 |
|
 |
|
 |
|
 |
|
 |
|
 |
|
Chapter 7 Review
Multiple Choice
Identify the letter of the choice that best completes the statement or answers the question.
____ 1. What is the formula for the compound formed by lead(II) ions and chromate ions?
| a. |
PbCrO4 |
c. |
Pb2(CrO4)3 |
| b. |
Pb2CrO4 |
d. |
Pb(CrO4)2 |
____ 2. What is the formula for tin(IV) chromate?
| a. |
Sn(CrO4)4 |
c. |
Sn2(CrO4)4 |
| b. |
Sn2(CrO4)2 |
d. |
Sn(CrO4)2 |
____ 3. What is the formula for barium hydroxide?
| a. |
BaOH |
c. |
Ba(OH)2 |
| b. |
BaOH2 |
d. |
Ba(OH) |
____ 4. Name the compound Zn3(PO4)2.
| a. |
zinc potassium oxide |
c. |
zinc phosphate |
| b. |
trizinc polyoxide |
d. |
zinc phosphite |
____ 5. Name the compound Hg2(NO3)2.
| a. |
mercury(II) nitrate |
c. |
mercury(I) nitrate |
| b. |
dimercury dinitrate |
d. |
mercuric nitrate |
____ 6. Name the compound CuCO3.
| a. |
copper(I) carbonate |
c. |
cuprous carbide |
| b. |
cupric trioxycarbide |
d. |
copper(II) carbonate |
____ 7. Name the compound SiO2.
| a. |
silver oxide |
c. |
silicon dioxide |
| b. |
silicon oxide |
d. |
monosilicon dioxide |
____ 8. Name the compound N2O4.
| a. |
sodium tetroxide |
c. |
nitrous oxide |
| b. |
dinitrogen tetroxide |
d. |
binitrogen oxide |
____ 9. Name the compound SO3.
| a. |
sulfur trioxide |
c. |
selenium trioxide |
| b. |
silver trioxide |
d. |
sodium trioxide |
____ 10. Which compound's name includes the Greek numerical prefixes di- and tri-?
| a. |
Fe2O3 |
c. |
N2O3 |
| b. |
Ca3(PO4)2 |
d. |
Al2S3 |
____ 11. What is the formula for nitrogen trifluoride?
| a. |
NiF3 |
c. |
N3F |
| b. |
NF3 |
d. |
Ni3F |
____ 12. What is the formula for dinitrogen trioxide?
| a. |
Ni2O3 |
c. |
N2O6 |
| b. |
NO3 |
d. |
N2O3 |
____ 13. What is the formula for diphosphorous pentoxide?
| a. |
P2PeO5 |
c. |
P2O4 |
| b. |
PO5 |
d. |
P2O5 |
____ 14. What is the formula for carbon disulfide?
| a. |
CaS2 |
c. |
S2C |
| b. |
CS2 |
d. |
SC2 |
____ 15. The oxidation number of fluorine is
| a. |
always 0. |
| b. |
–1 in all compounds |
| c. |
+1 in all compounds. |
| d. |
equal to the positive charge of all the metal ions in a compound. |
____ 16. What is the oxidation number of oxygen in most compounds?
| a. |
–8 |
c. |
0 |
| b. |
–2 |
d. |
+1 |
____ 17. What is the oxidation number of an uncombined element?
| a. |
–1 |
c. |
+1 |
| b. |
0 |
d. |
8 |
____ 18. What is the oxidation number of hydrogen in most compounds?
| a. |
–1 |
| b. |
0 |
| c. |
+1 |
| d. |
It is equal to the algebraic sum of the oxidation numbers of the nonmetals. |
____ 19. What is the oxidation number of hydrogen in KH?
| a. |
–1 |
c. |
+1 |
| b. |
0 |
d. |
+2 |
____ 20. What is the oxidation number of hydrogen in H2O?
| a. |
0 |
c. |
+2 |
| b. |
+1 |
d. |
+3 |
____ 21. What is the oxidation number of sulfur in SO2?
| a. |
0 |
c. |
+2 |
| b. |
+1 |
d. |
+4 |
____ 22. Name the compound N2O2 using the Stock system.
| a. |
dinitrogen monoxide |
c. |
nitrogen(II) oxide |
| b. |
nitrous oxide |
d. |
nitrogen oxide(II) |
____ 23. Name the compound CCl4 using the Stock system.
| a. |
carbon(IV) chloride |
c. |
carbon chloride |
| b. |
carbon tetrachloride |
d. |
carbon hypochlorite |
____ 24. Name the compound H2O using the Stock system.
| a. |
water |
c. |
hydrogen(I) oxide |
| b. |
hydrogen dioxide |
d. |
hydrogen(II) oxide |
____ 25. Name the compound N2O5 using the Stock system.
| a. |
nitrogen(II) oxide |
c. |
nitrogen(VII) oxide |
| b. |
nitrogen(V) oxide |
d. |
nitrogen pentoxide |
____ 26. Name the compound PBr5 using the Stock system.
| a. |
potassium hexabromide |
c. |
phosphorus(V) bromide |
| b. |
phosphorus(V) pentabromide |
d. |
phosphoric acid |
____ 27. The molar mass of an element is the mass of one
| a. |
atom of the element. |
c. |
gram of the element. |
| b. |
liter of the element. |
d. |
mole of the element. |
____ 28. What is the formula mass of ethyl alcohol, C2H5OH?
| a. |
30.328 amu |
c. |
45.061 amu |
| b. |
33.271 amu |
d. |
46.069 amu |
____ 29. What is the formula mass of (NH4)2SO4?
| a. |
114.09 amu |
c. |
128.06 amu |
| b. |
118.34 amu |
