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Honors Chemistry - Reading Guide
Chapter Eight: Basic Concepts of Chemical Bonding
Objectives: the student will be able to:
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Define ionic bonds and lattice energy.
Define covalent bonds and octet rule
Draw Lewis structures for chemical compounds
Describe single, double and triple bonds with Lewis structures.
Describe polar covalent compounds based on electronegativity
Understand the concept of resonance structures.
Identify those exceptions to the octet rule.
8.1 Chemical Bonds, Lewis Structures and the Octet Rule
1. Define chemical bond and identify/define the three types of chemical bonds?
2. Define Lewis structure, especially as it relates to valence electrons and give
several examples (Table 8.1).
3. What is the octet rule and how does it relate to valence electrons?
8.2 Ionic Bonding
1. Explain the relationship between ionization energy and electron affinity in the
electron transfer process associated with ionic bonds.
2. Define lattice energy.
3. Relate lattice energy of ionic compounds to their physical properties.
4. Identify the relationship of lattice energy to atomic radii and ion charge.
5. Relate the formation of ionic compounds to electron configuration for the
representative (s&p-block) elements.
6. Identify patterns for forming ions for the transition metals.
7. What is the Born-Haber Cycle?
8. Define polyatomic ions.
9. Practice Problems: Pg. 337: 15, 17, 21, 23, (Ionic bonds)
8.3 Covalent Bonds
1. Define the attractive and repulsive forces in covalent bonds.
2. How are covalent bonds represented by Lewis structures? Give an example.
3. What is the difference between single, double and triple bonds?
4. How does bond length relate to the number of shared electrons (single/double or
triple bond, for example)?
5. Practice Problems: Pg. 337: 31, 35, 37, 39 (covalent bond, electronegativity &
bond polarity)
8.4 Bond Polarity and Electronegativity
1. Explain why bond polarity applies to covalent and not ionic compounds. What
are non-polar and polar covalent bonds?
2. Define electronegativity as it relates to ionization energy and electron affinity.
3. Relate electronegativity to bond polarity.
4. Define dipole moment.
8.5 Drawing Lewis Structures
1. Outline the procedure for drawing Lewis structures.
2. Identify the process for assigning a formal charge for atoms in a molecule.
3. Pg. 338: 45, 49, 57, 61 (Lewis structure and exception to the octet rule)
8.6 Resonance Structures
1. Briefly, define resonance structures and give one example.
2. Relate resonance structures to the structure of benzene (organic, aromatic
compound).
8.7 Exceptions to the Octet Rule
1. Site the three main exceptions to the octet rule and give an example of each.
2. Pg 339: 65, 67, 71 (bond enthalpy)
8.8 Strengths of covalent bonds
1. How is bond strength determined for covalent compounds?
2. Relate bond enthalpy to chemical stability.
3. How is bond enthalpy applied to determine reaction enthalpy (ΔHrxn)?