1. All of the atoms of the elements in Period 2 have the same number of

Atomic Theory & Periodic Table Review

Name: Date:

1. All of the atoms of the elements in Period 2 have the same number of

A. protons B. neutrons

C. valence electrons

D. occupied principal energy levels

2. Which of these elements in Period 3 has the least tendency to attract electrons?

A. Mg B. Al C. S D. Cl

3. The elements from which two groups of the Periodic Table are most similar in their chemical properties?

A. 1 and 2 B. 1 and 17

C. 2 and 17 D. 17 and 18

4. Which element in Group 1 has the greatest tendency to lose an electron?

A. cesium B. rubidium

C. potassium D. sodium

5. As the elements in Group 2 are considered in order of increasing atomic number, the atomic radius of each successive element increases. This increase is primarily due to an increase in the number of

A. occupied principal energy levels B. electrons in the outermost shell C. neutrons in the nucleus

D. unpaired electrons

6. In the ground state, atoms of the elements in Group 15 of the Periodic Table all have the same number of

A. lled principal energy levels B. occupied principal energy levels C. neutrons in the nucleus

D. electrons in the valence shell

7. The elements in the modern Periodic Table are arranged according to their

A. atomic number B. oxidation number C. atomic mass D. nuclear mass 8. As atoms of elements in Group 16 are considered

in order from top to bottom, the electronegativity of each successive element

A. decreases B. increases C. remains the same

9. Most of the groups in the Periodic Table of the Elements contain

A. nonmetals, only B. metals, only

C. nonmetals and metals D. metals and metalloids 10. Which element is an alkali metal?

A. Na B. Mg C. Al D. Cl

11. The properties of carbon are expected to be most similar to those of

A. boron B. aluminum

C. silicon D. phosphorus

12. The elements known as the alkaline earth metals are found in Group

A. 1 B. 2 C. 16 D. 17

13. A substance that is composed only of atoms having the same atomic number is classi ed as

A. a compound B. an element

C. a homogeneous mixture D. a heterogeneous mixture

14. Which statement describes the general trends in electronegativity and rst ionization energy as the elements in Period 3 are considered in order from Na to Cl?

A. Electronegativity increases, and rst ionization energy decreases.

B. Electronegativity decreases, and rst ionization energy increases.

C. Electronegativity and rst ionization energy both increase.

D. Electronegativity and rst ionization energy both decrease.

15. Compared to the atoms of nonmetals in Period 3, the atoms of metals in Period 3 have

A. fewer valence electrons B. more valence electrons C. fewer electron shells D. more electron shells

16. Compared to the nonmetals in Period 2, the metals in Period 2 generally have larger

A. ionization energies B. electronegativities C. atomic radii D. atomic numbers 17. The elements in Period 3 all contain the same

number of

A. protons B. neutrons

C. valence electrons

D. occupied principal energy levels

18. In Period 2 of the Periodic Table, which Group contains the element with the highest rst ionization energy?

A. alkali metals B. alkaline earth metals C. halogens

D. noble gases

19. In general, atoms of transition elements in Period 5 are characterized by an incomplete

A. 3p subshell B. 4p subshell C. 3d subshell D. 4d subshell 20. Which statement describes the elements in

Period 3?

A. Each successive element has a greater atomic radius.

B. Each successive element has a lower electronegativity.

C. All elements have similar chemical properties.

D. All elements have valence electrons in the

same principal energy level.

21. Base your answer(s) to the following question(s) on the information below.

The atomic and ionic radii for sodium and chlorine are shown in the table below.

Atomic and Ionic Radii Particle Radius (pm) Na atom 190.

Na

ion 102

Cl atom 97

Cl ion 181

Write the ground state electron con guration for the ion that has a radius of l8l picometers.

22. What is the total number of protons in an atom with the electron con guration 2-8-18-32-18-1?

A. 69 B. 79 C. 118 D. 197

23. Base your answer(s) to the following question(s) on the electron con guration table shown.

Element Electron Con guration

X 2-8-8-2

Y 2-8-7-3

Z 2-8-8

What is the total number of valence electrons in an atom of electron con guration X?

