Important MCQs of Chemistry for higher marks in board and entry tests
Welcome to our latest blog post, where we will be providing 135 Chemistry MCQs on the chapter "Fundamentals of Chemistry". These questions cover a wide range of topics including Definition, and Branches of chemistry, History of Chemistry, Elements, Compounds, Mixtures, Atomic Mass, Atomic Number, Chemical Formula and its types, Relative atomic mass, Average Atomic mass, Chemical Species (Ions, Molecular Ions, and Free Radicals), Molecules and its classification, Mole, Avogardro's Number, and Chemical Calculations involving mole and Avogardo's Number. These MCQs have been designed to help students prepare for a variety of competitive and entrance exams, including the Board of Intermediate and Secondary Education (BISE), Federal Board Examination, EATA test preparation, NEET, NMDCAT, CSS, PMS, ASI, Cadet Colleges Preps, and more. Whether you're looking to improve your marks or simply want to test your knowledge of the subject, these MCQs are the perfect tool for achieving your goals. So, let's get started and take your Chemistry knowledge to the next level!
MCQs on some basic definitions.
1. What is the knowledge obtained through observations and experiments called?
A. ScienceB. Chemistry
C. Matter
D. Pure Substance
2. What is the branch of science that deals with the study of properties, structure, composition, and changes in matter, as well as the laws and principles governing these changes?
A. Science
B. Chemistry
C. Matter
D. Pure Substance
3. What is the definition of matter?
A. Anything that occupies space and has mass
B. The branch of science that deals with the study of properties, structure, composition, and changes in matter
C. A pure substance that can't be broken down into simpler substances by ordinary chemical or physical means
D. Anything that can be formed as well as can be separated by physical means only
4. What is the definition of a pure substance?
A. Anything that is obtained from different sources but has the same composition and properties
B. The branch of science that deals with the study of properties, structure, composition, and changes in matter
C. A pure substance that can't be broken down into simpler substances by ordinary chemical or physical means
D. Anything that can be formed as well as can be separated by physical means only
5. What is the definition of an element?
A. A pure substance that can't be broken down into simpler substances by ordinary chemical or physical means
B. The branch of science that deals with the study of properties, structure, composition, and changes in matter
C. Anything that is obtained from different sources but has the same composition and properties
D. Anything that can be formed as well as can be separated by physical means only
6. What is the definition of a compound?
A. A pure substance that can be only formed as well as broken down into simpler substances by chemical means only
B. The branch of science that deals with the study of properties, structure, composition, and changes in matter
C. Anything that is obtained from different sources but has the same composition and properties
D. Anything that can be formed as well as can be separated by physical means only
7. What is the definition of a mixture?
A. Anything that can be formed as well as can be separated by physical means only
B. The branch of science that deals with the study of properties, structure, composition, and changes in matter
C. Anything that is obtained from different sources but has the same composition and properties
D. A pure substance that can be only formed as well as broken down into simpler substances by chemical means only
A. The period of Muslim chemists
B. The period of Greek chemists
C. The period of Roman chemists
D. The period of Egyptian chemists
9. How did the knowledge of Alchemists and their techniques spread to Europe?
A. Through trade and commerce
B. Through invasions and conquests
C. Gradually over time
D. Through scientific collaboration
10. What was the term used for the knowledge of Alchemists before it changed to a purely English word?
A. Chemistry
B. Alchemistry
C. Arab science
D. Alchemy
11. What were some of the elements discovered by Al-Chemists?
A. Gold, Silver, Copper
B. Arsenic, Antimony, Bismuth
C. Oxygen, Hydrogen, Nitrogen
D. Carbon, Silicon, Germanium
12. What laboratory equipment did Al-Chemists invent?
A. Microscope, centrifuge, pipettes, test tubes
B. Bunsen burner, thermometer, barometer, hygrometer
C. Beaker, crucibles, retorts, furnaces
D. Spectrophotometer, chromatograph, oscilloscope, centrifuge
13. What laboratory procedures did Al-Chemists invent?
A. Sublimation, fermentation, filtration, calcination
B. Digestion, distillation, centrifugation, crystallization
C. Chromatography, electrophoresis, spectrophotometry, microscopy
D. Hydrogenation, oxidation, reduction, neutralization
14. What did Al-Chemists prepare?
A. Acids, Alkalies (Bases), medicines, and Alcohol
B. Gold, Silver, Copper
C. Oxygen, Hydrogen, Nitrogen
D. Carbon, Silicon, Germanium
15. Who is known as the father of Chemistry?
A. Jabir-Ibn-e-Hayyan
B. Robert Boyle
C. Antonie van Leeuwenhoek
D. John Dalton
16. In what year was Jabir-Ibn-e-Hayyan born?
A. 712 AD
B. 803 AD
C. 1021 AD
D. 721 AD
17. In what year did Jabir-Ibn-e-Hayyan die?
A. 721 AD
B. 803 AD
C. 1021 AD
D. 1203 AD
18. What was Jabir-Ibn-e-Hayyan's contribution to Chemistry?
A. He described the method of production of white lead
B. He invented a chemical and experimental procedure for the preparation of Nitric acid (HNO3) and Hydrochloric acid (HCl)
