Name
Class
Date
Assessment
Chapter Test B
Chapter: Chemical Formulas and Chemical Compounds
PART I In the space provided, write the letter of the term or phrase that best
completes each statement or best answers each question.
______ 1. Changing a subscript in a correctly written chemical formula will
a. change the electron configuration of that element.
b. change the charges on the other ions in the compound.
c. change the formula so that it no longer represents the same
compound.
d. have no effect on the formula.
______ 2. Using the Stock system of nomenclature, Cr2(SO4)3 is named
a. chromium(II) sulfate.
b. chromic sulfate.
c. dichromium trisulfate.
d. chromium(III) sulfate.
______ 3. In a polyatomic ion, the algebraic sum of the oxidation numbers of all
atoms is equal to
a. 0.
b. 10.
c. the number of atoms in the ion.
d. the charge on the ion.
______ 4. The first part of the name of a binary ionic compound is the
a. cation.
b. polyatomic ion.
c. oxyanion.
d. anion.
______ 5. The empirical formula may not represent the actual composition
of a(n)
a. ionic compound.
b. crystal.
c. salt.
d. molecular compound.
______ 6. The formula for phosphoric acid is
a. HPO4.
b. H(PO4)2.
c. H2PO3.
d. H3PO4.
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Chapter Test
Name
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Chapter Test B, continued
______ 7. The term formula mass can be applied to both ionic compounds and
molecular compounds because
a. ionic compounds exist as individual molecules.
b. not all molecular formulas are empirical formulas.
c. not all formulas represent individual molecules.
d. all molecular formulas are Lewis formulas.
______ 8. To determine the correct molecular formula of a compound from an
empirical formula, one must determine the
a. density.
b. formula mass.
c. structural formula.
d. crystal lattice.
PART II
Write the oxidation number for the given element in the space provided.
9. Sulfur in H2SO4
10. Oxygen in peroxides
11. Magnesium in MgO
12. Silicon in SiCl4
Write the formulas for the following compounds in the space provided.
13. Silicon dioxide
14. Carbon tetriodide
15. Tin(IV) chromate
16. Barium hydroxide
Write the names of the following compounds in the space provided. Use the Stock
system or prefixes, as indicated.
17. PI3, Stock system
18. N2O4, prefixes
19. Fe(NO2)2, Stock system
20. CCl4, prefixes
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Chapter Test
Name
Class
Date
Chapter Test B, continued
21. CO, prefixes
22. CuCO3, Stock system
Write the formulas and give the names of the compounds formed by the following
ions in the space provided.
23. Ca2 and Cl
24. Pb2 and CrO42
25. Al3 and SO42
26. Sn4 and PO43
Name each of the following ions in the space provided.
27. CN
28. O2
29. OH
Write the formulas and indicate the charges for the following ions in the space
provided.
30. sulfide ion
31. copper(I) ion
32. carbonate ion
Write each atom and its oxidation number in the space provided.
33. H2O2
34. CO2
3
35. NH
4
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62
Chapter Test
Name
Class
Date
Chapter Test B, continued
PART III Use the table of atomic masses to answer the following questions. Write
your answer on the line to the left, and show your work in the space
provided.
Element
Symbol
Atomic mass
Element
Symbol
Atomic mass
Aluminum
Al
26.98 amu
Lead
Pb
207.2 amu
Bromine
Br
79.90 amu
Lithium
Li
Carbon
C
12.01 amu
Magnesium
Mg
24.30 amu
Chlorine
Cl
35.45 amu
Manganese
Mn
54.94 amu
Chromium
Cr
52.00 amu
Nitrogen
N
14.01 amu
Copper
Cu
63.55 amu
Oxygen
O
16.00 amu
Fluorine
F
19.00 amu
Sodium
Na
22.99 amu
Hydrogen
H
1.01 amu
Sulfur
S
32.07 amu
6.94 amu
36.
What is the molar mass of tetraethyl lead, Pb(C2H5)4?
37.
What is the formula mass of copper(II) chloride, CuCl2?
38.
What is the percentage composition of CuCl2 by mass?
39.
What is the mass of 0.240 mol glucose, C6H12O6?
40.
What is the empirical formula for a sample of a
compound that contains 259.2 g F and 40.8 g C?
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Chapter Test
Name
Class
Date
Chapter Test B, continued
41.
The empirical formula for a compound is C2H5 and its
formula mass is 58 amu. What is its molecular formula?
42.
A sample of a compound is 80% carbon and 20%
hydrogen by mass. Its formula mass is 30 amu. What is
its molecular formula?
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