Take 5 chapter-wise practice tests of 25 questions each on Classification of Elements and Periodicity in Properties for NEET with +4/-1 scoring, answer review, and concise explanations.
5 original practice tests, 25 questions each, NEET 4/-1 marking, and answer review after submission.
Top banner before test cards for Classification of Elements and Periodicity in Properties.
1. Modern periodic law states that properties of elements are periodic functions of:
Explanation: Modern periodicity is based on atomic number.
2. Horizontal rows in the periodic table are called:
Explanation: Periods run left to right.
3. Vertical columns in the periodic table are called:
Explanation: Groups contain chemically similar elements.
4. Across a period, atomic radius generally:
Explanation: Effective nuclear charge rises across a period.
5. Down a group, atomic radius generally:
Explanation: Additional shells are added down a group.
6. Across a period, first ionization enthalpy generally:
Explanation: Smaller size and higher nuclear charge hold electrons more tightly.
7. Halogens generally have:
Explanation: They strongly attract an extra electron.
8. Fluorine has the highest:
Explanation: Fluorine is the most electronegative element.
9. Metallic character across a period generally:
Explanation: Elements become less willing to lose electrons.
10. Metallic character down a group generally:
Explanation: Larger atoms lose electrons more easily.
11. Valency across a period first increases and then:
Explanation: It follows the tendency to gain or lose electrons toward noble-gas configuration.
12. Across a period, oxides generally change from:
Explanation: Metallic oxides are basic while non-metallic oxides are acidic.
13. The main reason effective nuclear charge rises across a period is:
Explanation: Nuclear charge rises while added electrons go into same shell.
14. Lithium shows diagonal relationship mainly with:
Explanation: Lithium and magnesium share some anomalous similarities.
15. Electron gain enthalpy of chlorine is more negative than fluorine mainly because:
Explanation: Compact 2p orbitals in fluorine create repulsion for the incoming electron.
16. Elements in which the last electron enters a p-orbital belong to:
Explanation: Block classification depends on the differentiating electron.
17. Alkali metals belong to:
Explanation: They have outer configuration ns$^1$.
18. Noble gases are least reactive mainly because they have:
Explanation: Their valence shells are complete.
19. Among isoelectronic species, size decreases with increasing:
Explanation: Greater nuclear pull contracts the electron cloud.
20. Periodic classification works because properties repeat after certain intervals due to repetition of:
Explanation: Chemical properties mainly depend on outer-electron arrangement.
21. The most electropositive element lies toward:
Explanation: Metallic and electron-losing tendency grows in that direction.
22. The most non-metallic elements lie toward:
Explanation: Non-metallic and electron-accepting character peaks there.
23. Shielding effect down a group increases because:
Explanation: More inner electrons screen outer ones.
24. The first ionization enthalpy of oxygen is lower than nitrogen because oxygen has:
Explanation: Nitrogen's half-filled p$^3$ configuration is especially stable.
25. The best single predictor of a periodic trend is the competition between effective nuclear charge and:
Explanation: Most periodic trends reduce to that balance.
26. Modern periodic law states that properties of elements are periodic functions of:
Explanation: Modern periodicity is based on atomic number.
27. Horizontal rows in the periodic table are called:
Explanation: Periods run left to right.
28. Vertical columns in the periodic table are called:
Explanation: Groups contain chemically similar elements.
29. Across a period, atomic radius generally:
Explanation: Effective nuclear charge rises across a period.
30. Down a group, atomic radius generally:
Explanation: Additional shells are added down a group.
31. Across a period, first ionization enthalpy generally:
Explanation: Smaller size and higher nuclear charge hold electrons more tightly.
32. Halogens generally have:
Explanation: They strongly attract an extra electron.
33. Fluorine has the highest:
Explanation: Fluorine is the most electronegative element.
34. Metallic character across a period generally:
Explanation: Elements become less willing to lose electrons.
35. Metallic character down a group generally:
Explanation: Larger atoms lose electrons more easily.
36. Valency across a period first increases and then:
Explanation: It follows the tendency to gain or lose electrons toward noble-gas configuration.
37. Across a period, oxides generally change from:
Explanation: Metallic oxides are basic while non-metallic oxides are acidic.
38. The main reason effective nuclear charge rises across a period is:
Explanation: Nuclear charge rises while added electrons go into same shell.
39. Lithium shows diagonal relationship mainly with:
Explanation: Lithium and magnesium share some anomalous similarities.
40. Electron gain enthalpy of chlorine is more negative than fluorine mainly because:
Explanation: Compact 2p orbitals in fluorine create repulsion for the incoming electron.