C. He described methods of fractional distillation and a method for the extraction of metals
D. All of the above
19. What was the year of birth of Muhammad Ibne-Zikriya Al-Razi?
A. 864 AD
B. 930 AD
C. 800 AD
D. 700 AD
20. IWhat is the main topic of Al-Asrar, the famous book written by Muhammad Ibne-Zikriya Al-Razi?
A. Surgery
B. Philosophy
C. Chemistry
D. Physiology
21. How did Muhammad Ibne-Zikriya Al-Razi prepare alcohol?
A. Distillation
B. Synthesis
C. Fermentation
D. Extraction
22. Muhammad Ibne-Zikriya Al-Razi is known for dividing things into which two categories?
A. Living and non-living
B. Organic and inorganic
C. Natural and artificial
D. Solid and liquid
23. What was the year of birth of Al-Beruni?
A. 937 AD
B. 1048 AD
C. 900 AD
D. 1000 AD
24. In which field did Al-Beruni make contributions?
A. Chemistry
B. Mathematics
C. Physics
D. All of the above
25. What did Al-Beruni determine?
A. Densities of different substances
B. Volume of different substances
C. Mass of different substances
D. None of the above
26. What was the year of birth of Ibne Sina?
A. 980 AD
B. 1037 AD
C. 1000 AD
D. 900 AD
27. What nickname is commonly given to Ibne Sina?
A. The Muslim Aristotle
B. The Greek Philosopher
C. The Islamic Physicist
D. The Persian Mathematician
28. In which field did Ibne Sina make contributions?
A. Medicine
B. Mathematics
C. Astronomy
D. All of the above
29. What is Ibne Sina famous for rejecting?
A. The idea of alchemy
B. The concept of gravity
C. The notion that metals could be changed into gold
D. The theory of evolution
30. What was the year of death of Ibne Sina?
A. 980 AD
B. 1037 AD
C. 1000 AD
D. 900 AD
31. What was the year of death of Al-Beruni?
A. 937 AD
B. 1048 AD
C. 900 AD
D. 1000 AD
A) A pure substance that can be broken down into simpler substances by ordinary chemical or physical means
B) A mixture of different substances
C) A compound made up of atoms of different elements
D) A pure substance that can't be broken down into simpler substances by ordinary chemical or physical means
33. What are the smallest units of an element?
A) Molecules
B) Atoms
C) Ions
D) Compounds
34. How elements are represented by symbols?
A) By using the first letter of an element
B) By using the initial letters in capital together with a small any other letter from its name
