Here below some MCQ’s about “Molecular orbital theory” with answer which is well explained. Let’s check one by one.
- What does MO stand for in molecular orbital theory?
A) Magnetic Orbital
B) Molecular Orbital
C) Molecule Orbital
D) None of the above
Answer: B
Explanation: MO refers to the molecular orbital, which describes the behavior of electrons in a molecule.
2. Which principle states that electrons occupy the lowest energy orbitals first?
A) Hund’s Rule
B) Pauli Exclusion Principle
C) Aufbau Principle
D) Octet Rule
Answer: C
Explanation: The Aufbau Principle states that electrons fill the lowest available energy levels before occupying higher levels.
3. In which type of molecular orbitals are the electron densities concentrated between the nuclei?
A) Sigma (σ) orbitals
B) Pi (π) orbitals
C) Non-bonding orbitals
D) Antibonding orbitals
Answer: A
Explanation: Sigma orbitals have electron density concentrated along the internuclear axis, promoting bonding.
4. Which molecular orbital is formed by the head-on overlap of atomic orbitals?
A) Pi (π) orbital
B) Sigma (σ) orbital
C) Delta (δ) orbital
D) Sigma star (σ*) orbital
Answer: B
Explanation: Sigma orbitals result from the direct overlap of orbitals, allowing for strong bonding.
5. The bond order of a molecule is defined as:
A) (Number of bonding electrons – Number of antibonding electrons) / 2
B) Number of bonding electrons / Number of antibonding electrons
C) Total number of electrons / 2
D) Number of atoms in the molecule
Answer: A
Explanation: Bond order is a measure of the strength of a bond, calculated using the difference between bonding and antibonding electrons.
6. Which of the following molecules has a bond order of 1?
A) O2
B) N2
C) H2
D) He2
Answer: C
Explanation: H2 has one bond formed by a single pair of electrons, giving it a bond order of 1.
7. What type of molecular orbital results from the side-to-side overlap of p orbitals?
A) Sigma (σ) orbital
B) Pi (π) orbital
C) Delta (δ) orbital
D) Non-bonding orbital
Answer: B
Explanation: Pi orbitals are formed by the lateral overlap of p orbitals, contributing to double bonds.
8. Which of the following statements is true about antibonding molecular orbitals?
A) They stabilize the molecule.
B) They have higher energy than the corresponding bonding orbitals.
C) They contain electron density between the nuclei.
D) They can be occupied by a maximum of two electrons.
Answer: B
Explanation: Antibonding orbitals have higher energy and destabilize the molecule.
9. In which of the following molecules does the bond order equal 0?
A) O2
B) N2
C) He2
D) F2
Answer: C
Explanation: In He2, the bonding and antibonding electrons cancel out, resulting in a bond order of 0.
10. For which of the following species is the bond order 1?
A) B2
B) C2
C) N2
D) O2
Answer: A
Explanation: B2 has a bond order of 1 due to the presence of one bonding pair and no antibonding electrons.
11. Which molecular orbital is denoted by the notation σ?*
A) Non-bonding orbital
B) Antibonding sigma orbital
C) Antibonding pi orbital
D) Bonding sigma orbital
Answer: B
Explanation: The notation σ* indicates an antibonding orbital that results from the destructive interference of wave functions.
12. How many molecular orbitals are formed from two atomic orbitals?
A) 1
B) 2
C) 3
D) 4
Answer: B
Explanation: The combination of two atomic orbitals results in the formation of two molecular orbitals: one bonding and one antibonding.
13. Which of the following is not a characteristic of molecular orbitals?
A) They can be occupied by a maximum of two electrons.
B) They are localized between atoms.
C) They extend over a molecule.
D) They can be bonding or antibonding.
Answer: B
Explanation: Molecular orbitals are delocalized across the entire molecule, not localized between atoms.
14. In molecular orbital theory, the electronic configuration of O2 is:
A) 1s² 2s² 2p²
B) 1s² 2s² 2p⁴
C) 1s² 2s² 2p⁶
D) 1s² 2s² 2p³
Answer: B
Explanation: O2 has 16 total electrons, resulting in the configuration 1s² 2s² 2p⁴ in molecular orbitals.
15. What is the shape of the molecular orbital formed by the overlap of two p orbitals?
A) Spherical
B) Dumbbell
C) Linear
D) Tetrahedral
Answer: B
Explanation: P orbitals have a dumbbell shape, which is crucial for forming pi bonds.
