Naming Compounds, Writing Formulas, and the Mole Concept Review Sheet
Student should be able to:
1. Calculate the average atomic mass of an element given the percent abundance
and atomic mass of its isotopes.
2. Give the atomic number, mass number, number of electrons, number of protons,
and number of neutrons in the most abundant isotope of any element using the
periodic table.
3. Assign oxidation numbers to representative elements based on their location in
the periodic table. Remember, oxidation numbers are real charges on ions or
partial charges on atoms in molecules.
4. Locate metals, nonmetals and metalloids on the periodic table (make sure you
know which elements along the staircase are metalloids!).
5. Know and use names, formulas, and oxidation numbers of selected polyatomic
ions (the 12 you have memorized) in predicting formulas of stable ionic
compounds.
6. Predict formulas of stable ionic compounds using subscript numbers to indicate
how many of each kind of atom is needed to give each compound a net charge
of zero.
7. Write the names for ionic compounds from the formulas.
8. Write names and formulas of hydrates.
9. Write names and formulas for binary and tertiary acids.
10. Write names and formulas of covalent compounds. Know prefixes for 1-10.
11. Explain the concept of a mole. (How would you explain a mole to a friend?)
12. Differentiate between all the types of representative particles (formula units,
molecules, atoms, ions).
13. Calculate molar mass of any element or compound.
14. Calculate numerical relationships between mass, number of molecules, moles
and volume of gases (at STP) [you will NOT have your mole map].
15. Calculate the mass percent (percent composition) of a compound given its
formula.
16. Calculate the percent water in a hydrate given the formula.
17. Calculate the empirical formula of a hydrate from experimental data.
18. Determine the empirical and molecular formulas of compounds given percent
composition data or the gram analysis data from a lab.
19. Know which elements exist diatomically in nature (this is so you can calculate
correctly the molar masses of these elements).
Look over ALL notes taken in class and all homework assignments.
Review the following sections of your textbook. Be sure that you understand all
words in bold print. Section 4.3 (pp 110-118), Section 6.1 (pp 155-160),
Chapter 9 (all except pages 274-275), Chapter 10 (all)
Problems: Work out on a separate sheet of paper (SHOW ALL WORK!!)
1. Name the representative particle (atom, molecule or formula unit) of each
substance.
a. oxygen gas b. sodium sulfide
c. sulfur dioxide
d. potassium
2. Find the number of atoms present in 227.0 g of chlorine gas.
3. Find the mass, in grams, of 5.00 x 1023 molecules of fluorine.
4. At STP, how many liters does 364 g of argon occupy?
5. Find the number of representative particles in each substance.
a. 3.0 moles Sn
b. 0.40 moles KCl
c. 7.50 moles SO2
6. Calculate the molar mass of each of the following:
a. H3PO4
b. Bromine
c. (NH4)2SO4
7. How many moles in:
a. 937 g Ca(C2H3O2)2
b. 79.3 g of chlorine
8. Find the mass of:
a. 5.60 moles NaOH
b. 14.4 moles of fluorine
9. Calculate the volume of the following at STP:
a. 1.20 moles oxygen
b. 0.44 moles C2H6
10. Find each of the following quantities
a. The volume, in liters, of 835 g of SO3 at STP
b. The mass, in grams, of 1 molecule of aspirin (C9H8O4)
c. The number of atoms in 5.78 moles
11. What is the percent composition of calcium bromide?
12. A compound is found to have a molar mass of 42.08 grams and to be composed of
85.64% carbon and 14.35% hydrogen by mass. What are the empirical and
molecular formulas of the compound?
13. A sample of a compound analyzed in a chemistry laboratory consists of 5.34 g of
carbon, 0.42 g of hydrogen, and 47.08 g of chlorine. What is the percent
composition of this compound?
14. A compound called hydrazine is made up of nitrogen and hydrogen. If a 64 gram
sample of hydrazine contains 56 g of nitrogen and the rest is hydrogen, find:
a. The empirical formula of hydrazine
b. If the molar mass of hydrazine is 64.12 g/mole, what is its molecular
formula?
15. Find the mass percentage of water in ZnSO47H2O. Name this hydrate.
16. Page 117, #23 and 24
17. Give the number of protons, neutrons, electrons in Al+3, U-236, and S-2.
Name and classify the following:
a. CuCl
b. N2O3
c. KC2H3O2
g. CuSO45H2O
h. CCl4 i. (NH4)3(PO4)
d. H2SO4
j. Fe3P2
e. H2SO3
f. H2S
k. Na2CO310H2O
Write the formulas for the following compounds and classify them:
a. phosphorus tribromide
b. zinc hydroxide
c. phosphoric acid d. aluminum oxide
e. acetic acid
f. sulfur hexafluoride
g. magnesium sulfate heptahydrate
h. nitrous acid
i. hydrophosphoric acid
j. tin (IV) sulfate
k. lead (II) oxide