Take 5 chapter-wise practice tests of 25 questions each on Chemical Bonding and Molecular Structure 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. The octet rule is based on the tendency of atoms to attain:
Explanation: Atoms tend toward stable noble-gas-like valence shells.
2. A bond formed by transfer of electrons is:
Explanation: Electron transfer gives oppositely charged ions.
3. A bond formed by sharing of electron pairs is:
Explanation: Covalent bonding uses shared pairs.
4. Formal charge on an atom is based on:
Explanation: It is a bookkeeping tool for Lewis structures.
5. According to VSEPR theory, electron pairs around the central atom arrange to:
Explanation: Repulsion minimization determines geometry.
6. Shape of BeCl$_2$ in gaseous state is:
Explanation: Two bond pairs with no lone pairs give linear geometry.
7. Shape of BF$_3$ is:
Explanation: Three bond pairs and no lone pairs.
8. Shape of CH$_4$ is:
Explanation: sp$^3$ hybridization gives tetrahedral shape.
9. Shape of NH$_3$ is:
Explanation: One lone pair compresses the bond angle.
10. Shape of H$_2$O is:
Explanation: Two lone pairs on oxygen create a bent shape.
11. Hybridization of carbon in methane is:
Explanation: Four equivalent sigma bonds require sp$^3$ hybridization.
12. Hybridization of carbon in ethene is:
Explanation: Each carbon forms three sigma bonds and one pi bond.
13. Hybridization of carbon in ethyne is:
Explanation: Triple bond implies sp hybridization.
14. A molecule is polar when it has:
Explanation: Bond dipoles must not cancel overall.
15. CO$_2$ is non-polar because it is:
Explanation: Its equal bond dipoles cancel.
16. NH$_3$ is polar because it is:
Explanation: Its geometry leaves a net dipole.
17. Hydrogen bonding is strongest when H is bonded to:
Explanation: High electronegativity and small size favor H-bonding.
18. Resonance structures differ only in the arrangement of:
Explanation: The atomic framework remains fixed.
19. In molecular orbital theory, bond order is:
Explanation: This is the MO bond-order formula.
20. O$_2$ is paramagnetic because it has:
Explanation: MO theory explains its unpaired electrons.
21. A single bond is always a:
Explanation: Single covalent bonds are sigma bonds.
22. A double bond contains:
Explanation: The first overlap is sigma, second is pi.
23. Repulsion order among electron pairs is:
Explanation: Lone pairs occupy more space and repel more strongly.
24. Incomplete octet is shown by:
Explanation: Boron has only six electrons around it in BF$_3$.
25. The strongest quick route in this chapter is to connect Lewis structure, electron-pair repulsion, and:
Explanation: That trio explains shape, angle, and polarity.
26. The octet rule is based on the tendency of atoms to attain:
Explanation: Atoms tend toward stable noble-gas-like valence shells.
27. A bond formed by transfer of electrons is:
Explanation: Electron transfer gives oppositely charged ions.
28. A bond formed by sharing of electron pairs is:
Explanation: Covalent bonding uses shared pairs.
29. Formal charge on an atom is based on:
Explanation: It is a bookkeeping tool for Lewis structures.
30. According to VSEPR theory, electron pairs around the central atom arrange to:
Explanation: Repulsion minimization determines geometry.
31. Shape of BeCl$_2$ in gaseous state is:
Explanation: Two bond pairs with no lone pairs give linear geometry.
32. Shape of BF$_3$ is:
Explanation: Three bond pairs and no lone pairs.
33. Shape of CH$_4$ is:
Explanation: sp$^3$ hybridization gives tetrahedral shape.
34. Shape of NH$_3$ is:
Explanation: One lone pair compresses the bond angle.
35. Shape of H$_2$O is:
Explanation: Two lone pairs on oxygen create a bent shape.
36. Hybridization of carbon in methane is:
Explanation: Four equivalent sigma bonds require sp$^3$ hybridization.
37. Hybridization of carbon in ethene is:
Explanation: Each carbon forms three sigma bonds and one pi bond.
38. Hybridization of carbon in ethyne is:
Explanation: Triple bond implies sp hybridization.
39. A molecule is polar when it has:
Explanation: Bond dipoles must not cancel overall.
40. CO$_2$ is non-polar because it is:
Explanation: Its equal bond dipoles cancel.
41. NH$_3$ is polar because it is:
Explanation: Its geometry leaves a net dipole.
