Some Basic Concepts Of Chemistry NEET Questions with FREE PDF

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IMPORTANCE OF CHEMISTRY MCQS
NATURE OF MATTER MCQS
PROPERTIES OF MATTER AND THEIR MEASUREMENT MCQS
UNCERTAINTY IN MEASUREMENT MCQS
LAWS OF CHEMICAL COMBINATION MCQS
DALTON’S ATOMIC THEORY MCQS
ATOMIC AND MOLECULAR MASSES MCQS
MOLE CONCEPT AND MOLAR MASSES MCQS
PERCENTAGE COMPOSITION MCQS
STOICHIOMETRY AND STOICHIOMETRIC CALCULATIONS MCQS

Some Basic Concepts Of Chemistry NEET Questions

1. Philosophy of changing substances into another form is called as _______

a) Physiology

b) Anatomy

c) Alchemy

d) Transformation

Answer: Alchemy

2. Rasopanishada says how the gunpowder mixture is used in war.

a) True

b) False

Answer: False

3. What does the Elixir of life of do?

a) grants immortality

b) cures diseases

c) kills a person

d) cause an incurable disease

Answer: grants immortality

4. The paintings on the walls of Ajanta and Ellora cave were based on ________

a) Varahmihir’s Brihat Samhitha

b) Sushruta Samhita

c) Rasopanishada

d) Charaka Samhita

Answer: Varahmihir’s Brihat Samhitha

5. Seeds of Manhua plant and oil of Eranda were used in making ________

a) cosmetic powder

b) color dye

c) perfume

d) soap

Answer: soap

6. Charaka Samhita is the oldest known book of Ayurvedic in India.

a) True

b) False

Answer: True

7. Patients suffering from AIDS can be helped using which of the following drugs?

a) Cisplatin

b) AZT (Azidothymidine)

c) Taxol

d) Codeine

Answer: AZT (Azidothymidine)

8. What are the basic constituents of matter?

a) Atoms & Molecules

b) Atoms & Moles

c) Molecules & Ions

d) Nuclei & Ions

Answer: Atoms & Molecules

9. What are pure substances classified as?

a) Elements and Atoms

b) Molecules and Compounds

c) Elements and Compounds

d) Atoms and Molecules

Answer: Elements and Compounds

10. When two or more atoms of different elements combine with each other in a fixed ratio, the molecule of a ____ is obtained.

a) Compound

b) Element

c) Atom

d) Ion

Answer: Compound

11. Compounds cannot be separated by chemical methods.

a) True

b) False

Answer: False

12. Point out an example of a compound.

a) Sugar solution

b) Hydrogen

c) Ammonia

d) Sodium

Answer: Ammonia

13. Water is a/an _______

a) Element

b) Compound

c) Pure substance

d) Mixture

Answer: Compound

14. The substances whose compositions are not uniform and different components are mixed are called _______

a) Homogenous substances

b) Heterogeneous substances

c) Pure substances

d) Elements

Answer: Heterogeneous substances

15. A ________ is made up of two or more pure substances which may be in any ratio.

a) Mixture

b) Element

c) Molecule

d) Atom

Answer: Mixture

16. Matter can be divided into two types i.e. mixture and pure substance.

a) True

b) False

Answer: True

17. What is the symbol of the amount of substance’s S.I. unit?

a) K

b) s

c) mol

d) kg

Answer: mol

18. What are the multiples for the prefixes yocto, atto respectively?

a) 10-24, 10-18

b) 10-9, 10-15

c) 10-15, 10-24

d) 10-24, 10-21

Answer: 10-24, 10-18

19. 1Litre = _______ m3.

