1. Calculate the molar mass for the following compounds
a. silver nitrate
b. chromium (II) perchlorate
c. lead (II) carbonate
d. nickel (II) hydroxide
e. sodium sulfate
2. Perform the following conversions
a. 0.75 g silver nitrate  moles
b. 1.50 moles lead (II) carbonate  grams
c. 0.256 g nickel (II) hydroxide  atoms
d. 1.29x1018 atoms chromium (II) perchlorate  moles
e. 0.0259 g of sodium sulfate  moles
3. Convert 25.62 grams of hydrophosphoric acid to moles.
4. Calculate the % of oxygen in strontium phosphate
Calculate the % of potassium in potassium oxide
Calculate the percent of nitrogen in magnesium nitride.
5. Find the empirical and molecular of the compound given below.
1. 56.15 g C, 9.43 g H, 74.81 g O, 13.11 g N, and 21.49 g Na. ; molar mass = 591.2 amu
6a. The molecular formula of a compound is P6S4. What is the empirical formula of this
compound?
b. The molecular formula of a compound is C4H4. Determine the empirical formula of this
compound.
7. What is the molecular formula of a compound that has an empirical formula of C2H7 and a
molar mass of 93 g/mol.
8. Calculate the empirical formula for a compound that is found to contain 85.64% carbon and
14.36% hydrogen by mass.
9. Draw the following structures
Determine the shape
Determine the polarity
NH4+
CO32-
Carbon dioxide
Dihydrogen monoxide
Hydrofluoric acid
Nitrogen trihydride
Carbon tetrachloride
10. Be able to locate alkali metals, alkaline earth metals, transition metals, nonmetals, halogens,
and noble gases on the periodic table
11. Determine the oxidation number (charge) for the following:
Alkali metals
Alkaline earth metals
Halogens
Noble gases
12. Determine protons, neutrons, and electrons for the following:
Chlorine – 37
Copper – 66
54
Cr
14
N
31 3-
P
13. Define ionic bond.
14. Define covalent bond.