NumicornNumicornLearn, solve, progress

Chemistry Practice Tests

These Grade 12 Science practice tests develop Chemistry skills through atomic structure, periodic trends, bonding, stoichiometry, gases, thermochemistry, kinetics, equilibrium, acids, redox, organic chemistry, and laboratory reasoning.

Skills covered

  • Analyzing isotopes, electron configurations, valence electrons, periodic trends, electronegativity, Lewis structures, and intermolecular forces
  • Using moles, molar mass, limiting reactants, percent yield, gas laws, molarity, dilution, and calorimetry relationships
  • Explaining activation energy, catalysts, entropy, dynamic equilibrium, Le Châtelier’s principle, equilibrium constants, and Gibbs free energy
  • Applying Brønsted–Lowry acids and bases, pH, buffers, neutralization, oxidation, reduction, galvanic cells, and electrolysis
  • Recognizing functional groups, hydrocarbons, isomers, polymers, spectroscopy, chromatography, environmental chemistry, and laboratory safety

How to use these practice tests

Write the relevant equation, identify the known quantities and units, and check whether the answer matches the chemical relationship. For conceptual questions, connect particle-level structure to observable properties.

For more Grade 12 Science practice, return to the Grade 12 Science category.

Select a test

5 Tests
1. Test2. Test3. Test4. Test5. Test

1. Test

Grade 12 Chemistry Practice Tests

Practice Grade 12 Science questions about atomic structure, periodic trends, bonding, stoichiometry, gases, thermochemistry, kinetics, equilibrium, acids, redox, and organic chemistry.

Choose the best answer. Track units, chemical relationships, equations, and conditions carefully, and distinguish thermodynamic favorability from reaction rate.

10 Questions
0/10 Questions0 %
Correct 0
Incorrect 0
Unanswered 10
1. QuestionMultiple choice

What are isotopes of an element?

Please select an answer first.

Correct answer: A

The correct answer is Atoms with the same number of protons but different numbers of neutrons.

  1. Identify the chemistry concept: Determine whether the question concerns atomic structure, bonding, stoichiometry, gases, energy, kinetics, equilibrium, acids, redox, organic chemistry, or laboratory practice.
  2. Apply the chemical principle: Atomic number is set by protons, while neutron differences change mass number and create isotopes.
  3. Check units and relationships: The correct answer is Atoms with the same number of protons but different numbers of neutrons.

Atomic number is set by protons, while neutron differences change mass number and create isotopes.

2. QuestionMultiple choice

What does an electron configuration describe?

Please select an answer first.

Correct answer: B

The correct answer is How electrons are distributed among energy levels and orbitals.

  1. Identify the chemistry concept: Determine whether the question concerns atomic structure, bonding, stoichiometry, gases, energy, kinetics, equilibrium, acids, redox, organic chemistry, or laboratory practice.
  2. Apply the chemical principle: Electron configuration shows the arrangement of electrons and helps explain chemical behavior.
  3. Check units and relationships: The correct answer is How electrons are distributed among energy levels and orbitals.

Electron configuration shows the arrangement of electrons and helps explain chemical behavior.

3. QuestionMultiple choice

Why are valence electrons important?

Please select an answer first.

Correct answer: C

The correct answer is They are the outer electrons most involved in bonding and chemical reactions.

  1. Identify the chemistry concept: Determine whether the question concerns atomic structure, bonding, stoichiometry, gases, energy, kinetics, equilibrium, acids, redox, organic chemistry, or laboratory practice.
  2. Apply the chemical principle: Valence electrons control many patterns of reactivity, bonding, and periodic behavior.
  3. Check units and relationships: The correct answer is They are the outer electrons most involved in bonding and chemical reactions.

Valence electrons control many patterns of reactivity, bonding, and periodic behavior.

4. QuestionMultiple choice

What generally happens to atomic radius from left to right across a period?

Please select an answer first.

Correct answer: D

The correct answer is It decreases because the nucleus attracts electrons more strongly.

  1. Identify the chemistry concept: Determine whether the question concerns atomic structure, bonding, stoichiometry, gases, energy, kinetics, equilibrium, acids, redox, organic chemistry, or laboratory practice.
  2. Apply the chemical principle: Across a period, effective nuclear charge increases while electrons are added to the same principal energy level.
  3. Check units and relationships: The correct answer is It decreases because the nucleus attracts electrons more strongly.

