Maximizing Your Board Exams and Entry Tests Performance | 90 MCQs on Molecules, Chemical Bonds, and Intermolecular Forces for beginners
Welcome to our comprehensive guide on the 90 most important Chemistry MCQs for School and College level board examinations and entry test preparations. Chemistry is a fundamental subject that is vital to understanding the composition, properties, and reactions of substances at the molecular level. Whether you are preparing for BISE and Federal Board examinations, or tests like NEET, MDCAT, NTS, ETEA, CSS, PCS, or any other competitive exams, a strong grasp of the essential concepts of chemistry is critical for success.
In this article, we have compiled a list of the 90 most important multiple choice questions (MCQs) that cover a wide range of topics, including molecules, chemical bonds and their types, intermolecular forces (Dipole-Dipole, Hydrogen Bonding), and properties of Ionic Compounds, Covalent Compounds, and metals. These MCQs are designed to test your knowledge and understanding of key concepts and are an excellent resource for reinforcing your learning and preparing for your exams.
Whether you are a student or a professional, this guide will provide you with the essential tools and knowledge you need to succeed in your chemistry exams and tests. So, let's get started and explore the 90 most important Chemistry MCQs for School and College level board examinations and entry tests preparations.
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| 90 Important MCQs on Introduction to Chemical Bonding From the MCQs Library of H.E.S (Health, Education, and Skills) |
MCQs on Basic definitions and terms of the Structure of molecules
1. Which of the following statements is true about molecules?A. Molecules are composed of only one type of atom.
B. Molecules cannot exist in the form of liquids or solids.
C. Molecules have a distinct identity and can exist in various forms.
D. Molecules do not involve any chemical bonds between atoms.
2. Which of the following is an example of a synthetic molecule?
A. Vitamin C obtained from citrus fruits
B. Oxygen obtained from the atmosphere
C. Vitamin-C obtained from artificial sources
D. Glucose obtained from plants
3. What is the Octet rule?
A. Completion of two electrons in the outermost shell of an atom after bond formation
B. Completion of eight electrons in the outermost shell of an atom after bond formation
C. Completion of ten electrons in the outermost shell of an atom after bond formation
D. Completion of twelve electrons in the outermost shell of an atom after bond formation
4. Which of the following is an example of the Octet rule?
A. Hydrogen with one electron in its outermost shell
B. Chlorine with seven electrons in its outermost shell
C. Hydrogen and chlorine bonded with one electron in the outermost shell of each atom
D. Chlorine with eight electrons in its outermost shell after bonding with hydrogen
5. Why do atoms form chemical bonds?
A. Because they want to increase their energy levels.
B. To become unstable.
C. To disobey Universal law.
D. To lower their energy levels and gain stability.
6. What is the Universal law that atoms obey when forming chemical bonds?
A. Objects in the universe move from low to high energy levels.
B. Objects in the universe tend to increase their energy levels.
C. Objects in the universe tend to lower their energy levels to gain stability.
D. Objects in the universe have no tendency to lower their energy levels.
7. In what form do atoms have high energy?
A. In bounded form.
B. In unbounded form.
C. In a solid form.
D. In a gaseous form.
8. Which of the following is an example of an object moving from a higher to a lower energy level?
A. A hot body transfers heat to a cold body.
B. A ball rolling up a hill.
C. A rocket accelerating into space.
D. A plant growing towards the sun.
9. What happens to an object when it gains stability?
A. Its energy levels increase.
B. Its energy levels decrease.
C. Its energy levels stay the same.
D. It becomes more unstable.
MCQs on Valence Concept (Electron Theory of Valence)
10. What is the valence concept of chemical bonding?A. It states that atoms share or exchange electrons to attain stability.
