1. Chapter 11 Modern Atomic Theory Practice Problems

2. 2 All atoms of the same element have the same number of 1.Protons 2.Neutrons 3.Electrons 4.Protons and Neutrons 5.Protons and Electrons

3. 3 All atoms of the same element have the same number of 1.Protons this is a good choice, but not the best choice. 2.Neutrons 3.Electrons 4.Protons and Neutrons 5.Protons and Electrons

4. 4 In the symbol below, the number 33 is the 1.Atomic mass 2.Mass number 3.Atomic number 4.Charge 5.Number of X atoms attached to each other. X 33

5. 5 In the symbol below, the number 33 is the 1.Atomic mass 2.Mass number 3.Atomic number 4.Charge 5.Number of X atoms attached to each other. X 33

6. 6 In the symbol below, the number 60 is the __ which tells us this is 1.Atomic mass, Ni 2.Mass number, Ni 3.Mass number, Ni or Co 4.Mass number, possibly any element in the Ni & Cu “neighborhood.” 5.Atomic number, Ni or Co X 60

7. 7 In the symbol below, the number 60 is the __ which tells us this is 1.Atomic mass, Ni 2.Mass number, Ni 3.Mass number, Ni or Co 4.Mass number, possibly any element in the Ni & Cu “neighborhood.” 5.Atomic number, Ni or Co Mass number can not be used to identify which element, only atomic number can. X 60

8. 8 The number of neutrons can be known by 1.Dividing the mass number in half. 2.Subtracting the atomic number from the mass number. 3.Subtracting the number of protons from the atomic mass. 4.Looking at the atomic number. 5.It can not be known exactly because of isotopes.

9. 9 The number of neutrons can be known by 1.Dividing the mass number in half. 2.Subtracting the atomic number from the mass number. 3.Subtracting the number of protons from the atomic mass. 4.Looking at the atomic number. 5.It can not be known exactly because of isotopes.

10. 10 The element represented by [Ar] 4s 2 3d 10 4p 2 is 1. 20 Ca 2. 22 Ti 3. 32 Ge 4. 50 Sn 5. 35 Br

11. 11 The element represented by [Ar] 4s 2 3d 10 4p 2 is 1. 20 Ca 2. 22 Ti 3. 32 Ge All that you really need to look at is the 4p 2 to be able to identify. 4. 50 Sn 5. 35 Br

12. 12 The element represented by [Kr] 5s 2 4d 9 is 1. 29 Cu 2. 27 Co 3. 79 Au 4. 47 Ag 5. 45 Rh

13. 13 The element represented by [Kr] 5s 2 4d 9 is 1. 29 Cu 2. 27 Co 3. 79 Au 4. 47 Ag 5. 45 Rh

14. 14 The element represented by 5p 3 is (assuming all lower energy orbitals are filled) 1. 39 Y 2. 51 Sb 3. 33 As 4. 21 Sc 5. 83 Bi

15. 15 The element represented by 5p 3 is 1. 39 Y 2. 51 Sb 3. 33 As 4. 21 Sc 5. 83 Bi

16. 16 Give highest energy orbital to describe 74 W 1.6d 6 2.7d 6 3.6p 4 4.6d 4 5.5d 4

17. 17 Give highest energy orbital to describe 74 W 1.6d 6 2.7d 6 3.6p 4 4.6d 4 5.5d 4

18. 18 How many valence electrons in 15 P 1.15 2.8 3.3 4.4 5.5 6.I don’t know what the word valence means.

19. 19 How many valence electrons in 15 P 1.15 2.8 3.3 4.4 5.5 6.I don’t know what the word valence means. Valence means outermost electrons - the “s” and “p” electrons in the last energy level.

20. 20 When atoms turn into a positive ion 1.Protons are gained. 2.Protons are lost. 3.Electrons are gained 4.Electrons are lost. 5.Either protons are gained or electrons are lost.

21. 21 When atoms turn into a positive ion 1.Protons are gained. 2.Protons are lost. 3.Electrons are gained 4.Electrons are lost. 5.Either protons are gained or electrons are lost.

