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Class 11 Chemistry — Chapter 1: Some Basic Concepts of Chemistry Online Test

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Class 11 Chemistry: Some Basic Concepts of Chemistry 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. In the combustion of methane, , if 16 g CH₄ and 64 g O₂ are used, the limiting reagent is:

2 / 20

2. In the reaction , how many grams of AlCl₃ are produced from 54 g of Al?

3 / 20

3. In the reaction , how many moles of water are formed when 4 moles of hydrogen react with excess oxygen?

4 / 20

4. What mass of calcium carbonate is required to produce 44 g of CO₂ on decomposition? Reaction:

5 / 20

5. In the balanced combustion reaction of methane: , what is the coefficient of water?

6 / 20

6. Calculate the percentage of oxygen in water ().

7 / 20

7. In the synthesis of ammonia: , if 10 L of nitrogen is used, what volume of hydrogen is required at STP?

8 / 20

8. What is the atomicity of ammonium nitrate, ?

9 / 20

9. Determine the atomicity of (ammonium sulfate).

10 / 20

10. Which particle is directly rearranged during molecular chemical reactions?

11 / 20

11. Which of the following was a major merit of Dalton’s Atomic Theory?

12 / 20

12. Which of the following provides direct evidence for Avogadro’s Hypothesis?

13 / 20

13. In a closed system, 10 g of hydrogen reacts with 80 g of oxygen. What will be the total mass of water formed?

14 / 20

14. The Law of Definite Proportions states that:

15 / 20

15. According to the Law of Multiple Proportions, the ratios must always be:

16 / 20

16. In the reaction: the ratio of volumes of hydrogen, chlorine, and hydrogen chloride is:

17 / 20

17. What is the molecular mass of ?

18 / 20

18. The number is known as:

19 / 20

19. How many molecules of nitrogen gas are in 28 g of N₂?

20 / 20

20. What is the general formula for percentage composition of an element in a compound?

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Class 11 Chemistry: Some Basic Concepts of Chemistry 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.

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  • 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 percentage of carbon in carbon dioxide ()?

2 / 30

2. In NO and NO₂, 14 g of nitrogen combines with 16 g and 32 g of oxygen, respectively. The ratio of masses of oxygen is:

3 / 30

3. Which of the following is not true about molecular mass?

4 / 30

4. Which experiment did Lavoisier perform to establish the Law of Conservation of Mass?

5 / 30

5. Dalton’s postulate that atoms are indestructible fails in which processes?

6 / 30

6. If boron has two isotopes B-10 (20% abundance) and B-11 (80% abundance), what is its average atomic mass?

7 / 30

7. Which isotope is used as the standard reference for defining the atomic mass unit?

8 / 30

8. The molar volume of a gas at STP is:

9 / 30

9. How many molecules are there in 44 g of carbon dioxide (CO₂)?

10 / 30

10. What is the mass of 5.6 L of oxygen gas at STP? (Molar mass = 32 g/mol)

11 / 30

11. Which of the following shows chemistry’s role in understanding the environment?

12 / 30

12. Which is a polyatomic elemental molecule?

13 / 30

13. Avogadro’s number represents:

14 / 30

14. In , the percentage of chlorine is:

15 / 30

15. What is the percentage composition of nitrogen in ammonia ()?

16 / 30

16. Which particle is responsible for the chemical behavior of an atom?

17 / 30

17. Which observation directly contradicts Dalton’s claim that “atoms of the same element are identical in mass and properties”?

18 / 30

18. Which of the following is an example of an empirical formula?

19 / 30

19. Which atmospheric process is explained through chemistry?

20 / 30

20. In CO and CO₂, 12 g of carbon combines with 16 g and 32 g of oxygen, respectively. The ratio of masses of oxygen combining with the same mass of carbon is:

21 / 30

21. What is the stoichiometric coefficient of CO₂ in the equation ?

22 / 30

22. Which formula is derived from Avogadro’s Hypothesis?

23 / 30

23. Calculate the percentage of oxygen in calcium carbonate ().

24 / 30

24. Which formula is used to calculate molecular mass?

25 / 30

25. Which of the following best illustrates the Law of Multiple Proportions?

26 / 30

26. Which compound is the main active ingredient in common painkillers like aspirin?

27 / 30

27. The concept of alloys like brass and bronze shows the relation of chemistry with:

28 / 30

28. Why is the average atomic mass of chlorine not exactly 36 u, even though it has Cl-35 and Cl-37 isotopes?

29 / 30

29. Which is the correct molecular mass of ammonia ()?

30 / 30

30. Which statement about metals in the solid state and atomicity is most accurate?

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Class 11 Chemistry: Some Basic Concepts of Chemistry 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 allotrope of oxygen has atomicity 3?

