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Periodic Trends Name: Part 1: Summary of the Periodic Trends Property Definition Across a Period Down a Group Atomic Radius Ionic Radius 1st Ionization Energy Eletronegativity Electron Affinity Part 2: Explaining Periodic Trends 1. Why is it easier to remove an electron from a larger atom than from a smaller atom? 2. What happens to the amount of positive charge in the nucleus as you move from left to right across a period? What happens to Zeff as you move from left to right across a period? a. How does this account for the trend you discovered in atomic radius? b. How does this account for the trend you discovered in 1st ionization energy? c. How does this account for the trend you discovered in electron affinity? 3. What is different about the number of energy levels in an atom as you move down a group? How does that affect shielding? a. How does this account for the trend you discovered in atomic radius? b. How does this account for the trend you discovered in 1st ionization energy? c. How does this account for the trend you discovered in electronegativity? 4. What is the relationship between group (Groups 1, 2, and 3 -18) and the number of valence electrons? a. How does this account for the ions that are formed for each group? b. How does this account for the trend you discovered in ionic radius? c. What is the relationship between the number of valence electrons an atom has and its electronegativity? Part 3: Applying Periodic Trends 1. Which group on the periodic table has the largest atomic radii? 2. Which group on the periodic table has the largest 1st ionization energy? 3. Which element on the periodic table has the highest and lowest electron affinity? 4. Which element on the periodic table has the largest and smallest atomic radius? 5. Which element on the periodic table has the highest and lowest 1st ionization energy? 6. Which element on the periodic table has the highest and lowest electronegativity? 7. Compare the elements Fe and Cu in answering these questions. a. Which element has the smaller radius? b. Which element has the larger 1st ionization energy? c. Which element has the largest electronegativity? 8. In the following pairs of elements, which one has the larger atomic radius? a. Cs or Fr b. Sn or Pb c. Ag or Cd 9. In the following pairs of elements, which one has the larger 1st ionization energy? a. Cs or Ba b. Sb or Bi c. Au or Hg d. O or N 10. In the following pairs of elements, which one has the larger electron affinity? a. F or Cl b. Si or P c. Cu or Zn d. Mn or Fe 11. Place the following elements/ions in order of increasing radius. a. Na, K, Li b. Te, I, Xe c. Fe, P, O d. O, O-, O2e. Se2-, Ca2+, Br-, K+ 12. What is an isoelectronic series?
