Chemistry in Focus A Molecular View of Our World 6th Edition by Nivaldo J. Tro – Test Bank

 

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Sample Test

Chapter_03_Atoms_and_Elements     1. The most abundant element in the earth’s crust by mass is:   a. Hydrogen   b. Carbon   c. Oxygen   d. Silicon   e. Nitrogen   ANSWER:   c POINTS:   1

 

2. Which of these statements about atoms is incorrect?   a. Atoms are the smallest visible amount of an element.   b. Atoms are composed of protons, neutrons, and electrons.   c. Atoms are the building blocks of all matter.   d. Atoms are the smallest identifiable unit of an element.   e. There are 91 different naturally occurring atoms.   ANSWER:   a POINTS:   1

 

3. The number of protons in a neutral atom is equal to the _____ of the atom.   a. mass   b. atomic weight   c. atomic number   d. mass number   e. valence electron number   ANSWER:   c POINTS:   1

 

4. Which of these particles has a negative charge?   a. Proton   b. Neutron   c. Electron   d. Nucleus   e. An atom   ANSWER:   c POINTS:   1

 

5. Which of these statements about an atom is incorrect?   a. The number protons equals the number of electrons.   b. The number of protons equals the atomic number.   c. The number of protons equals the number of neutrons.   d. The mass number is the sum of protons and neutrons in the atom.   e. The mass number minus the atomic number equals the number of neutrons in the atom.   ANSWER:   c POINTS:   1

 

6. Which of these is the correct chemical symbol for carbon?   a. C   b. Ca   c. Cl   d. Cb   e. Co   ANSWER:   a POINTS:   1

 

7. Which of these is the correct chemical symbol for cobalt?   a. C   b. Cl   c. Co   d. Ca   e. Ce   ANSWER:   c POINTS:   1

 

8. Which of these is the correct chemical symbol for potassium?   a. K   b. Po   c. P   d. Pd   e. Pt   ANSWER:   a POINTS:   1

 

9. Which of the following is not true for an atom that has an atomic number of 19 and a mass number of 41?   a. The atom contains 22 neutrons.   b. The atom is potassium.   c. The atom contains 19 neutrons.   d. The atom contains 19 electrons.   e. The atom contains 19 protons.   ANSWER:   c POINTS:   1

 

10. Which statement about electrons is incorrect?   a. Electrons are negatively charged.   b. Electrons have a negligible mass compared to the rest of the atom.   c. Electrons exist in the nucleus of the atom.   d. The number of electrons equals the atomic number in a neutral atom.   e. Both B and D are incorrect statements.   ANSWER:   c POINTS:   1

 

11. Nonmetals tend to _____ electrons to form ions of _____ charge.   a. lose, negative   b. lose, positive   c. gain, positive   d. gain, negative   ANSWER:   d POINTS:   1

 

12. Metals tend to _____ electrons to form ions of _____ charge.   a. lose, negative   b. lose, positive   c. gain, positive   d. gain, negative   ANSWER:   b POINTS:   1

 

13. Determine the correct number of protons and electrons in P3− .   a. 3 protons, 6 electrons   b. 15 protons, 18 electrons   c. 15 protons, 12 electrons   d. 31 protons, 28 electrons   e. 31 protons, 34 electrons   ANSWER:   b POINTS:   1

 

14. Determine the correct number of protons and electrons in F−.   a. 9 protons, 10 electrons   b. 9 protons, 11 electrons   c. 10 protons, 9 electrons   d. 11 protons, 10 electrons   e. 19 protons, 20 electrons   ANSWER:   a POINTS:   1

 

15. A certain ion contains 47 protons and 46 electrons. The ion is:   a. Pd+   b. Pd−   c. Ag+   d. Ag−   e. Can’t tell from the given information   ANSWER:   c POINTS:   1

 

16. What is the charge on an ion that contains 16 protons and 18 electrons?   a. 0   b. +2   c. −2   d. It depends on the number of neutrons.   e. None of these.   ANSWER:   c POINTS:   1

 

17. How many electrons are there in 15N3−?   a. 15   b. 18   c. 12   d. 4   e. 10   ANSWER:   e POINTS:   1

 

18. Which of these particles has the smallest mass?   a. A proton   b. A neutron   c. An electron   d. A hydrogen atom   e. A hydrogen nucleus   ANSWER:   c POINTS:   1

 

