{"id":12756,"date":"2025-09-22T13:29:20","date_gmt":"2025-09-22T12:29:20","guid":{"rendered":"https:\/\/mcqsadda.com\/?p=12756"},"modified":"2025-10-22T10:16:24","modified_gmt":"2025-10-22T09:16:24","slug":"chemical-bonding-top-100-mcqs-with-answer-and-explanation","status":"publish","type":"post","link":"https:\/\/mcqsadda.com\/index.php\/2025\/09\/22\/chemical-bonding-top-100-mcqs-with-answer-and-explanation\/","title":{"rendered":"Chemical bonding Top 100 MCQs With Answer and Explanation"},"content":{"rendered":"\n

1. Which type of bond is formed by transfer of electrons?<\/mark><\/strong>
A) Ionic bond
B) Covalent bond
C) Metallic bond
D) Hydrogen bond
Answer: A<\/strong>
Explanation<\/strong>:<\/em> Ionic bonds form due to complete transfer of electrons from one atom to another.<\/p>\n\n\n\n

2. Ionic bond is generally formed between:<\/mark><\/strong>
A) Metal & Non-metal
B) Metal & Metal
C) Non-metal & Non-metal
D) Noble gases
Answer: A<\/strong>
Explanation<\/strong>: Metals lose electrons, non-metals gain electrons \u2192 ionic bond.<\/p>\n\n\n\n

3. Which of the following is an example of ionic compound?<\/mark><\/strong>
A) HCl
B) NaCl
C) H\u2082O
D) CO\u2082
Answer: B<\/strong>
Explanation<\/strong>: NaCl is ionic due to transfer of electron from Na to Cl.<\/p>\n\n\n\n

4. A covalent bond is formed due to:<\/mark><\/strong>
A) Transfer of electrons
B) Sharing of electrons
C) Overlapping of orbitals
D) Both B & C
Answer: D<\/strong>
Explanation<\/strong>: Covalent bond is formed by sharing electrons via orbital overlap.<\/p>\n\n\n\n

5. Which of the following is a covalent compound?<\/mark><\/strong>
A) NaCl
B) MgO
C) HCl
D) CaF\u2082
Answer: C<\/strong>
Explanation<\/strong>: HCl forms covalent bond by sharing electrons.<\/p>\n\n\n\n

6. The bond energy is:<\/mark><\/strong>
A) Energy released in bond formation
B) Energy required to break a bond
C) Energy of atom
D) None of these
Answer: B<\/strong>
Explanation<\/strong>: Bond energy = minimum energy needed to break one mole of bonds.<\/p>\n\n\n\n

7. Bond length is:<\/mark><\/strong>
A) Distance between nuclei of bonded atoms
B) Sum of radii
C) Difference of radii
D) None
Answer: A<\/strong>
Explanation: <\/strong>Bond length is internuclear distance at minimum energy.<\/p>\n\n\n\n

8. Bond order in N\u2082 molecule is:<\/mark><\/strong>
A) 1
B) 2
C) 3
D) 4
Answer: C<\/strong>
Explanation: N\u2082 has triple bond \u2192 bond order = 3.<\/p>\n\n\n\n

9. Higher bond order means:<\/mark><\/strong>
A) Shorter bond length
B) Higher bond energy
C) Stronger bond
D) All of these
Answer: D<\/strong>
Explanation<\/strong>: Bond order \u2191 \u2192 bond length \u2193, bond energy \u2191, strength \u2191.<\/p>\n\n\n\n

10. Which has highest bond order?<\/mark><\/strong>
A) O\u2082
B) O\u2082\u207a
C) O\u2082\u207b
D) O\u2082\u00b2\u207b
Answer: B<\/strong>
Explanation<\/strong>: O\u2082\u207a has bond order 2.5 (highest among these).<\/p>\n\n\n\n

11. Which is most stable?<\/mark><\/strong>
A) N\u2082
B) O\u2082
C) F\u2082
D) Cl\u2082
Answer: A<\/strong>
Explanation<\/strong>: N\u2082 has highest bond order (3) \u2192 most stable.<\/p>\n\n\n\n

12. Ionic compounds are generally:<\/mark><\/strong>
A) Soluble in non-polar solvents
B) Soluble in polar solvents
C) Insoluble in water
D) Covalent in nature
Answer: B<\/strong>
Explanation<\/strong>: Ionic compounds dissolve in polar solvents like water.<\/p>\n\n\n\n

13. Covalent compounds generally have:<\/mark><\/strong>
A) High melting point
B) Low melting point
C) Metallic properties
D) Conductivity in solid state
Answer: B<\/strong>
Explanation<\/strong>: Covalent compounds have weak intermolecular forces \u2192 low melting points.<\/p>\n\n\n\n

14. Which has the smallest bond length?<\/mark><\/strong>
A) N\u2261N
B) O=O
C) F\u2013F
D) Cl\u2013Cl
Answer: A<\/strong>
Explanation: Triple bond \u2192 shortest bond length.<\/p>\n\n\n\n

