1. Rank the following elements by increasing atomic radius: carbon, aluminum, oxygen, potassium.
2. Rank the following elements by increasing electronegativity: sulfur, oxygen, neon, aluminum.
3. Rank the following elements by increasing electron affinity: sulfur, oxygen, neon, aluminum.
4. Explain why fluorine has a higher ionization energy than iodine.
5. What is the relationship between atomic radius and ionization energy?
6. Why does removing an electron from an atom (ionization energy) require an input of energy?
7. What trend in atomic radius occurs down a group on the periodic table? What causes this trend?
8. What trend in atomic radius occurs across a period on the periodic table? What causes this trend?
9. Indicate whether the following properties increase or decrease from left to right across the
periodic table.
a. atomic radius (excluding noble gases)
b. first ionization energy
c. electronegativity
d. electron affinity
10. Why do you think elements in the same family generally have similar properties?