B. It states that atoms form chemical bonds to increase their energy levels.
C. It states that atoms form chemical bonds to become more reactive.
D. It states that atoms form chemical bonds to create new elements.
11. Who gave the electronic theory of valence?
A. G.N. Lewis and W. Kossel
B. Albert Einstein and Niels Bohr
C. Marie Curie and Dmitri Mendeleev
D. Isaac Newton and Galileo Galilei
12. What is the name of the theory of valence that states atoms tend to attain eight electrons in the outer shell?
A. Duplet's theory of valence
B. Octet's theory of valence
C. Noble gas theory of valence
D. Ionic theory of valence
13. Which of the following atoms would follow the Duplet rule of valence?
A. Lithium
B. Beryllium
C. Helium
D. Oxygen
14. How many valence electrons does an Oxygen atom have?
A. Two
B. Four
C. Six
D. Eight
15. What is the orbital concept of chemical bonding?
A. It is based on the sharing of electrons between atoms.
B. It is based on the combination of atomic orbitals to produce molecular orbitals.
C. It is based on the transfer of electrons from one atom to another.
D. It is based on the electrostatic attraction between oppositely charged ions.
16. What is the difference between endwise and sidewise overlapping of atomic orbitals?
A. Endwise overlapping produces a pi-bond, and sidewise overlapping produces a sigma bond.
B. Endwise overlapping produces a sigma bond, and sidewise overlapping produces a pi-bond.
C. Endwise overlapping produces an ionic bond, and sidewise overlapping produces a covalent bond.
D. Endwise overlapping produces a covalent bond, and sidewise overlapping produces an ionic bond.
MCQS on Chemical bonds and their types (Ionic, Covalent, Coordinate Covalent, and Metallic Bonds)
