SEMESTER
FINAL REVIEW!!!
Nomenclature and Bonding
Write the formula for the following compounds: REMEMBER THAT THEY MUST BE
BALANCED
1. carbonic acid
3. nitrogen monoxide
5. hydrosulfuric acid
2. calcium phosphide
4. aluminum sulfate
6. lead (III) oxide
Name for the following compound formulas. REMEMBER THAT THEY ARE NOT PROPER
NOUNS…DO NOT CAPATALIZE THEM!!!
7. P2O3
8. CaBr2
9. Mg(OH)2
10. N2O3
11. HF
12. Cu2S
13. HNO2
Reactions and Equations
Create BALANCED Equations with BALANCED Formulas.
1.
Ba I2
+
FrCl
2.
K(ClO3)
3.
MgS
4.
Al
5.
Au2O3
6.
Ba(HCO3)2



+
N2
+

Li


7.
Pb (IV)
+
8.
Al +
O2
9.
AgI +
SnS2 
10.
Li(HCO3) 
11.
Si(ClO3)4 
12.
CuCl2
+
O2


Al

Match the type of reaction with the following balanced equations, then, explain WHY.
a. synthesis
b. decomposition
c. single replacement
d. double replacement
e. combustion
13. 2 FeO  2 Fe + O2
16. CaCO3 + 2 KNO3  Ca(NO3) + K2CO3
14. SrO + 2K  K2O + Sr
17. Fe2O3 + 3 CuS  3 CuO + Fe2S3
15. Be + F2  BeF2
18. C2H8 + 8 O2  2 CO2 + 4 H2O
Write the word equations for each of the following reactions (HINT: BALANCE FORMULAS
AND EQUATIONS)
19.
NaCl + BeF2  NaF + BeCl2
21.
Fe + O2  Fe2O3
20.
Mg + Mn2O3  MgO + Mn
22.
KClO3  KCl + O2
Write the balanced formula equations for the following reactions (HINT: BALANCE
FORMULAS AND EQUATIONS)
23. sodium hydroxide + sulfuric acid yields sodium sulfate + water
24. zinc + sulfuric acid yields zinc sulfate + hydrogen
25. aluminum + hydrochloric acid yields aluminum chloride + hydrogen
26. sodium bicarbonate + acetic acid yields sodium acetate + water + carbon dioxide
Stoichiometry
1. Find the MOLAR RATIOS between the identified compounds. (Think about what you
should do first)
a. Cl2 + KI  KCl + I2
What is the molar ratio of chlorine to iodine?
b. BaCl2 + Na2SO4  NaCl + BaSO4
What is the molar ratio of sodium chloride to sodium sulfate?
c. Calcium plus aluminum chloride yields calcium chloride plus aluminum
What is the molar ratio of calcium to aluminum chloride?
d. Silver nitrate plus potassium chromate yields silver chromate plus potassium nitrate.
What is the molar ratio of potassium chromate to silver chromate?
2. CONVERT as the problem asks…
a. 4.50 moles of O2 into grams
b. 22.44 grams of HgO into moles
c. 2.37 moles of barium chromate into grams
d. 17.37 grams of iron (III) sulfide into moles
3. Complete the STOICHIOMETRY problems (show all your work!!!!)
a. You start with 26.50g of HCl, how many liters of AlCl3 do you have?
Al + HCl  AlCl3 + H2
b. How many grams of magnesium are needed to produce 150 grams of hydrogen?
Mg + HCl  MgCl2 + H2
c. What mass of Fe reacted if 6.00 moles of H2O were reacted?
H2O + Fe(III)  H2 + Fe2O3
d. If 4.5 moles of potassium bromide react, how many moles of potassium chloride are produced?
KBr + Cl2  KCl + Br2
4. Finish the LIMITING REAGENT Problems. Don’t forget your limiting reagent determines
the max amount!
a. If 5.20 moles of copper and 5.30 moles of silver nitrate are available to react, what is the limiting
reagent?
Cu + AgNO3  Cu(NO3)2 + Ag
b. What is the maximum mass of H2S which can be formed from these reactants?
Al2S3 + H2O  Al(OH)3 + H2S
c. How many grams of calcium hydroxide will be formed in this reaction when 3.33 g of calcium oxide
and 7.77 g of water are available to react? Then, identify the limiting and excess reactants.
CaO+ H2O  Ca(OH)2
Solutions
1. Define the following vocabulary terms.
A. soluble
C. aqueous
E. concentration
B. insoluble
D. saturated
F. diluted
G. molarity
H. molality
I. supersaturated
J. suspension
2. SOLUBILITY: Identify if the compound is soluble in water or insoluble in water.
a. PbCl2
b. K2S
c. Na2CO3
d. Pb(C2H3O2)2
e. Li2O
f. AgI
g. (NH4)2S
3. MOLARITY: Use your knowledge of stoichiometry and molarity knowledge to complete all
the following problems.
a. What is the molarity of a solution if 2.0L of solution contain 25 g of potassium permanganate?
b. What is the volume, in liters, of silver nitrate will be made for a 1.0 M solution, with 85g of solute?