24. Which electron con guration is correct for a sodium ion?

A. 2–7 B. 2–8 C. 2–8–1 D. 2–8–2 25. What is the electron con guration of a sulfur atom

in the ground state?

A. 2–4 B. 2–6 C. 2–8–4 D. 2–8–6 26. What is the total number of valence electrons

in an atom with the electron con guration 1s

2s

2p

3s

3p

?

A. 15 B. 2 C. 3 D. 5

27. What is the total number of valence electrons in an atom with the electron con guration 1s

2s

2p

3s

3p

?

A. 6 B. 2 C. 3 D. 5

28. An atom in the ground state has 7 valence electrons. Which electron con guration could represent the outermost principal energy level of this atom in the ground state?

A. 3s

3p

B. 3s

3p

C. 3s

3p

3d

D. 3s

3p

3d

29. The correct electron con guration of the O

ion is

A. 1s

2s

2p

B. 1s

2s

2p

C. 1s

2s

2p

D. 1s

2s

2p

30. The number of valence electrons in an atom with an electron con guration of 1s

2s

2p

3s

3p

is

A. 6 B. 2 C. 16 D. 4

31. Draw a Lewis electron-dot diagram for an atom of silicon.

32. Which Lewis electron-dot diagram represents a nitrogen atom in the ground state?

A. B. C. D.

33. An atom in the ground state contains a total of 5 electrons, 5 protons, and 5 neutrons. Which Lewis electron-dot diagram represents this atom?

A. B. C. D.

34. Which Lewis electron-dot diagram is correct for a S

ion?

A. B.

C. D.

35. Which symbol represents an atom in the ground state with the most stable valence electron con guration?

A. B B. O C. Li D. Ne

36. Which element has an atom in the ground state with a total of three valence electrons?

A. aluminum B. lithium

C. phosphorus D. scandium 37. Magnesium and calcium have similar chemical

properties because a magnesium atom and a calcium atom have the same

A. atomic number B. mass number

C. total number of electron shells D. total number of valence electrons

38. When an excited electron in an atom moves to the ground state, the electron

A. absorbs energy as it moves to a higher energy state

B. absorbs energy as it moves to a lower energy state

C. emits energy as it moves to a higher energy state

D. emits energy as it moves to a lower energy state

39. During a ame test, a lithium salt produces a characteristic red ame. This red color is produced when electrons in excited lithium atoms

A. are lost by the atoms B. are gained by the atoms

C. return to lower energy states within the atoms D. move to higher energy states within the atoms 40. The bright-line spectrum of an element in the

gaseous phase is produced as

A. protons move from lower energy states to higher energy states

B. protons move from higher energy states to lower energy states

C. electrons move from lower energy states to higher energy states

D. electrons move from higher energy states to lower energy states

41. Which quantity represents the number of protons in an atom?

A. atomic number B. oxidation number C. number of neutrons

D. number of valence electrons

42. Every chlorine atom has

A. 7 electrons B. 17 neutrons

C. a mass number of 35

D. an atomic number of 17

43. Each diagram below represents the nucleus of a di erent atom.

Which diagrams represent nuclei of the same element?

A. D and E, only B. D, E, and Q C. Q and R, only D. Q, R, and E 44. What can be determined if only the atomic number

of an atom is known?

A. the total number of neutrons in the atom, only B. the total number of protons in the atom, only C. the total number of protons and the total

number of neutrons in the atom

D. the total number of protons and the total number of electrons in the atom

45. The atomic mass of magnesium is the weighted average of the atomic masses of

A. all of the arti cially produced isotopes of Mg B. all of the naturally occurring isotopes of Mg C. the two most abundant arti cially produced

isotopes of Mg

D. the two most abundant naturally occurring isotopes of Mg

46. Which particles have approximately the same mass?

A. an electron and an alpha particle B. an electron and a proton

C. a neutron and an alpha particle D. a neutron and a proton

47. Which phrase describes an atom?

A. a negatively charged nucleus surrounded by positively charged protons

B. a negatively charged nucleus surrounded by positively charged electrons

C. a positively charged nucleus surrounded by negatively charged protons

D. a positively charged nucleus surrounded by negatively charged electrons

48. The notation for the nuclide

Cs gives information about

A. mass number, only B. atomic number, only

C. both mass number and atomic number D. neither mass number nor atomic number 49. What information is necessary to determine the

atomic mass of the element chlorine?

