Chemical Bonding MCQs set 3 for Ziauddin University Medical Entry Test Chemistry — 20 solved questions.
Q1. A materials scientist compares the melting points of various ionic solids. Which compound exhibits the highest lattice energy due to greater ionic charges?
Answer: MgO
Explanation: MgO has higher lattice energy due to +2/-2 charges; NaCl is tempting but its +1/-1 charges result in weaker electrostatic attraction.
Q2. During a VSEPR theory demonstration, a student models Ammonia (NH3). What is the observed bond angle resulting from lone pair-bond pair repulsion?
Answer: 107.5 degrees
Explanation: NH3 has 107.5 degrees due to lone pair-bond pair repulsion; CH4 is tempting but its 109.5 degrees is perfectly tetrahedral without lone pairs.
Q3. A laboratory technician measures the polarity of various gases. Despite containing highly polar B-F bonds, which molecule shows a net dipole moment of zero?
Answer: BF3
Explanation: BF3 has zero dipole moment due to its symmetrical trigonal planar geometry; NF3 is tempting but its lone pair prevents symmetry cancellation.
Q4. In a comparative study of halogen hydrides, which substance shows an anomalously high boiling point due to the presence of intermolecular hydrogen bonding?
Answer: HF
Explanation: HF has the highest boiling point due to strong hydrogen bonding; HI is tempting because of its larger mass and London forces.
Q5. A chemist investigates the geometry of water. Which bond angle is expected when two lone pairs exert maximum repulsion on two bond pairs?
Answer: 104.5 degrees
Explanation: The H-O-H angle in water is 104.5 degrees due to two lone pairs; NH3 is tempting but only has one lone pair.
Q6. A researcher measures bond dissociation energies for halogens. Which diatomic molecule shows an abnormally higher bond energy compared to the smaller fluorine molecule?
Answer: Cl2
Explanation: Cl2 has higher bond energy than F2 due to F2's lone pair-lone pair repulsion; F2 is tempting as it is more electronegative.
Q7. An organic chemist analyzes bond lengths in hydrocarbons. Which molecule contains the shortest carbon-carbon bond distance due to high electron density?
Answer: Ethyne
Explanation: Ethyne (C2H2) has the shortest C-C bond because it is a triple bond; Ethene is tempting but contains a longer double bond.
Q8. A physicist uses a magnetic field to test liquid gases. Which diatomic molecule is attracted to the magnet due to its paramagnetic nature?
Answer: O2
Explanation: Oxygen is paramagnetic due to two unpaired electrons in antibonding pi orbitals; Nitrogen is tempting but all its electrons are paired.
Q9. In a reaction between ammonia and a proton, a new bond is formed. What species represents the product containing a coordinate covalent bond?
Answer: NH4+
Explanation: The NH4+ ion forms through a coordinate covalent bond; CH4 is tempting but only involves standard sharing of valence electrons.
Q10. A metallurgist compares the hardness of different metals. Which element exhibits the strongest metallic bonding due to the involvement of (n-1)d electrons?
Answer: Iron
Explanation: Transition metals have strong metallic bonds involving d-electrons; Group IA metals are tempting but have weaker bonds with only one s-electron.
Q11. A student plots the boiling points of Period 2 and 3 hydrides. Which substance shows the highest boiling point due to extensive hydrogen bonding?
Answer: H2O
Explanation: H2O has the highest boiling point because it forms two hydrogen bonds per molecule; HF is tempting but forms only one.
Q12. During a lecture on orbital overlap, a professor discusses bond strengths. Which type of bond is characterized by maximum electron density between nuclei?
Answer: Sigma bond
Explanation: Sigma bonds are stronger than pi bonds because of head-on overlap; Pi bonds are tempting but involve weaker sideway orbital overlap.
Q13. A chemist investigates expanded octets in phosphorus compounds. Which molecule requires sp3d hybridization to explain its five equivalent equatorial and axial bonds?
Answer: PCl5
Explanation: PCl5 involves sp3d hybridization to accommodate five chlorine atoms; PCl3 is tempting but only uses sp3 hybridization for three bonds.
Q14. A student observes the physical states of halogens. Which halogen exists as a solid at room temperature due to exceptionally strong London dispersion forces?
Answer: Iodine
Explanation: Iodine is a solid at room temperature due to its high polarizability and London forces; Chlorine is tempting but is a gas.
Q15. A researcher compares triatomic molecules. Which molecule deviates from a linear shape and adopts an angular geometry due to a lone pair on the central atom?
Answer: SnCl2
Explanation: SnCl2 is V-shaped/angular due to the presence of a lone pair; CO2 is tempting but is perfectly linear with no lone pairs.
Q16. In a Molecular Orbital Theory calculation, a student determines bond orders. Which oxygen species possesses the highest bond order and shortest bond length?
Answer: O2+
Explanation: The bond order of O2+ is 2.5 because an electron is removed from an antibonding orbital; O2 is tempting but has a bond order of 2.
Q17. An analytical chemist measures carbon-carbon distances in various rings. Which molecule shows uniform bond lengths that are intermediate between single and double bonds?
Answer: Benzene
Explanation: Benzene has intermediate C-C bond lengths (1.397 A) due to resonance; Ethane is tempting but has a much longer single bond.
Q18. A biologist notes that aquatic life survives in frozen lakes. Which form of water occupies more volume than the liquid state due to hydrogen bonding?
Answer: Ice
Explanation: Ice has a lower density than water due to an open cage-like structure formed by hydrogen bonds; Liquid water is tempting but is denser.
Q19. A student calculates the percentage of ionic character in various salts. Which pair of elements forms the most purely ionic bond in the periodic table?
Answer: CsF
Explanation: The bond between Cesium and Fluorine is the most ionic due to the largest electronegativity difference; LiF is tempting but has a smaller difference.
Q20. During a study of the octet rule, a student identifies exceptions. Which molecule contains a central atom that is stable with fewer than eight valence electrons?
Answer: BCl3
Explanation: BCl3 is an electron-deficient molecule with only 6 electrons in its valence shell; PCl3 is tempting but follows the octet rule.
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