19. When an oxygen atom gains two electrons, it becomes a(n) _____ with a charge of _____.   a. anion, 2+   b. anion, 2−   c. cation, 2−   d. cation, 2+   e. cation, 0   ANSWER:   b POINTS:   1

 

20. When a strontium atom loses two electrons, it becomes a(n) _____ with a charge of _____.   a. anion, 2+   b. anion, 2−   c. cation, 2−   d. cation, 2+   e. cation, 0   ANSWER:   d POINTS:   1

 

21. Metals tend to form ions with a positive charge. The most likely way to form a positively charged ion from an atom is by doing which of the following?   a. Gaining electron(s).   b. Gaining proton(s).   c. Losing electron(s).   d. Losing proton(s).   e. Losing neutron(s).   ANSWER:   c POINTS:   1

 

22. Which of these statements best describes the formation of an anion?   a. An atom loses one or more electrons and becomes positively charged.   b. An atom loses one or more electrons and becomes negatively charged.   c. An atom gains one or more electrons and becomes positively charged.   d. An atom gains one or more electrons and becomes negatively charged.   e. None of these are correct.   ANSWER:   d POINTS:   1

 

23. Which of these statements best describes the formation of a cation?   a. An atom loses one or more electrons and becomes positively charged.   b. An atom loses one or more electrons and becomes negatively charged.   c. An atom gains one or more electrons and becomes positively charged.   d. An atom gains one or more electrons and becomes negatively charged.   e. None of these are correct.   ANSWER:   a POINTS:   1

 

24. The Ca2+ ion contains _____ protons and _____ electrons.   a. 20, 20   b. 20, 22   c. 22, 20   d. 18, 20   e. 20, 18   ANSWER:   e POINTS:   1

 

25. The Cl− ion contains _____ protons and _____ electrons.   a. 17, 17   b. 17, 18   c. 18, 16   d. 18, 18   e. 16, 17   ANSWER:   b POINTS:   1

 

26. How many protons, neutrons, and electrons are in an 25Mg+2 ion?.   a. 12 protons, 12 electrons, 13 neutrons   b. 12 protons, 10 electrons, 12 neutrons   c. 13 protons, 10 electrons, 12 neutrons   d. 12 protons, 10 electrons, 13 neutrons   e. 12 protons, 14 electrons, 13 neutrons   ANSWER:   d POINTS:   1

 

27. Which of these is the correct representation for the ion with Z=27, A=60, and C=2+ ?   a.   b.   c.   d.   e.   ANSWER:   a POINTS:   1

 

28. What are the Z and A values for an atom of silicon which contains 15 neutrons?   a. Z=14, A=15   b. Z=15, A=14   c. Z=29, A=14   d. Z=14, A=29   e. Z=15, A=29   ANSWER:   d POINTS:   1

 

29. Isotopes of an element have the same number of _____ but a different number of _____.   a. neutrons, protons   b. electrons, protons   c. protons, neutrons   d. neutrons, electrons   e. protons, electrons   ANSWER:   c POINTS:   1

 

30. What are the Z and A values for an atom of krypton which contains 46 neutrons?   a. Z=36, A=46   b. Z=46, A=36   c. Z=36, A=82   d. Z=82, A=36   e. Z=82, A=46   ANSWER:   c POINTS:   1

 

31. Radon −222 has _____ protons, _____ neutrons, and _____ electrons.   a. 86, 86, 86   b. 86, 222, 86   c. 86, 136, 86   d. 86, 136, 222   e. 86, 222, 308   ANSWER:   c POINTS:   1

 

32. How many protons (p), neutrons (n), and electrons (e) are in an atom of 235U?   a. 92 p, 146 n, 92 e   b. 92 p, 143 n, 92 e   c. 92 p, 92 n, 146 e   d. 92 p, 92 n, 92 e   e. 92 p, 51 n, 92 e   ANSWER:   b POINTS:   1

 

33. Carbon has three isotopes: 12C, 13C, and 14C. These isotopes each have _____ protons, _____ electrons and _____, _____, and _____ neutrons respectively.   a. 6, 6, and 6, 7, 8   b. 12, 12, and 6, 7, 8   c. 12, 12, and 12, 13, 14   d. 6, 6, and 12, 13, 14   e. 12, 12, and 24, 25, 26   ANSWER:   a POINTS:   1

 

