These are SELECTED questions from
Kotz and Moore that are related to our chapter 15. I restricted
them to multiple choice type questions.
1. Which of the following regions
of the electromagnetic spectrum have longer wavelengths than visible
light?
| 1. | FM radio waves |
| 2. | x-rays |
| 3. | microwaves |
| a. | 1 only |
| b. | 2 only |
| c. | 3 only |
| d. | 1 and 2 |
| e. | 1 and 3 |
ANS: E OBJ: 7.1 Electromagnetic Radiation
2. Which of the following regions of the electromagnetic spectrum has the longest wavelengths?
| a. | microwave |
| b. | infrared |
| c. | x-ray |
| d. | gamma ray |
| e. | visible |
ANS: A OBJ: 7.1 Electromagnetic Radiation
5. If an AM radio station broadcasts at 995 kHz, what is the wavelength of this radiation?
| a. | 6.59 × 10-28 m |
| b. | 1.01 × 10-6 m |
| c. | 3.32 × 10-3 m |
| d. | 301 m |
| e. | 2.98 × 1014 m |
ANS: D OBJ: 7.1 Electromagnetic Radiation
6. A microwave oven emits radiation at a wavelength of 0.500 cm. What is the frequency of this radiation?
| a. | 1.67 × 10-11 s-1 |
| b. | 6.67 × 10-7 s-1 |
| c. | 2.00 s-1 |
| d. | 1.50 × 106 s-1 |
| e. | 6.00 × 1010 s-1 |
ANS: E OBJ: 7.1 Electromagnetic Radiation
7. The ____ of a photon of light is ____ proportional to its frequency and ____ proportional to its wavelength.
| a. | amplitude, directly, inversely |
| b. | energy, inversely, directly |
| c. | energy, directly, inversely |
| d. | velocity, inversely, directly |
| e. | velocity, directly, inversely |
ANS: C OBJ: 7.2 Planck, Einstein, Energy,
and Photons
8. According to experiments concerned
with the photoelectric effect, which of the following will increase
the kinetic energy of an electron ejected from a metal surface?
| 1. | increasing the wavelength of the light striking the surface |
| 2. | increasing the frequency of the light striking the surface |
| 3. | increasing the number of photons of light striking the surface |
| a. | 1 only |
| b. | 2 only |
| c. | 3 only |
| d. | 1 and 2 |
| e. | 2 and 3 |
ANS: B OBJ: 7.2 Planck, Einstein, Energy,
and Photons
7.2
Planck, Einstein, Energy, and Photons
10. According to the Bohr model for the hydrogen atom, the energy necessary to excite an electron from n = 2 to n = 3 is ____ the energy necessary to excite an electron from n = 4 to n = 5.
| a. | less than |
| b. | greater than |
| c. | equal to |
| d. | either equal to or greater than |
| e. | either less than or equal to |
ANS: B OBJ: 7.3 Atomic Line Spectra
and Niels Bohr
11. Which of the following transitions in a hydrogen atom would emit the lowest energy photon?
| a. | n = 1 to n = 2 |
| b. | n = 3 to n = 2 |
| c. | n = 5 to n = 1 |
| d. | n = 2 to n = 8 |
| e. | n = 6 to n = 5 |
ANS: E OBJ: 7.3 Atomic Line Spectra
and Niels Bohr
12. For a hydrogen atom, calculate the energy of a photon in the Balmer series that results from the transition n = 3 to n = 2. What is the region of the electromagnetic spectrum? The Rydberg constant is -2.18 × 10-18 J.
| a. | 1.09 × 10-17 J; ultraviolet region |
| b. | 2.18 × 10-18 J; ultraviolet region |
| c. | 2.18 × 10-18 J; visible region |
| d. | 3.03 × 10-19 J; visible region |
| e. | 3.03 × 10-19 J; ultraviolet region |
ANS: D OBJ: 7.3 Atomic Line Spectra
and Niels Bohr
13. For a neutron (mass = 1.675 × 10-27 kg) moving with a velocity of 5.2 × 103 m/s, what is the de Broglie wavelength?
| a. | 7.6 × 10-11 m |
| b. | 4.5 × 10-9 m |
| c. | 2.1 × 10-6 m |
| d. | 486 m |
| e. | 1.3 × 1010 m |
ANS: A OBJ: 7.4 The Wave Properties
of the Electron
14. If the de Broglie wavelength of an electron is 555 nm, what is its velocity? The mass of an electron is 9.1 × 10-31 kg.
