An Ultimate Guide for School Grade IX and College Grade XI Level Students with MCQs on Periodic Table and Periodicity of Properties
As a student of chemistry, understanding the periodic table and the periodicity of properties is crucial for success in exams. Whether it be for BISE or Federal Board exams, or for entrance tests such as NMDCAT, ETEA, CSS, PCS, PMA, Cadet Colleges, Army Medical Colleges, and others, mastering these concepts will give you a solid foundation in the subject. In this article, we present a comprehensive review of the most important topics related to the periodic table and periodicity of properties, specifically designed for Grade IX and XI level students.
Our MCQs cover key areas such as the need and importance of the periodic table, its historical development, the groups and periods within it, the blocks of the periodic table, and the periodicity of properties such as atomic size, ionization energy, electron affinity, shielding effect, and electronegativity. With a focus on exam success, these MCQs provide students with the opportunity to test their knowledge and identify areas for further improvement. So, let's dive into the world of the periodic table and unlock its secrets together!
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| 130 important Chemistry MCQs on Periodic Table for beginners From MCQs Library of H.E.S (Health, Education, and Skills) |
MCQs on Introduction and Importance of Periodic table
1. What does the modern periodic law state about the elements in the periodic table?A. Their physical properties are a periodic function of their atomic masses.
B. Their chemical properties are a periodic function of their atomic masses.
C. Their physical and chemical properties are a periodic function of their atomic numbers.
D. Their physical and chemical properties are not related to their atomic numbers.
2. What are the vertical columns of the periodic table called?
A. Rows
B. Groups
C. Families
D. Periods
3. What are the horizontal rows of the periodic table called?
A. Rows
B. Groups
C. Families
D. Periods
4. What are the normal or representative elements in the periodic table?
A. Elements of Group-IA to VIIIA (d and f-block)
B. Elements of Group-IB to VIIIB (s and p-block)
C. Elements of Group-IA to VIIIA (s and p-block)
D. Elements of Group-IB to VIIIB (d and f-block)
5. What are the transition elements in the periodic table?
A. Elements of Group-IA to VIIIA (d and f-block)
B. Elements of Group-IB to VIIIB (s and p-block)
C. Elements of Group-IA to VIIIA (s and p-block)
D. Elements of Group-IB to VIIIB (d and f-block)
6. When was the need for arranging elements in a systematic manner felt?
A. 1800
B. 1870
C. 1974
D. 2000
7. How many elements were known in the year 1800?
A. 70
B. 105
C. 118
D. 34
8. How many elements were known in the year 1974?
A. 70
B. 105
C. 118
D. Almost double the number known in 1800
9. What was the main reason for arranging elements in a systematic manner?
A. To increase the number of elements known
B. To make it easier to study elements and obtain maximum information in less time
C. To decrease the number of elements known
D. To make it harder to study elements
MCQs on the History of Periodic table
10. Who was the first scientist to classify elements into metals and non-metals?A) Al-Razi
B) J.W.Dobereiner
C) John Dalton
D) Antoine Lavoisier
11. What is the name of the law presented by J.W.Dobereiner?
A) Law of Triads
B) Law of Atoms
C) Law of Al-Razi
D) Law of Elements
12. What was the characteristic of the elements in Dobereiner's Triads?
A) Similarity in properties
B) Difference in properties
C) Different atomic masses
D) No relation between the elements
13. What was the relationship between the atomic masses of the elements in Dobereiner's Triads?
A) They were equal
B) The middle element was the arithmetic mean of the other two elements
C) The middle element was the geometric mean of the other two elements
D) No relation between the elements
14. Who was J.W.Dobereiner?
A) A German physicist
B) A German chemist
C) A French chemist
D) An English chemist
15. Who presented the law of Octaves?
A) John Dalton
B) Antoine Lavoisier
C) Henry Newland
D) J.W. Dobereiner
16. What was the main idea behind Newland's law of Octaves?
A) The properties of every 8th element are similar to the first element
B) The properties of every 6th element are similar to the first element
C) The properties of every 3rd element are similar to the first element
D) The properties of every 12th element are similar to the first element
17. Who arranged the elements in order of increasing atomic masses and presented the periodic table?
A) Henry Newland
B) J.W. Dobereiner
C) Dmitri Mendeleev
D) John Dalton
18. What was the basis of Mendeleev's periodic table?
A) The physical and chemical properties of the elements are the periodic function of their atomic masses
B) The physical and chemical properties of the elements are the inverse function of their atomic masses
C) The physical and chemical properties of the elements are randomly related to their atomic masses
D) The physical and chemical properties of the elements are not related to their atomic masses
19. Who was the chemist who presented the periodic table that became the basis of the modern periodic table?
A) Henry Newland
B) J.W. Dobereiner
C) Dmitri Mendeleev
D) John Dalton
20. What is the modern periodic table also known as?
A) Short form of the periodic table
B) Long form of the periodic table
C) Modified form of the periodic table
D) Expanded form of the periodic table
21. What is the basis of the Modern periodic table?
A) Modern periodic law
B) Old periodic law
C) Modified periodic law
D) Expanded periodic law
22. Who proposed the Modern periodic table?
A) Henry Gwyn Jeffreys Moseley
B) J.J. Thomson
C) Max Planck
D) Robert Boyle
23. What are the rows of the periodic table called?
A) Columns
B) Groups
C) Families
D) Periods
24. Which organization recommended the modern periodic table?
A) International Union of Pure and Applied Chemistry
B) American Chemical Society
C) Royal Society of Chemistry
D) German Chemical Society
25. What are the vertical columns of the periodic table called?
A) Groups
B) Families
C) Columns
D) Both A and B
MCQs on Periods and Groups of Periodic Table
26. What is the number of elements in the first period?A) 2
B) 8
C) 18
D) 32
27. What is the first period of the periodic table called?
A) Short period
B) Long period
C) Incomplete period
D) Shortest period
28.What is the number of elements in the 2nd and 3rd period?
A) 2
B) 8
C) 18
D) 32
29. What are the 2nd and 3rd period of the periodic table called?
A) Short period
B) Long period
C) Incomplete period
D) Shortest period
30..What is the number of elements in the 4th and 5th period?
