Q&A Hero

Q: What are the possible values of n and ml for an electron in a 4d orbital? A) n = 1, 2, 3, or 4 and ml = 2 B) n = 1, 2, 3, or 4 and ml = -2, -1, 0, +1, or +2 C) n = 4 and ml = 2 D) n = 4 and ml = -2, -1, 0, +1, or +2

Q: The work function of cesium metal is 188 kJ/mol. What is the minimum frequency of light needed to eject electrons from cesium? A) 4.71 Hz B) 5.54 1 Hz C) 1.09 Hz D) 1.13 Hz

Q: Which one of these spheres represents an atom of B?A) sphere (a)B) sphere (b)C) sphere (c)D) sphere (d)

Q: Which one of these spheres represents an atom of Li? A) sphere (a) B) sphere (b) C) sphere (c) D) sphere (d)

Q: Which one of these spheres represents an atom of F? A) sphere (a) B) sphere (b) C) sphere (c) D) sphere (d)

Q: The spheres below represent atoms of Li, Be, B, and F (not necessarily in that order).Which one of these spheres represents an atom of Be?A) sphere (a)B) sphere (b)C) sphere (c)D) sphere (d)

Q: Which one of these spheres represents an atom of As?A) sphere (a)B) sphere (b)C) sphere (c)D) sphere (d)

Q: Which one of these spheres represents an atom of N? A) sphere (a) B) sphere (b) C) sphere (c) D) sphere (d)

Q: Which one of these spheres represents an atom of P? A) sphere (a) B) sphere (b) C) sphere (c) D) sphere (d)

Q: The spheres below represent atoms of Sb, As, P, and N (not necessarily in that order).Which one of these spheres represents an atom of Sb?A) sphere (a)B) sphere (b)C) sphere (c)D) sphere (d)

Q: Atoms of which element, indicated by letter on the periodic table, have the orbital-filling diagram shown below?A) AB) BC) CD) D

Q: Atoms of which element, indicated by letter on the periodic table, have the orbital-filling diagram shown below? A) A B) B C) C D) D

Q: 2Atoms of which element, indicated by letter on the periodic table, have the orbital-filling diagram shown below? A) A B) B C) C D) D

Q: Which orbital-filling diagram represents the anomalous ground state of chromium? A) B) C) D)

Q: Which orbital-filling diagram represents the ground state of vanadium? A) B) C) D)

Q: Which orbital-filling diagram represents the ground state of oxygen? A) B) C) D)

Q: Which orbital-filling diagram violates Hund's rule? A) B) C) D)

Q: Which orbital-filling diagram violates the Pauli exclusion principle? A) B) C) D)

Q: Which grouping of elements, indicated by letter on the periodic table above, represents the s-block elements? A) A B) B C) C D) D

Q: Which grouping of elements, indicated by letter on the periodic table above, represents the p-block elements? A) A B) B C) C D) D

Q: Which grouping of elements, indicated by letter on the periodic table above, represents the d-block elements? A) A B) B C) C D) D

Q: Which grouping of elements, indicated by letter on the periodic table above, represents the f-block elements?A) AB) BC) CD) D

Q: Which groups of elements, indicated by letter on the periodic table, have two unpaired p electrons in their valence shell?A) A and BB) A and CC) B and CD) B and D

Q: Which group of elements, indicated by letter on the periodic table, has electrons with the ground-state valence-shell electron configuration ns2 np4? A) A B) B C) C D) D

Q: Which period of elements, indicated by letter on the periodic table, has electrons whose highest principal quantum number n is 5? A) A B) B C) C D) D

Q: Which element, indicated by letter on the periodic table above, has the ground-state electron configuration [Ar]4s2 3d2? A) A B) B C) C D) D

Q: Which element, indicated by letter on the periodic table above, contains one f electron?A) AB) BC) CD) D