15. Metallic bond theory is explained by:<\/mark><\/strong>
A) Electron sea model
B) Valence bond theory
C) Hybridization
D) MOT
Answer: A<\/strong>
Explanation<\/strong>: Metallic bonding is explained by free electrons in a sea model.<\/p>\n\n\n\n

16. Which has both ionic & covalent bonds?<\/mark><\/strong>
A) NaCl
B) K\u2082SO\u2084
C) NH\u2084Cl
D) H\u2082O
Answer: C<\/strong>
Explanation<\/strong>: NH\u2084Cl has covalent N\u2013H bonds and ionic NH\u2084\u207aCl\u207b bonding.<\/p>\n\n\n\n

17. Bond angle in H\u2082O is approximately:<\/mark><\/strong>
A) 180\u00b0
B) 120\u00b0
C) 109.5\u00b0
D) 104.5\u00b0
Answer: D<\/strong>
Explanation<\/strong>: Due to 2 lone pairs, bond angle reduces to 104.5\u00b0.<\/p>\n\n\n\n

18. Bond angle in NH\u2083 is:<\/mark><\/strong>
A) 120\u00b0
B) 109.5\u00b0
C) 107\u00b0
D) 90\u00b0
Answer: C<\/strong>
Explanation<\/strong>: NH\u2083 (sp\u00b3 hybridised, 1 lone pair) \u2192 bond angle 107\u00b0.<\/p>\n\n\n\n

19. Which has linear geometry?
<\/mark><\/strong>A) CO\u2082
B) NH\u2083
C) H\u2082O
D) BF\u2083
Answer: A<\/strong>
Explanation<\/strong>: CO\u2082 is sp hybridised, linear (180\u00b0).<\/p>\n\n\n\n

20. Bond angle in BF\u2083 is:
<\/mark><\/strong>A) 120\u00b0
B) 109.5\u00b0
C) 104.5\u00b0
D) 90\u00b0
Answer: A<\/strong>
Explanation<\/strong>: BF\u2083 is sp\u00b2 hybridised \u2192 trigonal planar, 120\u00b0.<\/p>\n\n\n\n

21. Which bond is strongest?<\/mark><\/strong>
A) Ionic bond
B) Covalent bond
C) Metallic bond
D) Hydrogen bond
Answer: A<\/strong>
Explanation:<\/strong> Ionic bonds are generally strongest due to electrostatic attraction.<\/p>\n\n\n\n

22. Which molecule has polar covalent bond?<\/mark><\/strong>
A) H\u2082
B) Cl\u2082
C) HCl
D) O\u2082
Answer: C<\/strong>
Explanation: <\/strong>H\u2013Cl bond is polar due to electronegativity difference.<\/p>\n\n\n\n

23. Which molecule has non-polar covalent bond?<\/mark><\/strong>
A) HCl
B) H\u2082O
C) F\u2082
D) NH\u2083
Answer: C<\/strong>
Explanation<\/strong>:<\/strong><\/em> F\u2082 has equal sharing (same atoms) \u2192 non-polar.<\/p>\n\n\n\n

24. Lattice energy of ionic compounds depends on:<\/mark><\/strong>
A) Size of ions
B) Charge of ions
C) Distance between ions
D) All of these
Answer: D<\/strong>
Explanation: <\/strong>Lattice energy \u221d q\u2081q\u2082 \/ r.<\/p>\n\n\n\n

25. Which has highest lattice energy?<\/mark><\/strong>
A) NaCl
B) MgO
C) KCl
D) CaO
Answer: B<\/strong>
Explanation: <\/strong>Mg\u00b2\u207aO\u00b2\u207b has highest charges \u2192 highest lattice energy.<\/p>\n\n\n\n

26. The VSEPR theory is used to predict:<\/mark><\/strong>
A) Bond energy
B) Bond order
C) Shape of molecules
D) Lattice energy
Answer: C<\/strong>
Explanation:<\/strong> VSEPR theory predicts molecular geometry based on repulsion between electron pairs.<\/p>\n\n\n\n

27. According to VSEPR theory, shape of BeCl\u2082 is:<\/mark><\/strong>
A) Linear
B) Bent
C) Trigonal planar
D) Tetrahedral
Answer: A<\/strong>
Explanation:<\/strong> BeCl\u2082 has 2 bond pairs, no lone pairs \u2192 linear (180\u00b0).<\/p>\n\n\n\n

28. Shape of BF\u2083 is:<\/mark><\/strong>
A) Linear
B) Trigonal planar
C) Tetrahedral
D) Pyramidal
Answer: B
Explanation: <\/strong>BF\u2083 is sp\u00b2 hybridised, 120\u00b0 bond angle \u2192 trigonal planar.<\/p>\n\n\n\n

