Periodic Trends Worksheet
1. What trend do you see in atomic radius as you go down a group?
2. What causes this trend?
3. Circle the atom in each pair that has the largest atomic radius
a. Al or B
b. S or O
d. Na or Al
c. Br or
e. O or F
Cl
f. Mg or Ca
4. Define ionization energy
5. Why does sodium form a 1+ ion while magnesium forms a 2+ ion?
6. Circle the atom in each pair that has the greater ionization energy.
a. Li or Be
b. Na or K
c. Cl or Si
d. Ca or Ba
e. P or Ar
f. Li or K
7. Define electronegativity. What trend in electronegativity do you see moving across a period?
8. Circle the atom in each pair that has the greater electronegativity.
a. Ca or Ga
b. Li or O
c. Cl or S
d. Br or As
e. Ba or Sr
f. O or S
9. Rank the following elements by increasing atomic radius: carbon, aluminum, oxygen, potassium.
10. Rank the following elements by increasing electronegativity: sulfur, oxygen, neon, aluminum.
11. What is the difference between electronegativity and ionization energy?
12. Why does fluorine have higher ionization energy than iodine?