🧪 NCERT Class 11 • Chapter 4

Chemical Bonding & Molecular Structure
MCQs

JEE & NEET 2026
VSEPR • Hybridisation • Molecular Orbital Theory • Bond Parameters • Fajan’s Rules

60 expert-level questions with step-by-step explanations and exam-style traps.

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60
MCQs
3
Difficulty Levels
2026
Exam Aligned
NEET + JEE
Covered

Core Concepts

🔗

Lewis Structures

Electron dot structures reveal how atoms share or transfer electrons to achieve stability.

📐

VSEPR Theory

Molecular geometry depends on repulsion between electron pairs around the central atom.

🧬

Hybridisation

Atomic orbitals combine to form new hybrid orbitals like sp, sp² and sp³.

⚛️

Molecular Orbitals

Bonding and antibonding orbitals explain bond order, magnetism and stability.

Why Practice These MCQs

⚡ Identify geometry instantly using VSEPR rules.
🧠 Strengthen hybridisation recognition across molecules.
🎯 Avoid common exam traps involving lone pairs.
📊 Predict polarity, bond length and bond order correctly.
🧪 Master molecular orbital diagrams quickly.
🚀 Build intuition for structure → property relationships.

Exam Trend Analysis

VSEPR Geometry
Hybridisation
Bond Order (MO Theory)
Dipole Moment

🎯 Knowledge Check

Can you predict the geometry of XeF₄? What is the bond order of O₂⁺? Is BF₃ polar or non-polar?

If these questions feel uncertain, the MCQs below will expose exactly where your understanding needs sharpening.

Start Solving MCQs →

Quick Formula Sheet

Before attempting the MCQs, quickly revise the most important relationships from Chemical Bonding and Molecular Structure. These formulas and rules appear repeatedly in JEE and NEET questions.

⚛️ Bond Order (Molecular Orbital Theory)

\[ \text{Bond Order} = \frac{N_b - N_a}{2} \]

Where \(N_b\) = number of electrons in bonding orbitals \(N_a\) = number of electrons in antibonding orbitals

Higher bond order → stronger bond and shorter bond length.

⚡ Dipole Moment

\[ \mu = q \times r \]

\(q\) = magnitude of charge \(r\) = distance between charges

Unit: Debye (D)

🧪 Formal Charge

\[ FC = V - \left( L + \frac{B}{2} \right) \]

\(V\) = valence electrons \(L\) = lone pair electrons \(B\) = bonding electrons

Best Lewis structure has the lowest formal charge.

📏 Bond Order vs Bond Length

Bond Length ∝ \(\frac{1}{\text{Bond Order}}\)

As bond order increases:

  • Bond length decreases
  • Bond energy increases
  • Bond strength increases

🔬 Hybridisation Formula

\[ H = \frac{1}{2} (V + M - C + A) \]

\(V\) = valence electrons \(M\) = monovalent atoms \(C\) = positive charge \(A\) = negative charge

Hybridisation = number of electron domains around the central atom.

📐 VSEPR Rule

Electron pairs around a central atom repel each other and arrange themselves to minimise repulsion.

Repulsion order:

\[ LP-LP > LP-BP > BP-BP \]

