JEE Chemistry Chemical Bonding and Molecular Structure MCQs Set 29

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

View or download the dedicated Chemical Bonding and Molecular Structure MCQ resource below. Practicing these 50 objective questions regularly builds familiarity with standard exam patterns and helps secure higher marks in final Chemistry evaluations.

Multiple Choice Questions

Question 1: Amphoteric behaviour is shown by the oxides of
(a) Al and Ca
(b) Pb and Ba
(c) Cr and Mg
(d) Sn and Zn
Show Answer & Explanation

Answer: (d) Sn and Zn

Explanation:
1. SnO and ZnO are amphoteric
2. CaO, BaO and MgO are basic.

Teacher's Note:
1. Net polarity needs both polar bonds and an asymmetric shape; for ionic versus covalent character apply Fajans' rules (small, highly charged cation, large anion means more covalent).

Question 2: Which of the following oxides is neutral?
(a) \( \ce{SnO2} \)
(b) CO
(c) ZnO
(d) \( \ce{SiO2} \)
Show Answer & Explanation

Answer: (b) CO

Explanation:
1. CO does not react with acids or bases; \( \ce{SnO2} \) and ZnO are amphoteric and \( \ce{SiO2} \) is acidic.
2. Only option (b) agrees with this working.

Teacher's Note:
1. Net polarity needs both polar bonds and an asymmetric shape; for ionic versus covalent character apply Fajans' rules (small, highly charged cation, large anion means more covalent).

Question 3: Which of the following is polar and has an sp3 central atom?
(a) \( \ce{SiF4} \)
(b) \( \ce{HClO2} \)
(c) \( \ce{BF3} \)
(d) \( \ce{H2CO3} \)
Show Answer & Explanation

Answer: (b) \( \ce{HClO2} \)

Explanation:
1. In \( \ce{HClO2} \) Cl has 4 pairs (sp3) and the molecule is bent and polar
2. \( \ce{SiF4} \) is non-polar and \( \ce{BF3} \) is sp2. In \( \ce{H2CO3} \) the central C is sp2.

Teacher's Note:
1. Net polarity needs both polar bonds and an asymmetric shape; for ionic versus covalent character apply Fajans' rules (small, highly charged cation, large anion means more covalent).

Question 4: Which of the following is polar?
(a) \( \ce{XeF4} \)
(b) \( \ce{SO3} \)
(c) \( \ce{ICl4-} \)
(d) \( \ce{XeOF4} \)
Show Answer & Explanation

Answer: (d) \( \ce{XeOF4} \)

Explanation:
1. \( \ce{XeOF4} \) is square pyramidal with a lone pair, so it is polar
2. The other three are symmetric.

Teacher's Note:
1. Net polarity needs both polar bonds and an asymmetric shape; for ionic versus covalent character apply Fajans' rules (small, highly charged cation, large anion means more covalent).

Question 5: Which of the following is expected to have a zero dipole moment on the basis of symmetry?
(a) \( \ce{SOCl2} \)
(b) \( \ce{OF2} \)
(c) \( \ce{SeF6} \)
(d) \( \ce{ClF5} \)
Show Answer & Explanation

Answer: (c) \( \ce{SeF6} \)

Explanation:
1. \( \ce{SeF6} \) is octahedral and symmetrical
2. \( \ce{SOCl2} \) and \( \ce{OF2} \) are bent/pyramidal; \( \ce{ClF5} \) is square pyramidal.

Teacher's Note:
1. Net polarity needs both polar bonds and an asymmetric shape; for ionic versus covalent character apply Fajans' rules (small, highly charged cation, large anion means more covalent).

Question 6: If a molecule \( \ce{MX3} \) has zero dipole moment and M has atomic number below 21, the hybrid orbitals of M are
(a) pure p
(b) sp
(c) sp2
(d) sp3
Show Answer & Explanation

Answer: (c) sp2

Explanation:
1. A non-polar \( \ce{MX3} \) is trigonal planar (like \( \ce{BF3} \)) and uses sp2 hybrid orbitals.
2. Only option (c) agrees with this working.

Teacher's Note:
1. Net polarity needs both polar bonds and an asymmetric shape; for ionic versus covalent character apply Fajans' rules (small, highly charged cation, large anion means more covalent).

