Unit 4.2 Bonding, Lewis Structures, and Intermolecular Forces

Learning Objectives

You will be able to:

1. drawn an electron dot diagram for an atom or ion.
   explain the octet rule. What does the term "octet" mean and what does it have to do with electron configurations?

2. predict whether a compound will be ionic or covalent.
   explain the properties of compounds with ionic bonds.
   Note: the practice for Ionic Bonding is really wrapped up in the naming of 4.1

3. explain the properties of metallic bonds.
   Note: metallic bonding is theory that you are responsible for at a conceptual level.

4. distinguish between polar and nonpolar bonds.
   identify the elements which occur naturally as diatomic molecules.
   explain the properties of compounds with covalent bonds.

5. draw Lewis structures for molecular compounds and polyatomic ions.
   compute formal charges for atoms in any Lewis structure
   use formal charges to identify the most reasonable Lewis structure for a molecule.
   explain the concept of resonance and draw Lewis structures representing resonance forms for a molecule.
   identify sigma and pi bonds.

6. predict the hybridization for a given atom in a molecule.
   predict (draw and name) the correct geometry for a molecule or polyatomic ion.
   determine whether a given molecule or polyatomic ion is polar.

7. identify the type or types of intermolecular forces (IMFs) that a particular compound or functional group can demonstrate
   explain how these IMFs arise.
   predict molecular interactions based on molecular geometry.

Readings

1. 8.1  Electron Dot Diagrams
   8.2  Octet Rule

2. 8.6  Ionic Bond
   8.7  Ionic Crystal Structure
   8.9  Physical Properties of Ionic Compounds

3. 8.10  Metallic Bond

4. 9.2  Covalent Bond
   9.3  Molecular Compounds
   9.4  Energy and Covalent Bond Formation
   9.12  Bond Energy

5. 9.5  Lewis Electron-Dot Structures
   9.6  Single Covalent Bonds
   9.7  Multiple Covalent Bonds
   9.8  Coordinate Covalent Bond
   9.9  Covalent Bonding in Polyatomic Ions
   9.10  Resonance
   9.11  Exceptions to the Octet Rule

6. 9.13  VSEPR Theory
   9.14  Molecular Shapes: No Lone Pairs on Central Atom
   9.15  Molecular Shapes: Lone Pair(s) on Central Atom
   9.22  Hybrid Orbitals - sp3
   9.23  Hybrid Orbitals - sp and sp2
   9.24  Sigma and Pi Bonds

7. 9.16  Bond Polarity

9.17  Polar Molecules

9.18  Van der Waals Forces
9.19  Hydrogen Bonding
9.20  Physical Properties and Intermolecular Forces

Notes

Laboratory

Worksheets

Laboratory

Resources

Lewis Structures

VSEPR Theory