NEET Chemistry: Chemical Bonding and Molecular Structure Practice Questions
15 free multiple-choice questions on 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 Chemical Bonding and Molecular Structure questions in the app →Q1. What is the shape of the molecule of water (H₂O)?
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Correct answer: D — Bent
The central Oxygen atom has two bonding pairs and two lone pairs (four electron domains). According to VSEPR theory, the molecular geometry is bent.
Q2. Which type of anion generally exhibits a high polarizing power and is more likely to cause significant covalent character in the bond?
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Correct answer: B — Highly polarizable anions
Anions that are large and have low charge density are more polarizable and exert a stronger polarizing effect on the cation, leading to increased covalent character in the bond (Fajan's rule).
Q3. Hydrogen bonding is the strongest of the intermolecular forces. Which substance exhibits the strongest intermolecular forces among the following?
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Correct answer: D — Water (H₂O)
Water (H₂O) exhibits hydrogen bonding, which is the strongest intermolecular force, leading to higher boiling points and surface tension compared to the other options which rely primarily on van der Waals forces.
Q4. 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).
Q5. The dipole moment of a molecule is determined by the vector sum of individual bond dipoles. If two identical C-Cl bonds are arranged symmetrically about an axis, what is the resulting net molecular dipole moment?
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Correct answer: B — Zero
Due to the symmetry of the arrangement, the individual bond dipoles cancel each other out vectorially, resulting in a net molecular dipole moment of zero.
Q6. Which factor increases the tendency of a cation to act as a Lewis acid when interacting with an anion according to Fajan's rule?
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Correct answer: B — Increasing the polarizing ability of the anion
The polarizing ability of the anion directly influences the bond character. A higher polarizing ability increases the ability of the anion to withdraw electron density, which is related to the Lewis acidity of the cation.
Q7. In the bond between Oxygen (O) and Hydrogen (H) in the molecule H2O, what type of bond is primarily formed?
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Correct answer: D — Polar covalent
The electronegativity difference (ΔEN) between O (3.44) and H (2.20) is significant (1.24), indicating a polar covalent bond, where the electron density is unequally shared.
Q8. In the formation of an ionic compound, which of the following must be conserved?
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Correct answer: B — Total number of electrons (charge neutrality)
For an ionic bond to form, the overall charge of the resulting compound must be zero, meaning the total number of positive charges (cations) must equal the total number of negative charges (anions).
Q9. Which molecule possesses the most polar covalent bond among the following?
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Correct answer: A — O=O
In O=O, the difference in electronegativity between Oxygen atoms is the largest, resulting in the most polar covalent bond compared to the others listed.
Q10. If the electronegativity difference between two atoms is small, the resulting molecular structure is most likely to exhibit which type of bonding character?
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Correct answer: A — Nonpolar covalent
Small electronegativity differences imply shared electron density that is nearly equal, resulting in a predominantly nonpolar covalent bond character.
Q11. What is the predicted molecular geometry for the PCl₅ molecule based on VSEPR theory?
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Correct answer: A — Trigonal bipyramidal
In PCl₅, the central phosphorus atom has 5 bonding pairs (to Cl atoms) and 0 lone pairs. According to VSEPR theory, the arrangement of these 5 electron domains results in a trigonal bipyramidal molecular geometry.
Q12. When comparing two resonance structures for a species, the structure with the lower energy is identified as the:
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Correct answer: D — Thermodynamically preferred structure
The structure corresponding to the lower energy level is the thermodynamically preferred and most stable resonance contributor.
Q13. 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.
Q14. 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.
Q15. 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.
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