Chemistry Chapter 7 Test
Multiple Choice
Identify the choice that best completes the statement or answers the question.
____
1. A chemical formula includes the symbols of the elements in the compound and subscripts that indicate
a. atomic mass of each element.
b. number of atoms or ions of each element that are combined in the compound.
c. formula mass.
d. charges on the elements or ions.
____
2. A chemical formula for a molecular compound represents the composition of
a. a molecule.
c. the ions that make up the compound.
b. an atom.
d. the crystal lattice.
____
3. How many atoms of fluorine are present in a molecule of carbon tetrafluoride, CF4?
a. 1
c. 4
b. 2
d. 5
____
4. The formula for carbon dioxide, CO2, can represent
a. one molecule of carbon dioxide.
b. 1 mol of carbon dioxide molecules.
c. the combination of 1 atom of carbon and 2 atoms of oxygen.
d. all of the above.
____
5. What is the formula for zinc(II) fluoride?
a. ZnF
b. ZnF2
c. Zn2F
d. Zn2F3
____
6. What is the formula for the compound formed by calcium ions and chloride ions?
a. CaCl
c. CaCl3
b. Ca2Cl
d. CaCl2
____
7. 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
____
8. What is the formula for aluminum sulfate?
a. AlSO4
b. Al2SO4
c. Al2(SO4)3
d. Al(SO4)3
9. What is the formula for barium hydroxide?
a. BaOH
b. BaOH2
c. Ba(OH)2
d. Ba(OH)
____
____ 10. Name the compound Ni(ClO3)2.
a. nickel(II) chlorate
b. nickel(II) chloride
c. nickel(II) chlorite
d. nickel(II) peroxide
____ 11. Name the compound Zn3(PO4)2.
a. zinc potassium oxide
b. trizinc polyoxide
c. zinc phosphate
d. zinc phosphite
____ 12. Name the compound KClO3.
a. potassium chloride
b. potassium trioxychlorite
c. potassium chlorate
d. hypochlorite
____ 13. Name the compound Fe(NO3)2.
a. iron(II) nitrate
b. iron(II) nitrite
c. iron(III) nitrate
d. iron(III) nitride
____ 14. Name the compound Al2S3.
a. aluminum sulfate
b. aluminum sulfur
c. aluminum(II) sulfate
d. aluminum sulfide
____ 15. Name the compound CF4.
a. calcium fluoride
b. carbon fluoride
c. carbon tetrafluoride
d. monocalcium quadrafluoride
____ 16. Name the compound SiO2.
a. silver oxide
b. silicon oxide
c. silicon dioxide
d. monosilver dioxide
____ 17. Name the compound SO3.
a. sulfur trioxide
b. silver trioxide
c. selenium trioxide
d. sodium trioxide
____ 18. Name the compound N2O3.
a. dinitrogen oxide
b. nitrogen trioxide
c. nitric oxide
d. dinitrogen trioxide
____ 19. What is the formula for silicon dioxide?
a. SO2
b. SiO2
c. Si2O
d. S2O
____ 20. What is the formula for dinitrogen trioxide?
a. Ni2O3
b. NO3
c. N2O6
d. N2O3
____ 21. What is the formula for sulfur dichloride?
a. SCl
b. SCl2
c. S2Cl
d. S2Cl2
____ 22. What is the formula for diphosphorus pentoxide?
a. P2PeO5
c. P2O4
b. PO5
d. P2O5
____ 23. What is the formula for hydrochloric acid?
a. HF
b. HCl
c. HClO
d. H2CO3
____ 24. The oxidation number of fluorine is
a. always 0.
b. –1 in all compounds.
c. +1 in all compounds.
d. equal to the negative charge of all the metal ions in a compound.
____ 25. What is the oxidation number of oxygen in most compounds?
a. –8
c. 0
b. –2
d. +1
____ 26. What is the oxidation number of a pure element?
a. –1
c. +1
b. 0
d. 8
____ 27. In a compound, the algebraic sum of the oxidation numbers of all atoms equals
a. 0.
c. 8.
b. 1.
d. the charge on the compound.
