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Atomic Structure Practice Tests

These Grade 10 Science practice tests develop understanding of atomic models, protons, neutrons, electrons, atomic number, mass number, isotopes, ions, electron arrangements, energy levels, and atomic spectra.

Skills covered

  • Identifying the nucleus, protons, neutrons, electrons, atomic number, mass number, and neutral atoms
  • Calculating protons, neutrons, electrons, isotope mass numbers, and ion charges
  • Using valence electrons, energy levels, orbitals, Bohr models, electron clouds, and simple electron arrangements
  • Explaining ground states, excited states, photons, emission spectra, wavelength, frequency, and flame tests
  • Comparing Dalton, Thomson, Rutherford, Bohr, and modern quantum models of the atom

How to use these practice tests

Start with the atomic number and charge. Count protons, neutrons, and electrons carefully, then connect electron arrangement to energy, bonding, periodic position, and chemical behavior.

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

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Grade 10 Atomic Structure Practice Tests

Practice Grade 10 Science questions about atomic models, protons, neutrons, electrons, atomic number, isotopes, ions, electron arrangements, energy levels, and spectra.

Choose the best answer. Use atomic number, mass number, charge, electron arrangements, energy levels, and atomic models to evaluate each question.

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

What did Rutherford gold-foil experiments show about atomic structure?

Please select an answer first.

Correct answer: A

The correct answer is Atoms have a small, dense, positively charged nucleus and are mostly empty space..

  1. Identify the atomic quantity: Determine whether the question asks about the nucleus, subatomic particles, atomic number, mass number, charge, electrons, or energy levels.
  2. Use the atomic model: Most particles passed through the foil while a few deflected sharply, revealing a tiny dense nucleus.
  3. Check the calculation or relationship: The correct answer is Atoms have a small, dense, positively charged nucleus and are mostly empty space..

Most particles passed through the foil while a few deflected sharply, revealing a tiny dense nucleus.

2. QuestionMultiple choice

What did Thomson cathode-ray experiments help identify?

Please select an answer first.

Correct answer: B

The correct answer is The electron as a negatively charged subatomic particle.

  1. Identify the atomic quantity: Determine whether the question asks about the nucleus, subatomic particles, atomic number, mass number, charge, electrons, or energy levels.
  2. Use the atomic model: Cathode-ray evidence showed that atoms contain small negatively charged particles.
  3. Check the calculation or relationship: The correct answer is The electron as a negatively charged subatomic particle.

Cathode-ray evidence showed that atoms contain small negatively charged particles.

3. QuestionMultiple choice

What was a main idea of Dalton atomic theory?

Please select an answer first.

Correct answer: C

The correct answer is Matter is composed of atoms and chemical reactions rearrange atoms..

  1. Identify the atomic quantity: Determine whether the question asks about the nucleus, subatomic particles, atomic number, mass number, charge, electrons, or energy levels.
  2. Use the atomic model: Dalton model introduced atoms as basic units and reactions as rearrangements of atoms.
  3. Check the calculation or relationship: The correct answer is Matter is composed of atoms and chemical reactions rearrange atoms..

Dalton model introduced atoms as basic units and reactions as rearrangements of atoms.

4. QuestionMultiple choice

What did the Bohr model add to earlier nuclear models?

Please select an answer first.

Correct answer: D

The correct answer is Electrons occupy specific energy levels around the nucleus..

  1. Identify the atomic quantity: Determine whether the question asks about the nucleus, subatomic particles, atomic number, mass number, charge, electrons, or energy levels.
  2. Use the atomic model: Bohr proposed quantized electron energy levels to explain atomic spectra.
  3. Check the calculation or relationship: The correct answer is Electrons occupy specific energy levels around the nucleus..

Bohr proposed quantized electron energy levels to explain atomic spectra.

5. QuestionMultiple choice

What does the modern quantum model emphasize?

Please select an answer first.

Correct answer: A

The correct answer is Electron locations are described by probability regions called orbitals..

  1. Identify the atomic quantity: Determine whether the question asks about the nucleus, subatomic particles, atomic number, mass number, charge, electrons, or energy levels.
  2. Use the atomic model: The quantum model uses probability distributions rather than fixed electron paths.
  3. Check the calculation or relationship: The correct answer is Electron locations are described by probability regions called orbitals..

The quantum model uses probability distributions rather than fixed electron paths.

6. QuestionMultiple choice

What ion is a Group 1 metal most likely to form?

Please select an answer first.

Correct answer: B

The correct answer is A +1 ion.

  1. Identify the atomic quantity: Determine whether the question asks about the nucleus, subatomic particles, atomic number, mass number, charge, electrons, or energy levels.
  2. Use the atomic model: Group 1 metals usually lose one valence electron, forming a +1 cation.
  3. Check the calculation or relationship: The correct answer is A +1 ion.

Group 1 metals usually lose one valence electron, forming a +1 cation.

7. QuestionMultiple choice

What ion is a Group 17 nonmetal most likely to form?

Please select an answer first.

Correct answer: C

The correct answer is A −1 ion.

  1. Identify the atomic quantity: Determine whether the question asks about the nucleus, subatomic particles, atomic number, mass number, charge, electrons, or energy levels.
  2. Use the atomic model: Halogens usually gain one electron to complete their valence level, forming −1 anions.
  3. Check the calculation or relationship: The correct answer is A −1 ion.

Halogens usually gain one electron to complete their valence level, forming −1 anions.

8. QuestionMultiple choice

Why are noble gases generally stable?

Please select an answer first.

Correct answer: D

The correct answer is Their valence energy levels are filled or especially stable..

  1. Identify the atomic quantity: Determine whether the question asks about the nucleus, subatomic particles, atomic number, mass number, charge, electrons, or energy levels.
  2. Use the atomic model: A filled outer level reduces the tendency to gain, lose, or share electrons.
  3. Check the calculation or relationship: The correct answer is Their valence energy levels are filled or especially stable..

A filled outer level reduces the tendency to gain, lose, or share electrons.

9. QuestionMultiple choice

Which simple shell arrangement represents a neutral sodium atom with atomic number 11?

Please select an answer first.

Correct answer: A

The correct answer is [2, 8, 1].

  1. Identify the atomic quantity: Determine whether the question asks about the nucleus, subatomic particles, atomic number, mass number, charge, electrons, or energy levels.
  2. Use the atomic model: Sodium has 11 electrons arranged as 2 in the first level, 8 in the second, and 1 in the third.
  3. Check the calculation or relationship: The correct answer is [2, 8, 1].

Sodium has 11 electrons arranged as 2 in the first level, 8 in the second, and 1 in the third.

10. QuestionMultiple choice

Why do valence electrons strongly affect chemical behavior?

Please select an answer first.

Correct answer: B

The correct answer is They are the electrons gained, lost, or shared during bonding..

  1. Identify the atomic quantity: Determine whether the question asks about the nucleus, subatomic particles, atomic number, mass number, charge, electrons, or energy levels.
  2. Use the atomic model: Chemical bonds involve outer electrons, so their number and arrangement influence reactivity.
  3. Check the calculation or relationship: The correct answer is They are the electrons gained, lost, or shared during bonding..

Chemical bonds involve outer electrons, so their number and arrangement influence reactivity.

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