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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. The quantity in Schrödinger’s equation represents:

2 / 30

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

3 / 30

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

4 / 30

4. Who discovered the neutron?

5 / 30

5. How many orbitals are present in the p-subshell?

6 / 30

6. The dark Fraunhofer lines observed in sunlight are an example of:

7 / 30

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

8 / 30

8. The actual ground-state configuration of chromium (Z=24) is:

9 / 30

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

10 / 30

10. Which transition in the hydrogen atom gives the Lyman series?

11 / 30

11. Which scientist’s model of the atom is often referred to as the “plum pudding model”?

12 / 30

12. What is the general shape of p-orbitals?

13 / 30

13. The actual configuration of molybdenum (Z=42) is:

14 / 30

14. Which color of visible light diffracts the most?

15 / 30

15. Which region of the EM spectrum has the highest frequency?

16 / 30

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

17 / 30

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

18 / 30

18. Why does hydrogen emit line spectra instead of a continuous spectrum?

19 / 30

19. Which statement about electromagnetic waves is correct?

20 / 30

20. Which of the following is a major limitation of Bohr’s model?

21 / 30

21. What happens to the de Broglie wavelength of a particle if its velocity increases?

22 / 30

22. Which of the following orbital filling violates Hund’s rule?

23 / 30

23. Which of the following correctly expresses wave number?

24 / 30

24. Which hydrogen spectral line lies in the red region of the visible spectrum?

25 / 30

25. The line spectrum of hydrogen atom provides evidence for:

26 / 30

26. Which orbital is spherical in shape?

27 / 30

27. Which equation represents Einstein’s photoelectric effect?

28 / 30

28. For a subshell with , the possible values of are:

29 / 30

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

30 / 30

30. Which of the following notations is INCORRECT?

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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. Which hydrogen spectral series lies entirely in the visible region?

2 / 50

2. Which color of visible light diffracts the most?

3 / 50

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

4 / 50

4. Which of the following spectral series has the shortest wavelength limit?

5 / 50

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

6 / 50

6. The hydrogen emission spectrum is an example of:

7 / 50

7. Pauli’s exclusion principle explains which property of matter?

8 / 50

8. The notation “3p⁶” represents:

9 / 50

9. Which of the following sets of quantum numbers is NOT allowed?

10 / 50

10. Which orbital has no directional orientation in space?

11 / 50

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

12 / 50

12. What prevents electrons from spiraling into the nucleus in Bohr’s model?

13 / 50

13. Which letter notation corresponds to ?

14 / 50

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

15 / 50

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

16 / 50

16. Which equation represents Einstein’s photoelectric effect?

17 / 50

17. According to Planck’s quantum theory, energy is emitted or absorbed in:

18 / 50

18. The energy required to excite an electron in hydrogen atom from to is:

19 / 50

19. What is the significance of the spin quantum number in electronic configuration?

20 / 50

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

21 / 50

21. Which subatomic particle defines isotopes of an element?

22 / 50

22. The velocity of an electron in the first Bohr orbit of hydrogen is approximately:

23 / 50

23. Which quantum number determines the shape of an orbital?

24 / 50

24. Which concept replaced Bohr’s fixed orbits due to Schrödinger’s work?

25 / 50

25. What is the ionization energy of hydrogen atom in ground state?

26 / 50

26. Which of the following statements is correct?

27 / 50

27. The line at 656 nm in hydrogen spectrum corresponds to which transition?

28 / 50

28. How many orbitals are present in the d-subshell?

29 / 50

29. What is the frequency of radiation emitted when an electron jumps from to in hydrogen?

30 / 50

30. Which is the correct electronic configuration of chromium (Z=24)?

31 / 50

31. Which element has a fully filled d-subshell in its ground state configuration?

32 / 50

32. The maximum number of electrons that can be present in all orbitals with is:

33 / 50

33. Stable electronic configurations are generally associated with:

34 / 50

34. Which of the following correctly expresses wave number?

35 / 50

35. Which of the following best describes hydrogen line spectra?

36 / 50

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

37 / 50

37. Before the discovery of neutrons, which problem remained unresolved in atomic models?

38 / 50

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

39 / 50

39. What is the charge of a proton in coulombs?

40 / 50

40. Which of the following spectroscopic phenomena is explained using electron spin?

41 / 50

41. Which subatomic particle is responsible for chemical bonding and reactivity?

42 / 50

42. Which noble gas has the stable configuration [Xe] 6s² 4f¹⁴ 5d¹⁰ 6p⁶?

43 / 50

43. Which arrangement produces an absorption spectrum?

44 / 50

44. Which subatomic particle is positively charged?

45 / 50

45. The minimum energy needed to remove an electron from a metal surface is called:

46 / 50

46. What is an emission spectrum?

47 / 50

47. The magnetic quantum number () describes:

48 / 50

48. The ground-state configuration of copper (Z = 29) is:

49 / 50

49. The dark Fraunhofer lines observed in sunlight are an example of:

50 / 50

50. The difference between 1s and 2s orbitals is:

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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)

  • Do not refresh or close the tab during the test as it will interrupt your session.
  • Best experience: Use a modern browser and stable internet connection for optimal performance.
  • Allow cookies / local storage to save your progress.
  • 100% free: There are no hidden charges for taking this test.

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