Chemistry, 11e Chapter 6: Electronic Structure of Atoms Testbank

1) Electromagnetic radiation travels through vacuum at a speed of __________ m/s. A) 186,000 B) 125 C) 3.00 10ﾴ 8 D) 10,000 E) It depends on wavelength. Answer: C Diff: 1 Page Ref: Sec. 6.1 2) The wavelength of light that has a frequency of 1.20 10ﾴ 13 1s- is __________ m. A) 25.0 B) 2.50 10ﾴ -5 C) 0.0400 D) 12.0 E) 2.5 Answer: B Diff: 1 Page Ref: Sec. 6.1 3) Ham radio operators often broadcast on the 6-meter band. The frequency of this electromagnetic radiation is __________ MHz. A) 500 B) 200 C) 50 D) 20 E) 2.0 Answer: C Diff: 1 Page Ref: Sec. 6.1 4) What is the frequency (s-1) of electromagnetic radiation that has a wavelength of 0.53 m? A) 5.7ﾴ 108 B) 1.8 10ﾴ -9 C) 1.6 10ﾴ 8 D) 1.3 10ﾴ -33 E) 1.3 10ﾴ 33 Answer: A Diff: 1 Page Ref: Sec. 6.1 5) The energy of a photon of light is __________ proportional to its frequency and __________ proportional to its wavelength. A) directly, directly B) inversely, inversely C) inversely, directly D) directly, inversely E) indirectly, not Answer: D Diff: 1 Page Ref: Sec. 6.1 6) Of the following, __________ radiation has the shortest wavelength. A) X-ray B) radio C) microwave D) ultraviolet E) infrared Answer: A Diff: 1 Page Ref: Sec. 6.1 7) What is the frequency of light ( s-1) that has a wavelength of 1.23 10ﾴ -6cm ? A) 3.69 B) 2.44 10ﾴ 16 C) 4.10 10ﾴ -17 D) 9.62 10ﾴ 12 E) 1.04 10ﾴ -13 Answer: B Diff: 1 Page Ref: Sec. 6.1 8) What is the frequency of light ( s-1) that has a wavelength of 3.12×10-13cm ? A) 3.69 B) 2.44 10ﾴ 16 C) 9.62 10ﾴ 12 D) 4.10 10ﾴ -17 E) 1.04 10ﾴ -13 Answer: C Diff: 1 Page Ref: Sec. 6.1

9) What is the wavelength of light (nm) that has a frequency of3.22 10ﾴ 14 1s- ? A) 932 B) 649 C) 9.66 10ﾴ 22 D) 9.32 10ﾴ -7 E) 1.07 10ﾴ 6 Answer: A Diff: 1 Page Ref: Sec. 6.1 10) What is the wavelength of light (nm) that has a frequency 4.62 10ﾴ 14 1s- ? A) 932 B) 649 C) 1.39 10ﾴ 23 D) 1.54 10ﾴ -3 E) 1.07 10ﾴ 6 Answer: B Diff: 1 Page Ref: Sec. 6.1 11) The wavelength of a photon that has an energy of 5.25 10ﾴ -19J is __________ m. A) 3.79 10ﾴ -7 B) 2.64 10ﾴ 6 C) 2.38 10ﾴ 23 D) 4.21 10ﾴ -24 E) 3.79 10ﾴ 7 Answer: A Diff: 2 Page Ref: Sec. 6.2 12) The energy of a photon that has a wavelength of 9.0 m is __________ J. A) 2.2 10ﾴ -26 B) 4.5 10ﾴ 25 C) 6.0 10ﾴ -23 D) 2.7 10ﾴ 9 E) 4.5 10ﾴ -25 Answer: A Diff: 2 Page Ref: Sec. 6.2

13) The frequency of a photon that has an energy of 3.7 10ﾴ -18J is __________s-1. A) 5.6 10ﾴ 15 B) 1.8 10ﾴ -16 C) 2.5 10ﾴ -15 D) 5.4 10ﾴ -8 E) 2.5 10ﾴ 15 Answer: A Diff: 2 Page Ref: Sec. 6.2 14) The energy of a photon that has a wavelength of 12.3 nm is __________ J. A) 1.51 10ﾴ -17 B) 4.42 10ﾴ -23 C) 1.99 10ﾴ -25 D) 2.72 10ﾴ -50 E) 1.62 10ﾴ -17 Answer: E Diff: 2 Page Ref: Sec. 6.2 15) The energy of a photon that has a wavelength of 13.2 nm is __________ J. A) 9.55 10ﾴ -25 B) 1.62 10ﾴ -17 C) 1.99 10ﾴ -25 D) 4.42 10ﾴ -23 E) 1.51 10ﾴ -17 Answer: E Diff: 2 Page Ref: Sec. 6.2 16) The energy of a photon that has a frequency of 8.21 10ﾴ 15 1s- is __________ J. A) 8.08 10ﾴ -50 B) 1.99 10ﾴ -25 C) 5.44 10ﾴ -18 D) 1.24 10ﾴ 49 E) 1.26 10ﾴ -19 Answer: C Diff: 2 Page Ref: Sec. 6.2 17) The energy of a photon that has a frequency of 1.821 10ﾴ 16 1s- is __________ J. A) 5.44 10ﾴ -18 B) 1.99 10ﾴ -25 C) 3.49 10ﾴ -48 D) 1.21 10ﾴ -17 E) 5.44 10ﾴ -18 Answer: D Diff: 2 Page Ref: Sec. 6.2 18) What is the frequency (s-1) of a photon that has an energy of4.38 10ﾴ -18J ? A) 436 B) 6.61 10ﾴ 15 C) 1.45 10ﾴ -16 D) 2.30 10ﾴ 7 E) 1.31 10ﾴ -9 Answer: B Diff: 2 Page Ref: Sec. 6.2 19) What is the wavelength (angstroms) of a photon that has an energy of 4.38 10ﾴ -18 J? A) 454 B) 2.30 10ﾴ 7 C) 6.89 10ﾴ 15 D) 1.45 10ﾴ -16 E) 1.31 10ﾴ -9 Answer: A Diff: 2 Page Ref: Sec. 6.2 20) A mole of red photons of wavelength 725 nm has __________ kJ of energy. A) 2.74 10ﾴ -19 B) 4.56 10ﾴ -46 C) 6.05 10ﾴ -3 D) 165 E) 227 Answer: D Diff: 3 Page Ref: Sec. 6.2 21) A mole of yellow photons of wavelength 527 nm has __________ kJ of energy. A) 165 B) 227 C) 4.56 10ﾴ -46 D) 6.05 10ﾴ -3 E) 2.74 10ﾴ -19 Answer: B Diff: 3 Page Ref: Sec. 6.2 22) It takes 254 kJ/mol to eject electrons from a certain metal surface. What is the longest wavelength of light (nm) that can be used to eject electrons from the surface of this metal via the photoelectric effect? A) 471 B) 233 C) 165 D) 725 E) 552 Answer: A Diff: 3 Page Ref: Sec. 6.2