29. The shape of CH\u2084 molecule is:<\/mark><\/strong>
A) Trigonal planar
B) Square planar
C) Tetrahedral
D) Linear
Answer: C<\/strong>
Explanation: <\/strong>CH\u2084 is sp\u00b3 hybridised, tetrahedral (109.5\u00b0).<\/p>\n\n\n\n

30. Hybridisation of carbon in CH\u2084 is:<\/mark><\/strong>
A) sp
B) sp\u00b2
C) sp\u00b3
D) dsp\u00b2
Answer: C<\/strong>
Explanation: <\/strong>CH\u2084 has 4 sigma bonds \u2192 sp\u00b3 hybridisation.<\/p>\n\n\n\n

31. The shape of NH\u2083 molecule is:<\/mark><\/strong>
A) Linear
B) Trigonal planar
C) Pyramidal
D) Tetrahedral
Answer: C<\/strong>
Explanation:<\/strong> NH\u2083 has sp\u00b3 hybridisation, one lone pair \u2192 pyramidal (107\u00b0).<\/p>\n\n\n\n

32. The shape of H\u2082O molecule is:<\/mark><\/strong>
A) Linear
B) Bent
C) Tetrahedral
D) Trigonal planar
Answer: B<\/strong>
Explanation: <\/strong>H\u2082O has sp\u00b3 hybridisation, two lone pairs \u2192 bent (104.5\u00b0).<\/p>\n\n\n\n

33. Which has trigonal bipyramidal geometry?<\/mark><\/strong>
A) PCl\u2085
B) SF\u2086
C) ClF\u2083
D) XeF\u2082
Answer: A<\/strong>
Explanation: <\/strong>PCl\u2085 is sp\u00b3d hybridised \u2192 trigonal bipyramidal.<\/p>\n\n\n\n

34. Which has octahedral geometry?<\/mark><\/strong>
A) PCl\u2085
B) SF\u2086
C) XeF\u2082
D) IF\u2083
Answer: B<\/strong>
Explanation: <\/strong>SF\u2086 is sp\u00b3d\u00b2 hybridised \u2192 octahedral.<\/p>\n\n\n\n

35. Hybridisation of Xe in XeF\u2082 is:<\/mark><\/strong>
A) sp\u00b3
B) sp\u00b3d
C) sp\u00b3d\u00b2
D) sp\u00b3d\u00b3
Answer: B<\/strong>
Explanation: <\/strong>XeF\u2082 \u2192 sp\u00b3d hybridisation, linear shape.<\/p>\n\n\n\n

36. Shape of ClF\u2083 is:<\/mark><\/strong>
A) Linear
B) T-shaped
C) Trigonal planar
D) Octahedral
Answer: B
Explanation: <\/strong>ClF\u2083 has sp\u00b3d hybridisation with 2 lone pairs \u2192 T-shaped.<\/p>\n\n\n\n

37. Hybridisation in SF\u2084 is:<\/mark><\/strong>
A) sp\u00b3
B) sp\u00b3d
C) sp\u00b3d\u00b2
D) sp\u00b3d\u00b3
Answer: B<\/strong>
Explanation: <\/strong>SF\u2084 is sp\u00b3d hybridised, seesaw shape.<\/p>\n\n\n\n

38. Shape of SF\u2084 is:<\/mark><\/strong>
A) Linear
B) Seesaw
C) Square planar
D) T-shaped
Answer: B<\/strong>
Explanation: <\/strong>SF\u2084 (sp\u00b3d) has one lone pair \u2192 seesaw geometry.<\/p>\n\n\n\n

39. In XeF\u2084, the geometry is:<\/mark><\/strong>
A) Square planar
B) Octahedral
C) Tetrahedral
D) Trigonal bipyramidal
Answer: A<\/strong>
Explanation:<\/strong> <\/em>XeF\u2084 has sp\u00b3d\u00b2 hybridisation with 2 lone pairs \u2192 square planar.<\/p>\n\n\n\n

40. Which molecule has square pyramidal shape?<\/mark><\/strong>
A) XeF\u2082
B) XeF\u2084
C) IF\u2085
D) SF\u2086
Answer: C<\/strong>
Explanation:<\/strong> IF\u2085 is sp\u00b3d\u00b2 hybridised with one lone pair \u2192 square pyramidal.<\/p>\n\n\n\n

41. The shape of XeF\u2086 is:<\/mark><\/strong>
A) Octahedral
B) Distorted octahedral
C) Square planar
D) Trigonal bipyramidal
Answer: B<\/strong>
Explanation:<\/strong> XeF\u2086 is sp\u00b3d\u00b3 hybridised with one lone pair \u2192 distorted octahedral.<\/p>\n\n\n\n

42. Which of the following is non-linear?<\/mark><\/strong>
A) CO\u2082
B) BeCl\u2082
C) H\u2082O
D) C\u2082H\u2082
Answer: C<\/strong>
Explanation: <\/strong>H\u2082O has bent shape, others are linear.<\/p>\n\n\n\n

