Demonstrate:

• how electron dot structures represent shared electrons.

 

Describe:

• how atoms form double or triple covalent bonds.
• how electronegativity values determine the distribution of charge in a polar molecule.
• how electrons are shared to form covalent bonds and identify exceptions to the octet rule.
• how oxygen atoms are bonded in ozone.
• how VSEPR theory helps predict the shapes of molecules.
• the information provided by a molecular formula.
• the relationship between atomic and molecular orbitals.
• what happens to polar molecules when they are placed between oppositely charged metal plates.

 

Distinguish:

• between a covalent bond and a coordinate covalent bond and describe how the strength of a covalent bond is related to its bond dissociation energy.
• between the melting points and boiling points of molecular compounds and ionic compounds.

 

Evaluate:

• the strength of intermolecular attractions compared with the strength of ionic and covalent bonds.

 

Identify:

• the reason why network solids have high melting points.
• ways in which orbital hybridization is useful in describing molecules.