____ 28. What is the oxidation number of hydrogen in compounds containing metals?
a. –1
c. +1
b. 0
d. the charge on the metal ion
____ 29. In a polyatomic ion, the algebraic sum of the oxidation numbers of all atoms is equal to
a. 0.
c. 10.
b. the number of atoms in the ion.
d. the charge of the ion.
____ 30. What is the oxidation number of oxygen in H2O2?
a. –2
c. +2
b. –1
d. –4
____ 31. What is the oxidation number of hydrogen in KH?
a. –1
c. +1
b. 0
d. +2
____ 32. What is the oxidation number of hydrogen in H2O?
a. 0
c. +2
b. +1
d. +3
____ 33. What is the oxidation number of sulfur in SO2?
a. 0
c. +2
b. +1
d. +4
____ 34. What is the oxidation number of sulfur in H2SO4?
a. –2
c. +4
b. 0
d. +6
____ 35. What is the oxidation number of oxygen in CO2?
a. –4
c. 0
b. –2
d. +4
____ 36. Name the compound N2O2 using the Stock system.
a. dinitrogen monoxide
c. nitrogen(II) oxide
b. nitrogen dioxide
d. nitrogen oxide(II)
____ 37. Name the compound SO2 using the Stock system.
a. sulfur(II) oxide
c. sulfur dioxide
b. sulfur(IV) oxide
d. sulfur oxide
____ 38. Name the compound CCl4 using the Stock system.
a. carbon(IV) chloride
c. carbon chloride
b. carbon tetrachloride
d. carbon hypochlorite
____ 39. Name the compound H2O using the Stock system.
a. water
c. hydrogen(I) oxide
b. hydrogen dioxide
d. hydrogen(II) oxide
____ 40. Name the compound CO2 using the Stock system.
a. carbon(IV) oxide
c. monocarbon dioxide
b. carbon dioxide
d. carbon oxide
____ 41. Name the compound PBr5 using the Stock system.
a. potassium hexabromide
c. phosphorus(V) bromide
b. phosphorus(V) pentabromide
d. phosphoric acid
____ 42. The molar mass of an element is the mass of one
a. atom of the element.
c. gram of the element.
b. crystal of the element.
d. mole of the element.