23) Of the following, __________ radiation has the longest wavelength and __________ radiation has the greatest energy. gamma ultraviolet visible A) ultraviolet, gamma B) visible, ultraviolet C) gamma, gamma D) visible, gamma E) gamma, visible Answer: D Diff: 1 Page Ref: Sec. 6.2 24) What color of visible light has the longest wavelength? A) blue B) violet C) red D) yellow E) green Answer: C Diff: 1 Page Ref: Sec. 6.2 25) Of the following, __________ radiation has the shortest wavelength and __________ radiation has the greatest energy. gamma ultraviolet visible A) gamma, visible B) visible, gamma C) visible, ultraviolet D) ultraviolet, gamma E) gamma, gamma Answer: E Diff: 1 Page Ref: Sec. 6.2 26) What color of visible light has the highest energy? A) violet B) blue C) red D) green E) yellow Answer: A Diff: 1 Page Ref: Sec. 6.2 27) Which one of the following is considered to be ionizing radiation? A) visible light B) radio waves C) X-rays D) microwaves E) infrared radiation Answer: C Diff: 1 Page Ref: Sec. 6.2 28) Of the following transitions in the Bohr hydrogen atom, the __________ transition results in the emission of the highest-energy photon. A) n = 1 → n = 6 B) n = 6 → n = 1 C) n = 6 → n = 3 D) n = 3 → n = 6 E) n = 1 → n = 4 Answer: B Diff: 1 Page Ref: Sec. 6.3 29) Using Bohr's equation for the energy levels of the electron in the hydrogen atom, determine the energy (J) of an electron in the n = 4 level. A) -1.36 10ﾴ -19 B) -5.45 10ﾴ -19 C)-7.34 10ﾴ 18 D) -1.84 10ﾴ -29 E) +1.84 10ﾴ -29 Answer: A Diff: 1 Page Ref: Sec. 6.3 30) An electron in a Bohr hydrogen atom has an energy of -1.362 10ﾴ -19J The value of n for this electron is __________. A) 1 B) 2 C) 3 D) 4 E) 5 Answer: D Diff: 1 Page Ref: Sec. 6.3 31) The energy (J) required for an electronic transition in a Bohr hydrogen atom from n = 2 to n = 3 is __________ J. A) 4.00 10ﾴ -19 B) 3.00 10ﾴ -19 C) -3.00 10ﾴ -19 D) -7.90 10ﾴ -19 E) 4.60 10ﾴ 14 Answer: B Diff: 1 Page Ref: Sec. 6.3 32) Calculate the energy (J) change associated with an electron transition from n = 2 to n = 5 in a Bohr hydrogen atom. A) 6.5 10ﾴ -19 B) 5.5 10ﾴ -19 C) 8.7 10ﾴ -20 D) 4.6 10ﾴ -19 E) 5.8 10ﾴ -53 Answer: D Diff: 1 Page Ref: Sec. 6.3 33) The frequency of electromagnetic radiation required to promote an electron from n = 2 to n = 4 in a Bohr hydrogen atom is __________ Hz. A) 4.13 10ﾴ -19 B) 6.17 10ﾴ 14 C) 5.46 10ﾴ -19 D) 8.22 10ﾴ 14 E) 4.13 10ﾴ 19 Answer: B Diff: 1 Page Ref: Sec. 6.3 34) A spectrum containing only specific wavelengths is called a __________ spectrum. A) line B) continuous C) visible D) Rydberg E) invariant Answer: A Diff: 1 Page Ref: Sec. 6.3

