Exam-Style Online Test | Class 11: Chemical Bonding Test

Class 11 Chemistry — Chapter 4: Chemical Bonding and Molecular Structure Online Test

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Class 11 Chemistry: Chemical Bonding and Molecular Structure 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

Good luck! 👍

1 / 20

1. Which reaction correctly represents the preparation of XeF₆?

2 / 20

2. Which chemical equation represents the preparation of PCl₅, an sp³d hybridized molecule?

3 / 20

3. Which equation corresponds to the formation of a π bond in ethene (C₂H₄)?

4 / 20

4. Why do HF molecules form zig-zag chains in the solid state?

5 / 20

5. Which of the following best describes intermolecular hydrogen bonding?

6 / 20

6. What is the bond order of H₂⁺ ion?

7 / 20

7. Which of the following molecules is paramagnetic according to MOT?

8 / 20

8. Which geometry is predicted by sp³ hybridization when there are no lone pairs?

9 / 20

9. Which of the following molecules has both sigma and pi bonds?

10 / 20

10. The bond between two carbon atoms in C₂H₄ (ethene) contains:

11 / 20

11. The molecular geometry of NH₃ is:

12 / 20

12. Which oxygen species has the weakest O–O bond?

13 / 20

13. The bond angle in methane (CH₄) is approximately:

14 / 20

14. In H₂O, the Lewis structure shows oxygen atom with:

15 / 20

15. In aqueous solution, which pair most likely dissociates more due to weaker effective ionic attraction after solvation (hydration)?

16 / 20

16. Chlorine forms Cl⁻ ion because:

17 / 20

17. Which molecule is best represented by a resonance structure in Lewis notation?

18 / 20

18. The bond length order among single, double, and triple bonds of the same atoms is:

19 / 20

19. The bond enthalpy of O=O is less than that of N≡N because:

20 / 20

20. The shape of H₂O molecule is best described as:

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Class 11 Chemistry: Chemical Bonding and Molecular Structure 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.

Get new questions on each attempt

  • 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 does BF₃ violate the octet rule?

2 / 30

2. Which of the following correctly matches the molecule with its geometry?

3 / 30

3. In sp³ hybridization, the number of equivalent hybrid orbitals formed is:

4 / 30

4. Which statement explains why proteins and DNA depend on hydrogen bonding for their structure?

5 / 30

5. The reduction in bond angle from 109.5° in CH₄ to 104.5° in H₂O is due to:

6 / 30

6. When two atomic orbitals combine constructively in LCAO, the result is:

7 / 30

7. Which of the following is the correct bond angle in H₂O?

8 / 30

8. Which molecule exhibits stronger hydrogen bonding: NH₃ or H₂O?

9 / 30

9. Which molecule is expected to form the strongest hydrogen bond?

10 / 30

10. Which of the following is a limitation of VBT regarding orbital overlap?

11 / 30

11. The key difference between bonding and antibonding molecular orbitals is:

12 / 30

12. Which of the following molecules violates the octet rule?

13 / 30

13. Which of the following steps contributes negatively (exothermic) in the Born–Haber cycle for NaCl?

14 / 30

14. The bond angle in NH₃ is smaller than in CH₄ because:

15 / 30

15. Which of the following molecules contains a non-polar covalent bond?

16 / 30

16. Which of the following bonds is the most polar?

17 / 30

17. The shape of H₂O molecule is best described as:

18 / 30

18. In BeCl₂, the central atom beryllium is:

19 / 30

19. Which equation shows the formation of O₂ molecule according to Molecular Orbital Theory?

20 / 30

20. Which reaction illustrates the hydrogen bonding in carboxylic acids?

21 / 30

21. What is the hybridization of the central atom in XeF₂, and what is its molecular shape?

22 / 30

22. Which type of hydrogen bonding increases the volatility of a compound?

23 / 30

23. Lattice enthalpy of an ionic compound is defined as:

24 / 30

24. Which factor increases bond enthalpy?

25 / 30

25. The octet rule states that atoms tend to:

26 / 30

26. Which of the following statements about sp hybridization is true?

27 / 30

27. Which of the following shows the resonance structures of carbonate ion?

28 / 30

28. Which of the following symbols represents an antibonding orbital?

29 / 30

29. The geometry of IF₇ is described as:

30 / 30

30. Which statement about O₂ is correct according to its MO diagram?

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Class 11 Chemistry: Chemical Bonding and Molecular Structure 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 of the following molecules has both sigma and pi bonds?

