Exam-Style Online Test | 11 Chemistry: P-Block Elements

Class 11 Chemistry — Chapter 11: P-Block Elements Online Test

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Class 11 Chemistry: P-Block Elements 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. The reaction of elemental Silicon () with aqueous produces gas, but is unreactive toward dilute . This contrasting reactivity implies that is a substance with which characteristic chemical property?

2 / 20

2. The chemical equation describes the etching of glass (silica). In this reaction, the role of is unique because:

3 / 20

3. The ratio in a zeolite affects its properties. A higher ratio (e.g., vs. ):

4 / 20

4. Industrial production of is often a major byproduct of which large-scale chemical process involving calcium carbonate ()?

5 / 20

5. Single-walled carbon nanotubes (SWCNTs) are often bundled together into ropes. The individual tubes within a rope are held together by:

6 / 20

6. What is the total number of covalent bonds (single and double) present in the molecule?

7 / 20

7. Which statement is true regarding the acidity/hydrolysis of the oxides of Carbon and Silicon in the presence of strong base?

8 / 20

8. In the triple bond, how many bonds are present?

9 / 20

9. Which mineral is the most abundant compound of Silicon on the Earth's crust?

10 / 20

10. The chemical name of Borax () is:

11 / 20

11. Kernite (or Rasorite) is the second most important ore of boron. What is its chemical formula?

12 / 20

12. The first element of each p-block group shows anomalous behavior. This is primarily due to:

13 / 20

13. The first ionization enthalpy () of Group 13 elements shows a complex trend. What is the correct order?

14 / 20

14. The bond length in (130 pm) is shorter than expected for a single bond. This is attributed to:

15 / 20

15. The bridge bond angle () in diborane is approximately:

16 / 20

16. When reacts with a Lewis base such as ammonia (), what is the term for the resulting product?

17 / 20

17. The ionization enthalpy () generally decreases down a group. For Group 14, which element exhibits a slight increase in the first ionization enthalpy compared to the element immediately preceding it?

18 / 20

18. The stability of double bonds over single bonds is quantified by the difference in their bond enthalpies. For , the average bond enthalpy of is approximately:

19 / 20

19. How does the stability of multiple bonds compare to that of hypothetical multiple bonds?

20 / 20

20. The discovery of Buckminsterfullerene () in 1985 led to the awarding of the Nobel Prize in Chemistry in 1996 to which trio of scientists?

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Class 11 Chemistry: P-Block Elements 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. What is the maximum covalency that Boron (B) can exhibit?

2 / 30

2. Unlike , the hydrolysis of proceeds rapidly. If (Germanium tetrachloride) were subjected to the same conditions, what would be the expected relative rate of hydrolysis compared to ?

3 / 30

3. When Germanium forms chains (germanes, ), the maximum chain length observed is typically much shorter than that for alkanes. This is primarily because:

4 / 30

4. Silicones in the form of oils and greases are widely used as lubricants, especially for specialized equipment. This application is due to their stability in which two extreme conditions?

5 / 30

5. What is the "inert pair effect"?

6 / 30

6. Carbon () forms (carbon monoxide), a stable compound in the +2 oxidation state. Which factor contributes to the stability of despite Carbon's strong preference for the +4 state?

7 / 30

7. How does the density of graphite compare to that of diamond, and what is the structural reason for the difference?

8 / 30

8. The correct structural representation of the tetraborate anion present in crystalline Borax () is:

9 / 30

9. Which comparison of bond dissociation enthalpies for Group 14 single bonds is correct?

10 / 30

10. Moving down Group 14 (C to Pb), how does the change in atomic radius typically proceed?

11 / 30

11. When highly purified is treated with concentrated aqueous solution, the products are sodium silicate () and hydrogen gas (). This reaction classifies as a substance that is:

12 / 30

12. Kernite (or Rasorite) is the second most important ore of boron. What is its chemical formula?

13 / 30

13. Which exceptional property of silicones makes them widely used as waterproofing materials and sealants?

14 / 30

14. Feldspars and Zeolites are examples of which major class of silicates, characterized by a three-dimensional interlocking structure?

15 / 30

15. Orthoboric acid acts as a weak acid in water, but it is unique because it is not a proton donor. Instead, it acts as a Lewis acid by:

16 / 30

16. The reaction of elemental Silicon () with aqueous produces gas, but is unreactive toward dilute . This contrasting reactivity implies that is a substance with which characteristic chemical property?

