JEE Chemistry Chemical Bonding and Molecular Structure MCQs Set 06

Chemistry Objective Questions and Answers: Chemical Bonding and Molecular Structure

Access targeted multiple-choice questions for Chemical Bonding and Molecular Structure designed to align with the latest JEE academic syllabus for JEE Chemistry. These objective practice sets help students evaluate their conceptual understanding and improve exam readiness.

Download Chemical Bonding and Molecular Structure MCQs with Answers

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Multiple Choice Questions

Question 1: A dative bond is present in
(a) \( \ce{SO3} \)
(b) \( \ce{NH3} \)
(c) \( \ce{K2CO3} \)
(d) \( \ce{BF3} \)
Show Answer & Explanation

Answer: (a) \( \ce{SO3} \)

Explanation:
1. SO3 has an S -> O coordinate bond in its Lewis structure.

Teacher's Note:
1. NH3 and BF3 have normal covalent bonds.

Question 2: The compound containing a coordinate bond is
(a) \( \ce{H2SO4} \)
(b) \( \ce{O3} \)
(c) \( \ce{SO3} \)
(d) All of these
Show Answer & Explanation

Answer: (d) All of these

Explanation:
1. All three contain coordinate (dative) bonds in the Lewis structure.

Teacher's Note:
1. H2SO4 has S -> O bonds, O3 has an O -> O bond.

Question 3: In dry ice, the bond present between two molecules is
(a) Ionic
(b) Covalent
(c) Hydrogen bond
(d) Van der Waals
Show Answer & Explanation

Answer: (d) Van der Waals

Explanation:
1. Solid CO2 is a molecular solid held by weak van der Waals forces (London).

Teacher's Note:
1. CO2 is non-polar.

Question 4: Intermolecular hydrogen bonds are NOT present in
(a) \( \ce{CH3CH2OH} \)
(b) \( \ce{CH3COOH} \)
(c) \( \ce{C2H5NH2} \)
(d) \( \ce{CH3OCH3} \)
Show Answer & Explanation

Answer: (d) \( \ce{CH3OCH3} \)

Explanation:
1. Ethers have no H attached to O, so they cannot form intermolecular H bonds with each other.

Teacher's Note:
1. H on N, O or F is required.

Question 5: The correct order of volatility is
(a) HF > HCl > HBr > HI
(b) HCl > HBr > HI > HF
(c) HI > HBr > HCl > HF
(d) HBr < HCl < HI < HF
Show Answer & Explanation

Answer: (b) HCl > HBr > HI > HF

Explanation:
1. Boiling points: HCl 188 K, HBr 207 K, HI 237 K, HF 293 K. The higher the BP, the lower the volatility.

Teacher's Note:
1. HF has H bonding.

Question 6: The incorrect order of decreasing boiling points is
(a) \( \ce{NH3} \) > \( \ce{AsH3} \) > \( \ce{PH3} \)
(b) \( \ce{H2O} \) > \( \ce{H2Se} \) > \( \ce{H2S} \)
(c) \( \ce{Br2} \) > \( \ce{Cl2} \) > \( \ce{F2} \)
(d) \( \ce{CH4} \) > \( \ce{GeH4} \) > \( \ce{SiH4} \)
Show Answer & Explanation

Answer: (d) \( \ce{CH4} \) > \( \ce{GeH4} \) > \( \ce{SiH4} \)

Explanation:
1. The BPs of group 14 hydrides rise with molecular mass: GeH4 > SiH4 > CH4.
2. The other three orders are right.

Teacher's Note:
1. Without H bonding, boiling point follows size.

Question 7: Acetic acid exists as a dimer in benzene due to
(a) Condensation reaction
(b) Hydrogen bonding
(c) Presence of a carboxyl group
(d) None of the above
Show Answer & Explanation

Answer: (b) Hydrogen bonding

Explanation:
1. Two molecules are linked through two O-H...O hydrogen bonds.

Teacher's Note:
1. In water it forms H bonds with the solvent instead.

Question 8: The maximum number of hydrogen bonds formed by a water molecule in ice is
(a) 4
(b) 3
(c) 2
(d) 1
Show Answer & Explanation

Answer: (a) 4

Explanation:
1. Each water molecule is tetrahedrally bonded by 2 H bonds as donor and 2 as acceptor.