C) By using the last letter of an element
D) Both A and B
35. Who suggested the system for representing elements with symbols?
A) Berzelius
B) Avogadro
C) Mendeleev
D) Dalton
36. How a compound is formed?
A) By physical combination of elements
B) By chemical combination of elements
C) By mixing of elements
D) By heating of elements
37. How a compound can be decomposed?
A) By Physical means
B) By chemical means
C) By heating
D) By mixing
38. What is electrolysis?
A) A process through which electric current is passed through molten salt
B) A process through which electric current is passed through liquid
C) A process through which chemical reactions occur
D) A process through which elements combine
39. How the composition of a compound can be represented?
A) By its symbol
B) By its formula
40. What is the formula of a compound?
A) The collection of symbols of elements written in a specific way
B) The chemical name of a compound
41. How a mixture is formed?
A) By chemical combination of elements
B) By chemical reactions
C) By physical combination of substances
D) By heating of elements
42. How constituents of a mixture can be separated?
A) By chemical means
B) By physical means
C) By heating
D) By burning
43. Do the constituents of a mixture retain their characteristic properties?
A) No
B) Yes
44. What is the ratio of constituents in a mixture?
A) Fixed
B) Not fixed
C) Can vary
D) Not applicable
45. What is a homogeneous mixture?
A) A mixture in which composition is non-uniform throughout the mixture
B) A mixture in which composition is uniform throughout the mixture
C) A mixture that cannot be separated
D) A mixture that can be separated only by chemical means
46. What are the examples of homogeneous mixtures?
A) Iron and sand
B) Table salt and water
C) Ethyl alcohol and water
D) Both A and B
47. What is a heterogeneous mixture?
A) A mixture in which composition is non-uniform throughout the mixture
B) A mixture in which composition is uniform throughout the mixture
C) A mixture that cannot be separated
D) A mixture that can be separated only by chemical means
48. What are the examples of heterogeneous mixtures?
A) Table salt and water
B) Concrete
C) Oil and Water
D) Both B and C
49. What are the other names of homogeneous mixtures?
A) Colloids
B) Solutions
C) Heterogeneous mixtures
D) Suspensions
50. What are the other names of heterogeneous mixtures?
A) Colloids
B) Solutions
C) Colloidal solutions
D) Both A and C
A) Atomic mass
B) Mass number
C) Atomic number
D) Neutron number
52. What is the symbol used to represent the atomic number?
A) A
B) Z
C) X
D) C
53. How many protons and electrons are present in a Sodium atom?
A) 10 protons and 10 electrons
B) 11 protons and 11 electrons
C) 12 protons and 12 electrons
D) 13 protons and 13 electrons
54. What is the atomic number of Chlorine?
A) 12
B) 22
C) 17
D) 40
55. How do atoms of one element differ from those of other elements?
A) By the number of neutrons in their nuclei
B) By their mass number
C) By the number of protons in their nuclei
D) By the number of electrons in their nuclei
56. What is the sum of the number of protons and neutrons in an atom called?
A) Atomic mass
B) Mass number
C) Atomic number
D) Neutron number
57. What is the symbol used to represent the atomic mass of an element?
A) A
B) Z
C) X
D) C
58. What is the atomic mass of Carbon?
A) 12
B) 6
C) 8
D) 10
59. How are elements arranged in the modern periodic table?
A) On the basis of increasing atomic mass
B) On the basis of decreasing atomic mass
C) On the basis of increasing number of electrons
D) On the basis of increasing number of protons
60. What is the term used to describe the comparison of the atomic masses of all elements to the standard mass of C-12?
A) Isotopes
B) Relative atomic mass
C) Atomic numbers
D) Standard mass comparison
61. What is the range of the size of an atom in grams?
A) 1.67x10-24 g to 4.0x10-22 g
B) 1.67x10-22 g to 4.0x10-24 g
C) 4.0x10-24 g to 1.67x10-22 g
D) 4.0x10-22 g to 1.67x10-24 g
62. What is the reason for scientists preferring to compare atomic masses with the standard mass of C-12?
A) It is impossible to measure the size of atoms
B) It is impractical to work with extremely small values
C) C-12 is the most common element in nature
D) Both A and B
63. Atoms of an element having the same atomic numbers but different atomic masses are called what?
A) Isotopes
B) Relative atomic mass
C) Atomic numbers
D) Standard mass comparison
64. What is the term used to describe 1/12th the mass of an atom of C-12?
A) Atomic weight
B) Avogadro's number
C) Atomic mass unit (amu)
D) Relative atomic mass
65. What is the atomic weight of C-12 in grams?
A) 12 g
B) 1 mol
C) 6.023 x 10^23 atoms
D) 1.993 x 10^(-23) g
66. How many atoms are in 1 mol of C-12?
A) 12 g
B) 1 mol
C) 6.023 x 10^23 atoms
D) 1.993 x 10^(-23) g
67. What is the weight of 1 atom of C-12 in grams?
A) 12 g
B) 1 mol
C) 6.023 x 10^23 atoms
D) 1.993 x 10^(-23) g
68. What is the weight of 1 atomic mass unit in grams and kg?
A) 1.67 x 10^(-24) g
B) 1.67 x 10^(-27) kg
C) Both A and B
D) None of the above
69. What is the term used to describe the weighted average of atomic masses of naturally occurring isotopes of an element?
A) Isotopic forms
B) Atomic masses
C) Average atomic mass
D) Abundance in nature
70. What is the reason for the atomic masses of most elements being found in non-whole numbers?
A) Most elements are found in two or more isotopic forms.
B) The elements are found in rare forms.
C) The elements are found in only one isotopic form.
D) The elements are found in multiple forms but only one is naturally occurring.
71. What is the percentage abundance of Cl-35 in nature?
A) 25%
B) 35%
C) 37%
D) 75%
72. What is the percentage abundance of Cl-37 in nature?
A) 25%
B) 35%
C) 37%
D) 75%
73. What is the formula used to find the average atomic mass?
A) ((1st isotope x its %age) + (2nd isotpe x its %age) +⋯)/100
B) ((1st isotope x its %age) + (2nd isotpe x its %age) +⋯)*100
C) ((1st isotope x its %age) + (2nd isotpe x its %age)+⋯)-100
D) ((1st isotope x its %age) + (2nd isotpe x its %age)+⋯) x 100
74. What is the average atomic mass of chlorine using the provided data and formula?
A) 2625 amu
B) 925 amu
C) 3550 amu
D) 35.5 amu
75. How the average atomic mass is used in the study of elements?
A) To find the isotopic forms of an element
B) To find the atomic mass of an element
C) To find the naturally occurring isotopes of an element
D) To find the weighted average of atomic masses of naturally occurring isotopes of an element