17 / 30

17. Borax is widely used as a flux in metallurgy (e.g., soldering or welding). The function of Borax as a flux is to:

18 / 30

18. What is the general anion formula for a Cyclic Silicate (or Cyclosilicate), such as the ion found in the mineral beryl?

19 / 30

19. Compare the bond dissociation enthalpies () of the single bonds formed with Oxygen for Carbon and Silicon ( bond).

20 / 30

20. Carbon's maximum oxidation state of +4 is strongly preferred. While Silicon also prefers +4, it rarely shows a stable +2 state. This difference suggests that the Inert Pair Effect is:

21 / 30

21. Which statement correctly describes the nature of the halides () formed by Group 14 elements?

22 / 30

22. The unique bonding in diborane () involves the formation of bonds. What are these bonds commonly called?

23 / 30

23. The formation of stable ring and chain structures in Silicon chemistry is mainly achieved when the Silicon atoms are separated by which bridging element?

24 / 30

24. The classic qualitative test for the presence of gas involves bubbling the gas through limewater (aqueous ). The initial observation that confirms the presence of is:

25 / 30

25. When comparing the stability of the tetrahalides () and dihalides () of Lead (), which conclusion is correct?

26 / 30

26. What is the specific geometry surrounding each carbon atom in the diamond lattice?

27 / 30

27. When heated strongly in the presence of air or pure oxygen, diamond will react to form:

28 / 30

28. For industrial-scale production, Carbon Monoxide is typically prepared along with Hydrogen, forming a mixture known as water gas. Which reaction produces water gas?

29 / 30

29. The first ionization enthalpy () generally decreases down Group 14. Which element disrupts this smooth trend by exhibiting a higher than the element immediately above it?

30 / 30

30. The stability of the oxidation state among Group 14 elements:

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Class 11 Chemistry: P-Block Elements 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. Diamond possesses an exceptionally high melting point (subliming at around ). This is due to the need to overcome which forces/bonds?

2 / 50

2. What is the "inert pair effect"?

3 / 50

3. Which property of Carbon Dioxide makes it an effective agent in fire extinguishers?

4 / 50

4. The stability of the oxidation state among Group 14 elements:

5 / 50

5. Diborane () is an electron-deficient compound. What is its common classification in terms of chemical bonding?

6 / 50

6. What is the hybridization of the Boron atom in the anion formed when orthoboric acid reacts with water?

7 / 50

7. Which factor causes small cycloalkanes, such as cyclopropane (), to be highly reactive compared to larger rings like cyclohexane?

8 / 50

8. Which of the following elements, due to its configuration and access to vacant -orbitals, readily expands its covalency beyond 4?

9 / 50

9. What are the hybridization and geometry of the aluminium atom in the ion?

10 / 50

10. Carbon () forms (carbon monoxide), a stable compound in the +2 oxidation state. Which factor contributes to the stability of despite Carbon's strong preference for the +4 state?

11 / 50

11. When comparing the stability of the tetrahalides () and dihalides () of Lead (), which conclusion is correct?

12 / 50

12. The configuration results in a common oxidation state of +4 for all Group 14 elements. Which of the following is also a prominent and stable oxidation state, particularly for the heavier elements (Sn, Pb)?

13 / 50

13. Why does Silicon tetrachloride () readily undergo hydrolysis when exposed to moisture, while Carbon tetrachloride () is generally stable towards hydrolysis?

14 / 50

14. Which of the following compounds of Silicon is unstable and highly reactive, contrasting with the stable double-bonded organic compounds of Carbon?

15 / 50

15. Why is the atomic radius of Gallium (Ga) surprisingly smaller than that of Aluminium (Al)?

16 / 50

16. In the natural world, the most common form of ring structure containing Group 14 elements is found in silicates, specifically those where tetrahedra link to form closed rings. What is the structural classification for silicates containing the ion (like in Beryl)?

17 / 50

17. When Germanium forms chains (germanes, ), the maximum chain length observed is typically much shorter than that for alkanes. This is primarily because:

18 / 50

18. Why does Lead () show virtually no catenation?

19 / 50

19. Which comparison of bond dissociation enthalpies for Group 14 single bonds is correct?

20 / 50

20. In terms of chemical reactivity, how do the catenated hydrides of Carbon () compare to the catenated hydrides of Silicon ()?