A) 2
B) 8
C) 18
D) 32
31. What are the 4th and 5th period of the periodic table called?
A) Short period
B) Long period
C) Incomplete period
D) Shortest period
32. What is the number of elements in the 6th period?
A) 2
B) 8
C) 18
D) 32
33. What is the 6th period of the periodic table called?
A) Short period
B) Long period
C) Incomplete period
D) Longest period
34. What is the number of elements in the 7th period?
A) 2
B) 8
C) 18
D) 23
35. What is the 7th period of the periodic table called?
A) Short period
B) Long period
C) Incomplete period
D) Longest period
36. What is the number of elements in the upper part of the 6th period?
A) 2
B) 8
C) 18
D) 32
37. What is the number of elements in the lower part of the 6th period?
A) 2
B) 8
C) 18
D) 14
38. What is the name of the series in the lower part of the 6th period?
A) Actinide series
B) Rare earth elements
C) Transition elements
D) Normal elements
39. What is the number of valence electrons of the elements in the same period?
A) Increases gradually by two
B) Decreases gradually by two
C) Increases gradually by one
D) Decreases gradually by one
40. What is the relationship between group number and electronic structure in the periodic table?
A. Group number determines the number of electrons in the innermost shell
B. Group number determines the number of electrons in the outermost shell
C. Group number determines the number of electrons in the middle shell
D. Group number has no relationship with electronic structure
41. How are the elements in the periodic table arranged?
A. Randomly
B. Based on their atomic masses
C. Based on their isotopes
D. Based on the number of electrons in their outermost shell
42. What determines the number of valence electrons in an element?
A. Its atomic weight
B. Its position in the periodic table
C. Its electron configuration
D. Its physical properties
43. What is the main factor that makes elements in the same group similar in chemical properties?
A. The number of electrons in their innermost shell
B. The number of electrons in their middle shell
C. The number of electrons in their outermost shell
D. Their chemical properties are not related
44. Which of the following elements would likely have similar chemical properties?
A. Sodium and Chlorine
B. Sodium and Calcium
C. Sodium and Magnesium
D. Sodium and Potassium
45. Which of the following groups in the periodic table would likely have similar chemical properties?
A. Group 1 and Group 7
B. Group 2 and Group 8
C. Group 3 and Group 9
D. Group 4 and Group 10
46. What is the name of Group-IA elements in the periodic table?
A. Alkali metals
B. Alkaline earth metals
C. Boron family
D. Carbon family
47. What is the name of Group-IIA elements in the periodic table?
A. Alkali metals
B. Alkaline earth metals
C. Boron family
D. Carbon family
48. What is the name of Group-IIIA elements in the periodic table?
A. Alkali metals
B. Alkaline earth metals
C. Boron family
D. Carbon family
49. What is the name of Group-IVA elements in the periodic table?
A. Alkali metals
B. Alkaline earth metals
C. Boron family
D. Carbon family
50. What is the name of Group-VA elements in the periodic table?
A. Nitrogen family
B. Oxygen family
C. Halogens family
D. Noble gases
51. What is the name of Group-VIA elements in the periodic table?
A. Nitrogen family
B. Oxygen family
C. Chalcogens
D. Both B and C
52. What is the name of Group-VIIA elements in the periodic table?
A. Nitrogen family
B. Oxygen family
C. Halogens family
D. Noble gases
53. What is the name of Group-VIIIA elements in the periodic table?
A. Nitrogen family
B. Oxygen family
C. Halogens family
D. Noble gases
MCQs on Blocks of Periodic Table
54. Which group of elements is called s-block elements in the periodic table?
A. Group-IA and Group-IIA
B. Group-IIIA to Group-VIIIA
C. Group-IB to Group-VIIIB
D. Lanthanide and Actinide series
55. Which orbitals are involved in the bond formation of alkali metals in the periodic table?
A. d-orbital
B. p-orbital
C. s-orbital
D. f-orbital
56. What are the p-block elements called in the periodic table?
A. Group-IA and Group-IIA
B. Group-IIIA to Group-VIIIA
C. Group-IB to Group-VIIIB
D. Lanthanide and Actinide series
57. What orbitals are involved in the bond formation of p-block elements in the periodic table?
A. d-orbital
B. p-orbital
C. s-orbital
D. f-orbital
58. What are the d-block elements called in the periodic table?
A. Group-IA and Group-IIA
B. Group-IIIA to Group-VIIIA
C. Group-IB to Group-VIIIB
D. Lanthanide and Actinide series
59. What are the f-block elements called in the periodic table?
A. Group-IA and Group-IIA
B. Group-IIIA to Group-VIIIA
C. Group-IB to Group-VIIIB
D. Lanthanide and Actinide series
60. Which block of elements includes the Noble gases in the periodic table?
A. p-block elements
B. s-block elements
C. d-block elements
D. f-block elements
MCQs on Periodicity of Properties | Periodic Properties such as Atomic Size, Ionization Energy, Electron Affinity, Shielding Effect and Elctronegativity
61. What does the term "periodicity" mean in chemistry?
A. The arrangement of elements in the periodic table
B. The repetition of properties in all groups and periods of the periodic table
C. The chemical reaction between elements
D. The study of atomic structures
62. Which of the following is NOT a periodicity of properties in the periodic table?
A. Atomic Size
B. Reactivity
C. Electron Affinity
D. Chemical Bond Strength
63. Which property of elements is described as the measure of the tendency of an atom to attract electrons towards itself?
