Questions on Quantization of Energy
Multiple-Choice Questions: Quantization of Energy
1. What does it mean that energy is quantized?
A) Energy has no upper limit
B) Energy is continuous and infinite
C) Energy exists in fixed, discrete packets
D) Energy can be created or destroyed
E) Energy only applies to visible light
2. Who proposed the idea of energy quantization in blackbody radiation?
A) Albert Einstein
B) Niels Bohr
C) Max Planck
D) James Clerk Maxwell
E) Ernest Rutherford
3. The smallest amount of energy that can be emitted or absorbed as electromagnetic radiation is called a:
A) Photon
B) Neutron
C) Quark
D) Wavelet
E) Mole
4. What is the equation that relates energy and frequency in quantized form?
A) E = mc²
B) E = hv
C) E = h + v
D) E = λν
E) E = Fd
5. What is Planck's constant (h) approximately equal to?
A) 3.0 × 10⁸ J·s
B) 1.6 × 10⁻¹⁹ J
C) 9.8 m/s²
D) 6.63 × 10⁻³⁴ J·s
E) 1.0 × 10⁶ J·s
6. In the context of the photoelectric effect, a photon must have:
A) A mass larger than an electron
B) The correct wavelength
C) Energy greater than the work function
D) A charge opposite the electron
E) A negative spin
7. The quantization of energy explains why:
A) All colors are visible in atoms
B) Atoms can emit any energy level
C) Only certain frequencies of light are emitted
D) Energy levels are infinite
E) Atoms are unstable
8. The photoelectric effect supports the idea that light behaves as:
A) A sound wave
B) A magnetic field only
C) A stream of particles (photons)
D) A transverse wave only
E) A gravitational wave
9. What does the energy of a photon depend on?
A) Its mass
B) Its speed
C) Its wavelength or frequency
D) Its volume
E) Its temperature
10. If the frequency of radiation increases, what happens to photon energy?
A) It decreases
B) It remains the same
C) It increases
D) It becomes zero
E) It becomes negative
11. Quantized energy levels in atoms result in:
A) A white light spectrum
B) Continuous emission
C) Emission of line spectra
D) Emission of heat only
E) Gravitational waves
12. Which phenomenon is a direct result of energy quantization?
A) Doppler effect
B) Boiling point elevation
C) Atomic line spectra
D) Conduction of electricity
E) Elastic collisions
13. What happens when an electron absorbs a photon with the right energy?
A) It emits more light
B) It stays in the same state
C) It moves to a lower energy level
D) It jumps to a higher energy level
E) It gains mass
14. What happens when an electron moves from a higher to a lower energy level?
A) It absorbs energy
B) It gains kinetic energy
C) It loses charge
D) It emits a photon
E) It decays into a proton
15. The energy of a photon emitted by an atom corresponds to:
A) The total energy of the atom
B) The mass of the electron
C) The difference in energy levels
D) The number of protons in the nucleus
E) The gravitational field
16. In quantum theory, energy is said to be:
A) Random
B) Infinite
C) Finite and continuous
D) Discrete and quantized
E) Imaginary
17. What is the unit of energy when using Planck’s equation E = hv?
A) Newton
B) Joule
C) Coulomb
D) Kelvin
E) Tesla
18. What is the quantization condition in Bohr’s model of the hydrogen atom?
A) Only even-numbered orbits are allowed
B) The angular momentum is quantized
C) Protons can orbit the nucleus
D) The nucleus is in motion
E) Energy is proportional to atomic mass
19. What determines whether a photon can eject an electron from a metal surface?
A) The color of light
B) The pressure
C) The metal’s temperature
D) The photon’s energy compared to the work function
E) The time of exposure
20. In quantized systems, energy values are:
A) Continuous and unrestricted
B) Only dependent on mass
C) Discrete and specific
D) Irrelevant to the atomic model
E) Based on chemical bonds only
- Questions on Electromagnetic Spectrum
- Questions on Electromagnetic Induction
- Questions on Wavelength and Frequency Calculations
Answers with Extended Explanations
1. C – Quantization means energy exists in fixed packets, not continuous flow.
2. C – Max Planck introduced energy quantization to explain blackbody radiation.
3. A – A photon is the smallest energy packet of light.
4. B – E = hv, where h is Planck’s constant and v is frequency.
5. D – Planck’s constant is 6.63 × 10⁻³⁴ J·s.
6. C – A photon must have energy greater than the work function to eject electrons.
7. C – Only specific frequencies (colors) are emitted due to discrete energy levels.
8. C – The photoelectric effect shows light behaves as particles (photons).
9. C – Photon energy depends on wavelength/frequency.
10. C – Photon energy increases with frequency (E = hv).
11. C – Line spectra are caused by electrons moving between quantized energy levels.
12. C – Atomic line spectra are a result of energy quantization.
13. D – The electron jumps to a higher level when absorbing energy.
14. D – Moving to a lower energy level releases energy as a photon.
15. C – Emitted photon energy equals the difference between energy levels.
16. D – In quantum theory, energy is discrete and quantized.
17. B – Energy is measured in joules when using E = hv.
18. B – Bohr said angular momentum is quantized in specific orbits.
19. D – A photon can eject an electron only if its energy exceeds the work function.
20. C – Quantized systems allow specific (discrete) energy values only.
Share Online!