21 / 50

21. Which form of naturally occurring carbon is the hardest known natural substance and possesses a giant tetrahedral structure?

22 / 50

22. Orthoboric acid () can be prepared by treating Borax () with:

23 / 50

23. Where are the p-block elements located in the modern periodic table?

24 / 50

24. Which of the following carbon-containing ions derives its unique stability and planar structure from the presence of delocalized bonds?

25 / 50

25. The industrial preparation of water gas () from coke () and steam (): is an example of a reaction that is highly:

26 / 50

26. The reaction of elemental Silicon () with aqueous produces gas, but is unreactive toward dilute . This contrasting reactivity implies that is a substance with which characteristic chemical property?

27 / 50

27. Feldspars and Zeolites are examples of which major class of silicates, characterized by a three-dimensional interlocking structure?

28 / 50

28. Which set of reactants is preferred for the preparation of anhydrous aluminium chloride, ?

29 / 50

29. When orthoboric acid () is treated with excess ethanol () in the presence of concentrated , the product formed is:

30 / 50

30. Silicones are noted for their high thermal stability compared to most carbon-based organic polymers. This is attributed to the strength of the:

31 / 50

31. The stability of double bonds over single bonds is quantified by the difference in their bond enthalpies. For , the average bond enthalpy of is approximately:

32 / 50

32. What is the complete electronic configuration of Aluminium (Al, Z=13)?

33 / 50

33. What chemical reagent is added during the titration of a Boric acid solution to make it strong enough to be titrated against a strong base ()?

34 / 50

34. In the triple bond, how many bonds are present?

35 / 50

35. What is the maximum covalency that Boron (B) can exhibit?

36 / 50

36. In the Friedel-Crafts alkylation reaction, which species is created when the Lewis acid reacts with the alkyl halide ()?

37 / 50

37. Graphite is an excellent conductor of electricity. This property is due to the presence of:

38 / 50

38. What is the most characteristic and common oxidation state shown by all elements in Group 14?

39 / 50

39. Which statement accurately compares the natural occurrence of Boron (B) and Aluminium (Al)?

40 / 50

40. What is the hybridization of the carbon atoms in the diamond crystal structure?

41 / 50

41. What are the maximum covalent bonding capacities (covalencies) typically exhibited by Carbon and Silicon, respectively?

42 / 50

42. What is the most common and stable oxidation state for Boron (B) and Aluminium (Al)?

43 / 50

43. Unlike other Group 13 elements, Boron forms stable hydrides called boranes (e.g., Diborane, ). What is a key feature of these compounds?

44 / 50

44. What is the standard and most effective first-aid treatment for severe Carbon Monoxide poisoning?

45 / 50

45. Borane (), the monomer of diborane, is highly unstable at room temperature because:

46 / 50

46. Which exceptional property of silicones makes them widely used as waterproofing materials and sealants?

47 / 50

47. Diborane () can be prepared in the laboratory by the reaction of iodine () with which reducing agent?

48 / 50

48. The largest sink for anthropogenic is currently the world's oceans. What is the chemical consequence of the ocean absorbing large amounts of ?

49 / 50

49. When highly purified is treated with concentrated aqueous solution, the products are sodium silicate () and hydrogen gas (). This reaction classifies as a substance that is:

50 / 50

50. The zeolite, a key catalyst in the "Methanol-to-Gasoline" () process, is an example of a synthetic zeolite. This process demonstrates the zeolite's ability to selectively convert:

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Practice P-Block Elements MCQs
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Class 11 Chemistry — Chapter 11: P-Block Elements Online Test

The Class 11 Chemistry: Chapter 11 – P-Block Elements Online Test offers an extensive collection of 277 MCQs designed to deepen your understanding of p-block elements and their properties. This test is free, NCERT/CBSE-aligned, and lets you practice at your own pace with unlimited attempts. Whether you’re aiming for a quick revision or preparing for exams like JEE or NEET, this test is an ideal resource to evaluate your knowledge.

This page acts as a mini online mock test for Chapter 11. You can practice multiple-choice questions (MCQs) and instantly see your results along with detailed explanations. Think of it as a real exam simulation that helps you boost your confidence before the actual test. This test is also great for those who wish to strengthen their knowledge of p-block elements, their chemical properties, and trends in the periodic table.

