Structure of Atom Class 11 Case Study Questions Chemistry Chapter 2

Reading Time: 6 minutes

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 2 Structure of Atom.

Chapter	Structure of Atom
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 Structure of Atom

Case Study Question 1:

Discovery of Subatomic Particles

Passage:
In a physics lab, students observe two different experiments. One is J.J. Thomson’s cathode ray experiment, which led to the discovery of the electron, and the other is Goldstein’s canal ray experiment, which led to the identification of protons. Both experiments showed that atoms are not indivisible, as believed by Dalton.

Q1. What did Thomson conclude about the nature of cathode rays?
(a) They are neutral particles
(b) They are positively charged
(c) They are negatively charged
(d) They do not deflect in electric fields

Answer: (c)
Explanation: Cathode rays (electrons) are deflected by electric and magnetic fields, indicating a negative charge.

Q2. Goldstein’s canal rays led to the discovery of:
(a) Electrons
(b) Neutrons
(c) Protons
(d) Photons

Answer: (c)
Explanation: Canal rays (positive rays) were composed of positively charged particles → Protons.

Q3. Which model of the atom was first to describe the existence of both positive and negative particles within the atom?
(a) Dalton’s Model
(b) Thomson’s Plum Pudding Model
(c) Rutherford’s Model
(d) Bohr’s Model

Answer: (b)
Explanation: Thomson proposed a model with a positively charged sphere and embedded electrons (“plum pudding”).

Case Study Question 2:

Rutherford’s α-Scattering Experiment

Passage:
Rutherford performed an alpha particle scattering experiment by bombarding a thin gold foil with alpha particles. Most particles passed through, but some were deflected at large angles. This led to a nuclear model of the atom where a dense, positively charged nucleus was present at the center and electrons revolved around it.

Q1. What was the key conclusion from Rutherford’s experiment?
(a) Atom is a solid sphere
(b) Atom is mostly empty space
(c) Electrons are embedded in a positive sphere
(d) Nucleus is negatively charged

Answer: (b)
Explanation: Most alpha particles passed through → atoms are mostly empty space.

Q2. What caused the deflection of alpha particles in Rutherford’s experiment?
(a) Orbiting electrons
(b) Neutrons
(c) The dense nucleus
(d) The gold atoms’ mass

Answer: (c)
Explanation: Strong deflection occurred when alpha particles came close to the positively charged nucleus

Q3. Which drawback of Rutherford’s model led to the need for Bohr’s model?
(a) No explanation of neutron presence
(b) Unstable orbits for electrons
(c) No description of protons
(d) Could not explain alpha scattering

Answer: (b)
Explanation: Electrons revolving around the nucleus should lose energy and spiral in — Rutherford’s model couldn’t explain atom’s stability.

Case Study Question 3:

Quantum Numbers and Orbitals

Passage:
A student is asked to identify an orbital based on its quantum numbers:

– Principal quantum number $n=3$
– Azimuthal quantum number $l=2$
– Magnetic quantum number $m=0$

They also need to identify the number of orbitals possible in this subshell and determine the maximum number of electrons it can accommodate.

Q1. What is the type of orbital described by these quantum numbers?
(a) 3s
(b) 3p
(c) 3d
(d) 2d

Answer: (c)
Explanation: $l=2 \rightarrow \mathrm{~d}$-orbital, $n=3 \rightarrow 3 \mathrm{~d}$ orbital

Q2. How many orbitals are present in a 3d subshell?
(a) 1
(b) 3
(c) 5
(d) 7

Answer: (c)
Explanation: For $l=2$, magnetic quantum number $m=-2,-1,0,+1,+2 \rightarrow 5$ orbitals

Q3. What is the maximum number of electrons that can be accommodated in all 3d orbitals?
(a) 2
(b) 5
(c) 6
(d) 10

Answer: (d)
Explanation: Each orbital holds 2 electrons $\rightarrow 5 \times 2=10$ electrons in 3d

We hope the given case study questions for Structure of Atom 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

🚀 Boost Your Exam Prep: Get case study questions for all subjects (Class 6-12) now!

👉 Explore more resources on CBSE Class 11

Download eBooks for CBSE Class 12 Physics (Exam Special)

• 120 Case Study Questions for Class 12 Physics
• 320 Assertion Reasoning Questions for Class 12 Physics
• 95 Reasoning Based Questions for Class 12 Physics
• Important Derivation for Class 12 Physics
• MCQ Questions for Class 12 Physics
• Chapter Test for Class 12 Physics with Solutions
• 230 Important Numerical for Class 12 Physics
• 75 Important Diagrams & Graphs for Class 12 Physics

Topics from which case study questions may be asked

• Bohr’s model
• Quantum mechanical model
• Electronic configuration
• Quantum numbers

Understanding atomic structure unlocks the behavior of elements and the formation of compounds.

For further practice on case study questions related to Structure of Atom Class 11 Chemistry, we recommend exploring the link given below.

Frequently Asked Questions (FAQs) on Structure of Atom Case Study Questions