a) 1000

b) 0.001

c) 1

d) 10

Answer: 0.001

20. What is the difference in units between Kelvin and centigrade scales of temperature?

a) 212.15

b) 32

c) 298

d) 273.15

Answer: 273.15

21. What is the human body temperature in Fahrenheit?

a) 212

b) 98.6

c) 273.15

d) 32

Answer: 98.6

22. Convert 40°C to °F.

a) 104K

b) 313°F

c) 104°F

d) 313K

Answer: 104°F

23. Which of the following may not be a physical property?

a) Odor

b) Color

c) Density

d) Composition

Answer: Composition

24. The observation of __________ properties needs a chemical change to occur.

a) Chemical

b) Physical

c) Extrinsic

d) Intrinsic

Answer: Chemical

25. How many significant figures does 0.057 have?

a) 2

b) 4

c) 3

d) 0

Answer: 2

26. How many significant figures does 63180 have?

a) 5

b) 4

c) 1

d) 2

Answer: 4

27. The exact value is 150m. A students record it as 140.1m in 1st turn and 140.8m in the 2nd turn. Comment his/her recordings.

a) precise

b) accurate

c) neither precise nor accurate

d) both precise and accurate

Answer: precise

28. The exact value is 150m. A students record it as 149.1m in 1st turn and 150.8m in the 2nd turn. Comment his/her recordings.

a) precise

b) accurate

c) neither precise nor accurate

d) both precise and accurate

Answer: accurate

29. Multiply 1.2 and 3.91. Obtain the result as per the rules of significant figures.

a) 4.692

b) 4.69

c) 5

d) 4.7

Answer: 4.7

30. How many significant figures are there in 60.6?

a) 4

b) 2

c) 3

d) 1

Answer: 3

31. Write 6354000000 in scientific notation.

a) 6.354 x 109

b) 6354 x 106

c) 0.64 x 1010

d) 6354000 x 103

Answer: 6.354 x 109

32. _________ is referred to as the closeness of different measurements for the same quantity.

a) Accuracy

b) Precision

c) Analysis

d) Dimension

Answer: Precision

33. Who proposed the Law of Definite Composition?

a) Joseph Proust

b) Lorenzo Romano

c) Joseph Louis

d) Antoine Lavoisier

Answer: Joseph Proust

34. Law of Definite Composition is also known as ________

a) Law of Multiple Proportions

b) Avogadro’s Law

c) Law of Definite Proportion

d) Law of Conservation of Mass

Answer: Law of Definite Proportion

35. The volumes of hydrogen & oxygen when combined bear a simple ratio of 2:1.This is explained by ________

a) Law of Multiple Proportions

b) Avogadro’s Law

c) Law of Definite Proportion

d) Gay Lussac’s Law of Gaseous Volumes

Answer: Gay Lussac’s Law of Gaseous Volumes

36. Who proposed that equal volumes of all gases at the same temperature & given pressure should contain an equal number of molecules?

a) Antoine Lavoisier

b) Joseph Proust

c) Avogadro

d) Joseph Louis

Answer: Avogadro

37. Which of the following is not a law of chemical combination?

a) Law of Multiple Proportions

b) Avogadro’s Law

c) Law of Definite Proportion

d) Law of Conservation of volume

Answer: Law of Conservation of volume

38. Which of the following may be an incorrect statement?

a) Law of Definite Composition is also known as Law of Definite composition

b) Mass can neither be created nor destroyed is Law of Conservation of Volume

c) Antoine Lavoisier conducted many experiments regarding combustion

d) Five basic laws are required to govern the combination of elements to form compounds

Answer: Mass can neither be created nor destroyed is Law of Conservation of Volume