43. Hybridisation of C in C\u2082H\u2082 is:<\/strong><\/mark>
A) sp\u00b3
B) sp\u00b2
C) sp
D) dsp\u00b2
Answer: C<\/strong>
Explanation: <\/strong>C in acetylene (C\u2082H\u2082) is sp hybridised (linear).<\/p>\n\n\n\n

44. Hybridisation of C in C\u2082H\u2084 is:<\/mark><\/strong>
A) sp\u00b3
B) sp\u00b2
C) sp
D) dsp\u00b2
Answer: B<\/strong>
Explanation: <\/strong>Ethene has double bond \u2192 sp\u00b2 hybridisation.<\/p>\n\n\n\n

45. Hybridisation of C in C\u2082H\u2086 is:<\/mark><\/strong>
A) sp\u00b3
B) sp\u00b2
C) sp
D) dsp\u00b2
Answer: A<\/strong>
Explanation:<\/strong> Ethane has only single bonds \u2192 sp\u00b3 hybridisation.<\/p>\n\n\n\n

46. The bond angle in sp\u00b3 hybridisation (ideal) is:<\/strong><\/mark>
A) 90\u00b0
B) 109.5\u00b0
C) 120\u00b0
D) 180\u00b0
Answer: B<\/strong>
Explanation: <\/strong>sp\u00b3 \u2192 tetrahedral \u2192 109.5\u00b0.<\/p>\n\n\n\n

47. The bond angle in sp\u00b2 hybridisation is:<\/strong><\/mark>
A) 90\u00b0
B) 109.5\u00b0
C) 120\u00b0
D) 180\u00b0
Answer: C<\/strong>
Explanation:<\/strong> sp\u00b2 \u2192 trigonal planar \u2192 120\u00b0.<\/p>\n\n\n\n

48. The bond angle in sp hybridisation is:<\/strong><\/mark>
A) 90\u00b0
B) 109.5\u00b0
C) 120\u00b0
D) 180\u00b0
Answer: D<\/strong>
Explanation: <\/strong>sp \u2192 linear \u2192 180\u00b0.<\/p>\n\n\n\n

49. In NH\u2084\u207a ion, the hybridisation of N is:<\/mark><\/strong>
A) sp\u00b2
B) sp\u00b3
C) sp\u00b3d
D) sp\u00b3d\u00b2
Answer: B<\/strong>
Explanation: <\/strong>NH\u2084\u207a has 4 sigma bonds, no lone pairs \u2192 sp\u00b3 hybridisation.<\/p>\n\n\n\n

50. Which of the following is trigonal pyramidal?<\/mark><\/strong>
A) BF\u2083
B) NH\u2083
C) CH\u2084
D) CO\u2082
Answer: B<\/strong>
Explanation: <\/strong>NH\u2083 has sp\u00b3 hybridisation with one lone pair \u2192 trigonal pyramidal.<\/p>\n\n\n\n

51. Valence Bond Theory (VBT) explains bond formation by:<\/mark><\/strong>
A) Sharing of electrons
B) Transfer of electrons
C) Overlap of atomic orbitals
D) Lattice formation
Answer: C<\/strong>
Explanation: <\/strong>VBT states that covalent bonds are formed by overlapping of atomic orbitals containing unpaired electrons.<\/p>\n\n\n\n

52. The overlapping of orbitals along the internuclear axis forms:<\/mark><\/strong>
A) \u03c0-bond
B) \u03c3-bond
C) Ionic bond
D) Metallic bond
Answer: B<\/strong>
Explanation: <\/strong>End-to-end overlap \u2192 sigma (\u03c3) bond.<\/p>\n\n\n\n

53. Sidewise overlap of orbitals forms:<\/strong><\/mark>
A) \u03c3-bond
B) \u03c0-bond
C) Ionic bond
D) Hydrogen bond
Answer: B<\/strong>
Explanation: Side-by-side overlap \u2192 pi (\u03c0) bond.<\/p>\n\n\n\n

54. Which bond is stronger?<\/mark><\/strong>
A) \u03c3-bond
B) \u03c0-bond
C) Both equal
D) None
Answer: A<\/strong>
Explanation: \u03c3-bond is stronger due to greater overlap.<\/p>\n\n\n\n

55. A double bond contains:<\/mark><\/strong>
A) 1 \u03c3 + 1 \u03c0
B) 2 \u03c3
C) 1 \u03c3 only
D) 2 \u03c0
Answer: A<\/strong>
Explanation:<\/strong> Double bond = 1 sigma + 1 pi.<\/p>\n\n\n\n

56. A triple bond contains:<\/mark><\/strong>
A) 1 \u03c3 + 1 \u03c0
B) 1 \u03c3 + 2 \u03c0
C) 2 \u03c3 + 1 \u03c0
D) 3 \u03c3
Answer: B<\/strong>
Explanation:<\/strong> Triple bond = 1 sigma + 2 pi.<\/p>\n\n\n\n

