Chemical Bonding and Molecular Structure Class 11 MCQ Online Test, Set 1 (with Solutions)

Chemical Bonding and Molecular Structure: Practice Set 1

13 questions: MCQs, assertion–reason and a case study
Time: 15 minutes (submits by itself when time is up)
+1 for each correct answer, no negative marking
After submitting: score, correct answers and a full solution for every question

The hybridisation of P in PCl₅ is

(a) sp³(b) sp³d(c) sp³d²(d) dsp²

The shape of PCl₅ is

(a) trigonal bipyramidal(b) octahedral(c) square pyramidal(d) tetrahedral

NO and NO₂ are examples of

(a) expanded octet molecules(b) ionic compounds(c) odd-electron molecules(d) electron-deficient octets

The electronic theory of chemical bonding was developed by

(a) Kössel and Lewis(b) Bohr and Rutherford(c) Heitler and London(d) Pauling and Slater

Which molecule has an incomplete octet on the central atom?

(a) BF₃(b) NH₃(c) H₂O(d) CH₄

With increase in bond order, bond length

(a) increases(b) remains same(c) decreases(d) becomes zero

The dipole moment is the product of

(a) magnitude of charge and distance between the centres of charges(b) mass and velocity(c) charge and mass(d) bond energy and length

The shape of SF₆ is

(a) trigonal bipyramidal(b) octahedral(c) square planar(d) tetrahedral

9Assertion–Reason

Assertion (A): The bond angle in water (104.5°) is less than the tetrahedral angle.
Reason (R): Lone pair–lone pair repulsion is greater than bond pair–bond pair repulsion.

(a) Both Assertion (A) and Reason (R) are true and Reason (R) is the correct explanation of Assertion (A).(b) Both Assertion (A) and Reason (R) are true but Reason (R) is not the correct explanation of Assertion (A).(c) Assertion (A) is true but Reason (R) is false.(d) Assertion (A) is false but Reason (R) is true.

10Assertion–Reason

Assertion (A): NaCl is an ionic compound.
Reason (R): Sodium has a low ionisation enthalpy and chlorine has a high negative electron gain enthalpy.

Case study

Using the molecular orbital theory, a student compares O₂, O₂⁺ and O₂⁻.

The bond order of O₂⁺ is

(a) 2.5(b) 2(c) 1.5(d) 3

The bond order of O₂⁻ is

(a) 2(b) 1.5(c) 2.5(d) 1

Arranged in order of increasing bond length, the species are

(a) O₂⁻ < O₂ < O₂⁺(b) O₂ < O₂⁺ < O₂⁻(c) O₂⁺ < O₂ < O₂⁻(d) all equal