16. Which of the following molecules is paramagnetic?
A) N2
B) O2
C) CO
D) Ne2
Answer: B
Explanation: O2 has unpaired electrons in its molecular orbital configuration, making it paramagnetic.
17. What type of bond is formed by the overlap of two s orbitals?
A) Pi (π) bond
B) Sigma (σ) bond
C) Delta (δ) bond
D) No bond
Answer: B
Explanation: The overlap of two s orbitals forms a sigma bond, the strongest type of covalent bond.
18. Which molecular orbital is lower in energy, bonding or antibonding?
A) Bonding
B) Antibonding
C) They are equal
D) It depends on the molecule
Answer: A
Explanation: Bonding molecular orbitals are lower in energy than antibonding orbitals, which helps stabilize the molecule.
19. Which of the following molecules has a bond order of 2?
A) O2
B) N2
C) CO
D) B2
Answer: C
Explanation: CO has a bond order of 2, indicating a double bond.
20. What is the shape of the molecular orbital formed by the overlap of two s orbitals?
A) Spherical
B) Dumbbell
C) Linear
D) Tetrahedral
Answer: A
Explanation: The overlap of s orbitals creates a spherical molecular orbital.
21. Which of the following statements is true about bonding molecular orbitals?
A) They are formed from the combination of orbitals with opposite phases.
B) They are higher in energy than the atomic orbitals that formed them.
C) They stabilize the molecule.
D) They have no electron density between the nuclei.
Answer: C
Explanation: Bonding molecular orbitals lower the energy of the system and stabilize the molecule.
22. What is the electron configuration for the molecular ion O2⁻?
A) 1s² 2s² 2p⁶
B) 1s² 2s² 2p⁵
C) 1s² 2s² 2p⁴ 3s²
D) 1s² 2s² 2p⁵ 3s²
Answer: D
Explanation: O2⁻ has one additional electron compared to O2, so its configuration is 1s² 2s² 2p⁵.
23. Which element has the highest bond order in diatomic molecules?
A) He
B) H
C) N
D) O
Answer: C
Explanation: N2 has a bond order of 3, the highest among common diatomic molecules.
24. Which molecular orbital is filled last in the O2 molecule?
A) 1s
B) 2s
C) 2p
D) 3s
Answer: C
Explanation: In O2, the 2p orbitals are filled after the 1s and 2s orbitals, and contain unpaired electrons contributing to its paramagnetic property.
25. Which of the following species is isoelectronic with Ne?
A) O2⁻
B) F2
C) Na⁺
D) All of the above
Answer: D
Explanation: O2⁻, F2, and Na⁺ all have the same number of electrons as Ne (10 electrons).
26. Which molecular orbital has no nodal planes?
A) 1s
B) 2p
C) σ*
D) π*
Answer: A
Explanation: The 1s molecular orbital has no nodal planes, meaning it has continuous electron density without any regions of zero probability.
27. In which molecule is the bond order 3?
A) O2
B) N2
C) F2
D) He2
Answer: B
Explanation: N2 has a bond order of 3, indicating a triple bond due to three pairs of shared electrons.
28. Which of the following orbitals is non-bonding?
A) σ2s
B) π2p
C) σ2p
D) n2p
Answer: D
Explanation: Non-bonding orbitals do not contribute to bonding and typically have no electron density between the nuclei.
29. In which molecular orbital diagram do you expect a change in energy ordering for the p orbitals?
A) Diatomic molecules of the first period
B) Diatomic molecules of the second period
C) Diatomic molecules of the third period
D) None of the above
Answer: B
Explanation: In the second period (e.g., B2, C2, N2), the π2p orbitals are lower in energy than the σ2p orbital, whereas in O2 and F2, the order reverses.
30. Which of the following species has unpaired electrons?
A) N2
B) O2
C) CO
D) He2
Answer: B
Explanation: O2 has two unpaired electrons in its molecular orbital configuration, making it paramagnetic.
31. What does a bond order of 0 indicate?
A) No bond
B) Single bond
C) Double bond
D) Triple bond
Answer: A
Explanation: A bond order of 0 indicates that there is no net bonding interaction between the atoms, meaning they do not form a bond.
