Chemistry Quiz Questions for College Students

Introduction
Chemistry quiz questions for college students offer an engaging way to test knowledge, deepen understanding, and challenge concepts across topics in chemistry, from atomic structure to reactions.

Chemistry Quiz Questions for College Students

1. What is the atomic number of hydrogen?
2. Define isotopes with an example.
3. What is the molecular formula of water?
4. State Avogadro’s number.
5. Name the process by which gas changes to a liquid.
6. What is the molar mass of CO₂?
7. Define a covalent bond.
8. What is pH value of pure water?
9. Name the most abundant element in the Earth’s crust.
10. What is the valency of carbon?
11. What is a cation?
12. State the law of conservation of mass.
13. Define molarity.
14. What is the chemical formula for common salt?
15. Name the acid found in lemons.
16. What is the periodic table?
17. Identify the group and period of sodium in the periodic table.
18. Explain the octet rule.
19. Which gas is evolved during photosynthesis?
20. What is an electrolyte?
21. Define oxidation.
22. Name the scientist who developed the periodic table.
23. What is the unit of atomic mass?
24. Write the chemical formula for ammonia.
25. Define ionization energy.
26. What is the electron configuration of helium?
27. State the full form of IUPAC.
28. What are alkali metals?
29. Name a radioactive element.
30. What is electrolysis?
31. Describe a redox reaction.
32. What is a catalyst?
33. Define ionic bond with an example.
34. Name the main component of natural gas.
35. What is the pH range of acidic solutions?
36. State the properties of metals.
37. What is the color of phenolphthalein in basic solution?
38. Identify the element with the highest electronegativity.
39. What is an endothermic reaction?
40. Explain displacement reaction with an example.
41. What are noble gases?
42. What is meant by solubility?
43. Define functional group in organic chemistry.
44. What is allotropy?
45. State Boyle’s law.
46. What is a buffer solution?
47. Name the catalyst used in the Haber process.
48. What is the atomic mass of oxygen?
49. What does pH stand for?
50. Define chemical equilibrium.
51. What is a covalent compound?
52. State Charles’s law.
53. What is neutralization?
54. What is the symbol for sodium?
55. Define isotonic solutions.
56. What is electronegativity?
57. Name the heaviest naturally occurring element.
58. What is the formula for sulfuric acid?
59. Explain VSEPR theory.
60. Define enthalpy change.
61. Name an example of a transition metal.
62. What is a Lewis structure?
63. State the empirical formula.
64. What is amphoterism?
65. What are metalloids?
66. Define half-life in nuclear chemistry.
67. What is a polyatomic ion?
68. Name the gas responsible for acid rain.
69. Define resonance in chemistry.
70. What is chemical kinetics?
71. State Dalton’s atomic theory.
72. What is the freezing point of water in Celsius?
73. Define covalent radius.
74. What is a homogeneous mixture?
75. Name the law that governs gas diffusion.
76. What is ionization potential?
77. Define Lewis base.
78. Explain what hydrophilic means.
79. What is a structural isomer?
80. Describe an acidic buffer.
81. What is Raoult’s law?
82. Name a common amphoteric oxide.
83. Define chemical bonding.
84. What is specific heat capacity?
85. What is a diatomic molecule?
86. State the function of a spectrophotometer.
87. What is standard enthalpy of formation?
88. Define colloidal solution.
89. What is nuclear fusion?
90. Name the most electronegative element.
91. What is sublimation?
92. Define hydration energy.
93. What are hydrocarbons?
94. What is a limiting reagent?
95. Explain chemical decomposition.
96. What is Planck’s constant?
97. Define solute and solvent.
98. What is the purpose of a catalyst?
99. Name the allotropes of carbon.
100. What is corrosion?

