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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. Why is atomicity an important concept?

2 / 30

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

3 / 30

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

4 / 30

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

5 / 30

5. Which of the following correctly expresses the relation between moles and mass?

6 / 30

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

7 / 30

7. 1 mole of water contains how many hydrogen atoms?

8 / 30

8. In the reaction , what mass of AlCl₃ is formed from 54 g of Al (assuming 100% yield)?

9 / 30

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

10 / 30

10. Which of the following statements is false?

11 / 30

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

12 / 30

12. The Law of Definite Proportions states that:

13 / 30

13. Which merit of Dalton’s theory helped explain the Law of Definite Proportions?

14 / 30

14. Which of the following compounds has a formula mass of 142 u?

15 / 30

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

16 / 30

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

17 / 30

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

18 / 30

18. If 4 g of H₂ reacts with excess O₂, what is the mass of H₂O produced? Reaction:

19 / 30

19. Which of the following particles has the smallest mass in atomic mass units?

20 / 30

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

21 / 30

21. What is the molar mass of glucose ()?

22 / 30

22. How many liters of H₂ gas at STP are liberated when 2 g of Zn reacts with HCl? Reaction:

23 / 30

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

24 / 30

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

25 / 30

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

26 / 30

26. Which scientist first introduced the modern concept of the atom?

27 / 30

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

28 / 30

28. Which is correct about molar volume of gases at STP?

29 / 30

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

30 / 30

30. 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 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 fertilizer provides both nitrogen and phosphorus to crops?

2 / 50

2. The stoichiometric coefficients of reactants in the balanced equation are:

3 / 50

3. Why was the concept of atomic mass unit (amu) introduced?

4 / 50

4. Which of the following best explains the relation of chemistry with physics?

5 / 50

5. The study of pollutants in rivers and their effect on aquatic life shows the connection of chemistry with:

6 / 50

6. Which of the following is a diatomic molecule?

7 / 50

7. When 2 volumes of hydrogen combine with 1 volume of oxygen, the product formed is:

8 / 50

8. If 4 g of hydrogen reacts with 32 g of oxygen, which is the limiting reagent in ?

9 / 50

9. Why is percentage composition important in chemistry?

10 / 50

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

11 / 50

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

12 / 50

12. Which statement is correct about monoatomic molecules?

13 / 50

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

14 / 50

14. Why is the empirical formula important in chemistry?

15 / 50

15. Why is chemistry considered central among sciences?

16 / 50

16. The molecular mass of (ethane) is:

17 / 50

17. Which statement is true regarding the Law of Definite Proportions?

18 / 50

18. In the steel industry, chemistry is crucial for:

19 / 50

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

20 / 50

20. Which compound has the molar mass of 98 g/mol?

21 / 50

21. Which of the following is an incorrect pair of empirical and molecular formula?

22 / 50

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

23 / 50

23. Which information cannot be obtained directly from the molecular formula?

24 / 50

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

25 / 50

25. Which branch of science integrates chemistry and biology to study processes such as enzyme action?

26 / 50

26. Which of the following best defines a molecule?

27 / 50

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

28 / 50

28. Which statement is correct about molar mass?

29 / 50

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

30 / 50

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

31 / 50

31. Determine the atomicity of (ammonium sulfate).

32 / 50

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

33 / 50

33. Dalton’s fixed-composition view of compounds is limited because some solids are non-stoichiometric. Which is a classic example?

34 / 50

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

35 / 50

35. Why is atomicity an important concept?

36 / 50

36. For the reaction , what is the stoichiometric coefficient of ammonia?

37 / 50

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

38 / 50

38. Which statement correctly describes molecular composition?

39 / 50

39. Magnesium has three isotopes: Mg-24 (79%), Mg-25 (10%), and Mg-26 (11%). What is the average atomic mass?

40 / 50

40. Why is water (H₂O) classified as a molecule but not as an atom?

41 / 50

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

42 / 50

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

43 / 50

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

44 / 50

44. In the reaction , what is the stoichiometric coefficient of O₂?

45 / 50

45. 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?

46 / 50

46. Dalton assumed atoms of different elements have different masses. Which concept shows different elements can have the same mass number?

47 / 50

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

48 / 50

48. Which of the following correctly gives the percentage composition of oxygen in sulphur dioxide ()?

49 / 50

49. Why are atoms considered neutral?

50 / 50

50. Why is the Law of Multiple Proportions important in chemistry?

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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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