Questions on Bohr's Atomic Model
20 Multiple-Choice Questions – Bohr's Atomic Model
1. What key feature distinguishes Bohr’s atomic model from Rutherford’s?
A) Discovery of protons
B) Introduction of sublevels
C) Defined orbits for electrons
D) Use of magnetic fields
E) Discovery of neutrons
2. In Bohr’s model, electrons move in:
A) Random paths
B) Fixed orbits with specific energies
C) Elliptical orbits
D) Cloud-like regions
E) Helical spirals
3. What is the name given to the specific paths in which electrons revolve around the nucleus in Bohr's model?
A) Shells
B) Clouds
C) Orbitals
D) Energy fields
E) Lattices
4. What happens when an electron jumps from a higher to a lower energy level in Bohr’s model?
A) Absorbs a photon
B) Emits a photon
C) Becomes a neutron
D) Disappears
E) Increases in mass
5. The Bohr model primarily explains the spectral lines of which element?
A) Oxygen
B) Helium
C) Hydrogen
D) Carbon
E) Neon
6. According to Bohr, which of the following is quantized in an atom?
A) The number of protons
B) The mass of electrons
C) The energy levels of electrons
D) The atomic weight
E) The radius of the atom
7. What fundamental principle did Bohr introduce regarding electron energy?
A) Electrons can have any energy
B) Electron energy is continuous
C) Electron energy is quantized
D) Electrons stop moving
E) Electrons repel photons
8. In Bohr’s model, energy levels are labeled as:
A) Letters
B) Random numbers
C) Quantum numbers (n)
D) Colors
E) Fractions
9. Which of the following is a limitation of Bohr’s atomic model?
A) It can’t explain hydrogen’s spectrum
B) It doesn’t include electrons
C) It fails for multi-electron atoms
D) It ignores neutrons
E) It includes too many variables
10. The energy of an electron in a Bohr orbit depends on:
A) Its speed
B) Its temperature
C) The radius of the nucleus
D) The principal quantum number (n)
E) The color it emits
11. The larger the value of "n", the electron is:
A) Closer to the nucleus
B) Heavier
C) At rest
D) Further from the nucleus
E) No longer bound
12. Which scientist's quantum ideas influenced Bohr's model?
A) Newton
B) Faraday
C) Planck
D) Mendeleev
E) Curie
13. What experimental evidence supported Bohr's model?
A) Behavior of gases
B) Spectral lines of hydrogen
C) Solid-state physics
D) Radioactive decay
E) Atomic mass data
14. In Bohr’s model, what causes the emission of light?
A) Neutron decay
B) Proton movement
C) Electron transitions
D) Nucleus vibrations
E) Ionization
15. Bohr’s model treats electrons as:
A) Energy clouds
B) Static charges
C) Massless particles
D) Orbiting particles
E) Neutron companions
16. What happens to an electron when it absorbs a photon?
A) Falls to a lower level
B) Disappears
C) Gets ionized instantly
D) Jumps to a higher energy level
E) Changes into a proton
17. According to Bohr, energy levels are:
A) Overlapping
B) Continuous
C) Discrete
D) Undefined
E) Variable
18. Bohr’s atomic model does NOT explain:
A) Emission spectra of hydrogen
B) Stability of electrons in hydrogen
C) Spectra of multi-electron atoms
D) Discrete energy levels
E) Photon emission
19. Which concept did Bohr incorporate from classical physics?
A) Electric charge of the proton
B) Circular orbits of planets
C) Laws of thermodynamics
D) Magnetic poles
E) Strong nuclear force
20. In modern atomic theory, Bohr’s orbits were replaced by:
A) Isotopes
B) Energy clouds
C) Sub-shells
D) Orbitals (quantum model)
E) Protons
- Questions on Quantization of Energy
- Questions on Photoelectric Effect
- Questions on Atomic Emission Spectra
Answer Key with Extended Explanations
1. C – Bohr proposed electrons travel in specific orbits, unlike Rutherford’s random electron model.
2. B – Bohr's electrons move in fixed orbits with definite energies.
3. A – These paths are called shells or energy levels.
4. B – When electrons fall to a lower level, they release energy as photons.
5. C – The Bohr model was developed to explain hydrogen's line spectrum.
6. C – The energy levels in Bohr’s model are quantized, meaning only certain values are allowed.
7. C – Bohr introduced the idea that electron energy is quantized.
8. C – Energy levels are identified by principal quantum numbers (n).
9. C – Bohr's model only works well for hydrogen-like (single-electron) atoms.
10. D – Electron energy is directly related to the principal quantum number (n).
11. D – A higher n-value means the electron is farther from the nucleus.
12. C – Planck’s idea of energy quanta influenced Bohr’s model.
13. B – The hydrogen emission spectrum confirmed Bohr’s model.
14. C – Light emission results from electrons dropping to lower levels.
15. D – Bohr treated electrons as particles orbiting the nucleus.
16. D – A photon’s energy excites an electron to a higher level.
17. C – Energy levels in Bohr’s model are discrete (quantized).
18. C – Bohr’s model doesn’t explain multi-electron atom spectra.
19. B – Bohr adapted the idea of planet-like orbits from classical physics.
20. D – Modern theory replaces orbits with quantum orbitals (regions of probability).
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