Determine what factors determine the type of bond formed between atoms in a molecule or formula unit. Indicate how it is measured and the electronegativity increases or decreases as the elements move up and down a group or across a period. Discuss the ionic and covalent characteristics of molecules.
Using a series of examples, determine how to classify molecules as either ionic, pure nonpolar covalent, polar covalent and dipolar. Practice problems using the subtraction of electronegativity values to determine which class they fall into.

Outline and discuss how resonance bonding occurs as the non bonded lone electron pairs move between atoms. Show examples of a few molecules which exhibit this tendency. Discuss, show examples, and then define what a coordinate covalent bond is and how it forms.

Using a series of written molecular formulas, work through how to correctly present a Lewis dot formula for them. From the dot formula, indicate stepwise how to correctly sketch a structural formula, and then a condensed structural formula. Have Joshua work out a few more examples for practice. Check for each that the octet rule has been satisfied.

Through written examples, and the Arrhenius definition of an acid, Determine exactly how to name binaryt acids, binary polyatomic acids and oxyacids.

Use examples and examine the rules for naming binary covalent molecules. Discuss the rules for naming of oxyacids by using a series of oxyacid formulas.

Review bond length and compare it to bond strength. Discuss the nomenclature for covalent bonds forming a binary compound between two non metal atoms and achieving stability.
Discuss heat of formation, endothermic and exothermic reactions

Construct from models single, double, and triple bonded molecules. Measure the bond length from nucleus to nucleus. Determine why the bond lengths are different. Elicit the general rule that as bond length decreases, bond strength increases. Define the energy of dissociation, elicit the relationship between the bond length and the energy of dissociation. Discuss how the total energy of a compound is determined. Define endothermic and exothermic compound formations.

Construct, using molecular models, diatomic molecules containing a single covalent bond, a double covalent bond, and a triple covalent bond. Have Joshua write the electron configuration for each element, determine the number of covalent bonds based on the number of incomplete valence orbitals, and then construct.
Determine from the models which of the three bonds appeared to be the most stable.

Explain using electron configuration and Lewis formulas how the covalent bond forms. Define a single covalent bond form examples and construct one using molecular models from the kit.
Indicate that all group 17 elements will form a single covalent bond, and that they exist as diatomic molecules. Define Halogen. Show how each halogen will form a single covalent bond with other non metals, such as hydrogen.

Analyze the lab results and review the questions in the post lab.
Examine the 15 hw questions , each with multiple parts. Discuss and explain those questions found difficult to answer.
Introduce covalent bonding. Define covalent bonding and use examples of diatomic molecules covalently bonding to achieve a stable electron configuration.