TEMA 4: Electronic Spectroscopy

1. 1Why do we use electronic spectroscopy?

   1. AWe want to get information about the rotational and vibrational states.
   2. BWe want to get information about the rotational and electronic states.
   3. CWe want to get information about the electronic and vibrational states.
   4. DWe want to get information about the electronic structure and molecular information in some cases.
2. 2Electronic Spectroscopy shows up at the ultraviolet and visible regions of the electromagnetic spectrum (10.000-100.000cm-1).

   1. ATrue
   2. BFalse
3. 3The bands registered correspond to transitions between ro-vibrational energy levels.

   1. ATrue
   2. BFalse
4. 4Electronic Spectroscopy allows us to get information from atoms that are neither active in RAMAN nor IR.

   1. ATrue
   2. BFalse
5. 5When a transition takes place, there are noticeable changes in both vibrational and rotational states.

   1. ATrue
   2. BFalse
6. 6Regarding the electronic states in polielectronic atoms, we have to assume that...

   1. AElectrons keep occupying individual spin-orbitals, with effective nuclear charges (due to shielding )
   2. BElectrons keep occupying individual spin-orbitals, without effective nuclear charges (due to shielding )
7. 7Electronic states are obtained directly from...

   1. Athe electronic Schrödinger equation.
   2. Bfrom the eigen values of the Shrödinger equation derivative with respect the time.
8. 8The electronic structure is expressed through...

   1. Adiagrams of electronic states.
   2. Ba list of unoccupied orbitals.
   3. Cits electronic configuration.
9. 92s and 2p are both examples of subshells, while 1s is a shell.

   1. ATrue
   2. BFalse
10. 10Z*(2s)=Z*(2p)

    1. ATrue
    2. BFalse

11. 11For electronic configurations with a full subshell there are plenty of ways to place the electrons.

    1. ATrue
    2. BFalse
12. 12In the case of C, there is more than one way to place the electrons, because the subshell is not full.

    1. ATrue
    2. BFalse
13. 13If we pack 2 electrons in the same orbital, there'll be less repulsion rather than packing them in separated orbitals.

    1. ATrue
    2. BFalse
14. 14If we didn't take into consideration the repulsion between electrons, states would have the same energy.

    1. ATrue
    2. BFalse
15. 15States or microestates are defined by its Ms, ML and Mn value.

    1. ATrue
    2. BFalse
16. 16Which are the values of n,l and ml of the following state?
    Take into consideration that we are studying the ground state configuration of C.

    

    1. An=2, l=1, ml= -1,0,1
       n=2, l=0, ml= 0
       n=2, l=0, ml= -1,0,1
    2. Bn=2, l=1, ml= -2,0,1
       n=1, l=0, ml= 0
       n=2, l=1, ml= -1,0,1
    3. Cn=2, l=1, ml= -1,0,1
       n=2, l=0, ml= 0
       n=1, l=0, ml= 0
    4. Dn=2, l=1, ml= -1,0,1
       n=1, l=0, ml= 0
       n=2, l=1, ml= -1,0,1
17. 17We use this formula in order to calculate...

    

    1. Athe number of occupied orbitals.
    2. Bthe number of states associated to a particular electronic configuration.
    3. CThe number of states associated to all possible electronic configurations.
18. 18ML and MS are the result of the summatory of every ms and ml.

    1. ATrue
    2. BFalse
19. 19The configuration: (2s)1 (2p)1 has 14 states.

    1. ATrue
    2. BFalse
20. 20In atomic spectroscopy, in order to know the relative order of the energy of the different states, we should determine the S atomic term.

    1. ATrue
    2. BFalse
21. 21The states that belong to different spectral terms have different energy since...

    1. Athe magnitude of the intraelectronic repulsion is equal for each term.
    2. Bthe magnitude of the dipole moment is different for each term.
    3. Cthe magnitude of the interelectronic repulsion is different for each term.
22. 22An atomic term contains (2S+1)(2L+2) microstates.

    1. ATrue
    2. BFalse
23. 23Configurations with closed subshells contains spin-paired electrons, which means that there is a unique microstate.

    1. ATrue
    2. BFalse
24. 24Configurations with open subshells, where electrons are not equivalents, the exclusion principle does apply.

    1. ATrue
    2. BFalse
25. 25To determine atomic termis in configurations with open subshells, values of L and S goes from:
    L=[l1+l2] to [l1-l2]
    S=[s1+s2] to [s1-s2]

    1. ATrue
    2. BFalse
26. 26In open subshells, equivalent electrons (same subshell) has a unique microstate.

    1. ATrue
    2. BFalse
27. 27Considering the configuration: 2p1 3p1, we could...

    1. Ahave a spectral term with L=2.
    2. Bnot have a spectral term with L=2
28. 283D spectral term has...

    1. A10 states.
    2. B5 states.
    3. C9 states.
    4. D15 states.
29. 29If we sum all the states that com from the atomic terms of a certain configuration, we will obtain the total number of states of that electronic configuration.

    1. ATrue
    2. BFalse
30. 30We have more microstates in non-equivalent electrons open shells rather than in equivalent open shells.

    1. ATrue
    2. BFalse
31. 31When we build tables of Ms and Ml, what we are trying to do is find all the possible states of the configuration, and then gather them in the different atomic terms.