17. What are chemical bonds?A. Repulsive forces between atoms
B. Attractive forces between atoms
C. Neutral forces between atoms
D. Magnetic forces between atoms
18. What type of bond is formed by the electrostatic force of attraction between a metal and a non-metal?
A. Covalent bond
B. Metallic bond
C. Ionic bond
D. Coordinate covalent bond
19. What type of bond is formed when two non-metals share electrons?
A. Covalent bond
B. Metallic bond
C. Ionic bond
D. Coordinate covalent bond
20. What type of bond is formed between a metal cation and a delocalized sea of electrons?
A. Covalent bond
B. Metallic bond
C. Ionic bond
D. Coordinate covalent bond
21. What type of bond is formed when one atom donates a lone pair of electrons to another atom?
A. Covalent bond
B. Metallic bond
C. Ionic bond
D. Coordinate covalent bond
22. What is a Coordinate Covalent bond?
A. A bond in which both atoms share a pair of electrons equally.
B. A bond in which a shared pair of electrons is donated by the donor atom and accepted by the acceptor atom.
C. A bond in which one atom donates a pair of electrons and the other atom accepts two pairs of electrons.
D. A bond in which one atom donates an electron and the other atom accepts a proton.
23. What is the role of the donor atom in a Coordinate Covalent bond?
A. It accepts a pair of electrons.
B. It donates a pair of electrons.
C. It accepts a proton.
D. It donates a proton.
24. How is a Coordinate Covalent bond represented in a Lewis structure?
A. With a dotted line between the two atoms.
B. With a straight line between the two atoms.
C. With an arrow pointing from the donor atom to the acceptor atom.
D. With an arrow pointing from the acceptor atom to the donor atom.
25. Which of the following compounds contains a Coordinate Covalent bond?
A. NaCl
B. CO2
C. NH4+
D. H2SO4
26. In the formation of the Ammonium Ion (NH4)+1, which atom is the donor atom?
A. Nitrogen
B. Hydrogen
C. Oxygen
D. Chlorine
27. In the formation of the Hydronium Ion (H3O)+1, which atom is the acceptor atom?
A. Nitrogen
B. Hydrogen
C. Oxygen
D. Chlorine
28. Which of the following statements is true about a Coordinate Covalent bond?
A. It always involves two donor atoms and two acceptor atoms.
B. It is a type of bond in which electrons are not shared between two atoms.
C. It is a type of bond in which both atoms donate electrons.
D. It is a type of bond in which one atom donates a pair of electrons and the other atom accepts them.
29. What is a Polar Covalent bond?
A. A bond where electrons are shared equally
B. A bond where electrons are not shared
C. A bond where electrons are attracted towards the more electronegative atom
D. A bond where electrons are repelled by atoms
30. Which atom in Hydrochloric Acid has a partial negative charge?
A. Hydrogen
B. Chlorine
C. Both
D. None
31. What is a Non-Polar Covalent bond?
A. A bond where electrons are not shared
B. A bond where electrons are attracted towards the more electronegative atom
C. A bond where electrons are shared equally
D. A bond where electrons are repelled by atoms
32. Which bond has a partial positive charge on both bonded atoms?
A. Non-Polar Covalent bond
B. Polar Covalent bond
C. Ionic bond
D. Metallic bond
33. Which factor determines the polarity of a Covalent bond?
A. The number of atoms in the molecule
B. The distance between bonded atoms
C. The electronegativity difference between bonded atoms
D. The mass of bonded atoms
34. Which theory explains the arrangement of metal atoms in a metallic bond?
A. Electron cloud theory
B. Ionic theory
C. Covalent theory
D. Electron sea theory
35. According to the Electron sea theory, what are the electrons of the metal atoms known as?
A. Valence electrons
B. Covalent electrons
C. Free electrons
D. Ionic electrons
36. What is the role of free electrons in a metallic bond?
A. They cause the atoms to form molecules
B. They tightly bond the atoms to the nucleus
C. They make the metal atoms negatively charged
D. They allow the metal to conduct electricity
37. What is the reason why metal conducts electricity according to the Electron sea theory?
A. The metal atoms have a high electronegativity
B. The metal atoms have a low electronegativity
C. The free electrons belong to all the atoms in the metal
D. The metal atoms form strong covalent bonds with each other
MCQs on Intermolecular Forces
38. What are intermolecular forces?
A. Forces between atoms in a substance
B. Forces between molecules in a substance
C. Forces between ions in a substance
D. Forces between electrons and protons in a substance
39. What is the primary factor determining the strength of intermolecular forces?
A. Size of the molecules
B. Polarity of the molecules
C. Number of electrons in the molecules
D. Shape of the molecules
40. What is the intermolecular force called that exists between polar molecules?
A. London dispersion force
B. Dipole-dipole interaction
C. Hydrogen bonding
D. Metallic bonding
41. What type of intermolecular force is responsible for the high boiling point of water?
A. London dispersion force
B. Dipole-dipole interaction
C. Hydrogen bonding
D. Metallic bonding
42. Which of the following intermolecular forces is the weakest?
A. Hydrogen bonding
B. Dipole-dipole interaction
C. London dispersion force
D. All intermolecular forces have the same strength
43. Which of the following substances has the strongest intermolecular forces?
A. Methane (CH4)
B. Ethanol (CH3CH2OH)
C. Carbon dioxide (CO2)
D. Oxygen (O2)
44. What type of Intermolecular force is Hydrogen Bonding?
A. Force of attraction between charged particles
B. Force of attraction between polar molecules
C. Force of attraction between nonpolar molecules
D. Force of repulsion between
45. What type of bond is formed between the Hydrogen of one molecule and high electronegative atoms such as Nitrogen, Oxygen, and Fluorine?