57. In Molecular Orbital Theory (MOT), molecular orbitals are formed by:<\/mark><\/strong>
A) Mixing of nuclei
B) Mixing of atomic orbitals
C) Overlap of sigma bonds
D) Overlap of pi bonds
Answer: B<\/strong>
Explanation:<\/strong> MOT states molecular orbitals are linear combinations of atomic orbitals (LCAO).<\/p>\n\n\n\n

58. Which is true for bonding molecular orbital (BMO)?<\/mark><\/strong>
A) Higher energy than atomic orbital
B) Lower energy than atomic orbital
C) Destabilising
D) Anti-symmetric
Answer: B<\/strong>
Explanation:<\/strong> BMO has lower energy than atomic orbitals \u2192 stabilising.<\/p>\n\n\n\n

59. Which is true for antibonding molecular orbital?<\/mark><\/strong>
A) Higher energy
B) Lower energy
C) Stabilising
D) Increases bond order
Answer: A<\/strong>
Explanation: <\/strong>Antibonding orbitals have higher energy \u2192 destabilising.<\/p>\n\n\n\n

60. Bond order (MOT) =<\/mark><\/strong>
A) \u00bd (Nb \u2013 Na)
B) \u00bd (Na \u2013 Nb)
C) Nb + Na
D) Nb \/ Na
Answer: A<\/strong>
Explanation:<\/strong> Bond order = \u00bd (no. of bonding electrons \u2013 no. of antibonding electrons).<\/p>\n\n\n\n

61. In H\u2082 molecule, bond order is:<\/mark><\/strong>
A) 0
B) 1
C) 2
D) 3
Answer: B<\/strong>
Explanation: <\/strong>H\u2082 \u2192 2 bonding e\u207b, 0 antibonding e\u207b \u2192 (2\u20130)\/2 = 1.<\/p>\n\n\n\n

62. In He\u2082 molecule, bond order is:<\/mark><\/strong>
A) 0
B) 1
C) 2
D) 3
Answer: A<\/strong>
Explanation: <\/strong>He\u2082 \u2192 2 bonding e\u207b, 2 antibonding e\u207b \u2192 (2\u20132)\/2 = 0 (unstable).<\/p>\n\n\n\n

63. Bond order of O\u2082 molecule is:<\/mark><\/strong>
A) 1
B) 2
C) 3
D) 2.5
Answer: B<\/strong>
Explanation: <\/strong>O\u2082 \u2192 bond order = 2 (paramagnetic).<\/p>\n\n\n\n

64. O\u2082 molecule is:<\/mark><\/strong>
A) Diamagnetic
B) Paramagnetic
C) Ferromagnetic
D) None
Answer: B<\/strong>
Explanation: <\/strong>O\u2082 has 2 unpaired electrons in \u03c0 orbitals \u2192 paramagnetic.*<\/p>\n\n\n\n

65. Bond order of O\u2082\u207a is:<\/mark><\/strong>
A) 1.5
B) 2
C) 2.5
D) 3
Answer: C<\/strong>
Explanation: <\/strong>O\u2082\u207a \u2192 one electron removed from antibonding \u2192 bond order 2.5.<\/p>\n\n\n\n

66. Bond order of O\u2082\u207b is:<\/mark><\/strong>
A) 1.5
B) 2
C) 2.5
D) 3
Answer: A<\/strong>
Explanation:<\/strong> O\u2082\u207b \u2192 one electron added to antibonding orbital \u2192 bond order 1.5.<\/p>\n\n\n\n

67. Which is diamagnetic?<\/mark><\/strong>
A) O\u2082
B) O\u2082\u207a
C) O\u2082\u00b2\u207b
D) B\u2082
Answer: C<\/strong>
Explanation: <\/strong>O\u2082\u00b2\u207b has paired electrons \u2192 diamagnetic.<\/p>\n\n\n\n

68. Bond order of N\u2082 is:<\/mark><\/strong>
A) 1
B) 2
C) 3
D) 4
Answer: C<\/strong>
Explanation: <\/strong>N\u2082 bond order = 3 (triple bond, very stable).<\/p>\n\n\n\n

69. Bond order of N\u2082\u207a is:<\/mark><\/strong>
A) 2
B) 2.5
C) 3
D) 3.5
Answer: B<\/strong>
Explanation: <\/strong>N\u2082\u207a loses one electron from bonding orbital \u2192 bond order 2.5.<\/p>\n\n\n\n

70. Which molecule is paramagnetic according to MOT?<\/mark><\/strong>
A) N\u2082
B) O\u2082
C) CO\u2082
D) H\u2082O
Answer: B<\/strong>
Explanation:<\/strong> O\u2082 is paramagnetic (2 unpaired electrons).<\/p>\n\n\n\n

