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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. The electron dot structure of oxygen (O₂) shows how many shared pairs of electrons?

2 / 30

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

3 / 30

3. In acetylene (C₂H₂), the carbon–carbon triple bond consists of:

4 / 30

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

5 / 30

5. In the formation of an H₂ molecule, the type of overlap is:

6 / 30

6. Why does CH₄ have a tetrahedral shape with 109.5° bond angles?

7 / 30

7. According to VSEPR theory, the shape of CO₂ is:

8 / 30

8. Which of the following ionic compounds has the highest lattice enthalpy?

9 / 30

9. Which compound shows intramolecular hydrogen bonding?

10 / 30

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

11 / 30

11. A molecule with polar bonds may still be non-polar if:

12 / 30

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

13 / 30

13. Which species has the highest bond order?

14 / 30

14. The bond length of H–F (92 pm) is shorter than that of H–Cl (127 pm). This is mainly because:

15 / 30

15. According to MOT, bond order is given by the formula:

16 / 30

16. Which property is correctly associated with pi bonds?

17 / 30

17. The bond angles in PCl₅ are:

18 / 30

18. The lattice enthalpy of NaCl can be calculated using the Born–Haber cycle. Which of the following data is NOT required?

19 / 30

19. What is the bond order of O₂ molecule?

20 / 30

20. Which of the following factors increases lattice enthalpy?

21 / 30

21. Which molecule has a central atom with an expanded octet in its Lewis dot structure?

22 / 30

22. Why does H₂O exhibit extensive hydrogen bonding?

23 / 30

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

24 / 30

24. According to Valence Bond Theory, a covalent bond is formed when:

25 / 30

25. The bond angle in BF₃ is approximately:

26 / 30

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

27 / 30

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

28 / 30

28. Which reaction correctly represents the preparation of XeF₆?

29 / 30

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

30 / 30

30. Which reaction represents the lattice enthalpy of NaCl?

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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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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. According to VSEPR theory, the molecular shape of XeF₂ is:

2 / 50

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

3 / 50

3. Which of the following factors increases lattice enthalpy?

4 / 50

4. The lattice enthalpy of LiF is higher than that of LiI because:

5 / 50

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

6 / 50

6. The Lewis dot structure of CO₂ shows:

7 / 50

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

8 / 50

8. In the Lewis structure of CH₄, the central carbon atom is shown with:

9 / 50

9. According to MOT, which of the following species has the highest bond order?

10 / 50

10. What is the molecular shape of BF₃ according to VSEPR theory?

11 / 50

11. Which of the following molecules is represented in Lewis notation as containing a triple bond?

12 / 50

12. Which reaction correctly represents the preparation of XeF₆?

13 / 50

13. In F₂ molecule, the type of overlap responsible for bond formation is:

14 / 50

14. In a C=C double bond, how many sigma and pi bonds are present?

15 / 50

15. Which of the following compounds follows the octet rule completely?

16 / 50

16. Which of the following molecules is paramagnetic?

17 / 50

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

18 / 50

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

19 / 50

19. In the formation of an H₂ molecule, the type of overlap is:

20 / 50

20. Which molecule exhibits the weakest hydrogen bonding among H₂O, HF, and NH₃?

21 / 50

21. Which hybrid orbitals are formed when one s orbital mixes with two p orbitals?

22 / 50

22. According to Coulomb’s law, the strength of ionic attraction between two ions is directly proportional to:

23 / 50

23. Which best explains why noble gases are chemically inert?

24 / 50

24. Which property is correctly associated with pi bonds?

25 / 50

25. Which chemical equation corresponds to the hydrolysis of PCl₅?

26 / 50

26. Which of the following molecules is linear according to VSEPR theory?

27 / 50

27. Which of the following molecules shows sp hybridization?

28 / 50

28. Which of the following has the longest bond length?

29 / 50

29. Which compound forms the largest number of hydrogen bonds per molecule?

30 / 50

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

31 / 50

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

32 / 50

32. Which chemical equation represents the formation of ozone (O₃) from dioxygen?

33 / 50

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

34 / 50

34. Which one of the following pairs of elements forms an ionic compound by following octet rule?

35 / 50

35. Which of the following is an exception to the octet rule because it contains an odd number of valence electrons?

36 / 50

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

37 / 50

37. The energy difference between bonding and antibonding molecular orbitals depends mainly on:

38 / 50

38. What is the bond order of He₂ according to the molecular orbital energy-level diagram?

39 / 50

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

40 / 50

40. A covalent bond is called polar when:

41 / 50

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

42 / 50

42. Which of the following correctly represents the Lewis dot structure of oxygen (O₂)?

43 / 50

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

44 / 50

44. In SF₆, the sulfur atom undergoes:

45 / 50

45. Which chemical equation represents the formation of BeCl₂ molecule?

46 / 50

46. Considering Born–Lande equation , which change will most directly increase lattice energy in magnitude (more negative)?

47 / 50

47. Why is N₂ diamagnetic according to MOT?

48 / 50

48. Why does H₂O exhibit extensive hydrogen bonding?

49 / 50

49. Which statement explains why CaO has stronger ionic bonding than NaCl?

50 / 50

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

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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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