What is this Chapter 11: P-Block Elements Online Test?

This test consists of three exam-style MCQ papers for Chapter 11: P-Block Elements:

  • 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 277 MCQs
  • Paper 3 (Hard) — Challenge: 50 questions · 75 min · Pass 70% · Randomized from the same pool + Certificate on pass

Note: Each attempt gives you fresh mixes of questions in Paper 2 and Paper 3, ensuring a unique experience each time.

Topics covered in these online tests

The online test will guide you through a wide range of essential topics from Chapter 11: P-Block Elements. The key concepts include:

  • General Properties of p-block elements — their physical and chemical properties, and trends in groups and periods.
  • Electronic Configuration of p-block elements and how it relates to their properties.
  • Oxidation States of p-block elements, including trends and exceptions.
  • Trends in Group 13 Elements — Boron and its compounds, Aluminum, Gallium, etc.
  • Trends in Group 14 Elements — Carbon, Silicon, Germanium, Tin, Lead and their allotropes.
  • Trends in Group 15 Elements — Nitrogen, Phosphorus, Arsenic, Antimony, and their important compounds.
  • Trends in Group 16 Elements — Oxygen, Sulfur, Selenium, Tellurium, and Polonium.
  • Trends in Group 17 Elements — Halogens and their physical and chemical properties.
  • Group 18 Elements — Noble gases, their properties, compounds like Xenon compounds, etc.
  • Allotropes of Elements — Oxygen, Phosphorus, and Sulfur (e.g., allotropes of Carbon and Sulfur).
  • Industrial Applications — The industrial use of p-block elements, including the extraction of metals, and their role in chemical reactions.
  • Environmental Impact — The effects of p-block elements and their compounds on the environment (e.g., nitrogen oxides, sulfur compounds).

If you want more practice on the s-block elements, you can also visit the online test for S-Block Elements.

How This Exam-Style Online Test Works

  • Pick a paper → Answer MCQs within time → Submit → Get instant score and result with answer review.
  • MCQs: Each paper contains randomized questions from a large question pool.
  • Timer: Paper 1 is for 30 minutes, Paper 2 is for 45 minutes, and Paper 3 is for 75 minutes.
  • View Results: Get your score and an immediate review with correct answers.
  • Retake: You can retake the test as many times as needed to improve your score.

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, use Next/Prev to navigate.
  • Result Page: Instant result with correct/incorrect answers, detailed explanation, and the option to restart the 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 question pool; Paper 1 remains fixed.

Who can take this test?

  • Class 11 CBSE/NCERT students revising Chapter 11 on P-Block Elements.
  • JEE/NEET foundation aspirants building solid concepts in inorganic Chemistry.
  • Teachers and tutors using this as a practice tool for class assignments and quizzes.
  • Students from other boards and countries looking to practice P-Block Elements.
  • Students preparing for competitive exams seeking to solidify their knowledge of p-block elements.

Advantages of this online test

  • Real exam experience: Timed questions, instant feedback, and clear performance analysis.
  • Step-up difficulty: Foundation → Mixed → Challenge (+ certificate on Paper 3).
  • Unlimited attempts: Reattempt the test to improve your score with randomized questions in Paper 2 & 3.
  • Free of charge: No sign-up or payment required to access this comprehensive test.

How this test helps you study better

  • Step 1 – Concept check: Start with Paper 1 to check your grasp of basic P-Block element concepts.
  • Step 2 – Reinforce: Take Paper 2 for mixed concept and numerical questions.
  • Step 3 – Challenge yourself: Finish with Paper 3 to prepare for advanced-level questions and exams.
  • Step 4 – Analyze results: Study your missed questions and review the detailed answers to strengthen weak areas.

Important notes (read before you start)

  • Do not refresh / close the tab during the test.
  • Best experience: Use the latest version of Chrome/Edge and ensure a stable internet connection.
  • Allow cookies / local storage for a smooth experience and progress saving.
  • Safety: The test is 100% free, and there are no hidden charges or login requirements.

More practice for Class 11 Chemistry

After completing the P-Block Elements online test, continue your Chemistry practice with other resources: Class 11 Chemistry MCQ Collection or try the Class 11 Chemistry Online Test Index for other chapters.

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