Chemistry Atoms First 1st Edition Burdge Overby - Test bank Instant Download - Complete Test Bank With Answers Sample Questions Are Posted Below Chapter 5: Ionic and Covalent Compounds 1. The Lewis dot symbol consists of the symbol for the element surrounded by dot(s). What does the symbol represent? …
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Chemistry Atoms First 1st Edition Burdge Overby – Test bank
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Sample Questions Are Posted Below
Chapter 5: Ionic and Covalent Compounds
| 1. | The Lewis dot symbol consists of the symbol for the element surrounded by dot(s). What does the symbol represent? | |||
| A) | Electron configuration | D) | Atomic mass | |
| B) | Valence electrons | E) | Nucleus and core electrons | |
| C) | Atomic number | |||
| Ans: E Difficulty: Medium | ||||
| 2. | The Lewis dot symbol consists of the symbol for the element surrounded by dot(s). What does the dot or dots represent? | |||
| A) | Electron configuration | D) | Atomic mass | |
| B) | Valence electrons | E) | Core electrons | |
| C) | Atomic number | |||
| Ans: B Difficulty: Easy | ||||
| 3. | How many dots does the Lewis dot symbol for argon have around it? |
| A) 1 B) 2 C) 4 D) 6 E) 8 | |
| Ans: E Difficulty: Easy |
| 4. | How many dots does the Lewis dot symbol for sodium have around it? |
| A) 1 B) 2 C) 0 D) 3 E) 7 | |
| Ans: A Difficulty: Easy |
| 5. | How many dots does the Lewis dot symbol for magnesium have around it? |
| A) 1 B) 2 C) 0 D) 3 E) 7 | |
| Ans: B Difficulty: Easy |
| 6. | How many dots does the Lewis dot symbol for chlorine have around it? |
| A) 1 B) 2 C) 5 D) 7 E) 17 | |
| Ans: D Difficulty: Easy |
| 7. | How many dots does the Lewis dot symbol for carbon have around it? |
| A) 4 B) 2 C) 6 D) 3 E) 7 | |
| Ans: A Difficulty: Easy |
| 8. | How many dots does the Lewis dot symbol for oxygen have around it? |
| A) 4 B) 2 C) 6 D) 3 E) 7 | |
| Ans: C Difficulty: Easy |
| 9. | The Lewis dot symbol for the a lead atom is |
| A) B) C) D) E) | |
| Ans: C Difficulty: Easy |
| 10. | The Lewis dot symbol for the S 2– ion is |
| A) B) 2- C) S2– D) ¾¾ 2– E) ¾ | |
| Ans: B Difficulty: Medium |
| 11. | The Lewis dot symbol for the chloride ion is |
| A) B) – C) – D) – E) Cl– | |
| Ans: B Difficulty: Medium |
| 12. | The Lewis dot symbol for the calcium ion is |
| A) 2+ B) ¾Ca¾ C) 2+ D) Ca2+ E) Ca | |
| Ans: D Difficulty: Medium |
| 13. | Select the element whose Lewis symbol is correct. |
| A) a. B) b. C) c. D) d. E) e. | |
| Ans: B Difficulty: Medium |
| 14. | Select the element whose Lewis symbol is correct.