Q: What is the ground-state valence-shell electron configuration of the group of elements indicated by the shaded portion of the periodic table?A) ns2B) ns2np2C) ns2(n-1)d2D) ns2(n-2)f2

Q: What is the ground-state valence-shell electron configuration of the group of elements indicated by the shaded portion of the periodic table? A) ns2 B) ns2np2 C) ns2(n-1)d2 D) ns2(n-2)f2

Q: What is the ground-state valence-shell electron configuration of the group of elements indicated by the shaded portion of the periodic table? A) ns2 B) ns2np2 C) ns2(n-1)d2 D) ns2(n-2)f2

Q: For the fourth-shell orbital shown below, what are the principal quantum number, n, and the angular momentum quantum number, l? A) n = 4 and l = 0 B) n = 4 and l = 1 C) n = 4 and l = 2 D) n = 4 and l = 3

Q: For the fourth-shell orbital shown below, what are the principal quantum number, n, and the angular momentum quantum number, l? A) n = 4 and l = 0 B) n = 4 and l = 1 C) n = 4 and l = 2 D) n = 4 and l = 3

Q: For the fourth-shell orbital shown below, what are the principal quantum number, n, and the angular momentum quantum number, l? A) n = 4 and l = 0 B) n = 4 and l = 1 C) n = 4 and l = 2 D) n = 4 and l = 3

Q: For the fourth-shell orbital shown below, what are the principal quantum number, n, and the angular momentum quantum number, l? A) n = 4 and l = 0 B) n = 4 and l = 1 C) n = 4 and l = 2 D) n = 4 and l = 3

Q: Which of the above fourth-shell orbitals is a 4dyz orbital? A) orbital (a) B) orbital (b) C) orbital (c) D) orbital (d)

Q: Which of the above fourth-shell orbitals is a 4dx2-y2 orbital? A) orbital (a) B) orbital (b) C) orbital (c) D) orbital (d)

Q: Which of the above fourth-shell orbitals is a 4py orbital? A) orbital (a) B) orbital (b) C) orbital (c) D) orbital (d)

Q: Which of the above fourth-shell orbitals is a 4pz orbital?A) orbital (a)B) orbital (b)C) orbital (c)D) orbital (d)

Q: If wave (a) represents green light, wave (b) might representA) blue light.B) red light.C) ultraviolet radiation.D) X-rays.

Q: Wave (b) has the A) higher amplitude and greater intensity than wave (a). B) higher amplitude and weaker intensity than wave (a). C) lower amplitude and greater intensity than wave (a). D) lower amplitude and weaker intensity than wave (a).

Q: Wave (b) has the A) higher frequency and higher energy than wave (a). B) higher frequency and lower energy than wave (a). C) lower frequency and higher energy than wave (a). D) lower frequency and lower energy than wave (a).

Q: Wave (a) has the A) longer wavelength and higher frequency than wave (b). B) longer wavelength and lower frequency than wave (b). C) shorter wavelength and higher frequency than wave (b). D) shorter wavelength and lower frequency than wave (b).

Q: Two electromagnetic waves are represented below.Wave (a) has theA) longer wavelength and higher energy than wave (b).B) longer wavelength and lower energy than wave (b).C) shorter wavelength and higher energy than wave (b).D) shorter wavelength and lower energy than wave (b).

Q: Which atom in each group (I and II) has the smallest atomic radius?(I) Sr, Zr, I (II) N, P, AsA) Sr; NB) Sr; AsC) I; ND) I; As

Q: Of the following, which atom has the smallest atomic radius? A) Mg B) S C) Sr D) Te

Q: Of the following, which atom has the largest atomic radius? A) Na B) Cl C) K D) Br

Q: A neutral sulfur atom has how many valence electrons? A) 2 B) 4 C) 6 D) 16

Q: The element In has how many valence electrons? A) 1 B) 2 C) 3 D) 13

Q: Which of the following have the same number of valence electrons? A) K, As, Br B) B, Si, As C) N, As, Bi D) He, Ne, F

