Answer the following questions about nitrogen, oxygen, fluorine, and iodine using principles of atomic
and molecular structure
Element
N
O
F
I
First Ionization Energy (kJ/mol)
1402
1314
1681
???
Simply stating the trend is NOT sufficient! What is the reason we see the trend?
a. Explain why N has a smaller first ionization energy than F.
b. Explain why O has a smaller first ionization energy than N.
c. Would you predict the first ionization energy of atoms of iodine to be greater than, less than, or
equal to that of fluorine? Explain.
d. Which of the above atoms would have the largest atomic radius? Explain.
e. When bonded with fluorine, nitrogen atoms form the molecule NF3. However, atoms of iodine
can form IF3 and IF5 molecules. Explain.