32. Which molecular orbital results from the destructive interference of wave functions?
A) Bonding orbital
B) Antibonding orbital
C) Non-bonding orbital
D) Both A and C
Answer: B
Explanation: Antibonding orbitals arise from the destructive interference of wave functions from the combining atomic orbitals.
33. Which of the following has a bond length longer than that of O2?
A) F2
B) N2
C) CO
D) He2
Answer: A
Explanation: F2 has a single bond (bond order of 1) which is longer than the double bond in O2, leading to a longer bond length.
34. How many total electrons can occupy a molecular orbital?
A) 1
B) 2
C) 4
D) 8
Answer: B
Explanation: Each molecular orbital can hold a maximum of two electrons, according to the Pauli Exclusion Principle.
35. Which of the following molecules is likely to have a linear shape?
A) H2O
B) CO2
C) NH3
D) CH4
Answer: B
Explanation: CO2 has a linear molecular geometry due to the arrangement of the two double bonds around the central carbon atom.
36. What type of molecular orbital is formed by the overlap of two p orbitals?
A) Sigma (σ)
B) Pi (π)
C) Delta (δ)
D) Non-bonding
Answer: B
Explanation: The side-to-side overlap of p orbitals forms pi (π) molecular orbitals.
37. Which molecule is predicted to have a higher bond energy, N2 or O2?
A) N2
B) O2
C) They have equal bond energy.
D) Cannot be determined
Answer: A
Explanation: N2 has a triple bond (bond order of 3) compared to the double bond in O2, resulting in higher bond energy for N2.
38. Which element has the highest electronegativity?
A) Fluorine
B) Oxygen
C) Nitrogen
D) Chlorine
Answer: A
Explanation: Fluorine is the most electronegative element, meaning it has a strong tendency to attract electrons in a bond.
39. What type of molecular orbital is σ2p?
A) Bonding
B) Antibonding
C) Non-bonding
D) Both A and C
Answer: A
Explanation: σ2p is a bonding molecular orbital formed by the head-on overlap of p orbitals.
40. Which of the following molecular species is unstable?
A) He2
B) N2
C) O2
D) CO
Answer: A
Explanation: He2 is unstable because its bond order is 0, meaning there is no net bonding interaction.
41. Which of the following is an example of a homonuclear diatomic molecule?
A) CO
B) HCl
C) N2
D) NaCl
Answer: C
Explanation: N2 is a homonuclear diatomic molecule because it consists of two atoms of the same element.
42. How do bonding molecular orbitals affect the stability of a molecule?
A) They destabilize the molecule.
B) They have no effect on stability.
C) They stabilize the molecule.
D) They only affect ionic bonds.
Answer: C
Explanation: Bonding molecular orbitals lower the overall energy of the system, stabilizing the molecule.
43. Which molecule has a higher bond order than CO?
A) O2
B) N2
C) B2
D) H2
Answer: B
Explanation: N2 has a bond order of 3, which is higher than CO’s bond order of 2.
44. Which molecular orbital is filled first in a molecular orbital diagram?
A) σ*2s
B) π2p
C) σ2p
D) σ2s
Answer: D
Explanation: According to the Aufbau principle, the lowest energy orbitals are filled first, so σ2s is filled before π2p.
45. What is the primary reason for the bonding in a diatomic molecule?
A) Presence of lone pairs
B) Atomic size
C) Overlap of atomic orbitals
D) Electronegativity difference
Answer: C
Explanation: The overlap of atomic orbitals forms bonding molecular orbitals, leading to the formation of the molecule.
46. In a molecular orbital diagram, where would you find the antibonding orbitals?
A) Above the bonding orbitals
B) Below the bonding orbitals
C) At the same level as bonding orbitals
D) In a separate energy level
Answer: A
Explanation: Antibonding orbitals are always higher in energy than their corresponding bonding orbitals.
47. Which of the following species has the lowest bond energy?
A) F2
B) O2
C) N2
D) H2
Answer: A
Explanation: F2 has a single bond which is weaker than the double and triple bonds present in O2 and N2, leading to lower bond energy.
48. In the molecular orbital theory, what is meant by “degenerate” orbitals?
A) Orbitals that have different energies
B) Orbitals that have the same energy
C) Orbitals that cannot hold electrons
D) Orbitals that are non-bonding
Answer: B
Explanation: Degenerate orbitals have the same energy level, which is important for filling orbitals in accordance with Hund’s Rule.