| a. | 4.0 × 10-10 m/s |
| b. | 7.6 × 10-4 m/s |
| c. | 5.2 × 102 m/s |
| d. | 1.3 × 103 m/s |
| e. | 2.5 × 109 m/s |
ANS: D OBJ: 7.4 The Wave Properties
of the Electron
16. Which of the following types of experiments demonstrate that an electron has the properties of a particle?
| a. | nuclear fission |
| b. | electron diffraction |
| c. | light emission from atomic gases |
| d. | mass spectroscopy |
| e. | photoelectric effect |
ANS: E OBJ: 7.5 Quantum Mechanical View
of the Atom
17. The Schrödinger wave equation
| a. | calculates the position and momentum of an electron at any given time. |
| b. | can be solved to determine the probability of finding an electron in a region of space. |
| c. | proves that energy is equal to mass times the speed of light squared. |
| d. | incorrectly predicts circular orbits of electrons around nuclei. |
| e. | is used to calculate the velocity of an electron. |
ANS: B OBJ: 7.5 Quantum Mechanical View
of the Atom
18. Which of the following statements is INCORRECT?
| a. | The location and the energy of an electron in an atom can be simultaneously known with little or no uncertainty. |
| b. | The energies of an atom's electrons are quantized. |
| c. | Quantum numbers define the energy states and the orbitals available to an electron. |