Q: Which of the following have their valence electrons in the same shell? A) K, As, Br B) B, Si, As C) N, As, Bi D) He, Ne, F

Q: List all the elements that have a ground-state configuration with five unpaired electrons in the 3d subshell. A) Mn, Fe, Co, Cu, and Zn B) Cr and Mn C) Cr D) Mn

Q: Which have the largest number of unpaired electrons in p orbitals in their ground-state electron configurations? A) N, P, As B) F, Cl, Br C) Ne, Ar, Kr D) Te, I, Xe

Q: How many unpaired electrons are in an atom of Co in its ground state? A) 1 B) 2 C) 3 D) 7

Q: Which element has the ground-state electron configuration [Xe]6s245d1? A) Pt B) Eu C) Gd D) Tb

Q: What is the ground-state electron configuration of tellurium? A) [Kr]54d105p4 B) [Kr]5s25p65d8 C) [Kr]5s25p4 D) [Kr]4f144d105s25p4

Q: What is the ground-state electron configuration of Co? A) [Ar]3d9 B) [Ar]4s13d8 C) [Ar]4s23d7 D) [Ar]4s24p64d1

Q: What is the general valence-electron ground-state electron configuration for neutral alkaline earth metals? A) ns1 B) ns2 C) 1s22s1 D) 1s22s2

Q: Molybdenum has an anomalous electron configuration. Using the shorthand notation for electron configurations, write the electron configuration of Mo. A) [Kr] 5s0 4d6 B) [Kr] 5s0 4d0 5p6 C) [Kr] 5s1 4d5 D) [Kr] 5s2 4d4

Q: Which of the following elements would you predict to have an anomalous electron configuration? A) Ag B) Ce C) Se D) Sr

Q: Which of the following represent electron configurations that are allowed but do not represent ground-state configurations? (A) [Ne]3s13p5 (B) [Kr]4d125s25p3 (C) [Ar]43d104p2 A) only (A) B) only (B) C) (A) and (B) D) (B) and (C)

Q: The symbol [Kr] represents A) 4s24p6. B) 1s22s22p63s23p64s24p6. C) 1s22s22p63s23p643d104p6. D) 1s22s22p63s23p63d104p64d10.

Q: Which has the highest Zeff for its valence electrons? A) Na B) K C) Si D) P

Q: For a multielectron atom, a 3s orbital lies lower in energy than a 3p orbital because A) a 3p orbital has more nodal surfaces than a 3s orbital. B) other electrons more effectively shield electrons in the 3s orbital from the nucleus. C) other electrons more effectively shield electrons in the 3p orbital from the nucleus. D) there are more p orbitals than s orbitals in a given shell.

Q: Within a given shell of a multielectron atom, the lower l for an orbital, the A) higher the orbital energy and the higher Zeff for the electron. B) higher the orbital energy and the lower Zeff for the electron. C) lower the orbital energy and the higher Zeff for the electron. D) lower the orbital energy and the lower Zeff for the electron.

Q: Which of the following statements is true for energy level differences seen when comparing the s,p,d, and f orbitals in the hydrogen atom for a given value of n? A) There are no differences in energy between the s,p,d, and f orbitals. B) There are different values of quantum number l for each orbital which cause differences in energy. C) There are different values of quantum number for each orbital which cause differences in energy. D) There are different values of quantum number for each orbital which cause differences in energy.

Q: For a multielectron atom the energy differences between the s,p,d,and f orbitals is due to A) electron-electron repulsions. B) the different values of quantum number l for each orbital. C) the different values of quantum number for each orbital. D) the different values of quantum number for each orbital.