d. |
132.13 amu |
____ 30. The molar mass of MgI2 is
| a. |
the sum of the masses of 1 mol of Mg and 2 mol of I. |
| b. |
the sum of the masses of 1 mol of Mg and 1 mol of I. |
| c. |
the sum of the masses of 2 mol of Mg and 2 mol of I. |
| d. |
impossible to calculate. |
____ 31. The molar mass of LiF is 25.94 g/mol. How many moles of LiF are present in 10.37 g?
| a. |
0.3998 mol |
c. |
2.500 mol |
| b. |
1.333 mol |
d. |
36.32 mol |
____ 32. The molar mass of CS2 is 76.14 g/mol. How many grams of CS2 are present in 10.00 mol?
| a. |
0.13 g |
c. |
10.00 g |
| b. |
7.614 g |
d. |
761.4 g |
____ 33. How many OH– ions are present in 3.00 mol of Ca(OH)2?
| a. |
3.00 |
c. |
3.61 ´ 1024 |
| b. |
6.00 |
d. |
2.06 ´ 1023 |
____ 34. How many Mg2+ ions are found in 1.00 mol of MgO?
| a. |
3.01 ´ 1023 |
c. |
12.04 ´ 1023 |
| b. |
6.02 ´ 1023 |
d. |
6.02 ´ 1025 |
____ 35. If 0.500 mol of Na+ combines with 0.500 mol of Cl– to form NaCl, how many formula units of NaCl are present?
| a. |
3.01 ´ 1023 |
c. |
6.02 ´ 1024 |
| b. |
6.02 ´ 1023 |
d. |
1 |
____ 36. What is the percentage composition of CF4?
| a. |
20% C, 80% F |
c. |
16.8% C, 83.2% F |
| b. |
13.6% C, 86.4% F |
d. |
81% C, 19% F |
____ 37. The percentage composition of sulfur in SO2 is about 50%. What is the percentage of oxygen in this compound?
| a. |
25% |
c. |
75% |
| b. |
50% |
d. |
90% |
____ 38. What is the percentage composition of chlorine in NaCl?
| a. |
35.45% |
c. |
60.7% |
| b. |
50% |
d. |
64.5% |
____ 39. A formula that shows the simplest whole-number ratio of the atoms in a compound is the
| a. |
molecular formula. |
c. |
structural formula. |
| b. |
ideal formula. |
d. |
empirical formula. |
____ 40. What is the empirical formula for a compound that is 43.6% phosphorus and 56.4% oxygen?
| a. |
P3O7 |
c. |
P2O3 |
| b. |
PO3 |
d. |
P2O5 |
____ 41. What is the empirical formula for a compound that is 7.9% Li and 92.1% Br?
| a. |
LiBr |
c. |
LiBr3 |
| b. |
LiBr2 |
d. |
LiBr4 |
____ 42. A compound contains 64 g of O and 4 g of H. What is the empirical formula for this compound?
| a. |
H2O |
c. |
HO2 |
| b. |
H2O2 |
d. |
HO |
____ 43. What is the empirical formula for a compound that is 36.1% Ca and 63.9% Cl?
| a. |
CaCl |
c. |
CaCl2 |
| b. |
Ca2Cl |
d. |
Ca2Cl2 |
____ 44. To find the molecular formula from the empirical formula, one must determine the compound's
| a. |
density. |
c. |
structural formula. |
| b. |
formula mass. |
d. |
crystal lattice. |
____ 45. The empirical formula and the formula mass of a compound are needed to determine the compound's
| a. |
molecular formula. |
c. |
lattice structure. |
| b. |
bond energy. |
d. |
toxicity. |
____ 46. The molecular formula for vitamin C is C6H8O6. What is the empirical formula?
| a. |
CHO |
c. |
C3H4O3 |
| b. |
CH2O |
d. |
C2H4O2 |
____ 47. A compound's empirical formula is N2O5. If the formula mass is 108 amu, what is the molecular formula?
| a. |
N2O5 |
c. |
NO3 |
| b. |
N4O10 |
d. |
N2O4 |
____ 48. A compound's empirical formula is NO2. If the formula mass is 92 amu, what is the molecular formula?
| a. |
NO |
c. |
NO4 |
| b. |
N2O2 |
d. |
N2O4 |
____ 49. A compound's empirical formula is HO. If the formula mass is 34 amu, what is the molecular formula?
| a. |
H2O |
c. |
HO3 |
| b. |
H2O2 |
d. |
H2O3 |
Short Answer
50. Explain the term empirical formula. What is the empirical formula of strontium bromide, SrBr2?
Problem
51. The molar mass of aluminum is 26.98 g/mol and the molar mass of fluorine is 19.00 g/mol. Calculate the molar mass of aluminum trifluoride, AlF3.
52. The molar mass of copper is 63.55 g/mol, the molar mass of sulfur is 32.07 g/mol, and the molar mass of oxygen is 16.00 g/mol. Calculate the molar mass of copper(II) sulfate, CuSO4.
53. The molar mass of iron is 55.85 g/mol, the molar mass of silicon is 28.09 g/mol, and the molar mass of oxygen is 16.00 g/mol. Calculate the molar mass of iron(II) silicate, Fe2SiO4.
54. The molar mass of aluminum is 26.98 g/mol and the molar mass of oxygen is 16.00 g/mol. Determine the molar mass of Al2O3.
