NEET Chemistry: Bond order Practice Questions
14 free multiple-choice questions on Bond order (Chemical Bonding and Molecular Structure) for NEET Chemistry, each with the correct answer and a step-by-step explanation. Attempt a question, then reveal the solution to check your reasoning.
Practice thousands more NEET questions in the app →Q1. If a molecule has a bond order of 1.5, what type of bond is present between the atoms?
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Correct answer: D — Partial bond
A bond order between 1 and 2 indicates a bond that is intermediate, often described as a partial bond (e.g., in bond order calculations for complex systems).
Q2. Which pair of atoms results in the highest bond order among the following?
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Correct answer: A — N≡N
The triple bond between Nitrogen atoms (N≡N) has a bond order of 3.0, which is the highest among the given options.
Q3. What is the bond order of a single bond between two carbon atoms in methane (CH4)?
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Correct answer: A — 1.0
A single bond consists of one sigma (σ) bond. Therefore, the bond order is 1.0.
Q4. The bond order of a triple bond is:
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Correct answer: C — 3
A triple bond involves three shared electron pairs, resulting in a bond order of 3.
Q5. Which of the following compounds has the highest bond order? (Considering only simple diatomic molecules)
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Correct answer: B — N₂
The bond orders are 1 (H₂), 2 (O₂), 3 (N₂), and 1 (F₂). N₂ has the highest bond order among these common diatomic gases.
Q6. What is the bond order of a sigma (σ) bond?
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Correct answer: C — 1
A single covalent bond involves the sharing of electrons along the internuclear axis, which corresponds to one bond order.
Q7. The bond order for a double bond is always greater than the bond order for a single bond. This is due to:
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Correct answer: D — Greater overlap of atomic orbitals
Double bonds involve the lateral overlap of more atomic orbitals, leading to a greater number of shared electron pairs compared to single bonds.
Q8. The relationship between bond order and bond length is generally inversely proportional. Which statement best describes this relationship?
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Correct answer: A — Higher bond order means shorter bond length
As the number of shared electron pairs (bond order) increases, the attractive force between the nuclei increases, leading to a shorter bond length.
Q9. For a hypothetical molecule where the bond order is 4, what is the expected number of molecular orbitals involved in the bond formation?
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Correct answer: B — Five
A bond order of 4 implies a high degree of electron sharing, typically involving the combination of four atomic orbitals, often arising from sp³d² hybridization or similar scenarios.
Q10. The bond order for a triple bond is:
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Correct answer: D — 3
A triple bond involves the sharing of three pairs of electrons between two atoms, hence the bond order is 3.
Q11. The bond order of the bond in O₂ molecule is:
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Correct answer: C — 1.5
In the O₂ molecule, the bond order is 2.0 (sharing two pairs of electrons).
Q12. In the O₂ molecule, what is the bond order?
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Correct answer: B — 2
The oxygen molecule is formed by a double covalent bond, meaning two pairs of electrons are shared. Therefore, the bond order is 2.
Q13. If a diatomic molecule has a bond order of 2.5, what does this imply about the nature of the bond?
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Correct answer: A — It represents a partial bond
A bond order of 2.5 implies that the bond has significant double-bond character (2.0) and partial triple-bond character (0.5), representing a partial bond.
Q14. The bond order of a double bond is always greater than the bond order of a single bond. Which statement is correct regarding stability?
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Correct answer: A — The double bond is always stronger
A double bond involves more shared electron pairs (one σ and one π bond) compared to a single bond (one σ bond). Therefore, the bond order is higher (1.5 vs 1.0), indicating greater stability.
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