| d. | The behavior of an atom's electrons can be described by standing waves. |
| e. | Electrons have both wave and particle properties. |
ANS: A OBJ: 7.5 Quantum Mechanical View
of the Atom
19. What type of orbital is designated n = 3, l = 2, ml = -1?
| a. | 3s |
| b. | 3p |
| c. | 3d |
| d. | 2f |
| e. | 2d |
ANS: C OBJ: 7.5 Quantum Mechanical View
of the Atom
21. What type of orbital is designated n = 4, l = 3, ml = -3?
| a. | 4s |
| b. | 4p |
| c. | 4d |
| d. | 4f |
| e. | none |
ANS: D OBJ: 7.5 Quantum Mechanical View
of the Atom
22. What shell contains a total of 9 orbitals?
| a. | n = 1 |
| b. | n = 2 |
| c. | n = 3 |
| d. | n = 4 |
| e. | n = 5 |
ANS: C OBJ: 7.5 Quantum Mechanical View
of the Atom
23. Which of the following sets of quantum numbers refers to a 4p orbital?
| a. | n = 1, l = 1, ml = -1 |
| b. | n = 1, l = 2, ml = -1 |
| c. | n = 4, l = 1, ml = 0 |
| d. | n = 4, l = 2, ml = -1 |
| e. | n = 4, l = 3, ml = +2 |
ANS: C OBJ: 7.5 Quantum Mechanical View
of the Atom
24. How many orbitals have the following set of quantum numbers: n = 6, l = 3, ml = -2?
| a. | 0 |
| b. | 1 |
| c. | 3 |
| d. | 6 |
| e. | 7 |
ANS: B OBJ: 7.5 Quantum Mechanical View
of the Atom
25. All of the following sets of quantum numbers are allowed EXCEPT
| a. | n = 6, l = 0, ml = +1 |
| b. | n = 5, l = 4, ml = 0 |
| c. | n = 4, l = 1, ml = -1 |
| d. | n = 3, l = 2, ml = +2 |
| e. | n = 1, l = 0, ml = 0 |
ANS: A OBJ: 7.5 Quantum Mechanical View
of the Atom
26. All of the following sets of quantum numbers are allowed EXCEPT
| a. | n = 5, l = 3, ml = +2 |
| b. | n = 3, l = 2, ml = -1 |
| c. | n = 3, l = 0, ml = 0 |
| d. | n = 4, l = 4, ml = -2 |
| e. | n = 5, l = 3, ml = +3 |
ANS: D OBJ: 7.5 Quantum Mechanical View
of the Atom
27. What is the total number of orbitals having n = 5 and l = 1?
| a. | 1 |
| b. | 2 |
| c. | 3 |
| d. | 5 |
| e. | 10 |
ANS: C OBJ: 7.5 Quantum Mechanical View
of the Atom
28. Which of the following properties is associated with the value of the ml quantum number?
| a. | the number of electrons in an orbital |
| b. | the size of an orbital |
| c. | the shape of an orbital |
| d. | the energy of an orbital |
| e. | the orientation in space of an orbital |
ANS: E OBJ: 7.5 Quantum Mechanical View
of the Atom
29. Which of the following properties is associated with the value of the l quantum number?
| a. | the number of electrons in an orbital |
| b. | the size of an orbital |
| c. | the orientation in space of an orbital |
| d. | the energy of an orbital |
| e. | the shape of an orbital |
ANS: E OBJ: 7.5 Quantum Mechanical View
of the Atom
30. Which of the following orbitals might have ml = -2?
| a. | s |
| b. | s and p |
| c. | p and d |
| d. | d and f |
| e. | p, d, and f |
ANS: D OBJ: 7.5 Quantum Mechanical View
of the Atom
31. How many nodal planes exist for a 2p orbital?
| a. | 0 |
| b. | 1 |
| c. | 2 |
| d. | 3 |
| e. | 4 |
ANS: B OBJ: 7.5 Quantum Mechanical View
of the Atom
32. The n = ____ shell is the lowest that may contain p-orbitals.
| a. | 2 |
| b. | 3 |
| c. | 4 |
| d. | 5 |
| e. | 6 |
ANS: A OBJ: 7.5 Quantum Mechanical View
of the Atom
33. Which of the following shapes
represent d-orbitals?
| a. | (I) only |
| b. | (II) only |
| c. | (III) only |
| d. | (IV) only |
| e. | (I) and (IV) |
ANS: E OBJ: 7.5 Quantum Mechanical View
of the Atom
34. Which of the following shapes
represent p-orbitals?
| a. | (I) only |
| b. | (II) only |
| c. | (III) only |
| d. | (IV) only |
| e. | (I) and (II) |
ANS: B OBJ: 7.5 Quantum Mechanical View
of the Atom
35. Light has a frequency of 5.45 × 1014 hertz. What is its wavelength? The speed of light is 3.00 × 108 m/s.
| a. | 1.82 × 106 nm |
| b. | 1.82 × 10-3 nm |
| c. | 1.82 × 105 nm |
| d. | 5.50 × 10-7 nm |
| e. | 550 nm |
ANS: E OBJ: 07-1 Electromagnetic Radiation
and Matter
37. Arrange the following four electromagnetic
spectral regions in order of increasing energy.
| visible | ultraviolet | infrared | radio |
| a. | visible, ultraviolet, radio, infrared |
| b. | radio, ultraviolet, visible, infrared |
| c. | radio, infrared, visible, ultraviolet |
| d. | infrared, ultraviolet, visible, radio |
| e. | infrared, visible, ultraviolet, radio |
ANS: C OBJ: 07-2 Planck's Quantum Theory
38. Which wavelength of light is the fastest?
| a. | 418.6 nm |
| b. | 554.9 nm |
| c. | 626.1 nm |
| d. | 563.8 nm |
| e. | All have the same speed. |
ANS: E OBJ: 07-2 Planck's Quantum Theory
39. What is the phenomenon that occurs when certain metals emit electrons when illuminated by particular wavelengths of light?
| a. | Planck's constant |
| b. | photoelectric effect |
| c. | emission spectrum |
| d. | quantum theory |
| e. | electromagnetic spectrum |
ANS: B OBJ: 07-2 Planck's Quantum Theory
40. Which statement about light is true?
| a. | It oscillates back and forth between wave and particle-like behavior. |
| b. | It exhibits both wave and particle-like behavior at the same time. |
| c. | It has neither wave nor particle-like behavior. |
| d. | It behaves as a particle only. |
| e. | It behaves as a wave only. |
ANS: B OBJ: 07-2 Planck's Quantum Theory
42. Determine the energy of a photon that has a wavelength of 645 nm. The speed of light is 3.00 × 108 m/s and h = 6.63 × 10-34 J s.
