Atomic structure, term symbols, coupling schemes and spectra of many‑electron systems - Question Bank
1. Which of the following is a consequence of the electrostatic interaction between electrons in a many-electron atom?
2. In the context of atomic spectra, what does the term 'multiplet' refer to?
3. What is the fundamental principle behind the formation of Hund's rules?
4. The spectral lines from many-electron systems are often more complex than those from one-electron systems due to:
5. Which coupling scheme becomes more important as the atomic number increases due to the increasing strength of spin-orbit coupling?
6. In the term symbol 2S+1L_J, the number of possible values for J is (2S+1) if L >= S, and (2L+1) if S >= L. For a ³D term (S=1, L=2), what are the possible J values?
7. What is the term symbol for the ground state of a Carbon atom (atomic number 6)?
8. The fine structure of atomic spectra is primarily due to:
9. The spectral lines observed in the emission spectrum of hydrogen are due to transitions between different energy levels. These transitions are governed by:
10. What is the term symbol for the ground state of a Boron atom (atomic number 5)?
11. Spin-orbit coupling is more significant for atoms with:
12. Which phenomenon involves the splitting of spectral lines due to the interaction of electron spins with orbital angular momentum?
13. Another common selection rule for electric dipole transitions in atomic spectra is ΔJ = 0, ±1 (excluding J=0→J=0). What is the rule for Δl (change in orbital angular momentum quantum number of a single electron)?
14. The selection rules for electronic transitions in atomic spectra dictate which transitions are allowed. For electric dipole transitions, a common rule is ΔL = 0, ±1 (excluding 0→0). What is the rule for ΔS?
15. If L=1 and S=1, what are the possible J values?
16. If L=2 and S=1/2, what are the possible J values?
17. For a given term symbol, the number of possible J values depends on the relationship between L and S. If L > S, the possible J values range from:
18. What does the J-value (total angular momentum quantum number) represent in the context of atomic spectra?
19. The energy difference between two electronic states in an atom is related to the frequency (ν) of the absorbed or emitted photon by the equation:
20. Which type of spectroscopy is used to study electronic transitions in atoms and molecules?
21. Spectroscopy is the study of the interaction between:
22. Atomic spectra provide information about:
23. The splitting of spectral lines in an electric field is known as:
24. The splitting of spectral lines in a magnetic field is known as:
25. What is the ground state term symbol for a d² electron configuration?
26. Which of the following terms is NOT possible for a d¹ electron configuration?
27. What is the ground state term symbol for a p² electron configuration?
28. What is the term symbol for a p¹ electron configuration?
29. Hund's Rule of Maximum Multiplicity is a consequence of:
30. Hund's Rule of Maximum Multiplicity states that for a given electron configuration, the term with the highest multiplicity is:
31. Which coupling scheme is typically dominant for heavier atoms?
32. In jj-coupling, the individual electron orbital angular momentum (l_i) and spin angular momentum (s_i) are first coupled to form j_i, and then these are coupled to form:
33. In LS-coupling, the total orbital angular momentum (L) and total spin angular momentum (S) are coupled to form:
34. Which coupling scheme is typically dominant for lighter atoms?
35. What is the value of L for an S term?
36. What is the value of L for a P term?
37. What is the value of L for a D term?
38. For a system with total spin quantum number S=1, the multiplicity (2S+1) is:
39. For a system with total spin quantum number S=1/2, the multiplicity (2S+1) is:
40. The multiplicity of a term symbol (2S+1) indicates:
41. In a term symbol 2S+1L_J, what does the 'J' represent?
42. In a term symbol 2S+1L_J, what does the 'L' represent?
43. A term symbol is typically represented as 2S+1L_J. What does the 'S' in 2S+1 represent?
44. In the context of atomic structure, what does 'term symbol' represent?
45. What is the ground state electron configuration of Helium (He)?
46. According to the Pauli Exclusion Principle, no two electrons in an atom can have the same set of which quantum numbers?
47. The spin quantum number (ms) can have which values for an electron?
48. What does the magnetic quantum number (ml) specify for an electron in an atom?
49. The azimuthal quantum number (l) for a p orbital is:
50. Which quantum number describes the shape of an atomic orbital?