Question 7: Which of these statements about dipole moment is NOT correct?
(a) \( \ce{PF5} \) has a non-zero dipole moment
(b) Dipole moment is a vector quantity
(c) A lone pair on the central atom can lead to a dipole moment
(d) Electronegativity difference can lead to a dipole moment
Show Answer & Explanation

Answer: (a) \( \ce{PF5} \) has a non-zero dipole moment

Explanation:
1. \( \ce{PF5} \) is trigonal bipyramidal and symmetrical, so its dipole moment is zero.
2. Only option (a) agrees with this working.

Teacher's Note:
1. Net polarity needs both polar bonds and an asymmetric shape; for ionic versus covalent character apply Fajans' rules (small, highly charged cation, large anion means more covalent).

Question 8: Which of the following has the minimum melting point?
(a) CsF
(b) HF
(c) LiF
(d) HCl
Show Answer & Explanation

Answer: (d) HCl

Explanation:
1. HCl is a molecular compound with weak dipole forces; the others are ionic or strongly hydrogen bonded.
2. Only option (d) agrees with this working.

Teacher's Note:
1. Net polarity needs both polar bonds and an asymmetric shape; for ionic versus covalent character apply Fajans' rules (small, highly charged cation, large anion means more covalent).

Question 9: The correct order of increasing ionic character is
(a) \( \ce{BeCl2} \) < \( \ce{MgCl2} \) < \( \ce{BaCl2} \) < \( \ce{CaCl2} \)
(b) \( \ce{BeCl2} \) < \( \ce{MgCl2} \) < \( \ce{CaCl2} \) < \( \ce{BaCl2} \)
(c) \( \ce{BeCl2} \) < \( \ce{BaCl2} \) < \( \ce{MgCl2} \) < \( \ce{CaCl2} \)
(d) \( \ce{BaCl2} \) < \( \ce{MgCl2} \) < \( \ce{CaCl2} \) < \( \ce{BeCl2} \)
Show Answer & Explanation

Answer: (b) \( \ce{BeCl2} \) < \( \ce{MgCl2} \) < \( \ce{CaCl2} \) < \( \ce{BaCl2} \)

Explanation:
1. Cation size increases down the group, polarising power falls and ionic character rises.
2. Only option (b) agrees with this working.

Teacher's Note:
1. Net polarity needs both polar bonds and an asymmetric shape; for ionic versus covalent character apply Fajans' rules (small, highly charged cation, large anion means more covalent).

Question 10: The compound with the least melting point is
(a) \( \ce{PbCl2} \)
(b) \( \ce{NaCl} \)
(c) \( \ce{AlCl3} \)
(d) \( \ce{SnCl4} \)
Show Answer & Explanation

Answer: (d) \( \ce{SnCl4} \)

Explanation:
1. \( \ce{SnCl4} \) is a covalent molecular liquid (m.p. about -33 degrees C); the others are solids.
2. Only option (d) agrees with this working.

Teacher's Note:
1. Net polarity needs both polar bonds and an asymmetric shape; for ionic versus covalent character apply Fajans' rules (small, highly charged cation, large anion means more covalent).

Question 11: The percentage ionic character of LiF (observed dipole moment 6.32 D, bond length 156 pm; 1 D = \(3.336\times10^\( \ce{-30} \)\) C m) is nearest to
(a) 84%
(b) 63%
(c) 42%
(d) 100%
Show Answer & Explanation

Answer: (a) 84%

Explanation:
1. Ionic moment \(= ed = 1.602\times10^\( \ce{-19} \)\times156\times10^\( \ce{-12} \) = 2.50\times10^\( \ce{-29} \)\) C m \(= 7.49\) D. % ionic \(= 6.32/7.49\times100 = 84\%\).
2. Only option (a) agrees with this working.

Teacher's Note:
1. Net polarity needs both polar bonds and an asymmetric shape; for ionic versus covalent character apply Fajans' rules (small, highly charged cation, large anion means more covalent).

Question 12: The correct order of increasing dipole moment is
(a) \( \ce{H2O} \) < \( \ce{H2S} \) < \( \ce{BF3} \)
(b) \( \ce{H2S} \) < \( \ce{BF3} \) < \( \ce{H2O} \)
(c) \( \ce{BF3} \) < \( \ce{H2S} \) < \( \ce{H2O} \)
(d) \( \ce{BF3} \) < \( \ce{H2O} \) < \( \ce{H2S} \)
Show Answer & Explanation

Answer: (c) \( \ce{BF3} \) < \( \ce{H2S} \) < \( \ce{H2O} \)

Explanation:
1. \( \ce{BF3} \) is symmetrical (zero), \( \ce{H2S} \) is 0.97 D and \( \ce{H2O} \) is 1.85 D.
2. Only option (c) agrees with this working.