35) When the electron in a hydrogen atom moves from n = 6 to n = 2, light with a wavelength of __________ nm is emitted. A) 93.8 B) 434 C) 487 D) 657 E) 410 Answer: E Diff: 1 Page Ref: Sec. 6.3 36) When the electron in a hydrogen atom moves from n = 6 to n = 1, light with a wavelength of __________ nm is emitted. A) 487 B) 411 C) 434 D) 93.8 E) 657 Answer: D Diff: 2 Page Ref: Sec. 6.3 37) When the electron in a hydrogen atom moves from n = 8 to n = 2 light with a wavelength of __________ nm is emitted. A) 657 B) 93.8 C) 411 D) 487 E) 389 Answer: E Diff: 2 Page Ref: Sec. 6.3 38) The n = 2 to n = 6 transition in the Bohr hydrogen atom corresponds to the __________ of a photon with a wavelength of __________ nm. A) emission, 410 B) absorption, 410 C) absorption, 660 D) emission, 94 E) emission, 390 Answer: B Diff: 2 Page Ref: Sec. 6.3 39) The n = 5 to n = 3 transition in the Bohr hydrogen atom corresponds to the __________ of a photon with a wavelength of __________ nm. A) absorption, 657 B) absorption, 1280 C) emission, 657 D) emission, 1280 E) emission, 389 Answer: D Diff: 2 Page Ref: Sec. 6.3 40) The n = 8 to n = 4 transition in the Bohr hydrogen atom occurs in the __________ region of the electromagnetic spectrum. A) infrared B) visible C) ultraviolet D) microwave E) X-ray Answer: A Diff: 2 Page Ref: Sec. 6.3 41) The n = 8 to n = 2 transition in the Bohr hydrogen atom occurs in the __________ region of the electromagnetic spectrum. A) radio B) X-ray C) infrared D) microwave E) ultraviolet Answer: E Diff: 2 Page Ref: Sec. 6.4 42) The deBroglie wavelength of a particle is given by __________. A) h + mv B) hmv C) h/mv D) mv/c E) mv Answer: C Diff: 1 Page Ref: Sec. 6.4 43) What is the de Broglie wavelength (m) of a 2.0 kg object moving at a speed of 50 m/s? A) 6.6 10ﾴ -36 B) 1.5 10ﾴ 35 C) 5.3 10ﾴ -33 D) 2.6 10ﾴ -35 E) 3.8 10ﾴ 34 Answer: A Diff: 1 Page Ref: Sec. 6.4

44) What is the de Broglie wavelength (m) of a 25 g object moving at a speed of 5.0 m/s? A) 1.9 10ﾴ 32 B) 5.3 10ﾴ -33 C) 6.6 10ﾴ -36 D) 3.32 10ﾴ -36 E) 3.02 10ﾴ 45 Answer: B Diff: 1 Page Ref: Sec. 6.4 45) At what speed (m/s) must a 10.0 mg object be moving to have a de Broglie wavelength of 3.3 10ﾴ -41m ? A) 4.1 B) 1.9 10ﾴ -11 C) 2.0 10ﾴ 12 D) 3.3 10ﾴ -42 E) 9.1 10ﾴ 31 Answer: C Diff: 1 Page Ref: Sec. 6.4 46) At what speed (m/s) must a 3.0 mg object be moving in order to have a de Broglie wavelength of 5.4 10ﾴ -29 m? A) 1.6 10ﾴ -28 B) 3.9 10ﾴ -4 C) 2.0 10ﾴ 12 D) 4.1 E) 6.3 Answer: D Diff: 1 Page Ref: Sec. 6.4 47) The de Broglie wavelength of an electron is 8.7 10ﾴ -11m . The mass of an electron is 9.1 10ﾴ -31kg . The velocity of this electron is __________ m/s. A) 8.4 10ﾴ 3 B) 1.2 10ﾴ -7 C) 6.9 10ﾴ -5 D) 8.4 10ﾴ 6 E) 8.4 10ﾴ -3 Answer: D Diff: 1 Page Ref: Sec. 6.4 48) The de Broglie wavelength of a bullet (7.5 g) traveling at 700 m/s is __________ m. A) 7.7 10ﾴ 33 B) 1.3 10ﾴ -34 C) 6.2 10ﾴ -29 D) 1.3 10ﾴ -27 E) 1.3 10ﾴ -23 Answer: B Diff: 1 Page Ref: Sec. 6.4 49) The de Broglie wavelength of a car (1.0 10 kg)ﾴ 3 traveling at 75 km/hr is __________ m. A) 3.2 10ﾴ -38 B) 8.8 10ﾴ -39 C) 3.2 10ﾴ -35 D) 1.4 10ﾴ -35 E) 1.4 10ﾴ 35 Answer: A Diff: 1 Page Ref: Sec. 6.4 50) The wavelength of an electron whose velocity is 1.7 10ﾴ 4m/s and whose mass is 9.1 10ﾴ -28g is __________ m. A) 4.3 10ﾴ -11 B) 12 C) 4.3 10ﾴ -8 D) 2.3 10ﾴ 7 E) 2.3 10ﾴ -7 Answer: C Diff: 1 Page Ref: Sec. 6.4 51) The __________ quantum number defines the shape of an orbital. A)spin B) magnetic C) principal D) magnetic E) phi Answer: D Diff: 1 Page Ref: Sec. 6.5 52) There are __________ orbitals in the third shell. A) 25 B) 4 C) 9 D) 16 E) 1 Answer: C Diff: 1 Page Ref: Sec. 6.5 53) The __________ subshell contains only one orbital. A) 5d B) 6f C) 4s D) 3d E) 1p Answer: C Diff: 1 Page Ref: Sec. 6.5 54) There are __________ orbitals in the second shell. A) 1 B) 2 C) 4 D) 8 E) 9 Answer: C Diff: 1 Page Ref: Sec. 6.5 55) The azimuthal quantum number is 3 in __________ orbitals. A) s B) p C) d D) f E) a Answer: D Diff: 2 Page Ref: Sec. 6.5 56) The n = 1 shell contains __________ p orbitals. All the other shells contain __________ p orbitals. A) 3, 6 B) 0, 3 C) 6, 2 D) 3, 3 E) 0, 6 Answer: B Diff: 1 Page Ref: Sec. 6.5 57) The lowest energy shell that contains f orbitals is the shell with n = __________. A) 3 B) 2 C) 4 D) 1 E) 5 Answer: C Diff: 1 Page Ref: Sec. 6.5

