Pre CH8 HW for Silberberg
Followings are what you will find at the end of the chapter in your textbook.
For LEARNING OBJECTIVES: Highlight the main idea for EACH objective. Ready carefully so you
don’t highlight everything.
For MASTER THESE SKILLS: Highlight the main idea for each skill. Ready carefully so you don’t
highlight everything.
For KEY TERMS: Make sure you can define it and/or give an example of it. Pick TWO terms of your
choice and actually write the definition or an example.
For KEY EQUATIONS AND RELATIONSHIP: Next to EACH, define each term. Be very specific.
CHAPTER REVIEW GUIDE
Learning Objectives Relevant section (§) and/or sample problem (SP) numbers appear in parentheses.
Understand These Concepts
1.
2.
3.
4.
The meaning of the periodic law and the arrangement of elements by atomic number (Introduction)
The reason for the spin quantum number and its two possible values (§8.1)
How the exclusion principle applies to orbital filling (§8.1)
The effects of nuclear charge, shielding, and penetration on the splitting of energy levels; the meaning of
effective nuclear charge (§8.1)
5. How the arrangement of the periodic table is based on the order of sublevel energies (§8.2)
6. How sublevels are filled in main-group and transition elements; the importance of Hund's rule (§8.2)
7. How outer electron configuration within a group is related to chemical behavior (§8.2)
8. The distinction among inner, outer, and valence electrons (§8.2)
9. The meaning of atomic radius, ionization energy, and electron affinity (§8.3)
10. How n value and effective nuclear charge give rise to the periodic trends of atomic size and ionization
energy (§8.3)
11. The importance of core electrons to the pattern of successive ionization energies (§8.3)
12. How atomic properties relate to the tendency to form ions (§8.3)
13. The general properties of metals and nonmetals (§8.4)
14. How vertical and horizontal trends in metallic behavior are related to ion formation and oxide acidity
(§8.4)
15. How atomic size and IE relate to redox behavior (§8.4)
16. Why main-group ions are either isoelectronic with the nearest noble gas or have a pseudo–noble gas
electron configuration (§8.4)
17. Why transition elements lose ns electrons first (§8.4)
18. The origin of paramagnetic and diamagnetic behavior (§8.4)
19. The relation between ionic and atomic size and the trends in ionic size (§8.4)
Master These Skills
1.
2.
3.
4.
5.
6.
Correlating orbital diagrams and the set of quantum numbers for any electron in an atom (SP 8.1)
Writing full and condensed electron configurations for an element (SP 8.2)
Using periodic trends to rank elements by atomic size and first ionization energy (SPs 8.3, 8.4)
Identifying an element from its successive ionization energies (SP 8.5)
Writing electron configurations of main-group and transition metal ions (SPs 8.6, 8.7)
Using periodic trends to rank ions by size (SP 8.8)
Page 353
Key Terms Page numbers appear in parentheses.
Introduction
periodic law (323)
electron configuration (323)
Section 8.1
spin quantum number (ms) (324)
exclusion principle (325)
shielding (325)
effective nuclear charge (Zeff) (325)
penetration (326)
Section 8.2
aufbau principle (327)
orbital diagram (327)
Hund's rule (328)
transition elements (332)
inner (core) electrons (334)
outer electrons (334)
valence electrons (334)
inner transition elements (335)
lanthanides (rare earths) (335)
actinides (335)
Section 8.3
atomic size (336)
metallic radius (336)
covalent radius (336)
ionization energy (IE) (339)
electron affinity (EA) (343)
Section 8.4
amphoteric (346)
isoelectronic (347)
pseudo–noble gas configuration (347)
paramagnetism (349)
diamagnetism (349)
ionic radius (350)
Key Equations and Relationships Page numbers appear in parentheses.

8.1 Defining the energy order of sublevels in terms of the angular momentum quantum number (l value)
(326):

8.2 Meaning of the first ionization energy (339):
Answer the following questions. Show your work.
•
(a) The Figure 8.5 on page 327 has the ORDER for filling energy sublevels with electrons. Re-write the order
starting with 1s.
(b) Read about Exclusion Principle. Explain in your own words.
(c) Read about Aufbau Principle. Explain in your own words.
(d) Read about Hund's Rule. Explain in your own words.
(e) Write electron configuration for element #1 (Hydrogen) to element #10 (Neon).
(f) Summarize the periodic trends for (1) atomic size (2) ionization energy (3) electron affinity (4) metallic
behavior.