39. How many basic laws are required to govern the combination of elements to form compounds?

a) 6

b) 5

c) 4

d) 1

Answer: 5

40. Who proposed Law of Conservation of Mass?

a) Antoine Lavoisier

b) Joseph Proust

c) Lorenzo Romano

d) Joseph Louis

Answer: Antoine Lavoisier

41. Which of the following may not be explained by Dalton’s atomic theory?

a) reason for combining atoms

b) conservation of mass

c) chemical philosophy

d) indivisible atoms

Answer: reason for combining atoms

42. Law of conservation of mass isn’t explained in Dalton’s atomic theory.

a) True

b) False

Answer: False

43. What is 1 Dalton?

a) a unified mass unit, 1.360539040(20)×10−27kg

b) a unified mass unit, 1.640539040(20)×10−27kg

c) a unified mass unit, 1.660539040(20)×10−27kg

d) a unified mass unit, 1.660539040(20)×10−27kg

Answer: a unified mass unit, 1.660539040(20)×10−27kg

44. Could Dalton’s atomic theory explain the laws of chemical combinations?

a) No

b) Yes

c) Only a few

d) Except one

Answer: Yes

45. They are no limitations to Dalton’s atomic theory.

a) True

b) False

Answer: False

46. All atoms of a given element have identical __________ including identical _________

a) Properties, mass

b) Weight, volume

c) Volume, properties

d) Temperature, pressure

Answer: Properties, mass

47. According to Dalton’s Atomic Theory, matter consists of indivisible _______

a) Molecules

b) Atoms

c) Ions

d) Mixtures

Answer: Atoms

48. Atoms of different elements differ in mass.

a) True

b) False

Answer: True

49. A sample of carbon that contains 70% carbon-12 and 30% carbon-14. What do you think is the average atomic mass of this sample?

a) 14.5

b) 14.14

c) 14

d) 12

Answer: 14

50. ______ is the sum of atomic masses of the elements present in a molecule.

a) Average atomic mass

b) Atomic mass

c) Gram formula mass

d) Molecular mass

Answer: Molecular mass

51. What’s the molecular mass of carbon dioxide?

a) 43

b) 28

c) 44

d) 40

Answer: 44

52. What’s the formula mass of NaCl?

a) 23 u

b) 35.5 u

c) 58 u

d) 58.5 u

Answer: 58.5 u

53. Calculate the molecular mass of sucrose(C12H22O11) molecule?

a) 342 amu

b) 343 amu

c) 341 amu

d) 340 amu

Answer: 342 amu

54. As, per the current system, carbon-12 has been taken as the standard for measuring atomic masses.

a) True

b) False

Answer: True

55. What is the mass of hydrogen in terms of amu?

a) 1.0020 amu

b) 1.0180 amu

c) 1.0070 amu

d) 1.0080 amu

Answer: 1.0080 amu

56. What is the abbreviation of amu?

a) Atomic matter unit

b) Atomic mass unified

c) Atomic mass unit

d) At mass unity

Answer: Atomic mass unit

57. 12.044 x 1023 atoms of oxygen contains

a) 1 mole of oxygen

b) 2 moles of oxygen

c) 3 moles of oxygen

d) 4 moles of oxygen

Answer: 2 moles of oxygen

58. If one mole of ammonia contains “y” number of particles, then how many particles do 1 mole of glucose contain?

a) 2y

b) 0.5y

c) 3y

d) y

Answer: y

59. What’s the number of particles in 10 moles of hydrochloric acid?

a) 6.022 x 1022 particles

b) 6.022 x 1023 particles

c) 6.22 x 1023 particles

d) 3.22 x 1022 particles

Answer: 6.022 x 1022 particles

60. Which of the following statement is correct?

a) The value of Avogadro’s number is 6.022×1022 atoms

b) One molecule of any substance contains Avogadro’s number of particles

c) One mole is the amount of a substance that contains as many particles as there are atoms in exactly 12 g of the carbon atom

d) 1 u is not equal to Ma/NA

Answer: One mole is the amount of a substance that contains as many particles as there are atoms in exactly 12 g of the carbon atom

61. One mole of sucrose contains how many grams of sucrose?

a) 342g

b) 343g

c) 341g

d) 340g

Answer: 342g

62. 1 mole of ammonia is of 17 g. Then what is the mass of 0.3 moles of ammonia?

a) 21g

b) 2.1g

c) 17g

d) 1g

Answer: 2.1g

63. According to S.I. the system, ______ was used to measure the amount of substance.

a) mole

b) weight machine

c) weight

d) mass

Answer: mole

64. What’s the number of entities or particles together in mole concept known as?

a) Boltzmann constant

b) Avogadro’s number

c) Universal gas constant

d) Reynold’s number

Answer: Avogadro’s number

65. The molecular formula of a compound is C6H12O6. What’s the empirical formula for this compound?

a) C6H12O6

b) CHO

c) C2H6O2

d) CH2O

Answer: CH2O

66. A compound consists of 52.17% of carbon, 13.04% of hydrogen and 34.78% of oxygen. Find the molecular formula if the given molecular weight of the compound is 46g.

