Exam-Style Online Test | Chemistry: Structure Of Atom Test

Class 11 Chemistry — Chapter 2: Structure of Atom Online Test

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Class 11 Chemistry: Structure of Atom Online Test (Paper 1)

Welcome to Paper 1! This is your foundation to build confidence and get you ready to tackle the challenges ahead.

  • Total Questions: 20
  • Time Allotted: 30 minutes
  • Passing Score: 40%
  • Randomization: No
  • Certificate: No
  • Retake: Allowed
  • Price: 100% Free

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1 / 20

1. For hydrogen atom, the ratio of radii of 1st and 3rd orbit is:

2 / 20

2. The number of radial nodes in 5d orbital is:

3 / 20

3. The ionization energy of hydrogen atom in the ground state is:

4 / 20

4. The electronic configuration of neon (Z=10) is:

5 / 20

5. The electronic configuration of helium (Z=2) is:

6 / 20

6. Why do electrons prefer to occupy different orbitals of equal energy before pairing?

7 / 20

7. When two subshells have the same value, the one that fills first is the one with:

8 / 20

8. Which d-orbitals have lobes oriented between the axes (at 45° angles)?

9 / 20

9. The radial probability distribution curve of a 2s orbital shows:

10 / 20

10. The value of is associated with:

11 / 20

11. The azimuthal quantum number primarily determines the:

12 / 20

12. If , how many orbitals are possible in that shell?

13 / 20

13. The three dumbbell-shaped orbitals oriented along x, y, and z axes are:

14 / 20

14. What physical meaning does the wave function itself have?

15 / 20

15. The first line of the Brackett series corresponds to which transition?

16 / 20

16. Which equation represents Einstein’s photoelectric effect?

17 / 20

17. What is the wavelength of a radio wave with frequency ?

18 / 20

18. Which of the following is a correct postulate of Bohr’s atomic model?

19 / 20

19. In Chadwick’s experiment, which element was bombarded with alpha particles to discover the neutron?

20 / 20

20. What conclusion did Rutherford draw from the gold foil experiment?

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Class 11 Chemistry: Structure of Atom Online Test (Paper 2)

Welcome to Paper 2! You’ve mastered the basics, and now it’s time to test your understanding with a more challenging set of questions.

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  • Total Questions: 30
  • Time Allotted: 45 minutes
  • Passing Score: 50%
  • Randomization: Yes
  • Certificate: No
  • Retake: Allowed
  • Price: 100% Free

Good luck! 👍

1 / 30

1. Which element has the configuration 1s² 2s² 2p⁶ 3s² 3p⁶ 4s²?

2 / 30

2. The Balmer- line (H) in the hydrogen spectrum is produced by the transition:

3 / 30

3. The wavelength of the shortest line in the Lyman series is:

4 / 30

4. The number of orbitals in a subshell is given by:

5 / 30

5. Which type of spectrum is obtained from an incandescent solid or liquid?

6 / 30

6. The Brackett series of hydrogen lines appears in which region?

7 / 30

7. If the time period of an EM wave is , its frequency is:

8 / 30

8. Why was the concept of orbit replaced by orbital?

9 / 30

9. Which of the following notations is INCORRECT?

10 / 30

10. How many orientations are possible for f-orbitals?

11 / 30

11. Which element has the configuration [Ar] 3d⁵ 4s²?

12 / 30

12. The electronic configuration of fluorine (Z=9) is:

13 / 30

13. In multi-electron atoms, the order of increasing energy of orbitals is best represented as:

14 / 30

14. The three p-orbitals are oriented:

15 / 30

15. The electronic configuration of helium (Z=2) is:

16 / 30

16. Why could Bohr’s model not explain the Zeeman effect?

17 / 30

17. What is the wavelength of the first line of the Lyman series ()?

18 / 30

18. For a given value of , the maximum number of electrons that can be accommodated is:

19 / 30

19. A stellar spectrum shows strong dark Na “D” lines near and . This most directly indicates:

20 / 30

20. Which subatomic particle has the least mass?

21 / 30

21. Which parameter of a wave is directly proportional to photon energy?

22 / 30

22. Which orbital is spherical in shape and smallest in size?

23 / 30

23. Which scientist measured the charge of an electron after Thomson’s work?

24 / 30

24. The orientation of orbital is:

25 / 30

25. What is an emission spectrum?

26 / 30

26. Which direct conceptual weakness led to the rejection of the plum pudding model after scattering experiments?

27 / 30

27. Which experiment led to the discovery of the nucleus?

28 / 30

28. Which concept explains the extra stability of half-filled and fully filled subshells?

29 / 30

29. Who formulated the wave equation that describes the behavior of an electron in an atom?

30 / 30

30. In transition metal complexes, splitting of d-orbitals into and sets is due to:

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Class 11 Chemistry: Structure of Atom Online Test (Paper 3)

