Section 30.5 The Quantum Mechanical Picture of the Hydrogen Atom

 26. According to the quantum mechanical picture of the atom, which one of the following is a true statement concerning the ground state electron in a hydrogen atom?

(a) The ground state electron has zero kinetic energy.

(b) The ground state electron has zero binding energy.

(c) The ground state electron has zero ionization energy.

(d) The ground state electron has zero spin angular momentum.

(e) The ground state electron has zero orbital angular momentum.

 27. A hydrogen atom is in a state for which the principle quantum number is n = 3. How many possible such states are there for which the magnetic quantum number is ?

(a) 2 (c) 6 (e) 10

(b) 4 (d) 8

 28. According to the quantum mechanical picture of the atom, which one of the following statements is true concerning the magnitude of the angular momentum L of an electron in the n = 3 level of the hydrogen atom?

(a) L is 0.318h. (d) L could be 0.225h or 0.276h.

(b) L is 0.477h. (e) L could be 0.225h or 0.390h.

(c) L could be 0.159h or 0.318h.

 29. An electron in a hydrogen atom is described by the quantum numbers: n = 8 and .

What are the possible values for the orbital quantum number ?

(a) only 0 or 4 (d) only 4, 5, 6, or 7

(b) only 4 or 7 (e) only 5, 6, 7, or 8

(c) only 5 or 8

 30. Which one of the following sets of quantum numbers is not possible?

n m_s

(a) 2 3 –2 +1/2

(b) 4 3 +2 +1/2

(c) 3 1 0 –1/2

(d) 6 2 –1 +1/2

(e) 5 4 –4 –1/2

 31. The principle quantum number for the electron in a hydrogen atom is n = 4. According to the quantum mechanical picture of the atom, what is the maximum possible value for the magnitude of the z-component of the angular momentum of the electron?

(a) 3.17  10^34 kg  m²/s (c) 1.99  10^34 kg  m²/s (e) 2.11  10^33 kg  m²/s

(b) 4.22  10^34 kg  m²/s (d) 1.06  10^34 kg  m²/s

 32. Which quantum number applies to most of the electrons in a collection of hydrogen atoms at room temperature?

(a) n = 1 (c) n = 3 (e) n = 5

(b) n = 2 (d) n = 4

 33. How many electron states (including spin states) are possible in a hydrogen atom if its energy is –3.4 eV?

(a) 2 (c) 6 (e) 10

(b) 4 (d) 8

 34. Determine the maximum number of electron states with principal quantum number n = 3?

(a) 2 (c) 6 (e) 18

(b) 3 (d) 9

 35. Which one of the following values of is not possible for = 2?

(a) zero (c) +1 (e) +3

(b) –1 (d) +2

 36. Two possible states for the hydrogen atom are labeled A and B. The maximum magnetic quantum number for state A is +3. For state B, the maximum value is +1. What is the ratio of the magnitudes of the orbital angular momenta, L_A/L_B, of an electron in these two states?

(a) 1.22 (c) 2.00 (e) 3.46

(b) 1.73 (d) 2.45

Section 30.6 The Pauli Exclusion Principle and the Periodic Table of the Elements

 37. To which model of atomic structure does the Pauli exclusion principle apply?

(a) the nuclear atom (d) the plum-pudding model

(b) the quantum mechanical atom (e) the planetary model

(c) the billiard ball atom

 38. Which one of the following factors best explains why the six electrons of a carbon atom are not all in the 1s state?

(a) electron spin (d) Heisenberg uncertainty principle

(b) Coulomb's law (e) Rutherford model of atomic structure

(c) Pauli exclusion principle

 39. Which one of the following statements concerning the electrons specified by the notation 3p⁴ is true?

(a) The electrons are in the M shell.

(b) The electrons are in the = 2 subshell.

(c) The electrons are necessarily in an excited state.

(d) They have principal quantum number 4.

(e) There are 3 electrons in the specified subshell.

 40. How many electrons could be accommodated in a g subshell?

(a) 4 (c) 8 (e) 18

(b) 5 (d) 9

 41. Which one of the following subshells is not compatible with a principle quantum number of n = 4?

(a) s (c) d (e) g

(b) p (d) f

 42. Which one of the following electronic configurations corresponds to an atomic ground state?

(a) 1s² 2s¹ 2p⁶ (c) 1s¹ 2s² 3p¹ (e) 1s¹ 2s² 2p¹

(b) 1s¹ 2s¹ 2p¹ (d) 1s² 2s² 2p¹

 43. An h subshell refers to orbital quantum number

(a) = 1 (c) = 3 (e) = 5

(b) = 2 (d) = 4

 44. What is the total number of subshells in the n = 3 level?

(a) 3 (c) 7 (e) 18

(b) 6 (d) 9

 45. Name the physicist credited with the following statement: No two electrons in an atom can have the same set of values for the four quantum numbers.

(a) Werner Heisenberg (c) Arthur Compton (e) Erwin Schrödinger

(b) Wolfgang Pauli (d) Niels Bohr

 46. The ground state electronic configuration of a neon atom is 1s² 2s² 2p⁶. How many of these electrons have magnetic quantum number m_l = 0?

(a) 2 (c) 6 (e) 10

(b) 4 (d) 8

Questions 47 through 49 pertain to the statement below:

A neutral atom has the following electronic configuration: 1s² 2s² 2p⁶ 3s² 3p⁵

 47. How many electrons are in the M shell?

(a) 2 (c) 6 (e) 8

(b) 5 (d) 7

 48. How many protons are in the atomic nucleus?

(a) 4 (c) 12 (e) 34

(b) 7 (d) 17

 49. To which group of the periodic table does this element belong?

(a) I (c) III (e) VII

(b) II (d) VI

Questions 50 through 52 pertain to the statement below:

An electron in an atom has the following set of quantum numbers:

n = 3, = 2, = +1, m_s = +1/2.

 50. What shell is this electron occupying?

(a) K shell (c) M shell (e) O shell

(b) L shell (d) N shell

 51. In which subshell can the electron be found?

(a) s (c) d (e) g

(b) p (d) f

 52. According to the quantum mechanical picture of the atom, which quantum number(s) could be different for electrons in this same atom that have exactly the same energy?

(a) n, , and m_s (c) only and (e) m_s

(b) only , and m_s (d) only and m_s

Questions 53 through 57 pertain to the statement below

Consider the following list of electron configurations:

(1) 1s² 2s² 3s² (4) 1s² 2s² 2p⁶ 3s² 3p⁶ 4s²

(2) 1s² 2s² 2p⁶ (5) 1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d⁶

(3) 1s² 2s² 2p⁶ 3s¹

 53. Which one of the above lists represents the electronic configuration for the ground state of the atom with Z = 11?

(a) 1 (c) 3 (e) 5

(b) 2 (d) 4

 54. Which electronic configuration is characteristic of noble gases?

(a) 1 (c) 3 (e) 5

(b) 2 (d) 4

 55. Which one of the above configurations represents a neutral atom that readily forms a singly charged positive ion?

(a) 1 (c) 3 (e) 5

(b) 2 (d) 4

 56. Which one of the above configurations represents an excited state of a neutral atom?

(a) 1 (c) 3 (e) 5

(b) 2 (d) 4

 57. Which one of the above configurations represents a transition element?

(a) 1 (c) 3 (e) 5

(b) 2 (d) 4