The document discusses atomic physics concepts including quantum numbers, electron configurations, energy levels, and selection rules. It contains 25 multiple choice questions about these topics, covering hydrogen and lithium ion energy levels, electron spin and orbital angular momentum, and x-ray emission. It also contains conceptual problems about photon emission, electron excitation of hydrogen atoms, and filling of atomic subshells.
The document discusses atomic physics concepts including quantum numbers, electron configurations, energy levels, and selection rules. It contains 25 multiple choice questions about these topics, covering hydrogen and lithium ion energy levels, electron spin and orbital angular momentum, and x-ray emission. It also contains conceptual problems about photon emission, electron excitation of hydrogen atoms, and filling of atomic subshells.
The document discusses atomic physics concepts including quantum numbers, electron configurations, energy levels, and selection rules. It contains 25 multiple choice questions about these topics, covering hydrogen and lithium ion energy levels, electron spin and orbital angular momentum, and x-ray emission. It also contains conceptual problems about photon emission, electron excitation of hydrogen atoms, and filling of atomic subshells.
The document discusses atomic physics concepts including quantum numbers, electron configurations, energy levels, and selection rules. It contains 25 multiple choice questions about these topics, covering hydrogen and lithium ion energy levels, electron spin and orbital angular momentum, and x-ray emission. It also contains conceptual problems about photon emission, electron excitation of hydrogen atoms, and filling of atomic subshells.
1. One of the main problems with the Bohr model of the hydrogen atom when compared with the results of the methods of quantum mechanics used to describe atoms, was that the Bohr model predicted
a . the ground state angular momentum was L = 1 h.
b. the frequency of the radiation emitted when an electron "jumps" from one allowed orbit to another was hf = Ei - Ef. c. the potential energy function for the hydrogen atom was given by V(r) = –ke2/r. d. the energy of the ground state of the hydrogen atom was En = –13.6 eV.
2. The allowed values of n for the Li2+ ion are
a. 1 to ∞ b. 2 to ∞ c. 3 to ∞ d. any real number e. 1 to 10
3. The allowed values of l for a Li2+ ion in the n = 3 shell is
a. 1, 2 b. 0, 1 c. 0, 1, 2 d. 0, 1, 2, 3 e. 1, 2, 3
4. The allowed values of ml for a Li2+ ion are
a. –l to l b. –(l + 1) to (l + l) c. –(l + 2) to (l + 2) d. –(l + 3) to (l + 3) e. 0 to n – 1
5. The permitted values of ml for n = 3 are
a. –1, 0, 1 b. 2, 1, 0 c. 2, 1, 0, –1, –2 d. 0 e. 3, 2, 1, 0, –1, –2, –3
a. n-quantum numbers b. l-quantum numbers c. ml-quantum numbers d. ms-quantum numbers e. mj-quantum numbers
7. The s, p, d, f, symbols correspond to
a. ms-quantum numbers b. n-quantum numbers c. ml-quantum numbers d. l-quantum numbers e. mj-quantum numbers
8. The number of states in the He+ ion corresponding to the principle quantum number n = 5 are
a. 18 b. 25 c. 50 d. 9 e. 11
9. The energy needed to remove an electron from the first excited state of a Li2+ ion is
a. 53 eV b. 31 eV c. 92 eV d. 122 eV e. 61 eV
10. Of the following states, 5s, 3p, 4f, 5p, 4g, 3d, and 2p, the one which is NOT allowed is
a. 3p b. 4f c. 3d d. 4g e. 2p
11. For the following allowed transitions, which photon would have the largest wavelength when an electron "jumps" from one energy level, characterized by the quantum number n, to another?
a. n = 2 to n = 1 b. n = 3 to n = 2 c. n = 3 to n = 1 d. n = 1 to n = 3
12. The energy needed to change a He+ ion into a He2+ ion is
a. 13.6 eV b. 54.4 eV c. 112.4 eV d. 92.9 eV
13. A Li2+ ion undergoes a transition from the n = 4 to the n = 3 state. The energy of the emitted photon is
a. 4.5 eV b. 10.2 eV c. 5.95 eV d. 2.6 eV e. 0.66 eV
14. The probability density for the 1 s state is given by |Ψ1s|2. The probability of finding the particle is
a. ⌠ ⌡|Ψ1s|2 4πr2dr
b. ⌠|Ψ1s|2 dr ⌡
c. ⌠ ⌡|Ψ1s|2 r dr
d. ⌠ ⌡|Ψ1s|2 r2dr
e. ⌠ ⌡|Ψ1s|2 r3dr
15. If P(r) is the radial probability density function for an electron in the ground state of a hydrogen atom, the most probable value for r can be found from
a . dP/dt b. dP/dr
c. ⌠ rP(r)4πr2 dr ⌡
d. ⌠ ⌡ rP(r)dr e. d2P/dr2
16. The radial portion of the de Broglie wavefunction for an electron in the ground state of the hydrogen atom is Ψ 1s(r) = 1/(πa03)1/2 exp(–r/a0) where a0 is the Bohr radius. The probability of finding the electron is
17. The probability density of a particle at a distance r from the nucleus is essentially the
a. probability of finding the particle.