Teacher's Note:
1. This gives the open cage structure of ice.

Question 9: The strongest hydrogen bond is shown by
(a) Water
(b) Ammonia
(c) Hydrogen fluoride
(d) Hydrogen sulphide
Show Answer & Explanation

Answer: (c) Hydrogen fluoride

Explanation:
1. F is the most electronegative and smallest, so H-F...H is the strongest hydrogen bond.

Teacher's Note:
1. Strength order: F-H...F > O-H...O > N-H...N.

Question 10: \( \ce{NH3} \) has an abnormally high boiling point because it has
(a) Alkaline nature
(b) Distorted shape
(c) sp3 hybridisation
(d) Hydrogen bonding
Show Answer & Explanation

Answer: (d) Hydrogen bonding

Explanation:
1. Intermolecular N-H...N hydrogen bonds raise the boiling point.

Teacher's Note:
1. Compare with PH3.

Question 11: Which of the following is soluble in water?
(a) \( \ce{CS2} \)
(b) \( \ce{C2H5OH} \)
(c) \( \ce{CCl4} \)
(d) \( \ce{CHCl3} \)
Show Answer & Explanation

Answer: (b) \( \ce{C2H5OH} \)

Explanation:
1. Ethanol forms hydrogen bonds with water.

Teacher's Note:
1. Non-polar liquids do not dissolve.

Question 12: KF combines with HF to form \( \ce{KHF2} \). The compound contains the species
(a) \( \ce{K+} \), \( \ce{F^-} \) and \( \ce{H+} \)
(b) \( \ce{K+} \), \( \ce{F^-} \) and HF
(c) \( \ce{K+} \) and \( \ce{HF2^-} \)
(d) \( \ce{KHF} \)+ and \( \ce{F2} \)
Show Answer & Explanation

Answer: (c) \( \ce{K+} \) and \( \ce{HF2^-} \)

Explanation:
1. The anion is the bifluoride \( \ce{HF2^-} \) (F-H...F-), held by a strong H bond.

Teacher's Note:
1. KHF2 is an ionic compound with a hydrogen-bonded anion.

Question 13: Which is the correct statement about the solubility of \( \ce{MgSO4} \) in water?
(a) Hydration energy of \( \ce{MgSO4} \) is higher than its lattice energy
(b) The ionic potential of \( \ce{Mg^2+} \) is very low
(c) \( \ce{SO4^2-} \) ion mainly contributes to hydration energy
(d) The size of \( \ce{Mg^2+} \) and \( \ce{SO4^2-} \) are similar
Show Answer & Explanation

Answer: (a) Hydration energy of \( \ce{MgSO4} \) is higher than its lattice energy

Explanation:
1. A compound dissolves when the hydration energy exceeds the lattice energy; for MgSO4 this is so because Mg2+ is small.

Teacher's Note:
1. Group 2 sulphate solubility falls as hydration energy falls down the group.

Question 14: The capacity of a solvent to neutralise the charge on ionic compounds is called
(a) Solvation energy
(b) Dielectric constant
(c) Dipole moment
(d) Solubility
Show Answer & Explanation

Answer: (b) Dielectric constant

Explanation:
1. A high dielectric constant reduces the force between ions and dissolves them.

Teacher's Note:
1. Water has a dielectric constant of about 80.

Question 15: The force responsible for dissolution of an ionic compound in water is
(a) Dipole-dipole forces
(b) Ion-dipole forces
(c) Ion-ion force
(d) Hydrogen bond
Show Answer & Explanation

Answer: (b) Ion-dipole forces

Explanation:
1. Water dipoles surround the ions: ion-dipole attraction.

Teacher's Note:
1. Hydration energy comes from these interactions.

Question 16: The Born-Haber cycle is mainly used to determine
(a) Lattice energy
(b) Electron affinity
(c) Ionisation energy
(d) Electronegativity
Show Answer & Explanation

Answer: (a) Lattice energy

Explanation:
1. Lattice energy cannot be measured directly; it is obtained from the Born-Haber cycle.

Teacher's Note:
1. The cycle uses Hess's law.

