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

2 / 30

2. The orientation of an orbital in space is determined by:

3 / 30

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

4 / 30

4. Which transition produces the first line of the Balmer series?

5 / 30

5. Which scientist gave the photon explanation of the photoelectric effect?

6 / 30

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

7 / 30

7. The electronic configuration of chlorine (Z=17) is:

8 / 30

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

9 / 30

9. Which of the following phenomena is explained by particle nature of light?

10 / 30

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

11 / 30

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

12 / 30

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

13 / 30

13. Which element’s ground-state configuration demonstrates Hund’s rule?

14 / 30

14. Which experiment first gave evidence of electron spin?

15 / 30

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

16 / 30

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

17 / 30

17. Which radiation is most dangerous due to its high penetration power and ionizing ability?

18 / 30

18. What is an emission spectrum?

19 / 30

19. What is the charge on a neutron?

20 / 30

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

21 / 30

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

22 / 30

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

23 / 30

23. The electronic configuration of copper (Z=29) is:

24 / 30

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

25 / 30

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

26 / 30

26. The maximum number of electrons that can be accommodated in a shell with principal quantum number is:

27 / 30

27. Which subatomic particle has the least mass?

28 / 30

28. The uncertainty in the position of an electron is . What is the minimum uncertainty in its momentum (h = )?

29 / 30

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

30 / 30

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

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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. What is the value of Planck’s constant ?

2 / 50

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

3 / 50

3. The line spectrum of hydrogen is due to:

4 / 50

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

5 / 50

5. The hydrogen emission spectrum is an example of:

6 / 50

6. Which statement about Schrödinger’s wave equation is correct?

7 / 50

7. The electronic configuration of chlorine (Z=17) is:

8 / 50

8. Which relation is correct for photon momentum?

9 / 50

9. Which unit combination correctly represents frequency?

10 / 50

10. Which subatomic particle has the least mass?

11 / 50

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

12 / 50

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

13 / 50

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

14 / 50

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

15 / 50

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

16 / 50

16. The principal quantum number () primarily describes:

17 / 50

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

18 / 50

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

19 / 50

19. In the photoelectric effect, electrons are emitted from a metal surface when:

20 / 50

20. The electronic configuration of silver (Z=47) is anomalous and written as:

21 / 50

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

22 / 50

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

23 / 50

23. The maximum number of electrons that can be accommodated in a shell with principal quantum number is:

24 / 50

24. What is the SI unit of wave number?

25 / 50

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

26 / 50

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

27 / 50

27. What is the relative charge of a proton compared to an electron?

28 / 50

28. Who discovered the neutron?

29 / 50

29. If the wavelength of a wave is doubled, its frequency (in vacuum):

30 / 50

30. Which orbital has a spherical shape around the nucleus?

31 / 50

31. The number of angular and radial nodes in a 4p orbital are:

32 / 50

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

33 / 50

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

34 / 50

34. The effective nuclear charge experienced by a 2p electron in oxygen atom (Z=8) using Slater’s rules is approximately:

35 / 50

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

36 / 50

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

37 / 50

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

38 / 50

38. Which subshell fills earlier on the basis of the rule (use tie-breaker if needed): or ?

39 / 50

39. The configuration [Ne] 3s² 3p⁵ corresponds to which element?

40 / 50

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

41 / 50

41. Sodium (Z=11) has which electronic configuration?

42 / 50

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

43 / 50

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

44 / 50

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

45 / 50

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

46 / 50

46. What is the condition for allowed orbits in Bohr’s theory?

47 / 50

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

48 / 50

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

49 / 50

49. The Balmer series of hydrogen corresponds to transitions ending at:

50 / 50

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

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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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