58) The principal quantum number of the first d subshell is __________. A) 1 B) 2 C) 3 D) 4 E) 0 Answer: C Diff: 1 Page Ref: Sec. 6.5 59) The total number of orbitals in a shell is given by __________. A) I2 B) n2 C) 2n D) 2n +1 E) 2l+1 Answer: B Diff: 1 Page Ref: Sec. 6.5 60) In a hydrogen atom, an electron in a __________ orbital can absorb a photon, but cannot emit a photon. A) 3s B) 2s C) 3p D) 1s E) 3f Answer: D Diff: 1 Page Ref: Sec. 6.5 61) __________-orbitals are spherically symmetrical. A) s B) p C) d D) f E) g Answer: A Diff: 1 Page Ref: Sec. 6.6 62) How many p-orbitals are occupied in a Ne atom? A) 5 B) 6 C) 1 D) 3 E) 2 Answer: E Diff: 1 Page Ref: Sec. 6.7 63) Each p-subshell can accommodate a maximum of __________ electrons. A) 6 B) 2 C) 10 D) 3 E) 5 Answer: A Diff: 1 Page Ref: Sec. 6.7 64) How many quantum numbers are necessary to designate a particular electron in an atom? A) 3 B) 4 C) 2 D) 1 E) 5 Answer: B Diff: 1 Page Ref: Sec. 6.7 65) A __________ orbital is degenerate with a 5dz2 in a many-electron atom. A) 5pz B) 4dz2 C) 5s D) 5dxy E) 4dzz Answer: D Diff: 2 Page Ref: Sec. 6.8 66) The 3p subshell in the ground state of atomic xenon contains __________ electrons. A) 2 B) 6 C) 8 D) 10 E) 36 Answer: B Diff: 1 Page Ref: Sec. 6.8 67) The second shell in the ground state of atomic argon contains __________ electrons. A) 2 B) 6 C) 8 D) 18 E) 36 Answer: C Diff: 1 Page Ref: Sec. 6.8 68) The 4d subshell in the ground state of atomic xenon contains __________ electrons. A) 2 B) 6 C) 8 D) 10 E) 36 Answer: D Diff: 1 Page Ref: Sec. 6.8 69) [Ar]4s 3d 4p2 10 3 is the electron configuration of a(n) __________ atom. A) As B) V C) P D) Sb E) Sn Answer: A Diff: 3 Page Ref: Sec. 6.8 70) There are __________ unpaired electrons in a ground state phosphorus atom. A) 0 B) 1 C) 2 D) 3 E) 4 Answer: D Diff: 1 Page Ref: Sec. 6.8

71) There are __________ unpaired electrons in a ground state fluorine atom. A) 0 B) 1 C) 2 D) 3 E) 4 Answer: B Diff: 1 Page Ref: Sec. 6.8 72) In a ground-state manganese atoms, the __________ subshell is partially filled. A) 3s B) 4s C) 4p D) 3d E) 4d Answer: D Diff: 1 Page Ref: Sec. 6.8 73) The principal quantum number for the outermost electrons in a Br atom in the ground state is __________. A) 2 B) 3 C) 4 D) 5 E) 1 Answer: C Diff: 2 Page Ref: Sec. 6.8 74) The azimuthal quantum number for the outermost electrons in a nitrogen atom in the ground state is __________. A) 0 B) 1 C) 2 D) 3 E) -1 Answer: B Diff: 3 Page Ref: Sec. 6.8 75) The electron configuration of a ground-state Ag atom is __________. A) [Ar]4s 4d2 9 B) [Kr]5s 4d1 10 C) [Kr]5s 3d2 9 D) [Ar]4s 4d1 10 E) [Kr]5s 4d2 10 Answer: B Diff: 2 Page Ref: Sec. 6.9 76) The ground state electron configuration for Zn is __________. A) [Kr]4s 3d2 10 B) [Ar]4s 3d2 10 C) [Ar]4s 3d1 10 D) [Ar]3s 3d2 10 E) [Kr]3s 3d2 10 Answer: B Diff: 1 Page Ref: Sec. 6.9 77) Which is the correct ground-state electron configuration for silver? A) [Kr]5s 4d2 9 B) [Kr]5s 4d1 10 C) [Kr]5s 4d2 10 D) [Xe]5s 4d2 9 E) [Xe]5s 4d1 10 Answer: B Diff: 2 Page Ref: Sec. 6.9 78) What is the correct ground-state electron configuration for molybdenum? A) [Kr]5s 4d1 10 B) [Kr]5s 4d2 4 C) [Kr]5s 4d1 5 D) [Kr]5s 4d2 9 E) [Kr]5s 4d2 9 Answer: C Diff: 2 Page Ref: Sec. 6.9 79) All of the __________ have a valence shell electron configuration ns1. A) noble gases B) halogens C) chalcogens D) alkali metals E) alkaline earth metals Answer: D Diff: 1 Page Ref: Sec. 6.9