76. What is the formula mass of MgCl2 in grams?
A. 24 g
B. 71 g
C. 95 g
D. 140 g
77. How many grams of Cl are there in 6 moles of MgCl2?
A. 210 g
B. 126 g
C. 95 g
D. 71 g (Correct answer)
78. How many moles of Mg are there in 24 grams of MgCl2?
A. 1 mol
B. 0.5 mol
C. 0.25 mol
D. 0.125 mol
79. What is the gram atomic mass of chlorine?
A. 24 g
B. 35.5 g
C. 71 g
D. 95 g
80. What is the sum of the relative atomic masses of all the atoms of a molecular formula called?
A. Atomic mass
B. Formula mass
C. Molecular mass
D. Gram formula mass
81. What is the unit used to express gram molecular mass?
A. amu
B. g
C. mol
D. kg
82. What is the molecular mass of C2H2?
A. 26.016 amu
B. 24 amu
C. 2.016 amu
D. 18 amu
83. What is the gram molecular mass of H2O?
A. 18 g
B. 44 g
C. 98 g
D. 26.016 g
84. What is the sum of the relative atomic masses of all the atoms of a formula unit called?
A. Formula mass
B. Atomic mass
C. Molecular mass
D. Gram formula mass
85. What is the formula mass of NaCl?
A. 58.5 amu
B. 35.5 amu
C. 23 amu
D. 72 amu
86. What is the gram formula mass of CaCl2?
A. 111 g
B. 58.5 g
C. 35.5 g
C. 72 g
87. What is the molecular mass of C6H12O6 in grams?
A. 180 g
B. 72 g
C. 96 g
D. 12 g
88. What is the formula mass of MgCl2 in grams?
A. 95 g
B. 24 g
C. 71 g
D. 140 g
A. CH
B. CH2O
C. C6H12O6
D. C6H6
90. The formula of salt (NaCl) is an example of which type of chemical formula?
A. Empirical formula
B. Formula unit
C. Structural formula
D. Both A and B
91. The simplest formula that gives the smallest whole number ratio of atoms in a compound is called:
A. Empirical formula
B. Molecular formula
C. Structural formula
D. None of the above
92. The molecular formula of a compound shows the:
A. Simplest ratio of atoms
B. Actual number of atoms
C. Number of ions
D. None of the above
93. The empirical formula of Benzene is:
A. C1H1
B. C6H6
C. CH
D. Both A and C
94. The relation between the molecular and empirical formula is given as:
A. Molecular mass = n x Empirical formula mass
B. Empirical mass = n x Molecular formula mass
C. Molecular mass = n x Structural formula mass
D. Empirical mass = n x Structural formula mass
95. The molecular mass of a compound can be determined by dividing the molecular formula mass by the:
A. Empirical formula mass
B. Structural formula mass
C. Atomic mass
D. None of the above
96. The actual formula of a compound is also known as its:
A. Empirical formula
B. Molecular formula
C. Structural formula
D. None of the above
97. What is a chemical species?
A) A neutral particle
B) A group of atoms that take part in a chemical reaction
C) An ionized atom
D) All of the above
98. What is an ion?
A) A neutral particle
B) A charged particle formed by an atom after losing or gaining electrons in bond formation
C) A negatively charged particle
D) A positively charged particle
99. What are the two types of ions?
A) Cations and Anions
B) Protons and Electrons
C) Negatively charged and Positively charged
D) None of the above
100. What is a cation?
A) A negatively charged particle
B) A positively charged particle formed on an atom after losing valence electrons
C) A neutral particle
D) None of the above
101. What is an anion?
A) A negatively charged particle formed on an atom after gaining valence electrons
B) A positively charged particle
C) A neutral particle
D) None of the above
102. How is an ion formed?
A) By losing or gaining electrons in bond formation
B) By gaining protons
C) By losing protons
D) None of the above
103. What is the result of an atom becoming an ion?
A) The balance between protons and electrons is destroyed
B) The balance between protons and electrons is maintained
C) The number of protons and electrons remain the same
D) None of the above
104. What is an example of a cation?
A) Sodium (Na)
B) Chlorine (Cl)
C) Oxygen (O)
D) None of the above
105. What is an example of an anion?
A) Chlorine (Cl)
B) Sodium (Na)
C) Calcium (Ca)
D) None of the above
106. What is the name given to the net charge formed on a molecule after losing or gaining electrons in bond formation?
A. Molecular Ion
B. Cationic Molecular Ion
C. Anionic Molecular Ion
D. Free Radical
107. Which type of molecular ion is formed when a molecule gains electrons in bond formation?
A. Cationic Molecular Ion
B. Anionic Molecular Ion
C. Free Radical
D. None of the above
108. Which type of molecular ion is formed when a molecule loses electrons in bond formation?
A. Cationic Molecular Ion
B. Anionic Molecular Ion
C. Free Radical
D. None of the above
109. What is the name given to the highly reactive species that are formed by the breaking of stable molecules?
A. Molecular Ion
B. Cationic Molecular Ion
C. Anionic Molecular Ion
D. Free Radical
110. Which type of free radical is formed in the reaction of Chlorine free radical with Methane (CH4)?
A. Chlorine free radical
B. Methyl free radical
C. Both A and B
D. None of the above
111. What is the final product of the reaction of Chlorine molecule (Cl2) with Methane (CH4)?
A. Chlorine free radical
B. Methyl free radical
C. Chloromethane(CH3Cl)
D. None of the above
112. Give an example of Cationic Molecular Ions
A. CO+1
B. O2+1
C. CH4+1
D. All of the above
113. Give an example of Anionic Molecular Ions
A. (HOCH2-CH2OH)+1
B. (C2H5OH)-1
C. Cl2
D. None of the above
A) Atom
B) Mixture
C) Element
D) Molecule
115. What are examples of molecules?
A) He, H2, NH3, H2SO4, CH4
B) Na, Cl, K, Ca
C) CO2, O2, H2O
D) Both A and C
116. What are monoatomic molecules?
A) Those made up of only one atom
B) Those made up of more than one atom
C) Those made up of different atoms
D) Those made up of the same atoms
117. What are examples of monoatomic molecules?
A) Helium (He), Neon (Ne), Argon (Ar)
B) H2, NH3, H2SO4
C) CO2, O2, H2O
D) C6H12O6, CH3COOH
118. What are polyatomic molecules?
A) Those made up of only one atom
B) Those made up of more than one atom
C) Those made up of different atoms
D) Those made up of the same atoms
119. What are examples of polyatomic molecules?
A) Helium (He), Neon (Ne), Argon (Ar)
B) H2, NH3, H2SO4, H2O (Correct)
C) C6H12O6, CH3COOH
D) Both B and C
120. What are triatomic molecules?
A) Those made up of three atoms
B) Those made up of one atom
C) Those made up of two atoms
D) Those made up of more than four atoms
121. What are examples of triatomic molecules?
A) H2O, CO2, NO2
B) H2, Cl2, CO
C) NH3, H2SO4, H2O
D) C6H12O6, CH3COOH
122. What type of molecule is made up of the same atoms?
A. Monoatomic Molecule
B. Polyatomic Molecule
C. Homoatomic Molecule
D. Heteroatomic Molecule
123. What type of molecule is made up of different atoms?
A. Monoatomic Molecule
B. Polyatomic Molecule
C. Homoatomic Molecule
D. Heteroatomic Molecule
124. Which of the following is not an example of a homoatomic molecule?
A. O2
B. O3
C. H2SO4
D. NH3
A) Dozen
B) Gross
C) Mole
D) Pound
126. What is the molecular mass of Oxygen in grams?
A) 16
B) 18
C) 44
D) 1
127. What is the molecular mass of H2O in grams?
A) 16
B) 18
C) 44
D) 1
128. What is the molecular mass of CO2 in grams?
A) 16
B) 18
C) 44
D) 1
129. What is the formula for calculating number of moles?
A) mass (in grams)/ Molar mass
B) mass (in grams) x Molar mass
C) Number of atoms or molecules / Avogadro’s Number
D) Both A and C
130. What is Avogadro's number?
A) 12
B) 144
C) 6.022×1023
D) 1
131. How many atoms, molecules or ions are there in one mole of a substance?
A) 12
B) 144
C) 6.022×1023
D) 1
132. Who experimentally proved that one mole of any substance has 6.022×1023 atoms, molecules, or ions?
A) Amedeo Avogadro
B) Isaac Newton
C) Albert Einstein
D) Marie Curie
133. How many atoms are there in 1 mole of Hydrogen?
A) 12
B) 144
C) 6.022×1023
D) 1
134. How many atoms are there in 16g of Oxygen?
A) 12
B) 144
C) 6.022×1023
D) 1
135. How many molecules are there in 44g of CO2?
A) 12
B) 144
C) 6.022×1023
D) 1
D. Pure Substance
2. What is the branch of science that deals with the study of properties, structure, composition, and changes in matter, as well as the laws and principles governing these changes?