34. An element has two naturally occurring isotopes. One has an abundance of 37.4% and an isotopic mass of 184.953 amu. The other has an abundance of 62.6% and a mass of 186.956 amu. What is the atomic weight of the element?   a. 185.702 amu   b. 185.954 amu   c. 186.207 amu   d. 186.956 amu   e. 190.234 amu   ANSWER:   c POINTS:   1

 

35. Chlorine has two isotopes, 35Cl and 37Cl that have the respective percent abundance’s of 75.77% and 24.23% and masses of 34.9688 amu and 36.9659 amu. Calculate the atomic weight of chlorine.   a. 37.54 amu   b. 36.65 amu   c. 35.45 amu   d. 34.97 amu   e. 36.97 amu   ANSWER:   c POINTS:   1

 

36. Rubidium consists of two naturally occurring isotopes rubidium-85 and rubidium-87. Rubidium-85 (85Rb) has an isotopic mass of 84.9117 amu and a 72.15% abundance. Rubidium-87(87Rb) has a 27.85% abundance. The atomic weight of rubidium is 85.4768 amu. Determine the isotopic mass of 87Rb?   a. 86.72371 amu   b. 86.8013 amu   c. 86.8220 amu   d. 86.8621 amu   e. 86.9085 amu   ANSWER:   e POINTS:   1

 

37. Copper has two naturally occurring isotopes. Cu-63 has a mass of 62.939 amu and Cu-65 has a mass of 64.928 amu. Based on the atomic mass of copper, which isotope has a higher fractional abundance?   a. Cu-63   b. Cu-65   c. Both have the same fractional abundance.   d. Not enough information to tell.   ANSWER:   a POINTS:   1

 

38. There are three isotopes of neon. Assuming the mass of each isotope is very close to its mass number, which isotope is most abundant based on the atomic mass of neon (Ne)?   a. Ne-20   b. Ne-21   c. Ne-22   d. Can’t tell from the given information.   ANSWER:   a POINTS:   1

 

39. Mendeleev organized the elements of the periodic table   a. by increasing atomic number and similar properties.   b. by increasing atomic weight and similar properties.   c. by increasing number of electrons.   d. by increasing number of isotopes.   e. alphabetically.   ANSWER:   b POINTS:   1

 

40. Which scientist is responsible for the organization of the modern periodic table?   a. Bohr   b. Galileo   c. Dalton   d. Avogadro   e. Mendeleev   ANSWER:   e POINTS:   1

 

41. Which of these elements is a metal?   a. Mg   b. Br   c. Ar   d. Ge   e. B   ANSWER:   a POINTS:   1

 

42. Which of these statements concerning atomic mass is correct?   a. Atomic mass is the same as the mass number of the most common isotope.   b. Atomic mass is derived from the weight of the most common isotope of the element.   c. Atomic mass is determined by adding the masses of the protons, electrons, and neutrons in the atom.   d. Atomic mass is calculated from the atomic mass of the two most common isotopes.   e. Atomic mass is a weighted average of the masses of the naturally occurring isotopes.   ANSWER:   e POINTS:   1

 

43. Which of these elements is a metalloid?   a. Ge   b. Br   c. Ar   d. Ca   e. Fe   ANSWER:   a POINTS:   1

 

44. Which of these is a nonmetal?   a. Mg   b. Br   c. Cu   d. Ge   e. Li   ANSWER:   b POINTS:   1

 

45. Which element is not a nonmetal?   a. P   b. I   c. N   d. K   e. Cl   ANSWER:   d POINTS:   1

 

46. Which scientist is responsible for the theory which explains why properties of elements recur in a periodic fashion?   a. Bohr   b. Galileo   c. Dalton   d. Avogadro   e. Mendeleev   ANSWER:   a POINTS:   1

 

47. Which of the following elements is generally not found in diatomic form in nature?   a. C   b. N   c. O   d. F   ANSWER:   a POINTS:   1

 

48. What is the maximum number of electrons which can occupy the orbit n=2?   a. 2   b. 6   c. 8   d. 10   e. 18   ANSWER:   c POINTS:   1

 

49. What is the total number of electrons which can occupy the first and second principal energy levels (n=1, n=2)?   a. 2   b. 6   c. 8   d. 10   e. 18   ANSWER:   d POINTS:   1

 