71. The increasing bond order in O\u2082 species is:<\/mark><\/strong>
A) O\u2082 < O\u2082\u207a < O\u2082\u00b2\u207b
B) O\u2082\u00b2\u207b < O\u2082 < O\u2082\u207a
C) O\u2082 < O\u2082\u00b2\u207b < O\u2082\u207a
D) O\u2082\u207a < O\u2082 < O\u2082\u00b2\u207b
Answer: B<\/strong>
Explanation: <\/strong>Bond order: O\u2082\u00b2\u207b (1) < O\u2082 (2) < O\u2082\u207a (2.5).<\/p>\n\n\n\n

72. According to MOT, which species is least stable?<\/mark><\/strong>
A) N\u2082
B) O\u2082
C) He\u2082
D) CO
Answer: C<\/strong>
Explanation:<\/strong> He\u2082 bond order = 0 \u2192 unstable.<\/p>\n\n\n\n

73. In B\u2082 molecule, magnetic property is:<\/mark><\/strong>
A) Diamagnetic
B) Paramagnetic
C) Ferromagnetic
D) None
Answer: B<\/strong>
Explanation: B\u2082 has 2 unpaired electrons in \u03c0 orbitals \u2192 paramagnetic.<\/p>\n\n\n\n

74. CO molecule is isoelectronic with:<\/mark><\/strong>
A) N\u2082
B) O\u2082
C) F\u2082
D) Ne\u2082
Answer: A<\/strong>
Explanation:<\/strong> <\/em>CO (14 e\u207b) is isoelectronic with N\u2082 (14 e\u207b).<\/p>\n\n\n\n

75. Which has highest bond energy?<\/mark><\/strong>
A) O\u2082
B) N\u2082
C) F\u2082
D) Cl\u2082
Answer: B<\/strong>
Explanation: <\/strong>N\u2082 has bond order 3 (triple bond) \u2192 highest bond energy.<\/p>\n\n\n\n

76. Resonance in molecules occurs due to:<\/mark><\/strong>
A) Rapid interconversion of isomers
B) Delocalization of electrons
C) Vibrations of nuclei
D) Hybridization of orbitals
Answer:<\/strong> B
Explanation:<\/strong> Resonance represents electron delocalization across different positions without actual movement of atoms.<\/p>\n\n\n\n

77. The resonance energy of benzene is approximately:<\/mark><\/strong>
A) 36 kcal\/mol
B) 50 kcal\/mol
C) 100 kcal\/mol
D) 10 kcal\/mol
Answer:<\/strong> A
Explanation:<\/strong> Benzene is more stable than expected due to resonance energy (~36 kcal\/mol).<\/p>\n\n\n\n

78. Which ion shows resonance?<\/mark><\/strong>
A) NH\u2084\u207a
B) CO\u2083\u00b2\u207b
C) Na\u207a
D) Cl\u207b
Answer:<\/strong> B
Explanation:<\/strong> Carbonate ion has delocalized \u03c0-electrons across three oxygen atoms.<\/p>\n\n\n\n

79. The most stable resonance structure is the one with:<\/mark><\/strong>
A) Maximum number of covalent bonds
B) Least formal charge
C) Negative charge on more electronegative atom
D) All of the above
Answer:<\/strong> D
Explanation:<\/strong> Stability depends on bond maximization, proper charge placement, and minimal separation.<\/p>\n\n\n\n

80. In resonance, the actual structure of a molecule is:<\/mark><\/strong>
A) One of the resonance forms
B) A mixture of resonance forms
C) An intermediate hybrid
D) Rapidly interchanging isomers
Answer:<\/strong> C
Explanation:<\/strong> The real structure is a resonance hybrid, more stable than any single canonical form.<\/p>\n\n\n\n

81. Which of the following molecules has resonance?<\/mark><\/strong>
A) SO\u2082
B) NH\u2083
C) H\u2082O
D) CH\u2084
Answer:<\/strong> A
Explanation:<\/strong> SO\u2082 has multiple resonance structures with delocalized \u03c0-bonds.<\/p>\n\n\n\n

82. Hydrogen bonding is strongest in:<\/mark><\/strong>
A) H\u2082S
B) H\u2082Se
C) H\u2082O
D) H\u2082Te
Answer:<\/strong> C
Explanation:<\/strong> Due to high electronegativity and small size of oxygen, H\u2082O shows strong H-bonding.<\/p>\n\n\n\n

83. Hydrogen bonding leads to:<\/mark><\/strong>
A) Higher boiling points
B) Higher viscosity
C) Higher surface tension
D) All of the above
Answer:<\/strong> D
Explanation:<\/strong> H-bonding creates strong intermolecular forces, increasing these physical properties.<\/p>\n\n\n\n

84. Which of the following exhibits intramolecular hydrogen bonding?<\/mark><\/strong>
A) o-nitrophenol
B) p-nitrophenol
C) m-nitrophenol
D) Phenol
Answer:<\/strong> A
Explanation:<\/strong> o-Nitrophenol has intramolecular H-bonding between \u2013OH and \u2013NO\u2082 group.<\/p>\n\n\n\n