|
| A) a. B) b. C) c. D) d. E) e. | |
| Ans: C Difficulty: Medium |
| 15. | Which of these compounds is most likely to be ionic? |
| A) KF B) CCl4 C) CS2 D) CO2 E) ICl | |
| Ans: A Difficulty: Easy |
| 16. | Which of these compounds is most likely to be ionic? |
| A) GaAs B) SrBr2 C) NO2 D) CBr4 E) H2O | |
| Ans: B Difficulty: Easy |
| 17. | Which of these compounds is most likely to be ionic? |
| A) NCl3 B) BaCl2 C) CO D) SO2 E) SF4 | |
| Ans: B Difficulty: Easy |
| 18. | Which of these pairs of elements would be most likely to form an ionic compound? |
| A) Cl and I B) Al and K C) Cl and Mg D) C and S E) Al and Mg | |
| Ans: C Difficulty: Easy |
| 19. | Which of the following contains ionic bonding? |
| A) CO B) SrF2 C) Al D) OCl2 E) HCl | |
| Ans: B Difficulty: Easy |
| 20. | Which of the following is an ionic compound? |
| A) H2S B) NH3 C) I2 D) KI E) CCl4 | |
| Ans: D Difficulty: Easy |
| 21. | Which of these ionic solids would have the largest lattice energy? |
| A) NaCl B) NaF C) CaBr2 D) CsI E) CaCl2 | |
| Ans: E Difficulty: Medium |
| 22. | Which of these ionic solids would have the largest lattice energy? |
| A) SrO B) NaF C) CaBr2 D) CsI E) BaSO4 | |
| Ans: A Difficulty: Medium |
| 23. | The lattice energy for ionic crystals increases as the charge on the ions _____________ and the size of the ions __________________ . | |||
| A) | increases, increases | D) | decreases, decreases | |
| B) | increases, decreases | E) | none of these is generally correct | |
| C) | decreases, increases | |||
| Ans: B Difficulty: Medium | ||||
| 24. | Select the compound with the highest (i.e., most negative) lattice energy. |
| A) CaS(s) B) BaO(s) C) NaI(s) D) LiBr(s) E) MgO(s) | |
| Ans: E Difficulty: Medium |
| 25. | Select the compound with the lowest (i.e., least negative) lattice energy. |
| A) CsBr(s) B) NaCl(s) C) SrO(s) D) CaO(s) E) KBr(s) | |
| Ans: A Difficulty: Medium |
| 26. | An anion is defined as | |
| A) | a charged atom or group of atoms with a net negative charge. | |
| B) | a stable atom. | |
| C) | a group of stable atoms. | |
| D) | an atom or group of atoms with a net positive charge. | |
| E) | neutral. | |
| Ans: A Difficulty: Easy | ||
| 27. | Which one of these species is an ion? |
| A) B3+ B) NaCl C) He D) 14C E) none of the above | |
| Ans: A Difficulty: Easy |
| 28. | Which of these pairs of elements would be most likely to form an ionic compound? |
| A) P and Br B) Cu and K C) C and O D) O and Zn E) Al and Rb | |
| Ans: D Difficulty: Easy |
| 29. | Which pair of elements would be most likely to form an ionic compound? |
| A) P and Br B) Zn and K C) F and Al D) C and S E) Al and Rb | |
| Ans: C Difficulty: Easy |
| 30. | What is the formula for the ionic compound formed by calcium ions and nitrate ions? |
| A) Ca3N2 B) Ca(NO3)2 C) Ca2NO3 D) Ca2NO2 E) CaNO3 | |
| Ans: B Difficulty: Medium |
| 31. | What is the formula for the ionic compound formed by calcium and selenium? |
| A) CaSe B) Ca2Se C) CaSe2 D) Ca3Se E) CaSe3 | |
| Ans: A Difficulty: Easy |
| 32. | Which is the correct formula for copper (II) phosphate? |
| A) Cu2PO4 B) Cu3(PO4)2 C) Cu2PO3 D) Cu(PO4)2 E) Cu(PO3)2 | |
| Ans: B Difficulty: Medium |
| 33. | The chemical name for ClO3– is “chlorate ion”. What is the common name for HClO3? | |||