c. What mass of iron (II) sulfate is needed to make 200mL of a 0.25M solution?
4. MOLALITY: Use your knowledge of stoichiometry and molality knowledge to complete all
the following problems.
a. What mass of water is needed to prepare 1.25m solution with 50.0 grams of sucrose, C12H22O11
dissolved in it.
b. What mass of water is required to dissolve 175g KNO3 to produce 2.25m solution?
c. What is the molality of a solution of 13.7 g sodium chloride dissolved in 500.0g of water?
Acids and Bases
Answer the following problems in complete sentences. Be detailed, remember this quiz was tough!
1. Compare and contrast acid and base properties with a Venn diagram.
2. What is the pH scale for acids, neutral, and bases?
3. List three strong acids, what makes them strong?
4. List three weak acids, why are they weak?
5. List three strong bases, what makes them strong?
6. List three weak bases, why are they weak?
7. Describe how litmus paper reacts with an acid and base.
8. Define a cation.
9. Define an anion.
10. List five properties of an acid.
11. List fiveproperties of a base.
12. What acid is manufactured in the largest quantity?
13. What acid is used to make fertilizers and detergents and is a flavoring agent in beverages?
14. What acid is used mainly in the manufacture of explosives, rubber, plastics, dyes, and drugs?
15. What acid is produced in the stomach?
16. What acid is found in vinegar?
17. What is titration?
18. Define neutralization and include the word formula for the reaction.
19. What is the difference between equivalence point and end point? How are they related?
20. What unknown quantity can be calculated after performing titration?
21. Which quantity is directly measured in titration?
Gas Laws
1. What is the conversation of OC to K?
2. What does STP stand for? What are the values for STP?
1. List the four variables of gas laws.
3. Complete the following for our laws
i. Give the law’s formula
ii. Identify the constant(s) for the law
iii. Explain how the variables are proportional (i.e. temperature goes up = volume goes up)
a. Boyle’s Law
b. Charles’s Law
c. Gay-Lussac’s Law
d. Combined Gas Law
3. Do the following problems to practice for your test.
Remember:
 2 places after the decimal for the final answer! UNITS!!!!
 Do NOT round until the very final answer (show your rounding step)
 Temperature HAS to be in Kelvin
a. The temperature inside my refrigerator is about 30 Celsius. If I place a balloon in my fridge that
initially has a temperature of 290 C and a volume of 0.7 liters, what will be the volume of the balloon
when it is fully cooled by my refrigerator?
b. A gas is held at a pressure of 700mm Hg inside a syringe. The plunger is pushed down to read 7
mL. What is the volume if the pressure is increased to 800 mm Hg and the temperature remains
constant?
c. A toy rocket launches with 3.5 liters of fuel under a pressure of 1.3 atmospheres, and a temperature
of 278 K. If the temperature on its way up is only 200 K, what is the volume when the pressure
decreases to 0.8 atm?
d. Seven liters of a gas are measured under standard conditions. What temperature would be needed
to expand the gas to 11 liters, if the pressure remains the same throughout?
e. A gas is collected at standard temperature and standard pressure. What is the new pressure in
atmosphere, if the new temperature is 300 K?
f. Fluorine gas is under a pressure of 763 torr and takes up a space of 1985 milliliters. What pressure
would result if the space shrinks to 2 liters and temperature remains constant?
g. Four liters of neon are registered at 232 K and 925 mm Hg. The following day this same volume is
registered at 250 K. What is the pressure?
h. A large balloon holds 8 liters of hydrogen and is under a pressure of 580 torr and a temperature of
126 K. The pressure on the balloon is increased to 600 torr, and the volume decreases to 3 liters.
What is the new temperature?