Chemistry An Atoms First Approach 2nd Edition by Steven S. Zumdahl – Test Bank

 

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Sample Test

Chapter_3_Bonding_General_Concepts     1. The force between two bodies having identical electric charges _____.   a. is a force of repulsion   b. is a force of repulsion if the charges are negative, and one of attraction if they are positive   c. increases as the bodies are moved further apart   d. is independent of the distance between them   e. is directly proportional to the distance between them   ANSWER:   a POINTS:   1

 

2. In which pair do both compounds exhibit predominantly ionic bonding?   a. PCl3 and HF   b. Na2SO3 and CH4   c. KI and O3   d. BaF2 and H2O   e. CsCl and MgO   ANSWER:   e POINTS:   1

 

3. When a metal reacts with a nonmetal a covalent bond is formed.   a. True   b. False   ANSWER:   False POINTS:   1

 

4. A nonpolar covalent bond results from the unequal sharing of a pair of electrons between atoms in a molecule.   a. True   b. False   ANSWER:   False POINTS:   1

 

5. Atoms with greatly different electronegativity values are expected to form _____.   a. no bonds   b. covalent bonds   c. triple bonds   d. ionic bonds   e. none of these   ANSWER:   d POINTS:   1

 

6. For the elements Ba, F, and N, the order of increasing electronegativity is:   a. Ba < F < N.   b. Ba < N < F.   c. N < F < Ba.   d. F < Ba < N.   e. none of these.   ANSWER:   b POINTS:   1

 

7. For the elements Cs, F, and Cl, the order of increasing electronegativity is:   a. F < Cl < Cs.   b. Cs < Cl < F.   c. Cl < Cs < F.   d. F < Cs < Cl.   e. none of these.   ANSWER:   b POINTS:   1

 

8. In which case is the bond polarity incorrect?   a. δ+H–Fδ–   b. δ+K–Oδ–   c. δ+Mg–Hδ–   d. δ+Cl–Iδ–   e. δ+Si–Sδ–   ANSWER:   d POINTS:   1

 

9. Based on electronegativity differences, which of the following is most likely to be ionic?   a. CaF2   b. I2   c. BH3   d. NO2   e. CF4   ANSWER:   a POINTS:   1

 

10. Choose the compound with the most ionic bond.   a. LiCl   b. KF   c. NaCl   d. LiF   e. KCl   ANSWER:   b POINTS:   1

 

11. Which of the following bonds is least polar?   a. C—O   b. H—C   c. S—Cl   d. Br—Br   e. They are all nonpolar.   ANSWER:   d POINTS:   1

 

12. In the gaseous phase, which of the following diatomic molecules would be the most polar?   a. CsF   b. CsCl   c. NaCl   d. NaF   e. LiF   ANSWER:   a POINTS:   1

 

13. Based on electronegativities, which of the following would you expect to be most ionic?   a. N2   b. CaF2   c. CO2   d. CH4   e. CF4   ANSWER:   b POINTS:   1

 

14. In which of the following compounds does the bond between the central atom and bromine have the greatest ionic character?   a. LiBr   b. KBr   c. SeBr2   d. AsBr3   e. CaBr2   ANSWER:   b POINTS:   1

 

15. What is the correct order of the following bonds in terms of decreasing polarity?   a. N-Cl, P-Cl, As-Cl   b. P-Cl, N-Cl, As-Cl   c. As-Cl, N-Cl, P-Cl   d. P-Cl, As-Cl, N-Cl   e. As-Cl, P-Cl, N-Cl   ANSWER:   e POINTS:   1

 

16. Which of the following bonds would be the most polar without being considered ionic?   a. Mg-O   b. C-O   c. O-O   d. Si-O   e. N-O   ANSWER:   d POINTS:   1

 

17. Which of the following bonds would be the least polar, yet still be considered polar covalent?   a. Mg-O   b. C-O   c. O-O   d. Si-O   e. N-O   ANSWER:   e POINTS:   1

 

18. Which of the following statements is incorrect?   a. Ionic bonding results from the transfer of electrons from one atom to another.   b. Dipole moments result from the unequal distribution of electrons in a molecule.   c. The electrons in a polar bond are found nearer to the more electronegative element.   d. A molecule with very polar bonds can be nonpolar.   e. Linear molecules cannot have a net dipole moment.   ANSWER:   e POINTS:   1

 