A. Electron Affinity
B. Shielding Effect
C. Electronegativity
D. Ionization Energy
64. What is the periodic repetition of properties in the periodic table called?
A. Periodic Law
B. Periodic Series
C. Periodic Pattern
D. Periodic Properties
65. Which property of elements refers to the energy required to remove an electron from a neutral atom?
A. Electron Affinity
B. Electronegativity
C. Ionization Energy
D. Shielding Effect
66. What is the size of an atom called?
A) Atomic volume
B) Atomic radius
C) Atomic size
D) Covalent radius
67. What is the distance between the nucleus and the valence shell of an atom called?
A) Atomic volume
B) Atomic radius
C) Atomic size
D) Covalent radius
68. What does the symbol “r” represent in terms of an atom?
A) Atomic volume
B) Atomic radius
C) Atomic size
D) Covalent radius
69. Is the atomic radius directly proportional to the number of shells in an atom?
A) Yes
B) No
70. In what unit is the atomic radius expressed?
A) Nanometer
B) Pico meter
C) Both A and B
D) Neither A nor B
71. How can the atomic and covalent radii be determined?
A) Spectroscopy and X-ray studies
B) Nuclear magnetic resonance and X-ray crystallography
C) Electron microscopy and X-ray diffraction
D) None of the above
72. What is the size of an atom expressed in terms of?
A) Atomic volume
B) Atomic radius
C) Atomic size
D) All of the above
73. What is the difference between atomic size and covalent radii?
A) Atomic size is the size of an atom in isolation while covalent radii are the size of an atom in combination with other atoms
B) Atomic size is the size of an atom in combination with other atoms while covalent radii are the size of an atom in isolation
