General instructions: all math problems require work – complete
setups labeled with units and attention paid to significant figures!
Chapter One: Chemical Foundations
1. An ancient cylindrical gold coin is 2.2 cm in diameter and 3.0 mm thick. If the density of
gold is 19.3 g/cm3, what is the mass of the coin in grams? Assuming the price of gold is
$410 per troy ounce, how much is the gold in the coin worth? (1 troy ounce = 31.10
2. The density of a solution of sulfuric acid is 1.285 g/cm3 and it is 38.08% (by weight)
acid. How many milliliter of the acid solution do you need to supply 125 grams of
3. Copper has a density of 8.94 g/cm3. If a factory has an ingot of copper with a mass of
125 pounds and the ingot is drawn into a wire with a diameter of 9.50 mm, how many
feet of wire can be produced? (454 grams = 1 pound)
Chapter Two: Atoms, Molecules, and Ions
Complete the following chart:
Symbol # protons # neutrons # electrons Net charge
20 20 2+
23 28 20
35 44 36
15 16 3-
Refresh your chemical nomenclature. When a formula has been given, write the name.
When the name has been given, write a balanced formula.
Metal and Nonmetal – a salt
NaBr _____________________________ CdS _____________________________
Zn3N2 _____________________________ SrCl2 _____________________________
CuCl _____________________________ Ag2O _____________________________
AlI3 _____________________________ FeO _____________________________
Magnesium phosphide ___________ potassium nitride ___________
Lead(IV) sulfide ___________ nickel(III) chloride ___________
SiO2 _____________________________ BF3 _____________________________
N2O5 _____________________________ AsBr5 _____________________________
Sulfur hexafluoride ___________ tetraphosphorus heptoxide ___________
Carbon tetrachloride ___________ diphosphorus pentoxide ___________
Binary Acids – you’ll get to these in a bit
Metal Cation (or ammonium) and a Polyatomic Ion
K2SO4 ___________________________ Ag2CrO4____________________________
Ca(OH)2 ___________________________ Zn(ClO3)2___________________________
Al2(S2O3)3 ___________________________ Cu2CO3 ____________________________
Sn(SCN)4 ___________________________ Li3PO4 _____________________________
KMnO4 ___________________________ NaClO______________________________
magnesium dichromate _______________ ammonium carbonate __________________
barium oxalate _______________ lead(II) nitrite __________________
zinc phosphate _______________ tin(II) cyanide __________________
cobalt(III) sulfite _______________ aluminum acetate __________________
Oxyacids – see next section
Acids are named based on their anion ending
-IC FROM –ATE
-OUS FROM –ITE
HYDRO-, -IC , -IDE
Name of Acid Formula of Acid Name of Anion
hydrochloric acid HCl chloride
sulfuric acid H2SO4 sulfate
Chapter Three: Stoichiometry
Write, complete and balance equations for the following reactions:
1. Diphosphorus trioxide is formed from the direct combination of its elements.
2. Aluminum replaces hydrogen when the metal is placed in hydrochloric acid.
3. Barium hydroxide solution is neutralized with sulfuric acid.
4. Propane, C3H8, burns in air to produce carbon dioxide and water.
5. Ammonium nitrate may be decomposed into nitrogen and water.
6. Barium carbonate precipitates when solutions of barium chloride and ammonium carbonate are
7. Ammonium sulfate is the only product of the reaction between ammonia (NH3) and sulfuric acid.
8. Potassium chlorate decomposes into potassium chloride and oxygen.
9. Zinc replaces lead when it reacts with lead(II) nitrate solution.
10. Lithium oxide reacts with water to form lithium hydroxide solution.
11. Carbon dioxide and water are two of the three products of a reaction between magnesium
carbonate and hydrochloric acid.
12. Carbon disulfide is oxidized to produce both carbon dioxide and sulfur dioxide.
13. Butanal, C3H7CHO, is burned completely in air.
1. Magnesium is commonly extracted from seawater. Magnesium-24 is its most abundant isotope
(78.70%); its exact mass is 23.985 amu. If the atomic weight of magnesium is 24.305 amu, what
are the relative abundances of magnesium-25 (mass of 24.986 amu) and magnesium-26 (mass of
2. The Statue of Liberty is made up of 2.00 X 105 pounds of copper sheets bolted to an iron
framework. How many atoms of copper make up the fair lady of the New York harbor?
3. Monosodium glutamate, MSG, is a common food additive that serves as a flavor enhancer. Its
formula is HOOCCH2CH2CH(NH2)COONa.
(a) Calculate the molar mass of MSG.
(b) How many moles are there in 2.00 g (about 1 teaspoonful) of MSG?
(c) How many atoms of O are there in 2.00 g (about 1 teaspoonful) of MSG?
4. The most common beryllium-containing mineral is beryl, which occurs mostly as large blue-
green crystals with the formula Be3Al2(SiO3)6.
(a) What is the molar mass of beryl?
(b) How many moles are there in a 0.25 g crystal?
(c) How many grams of beryl must you have in order to have 10. g of beryllium?
5. A major oil company has used a gasoline additive called MMT to boost the octane rating of its
gasoline. What is the empirical formula of MMT if it is 49.6% C, 3.20% H, 22.0% O, and
6. Vanillin is a common flavoring agent. It has a molar mass of 152 g/mol and is 63.15% carbon,
and 5.20 % hydrogen. The remainder is oxygen. Determine the molecular formula of vanillin.
7. Over the years the thermite reaction has been used for welding railroad rails, in incendiary
bombs, and to ignite solid fuel rocket motors. The reaction is
Fe 2 O 3 (s) 2Al(s) 2Fe(l) Al 2 O 3 (s)
(a) What masses of iron(III) oxide and aluminum must be used to produce 15.0 g iron?
(b) What is the maximum mass of aluminum oxide that could be produced?
8. Calculate the masses of Cr2O3, N2, and H2O produced from the decomposition of 10.8 g
9. Mercury and bromine will react with each other to produced mercury(II) bromide.
Hg(l) Br2 (l) HgBr 2 (s)
(a) What mass of mercury(II) bromide can be produced from the reaction of 10.0 g Hg and 9.00
g Br2? What mass of which reactant is left unreacted?
(b) What mass of mercury(II) bromide can be produced from the reaction of 5.00 mL of mercury
(density 13.6 g/mL) and 5.00 mL (density 3.10 g/mL)?