A. Ionic bond
B. Covalent bond
C. Hydrogen bond
D. Metallic bond
46. In which molecule, Hydrogen bonding is not found?
A. H2O (Water)
B. NH3 (Ammonia)
C. H2S (Hydrogen Sulfide)
D. HF (Hydrogen Fluoride)
47. Which one is stronger than Hydrogen Bonding?
A. Dipole-Dipole Interaction
B. London dispersion forces
C. Ionic bond
D. Covalent bond
48. Hydrogen bonding is roughly _____ times stronger than Dipole-Dipole Interaction.
A. 2 times
B. 5 times
C. 10 times
D. 15 times
49. Which acid exhibits the weakest acidic strength due to hydrogen bonding?
A) HCl
B) HF
C) HI
D) HBr
50. Which molecules contain thousands of hydrogen bonds?
A) Lipids
B) Carbohydrates
C) Proteins
D) DNA and RNA nucleotides
51. In which materials is hydrogen bonding responsible for increasing their adhesive and sticky property?
A) Metals
B) Polymers
C) Ceramics
D) Paints, dyes, and glue
52. What is Dipole-Dipole interaction?
A) Forces of attraction between two non-polar molecules
B) Forces of attraction between two weakly polar molecules
C) Forces of attraction between two strongly polar molecules
D) Forces of attraction between two ionic compounds
53. Which type of molecule has a weak polar covalent bond?
A) H2O
B) NH3
C) CO2
D) HF
54. Which type of molecule has a stronger Dipole-Dipole interaction?
A) Gases
B) Liquids
C) Both have the same strength of Dipole-Dipole interaction
D) Neither has Dipole-Dipole interaction
55. What is the effect of increasing the intermolecular distance on Dipole-Dipole interaction?
A) It weakens the interaction
B) It strengthens the interaction
C) It has no effect on the interaction
D) It reverses the interaction
56. What is the effect of increasing the electronegativity difference between bonded atoms on Dipole-Dipole interaction?
A) It weakens the interaction
B) It strengthens the interaction
C) It has no effect on the interaction
D) It reverses the interaction
57. What is the factor that determines whether a molecule has Dipole-Dipole interaction or Hydrogen bonding?
A) The type of atoms present in the molecule
B) The polarity of the molecule
C) The size of the molecule
D) The temperature of the molecule
MCQs on Properties of Ionic compounds, Covalent compounds, and metals.