| a. | 1.43 × 10-48 J |
| b. | 3.08 × 10-28 J |
| c. | 1.99 × 10-25 J |
| d. | 3.08 × 10-19 J |
| e. | 4.65 × 1014 J |
ANS: D OBJ: 07-2 Planck's Quantum Theory
43. What is a photon?
| a. | light that comes from a cathode ray tube |
| b. | a high speed electron that gives off light when it strikes an object |
| c. | very high frequency light |
| d. | very long wavelength light |
| e. | a massless "particle" or bundle of energy that moves at the speed of light |
ANS: E OBJ: 07-2 Planck's Quantum Theory
44. Which of the following is not a characteristic of the Bohr model of the atom?
| a. | An electron is located in an orbit around the nucleus. |
| b. | Each orbit has a discrete energy associated with it. |
| c. | Orbits have defined radii. |
| d. | There is a continuum of energy levels that an electron can have around a nucleus. |
| e. | Orbits have a defined circumference. |
ANS: D OBJ: 07-3 The Bohr Model of the Hydrogen
Atom
45. Which statement regarding the Bohr model of the atom is false?
| a. | Atoms produce line spectra. |
| b. | When the electron in hydrogen gains a quantized amount of energy, it moves to the ground state. |
| c. | Electrons cannot be located between energy levels. |
| d. | Light is emitted when an electron moves from the excited to the ground state. |
| e. | Electrons in the lowest energy level are in the ground state. |
ANS: B OBJ: 07-3 The Bohr Model of the Hydrogen
Atom
49. Which statement regarding an orbital is false?
| a. | An orbital is three dimensional. |
| b. | Only one electron is allowed per orbital. |
| c. | An electron shell consists of a collection of orbitals with the same principal quantum number. |