22. Fluorine (F) Does 9 F want to lose or gain electrons? How many? What will the new charge be? 1.Lose 6 e -, 6 +, cation 2.Gain 6 e -, 6 -, anion 3.Lose 1 e -, 1 +, cation 4.Gain 1 e -, 1 -, anion 5.Lose 7 e -, 7 +, cation 6.Gain 7 e -, 7 -, anion 7.Will not lose or gain. It is happy(stable)! 22

23. Fluorine (F) Does 9 F want to lose or gain electrons? How many? What will the new charge be? 1.Lose 6 e -, 6 +, cation 2.Gain 6 e -, 6 -, anion 3.Lose 1 e -, 1 +, cation 4.Gain 1 e -, 1 -, anion 5.Lose 7 e -, 7 +, cation 6.Gain 7 e -, 7 -, anion 7.Will not lose or gain. It is happy(stable)! 23

24. Gallium (Ga) Does 31 Ga want to lose or gain electrons? How many? What will the new charge be? 24 1.Lose 4 e -, 4 +, cation 2.Gain 3 e -, 3 -, anion 3.Lose 1 e -, 1 +, cation 4.Gain 1 e -, 1 -, anion 5.Lose 3 e -, 3 +, cation 6.Gain 4 e -, 4 -, anion 7.Will not lose or gain. It is happy(stable)!

25. Gallium (Ga) Does 31 Ga want to lose or gain electrons? How many? What will the new charge be? 25 1.Lose 4 e -, 4 +, cation 2.Gain 3 e -, 3 -, anion 3.Lose 1 e -, 1 +, cation 4.Gain 1 e -, 1 -, anion 5.Lose 3 e -, 3 +, cation 6.Gain 4 e -, 4 -, anion 7.Will not lose or gain. It is happy(stable)!

26. Radon (Rn) Does 86 Rn want to lose or gain electrons? How many? What will the new charge be? 26 1.Lose 2 e -, 2 +, cation 2.Gain 3 e -, 3 -, anion 3.Lose 1 e -, 1 +, cation 4.Gain 1 e -, 1 -, anion 5.Lose 3 e -, 3 +, cation 6.Gain 2 e -, 2 -, anion 7.Will not lose or gain. It is happy(stable)!

27. Radon (Rn) Does 86 Rn want to lose or gain electrons? How many? What will the new charge be? 27 1.Lose 2 e -, 2 +, cation 2.Gain 3 e -, 3 -, anion 3.Lose 1 e -, 1 +, cation 4.Gain 1 e -, 1 -, anion 5.Lose 3 e -, 3 +, cation 6.Gain 2 e -, 2 -, anion 7.Will not lose or gain. It is happy(stable)!

28. Forming Bonds 28 1. Sodium Chloride NaCl 2. Magnesium Oxide MgO 3. Calcium Iodide CaI 2 4. Aluminum Oxide Al 2 O 3

29. 29 Which light has the most energy? 1.Red 2.Orange 3.Yellow 4.Green 5.Blue

30. 30 Which light has the most energy? 1.Red 2.Orange 3.Yellow 4.Green 5.Blue - most energy, highest frequency, shortest wavelength.

31. 31 Which light has the highest frequency? 1.Red 2.Orange 3.Yellow 4.Green 5.Blue

32. 32 Which light has the highest frequency? 1.Red 2.Orange 3.Yellow 4.Green 5.Blue

33. 33 Which light has the longest wavelength? 1.Red 2.Orange 3.Yellow 4.Green 5.Blue

34. 34 Which light has the longest wavelength? 1.Red 2.Orange 3.Yellow 4.Green 5.Blue

35. 35 Which light has the least energy? 1.infrared 2.micro waves 3.green light 4.gamma 5.ultraviolet

36. 36 Which light has the least energy? 1.infrared 2.micro waves 3.green light 4.gamma 5.ultraviolet

37. 37 In a hydrogen atom, an electron undergoing the transition between which energy levels would emit the most energy? 1.3 - 2 2.5 - 2 3.1 - 2 4.4 - 5 5.4 - 1 6.2 - 1

38. 38 In a hydrogen atom, an electron undergoing the transition between which energy levels would emit the most energy? 1.3 - 2 2.5 - 2 3.1 - 2 4.4 - 5 5.4 - 1 energy is emitted only for transitions from higher to lower energy levels. transitions to the first energy level are always more energy than to other energy levels 6.2 - 1

39. 39 Which graph best represents the relationship between wavelength and frequency for “light” aka EMR (ElectroMagnetic Radiation)? 12341234 ν ν ν ν lamba, λ, wavelength nu, v, frequency

40. 40 Which graph best represents the relationship between wavelength and frequency? ABCD Wavelength ( ) and frequency ( ν ) are inversely related. ν ν ν ν

