JEE Chemistry Chemical Bonding And Molecular Structure MCQs Set 23

Chemistry Objective Questions and Answers: Chemical Bonding and Molecular Structure

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Multiple Choice Questions

Question 1: Which of the following species has a tetrahedral geometry?
(a) BH4−
(b) NH2−
(c) CO32−
(d) H3O+
Show Answer & Explanation

Answer: (a) BH4−

Explanation:
1. BH4− has four bond pairs on boron and no lone pair (sp³), so it is tetrahedral.
2. NH2− is bent, CO32− is trigonal planar and H3O+ is pyramidal.

Teacher's Note:
1. Convert every quantity to moles or equivalents first.
2. Then apply the stoichiometric ratio or the definition asked for.

Question 2: Which of the following has a square planar structure?
(a) NH4+
(b) BF4−
(c) XeF4
(d) SCl4
Show Answer & Explanation

Answer: (c) XeF4

Explanation:
1. NH4+ and BF4− are tetrahedral and SCl4 is see-saw.
2. XeF4, with two lone pairs, is square planar.

Teacher's Note:
1. Eliminate options that disagree with the basic definition.
2. Confirm the remaining option by a quick calculation.

Question 3: The shapes of SF4, CF4 and XeF4 are
(a) The same, with 2, 0 and 1 lone pairs of electrons on the central atom respectively
(b) The same, with 1, 1 and 1 lone pairs respectively
(c) Different, with 0, 1 and 2 lone pairs respectively
(d) Different, with 1, 0 and 2 lone pairs respectively
Show Answer & Explanation

Answer: (d) Different, with 1, 0 and 2 lone pairs respectively

Explanation:
1. SF4: 4 bond pairs + 1 lone pair, see-saw. CF4: 4 bond pairs + 0 lone pairs, tetrahedral. XeF4: 4 bond pairs + 2 lone pairs, square planar.
2. The shapes are different, with 1, 0 and 2 lone pairs respectively.

Teacher's Note:
1. Read the data carefully and write the relevant formula before substituting.
2. Check units and the order of magnitude of the answer.

Question 4: The geometry of the sulphate ion SO42− is
(a) Square planar
(b) Tetrahedral
(c) Trigonal bipyramidal
(d) Hexagonal
Show Answer & Explanation

Answer: (b) Tetrahedral

Explanation:
1. Sulphur has four bond pairs and no lone pair, giving a tetrahedral ion.

Teacher's Note:
1. Convert every quantity to moles or equivalents first.
2. Then apply the stoichiometric ratio or the definition asked for.

Question 5: The shape of ICl3 and the hybridisation of iodine are
(a) Trigonal planar, sp²
(b) Pyramidal, sp³
(c) T-shaped, sp³d
(d) Trigonal bipyramidal, sp³d
Show Answer & Explanation

Answer: (c) T-shaped, sp³d

Explanation:
1. Iodine has 3 bond pairs and 2 lone pairs (5 electron pairs, sp³d).
2. The two lone pairs occupy equatorial positions, giving a T-shaped molecule.

Teacher's Note:
1. Eliminate options that disagree with the basic definition.
2. Confirm the remaining option by a quick calculation.

Question 6: The shape of the ClF3 molecule is
(a) Trigonal planar
(b) Pyramidal
(c) T-shaped
(d) Tetrahedral
Show Answer & Explanation

Answer: (c) T-shaped

Explanation:
1. Chlorine has 3 bond pairs and 2 lone pairs (sp³d).
2. The lone pairs take equatorial positions, giving a T-shape.

Teacher's Note:
1. Read the data carefully and write the relevant formula before substituting.
2. Check units and the order of magnitude of the answer.

Question 7: The structure of XeF2 is
(a) Bent
(b) Linear
(c) Trigonal planar
(d) Pyramidal
Show Answer & Explanation

Answer: (b) Linear

Explanation:
1. Xe has 2 bond pairs and 3 lone pairs (sp³d).
2. The three lone pairs occupy the equatorial plane, so the molecule is linear.