80) The elements in the __________ period of the periodic table have a core-electron configuration that is the same as the electron configuration of neon. A) first B) second C) third D) fourth E) fifth Answer: C Diff: 2 Page Ref: Sec. 6.9 81) The largest principal quantum number in the ground state electron configuration of iodine is __________. A) 1 B) 4 C) 5 D) 6 E) 7 Answer: C Diff: 1 Page Ref: Sec. 6.9 82) The largest principal quantum number in the ground state electron configuration of barium is __________. A) 1 B) 2 C) 4 D) 5 E) 6 Answer: E Diff: 1 Page Ref: Sec. 6.9 83) The largest principal quantum number in the ground state electron configuration of cobalt is __________. A) 2 B) 3 C) 4 D) 7 E) 9 Answer: C Diff: 1 Page Ref: Sec. 6.9 84) Elements in group __________ have a np6 electron configuration in the outer shell. A) 4A B) 6A C) 7A D) 8A E) 5A Answer: D Diff: 1 Page Ref: Sec. 6.9

85) Which group in the periodic table contains elements with the valence electron configuration of ns np2 1? A) 1A B) 2A C) 3A D) 4A E) 8A Answer: C Diff: 1 Page Ref: Sec. 6.9 6.2 Multiple-Choice Questions 1) Which one of the following is correct? A) ν + =λ c B) ν ﾴ =λ c C) ν =cλ D) λ =cν E) νλ =c Answer: E Diff: 1 Page Ref: Sec. 6.1 2) The photoelectric effect is __________. A) the total reflection of light by metals giving them their typical luster B) the production of current by silicon solar cells when exposed to sunlight C) the ejection of electrons by a metal when struck with light of sufficient energy D) the darkening of photographic film when exposed to an electric field E) a relativistic effect Answer: C Diff: 1 Page Ref: Sec. 6.2 3) Low-frequency electromagnetic fields with potential biological effects have frequencies of __________ Hz. A) 10 - 10-3 -5 B) 10 - 10-5 -9 C) 100-10,000 D) 400-700 E) 1-1000 Answer: E Diff: 1 Page Ref: Sec. 6.2 4) The wavelength of light emitted from a traffic light having a frequency of 5.75 10ﾴ 14Hz is _________. A) 702 nm B) 641 nm C) 674 nm D) 521 nm E) 583 nm Answer: D Diff: 1 Page Ref: Sec. 6.2 5) A radio station broadcasts at 103.5 MHz . The wavelength of the signal is __________ m. A) 3.10 B) 2.90 C) 4.71 D) 2.75 E) 3.84 Answer: B Diff: 1 Page Ref: Sec. 6.2 6) In the Bohr model of the atom, __________. A) electrons travel in circular paths called orbitals B) electrons can have any energy C) electron energies are quantized D) electron paths are controlled by probability E) both A and C Answer: C Diff: 1 Page Ref: Sec. 6.3 7) The de Broglie wavelength of a 6.0 gram bullet traveling at the speed of sound is _________. The speed of sound is 331 m/sec. A) 2.7 10ﾴ -34 m B) 3.3 10ﾴ -34m C) 3.35 10ﾴ -33m D) 2.7 10ﾴ -37m E) 6.6 10ﾴ -31m Answer: B Diff: 1 Page Ref: Sec. 6.4

8) According to the Heisenberg Uncertainty Principle, it is impossible to know precisely both the position and the __________ of an electron. A) mass B) color C) momentum D) shape E) charge Answer: C Diff: 1 Page Ref: Sec. 6.4 9) The de Broglie wavelength of a __________ will have the shortest wavelength when traveling at 30 cm/s. A) marble B) car C) planet D) uranium atom E) hydrogen atom Answer: C Diff: 1 Page Ref: Sec. 6.4 10) The uncertainty principle states that __________. A) matter and energy are really the same thing B) it is impossible to know anything with certainty C) it is impossible to know the exact position and momentum of an electron D) there can only be one uncertain digit in a reported number E) it is impossible to know how many electrons there are in an atom Answer: C Diff: 1 Page Ref: Sec. 6.5 11) All of the orbitals in a given electron shell have the same value of the __________ quantum number. A) principal B) azimuthal C) magnetic D) spin E) psi Answer: A Diff: 1 Page Ref: Sec. 6.5 12) All of the orbitals in a given subshell have the same value of the __________ quantum number. A) principal B) azimuthal C) magnetic D) A and B E) B and C Answer: D Diff: 1 Page Ref: Sec. 6.5

