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MDCAT Fundamental Concepts of Chemistry Test Online MCQs

Maan AliLast Updated: July 12, 2025

MDCAT Fundamental Concepts of Chemistry Online Test

Prepare for MDCAT Chemistry with this online MCQ test on Fundamental Concepts of Chemistry. This quiz covers key basics such as atomic mass, moles, empirical and molecular formulas, and chemical calculations, aligned with the MDCAT 2025 syllabus to build a strong foundation for the subject.

MDCAT 2025 Basic Concepts Online Test

Total Questions:	71
Time Allowed:	30 Minutes
Total Marks:	71
How to Attempt Test:	Please choose the right Option in MCQ-type question.
Test Helpful For:	MDCAT Entry Test Chemistry Online Test Interview Questions about Chemisttry All Universities Entrance Test Recruitments Tests

MDCAT Chemistry Basic Concepts Test Question with Answer

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Page 1 of 3

1. What is the net charge on ferrous ion?

2. How do you calculate the number of neutrons in an atom?

The atomic mass subtracted the number of protons

The atomic mass plus the number of electrons

The atomic mass plus the number of protons

The atomic mass subtracted the number of electrons

3. How many number of ions are there in 98 grams of sulphate ions?

6.02 x 10²³ x 2

4 x 6.02 x 10²³

6.02 x 10²³

3 x 6.02 x 10²³

4. Ayesha required an aqueous solution of sodium chloride. She made the solution by dissolving salt in:

Water

Oxygen gas

Air

Vinegar

5. The compound having highest percent of oxygen is

H₂O

CH₃COCH₃

C₂H₅OH

CH₃COOH

6. How many moles of Helium gas occupy 22.4 L at 0°C at 1 atm. Pressure?

1.11

0.11

1.0

0.90

7. Copper (II) oxide is mixed with organic compound during combustion. The purpose is

To reduce the economy of the process

All of these

To reduce the time for completion of the reaction

To carry out compete combustion

8. What are the two different types of ions?

Polyatomic and compound ions

Negative and positive

Polyatomic and multivalent

Electrons and protons

9. Molecular compounds can be found in all three states of matter at room temperature. Which molecule compound is a liquid at room temperature?

Methane

Carbon dioxide

Water

Sugar

10. The Number of oxygen atoms in 4.4 g of CO2 is approximately

12 x 10²³

1.2 x 10²³

6 x 10²²

11. Isotopes differ in the

Number of electrons

Number of atoms

Number of protons

Number of neutrons

12. Which of the following represents a compound?

Pure substances made up to of 2 or more types of atoms

Two words in one word

A pure substance made up of one type of atom

Made up of 10 atoms

13. What does the atomic number of an atom represent?

Protons and neutrons

Electrons and shells

Protons and electrons

Neutrons and electrons

14. If the empirical formula of compound is CH₂. Which of the following is true about its molecular formula?

Its molecular formula does not exist

Only one molecular formula (C2H2) is possible

More than one could be a molecular formula for CH₂

Only one molecular formula (CH2) is possible

15. What is a multivalent ion?

Some ions can have only one charge

Only negatively charged

Ions that are made of more than one type of atom and act as one

An ion that can have more than one charge

16. Which of the following is NOT a pure substance?

Water

Gold

Soil

Sodium Chloride

17. The hydrogen phosphate of certain metal has formula MHPO₄. The formula of metal chloride would be

M₂C1₂

MC1₃

MC1

MCL₂

18. A gaseous mixture contains 50% helium and 50% methane by volume. What is the percent by weight of methane in the mixture?

20.05%

50%

19.97%

80.03%

19. Balance the following equation using minimum integral coefficients: (NH₃ + O₂ → NO₂ + H₂O) Find the stoichiometric coefficient for oxygen gas O₂:

20. Difference in density is the basis of

Ultrafiltration

Molecular attraction

Gravity separation

Molecular sieving

21. Indicate the incorrect statement form the following

The empirical and molecular formula of some of the compounds are same

A limiting reactant is used at the end of reaction

Actual yield is always less than theoretical yield

Stoichiometric calculation can only be done if no side reaction happen

22. How many moles of CO₂ are present in 220 mg?

5 moles

0.005 mole

5000 mole

10 moles

23. What is the percent water in hydrated calcium chloride (CaC1₂ 2H₂O)?

66.67%

32.47%

12.26%

24.51%

24. Bromine has two isotopes having the relative abundances as ⁷⁵₃₉Br = 50.51% and ⁸¹₃₅Br= 49.49%. The average atomic mass of bromine is

