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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. Which of the following explains why average atomic masses are often decimal numbers?

2 / 30

2. Which statement best describes the Law of Multiple Proportions?

3 / 30

3. Which statement is true about empirical and molecular formulas?

4 / 30

4. How many atoms are present in 2 moles of aluminium?

5 / 30

5. Which chemical is commonly used as an octane booster in fuels?

6 / 30

6. What is the formula mass of magnesium hydroxide ()?

7 / 30

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

8 / 30

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

9 / 30

9. Two oxides of nitrogen contain 30 g of nitrogen each. In one, oxygen is 34.3 g, and in the other, oxygen is 68.6 g. The ratio of masses of oxygen combining with nitrogen is:

10 / 30

10. Why was Dalton’s Atomic Theory considered revolutionary at the time?

11 / 30

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

12 / 30

12. Which of the following best defines a molecule?

13 / 30

13. The mass of a hydrogen atom is approximately:

14 / 30

14. Which of the following is a molecule and not a compound?

15 / 30

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

16 / 30

16. In the reaction , if 44 g of propane burns, how many liters of CO₂ at STP are produced?

17 / 30

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

18 / 30

18. Which allotrope of oxygen has atomicity 3?

19 / 30

19. Which of the following is monoatomic at STP?

20 / 30

20. Which of the following correctly lists the three fundamental subatomic particles in an atom?

21 / 30

21. Which statement about atomic mass unit is correct?

22 / 30

22. The molar mass of calcium carbonate () is:

23 / 30

23. How many moles of oxygen gas are present in 44.8 L of O₂ at STP?

24 / 30

24. Calculate the percentage of calcium in 20 g of CaCO₃.

25 / 30

25. In the reaction , 12 g Mg reacts with 16 g O₂. Which is limiting?

26 / 30

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

27 / 30

27. The Law of Definite Proportions states that:

28 / 30

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

29 / 30

29. If 10 g of CaCO₃ is decomposed, what volume of CO₂ at STP is theoretically produced? Reaction:

30 / 30

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

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

2 / 50

2. What is the molar mass of nitrogen gas ()?

3 / 50

3. Why is molecular formula considered more informative than empirical formula?

4 / 50

4. Which merit of Dalton’s theory laid the foundation for modern chemistry?

5 / 50

5. Which of the following pairs correctly shows “atom vs molecule”?

6 / 50

6. Which compound is often cited as an example of the Law of Definite Proportions?

7 / 50

7. In carbon dioxide (CO₂), the mass ratio of carbon to oxygen is:

8 / 50

8. 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:

9 / 50

9. The approximate mass of one proton is:

10 / 50

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

11 / 50

11. The SI unit of molar mass is:

12 / 50

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

13 / 50

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

14 / 50

14. Which of the following is true about the mole concept?

15 / 50

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

16 / 50

16. Which of the following is monoatomic at STP?

17 / 50

17. Which statement about atoms in chemical reactions is correct?

18 / 50

18. Which of the following correctly represents the atomic composition of oxygen-16?

19 / 50

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

20 / 50

20. One key merit of Dalton’s theory was that it provided:

21 / 50

21. Calculate the percentage of calcium in 20 g of CaCO₃.

22 / 50

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

23 / 50

23. Which of the following compounds requires the use of formula mass rather than molecular mass?

24 / 50

24. How many liters of oxygen gas are present at STP in 0.5 mole?

25 / 50

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

26 / 50

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

27 / 50

27. Which of the following fuels is considered the cleanest source of energy?

28 / 50

28. The Solvay process is used in the chemical industry to produce:

29 / 50

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

30 / 50

30. In the reaction , if 10 moles of N₂ and 15 moles of H₂ are available, what is the limiting reagent?

31 / 50

31. Which of the following statements is true about empirical formulas?

32 / 50

32. How many grams of NaOH are required to neutralize 49 g of H₂SO₄? Reaction:

33 / 50

33. Which discovery first showed that atoms are divisible, contradicting Dalton’s “indivisible atom” postulate?

34 / 50

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

35 / 50

35. Which of the following statements is false?

36 / 50

36. Why is molar mass important in stoichiometric calculations?

37 / 50

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

38 / 50

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

39 / 50

39. In the reaction , 160 g Fe₂O₃ reacts with 84 g CO. Which is the limiting reagent?

40 / 50

40. Which is a polyatomic elemental molecule?

41 / 50

41. Which branch of chemistry is most relevant for developing renewable energy technologies like solar cells?

42 / 50

42. What is the main difference between an empirical formula and a molecular formula?

43 / 50

43. What is the value of 1 atomic mass unit (amu) in grams?

44 / 50

44. What is the first step in determining the empirical formula of a compound from experimental data?

45 / 50

45. Gay-Lussac’s law of gaseous volumes was one of the foundations for which later concept?

46 / 50

46. In , the percentage of chlorine is:

47 / 50

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

48 / 50

48. Which of the following is the correct SI unit of amount of substance?

49 / 50

49. The Law of Conservation of Mass is not strictly valid in:

50 / 50

50. The formula mass of aluminium hydroxide is:

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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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  • Allow cookies / local storage to save your progress and results.
  • Safety: This test is 100% free, and there are no hidden charges.

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