50. Which of these statements about Bohr’s model of the atom is incorrect?   a. Electrons fill lower energy orbits first.   b. The greater the quantum number the higher the energy of an orbit.   c. Electrons occupy orbits with certain radii corresponding to discrete energies.   d. Elements with the same number of electrons in their outer orbit have similar properties.   e. All of these statements are correct.   ANSWER:   e POINTS:   1

 

51. He has the same number of valence electrons as _____.   a. H   b. Ne   c. Be   d. F   ANSWER:   c POINTS:   1

 

52. Elements in the same group have the same _____.   a. mass number   b. atomic number   c. number of protons   d. number of electrons   e. number of valence electrons   ANSWER:   e POINTS:   1

 

53. The elements of group IA will all form ions. These ions will be _____ and will have a charge of _____.   a. cations, 2+   b. anions, 2−   c. cations, 3+   d. anions, 1−   e. cations, 1+   ANSWER:   e POINTS:   1

 

54. The elements of group 7A will all form ions. These ions will be _____ and will have a charge of _____.   a. cations, 2+   b. anions, 2−   c. cations, 3+   d. anions, 1−   e. cations, 1+   ANSWER:   d POINTS:   1

 

55. Which of these elements has two valence electrons?   a. Mg   b. Li   c. Al   d. S   e. Cl   ANSWER:   a POINTS:   1

 

56. Which of these elements has three valence electrons?   a. Mg   b. Li   c. Al   d. S   e. Cl   ANSWER:   c POINTS:   1

 

57. Which of these elements has seven valence electrons?   a. Mg   b. Li   c. Al   d. S   e. Cl   ANSWER:   e POINTS:   1

 

58. Which of the following is true?   a. Argon and chlorine have the same number of electrons.   b. Argon and chlorine have the same number of valence electrons.   c. Argon and neon have the same number of electrons.   d. Argon and neon have the same number of valence electrons.   e. There is more than one correct statement.   ANSWER:   d POINTS:   1

 

59. Which of the following is true?   a. Argon and chlorine have a different number of electrons.   b. Argon and chlorine have a different number of valence electrons.   c. Argon and neon have a different number of electrons.   d. Argon and neon have a different number of valence electrons.   e. There is more than one correct statement.   ANSWER:   e POINTS:   1

 

60. These elements Li, Na, K, Rb, and Cs are members of what group/family?   a. halogens   b. noble gases   c. alkali metals   d. transition metals   e. alkaline earth metals   ANSWER:   c POINTS:   1

 

61. Strontium is a member of what group/family?   a. halogens   b. noble gases   c. alkali metals   d. transition metals   e. alkaline earth metals   ANSWER:   e POINTS:   1

 

62. Bromine is a member of what group/family?   a. halogens   b. noble gases   c. alkali metals   d. transition metals   e. alkaline earth metals   ANSWER:   a POINTS:   1

 

63. Which of these elements is not a transition metal?   a. Cu   b. Fe   c. Na   d. Ag   e. Hg   ANSWER:   c POINTS:   1

 

64. Which family/group is largely unreactive?   a. Halogens   b. Noble gases   c. Alkali metals   d. Transition metals   e. Alkaline earth metals   ANSWER:   b POINTS:   1

 

65. Which of the following is true?   a. Oxygen and sulfur are in the same group.   b. Oxygen and sulfur are in different groups.   c. Oxygen and sulfur are in the same period.   d. Oxygen and sulfur are in different periods.   e. Both A and D are correct.   ANSWER:   e POINTS:   1

 

66. Which of these groups is incorrectly matched with its group/family name?   Group Name I. 2A alkaline earth metals II. 3A alkali metals III. 7A halogens IV. 8A noble gases V. 2B – 3B transition metals     a. I   b. II   c. III   d. IV   e. V   ANSWER:   b POINTS:   1

 

67. The atomic mass of fluorine (F) is 19.00. Which of the following is not true?   a. An atom of F has a mass of 19.00 amu.   b. One mole of F has a mass of 19.00 g.   c. 6.02 x 1023 atoms of F has a mass of 19.00 g.   d. 6.02 x 1023 atoms of F has a mass of 19.00 amu.   ANSWER:   d POINTS:   1

 

68. What is the correct number of atoms in one mole of aluminum?   a. 12   b. 26.98   c. 6.022 × 1023   d. 13   e. 14   ANSWER:   c POINTS:   1

 

69. What is the correct number of atoms in one mole of neon?   a. 10   b. 11   c. 6.022 × 1023   d. 20   e. 12   ANSWER:   c POINTS:   1

