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MDCAT Fundamental Concepts of Chemistry Online Test

Umaima Harmain RaoLast Updated: May 24, 2025

Chemistry Basic Concepts MCQS Online Test

MDCAT Chemistry Basic Concepts Chapter 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

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Page 1 of 3

Chemistry

1. Diameter of an atom is in the range of

0.2 Pm

0.2 nm

0.2 m

2 x10¯¹⁰

2. Which one of the following is ambiguous?

A mole of potassium ions

A mole of electrons

A mole of hydrogen

A mole of sodium atoms

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

3 x 6.02 x 10²³

6.02 x 10²³

6.02 x 10²³ x 2

4 x 6.02 x 10²³

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

One moles of N₂ will produce two moles of NH₃.

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

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

5. Which of the following represents a compound?

Made up of 10 atoms

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

A pure substance made up of one type of atom

Two words in one word

6. The modern atomic weight scale is based on

H¹

C¹³

C¹²

O¹⁶

7. Which of the following represents an element?

The periodic table

A pure substance made up of one type of atom

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

A compound made up of one type of element

8. 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

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

7.31 x 10¯²³

1.37 x 10²²

1.99 x 10¯²³

4.65 x 10¯²³

10. The compound having highest percent of oxygen is

H₂O

C₂H₅OH

CH₃COOH

CH₃COCH₃

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

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

They possess same chemical properties

They possess same position in the periodic table

They possess same physical properties

They possess different mass number

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

Osmosis

Fractional distillation technique

Chromatography

Graham’s law of diffusion technique

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

It can be applied to all

NaC1

H₂O

CC1₄

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

1, 1, 2, 2, 1

2, 2, 1, 1, 1

2, 2, 1, 2, 1

2, 1, 1, 2, 1

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

Ultraviolet spectrometer

Infra-red spectrometer

Atomic absorption spectrometer

Mass spectrometer

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

3.01 x 10²³

6.02 x 10²²

6.02 x 10²³

3.01 x 10²²

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

Ionic charges

Ionic compounds

Ionic atoms

Ionic element

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

The atomic mass subtracted the number of electrons

The atomic mass plus the number of electrons

The atomic mass subtracted the number of protons

The atomic mass plus the number of protons

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

Gain electrons and protons

None of these

Lose electrons

Lose electrons and protons

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

5000 mole

0.005 mole

5 moles

10 moles

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

Carbon dioxide

Methane

Water

Sugar

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

0.75

1.00

0.5

0.25

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

Neutrons and electrons

Protons and electrons

Electrons and shells

Protons and neutrons

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

All of these

To reduce the economy of the process

To reduce the time for completion of the reaction

To carry out compete combustion

Page 2 of 3

26. Difference in density is the basis of

Ultrafiltration

Gravity separation

Molecular sieving

Molecular attraction

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

SO₂

SO₃

S₂O₃

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

83% hydrogen and 17% carbon

14% hydrogen and 86% carbon

86% hydrogen and 14% carbon

17% hydrogen and 83% carbon

29. 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,

Nil, it is dimensionless constant

Nm¯²s¯²

Newton

Kg m¯¹s¯¹

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

2 elements and a total of 3 atoms

2 elements and a total of 2 atoms

3 elements and a total of 3 atoms

3 elements and a total of 2 atoms

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

Molecular formula /n = Empirical formula

Empirical formula x n² = Molecular formula

Empirical formula /n = Molecular formula

Empirical formula x √n = Molecular formula

32. 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?

