Review 08
REVIEW QUESTIONS
Chapter 8
Use only a periodic table to answer the following questions.
- Write complete electron configuration for each of the following elements:
a) Aluminum (Al)
b) Sulfur (S)
c) Manganese (Mn) - Write condensed orbital diagrams for each of the following elements and determine the number of unpaired electrons in each:
a)Zinc
b) Selenium (Se)
c) Lead (Pb) - Identify the element that belongs to each of the following electron configurations:
a)
b)
c)
d) - A section of the periodic table with all identification features removed is shown below.
| V | W | X |
| Y | Z |
Which element has the smallest atomic radius? Give a brief explanation for your choice.
5. A period 3 element has the following ionization energies. What is the identity of this element?
6. Arrange each of the following elements in order of increasing atomic radius.
a)
b) B, Ca, Ga, Cs
c)
7. Arrange the following in order of increasing first ionization energy.
a)
b)
c)
8. The first four ionization energies of yttrium (
a) Explain the increasing trend in the successive energies of yttrium.
b) Explain the large increase in
c) Explain the large increase in
9. Explain why alkali metals have a greater electron affinity than alkaline earth-metals.
10. Which element in each of the following sets would you expect to have the highest second ionization energy (
a)
b)
11. Until the early 1960s the group 8A elements were called inert gases. They are no longer referred to as such, since Xe and Kr were found to react with some substances. Suggest a reason why Xe would react with fluorine, but Ne would not.
12. The table below gives the electron affinities in
5. A period 3 element has the following ionization energies. What is the identity of this element?
6. Arrange each of the following elements in order of increasing atomic radius.
a)
b) B, Ca, Ga, Cs
c)
7. Arrange the following in order of increasing first ionization energy.
a)
b)
c)
8. The first four ionization energies of yttrium (
a) Explain the increasing trend in the successive energies of yttrium.
b) Explain the large increase in
c) Explain the large increase in
9. Explain why alkali metals have a greater electron affinity than alkaline earth-metals.
10. Which element in each of the following sets would you expect to have the highest second ionization energy (
a)
b)
11. Until the early 1960s the group 8A elements were called inert gases. They are no longer referred to as such, since Xe and Kr were found to react with some substances. Suggest a reason why Xe would react with fluorine, but Ne would not.
12. The table below gives the electron affinities in
| 1 B | 2 B |
| Cu | Zn |
| -119 |
|
| Ag | Cd |
| -126 |
|
| Au | Hg |
| -223 |
|
a) Explain why group 1 B elements have negative electron affinities, while group 2 B elements have positive values.
b) Explain why group 1B electron affinities become more negative moving down the group.
13. For each set shown below, select the atoms or ions that are isoelectronic with each other, and write their electron configuration:
a)
b)
c)
14. Explain each of the following trends in ionic radii:
a)
b)
15. Arrange the atoms or ions in each of the following sets in order of increasing radius:
a)
b)
c)
d)
b) Explain why group 1B electron affinities become more negative moving down the group.
13. For each set shown below, select the atoms or ions that are isoelectronic with each other, and write their electron configuration:
a)
b)
c)
14. Explain each of the following trends in ionic radii:
a)
b)
15. Arrange the atoms or ions in each of the following sets in order of increasing radius:
a)
b)
c)
d)