Nature of electromagnetic radiation, photoelectric effect, spectrum of hydrogen atom, Bohr model and its limitations - Question Bank
1. The Bohr model was a significant step forward because it introduced the concept of:
2. The photoelectric effect provides evidence for the quantization of light energy, meaning light energy is delivered in discrete units called:
3. 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:
4. The Bohr model's limitation in explaining the fine structure of spectral lines was later addressed by the development of:
5. Which spectral series of hydrogen lies entirely in the visible region?
6. 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:
7. The ultraviolet catastrophe, which classical physics could not explain but quantum mechanics did, related to:
8. The Bohr model introduces the idea of stationary states, meaning that electrons in these states:
9. The wave-particle duality of light means that light can exhibit properties of both:
10. Which of the following statements about the photoelectric effect is true?
11. The Pfund series of hydrogen spectrum corresponds to electron transitions ending at which energy level?
12. In the Bohr model, the radius of the nth orbit is proportional to:
13. The kinetic energy of photoelectrons emitted is given by KE = hν - Φ, where Φ is the:
14. What is the relationship between wavelength (λ) and frequency (ν) for electromagnetic radiation?
15. The Bohr model failed to explain the spectra of atoms with more than one electron because:
16. 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?
17. The energy difference between two energy levels in an atom is related to the frequency of the emitted or absorbed photon by the equation:
18. The concept of wave-particle duality was introduced by:
19. Which of the following statements about the Bohr model is INCORRECT?
20. The Paschen series of hydrogen spectrum corresponds to electron transitions ending at which energy level?
21. In the hydrogen spectrum, the transition from n=3 to n=1 corresponds to emission in which region?
22. The energy of a photon is directly proportional to its:
23. 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:
24. Planck's quantum hypothesis, crucial for understanding the photoelectric effect and atomic spectra, states that energy is emitted or absorbed in discrete packets called:
25. The particle nature of light is best exemplified by:
26. The wave nature of light is demonstrated by phenomena like:
27. Which experimental observation could NOT be explained by the Bohr model?
28. The Bohr model is a semi-classical model because it:
29. According to the Bohr model, as the principal quantum number 'n' increases, the energy of the electron's orbit:
30. What does 'n' represent in the Bohr model's energy level formula?
31. The Bohr model assumes that the angular momentum of an electron in an orbit is quantized. This is expressed as:
32. Which of the following is a limitation of the Bohr model?
33. The Bohr model successfully explained the spectrum of which atom?
34. In the Bohr model, when an electron jumps from a lower energy orbit to a higher energy orbit, the atom:
35. A fundamental postulate of the Bohr model is that electrons can only exist in states with specific, quantized energy values. This is known as:
36. According to the Bohr model, electrons orbit the nucleus in specific, fixed paths called:
37. The Brackett series of hydrogen spectrum corresponds to transitions ending at which energy level?
38. The Balmer series of spectral lines for hydrogen corresponds to electron transitions from higher energy levels to which principal energy level?
39. Which series of spectral lines in the hydrogen atom spectrum lies in the ultraviolet region?
40. The emission spectrum of hydrogen consists of distinct lines. What does each line represent?
41. The spectrum of hydrogen atom is:
42. Which phenomenon demonstrates that light behaves as both a wave and a particle?
43. The photoelectric effect provides strong evidence for:
44. When monochromatic light shines on a metal surface and ejects electrons, the kinetic energy of the emitted electrons is dependent on:
45. According to the photoelectric effect, if the frequency of incident light is below the threshold frequency, what happens?
46. In the photoelectric effect, what is the minimum frequency of incident light required to eject electrons from a metal surface called?
47. 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?
48. What is the primary characteristic that distinguishes different types of electromagnetic radiation (e.g., radio waves, visible light, X-rays)?
49. Which of the following statements best describes the wave nature of electromagnetic radiation?