| A) | hydrochloric acid | D) | chlorous acid | |
| B) | chloroform | E) | chloric acid | |
| C) | hydrogen trioxychloride | |||
| Ans: E Difficulty: Medium | ||||
| 34. | The formula for magnesium sulfate is |
| A) MnS B) MgS C) MnSO3 D) MgSO4 E) MnSO4 | |
| Ans: D Difficulty: Medium |
| 35. | The formula for sodium sulfide is |
| A) NaS B) K2S C) NaS2 D) Na2S E) SeS | |
| Ans: D Difficulty: Medium |
| 36. | The chemical formula for iron (II) nitrate is |
| A) Fe2(NO3)3 B) Ir(NO2)2 C) Fe2N3 D) Fe(NO3)2 E) Fe(NO2)2 | |
| Ans: D Difficulty: Medium |
| 37. | Which one of the following formulas of ionic compounds is the least likely to be correct? |
| A) NH4Cl B) Ba(OH)2 C) Na2SO4 D) Ca2NO3 E) Cu(CN)2 | |
| Ans: D Difficulty: Medium |
| 38. | What is the formula for lead (II) oxide? |
| A) PbO B) PbO2 C) Pb2O D) PbO4 E) Pb2O3 | |
| Ans: A Difficulty: Medium |
| 39. | Potassium permanganate is a strong oxidizer that reacts explosively with easily oxidized materials. What is its formula? |
| A) KMnO3 B) KMnO4 C) K2MnO4 D) K(MnO4)2 E) K2Mn2O7 | |
| Ans: B Difficulty: Medium |
| 40. | Ferric oxide is used as a pigment in metal polishing. Which of the following is its formula? |
| A) FeO B) Fe2O C) FeO3 D) Fe2O5 E) Fe2O3 | |
| Ans: E Difficulty: Medium |
| 41. | What is the name of Mn(CO3)2? | |||
| A) | manganese carbide | D) | magnesium (II) carbonate | |
| B) | magnesium (IV) carbonate | E) | manganese (IV) carbonate | |
| C) | manganese (II) carbonate | |||
| Ans: E Difficulty: Medium | ||||
| 42. | Iron (III) chloride hexahydrate is used as a coagulant for sewage and industrial wastes. What is its formula? | |||
| A) | Fe(Cl·6H2O)3 | D) | Fe3Cl(H2O)6 | |
| B) | Fe3Cl·6H2O | E) | FeCl3·6H2O | |
| C) | FeCl3(H2O)6 | |||
| Ans: E Difficulty: Difficult | ||||
| 43. | Which of the following is the oxoanion of bromine called the bromate ion? |
| A) BrO3– B) BrO32- C) BrO42- D) BrO2– E) BrO– | |
| Ans: A Difficulty: Medium |
| 44. | Which of these compounds is most likely to be covalent? |
| A) Rb2S B) SrCl2 C) CS2 D) CaO E) MgI2 | |
| Ans: C Difficulty: Easy |
| 45. | Which of these compounds is most likely to be covalent? |
| A) KF B) CaCl2 C) SF4 D) Al2O3 E) CaSO4 | |
| Ans: C Difficulty: Easy |
| 46. | Which of these compounds is most likely to be covalent? |
| A) CsOH B) NF3 C) Sr(NO3)2 D) CaO E) LiF | |
| Ans: B Difficulty: Easy |
| 47. | Which of the following is a covalent compound? |
| A) Na2O B) CaCl2 C) Cl2O D) CsCl E) Al2O3 | |
| Ans: C Difficulty: Easy |
| 48. | Which of the following contains covalent bonds? |
| A) BaO B) IBr C) Mg D) LiBr E) Cu | |
| Ans: B Difficulty: Easy |
| 49. | What types of elements undergo ionic bonding? | |||
| A) | 2 metals | D) | 2 Group IA elements | |
| B) | a nonmetal and a metal | E) | 2 Noble gases | |
| C) | 2 nonmetals | |||
| Ans: B Difficulty: Easy | ||||
| 50. | What types of elements undergo covalent bonding? | |||
| A) | 1 metal and noble gas | D) | 2 Group IA elements | |
| B) | a nonmetal and a metal | E) | an actinide | |
| C) | 2 nonmetals | |||
| Ans: C Difficulty: Easy | ||||
| 51. | What is the name of PCl3? | |||
| A) | phosphorus chloride | D) | trichlorophosphide | |
| B) | phosphoric chloride. | E) | phosphorus trichloride. | |