C) There is no difference between atomic size and covalent radii
74. What is the trend of atomic size in periods of the periodic table?
A. Increases
B. Decreases
C. Remains the same
D. None of the above
75. What is the reason for the decrease in atomic size from left to right in the periods of the periodic table?
A. The number of shells decreases
B. The number of protons and electrons decreases
C. The number of protons and electrons increases
D. None of the above
76. What is the trend of atomic size in groups of the periodic table?
A. Increases
B. Decreases
C. Remains the same
D. None of the above
77. What is the reason for the increase in atomic size from top to bottom in the groups of the periodic table?
A. The number of shells decreases
B. The number of protons and electrons decreases
C. The number of shells increases
D. None of the above
78. What is covalent radii?
A. The distance between two similar atoms of different molecules
B. The distance between two similar atoms of the same molecule containing a single covalent bond
C. The distance between two different atoms of the same molecule containing a single covalent bond
D. None of the above
79. What is Ionization energy?
A. The energy required to add electrons to an atom
B. The energy required to remove electrons from an atom
C. The energy required to move electrons within an atom
D. The energy required to bond two atoms together
80. What is the minimum amount of energy required to form a positive ion from a gaseous atom?
A. Ionization energy
B. Electron Affinity
C. Electronegativity
D. Covalent radius
81. What are the units used to measure Ionization energy?
A. Newtons
B. Joules
C. Pascals
D. Kilojoules per mole
82. What is the ionization energy of Sodium (Na)?
A. +496kjmol-1
B. -496kjmol-1
C. 1496kjmol-1
D. -496kJ
83. What is an example of 2nd ionization energy?
A. Na ...............> Na+ + e- I.E = +496 kJ mol-1
B. Cl ...............> Cl- + e- I.E = -348 kJ mol-1
C. Mg ...............> Mg+ + e- I.E = +738 kJ mol-1
D. Mg ...............> Mg+2 + 1e- I.E = +1450 kJ mol-1
84. What affects the ionization energy of an atom?
A. The atomic mass of the atom
B. The atomic radius of the atom
C. The number of neutrons in the nucleus of the atom
D. Both B and C
85. Which factor affects the ionization energy of an atom more, the nuclear charge or the shielding effect?
A. The shielding effect
B. The nuclear charge
C. Both affect ionization energy equally
D. None of the above
86. Does the shielding effect of electrons have a direct or inverse relationship with the ionization energy of an atom?
A. Direct relationship
B. Inverse relationship
C. No relationship
D. It depends on the other factors affecting ionization energy
87. Can the ionization energy of an atom be affected by its distance from the nucleus?
A. Yes, it affects the ionization energy
B. No, it does not affect the ionization energy
C. It depends on the other factors affecting ionization energy
D. There is not enough information to determine
88. What is the trend of ionization energy across periods in the periodic table?
A. Decreases
B. Increases
C. No change
D. It depends on the other factors affecting ionization energy
89. What is the reason for the increase in ionization energy across periods in the periodic table?
A. Increased atomic size
B. Decreased nuclear charge
C. Increased shielding effect of electrons
D. Decreased atomic size
90. What is the trend of ionization energy across groups in the periodic table?
A. Decreases
B. Increases
C. No change
D. Both A and B
91. What is the reason for the decrease in ionization energy across groups in the periodic table?
A. Increased atomic size
B. Decreased nuclear charge
C. Increased shielding effect of electrons D. Decreased atomic size
92. What is the effect of increased nuclear charge on the ionization energy of an atom?
A. Increases ionization energy
B. Decreases ionization energy
C. No change in ionization energy
D. It depends on the other factors affecting ionization energy
93. What is the effect of the increased shielding effect of electrons on the ionization energy of an atom?
A. Increases ionization energy
B. Decreases ionization energy
C. No change in ionization energy
D. It depends on the other factors affecting ionization energy
94. What is Electron Affinity?
A. The energy absorbed by an electron
B. The amount of energy evolved when an electron enters into a gaseous atom to form an anion
C. The energy released by the addition of the protons
D. None
95. What is the unit of measurement for Electron Affinity?
A. Kilograms
B. Meters
C. Joules or kilojoules per mol
D. Watt
96. What is an example of Electron Affinity?
A. Mg + e- >>>>>>> O- E.A = -348.8 kJ mol-1
B. Cl + e- >>>>>>> Cl- E.A = -348.8 kJ mol-1
C. Na + e- >>>>>>> Na- E.A = -348.8 kJ mol-1
D. Ca + e- >>>>>>> Ca- E.A = -348.8 kJ mol-1
97. What does the negative sign indicate in Electron Affinity?
A. Energy is absorbed
B. Energy is neutral
C. Energy is released
D. Energy is stored
98. What are the factors that determine Electron Affinity?
A. Element type and its electron-gaining ability
B. Element weight and its electron-gaining ability
C. Element height and its electron-gaining ability
D. Element color and its electron-gaining ability
99. How is Electron Affinity different from electron-gaining ability?
A. Electron Affinity is the energy absorbed by an electron, and electron-gaining ability is the ability to release energy
B. Electron Affinity is the amount of energy evolved when an electron enters into a gaseous atom to form an anion, and electron-gaining ability is the energy released by the addition of the first electron
C. Electron Affinity is the energy released by the addition of the second electron, and electron-gaining ability is the amount of energy evolved when an electron enters into a gaseous atom to form an anion
D. Electron Affinity is the amount of energy evolved when an electron enters into a gaseous atom to form an anion, and electron-gaining ability is the ability to absorb an electron
