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

2 / 30

2. The bond angle in NH₄⁺ ion is:

3 / 30

3. Which hybridization and geometry are shown in XeF₄?

4 / 30

4. The difference between the geometry of SF₆ and IF₇ is:

5 / 30

5. Which of the following best describes diamagnetism?

6 / 30

6. The molecular geometry of NH₃ is:

7 / 30

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

8 / 30

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

9 / 30

9. Why is the extent of overlap important in VBT?

10 / 30

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

11 / 30

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

12 / 30

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

13 / 30

13. Which of the following molecules is predicted by VSEPR theory to have a trigonal planar geometry?

14 / 30

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

15 / 30

15. In the formation of H₂ molecule, the type of orbital overlap is:

16 / 30

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

17 / 30

17. The bond order of O₂⁺ ion is:

18 / 30

18. Which molecule shows the strongest hydrogen bonding among H₂O, NH₃, and HF?

19 / 30

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

20 / 30

20. Which is the bond angle in BF₃?

21 / 30

21. Sodium forms Na⁺ ion because:

22 / 30

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

23 / 30

23. In MgO, how do magnesium and oxygen achieve octet?

24 / 30

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

25 / 30

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

26 / 30

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

27 / 30

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

28 / 30

28. Which property is strongly influenced by molecular polarity?

29 / 30

29. Which of the following is an exception to the octet rule due to odd number of electrons?

30 / 30

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

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

2 / 50

2. Bond enthalpy is defined as:

3 / 50

3. In BeCl₂, why does Be undergo sp hybridization?

4 / 50

4. Which of the following is the best example of ionic bond formation?

5 / 50

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

6 / 50

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

7 / 50

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

8 / 50

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

9 / 50

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

10 / 50

10. Which of the following factors increases lattice enthalpy?

11 / 50

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

12 / 50

12. Which statement best describes a chemical bond?

13 / 50

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

14 / 50

14. Which of the following molecules has a correct Lewis dot structure showing a lone pair on the central atom?

15 / 50

15. The geometry of PCl₅ as predicted by VSEPR theory is:

16 / 50

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

17 / 50

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

18 / 50

18. The presence of electrons in antibonding orbitals:

19 / 50

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

20 / 50

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

21 / 50

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

22 / 50

22. Which of the following metals is most likely to form an ionic bond with oxygen?

23 / 50

23. Why are sigma bonds stronger than pi bonds?

24 / 50

24. In LCAO, the number of molecular orbitals formed is always:

25 / 50

25. Which type of overlap forms the strongest bond according to VBT?

26 / 50

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

27 / 50

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

28 / 50

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

29 / 50

29. Why is ice less dense than liquid water?

30 / 50

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

31 / 50

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

32 / 50

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

33 / 50

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

34 / 50

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

35 / 50

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

36 / 50

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

37 / 50

37. Which best describes the occupancy of bonding and antibonding orbitals in O₂?

38 / 50

38. Which of the following molecules contains both single and double bonds?

39 / 50

39. The geometry of SF₆ is described as:

40 / 50

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

41 / 50

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

42 / 50

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

43 / 50

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

44 / 50

44. Why does H₂O exhibit extensive hydrogen bonding?

45 / 50

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

46 / 50

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

47 / 50

47. Which of the following correctly pairs LCAO results?

48 / 50

48. Which has the lowest bond enthalpy among the following?

49 / 50

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

50 / 50

50. Which of the following is an exception to the octet rule due to expanded octet?

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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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