Teacher's Note:
1. Net polarity needs both polar bonds and an asymmetric shape; for ionic versus covalent character apply Fajans' rules (small, highly charged cation, large anion means more covalent).

Question 13: The increasing order of acidic character of \( \ce{CO2} \), \( \ce{N2O5} \), \( \ce{SiO2} \) and \( \ce{SO3} \) is
(a) \( \ce{CO2} \) < \( \ce{SiO2} \) < \( \ce{SO3} \) < \( \ce{N2O5} \)
(b) \( \ce{N2O5} \) < \( \ce{SO3} \) < \( \ce{CO2} \) < \( \ce{SiO2} \)
(c) \( \ce{SiO2} \) < \( \ce{CO2} \) < \( \ce{SO3} \) < \( \ce{N2O5} \)
(d) \( \ce{SiO2} \) < \( \ce{CO2} \) < \( \ce{N2O5} \) < \( \ce{SO3} \)
Show Answer & Explanation

Answer: (c) \( \ce{SiO2} \) < \( \ce{CO2} \) < \( \ce{SO3} \) < \( \ce{N2O5} \)

Explanation:
1. Acidity rises with the oxidation state and electronegativity of the non-metal: Si < C < S < N.
2. Only option (c) agrees with this working.

Teacher's Note:
1. Net polarity needs both polar bonds and an asymmetric shape; for ionic versus covalent character apply Fajans' rules (small, highly charged cation, large anion means more covalent).

Question 14: Which molecule has a non-zero dipole moment: \( \ce{XeF2} \), \( \ce{ClF3} \), \( \ce{XeO2F4} \) (trans isomer) or \( \ce{XeF4} \)?
(a) \( \ce{XeF2} \)
(b) \( \ce{XeF4} \)
(c) \( \ce{XeO2F4} \)
(d) \( \ce{ClF3} \)
Show Answer & Explanation

Answer: (d) \( \ce{ClF3} \)

Explanation:
1. \( \ce{ClF3} \) is T-shaped with two lone pairs, so it is polar
2. \( \ce{XeF2} \) and \( \ce{XeF4} \) are symmetric; \( \ce{XeO2F4} \) with trans oxygens is non-polar.

Teacher's Note:
1. Net polarity needs both polar bonds and an asymmetric shape; for ionic versus covalent character apply Fajans' rules (small, highly charged cation, large anion means more covalent).

Question 15: The dipole moment of a triatomic molecule AX\(_2\) equals the dipole moment of one A-X bond. The X-A-X angle is
(a) linear (180 degrees)
(b) 120 degrees
(c) 90 degrees
(d) cannot be predicted
Show Answer & Explanation

Answer: (b) 120 degrees

Explanation:
1. For two equal bond moments m at angle theta, the resultant is \(2m\cos(\theta/2)\)
2. Setting this equal to m gives \(\cos(\theta/2) = 1/2\), so theta = 120 degrees.

Teacher's Note:
1. Net polarity needs both polar bonds and an asymmetric shape; for ionic versus covalent character apply Fajans' rules (small, highly charged cation, large anion means more covalent).

Question 16: Which inter-halogen compound is non-polar?
(a) \( \ce{ClF3} \)
(b) \( \ce{IF7} \)
(c) \( \ce{BrF5} \)
(d) BrCl
Show Answer & Explanation

Answer: (b) \( \ce{IF7} \)

Explanation:
1. \( \ce{IF7} \) is pentagonal bipyramidal and symmetrical
2. \( \ce{ClF3} \) is T-shaped, \( \ce{BrF5} \) square pyramidal and BrCl a heteronuclear diatomic: all polar.

Teacher's Note:
1. Net polarity needs both polar bonds and an asymmetric shape; for ionic versus covalent character apply Fajans' rules (small, highly charged cation, large anion means more covalent).

Question 17: The most covalent of \( \ce{NaCl} \), \( \ce{Na2S} \), \( \ce{MgCl2} \) and \( \ce{MgS} \) is
(a) \( \ce{NaCl} \)
(b) \( \ce{Na2S} \)
(c) \( \ce{MgCl2} \)
(d) \( \ce{MgS} \)
Show Answer & Explanation

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

Explanation:
1. The small, doubly charged \( \ce{Mg^2+} \) polarises a large, doubly charged, highly polarisable \( \ce{S^2-} \) the most.
2. Only option (d) agrees with this working.

Teacher's Note:
1. Net polarity needs both polar bonds and an asymmetric shape; for ionic versus covalent character apply Fajans' rules (small, highly charged cation, large anion means more covalent).

