Problem Set
Periodic Table Review
Complete all questions on your own sheet(s) of paper.
1. Draw a periodic table and indicate the trends in terms of atomic radii, ionic radii, ionization energy, and
metallic character. Be sure to show the trends down the table as well as across the table.
2. State the Periodic Law.
3. How do metal atoms and metal ions compare in terms of atomic (ionic) radius? Explain why using the
factors that affect atomic radius.
4. Nearly all elements react with fluorine. Write the formulas of the compounds that form with the
elements of the 3 period when reacted with fluorine.
5. State the meaning of the terms: nuclear charge, shielding effect, electron-electron repulsions.
6. What two statements can be made about the structure of the periodic table as it relates to electron
structure of atoms?
7. What is the group name (chemical family) that the following elements are located in:
a) Ba
b) Fe
c) Kr
d) Cl
e) Pu
f) Rb
8. Explain the trend of the atomic radius as you move from left to right on the periodic table. Provide
reasons why this trend exists.
9. a) What does ionization energy refer to?
b) Write an equation to show the first ionization of a chlorine atom
10. Explain which is larger and why it is:
a) Ca and Br atoms
b) Br and I atoms
c) As ion and Se ion
d) Sr ion and Sr atom
11. Explain why magnesium has a 1st ionization energy of 418 kJ/mol and 2nd ionization energy of 789
kJ/mol while its 3rd ionization energy is 4067 kJ/mol.
12. a) Name the element with the largest atomic radius.
b) Name the element with the largest ionization energy (excluding noble gases).
13. How do non-metal atoms and non-metal ions compare in terms of atomic (ionic) radius? Explain why
using the factors that affect atomic radius.
14. Predict some of the chemical properties and physical properties for each element: francium, bromine,
and neon.
15. Which element would be more metallic: Beryllium or Calcium? Why?
16. If shown a graph of ionization energy vs. atomic number of the first 54 elements, what would you expect
its shape to be? Sketch it and explain how you arrived at the your answer.
17. Where would one expect to find the noble gases on this graph of Ionization Energy vs. Atomic Number?
18. Oxygen and sulphur are very different elements in that one is a colourless gas and the other is a yellow
crystalline solid. Why are they both in Group VIA?
19. What does the term isoelectronic mean?
20. Why would it be so much more difficult to remove the a second electron (called the second ionization
energy (IE 2) from an ion than the first (IE 1)?
21. Explain why the element fluorine is the most reactive element on the periodic table.
22. Explain why the ionization energy will decrease as you go down a family?
23. The radius of P is much smaller than the ionic radius of P3-. Why is this?