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

2 / 30

2. Which of the following molecules cannot be explained satisfactorily by Valence Bond Theory but is explained by Molecular Orbital Theory?

3 / 30

3. Which observation provided strong experimental support for MOT over VBT?

4 / 30

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

5 / 30

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

6 / 30

6. In the Lewis dot structure of H₂O, how many lone pairs are present on the oxygen atom?

7 / 30

7. In BeCl₂, the central atom beryllium is:

8 / 30

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

9 / 30

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

10 / 30

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

11 / 30

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

12 / 30

12. Which of the following molecules contains only single covalent bonds?

13 / 30

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

14 / 30

14. A double bond consists of:

15 / 30

15. Which is the limitation of the Lewis dot structure representation?

16 / 30

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

17 / 30

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

18 / 30

18. Which of the following statements about bond order is correct?

19 / 30

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

20 / 30

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

21 / 30

21. Which of the following statements correctly relates bond order with bond length?

22 / 30

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

23 / 30

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

24 / 30

24. The bond order of O₂⁺ ion is:

25 / 30

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

26 / 30

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

27 / 30

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

28 / 30

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

29 / 30

29. Which trend correctly ranks the expected lattice energy (highest to lowest) for halides of Li⁺?

30 / 30

30. Which molecule involves s–p overlap in bond formation?

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

2 / 50

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

3 / 50

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

4 / 50

4. Which overlap is present in the N–H bond of NH₃?

5 / 50

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

6 / 50

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

7 / 50

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

8 / 50

8. Which of the following best describes diamagnetism?

9 / 50

9. In SF₆, the sulfur atom undergoes:

10 / 50

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

11 / 50

11. Lattice enthalpy is most useful for predicting:

12 / 50

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

13 / 50

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

14 / 50

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

15 / 50

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

16 / 50

16. Which type of hydrogen bonding is present in HF?

17 / 50

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

18 / 50

18. Which pair is expected to have the strongest ionic bond (highest lattice energy), assuming the same crystal type?

19 / 50

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

20 / 50

20. Which of the following molecules is paramagnetic according to its MO diagram?

21 / 50

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

22 / 50

22. Which of the following best describes the shape of H₂O according to VSEPR theory?

23 / 50

23. In BeCl₂, the central atom beryllium is:

24 / 50

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

25 / 50

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

26 / 50

26. Which of the following pairs correctly illustrates both types of hydrogen bonding?

27 / 50

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

28 / 50

28. Which fundamental force is responsible for chemical bonding?

29 / 50

29. Which molecule among the following violates the octet rule by having an odd number of electrons?

30 / 50

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

31 / 50

31. What is the bond order of the superoxide ion, O₂⁻, according to Molecular Orbital Theory?

32 / 50

32. Which reaction represents the formation of the peroxide ion?

33 / 50

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

34 / 50

34. Which principle forms the basis of Molecular Orbital Theory (MOT)?

35 / 50

35. Which molecule shows incomplete octet in the central atom?

36 / 50

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

37 / 50

37. Which statement best describes a chemical bond?

38 / 50

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

39 / 50

39. Which of the following best explains why covalent bond formation is exothermic?

40 / 50

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

41 / 50

41. Which of the following molecules is predicted to be unstable by MO theory?

42 / 50

42. Which orbitals overlap in the bond formation of Cl₂ molecule?

43 / 50

43. Which reaction represents the lattice enthalpy of NaCl?

44 / 50

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

45 / 50

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

46 / 50

46. Intermolecular hydrogen bonding is mainly responsible for:

47 / 50

47. Which of the following species has the highest bond order?

48 / 50

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

49 / 50

49. Which equation shows the formation of ammonium chloride through acid–base reaction?

50 / 50

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

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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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