Welcome to Paper 3! You’ve warmed up—now it's time to step up your game and conquer the challenge with tougher questions!

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  • Total Questions: 50
  • Time Allotted: 75 minutes
  • Passing Score: 70%
  • Randomization: Yes
  • Certificate: Yes
  • Retake: Allowed
  • Price: 100% Free

Good luck! 👍

1 / 50

1. The number of angular nodes in 4d orbital is:

2 / 50

2. The Schrödinger wave equation gives information about:

3 / 50

3. For a given element and electronic transition, how do emission and absorption wavelengths compare?

4 / 50

4. The wavelength of the second line of Balmer series in hydrogen is approximately:

5 / 50

5. Which orbital fills immediately after 4p according to Aufbau sequence?

6 / 50

6. The azimuthal quantum number () signifies:

7 / 50

7. Which device is commonly used to obtain a spectrum of light?

8 / 50

8. Which experiment indirectly supported Pauli’s exclusion principle?

9 / 50

9. Which of the following sets correctly matches the charge of subatomic particles?

10 / 50

10. How many d-orbitals exist in a given shell?

11 / 50

11. Which experiment led to the discovery of electrons?

12 / 50

12. For hydrogen atom, the ratio of radii of 1st and 3rd orbit is:

13 / 50

13. What is the total number of orbitals in the second shell ()?

14 / 50

14. Who discovered the neutron?

15 / 50

15. The electronic configuration of hydrogen (Z=1) is:

16 / 50

16. Which quantum number decides the number of orbitals in a subshell?

17 / 50

17. The significance of quantum numbers is that they:

18 / 50

18. The wave number () for the first line of Balmer series in hydrogen is:

19 / 50

19. Which statement is true about the nodal plane in a p-orbital?

20 / 50

20. Which of the following is correct about the principal quantum number?

21 / 50

21. How many maximum electrons can occupy a single orbital?

22 / 50

22. What is the SI unit of wave number?

23 / 50

23. The energy of an electron in the hydrogen atom is proportional to:

24 / 50

24. The visible region of the EM spectrum lies approximately between:

25 / 50

25. How many quantum numbers are required to specify an electron completely in an atom?

26 / 50

26. Who discovered the neutron?

27 / 50

27. The stopping potential in a photoelectric experiment is directly related to:

28 / 50

28. Why was the discovery of the neutron important?

29 / 50

29. In Thomson’s experiment, what was the value of e/m ratio obtained for the electron?

30 / 50

30. Which d-orbital lies along the x and y axes?

31 / 50

31. Which region of the electromagnetic spectrum has the longest wavelength?

32 / 50

32. Which phenomenon cannot be explained by the wave theory of light?

33 / 50

33. The term “maximum multiplicity” in Hund’s rule refers to:

34 / 50

34. Which noble gas configuration is equivalent to neon (Z=10)?

35 / 50

35. What did the plum pudding model successfully account for?

36 / 50

36. Which electromagnetic radiation has wavelengths slightly longer than visible red light?

37 / 50

37. In nitrogen (Z=7), how are the three 2p electrons distributed according to Hund’s rule?

38 / 50

38. Which is NOT a characteristic of orbitals?

39 / 50

39. Which statement is correct according to Pauli’s principle?

40 / 50

40. The splitting of white light into its component colors is called:

41 / 50

41. What experimental evidence confirmed de Broglie’s hypothesis?

42 / 50

42. The ionization energy of He⁺ ion is:

43 / 50

43. For a hydrogen-like atom (one electron), energy of an orbital depends on:

44 / 50

44. Which transition in hydrogen atom produces radiation of frequency ? (h = , 1 eV = )

45 / 50

45. Which of the following quantum numbers is not possible for any electron?

46 / 50

46. The energy difference between and levels in hydrogen atom is:

47 / 50

47. The splitting of spectral lines in a magnetic field is explained by:

48 / 50

48. Which of the following shows an anomalous configuration due to fully filled d-subshell?

49 / 50

49. The number of orbitals present in the 3rd shell () is:

50 / 50

50. Which orbital is oriented along the z-axis with a unique donut-shaped ring?

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Practice Structure of Atom MCQs
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Class 11 Chemistry: Chapter 2 — Structure of Atom Online Test

