HW05 Quantum Numbers and Orbitals – mccord – (51315)

thomas (tt9669) – HW05 Quantum Numbers and Orbitals – mccord – (51315)This print-out should have 30 questions.Multiple-choice questions may continue onthe next column or page – find all choicesbefore answering.001 10.0 pointsWhich of the following provided evidence thatthe electrons in atoms are arranged in distinctenergy levels?11. 486 nm2. 2.45 nm3. 205 nm4. 8.63 nm5. 94.9 nm1. the results of the Millikan oil-drop experiment2. the observation of line spectra from gasdischarge tubes004 (part 2 of 3) 10.0 pointsWhat is the name given to the spectroscopeseries to which this transition belongs?1. Balmer series3. the existence of elements with nonintegervalues for atomic weights4. the scattering of α particles by a metalfoil2. Paschen series3. Pfund series4. Brackett series5. the deflection of ions in a mass spectrometer002 10.0 pointsAssume n1 and n2 are two adjacent energylevels of an atom. The emission of radiationwith the longest wavelength would occur forwhich two values of n1 and n2 ?5. Lyman series005 (part 3 of 3) 10.0 pointsIn what region will the light lie?1. visible, red2. infrared1. 4,33. ultraviolet2. 3,24. x-ray, gamma ray3. 2,15. visible, blue4. 6,56. visible, yellow5. 5,46. 7,67. 8,7003 (part 1 of 3) 10.0 pointsUse the Rydberg formula for atomic hydrogento calculate the wavelength for the transitionfrom n = 4 to n = 2.006 10.0 pointsThe graph shows the radial distribution plotsfor the 1s wavefunctions for H, He, and He+ .thomas (tt9669) – HW05 Quantum Numbers and Orbitals – mccord – (51315)4πr 2Ψ2AB25. 3pC009 10.0 pointsThe number that describes the main energylevel of an electron in an atom is1. the magnetic quantum number m .radiusWhich plot is the 1s wavefunction for the He+ion?1. B2. C3. A4. There is no way to know007 10.0 pointsHow many electrons can have the quantumnumbers n = 3; = 2; m = +1 in an atom?2. the atomic number Z.3. the mass number A.4. the angular momentum (or subsidiary)quantum number .5. the principal quantum number n.010 10.0 pointsCan an electron in an atom be in an energylevel described by the set of quantum numbersn = 5, = 3, m = −2?1. Yes2. No, because m must be equal to ±1.1. 33. No, because must be equal to n −1.2. 54. No, because m cannot be negative.3. 25. No, because n cannot be as large as 5.4. 65. 4008 10.0 pointsThe three quantum numbers for an electron ina hydrogen atom in a certain state are n = 4,= 2, m = 1. The electron is located inwhat type of orbital?011 10.0 pointsAn electron in a 3d orbital could have whichof the following quantum numbers?= 2; m = 02. n = 3;= 1; m = −13. n = 3;= 0; m = 04. n = 3;= 2; m = −35. n = 2;1. 4p1. n = 3;= 2; m = 66. n = 3;= 3; m = 12. 4d3. 3d4. 4sthomas (tt9669) – HW05 Quantum Numbers and Orbitals – mccord – (51315)7. n = 3;= 1; m = 2012 10.0 pointsHow many p electrons does Se (atomic number 34) possess?ground-state2s2 2p2 ?electronconfiguration3[He]1. beryllium2. fluorine1. 63. hydrogen2. 124. lithium3. 345. oxygen4. 06. neon5. 107. boron6. 168. carbon7. 49. helium013 10.0 pointsFor which H-atom wavefunction are you mostlikely to find the electron farthest from thenucleus?1. 1s10. nitrogen016 10.0 pointsWhich of the following is the valence electronic structure for a halogen?2. 2p1. n s23. 3p2. n s2 n p54. 2s3. n s2 n d105. 4p4. n s1014 10.0 pointsThe transition metals are elements with partially filled1. f subshells.5. n s2 n p6017 10.0 pointsIn the Aufbau order of occupancy of electronicenergy levels, the level occupied just after 4pis2. p subshells.1. 4d.3. s subshells.2. 6p.4. d subshells.3. 3f .015 10.0 pointsWhich element is predicted to have the4. 5p.thomas (tt9669) – HW05 Quantum Numbers and Orbitals – mccord – (51315)5. 5s.018 10.0 pointsThe electron configuration for the Mn atom is1. 1s2 2s2 2p6 2d10 3s2 3p3 .4021 10.0 pointsAs an atom’s radius decreases,1. its ionization energy does not change.2. its ionization energy increases or decreases depending on whether you are goingup a column or across a row.2. None of these3. its ionization energy increases.3. 1s2 2s2 2p6 3s2 3p6 4s2 4p5 .4. its ionization energy decreases.4. 1s2 2s2 2s6 3s6 3d7 .5. 1s2 2s2 2p6 3s2 3p6 4s2 3d5 .019 10.0 pointsThe ground state electron configuration ofthe silver atom is [Kr] 5s1 4d10 instead of [Kr]5s2 4d9 . The observation can be explained(theoretically) by the fact that022 10.0 pointsWhich of the following would be expected tohave the highest first ionization energy?1. Xe2. Si3. Na1. only one electron can occupy a 5s orbital.2. the 4d subenergy level has higher energythan the 5s subenergy level.3. an enhanced stability is associated withfilled sets of equivalent orbitals.4. the magnetism measurement shows oneunpaired electron.4. Ar5. Cl023 10.0 pointsHow many s electrons does P (atomic number15) possess?1. 62. 155. the 4d subenergy level always has 10 electrons.020 10.0 pointsWhich of the following atoms has the largestradius?1. Br2. Ne3. F4. Cl3. 24. 45. 06. 5024 (part 1 of 4) 10.0 pointsHow many values of the quantum numberare possible when n = 7?1. 6thomas (tt9669) – HW05 Quantum Numbers and Orbitals – mccord – (51315)52. 73. 4028 10.0 pointsThe diameter of the electron density of anatom is roughly4. 51. None of these5. 32. 1 nm.025 (part 2 of 4) 10.0 pointsHow many values of m are allowed for anelectron in a 5 f subshell?3. 0.1 nm.4. 100 nm.1. 35. 10 nm.2. 43. 74. 65. 5026 (part 3 of 4) 10.0 pointsHow many values of m are allowed for anelectron in a 2 s subshell?029 10.0 pointsFor which of the following elements would thesize of the neutral atom (atomic radius) belargest?1. K2. Rb3. Sr1. 14. Ca2. None of these5. Na3. 44. 35. 2027 (part 4 of 4) 10.0 pointsHow many subshells are there in the shell withn = 3?030 10.0 pointsWrite an equation that represents the secondionization energy of copper.1. Cu(g) −→ Cu2+ (g) + 2 e−2. Cu+ (g) −→ Cu2+ (g) + 2 e−3. Cu(g) −→ Cu+ (g) + e−1. 34. Cu(g) −→ Cu2+ (g) + e−2. 45. Cu+ (g) −→ Cu2+ (g) + e−3. 64. 25. 5