| d. | An orbital may be designated with the letters s, p, d, f. |
| e. | An orbital describes the location of the electron 90% of the time. |
ANS: C OBJ: 07-5 Quantum Numbers, Energy
Levels and Orbitals
50. The designation for the principal quantum number is:
| a. | n |
| b. | s |
| c. | ml |
| d. | l |
| e. | ms |
ANS: A OBJ: 07-5 Quantum Numbers, Energy
Levels and Orbitals
51. Which orbital angular momentum (azimuthal) quantum numbers can exist for n = 3?
| a. | l = 0 |
| b. | l = 0, 1 |
| c. | l = 0, 1, 2 |
| d. | l = 0, 1, 2, 3 |
| e. | l = 0, 1, 2, 3, 4 |
ANS: C OBJ: 07-5 Quantum Numbers, Energy
Levels and Orbitals
52. If l = 1, what value can ml have?
| a. | ml = -1 |
| b. | ml = +1 |
| c. | ml = 0, +1 |
| d. | ml = 0 |
| e. | ml = -1, 0, +1 |
ANS: E OBJ: 07-5 Quantum Numbers, Energy
Levels and Orbitals
53. How many electrons can the second principal quantum level hold?
| a. | 2 |
| b. | 8 |
| c. | 16 |
| d. | 18 |
| e. | 32 |
ANS: B OBJ: 07-5 Quantum Numbers, Energy
Levels and Orbitals
54. How many orbitals are contained in the 4d subshell?
| a. | 2 |
| b. | 5 |
| c. | 6 |
| d. | 10 |
| e. | 14 |
ANS: B OBJ: 07-5 Quantum Numbers, Energy
Levels and Orbitals
55. How many electrons can be contained in the 2p subshell?
| a. | 1 |
| b. | 2 |
| c. | 3 |
| d. | 4 |
| e. | 6 |
ANS: E OBJ: 07-5 Quantum Numbers, Energy
Levels and Orbitals
56. Which statement is false?
| a. | The d orbitals occur in groups of 3. |
| b. | The 3p orbitals have higher energy than the 2p orbitals. |
| c. | The 3d and 4d orbitals hold the same number of electrons. |
| d. | Two electrons in the same orbital will have opposite spin. |
| e. | The 1s orbital holds up to 2 electrons. |
ANS: A OBJ: 07-5 Quantum Numbers, Energy
Levels and Orbitals
57. The d orbitals occur in groups of _________ and hold up to _________ electrons.
| a. | 3, 6 |
| b. | 4, 8 |
| c. | 5, 10 |
| d. | 6, 12 |
| e. | 7, 14 |
ANS: C OBJ: 07-5 Quantum Numbers, Energy
Levels and Orbitals
58. Which set of quantum numbers is not allowed?
| a. | n = 0, l = 0, ml = 0, ms = +1/2 |
| b. | n = 1, l = 0, ml = 0, ms = +1/2 |
| c. | n = 2, l = 1, ml = 1, ms = +1/2 |
| d. | n = 3, l = 1, ml = 0, ms = +1/2 |
| e. | n = 4, l = 3, ml = 0, ms = -1/2 |
ANS: A OBJ: 07-5 Quantum Numbers, Energy
Levels and Orbitals
59. What is the correct electron configuration for beryllium (Be)?
| a. | 1s22s2 |
| b. | 1s22s22p1 |
| c. | 1s22s22p2 |
| d. | 1s22s22p4 |
| e. | 1s22s22p6 |
ANS: A OBJ: 07-6 Atom Electron Configurations
60. What is the correct electron configuration for aluminum?
| a. | 1s22s1 |
| b. | 1s22s22p43s23p3 |
| c. | 1s22s22p63s23p1 |
| d. | 1s22s22p23s23p23d24s1 |
| e. | 1s22s22p23s23p24s25s1 |
ANS: C OBJ: 07-6 Atom Electron Configurations
61. What is the correct electron configuration for bromine?
| a. | 1s22s22p5 |
| b. | 1s22s22p63s23p63d94s24p6 |
| c. | 1s22s22p63s23p63d104s24p5 |
| d. | 1s22s22p63s23p64s23d54p64d25s2 |
| e. | 1s22s22p63s23p64s24p65s25p66s1 |
ANS: C OBJ: 07-6 Atom Electron Configurations
62. Give the element that has the electron configuration:
1s22s22p63s23p63d104s24p65s2
| a. | In |
| b. | Pd |
| c. | Fe |
| d. | Ni |
| e. | Sr |
ANS: E OBJ: 07-6 Atom Electron Configurations
63. Which of the following corresponds to the electron configuration of a noble gas?
| a. | 1s22s2 |
| b. | 1s22s22p4 |
| c. | 1s22s22p63s23p63d104s24p2 |
| d. | 1s22s22p63s23p63d104s24p3 |
| e. | 1s22s22p63s23p6 |
ANS: E OBJ: 07-6 Atom Electron Configurations
64. What is the correct shorthand notation for the electron configuration given?
1s22s22p63s23p64s23d104p1
| a. | [Ca]3d104p1 |
| b. | [Zn]4p1 |
| c. | [Ne]3s23p63d104s24p1 |
| d. | [Ar] 3d104s24p1 |
| e. | all of the above |