The Class 11 Chemistry: Chapter 2 — Structure of Atom Online Test is designed to give you a thorough understanding of atomic structure. With a pool of 475 MCQs, this test covers the fundamental concepts of atomic theory, electron configuration, and subatomic particles. This test is completely free, CBSE/NCERT-aligned, and provides instant results after each attempt. It is divided into three difficulty levels to help you build confidence and gradually progress to more challenging questions.

What is this Chapter 2 Online Test?

This test contains three exam-style MCQ papers for Chapter 2: Structure of Atom:

  • Paper 1 (Easy) — Foundation: 20 questions · 30 min · Pass 40% · Fixed set
  • Paper 2 (Medium) — Mixed: 30 questions · 45 min · Pass 50% · Randomized from a pool of ~475 questions
  • Paper 3 (Hard) — Challenge: 50 questions · 75 min · Pass 70% · Randomized from the same pool + Certificate on pass

Note: You get new question mixes in Paper 2 and Paper 3 on every attempt. Each attempt is timed, auto-evaluated, and shows your score with an answer review.

Topics Covered in These Online Tests

In this online test, you will practice key topics from Chapter 2: Structure of Atom, which include:

  • Discovery of Subatomic Particles — Electrons, Protons, Neutrons, and their properties
  • Thomson’s Model of Atom — Plum pudding model and its limitations
  • Rutherford’s Model of Atom — Gold foil experiment and its conclusions
  • Bohr’s Model of Atom — Energy levels, quantization of energy, and hydrogen spectrum
  • Dual Nature of Matter — Wave-particle duality of electrons, de Broglie hypothesis
  • Quantum Mechanical Model — Schrödinger’s equation, orbitals and quantum numbers
  • Electron Configuration — Aufbau principle, Pauli exclusion principle, Hund’s rule
  • Atomic Orbitals and Quantum Numbers — Types of orbitals (s, p, d, f) and their significance

How This Exam-Style Online Test Works

  • Pick a paper → Answer MCQs within time → Submit → Get instant score and answer review.
  • Timed MCQs: Paper 1: 30 minutes, Paper 2: 45 minutes, Paper 3: 75 minutes.
  • Instant feedback: Your score and detailed summary with answers are available immediately.
  • Unlimited retakes: You can retake the test as many times as you like. Paper 2 and Paper 3 offer fresh mixes on each attempt.
  • Certificate: A certificate is awarded after successfully passing Paper 3 with a score of 70% or more.

Who Can Take This Test?

  • Class 11 CBSE/NCERT students preparing for unit tests, mid-term exams, and final exams.
  • JEE Main/Advanced & NEET aspirants seeking a strong foundation in Chemistry concepts.
  • School students wanting to improve their understanding of atomic structure and related topics.
  • Teachers and tutors who need practice tests for their students.
  • Self-learners and home-schoolers wanting an online resource for Chapter 2 practice.

Advantages of this Online Test

  • Real exam feel: Timed tests help you simulate the real exam environment, improving time management.
  • Step-up difficulty: Progress from Paper 1 (easy) to Paper 3 (hard) to master the topic.
  • Instant feedback: You’ll get a score, review your answers, and learn where you need improvement.
  • Unlimited attempts: Take the test as many times as you want, improving with each attempt.
  • Completely free: No charges, no sign-in required—just unlimited access to the online test.

How This Test Helps You Study Better

  • Step 1 – Concept check: Take Paper 1 after reading the chapter to gauge your understanding.
  • Step 2 – Reinforce learning: Take Paper 2 for a balanced mix of theory and numerical questions.
  • Step 3 – Challenge yourself: Take Paper 3 to assess your mastery of the chapter.
  • Step 4 – Review: Analyze your results and reattempt the test to improve your knowledge.

Important Notes (Read Before You Start)

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