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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 dark Fraunhofer lines observed in sunlight are an example of:

2 / 30

2. Which hydrogen series falls in the infrared region?

3 / 30

3. Who proposed the dual nature of matter, introducing the concept of matter waves?

4 / 30

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

5 / 30

5. Which key limitation made the plum pudding model incompatible with atomic emission spectra?

6 / 30

6. Who discovered the neutron?

7 / 30

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

8 / 30

8. The significance of quantum numbers is that they:

9 / 30

9. Which element has the stable configuration [Ar] 3d¹⁰ 4s² 4p⁶ 5s²?

10 / 30

10. The electronic configuration of oxygen (Z=8) can be written as:

11 / 30

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

12 / 30

12. Which of the following has a noble gas configuration in its ground state?

13 / 30

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

14 / 30

14. If , what is the only possible value of ?

15 / 30

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

16 / 30

16. The number of atomic orbitals in the shell is given by:

17 / 30

17. The energy of emitted photon in hydrogen spectrum is related to:

18 / 30

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

19 / 30

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

20 / 30

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

21 / 30

21. Which concept is compatible with Heisenberg’s uncertainty principle?

22 / 30

22. The principal quantum number () signifies:

23 / 30

23. Which unit combination correctly represents frequency?

24 / 30

24. Stable electronic configurations are generally associated with:

25 / 30

25. Which of the following is NOT true about atomic orbitals?

26 / 30

26. The orientation of d-orbitals in space is determined by which quantum number?

27 / 30

27. The Rydberg formula for hydrogen spectral lines is:

28 / 30

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

29 / 30

29. Which of the following statements about d-orbitals is CORRECT?

30 / 30

30. The general formula for hydrogen spectral series is:

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

2 / 50

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

3 / 50

3. Which is the correct ground-state configuration of sodium (Z=11)?

4 / 50

4. The Pfund series of hydrogen corresponds to electron transitions to:

5 / 50

5. Which of the following is a direct consequence of Pauli’s exclusion principle?

6 / 50

6. If , what is the only possible value of ?

7 / 50

7. Which orbital has no directional orientation in space?

8 / 50

8. The energy required to remove an electron from level of hydrogen atom is:

9 / 50

9. Which of the following is NOT a correct statement about orbitals?

10 / 50

10. Which of the following is not a property of cathode rays?

11 / 50

11. According to the uncertainty principle, increasing the accuracy of measuring a particle’s position will:

12 / 50

12. Which of the following statements about s-orbitals is correct?

13 / 50

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

14 / 50

14. Which statement about emission vs absorption for the same transition is correct?

15 / 50

15. Bohr’s model fails for heavier atoms because:

16 / 50

16. Which statement about electromagnetic waves is correct?

17 / 50

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

18 / 50

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

19 / 50

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

20 / 50

20. Which of the following species has the smallest radius?

21 / 50

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

22 / 50

22. The Schrödinger wave equation gives information about:

23 / 50

23. Which of the following is NOT a postulate of Bohr’s model?

24 / 50

24. Upon forming cations for first-row transition metals, electrons are removed first from:

25 / 50

25. If , how many orientations of orbitals are possible?

26 / 50

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

27 / 50

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

28 / 50

28. Which of the following quantum numbers decides the shape of an orbital?

29 / 50

29. What is the SI unit of wave number?

30 / 50

30. Pauli’s exclusion principle states that:

31 / 50

31. The orientation of p-orbitals in space is given by:

32 / 50

32. The maximum number of electrons that can occupy all five d-orbitals is:

33 / 50

33. Which of the following d-orbitals has a different shape compared to the others?

34 / 50

34. Which of the following transition metals also shows an anomalous configuration similar to copper?

35 / 50

35. The configuration [Ne] 3s² corresponds to:

36 / 50

36. Which of the following phenomena can be explained using the uncertainty principle?

37 / 50

37. In Schrödinger’s model, the mathematical function describes:

38 / 50

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

39 / 50

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

40 / 50

40. Which type of spectrum shows bright lines against a dark background?

41 / 50

41. What is the general shape of most d-orbitals?

42 / 50

42. What is meant by the term “spectrum” in physics?

43 / 50

43. How many p-orbitals exist in each shell where ?

44 / 50

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

45 / 50

45. For , how many subshells are present?

46 / 50

46. Which subshell is filled immediately after in the neutral-atom filling order?

47 / 50

47. Which experimental fact could not be explained by Bohr’s model?

48 / 50

48. Which subshell can accommodate a maximum of 14 electrons?

49 / 50

49. Which key observation of photoelectric effect contradicted classical wave theory?

50 / 50

50. In Rutherford’s gold foil experiment, what was the source of alpha particles?

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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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