100. What is the relationship between atomic radii and electron affinity?
A. Greater atomic radii lead to greater electron affinity
B. Greater atomic radii lead to lesser electron affinity
C. No relationship between atomic radii and electron affinity
D. Opposite relationship between atomic radii and electron affinity
101. What is the relationship between nuclear charge and electron affinity?
A. Greater nuclear charge leads to greater electron affinity
B. Greater nuclear charge leads to lesser electron affinity
C. No relationship between nuclear charge and electron affinity
D. None
102. Which of the following factors has the greatest effect on electron affinity?
A. Atomic radii
B. Nuclear charge
C. Shielding effect
D. All have equal effect on electron affinity
103. What is the trend of electron affinity in the periods of the periodic table?
A. Decreases from left to right
B. Increases from left to right
C. No trend
D. Increases and then decreases
104. What is the trend of electron affinity in the groups of the periodic table?
A. Decreases from top to bottom
B. Increases from top to bottom
C. No trend
D. Increases and then decreases
105. What is the shielding effect?
A. The inner electrons repel the outer electrons from the nucleus
B. The inner electrons shield the outer electrons from the nucleus
C. The outer electrons repel the inner electrons from the nucleus
D. The outer electrons shield the inner electrons from the nucleus
106. What is the result of the shielding effect on outer electrons?
A. Increased force of attraction from the nucleus
B. Decreased force of attraction from the nucleus
C. No effect on the force of attraction from the nucleus
D. First increased and then decreased force of attraction from the nucleus
107. What is the relationship between the number of inner electrons and the strength of the shielding effect?
A. More inner electrons, the stronger the shielding effect
B. Lesser the inner electrons, the stronger the shielding effect
C. The number of inner electrons has no effect
D. None
108. How does the shielding effect affect ionization energy?
A. Increases the ionization energy
B. Decreases the ionization energy
C. No effect on ionization energy
D. First increases and then decreases the ionization energy
109. How does the shielding effect affect electron affinity?
A. Increases the electron affinity
B. Decreases the electron affinity
C. No effect on electron affinity
D. First increases and then decreases the electron affinity
110. Why does the shielding effect decrease electron affinity?
A. Increased force of attraction for incoming electrons
B. Decreased force of attraction for incoming electrons
C. No effect on the force of attraction for incoming electrons
D. First increased and then decreased force of attraction for incoming electrons
111. How does the shielding effect change as you move from left to right in the periodic table?
A. Increases
B. Decreases
C. Remains constant
D. Increases and then decreases
112. Why does the shielding effect remain constant as you move from left to right in the periodic table?
A. Decrease in the number of inner electrons
B. Increase in the number of inner
C. No change in the number of inner electrons
D. First decreases and then increases the number of inner electrons
113. How does the shielding effect change as you move down the groups in the periodic table?
A. Increases
B. Decreases
C. Remains constant
D. Increases and then decreases
114. Does the shielding effect have the same trend in both periods and groups of the periodic table?
A. Yes, the trend is the same in both
B. No, the trend is different in both
C. It depends on the element
D. It depends on the type of shielding effect
115. What is electronegativity?
A. The ability of an atom to gain electrons
B. The ability of an atom to lose electrons
C. The ability of an atom to attract the shared pair of electrons in a Covalent bond
D. The ability of an atom to repel electrons
116. What is a polar covalent bond?
A. A bond where the shared pair of electrons is attracted more towards a more electronegative atom.