58. Which of the following is a characteristic property of ionic compounds?A. They have low melting and boiling points
B. They conduct electricity in solid form
C. They dissociate into ions in molten form
D. They are always soluble in nonpolar solvents
59. What is the state of ionic compounds at room temperature and normal atmospheric pressure?
A. Liquid
B. Gas
C. Solid
D. Plasma
60. Which of the following solvents are ionic compounds typically soluble in?
A. Nonpolar solvents
B. Polar solvents
C. Neutral solvents
D. Basic solvents
61. What is the electrical conductivity of ionic compounds in solid form?
A. Good conductors
B. Poor conductors
C. Partial conductors
D. None of the above
62. What is the primary reason for the high melting and boiling points of ionic compounds?
A. Strong covalent bonds
B. Weak ionic bonds
C. Metallic bonding
D. Strong electrostatic forces
63. What factor(s) affect the properties of covalent compounds?
A. Bond type
B. Shape of the molecule
C. Polarity of the molecule
D. All of the above
64. Which type of covalent compounds is soluble in polar solvents?
A. Non-polar covalent compounds
B. Partially dissociating covalent compounds
C. Polar covalent compounds
D. Both A and B Correct
65. Which of the following solvents dissolves Naphthalene?
A. Water
B. CCl4
C. Benzene
D. Both B and C
66. What type of crystals do solid covalent compounds form?
A. Ionic crystals
B. Metallic crystals
C. Molecular crystals
D. None of the above
67. Are covalent compounds usually fast or slow in their reactions?
A. Fast
B. Slow
C. It depends on the compound
D. They don't react at all
68. Which of the following metals is liquid at room temperature and at normal atmospheric pressure?
A) Iron
B) Copper
C) Gold
D) Mercury
69. Which of the following terms refers to the ability of metals to be folded into thin sheets?
A) Ductility
B) Luster
C) Sonorous
D) Malleability
70. Which of the following metals is commonly used in wire formation due to its ductile nature?
A) Zinc
B) Silver
C) Copper
D) Aluminum
71. What property of metals allows them to be good conductors of heat and electricity?
A) Ductility
B) Malleability
C) Luster
D) Free electrons
72. What property of metals gives them a shiny surface?
A) Ductility
B) Luster
C) Sonorous
D) Malleability
73. Which property of metals allows them to produce a ringing sound when struck?
A) Ductility
B) Luster
C) Sonorous
D) Malleability
74. What is an Ionic bond?
A) A bond formed by sharing of electrons between two atoms
B) A bond formed by the transfer of electrons from an electropositive to an electronegative atom
C) A bond formed by overlapping of atomic orbitals
D) A bond formed by sharing of protons between two atoms
75. Who introduced the concept of the Ionic bond?
A) W. Kossel
B) J.J. Thomson
C) Niels Bohr
D) Marie Curie
76. What is the electronic configuration of Na?
A) 1s2, 2s2, 2p6, 3s1
B) 1s2, 2s2, 2p6, 3s2, 3p5
C) 2s2, 2p6, 3s1
D) 2s2, 2p6, 3s2, 3p5
77. What is the electronic configuration of Cl?
A) 1s2, 2s2, 2p6, 3s1
B) 1s2, 2s2, 2p6, 3s2, 3p5
C) 2s2, 2p6, 3s1
D) 2s2, 2p6, 3s2, 3p5
78. What is the charge on Na after the formation of an Ionic bond with Cl in NaCl?
A) Na has no charge
B) Na has a positive charge
C) Na has a negative charge
D) Na has a double positive charge
79. What is the electronic configuration of Na+ ion after the formation of an Ionic bond with Cl in NaCl?
A) 1s2, 2s2, 2p6
B) 2s2, 2p6
C) 2s2, 2p6, 3s1
D) 2s2, 2p6, 3s2, 3p5
80. What is the force that holds the ions together in an Ionic bond?
A) Covalent force
B) Metallic force
C) Hydrogen bonding force
D) Electrostatic force of attraction
81. What is a covalent bond?
A. A chemical bond formed between oppositely charged ions
B. A chemical bond in which two or more bonded atoms mutually share their valence electrons
C. A chemical bond formed by the transfer of electrons from an electropositive to an electronegative atom
D. A chemical bond in which the bonded atoms share four electrons
82. Who introduced the concept of the covalent bond?
A. G.N Lewis
B. W.Kossel
C. J.J. Thomson
D. Niels Bohr
83. How many types of covalent bonds are there based on the number of shared pairs of electrons?
A. One
B. Two
C. Three
D. Four
84. What is a single covalent bond?
A. A bond in which the bonded atoms share four electrons
B. A bond in which the bonded atoms share six electrons
C. A bond in which the bonded atoms share two electrons
D. A bond in which the bonded atoms have opposite charges
85. How is a single covalent bond represented?
A. By two dots or a single bar line
B. By four dots or a double bar line
C. By six dots or a triple bar line
D. By three dots or a double bar line
86. What is an example of a molecule formed by a single covalent bond?
A. Oxygen molecule (O2)
B. Nitrogen molecule (N2)
C. Chlorine molecule (Cl2)
D. Carbon dioxide molecule (CO2)
87. What is an example of a molecule formed by a double covalent bond?
A. Oxygen molecule (O2)
B. Nitrogen molecule (N2)
C. Chlorine molecule (Cl2)
D. Carbon dioxide molecule (CO2)
88. What is a triple covalent bond?
A. A bond in which the bonded atoms share four electrons
B. A bond in which the bonded atoms share six electrons
C. A bond in which the bonded atoms share two electrons
D. A bond in which the bonded atoms share eight electrons
89. How is a triple covalent bond represented?
A. By two dots or a single bar line
B. By four dots or a double bar line
C. By six dots or a triple bar line
D. By three dots or a double bar line
90. What is an example of a molecule formed by a triple covalent bond?
A. Oxygen molecule (O2)
B. Nitrogen molecule (N2)
C. Chlorine molecule (Cl2)
D. None
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