A. Science
B. Chemistry
C. Matter
D. Pure Substance
3. What is the definition of matter?
A. Anything that occupies space and has mass
B. The branch of science that deals with the study of properties, structure, composition, and changes in matter
C. A pure substance that can't be broken down into simpler substances by ordinary chemical or physical means
D. Anything that can be formed as well as can be separated by physical means only
4. What is the definition of a pure substance?
A. Anything that is obtained from different sources but has the same composition and properties
B. The branch of science that deals with the study of properties, structure, composition, and changes in matter
C. A pure substance that can't be broken down into simpler substances by ordinary chemical or physical means
D. Anything that can be formed as well as can be separated by physical means only
5. What is the definition of an element?
A. A pure substance that can't be broken down into simpler substances by ordinary chemical or physical means
B. The branch of science that deals with the study of properties, structure, composition, and changes in matter
C. Anything that is obtained from different sources but has the same composition and properties
D. Anything that can be formed as well as can be separated by physical means only
6. What is the definition of a compound?
A. A pure substance that can be only formed as well as broken down into simpler substances by chemical means only
B. The branch of science that deals with the study of properties, structure, composition, and changes in matter
C. Anything that is obtained from different sources but has the same composition and properties
D. Anything that can be formed as well as can be separated by physical means only
7. What is the definition of a mixture?
A. Anything that can be formed as well as can be separated by physical means only
B. The branch of science that deals with the study of properties, structure, composition, and changes in matter
C. Anything that is obtained from different sources but has the same composition and properties
D. A pure substance that can be only formed as well as broken down into simpler substances by chemical means only
MCQs on Brief History of Chemistry and Muslim Scientists
8. What is the period known as in the history of chemistry from 600 to 1600 AD?A. The period of Muslim chemists
B. The period of Greek chemists
C. The period of Roman chemists
D. The period of Egyptian chemists
9. How did the knowledge of Alchemists and their techniques spread to Europe?
A. Through trade and commerce
B. Through invasions and conquests
C. Gradually over time
D. Through scientific collaboration
10. What was the term used for the knowledge of Alchemists before it changed to a purely English word?
A. Chemistry
B. Alchemistry
C. Arab science
D. Alchemy
11. What were some of the elements discovered by Al-Chemists?
A. Gold, Silver, Copper
B. Arsenic, Antimony, Bismuth
C. Oxygen, Hydrogen, Nitrogen
D. Carbon, Silicon, Germanium
12. What laboratory equipment did Al-Chemists invent?
A. Microscope, centrifuge, pipettes, test tubes
B. Bunsen burner, thermometer, barometer, hygrometer
C. Beaker, crucibles, retorts, furnaces
D. Spectrophotometer, chromatograph, oscilloscope, centrifuge
13. What laboratory procedures did Al-Chemists invent?
A. Sublimation, fermentation, filtration, calcination
B. Digestion, distillation, centrifugation, crystallization
C. Chromatography, electrophoresis, spectrophotometry, microscopy
D. Hydrogenation, oxidation, reduction, neutralization
14. What did Al-Chemists prepare?
A. Acids, Alkalies (Bases), medicines, and Alcohol
B. Gold, Silver, Copper
C. Oxygen, Hydrogen, Nitrogen
D. Carbon, Silicon, Germanium
15. Who is known as the father of Chemistry?
A. Jabir-Ibn-e-Hayyan
B. Robert Boyle
C. Antonie van Leeuwenhoek
D. John Dalton
16. In what year was Jabir-Ibn-e-Hayyan born?
A. 712 AD
B. 803 AD
C. 1021 AD
D. 721 AD
17. In what year did Jabir-Ibn-e-Hayyan die?
A. 721 AD
B. 803 AD
C. 1021 AD
D. 1203 AD
18. What was Jabir-Ibn-e-Hayyan's contribution to Chemistry?
A. He described the method of production of white lead
B. He invented a chemical and experimental procedure for the preparation of Nitric acid (HNO3) and Hydrochloric acid (HCl)