ANS: D OBJ: 07-6 Atom Electron Configurations
65. What is the electron configuration of Br-?
| a. | 1s22s22p4 |
| b. | 1s22s22p6 |
| c. | 1s22s22p63s23p63d104s24p6 |
| d. | 1s22s22p63s23p63d104s24p5 |
| e. | 1s22s22p63s23p63d104s24p4 |
ANS: C OBJ: 07-7 Ion Electron Configurations
66. What is the electron configuration of O2-?
| a. | 1s22s22p5 |
| b. | 1s22s22p6 |
| c. | 1s22s22p4 |
| d. | 1s22s22p2 |
| e. | 1s22s22p3 |
ANS: B OBJ: 07-7 Ion Electron Configurations
67. What is the electron configuration of Li+?
| a. | 1s1 |
| b. | 1s2 |
| c. | 1s22s1 |
| d. | 1s22s2 |
| e. | 1s22s22p1 |
ANS: B OBJ: 07-7 Ion Electron Configurations
68. What is the electron configuration of Al3+?
| a. | 1s22s22p5 |
| b. | 1s22s22p4 |
| c. | 1s22s22p2 |
| d. | 1s22s22p6 |
| e. | 1s22s22p63s23p1 |
ANS: D OBJ: 07-7 Ion Electron Configurations
69. Which of the following has the electron configuration 1s22s22p63s23p6?
| a. | Ca |
| b. | Cl |
| c. | Ar |
| d. | K+ |
| e. | Both c and d |
ANS: E OBJ: 07-7 Ion Electron Configurations
70. Substances that have the same electron configuration are:
| a. | paramagnetic. |
| b. | diamagnetic. |
| c. | ferromagnetic. |
| d. | lanthanides. |
| e. | isoelectronic. |
ANS: E OBJ: 07-7 Ion Electron Configurations
71. Atoms or ions without unpaired electrons are:
| a. | isoelectronic. |
| b. | paramagnetic. |
| c. | diamagnetic. |
| d. | ferromagnetic. |
| e. | lanthanides. |
ANS: C OBJ: 07-7 Ion Electron Configurations
73. Xenon, the iodide negative ion and the cesium positive ion are:
| a. | paramagnetic. |
| b. | diamagnetic. |
| c. | ferromagnetic. |
| d. | lanthanides. |
| e. | isoelectronic. |
ANS: E OBJ: 07-7 Ion Electron Configurations
74. Which element has the largest atomic radius?
| a. | F |
| b. | He |
| c. | O |
| d. | H |
| e. | Na |
ANS: E OBJ: 07-8 Periodic Trends: Atomic
Radii
76. Arrange the elements given in order
from largest to smallest atomic radii.
| Al | Ca | Sr | Mg | S |
| a. | Sr > Ca > Mg > Al >S |
| b. | Sr > Ca > S > Al > Mg |
| c. | Al > Sr > S > Ca > Mg |
| d. | Ca > Mg > Sr > Al > S |
| e. | Mg > Al > S > Ca > Sr |
ANS: A OBJ: 07-8 Periodic Trends: Atomic
Radii
77. Which of the following has the largest ionic radius?
| a. | Li+ |
| b. | F- |
| c. | S2- |
| d. | Na+ |
| e. | Cl- |
ANS: C OBJ: 07-9 Periodic Trends: Ionic
Radii
78. Which statement is false?
| a. | Cations are smaller than their corresponding neutral atom. |
| b. | Anions are smaller than their corresponding neutral atom. |
| c. | Mg2+ is larger than Be2+. |
| d. | O2- is larger than F-. |
| e. | Br- is smaller than I-. |
ANS: B OBJ: 07-9 Periodic Trends: Ionic
Radii
79. Which element has the largest first ionization energy?
| a. | Be |
| b. | Ca |
| c. | Mg |
| d. | Sr |
| e. | Ba |
ANS: A OBJ: 07-10 Periodic Trends: Ionization
Energies
80. Arrange the following in order of
increasing ionization energy.
| Ar | Cl | Li | Na | P |
| a. | P < Cl < Ar < Li < Na |
| b. | Na < Li < P < Cl < Ar |
| c. | Ar < Cl < Na < Li < P |
| d. | Cl < Ar < Na < Li < P |
| e. | P < Cl < Ar < Na < Li |
ANS: B OBJ: 07-10 Periodic Trends: Ionization
Energies
82. The Pauli exclusion principle states that
spins.ANS: A OBJ: 8.2 The Pauli Exclusion
Principle
83. How many electrons can be described by the following quantum numbers: n = 4, l = 3, ml = -2, ms = +1/2?
| a. | 0 |
| b. | 1 |
| c. | 2 |
| d. | 3 |
| e. | 6 |
ANS: B OBJ: 8.2 The Pauli Exclusion
Principle
84. What is the maximum number of electrons that can occupy the n = 5 shell?
| a. | 5 |
| b. | 10 |
| c. | 14 |
| d. | 25 |
| e. | 50 |
ANS: E OBJ: 8.2 The Pauli Exclusion
Principle
85. Which of the following statements
regarding subshell filling order are CORRECT?