85. Which of the following exhibits intermolecular hydrogen bonding?<\/mark><\/strong>
A) o-nitrophenol
B) p-nitrophenol
C) Both A and B
D) None
Answer:<\/strong> B
Explanation:<\/strong> p-Nitrophenol molecules form H-bonds with neighboring molecules.<\/p>\n\n\n\n

86. Ice floats on water due to:<\/mark><\/strong>
A) Lower density of ice because of H-bonding
B) Higher density of ice because of H-bonding
C) Presence of covalent bonds
D) Resonance in H\u2082O
Answer:<\/strong> A
Explanation:<\/strong> H-bonding in ice creates an open lattice structure, lowering density.<\/p>\n\n\n\n

87. Which of the following molecules shows resonance stabilization?<\/mark><\/strong>
A) CH\u2082=CH\u2082
B) CH\u2083\u2013CH\u2083
C) C\u2086H\u2086
D) CH\u2084
Answer:<\/strong> C
Explanation:<\/strong> Benzene has delocalized \u03c0-electrons and resonance stabilization.<\/p>\n\n\n\n

88. Which type of hydrogen bond is stronger?<\/mark><\/strong>
A) Intermolecular
B) Intramolecular
C) Both equal
D) None
Answer:<\/strong> A
Explanation:<\/strong> Intermolecular H-bonds generally lead to higher stability and stronger interactions.<\/p>\n\n\n\n

89. Which factor is not essential for hydrogen bonding?<\/mark><\/strong>
A) High electronegativity
B) Small size of atom
C) Presence of lone pairs
D) High atomic mass
Answer:<\/strong> D
Explanation:<\/strong> Atomic mass doesn\u2019t influence hydrogen bonding; electronegativity and size do.<\/p>\n\n\n\n

90. Which of the following shows hydrogen bonding in liquid state?<\/mark><\/strong>
A) HF
B) NH\u2083
C) H\u2082O
D) All of these
Answer:<\/strong> D
Explanation:<\/strong> HF, NH\u2083, and H\u2082O all form intermolecular hydrogen bonds in liquid state.<\/p>\n\n\n\n

91. The abnormal high boiling point of water is due to:<\/mark><\/strong>
A) Ionic bonding
B) Covalent bonding
C) Hydrogen bonding
D) van der Waals forces
Answer:<\/strong> C
Explanation:<\/strong> Strong hydrogen bonds between water molecules increase its boiling point.<\/p>\n\n\n\n

92. Which of the following molecules does not show resonance?<\/mark><\/strong>
A) O\u2083
B) NO\u2082\u207b
C) H\u2082O
D) CO\u2083\u00b2\u207b
Answer:<\/strong> C
Explanation:<\/strong> Water has localized bonds, no delocalization of electrons.<\/p>\n\n\n\n

93. Which of the following molecules shows extensive hydrogen bonding leading to dimer formation?<\/mark><\/strong>
A) Acetic acid
B) Methanol
C) Phenol
D) Ammonia
Answer:<\/strong> A
Explanation:<\/strong> Acetic acid forms strong dimeric structures via intermolecular H-bonds.<\/p>\n\n\n\n

94. Hydrogen bonding is absent in:<\/mark><\/strong>
A) HCl
B) HF
C) NH\u2083
D) H\u2082O
Answer:<\/strong> A
Explanation:<\/strong> Chlorine is large and less electronegative, so HCl does not form H-bonds.<\/p>\n\n\n\n

95. Which of the following explains the planarity of benzene?<\/mark><\/strong>
A) Hybridization
B) Resonance
C) Hydrogen bonding
D) Ionic nature
Answer:<\/strong> B
Explanation:<\/strong> Delocalized \u03c0-electrons in resonance enforce planarity in benzene.<\/p>\n\n\n\n

96. Which bond order indicates resonance stabilization?<\/mark><\/strong>
A) 1
B) 1.33
C) 2
D) 3
Answer:<\/strong> B
Explanation:<\/strong> Bond orders like 1.33 (e.g., CO\u2083\u00b2\u207b, NO\u2083\u207b) arise due to resonance.<\/p>\n\n\n\n

97. The anomalous high viscosity of glycerol is due to:<\/mark><\/strong>
A) Ionic bonding
B) Extensive hydrogen bonding
C) Resonance
D) van der Waals forces
Answer:<\/strong> B
Explanation:<\/strong> Glycerol has three \u2013OH groups, forming multiple H-bonds \u2192 high viscosity.<\/p>\n\n\n\n

98. The bond angle in water decreases from tetrahedral angle due to:<\/mark><\/strong>
A) Resonance
B) Lone pair\u2013bond pair repulsion and H-bonding
C) Hydrogen bonding only
D) Ionic bonding
Answer:<\/strong> B
Explanation:<\/strong> Strong lone pair repulsions reduce bond angle to ~104.5\u00b0.<\/p>\n\n\n\n