Teacher's Note:
1. Convert every quantity to moles or equivalents first.
2. Then apply the stoichiometric ratio or the definition asked for.

Question 8: The hybridisation of the central atom and the shape of the IF7 molecule are
(a) sp³d³, pentagonal bipyramidal
(b) sp³d², octahedral
(c) sp³d, trigonal bipyramidal
(d) sp³, tetrahedral
Show Answer & Explanation

Answer: (a) sp³d³, pentagonal bipyramidal

Explanation:
1. Iodine has seven bond pairs and no lone pair (sp³d³).
2. The shape is pentagonal bipyramidal.

Teacher's Note:
1. Eliminate options that disagree with the basic definition.
2. Confirm the remaining option by a quick calculation.

Question 9: Which of the following hybridisations gives bond angles of 120° in a plane?
(a) sp
(b) sp²
(c) sp³
(d) sp³d²
Show Answer & Explanation

Answer: (b) sp²

Explanation:
1. Three sp² hybrid orbitals lie in one plane at 120° to each other.

Teacher's Note:
1. Read the data carefully and write the relevant formula before substituting.
2. Check units and the order of magnitude of the answer.

Question 10: The type of hybridisation of the two carbon atoms marked * in H3C–C*≡C*–CH3 is
(a) sp³
(b) sp²
(c) sp
(d) s
Show Answer & Explanation

Answer: (c) sp

Explanation:
1. Each carbon in the triple bond forms one sigma bond to carbon and one to another carbon (two sigma bonds), so it is sp hybridised.

Teacher's Note:
1. Convert every quantity to moles or equivalents first.
2. Then apply the stoichiometric ratio or the definition asked for.

Question 11: Which of the following has the longest C–H bond distance?
(a) C2H2
(b) C2H4
(c) C2H4Br2
(d) C6H6
Show Answer & Explanation

Answer: (c) C2H4Br2

Explanation:
1. Bond length decreases with increasing s-character of the carbon orbital: sp (50%) < sp² (33%) < sp³ (25%).
2. In C2H4Br2 the carbon is sp³, so its C–H bond is longest.

Teacher's Note:
1. Eliminate options that disagree with the basic definition.
2. Confirm the remaining option by a quick calculation.

Question 12: In which of the following compounds is the central atom not sp³ hybridised?
(a) BF4−
(b) H3O+
(c) NH2−
(d) BF3
Show Answer & Explanation

Answer: (d) BF3

Explanation:
1. BF4−, H3O+ and NH2− all have four electron pairs around the central atom (sp³).
2. BF3 has three bond pairs (sp²).

Teacher's Note:
1. Read the data carefully and write the relevant formula before substituting.
2. Check units and the order of magnitude of the answer.

Question 13: The hybridisation of sulphur in SO3 is
(a) sp³d
(b) sp³
(c) sp³d²
(d) sp²
Show Answer & Explanation

Answer: (d) sp²

Explanation:
1. SO3 has three bond pairs and no lone pair on sulphur.
2. The hybridisation is sp², and the shape is trigonal planar.

Teacher's Note:
1. Convert every quantity to moles or equivalents first.
2. Then apply the stoichiometric ratio or the definition asked for.

Question 14: In the complex ion [Cu(NH3)4]2+ the Cu(II) ion is most commonly described with which geometry?
(a) Tetrahedral
(b) Square planar
(c) Octahedral
(d) Linear
Show Answer & Explanation

Answer: (b) Square planar

Explanation:
1. Cu(II) is d⁹ and forms four-coordinate square planar complexes with strong ligands such as NH3 (dsp² hybridisation).

Teacher's Note:
1. Eliminate options that disagree with the basic definition.
2. Confirm the remaining option by a quick calculation.