| C) | phosphorus trichlorate. | |||
| Ans: E Difficulty: Easy | ||||
| 52. | The compound, P4S10, is used in the manufacture of safety matches. What is its name? | |||
| A) | phosphorus sulfide | D) | tetraphosphorus decasulfide | |
| B) | phosphoric sulfide | E) | phosphorus sulfite | |
| C) | phosphorus decasulfide | |||
| Ans: D Difficulty: Medium | ||||
| 53. | Diiodine pentaoxide is used as an oxidizing agent that converts carbon monoxide to carbon dioxide. What is its chemical formula? |
| A) I2O5 B) IO5 C) 2IO5 D) I5O2 E) (IO5)2 | |
| Ans: A Difficulty: Medium |
| 54. | What is the name of P4Se3? | |||
| A) | phosphorus selenide | D) | phosphoric selenide | |
| B) | phosphorus triselenide | E) | tetraphosphorus triselenide | |
| C) | tetraphosphorus selenide | |||
| Ans: E Difficulty: Easy | ||||
| 55. | What is the name of ClO–? |
| A) hypochlorite B) chlorate C) chlorite D) perchlorate E) perchlorite | |
| Ans: A Difficulty: Medium |
| 56. | What is the formula for the permanganate ion? |
| A) MnO2– B) MnO4– C) MgO42- D) Mn2O7– E) MgO22- | |
| Ans: B Difficulty: Medium |
| 57. | Tetrasulfur dinitride decomposes explosively when heated. What is its formula? |
| A) S2N4 B) S4N2 C) 4SN2 D) S4N E) S2N | |
| Ans: B Difficulty: Medium |
| 58. | Which of the following is the empirical formula for hexane, C6H14? |
| A) C12H28 B) C6H14 C) C3H7 D) CH2.3 E) C0.43H | |
| Ans: C Difficulty: Medium |
| 59. | Which of the following is a molecular formula for CH? |
| A) C2H6 B) C3H9 C) C4H10 D) C6H6 E) None of the answers are correct | |
| Ans: D Difficulty: Easy |
| 60. | Calcium fluoride, CaF2, is a source of fluorine and is used to fluoridate drinking water. Calculate its formula mass. | |||
| A) | 118.15 g/mol | D) | 59.08 g/mol | |
| B) | 99.15 g/mol | E) | 50.01 g/mol | |
| C) | 78.07 g/mol | |||
| Ans: C Difficulty: Easy | ||||
| 61. | Calculate the molecular mass of tetraphosphorus decaoxide, P4O10, a corrosive substance which can be used as a drying agent. | |||
| A) | 469.73 amu | D) | 139.88 amu | |
| B) | 283.89 amu | E) | 94.97 amu | |
| C) | 190.97 amu | |||
| Ans: B Difficulty: Medium | ||||
| 62. | Calculate the molecular or formula mass of rubidium carbonate, Rb2CO3. | |||
| A) | 340.43 amu | D) | 145.47 amu | |
| B) | 255.00 amu | E) | 113.48 amu | |
| C) | 230.94 amu | |||
| Ans: C Difficulty: Medium | ||||
| 63. | Calculate the molecular or formula mass of (NH4)3AsO4. | |||
| A) | 417.80 amu | D) | 156.96 amu | |
| B) | 193.03 amu | E) | 108.96 amu | |
| C) | 165.02 amu | |||
| Ans: B Difficulty: Difficult | ||||
| 64. | Aluminum sulfate, Al2(SO4)3, is used in tanning leather, purifying water, and manufacture of antiperspirants. Calculate its molecular or formula mass. | |||
| A) | 450.06 amu | D) | 278.02 amu | |
| B) | 342.15 amu | E) | 74.98 amu | |
| C) | 315.15 amu | |||
| Ans: B Difficulty: Difficult | ||||
| 65. | Calculate the molar mass of Ca(BO2)2·6H2O. | |||
| A) | 273.87 g/mol | D) | 174.89 g/mol | |
| B) | 233.79 g/mol | E) | 143.71 g/mol | |
| C) | 183.79 g/mol | |||
| Ans: B Difficulty: Difficult | ||||
| 66. | Calculate the molecular mass of potassium permanganate, KMnO4. |
| A) 52 amu B) 70 amu C) 110 amu D) 158 amu E) 176 amu | |
| Ans: D Difficulty: Easy |
