Atomic Theory and Structure Atomic Theory IV: _{Quantum numbers and orbitals} by Adrian Dingle, B.Sc., Anthony Carpi, Ph.D. Reading Quiz Teach with this The Heisenberg Uncertainty Principle considers which properties of the electron? Its position and momentum Only its position Only its momentum The reduced Planck constant The position of an electron in an atom at any given time can be precisely known. true false Given the following table of data, which of the following is a permissible set of the quantum numbers n, l, m, and s? (Note: though not shown in the table, s can equal -½ or +½.) n = 0, l = 0, m = 0, s = +½ n = 1, l = 1, m = 0, s = +½ n = 1, l = 0, m = 1, s = +½ n = 1, l = 0, m = 0, s = +½ How many d orbitals are there in a d-subshell of any given atom? 1 3 5 7 When considering the Aufbau process of filling electron orbitals, which of the following sets of quantum numbers for n, l, m, and s are feasible in order for the final electron to enter a nitrogen atom? (A nitrogen atom has 7 electrons.) n = 1, l = 0, m = 0, and s = +½ n = 1, l = 1, m = 0, and s = +½ n = 2, l = 0, m = 0, and s = +½ n = 2, l = 1, m = 1, and s = +½ Which of the following represents a set of degenerate orbitals? 1s, 2s, and 3s 2p_{x}, 2p_{y}, and 2p_{z} 3s and 3p 3s, 3p, and 3d Keeping in mind Hund’s rule, how many occupied orbitals, and how many unpaired electrons, are expected in an atom of oxygen (atomic number 8) in the ground state? Occupied orbitals = 4; unpaired electrons = 0 Occupied orbitals = 3; unpaired electrons = 2 Occupied orbitals = 5; unpaired electrons = 2 Occupied orbitals = 5; unpaired electrons = 0 When the absorption spectrum of hydrogen atoms in their ground state is examined, the only lines that are observed are in the Lyman series (not the Balmer, Paschen or Pfund series). Which of the following is the best explanation for this observation? There is only one electron in a hydrogen atom. An electron in a hydrogen atom can only fall back to n = 1. When hydrogen atoms absorb energy, the electrons fall to the n = 1 level. In the ground state, hydrogen’s single electron always has n = 1. Which of the following hydrogen atom electronic transitions would release the greatest amount of energy? From n = 1 to n = 2 From n = 2 to n = 3 From n = 3 to n = 2 From n = 6 to n = 5 Which of the following electronic configurations represents an excited state of neon (atomic number 10)? 1s^{2} 2s^{2} 2p^{5} 3s^{1} 1s^{2} 2s^{2} 2p^{5} 1s^{2} 2s^{2} 2p^{6} 1s^{2} 2s^{2} 2p^{6} 3s^{1} Score Quiz