____ 43. What is the formula mass of magnesium chloride, MgCl2?
a. 46 amu
c. 95.21 amu
b. 59.76 amu
d. 106.35 amu
____ 44. What is the formula mass of ethyl alcohol, C2H5OH?
a. 30.33 amu
c. 45.06 amu
b. 33.27 amu
d. 46.08 amu
____ 45. What is the formula mass of (NH4)2SO4?
a. 114.09 amu
b. 118.34 amu
c. 128.06 amu
d. 132.16 amu
____ 46. The molar mass of NO2 is 46.01 g/mol. How many moles of NO2 are present in 114.95 g?
a. 0.4003 mol
c. 2.498 mol
b. 1.000 mol
d. 114.95 mol
____ 47. The molar mass of CCl4 is 153.81 g/mol. How many grams of CCl4 are needed to have 5.000 mol?
a. 5 g
c. 769.0 g
b. 30.76 g
d. 796.05 g
____ 48. The molar mass of H2O is 18.02 g/mol. How many grams of H2O are present in 0.20 mol?
a. 0.2 g
c. 35.9 g
b. 3.6 g
d. 89.9 g
____ 49. 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
____ 50. The molar mass of CS2 is 76.15 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. 761.5 g
____ 51. The molar mass of NH3 is 17.03 g/mol. How many moles of NH3 are present in 107.1 g?
a. 0.1623 mol
c. 6.289 mol
b. 3.614 mol
d. 107.1 mol
____ 52. What is the mass of 0.240 mol glucose, C6H12O6?
a. 24.0 g
b. 43.2 g
c. 180.16 g
d. 750. g
____ 53. How many oxygen atoms are there in 0.500 mol of CO2?
a. 6.02 1023
c. 15.9994
b. 3.01 1023
d. 11.0
____ 54. How many molecules are there in 5.0 g of methyl alcohol, CH3OH?
a. 9.4 1022
c. 3.6 1024
24
b. 3.0 10
d. 3.8 1024
____ 55. What is the percentage composition of CF4?
a. 20% C, 80% F
b. 13.6% C, 86.4% F
c. 16.8% C, 83.2% F
d. 81% C, 19% F
____ 56. What is the percentage composition of CO?
a. 50% C, 50% O
b. 12% C, 88% O
c. 25% C, 75% O
d. 43% C, 57% O
____ 57. What is the percentage composition of CuCl2?
a. 33% Cu, 66% Cl
c. 65.50% Cu, 34.50% Cl
b. 50% Cu, 50% Cl
d. 47.27% Cu, 52.73% Cl
____ 58. 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%
____ 59. What is the mass percentage of OH– in Ca(OH)2?
a. 45.9%
c. 75%
b. 66.6%
d. 90.1%
____ 60. What is the mass percentage of chlorine in NaCl?
a. 35.45%
c. 60.7%
b. 50%
d. 64.5%
____ 61. A formula that shows the simplest whole-number ratio of the atoms in a compound is the
a. molecular formula.
c. experimental formula.
b. ideal formula.
d. empirical formula.
____ 62. The empirical formula for a compound shows the symbols of the elements with subscripts indicating the
a. actual numbers of atoms in a molecule.
b. number of moles of the compound in 100 g.
c. smallest whole-number ratio of the atoms.
d. atomic masses of each element.
____ 63. What is the empirical formula for a compound that is 31.9% potassium, 28.9% chlorine, and 39.2% oxygen?
a. KClO2
c. K2Cl2O3
b. KClO3
d. K2Cl2O5
____ 64. 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
____ 65. What is the empirical formula for a compound that is 53.3% O and 46.7% Si?
a. SiO
c. Si2O
b. SiO2
d. Si2O3
____ 66. A compound contains 259.2 g of F and 40.8 g of C. What is the empirical formula for this compound?
a. CF4
c. CF
b. C4F
d. CF2
____ 67. A compound contains 64 g of O and 8 g of H. What is the empirical formula for this compound?
a. H2O
c. HO2
b. H2O2
d. HO
____ 68. 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
____ 69. A compound contains 27.3 g of C and 72.7 g of O. What is the empirical formula for this compound?
a. CO
c. C2O
b. CO2
d. C2O4
____ 70. A molecular compound has the empirical formula XY3. Which of the following is a possible molecular
formula?
a. X2Y3
c. X2Y5
b. XY4
d. X2Y6
____ 71. The molecular formula for vitamin C is C6H8O6. What is the empirical formula?
a. CHO
c. C3H4O3
b. CH2O
d. C2H4O2
____ 72. Of the following molecular formulas for hydrocarbons, which is an empirical formula?
a. CH4
c. C3H6
b. C2H2
d. C4H10
____ 73. Which of the following molecular formulas does not have the corresponding empirical formula XY2Z?
a. X2Y4Z2
c. X6Y12Z6
b. XYZ
d. X3Y6Z3
____ 74. A compound's empirical formula is C2H5. If the formula mass is 58 amu, what is the molecular formula?
a. C3H6
c. C5H8
b. C4H10
d. C5H15
____ 75. 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
____ 76. A compound's empirical formula is CH. If the formula mass is 26 amu, what is the molecular formula?
a. C2H2
c. CH4
b. CH3
d. C4H
____ 77. 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
____ 78. A compound's empirical formula is CH3. If the formula mass is 30 amu, what is the molecular formula?
a. CH3
b. CH4
c. C2H6
d. C3H9
____ 79. 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
____ 80. What is the molecular formula of a compound that has a formula mass of 50.48 amu and an empirical formula
of CH3Cl?
a. CHCl
c. CH3Cl
b. CH2Cl
d. CH2Cl2
Problem
1. 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.
2. 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.
3. The molar mass of iron is 55.85 g/mol, the molar mass of silicon is 28.08 g/mol, and the molar mass of
oxygen is 16.00 g/mol. Calculate the molar mass of iron(II) silicate, Fe2SiO4.
4. 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.
Completion
Complete each statement.
1. The name and formula for the compound formed by strontium ions and sulfite ions are
____________________.
2. The Stock name for the compound P2O5 is ____________________.
3. The name for the
ion is ____________________.
4. The oxidation numbers for each atom in
are ____________________.
5. The oxidation numbers for each atom in H2CO3 are ____________________.
Essay
1. HO and H2O2 are examples of the empirical and molecular formula of a compound, respectively. Explain the
relationship between these two types of formulas.