Question 17: The pair of elements which on combination are most likely to form an ionic compound is
(a) Na and Ca
(b) K and O
(c) O and Cl
(d) Al and I
Show Answer & Explanation

Answer: (b) K and O

Explanation:
1. K (strongly electropositive) and O (strongly electronegative) form K2O.
2. Na and Ca are both metals; O and Cl are both non-metals; AlI3 is largely covalent.

Teacher's Note:
1. Greater EN difference means more ionic.

Question 18: The highest melting point would be of
(a) \( \ce{AlCl3} \)
(b) LiCl
(c) NaCl
(d) \( \ce{BeCl2} \)
Show Answer & Explanation

Answer: (c) NaCl

Explanation:
1. NaCl is the most ionic of these (large cation, charge 1), with a strong lattice (m.p. 801 C). AlCl3 and BeCl2 are covalent; LiCl is partly covalent.

Teacher's Note:
1. Covalent character lowers the melting point.

Question 19: Which substance will have the highest boiling point?
(a) He
(b) CsF
(c) \( \ce{NH3} \)
(d) \( \ce{CHCl3} \)
Show Answer & Explanation

Answer: (b) CsF

Explanation:
1. CsF is an ionic solid with a very strong lattice. He is monatomic, NH3 and CHCl3 are molecular.

Teacher's Note:
1. Ionic substances have high boiling points.

Question 20: As compared to covalent compounds, electrovalent compounds generally possess
(a) High m.p. and high b.p.
(b) Low m.p. and low b.p.
(c) Low m.p. and high b.p.
(d) High m.p. and low b.p.
Show Answer & Explanation

Answer: (a) High m.p. and high b.p.

Explanation:
1. Strong electrostatic forces in the lattice need a lot of energy.

Teacher's Note:
1. Ionic solids are hard and brittle.

Question 21: For two ionic solids CaO and KI, identify the wrong statement
(a) Lattice energy of CaO is much larger than that of KI
(b) KI is soluble in benzene
(c) CaO has a higher melting point
(d) KI has a lower melting point
Show Answer & Explanation

Answer: (b) KI is soluble in benzene

Explanation:
1. KI is ionic and insoluble in benzene (non-polar). The other statements are correct.

Teacher's Note:
1. Ionic compounds dissolve in polar solvents.

Question 22: Which of the following does NOT show electrical conduction?
(a) Diamond
(b) Graphite
(c) Sodium chloride (fused)
(d) Potassium
Show Answer & Explanation

Answer: (a) Diamond

Explanation:
1. Diamond has all four valence electrons in localised bonds; graphite has delocalised electrons.

Teacher's Note:
1. Molten NaCl conducts through ions.

Question 23: The most covalent halide is
(a) \( \ce{AlF3} \)
(b) \( \ce{AlCl3} \)
(c) \( \ce{AlBr3} \)
(d) \( \ce{AlI3} \)
Show Answer & Explanation

Answer: (d) \( \ce{AlI3} \)

Explanation:
1. The large, easily polarised I- ion gives the highest covalent character (Fajans' rules).

Teacher's Note:
1. Covalent character: AlF3 < AlCl3 < AlBr3 < AlI3.

Question 24: The ionic potential (charge / radius) of an electropositive element will be highest in which compound?
(a) CsCl
(b) \( \ce{MgCl2} \)
(c) \( \ce{AlF3} \)
(d) \( \ce{SF6} \)
Show Answer & Explanation

Answer: (c) \( \ce{AlF3} \)

Explanation:
1. Al3+ has the highest charge and a small radius, so the highest ionic potential.

Teacher's Note:
1. Higher ionic potential means more polarising power.

Question 25: The most stable carbonate is
(a) \( \ce{Li2CO3} \)
(b) \( \ce{BeCO3} \)
(c) \( \ce{CaCO3} \)
(d) \( \ce{BaCO3} \)
Show Answer & Explanation

Answer: (d) \( \ce{BaCO3} \)

Explanation:
1. Thermal stability of carbonates increases down group 2 (less polarising cations).

Teacher's Note:
1. BeCO3 is the least stable.

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Multiple Choice Questions (MCQs) for JEE Chemistry Chemical Bonding and Molecular Structure

JEE Chemistry Chemical Bonding and Molecular Structure Objective Test Questions

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