Nature of electromagnetic radiation, photoelectric effect, spectrum of hydrogen atom, Bohr model and its limitations - One Line Questions

1. Which series of spectral lines in the hydrogen atom spectrum lies in the ultraviolet region? — Lyman series
2. The spectrum of hydrogen atom is: — Line spectrum
3. The Bohr model introduces the idea of stationary states, meaning that electrons in these states: — Do not radiate energy.
4. If the intensity of light incident on a metal surface is increased, while keeping the frequency constant and above the threshold frequency, the number of photoelectrons emitted per second will: — Increase
5. According to the Bohr model, as the principal quantum number 'n' increases, the energy of the electron's orbit: — Increases
6. Which phenomenon demonstrates that light behaves as both a wave and a particle? — Photoelectric effect
7. Which of the following statements best describes the wave nature of electromagnetic radiation? — Electromagnetic radiation exhibits properties like reflection, refraction, and diffraction.
8. The Bohr model was a significant step forward because it introduced the concept of: — Electron shells and quantized energy levels
9. According to the photoelectric effect, if the frequency of incident light is below the threshold frequency, what happens? — No electrons are emitted.
10. Which of the following statements about the Bohr model is INCORRECT? — Electrons emit radiation continuously while orbiting.
11. In the Bohr model, when an electron jumps from a lower energy orbit to a higher energy orbit, the atom: — Absorbs energy
12. According to the Bohr model, the energy of an electron in the nth orbit of a hydrogen atom is given by E_n = -R_H/n², where R_H is the Rydberg constant. This indicates that: — Energy levels are discrete and negative.
13. The red line in the visible spectrum of hydrogen (Balmer series) corresponds to the transition from n=3 to n=2. If the frequency of this light is ν, what is the energy of the emitted photon? — hν
14. The Bohr model successfully explained the spectrum of which atom? — Hydrogen
15. In the hydrogen spectrum, the transition from n=3 to n=1 corresponds to emission in which region? — Ultraviolet
16. The kinetic energy of photoelectrons emitted is given by KE = hν - Φ, where Φ is the: — Work function of the metal
17. The particle nature of light is best exemplified by: — The photoelectric effect
18. Which of the following is a limitation of the Bohr model? — It failed to explain the fine structure of spectral lines.
19. The Bohr model failed to explain the spectra of atoms with more than one electron because: — It did not account for electron-electron repulsion.
20. Which spectral series of hydrogen lies entirely in the visible region? — Balmer series
21. The concept of wave-particle duality was introduced by: — Albert Einstein
22. The Bohr model assumes that the angular momentum of an electron in an orbit is quantized. This is expressed as: — mvr = nh/2π
23. In the Bohr model, the radius of the nth orbit is proportional to: — n^2
24. The Balmer series of spectral lines for hydrogen corresponds to electron transitions from higher energy levels to which principal energy level? — n=2
25. The Brackett series of hydrogen spectrum corresponds to transitions ending at which energy level? — n=4
26. The Paschen series of hydrogen spectrum corresponds to electron transitions ending at which energy level? — n=3
27. The Pfund series of hydrogen spectrum corresponds to electron transitions ending at which energy level? — n=5
28. According to the Bohr model, electrons orbit the nucleus in specific, fixed paths called: — Energy shells
29. The wave-particle duality of light means that light can exhibit properties of both: — Particles and waves
30. The Bohr model's limitation in explaining the fine structure of spectral lines was later addressed by the development of: — Quantum mechanics
31. The emission spectrum of hydrogen consists of distinct lines. What does each line represent? — The emission of a photon when an electron transitions from a higher energy level to a lower one.
32. Which of the following statements about the photoelectric effect is true? — There is a minimum frequency of light below which no electrons are emitted, regardless of intensity.
33. Which experimental observation could NOT be explained by the Bohr model? — The Zeeman effect (splitting of spectral lines in a magnetic field).
34. When monochromatic light shines on a metal surface and ejects electrons, the kinetic energy of the emitted electrons is dependent on: — The frequency of the light
35. The wave nature of light is demonstrated by phenomena like: — Diffraction and interference
36. The ultraviolet catastrophe, which classical physics could not explain but quantum mechanics did, related to: — Blackbody radiation
37. What does 'n' represent in the Bohr model's energy level formula? — The principal quantum number
38. A fundamental postulate of the Bohr model is that electrons can only exist in states with specific, quantized energy values. This is known as: — The quantization of energy
39. The photoelectric effect provides strong evidence for: — The existence of photons
40. What is the primary characteristic that distinguishes different types of electromagnetic radiation (e.g., radio waves, visible light, X-rays)? — Their wavelength or frequency
41. In the photoelectric effect, what is the minimum frequency of incident light required to eject electrons from a metal surface called? — Threshold frequency
42. The Bohr model is a semi-classical model because it: — Treats electrons as particles with quantized orbits.
43. The energy of a photon is given by the equation E = hν, where 'h' is Planck's constant and 'ν' is the frequency. This equation supports which concept? — The quantization of energy
44. The energy of a photon is directly proportional to its: — Frequency
45. Planck's quantum hypothesis, crucial for understanding the photoelectric effect and atomic spectra, states that energy is emitted or absorbed in discrete packets called: — Quanta
46. The photoelectric effect provides evidence for the quantization of light energy, meaning light energy is delivered in discrete units called: — Photons
47. The energy difference between two energy levels in an atom is related to the frequency of the emitted or absorbed photon by the equation: — ΔE = hc/λ
48. What is the relationship between wavelength (λ) and frequency (ν) for electromagnetic radiation? — λν = c
49. The frequency of the emitted photon when an electron jumps from a higher energy level E₂ to a lower energy level E₁ is given by: — ν = (E₂ - E₁)/h
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