42. Hydrogen bonding is strongest when H is bonded to:
Explanation: High electronegativity and small size favor H-bonding.
43. Resonance structures differ only in the arrangement of:
Explanation: The atomic framework remains fixed.
44. In molecular orbital theory, bond order is:
Explanation: This is the MO bond-order formula.
45. O$_2$ is paramagnetic because it has:
Explanation: MO theory explains its unpaired electrons.
46. A single bond is always a:
Explanation: Single covalent bonds are sigma bonds.
47. A double bond contains:
Explanation: The first overlap is sigma, second is pi.
48. Repulsion order among electron pairs is:
Explanation: Lone pairs occupy more space and repel more strongly.
49. Incomplete octet is shown by:
Explanation: Boron has only six electrons around it in BF$_3$.
50. The strongest quick route in this chapter is to connect Lewis structure, electron-pair repulsion, and:
Explanation: That trio explains shape, angle, and polarity.
51. The octet rule is based on the tendency of atoms to attain:
Explanation: Atoms tend toward stable noble-gas-like valence shells.
52. A bond formed by transfer of electrons is:
Explanation: Electron transfer gives oppositely charged ions.
53. A bond formed by sharing of electron pairs is:
Explanation: Covalent bonding uses shared pairs.
54. Formal charge on an atom is based on:
Explanation: It is a bookkeeping tool for Lewis structures.
55. According to VSEPR theory, electron pairs around the central atom arrange to:
Explanation: Repulsion minimization determines geometry.
56. Shape of BeCl$_2$ in gaseous state is:
Explanation: Two bond pairs with no lone pairs give linear geometry.
57. Shape of BF$_3$ is:
Explanation: Three bond pairs and no lone pairs.
58. Shape of CH$_4$ is:
Explanation: sp$^3$ hybridization gives tetrahedral shape.
59. Shape of NH$_3$ is:
Explanation: One lone pair compresses the bond angle.
60. Shape of H$_2$O is:
Explanation: Two lone pairs on oxygen create a bent shape.
61. Hybridization of carbon in methane is:
Explanation: Four equivalent sigma bonds require sp$^3$ hybridization.
62. Hybridization of carbon in ethene is:
Explanation: Each carbon forms three sigma bonds and one pi bond.
63. Hybridization of carbon in ethyne is:
Explanation: Triple bond implies sp hybridization.
64. A molecule is polar when it has:
Explanation: Bond dipoles must not cancel overall.
65. CO$_2$ is non-polar because it is:
Explanation: Its equal bond dipoles cancel.
66. NH$_3$ is polar because it is:
Explanation: Its geometry leaves a net dipole.
67. Hydrogen bonding is strongest when H is bonded to:
Explanation: High electronegativity and small size favor H-bonding.
68. Resonance structures differ only in the arrangement of:
Explanation: The atomic framework remains fixed.
69. In molecular orbital theory, bond order is:
Explanation: This is the MO bond-order formula.
70. O$_2$ is paramagnetic because it has:
Explanation: MO theory explains its unpaired electrons.
71. A single bond is always a:
Explanation: Single covalent bonds are sigma bonds.
72. A double bond contains:
Explanation: The first overlap is sigma, second is pi.
73. Repulsion order among electron pairs is:
Explanation: Lone pairs occupy more space and repel more strongly.
74. Incomplete octet is shown by:
Explanation: Boron has only six electrons around it in BF$_3$.
75. The strongest quick route in this chapter is to connect Lewis structure, electron-pair repulsion, and:
Explanation: That trio explains shape, angle, and polarity.
76. The octet rule is based on the tendency of atoms to attain:
Explanation: Atoms tend toward stable noble-gas-like valence shells.
77. A bond formed by transfer of electrons is:
Explanation: Electron transfer gives oppositely charged ions.
78. A bond formed by sharing of electron pairs is:
Explanation: Covalent bonding uses shared pairs.
79. Formal charge on an atom is based on:
Explanation: It is a bookkeeping tool for Lewis structures.
80. According to VSEPR theory, electron pairs around the central atom arrange to:
Explanation: Repulsion minimization determines geometry.
81. Shape of BeCl$_2$ in gaseous state is:
Explanation: Two bond pairs with no lone pairs give linear geometry.
82. Shape of BF$_3$ is:
Explanation: Three bond pairs and no lone pairs.
83. Shape of CH$_4$ is:
Explanation: sp$^3$ hybridization gives tetrahedral shape.
