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, CF 4? a. 1 c. 4 b. 2 d. 5 4. The formula for carbon dioxide, CO 2, 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 c. Zn 2 F b. ZnF 2 d. Zn 2 F 3 6. What is the formula for the compound formed by calcium ions and chloride ions? a. CaCl c. CaCl 3 b. Ca 2 Cl d. CaCl 2 7. What is the formula for the compound formed by lead(ii) ions and chromate ions? a. PbCrO 4 c. Pb 2 (CrO 4 ) 3 b. Pb 2 CrO 4 d. Pb(CrO 4 ) 2 8. What is the formula for aluminum sulfate? a. AlSO 4 c. Al 2 (SO 4 ) 3 b. Al 2 SO 4 d. Al(SO 4 ) 3 9. What is the formula for barium hydroxide? a. BaOH c. Ba(OH) 2 b. BaOH 2 d. Ba(OH) 10. Name the compound Ni(ClO 3 ) 2. a. nickel(ii) chlorate c. nickel(ii) chlorite b. nickel(ii) chloride d. nickel(ii) peroxide 11. Name the compound Zn 3 (PO 4 ) 2. a. zinc potassium oxide c. zinc phosphate b. trizinc polyoxide d. zinc phosphite
12. Name the compound KClO 3. a. potassium chloride c. potassium chlorate b. potassium trioxychlorite d. hypochlorite 13. Name the compound Fe(NO 3 ) 2. a. iron(ii) nitrate c. iron(iii) nitrate b. iron(ii) nitrite d. iron(iii) nitride 14. Name the compound Al 2 S 3. a. aluminum sulfate c. aluminum(ii) sulfate b. aluminum sulfur d. aluminum sulfide 15. Name the compound CF 4. a. calcium fluoride c. carbon tetrafluoride b. carbon fluoride d. monocalcium quadrafluoride 16. Name the compound SiO 2. a. silver oxide c. silicon dioxide b. silicon oxide d. monosilver dioxide 17. Name the compound SO 3. a. sulfur trioxide c. selenium trioxide b. silver trioxide d. sodium trioxide 18. Name the compound N 2 O 3. a. dinitrogen oxide c. nitric oxide b. nitrogen trioxide d. dinitrogen trioxide 19. What is the formula for silicon dioxide? a. SO 2 c. Si 2 O b. SiO 2 d. S 2 O 20. What is the formula for dinitrogen trioxide? a. Ni 2 O 3 c. N 2 O 6 b. NO 3 d. N 2 O 3 21. What is the formula for sulfur dichloride? a. SCl c. S 2 Cl b. SCl 2 d. S 2 Cl 2 22. What is the formula for diphosphorus pentoxide? a. P 2 PeO 5 c. P 2 O 4 b. PO 5 d. P 2 O 5 23. What is the formula for hydrochloric acid? a. HF c. HClO b. HCl d. H 2 CO 3 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 H 2 O 2? 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 H 2 O? a. 0 c. +2 b. +1 d. +3 33. What is the oxidation number of sulfur in SO 2? a. 0 c. +2 b. +1 d. +4 34. What is the oxidation number of sulfur in H 2 SO 4? a. 2 c. +4 b. 0 d. +6 35. What is the oxidation number of oxygen in CO 2? a. 4 c. 0 b. 2 d. +4 36. Name the compound N 2 O 2 using the Stock system. a. dinitrogen monoxide c. nitrogen(ii) oxide b. nitrogen dioxide d. nitrogen oxide(ii) 37. Name the compound SO 2 using the Stock system. a. sulfur(ii) oxide c. sulfur dioxide b. sulfur(iv) oxide d. sulfur oxide 38. Name the compound CCl 4 using the Stock system. a. carbon(iv) chloride c. carbon chloride
b. carbon tetrachloride d. carbon hypochlorite 39. Name the compound H 2 O using the Stock system. a. water c. hydrogen(i) oxide b. hydrogen dioxide d. hydrogen(ii) oxide 40. Name the compound CO 2 using the Stock system. a. carbon(iv) oxide c. monocarbon dioxide b. carbon dioxide d. carbon oxide 41. Name the compound PBr 5 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, MgCl 2? a. 46 amu c. 95.21 amu b. 59.76 amu d. 106.35 amu 44. What is the formula mass of ethyl alcohol, C 2 H 5 OH? a. 30.33 amu c. 45.06 amu b. 33.27 amu d. 46.08 amu 45. What is the formula mass of (NH 4 ) 2 SO 4? a. 114.09 amu c. 128.06 amu b. 118.34 amu d. 132.16 amu 46. The molar mass of NO 2 is 46.01 g/mol. How many moles of NO 2 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 CCl 4 is 153.81 g/mol. How many grams of CCl 4 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 H 2 O is 18.02 g/mol. How many grams of H 2 O 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 CS 2 is 76.15 g/mol. How many grams of CS 2 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 NH 3 is 17.03 g/mol. How many moles of NH 3 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, C 6 H 12 O 6?