| 67. | Calculate the molecular mass of menthol, C10H20O. |
| A) 156 amu B) 140 amu C) 29 amu D) 146 amu E) 136 amu | |
| Ans: A Difficulty: Easy |
| 68. | What is the molecular mass of acetaminophen, C8H9NO2? |
| A) 43 amu B) 76 amu C) 151 amu D) 162 amu E) 125 amu | |
| Ans: C Difficulty: Medium |
| 69. | What is the molar mass of nicotine, C10H14N2? |
| A) 134 g/mol B) 148 g/mol C) 158 g/mol D) 210 g/mol E) 162 g/mol | |
| Ans: E Difficulty: Easy |
| 70. | Household sugar, sucrose, has the molecular formula C12H22O11. What is the % of carbon in sucrose, by mass? |
| A) 26.7 % B) 33.3 % C) 41.4 % D) 42.1 % E) 52.8 % | |
| Ans: D Difficulty: Medium |
| 71. | What is the percent carbon in CH3CH2OH? |
| A) 13% B) 24% C) 35% D) 46% E) 52% | |
| Ans: E Difficulty: Medium |
| 72. | What is the percent sodium in sodium carbonate? |
| A) 43.4% B) 11.3% C) 45.3% D) 27.7% E) 23% | |
| Ans: A Difficulty: Difficult |
| 73. | What is the mass percent of oxygen in barium perchlorate? |
| A) 4.7% B) 8.5% C) 23.4% D) 38% E) 18.7% | |
| Ans: D Difficulty: Difficult |
| 74. | What is the percent sulfur in iron (III) sulfate? |
| A) 28% B) 32% C) 24% D) 48% E) 42% | |
| Ans: C Difficulty: Difficult |
| 75. | Calculate the number of moles in 17.8 g of the antacid magnesium hydroxide, Mg(OH)2. |
| A) 3.28 mol B) 2.32 mol C) 0.431 mol D) 0.305 mol E) 0.200 mol | |
| Ans: D Difficulty: Medium |
| 76. | How many moles are present in 17.4 g of lead? | |||
| A) | 0.0994 moles | D) | 10.06 moles | |
| B) | 1.05 ´ 1025 moles | E) | 11.9 moles | |
| C) | 0.0840 moles | |||
| Ans: C Difficulty: Easy | ||||
| 77. | How many grams are present in 0.885 moles of manganese? |
| A) 62.1 g B) 48.6 g C) 21.5 g D) 27.5 g E) 0.016 g | |
| Ans: B Difficulty: Easy |
| 78. | How many moles of aspirin, C9H8O4, are in a 325 mg tablet that is 100% aspirin? | |||
| A) | 0.00180 moles | D) | 0.357 moles | |
| B) | 0.555 moles | E) | 2.80 moles | |
| C) | 0.467 moles | |||
| Ans: A Difficulty: Medium | ||||
| 79. | How many grams are contained in a 0.893 mol sample of methane, CH4? |
| A) 1.48 ´ 10-24 g B) 5.38 ´ 1023 g C) 8.64 ´ 1024 g D) 14.3 g E) 18.0 g | |
| Ans: D Difficulty: Easy |
| 80. | How many moles of ammonia, NH3, are in 13.81 g of NH3? | |||
| A) | 1.234 moles | D) | 4.881 ´ 1023 moles | |
| B) | 0.8104 moles | E) | 235.3 moles | |
| C) | 8.316 ´ 1024 moles | |||
| Ans: B Difficulty: Easy | ||||
| 81. | How many grams are contained in a 0.183 mol sample of ammonium phosphate? |
| A) 1.23 ´ 10-3 g B) 617 g C) 20.7 g D) 27.3 g E) 815.1 g | |
| Ans: D Difficulty: Medium |
| 82. | Phosphorus pentachloride, a white solid that has a pungent, unpleasant odor, is used as a catalyst for certain organic reactions. Calculate the number of moles in 38.7 g of phosphorus pentachloride. |
| A) 5.38 mol B) 3.55 mol C) 0.583 mol D) 0.282 mol E) 0.186 mol | |
| Ans: E Difficulty: Medium |
| 83. | Aluminum oxide, Al2O3, is used as a filler for paints and varnishes as well as in the manufacture of electrical insulators. Calculate the number of moles in 47.51 g of Al2O3. |
| A) 2.377 mol B) 2.146 mol C) 1.105 mol D) 0.4660 mol E) 0.4207 mol | |
| Ans: D Difficulty: Medium |
| 84. | What is the mass in grams of 0.250 mol of the common antacid calcium carbonate? |