84. Shape of NH$_3$ is:
Explanation: One lone pair compresses the bond angle.
85. Shape of H$_2$O is:
Explanation: Two lone pairs on oxygen create a bent shape.
86. Hybridization of carbon in methane is:
Explanation: Four equivalent sigma bonds require sp$^3$ hybridization.
87. Hybridization of carbon in ethene is:
Explanation: Each carbon forms three sigma bonds and one pi bond.
88. Hybridization of carbon in ethyne is:
Explanation: Triple bond implies sp hybridization.
89. A molecule is polar when it has:
Explanation: Bond dipoles must not cancel overall.
90. CO$_2$ is non-polar because it is:
Explanation: Its equal bond dipoles cancel.
91. NH$_3$ is polar because it is:
Explanation: Its geometry leaves a net dipole.
92. Hydrogen bonding is strongest when H is bonded to:
Explanation: High electronegativity and small size favor H-bonding.
93. Resonance structures differ only in the arrangement of:
Explanation: The atomic framework remains fixed.
94. In molecular orbital theory, bond order is:
Explanation: This is the MO bond-order formula.
95. O$_2$ is paramagnetic because it has:
Explanation: MO theory explains its unpaired electrons.
96. A single bond is always a:
Explanation: Single covalent bonds are sigma bonds.
97. A double bond contains:
Explanation: The first overlap is sigma, second is pi.
98. Repulsion order among electron pairs is:
Explanation: Lone pairs occupy more space and repel more strongly.
99. Incomplete octet is shown by:
Explanation: Boron has only six electrons around it in BF$_3$.
100. The strongest quick route in this chapter is to connect Lewis structure, electron-pair repulsion, and:
Explanation: That trio explains shape, angle, and polarity.
101. The octet rule is based on the tendency of atoms to attain:
Explanation: Atoms tend toward stable noble-gas-like valence shells.
102. A bond formed by transfer of electrons is:
Explanation: Electron transfer gives oppositely charged ions.
103. A bond formed by sharing of electron pairs is:
Explanation: Covalent bonding uses shared pairs.
104. Formal charge on an atom is based on:
Explanation: It is a bookkeeping tool for Lewis structures.
105. According to VSEPR theory, electron pairs around the central atom arrange to:
Explanation: Repulsion minimization determines geometry.
106. Shape of BeCl$_2$ in gaseous state is:
Explanation: Two bond pairs with no lone pairs give linear geometry.
107. Shape of BF$_3$ is:
Explanation: Three bond pairs and no lone pairs.
108. Shape of CH$_4$ is:
Explanation: sp$^3$ hybridization gives tetrahedral shape.
109. Shape of NH$_3$ is:
Explanation: One lone pair compresses the bond angle.
110. Shape of H$_2$O is:
Explanation: Two lone pairs on oxygen create a bent shape.
111. Hybridization of carbon in methane is:
Explanation: Four equivalent sigma bonds require sp$^3$ hybridization.
112. Hybridization of carbon in ethene is:
Explanation: Each carbon forms three sigma bonds and one pi bond.
113. Hybridization of carbon in ethyne is:
Explanation: Triple bond implies sp hybridization.
114. A molecule is polar when it has:
Explanation: Bond dipoles must not cancel overall.
115. CO$_2$ is non-polar because it is:
Explanation: Its equal bond dipoles cancel.
116. NH$_3$ is polar because it is:
Explanation: Its geometry leaves a net dipole.
117. Hydrogen bonding is strongest when H is bonded to:
Explanation: High electronegativity and small size favor H-bonding.
118. Resonance structures differ only in the arrangement of:
Explanation: The atomic framework remains fixed.
119. In molecular orbital theory, bond order is:
Explanation: This is the MO bond-order formula.
120. O$_2$ is paramagnetic because it has:
Explanation: MO theory explains its unpaired electrons.
121. A single bond is always a:
Explanation: Single covalent bonds are sigma bonds.
122. A double bond contains:
Explanation: The first overlap is sigma, second is pi.
123. Repulsion order among electron pairs is:
Explanation: Lone pairs occupy more space and repel more strongly.
124. Incomplete octet is shown by:
Explanation: Boron has only six electrons around it in BF$_3$.
125. The strongest quick route in this chapter is to connect Lewis structure, electron-pair repulsion, and:
Explanation: That trio explains shape, angle, and polarity.