79.5

25. Which of the following represents an element?

A compound made up of one type of element

A pure substance made up of two or more types of atoms

The periodic table

A pure substance made up of one type of atom

Page 2 of 3

26. Among the following pairs, the one which illustrates the law of multiple proportions is

H₂S, SO₂

CS₂, FeSO₄

CuO, Cu₂O

NH₃, HC1

27. An anhydrous salt of copper is found to contain 52.7% chlorine and 47.3% copper by mass. What is the empirical formula for this salt?

Cu₂Cl₃

CuCl₂

CuCl

CuCl₃

28. For which of the following terms empirical formula cannot be applied?

It can be applied to all

CC1₄

NaC1

H₂O

29. What is correct relationship between empirical and molecular formulas?

Empirical formula x √n = Molecular formula

Molecular formula /n = Empirical formula

Empirical formula x n² = Molecular formula

Empirical formula /n = Molecular formula

30. Diameter of an atom is in the range of

0.2 Pm

2 x10¯¹⁰

0.2 nm

0.2 m

31. How many elements are present in two molecules of aspirin? The formula for aspirin is C₉H₈O₄.

32. How can you separate the mixture of two gases of different atomic masses?

Crystallization

Chromatography

Sublimation

Graham’s Law of diffusion

33. The modern atomic weight scale is based on

C¹²

H¹

O¹⁶

C¹³

34. Percent of calcium in calcium carbonate is

80%

40%

30%

20%

35. Most atoms are neutral, to become a positive ion the atom must:

Lose electrons and protons

Lose electrons

Gain electrons and protons

None of these

36. Since atoms are neutral, the number of electrons is equal to the number of:

Protons

Ions

Nucleus

Neutrons

37. A ring contains 1.2g of diamond. How many number of carbon atoms are in diamond?

6.02 x 10²³

3.01 x 10²²

6.02 x 10²²

3.01 x 10²³

38. Which one of the following is ambiguous?

A mole of potassium ions

A mole of sodium atoms

A mole of hydrogen

A mole of electrons

39. The empirical formula of a compound is CH₂O and its molecular mass is 120. The molecular formula of the compound is

C₃H₆O₃

C₄H₈O₄

C₂H₄O₂

CH₂O

40. Which of the following is an element?

Water

Gold

Common Salt

Sugar

41. The percentage of oxygen in NaOH is

42. Calculate the weight, in grams, of one molecule of carbon dioxide, CO₂.

4.65 x 10¯²³

1.99 x 10¯²³

7.31 x 10¯²³

1.37 x 10²²

43. If Na is Avogadro’s number, then number of valence electrons in 4.2 g of nitride ions N³¯ is

3.2 Na

2.4 Na

1.6 Na

4.2 Na

44. How will you separate a mixture of two gases?

Chromatography

Fractional distillation technique

Graham’s law of diffusion technique

Osmosis

45. Which of the following is NOT true of matter on the Earth?

Matter is always composed of atoms

All matter contains chemical elements

Matter always consists of molecules

All substances are made of matter

46. Which of the following is a pure substance made up of two or more types of atoms or elements?

Mixture

Element

Compound

Crystal

47. Vapor density of a gas is 22. What is its molecular mass?

48. A compound contains 6.0 g of carbon and 1.0 g of hydrogen. The percent composition of the compound is:

86% hydrogen and 14% carbon

14% hydrogen and 86% carbon

83% hydrogen and 17% carbon

17% hydrogen and 83% carbon

49. Which of the following statements is FALSE for the chemical equation given below in which nitrogen gas reacts with hydrogen gas to form ammonia gas assuming the reaction goes to completion?
N₂ + 3H₂ → 2NH₃

One moles of N₂ will produce two moles of NH₃.

One molecule of nitrogen requires three molecules of hydrogen for complete reaction.

The reaction of three moles of hydrogen gas will produce 17 g of ammonia

The reaction of one mole of H₂ will produce 2/3 moles of NH₃.