a. 24.0 g c. 180.16 g b. 43.2 g d. 750. g 53. How many oxygen atoms are there in 0.500 mol of CO 2? a. 6.02 10 23 c. 15.9994 b. 3.01 10 23 d. 11.0 54. How many molecules are there in 5.0 g of methyl alcohol, CH 3 OH? a. 9.4 10 22 c. 3.6 10 24 b. 3.0 10 24 d. 3.8 10 24 55. What is the percentage composition of CF 4? a. 20% C, 80% F c. 16.8% C, 83.2% F b. 13.6% C, 86.4% F d. 81% C, 19% F 56. What is the percentage composition of CO? a. 50% C, 50% O c. 25% C, 75% O b. 12% C, 88% O d. 43% C, 57% O 57. What is the percentage composition of CuCl 2? 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 SO 2 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. KClO 2 c. K 2 Cl 2 O 3 b. KClO 3 d. K 2 Cl 2 O 5 64. What is the empirical formula for a compound that is 43.6% phosphorus and 56.4% oxygen? a. P 3 O 7 c. P 2 O 3 b. PO 3 d. P 2 O 5
65. What is the empirical formula for a compound that is 53.3% O and 46.7% Si? a. SiO c. Si 2 O b. SiO 2 d. Si 2 O 3 66. A compound contains 259.2 g of F and 40.8 g of C. What is the empirical formula for this compound? a. CF 4 c. CF b. C 4 F d. CF 2 67. A compound contains 64 g of O and 8 g of H. What is the empirical formula for this compound? a. H 2 O c. HO 2 b. H 2 O 2 d. HO 68. What is the empirical formula for a compound that is 36.1% Ca and 63.9% Cl? a. CaCl c. CaCl 2 b. Ca 2 Cl d. Ca 2 Cl 2 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. C 2 O b. CO 2 d. C 2 O 4 70. A molecular compound has the empirical formula XY 3. Which of the following is a possible molecular formula? a. X 2 Y 3 c. X 2 Y 5 b. XY 4 d. X 2 Y 6 71. The molecular formula for vitamin C is C 6 H 8 O 6. What is the empirical formula? a. CHO c. C 3 H 4 O 3 b. CH 2 O d. C 2 H 4 O 2 72. Of the following molecular formulas for hydrocarbons, which is an empirical formula? a. CH 4 c. C 3 H 6 b. C 2 H 2 d. C 4 H 10 73. Which of the following molecular formulas does not have the corresponding empirical formula XY 2 Z? a. X 2 Y 4 Z 2 c. X 6 Y 12 Z 6 b. XYZ d. X 3 Y 6 Z 3 74. A compound's empirical formula is C 2 H 5. If the formula mass is 58 amu, what is the molecular formula? a. C 3 H 6 c. C 5 H 8 b. C 4 H 10 d. C 5 H 15 75. A compound's empirical formula is N 2 O 5. If the formula mass is 108 amu, what is the molecular formula? a. N 2 O 5 c. NO 3 b. N 4 O 10 d. N 2 O 4 76. A compound's empirical formula is CH. If the formula mass is 26 amu, what is the molecular formula? a. C 2 H 2 c. CH 4 b. CH 3 d. C 4 H 77. A compound's empirical formula is NO 2. If the formula mass is 92 amu, what is the molecular formula? a. NO c. NO 4 b. N 2 O 2 d. N 2 O 4 78. A compound's empirical formula is CH 3. If the formula mass is 30 amu, what is the molecular formula?
a. CH 3 c. C 2 H 6 b. CH 4 d. C 3 H 9 79. A compound's empirical formula is HO. If the formula mass is 34 amu, what is the molecular formula? a. H 2 O c. HO 3 b. H 2 O 2 d. H 2 O 3 80. What is the molecular formula of a compound that has a formula mass of 50.48 amu and an empirical formula of CH 3 Cl? a. CHCl c. CH 3 Cl b. CH 2 Cl d. CH 2 Cl 2 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, AlF 3. 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, CuSO 4. 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, Fe 2 SiO 4. 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 Al 2 O 3. 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 P 2 O 5 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 H 2 CO 3 are. Essay 1. HO and H 2 O 2 are examples of the empirical and molecular formula of a compound, respectively. Explain the relationship between these two types of formulas.