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Chemical Bonding Practice Tests

These Grade 10 Science practice tests develop ionic, covalent, and metallic bonding, valence electrons, the octet rule, Lewis structures, compound formulas, polarity, molecular shape, and intermolecular forces.

Skills covered

  • Distinguishing ionic, covalent, and metallic bonds by tracking electron transfer, sharing, and mobility
  • Using valence electrons, the octet rule, Lewis structures, lone pairs, and bond order
  • Writing neutral ionic formulas for common cations and anions using charge balance
  • Explaining electronegativity, polar and nonpolar bonds, molecular polarity, and molecular shape
  • Comparing hydrogen bonding, dipole-dipole forces, London dispersion forces, and intramolecular bonds

How to use these practice tests

Count valence electrons first, then decide whether atoms transfer or share electrons. For formulas, balance charges; for molecular polarity, consider both bond polarity and the overall shape.

For more Grade 10 Science practice, return to the Grade 10 Science category.

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Grade 10 Chemical Bonding Practice Tests

Practice Grade 10 Science questions about ionic, covalent, and metallic bonding, valence electrons, octet rule, Lewis structures, formulas, polarity, and intermolecular forces.

Choose the best answer. Track valence electrons, charge, sharing or transfer, Lewis structures, molecular shape, polarity, and compound formulas.

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

What happens in a single covalent bond?

Please select an answer first.

Correct answer: A

The correct answer is Two atoms share one pair of electrons..

  1. Identify the bonding concept: Determine whether the question asks about ionic, covalent, or metallic bonding, Lewis structures, polarity, formulas, or intermolecular forces.
  2. Track electrons and charge: A single covalent bond consists of one shared electron pair.
  3. Check the structure or property: The correct answer is Two atoms share one pair of electrons..

A single covalent bond consists of one shared electron pair.

2. QuestionMultiple choice

What does a double covalent bond contain?

Please select an answer first.

Correct answer: B

The correct answer is Two shared pairs of electrons.

  1. Identify the bonding concept: Determine whether the question asks about ionic, covalent, or metallic bonding, Lewis structures, polarity, formulas, or intermolecular forces.
  2. Track electrons and charge: A double bond includes two pairs of electrons shared between the bonded atoms.
  3. Check the structure or property: The correct answer is Two shared pairs of electrons.

A double bond includes two pairs of electrons shared between the bonded atoms.

3. QuestionMultiple choice

What does a triple covalent bond contain?

Please select an answer first.

Correct answer: C

The correct answer is Three shared pairs of electrons.

  1. Identify the bonding concept: Determine whether the question asks about ionic, covalent, or metallic bonding, Lewis structures, polarity, formulas, or intermolecular forces.
  2. Track electrons and charge: A triple bond has three shared electron pairs between two atoms.
  3. Check the structure or property: The correct answer is Three shared pairs of electrons.

A triple bond has three shared electron pairs between two atoms.

4. QuestionMultiple choice

What does a Lewis structure represent?

Please select an answer first.

Correct answer: D

The correct answer is Valence electrons, shared bonding pairs, and lone pairs.

  1. Identify the bonding concept: Determine whether the question asks about ionic, covalent, or metallic bonding, Lewis structures, polarity, formulas, or intermolecular forces.
  2. Track electrons and charge: Lewis structures show how valence electrons are arranged around bonded atoms.
  3. Check the structure or property: The correct answer is Valence electrons, shared bonding pairs, and lone pairs.

Lewis structures show how valence electrons are arranged around bonded atoms.

5. QuestionMultiple choice

How does a Lewis structure help apply the octet rule?

Please select an answer first.

Correct answer: A

The correct answer is It lets a writer count electrons around each atom and check for stable outer levels..

  1. Identify the bonding concept: Determine whether the question asks about ionic, covalent, or metallic bonding, Lewis structures, polarity, formulas, or intermolecular forces.
  2. Track electrons and charge: Counting bonding and lone-pair electrons shows whether an atom reaches a typical stable arrangement.
  3. Check the structure or property: The correct answer is It lets a writer count electrons around each atom and check for stable outer levels..

Counting bonding and lone-pair electrons shows whether an atom reaches a typical stable arrangement.

6. QuestionMultiple choice

Why can hydrogen follow a duet rule rather than an octet rule?

Please select an answer first.

Correct answer: B

The correct answer is Its first energy level is full with two electrons..

  1. Identify the bonding concept: Determine whether the question asks about ionic, covalent, or metallic bonding, Lewis structures, polarity, formulas, or intermolecular forces.
  2. Track electrons and charge: The first energy level has only one orbital and can hold two electrons.
  3. Check the structure or property: The correct answer is Its first energy level is full with two electrons..

The first energy level has only one orbital and can hold two electrons.

7. QuestionMultiple choice

What is the approximate shape of a water molecule, H₂O?

Please select an answer first.

Correct answer: C

The correct answer is Bent.

  1. Identify the bonding concept: Determine whether the question asks about ionic, covalent, or metallic bonding, Lewis structures, polarity, formulas, or intermolecular forces.
  2. Track electrons and charge: Two bonding pairs and two lone pairs around oxygen produce a bent molecular shape.
  3. Check the structure or property: The correct answer is Bent.

Two bonding pairs and two lone pairs around oxygen produce a bent molecular shape.

8. QuestionMultiple choice

What is the approximate shape of carbon dioxide, CO₂?

Please select an answer first.

Correct answer: D

The correct answer is Linear.

  1. Identify the bonding concept: Determine whether the question asks about ionic, covalent, or metallic bonding, Lewis structures, polarity, formulas, or intermolecular forces.
  2. Track electrons and charge: Carbon dioxide has two electron regions around central carbon, producing a linear shape.
  3. Check the structure or property: The correct answer is Linear.

Carbon dioxide has two electron regions around central carbon, producing a linear shape.

9. QuestionMultiple choice

What is a polar covalent bond?

Please select an answer first.

Correct answer: A

The correct answer is A covalent bond in which electrons are shared unequally.

  1. Identify the bonding concept: Determine whether the question asks about ionic, covalent, or metallic bonding, Lewis structures, polarity, formulas, or intermolecular forces.
  2. Track electrons and charge: Different electronegativities pull the shared electrons unequally in a polar covalent bond.
  3. Check the structure or property: The correct answer is A covalent bond in which electrons are shared unequally.

Different electronegativities pull the shared electrons unequally in a polar covalent bond.

10. QuestionMultiple choice

What is a nonpolar covalent bond?

Please select an answer first.

Correct answer: B

The correct answer is A bond in which electrons are shared equally or nearly equally.

  1. Identify the bonding concept: Determine whether the question asks about ionic, covalent, or metallic bonding, Lewis structures, polarity, formulas, or intermolecular forces.
  2. Track electrons and charge: Atoms with equal or very similar electronegativities share bonding electrons nearly equally.
  3. Check the structure or property: The correct answer is A bond in which electrons are shared equally or nearly equally.

Atoms with equal or very similar electronegativities share bonding electrons nearly equally.

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