b. probability per unit area of finding the particle. c. probability per unit length of finding the particle. d. probability per unit volume of finding the particle. 2 e. ⌠ ⌡0Ψ 2 4π r2dr s
18. Of the following states of the hydrogen atom, 1s, 2p, 3d, 4f, 4s, which ones are not spherically symmetrical?
a. 1s, 4s b. 3d, 4f c. 2p, 3d, 4f d. 2p, 3d, 4f, 4s
19. A hydrogen atom in the 4f state has a total angular momentum (in terms of h) of magnitude
a. 2 3 b. 3 c. 6 d. 3 e. 12
20. Which of the following statements is true?
a. L can never be perpendicular to B.
b. L can be aligned parallel to B. c. L must be perpendicular to B. d. L can never be aligned parallel to B.
21. In 1921, Stern and Gerlach performed an experiment that first demonstrated
a. orbital angular momentum quantization
b. energy quantization c. space quantization d. magnetic orbital quantization e. that particles behave like waves
22. The magnitude of the spin angular momentum for an electron is equal to
23. When using the Pauli Exclusion Principle, we assume the particle's spin angular momentum is of magnitude
a . 1/2 h b. 3 /2 h c. h d. ±h e. –1/2 h
24. What angle does the orbital angular momentum make with the z axis of a hydrogen atom in the state n = 3, l = 2, ml = –1?
a. –66° b. 66° c. 24° d. 114° e. 73°
25. The total angular momentum for a 3P3/2 electron is
a . ( 15 /2) h b. ( 3 /2) h c. (3/2) h d. 3h e. 3 h
26. The Pauli Exclusion Principle states
a . No two electrons can have the same set of quantum numbers.
b. There is an inherent uncertainty in the position and momentum of a particle. c. When an atom has orbitals of equal energy, the maximum number of electrons will have unpaired spins. d. When an atom has orbitals of equal energy, the maximum number of electrons will be paired spins.
27. Forbidden transitions and selection rules suggest that
a. a photon has linear momentum.
b. a photon has energy. c. a photon has angular momentum. d. a photon has parity. e. a photon has mass.
28. Characteristic x-rays can be produced by bombarding targets with electrons. These x-rays occur when
a. electrons from higher shells fill the vacant lower shell
b. electrons fill the vacant valence shell c. photons are emitted with energies on the order of 103 eV d. photons are emitted with wavelengths on the order of 103 nm
29. Suppose a beam of electrons is incident on a collection of hydrogen atoms, all of which are in the lowest energy state (n = 1). What is the minimum energy the electrons can have if they are to excite the hydrogen atoms into the n = 2 state?
30. The energy difference between the upper and lower levels in a certain laser is 1.9593 eV. What is the wavelength of the light emitted by the laser?
31. A hydrogen atom emits a photon of wavelength 657.7 nm. From what energy state to what lower energy state did the electron jump?
32. The ground state configuration of chlorine (Z = 17) is
a. 1s2 2s2 2p5 3s2 3p6
b. 1s2 2s2 2p6 3s2 3p5 c. 1s2 2s2 2p6 3s2 3p4 3d1 d. 1s2 2s2 2p6 3s2 3p5 4s1 e. 1s2 2s2 2p6 3s1 3p7
33. Rubidium (Z = 37) and potassium (Z = 19) are similar to sodium in that they have
a. five p b. three p c. two s d. one d e. one s
electron(s) in the outermost shell.
34. When electrons fill a subshell in which the orbitals have equal energy, the order in which the orbitals are filled is such that
a. a minimum number of electrons has unpaired spins.
b. a minimum number of electrons has intrinsic angular momentum. c. a maximum number of electrons has unpaired spins. d. a maximum number of electrons first fills the next energy level. e. the maximum number of electrons has the same set of quantum numbers.
35. In a completely filled atomic shell,
a. the intrinsic spin of the electrons does not produce a resultant magnetic moment. b. the orbital motion of the electrons does not produce a resultant magnetic moment. c. the electrons do not contribute to paramagnetic or ferromagnetic effects. d. all of the above are correct. e. none of the above are correct.