 

70. One mole of nickel (Ni) has a mass of _____.   a. 28 amu   b. 28 g   c. 58.71 amu   d. 58.71 g   ANSWER:   d POINTS:   1

 

71. Determine the mass of one mole of silver.   a. 107.87 amu   b. 107.87 g   c. 47 amu   d. 47 g   e. 6.022 × 1023 amu   ANSWER:   b POINTS:   1

 

72. Calculate the number of moles in a 2.98 g sample of aluminum.   a. 0.0124 moles   b. 0.110 moles   c. 80.4 moles   d. 1.79 × 1024 moles   e. 1.62 × 1025 moles   ANSWER:   b POINTS:   1

 

73. Calculate the number of moles in a 233 gram sample of barium.   a. 0.589 moles   b. 1.70 moles   c. 3.20 × 104   d. 6.022 × 1023 moles   e. 1.02 × 1024 moles   ANSWER:   b POINTS:   1

 

74. Calculate the number of moles of lead in a 442 gram lead anvil.   a. 0.468 moles   b. 2.13 moles   c. 96.97 moles   d. 6.022 × 1023 moles   e. 1.28 × 1024 moles   ANSWER:   b POINTS:   1

 

75. Calculate the number of moles in a 25.0 g sample of carbon.   a. 2.08 moles   b. 13.0 moles   c. 300 moles   d. 1.51 × 1025 moles   e. 3.33 × 10−3 moles   ANSWER:   a POINTS:   1

 

76. Determine the number of atoms in a copper strip that has a mass of 35.0 grams.   a. 3.33 × 1025 atoms   b. 2.11 × 1025 atoms   c. 2.71 × 1020 atoms   d. 3.32 × 1023 atoms   e. 0.551 atoms   ANSWER:   d POINTS:   1

 

77. Determine the number of atoms in a piece of ultrapure silicon that has a mass of 15.0 grams.   a. 1.13 × 1024 atoms   b. 1.69 × 1025 atoms   c. 2.54 × 1020 atoms   d. 3.21 × 1023 atoms   e. 9.03 × 1024 atoms   ANSWER:   d POINTS:   1

 

78. Determine the mass in grams of 1.15 × 1023 atoms of cobalt.   a. 0.191 grams   b. 5.23 grams   c. 11.2 grams   d. 12.4 grams   e. 308 grams   ANSWER:   c POINTS:   1

 

79. Determine the mass in grams of 3.45 × 1025 molecules of oxygen, O2.   a. 0.556 grams   b. 57.2 grams   c. 458 grams   d. 916 grams   e. 1.83 × 103 grams   ANSWER:   e POINTS:   1

 

80. Determine the mass in grams of one molecule of water, H2O.   a. 2.99 × 10−23 g   b. 1.08 × 1025 g   c. 10 grams   d. 18 grams   e. None of the above.   ANSWER:   a POINTS:   1

 

81. Which of the following has the largest mass of oxygen?   a. 16.0 g of O2   b. 0.500 mole of O2   c. 6.022 × 1023 molecules of O2   d. 10 grams of carbon dioxide CO2   e. All of these have the same mass of oxygen.   ANSWER:   c POINTS:   1

 

82. Which of these is not equivalent to one mole?   a. 6.022 × 1023 marbles   b. 12 grams of carbon   c. Avogadro’s number   d. 12 grams of magnesium   e. 28 grams of nitrogen, N2   ANSWER:   d POINTS:   1

 

83. Which scientist is credited with developing the mole concept?   a. Bohr   b. Galileo   c. Dalton   d. Avogadro   e. Mendeleev   ANSWER:   d POINTS:   1

 

Chapter_05_Chemical_Bonding     1. Which of these theories is utilized in the prediction of molecular shapes?   a. Dalton’s Theory   b. VSEPR Theory   c. Bohr’s Atomic Theory   d. Lewis Bonding Theory   e. Einstein’s Theory of Relativity   ANSWER:   b POINTS:   1

 

2. What does the V in VSEPR theory stand for?   a. Very   b. Variable   c. Valence   d. Vanadium   e. Volume   ANSWER:   c POINTS:   1

 

3. Which of these substances is/are ionic compound(s)? I. NCl3 II. MgF2 III. AlBr3 IV. CH4     a. I and II   b. II and III   c. II and IV   d. II, III, and IV   e. II only   ANSWER:   b POINTS:   1