🎯 Knowledge Check

Chemistry — CHEMICAL BONDING AND MOLECULAR STRUCTURE

50 Questions Class 11 MCQs
25:00 ⏱ Time
⚡ Progress 0 / 50 answered
1
what is the maximum number of elections that can occupy the outer shell according to Lewis's Model
2
what is the stable electronic arrangement that Levis postulated atom achieve when linked by chemical bond
3
In lewis symbols, what do the dots around the symbol represent
4
According to Kossel, what separates the highly electronegative halogens and the highly positive alkali metals in the periodic table
5
what types of bond is formed as a result of electrostatic attraction between positive and negative ions
6
what is the electronic configuration of a noble gas, excluding Helium according to Kossel
7
In the formation of Nacl, what happens to sodium atom?
8
What is the charge on Calcium ion in the formation of \(CaF_2\)
9
what is the configuration of the chloride ion after gaining an electron
10
what is the term used for the bond formed by sharing of a pair of elections between atoms?
11
what is the main concept behind electronic theory of chemical bonding developed by Kossel Lewis
12
what is the purpose of atom counter ning according to the octet rule?
13
which of the following is a method by which atoms can achaine an octet according to Kossel and Lewis
14
Write the electronic configuration of chlorine
15
what type of bond is formed when two atoms share one electron pair
16
In a carbon dioxide molecule, what type of bond exists between carbon and oxygen atom?
17
what is the term used to describe the representation of molecules using dots for elections?
18
How many valence electrons are available for bonding in Methane molecule
19
In the formation of CL2, molecule, how many electrons are shared before the two chlorine atoms
20
what is the central atom of the NF3 molecule
21
what happens to the total number of valence electrons when a molecule forms an anion?
22
which atom type occupies the
23
what is the result of sharing two pairs of elections between two atoms
24
which of the following is an example of a molecule with an in complete octet
25
what is the main purpose of indicating formal charge in a Lewis structure
26
which element is likely to have expanded octet
27
which of the following compound is an example of an odd electron molecule
28
what is a limitation of octet rule
29
which noble gas can form compound with Oxygen and Fluorine
30
what is octet-rule based upon
31
which of the following is not a type of exception of the octet rule
32
In which compond does sulphur obey the octet rule
33
What does lattice enthalpy measure in an ionic solid
34
What in the covalent radius of chlorine if the bond length in a chlorine molecule is 198 pm
35
which of the following is true about covalent radii
36
What is the bond angle in a water molecule?
37
which molecule has the highest bond enthalpy among the following
38
Which bond has the shortest bond length among the following
39
What is the bond order of molecule CO
40
what is the concept introduced to address the inadequacy of a single Lewis structure in representing certain molecule
41
what is the bond type between oxygen atoms in the resonance hybrid of ozone
42
what is the unit used to express dipole moment
43
what is the shape of molecule with the formula \(AB)2\) according to VSEPR theory when central atom has no lone pair
44
According to VSEPR theory, which type of election pain repulsion is the strongest
45
Which atomic orbitals overlap to form a Hydrogen molecule
46
Which type of overlapping occurs between two half-filled S-orbitals
47
What is the geometry of a molecule with sp hybridization
48
What is the bond angle in a molecule with sps hybridization
49
what is the geometry of a molecule with \(sp^2\) hybridization
50
what is the geometry of a molecule with \(sp^3\) hybridization

Frequently Asked Questions

A chemical bond is the attractive force that holds atoms or ions together in a molecule or compound due to electrostatic interactions between charged particles.

Atoms form bonds to attain lower potential energy and greater stability, often by achieving a noble gas configuration (octet or duplet).

The octet rule states that atoms tend to gain, lose, or share electrons to acquire eight electrons in their valence shell.

The duplet rule applies to hydrogen and helium, which attain stability with two electrons in their outermost shell.

An ionic bond is formed by complete transfer of electron(s) from one atom to another, resulting in oppositely charged ions held by electrostatic attraction.

A covalent bond is formed by mutual sharing of one or more pairs of electrons between two atoms.

Bond order is defined as half the difference between the number of bonding and antibonding electrons: \( \text{Bond Order} = \frac{N_b - N_a}{2} \).

Higher bond order generally implies stronger bond and shorter bond length.

Bond length is the equilibrium distance between the nuclei of two bonded atoms.

Bond enthalpy is the energy required to break one mole of bonds in gaseous state.

Lattice energy \( U \propto \frac{q_1 q_2}{r} \), where \( q_1, q_2 \) are ionic charges and \( r \) is interionic distance.

Formal charge \( = V - L - \frac{B}{2} \), where \( V \) = valence electrons, \( L \) = lone pair electrons, \( B \) = bonding electrons.

Resonance is the phenomenon in which a molecule cannot be represented by a single Lewis structure but by multiple contributing structures.

Resonance hybrid is the actual structure of a molecule represented as a weighted average of contributing resonance structures.

Valence Shell Electron Pair Repulsion (VSEPR) theory predicts molecular geometry based on repulsion between electron pairs around the central atom.

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