I Chemical Equations (Ch 4)

A) Balancing

B) Balancing combustion reactions

C) Ions in aquous soln.
 

1) Solubility rules (Chart given on test)

2) Acids and bases

• examples of strong acids and bases

D) Classification by reaction type & will a reaction occur

a) combination
b) decomposition
c) single displacement

• Activity series
• oxidation numbers
• what is oxidized, what is reduced

• formation of a solid
• formation of a gas
• formation of water
E) endo vs exothermic
F) molecular equations, total ionic and net ionic equations

How much of the reagents do we need? How much of the products do we get?

 
A) Micro vs the macroscopic world.
B)Formula wt (a conversion factor)
C) The mole
D) % yield
E) If given a certain amount of A, how much P is produced?  If given a certain amount of A, How much B is used up?
F) limiting reagent
G) Solutions and concentration

• Molarity
1. Solution from a solid.
2. Dilutions (Going from more concentrated to less concentrated.)
3. Titrations - Finding the concentration of a solution.
4. equivalence point- The point at which stochiometrically equivalent amounts of the two reactants have been mixed.
5. pH a method for measuring the acidity of the solution; the amount of H+/ H3O+ in solution.

H) Stochiometry of reactions in aquous solutions.

III Energy

• Specific heat
• Heats of fusion and heats of vaporzation (p272, fig 6.9)
• enthalpy and heats of reactions (energy diagrams)
• Hess's Law
• Heats of formation
• Bond energies
• calorimetry