NEET Chemistry: Valence bond theory Practice Questions
15 free multiple-choice questions on Valence bond theory (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. Which hybridization state is associated with a tetrahedral geometry in molecules like methane (CH4)?
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Correct answer: C — sp3
The sp3 hybridization results in four equivalent bond directions and a tetrahedral geometry, which is characteristic of the central atom in methane.
Q2. What is the primary consequence of the overlap of p-orbitals in forming a π bond?
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Correct answer: B — Formation of delocalized electron density above and below the internuclear axis
π bonds arise from the side-by-side overlap of p-orbitals, resulting in electron density residing in the regions perpendicular to the internuclear axis.
Q3. The existence of a bond implies that the atomic orbitals involved must possess:
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Correct answer: D — Appropriate spatial and energy compatibility
For effective bonding in VBT, the orbitals must have compatible spatial orientation and energy levels to allow for significant electron sharing.
Q4. The concept of electron domains in VBT is primarily used to predict which feature of the molecule?
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Correct answer: D — Molecular geometry
Electron domain theory (VSEPR, derived from VBT) is used to predict the three-dimensional shape (molecular geometry) around the central atom.
Q5. In the formation of a double bond, the bond involves the side-by-side overlap of which types of orbitals?
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Correct answer: B — p and p
Double bonds are formed by the side-by-side overlap of p orbitals, leading to pi (π) bond formation alongside the sigma (σ) bond.
Q6. The fundamental basis of Valence Bond Theory is based on the concept that electrons reside in:
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Correct answer: C — Orbitals that are localized in the region between the nuclei
VBT views the molecular structure as resulting from the combination and overlap of atomic orbitals (which form molecular orbitals), focusing on localized electron density between nuclei.
Q7. The existence of a molecular orbital is a direct consequence of the interaction between atomic orbitals. Which pair of orbitals is typically involved in the formation of a sigma bond?
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Correct answer: C — s and p
Sigma (σ) bond formation involves the end-on, head-on overlap of orbitals, typically involving s-s or s-p interactions, leading to a cylindrical overlap.
Q8. In Valence Bond Theory (VBT), the formation of a covalent bond primarily involves the overlap of which atomic orbitals?
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Correct answer: C — s-p overlap
Covalent bond formation occurs through the sideways overlap of atomic orbitals. For σ bonding, end-to-end overlap (like s-s or s-p) is involved, while π bonding involves side-by-side overlap (like p-p).
Q9. The primary cause of molecular shape deviation from ideal geometry in VBT is:
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Correct answer: A — Repulsion between electron pairs
Molecular shape and bond angles are determined by the repulsion between all bonding and lone pairs (VSEPR concept), which affects the electron domain geometry.
Q10. Which of the following types of covalent bonds are formed by the head-on (end-to-end) overlap of atomic orbitals?
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Correct answer: D — Sigma (σ) bond
Sigma (σ) bonds are formed by the direct, end-to-end (head-on) overlap of atomic orbitals, resulting in a cylindrical electron density region along the internuclear axis.
Q11. Which type of hybridization results in a trigonal planar geometry?
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Correct answer: B — sp²
sp² hybridization results in three approximately equal bond angles of 120°, leading to a trigonal planar geometry.
Q12. In Valence Bond Theory (VBT), the geometry of a molecule is primarily determined by the arrangement of:
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Correct answer: D — the electron domains (bonding and lone pairs)
Molecular geometry in VBT is determined by the repulsion between all electron domains (both bonding pairs and lone pairs) around the central atom, which dictates the spatial arrangement.
Q13. In a VSEPR arrangement, the bond angle in a perfectly tetrahedral structure is approximately:
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Correct answer: A — 109.5°
The ideal bond angle for a perfectly symmetrical tetrahedral arrangement, as described by VBT principles, is 109.5 degrees.
Q14. What is the hybridization of the central atom in methane (CH₄)?
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Correct answer: D — sp3
Methane has four sigma bonds formed by the central carbon atom, requiring four equivalent hybrid orbitals, which corresponds to sp³ hybridization.
Q15. Which hybridization is associated with the formation of tetrahedral geometry in molecules like Methane (CH4)?
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Correct answer: B — sp3
Methane has four sigma bonds and four lone pairs, resulting in sp³ hybridization and a tetrahedral geometry.
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