41. Elements in which the last electron enters a p-orbital belong to:
Explanation: Block classification depends on the differentiating electron.
42. Alkali metals belong to:
Explanation: They have outer configuration ns$^1$.
43. Noble gases are least reactive mainly because they have:
Explanation: Their valence shells are complete.
44. Among isoelectronic species, size decreases with increasing:
Explanation: Greater nuclear pull contracts the electron cloud.
45. Periodic classification works because properties repeat after certain intervals due to repetition of:
Explanation: Chemical properties mainly depend on outer-electron arrangement.
46. The most electropositive element lies toward:
Explanation: Metallic and electron-losing tendency grows in that direction.
47. The most non-metallic elements lie toward:
Explanation: Non-metallic and electron-accepting character peaks there.
48. Shielding effect down a group increases because:
Explanation: More inner electrons screen outer ones.
49. The first ionization enthalpy of oxygen is lower than nitrogen because oxygen has:
Explanation: Nitrogen's half-filled p$^3$ configuration is especially stable.
50. The best single predictor of a periodic trend is the competition between effective nuclear charge and:
Explanation: Most periodic trends reduce to that balance.
51. Modern periodic law states that properties of elements are periodic functions of:
Explanation: Modern periodicity is based on atomic number.
52. Horizontal rows in the periodic table are called:
Explanation: Periods run left to right.
53. Vertical columns in the periodic table are called:
Explanation: Groups contain chemically similar elements.
54. Across a period, atomic radius generally:
Explanation: Effective nuclear charge rises across a period.
55. Down a group, atomic radius generally:
Explanation: Additional shells are added down a group.
56. Across a period, first ionization enthalpy generally:
Explanation: Smaller size and higher nuclear charge hold electrons more tightly.
57. Halogens generally have:
Explanation: They strongly attract an extra electron.
58. Fluorine has the highest:
Explanation: Fluorine is the most electronegative element.
59. Metallic character across a period generally:
Explanation: Elements become less willing to lose electrons.
60. Metallic character down a group generally:
Explanation: Larger atoms lose electrons more easily.
61. Valency across a period first increases and then:
Explanation: It follows the tendency to gain or lose electrons toward noble-gas configuration.
62. Across a period, oxides generally change from:
Explanation: Metallic oxides are basic while non-metallic oxides are acidic.
63. The main reason effective nuclear charge rises across a period is:
Explanation: Nuclear charge rises while added electrons go into same shell.
64. Lithium shows diagonal relationship mainly with:
Explanation: Lithium and magnesium share some anomalous similarities.
65. Electron gain enthalpy of chlorine is more negative than fluorine mainly because:
Explanation: Compact 2p orbitals in fluorine create repulsion for the incoming electron.
66. Elements in which the last electron enters a p-orbital belong to:
Explanation: Block classification depends on the differentiating electron.
67. Alkali metals belong to:
Explanation: They have outer configuration ns$^1$.
68. Noble gases are least reactive mainly because they have:
Explanation: Their valence shells are complete.
69. Among isoelectronic species, size decreases with increasing:
Explanation: Greater nuclear pull contracts the electron cloud.
70. Periodic classification works because properties repeat after certain intervals due to repetition of:
Explanation: Chemical properties mainly depend on outer-electron arrangement.
71. The most electropositive element lies toward:
Explanation: Metallic and electron-losing tendency grows in that direction.
72. The most non-metallic elements lie toward:
Explanation: Non-metallic and electron-accepting character peaks there.
73. Shielding effect down a group increases because:
Explanation: More inner electrons screen outer ones.
74. The first ionization enthalpy of oxygen is lower than nitrogen because oxygen has:
Explanation: Nitrogen's half-filled p$^3$ configuration is especially stable.
75. The best single predictor of a periodic trend is the competition between effective nuclear charge and:
Explanation: Most periodic trends reduce to that balance.
76. Modern periodic law states that properties of elements are periodic functions of:
Explanation: Modern periodicity is based on atomic number.
77. Horizontal rows in the periodic table are called:
Explanation: Periods run left to right.
78. Vertical columns in the periodic table are called:
Explanation: Groups contain chemically similar elements.
79. Across a period, atomic radius generally:
Explanation: Effective nuclear charge rises across a period.
80. Down a group, atomic radius generally:
Explanation: Additional shells are added down a group.
81. Across a period, first ionization enthalpy generally:
Explanation: Smaller size and higher nuclear charge hold electrons more tightly.
82. Halogens generally have:
Explanation: They strongly attract an extra electron.
83. Fluorine has the highest:
Explanation: Fluorine is the most electronegative element.