49. Which molecule has a bond angle of approximately 120°?
A) H2O
B) NH3
C) BCl3
D) CH4
Answer: C
Explanation: BCl3 has a trigonal planar geometry, leading to bond angles of approximately 120°.
50. What is the hybridization of the central atom in CH4?
A) sp
B) sp²
C) sp³
D) dsp²
Answer: C
Explanation: The central carbon atom in CH4 undergoes sp³ hybridization to form four equivalent bonds.
51. Which molecular orbital is characterized by having a nodal plane between the two nuclei?
A) σ2s
B) π2p
C) σ2s D) π2p
Answer: C
Explanation: The σ*2s orbital has a nodal plane between the two nuclei, indicating destructive interference in the bonding.
52. What happens to the bond order if one electron is added to an antibonding molecular orbital?
A) It increases
B) It decreases
C) It stays the same
D) It becomes zero
Answer: B
Explanation: Adding an electron to an antibonding orbital reduces the bond order, weakening the bond.
53. Which molecular species is expected to have the shortest bond length?
A) O2
B) N2
C) H2
D) F2
Answer: B
Explanation: N2 has a triple bond, which results in a shorter bond length compared to O2 and H2.
54. What type of overlap is required for the formation of a sigma bond?
A) Side-to-side
B) End-to-end
C) Random
D) None
Answer: B
Explanation: Sigma bonds are formed by the end-to-end overlap of atomic orbitals, resulting in a strong bond.
55. In a molecular orbital diagram, how many total orbitals are formed from four atomic orbitals?
A) 2
B) 3
C) 4
D) 8
Answer: C
Explanation: The combination of four atomic orbitals produces four molecular orbitals (two bonding and two antibonding).
56. Which of the following molecules would you expect to have a bond angle of approximately 109.5°?
A) H2O
B) CH4
C) NH3
D) SO2
Answer: B
Explanation: CH4 has a tetrahedral shape with bond angles of about 109.5° due to sp³ hybridization.
57. Which of the following statements is true about the 2p molecular orbitals?
A) They have a spherical shape.
B) They are formed by the overlap of s orbitals.
C) They can form both bonding and antibonding orbitals.
D) They have only one nodal plane.
Answer: C
Explanation: 2p orbitals can form both bonding (π) and antibonding (π*) molecular orbitals through their lateral overlap.
58. Which type of bonding is primarily responsible for the structure of diamond?
A) Ionic bonding
B) Metallic bonding
C) Covalent bonding
D) Hydrogen bonding
Answer: C
Explanation: Diamond has a tetrahedral structure formed by strong covalent bonds between carbon atoms.
59. What is the molecular shape of SF6?
A) Octahedral
B) Tetrahedral
C) Trigonal planar
D) Linear
Answer: A
Explanation: SF6 has an octahedral molecular geometry due to sp³d² hybridization of the central sulfur atom.
60. Which of the following pairs of atoms can form a bond with the highest bond order?
A) C-C
B) N-N
C) O-O
D) C=N
Answer: B
Explanation: N-N can form a triple bond, giving it the highest bond order compared to the other pairs.
61. Which molecular orbital is filled last in the O2 molecule according to the molecular orbital theory?
A) σ2s
B) π2p
C) σ2p
D) π*2p
Answer: D
Explanation: In O2, the π*2p orbitals are filled last, containing the unpaired electrons.
62. Which of the following molecules is expected to be diamagnetic?
A) O2
B) N2
C) H2
D) F2
Answer: C
Explanation: H2 has no unpaired electrons, making it diamagnetic, while O2 has unpaired electrons and is paramagnetic.
63. Which type of hybridization is present in the central atom of PCl5?
A) sp
B) sp²
C) sp³
D) sp³d
Answer: D
Explanation: PCl5 involves sp³d hybridization, allowing the phosphorus atom to form five bonds.
64. Which molecule has a bond order of 1 and is an example of a single bond?
A) O2
B) H2
C) N2
D) CO
Answer: B
Explanation: H2 has a bond order of 1, representing a single covalent bond between two hydrogen atoms.
65. Which molecular orbital theory describes the arrangement of electrons in molecules?
A) Valence Shell Electron Pair Repulsion Theory
B) Molecular Orbital Theory
C) Hybridization Theory
D) Crystal Field Theory
Answer: B
Explanation: Molecular Orbital Theory provides a method for understanding how electrons are arranged in molecules.
