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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 comparison is correct regarding Thomson vs. Rutherford models?

2 / 30

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

3 / 30

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

4 / 30

4. Which transition produces the shortest wavelength line in a hydrogen series?

5 / 30

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

6 / 30

6. The value of is associated with:

7 / 30

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

8 / 30

8. The Paschen series corresponds to transitions of electrons ending at:

9 / 30

9. Which type of electromagnetic wave is mainly responsible for sunburn?

10 / 30

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

11 / 30

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

12 / 30

12. The allowed magnetic quantum numbers for are:

13 / 30

13. What was the key observation from Rutherford’s gold foil experiment?

14 / 30

14. What type of radiation was observed in Chadwick’s experiment that proved the existence of neutrons?

15 / 30

15. Which species has the same electronic configuration as helium?

16 / 30

16. Which statement correctly defines an orbital?

17 / 30

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

18 / 30

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

19 / 30

19. The Paschen series of hydrogen lies in which region of the electromagnetic spectrum?

20 / 30

20. In Bohr’s atomic model, an orbit refers to:

21 / 30

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

22 / 30

22. The degeneracy of the energy level with in hydrogen atom is:

23 / 30

23. Why was the discovery of the neutron important?

24 / 30

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

25 / 30

25. The values of indicate:

26 / 30

26. Which subatomic particle is positively charged?

27 / 30

27. Which subatomic particle contributes to both the mass and stability of the nucleus but not to the atomic number?

28 / 30

28. Which subatomic particle defines isotopes of an element?

29 / 30

29. What is the shape of an s-orbital?

30 / 30

30. The electron density in an s-orbital is maximum at:

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

2 / 50

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

3 / 50

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

4 / 50

4. The frequency of visible light of wavelength 600 nm is approximately:

5 / 50

5. Which of the following statements about orbitals is correct?

6 / 50

6. Which particle has no charge but nearly the same mass as a proton?

7 / 50

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

8 / 50

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

9 / 50

9. The configuration [Kr] 5s² 4d¹⁰ 5p⁵ corresponds to:

10 / 50

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

11 / 50

11. Which is NOT a characteristic of orbitals?

12 / 50

12. The Paschen series of hydrogen lies in which region of the electromagnetic spectrum?

13 / 50

13. Which of the following could not be justified by Bohr’s model?

14 / 50

14. The concept of standing electron waves inside the atom was used by:

15 / 50

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

16 / 50

16. Which equation represents the condition for constructive interference in a double-slit experiment?

17 / 50

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

18 / 50

18. Hund’s rule of maximum multiplicity states that:

19 / 50

19. Who discovered the neutron?

20 / 50

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

21 / 50

21. In Bohr’s theory, electrons revolve in orbits because:

22 / 50

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

23 / 50

23. How does increasing gas pressure typically affect spectral lines (emission or absorption)?

24 / 50

24. In quantum mechanics, an orbital is defined as:

25 / 50

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

26 / 50

26. Which orbital is non-spherical in shape and has 3 orientations?

27 / 50

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

28 / 50

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

29 / 50

29. The ratio of velocities of electron in 2nd and 4th orbits of hydrogen atom is:

30 / 50

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

31 / 50

31. If a photon has wavelength , its energy is approximately:

32 / 50

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

33 / 50

33. The probability distribution of electrons in an s-orbital depends on:

34 / 50

34. Which type of electromagnetic wave is mainly responsible for sunburn?

35 / 50

35. Which letter notation corresponds to ?

36 / 50

36. The ionization energy of He⁺ ion is:

37 / 50

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

38 / 50

38. Which formula represents the condition for allowed electron orbits according to de Broglie?

39 / 50

39. What is the value of Planck’s constant ?

40 / 50

40. If an electron is in shell, it is in which orbital?

41 / 50

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

42 / 50

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

43 / 50

43. The wave–particle duality of electron means:

44 / 50

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

45 / 50

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

46 / 50

46. Which observation supported that most of the atom is empty space?

47 / 50

47. Which of the following best explains the difference between orbit and orbital?

48 / 50

48. Which principle explains the interference of light waves?

49 / 50

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

50 / 50

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

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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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