50. How many moles of KBrO₃ are required to prepare 0.0700 moles of Br₂ according to the reaction: KBrO₃ + 5KBr + 6HNO₃ → 6KNO₃ + 3Br₂ + 3H₂O

0.0704

0.210

0.0233

0.0732

Page 3 of 3

51. The empirical formula of the compound having 50% sulphur and 50% oxygen by mass is

SO₃

SO₂

S₂O₃

52. 1 mole of CH₄ contains

4 g-atom of hydrogen

6.02 x 10²³ atoms of H

3.0 g of carbon

1.81 x 10²³ molecules of CH₄

53. Which law directly explains the law of conservation of mass?

Newton’s law

Moley’s law

Dalton’s law

Hund’s rule

54. The set of numerical coefficients that balances the chemical equation K₂CrO₄ + CH1 → K₂Cr₂O₇ + KC1 + H₂O

2, 2, 1, 1, 1

2, 1, 1, 2, 1

1, 1, 2, 2, 1

2, 2, 1, 2, 1

55. Which of the following could be an empirical formula?

C₆H₁₂O₆

C₂H₄

H₂O₂

BaO₂

56. What are the ratios among the volumes of gases of ³²O₂,²H₂, and ¹⁶CH₄ if equal mass of each gas is taken?

2:16:1

2:16:2

1:1:1

1:16:2

57. Irrespective of the source, pure sample of water always yields 88.89% mass of oxygen and 11.11% mass of hydrogen. This is explained by the law of

Multiple proportions

Conservation of mass

Definite proportions

Constant volume

58. Empirical formula of chloroform is

CH₂C₁₂

CHCl₃

CH₃cl

CHCl

59. Which of the following statements is wrong about isotopes?

They possess same physical properties

They possess different mass number

They possess same position in the periodic table

They possess same chemical properties

60. Water (H₂O) is a common compound made up of:

3 elements and a total of 2 atoms

3 elements and a total of 3 atoms

2 elements and a total of 3 atoms

2 elements and a total of 2 atoms

61. What are the parts of an atom?

Protons, neutrons, electrons, nucleus

Nucleus, element, carbon, space

Ions, electrons, neutrons, water

Protons, neutrons, nucleus, mass

62. Which of the following method is used to estimate oxygen in an organic compound?

Combustion method

K. Jeldahl’s method

Duma’s method

All of above

63. What is a chemical compound?

A combination of two protons and two electrons

A mixture of two or more substance

A subatomic particle

A combination of two or more chemical elements

64. The volume occupied by 28 gram of N₂ at STP?

22.4 dm³

112 Cm³

2.24 dm³

1.12 dm³

65. Calculate the number of moles of CaCO₃ (Formula weight = 100) in a sample that weighs 25.0 grams.

0.25

1.00

0.5

0.75

66. The prefix 10¹⁸ is

Exa

Giga

Kilo

Nano

67. An oxide of nitrogen contain 36.8% nitrogen and 63.2% oxygen by mass. Calculate its empirical formula.

N₂O

NO₂

N₂O₃

68. One of the substances is used to absorb CO₂ gas in combustion analysis. Which is that substance?

SiO₂

Mg(ClO₄)₂

KOH

Al₂O₃

69. The coefficient of viscosity η of a fluid moving steadily between two surfaces is given by the formula, f = η dV/dx where f is the frictional force on the fluid. A is an area in the fluid and dV/dx is the velocity gradient inside the fluid at that area. The S.I. unit of viscosity coefficient η is given as,

Newton

Nil, it is dimensionless constant

Nm¯²s¯²

Kg m¯¹s¯¹

70. To differentiate between C-12, C-13 and C-14, the instrument that you would use is

Ultraviolet spectrometer

Infra-red spectrometer

Mass spectrometer

Atomic absorption spectrometer

71. What do you call pure substances that are formed from the attraction between positive ions and negative ions?

Ionic atoms

Ionic element

Ionic charges

Ionic compounds

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Maan AliLast Updated: July 12, 2025

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33 Comments

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October 26, 2022 at 2:22 pm

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October 26, 2022 at 1:52 pm

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August 13, 2022 at 11:27 am

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November 16, 2021 at 9:34 am

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October 12, 2020 at 4:43 pm

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Momo says:

December 9, 2018 at 11:24 am

Mass of one mole of iodine is 254g not 245g. (127*2=254g)

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MDCAT Fundamental Concepts of Chemistry Test Online MCQs

MDCAT Fundamental Concepts of Chemistry Online Test

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