66. What type of bond does Cl2 have?
A) Ionic
B) Covalent
C) Metallic
D) Hydrogen
Answer: B
Explanation: Cl2 is formed by a covalent bond due to the sharing of electrons between two chlorine atoms.
67. Which of the following statements is true regarding the bonding in O2?
A) It has a triple bond.
B) It has a double bond.
C) It has a single bond.
D) It has no bond.
Answer: B
Explanation: O2 has a double bond, resulting from two shared pairs of electrons.
68. What is the effect of adding electrons to antibonding molecular orbitals?
A) It strengthens the bond.
B) It has no effect.
C) It weakens the bond.
D) It creates new bonds.
Answer: C
Explanation: Adding electrons to antibonding orbitals weakens the overall bond in the molecule.
69. What type of molecular orbital is π2p?
A) Bonding
B) Antibonding
C) Non-bonding
D) Both A and C
Answer: A
Explanation: π2p is a bonding molecular orbital formed by the lateral overlap of p orbitals.
70. What is the bond order of CO?
A) 1
B) 2
C) 3
D) 4
Answer: C
Explanation: CO has a bond order of 3, indicating a triple bond.
71. Which of the following molecules is isoelectronic with O2?
A) N2
B) CO
C) F2
D) Ne
Answer: B
Explanation: CO has the same number of electrons as O2, making it isoelectronic.
72. What is the shape of the molecular orbital formed by the overlap of two d orbitals?
A) Spherical
B) Linear
C) Delta (δ)
D) Trigonal planar
Answer: C
Explanation: The overlap of two d orbitals can form delta (δ) bonds, typically found in heavier transition metals.
73. Which of the following statements is true about the σ2p molecular orbital?
A) It is a non-bonding orbital.
B) It is lower in energy than the π2p orbital.
C) It is higher in energy than the π2p orbital.
D) It has no electrons.
Answer: B
Explanation: The σ2p orbital is lower in energy than the π2p orbitals in most cases.
74. What is the primary characteristic of a covalent bond?
A) Transfer of electrons
B) Sharing of electrons
C) Formation of ions
D) Formation of metallic bonds
Answer: B
Explanation: Covalent bonds are characterized by the sharing of electron pairs between atoms.
75. Which of the following has the highest bond dissociation energy?
A) N2
B) O2
C) F2
D) H2
Answer: A
Explanation: N2 has a triple bond, resulting in the highest bond dissociation energy compared to the others.
76. In terms of molecular orbital theory, what does a bond order of 2 indicate?
A) Single bond
B) Double bond
C) Triple bond
D) No bond
Answer: B
Explanation: A bond order of 2 indicates the presence of a double bond between the atoms.
77. What molecular shape is expected for a molecule with sp hybridization?
A) Linear
B) Trigonal planar
C) Tetrahedral
D) Octahedral
Answer: A
Explanation: Molecules with sp hybridization have a linear shape with a bond angle of 180°.
78. Which of the following best describes a non-bonding molecular orbital?
A) Contains a high electron density between nuclei
B) Contributes to bond formation
C) Does not participate in bonding
D) Has a positive energy contribution
Answer: C
Explanation: Non-bonding molecular orbitals do not contribute to bond formation and typically have no net bonding interaction.
79. Which element is commonly known to form pi bonds?
A) Sodium
B) Chlorine
C) Carbon
D) Helium
Answer: C
Explanation: Carbon is well-known for its ability to form pi bonds, particularly in multiple bonds (double and triple).
80. Which molecule exhibits resonance?
A) H2O
B) CO2
C) O3
D) NH3
Answer: C
Explanation: O3 (ozone) exhibits resonance, as it has multiple valid Lewis structures that contribute to its bonding.
81. What is the hybridization of the central atom in a molecule with a trigonal bipyramidal shape?
A) sp
B) sp²
C) sp³d
D) sp³d²
Answer: C
Explanation: The central atom in a trigonal bipyramidal geometry has sp³d hybridization.
82. Which of the following molecules has a bond angle of approximately 120°?
A) CH4
B) NH3
C) BCl3
D) H2O
Answer: C
Explanation: BCl3 has a trigonal planar structure with bond angles of approximately 120°.
83. Which molecular orbital theory describes the energy levels of bonding and antibonding orbitals?
A) Lewis Theory
B) Valence Shell Electron Pair Repulsion Theory
C) Molecular Orbital Theory
D) Crystal Field Theory
Answer: C
Explanation: Molecular Orbital Theory focuses on the energy levels and properties of bonding and antibonding molecular orbitals.