B. A bond where the shared pair of electrons is attracted more towards a less electronegative atom.
C. A bond where the shared pair of electrons is equally attracted by both the bonded atoms.
D. None of the above
117. What is a non-polar covalent bond?
A. A bond where the shared pair of electrons is attracted more towards a more electronegative atom.
B. A bond where the shared pair of electrons is attracted more towards a less electronegative atom.
C. A bond where the shared pair of electrons is equally attracted by both the bonded atoms.
D. None of the above
118. What is the effect of atomic size on electronegativity?
A. Electronegativity increases with the increase in atomic size.
B. Electronegativity decreases with the increase in atomic size.
C. Electronegativity remains constant with the change in atomic size.
D. None of the above
119. What is the effect of nuclear charge on electronegativity?
A. Electronegativity increases with the increase in nuclear charge.
B. Electronegativity decreases with the increase in nuclear charge.
C. Electronegativity remains constant with the change in nuclear charge.
D. None of the above
120. What is the effect of shielding effect on electronegativity?
A. Electronegativity increases with the increase in the shielding effect.
B. Electronegativity decreases with the increase in the shielding effect.
C. Electronegativity remains constant with the change in shielding effect.
D. None of the above
121. What is the effect of electronic configuration on electronegativity?
A. Electronegativity increases with the change in electronic configuration.
B. Electronegativity decreases with the increasing electronic configuration.
C. Electronegativity remains constant with the change in electronic configuration.
D. None of the above
122. What is the highest electronegativity according to Pauling's electronegativity scale?
A. Fluorine
B. Cesium
C. Sodium
D. Chlorine
123. What is the lowest electronegativity according to Pauling's electronegativity scale?
A. Fluorine
B. Cesium
C. Sodium
D. Chlorine
124. What is the electronegativity of Sodium according to Pauling's electronegativity scale?
A. 4.0
B. 0.70
C. 0.93
D. 1.01
125. What is the electronegativity of Chlorine according to Pauling's electronegativity scale?
A. 4.0
B. 0.70
C. 3.16
D. 1.01
126. In which direction does the electronegativity of elements increase in periods of the periodic table?
A) Left to right
B) Right to left
C) Up to down
D) Down to up
127. Why does the electronegativity of elements increase from left to right in periods of the periodic table?
A) Due to increasing atomic size
B) Due to a decrease in atomic size
C) Due to increasing nuclear charge
D) Due to a decrease in nuclear charge
128. In which direction does the electronegativity of elements decrease in groups of the periodic table?
A) Left to right
B) Right to left
C) Up to down
D) Down to up
129. Why does the electronegativity of elements decrease from top to bottom in groups of the periodic table?
A) Due to increasing in atomic size
B) Due to a decrease in atomic size
C) Due to increasing in nuclear charge
D) Due to a decrease in nuclear charge
130. What is the electronegativity value of Florine?
A. 2
B. 4
C. 6
D. 8
Answers
1. C 2. C 3. D 4. C 5. D 6. B 7. D 8. B 9. B 10. A 11. A 12. A 13. 14. B 15. C 16. A 17. C 18. A19. C 20. B 21. A 22. A 23. D 24. A 25. D 26. A 27. D 28. B 29. A 30. C 31. B 32. D 33. D 34. D 35. C 36. C 37. D 38. B 39. C 40. B 41. D 42. B 43. C 44. D 45. B 46. A 47. B 48. C 49. D 50. A 51. D 52. C 53. D 54. A 55. C 56. B 57. B 58. C 59. D 60. A 61. B 62. D 63. C 64. D 65. C 66. C 67. B 68. B 69. A 70. C 71. A 72. D 73. A 74. B 75. C 76. A 77. C 78. B 79. B 80. A 81. D 82. A 83. D 84. B 85. B 86. B 87. B 88. B 89. D 90. A 91. A 92. A 93. B 94. B 95. C 96. A 97. C
98. A 99. D 100. B 101. A 102. A 103. B 104. A 105. B 106. B 107. B 108. B 109. B.110. B
111. C 112. C 113. A 114. B 115. C 116. A 117. C 118. B 119. A 120. A 121. B 122. A 123. B
124. D 125. C 126. A 127. B 128. D 129. A 130. B
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