Structure of Atom Quiz - CBSE Class 12 Physics

Free practice quiz: Structure of Atom (CBSE Class 12 Physics). 20 multiple-choice questions with answers and explanations. Play online, no sign-up needed.

This CBSE Class 12 Physics practice quiz has 20 multiple-choice questions on Structure of Atom, and 20 of them come with an explanation. Try the 5 sample questions below (tap an option to check yourself), then play the full quiz online. No sign-up needed.

Sample questions

1. Which subatomic particle has a positive charge?

   1. Electron
   2. Neutron
   3. Proton
   4. Photon
   Show answer

   Answer: C. Proton

   Protons are positively charged particles found in the nucleus of an atom.

2. According to Bohr's model, what determines the energy level of an electron?

   1. Its mass
   2. Its charge
   3. Its principal quantum number
   4. Its velocity
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   Answer: C. Its principal quantum number

   In Bohr's model, the energy level of an electron is quantized and is determined by its principal quantum number (n).

3. Explain the concept of quantization of energy in the context of the Bohr model.

   1. Electrons can exist in any energy level.
   2. Electrons can only exist in discrete energy levels.
   3. Electrons continuously lose energy.
   4. Electrons continuously gain energy.
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   Answer: B. Electrons can only exist in discrete energy levels.

   The Bohr model postulates that electrons can only exist in specific, quantized energy levels, not in between.

4. How does the Heisenberg uncertainty principle affect our understanding of electron location in an atom?

   1. It allows us to pinpoint the exact location of an electron.
   2. It makes it impossible to simultaneously know both the position and momentum of an electron.
   3. It is irrelevant to the location of an electron.
   4. It determines the energy level of an electron.
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   Answer: B. It makes it impossible to simultaneously know both the position and momentum of an electron.

   The Heisenberg uncertainty principle states that it's impossible to simultaneously know both the position and momentum of an electron with perfect accuracy.

5. Explain the concept of atomic orbitals and their shapes (s, p, d). How are these shapes related to the probability of finding an electron?

   1. Atomic orbitals have definite shapes and locations for electrons.
   2. Atomic orbitals are regions of space where there is a high probability of finding an electron; s orbitals are spherical, p orbitals are dumbbell-shaped, and d orbitals are more complex.
   3. Atomic orbitals are not relevant to electron location.
   4. Atomic orbitals have no relation to probability.
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   Answer: B. Atomic orbitals are regions of space where there is a high probability of finding an electron; s orbitals are spherical, p orbitals are dumbbell-shaped, and d orbitals are more complex.

   Atomic orbitals represent regions where there's a high probability of finding an electron. The shapes reflect the probability distribution.

More questions in this quiz

Answers and explanations are in the full quiz.

1. Which subatomic particle has negligible mass compared to protons and neutrons?
2. What is the charge of an electron?
3. What is the approximate radius of a nucleus?
4. What is the significance of the principal quantum number (n) in the Bohr model?
5. What is the maximum number of electrons that can occupy a p subshell?
6. What is the maximum number of electrons that can be accommodated in an energy level with principal quantum number n=3?
7. Describe the limitations of the Bohr model of the atom.
8. What is the significance of de Broglie's hypothesis in understanding atomic structure?
9. Explain the concept of electron shells and subshells.
10. Explain the significance of quantum numbers in describing the state of an electron in an atom.
11. Derive the expression for the radius of the nth Bohr orbit using the Bohr model postulates.
12. Compare and contrast the Bohr model and the quantum mechanical model of the atom.
13. Discuss the limitations of the quantum mechanical model of the atom and the challenges in its application to complex atoms.
14. Apply the Aufbau principle, Hund's rule, and the Pauli exclusion principle to predict the electron configuration of a transition metal like Chromium (Cr). Explain any exceptions to the Aufbau principle observed.
15. Using advanced quantum mechanics, explain the origin of the fine structure of spectral lines in atomic spectra and its dependence on spin-orbit coupling. Discuss the role of relativistic effects.

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