Q: Which statement is false? A) For any atom, the 4s orbital lies lower in energy than the 5s orbital. B) For a hydrogen atom, a 4s orbital, a 4p orbital, and a 4d orbital all have the same energy. C) The 4s orbital lies lower in energy than the 3d orbital for atoms K, Ca, Sc, and Ti. D) The 4s orbital lies lower in energy than the 3d orbital for Cu and Fe2+.

Q: Which of the following represent electron configurations that violate the Pauli exclusion principle? (A) [Ne]3s13p5 (B) [Kr]4d125s25p3 (C) [Ar]3d104s24p2 A) only (A) B) only (B) C) (A) and (B) D) (B) and (C)

Q: The first vibrational level for NaH lies at 1.154 10-20 J and the second vibrational level lies at What is the frequency of the photon emitted when a molecule of NaH drops from the second vibrational level to the first vibrational level? A) 1.742 1013 Hz B) 3.399 1013 Hz C) 5.140 1013 Hz D) 6.882 1013 Hz

Q: The absorption of a photon of wavelength 4.67 10-6 m is necessary for a CO molecule to pass from the lowest vibrational energy level to the next highest vibrational level. If this higher vibrational level has an energy of what is the energy of the lowest vibrational level? h = 6.626 10-34 J sA) 1.60 10-20 JB) 2.15 10-20 JC) 3.20 10-20 JD) 4.26 10-20 J

Q: The absorption of light of frequency 1.16 1011 Hz is required for CO molecules to go from the lowest rotational energy level to the next highest rotational energy level. Determine the energy for this transition in kJ/mol. h = 6.626 10-34 J s A) 7.69 10-23 kJ/mol B) 0.0463 kJ/mol C) 46.3 kJ/mol D) 949 kJ/mol

Q: Molecular vibrational energy transitions are observed in the infrared, molecular rotational transitions in the microwave, and electronic transitions in the ultraviolet-visible range. Which transitions require the most energy and which the least energy? A) Electronic transitions require the least energy and vibrational transitions the most. B) Rotational transitions require the least energy and electronic transitions the most. C) Vibrational transitions require the least energy and electronic transitions the most. D) Vibrational transitions require the least energy and rotational transitions the most.

Q: For hydrogen, what is the wavelength of the photon emitted when an electron drops from a 4d orbital to a 2p orbital in a hydrogen atom? The Rydberg constant is 1.097 10-2 nm-1. A) 656.3 nm B) 486.2 nm C) 364.6 nm D) 2.057 10-3 nm

Q: What is the first ionization energy for a hydrogen atom in the ground state? The Rydberg constant is A) 7.27 10-36 J B) 1.63 10-27 J C) 2.18 10-18 J D) 0.00823 J

Q: The Balmer-Rydberg equation can be extended to ions with only one electron, such as He+. In that case it has the form: where Z is the atomic number. What is the energy of the photon required to promote an electron in He+ from a 1s orbital to a 2p orbital? A) (3/4)hcR B) 3hcR C) 4hcR D) 12hcR

Q: For a hydrogen atom, which electronic transition would result in the emission of a photon with the highest energy?A) 2s -> 3pB) 3p -> 6dC) 4p -> 2sD) 5f -> 3d

Q: Which of the following is true? The probability density A) for all s orbitals is independent of direction from the nucleus. B) for all s orbitals is independent of distance from the nucleus. C) is independent of direction from the nucleus for 1s orbitals only. D) is independent of distance from the nucleus for 1s orbitals only.

Q: For a particular orbital, as one goes away from the nucleus along the z-axis, the probability density decreases to zero, then increases, and finally decreases without increasing a second time. This is consistent with a A) 2s orbital. B) 2pz orbital. C) 2s or a 2pz orbital. D) 3s orbital.

Q: For an orbital, a node is A) the midpoint of the orbital. B) a surface inside which there is a 90% chance of finding the electron. C) a surface where there is a maximum probability of finding the electron. D) a surface where there is no chance of finding the electron.

Q: What is the number of spherical nodes in a 4s orbital? A) zero B) two C) three D) four