C. He described methods of fractional distillation and a method for the extraction of metals
D. All of the above
19. What was the year of birth of Muhammad Ibne-Zikriya Al-Razi?
A. 864 AD
B. 930 AD
C. 800 AD
D. 700 AD
20. IWhat is the main topic of Al-Asrar, the famous book written by Muhammad Ibne-Zikriya Al-Razi?
A. Surgery
B. Philosophy
C. Chemistry
D. Physiology
21. How did Muhammad Ibne-Zikriya Al-Razi prepare alcohol?
A. Distillation
B. Synthesis
C. Fermentation
D. Extraction
22. Muhammad Ibne-Zikriya Al-Razi is known for dividing things into which two categories?
A. Living and non-living
B. Organic and inorganic
C. Natural and artificial
D. Solid and liquid
23. What was the year of birth of Al-Beruni?
A. 937 AD
B. 1048 AD
C. 900 AD
D. 1000 AD
24. In which field did Al-Beruni make contributions?
A. Chemistry
B. Mathematics
C. Physics
D. All of the above
25. What did Al-Beruni determine?
A. Densities of different substances
B. Volume of different substances
C. Mass of different substances
D. None of the above
26. What was the year of birth of Ibne Sina?
A. 980 AD
B. 1037 AD
C. 1000 AD
D. 900 AD
27. What nickname is commonly given to Ibne Sina?
A. The Muslim Aristotle
B. The Greek Philosopher
C. The Islamic Physicist
D. The Persian Mathematician
28. In which field did Ibne Sina make contributions?
A. Medicine
B. Mathematics
C. Astronomy
D. All of the above
29. What is Ibne Sina famous for rejecting?
A. The idea of alchemy
B. The concept of gravity
C. The notion that metals could be changed into gold
D. The theory of evolution
30. What was the year of death of Ibne Sina?
A. 980 AD
B. 1037 AD
C. 1000 AD
D. 900 AD
31. What was the year of death of Al-Beruni?
A. 937 AD
B. 1048 AD
C. 900 AD
D. 1000 AD
MCQs on Elements, Compounds, and Mixtures
32. What is an element?A) A pure substance that can be broken down into simpler substances by ordinary chemical or physical means
B) A mixture of different substances
C) A compound made up of atoms of different elements
D) A pure substance that can't be broken down into simpler substances by ordinary chemical or physical means
33. What are the smallest units of an element?
A) Molecules
B) Atoms
C) Ions
D) Compounds
34. How elements are represented by symbols?
A) By using the first letter of an element
B) By using the initial letters in capital together with a small any other letter from its name
C) By using the last letter of an element
D) Both A and B
35. Who suggested the system for representing elements with symbols?
A) Berzelius
B) Avogadro
C) Mendeleev
D) Dalton
36. How a compound is formed?
A) By physical combination of elements
B) By chemical combination of elements
C) By mixing of elements
D) By heating of elements
37. How a compound can be decomposed?
A) By Physical means
B) By chemical means
C) By heating
D) By mixing
38. What is electrolysis?
A) A process through which electric current is passed through molten salt
B) A process through which electric current is passed through liquid
C) A process through which chemical reactions occur
D) A process through which elements combine
39. How the composition of a compound can be represented?
A) By its symbol
B) By its formula
40. What is the formula of a compound?
A) The collection of symbols of elements written in a specific way
B) The chemical name of a compound
41. How a mixture is formed?
A) By chemical combination of elements
B) By chemical reactions
C) By physical combination of substances
D) By heating of elements
42. How constituents of a mixture can be separated?
A) By chemical means
B) By physical means
C) By heating
D) By burning
43. Do the constituents of a mixture retain their characteristic properties?
A) No
B) Yes
44. What is the ratio of constituents in a mixture?
A) Fixed
B) Not fixed
C) Can vary
D) Not applicable
45. What is a homogeneous mixture?
A) A mixture in which composition is non-uniform throughout the mixture
B) A mixture in which composition is uniform throughout the mixture
C) A mixture that cannot be separated
D) A mixture that can be separated only by chemical means
46. What are the examples of homogeneous mixtures?
A) Iron and sand
B) Table salt and water
C) Ethyl alcohol and water
D) Both A and B
47. What is a heterogeneous mixture?
A) A mixture in which composition is non-uniform throughout the mixture
B) A mixture in which composition is uniform throughout the mixture
C) A mixture that cannot be separated
D) A mixture that can be separated only by chemical means
48. What are the examples of heterogeneous mixtures?
A) Table salt and water
B) Concrete
C) Oil and Water
D) Both B and C
49. What are the other names of homogeneous mixtures?
A) Colloids
B) Solutions
C) Heterogeneous mixtures
D) Suspensions
50. What are the other names of heterogeneous mixtures?
A) Colloids
B) Solutions
C) Colloidal solutions
D) Both A and C
MCQs on Atomic number, Atomic mass, Relative atomic mass, Atomic mass unit, Average atomic mass, Molecular mass, Gram Molecular mass, Formula mass, Gram Formula mass