2 / 50

2. Which statement best summarizes Gay-Lussac’s Law of Gaseous Volumes?

3 / 50

3. One mole of sodium chloride (NaCl) contains how many ions?

4 / 50

4. Which of the following combinations does NOT illustrate the Law of Reciprocal Proportions?

5 / 50

5. Which of the following is a diatomic molecule?

6 / 50

6. Which law of chemical combination is directly explained by Dalton’s Atomic Theory?

7 / 50

7. What is meant by molecular mass of a substance?

8 / 50

8. The approximate mass of one proton is:

9 / 50

9. Which statement is true about formula mass?

10 / 50

10. Who proposed Avogadro’s Hypothesis?

11 / 50

11. Which concept directly arises from Avogadro’s Hypothesis?

12 / 50

12. The empirical formula of a compound is NO₂ and its molecular mass is 92 g/mol. What is its molecular formula?

13 / 50

13. Which element exists as a polyatomic molecule under normal conditions?

14 / 50

14. Which statement correctly describes molecular composition?

15 / 50

15. Which of the following laws is directly supported by the Law of Reciprocal Proportions?

16 / 50

16. What is meant by average atomic mass of an element?

17 / 50

17. How many molecules of CO₂ are present in 22.4 L of CO₂ at STP?

18 / 50

18. If the empirical formula of a compound is CH₂ and its molecular mass is 42, what is the molecular formula?

19 / 50

19. Who proposed the Law of Definite Proportions?

20 / 50

20. Why is Dalton’s Atomic Theory still important today despite its limitations?

21 / 50

21. Who is credited with proposing the first modern atomic theory?

22 / 50

22. Which of the following shows chemistry’s importance in modern agriculture?

23 / 50

23. Who is credited with introducing the concept of the “mole” in chemistry?

24 / 50

24. Which statement about halogens is correct regarding atomicity at standard conditions?

25 / 50

25. Which of the following compounds does not obey the Law of Definite Proportions strictly?

26 / 50

26. The role of chemistry in engineering is most clearly seen in which example?

27 / 50

27. Which of the following is the correct order of steps to determine an empirical formula?

28 / 50

28. In the reaction , if 5 moles of H₂ and 2 moles of O₂ are mixed, which is the limiting reagent?

29 / 50

29. Who proposed the Law of Reciprocal Proportions?

30 / 50

30. What is the formula mass of sodium chloride ()?

31 / 50

31. Which reaction verifies Gay-Lussac’s Law?

32 / 50

32. Which of the following is a natural antioxidant found in green tea?

33 / 50

33. Which of the following is true about the relation between mole, mass, and volume?

34 / 50

34. The molar mass of ammonia () is:

35 / 50

35. In the reaction , how many moles of water are formed when 4 moles of hydrogen react with excess oxygen?

36 / 50

36. Which is a polyatomic elemental molecule?

37 / 50

37. Why is the molar volume of gases important in chemical calculations?

38 / 50

38. The mass of a hydrogen atom is approximately:

39 / 50

39. Which of the following equations links mole, mass, and molar mass?

40 / 50

40. Which statement about atomic mass unit is correct?

41 / 50

41. Which example shows a variable composition compound that challenges Dalton’s fixed whole-number ratios?

42 / 50

42. Which of the following best describes how Dalton’s theory supported the Law of Multiple Proportions?

43 / 50

43. The empirical formula of acetic acid is CH₂O. If its molar mass is 60 g/mol, what is its molecular formula?

44 / 50

44. Which chemical compound is responsible for the pungent smell of onions?

45 / 50

45. Which of the following is used as an antacid to reduce acidity in the stomach?

46 / 50

46. What is meant by molar mass of a substance?

47 / 50

47. Who proposed the Law of Gaseous Volumes?

48 / 50

48. Which of the following chemicals is widely used in the fertilizer industry to enhance nitrogen content in soil?

49 / 50

49. The concept of alloys like brass and bronze shows the relation of chemistry with:

50 / 50

50. Which of the following reactions best demonstrates the Law of Conservation of Mass?

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Practice Some Basic Concepts of Chemistry MCQs
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Class 11 Chemistry: Chapter 1 — Some Basic Concepts of Chemistry Online Test

