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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. Which quantum number determines the shape of an orbital?

2 / 30

2. What is the relative mass of a proton compared to an electron?

3 / 30

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

4 / 30

4. The possible values of the spin quantum number () are:

5 / 30

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

6 / 30

6. The Rydberg formula for hydrogen spectral lines is:

7 / 30

7. Which comparison is correct regarding Thomson vs. Rutherford models?

8 / 30

8. Which factor does not affect the kinetic energy of emitted photoelectrons?

9 / 30

9. Which of the following statements about the uncertainty principle is incorrect?

10 / 30

10. What conclusion did Thomson draw from cathode ray experiments?

11 / 30

11. Which statement best summarizes the limitation of Bohr’s theory?

12 / 30

12. Which limitation of Bohr’s model was later resolved by quantum mechanics?

13 / 30

13. What is the mass of a proton?

14 / 30

14. What is the mass of a neutron compared to a proton?

15 / 30

15. The magnetic quantum number () signifies:

16 / 30

16. Microwaves are commonly used in:

17 / 30

17. Which model introduced the concept of atomic orbitals instead of fixed orbits?

18 / 30

18. Why is copper (Z=29) an exception to the normal Aufbau filling?

19 / 30

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

20 / 30

20. The principal quantum number () primarily describes:

21 / 30

21. In Bohr’s model, the energy of the orbit of hydrogen is given by:

22 / 30

22. Which shell corresponds to ?

23 / 30

23. Which electromagnetic theory of light was given by Maxwell?

24 / 30

24. The Lyman series of hydrogen spectral lines lies in which region of the electromagnetic spectrum?

25 / 30

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

26 / 30

26. Which principle is directly related to the spin quantum number?

27 / 30

27. Which statement correctly defines an orbital?

28 / 30

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

29 / 30

29. Who discovered the neutron?

30 / 30

30. Which sequence correctly lists the filling order up 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. Which model introduced the concept of atomic orbitals instead of fixed orbits?

2 / 50

2. The principal quantum number () signifies:

3 / 50

3. According to Bohr, when is radiation emitted or absorbed by an atom?

4 / 50

4. Which subatomic particle orbits outside the nucleus?

5 / 50

5. The magnitude of orbital angular momentum for a given is:

6 / 50

6. According to de Broglie, the wavelength of a particle is given by:

7 / 50

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

8 / 50

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

9 / 50

9. The general formula for hydrogen spectral series is:

10 / 50

10. What kind of spectrum is produced when white light passes through a cold gas before entering a spectroscope?

11 / 50

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

12 / 50

12. How many radial nodes does the 3s orbital have?

13 / 50

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

14 / 50

14. For , how many subshells are present?

15 / 50

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

16 / 50

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

17 / 50

17. The magnetic quantum number () signifies:

18 / 50

18. Heisenberg’s uncertainty principle is a direct consequence of:

19 / 50

19. The maximum number of electrons in a p-subshell is:

20 / 50

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

21 / 50

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

22 / 50

22. Which of the following quantum numbers emerge from solving Schrödinger’s equation for the hydrogen atom?

23 / 50

23. The electronic configuration of chromium (Z=24) is anomalous because it is:

24 / 50

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

25 / 50

25. Which rule is based directly on quantum numbers to fill atomic orbitals?

26 / 50

26. What is the SI unit of wave number?

27 / 50

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

28 / 50

28. Which statement about electromagnetic waves is correct?

29 / 50

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

30 / 50

30. According to the rule, which orbital fills before ?

31 / 50

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

32 / 50

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

33 / 50

33. Stable electronic configurations are generally associated with:

34 / 50

34. The hydrogen emission spectrum is an example of:

35 / 50

35. For an atom with embedded electrons in Thomson’s model, which expresses charge neutrality?

36 / 50

36. Which relation is correct between frequency and time period ?

37 / 50

37. Which of the following is NOT correct about p-orbitals?

38 / 50

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

39 / 50

39. The allowed magnetic quantum numbers for are:

40 / 50

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

41 / 50

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

42 / 50

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

43 / 50

43. The probability distribution of a p-orbital is:

44 / 50

44. The frequency of radiation emitted when an electron in hydrogen atom jumps from to is approximately:

45 / 50

45. What is the mass of a proton?

46 / 50

46. Which of the following is a correct implication of the uncertainty principle?

47 / 50

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

48 / 50

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

49 / 50

49. The ground-state electronic configuration of lithium (Z=3) is:

50 / 50

50. Who first proposed the concept of atom as an indivisible particle?

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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.
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