    1. ATrue
    2. BFalse
32. 32All the states inside an atomic termal are degenerated in regards the energy.

    1. ATrue
    2. BFalse
33. 33From these atomic terms, the most stable on is...
    1S, 3P, 1D

    1. A1S
    2. B3P
    3. C1D
34. 34Regarding the selection rules in order to have allowed transitions AS=0 and AL=0,1.

    1. ATrue
    2. BFalse
35. 35Regarding Hund's Empirical Rule, if there is more than one term with the largest S, then the term with the largest S and the lowest L is more stable.

    1. ATrue
    2. BFalse
36. 36(GREEN SLIDES) Spin-orbit Interaction arises because of the dynamic moment caused by the orbital motion around the nucleus, and the dynamic moment caused by the spin angular moment.

    1. ATrue
    2. BFalse
37. 37(GREEN SLIDES) The spin-orbit interaction denpds on the total angular momentum of the electron J .

    1. ATrue
    2. BFalse
38. 38(GREEN SLIDES) It is acceptable to compute the total angular momentum (J) by summing the total electronic angular momentum (L) and the total spin angular momentum (S) when the Spin-Orbit interaction is small.

    1. ATrue
    2. BFalse
39. 39(GREEN SLIDES) Values of J go from the sum to the [rest] (els corxets indica valor absolut) of L and S values. 2J+1 are the states in a certain level, corresponding to the possible values of Mj.

    1. ATrue
    2. BFalse
40. 40(GREEN SLIDES)
    3P has 3 spin-orbit interaction energy levels, which are 3P2 (5 states), 3P1(3 states) and 3P0(1 state. )

    1. ATrue
    2. BFalse
41. 41(GREEN SLIDES) The State is a sum of H^º + H^repulsion + H^spin-orbit + H^B.

    1. ATrue
    2. BFalse
42. 42The selection rules for the allowed transitions have to accomplish: AS=0, AL=-1,0,1 ,AJ=-1,0,1 ,AMj=-1,0,1. There is 2 exceptions: Transition J= 0 --> 0 / Transition Mj= 0-->0 if AJ=0
    

    1. ATrue
    2. BFalse
43. 43For diatomic molecules with little Z, it is not necessary to apply the Born-Oppenheimer approximation.

    1. ATrue
    2. BFalse
44. 44The Slater Determinant is ...

    1. Aan antisimetrized product of molecular orbitals.
    2. Ba simetrized product of molecular orbitals.
    3. Can antisimetrized sum of molecular orbitals.
    4. Da simetrized sum of molecular orbitals.
45. 45We use the Slater Determinant in order to accomplish the antisymmetry principle.

    1. ATrue
    2. BFalse
46. 46We could say that a HOMO-LUMO transition is an electronic transition because one electron is shifted from one occupied to a virtual one.

    1. ATrue
    2. BFalse
47. 47(GREEN SLIDES) Atomic structures build upon the hydrogenoid atom (energies and orbitals) while diatomics rely on the only solvable molecule within Born-Oppenheimer (H2).

    1. ATrue
    2. BFalse
48. 48(GREEN SLIDES) In monoatomic molecules, the orbitals are named with greek letter (sigma, pi, delta), while in diatomic the orbitals are named with s,p,d,f.

    1. ATrue
    2. BFalse
49. 49(GREEN SLIDES) In diatomic molecules, states are eigenfunctions of the Hamiltonian and Lz, not L^2.

    1. ATrue
    2. BFalse
50. 50(GREEN SLIDES)
    -m: quantizes the angular momentum component on the internuclear axis .
    -landa: equals the number of nodal planes that contain the internuclear axis.

    1. ATrue
    2. BFalse
51. 51An homonuclear molecule would have a "D infinit h" symmetry group, and it has an inversion center, so there are gerade and ungerade orbitals.

    1. ATrue
    2. BFalse
52. 52Heteronuclear diatomic molecules would have a symmetry group of "C infinit H".

    1. ATrue
    2. BFalse
53. 53(GREEN SLIDES) Spectral terms are actually the same as atomic terms but L=^ and these are named with capital greek letters.

    1. ATrue
    2. BFalse
54. 54(GREEN SLIDES) As well as in monoatomic molecules, in diatomic molecules, the closed shells have only one possible microstate (1SIGMAg), while in open shells you can do the table and get the spectral terms that contain different microstates.

    1. ATrue
    2. BFalse
55. 55(GREEN SLIDES) Transitions allowed selection rules are the same for both di and monoatomic molecules, in exception that in diatomic we have as well the transition g-->u.

    1. ATrue
    2. BFalse
56. 56All transitions between vibrational states are allowed, there's no selection rule governing the vibrational and rotational part of the transition.

    1. ATrue
    2. BFalse
57. 570<--0 and 1<--1 would be examples of progressions .
    0<--0 and 1<--0 would be examples of sequences.

    1. ATrue
    2. BFalse
58. 58The intensity depends on two factors: the transition dipole moment and the population of vibrational levels.

    1. ATrue
    2. BFalse
59. 59The Dipole moment has both nuclear and electronic contribution.

    1. ATrue
    2. BFalse
60. 60Molecular wavefunction has one component: the electronic one.

    1. ATrue
    2. BFalse

Description

Quiz on TEMA 4: Electronic Spectroscopy, created by Montse Montané Garcia on 17/06/2018.

Author

Montse Montané Garcia

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