2 / 50

2. A molecule with bond order 0 according to MOT will be:

3 / 50

3. In BeCl₂, the central atom beryllium is:

4 / 50

4. Which of the following species is diamagnetic according to MO theory?

5 / 50

5. In NH₃, the shape is not perfectly tetrahedral but:

6 / 50

6. Which of the following steps contributes negatively (exothermic) in the Born–Haber cycle for NaCl?

7 / 50

7. Which trend correctly matches bond order, bond length, and bond enthalpy?

8 / 50

8. Which of the following factors increases lattice enthalpy?

9 / 50

9. The bond order of N₂ molecule is:

10 / 50

10. Which molecule has a triple bond in its Lewis structure?

11 / 50

11. The bond enthalpy of O=O is less than that of N≡N because:

12 / 50

12. Which of the following correctly matches species with its magnetic property?

13 / 50

13. Which equation shows the formation of O₂ molecule according to Molecular Orbital Theory?

14 / 50

14. In the Lewis dot structure of BeCl₂, the central atom beryllium has how many electrons?

15 / 50

15. Which factor explains why CO has a shorter bond length than CO₂?

16 / 50

16. Which chemical equation represents the bond dissociation enthalpy of oxygen?

17 / 50

17. Which of the following molecules is polar?

18 / 50

18. Which of the following statements about sp hybridization is true?

19 / 50

19. Which noble gas configuration is usually achieved through the octet rule?

20 / 50

20. In MOT, how many molecular orbitals are formed when two atomic orbitals combine?

21 / 50

21. The bond order of F₂ molecule is:

22 / 50

22. Which reaction illustrates the hydrogen bonding in carboxylic acids?

23 / 50

23. Which of the following correctly represents the disproportionation of chlorine in water?

24 / 50

24. Which hydrogen-bonded system explains why DNA strands are held together?

25 / 50

25. Which of the following compounds will have the lowest boiling point due to intramolecular hydrogen bonding?

26 / 50

26. Which of the following bonds has the highest bond enthalpy?

27 / 50

27. Why is the bond angle in H₂O smaller than that in NH₃?

28 / 50

28. Why does HF have a much higher boiling point than HCl, HBr, and HI?

29 / 50

29. The strength order of bonds (same atoms) is:

30 / 50

30. Why is N₂ diamagnetic according to MOT?

31 / 50

31. Which of the following explains why glycerol (C₃H₅(OH)₃) is highly viscous?

32 / 50

32. Which of the following best describes the limitation of the octet rule?

33 / 50

33. Which of the following correctly represents the electron transfer in the formation of CaCl₂?

34 / 50

34. For two isoelectronic salts with monovalent ions, which factor most strongly reduces ionic bond strength?

35 / 50

35. The presence of a node between two nuclei is characteristic of:

36 / 50

36. Which type of bond is formed by complete transfer of electrons?

37 / 50

37. Which of the following correctly pairs LCAO results?

38 / 50

38. Which of the following is a consequence of hydrogen bonding in liquids?

39 / 50

39. The Lewis dot structure of carbonate ion (CO₃²⁻) requires how many valence electrons in total?

40 / 50

40. Why is B₂ paramagnetic?

41 / 50

41. Which reaction represents the lattice enthalpy of NaCl?

42 / 50

42. In which of the following molecules does the central atom have less than 8 electrons?

43 / 50

43. Which molecule is paramagnetic according to MO theory but wrongly predicted as diamagnetic by VBT?

44 / 50

44. Which molecule cannot be represented fully by a single Lewis structure but requires resonance structures?

45 / 50

45. Why is ice less dense than liquid water?

46 / 50

46. Which of the following correctly matches the molecule with its predicted geometry?

47 / 50

47. Why is NH₃ less strongly hydrogen-bonded than H₂O?

48 / 50

48. Which of the following explains the higher boiling point of NH₃ compared to PH₃?

49 / 50

49. What is the hybridization of the central atom in XeF₂, and what is its molecular shape?

50 / 50

50. Which equation relates lattice enthalpy to enthalpies of other processes in an ionic solid?

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Practice Chemical Bonding and Molecular Structure MCQs
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Class 11 Chemistry — Chapter 4: Chemical Bonding and Molecular Structure Online Test

The Class 11 Chemistry: Chapter 4 — Chemical Bonding and Molecular Structure Online Test offers a comprehensive pool of 395 MCQs designed to assess your understanding of the fundamental concepts in Chemical Bonding. This test is free, CBSE/NCERT-aligned, and is perfect for students preparing for exams. You can practice timed MCQs, see your result instantly, review answers, and—if you pass Paper 3—download a certificate. It’s an excellent way to prepare for both school exams and competitive tests like JEE and NEET.

Struggling with types of chemical bonds, Lewis structures, or VSEPR theory? Don’t worry, this page is your safe space to practice Chemical Bonding concepts at your own pace. Think of it like a small online mock test you can take at home, on your phone or laptop. Every attempt is a quick online exam with objective questions, providing you with immediate feedback. Each retake will help you understand the core concepts better. When you’re ready, attempt Paper 3 and earn a certificate. Let’s get started on your Chemistry journey!