19) Which one of the following is an incorrect orbital notation? A) 2s B) 3py C) 3f D) 4dxy E) 4s Answer: C Diff: 1 Page Ref: Sec. 6.5 20) Which quantum number determines the energy of an electron in a hydrogen atom? A) n B) E C) ml D) l E) n and l Answer: A Diff: 2 Page Ref: Sec. 6.5 21) Which one of the quantum numbers does not result from the solution of the Schrodinger equation? A) principal B) azimuthal C) magnetic D) spin E) angular momentum Answer: D Diff: 1 Page Ref: Sec. 6.5, 6.7 22) Which quantum numbers must be the same for the orbitals that they designate to be degenerate in a one-electron system (such as hydrogen)? A) n, l, and ml B) n and l only C) l and ml D) ml only E) n only Answer: E Diff: 1 Page Ref: Sec. 6.6 23) In a px orbital, the subscript x denotes the __________ of the electron. A) energy B) spin of the electrons C) probability of the shell D) size of the orbital E) axis along which the orbital is aligned Answer: E Diff: 1 Page Ref: Sec. 6.6 24) The __________ orbital is degenerate with 5py in a many-electron atom. A) 5s B) 5px C) 4py D) 5dxy E) 5d2 Answer: B Diff: 1 Page Ref: Sec. 6.6 25) Which set of three quantum numbers (n, l, ml) corresponds to a 3d orbital? A) 3, 2, 2 B) 3, 3, 2 C) 3, 2, 3 D) 2, 1, 0 E) 2, 3, 3 Answer: A Diff: 1 Page Ref: Sec. 6.6

26) At maximum, an f-subshell can hold __________ electrons, a d-subshell can hold __________ electrons, and a p-subshell can hold __________ electrons. A) 14, 10, 6 B) 2, 8, 18 C) 14, 8, 2 D) 2, 12, 21 E) 2, 6, 10 Answer: A Diff: 2 Page Ref: Sec. 6.7 27) If an electron has a principal quantum number (n) of 3 and an azimuthal quantum number (l) of 2, the subshell designation is _________. A) 3p B) 3d C) 4s D) 4p E) 4d Answer: B Diff: 1 Page Ref: Sec. 6.7 28) Which one of the following represents an acceptable set of quantum numbers for an electron in an atom? (arranged as n, l, ml, and ms) A) 2, 2, -1, -1/2 B) 1, 0, 0, 1/2 C) 3, 3, 3, 1/2 D) 5, 4,- 5, 1/2 E) 3, 3, 3, -1/2 Answer: B Diff: 1 Page Ref: Sec. 6.7 29) Which one of the following represents an acceptable possible set of quantum numbers (in the order n, l, ml, and ms) for an electron in an atom? A) 2, 1, -1, 1/2 B) 2, 1, 0, 0 C) 2, 2, 0, 1/2 D) 2, 0, 1, -1/2 E) 2, 0, 2, +1/2 Answer: A Diff: 1 Page Ref: Sec. 6.7 30) Which one of the following orbitals can hold two electrons? A) 2px B) 3s C) 4dxy D) all of the above E) none of the above Answer: D Diff: 1 Page Ref: Sec. 6.7 31) Which quantum numbers must be the same for the orbitals that they designate to be degenerate in a many-electron system? A) n, l, and ml B) n only C) n, l, ml,and ms D) ms only E) n and l only Answer: E Diff: 2 Page Ref: Sec. 6.7 32) Which one of the following represents an impossible set of quantum numbers for an electron in an atom? (arranged as n, l, ml, and ms) A) 2, 1, -1, -1/2 B) 1, 0, 0, 1/2 C) 3, 3, 3, 1/2 D) 5, 4, - 3, 1/2 E) 5, 4, -3, -1/2 Answer: C Diff: 1 Page Ref: Sec. 6.7 33) Which of the following is not a valid set of four quantum numbers? (n, l, ml, ms ) A) 2, 0, 0, +1/2 B) 2, 1, 0, -1/2 C) 3, 1, -1, -1/2 D) 1, 0, 0, +1/2 E) 1, 1, 0, +1/2 Answer: E Diff: 2 Page Ref: Sec. 6.7 34) Which of the following is a valid set of four quantum numbers?(n, l, ml, ms) A) 2, 1, 0, +1/2 B) 2, 2, 1, -1/2 C) 1, 0, 1, +1/2 D) 2, 1, +2, +1/2 E) 1, 1, 0, -1/2 Answer: A Diff: 2 Page Ref: Sec. 6.7

A) B) C) D) E) Answer: C Diff: 1 Page Ref: Sec. 6.8 A) B) C) D) E) Answer: B Diff: 1 Page Ref: Sec. 6.8 A) B) C) D) E) Answer: C Diff: 1 Page Ref: Sec. 6.8