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Answers

1. 1
2. Isotopes are atoms of the same element with different numbers of neutrons, e.g., Carbon-12 and Carbon-14.
3. H₂O
4. (6.022 \times 10^{23}) mol(^{-1})
5. Condensation
6. 44 g/mol
7. A covalent bond is formed by the sharing of electrons.
8. 7
9. Oxygen
10. 4
11. A positively charged ion
12. Mass cannot be created or destroyed.
13. Number of moles of solute per liter of solution.
14. NaCl
15. Citric acid
16. A table of chemical elements arranged by atomic number.
17. Group 1, Period 3
18. Atoms combine to achieve eight electrons in their valence shell.
19. Oxygen
20. A substance that conducts electricity when dissolved.
21. Loss of electrons.
22. Dmitri Mendeleev
23. Atomic Mass Unit (amu)
24. NH₃
25. Energy required to remove an electron from an atom.
26. 1s²
27. International Union of Pure and Applied Chemistry
28. Group 1 elements of the periodic table.
29. Uranium
30. Decomposition of a compound using electricity.
31. Reaction involving oxidation and reduction.
32. Substance that increases reaction rate without being consumed.
33. Bond formed by the transfer of electrons, e.g., NaCl.
34. Methane (CH₄)
35. Less than 7
36. Ductile, malleable, conduct heat and electricity.
37. Pink
38. Fluorine
39. Reaction that absorbs energy.
40. A more reactive element displaces a less reactive one.
41. Elements in Group 18 with full valence shells.
42. Ability of a substance to dissolve.
43. Specific atom group causing chemical properties.
44. Existence in different forms, e.g., Carbon (diamond and graphite).
45. Pressure of gas inversely proportional to volume at constant temperature.
46. Resists pH change.
47. Iron
48. 16 amu
49. Power of hydrogen.
50. State where forward and reverse reactions occur at equal rates.
51. Compound formed by shared electrons.
52. Volume of gas is proportional to its temperature.
53. Reaction between acid and base forming salt and water.
54. Na
55. Same osmotic pressure solutions.
56. Tendency of an atom to attract electrons.
57. Uranium
58. H₂SO₄
59. Valence Shell Electron Pair Repulsion theory.
60. Heat change at constant pressure.
61. Iron, Copper, etc.
62. Representation of covalent bonding in molecules.
63. Simplest ratio of atoms in a compound.
64. Substance acting as acid and base.
65. Elements with metal and nonmetal properties.
66. Time for half of a radioactive substance to decay.
67. Ion with multiple atoms.
68. Sulfur dioxide (SO₂)
69. Stabilization of electron distribution in molecules.
70. Study of reaction rates.
71. Atoms are indivisible and indestructible particles.
72. 0°C
73. Half the distance between nuclei of two bonded atoms.
74. Mixture with uniform composition.
75. Graham’s Law.
76. Energy to remove outer electron from a neutral atom.
77. Electron donor in Lewis theory.
78. Water-attracting property.
79. Compounds with the same formula, different structures.
80. Mixture maintaining acidic pH.
81. Relation of vapor pressure to mole fraction.
82. Aluminum oxide
83. Formation of bonds between atoms.
84. Heat required to change temperature of 1g of substance by 1°C.
85. Molecule with two atoms.
86. Measures light absorption of a solution.
87. Heat change when one mole of substance forms.
88. Mixture with dispersed particles in a medium.
89. Reaction of hydrogen nuclei into helium.
90. Fluorine
91. Solid changing to vapor without liquid state.
92. Energy released when ions dissolve.
93. Compounds with carbon and hydrogen.
94. Reactant completely consumed in reaction.
95. Breaking down of a compound.
96. (6.626 \times 10^{-34}) Js
97. Solute dissolves, solvent dissolves other.
98. Speeds up chemical reactions.
99. Diamond, graphite, and fullerene.
100. Gradual degradation of metals.

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Chemistry Quiz Questions for College Students: Key Takeaways

1. Chemical bonding defines how atoms combine.
2. pH is vital for measuring acidity and basicity.
3. Elements are classified in the periodic table.
4. Redox reactions involve electron transfer.
5. Atomic theory is foundational in chemistry.
6. Reaction rates depend on catalysts and conditions.
7. Periodic trends guide chemical reactivity.
8. Molarity measures solution concentration.
9. States of matter transition via energy change.
10. Acids and bases neutralize to form salt.

Also Read: Chemistry Quiz Class 12

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