| A) 4.00 ´ 102 g B) 25.0 g C) 17.0 g D) 4.00 ´ 10-2 g E) 2.50 ´ 10-3 g | |
| Ans: B Difficulty: Medium |
| 85. | What is the mass of 0.0250 mol of P2O5? |
| A) 35.5 g B) 5676 g C) 0.0250 g D) 1.51 ´ 1022 g E) 3.55 g | |
| Ans: E Difficulty: Medium |
| 86. | Calculate the mass of 3.00 moles of CF2Cl2. |
| A) 3.00 g B) 174 g C) 363 g D) 1.81 ´ 1024 g E) 40.3 | |
| Ans: C Difficulty: Medium |
| 87. | Determine the number of ammonia molecules in 4.85g of ammonia (NA = 6.022 ´ 1023 mol-1). | |||
| A) | 2.92 ´ 1023 | D) | 5.83 ´ 10-24 | |
| B) | 4.73 ´ 10-25 | E) | 1.71 ´ 1023 | |
| C) | 1.24 ´ 1023 | |||
| Ans: E Difficulty: Medium | ||||
| 88. | What is the average mass, in grams, of one atom of iron (NA = 6.022 ´ 1023 mol-1)? | |||
| A) | 6.02 ´ 1023 g | D) | 55.85 g | |
| B) | 1.66 ´ 10–24 g | E) | 55.85 ´ 10 –23 g | |
| C) | 9.28 ´ 10–23 g | |||
| Ans: C Difficulty: Medium | ||||
| 89. | What is the mass, in grams, of one arsenic atom (NA = 6.022 ´ 1023 mol-1)? |
| A) 5.48 ´ 10–23 g B) 33.0 g C) 74.9 g D) 1.24 ´ 10–22 g E) 8.04 ´ 1021 g | |
| Ans: D Difficulty: Medium |
| 90. | What is the mass of one copper atom (NA = 6.022 ´ 1023 mol-1)? | |||
| A) | 1.055 ´ 10–22 g | D) | 1.66 ´ 10–24 g | |
| B) | 63.55 g | E) | 9.476 ´ 1021 g | |
| C) | 1 amu | |||
| Ans: A Difficulty: Medium | ||||
| 91. | The mass of 1.21 ´ 1020 atoms of sulfur is (NA = 6.022 ´ 1023 mol-1) |
| A) 3.88 ´ 1021 g B) 2.00 mg C) 32.06 g D) 6.44 mg E) 2.00 ´ 10–4 g | |
| Ans: D Difficulty: Medium |
| 92. | The mass of 1.63 ´ 1021 silicon atoms is (NA = 6.022 ´ 1023 mol-1) | |||
| A) | 2.71 ´ 10–23 g | D) | 1.04 ´ 104 g | |
| B) | 4.58 ´ 1022 g | E) | 7.60 ´ 10–2 g | |
| C) | 28.08 g | |||
| Ans: E Difficulty: Medium | ||||
| 93. | What is the mass of 7.80 ´ 1018 carbon atoms (NA = 6.022 ´ 1023 mol-1)? | |||
| A) | 1.30 ´ 10 –5 g | D) | 1.56 ´ 10 –4 g | |
| B) | 6.43 ´ 103 g | E) | 12.01 g | |
| C) | 7.80 ´ 1018 g | |||
| Ans: D Difficulty: Medium | ||||
| 94. | Sulfur trioxide can react with atmospheric water vapor to form sulfuric acid that falls as acid rain. Calculate the mass in grams of 3.65 ´ 1020 molecules of sulfur trioxide. |
| A) 6.06 ´ 10-4 g B) 2.91 ´ 10-2 g C) 4.85 ´ 10-2 g D) 20.6 g E) 1650 g | |
| Ans: C Difficulty: Medium |
| 95. | Calculate the mass in grams of 8.35 ´ 1022 molecules of CBr4. |
| A) 0.0217 g B) 0.139 g C) 7.21 g D) 12.7 g E) 46.0 g | |
| Ans: E Difficulty: Medium |
| 96. | Ionic compounds tend to form between metals and nonmetals when electrons are transferred from an element with high ionization energy (metal) to an element with a low electron affinity (nonmetal). |
| Ans: False Difficulty: Medium |
| 97. | Ionic compounds may carry a net positive or negative charge. |
| Ans: False Difficulty: Medium |
| 98. | When an alkali metal combines with a non-metal, a covalent bond is normally formed. |
| Ans: False Difficulty: Easy |
| 99. | The empirical formula of C6H6 is CH? |
| Ans: True Difficulty: Easy |
| 100. | The empirical formula is the simplest whole number ratio of atoms representing a chemical formula of a molecule. |
| Ans: True Difficulty: Easy |
| 101. | Many compounds can be represented with the same empirical formula. |
| Ans: True Difficulty: Easy |