19. Which of the following molecules has no dipole moment?   a. CO2   b. NH3   c. H2O   d. all   e. none   ANSWER:   a POINTS:   1

 

20. Which of the following has the smallest radius?   a. Br–   b. S2–   c. Xe   d. Ca2+   e. Kr   ANSWER:   d POINTS:   1

 

21. Which of the following has the smallest radius?   a. K+   b. Cl–   c. Rb+   d. S2–   e. Ar   ANSWER:   a POINTS:   1

 

22. Which of the following has the smallest radius?   a. F–   b. Ne   c. O2–   d. Mg2+   e. Na+   ANSWER:   d POINTS:   1

 

23. In the reaction between magnesium and sulfur, the magnesium atoms _____.   a. become anions   b. become cations   c. become part of polyatomic ions   d. share electrons with sulfur   e. crystallize   ANSWER:   b POINTS:   1

 

24. Which of the following statements are true concerning ionic bonding?   a. Ionic bonding occurs between a metal, which has a high affinity for electrons, and a nonmetal, which loses electrons relatively easy.   b. CaCl2 forms because Ca2+ is always a more stable species than the calcium atom alone.   c. Compounds with ionic bonds tend to have low melting points.   d. The electronegativity difference between the bonding atoms of ionic compounds is small since the electrons are not shared but rather held together by electrostatic forces.   e. All of the above statements are false.   ANSWER:   e POINTS:   1

 

25. Which of the following statements is false?   a. Models are human interpretations, not the same as reality.   b. Models are often wrong.   c. Models usually start out simple and become more complex over time.   d. We often learn more when a model is wrong than when it is right.   e. A model should be discarded when any exception to it is found.   ANSWER:   e POINTS:   1

 

26. When electrons in a molecule are not found between a pair of atoms but move throughout the molecule, this is called _____.   a. ionic bonding   b. covalent bonding   c. polar covalent bonding   d. delocalization of the electrons   e. a dipole moment   ANSWER:   d POINTS:   1

 

27. Choose the molecule with the strongest bond.   a. F2   b. Cl2   c. Br2   d. I2   e. All are equal.   ANSWER:   b POINTS:   1

 

28. Choose the molecule with the strongest bond.   a. HF   b. HCl   c. HBr   d. HI   e. All are equal.   ANSWER:   a POINTS:   1

 

29. Choose the molecule with the strongest bond.   a. CH4   b. H2O   c. NH3   d. HF   e. All are equal   ANSWER:   d POINTS:   1

 

30. Which of the following molecules exhibits the greatest bond energy?   a. F2   b. Cl2   c. Br2   d. I2   e. all the same   ANSWER:   b POINTS:   1

 

31. As the number of bonds between two carbon atoms increases, which one of the following decreases?   a. Number of electrons between the carbon atoms   b. Bond energy   c. Bond length   d. All of these   e. None of these   ANSWER:   c POINTS:   1

 

32. Using the following data reactions:   ΔH° (kJ) H2(g) + Cl2(g) → 2HCl(g) –184 H2(g) → 2H(g) 432 Cl2(g) → 2Cl(g) 239 calculate the energy of an H-Cl bond.   a. 855 kJ   b. 244 kJ   c. 487 kJ   d. 92 kJ   e. 428 kJ   ANSWER:   e POINTS:   1

 

33. Given the following information:   Cl2 bond energy = 239 kJ/mol     F2 bond energy = 154 kJ/mol     Cl2(g) + F2(g) → ClF3(g) ΔH° = –409 kJ/mol calculate the Cl-F bond energy.   a. 267 kJ/mol   b. 253 kJ/mol   c. 760 kJ/mol   d. 136 kJ/mol   e. none of these   ANSWER:   b POINTS:   1

 

34. Consider the following reaction: A2 + B2 → 2AB          ΔH = –377 kJ The bond energy for A2 is half the amount of AB. The bond energy of B2 = 405 kJ/mol. What is the bond energy of A2?   a. 782 kJ/mol   b. 594 kJ/mol   c. 261 kJ/mol   d. –189 kJ/mol   e. none of these   ANSWER:   c POINTS:   1

 

35. In the Lewis structure for elemental nitrogen there is (are):   a. a single bond between the nitrogens.   b. a double bond between the nitrogens.   c. a triple bond between the nitrogens.   d. three unpaired electrons.   e. none of the above.   ANSWER:   c POINTS:   1