84. Metallic character across a period generally:
Explanation: Elements become less willing to lose electrons.
85. Metallic character down a group generally:
Explanation: Larger atoms lose electrons more easily.
86. Valency across a period first increases and then:
Explanation: It follows the tendency to gain or lose electrons toward noble-gas configuration.
87. Across a period, oxides generally change from:
Explanation: Metallic oxides are basic while non-metallic oxides are acidic.
88. The main reason effective nuclear charge rises across a period is:
Explanation: Nuclear charge rises while added electrons go into same shell.
89. Lithium shows diagonal relationship mainly with:
Explanation: Lithium and magnesium share some anomalous similarities.
90. Electron gain enthalpy of chlorine is more negative than fluorine mainly because:
Explanation: Compact 2p orbitals in fluorine create repulsion for the incoming electron.
91. Elements in which the last electron enters a p-orbital belong to:
Explanation: Block classification depends on the differentiating electron.
92. Alkali metals belong to:
Explanation: They have outer configuration ns$^1$.
93. Noble gases are least reactive mainly because they have:
Explanation: Their valence shells are complete.
94. Among isoelectronic species, size decreases with increasing:
Explanation: Greater nuclear pull contracts the electron cloud.
95. Periodic classification works because properties repeat after certain intervals due to repetition of:
Explanation: Chemical properties mainly depend on outer-electron arrangement.
96. The most electropositive element lies toward:
Explanation: Metallic and electron-losing tendency grows in that direction.
97. The most non-metallic elements lie toward:
Explanation: Non-metallic and electron-accepting character peaks there.
98. Shielding effect down a group increases because:
Explanation: More inner electrons screen outer ones.
99. The first ionization enthalpy of oxygen is lower than nitrogen because oxygen has:
Explanation: Nitrogen's half-filled p$^3$ configuration is especially stable.
100. The best single predictor of a periodic trend is the competition between effective nuclear charge and:
Explanation: Most periodic trends reduce to that balance.
101. Modern periodic law states that properties of elements are periodic functions of:
Explanation: Modern periodicity is based on atomic number.
102. Horizontal rows in the periodic table are called:
Explanation: Periods run left to right.
103. Vertical columns in the periodic table are called:
Explanation: Groups contain chemically similar elements.
104. Across a period, atomic radius generally:
Explanation: Effective nuclear charge rises across a period.
105. Down a group, atomic radius generally:
Explanation: Additional shells are added down a group.
106. Across a period, first ionization enthalpy generally:
Explanation: Smaller size and higher nuclear charge hold electrons more tightly.
107. Halogens generally have:
Explanation: They strongly attract an extra electron.
108. Fluorine has the highest:
Explanation: Fluorine is the most electronegative element.
109. Metallic character across a period generally:
Explanation: Elements become less willing to lose electrons.
110. Metallic character down a group generally:
Explanation: Larger atoms lose electrons more easily.
111. Valency across a period first increases and then:
Explanation: It follows the tendency to gain or lose electrons toward noble-gas configuration.
112. Across a period, oxides generally change from:
Explanation: Metallic oxides are basic while non-metallic oxides are acidic.
113. The main reason effective nuclear charge rises across a period is:
Explanation: Nuclear charge rises while added electrons go into same shell.
114. Lithium shows diagonal relationship mainly with:
Explanation: Lithium and magnesium share some anomalous similarities.
115. Electron gain enthalpy of chlorine is more negative than fluorine mainly because:
Explanation: Compact 2p orbitals in fluorine create repulsion for the incoming electron.
116. Elements in which the last electron enters a p-orbital belong to:
Explanation: Block classification depends on the differentiating electron.
117. Alkali metals belong to:
Explanation: They have outer configuration ns$^1$.
118. Noble gases are least reactive mainly because they have:
Explanation: Their valence shells are complete.
119. Among isoelectronic species, size decreases with increasing:
Explanation: Greater nuclear pull contracts the electron cloud.
120. Periodic classification works because properties repeat after certain intervals due to repetition of:
Explanation: Chemical properties mainly depend on outer-electron arrangement.
121. The most electropositive element lies toward:
Explanation: Metallic and electron-losing tendency grows in that direction.
122. The most non-metallic elements lie toward:
Explanation: Non-metallic and electron-accepting character peaks there.
123. Shielding effect down a group increases because:
Explanation: More inner electrons screen outer ones.
124. The first ionization enthalpy of oxygen is lower than nitrogen because oxygen has:
Explanation: Nitrogen's half-filled p$^3$ configuration is especially stable.
125. The best single predictor of a periodic trend is the competition between effective nuclear charge and:
Explanation: Most periodic trends reduce to that balance.