The Class 11 Chemistry: Chapter 1 – Some Basic Concepts of Chemistry Online Test provides a comprehensive pool of 394 MCQs designed to test and enhance your understanding of fundamental concepts in Chemistry. This test is free, CBSE/NCERT-aligned, and helps you assess your grasp on the key topics that form the foundation of the subject. With three difficulty levels, you can progressively challenge yourself and track your improvement over time.

What is this Chapter 1 Online Test?

This test contains three exam-style MCQ papers for Chapter 1: Some Basic Concepts of Chemistry:

  • 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 ~394 questions
  • Paper 3 (Hard) — Challenge: 50 questions · 75 min · Pass 70% · Randomized from the same pool + Certificate on pass

Note: Each paper is timed, auto-evaluated, and displays your score with answer reviews right after submission.

Topics covered in these online tests

In this test, you will practice essential topics from Chapter 1: Some Basic Concepts of Chemistry, which include:

  • Importance of Chemistry — Introduction to Chemistry, its relevance in real life and scientific advancements
  • Laws of Chemical Combination — Law of Mass Conservation, Law of Definite Proportions
  • Dalton’s Atomic Theory — Basic postulates, understanding atoms, and molecules
  • Mole Concept — Mole, Avogadro’s Number, Concept of Molar Mass, and Concept of Chemical Calculations
  • Molar Mass — Determining molar mass and its importance in chemical reactions
  • Percentage Composition — Calculation of percentage composition of compounds
  • Empirical & Molecular Formula — Concepts of empirical formula and molecular formula derivation
  • Stoichiometry — Concept of limiting reagent, and calculation of quantities involved in chemical reactions
  • Limiting Reagent — Importance in chemical reactions and stoichiometric calculations

How This Exam-Style Online Test Works

  • Pick a paper → Answer MCQs within time → Submit → Get instant score and answer review.
  • Timed MCQs: The test is timed, with Paper 1 being 30 minutes, Paper 2 being 45 minutes, and Paper 3 being 75 minutes.
  • Instant Feedback: After each paper, view your score along with a detailed summary and answer explanation.
  • Unlimited Retakes: You can retake the test as many times as you like, with fresh questions in Paper 2 and Paper 3.
  • Certificate: You will earn a certificate after passing Paper 3 with a score of 70% or more.

Who Can Take This Test?

  • Class 11 CBSE/NCERT students who are preparing for unit tests, mid-term exams, or final exams.
  • Students seeking to build a strong foundation in Chemistry for JEE/NEET or other competitive exams.
  • School students who need extra practice and want to assess their understanding of Chapter 1.
  • Teachers and tutors who want to provide students with extra practice and assess their skills.
  • Self-learners and home-schoolers who want a structured, easy-to-use resource to practice Chapter 1 topics.

Advantages of this Online Test

  • Real exam feel: Timed questions and instant feedback help you practice effectively under exam-like conditions.
  • Step-up difficulty: Start with easy questions in Paper 1, move to medium in Paper 2, and take the final challenge in Paper 3.
  • Unlimited attempts: Practice as many times as you like to perfect your skills and improve your score.
  • Completely free: No fees, no charges—just unlimited access to the online test.

How This Test Helps You Study Better

  • Step 1 – Concept Check: Take Paper 1 to check your understanding of basic concepts.
  • Step 2 – Reinforce Learning: Attempt Paper 2 for a mix of concept and numerical questions.
  • Step 3 – Challenge Yourself: Attempt Paper 3 to assess your readiness for exams.
  • Step 4 – Review: Carefully analyze your results and revisit concepts you missed.

Important Notes (Read Before You Start)

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