 

36. Which of the following molecules contains a double bond?   a. CO2   b. NH3   c. H2O   d. all   e. none   ANSWER:   a POINTS:   1

 

37. When molten sulfur reacts with chlorine gas, a vile-smelling orange liquid forms that is found to have the empirical formula SCl. Which of the following could be the correct Lewis structure for this compound?   a.   b.   c.   d.   e. :   ANSWER:   e POINTS:   1

 

38. As indicated by Lewis structures, which of the following would probably not exist as a stable molecule?   a. CH3OH   b. CH2O   c. CH3O   d. C2H2   e. C3H4   ANSWER:   c POINTS:   1

 

39. Complete the Lewis structure for the molecule: This molecule has __________ single bonds and __________ multiple bonds.   a. 4, 2   b. 6, 3   c. 11, 5   d. 11, 2   e. 13, 0   ANSWER:   d POINTS:   1

 

40. Which of the following compounds contains only one unshared pair of valence electrons?   a. NH3   b. H2O   c. CH4   d. NaCl   e. BF3   ANSWER:   a POINTS:   1

 

41. Draw the Lewis structures of the molecules below and use them to answer the following questions: I. BH3 II. NO2 III. SF6 IV. O3 V. PCl5   Reference: Ref 4-2     a. I   b. II   c. III   d. IV   e. V   ANSWER:   d POINTS:   1

 

42. Draw the Lewis structures of the molecules below and use them to answer the following questions: I. BH3 II. NO2 III. SF6 IV. O3 V. PCl5   Reference: Ref 4-2     a. 1   b. 2   c. 3   d. 4   e. They are all polar.   ANSWER:   c POINTS:   1

 

43. Draw the Lewis structures of the molecules below and use them to answer the following questions: I. BH3 II. NO2 III. SF6 IV. O3 V. PCl5   Reference: Ref 4-2     a. I, II   b. II, IV   c. II, V   d. III, IV   e. III, V   ANSWER:   b POINTS:   1

 

44. Using the following electronegativity values:   C   2.5   Cl 3.0   H   2.1   O 3.5 select from the following group the molecule that fits the given statement: a) CH3CHO b) CO2 c) CH3Cl d) C2H6   e)   none   Reference: Ref 4-1     a. CH3CHO   b. CO2   c. CH3Cl   d. C2H6   e. none of these   ANSWER:   a POINTS:   1

 

45. Using the following electronegativity values:   C   2.5   Cl 3.0   H   2.1   O 3.5 select from the following group the molecule that fits the given statement: a) CH3CHO b) CO2 c) CH3Cl d) C2H6   e)   none   Reference: Ref 4-1     a. CH3CHO   b. CO2   c. CH3Cl   d. C2H6   e. All are nonpolar.   ANSWER:   a POINTS:   1

 

46. Using the following electronegativity values:   C   2.5   Cl 3.0   H   2.1   O 3.5 select from the following group the molecule that fits the given statement: a) CH3CHO b) CO2 c) CH3Cl d) C2H6   e)   none   Reference: Ref 4-1     a. CH3CHO   b. CO2   c. CH3Cl   d. C2H6   e. All have zero lone pairs.   ANSWER:   d POINTS:   1

 

47.   Consider the compound crotonaldehyde, whose skeleton is:     Reference: Ref 4-3     a. 12   b. 18   c. 24   d. 28   e. 32   ANSWER:   d POINTS:   1

 

48.   Consider the compound crotonaldehyde, whose skeleton is:     Reference: Ref 4-3     a. 2   b. 4   c. 6   d. 8   e. 10   ANSWER:   b POINTS:   1

 

49.   Consider the compound crotonaldehyde, whose skeleton is:     Reference: Ref 4-3     a. 1   b. 2   c. 3   d. 4   e. all   ANSWER:   a POINTS:   1

 

50. Given the following Lewis structure: Reference: Ref 4-4     a. 0   b. 1   c. 2   d. 3   e. 4   ANSWER:   a POINTS:   1

 

51. Given the following Lewis structure: Reference: Ref 4-4     a. 0   b. 2   c. 4   d. 6   e. 8   ANSWER:   c POINTS:   1

 

52. Which of the following atoms cannot exceed the octet rule in a molecule?   a. N   b. S   c. P   d. I   e. All of the atoms (A-D) can exceed the octet rule.   ANSWER:   a POINTS:   1