38) Which one of the following is the correct electron configuration for a ground-state nitrogen atom? A) B) C) D) E) None of the above is correct. Answer: D Diff: 1 Page Ref: Sec. 6.8 39) Which electron configuration denotes an atom in its ground state? A) B) C) D) E) Answer: D Diff: 1 Page Ref: Sec. 6.8 40) The ground state electron configuration of Fe is __________. A) 1s 2s 3s 3p 3d2 2 2 6 6 B) 1s 2s 2p 3s 3p 3d 4s2 2 6 2 6 6 2 C) 1s 2s 2p 3s 3p 4s2 2 6 2 6 2 D) 1s 2s 2p 3s 3p 4s 4d2 2 6 2 6 2 6 E) 1s 2s 3s 3p2 2 2 10 Answer: B Diff: 1 Page Ref: Sec. 6.8 41) The ground state electron configuration of Ga is __________. A) 1s 2s 3s 3p 3d 4s 4p2 2 2 6 10 2 1 B) 1s 2s 2p 3s 3p 4s 4d 4p2 2 6 2 6 2 10 1 C) 1s 2s 2p 3s 3p 3d 4s 4p2 2 6 2 6 10 2 1 D) 1s 2s 2p 3s 3p 3d 4s 4d2 2 6 2 6 10 2 1 E) [ Ar 4s 3d] 2 11 Answer: C Diff: 1 Page Ref: Sec. 6.8 42) The ground-state electron configuration of the element __________ is [kr]5s 4d1 5 . A) Nb B) Mo C) Cr D) Mn E) Tc Answer: B Diff: 1 Page Ref: Sec. 6.8 43) The ground-state electron configuration of __________ is [Ar]4s 3d1 5 A) V B) Mn C) Fe D) Cr E) K Answer: D Diff: 1 Page Ref: Sec. 6.8 44) Which one of the following configurations depicts an excited oxygen atom? A) 1s 2s 2p2 2 2 B) 1s 2s 2p 3s2 2 2 2 C) 1s 2s 2p2 2 1 D) 1s 2s 2p2 2 4 E) [ He 2s 2p] 2 4 Answer: B Diff: 2 Page Ref: Sec. 6.8 45) Which one of the following configurations depicts an excited carbon atom? A) 1s 2s 2p 3s2 2 1 1 B) 1s 2s 2p2 2 3 C) 1s 2s 2p2 2 1 D) 1s 2s 3s2 2 1 E) 1s 2s 2p2 2 2 Answer: A Diff: 1 Page Ref: Sec. 6.8

A) B) C) D) E) Answer: C Diff: 1 Page Ref: Sec. 6.8 A) B) C) D) E) Answer: B Diff: 1 Page Ref: Sec. 6.8 A) B) C) D) E) Answer: D Diff: 1 Page Ref: Sec. 6.8 49) The ground state configuration of fluorine is __________. A) [He]2s22p2 B) [He]2s22p3 C) [He]2s22p4 D) [He]2s22p5 E) [He]2s22p6 Answer: D Diff: 2 Page Ref: Sec. 6.8

50) The ground state configuration of tungsten is __________.

A) [Ar]4s23d3

B) [Xe]6s24f145d4

C) [Ne]3s1

D) [Xe]6s24f7

E) [Kr]5s24d105p5

Answer: B

Diff: 2

Page Ref: Sec. 6.8

51) The lowest orbital energy is reached when the number of electrons with the same spin is maximized. This statement describes __________.

A) Pauli Exclusion Principle

B) Planck's constant

C) deBroglie hypothesis

D) Heisenberg Uncertainty Principle

E) Hund's rule

Answer: E

Diff: 3

Page Ref: Sec. 6.8

52) The element that has a valence configuration of 4s1 is _________.

A) Li

B) Na

C) K

D) Rb

E) Cs

Answer: C

Diff: 2

Page Ref: Sec. 6.8

53) Which of the following elements has a ground-state electron configuration different from the predicted one?

A) Cu

B) Ca

C) Xe

D) Cl

E) Ti

Answer: A

Diff: 2

Page Ref: Sec. 6.8

54) Which two elements have the same ground-state electron configuration?

A) Pd and Pt

B) Cu and Ag

C) Fe and Cu

D) Cl and Ar

E) No two elements have the same ground-state electron configuration.

Answer: E

Diff: 1

Page Ref: Sec. 6.8

55) How many different principal quantum numbers can be found in the ground state electron configuration of nickel?

A) 2

B) 3

C) 4

D) 5

E) 6

Answer: C

Diff: 1

Page Ref: Sec. 6.9

56) The valence shell of the element X contains 2 electrons in a 5s subshell. Below that shell, element X has a partially filled 4d subshell. What type of element is X?

A) main group element

B) chalcogen

C) halogen

D) transition metal

E) alkali metal

Answer: D

Diff: 1

Page Ref: Sec. 6.9

6.3 Short Answer Questions

1) What wavelengths correspond to the visible region of the electromagnetic spectrum?

Answer: About 400 to 700 nm.

Diff: 1

Page Ref: Sec. 6.1

2) In the deBroglie formula describing the movement of an electron about the nucleus, the quantity "mv" is called its __________.

Answer: momentum

Diff: 2

Page Ref: Sec. 6.2

3) A spectrum containing radiation of specific wavelengths is called a __________.

Answer: line spectrum

Diff: 2

Page Ref: Sec. 6.3

4) The shape of an orbital is defined by the azimuthal quantum number which is represented as letter __________

Answer: l

Diff: 1

Page Ref: Sec. 6.5

5) All of the subshells in a given shell have the same energy in the hydrogen atom. In a many-electron atom, the subshells in a given shell do not have the same energy. Why?

Answer: Hydrogen atoms have only one electron. Therefore, in a hydrogen atom, the energy of orbitals depends only on n. In many-electron atoms, electron-electron repulsion causes the energies of subshells in a given shell to differ.

Diff: 1

Page Ref: Sec. 6.7

6) The largest principal quantum number in the ground state electron configuration of francium is __________.

Answer: 7

Diff: 1

Page Ref: Sec. 6.8

7) The ground state electron configuration of scandium is __________.

Answer: [Ar]4s 3d2 1

Diff: 1

Page Ref: Sec. 6.8

8) The electron configuration of the valence electrons of an atom in its ground state isns np2 3 . This atom is a group __________ element.

Answer: 5A

Diff: 1

Page Ref: Sec. 6.8

9) Elements in group __________ have a np5 electron configuration in the outer shell.

Answer: 7A

Diff: 1

Page Ref: Sec. 6.8

10) The ground state electron configuration of copper is __________.