a) C2H5OH

b) C2H6

c) C6H12O6

d) CH2O

Answer: C2H5OH

67. Which of the following cannot be a molecular formula for an empirical formula HO?

a) H2O

b) H2O2

c) HO

d) HO2

Answer: H2O2

68. In glucose simplest ratio between C, H and O is ________

a) 6:12:6

b) 3:4:3

c) 1:2:1

d) 2:3:2

Answer: 1:2:1

69. Which of the following is true regarding molecular formula?

a) actual whole numbered ratio

b) rational numbered ratio

c) simplest possible whole numbered ratio

d) the same as the empirical ratio

Answer: actual whole numbered ratio

70. Which of the following cannot be an empirical formula?

a) NH3

b) C5H10

c) H2O

d) NaCl

Answer: C5H10

71. A _______ formula represents a whole number ratio to the simplest form.

a) Molecular

b) Empirical

c) Simpler

d) Shorter

Answer: b

72. Even without knowing the mass percent of each element, we can calculate the empirical formula.

a) True

b) False

Answer: b

73. Calculate the mass percent of magnesium in the formation of magnesium oxide.

a) 0.3

b) 1.5

c) 0.67

d) 0.6

Answer: 0.6

74. A solution contains 8 moles of solute and the mass of the solution is 4 kg. What’s the molality of this solution?

a) 5 mol/kg

b) 8 mol/kg

c) 4 mol/kg

d) 0.5 mol/kg

Answer: 0.5 mol/kg

75. In a container, there are 4 moles of nitrogen, 3 moles of oxygen and 7 moles of hydrogen; find out the mole fraction of oxygen in this reaction.

a) 0.2143

b) 0.2142

c) 0.1234

d) 0.2434

Answer: 0.2143

76. Find the amount of carbon dioxide produced by the combustion of 20g of methane.

a) 44g

b) 20g

c) 66g

d) 22g

Answer: 66g

77. What’s the balanced equation of CO2 + H2O → C6H12O6 + O2?

a) CO2 + H2O → C6H12O6 + O2

b) 6 CO2 + 6 H2O → C6H12O6 + 6 O2

c) 6 CO2 + 6 H2O → C6H12O6 + 2 O2

d) 3 CO2 + 2H2O → C6H12O6 + O2

Answer: 6 CO2 + 6 H2O → C6H12O6 + 6 O2

78. In a particular reaction, one of the reactants limits the number of products formed. That is called as _______

a) Limiting reagent

b) Limiting product

c) Excessive reagent

d) Excessive reactant

Answer: Limiting reagent

79. Which of the following is not true regarding balanced chemical equations?

a) They contain the same number of atoms on each side

b) Electrons are also balanced

c) An equal number of molecules on both the side

d) Follows the law of conservation of mass

Answer: An equal number of molecules on both the side

80. Which of the given reactions are counted as balanced reactions?

a) H2 + O2 → 2H2O

b) 4Al + 3O2 → 2Al2O3

c) Mg(OH)2 + 2HNO3 → 2Mg(NO3)2 + 2H2O

d) N2 + 3H2 → NH3

Answer: 4Al + 3O2 → 2Al2O3

Some Basic Concepts Of Chemistry NEET Questions PDF Download

Complete Class 11 Chemistry Chapterwise Questions and Answers List

Some Basic Concepts of Chemistry
Structure of Atom
Classification of Elements and Periodicity in Properties
Chemical Bonding and Molecular Structure
States of Matter
Thermodynamics
Equilibrium
Redox Reactions
Hydrogen
s-Block Elements
p-Block Elements
Organic Chemistry – Basic Principles and Technique
Hydrocarbons
Environmental Chemistry

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