41. 41 Select the largest atom from the group: 3 Li, 11 Na, 38 Sr, 53 I Be ready to explain your choice. 1. 3 Li 2. 11 Na 3. 38 Sr 4. 53 I 5.Cannot be determined since they are in different families and different periods

42. 42 Select the largest atom from the group: 3 Li, 11 Na, 38 Sr, 53 I 1. 3 Li 2. 11 Na 3. 38 Sr Since Sr and I both have a 5th energy level, yet Sr has a lower effective nuclear charge, so it has larger size. 4. 53 I 5.Cannot be determined since they are in different families and different periods

43. 43 Select the largest particle from the group: 54 Xe, 53 I -1, 56 Ba +2, 52 Te -2 Be ready to explain your choice. 1. 54 Xe 2. 53 I -1 3. 56 Ba +2 4. 52 Te -2 5.They are all the same size because they are isoelectronic. 6.I can’t choose because I don’t know what isoelectronic means and I don’t know about the size of charged particles.

44. 44 Select the largest particle from the group: 54 Xe, 53 I -1, 56 Ba +2, 52 Te -2 1. 54 Xe 2. 53 I -1 3. 56 Ba +2 4. 52 Te -2 This ion has less protons, only 52 to hold the 54 electrons, thus the e- repel each other and cause larger size 5.They are all the same size because they are isoelectronic. 6.I can’t choose because I don’t know what isoelectronic means and I don’t know about the size of charged particles.

45. 45 16 S is smaller than 11 Na because 1. 16 S has more protons and more electrons. 2. 16 S has more electrons. 3. 16 S has more protons pulling on electrons in the same energy level. 4. 16 S has fewer energy levels. 5. 16 S has more neutrons to allow the atom to squeeze in more.

46. 46 16 S is smaller than 11 Na because 1. 16 S has more protons and more electrons. 2. 16 S has more electrons. 3. 16 S has more protons (blocked by the same core of 10 e- electrons that the Na nucleus is shielded by) pulling on electrons in the same energy level. 4. 16 S has fewer energy levels. 5. 16 S has more neutrons to allow the atom to squeeze in more.

47. 47 Select the atom below with the lowest first ionization energy. Be ready to explain your choice. 1. 11 Na 2. 12 Mg 3. 13 Al 4. 14 Si 5. 15 P

48. 48 Select the atom below with the lowest first ionization energy. 1. 11 Na because it is largest in size 2. 12 Mg 3. 13 Al 4. 14 Si 5. 15 P

49. 49 The atom that has a really large increase for its 3rd ionization energy would be 1. 11 Na 2. 12 Mg 3. 13 Al 4. 14 Si 5. 15 P

50. 50 The atom with the largest increase for its 3rd ionization energy would be 1. 11 Na (for Na it would be the 2nd IE) 2. 12 Mg because it has 2 valence electrons and stealing the third electron comes from a full energy level. 3. 13 Al (for Al it would be the 4th IE) 4. 14 Si (for Si it would be the 5th IE) 5. 15 P (for P it would be the 6th IE) All successive IE are larger than the previous, however,the really large increase occurs for the electron that is one more than the number of valence electrons.

51. 51 In which set of elements would all the atoms have very similar chemical properties? (Choose all that apply.) 1. 11 Na, 12 Mg, 13 Al 2. 14 Si, 32 Ge, 50 Sn 3. 90 Th, 91 Pa, 92 U 4. 26 Fe, 27 Co, 28 Ni 5. 7 N, 8 O, 9 F 6. 16 S, 34 Se, 52 Te 7.I have no idea how to even begin to answer this question.

52. 52 In which set of elements would all the atoms have very similar chemical properties? 1. 11 Na, 12 Mg, 13 Al 2. 14 Si, 32 Ge, 50 Sn this family crosses the metal nonmetal barrier and thus would have different chemical properties 3. 90 Th, 91 Pa, 92 U 4. 26 Fe, 27 Co, 28 Ni 5. 7 N, 8 O, 9 F 6. 16 S, 34 Se, 52 Te These elements are all in the same chemical family which all have the same number of valence electrons. 7.I have no idea how to even begin to answer this question.