Answer: [Ar]3d 4s 10 1

Diff: 2

Page Ref: Sec. 6.9

6.4 True/False Questions

1) The wavelength of radio waves can be longer than a football field. Answer: True

Diff: 1

Page Ref: Sec. 6.1

2) Black body radiation is the emission of light from metal surfaces. Answer: False

Diff: 1

Page Ref: Sec. 6.2

3) If a hydrogen atom electron jumps from the n=6 orbit to the n=2 orbit, energy is released. Answer: True

Diff: 1

Page Ref: Sec. 6.3

4) The square of Schrodinger's wave equation is called an orbital. Answer: True

Diff: 1

Page Ref: Sec. 6.4

5) The electron density of the 2s orbital is asymmetric. Answer: False

Diff: 1

Page Ref: Sec. 6.5

6) The larger the principal quantum number of an orbital, the lower is the energy of the electrons in that orbital. Answer: False

Diff: 2

Page Ref: Sec. 6.7

7) When the value of n is greater than or equal to 3, electrons can reside in d orbitals. Answer: True

Diff: 2

Page Ref: Sec. 6.7

8) An NMR spectrum results from photon irradiation in which the nuclear spin alignmentis flipped. Answer: True

Diff: 3

Page Ref: Sec. 6.8

6.5 Algorithmic Questions

1) Electromagnetic radiation with a wavelength of 525 nm appears as green light to the human eye. The frequency of this light is __________s-1.

A) 5.71 10ﾴ 14

B) 5.71 10ﾴ 5

C) 1.58 10ﾴ 2

D) 1.58 10ﾴ 11

E) 1.75 10ﾴ -15

Answer: A

Diff: 1

Page Ref: Sec. 6.1

2) An FM radio station broadcasts electromagnetic radiation at a frequency of 100.6 MHz. The wavelength of this radiation is __________ m.

A) 2.982 10ﾴ 6

B) 2.982

C) 3.018 10ﾴ 16

D) 3.018 10ﾴ 10

E) 0.3353

Answer: B

Diff: 1

Page Ref: Sec. 6.1

3) Electromagnetic radiation with a wavelength of 525 nm appears as green light to the human eye. The energy of one photon of this light is __________ J.

A) 1.04 10ﾴ -31

B) 3.79 10ﾴ -28

C) 3.79 10ﾴ -19

D) 1.04 10ﾴ -22

E) 2.64 10ﾴ 18

Answer: C

Diff: 2

Page Ref: Sec. 6.2

4) Electromagnetic radiation with a wavelength of 531 nm appears as green light to the human eye. The energy of one photon of this light is 3.74 10ﾴ -19J Thus, a laser that emits

1.3 10ﾴ -2J of energy in a pulse of light at this wavelength produces __________ photons in each pulse.

A) 2.9 10ﾴ -17

B) 9.2 10ﾴ -24

C) 1.8 10ﾴ 19

D) 3.5 10ﾴ 16

E) 6.5 10ﾴ 13

Answer: D

Diff: 1

Page Ref: Sec. 6.2

5) The de Broglie wavelength of an electron with a velocity of 6.00 10ﾴ 6m/s is __________ m. The mass of the electron is 9.11 10ﾴ -28g

A) 8.25 10ﾴ 9

B) 8.25 10ﾴ 12

C) 1.21 10ﾴ -16

D) 1.21 10ﾴ -13

E) 1.21 10ﾴ -10

Answer: E

Diff: 2

Page Ref: Sec. 6.4

6) The element that corresponds to the electron configuration 1s 2s 2p2 2 6 is __________.

A) sodium

B) magnesium

C) lithium

D) beryllium

E) neon

Answer: E

Diff: 1

Page Ref: Sec. 6.8

7) The complete electron configuration of argon, element 18, is __________.

A) 1s 2s 2p 3s 3p2 2 6 2 6

B) 1s 2s 2p 3s 3p2 2 10 2 2

C) 1s 2s 2p 3s4 4 6 4

D) 1s 2s 2p4 4 10

E) 1s 2s 2p 3s6 6 2 4

Answer: A

Diff: 1

Page Ref: Sec. 6.8

8) The complete electron configuration of gallium, element 31, is __________.

A) 1s 2s 2p 3s 3p 4s 3d2 2 10 2 10 2 3

B) 1s 2s 2p 3s 3p 3d 4s 4P2 2 6 2 6 10 2 1

C) 1s 2s 2p 3s 3p 4s 3d4 4 6 4 6 4 3

D) 1s 2s 2p 3s 3p4 4 10 4 9

E) 1s 2s 2p 3s 3p 4s4 4 8 4 8 3

Answer: B

Diff: 1

Page Ref: Sec. 6.8

9) The condensed electron configuration of silicon, element 14, is __________.

A) [ He 2s 2p] 4 6

B) [ Ne 2p] 10

C) [ Ne 3s 3p] 2 2

D) [ He 2s] 4

E) [ He 2s 2p] 6 2

Answer: C

Diff: 1

Page Ref: Sec. 6.8

10) The condensed electron configuration of krypton, element 36, is __________.

A) [ Kr 4s 3d] 2 8

B) [ Ar 4s] 4

C) [ Kr 4s 3d] 4 8

D) [ Ar 3d 4s 4p] 10 2 6

E) [ Ar 4s 3d] 4 4

Answer: D

Diff: 1

Page Ref: Sec. 6.8