| 1. | Electrons are assigned to the 4s subshell before they are assigned to the 3d subshell. |
| 2. | Electrons are assigned to the 4f subshell before they are assigned to the 6s subshell. |
| 3. | Electrons are assigned to the 5d subshell before they are assigned to the 6p subshell. |
| a. | 1 only |
| b. | 2 only |
| c. | 3 only |
| d. | 1 and 3 |
| e. | 1, 2, and 3 |
ANS: D OBJ: 8.3 Atomic Subshell Energies
and Electron Assignments
86. Which of the following statements
concerning ground state electron configurations are CORRECT?
| 1. | In a hydrogen atom with one electron, the 2s and 2p orbitals have different energy. |
| 2. | For a lithium atom with three electrons, the 2s and 2p orbitals have different energies. |
| 3. | The effective nuclear charge felt by an electron in a 2p orbital is larger for carbon than for fluorine. |
| a. | 1 only |
| b. | 2 only |
| c. | 3 only |
| d. | 1 and 3 |
| e. | 1, 2, and 3 |
ANS: B OBJ: 8.3 Atomic Subshell Energies
and Electron Assignments
87. Which of the following elements is an s-block element?
| a. | C |
| b. | Cd |
| c. | Cs |
| d. | Cl |
| e. | Cf |
ANS: C OBJ: 8.4 Atomic Electron Configurations
89. Which of the following atoms is paramagnetic?
| a. | Se |
| b. | Cd |
| c. | Ar |
| d. | He |
| e. | Ca |
ANS: A OBJ: 8.4 Atomic Electron Configurations
90. Which of the following atoms is diamagnetic?
| a. | Rb |
| b. | C |
| c. | F |
| d. | Cu |
| e. | Sr |
ANS: E OBJ: 8.4 Atomic Electron Configurations
91. Hund's rule states that the most stable arrangement of electrons (for a ground state electron configuration)
| a. | has a filled valence shell of electrons. |
| b. | has two electrons per orbital, each with identical spins. |
| c. | has m? values greater than or equal to zero. |
| d. | has the maximum number of unpaired electrons, all with the same spin. |
| e. | has two electrons per orbital, each with opposing spins. |
ANS: D OBJ: 8.4 Atomic Electron Configurations
92. Which element has the following
electron configuration?
| a. | P |
| b. | S |
| c. | O |
| d. | N |
| e. | F |
ANS: D OBJ: 8.4 Atomic Electron Configurations
93. Which element has the following
electron configuration?
| a. | Br |
| b. | Se |
| c. | S |
| d. | Cl |
| e. | Ge |
ANS: B OBJ: 8.4 Atomic Electron Configurations
94. What is a possible set of quantum
numbers for the unpaired electron in the orbital box diagram below?
| a. | n = 3, l = 1, ml = -1, ms = +1/2 |
| b. | n = 3, l = 2, ml = -1, ms = -1/2 |
| c. | n = 3, l = 2, ml = -2, ms = +1/2 |
| d. | n = 4, l = 0, ml = 0, ms = +1/2 |
| e. | n = 4, ? = 1, m? = -1, ms = +1/2 |
ANS: E OBJ: 8.4 Atomic Electron Configurations
96. Which 3+ ion has the ground state electron configuration [Kr]4d5?
| a. | Ru |
| b. | Fe |
| c. | Ag |
| d. | Tc |
| e. | Nb |
ANS: A OBJ: 8.5 Electron Configurations
of Ions
97. What is the ground state electron configuration for Sn2+?
| a. | [Kr]4d105s2 |
| b. | [Kr]4d105p2 |
| c. | [Kr]5s2 |
| d. | [Kr]4f145d10 |
| e. | [Kr]4f145d105s2 |
ANS: A OBJ: 8.5 Electron Configurations
of Ions
98. Which of the following ions have the same ground state electron configuration: Sn4+, Pb4+, Sr2+, and Br-?
| a. | Sn4+ and Pb4+ |
| b. | Pb4+ and Sr2+ |
| c. | Sr2+ and Br- |
| d. | Pb4+ and Br- |
| e. | Sn4+, Sr2+, and Br- |
ANS: C OBJ: 8.5 Electron Configurations
of Ions
99. What 3- ion has the following
ground state electron configuration?