A. the atomic mass of each arti cially produced isotope of chlorine, only

B. the relative abundance of each naturally occurring isotope of chlorine, only

C. the atomic mass and the relative abundance of each naturally occurring isotope of chlorine D. the atomic mass and the relative abundance

of each naturally occurring and arti cially produced isotope of chlorine

50. Which particle has the least mass?

A.

He B.

H C.

n D.

e 51. What is the mass number of an alpha particle?

A. 1 B. 2 C. 0 D. 4

52. Which isotopic notation represents an atom of carbon-14?

A.

C B.

C C.

C D.

C 53. Which diagram represents the nucleus of an atom

of

Al ?

A. B.

C. D.

54. What is the mass number of an atom that has six protons, six electrons, and eight neutrons?

A. 6 B. 12 C. 14 D. 20

55. An atom of lithium-7 has an equal number of

A. electrons and neutrons B. electrons and protons C. positrons and neutrons D. positrons and protons

56. As a result of the gold foil experiment, it was concluded that an atom

A. contains protons, neutrons, and electrons B. contains a small, dense nucleus

C. has positrons and orbitals D. is a hard, indivisible sphere

57. What is the net charge of an ion that has 8 protons, 9 neutrons, and 10 electrons?

A. 1+ B. 2+ C. 1 D. 2

58. Which statement compares the masses of two subatomic particles?

A. The mass of an electron is greater than the mass of a proton.

B. The mass of an electron is greater than the mass of a neutron.

C. The mass of a proton is greater than the mass of an electron.

D. The mass of a proton is greater than the mass of a neutron.

59. Which subatomic particles are located in the nucleus of an He-4 atom?

A. electrons and neutrons B. electrons and protons C. neutrons and protons

D. neutrons, protons, and electrons

60. The mass of a proton is approximately equal to the mass of

A. an alpha particle B. a beta particle C. a positron D. a neutron 61. Which two particles have opposite charges?

A. an electron and a neutron B. an electron and a proton C. a proton and a neutron D. a proton and a positron

62. What is the total charge of the nucleus of a carbon atom?

A. 6 B. 0 C. +6 D. +12

63. The total mass of the protons in an atom of gold-198 is approximately

A. 79 atomic mass units B. 119 atomic mass units C. 198 atomic mass units D. 277 atomic mass units

64. Which statement describes the relative masses of two di erent particles?

A. A neutron has less mass than a positron.

B. A beta particle has less mass than a neutron.

C. An alpha particle has less mass than a positron.

D. An alpha particle has less mass than a beta particle.

65. Which particle has no charge?

A. electron B. neutron

C. positron D. proton

66. What is the total number of neutrons in an atom of O-18?

A. 18 B. 16 C. 10 D. 8

67. What is the total number of neutrons in an atom of

Fe ?

A. 26 B. 31 C. 57 D. 83

68. In which two atoms do both nuclides contain the same number of neutrons?

A.

Ne and

Ar B.

Cu and

Zn C.

Mg and

Mg D.

C and

O

69. An orbital of an atom is de ned as the most probable location of

A. an electron B. a neutron C. a positron D. a proton

70. What is the number of electrons in an atom that has 3 protons and 4 neutrons?

A. 1 B. 7 C. 3 D. 4

71. Which particle has the least mass?

A. alpha particle B. beta particle

C. neutron D. proton

72. When an atom of lithium loses an electron, the atom becomes a

A. negative ion with a radius smaller than the radius of the atom

B. negative ion with a radius larger than the radius of the atom

C. positive ion with a radius smaller than the radius of the atom

D. positive ion with a radius larger than the radius of the atom

73. An atom of which element has the largest atomic radius?

A. Fe B. Mg C. Si D. Zn

74. In the late 1800s, experiments using cathode ray tubes led to the discovery of the

A. electron B. neutron

C. positron D. proton

75. What is the total number of valence electrons in a calcium atom in the ground state?

A. 8 B. 2 C. 18 D. 20

76. What is the total number of electrons in a Mg

ion?

