Take 5 chapter-wise practice tests of 25 questions each on Some p-Block Elements 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.
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1. p-Block elements have valence electrons entering the:
Explanation: Their differentiating electron enters a p-orbital.
2. The p-block occupies groups:
Explanation: It lies on the right side of the periodic table.
3. General valence-shell configuration of group 13 is:
Explanation: Group 13 starts with boron.
4. General valence-shell configuration of group 14 is:
Explanation: These elements have four valence electrons.
5. The inert pair effect refers to reluctance of the:
Explanation: It stabilizes lower oxidation states in heavier p-block elements.
6. In group 13, the +1 oxidation state becomes more stable down the group because of:
Explanation: Heavier members resist using the ns$^2$ pair.
7. BF$_3$ is electron-deficient because boron has only:
Explanation: Boron often forms incomplete octets.
8. Boron differs from aluminium mainly because boron:
Explanation: Its small size makes it quite different from Al.
9. Carbon shows catenation strongly because of its:
Explanation: C-C bonds are strong and directional.
10. Diamond and graphite are allotropes of:
Explanation: They differ in structure and properties.
11. Graphite conducts electricity because it has:
Explanation: One electron per carbon is mobile in each sheet.
12. Silicon occurs in nature mainly as:
Explanation: Free silicon is not common in nature.
13. Nitrogen differs from phosphorus mainly because nitrogen:
Explanation: Second-period elements lack d orbitals.
14. Shape of NH$_3$ is:
Explanation: One lone pair distorts the tetrahedral arrangement.
15. Concentrated nitric acid acts as a:
Explanation: It oxidizes many metals and non-metals.
16. Basicity of an oxoacid generally depends on the number of:
Explanation: Only acidic hydrogens bonded through oxygen count.
17. Oxygen family elements belong to:
Explanation: They are called chalcogens.
18. Halogens have valence-shell configuration:
Explanation: They need one electron to complete the octet.
19. Oxidising power among halogens decreases down the group because:
Explanation: Fluorine is the strongest oxidizing halogen.
20. An interhalogen compound contains:
Explanation: Examples include ClF and ICl.
21. Xenon forms compounds more readily than helium because xenon has:
Explanation: Heavier noble gases are more polarizable and easier to ionize.
22. Many p-block exceptions arise because of catenation, multiple bonding, and:
Explanation: This idea explains several lower oxidation states.
23. Across a period in the p-block, oxide character generally shifts toward:
Explanation: Non-metallic character rises across the period.
24. Boric acid is best described as a:
Explanation: It accepts hydroxide ion and behaves as a Lewis acid.
25. The safest high-scoring route in p-block is to organize facts by group trends, key compounds, and:
Explanation: Anomalies dominate many chapter questions.
26. p-Block elements have valence electrons entering the:
Explanation: Their differentiating electron enters a p-orbital.
27. The p-block occupies groups:
Explanation: It lies on the right side of the periodic table.
28. General valence-shell configuration of group 13 is:
Explanation: Group 13 starts with boron.
29. General valence-shell configuration of group 14 is:
Explanation: These elements have four valence electrons.
30. The inert pair effect refers to reluctance of the:
Explanation: It stabilizes lower oxidation states in heavier p-block elements.
31. In group 13, the +1 oxidation state becomes more stable down the group because of:
Explanation: Heavier members resist using the ns$^2$ pair.
32. BF$_3$ is electron-deficient because boron has only:
Explanation: Boron often forms incomplete octets.
33. Boron differs from aluminium mainly because boron:
Explanation: Its small size makes it quite different from Al.
34. Carbon shows catenation strongly because of its:
Explanation: C-C bonds are strong and directional.
35. Diamond and graphite are allotropes of:
Explanation: They differ in structure and properties.
36. Graphite conducts electricity because it has:
Explanation: One electron per carbon is mobile in each sheet.
37. Silicon occurs in nature mainly as:
Explanation: Free silicon is not common in nature.
38. Nitrogen differs from phosphorus mainly because nitrogen:
Explanation: Second-period elements lack d orbitals.
39. Shape of NH$_3$ is:
Explanation: One lone pair distorts the tetrahedral arrangement.
40. Concentrated nitric acid acts as a:
Explanation: It oxidizes many metals and non-metals.
41. Basicity of an oxoacid generally depends on the number of:
Explanation: Only acidic hydrogens bonded through oxygen count.