CuCl₃

Cu₂Cl₃

CuCl₂

CuCl

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

More than one could be a molecular formula for CH₂

Its molecular formula does not exist

Only one molecular formula (C2H2) is possible

Only one molecular formula (CH2) is possible

34. 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

35. Percent of calcium in calcium carbonate is

80%

30%

40%

20%

36. What are the parts of an atom?

Nucleus, element, carbon, space

Ions, electrons, neutrons, water

Protons, neutrons, nucleus, mass

Protons, neutrons, electrons, nucleus

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

C₄H₈O₄

CH₂O

C₂H₄O₂

C₃H₆O₃

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

C₆H₁₂O₆

H₂O₂

C₂H₄

BaO₂

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

Hund’s rule

Dalton’s law

Moley’s law

Newton’s law

40. 1 mole of CH₄ contains

1.81 x 10²³ molecules of CH₄

3.0 g of carbon

4 g-atom of hydrogen

6.02 x 10²³ atoms of H

41. What is a chemical compound?

A combination of two protons and two electrons

A combination of two or more chemical elements

A mixture of two or more substance

A subatomic particle

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

MC1

MC1₃

MCL₂

M₂C1₂

43. What is the net charge on ferrous ion?

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

1.0

1.11

0.90

0.11

45. Indicate the incorrect statement form the following

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

Actual yield is always less than theoretical yield

Stoichiometric calculation can only be done if no side reaction happen

A limiting reactant is used at the end of reaction

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

Nucleus

Ions

Neutrons

Protons

47. Isotopes differ in the

Number of neutrons

Number of electrons

Number of atoms

Number of protons

48. What is a multivalent ion?

Some ions can have only one charge

Only negatively charged

An ion that can have more than one charge

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

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

All of above

Combustion method

Duma’s method

K. Jeldahl’s method

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

Water

Gold

Sodium Chloride

Soil

Page 3 of 3

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

Oxygen gas

Vinegar

Air

Water

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

Graham’s Law of diffusion

Sublimation

Crystallization

Chromatography

53. Empirical formula of chloroform is

CH₃cl

CHCl

CHCl₃

CH₂C₁₂

54. 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

Constant volume

Definite proportions

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

N₂O

N₂O₃

NO₂

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

80.03%

20.05%

19.97%

50%

57. The prefix 10¹⁸ is

Nano

Giga

Exa

Kilo

58. The percentage of oxygen in NaOH is

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

12 x 10²³

1.2 x 10²³

6 x 10²²

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

CuO, Cu₂O

CS₂, FeSO₄

H₂S, SO₂

NH₃, HC1

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

KOH

Mg(ClO₄)₂

Al₂O₃

SiO₂

62. Which of the following is an element?

Gold

Water

Common Salt

Sugar

63. What are the two different types of ions?

Negative and positive

Polyatomic and compound ions

Polyatomic and multivalent

Electrons and protons

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

32.47%

12.26%

24.51%

66.67%

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

Crystal

Compound

Mixture

Element

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

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

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

1.12 dm³

112 Cm³

2.24 dm³

22.4 dm³

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

All substances are made of matter

Matter always consists of molecules

All matter contains chemical elements

Matter is always composed of atoms

70. 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

71. 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

1:1:1

1:16:2

2:16:2

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Umaima Harmain RaoLast Updated: May 24, 2025

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15 Comments

jaweria says:

November 9, 2022 at 5:11 pm

Got 97 %

Rom says:

September 4, 2021 at 6:55 pm

No bro the right ans is what is in test bcz *n* integer must be multiplied with E F to form MF and when it go towards other side it will be as a denominator of MF.

Saira sahfi says:

August 16, 2021 at 8:26 pm

Good experience and good practice test is very nice entry test practice .

1. Saira shafi says:
  
  August 16, 2021 at 8:30 pm
  
  Good experience test
  
Tarique Hussain says:

July 15, 2021 at 9:18 pm

Sir question to show nhn ho rhy hn

RK Durrani says:

August 29, 2020 at 7:39 am

Too much helpful for preparation

m.umair says:

August 21, 2020 at 9:21 am

Just want improvement

Rajab Ali says:

July 5, 2017 at 1:08 pm

Got 95%

1. Sara says:
  
  June 24, 2021 at 8:04 pm
  
  Did you get admission in medical college?
  
Afifa zahid says:

August 20, 2016 at 10:01 pm

Absolutely,mine the 1st most qs is wrong,now i am not going to give this test

zubair khalid says:

August 17, 2016 at 1:35 am

question no. 19 is incorrect plzz correct it….

zubair khalid says:

August 17, 2016 at 1:33 am

EMPIRICAL FORMULA/n=molecular formula it’s the correct answer but they concider it as wrong what a LOL..

1. NotSuitableHere says:
  
  August 26, 2021 at 9:05 am
  
  You are wrong man, they are correct.
  
2. Rom says:
  
  September 4, 2021 at 6:54 pm
  
  No bro the right ans is what is in test bcz *n* integer must be multiplied with E F to form MF and when it go towards other side it will be as a denominator of MF.
  
3. Erana emra says:
  
  April 26, 2022 at 11:54 pm
  
  Broo it is
  Molecular formula = n ( emperical formula)
  Soo….
  MF/n = emperical formula

MDCAT Fundamental Concepts of Chemistry Online Test

Chemistry Basic Concepts MCQS Online Test

MDCAT Chemistry Basic Concepts Chapter Online Test

MDCAT Chemistry Basic Concepts Test

Chemistry

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Umaima Harmain Rao

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Chemistry Basic Concepts MCQS Online Test

MDCAT Chemistry Basic Concepts Chapter Online Test

MDCAT Chemistry Basic Concepts Test

Chemistry

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