51. What is the total number of protons present in the nucleus of an atom called?A) Atomic mass
B) Mass number
C) Atomic number
D) Neutron number
52. What is the symbol used to represent the atomic number?
A) A
B) Z
C) X
D) C
53. How many protons and electrons are present in a Sodium atom?
A) 10 protons and 10 electrons
B) 11 protons and 11 electrons
C) 12 protons and 12 electrons
D) 13 protons and 13 electrons
54. What is the atomic number of Chlorine?
A) 12
B) 22
C) 17
D) 40
55. How do atoms of one element differ from those of other elements?
A) By the number of neutrons in their nuclei
B) By their mass number
C) By the number of protons in their nuclei
D) By the number of electrons in their nuclei
56. What is the sum of the number of protons and neutrons in an atom called?
A) Atomic mass
B) Mass number
C) Atomic number
D) Neutron number
57. What is the symbol used to represent the atomic mass of an element?
A) A
B) Z
C) X
D) C
58. What is the atomic mass of Carbon?
A) 12
B) 6
C) 8
D) 10
59. How are elements arranged in the modern periodic table?
A) On the basis of increasing atomic mass
B) On the basis of decreasing atomic mass
C) On the basis of increasing number of electrons
D) On the basis of increasing number of protons
60. What is the term used to describe the comparison of the atomic masses of all elements to the standard mass of C-12?
A) Isotopes
B) Relative atomic mass
C) Atomic numbers
D) Standard mass comparison
61. What is the range of the size of an atom in grams?
A) 1.67x10-24 g to 4.0x10-22 g
B) 1.67x10-22 g to 4.0x10-24 g
C) 4.0x10-24 g to 1.67x10-22 g
D) 4.0x10-22 g to 1.67x10-24 g
62. What is the reason for scientists preferring to compare atomic masses with the standard mass of C-12?
A) It is impossible to measure the size of atoms
B) It is impractical to work with extremely small values
C) C-12 is the most common element in nature
D) Both A and B
63. Atoms of an element having the same atomic numbers but different atomic masses are called what?
A) Isotopes
B) Relative atomic mass
C) Atomic numbers
D) Standard mass comparison
64. What is the term used to describe 1/12th the mass of an atom of C-12?
A) Atomic weight
B) Avogadro's number
C) Atomic mass unit (amu)
D) Relative atomic mass
65. What is the atomic weight of C-12 in grams?
A) 12 g
B) 1 mol
C) 6.023 x 10^23 atoms
D) 1.993 x 10^(-23) g
66. How many atoms are in 1 mol of C-12?
A) 12 g
B) 1 mol
C) 6.023 x 10^23 atoms
D) 1.993 x 10^(-23) g
67. What is the weight of 1 atom of C-12 in grams?
A) 12 g
B) 1 mol
C) 6.023 x 10^23 atoms
D) 1.993 x 10^(-23) g
68. What is the weight of 1 atomic mass unit in grams and kg?
A) 1.67 x 10^(-24) g
B) 1.67 x 10^(-27) kg
C) Both A and B
D) None of the above
69. What is the term used to describe the weighted average of atomic masses of naturally occurring isotopes of an element?
A) Isotopic forms
B) Atomic masses
C) Average atomic mass
D) Abundance in nature
70. What is the reason for the atomic masses of most elements being found in non-whole numbers?
A) Most elements are found in two or more isotopic forms.
B) The elements are found in rare forms.
C) The elements are found in only one isotopic form.
D) The elements are found in multiple forms but only one is naturally occurring.
71. What is the percentage abundance of Cl-35 in nature?
A) 25%
B) 35%
C) 37%
D) 75%
72. What is the percentage abundance of Cl-37 in nature?
A) 25%
B) 35%
C) 37%
D) 75%
73. What is the formula used to find the average atomic mass?
A) ((1st isotope x its %age) + (2nd isotpe x its %age) +⋯)/100
B) ((1st isotope x its %age) + (2nd isotpe x its %age) +⋯)*100
C) ((1st isotope x its %age) + (2nd isotpe x its %age)+⋯)-100
D) ((1st isotope x its %age) + (2nd isotpe x its %age)+⋯) x 100
74. What is the average atomic mass of chlorine using the provided data and formula?
A) 2625 amu
B) 925 amu
C) 3550 amu
D) 35.5 amu
75. How the average atomic mass is used in the study of elements?
A) To find the isotopic forms of an element
B) To find the atomic mass of an element
C) To find the naturally occurring isotopes of an element
D) To find the weighted average of atomic masses of naturally occurring isotopes of an element
76. What is the formula mass of MgCl2 in grams?
A. 24 g
B. 71 g
C. 95 g
D. 140 g
77. How many grams of Cl are there in 6 moles of MgCl2?
A. 210 g
B. 126 g
C. 95 g
D. 71 g (Correct answer)
78. How many moles of Mg are there in 24 grams of MgCl2?
A. 1 mol
B. 0.5 mol
C. 0.25 mol
D. 0.125 mol
79. What is the gram atomic mass of chlorine?
A. 24 g
B. 35.5 g
C. 71 g
D. 95 g
80. What is the sum of the relative atomic masses of all the atoms of a molecular formula called?
A. Atomic mass
B. Formula mass
C. Molecular mass
D. Gram formula mass
81. What is the unit used to express gram molecular mass?
A. amu
B. g
C. mol
D. kg
82. What is the molecular mass of C2H2?
A. 26.016 amu
B. 24 amu
C. 2.016 amu
D. 18 amu
83. What is the gram molecular mass of H2O?
A. 18 g
B. 44 g
C. 98 g
D. 26.016 g
84. What is the sum of the relative atomic masses of all the atoms of a formula unit called?
A. Formula mass
B. Atomic mass
C. Molecular mass
D. Gram formula mass
85. What is the formula mass of NaCl?
A. 58.5 amu
B. 35.5 amu
C. 23 amu
D. 72 amu
86. What is the gram formula mass of CaCl2?
A. 111 g
B. 58.5 g
C. 35.5 g
C. 72 g
87. What is the molecular mass of C6H12O6 in grams?
A. 180 g
B. 72 g
C. 96 g
D. 12 g
88. What is the formula mass of MgCl2 in grams?
A. 95 g
B. 24 g
C. 71 g
D. 140 g
MCQs on Chemical Formula and its types
89. A compound with a formula of C6H12O6 has a molecular formula of:A. CH
B. CH2O
C. C6H12O6
D. C6H6
90. The formula of salt (NaCl) is an example of which type of chemical formula?
A. Empirical formula
B. Formula unit
C. Structural formula
D. Both A and B
91. The simplest formula that gives the smallest whole number ratio of atoms in a compound is called:
A. Empirical formula
B. Molecular formula
C. Structural formula
D. None of the above
92. The molecular formula of a compound shows the:
A. Simplest ratio of atoms
B. Actual number of atoms
C. Number of ions
D. None of the above
93. The empirical formula of Benzene is:
A. C1H1
B. C6H6
C. CH
D. Both A and C
94. The relation between the molecular and empirical formula is given as:
A. Molecular mass = n x Empirical formula mass
B. Empirical mass = n x Molecular formula mass
C. Molecular mass = n x Structural formula mass
D. Empirical mass = n x Structural formula mass
95. The molecular mass of a compound can be determined by dividing the molecular formula mass by the:
A. Empirical formula mass
B. Structural formula mass
C. Atomic mass
D. None of the above
96. The actual formula of a compound is also known as its:
A. Empirical formula
B. Molecular formula
C. Structural formula
D. None of the above
97. What is a chemical species?
A) A neutral particle
B) A group of atoms that take part in a chemical reaction
C) An ionized atom
D) All of the above
98. What is an ion?
A) A neutral particle
B) A charged particle formed by an atom after losing or gaining electrons in bond formation
