Last Updated on April 20, 2025 by XAM CONTENT
Hello students, we are providing case study questions for class 11 Chemistry. Case study questions are the new question format that is introduced in CBSE board. The resources for case study questions are very less. So, to help students we have created chapterwise case study questions for class 11 Chemistry. In this article, you will find case study questions for cbse class 11 Chemistry chapter 4 Chemical Bonding and Molecular Structure.
| Chapter | Chemical Bonding and Molecular Structure |
| Type of Questions | Case Study Questions |
| Nature of Questions | Competency Based Questions |
| Board | CBSE |
| Class | 11 |
| Subject | Chemistry |
| Useful for | Class 11 Studying Students |
| Answers provided | Yes |
| Difficulty level | Mentioned |
| Important Link | Class 11 Chemistry Chapterwise Case Study |
Case Study Questions on Chemical Bonding and Molecular Structure
Case Study Question 1
Passage:
In the reaction between sodium and chlorine, sodium (Na) loses one electron to form Na⁺, and chlorine (Cl) gains an electron to form Cl⁻. These ions are held together by strong electrostatic forces, forming NaCl, a typical ionic compound. Ionic compounds have high melting and boiling points and conduct electricity in molten or aqueous state.
Q1. What type of bond is formed in NaCl?
(a) Covalent bond
(b) Coordinate bond
(c) Ionic bond
(d) Metallic bond
Answer: (c) Ionic bond
Explanation: Electron is transferred from Na to Cl → Ionic bond formed via electrostatic attraction.
Q2. Why do ionic compounds conduct electricity only in molten or aqueous form?
(a) Ions are free to move
(b) Electrons are loosely bound
(c) Molecules are polar
(d) Water makes them volatile
Answer: (a) Ions are free to move
Explanation: In solid state, ions are fixed in lattice. In molten/aqueous state, free ions carry current.
Q3. Which of the following has the highest lattice energy?
(a) NaCl
(b) KCl
(c) RbCl
(d) CsCl
Answer: (a) NaCl
Explanation: Lattice energy ∝ smaller ion size & higher charge. Na⁺ is smaller, so NaCl has highest lattice energy.
Case Study Question 2
Passage:
Ammonia (NH₃) is a covalently bonded molecule with a lone pair of electrons on nitrogen. Its molecular geometry is predicted by the VSEPR theory. Although NH₃ has 4 regions of electron density (3 bond pairs + 1 lone pair), its shape is not tetrahedral, but trigonal pyramidal due to lone pair-bond pair repulsion.
Q1. What is the hybridisation of nitrogen in NH₃?
(a) sp
(b) sp²
(c) sp³
(d) sp³d
Answer: (c) sp³
Explanation: 4 electron domains = sp³ hybridisation
Q2. What is the bond angle in NH₃?
(a) 90°
(b) 109.5°
(c) 107°
(d) 120°
Answer: (c) 107°
Explanation: Ideal angle for sp³ = 109.5° but lone pair repulsion reduces it to ~107°
Q3. What is the shape of NH₃ molecule?
(a) Tetrahedral
(b) Trigonal planar
(c) Bent
(d) Trigonal pyramidal
Answer: (d) Trigonal pyramidal
Explanation: Due to 1 lone pair, the molecular shape becomes trigonal pyramidal as per VSEPR theory.
Case Study Question 3
Passage:
The molecule H₂O has a bent shape due to two lone pairs on oxygen. Each O–H bond is polar because of oxygen’s high electronegativity. The net dipole moment is not zero due to the asymmetrical geometry, making H₂O a polar molecule. In contrast, CO₂, despite having polar bonds, is non-polar overall due to its linear geometry.
Q1. Which of the following best explains why H₂O is polar but CO₂ is not?
(a) H₂O has ionic bonds
(b) CO₂ has no dipole moment
(c) H₂O has lone pairs causing bent shape
(d) CO₂ has unshared electrons
Answer: (c) H₂O has lone pairs causing bent shape
Explanation: Bent shape causes dipoles not to cancel → net polarity in H₂O
Q2. Which property depends directly on molecular polarity?
(a) Boiling point
(b) Molar mass
(c) Ionisation energy
(d) Bond enthalpy
Answer: (a) Boiling point
Explanation: Polar molecules have stronger intermolecular forces (H-bonding) → higher boiling point.
Q3. The bond angle in H₂O is approximately:
(a) 180°
(b) 120°
(c) 109.5°
(d) 104.5°
Answer: (d) 104.5°
Explanation: Due to 2 lone pairs on oxygen → more repulsion → bond angle reduced to 104.5°
We hope the given case study questions for Chemical Bonding and Molecular Structure Class 11 helps you in your learning.
Also check
- Chemical Thermodynamics Class 11 Case Study Questions Chemistry Chapter 5
- Chemical Bonding and Molecular Structure Class 11 Case Study Questions Chemistry Chapter 4
- Classification of Elements and Periodicity in Properties Class 11 Case Study Questions Chemistry Chapter 3
- Structure of Atom Class 11 Case Study Questions Chemistry Chapter 2
- Some Basic Concepts of Chemistry Class 11 Case Study Questions Chemistry Chapter 1
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Topics from which case study questions may be asked
- Lewis structures
- VSEPR theory
- Hybridization
- Molecular orbital theory
Chemical bonding explains how atoms combine to form stable substances.
For further practice on case study questions related to Chemical Bonding and Molecular Structure Class 11 Chemistry, we recommend exploring the link given below.
Frequently Asked Questions (FAQs) on Chemical Bonding and Molecular Structure Case Study Questions
Q1: What are case study questions in Chemical Bonding and Molecular Structure?
A1: These are application-based questions that assess understanding of Chemical Bonding and Molecular Structure concepts.
Q2: Are case study questions part of CBSE Class 11 Chemistry?
A2: Yes, CBSE includes case study/competency-based questions in exams.
Q3: How can I prepare for Chemistry case study questions?
A3: Focus on conceptual clarity, real-life applications, and NCERT-based understanding.
Q4: Are answers provided for Chemical Bonding and Molecular Structure case study questions?
A4: Yes, detailed answers are provided for all case study questions.
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