53. 53 When rubidium ( 37 Rb) turns into its preferred ion by losing an electron, (Select all that apply.) 1.It is isoelectronic with 35 Br -1 2.It becomes positively charged 3.It turns into Kr 4.The resulting ion will be smaller than the atom it came from 5.Its electrons will be the same as the strontium ion’s electrons ( 38 Sr +2 )

54. 54 When rubidium ( 37 Rb) turns into its preferred ion by losing an electron, 1.It is isoelectronic with 35 Br -1 »The bromide ion has gained one e- making 36 electrons 2.It becomes positively charged »because it lost one electron: 37+ and 36- 3.It turns into Kr »(Of course the Rb +1 ion does not become Kr because it still only has 37 protons, not 36 like Kr) 4.The resulting ion will be smaller than the atom it came from »Cations (+ ions) are always smaller than their parent atom. 5.Its electrons will be the same as the strontium ion’s electrons ( 38 Sr +2 ) »The electrons for both of these ions will be the same as Kr’s electrons: 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 6

55. 55 Which is more reactive? 1. 3 Li 2. 11 Na 3. 19 K 4. 37 Rb 5.They are equally reactive because they are in the same chemical family. 6.I have no knowledge of how I might even decide this.

56. 56 Which is more reactive? 1. 3 Li 2. 11 Na 3. 19 Na 4. 37 Rb rubidium would be most reactive because the alkali metals are losing an electron, and it will be lost most vigorously when the electron being lost is furthest from the + pull of the nucleus. 5.They are equally reactive because they are in the same chemical family. 6.I have no knowledge of how I might even decide this.

57. 57 Which is more reactive? 1. 9 F 2. 17 Cl 3. 35 Br 4. 53 I 5.They are equally reactive because they are in the same chemical family. 6.I have no knowledge of how I might even decide this.

58. 58 Which is more reactive? 1. 9 F Halogens like to gain electrons and a smaller atom does that more vigorously because it is the nucleus (protons) pulling in the electron to be gained, and the closer it comes to the nucleus, the more vigorously it comes. 2. 17 Cl 3. 35 Br 4. 53 I 5.They are equally reactive because they are in the same chemical family. 6.I have no knowledge of how I might even decide this.

59. 59 Which is more reactive? 1. 8 O 2. 16 S 3. 34 Se 4. 52 Te 5.They are equally reactive because they are in the same chemical family.

60. 60 Which is more reactive? 1. 8 O Like the halogens, these atoms like to gain electrons and a smaller atom does that more vigorously because it is the nucleus (protons) pulling in the electron to be gained, and the closer it comes to the nucleus, the more vigorously it comes. 2. 16 S 3. 34 Se 4. 52 Te 5.They are equally reactive because they are in the same chemical family.

61. 61 1.1s 2 2s 2 2p 6 3s 2 2.1s 2 2s 2 2p 6 3s 1 3.1s 2 2s 2 2p 6 4. 1s 2 2s 2 2p 4 5. 1s 2 2s 2 2p 3 6. 1s 2 2s 2 2p 6 3s 2 3p 1 Which will normally form a negative ion? ( Select as many as apply.)

62. 62 1.1s 2 2s 2 2p 6 3s 2 2.1s 2 2s 2 2p 6 3s 1 3.1s 2 2s 2 2p 6 4. 1s 2 2s 2 2p 4 5. 1s 2 2s 2 2p 3 6. 1s 2 2s 2 2p 6 3s 2 3p 1 Which will normally form a negative ion? ( Select as many as apply.)

63. 63 1.[Ar] 4s 1 2.[Ar] 4s 2 3. [Ar] 4s 2 3d 10 4p 6 4. [Ar] 4s 2 3d 10 4p 5 5. [Ar] 4s 2 3d 10 4p 2 6. [Ar] 4s 2 3d 6 Which will normally form a negative ion? Select as many as apply.

64. 64 1.[Ar] 4s 1 2.[Ar] 4s 2 3. [Ar] 4s 2 3d 10 4p 6 4. [Ar] 4s 2 3d 10 4p 5 5. [Ar] 4s 2 3d 10 4p 2 6. [Ar] 4s 2 3d 6 Which will normally form a negative ion? Select as many as apply.

65. 65 1.1s 2 2s 2 2p 6 3s 2 2.1s 2 2s 2 2p 6 3s 1 3.1s 2 2s 2 2p 6 4. 1s 2 2s 2 2p 4 5. 1s 2 2s 2 2p 3 6. 1s 2 2s 2 2p 1 Which will have the lowest ionization energy?

66. 66 1.1s 2 2s 2 2p 6 3s 2 2.1s 2 2s 2 2p 6 3s 1 3.1s 2 2s 2 2p 6 4. 1s 2 2s 2 2p 4 5. 1s 2 2s 2 2p 3 6. 1s 2 2s 2 2p 1 Which will have the lowest ionization energy?

