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. In ionic bond formation, the role of lattice energy is:

2 / 30

2. Which pair illustrates the role of cation size in ionic bond strength, holding anion constant?

3 / 30

3. Which of the following correctly represents the formation of ammonium ion (NH₄⁺)?

4 / 30

4. Which best describes the difference between polar covalent and non-polar covalent bonds?

5 / 30

5. Which of the following molecules has electrons in antibonding orbitals?

6 / 30

6. Which of the following best describes diamagnetism?

7 / 30

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

8 / 30

8. Which factor makes hydrogen bonding in HF stronger than in NH₃?

9 / 30

9. Which rule helps predict the most stable structure of molecules?

10 / 30

10. Which of the following is a direct chemical consequence of hydrogen bonding?

11 / 30

11. In CH₄, the central carbon atom undergoes which type of hybridization?

12 / 30

12. The geometry of SF₆ is described as:

13 / 30

13. In H₂, the bonding molecular orbital is formed from:

14 / 30

14. Which molecule has an octahedral shape according to VSEPR theory?

15 / 30

15. Which of the following steps is involved in the formation of NaCl crystal from Na and Cl atoms?

16 / 30

16. What is the shape of BF₃ molecule as predicted by VSEPR theory?

17 / 30

17. Which molecular orbital has higher energy in diatomic molecules up to nitrogen (Z ≤ 7)?

18 / 30

18. Which of the following is true about the nodal plane in antibonding orbitals?

19 / 30

19. The formula for calculating bond order in Molecular Orbital Theory is:

20 / 30

20. Which of the following species has the shortest bond length?

21 / 30

21. Which of the following correctly represents the Lewis dot structure of N₂?

22 / 30

22. Which of the following chemical equations shows the amphoteric nature of Al₂O₃?

23 / 30

23. In the Born–Haber cycle, which of the following is calculated indirectly using Hess’s law?

24 / 30

24. Which of the following molecules does NOT obey the octet rule?

25 / 30

25. The octet rule states that atoms tend to:

26 / 30

26. Which of the following correctly shows the bond formation in CO molecule?

27 / 30

27. Why are sigma bonds stronger than pi bonds?

28 / 30

28. The bond order of F₂ molecule is:

29 / 30

29. The molecular geometry of H₂O according to sp³ hybridization is:

30 / 30

30. What is the bond order of O₂⁺ ion?

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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!

Earn a certificate upon passing

Get new questions with every attempt

  • Total Questions: 50
  • Time Allotted: 75 minutes
  • Passing Score: 70%
  • Randomization: Yes
  • Certificate: Yes
  • Retake: Allowed
  • Price: 100% Free

Good luck! 👍

1 / 50

1. In a Born–Haber cycle, the enthalpy of formation of an ionic solid equals:

2 / 50

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

3 / 50

3. Which of the following best defines hydrogen bonding?

4 / 50

4. Which factor increases bond enthalpy?

5 / 50

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

6 / 50

6. Which molecule has a square planar shape according to VSEPR theory?

7 / 50

7. Which of the following is a correct postulate of VSEPR theory?

8 / 50

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

9 / 50

9. Which of the following is the correct order of hydrogen bonding strength?

10 / 50

10. What is the bond order of N₂ molecule and how does it relate to its bond length?

11 / 50

11. In ionic bond formation, the role of lattice energy is:

12 / 50

12. What is the shape of BF₃ molecule as predicted by VSEPR theory?

13 / 50

13. In acetylene (C₂H₂), each carbon atom undergoes:

14 / 50

14. Which of the following bonds is formed due to sideways overlap of orbitals?

15 / 50

15. Which molecule has a bond angle of exactly 180°?

16 / 50

16. In BeCl₂, the central atom beryllium is:

17 / 50

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

18 / 50

18. Which of the following statements about sigma (σ) bonds is correct?

19 / 50

19. In covalent bonding, a single bond involves the sharing of:

20 / 50

20. Which is the correct formula to calculate bond order in Molecular Orbital Theory?

21 / 50

21. Which of the following molecules is paramagnetic?

22 / 50

22. When two atomic orbitals combine destructively in LCAO, the result is:

23 / 50

23. Why is the boiling point of ethanol higher than that of dimethyl ether, though both have the same molecular formula (C₂H₆O)?

24 / 50

24. In ethene (C₂H₄), the bond between two carbon atoms is:

25 / 50

25. Which equation shows the hydrogen bonding responsible for dimer formation of carboxylic acids?

26 / 50

26. Which property determines whether a molecule is paramagnetic or diamagnetic?

27 / 50

27. The stability order of the species B₂, B₂⁺, and B₂⁻ based on bond order is:

28 / 50

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

29 / 50

29. Which condition must be satisfied for two atomic orbitals to combine effectively under LCAO?

30 / 50

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

31 / 50

31. The geometry of PCl₅ according to sp³d hybridization is:

32 / 50

32. Which of the following species has the shortest bond length?

33 / 50

33. The bond angle in BeCl₂ according to hybridization is approximately:

34 / 50

34. What symbol is used to represent an antibonding molecular orbital?

35 / 50

35. In the case of Li₂ molecule (6 electrons), using LCAO, the bond order is:

36 / 50

36. In a triple bond (C≡C), the bonding consists of:

37 / 50

37. Which statement about the energy levels of bonding vs antibonding orbitals is correct?

38 / 50

38. The formula for calculating bond order in Molecular Orbital Theory is:

39 / 50

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

40 / 50

40. In NH₃, hydrogen bonding is weaker than in H₂O because:

41 / 50

41. Why does NaCl have a high melting point?

42 / 50

42. Which of the following species will be diamagnetic based on bond order?

43 / 50

43. Which of the following molecules is best represented by a Lewis structure showing a double bond?

44 / 50

44. Which species has the highest bond order and therefore the shortest bond length?

45 / 50

45. Which chemical equation correctly represents the formation of XeF₂?

46 / 50

46. The bond angle in CH₄ according to sp³ hybridization is:

47 / 50

47. The molecular geometry of SF₆ according to VSEPR and hybridization is:

48 / 50

48. The bond order of O₂⁺ ion is:

49 / 50

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

50 / 50

50. Which molecular orbital is lower in energy when two atomic orbitals overlap constructively?

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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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