Across a period, effective nuclear charge increases while electrons are added to the same principal energy level.

5. QuestionMultiple choice

What is the general trend for first ionization energy across a period?

Please select an answer first.

Correct answer: A

The correct answer is It tends to increase.

  1. Identify the chemistry concept: Determine whether the question concerns atomic structure, bonding, stoichiometry, gases, energy, kinetics, equilibrium, acids, redox, organic chemistry, or laboratory practice.
  2. Apply the chemical principle: Stronger effective nuclear attraction generally makes an electron more difficult to remove across a period.
  3. Check units and relationships: The correct answer is It tends to increase.

Stronger effective nuclear attraction generally makes an electron more difficult to remove across a period.

6. QuestionMultiple choice

What does electronegativity measure?

Please select an answer first.

Correct answer: B

The correct answer is An atom’s tendency to attract shared electrons in a chemical bond.

  1. Identify the chemistry concept: Determine whether the question concerns atomic structure, bonding, stoichiometry, gases, energy, kinetics, equilibrium, acids, redox, organic chemistry, or laboratory practice.
  2. Apply the chemical principle: Electronegativity describes the relative pull on bonding electrons and helps predict bond polarity.
  3. Check units and relationships: The correct answer is An atom’s tendency to attract shared electrons in a chemical bond.

Electronegativity describes the relative pull on bonding electrons and helps predict bond polarity.

7. QuestionMultiple choice

What is an ionic bond?

Please select an answer first.

Correct answer: C

The correct answer is Electrostatic attraction between oppositely charged ions after electron transfer.

  1. Identify the chemistry concept: Determine whether the question concerns atomic structure, bonding, stoichiometry, gases, energy, kinetics, equilibrium, acids, redox, organic chemistry, or laboratory practice.
  2. Apply the chemical principle: Ionic bonding commonly forms when one atom transfers electrons to another, producing oppositely charged ions.
  3. Check units and relationships: The correct answer is Electrostatic attraction between oppositely charged ions after electron transfer.

Ionic bonding commonly forms when one atom transfers electrons to another, producing oppositely charged ions.

8. QuestionMultiple choice

What makes a covalent bond polar?

Please select an answer first.

Correct answer: D

The correct answer is The bonded atoms share electrons unequally because of different electronegativities.

  1. Identify the chemistry concept: Determine whether the question concerns atomic structure, bonding, stoichiometry, gases, energy, kinetics, equilibrium, acids, redox, organic chemistry, or laboratory practice.
  2. Apply the chemical principle: Unequal electron sharing creates partial charges and a bond dipole.
  3. Check units and relationships: The correct answer is The bonded atoms share electrons unequally because of different electronegativities.

Unequal electron sharing creates partial charges and a bond dipole.

9. QuestionMultiple choice

What is the purpose of a Lewis structure?

Please select an answer first.

Correct answer: A

The correct answer is To represent valence electrons, bonds, and lone pairs in a molecule or ion.

  1. Identify the chemistry concept: Determine whether the question concerns atomic structure, bonding, stoichiometry, gases, energy, kinetics, equilibrium, acids, redox, organic chemistry, or laboratory practice.
  2. Apply the chemical principle: Lewis structures help predict bonding, lone pairs, formal charge, and molecular geometry.
  3. Check units and relationships: The correct answer is To represent valence electrons, bonds, and lone pairs in a molecule or ion.

Lewis structures help predict bonding, lone pairs, formal charge, and molecular geometry.

10. QuestionMultiple choice

What are intermolecular forces?

Please select an answer first.

Correct answer: B

The correct answer is Attractions between separate molecules or particles.

  1. Identify the chemistry concept: Determine whether the question concerns atomic structure, bonding, stoichiometry, gases, energy, kinetics, equilibrium, acids, redox, organic chemistry, or laboratory practice.
  2. Apply the chemical principle: Intermolecular forces influence boiling point, melting point, viscosity, and solubility.
  3. Check units and relationships: The correct answer is Attractions between separate molecules or particles.

Intermolecular forces influence boiling point, melting point, viscosity, and solubility.

Previous testNext test