Question 18: Which of the following statements are correct about halogen compounds XX\(^\prime_n\): XX' linear polar; XX'\(_3\) T-shaped polar; XX'\(_5\) square pyramidal polar; XX'\(_7\) pentagonal bipyramidal non-polar?
(a) Only the first two
(b) Only the last two
(c) All four are correct
(d) Only the first and the last
Show Answer & Explanation

Answer: (c) All four are correct

Explanation:
1. XX' is a heteronuclear diatomic (polar), XX'3 is T-shaped (polar), XX'5 is square pyramidal (polar) and XX'7 is pentagonal bipyramidal and symmetrical (non-polar).
2. Only option (c) agrees with this working.

Teacher's Note:
1. Net polarity needs both polar bonds and an asymmetric shape; for ionic versus covalent character apply Fajans' rules (small, highly charged cation, large anion means more covalent).

Question 19: Which statements about dipole moment are correct? (I) A lone pair on the central atom can cause it; (II) it is a vector; (III) \( \ce{CO2} \) has a dipole moment; (IV) an electronegativity difference can cause it.
(a) I and II only
(b) II, III and IV only
(c) I, II and IV only
(d) All four
Show Answer & Explanation

Answer: (c) I, II and IV only

Explanation:
1. \( \ce{CO2} \) is linear and symmetrical, so its dipole moment is zero; statement III is false.
2. Only option (c) agrees with this working.

Teacher's Note:
1. Net polarity needs both polar bonds and an asymmetric shape; for ionic versus covalent character apply Fajans' rules (small, highly charged cation, large anion means more covalent).

Question 20: Which of the following are polar: \( \ce{XeF4} \), \( \ce{XeF6} \), \( \ce{XeOF4} \) and \( \ce{XeF5-} \)?
(a) \( \ce{XeF6} \) and \( \ce{XeOF4} \)
(b) \( \ce{XeF4} \) and \( \ce{XeF5-} \)
(c) \( \ce{XeF4} \) and \( \ce{XeOF4} \)
(d) \( \ce{XeF6} \) and \( \ce{XeF5-} \)
Show Answer & Explanation

Answer: (a) \( \ce{XeF6} \) and \( \ce{XeOF4} \)

Explanation:
1. \( \ce{XeF4} \) is square planar and \( \ce{XeF5-} \) is pentagonal planar, both non-polar
2. \( \ce{XeF6} \) (distorted octahedral) and \( \ce{XeOF4} \) (square pyramidal) have a lone pair that makes them polar.

Teacher's Note:
1. Net polarity needs both polar bonds and an asymmetric shape; for ionic versus covalent character apply Fajans' rules (small, highly charged cation, large anion means more covalent).

Question 21: Which factors do NOT favour the formation of an ionic bond?
(a) Low charge on ions
(b) A large cation and a small anion
(c) High lattice energy
(d) High charge on ions and a small cation with a large anion
Show Answer & Explanation

Answer: (d) High charge on ions and a small cation with a large anion

Explanation:
1. Ionic bonds are favoured by low charges, a large cation with a small anion and high lattice energy
2. High charges and a small cation with a large anion raise polarisation and covalent character.

Teacher's Note:
1. Net polarity needs both polar bonds and an asymmetric shape; for ionic versus covalent character apply Fajans' rules (small, highly charged cation, large anion means more covalent).

Question 22: The number of acidic oxides among \( \ce{Mn2O7} \), \( \ce{SO2} \), CO, \( \ce{N2O} \), \( \ce{NO2} \), \( \ce{PbO2} \), \( \ce{Na2O} \), \( \ce{CrO3} \), ZnO, \( \ce{Fe2O3} \), \( \ce{SiO2} \) and SnO is
(a) 4
(b) 5
(c) 6
(d) 7
Show Answer & Explanation

Answer: (b) 5

Explanation:
1. The acidic oxides are \( \ce{Mn2O7} \), \( \ce{SO2} \), \( \ce{NO2} \), \( \ce{CrO3} \) and \( \ce{SiO2} \)
2. CO and \( \ce{N2O} \) are neutral; \( \ce{PbO2} \), ZnO, SnO and (weakly) \( \ce{Fe2O3} \) are amphoteric; \( \ce{Na2O} \) is basic.

Teacher's Note:
1. Net polarity needs both polar bonds and an asymmetric shape; for ionic versus covalent character apply Fajans' rules (small, highly charged cation, large anion means more covalent).

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

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