42. Oxygen family elements belong to:
Explanation: They are called chalcogens.
43. Halogens have valence-shell configuration:
Explanation: They need one electron to complete the octet.
44. Oxidising power among halogens decreases down the group because:
Explanation: Fluorine is the strongest oxidizing halogen.
45. An interhalogen compound contains:
Explanation: Examples include ClF and ICl.
46. Xenon forms compounds more readily than helium because xenon has:
Explanation: Heavier noble gases are more polarizable and easier to ionize.
47. Many p-block exceptions arise because of catenation, multiple bonding, and:
Explanation: This idea explains several lower oxidation states.
48. Across a period in the p-block, oxide character generally shifts toward:
Explanation: Non-metallic character rises across the period.
49. Boric acid is best described as a:
Explanation: It accepts hydroxide ion and behaves as a Lewis acid.
50. The safest high-scoring route in p-block is to organize facts by group trends, key compounds, and:
Explanation: Anomalies dominate many chapter questions.
51. p-Block elements have valence electrons entering the:
Explanation: Their differentiating electron enters a p-orbital.
52. The p-block occupies groups:
Explanation: It lies on the right side of the periodic table.
53. General valence-shell configuration of group 13 is:
Explanation: Group 13 starts with boron.
54. General valence-shell configuration of group 14 is:
Explanation: These elements have four valence electrons.
55. The inert pair effect refers to reluctance of the:
Explanation: It stabilizes lower oxidation states in heavier p-block elements.
56. In group 13, the +1 oxidation state becomes more stable down the group because of:
Explanation: Heavier members resist using the ns$^2$ pair.
57. BF$_3$ is electron-deficient because boron has only:
Explanation: Boron often forms incomplete octets.
58. Boron differs from aluminium mainly because boron:
Explanation: Its small size makes it quite different from Al.
59. Carbon shows catenation strongly because of its:
Explanation: C-C bonds are strong and directional.
60. Diamond and graphite are allotropes of:
Explanation: They differ in structure and properties.
61. Graphite conducts electricity because it has:
Explanation: One electron per carbon is mobile in each sheet.
62. Silicon occurs in nature mainly as:
Explanation: Free silicon is not common in nature.
63. Nitrogen differs from phosphorus mainly because nitrogen:
Explanation: Second-period elements lack d orbitals.
64. Shape of NH$_3$ is:
Explanation: One lone pair distorts the tetrahedral arrangement.
65. Concentrated nitric acid acts as a:
Explanation: It oxidizes many metals and non-metals.
66. Basicity of an oxoacid generally depends on the number of:
Explanation: Only acidic hydrogens bonded through oxygen count.
67. Oxygen family elements belong to:
Explanation: They are called chalcogens.
68. Halogens have valence-shell configuration:
Explanation: They need one electron to complete the octet.
69. Oxidising power among halogens decreases down the group because:
Explanation: Fluorine is the strongest oxidizing halogen.
70. An interhalogen compound contains:
Explanation: Examples include ClF and ICl.
71. Xenon forms compounds more readily than helium because xenon has:
Explanation: Heavier noble gases are more polarizable and easier to ionize.
72. Many p-block exceptions arise because of catenation, multiple bonding, and:
Explanation: This idea explains several lower oxidation states.
73. Across a period in the p-block, oxide character generally shifts toward:
Explanation: Non-metallic character rises across the period.
74. Boric acid is best described as a:
Explanation: It accepts hydroxide ion and behaves as a Lewis acid.
75. The safest high-scoring route in p-block is to organize facts by group trends, key compounds, and:
Explanation: Anomalies dominate many chapter questions.
76. p-Block elements have valence electrons entering the:
Explanation: Their differentiating electron enters a p-orbital.
77. The p-block occupies groups:
Explanation: It lies on the right side of the periodic table.
78. General valence-shell configuration of group 13 is:
Explanation: Group 13 starts with boron.
79. General valence-shell configuration of group 14 is:
Explanation: These elements have four valence electrons.
80. The inert pair effect refers to reluctance of the:
Explanation: It stabilizes lower oxidation states in heavier p-block elements.
81. In group 13, the +1 oxidation state becomes more stable down the group because of:
Explanation: Heavier members resist using the ns$^2$ pair.
82. BF$_3$ is electron-deficient because boron has only:
Explanation: Boron often forms incomplete octets.
83. Boron differs from aluminium mainly because boron:
Explanation: Its small size makes it quite different from Al.