 

53. In the Lewis structure for ICl2–, how many lone pairs of electrons are around the central iodine atom?   a. 0   b. 1   c. 2   d. 3   e. 4   ANSWER:   d POINTS:   1

 

54. In the Lewis structure for SF6, the central sulfur atom shares __________ electrons.   a. 4   b. 8   c. 10   d. 12   e. None of the above, because SF6 is an ionic compound.   ANSWER:   d POINTS:   1

 

55. Which of the following Lewis structures best describes BF3?   a.   b.   c.   d.   e.   ANSWER:   a POINTS:   1

 

56. Which of the following has an incomplete octet in its Lewis structure?   a. SO2   b. ICl   c. CO2   d. F2   e. NO   ANSWER:   e POINTS:   1

 

57. As indicated by Lewis structures, which of the following species could probably not exist as a stable molecule?   a. NH3   b. N2H2   c. N2H4   d. N2H6   e. N2O4   ANSWER:   d POINTS:   1

 

58. The Lewis structure for H3BO3 is   a.   b.   c.   d.   e.   ANSWER:   d POINTS:   1

 

59. Select the best Lewis structure for acetone, CH3COCH3.   a.   b.   c.   d.   e.   ANSWER:   b POINTS:   1

 

60. In the cyanide ion (CN–), the nitrogen has a formal charge of _____.   a. -2   b. -1   c. 0   d. 2   e. More information is needed.   ANSWER:   c POINTS:   1

 

61. Which of the following exhibits resonance?   a. BH3   b. SCl6   c. H2O   d. NO2   e. At least two of the molecules (A-D) exhibit resonance.   ANSWER:   d POINTS:   1

 

62. Which of the following species is best described by drawing resonance structures?   a. PH3   b. NH4+   c. O3   d. SO3   e. HCN   ANSWER:   c POINTS:   1

 

63. How many resonance structures can be drawn for the molecule O3?   a. 1   b. 2   c. 3   d. 4   e. 5   ANSWER:   b POINTS:   1

 

64. Which of the following is not a valid resonance structure for N3–?   a.   b.   c.   d.   e. all are correct   ANSWER:   a POINTS:   1

 

65. Which has the greater N–O bond length, NO2– or NO3–?   a. NO2–   b. NO3–   c. The bond lengths are the same.   d. More information is needed.   e. None of these (A-D).   ANSWER:   b POINTS:   1

 

66. Which of the following has a Lewis structure most like that of CO32–?   a. CO2   b. SO32–   c. NO3–   d. O3   e. NO2   ANSWER:   c POINTS:   1

 

67. The size in a series of isoelectronic ions increases as the nuclear charge increases.   a. True   b. False   ANSWER:   False POINTS:   1

 

68. A double bond occurs when two atoms share two pairs of electrons.   a. True   b. False   ANSWER:   True POINTS:   1

 

69. The Lewis structure for CHCl3 has nine lone electron pairs.   a. True   b. False   ANSWER:   True POINTS:   1

 

70. When nonmetals chemically combine, they tend to form what type of bond? ANSWER:   covalent POINTS:   1

 

71. The ability of an atom in a molecule to attract shared electrons to itself is called __________. ANSWER:   electronegativity POINTS:   1

 

72. A molecule that has a center of positive charge and a center of negative charge is said to be __________. ANSWER:   polar POINTS:   1

 

73. Match the ions below with the pictures that represent their relative sizes. Justify your answers. Ions: Se2–        K+      Ga3+        Br–           Ca2+ ANSWER:   ​ ​ ​ ​ K+        Ca2+     Ga3+           Se2–        Br– Se2– and Br– each have the electron configuration of Kr. K+, Ca2+, and Ga3+ each have the electron configuration of Ar. The Se2– and Br– contain electrons in a higher energy level, therefore making their radii larger than the other three ions. Since Br– has more protons, this will draw the electrons in slightly more than Se2– (due to a slightly higher effective nuclear charge). For the other three ions, Ga3+ will be the smallest because it has the highest number of protons. K+ has the least number of protons and is thus the biggest ion of the three.   ​ ​ POINTS:   1

 

74. The __________ is the change in energy that takes place when separated gaseous ions are packed together to form an ionic solid. ANSWER:   lattice energy POINTS:   1

 

75. Stable molecules usually contain atoms that have filled __________ orbitals. ANSWER:   valence POINTS:   1

 