 

4. Which of the following is true for sodium?   a. It is most stable as an atom.   b. It is most stable as a negatively charged ion.   c. It is most stable as a positively charged ion.   d. All forms of sodium are very stable.   e. All forms of sodium are very unstable.   ANSWER:   c POINTS:   1

 

5. Which of these substances is/are covalent compound(s)? I. CaO II. H20 III. PF3 IV. CH4     a. I and II   b. II and III   c. II and IV   d. II, III, and IV   e. II only   ANSWER:   d POINTS:   1

 

6. Which of these is not a fundamental postulate of bonding proposed by Lewis?   a. Valence electrons are shared in covalent bonding.   b. The valence shell is involved in chemical bonding.   c. Atoms bond to achieve a more stable configuration.   d. Atoms bond to achieve an octet of electrons in the valence shell.   e. A stable electron configuration has six electrons in the valence shell.   ANSWER:   e POINTS:   1

 

7. Which of these is the correct Lewis dot structure for chlorine?   a.   b.   c.   d.   e.   ANSWER:   c POINTS:   1

 

8. Which of these is the correct Lewis dot structure for sulfur?   a.   b.   c.   d.   e.   ANSWER:   d POINTS:   1

 

9. Which of these is the most likely identity of element A in the Lewis dot structure?   a. Ca   b. Li   c. Al   d. Cs   e. P   ANSWER:   a POINTS:   1

 

10. Which of these is the most likely identity of element A in the Lewis dot structure?   a. Ca   b. K   c. N   d. Cl   e. O   ANSWER:   d POINTS:   1

 

11. Which of these will not form a positive ion in an ionic compound?   a. Ba   b. Rb   c. P   d. Sn   e. Mg   ANSWER:   c POINTS:   1

 

12. An element which has two valence electrons as an atom will most likely:   a. lose 2 electrons to become negatively charged and combine with a cation.   b. lose 2 electrons to become positively charged and combine with an anion.   c. gain 2 electrons to become negatively charged and combine with a cation.   d. gain 2 electrons to become positively charged and combine with an anion.   e. All of the above can occur.   ANSWER:   b POINTS:   1

 

13. Which of these is the correct formula for aluminum oxide?   a. AlO   b. Al2O   c. AlO2   d. Al2O3   e. Al2O2   ANSWER:   d POINTS:   1

 

14. Which of these is the correct formula for strontium iodide?   a. SrI   b. SrI2   c. Sr2I   d. SrI3   e. Sr2I2   ANSWER:   b POINTS:   1

 

15. Which of these is the correct formula for sodium phosphide?   a. NaP   b. NaP2   c. Na3P   d. NaP3   e. Na3P2   ANSWER:   c POINTS:   1

 

16. Ionic bonds are formed when electrons are ____.   a. transferred   b. split   c. shared   d. destroyed   e. heated   ANSWER:   a POINTS:   1

 

17. Covalent bonds are formed when electrons are ____.   a. transferred   b. split   c. shared   d. destroyed   e. heated   ANSWER:   c POINTS:   1

 

18. Which of these is the correct Lewis dot structure for carbon monoxide?   a.   b.   c.   d.   e.   ANSWER:   d POINTS:   1

 

19. How many total valence electrons are there in the Lewis structure of NO3−1?   a. 32   b. 30   c. 20   d. 22   e. None of these.   ANSWER:   e POINTS:   1

 

20. The total number of valence electrons in NO2−1 is   a. 16   b. 17   c. 18   d. none of the above   ANSWER:   c POINTS:   1

 

21. Which of these is the correct Lewis dot structure for sulfur trioxide?   a.   b.   c.   d.   e.   ANSWER:   c POINTS:   1

 

22. Which of these is the correct Lewis dot structure for nitrogen, N2?   a.   b.   c.   d.   ANSWER:   a POINTS:   1

 

23. How many lone pairs of electrons are around the central atom in PCl3?   a. 0   b. 1   c. 2   d. 3   e. 20   ANSWER:   b POINTS:   1

 

24. How many lone pairs of electrons are around the central atom in CO2?   a. 0   b. 1   c. 2   d. 3   e. 4   ANSWER:   a POINTS:   1

 

25. How many lone pairs of electrons are around the central atom in H2O?   a. 0   b. 1   c. 2   d. 3   e. 4   ANSWER:   c POINTS:   1