Electron Configuration Part I

Electron Configuration Part I Page 1 ELECTRON CONFIGURATION PART I Name __________________________________ 1. Write the electronic configuration for the valence electrons for each of the following elements and ions and their Lewis Dot Structure: Period Group IA Group IIA Group IIIA Group VIA GroupVII A Atom Ion Atom Ion Atom Ion Atom Ion Atom Ion 2 Li Li+ Be Be2+ B B3+ O O2-F F-3 Na Na+ Mg Mg2+ Al Al3+ S S2-Cl Cl-4 K K+ Ca Ca2+ Ga Ga3+ Se Se2-Br Br-If you want to learn and not just memorize rules, it is CRITICAL that you don’t use notes or the text for the rest of the problem! 2. The periodic table below shows the periodic trends for the atomic radius and the ionization energy (IE) Electron Configuration Part I Page 2 Based on the table that you built in Question 1, the periodic trends shown above and the two pictures below explain: a. why the radii of atoms decrease across a period. b. why the radii of atoms increase down a group. c. why the ionization energy increases across a period. d. why the ionization energy decreases down a group. 3. The radius of a cation (positive ion) is always smaller than that of the atom from which it is derived. On the other hand, the radius of an anion (negative ion) is always bigger than that of the atom from which it is derived. Using the information provided above, explain why. 4. Write the electronic configuration of the following elements and ions (Watch for the exceptions!): Cr Cr3+ Fe Fe2+ Ne Fe3+ Cu Cu+ C Cu2+ Electron Configuration Part I Page 3