84. Carbon shows catenation strongly because of its:
Explanation: C-C bonds are strong and directional.
85. Diamond and graphite are allotropes of:
Explanation: They differ in structure and properties.
86. Graphite conducts electricity because it has:
Explanation: One electron per carbon is mobile in each sheet.
87. Silicon occurs in nature mainly as:
Explanation: Free silicon is not common in nature.
88. Nitrogen differs from phosphorus mainly because nitrogen:
Explanation: Second-period elements lack d orbitals.
89. Shape of NH$_3$ is:
Explanation: One lone pair distorts the tetrahedral arrangement.
90. Concentrated nitric acid acts as a:
Explanation: It oxidizes many metals and non-metals.
91. Basicity of an oxoacid generally depends on the number of:
Explanation: Only acidic hydrogens bonded through oxygen count.
92. Oxygen family elements belong to:
Explanation: They are called chalcogens.
93. Halogens have valence-shell configuration:
Explanation: They need one electron to complete the octet.
94. Oxidising power among halogens decreases down the group because:
Explanation: Fluorine is the strongest oxidizing halogen.
95. An interhalogen compound contains:
Explanation: Examples include ClF and ICl.
96. Xenon forms compounds more readily than helium because xenon has:
Explanation: Heavier noble gases are more polarizable and easier to ionize.
97. Many p-block exceptions arise because of catenation, multiple bonding, and:
Explanation: This idea explains several lower oxidation states.
98. Across a period in the p-block, oxide character generally shifts toward:
Explanation: Non-metallic character rises across the period.
99. Boric acid is best described as a:
Explanation: It accepts hydroxide ion and behaves as a Lewis acid.
100. The safest high-scoring route in p-block is to organize facts by group trends, key compounds, and:
Explanation: Anomalies dominate many chapter questions.
101. p-Block elements have valence electrons entering the:
Explanation: Their differentiating electron enters a p-orbital.
102. The p-block occupies groups:
Explanation: It lies on the right side of the periodic table.
103. General valence-shell configuration of group 13 is:
Explanation: Group 13 starts with boron.
104. General valence-shell configuration of group 14 is:
Explanation: These elements have four valence electrons.
105. The inert pair effect refers to reluctance of the:
Explanation: It stabilizes lower oxidation states in heavier p-block elements.
106. In group 13, the +1 oxidation state becomes more stable down the group because of:
Explanation: Heavier members resist using the ns$^2$ pair.
107. BF$_3$ is electron-deficient because boron has only:
Explanation: Boron often forms incomplete octets.
108. Boron differs from aluminium mainly because boron:
Explanation: Its small size makes it quite different from Al.
109. Carbon shows catenation strongly because of its:
Explanation: C-C bonds are strong and directional.
110. Diamond and graphite are allotropes of:
Explanation: They differ in structure and properties.
111. Graphite conducts electricity because it has:
Explanation: One electron per carbon is mobile in each sheet.
112. Silicon occurs in nature mainly as:
Explanation: Free silicon is not common in nature.
113. Nitrogen differs from phosphorus mainly because nitrogen:
Explanation: Second-period elements lack d orbitals.
114. Shape of NH$_3$ is:
Explanation: One lone pair distorts the tetrahedral arrangement.
115. Concentrated nitric acid acts as a:
Explanation: It oxidizes many metals and non-metals.
116. Basicity of an oxoacid generally depends on the number of:
Explanation: Only acidic hydrogens bonded through oxygen count.
117. Oxygen family elements belong to:
Explanation: They are called chalcogens.
118. Halogens have valence-shell configuration:
Explanation: They need one electron to complete the octet.
119. Oxidising power among halogens decreases down the group because:
Explanation: Fluorine is the strongest oxidizing halogen.
120. An interhalogen compound contains:
Explanation: Examples include ClF and ICl.
121. Xenon forms compounds more readily than helium because xenon has:
Explanation: Heavier noble gases are more polarizable and easier to ionize.
122. Many p-block exceptions arise because of catenation, multiple bonding, and:
Explanation: This idea explains several lower oxidation states.
123. Across a period in the p-block, oxide character generally shifts toward:
Explanation: Non-metallic character rises across the period.
124. Boric acid is best described as a:
Explanation: It accepts hydroxide ion and behaves as a Lewis acid.
125. The safest high-scoring route in p-block is to organize facts by group trends, key compounds, and:
Explanation: Anomalies dominate many chapter questions.