               - NO BONDS!

     - collision theory

 

          B. Boyles Law – as pressure increases, volume decreases (constant T)

                   PV = constant

 

C. Charles Law – as temperature increases, volume increases (constant P)

V  = constant

                   T

 

D.   Combined Gas Law

          P1V1   =   P2V2

                      T1          T2

 

E.    Daltons Law

The sum of the partial pressures of a gas mixture is equal to the total pressure of the mixture.

 

F.    Avogadros Law

Equal volumes of gases under the same temperature and pressure contain the same number of particles.

 

At STP, 1 mole of a gas = 22.4 liters