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

2 / 30

2. Why are noble gases (e.g., Ar, Ne) classified as atoms rather than molecules?

3 / 30

3. Which discovery challenged Dalton’s idea that atoms are indivisible?

4 / 30

4. Dalton’s theory helped chemistry advance because it:

5 / 30

5. Which of the following correctly represents the atomicity of ozone?

6 / 30

6. Dalton’s Atomic Theory helped in the development of:

7 / 30

7. Which condition is necessary to apply Gay-Lussac’s Law of Gaseous Volumes correctly?

8 / 30

8. Why is the Law of Conservation of Mass fundamental to balancing chemical equations?

9 / 30

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

10 / 30

10. What is the mass of water formed when 2 g of H₂ reacts with excess O₂? Reaction:

11 / 30

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

12 / 30

12. Which fertilizer provides both nitrogen and phosphorus to crops?

13 / 30

13. The average atomic mass of lithium is 6.94 u. Which isotopes contribute to this value?

14 / 30

14. The molar mass of sodium hydroxide (NaOH) is:

15 / 30

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

16 / 30

16. Which of the following correctly distinguishes molecular mass and formula mass?

17 / 30

17. How many hydrogen atoms are in 1 mole of methane ()?

18 / 30

18. Chlorine occurs in two isotopes: Cl-35 (75% abundance) and Cl-37 (25% abundance). What is the average atomic mass of chlorine?

19 / 30

19. Which discovery proved Dalton wrong about atoms of an element being identical?

20 / 30

20. Which of the following samples contains the largest number of molecules?

21 / 30

21. What is the atomicity of ammonium nitrate, ?

22 / 30

22. Which reaction shows molecular decomposition?

23 / 30

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

24 / 30

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

25 / 30

25. Which of the following gases is monoatomic in nature?

26 / 30

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

27 / 30

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

28 / 30

28. In a neutralization reaction, 49 g of H₂SO₄ reacts with NaOH. How many grams of NaOH are required? Reaction:

29 / 30

29. In a reaction, 5 g of calcium reacts with 2 g of oxygen to form calcium oxide. The mass of CaO produced will be:

30 / 30

30. Which of the following is an industrial use of sulphuric acid, often called the “king of chemicals”?

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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. The formula mass of aluminium hydroxide is:

2 / 50

2. Which branch of physics directly supports chemistry in explaining atomic orbitals?

3 / 50

3. Which chemical process is the basis of the cement industry?

4 / 50

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

5 / 50

5. Avogadro’s number represents:

6 / 50

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

7 / 50

7. Which data is essential to calculate an empirical formula?

8 / 50

8. Which of the following shows the correct relation between mole and volume of a gas at STP?

9 / 50

9. In an experiment, 10 g of a hydrocarbon is completely burnt in oxygen to form 30 g of CO₂ and 9 g of H₂O. What is the mass of oxygen consumed?

10 / 50

10. The molar mass of ammonia () is:

11 / 50

11. Who proposed the Law of Multiple Proportions?

12 / 50

12. Which law explains why all gases occupy 22.4 L per mole at STP?

13 / 50

13. The mass of a hydrogen atom is approximately:

14 / 50

14. Which of the following correctly links Avogadro’s number and molar mass?

15 / 50

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

16 / 50

16. Which calculation correctly shows the number of oxygen atoms in 0.5 mole of O₂?

17 / 50

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

18 / 50

18. Which set contains only triatomic molecules?

19 / 50

19. Which pair of gases would contain the same number of molecules at STP if taken in equal volumes?

20 / 50

20. The Law of Reciprocal Proportions states that:

21 / 50

21. What is the relation between 1 mole of carbon-12 atoms and amu?

22 / 50

22. Which contribution of Dalton’s theory led to the calculation of relative atomic masses?

23 / 50

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

24 / 50

24. Which step is not necessary to determine an empirical formula experimentally?

25 / 50

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

26 / 50

26. What is the atomicity of calcium hydroxide, ?

27 / 50

27. In the reaction , if 1 mole C₂H₆ is burned with 2 moles O₂, which is limiting?

28 / 50

28. Sulfur vapour at very high temperature contains . The atomicity of is:

29 / 50

29. If 88 g of CO₂ are taken, how many moles are present? (Molar mass of CO₂ = 44 g/mol)

30 / 50

30. Which of the following is the correct difference between atoms and molecules?

31 / 50

31. Avogadro’s number is numerically equal to:

32 / 50

32. In H₂O, 2 g of hydrogen combines with 16 g of oxygen. In H₂S, 2 g of hydrogen combines with 32 g of sulphur. According to Richter’s law, the ratio of masses of oxygen and sulphur that combine with each other should be:

33 / 50

33. Which statement about atomic mass unit is correct?

34 / 50

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

35 / 50

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

36 / 50

36. Why was the Law of Reciprocal Proportions important historically?

37 / 50

37. Which polymer is commonly used for making plastic bottles?

38 / 50

38. The formula for percentage yield is:

39 / 50

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

40 / 50

40. Which environmental issue is directly related to chemical use of chlorofluorocarbons (CFCs)?

41 / 50

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

42 / 50

42. Which of the following is the first step in calculating percentage composition of a compound?

43 / 50

43. If 67.2 L of hydrogen gas is taken at STP, how many moles does it represent?

44 / 50

44. Which of the following samples contains the largest number of molecules?

45 / 50

45. What is the relation between a molecular formula and an empirical formula?

46 / 50

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

47 / 50

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

48 / 50

48. What is meant by the molecular formula of a compound?

49 / 50

49. Find the percentage of carbon in carbon dioxide ().

50 / 50

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

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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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  • Safety: This test is 100% free, and there are no hidden charges.

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