| 102. | There is only one distinct empirical formula for each compound that exists. |
| Ans: True Difficulty: Easy |
| 103. | The molecular formula is a whole number multiple of the empirical formula. |
| Ans: True Difficulty: Easy |
| 104. | What is the electrostatic attraction called that holds oppositely charged ions together in a compound? | |
| Ans: | ionic bond | |
| Difficulty: Easy | ||
| 105. | What name is given to sharing of electrons between two atoms? | |
| Ans: | covalent bonding | |
| Difficulty: Easy | ||
| 106. | What is the law that describes different samples of a given compound that always contain the same elements in the same mass ratio? | |
| Ans: | law of definite proportions | |
| Difficulty: Easy | ||
| 107. | What name is given to the simplest organic compounds which only contain carbons and hydrogens? | |
| Ans: | hydrocarbons | |
| Difficulty: Easy | ||
| 108. | What is the name of Cu2O? | |
| Ans: | Copper (I) oxide | |
| Difficulty: Medium | ||
| 109. | What is the formula for sodium dichromate? | |
| Ans: | Na2Cr2O7 | |
| Difficulty: Medium | ||
| 110. | Analysis of a white solid produced in a reaction between chlorine and phosphorus showed that it contained 77.44% chlorine and 22.56% phosphorus. What is its empirical formula? | |
| Ans: | PCl3 | |
| Difficulty: Medium | ||
| 111. | The number of dots in the Lewis dot for a main group element is the same as the ___________ ___________. | |
| Ans: | group number | |
| Difficulty: Easy | ||
| 112. | ______________ is defined by the following equation
# of atoms ´ atomic mass of element ´ 100% molecular or formula mass of compound |
|
| Ans: | percent by mass of an element | |
| Difficulty: Medium | ||
| 113. | Atoms of elements with low ionization energies tend to form ____________ while those with positive electron affinities tend to form _________. | |
| Ans: | cations; anions | |
| Difficulty: Medium | ||
| 114. | Describe, with appropriate explanations, the key factors which affect the magnitude of the lattice energy of an ionic substance. | |
| Ans: | By Coulomb’s law, the energy of two electrical charges is proportional to the product of their charges and inversely proportional to the distance separating them. If one approximates the lattice energy by considering only nearest neighbor interactions, the energy will be proportional to the product of the charges and inversely proportional to their separation. Thus a lattice consisting of small ions with multiple charges will have the greatest (negative) lattice energy. | |
| Difficulty: Medium | ||
| 115. | Describe the difference between an empirical formula and a molecular formula. | |
| Ans: | An empirical formula is the simplest chemical formula that has the smallest possible whole number ratio of atoms in the formula and a molecular formula is the true formula of a molecule which is a whole number multiple of its empirical formula. | |
| Difficulty: Easy | ||
Original price was: $30.00.$20.00Current price is: $20.00.
Original price was: $30.00.$20.00Current price is: $20.00.
Original price was: $30.00.$20.00Current price is: $20.00.
Original price was: $30.00.$20.00Current price is: $20.00.
Original price was: $30.00.$20.00Current price is: $20.00.
Original price was: $30.00.$20.00Current price is: $20.00.