| a. | oxide ion |
| b. | nitride ion |
| c. | sodium ion |
| d. | aluminum ion |
| e. | phosphide ion |
ANS: E OBJ: 8.5 Electron Configurations
of Ions
100. What 2+ ion has the following
ground state electron configuration?
| a. | Ni2+ |
| b. | Co2+ |
| c. | Ca2+ |
| d. | Cu2+ |
| e. | Mn2+ |
ANS: B OBJ: 8.5 Electron Configurations
of Ions
101. What 1+ ion has the following
ground state electron configuration?
| a. | K+ |
| b. | Rb+ |
| c. | In+ |
| d. | Tl+ |
| e. | Y+ |
ANS: C OBJ: 8.5 Electron Configurations
of Ions
102. Which of the following cations has four unpaired electrons in the ground state?
| a. | Ni2+ |
| b. | Fe2+ |
| c. | Pb2+ |
| d. | Mn2+ |
| e. | Cu2+ |
ANS: B OBJ: 8.5 Electron Configurations
of Ions
104. Place the following atoms in order of increasing atomic radii: Ca, Mg, P, and Cl.
| a. | Cl < P < Mg < Ca |
| b. | Mg < P < Cl < Ca |
| c. | Ca < Mg < P < Cl |
| d. | P < Cl < Mg < Ca |
| e. | Ca < Cl < P < Mg |
ANS: A OBJ: 8.6 Atomic Properties and
Periodic Trends
106. Which one of the following statements is INCORRECT?
| a. | Ionization energy is always a positive value. |
| b. | Ionization energy is the energy required to remove an electron from a gaseous atom. |
| c. | For any element, the second ionization energy is larger than the first ionization energy. |
| d. | Ionization energy decreases across a periodic of the periodic table. |
| e. | Ionization energy decreases down a group of the periodic table |
ANS: D OBJ: 8.6 Atomic Properties and
Periodic Trends
107. Which of the following chemical equations refers to the second ionization of Mg?
| a. | Mg(s) + 2e- ? Mg2-(s) |
| b. | Mg(s) ? Mg+(s) + e- |
| c. | Mg(g) ? Mg2+(g) + 2e- |
| d. | Mg+(g) ? Mg2+(g) + e- |
| e. | Mg2+(g) + e- ? Mg+(g) |
ANS: D OBJ: 8.6 Atomic Properties and
Periodic Trends
108. Which of the following elements would have the greatest difference between the first and the second ionization energies?
| a. | Mg |
| b. | Al |
| c. | K |
| d. | Ca |
| e. | Sr |
ANS: C OBJ: 8.6 Atomic Properties and
Periodic Trends
109. Rank K, Li, and Cs in order of increasing first ionization energy.
| a. | K < Cs < Li |
| b. | Cs < K < Li |
| c. | Cs < Li < K |
| d. | Li < Cs < K |
| e. | Li < K < Cs |
ANS: B OBJ: 8.6 Atomic Properties and
Periodic Trends
110. The change in energy for the
following reaction is referred to as the ____ for fluorine.
F(g) + e- ? F-(g)
| a. | oxidation energy |
| b. | electron affinity |
| c. | electronegativity energy |
| d. | first ionization energy |
| e. | second ionization energy |
ANS: B OBJ: 8.6 Atomic Properties and
Periodic Trends
112. Which group of the periodic table of elements forms only 2+ ions?
| a. | group 1A |
| b. | group 2A |
| c. | group 7B |
| d. | group 7A |
| e. | group 8A |
ANS: B OBJ: 8.6 Atomic Properties and
Periodic Trends
113. Place the following ions in order from smallest to largest ionic radii: P3-, K+, Na+, and Cl-.
| a. | Na+ < K+ < Cl- < P3- |
| b. | K+ < Na+ < Cl- < P3- |
| c. | Cl- < P3- < Na+ < K+ |
| d. | Cl- < P3- < K+ < Na+ |
| e. | P3- < Cl- < K+ < Na+ |
ANS: A OBJ: 8.6 Atomic Properties and
Periodic Trends