99. Which of the following molecules exhibits both resonance and hydrogen bonding?<\/strong><\/mark>
A) Benzene
B) Acetic acid
C) Methane
D) Ethylene
Answer:<\/strong> B
Explanation:<\/strong> Acetic acid has resonance in \u2013COOH and hydrogen bonding between molecules.<\/p>\n\n\n\n

100. Which property of DNA structure is due to hydrogen bonding?<\/mark><\/strong>
A) Double helix stability
B) Base pairing specificity
C) Complementary strand binding
D) All of the above
Answer:<\/strong> D
Explanation:<\/strong> H-bonding between bases stabilizes double helix and ensures specific base pairing.<\/p>\n","protected":false},"excerpt":{"rendered":"

1. Which type of bond is formed by transfer of electrons?A) Ionic bondB) Covalent bondC) Metallic bondD) Hydrogen bondAnswer: AExplanation: Ionic bonds form due to complete transfer of electrons from one atom to another. 2. Ionic bond is generally formed between:A) Metal & Non-metalB) Metal & MetalC) Non-metal & Non-metalD) Noble gasesAnswer: AExplanation: Metals lose<\/p>\n","protected":false},"author":1,"featured_media":0,"comment_status":"open","ping_status":"open","sticky":false,"template":"","format":"standard","meta":{"footnotes":""},"categories":[9],"tags":[15924,15926,15922,15915,10966,15886,15892,15876,15898,15901,15887,15899,15879,15883,15928,15914,15916,15884,15918,15921,15919,4029,15897,5649,5623,15923,15913,15927,15920,15900,15896,15894,15917,15925],"class_list":{"0":"post-12756","1":"post","2":"type-post","3":"status-publish","4":"format-standard","6":"category-chemistry","7":"tag-bond-energy","8":"tag-bond-length","9":"tag-chemical-bonding","10":"tag-chemical-bonding-problems","11":"tag-chemical-bonding-top-100-mcqs-with-answer-and-explanation","12":"tag-chemistry-formulas","13":"tag-chemistry-learning","14":"tag-chemistry-mcqs","15":"tag-chemistry-preparation-material","16":"tag-chemistry-questions-and-answers","17":"tag-chemistry-quiz","18":"tag-chemistry-revision","19":"tag-chemistry-study-material","20":"tag-competitive-exam-chemistry","21":"tag-covalent-bond","22":"tag-covalent-compounds","23":"tag-hybridization","24":"tag-intermolecular-forces","25":"tag-ionic-bond","26":"tag-ionic-compounds","27":"tag-lewis-structure","28":"tag-mcqs-adda","29":"tag-mcqs-for-chemistry-exam","30":"tag-mcqs-for-pc-psi-sda-fda-pdo-vao-banking-kas-ias-ssc-gd-ssc-chsl-ssc-cgl-for-all-compitative-exams","31":"tag-mcqs-for-sda-fda-pdo-vao-banking-kas-ias-ssc-gd-ssc-chsl-ssc-cgl-for-all-compitative-exams","32":"tag-metallic-bond","33":"tag-molecular-geometry","34":"tag-molecular-structure","35":"tag-polar-and-nonpolar-bonds","36":"tag-psc-chemistry-mcqs","37":"tag-ssc-chemistry-mcqs","38":"tag-upsc-chemistry-mcqs","39":"tag-valence-electrons","40":"tag-vsepr-theory"},"_links":{"self":[{"href":"https:\/\/mcqsadda.com\/index.php\/wp-json\/wp\/v2\/posts\/12756","targetHints":{"allow":["GET"]}}],"collection":[{"href":"https:\/\/mcqsadda.com\/index.php\/wp-json\/wp\/v2\/posts"}],"about":[{"href":"https:\/\/mcqsadda.com\/index.php\/wp-json\/wp\/v2\/types\/post"}],"author":[{"embeddable":true,"href":"https:\/\/mcqsadda.com\/index.php\/wp-json\/wp\/v2\/users\/1"}],"replies":[{"embeddable":true,"href":"https:\/\/mcqsadda.com\/index.php\/wp-json\/wp\/v2\/comments?post=12756"}],"version-history":[{"count":7,"href":"https:\/\/mcqsadda.com\/index.php\/wp-json\/wp\/v2\/posts\/12756\/revisions"}],"predecessor-version":[{"id":12925,"href":"https:\/\/mcqsadda.com\/index.php\/wp-json\/wp\/v2\/posts\/12756\/revisions\/12925"}],"wp:attachment":[{"href":"https:\/\/mcqsadda.com\/index.php\/wp-json\/wp\/v2\/media?parent=12756"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/mcqsadda.com\/index.php\/wp-json\/wp\/v2\/categories?post=12756"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/mcqsadda.com\/index.php\/wp-json\/wp\/v2\/tags?post=12756"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}