C) A negatively charged particle
D) A positively charged particle
99. What are the two types of ions?
A) Cations and Anions
B) Protons and Electrons
C) Negatively charged and Positively charged
D) None of the above
100. What is a cation?
A) A negatively charged particle
B) A positively charged particle formed on an atom after losing valence electrons
C) A neutral particle
D) None of the above
101. What is an anion?
A) A negatively charged particle formed on an atom after gaining valence electrons
B) A positively charged particle
C) A neutral particle
D) None of the above
102. How is an ion formed?
A) By losing or gaining electrons in bond formation
B) By gaining protons
C) By losing protons
D) None of the above
103. What is the result of an atom becoming an ion?
A) The balance between protons and electrons is destroyed
B) The balance between protons and electrons is maintained
C) The number of protons and electrons remain the same
D) None of the above
104. What is an example of a cation?
A) Sodium (Na)
B) Chlorine (Cl)
C) Oxygen (O)
D) None of the above
105. What is an example of an anion?
A) Chlorine (Cl)
B) Sodium (Na)
C) Calcium (Ca)
D) None of the above
106. What is the name given to the net charge formed on a molecule after losing or gaining electrons in bond formation?
A. Molecular Ion
B. Cationic Molecular Ion
C. Anionic Molecular Ion
D. Free Radical
107. Which type of molecular ion is formed when a molecule gains electrons in bond formation?
A. Cationic Molecular Ion
B. Anionic Molecular Ion
C. Free Radical
D. None of the above
108. Which type of molecular ion is formed when a molecule loses electrons in bond formation?
A. Cationic Molecular Ion
B. Anionic Molecular Ion
C. Free Radical
D. None of the above
109. What is the name given to the highly reactive species that are formed by the breaking of stable molecules?
A. Molecular Ion
B. Cationic Molecular Ion
C. Anionic Molecular Ion
D. Free Radical
110. Which type of free radical is formed in the reaction of Chlorine free radical with Methane (CH4)?
A. Chlorine free radical
B. Methyl free radical
C. Both A and B
D. None of the above
111. What is the final product of the reaction of Chlorine molecule (Cl2) with Methane (CH4)?
A. Chlorine free radical
B. Methyl free radical
C. Chloromethane(CH3Cl)
D. None of the above
112. Give an example of Cationic Molecular Ions
A. CO+1
B. O2+1
C. CH4+1
D. All of the above
113. Give an example of Anionic Molecular Ions
A. (HOCH2-CH2OH)+1
B. (C2H5OH)-1
C. Cl2
D. None of the above
MCQs on Molecules and its classification
114. What is the smallest particle of an element or compound which can exist as an independent distinguishable entity called?A) Atom
B) Mixture
C) Element
D) Molecule
115. What are examples of molecules?
A) He, H2, NH3, H2SO4, CH4
B) Na, Cl, K, Ca
C) CO2, O2, H2O
D) Both A and C
116. What are monoatomic molecules?
A) Those made up of only one atom
B) Those made up of more than one atom
C) Those made up of different atoms
D) Those made up of the same atoms
117. What are examples of monoatomic molecules?
A) Helium (He), Neon (Ne), Argon (Ar)
B) H2, NH3, H2SO4
C) CO2, O2, H2O
D) C6H12O6, CH3COOH
118. What are polyatomic molecules?
A) Those made up of only one atom
B) Those made up of more than one atom
C) Those made up of different atoms
D) Those made up of the same atoms
119. What are examples of polyatomic molecules?
A) Helium (He), Neon (Ne), Argon (Ar)
B) H2, NH3, H2SO4, H2O (Correct)
C) C6H12O6, CH3COOH
D) Both B and C
120. What are triatomic molecules?
A) Those made up of three atoms
B) Those made up of one atom
C) Those made up of two atoms
D) Those made up of more than four atoms
121. What are examples of triatomic molecules?
A) H2O, CO2, NO2
B) H2, Cl2, CO
C) NH3, H2SO4, H2O
D) C6H12O6, CH3COOH
122. What type of molecule is made up of the same atoms?
A. Monoatomic Molecule
B. Polyatomic Molecule
C. Homoatomic Molecule
D. Heteroatomic Molecule
123. What type of molecule is made up of different atoms?
A. Monoatomic Molecule
B. Polyatomic Molecule
C. Homoatomic Molecule
D. Heteroatomic Molecule
124. Which of the following is not an example of a homoatomic molecule?
A. O2
B. O3
C. H2SO4
D. NH3
MCQs on Mole, Avogadro's Number, and basic Chemical Calculations
125. What is the unit used by chemists to measure the amount of substance?A) Dozen
B) Gross
C) Mole
D) Pound
126. What is the molecular mass of Oxygen in grams?
A) 16
B) 18
C) 44
D) 1
127. What is the molecular mass of H2O in grams?
A) 16
B) 18
C) 44
D) 1
128. What is the molecular mass of CO2 in grams?
A) 16
B) 18
C) 44
D) 1
129. What is the formula for calculating number of moles?
A) mass (in grams)/ Molar mass
B) mass (in grams) x Molar mass
C) Number of atoms or molecules / Avogadro’s Number
D) Both A and C
130. What is Avogadro's number?
A) 12
B) 144
C) 6.022×1023
D) 1
131. How many atoms, molecules or ions are there in one mole of a substance?
A) 12
B) 144
C) 6.022×1023
D) 1
132. Who experimentally proved that one mole of any substance has 6.022×1023 atoms, molecules, or ions?
A) Amedeo Avogadro
B) Isaac Newton
C) Albert Einstein
D) Marie Curie
133. How many atoms are there in 1 mole of Hydrogen?
A) 12
B) 144
C) 6.022×1023
D) 1
134. How many atoms are there in 16g of Oxygen?
A) 12
B) 144
C) 6.022×1023
D) 1
135. How many molecules are there in 44g of CO2?
A) 12
B) 144
C) 6.022×1023
D) 1
0 Comments:
Post a Comment