Pre CH9 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.
How differences in atomic properties lead to differences in bond type; the basic distinctions among the three types of bonding (§9.1)
2.
The essential features of ionic bonding: electron transfer to form ions, and their electrostatic attraction to form a solid (§9.2)
3.
How lattice energy is ultimately responsible for the formation of ionic compounds (§9.2)
4.
How ionic compound formation is conceptualized as occurring in hypothetical steps (a Born-Haber cycle) to calculate the lattice energy (§9.2)
5.
How Coulomb's law explains the periodic trends in lattice energy (§9.2)
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6.
Why ionic compounds are brittle and high melting and conduct electricity only when molten or dissolved in water (§9.2)
7.
How nonmetal atoms form a covalent bond (§9.3)
8.
How bonding and lone electron pairs fill the outer (valence) level of each atom in a molecule (§9.3)
9.
The interrelationships among bond order, bond length, and bond energy (§9.3)
10.
How the distinction between bonding and nonbonding forces explains the properties of covalent molecules and network covalent solids (§9.3)
11.
How changes in bond strength account for the enthalpy of reaction (§9.4)
12.
How a reaction can be divided conceptually into bond-breaking and bond-forming steps (§9.4)
13.
The periodic trends in electronegativity and the inverse relationship of EN values to atomic sizes (§9.5)
14.
How bond polarity arises from differences in the electronegativities of bonded atoms; the direction of bond polarity (§9.5)
15.
The change in partial ionic character with ∆EN and the change from ionic to polar covalent to nonpolar covalent bonding across a period (§9.5)
16.
The role of delocalized electrons in metallic bonding (§9.6)
17.
How the electron-sea model explains why metals bend, have very high boiling points, and conduct electricity in solid or molten form (§9.6)
Master These Skills
1.
Using Lewis electron-dot symbols to depict main-group atoms (§9.1)

2.
Depicting the formation of ions with electron configurations, orbital diagrams, and Lewis symbols, and writing the formula of the ionic compound (SP 9.1)
3.
Calculating lattice energy from the enthalpies of the steps to ionic compound formation (§9.2)
4.
Ranking lattice energies from ionic properties (SP 9.2)
5.
Ranking similar covalent bonds according to their length and strength (SP 9.3)
6.
Using bond energies to calculate (SP 9.4)
7.
Determining bond polarity from EN values (SP 9.5)
Key Terms Page numbers appear in parentheses.
Section 9.1
ionic bonding (360) covalent bonding (360) metallic bonding (361)
Lewis electron-dot symbol (361) octet rule (362)
Section 9.2
lattice energy ( ) (364)
Born-Haber cycle (364)
Coulomb's law (365) ion pairs (368)
Section 9.3
covalent bond (369) bonding (shared) pair (370) lone (unshared) pair (370) bond order (370) single bond (370) double bond (370) triple bond (370) bond energy (BE) (370) bond length (371)

infrared (IR) spectroscopy (374)
Section 9.5
electronegativity (EN) (380) polar covalent bond (382) nonpolar covalent bond (382) electronegativity difference (∆EN) (382) partial ionic character (382)
Section 9.6
electron-sea model (385) alloys (386)
Key Equations and Relationships Page numbers appear in parentheses.
 9.1 Relating the energy of attraction to the lattice energy ( 365 ):
 9.2 Calculating enthalpy of reaction from bond enthalpies or bond energies ( 377 ):
• (a) List three ways elements combine (i.e. list three types of bonds). Give example of each.
(b) Read about Lattice Energy. Explain in your own words.
(c) Bond energy is a short term for bond dissociation energy. All bond energies are positive. What does it mean?

(d) Read about Electronegativity. Explain in your own words.
(e) Defind "Polar Bond". Give two examples of polar bonds.