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. Which has the lowest bond enthalpy among the following?

2 / 30

2. Which of the following properties is directly affected by the number of bonds (single, double, triple) between atoms?

3 / 30

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

4 / 30

4. The Lewis representation of NH₃ shows nitrogen with:

5 / 30

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

6 / 30

6. Chlorine forms Cl⁻ ion because:

7 / 30

7. In methane (CH₄), the H–C–H bond angle is:

8 / 30

8. What conclusion can be drawn if the experimental lattice enthalpy differs significantly from the calculated Born–Lande value?

9 / 30

9. In SF₆, the sulfur atom undergoes:

10 / 30

10. Which of the following molecules has a bent geometry according to VSEPR theory?

11 / 30

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

12 / 30

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

13 / 30

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

14 / 30

14. Which of the following molecules is an exception to the octet rule due to an incomplete octet?

15 / 30

15. Which property is correctly associated with pi bonds?

16 / 30

16. Rotation around a C=C double bond is restricted because:

17 / 30

17. Why does H₂O exhibit extensive hydrogen bonding?

18 / 30

18. The bond angle in SF₆ is:

19 / 30

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

20 / 30

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

21 / 30

21. Why does BF₃ violate the octet rule?

22 / 30

22. In bonding orbitals, the wave functions of atomic orbitals combine:

23 / 30

23. Bond length in a covalent bond is defined as:

24 / 30

24. According to MO theory, N₂ has:

25 / 30

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

26 / 30

26. Which type of overlap is stronger?

27 / 30

27. According to MOT, the correct molecular orbital configuration for H₂ is:

28 / 30

28. Why does ice float on water?

29 / 30

29. Which ion has higher magnetic moment due to unpaired electrons?

30 / 30

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

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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 property is correctly associated with pi bonds?

2 / 50

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

3 / 50

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

4 / 50

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

5 / 50

5. The Lewis dot structure of CO₂ shows:

6 / 50

6. What is the shape of SF₆ molecule?

7 / 50

7. Which property of water is primarily due to hydrogen bonding?

8 / 50

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

9 / 50

9. Why does HF exhibit higher viscosity than HCl, HBr, or HI?

10 / 50

10. The presence of electrons in antibonding orbitals:

11 / 50

11. Which of the following chemical equations shows intramolecular hydrogen bonding?

12 / 50

12. During ionic bond formation, the energy released when an electron is added to a gaseous atom is called:

13 / 50

13. The octet rule states that atoms tend to:

14 / 50

14. Which of the following relationships is correct between bond order, bond length, and bond enthalpy?

15 / 50

15. In PCl₅, the central phosphorus atom undergoes which type of hybridization?

16 / 50

16. In VSEPR theory, double and triple bonds are treated as:

17 / 50

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

18 / 50

18. In NH₃, the bond angle is slightly less than tetrahedral because:

19 / 50

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

20 / 50

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

21 / 50

21. In the Lewis representation of a covalent bond, a shared pair of electrons between two atoms is shown as:

22 / 50

22. Which of the following correctly represents the decreasing order of bond angle?

23 / 50

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

24 / 50

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

25 / 50

25. The lattice enthalpy of NaCl is calculated to be about −787 kJ mol⁻¹. This high value indicates:

26 / 50

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

27 / 50

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

28 / 50

28. Why is the octet rule not strictly applicable to transition elements?

29 / 50

29. Which of the following molecules is an exception to the octet rule due to an incomplete octet?

30 / 50

30. Why does water have an unusually high boiling point compared to H₂S?

31 / 50

31. In SF₆, the sulfur atom undergoes:

32 / 50

32. Which of the following molecules is diamagnetic?

33 / 50

33. What is the electron-pair geometry of H₂O according to VSEPR theory?

34 / 50

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

35 / 50

35. The bond angle in BF₃ is approximately:

36 / 50

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

37 / 50

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

38 / 50

38. Which ion has higher magnetic moment due to unpaired electrons?

39 / 50

39. Which factor is essential for an element to act as a cation in ionic bond formation?

40 / 50

40. Which of the following correctly represents the process for defining lattice enthalpy of NaCl?

41 / 50

41. The shape of BeCl₂ molecule is:

42 / 50

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

43 / 50

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

44 / 50

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

45 / 50

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

46 / 50

46. Which of the following factors increases lattice enthalpy?

47 / 50

47. Which compound is an example of an expanded octet?

48 / 50

48. In the Lewis representation, coordinate covalent bonds are shown as:

49 / 50

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

50 / 50

50. The Linear Combination of Atomic Orbitals (LCAO) approach states that:

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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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