(use SF, units; show all work; answers in box) 1: a: What is the frequency of light with a wavelength of 357.2 m? b: What is the energy of the photon from part a? 2: a: What is the frequency (in Hertz) of an x-ray with an energy of 3.573 x 10-17 J? b: What is the wavelength of the x-ray from part a in nanometers? 3: a: What is the wavelength (in nm) of a proton moving at 35.8 Mm/s? b: What is the energy in J of a single fluorine atom moving at 4.470 x 10 5 m/min? 4: Sketch the shapes of an s orbital, a p orbital, and a d orbital in that order. 5: Give the possible values of all four quantum numbers for the following subshells: a: 4p b: 2s c: 7d d: 5f 6: How many electrons maximum could you fit into each of the following subshells: a: 3p b: 6s c: 2d d: 7f 7: Which of the following sets of quantum numbers are unacceptable? Briefly explain. a: (5, 0, 1, ½) b: (3, 2, -1, -1/2) c: (3, 3, 1, +1/2) d: (5, 1, -1, +1/2) e: (2, 1, 1, 1) 8: List all six transition metals that you would expect to experience the promotion effect. 9: Do the complete orbital diagram for germanium at the bottom of the page. From it, answer all of the following questions. a: # of occupied shells b: # of occupied subshells c: # of occupied orbitals d: # of filled shells e: # of filled subshells f: # of filled orbitals g: # of unpaired electrons h: Is it diamagnetic or paramagnetic? 10: Do electron configurations for the following elements. (Abbreviated is fine.) a: Co b: Ca c: Cl d: W e: Hg f: Sn g: Ag h: Ar i: Am (element 95) 11: Do orbital diagrams for each of the following elements, then determine the number of unpaired electrons. (Abbreviated is fine.) a: Si b: Ga c: Ti d: Sr e: Kr f: Au 1: Which of these electron configurations have similar chemical properties? a: 1s22s22p63s23p2 b: 1s22s2 c: 1s22s22p63s23p64s23d104p6 d: 1s2 e: 1s22s22p63s23p6 f: 1s22s22p63s23p64s23d104p2 g: 1s22s22p63s2 Briefly explain your reasoning: 2: Find the electron configurations of each of the following species (many are not stable). Ca Kr Rb+ S Se2- Si2- Ti2+ Zr4+ Determine which are isoelectronic with each other. 3: Specify the group number for each of the following elements: a: [Xe] 6s2 4f14 5d2 b: [Ne] 3s23p4 c. [Ar]4s23d10 4p5 d: [Kr] 5s1 4d5 4: How many core and valence electrons do each of the elements in problem 3 have? a: core: valence: b: core: valence: c: core: valence: d: core: valence: 5: Using just the periodic table, circle which atom in each pair has a larger atomic radius (size). For each pair briefly explain your reasoning. a: Al or P b: Ga or Tl c: Ne or Sn d: I Se or e: Ar or Li 6: Write the electron configurations for these ions: a: Ti4+ b: Zr2+ c: Pd5+ d: Co6+ e: Tc2+ f: W6+ g: Pb2+ h: As3i: C4j: Nb5+ k: Cu2+ 7: The first and second ionization energies of K are 419 kJ/mol and 3052kJ/mol, and those of Ca are 590 kJ/mol and 1145 kJ/mol, respectively. Explain why the second ionization energies are higher than the first ionization energies for both elements. Explain why the first ionization energy of K is lower than the first ionization of Ca. Explain why the second ionization energy of K is higher than the second ionization energy of Ca. 8: In each of the following pairs, circle whichever of these two species is smaller. Briefly explain why for each. a: S or S-2 b: Mg or Mg+2 c: Br1- or Cl1d: Ba2+ or Ie: Ca or Ti2+ 9: Which of these cations is larger, Mn+2 or Mn+7? Explain your reasoning. 10: Using only a periodic table arrange the elements in each of these groups in order of increasing electron affinity: a: Ca, Ga, Si, Sr b: Cl, Kr, Mg, Rb 11: What are degenerate orbitals? According to Hund’s rule, how are degenerate orbitals occupied? 12: Using only a periodic table put the following elements in order of increasing ionization energy: As, Cs, He, Mg, S 13: What are the valence electrons? Why are they important? 14: Use the periodic table to determine the element corresponding to each electron configuration. a: [Ar] 4s23d104p2 b: [Kr] 5s1 4d10 c: [Xe] 6s2 4f14 5d10 d: [Rn] 7s2 5f5 6d1 15: What is the approximate effective nuclear charge (Zeff) for each of the following? a: Mo b: Ba c: Se d: Si 16: Write the complete orbital diagram for each element. a: Cl b: V c: O d: C 17: Write orbital diagrams for each ion and determine if the ion is diamagnetic or paramagnetic. a. Zn2+ b. Hg+2 c. Mo4+ d. Nb2+ 
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