What is this Class 11 Chemistry: Chemical Bonding and Molecular Structure Online Test?

This page contains three exam-style MCQ papers for Chapter 4:

  • 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 ~395 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 answer review.

Topics covered in these online tests

The online tests are designed to assess your understanding of key concepts from Chapter 4: Chemical Bonding and Molecular Structure. You will practice the following topics:

  • Nature of Chemical Bonds — ionic bonds, covalent bonds, and coordinate covalent bonds
  • Lewis Structures — drawing Lewis structures, octet rule, and resonance structures
  • Valence Shell Electron Pair Repulsion (VSEPR) Theory — predicting molecular geometry and bond angles
  • Hybridization — sp, sp², sp³ hybridization and their implications in bonding and geometry
  • Molecular Orbital Theory — bonding and anti-bonding orbitals, energy-level diagrams
  • Bonding in Solids — ionic solids, covalent solids, metallic solids, and molecular solids
  • Polarity of Molecules — dipole moment, molecular polarity and its relation to geometry
  • Intermolecular Forces — hydrogen bonding, van der Waals forces, and dipole-dipole interactions
  • Bond Order — calculation and significance of bond order in molecular stability
  • Anomalous Properties of Water — high boiling point, surface tension, and solubility effects

For more detailed practice, explore: Chemical Bonding and Molecular Structure MCQs and the full Class 11 Chemistry MCQ Question Bank.

How This Exam-Style Online Test Works

Short version: Pick a paper → answer MCQs within time → submit → get instant score and review. Pass Paper 3 to get a certificate.

What you’ll see during the test

  • MCQs: One question with four options (A, B, C, D).
  • Timer on top: P1: 30 min • P2: 45 min • P3: 75 min.
  • Pagination: Typically 10 questions per page (move to next group using page controls).
  • Navigation: Use Next/Prev buttons or question map to revisit before submitting.
  • View Result: Click View Result to see marks and detailed summary.
  • Result page shows: score %, correct / incorrect / unanswered count, answer-key/review, and share options.
  • Restart: Click Restart Test to try again with a new mix of questions (P2 & P3).

Note: Please share your feedback on the result page after completing a test.

Marking & pass criteria

  • Scoring: +1 for correct, 0 for incorrect (no negative marking).
  • Passing marks: Paper 1 — 40% • Paper 2 — 50% • Paper 3 — 70%.
  • Randomization: Paper 2 & 3 shuffle questions from a large Chapter 4 question pool on every attempt; Paper 1 stays fixed.

Who can take this test?

  • CBSE Class 11 students revising Chapter 4 (Chemical Bonding and Molecular Structure).
  • Class 12 bridge / revision learners who want to improve their understanding of bonding concepts.
  • JEE/NEET foundation aspirants building strong command over chemical bonding concepts.
  • Teachers / tutors needing ready-made chapter tests for assignments and quizzes.
  • Students from other boards & countries who want extra practice on bonding and molecular structure topics.
  • Competitive exam aspirants revising core concepts of Chemical Bonding and Molecular Structure.

Advantages of this online test

  • Real exam feel: timer, pass %, and auto-submit on time out.
  • Instant feedback: get your score, see correct answers, and spot weak areas immediately.
  • Step-up difficulty: Easy → Mixed → Challenge (+ certificate on Paper 3).
  • Unlimited attempts: practice till perfect; fresh randomized sets in Paper 2 & 3.
  • Zero cost & safe: completely free; no payment, no signup required.

How this test helps you study better

Use this simple plan for Chapter 4:

  • Step 1 – Concept check: Attempt Paper 1 after studying the chapter. Note weak sub-topics (e.g., VSEPR theory, hybridization).
  • Step 2 – Reinforce: Attempt Paper 2 (randomized) to stabilize accuracy in bonding and structure concepts.
  • Step 3 – Exam readiness: Attempt Paper 3 strictly within time. Target ≥ 70% and earn the certificate.
  • Step 4 – Review: Read solutions carefully, maintain a short error-log notebook, revise only missed ideas.
  • Step 5 – Retake smartly: Re-attempt after 1–2 days to test long-term recall and real improvement.

Important notes (read before you start)

  • Do not refresh / close the tab during the test.
  • Best experience: latest Chrome/Edge, stable internet, distraction-free screen.
  • Allow cookies / local storage so your progress and settings work smoothly.
  • Safety: This test is 100% FREE. Ignore any payment or login requests.

More practice for Class 11 Chemistry

After finishing this online test, strengthen your Chemistry further: visit the full Class 11 Chemistry Online Test Index or practice all chapters from the Class 11 Chemistry MCQ Collection.

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