Question 15: Boron forms the compound BF3, whose structure is
(a) Linear
(b) Planar
(c) Tetrahedral
(d) Square pyramidal
Show Answer & Explanation

Answer: (b) Planar

Explanation:
1. Boron uses three sp² hybrid orbitals to bond to fluorine atoms.
2. The molecule is trigonal planar with 120° angles.

Teacher's Note:
1. Read the data carefully and write the relevant formula before substituting.
2. Check units and the order of magnitude of the answer.

Question 16: The bond angle in methane is
(a) 180°
(b) 90°
(c) 120°
(d) 109°
Show Answer & Explanation

Answer: (d) 109°

Explanation:
1. Carbon in CH4 is sp³ hybridised with four equivalent bonds, directed to the corners of a regular tetrahedron at 109.5°.

Teacher's Note:
1. Convert every quantity to moles or equivalents first.
2. Then apply the stoichiometric ratio or the definition asked for.

Question 17: Which molecule has zero dipole moment?
(a) H2O
(b) CO2
(c) HF
(d) HBr
Show Answer & Explanation

Answer: (b) CO2

Explanation:
1. CO2 is linear, so the two C=O bond dipoles cancel.
2. H2O is bent, and HF and HBr are polar diatomic molecules.

Teacher's Note:
1. Eliminate options that disagree with the basic definition.
2. Confirm the remaining option by a quick calculation.

Question 18: Which of the following molecules has a permanent dipole moment?
(a) BF3
(b) SiF4
(c) SF4
(d) XeF4
Show Answer & Explanation

Answer: (c) SF4

Explanation:
1. BF3 (planar), SiF4 (tetrahedral) and XeF4 (square planar) are symmetrical, so their bond dipoles cancel.
2. SF4 is see-saw shaped and has a net dipole moment.

Teacher's Note:
1. Read the data carefully and write the relevant formula before substituting.
2. Check units and the order of magnitude of the answer.

Question 19: Which of the following has zero dipole moment?
(a) CH2Cl2
(b) CH4
(c) NH3
(d) PH3
Show Answer & Explanation

Answer: (b) CH4

Explanation:
1. The four C–H bond dipoles in tetrahedral CH4 cancel.
2. The others are unsymmetrical.

Teacher's Note:
1. Convert every quantity to moles or equivalents first.
2. Then apply the stoichiometric ratio or the definition asked for.

Question 20: The dipole moment of HBr is 1.6 × 10−30 C m and the interatomic spacing is 1 Å. The percentage ionic character of HBr is (e = 1.6 × 10−19 C)
(a) 7
(b) 10
(c) 15
(d) 27
Show Answer & Explanation

Answer: (b) 10

Explanation:
1. For 100% ionic character μ = e × d = 1.6 × 10−19 × 10−10 = 1.6 × 10−29 C m.
2. % ionic = 1.6 × 10−30/1.6 × 10−29 × 100 = 10%.

Teacher's Note:
1. Eliminate options that disagree with the basic definition.
2. Confirm the remaining option by a quick calculation.

Question 21: HCl is expected to have a dipole moment of 6.12 D if completely ionic, but the experimental value is 1.03 D. The percentage ionic character is approximately
(a) 17
(b) 83
(c) 50
(d) 90
Show Answer & Explanation

Answer: (a) 17

Explanation:
1. % ionic character = (1.03/6.12) × 100 = 16.8, i.e. about 17%.

Teacher's Note:
1. Read the data carefully and write the relevant formula before substituting.
2. Check units and the order of magnitude of the answer.

Question 22: Which one has the minimum (nearly zero) dipole moment?
(a) Butene-1
(b) cis-Butene-2
(c) trans-Butene-2
(d) 2-Methylpropene
Show Answer & Explanation

Answer: (c) trans-Butene-2

Explanation:
1. In trans-2-butene the two methyl groups lie on opposite sides of the double bond, so the bond dipoles cancel almost completely.
2. The cis isomer and the other two alkenes have a net dipole moment.

Teacher's Note:
1. Convert every quantity to moles or equivalents first.
2. Then apply the stoichiometric ratio or the definition asked for.

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