76. The __________ of a molecule shows how the valence electrons are arranged among the atoms in the molecule. ANSWER:   Lewis structure POINTS:   1

 

77. When several nonequivalent Lewis structures can be drawn for a molecule, __________ is used to determine the most appropriate structure(s). ANSWER:   formal charge POINTS:   1

 

78. ​For which compound does 0.256 mole weigh 12.8 g?   a. ​C2H4O   b. ​CO2   c. ​CH3Cl   d. ​C2H6   e. ​none of these   ANSWER:   c POINTS:   1

 

79. ​Which of the following names is incorrect?   a. ​Cobalt(II) chloride   b. ​Magnesium oxide   c. ​Aluminum(III) oxide   d. ​Diphosphorus pentoxide   e. ​All of the above names are correct   ANSWER:   c POINTS:   1

 

80. ​Which of the following pairs is incorrect?   a. ​Iodine trichloride, ICl3   b. ​Phosphorus pentoxide, P2O5   c. ​Ammonia, NH3   d. ​Sulfur hexafluoride, SF6   e. ​All of the above pairs are correct   ANSWER:   b POINTS:   1

 

81. ​The correct name for LiCl is _____.   a. ​lithium monochloride   b. ​lithium(I) chloride   c. ​monolithium chloride   d. ​lithium chloride   e. ​lithium chloride   ANSWER:   d POINTS:   1

 

82. ​The correct name for FeO is _____.   a. ​iron oxide   b. ​iron(II) oxide   c. ​iron(III) oxide   d. ​iron monoxide   e. ​iron(I) oxide   ANSWER:   b POINTS:   1

 

83. ​The correct name for Ca2+ is _____.   a. ​calcium   b. ​calcium(II) ion   c. ​calcium ion   d. ​calcium(I) ion   e. ​calcium(I) ion   ANSWER:   c POINTS:   1

 

84. ​The correct name for V3+ is _____.   a. ​vanadide   b. ​vanadite ion   c. ​vanadium(III) ion   d. ​vanadium(V) ion   e. ​trivanadium ion   ANSWER:   c POINTS:   1

 

85. ​The correct name for N3– is _____.   a. ​nitride ion   b. ​nitrogen ion   c. ​nitrogen(III) ion   d. ​nitro(III) ion   e. ​nitrite   ANSWER:   a POINTS:   1

 

86. ​Which metals form cations with varying positive charges?   a. ​Transition metals   b. ​Group 1 metals   c. ​Group 2 metals   d. ​Group 3 metals   e. ​Metalloids   ANSWER:   a POINTS:   1

 

87. ​The formula for calcium bisulfate is _____.   a. ​Ca(SO4)2   b. ​Ca(SO4)2   c. ​Ca(SO4)2   d. ​Ca2HSO4   e. ​Ca2S   ANSWER:   c POINTS:   1

 

88. ​The formula for potassium dihydrogen phosphate is _____.   a. ​KH2PO4   b. ​K(HPO4)2   c. ​KHPO4   d. ​K2HPO4   e. ​K2H2PO4   ANSWER:   a POINTS:   1

 

89. ​Which of the following is incorrectly named?   a. ​Pb(NO3)2, lead(II) nitrate   b. ​NH4ClO4, ammonium perchlorate   c. ​PO43–, phosphate ion   d. ​Mg(OH)2, magnesium hydroxide   e. ​NO3–, nitrite ion   ANSWER:   e POINTS:   1

 

90. ​Which of the following is incorrectly named?   a. ​SO32–, sulfite ion   b. ​C2O42–, oxalate ion   c. ​PO43–, phosphate ion   d. ​ClO3–, chlorite ion   e. ​CN–, cyanide ion   ANSWER:   d POINTS:   1

 

91. ​Which of the following pairs is incorrect?   a. ​NH4Br, ammonium bromide   b. ​K2CO3, potassium carbonate   c. ​BaPO4, barium phosphate   d. ​CuCl, copper(I) chloride   e. ​MnO2, manganese(IV) oxide   ANSWER:   c POINTS:   1

 

92. ​All of the following are in aqueous solution. Which is incorrectly named?   a. ​H2SO4, sulfuric acid   b. ​H2CO3, carbonic acid   c. ​H3PO4, phosphoric acid   d. ​HCN, cyanic acid   e. ​HCl, hydrochloric acid   ANSWER:   d POINTS:   1