A. 10 B. 12 C. 14 D. 24

77. What can be concluded if an ion of an element is smaller than an atom of the same element?

A. The ion is negatively charged because it has fewer electrons than the atom.

B. The ion is negatively charged because it has more electrons than the atom.

C. The ion is positively charged because it has fewer electrons than the atom.

D. The ion is positively charged because it has more electrons than the atom.

78. Which symbol represents a particle with a total of 10 electrons?

A. N B. N

C. Al D. Al

79. How many electrons are in an Fe

ion?

A. 24 B. 26 C. 28 D. 56

80. What is the total number of electrons found in an atom of sulfur?

A. 6 B. 8 C. 16 D. 32

81. What must occur when an electron in an atom returns from a higher energy state to a lower energy state?

A. A speci c amount of energy is released.

B. A random amount of energy is released.

C. The atom undergoes transmutation.

D. The atom spontaneously decays.

82. Which atom in the ground state has an outermost electron with the most energy?

A. Cs B. K C. Li D. Na

83. The characteristic bright-line spectrum of an element is produced when electrons

A. absorb quanta and return to lower energy levels

B. absorb quanta and move to higher energy levels

C. release quanta and return to lower energy levels

D. release quanta and move to higher energy levels

84. What is the maximum number of electrons that can occupy the fourth principal energy level of an atom?

A. 6 B. 8 C. 18 D. 32

85. An element with a partially lled d sublevel in the ground state is classi ed as

A. a halogen B. a transition metal C. an alkali metal D. an alkaline earth metal

86. An electron will emit energy in quanta when its energy state changes from 4p to

A. 5s B. 5p C. 3s D. 6p

87. What is the total number of occupied sublevels in the third principal energy level of a zinc atom in the ground state?

A. 1 B. 2 C. 3 D. 4

88. As an electron moves from a 3s orbital to a 2s orbital, the energy of the atom

A. decreases B. increases

C. remains the same

89. What is the number of electrons in a completely lled second shell of an atom?

A. 32 B. 2 C. 18 D. 8

90. What is the total number of orbitals containing only one electron in an atom of nitrogen in the ground state?

A. 1 B. 2 C. 3 D. 4

91. Which orbital notation represents a noble gas in the ground state?

A.

B.

C.

D.

92. Which electron con guration represents an element with the highest rst ionization energy?

A. 1s

2s

B. 1s

2s

C. 1s

2s

2p

3s

D. 1s

2s

2p

3s

93. The orbital notation of an atom in the ground state

is .

Which atom is represented by this notation?

A. C B. N C. B D. Be

94. Which element has atoms with the strongest attraction for electrons in a chemical bond?

A. chlorine B. nitrogen

C. uorine D. oxygen

95. Which term represents the attraction one atom has for the electrons in a bond with another atom?

A. electronegativity B. electrical conductivity C. rst ionization energy D. mechanical energy

96. Which term represents the attraction one atom has for the electrons in a bond with another atom?

A. electronegativity B. electrical conductivity C. rst ionization energy D. mechanical energy

97. Samples of four Group 15 elements, antimony, arsenic, bismuth, and phosphorus, are in the gaseous phase. An atom in the ground state of which element requires the least amount of energy to remove its most loosely held electron?