84. Which of the following molecules is expected to be paramagnetic?
A) Ne
B) O2
C) F2
D) He2
Answer: B
Explanation: O2 has unpaired electrons in its molecular orbital configuration, making it paramagnetic.
85. What is the molecular geometry of a molecule with sp³ hybridization?
A) Linear
B) Trigonal planar
C) Tetrahedral
D) Octahedral
Answer: C
Explanation: Molecules with sp³ hybridization adopt a tetrahedral geometry.
86. Which of the following correctly describes the bond order of F2?
A) 1
B) 2
C) 3
D) 4
Answer: A
Explanation: F2 has a bond order of 1, indicating a single bond between the two fluorine atoms.
87. Which of the following statements is true regarding π bonds?
A) They can only be formed by p orbitals.
B) They are stronger than sigma bonds.
C) They can be formed by the overlap of s and p orbitals.
D) They can exist independently of sigma bonds.
Answer: A
Explanation: π bonds are formed by the side-to-side overlap of p orbitals and cannot exist without a sigma bond.
88. Which molecular orbital is represented by the notation π?*
A) Bonding molecular orbital
B) Antibonding molecular orbital
C) Non-bonding molecular orbital
D) Both A and C
Answer: B
Explanation: The π* notation indicates an antibonding molecular orbital formed from p orbitals.
89. What is the bond order of a molecule with 4 bonding electrons and 2 antibonding electrons?
A) 0
B) 1
C) 2
D) 3
Answer: B
Explanation: Bond order = (number of bonding electrons – number of antibonding electrons) / 2 = (4 – 2) / 2 = 1.
90. In which molecular orbital are the electrons responsible for the bond in H2 located?
A) σ1s
B) σ*1s
C) π2p
D) σ2p
Answer: A
Explanation: In H2, the electrons are located in the bonding molecular orbital σ1s, which contributes to the bond formation.
91. Which of the following molecules has a bond angle of approximately 180°?
A) CO2
B) H2O
C) NH3
D) CH4
Answer: A
Explanation: CO2 has a linear molecular geometry with bond angles of approximately 180°.
92. Which of the following has a higher bond energy, N2 or O2?
A) N2
B) O2
C) They have equal bond energy.
D) Cannot be determined
Answer: A
Explanation: N2 has a triple bond, which results in higher bond energy compared to the double bond in O2.
93. What type of bond is formed when two atomic orbitals combine in a head-on manner?
A) Pi bond
B) Sigma bond
C) Delta bond
D) Hydrogen bond
Answer: B
Explanation: Sigma bonds are formed by the head-on overlap of atomic orbitals.
94. Which molecule has the highest bond order?
A) O2
B) N2
C) H2
D) F2
Answer: B
Explanation: N2 has a bond order of 3 (triple bond), which is the highest among the given options.
95. Which molecular orbital results from the combination of two p orbitals?
A) σ2p
B) π2p
C) σ*2p
D) Both A and B
Answer: B
Explanation: π2p molecular orbitals are formed from the lateral overlap of two p orbitals.
96. Which of the following species has a bond order of 0?
A) He2
B) H2
C) Li2
D) N2
Answer: A
Explanation: He2 has no net bonding interaction, resulting in a bond order of 0.
97. Which molecule exhibits hybridization of sp²?
A) BeCl2
B) CH2O
C) C2H4
D) NH3
Answer: C
Explanation: C2H4 (ethylene) exhibits sp² hybridization due to the presence of a double bond.
98. What is the primary reason for the formation of a double bond?
A) Overlap of s orbitals
B) Overlap of p orbitals
C) Both A and B
D) None of the above
Answer: C
Explanation: A double bond is formed by one sigma bond and one pi bond, requiring the overlap of both s and p orbitals.
99. Which molecular orbital diagram shows a transition between bonding and antibonding orbitals?
A) O2
B) N2
C) CO
D) He2
Answer: A
Explanation: O2 shows a transition in the energy levels of bonding and antibonding orbitals due to its unique electronic configuration.
100. Which molecule has a bond order of 3?
A) O2
B) N2
C) F2
D) He2
Answer: B
Explanation: N2 has a bond order of 3, indicating a triple bond between the two nitrogen atoms
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