67. 67 1.1s 2 2s 2 2p 6 3s 2 2.1s 2 2s 2 2p 6 3s 1 3.1s 2 2s 2 2p 6 4. 1s 2 2s 2 2p 4 5. 1s 2 2s 2 2p 3 6. 1s 2 2s 2 2p 1 Which has(have) the greatest number of unpaired electrons? Select more than one in the case of a tie.

68. Draw orbital notation to help with this question. 1.1s 2 2s 2 2p 6 3s 2 2.1s 2 2s 2 2p 6 3s 1 3.1s 2 2s 2 2p 6 4. 1s 2 2s 2 2p 4 5. 1s 2 2s 2 2p 3 6. 1s 2 2s 2 2p 1 68 Which has(have) the greatest number of unpaired electrons? Select more than one in the case of a tie. ↑↓ ↑ ↑ ↑ ↑↓

69. 69 Which model below best represents the valence electrons for oxygen? 1. 2. 3. 4. 5. 6. ↑↓ ↑↓ ↑↓ ↑ ↑↓ ↑↓ ↑↓ ↑ ↑↓ ↑↓ ↑ ↑↓ ↑↓ ↑↓ ↑ ↑ ↑↓ ↑↓ ↑ ↑ ↑ ↑↓

70. 70 Which model below best represents the valence electrons for oxygen? 1. 2. 3. 4. 5. 6. ↑↓ ↑↓ ↑↓ ↑ ↑↓ ↑↓ ↑↓ ↑ ↑↓ ↑↓ ↑ ↑↓ ↑↓ ↑↓ ↑ ↑ ↑↓ ↑↓ ↑ ↑ ↑ ↑↓

71. 71 1.1s 2 2s 2 2p 6 3s 2 2.1s 2 2s 2 2p 6 3s 1 3.1s 2 2s 2 2p 6 4. 1s 2 2s 2 2p 4 5. 1s 2 2s 2 2p 3 6. 1s 2 2s 2 2p 1 Which metal would combine with oxygen in a one to one ratio. Select as many as apply.

72. 72 1.1s 2 2s 2 2p 6 3s 2 2.1s 2 2s 2 2p 6 3s 1 3.1s 2 2s 2 2p 6 4. 1s 2 2s 2 2p 4 5. 1s 2 2s 2 2p 3 6. 1s 2 2s 2 2p 1 Which metal would combine with oxygen in a one to one ratio. Select as many as apply.

73. 73 1.ns 1 2.ns 2 3. ns 2 np 1 4. ns 2 np 4 5. ns 2 np 5 6. ns 2 np 6 7. Without knowing which halogen, an answer can not be given. Which represents the valence electron configuration of the halogens? n represents the energy level

74. 74 1.ns 1 2.ns 2 3. ns 2 p 1 4. ns 2 p 4 5. ns 2 p 5 6. ns 2 p 6 7. Without knowing which halogen, an answer can not be given. Which represents the valence electron configuration of the halogens? n represents the energy level

75. 75 A certain nonmetallic element forms a compound with gallium having the general formula Ga 2 X 3. Element X must be a member of which group? 1.1A 2.2A 3.3A 4.4A 5.5A 6.6A 7.7A

76. 76 A certain nonmetallic element forms a compound with gallium having the general formula Ga 2 X 3. Element X must be a member of which group? 1.1A 2.2A 3.3A 4.4A 5.5A 6.6A 7.7A

77. 77 How many p orbitals are occupied in 6 C? 1.1 2.2 3.3 4.none

78. 78 How many p orbitals are occupied in 6 C? 1.1 2.2 both are half full, 1 e- each 3.3 4.none

79. 79 How many p orbitals are occupied in 16 S? 1.2 2.3 3.4 4.5 5.6 6.10 7.none

80. 80 How many p orbitals are occupied in 16 S? 1.2 2.3 3.4 4.5 5.6 1s 2 2s 2 2p 6 3s 2 3p 4 ↑↓ ↑↓ ↑↓ ↑↓ ↑↓ ↑↓ ↑↓ ↑ ↑ 7.10 8.none

81. 81 How many unpaired electrons in 16 S? 1.1 2.2 3.3 4.4 5.5 6.6

82. 82 How many unpaired electrons in 16 S? 1.1 2.2 [Ne] 3s 2 3p 4 ↑↓ ↑↓ ↑ ↑ 3.3 4.4 5.5 6.6