A. As B. Bi C. P D. Sb

98. From which of these atoms in the ground state can a valence electron be removed using the least amount of energy?

A. nitrogen B. carbon

C. oxygen D. chlorine

99. As elements of Group 1 of the Periodic Table are considered in order from top to bottom, the ionization energy of each successive element decreases. This decrease is due to

A. decreasing radius and decreasing shielding e ect

B. decreasing radius and increasing shielding e ect

C. increasing radius and decreasing shielding e ect

D. increasing radius and increasing shielding

e ect

100. What occurs when an atom of chlorine forms a chloride ion?

A. The chlorine atom gains an electron, and its radius becomes smaller.

B. The chlorine atom gains an electron, and its radius becomes larger.

C. The chlorine atom loses an electron, and its radius becomes smaller.

D. The chlorine atom loses an electron, and its radius becomes larger.

101. Which change occurs when a barium atom loses two electrons?

A. It becomes a negative ion and its radius decreases.

B. It becomes a negative ion and its radius increases.

C. It becomes a positive ion and its radius decreases.

D. It becomes a positive ion and its radius increases.

102. What is the overall charge of an ion that has 12 protons, 10 electrons, and 14 neutrons?

A. 2 B. 2+ C. 4 D. 4+

103. Which ion has the smallest radius?

A. O

B. S

C. Se

D. Te

104. An atom that has 13 protons and 15 neutrons is an

isotope of the element

A. nickel B. silicon

C. aluminum D. phosphorus

105. Which notations represent di erent isotopes of the element sodium?

A.

S and

S B. S

and S

C. Na

and Na

D.

Na and

Na 106. Atoms of di erent isotopes of the same element

di er in their total number of

A. electrons B. neutrons

C. protons D. valence electrons 107. A 100.00-gram sample of naturally occurring

boron contains 19.78 grams of boron-10 (atomic mass = 10.01 atomic mass units) and 80.22 grams of boron-11 (atomic mass = 11.01 atomic mass units). Which numerical setup can be used to determine the atomic mass of naturally occurring boron?

A. (0.1978)(10.01) + (0.8022)(11.01) B. (0.8022)(10.01) + (0.1978)(11.01) C. (0 : 1978)(10:01)

(0:8022)(11:01) D. (0 : 8022)(10:01) (0:1978)(11:01)

108. The atomic mass of an element is the weighted average of the

A. number of protons in the isotopes of that element

B. number of neutrons in the isotopes of that element

C. atomic numbers of the naturally occurring isotopes of that element

D. atomic masses of the naturally occurring

isotopes of that element

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Atomic Theory & Periodic Table Review 09/02/2015 1. Answer: D

2. Answer: A 3. Answer: A 4. Answer: A 5. Answer: A 6. Answer: D 7. Answer: A 8. Answer: A 9. Answer: B 10. Answer: A 11. Answer: C 12. Answer: B 13. Answer: B 14. Answer: C 15. Answer: A 16. Answer: C 17. Answer: D 18. Answer: D 19. Answer: D 20.

21. Answer: 2-8-8 22. Answer: B 23. Answer: 2 24. Answer: B 25. Answer: D 26. Answer: D 27. Answer: D 28. Answer: B 29. Answer: D 30. Answer: A 31. Answer:

32. Answer: C

33. Answer: C

34. Answer: D

35. Answer: D

36. Answer: A

37. Answer: D

38. Answer: D

Teacher's Key Page 2 39. Answer: C

40. Answer: D 41. Answer: A 42. Answer: D 43. Answer: B 44. Answer: D 45. Answer: B 46. Answer: D 47. Answer: D 48. Answer: C 49. Answer: C 50. Answer: D 51. Answer: D 52. Answer: D 53. Answer: B 54. Answer: C 55. Answer: B 56. Answer: B 57. Answer: D 58. Answer: C 59. Answer: C 60. Answer: D 61.

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83. Answer: C

Teacher's Key Page 3 84. Answer: D

85. Answer: B 86. Answer: C 87. Answer: C 88. Answer: A 89. Answer: D 90. Answer: C 91. Answer: A 92. Answer: B 93. Answer: D 94. Answer: C 95. Answer: A 96. Answer: A 97. Answer: B 98. Answer: B 99. Answer: D 100. Answer: B 101. Answer: C 102. Answer: B 103. Answer: A 104. Answer: C 105. Answer: D 106.

107. Answer: A

108. Answer: D