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AP Chemistry
Chapter 8
Concepts
Details
Types of
A. Ionic Bonding
Chemical
Bonds
B. Coulomb’s Law
C. Bond Length
D. Covalent Bonds
Electro –
A. Electronegativity
negativity
B. Electronegativity Trends
1
AP Chemistry
Chapter 8
C. Characterizing bonds
Practice

Problem
Order the following bonds according to polarity:
H-H, O-H, H-Cl, H-S and F-H
#1
Bond
A.
Dipolar Molecules
Polarity
and Dipole
Moments
B. Molecules with Polar Bonds but no Dipole Moment
Ion
A. Bonding and Noble Gas Electron Configurations
Electron
Configurati
on and
B. Predicting Formulas of Ionic Compounds
Sizes
C. Sizes of Ions
2
AP Chemistry
Chapter 8
Practice
Choose the largest ion in each of the following groups. Explain why it
Problem
is the largest ion.
#2
A) Li+, Na+, K+, Rb+, Cs+
B) Ba2+, Cs+, I-, Te2Formation
A. Lattice Energy
of Binary
Ionic
Compounds
B. Lattice Energy Calculations
Partial
A. Calculating Percent Ionic Character
Ionic
Character
of Covalent
B. Ionic vs. Covalent
Bonds
3
AP Chemistry
Chapter 8
The
A. Strengths of the Bond Model
Chemical
covalent
bond: A
model
B. Weaknesses of Bond Model
Covalent
A. Average Bond Energies
Bond
Energies
and
Chemical
Reactions
B. Multiple Bonds
C. Bond Energy and Enthalpy
4
AP Chemistry
Chapter 8
Practice
Using the bond energies listed in table 8.4, calculate the H for the
Problem
reaction of methane with chlorine and fluorine gas to give Freon-12
#3
(CF2Cl2).
CH4 (g) + 2Cl2 (g) + 2F2 (g)  CF2Cl2 (g) + 2 HF (g) + 2HCl (g)
The
A. Lone Electron Pairs
Localized
Electron
Bonding
B. Bonding Electron Pairs
Model
C. Localized Electron Model
D. Derivations of the Localized Model
Lewis
A. Electrons and Stability
Structures
B. Writing Lewis Structures
Rules
5
AP Chemistry
Chapter 8
Practice
Give the Lewis structure for each of the following:
Problem
HF, N2, NH3, CH4, CF4, NO+
#4
Exceptions
A. Boron Trifluoride
to the octet
rule
B.
Sulfur Hexaflouride
C. More about the octet rule
6
AP Chemistry
Chapter 8
Practice
Write the Lewis structure for each of the following:
Problem
PCl5, ClF3, XeO3, RnCl2, BeCl2, ICl4-
#5
Resonance
A. Nitrate Ion
Structures
B. Resonance
Practice
Describe the electron arrangement in the in the nitrite anion (NO2-)
Problem
using the localized electron model.
#6
7
AP Chemistry
Chapter 8
Molecular
A. Valence Shell Electron Pair Repulsion
Structure:
The VSEPR
Model
B. Effect of unshared pairs
C. VSEPR and Multiple Bonds
8
AP Chemistry
Chapter 8
D. Molecules Containing no Single Central Atom
E. How well does VSEPR work?
Describe the molecular structure of a water molecule.
When phosphorous reacts with excess chlorine gas, the compound
phosphorous pentachloride (PCl5) is formed. In the gaseous and
liquid states, this substance consists of PCl5 molecules,
But in the solid state is consists of a 1:1 mixture of PCl4- and PCl6ions. Predict the geometric structures of PCl5, PCl4- and PCl6-.
Practice
Problem
#7
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