Untitled - Kelly Walsh High School

Periodic Trends 125
in its ground state is the electron affinity (EA). The electron affinities tend to
increase going up a family and are greater on the right side of the periodic table.
There are exceptions for the trends of both the IE and EA. Many of these
exceptions involve a filled shell or subshell or a half-filled subshell.
1. Define effective nuclear charge.
2. What term refers to a column on the periodic table?
3. How does the effective nuclear charge change among the members of a
period on the periodic table?
4. True/False. The ionization energy may be either endothermic or exothermic.
5. True/False. The ionization energy is higher than expected for filled and
half-filled subshells.
6. The products resulting from the action of the ionization energy on a
gaseous atom are an electron and
a. an anion b. another atom c. a cation
d. a polyatomic ion e. an octet.
7. How does the effective nuclear charge affect the ionization energies of the
elements in a period on the periodic table?
8. How does the atomic radius affect the ionization energies of the elements
in a family on the periodic table?
9. Which elements in the third period of the periodic table are likely to have
unusually high ionization energies?
10. How does the ionic radius of K + compare to the atomic radius of K?
11. True/False. The electron affinity may be either endothermic or exothermic.
12. The product resulting from the action of the electron affinity and an electron
on a gaseous atom are:
a. an anion b. another atom c. a cation
d. a polyatomic ion e. an octet.
13. How does the effective nuclear charge affect the electron affinities of the
elements in a period on the periodic table?
14. How does the atomic radius affect the electron affinities of the elements in
a family on the periodic table?
15. How does the ionic radius of Cl compare to the atomic radius of Cl?
16. Rank the following elements in order of increasing ionization energy:
Ar, K, and Br.
17. Rank the following elements in order of increasing electron affinity:
Ar, K, and Br.
18. Rank the following in order of increasing radius:
O 2 , Ne, F , Mg 2 , and Na .
19. How would the energy necessary to convert a gaseous Al atom to a gaseous
Al 3 ion be found?
20. Why is the electron configuration of chromium, 1s 2 2s 2 2p 6 3s 2 3p 6 4s 1 3d 5 , an
exception to the Aufbau principle?