J. Muench WORKSHEET #8 CHEM 161 1. For each of the elements, give the shorthand electronic configuration. Then, for the valence electrons, draw the orbital diagram. Based on this diagram, how many unpaired electron does each element have? Element Shorthand Configuration Valence Shell Orbital Diagram # Unpaired F P Mn Co Br 2. For the following four elements, place them in order of increasing size. Mg, P, Ne, Ar 3. Circle the element or ion in EACH pair that has the larger radii. a. Ca+2 , Ca b. S-2 , S c. Cl- , I- d. Cl- , K+ 4. Circle the element in EACH pair that has the larger ionization energy. a. Ar , Ne b. N , O c. Al , Cl d. Na , Ar 5. The IE for Al is less than that for Mg. Explain why this occurs. 6. The third ionization energy for magnesium is +7730kJ whereas the third ionization energy for aluminum is only +2750kJ. Explain why this occurs.J. Muench 7. What is the shorthand electron configuration for each of the ions? a. S-2 b. Cr+3 c. Al+3 d. Zn+2 8. Circle the element in EACH pair that has the larger electron affinity. a. C , F b. B , Be c. Li , N d. Cl , Ar 9. Match the following descriptions to one of the elements. Each element will be used only once. Your choices are: Mg, F2, N2, Si, and Ne. a. ___ - This element is an unreactive gas, has a moderate I.E., no E.A., and forms an acidic oxide. b. ___ - This element has the largest radii of the five, has a low I.E. and no E.A.. c. ___ - This element is very reactive gas, has a large I.E., and a large E.A.. d. ___ - This element is an unreactive gas, has a very large I.E., and no E.A.. e. ___ - This element unreactive, tends to form covalent compounds, has a moderate I.E. and E.A.. 10. Explain each of the following observations. Hint: apply what you have learned about relative IE and/or EA’s. a. Ca is much more reactive than C b. K is more reactive than Li c. F2 is more reactive than